We provide solutions practice exercises, instructions, and a learning material that allows learners to study outside of the classroom. We focus on solutions skills mastery so, below you will get all questions that are also asking in the competition exam beside that classroom.

#### List of solutions Questions

Question No | Questions | Class |
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1 | Henry’s law constant for the solubility of ( N_{2} ) gas in water at ( 298 mathrm{K} ) is ( 1.0 times 10^{5} ) atm. The mole fraction of ( N_{2} ) in air is 0.6 The number of moles of ( N_{2} ) from air dissolved in 10 moles of water at ( 298 mathrm{K} ) and 5 atm pressure is: A ( .3 .0 times 10^{-4} ) В. ( 4.0 times 10^{-4} ) c. ( 5.0 times 10^{-4} ) D. ( 4.0 times 10^{-5} ) |
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2 | One litre hard water contains ( 1 mathrm{mg} ) ( mathrm{CaCl}_{2} ) and ( 1 mathrm{mg} M mathrm{g} S mathrm{O}_{4} ). The hardness of water is: A . 1.743 ppm в. 1.745 ppm c. 1.734 ppm D. none of the above |
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3 | 2.51 Assertion (A) Molarity of a solution in liquid state changes with temperature. Reason (R) The volume of a solution changes with change in temperature. |
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4 | ( X, Y ) and ( Z ) in the given graph are? ( mathbf{x}_{2}=(mathbf{Y}) quad ) Mole fraction ( longrightarrow quad mathbf{y}_{2}=(mathbf{Z}) ) A. ( X=p_{1}+p_{2}, Y=1, Z=0 ) B . ( X=p_{1}+p_{2}, Y=0, Z=0 ) C ( cdot X=p_{1} times p_{2}, Y=0, Z=0 ) D. ( X=p_{1}-p_{2}, Y=1, Z=0 ) |
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5 | Among ( 0.1 ~ M ) solutions of ( N a C l, C a C l_{2} ) and ( A l_{2}(S O)_{3}, ) the one with highest vapour pressure is: A ( . N a C l ) в. ( C a C l_{2} ) c. ( A l_{2}(S O)_{3} ) D. All have equal vapour pressure |
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6 | Vapour pressure of water at certain temperature is ( 155 mathrm{mm} ) Hg and that of the another solvent ‘X’ is ‘p’ mm Hg. Molecular weight of ‘X’ is 128. An aqueous solution of ‘X'(64% by wt) has a vapour pressure of ( 145 mathrm{mm} ) Hg. What is ‘p’? |
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7 | Given below are few mixtures formed by mixing two components. Which of the following binary mixtures will have same composition in liquid and vapour phase? (i) Ethanol ( + ) Chloroform (ii) Nitric acid + Water (iii) Benzene + Toluene (iv) Ethyl chloride ( + ) Ethyl bromide A. (i) and (iii) B. (i) and (ii) c. (i), (ii) and (iii) D. (iii) and (iv) |
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8 | What is the molality of a solution containing ( 200 m g ) of urea (molar mass ( 60 g m o l^{-1} ) ) dissolved in ( 40 g ) of water? A . 0.0833 B. 0.825 c. 0.498 D. 0.0013 |
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9 | A mixture of volatile components ( A ) and B has total vapour pressure (in torr) as ( boldsymbol{P}=mathbf{2 5 4}-mathbf{1 1 9} chi_{A}, ) where ( chi_{A} ) is the mole fraction of ( A ) in the mixture. Hence, ( P_{A}^{o} ) and ( P_{B}^{o} ) respectively are (in torr): A. 254,119 в. 119,254 C. 135,254 D. 154, 119 |
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10 | State True or False. Lowering of vapour pressure is proportional to the mole fraction of the solute. A. True B. False |
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11 | Two liquids ( A ) and ( B ) form type II non ideal solution which shows a minimum in its temperature-mole fraction plot ( T-chi text { diagram }) . ) Can the two liquids be completely separated by fractional distillation? |
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12 | Q. 6 If the concentration of glucose (CGH206) in blood is 0.9 g L”, what will be the molarity of glucose in blood? (a) 5M (b) 50 M (c) 0.005 M (d) 0.5 M |
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13 | Van’t Hoff factor for ( boldsymbol{T} boldsymbol{H}left(boldsymbol{N} boldsymbol{O}_{3}right)_{4} ) in an aqueous solution is : |
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14 | Illustration 2.66 Can we separate the components of azeotropic mixture by distillation? |
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15 | Does a new substance form when a solute dissolves in a solvent? |
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16 | Which of the following conditions are correct for real solutions showing negative deviation from Raoult’s law? A ( cdot Delta H_{M i x}0 ) B. ( Delta H_{M i x}>0 ; Delta V_{M i x}>0 ) c. ( Delta H_{M i x}>0 ; Delta V_{M i x}<0 ) D. ( Delta H_{M i x}<0 ; Delta V_{M i x}<0 ) |
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17 | An ideal aqueous solution containing liquid ( boldsymbol{A}(M cdot W boldsymbol{t}=mathbf{1 2 8}) mathbf{6 4 %} ) by weight has a vapour pressure of ( 145 m m H g ). If the vapour pressure of ( boldsymbol{A} ) is ( boldsymbol{x} ) mm of ( H g ) and that of water is ( 155 m m H g ) at the same temperature. Then find ( frac{x}{5} . ) The solutions is ideal. |
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18 | When mercuric iodide is added to an aqueous solution of ( K I ) then: A. boiling point increase B. boiling point decrease c. freezing point increase D. osmotic pressure increase |
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19 | The vapour pressure of solution at 293 ( mathrm{K} ) A .0 .0229 B. 0.4 ( c .0 .6 ) D. 0.9 |
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20 | ( 0.124 g m ) of an organic compound containing phosphorus gave ( 0.222 g m ) of ( M g_{2} P_{2} O_{7} ) the usual analysis. Calculate the percentage of phosphorous in the compound. ( (M g= ) ( mathbf{2 4}, boldsymbol{P}=mathbf{3 1}) ) A .25 в. 15 ( c .62 ) D. 50 |
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21 | When a solution is diluted at constant temperature, its vapour pressure: A. increases B. decreases c. remains same D. may increase or decrease |
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22 | At ( 100^{circ} mathrm{C} ), benzene ( & ) toluene have vapour pressure of ( 1375 & 558 ) Torr respectively. Assuming these two form an ideal binary solution, calculate the composition of Ithe solution that boils at 1 atm ( & 100^{circ} mathrm{C} ). What is the composition of vapour issuing at these conditions? A . ( x_{b}=0.2472, Y_{b}=0.4473 ) B. ( x_{b}=0.4473, Y_{b}=0.2472 ) c. ( x_{b}=0.362, Y_{b}=0.321 ) D. None of these |
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23 | Calculate the mole fraction of glucose in an aqueous solution that contains 45 g of glucose in 45 g of water. Find out the weight of NaOH required to be disolved in 90 g of water in order to get a solution of the same mole fraction. A ( cdot frac{1}{11}, 20 g ) в. ( frac{1}{11}, 10 g ) c. ( frac{1}{10}, 10 g ) D. ( frac{1}{10}, 20 g ) |
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24 | is measured in moles per litre. A. Molality B. Molar concentration c. Number of moles D. None of these |
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25 | Q. 30 van’t Hoff factor (i) is given by the expression (a) – normal molar mass (b); – abnormal molar mass abnormal molar mass normal molar mass observed colligative property (d) i = calculated colligative property calculated colligative property observed colligative property (C)= |
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26 | Illustration 2.200 To 250 mL of water, x g of acetic acid is added. If 11.5% of acetic acid is dissociated, the depression in freezing point comes out 0.416. What will be the value of x if K. (water) = 1.86 K kg- mol-1 and density of water is 0.997 g mL-1 |
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27 | has the highest boiling point. A. ( 0.2 mathrm{m} mathrm{CaCl}_{2} ) B. 0.2 ( mathrm{m} ) NaCl c. ( 0.1 mathrm{m} ) Al ( C l_{3} ) D. ( 0.2 mathrm{m} mathrm{CH}_{3} mathrm{OH} ) E. ( 0.2 mathrm{m} mathrm{NaC}_{2} mathrm{H}_{3} mathrm{O}_{2} ) |
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28 | Write the formula to calculate the molality. |
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29 | Which of the following solution in water will have the lowest vapour pressure? A. ( 0.1 M, ) NaCI B. ( 0.1 M, ) Sucrose с. ( 0.1 M, )ВаС( I_{2} ) D. ( 0.1 M N a_{3} P O_{4} ) |
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30 | The van’t Hoff factor of ( 0.005 M ) aqueous solution of ( K C l ) is ( 1.95 . ) The degree of ionisation of ( K C l ) is: A . 0.95 В. 0.97 ( c .0 .94 ) D. 0.96 |
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31 | The Henry’s law constant for the solubility of ( mathbf{N}_{2} ) gas in water at ( mathbf{2 9 8 K} ) is ( 1.0 times 10^{5} ) atm. The mole fraction of ( mathbf{N}_{2} ) in air is ( 0.8 . ) The number of moles of ( mathbf{N}_{2} ) from air dissolved in 10 moles of water at ( 298 mathrm{K} ) and 5 atm pressure is: A ( cdot 4.0 times 10^{-4} ) В. ( 4.0 times 10^{-5} ) c. ( 5.0 times 10^{-4} ) D. ( 4.0 times 10^{-6} ) |
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32 | Question 1. Calculate the mass percentage of benzene (CH) and carbon tetrachloride (CC14) if 22 g of benzene is dissolved in 122 g carbon tetrachloride. (0) We have mass of CH6 and CCIA, so calculate the mass of solution by adding these two. (ii) Then, calculate the mass percentage from the formula, Mass of one component 100 Mass %= Mass of solution |
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33 | The density of ( 3 M ) solution of sodium thiosulphate ( left(N a_{2} S_{2} O_{3}right) ) is ( 1.56 g / m L ) Calculate (i) amount of ( N a_{2} S_{2} O_{3} ) in ( % ) w/w (ii) mole fraction of ( N a_{2} S_{2} O_{3} ) (iii) Molality of ( N a^{+} ) and ( S_{2} O_{3}^{2-} ) ions |
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34 | Mustration 2.104 Define molal depression constant or cryoscopic constant. |
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35 | For dilute solution, Raoult’s law states that: A. the relative lowering of vapour pressure is equal to mole fraction of solute B. the vapor pressure of the solution is equal to mole fraction of the solvent C. the relative lowering of vapour pressure is proportional to amount of solute D. the lowering of vapor pressure is equal to the mole fraction of solute in solution |
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36 | A sample of ( boldsymbol{H}_{2} boldsymbol{O}_{2} ) solution labelled as 28 volume has density of 265 g/L. Mark the correct option(s) representing concentration of same solution in other units. This question has multiple correct options A. Molarity of ( H_{2} O_{2}=2.5 ) B. Percentage ( w / v=17 ) C. Mole fraction of ( H_{2} O_{2}=0.2 ) D. Molality of ( H_{2} O_{2}=13.88 ) |
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37 | Distinguish between the saturated and unsaturated solution using the data given below: a) 16 g ( N a C l ) in 100 g water. b) 36 g ( N a C l ) in 100 g water (Note – Solubility of ( N a C l ) is ( 36 g ) ) |
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38 | 7. Increasing amount of solid Hgl, is added to 1 L of an aqueous solution containing 0.1 mol KI. Which of the following graphs do represent the variation of freezing point of the resulting with the amount of Hgl, added? a. If b. If 0.05 0.10 Mol of Hgl2 → 0.05 0.10 Mol of Hgl2 → c. Te d. Tf 0.05 0.10 Mol of Hgl2 –> 0.05 0.10 Mol of Hgl2 -> |
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39 | Raoult’s law is obeyed by each constituent of a binary liquid solution when: A. the forces of attractions between like molecules are greater than those between unlike molecules B. the forces of attractions between like molecules are smaller than those between unlike molecules C. the forces of attractions between like molecules are identical with those between unlike molecules D. the volume occupied by unlike molecules are different |
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40 | A plant cell shrinks when it is kept in a? A. hypotonic solution B. hypertonic solution C. isotonic solution D. pure water |
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41 | Which of the following solutions shows positive deviation from Raoult’s law? A. Acetone + Aniline B. Acetone + Ethanol c. water + Nitric acid D. Chloroform + Benzene |
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42 | How many grams of sucrose must be added to ( 320 g ) of water to lower the vapour pressure by ( 1.5 m m H g ) at ( 25^{circ} C ) ( ? ) (Given: The vapour pressure of water at ( 25^{circ} mathrm{C} ) is ( 23.8 mathrm{mm} ) Hg and molar mass of sucrose is ( 324.3 g / m o l ) ) A. ( 21.5 g ) в. ( 140 g ) c. ( 363.36 g ) D. ( 160.12 g ) |
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43 | Which of the following aqueous solutions will have maximum freezing point. [Assume dilute solutions] A. ( C_{6} H_{5} N H_{3} C I ) solution having ( 0.01 m ) B. ( C aleft(N O_{3}right)_{2} ) solution having ( 0.005 m ) C. ( A Ileft(N O_{3}right)_{3} ) solution having ( 0.004 m ) D. Glucose solution having ( 0.04 mathrm{m} ) |
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44 | The freezing point of mercury is: ( A cdot 100 K ) в. 234.3 к c. ( 123.5 mathrm{k} ) D. 450 K |
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45 | On increase of temperature, a saturated solution converts into solution. |
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46 | Assertion Aquatic species are more comfortable in warm waters than cold waters. Reason ( boldsymbol{K}_{boldsymbol{H}} ) values for both ( boldsymbol{N}_{2} ) and ( boldsymbol{O}_{2} ) decrease with increase of temperature. A. Both Assertion and Reason are correct and Reason is the correct explanation for Assertion B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion c. Assertion is correct but Reason is incorrect D. Both Assertion and Reason are incorrect |
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47 | The fundamental cause of all colligative properties is: A. higher entropy of the solution relative to that of pure solvent B. lower entropy of the solution relative to that of pure solvent c. higher enthalpy of the solution relative to that of pure solvent D. lower enthalpy of the solution relative to that of pure solvent |
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48 | The vapour pressure of two liquids ‘P and ‘Q’ are 80 and 60 torr, respectively. The total vapour pressure of solution obtained by mixing 3 mole of ( P ) and 2 mole of Q would be: A. 68 torr B. 140 torr c. 72 torr D. 20 torr |
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49 | Q. 6 Low concentration of oxygen in the blood and tissues of people living at high altitude is due to ….. (a) low temperature (b) low atmospheric pressure (c) high atmospheric pressure (d) Both low temperature and high atmospheric pressure f lo linat high altitudin |
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50 | Illustration 2.134 Given that the latent heat of fusion of naphthalene is 19.0 kJ mol-1 and its melting point is 80.2°C. Estimate the solubility of naphthalene in benzene at 76.2°C. |
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51 | Van’t Hoff factor of ( boldsymbol{H} boldsymbol{g}_{2} boldsymbol{C l}_{2} ) in its aqueous solution will be ( left(H g_{2} C l_{2} ) is right. ( 80 % ) ionized in the solution): A . 1.6 B . 2. ( c .3 .6 ) D. 4.6 |
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52 | Hlustration 2.91 12.2 g of benzoic acid is dissolved in (i) 1 kg acetone (K6 = 1.9 K kg mol-1) and (ii) 1 kg benzene (K) = 2.6 K kg mol-1). The elevations of boiling points are 0.19°C and 0.13°C, respectively. a. What are the molar masses of benzoic acid in the two solutions? b. What are the structures of benzoic acid in the two solutions? |
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53 | Illustration 2.160 The osmotic pressure of decimolar solution of urea at 27°C is a. 2.49 bar b. 5 bar c. 3.4 bar d. 1.25 bar |
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54 | The ammonia evolved from the treatment of ( 0.30 g ) of an organic compound for the estimation of nitrogen was passed in 100 m ( L ) of 0.1 ( M ) sulphuric acid. The excess of acid required ( 20 m L ) of 0.5 sodium hydroxide solution hydroxide solution for complete neutralization. The organic compound is: A. acetamide B. thiourea c. urea D. benzamide |
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55 | I. A ( 2 M ) solution of urea ( left(C H_{4} N_{2} Oright) ) can be prepared by dissolving 1 mole of urea in ( 500 m L ) of water. II. Urea is a non-polar molecular compound A. Statement ( I ) is true, Statement ( I I ) is true B. Statement I is true, Statement II is false c. statement ( I ) is false, statement ( I I ) is true D. Statement I is false, Statement II is false |
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56 | The vapour pressure of a mixture of diethyl aniline and water is ( 1.013 times ) ( 10^{5} N m^{-2} ) at ( 99.4^{circ} C . ) The vapour pressure of water at this temperature is ( 0.992 times 10^{5} N m^{-2} . ) The grams of steam are necessary to distill over 100 g of diethylaniline are (write answer as nearest integer after dividing by 60 ). |
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57 | On diluting solution, its normality and molarity changes but molality remains constant. A. True B. False |
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58 | 8. The vapour pressure of pure benzene C H at 50°C is 268 torr. How many moles of non-volatile solute per mole of benzene are required to prepare a solution of benzene having a vapour pressure of 167 torr at 50°C? a. 0.377 b. 0.605 c. 0.623 d. 0.395 |
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59 | Density of ( 2.03 M ) aqueous solution of acetic acid is ( 1.017 g m L^{-1} ) molecular mass of acetic is ( 60 . ) Calculate the molality of the solution. A . 2.27 B. 1.27 c. 3.27 D. 4.27 |
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60 | If the Vant Hoff factor for ( mathbf{0 . 1} mathbf{M} ) ( B aleft(N O_{3}right)_{2} ) solution is 2.74 , the degree of dissociation is: A . 0.87 в. 0.74 c. 0.91 D. 87 |
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61 | Q. 8 Colligative properties depend on …….. (a) the nature of the solute particles dissolved in solution (b) the number of solute particles in solution (C) the physical properties of the solute particles dissolved in solution (d) the nature of solvent particles |
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62 | toppr Q Type your question Assurite muldy unly A 2 anu ( cup cup 2 ) art present ( A ) B. ( c ) ( D ) |
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63 | At ( 300 mathrm{K}, 36 mathrm{g} ) of glucose present per litre in its solution has an osmotic pressure of 4.98 bar. If the osmotic pressure of the solution is 1.58 bar at the same temperature, what would be its concentration? |
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64 | A solution is made by dissolving 49 g of ( H_{2} S O_{4} ) in ( 250 mathrm{mL} ) of water. The molarity of solution prepared is: ( A cdot 2 M ) в. 1 ( c cdot 4 M ) D. 5 M |
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65 | The Henry’s law constant for the solubility of ( N_{2} ) gas in water at ( 298 K ) is ( 1 times 10^{5} ) atm. The mole fraction of ( N_{2} ) in air is ( 0.8 . ) Calculate the number of moles of ( N_{2} ) dissolved in 10 moles of water at ( 298 K ) and 5 atm. A ( cdot 5 times 10^{-4} ) В. ( 3 times 10^{-5} ) c. ( 4 times 10^{-4} ) D. ( 4 times 10^{-5} ) |
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66 | Mustration 2.51 Why is an increase in temperature observed on mixing chloroform with acetone? |
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67 | If the molar concentration of ( boldsymbol{P b I}_{2} ) is ( 1.5 times 10^{-3} ) mol ( L^{-1}, ) then the concentration of iodide ions of ( g ) ion ( L^{-1} ) is ? A. ( 3.0 times 10^{-3} ) В. ( 6.0 times 10^{-3} ) c. ( 0.3 times 10^{-3} ) D. ( 0.6 times 10^{-6} ) |
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68 | Ways of expressing the concentration of a solution are: ( frac{text {Mass of solute}}{text {Mass of solution}} times 100 ) II) ( frac{text { Mass of solute }}{text {Volume of solution}} times 100 ) ( A ) B. I ( c cdot 1,1 ) D. none of the above |
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69 | ( 20 mathrm{ml} ) of ( 0.2 mathrm{M} A l_{2}left(S O_{4}right)_{3} ) is mixed with ( 20 mathrm{ml} ) of ( 6.6 mathrm{M} mathrm{BaCl}_{2} ), the concentration of ( C l^{-} ) in solution is: A. ( 0.2 mathrm{M} ) B. 6.6 ( M ) c. ( 0.02 mathrm{M} ) D. 0.06 м |
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70 | Which of the following aqueous solutions will exhibit the highest boiling point? A . ( 0.01 M ) urea в. ( 0.01 M ) К ( N O_{3} ) c. ( 0.01 M ) Na( _{2} ) SO ( _{4} ), D. ( 0.015 M C_{6} H_{12} O_{6} ) |
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71 | Which of the following units can be used to represent solubility? ( mathbf{A} cdot mathbf{g} ) B. mol c. ( m o l / L ) ( mathbf{D} cdot m L / s ) |
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72 | Two liquids ( X ) and ( Y ) from an ideal solution. At ( 300 K, ) a vapour pressure of the solution containing 1 mol of ( X ) and 3 mol of ( Y ) is 550 mm ( H g . ) At the same temperature, if 1 mol of ( Y ) is further added to this solution, a vapour pressure of the solution increased by 10 mm Hg. Vapour pressure ( in mmHg) of ( X ) and ( Y ) in their pure states will be respectively: A. 300 and 400 B. 400 and 600 c. 500 and 600 D. 200 and 300 |
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73 | Which substance has a higher solubility in cold water and a lower solubility in hot water? A. Licl ( mathbf{B} cdot C a(O H)_{2} ) ( c cdot C O_{2} ) D. ( C_{6} H_{12} O_{6} ) |
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74 | A solution containing ( 30 g ) of a nonvolatile solute in exactly ( 90 g ) water has a vapour pressure of 21.85 mm ( H g ) at ( 25^{circ} mathrm{C} . ) Further 18 gm of water is then added to the solution. The resulting solution has a vapour pressure of 22.18 ( mathrm{mmHg} ) at ( 25^{circ} mathrm{C} ). Calculate (a) molar mass of the solute, and (b) vapour pressure of water at ( 25^{circ} mathrm{C} ) В. ( (a) 61.21 g ) тод( ^{-1} ), (b) 23.99 ( mathrm{mm} ) Н ( g ) ( (b) 28.87 mathrm{mm} mathrm{Hg} ) D. ( (a) 84.87 g ) mol ( ^{-1} ), |
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75 | Example 2.8 Two liquids A and B form an idea solution. What will be the vapour pressure at 27°C of a solution having 1.5 mol of A and 4.5 mol of B? The vapour pressure of A and B at 27°C is 0.116 atm and 0.140 atm, respectively. |
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76 | A Mixture of nitrogen and oxygen has a density of ( 1.00 g / 1 ) and the average molecular weight ( left(M_{a y}right) ) of ( 31.2 g ) at ( 27^{circ} C ) and ( 600 mathrm{mm} ) Hg per mole pressure What is the mole fraction of nitrogen? (Assume ideal gas behavior) A . 0.8 B. 0.6 ( c .0 .4 ) D. 0.2 |
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77 | Determine the osmotic pressure of a solution prepared by dissolving ( 2.5 times ) ( 10^{-2} g ) of ( K_{2} S O_{4} ) in ( 2 L ) of water at 25 assuming that it is completely dissociated ( left(R=0.0821 L operatorname{atm} K^{-1} m o l^{-1}, ) Molar right. ( operatorname{mass} ) of ( K_{2} S O_{4}=174 mathrm{g} m o l^{-1} ) ). |
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78 | By dissolving 13.6 g of a substance in 20 ( g ) of water, the freezing point decreased by ( 3.7^{circ} mathrm{C} ). Calculate the molecular mass of the substance. (Molal depression constant for water = ( 1.863 mathrm{K} mathrm{kg} mathrm{mol}^{-1} ) ) |
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79 | The equation of the curve obtained by connecting all those points where the vapors of above mixture (all mixtures of different composition are taken) just start forming will be A ( cdot P=P_{C}^{o}+left(P_{B}^{o}-P_{C}^{o}right) X_{B}^{l} ) B . ( P=P_{B}^{o}+left(P_{B}^{o}-P_{C}^{o}right) X_{B}^{l} ) ( ^{mathrm{c}} cdot p=frac{P_{B}^{o} P_{C}^{o}}{X_{B}^{o}left(P_{C}^{o}-P_{B}^{o}right)+P_{B}^{o}} ) D. ( P=frac{P_{B}^{o} P_{C}^{o}}{X_{B}^{l}left(P_{C}^{o}-P_{B}^{o}right)+P_{B}^{o}} ) |
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80 | A sample of drinking was found to be severely contaminated with chloroform, ( C H C l_{3}, ) supposed to be a carcinogen The level of contamination was 15 ppm (by mass). Express this in percent by mass. A. ( 1.5 times 10^{-3} ) В. ( 4.0 times 10^{-3} ) c. ( 6 times 10^{-3} ) D. ( 0.75 times 10^{-3} ) |
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81 | The solution showing positive deviation from ideal behaviour has azeotrope. A. negative B. positive c. neutral D. ideal |
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82 | State true or false. 1 ppm is equal to 1 mg per ( mathrm{kg} ) A. True B. False |
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83 | Define an ideal solution | 12 |

84 | The experiment value for the molar mass of a non-volatile solute is twice the theoretic value. What is Vant Hoff factor for the solute? |
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85 | Vapour Pressure of a mixture of benzene and toluene is given by ( boldsymbol{P}= ) ( mathbf{1 7 9 X}_{B}+mathbf{9 2}, ) Where ( boldsymbol{X}_{B} ) is mole fraction of benzene. If Vapours are removed and condensed in to liquid then what will be the ratio of mole fraction of benzene and toluene in first condensate: A . 2.8 B. 1.5 c. 3. D. 4.5 |
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86 | A gas mixture contains ( 24 % ) nitrogen, ( 32 % ) oxygen and remaining is hydrogen by volumes at a given temperature and pressure then what is the mole fraction of hydrogen? (assume there is no reaction between the gases) A .0 .44 B. 0.24 c. 0.91 D. 0.56 |
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87 | How many ( N a^{+} ) ions are present in ( 100 m L ) of ( 0.25 M ) of ( N a C l ) solution? A. ( 0.25 times 10^{23} ) В. ( 1.505 times 10^{22} ) C. ( 15 times 10^{22} ) D. ( 2.5 times 10^{23} ) |
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88 | The vapour pressure of water at ( 20^{circ} mathrm{C} ) is 17.54 ( m m H g ). Then the vapour pressure of the water in the apparatus is lowered, decreasing the volume of the gas above the liquid to one half of its initia volume (temp. constant) is: A. ( 5.77 mathrm{mmHg} ) в. ( 16 mathrm{mmHg} ) c. 35.08 mmHg D. between 8.77 and ( 15.54 mathrm{mmHg} ) |
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89 | Equal weights of mercury and ( l_{2} ) are allowed to react completely to form a mixture of mercurous and mercuric iodide leaving none of the reactants. Calculate the ratio of the weights of ( H g_{2} l_{2} ) and ( H g l_{2} ) formed A . 1: 0653 B . 0.732: 1 c. 1: 0.523 D. 0.532: 1 |
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90 | The quantity of solute dissolved in a given mass or volume of the solution is called: A. parameter of solution B. concentration of solution c. similarity of solution D. massive mass |
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91 | At a particular temperature, the vapour pressures of two liquids ( A ) and ( B ) are respectively 120 and 180 mm of mercury. If 2 moles of ( A ) and 3 moles of Bare mixed to form an ideal solution, the vapour pressure of the solution at the same temperature will be (in mm of mercury) : A . 156 в. 145 ( c .150 ) D. 108 |
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92 | Example 2.12 A solution containing 25.6 g of sulphur, dissolved in 1000 g of naphthalene whose melting point is 80.1°C gave a freezing point lowering of 0.680°C. Calculate the formula of sulphur (K, for naphthalene = 6.8 Km). |
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93 | ( 0.2 mathrm{L} ) of aqueous solution of a protein contains ( 1.26 mathrm{g} ) of the protein. The osmotic pressure of such a solution at ( 300 mathrm{K} ) is found to be ( 2.57 times 10^{-3} ) bar. Calculate the molar mass of the protein. ( left(boldsymbol{R}=mathbf{0 . 0 8 3} boldsymbol{L} text { bar } boldsymbol{m o l}^{-1} boldsymbol{K}^{-1}right) ) |
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94 | 7. The concentration of fluoride, lead, nitrate and iron in a water sample from an underground lake was found to be 1000 ppb, 40 ppb, 100 ppm and 0.2 ppm, respectively. This water is unsuitable for drinking due to high concentration of: (JEE Main 2016) (a) Iron (b) Fluoride (c) Lead (d) Nitrate |
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95 | Azeotropic mixtures can be seperated by distillation of solution. If true enter 1 , else enter 0 . | 12 |

96 | DHOKALA is a ( ——— ) type of solution. A. solid-in-solid B. solid-in-gas c. solid-in-liquid D. gas-in-solid |
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97 | ( 10^{24} ) molecules of solute are dissolved in ( 10^{25} ) molecules of solvent, the mole fraction of solute in solution is : A . 0.09 B. 0.08 c. 0.07 D. 0.9 |
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98 | Illustration 2.99 Molal elevation constant (K) values of following alcohols are in the order: CH,CH,CH,CH,OH>(CH3),CH-CH,OH>(CH3),C-OH Explain in brief. |
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99 | Calculate the molarity and molality of ( 20 % ) aqueous ethanol ( left(C_{2} H_{5} O Hright) ) solution by volume. (Density of solution ( =0.96 mathrm{g} / mathrm{mL}) ) A. Molarity ( =3.48 ), Molality ( =4.35 ) B. Molarity = 4.35, Molality = 3.48 C. Molarity ( =4.48 ), Molality ( =3.35 ) D. None of the above |
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100 | In an experiment, 18.0 g of mannitol was dissolved in 100 g of water. The vapour pressure of solution at ( 20^{circ} mathrm{C} ) was 17.226 mm of mercury. Calculate the molecular mass of mannitol. The vapour pressure of water at ( 20^{circ} mathrm{C} ) is ( 17.535 mathrm{mm} ) of mercury. A. Molecular mass of mannitol = 171.02 B. Molecular mass of mannitol = 181.02 c. Molecular mass of mannitol = 161.02 D. Molecular mass of mannitol = 121.02 |
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101 | When a gas is bubbled through water at ( 298 K, ) a very dilute solution of gas is obtained. Henry’s law constant for the gas is ( 100 k ) bar. If gas exerts a pressure of 1 bar, number of moles of gas dissolved in 1 litre of water is : A. 0.555 В. ( 55.55 times 10^{-5} ) c. ( 55.55 times 10^{-3} ) D. ( 5.55 times 10^{-5} ) |
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102 | Pure water can be obtained from sea water by: A . centrifugation B. plasmolysis c. reverse osmosis D. sedimentation |
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103 | How solubility of a gas in liquid varies with i) Temperature ii) pressure? | 12 |

104 | Q. 18 The value of Henry’s constant, KH 1S….. (a) greater for gases with higher solubility (b) greater for gases with lower solubility (c) constant for all gases (d) not related to the solubility of gases |
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105 | Calculate the freezing point of a solution containing ( 60 g ) of glucose (Molar mass ( =180 g ) mol ( ^{-1} ) ) in ( 250 g ) of water ( left(K f text { of water }=1.86 K k g m o l^{-1}right) ) |
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106 | The ( boldsymbol{K}_{s p}left(mathbf{2 5}^{o} boldsymbol{C}right) ) of sparingly salt [ boldsymbol{X} boldsymbol{Y}_{2}(boldsymbol{s}) text { is } boldsymbol{3} . mathbf{5 6} times mathbf{1 0}^{-5}left(boldsymbol{m o l} quad boldsymbol{L}^{-1}right)^{3} ] and at ( 30^{circ} mathrm{C} ),the vapour pressure of its saturated solution in water is ( 31.78 mathrm{mm} ) of Hg.Calculate the enthalpy change of the reaction.( write your answer to nearest integer) [ boldsymbol{X} boldsymbol{Y}_{2}(boldsymbol{s}) rightleftharpoons boldsymbol{X}^{2+}(boldsymbol{a} boldsymbol{q})+boldsymbol{2} boldsymbol{Y}^{ominus}(boldsymbol{a} boldsymbol{q}) ] Given : Vapour pressure of pure water ( =31.82 mathrm{mm} ) of ( mathrm{Hg} ) |
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107 | Benzene and naphthalene form an ideal solution at room temperature. For this process, the true statement(s) is(are): This question has multiple correct options A. ( Delta G ) is positive B . ( Delta S_{text {system}} ) is positive C. ( Delta S_{text {surroundings}}=0 ) D. ( Delta H=0 ) |
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108 | A solution containing 4 g of a nonvolatile organic solute per ( 100 mathrm{mL} ) was found to have an osmotic pressure equal to ( 500 mathrm{cm} ) of mercury at ( 27^{circ} mathrm{C.The} ) molecular weight of solute is: A . 14.97 B. 149.7 c. 1697 D. 1.497 |
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109 | Assertion When methanol is added to water, boiling point of water increases. Reason When a volatile solute is added to a volatile solvent, elevation in boiling point is observed. A. Both Assertion and Reason are correct and Reason is the correct explanation for Assertion B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion c. Assertion is correct but Reason is incorrect D. Both Assertion and Reason are incorrect |
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110 | The density of a ( 3 mathrm{M} ) solution of NaCl is 1.25g/ml. Calculate the molality of the solution. | 12 |

111 | Sugar and Salt solutions a re |
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112 | Units of parts per million (ppm) or parts per billion (ppb) are often used to describe the concentrations of solutes in very dilute solutions. The units are defined as the number of grams of solute per million or per billion grams of solvent. Bay of Bengal has 1.89 ppm of lithium ions. The molality of ( L i^{+} ) in this water is (atomic number of ( L ) i ( =7 ) ): A ( cdot 1.5 times 10^{-4} m ) В. ( 1.7 times 10^{-4} mathrm{m} ) c. ( 2.5 times 10^{-4} m ) D. ( 2.7 times 10^{-4} m ) |
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113 | ( 520 mathrm{gm} ) mixture of ( F e_{2} O_{3} ) and ( mathrm{Fe} 0 ) reacts completely with 158 gm ( K M n O_{4} ) in acidic medium. Calculate the mole ( % ) of ( F e_{2} O_{3} ) in mixture |
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114 | A solution of glucose ( left(mathbf{C}_{6} mathbf{H}_{mathbf{1 2}} mathbf{O}_{mathbf{6}}right) ) in water is labelled as ( 10 % ) by weight. What would be the molality of the solution? (Molar mass of glucose ( =180 mathrm{g} mathrm{mol}^{-1} ) ) A. 0.4 B. 0.6 ( c .0 . ) D. 0.5 |
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115 | A ( 5 % ) solution of cane sugar is isotonic with ( 0.877 % ) solution of ( X . ) Calculate the molecular mass of ( X ), if the molecular mass of cane sugar is 342 g/mol. A ( .60 mathrm{g} / mathrm{mol} ) B. ( 120 mathrm{g} / mathrm{mol} ) c. 78 g/mol D. 30 g/mol |
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116 | Illustration 2.135 If a solution containing 6 g of triphenyl methane, (C H2) CH (molecular weight = 244), in 1000 g of benzene is cooled to 0.22°C below the freezing point of benzene, how much solvent will crystallize out and what will be the molality of residual solution? (K. = 5.1 K m-1) |
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117 | A true solution (or simply a solution) is a homogeneous mixture, in which the solute and solvent molecules cannot be distinguished even under a microscope. A. True B. False |
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118 | Example 2.24 A 0.1 M solution of glucose (molecular weight 180 g mol-l) and a 0.1 M solution of urea (molecular weight = 60 g mol-l) are placed on the two sides of a semi-permeable membrane to equal heights. In this context, which of the following statements is correct? a. Glucose will flow across the membrane into the urea solution. b. Urea will flow across the membrane into the glucose solution. c. Water will flow across the membrane from the urea solution into the glucose solution. d. There will be no net movement across the membrane. sol |
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119 | ( 0.4 g ) of ( mathrm{NaOH} ) is present in one litre of the solution shows that ( boldsymbol{H}^{+} ) concentration of the solution is? |
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120 | Illustration 2.71 Calculate the vapour pressure of an aqueous solution of 1.0 molal glucose solution at 100°C. |
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121 | Question 22. At 300 K, 36 g of glucose present in a litre of its solution has an osmotic pressure of 4.98 bar. If the osmotic pressure of the solution is 1.52 bar at the same temperature, what would be its concentration? We Apply a = CRT and C – V MB XV |
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122 | Five hundred milliliters of solution of 0.1 M Na Br has how many milligrams of bromine? A. 200 ( mathrm{mg} ) B. 400 mg c. ( 2,000 mathrm{mg} ) D. ( 4,000 mathrm{mg} ) E. 20,000 ( mathrm{mg} ) |
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123 | Phenol associates in ( C_{6} H_{6} ) to double molecules. A solution of 2 g of phenol in 100 g ( C_{2} H_{6} ) has its f.pt. lowered by 0.72 K. ( boldsymbol{K}_{f} ) for ( boldsymbol{C}_{boldsymbol{6}} boldsymbol{H}_{boldsymbol{6}} ) is ( mathbf{5 . 1 2} boldsymbol{K} boldsymbol{m o l}^{-1} boldsymbol{k} boldsymbol{g} ) Percentage degree of association of phenol is (write the integer at tens place, e.g., if percentage degree of dissociation is ( x y % ) then answer would be ( x ) ) |
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124 | When ( 1.20 g ) of sulphur is melted with ( 15.00 g ) of naphthalene, the solution freezes at ( 77.2^{circ} mathrm{C} ).. What is the molar mass of this form of sulphur? Data for Naphthalene: Melting point, ( mathrm{M} . mathrm{P}=80^{circ} mathrm{C} ) Freezing point depression constant, ( k_{f}=6.80^{circ} mathrm{C} boldsymbol{m}^{-1} ) A . ( 180 g ) mol ( ^{-1} ) B. ( 194 g ) mol ( ^{-1} ) c. ( 260 g ) mol ( ^{-1} ) D. ( 450 mathrm{g} ) mol ( ^{-1} ) |
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125 | Molecules of ethanoic acid dimerises in benzene due to ( H- ) bonding if al molecules of ethanoic acid associated in benzene then: A. boiling boiling of ethanoic acid become half of norma value B. freezing point of ethanoic acid become twice of normal value c. molar mass become twice of normal value D. vapour pressure of solution decreases due to dimerisation |
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126 | The molality of an aqueous dilute solution containing non-volatile solute is 0.1 m. What is the boiling temperature (in ( ^{circ} boldsymbol{C} ) ) of solution? (Boiling point elevation constant, ( boldsymbol{K}_{boldsymbol{b}}= ) ( 0.52 k g m o l^{-1} K ; ) boiling temperature of water ( =100^{circ} mathrm{C} ) ) A. 100.0052 в. 100.052 c. 100.0 D. 100.52 |
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127 | Which of the following relation is not correctly matched with the formula? A ( cdot ln ) case of association, ( alpha=frac{i-1}{frac{1}{n}-1} ) B. ( _{text {In case of dissociation, } alpha}=frac{i-1}{n+1} ) ( i frac{n_{B}}{n_{A}+n_{B}} ) Devation in boiling point, ( Delta T=K_{b} times frac{W_{B} times 1000}{M_{B} times W_{A}} ) |
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128 | The molarity of ( C l^{-}(100 mathrm{ml}) ) ions in the solution after 0.2 moles ( H C l ) are mixed with 0.1 moles ( C a C l_{2} ) solution? A. 0.8 m B. 0.04 М ( c .0 .4 mathrm{M} ) D. 0.08 м |
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129 | Name the type of solution formed in the following cases: i) ( 20 g ) of ( N a C l ) in ( 100 g ) of water. ii) ( 36 g ) of ( N a C l ) in ( 100 g ) of water. iii) ( 45 g ) of ( N a C l ) in ( 100 g ) of water at ( 80^{circ} mathrm{C} ) iv) Sulphur dissolved in ( C S_{2} ) v) Nitrogen in soil |
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130 | Q Type your question Clapeyron equation describes this relationship. The Clausius-Clapeyron equation is : ( ln left(P_{v a p o u r}right)=-frac{Delta H_{v a p o u r}}{R}left[frac{1}{T}right]+C ) According to the graph, at high temperatures, which substance has the greatest vapour pressure? ( A cdot w ) B. ( x ) ( c ) ( D ) |
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131 | The boiling point of a solution of 5 g sulphur in 100 g ( C S_{2} ) is ( 0.5^{circ} C ) above pure solvent. If the ( K_{b} ) of ( C S_{2} ) is 2.56 ( mathrm{K} / mathrm{m}, ) then find the atomicity of the sulphur in the solvent. |
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132 | 1000 g aqueous solution of ( C a C O_{3} ) contains 10 g of calcium carbonate. ( mathbf{A} ) concentration of the solution is: A. 10 ppm B. 100 ppm c. 1000 ppm D. 10000 ppm |
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133 | A 3.4 g sample of ( H_{2} O_{2} ) solution containing ( boldsymbol{x} % boldsymbol{H}_{2} boldsymbol{O}_{2} ) by mass requires ( x ) mL of a ( K M n O_{4} ) solution for complete oixidation under acidic condition.The molarity of ( boldsymbol{K} boldsymbol{M} boldsymbol{n} boldsymbol{O}_{4} ) solution is: ( A ) B. 0.5 ( c cdot 0.4 ) D. 0.2 |
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134 | Water is added to the solution M such that the mole fraction of water in the solution becomes 0.9. The boiling point of this solution is : A . ( 380.4 mathrm{k} ) B . 376.35 К c. 375.5 к D. 354.7 к |
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135 | If 3.65 got ( mathrm{HCl} ) is dissolved in ( 16.2 mathrm{g} ) of water then the mole fraction of HCl in the resulting solution is: |
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136 | Which of the following pairs of solutions is isotonic? A. ( 6 % ) urea and ( 6 % ) glucose ( (w / v) ) B. ( 18 % ) urea and ( 18 % ) glucose ( (w / v) ) ( c .6 % ) urea and ( 18 % ) fructose ( (w / v) ) D. ( 34.2 % ) sucrose and ( 60 % ) glucose ( (w / v) ) |
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137 | Positive deviation from Raoult’s law is shown by which of the following mixtures? A. Benzene and toluene B. ( C H C l_{3} ) and acetone c. Ethanol and water D. ( H C l ) and water |
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138 | The ratio of the actual value of a colligative property to the value calculated, assuming the substance to be a nonelectrolyte, is referred to as A. Henry’s law B. vapor pressure lowering c. the van’t Hoff factor D. freezing point depression E . osmotic pressure |
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139 | ( 10^{-1} M ) HCl is diluted to 100 times. Its pHis: ( A cdot 3 ) B. 8 ( c cdot 6.98 ) D. 7.02 |
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140 | The total vapour pressure of a mixture of 1 mol ( Aleft(P_{A}^{O}=150 text { tor } rright) ) and 2 mol ( B ) ( left(P_{B}^{o}=240 text { tor } rright) ) is ( 200 mathrm{mm} . ) In this case: A. there is positive deviation from Raoult’s law B. there is negative deviation from Raoult’s law. c. there is no deviation from Raoult’s law D. molecular masses of A and B are also required. |
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141 | Illustration 2.86 Two liquids A and B boil at 130°C and 160°C, respectively. Which of the them has higher vapour pressure at 80°C. |
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142 | When no more of a solid can be dissolved in a solvent ,it is called: A. unsaturated solution B. colloidal solution c. saturated solution D. none of the above |
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143 | Mole fraction = A. ( frac{text { Number of moles of constituent }}{text { Number of moles of all constituents }} ) B. Number of molecule of constituent + Total number of moles of all constituents C. Both (A) and (B) above D. None of the above |
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144 | Illustration 2.112 The freezing point of a solution containing 50 cm of ethylene glycol in 50 g of water is found to be -34°C. Assuming ideal behaviour, calculate the density of ethylene glycol (K, for water = 1.86 K kg mol-!). |
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145 | ( 19.5 g ) of ( C H_{2} F C O O H ) is dissolved in ( mathbf{5 0 0} g ) of water. The depression in the freezing point of water observed is ( 1.00^{0} C . ) Calculate the van’t Hoff factor and dissociation constant of fluoroacetic acid. |
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146 | ( 18.0 g ) of ( operatorname{glucose}left(C_{6} H_{12} O_{6}right) ) is added to ( 178.2 g ) of water. The vapour pressure of water for this aqueous solution at ( 100^{circ} mathrm{C} ) is : A . ( 759 . .00 ) Torr B. 7.60 Torr c. 76.00 torr D. 752.40 Torr |
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147 | Assertion: A 1 m NaCl(aq) solution will freeze at a temperature below ( 273 K ) Reason: As a solute is added to a Solvent, the boiling point increases while the freezing point decreases. A. Both Assertion and Reason are true and Reason is the correct explanation of Assertion. B. Both Assertion and Reason are true but Reason is not the correct explanation of Assertion. C. Assertion is true but Reason is false. D. Assertion is false but Reason is true. E. Both Asssertion and Reason are false |
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148 | Colligative molality ( = ) molality ( times ) Van’t Hoff factor If true enter ( 1, ) if false enter 0 |
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149 | ( boldsymbol{P}_{boldsymbol{A}}=boldsymbol{X}_{boldsymbol{A}} boldsymbol{P}_{boldsymbol{A}} ) and ( boldsymbol{P}_{boldsymbol{B}}=boldsymbol{X}_{boldsymbol{B}} boldsymbol{P}_{boldsymbol{B}} ) ( boldsymbol{P}_{boldsymbol{T}}=boldsymbol{X}_{boldsymbol{A}} boldsymbol{P}_{boldsymbol{A}}+boldsymbol{X}_{boldsymbol{B}} boldsymbol{P}_{boldsymbol{B}_{boldsymbol{B}}} ) Vapour pressure of mixtures of Benzene ( left(C_{6} H_{6}right) ) and toluene ( left(C_{7} H_{8}right) ) at ( 50^{circ} C ) are given by ( boldsymbol{P}_{M}=mathbf{1 7 9} boldsymbol{X}_{boldsymbol{B}}+mathbf{9 2} ) where ( X_{B} ) is mole fraction of ( C_{6} H_{6} ) What is the vapour pressure of pure liquids? A ( cdot P_{B}=92 m m, P_{T}=179 m m ) B . ( P_{B}=271 mathrm{mm}, P_{T}=92 mathrm{mm} ) c. ( P_{B}=180 m m, P_{T}=91 m m ) D. None of these |
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150 | If the maximum concentration of ( boldsymbol{P b C l}_{2} ) in water is ( 0.01 M ) at ( 298 K ), Its maximum concentration in ( mathbf{0 . 1} boldsymbol{M} boldsymbol{N} boldsymbol{a} boldsymbol{C l} ) will be: A ( cdot 4 times 10^{-3} M ) В. ( 0.4 times 10^{-4} M ) ( mathbf{c} cdot 4 times 10^{-2} M ) D. ( 4 times 10^{-4} M ) |
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151 | The vapour pressure of a dilute aqueous solution of glucose is ( 750 mathrm{mm} ) Hg at ( mathbf{3 7 3} mathbf{K} ) Calculate (i) molality, (ii) mole fraction of the solute. в. 0.078,0.02 ( c .0 .0729,0.0187 ) 7 D. 0.0779,0.3 |
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152 | For an ideal binary solution ( (A) ) and ( (B) ) ( boldsymbol{y}_{A} ) is the mole fraction of ( boldsymbol{A} ) in vapor phase. Which of the following plot should be linear? A ( cdot P_{text {total }} ) vs ( y_{A} ) B. ( P_{text {total }} ) vs ( y_{B} ) ( ^{c} frac{1}{P_{text {total}}} ) vs ( y_{A} ) D. ( frac{1}{P_{text {total }}} ) vs ( y_{B}+y_{A} ) |
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153 | Mustration 2.101 Sodium chloride solution freezes at lower temperature than water but boils at higher temperature than water. Explain. |
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154 | To aqueous solution of Nal, increasing amounts of solid ( H g I_{2} ) is added. The vapor pressure of the solution- A. Decreases to a constant value. B. Increases to a constant value c. Increases first and then decreases. D. Remains constant because ( H g I_{2} ) is sparingly soluble in water. |
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155 | Density of ( H_{2} O ) is ( 1 g m L^{-1} . ) If we have ( 1 m L H_{2} O ) then: This question has multiple correct options A . It is 55.55 mol ( L^{-1} ) B . It has ( 3.33 times 10^{22} mathrm{H}_{2} mathrm{O} ) molecules c. It has ( 3.33 times 10^{22} ) H-atoms D. It has ( 6.66 times 10^{22} ) O-atoms |
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156 | The system that forms maximum boiling azeotrope is : A. acetone-chloroform B. ethanol- acetone C. n-hexane- n- heptane D. carbon disulphide – acetone |
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157 | A ( 10 % ) (mass/mass) solution of cane sugar undergoes partial conversion into glucose and fructose to show an inversion of cane sugar as: Sucrose( + )Water( rightarrow )Glucose( + ) Fructose The solution boils at ( 100.27^{circ} mathrm{C} ) at this state. What fraction of the sugar has inverted? ( left(text { Given } boldsymbol{K}_{boldsymbol{b}} text { for } boldsymbol{H}_{mathbf{2}} boldsymbol{O} ) is right. ( left.0.512 K m o l^{-1} k gright) ) Multiply answer with 10 and write the nearest integer value. |
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158 | A 0.5 molal solution of ethylene glycol in water is used as the coolant in a car. If the freezing point constant of water is ( 1.86 mathrm{K} . mathrm{kg} / mathrm{mol} ), the mixture will freeze at: ( mathbf{A} cdot 0.93^{0} C ) B. ( -0.93^{0} C ) c. ( 1.86^{0} C ) D. ( -1.86^{0} C ) |
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159 | Van’t Hoff factor is: A. more than one in case of association B. less than one in case of dissociation C. ( frac{text { normal molecular mass }}{text { observed molecular mass }} ) D. ( frac{text { observed molecular mass }}{text { normal molecular mass }} ) |
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160 | Q13. What is the effect of temperatures on the vapour pressure of a liquid? | 12 |

161 | Illustration 2.132 The freezing point of 0.02 mole fraction acetic acid in benzene is 277.4 K. Acetic acid exists partly as dimer. Calculate the equilibrium constant for dimerization. The freezing point of benzene is 278.4 K and the heat of fusion of benzene is 10.042 kJ mol-1. Assume molarity and molality same. |
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162 | containing 8.19g d from pure water Illustration 2.201 A 250-ml water solution containing of sodium chloride at 300 K is separated from pure by means of a semi-permeable membrane. The pressure must be applied above this solution in order to just prevent osmosis is (R = 0.0821 L atm moll K-1) a. 13.80 atm b. 27.58 atm c. 23.34 atm d. 9.80 atm |
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163 | The cryoscopic constant for acid is ( 3.6 mathrm{K} ) kg/mol. A solution of 1 g of a hydrocarbon in 100 g of acetic acid freezes at ( 16.60^{circ} mathrm{C} ). The hydrocarbon contains ( 92.3 % ) carbon.lf the molecular formula is ( C_{x} H_{y} ). Find the value of ( x ) and ( y: ) A. ( x=2, y=4 ) В. ( x=3, y=8 ) c. ( x=4, y=10 ) D. ( x=6, y=6 ) |
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164 | A mixture of 2 moles of ( N_{2} ) and 8 moles of ( H_{2} ) are heated in a 2 lit vessel, till equilibrium is established. At equilibrium 0.4 moles of ( N_{2} ) was present. What will be the equilibrium concentration of ( boldsymbol{H}_{2} ? ) ( A cdot 2 ) mole/lit B. 4 mole/lit c. 1.6 mole/lit D. 1 mole/lit |
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165 | Which of the following form is an ideal solution? This question has multiple correct options A. Ethyl bromide + Ethyl iodide B. Ethyl alcohol + Water c. chloroform + Benzene D. Benzene + Toluene |
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166 | In a saturated solution: A. dissolved solute ( >>> ) undissolved solute B. dissolved solute ( <<< ) undissolved solute C. dissolved solute and undissolved solutes are in equilibrium with each other D. none of the above |
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167 | How are 0.50 mol ( N a_{2} C O_{3} ) and ( 0.50 mathrm{M} ) ( N a_{2} C O_{3} ? ) |
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168 | Which of the following choices will favor the melting of ice in a closed container if all other parameters are kept constant? A. Adding water with a temperature of ( 0^{circ} mathrm{C} ) B. Lowering the temperature below ( 0^{circ} mathrm{C} ) c. Lowering the pressure D. Raising the pressure E. Decreasing the amount of ice |
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169 | Which of the following is a true solution? A. Copper in gold B. Sulphur in water c. мilk D. water in sulphur dioxide |
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170 | What will be the mass of a ( 0.500 mathrm{m} ) solution of sodium acetate in water containing ( 0.5 mathrm{Kg} ) sodium acetate? |
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171 | Question 8. How does sprinkling of salt help in clearing the snow covered roads in hilly areas? Explain the phenomenon involved in the process. |
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172 | 75.2 ( g ) of ( C_{6} H_{5} O H ) (phenol) is dissolved in a solvent of ( K_{f}=14 . ) If the depression in freezing point is ( 7 mathrm{K} ) then find the ( % ) of phenol that dimerises. |
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173 | The degree of dissociation of ( C aleft(N O_{3}right)_{2} ) in a dilute aqueous solution containing 7 gm of the salt per 100 gm of water at ( 100^{circ} mathrm{C} ) is 70 per. If the vapour pressure of water at ( 100^{circ} mathrm{C} ) is ( 760 mathrm{mm} ) Calculate the vapour pressure of the solution. A. ( 373.12 mathrm{mm} / mathrm{Hg} ) в. ( 524.89 mathrm{mm} / mathrm{Hg} ) ( mathbf{c} .746 .24 mathrm{mm} / mathrm{Hg} ) D. ( 1049.6 mathrm{mm} / mathrm{Hg} ) |
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174 | (i) Prove that osmotic presser is a colligative property (ii) Calculate the molar concentration of urea solution if it exerts an osmotic pressure of 2.45 atmosphere at ( 300 mathrm{K} ) ( left[mathrm{R}=0.0821 mathrm{I} . text { atm. } operatorname{mol}^{1} boldsymbol{K}^{-1}right] ) |
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175 | Which solution would have the most altered boiling point? A ( cdot 1 M L i_{2} S O_{4} ) в. ( 1 mathrm{M} mathrm{CuSO}_{4} ) ( mathrm{c} cdot 1 mathrm{M} C_{6} mathrm{H}_{12} mathrm{O}_{6} ) D. 1 ( M ) NaCl |
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176 | Henry’s law constant for solubility of methane in benzene is ( 4.27 times 10^{-5} ) ( m m^{-1} H g m o l d m^{-3} ) at constant temperature. Calculate solubility of methane at 760 mm ( H g ) pressure at same temperature |
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177 | The hardness of water due to ( H C O_{3}^{ominus} ) is 122 ppm. Select the correct statement(s). This question has multiple correct options A. The hardness of water in terms of ( C a C O_{3} ) is 200 ppm. B. The hardness of water in terms of ( C a C O_{3} ) is 100 ppm. C. The hardness of water in terms of ( C a C l_{2} ) is 222 ppm. D. The hardness of water in terms of ( M g C l_{2} ) is 95 ppm. |
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178 | Q. 37 Explain why on addition of 1 mole of NaCl to 1 L of water, the boiling point of water increases, while addition of 1 mole of methyl alcohol Lo 1 L of water decreases its boiling point. |
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179 | 12.2 ( g ) of benzoic acid ( (M=122) ) in 100 g water has elevation in the boiling point of ( 0.27 mathrm{K} . K_{b}=0.54 mathrm{K} mathrm{kg} mathrm{mol}^{-1} . ) If there is ( 100 % ) polymerisation, the number of molecules of benzoic acid in the associated state is: A. B. 2 ( c cdot 3 ) ( D ) |
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180 | The relationship between osmotic pressure at ( 273 mathrm{K} ) when 10 g glucose ( left(P_{1}right), 10 ) g urea ( left(P_{2}right) ) and 10 g sucrose ( left(P_{3}right) ) are dissolved in ( 250 mathrm{mL} ) of water is A ( . P_{1}>P_{2}>P_{3} ) в. ( P_{3}>P_{1}>P_{2} ) c. ( P_{2}>P_{1}>P_{3} ) D. ( P_{2}>P_{3}>P_{1} ) |
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181 | The molarity of ( H_{2} S O_{4} ) is ( 18 M . ) Its density is ( 1.8 g m L^{-1} . ) Hence, molality is : ( A cdot 36 m ) B. 200 ( mathrm{m} ) c. ( 500 mathrm{m} ) D. ( 18 mathrm{m} ) |
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182 | A salt which in solution gives a bluish white precipitate with ( N a O H ) solution and a white precipitate with ( B a C l_{2} ) solution is: A ( . C u S O_{4} ) в. ( F e S O_{4} ) c. ( F e_{2}left(S O_{4}right)_{3} ) D. ( C u C l_{2} ) |
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183 | ( 10 mathrm{L} ) of hard water required ( 0.56 mathrm{g} ) of lime ( (C a O) ) for removing hardness. Hence, temporary hardness in ppm of ( boldsymbol{C a C O}_{3} ) is : A . 100 в. 200 c. 10 D. 20 |
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184 | Equal volumes of ( 0.1 M A g N O_{3} ) and ( 0.2 M N a C l ) are mixed. The concentration of ( N O_{3}^{-} ) ions in the mixture will be: ( mathbf{A} cdot 0.1 M ) B. ( 0.05 M ) ( c cdot 0.2 M ) D. ( 0.15 M ) |
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185 | Benzene and toluene form an ideal solution over the entire range of composition. The vapour pressure of pure benzene and toluene at ( 300 K ) are ( 50.71 m m H g ) and ( 32.06 m m H g ) respectively. Calculate the mole fraction of benzene in vapour phase if ( 80 g ) of benzene is mixed with ( 100 g ) of toluene. |
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186 | ( 100 mathrm{ml} ) of ( 2 mathrm{M} ) NaOH solution is diluted by water and the final molarity becomes 0.5. The volume of water added to the solution is: A . ( 400 mathrm{ml} ) B. 300 m c. ( 500 mathrm{ml} ) D. 200 m1 |
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187 | Q. 33 Volume of a solution changes with change in temperature, then what will the molality of the solution be affected by temperature? Give reason for your answer. |
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188 | A ( 0.5 g ) sample of ( K H_{2} P O_{4} ) is titrated with ( 0.1 M ) NaOH.The volume of base required to do this is ( 25.0 m l ) The reaction is represented as: ( boldsymbol{H}_{2} boldsymbol{P} boldsymbol{O}_{4}^{-}+boldsymbol{O} boldsymbol{H}^{-} rightarrow boldsymbol{H} boldsymbol{P} boldsymbol{O}_{4}^{2-}+boldsymbol{H}_{2} boldsymbol{O} ) The percentage purity of ( K H_{2} P O_{4} ) is ( (boldsymbol{K}=mathbf{3 9}, boldsymbol{P}=mathbf{3 1}) ) A . ( 68 % ) B. 34% c. ( 85 % ) D. 51% |
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189 | The phase diagram for solvent and solutions is shown in the figure. What represents the normal boiling point of the solution? ( A ) B. ( c cdot c ) ( D ) |
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190 | Which one of the following electrolytes has the same value of van’t Hoff’s factor (i) as that of ( A l_{2}left(S O_{4}right)_{3} ) (if all are ( 100 % ) ionised)? ( mathbf{A} cdot A lleft(N O_{3}right)_{3} ) B . ( K_{4}left[F e(C N)_{6}right] ) ( mathrm{c} cdot mathrm{K}_{2} mathrm{SO}_{4} ) D. ( K_{3}left[F e(C N)_{6}right] ) |
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191 | An aqueous solution contains 0.53 g of anhydrous ( N a_{2} C O_{3}(text { Mol. wt. } 106) ) dissolved in ( 100 mathrm{ml} ) of solution. The molarity of the solution is: ( mathbf{A} cdot 0.1 M ) в. ( 0.05 M ) ( mathbf{c} cdot 0.2 M ) D. ( 0.4 M ) |
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192 | Illustration 2.38 An aqueous solution containing 28% by weight of a liquid A (molecular mass = 140) has a vapour pressure of 0.200 bar at 37°C. Calculate the vapour pressure of pure liquid (vapour pressure of water at 37°C = 0.100 bar). |
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193 | 3. 10.0 g of glucose (tt,), 10.0 g of urea (Tx), and 10.0 g of sucrose (Ttz) are dissolved in 250.0 mL of water at 273 K (Tt = osmotic pressure of a solution). The relationship between the osmotic pressure of the solutions is a. Ty > T2 > Tz b. nz > , > T2 C. Ty > Ty > Tz d. Tey > Tz > TT, |
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194 | The osmotic pressure of a dilute solution is given by : A. ( P=P_{0} times N_{1} ) B . ( pi V=n R T ) c. ( Delta P=P_{0} N_{2} ) D. ( frac{Delta P}{P^{o}}=frac{P^{o}-P_{S}}{P^{o}} ) |
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195 | Cane sugar underoges the inversion as follow: ( boldsymbol{C}_{12} boldsymbol{H}_{22} boldsymbol{O}_{11}+boldsymbol{H}_{2} boldsymbol{O} rightarrow boldsymbol{C}_{6} boldsymbol{H}_{12} boldsymbol{O}_{6}+ ) ( boldsymbol{C}_{boldsymbol{6}} boldsymbol{H}_{mathbf{1 2}} boldsymbol{O}_{boldsymbol{6}} ) If solution of 0.025 moles of sugar in ( 200 mathrm{gm} ) of water show depression in freezing point ( 0.372^{circ} mathrm{C}, ) then what ( % ) sucrose has inverted. ( left(boldsymbol{K}_{f}left(boldsymbol{H}_{2} boldsymbol{O}right)=right. ) 1.86 ( left.K k g m o l^{1}right) ) |
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196 | Maltose is converted to ‘A’ by Maltase. The mole fraction of ‘A’ in ( 10 % ) (w/w) aq solution is approximately. ( mathbf{A} cdot 0.989 ) B. 0.012 c. ( 0 . ) D. 0.017 |
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197 | ( 3 mathrm{g} ) of salt of molar mass 30 is dissolved in 250 g of water. The molality of a solution is ( x ) M. The value of ( 10 x ) is | 12 |

