We provide equilibrium practice exercises, instructions, and a learning material that allows learners to study outside of the classroom. We focus on equilibrium skills mastery so, below you will get all questions that are also asking in the competition exam beside that classroom.
List of equilibrium Questions
| Question No | Questions | Class |
|---|---|---|
| 1 | The solubility product of ( M g F_{2} ) is ( 7.4 x ) ( 10^{-11} . ) Calculate the solubility of ( M g F_{2} ) in ( 0.1 mathrm{M} ) NaF solution. A ( .7 .4 times 10^{-9} ) В. ( 3.7 times 10^{-9} ) c. ( 3.7 times 10^{-11} ) D. ( 7.4 times 10^{-11} ) |
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| 2 | Equilibrium constants for four different reactions are given as: ( boldsymbol{K}_{mathbf{1}}=mathbf{1 0}^{mathbf{6}}, boldsymbol{K}_{mathbf{2}}=mathbf{1 0}^{-mathbf{4}}, boldsymbol{K}_{mathbf{3}}=mathbf{1 0}, boldsymbol{K}_{mathbf{4}}= ) 1. Which reaction will take maximum time to attain equilibrium? A ( cdot K_{1}=10^{6} ) B ( cdot K_{2}=10^{-4} ) ( mathbf{c} cdot K_{3}=10 ) D. can’t predict |
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| 3 | A solution contaming ( N H_{4} C l ) and ( N H_{4} O H ) has ( [stackrel{ominus}{O} H]=10^{-6} m o l L^{-1} ) which of the following hydroxides would be precipitated when this solution in added in equal volume to a solution containing ( 0.1 mathrm{M} ) of metal ions? A ( cdot M g(O H)_{2},left(K_{s p}=3 times 10^{-11}right) ) B. ( F e(O H)_{2}left(K_{s p}=8 times 10^{-16}right) ) c. ( C d(O H)_{2}left(K_{s p}=8 times 10^{-6}right) ) D. ( operatorname{AgOH}left(K_{s p}=5 times 10^{-3}right) ) |
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| 4 | Q14. H, (g) + 1,(g) + 2HI () What is the relationship between K, and K? |
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| 5 | 14. The value of log K for a reaction A B is: (Given: AH,09 x = -54.07 kJ mol!, A.S… x = + 10 J mof, and R= 8.31 JK-mol-1; 2.3030 ~ 8.314 x 298 = 5705) (a) 5 (b) 10 (c) 95 (d) 100 |
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| 6 | Give the molecular formula for bleaching powder. |
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| 7 | Calculate ( K_{C} ) for the reaction: ( 2 H_{2}(g)+S_{2}(g) rightleftharpoons 2 H_{2} S(g) ) if ( 1.58 mathrm{mol} ) ( boldsymbol{H}_{2} boldsymbol{S}, 1.27 mathrm{mol} boldsymbol{H}_{2}, ) and ( mathbf{2 . 7 8} times mathbf{1 0}^{-mathbf{6}} ) mol of ( S_{2} ) are in equilibrium in a flask of capacity ( 180 mathrm{L} ) at ( 750 mathrm{C} ) A ( cdot K_{C}=124 times 10^{8} L ) mol ( ^{-1} ) B. ( K_{C}=1 times 10^{8} L ) mol( ^{-1} ) c. ( K_{C}=1 times 10^{-8} L mathrm{mol}^{-1} ) D. ( K_{C}=1 times 10^{7} L mathrm{mol}^{-1} ) |
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| 8 | In some solutions, the concentration of ( H_{3} O^{+} ) remains constant even when small amounts of strong acid or strong base are added to them. These solutions are known as: A. colloidal solutions B. buffer solutions c. true solutions D. ideal solutions |
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| 9 | How many moles of acetic acid and sodium acetate each should be dissolved to prepare one litre of 0.063 molar buffer solution of pH ( 4.5 ? ) ( left(K_{a} text { for } C H_{3} C O O H=1.8 times 10^{-5}right) ) |
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| 10 | An increase in pressure will change the equilibrium by: A. shifting to the side where a smaller volume results B. shifting to the side where a larger volume results C. favoring the endothermic reaction D. favoring the exothermic reaction E. none of the above |
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| 11 | Solubility of Potassium nitrate: A. increases with temperature B. decreases with temperature C. remains constant with temperature D. is not related to the temperature fluctuations |
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| 12 | Consider the reaction equilibrium Ice( rightleftharpoons_{text {Lesservier}}-boldsymbol{X k c a l} ) Greatervolume The favourable condition for forward reaction are: A. low temperature, high pressure and excess of ice B. low temperature, low pressure and excess of ice c. high temperature, low pressure and excess of ice D. high temperature, high pressure and excess of ice |
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| 13 | At ( 373 mathrm{K} ), steam and water are in equilibrium and ( Delta H=40.98 mathrm{kJ} ) mol( ^{-1} ) What will be ( Delta S ) fro conversion of water into steam? ( boldsymbol{H}_{2} boldsymbol{O}_{(l)} rightarrow boldsymbol{H}_{2} boldsymbol{O}_{(g)} ) A ( cdot 109.8 ) J ( K^{-1} m o l^{-1} ) B . 31 J ( K^{-1} ) mol ( ^{-1} ) c. 21.98 J ( K^{-1} m o l^{-1} ) D. 326 J ( K^{-1} ) mol ( ^{-1} ) |
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| 14 | Which of the following mixtures in aqueous solution of equimolar concentration acts as a buffer solution? A. ( H N O_{3}+N a O H ) в. ( H_{2} S O_{4}+K O H ) c. ( N H_{4} O H(text {excess})+H C l ) D. ( C H_{3} C O O H+N a O H(e x c e s s) ) |
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| 15 | Which of the following represents a conjugate acid/base pair? A. ( N a^{+} / C l^{-} ) в. ( H C l / H^{+} ) c. ( H_{2} C O_{3} / C O_{3}^{2} ) D. ( N H_{3} / N H_{4}^{+} ) E . ( K^{+} / O H^{-} ) |
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| 16 | When equilibrium is attained, the concentration of each of the reactants and products become equal. A. True B. False c. Ambiguous D. None of these |
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| 17 | Q. 25 Ionisation constant of a weak base MOH, is given expression [M”] [OH-] [MOH] Values of ionisation constant of some weak bases at a particular temperature are given below Base Dimethylamine Urea Pyridine Ammonia no 5.4 x 10- 4 1 .3 x 10 * 1.77 x 10-9 1.77 x 10-5 Arrange the bases in decreasing order of the extent of their jonisation at equilibrium. Which of the above base is the strongest? |
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| 18 | If ( K_{a 1} ) and ( K_{a 2} ) are the ionization constants of ( boldsymbol{H}_{3} stackrel{+}{boldsymbol{N}} boldsymbol{C} boldsymbol{H} boldsymbol{R} boldsymbol{C O O} boldsymbol{H} ) and ( boldsymbol{H}_{3}^{+} boldsymbol{N} boldsymbol{C} boldsymbol{H} boldsymbol{R} boldsymbol{C O O}^{-}, ) respectively, the ( boldsymbol{p} boldsymbol{H} ) of the solution at the isoelectric point is: A ( cdot p H=p K_{a 1}^{circ}+p K_{a 2}^{circ} ) в. [ p H=left(p K_{a 1}^{circ} p K_{a 2}^{circ}right)^{frac{1}{2}} ] c. [ p H=left(p K_{a_{1}}^{circ}+p K_{a 2}^{circ}right)^{frac{1}{2}} ] D. ( _{p H}=frac{left(p K_{a 1}^{circ}+p K_{a 2}^{circ}right)}{2} ) |
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| 19 | saturated solution of ( A g C l ) then which of the following plot is correct? ( A ) B. ( c ) ( D ) |
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| 20 | On passing ( boldsymbol{H}_{2} boldsymbol{S} ) into a solution containing both ( Z n^{2-} ) and ( C u^{2-} ) in acidic medium, only CuS gets precipitated. This is because: ( mathbf{A} cdot K_{s p} ) of ( C u SK_{s p} ) of ZnS D. cus is more stable then zns |
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| 21 | People use bases called antacids due to: A. get rid of stomach pain B. irritation c. both ( (A) ) and ( (B) ) D. none of the above |
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| 22 | The equilibrium constant of a reaction is 300 , if the volume of the reaction flask is tripled, the equilibrium constant will be: A . 100 B. 300 ( c .250 ) D. 150 |
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| 23 | 6. Consider the following equilibrium in a closed container: N204(8) 2NO2(g) At a fixed temperature, the volume of the reaction container is halved. For this change, which of the given statements holds true regarding the equilibrium constant (KD) and degree of dissociation (a)? (a) Neither K, nor a changes (b) Both Ko and a change (c) K, changes, but a does not change (d) K, does not change, but a changes |
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| 24 | Maximum change in ( p H ) is observed when 50 of ( 1 M K O H ) solution is added to A . 25 ml. of ( 2.5 N ) HCl B. ( 50 mathrm{ml} ) of ( 1 mathrm{N} ) HCl c. ( 30 mathrm{ml} ) of ( 2 mathrm{N} ) HCl D. ( 50 mathrm{ml} ) distilled water |
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| 25 | The label of a bottle containing a dilute aqueous solution of an acid become damage Only its concentration was readable ( A ) pH meter was nearby, and a quick measurement showed that the hydrogen ion concentration is equal to the value on the label. Which of the following four acids that could have been the solution if the pH changed one unit after a tenfold dilution? This question has multiple correct options ( mathbf{A} cdot H C l O_{4} ) B. ( H_{3} B O_{3} ) с. ( C H_{3} ) СООН D. ( H N O_{3} ) |
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| 26 | In aqueous solution, the proton exists as a (acid/base) |
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| 27 | For the reaction, ( boldsymbol{S n O}_{2}(boldsymbol{s})+boldsymbol{2} boldsymbol{H}_{2}(boldsymbol{g}) rightleftharpoons ) ( boldsymbol{S} boldsymbol{n}(l)+boldsymbol{2} boldsymbol{H}_{2} boldsymbol{O}(boldsymbol{g}) ) the equilibrium mixture of steam and hydrogen contained ( 45 % ) and ( 24 % H_{2} ) at ( 900 mathrm{K} ) and ( 1100 mathrm{K} ) respectively. Calculate ( boldsymbol{K}_{boldsymbol{P}} ) at both the temperatures. Generally should it be higher or lower temperatures for better reduction of ( boldsymbol{S} boldsymbol{n} boldsymbol{O}_{2} ? ) ( mathbf{A} cdot therefore K_{C_{2}}=1.03 ) ( mathbf{B} cdot therefore K_{C_{2}}=5.02 ) ( mathbf{c} cdot therefore K_{C_{2}}=15.01 ) ( mathbf{D} cdot therefore K_{C_{2}}=10.03 ) |
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| 28 | ( C O_{2} ) gas along with solid (Y) is obtained when sodium salt (X) is heated. ( (X) ) is again obtained when ( C O_{2} ) gas is passed into aqueous solution of (Y). Identify ( (X) ) and ( (Y) ) respectively. A. ( N a_{2} C O_{3}, N a_{2} O ) в. ( N a_{2} C O_{3}, ) NaOH с. ( N a H C O_{3}, N a_{2} C O_{3} ) D. ( N a_{2} C O_{3}, N a H C O_{3} ) |
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| 29 | In the reaction ( C(s)+C O_{2}(g) rightleftharpoons ) ( 2 C O(g), ) the equilibrium pressure is 12 atm. If ( 50 % ) of ( C O_{2} ) reacts till equilibrium then ( boldsymbol{K}_{boldsymbol{p}} ) will be : A . 12 atm B. 6 atm ( c .20 ) atm D. 24 atm |
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| 30 | State True or False. Almost every liquid is either an acid or a base. A. True B. False |
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| 31 | If the equilibrium constant of the reaction of weak acid ( boldsymbol{H} boldsymbol{A} ) with strong base is ( 10^{9} ), then ( mathrm{pH} ) in ( 0.1 M ) NaA is: A . 5 B. 9 ( c cdot 7 ) D. |
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| 32 | For the reaction ( boldsymbol{C u} boldsymbol{S O}_{4} cdot boldsymbol{5} boldsymbol{H}_{2} boldsymbol{O}(boldsymbol{s}) rightleftharpoons ) ( boldsymbol{C u} boldsymbol{S O}_{4} cdot boldsymbol{3} boldsymbol{H}_{2} boldsymbol{O}(boldsymbol{s})+boldsymbol{2} boldsymbol{H}_{2} boldsymbol{O}(boldsymbol{g}) ) which one is correct representation: A ( cdot K_{P}=left(P_{H_{2}} partialright)^{2} ) в. ( K_{C}=left[H_{2} Oright]^{2} ) ( mathbf{c} cdot K_{p}=K_{c}(R T)^{2} ) D. all of these |
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| 33 | ( A t 817, K_{p} ) for the reaction between ( C O_{2}(g) ) and excess hot graphite ( (s) ) is 10 atm. (a) The sum of equilibrium concentration of the gases at ( 817^{circ} mathrm{C} ) is ( X M ) and a total pressure of 5 atm. (b) At ( Y ) atm total pressure, the gas contains ( 5 % C O_{2} ) by volume. The value of ( 1000(X+Y) ) is |
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| 34 | Which of the following compounds can be called as non-electrolytes? A. ( C_{6} H_{12} O_{6} ) в. ( C_{2} H_{5} O H ) ( mathbf{c} cdot C_{2} H_{6} ) D. All of the above |
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| 35 | The progress of reaction ( boldsymbol{A}(boldsymbol{g}) rightleftharpoons ) ( boldsymbol{x} boldsymbol{B}(boldsymbol{g})+boldsymbol{y} boldsymbol{C}(boldsymbol{g}) ) with time is presented in figure. What is the value of ( boldsymbol{K}_{c}^{0} ) at ( mathbf{3 0 0 K} ? ) ( A ) B. ( c .3 ) ( D ) |
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| 36 | Many lead salts are often used as pigments. If ( boldsymbol{P b S O}_{4}left(boldsymbol{K}_{s p}=mathbf{1 . 6} times mathbf{1 0}^{-8}right) ) were used in an unglazed ceramic bowl how many milligrams of lead (II) could dissolve per liter of water? ( A cdot 43 ) B. 35 ( c cdot 11 ) D. 38 |
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| 37 | How many mole of ( boldsymbol{H} boldsymbol{C} boldsymbol{N} ) will be required to prepare one litre buffer solution of ( boldsymbol{p} boldsymbol{H}=mathbf{1 0 . 4} ) using ( mathbf{0 . 0 1} ) mol NaC N? (Given: ( left.boldsymbol{K}_{boldsymbol{a}}(boldsymbol{H} boldsymbol{C N})=boldsymbol{4} times mathbf{1 0}^{-10}right) ) ( mathbf{A} cdot 2 times 10^{-2} mathbf{M} ) В. ( 9 times 10^{-4} ) М ( mathbf{c} cdot 4 times 10^{-4} mathrm{M} ) D. ( 9 times 10^{-3} mathrm{M} ) |
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| 38 | The solubility product of ( B a S O_{4} ) is ( 1.5 times 10^{-9} . ) The precipitation in a ( 0.01 M B a^{2+} ) solution will start on adding ( H_{2} S O_{4} ) of concentration: A ( cdot 1 times 10^{-9} M ) в. ( 1.5 times 10^{-7} M ) c. ( 2 times 10^{-7} M ) D. ( 1 times 10^{-6} M ) |
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| 39 | The number of ( boldsymbol{H}^{+} ) ions in ( 1 mathrm{cc} ) of ( mathrm{a} ) solution of ( p H=13 ) is: A. ( 6.023 times 10^{7} ) B. ( 1 times 10^{-13} ) c. ( 6.023 times 10^{13} ) D. ( 1 times 10^{16} ) |
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| 40 | The ( p H ) of an acid buffer can be raised by 2 units by A. Increaseing the concentration of both weak acid and salt by two moles B. Increasing the concentration of both the acid and salt by 10 times c. Diluting the solution by 10 times D. Increasing the concentration of the salt by 10times and decreasing concentration of the acid by 10 times |
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| 41 | To a solution of acetic acid, solid sodium acetate is added gradually. When ( x ) mole of salt is added, the pH has a certain value. If y mole of salt is added, the pH change by 0.6 units to the previous pH. What is the ratio of ( x ) and y? |
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| 42 | Which of the following reactions have ( boldsymbol{K}_{boldsymbol{p}}<boldsymbol{K}_{boldsymbol{c}} ) This question has multiple correct options A ( cdot H_{2}(g)+I_{2}(g) rightleftharpoons 2 H I(g) ) в. ( C O(g)+C l_{2}(g) rightleftharpoons C O C l_{2}(g) ) c. ( 2 B r C l(g) rightleftharpoons B r_{2}(g)+C l_{2}(g) ) D. ( N_{2}(g)+3 H_{2}(g) rightleftharpoons 2 N H_{3}(g) ) |
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| 43 | Polar covalent compounds are in gaseous state, but ionizes in aqueous solution state. A. electrolytes B. non-electrolytes c. soluble D. none of the above |
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| 44 | When we add a pinch of sodium hydrogen carbonate in a flask containing ethanoic acid a reaction takes place. What will be the observation when we carry out the reaction? A. Milky solution B. Bubble formation c. Solution turns red D. Brisk effervescence |
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| 45 | The species among the following, which can act as acid as well as base is? A ( . H S O_{4}^{-} ) B. ( S O_{4}^{2} ) c. ( H_{3} O^{+} ) D. ( C l ) |
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| 46 | An equilibrium constant of ( 10^{-4} ) for a reaction means, the equilibrium is A. largely towards backward direction B. largely towards forward direction c. equally poised D. never established |
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| 47 | The pH of 0.001M HCN is: ( A cdot 3 ) в. 1 c. between 3 & 7 D. 7 |
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| 48 | Q6. Define solubility product. | 11 |
| 49 | For the reaction ( mathbf{2} boldsymbol{A}+boldsymbol{B} rightleftharpoons mathbf{3} boldsymbol{C} ) at ( mathbf{2} mathbf{9 8} boldsymbol{K}, boldsymbol{K}_{boldsymbol{c}}=mathbf{4 9} ) A ( 3 L ) vessel contains 2,1 and 3 moles of ( A, B ) and ( C ) respectively. The reaction at the same temperature: A. must proceed in forward direction B. must proceed in backward direction c. must be in equilibrium D. cannot be predicted |