198 | Tritium, ( T ) (an isotope of ( H ) ) combines with fluorine to form weak acid TF, which ionizes to give Tritium is radioactive and is ( alpha beta- )emitter. freshly prepared aqueous solution of TF has pT (an equivalent of pH) of 1.5 and freezes at ( -0.372^{circ} mathrm{C} . ) If ( 600 mathrm{ml} ) of freshly prepared solution were allowed to stand for 24.8 years. Calculate (i) ionization constant of TF. (ii)Number of lbeta-particles emitted?(Given ( boldsymbol{K}_{f} ) forwater ( =mathbf{1 . 8 6 k g m o l} boldsymbol{K}^{-1}, boldsymbol{t}_{1 / 2} ) for tritium ( =12.4 y ) ears A ( cdot(i) K_{a}=7.3 times 10^{-3}(i i) 4.55 times 10^{22} ) B . (i)K ( _{a}=7.3 times 10^{-5}(i i) 4.55 times 10^{24} ) C . ( (i) K_{a}=14.3 times 10^{-3}(i i) 9.1 times 10^{22} ) D . (i) ( K_{a}=14.3 times 10^{-5}(i i) 9.1 times 10^{24} ) |
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199 | Ilustration 2.169 At 300 K, 36 g of glucose present per litre in its solution has an osmotic pressure of 4.98 bar. If the osmotic pressure of the solution is 1.52 bar at the same temperature, what would be its concentration? |
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200 | Which of the following aqueous solution will show maximum vapour pressure at 300K? ( mathbf{A} cdot 1 M N a C l ) в. ( 1 mathrm{M} mathrm{CaCl}_{2} ) c. ( 1 M A l C l_{3} ) D. ( 1 M C_{12} H_{22} O_{11} ) |
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201 | An aqueous solution of a non-volatile solute boils as ( 100.17^{circ} mathrm{C} ). What is the depression in the freezing point for the solution in ( ^{circ} mathrm{C} ) ? ( left[K_{b} text { and } K_{f} text { for water is } 0.512 ) and right. ( mathbf{1 . 8 6}^{circ} boldsymbol{C} / boldsymbol{m} ) respectively A . 0.93 B. 0.11 ( c cdot 0.62 ) D. 0.31 |
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202 | Illustration 2.209 The freezing point of a solution containing 0.3 g of acetic acid in 43 g of benzene reduces by 0.3°. Calculate the Van’t Hoff factor. (K, for benzene = 5.12 K kg moll) |
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203 | Which of the following alkali metal ions has lowest ionic mobility in aqueous solutions? ( mathbf{A} cdot R b^{+} ) B. ( C s^{ } ) c. ( N a^{+} ) ( mathbf{D} cdot L i^{+} ) |
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204 | If the ionic product of ( M(O H)_{2} ) is ( 5 times ) ( 10^{-10}, ) then the molar solubility of ( M(O H)_{2} ) in ( 0.1 M N a O H ) is: A ( .5 times 10^{-12} mathrm{M} ) В. ( 5 times 10^{-8} ) М c. ( 5 times 10^{-10} M ) D. ( 5 times 10^{-9} M ) E ( .5 times 10^{-16} M ) |
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205 | Calculate the vapour pressure of an aqueous solution of 1.0 molal glucose solution at ( 100^{circ} mathrm{C} ) |
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206 | Which of the following is not an air pollutant? A. ( N_{2} ) в. ( N_{2} ), c. ( N O ) D. ( C O ) |
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207 | The freezing point of equimolal aqueous solution will be highest for: A. ( C_{6} H_{5} N H_{3}^{+} C l^{-} ) в. ( quad C aleft(N O_{3}right)_{2} ) c. ( _{L a}left(N O_{3}right)_{2} ) D. ( C_{6} H_{12} O_{6} ) |
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208 | | Illustration 2,90 The boiling point elevation constant for benzene is 2.57°C/m. The boiling point of benzene is 81.0°C. Determine the boiling point of a solution formed when 5 g of C2H,, is dissolved in 15 g of benzene. |
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209 | A 0.001 molal solution of a complex represented as ( P tleft(N H_{3}right)_{4} C l_{4} ) in water had freezing point depression of ( mathbf{0 . 0 0 5 3 ^ { circ }} mathbf{C .} ) Given, ( boldsymbol{K}_{f} ) for ( boldsymbol{H}_{2} boldsymbol{O}= ) 1.86 Kmolality ( ^{-1} ). Assuming 100% ionisation of the complex, write the ionisation nature and formula of complex A ( cdot P tleft[left(N H_{3}right)_{4} C l_{2}right] C l_{2} rightarrow P tleft[left(N H_{3}right)_{4} C l_{2}right]^{2+} 2 C l ) B . ( P tleft[left(N H_{3}right)_{4} C l_{2}right] C l_{2} rightarrow P tleft[left(N H_{3}right)_{4} C l_{2}right]^{+} C l ) c. ( P tleft[left(N H_{3}right)_{4} C l_{2}right] C l_{2} rightarrow 2 P tleft[left(N H_{3}right)_{4} C l_{2}right]^{+} C l ) D. ( P tleft[left(N H_{3}right)_{4} C l_{2}right] C l_{2} rightarrow P tleft[left(N H_{3}right)_{4} C l_{2}right]^{3+} 3 C l ) |
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210 | A 0.2 molal solution of KCl freezes at ( -0.68^{circ} mathrm{C} . ) If ( K_{f} ) for ( H_{2} O ) is ( 1.86, ) the degree of dissociation of ( boldsymbol{K} boldsymbol{C l} ) is: A . ( 75 % ) B. ( 83 % ) ( c .65 % ) D. ( 92 % ) |
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211 | 1 L sample of impure water containing sulphide ion is made ammonial and is titrated with ( 300 mathrm{mL} ) of ( 0.1 M A g N O_{3} ) solution. Which of the following statements is/are correct about the above reaction? This question has multiple correct options A. The strength of ( H_{2} S ) in water is ( 0.51 mathrm{g} / mathrm{L} ) B. The strength of ( H_{2} S ) in water is ( 5.1 mathrm{g} / mathrm{L} ) C. The concentration of ( H_{2} ) S in water in ppm is 510 D. The concentration of ( H_{2} S ) in water in ppm is 51 |
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212 | A ( 5 % ) solution of cane sugar is isotonic with ( 0.877 % ) of ( X . ) The molecular weight of substance X is: ( mathbf{A} cdot 58.98 ) B. 119.96 ( mathbf{c} .95 .58 ) D . 126.98 |
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213 | Two liquids ( A ) and ( B ) form an ideal solution at temperature T. When the total vapour pressure above the solution is 400 torr, the mole fraction of ( A ) in the vapour phase is 0.40 and in the liquid phase ( 0.75 . ) What are the vapour pressure of pure ( A ) and pure ( B ) at temperature T? |
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214 | Illustration 2.151 Addition of Hgl, to the aqueous solution of KI shows an increase in the osmotic pressure, why? |
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215 | Question 2. Explain why on addition of 1 mole of NaCl to 1L of water, the boiling point of water increases, while addition of 1 mole of methyl alcohol to 1 L of water decreases its boiling point. |
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216 | Illustration 2.128 The molal freezing point depression constant of benzene (CH) is 4.90 K kg mol-!. Selenium exists as a polymer of the type Se. When 3.26 g of selenium is dissolved in 226 g of benzene, the observed freezing point is 0.112°C lower than pure benzene. Deduce the molecular formula of selenium. (Atomic mass of Se = 78.8 g mol-‘) |
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217 | ( 58.5 g m ) of ( N a C l ) and ( 180 g m ) of glucose were separately dissolved in 1000 ( m l ) of water. Identify the correct statement regarding the elevation of boiling point (b.p.) of the resulting solutions. A. ( N a C l ) solution will show higher elevation of b.p. B. Glucose solution will show higher elevation of b.p. C. Both the solutions will show equal elevation of b.p. D. The b.p. elevation will be shown by neither of the solutions |
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218 | ( 250 m l ) of a sodium carbonate solution contains 2.65 grams of ( N a_{2} C O_{3} .10 m l ) of this solution is added to ( ^{prime} x^{prime} m l ) of water to obtain ( 0.001 M N a_{2} C O_{3} ) solution. What is the value of ( ^{prime} x^{prime} ) in ( m l ) ? [Molecular weight of ( left.boldsymbol{N} boldsymbol{a}_{2} boldsymbol{C O}_{3}=mathbf{1 0 6}right] ) A. 1000 в. 990 c. 9990 D. 90 |
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219 | Two liquids ( A ) and ( B ) form an ideal solution. What is the vapour pressure of solution containing 2 moles of ( A ) and 3 moles of ( B ) at ( 300 K ? ) [Given: At ( 300 K ), vapour pressure of pure liquid ( boldsymbol{A}left(boldsymbol{P}_{A}^{circ}right)=mathbf{1 0 0} ) torr, Vapour pressure of pure liquid ( Bleft(P_{B}^{circ}right)= ) ( 300 text { tor } r] ) A. 200 torr B. 220 torr c. 180 tor D. None of these |
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220 | In an auto engine with no pollution controls, about ( 5 % ) of the fuel ( left(C_{8} H_{18}right) ) is unburned. Molar ratio of ( C O ) and ( left(C_{8} H_{18}right), ) emitted in the exhaust gas is: A . 100 B. 152 ( c .50 ) D. 5 |
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221 | lce begins to separate at ( -0.744^{circ} mathrm{C} ) from a solution containing 2.4 g of nonvolatile, non-electrolyte in 100 g water. Calculate the molar mass of solute, ( boldsymbol{K}_{boldsymbol{f}} ) for ( boldsymbol{H}_{2} boldsymbol{O} ) is ( 1.86 mathrm{K} ) mol( ^{-1} boldsymbol{k} boldsymbol{g} ). Assume mass of solvent is equal to mass of solution. Answer in g/mol.(Enter the answer as ( frac{M a s s}{10} ) ). |
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222 | Illustration 2.92 The ebullioscopic constant for benzene is 2.52 Km-1. A solution of an organic substance in benzene boils at 0.125°C higher than benzene. Calculate the molality of solution? |
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223 | For a solution of density, ( d ) in ( g / m ) containing solute of molecular weight ( W, ) the molarity ( M ) and molality ( m ) are related by: A ( cdot frac{d}{M}=frac{1}{m}+frac{W}{1000} ) в. ( frac{d}{m}=frac{1}{M}+frac{W}{1000} ) c. ( frac{W}{M}=frac{1}{m}+frac{d}{1000} ) D. ( frac{d}{m}=frac{W}{M}+frac{1}{1000} ) |
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224 | The Vant Hoff factor (i) for a dilute solution of ( boldsymbol{K}_{mathbf{3}}left[boldsymbol{F} boldsymbol{e}(boldsymbol{C} boldsymbol{N})_{boldsymbol{6}}right] ) is (Assuming ( 100 % text { ionsation }) ) A . 10 B. 4 c. 5 D. 0.25 |
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225 | The concentration of ( mathrm{CO}_{2} ) in a soft drink bottled with a partial pressure of ( mathrm{CO}_{2} ) of 4.0 atm over the liquid at ( 25^{circ} mathrm{C} ) is ( 1.2 times ) ( 10^{-1} ) M. The Henry’s law constant for ( C O_{2} ) at this temperature is A ( cdot 3.0 times 10^{-2} mathrm{mol} / mathrm{L}- ) atm B . ( 4.5 times 10^{-3} ) mol ( / L- ) atm c. ( 5.6 times 10^{-3} mathrm{mol} / mathrm{L}- ) atm D. ( 2.3 times 10^{-2} mathrm{mol} / mathrm{L}- ) atm E. More information is needed to solve the problem. |
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226 | The increase in boiling point of a solution containing ( 0.6 g ) urea in ( 200 g ) water is ( 0.50^{circ} mathrm{C} ). Find the molal elevation constant. A ( cdot 10 K ) kg mol( ^{-1} ) в. ( 10 mathrm{K} ) g ( mathrm{mol}^{-1} ) c. ( 10 K ) kg moll ( l ) D. ( 1.0 K ) kg mol( ^{-1} ) |
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227 | Illustration 2.72 The vapour pressure of pure benzene at 50°C is 268 mm of Hg. How many moles of non-volatile solute per mole of benzene are required to prepare a solution of benzene having a vapour pressure of 160.0 mm of Hg at 50°C? |
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228 | Q13. Why ethyl alcohol is completely miscible with water? Ang Tu. . 1 |
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229 | Which of the following solutions is an example of negative deviation from Raoult’s law? A. Acetone + Ethanol B. Carbon tetrachloride + Chloroform c. Acetone + chloroform D. water + Ethanol |
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230 | Molarity of a substance decreases with increase in temperature. A. True B. False |
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231 | Equal weights of methane and oxygen are mixed in an empty container at ( 25^{circ} mathrm{C} . ) The fraction of the total pressure exerted by oxygen is: A ( cdot frac{1}{3} ) B. ( frac{1}{2} ) ( c cdot frac{2}{3} ) D. |
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232 | A solution containing 0.5 g of naphthalene in 50 g ( C C l_{4} ) yield a boiling point elevation of ( 0.4 mathrm{K}, ) while a solution of ( 0.6 mathrm{g} ) of an unknown solute in the same mass of the solvent gives a boiling point elevation of 0.65 K. Find the molar mass of the unknown solute. |
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233 | Statement 1: A supersaturated solution of glucose in boiling water crystallizes as it cools.
Statement 2 : The solubility increases as the temperature increases. |
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234 | An ideal solution has two components ( A ) and ( B . A ) is more volatile than ( B ), i.e. ( boldsymbol{P}_{A}^{circ}>boldsymbol{P}_{B}^{circ} ) and also ( boldsymbol{P}_{A}^{circ}>boldsymbol{P}_{text {total}} . ) If ( boldsymbol{X}_{boldsymbol{A}} ) and ( Y_{A} ) are mole fractions of components ( A ) in liquid and vapour phases, then : A. ( X_{A}=Y_{A} ) в. ( X_{A}>Y_{A} ) c. ( X_{A}<Y_{A} ) D. Data insufficient |
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235 | Q. 45 What is “semipermeable membrane”? | 12 |

236 | ( Delta_{f} G^{o} ) at ( 500 K ) for substance ( S ) in liquid state and gaseous state are ( +100.7 k c a l m o l^{-1} ) and ( +103 k c a l ) mol( ^{-1} ) respectively. Vapour pressure of liquid ( S ) at ( 500 K ) is approximately equal to: ( (R= ) ( left.2 operatorname{cal} K^{-1} m o l^{-1}right) ) A. 0.1 atm B. 1 atm c. 10 atm D. 100 atm |
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237 | State Henry’s law. | 12 |

238 | For a dilute solution, Raoult’s law states that: A. The relative lowering of vapour pressure is equal to the mole fraction of solute B. The relative lowering of vapour pressure is equal to the mole fraction of solvent C. The relative lowering of vapour pressure is proportional to the amount of solute in solution D. The vapour pressure of the solution is equal to the mole fraction of solvent |
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239 | If in a solvent, n simple molecules of solute combine to form an associated molecule, ( alpha ) is the degree of association, the van’t Hoff’s factor is equal to: A. ( frac{1}{1-n alpha} ) B. ( 1-alpha+n alpha ) ( c cdot_{1-alpha+frac{alpha}{n}} ) D. ( frac{alpha}{n}-1+alpha ) |
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240 | Which of the following does not define solubility? A. The concentration of solute in a saturated solution B. The moles of solute dissolved in a given volume of solution C. The maximum mass of solute that can dissolve in a given volume of solution D. The minimum moles of solute needed to produce one litre of a saturated solution |
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241 | At ( 25^{circ} mathrm{C} ) the saturated vapour pressure of water is 3.165 kPa ( (23.75 mathrm{mm} mathrm{Hg}) ) Find the saturated vapour pressure of a ( 5 % ) aqueous solution of urea (carbamide) at the same temperature. (Molar mass of urea ( =mathbf{6 0 . 0 5} ) g ( boldsymbol{m o l}^{-1} ) ) |
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242 | The mole fraction of ( H N O_{3} ) in an aqueous binary solution is ( 0.15> ) The ratio of moles of ( H N O_{3} ) to ( H_{2} O ) in the solution is nearly: ( mathbf{A} cdot 17: 3 ) B. 3: 17 c. 1: 1 D. 15: 100 |
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243 | A water sample contains 81 ppm of ( boldsymbol{C a}left(boldsymbol{H} boldsymbol{C O}_{3}right)_{2}, 73 ) ppm of ( boldsymbol{M} boldsymbol{g}left(boldsymbol{H} boldsymbol{C O}_{3}right)_{2} ) 68 ppm of ( C a S O_{4} ) and 60 ppm of ( M g S O_{4} . ) What is the hardness of the Water sample? (Atomic weights of calcium, magnesium and sulphur are respectively 40,24 and 32 ). A. 50 ppm B. 100 ppm c. 150 ppm D. 200 ppm |
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244 | A liquid will boil when: A. enough salt has been added to it B. the vapor pressure of the liquid is equal to the atmospheric or surrounding pressure C. the vapor pressure of the liquid reaches ( 760 mathrm{mmHg} ) D. conditions favor the liquids molecules to be closer together E. it has been brought up to a higher elevation |
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245 | Assuming that concentration of ( C a^{2+} ) ions in solution is in equal equivalence ratio to chloride ions, the hardness of water is : A ( .9 .180 times 10^{3} ) ppm B . ( 6.180 times 10^{3} ) ppm c. ( 12.180 times 10^{3} ) ppm D. ( 4.180 times 10^{3} ) ppm |
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246 | 0.6 ml of glacial acetic acid with density ( 1.06 g / m l ) is dissolved in ( 1 k g ) water and the solution froze at ( -0.0205^{circ} mathrm{C} . ) Calculate van’t Hoff factor: ( boldsymbol{K}_{f} ) for water is ( 1.86 boldsymbol{K} boldsymbol{k g} boldsymbol{m o l}^{-1} ) |
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247 | Which of the following is weakly acidic? В. ( 0.1 M ) NaCl ( mathrm{c} cdot 0.1 mathrm{M} quad mathrm{HC}_{2} mathrm{H}_{3} mathrm{O}_{2} ) D. ( 0.1 M quad C H_{3} O H ) E. ( 0.1 M ) KOH |
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248 | If ( 684 g ) of sucrose ( (M M=342 g) ) is dissolved in ( 2000 g ) of ( H_{2} O ) (essentially ( 2 L), ) what will be the freezing point of this solution? A . -0.51 B . -1.86 c. -3.72 D. – 6.58 |
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249 | A mixture of ethyl alcohol and propyl alcohol has a vapour pressure of 290 ( mathrm{mm} ) at ( 300 mathrm{K} . ) The vapour pressure of propyl alcohol is ( 200 mathrm{mm} ). If the mole fraction of ethyl alcohol is ( 0.6, ) its vapour pressure(in ( mathrm{mm} ) ) at the same temperature will be: A . 350 в. 300 c. 700 D. 360 |
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250 | Which of the following weak electrolytes would give aqueous solution having ( 3 C alpha ) anion concentration? A ( . A_{3} B ) B. ( A_{3} B_{2} ) ( mathrm{c} cdot A B_{3} ) D. ( A_{3} B_{4} ) |
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251 | A closed vessel is maintained at a constant temperature. It is first evacuated and then vapour is injected into it continuously. The pressure of the vapour in the vessel is: A. increases continuously B. first increases and then remains constant c. first increases and then decreases D. none of the above |
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252 | True or False. The components of a mixture can never be separated by physical methods. |
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253 | Calculate osmotic pressure of a solution (write only integer part) obtained on mixing ( 100 mathrm{mL} ) of ( 3.4 % ) (mass/vol) solution of urea (molar mass 60 ) and ( 50 mathrm{mL} ) of ( 1.6 % ) (mass/vol) solution of cane sugar (molar mass 342 ( operatorname{at} 27^{circ} C ) |
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254 | What type of deviation from Raoult’s law is exected? (a) when equal volume of acetone and ethanol is mixed? (b) when equal volume of acetone and chloroform is mixed? |
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255 | Select incorrect statements. A. ( N H_{3} ) is soluble in water due to hydrogen bonding as well as due to formation of ions. B. Gases which can be liquefied easily are more soluble in water then the gases which cannot be liquefied. C. The solute follows Henry law at all pressure of gas. D. The solute follows Henry law at low pressure of gas. |
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256 | 1 L of ( 0.15 M H C l ) and 1 L of ( 0.3 M ) ( H C l ) is given. What is the maximum volume of ( 0.2 M H C l ) which one can make from these two solutions? No water is added. ( mathbf{A} cdot 1.2 L ) B. ( 1.5 L ) c. ( 1.3 L ) D. ( 1.4 L ) |
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257 | Sea water is found to conatin ( mathbf{5 . 8 5 %} ) Nacl and ( mathbf{9 . 5 0 %} boldsymbol{M g C l}_{2} ) by weight of solution. Calculate its normal boiling point assuming ( 80 % ) ionisation for ( N a C l ) and ( 50 % ) ionisation of ( M g C l_{2} ) ( left[boldsymbol{K}_{boldsymbol{b}}left(boldsymbol{H}_{2} boldsymbol{O}right)=mathbf{0 . 5 1} boldsymbol{k g} boldsymbol{m o l}^{-1} boldsymbol{K}right] ) A. ( T_{b}=51.15^{circ} mathrm{C} ) в. ( T_{b}=78.6^{circ} mathrm{C} ) c. ( T_{b}=102.3^{circ} mathrm{C} ) D. ( T_{b}=157.2^{circ} mathrm{C} ) |
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258 | ( H_{2} S, ) a toxic gas with rotten egg like smell, is used for the qualitative analysis. If the solubility of ( H_{2} S ) in water at STP is ( 0.195 mathrm{m} ), Calculate Henry’s law constant. A. 282.0 bar B. 324.8 bar c. 462.9 bar D. 534.8 bar |
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259 | A certain liquid mixture of two liquids ( A ) and B (behaving ideally) has a vapour pressure 70 torr ( (1 text { torr }=1 mathrm{mm}) ) at ( 25^{circ} mathrm{C} ) for a certain mole fraction ( X ) of ( A ). For the same mole fraction ( X ) for ( B ) in the mixture, the vapour pressure of mixture is 90 torr at ( 25^{circ} mathrm{C} . ) If ( boldsymbol{P}_{A}^{0}-boldsymbol{P}_{B}^{0}=mathbf{4 0} ) torr calculate ( P_{A}^{0}, P_{B}^{0} ) and ( X ) A . 100 torr, 60 torr, 0.25 B. 120 torr, 80 torr, 0.25 c. 200 torr, 160 torr, 0.25 D. 220 torr, 180 torr, 0.25 |
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260 | Henry’s law constant for oxygen dissolved in water is ( 4.34 times 10^{4} ) atm at ( 25^{C} . ) If the partial pressure of oxygen in air is 0.4 atm. Calculate the concentration (in moles per litre) of the dissolved oxygen in water in equilibrium with air at ( 25^{circ} C ) ( mathbf{A} cdot 5.11 times 10^{-4} ) В. ( 5.11 times 10^{-3} ) c. ( 9.2 times 10^{-6} ) D. ( 0.92 times 10^{-6} ) |
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261 | Illustration 2.188 0.1 M aqueous solution of MgCl, at 300K is 4.92 atm. What will be the percentage ionization of the salt? a. 49% b. 59% c. 79% d. 69% |
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262 | ( 56 mathrm{g} ) of nitrogen and ( 96 mathrm{g} ) of oxygen are mixed isothermally and at a total pressure of 10 atm. The partial pressures of oxygen and nitrogen (in atm) are ( _{text {- – }} ) -respectively ( A cdot 4,6 ) B. 5,5 c. 2,8 ( D cdot 6,4 ) |
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263 | When acetone and chloroform are mixed, hydrogen bonding takes place between them. Such a liquid pair will cause: A. Positive deviation from Raoult’s law B. Negative deviation from Raoult’s law c. No deviation from Raoult’s law D. cannot be predicted |
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264 | Find the freezing point of a solution containing 0.5 mole of glucose dissolved in 200 g of ( H_{2} ) O? (Given that ( boldsymbol{K}_{f} ) for water is ( 1.86 quad boldsymbol{K} boldsymbol{m}^{-1} ) A . -4.65 B . -2.65 c. -14.65 D. -8.65 |
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265 | Example 2.28 0.5 g KCl was dissolved in 100 g water, and the solution, originally at 20°C froze at -0.24°C. Calculate the percentage ionization of salt. K. per 1000 g of water = 1.86°C. |
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266 | Assuming each salt to be ( 90 % ) dissociated which of the followings will have highest osmotic pressure? A. Decimolar ( A l_{2}left(S O_{4}right)_{3} ) B. Decimolar ( B a C l_{2} ) c. Decimolar ( N a_{2} S O_{4} ) D. A solution obtained by mixing equal volumes of ( (b) ) and (c) and filtering |
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267 | What is a mixture? A. Substance with two or more different particles B. Substance that is insoluble c. substance with a single homogenous particle D. None of above |
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268 | Which of the following aqueous solutions should have the highest boiling point? A. ( 1.0 M ) NaOH в. ( 1.0 M ) Na( _{2} ) SO ( _{4} ). с. ( 1.0 M ) NH( _{4} N O_{3} ) |
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269 | 9. The molal boiling point constant for water is 0.513 Km-‘, When 0.1 mole of sugar is dissolved in 200.0 g of water, the solution boils under a pressure 1.0 atm at a. 100.513°C b. 100.0513°C c. 100.256°C d. 101.025°C |
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270 | To ( 500 c m^{3} ) of water ( 3.0 times 10^{-3} k g ) of acetic acid is added. If ( 23 % ) of acetic acid is dissociated, what will be the depression of freezing point? ( left[K_{f} ) and density of water are right. ( 1.86 K k g m o l^{-1} ) and ( 0.997 g c m^{-3} ) respectively в. ( 0.33 K ) c. ( 0.98 K ) D. ( 0.68 K ) |
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271 | Two elements ( A ) and ( B ) form compounds having molecular formulae ( A B_{2} ) and ( A B_{4} . ) When dissolved in 20.0 g of benzene, 1.0 g of ( A B_{2} ) lowers the freezing point by ( 2.3^{circ} mathrm{C} ), whereas ( 1.0 mathrm{g} ) of ( A B_{4} ) lowers the freezing point by ( 1.3^{circ} mathrm{C} . ) The molal depression constant for benzene in 1000 g is ( 5.1 . ) Calculate the atomic masses of ( A ) and ( B ) |
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272 | The concentration of which of the following solution has the highest value? A. Dilute solution B. Concentration solution c. saturated solution D. Supersaturated solution |
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273 | We separate mixtures to: A. remove unwanted components B. to get pure substances C. Both of the above D. None of the above |
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274 | Hlustration 2.114 A solution of urea in water has boiling point of 100.15°C. Calculate the freezing point of the same solution if K, and K, for water are 1.87 K kg mol-1 and 0.52 K kg mol-, respectively. |
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275 | At temperature ( T_{1} ) and composition Q,which of the following is true? This question has multiple correct options A. Vapour phase is richer in B while liquid phase is richer in ( A ) B. Distillation of composition Q gives only pure A C. Distillation of composition ( Q ) gives pure ( A ) and pure ( B ) D. Distillation of composition Q gives higher percentage of B than A. |
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276 | Predict whether van’t HOff factor ( (i) ) is less than one or greater than one in the following: (i) ( C H_{3} C O O H ) dissolved in water (ii) ( C H_{3} C O O H ) dissolved in benzene |
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277 | A ( 5.8 % ) solution of ( N a C l ) has vapour pressure closest to A . ( 5.8 % ) solution of urea B. 2 ( M ) solution of glucose c. ( 1 M ) solution of urea D. 5.8 % solution of glucose |
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278 | Which of the following substances will lose its solutbility with increase in temperature? A . ( N a O H ) в. ( N a_{2} C O_{3} ) c. ( N a_{2} S O_{4} ) D. All |
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279 | Which one is not equal to zero for an ideal solution? A. ( Delta V_{operatorname{mix}} ) B. ( Delta P=P_{text {observed }}-P_{text {Rooult}} ) c. ( Delta H_{operatorname{mix}} ) D. ( Delta S_{text {mix }} ) |
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280 | Dry air was drawn through bulbs containing a solution of 40 grams of urea in 300 grams of water, then through bulbs containing pure water at the same temperature and finally through a tube in which pumice moistened with strong ( H_{2} S O_{4} ) was kept. The water bulbs lost ( 0.0870 g r a m s ) and the sulphuric acid tube gained 2.036 grams. Calculate the molecular weight of urea. A. ( quad M=26.9 ) В. ( quad M=46.8 ) c. ( quad M=53.8 ) D. ( M=93.6 ) |
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281 | The vapour pressure of ethanol and methanol are 44.5 mm ( H g ) and 88.7 mm ( H g ) respectively. An ideal solution is formed at the same temperature by mixing ( 60 g ) of ethanol with ( 40 g ) of methanol. The total vapour pressure of the solution and the mole fraction of methanol in the vapour are respectively: A. ( 43.46 mathrm{mm} ) and 0.51 в. ( 66.13 mathrm{mm} ) and 0.657 c. ( 66.15 mathrm{mm} ) and 0.791 D. 70.59 ( m m ) and 0.657 |
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282 | The vapour pressure of a dilute aqueous solution of glucose is ( 750 mathrm{mm} ) of ( mathrm{Hg} ) at ( 373 mathrm{K} ). Calculate molality. |
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283 | 0.19 Consider the figure and mark the correct option. Piston (AJ Piston (8) SPM Fresh water (A) Concentrated sodium chloride solution in water (B) (a) Water will move from side (A) to side (B) if a pressure lower osmotic pressure is applied on piston (B) (b) Water will move from side (B) to side (A) if a pressure greater than osmotic pressure is applied on piston (B) (c) Water will move from side (B) to side (A) if a pressure equal to osmotic pressure is applied on piston (B) (d) Water will move from side (A) to side (B) if pressure equal to osmotic pressure is applied on piston (A) |
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284 | When acetone and chloroform are mixed together, hydrogen bonds are formed between them. Which of the following statements is correct about the solution made by mixing acetone and chloroform ? A. on mixing acetone and chloroform will form an ideal solution B. On mixing acetone and chloroform positive deviation is shown since the vapour pressure increases c. on mixing acetone and chloroform negative deviation is shown since there is decrease in vapour pressure D. At a specific composition, acetone and chloroform will form minimum boiling azeotrope |
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285 | Question 4. Concentrated nitric acid used in laboratory work is 68% nitric acid by aqueous solution. What should be the molarity of such a sample of the acid if the density of the solution is 1.504 g L-lo w () Since mass percentage i.e., mass of solute (HNO.) in 100 g solution is given, find mass of HNO3; then calculate its molar mass and number of moles. (ii) From density, find the volume of solution (iii) Calculate the molarity by applying the formula, Moles of solute Molarity = 7 Volume of solution (in ) |
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286 | A non ideal solution was prepared by mixing ( 30 mathrm{ml} ) chloroform and ( 50 mathrm{ml} ) acetone. The volume of mixture will be : ( A cdot>80 m l ) в. ( 80 m l ) |
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287 | Some liquids on mixing form ‘azeotropes’. What are ‘azeotropes’? |
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288 | Out of 0.1 molal aqueous solution of glucose and 0.1 molal aqueous solution of ( K C l, ) which one will have higher boiling point and why? |
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289 | Calculate the vapour pressure of solution having 3.42 g of canesugar in 180 g water at ( 40^{circ} C ) and ( 100^{circ} ) C. Given that, the boiling point of water is ( 100^{circ} mathrm{C} ) and heat of vaporisation is 10 kcal ( m o l^{-1} ) in the given temperature range. Also, calculate the lowering in vapour pressure of 0.2 molal cane-sugar at ( 40^{circ} C: ) ( mathbf{A} .58 mathrm{mm} ) B. ( 13 mathrm{mm} ) c. ( 78 mathrm{mm} ) D. none of these |
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290 | Question 30. Calculate the amount of benzoic acid (CH-COOH) required for preparing 250 mL of 0.15 M solution in methanol. As molarity is given, apply the formula for molarity, to find the mass of es benzoic acid. |
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291 | ( 50 mathrm{mL} ) of sample of hard water gave good lather with ( 6 mathrm{mL} ) of standard soap solution (1 mL soap solutions = 1 mg ( mathrm{CaCO}_{3} ). If the hardness is only due to ( M gleft(H C O_{3}right)_{2}, ) the weight of milk of lime required to remove the hardness completely from ( 100 mathrm{kg} ) of that sample of water is: A. ( 17.8 mathrm{g} ) в. ( 8.9 mathrm{g} ) c. ( 178 g ) D. 89 ( g ) |
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292 | What is the molarity of ( H C l ) in a solution prepared by dissolving ( 5.5 mathrm{g} ) ( H C l ) in 200 g ethanol if the density of the solution is 0.79 g/ mL? A . 0.58 M B. 0.21 c. 0.93 M D. 1.7 м |
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293 | Q Type your question ( mathbf{A} ) B. ( mathbf{C} ) ( D ) |
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294 | The decrease in the freezing point of an aqueous solution of a substance is ( 1.395 k ) and that in the freezing point of benzene solution of the same substance is ( 1.280 k . ) Explain the difference in ( Delta T ). The substance: A. dissociates in the aqueous solutio as well as in the benzene solution B. forms complex in solution c. associates in the benzene solution D. dissociates in the aqueous solution and not in the benzene solution |
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295 | For weak electrolytes, van’t Hoff factor ‘i is a measure of the degree of dissociation of weak electrolyte. If true enter 1 , if false enter 0 . |
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296 | Illustration 2.78 At 25°C, the vapour pressure of pure water is 25.0 mm Hg and that of an aqueous dilute solution of urea is 20 mm Hg. Calculate the molality of the solution. |
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297 | ( mathbf{H}_{2} mathrm{O}_{2} ) is sold as a solution of approximately ( 5.0 mathrm{g} mathrm{H}_{2} mathrm{O}_{2} ) per ( 100 mathrm{ml} ) of the solution the molecular mass of ( mathbf{H}_{2} mathbf{O}_{2} ) is ( mathbf{3 4} . ) The molarity of this solution is approximately: A . ( 1.15 mathrm{M} ) в. 1.5 М. c . ( 3.0 mathrm{M} ) D. 3.4M |
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298 | For a very dilute aqueous solution of ( boldsymbol{K}_{4}left[boldsymbol{F} boldsymbol{e}(boldsymbol{C} boldsymbol{N})_{6}right], ) van’t Hoff factor is : ( mathbf{A} cdot i=11 ) в. ( i=5 ) ( c cdot_{i}=frac{1}{11} ) D. ( i=10 ) |
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299 | The freezing point of a 0.05 molal solution of a non-electrolyte in water is: ( mathbf{A} cdot-0.093^{circ} mathrm{C} ) B . ( 1.86^{circ} mathrm{C} ) ( mathbf{c} cdot 0.93^{circ} mathrm{C} ) D. ( 0.093^{circ} mathrm{C} ) |
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300 | What is the amount of urea dissolved per litre, if aqueous solution is isotonic with ( 10 % ) cane sugar solution: (mol. wt of urea ( =mathbf{6 0} ) )? A ( .200 g / L ) в. ( 19.2 g / L ) c. ( 17.54 g / L ) D. ( 16.7 g / L ) |
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301 | The osmotic pressure of solution increases if: A. temperature is decreased B. concentration is decreased c. number of solute molecules are increased D. volume is increased |
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302 | A solution containing ( 0.122 mathrm{kg} ) of benzoic acid in ( 1 k g ) of benzene (b.pt.353 K) boils at ( 354.5 K ) Determine the apparent molar mass of benzoic acid (which dimerizes) in the solution and the degree of dimerization Given: ( Delta_{v a p} H_{1 m}(text {benzene})= ) ( mathbf{3 9 4 . 5 7} boldsymbol{J} boldsymbol{g}^{-1} ) A. 0.214 kg ( mathrm{mol}^{-1}, 0.86 ) в. 0.257 kg ( m o l^{-1}, 0.932 ) c. ( 0.428 mathrm{kg} mathrm{mol}^{-1}, 0.956 ) D. ( 0.454 mathrm{kg} mathrm{mol}^{-1}, 0.986 ) |
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303 | Mlustration 2.117 In a cold climate water gets frozen causing damage to radiator of a car. Ethylene glycol is used as an antifreezing agent. Calculate the amount of ethylene glycol to be added to 4 kg of water to prevent it from freezing at -6°C. (K for water = 1.85 K kg mol-!) |
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304 | Pick out the mixture from the following. A. water B. Oxygen c. Carbon dioxide D. Air |
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305 | The mass of ( N a_{2} C O_{3} ) required to prepare ( 500 mathrm{ml} ) of ( 0.1 mathrm{M} ) solution is: A . 10.6 g B. ( 5.3 mathrm{g} ) c. ( 2.65 mathrm{g} ) D. 7.95 |
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306 | A ( 5 % ) solution (w/v) of cane-sugar (Mol. weight ( =342 ) ) is isotonic with ( 0.877 % ) ( (w / v) ) of urea solution. Find molecular weight of urea (round off to the nearest integer). |
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307 | 18 g glucose ( left(C_{6} H_{12} O_{6}right) ) is added to ( 178.2 mathrm{g} ) of water. The vapour pressure of this aqueous solution at ( 100^{0} C ) in torr is: A . 7.60 B. 76.00 c. 752.40 D. 759.00 |
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308 | ( 14.2 mathrm{g} N a_{2} S O_{4} ) is present in ( 10^{2} mathrm{kg} ) water. Its concentration in ppm is: A. 10 ppm B. 100 ppm c. 142 ppm D. ( 14.2 mathrm{ppm} ) |
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309 | The osmotic pressure of the solution obtained by mixing ( 200 mathrm{cm}^{3} ) of ( 2 % ) (mass-volume) solution of urea with ( 200 mathrm{cm}^{3} ) of ( 3.42 % ) solution of sucrose at ( mathbf{2 0} ) is? A ( .421 P a ) в. ( 267 P a ) ( c .5240 P a ) D. ( 153 P a ) |
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310 | A student mixes ( 10.0 m L ) of ( 0.10 M A g N O_{3} ) with excess copper metal. The reaction should produce 0.107 gram of silver; however, the student obtains a mass of 150 grams of silver. Plausible explanations for this yield ( >100 % ) might include : I. the student did not subtract the mass of the filter paper before recording results. II. the student did not thoroughly dry the sample before massing. III. the copper metal did not react completely. A . I only B. II only c. I and II only D. I and III only E. I, II, and III |
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311 | An electrolyte ( A ) gives 3 ions and ( B ) is a non- electrolyte. If ( 0.1 ~ M ) solution of ( B ) produces an osmotic pressure ( P, ) then ( 0.05 M ) solution of ( A ) will produce an osmotic pressure, assuming that the electrolyte is completely ionised: A . ( 1.5 P ) в. ( P ) ( c .0 .5 P ) D. ( 0.75 P ) |
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312 | What is a de-icing agent? How does it work? |
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313 | The vapour pressure is a solvent decreased by ( 10 mathrm{mm} ) of mercuity when a non velocity was added to the solvent. The mole traction of the solve in the solution is ( 0.2 . ) What would be the mole traction of the solvent.if decrease in the vaspour pressure is t be ( 20 mathrm{mm} ) of mercurity? A. 0.8 B. 0.6 ( c cdot 0.4 ) ( D cdot 0.2 ) |
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314 | Molarity of the situation is depend on: A. temperature B. nature of solute dissolved c. mass of solvent D. pressure |
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315 | Wustration 2.136 A very small amount of a non-volatile solute (that does not dissociate) is dissolved in 56.8 cm of benzene (density 0.889 g cm-). At room temperature, vapour pressure of this solution is 98.88 mm Hg while that of benzene is 100 mm Hg. Find the molality of this solution. If the freezing temperature of this solution is 0.73 degree lower than that of benzene, what is the value of molal the freezing point depression constant of benzene? |
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316 | Molality of a solution in aqueous medium is ( 0.8 . ) Calculate its mole fraction and the percentage by mass of solute if molar mass of solute is 60 . A. ( 0.014,4.8 % ) В. ( 0.014,5 % ) c. ( 0.1,4.8 % ) D. ( 0.4,8 % ) |
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317 | When 100 g of a saturated solution is evaporated at ( 50^{circ} mathrm{C}, 50 mathrm{g} ) of solid is left over. Find the solubility of the substance at ( 50^{circ} mathrm{C} ) A . 100 B. 50 c. 75 D. 28 |
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318 | A 100 solution of ( N a_{2} C O_{3} ) is prepared by dissolved 8.653 of the salt in water. The density of the solution is ( 1.0816 / ) What are the Molarity and Molality of the solution? (Atomic mass of Na is 23 , e is 12 and of O is 14 ) |
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319 | Based on solute-solvent interactions, arrange the following in order of increasing solubility in n-octane and explain. Cyclohexane, ( boldsymbol{K} boldsymbol{C l}, boldsymbol{C H}_{3} boldsymbol{O H}, boldsymbol{C H}_{3} boldsymbol{C N} ) |
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320 | An aqueous solution is 1 molal in ( K I ) Which change will cause the vapour pressure of the solution to increase? A. Addition of ( N a C l ) B. Addition of ( N a_{2} S O_{4} ) c. Addition of 1 molal ( K I ) D. Addition of water |
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321 | State True or False. A binary solution which has same composition in liquid, as well as vapour phase, is called azeotropic mixture. A. True B. False |
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322 | 0.5 Faraday of electricity was passed to deposit all the copper present in ( 500 mathrm{m} ) of ( C u S O_{4} ) solution. What was the molarity of this solution? A. 1 м B. 0.5 M c. ( 0.25 mathrm{M} ) D. 2.5м |
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323 | Illustration 2.85 Define molal elevation constant or ebullioscopic constant. |
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324 | Isotonic solutions have: A. same boiling point B. same vapour pressure c. same melting point D. same osmotic pressure |
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325 | Which of the following conditions is not correct for ideal solution A. no change in volume on mixing B. no change in enthalpy on mixing c. it obeys Raoults law D. lonisation of solute should occurs to a small extent |
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326 | ( p H ) of a ( 0.1 mathrm{M} ) monobasic acid is measured to be ( 2 . ) Its osmotic pressure at a given temperature of ( boldsymbol{T} ) Kis: A . 0.1 RT в. 0.11 RТ c. ( 1.1 mathrm{RT} ) D. 0.01 RT |
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327 | Question 2. Calculate the mole fraction of benzene in solution containing 30% by mass in carbon tetrachloride. ( Concentration 30% by mass shows that 30 g C He is dissolved in 100 g solution or 70 g CCI. So, calculate the moles of each by dividing their mass with their molecular mass. (1) Then calculate the mole fraction by using the formula, Number of moles of the component Mole fraction of a component = = Total number of moles of all components A NA+ no |
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328 | Solid ( B eleft(N O_{3}right)_{2} ) is gradually dissolved in a ( 1.0 times 10^{-4} M N a_{2} C O_{3} ) solution. At what concentration of ( B a^{2+} ) will a percipitate begin to form? ( left(K_{S P} text { for } B a C O_{3}=5 times 10^{-9}right) ) A. ( 8.1 times 10^{-8} M ) в. ( 8.1 times 10^{-7} M ) c. ( 4.1 times 10^{-5} M ) D. ( 5.1 times 10^{-5} M ) |
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329 | The mole fraction of water in ( 20 % ) aqueous hydrogen peroxide solution is: A . 0.2 B. 0.8 ( mathbf{c} .0 .883 ) D. 0.117 |
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330 | Assertion Amalgam of mercury with sodium is an example of solid solutions Reason Mercury is solvent and sodium is solute in the solution A. Both Assertion and Reason are correct and Reason is the correct explanation for Assertion B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion C. Assertion is correct but Reason is incorrect D. Both Assertion and Reason are incorrect |
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331 | . 46 Give an example of a material used for making semipermeable membrane for carrying out reverse osmosis. ble motorial is used |
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332 | In a saturated solution the relative amount of solute when compared to the unsaturated solution. A. More B. Less c. Equal D. ( C, D ) |
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333 | 1. Pressure of 0.210 bat ar 37°C. The vapour pressure of pure liquid (vapour pressure of water at 37°C = 0.198 bar) in bar is a. 0.448 b. 44.8 c. 0.224 d. 2.24 |
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334 | ollowing factor(s)affect the solubility of a gaseous solute Q. 27 Which of the following factor(s)affect the in the fixed volume of liquid solvent? (i) Nature of solute (ii) Temperature (iii) Pressure (a) (i) and (iii) at constant T (b) (i) and (ii) at constant p (c) (ii) and (iii) (d) Only (iii) |
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335 | What is the sum of the mole fractions of all the components in a three component system? ( A ) B. 2 ( c cdot 3 ) ( D cdot 1 / 3 ) |
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336 | Two liquids ( A ) and ( B ) form ideal solutions. At ( 300 K ), the vapour pressure of solution containing 1 mole of ( A ) and 3 mole of ( B ) is 550 mm ( H g . A t ) the same temperature, if one more mole of ( B ) is added to this solution, the vapour pressure of the solution increases by 10 mm ( H g . ) Determine the vapour pressure of ( A ) and ( B ) in the pure ( operatorname{states}(operatorname{in} operatorname{mm} H g) ) A .400,600 B .500,500 ( mathbf{c} .600,400 ) D. None of these |
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337 | NLERI Q. 15 The values of van’t Hoff factors for KCL, N s for KCl, NaCl and K SO, respectively are (a) 2, 2 and 2 Ans. (h) Number (b) 2. 2 and 3 (d) 1, 1 and 1 (c) 1, 1 and 2 (c) 1, 1 and 2 off factors (1) |
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338 | The solubility of solutions which are neither exothermic nor endothermic increases with increase in temperature A. True B. False |
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339 | The molarity ( (M) ) of ( K M n O_{4} ) solution in basic medium is : ( mathbf{A} cdot 0.8 M ) в. ( 0.08 M ) c. ( 0.26 M ) D. ( 0.026 M ) |
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340 | The mole percentage of oxygen in a mixture of ( 7 g N_{2} ) and ( 8 g O_{2} ) is : A . 25 B. 75 c. 50 D. 40 |
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341 | Question 1. Define the term solution. How many types of solutions are formed? Write briefly about each type with an example. |
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342 | For an ideal solution with ( boldsymbol{p}_{boldsymbol{A}}>boldsymbol{p}_{boldsymbol{B}} ) which of the following is true? ( mathbf{A} cdotleft(x_{A}right)_{l i q}=left(x_{B}right)_{v a p} ) B . ( left(x_{A}right)_{l i q}>left(x_{B}right)_{v a p} ) C . ( left(x_{A}right)_{l i q}<left(x_{B}right)_{v a p} ) D. ( left(x_{A}right) ) liqand ( left(x_{B}right)_{v a p} ) do not bear any ralationship with each other |
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343 | AT ( 25^{circ} C, ) a solution containing 0.2 g of polyisobutylene in ( 100 mathrm{mL} ) of benzene developed a rise of ( 2.4 mathrm{mm} ) at osmotic equilibrium. The molar mass of polyisobutylene if the density of the solution is ( 0.88 mathrm{g} / mathrm{mL} ) is : A ( cdot 2.39 times 10^{5} g m o l^{-1} ) B . ( 7.36 times 10^{5} mathrm{g} ) mol ( ^{-1} ) c. ( 5.45 times 10^{5} g ) mol ( ^{-1} ) D. None of these |
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344 | Vapour pressure of a liquid increases with : A. decrease in temperature B. increase in temperature c. increase in surface area D. increase in volume |
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345 | Describes a solution containing solute particles of intermediate size that do not settle but do scatter light A. Miscible B. Suspension c. colloid D. Saturated E. Supersaturated |
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346 | Mustration 2.95 The boiling point of benzene is 353.22 K. When 1.80 g of a non-volatile solute was dissolved in 90, benzene, the boiling point is raised to 354.11 K. Calculate the molar mass of the solute. (K, for benzene is 2.53 K kg mol-1) |
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347 | Q. 7 Considering the formation, breaking and strength of hydrogen bond, predict which of the following mixtures will show a positive deviation from Raoult’s law? (a) Methanol and acetone (b) Chloroform and acetone (c) Nitric acid and water (d) Phenol and aniline Ans. (a) In pure methanol molecules are hydrogen bonded. On adding acetone, its molecules |
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348 | The vapour pressure of the solution of two liquids ( Aleft(P^{circ}=80 m mright) ) and ( Bleft(p^{circ}=120 m mright) ) is found to be ( 100 m m ) when ( x_{A}=0.4 . ) The result shows that: A. Solution exhibits ideal behaviour B. Solution shows positive deviations c. Solution shows negative deviations D. Solution will show positive deviations for lower concentration and negative deviations for higher concentrations |
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349 | Take small amounts of salt and add it to large amounts of water. ( X ) is formed. The substance present in small amount is called ( Y ) whereas the substance present in large amounts is called ( Z ) and the salt solution formed is called ( A ) The solution in which more of the solute can be dissolved at a given temperature is called ( B ) solution. The solution which cannot be dissolved any more of the solute at a given temperature is ( C ) solution. What is ( B ) ? A. Salt solution B. Unsaturated c. Saturated D. Super saturated solution |
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350 | A solution is prepaired by mixing ( 8.5 g ) of ( C H_{2} C l_{2} ) and ( 11.95 g ) of ( C H C l_{3} ). If vapour pressure of ( boldsymbol{C H}_{2} boldsymbol{C l}_{2} ) and ( C H C l_{3} ) at ( 4298 K ) are 415 and ( 200 m m H g ) respectively, the mole fraction of ( boldsymbol{C H C l}_{3} ) in vapour form is : (molar mass of ( left.boldsymbol{C l}=mathbf{3 5 . 5} boldsymbol{g} boldsymbol{m o l}^{-1}right) ) ( mathbf{A} cdot 0.162 ) B. 0.675 c. 0.325 D. 0.486 |
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351 | Example 2.27 The K. (25°C) of sparingly soluble salt XY,(s) is 3.56 x 10-5 (mol L-1)3 and at 30°C, the vapour pressure of its saturated solution in water is 31.78 mm of Ho Calculate the enthalpy change of the reaction XY,(s) = X2+(aq) + 2Y (aq) Given: Vapour pressure of pure water = 31.82 mm of Hg |
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352 | Illustration 2.45 Ethylene bromide C,H,Br2, and 1,2-dibromopropane, C H Br,, form a series of ideal solutions over the whole range of composition. At 85°C, the vapour pressure of these two pure liquids are 173 and 127 torr, respectively. a. If 10.0 g of ethylene bromide is dissolved in 80.0 g of 1,2-dibromopropane, calculate the partial pressure of each component and the total pressure of the solution at 85°C. b. Calculate the mole fraction of ethylene bromide in the vapour in equilibrium with the above solution. c. What would be the mole fraction of ethylene bromide in a solution at 85°C equilibrated with a 50 : 50 mole mixture in the vapour? |
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353 | Define an ideal solution and write one of its characteristics. |
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354 | Consider seperate solutions of ( mathbf{0 . 5 0 0} boldsymbol{M} boldsymbol{C}_{mathbf{2}} boldsymbol{H}_{mathbf{5}} boldsymbol{O H}(boldsymbol{a q}), mathbf{0 . 2 5 0} boldsymbol{M} boldsymbol{K} boldsymbol{B r} ) ( mathbf{0 . 1 2 5} boldsymbol{M} boldsymbol{N a _ { 3 }} boldsymbol{P O}_{4}(boldsymbol{a q}) ) and ( mathbf{0 . 1} boldsymbol{M} boldsymbol{M} boldsymbol{g}_{3}left(boldsymbol{P} boldsymbol{O}_{4}right)_{2} ) at ( mathbf{2 5}^{circ} boldsymbol{C} ) Which statement is true about these solutions, assuming all salts to be strong electrolytes? A ( cdot 0.125 M N a_{3} P O_{4}(a q) ) has the highest osmotic pressure B. ( 0.500 M C_{2} H_{5} O H(a q) ) has the highest osmotic pressure. C. They all have the same osmotic pressure. D. ( 0.100 M M g_{3}left(P O_{4}right)_{2}(a q) ) has the highest osmotic pressure |
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355 | gulo yuu. Question 12. State Henry’s law and mention some important applications? Henry’s law is, p x, State this in the form of statement and give its applications, like dissolution of Co, in soda water, less oxygen intake at high altitudes etc. |
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356 | What weight of the non-volatile solute urea ( left(N H_{2}-C O-N H_{2}right) ) needs to be dissolved in 100 g of water by ( 25 % ) ? (in ( g m) ) |
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357 | The vapour pressure of a pure liquid ( mathbf{A} ) is ( 80 mathrm{mmHg} ) at ( 300 K . ) It forms an ideal solution with liquid B. When the mole fraction of ( mathrm{B} ) is ( 0.4, ) the total pressure was to be ( 88 mathrm{mmHg} ). The vapour pressure of liquid B would be? |
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358 | How much ammonia 1 M solution of ammonium hydroxide contains? (in g) ( A cdot 35 g ) B. 17 g ( c cdot 348 ) D. None of these |
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359 | Depression of freezing point of which of the following solutions does represent the cryoscopic constant of water? A. ( 6 % ) by mass of urea in aqueous solution. B. 100 g of aqueous solution containing 18 g of glucose. c. 59 g of aqueous solution containing 9 g of glucose. D. 1 M ( K C l ) solution in water. |
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360 | A solution at ( 20^{circ} mathrm{C} ) is composed of 1.5 mol of benzene and 3.5 mol of toluene. If the vapour pressure of pure benzene of pure benzene and pure toluene at this temperature are 74.7 torr and 22.3 torr. respectively, then the total vapour pressure of the solution and the benzene mole fraction in equilibrium with it will be, respectively. A. 38.0 torr and 0.589 B. 30.5 torr and 0.389 c. 35.8 torr and 0.280 D. 35.0 torr and 0.480 |
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361 | What is the molarity of ( 11.2 V ) of ( H_{2} O_{2} ) ( ? ) ( mathbf{A} cdot mathbf{1} ) B. 2 ( c .5 .6 ) D. 11.2 |
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362 | Molecular mass of a non-volatile solute can be determined by which of the following method? A. cryoscopic method B. Victor-Meyer’s method c. Graham’s method D. Duma’s method |
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363 | The osmotic pressure of an aqueous solution of sucrose is 2.47 atm at ( 303 mathrm{K} ) and the molar volume of the water present is ( 18.10 mathrm{cm}^{3} . ) Given ( Delta H_{v a p}= ) ( mathbf{5 4 0} ) cal / g. Assume the volume of solvent equal to the volume of the solution. The elevation in the boiling point of the solution is : A ( .5 .145 times 10^{-2} ) B. ( 7.565 times 10^{-2} ) c. ( 6.355 times 10^{-2} ) D. None of these |
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364 | Calculate the mass in mole of ( C O_{2} ) that will dissolve in enough water to form ( 900 m L ) of solution at ( 20^{circ} mathrm{C} ) if the partial pressure of ( boldsymbol{C O}_{2} ) is 1 atm. ( boldsymbol{K}_{boldsymbol{H}} ) for ( C O_{2} ) is ( 2.3 times 10^{-2} ) mol ( / ) litre ( a t m ) A . 0.0401 mole B. 0.0301 mole c. 0.0217 mole D. 0.0207 mole |
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365 | Q. 14 Which of the following statements is false? (a) Two different solutions of sucrose of same molality prepared in different solvents will have the same depression in freezing point. (b) The osmotic pressure of a solution is given by the equation i = CRT (where, C is the molarity of the solution) (c) Decreasing order of osmotic pressure for 0.01 M aqueous solutions of barium chloride, potassium chloride, acetic acid and sucrose is BaCl, > KCI > CH,COOH > sucrose (d) According to Raoult’s law, the vapour pressure exerted by a volatile component of a solution is directly proportional to its mole fraction in the solution |
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366 | The solubility of solid in a liquid solution ( _{-1-} ) with a decrease in pressure. A . increases B. decreases c. remains same D. none of these |
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367 | The van’t Hoff factor for a dilute solution of ( boldsymbol{K}_{3}left[boldsymbol{F} boldsymbol{e}(boldsymbol{C} boldsymbol{N})_{6}right] ) is likely to be: A . 10 B. 4 ( c cdot frac{1}{4} ) D. |
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368 | Solubility of salt ( X ) in water is 32 at ( 30^{circ} ) C. Calculate the amount of solvent present in 500 g of saturated solution of ( X ) A. ( 160 mathrm{g} ) в. 379 g c. ( 460 mathrm{g} ) ( D cdot 68 g ) |
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369 | When a substance is dissolved in a solvent, the vapour pressure of solvent decrease. It brings This question has multiple correct options A. a decrcase in boilings point of solution B. an increase in boiling point of the solution c. a decrease in freezing point of the solution D. an increase in freezeing point of the solution |
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370 | Which of the following changes decreases the vapour pressure of water kept in a sealed vessel? A. Decreasing the quantity of water B. Increasing the quantity of water c. Decreasing the volume of vessel to one-half D. Decreasing the temperature of water |
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371 | 27 Calculate the mass per cent of calcium, phosphorus and oxygen in calcium phosphate Caz(PO4)2. |
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372 | At ( 10^{circ} mathrm{C}, ) the osmotic pressure of urea solution is 500 mm. The solution is diluted and the temperature is raised to ( 25^{circ} C, ) when the osmotic pressure is found to be 105.3 mm. Determine extent of dilution? A. Sol. ( left(V_{text {final}}=5 V_{text {original}}right) ) B. Sol. ( ( left.V_{text {final}}=7 V_{text {original}}right) ) c. sol. ( left(V_{text {final}}=3 V_{text {original}}right) ) D. None of the above |
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373 | A certain substance ‘A’ tetramerises in water to the extent of ( 80 % ). A solution of 2.5 g of ( A ) in 100 g of water lowers the freezing point by ( 0.3^{circ} mathrm{C} ). The molar mass of ( A ) is: A .122 B. 31 c. 244 D. 62 |
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374 | Two liquids ( A ) and ( B ) form ideal solutions. At ( 300 K ), the vapour pressure of a solution containing 1 mole of ( A ) and 3 moles of ( B ) is 550 mm Hg. At the same temperature, if one more mole of ( B ) is added to this solution, the vapour pressure of the solution increases by 10 mm ( H g ). The vapour pressure of ( A ) and ( B ) in their pure states are respectively: A ( cdot p_{A}^{o}=600 mathrm{mm} mathrm{Hg} ) and ( p_{B}^{o}=400 mathrm{mm} mathrm{Hg} ) B . ( p_{A}^{o}=500 mathrm{mm} mathrm{Hg} ) and ( p_{B}^{o}=560 mathrm{mm} mathrm{Hg} ) C ( cdot p_{A}^{o}=450 mathrm{mm} mathrm{Hg} ) and ( p_{B}^{o}=650 mathrm{mm} mathrm{Hg} ) D . ( p_{A}^{o}=400 mathrm{mm} mathrm{Hg} ) and ( p_{B}^{o}=600 mathrm{mm} mathrm{Hg} ) |
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375 | Which of the following statement is correct? A. Dilution increases the extent of deviation of ideality B. Dilution has no effect on deviation c. Dilution decreases the extent of deviation from ideality D. More concentrated the solution is, lesser will be the deviation |
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376 | ( 1 mathrm{kg} ) of ( mathrm{NaOH} ) solution contains ( 4 mathrm{g} ) of NaOH. The approximate concentration of the solution is: A. 0.1 molar B. 0.1 molal c. decinormal D. about 0.1 N |
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377 | Elevation in boiling point of ( boldsymbol{C a}left(boldsymbol{N} boldsymbol{O}_{3}right)_{2} ) gives molar mass as ( 131.2 . ) The degree of dissociation of ( boldsymbol{C a}left(boldsymbol{N} boldsymbol{O}_{3}right)_{2} ) is: A. ( 100 % ) B. ( 75 % ) ( c .50 % ) D. ( 12.5 % ) |
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378 | Find the amount of sodium nitrate dissolved in ( 200 g ) of solvent if the mass by mass percent of solute in solution is ( mathbf{2 0 %} ) A . ( 20 g ) в. ( 50 g ) c. ( 30 g ) D. ( 40 g ) |
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379 | 0.3 At equilibrium the rate of dissolution of a solid solute in a volatile liquid solvent is (a) less than the rate of crystallisation (b) greater than the rate of crystallisation (c) equal to the rate of crystallisation (d) zero |
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380 | ( 1.4 mathrm{g} ) of acetone dissolved in ( 100 mathrm{g} ) of benzene gave a solution which freezes at ( 277.12 mathrm{K} . ) Pure benzene freezes at ( 278.4 mathrm{K} .2 .8 mathrm{g} ) of a solid (A) dissolved in ( 100 mathrm{g} ) of benzene gave a solution which froze at ( 277.76 mathrm{K} ). Calculate the molar mass of ( (A) ) |
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381 | Vapour pressure of a solvent containing nonvolatile solute is A. more than the vapour pressure of a solvent B. less than the vapour pressure of solvent C. equal to the vapour pressure of solvent D. none |
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382 | Q. 35 Colligative properties are observed when …….. (a) a non-volatile solid is dissolved in a volatile liquid (b) a non-volatile liquid is dissolved in another volatile liquid (c) a gas is dissolved in non-volatile liquid (d) a volatile liquid is dissolved in another volatile liquid |
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383 | The vapor pressure of water is ( 12.3 K P a ) at ( 300 K . ) Calculate the vapor pressure of 1 molal solution of a non- volatile solute in it. |
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384 | Q Type your question- account for this effect we define a quantity called the Van’t Hoff factor given by : [ boldsymbol{i}= ] Actual number of particles in solution Number of formula units initiall ( i=1 ) (for non-electrolytes) ( i>1 ) (for non-electrolytes, undergoing dissociation) ( i<1 ) (for solutes, undergoing dissociation) Answer the following questions: |
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385 | The van’t Hoff factor of the benzoic acid solution in benzene is ( 0.5 . ) In this solution, benzoic acid: A. dissociates B. forms dimer c. remains unchanged D. forms tetramer |
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386 | The osmotic pressure of ( 40 % ) (weight/volume) urea solution is 1.64 ( operatorname{atm} ) and that of ( 3.42 % ) (weight/volume) cane sugar is 2.46 atm. When equal volumes of the above two solutions are mixed, the osmotic pressure of the resulting solution is: A. 1.64 atm B. 2.46 atm c. 4.10 atm D. 2.05 atm |
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387 | The Henry’s law constant for the solubility of ( N_{2} ) gas in water at ( 298 mathrm{K} ) is ( 1 times 10^{5} ) atm. The mole fraction of ( N_{2} ) in air is ( 0.8 . ) The number of moles of ( N_{2} ) from a dissolved in 100 moles of water at ( 298 mathrm{K} ) and 5 atm pressure is? A. ( 4 times 10^{-4} ) В. ( 4 times 10^{-5} ) c. ( 4 times 10^{-3} ) D. ( 5 times 10^{-4} ) |
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388 | 0.5 Maximum amount of a solid solute that can be dissolved in a specified amount of a given liquid solvent does not depend upon ……… (a) temperature (b) nature of solute (c) pressure (d) nature of solvent unt of given |
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389 | A current of ( 965 A ) is passed for 100 sec between inert electrodes in ( 500 m L ) solution of ( 2 M C u S O_{4} . ) The molarity of solution after electrolysis would be: (Assume no change in volume) A ( .2 M ) в. ( 1 M ) c. ( 4 M ) D. ( 0.5 M ) |
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390 | Consider following cases: I. ( 2 mathrm{M} C H_{3} mathrm{COOH} ) solution in benzene at ( 27^{0} ) where there is dimer formation to the extent of ( 100 % ) Il. ( 0.5 mathrm{M} ) KCl aq. solution at ( 27^{0}, ) which ionises ( 100 % ) Which is lare true statements(s): A. both are isotonic B. I is hypertonic c. I lis hypertonic D. none is correct |
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391 | Two solutions of glucose have osmotic pressures 1.5 and ( 2.5 a t m .1 L ) of first is mixed with ( 2 L ) of second solution, the osmotic pressure of the resultant solution is: A . ( 2.5+1.5 a t m ) B. 2.5 – 1.5atm c. ( frac{2.5+1.5}{2} ) at D. ( 2.16 a t m ) |
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392 | Which facts are true when we use van’t Hoff equation ( P V=C S T ) for osmotic pressure ( mathrm{P} ) of dilute solutions? This question has multiple correct options A. The equation is identical to that of ideal gas equation B. The solute particles in solution are analogous to the gas molecules and the solvent is analogous to the empty space between the gas molecules C. Solute molecules are dispersed in the solvent, the way the gas molecules are dispersed in empty space D. The equation is not identical to that of ideal gas equation |
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393 | Illustration 2.214 Calculate the Van’t Hoff factor (i) for the following if: i. 100% ionization or association takes place ü. 50% ionization or association takes place a. S b. Se с. Те d. P e. As f. Sb g. B h. AICI, i. Hg, Cl, j. HgCl, k. Be2C 1. A1.Cz m. CaC, n. Mg,C, |
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394 | Under what condition the van’t Hoff factor is greater than one? |
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395 | The molarity of ( boldsymbol{H} boldsymbol{N} boldsymbol{O}_{3} ) in a sample which has density ( 1.4 mathrm{g} / mathrm{mL} ) and mass percentage of ( 63 % ) is [Molecular Weight of ( left.boldsymbol{H} boldsymbol{N} boldsymbol{O}_{3}=boldsymbol{6 3}right] ) |
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396 | Solutions that have the same osmotic pressure are called (isotonic/isometric) solutions |
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397 | Calculate the vapour pressure lowering caused by addition of 50 g of sucrose (molecular mass ( =342 ) ) to 500 g of water if the vapour pressure of pure water at ( 25^{circ} mathrm{C} ) is ( 23.8 mathrm{mm} mathrm{Hg} ) |
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398 | Super heating is minimized by stirring and indirect ( _{—} ) (heating/cooling) | 12 |

399 | Molar ratio of a mixture of water and absolute alcohol is ( 0.2 . ) The mole fraction ratio of alcohol and water is : |
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400 | Calculate the weight of ( C a O ) required to remove the hardness of 1000000 litre of water containing 1.62 g of ( C a C O_{3} ) per litre. |
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401 | Choose the correct statement from the following. This question has multiple correct options A. Liquor ammonia and soda water are examples of liquid-gas type mixtures. B. Mixture of coconut oil and water can be separated using separating funnel C. A mixture of iodine and sulphur can be separated using magnetic separation. D. A mixture of sand and sawdust can be separated using solvent extraction. |
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402 | In a glass of water, we cannot dissolve sugar more than a certain limit. At this stage, the solution is said to be: A. saturated B. unsaturated c. supersaturated D. complete solution |
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403 | Question 1. Components of a binary mixture of mponents of a binary mixture of two liquids A and B were being separated by distillation. After some time separation of components stopped and composition of vapour phase became same as that of liquid phase. Both the components started coming in the distillate. Explain why this happened. the distillate and |
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404 | A solution of urea (mol. mass 56 ( left.g m o l^{-1}right) ) boils at ( 100.18^{circ} C ) at the atmospheric pressure. If ( boldsymbol{K}_{f} ) and ( boldsymbol{K}_{boldsymbol{b}} ) for water are 1.86 and 0.52 Kkg.mol( ^{-1} ) respectively, the above solution will freeze at: A. ( -6.54^{circ} ) B. ( 6.54^{circ} mathrm{C} ) ( c cdot 0.654^{circ} C ) D. ( -0.654^{circ} mathrm{C} ) |
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405 | Benzoic acid undergoes dimerisation in benzene solution.The vant Hoff factor is related to the degree of association ( alpha^{prime} ) of the acid as : A ( . i=1-alpha ) B . ( i=1+alpha ) C ( i=1-frac{alpha}{2} ) D. ( i=1+frac{alpha}{2} ) |
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406 | Which of the following cannot be dissolved in water? A . Ice B. Sugar c. wood D. salt |
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407 | Calculate the mole fraction of ( N_{2} ) gas in a mixture of ( N_{2} ) and ( O_{2} ). If the partial pressure of ( boldsymbol{O}_{2} ) is ( 63 mathrm{cm} ) of ( mathrm{Hg} ) and the total pressure of the mixture is ( 90 mathrm{cm} ) of Hg. |
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408 | The incorrect statement is : A. Vapour pressure of a liquid always increases by increasing temperature. B. Vapour pressure onlydepends on temperature and not on the nature of substance. C. Vapour pressure does not depend on the quantity of the liquid taken and the surface area of the liquid. D. Vapour pressure is not a colligative property & is independent of the concentration of the liquid. |
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409 | An aqueous solutions of diabasic acid (molecular mass ( =118 ) ) containing ( 35.4 mathrm{g} ) of acid per litre of the solution has density ( 1.0077 g m L^{-1} ). Find the mole fraction of the solvent. |
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410 | The Molarity of ( 200 m l ) of ( H C l ) solution which can neutralise ( 1.6 g ) of anhydrous ( N a_{2} C O_{3} ) is: ( mathbf{A} cdot 1 M ) B. ( 0.1 M ) c. ( 0.6 M ) D. ( 0.75 M ) |
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411 | Example 2.9 A4% solution of sucrose C,H,O,, is isotonic with 3% solution of an unknown organic substance. Calculate the molecular mass of the unknown substance. |
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412 | Ratio of solubilities of gases ( N_{2} & O_{2} ) in water from air at ( 25^{circ} ) and 1 atm will be if air is ( 20 % ) by volume of ( O_{2} ) and ( 80 % ) by volume of ( N_{2} ) is: [ begin{array}{c} text { Given }: boldsymbol{K}_{boldsymbol{H}}left(boldsymbol{N}_{mathbf{2}}right)=mathbf{2} times mathbf{1 0}^{mathbf{4}} boldsymbol{a} boldsymbol{t} boldsymbol{m} \ boldsymbol{K}_{boldsymbol{H}}left(boldsymbol{O}_{2}right)=mathbf{1 0}^{4} boldsymbol{a} boldsymbol{t} boldsymbol{m} end{array} ] ( A cdot 8: 1 ) B. 1: 8 c. 2: 1 D. 1: 2 |
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413 | 8. Equimolal solutions KCl and compound X in water show depression in freezing point in the ratio of 4:1. Assuming KCI to be completely ionized, the compound X in solution must a. Dissociate to the extent of 50% b. Hydrolyze to the extent of 80% c. Dimerize to the extent of 50% d. Trimerize to the extent of 75% |
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414 | For a given value of the degree of dissociation ( (alpha), ) which of the following have correct van’t Hoff factor? This question has multiple correct options A. ( N a C l ; i=2+alpha ) в. ( C aleft(N O_{3}right)_{2} ; i=1+2 alpha ) c. ( K_{4}left[left(F e(C N)_{6}right] ; i=1+4 alpharight. ) D. ( left(N H_{4}right)_{3} P O_{4} ; i=3+alpha ) |
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415 | If the above process is repeated for all other compositions of mixture of ( mathrm{C} ) and B. If all the points where vapours start converting into liquid are connected and all the points where vapours get completely converted into liquid are connected then obtained graph will look like ( A ) B. b- ( c cdot c ) ( D cdot d ) |
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416 | A 0.001 molal solution of ( left[boldsymbol{P t}left(boldsymbol{N} boldsymbol{H}_{3}right)_{4} boldsymbol{C l}_{4}right] ) in water has a freezing point depression of ( 0.0054^{0} C . ) If ( K_{f} ) for water is ( 1.80, ) the correct formulation of the above molecule is: ( mathbf{A} cdotleft[P tleft(N H_{3}right)_{4} C l_{3}right] C l ) B . ( left[P tleft(N H_{3}right)_{4} C l_{2}right] C l_{2} ) c. ( left[P tleft(N H_{3}right)_{4} C l_{2}right] C l_{3} ) D ( cdotleft[P tleft(N H_{3}right)_{4} C l_{4}right] ) |
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417 | 2.5 molar sulphuric acid contains: This question has multiple correct options A. ( 29.5 mathrm{g} ) of sulphuric acid per litre of solution. B. ( 245.0 mathrm{g} ) of sulphuric acid per ( 1000 mathrm{ml} ) of solution. C. ( 24.5 mathrm{g} ) of sulphuric acid per ( 100 mathrm{ml} ) of solution. D. 59.0 g of sulphuric acid per litre of solution. |
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418 | mum boiling azeotrope at some specinc (b) 2.28 IT two liquids A and B form minimum boiling azeotro composition then A B interactions are stronger than those between A-A or B apour pressure of solution increases because more number on liquids A and B can escape from the solution (C) vapour pressure of solution decreases because less number of molecules one of the liquids escape from the solution (d) A-B interactions are weaker than those between A-A or B-B because more number of molecules of ses because less number of molecules of only |
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419 | Which choice is a gas which has a low solubility in water? A ( cdot N H_{3} ) в. ( C s H ) c. ( C H_{4} ) D. ( G a H_{3} ) |
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420 | 0.002 molar solution of NaCl having degree of dissociation of ( 90 % ) at ( 27^{circ} C ) has osmotic pressure equal to A. 0.94 bar B. 9.4 bar c. 0.0934 bar D. ( 9.4 times 10^{-4} ) bar |
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421 | Illustration 2.111 1.4 g of acetone dissolved in 100 g of benzene gave a solution which freezes at 277.12 K. Pure benzene freezes at 278.4 K. 2.8 of solid (A) dissolved in 100 g of benzene gave a solution which froze at 277.76 K. Calculate the molecular mass of (A). |
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422 | The molar conductivity of acetic acid at infinite dilution is 390.7 and for ( 0.1 mathrm{M} ) acetic acid solution is ( 5.2 mathrm{mhocm}^{2} ) mol ( -1 . ) The degree of dissociation of ( 0.1 mathrm{M} ) ( mathrm{CH}_{3} mathrm{COOH} ) solution is: A . ( 13.3 % ) B. 0.0133% c. 1.33% D. 133% |
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423 | The vapour pressure of pure benzene at a certain temperature is 640 mm ( H g ). A non-volatile solid weighing ( 2.715 g ) is added to ( 39.0 g ) of benzene. The vapour pressure of the solution is |
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424 | Match the following: List – List – II 1) Molality A) unity 2) Relative B) dilute solutions vapour lowering 3) Raoult’s law C) independent of temperature 4) ( X_{text {solute}} X_{text {solvent}} ) D) Mole fraction of solute ( mathbf{A} cdot 1-C, 2-D, 3-B, 4-A ) B . ( 1-A, 2-C, 3-D, 4-B ) C ( .1-C, 2-B, 3-A, 4-D ) D . ( 1-D, 2-A, 3-B, 4-C ) |
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425 | The solubility of gas in liquid is directly proportional to the pressure over the solutions at a given temperature. A. True B. False |
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426 | ( mathbf{A} ) is a mixture of two or more substances in a single phase. A. Element B. Compound c. Solution D. None of above |
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427 | Question 9. What is semipermeable membrane? | 12 |

428 | The boiling point of ( 95 % ) ethanol is higher than that of absolute ethanol. A. True B. False |
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429 | What is the mole fraction of the solution in a ( 1.00 m ) aqueous solution? A. 1.770 B. 0.0354 c. 0.0177 D. 0.177 |
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430 | Which one is true for solutions showing positive deviation from raoult’s law? A. A-B interaction has nothing to do with positive deviations B. A-B interactions are weaker than than those between A-A and B-B C. A-B interactions are stronger than those between A-A and B-B D. A-B interactions are same as those between A-A and B- ( B ) |
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431 | The value of Henry’s law constant for some gases at ( 293 K ) is given below. Arrange the gases in the increasing order of their solubility. ( boldsymbol{H} boldsymbol{e}= ) ( mathbf{1 4 4 . 9 7 k b a r} ; mathbf{H}_{mathbf{2}}=mathbf{6 9 . 1 6 k b a} ) ( N_{2}=76.48 k b a r ; O_{2}=34.86 k b a r ) A. ( H e<N_{2}<H_{2}<O_{2} ) B. ( O_{2}<H_{2}<N_{2}<H e ) c. ( H_{2}<N_{2}<O_{2}<H e ) D. ( H e<O_{2}<N_{2}<H_{2} ) |
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432 | Hlustration 2.44 A liquid mixture of benzene and toluene is composed of 1 mol of benzene and 1 mol of toluene. a. If the pressure over the mixture at 300 K is reduced, at what pressure does the first vapour form? b. What is the composition of the first trace of vapour formed? c. If the pressure is reduced further, at what pressure does the last trace of liquid disappear? d. What is the composition of the last trace of liquid? e. What will be the pressure, the composition of the liquid, and the composition of the vapour, when 1 mol of the mixture is vapourized? Given: Prº = 32.05 mm Hg, PR° = 103 mm Hg |
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433 | Assuming the compounds to be completely dissociated in aqueous solution, identify the pair of the solutions that can be expected to be isotonic at the same temperature. A . ( 0.1 mathrm{M} ) Urea and ( 0.01 mathrm{M} ) Nac B. 0.02 M NaCl and 0.01 M ( N a_{2} S O_{4} ) D. 0.01 M Sucrose and 0.02 M glucose |
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434 | Q. 14 Which of the following statements is false? (a) Two different solutions of sucrose of same molality prepared in different solvents will have the same depression in freezing point. (b) The osmotic pressure of a solution is given by the equation t = CRT (where, C is the molarity of the solution) | (c) Decreasing order of osmotic pressure for 0.01 M aqueous solutions of barium chloride, potassium chloride, acetic acid and sucrose is BaCl, > KCI > CH2COOH > sucrose (d) According to Raoult’s law, the vapour pressure exerted by a volatile component of a solution is directly proportional to its mole fraction in the solution CAFE |
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435 | Question 5. What is the significance of Henry’s law constant Ky? | 12 |

436 | The ratio of the value of any colligative property for ( N a C l ) solution of that of an equimolal solution of sugar is nearly ( mathbf{2}: mathbf{1} ) A. True B. False |
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437 | The molality of ( boldsymbol{H}_{2} boldsymbol{S} boldsymbol{O}_{4} ) solution is ( boldsymbol{9} ). The weight of the solute in ( 1 mathrm{kg} H_{2} S O_{4} ) solution is: A . ( 900.0 mathrm{g} ) в. ( 469 mathrm{g} ) c. ( 882.0 mathrm{g} ) D. ( 9.0 mathrm{g} ) |
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438 | Which of the following is NOT soluble in water? A. Salt B. Sugar c. oxygen D. None of these |
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439 | Which of the following solutions at the same temperature will be isotonic? A. ( 3.42 mathrm{g} ) of cane sugar in one litre water and ( 0.18 mathrm{g} ) of glucose in one litre water B. 3.42 of cane sugar in one litre water and 0.18 g of glucose in 0.1 litre water c. ( 3.42 mathrm{g} ) of cane sugar in one litre water and ( 0.585 mathrm{g} ) of NaCl in one litre water D. 3.42 g of cane sugar in one litre water and 1.17 g of NaCl in one litre water |
12 |

440 | For an ideal solution, ( Delta_{m i x} H ) is | 12 |

441 | Example 2.3 The vapour pressure of a 5% aqueous solution of a non-volatile organic substance at 373 K is 745 mm. Calculate the molecular mass of the solute. |
12 |

442 | A 3.4 g sample of ( mathrm{H}_{2} mathrm{O}_{2} ) solution containing ( x % mathrm{H}_{2} mathrm{O}_{2} ) by mass requires ( mathrm{x} ) ( mathrm{ml} ) of a ( mathrm{KMnO}_{4} ) solution for complete oxidation under acidic condition. The molarity of ( mathrm{KMnO}_{4} ) solution is : ( A ) B. 0.5 ( c cdot 0.4 ) D. 0.2 |
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443 | The osmotic pressure of ( 0.1 mathrm{M} ) aqueous solution of ( M g C l_{2} ) at ( 300 mathrm{K} ) is ( 4.92 mathrm{atm} ) What will be the percentage ionization of the salt? A . ( 49 % ) B. ( 29 % ) ( c .39 % ) D. ( 69 % ) |
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444 | Mixtures on separation can give A. elements B. compounds c. both elements and compounds D. impure substances |
12 |

445 | The correct relationship between the boiling points of very dilute solutions of ( A l C l_{3}left(t_{1}right) ) and ( C a C l_{2}left(t_{2}right), ) having the same molar concentration, is : A ( cdot t_{1}=t_{2} ) В. ( t_{1}>t_{2} ) c. ( t_{2}>t_{1} ) D. ( t_{2} geq t_{1} ) |
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446 | Molarity is expressed as: A. Gram/litre B. Moles/litre c. Litre/mole D. Moles/1000 gms |
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447 | , (d) and L) both are correct. Q. 28 Intermolecular forces between two benzene mo strength as those between two toluene molecule benzene and toluene, which of the following are not (a) Amix H = zero (b) Amix V = zero (c) These will form minimum boiling azeotrope (d) These will not form ideal solution nzene molecules are nearly of same lene molecules. For a mixture of ng are not true? |
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448 | Illustration 2.123 How many grams of sucrose (molecular weight 342) should be dissolved in 100 g water in order to produce a solution with 105°C difference between the freezing point and the boiling point? (K = 0.51°C m-1,K, = 1.86°C m-1) |
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449 | Calculate the mole fraction of benzene in solution containing ( 30 % ) by mass in ( boldsymbol{C C l}_{4} ? ) |
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450 | What are isotonic solutions? Give an example. |
12 |

451 | A mixture of two immiscible liquids at a constant pressure of 1.0 atm boils at temperature A. Equal to the normal boiling point of more volatile liquid B. Equal to the mean of the normal boiling points of two liquids. C. Greater than normal boiling point of either of liquids. D. Smaller than the normal boiling point of either of liquids. |
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452 | Relative decrease in vapor pressure is 0.4 for a solution containing 1 mole AB in 3 mol ( H_{2} O ), therefore ( A B ) is ionised at the extent(percentage) of: ( mathbf{A} cdot 60 % ) B. ( 50 % ) ( c cdot 100 % ) D. ( 40 % ) |
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453 | One litre of ( C O_{2} ) ia passed through red hot coke. The volume become 1.4 litres at same temperature and pressure The composition of product is A. 0.8 litre of ( C O_{2} ) and 0.6 litre of ( C O ) B. 0.7 litre of ( C O_{2} ) and 0.7 litre of ( C O ) c. 0.6 litre of ( C O_{2} ) and 0.8 litre of ( C O ) D. 0.4 litre of ( C O_{2} ) and 1.0 litre of ( C O ) |
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454 | In a mixture A and B components show negative deviation as: ( mathbf{A} cdot Delta V_{m i x}=+v e ) B. ( Delta H_{text {mix}}=- )ve. C. A-B interaction is weaker than A-A and B-B interaction. D. None of the above reason is correct. |
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455 | Illustration 2.210 The freezing point of a 0.08 molal solution of NaHSO, is -0.372°C. Calculate the dissociation constant for the reaction. HSO = H® + s0,2- K, for water = 1.86 Km-1 |
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456 | Molarity is defined as: A. the number of moles of solute dissolved in one ( d m^{3} ) of the solution. B. the number of moles of solute dissolved in ( 1 mathrm{kg} ) of solvent C. the number of moles of solute dissolved in ( 1 d m^{3} ) of the solvent. D. the number of moles of solute dissolved in 100 ml of the solvent. |
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457 | The vapour pressure of a solvent decreased by ( 10 mathrm{mm} ) of mercury when a non-volatile solute was added to the solvent. The mole fraction of the solute in the solution is 0.2. What should be the mole fraction of the solvent if the decrease in the vapour pressure is to be ( 20 mathrm{mm} ) of mercury? A. 0.4 B. 0.6 ( c cdot 0.8 ) ( D cdot 0.2 ) |
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458 | Solute ( A ) is a ternary electrolyte and solute B is a non-electrolyte. If ( 0.1 mathrm{M} ) solution of solute B produces an osmotic pressure of ( 2 P, ) then 0.05 M solution of ( A ) at the same temperature will produce an osmotic pressure equal to: A . ( 1.5 P ) B. 2P ( c cdot 3 P ) D. |
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459 | Illustration 2.162 3% solution of glucose is isotonic with 1% solution of non-volatile non-electrolyte solute. The molecular mass of the solute would be a. 180 b. 160 c. 120 d. 60 |
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460 | The vapour pressure of a liquid decreases by 10 tor ( r ) when a nonvolatile solute is dissolved. The mole fraction of the solute in solution is 0.1 What would be the mole fraction of the liquid if the decrease in vapour pressure is 20 tor ( r, ) the same solute being dissolved? A . 0.2 B. 0.9 ( c .0 .8 ) D. 0.6 |
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461 | Mass and percentage by weight do not change with temperature. A. True B. False |
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462 | The solubility of gases in water is proportional to pressure and ( _{-}—- ) proportional to temperature. A. directly B. inversely C . directly, inversely D. inversely, directly |
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463 | 4 A beaker contains a solution of substance ‘A’. Precipitation of substance A takes place when small amount of ‘A’ is added to the solution. The solution 15 ……… (a) saturated (b) supersaturated (c) unsaturated (d) concentrated Thinking Process This problem includes concept of saturated unsaturated, supersaturated and concentrated solution. (b) When solute is added to the solution three |
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464 | Two samples of HCl of ( 1.0 mathrm{M} ) and ( 0.25 mathrm{M} ) are mixed. Find volumes of these samples taken in order to prepare 0.75 M HCI solution. Assume no water is added. (1) ( 20 mathrm{mL}, 10 mathrm{mL} ) (III) ( 100 mathrm{mL}, 50 mathrm{mL}(mathrm{III}) ) ( 40 mathrm{mL}, 20 mathrm{mL}(mathrm{IV}) 50 mathrm{mL}, 25 mathrm{mL} ) A . ।, ॥।, IV B. ।, ॥ c. ॥, ॥ा, । v D. I, II, III, IV |
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465 | Higher is the (mass/volume) of solute in a solution lower is its vapour pressure. |
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466 | Illustration 2.35 100 g of water contains 1.0 g urea and 2.0 g sucrose at 298 K. The vapour pressure of water at 298 K is 0.3 atm. Calculate the vapour pressure of the solution. (Molecular weight of urea = 60; Molecular weight of sucrose = 342) |
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467 | Illustration 2.191 When cells of skeletal vacuoles of a frog were placed in a series of NaCl solutions of different concentration solution at 25°C, it was observed microscopically that they remained unchanged in 0.7% solution, shrank in a more concentrated and swelled in more dilute solutions. Water freezes from the 0.7% salt solutions at -0.406°C. What is the osmotic pressure of the cell cytoplasm at 25°C. (K= 1.86 kg mol-1 K) |
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468 | 3 grams of salt of molecular weight 30 is dissolved in 250 g of water. Find the molality of the solution.(Multiply the answer by 10 ) |
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469 | The azeotropic mixture of water (boiling point ( =100^{circ} mathrm{C} ) ) and ( H C l ) (boiling point ( left.=85^{circ} mathrm{C}right) ) boils at about ( 110^{circ} mathrm{C} . ) During distillation of this mixture, it is possible to obtain: A. pure ( H C l ) B. pure ( H_{2} O ) c. pure ( H C l ) as well as ( H_{2} O ) D. neither pure ( H_{2} O ) nor pure ( H C l ) |
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470 | ( 5 % ) solution of cane sugar is isotonic with ( 0.877 % ) of ( X . ) The molecular weight of substance ( boldsymbol{X} ) is: A . 126.98 B. 119.96 c. 95.5 D. 59.98 |
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471 | According to Henry’s law, the solubility of a gas in a given volume of liquid increases with increase in : A. temperature B. pressure c. both A and B D. none of the above |
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472 | The magnitude of colligative properties in all colloidal dispersions is than solution. A. lower B. higher c. Both D. None of the above |
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473 | 8. The vapour pressure of a solution containing 5.0 g of a non- electrolyte in 100.0 g of water at a particular emperature is 2985 Nm-2. If the vapour pressure of pure water is 3000 N m-2, the molecular weight of the solute is a. 60.0 b. 120.0 c. 180.0 d. 380.0 |
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474 | The normal boiling of water is ( 373 K ) Vapour pressure of water at temperature ( boldsymbol{T} ) is ( 19 mathrm{mm} ) Hg. If enthalpy of evaporation is ( 40.67 k J / m o l, ) then temperature ( boldsymbol{T} ) would be: (Use ( log 2=mathbf{0 . 3}, boldsymbol{R}=mathbf{8 . 3} boldsymbol{J} boldsymbol{K}^{-1} mathbf{)} ) |
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475 | The azeotropic solution of two miscible liquids: This question has multiple correct options A. Can be seperated by simple distillation B. May show positive or negative deviation from Raoult’s law C . Are supersaturated D. Behave like single pure component and boil at a fixed temperature |
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476 | When 45 gm of a solute is added to 900 ( mathrm{gm} ) of water, its vapour pressure decreased from ( 30 mathrm{mm} ) to ( 24 mathrm{mm} ). The mole fraction of the solvent in the solution is : A . 0.2 B. 0.8 ( c .0 . ) D. 0.9 |
12 |

477 | Assertion Perfectly ideal solution is not possible with respect to binary solution of two liquids. Reason No two substances can have exactly the same nature of intermolecular forces and also of the same magnitude. A. Both Assertion and Reason are correct and Reason is the correct explanation for Assertion B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion c. Assertion is correct but Reason is incorrect D. Assertion is incorrect but Reason is correct |
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478 | Pick out the correct statements This question has multiple correct options A. The ratio of vapour pressure over solution phase on mixing two immiscible liquids is equal to ratio of their moles in vapour phase B. The ratio of vapour pressure over solution phase on mixing two miscible liquids is equal to ratio of their moles in liquid phase C. The ratio of vapour pressure over solution phase on mixing two miscible liquids is equal to ratio of the product of their vapour pressure and their moles fraction in a liquid phase D. The ratio of vapour pressure over solution phase on mixing two miscible liquids is equal to ratio of the product of their vapour pressure and their mole fraction in vapour phase |
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479 | toppr Q Type your question are taken in ( A ) and ( B ). How many of the following statement(s) is/are correct? ( mathbf{P}_{X}^{0}=mathbf{2 0 0} ) tor ( r ) ( mathbf{P}_{Y}^{0}=mathbf{5 0} ) tor ( r ) (i) If ( mathrm{NaCl} ) is added to vessel ( mathrm{B} ), the lowering of vapour pressure takes place. (ii) If glucose is added to vessel ( A, ) the boiling point of the solution increases. (iii) If the valve connecting ( A ) and ( B ) is opened, then ( mathbf{P}_{T} ) in both the vessel becomes equal and is given by Raoult’s law. (iv) After opening the valve, the level of liquid in both the container decreases (even a slight decrease is to be considered) (v) After opening the valve, the final pressure in vessel B is more than 50 torr. (vi) After opening the valve, the final pressure in vessel ( A ) is more than 200 torr ( A cdot 2 ) B. 3 ( c ) ( D ) |
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480 | The melting points of most of the solid substances increase with an increase of pressure acting on them. However, ice melts at a temperature lower than its usual melting point, when the pressure increases. This is because: A. ice is less denser than water B. pressure generates heat C. the bounds break under pressure D. ice is not a true solid |
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481 | A drop ( (0.05 mathrm{mL}) ) of ( 12.0 mathrm{M} ) HCl is spread over a sheet of thin aluminium foil. Assuming that the acid dissolves through the foil, the area is ( x times ) ( 10^{-1} mathrm{cm}^{2} ) of the hole produced, then ( x ) is : (Density of ( A l=2.70 g c m^{-3} ) thickness of the foil ( =0.10 mathrm{mm} ) |
12 |

482 | Calculate the amount of oxygen at 0.20 atm dissolved in 1 kg of water at 293 K. The Henry’s law constant for oxygen is ( 4.58 times 10^{4} ) atmosphere at ( 293 mathrm{K} ) ( mathbf{A} cdot 7.07 times 10^{-6} mathrm{kg} ) В. ( 7.27 times 10^{-6} mathrm{kg} ) C ( .7 .57 times 10^{-6} mathrm{kg} ) D. ( 7.77 times 10^{-6} mathrm{kg} ) |
12 |

483 | What is saturated solution explain with one example? | 12 |

484 | A mixture of two immiscible liquids nitrobenzene and water boiling at ( 99^{circ} C ) has a partial pressure of water ( 733 mathrm{mm} ) and of nitrobenzene ( 27 mathrm{mm} ). The ratio of masses of water and nitrobenzene in mixture is : |
12 |

485 | Calculate the mass of compound (molar mass ( =256 g m o l^{-1} ) ) to be dissolved in ( 75 g ) of benzene to lower its freezing point by ( 0.48 Kleft(K_{f}=5.12 K k g m o l^{-1}right) ) |
12 |

486 | Two glass bulbs of internal volume 0.5 and ( 0.2 L ) respectively are connected by a narrow tube of negligible volume. The pressure of air in the vessel is ( 75 mathrm{cm} ) at ( 17^{circ} mathrm{C} . ) The smaller bulb is immersed in melting ice and the larger bulb in boiling water. Calculate final pressure in the bulbs neglecting the expansion of glass. |
12 |

487 | Azeotropic mixtures? A. Boil at different temperatures B. Are mixtures of solids C . Are constant boiling mixtures D. None of the above |
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488 | 1 ( g ) of same non volatile solute is added to ( 100 g ) o two different solvents ( A ) and ( B ) ( boldsymbol{K}_{boldsymbol{b}} ) of ( boldsymbol{A}: boldsymbol{B}=mathbf{1}: mathbf{5} ) find out ( frac{left(Delta T_{b}right)_{A}}{left(Delta T_{b}right)_{B}} ) ( mathbf{A} cdot 1: 10 ) B. 1: 5 c. 1: 20 D. 2: 5 |
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489 | The depression in freezing point for ( 1 mathrm{M} ) urea, 1 M glucose and 1 M ( N a C l ) are in the ratio: A. 1: 2: 3 B. 3: 2: 2 ( mathrm{c} cdot 1: 1: 2 ) D. 2: 3: 2 |
12 |

490 | 2.82 ( mathrm{g} ) of glucose is dissolved in 30 g of water. The mole fraction of glucose in the solution is: A . 0.01 B. 0.99 c. 0.52 D. 1.66 |
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491 | A ( 5 % ) solution of cane sugar ( (text { mol. } boldsymbol{w} boldsymbol{t}= ) 342) is isotonic with ( 1 % ) solution of substance ( X . ) The molecular weight of ( boldsymbol{X} ) is: A . 34.2 B. 171.2 ( c .68 .4 ) D. 136.8 |
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492 | Which of the following sequences lists the relative sizes of particles in a water mixture from smallest to largest? A. Solutions, suspensions, colloids B. Solutions, colloids, suspensions c. colloids, solutions, suspensions D. Colloids, suspensions, solutions E. Suspensions, colloids, solutions |
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493 | The pair of boiling point and compound are given as, ( boldsymbol{C}_{6} boldsymbol{H}_{6}, quad boldsymbol{C H}_{3} boldsymbol{O H} quad boldsymbol{C}_{6} boldsymbol{H}_{5} boldsymbol{N O}_{2} ) ( boldsymbol{C}_{boldsymbol{6}} boldsymbol{H}_{boldsymbol{5}} boldsymbol{N} boldsymbol{H}_{boldsymbol{2}} ) ( mathbf{8 0}^{circ} boldsymbol{C} quad mathbf{6 5}^{circ} boldsymbol{C} quad mathbf{2 1 2}^{boldsymbol{o}} boldsymbol{C} ) ( 184^{circ} mathrm{C} ) (1) ( (|) ) (III) Which will show lowest vapour pressure at room temperature? A. ( C_{6} H_{6} ) в. ( C H_{3} ) ОН ( mathbf{c} cdot C_{6} H_{5} N O_{2} ) D. ( C_{6} H_{5} N H_{2} ) |
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494 | For an ideal binary liquid system: This question has multiple correct options A. the change in temperature ( (Delta H) ) is zero B. Raoult’s law is obeyed c. change in volume ( (Delta V) ) is zero D. none of the above |
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495 | Van’t Hoff’s factor for ( 0.01 M ) aqueous solution of acetic acid is ( 1.04, ) then ( p H: ) A . 3.4 B. 6.4 ( c .9 .6 ) D. 10.6 |
12 |

496 | 3.65 grams of HCl is dissolved in 16.2 grams of water. The mole fraction of HCI in the resulting solution is: A . 0.4 B. 0.3 ( c .0 .2 ) D. ( 0 . ) |
12 |

497 | In an experiment, 18.04 g of mannitol were dissolved in 100 g of water. The vapour pressure of water was lowered by ( 0.309 mathrm{mm} ) Hg from ( 17.535 mathrm{mm} ) Hg. Calculate the molar mass of manitol. A. ( 150.0 mathrm{g} / mathrm{mol} ) в. ( 184.3 mathrm{g} / mathrm{mol} ) c. ( 140.4 mathrm{g} / mathrm{mol} ) D. 123.21 g/mol |
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498 | A solution contains 200 g ppm ( C a C O_{3} ) If there is ( frac{boldsymbol{x} times boldsymbol{N}_{boldsymbol{A}}}{mathbf{1 0}^{boldsymbol{6}}} boldsymbol{C a C} boldsymbol{O}_{3} ) molecules per gram, what is the value of ( x ? ) |
12 |

499 | Illustration 2.73 Lowering of vapour pressure due to a solute in 1 molal aqueous solution at 100°C is a. 13.44 mm Hg b. 14.12 mm Hg c. 13.2 mm Hg d. 35.2 mm Hg |
12 |

500 | Carbon tetrachloride and benzene are: A . immiscible in water B. miscible in water c. both ( A ) and ( B ) D. none of these |
12 |

501 | 0.38 Explain the solubility rule “like dissolves like” in terms of intermolecular forces that exist in solutions. |
12 |

502 | Vapour pressure of water at ( 293 K ) is 17.535 mm ( H g . ) Calculate the vapour pressure of water at ( 293 K ) when ( 25 g ) of glucose is dissolved in ( 450 g ) of water. |
12 |

503 | A solution contains ( 20 % ) solute by weight at ( 60^{circ} ) C. When cooled to ( 30^{circ} mathrm{C} ) the solution contains ( 10 % ) solute by weight. When 45 g solution is cooled from ( 60^{circ} mathrm{C} ) to ( 30^{circ} mathrm{C} ), the mass of solute deposited is : A. ( 4.5 mathrm{g} ) B. 48 ( c cdot 5 g ) D. ( 4.75 mathrm{g} ) |
12 |

504 | lute dissolved of benzene by Illustration 2.126 1.0 g of non-electrolyte solute diss in 50.0 g of benzene lowered the freezing point of benzer 0.40 K. The freezing point depression constant of benzer 5.12 kg mol-1. Find the molecular mass of the solute. |
12 |

505 | ( 4.9 g ) of ( H_{2} S O_{4} ) is present in ( 100 m L ) of the solution. What is the molarity of the solution? Calculate its normality also. |
12 |

506 | A solution is prepared by urea and water. If mole fraction of water is 0.8 in the solution. Find the ratio of mass of water and urea. A ( cdot frac{5}{6} ) B. ( frac{6}{5} ) ( c cdot frac{1}{4} ) D. ( frac{4}{1} ) |
12 |

507 | In an endothermic process, solubility increases with temperature. ( A ). increase B. decrease c. no change in temperature D. none of the above |
12 |

508 | What are the conditions for an ideal solution which obeys Raoult’s law over the entire range of concentration? A ( cdot Delta_{m i x} H=0, Delta_{m i x} V=0, P_{text {Total}}=p_{A}^{o} x_{A}+p_{B}^{o} x_{B} ) B. ( Delta_{operatorname{mix}} H=+v e, Delta_{operatorname{mix}} V=0, P_{text {Total}}=p_{A}^{o} x_{A}+p_{B}^{o} x_{B} ) C. ( Delta_{operatorname{mix}} H=0, Delta_{operatorname{mix}} V=+v e, P_{text {Total}}=p_{A}^{circ} x_{A}+p_{B}^{o} x_{B} ) D. ( Delta_{text {mix}} H=0, Delta_{text {mix}} V=0, P_{text {Total}}=p_{B}^{o} x_{B} ) |
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509 | The volume of water required to make ( 0.20 mathrm{M} ) solution from ( 16 mathrm{ml} ) of ( 0.5 mathrm{M} ) solution is: A . ( 40 mathrm{ml} ) B. 16 ( mathrm{ml} ) c. ( 50 mathrm{ml} ) D. 24 m |
12 |

510 | Volume percentage decreases with increase in temperature. A. True B. False |
12 |

511 | Question 23. Suggest the most important type of intermolec attractive interaction in the following pairs. (i) n-hexane and n-octane (ii) I, and CCIA (ii) NaCIO, and water (iv) Methanol and acetone (v) Acetonitrile (CH3CN) and acetone (CzH60) Recall different types of intermolecular forces. London’s forces exist between the non-polar molecules, ionic interactions are found in ionic compound and dipole interactions are found in polar compounds.-OH, -NH or HF bond if present, the molecule can form H-bond. |
12 |

512 | The above experiment is done at ( N T P ) The stop cock is opened for certain time and then closed. After effusion, the bulb ( A ) contains ( 0.1 g m ) of ( D_{2} ). Find out the number of mole of ( H_{2} ) in bulb ( B ). |
12 |

513 | A 0.15 molal solution of ( K_{4}left[F e(C N)_{6}right. ) in water freezes at ( -0.65^{circ} mathrm{C} ). What is the apparent percentage of dissociation of this compound in this solution? ( left[boldsymbol{K}_{f} text { for water }=mathbf{1 . 8 6}^{circ} boldsymbol{C} boldsymbol{m o l}^{-1}right] ) A . 0.33 B. 0.52 ( c .0 .63 ) D. 0.79 |
12 |

514 | The freezing point of benzene decrease by ( 0.45^{circ} mathrm{C} ) when ( 0.2 g ) of acetic acid is added to ( 20 g ) of benzene. If acetic acid associates to form a dimer in benzene, percentage association of acetic acid in benzene will be: ( left(K_{f} text { for benzene }=right. ) ( left.mathbf{5 . 1 2} boldsymbol{K} boldsymbol{k g} boldsymbol{m o l}^{-1}right) ) A. ( 64.6 % ) B. ( 80.4 % ) c. ( 74.6 % ) D. ( 94.6 % ) |
12 |

515 | Illustration 2.155 Blood freezes at 272.44 K and a solution of 3.0 g of urea in 250 g of water freezes at 272.63 K. Calculate the osmotic pressure of blood at 300 K. (Assume density of blood at 300 K to be 1 g cc-1) |
12 |

516 | The freezing point of a solution containing 5.85 g of ( N a C l ) in ( 100 g ) of water is ( -3.348^{circ} mathrm{C} . ) Calculate van’t Hoff factor ‘i’ for this solution. What will be the experimental molecular weight of NaCl? ( left(K_{f} text { for water }=1.86 K k g m o l^{-1}, ) at. wt. right. ( mathrm{Na}=23, mathrm{Cl}=35.5) ) |
12 |

517 | What will be the molarity of the solution in which 0.365 g of HCl gas is dissolved in ( 100 mathrm{mL} ) of solution? A. 2 M B. 0.2 ( M ) ( c cdot 1 M ) D. 0.1 M |
12 |

518 | A candle is burnt in a beaker until it extinguishes itself. A sample of gaseous mixture in the beaker contains ( 6.08 times 10^{20} ) molecules of ( N_{2}, 0.76 times ) ( 10^{20} ) molecules of ( O_{2}, ) and ( 0.50 times 10^{20} ) molecules of ( C O_{2} . ) The total pressure is ( 734 mathrm{mm} ) of Hg. The partial pressure of ( O_{2} ) would be: A. ( 760.0 mathrm{mm} ) of ( mathrm{Hg} ) B. 76.0 mm of Hg c. ( 7.6 mathrm{mm} ) of ( mathrm{Hg} ) D. ( 0.76 mathrm{mm} ) of ( mathrm{Hg} ) |
12 |

519 | POLIUNTV UOVICUT Q.58 Why is it not possible to obtain pure ethanol by tras What general name is given to binary mixtures whic from Raoult’s law and whose components cannot fractional distillation. How many types of such mixtures e ethanol by fractional distillation? y mixtures which show deviation mponents cannot be separated by es of such mixtures are there? ac |
12 |

520 | The Henry’s law constant for the solubility of ( mathrm{N}_{2} ) gas in water at ( 298 mathrm{K} ) is ( 1.0 times 10^{5} ) atm. The mole fraction of ( mathrm{N}_{2} ) in air is ( 0.8 . ) The number of moles of ( mathrm{N}_{2} ) from air dissolved in 10 moles of water at ( 298 mathrm{K} ) and 5 atm pressure is? A ( cdot 4.0 times 10^{-4} ) B . ( 4.0 times 10^{-5} ) c. ( 5.0 times 10^{-4} ) D. ( 4.0 times 10^{-6} ) |
12 |

521 | The solubility of ( N_{2} ) in water is ( 2.2 times ) ( 10^{-4} g ) in ( 100 g ) of ( H_{2} O ) at ( 20^{circ} C ) when the pressure of ( N_{2} ) over the solution is 1.2 atm. Calculate the solubility at ( 20^{circ} mathrm{C} ) when |
12 |

522 | Illustration 2.119 1.355 g of a substance dissolved in 55 g of CH,COOH produced a depression in the freezing point of 0.618°C. Calculate the molecular weight of the substance (K. = 3.85) |
12 |

523 | Illustration 2.164 The solution containing 10 g of an organic compound per litre showed an osmotic pressure of 1.18 atm at 0°C. Calculate the molecular mass of the compound ( 0.0821 litre atm per degree per mol) |
12 |

524 | Which of the following liquid pairs shows a positive deviation from Raoult’s law? A. Acetone-chloroform B. Benzene-methanol c. water-nitric acid D. water-hydrochloric acid |
12 |

525 | What will be the solubility of the ( boldsymbol{C a}(boldsymbol{O H})_{2} ) solution when ( boldsymbol{N a O H} ) is dissolved in it, compared with that in pure water? A. Unaffected B. Increased c. Decreased D. None |
12 |

526 | Define Raoult’s law for the elevation of boiling point of a solution. |
12 |

527 | The normality of a solution of a mixture containing ( boldsymbol{H} boldsymbol{C l} ) and ( boldsymbol{H}_{2} boldsymbol{S} boldsymbol{O}_{4} ) is ( boldsymbol{N} / mathbf{5} ) Twenty millilitres of this solution reacts with an excess of ( A g N O_{3} ) solution to give ( 0.287 g ) of silver chloride. The percentage of ( H C l ) in the mixture by mass, is ( (A g=108) ) A . ( 42.69 % ) B. ( 57.31 % ) c. ( 50 % ) D. 25% |
12 |

528 | Question 10. Give an example of a material used for making semipermeable membrane for carrying out reverse osmosis. |
12 |

529 | For an ideal binary liquid solution with ( boldsymbol{p}_{boldsymbol{x}}^{0}>boldsymbol{p}_{boldsymbol{y}}^{0} ) in which relation between ( boldsymbol{X}_{boldsymbol{x}} ) (mole fraction of ( x ) in liquid phase) and ( Y_{x} ) (mole of fraction of ( x ) in vapour phase) is correct where ( boldsymbol{X}_{boldsymbol{y}} ) and ( boldsymbol{Y}_{boldsymbol{y}} ) are mole fraction of ( y ) in liquid and vapour phase respectively. A ( cdot X_{x}>Y_{x} ) в. ( X_{x}=Y_{x} ) с. ( frac{X_{x}}{X_{y}}<frac{Y_{x}}{Y_{y}} ) D. ( X_{x}, Y_{x}, X_{y} ) and ( Y_{y} ) cannot be correlated |
12 |

530 | A very dilute saturated solution of a sparingly soluble salt ( A_{3} B_{4} ) has a vapour pressure of 20 mm of ( H g ) at temperature ( T, ) while pure water exerts a pressure of 20.126 mm ( H g ) at the same temperature The solubility product constant of ( boldsymbol{A}_{3} boldsymbol{B}_{4} ) |
12 |

531 | 12. Substance used as an anti- freeze in radiators of automobiles is : (1) Methyl alcohol and H,O (2) Methyl alcohol (3) Ethyl alcohol (4) Ethyl alcohol and H,O |
12 |

532 | 1 ( g ) of ( N a C l ) dissolved in ( 100 g ) of water to prepare a mixture. What is the mass percentage of sodium chloride? | 12 |

533 | Air contains ( O_{2} ) and ( N_{2} ) in the ratio of 1:4. Calculate the ratio of solubilities in terms of mole fraction of ( boldsymbol{O}_{2} ) and ( boldsymbol{N}_{2} ) dissolved in water at atmospheric pressure and room temperature at which Henry’s constant for ( boldsymbol{O}_{2} ) and ( boldsymbol{N}_{2} ) are ( 3.30 times 10^{7} ) torr and ( 6.60 times 10^{7} ) tor respectively. |
12 |

534 | Illustration 2.157 The osmotic pressure of a solution is 1.3 atm. The density of solution is 1.3 g cm . Calculate the osmotic pressure rise. (1 atm = 76 cm Hg, dwg = 13.6 g cm-3) |
12 |

535 | A chemist is preparing to analyse samples that will contain no more than ( 0.5 mathrm{g} ) of uranium. His procedure calls for preparing the uranium as ( U^{4+} ) ion and oxidizing it by ( M n O_{4}^{-} ) in acid solution: ( boldsymbol{U}^{4+}+boldsymbol{M} boldsymbol{n} boldsymbol{O}_{4}^{-}+boldsymbol{H}_{2} boldsymbol{O} rightarrow boldsymbol{U} boldsymbol{O}_{2}^{2+}+ ) ( boldsymbol{M} boldsymbol{n}^{2+}+boldsymbol{H}_{3} boldsymbol{O}^{+} ) If he wants to react the total ( U^{4+} ) sample with a maximum of ( 50 mathrm{ml} ) of ( K M n O_{4} ) solution, what concentration does he choose? ( (mathrm{U}=238) ) A. 0.0336 M B. 0.0168 М c. 0.168 м D. 0.0672 M |
12 |

536 | At ( 80^{circ} mathrm{C}, ) the vapour pressure of pure liquid ( A ) is 520 mmHg and that of pure liquid ( B ) is 1000 mmHg. If a mixture solution of ( A ) and ( B ) boils at ( 80^{circ} ) and 1 atm pressure, the amount of ( A ) (mole percent) in the mixture is: A . ( 50 % ) B. 54% c. ( 32 % ) D. 44% |
12 |

537 | According to Henry’s law, the partial pressure of ( operatorname{gas}left(mathrm{P}_{text {gas}}right) ) is directly proportional to mole fraction of gas in dissolved state, i.e., ( boldsymbol{P}_{text {gas}}=boldsymbol{K}_{boldsymbol{H}} cdot boldsymbol{X}_{boldsymbol{g a s}} ) where ( K_{H} ) is Henry’s constant. Now, choose the correct option(s). This question has multiple correct options ( mathbf{A} cdot K_{H} ) is characteristic constant for a given gas-solvent system. B. Higher is the value of ( K_{H} ), lower is the solubility of gas for a given partial pressure of gas. ( mathbf{C} cdot K_{H} ) is temperature dependent D. ( K_{H} ) increases with temperature. |
12 |

538 | Illustration 2.187 0.002 molar solution of NaCl having degree of dissociation of 90% at 27°C has osmotic pressure equal to a. 0.94 bar b. 9.4 bar c. 0.094 bar d.9.4 x 10-4 bar |
12 |

539 | At ( 30^{circ} C, ) the solubility of ( A g_{2} C O_{3}left(K_{s p}=8 times 10^{-2}right) ) will be maximum in: A. 0.05 M ( mathrm{Na}_{2} mathrm{CO}_{3} ) B. ( 0.05 M A g N O_{3} ) c. Pure water D. ( 0.05 N H_{3} ) |
12 |

540 | A solution containing ( 10 g d m^{-3} ) of urea (molecular mass ( =60 g m o l^{-1} ) ) is isotonic with a ( 5 % ) solution of a nonvolatile solute. The molecular mass of this is nonvolatile solute is: A ( cdot 250 g m o l^{-1} ) в. 300 gmol-( ^{-1} ) c. 350 gmol-( ^{-1} ) D. ( 200 g ) mol ( ^{-1} ) |
12 |

541 | ( A ) ( 0.1(mathrm{M}) ) solution of an acid HA of density ( 1.01 mathrm{gm} / mathrm{ml} ) is taken in a beaker. The molec ular mass of HA is ( 300 mathrm{g} / mathrm{mol} ) The freezing point of solution is ( 0.2087^{circ} mathrm{C} . ) For ( mathrm{H}_{2} mathrm{O}, quad K_{f}=1.86 mathrm{K} / mathrm{m} ) What is the degree of dissociation of HA i n its ( 0.1(mathrm{M}) ) aqueous solution (in percentage) ? A . ( 10 % ) B. 20% c. ( 25 % ) D. ( 55.56 % ) |
12 |

542 | An ideal gas is mixture of ( C_{2} H_{6} ) and ( C_{2} H_{4} ) occupies 281 at 1 atm 8273 k. The mixture reacts completely with 128 g of ( O_{2} ) to produce ( C O_{2} ) pf water vapour Mole fraction of ( C_{2} H_{6} ) in the mixture will be: A. 0.4 B. 0.6 ( c cdot 0.2 ) D. 0.8 |
12 |

543 | 0.24 4 L of 0.02 M aqueous solution of NaCl was diluted by adding 1 L of water. The molality of the resultant solution is ………. (a) 0.004 0 .008 0.012 (d) 0.016 Thinking Process To calculate the strength of solution when it is diluted by adding solvent. Write all the given values M.V.M and Then calculate required parameter using formula, MY, MY, where i volume of solution before dilution = volume of solution after dilution M = strength of solution before dilution M = strength of solution after dilution |
12 |

544 | Illustration 2.124 A liquid possessing which of the following characteristics will be most suitable for determining the molecular mass of a compound by cryoscopic meas! a. That having low freezing point and small enthalpy Ol fusion b. That having high freezing point and small enthalpy of fusion c. That having high freezing point and small enthalpy of vapourization d. That having large surface tension |
12 |

545 | The composition of the solution whose normal boiling point is ( T ) A ( cdot X_{A}=0.08, X_{B}=0.92 ) В. ( X_{A}=0.92, X_{B}=0.18 ) C ( . X_{A}=0.18, X_{B}=0.82 ) D. None of these |
12 |

546 | ( R H_{2} ) (ion exchange resin) can replace ( C a^{2+} ) in hard water: [ boldsymbol{R} boldsymbol{H}_{2}+boldsymbol{C} boldsymbol{a}^{2+} rightarrow boldsymbol{R} boldsymbol{C} boldsymbol{a}+boldsymbol{2} boldsymbol{H}^{+} ] ( 1 L ) of hard water after passing through ( R H_{2} ) has ( p H=2 . ) Hence, hardness in ppm of ( boldsymbol{C a}^{2+} ) is : A . 200 в. 100 c. 50 D. 125 |
12 |

547 | Two liquids ( X ) and ( Y ) are perfectly immiscible. If ( X ) and ( Y ) have molecular masses in ration ( 1: 2, ) the total vapour pressure of a mixture of ( boldsymbol{X} ) and ( boldsymbol{Y} ) prepared in weight ratio 2: 3 should be: ( left(boldsymbol{P}_{X}^{0}=mathbf{4 0 0} text { torr }, boldsymbol{P}_{boldsymbol{Y}}^{0}=mathbf{2 0 0} text { torr }right) ) A. 314 torr B. 466.7 torr c. 600 torr D. 700 torr |
12 |

548 | Fill in the blanks with appropriate words. Azeotropic mixtures boil without change in their ( _{text {一一一一一一一. }} ) Azeotropic mixtures exist in solutions showing |
12 |

549 | 0.17 Sulphuric acid reacts with sodium hydroxide as follows H2SO4 + 2NaOH → Na2SO4 + 2H,0 When 1 of 0.1M sulphuric acid solution is allowed to react with 1L of 0.1M sodium hydroxide solution, the amount of sodium sulphate formed and its molarity in the solution obtained is (a) 0.1 mol L-1 (b) 7.10 g (c) 0.025 mol L- (d) 3.55 g |
12 |

550 | At ( 300 mathrm{K} ), the vapour pressure of an ideal solution containing 3 mole of ( A ) and 2 mole of ( mathrm{B} ) is 600 torr. At the same temperature, if 1.5 mole of ( A & 0.5 ) mole of ( mathrm{B} ) (non-volatile) are added to this solution the vapour pressure of solution increases by 30 torr. What is the value of ( P_{B}^{circ} ? ) A . 150 в. 405 c. 90 D. none of these |
12 |

551 | Ideal solution is formed when its components: A. have zero heat of mixing only B. have zero volume change on mixing only C. have zero heat of mixing and zero volume change D. can be converted into gases |
12 |

552 | Assuming the complete dissociation of HCl and lead salt, calculate how much ( mathrm{HCl} ) is added to ( 0.001 mathrm{m} ) lead salt solution to just precipitate when saturated with ( H_{2} S . ) The concentration of ( boldsymbol{H}_{2} boldsymbol{S} ). The concentration of ( boldsymbol{H}_{2} boldsymbol{S} ) is ( boldsymbol{0 . 1} ) ( mathbf{M} ) |
12 |

553 | A mixture of benzene and toluene forms A. An ideal solution B. Non-ideal solution c. suspension D. Emulsion |
12 |

554 | A storage battery contains a solution of ( H_{2} S O_{4} 38 % ) by weight. What will be the Vant Hoff factor if the ( Delta T_{f(e x p e r i m e n t)} ) in ( mathbf{2 9 . 0 8} .left[text {Given } boldsymbol{K}_{mathbf{1}}=mathbf{1 . 8 6 m o l}^{-mathbf{1}} mathbf{K} boldsymbol{g}right] ) |
12 |

555 | ( p H ) of a ( 0.1 M ) monobasic acid is found to be ( 2 . ) Hence its osmotic pressure at a given temp. ( boldsymbol{T} boldsymbol{K} ) is: A. ( 0.1 R T ) ( T ) в. ( 0.11 R T ) c. ( 1.1 R T ) D. ( 0.01 R T ) |
12 |

556 | If relative decrease in vapour pressure is 0.4 for a solution containing 1 mol NaCl in 3 mol ( H_{2} ) O. NaCl is ( % ) ionised. A . ( 60 % ) B. 50% c. ( 100 % ) D. 40% |
12 |

557 | For an ideal solution, the correct option is : A ( cdot Delta_{operatorname{mix}} S=0 ) at constant T and ( mathrm{P} ) B. ( Delta_{operatorname{mix}} V neq 0 ) at correct T and P C. ( Delta_{operatorname{mix}} H=0 ) at constant ( mathrm{T} ) and ( mathrm{P} ) D. ( Delta_{text {mix}} G=0 ) at constant T and ( P ) |
12 |

558 | If the pH of ( 0.2 M ) dibasic acid ( left(H_{2} Aright) ) is ( 1.699, ) than its osmotic pressure at ( T ) K temperature will be? в. ( 0.02 R T ) c. ( 0.4 R T ) D. ( 0.1 R T ) |
12 |

559 | g of sodium hydroxide is present in 1 litre of ( 1 mathrm{M} ) solution. A . 20 B. 40 ( c .30 ) D. 10 |
12 |

560 | Which is the condition, unrelated to quantities, that indicates that the rate going into solution is equal to the rate coming out of solution? A . Dilute B. concentrated c. Unsaturated D. Saturated E. Supersaturated |
12 |

561 | Find mole fraction of ( N a O H ) in its ( 10 % ) aqueous solution. |
12 |

562 | 2.5 litre of ( 1 mathrm{M} ) NaOH solution mixed with another 3 litre of ( 0.5 ~ M ) NaOH solution. Then find out molarity of resultant solution. в. ( 1.0 mathrm{M} ) c. 0.73 М D. ( 0.50 M ) |
12 |

563 | Illustration 2.87 Match the following if the molar mass of X, Y, and Z are same: Solvent T(°C) K(kg K mol-1) Х 127 0.73 27 0.53 253 0.98 |
12 |

564 | Addition of 0.643 g of a compound to 50 mL of benzene (density 0.879 glmL) lowers the freezing point from ( 5.51^{circ} mathrm{C} ) to ( 5.03^{circ} mathrm{C} . ) If ( K_{f} ) for benzene is 5.12 calculate the molecular mass of the compound. A . 126 B. 166 ( c cdot ) १५ D. 146 |
12 |

565 | Q.43 Why is the vapour pressure of an aqueous solution of glucos that of water? of water. When a aqueous solution of glucose lower than |
12 |

566 | For an ideal solution of two components A and B, which of the following is true? ( mathbf{A} cdot Delta H_{m i x i n g}0(z text {ero}) ) C. ( A ) – ( B ) interaction is stronger than ( A-A ) and ( B-B ) interactions D. ( A-A, B-B ) and ( A-B ) interactions are identical |
12 |

567 | Which of the following solutions is more concentrated than the others? A. ( 5.3 mathrm{gm} ) of ( mathrm{Na}_{2} mathrm{CO}_{3} ) in ( 500 mathrm{ml} ) solution B. 5 gm of ( N a O H ) in 100 ml solution c. 3.65 gm of ( H C l ) in 750 ml solution D. 4.9 gm of ( H_{2} S O_{4} ) in ( 1000 mathrm{ml} ) solution |
12 |

568 | Derive van’t Hoff general solution equation. |
12 |

569 | The mass of non-volatile, non-elctrolyte solute (molar mass ( 50 g ) mol ( ^{-1} ) ) needed to be dissolved in ( 114 g ) octane to reduce its vapour pressure to ( 75 % ), is A . ( 150 g ) в. ( 75 g ) c. ( 37.5 g ) D. ( 50 g ) |
12 |

570 | The cryoscopic constant for acetic acid is ( 3.6 K k g / ) mol. A solution of ( 1 g ) of a hydrocarbon in ( 100 g ) of acetic acid freezes at ( 16.14^{circ} mathrm{C} ) instead of the usual ( 16.60^{circ} mathrm{C} . ) The hydrocarbon contains ( 92.3 % ) carbon. If the molecular formula is ( C_{6} H_{6} . ) Find the value of ( x ) and ( y ) A. ( x=2, y=4 ) В. ( x=3, y=5 ) c. ( x=4, y=4 ) D. ( x=6, y=6 ) |
12 |

571 | The van’t hoff factor for a very dilute solution of ( boldsymbol{F e}_{2}left(boldsymbol{S O}_{4}right)_{3} ) is: ( mathbf{A} cdot mathbf{9} ) B. 5 ( c cdot 24 ) D. 16 |
12 |

572 | When ( 25 g ) of ( N a_{2} S O_{4} ) is dissolved in ( 10^{3} k g ) of solution, its concentration will be : A . 2.5 ppm в. 25 ррт c. 250 ppm D. 100 ppm |
12 |

573 | Q. 14 Which of the following statements is false? (a) Two different solutions of sucrose of same molality prepared in different solvents will have the same depression in freezing point. (b) The osmotic pressure of a solution is given by the equation it = CRT (where, C is the molarity of the solution) (c) Decreasing order of osmotic pressure for 0.01 M aqueous solutions of barium chloride, potassium chloride, acetic acid and sucrose is Bacl, > KCI > CH. COOH > sucrose (d) According to Raoult’s law, the vapour pressure exerted by a volatile component of a solution is directly proportional to its mole fraction in the solution |
12 |

574 | Ideal solution is formed when its components: This question has multiple correct options A. have zero heat of mixing B. have zero volume change c. obey Raoult’s law D. can be converted into gases |
12 |

575 | A solution having ( Delta boldsymbol{H}_{m i x}=+ ) ve will exhibit deviation from ideal behaviour A. negative B. positive ( c cdot ) no D. depends upon the properties of the mixing components |
12 |

576 | Ilustration 2.54 Why does a solution of ethanol and cyclohexane show positive deviation from Raoult’s law? |
12 |

577 | What amount of ( C a C l_{2}(i=2.47) ) is dissolved in 2 litres of water so that its osmotic pressure is 0.5 at ( m ) at ( 27^{circ} C ) A. ( 3.42 g ) B. ( 9.24 g ) c. ( 2.834 g ) D. ( 1.820 g ) |
12 |

578 | If ( alpha ) is the degree of dissociation of ( N a_{2} S O_{4}, ) the vant Hoff’s factor ( (i) ) used for calculating the molecular mass is: ( mathbf{A} cdot 1+alpha ) B. ( 1-alpha ) ( c cdot 1+2 alpha ) D. ( 1-2 alpha ) |
12 |

579 | Illustration 2.173 The osmotic pressure of a solution containing 5 g of substance (molar mass = 100) in 308 ml of solution was found to be 4.0 atm at 300 K. Calculate the value of solution constant (R). |
12 |

580 | A solution containing ( 25.6 g m ) of sulphur dissolved in ( 1000 g ) of naphthalene gave a freezing point lowering of 0.680 , then molecular formula of sulphur is: ( A cdot S_{2} ) в. ( S_{4} ) c. ( S_{6} ) D. ( S_{8} ) |
12 |

581 | In the azeotropic mixture of ( H C l ) and water, the percentage of ( H C l ) is: A . 20.2% B . 11.1% c. 44.4% D. 10% |
12 |

582 | Benzene and naphthalene form an ideal solution at room temperature. For this process, the true statements are: (i) ( Delta G ) is positive (ii) ( Delta S_{s y s t e m} ) is positive (iii) ( Delta S_{text {surroundings}}=0 ) (iv) ( Delta boldsymbol{H}=mathbf{0} ) A. (ii) and (iv) only B. (i) and (iii) only C. (ii), (iii) and (iv) only D. all of these |
12 |

583 | The volume of ( boldsymbol{H}_{2} boldsymbol{S} boldsymbol{O}_{4} ) acid ( (boldsymbol{9} boldsymbol{8} % ) by mass, ( d=1.80 mathrm{g} / mathrm{mL} ) ) required to prepare 1 litre of ( 0.1 M H_{2} S O_{4} ) solution is: A ( .16 .65 mathrm{mL} ) B . ( 22.20 mathrm{mL} ) ( c .5 .55 mathrm{mL} ) D. ( 11.10 mathrm{mL} ) |
12 |

584 | Dimerization of benzoic acid occurs in benzene solution, then the relation between van’t Hoff factor ( i ) and amount of association ( x ) is: A ( cdot i=(1-x) ) B . ( i=(1+x) ) c. ( i=left(1-frac{x}{2}right) ) D. ( i=left(1+frac{x}{2}right) ) |
12 |

585 | mospheric pressure and osmotic pressure are the same Q. 16 Which of the following statements is false (a) Units of atmospheric pressure and osmotic pre (b) In reverse Osmosis, solvent molecules move membrane from a region of lower concen concentration (c) The value of molal depression constant depends on na (a) Kelative lowering of vapour pressure is a dimensionless quantity molecules move through a semipermeable of lower concentration of solute to a region of higher al depression constant depends on nature of solvent lo membrane |
12 |

586 | On mixing ( 10 mathrm{mL} ) of acetone with ( 40 mathrm{mL} ) of chloroform, the total volume of the solution is: ( A cdot 50 ( m ) L ( c_{c}=50 mathrm{mL} ) D. Can not be predicted |
12 |

587 | Acetic acid dissolved in benzene shows a molecular weight of A . 60 B. 120 c. 180 D. 240 |
12 |

588 | Arrange the following aqueous solutions in the order of their increasing boiling points ( (mathrm{i}) 10^{-4} M N a C l ) (ii) ( 10^{-4} M ) Urea ( (text { iii }) 10^{-3} M M g C l_{2} ) (iv) ( 10^{-2} M N a C l ) A ( cdot(i)<(i i)<(i v)<(i i i) ) B. ( (i i)<(i)<(i i i)<(i v) ) c. ( (i i i)<(i)<(i i)<(i v) ) D. ( (i v)<(i i i)<(i)=(i i) ) |
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589 | Lowering in vapour pressure is highest for: A. ( 0.2 mathrm{m} ) urea B. 0.1 m glucose ( mathrm{c} cdot 0.1 mathrm{m} mathrm{MgSO}_{4} ) D. ( 0.1 mathrm{m} ) BaCl ( _{2} ) |
12 |

590 | Caffeine has a molecular weight of 194 If it contains ( 28.9 % ) by mass of nitrogen, the number of atoms of nitrogen in one molecule of caffeine is: ( A cdot 4 ) B. 6 ( c cdot 2 ) D. |
12 |

591 | The molarity of ( boldsymbol{H} boldsymbol{C l} ) solution containing 0.4 moles in 200 ml of the solution is: A. 2 M в. 1 ( c cdot 3 M ) D. 4 M |
12 |

592 | A mixture of ( C_{3} H_{8} ) and ( C H_{4} ) exerts a pressure of ( 320 mathrm{mm} ) Hg at temperature ( boldsymbol{T}(boldsymbol{K}) ) in a ( boldsymbol{V} ) litre flask. On complete combustion, gaseous mixture contains ( C O_{2}, ) only and exerts a pressure of 448 ( mathrm{mm} ) Hg under identical condition. Hence, mole fraction of ( C_{3} H_{8} ) in the mixture is : A . 0.2 B. 0.8 c. 0.25 D. 0.75 |
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593 | What concentration of ( boldsymbol{F}- ) ( boldsymbol{C H}_{2} boldsymbol{C O O H},left(boldsymbol{K}_{a}=mathbf{2 . 6} times mathbf{1 0}^{-3}right) ) is needed so that ( left[boldsymbol{H}^{+}right]=mathbf{2} times mathbf{1 0}^{-mathbf{3}} ) ? в. ( 2.6 times 10^{-3} M ) c. ( 5.2 times 10^{-3} M ) D. ( 3.53 times 10^{-3} M ) |
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594 | Illustration 2.64 What are minimum boiling azeotropes? Give one example. |
12 |

595 | Determine the amount of ( C a C l_{2}(i= ) 2.47) dissolved in 2.5 litre of water such that its osmotic pressure is 0.75 atm at ( 27^{circ} C ) |
12 |

596 | Study the figures given below and mark the correct statement A. (i) Nitric acid + Water; (i) Acetone + Ethyl alcohol B. (i) Water + Ethyl alcohol (ii) Acetone + Benzene C. (i) Acetone + Ethyl alcohol; (ii) Acetone + Chloroform D. (i) Benzene + Chloroform (ii) Acetone + Chloroform |
12 |

597 | What is the effect of temperature on solubility of a gas? A. Solubility of a gas increase with rise in temperature B. Solubility of a gas decreases with rise in temperature c. No effect D. Sometimes increases with increase in temperature sometimes decreases |
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598 | Find the volume of a 0.2 molar solution of sodium hydroxide, which is used to neutralize 40 liters of a 0.3 molar hydrochloric acid solution. A. 10 liters B. 20 liters c. 40 liters D. 60 liters E. 120 liters |
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599 | Question 35. Henry’s law constant for the molality of methane in benzene at 298 K is 4.27 x10 mm Hg Calculate the solubility of methane in benzene at 298 K under 760 mm Hg. Apply Henry’s law, p = Ky* |
12 |

600 | Find out ( % ) strength of ( 11.2 V H_{2} O_{2} ) A . ( 34 % ) B. 3.4% c. ( 1.7 % ) D . 13.8% |
12 |

601 | Illustration 2.32 At a certain temperature, the vapour pressure of pure ether is 640 mm and that of pure acetone is 280 mm. Calculate the mole fraction of each component in the vapour state if the mole fraction of ether in the solution is 0.50. |
12 |

602 | 10. The vapour pressure of a pure liquid A is 40 mm Hg at 310 K. The vapour pressure of this liquid in a solution with liquid B is 32 mm Hg. The mole fraction of A in the solution, if it obeys Raoult’s law, is: a. 0.8 b. 0.5 c. 0.2 d. 0.4 |
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603 | At STP, a container has 1 mole of ( A r, 2 ) moles of ( C O_{2}, 3 ) moles of ( O_{2} ) and 4 moles of ( N_{2} . ) Without changing the total pressure of ( boldsymbol{O}_{2} ) is removed, the partial pressure of ( boldsymbol{O}_{2} ) is: A. changed by about ( 16 % ) B. halvedd c. changed by ( 26 % ) D. unchanged. |
12 |

604 | The vapour pressure of pure benzene at ( 88 C ) is ( 960 mathrm{mm} ) and that of toluene at the same temperature is ( 380 mathrm{mm} ) of benzene. At what mole fraction of benzene. the mixture will boil at ( 88^{circ} mathrm{C} ) ? A . 0.655 B. 0.345 ( c cdot 0.05 ) D. 0.25 |
12 |

605 | Question 13. Why is the mass determined by measuring a colligative property in case of some solutes abnormal? Discuss it with the help of van’t Hoff factor. oble molente |
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606 | An aqueous solution is 1.00 molal in ( mathrm{Kl} ) Which change will cause the vapour pressure of the solution to increase? A. Addition of Nacı B. Addition of ( mathrm{Na}_{2} mathrm{SO}_{4} ) c. Addition of 1.00 molal KI D. Addition of water |
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607 | ( 6 g ) urea and ( 11.8 g ) glucose are dissolved in ( 100 m l H_{2} O . ) What is the osmotic pressure at ( 300 K ) A. 27.06 atm B. 30 atm c. 45 atm D. 13.07 atm |
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608 | Question 9. Vapour pressure of pure water at 298 K is 23.8 mm Hg. 50 g urea (NH,CONH) is dissolved in 850 g of water. Calculate the vapour pressure of water for this solution and its relative lowering. Consider Raoult’s law and formula for relative lowering in vapour pressure, PA – Ps – NB _WB MA På NA MBWA where, PA Ps is called relative lowering in vapour pressure. |
12 |

609 | Illustration 2.156 x g of non-electrolytic compound (molar mass = 200) is dissolved in 1.0 L of 0.05 M NaCl solution. The osmotic pressure of this solution is found to be 4.92 atm at 27°C. Calculate the value of x. Assume complete dissociation of NaCl and ideal behaviour of this solution. |
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610 | Molecules of benzoic acid ( left(C_{6} H_{5} C O O Hright) ) dimerise in benzene. g of the acid dissolved in 30 g of benzene shows a depression in freezing point equal to ( 2 mathrm{K} ). If the percentage association of the acid to form a dimer in the solution is ( 80, ) then ( w ) is: (Given that ( boldsymbol{K}_{f}=mathbf{5} mathrm{K} ) kg ( boldsymbol{m o l}^{-1} ), Molar mass of benzoic acid ( =122 ) g ( m o l^{-1} ) A . ( 1.8 g ) в. 2.4g c. ( 1.0 g ) D. ( 1.5 mathrm{g} ) |
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611 | The van’t Hoff’s factor for ( 0.1 mathrm{M} ) ( B aleft(N O_{3}right)_{2} ) solution is ( 2.74 . ) The degree of dissociation is: A . ( 91.3 % ) B. 87% c. ( 100 % ) D. 74% |
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612 | ( C H_{3} C O O H ) dimerizes in benzene when ( 1.65 g ) of ( C H_{3} C O O H ) dissolved in ( 100 g ) of benzene the elevation of ( B p s ) of the solution was found ( 0.36 K . ) If ( K_{b} ) for benzene in 2.85 K.kgl mol. Then find Vant Hoff factor and degree of association of ( boldsymbol{C} boldsymbol{H}_{3} boldsymbol{C O O H} ) |
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613 | The following substances were all dissolved in 100 grams of water at ( 290 mathrm{K} ) to produce saturated solutions.lf the solution is heated to ( 310 mathrm{K} ), which substance will have a decrease in its solubility: ( mathbf{A} cdot N a C I ) в. ( K I ) c. ( mathrm{CaCl}_{2} ) D. ( H C I ) E . ( K N O_{3} ) |
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614 | Illustration 2.48 What is the composition of the vapour which is in equilibrium at 30°C with a benzene-toluene solution with a mole fraction of benzene of (a) 0.400 and (b) 0.600? Po° = 119 torr, p.° = 37.0 torr |
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615 | The Henry law constant for dissolution of a gas in an aqueous medium is ( 3 times ) ( 10^{2} ) atm. At what partial pressure of the gas (in atm), the molality of gas in aqueous solution will be ( frac{5}{9} M ? ) A . 2.2 M в. 9 м ( c .3 ) м D. none |
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616 | At a given temperature, total vapour pressure (in torr) of a mixture of volatile components ( A ) and ( B ) is given by ( P_{T o t a l}=120-75 X_{B} ) hence, the vapour pressure of pure ( A ) and ( B ) respectively (in Torr) are: A .120,75 в. 120,195 c. 120,45 D. 75,45 |
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617 | ( mathbf{3 0} boldsymbol{m} boldsymbol{L} ) of ( boldsymbol{C H}_{3} boldsymbol{O H}left(boldsymbol{d}=mathbf{0 . 8} boldsymbol{g} / boldsymbol{c m}^{3}right) ) is mixed with ( 60 m L ) of ( C_{2} H_{5} O H(d= ) ( left.0.92 g / c m^{3}right) ) at ( 25^{circ} C ) to form a solution of density ( 0.88 g / c m^{3} . ) Select the correct option. This question has multiple correct options A. Molarity and molality of resulting solution are 6.33 and 13.59 respectively B. The mole fraction of solute and molality are 0.385 and 13.59 respectively c. Molarity and % change in volume are 13.59 and zero respectively D. Mole fraction of solvent and molality are 0.615 and 13.59 respectively |
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618 | During dissolution when a solute is added to the solvent, some solute particles separate out from the solution as a result of crystallization. At the stage of equilibrium, the concentration of solute in the solution at a given temperature and pressure: A. increases B. decreases c. remains constant D. keeps changing |
12 |

619 | Which is least soluble? A ( cdot N a_{2} S ) в. ( M g S ) c. ( M g C l_{2} ) D. ( N a C l ) |
12 |

620 | The vapour pressure of benzene C,H, at 298 K is 95 torr. After 10.00 g of benzene is injected into a 10.0 L bulb at 298 K, how many grams of benzene remain as liquid? |
12 |

621 | What is Henry’s constant for neon dissolved in water given ( C_{N e}= ) ( 23.5 m L / L ) solution and STP volume ( 22,414 mathrm{mL} / text { mole gas }) ) and pressure ( operatorname{atm}) ? ) A. 0.00105 5 В. 0.11004 begin{tabular}{l} ( c .0 .00115 ) \ hline end{tabular} D. 0.00015 |
12 |

622 | The boiling point of an azeotropic mixture of water and ethyl alcohol is less than that of theoritical value of water and alcohol mixture. Hence the mixture shows: A. that solution is saturated B. positive deviation from Raolt’s law c. negative deviation from Raoult’s law D. that solution is super saturated |
12 |

623 | How many moles of ( N a O H ) are required to neutralize 1.2 moles of ( boldsymbol{H}_{2} boldsymbol{S} boldsymbol{O}_{4} ? ) A. 0.6 mole B. 1.2 mole c. 2.4 mole D. 3.6 mole E . 4.8 mole |
12 |

624 | The concentration of ( C aleft(H C O_{3}right)_{2} ) in a sample of hard water is 486 ppm. The density of water sample is ( 1.0 mathrm{g} / mathrm{ml} ). The molarity of the solution is : A . ( 3.0 times 10^{-3} M ) в. ( 5.0 times 10^{-3} M ) c. ( 2.0 times 10^{-3} M ) D. ( 6.0 times 10^{-3} M ) |
12 |