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| 50 | 1.0 ( mathrm{ml} ) of a solution of ( mathrm{H} C l ) with a ( p H ) of 4.0 is added it to ( 9.0 mathrm{ml} ) of distilled water, the ( p H ) of the final solution will be: A. The pH would remain unchanged. B. The pH would rise to 5.5 c. The pH would rise to 5.0 D. The pH would be unmeasurable due to the amount of dilution E. The pH would rise to 7.0 |
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| 51 | If volume ratio of ( 0.02 M H C l ) and ( 0.02 M B O H ) (a weak base) mixed to make ( 200 mathrm{mL} ) of buffer of ( p H=7 ) is ( 2.23: X . ) The value of ( X ) is: ( boldsymbol{K}_{b} ) for ( boldsymbol{B O H}=mathbf{8 . 1} times mathbf{1 0}^{-mathbf{8}} ) ( A ) B. 5 ( c cdot 0.2 ) D. 2.5 |
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| 52 | Assertion ( H C l rightarrow H^{+}+C l^{-} ) is an ionization Reason The electron is initially shared between both atoms, thus the dissociation event into ions involves the transfer of an electron from one atom to the other. 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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| 53 | lonic solutions are good conductors of Electricity. A. True B. False |
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| 54 | Buffer solution is prepared by mixing: A. Strong acid + its salt of strong base B. Weak acid + its salt of strong base. c. Strong acid + its salt of weak base D. None of the above |
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| 55 | Five solutions ( A, B, C, D, E ) when tested with universal indicator showed ( p H ) as 4,1,11,7 and 9 respectively. Which solution is weakly acidic? ( A cdot A ) B. B ( c cdot c ) ( D . ) D |
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| 56 | The solubility of ( A_{2} X_{5} ) is ( x ) mol ( d m^{-3} ) Its solubility product is: A ( cdot 36 x^{6} ) В. ( 64 times 10^{4} x^{7} ) c. ( 126 x^{7} ) D. ( 1.25 times 10^{4} x^{7} ) |
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| 57 | Q9. Give two characteristics of a buffer solution. Ana L. IT |
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| 58 | For which of the following reactions will the equilibrium mixture contain an appreciable concentration of both reactants and products? A ( cdot C l_{2}(g) rightleftharpoons 2 C l(g) ; K_{c}=6.4 times 10^{-39} ) B. ( C l_{2}(g)+2 N O(g) rightleftharpoons 2 N O C l(g) ; K_{c}=3.7 times 10^{8} ) c. ( C l_{2}(g)+2 N O(g) rightleftharpoons 2 N O_{2} C l(g) ; K_{c}=1.8 ) D. ( H_{2}(g)+I_{2}(g) rightleftharpoons 2 H I(g) . K_{c}=49 ) |
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| 59 | For the reaction ( 2 H I(g) Leftrightarrow H_{2}(g)+ ) ( I_{2}(g), ) the degree of dissociation ( (alpha) ) of ( H I(g) ) is related to the equilibrium constant, ( boldsymbol{K}_{boldsymbol{p}} ) by the expression: ( ^{mathrm{A}} cdot frac{1+2 sqrt{K_{p}}}{2 sqrt{K_{p}}} ) B. ( sqrt{frac{1+2 K_{p}}{2}} ) ( ^{mathrm{c}} cdot sqrt{frac{2 K_{p}}{1+2 K_{p}}} ) D. ( frac{2 sqrt{K_{p}}}{1+2 sqrt{K_{p}}} ) |
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| 60 | The standard reduction potential of two reactions are given. ( boldsymbol{A} boldsymbol{g} boldsymbol{C l}_{(s)}+boldsymbol{e}^{-} rightarrow boldsymbol{A} boldsymbol{g}_{(s)}+boldsymbol{C l}_{(a q)}^{-} ; boldsymbol{E}^{ominus}= ) ( mathbf{0 . 2 2 V} ) (i) ( boldsymbol{A} boldsymbol{g}_{(a q)}^{+}+boldsymbol{e}^{-} rightarrow boldsymbol{A} boldsymbol{g}_{(s)} ; boldsymbol{E}^{ominus}=mathbf{0 . 8 0 V} ) The solubility product of ( A g C l ) under standard conditions of temperature is: A ( .1 .6 times 10^{-5} ) В. ( 1.5 times 10^{-8} ) c. ( 3.2 times 10^{-10} ) D. ( 1.5 times 10^{-10} ) |
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| 61 | What weight of sodium nitrate will separate when a saturated solution containing 50 gram of water is cooled from ( 50^{circ} mathrm{C} ) to ( 30^{circ} mathrm{C} ) ? The solubility of ( N a N O_{3} ) at ( 50^{circ} C ) and ( 30^{circ} C ) is 114 g and 86 g respectively. |
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| 62 | lonization of phosphoric acid gives: A ( cdot H_{2} P O_{4}^{-} ) в. ( H P O_{4}^{-2} ) ( mathrm{c} cdot P O_{4}^{-3} ) D. all of these |
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| 63 | Assertion ( : H C O_{3}^{-} ) can act as a Bronsted acid or a Bronsted base. Reason ( : H C O_{3}^{-} ) can donate a proton to form ( C O_{3}^{2-} ) or accept a proton to form ( boldsymbol{H}_{2} boldsymbol{C} boldsymbol{O}_{3} ) A. Both Assertion and Reason are correct and Reason is the correct explanation for Assertion B. Both Assertion and Reason are correct and Reason is not the correct explanation for Assertion c. Assertion is correct but Reason is incorrect D. Assertion is incorrect but Reason is correct E. Both Assertion and Reason are incorrect |
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| 64 | Calculate the degree of ionization and ( left[boldsymbol{H}_{3} boldsymbol{O}^{+}right] ) of ( mathbf{0 . 0 1} boldsymbol{M} boldsymbol{C H}_{3} boldsymbol{C O O H} ) solution. The equilibrium constant of acetic acid is ( 1.8 times 10^{-5} ) |
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| 65 | Which among the following resists a rapid change of pH? A. Buffer B. Indicator C. Arrhenius acid D. Arrhenius base E. Neutral condition |
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| 66 | 100ml of a solution of HCl with pH value 3 is diluted with ( 400 mathrm{ml} ) of water. The new pH of the solution is? A. 3.7 B. 5.3 c. 4.2 D. 5.6 |
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| 67 | Calculate the ratio of ( H C O O^{-} ) and ( F^{-} ) in a mixture of ( 0.2 M ) HCOOH ( left(K_{a}=right. ) ( left.2 times 10^{-4}right) ) and ( 0.1 M H Fleft(K_{a}=6.6 timesright. ) ( left.10^{-4}right) ) A .1: 6.6 B. 1: 3.3 c. 2: 3.3 D. 3.3 : 2 |
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| 68 | How much ( N a F ) should be added to 100 mL of solution having ( 0.016 M ) in ( S r^{2}+ ) ions to reduce its concentration to ( 2.5 times 10^{-3} M ?left(K_{s p} S r F_{2}=8 times 10^{-10}right) ) A. 0.098 g ggg ( . . .998 ) B. 0.168 g c. 0.177 g D. 0.118 g |
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| 69 | For the reaction, ( 2 N O(g)+2 H_{2}(g) rightarrow ) ( N_{2}(g)+2 H_{2} O(g) ) the rate expression can be written in the following ways: ( left{boldsymbol{d t}left[boldsymbol{N}_{2}right] / boldsymbol{d} tright}= ) ( boldsymbol{k}_{1}[boldsymbol{N} boldsymbol{O}]left[boldsymbol{H}_{2}right] ;left{boldsymbol{d}left[boldsymbol{H}_{2} boldsymbol{O}right] / boldsymbol{d} boldsymbol{t}right)= ) ( boldsymbol{k}[boldsymbol{N} boldsymbol{O}]left[boldsymbol{H}_{2}right] ) ( {-boldsymbol{d}[boldsymbol{N} boldsymbol{O}] / boldsymbol{d} boldsymbol{t}}= ) ( boldsymbol{k}_{mathbf{1}}^{prime}[boldsymbol{N} boldsymbol{O}]left[boldsymbol{H}_{2}right] ;left{-boldsymbol{d}left[boldsymbol{H}_{2}right] / boldsymbol{d} tright}= ) ( k_{1}^{prime prime}[N O]left[H_{2}right] ) The relation ship between ( k, k_{1}, k_{1}^{prime} ) and ( k_{1}^{prime prime} ) is: |
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| 70 | Which one of the following is not a Lewis Acid? ( mathbf{A} cdot B F_{3} ) в. ( A l C l_{3} ) c. ( B e C l_{2} ) D. ( operatorname{SnCl}_{2} ) |
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| 71 | The term ( p H ) comes from: A. hydrogen purity B. pure Hydrogen c. hydrogen power D. purity of Hydrogen |
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| 72 | In a reaction, ( boldsymbol{A}+mathbf{2} boldsymbol{B} rightleftharpoons mathbf{2} boldsymbol{C}, mathbf{2 . 0} ) mole of ( A 3.0 ) mole of ( B ) and 2.0 mole of ( C ) are placed in a ( 2.0 L ) flask and the equilibrium concentration of ( boldsymbol{C} ) is 0.5 mole ( / L . ) The equilibrium constant ( K ) for the reaction is ( mathbf{A} cdot 0.073 ) B. 0.147 ( c .0 .05 ) D. 0.026 |
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| 73 | The dissociation constant of uric acid is ( boldsymbol{K}_{boldsymbol{a}}=mathbf{4 . 0} times mathbf{1 0}^{-mathbf{6}} boldsymbol{M} . ) The ( boldsymbol{p} boldsymbol{H} ) of a sample is ( 6.0 . ) What is the ratio of urate ion to uric acid in the urine?? |
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| 74 | The specific conductance at ( 298 mathrm{K} ) of AgCl solution In water was determined to be ( 1.826 times 10^{-6} ) ohm ( ^{-1} mathrm{cm}^{-1} . ) The ionic conductances ( A g^{+} ) and ( C l^{-} ) are 61.92 and 76.34 respectively. What is the solubility of AgCl in water? A ( cdot 2.1 times 10^{-4} mathrm{gL}^{-1} ) B . ( 1.32 times 10^{-5} mathrm{gL}^{-1} ) c. ( 1.9 times 10^{-3} mathrm{gL}^{-1} ) D. 2.1 ( times 10^{-6} mathrm{gL}^{-1} ) |
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| 75 | One mole of ( boldsymbol{H}_{2}, boldsymbol{2} ) moles of ( boldsymbol{I}_{2} ) and ( boldsymbol{3} ) moles of ( H I ) are injected in a one litre flask. What will be the concentration of ( boldsymbol{H}_{2}, boldsymbol{I}_{2} ) and ( boldsymbol{H} boldsymbol{I} ) at equilibrium when ( boldsymbol{K}_{boldsymbol{c}} ) is ( 45.9 ? ) |
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| 76 | An equilibrium mixture in a vessel of capacity 100 litre contain 1 mol ( N_{2}, 2 ) mol ( O_{2} ) and 3 mol ( N O . ) Number of moles of ( O_{2} ) to be added so that at new equilibrium the conc. of ( N O ) is found to be 0.04 mol/lit is: A . ( 101 / 18 ) в. ( 101 / 9 ) c. ( 202 / 9 ) D. none of these |
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| 77 | A reaction system in equilibrium according to the equation ( 2 S O_{2}+ ) ( O_{2} rightleftharpoons 2 S O_{3} ) in 1 litre reaction vessel at a given temperature was found to contain 0.11 mol of ( S O_{2}, 0.12 ) of ( S O_{3} ) and 0.05 mol of ( O_{2 .} ) Another 1 litre reaction vessel contains 64 g of ( S O_{2} ) at the same temperature. What mass of ( boldsymbol{O}_{2} ) must be added to this vessel in order that at equilibrium half of ( S O_{2} ) is oxidised to ( boldsymbol{S O}_{3} ) ? A. 9.34 g в. 10.87 c. ( 21.3 mathrm{g} ) D. 32.4 g |
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| 78 | Calculate : ( K_{a} ) for ( H C N ) given ( boldsymbol{K}_{b}left(boldsymbol{C N}^{-}right)=mathbf{2 . 5} times mathbf{1 0}^{-mathbf{5}} ) A ( cdot 10^{-5} ) В. ( 2 times 10^{-7} ) c. ( 4 times 10^{-10} ) D. None of these |
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| 79 | A monoprotic acid in ( 100 M ) solution is ( 0.001 % ) ionized. The dissociation constant of this acid is: A ( cdot 1.0 times 10^{-3} ) B. ( 1.0 times 10^{3} ) c. ( 1.0 times 10^{-8} ) D. ( 1.0 times 10^{-10} ) |
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| 80 | Select the correct statements: This question has multiple correct options A. The value of ( Q_{c} ) for a given reaction is constant. B. A change in the physical state of a gaseous product shows a change in the value of equilibrium constant of that reaction. C the value of ratio ( frac{Q_{c}}{K_{c}} ) can be used to predict the direction in which a system will proceed spontaneously towards equilibrium. D. The rate constants for forward and backward reaction for a reversible reaction always increases with temperature but their ratio ( left(i . e ., frac{K_{f}}{K_{b}}right) ) may increase or decrease with temperature. |
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| 81 | In order to prepare a buffer of ( P^{H} 8.26 ) the amount of ( left(N H_{4}right)_{2} S O_{4} ) required to be mixed with 1L of 0.1 M ( boldsymbol{N} boldsymbol{H}_{mathbf{3}}left(boldsymbol{p} boldsymbol{K}_{boldsymbol{b}}=right. ) 4.74) is: A . 5 mol B. 0.5 mol c. 10 mol D. 1 mol |
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| 82 | A solution contains ( 0.4 M C H_{3} C O O H ) and ( 0.2 M C H_{3} C O O N a . ) Calculate the concentration of ( boldsymbol{H}^{+} ) ions. The ionisation constant of acetic acid is ( 1.8 times 10^{-5} ) |
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| 83 | Which among the following represent the conjugate acid/base pairs? This question has multiple correct options A ( cdot H_{3} O^{+} / H_{2} O ) в. ( H_{2} S O_{4} / S O_{4}^{2} ) c. ( H C O_{3}^{-} / C O_{3}^{2} ) D. All are conjugate acid/ base pairs |
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| 84 | Assertion Assertion: Higher order ionization constants ( left(boldsymbol{K}_{a_{2}}, boldsymbol{K}_{a_{3}}right) ) are smaller than the lower order ionization constant ( boldsymbol{K}_{boldsymbol{a}_{mathbf{1}}} ) of polyprotic acid. Reason Reason: Polyprotic acid solutions contain a mixture of acids. A. If both the assertion and reason are true and reason is the correct explanation of assertion B. If both the assertion and reason are true but reason is not the correct explanation of assertion. c. If assertion is true but reason is false D. If both assertion and reason are false |
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| 85 | Calculate the degree of ionization of ( 0.05 mathrm{M} ) acetic acid of its ( _{p} boldsymbol{K}_{a} ) value is 4.74. How is the degree of dissociation affected when its solution is also (a) ( 0.01 mathrm{M} ) and (b) ( 0.1 mathrm{M} ) in hydrochloric acid? |
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| 86 | Which of the following expressions is/are not true? ( mathbf{A} cdotleft[H^{+}right]=left[O H^{-}right]=sqrt{K_{w}} ) for a neutral solution at al temperatures B ( cdotleft[H^{+}right]>sqrt{K_{w}} &left[O H^{-}right]<sqrt{K_{w}} ) for an acidic solution ( mathbf{C} cdotleft[H^{+}right]sqrt{K_{w}} ) for an alkaline solution D ( cdotleft[H^{+}right]=left[O H^{-}right]=10^{-7} M ) for a neutral solution at all temperatures |
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| 87 | Calculate the dissociation constant of ( N H_{4} O H ) at ( 298 mathrm{K}, ) if ( triangle H^{ominus} ) and ( Delta S^{ominus} ) for the given changes are as follows: ( boldsymbol{N} boldsymbol{H}_{3}+boldsymbol{H}^{oplus} rightleftharpoons stackrel{oplus}{boldsymbol{N}} boldsymbol{H}_{4} ) ( Delta H^{ominus}=-52.2 k J m o l^{-1}, Delta S^{ominus}= ) ( mathbf{1 . 6 7} boldsymbol{J} boldsymbol{K}^{-1} boldsymbol{m o l}^{-1} ) ( boldsymbol{H}_{2} boldsymbol{O} rightleftharpoons boldsymbol{H}^{oplus}+stackrel{ominus}{boldsymbol{O}} boldsymbol{H} ; boldsymbol{Delta} boldsymbol{H}^{ominus}= ) ( mathbf{5 6 . 6} k J mathbf{m o l}^{-1} ) ( Delta S^{ominus}=-76.53 J K^{-1} m o l^{-1} ) begin{tabular}{l} A. ( K_{b}=1.7 times 10^{-5} ) \ hline end{tabular} в. ( K_{b}=1.7 times 10^{-3} ) c. ( K_{b}=1.7 times 10^{-1} ) D. ( K_{b}=3.4 times 10^{-5} ) |
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| 88 | LIO 5 D.LT 025. Does the number of moles of reaction products increase, decrease or remain same when each of the following equilibria is subjected to a decrease in pressure by increasing the volume? (i) PC (g) = PCI,() + C1 (8) (ii) CaO(s) + CO.(g) – CaCO3(s) (iii) 3Fe(s) + 4H2O(g) = Fe, (s) + 4H2 (8) |
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| 89 | ( 20 mathrm{ml} ) of ( 0.2 mathrm{M} H C N ) mix with ( 10 mathrm{ml} ) of 0.2 M ( N a O H, ) then calculate ( p H ) of resulting mixture, ( p K a ) value of ( H C N ) is ( 5:- ) A . 6 B. 7.5 ( c .5 ) D. 11 |
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| 90 | Conjugate base of a weak acid has ( boldsymbol{K}_{b}=mathbf{1 0}^{-9} . ) The equilibrium constant for the reaction of acid with strong base is: ( mathbf{A} cdot 10^{-19} ) B . ( 10^{-3} ) ( c cdot 10^{9} ) D. ( 10^{5} ) |
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| 91 | Calcium lactate is a salt of weal organic acid and strong base represented as ( boldsymbol{C} boldsymbol{a}(boldsymbol{L} boldsymbol{a} boldsymbol{C})_{2} cdot boldsymbol{A} ) saturated solution of ( boldsymbol{C} boldsymbol{a}(boldsymbol{L} boldsymbol{a} boldsymbol{C})_{2} ) contains ( boldsymbol{0} . boldsymbol{6} ) mole in ( boldsymbol{2} ) litre solution. ( p O H ) of solution is ( 5.60 . ) If ( 90 % ) dissociation of the salt takes place then what is ( p K_{a} ) of lactic acid? A. ( 2.8-log (0.54) ) B. ( 2.8+log (0.54) ) c. ( 2.8+log (0.27) ) D. None of these |
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| 92 | The equilibrium expression, ( boldsymbol{K}=left[boldsymbol{C O}_{2}right] ) represents the reaction: A. ( C(s)+O_{2}(g) rightleftharpoons C O_{2}(g) ) B. ( C O(g)+frac{1}{2} O_{2}(g) rightleftharpoons C O_{2}(g) ) c. ( operatorname{CaCO}_{3}(s) rightleftharpoons C a O(s)+C O_{2}(g) ) D. ( C O_{2}(g) rightleftharpoons C(s)+O_{2}(g) ) E ( cdot operatorname{CaO}(s)+C O_{2}(g) rightleftharpoons operatorname{CaCO}_{3}(s) ) |
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| 93 | toppr Q Type your ques to the processes that occur in living organisms. This primarily because the functioning of enzymes-catalysts for these processes – is sharply pH dependent. The normal pH value of blood plasma is ( 7.4 . ) Severe illness or death can result from sustained variations of a few tenths of pH unit. Among the factors that lead to a condition of acidosis, in which there is a decrease in the pH of blood are heart failure, kidney failure diabetes mellitus persistent diarrhoea or a long term high protein diet.A temporary condition of acidosis may result from prolonged, intensive exercise. Alkalosis, which causes increase in pH of blood may occur as a result of severe vomiting over breathing or exposure to high altitudes. Several factors are involved in the |
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| 94 | Which of the following mixtures in aqueous solution acts as a buffer? A. ( H N O_{3}+K N O_{3} ) в. ( H_{2} S O_{4}+K_{2} S O_{4} ) c. ( N H_{4} O H+N H_{4} C l ) D. ( C H_{3} ) СООН ( + ) NaCl |
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| 95 | Calculate the percent of hydrolysis in a ( mathbf{0 . 0 6} M ) solution of ( boldsymbol{K} boldsymbol{C} boldsymbol{N} ) Use ( :left[boldsymbol{K}_{a(boldsymbol{H} C N)}=boldsymbol{6} times mathbf{1 0}^{-mathbf{1 0}}right] ) A . ( 1.667 % ) B . ( 7.45 % ) c. ( 34.67 % ) D. None of these |
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| 96 | Q55. Calculate the hydrogen ion concentration in the following biological fluids whose pH are given below: (a) Human muscle-fluid, 6.83 (6) Human stomach fluid, 1.2 (c) Human blood, 7.38 (6) Human saliva, 6.4 |
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| 97 | Assertion On passing ( boldsymbol{H} boldsymbol{C l}(boldsymbol{g}) ) through a saturated solution of ( B a C l_{2}, ) a white turbidity appears Reason The common ion effect is responsible for white turbidity 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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| 98 | Identify the correct statement(s) for the given reaction. ( boldsymbol{H} boldsymbol{C l}+boldsymbol{H}_{2} boldsymbol{O} rightarrow boldsymbol{H}_{3} boldsymbol{O}^{+}+boldsymbol{C l}^{-} ) a) Conjugate base of ( boldsymbol{H} boldsymbol{C l} ) is ( boldsymbol{C l}^{-} ) b) Conjugate acid-base pair is ( boldsymbol{H}_{3} boldsymbol{O}^{+} ) and ( boldsymbol{H}_{2} boldsymbol{O} ) c) Conjugate base of ( boldsymbol{H}_{2} boldsymbol{O} ) is ( boldsymbol{H}_{3} boldsymbol{O}^{+} ) d) Conjugate acid-base pair is ( boldsymbol{H} boldsymbol{C l} ) and ( boldsymbol{H}_{3} boldsymbol{O}^{+} ) ( A cdot a ) and ( b ) are correct B. a and c are correct c. ( c ) and ( d ) are correct D. a and d are correct |
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| 99 | A ( 0.1 ~ M ) aqueous solution of a weak acid is ( 2 % ) ionized. If the ionic product of water is ( 1 times 10^{-14}, ) the ( left[O H^{-}right] ) is: A ( cdot 5 times 10^{-12} mathrm{M} ) В. ( 2 times 10^{-3} ) М c. ( 1 times 0^{-14} mathrm{M} ) D. none of these |
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| 100 | 0.43 Match the Column I with Column II. RO Column II 1. AG>0, K1 Column A. Equilibrium B. Spontaneous reaction C. Non-spontaneous reaction 2. AG=0 3. AGⓇ = 0 4. AG 1 |
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| 101 | Question 27. If the solubility product of CuS is 6 *10-6, calculate the maximum molarity of CuS in aqueous solution. the Write the reaction for dissociation of Cus. Find the concentration (molarity) according to it. (See Chap. equilibrium of XI part 1) |
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| 102 | ( 40 mathrm{mL} ) of ( 0.1 mathrm{M} ) ammonia solution is mixed with ( 20 mathrm{mL} ) of ( 0.1 mathrm{M} ) HCl What is the ( p H ) of the mixture? A . 5.74 B. 9.26 c. 4.56 D. 7.06 |
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| 103 | For making cake, baking powder is taken. If at home your mother uses baking soda instead of baking powder in cake, what is the role of tartaric acid added to baking soda? A. Make it more acidic B. Make it more basic c. Neutralise it D. None of these |
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| 104 | The colour of bleaching powder is : A. green B. pale yellow c. blue D. white |
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| 105 | Calculate the ( p H ) of a ( 0.033 mathrm{M} ) ammonia solution, if ( 0.033 mathrm{M} N H_{4} C l ) is introduced in this solution at the same temperature. ( left(k_{b} text { for } N H_{3}=1.77 timesright. ) ( left.10^{-5}right) ) |
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| 106 | What is pH formula? A. ( -log _{e}left[H^{+}right] ) B. ( -log _{10}left[H^{-}right] ) c. ( -log _{10}left[O H^{-}right] ) D. ( -log _{10}left[H^{+}right] ) |
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| 107 | The degree of dissociation of ( N_{2} O_{4} ) into ( N O_{2} ) at 1 atmosphere and ( 40^{circ} C ) is 0.25 Calculate its ( boldsymbol{K}_{boldsymbol{p}} ) at ( boldsymbol{4} boldsymbol{0}^{circ} boldsymbol{C} ) |
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| 108 | ( mathrm{NH}_{3}+mathrm{HCl} rightarrow ) | 11 |
| 109 | Calculate the solubility of ( A g C N ) in a buffer solution of ( boldsymbol{p} boldsymbol{H}=mathbf{3 . 0} ) ( boldsymbol{K}_{s p}(boldsymbol{A} boldsymbol{g} boldsymbol{C} boldsymbol{N})=mathbf{1 . 2} times ) ( mathbf{1 0}^{-16}, boldsymbol{K}_{boldsymbol{a}}(boldsymbol{H} boldsymbol{C N})=mathbf{4 . 8} times mathbf{1 0}^{-mathbf{1 0}} . ) There is no ( C N^{-} ) or ( A g^{+} ) ion in the buffer previously. |
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| 110 | The expression for equilibrium constant, ( K_{c} ) for the following reaction is : ( left.boldsymbol{F} boldsymbol{e}_{(}^{boldsymbol{3}+} boldsymbol{a} boldsymbol{q}right)+boldsymbol{3} boldsymbol{O} boldsymbol{H}_{(boldsymbol{a} boldsymbol{q})}^{-} rightleftharpoons boldsymbol{F} boldsymbol{e}(boldsymbol{O} boldsymbol{H})_{boldsymbol{3}(boldsymbol{s})} ) A ( cdot K_{c}=frac{left[F eleft(O H_{3}right)right]}{left[F e^{3+} mid D P Hright]^{5}} ) C . ( K_{c}=frac{1}{left[F e^{s+1}right]left(0 H^{-}right]^{s}} ) D. ( K_{c}=left[mathrm{Fe}left(mathrm{OH}_{3}right)right] ) |
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| 111 | 6. In a closed system A(S) – 4 B(g) + 3 C(g) If partial pressure of Cis doubled, then partial pressure of B will be (@) 202 times the original value (b) times the original value (©) 2 times of the original value (d) times of the original value |
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| 112 | The volume of the reaction vessel containing an equilibrium mixture in the reaction is increased, when equilibrium is re-established: ( boldsymbol{S} boldsymbol{O}_{2} boldsymbol{C l}_{2}(boldsymbol{g}) leftrightharpoons boldsymbol{S} boldsymbol{O}_{2}(boldsymbol{g})+boldsymbol{C l}_{2}(boldsymbol{g}) ) A. the amount of ( S O_{2} ) will have decreased B. the amount of ( S O_{2} C l_{2} ) will have increased c. the amount of ( C l_{2} ) will have increased D. the amount of ( C l_{2} ) will have remained unchanged |
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| 113 | Amphetamine ( left(C_{3} H_{13} Nright) ) is a weak base with ( p K_{b} ) of ( 4.2 . ) Calculate the ( p H ) of a solution containing an amphetamine concentration of ( 220 m g / L ) A . 3.49 B. 5.21 c. 10.5 D. 13.7 |
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| 114 | In a closed container rates of evaporation and condensation are same. What this statement indicate? A. A general rule for predicting solubility B. Conversion of solid phase to the liquid phase C. It represents relationship between absolute temperature and the kinetic energy of particles D. It represents relationship between volume and temperature at constant pressure E. A state in which the liquid and gas phases are in equilibrium |
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| 115 | For water at ( 25^{circ} mathrm{C}, 2 times 10^{-7} ) moles per litre is the correct answer for which one of the following? ( mathbf{A} cdotleft[H^{+}right]+left[O H^{-}right] ) B . ( left[H^{+}right]^{2} ) c. ( left[O H^{-}right]^{2} ) ( mathbf{D} cdotleft[H^{+}right]-left[O H^{-}right] ) |
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| 116 | mole of gas ( A B ) dissociates to an extent of ( 10 % ) at ( 127^{0} C ) according to ( A B rightleftharpoons A+B ) occupies a volume of ( 4 times 10^{4} ) ml. Find the total pressure at this temp, assuming ideal gas behaviour. |
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| 117 | Which reaction below demonstrates the lewis definition of acids and bases? ( mathbf{A} cdot H C l+N a O H rightarrow H O H+N a C l ) B. ( H_{2} O+N H_{3} rightarrow O H^{-}+N H_{4}^{+} ) ( mathbf{C} cdot N H_{3}+B F_{3} rightarrow N H_{3} B F_{3} ) D. ( H I+K O H rightarrow H_{2} O+K I ) E ( cdot H^{+} O H^{-} rightarrow H_{2} O ) |
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| 118 | Calculate pH of a solution whose ( 100 mathrm{m} ) contains ( 0.2 mathrm{g} ) NaOH dissolved in it? A . 10.699 в. 11.699 c. 12.699 D. 13.699 |
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| 119 | The pH of pure water at ( 25^{circ} mathrm{C} ) is close to: ( A cdot O ) B. 7 ( c cdot 2 ) D. 9 |
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| 120 | The ionic product of a saturated solution is ( _{-}-_{-}-_{-} ) the solubility product constant of its solute. A. lesser than B. greater than c. equal to D. not related to |
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| 121 | Acid buffer can be prepared by mixing solutions of: A ( . quad N a C l+N a O H ) в. ( H_{2} S O_{4}+N a_{2} S O_{4} ) c. ( N H_{4} O H+N H_{4} C l ) D. ( C H_{3} C O O N a+C H_{3} C O O H ) |
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| 122 | The pH of an aqueous solution of ( boldsymbol{C H}_{3} boldsymbol{C O O N} boldsymbol{a} ) of concentration ( boldsymbol{C}(boldsymbol{M}) ) if given by A ( cdot quad 7-frac{1}{2} p K_{a}-frac{1}{2} log C ) B. ( frac{1}{2}^{p K_{w}}+frac{1}{2} p K_{b}+frac{1}{2} log C ) ( ^{mathrm{c}} cdot frac{1}{2}^{p} K_{w}-frac{1}{2} p K_{b}-frac{1}{2} log C ) ( ^{mathrm{D} cdot frac{1}{2} p K_{w}+frac{1}{2} p K_{a}+frac{1}{2} log C} ) |
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| 123 | Give chemical name, formula, and uses of Washing soda. |
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| 124 | State True or False. According to Bronsted-Lowry theory, neutralization reaction is the formation of a conjugate acid base pair. A. True B. False |
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| 125 | Assertion The value of equilibrium constant depends on the stoichiometry of the equation. BECAUSE Reason The value of equilibrium constant does not change when the equation is multiplied or divided by a number. 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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| 126 | The solubility of ( N a C l ) in water is ( 38 g ) in ( 100 m L ) at ( 50^{circ} C ) I. If ( 50 g ) of salt is added to water, a dynamic equilibrium will be reached. II. A dissociation equilibrium will result in ( 50 % ) of the solute being in the aqueous state and ( 50 % ) being in the solid state. 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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| 127 | In which of the following reaction, the value of ( boldsymbol{K}_{boldsymbol{p}} ) will be equal to ( boldsymbol{K}_{c} ) ? A ( cdot H_{2}+I_{2} rightleftharpoons 2 H I ) в. ( P C l_{5} rightleftharpoons P C l_{3}+C l_{2} ) ( mathrm{c} cdot 2 N H_{3} rightleftharpoons N_{2}+3 H_{2} ) D. ( 2 S O_{2}+O_{2} rightleftharpoons 2 S O_{3} ) |
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| 128 | The bleaching action of bleaching powder is due to: A . oxidation B. reduction c. both A and B D. none of these |
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| 129 | For the reaction ( 2 A rightarrow B+3 C ); if ( -frac{boldsymbol{d}[boldsymbol{A}]}{boldsymbol{d} t}=boldsymbol{k}_{1}[boldsymbol{A}]^{2} ; frac{boldsymbol{d}[boldsymbol{B}]}{boldsymbol{d} t}= ) ( boldsymbol{k}_{2}[boldsymbol{A}]^{2} ; frac{boldsymbol{d}[boldsymbol{C}]}{boldsymbol{d} boldsymbol{t}}=boldsymbol{k}_{3}[boldsymbol{A}]^{2} ) the correct relation between ( k_{1}, k_{2} ) and ( k_{2} ) is: A ( cdot k_{1}=k_{2}=k_{2} ) B. ( 2 k_{1}=k_{2}=3 k_{2} ) ( mathbf{c} cdot 4 k_{1}=k_{2}=3 k_{2} ) D. ( frac{k_{1}}{2}=k_{2}=frac{k_{3}}{3} ) |
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| 130 | The main product obtained when a solution of sodium carbonate reacts with mercuric chloride is : ( mathbf{A} cdot H g(O H)_{2} ) в. ( H g C O_{3} . H g O ) ( mathrm{c} . mathrm{Hg} mathrm{CO}_{3} ) D. ( H g C O_{3} . H g(O H)_{2} ) |
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| 131 | The molecular formula of acetic acid is A. ( H C O O H ) в. ( C H_{3}-C H_{3} ) ( mathbf{c} cdot C_{6} H_{6} ) D. ( C_{2} H_{4} O 2 ) |
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| 132 | pH of ( 1 mathrm{M} ) HA (weak acid) is 2 . Hence, vant Hoff factor is A . 1.2 B. 1.02 c. ( 1 . ) D. 1.01 |
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| 133 | ( O H^{-} ) lon concentration in a acidic buffer solution is: ( ^{text {A } cdot} frac{K w[A]}{K a[S]} ) в. ( frac{K a[A]}{K w[S]} ) c. ( frac{K w[S]}{K a[A]} ) D. ( frac{K a[S]}{K w[A]} ) |
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| 134 | A solution is made of ( 0.1 ~ M C l^{-} ) and ( mathbf{1 0}^{-4} mathbf{M} mathbf{C r} mathbf{O}_{mathbf{4}}^{mathbf{2 -}} . ) If solid ( boldsymbol{A} boldsymbol{g} boldsymbol{N} boldsymbol{O}_{3} ) is gradually added to this solution, then what will be the concentration of ( C l^{-} ) when ( A g_{2} C r O_{4} ) begins to precipitate? ( left[boldsymbol{K}_{s p}(boldsymbol{A} boldsymbol{g} boldsymbol{C l})=right. ) ( mathbf{1 0}^{-mathbf{1 0}} boldsymbol{M}^{mathbf{2}} ; boldsymbol{K}_{boldsymbol{s p}}left(boldsymbol{A} boldsymbol{g}_{2} boldsymbol{C r} boldsymbol{O}_{4}right)= ) ( left.mathbf{1 0}^{-mathbf{1 2}} mathbf{M}^{mathbf{3}}right] ) В. ( 10^{-4} ) М ( mathbf{c} cdot 10^{-5} M ) D. ( 10^{-9} M ) |
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| 135 | ( left[B a^{2+}right] ) when ( C a S O_{4} ) starts just precipitation will be: ( mathbf{A} cdotleft[B a^{2+}right]=4.58 times 10^{-7} M ) B . ( left[B a^{2+}right]=5.58 times 10^{-7} M ) C ( cdotleft[B a^{2+}right]=4.85 times 10^{-7} M ) D. None of these |
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| 136 | ( 28 g ) of ( N_{2} ) and ( 6 g ) of ( H_{2} ) were kept at ( 400^{circ} mathrm{C} ) in 1 litre vessel, the equilibrium mixture contained ( 27.54 g ) of ( N H_{3} . ) The appropriate value of ( boldsymbol{K}_{c} ) for the above reaction can be (in mole( ^{-2} ) litre( ^{2} ) ) ( mathbf{A} cdot 75 ) B. 50 c. 25 D. 100 |
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| 137 | Neutral litmus solution have A. no effect of acidic solution B. no effect of alkaline solution C. both ( A ) and ( B ) D. none of these |
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| 138 | The two equilibrium ( boldsymbol{A B} leftrightharpoons boldsymbol{A}^{+}+boldsymbol{B}^{-} ) and ( A B+B^{-} leftrightharpoons A B_{2}^{-} ) are simultaneously maintained in a solution with equilibrium constant ( boldsymbol{K}_{mathbf{1}} ) and ( K_{2} ) respectively. The ratio of ( left[A^{+}right] ) to ( left[A B_{2}^{-}right] ) in the solution is: A. directly proportional to the concentration of ( B ) B . inversely proportional to the concentration of ( B ) c. directly proportional to the square of the concentration of ( B ) D. inversely proportional to the square of the concentration of ( B ) |
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| 139 | When chlorine is passed over dry slaked lime at room temperature, the main reaction product is: A ( cdot C aleft(C l O_{2}right)_{2} ) в. ( C a C l_{2} ) c. ( C a O C l ) D. ( operatorname{Ca}left(O C l_{2}right)_{2} ) |
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| 140 | Q28. Hydrogen gas is obtained from the natural gas by partial oxidation with steam as per following endothermic reaction: | CH, (g) + H20g) + COg) + 3H, (g) Write the expression for K, for the above reaction How will the value of K, and composition of equilibrium mixture be affected by: (i) increasing the pressure. (ii) increasing the temperature, (iii) using a catalyst? |