625 | Two components in the ratio of ( x: y ) form an azeotropic mixture. They are mixed in the ratio of ( x: 2 y, ) how many moles one of the pure component ( boldsymbol{y} ) will be evaporated before getting azeotropic solution? |
12 |

626 | At a particular temp, a solution that has dissolved as much solute as it is capable of dissolving is said to be a : A. saturated solution B. unsaturated solution c. both ( A ) and ( B ) D. none of the above |
12 |

627 | Due to low concentration of oxygen in blood, climber become weak and unable to think clear – (i) Write specific name of above condition? (ii) Explain the reason of such condition? |
12 |

628 | When an electrolyte is dissociated in solution, the van’t Hoff’s factor ( ( i ) ) is : ( A cdot>1 ) B. ( <1 ) ( mathrm{c} cdot=0 ) ( mathrm{D} cdot=1 ) |
12 |

629 | mole ( A_{X} B_{Y} ) when added to ( 1.08 mathrm{kg} ) of water, lowers its vapour pressure by 35 torr to 700 torr. If further 1184 g of methanol is added, then the vapour pressure increase by 37 torr. Consider only few vapors are formed, and ( boldsymbol{A}_{boldsymbol{X}} boldsymbol{B}_{boldsymbol{Y}} ) is a non volatile solute. What is the value of a if the vapour pressure of pure methanol is ( a times 10^{2} ) torr. |
12 |

630 | llustration 2.146 What are isotonic solutions? | 12 |

631 | Example 2.10 Calculate the osmotic pressure of a solution obtained by mixing 100 cm of 1.5% solution of urea (mol. mass=60) and 100 cm of 3.42% solution by cane sugar (mol. mass = 342) at 20°C. (R = 0.082 litre atm/deg/mole) |
12 |

632 | Q. 10 The unit of ebullioscopic constant is (a) K kg mol-‘or K(molality) (b) mol kg K-‘or K-‘ (molality) (c) kg mol-‘K-‘ork-‘(molality)-! (d) K mol kg- or K (molality) Thinking Process Write the formula of ebullioscopic constant then put the values of their unit and then calculate unit of ebullioscopic constant. |
12 |

633 | For a dilute solution containing ( 2.5 g m ) of a non-volatile non-electrolyte solute in ( 100 g m ) of water, the elevation in boiling point at 1 atm pressure is ( 2^{circ} C ) Assuming concentration of solute is much lower than the concentration of solvent, the vapour pressure (mm of ( boldsymbol{H} boldsymbol{g} ) of the solution is ( left(boldsymbol{K}_{boldsymbol{b}}=right. ) ( left.0.76 K k g m o l^{-1}right) ) A .724 в. 740 ( c .736 ) D. 718 |
12 |

634 | Vant Hoff factor (i) for dimerisation of benzoic acid insome solvent assuming ( 30 % ) degree of association A . 0.85 B. 0.95 ( c .0 .90 ) D. |
12 |

635 | Depression in f.pt. is more pronounced if camphor is used as a solvent in place of water for same mass of solute and solvent. If true enter ( 1, ) if false enter 0 |
12 |

636 | What is the difference between lyophobic sol and lyophilic sol? |
12 |

637 | If you mix 3 litres of 0.5M ( N a C l ) with 9 litres of ( 0.2777 mathrm{M} N a C l ) what will the concentration of the final solution be assuming that volumes are additive? в. 0.39 м c. ( 0.5777 mathrm{M} ) D. 0.6777 M E. None of the above |
12 |

638 | A current of ( 4.0 A ) is passed for 5 hours through ( 1 L ) of ( 2 M ) solution of nickel nitrate using two nickel electrodes. The molarity of the solution at the end of the electrolysis will be: ( mathbf{A} cdot 1.6 M ) в. ( 1.2 M ) c. ( 2.5 M ) D. ( 2.0 M ) |
12 |

639 | In a very ideal imaginary condition, a sample of ice was taken, and its osmotic pressure was found to be 0.274 ( operatorname{atm} ) at ( 300 mathrm{K} ) (density ( =1 mathrm{g} / mathrm{mL} ) ). Thus, number of water units attached to one water unit is ( A cdot 4 ) B. 3 ( c cdot 6 ) ( D .5 ) |
12 |

640 | Tlustration 2.185 A 1.17% solution of NaCl is isotonic with 7.2% solution of glucose. Calculate the Van’t Hoff factor of NaCl. |
12 |

641 | Why does solution of chloroform & acetone show negative deviation from Raoult’s law? Illustrate the deviation with the help of diagrams |
12 |

642 | If observed vapour pressure is greater than ideal vapour pressure then: A. it is known as negative deviation from Raoult’s law B. it is known as ideal solution C. it is known as positive deviation from Raoult’s law D. None of these |
12 |

643 | A mixture of ethanol and water contains ( 54 % ) water by mass. Calculate the mole fraction of ethanol in this solution. A. 0.25 B. 0.15 ( c cdot 0.20 ) D. 0.30 |
12 |

644 | The boiling point of water at 735 torr is ( 99^{circ} mathrm{C} . ) The mass of ( mathrm{NaCl} ) added in 100 ( operatorname{gmof} sin operatorname{tar}left(K_{b}=0.51 K k g m o l^{-3}right) ) to make its boiling point at ( 100^{circ} mathrm{C} ) is: A ( .10 .68 mathrm{g} ) B. ( 5.34 mathrm{g} ) c. 2.67 g D. 26.7 g |
12 |

645 | Statement – I: ( 1 mathrm{M} ) solution of NaCl has a higher osmotic pressure than 1 M solution of glucose at the same temperature. Statement – II: The number of particles present in 1 M NaCl solution are more than those present in 1 M glucose solution and osmotic pressure depends upon number of particles present in the solution. A. Statement-lis True, Statement – II is True; Statement I is a correct explanation for Statement – B. Statement-lis True, Statement – /I is True; Statement I is NOT a correct explanation for Statement- – c. Statement – – is True, Statement – II is False D. Statement-lis False, Statement – II is True |
12 |

646 | Flour, salt, sugar, eggs and baking powder are ingradients for baking a cake, when you mix these ingradients, you get batter. Is batter a mixture or a compound? The batter is put into an oven to bake into a cake. Is the cake a mixture or a compound? Explain your answers. |
12 |

647 | The vapour pressure of pure benzene at a certain temperature is 0.850 bar. ( A ) non-volatile, non-electrolyte solid weighing ( 0.5 g ) is added to ( 39.0 g ) of benzene (molar mass ( 78 g / )mol ). The vapour pressure of the solution then is ( mathbf{0 . 8 4 5} ) bar. What is the molecular mass of the solid substance? ( mathbf{A} .58 ) в. 180 ( c .170 ) D. 145 |
12 |

648 | The difference in height of the mercury column in two arms of U tube manometer in the arrangement – lis ( boldsymbol{h}_{1}=mathbf{6 6 0} mathrm{mm} . ) In another arrangement – Il at same temperature, 222 gm of ( mathrm{CaCl}_{2} ) is dissolved in ( 324 mathrm{gm} ) of water and difference in height of mercury column in two arms is found to be ( h_{2}= ) ( 680 mathrm{mm} . ) If the value of degree of dissociation for ( C a C l_{2} ) in arrangement -11 is ( alpha, ) then the value of ( 64 alpha ) is: [Atmospheric pressure ( =1 ) atm] A . 40 B. 38 c. 45 D. 50 |
12 |

649 | In case of an electrolyte which dissociates in the solution, the van’t hoff factor ( i ) is : ( A cdot>1 ) в. ( 1 ) or ( <1 ) |
12 |

650 | The solubility curve of ( boldsymbol{K} boldsymbol{N} boldsymbol{O}_{3} ) in water is shown below.
The amount of ( K N O_{3} ) that dissolves in |
12 |

651 | Assertion The solubility of ammonium chloride increases with increase in temperature Reason In case of substances whose solubility increases with increase in temperature is due to the dissolution process being endothermic. A. Both Assertion and Reason are correct and Reason is the correct explanation for Assertion B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion c. Assertion is correct but Reason is incorrect D. Both Assertion and Reason are incorrect |
12 |

652 | What is meant by positive and negative deviations from Raoult’s law and how is the sign of ( Delta_{m i x} H ) related to positive and negative deviations from Raoult’s law? |
12 |

653 | ( boldsymbol{H}_{2} boldsymbol{S} ) a toxic gas with rottenegg like smell is used for the qualetative analysis, if the solubility of ( H_{2} S ) in water,at STP is 0.195mole.kg ( ^{-1} ), the Henry’s law constant is: A. 282 bar B. 324.8 bar c. 462.9 bar D. 534.8 bar |
12 |

654 | The standard reduction potential of the ( A g^{+} mid A g ) electrode at ( 298 mathrm{K} ) is ( 0.80 mathrm{V} ) The solubility product of ( A g l ) is ( 6.4 times ) ( 10^{-17} ) at ( 298 mathrm{K} .(2.303 mathrm{RT} / mathrm{F}=0.06) ) The potential of ( A g^{+} mid A g ) electrode in a saturated solution of Agl at ( 298 mathrm{K} ) is ( mathbf{A} cdot-0.314 V ) B . ( +0.314 V ) c. ( -0.172 V ) D. ( +0.172 mathrm{V} ) |
12 |

655 | The osmotic pressure of a solution in atm obtained on mixing each 50 mL of ( 1.2 % ) mass/volume urea solution and ( 2.4 % ) mass/volume glucose solution at ( mathbf{3 0 0} mathrm{K} ) is: ( (boldsymbol{R}=mathbf{0 . 0 8} ) litre atm ( left.boldsymbol{K}^{-1} boldsymbol{m o l}^{-1}right) ) |
12 |

656 | Two moles of ( O_{2} ) gas is collected over water at ( 400 mathrm{K} ) temperature in 2 litre vessel. If the pressure of dry ( O_{2} ) gas is 32.20 bar then find the vapour pressure of water under the same conditions. |
12 |

657 | An aqueous solution of hydrochloric acid A. obeys Raoult’s law B. shows negative deviation from Raoult’s law C. shows positive deviation from Raoult’s law D. obeys Henry’s law at all compositions |
12 |

658 | If we add potassium nitrate to ice it will result in (a) Increase in m.p. of ice. (b) Decrease in m.p. ofice (c) Neither (a) nor (b) (d) Change in colour of ice |
12 |

659 | Which of the following is true about a solution that has ( [boldsymbol{O H}]=mathbf{1 . 0} times mathbf{1 0}^{-mathbf{8}} ) M? A. The pHis 8 and the solution is acidic B. The ( left[H^{+}right]=1.0 times 10^{-8} mathrm{M} ) and the solution is basic c. The pHis 6 and the solution is acidic D. The ( left[H^{+}right]=1.0 times 10^{-6} mathrm{M} ) and the solution is basic E . The ( left[H^{+}right]=1.0 times 10^{-14} mathrm{M} ) and the solution is neutral |
12 |

660 | 0.1 molal-equeous solution of an electrolyte ( mathrm{FeCl}_{2} ) is ( 80 % ) ionised. The boiling point of the solution at 1 atm is: ( left[mathbf{K}_{mathbf{6}}left(mathbf{H}_{2} mathbf{O}right)=mathbf{0 . 5 2} mathbf{K} mathbf{k g} mathbf{m o l}^{-mathbf{1}}right] ) A. ( 273.17 K ) B . ( 273.19^{circ} mathrm{C} ) c. ( 373.19^{circ} mathrm{C} ) D. ( 100.17^{circ} mathrm{C} ) |
12 |

661 | (1) Define the following (i) Henry’s law (ii) Normality. |
12 |

662 | . 32 The density of 3 molal solution of NaOH is 1.110 g mL . Calculate the molarity of the solution. |
12 |

663 | The Van’t Hoff factor of ( 0.1 mathrm{M} mathrm{Ba}left(mathrm{NO}_{3}right)_{2} ) solutions is ( 2.74 . ) The degree of dissociation will be A . 91.3% B. 87% c. ( 100 % ) D. 74% |
12 |

664 | Henry’s law constant for molality of methane in benzene at ( 298 K ) is ( 4.27 times ) ( 10^{5} ) mm ( H g . ) The mole fraction of methane in benzene at ( 298 K ) under ( 760 m m H g ) is: A. ( 1.78 times 10^{-3} ) B. 17.43 c. 0.114 D. 2.814 |
12 |

665 | When ( 100 m l ) of ( 0.06 m mathrm{Fe}left(N O_{3}right)_{3}, 50 m l ) of ( 0.2 m l F e C l_{3} ) and ( 100 m l ) of ( 0.26 m m gleft(N O_{3}right)_{2} ) are mixed, then calculate molarity of reaction in final solution. |
12 |

666 | Sulphuric acid reacts with sodium hydroxide as follows ( H_{2} S O_{4}+2 N a O H rightarrow N a_{2} S O_{4}+2 H_{2} O ) When 1 L of 0.1 M sulphuric acid solution is allowed to react with 1 L of ( 0.1 mathrm{M} ) sodium hydroxide solution, the amount of sodium sulphate formed and its molarity in the solution obtained is ? A. ( 0.1 mathrm{molL}^{-1} ) B. ( 7.10 g ) c. 0.025 mol ( L^{-1} ) D. ( 3.55 g ) |
12 |

667 | A ( 500 g ) tooth paste sample has ( 0.02 g m ) fluoride concentration. What is the concentration of fluorine in terms of ppm levels? A .250 B. 40 c. 400 D. 1000 |
12 |

668 | The vapour pressure of two pure liquids ( A ) and ( B ) are 50 and 40 torr respectively. If 8 moles of ( A ) is mixed with ( x ) moles of B, then vapour pressure of solution obtained is 48 torr. What is the value of x? |
12 |

669 | Which of the following dissolves more rapidly in blood haemoglobin than oxygen? A. Ozone B. Nitrous oxide c. sulphur dioxide D. Carbon monoxide |
12 |

670 | 1. What should be the boiling point of 1.0 molal aqueous KCl solution (assuming complete dissociation of KCT)if| K, HO is 0.52 K m-l? a. 100.52°C b. 101.04°C c. 99.48°C d. 98.96°C |
12 |

671 | The normal boiling point of a liquid is that temperature at which vapour pressure of the liquid is equal to: A. zero B. 380 mm of Hg c. ( 760 mathrm{mm} ) of ( mathrm{Hg} ) D. ( 100 mathrm{mm} ) of ( mathrm{Hg} ) |
12 |

672 | A ( 5.25 % ) solution of a substance is isotonic with a ( 1.5 % ) solution of urea (molar mass ( =60 g ) mol ( ^{-1} ) ) in the same solvent. If the densities of both the solutions are assumed to be equal to ( 1.0 g c m^{-3}, ) molar mass of the substance will be: в. ( 90.0 g ) mol( ^{-1} ) c. ( 115.0 g ) mol ( ^{-1} ) D. ( 105.0 g ) mol ( ^{-1} ) |
12 |

673 | How many grams of NaCl will be required to make a ( 100 . ) milliliters of ( 2 mathrm{M} ) solution? A . 5.85 в. 11.7 c. 29.2 D. 58.5 E .117 |
12 |

674 | If 1 mole of ethyl alcohol in 1,000 grams of water depresses the freezing point by ( 1.86^{circ} mathrm{C}, ) what will be the freezing point of a solution of 1 mole of ethyl alcohol in ( mathbf{5 0 0} ) grams of water? A ( .-0.93^{circ} mathrm{C} ) В. ( -1.86^{circ} mathrm{C} ) ( mathbf{c} cdot-2.79^{circ} mathrm{C} ) D. ( -3.72^{circ} mathrm{C} ) E . ( -5.58^{circ} mathrm{C} ) |
12 |

675 | The mole fraction of methanol in 4.5 molal aqueous solution is: A. 0.250 B. 0.125 c. 0.100 D. 0.075 E. 0.055 |
12 |

676 | A solution is prepared by dissolving ( 5.64 mathrm{g} ) of glucose in ( 60 mathrm{g} ) of water. Calculate the molality of the solution. A. ( 0.281 mathrm{m} ) B. 1.21 ( mathrm{m} ) ( c cdot 1.044 mathrm{m} ) D. 0.522 ( mathrm{m} ) |
12 |

677 | A ( 0.01 m ) aqueous solution of ( boldsymbol{K}_{3}left[boldsymbol{F} boldsymbol{e}(boldsymbol{C} boldsymbol{N})_{6}right] ) freezes ( mathbf{a t}-mathbf{0 . 0 6 2}^{circ} boldsymbol{C} ) What is the apparent percentage of dissociation? ( left[boldsymbol{K}_{f} text { for water }=mathbf{1 . 8 6}right] ) [Note : write the value to the nearest integer |
12 |

678 | What is the molarity of a solution that has 29.25 grams of NaCl dissolved to make ( 1.5 mathrm{L} ) of a solution? A . 19.5 М B. 3.0 М c. 1.75 М D. 0.33 м E ( .1 .0 mathrm{M} ) |
12 |

679 | Van’t Hoff factor of a mixture of two moles of KI with 1 mole ( H g I_{2} ) in a solution of water is : |
12 |

680 | An aqueous solution of glucose is ( 10 % ) (w/v). The volume in which 1 mole of glucose is dissolved, will be: ( mathbf{A} cdot 180 mathrm{L} ) B. 91 L c. ( 0.91 mathrm{L} ) D. 1.8 L |
12 |

681 | Vapour pressure of chloroform ( left(C H C l_{3}right) ) and dichloromethane ( left(C H_{2} C l_{2}right) ) at ( 298 K ) are ( 200 m m H g ) and 415 mm ( H g ) respectively. (i) Calculate the vapour pressure of the solution prepared by mixing ( 25.5 g ) of ( boldsymbol{C H} boldsymbol{C l}_{3} ) and ( mathbf{4 0} boldsymbol{g} ) of ( boldsymbol{C H}_{2} boldsymbol{C l}_{2} ) at ( boldsymbol{2} boldsymbol{9 0} boldsymbol{K} ) and (ii) Mole fraction of each component in solution. |
12 |

682 | In the system ( : boldsymbol{F e}(boldsymbol{O H})_{3(s)} rightleftharpoons boldsymbol{F e}_{(a q)}^{3+}+ ) ( 3 O H_{(a q)}^{-}, ) decreasing the conc. of ( O H^{-} ) ions ( frac{1}{3} ) times will cause the equilibrium conc of ( F e^{3+} ) to increase times. ( A cdot 3 ) B. 9 c. 18 D. 27 |
12 |

683 | In reverse osmosis the flow of solvent molecules is from: A. solution side to solvent side B. solvent side to solution side c. solvent molecules stay unmoving D. none of these |
12 |

684 | ( 1 times 10^{-3} mathrm{kg} ) of urea is present in 400 cubic centimetre solution at ( 310 mathrm{K} ) Calculate the approximate osmotic pressure of the solution. ( left(boldsymbol{R}=mathbf{8 . 3 1 4} boldsymbol{J} boldsymbol{m o l}^{-1} boldsymbol{K}^{-1}, ) molecular right. weight of urea ( =60 ) ) ( A cdot 1 ) atm B. 2 atm ( c cdot 4 a t m ) ( D cdot 5 ) atm |
12 |

685 | The potential of hydrogen electrode is ( -118.5 mathrm{mV} . ) The ( H^{+} ) concentration of the solution is: A . 0.01 M в. 2 м ( c cdot 10^{-4} ) м D. 1 M |
12 |

686 | Hlustration 2.113 An aqueous solution of a non-volatile solute boils at 100.17°C.At what temperature will the solution freeze? (Given: K = 0.512 and K. = 1.86) |
12 |

687 | The Henry’s law constant for helium gas in water at ( 30^{circ} mathrm{C} ) is ( 3.70 times 10^{-4} mathrm{M} / mathrm{atm} ) When the partial pressure of helium above a sample of water is 0.650 at ( mathrm{m} ) the concentration of helium in the water is M. A. ( 5.69 times 10^{-4} ) В. ( 1.76 times 10^{3} ) c. 1.30 D. ( 2.41 times 10^{-4} ) E . ( 3.70 times 10^{-4} ) |
12 |

688 | The value of van’t Hoff factor for ( 0.1 mathrm{M} ) ( B aleft(N O_{3}right)_{2} ) solution is ( 2.74 . ) The degree of dissociation is: ( mathbf{A} cdot 100 % ) B. ( 92 % ) c. ( 87 % ) D. ( 74 % ) |
12 |

689 | Which of the following forms ideal solution?
This question has multiple correct options |
12 |

690 | The freezing point depression of 0.1 molal solution of acetic acid in benzene is ( 0.256 mathrm{K}, K_{f} ) for benzene is ( 5.12 K K g m o l^{-1} . ) What condition can you draw about the molecular state of acetic acid in benzene? A. Acetic acid is doubly associated B. Benzene is doubly associated c. Both are equally associated D. None of the above |
12 |

691 | Henry’s Law constant for ( C O_{2} ) in water is ( 1.67 times 10^{8} ) Pa at ( 298 mathrm{K} ). Calculate the quantity in 1 L of soda water when packed under 2.5 atm pressure at 298 ( mathrm{K} ) |
12 |

692 | ( F e C l_{3} ) on reaction with ( K_{4}left[F e(C N)_{6}right] ) in aqueous solution gives blue colour These are separated by a semipermeable membrane AB as shown. Due to osmosis, there is: A. Blue color formation in side ( x ) B. Blue color formation in side Y. c. Blue colour formation in both of the sides ( x ) and D. No blue colour formation |
12 |

693 | Vapor pressure of pure water at ( 25^{circ} mathrm{C} ) is ( 20.0 mathrm{mm} ) of ( H g % . ) And the lowering of vapor pressure of a sugar solution is ( 0.070 mathrm{mm} ) of ( H g . ) What will be the mole fraction of water? A . 0.9965 B. 0.0035 c. 0.0024 D. 0.7785 |
12 |

694 | An aqueous solution of a weak monobasic acid containing 0.1 g in 21.7 g of water freezes at ( 272.813 mathrm{K} ). If the value of ( K_{f} ) for water is ( 1.86 mathrm{K} / mathrm{m}, ) what is the molecular mass of the monobasic acid. |
12 |

695 | If the various terms in the below-given expressions have usual meanings, the van’t Hoff factor ( ( i ) ) cannot be calculated by which of the following expression? A ( . pi V=sqrt{i n R T} ) B. ( Delta T_{f}=i K_{f}-m ) c. ( Delta T_{b}=i K_{b}-m ) ( frac{P_{text {solvent}}^{o}-P_{text {solution}}}{P_{text {solvent}}^{o}}=ileft(frac{n}{N+n}right) ) |
12 |

696 | Illustration 2.153 What is osmotic pressure and how is it related with the molecular mass of a non-volatile substance? What advantage the osmotic pressure method has over the elevation of boiling point method for determining molecular masses? |
12 |

697 | If ( mathrm{SR}=100 ) torr and ( mathrm{PR}=350 ) torr, then which of the following cannot be a mole fraction of ( A ) in vapour phase and a mole fraction of ( A ) in liquid phase respectively? This question has multiple correct options A ( cdot frac{3}{10} ) and ( frac{2}{9} ) B. ( frac{7}{9} ) and ( frac{3}{10} ) c. ( frac{2}{9} ) and ( frac{7}{10} ) D. ( frac{2}{9} ) and ( frac{3}{10} ) |
12 |

698 | Illustration 2.180 A 0.5% aqueous solution of KCl was found to freeze at -0.24°C. Calculate the Van’t Hoff factor and degree of dissociation of the solute at this concentration. (K, for water = 1.86 K kg mol-l) |
12 |

699 | The solubility of ( N_{2} ) in water at ( 300 mathrm{K} ) and 500 torr, partial pressure is ( 0.01 mathrm{g} ) ( L^{-1} . ) The solubility ( left(operatorname{in} g L^{-1}right) ) at 750 torr partial pressure is: A. 0.0075 B. 0.015 c. 0.02 D. 0.005 |
12 |

700 | The freezing point depression constant for water is ( 1.86^{circ} mathrm{C} boldsymbol{m}^{-1} . ) If ( 5 mathrm{g} N a_{2} mathrm{SO}_{4} ) is dissolved in 45 g ( H_{2} O ), the freezing point is changed by ( -3.82^{circ} mathrm{C} ) Calculate the van’t Hoff factor for ( N a_{2} S O_{4} ) A .0 .381 B . 2.05 ( c .2 .63 ) D. 3.11 |
12 |

701 | Which one of the following is the ratio of the lowering of vapour pressure of ( 0.1 M ) aqueous solution of ( B a C l_{2}, N a C l ) and ( A l_{2}left(S O_{4}right)_{3} ) respectively? A .3: 2: 5 B. 5: 2: 3 ( mathrm{c} .5: 3: 2 ) D. 2: 3: 5 |
12 |

702 | If the concentration of ( O H^{-} ) ions in the reaction ( boldsymbol{F e}(boldsymbol{O H})_{3}(boldsymbol{s}) rightleftharpoons boldsymbol{F} boldsymbol{e}^{+3}(boldsymbol{a q} cdot)+ ) ( 3 O H^{-}(a q .) ) is decreased upto ( frac{1}{4} ) times then equilibrium concentration of ( boldsymbol{F} boldsymbol{e}^{+} ) will increase upto: A. 16 times B. 64 times c. 4 times D. 8 times |
12 |

703 | An azeotropic solution of two liquids has boiling point lower than either of them when it: A. shows a negative deviation from Raoult’s law B. shows no deviation from Raoult’s law c. shows positive deviation from Raoult’s law D. is saturated |
12 |

704 | Ulustration 2.147 Outer hard shells of two eggs are removed. One of the eggs is placed in pure water and the other is placed in saturated solution of sodium chloride. What will be observed and why? |
12 |

705 | In a mixture of kerosene and water, kerosene forms the: A. Lower layer B. Upper layer c. It mixes with water and forms no layer D. Data insufficient |
12 |

706 | Vapour pressure of a pure liquid ( X ) is 2 ( operatorname{atm} ) at ( 300 mathrm{K} ). It is lowered to 1 atm on dissolving 1 g of ( Y ) in ( 20 g ) of liquid ( X ). If molar mass of ( X ) is 200 , what is the molar mass of ( Y ? ) A . 20 B. 10 c. 100 D. 30 |
12 |

707 | Which of the following solution has the highest boiling point? A. ( 1 % ) glucose B . ( 1 % ) NaCl c. ( 1 % ) sucrose D. ( 1 % ) CaCl( _{2} ), |
12 |

708 | Assertion: The rate at which sugar dissolves in water increases with stirring Reason: Stirring exposes the surface of a solute crystal to a less concentrated layer of solution. A. Both Assertion and Reason are correct and Reason is the correct explanation of Assertion B. Both Assertion and Reason are correct but Reason is the correct explanation of Assertion c. Assertion is correct but Reason is not correct D. Assertion is not correct but Reason is correct E. Both Assertion and Reason are not correct |
12 |

709 | ( 2 S O_{3} rightleftharpoons 2 S O_{2}+O_{2} . ) If ( K_{c}=100, alpha=1 ) half of the reaction is completed, the concentration of ( S O_{3} ) and ( S O_{2} ) are equal, the concentration of ( O_{2} ) is ? A. ( 0.001 M ) M в. ( frac{1}{2} S O_{2} ) ( mathrm{c} cdot 2 ) times of ( mathrm{SO}_{2} ) D. Data incomplete |
12 |

710 | Why do gases always tend to be less soluble in liquids as the temperature is raised? |
12 |

711 | Van’t Hoffs factor for a solution is less than one, what is the conclusion drawn from it. |
12 |

712 | Ethanol-Water mixture(95% by volume of ethanol) forms: A. maximum boiling azeotrope B. minimum boiling azeotrope c. solution which shows negative deviation D. ideal solutions |
12 |

713 | Calculate the molarity of ( 9.8 % ) solution of ( mathbf{H}_{2} mathbf{S O}_{4} ) if the density of the solution is ( 1.02 mathrm{gmL}^{-1} ) |
12 |

714 | ( mathbf{A} ) (homogeneous/heterogeneous) mixture of solute and solvent is known as solution. |
12 |

715 | toppr Q Type your question_ 1. of certain molarity was added gradually. The mass of precipitate produced (in g) were measured and it was plotted against volume of ( A g N O_{3} ) solution added (in ml). Its known that ( A g I ) is precipitated first. Precipitation of ( boldsymbol{B} boldsymbol{r} ) does not start until the already precipitating ( boldsymbol{I}^{-} ) precipitates completely. Find out the value of ( boldsymbol{A B} times ) CD where: ( A B= ) Atomic weight of metal ( M ) ( C D= ) Mole percent of ( N a l ) in original mixture. ( mathbf{A} cdot 4994 ) B . 2040 c. 3202 D. 3332 |
12 |

716 | Total vapour pressure of mixture of 1 mole of ( boldsymbol{A}left(boldsymbol{P}_{A}^{0}=mathbf{1 5 0 m m}right) ) and 2 mole of B ( left(P_{B}^{0}=240 m mright) ) is ( 200 m m . ) In this case: A. There is a positive deviation from Raoult’s law B. There is a negative deviation from Raoult’s law c. There is no deviation from Raoult’s law D. Molecular masses of A & B are also required for calculating deviation |
12 |

717 | A salt is made by adding an excess of an insoluble metal oxide to an acid. How is the excess metal oxide removed from the mixture? A. chromatography B. crystallisation c. distillation D. filtration |
12 |

718 | Concentration 1 microgram per gram is ( boldsymbol{x} ) ppm. Then, the value of ( boldsymbol{x} ) is : | 12 |

719 | 2. The ratio of freezing point depression values of 0.01 M solutions of urea, common salt, and Na SO4 are a. 1:1:1 b. 1:2:1 c. 1:2:3 d. 2:2:3 |
12 |

720 | Select the correct statements. (I) Increase in relative humidity decreases the density of air (II) Increase in relative humidity decreases the rate of evaporation of water (III) Increase in relative humidity decreases the velocity of sound (IV) Increase in relative humidity increases the velocity of sound A . ।, ॥, । v в. ।, и, III ( c cdot 1,1 ) D. I, IV |
12 |

721 | Mention the enthalpy of mixing ( left(triangle_{m i x} Hright) ) value to form an ideal solution. |
12 |

722 | Q. 13 At a given temperature, osmotic pressure of a concentrated solution of a substance ………. (a) is higher than that of a dilute solution (b) is lower than that of a dilute solution (c) is same as that of a dilute solution (d) cannot be compared with osmotic pressure of dilute solution |
12 |

723 | A solution prepared by dissolving a ( 2.50 g ) sample of an unknown compound dissolved in ( 34.0 g ) of benzene, ( C_{6} H_{6} ) boils at ( 1.38^{circ} C ) higher than pure benzene. Which expression gives the molar mass of the unknown compound ( ? ) Compound ( K_{b} ) ( boldsymbol{C}_{6} boldsymbol{H}_{6} quad boldsymbol{2 . 5 3}^{circ} boldsymbol{C} cdot boldsymbol{m}^{-1} ) A ( cdot 2.53 times frac{2.50}{1.38} ) в. ( _{1.38} times frac{34.0}{2.53} times 2.50 ) c. ( 2.50 times 10^{3} times frac{2.53}{34.0} times frac{1}{1.38} ) D. ( 2.50 times 10^{3} times frac{1.38}{34.0} times 2.53 ) |
12 |

724 | When ( 1.88 g ) of ( operatorname{AgBr}(s) ) is added to a ( 10^{-3} M ) aqueous solution of ( K B r, ) the concentration of ( mathrm{Ag} ) is ( 5 times 10^{-10} mathrm{M} ). If the same amount of ( A g B r(s) ) is added to a ( 10^{-2} ) M aqueous solution of ( A g N O_{F} ) the concentration of ( B r^{-} ) is: A . ( 9.4 times 10^{-9} M ) В. ( 5 times 10^{-10} M ) c. ( 1 times 10^{-11} M ) D. ( 5 times 10^{-11} M ) |
12 |

725 | Example 2.15 A 10 g mixture of glucose and urea present in 250 mL solution shows the osmotic pressure of 7.4 atm at 27°C. Calculate % composition of mixture. |
12 |

726 | The sum of mole fractions of solute and solvent of a solution is equal to: A. number of moles of solute B. number of moles of solvent c. number of mole of solution D. unity |
12 |

727 | The plots of ( frac{1}{X_{A}} v s cdot frac{1}{Y_{A}}left(text { where }, X_{A} text { and } Y_{A}right. ) are the mole fraction of liquid ( A ) in liquid and vapour phase respectively) is linear with slope and intercepts respectively ( ^{mathbf{A}} cdot p_{A}^{0} / P_{B}^{0} ) and ( frac{left(P_{A}^{0}-P_{B}^{0}right)}{P_{B}^{0}} ) в. ( quad P_{A}^{0} / P_{B}^{0} ) and ( frac{left(P_{B}^{0}-P_{A}^{0}right)}{P_{B}^{0}} ) ( ^{mathbf{c}} P_{B}^{0} / P_{A}^{0} ) and ( frac{left(P_{A}^{0}-P_{B}^{0}right)}{P_{B}^{0}} ) ( P_{B}^{0} / P_{A}^{0} ) and ( frac{left(P_{B}^{0}-P_{A}^{0}right)}{P_{B}^{0}} ) |
12 |

728 | A solution contains ( 3.22 g ) of ( H C l O_{2} ) in ( 47.0 g ) of water. The freezing point of the solution is ( 271.10 K ) Calculate the fraction of ( H C l O_{2} ) that |
12 |

729 | 0.4 If 500 mL of a 5M solution is diluted to 1500 mL, what will be the molarity of the solution obtained? (a) 1.5 M (b) 1.66 M (c) 0.017 M (d) 1.59 M Thinking |
12 |

730 | The van’s Hoff factor for 0.1 molar ( B aleft(N O_{3}right)_{2} ) solutions is ( 2.74 . ) Its degree of dissociation is: A . 0.74 в. 0.87 c. 0.91 D. 1.0 |
12 |

731 | a. Which gas is dissolved in soft drinks? What will you do to increase the solubility of this gas? |
12 |

732 | Which of the following statment is incorrect? A. Greater the lowering of vapour pressure, greater is the boiling point of the solution B. Greater the lowering of vapour pressure, greater is the freezing point of the solution C. At the freezing point, the solute and the solvent have same vapour pressure D. The units of molal depression constant are ( K m^{-1} ) |
12 |

733 | A tube of uniform cross-sectional area ( 1 c m^{2} ) is closed at one end with the semipermeable membrane. a solution of 5 g glucose per 100 mL is placed inside the tube and is dipped in pure water at ( 27^{circ} mathrm{C} ). When equilibrium is established the height developed in a vertical column in cm is ( 1000 x ). (Assume the density of final glucose solution ( 18 / mathrm{mL} ) Find the value of ( X ) |
12 |

734 | A solution containing 8 g of a substances in 100 g of diethyl ether boils at ( 36.86^{circ} mathrm{C} ). Where as pure ether boils at ( 35.60^{circ} mathrm{C} ). Determine the molecular mass of the solute. (For ether, ( boldsymbol{K}_{boldsymbol{b}}=mathbf{2 . 0 2 mathrm { k }} mathrm{kh} boldsymbol{m o l}^{-1} mathbf{)} ) |
12 |

735 | Example 2.11 A solution containing 6 g of a solute dissolved in 250 cm of water gave an osmotic pressure of 4.5 atm at 27°C. Calculate the boiling point of the solution. The molal elevation constant for water is 0.52°C per 1000 g. |
12 |

736 | Illustration 2.40 Two liquids A and B have vapo pressures in the ratio of paº; PR° = 1: 2 at a certain temperature. Suppose we have an ideal solution of A and B in the mole fraction ratio A:B=1: 2. What would be the mole fraction of A in the vapour in equilibrium with the solution at a given temperature? a. 0.25 b. 0.2 c. 0.5 d. 0.33 |
12 |

737 | . 34 For a binary ideal liquid solution, the variation in total vape versus composition of solution is given by which of the curve (C) p 12- |
12 |

738 | One mole of sugar is dissolved in two moles of water. The vapour pressure of the solution relative to that of pure water is: ( A cdot 2 / 3 ) B. ( 1 / 3 ) c. ( 3 / 2 ) D. ( 1 / 2 ) |
12 |

739 | At a given temperature, total vapour pressure in Torr of a mixture volatile components A and B is given by ( boldsymbol{P}_{text {Total}}=mathbf{1 2 0}-mathbf{7 5 X}_{boldsymbol{B}} ) Hence, vapour pressure of pure ( A ) and ( B ) respectively (in Torr) are? A . 120,75 в. 120, 195 ( c cdot 120,45 ) D. 75, 45 |
12 |

740 | Example 2.32 0.5 m solution of acetic acid (Mw = 60) in benzene (Mw=78) boils at 80.80°C. The normal boiling point of benzene is 80.10°C and Ava H=30.775 kJ mol-1. Calculate the percent of association of acetic acid in benzene. |
12 |

741 | A mixture of ( a ) mol of ( C_{3} H_{8} ) and ( b ) mol of ( C_{2} H_{4} ) was kept is a container of ( V ) L which exerts a pressure of 4.93 atm at temperature T. Mixture was burnt in presence of ( O_{2} ) to convert ( C_{3} H_{8} ) and ( C_{2} H_{4} ) into ( C O_{2} ) in the container at the same temperature. The pressure of gases after the reaction and attaining the thermal equilibrium with atmosphere at temperature T was found to be 11.08 atm. The mole fraction of ( C_{3} H_{8} ) in the |
12 |

742 | Which of the following graph shows the best relationship of the number of grams of a solid that are soluble in 100 ( operatorname{grams} ) of ( H_{2} O ) at varying temperature if the solubility begins at a small quality and increases at a slow, steady pace as the temperature is increased? ( A cdot A ) B. B ( c cdot c ) D. E. |
12 |

743 | There is ( 50 % ) dimer formation of benzoic ( operatorname{acid}left(C_{6} H_{5} C O O Hright) ) in benzene solution. ( 2 C_{6} H_{5} C O O H rightleftharpoonsleft(C_{6} H_{5} C O O Hright)_{2} ) Hence the abnormal molecular weight of benzoic acid ( theoretical value ( =122 ) ( left.g m o l^{-1}right) ) is: A. ( 61 mathrm{g} ) mol ( ^{-1} ) B. 244 g mol- c. ( 163 mathrm{g} ) mol ( ^{-1} ) D. 81 g ( m o l^{-1} ) |
12 |

744 | ( 2 mathrm{g} ) benzoic acid ( left(C_{6} H_{5} C O O Hright) ) dissolved in 25 g of benzene shoes a depression in freezing point equal to 1.62 K. Molal depression constant for benzene is ( 4.9 mathrm{K} mathrm{kg} ) mol( ^{-1} . ) What is the percentage association of acid if it forms dimer in solution? |
12 |

745 | If quantities ( Delta T_{f}, Delta T_{b}, Delta p ) and ( pi ) without subscript refer to the electrolyte solution and these with subscript refer to non-electrolyte solution then which one is wrong? ( ^{mathbf{A}} cdot_{i}=frac{Delta T_{f}}{left(Delta T_{f}right)_{0}} ) в. ( _{i}=frac{Delta T_{b}}{left(Delta T_{b}right)_{0}} ) c. ( _{i}=frac{Delta P}{left(P^{0}right)_{0}} ) D. ( _{i}=frac{pi}{(pi)_{0}} ) |
12 |

746 | If ( 6.022 times 10^{23} ) molecules of urea are present in 100 ml of its solution, then calculate the concentration of the solution (Molecular mass of urea ( =mathbf{6 0} ) ) |
12 |

747 | 0.56 Using Raoult’s law explain how the total vapour pressure over the solution is related to mole fraction of components in the following solutions. (a) CHCL3 (L) and CH,CL, (l) (b) NaCl(s) and H20 (1) |
12 |

748 | A ( 500 mathrm{mL} ) solution is prepared by dissolving 20 g sodium hydroxide in water. This is mixed in another ( 200 mathrm{mL} ) solution of ( N a O H ) having molarity 0.2 M. The molarity of resulting solution is: A. 0.66 M в. 0.77 М c. ( 1.80 mathrm{M} ) D. 1.97 М |
12 |

749 | Illustration 2.88 The boiling point of a solution made by dissolving 12.0 g of glucose in 100 g of water is 100.34°C. Calculate the molecular weight of glucose; K, for water = 0.52°C/m. |
12 |

750 | Which of the following may be dissolved in water? A. Alcohol B. Ether c. Amine D. all of these |
12 |

751 | Unsaturated solvents are filled with solutes. A. completely B. not completely c. Both a and D. None of the above |
12 |

752 | A solution of a substance containing 1.05 g per 100 mL was found to be isotonic with ( 3 % ) glucose solution. The molecular mass of the substance is: A . 31.5 B. 6.3 ( c .630 ) D. 63 |
12 |

753 | Two liquids ( A ) and ( B ) have vapour pressures in the ratio ( P_{A}^{0}: P_{B}^{0}=2: 3 ) at a certain temperature. Assuming that ( mathbf{A} ) and ( mathrm{B} ) form an ideal solution and ratio of mole fractions of ( A ) and ( B ) in the vapour phase is ( 1: 3, ) then the mole fraction of ( mathbf{A} ) in the solution at the same temperature is : A ( cdot frac{1}{3} ) B. ( frac{2}{3} ) c. ( frac{1}{4} ) D. ( frac{3}{4} ) |
12 |

754 | A mixture of ethanol and ( C C l_{4} ) has ( 30 % ) ( C C l_{4} ) by weight, what is mole fraction of ( boldsymbol{C C l}_{4} ) in the mixture? A . 0.11 B. 0.89 c. 0.25 D. 0.67 |
12 |

755 | Which one is correct for a solution? A. Saturated and dilute B. Supersaturated and saturated C. Saturated and unsaturated D. Dilute and concentrated |
12 |

756 | An ideal gas, of volume ( 189 m L ), is collected over water. The temperature is ( 27^{circ} mathrm{C}, ) and the barometric pressure is ( 756 m m H g . A t 27^{circ} C, ) the vapor pressure of water is 27 mm ( H g ) Which of the following CORRECTLY gives the mole fraction of water vapor in the collection vessel? A ( cdot frac{27}{756} ) в. ( frac{27}{729} ) c. ( frac{729}{756} ) D. ( frac{729}{27} ) |
12 |

757 | Which of the following correctly represent solubility of ( N_{2} ) in water (in terms of mmole/litre) if ( N_{2} ) is bubbled through water at ( 293 K ) at a pressure of 0.768 bar and Henry’s constant is ( mathbf{7 6 . 8} K ) at ( mathbf{2 9 3} mathbf{K} ? ) A ( cdot 10^{-5} ) 5 В. ( 5.56 times 10^{-4} ) ( c cdot 10^{-2} ) D. ( 4.3 times 10^{-4} ) |
12 |

758 | Assertion Decrease in the vapour pressure of water by adding 1 mol of sucrose to one jg of water is higher to that produced by adding 1 mol of urea to the same quantity of water at the same temperature. Reason Molecular mass of sugar is less than that of urea. A. Both Assertion and Reason are correct and Reason is the correct explanation for Assertion B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion C. Assertion is correct but Reason is incorrect D. Both Assertion and Reason are incorrect |
12 |

759 | ml were taken. One of these beakers, h 400 mL water whereas the beaker labelled 2. 22 Two beakers of capacity 500 mL were taken. One labelled as “A”, was filled with 400 mL water whereas the “B’ was filled with 400 mL of 2M solution o h 400 mL of 2M solution of NaCl. At the same temperature both the beakers were placed in closed ne beakers were placed in closed containers of same material and same capacity as shown in figure. Water NaCl solution At a given temperature, which of the following statement is correct about the vapour pressure of pure water and that of NaCl solution? (a) Vapour pressure in container (A) is more than that in container (B) (b) Vapour pressure in container (A) is less than that in container (B) (c) Vapour pressure is equal in both the containers (d) Vapour pressure in container (B) is twice the vapour pressure in container (A) Com |
12 |

760 | The amount of the solute present in the saturated solution at a particular temperature is called its: A. solubility B. saturation c. solvent concentration D. none of the above |
12 |

761 | Mlustration 2.81 2 g each of two solutes A and B (molar mass of A is greater than that of B) are dissolved separately in 50 g each of the same solvent. Which will show greater elevation in the boiling point? |
12 |

762 | Illustration 2.75 Calculate the vapour pressure of an aqueous solution which contains 5 mass per per cent of urea. The vapour pressure of pure water is 23.5 mm Hg. The molar mass of urea is 60. |
12 |

763 | Which option is inconsistent for Raoult’s Jaw? A. The change in heat of dilution for solution ( =0 ) B. Volume of liquid solvent + volume of liquid solute = volume of solution C. Solute does not undergo association in solution D. Solute undergoes dissociation in solution |
12 |

764 | Illustration 2.67 What mass of non-volatile solute (urea) needs to be dissolved in 100 g of water in order to decrease the vapour pressure of water by 30%. What will be the molality of solution? |
12 |

765 | Example 2.19 Calculate osmotic pressure of a solution obtained by mixing 100 mL of 3.4% solution (weight/volume) of urea (molecular weight 60) and 100 mL of 1.6% solution (weight/volume) of cane sugar (molecular weight 342) at 20°C. |
12 |

766 | Assertion Acetone-Carbon disulphide solution shows positive deviation from Raoult’s law. Reason Acetone ( + ) Aniline solution shows positive deviation from Raoult’s law. A. Both Assertion and Reason are correct and Reason is the correct explanation for Assertion B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion c. Assertion is correct but Reason is incorrect D. Both Assertion and Reason are incorrect |
12 |

767 | ( boldsymbol{F} boldsymbol{e} boldsymbol{C l}_{3} ) on reaction with ( boldsymbol{K}_{boldsymbol{4}}left[boldsymbol{F} boldsymbol{e}(boldsymbol{C} boldsymbol{N})_{boldsymbol{6}}right] ) in aqueous solution gives blue colour. These are separated by a semipermeable membrane ( A B ) as shown. Due to osmosis there is: A. blue colour formation in side ( X ) B. blue colour formation in side ( Y ). c. blue colour formation in both of the sides ( X ) and ( Y ). D. no blue colour formation |
12 |

768 | Vapour is injected at a uniform rate in a closed vessel which was initially evacuated. The pressure in the vessel A. Increases continuously B. Decreases continuously c. First increases and then decreases D. First increases and then becomes cosntant |
12 |

769 | A solution containing 3.3 g of a substance in 125 g of benzene (b.pt. ( = ) ( 80^{circ} mathrm{C} ) ) boils at ( 80.66^{circ} mathrm{C} ). If ( mathrm{K}_{b} ) for benzene is ( 3.28 mathrm{K} mathrm{kg} ) mol( ^{-1} ) the molecular mass of the substance will be: A . 130.20 B. 129.20 c. 132.20 D. 131.20 |
12 |

770 | Ilustration 2.192 A saturated solution of Mg(OH), has a vapour pressure of 759.5 mm at 373 K. Calculate the solubility and Kp of Mg(OH)2. (Assume molarity equals molality) |
12 |

771 | Define mole fraction. A solution of sucrose in water is labelled as ( 20 % ) w/w. What would be the mole fraction of each component in the solution? |
12 |

772 | For electrolytic solution, the Van’t Hoff factor (i) is always equals to unity. A. True B. False |
12 |

773 | With increase in pressure This question has multiple correct options A. solubility of solids in liquids is unaffected B. solubility of solids decreases C . solubility of gases decreases in liquids D. solubility of gases in liquids increases |
12 |

774 | The ratio of the molar amounts of ( boldsymbol{H}_{2} boldsymbol{S} ) needed to precipitate the metal ions from ( 20 mathrm{ml} ) each of ( 1 mathrm{M} C dleft(N O_{3}right)_{2} ) and ( mathbf{0 . 5} boldsymbol{M} boldsymbol{C u} boldsymbol{S O}_{4} ) is: A . 1: B. 2:1 ( c cdot 1: 2 ) D. indefinite |
12 |

775 | Two elements ( A ) and ( B ) form ideal compounds of formula ( A B_{2} ) and ( A B_{4} ) When dissolved in ( 20.0 g ) of benzene 1.0 ( g ) of ( A B_{2} ) lowers freezing point by ( 2.3^{0} C ) whereas ( 1.0 g ) of ( A B_{4} ) lowers freezing point by ( 1.3^{0} mathrm{C} ). The ( K_{f} ) for benzene is ( 5.4 . ) The atomic masses of ( A ) and ( B ) are: A .27,45 в. 42,25 c. 52,48 D. 48,52 |
12 |

776 | ( mathrm{CoCl}_{3} cdot 3 mathrm{NH}_{3} ) does not form any precipitate with excess ( A g N O_{3} ) solution, whereas 1 mole of ( mathrm{CoCl}_{3} cdot 5 mathrm{NH}_{3} ) gives two moles of ( mathrm{AgCl} ) with excess ( A g N O_{3} . ) The van’t Hoff factor for both the compounds respectively are: A. 0 and 2 B. O and 3 ( c cdot 1 ) and 3 D. 1 and 2 |
12 |

777 | For one mole of a pure substance free energy is identical with: | 12 |

778 | Azeotropic mixture: A. Boil at different temperature B. Are mixture of solids C. Are constant boiling mixture D. Gaseous mixture |
12 |

779 | A mixture of ethanol and propanol has vapor pressure ( 279 mathrm{mm} ) of ( mathrm{Hg} ) at ( 300 mathrm{K} ) The mol fraction of ethanol in the solution is 0.6 and vapour pressure of pure propanol is ( 210 mathrm{mm} ) of Hg. Vapour pressure of pure ethanol will be: ( mathbf{A} cdot 336.6 mathrm{mm} ) B . ( 325 mathrm{mm} ) c. ( 375 mathrm{mm} ) D. ( 415 mathrm{mm} ) |
12 |

780 | Illustration 2.195 A 0.025 m solution of monobasic acids has a freezing point of -0.060°C. What are K, and pk of the acid? (K. = 1.86°C) |
12 |

781 | At ( 80^{0} mathrm{C}, ) the vapour pressure of pure liquid ( A ) is ( 250 m m ) of ( H g ) and that of pure liquid B is ( 1000 mathrm{mm} ) of Hg. If a solution of ( A ) and ( B ) boils at ( 80^{circ} mathrm{C} ) and 1 atm pressure, the amount of A in the mixture is : ( (1 a t m=760 m m H g) ) A . 50 mole percent B. 52 mole percent c. 32 mole percent D. 48 mole percent |
12 |

782 | Pick out the liquid-in-gas type of mixture from the following. A. Dissolved carbon dioxide in water B. Droplets of water in air C. Oxygen dissolved in water D. All of the above |
12 |

783 | The values of van’t Hoff factors for ( K C l, N a C l ) and ( K_{2} S O_{4} ) respectively are: A. 1,1,2 B. 1,1,1 c. 2,2,3 D. 2,3,2 |
12 |

784 | ( mathbf{0 . 1} boldsymbol{M} boldsymbol{K}_{mathbf{4}}left[boldsymbol{F} e(boldsymbol{C} boldsymbol{N})_{mathbf{6}}right] ) is 60% ionized. What will be its van’t Hoff factor? A . 1.4 B. 2.4 c. 3.4 D. 4.4 |
12 |

785 | How much ( B a C l_{2} ) would be needed to make 250 ml of a solution having the same concentration of ( C l^{-} ) as one containing ( 3.78 g N a C l ) per 100 ml? ( (B a=137) ) A. ( 22.4 g ) в. ( 16.8 g ) c. ( 67.2 g ) D. 33.6 ( g ) |
12 |

786 | Heptane and octane form an ideal solution. At ( 373 K ), the vapour pressures of the two liquid components are ( 105.2 k P a ) and ( 46.8 k P a ) respectively. What will be the vapour pressure of a mixture of ( 26.0 mathrm{g} ) of heptane and ( 35 g ) of octane? |
12 |

787 | Q. 9 What is the mass per cent of carbon in carbon dioxide? (a) 0.034% (b) 27.27% (c) 3.4% (d) 28.7% |
12 |

788 | At ( 80^{circ} mathrm{C}, ) the vapour pressure of pure liquid ( mathbf{A}^{prime} ) is ( mathbf{5} mathbf{2 0} mathbf{m m} mathbf{H} boldsymbol{g} ) and that of pure liquid B’ is 1000 mm ( H g ). If a mixture solution of ( mathbf{A}^{prime} ) and ( mathbf{B}^{prime} ) boils at ( 80^{circ} mathrm{C} ) and 1 atm pressure, the amount of A’ in the mixture is: ( [1 a t m=760 m m H g] ) A. 48 mol% B . 50 mol% c. 52 mol% D. 34 mol% |
12 |

789 | The correct relation between elevation of boiling point and molar mass of solute is: A ( ldots_{M_{2}}=frac{K_{b} times W_{2}}{Delta T_{b} times W_{1}} ) В. ( M_{2}=frac{K_{b} times W_{1}}{Delta T_{b} times W_{2}} ) ( ^{mathrm{C}} cdot_{M_{2}}=frac{Delta T_{b} times K_{b}}{W_{1} times W_{2}} ) D. ( M_{2}=frac{Delta T_{b} times W_{1}}{K_{b} times W_{2}} ) |
12 |

790 | Q. 3 What will be the molarity of a solution, which contains 5.85 g of NaCl(s per 500 mL? (a) 4 mol L-1 (b) 20 mol L-1 (c) 0.2 mol L-1 (d) 2 mol L-1 |
12 |

791 | Compute the molar solubility of water that is saturated with air. ( left[text { Given: } k=0.00105 mathrm{M} / mathrm{atm}, P_{N e} text { in air }=right. ) ( 0.0341 mathrm{atm}] ) A ( .2 .56 times 10^{-2} M ) в. ( 3.58 times 10^{-5} M ) c. ( 4.44 times 10^{-6} M ) D. ( 2.78 times 10^{-4} M ) |
12 |

792 | State True or False. For a non-ideal solution, ( Delta_{m i x} V ) and ( Delta_{m i x} H ) are zero. A . True B. False |
12 |

793 | Estimate the lowering of vapour pressure due to the solute (glucose) in a ( 1.0 mathrm{M} ) aqueous solution at ( 100^{circ} mathrm{C} ) A . 10 torr B. 18 torr c. 13.45 torr D. 24 torr |
12 |

794 | At ( 400^{circ} mathrm{C}, ) the vapour pressure of water is 55.3 mm ( H g ). Calculate the vapour pressure at the same temperature over ( 10 % ) aqueous solution of urea ( left[boldsymbol{C O}left(boldsymbol{N} boldsymbol{H}_{2}right)_{2}right] ? ) |
12 |

795 | When 3 L of ( 0.5 ~ M ) NaCl is mixed with ( 9 mathrm{L} ) of ( 0.2777 M N a C l, ) determine the concentration of the final solution, assuming that volumes are additive? A. 0.33 M . В. 0.39 М c. ( 0.5777 M ) D. ( 0.7777 M ) E. None of the above |
12 |

796 | When an azeotropic mixture is distilled, its composition remains unchanged If true enter ( 1, ) if false enter 0 |
12 |

797 | Question 41. Determine the osmotic pressure of a solution prepared by dissolving 25 mg of K2SO4 in 2 L of water at 25°C, assuming that it is completely dissociated. Apply van’t Hoff equation, n = iCRT, where, i = Number of ions produced by K2SO4). |
12 |

798 | Increase of temperature of an aqueous solution will cause: A. decrease in molality of the solution B. decrease in molarity of the solution c. decrease in mole fraction of the solution D. decrease in percentage (w/w) of the solution |
12 |

799 | 3. From a measurement of the freezing point depression of benzene, the molecular weight of acetic acid in a benzene solution was determined to be 100. The percentage association of acetic acid is a. 79% b. 93% c. 80% d. 100% |
12 |

800 | Illustration 2.59 Two liquids A and B on mixing produce a warm solution. Which type of deviation from Raoult’s law does it show? |
12 |

801 | Positive deviation from ideal behaviour takes place because of : A . molecular interaction between atoms and ( frac{P V}{n R T}>1 ) B. molecular interaction between atoms and ( frac{P V}{n R T}1 ) D tinite size of atoms and ( frac{P V}{n R T}<1 ) |
12 |

802 | Dilute ( 20.8 mathrm{mL} ) of ( 6.0 mathrm{M} mathrm{H}_{2} mathrm{SO}_{4} ) to a volume of 1 L. The concentration of the resultant ( boldsymbol{H}_{2} boldsymbol{S} boldsymbol{O}_{4} ) solution is ( boldsymbol{2 5} boldsymbol{y} times ) ( 10^{-3} M, ) then ( y ) is |
12 |

803 | ( 1.5 mathrm{g} ) of a monobasic acid, when dissolved in 150 g of water, lowers the freezing point by ( 0.165^{circ} mathrm{C} .0 .5 mathrm{g} ) of the same acid when titrated, after dissolution in water, requires ( 37.5 mathrm{ml} ) of N/10 alkali. Calculate the degree of dissociation of the acid ( ?left(K_{f} text { for water }=right. ) ( left.1.86^{circ} mathrm{C} mathrm{mol}^{-1}right) ) A . ( 11.34 % ) в. ( 34.64 % ) c. ( 65.36 % ) D. ( 89.64 % ) |
12 |

804 | How many grams of ( N a O H ) are needed to make ( 100 g ) of a ( 5 % ) solution? ( A cdot 2 ) B. 5 c. 20 D. 40 E . 95 |
12 |

805 | Illustration 2.49 Two liquids A and B form an ideal solution at temperature T. When the total vapour pressure above the solution is 600 torr, the amount fraction of A in the vapour phase is 0.40 and in the liquid phase is 0.60. What are the vapour pressures of pure A and pure B at temperature T? 11 |
12 |

806 | The azeotropic mixture of water and HCl boils at ( 108.5^{circ} mathrm{C} ). When this mixture is distilled, it is possible to obtain A. pure ( H C l ) B. pure water c. neither pure HCI nor pure water D. both pure HCl and pure water |
12 |

807 | Ilustration 2.120 What mass of sugar C, H,0,(M,=342) must be dissolved in 4.0 kg of 1,0 to yield a solution that will freeze at -3.72°C. (Take Kg = 1.86°C m-1) |
12 |

808 | e. 17 Value of Henry’s constant KH ……….. (a) increases with increase in temperature (b) decreases with increase in temperature (c) remains constant (d) first increases then decreases |
12 |

809 | The relationship between the values of osmotic pressure of ( 0.1 mathrm{M} ) solutions of ( boldsymbol{K} boldsymbol{N} boldsymbol{O}_{3}left(boldsymbol{P}_{1}right) ) and ( boldsymbol{C} boldsymbol{H}_{3} boldsymbol{C O O H}left(boldsymbol{P}_{2}right) ) is: A ( cdot P_{1}>P_{2} ) в. ( P_{2}>P_{1} ) ( mathrm{c} cdot P_{1}=P_{2} ) D. ( frac{P_{1}}{P_{1}+P_{2}}=frac{P_{2}}{P_{1}+2 P_{2}} ) |
12 |

810 | What is Raoult’s Law? Derive Raoult’s Law for solution which contain non-volatile solute. |
12 |

811 | Illustration 2.186 Calculate the amount of NaCl which must be added to 100 g water so that the freezing point, depressed by 2 K. For water K = 1.86 K kg mol-1. |
12 |

812 | ( mathbf{A} ) 1.00 molal aqueous solution of trichloroacetic acid ( left(C C l_{3} C O O Hright) ) is heated to its boiling point. The solution has the boiling point of ( 100.18^{circ} mathrm{C} ) Determine the van’t Hoff factor for trichloroacetic acid. ( left(K_{b} text { for water }=right. ) ( 0.512 mathrm{K} mathrm{kg} mathrm{mol}^{-1} ) ) |
12 |

813 | Osmotic pressure of a solution is: This question has multiple correct options A. directly proportional to the molar concentration of the solution B. inversely proportional to the molecular weight of the solute C. inversely proportional to the temperature D. directly proportional to the volume of the solution |
12 |

814 | What concentration of nitrogen should be present in a glass of water at room temperature? Assume a temperature of ( 25^{circ} mathrm{C}, ) a total pressure of 1 atmosphere and mole fraction of nitrogen in air of ( 0.78 .left(K_{H} text { for nitrogen }=8.42 times 10^{-7}right. ) ( mathrm{M} / mathrm{mm} mathrm{Hg} ) |
12 |

815 | Illustration 2.208 The vapour pressure of benzene at 30°C is 164.88 mm of Hg. In 3 mol of benzene, when 6 g of acetic acid was dissolved, the vapour pressure of the solution became 162.04 mm of Hg. Calculate a. Van’t Hoff factor b. The degree of association of acetic acid in benzene at 30°C |
12 |

816 | The percentage of ( F e(I I I) ) present in iron ore ( F e_{0} .9301 .00 ) is ( (F e=56) ) A . 94 B. 6 c. 21.5 D. 15 |
12 |

817 | When ( H g I_{2} ) is added to aqueous solution of ( mathrm{KI} ), why there is an increase in vapour pressure of solution? |
12 |

818 | Explain with a suitable diagram and appropriate examples why some nonideal solutions show positive deviation from ideal behaviour. |
12 |

819 | 4. 0.6 g of a solute is dissolved in 0.1 L of a solvent which develops an osmotic pressure of 1.23 atm at 27°C. The molecular weight of the solute is a. 149.5 g mol- b. 120.0 g mol-1 c. 430.0 g mol-1 d. None of these |
12 |

820 | Which one will have highest boiling point, if 1 mole of each of the following substances was discovered in 1,000 grams of water? A. Nacı в. кс। c. ( C a C l_{2} ) D. ( C_{6} H_{10} O_{5} ) E ( cdot C_{12} H_{22} O_{11} ) |
12 |

821 | What will be the vapour pressure of a solution containing 5 moles of sucrose ( left(C_{12} H_{22} O_{11}right) ) in ( 1 k g ) of water, if the vapour pressure of pure water is ( 4.57 m m ) of ( H g ?[C=12, H=1, O= ) ( mathbf{1 6}] ) |
12 |

822 | If liquids ( A ) and ( B ) form an ideal solution, then : A. the entropy of mixing will be zero B. the Gibbs free energy of mixing will be zero C. the Gibbs free energy as well as the entropy of mixing both will be zero D. the enthalpy of mixing will be zero |
12 |

823 | Pressure over ideal binary liquid mixture containing 10 moles each of liquid ( A ) and ( B ) is gradually decreased isothermally. If ( P_{A}^{circ}=200 m m H g ) and ( P_{B}^{circ}=100 m m H g, ) the pressure at which half of the liquid is converted into vapour is: A. ( 150 mathrm{mm} ) Hg в. ( 166.5 mathrm{mm} ) ну c. ( 133 mathrm{mm} ) нg D. 141.4 mm нg |
12 |

824 | 5. The Van’t Hoff factor for a 0.1 MALL(SO2)2 solution is 4.20. The degree of dissociation is a. 80% b. 90% c. 78% d. 83% |
12 |

825 | A solution containing ( 62 g ) ethyl glycol in ( 250 g ) water is cooled to ( -10^{circ} mathrm{C} ). If ( K_{f} ) for water is ( 1.86 K k g m o l^{-1}, ) the amount of water ( (text { in } g ) ) separated as ice is: A . 32 B. 48 ( c cdot 16 ) D. 64 |
12 |

826 | Assertion The solubility of Ammonium chloride increases with increase in temperature Reason In case of substances whose solubility increases with increase in temperature is due to the dissolution process being endothermic. A. Both Assertion and Reason are correct and Reason is the correct explanation for Assertion B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion c. Assertion is correct but Reason is incorrect D. Both Assertion and Reason are incorrect |
12 |

827 | Assertion Salt dissolved in water lowers the freezing point. Reason The change in freezing point is given by: ( Delta boldsymbol{T}_{boldsymbol{f}}=boldsymbol{i} boldsymbol{K}_{boldsymbol{f}} boldsymbol{m} ) A. Both Assertion and Reason are correct and Reason is the correct explanation for Assertion B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion C. Assertion is correct but Reason is incorrect D. Both Assertion and Reason are incorrect |
12 |

828 | Illustration 2.190 A certain substance A tetramerizes in water to the extent of 80%. A solution of 2.5 g of A in 100 g of water lowers the freezing point by 0.3°C. The molar mass of A is a. 120 b. 61 c. 60 d. 62 |
12 |

829 | Calculate the amount of ( C a C l_{2} ) (van’t Hoff factor ( i=2.47 ) ) dissolved in ( 2.5 L ) solution so that its osmotic pressure at ( 300 K ) is 0.75 atmosphere Given: Molar mass of ( C a C l_{2} ) is ( 111 g cdot m o l^{-1} ) ( boldsymbol{R}=mathbf{0 . 0 8 2} boldsymbol{L} . boldsymbol{a t m} . boldsymbol{K}^{-1} boldsymbol{m o l}^{-1} ) |
12 |

830 | Van’t Hoff factor, when benzoic acid is dissolved in benzene, will be: A . 2 B. ( c .0 .5 ) D. 1.5 |
12 |

831 | State True or False. ( C_{2} H_{5} O H ) and cyclohexane mixture shows positive deviation from Raoult’s law. A. True B. False |
12 |

832 | The vapour pressure of two pure liquids ( A ) and ( B ) which from an ideal solution are 500 and 800 torr respectively at ( 300 K . ) A liquid solution ( A ) and ( B ) for which the mole fraction of ( A ) is 0.60 is contained in a cylinder closed by a piston on which the pressure can be varied. What will be the pressure when 1 mol of the mixture has been vaporized? |
12 |

833 | Question 17. The vapour pressure of water is 12.3 kPa at 300 K. Calculate vapour pressure of 1 molal solution of a non-volatile solute in it. (1) In order to calculate vapour pressure, mole fraction is required but we have molality. So, convert molality into mole fraction by using following steps. (a) Find the moles of solute and mass of solvent from molality. (b) Find of moles of solvent, i.e., water by dividing its mass by molar mass. (c) Find mole fraction of solute, Xo = — o At no (ii) Find mole fraction of solvent xa as XA + X8 = 1 (iii) Finally calculate the vapour pressure by using Raolut’s law, p = pºx. |
12 |

834 | Aquatic species are more comfortable in cold water because of: A. as the temperature decreases, the solubility of dissolved oxygen increases B. as the temperature increases, the solubility of dissolved oxygen increases. c. as the temperature increases, the solubility of dissolved oxygen decreases D. none of the above |
12 |

835 | Concentrated hydrochloric acid is ( 36.5 % ) by weight. What is the molality of the solution? A . 1.575 molal B. 15.75 molall c. 157.5 molal D. 1575 molal |
12 |

836 | A liquid mixture of benzene ( (B) ) and toluene ( (T) ) contains 1 mole each of ( B ) and ( T ) ( boldsymbol{P}_{boldsymbol{T}}^{boldsymbol{o}}=mathbf{4 . 2 7 4} boldsymbol{k} boldsymbol{N} boldsymbol{m}^{-2} ) and ( boldsymbol{P}_{boldsymbol{B}}^{boldsymbol{o}}= ) ( mathbf{1 3 . 7 3 4} mathbf{k} mathbf{N m}^{-mathbf{2}} ) If the pressure is reduced further, pressure ( left(text { in } k N m^{-2}right) ) (write only integer part) at which the last trace of liquid does disappear is |
12 |