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| 141 | Backward reaction is favoured by increase in the pressure of which of the following equilibrium? A ( cdot 2 S O_{2}+O_{2} leftrightharpoons 2 S O_{3} ) в. ( N_{2}+O_{2} leftrightharpoons 2 N O ) c. ( N_{2}+3 H_{2} leftrightharpoons 2 N H_{3} ) D. ( P C l_{5} leftrightharpoons P C l_{3}+C l ) |
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| 142 | The precipitate of ( boldsymbol{C a} boldsymbol{F}_{2}left(boldsymbol{K}_{s p}=1.7 times 10^{-10}right) ) is obtained when equal volumes of the following are ( operatorname{mixed} ) ( begin{array}{lll}text { A. } 10^{-4} M & C a^{2-}+10^{-4} M & F^{-}end{array} ) ( begin{array}{lll}text { В. } 10^{-2} M & C a^{2-}+10^{-3} M & F^{-} \ & end{array} ) |
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| 143 | 1. The equilibrium expression, K = [CO] represents the reaction. (a) C(s) + O2(8) = CO2(8) (b) CaCO3(s) = Cao(s) + CO2(8) (C) CO(g) + 026) = 00,(8) (a) CaC(s) + CO2(g) = CaCO3(6) |
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| 144 | ( H_{2} O_{2} ) is decomposed to ( H_{2} O ) and ( O, ) in the following sequence of reactions: ( mathbf{I} boldsymbol{H}_{2} boldsymbol{O}_{2(boldsymbol{a q})}+boldsymbol{I}_{(boldsymbol{a} q)}^{-} rightarrow boldsymbol{H}_{2} boldsymbol{O}_{(l)}+boldsymbol{I} boldsymbol{O}_{(boldsymbol{a} boldsymbol{q})}^{-} ) ii) ( boldsymbol{H}_{2} boldsymbol{O}_{2(a q)}+boldsymbol{I}_{(a q)}^{-} rightarrow boldsymbol{H}_{2} boldsymbol{O}_{(l)}+ ) ( boldsymbol{O}_{2}(boldsymbol{g})+boldsymbol{I} boldsymbol{O}_{(boldsymbol{a} boldsymbol{q})}^{-} ) (a) Write the chemical equation for the overall reaction. (b) Identify the species that acts as a catalyst. (c) Identify the intermediate. |
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| 145 | Assertion An aqueous solution of ammonium acetate can act as a buffer. Reason Acetic acid is a weak acid and ( N H_{4} O H ) is a weak base. 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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| 146 | The ( K_{s p} ) for ( A g C l ) is ( 2.8 times 10^{-10} ) at a given temperature. The solubility of ( A g C l ) in 0.01 molar ( H C l ) solution at this temperature will be: A. ( 2.8 times 10^{-12} ) mol ( L^{-1} ) – B . ( 2.8 times 10^{-8} mathrm{mol} mathrm{L}^{-1} ) c. ( 5.6 times 10^{-8} ) mol ( L^{-1} ) D. 2.8 ( times 10^{-4} mathrm{mol} mathrm{L}^{-1} ) |
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| 147 | Which one of the following solutions will have the highest pH value? A. ( 0.01 M ) NaOH в. ( 0.02 M ) СН( _{3} ) СОО Na . c. ( 0.01 M ) NaHCO( _{3} ) D. ( 0.01 M H_{2} S O_{4} ) |
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| 148 | The van’t Hoff factor (i) for a dilute aqueous solution of the strong electrolyte barium hydroxide is : ( A cdot 2 ) B. 3 ( c cdot 0 ) D. |
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| 149 | The pH of an ( H C l ) solution is 2 Sufficient water is added to make the pH of new solutions. The hydrogen ion concentration is reduced: A. ten fold B. seven fold c. thousand fold D. hundred fold |
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| 150 | Which of the following expressions is correct? ( boldsymbol{A} cdot ldots_{p}=K_{c}left(frac{R T}{sum n}right)^{Delta n} ) ( mathrm{B} cdot quad K_{p}=K_{x}left(frac{P}{sum n}right)^{Delta n} ) ( mathrm{C} cdot_{p}=K_{n}left(frac{P}{sum n}right)^{Delta n-1} ) ( mathrm{D} cdot_{p}=K_{c}left(frac{P}{sum n}right)^{-Delta n+1} ) |
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| 151 | Which one of the following statements is not correct? A. The pH of ( 1.0 times 10^{-8} mathrm{M} mathrm{HCl} ) is less than 7 B. The ionic product of water at ( 25^{0} C ) is ( 1.0 times ) ( 10^{-14} mathrm{mol}^{2} L^{-2} ) C ( cdot C l^{-} ) is a Lewis acid D. Bronsted-Lowry theory cannot explain the acidic character of ( A l C l_{3} ) |
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| 152 | If ( K_{p} ) for a reaction is ( frac{1}{9} times 10^{-2} a t m^{-2} ) at 500K. Magnitude of ( K_{c} ) will be [Take ( R= ) 0.08] A. ( 3 times 10^{-1} ) В . ( frac{1}{9} times 10^{-2} ) ( c cdot frac{16}{9} ) D. Data insufficient |
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| 153 | In manufacture of sodium carbonate from Solvay (or ammonia soda) process the raw material used is: A . ( N a O H ) в. ( N a_{2} S O_{4} ) c. ( N a C l ) D. ( operatorname{NaH} mathrm{CO}_{3} ) |
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| 154 | Q58. The solubility of Sr (OH), at 298 K is 19.239/L of solution. Calculate the concentrations of strontium and hydroxyl ions and the pH of the solution. (Atomic mass of Sr = 87.6) 6 Chemistry. YI |
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| 155 | Assertion The melting point of ice decreases with increase of pressure. Reason Ice contracts on melting. 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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| 156 | 43. The degree of dissociation of an electrolyte depends on (1) dilution (2) impurities (3) atmospheric pressure (4) method of dissolution |
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| 157 | Consider the following salts: ( N a C l, H g C l_{2}, H g_{2} C l_{2}, C u C l_{2}, C u C l ) and ( A g C l ). Identify the correct set of insoluble salts in water. A. ( H g_{2} C l_{2}, C u C l, A g C l ) в. ( H g C l_{2}, C u C l, A g C l ) c. ( H g_{2} C l_{2}, C u C l_{2}, A g C l ) D. ( H g_{2} C l_{2}, C u C l, N a C l ) |
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| 158 | In a 20 litre vessel initially 1,1,1 mole of ( C O, H_{2} O, C O_{2} ) are present, then for the equilibrium of ( boldsymbol{C O}+boldsymbol{H}_{2} boldsymbol{O} rightleftharpoons ) ( C O_{2}+H_{2} . ) Which of the following is true? A. ( H_{2} ) more then 1 mole B. ( C O, H_{2} O, H_{2} ) less then 1 mole c. ( C O_{2} ) and ( H_{2} O ) both more than 1 mole D. All of these |
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| 159 | In the hydrolytic equilibrium; ( boldsymbol{B}^{+}+boldsymbol{H}_{2} boldsymbol{O} rightleftharpoons boldsymbol{B} boldsymbol{O} boldsymbol{H}+boldsymbol{H}^{+} ) ( K_{b}=1 times 10^{-5} . ) The hydrolysis constant is: A ( cdot 10^{-5} ) ( ^{5} ) B . ( 10^{-19} ) c. ( 10^{-10} ) D. ( 10^{-9} ) |
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| 160 | Consider the following solubility data for various chromates at ( 25^{circ} mathrm{C} ) [ begin{array}{cc} boldsymbol{K}_{boldsymbol{s} boldsymbol{p}} \ boldsymbol{A} boldsymbol{g}_{boldsymbol{2}} boldsymbol{C r} boldsymbol{O}_{boldsymbol{4}} & boldsymbol{9 . 0} times mathbf{1 0}^{-mathbf{1 2}} \ boldsymbol{B a C r} boldsymbol{O}_{boldsymbol{4}} & boldsymbol{2 . 0} times mathbf{1 0}^{-mathbf{1 0}} \ boldsymbol{P b C r O}_{boldsymbol{4}} & boldsymbol{1 . 8} times mathbf{1 0}^{-mathbf{1 4}} end{array} ] The chromate that is the most soluble in water at ( 25^{circ} mathrm{C} ) on a molar basis is ( mathbf{A} cdot A g_{2} C r O_{4} ) B ( . ) BaCr ( mathrm{O}_{4} ) ( mathbf{c} cdot P b C r O_{4} ) D. impossible to determine E. none of these |
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| 161 | In the reaction, ( boldsymbol{A}+mathbf{2} boldsymbol{B} rightleftharpoons mathbf{2} boldsymbol{C}, ) if ( mathbf{2} ) moles of ( A, 3.0 ) moles of ( B ) and 2.0 moles of ( C ) are placed in a ( 2 L ) flask and the equilibrium concentration of ( mathrm{C} ) is 0.5 mol ( / L . ) The equilibrium constant ( left(K_{c}right) ) for the reaction is: ( mathbf{A} cdot 0.073 ) B. 0.1470 c. 0.0500 D. 0.0080 |
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| 162 | For reactions involving gaseous reactants and products, the equilibrium constant ( boldsymbol{K}_{boldsymbol{p}} ) is written in terms of: A. the pressure of the gases B. the molar volumes of the gases c. the partial pressures of the gases D. the mole fraction of the gases |
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| 163 | Two flasks ( A ) and ( B ) of an equal volume containing 1 mole and 2 moles of ( 0_{3} ) respectively are heated to the same temperature. When the reaction ( 2 O_{3} rightleftharpoons ) ( 30_{2} ) practically stops, then both the flasks shall have A ( . ) the same ratio: ( left[O_{2}right] /left[O_{3}right] ) B. the same ratio: ( left[O_{2}right]^{3 / 2} /left[O_{3}right] ) c. only ( O_{2} ) D. the same time to reach equilibrium |
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| 164 | If first dissociation of ( boldsymbol{X}(boldsymbol{O} boldsymbol{H})_{3} ) is ( mathbf{1 0 0 %} ) whereas second dissociation is ( 50 % ) and third dissociation is negligible then the ( p H ) of ( 4 times 10^{-3} M X(O H)_{3} ) is : A. 11.78 B. 10.78 c. 2.5 D. 2.22 |
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| 165 | If the equilibrium constant of the reaction of weak acid ( boldsymbol{H} boldsymbol{A} ) with a strong base is ( 10^{9} ), then the ( p H ) of ( 0.1 M N a A ) solution will be: |
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| 166 | The solubility of ( A g C l ) is ( 1 times ) ( 10^{-5} ) mol ( / L . ) Its solubility in 0.1 molar sodium chloride solution is: A ( cdot 1 times 10^{-10} ) В. ( 1 times 10^{-5} ) c. ( 1 times 10^{-9} ) D. ( 1 times 10^{-4} ) |
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| 167 | The equilibrium constant for the reaction ( boldsymbol{C H}_{3} boldsymbol{C O O H}(boldsymbol{a q})+boldsymbol{C}_{2} boldsymbol{H}_{5} boldsymbol{O H}(boldsymbol{a q}) Leftrightarrow ) ( boldsymbol{C H}_{3} boldsymbol{C O O C}_{2} boldsymbol{H}_{5}(boldsymbol{a q})+boldsymbol{H}_{2} boldsymbol{O}(l) ) is 16 The initial concentration of each of ( C H_{3} C O O H ) and ( C_{2} H_{5} O H ) is two (mole/lit). What is the concentration of ( C H_{3} C O O C_{2} H_{5} ) at equilibrium in moles / lit? A. 0.9 B. 0.6 ( c cdot 1.6 ) D. 0.7 |
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| 168 | Q. 10 Acidity of BF, can be explained on the basis of which of the following concepts? (a) Arrhenius concept a (a) Arrhenius concept n d Us OTTO (b) Bronsted Lowry concept (c) Lewis concept (d) Bronsted Lowry as well as Lewis concept o n to prison |
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| 169 | The reaction quotient ( (Q) ) at equilibrium is: ( A cdot=1 ) в. ( =K ) ( c cdot>K ) ( mathrm{D} cdot<K ) |
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| 170 | Which of the following properties of a solution of ( N a C l ) will not vary as the concentration of salt is increased? A ( . p H ) B. Density c. Refractive index D. Electrical conductivity |
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| 171 | Ammonium hydrogen sulphide dissociates as follows ( N H_{4} H S(s) rightleftharpoons N H_{3}(g)+H_{2} S(g) ) If solid ( N H_{4} H S ) is placed in an evacuated flask at certain temperature it will dissociate until the total pressure is 600 torr. a) Calculate the value of equillibrium constant for the dissociation reaction b) Addional ( N H_{3} ) is introduced into the equillibrium mixture without changing the temperature until partial pressure of ( N H_{3} ) is 750 torr, what is the partial pressure of ( boldsymbol{H}_{2} boldsymbol{S} ) under these conditions? What is the total pressure in the flask? |
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| 172 | For the reaction, ( boldsymbol{A}(boldsymbol{g})+boldsymbol{B}(boldsymbol{g}) rightarrow ) ( C(g)+D(g) ) ( Delta H^{0} ) and ( Delta S^{0} ) are,respectively ( -29.8 k J m o l^{-1} ) and ( -0.100 k J K^{-1} ) ( operatorname{mol}-1 ) at ( 298 mathrm{K} ) The equilibrium constant for the reaction at ( 298 K ) is : |
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| 173 | Consider the following gas phase reaction: ( boldsymbol{H}_{2}(boldsymbol{g})+boldsymbol{B r}_{2}(boldsymbol{g}) rightleftharpoons 2 boldsymbol{H} boldsymbol{B} boldsymbol{r}(boldsymbol{g}) ) The concentrations of ( boldsymbol{H}_{2}, boldsymbol{B} boldsymbol{r}_{2}, ) and HBr are ( 0.05 M, 0.03 M, ) and ( 500.0 M ) respectively. The concentration equilibrium constant for this reaction ( operatorname{at} 400^{circ} mathrm{C} ) is ( 2.5 times 10^{3} . ) Is this system at equilibrium? A. Yes, the system is at equilibrium. B. No, the reaction must shift to the right in order to reach equilibrium. c. No, the reaction must shift to the left in order to reach equilibrium. D. It cannot be determined |
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| 174 | What is ( left[boldsymbol{H}^{+}right] ) in mol/L of a solution that is ( 0.20 mathrm{M} ) in ( C H_{3} C O O N a ) and ( 0.10 mathrm{M} ) in ( boldsymbol{C H}_{3} boldsymbol{C O O H} ? ) ( boldsymbol{K}_{a} ) for ( boldsymbol{C} boldsymbol{H}_{3} boldsymbol{C O O H}=mathbf{1 . 8} times mathbf{1 0}^{-mathbf{5}} ) A ( .3 .5 times 10^{-4} ) В. ( 1.1 times 10^{-5} ) c. ( 1.8 times 10^{-5} ) D. ( 9.0 times 10^{-6} ) |
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| 175 | Assertion ( N H_{3} ) is a Lewis base. Reason Ammonia can accept a proton. A. Both Assertion and Reason are correct and the Reason is the correct explanation of the Assertion B. Both Assertion and Reason are correct but the Reason is not the correct explanation of the Assertion C. The Assertion is correct but the Reason is incorrect D. The Assertion is incorrect and the Reason is correct |
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| 176 | For the reaction, ( boldsymbol{C O}_{(boldsymbol{g})}+boldsymbol{C l}_{2(boldsymbol{g})} rightleftharpoons ) ( C O C l_{2(g)}, ) the value of ( K_{p} / K_{c} ) is equal to? A . 1.0 в. RT c. ( sqrt{R T} ) D. ( frac{1}{R T} ) |
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| 177 | Calculate the ( p H ) after the addition of ( 90 m l ) and ( 100 m l ) respectively of ( mathbf{0 . 1} N ) NaOH to ( 100 m l 0.1 N C H_{3} C O O H ) (Given ( left.p K_{a} text { for } C H_{3} C O O H=4.74right) ) |
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| 178 | A mixture of three gases P (density 0.90)( , Q(text { density } 0.178) ) and ( R( ) density 0.42) is enclosed in a vessel at the constant temperature. When the equilibrium is established: A. the gas P will be at the top of the vessel B. the gas Q will be at the top of the vessel c. the gas ( R ) will be at the top of the vessel D. the gases will mix homogeneously throughout the vessel |
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| 179 | The pH of a tomato juice is: A . B. 4 ( c cdot 7 ) D. 14 |
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| 180 | If the ( K_{b} ) value in the hydrolysis reaction, ( boldsymbol{B}^{+}+boldsymbol{H}_{2} boldsymbol{O} rightleftharpoons boldsymbol{B O H}+boldsymbol{H}^{+} ) is ( 1.0 times 10^{-6}, ) then the hydrolysis constant of the salt would be: A ( .1 .0 times 10^{-6} ) В. ( 1.0 times 10^{-7} ) c. ( 1.0 times 10^{-8} ) D . ( 1.0 times 10^{-9} ) |
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| 181 | Equilibrium constant for an equilibrium reaction is ( 100 . ) Its forward reaction rate constant ( boldsymbol{K}_{boldsymbol{f}}=mathbf{1 0}^{mathbf{5}} . ) Its backward reaction rate constant ( boldsymbol{K}_{boldsymbol{b}} ) is; A ( cdot 10^{2} ) B. 10 ( c cdot 10^{4} ) D. ( 10^{3} ) |
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| 182 | ( M Y ) and ( N Y_{3}, ) two nearly insoluble salts, have the same ( boldsymbol{K}_{s p} ) values of ( 6.2 times 10^{-13} ) at room temperature Which statement would be true in regards to ( M Y ) and ( N Y_{3} ? ) A. The molar solubilities of ( M Y ) and ( N Y_{3} ) in water are identical. B. The molar solubility of ( M Y ) in water is less than that of ( N Y_{3} ) C. The salts ( M Y ) and ( N Y_{3} ) are more soluble in ( 0.5 M K Y ) than in pure water. D. The addition of the salt of KY to solution of ( M Y ) and ( N Y_{3} ) will have no effect on their solubilities |
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| 183 | A strong electrolyte in aqueous solution exhibit: This question has multiple correct options A. almost completely dissociated B. hydration c. partial dissociation D. none of the above |
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| 184 | Carbonic acid generally displaces another acid when the acid is heated with a salt. A. True B. False |
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| 185 | ( K_{a} ) for acetic acid in water is ( 1.7 times ) ( 10^{-5} ) at ( 25^{circ} mathrm{C} . ) The ( mathrm{pH} ) of a mixture of 25 ( mathrm{ml} ) of ( 0.02 mathrm{N} ) acetic acid and ( 2.5 mathrm{ml} ) of 0.1N NaOH (neglecting volume change) will be ( (log 1.7=0.23) ) A . 2. B. 4.8 ( c .7 .5 ) D. 1.0. |
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| 186 | In general, as the temperature increases, the solubility of gases in water ( _{text {十一一一一一一一一一 }} ) and the solubility of most solids in water A. decreases, decreases B. decreases, increases c. increases, decreases D. increases, increases |
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| 187 | Write the application of sodium bicarbonate (baking soda)? |
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| 188 | What is the ( K_{c} ) for the reaction: ( boldsymbol{M} boldsymbol{g}(boldsymbol{O} boldsymbol{H})_{2(s)}+boldsymbol{2} boldsymbol{N} boldsymbol{H}_{4(a q)}^{+} rightleftharpoons ) ( mathbf{2} boldsymbol{N} boldsymbol{H}_{3(boldsymbol{g})}+mathbf{2 H}_{mathbf{2}} boldsymbol{O}_{(boldsymbol{a q})}+boldsymbol{M} boldsymbol{g}_{(boldsymbol{a q})}^{mathbf{2 +}} ) (Given that the solubility product for ( M g(O H)_{2}, K_{s p} ) is ( 6 times 10^{-12} ) mol ( ^{3} L^{-3} ) and the base dissociation constant for ( N H_{4} O H, K_{b} ) is ( 1.8 times 10^{-5} m o l L^{-1} ) A ( cdot 2.05 times 10^{-2} ) В. ( 1.65 times 10^{-2} ) c. ( 1.85 times 10^{-2} ) D. None of these |
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| 189 | The total number of basic groups in the following form of lysine is: ( A ) B. ( c cdot 2 ) ( D ) ( E cdot 4 ) ( F .5 ) ( G cdot 6 ) H. 8 |
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| 190 | Predict which of the following reaction will have appreciable concentration of reactants and products: a) ( C l_{2}(g) rightleftharpoons 2 C l(g) ; K_{c}=5 times 10^{-39} ) b) ( C l_{2}(g)+2 N O(g) rightleftharpoons ) ( mathbf{2} boldsymbol{N} boldsymbol{O} boldsymbol{C l}(boldsymbol{g}) ; boldsymbol{K}_{c}=mathbf{3 . 7} times mathbf{1 0}^{mathbf{8}} ) c) ( C l_{2}(g)+2 N O_{2}(g) rightleftharpoons ) ( mathbf{2} boldsymbol{N} boldsymbol{O}_{2} boldsymbol{C l}(boldsymbol{g}) ; boldsymbol{K}_{c}=mathbf{1 . 8} ) |
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| 191 | Which of the following will occur if a 1.0 M solution of a weak acid is diluted to ( 0.01 mathrm{M} ) at constant temperature: A. Percentage ionisation will increase B. [H+] will decrease to 0.01 M c. ( K_{a} ) will increase D. pH will decrease by 2 units |
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| 192 | The state of equilibrium refers to: A. State of rest B. Dynamic state c. Stationary state D. State of inertness |
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| 193 | In aqueous solution, the following mixture acts as buffer: A. ( H N O_{3}+K N O_{3} ) в. ( H_{2} S O_{4}+K_{2} S O_{4} ) c. ( N H_{4} O H+N H_{4} C l ) D. ( C H_{3} C O O H+N a C l ) |
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| 194 | An equilibrium mixture for the reaction ( mathbf{2} boldsymbol{H}_{2} boldsymbol{S}(boldsymbol{g}) rightleftharpoons mathbf{2} boldsymbol{H}_{2}(boldsymbol{g})+boldsymbol{S}_{2}(boldsymbol{g}) ) has 1 mole of ( H_{2} S, 0.2 ) mole of ( H_{2} ) and 0.8 mole of ( S_{2} ) in a 2 litre flask. The value of ( boldsymbol{K}_{c} ) in mol ( boldsymbol{L}^{-1} ) is ( mathbf{A} cdot 0.004 ) B. 0.08 c. 0.016 D. 0.160 |
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| 195 | Calculate the amount of ammonium chloride required to dissolve in ( 500 m L ) water to have ( boldsymbol{p} boldsymbol{H}=mathbf{4 . 5}left(boldsymbol{K}_{boldsymbol{b}} ) for right. ( left.N H_{4} O H text { is } 1.8 times 10^{-5}right) ) |
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| 196 | Which of the following solutions will be acidic? (1) ( 0.1 M F e S O_{4} ) (2) ( 0.1 Mleft(N H_{4}right)_{2} S O_{4} ) (3) ( 0.1 M C H_{3} C O O N a ) (4) ( 0.1 M N H_{4} O H ) A ( cdot 1,2 ) and 3 are correct B. 1 and 2 are correct ( c cdot 2 ) and 4 are correct D. 1 and 3 are correct |
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| 197 | The molar concentrations of ( A, B ) and ( C ) at equilibrium for the reaction ( boldsymbol{A}+ ) ( 2 B Leftrightarrow 3 C ) are 2,3 and 4 moles/lit respectively. Its ( boldsymbol{K}_{c} ) is: ( A cdot 2 ) в. 3.56 ( c cdot 0.2 ) D. 0.026 |
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| 198 | A weak acid HA after treatment with 12 mL of 0.1 M strong base has a pH of ( 5 . ) At the end point, the volume of same base required is ( 26.6 mathrm{mL} ). The value of ( K_{a} ) is: A ( .8 .2 times 10^{-6} ) B . ( 6.4 times 10^{-6} ) ( mathbf{c} cdot 5.3 times 10^{-5} ) D. ( 2.4 times 10^{-6} ) |
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| 199 | 1 mole of ( C H_{3} C O O H ) and 1 mole of ( C H_{3} C O O N a ) are dissolved in water to form 1 litre aqueous solution. The pH of the resulting solution will be: A . 9.2553 в. 4.7447 c. 14 D. |
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| 200 | The concentration of a solution is ( mathbf{1 0}^{-4} boldsymbol{M} ) for ( boldsymbol{C l}^{-}, mathbf{1 0}^{-mathbf{5}} boldsymbol{M} ) for ( boldsymbol{B r}^{-} ) and ( 10^{-3} mathrm{M} ) for ( I^{-} . A g N O_{3}(s) ) is added slowly to the solution. If the minimum concentration of ( boldsymbol{A} boldsymbol{g}^{+} ) required to start precipitation of all three ions is ( 10^{-x} ) then the value of ( x ) is ( left[text { Given, } boldsymbol{K}_{s p(A g C l)}=mathbf{1 0}^{-mathbf{1 0}}, boldsymbol{K}_{s p(A g B r)}=right. ) ( left.mathbf{1 0}^{-mathbf{1 3}}, boldsymbol{K}_{boldsymbol{s p}(boldsymbol{A g I})}=mathbf{1 0}^{-mathbf{1 7}}right] ) |
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| 201 | A vessel of 250 litre was filled with 0.01 mole of ( S b_{2} S_{3} ) and 0.01 mole of ( H_{2} ) to attain the equilibrium at ( 440^{circ} mathrm{C} ) as : [ begin{array}{r} boldsymbol{S b}_{2} boldsymbol{S}_{3}(boldsymbol{s})+mathbf{3} boldsymbol{H}_{2}(boldsymbol{g}) rightleftharpoons mathbf{2} boldsymbol{S} boldsymbol{b}(boldsymbol{s})+ \ mathbf{3} boldsymbol{H}_{2} boldsymbol{S}(boldsymbol{g}) end{array} ] After equilibrium, the ( H_{2} S ) formed was analysed by dissolved it in water and treating with excess of ( P b^{2+} ) to give 1.19g of ( P b S ) as precipitate. What is the value of ( boldsymbol{K}_{c} ) at ( mathbf{4 4 0}^{circ} boldsymbol{C} ) A . B. 2 ( c cdot 4 ) D. |
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| 202 | Arrange the following acids in increasing order of their acid strength: I. ( boldsymbol{H} boldsymbol{C l O}_{mathbf{4}} ) II. ( quad H_{2} S O_{4} ) III ( . ) A. ( I I I<I I<I ) B. ( I<I I<I I I ) c. ( I I<I I I<I ) D. III ( <I<I I ) |
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| 203 | The solubility ( A g C l ) is maximum in: A. acidic buffer solution B. basic buffer solution c. In pure water D. equal in all solutions |
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| 204 | If ( K_{a} ) is more (or) ( p k_{a} ) is less then more stronger is the acid. lonic order: ( boldsymbol{H} boldsymbol{C O O H}>boldsymbol{C}_{mathbf{6}} boldsymbol{H}_{mathbf{5}} boldsymbol{C O O H} ) |
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| 205 | Anhydrous sodium carbonate is commonly known as: A. baking soda B. washing soda c. chalk D. paris white |
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| 206 | Which of the following salt undergoes hydrolysis? A. ( C H_{3} ) СООК в. ( operatorname{NaNO}_{3} ) c. ( K C l ) D. ( K_{2} S O_{4} ) |
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| 207 | At equilibrium,in solution a certain ( operatorname{acid}, boldsymbol{H} boldsymbol{A}, ) yields ( [boldsymbol{H} boldsymbol{A}]=mathbf{0 . 9 4} boldsymbol{M} ) and ( left[A^{-}right]=0.060 M . ) On the basis of the above data given (A) Calculate ( K_{a} ) (B) Is this acid stronger or weaker than sulfurous acid ( left(boldsymbol{K}_{boldsymbol{a}}=mathbf{1 . 7} times mathbf{1 0}^{-mathbf{2}}right) ? ) (C) Calculate ( K_{b} ) (D) Calculate pH |
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| 208 | The amount of ( left(N H_{4}right)_{2} S O_{4} ) having degree of dissocation ( 75 % ) which should be dissolved in ( 1500 mathrm{ml} ) of ( 1 mathrm{M} N H_{4} mathrm{OH} ) to decrease its degree of dissociation by 200 times, is ( left[k_{b} text { of } N H_{4} O H=1.8right. ) ( left.times 10^{-5}right]: ) A . ( 112.1 mathrm{gm} ) B. 224.2 gm c. ( 56.0 mathrm{gm} ) D. 65.4gm |
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| 209 | A two litre vessel contains 0.48 mole of ( C O_{2}, 0.48 ) mole of ( H_{2}, 0.96 ) mole of ( C O ) at equilibrium [ boldsymbol{C O}_{2}(boldsymbol{g})+boldsymbol{H}_{2}(boldsymbol{g}) rightleftharpoons boldsymbol{H}_{2} boldsymbol{O}(boldsymbol{g})+ ] ( boldsymbol{C O}(boldsymbol{g}) ) How many ( g m ) (only integer part) of ( boldsymbol{H}_{2} ) must be added to bring the concentration of ( C O ) to ( 0.6 M ? ) |
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| 210 | At a particular temperature and atmospheric pressure, the solid and liquid phases of a pure substance can exist in equilibrium. Which of the following term defines this temperature? (a) Normal melting point (b) Equilibrium temperature (c) Boiling point (d) Freezing point |
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| 211 | Predict if there will be any precipitate by mixing ( 50 mathrm{mL} ) of ( 0.01 mathrm{M} ) NaCl and 50 mL of ( 0.01 mathrm{M} A g N O_{3} ) solution. The solubility product of ( A g C l ) is ( 1.5 times ) ( 10^{-10} ) A. since ionic product is greater than solubility product no precipitate will be formed B. since ionic product is lesser than solubility product. precipitation will occur c. since ionic product is greater than solubility product. precipitation will occur. D. since ionic product and solubility product are same, precipitation will not occur |
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| 212 | The ionisation of strong electrolytes in acetic acid compared to that in water is A. weak B. Strong c. Medium D. No ionisation |
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| 213 | A weak acid ( boldsymbol{H} boldsymbol{X}left(boldsymbol{K}_{boldsymbol{a}}=mathbf{1} times mathbf{1 0}^{-mathbf{5}}right) ) on reaction with NaOH gives NaX. For ( 0.1 mathrm{M} ) aqueous solution of NaX, the % hydrolysis is: A . 0.001% B . 0.01% c. ( 0.15 % ) D. 1% |
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| 214 | A sulphate salt of group 2 element of the periodic table is a white, soft substance, which can be moulded into different shapes by making its dough. When this compound is left in open for some time, it becomes a solid mass and cannot be used for moulding purposes. Identify the sulphate salt. A. White paris B. Plaster of paris c. Calcium hydroxide D. Calcium carbonate |
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| 215 | Initially the reactions in the containers a and b are at equilibrium when the products and reactants are put together in a container ( c ) than at the equilibrium the total number of different chemical compounds are? A. 5 B. 7 ( c cdot 6 ) ( D ) |
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| 216 | Predict the direction of the reaction from the comparison of ( Q_{c}, K_{c} . ) Mark the incorrect statement. A ( cdot ) If ( Q_{c}K_{c} ), net reaction goes from right to left D. If ( Q_{c}=K_{c} ), reactants and products are at equilibrium. |
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| 217 | ( P C l_{5} ) dissociates according to the reaction ( boldsymbol{P} boldsymbol{C l}_{5} rightleftharpoons boldsymbol{P} boldsymbol{C l}_{3}(boldsymbol{g})+boldsymbol{C l}_{2}(boldsymbol{g}) cdot mathbf{A t} ) ( mathbf{5} mathbf{2 3} boldsymbol{K}, boldsymbol{K}_{boldsymbol{p}}=mathbf{1 . 7 8} boldsymbol{a t m} . ) Find the density of the equilibrium mixture at a total pressure of 1 atm. A. 2.96 g/ml B. 4.51 ( g / m ) । c. 6.73 g/ml D. 3.44 g/ml |
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| 218 | At ( 80^{circ} C, ) distilled water has hydronium ( operatorname{ion}left(H_{3} O^{+}right) ) concentration equal to ( 1 times ) ( 10^{-6} ) mol ( / l . ) The value of ( K_{w} ) at this temperature would be: A ( cdot 1 times 10^{-6} ) В. ( 1 times 10^{-12} ) c. ( 1 times 10^{-9} ) D. ( 1 times 10^{-14} ) |
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| 219 | Addition of ( H C l ) will not suppress the ionization of: A . acetic acid B. benzoic acid ( mathrm{c} cdot mathrm{H}_{2} ) D. sulphuric acid |
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| 220 | For a reversible equilibrium reaction ( K_{C}>K_{P} ) at ( 298 K ) and ( Delta H=+200 ) ( K J, ) the forward reaction is favoured if: (i) Pressure is increased (ii) Temperature is increased (iii) Temperature is decreased (iv) Increasing the concnetration of reactants A . i, i i, iv B. i, ii c. ii, iv D. i, iii, iv |
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| 221 | The equilibrium constant ( K_{C} ) for the reaction, ( A(g)+2 B(g) rightleftharpoons 3 C(g) ) is ( 2 times 10^{-3} ) What would be the equilibrium partial pressure of gas ( C ) if initial pressure of ( operatorname{gas} A ) and ( B ) are 1 and 2 |
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| 222 | The equilibrium concentration of ( C_{2} H_{4} ) in the following gas phase reaction can be increased by: ( boldsymbol{C}_{2} boldsymbol{H}_{4}(boldsymbol{g})+boldsymbol{H}_{2}(boldsymbol{g}) rightleftharpoons ) ( boldsymbol{C}_{2} boldsymbol{H}_{6}(boldsymbol{g}), quad boldsymbol{Delta} boldsymbol{H}=-mathbf{3 2 . 7} boldsymbol{k} boldsymbol{c a l} ) A ( cdot ) removal of ( C_{2} H_{6} ) B. removing ( H_{2} ) c. decrease in temperature D. increase in pressure |
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| 223 | Which are general property of Bronsted acids? This question has multiple correct options A. They turn litmus red B. They react with alkalies c. They burn the skin D. They contain ( H ) -atom replaceable with metal |
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| 224 | One litre solution contains ( 1 M ) HOCl ( left[boldsymbol{K}_{a}=mathbf{1 0}^{-8}right] ) and ( 1 M ) NaOH.What is the ( p H ) of the solution? A. 8 B. 1 ( c cdot 5 ) D. 2 |
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| 225 | The ( p K_{a} ) of acetic acid and ( p K_{b} ) of ( N H_{4} O H ) are 4.76 and ( 4.75 . ) Calculate the ( p H ) of ammonium acetate ions. |
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| 226 | About buffer solution which is correct? This question has multiple correct options A. It contains a weak acid and its conjugate base B. It contains a weak base and its conjugate acid C. It shows change in ( mathrm{pH} ) on adding small amount of acid or base D. All of the above |
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| 227 | At ( 800 mathrm{K} ) a reaction mixture contained 0.5 mole of ( S O_{2} .0 .12 ) mole of ( O_{2} ) and 5 mole of ( S O_{3} ) at equilibrium. ( K_{c} ) for the equilibrium ( 2 S O_{2}+O_{2} rightleftharpoons 2 S O_{3} ) is 833 lit/ mole. If the voiume of the container is 1 litre, calculate how much ( O_{2} ) is to be added at this equilibrium in order to get 5.2 moles of ( S O_{3} ) at the same temperature. A. 2.34 mole B. 0.34 mole c. 1.43 mole D. 3.23 mole |
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| 228 | On the addition of a solution containing ( C r O_{4}^{2-} ) ions to the solution of ( B a^{2+}, S r^{2+}, C a^{2+} ) ions, the precipitate obtained first will be of: A. ( C a C r O_{4} ) B ( . ) SrCrO ( _{4} ) ( mathrm{c} cdot B a C r O_{4} ) D. A mixture of all the three |
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| 229 | Which of the following reactions proceed in forward direction with an increase in temperature? ( mathbf{A} cdot H_{2}(g)+I_{2}(g) rightleftharpoons 2 H I(g)+3000 c a l ) B ( cdot N_{2}(g)+O_{2}(g) rightleftharpoons 2 N O(g)-43200 c a l ) ( mathbf{c} cdot N_{2}(g)+3 H_{2}(g) rightleftharpoons 2 N H_{3}(g)+22400 c a l ) ( mathbf{D} cdot C(g)+O_{2}(g) rightleftharpoons C O_{2}(g)+94300 c a l ) |
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| 230 | For which one of the following reactions will ( boldsymbol{K}_{boldsymbol{C}}=boldsymbol{K}_{boldsymbol{P}} ) A ( cdot C O(g)+2 H_{2}(g) rightleftharpoons C H_{3} O H(g) ) в. ( Z n O(s)+C O(g) rightleftharpoons Z n(s)+C O_{2}(g) ) ( mathrm{c} cdot 2 mathrm{O}_{3}(g) rightleftharpoons 3 mathrm{O}_{2}(g) ) D. ( operatorname{COCl}_{2}(g) rightleftharpoons operatorname{CO}(g)+C l_{2}(g) ) |
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| 231 | Drive the following relation: ( boldsymbol{K} boldsymbol{p}=boldsymbol{K} boldsymbol{c}(boldsymbol{R} boldsymbol{T})^{n} ) |