837 | The ratio of the value of any colligative property for ( B a C l_{2} ) solution to that for urea solution under similar condition is: A .2 B. 3 ( c ) ( D ) |
12 |

838 | What is the density (in ( g m / )lit ) of wet air with ( 75 % ) relative humidity at 1 at and ( 300 K ? ) Given : vapour pressure of ( H_{2} O ) is 30 torr and average molar mass of air is ( 29 g / ) mol. Write as the nearest integer: |
12 |

839 | The melting point of ice is (a) 273K c) 300K (b) 373K (d) 298 K |
12 |

840 | toppr Q Type your question acids pictured, which of the following would be the LEAST soluble in water? A. Histidine B. Lysine C. Alanine D. Cysteine |
12 |

841 | Derive the relation between elevation of boiling point and molar mass of solute. |
12 |

842 | Elevation in boiling point was ( 0.52^{circ} mathrm{C} ) when 6 g of a compound ( X ) was dissolved in 100 g of water. Molecular mass of the compound M in ( g ) mol ( ^{-1} ) is: ( K_{b} ) for water is ( 0.52 mathrm{Km}^{-1} ).) A . 120 B. 60 ( c cdot 600 ) D. 180 |
12 |

843 | A ( 10 % ) solution (by mass) of sucrose in water has a freezing point of ( 269.15 K ) Calculate the freezing point of ( 10 % ) glucose in water if the freezing point of pure water is ( 273.15 K ) (Given : molar mass of sucrose ( = ) ( 342 g ) mol ( ^{-} ?, ) Molar mass of glucose ( = ) ( left.180 g m o l^{-1}right) ) A. 275. 53 K B. 265. 53 K c. २७१. 32 ( mathrm{K} ) D. 282.43 K |
12 |

844 | When the concentration of ( boldsymbol{K}^{+} ) across a cell membrane drops from ( 0.01 M ) to ( 0.001 M, ) the potential difference across the membrane is: A . ( 0.0 V ) B. ( 0.0059 V ) c. ( 0.059 V ) D. ( 0.59 V ) |
12 |

845 | Illustration 2.143 What is reverse osmosis? | 12 |

846 | 18g glucose and 6 g urea are dissolved in 1 litre aqueous solution at ( 27^{circ} C . ) The osmotic pressure of the solution will be ( mathbf{A} cdot 3.826 mathrm{atm} ) B. 4.926 atm c. 2.92 atm D. 9.42 atm |
12 |

847 | If benzoic acid (mol. mass = 122) is associated into double molecules when dissolved in benzene and the osmotic pressure of a solution of 5 g of benzoic acid in ( 100 mathrm{mL} ) benzene is 5.73 atm at ( 10^{circ} mathrm{C}, ) what is the percentage association of benzoic acid? ( mathbf{A} cdot 60 % ) B. ( 70 % ) ( c .80 % ) D. ( 85 % ) |
12 |

848 | The molal lowering of vapour pressure( in cm to nearest integer) for ( boldsymbol{H}_{2} boldsymbol{O} ) at ( 100^{circ} mathrm{C} ) is |
12 |

849 | If the concentration of water vapour in the air is ( 1 % ) and the total atmospheric pressure equals 1 atm, then the partial pressure of water vapour is? A. ( 0.1 mathrm{atm} ) В. ( 1 mathrm{mm} ) нв ( mathbf{c} .7 .6 mathrm{mm} mathrm{Hg} ) D. 100 atm |
12 |

850 | Assertion The molecules of the dissolved gas present in a liquid gain kinetic energy as temperature is raised. Reason Gases tends to be more soluble in liquids as the temperature is raised. A. Both Assertion and Reason are correct and Reason is the correct explanation for Assertion B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion c. Assertion is correct but Reason is incorrect D. Assertion is incorrect but Reason is correct |
12 |

851 | If relative decrease in ( mathrm{V} . mathrm{P} ) is 0.4 for ( mathrm{a} ) solution containing 1 mol ( N a C l ) in 3 mol of ( mathrm{H}_{2} mathrm{O} ). Calculate ( % ) ionization of NaCl. A . 100 B. 95 c. 90 D. 85 |
12 |

852 | 3. At 27°C. the vapour pressure of an ideal solution containing 1 mole of A and 1 mole of B is 500 mm of Hg. At the same temperature, if 2 mol of B is added to this solution the vapour pressure of solution increases by 50 mm of Hg. The vapour pressure of A and B in their pure states is respectively, a. 600 mm, 400 mm b. 400 mm, 600 mm c. 300 mm, 700 mm d. 200 mm, 800 mm |
12 |

853 | A volume of ( 6 L H_{2} O ) is placed in a closed evacuated room of volume ( 827 L ) at the temperature ( 300 mathrm{K} ). The density of liquid water at ( 300 mathrm{K} ) is ( 1.0 mathrm{g} / mathrm{ml} ). The vapour pressure of water at ( 300 mathrm{K} ) is ( 22.8 mathrm{mm} ) Hg. Neglect the change in volume of liquid water by vaporization. |
12 |

854 | For a non-volatile solute: A. vapour pressure of solution is more than vapour pressure of solvent B. vapour pressure of solvent is zero C. vapour pressure of solute is zero D. all of the above |
12 |

855 | Ilustration 2.89 A solution containing 0.2563 g of naphthalene (molecular mass = 128) in 50 g of carbon tetrachloride yields a boiling point elevation of 0.201°C while a solution of 0.6216 g of an unknown solute in the same mass of the solvent gives a boiling point elevation of 0.647°С. Find the molecular mass of unknown solute. |
12 |

856 | For a dilute solution, mole fraction of solute is given as ( (n= ) no. of moles of solute and ( N=text { no. of moles of solvent }) ) A ( cdot frac{n}{N} ) в. ( frac{N}{n} ) c. ( frac{N}{n+N} ) D. Both B and C |
12 |

857 | Illustration 2.167 A 5% solution of cane sugar is isotonic with 0.877% solution of urea. Calculate the molecular mass of urea if the molecular mass of cane sugar is 342. |
12 |

858 | In the solvation of ( N a C l ) in water, which of the following occur? A. Hydrogen atom interacts with ( C l^{-} ) atom B. Oxygen atom interacts with ( N a^{+} ) atom c. Both ( A ) and ( B ) D. None of these |
12 |

859 | Ulustration 2.176 What will be the osmotic pressure of 0.1 M monobasic acid its pH is 2 at 25°C? |
12 |

860 | Illustration 2.193 The freezing point of an aqueous solution of KCN containing 0.1892 mol kg-1 was found to be -0.704°C. On adding 0.095 mol of Hg(CN), the freezing point of the solution was found to be -0.530°C. If the complex formation takes place according to the following equation: Hg(CN)2 + nKCN K,[Hg(CN)n+2] What is the formula of the complex? [K, (H2O) is 1.86 K kg mol-1 |
12 |

861 | The relationship between the value of Osmotic pressure ( (pi) ) of the solution obtained by dissolving ( 6 g . mathrm{L}^{-1} ) of acetic ( operatorname{acid}left(pi_{1}right) ) and 7.45 g.L ( ^{-1} ) of ( mathrm{KCl}left(pi_{2}right) ) is : A ( cdot pi_{1}pi_{2} ) ( mathbf{c} cdot pi_{1}=pi_{2} ) D. ( frac{pi_{1}}{pi_{1}+pi_{2}}=frac{pi_{2}}{pi_{1}+pi_{2}} ) |
12 |

862 | i. ( 0.1 M ) ethanol ii. ( mathbf{0 . 1} boldsymbol{M} boldsymbol{B} boldsymbol{a}_{3}left(boldsymbol{P} boldsymbol{O}_{4}right)_{3} ) ¡¡ii.0.1 ( M N a_{2} S O_{4} ) Increasing order of freezing point A ( cdot(i i)<(i i i)<(i) ) B. ( (i i i)<(i i)<(i) ) c. ( (i)<(i i)<(i i i) ) D. ( (i i)<(i)<(i i i) ) |
12 |

863 | The azeotropic mixture of water and ( H C l ) boils at ( 108.5^{0} C . ) This solution is: A . ideal B. non-ideal with positive deviation c. non-ideal with negative deviation D. cannot be predicated |
12 |

864 | ( 252 mathrm{gm} ) of oxalic acid with molecular formula ( C_{2} H_{2} O_{4} cdot 2 H_{2} O ) dissolve in water to form ( 250 mathrm{ml} ). of the solution. Its molarity will be: A . 16 м B. 8 M c. 32 м D. 24 M |
12 |

865 | The maximum amount of solute that will saturate ( 100 mathrm{g} ) of solvent at that temperature is known as: A. solubility B. soluble c. solution D. none of the above |
12 |

866 | A storage battery contains a solution of ( H_{2} S O_{4}, 38 % ) by mass. At this concentration, van’t Hoff factor is 2.50 The temperature at which battery contents freeze will be: ( left(boldsymbol{K}_{f}=mathbf{1 . 8 6} boldsymbol{K} boldsymbol{m o l}^{-1} boldsymbol{k g}right) ) A ( .-29.08^{circ} mathrm{C} ) B . ( -25.18^{circ} mathrm{C} ) c. ( -17.25^{circ} mathrm{C} ) D. none of these |
12 |

867 | If ( 200 mathrm{ml} ) solution of ( 0.5 mathrm{M} ) NaOH is diluted to ( 800 mathrm{ml} ) then find molarity of resultant solution. A. 0.250 М в. 0.125 м c. 0.225 м D. ( 0.4 mathrm{M} ) |
12 |

868 | A solution is prepared by dissolving ( 5.64 mathrm{g} ) of glucose in ( 60 mathrm{g} ) of water. Calculate the molality of the solution. A. ( 0.2611 mathrm{m} ) B. 1.21 ( mathrm{m} ) ( c cdot 1.044 mathrm{m} ) D. 0.522 ( mathrm{m} ) |
12 |

869 | Calculate the mole fraction of Benzene ( left(C_{6} H_{6}right) ) in a solution containing ( 30 % ) by ( operatorname{mass} operatorname{in} H C l .(C l=35.5) ) |
12 |

870 | toppr Q Type your question solution? ( A ) 3 ( c ) ( D ) |
12 |

871 | Benzoic acid (molecular weight ( =122 ) g mol ( ^{-1} ) ) associates to form dimer when dissolved in benzene and the osmotic pressure of a solution of 5 g of benzoic acid in ( 100 mathrm{ml} ) benzene is 5.73 atm at ( 10^{circ} mathrm{C} . ) What is the percentage association of benzoic acid? A . ( 8 % ) B. ( 80 % ) c. ( 40 % ) D. ( 20 % ) |
12 |

872 | Calculate the concentration of nitric acid in moles per litre in a sample which has a density, ( 1.41 g m L^{-1} ) and the mass per cent of nitric acid in it being ( 69 % ) |
12 |

873 | Negative deviation from Raoult’s law is observed in which one of the following binary liquid mixtures? A. Ethanol and acetone B. Benzene and toluene c. Acetone and chloroform D. Chloroethane and bromoethane |
12 |

874 | When a solution of ( C H C l_{3} ) and acetone is formed, the solution is non-ideal with deviation from Raoult’s law.The vapour pressure of such a solution will be corresponding ideal solution. A. Positive, more B. Negative, more c. Negative ,less D. Positive , less |
12 |

875 | Vapour pressure of water is ( 360 mathrm{mm} mathrm{Hg} ) how much urea should be added to 200 mL water to reduce its vapour pressure by ( 0.5 % ?(text { Molecular wt. of urea }=60) ) A . ( 2.52 g ) в. 3.33 g c. ( 3.96 g ) D. None of these |
12 |

876 | Determine the degree of association (polymerisation) for the reaction in aqueous solution ( 6 H C H O rightleftharpoons ) ( boldsymbol{C}_{boldsymbol{6}} boldsymbol{H}_{mathbf{1 2}} boldsymbol{O}_{boldsymbol{6}} ) If observed(mean) molar mass of ( H C H O ) and ( C_{6} H_{12} O_{6} ) is 150 A . 0.50 B. 0.833 c. 0.90 D. 0.96 |
12 |

877 | ( 10 mathrm{L} ) of hard water required ( 0.56 mathrm{g} ) of lime (CaO) for removing hardness. Hence, the temporary hardness in ppm (part per million) of ( C a C O_{3} ) is : A. 100 в. 200 c. 10 D. 20 |
12 |

878 | Molarity of a liquid ( H_{2} S O_{4} ) with density ( 1.2 g / c c ) is A . 36. B. 12.24 c. 1.224 D. 5.0 |
12 |

879 | What should be the density of an aqueous solution of urea ( (text {molarmass}=mathbf{6 0} boldsymbol{g} / text { mol}) ) such that the molarity and molarity of the solution become equal? A. ( 16.0 g / m l ) в. ( 1.6 g / m l ) c. ( 1.06 g / m l ) D. ( 1.16 g / m l ) |
12 |

880 | Solutions distilled without change in composition at a temperature are called A. Amorphous B. Azeotropic mixture c. Ideal solution D. Super saturated solution |
12 |

881 | What is the composition of last droplet of liquid remaining in equilibrium with vapour? A ( . x_{A}=0.6 ; x_{B}=0.4 ) B . ( x_{A}=0.5 ; x_{B}=0.5 ) c. ( x_{A}=0.7 ; x_{B}=0.3 ) D. ( x_{A}=0.3 ; x_{B}=0.7 ) |
12 |

882 | An aqueous solution of methanol in water has vapour pressure: A. less than that of water B. equal to that of water c. more than that of water D. equal to that of methano |
12 |

883 | The mole fraction of ( A ) in ( 10 %(w / w) ) aq. solution of glucose is: A . 0.18 B. 0.011 ( c .0 . ) D. 0.017 |
12 |

884 | Ethylene glycol is used as an antifreeze in a cold climate. Mass of ethylene glycol which should be added to 4 kg of water to prevent it from freezing at ( -6^{o} C ) will be : ( left(K_{f} text { for water }=1.86 mathrm{K} mathrm{kg} / mathrm{mol} ) and molar right. mass of ethylene glycol ( =62 ) g mol ( ^{-1} ) ) A . ( 304.6 mathrm{g} ) в. ( 800 mathrm{g} ) c. 204.3 g D. ( 400.00 mathrm{g} ) |
12 |

885 | The boiling point ( T_{b}^{*} ) of a solvent becomes ( T_{b} ) on addition of ( X_{1} ) mole fraction of solute. Heat of vaporisation of solvent is ( Delta boldsymbol{H}_{boldsymbol{v} boldsymbol{a} boldsymbol{p}} . ) The relation between elevation in b.pt. ( Delta T_{b}left(=T_{b}-right. ) ( left.T_{B}^{*}right) ) can be given by: ( frac{Delta T_{b}}{T_{b} times T_{b}^{*}}=-frac{R I n X_{1}}{Delta H_{v a p}} ) A graph plotted between ( log _{10} X_{1} ) vs. ( frac{1}{T_{b}} ) gives: A. [ text { straight line with slope } frac{R}{Delta H_{v a p}} text { and intercept } T_{b}^{*} ] B. a straight line with slope ( frac{2.303 R}{Delta H_{v a p}} ) and intercept ( frac{1}{T_{b}} ) c. a straight line with slope ( frac{Delta H_{v a p}}{2.303 R} ) and intercept ( frac{1}{T_{b}^{*} times 2.303} ) D. a straight line with slope ( frac{Delta H_{v a p}}{2.303 R} ) and intercept ( -frac{Delta H_{v a p}}{2.303 R T_{b}^{*}} ) |
12 |

886 | For a gas in equilibrium with a liquid, the ratio of the concentration of the gas in the solution phase to that in the gaseous phase is constant at constant temperature, only if molecules undergo: A. ionisation B. dissociation c. isolation D. reaction with solvent |
12 |

887 | A 1.00 molal aqueous solution of trichloroacetic acid ( left(C C l_{3} C O O Hright) ) is heated to its boiling point. The solution has the boiling point of ( 100.8^{circ} mathrm{C} ). Determine the van ‘t Hoff factor for trichloroacetic acid. ( left(K_{b} text { for water } 0.512 mathrm{K}right. ) ( left.operatorname{kg} M o l^{-1}right) ) Define the following terms: (i) Mole fraction (ii) Isotonic solutions (iii) Van ‘t Hoff factor (iv) Ideal solution |
12 |

888 | The difference in height of the mercury column in two arms of a U tube manometer in arrangement-lis ( boldsymbol{h}_{mathbf{1}}= ) ( 660 mathrm{mm} . ) In another arrangement -II at the same temperature, 222 gm of ( mathrm{CaCl}_{2} ) is dissolved in ( 324 mathrm{gm} ) of water and the difference in height of mercury column in two arms is found to be ( h_{2}= ) ( 680 mathrm{mm} . ) If the value of degree of dissociation for ( C a C l_{2} ) in arrangement -II is ( alpha, ) then the value of ( 64 alpha ) is: [Atmospheric pressure ( =1 text { atm }] ) ( : mathbb{1} ) |
12 |

889 | Mole fraction of ethanol ( left(C_{2} H_{5} O Hright) ) in ethanol-water system is ( 0.25 . ) Thus, it has: This question has multiple correct options A. ( 25 % ) ethanol by weight of solution B. ( 75 % ) water by weight of solution c. ( 46 % ) ethanol by weight of solution D. 54% water by weight of solution |
12 |

890 | Which of the following plots represents an ideal binary mixture? ( mathbf{A} cdot ) Plot of ( P_{text {total}} v / s 1 / X ) is linear ( left(X_{B}= ) mole fraction of right. ‘B’ in liquid phase). B. Plot of ( P_{text {total}} v / s Y_{A} ) is linear ( left(Y_{B}= ) mole fraction of ‘A’ right. in vapour phase) C ef of ( frac{1}{P_{text {total}}} v / s Y_{A} ) is linear D. plot of ( frac{1}{P_{text {total}}} v / s Y_{B} ) is non linear |
12 |

891 | Statement – I: The mixing of two completely miscible liquid. A and B showing positive deviation from Raoult’s law is followed by an absorption of heat Statement – ll: The A- B molecular interaction forces are stronger than the A-A or B-B molecular interaction forces. A. Statement-lis true, Statement- – 2 is true; Statement 2 is a correct explanation for Statement- – B. Statement-1 is true, Statement – 2 is true; Statement 2 is not a correct explanation for Statement – – c. statement-lis true, Statement- – 2 is false D. Statement-lis false, Statement- – 2 is true |
12 |

892 | room temperature solution feels cool to Q. 2 On dissolving sugar in water at room temperature solutio touch. Under which of the following cases dissolution of sugar most rapid? (a) Sugar crystals in cold water (b) Sugar crystals in hot water (c) Powdered sugar in cold water (d) Powdered sugar in hot water Thinking Process Use the concept of solubility and effect of temperature on solubility to answer this question diocoladin |
12 |

893 | Two liquids ( H N O_{3}(A) ) and water ( (B) ) form a maximum boiling azeotrope when mixed in the ratio of ( 68 % ) and ( 32 % ) respectively. It means: A. A-B interactions are stronger than ( A ) -A and B-B interactions B. A-B interactions are weaker than A-A and B-B interactions c. vapour pressure of solution is more than the pure components D. vapour pressure of solution is less since only one component vaporises |
12 |

894 | r at Question 39. The air is a mixture of a number of gase air is a mixture of a number of gases. The major components are oxygen and nitrogen with a are oxygen and nitrogen with approximate proportion of 20% is to 79% by volume at 298 K. The water is in equilibrium a pressure of 10 atm. At 298 K if the Henry’s law constants for oxygen and nitrogen at 298 K are 3.30 x107 mm and 6.51 x10 mm respecuve, calculate the composition of these gases in water. First find the partial pressure of oxygen and nitrogen from Henry’s law, p= K X and the find their mole fraction (again applying the Henry’s law). |
12 |

895 | Hlustration 2.212 Under what conditions Van’t Hoff factor (i) is (a) equal to unity, (b) less than 1, and (c) greater than 1. Explain your answer. |
12 |

896 | In amalgam of mercury with sodium, solvent is; A. mercury B. sodium c. amalgam D. none of these |
12 |

897 | A solution of ( 50 % ) of ( A ) and ( 50 % ) of ( B ) on distillation results into A. Seperation of an azeotropic mixture and pure ( A ) B. Seperation of an azeotropic mixture and pure B. C. Seperation of both pure ( A ) and pure ( B ) D. None. |
12 |

898 | A solution is prepared by dissolving 9.8 ( g ) of ( H_{2} S O_{4} ) in 54 g of water. What is the mole fraction of ( boldsymbol{H}_{2} boldsymbol{S O}_{4} ? ) A. 0.03 B. 0.04 c. 0.01 D. 0.02 |
12 |

899 | The Van’t Hoff factor of ( N a C l ) assuming ( 100 % ) dissociation is : A . ( 1 / 2 ) B . 2 c. 1 D. 3 |
12 |

900 | If equal volume of ( B a C l_{2} ) and ( N a F ) solutions are mixed, which of these combination will give a precipitate? ( boldsymbol{K}_{s p} ) of ( boldsymbol{B a} boldsymbol{F}_{2}=mathbf{1 . 7} times mathbf{1 0}^{-mathbf{7}} ) |
12 |

901 | Calculate Vant Hoff factor for ( 0.2 m ) aqueous solution of KCl which freezes at ( -mathbf{0 . 6 8 0}^{circ} mathbf{C} .left(boldsymbol{K}_{boldsymbol{f}}=mathbf{1 . 8 6} mathbf{K} mathbf{k g} boldsymbol{m o l}^{-mathbf{1}} mathbf{)}right. ) A . 3.72 в. 1.83 ( c .6 .8 ) D. 1.86 |
12 |

902 | What is the relative lowering in vapour pressure of ( 10 % ) aqueous solution of glucose : A ( .1 / 10 ) B. 1/90 c. ( 1 / 20 ) D. 1/30 |
12 |

903 | VLASOV UUTUUUUUUUUUU Illustration 2.60 . . . What type of liquids form ideal solutions? 1 colonitione |
12 |

904 | Fizziness appears on opening a bottle of cold drink. |
12 |

905 | A mixture has 18 g water and 414 g ethanol. The mole fraction of water in mixture is (assume ideal behaviour of the mixture): A . ( 0 . ) B. 0.4 ( c . ) о. D. 0.9 |
12 |

906 | A solution containing 0.1 mole of naphthalene and 0.9 mole of benzene is cooled out until some benzene freezes out. The solution is then decanted off from the solid and warmed up to ( 353 mathrm{K} ) where its vapour pressure was found to be 670 torr. The freezing point and boiling point of benzene are ( 278.5 mathrm{K} ) and ( 353 mathrm{K} ) respectively and its enthalpy of fusion is ( 10.67 mathrm{kJ} ) mol ( ^{-1} ). Calculate the depression in freezing point for original solution to the nearest integer. Assume ideal behaviour |
12 |

907 | ( 0.6 mathrm{g} ) of an organic compound when dissolved in 21.7 g water freezes at 272.187 K. The molar mass of the organic compound is close to: ( left(K_{f} text { of water is } 1.86 ) deg/molality; right. freezing point is ( 273 mathrm{K} ) ) A. ( 61 mathrm{g} ) mol ( ^{-1} ) B. ( 63 mathrm{g} ) mol ( ^{-1} ) ( mathbf{c} cdot 65 mathrm{g} m o l^{-1} ) D. ( 67 mathrm{g} ) mol ( ^{-1} ) |
12 |

908 | The solubility of gases in liquids is not affected by the pressure because the vapor pressure of a substance is not a function of external pressure. A . True B. False |
12 |

909 | Illustration 2.82 Distinguish between the boiling point of a liquid and the normal boiling point of a liquid. |
12 |

910 | An aqueous solution of methanol in water has vapour pressure: A. equal to that of water B. equal to that of methanol c. more than that of water D. less than that of water |
12 |

911 | Explain with suitable diagram and appropriate examples why some nonideal solution show positive deviation from ideal behavior: | 12 |

912 | A solution containing ( 4 g ) of a non- volatile organic solute per ( 100 m L ) was found to have an osmotic pressure equal to ( 500 mathrm{cm} ) of mercury at ( 27^{circ} mathrm{C} ) The molecular weight of solute is: A .14 .97 B. 149.7 ( c .1697 ) D. 1.497 |
12 |

913 | When a non volatile solute is added to a pure solvent, the: A. vapour pressure of the solution becomes lower then that of the pure solvent B. rate of evaporation of the pure solvent is reduced C. solute does not effect the rate of condensation D. rate of the evaporation of the solution is equal to the rate of condensation of the solution at a lower vapour pressure than that in the case of the pure solvent |
12 |

914 | When ( 1.04 g ) of ( B a C l_{2} ) is present in ( 10^{5} g ) of solution, the concentration of solution is: A. 0.104 ppm в. 10.4 ррт c. 0.0104 ppm D. 104 ppm |
12 |

915 | A ( 0.0020 M ) aqueous solution of an ionic compound ( boldsymbol{C} boldsymbol{o}left(boldsymbol{N} boldsymbol{H}_{3}right)_{5}left(boldsymbol{N} boldsymbol{O}_{2}right) boldsymbol{C l} ) freezes at ( -0.00732^{circ} mathrm{C} . ) Number of moles of ions which 1 mole of ionic compound produces on being dissolved in water will be: ( left[k_{f}=1.86^{circ} C / mright] ) A . 1 B. 2 ( c .3 ) D. 4 |
12 |

916 | A ( 5 % ) solution of glucose is isotonic with ( 1.1 % ) solution of ( mathrm{KCl} ) at ( 30^{circ} mathrm{C} ) Calculate the degree of ionisation of KCI. A . ( 90 % ) в. ( 88 % ) c. ( 78 % ) D. ( 80 % ) |
12 |

917 | 1. An aqueous solution freezes at -2.55°C. What is its boiling point (K 4,0 = 0.52 K m-!; KH20 = 1.86 Km-!)? a. 107.0°C b. 100.6°C c.100.1°C d. 100.7°C |
12 |

918 | Illustration 2.139 A 10 m solution of urea is cooled to -13.02°C. What amount of urea will separate out if the mass of solution taken is 100 g? [K, (water) = 1.86 K kg mol-‘) S |
12 |

919 | Henry law constant for the solubility of methane in benzene at ( 298 mathrm{K} ) is ( 4.27 times ) ( 10^{5} mathrm{mm} ) Hg then the solubility of methane in benzene at ( 298 mathrm{K} ) under 760mm Hg is: A ( cdot 7.8 times 10^{-2} ) mole ( / mathrm{kg} ) B . ( 7.8 times 10^{-3} ) mole / kg c. ( 7.8 times 10^{-4} ) mole ( / mathrm{kg} ) D. ( 1.78 times 10^{-3} ) mole ( / mathrm{kg} ) |
12 |

920 | yuuuu 10 OUVOU Q. 44 How does sprinkling of salt help in clearing the snow co hilly areas? Explain the phenomenon involved in the process Anchon polt from the surface lp in clearing the snow covered roads in |
12 |

921 | What is the concentration of a solution of 2,000 grams of water in which 684 grams of sucrose, ( C_{12} H_{22} O_{11} ) is dissolved? A. 25 molar B. 0.5 molal c. 1 molal D. 5 molar E. 1 molar |
12 |

922 | The vapour pressure of pure liquid is 70 Torr at ( 27^{circ} mathrm{C} ). The vapour pressure of a solution of this liquid and another liquid (mole fraction 0.2) is 84 Torr at ( 27^{circ} mathrm{C} . ) The vapour pressure of pure liquid ( B ) at ( 27^{circ} C ) is? A. 140 Torr B. 280 Torr c. 160 Torr D. 200 Torr |
12 |

923 | Which of the following liquid pairs shows a positive deviation from Raoult’s law? A. Water – hydrochloric acid B. Benzene – methanol c. water – nitric acid D. Acetone – chloroform |
12 |

924 | The density of 3 M solution of NaCl is 1.2 ( mathrm{g} m L^{-1} . ) The molality of the solution is? A. 2.79 ( mathrm{m} ) B. 1.79 ( m ) c. ( 3.5 mathrm{m} ) D. 5.58 m |
12 |

925 | 0.53 Assertion (A) When NaCl is added to water a depression in freezing point is observed. Reason (R) The lowering of vapour pressure of a solution causes depression in the freezing point. |
12 |

926 | To determine whether a water solution of ( N a_{2} S_{2} O_{3} ) at room temperature is supersaturated, one can : A. heat the solution to its boiling point B. add water to the solution c. add a crystal of ( N a_{2} S_{2} O_{3} ) to the solution D. acidify the solution E. cool the solution to its freezing point |
12 |

927 | Teleases WIL HUILast Ulumpur Assertion : During extreme winter season the roads get blocked in Jammu and Kashmir due to snowfall and to remove ice on roads some salt water is sprinkled on ice. Reason: The addition of any soluble impurity results in decrease in melting point. |
12 |

928 | Write the formula to calculate the mole fraction? |
12 |

929 | The vapour pressure of a certain liquid is given by the equation: ( log _{10} P=3.54595-frac{313.7}{T}+ ) ( mathbf{1} . mathbf{4 0 6 5 5} log _{mathbf{1 0}} boldsymbol{T} ) where ( P ) is the vapour pressure in ( mathrm{mm} ) and ( T=K ) elvin temperature. Determine the molar latent heat of vaporisation at ( boldsymbol{T}=mathbf{8 0} boldsymbol{K} ) |
12 |

930 | If an excess of ( A g N O_{3} ) solution is added to ( 100 mathrm{ml} ) of ( 0.024 mathrm{M} ) solution of dichlorobis (ethylene diamine) cobalt (III) chloride, how many moles of ( A g C l ) will be precipitated? A . 0.0012 B. 0.0016 c. 0.0024 D. 0.0048 |
12 |

931 | An azeotropic mixture of two liquids boils at a lower temperature than either of them when : A . it is saturated B. it does not deviate from Raoult’s law c. it shows negative deviation from Raoult’s law D. it shows positive deviation from Raoult’s law |
12 |

932 | Which substance does NOT dissolve well in water? A ( cdot N H_{3} ) B. ( C_{4} H_{10} ) c. ( C_{12} H_{22} O_{11} ) D. ( H_{2} S O_{4} ) |
12 |

933 | The vapour pressure of a pure liquid ( boldsymbol{A} ) is 70 torr at ( 27^{circ} mathrm{C} ). It forms an ideal solution with another liquid ( B ). The mole fraction of ( B ) is 0.2 and total vapour pressure of the solution is 84 torr at ( 27^{circ} mathrm{C} . ) The vapour pressure of pure liquid ( B ) at ( 27^{circ} mathrm{C} ) is: A . 14 B. 56 ( c .140 ) D. 70 |
12 |

934 | If the elevation in boiling point of a solution of non-volatile, non-electrolytic and non-associating solute in a solvent ( left(K_{b}=x K k g m o l^{-1}right) ) is ( y K, ) then the depression in freezing point of solution of same concentration would be: ( left[boldsymbol{K}_{f} text { of the solvent }=boldsymbol{z} boldsymbol{K} boldsymbol{k} boldsymbol{g} boldsymbol{m o l}^{-1}right] ) A ( cdot frac{2 x z}{y} ) в. ( frac{y z}{x} ) c. ( frac{x z}{y} ) D. ( frac{y z}{2 x} ) E ( cdot frac{x z}{2 y} ) |
12 |

935 | Equal volumes of ( 1 mathrm{M} K_{2} S O_{4} ) and ( 1 mathrm{M} ) ( A l_{2}left(S O_{4}right)_{3} ) solutions are mixed. Which of the following is incorrect? A. The concentration of ( K^{+} ) is 1 M B. The concentration of ( A l^{3+} ) is 1M C. The concentration of ( S O_{4}^{2-} ) is 2 M D. The concentration of all the three ions is 1 M |
12 |

936 | Illustration 2.97 On dissolving 3.24 g of sulphur in 40 g of benzene, the boiling point of the solution was higher than that of benzene by 0.81 K. What is the molecular formula of sulphur? (K, for benzene = 2.53 K kg mol-, atomic mass of sulphur = 32 g mol-?). |
12 |

937 | Which of the following condition is not followed for an ideal solution? A ( cdot Delta H_{text {mixing}}=0 ) B. ( Delta S_{text {mixing}}=0 ) C. ( Delta v_{text {mixing}}=0 ) D. All A, B, and C are followed |
12 |

938 | Addition of ethylene glycol (non-volatile) to water lowers the freezing point of water and hence it is used as antifreeze. Addition of any substance to water lowers its freezings point of water. A. Statement-1 is true, statement-2 is true and statement-2 is correct explanation for statement- B. Statement-1 is true, statement-2 is true and statement-2 is NOT the correct explanation for statement-1 C. Statement-1 is true, statement-2 is false D. Statement-1 is false, statement-2 is true |
12 |

939 | Question 5. A solution of glucose in water is labelled as 10% w/w. What should be the molality and mole fraction of each component in the solution? If the density of solution is 12 g mL, then what shall be the molarity of the solution? 0 As percentage by weight is given find weight of solute (Wa) and solvent (WA) from it and calculate molar mass of solute (glucose), MB by adding atomic masses of different elements, (ii) Calculate molality by using, m = WA (iii) In order to calculate mole fraction, calculate the number of moles of solute and solvent. (iii) Calculate the volume by the formula of density and then molarity by using moles of solute and volume of solution. |
12 |

940 | ( 20 mathrm{ml} ) of ( 1 mathrm{M} mathrm{BaCl}_{2} ) solution and ( 25 mathrm{m} ) of ( 0.1 mathrm{M} mathrm{Na}_{2} mathrm{SO}_{4} ) are mixed to form ( B a S O_{4} . ) The amount of ( B a S O_{4} ) precipitated are: A . 2.5 g B. 2.5 moles c. 2.5 millimoles D. 0.05 millimoles |
12 |

941 | A ( 5 % ) solution (w/W) of cane sugar (molar mass ( =342 g ) mol ( ^{-1} ) ) has freezing point ( 271 K . ) What will be the freezing point of ( 5 % ) glucose (molar mass ( =18 g ) mol ( ^{-1} ) ) in water if freezing point of pure water is ( 273.15 K ? ) ( mathbf{A} cdot 273.07 K ) в. ( 269.07 K ) c. ( 273.15 K ) D. ( 260.09 K ) |
12 |

942 | Clothes do not protect us from A. heat B. cold c. blood pressure D. dust and germs |
12 |

943 | Q. 42 (a) Explain the following phenomena with the help of Henry’s law. (i) Painful condition known as bends. (ii) Feeling of weakness and discomfort in breathing at high altitude. (b) Why soda water bottle kept at room temperature fizzes on opening? |
12 |

944 | Illustration 2.34 The vapour pressure of acetone at 298 K is 40 mm of Hg. Its mole fraction in a solution with alcohol is 0.80. What is its vapour pressure in solution if the mixture obey Raoult’s law? |
12 |

945 | An example of solid in non-aqueous solvent is : A. sugar in Ethanol B. blood c. starch D. sugar sol |
12 |

946 | Solutions ( A, B, C ) and ( D ) are respectively ( 0.1 M ) glucose, ( mathbf{0 . 0 5} M N a C l, 0.05 M B a C l_{2} ) and ( 0.1 M A l C l_{3} . ) Which one of the following pairs is isotonic? A. ( A ) and ( B ) B. ( B ) and ( C ) c. ( A ) and ( D ) D. ( A ) and ( C ) |
12 |

947 | On mixing equal volumes of acetone and ethanol, what type of deviation from Raoult’s law is expected? | 12 |

948 | The binary mixture of a particular composition in both liquid and vapour state is known as a/an azeotropic mixture. If true enter 1 , if false enter 0 . |
12 |

949 | Ratio of solubilities of ( operatorname{gases} N_{2} & O_{2} ) in water from air at ( 25^{circ} & 1 ) atm will be if air is ( 20 % ) by volume of ( O_{2} ) and ( 80 % ) by volume of ( boldsymbol{N}_{2} ) [ begin{aligned} operatorname{Given} &: boldsymbol{K}_{boldsymbol{H}}left(boldsymbol{N}_{2}right)=boldsymbol{2} times mathbf{1 0}^{4} boldsymbol{a t m} \ boldsymbol{K}_{boldsymbol{H}}left(boldsymbol{O}_{2}right) &=mathbf{1 0}^{4} boldsymbol{a t m} end{aligned} ] A . 8: 1 B. 1: 8 ( c cdot 1: 2 ) D. 2: 1 |
12 |

950 | To determine the solubility of a solute in water, a solution must be prepared that is A. saturated B. unsaturated c. concentrated D. supersaturated |
12 |

951 | The van’t Hoff factor for a very dilute aqueous solution of ( boldsymbol{K}left[boldsymbol{A} boldsymbol{g}(boldsymbol{C} boldsymbol{N})_{2}right] ) is: A . 4 B. 3 c. 2 D. 5 |
12 |

952 | Calculate the freezing temperature of an aqueous solution having its boiling temperature ( 100.1^{circ} mathrm{C} ). The mola ebullioscopic constant and the molal cryoscopic constant are 0.513 deg and 1.86 deg, respectively. The answer is ( -0 . m n ) then ( m+n= ) |
12 |

953 | When ( 12.044 times 10^{23} ) molecule of ( H_{2} S O_{4} ) is dissolve in ( 195 mathrm{cm}^{3} ) solution. What is mass percent ( boldsymbol{H}_{2} boldsymbol{S} boldsymbol{O}_{4} ) in the solution. If the density of the solution is ( 1.25 g c m^{-3} ) |
12 |

954 | A solution of glucose ( left(C_{8} H_{12} O_{6}right) ) is isotonic with ( 5 g ) of urea ( left(N H_{2} C O N H_{2}right) ) per litre of solution The concentration of glucose is: A. ( 48 / L ) B. 8 g/L c. 12 g/L D. ( 15 mathrm{g} / mathrm{L} ) |
12 |

955 | ciuneadlie, Question 25. Among the following compounds, identify which are insoluble, partially soluble and highly soluble in water? (1) Phenol (ii) Toluene (ii) Formic acid (iv) Ethylene glycol (v) Chloroform (vi) Pentanol Consider different types of molecular forces. |
12 |

956 | An aqueous solution of a substance molar mass 240 has osmotic pressure ( 0.2 mathrm{atm} ) at ( 300 mathrm{K} ). The density of solution ( operatorname{in} g cdot d m^{3} ) is: ( (R= ) ( left.0.08 text { litre atm } K^{-1} m o l^{-1}right) ) |
12 |

957 | g mixture of glucose and urea present in ( 250 mathrm{mL} ) aqueous solution shows the osmotic pressure of 0.74 atm at ( 27^{circ} C ) Assuming solution to be diluted, which are correct? 1. Percentage of urea in the mixture is 17.6 2. Relative lowering of the vapour pressure of this solution is ( 5.41 times 10^{-4} ) 3. The solution will boil at ( 100.015^{circ} C ), if ( K_{b} ) of water is ( 0.5 mathrm{K} ) molality ( ^{-1} ) 4. If glucose is replaced by the same amount of sucrose, the solution will show higher osmotic pressure at ( 27^{circ} C ) 5. If glucose is replaced by the same amount of ( N a C l ), the solution will show lower osmotic pressure at ( 27^{circ} mathrm{C} ) A. 1,2,3 в. 1,2,3,5 c. 2,4,5 D. 1,4,5 |
12 |

958 | A substance is completely trimerized on dissolution in a solvent. The Van’t Hoff factor ( (i) ) for such change is: A . 1 B . 2 ( c .3 ) D. ( 1 / 3 ) |
12 |

959 | Molarity of ( 4 % ) (w/v) solution of ( N a O H ) is: A . ( 0 . ) B. 0.5 c. 0.001 D. 1.0 |
12 |

960 | 0.5 Maximum amount of a solid solute that can be dissolved in a specified amount of a given liquid solvent does not depend upon …….. (a) temperature (b) nature of solute (c) pressure (d) nature of solvent |
12 |

961 | Tlustration 2.115 By dissolving 13.6 g of a substance in 20g of water, the freezing point decreased by 3.7°C. Calculate the molecular mass of the substance. (Molal depression constant for water = 1.863 K kg mol-l) |
12 |

962 | ( 10^{-3} ) mol of ( C u S O_{4} cdot 5 H_{2} O ) is introduced in a ( 1.9 L ) vessel maintained at a constant temperature of ( 27^{circ} mathrm{C} ) containing moist air at relative humidity of ( 12.5 % . ) What is the final molar composition of solid mixture? For ( boldsymbol{C u} boldsymbol{S O}_{4} cdot boldsymbol{5} boldsymbol{H}_{2} boldsymbol{O}(boldsymbol{s}) rightleftharpoons boldsymbol{C u} boldsymbol{S} boldsymbol{O}_{4}(boldsymbol{s})+ ) ( mathbf{5} H_{2} O(boldsymbol{g}), boldsymbol{K}_{p}(boldsymbol{a} boldsymbol{t m})=mathbf{1 0}^{-10} . ) Take vapor pressure of water at ( 27^{circ} mathrm{C} ) as 28 torrs. |
12 |

963 | A solution is obtained by mixing ( 200 g ) of ( 30 % ) and ( 300 g ) of ( 20 % ) solution by weight What is the percentage of solute in the final solution? A . ( 50 % ) B . 28% c. ( 64 % ) D. 24% |
12 |

964 | The vapour pressure of a deliquescent substance is: A. equal to the atmospheric pressure B. equal to that of the water vapour in air C . greater than that of the water vapour in air D. less than that of the water vapour in air |
12 |

965 | ( 0.24 mathrm{g} ) of a volatile gas upon vaporization gives 45 mL vapour at ( mathrm{NTP} ) What will be the vapour density of the substances? (density of ( boldsymbol{H}_{2}=mathbf{1} ) ) (a) 95.39 (b) 5.973 (c) 95.93 (d) 59.73 |
12 |

966 | What is a vitreous state? | 12 |

967 | Example 2.22 At 17°C, the osmotic pressure of sugar solution is 580 torr. The solution is diluted and the temperature is raised to 57°C, when the osmotic pressure is found to be 165 torr. The extent of dilution is a. 2 times b. 3 times c. 4 times d. 5 times |
12 |

968 | Question 5. Calculate (a) molality (b) molarity and (c) mole fraction of KI if the density of 20% (mass/mass) aqueous KI is 1.202 g mL-. (0) As density and % by mass is given, so find the mass of solute and solvent (as x % solution contains xg solute in (100 – x)g solvent). (ii) Find volume of the solution, by using, Volume = Mass on Density (iii) Recall the formulae of molality, molarity and mole fraction, to calculate them. |
12 |

969 | A solution of 0.2 mole ( mathrm{Kl}(alpha=100 %) ) in 1000 g water freezes at ( T_{1}^{circ} ) C. Now to this solution 0.1 mole ( H g I_{2} ) is added and the resulting solution freezes at ( T_{2}^{circ} mathrm{C} . ) Which of the following is correct? A ( cdot T_{1}=T_{2} ) в. ( T_{1}>T_{2} ) c. ( T_{1}<T_{2} ) D. can't be prediced |
12 |

970 | so Components of a binary mixture of two liquids A and B were being separated by distillation. After some time separation of components stopped and composition of vapour phase became same as that o ur phase. Both the components started coming in the distillate. Explam why this happened? |
12 |

971 | Question 3. Explain the solubility rule ‘like dissolves like’ in terms of intermolecular forces that exist in solutions. |
12 |

972 | The expression relating mole fraction of solute ( left(chi_{2}right) ) and molarity ( (mathrm{M}) ) of the solution is (where dis the density of the solution in ( g L^{-1} ) and ( M w_{1} ) and ( M w_{2} ) are the molar masses of solvent and solute, respectively A ( cdot x_{2}=frac{M times M w_{1}}{Mleft(M w_{1}-M w_{2}right)+1000 d} ) B. ( x_{2}=frac{M times M w_{1}}{Mleft(M w_{1}-M w_{2}right)+d} ) c. ( _{x_{2}}=frac{M times M w_{1}}{Mleft(M w_{1}-M w_{2}right)-1000 d} ) D. ( _{x_{2}}=frac{M times M w_{1}}{Mleft(M w_{1}-M w_{2}right)-d} ) |
12 |

973 | Which of the following azeotropes is not correctly matched? ( mathbf{A} cdot H N O_{3}(68 %)+H_{2} O(32 backslash %): ) Maximum boiling azerotrope, boiling point ( =393.5 K ) B ( cdot H_{2} O(43 %)+H I(57 %): ) Minimum boiling azeotrope, boiling point ( =290 K ) C ( cdot C_{2} H_{5}(95.5 %)+H_{2} O(4.5 %): ) Minimum boiling azerotrope, boiling point ( =351.15 K ) D. Chloroform (93.2%) ( +C_{2} H_{5} O H ) (6.8%): Minimum boiling azeotrope, boiling point ( =332.3 K ) ) |
12 |

974 | Illustration 2.76 The relative lowering of the vapour pressure of an aqueous solution containing a non-volatile solute is 0.0125. The molality of the solution is a. 0.80 b. 0.50 c. 0.70 d. 0.40 |
12 |

975 | If mole fraction of urea in 11.11 mola aqueous solution? A . 0.1 B. 0.17 ( c .0 .2 ) D. 0.37 |
12 |

976 | Illustration 2.184. A solution of non-volatile solute in water freezes at -0.80°C. The vapour pressure of pure water at 298 K is 23.51 mm Hg and K, for water is 1.86 degree per molal. Calculate the vapour pressure of this solution at 298 K. |
12 |

977 | A solution containing 500 g of a protein per liter is isotonic with a solution containing 3.42 g of sucrose per liter. The molecular mass of protein is: ( A cdot 58 ) B. ( 146 mathrm{g} ) c. ( 34200 mathrm{g} ) D. 50000 ( g ) |
12 |

978 | If you dilute ( 25.0 mathrm{mL} ) of ( 1.5 mathrm{M} H C l ) to ( 500 mathrm{mL}, ) then the molar concentration of each ions becomes ( boldsymbol{Y} times mathbf{1 0}^{-mathbf{3}} boldsymbol{M} . ) Here ( boldsymbol{Y} ) is: |
12 |

979 | The substance ( A ), when dissolved in solvent ( mathrm{B} ), shows the molecular mass corresponding to ( A_{3} . ) The Vant Hoff’s factor will be: A . 1 B. 2 ( c cdot 3 ) D. ( 1 / 3 ) |
12 |

980 | A solution of 1.25 g of ( mathrm{P} ) in 50 g of water lowers freezing point by 0.3. Molar mass of ‘Pis 94. ( boldsymbol{K}_{f(text {water})}=mathbf{1 . 8 6} mathrm{K} mathrm{kg} mathrm{mol}^{-1} ) The degree of association of P in water is: A . ( 60 % ) B. 75% c. ( 80 % ) D. 65% |
12 |

981 | On mixing, heptane and octane form an ideal solution. At ( 373 mathrm{K} ), the vapour pressures of the two liquid components (heptane and octane) are 105 kPa and 45 kPa respectively. Vapour pressure of the solution obtained by mixing 25.0 gm of heptane and 35 gm of octane will be:(molar mass of heptane ( = ) ( 100 mathrm{gmo} 1^{-1} ) and of octane ( = ) ( left.114 operatorname{gmol}^{-1}right) ) ( mathbf{A} cdot 72.0 mathrm{kPa} ) B . ( 36.1 mathrm{kPa} ) c. ( 96.2 mathrm{kPa} ) D. ( 144.5 mathrm{kPa} ) |
12 |

982 | Illustration 2.121 Calculate the freezing point depression and boiling point elevation of a solution of 10.0 g of urea (MR = 60) in 50.0 g of water at 1 atm. pressure. K and K, for water 0.52°C m-1 and 1.86°C m-1 respectively. |
12 |

983 | A volume of 50 lof dry ( N_{2} ) is passed through ( 36 g ) of water at 300 K. After passage of gas, there is a loss of 1.20 g in water. The vapour pressure of water at ( 300 mathrm{K} ) is? в. ( 24.96 mathrm{mm} ) Н ( mathrm{g} ) c. ( 16.05 mathrm{mm} ) нв D. ( 38.73 mathrm{mm} ) Hg |
12 |

984 | When 1 mole of a substance is present in 1 L of the solution, it is known as: A. normal solution B. molar solution c. molal solution D. None of the above |
12 |

985 | What is the concentration of a cobalt (II) nitrate solution whose absorbance was measured at 0.55 in a ( 1.1 mathrm{cm} ) cuvette with a molar extinction coefficient of ( mathbf{1 . 5} / boldsymbol{M} mathbf{c m} ? ) в. ( 0.60 M ) c. ( 0.90 M ) D. ( 1.2 M ) |
12 |

986 | Hardness in water is expressed in terms of ppm of ( C a C O_{3} . ) If hardness is 200 ppm ( C a C O_{3}, ) then in terms of molarity, it is: A. ( 0.004 mathrm{M} ) B. ( 0.002 M ) c. ( 0.001 M ) D. ( 0.0005 M ) |
12 |

987 | What do you mean by the “concentration” of a substance? A. It is the measure of undissolved substances B. It refers to the impurities C. Concentration refers to the amount of substance per defined space D. It means total mass of the un dissolved gases |
12 |

988 | What is the equivalent mass ( I O_{4}^{-} ) when it is converted into ( I_{2} ) in acid medium? A. M/6 в. м/7 c. м/5 D. M/4 |
12 |

989 | An ideal gaseous mixture of ethane and ethene occupy ( 28 L ) as STP. The mixture required ( 128 g O_{2} ) combustion, mole fraction of ethene in the mixture is: A . 0.4 B. 0.5 c. 0.6 D. 0.8 |
12 |

990 | Define molarity. | 12 |

991 | If the formula weight of ( boldsymbol{H}_{2} boldsymbol{S} boldsymbol{O}_{4} ) is 98 then the amount of acid present in 400 ( mathrm{ml} ) of 0.1 molar solution of acid will be: A. ( 2.45 g ) B . ( 3.92 g ) c. ( 4.90 g ) D. ( 9.80 g ) |
12 |

992 | A mixture of ( N a_{2} C_{2} O_{4}(A) ) and ( K H_{2} C_{2} O_{4} cdot 2 H_{2} O(B) ) required equal volumes of ( 0.1 mathrm{M} K M n O_{4} ) and ( 0.1 mathrm{M} ) NaOH separately. Molar ratio of ( A ) and ( B ) in the mixture is : A . 1: 1 B. 1: 5.5 c. 5.5: 1 D. 3.1 : 1 |
12 |

993 | Find out the correct statement regarding a saturated solution of salt in water? A. All dissolving has stopped B. Crystals begin to grow C. An equilibrium has been established D. Crystals of the solute will visibly continue to dissolve E. The solute is exceeding its solubility |
12 |

994 | Illustration 2.31 Assuming ideal behaviour, calculate the pressure of 1.0 molal solution of a non-volatile molecular solute in water at 50°C. The vapour pressure of water at 50° C is 0.222 atm. |
12 |

995 | The mole fraction of ( N_{2} O ) In a mixture of ( N_{2} O ) and ( N O ) is ( frac{1}{3} . ) The mole fraction of ( N O ) in a mixture of ( N O ) and ( N O_{2} ) is 3. The two mixtures are mixed in 3: 4 ( overline{mathbf{4}} ) molar ratio. the mole fraction of ( N O_{2} ) in the resulting mixture is: |
12 |

996 | At ( 10^{0} C, ) the osmotic pressure of urea solution is ( 500 mathrm{mm} ). The solution is diluted and the temperature is raised to ( 25^{0} C, ) so that the osmotic pressure became ( 105.3 mathrm{mm} . ) The number of times, the solution diluted is: A . 6 B. 5 ( c cdot 4 ) D. 3 |
12 |

997 | The main reason for the extremely low solubility of carbon dioxide in benzene ( left(C_{6} H_{6}right) ) at room temperature is due to which of the following? A. The increased disorder due to mixing of the solute and solvent B. The relatively low strength of the intermolecular forces between carbon dioxide and benzene c. The strong hydrogen bonding in benzene D. The weak solvation of carbon and oxygen ions by benzene |
12 |

998 | Find the degree of association when 1.0 gram benzoic acid, dissolved in 25 gram benzene is having depression in freezing point ( 0.81 k . ) The mola depression constant for solvent is ( 4.9 K ) kg mole ( ^{-1} ) |
12 |

999 | Which of the following is a mixture? A. water B. Oxygen c. Carbon dioxide D. Air |
12 |

1000 | Molal elevation constant and molal depression constant of water respectively ( left(text { in } quad K m^{-1}right) ) are: A. 0.52,1.86 В. 1.86,0.52 c. 1.52,0.86 D. 0.86,1.52 |
12 |

1001 | The total pressure or a mixture of oxygen and hydrogen is 1.0 atm. The mixture is ignited and the water is removed. The remaining gas is pure hydrogen and exerts a pressure of 0.40 when measured at the same values of ( T ) and ( mathrm{V} ) as the original mixture. What was the composition of the original mixture in mole per cent? A ( cdot x_{O_{2}}=0.2 ; x_{H_{2}}=0.8 ) в. ( x_{0}_{0}=0.4 ; x_{H_{2}}=0.6 ) c. ( x_{o_{2}}=0.6 ; x_{H_{2}}=0.4 ) D. ( x_{O_{2}}=0.8 ; x_{H_{2}}=0.2 ) |
12 |

1002 | Volume (in litres) of ( 0.1 mathrm{M} boldsymbol{H}_{2} boldsymbol{S O}_{4} ) required to completely neutralize 1 litres of ( 0.5 mathrm{M} ) NaOH is: ( mathbf{A} cdot mathbf{5} ) в. 2. c. 0.5 D. 10 |
12 |

1003 | Example 2.7 In a study of aqueous solution of thorium nitrate, the freezing point depression of 0.0703 °C is observed for a 9.6 mmol kg of the solution. How many ions are present in one thorium nitrate unit? (K, for H,0 = 1.86 Km !) |
12 |

1004 | If molality of the dilute solution is doubled, the value of molal depression constant ( left(boldsymbol{K}_{boldsymbol{f}}right) ) will be : A. unchanged B. doubled c. halved D. tripled |
12 |

1005 | Illustration 2.110 If the boiling point of an aqueous solution containing a non-volatile solute is 100.15°C. What is its freezing point? Given latent heat of fusion and vapourization of water 80 cal g1 and 540 cal g, respectively. |
12 |

1006 | The above laboratory setup can be used to prepare: A. gas lighter than air and soluble in water B. gas heavier than air and soluble in water c. gas soluble in water that reacts with water D. gas insoluble in water E. gas that reacts with water |
12 |

1007 | Which characteristic the weak intermolecular forces of attraction in a liquid? A. High boiling point B. High vapour pressure c. High critical temperature D. High heat of vaporization |
12 |

1008 | A solution containing 5 g acetic acid in 100 g ( boldsymbol{H}_{2} boldsymbol{O}left(boldsymbol{O}_{boldsymbol{H}_{2}}^{0} boldsymbol{O}=mathbf{2} boldsymbol{3} . mathbf{7} mathbf{5} boldsymbol{6} boldsymbol{m} boldsymbol{m} text { at } mathbf{2} mathbf{5}^{boldsymbol{o}} boldsymbol{C}right. ) shows a vapour pressure of ( 23.40 mathrm{mm} ) whereas same mass of acetic acid in ( 100 mathrm{g} C_{6} H_{6}left(P_{C_{6} H_{6}}^{0}=72.5 m m text { at } 25^{circ} Cright) ) shows a vapour pressure of ( 70.0 mathrm{mm} ) Assuming non-volatile nature of ( C H_{3} C O O H, ) discuss the data given to discuss hydrogen bonding: A. acetic acid exists as a monomer B. acetic acid exists as a dimer c. acetic acid is dissociated D. acetic acid exists as an anhydride |
12 |

1009 | Tlustration 2.171 A solution was prepared by dissolving 6.0 g an organic compound in 100 g of water. Calculate the osmotic pressure of this solution at 298 K, when the boiling point of the Solution is 100.2°C. (K, for water = 0.52 K m-, R = 0.082 L atm K-1 mol1) |
12 |

1010 | An unknown composition of a mixture of carbon disulphide and hydrogen sulphide was burnt in sufficient amount of oxygen. The resulting gases found to exert a pressure of 1.97 atm in a 20 I vessel at 400 K. The gaseous mixture required 2.8 M iodine solution and ( 250 mathrm{ml} ) of it was required to reach the end point, forming ( boldsymbol{I}^{-} ). Calculate the mole fraction of ( boldsymbol{C} boldsymbol{S}_{2} ) in the original mixture. A. 0.2 B. 0.4 c. 0.6 D. 0.8 |
12 |

1011 | Van’t Hoff’s factor of aq. ( K_{2} S O_{4} ) at infinite dilution has value equal to: ( mathbf{A} cdot mathbf{1} ) B. 2 ( c .3 ) D. Between 2 and 3 |
12 |

1012 | Q.59 When kept in water, raisin swells in size. Name phenomenon involved with the help of a diagrami. applications of the phenomenon. un incide the raisin and swells in size. Name and explain the the help of a diagram. Give three |
12 |

1013 | The osmotic pressure of a solution containing 40 g of solute (molecular mass 246 ) per litre at ( 27^{circ} C ) is: ( left[boldsymbol{R}=mathbf{0 . 0 8 2 2} boldsymbol{operatorname { a t m }} boldsymbol{L} boldsymbol{m o l}^{-mathbf{1}}right] ) A. 3.0 atm B. 4.0 atm c. 2.0 atm D. 1.0 atm |
12 |

1014 | Which has the highest boiling point? A. ( 0.1 mathrm{M} mathrm{Na}_{2} mathrm{SO}_{4} ) В. ( 0.1 M C_{6} H_{12} O_{6} ) c. ( 0.1 mathrm{M} ) М ( g ) Са( _{2} ) D. ( 0.1 mathrm{M} ) Аl ( left(mathrm{NO}_{3}right)_{3} ) |
12 |

1015 | The solution with the highest boiling point temperature is: в. ( 0.1 mathrm{M} ) НС ( mathrm{CO}_{4} ) c. ( 0.1 mathrm{M} mathrm{NH}_{4} mathrm{OH} ) D. 0.1 М КОН E. ( 0.1 mathrm{M} ) LiNO ( _{3} ) |
12 |

1016 | The vapour pressure in ( mathrm{mm} ) of ( boldsymbol{H} boldsymbol{g} ), of an aqueous solution obtained by adding 18 g of glucose ( left(C_{6} H_{12} O_{6}right) ) to 180 gof water at ( left(100^{circ} mathrm{C}right) ) is: A . 7.60 B. 76.0 c. 759 D. 752.4 |
12 |

1017 | 0.39 Concentration terms such as mass percentage, ppm, mole fraction and molality are independent of temperature, however molarity is a function of temperature. Explain. Thinking Process To solve this problem notice the role of temperature in component of concentration term such as volume, mass, number of moles etc. H ali |
12 |

1018 | For an ideal solution with ( boldsymbol{p}_{boldsymbol{A}}^{boldsymbol{o}}>boldsymbol{p}_{boldsymbol{B}}^{boldsymbol{o}} ) which of the following is true? A ( cdotleft(x_{A}right)_{text {liquid}}=left(x_{A}right)_{text {vapour}} ) В . ( left(x_{A}right)_{text {liquid }}>left(x_{A}right)_{text {vapour }} ) C ( cdotleft(x_{A}right)_{text {liquid}}<left(x_{A}right)_{text {vapour}} ) D cdot ( left(x_{A}right)_{text {liquid }} ) and ( left(x_{A}right)_{text {vapour }} ) cannot be correlated with each other |
12 |

1019 | Which substance would dissolve fastest in water? A ( .1 g ) granulated sugar B. ( 1 ~ g ) powdered sugar C. ( 1 ~ g ) sugar cube D. ( 1 g ) piece of crystallized sugar |
12 |

1020 | PADoco 32 elone 37. Vapour pressures of pure acetone and chloroform at are 141.8 mm Hg and 632.8 mm Hg respectively. Assuming that they form ideal solution over the entire range of composition, P. total Pchloroform and Pacetone as function of Xane. The experimental data observed for different compositions of mixture is : 0 11.8 23.4 36.0 50.8 58.2 645 721 Pacetone/ mm Hg 0 54.9 110.1 202.4 322.7 405.9 4541 521.1 Pchloroform/mm Hg 632.8 548.1 469.4 359,7 257.7 193.6 161.2 120.7 Plot this data also on the same graph paper. Indicate whether it has positive deviation or negative deviation from the ideal solution. 100 x acetone Find Ptotal and x acetone and then plot the graph. |
12 |

1021 | If we take ( 44 mathrm{g} ) of ( C O_{2} ) and ( 14 mathrm{g} ) of ( N_{2} ) what will be the mole fraction of ( C O_{2} ) in the mixture? A . ( 1 / 5 ) в. ( 1 / 3 ) c. ( 2 / 3 ) D. ( 1 / 4 ) |
12 |

1022 | Concentration terms like mass percentage, ppm, mole fraction and molality do not depend on temperature. However, molarity is a function of temperature because: A. volume depends on temperature and molarity involves volume B. molarity involves non-volatile solute while all other terms involve volatile solute C. number of moles of solute change with change in temperature D. molarity is used for polar solvents only |
12 |

1023 | A solution of sugar in which some more sugar could be dissolved without changing its temperature is called a/an A. unsaturated solution B. saturated solution c. solid solution D. true solution |
12 |

1024 | The solubility of the gas in a liquid solution with an increase in temperature. A . decreases B. increases c. remains same D. none of these |
12 |

1025 | The density of ( 85 % ) Phosphoric acid is ( 1.70 g c m^{-3} . ) What is the volume of a solution that contains ( 17 g m ) Phosphoric acid? |
12 |

1026 | How many kg (nearest integer value) of wet ( N a O H ) containing ( 12 % ) water is required to prepare 60 L of ( 0.50 M ) Na ( O H ) solution? If the answer is ( x ) then the nearest integral value of ( 1000 x ) |
12 |

1027 | Number of moles of ( S_{2} O_{3}^{2-} ) present in the sample is: A . 0.0005 B. 0.01 c. 0.0025 D. 0.02 |
12 |

1028 | Which among the following has lowest vapour pressure? A ( .0 .5 M A l_{2}left(S O_{4}right)_{3} ) B. ( 12 % ) Urea solution c. ( 1 M ) NaCl ( (a q) ) D. ( 18 % ) Glucose solution |
12 |

1029 | The molarity of a NaOH solution by dissolving ( 4 g ) of it on ( 250 m L ) water is: A ( .0 .4 M ) B. ( 0.8 M ) c. ( 0.2 M ) D. ( 0.1 M ) |
12 |

1030 | 9. The vapour pressure of pure liquid solvent A is 0.80 atm. When a non-volatile substance B is added to the solvent, its vapour pressure drops to 0.60 atm; the mole fraction of component B in the solution is b. 0.25 c. 2.0 d. 3.0 a. 0 |
12 |

1031 | The vapour pressure of three liquids ( P, Q ) and ( R, ) of nearly equal molecular masses is shown as a function of temperature The correct statement is: A. The normal boiling points follow the order ( P>Q>R ) B. The variation of pressure with respect to temperature for each liquid is given by ( frac{d P}{d T}=frac{K}{T^{2}}, ) where ( K ) is a constant c. The strength of intermolecular interactions follows the order ( P>Q>R ) D. The normal boiling point of ( Q ) is close to ( 65^{circ} mathrm{C} ) |
12 |

1032 | Answer the following questions: 1. Derive the mathematical expression between molar mass of a non-volatile solute and elevation of boiling point 2. State and explain van’t Hoff- Avogadro’s law. |
12 |

1033 | What is the total pressure of the dry gas collected if the vapor pressure due to water at ( 25^{circ} C ) is 24 mm Hg( ? ) A. ( 24 mathrm{mm} mathrm{Hg} ) в. ( 240 mathrm{mm} mathrm{Hg} ) ( mathbf{c} .736 mathrm{mm} mathrm{Hg} ) D. ( 760 mathrm{mm} mathrm{Hg} ) |
12 |

1034 | Illustration 2.206 Van’t Hoff factors of aqueous solutions of X, Y, and Z are 2.8, 1.8, and 3.5, respectively. Which of the following statement(s) is(are) correct? a. BP: X<Y<Z b. FP: Z<X<Y c. Osmotic pressure: X=Y= Z d. VP: Y<3 <3 |
12 |

1035 | What is the concentration of nitrate ions if equal volumes of ( 0.1 M A g N O_{3} ) and ( 0.1 M ) NaCl are mixed together? ( mathbf{A} cdot 0.1 mathrm{M} ) B. 0.2 М c. 0.05 M D. 0.25 м |
12 |

1036 | At high altitudes, the boiling of water takes place below ( 100^{circ} mathrm{C} ) because : A. the atmospheric pressure is low B. the temperature is low c. the atmospheric pressure is high D. none of the above |
12 |

1037 | A mixture contains 1 mole of volatile liquid ( Aleft(P_{A}^{circ}=100 m m H gright) ) and 3 moles of volatile liquid ( boldsymbol{B}left(boldsymbol{P}_{boldsymbol{B}}^{circ}=right. ) ( 80 m m H g) . ) If solution behaves ideally the total vapour pressure of the distillate is : A. ( 85 mathrm{mm} ) Hg B. ( 85.88 mathrm{mm} ) Н ( mathbf{c} .90 mathrm{mm} mathrm{Hg} ) D. ( 92 mathrm{mm} ) Hg |
12 |

1038 | What is the molarity of ( 2.00 g ) of ( N a O H ) dissolved in a total solution volume of ( 250 m L ? ) ( mathbf{A} cdot 0.2 M ) в. ( 0.5 mathrm{M} ) c. ( 0.008 M ) D. 252 М |
12 |

1039 | Formation of a solution from two components can be considered as: (i) Pure solvent ( rightarrow ) separated solvent molecules, ( Delta boldsymbol{H}_{mathbf{1}} ) (ii) Pure solvent ( rightarrow ) separated solute molecules, ( Delta boldsymbol{H}_{2} ) (ii) Separated solvent and solute molecules ( rightarrow ) solution, ( Delta boldsymbol{H}_{3} ) Solution so formed will be ideal if |
12 |

1040 | Example 2.4 At 298 K, the vapour pressure of water is 23.75 mm Hg. Calculate the vapour pressure at the same temperature over 5% aqueous solution of urea. – [CO (NH2)2). |
12 |

1041 | Which of the following plot is correct for an ideal binary solution of liquids ( A ) and B with ( boldsymbol{P}_{A}^{o}>boldsymbol{P}_{B}^{o} ) ( A ) в. ( c ) D. |
12 |

1042 | Which of the following solution contains approximately equal hydrogen ion concentration? This question has multiple correct options A. ( 100 mathrm{mL} ) of ( 0.1 mathrm{M} mathrm{HCl}+50 mathrm{mL} mathrm{H}_{2} mathrm{O} ) B. ( 75 mathrm{mL} ) of ( 0.1 mathrm{M} mathrm{HCl}+75 mathrm{mL} mathrm{H}_{2} mathrm{O} ) c. ( 50 mathrm{mL} ) of ( 0.1 mathrm{M} mathrm{H}_{2} mathrm{SO}_{4}+100 mathrm{mL} mathrm{H}_{2} mathrm{O} ) D. ( 100 mathrm{mL} ) of ( 0.1 mathrm{N} mathrm{H}_{2} mathrm{SO}_{4}+50 mathrm{mL} mathrm{H}_{2} mathrm{O} ) |
12 |