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| 232 | A solution has ( p H ) 2. It contains: A. ( C H_{3} ) СООН в. ( H_{2} C O_{3} ) c. ( H N O_{3} ) ( mathrm{D} cdot mathrm{H}_{2} mathrm{C}_{2} mathrm{O}_{4} ) |
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| 233 | Study the figure given below and mark the correct statement about ( K_{c} ) and dependence of extent of reaction on it. A. ( x ) – Reaction does not occur Y – Reaction proceeds to completion; Z – Reaction does not occur B. X- Reaction completes; Y – Reaction does not occur; Z Reactants and products are at equilibrium c. ( x ) – Reaction hardly occurs; Y – Reactants and products are at equilibrium; Z – Reaction proceeds completion D. ( x ) – Reaction proceeds completion; ( Y ) – Reactants and products are at equilibrium; Z – Reaction hardly occurs |
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| 234 | A monoprotic acid in ( 1.00 M ) solution is ( 0.001 % ) ionised. The dissociation constant of acid is: A. ( 1 times 10^{-3} ) В. ( 1 times 10^{-6} ) c. ( 1 times 10^{-8} ) D. ( 1 times 10^{-10} ) |
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| 235 | Fresh milk has a pH of 6. Explain why the pH changes as it turns into curd? | 11 |
| 236 | The reaction is of first order in each diagram, with an equilibrium constant of ( 10^{4} . ) For the conversion of chair form to boat form ( e^{-E a / R T}=4.35 times 10^{-8} mathrm{at} ) ( 298 K ) with pre-exponential factor of ( 10^{12} s^{-1} . ) Apparent rate constant ( left(=k_{A}right) ) at ( 298 K ) is: A. ( 4.35 times 10^{4} s^{-1} ) в. ( 4.35 times 10^{8} s^{-1} ) c. ( 4.35 times 10^{-8} s^{-1} ) D. ( 4.35 times 10^{12} s^{-1} ) |
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| 237 | The solubility product expression for silver (I) sulfide, using x to represent the molar concentration of silver (I) and y to represent the molar concentration of sulfide, is formulated as A ( . x y ) B . ( x^{2} y ) c. ( x y^{2} ) D. ( x^{2} y^{2} ) E ( cdot x y^{3} ) |
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| 238 | Ammonium sulfate is an example of: A. an acid B. a base c. an acidic salt D. a basic salt |
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| 239 | Which of the following according to LeChatelier’s principle is correct? A. Increase in temperature favours the endothermic reaction B. Increase in temperature favours the exothermic reaction c. Increase in pressure shifts the equilibrium in that side in which number of gaseous moles increases D. All of the above are true |
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| 240 | The value of ( K_{c}=4.24 ) at ( 800 K ) for the reaction ( boldsymbol{C O}(boldsymbol{g})+boldsymbol{H}_{2} boldsymbol{O}(boldsymbol{g}) rightleftharpoons boldsymbol{C} boldsymbol{O}_{2}(boldsymbol{g})+boldsymbol{H}_{2}(boldsymbol{g}) ) Calculate equilibrium concentrations of ( C O_{2}, H_{2}, C O ) and ( H_{2} O ) at ( 800 K, ) if only ( C O ) and ( H_{2} O ) are present initially at concentration of ( 0.10 M ) each? |
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| 241 | ( mathbf{5 0 m} boldsymbol{L} ) of ( mathbf{0 . 1 0} boldsymbol{M} boldsymbol{N} boldsymbol{a}_{3} boldsymbol{P} boldsymbol{O}_{4}+mathbf{5 0 m} boldsymbol{L} ) of ( mathbf{0 . 1 0} boldsymbol{M} boldsymbol{N a H}_{2} boldsymbol{O}_{4} ) |
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| 242 | The unit of equilibrium constant for the following reaction is: ( mathbf{2} N boldsymbol{O}_{2}(boldsymbol{g}) rightleftharpoons boldsymbol{N}_{2} boldsymbol{O}_{4}(boldsymbol{g}) ) A ( . ) mol ( L^{-1} ) B. ( L ) mol ( ^{-1} ) c. ( m o l^{-1} L^{-1} ) D. Equilibrium constant is unitless |
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| 243 | The order of pH of ( 0.200 mathrm{M} ) solutions of ( N H_{4} N O_{3}, N a N O_{3} ) and ( N a_{2} C O_{3} ) is : A. ( N H_{4} N O_{3}<N a_{2} C O_{3}<N a N O_{3} ) в. ( N H_{4} N O_{3}<N a N O_{3}<N a_{2} C O_{3} ) c. ( N a_{2} C O_{3}<N a N O_{3}<N H_{4} N O_{3} ) D. ( N a_{2} N O_{3}<N H_{4} N O_{3}<N a_{2} C O_{3} ) |
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| 244 | When ( N a N O_{3} ) is heated in a closed vessel, ( O_{2} ) is liberated and ( N a N O_{2} ) is left behind. At equilibrium: A. increased temperature favours forward reaction B. addition of ( N a N O_{2} ) favours reverse reaction c. increased pressure favours forward reaction D. adding of ( N a N O_{2} ) favours forward reaction |
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| 245 | ( p H ) of a ( 0.001 mathrm{M} ) NaOH solution will be: ( A cdot 9 ) B. 3 ( c ) D. 12 |
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| 246 | The value of ( K_{c}=4.24 ) at ( 800 K ) for the reaction ( boldsymbol{C O}(boldsymbol{g})+boldsymbol{H}_{2} boldsymbol{O}(boldsymbol{g}) rightleftharpoons boldsymbol{C} boldsymbol{O}_{2}(boldsymbol{g})+boldsymbol{H}_{2}(boldsymbol{g}) ) Calculate equilibrium concentrations of ( C O_{2}, H_{2}, C O ) and ( H_{2} O ) at ( 800 K, ) if only ( C O ) and ( H_{2} O ) are present initially at concentration of ( 0.10 M ) each? |
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| 247 | The value of ( K_{c} ) for the reaction: ( 2 A rightleftharpoons ) ( B+C ) is ( 2 times 10^{-3} ). At a given time the composition of reaction mixture is ( [boldsymbol{A}]=[boldsymbol{B}]=[boldsymbol{C}]=mathbf{3} times mathbf{1 0}^{-4} boldsymbol{M} . ) In which direction the reaction will proceed? A. Forward B. Backward c. At equilibrium D. Forward or Backward |
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| 248 | The amount of ( left(N H_{4}right)_{2} S O_{4} ) to be added to ( 500 mathrm{mL} ) of ( 0.01 mathrm{m} N H_{4} O H ) solution ( boldsymbol{p} boldsymbol{K}_{boldsymbol{a}} ) for ( boldsymbol{N} boldsymbol{H}_{4}^{+} ) is ( boldsymbol{9} .2 boldsymbol{6} ) ) prepare a buffer of ( p H=8.26 ) is? A. 0.05 mole B. 0.025 mole c. 0.10 mole D. 0.005 mole |
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| 249 | To ( 500 m L ) of ( 0.150 M A g N O_{3} ) solution were added ( 500 m L ) of ( 1.09 M F e^{2+} ) solution and the reaction is allowed to reach an equilibrium at 25 [ begin{array}{r} boldsymbol{A} boldsymbol{g}^{+}(boldsymbol{a} boldsymbol{q})+boldsymbol{F} boldsymbol{e}^{2+}(boldsymbol{a} boldsymbol{q}) rightleftharpoons \ boldsymbol{F} boldsymbol{e}^{3+}(boldsymbol{a} boldsymbol{q})+boldsymbol{A} boldsymbol{g}(boldsymbol{s}) end{array} ] For ( 25 m L ) of the solution, ( 30 m L ) of ( 0.0832 M K M n O_{4} ) were required for oxidation. The equilibrium constant for the reaction at ( 25^{circ} mathrm{C} ) is |
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| 250 | The homogeneous reaction is carried out in a 2 -litre container at a particular temperature by taking 1 mole each of A, B, ( C ) and ( D ) respectively. If ( K_{C} ) for the reaction is ( frac{1}{4} ) then the equilibrium concentration of ( mathrm{C} ) is : ( boldsymbol{A}(boldsymbol{g})+boldsymbol{B}(boldsymbol{g}) rightleftharpoons boldsymbol{C}(boldsymbol{g})+boldsymbol{D}(boldsymbol{g}) ) A ( cdot frac{1}{3} M ) в. ( frac{2}{3} ) ( ^{c} cdot frac{4}{3}^{M} ) D. ( frac{1}{2} M ) |
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| 251 | Which of the following is a true statement: A. The ionisation constant and ionic product of water are same. B. Water is a strong electrolyte. C. The value of ionic product of water is less than that of its ionisation constant D. At ( 298 K ), the number of ( H^{+} ) ions in a litre of water is ( 6.023 times 10^{16} ) |
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| 252 | When heating ( P C l_{5}, ) it decompose ( P C l_{3} ) and ( C l_{2} ) in form of gas. The vapour density of gas mixture is 70.2 and 57.9 at ( 200^{circ} mathrm{C} ) and ( 250^{circ} mathrm{C} ). The degree of dissociation of ( P C l_{5} ) at ( 200^{circ} C ) at ( 250^{circ} C ) is: A . ( 48.50 % ) and ( 80 % ) B. 60% and 70% c. ( 70 % ) and ( 80 % ) D. 80% and 90% |
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| 253 | The rate constant for the forward and backward reactions of hydrolysis of ester are ( 1.1 times 10^{-2} ) and ( 1.5 times 10^{-3} ) respectively. The equilibrium constant of the following reaction is: ( boldsymbol{C H}_{3} boldsymbol{C O O C}_{2} boldsymbol{H}_{5}+boldsymbol{H}^{+} rightleftharpoons ) ( boldsymbol{C H}_{3} boldsymbol{C O O H}+boldsymbol{C}_{2} boldsymbol{H}_{5} boldsymbol{O H} ) A . 6.33 в. 7.75 ( c .7 .33 ) D. 8.33 |
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| 254 | Consider the two gaseous equilibrium involving ( S O_{2} ) and the corresponding equilibrium constants at ( 299 mathrm{K} ) ( boldsymbol{S} boldsymbol{O}_{2}(boldsymbol{g})+mathbf{1} / boldsymbol{2} boldsymbol{O}_{2}(boldsymbol{g}) rightleftharpoons boldsymbol{S} boldsymbol{O}_{3}(boldsymbol{g}) ; boldsymbol{K}_{1} ) ( mathbf{4} boldsymbol{S} boldsymbol{O}_{3}(boldsymbol{g}) rightleftharpoons boldsymbol{4} boldsymbol{S} boldsymbol{O}_{2}(boldsymbol{g})+boldsymbol{2} boldsymbol{O}_{2}(boldsymbol{g}) ; boldsymbol{K}_{2} ) The value of the equilibrium constant are related by :- A ( cdot_{K_{2}}=frac{1}{left(K_{1}right)^{4}} ) B. ( K_{2}=K_{1}^{4} ) c. ( _{K_{2}}=left(frac{1}{K_{1}}right)^{1 / 4} ) D. ( _{K_{2}}=frac{1}{K_{1}} ) |
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| 255 | Which of the following salts when dissolved in water will produce an acidic solution? ( mathbf{1} cdot boldsymbol{N} boldsymbol{H}_{mathbf{4}} boldsymbol{C l} ) 2. ( boldsymbol{K} boldsymbol{H} boldsymbol{S} boldsymbol{O}_{4} ) 3. ( boldsymbol{N a C N} ) A .2 and 3 B. 1 and 2 c. only 3 D. 2 and 4 |
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| 256 | 2 moles of ( P C l_{5} ) when heated in a closed vessels of 2 litre capacity at equilibrium ( 40 % ) of ( P C l_{5} ) dissociated in ( P C l_{3} ) and ( C l_{2} . ) What is the value of the equilibrium constant? A. 0.267 B. 0.786 c. 0.345 D. 1.879 |
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| 257 | 9.2 grams of ( N_{2} O_{4}(g) ) is taken in a closed one litre vessel and heated till the following equilibrium is reached, ( N_{2} O_{4}(g) rightleftharpoons 2 N O_{2}(g) . ) At equilibrium, ( 50 % N_{2} O_{4}(g) ) is dissociated. What is the equilibrium constant? (in ( M) ) (molecular weight of ( N_{2} O_{4}=92 ) ) A . ( 0 . ) B. 0.4 c. 0.3 D. 0.2 |
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| 258 | Electrolytes include which of the following types of compounds? A. Acids B. Bases c. Salts D. All of the above |
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| 259 | Which of the following is an example of mineral acid? A. Sulphuric acid B. Acetic acid c. Tartaric acid D. All of above |
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| 260 | In the reaction, ( boldsymbol{N} boldsymbol{H}_{3}(boldsymbol{a} boldsymbol{q})+boldsymbol{H}_{2} boldsymbol{O}(boldsymbol{I})= ) ( N H_{4}^{+}+O H^{-} ) the water is a A. bronsted acid B. bronsted base c. conjugate acid D. conjugate base |
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| 261 | Passing ( boldsymbol{H}_{2} boldsymbol{S} ) gas into a mixture of ( M n^{2+}, N i^{2+}, C u^{2+} ) and ( H g^{2+} ) ions in an acidified aqueous solution precipitates. A. CuS and Hgs B. MnS and cus c. Mns and Nis D. Nis and Hgs |
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| 262 | For the equilibrium in a closed vessel ( boldsymbol{P C l}_{5}(boldsymbol{g}) rightleftharpoons boldsymbol{P} boldsymbol{C l}_{3}(boldsymbol{g})+boldsymbol{C l}_{2}(boldsymbol{g}) ) ( K_{p} ) is found to be double of ( K_{c cdot} ) This is attained when: A. ( T=2 K ) в. ( T=12.18 K ) c. ( T=24.36 K ) D. ( T=27.3 K ) |
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| 263 | What is the pH of ( 0.001 M H C l ? ) ( A cdot 1 ) B. 2 ( c .3 ) D. 4 |
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| 264 | The equilibrium constant for the reaction is 9.40 at ( 900^{circ} C ) ( boldsymbol{S}_{2}(boldsymbol{g})+boldsymbol{C}(s) rightleftharpoons boldsymbol{C} boldsymbol{S}_{2}(boldsymbol{g}) ) Calculate the pressure of two gases at equilibrium, when 1.42 at ( m ) of ( S_{2} ) and excess of ( C(s) ) come to equilibrium. |
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| 265 | If the equilibrium constant for ( N_{2}(g)+ ) ( O_{2}(g) rightleftharpoons 2 N O(g) ) is ( K, ) the equilibrium constant for ( frac{1}{2} N_{2}(g)+frac{1}{2} O_{2}(g) rightleftharpoons ) ( N O(g) ) will be: A. ( K ) B. ( K^{2} ) c. ( K^{frac{1}{2}} ) D・( frac{1}{2} K ) |
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| 266 | Q52. What is the pH of 0.001 M aniline solution? The ionization constant of aniline is 4.27 x 10-10. Calculate degree of ionization of aniline in the solution. Also calculate the ionization constant of the conjugate acid of aniline. (1) Сттл |
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| 267 | A constant temperature, the equilibrium constant ( left(boldsymbol{K}_{boldsymbol{p}}right) ) for the decomposition reaction ( N_{2} O_{4} rightleftharpoons 2 N O_{2} ) is expressed by ( boldsymbol{K}_{boldsymbol{p}}=left(boldsymbol{4} boldsymbol{x}^{2} boldsymbol{p}right) /left(1-boldsymbol{x}^{2}right) ) where ( p= ) pressure and ( x= ) extent of decomposition. Which one of the following statements is true? A. ( K_{p} ) increases with increase in ( mathrm{p} ) B. ( K_{p} ) increases with increase in ( x ) C. ( K_{p} ) increases with decrease in ( x ) D. ( K_{p} ) remains constant with change in p and ( x ) |
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| 268 | Litmus paper is turned red by the action of: ( mathbf{A} cdot C H_{3} C H_{2} C H_{2} O H ) B ( cdot C H_{3} C H(B r) C H(B r) C H_{3} ) ( mathbf{c} cdot C H_{3} C H_{2} C H(B r) C H_{3} ) D. ( C H_{3} C H_{2} C H_{2} C O O H ) ( mathbf{E} cdot C H_{3} C H_{2} C H_{2} C H_{3} ) |
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| 269 | In which of the following solution, ( A g C l ) has minimum solubility: A. ( 0.05 M A g N O_{3} ) в. ( 0.01 M ) Са ( C l_{2} ) c. ( 0.01 M ) NaCl D. ( 0.01 M N H_{4} O H ) |
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| 270 | For a weak electrolyte molar conductance in dilute solution increases sharply as its concentration in solution is decreased. Give reason. |
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| 271 | Law of mass action cannot be applied to: A. decomposition of gaseous ( H I ) B. decomposition of gaseous ( P C l_{5} ) C. transition of Rhombic Sulphur to Monoclicnic sulphur D. decomposition of Calcium carbonate |
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| 272 | At ( 80^{circ} C, ) distilled water ( left(H_{3} O^{+}right) ) has concentration equal to ( 1 times ) ( 10^{-6} ) mol/litre. The value of ( K_{w} ) at this temperature will be: A ( cdot 1 times 10^{-6} ) B. ( 1 times 10^{-12} ) c. ( 1 times 10^{-9} ) D. ( 1 times 10^{-15} ) |
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| 273 | Calculate the percentage ionization of ( 0.01 mathrm{M} ) acetic acid in ( 0.1 mathrm{M} ) HCl. ( boldsymbol{K}_{boldsymbol{a}} ) of acetic acid is ( 1.8 times 10^{-5} ) A . ( 0.18 % ) B. 0.018% c. ( 1.8 % ) D. 18% |
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| 274 | ( mathrm{Ca}_{3}left(mathrm{PO}_{4}right)_{2}(mathrm{s}) leftrightharpoons 3 mathrm{Ca}^{2+}(mathrm{aq})+2 mathrm{PO}_{4}^{3-}(mathrm{aq}) ) Find the equilibrium expression for the dissolution of ( boldsymbol{C a}_{3}left(boldsymbol{P} boldsymbol{O}_{4}right)_{2} ? ) ( mathbf{A} cdot mathbf{K}_{s p}=left[mathbf{C} mathbf{a}^{2+}right]^{3}left[mathbf{P} mathbf{O}_{4}^{3-}right]^{2} ) B. ( kappa_{s p}=left[mathrm{Ca}^{2+}right]^{2}left[mathrm{PO}_{4}^{3-}right]^{3} ) C. ( kappa_{s p}=left[mathrm{Ca}^{2+}right]left[mathrm{PO}_{4}^{3-}right] /left[mathrm{Ca}_{3}left(mathrm{PO}_{4}right)_{2}right] ) D. ( kappa_{s p}=left[mathrm{Ca}^{2+}right]^{3}left[mathrm{PO}_{4}^{3-}right]^{2} /left[mathrm{C} mathrm{ca}_{3}left(mathrm{PO}_{4}right)_{2}right] ) E ( cdot K_{s p}=left[mathrm{Ca}^{2+}right]^{2}left[mathrm{PO}_{4}^{3-]}right]^{3} /left[mathrm{Ca}_{3}left(mathrm{PO}_{4}right)_{2}right] ) |
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| 275 | ( operatorname{Given} boldsymbol{A} boldsymbol{g}left(boldsymbol{N} boldsymbol{H}_{3}right)_{2}^{+} rightleftharpoons boldsymbol{A} boldsymbol{g}^{+}+boldsymbol{2} boldsymbol{N} boldsymbol{H}_{3} ) ( boldsymbol{K}_{c}=mathbf{6 . 2} times mathbf{1 0}^{-8} ) and ( boldsymbol{K}_{s p} ) of ( boldsymbol{A} boldsymbol{g} boldsymbol{C l} ) is ( 1.8 times 10^{-10} ) at ( 298 K . ) Calculate concentration of the complex in ( 1 M ) aqueous ammonia. |