1043 | A sample of wustite ( F e_{x} O ) contains one ( boldsymbol{F} e(boldsymbol{I} boldsymbol{I} boldsymbol{I}) ) for every three ( boldsymbol{F} boldsymbol{e}(boldsymbol{I} boldsymbol{I}) . ) The value of ( x ) is: ( mathbf{A} cdot 9 / 8 ) в. ( 8 / 9 ) c. ( 3 / 4 ) D. ( 4 / 3 ) |
12 |

1044 | Illustration 2.137 Calculate the amount of ice that will separate out on cooling containing 50 g of ethylene glycol in 200 g of water to -9.3°C. (K, for water = 1.86 K mol-1 kg) |
12 |

1045 | Example 2.2 The vapour pressure of water at 293 K is 17.51 mm. The lowering of vapour pressure of sugar is 0.0614 mm. Calculate: a. The relative lowering of vapour pressure b. The vapour pressure of the solution c. The mole fraction of water |
12 |

1046 | A solution with negative deviation among the following is: A. ethanol- acetone B. chlorobenzene-bromobenzene c. chloroform-acetone D. benzene-toluene |
12 |

1047 | The vapour pressure of a dilute solution of a solute is not influenced by: A. temperature of solution B. melting point of solute c. mole fraction of solute D. degree of dissociation of solute |
12 |

1048 | At ( 90^{circ} mathrm{C} ), the vapour pressure of toluene is 400 torr and that of ( sigma-x y ) lene is 150 torr. What is the composition of the liquid mixture the boils at ( 90^{circ} mathrm{C}, ) when the pressure is 0.50 atm? What is the composition of vapour produced? A. Toluene 8 mol%, Toluene=3.2 mol% B. Toluene 15mol%, Toluene=36 mol% c. Toluene 85 mol%, Toluene=64 mol% D. Toluene 92 mol%, Toluene ( =96.8 mathrm{mol%} ) |
12 |

1049 | Each pair forms ideal solution except : A. ( C_{2} H_{5} B r ) and ( C_{2} H_{5} I ) в. ( C_{6} H_{5} C l ) and ( C_{6} H_{5} B r ) c. ( C_{6} H_{6} ) and ( C_{6} H_{5} C H_{3} ) D. ( C_{2} H_{6} I ) and ( C_{2} H_{5} O H ) |
12 |

1050 | The vapour pressure of a mixture of two volatile liquids is expressed as ( boldsymbol{P}_{boldsymbol{m}}= ) ( 6.0+1.5 X_{B}, ) where, ( X_{B} ) is mole fraction of ( boldsymbol{B} ) is a mixture. The vapour pressure of ( boldsymbol{A} ) at the same temperature is: |
12 |

1051 | Ilustration 2.125 45 g of ethylene glycol C,H,O, is mixed with 600 g of water. Calculate (a) the freezing point depression and (b) the freezing point of the solution. Given K= 1.86 K kg moll (NCERT Example 2.9) |
12 |

1052 | State and explain Avogadro’s law | 12 |

1053 | At ( 25^{circ} mathrm{C}, 1 ) mol of ( A ) having a vapour pressure of 100 torr and 1 mol of ( B ) having a vapour pressure of 300 torr were mixed. The vapour at equilibrium is removed, condensed and the condensate is heated back to ( 25^{circ} C ) The vapour now formed are again removed, recondensed and analyzed.If the mole fraction of ( A ) in this |
12 |

1054 | A solution contains ( 75 mathrm{mg} ) of ( mathrm{NaCl} ) per mL. To what extent must it be diluted to give a solution of concentration ( 15 mathrm{mg} ) of ( N a C l ) per mL of solution? |
12 |

1055 | Question 9. A sample of drinking water was found to be several contaminated with chloroform (CHCIZ) supposed to a carcinogen. level of contamination was 15 ppm (by mass): (i) Express this in per cent by mass. (ü) Determine the molality of chloroform in the water sample. ppm= parts per million = 10 units Determine mass % and molality as in previous problems. |
12 |

1056 | In an expression of the equilibrium constant, units for concentrations are: A. mol/mL B. mol/L ( c cdot g / L ) D. gram-equivalents/L |
12 |

1057 | An Unsaturated solution can be converted into saturated solution A. by adding more solute to the solvent B. by removing solute from the solvent c. by increasing temperature D. Both b and c |
12 |

1058 | Two glucose solutions are mixed of ( 1 M ) and ( 2 M ) respectively in equal volume ratio then the new molarity will be: ( mathbf{A} cdot 1.4 M ) в. ( 1.25 M ) c. ( 1.5 M ) D. ( 1.27 M ) |
12 |

1059 | At ( 80 C, ) the vapour pressure of pure benzene is ( 753 mathrm{mm} ) Hg and of pure toluene ( 290 mathrm{mm} ) Hg. Calculate the composition of a liquid in mole per cent which at ( 80 C ) is in equilibrium with the vapour containing 30 mole per cent of benzene. |
12 |

1060 | The sum of mole fractions of solute and solvent of a solution is equal to: A. number of moles of solute B. number of moles of solvent c. number of moles of solution D. unity |
12 |

1061 | Percentage of ( K_{2} S O_{4} ) in the sample is: A . ( 65.75 % ) в. 72 % ( c .60 .35 % ) D. 78.74 % |
12 |

1062 | The molarity of a glucose solution containing 36 g of glucose per ( 400 mathrm{mL} ) of the solution is: A . 1.0 B. 0.5 c. ( 2 . ) D. 0.05 |
12 |

1063 | What is the vapour pressure of the solution containing ( 34.2 mathrm{g} ) of sucrose per 100 g of water at ( 25^{circ} mathrm{C} ) ? The vapour pressure of water at ( 25^{circ} mathrm{C} ) is ( 23.75 mathrm{mm} ) ( A cdot 20.3 mathrm{mm} ) B. 23.10 mm c. Unpredictable D. 23.33 mm |
12 |

1064 | For a given value of degree of dissociation,which of the following have correct Van’t Hoff factor? This question has multiple correct options A. ( N a C l, i=2+alpha ) в. ( C aleft(N O_{3}right)_{2}, i=1+2 alpha ) C . ( K_{4}left[F e_{3}(C N)_{6}right], i=1+4 alpha ) D. ( left(N H_{3}right)_{3} P O_{4}, i=3+alpha ) |
12 |

1065 | ( Y ) molal solution of a compound in benzene has mole fraction of solute equal to ( 0.2 . ) The value of ( ? ) A . 14 B. 3. c. 1.4 D. 2 |
12 |

1066 | Illustration 2.148 When dehydrated fruits and vegetables are placed in water, they slowly swell and return to original form. Why? Would a temperature increase accelerate the process? Explain. |
12 |

1067 | Illustration 2.105 What is an antifreeze? | 12 |

1068 | The vapour pressure of pure water at ( 26^{circ} mathrm{C} ) is 25.21 torr. The vapour pressure of a solution which contains 20.0 g glucose, ( C_{6} H_{12} O_{6}, ) in 70 g water is : A .22 .5 torr B . 23.4 torr c. 24.4 torr D. 24.5 torr |
12 |

1069 | A solution is prepared by dissolving ( 5.64 mathrm{g} ) of glucose in ( 60 mathrm{g} ) of water. Calculate the mole fraction of each of glucose and water respectively. B. 0.009, 0.991 c. 1.12,0.08 D. 0.789, 0.211 |
12 |

1070 | The vapour pressure of two miscible liquids ( (A) ) and ( (B) ) are 300 and ( 500 m m ) of ( H g ) respectively. In a flask 10 mole of ( (A) ) is mixed with 12 mole of ( (B) . ) However, as soon as ( (B) ) is added, ( (A) ) starts polymerising into a completely insoluble solid. The polymerisation follows first-order kinetics. After 100 minute, 0.525 mole of a solute is dissolved which arrests the polymerisation completely. The final vapour pressure of the solution is 400 mm of ( H g . ) Estimate the rate constant of the polymerisation reaction. Assume negligible volume change on mixing and polymerisation and ideal behaviour for the final solution. A . ( 1.3 times 10^{-2} ) B . ( 15 times 10^{-3} ) c. ( 2.0 times 10^{-4} ) D. ( 1.0 times 10^{-4} ) |
12 |

1071 | The vapour pressure of water at ( 293 mathrm{k} ) is 2438 Pa and the vapour pressure of an aqueous solution is 2395.8 Pa. If solution density is ( 1080 mathrm{kg} / mathrm{m}^{3} ) at ( 313 mathrm{K} ) Calculate the osmotic pressure at 313 K. The molecular weight of solute =60. A .24 .54 Pa B . ( 24.54 times 10^{5} ) Pa c. 0.955 Pa D. None of these |
12 |

1072 | The b.p. of a solution of ( 5 g ) of sulphur in 100g of carbon disulphide is ( 0.476^{circ} ) above that of pure solvent. Determine the moles of sulphur in this solvent. The b.p. of pure carbon disulphide is ( 46.30^{circ} mathrm{C} ) and its heat of vaporation is 84.1 calories per gram. |
12 |

1073 | Illustration 2.122 1 g of monobasic acid in 100 g of water lowers the freezing point by 0.168º. If 0.2 g of same acid requires 15.1 mL mol-l of N/10 alkali for complete neutralization, calculate the degree of dissociation of acid. K for H,O is 1.86 K mol-1 kg. |
12 |

1074 | | Example 2.16 A tube of uniform cross-sectional area 1 cm2 is closed at one end with semi-permeable membrane. A solution of 5 g glucose per 100 mL is placed inside the tube and is dipped in pure water at 27°C. When equilibrium is established, calculate: a. The osmotic pressure of solution. b. The height developed in vertical column. Assume the density of final glucose solution 1 g mL-1 |
12 |

1075 | A solution contains ( 20 % ) solute by weight at ( 60^{circ} mathrm{C} ). Whencooled to ( 30^{circ} mathrm{C} ) the solution contains ( 10 % ) solute by weight. When ( 45 g ) solution is cooled from ( 60^{circ} mathrm{C} ) to ( 30^{circ} mathrm{C} ), the mass of solute deposited is: |
12 |

1076 | Question 11. Why do gases always tend to be less soluble in liquids as the temperature is raised? Consider the heat exchange during dissolution of gases in liquids and give answer on the basis of Le-Chatelier’s principle. |
12 |

1077 | The moles of ( B aleft(N O_{3}right)_{2} ) which on dissolving in 12 moles of water lowers the vapour pressure of water to ( 80 % ) are |
12 |

1078 | A mixture of hydrogen and oxygen contains ( 20 % ) by mass of hydrogen. What is the total number of molecules present per gram of the mixture? |
12 |

1079 | Which of the following aqueous solutions has the highest boiling point? A ( .0 .1 mathrm{M} ) К ( mathrm{NO}_{3} ) В. ( 0.1 mathrm{M} ) Na ( _{3} mathrm{PO}_{4} ) c. ( 0.1 mathrm{M} ) ВаСг D. ( 0.1 mathrm{M} mathrm{K}_{2} mathrm{SO}_{4} ) |
12 |

1080 | A solution of ( X Y(100 % ) ionised has osmotic pressure equal to four times the osmotic pressure of ( 0.01 mathrm{MBaCl}_{2} ) 100% ionised ). Find the molarity of ( boldsymbol{X} boldsymbol{Y} ) A ( cdot 6 times 10^{-2} M ) В. ( 3 times 10^{-2} M ) c. ( 4 times 10^{-2} M ) D. ( 12 times 10^{-2} M ) |
12 |

1081 | The depressions in freezing point for ( 1 mathrm{m} ) urea, ( 1 mathrm{m} ) glucose and ( 1 mathrm{m} ) NaCl are in the ratio: A .1: 2: 3 B. 3:2:2 c. 1: 1: 2 D. None of these |
12 |

1082 | (Molarity/Molality) is the number of moles of solute dissolved per kg of solvent. |
12 |

1083 | For an ideal solution containing a nonvolatile solute, which of the followig expressions represents the vapour pressure of the solution? ( left(x_{1} rightarrowright. ) mole fraction of solvent A ( . p=x_{2} p_{2} ) В . ( p=x_{1} p_{2}^{*} ) c. ( p=x_{1} p_{1}^{*} ) D. ( p_{1}^{*}-p=x_{2} ) |
12 |

1084 | Ilustration 2.84 What happens to the vapour pressure of water if a table spoon of sugar is added to it? |
12 |

1085 | A solution containing 7 g of a solute (molar mass 210 g ( m o l^{-1} ) ) in 350 g of acetone raised the boiling point of acetone from ( 56^{circ} mathrm{C} ) to ( 56.3^{circ} mathrm{C} ). The value of ebullioscopic constant of acetone in ( mathrm{K} mathrm{kg} operatorname{mol}^{-1} ) is : A . 2.66 B. 3.15 c. 4.12 D. 2.86 |
12 |

1086 | A student slowly mixes salt into ( 25 mathrm{m} ) of water until no more salt dissolves in it. The student could make more salt dissolve in the solution by: A. cooling it B. evaporating it c. heating it D. stirring it |
12 |

1087 | ( R H_{2} ) (ion exchange resin) can replace ( C a^{2+} ) ions in hard water as: ( R H_{2}+ ) ( C a^{2+} rightarrow R C a+2 H^{+} ) If ( 1 L ) of hard water after passing through ( R H_{2} ) has ( p H=3, ) then hardness in parts per million of ( C a^{2+} ) is: A. 80 B. 10 ( c cdot 40 ) D. 100 |
12 |

1088 | A mixture of ( N a O H ) and ( M g(O H)_{2} ) weights 2.325 g. It requires 3 g of ( H_{2} S O_{4} ) for its neutralization. What is the percentage composition of mixture? |
12 |

1089 | Van’t Hoff factor of ( 0.01 M B a C l_{2} ) is 1.98, percentage dissociation of ( B a C l_{2} ) on this concentration will be: ( mathbf{A} cdot 69 ) в. 100 c. 49 D. 98 |
12 |

1090 | Vapour pressures of pure acetone and chloroform at ( 328 K ) are 741.8 mm ( H g ) and 632.8 mm ( H g ) respectively. Assuming that they form ideal solution over the entire range of composition, plot ( boldsymbol{p}_{text {total}}, boldsymbol{p}_{text {chloroform}}, ) and ( boldsymbol{p}_{text {acetone}} ) as a function of ( x_{text {acetone}} . ) The experimental data observed for different compositions of mixture is: 100x ( x_{text {acetone }} ) What is and ( P_{text {actone}} / m m H g ) 54 ( P_{text {chloro}} ) of or ( / m m ) ( H g ) 632.8 548.1 Plot this data also on the same graph paper. Indicate whether it has positive deviation or negative deviation from the ideal solution. |
12 |

1091 | Osmotic pressure of the solution obtained by dissolving ( 100 g m ) of an organic compound in 1 litre solution is ( 2.414 times 10^{5} frac{N}{m^{2}} ) at ( 298 K . ) The organic compound can be: A. glucose B. urea c. maltose D. Nacl |
12 |

1092 | Q. 26 What is the difference between molality and molarity? | 12 |

1093 | ( 200 mathrm{mL} ) of an aqueous solution of a protein contains its 1.26 g. The osmotic pressure of this solution at ( 300 mathrm{K} ) is found to be ( 2.57 times 10^{-3} ) bar. The molar mass of protein will be: ( left(boldsymbol{R}=mathbf{0 . 0 8 3} boldsymbol{L} boldsymbol{b a r} boldsymbol{m o l}^{-1} boldsymbol{K}^{-1}right) ) ( A cdot 61038 ) g mol ( ^{-1} ) B. 51022 g mol-1 C. ( 122044 mathrm{g} mathrm{mol}^{-1} ) D. 31011 g mol- |
12 |

1094 | A binary liquid solution is prepared by mixing n-heptane and ethanol. Which one of the following statement is correct regarding the behavior of the solution? A. The solution formed is an ideal solution B. The solution is non-ideal, showing +ve deviation from Raoults Law c. The solution is non-ideal, showing ve deviation from Raoults Law D. n-heptane shows +ve deviation while ethanol shows ve deviation from Raoults Law |
12 |

1095 | The ( boldsymbol{K}_{s p} ) for ( boldsymbol{C r}(boldsymbol{O H})_{3} ) is ( 1.6 times 10^{-30} ) The solubility of this compound in water is: ( mathbf{A} cdot 4 sqrt{1.6 times 10^{-30}} ) в. ( 4 sqrt{1.6 times 10^{-30} / 27} ) c. ( 1.6 times 10^{-9} ) D. ( 2 sqrt{1.6 times 10^{-30}} ) |
12 |

1096 | A complex is represented as ( C o C l_{3} ) ( X N H_{3} . ) Its 0.1 molal solution in water shows ( Delta T_{f}=0.558^{circ} C . K_{f} ) of ( H_{2} O ) is ( 1.86 mathrm{K} / mathrm{m} . ) Assuming ( 100 % ) ionisation, the number of ( N H_{3} ) molecules associated with Co is: |
12 |

1097 | A china dish weighs 25 g when empty. When a saturated solution of potassium chloride is poured into it at ( 40^{circ} mathrm{C}, ) the weight of the dish is 63 g. When the solution is totally evaporated, the chine dish along with the crystals weighs 40 g. Find the solubility of potassium chloride at ( 40^{0} mathrm{C} ) A . 35 B. 65.2 c. 39.5 D. 7.5 |
12 |

1098 | Calculate the concentration of solution which contains 5 g of salt dissolved in 100 g water A . 5.26 B. 9.52 ( c cdot 4.54 ) D. 4.76 |
12 |

1099 | For the two compounds, the vapour pressure of (2) at a particular temperature is expected to be:- ( (i) ) (ii) A. Higher than (i) B. Lower than that of (i) c. Same as that of (i) D. Can be ‘higher or lower depending upon the size of the vessel |
12 |

1100 | A decimolar solution of potassium ferrocyanide is ( 50 % ) dissociated at 300 K. Calculate the osmotic pressure of the solution. |
12 |

1101 | The density of lake water is 1.3 g/cc. and it contains 69 g of ( N a^{+} ) ions per kg of water. What is molality of ( N a^{+} ) ion in the lake? ( A cdot 1 m ) B. 3 ( m ) ( c cdot 2 m ) D. ( 4 mathrm{m} ) |
12 |

1102 | The mole fraction of benzene in a solution containing ( 39 % ) by mass in an organic solvent of molecular mass 122 is : A . 0.5 B. 0.6 ( c .0 .4 ) D. 0.35 |
12 |

1103 | The largest value of Henry’s law constant for the liquid solvent ( mathrm{H}_{2} mathrm{O} ) will be obtained with …………… gas as the solute and a temperature of ( ldots ) A. ( C_{2} H_{4}, 45 ) B. ( A r, 11 ) с. ( H C l, 49 ) D. ( C O_{2}, 32 ) |
12 |

1104 | What is the degree of hardness of a sample of water containing 24 mg of ( M g S O_{4}(text { mol. mass } 120) ) per kg of water? A . 10 pp в. 15 ррт c. 20 ppm D. 25 ppm |
12 |

1105 | Example 2.6 A certain solution of 1 m benzoic acid in benzene has a freezing point of 3.1°C and a normal boiling point of 82.6°C. The freezing point of benzene is 5.5°C and its boiling point is 80.1°C. Analyze the state of the solute (benzoic acid) at two temperatures and comment. |
12 |

1106 | A current of dry air was passed through a series of bulbs containing 1.25 g of a solute ( A_{2} B ) in 50 g of water and then through pure water. The loss in mass of the former series of bulbs was 0.98 g and in the later series 0.01 g. If the molar mass of ( A_{2} B ) is ( 80, ) the degree of dissociation of ( A_{2} B ) is (divide answer by ( 10): ) |
12 |

1107 | A maxima or minima obtained in the temperature composition curve of a mixture of two liquids indicates: A. an azeotropic mixture B. an eutectic formation c. that the liquids are immiscible with one another D. that the liquids are partially miscible at the maximumm or minimum |
12 |

1108 | Addition of which of the following material to water does not make it hard? ( mathbf{A} cdot M g_{3}left(P O_{4}right)_{2} ) B. ( operatorname{Fe}left(mathrm{NO}_{3}right)_{3} ) c. ( Vleft(N O_{3}right)_{3} ) D. ( T ileft(C l O_{4}right)_{4} ) |
12 |

1109 | The mole fraction of water in ( 98 % ) (w/w) ( H_{2} S O_{4} ) solution is : A . ( 0 . ) B. 0.9 ( c cdot 0.8 ) D. 0.02 |
12 |

1110 | Ice skating can be used to demonstrate that when ice is under pressure, its: A. Melting point remains unchanged B. Melting point is raised c. Melting point is lowered D. coefficient of friction with metal is reduced |
12 |

1111 | The osmotic pressure of equimolar solutions of urea, ( B a C l_{2} ) and ( A l C l_{3} ) will be in the order of: A ( cdot A l C l_{3}>U r e a>B a C l_{2} ) в. Urea( >B a C l_{2}> )АlСl( _{3} ) c. ( A l C l_{3}>B a C l_{2}>U r e a ) D. ( B a C l_{2}>A l C l_{3}>U r e a ) |
12 |

1112 | The Van’t Hoff’s factor ( ^{prime} boldsymbol{i}^{prime} ) accounts for: A. extent of dissolution of solute B. extent of mobility of solute c. extent of solubility of solute D. extent of dissociation of solute |
12 |

1113 | Assertion The solubility of a solid in a liquid increases with increase of pressure. Reason Solubility of gas in a liquid is directly proportional to the pressure of the gas. |
12 |

1114 | Which of the following equimolar solution have highest vapour pressure? A. Glucose B. ( N a C l ) c. ( K_{2} S O_{4} ) D. ( K_{4} ) Fe ( (C N)_{6} ) |
12 |

1115 | Example 2.31 Calculate the Van’t Hoff factor when 0.1 mol NH,Cl is dissolved in 1 L of water. The degree of dissociation of NH 1,Cl is 0.8 and its degree of hydrolysis is 0.1. |
12 |

1116 | Example 2.18 2.5 g of a substance is present in 200 mL of solution showing the osmotic pressure of 60 cm Hg at 15°C. Calculate the molecular weight of substance. What will be the osmotic pressure if temperature is raised to 25°C? |
12 |

1117 | The vapour pressure of a solvent decreased by ( 10 mathrm{mm} ) of mercury when a non-volatile solute was added to the solvent. The mole fraction of the solute in the solution is ( 0.2 . ) What should be the mole fraction of the solvent, if the decrease in the vapour pressure is to be 20 mm of mercury? A . 0.8 B. 0.6 ( c .0 .4 ) D. 0.2 |
12 |

1118 | Dissolving 120 gm of a compound of (mol.wt. 60 ) in 1000 g of water gave a solution of density ( 1.5 mathrm{g} / mathrm{mL} ). The molarity of the solution is: A ( .1 .00 M ) в. ( 1.78 M ) ( c .2 .50 M ) D. ( 4.00 M ) |
12 |

1119 | A solution in which, still more number of solute can be dissolved, is known as: A. unsaturated B. super saturated c. saturated D. dilute E. concentrated |
12 |

1120 | Which one of the following statements regarding Henry’s law is not correct? A. The value of ( K_{H} ) increases with the function of the nature of the gas B. Higher the value of ( K_{H} ) at a given pressure, higher is the solubility of the gas in the liquids C. The partial of the gas in vapour phase is proportional to the mole fraction of the gas in the solution D. Different gases have different ( K_{H} ) (Henry’s law constant) values at the same temperature |
12 |

1121 | Water and chlorobenzene are immiscible liquids. Their mixture boils at ( 89^{circ} mathrm{C} ) under a reduced pressure of ( 7.7 times 10^{4} ) Pa. The vapour pressure of pure water at ( 89^{circ} mathrm{C} ) is ( 7 times 10^{4} mathrm{Pa} ) Weight percent of chlorobenzene in the distillate is: A . 50 B. 60 c. 79 D. 38.46 |
12 |

1122 | The Henry’s law constant for the solubility of ( N_{2} ) gas in water at ( 298 K ) is ( 1.0 times 105 ) atm. The mole fraction of ( N_{2} ) in air is ( 0.8 . ) The number of moles of ( N_{2} ) from air dissolved in 10 moles of water at ( 298 K ) and 5 atm pressure is A ( cdot 4 times 10^{-4} ) B . ( 4 times 10^{-5} ) ( mathbf{c} cdot 5 times 10^{-4} ) D. ( 4 times 10^{-6} ) |
12 |

1123 | Equimolal solutions ( A ) and ( B ) show depression in freezing point in the ratio 2:1. A remains in the normal state in solution B will be : A. Normal in solution B. Dissociated in solution C. Associated in solution D. Hydrolysed in solution |
12 |

1124 | Match the mixture given in column with the corresponding type of solutions given in column II | 12 |

1125 | A solution containing 0.2563 g of naphthalene (molecular mass = 128) in ( 50 mathrm{g} ) of carbon tetrachloride yields a boiling point elevation of ( 0.201^{circ} mathrm{C} ) while a solution of 0.6216 g of an unknown solute in the same mass of the solvent gives a boiling point elevation of ( 0.647^{circ} mathrm{C} . ) Find the molecular mass of the unknown solute. |
12 |

1126 | State True or False. For two solutions to be isotonic, ( boldsymbol{C}_{mathbf{1}}= ) ( C_{2} ) in all the cases. A. True B. False |
12 |

1127 | Illustration 2.198 1575.2 g of C,H,OH (phenol) is dissolved in 960 g of a solvent of K. = 14 K kg mol-1. If the depression in freezing point is 7 K, then find the percentage of phenol that dimerizes. |
12 |

1128 | When ethanol mixes in cyclohexane, the intermolecular forces reduces between ethanol molecule. In this, liquid pair shows: A. positive deviation from Raoult’s law B. negative deviation from Raoult’s law c. no deviation from Raoult’s law D. decrease in volume |
12 |

1129 | Which condition is not satisified by an ideal solution? A ( cdot Delta H_{operatorname{mixing}}=0 ) B. ( Delta V_{text {mixing}}=0 ) C. ( Delta S_{text {mixing}}=0 ) D. obeyance of Raoult’s law |
12 |

1130 | To what temperature should water be heated so that its vapor pressure equals the vapor pressure chloroform at ( 40^{circ} mathrm{C} ? ) ( mathbf{A} cdot 40^{circ} C ) ( mathbf{B} cdot 50^{circ} C ) ( mathbf{c} cdot 60^{circ} C ) D. ( 70^{circ} mathrm{C} ) ( E cdot 80^{circ} C ) |
12 |

1131 | Illustration 2.63 What are maximum boiling azeotropes? Give one example. |
12 |

1132 | In an ideal solution of non-volatile solute ( mathrm{B} ) in solvent ( mathrm{A} ) in 2: 5 molar ratio has vapour pressure ( 250 mathrm{mm} ). If another solution in ratio 3: 4 prepared then vapour pressure above this solution is: ( A cdot 200 mathrm{mm} ) B. 250 mm c. 350 ( mathrm{mm} ) D. ( 400 mathrm{mm} ) |
12 |

1133 | ( 0.2 g ) of fine animal charcoal is mixed with half litre of acetic acid ( (2 M) ) solution and shaken for 30 minutes? A. Concentration remains same B. Concentration increases c. concentration of the solution decreases D. None of above |
12 |

1134 | The vapour pressure of water is ( 12.3 k P a ) at ( 300 K . ) Calculate the vapour pressure 1 molal solution of a non- volatile solute in it ( mathbf{A} cdot 12.08 k P a ) B. 1.208 Ppa ( mathrm{c} .2 .4 mathrm{kPa} ) D. ( 0.4 k P a ) |
12 |

1135 | Which of the following pairs of solutions are expected to be isotonic, temperature being the same? A ( cdot 0.1 mathrm{M} ) glucose and ( 0.1 mathrm{M} mathrm{C}_{6} mathrm{H}_{5} mathrm{N}^{+} mathrm{H}_{3} mathrm{Cl} ) B. ( 0.1 mathrm{M} ) NaCl and ( 0.05 mathrm{M} ) BaCl , c. ( 0.1 mathrm{M} mathrm{Na}_{2} mathrm{SO}_{4} ) and ( 0.1 mathrm{M} mathrm{KNO} ) D. ( 0.1 mathrm{M} ) BaCl( _{2} ) and ( 0.075 mathrm{M} ) FeCl( _{3} ), |
12 |

1136 | Two liquids ( A ) and ( B ) form a non ideal solution which obey the equation: ( boldsymbol{P}_{boldsymbol{T}}+boldsymbol{P}_{boldsymbol{A}}^{boldsymbol{o}}+boldsymbol{3}left(boldsymbol{P}_{boldsymbol{B}}^{boldsymbol{o}}-boldsymbol{P}_{boldsymbol{A}}^{boldsymbol{o}}right) boldsymbol{X}_{boldsymbol{B}}+boldsymbol{2}left(boldsymbol{P}_{boldsymbol{A}}^{boldsymbol{o}}-right. ) ( left.P_{B}^{o}right) X_{B}^{2} ) When an equimolar mixture of ( A ) and ( B ) is distilled, find the composition (by mole) when this mixture will have a single boiling point. ( left(P_{B}^{o}>P_{A}^{o}right) ) where ( P_{A}^{o} ) and ( P_{B}^{o} ) are vapour pressure of pure ( A ) and ( B ) respectively and ( X_{B}= ) is the mole fraction of ( B ) in the liquid phase. A. 3: B. 2:3 c. 1: 2 D. 1: 3 |
12 |

1137 | 3 moles of ( boldsymbol{P} ) and 2 moles of ( boldsymbol{Q} ) are mixed, what will be their total vapour pressure in the solution if their partial vapour pressures are 80 and 60 torr respectively? A. 80 torr B. 140 torr c. 72 torr D. 70 torr |
12 |

1138 | The ppm strength of ( C O_{2}(g) ) volume by volume ( left(mathrm{mL} text { of } C mathrm{O}_{2} text { per } 10^{6} mathrm{mL} ) of air) is: right. A .224 в. 2240 c. 100 D. 1000 |
12 |

1139 | ( mathbf{A} mathbf{5} . mathbf{8 5} %(mathbf{w} mathbf{t} / mathbf{v} text { ol }) mathbf{N} boldsymbol{a} boldsymbol{C l} ) solution will exert an osmotic pressure closet to which one of the following. A. ( 5.85 % ) (wt/vol) sucrose solution B. ( 5.85 % ) (wt/vol) glucose solution c. 2 m sucrose solution D. ( 1 mathrm{m} ) glucose solution |
12 |

1140 | ( 16.0 mathrm{g} ) of NaOH is present in ( 100 mathrm{ml} ) of an aqueous solution. Its density is 1.06 g/ml. Mole fraction of the solute is approximately: ( mathbf{A} cdot 25 / 27 ) B. 2 /27 c. ( 1 / 27 ) D. ( 26 / 27 ) |
12 |

1141 | A solution of acetone is ethanol: A. shows a negative deviation from Raoult’s law B. shows a positive deviation from Raoult’s law C. behaves like a near ideal solution D. obeys Raoult’s law |
12 |

1142 | Illustration 2.175 A solution of an organic compound is prepared by dissolving 30 g in 100 g water. Calculate the molecular mass of compound and the osmotic pressure of solution at 300 K, when the elevation in boiling point is 0.52 and K, for water is 0.52 K m-1. |
12 |

1143 | The molality ( (mathrm{m}) ) of each ion ( left(mathrm{N} boldsymbol{H}_{4}^{+} ) and right. ( left.C l^{-}right), ) respectively, present in the aqueous solution of ( 2 M N H_{4} C l ) assuming ( 100 % ) dissociation according to given reaction is, ( N H_{4} C l(a q) rightarrow N H_{4}^{+}(a q)+C l^{-}(a q) ) Given that density of solution ( =3.107 ) ( mathrm{g} / mathrm{ml} ) A ( .0 .45 mathrm{m}, 0.67 mathrm{m} ) в. ( 0.67 mathrm{m}, 0.45 mathrm{m} ) ( c .0 .67 m, 0.67 m ) ( m ) D. ( 0.45 mathrm{m}, 0.45 mathrm{m} ) |
12 |

1144 | ( mathbf{A} ) 0.1 molar solution of ( N a C l ) is found to be isotonic with ( 1 % ) urea solution. Calculate (a) Van’t Hoff factor (b)Degree of dissociation of sodium chloride. Assume density of ( 1 % ) urea equal to |
12 |

1145 | The azeotropic solutions of two miscible liquids: A. can be separated by simple distillation B. are supersaturated solutions C. behave like a single component and boil at a constant temperature D. none of the above |
12 |

1146 | The total pressure when this drop formed in torr is | 12 |

1147 | The osmotic pressure of equimolar solutions of ( mathrm{BaCl}_{2}, ) NaCl and glucose will be in the order: A ( . ) glucose ( >N a C l>B a C l_{2} ) в. ( B a C l_{2}>N a C l> ) glucose c. ( N a C l>B a C l_{2}>g l u operatorname{cose} ) D. ( N a C l>g l u c o s e>B a C l_{2} ) |
12 |

1148 | Which of the following combinations of ( 0.20 M ) aqueous solutions will form a precipitate on mixing? I. ( A g N O_{2} ) and ( H C l ) Il. ( B a C_{2} H_{2} O_{2} ) and ( M g S O_{4} ) III. ( boldsymbol{K} boldsymbol{I} ) and ( boldsymbol{P b}left(boldsymbol{N} boldsymbol{O}_{3}right)_{2} ) A. I only B. I and II only c. I and III only D. II and III only E . ।, II, and III |
12 |

1149 | Saturated solution of NaCl on heating: A. becomes supersaturated B. becomes unsaturated c. remains saturated D. vaporises |
12 |

1150 | Calculate the molality of 1 litre solution containing ( 93 % H_{2} S O_{4}(W / V) ) if the density of the solution is ( 1.84 g m L^{-1} ) |
12 |

1151 | The elevation in boiling point of a solution of 13.44 g of ( C u C l_{2} ) (Molar mass 134.4 ) in ( 1 mathrm{kg} ) water is: ( left[boldsymbol{K}_{boldsymbol{b}}=mathbf{0 . 5 2} mathrm{K} text { molality }^{-1}right] ) A . 0.16 B. 0.05 c. ( 0 . ) D. 0.2 |
12 |

1152 | The weight (in-grams) of ( A g N O_{3} ) present in ( 100 mathrm{ml} ) of ( 0.25 mathrm{M} ) solution: A . 4.25 B. 2 c. 17 D. 1. |
12 |

1153 | ( 33.6 mathrm{L} ) of water vapour at STP are condensed to liquid state. The volume occupied by it is approximately: A . ( 1 mathrm{mL} ) B. 18 mL c. 27 ( mathrm{mL} ) D. 127 mL |
12 |

1154 | The vapour pressure of pure benzene is ( 639.7 mathrm{mm} mathrm{Hg} ) and the vapour pressure of a solution of a solute in benzene at the temperature is ( 631.9 mathrm{mm} ) Hg. If the molality of the solution is ( 156 times 10^{-x} ) then what is the value of ( x ? ) |
12 |

1155 | To cool a liquid just below its f.pt. is called super cooling. If true enter 1 , if false enter 0 . |
12 |

1156 | A ( 10 % ) solution of ( N a C l ) means that in ( 100 g ) of solution there is: A. ( 5.85 g ) NaCl в. ( 58.5 g ) NaCl c. ( 10 g ) NaCl D. ( 94 g ) NaCl |
12 |

1157 | Illustration 2.37 At 20°C, the vapour pressure of pure liquid A is 22 mm Hg and that of pure liquid B is 75 mm Hg. What is the composition of the solution of these two components that has vapour pressure of 48.5 mm Hg at this temperature? |
12 |

1158 | Hlustration 2.127 Addition of 0.40 g of a compound to 45.5 mL of benzene (density 0.879 g mL-1) lowers the freezing point from 5.51°C to 4.998°C. If K, for benzene is 5.12 K kg mol-1, calculate the molar mass of the compound. |
12 |

1159 | The vapour pressure of water at ( 23^{circ} C ) is ( 19.8 mathrm{mm} .0 .1 mathrm{mole} ) glucose is dissolved in ( 178.2 mathrm{g} ) water. What is the vapour pressure (in ( mathrm{mm} ) ) of the resultant solution? ( A cdot 19 ) B. 19.602 c. 19.402 D. 19.202 |
12 |

1160 | Match the following Column – I Column – II a) A nearly ideal solution p) ( H_{2} O+ ) [ C_{2} H_{5} O H ] b) A solution q) ( C_{6} H_{6}+ ) showing positive deviation ( quad C_{6} H_{5} C H_{3} ) c) A solution r) ( C_{6} H_{6}+C H C l_{3} ) showing negative deviation s) ( C H_{3} C O C H_{3}+ ) d) An azeotropic mixture [ C_{2} H_{5} O H ] ( t ) ( Delta H ) and ( Delta V ) are positive and ( Delta V ) ( Delta H ) u) are negative ( mathbf{A} cdot mathrm{A}-mathrm{q} ; mathrm{B}-mathrm{s}, mathrm{t} ; mathrm{C}-mathrm{r}, mathrm{u} ; mathrm{D}-mathrm{p} ) B. ( A-s ; B-s, t ; C-r ; D-q, p ) ( mathbf{C} cdot A-q ; B-s ; C-r ; D-p, t ) D. ( A-r ; B-p ; C-s, t ; D-q ) |
12 |

1161 | The density of ( 3 M ) solution of ( N a C l ) is ( 1.25 g m l^{-1} . ) The molality of the solution is: A ( .2 .79 mathrm{m} ) В. 1.79 m c. ( 3.5 mathrm{m} ) D. 5.58 m |
12 |

1162 | What is molal elevation constant? Drive its equation and give its unit. |
12 |

1163 | Solutions which distill without change in composition or temperature are called: A. amorphous B. azeotropic mixture c. ideal D. super saturated |
12 |

1164 | The van’t Hoff factor for ( 0.1 M ) barium nitrate is ( 2.74 . ) The percentage of dissociation of barium nitrate is: A . ( 91.3 % ) B. ( 87 % ) c. ( 100 % ) D. ( 74 % ) |
12 |

1165 | Assertion The molecular weight of acetic acid determined by depression in freezing point method in benzene and water was found to be different. Reason Water is polar and benzene is non-polar. A. Both Assertion and Reason are correct and Reason is the correct explanation for Assertion B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion c. Assertion is correct but Reason is incorrect D. Assertion is incorrect but Reason is correct |
12 |

1166 | Dissolving ( 120 g ) of urea in ( 1000 g ) of water gave a solution of density ( mathbf{1 . 1 5} g / boldsymbol{m} boldsymbol{L} . ) The molarity of the solution is: A ( .1 .79 M ) в. ( 2 M ) ( c .2 .05 M ) D. 2.22 ( M ) |
12 |

1167 | Relative lowering of vapour pressure is maximum for: A. ( 0.1 mathrm{m} ) urea B. 0.1m Nacı ( mathbf{c} cdot 0.1 m quad M g C I_{2} ) D. ( 0.1 m quad A I_{2}left(S O_{4}right)_{3} ) |
12 |

1168 | Calculate the molarity of each of the following solutions: (a) ( 30 g ) of ( C oleft(N O_{3}right)_{2} cdot 6 H_{2} O ) in ( 4.3 mathrm{L} ) of solution (b) ( 30 mathrm{mL} ) of ( 0.5 mathrm{M} H_{2} S O_{4} ) diluted to 500 mL. |
12 |

1169 | When 5.0 gram of ( B a C l_{2} ) is dissolved in water to have ( 10^{6} ) gram of solution. The concentration of a solution is: A . 2.5 ppm в. 5 ррт ( c .5 M ) D. ( 5 g L^{-1} ) |
12 |

1170 | Question 7. A solution is obtained by mixing 300 g of 25% solution and 400 g of 40% solution by mass. Calculate the mass percentage of the resulting solution. (i) Calculate the masses of solute in both the solutions separately. (ii) Find the mass of solute and solution after mixing. (iii) And then mass % of solute and solvent in the resulting solution. 25 |
12 |

1171 | Calculate the molality of 1 L solution of ( 93 % H_{2} S O_{4} ) (weight/volume). The density of the solution is 1.84 g. (If the answer is ( x, text { then find }[x]) ) |
12 |

1172 | The elevation in boiling point of a solution ( d T_{b} ) is related with molality of solution ( (mathrm{m}) ) by the relation: ( boldsymbol{d} boldsymbol{T}_{boldsymbol{b}}=left[frac{boldsymbol{R} boldsymbol{T}_{boldsymbol{b}}^{2}}{boldsymbol{Delta} boldsymbol{H}_{boldsymbol{v a p}}}right]left[frac{boldsymbol{M}_{mathbf{1}}}{mathbf{1}+boldsymbol{m} boldsymbol{M}_{mathbf{1}}}right], ) where ( M_{1} ) is molar mass of solvent and ( Delta boldsymbol{H}_{boldsymbol{v} boldsymbol{a} boldsymbol{p}} ) is heat of vaporisation of solvent. For a dilute solution, the relation ( left(frac{partial T_{b}}{partial m}right)_{m rightarrow 0} ) gives: A. molal ebullioscopic constant B. elevation in boiling point C. elevation in boiling point ( partial T_{b} ) becomes more predominant D. boiling point of solvent |
12 |

1173 | The solution which has the highest boiling point temperature is: ( begin{array}{lll}text { A. } 0.1 & M & M g C l_{2}end{array} ) ( begin{array}{lll}text { В. } 0.1 & M & H C l O_{4}end{array} ) ( begin{array}{llll}text { c. } 0.1 & M & N H_{4} O Hend{array} ) ( begin{array}{lll}text { D. } 0.1 & M & text { KOH }end{array} ) ( begin{array}{lll}text { E. } 0.1 & M & L i N O_{3}end{array} ) |
12 |

1174 | 01 M solution of glucose, the depression is (d) about six times freezing point of a 0.01 M MgCl2 solution is (a) the same (b) about twice (c) about three times Thinking Process Calculate value of van’t Hoff factor then correlate it with colla solution e it with colligative property of given |
12 |

1175 | What will be the molality of the solution containing 18.25 g of ( H C l ) gas in 500 g of water? ( mathbf{A} cdot 0.1 mathrm{m} ) B. ( 1 mathrm{m} ) c. ( 0.5 mathrm{m} ) D. 2 ( m ) |
12 |

1176 | The vapour pressure of water is ( 92 mathrm{mm} ) at ( 323 mathrm{K} .18 .1 mathrm{g} ) of urea are dissolved in 100g of water. The vapour pressure is reduced by ( 5 mathrm{mm} ). Calculate the molar mass of urea. |
12 |

1177 | If in the fermentation of sugar in an enzymatic solution that is ( 0.2 M ), the concentration of the sugar is reduced to ( 0.06 M ) in ( 10 h ) to ( 0.03 M ) in ( 20 h, ) what is the order of the reacation: A . 1 B. 2 ( c .3 ) D. |
12 |

1178 | Van’t-Hoff factor(i) for this reaction is: A .2 B. ( c ) ( D ) |
12 |

1179 | Lowering in vapour pressure is highest for: A. ( 0.2 m ) urea B. ( 0.1 m ) glucose c. ( 0.1 m ) M ( g S O_{4} ) D. ( 0.1 m B a C l_{2} ) |
12 |

1180 | ( mathbf{A} ) 42 molal solution of sodium chloride in water causes an elevation in the boiling point of water by ( 1.88 mathrm{K} ). What is the value of Van’t Hoff factor? What does it signify? ( left[boldsymbol{K}_{boldsymbol{b}}=mathbf{0 . 5 2} boldsymbol{K} mathbf{k g} boldsymbol{m o l}^{-mathbf{1}}right] ) |
12 |

1181 | Enough ( N a_{2} S O_{4} ) is dissolved in water at ( 40^{circ} C ) to saturated the solution. When this occurs heat is given off. All of the following statements are true EXCEPT: A. The enthalpy change of this process is negative B. The boiling point of the solution is higher than that of pure water C. The freezing point of the solution is lower than that of pure water D. If the temperature of the water is lowered, then the solubility of ( N a_{2} S O_{4} ) decreases |
12 |

1182 | By dissolving 0.35 mole of sodium chloride in water, ( 1.30 l ) of salt solution is obtained. The molarity of the resulting solution should be reported as: A . 0.3 B. 0.269 c. 0.27 D. 0.2692 |
12 |

1183 | When ( 400 g ) of a ( 20 % ) Solution was cooled ( 50 g ) of the solute precipitated. What is the percent concentration of the remaining solution. |
12 |

1184 | The number of moles of ( C O_{2} ) that can be dissolved in a liter of water increases when the (1) pressure of the ( C O_{2} ) is increased (2) temperature of the water is increased (3) liquid is stirred A. If 1,2 and 3 are correct B. If only 1 and 2 are correct c. If only 2 and 3 are correct D. If only 1 is correct E. If only 3 is correct |
12 |

1185 | The concentration of a solution is ( 8 % ) ( (w / w) ) and ( 10 %(w / v) . ) Calculate density ( (text { in } g / m l) ) of solution. |
12 |

1186 | If for a sucrose,elevation in boiling point is ( 1.0^{circ} mathrm{C} ),then what will be the boiling point of ( N a C l ) solution for same molal concentration? ( mathbf{A} cdot 1.0^{circ} mathrm{C} ) B . ( 2.0^{circ} mathrm{C} ) ( mathbf{c} cdot 3.0^{circ} mathrm{C} ) D. ( 4.0^{circ} mathrm{C} ) |
12 |

1187 | Calculate the concentration of nitric acid in moles per litre in a sample which has a density. 1.41 g ( m L^{-1} ) and the mass per cent of nitric acid in it being ( 69 % ) |
12 |

1188 | Average osmotic pressure of human blood is 7.4 at ( m ) at ( 27^{circ} C, ) then total concentration of various solutes is: ( mathbf{A} cdot 0.1 mathrm{molL}^{-1} ) B. 0.2 molL( ^{-1} ) c. 0.3 molL ( ^{-1} ) D. 0.4 molL( ^{-1} ) |
12 |

1189 | ( D 5 W ) refers to one of the solution used as an intravenous fluid. It is a ( 5 % ) by mass solution of dextrose, ( C_{6} H_{12} O_{6} ) in water. The density of ( D 5 W ) is ( 1.08 g / m l ) The molarity of the solution is ( mathbf{A} cdot 0.3 M ) в. ( 0.6 M ) c. ( 0.28 M ) D. ( 0.26 ~ M ) |
12 |

1190 | Which of the following pair will form an ideal solution? A. Chlorobenzen, chloro ethane B. Benzene, Toluene c. Acetone, chloroform D. water, HCl |
12 |

1191 | Molarity and molality of a solution of a liquid (mol wt=50) in aqueous solution is 9 and 10 respectively. What is the density of solution? ( mathbf{A} cdot 1 g / c c ) в. ( 0.95 g / c c ) c. ( 1.05 g / c c ) D. ( 1.35 g / c c ) |
12 |

1192 | In an endothermic process, solubility increases with temperature. ( A ). increase B. decrease c. remains same D. none of the above |
12 |

1193 | Solubility of ( K B r ) shows slow rise in solubility with increase in temperature A. True B. False |
12 |

1194 | The osmotic pressure of urea solution at ( 10^{circ} mathrm{C} ) is ( 200 mathrm{mm} ) becomes ( 105.3 mathrm{mm} ) when it is diluted and the temperature raised to ( 25^{circ} mathrm{C} ). The extent of dilution is: A. 8 times B. 5 times c. 4 times D. 2 times |
12 |

1195 | A solution contains ( 15 % ) glucose ( left[boldsymbol{C}_{6} boldsymbol{H}_{12} boldsymbol{O}_{6}right] ) in water and has density ( mathbf{1 . 5} ) ( mathrm{g} / mathrm{ml} . ) Find the molarity and molality of this solution ( [boldsymbol{C}=mathbf{1 2}, boldsymbol{H}=mathbf{1}, boldsymbol{O}=mathbf{1 6}] ) |
12 |

1196 | Two liquids ( A ) and ( B ) form an ideal solution at temperature ( T . ) When the total vapour pressure above the solution if 600 torr, the amount fraction of ( A ) in the vapour phase is 0.40 and in the liquid phase is ( 0.6 . ) What are the vapour pressure of pure ( A ) and ( B ) at temperature ( T ? ) |
12 |

1197 | Solubility of which among the following substances in water increases slightly with rise in temperature? A. Potassium bromide B. Potassium chlorid c. Potassium nitrate D. Sodium nitrate |
12 |

1198 | 18 g glucose ( left(C_{6} H_{12} O_{6}right) ) is added to 178.2 ( g ) water. The vapor pressure of water (in torr) for this aqueous solution is: A . 76.0 B. 752.4 c. 759.0 D. 7.6 |
12 |

1199 | State True or False. ( C H C l_{3} ) and acetone mixture shows negative deviation from Raoult’s law. A. True B. False |
12 |

1200 | From the table given below, furnish your points of inference. begin{tabular}{ll} Substance & Solubility at ( 25^{circ} mathrm{C} ) \ ( mathrm{NaCl} ) & ( 36 mathrm{g} ) \ ( mathrm{NaBr} ) & ( 95 mathrm{g} ) \ ( mathrm{Nal} ) & ( 184 mathrm{g} ) \ hline end{tabular} |
12 |

1201 | One litre of a sample of hard water ( (d=1 ) ( g / m L ) contains 136 mg of ( C a S O_{4} ) and ( 190 mathrm{mg} ) of ( M g C l_{2} . ) What is the total hardness of water in terms of ( C a C O_{3} ? ) A. 100 ppm B. 200 ppm c. 300 ppm D. None of the above |
12 |

1202 | Illustration 2.202 Calculate the osmotic pressure of a solution containing 0.02 mol of NaCl and 0.03 mol of glucose in 500 mL at 27°C. |
12 |

1203 | How many milli moles of sucrose should be dissolved in 500 gms of water so that the difference between the boiling point and freezing point of the solution becomes ( 103.57^{circ} mathrm{C} ?left(K_{f}=right. ) ( mathbf{1} . mathbf{8 6}^{circ} boldsymbol{C} / boldsymbol{m}, boldsymbol{K}_{boldsymbol{b}}=mathbf{0 . 5} mathbf{2}^{boldsymbol{o}} boldsymbol{C} / boldsymbol{m} ) A. 500 moles B. 90 mmoles c. 1330 mmoles D. 1330 moles |
12 |

1204 | The depression in freezing point for ( 0.01 m ) aqueous solution of ( boldsymbol{K}_{boldsymbol{x}}left[boldsymbol{F} boldsymbol{e}(boldsymbol{C} boldsymbol{N})_{boldsymbol{6}}right] ) is ( boldsymbol{0 . 0 7 4 4} boldsymbol{K} . ) The motal depression constant for solvent is ( 1.86 K k g ) mol( ^{-1} . ) If the solute undergoes complete dissociation, what is the correct molecular formula for the solute? ( A cdot_{K_{2}left[F e(C N)_{6}right]} ) B ( cdot_{K_{3}}left[F e(C N)_{6}right] ) c. ( left._{Kleft[F e(C N)_{6}right.}right] ) D ( quad K_{4}left[F e(C N)_{6}right] ) |
12 |

1205 | The freezing point ( left(text { in }^{circ} Cright) ) of a solution containing 0.1 g of ( K_{3}left[F e(C N)_{6}right] ) (molar ( operatorname{mass} 329) ) in 100 g of water ( left(boldsymbol{K}_{boldsymbol{f}}=right. ) 1.86 ( K . k g . m o l^{-1} ) ) is : A. ( -2.3 times 10^{-2} ) о ( C ) В. ( -5.7 times 10^{-2} ) о ( C ) c. ( -5.7 times 10^{-3} ) о ( C ) D. ( -1.2 times 10^{-2} ) о ( C ) |
12 |

1206 | The vapour pressure of a solvent at 293 K is 100 mm Hg. Then the vapour pressure of a solution containing 1 mole of a strong electrolyte ( left(A B_{2}right) ) in 99 moles of the solvent at ( 293 mathrm{K} ) is: (Assume complete dissociation of solute) A. ( 103 mathrm{mm} ) Hg в. ( 99 mathrm{mm} ) Нв ( mathbf{c} .97 mathrm{mm} mathrm{Hg} ) D. ( 101 mathrm{mm} ) Н |
12 |

1207 | Q. 47 Match the items given in Column I and Column II. Column 1 Column II A. Saturated solution 1 Solution having same osmotic pressure at a given temperature as that of given solution B. Binary solution 2. A solution whose osmotic pressure is less than that of another C Isotonic solution 3 Solution with two components D. Hypotonic solution 4. A solution which contains maximum amount of solute that can be dissolved in a given amount of solvent at a given temperature. E Solid solution 5. A solution whose osmotic pressure is more than that of another. F. Hypertonic solution 6. A solution in solid phase, |
12 |

1208 | 0.48 Match the items given in Column I with the type of solutions given in Column II. Column 1 Column II A Soda water 1. A solution of gas in solid B. Sugar solution 2. A solution of gas in gas C German silver 3. A solution of solld in liquid D. Air 4. A solution of solid in solid E Hydrogen gas in palladium 5. A solution of gas in liquid 6. A solution of liquid in solid |
12 |

1209 | State Raoult’s law for the solution containing volatile components. What is the similarity between Raoult’s law and Henry’s law? |
12 |

1210 | When ( 100 g ) of saturated solution is evaporated at ( 50^{circ} mathrm{C}, 50 mathrm{g} ) of solid is left over. Find the solubility of the substance at ( 50^{circ} mathrm{C} ) A . 100 B. 50 c. 75 D. 25 |
12 |

1211 | Illustration 2.57 Cutting onions taken from the fridge is more comfortable than cutting those lying at room temperature. Explain why. |
12 |

1212 | A 0.004 M solution of ( N a_{2} S O_{4} ) is isotonic with a ( 0.010 mathrm{M} ) solution of glucose at same temperature. The apparent degree of dissociation of ( N a_{2} S O_{4} ) is: A . ( 25 % ) B. ( 50 % ) c. ( 75 % ) D. ( 85 % ) |
12 |

1213 | Explain homogenous and heterogenous conditions with an example. |
12 |

1214 | The correct value for the relative lowering of vapour pressure of a very dilute solution is equal to: This question has multiple correct options A. mole fraction of solute B. mole fraction of solvent C. ratio of moles of solute to moles of solvent D. ratio of moles of solvent to moles of solute |
12 |

1215 | Which of the following is a type of mixture in which constituent elements are not uniformly distributed? A. Blood B. Salt and water c. Bronze D. None of the above |
12 |

1216 | Amount in g of simple containing ( 80 % ) NaOH required to prepare 60 litre of 0.5 M solution is : A . 1000 B. 1200 ( c cdot 1500 ) D. 1600 |
12 |

1217 | A 0.1 molal solution of a monobasic acid is ( 45 % ) ionized. Calculate the depression in freezing point: (Molecular weight of the acid ( =300 ) ( left.mathrm{g} / mathrm{mol}, boldsymbol{K}_{f}=mathbf{1 . 8 6} boldsymbol{K} boldsymbol{m o l}^{-1} boldsymbol{k g}right) ) A ( .–0.199^{circ} mathrm{C} ) B . ( 2.00^{circ} mathrm{C} ) ( mathrm{c} cdot 0^{circ} mathrm{C} ) D. ( 0.269^{circ} mathrm{C} ) |
12 |

1218 | The concentration of a solution can be expressed in molarity, normality, formality and molality. Among them, which mode of expression is the most accurate for the all conditions? A. Molarity B. Formality c. Normality D. Molality |
12 |

1219 | An aqueous solution of ( 2 % ) non-volatile solute exerts a pressure of 1.004 bar at the normal boiling point of the solvent. What is the molecular mass of the solute? A ( .23 .4 mathrm{gmol}^{-1} ) B . ( 41.35 mathrm{gmol}^{-1} ) c. ( 10 mathrm{gmol}^{-1} ) D. 20.8 gmol- |
12 |

1220 | Q. 60 Discuss biological and industrial applications of osmosis. | 12 |

1221 | Two solvent ( A ) and ( B ) have ( K_{f} ) values 1.86 and ( 2.79 mathrm{K} ) mol( ^{-1} ) kg respectively. given amount of substance when dissolved in 500 g of ( A, ) it completely dimerizes and when same mass of substance is dissolved in 500 g of ( mathrm{B} ), the solute undergoes trimerization. The ratio of observed lowering of freezing points in two cases is ( 1:(?) ) |
12 |

1222 | Q. 32 Which of the following binary mixtures will have same composition in liquid and vapour phase? (a) Benzene-toluene (b) Water-nitric acid (c) Water-ethanol (d) n-hexane-n-heptane |
12 |

1223 | Vapour pressure of pure benzene at any temperature is 640 mm ( H g . ) A non volatile, non-electrolyte solid whose weight is ( 2.75 g m, ) is added to ( 39.0 g m ) of benzene. Vapour pressure of solution is 600 mm ( H g ). Calculate the molecular weight of the solid? |
12 |

1224 | Illustration 2.177 100 mL of 1.0 g sample of a drug having compound C,H,O,N as drug is coated with sugar lactose (mol. wt. 342) exerts the osmotic pressure of 0.70 atm at 27°C. What is the drug percentage in sample? |
12 |

1225 | If a mixture of ( O_{2} ) and ( O_{3} ) is having ( V_{r m s}=12.92 m / s ) at ( 300 K . ) Calculate mole percentage of ( O_{2} ) in the mixture. A. 35 % B. 20% c. ( 66.67 % ) % D. none of these |
12 |

1226 | Mustration 2.58 Define an ideal solution. |
12 |

1227 | 117 grams of ( N a C l ) are dissolved in water to make ( 500 m L ) of solution. Water is then added to this solution to make a total of one liter of solution. The final molarity of the solution is : ( A cdot 4 M ) в. 2 М ( c cdot 1 M ) D. ( 0.5 ~ M ) E . 0.585 М |
12 |

1228 | The vapour pressure of an aqueous solution is found to be 750 torrs at certain temperature ‘T’. If ‘T’ is the temperature at which pure water boils under atmospheric pressure and same solution show elevation in the boiling point ( Delta T_{b}=1.04 K, ) find the atmospheric pressure? ( left[boldsymbol{K}_{boldsymbol{b}}=mathbf{0 . 5 2} boldsymbol{K} boldsymbol{k g m o l}-mathbf{1}right] ) A . 77 в. 779 ( c .782 ) D. 746 |
12 |

1229 | ( 4.6 mathrm{cm}^{3} ) of methyl alcohol is dissolved in ( 25.2 mathrm{g} ) of water. Calculate mole fraction of methyl alcohol and water. (Given density of methyl alcohol = ( mathbf{0 . 7 9 5 2 g c m}^{-mathbf{3}} ) and ( boldsymbol{C}=mathbf{1 2}, boldsymbol{H}=mathbf{1}, boldsymbol{O}= ) ( mathbf{1 6}) ) |
12 |

1230 | Assuming ideal behaviour, the enthalpy and volume of mixing of two liquids, respectively, are: A. zero and zero B. +ve and zero c. -ve and zero D. -ve and -ve |
12 |

1231 | The relative decrease in VP of an aqueous glucose dilute solution is found to be 0.018. Hence, the elevation in boiling point is (it is given 1 molal aqueous urea solution boils at 100.54°C at 1 atm pressure) a. 0.018° b. 0.18° c.0.54° d. 0.030 |
12 |

1232 | Illustration 2.205 A 0.1 M solution of potassium sulphate K,SO, is dissolved to the extent of 80%. What would be its osmotic pressure at 27°C? |
12 |

1233 | What is the density of wet air with ( 75 % ) relative humidity at 1 atm and ( 300 mathrm{K} ) ? Given : vapour pressure of ( H_{2} O ) is 30 torr and average molar mass of air is ( 29 g / m o l ) A. ( 1.614 g / L ) в. ( 0.96 g / L ) c. ( 1.06 g / L ) D. ( 1.164 g / L ) |
12 |

1234 | Example 2.25 If the radiator of an automobile contains 12 L of water, how much would the freezing point be lowered by the addition of 5 kg of prestone (glycol C,H,OH)2). How many kg of Zeron (methyl alcohol) would be required to produce the same result? |
12 |

1235 | The degree of dissociation of ( boldsymbol{C a}left(boldsymbol{N} boldsymbol{O}_{3}right)_{2} ) in a dilute aqueous solution containing 7 g of salt per 100 g of water at ( 100^{circ} mathrm{C} ) is ( 75 % ). The vapour pressure of solution in ( mathrm{mm} ) is ( x, ) then find the value of ( x / 150 ) to the nearest integer. |
12 |

1236 | If ‘ ( alpha ) ‘ is degree of dimerisation of ( C H_{3} C O O H ) in benzene, then van’t Hoff factor ‘i’ for circulation of colligative properties is: ( mathbf{A} cdot 1+alpha ) B ( cdot 1-frac{alpha}{2} ) ( c cdot 1+frac{alpha}{2} ) D. ( 1+2 alpha ) |
12 |

1237 | Which one of the following mixture is non-ideal solution? A. Chloroform and acetone B. Benzene and toulene c. Chlorobenzene and bromobenzene D. Bromoethane and chloroethane |
12 |

1238 | 7. A solution of common salt is prepared and freezed by Raj. (a) It occurs by evolution of heat (b) Freezing point of solvent is higher than solution. (C) No heat change occurs in this process (d) Kinetic energy of Liquid molecule increases. |
12 |

1239 | 10 g of cane sugar (molecular mass = 342) in ( 1 times 10^{-3} m^{3} ) of solution produces an osmotic pressure of ( 6.68 times 10^{4} N m^{-2} ) at ( 273 mathrm{K} . ) Calculate the value of ( mathrm{R} ) in SI units. A. ( 8.3684 J K^{-1} mathrm{mol}^{-1} ) B . ( 9.3684 J K^{-1} ) mol ( ^{-1} ) c. ( 7.3684 J K^{-1} ) mol ( ^{-1} ) D. ( 5.3684 J K^{-1} ) mol ( ^{-1} ) |
12 |

1240 | What type of deviation is shown by a mixture of ethanol and acetone? What type of azeotrope is formed by mixing ethanol and acetone? |
12 |

1241 | How much AgBr could dissolve in 1.0L of ( 0.40 mathrm{M} N H_{3} ? ) Assume that ( A gleft(N H_{3}right)_{2}^{-} ) is the only complex formed. ( left[boldsymbol{K}_{f}left(boldsymbol{A} boldsymbol{g}left(boldsymbol{N} boldsymbol{H}_{3}right)_{2}^{+}right)=mathbf{1} times mathbf{1 0}^{8}right. ) ( left.boldsymbol{K}_{s p}(boldsymbol{A} boldsymbol{g} boldsymbol{B r})=mathbf{5} times mathbf{1 0}^{-mathbf{1 3}}right] ) ( [sqrt{mathbf{5 0}}=mathbf{7}] ) |
12 |

1242 | ( 0.1 M ) solution of urea would be with ( 0.1 ~ M ) solution of ( N a C l ) A. hypotonic B. hypertonic c. isotonic D. none of these |
12 |

1243 | Assuming the formation of an ideal solution, the boiling point of a mixture containing 1560 g benzene (molar mass =78) and 1125 g chlorobenzene (molar” mass ( =112.5)^{prime} ) using the given vapour pressure vs. temperature diagram against anexternal pressure of 1000 torr, is : ( mathbf{A} cdot 90^{circ} C ) B. ( 100^{circ} mathrm{C} ) ( mathbf{c} cdot 110^{circ} C ) D. ( 120^{circ} mathrm{C} ) |
12 |

1244 | How many grams of concentrated sulphuric acid ( (80 % w / w) ) should be used to prepare ( 100 m L ) of one molar ( boldsymbol{H}_{2} boldsymbol{S} boldsymbol{O}_{4} ? ) A . ( 10 g ) в. 12.25 g c. ( 15 g ) D. ( 17.5 g ) |
12 |

1245 | Equal volumes of ( 0.1 M A g N O_{3} ) and ( 0.2 M N a C l ) are mixed. The concentration of ( N O_{3}^{-} ) ion in the mixture will be: A . ( 0.1 M ) B. ( 0.05 M ) c. ( 0.2 M ) D. 0.15 М |
12 |

1246 | g of a substance when dissolved in Illustration 2.30 4.375 g of a substance when diss 36.0 g of water, lowered its vapour pressure by 0.5 mm a a given temperature. The vapour pressure of wat temperature is 25.0 mm. Calculate the molecular weight 01 solute. |
12 |

1247 | To from a super saturated solution of salt one must: A. cool slowly B. cool rapidly c. add some salt to cold solution D. use a clear vesse |
12 |

1248 | The molecular weight of benzoic acid in benzene as determined by depression in the freezing point method corresponds to: A. ionization of benzoic acid B. dimerization of benzoic acid c. trimerization of benzoic acid D. solvation of benzoic acid |
12 |

1249 | Equal volumes of M/20 urea solution and M/20 glucose solution are mixed. The mixture will have osmotic pressure: A. equal to either of the solution B. less than either of the solution c. higher than either of the solution D. zero |
12 |

1250 | When acetone and chloroform are mixed together, which of the following observations is correct? ( (mathbf{A}) ) A. A-A and B-B interactions are stronger than A-B interactions B. A-A and B-B interactions are weaker than A-B interactions C. A-A and B-B interactions are equal D. The liquid form separate layers and are immiscible |
12 |

1251 | Valli took some common salt, naphthalene balls, camphor, baking soda and washing soda. She attempted to dissolve these substances either in water or in acetone. Complete the table with the expected results. |
12 |

1252 | ( 5 mathrm{g} ) of a polymer of molar mass ( 50 k g m o l^{-1} ) is dissolved in ( 1 d m^{3} ) solution. The height of solution ( (m m) ) that will represent its osmotic pressure if density of solution at equilibrium is ( 0.96 mathrm{kg} mathrm{dm}^{-3} ) is (divide answer by 5 and write nearest integer value). |
12 |

1253 | Which is the descriptive term that indicates there is a large quantity of solute, compared with the amount of solvent, in a solution? A . Dilute B. concentrated c. Unsaturated D. Saturated E. Supersaturated |
12 |

1254 | The correct statement among the following is: A. smoke is carbon dispersed in air B. butter is water dispersed in fat C . greater is the valency of ion more will be its coagulating power D. more is the gold number of a lyophobic sot, more is protecting power |
12 |

1255 | Explain the following giving example Saturated solution, Pure substance, colliod. |
12 |

1256 | For which of the following solutes the van’t Hoff factor is not greater than one? A. ( N a N O_{3} ) в. ( B a C l_{2} ) ( mathbf{c} cdot_{K_{4}}left[F e(C N)_{6}right] ) D. ( N H_{2} C O N H_{2} ) |
12 |

1257 | Illustration 2.149 Why is great care taken in intravenous injections to have comparable concentration of solutions to be injected to that of blood plasma? |
12 |

1258 | The mole fraction of water in a sulphuric acid solution is 0.85 Calculate the molality of the solution: |
12 |

1259 | The vapour prerssure of pure liquids ( A ) and B are 400 and ( 600 m m H g ) respectively at ( 298 K . ) On mixing the two liquids, the sum of their initial volumes is equal to the volume of the final mixture. The mole fraction of liquids B is 0.5 in the mixture. The vapour pressure of the final solution,the mole fraction of components ( A ) and ( B ) in vapour phase, respectively are: A. ( 500 mathrm{mmHg}, 0.5,0.5 ) в. 450 ттН ( g, 0.4,0.6 ) c. 450 mmHg ( , 0.5,0.5 ) D. ( 500 mathrm{mmHg}, 0.4,0.6 ) |
12 |

1260 | State True or False. Mixture of ( H N O_{3} ) and ( H C l ) is an example of maximum boiling point azeotrope A. True B. False |
12 |

1261 | Illustration 2.130 In a cold climate water gets frozen causing damages to the radiator of a car. Ethylene glycol is used as an antifreezing agent. Calculate the amount of ethylene glycol the added to 2 kg of water to prevent it from freezing at -8°C. (K, for water = 1.8 K m-!) |
12 |

1262 | Washing soda ( left(N a_{2} C O_{3} .10 H_{2} Oright) ) is widely used in softening of hard water. If 1 L of hard water requires 0.0286 g of washing soda, the hardness of ( C a C O_{3} ) in ppm is : A . 10 B. 5 c. 8 D. 6 |
12 |

1263 | The mole fraction of solute in ( 10 % ) (w/w) aqueous NaOH solution is: A . 0.1 B. 0.05 c. 0.0476 D. 0.075 |
12 |

1264 | The van’t Hoff factor indicates the number of solute particles produced per formula unit that dissolves. If true enter 1 , if false enter 0 . |
12 |

1265 | ( 4.6 mathrm{cm}^{3} ) of methyl alcohol is dissolved in ( 25.2 mathrm{g} ) of water. Calculate mole fraction of methyl alcohol. A. 0.1232 B. 0.0759 c. 0.0932 D. 0.0562 |
12 |

1266 | 5. Negative deviations from Raoult’s law are exhibited by binary mixtures a. in which the molecules tend to attract each other and hence their escape into the vapour phase is retarded. b. in which the molecules tend to repel each other and hence their escape into the vapour phase is retarded. c. in which the molecules tend to attract each other and hence their escape into the vapour phase is speeded up. d. in which the molecules tend to repel each other and hence their escape into the vapour phase is speeded up. |
12 |

1267 | One millimole ( O_{2} ) gas is dissolved in ( mathbf{5 4 0 0} mathrm{ml} ) water at ( 25^{circ} mathrm{C} ). Calculate the Henry’s law constant ( boldsymbol{K}_{boldsymbol{H}} ) for this solution. ( p_{O_{2}}=2 times 10^{-8} ) bar. |
12 |

1268 | When mango is placed in dilute aqueous solution of hydrochloric acid, it A. shrinks B. swells c. bursts D. nothing happens |
12 |

1269 | Justify the following statements with an explanation: ¡) Solubility of calcium oxide decreases with increase in temperature. ii) What happens to the solubility in exothermic process with regard to temperature? iii) In endothermic process, solubility increases with increase in temperature. iv) At a given temperature, increase in pressure increases the solubility of the gas |
12 |

1270 | Which of the following substance(s) dissolves in water? This question has multiple correct options A. Vinegar B. Groundnut Oi c. Lemon Juice D. Kerosene |
12 |

1271 | If in solvent, n simple molecules of solute combine to form an associated molecule, ( x ) is degree of association the Van’t Hoff’s factor ( ^{prime} boldsymbol{i}^{prime} ) is equal to: A ( cdot frac{1}{1-n x} ) в. ( frac{1-x+n x}{1} ) c. ( frac{1-x+frac{x}{n}}{1} ) D. ( frac{x}{frac{n}{1}-1+x} ) |
12 |

1272 | Example 2.13. A mixture which contains 0.550 g of camphor and 0.090 g of an organic solute melts at 161°C. The solute contains 93.75% C and 6.25% H by weight. What is the molecular formula of compound? K, for camphor is 37.5°C mol-1 kg. The melting point of camphor is 209°C. |
12 |

1273 | ( 100 mathrm{ml} ) of liquid ( mathrm{A} ) and ( 50 mathrm{ml} ) of liquid ( mathrm{B} ) are mixed to form ( 138 mathrm{ml} ) of solution. It is : A. Ideal solution B. High boiling azeotrope c. Low boiling azeotrope D. None of these |
12 |

1274 | What will be the value of Van’t Hoff factor for ethanoic acid in benzene? |
12 |

1275 | An aqueous solution of a salt ( M X_{2} ) at certain temperature has a van’t Hoff factor of ( 2 . ) The degree of dissociation for this solution of the salt is: A . 0.50 B. 0.33 c. 0.67 D. 0.80 |
12 |

1276 | What are the materials which contain at least two pure substances and show the properties of their constituents called? A. A compound B. An element c. A mixture D. A solution |
12 |

1277 | A solution is ( 25 % ) water, ( 25 % ) ethanol and ( 50 % ) acetic acid by mass. Calculate the mole fraction of each component. |
12 |

1278 | Identify the solute ( & ) the solvent in the following solutions: (a) Sugar solution (b) Air (c) Grains (d) Aerated drinks. |
12 |

1279 | Illustration 2.80 Consider the following vapour pressure composition graph. SP is equal to: a. PQ + RS b. PQ + QR c. SR + SQ d. PQ + QR + RS Total vapour pressure P — PB ok APB P 0 X – S 1 |
12 |

1280 | Match the items of Column-I with its proportional term in the items of Column-II: Column-I (a) Kinetic energy (p) Mole fraction (b) Partial pressure of a (q) Density gas (c) Rate of diffusion (r) Molar mass (d) Vapour pressure of a (s) Absolute liquid ( quad ) temperature |
12 |

1281 | The simplest way to describe the concentration of solution is : I) mass by mass Il) mass by volume III) volume by pressure A . ।, ॥ в. ॥, III ( c cdot ) ।, ॥ D. I, II, III |
12 |

1282 | What will be the value of van’t Hoff factor (i) of benzoic acid if it demerises in aqueous solution? How will the experimental molecular weight vary as compared to the normal molecular weight? |
12 |

1283 | • 29 Relative lowering of vapour pressure is a colligative property pour pressure is a colligative property because (a) it depends on the concentration of a non-electrolyte solute in solution and does not depend on the nature of the solute molecules (b) it depends on number of particles of electrolyte solute in solution and does not depend on the nature of the solute particles (c) it depends on the concentration of a non-electrolyte solute in solution as well as on the nature of the solute molecules (d) it depends on the concentration of an electrolyte or non-electrolyte solute in solution as well as on the nature of solute molecules ( ahl |
12 |

1284 | The molal elevation constant is the ratio of the elevation in boiling point to: A. molarity B. molality c. mole fraction of solute D. mole fraction of solvent |
12 |

1285 | The solubility of a solid solute in a liquid solvent increases with increase in temperature A. True B. False |
12 |

1286 | Which pair(s) of liquids on mixing is/are expected to show no net volume change and no heat effect? This question has multiple correct options A. Acetone and ethanol. B. Chlorobenzene and bromobenzene c. chloroform and benzene D. n-Butyl chloride and n-butyl bromide |
12 |

1287 | Q. 7 What will be the molality of the solution containing 18.25 g of HCL gas in 500 g of water? (a) 0.1 m (b) 1 M (c) 0.5 m (d) 1 m |
12 |

1288 | The weight in grams of a non-volatile solute ( (M . w t: 60) ) to be dissolved in ( 90 g ) of water to produce a relative lowering of the vapour pressure of 0.02 is: A . 4 B. 8 ( c .6 ) D. 10 |
12 |

1289 | A ( 6.90 M ) KOH solution in water has ( 30 % ) by weight of ( K O H . ) The density of KOH solution is: A. ( 1.288 g / m L ) в. ( 12.88 g / m L ) c. ( 0.1288 g / m L ) D. none of these |
12 |

1290 | The solubility of gases in water with rise in temperature A . increases B. decreases c. no change D. None of the above |
12 |

1291 | The vapour pressure of ( 2.1 % ) of an aqueous solution of a non-electrolyte at ( 373 K ) is ( 755 mathrm{mm} ). Calculate the molar mass of solution ( left(M_{2}right) ) A . ( 46.1 mathrm{gm} / mathrm{mol} ) le B. ( 57.456 mathrm{gm} / mathrm{mole} ) c. ( 10 mathrm{gm} / mathrm{mole} ) D. ( 87.12 mathrm{gm} / mathrm{mole} ) |
12 |

1292 | ‘The extent to which a solute is dissociated or associated can be expressed by Van ‘t Hoff factor’. Substantiate the statement. |
12 |

1293 | Vant Hoff factor for a dilute solution of glucose is: A . 0 B. c. 1.5 ( D ) |
12 |

1294 | The vapour pressure of a solution containing 2 g of an electrolyte BA in 100 g water which dissociates in one ( B^{+} ) and one ( A^{-} ) ion in water is ( 751 mathrm{mm} ) at ( 100^{circ} mathrm{C} . ) Percentage degree of ionisation of BA if its molar mass is 56 g ( m o l^{-1} ) (write answer after dividing degree of dissociation by 80 to the nearest integer) is |
12 |

1295 | What will be density ( left(operatorname{in} g m L^{-1}right) ) of 3.60 molar sulphuric acid having ( 29 % ) by mass? ( left(text {Molar mass}=mathbf{9 8 g m L}^{-1}right) ) A . 1.88 B. 1.22 ( c cdot 1.45 ) D. 1.64 |
12 |

1296 | Illustration 2.145 State how does osmotic pressure vary with temperature? |
12 |

1297 | Q Type your question- thermodynamic properties during the formation of 1 mol of an ideal binary solution. ( A ) ( (mathbf{A}) ) B. ( (mathbf{A}) ) ( c ) ( (mathbf{A}) ) ( D ) (A) |
12 |

1298 | I. Agitation and stirring will increase the rate at which salt dissolves in water ( I I . ) Increased movement of water molecules allow sodium ions and chloride ions to be pulled apart as shells of hydration are formed. A. Statement I is true, Statement ( I I ) is true and is a correct explanation of the phenomena described in ( I ) B. Statement I is true, Statement II is false c. statement ( I ) is false, statement ( I I ) is true D. Statement I is false, Statement II is false |
12 |

1299 | A solution contains 2.80 moles of acetone ( left(C H_{3} C O C H_{3}right) ) and 8.20 moles of ( C H C l_{3} ). Calculate the mole fraction of acetone.(give answer in ( 110 X) ) |
12 |

1300 | 0.21 On the basis of information given below mark the correct option. Information (i) In bromoethane and chloroethane mixture intermolecular interactions of A-A and B-B type are nearly same as A-B type interactions. (ii) In ethanol and acetone mixture –A or B-B type intermolecular interactions are stronger than A-B type interactions. (iii) In chloroform and acetone mixture A-A or B-B type intermolecular interactions are weaker than A-B type interactions. (a) Solution (ii) and (iii) will follow Raoult’s law (b) Solution (i) will follow Raoult’s law (c) Solution (ii) will show negative deviation from Raoult’s law (d) Solution (iii) will show positive deviation from Raoult’s law |
12 |

1301 | 1 kg of water under a nitrogen pressure of 1 atmosphere dissolves 0.02 gm of nitrogen at ( 293 mathrm{K} ) Calculate Henry’s law constant. A ( cdot 7.2 times 10^{-4} ) atm B . ( 7.5 times 10^{4} ) atm ( c cdot 7.4 times 10^{4} operatorname{atm} ) D. ( 7.2 times 10^{4} ) atm |
12 |

1302 | The freezing point of one molal ( N a C l ) solution assuming ( N a C l ) to be ( 100 % ) dissociated in water is: [Molal depression constant is ( 1.86] ) A ( .-2.72^{2} C ) В. ( -3.72^{2} C ) c. ( 2.72^{2} C ) D. ( 3.72^{2} C ) |
12 |

1303 | Illustration 2.158 Two solutions of glucose have osmotic pressure 1.5 and 2.5 atm, respectively. 1 L of first solution is mixed with 2 L of second solution. The osmotic pressure of the resultant solution will be |
12 |

1304 | How many grams of ( N a O H ) should be added to water to prepare ( 250 mathrm{ml} ) solution of 2 M NaOH ? A ( cdot 9.6 times 10^{3} ) В. ( 2.4 times 10^{3} ) c. 20 D . 24 |
12 |

1305 | Question 12. Calculate the osmotic pressure in pascals exerted by a solution prepared by dissolving 10 g of polymer of molar mass 185000 in 450 mL of water at 37° C. Use the formula for osmotic pressure (T) = CRT, and C and na MB |
12 |

1306 | ( mathbf{A} ) ( 3 mathrm{M} ) 3L solution of NaOH is mixed with another ( 3 mathrm{M} ) 5L solution of ( mathrm{NaOH} ). How much should the mixture be diluted so that the final molarity of the solution becomes 1M? |
12 |

1307 | The value of Henry’s constant ( boldsymbol{K}_{boldsymbol{H}} ) is : A. greater for gases with higher solubility B. greater for gases with lower solubility c. constant for all gases D. not related to the solubility of gases |
12 |

1308 | The osmotic pressure at ( 293 mathrm{K} ) ( A cdot 2 ) B. 3 ( c cdot 4 ) D. 4.805 |
12 |

1309 | A solution containing 10 g per ( mathrm{dm}^{3} ) of urea (m.w. = 60) is isotonic with a 5% solution of a non-volatile solute. The molecular mass of this non-volatile solute is: A . ( 250 mathrm{g} mathrm{mol}^{-1} ) B . 300 g mol- c. ( 350 mathrm{g} ) mol ( ^{-1} ) D. ( 200 mathrm{g} mathrm{mol}^{-1} ) |
12 |

1310 | us solution is Example 2.26 If the boiling point of an aqueous solutie 100.1°C, what is its freezing point? Givenly = 80,1, = 540 cal g’ respectively, of H20. |
12 |

1311 | The answer to this question is a single digit integer, ranging from 0 to 9 The van’t Hoff factor for aqueous solution of ( C u S O_{4} cdot 5 H_{2} O ) will be |
12 |

1312 | Which of the liquids in each of the following pairs has a higher vapour pressure? A. Alcohol, glycerine B. Mercury, water c. petrol, kerosene D. None of these |
12 |

1313 | Example 2.5 Liquids A and B form an ideal mixture, in which the mole fraction of A is 0.25. At temperature T, a small quantity of the vapour in equilibrium with the liquid is collected and condensed. This process is repeated for a second time with the first condensate. The second condensate now contains 0.645 mole fraction of A. Calculate the ratio ( P P ). What will be the mole fraction of B in the third condensate? |
12 |

1314 | The molecular weight of an organic compound is 58.0 g/mol. Compute the boiling point of a solution containing ( 24.0 mathrm{g} ) of the solute and ( 600 mathrm{g} ) of water when the barometric pressure is such that pure water boils at ( 99.725^{circ} mathrm{C} .left(K_{6} text { forwater } 0.513^{circ} mathrm{C} / mathrm{m}right) ) ( mathbf{A} cdot 50^{circ} C ) B . ( 100.08^{circ} mathrm{C} ) ( c cdot 150.1^{circ} C ) D. ( 180.34^{circ} mathrm{C} ) |
12 |

1315 | is soluble in water, ethanol and methanol. A . ( N a O H ) в. ( N a H ) ( c . N a O ) D. None of these |
12 |

1316 | 6. Mole fraction of component A in vapour phase is X1 and mole fraction of component A in liquid mixture is X2(PA°= vapour pressure of pure A), then the total vapour pressure of the liquid mixture is 2 PAX2 h. PAXI s. PBRI d. PB 22 Xi X2 22 |
12 |

1317 | Blood is isotonic with. A. ( 0.16 M ) NaCl ( l ) B. Conc.NaCl c . ( 30 % ) NaCl ( l ) D. ( 50 % ) NaCl |
12 |

1318 | What is the number of mole of benzene ( left(P_{B}^{0}=150 text { torrs }right) ) per mole of toluene ( left(P_{T}^{0}=50 text { tor } r sright) ) in vapour phase if the given solution has a vapour pressure of 120 torrs in equilibrium with its vapour? ( A cdot 7 ) B. 8 c. 9 D. 10 |
12 |

1319 | What would be the freezing point of a solution that has 684 grams of sucrose ( (1 mathrm{mol}=342 mathrm{g}) ) dissolved in 2,000 grams of water (1 mole= 18 grams)? B. ( -0.93^{circ} mathrm{C} ) or ( 272.07 mathrm{K} ) ( mathbf{c} .-1.39^{circ} mathrm{C} ) or ( 271.61 mathrm{K} ) D. ( -2.48^{circ} mathrm{C} ) or ( 270.52 mathrm{K} ) E. ( -3.72^{circ} mathrm{C} ) or ( 269.28 mathrm{S} ) |
12 |

1320 | Identify the solute ( & ) the solvent in the following solution: a) sugar solution b) Air c) Rain water d) Aerated drinks |
12 |

1321 | Question 28cm Casa, the remaining of emotion de em Question 28. Calculate the mass percentage of aspirin (C9Hg04) in acetonitrile (CH3CN) when 6.5 g of C,H,O, is dissolved in 450 g of CH3CN. Mass of solute We know that mass %= 2 x 100 Mass of solution and mass of solution = mass of solute + mass of solvent. So, calculate mass of solution and then mass percentage. |
12 |

1322 | Acetic acid undergoes dimerisation, when dissolved in benzene (as shown in figure) Molecular mass of acetic acid is found to be 120 . Which among the following relation is correct? |
12 |

1323 | A sample of water has a hardness expressed as 77.5 ppm ( C a^{2+} . ) This sample is passed through an ion exchange column and ( C a^{2+} ) is replaced by ( boldsymbol{H}^{+} . ) Select correct statement(s). This question has multiple correct options A. pH of the water after it has been so treated is 2.4 B. Every ( C a^{2+} ) ion is replaced by one ( H^{+} ) ion. C . Every ( C a^{2+} ) ion is replaced by two ( H^{+} ) ions. D. pH of the solution remains unchanged. |
12 |

1324 | The exact mathematical expression of Raoult’s law is: ( ^{text {A }} cdot frac{P_{0}-P_{s}}{P_{0}}=frac{n}{N} ) в. ( frac{P_{0}-P_{s}}{P_{0}}=frac{N}{n} ) c. ( frac{P_{0}-P_{s}}{P_{s}}=frac{n}{N} ) D. ( frac{P_{0}-P_{s}}{P_{0}}=n times N ) |
12 |

1325 | If the observed and theoretical molecular mass of NaCl is found to be 31.80 and ( 58.50, ) then the degree of dissociation of NaCl is: A . 83.96% B . 8.39% c. ( 90 % ) D. 100% |
12 |

1326 | Define solubility and write the factors which influence the solubility. | 12 |

1327 | State True or False. Elevation in boiling point is directly proportional to the molality of the solution. A. True B. False |
12 |

1328 | A solution is prepared by dissolving ( 11 g ) glucose in ( 250 c m^{3} ) water at ( 30^{circ} C ) what is mass percent glucose in solution. The density of water at ( 30^{circ} ) is ( mathbf{0 . 9 9 6} boldsymbol{g} / boldsymbol{c m}^{mathbf{3}} ) |
12 |

1329 | ( p H ) of a dilute solution of ( H C l ) is 6.95 Calculate molarity of ( H C l ) solution. ( left[begin{array}{c}10^{-6.95}=11.22 times 10^{-8} \ 10^{-7.05}=8.90 times 10^{-8}end{array}right] ) |
12 |

1330 | A solution contain ( 36 % ) water and ( 64 % ) acetaldehyde ( left(C H_{2} C H Oright) ) by mass. The mole fraction of acetaldehyde is: A . 0.42 B. 0.2 c. 4.2 D. 2.1 |
12 |

1331 | A sample of air is saturated with benzene (vapour pressure =100 mm Hg at ( 298 mathrm{K} ) ) at ( 298 mathrm{K}, 750 mathrm{mm} ) Hg pressure. If it is isothermally compressed to one third of its initial volume, the final pressure of the system is: A. 2250 torr B . 2150 torr c. 2050 torr D. 1950 torr |
12 |

1332 | The normality of ( 10 % ) ( weight / volume) acetic acid is: ( A cdot 1 N ) B. 10 N c. ( 1.67 mathrm{N} ) D. 0.83 |
12 |

1333 | Pure water boils at ( 99.725^{circ} C ) at shimla. If ( K_{b} ) for water is ( 0.51 K m o l^{-1} k g, ) the boiling point of 0.69 molal urea solution will be: A . 100.35 B. 100.08 c .99 .37 D. None of these |
12 |

1334 | A solution of sucrose (molar mass ( =342 ) ( left.g m o l^{-1}right) ) has been prepared by dissolving 68.5 g of sucrose in 1000 g of water. The freezing point of the solution obtained will be: ( left[mathrm{K}_{f} text { for water }=1.86 mathrm{K} mathrm{kg} mathrm{mol}^{-1}right] ) A . – ( 0.372 mathrm{c} ) B. 0.520C c. ( +0.372 c ) D. 0.570C |
12 |

1335 | Question 3. Calculate the molarity of each of the following solutions : (a) 30 g of Co(NO3)2.6H 0 in 4.3 L of solution. (b) 30 mL of 0.5 M H2SO, diluted to 500 mL. |
12 |

1336 | 111.1g of the non-volatile solute, urea needs to be dissolved in 100 g of water, in order to decrease the vapour pressure of water by ( 25 % ). The molarity of the solution will be: A. 18.52 м в. 18.92 c. 19.52 м D. None of the above |
12 |

1337 | Hlustration 2.161 The osmotic pressure of a solution at 0°C is 4 atm. What will be its osmotic pressure at 546 K under similar conditions? a. 4 atm b. 9 atm c. 8 atm d. 6 atm |
12 |

1338 | Ferrous sulphate heptahydrate is used to fortify foods with iron. The amount (in grams) of the salt required to achieve 10 ppm of iron in 100 kg of wheat is [Atomic weight ( : mathrm{Fe}=mathbf{5 5 . 8 5} mathrm{S}=mathbf{3 2 . 0 0} mathrm{O} ) ( =mathbf{1 6 . 0 0}] ) |
12 |

1339 | 1 mol benzene ( left(P_{text {benzene }}^{o}=42 mathrm{mm}right) ) and 2 mol toluene ( left(P_{text {toluene}}^{o}=36 mathrm{mm}right) ) will have This question has multiple correct options A. total pressure of 38 mm. B. mole fraction of vapour of benzene above liquid mixture is ( 7 / 19 ) c. positive deviation from Raoult’s law D. negative deviation from Raoult’s law |
12 |

1340 | The freezing point depression constant for water is ( -1.86^{0} mathrm{Cm}^{-1} . ) If ( 5.00 mathrm{g} ) ( N a_{2} S O_{4} ) is dissolved in 45.0 g ( H_{2} O, ) the freezing point is changed by ( 3.82^{0} C ) Calculate the vant Hoff factor for ( N a_{2} S O_{4} ) A . 2.05 B . 2.63 c. 3.11 D. 0.381 |
12 |

1341 | Two liquids ( A ) and ( B ) form an ideal solution. At ( 300 mathrm{K} ), the vapour pressure of a solution containing 1 mole of A and 3 mole of ( mathrm{B} ) is ( 550 mathrm{mm} ) of Hg. At the same temperature, if one more mole of ( mathrm{B} ) is added to this solution, the vapour pressure of the solution increases by 10 ( mathrm{mm} ) of Hg. Determine the vapour pressure of ( A ) and ( B ) in their pure states. |
12 |

1342 | If the density of methanol is ( 0.793 mathrm{kg} L^{-1}, ) what is its volume needed for making 2.5 L of its 0.25 M solution? |
12 |

1343 | A solution of ( N a_{2} S_{2} O_{3} ) is saturated iodometrically against 0.334 g of pure ( K B r O_{3}left(text { converted to } B r^{-}right) ) requiring 40 ( mathrm{ml} . mathrm{Na}_{2} mathrm{S}_{2} mathrm{O}_{3} ) solution. What is the molarity of ( N a S_{2} O_{3} ) solution? (Molar mass of ( boldsymbol{K} boldsymbol{B} boldsymbol{r} boldsymbol{O}_{3}=mathbf{1 6 7} ) g ( boldsymbol{m o l}^{-1} ) ) |
12 |

1344 | If the mass ratio of non-reacting gases ( O_{2} ) and ( N_{2} ) in a vessel is ( 2: 7, ) then the ratio of their molecules will be: A ( cdot 1: 2 ) B. 3:5 c. 2: 7 D. 1: 4 |
12 |

1345 | ( 380 mathrm{mL} ) of a gas at ( 27^{0} mathrm{C}, 800 mathrm{mm} ) of ( mathrm{Hg} ) weight ( 0.455 mathrm{g} . ) the mol.wt.of gas is: A .27 B . 28 c. 29 D. 30 |
12 |

1346 | Illustration 2.174 The osmotic pressure of a solution was found to be 8 atm when 8 mol of a non-volatile solute was dissolved in V L of solution at 300 K. Calculate the volume of solution (R = 0.0821 L-atm K-1 mol-1) |
12 |

1347 | The freezing point of a 0.05 molal solution of non-electrolyte in water is: ( left[boldsymbol{K}_{f}=mathbf{1 . 8 6} boldsymbol{K} boldsymbol{m}^{-1}right] ) ( mathbf{A} cdot-1.86^{circ} mathrm{C} ) B. ( -0.93^{circ} mathrm{C} ) с. ( -0.093^{circ} mathrm{C} ) и. ( -0.093^{circ} ). D. ( 0.093^{circ} mathrm{C} ) |
12 |

1348 | Illustration 2.140 The melting point of phenol is 40°C. A solution containing 0.172 g acetanilide (C,H,OH) in 12.54 g phenol freezes at 39.25°C. Calculate the freezing point constant and the latent heat of fusion of phenol. |
12 |

1349 | In a solvent ( 50 % ) of benzoic acid dimerises while rest ionises, determines molar mass of acid which is observed and also its van’t Hoff factor. |
12 |

1350 | h expressions given in Column II. Q.49 Match the laws given in Column I with expressions giv Column Column Il A Raoult’s law 1. AT, = Km B. Henry’s law 2. T = CRT C. Elevation of boiling point 3 p=xp; + X, D. Depression in freezing point 4. AT, E. Osmotic pressure 15. DEK, X |
12 |

1351 | The vapour pressure of pure water at ( 25^{circ} mathrm{C} ) is 23.76 torr. The vapour pressure of a solution containing 5.40 g of a nonvolatile substance in 90.0 g water is 23.32 torr. The molecular weight of the solute is: A. ( 97.24 mathrm{g} / mathrm{mol} ) B. 24.29 g/mol c. ( 50.44 mathrm{g} / mathrm{mol} ) D. ( 57.24 mathrm{g} / mathrm{mol} ) |
12 |

1352 | The unit of ebullioscopic constant is? A . ( K ) kg mol ( ^{-1} ) or ( K(text { molality })^{-1} ) B . mol kg ( K^{-1} ) or ( K^{-1} ) (molality) c. ( k g ) mol ( ^{-1} K^{-1} ) or ( K^{-1} ) (molality) ( ^{-1} ) D. ( K ) mol ( k g^{-1} ) or ( K(text { molality }) ) |
12 |

1353 | ( 6.02 times 10^{20} ) molecules of urea are present in ( 100 mathrm{mL} ) of its solution. The molarity of urea solution is : A . ( 0 . ) B. 0.01 c. 0.02 D. 0.001 |
12 |

1354 | A solution of benzene and toluene is an example of solution. A. Ideal B. non ideal c. azeotrope D. none |
12 |

1355 | Define the term : isotonic solution | 12 |

1356 | 0.40 What is the significance of Henry’s law constant Kh? Ans According to Henry’s law n |
12 |

1357 | The vapour pressure of o-nitrophenol at any given temperature is predicted to be: A. Higher than that of p-nitrophenol B. Lower than that of p-nitropheno c. Same as that of p-nitrophenol D. Higher or lower depending upon the size of the vesse |
12 |

1358 | Define azeotropes.What type of azeotrope is formed by a positive deviation from Raoult’s law? Give an example |
12 |

1359 | ( mathbf{0 . 1} boldsymbol{M} boldsymbol{K}_{4}left[boldsymbol{F} e(boldsymbol{C} boldsymbol{N})_{6}right] ) is ( 60 % ) ionized What will be its Van’t Hoff factor? A . 1.4 в. 3.4 c. 2.4 D. 4. |
12 |

1360 | Benzoic acid undergoes dimerization in benzene solution. The Van’t Hoff factor ( i ) is related to the degree of assoication ( alpha ) of the acid as : B. ( i=1+(alpha / 3) ) c. ( i=1-(alpha / 2) ) D. ( i=1+(alpha / 2) ) |
12 |

1361 | An aqueous solution freezes at ( 272.4 K ) while pure water freezes at ( 273.0 K ) while pure water freezes at ( 273.0 K ) Determine (a) the molality of the solution (ii) boiling point of the solution (iii) lowering of vapour pressure of water at ( 298 K ) (Given, ( boldsymbol{K}_{boldsymbol{f}}=mathbf{1 . 8 6 K} boldsymbol{k g} boldsymbol{m o l}^{-1}, boldsymbol{K}_{boldsymbol{b}}= ) ( 0.512 K k g ) mol( ^{-1} ) and vapour pressure of water at ( 298 K=22.756) ) |
12 |

1362 | A mixture from which some of the solute particles will settle on standing: A. Miscible B. Suspension c. colloid D. Saturated E. Supersaturated |
12 |

1363 | Hustration 2.163 300 cm? of an aqueous solution contains 1.26 g a polymer. The osmotic pressure of such solution at 300 K is found to be 1.26 x 10-3 bar. Calculate the molar mass of the polymer. |
12 |

1364 | The vapour pressure of water at room temperature is ( 23.8 mathrm{mm} ) Hg. The vapour pressure of an aqueous solution of sucrose with mole fraction 0.1 is equal to: ( mathbf{A} cdot 23.9 mathrm{mm} mathrm{Hg} ) B. ( 24.2 mathrm{mm} ) Hg c. ( 21.42 mathrm{mm} ) Hg D. ( 31.44 mathrm{mm} ) нв |
12 |

1365 | Determine the osmotic pressure of a solution a solution prepared by dissolving ( 2.5 times 10^{-2} g ) of ( K_{2} S O_{4} ) in ( 2 L ) of water at ( 25^{0} C ), assuming that it is completely dissociated ( left(R=0.0821 L text { at } m K^{-1} m o l^{-1}, ) Molar right. mass of ( K_{2} S O_{4}=174 g m o l^{-1} ) |
12 |

1366 | One mole of non volatile solute is dissolved in two moles of water. The vapour pressure of the solution relative to that of water is: A ( cdot frac{2}{3} ) в. ( frac{1}{3} ) ( c cdot frac{1}{2} ) D. ( frac{3}{1} ) |
12 |

1367 | Which one of the following statements is false? A. Raoult’s law states that the vapour pressure of a component over a solution is proportional to its mole fraction B. The osmotic pressure ( ( pi ) ) of a solution is given by the equation ( pi=M R T ), where, ( M ) is the molarity of the solution C. The correct order of osmotic pressure for ( 0.01 mathrm{M} ) aqueous solution of each compound is ( B a C l_{2}> ) ( K C l>C H_{3} C O O H> )sucrose D. Two sucrose solutions of same molality prepared in different solvents will have the same freezing point depression |
12 |

1368 | The vapour pressure of water depends upon: A. surface area of container B. volume of container c. temperature D. all of the above |
12 |

1369 | Question 8. The vapour pressure of pure liquids A and B are 450 and 700 mm Hg respectively, at 350 K. Find out the composition of the liquid mixture if total vapour pressure is 600 mm Hg. Also find the composition of the vapour phase. Apply Raoult’s law Pa = PÅ XA + P8XB = PÅ XA+ P8 (1 – Xa) to calculate mole fraction of A(XA) and B (XB). In vapour phase, partial pressures are used instead of number of moles. |
12 |

1370 | Illustration 2.154 Why a person suffering from high blood pressure is advised to take minimum quantity of common salt? |
12 |

1371 | Which has the highest freezing point? A ( cdot operatorname{lm} K_{4}left[F e(C N)_{6}right] quad ) solution B. ( 1 m C_{6} H_{12} O_{6} ) solution c. ( 1 m K C l ) solution D. ( 1 m ) rock salt solution |
12 |

1372 | For a non-ideal solution exhibiting positive deviation from Raoult’s law, ( Delta_{m i x} H ) has a (nonzero) A. positive B. negative c. zero D. none |
12 |

1373 | Two liquids ( X ) and ( Y ) form an ideal solution at ( 300 K ), the vapour pressure of the solution containing 1 mole of ( X ) and 3 moles of ( Y ) is 550 mm Hg. At the same temperature, if 1 mole of ( Y ) is further added to this solution, the vapour pressure of the solution increases by 10 mm ( H g . ) Vapour pressure (in ( mathrm{mm} ) Hg ) of ( boldsymbol{X} ) and ( boldsymbol{Y} ) in their pure states will be respectively: A . 200 and 300 B. 300 and 400 c. 400 and 600 D. 500 and 600 |
12 |

1374 | In the reaction; ( boldsymbol{A}+mathbf{2} boldsymbol{B} rightarrow mathbf{3} boldsymbol{C}+boldsymbol{D} ) which of the following expression does not describe changes in the concentration of various species as a function of time? A ( cdot{d[C] / d t}=-{3 d[A] / d t} ) B . ( {3 d[D] / d t}={d[C] / d t} ) c. ( {3 d[B] / d t}=-{2 d[C] / d t} ) D . ( {2 d[B] / d t}=-{d[A] / d t} ) |
12 |

1375 | Assertion For rubber and water, ( V(I)<V(s) ) Reason The density of both rubber and water is more in liquid state. A. Both Assertion and Reason are correct and Reason is the correct explanation for Assertion B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion C. Assertion is correct but Reason is incorrect D. Assertion is incorrect but Reason is correct |
12 |

1376 | The vapour pressure of two miscible liquids ( A ) and ( B ) are 300 and 500 mm of Hg respectively. In a flask, 10 moles of ( A ) is mixed with 12 moles of ( B ). However, as soon as ( B ) is added, ( A ) starts polymerizing into a completely insoluble solid. After 100 minutes, 0.525 moles of a non-volatile solute is dissolved which arrests the polymerization completely. The final vapour pressure of the solution is 400 mm of Hg. Assume negligible volume change on mixing, polymerization and ideal behaviour for the final solution. If a number of moles of ( boldsymbol{A} ) polymerized in 100 minutes are expressed as ( x, ) then a value of ( 10 x ) is: ( mathbf{A} cdot mathbf{1} ) B . 2 ( c .3 ) D. 4 |
12 |

1377 | ( 100 mathrm{ml} ) of ( 0.1 mathrm{M} ) solution of a weak acid ( H A ) has molar conductivity ( 5 S c m^{2} m o l^{-1} . ) The osmotic pressure of the resulting solution obtained after dilution of original solution upto 1 litre at ( 500 mathrm{K}, ) assuming ideal solution is: ( left(G i v e n: lambda_{m}^{infty}left(H^{+}right)=right. ) ( 450 S c m^{2} m o l^{-1}, lambda_{m}^{infty}left(A^{-}right)= ) ( mathbf{5 0} boldsymbol{S c m}^{2} boldsymbol{m o l}^{-1}, boldsymbol{R}= ) ( left.0.08 L text { atm } operatorname{mole}^{-1} K^{-1}, sqrt{10}=3.2right) ) A. 0.3128 atm B. 0.4128 atm c. 0.5128 atm D. 0.6128 atm |
12 |

1378 | ( 2.0 mathrm{g} ) of bensoic acid dissolved in ( 25.0 mathrm{g} ) of benzene shows a depression in freezing point to 1.62K. Mollal depression constant ( left(K_{f} ) of bezene is right. 4.9 K.kg. ( m o l^{-1} . ) What is the percentage association of the acid? A. ( (alpha)=90.8 % ) B. ( (alpha)=99.2 % ) c. ( (alpha)=9.8 % ) D. ( (alpha)=49.6 % ) |
12 |

1379 | Which aqueous solution has minimum freezing point? в. 0.005 М ( C_{2} ) Н ( _{5} ) ОН c. 0.005 М ( M g I_{2} ) D. ( 0.005 mathrm{M} mathrm{MgSO}_{4} ) |
12 |

1380 | pH of a ( 0.1 mathrm{M} ) monobasic acid is found to be ( 2 . ) Hence, its osmotic pressure at a given temperature T K is : ( mathbf{A} cdot 0.1 mathrm{RT} ) B. 0.11RT c. ( 1.1 mathrm{RT} ) D. 0.01RT |
12 |

1381 | Which salt shows maximum osmotic pressure in its ( 1 mathrm{m} ) solution. A ( . A g N O_{3} ) в. ( N a_{2} S O_{4} ) ( mathrm{c} cdotleft(N H_{4}right)_{3} P O_{4} ) D. ( M g C l_{2} ) |
12 |

1382 | Question 10. Boiling point of water 750 mm Hg is 99.63°C. How much sucrose is to be added to 500 g of water such that it boils at 100° C. [K, for water is 0.52 K kg mol-‘). |
12 |

1383 | Pure water can be obtain from sea water by: A. Centrifugation B. Plasmolysis c. Reverse osmosis D. Sedimentation |
12 |

1384 | If the vapour pressure of solutions of two liquids are less than those expected from ideal solution they are said to have: A. negative deviation from ideal behaviour B. positive deviations from ideal behaviour c. ideal behaviour D. positive deviation for lower concentration and negative deviations for higher concentration |
12 |

1385 | Which of the following are dilution dependent but temperature independent? This question has multiple correct options A. Formality B. Molality c. Mole fraction D. Molarity |
12 |

1386 | An azeotropic mixture of HCl and water has: A . ( 84 % ) of ( mathrm{HCl} ) в. 22.2% НС। c. 63% of HCI D. 20.2% HCI |
12 |

1387 | Considering the formation, breaking and strength of hydrogen bond, predict which of the following mixtures will show a positive deviation from Raout’s law? A. Methanol and acetone B. Chloroform and acetone c. Nitric acid and water D. Phenol and aniline |
12 |

1388 | Maximum depression in freezing point is caused by: A. potassium chloride B. sodium sulphate c. magnesium sulphate D. magneisum carbonate |
12 |

1389 | A solution that is at equilibrium and contains the maximum amount of solute for a given amount of solvent at constant temperature and pressure. What type of solution is it? A. Miscible B. Suspension c. colloid D. Saturated |
12 |

1390 | ( 4 g ) of hydrogen and ( 128 g ) of hydrogen iodide are present in a 2 litre flask. What are their active masses? | 12 |

1391 | Out of ( 1 M B a C l_{2} ) and ( 1 M A l C l_{3}, ) which one has higher freezing point and why? |
12 |

1392 | 6. What mass of urea be dissolved in 171 g of water so as to decrease the vapour pressure of water by 5%? a. 15 g b. 20 g c. 25 g d. 30 g |
12 |

1393 | Illustration 2.168 200 cm of an aqueous solution of a protein contains 1.26 g of the protein. The osmotic pressure of such a solution at 300 K is found to be 2.57 x 10-3 bar. Calculate the molar mass of the protein. |
12 |

1394 | If molality of ethyl alcohol in aqueous solution is 4.45 then the mole fraction of ethyl alcohol in the solution is |
12 |

1395 | Illustration 2.178 At 10°C, the osmotic pressure of urea solution is 500 mm. The solution is diluted and the temperature is raised to 25°C, when the osmotic pressure is found to be 105.3 mm. Determine the extent of dilution. |
12 |

1396 | Assertion The solubility of a substance changes with temperature. Reason Heat is required to break the bonds holding molecules together so solubility is dependent on temperature.in dissolution, energy, in the form of heat, is required to break the bonds joining the molecules in the solid together. A. Both Assertion and Reason are correct and Reason is the correct explanation for Assertion B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion C. Assertion is correct but Reason is incorrect D. Both Assertion and Reason are incorrect |
12 |

1397 | Generally solubility of gases in liquids is decreases as increasing temperature. Give reason | 12 |

1398 | ( mathbf{0 . 0 0 1} ) molal solution of ( left[boldsymbol{P t}left(boldsymbol{N} boldsymbol{H}_{3}right)_{4} boldsymbol{C l}_{4}right] ) in water had a freezing point depression of ( 0.0054 quad^{o} C . ) If ( K_{f} ) for water is 1.80 the correct formula of the compound is : ( mathbf{A} cdotleft[P tleft(N H_{3}right)_{4} C l_{3}right] C l ) ( ^{mathbf{B}} cdotleft[P tleft(N H_{3}right)_{4} C l_{4}right] ) c. ( left[P tleft(N H_{3}right)_{4} C l_{2}right] C l_{2} ) D. ( left[P tleft(N H_{3}right)_{4} C lright] C l_{3} ) |
12 |

1399 | ( 25.6 mathrm{g} ) of sulphur in 100 g benzene shows depression in freezing point of ( 5.12^{circ} mathrm{C} . K_{f} ) for benzene is ( 5.12^{circ} mathrm{Ckg} ) mol( ^{-1} . ) The molecular formula of sulphur in benzene is: ( A cdot S_{2} ) в. ( S_{6} ) ( mathrm{c} cdot S_{8} ) D. ( S_{12} ) |
12 |

1400 | 2.21 Which of the following terms are unitless? (a) Molality (b) Molarity (c) Mole fraction (d) Mass per cent |
12 |

1401 | Vapour pressure of ( C C l_{4} ) at ( 25^{circ} C ) is 143 mm ( H g ). If ( 0.5 g m ) of non-volatile solute (mol. mass 65 ) is dissolved in ( 100 m l C C l_{4}, ) then the vapour pressure of the solution at ( 25^{circ} mathrm{C} ) is: [Given: density of ( left.C C l_{4}=1.58 g / c m^{3}right] ) ( mathbf{A} cdot 141.93 m m ) B . ( 94.39 mathrm{mm} ) c. ( 199.34 mathrm{mm} ) D. ( 143.99 mathrm{mm} ) |
12 |

1402 | Why do soaps not work in hard water? | 12 |

1403 | The van’t Hoff factor of ( 0.1 M L aleft(N O_{3}right)_{3} ) solution is found to be 2.74 , the percentage dissociation of the salt is: A. ( 85 % ) в. ( 58 % ) c. ( 65.8 % ) D. ( 56.8 % ) |
12 |

1404 | The freezing point of equimolal solution will be highest for: A ( cdot C_{6} H_{5} N H_{3} C l ) в. ( A g N O_{3} ) ( mathbf{c} cdot C aleft(N O_{3}right)_{2} ) ( mathbf{D} cdot L aleft(N O_{3}right) ) E. ( D- ) fructose |
12 |

1405 | A solution is prepared by dissolving ( 5.64 mathrm{g} ) of glucose in ( 60 mathrm{g} ) of water. Calculate the mole fraction of each of glucose and water respectively. B. 0.01,0.99 c. 0.92,0.08 D. 0.789, 0.211 |
12 |

1406 | The ratio of lowering of vapour pressure of ( 0.1 ~ M ) aqueous solutions of ( K C l ) ( boldsymbol{C u} boldsymbol{S O}_{4} & boldsymbol{N a}_{2} boldsymbol{S O}_{4} ) is: A. 1: 2: 3 B. 2: 2: 3 ( mathrm{c} cdot 1: 1: 1 ) D. 3: 2: 1 |
12 |

1407 | The solubility of a gas in a liquid is directly proportional to the pressure of the gas. This statement is: A. Raoult’s law B. Henry’s law c. van’t Hoff’s law D. None of these |
12 |

1408 | Example 2.23 Among the following, the solution which shows the lowest osmotic pressure is a. 0.10 M NaCI b. 0.05 M CaCl, c. 0.04 M K [Fe(CN)] d. 0.03 M FeCl2 |
12 |

1409 | Illustration 2.165 Calculate the osmotic pressure of 5% solution of cane sugar (sucrose) at 300 K. |
12 |

1410 | Dissolution of a non-volatile solute into a liquid leads to the- A. Decrease of entropy. B. Increase in tendency of the liquid to freeze c. Increase in tendency to pass into the vapour phase. D. Decrease in tendency of the liquid to freeze |
12 |

1411 | When a non-volatile solute is dissolved in a solvent, the relative lowering of vapour pressure is equal to : A. mole fraction of solvent B. mole fraction of solute c. molarity of solution D. molality of solution |
12 |

1412 | Write two differences between ideal solutions and non-ideal solutions. |
12 |

1413 | The freezing point of equimolal aqueous solution will be highest for : A. ( C_{6} H_{5} N H_{3} C l ) в. ( C aleft(N O_{3}right)_{2} ) c. ( L aleft(N O_{3}right)_{3} ) D. ( C_{6} H_{12} O_{6} ) |
12 |

1414 | Hlustration 2.170 The osmotic pressure of blood is 8.21 atm at 310 K. How much glucose should be used per L for an intravenous injection that is isotopic with blood? |
12 |

1415 | A well stirred ( (1 L) ) solution of ( 0.1 M C u S O_{4} ) is electrolysed at ( 25^{circ} C ) using copper electrodes with a current of 25 m ( A ) for 6 hours. If current efficiency is ( 50 % ). At the end of the duration what would be the concentration of copper ions in the solution? A ( .0 .0856 M ) В. ( 0.092 mathrm{M} ) c. ( 0.0986 M ) D. ( 0.1 M ) |
12 |

1416 | Which of the following 0.1 M aqueous solutions will have the lowest freezing point? A. Potassium sulphate B. Sodium chloride c. urea D. Glucose |
12 |

1417 | ( 0.3500 g ) of potassium oxalate is titrated with ( 37.40 m L ) of sodium permaganate to reach a pink end point in the following reaction: ( mathbf{5} C_{2} O_{4(a q)}+2 M n O_{4(a q)}^{-}+16 H_{(a q)}^{+} rightarrow ) ( mathbf{2} M boldsymbol{n} boldsymbol{S} boldsymbol{O}_{4(a q)}+boldsymbol{6} boldsymbol{S} boldsymbol{O}_{4(a q)}^{2-}+mathbf{1 0} boldsymbol{C} boldsymbol{O}_{2(boldsymbol{g})}+ ) ( mathbf{8} boldsymbol{H}_{2} boldsymbol{O}_{(l)} ) What was the concentration of the sodium permanganate? |
12 |

1418 | Choose the correct statement with respect to the vapour pressure of a liquid among the following. A. Increases linearly with increasing temperature. B. Increases non-linearly with increasing temperature. c. Decreases linearly with increasing temperature D. Decreases non-linearly with increasing temperature. |
12 |

1419 | Match column I with column II. | 12 |

1420 | Which of the following will form an ideal solution? A ( cdot C_{2} H_{5} O H ) and water B. ( H N O_{3} ) and water c. ( C H C l_{3} ) and ( C H_{3} C O C H_{3} ) D. ( C_{6} H_{6} ) and ( C_{6} H_{5} C H_{3} ) |
12 |

1421 | We define p value of a term (say ( x ) ) as ( boldsymbol{p}_{boldsymbol{x}}=-log boldsymbol{x} ) Calculate the value of ( 1000 p ) for ( N O_{3} ) in a solution that is ( 4.78 times 10^{-2} mathrm{M} ) in ( boldsymbol{C u}left(boldsymbol{N} boldsymbol{O}_{3}right)_{2} ) and ( boldsymbol{0 . 1 0 4} boldsymbol{M} ) in ( boldsymbol{Z} boldsymbol{n}left(boldsymbol{N} boldsymbol{O}_{3}right)_{2} ) |
12 |

1422 | ( 100 mathrm{ml} ) of ( 10 mathrm{V} mathrm{H}_{2} mathrm{O}_{2} ) solution is heated. The evolved gas is completely reacted with Ca to form CaO. The aqueous solution of Cao is neutralised by ( 50 mathrm{m} ) of ( boldsymbol{H}_{2} boldsymbol{S} boldsymbol{O}_{4} ) solution. The molarity of ( boldsymbol{H}_{2} boldsymbol{S O} mathbf{4} ) is: A. 2.43 M B. 1.78 M c. ( 1.55 mathrm{M} ) D. 2.78 м |
12 |

1423 | A molal solution is one that contains one mole of a solute in : A. 1000 g of the solvent B. 1000 ( mathrm{mL} ) of the solution c. 1 litre of the solvent D. 1000 g of the solution |
12 |

1424 | The density ( left(operatorname{in} g m l^{-1}right) ) of a 3.60 M sulphuric acid solution that is ( 29 % ) ( H_{2} S O_{4}left(text { Molar mass }=98 mathrm{g} mathrm{mol}^{-1}right) mathrm{by} ) mass will be: A .1 .64 B. 1.88 c. 1.22 D. 1.45 |
12 |

1425 | Calculate the amount of ( C a C l_{2} ) (molar mass ( =111 g ) mol ( ^{-1} ) ) which must be added to ( 500 g ) of water to lower its freezing point by ( 2 K, ) assuming ( C a C l_{2} ) is completely dissociated. ( left(K_{f} ) for right. water ( =1.86 K k g m o l^{-1} ) ) |
12 |

1426 | The vapour pressure of pure benzene and toluene at a particular temperature are ( 100 m m ) and 50 mm respectively. Then the mole fraction of benzene in vapour phase in contact with equimolar solution of benzene and toluene is : A . 0.67 B. 0.75 c. 0.33 D. 0.50 E . 0.20 |
12 |

1427 | Illustration 2.41 A certain ideal solution of two liquids A and B has mole fraction of 0.3 and 0.5 for the vapour phase and liquid phase, respectively. What would be the mole fraction of B in the vapour phase, when the mole fraction of A in the liquid is 0.25? |
12 |

1428 | ustration 2.181 Two grams of benzoic acid (CH-COOH) dissolved in 25.0 g of benzene shows a depression in freezing point equal to 1.62 K. Molal depression constant for benzene is 4.9 K kg-moll. What is the percentage association of acid if it forms dimer in solution? (NCERT Example 2.12) |
12 |

1429 | An ammonia solution has a density of ( 0.910 mathrm{g} mathrm{cm}^{-3} ) and is ( 25.0 % mathrm{NH}_{3} ) by mass. What is the molarity of the solution? A . ( 12.1 mathrm{M} ) B. 13.4 M c. ( 14.5 mathrm{M} ) D. 15.5 M |
12 |

1430 | The boiling point of 0.1molal ( boldsymbol{K}_{4}left[boldsymbol{F} boldsymbol{e}(boldsymbol{C} boldsymbol{N})_{6}right] ) solution will be : ( left(text {Given } boldsymbol{K}_{boldsymbol{b}} text {for water}=mathbf{0 . 5 2 K k g} mathbf{m o l}right. ) A ( cdot 100.52^{0} C ) В. ( 100.104^{0} C ) c. ( 100.26^{circ} mathrm{C} ) D. ( 102.6^{circ} mathrm{C} ) |
12 |

1431 | ( frac{pi}{4} ) | 12 |

1432 | The quantity of ( C O_{2} ) in ( 500 mathrm{ml} ) of soda water when packed under 2.5 atm ( C O_{2} ) pressure at ( 298 mathrm{K} ) is gm ( Henry’s law constant ( 1.67 times 10^{8} ) pa at ( 298 mathrm{K} ) ) A . 0.64 B. 1.86 ( c cdot 6.4 ) D. 18.6 |
12 |

1433 | Number of moles of solute in solution is represented by : A. ( M times V(L) ) в. ( M times V(m l) ) c. ( m times V(L) ) D. ( N times V(m l) ) |
12 |

1434 | Two liquids ( A ) and ( B ) are miscible over the whole range of composition and may be treated as ideal (obeying Raoult’s Law). At ( 350 mathrm{K} ) the vapour pressure of pure ( A ) is ( 24.0 mathrm{kPa} ) and of pure B is 12.0 kPa. A mixture of 60% A and ( 40 % mathrm{B} ) is distilled at this temperature; what is the pressure in a closed distillation apparatus from which air is excluded? in KPa |
12 |

1435 | The composition of a sample of Wustite is ( F e_{0.93} ) O. What is the percentage of iron present as ( F e^{3+} ) in total iron? A . ( 15.05 % ) B. 25% ( c .35 % ) D. ( 45 % ) |
12 |

1436 | Vapour pressure of ( C C l_{4} ) at ( 25^{circ} mathrm{C} ) is 143 ( mathrm{mm} ) of Hg. ( 0.5 mathrm{g} ) of a non-volatile solute (mol. Mass ( =mathbf{6 5} ) ) is dissolved in ( 100 mathrm{mL} ) ( boldsymbol{C C l}_{4} . ) Find the vapour pressure of the solution: (Density of ( boldsymbol{C} boldsymbol{C l}_{4}= ) ( 1.58 g / c m^{3} ) ( mathbf{A} cdot 141.93 mathrm{mm} ) B. ( 94.39 mathrm{mm} ) c. ( 199.34 mathrm{mm} ) D. ( 143.99 mathrm{mm} ) |
12 |

1437 | Illustration 2.108 What do you understand by the term that K, for water is 1.86 K kg mol-l? |
12 |

1438 | What mass of an organic compound ( left(M w_{0}=156right) ) must be dissolved in 50 ( mathrm{mL} ) of an organic solvent ( left(boldsymbol{d}=mathbf{0 . 9 g c c}^{-1}right) ) water to lower the freezing point by ( 0.48^{circ} mathrm{C} . K_{f} ) of benzene ( =5.12 ) |
12 |

1439 | Solubility of a gas in a liquid increases on: A. increasing temperature. B. decreasing pressure. C. increasing pressure. D. increasing temperature and pressure |
12 |

1440 | Illustration 2.194 One mole of triphenyl methanol lowers the freezing point of 1000 g of 100% sulphuric acid twice as much as one mole of methanol. Why? |
12 |

1441 | Question 40. Determine the amount of CaCl, (i=2.47) dissolved in 2.5 L of water such that its osmotic pressure is 0.75 atm at 27°C. First calculate the moles of CaCl, by applying van’t Hoff equation, T = iCRT and C = MB Then calculate amount of CaCl, by multiplying the moles with molar mass. |
12 |

1442 | Which of the following statements is true for a solution containing components ( A ) and ( B ) and following Raoult’s law: A. ( A-B ) attraction force is greater than ( A-A ) and ( B- ) ( B ) B. ( A-B ) attraction force is less than ( A-A ) and ( B-B ) c. ( A-B ) attraction force remains same as ( A-A ) and ( B-B ) D. Volume of solution is different from sum of volume of solute and solvent |
12 |

1443 | The volume vs. temperature graph of mole of an ideal gas is given below. The pressure of the gas (in atm) at ( X, Y ) and ( Z, ) respectively, are: A. 0.328,0.820,0.820 0 B. 3.28,8.20,3.28 c. 0.238,0.280,0.280 D. 32.8,0.280,82.0 |
12 |

1444 | For a dilute solution containing 2.5 g of a non-volatile non-electrolyte solute in ( 100 g ) of water, the elevation in boiling point at 1 atm pressure is 2 ?. Assuming that the concentration of solute is much lower than the concentration of solvent, the vapour pressure (in ( mathrm{mm} ) of ( mathrm{Hg} ) ) of the solution is: [Take ( : K_{b}=0.76 K k g ) mol ( ^{-1} ) ] |
12 |

1445 | In which of the following solvent, the solubility of ( N a C l ) is maximum? A. Methanol B. water c. Formic acid D. Formamide |
12 |

1446 | The vapour if an aqueous solution of glucose is ( 750 m m ) of ( mathrm{Hg} ) at ( 373 mathrm{K} ) Calculate molality of the solution? A. 0.523 mol/kg в. 0.617 mol / ( / k g ) c. 0.731 mol ( / mathrm{kg} ) D. 0.836 mol / ( / k g ) |
12 |

1447 | a) A solution containing ( 18 g ) of nonvolatile non-electrolyte solute is dissolved in 200 g of water freezes at 272.07 K. Calculate the molecular mass of the solute. Given ( : boldsymbol{K}_{boldsymbol{f}}=mathbf{1 . 8 6} mathrm{K} mathrm{kg} / mathrm{mol} ) The freezing point of water ( =273 mathrm{K} ) b) Define the isotonic solution. What happens when the blood cell is dipped in a solution containing more than normal saline concentration? |
12 |

1448 | In case a solute associates in solution, the van’t Hoff factor is : A ( . i>1 ) в. ( i=1 ) ( c cdot i<1 ) D. None of these |
12 |

1449 | Determine the pH value of ( 0.001 M ) acetic acid solution if it is ( 2 % ) ionised at this concentration. How can the degree of dissociation of this acetic acid solution be increased? |
12 |

1450 | Mustration 2.129 Two elements A and B form compounds having molecular formula AB, and AB, When dissolved in 20 g of benzene, 1 g of AB, lowers the freezing point by 2.3 K, whereas 1.0 g of AB, lowers it by 1.3 K. The molar depression constant for benzene is 5.1 K kg mol-1. Calculate the atomic mass of A and B. |
12 |

1451 | Aqueous ( N a O H ) solution is labelled as ( 10 % ) by weight mole fraction of the solute in it is: A . 0.05 B. 0.0476 c. 0.052 D. 0.52 |
12 |

1452 | The osmotic pressure of a decimolar solution of glucose at ( 30^{circ} mathrm{C} ) is : ( mathbf{A} cdot 24.88 mathrm{atm} ) B. 2.488 atm ( mathbf{c} .0 .248 mathrm{atm} ) D. ( 189.09 mathrm{cm} ) |
12 |

1453 | The mass percentage of nitrogen in histamine is |
12 |

1454 | Hlustration 2.102 Why is camphor preferred as a solvent for measuring the molecular mass of naphthalene by Rast method? |
12 |

1455 | The vapour pressure of water at ( 20^{circ} mathrm{C} ) is 17 mm Hg. Calculate the vapour pressure of a solution containing 2.8 g of urea ( left(N H_{2} C O N H_{2}right) ) in 50 g of water ( mathrm{N}=14, mathrm{C}=12,0=16, mathrm{H}=1(16.71 mathrm{mm} mathrm{Hg}) ) |
12 |

1456 | The partial pressure of ( boldsymbol{O}_{2} ) in air is 0.21 at ( m ) at sea level. If aquatic life requires a concentration of ( boldsymbol{O}_{2} ) at least 4.16 ( m g / ) litre, will the aquatic life sustain in sea level lake. ( boldsymbol{K}_{boldsymbol{H}} ) for ( boldsymbol{O}_{2} ) is ( 1.3 times 10^{-3} ) mol / litre – atm. A. 0.82 mg/litre в. ( 0.87 mathrm{mg} / ) litre c. 0.95 mg/litre D. ( 0.9 mathrm{mg} / ) litre |
12 |

1457 | The plot of ( frac{1}{X_{A}} ) vs ( frac{1}{Y_{A}} ) (where ( X_{A} ) and ( boldsymbol{Y}_{A} ) are the mole fractions of liquid ( mathrm{A} ) in liquid and vapour phase, respectively) is linear. The slope and intercept of this plot are respectively: ( ^{mathrm{A}} cdot frac{P_{d}^{0}}{P_{B}^{0}} ) and ( frac{P_{A}^{0}-P_{B}^{0}}{P_{B}^{0}} ) в. ( frac{P_{d}^{0}}{P_{B}^{0}} ) and ( frac{P_{B}^{0}-P_{A}^{0}}{P_{B}^{0}} ) c. ( frac{P_{B}^{0}}{P_{A}^{0}} ) and ( frac{P_{A}^{0}-P_{B}^{0}}{P_{B}^{0}} ) D. ( frac{P_{B}^{0}}{P_{A}^{0}} ) and ( frac{P_{B}^{0}-P_{A}^{0}}{P_{B}^{0}} ) |
12 |

1458 | 18 g glucose is added to 178.2 g of water the vapour pressure of water for this aqueous solution at ( 100^{0} C ) is: A. 704 torr B. 759 torr c. 7.6 torr D. None of these |
12 |

1459 | The correct relationship between enthalpy (in cal mol-1) of vaporisation of liquid and its boiling points is? |
12 |

1460 | A metal ( M ) of molar mass 96 g ( m o l^{-1} ) reacts with fluorine to form a salt that can be represented as ( M F_{x} ). In order to determine ( x .9 .18 mathrm{g} ) of the sample of the salt is dissolved in 100 g of water and its boiling point was determined to be ( 374.38 mathrm{K} ). What is the value of ( x ) ? Given: ( boldsymbol{K}_{boldsymbol{b}}(boldsymbol{w} boldsymbol{a} boldsymbol{t e r})=mathbf{0 . 5 1 2} boldsymbol{K} boldsymbol{k g m o l}^{-1} ) Assume complete dissociation of salt A . ( x=2 ) в. ( x=4 ) c. ( x=5 ) D. ( x=7 ) |
12 |

1461 | Pure benzene freezes at ( 5.3^{circ} mathrm{C} ). A solution of 0.223 g of phenyl acetic acid ( left(C_{6} H_{5} C H_{2} C O O Hright) ) in 4.4 g of benzene ( left(K_{f} 5.12 mathrm{K} mathrm{kg} mathrm{mol}^{-1}right) ) freezes at ( 4.47^{circ} mathrm{C} ) From the observation one can conclude that: A. phenyl acetic acid exists as such in benzene B. phenyl acetic acid undergoes partial ionization in benzene c. phenyl acetic acid undergoes complete ionization in benzene D. phenyl acetic acid dimerizes in benzene |
12 |

1462 | At ( 300 K ), two pure liquids ( A ) and ( B ) have vapour pressures ( 150 mathrm{mm} mathrm{Hg} ) and 100 mm ( H g ) respectively. In an equimolar liquid mixture of ( boldsymbol{A} ) and ( boldsymbol{B} ) the mole fraction of ( B ) in the vapour mixture at this temperature is: A . 0.6 B. 0.5 c. 0.8 D. 0.4 |
12 |

1463 | Henry’s law constant for the molality of methane in benzene at ( 298 mathrm{K} ) is ( 4.27 times ) 105 mm ( H g ). Calculate the solubility of methane in benzene at ( 298 K ) under ( 760 m m H g ) |
12 |

1464 | What is the molarity of ( 11.2 ~ V ) of ( H_{2} O_{2} ? ) ( A cdot 1 M ) в. ( 2 M ) c. ( 5.6 M ) D. ( 11.2 M ) |
12 |

1465 | A mixture of two miscible liquids ( A ) and B is distilled under equilibrium conditions at 1 atm pressure. The mole fraction of ( A ) in solution and vapour phase are 0.30 and 0.60 respectively. Assuming ideal behaviour of the solution and the vapour. Calculate the ratio of the vapour pressure of pure ( A ) to that of pure ( B ) |
12 |

1466 | Hlustration 2.36 Benzene and toluene form nearly ideal solution. At 298 K, the vapour pressure of pure benzene is 150 torr and of pure toluene is 50 torr. Calculate the vapour pressure of the solution, containing equal weights of two substances at this temperature? |
12 |

1467 | 0.62 Why is the mass determined by measuring a colligative property in case of some solutes abnormal? Discuss it with the help of van’t Hoff factor. |
12 |

1468 | tion 2.42 Solution of two volatile liquids x and y by Raoult’s law. At a certain temperature it is found that when the total pressure above a given solution is 400 mm of Ho the mole fraction of x in the vapour is 0.45 and in the liquid is 0.65. What are the vapour pressures of two pure liquids at the given temperature? |
12 |

1469 | The Van’t Hoff factor (i) for ( K_{2} S O_{4} ) is ( A ) B. 2 ( c cdot 0 ) D. 3 |
12 |

1470 | Vapour pressure of water is ( 360 mathrm{mm} mathrm{Hg} ) how much urea should be added to 200 ml. water to reduce its vapour pressure by ( 0.5 % ?(text { Molecular weight of urea }=60) ) |
12 |

1471 | Illustration 2.141 How much ethyl alcohol must be added to 1.00 L of water so that the solution will not freeze at -4°F ? |
12 |

1472 | The molarity of ( 98 % ) ( mathbf{H}_{2} mathbf{S O}_{4}(boldsymbol{d}=mathbf{1} . mathbf{8} boldsymbol{g} / boldsymbol{m} boldsymbol{L}) ) by weight is: A. 6 . B. 18M c. 10 м D. 4 M |
12 |

1473 | DULULUI CUI Valen. Ouestion 7. Why is vapour pressure of an aqueous solution of glucose lower than that of water? |
12 |

1474 | The unit of concentration may be given by : A. gram per millilitre (g/mı) B. kilogram per litre (kg/I) c. gram per litre (g/I) D. all of the above |
12 |

1475 | On the basis of composition of matter, milk is considered to be: A . a pure substance B. an impure substance c. an element D. a compound |
12 |

1476 | Assertion Van’t Hoff factor for solute showing dissociation is always greater than for solute showing association. Reason Dissociation leads to increase in number of particles whereas, association leads to a decrease in number of particles. A. Both Assertion and Reason are correct and Reason is the correct explanation for Assertion B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion C. Assertion is correct but Reason is incorrect D. Assertion is incorrect but Reason is correct |
12 |

1477 | I to ice 2. When potassium nitrate is added to ice, it (a) increases the melting point of ice (b) decreases the melting point of ice (c) does not effect the melting point of ice (d) None of the above is correct |
12 |

1478 | ( 4 L ) of ( 0.02 M ) aqueous solution of ( N a C l ) was diluted by adding ( 1 L ) of water. The molarity of the resultant solution is: ( mathbf{A} cdot 0.004 ) B. 0.008 c. 0.012 D. 0.016 |
12 |

1479 | What will be the molarity of ( 30 m L ) of ( 0.5 M H_{2} S O_{4} ) solution diluted to ( 500 m L ? ) ( mathbf{A} cdot 0.3 M ) в. ( 0.03 M ) ( c .3 M ) D. ( 0.103 M ) |
12 |

1480 | One litre of a sample of hard water contains ( 55.5 mathrm{mg} ) of ( mathrm{CaCl}_{2} ) and ( 4.75 mathrm{mg} ) of ( M g C l_{2} . ) The total hardness in terms of ppm of ( C a C O_{3} ) is : A. 5 ppm в. ( 10 mathrm{ppm} ) c. 20 ppm D. none of the above |
12 |

1481 | Two liquids ( A ) and ( B ) form an ideal solution. The vapour pressure of pure ( mathbf{A} ) and pure B are 66mm of Hg and 88mm of Hg, respectively. Calculate the composition of vapour ( A ) in the solution which is equilibrium and whose molar volume is ( 36 % ) A. 0.43 B. 0.70 c. 0.30 D. 0.50 |
12 |

1482 | Addition of which solute in 1.0 molar ( K I ) solution will not cause a change in vapour pressure: A ( cdot I_{2} ) B. water c. ( H g I_{2} ) D. addition of ( N a_{2} S O_{4} ) |
12 |

1483 | How many grams of potassium chloride ( (K C l) ) must be added to make ( 500 mathrm{mL} ) of ( 1.00 mathrm{M} K C l ) solution? A ( .1 .00 mathrm{g} ) B. 18.6 ( g ) c. ( 37.3 mathrm{g} ) D. 74.5 g E. ( 149 mathrm{g} ) |
12 |

1484 | Assertion Helium shows only positive deviation from ideal behaviour at room temperature. Reason Helium is an inert gas. A. Both Assertion and Reason are correct and Reason is the correct explanation for Assertion B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion c. Assertion is correct but Reason is incorrect D. Both Assertion and Reason are incorrect |
12 |