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| 276 | 7. At constant temperature, the equilibrium constant (Kp) for the decomposition reaction. NO. 2NO2 18 expressed by, (44²P) ano ano to (1-x²) Кр where P = pressure, x = extent of decomposition. Which of the following statements is true? (a) Kp increases with increase of P (b) K, increases with increase of x (C) K, increase with decrease of x (d) K, remains constant with change in P or x |
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| 277 | Aqua regia consists of: A. hydrochloric acid B. carbonic acid C. nitric acid D. both ( A ) and ( C ) |
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| 278 | State whether the given statement is true or false: ( boldsymbol{H} boldsymbol{g}_{2} boldsymbol{C l}_{2} ) is precipitated if ( left[boldsymbol{H} boldsymbol{g}_{2}^{2+}right]left[boldsymbol{C l}^{-}right]^{2} ) is greater than ( boldsymbol{K}_{boldsymbol{s p}}left(boldsymbol{H} boldsymbol{g}_{2} boldsymbol{C l}_{2}right) ) |
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| 279 | Consider following reaction in equilibrium with equilibrium concentration ( 0.01 mathrm{M} ) of every species (।) ( boldsymbol{P} boldsymbol{C l}_{5}(boldsymbol{g}) rightleftharpoons boldsymbol{P} boldsymbol{C l}_{3}(boldsymbol{g})+boldsymbol{C l}_{2}(boldsymbol{g}) ) (II) ( 2 H I(g) rightleftharpoons H_{2}(g)+I_{2}(g) ) (III) ( N_{2}(g)+3 H_{2}(g) rightleftharpoons 2 N H_{3}(g) ) Extend of the reaction taking place is: A. ( I>I I>I I I ) в. ( I<I I<I I I ) c. ( I I<I I I<I ) D. III ( <I<I I ) |
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| 280 | A sample of hard water contains 0.005 moles of ( C a C l_{2} ) per litre. What is the minimum concentration Of ( N a_{2} S O_{4} ) which must be added for removing ( C a^{2+} ) ions from the water sample? ( left[K_{s p} text { for } C a S O_{4} text { is } 2.4 times 10^{-5} text {at } 25^{circ} Cright] ) A ( .2 .8 times 0^{-5} M ) В. ( 4.8 times 10^{-3} M ) c. ( 6.1 times 10^{-3} M ) D. ( 4.1 times 10^{-5} M ) |
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| 281 | Molar solubility of ( mathbf{C a}(mathbf{O} mathbf{H})_{2} ) in a solution that has a pH of 12. ( left[boldsymbol{K}_{boldsymbol{S P}}left[mathbf{C a}(mathbf{O H})_{2}right]=mathbf{5 . 6} times mathbf{1 0}^{-12}right] ) в. ( 5.6 times 10^{-8} M ) c. ( 4 times 10^{-4} M ) D. None |
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| 282 | Q50. The degree of ionization of a 0.1 M bromoacetic acid solution is 0.132. Calculate the pH of the solution and the pk of bromoacetic acid. TO |
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| 283 | For the reaction, ( boldsymbol{P C l}_{5}(boldsymbol{g}) rightleftharpoons boldsymbol{P} boldsymbol{C l}_{3}(boldsymbol{g})+ ) ( C l_{2}(g), ) the position of equilibrium can be shifted to the right by: A. doubling the volume B. increasing the temperature c. addition of equimolar quantities of ( P C l_{3} ) and ( P C l_{5} ) D. addition of ( C l_{2} ) at constant volume |
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| 284 | The correct order of increasing basicity of the given conjugate bases ( left(R=C H_{3}right. ) is: A ( cdot mathrm{RCOO}^{-}<mathrm{HC}=mathrm{C}^{-}<mathrm{R}^{-}<mathrm{NH}_{2}^{-} ) B . ( mathrm{R}^{-}<mathrm{HC} equiv mathrm{C}^{-}<mathrm{RCOO}^{-}<mathrm{NH}_{2}^{-} ) C. ( mathrm{RCOO}^{-}<mathrm{NH}_{2}^{-}<mathrm{HC} equiv mathrm{C}^{-}<mathrm{R} ) D. ( mathrm{RCOO}^{-}<mathrm{HC} equiv mathrm{C}^{-}<mathrm{NH}_{2}^{-}<mathrm{R} ) |
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| 285 | The reaction ( : boldsymbol{C a} boldsymbol{C O}_{3}(boldsymbol{g}) rightleftharpoons ) ( boldsymbol{C a O}(s)+boldsymbol{C O}_{2}(boldsymbol{g}), ) would proceed to completion if the reaction vessel is connected to bottle containing ( K O H ) solution or carried out in open vessel. If true enter ( 1, ) if false enter 0 |
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| 286 | pH signifies A. Power of hydrogen B ( .-log left[H^{+}right] ) c. ( 14- ) pOH D. All of the above |
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| 287 | A chemical reaction is said to have attained equilibrium when: A. equal amounts of reactants and products are formed B. reactants are completely converted to products C. the rate of forward reaction is equal to the rate of backward reaction D. the concentration of the reactants and products is the same |
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| 288 | When ( 16.8 g ) of white solid ( X ) was heated ( 4.4 g ) of acid gas : ( (A) ) that turned lime water milky was driven of together with ( 1.8 g ) of a gas ( (B) ) which condensed to a colourless liquid the solid that remained ( (Y) ) dissolved in water to give an alkaline solution, which with excess of ( B a C l_{2} ) solution gave a white precipitate ( (Z) . ) The precipitate effervescence with acid giving of ( boldsymbol{C O}_{2} ) gas. Identify the compound ( A, B ) and write the chemical equations for the thermal decomposition of ( X ) ( mathbf{A} cdot(A)-C O_{2} ) ( (B)-H_{2} O quad X rightarrow N a_{2} C O_{3} ) B. ( (A)-C O_{2} ) ( (B)-H_{2} O_{2} quad X rightarrow N a C O_{3} ) ( mathbf{c} cdot(A)-C O_{2} ) ( (B)-H_{2} O_{2} quad X rightarrow N a_{2} C O_{3} ) D. ( (A)-C O_{2} ) ( (B)-H_{2} O quad X rightarrow N a C O_{3} ) |
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| 289 | The degree of dissociation of ( boldsymbol{P C l}_{5} ) will be more at A. constant pressure B. low pressure c. high pressure D. none of these |
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| 290 | Assertion: Amphoteric species acts as either an acid or a base.
Reason: It contains both hydrophobic and hydrophilic regions. |
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| 291 | Consider the equilibrium set up: ( mathbf{2} boldsymbol{H}_{mathbf{2}(boldsymbol{g})}+boldsymbol{C} boldsymbol{O}_{(boldsymbol{g})} rightleftharpoons boldsymbol{C} boldsymbol{H}_{boldsymbol{3}} boldsymbol{O} boldsymbol{H}_{(boldsymbol{g})} ) What will be the effect of the following on the equilibrium of the reaction? (i) Addition of ( boldsymbol{H}_{2} ) (ii) Addition of ( boldsymbol{C H}_{3} boldsymbol{O H} ) (iii) Removal of ( mathrm{CO} ) (iv) Removal of ( boldsymbol{C} boldsymbol{H}_{3} boldsymbol{O} boldsymbol{H} ) A. (i) – Forward direction (ii) – Backward direction (iii) Backward direction (iv) – Forward direction B. (i) – Backward direction (ii) – Backward direction (iii) Forward direction (iv) – Forward direction c. (i) – Forward direction (ii) – Forward direction (iii) Backward direction (iv) – Backward direction D. (i) – Backward direction (ii) – Forward direction (iii) Forward direction (iv) – Backward direction |
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| 292 | Which of the following expressions for ( % ) ionization of a monoacidic base ( (B O H) ) in aqueous solution is not correct at appreciable concentration? A ( cdot_{100} times sqrt{frac{K_{b}}{c}} ) В. ( frac{1}{1+10left(p K_{b}-p O Hright)} ) с. ( frac{K_{w}left[H^{+}right]}{K_{b}+K_{w}} ) D. ( frac{K_{b}}{K_{b}+left[O H^{-}right]} ) |
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| 293 | A well is dug in a bed of rock containing fluorspar ( left(C a F_{2}right) . ) If the well contains ( 20000 mathrm{L} ) of water, what is the amount of ( boldsymbol{F}^{-} ) in it ( ?left(boldsymbol{K}_{s p}=boldsymbol{4} times mathbf{1 0}^{-11}right) ) A . 4.2 mol B . 13.6 mol c. 8.6 mol D. 10 mol |
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| 294 | An equilibrium expression may be forced to completion by: A. adding a catalyst B. increasing the pressure C. increasing the temperature D. removing the products from the reaction mixture as they are formed E. decreasing the reactant concentration |
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| 295 | In an equilibrium reaction for which ( Delta G^{circ}=0 . ) Determine the value of equilibrium constant ( mathrm{K} . delta G=0 ) A . 1.0 B. 2.7 ( c .7 .6 ) D. 8.5 |
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| 296 | The pH value of ( 10^{-7} ) M solution ( H C l ) is: A. equal to 1 B. equal to 2 c. less than 7 D. equal to 0 |
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| 297 | Common salt is chemically sodium chloride ( (N a C l) ) A. True B. False |
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| 298 | 2. 41 Match the following species with the corresponding conjugate acid. Species Conjugate acid A. NH4 1. co- B. HCO3 2. NHỜ с. Но 3. H₂O+ D. HSO: 4. H2SO4 5. H, COW |
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| 299 | The solubility of ( M g(O H)_{2} ) in pure water is ( 9.57 times 10^{-3} g L^{-1} . ) Calculate its solubility in ( g L^{-1} ) in ( 0.02 M ) ( M gleft(N O_{3}right)_{2} ) solution. |
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| 300 | Chemical equation of the industrial preparation of ( boldsymbol{S} boldsymbol{O}_{3} ) is given? ( 2 S O_{2}+O_{2} rightleftharpoons 2 S O_{3}+ ) Heat What is the influence of the following factors in this system at equilibrium? (a) Increasing the amount of ( boldsymbol{O}_{2} ) (b) ( S O_{2} ) is removed from the system. (c) Decreasing the temperature. |
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| 301 | On decomposition of ( N H_{4} H S, ) the following equilibrium is established: ( boldsymbol{N} boldsymbol{H}_{4} boldsymbol{H} boldsymbol{S}(boldsymbol{s}) rightleftharpoons boldsymbol{N} boldsymbol{H}_{3}(boldsymbol{g})+boldsymbol{H}_{2} boldsymbol{S}(boldsymbol{g}) ) If the total pressure is ( P ) atm, then the equilibrium constant ( boldsymbol{K}_{boldsymbol{P}} ) is equal to: ( A cdot P ) atm B. ( P^{2} a t m^{2} ) ( mathbf{c} cdot P^{2} / 4 a t m^{2} ) D. 2P atm |
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| 302 | An equilibrium mixture in a vessel of capacity 100 litre contain 1 mol ( N_{2}, 2 ) mol ( O_{2} ) and 3 mol NO.No. of moles of ( 0_{2} ) to be added so that at new equilibrium the conc. of NO is found to be 0.04 mol/lit : A ( .(101 / 18) ) B. (101/9) c. (202/9) D. None of these |
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| 303 | Any salt ( M C l_{2} ) is soluble in water, if it’s hydration energy exceeds the lattice energy of ( M C l_{2} ) A. True B. False |
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| 304 | Q38. Write the conjugate acids for the following Bronsted bases: NH, NH, and HCOO- |
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| 305 | Hydronium exist even in pure water A. True B. False |
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| 306 | ( H_{3} B O_{3} ) is named as A. boric acid B. monobasic and weak bronsted acid c. dibasic and strong lewis acid D. tribasic and weak bronsted acid |
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| 307 | (A) pH of ( 10^{-7} ) M NaOH solution exists between 7 to 7.3 at ( 25^{circ} C ) (R) Due to common ion effect ionization of water is suppressed. A. Both (R) and (A) are true and reason is the correct explanation of assertion B. Both (R) and (A) are true but reason is not correct explanation of assertion c. Assertion (A) is true but reason (R) is false D. Assertion (A) and reason (R) both are false E. Assertion (A) is false but reason (R) is true |
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| 308 | What is the ( K_{b} ) of a weak base that produces an ( O H^{-} ) per molecule if a 0.05 M solution is ( 2.5 % ) ionized? ( mathbf{A} cdot 7.8 times 10^{-8} ) B . ( 1.6 times 10^{-6} ) c. ( 3.125 times 10^{-5} ) D. ( 1.2 times 10^{-3} ) |
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| 309 | Assertion The energy profile of the reaction ( boldsymbol{A}+ ) ( B rightleftharpoons C ) is given as above, then the K of the above equilibrium increases with increase of temperature Reason Endothermic reaction is favoured by increase of temperature A. Both assertion and reason are true but reason is the correct explanation for assertion B. Both assertion and reason are true but reason is not the correct explanation for assertion c. Assertion is true but reason is false D. Assertion is false but the reason is true |
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| 310 | Assertion It is difficult to distinguish the strengths of the strong acids such as ( boldsymbol{H} boldsymbol{C l}, boldsymbol{H}_{2} boldsymbol{S} boldsymbol{O}_{4}, boldsymbol{H} boldsymbol{N} boldsymbol{O}_{3} boldsymbol{H} boldsymbol{B} boldsymbol{r}, boldsymbol{H} boldsymbol{I} ) or ( boldsymbol{H} boldsymbol{C l O}_{4} ) in dilute aqueous solutions. Reason In dilute aqueous solution all strong acids donate a proton to water and are |
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| 311 | Available chlorine can be liberated from bleaching powder by the reaction with: This question has multiple correct options A ( cdot ) conc. ( H_{2} S O_{4} ) в. ( d i l . H_{2} S O_{4} ) ( c cdot C O_{2} ) D. ( d i l . H N O_{3} ) |
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| 312 | mole of ( A(g) ) is heated to ( 300^{circ} C ) in closed one litre vessel till the following equilibrium is reached: ( boldsymbol{A}(boldsymbol{g}) Leftrightarrow boldsymbol{B}(boldsymbol{g}) ) The equilibrium constant for the reaction at ( 300^{circ} mathrm{C} ) is ( 4 . ) What is the concentration of ( mathrm{B}left(text { in } operatorname{mol} . l i t^{-1}right) ) at equilibrium? A . 0.2 B. 0.6 ( c cdot 0.8 ) D. 0.1 |
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| 313 | Match the column I with column II and mark the appropriate choice. Column I (i) Saturated (A) Liquid ( leftrightarrow ) Vapour (B) Solid ( leftrightarrow ) Liquid (ii) Boiling point (C) Solid ( leftrightarrow ) (iii) Sublimation vapour ( quad ) point (D) Solute ( (s) leftrightarrow ) (iv) Melting point Solute(solution) ( A cdot(A)-(i),(B)-(i i i),(C)-(i i),(D)-(i v) ) B. (A) – (ii), (B) – (iv), (C) – (iii), (D) – (i) C. ( (A)-(i v),(B)-(i i),(C)-(i),(D)-(i i i) ) D. (A) – (iii), (B) – (iv), (C) – (ii), (D) – (i) |
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| 314 | The equilibrium constant for the reaction ( boldsymbol{w}+boldsymbol{x} rightleftharpoons boldsymbol{y}+boldsymbol{z} ) is ( 9 . ) If one mole of each of wand ( x ) are mixed and there is no change in volume, the number of moles of y for formed is : A . 0.10 B. 0.50 c. 0.75 D. 0.54 |
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| 315 | 12 lowerg we dluvallun energyu) HILU 5. What is the correct expression for the representation of the solubility product constant of Ag, Cro? (a) [Ag+12 [Cro1(b) [2Ag 1 [Cro21 (c) (Ag 1 [Cro2-1 (d) [2Ag+1? [Cro21 |
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| 316 | 16. Amphoprotic substances are those (a) which can donate a proton (b) which can accept a proton (c) which can accept and donate proton (d) which can donate hydroxyl ion |
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| 317 | 0.010 Q10. At 450 K, K, = 2.0 < 1010 bar-1 for the equilibrium reaction: 250, (g) + 02 (8) = 250, (8) What is K at this temperature? |
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| 318 | Q62. A 0.02 M solution of pyridinium hydrochloride has pH = 3.44. Calculate the ionization constant of pyridine. TT 1+1 10-4 M |
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| 319 | The ( K_{p} ) value for ( 2 S O_{2}(g)+O_{2}(g) rightleftharpoons ) ( 2 S O_{3}(g) ) is ( 5.0 a t m^{-1} ) If the equilibrium pressures of ( S O_{2} ) and ( boldsymbol{S} boldsymbol{O}_{3} ) are equal. What is the equilibrium pressure of ( boldsymbol{O}_{2} ? ) A. 0.2 atm B. 0.3 atm ( c .0 .4 ) atm D. ( 0.1 mathrm{atm} ) |
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| 320 | Mark the correct statement(s) based on the phase diagram of ( C O_{2} ) shown in the graph. rhis question has multiple correct options A ( cdot 298 mathrm{K} ) is the normal boiling point of liquid ( C O_{2} ) B. At 1 atm & 190 K ( C O_{2} ) will exist as gas. ( mathrm{c} cdot mathrm{CO}_{2}(s) ) will sublime above ( 195 mathrm{K} ) under norma atmospheric pressure D. Melting point & boiling point of ( C O_{2} ) will increase on increasing pressure. |
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| 321 | A vessel contains 1 mole ( boldsymbol{P} C l_{5}(g) ) at 4 ( operatorname{atm} ) and 0.5 mole ( P C l_{3} ) formed at equilibrium. Now, equilibrium pressure of mixture is (assume ideal behavior) ( A cdot 16 ) atm B. 6 atm ( c cdot 2 ) atm D. 4.5 atm |