1485 | The Henry’s law constant for the solubility of oxygen in water is ( 3.3 times ) ( 10^{-4} ) M ( / ) atm at ( 12^{circ} mathrm{C} ). Air is ( 21 mathrm{mol} % ) oxygen. How many grams of oxygen can be dissolved in one litre of a trout stream at ( 12^{circ} mathrm{C} ) at an air pressure of 1.00 atm? A. 0.222 g gg ( . . .222 ) В. 0.11222 g c. 0.333 g D. 0.422 g |
12 |

1486 | Illustration 2.196 A 0.2 molal solution of KCl freezes at -0.68°C. If K, for H,O is 1.86, the degree of dissociation of KCl is a. 85% b. 83% c. 65% d. 90% |
12 |

1487 | The Van’t Hoff factor for a dilute aqueous solution of glucose is : A. Zero в. 1.0 c. 1.5 D. 2.0 |
12 |

1488 | The substance ( A ), when dissolved in solvent ( mathrm{B} ), shows the molecular mass corresponding to ( A_{3} . ) The van”t Hoffs factor will be: A. B. 2 ( c cdot 3 ) ( D cdot 1 / 3 ) |
12 |

1489 | The vapour pressure of a pure liquid ( mathbf{A} ) is ( 40 mathrm{mm} ) of ( mathrm{Hg} ) at ( 310 mathrm{K} ). The vapour pressure of this liquid in a solution with liquid B is 32 mm of Hg. The mole fraction of ( A ) in the solution, if it obey’s Raoult’s law, is? A . 0.8 B. 0.5 ( c cdot 0.2 ) D. 0.4 |
12 |

1490 | Illustration 2.50 The vapour pressure of chloroform (CHCI), and dichloromethane (CH,C1,) at 298 K is 200 mm Hg and 415 mm Hg, respectively. Calculate a. The vapour pressure of the solution prepared by mixing 25.5 g of CHCI, and 40 g of CH,Cl, at 298 K. b. Mole fractions of each component in vapour phase. (NCERT Example 2.5) |
12 |

1491 | In a mixture, ( ^{prime} A^{prime} ) and ‘ ( B^{prime} ) components show the negative deviations as: ( mathbf{A} cdot triangle V_{operatorname{mix}}>0 ) ( mathbf{B} cdot triangle V_{operatorname{mix}}<0 ) C. ( A ) – ( B ) interaction is weaker than ( A-A ) and ( B-B ) interactions D. None of the above reasons is correct |
12 |

1492 | Define Henry’s law. | 12 |

1493 | What is vapour pressure? | 12 |

1494 | To make ( 50 mathrm{mL} ) solution of ( K C l ) of ( 1 mathrm{M} ) how many grams of ( K C l ) are required to add to this solution? A ( .1 .00 mathrm{g} ) В. ( 1.86 mathrm{g} ) c. ( 3.73 mathrm{g} ) D. 7.45 g E . ( 1.49 mathrm{g} ) |
12 |

1495 | In the following equilibrium ( N_{2} O_{4(g)} rightleftharpoons ) ( mathbf{2} N boldsymbol{O}_{2(boldsymbol{g})} boldsymbol{N} boldsymbol{O}_{2(g)} ) is ( mathbf{5 0 1 %} ) of the total volume. hence degree of dissociation and vant hoff factor (i) respectively are: A. 0.5,1.5 B. 0.25,1.25 c. 0.33,1.33 D. 0.66,1.66 |
12 |

1496 | Solution (by mass) of cane sugar in water has ulate freezing point of 5% glucose in water if Question 20. A 5% solution (by mass) of cane freezing point 271 K. Calculate freezing point of 5% 810 freezing point of pure water is 273.15 K. Freezing point of pure water is 273 15 K (0°C) and that of given solution is 271 K, i.e., we have depression in freezing point. So. 0 Apply the formula of depression in freezing point for cane sugar and make it eq (0) (ii) Similarly, find the depression in freezing point for glucose and make it eq (1) (iii) Compare the two equations to find the freezing point of glucose. |
12 |

1497 | ( 40 % ) by weight solution will contain how much mass of the solute in 1 L solution? Density of the solution is ( 1.2 mathrm{g} / mathrm{mL} ) A. ( 480 g ) B. ( 48 g ) ( c cdot 38 g ) D. ( 380 g ) |
12 |

1498 | Determine the osmotic pressure of a solution prepared by dissolving 2.5 ( times 10^{-2} ) of ( K_{2} S O_{4} ) in ( 2 L ) of water at ( 25^{circ} mathrm{C}, ) assuming that it is completely dissociated ( left(R=0.0821 mathrm{L} operatorname{atm} K^{-1} m o l e^{-1}, ) Molar right. ( operatorname{mass} K_{2} S O_{4}=174 mathrm{g} operatorname{mol} e^{-1} ) |
12 |

1499 | For a dilute solution containing 2.5 g of a non-volatile non-electrolyte solute in ( 100 mathrm{g} ) of water, the elevation in boiling point at 1 atm pressure is ( 2^{circ} C ) Assuming concentration of solute is much lower than the concentration of solvent, the vapour pressure (mm of Hg) of the solution is: ( left[boldsymbol{K}_{boldsymbol{b}}=mathbf{0 . 7 6} boldsymbol{K} boldsymbol{K} boldsymbol{g} boldsymbol{m o l}^{-1}right] ) A . 724 в. 740 ( c cdot 736 ) D. 718 |
12 |

1500 | A solution of 10 g of a nonvolatile binary electrolyte (mat. wt. ( =100 ) ) in 500 g of water freezes at ( -0.74^{circ} mathrm{C} ). What is the degree of ionisation? ( left[k_{f} text { of water }=1.85 K text { molality }^{-1}right] ) A . 50% B. 75% c. ( 100 % ) D. 0% |
12 |

1501 | Mole fraction of solute present in an aqueous solution having molality equal to 2 is: A . 0.9653 B. 0.347 c. 0.653 D. 0.0347 |
12 |

1502 | f at a particular temperature, the density of ( 18 ~ M ~ H_{2} S O_{4} ) is ( 1.8 ~ g c m^{-3} ) then calculate the molality of the solution: |
12 |

1503 | How many moles of glucose ( left(C_{6} H_{12} O_{6}right) ) should be dissolved into a solution with a total volume of ( 0.500 L ) to produce a 1 ( M ) glucose solution? ( mathbf{A} cdot 1 mathrm{mol} ) B. 24mol ( c .0 .5 mathrm{mol} ) D. 0.25 mol |
12 |

1504 | How much water, in liters, must be added to 0.5 L of 6 M HCl to make it 2 M? A . 0.33 B. 0.5 ( c cdot 1 ) D. 1.5 ( E cdot 2 ) |
12 |

1505 | Which of the following statements is correct, if the intermolecular force of attraction between the particles in liquid ( A, B, C ) is in the order ( A<B<C ? ) This question has multiple correct options A. All the three evaporate at the same rate B. B evaporates faster than A c. B evaporates more readily than ( c ) D. A evaporates more readily than |
12 |

1506 | Q. 52 Assertion (A) When methyl alcohol is added to water, boiling point of water increases. Reason (R) When a volatile solute is added to a volatile solvent elevation in boiling point is observed. |
12 |

1507 | A sugar syrup of weight ( 214.2 mathrm{g} ) contains 34.2 g of sugar ( left(C_{12} H_{22} O_{11}right) ) Calculate. the molal concentration (Write your answer as ( 18 X ), where, ( X= ) molality) |
12 |

1508 | In which of the following pairs of solutions will the values of the Van’t Hoff factor be the same? A ( cdot_{0.05} ) M ( K_{4}left[text { Fe }(C N)_{6}right] ) and 0.10 M FeSO( _{4} ) B. 0.20 М NaCl and 0.10 М Ва С( l_{2} ), c. ( _{0.05} ) M FeSO( _{4}left(N H_{4}right)_{2} ) SO( _{4} ). ( 6 H_{2} ) O and 0.02 M КСl.М ( g C l_{2} .6 H_{2} O ) D. All have same value |
12 |

1509 | The degree of dissociation of ( boldsymbol{C a}left(boldsymbol{N O}_{3}right)_{2} ) in a dilute aqueous solution containing ( 7 g ) of the salt per ( 100 g ) of water at ( 100^{circ} C ) is ( 70 % ). If the vapour pressure of water at ( 100^{circ} mathrm{C} ) is ( mathbf{7 6 0} boldsymbol{m m}, ) calculate the vapour pressure of the solution. ( mathbf{A} .378 .5 mathrm{mm} ) В. ( 492.8 mathrm{mm} ) c. ( 746.10 m m ) D. ( 985.6 mathrm{mm} ) |
12 |

1510 | The values of the Henry’s law constant of ( A r, C O_{2}, C H_{4} ) and ( O_{2} ) in water at ( 25^{0} C ) are 40.30,1.67,0.41 and ( 34.86 k b a r, ) respectively. The order of their solubility in water at the same temperature and pressure is: A. ( A r>O_{2}>C O_{2}>C H_{4} ) в. ( C H_{4}>C O_{2}>A r>O_{2} ) c. ( C H_{4}>C O_{2}>O_{2}>A r ) D. ( A r>C H_{4}>O_{2}>C O_{2} ) |
12 |

1511 | Which of the following statements is false? A. Two different solutions of sucrose of same molality prepared in different solvents will have the same depression in freezing point. B. The osmotic pressure of a solution is given by the equation ( pi=C R T ) (where ( C ) is the molarity of the solution) C. Decreasing order of osmotic pressure for ( 0.01 M ) aqueous solutions of barium chloride, potassium chloride, acetic acid and sucrose is ( B a C l_{2}>K C l> ) ( C H_{3} C O O H> ) sucrose D. According to Raout’s law the vapour pressure exerted by a volatile component of a solution is directly proportional to its mole fraction in the solution |
12 |

1512 | Van’t Hoff factor, (i), of a ( 0.5 % ) (w/W) aqueous solution of ( K C l ) which freezes at ( -0.24^{circ} mathrm{C} ) is: ( left(K_{f} text { of water }=1.86 mathrm{K} mathrm{kg} text { mol}^{-1}right. ) molecular weight of ( K C l=74.5 ) ) A . 1.52 B. 2.32 c. 1.92 D. 1.32 |
12 |

1513 | A compound ( M X_{2} ) has observed and normal molar masses 65.6 and 164 respectively. The apparent degree of ionization of ( M X_{2} ) is: A . ( 75 % ) B. ( 85 % ) c. ( 65 % ) D. ( 25 % ) |
12 |

1514 | An ideal binary solution is prepared by two liquids ( A ) and ( B, ) with ( p_{A}^{o}>p_{B}^{o} . ) Then : A. A-B interactions are stronger than A-A and B-B B. A and B have same molecular masses c. A-B interactions are similar to A-A and B-B interactions D. Both A and B are non-polar substances |
12 |

1515 | Illustration 2.74 Calculate the vapour pressure lowering caused by the addition of 68.4 g of sucrose (molecular mass = 342) to 500 g of water if the vapour pressure of pure water at 25°C is 20.0 mm Hg. |
12 |

1516 | ( 68 % H N O_{3} ) and ( 32 % H_{2} O ) by mass forms: A. Maximum boiling azeotrope B. Minimum boiling azeotrope C. mixture which shows positive deviation D. Ideal solution |
12 |

1517 | Each pair forms ideal solution except : A ( cdot C_{2} H_{5} B r ) and ( C_{2} H_{5} ) B . ( C_{6} H_{5} C l ) and ( C_{6} H_{5} B r ) c. ( C_{6} H_{6} ) and ( C_{6} H_{5} cdot C H_{3} ) D. ( C_{2} H_{5} I ) and ( C_{2} H_{5} O H ) |
12 |

1518 | The vapor pressure of water at ( 80^{circ} mathrm{C} ) is 355 torr. ( A ) 100 ( m l ) vessel contained water-saturated oxygen at ( 80^{circ} mathrm{C} ) the total gas pressure being 760 torr. The contents of the vessel were pumped into a ( 50.0 mathrm{ml} ), vessel at the same temperature, What were the partial pressure of oxygen and of water vapor what was the total pressure in the final equilibrated state? Neglect the volume of any water which might condense. |
12 |

1519 | Derive the relationship between relative lowering of vapour pressure and molar mass of non-volatile solute. | 12 |

1520 | A concentrated solution of lead nitrate in water can be stored in A. an iron vessel B. a copper vessel c. a zinc vessel D. a magnesium vessel |
12 |

1521 | ( 25 mathrm{cm}^{3} ) of oxalic acid completely neutralised ( 0.064 g ) of sodium hydroxide. Molarity of the oxalic acid solution is : в. 0.032 м c. 0.064 м D. 0.015 М |
12 |

1522 | Hlustration 2.197 A mixture of 0.1 mol of Na, and 0.1 mol of BaO is dissolved in 1000 g of H,O. Calculate the vapour pressure of solution at 373 K. |
12 |

1523 | Illustration 2.96 Calculate the molar mass of a substance 1g of which when dissolved in 100 g of water gave a solution boiling at 100.1°C at a pressure of 1 atm (Kfor water = 0.52 K kg mol-l) |
12 |

1524 | In a 0.2 molal aqueous solution of a weak acid HX, the degree of ionization is ( 0.3 . ) taking ( K_{f} ) for water as ( 1.85, ) the freezing point of the solution will be nearest to: A. -0.360 B. -0.260 c. +0.480 D. -0.481 |
12 |

1525 | Solute when dissolved in water: A. increases the vapour pressure of water B. decreases the boiling point of water C . decreases the freezing point of water D. all of the above |
12 |

1526 | State True or False. In association of solute, the Van’t Hoff factor is greater than unity. A. True B. False |
12 |

1527 | What would be the change in the freezing point of ( H_{2} O ) in a solution of ( 1 m N a C l(a q) ? ) ( mathbf{A} cdot-1.86^{circ} mathrm{C} ) B. ( -0.52^{circ} mathrm{C} ) c. ( -3.72^{circ} mathrm{C} ) D. ( 1.86^{circ} mathrm{C} ) E ( .3 .72^{circ} mathrm{C} ) |
12 |

1528 | ( K_{2} H g I_{4} ) is ( 40 % ) ionised in aqueous solution. The value of its van’t Hoff factor (i) is: A. 1.8 B. 2. c. 2.0 D. 1. |
12 |

1529 | For a very dilute solution of ( boldsymbol{H}_{3} boldsymbol{P} boldsymbol{O}_{3} ) Van’t Hoff factor is: ( mathbf{A} cdot i=7 ) B. ( i=3 ) ( c cdot i=4 ) ( mathbf{D} cdot i=5 ) |
12 |

1530 | 5. A 5% solution of cane sugar (molecular weight = 342) is isotonic with a 1% solution of substance X. The molecular weight of X is a. 342 b. 171.12 c. 65.6 d. 136.8 |
12 |

1531 | The conductivity of 0.001 mol ( L^{-1} ) acetic acid is ( 5 times 10^{-5} s c m^{-1} ). Calculate it’s dissociation constant if ( lambda_{m}^{o} ) m for acetic ( operatorname{acid} ) is ( 250 operatorname{scm}^{2} m o l^{-1} ? ) |
12 |

1532 | Illustration 2.131 Two aqueous solution containing, respectively, 7 g urea (molar mass = 60 g) and 42 g of substance X in 100 g of water freeze at the same temperature. Calculate the molecular weight of X. |
12 |

1533 | The addition of 0.643 g of a compound to ( 50 mathrm{mL} ) of benzene (density ( 0.879 g m L^{-1} ) ) lowers the freezing point from 5.51 to ( 5.03^{circ} mathrm{C} . ) If ( K_{f} ) for benzene is ( mathbf{5 . 1 2} boldsymbol{K} / boldsymbol{m}, ) calculate the molecular weight of the compound. |
12 |

1534 | The strength of 11.2 volume solution of ( H_{2} O_{2} ) is: ( [ ) Given that molar mass of ( boldsymbol{H}=mathbf{1} boldsymbol{g} boldsymbol{m o l}^{-1} ) and ( boldsymbol{O}=mathbf{1 6} boldsymbol{g} boldsymbol{m o l}^{-1} mathbf{j} ) A . ( 13.6 % ) в. ( 3.4 % ) ( c .34 % ) D. ( 1.7 % ) |
12 |

1535 | The degree of dissociation of an electrolyte is ( alpha ) and its van’t Hoff factor is ( i ). The number of ions obtained by complete dissociation of 1 molecule of the electrolyte is: A. ( frac{i+alpha-1}{alpha} ) B. ( i-alpha-1 ) c. ( frac{i-1}{alpha} ) D. ( frac{i+alpha+1}{1-alpha} ) |
12 |

1536 | State Henry’s law and mention some important applications? |
12 |

1537 | 34. Vapour pressure of water at 293 K is 17.535 mm Hg. alculate the vapour pressure of water at 293 K when 25 g of glucose is dissolved in 450 g of water. As vapour pressure is changing, Apply Raoult’s law, for the relative l owering of vapour pressure to calculate vapour pressure of water. F |
12 |

1538 | ( 100 mathrm{ml} ) of liquid ( mathrm{A} ) and ( 25 mathrm{ml} ) of liquid ( mathrm{B} ) is mixed to give a solution which does not obey Raoult’s law. The volume of the solution: A. will be 125 ( mathrm{m} ) । B. can be > or < than 125 ( mathrm{m} ) c. can be greater than, equal to or less than ( 125 mathrm{m} ) D. will be less than 125 ( mathrm{m} ) । |
12 |

1539 | A 0.5 m solution could be prepared by dissolving 20 g NaOH in: A . 0.5 L water B. 0.5 kg water c. 1 L water D. 1 kg water E. 2 L water |
12 |

1540 | A monoprotic acid in a ( 0.1 mathrm{M} ) solution ionizes to ( 0.001 % ). Its ionization constant is: A ( cdot 1.0 times 10^{-3} ) В. ( 1.0 times 10^{-6} ) c. ( 1.0 times 10^{-8} ) D. ( 1.0 times 10^{-1} ) |
12 |

1541 | How many mL of a solution of concentration ( 100 mathrm{mg} ) Co( ^{2+} ) per mL is needed to prepare ( 10 mathrm{mL} ) of a solution of concentration ( 20 mathrm{mg} mathrm{Co}^{2+} ) per ( mathrm{mL} ) ? |
12 |

1542 | ( 10 % ) of urea is isotonic with ( 6 % ) solution of a non-volatile solute ( X . ) What is the molecular mass of solute ( boldsymbol{X} ) ? A ( cdot 6 g ) mol ( ^{-1} ) B. ( 60 g ) mol ( ^{-1} ) c. ( 36 g ) mol ( ^{-1} ) D. ( 32 g ) mol ( ^{-1} ) |
12 |

1543 | If ( N_{2} ) gas is bubbled through water at ( 293 K ), Calculate solubility of ( N_{2} ) gas? Assume that ( N_{2} ) exerts a partial pressure of 0.987 bar. Given that Henry’s law constant for ( N_{2} ) at ( 293 K ) is ( mathbf{7 6 . 4 8} frac{boldsymbol{k} text { bar }}{text { mole } / text { litre }} ) A ( cdot 1.29 times 10^{-5} ) litree В. ( _{1.29} times 10^{-4} frac{text { тоде }}{text { litre }} ) с. ( _{2.9} times 10^{-3} ) mole D. ( 2.9 times 10^{-5} ) mole |
12 |

1544 | Assertion Azeotropic mixtures are formed only by non-ideal solutions and they may have boiling points either greater than both the components or lesser than both the components. Reason The composition of the vapour phase is same as that of the liquid phase of an azeotropic mixture. A. Both Assertion and Reason are correct and Reason is the correct explanation for Assertion B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion C. Assertion is correct but Reason is incorrect D. Both Assertion and Reason are incorrect |
12 |

1545 | What osmotic pressure would the 1.25 molal sucrose solution exhibit at ( 25^{circ} mathrm{C} ) ? (The density of this solution is 1.34 ( g / m L ) ( mathbf{A} cdot 28.70 mathrm{atm} ) B. 30.22 atm c. 21.72 atm D. 24.55 atm |
12 |

1546 | A super saturated solution is a meta stable state of solution in which solute concentration: A. is equal to the solubility of that substance in water B. is more than its solubility c. is less than its solubility D. continuously changes |
12 |

1547 | ( 1.525 g ) of an organic compound was kjeblahlised and the ammonia so produced was passed through ( 30 m l ) of 1 ( N ) HCl.The remaining ( H C l ) was further neutralised by 120 ml of ( frac{N}{10} N a O H ) solution. Calculate the ( % ) nitrogen in the compound. |
12 |

1548 | The concentration of ( K^{+} ) ion in ( 0.1 mathrm{M} ) ( K_{2} C r_{2} O_{7} ) solution is ( x ) M. The value of ( 10 x ) is |
12 |

1549 | The boiling point of a solution containing ( 68.4 mathrm{g} ) of sucrose (molar ( left.operatorname{mass}=342 g operatorname{mol}^{-1}right) operatorname{in} 100 ) g of water is: ( left[K_{b} text { for water }=0.512 mathrm{K} mathrm{kg} text { mol}^{-1}right] ) A ( cdot 101.02^{circ} mathrm{C} ) B . ( 100.512^{circ} mathrm{C} ) c. ( 100.02^{circ} mathrm{c} ) D. ( 98.98^{circ} mathrm{C} ) |
12 |

1550 | Which of the following is most soluble? A ( cdot B i_{2} S_{3}left(K_{s p}=1 times 10^{-17}right) ) B . ( operatorname{MnS}left(K_{s p}=7 times 10^{-16}right) ) c. ( C u Sleft(K_{s p}=8 times 10^{-37}right) ) D. ( A g_{2} Sleft(K_{s p}=6 times 10^{-51}right) ) |
12 |

1551 | Illustration 2.109 Calculate the molal depression constant of a solvent which has a. Freezing point 16.6°C and latent heat of fusion 180.75 J g-1. b. Freezing point 20.0°C and latent heat of fusion 200.00 Jg-1 |
12 |

1552 | If the mole fraction of a solute is changed from ( frac{1}{4} ) to ( frac{1}{2} ) by adding some solute in 800 g of ( H_{2} O ) solvent, then the ratio of molarity of two solutions will be: A . 1: 3 B. 1: 4 ( c cdot 2: 3 ) D. 1: 2 |
12 |

1553 | State True or False. On hills, water boils quickly. A. True B. False |
12 |

1554 | If air is taken as a binary solution, the solvent is: ( A cdot N_{2} ) B. ( 0_{2} ) ( c cdot c O_{2} ) D. Ar |
12 |

1555 | Q. 41 Why are aquatic species more comfortable in cold water in comparision to warm water? |
12 |

1556 | The Henr’s law constant for ( mathrm{N}_{2}, mathrm{O}_{2} ) and ( mathrm{CO}_{2} ) in water are 1600,780 and 29 atm M-1, respectively. Which of these gases has the highest concentration in a sample of water at 25 degrees ( C ) when the gas pressure over the water is 1.0 atm? ( A cdot N_{2} ) B. 0,2 ( c cdot c O_{2} ) D. can’t tell without more information about the samples |
12 |

1557 | Solubility is the amount of the present in the saturated solution at a particular temperature A. solute B. solvent c. dispersed phase D. dispersed medium |
12 |

1558 | What will be the abnormal molecular ( operatorname{mass} ) of ( mathrm{K}_{3}left[mathrm{Fe}(mathrm{CN})_{6}right] . ) If in a aqueous solution it is ( 40 % ) dissociated? (Given, normal molecular weight of ( left.mathbf{K}_{3}left[mathbf{F e}(mathbf{C N})_{6}right] text { is } 329right) ) A . 149.54 B. 723.8 c. 82.25 D. 329.0 |
12 |

1559 | Which of the following solutions has the more capacity dissolve the solute in the solvent? A. Saturated solution B. Unsaturated solution c. super saturated solution D. None of the above |
12 |

1560 | Which gas is more soluble in water, ( boldsymbol{O}_{2} ) or ( N_{2} ? ) |
12 |

1561 | When ( C u S O_{4} ) is added to a solution of ammonia? A. Freezing point is lowered B. Freezing point is raised c. Boiling point is raised D. Both (1) and (2) |
12 |

1562 | Question 4. Concentration terms such as mass percentage, ppm, mole fraction and molality are independent of temperature. However, molarity is a function of temperature. Explain. |
12 |

1563 | Calculate the osmotic pressure at ( 25^{circ} mathrm{C} ) of a solution containing 1 g of glucose and 1 g of sucrose in 1 litre of solution. If it were not known that the solute was a mixture of glucose and sucrose, what would be the molecular weight of solute corresponding to the calculated osmotic pressure? |
12 |

1564 | How many grams of carbon dioxide gas is dissolved in a 1 L bottle of carbonated water if the manufacturer uses a pressure of 2.4 atm in the bottling process at ( 25^{circ} mathrm{C} ? ) Given: ( K_{H} ) of ( C O_{2} ) in water ( =29.76 ) |
12 |

1565 | Illustration 2.43 Liquids X and Y form an ideal solution. The vapour pressure of X and Y at 100°C are 300 and 100 mm of Hg, respectively. Suppose that a solution composed of 1 mol of X and 1 mol of Y at 100°C is collected and condensed. This condensate is then heated at 100°C and vapour is again condensed to form a liquid A. What is the mole fraction of X in A? |
12 |

1566 | (a) Give two differences between Ideal and non-Ideal solutions. (b) Find out osmotic pressure of Glucose solutions of ( 5 % ) solution at ( 25^{circ} mathrm{C} ) temperature while molecular mass of Glucose 180 and ( R=0.0821 ) Litre Atmosphere. |
12 |

1567 | Define the following terms: (i) Molality (m) (ii) Abnormal molar mass |
12 |

1568 | A mixture of ethyl alcohol and propyl alcohol has vapour pressure of ( 290 m m ) at ( 300 K . ) The vapour pressure of propyl alcohol is 200 mm. If mole fraction of ethyl alcohol is 0.6 its vapour presssure at same temperature will be:- A . 360 в. 350 ( c .300 ) D. 700 |
12 |

1569 | The mole fraction of ( C_{2} H_{4} ) in the mixture is : A . 0.25 в. 0.75 ( c .0 .45 ) D. 0.55 |
12 |

1570 | A solution of known concentration is known as: A. molar solution B. normal solution C. mole solution D. standard solution |
12 |

1571 | For strong electrolytes, van’t Hoff factor i’ equals to total number of (ions/atoms) in the formula unit |
12 |

1572 | A solution made by dissolving 0.32 g of a new compound in 25 g of water has freezing point ( -2.201^{circ} mathrm{C} . ) Calculate the molecular mass of the new compound. A . 218.4 в. ( 118 . ) c. 318.4 D. 10.81 |
12 |

1573 | If two liquids ( A ) and ( B ) form minimum boiling azeotrope at some specific composition then: A. ( A ) -B interactions are stronger than those between ( A-A ) or B-B B. vapour pressure of solution increases because more number of molecules of liquids ( A ) and ( B ) can escape from the solution C. vapour pressure of solution decreases because less number of molecules of liquids ( A ) and ( B ) can escape from the solution D. show a large positive deviation from Raoult’s law |
12 |

1574 | Column II gives method to separate phases mentioned in column I. Match them and select the correct answer from the codes given below. Column Column I (a) Miscible liquids (p) Distillation ( (q) ) (b) Immiscible liquids ( quad ) Crystallization (c) Pure copper sulphate from ( (r) ) an impure sample Sublimation (s) Separating (d) Salt and ammonium chloride funnel ( A cdot(a)-(q),(b)-(s),(c)-(p),(d)-(r) ) B. ( (a)-(p),(b)-(s),(c)-(q),(d)-(r) ) ( c cdot(a)-(r),(b)-(s),(c)-(p),(d)-(q) ) D. (a) – (r), (b) – (s), (c) – (q), (d) – (p) |
12 |

1575 | A solution that obeys Raoult’s law is: A. non-ideal B. colliod ( c . ) ideal D. saturate |
12 |

1576 | For an ideal liquid solution, which of the following is unity? A. Activity coefficient B. Fugacity coefficient c. Fugacity D. Activity |
12 |

1577 | Tlustration 2.116 On dissolving 0.25 g of a non-volatile substance in 30 mL benzene (density 0.8 g mL-‘), its freezing point decreases by 0.25°C. Calculate the molecular mass of non-volatile substance (K, = 5.1 K kg mol-?). |
12 |

1578 | ( 5 g ) of ( N a C l ) can be dissolved in ( 50 g ) water Then the solubility of ( N a C l ) is: ( mathbf{A} cdot 10 g ) B. ( 5 g ) c. ( 20 g ) D. none of the above |
12 |

1579 | What is the quantity of NaOH present in ( 250 mathrm{cc} ) of the solution, so that it gives a ( mathrm{pH}=13 ? ) A ( cdot 10^{-13} mathrm{g} ) B . ( 10^{-1} mathrm{g} ) ( c .1 .0 mathrm{g} ) D. ( 4.0 mathrm{g} ) |
12 |

1580 | In 1 L saturated solution of ( A g C lleft[K_{s p}(A g C l)=1.6 times 10^{10}right], 0.1 mathrm{mol} ) of ( boldsymbol{C u} boldsymbol{C l}left[boldsymbol{K}_{s p}(boldsymbol{C u} boldsymbol{C l})=mathbf{1 . 0} times mathbf{1 0}^{-mathbf{6}}right] ) is added. The resultant concertraion of ( A g^{+} ) in the solution is ( 1.6 times 10^{-x} ). The value of ( x ) is: |
12 |

1581 | A ( 10 % ) (w/w) solution of cane sugar has undergone partial inversion according to the reaction: sucrose ( + ) water ( rightarrow ) glucose ( + ) fructose The boiling point of the solution is ( 100.7^{circ} mathrm{C} . ) What fraction of sugar has inverted? ( left[boldsymbol{K}_{boldsymbol{b}}left(boldsymbol{H}_{mathbf{2}} boldsymbol{O}right)=mathbf{1 . 8} boldsymbol{K} boldsymbol{g} boldsymbol{K} boldsymbol{m o l}^{-1}right] ) A. 0.5 B. 0.2 ( c cdot 0.3 ) D. 0.4 |
12 |

1582 | For an infinitely dilute aqueous solution, molality will be equal to: A. formality B. molarity c. mole fraction D. ppm |
12 |

1583 | Illustration 2.152 What will happen if pressure greater than the osmotic pressure is applied on the solution separated by a semi-permeable membrane from the solvent? |
12 |

1584 | When ( C a(O H)_{2} ) attains solubility equilibrium, the: A. solution is saturated B. ( p H ) will be less than 7 C . trial ( K_{s p} ) is less than the ( K_{s p} ) D. concentrations of the ions are equal |
12 |

1585 | The osmotic pressure of a ( 5 % ) solution of cane sugar (molecular mass 342 ) at ( 15^{circ} C ) is: ( A cdot 3.46 ) atm B. 3.64 atm c. 4.0 atm D. 2.45 atm |
12 |

1586 | The latent heat of fusion of ice is 80 calories per gram at ( 0^{circ} ) C. What is the freezing point of a solution of KCl in water containing 7.45 grams of solute 500 grams of water, assuming that the salt is dissociated to the extent of ( 95 % ? ) ( mathbf{A} cdot T_{f}=-0.73^{circ} mathrm{C} ) B. ( T_{f}=-0.92^{circ} mathrm{C} ) c. ( T_{f}=-1.46^{circ} mathrm{C} ) ( mathbf{D} cdot T_{f}=-1.84^{circ} mathrm{C} ) |
12 |

1587 | Some substances completely disappear or dissolve in water. We say that these substances are in water. A . immiscible B. soluble c. insoluble D. none of the above |
12 |

1588 | The volume of ( 1.5 mathrm{M} mathrm{H}_{2} mathrm{SO}_{4} ) required to completely neutralize ( 150 mathrm{mL} ) of ( 2 mathrm{M} ) NaOH solution is A . 150 ( mathrm{mL} ) B. 200 mL ( c .100 mathrm{mL} ) D. 250 mL |
12 |

1589 | The mole fraction of a solute in a solution is ( 0.1 . ) At ( 298 mathrm{K} ), molarity of this solution is the same as its molality Density of this solution at ( 298 K ) is ( 2.0 g mathrm{cm}^{-3} . ) The ratio of the molecular weights of the solute and solvent, ( left(frac{M W_{text {solute}}}{M W_{text {solvent}}}right) ) is: |
12 |

1590 | The molarity of 600 g ( H_{2} ) O is ? A. 50 B. 55.5 M c. 33.10 D. Cannot be calculated |
12 |

1591 | 0.61 How can you remove the hard calcium carbonate layer of the egg without damaging its semipermeable membrane? Can this egg be inserted into a bottle with a narrow neck without distorting its shape? Explain the process involved. Thinking Process The question can be answered using the concept of solubility, osmosis, reverse-osmosis, hypertonic solution and hypotonic solution |
12 |

1592 | The vapour pressure of ethanol and methanol are ( 44.5 mathrm{mm} ) and ( 88.7 mathrm{mm} mathrm{Hg} ) respectively. An ideal solution is prepared at the same temperature by mixing 60 g of ethanol with 40 gof methanol. The total vapour pressure of the solution is: A. ( 67.13 mathrm{mm} ) Hg B. 66.13 ( mathrm{mm} ) Нв c. ( 76.13 mathrm{mm} ) нв D. None of the above |
12 |

1593 | ( 5.5 m g ) of nitrogen gas dissolves in ( 180 g ) of water at ( 273 K ) and one atm pressure due to nitrogen gas. The mole fraction of nitrogen in ( 180 g ) of water at 5 atm nitrogen pressure is approximately: A ( cdot 1 times 10^{-5} ) B. ( 1 times 10^{-4} ) c. ( 1 times 10^{-6} ) D. ( 1 times 10^{-3} ) |
12 |

1594 | Find the correct statement about the solubility of a solution? A. Gases decrease in solubility with an increase in temperature B. ( N a C l ) is insoluble in water ( mathbf{C} cdot P b l_{2} ) is soluble in water D. All nitrates are insoluble in water E. Solubility depends solely upon the amount of solvent used |
12 |

1595 | (i) What is meant by positive deviations from Raoult’s Law ? Give an example. (ii) What is the sign of ( Delta_{m i x} H ) for positive derivation? |
12 |

1596 | At ( 25^{circ} C, ) the total pressure of an ideal solution obtained by mixing 3 mole of ( A ) and 2 mole of ( mathrm{B} ), is 184 torr. What is the vapour pressure (in torr) of pure ( mathrm{B} ) at the same temperature (Vapour pressure of pure ( A ) at ( 25^{circ} C ) is 200 torr.)? A . 180 B. 160 ( c cdot 16 ) D. 100 |
12 |

1597 | For an ideal binary liquid solution with ( P_{A}^{circ}>P_{B}^{circ}, ) which relation between ( X_{A} ) (mole fraction of ( A ) in liquid phase) and ( Y_{A}(text { mole fraction of } A text { in vapour phase }) ) is correct? ( mathbf{A} cdot Y_{A}X_{B} ) c. ( frac{Y_{A}}{Y_{B}}>frac{X_{A}}{X_{B}} ) D. ( frac{T_{A}}{Y_{B}}<frac{X_{A}}{X_{B}} ) |
12 |

1598 | At ( 25^{circ} C, ) the vapour pressure of methyl alcohol is 96.0 torr. The mole fraction of ( C H_{3} O H ) in solution in which the (partial) vapor pressure of ( boldsymbol{C} boldsymbol{H}_{3} boldsymbol{O H} ) is 23.0 torr at ( 25^{circ} C ) is ( frac{x}{y} . ) Find ( y-x ) |
12 |

1599 | A 0.4 molal aqueous solution of ( boldsymbol{M}_{boldsymbol{x}} boldsymbol{A} ) has freezing point ( 3.72^{circ} mathrm{C} ). The ( K_{f} ) of ( H_{2} O ) is ( 1.86 K m o l a l i t y^{-1} . ) The value of ( x ) is : |
12 |

1600 | Calculate the concentration of ( C O_{2} ) in a soft drink that is bottled with a partial pressure of 4 atm over the liquid at ( 25^{circ} mathrm{C} . ) The Henry’s law constant for ( C O_{2} ) in water at ( 25^{circ} mathrm{C} ) is ( 3.1 times ) ( 10^{-2} ) atm / mole ( – ) litre. A. 0.129 mol/litre в. 129.03 mol/litre c. 0.224 mol / litre D. 224.3 mol/litre |
12 |

1601 | Q. 26 Kh value for Ar(g), CO2 (g), HCHO (g) and CH. (g) are 40.39, 1.67, 1.83 x 10-5 and 0.413 respectively. Arrange these gases in the order of their increasing solubility. (a) HCHO < CH, <CO, < Ar (b) HCHO < CO, < CH, < AT (c) A < CO,< CH < HCHO (d) AC – CH = CO2 < HCHO Thinking Process Higher the value of Ky at a given pressure, the lower is the solubility of the gas in the liquid |
12 |

1602 | The vapour pressure of a solution having ( 2.0 g ) of solute ( X ) (gram atomic ( left.operatorname{mass}=32 g operatorname{mol}^{-1}right) operatorname{in} 100 g ) of ( C S_{2} ) (vapour pressure ( =854 text { torr }) ) is 848.9 torr. The molecular formula of the solute is: ( mathbf{A} cdot X ) в. ( X_{2} ) ( c cdot X_{4} ) D. ( X_{8} ) |
12 |

1603 | Illustration 2.159 18 g glucose and 6 g urea are dissolved in 1 L aqueous solution at 27°C. The osmotic pressure of the solution will be a. 8.826 atm b. 4.926 atm c. 2.92 atm d. 4.42 atm |
12 |

1604 | I. ( 2 M n^{2+}(a q)+4 O H^{-}(a q)+ ) ( O_{2}(g) rightarrow 2 M n O_{2}(s)+2 H_{2} O(l) ) II. ( M n O_{2}(s)+2 I^{-}(a q)+ ) ( 4 H^{+}(a q) rightarrow M n^{2+}(a q)+I_{2}(a q)+ ) ( 2 H_{2} O(l) ) III. ( 2 S_{2} O_{3}^{2-}(a q)+I_{2}(a q) rightarrow ) ( boldsymbol{S}_{4} boldsymbol{O}_{mathbf{6}}^{2-}(boldsymbol{a} boldsymbol{q})+boldsymbol{2} boldsymbol{I}^{-}(boldsymbol{a} boldsymbol{q}) ) Dissolved oxygen in water is determined by using the given redox reactions.When ( 3 times 10^{3} ) moles ( O_{2} ) is dissolved per litre of water, then what will be the molarity of ( I^{-} ) produced in the given reaction? A ( cdot 3 times 10^{-3} ) М В. ( 4 times 3 times 10^{-3} mathrm{M} ) c. ( 2 times 3 times 10^{-3} ) М D. ( frac{1}{2} times 3 times 10^{-3} mathrm{M} ) |
12 |

1605 | What will be the molality of a solution of glucose in water which is ( 10 % boldsymbol{w} / W ? ) ( mathbf{A} cdot 0.01 m ) в. 0.617 т ( c .0 .668 m ) D. 1.623 m |
12 |

1606 | If a solute under goes dimerization and trimerization, the minimum values of the vant Hoff factors are: A. 0.50 and 1.50 B. 1.50 and 1.33 ( c .0 .50 ) and 0.33 D. 0.25 and 0.67 |
12 |

1607 | A soluction contains ( 7 g ) of solute (molar ( operatorname{mass} 210 g operatorname{mol}^{-1} ) ) in ( 350 g ) of acetone raised the boiling point of acetone from ( 56^{circ} C ) to ( 56.3^{circ} C ) The value of ebullioscopic constant of acetone in ( K . K g m o l^{-1} ) is: A . 2.66 в. 3.15 c. 4.12 D. 2.86 |
12 |

1608 | Number of moles of the solute per kilogram of the solvent is: A. mole fraction B. molality c. molarity D. molar mass |
12 |

1609 | Two closed vessels of an equal volume containing air at pressure ( P_{1} ) and temperature ( T_{1} ) are connected to each other through a narrow tube. If the temperature in one of the vessels is now maintained at ( T_{1} ) and that in the other at ( T_{2}, ) what will be the pressure in the vessels? A ( cdot frac{2 P_{1} T_{1}}{T_{1}+T_{2}} ) в. ( frac{T_{1}}{2 P_{1} T_{2}} ) c. ( frac{2 P_{1} T_{2}}{T_{1}+T_{2}} ) D. ( frac{2 P_{1}}{T_{1}+T_{2}} ) |
12 |

1610 | 7. The vapour pressure at a given temperature of an ideal solution containing 0.2 mol of non-volatile solute and 0.8 mol of a solvent is 60 mm of Hg. The vapour pressure of the pure solvent at the same temperature will be a. 120 mm Hg b. 150 mm Hg c. 60 mm Hg d. 75 mm Hg |
12 |

1611 | Which of the following liquid pairs shows a positive deviation from Raoults law? A. Water hydrochloric acid B. Acetone chloroform c. water nitric acid D. Benzene methanol |
12 |

1612 | Sulphuric acid is ( 95.8 % ) by mass. Calculate mole fraction of ( boldsymbol{H}_{2} boldsymbol{S} boldsymbol{O}_{4} ) of density ( 1.91 mathrm{cm}^{-3} .(H=1, S= ) ( mathbf{3 2}, boldsymbol{O}=mathbf{1 6}) ) A . 0.8950 B. 0.2982 c. 0.2056 D. 0.8075 |
12 |

1613 | Hlustration 2.33 The vapour pressure of methyl alcohol at 298 K is 0.158 bar. The vapour pressure of this liquid in solution with liquid B is 0.095 bar. Calculate the mole fraction of methyl alcohol in the solution if the mixture obeys Raoult’s law. |
12 |

1614 | ( 4.28 mathrm{g} ) of ( mathrm{NaOH} ) is dissolved in water and the solution is made to 250 cc. What will be the molarity of the solution? A . 0.615 mol ( L^{-1} ) B. 0.428 mol ( L^{-1} ) c. 0.99 mol ( L^{-1} ) D. 0.301 mol ( L^{-1} ) |
12 |

1615 | Deliquescent substances absorb moisture from the air ( & ) changes into a solution. A. True B. False |
12 |

1616 | The equilibrium constant for the reaction: ( N_{2(g)}+3 H_{2(g)} rightleftharpoons 2 N H_{3(g)} ) at ( mathbf{7} 15 K, ) is ( 6.0 times 10^{-2} . ) If, in a particular reaction, there are 0.25 mol ( L^{-1} ) of ( H_{2} ) and ( 0.06 m o l L^{-1} ) of ( N H_{3} ) present calculate the concentration of ( N_{2} ) at equilibrium. |
12 |

1617 | Illustration 2.53 Two liquids X and Y boil at 110°C and 130°C, respectively. Which one of them has higher vapour pressure at 50°C? |
12 |

1618 | Illustration 2.207 Acetic acid associates in benzene to form a dimer. 1.65 g of acetic acid when dissolved in 100 g of benzene raised the boiling point by 0.36°C. Calculate the Van’t Hoff factor and degree of association of acetic acid. (K, for benzene = 2.57°C m-1) |
12 |

1619 | The depression in freezing point is maximum if the solvent used is: A. Camphor B. Naphthalene c. Benzene D. water |
12 |

1620 | Can a solution be heterogeneous? | 12 |

1621 | The initial pressure inside the flask is: A. near zero (vacuum) В. 27 тт Н( g ) c. 760 mm ( H g ) D. ( (760-27) ) mm ( H g ) |
12 |

1622 | Which of the following will show a negative deviation from Raoult’s law? A. Acetone-benzene B. Acetone-ethanol c. Benzene-methanol D. Acetone-chloroform |
12 |

1623 | Mass of glucose in ( g ) must be present in 0.5 litre of a solution for its osmotic pressure be same as that of 8 g glucose in 1 litre is : |
12 |

1624 | Example 2.1 Calculate the mole fraction of solute in a dilute aqueous solution from which ice begins to separate out at -0.46°C. (K, of H,0 = 1.86 Km-l) |
12 |

1625 | Illustration 2.47 Calculate the vapour pressure lowering of a 0.1 m aqueous solution of non-electrolyte at 75°C. AH = 9.720 kcal mol-1, P, = 742.96 torr |
12 |

1626 | At ( 20^{circ} C ) the vapour pressure of ( C H_{3} O H ) and ( C_{2} H_{5} O H ) is ( 94 mathrm{mm} ) and ( 44 mathrm{mm}, ) respectively. If 20 g of ( C H_{3} O H ) is mixed with 100 g |
12 |

1627 | A solution of sulphuric acid in water exhibits: A. negative deviations from Raoult’s law B. positive deviations from Raoult’s law c. ideal properties D. the applicability of Henry’s law |
12 |

1628 | The boiling point of liquid ( A, B, C ) and ( D ) ( operatorname{are} 80^{circ} C, 60^{circ} C, 90^{circ} C ) and ( 100^{circ} C ) respectively. Which will show highest vapour pressure at room temperature? ( A cdot A ) B. B ( c cdot c ) ( D . ) D |
12 |

1629 | ( M X_{2} ) dissociates in ( M^{2+} ) and ( X^{-} ) ions in an aqueous solution with a degree of dissociation ( 0.5(alpha) . ) The ratio of the observed depression of the freezing point of the aqueous solution to the value of the depression of freezing point in the absence of ionic dissociation is |
12 |

1630 | Calculate mole fraction of solute if molarity of solution is ( 20 %left(frac{W %}{W}right) ) aqueous solution of NaOH. A. 0.2 B. 0.15 c. ( 0 . ) D. none of these |
12 |

1631 | Which of the following are correct about mixture of two miscible liquids forming azeotopes? This question has multiple correct options A. Has the lowest temperature at which the two liquids can exist in the liquid state B. Has the lowest temperature attainable at which two liquids forms eutectic mixture C. Eutectic point has found application to attain low melting point solids which are eutectic mixture D. Composition of azeotrope and their b.pt. vary with the external pressure |
12 |

1632 | Why doesn’t sea water freeze so easily? | 12 |

1633 | Statement ( 1: A ) salt dissolved in an organic solvent will be a good electrical conductor. Statement 2: Salts will not dissolve appreciably in an organic solvent. A. Statement 1 and Statement 2 are correct and Statement 2 is the correct explanation of Statement 1 B. Both the Statement 1 and Statement 2 are correct, but Statement 2 is not the correct explanation of Statement 1. c. statement 1 is correct, but statement 2 is not correct D. Statement 1 is not correct, but Statement 2 is correct |
12 |

1634 | If ( N_{2} ) gas bubbled through water at ( 293 K ) how many millimoles of ( N_{2} ) gas would dissolve in 1 litre of water? Assume that exerts a partial pressure |
12 |

1635 | illustration 2.133 The freezing point of 0.08 molal NaHSO4 is -0.345°C. Calculate the percentage of HSO, ions that transfers a proton to water. Assume 100% ionization of NaHSO, and K, for H,0 = 1.86 K molality: |
12 |

1636 | . 19 Which of the following solutions have the same concentration? (a) 20 g of NaOH in 200 mL of solution (b) 0.5 mol of KCl in 200 mL of solution (C) 40 g of NaOH in 100 mL of solution (d) 20 g of KOH in 200 mL of solution |
12 |

1637 | Which of the following shows positive deviation from Raoult’s law? A. ( C_{6} H_{6} ) and ( C_{6} H_{5} C H_{3} ) B . ( C_{6} H_{6} ) and ( C C l_{4} ) c. ( C H C l_{3} ) and ( C_{2} H_{5} O H ) D. ( C H C_{3} ) and ( C H_{3} C O C H_{3} ) |
12 |

1638 | The vapour pressure is least for? A. pure water B. ( 0.1 mathrm{m} ) aqueous urea c. ( 0.2 mathrm{m} ) aqueous urea D. 0.3m aqueous urea |
12 |

1639 | 1 Which of the following units is useful in relating concentration of solution with its vapour pressure? (a) Mole fraction (b) Parts per million (c) Mass percentage (d) Molality An ution in oronortional to the |
12 |

1640 | On mixing, heptane and octane form an ideal solution. At ( 373 mathrm{K} ), the vapour pressure of the two liquid components (heptane and octane) are ( 105 mathrm{kPa} ) and 45 kPa respectively. Vapour pressure of the solution obtained by mixing 25 g of heptane and 35 g of octane will be : (molar mass of heptane ( =100 ) g ( m o l^{-2} ) and of octane ( =114 ) g ( m o l^{-1} ) A ( .96 .2 k P a ) в. ( 144.5 k P a ) c. ( 72 k P a ) D. ( 36.1 k P a ) |
12 |

1641 | Which one has same Van’t Hoff factor ( ‘ i^{prime} ) as that of ( boldsymbol{H} boldsymbol{g}_{2} boldsymbol{C l}_{2} ) ? A . ( N a C l ) в. ( N a_{2} S O_{4} ) c. ( A lleft(N O_{3}right)_{3} ) D. ( A l_{2}left(S O_{4}right)_{3} ) |
12 |

1642 | Excess of ( K l ) was added to ( 100 m l H_{2} O_{2} ) solution of unknown strength along with sufficient ( boldsymbol{H}_{2} boldsymbol{S} boldsymbol{O}_{4} ) lodine liberated was titrated against ( 40 m l ) of ( 0.1 M ) hypo solution. The concentration of ( boldsymbol{H}_{2} boldsymbol{O}_{2} ) solution is: A ( .0 .04 mathrm{N} ) в. 0.04 М c. ( 0.68 g m / L ) D. ( 0.02 mathrm{M} ) |
12 |

1643 | 0.2 molal acid ( H X ) is ( 20 % ) ionised in solution. ( boldsymbol{K}_{boldsymbol{f}}=mathbf{1 . 8 6 K} ) molality ( ^{-1} ). The freezing point of the solution is: A. ( -0.45^{circ} mathrm{C} ) B . ( -0.90^{circ} mathrm{C} ) c. ( -0.31^{circ} mathrm{C} ) D. ( -0.53^{circ} mathrm{C} ) |
12 |

1644 | For which among the following equimolar aqueous solutions Van’t Hoff factor has the lowest value? A. Aluminium Chloride B. Potassium Sulphate c. Ammonium chloride D. urea |
12 |

1645 | Illustration 2.142 Define osmotic pressure. | 12 |

1646 | A solution ( X ) is prepared by dissolving three moles of glucose in one litre of water and a solution Y is prepared by dissolving 1.5 moles of sodium chloride in one litre of water. Will the osmotic pressure of ( mathrm{X} ) be higher, lower or equal to that of Y? Give a reason for your answer |
12 |

1647 | 0.1 normal solution of ( N a C l ) is found to be isotonic with ( 1.1 % ) solution of Urea. Calculate the apparent degree of ionisation of ( N a C l ) ( mathbf{A} cdot 0.083 ) B. 8.3 c. 0.83 D. 0.42 |
12 |

1648 | Illustration 2.166 A solution is prepared by dissolving 1.08 g of human serum albumin, a protein obtained from blood plasma, in 50 cm of aqueous solution. The solution has an osmotic pressure of 5.85 mm Hg at 298 K. a. What is the molar mass of albumin? b. What is the height of water column placed in solution? d99,0) = 1 g cm-3 |
12 |

1649 | Loss of a beta particle is equivalent to: A. increase of one neutron only B. decrease of one neutron only ( c . ) both 1 and 2 D. none of these |
12 |

1650 | The freezing point of aqueous solution that contains ( 3 % ) urea, ( 7.45 % K C l ) and ( 9 % ) of glucose is: ( left(operatorname{given} K_{1} text { of water }=right. ) 1.86 and assume molarity ( = ) molality ). A . ( 290 K ) в. 285.5 К c. ( 267.42 K ) D. 250 K |
12 |

1651 | Prachi makes a saturated solution of potassium chloride in water at ( 353 mathrm{K} ) and leaves the solution to cool at room temperature. What would she observe as the solution cools? Explain. |
12 |

1652 | The freezing point of a solution containing 0.2 g of acetic acid in 20.0 g benzene is lowered by ( 0.45^{circ} mathrm{C} ). The degree of association of acetic acid in benzene is: [Assume acetic acid dimerizes in benzene and ( K_{f} ) for benzene ( =mathbf{5 . 1 2} mathbf{K} ) ( left.mathrm{kg} mathrm{mol}^{-1}right] ) A. ( 94.5 % ) B . ( 54.9 % ) c. ( 78.2 % ) D. 100% |
12 |

1653 | The osmotic pressure of a solution of benzoic acid dissolved in benzene is less than expected because A. benzoic acid is an organic solute B. benzene is a non-polar solvent c. benzoic acid dissociates in benzene D. benzoic acid gets associated in benzene |
12 |

1654 | Illustration 2.199 Following are equimolal aqueous solutions: a. 1 m urea b. 1 m KCI c. 1 m MgCl2 d. 1 m Na,PO4 Arrange them in increasing i. Boiling point Ïi. Freezing point ü. Osmotic pressure iv. Vapour pressure |
12 |

1655 | Which of the following units could be used to describe solubility? ( A cdot g / s ) в. ( g / l ) ( c cdot k g / s ) D. mol/s |
12 |

1656 | i). State Raoult’s Law. ii). The vapour pressure of pure benzene at a certain temperature is 0.850 bar. ( A ) non-volatile non-electrolyte solid weighing 0.5 g when added to 39.0 gof benzene (molar mass 78 g ( m o l^{-1} ) ). Vapour pressure of the solution, then is 0.845 bar. What is the molar mass of the solid substance? |
12 |

1657 | By adding a non-volatile salute into a solution vapour pressure is reduces. | 12 |

1658 | The vapour pressures of two liquids ( A ) and B in their pure states are in the ratio of ( 1: 2 . ) A binary solution of ( A ) and ( B ) contains ( A ) and ( B ) in the mole proportion of ( 1: 2 . ) The mole fraction of ( A ) in the vapour phase of the solution will be: A . 0.33 B. 0.2 c. 0.25 D. 0.52 |
12 |

1659 | For the standardization of ( B a(O H)_{2} ) solution, 0.204 g of potassium acid phthalate was weighed which was then titrated with ( B a(O H)_{2} ) solution. The titration indicated equivalence at 25.0 ( mathrm{ml} ) of ( B a(O H)_{2} ) solution. The reaction involved is: ( boldsymbol{K} boldsymbol{H} boldsymbol{C}_{8} boldsymbol{H}_{4} boldsymbol{O}_{4}+boldsymbol{B} boldsymbol{a}(boldsymbol{O} boldsymbol{H})_{2} rightarrow boldsymbol{H}_{2} boldsymbol{O}+ ) ( boldsymbol{K}^{+}+boldsymbol{B} boldsymbol{a}^{2+}+boldsymbol{C}_{8} boldsymbol{H}_{4} boldsymbol{O}_{4}^{2-} ) The molarity of the base solution is ( (K= ) 39) A. ( 0.04 mathrm{M} ) в. о.озм c. о.о२м D. 0.01M |
12 |

1660 | At ( 20^{circ} mathrm{C} ) and a pressure of 1 atm each gas, 1 litre of water dissolves 0.043 g of pure ( O_{2} ) or 0.019 g of pure ( N_{2} . ) Assuming that dry air is composed of ( 20 % mathrm{O}_{2} ) and ( 80 % N_{2} ) (by volume) determine the masses of ( boldsymbol{O}_{2} ) and ( boldsymbol{N}_{2} ) dissolved by 1 litre of water at ( 20^{circ} mathrm{C} ) exposed to air at a total pressure of 1 atm. Assume ( V . P . ) of ( H_{2} ) at ( 20^{circ} C ) be ‘b’ atm A ( cdot O_{2}=4.3 times 10^{-3} g / L, N H 2=0.75 times 10^{-2} g / L ) B. ( O_{2}=5.25 times 10^{-4} g / L, N H 2=1.7 times 10^{-3} g / L ) C ( cdot O_{2}=8.6 times 10^{-3} g / L, N H 2=1.5 times 10^{-2} g / L ) D. ( O_{2}=10.5 times 10^{-4} g / L, N H 2=3.4 times 10^{-3} g / L ) |
12 |

1661 | Mass ( % ) of carbon in ethanol is: A . 52 B. 13 c. 34 D. 90 E . 80 |
12 |

1662 | A complex is represented as ( mathrm{CoCl}_{3} cdot x N H_{3} ) its 0.1 molal solution in aq. solution shows ( Delta T_{f}=0.558^{0} C . K_{f} ) for ( boldsymbol{H}_{2} boldsymbol{O} ) is ( 1.86 boldsymbol{K} boldsymbol{m o l}^{-1} boldsymbol{k g} . ) Assuming ( 100 % ) ionisation of complex and coordination no. of ( C o ) is six, calculate formula of complex. |
12 |

1663 | Give an example of a solid solution in which the solute is a gas. | 12 |

1664 | Which solutions have a concentratoin of ( 1.0 mathrm{M} ? ) i. 74 grams of calcium hydroxide dissolved to make 1 liter of Solution ii. 74.5 grams of potassium chloride dissolved to maek 1 liter of Solution iii. 87 grams of lithium bromide dissolved to make 1 liter of solution A. i only B. iii only c. i and iii only D. ii and iii only E. i, ii and iii |
12 |

1665 | The phenol-water system has a upper critical solution temperature. A. True B. False |
12 |

1666 | wustration 2.79 Equal amounts of a solute are dissol in equal amounts of two solvents A and B. The lowering of vapour pressure for solution A has twice the lowering of vapour pressure for solution B. If MwA and Mws are the molecular weights of solvents A and B, respectively, then a. Mwa = MWB b. Mwa = Mwg/2 c. Mw = 4Mw d. Mw = 2MWB And D |
12 |

1667 | ( boldsymbol{C u} boldsymbol{S O}_{4} cdot boldsymbol{5} boldsymbol{H}_{2} boldsymbol{O}(s) rightleftharpoons boldsymbol{C u S O}_{4} cdot boldsymbol{3} boldsymbol{H}_{2} boldsymbol{O}(boldsymbol{s}) ) ( +2 H_{2} O(g) ; K_{p}=4 times 10^{-4} a t m^{2} ) if the vapour pressure of water is 38 torr then percentage of relative humidity is: Assume all data at constant temperature) ( mathbf{A} cdot mathbf{4} ) B. 10 c. 40 D. none of these |
12 |

1668 | A mixture of chlorobenzene and wate (immiscible) boils at ( 90.3^{circ} mathrm{C} ) at an external pressure of ( 740.2 mathrm{mm} . ) The vapour pressure of pure water at ( 90.3^{circ} mathrm{C} ) is ( 530.1 mathrm{mm} ). Calculate the ( % ) composition of distillate: A. ( H_{2} O=35 % ) в. ( H_{2} O= ) 22% c. ( H_{2} O= ) २९% ( %= ) D. ( H_{2} O=71 % ) |
12 |

1669 | Calculate the molarity of each of the following: (a) ( 30 g ) of ( C oleft(N O_{3}right)_{2} .6 H_{2} O ) in ( 4.3 L ) of solution (b) ( 30 m L ) of 0.5 ( M H_{2} S O_{4} ) diluted to ( 500 m L ) |
12 |

1670 | Total vapour pressure of mixture of mol of ( Aleft(P_{A}^{0}=150 text { tor } rright) ) and 2 mol of ( B ) ( left(P_{B}^{0}=240 text { tor } rright) ) is 200 torr. In this case A. there is positive deviation from Raoult’s law B. there is negative deviation from Raoult’s law c. there is no deviation from Raoult’s law D. molecular masses of A and B are also required for calculating the deviation |
12 |

1671 | Which of the following would show the LARGEST increase in solubility with increasing pressure based on intermolecular force knowledge? ( A ). Ammonia B. Calcium oxide c. Potassium bromide D. Sodium hydroxide |
12 |

1672 | Which characteristics the weak inter molecular forces of attraction in a liquid? A. High boiling point B. High vapour pressure c. High critical temperature D. High heat of vapourisation |
12 |

1673 | A storage battery contains a solution of ( H_{2} S O_{4} 38 % ) by weight. What will be the Van’t Hoff factor if the ( boldsymbol{Delta} boldsymbol{T}_{f text {experiment}} ) is ( mathbf{2 9 . 0 8} .left[text { Given } boldsymbol{K}_{f}=mathbf{1}right. ) B . ( i=2.5 ) c. ( i=3 ) D. ( i=3.5 ) |
12 |

1674 | (a) Explain the following (i) Henry’s law about a dissolution of a gas in a liquid. (ii) Boiling paint elevation constant for a solvent. (b) A solution of glycerol ( left(C_{3} H_{8} O_{3}right) ) in water was prepared by dissolving some glycerol in 500 g of water. This solution has a boiling point of ( 100.42^{circ} mathrm{C} ). What mass of glycerol was dissolved to make this solution? ( left(K_{b} text { for water }=0.512 mathrm{K} mathrm{kg}right. ) ( left.operatorname{mol}^{-1}right) ) |
12 |

1675 | The mole fraction of water in ( 20 % ) (wt. ( / ) wt.) aqueous solution of ( boldsymbol{H}_{2} boldsymbol{O}_{2} ) is: A ( cdot frac{77}{68} ) в. ( frac{68}{77} ) c. ( frac{20}{80} ) D. ( frac{80}{20} ) |
12 |

1676 | Example 2.14 A solution containing 0.1 mol of naphthalene and 0.9 mol of benzene is cooled out until some benzene freezes out. The solution is then decanted off from the solid and warmed upto 353 K where its vapour pressure was found to be 670 mm. The freezing point and boiling point of benzene are 278.5 K and 353 K respectively, and its enthalpy of fusion is 10.67 kJ mol-1. Calculate the temperature to which the solution was cooled originally and the amount of benzene that must have frozen out. Assume ideal behaviour. |
12 |

1677 | How much water must be added to 0.50 litre of ( 6.0 mathrm{M} ) H ( C l ) to make the solution 2.0M ? Answer in liters. A . 0.33 B. 0.50 c. ( 1 . ) D. 1.5 E . 2.0 |
12 |

1678 | Define cryoscopic constant. | 12 |

1679 | For a solution of a non-electrolyte in water, the Van’t Hoff factor is : A. Always equal to 0 в. ( leq 1 ) c. Always equal to D. ( >1 ) but ( <2 ) |
12 |

1680 | The osmotic pressure of ( 400 mathrm{ml} ) urea and ( 600 mathrm{ml} ) glucose solutions are respectively 0.3 atm and 0.4 atm. The osmotic pressure of the solution obtained by mixing them will be? A. 0.24 atm B. 0.36 atm c. 0.48 atm D. 0.52 atm |
12 |

1681 | 3 moles of ( boldsymbol{P} ) and 2 moles of ( boldsymbol{Q} ) are mixed, what will be their total vapour pressure in the solution if their partial vapour pressures are 80 and 60 respectively. A. 80 torr B. 140 torr ( c .720 ) torr D. 70 torr |
12 |

1682 | Arrange the following compounds in increasing order of solubility in water: ( boldsymbol{C}_{6} boldsymbol{H}_{5} boldsymbol{N} boldsymbol{H}_{2},left(boldsymbol{C}_{2} boldsymbol{H}_{5}right)_{2} boldsymbol{N} boldsymbol{H}, boldsymbol{C}_{2} boldsymbol{H}_{5} boldsymbol{N} boldsymbol{H}_{2} ) |
12 |

1683 | We define p value of a term (say ( x ) ) as ( boldsymbol{p}_{boldsymbol{x}}=-log boldsymbol{x} ) Calculate ( boldsymbol{p}_{left(C l^{-}right)} ) value as ( boldsymbol{x} times mathbf{1 0}^{-1} ) in a solution that is ( 2.00 times 10^{-3} mathrm{Min} ) NaCl and ( 5.4 times 10^{-4} ) M ( H C l ) |
12 |

1684 | Deep sea divers use ( left(O_{2}+H eright) ) mixture as preference to ( left(O_{2}+N_{2}right) ) mixture. This is because: A. helium is lighter than nitrogen B. helium is less soluble in blood than nitrogen c. helium is more soluble in blood. D. helium provides a better inert atmosphere than nitrogen. |
12 |

1685 | ( 1000 mathrm{g} ) aqueous solution of ( mathrm{CaCO}_{3} ) contain ( 10 g ) of calcium carbonate concentration of the solution is? A. 10 ppm B. 100 ppm c. 1000 ppm D. 10,000 ppm |
12 |

1686 | Assertion The sum of mole fractions of all the components of a solution is unity. Reason Mole fraction is a temperature dependent mode of concentration. Choose the correct option. A. Both Assertion and Reason are correct and Reason is the correct explanation for Assertion B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion C. Assertion is correct but Reason is incorrect D. Assertion is incorrect but Reason is correct |
12 |

1687 | The vapour density of undecomposed ( N_{2} O_{4} ) is ( 46 . ) When heated, vapour density decreases to 24.5 due to its dissociation to ( N O_{2} . ) The percentage dissociation of ( N_{2} O_{4} ) at the final temperature is: ( mathbf{A} cdot 88 ) B. 60 c. 40 D. 70 |
12 |

1688 | Which will have the lowest freezing point? A. A 0.01-molar solution of HNO B. A 0.01-molar solution of ( mathrm{HC}_{2} mathrm{H}_{3} mathrm{O}_{2} ) C. A 0.01-molar solution of Cu(NO ( _{3} ) ) D. A 0.01-molar solution of NaNO |
12 |

1689 | The volume of ethyl alcohol (density ( 1.15 g / c c) ) that has to be added to prepare ( 100 mathrm{cc} ) of ( 0.5 mathrm{M} ) ethyl alcohol solution in water is : A . ( 1.15 c c ) B. ( 2 c c ) c. ( 2.15 c c ) D. 2.30 ( c c ) |
12 |

1690 | Dry ( N_{2} ) was passed successively through a solution of solute ( A_{2} B ) in water at ( 27^{circ} C ) and then through pure water. The loss in mass of solution was ( 2.5 mathrm{g} ) and that of pure water was ( 0.04 mathrm{g} ) Find the degree of dissociation of salt ( A_{2} B ) when solution of ( A_{2} B ) has same concentration as ( 1.86 % ) (mass/vol) solution of urea at ( 27^{circ} C . ) Assume molarity is equal to molality. Divide answer by 10 and write the nearest integer. |
12 |

1691 | ( H_{2} S ) a toxic gas with rotten egg like smell, is used for the qualitative analysis. If the solubility of ( H_{2} S ) in water at ( S T P ) is 0.195 m, calculate Henry’s law constant. |
12 |

1692 | Assertion ( 1 M ) solution of ( K C l ) has greater osmotic pressure than ( 1 M ) solution of glucose at the same temperature. Reason In solution ( K C l ) dissociates to produce more number of particles. A. Both Assertion and Reason are correct and Reason is the correct explanation for Assertion B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion c. Assertion is correct but Reason is incorrect D. Both Assertion and Reason are incorrect |
12 |

1693 | Select the one which describe the best among all the given options. To determine whether a water solution of ( N a_{2} S_{2} O_{3} ) at room temperature is supersaturated, one can: A. heat the solution to its boiling point B. add water to the solution c. add a crystal of ( N a_{2} S_{2} O_{3} ) to the solution D. acidify the solution E. cool the solution to its freezing point |
12 |

1694 | Which of the following is an example of gaseous solution? A. Camphor in nitrogen gas B. Solution of hydrogen in palladium c. chloroform mixed with nitrogen gas D. Both (A) and (C) |
12 |

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