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| 322 | 4 moles of ( H_{2} ) at ( 500 mathrm{K} ) is kept in an adiabatic rigid container.After some time it was found that 1 mole of the gas dissociated intoHatoms. The dissociation energy permole of ( boldsymbol{H}_{2} ) gas is 2000 cal,Let the new temperature of the gas be 100 T. The integral value of ( T ) is : (Use ( mathrm{R}=2 mathrm{cal} / mathrm{mole}-mathrm{K}) ) A. 3 B. 4 ( c cdot 5 ) D. 6 E. 2 |
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| 323 | If the solubility of the salt ( boldsymbol{L} boldsymbol{i}_{3} boldsymbol{N} boldsymbol{a}_{3}left(boldsymbol{A l} boldsymbol{F}_{6}right)_{2} ) is ( boldsymbol{x}, ) then its solubility product would be: A ( cdot 26 x^{8} ) B . ( 2916 x^{8} ) ( mathbf{c} cdot 256 x^{6} ) D. none of these |
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| 324 | An exothermic reaction which proceeds with decrease in volume will give maximum yield at high ( P ) and low ( T ) If true enter 1 , if false enter 0 . |
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| 325 | What is buffer solution? Give an example. |
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| 326 | A buffer solution is prepared in which the concentration of ( N H_{3} ) is ( 0.30 M ) and the concentration of ( N H_{4}^{+} ) is ( 0.20 M . ) If the equilibrium constant, ( boldsymbol{K}_{boldsymbol{b}} ) for ( boldsymbol{N} boldsymbol{H}_{3} ) equals ( 1.8 times 10^{-5}, ) what is the pH of this solution? ( (log 2.7=0.433) ) A . 9.08 B. 9.43 c. 11.72 D. 8.73 |
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| 327 | In a three litre vessel, 2 moles of ( N_{2} ) and 3 moles of length ( boldsymbol{H}_{2} ) are taken. If at equilibrium ( x ) moles of ( N_{2} ) were obtained then the concentration of ( N H_{3} ) at equilibrium will be: ( mathbf{A} cdot 2-x ) B. ( 4-2 x ) c. ( frac{2 x}{3} ) D. ( frac{4-2 x}{3} ) |
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| 328 | When one mole of ( P(g) ) is introduced in one litre closed rigid vessel maintained at constant temperature, the following equilibrium is established. ( boldsymbol{P}(boldsymbol{g}) rightleftharpoons boldsymbol{Q}(boldsymbol{g})+boldsymbol{R}(boldsymbol{g}) quad Longrightarrow boldsymbol{K}left(boldsymbol{C}_{1}right) ) ( boldsymbol{R}(boldsymbol{g}) rightleftharpoons boldsymbol{S}(boldsymbol{g})+boldsymbol{Q}(boldsymbol{g}) quad Longrightarrow boldsymbol{K}left(boldsymbol{C}_{2}right) ) f the final equilibrium pressure is 2 times of the initial pressure, then the value of ( frac{boldsymbol{K}left(boldsymbol{C}_{2}right)}{boldsymbol{K}left(boldsymbol{C}_{1}right)} ) is [Ratio of the equilibrium concentration of ( Q text { and } R text { is } 5] ) |
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| 329 | Calculate the weight of ( left(N H_{4}right)_{2} S O_{4} ) which must be added to ( 500 mathrm{mL} ) of ( 0.2 mathrm{M} ) ( N H_{3} ) to yield a solution of ( mathrm{pH}=9.35, K_{b} ) for ( boldsymbol{N} boldsymbol{H}_{3}=mathbf{1 . 7 8} times mathbf{1 0}^{-mathbf{5}} ) (in ( mathrm{gm} ) )(Write answer upto 3 decimal places) |
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| 330 | The solubility in water of a sparingly soluble salt ( A B_{2} ) is ( 1.0 times 10^{-5} ) mol ( L^{-1} ) Its solubility product will be: A ( cdot 4 times 10^{-15} ) В. ( 4 times 10^{-10} ) c. ( 1 times 10^{-15} ) D. ( 1 times 10^{-10} ) |
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| 331 | Iron filling and water were placed in a 5 litre vessel and sealed. The tank was heated to ( 1000^{circ} mathrm{C} ). Upon analysis the tank was found to contain ( 1.1 mathrm{g} ) of hydrogen and 42.5 g of water vapour. If the reaction in the tank is represented by ( 3 mathrm{Fe}(mathrm{s})+4 boldsymbol{H}_{2} boldsymbol{O}_{(g)} rightleftharpoons boldsymbol{F} boldsymbol{e}_{3} boldsymbol{O}_{4}(boldsymbol{s})+ ) ( mathbf{4} boldsymbol{H}_{2}(boldsymbol{g}) ) The value of equilibrium constant, ( boldsymbol{K}_{c} ) is: A . 30 B. 0.03 ( c cdot 3 ) D. 0.003 |
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| 332 | If the solubility product of a sparingly soluble salt ( M X_{2} ) at ( 25^{circ} C ) is ( 1.0 times ) ( mathbf{1 0}^{-11}, ) the solubility of the salt in moles ( L^{-1} ) at this temperature will be: A ( .2 .46 times 10^{14} ) B . ( 1.36 times 10^{-4} ) c. ( 2.60 times 10^{-7} ) D. ( 1.20 times 10^{-10} ) |
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| 333 | At ( 25^{circ} C,_{-}-_{-}– ) produces an aqueous solution with ( p H>7 ) A. Arrhenius acid B. Arrhenius base c. Buffer D. Indicator E. Salt |
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| 334 | A buffer solution with ( p H=9 ) is to be prepared by mixing ( N H_{4} C I ) and ( N H_{4} O H . ) Calculate the number of moles of ( N H_{4} C I ) that should be added to one litre pf ( 1.0 M N H_{4} O H .left[K_{b}=right. ) ( left.1.8 times 10^{-5}right] ) A . 3.4 B . 2. c. 1.5 D. 1.8 |
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| 335 | A beaker contains a saturated solution of copper(l) chloride. Copper(l) chloride is slightly soluble salt with a solubility product of ( 1.2 times 10^{-6} ) Which of the following salts when added to the solution would precipitate copper(l) chloride? A. Sodium chloride B. Potassium bromide c. Silver(I) nitrate D. Lead(II) acetate E. Magnesium iodide |
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| 336 | What is the ( p H ) of ( 0.001 mathrm{M} ) aniline solution ? The ionization constant of aniline can be taken from Table 7.7 Calculate the degree of ionization of aniline in the solution. Also calculate the ionization constant of the conjugate acid of aniline. |
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| 337 | The ( p H ) of ( 0.1 M ) solution of the following salts increases in the order: A ( cdot operatorname{NaCl}<N H_{4}^{+}<N a C N<H C l ) в. ( H C l<N H_{4}^{+}<N a C l<N a C N ) c. ( operatorname{NaCN}<N H_{4}^{+}<N a C l<H C l ) D. ( H C l<N a C l<N a C N<N H_{4} ) |
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| 338 | Acetyl salicylic acid (aspirin) ionises in water as: ( boldsymbol{H} boldsymbol{C}_{9} boldsymbol{H}_{7} boldsymbol{O}_{4}+boldsymbol{H}_{2} boldsymbol{O} rightarrow ) ( boldsymbol{H}_{3} boldsymbol{O}^{+}+boldsymbol{C}_{9} boldsymbol{H}_{7} boldsymbol{O}_{4}^{-} ;left(boldsymbol{K}_{a}=boldsymbol{2} . boldsymbol{7} boldsymbol{5} times mathbf{1} boldsymbol{0}^{-boldsymbol{9}}right) ) If two tablets of aspirin each of 0.32 g is dissolved in water to produce ( 250 mathrm{mL} ) solution, calculate ( [stackrel{ominus}{boldsymbol{O}} boldsymbol{H}] ) A ( cdot 1.61 times 10^{-9} M ) В. ( 1.61 times 10^{-7} ) М c. ( 1.61 times 10^{-3} M ) D. ( 1.61 times 10^{-5} M ) |
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| 339 | What is the concentration of ( C H_{3} C O O H ) which can be added to 0.5 M HCOOH solution so that dissociation of both is same. [Given that ( : boldsymbol{K}_{boldsymbol{C H}_{3} text { COOH}}=mathbf{1 . 8} times ) ( mathbf{1 0}^{-5}, quad boldsymbol{K}_{boldsymbol{H} mathrm{COOH}}=mathbf{2 . 4} times mathbf{1 0}^{-4} mathbf{j} ) (as nearest integer) |
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| 340 | Extent of a reaction can always be increased by increasing the temperature. A. True B. False |
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| 341 | ( p K_{a} ) values of four acids are given below at ( 25^{circ} mathrm{C} ). The strongest acid is: A . 2.0 в. 2. c. 3.0 D. 4.0 |
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| 342 | At ( 25^{circ} C, K_{p} ) for the reaction: ( N_{2} O_{4}(g) leftrightharpoons 2 N O_{2}(g) ) has a value of 0.14 atm. Calculate the value of ( K_{c} ) in which the concentrations are measured in mol ( boldsymbol{L}^{-1} ) |
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| 343 | Which information can be obtained from Le Chatelier’s principle? A. Shift in equilibrium position on changing ( P, T ) and concentration B. Dissociation constant of a weak acid c. Energy change in a reaction D. Equilibrium constant of a chemical reaction |
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| 344 | Which one of the following is a strong electrolyte? A. ( C H_{3} ) СООН в. ( H C O O H ) c. ( H_{2} C O_{3} ) D. ( N a O H ) |
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| 345 | ( X Y_{2} ) dissociates as: ( X Y_{2}(g) rightleftharpoons ) ( boldsymbol{X} boldsymbol{Y}(boldsymbol{g})+boldsymbol{Y}(boldsymbol{g}) ) Initial pressure of ( boldsymbol{X} boldsymbol{Y}_{2} ) is ( boldsymbol{6} boldsymbol{0} boldsymbol{0} boldsymbol{m} boldsymbol{m} boldsymbol{H} boldsymbol{g} ) The total pressure at equilibrium is ( 800 m m H g . ) Assuming volume of system to remain constant, the value of ( boldsymbol{K}_{p} ) is: A . 50 в. 100 c. 200 D. 400 |
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| 346 | Q. 38 Match the following equilibria with the corresponding condition. A Liquid Vapour Saturated solution B. Solid Liquid 2. Boiling point C. Solid Vapour 3. Sublimation point D. Solute (s) Solute (solution) 4. Melting point 5. Unsaturated solution |
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| 347 | In a 0.25 -liter tube dissociation of 4 moles of NO is took place. If its degree of dissociation is ( 10 % . ) The value of ( boldsymbol{K}_{boldsymbol{p}} ) for reaction ( 2 N O rightleftharpoons N_{2}+O_{2} ) is: A ( cdot frac{1}{(18)^{2}} ) в. ( frac{1}{(8)^{2}} ) c. ( frac{1}{(16)} ) D. ( frac{1}{(32)} ) |
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| 348 | By which method you can dilute a concentrated acid properly? A. Carefully replace unused or excess chemicals into their properly labeled containers from which they came B. The rule is to add water to the concentrated acid slowly C. Dispose of chemicals in the proper places following posted procedures. Do not return them to their original containers D. Flush eyes with water at the eyewash fountain for at least 15 minutes, and then report the accident for further help E. The rule is to add concentrated acid to water slowly |
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| 349 | In the reaction ( 2 P(g)+Q(g) rightleftharpoons ) ( 3 R(g)+S(g) . ) If 2 moles each of ( P ) and ( Q ) is taken initially in a 1 litre flask. At equilibrium which of the following is true? ( mathbf{A} cdot[P]<[Q] ) B ( cdot[P]=[Q] ) ( mathbf{c} cdot[Q]=[R] ) D. None of these |
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| 350 | ( N a H C O_{3} ) can be used on its own to make cakes or bread. Baking powder is more commonly used, and contains ( N a H C O_{3}, C aleft(H_{2} P O_{4}right)_{2} ) and starch. An improved combination baking powder contains about ( 40 % ) starch, ( 30 % ) ( N a H C O_{3} 20 % N a A lleft(S O_{4}right)_{2} ) and ( 10 % ) ( boldsymbol{C a}left(boldsymbol{H}_{2} boldsymbol{P} boldsymbol{O}_{4}right)_{2} ) Answer the following questions based on above study. ( boldsymbol{C} boldsymbol{a}left(boldsymbol{H}_{2} boldsymbol{P} boldsymbol{O}_{4}right)_{2} ) in baking powder: A. behaves as an acid in moist condition and decomposes ( N a H C O_{3} ) to give ( C O_{2} ) B. behaves as a base in moist condition and gives ( H_{3} P O_{4} ) c. behaves as a binder D. behaves as a filler |
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| 351 | One mole of nitrogen and three moles of hydrogen are mixed in a 4 litre container. If 0.25 percent of nitrogen is converted to ammonia by the following reaction ( N_{2}(g)+3 H_{2}(g) rightleftharpoons 2 N H_{3}(g) ) What will be the value of ( K ) for the following equilibrium? ( frac{1}{2} N_{2}(g)+frac{3}{2} H_{2}(g) rightleftharpoons N H_{3}(g) ) A ( cdot 1.49 times 10^{-5} L ) mol ( ^{-1} ) В . ( 2.22 times 10^{-10} L ) mol ( ^{-1} ) D. None of these |
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| 352 | The equilibrium ( boldsymbol{A}_{4}(boldsymbol{g})+boldsymbol{6} boldsymbol{B}_{2}(boldsymbol{g}) rightleftharpoons ) ( 4 A B_{3}(g) ) is established in a closed container by taking equal moles of ( A_{4}(g) ) and ( B_{2}(g) . ) Which of the following options must be correct at equilibrium? ( mathbf{A} cdotleft[A_{4}right]left[A B_{3}right] ) c. ( left[A_{4}right]<left[A B_{3}right] ) D. None of the above |
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| 353 | Some of alkali metal salts are coloured ( N a_{2} C r O_{4}- ) yellow, ( K M n O_{4}- ) pink ( K_{2} M n O_{4} ) -green. It is due to: A. cations are coloured ions B. anions are coloured ions c. both ( A ) and ( B ) D. none of the above |
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| 354 | In the reaction :- [ begin{array}{r} boldsymbol{C u} boldsymbol{S O}_{4} cdot boldsymbol{3} boldsymbol{H}_{2} boldsymbol{O}(boldsymbol{s}) rightleftharpoons mathbf{2} boldsymbol{C u} boldsymbol{S} boldsymbol{O}_{4} \ boldsymbol{H}_{2} boldsymbol{O}(boldsymbol{s})+mathbf{2} boldsymbol{H}_{2} boldsymbol{O}(boldsymbol{v}) end{array} ] Dissociation pressure is ( 7 times 10^{-3} ) atm at 25 and ( Delta H=2700 ) cal. If the dissociation pressure at 127 is ( X times ) [ 10^{-3} text {atm, then } 100 X ] is |
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| 355 | The solubility of ( C a C O_{3} ) is ( 7 m g / )litre. Calculate the solubility product of ( B a C O_{3} ) from this information and from the fact that when ( N a_{2} C O_{3} ) is added slowly to a sloution containing equimolar concentration of ( C a^{2+} ) and ( B a^{2+}, ) no precipitate is formed until 90 ( % ) of ( B a^{2+} ) has been precipitated as ( B a C O_{3} . ) The solubility product of ( B a C O_{3} ) is ( X times 10^{-10} ) mol ( ^{2} l i t r e^{-2}, ) the value of integer nearest to ( boldsymbol{X} ) is: |
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| 356 | The relative strength of two weak bases at same concentration may be given as: This question has multiple correct options ( ^{mathbf{A}} cdot frac{K_{b_{1}}}{K_{b_{2}}} ) ( ^{mathrm{B}} cdotleft[frac{left[O H^{-}right]_{1}}{left[O H^{-}right]_{2}}right. ) c. ( frac{alpha_{1}}{alpha_{2}} ) D. ( frac{sqrt{K_{b_{1}}}}{sqrt{K_{b_{2}}}} ) |
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| 357 | Q54. The ionization constant of dimethylamine is 5.4 x 104. Calculate its degree of ionization in its 0.02 M solution. What percentage of dimethylamine is ionized if the solution is also 0.1 Min NaOH? 054. Trezimi solution. W |
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| 358 | Match the following ( begin{array}{lll}text { S.No } & text { Source } & text { Acid present } \ 1 . & text { Apple } & text { Oxalic acid } \ 2 . & text { Lemon } & text { Tartaric acid } \ 3 . & text { Grape } & text { Malic Acid } \ 4 . & text { Tomato } & text { Citric Acid }end{array} ) |
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| 359 | What is the minimum pH of a solution ( 0.10 M ) in ( M g^{2+} ) from which ( M g(O H)_{2} ) will not precipitate? ( boldsymbol{K}_{s p} boldsymbol{M} boldsymbol{g}(boldsymbol{O} boldsymbol{H})_{2}= ) ( mathbf{1} . mathbf{2} times mathbf{1 0}^{-mathbf{1 1}} mathbf{M}^{mathbf{3}} ) |
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| 360 | Determine the number of moles of ( boldsymbol{A} boldsymbol{g} boldsymbol{I} ) which may be dissolved in 1 litre of ( 1 M ) of ( C N^{-} ) solution ( K_{s p} ) for ( A g I ) and ( K_{c} ) for ( A g(C N)_{2}^{-} 1.2 times 10^{-17} M^{2} ) and ( 7.1 times ) ( 10^{-19} M^{-2} ) respectively. |
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| 361 | Calculate percentage degree of hydrolysis in a ( 0.1 ~ M ) solution of ( boldsymbol{C H}_{3} boldsymbol{C O O N a} ) Given that ( :left[boldsymbol{K}_{boldsymbol{a}} boldsymbol{o} boldsymbol{f} boldsymbol{C H}_{3} boldsymbol{C O O H}=right. ) ( left.mathbf{1 0}^{-mathbf{5}}right] ) A . 1.0 B. 0.01 ( c cdot 10^{-4} ) D. None of these |
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| 362 | The dissociation constants for acetic acid and ( H C N ) at ( 25^{circ} C ) are ( 1.5 times 10^{-5} ) and ( 4.5 times 10^{-10} ) respectively. The equilibrium constant for the following equilibrium would be: [ begin{array}{r} C N^{-}+C H_{3} C O O H rightleftharpoons \ H C N+C H_{3} C O O^{-} end{array} ] A ( cdot 3 times 10^{4} ) B. ( 3 times 10^{5} ) ( mathrm{c} cdot 3 times 10^{-5} ) D. ( 3 times 10^{-4} ) |
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| 363 | The compounds ( A ) and ( B ) are mixed in equimolar proportion to form the products, ( boldsymbol{A}+boldsymbol{B} rightleftharpoons boldsymbol{C}+boldsymbol{D} . ) At equilibrium, one-third of ( A ) and ( B ) are consumed. The equilibrium constant for the reaction is: A . 0.5 в. 4.0 c. 2.5 D. 0.25 |
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| 364 | The solubility product of ( A g B r ) is ( 4.9 times ) ( 10^{-9} . ) The solubility of AgBr will be: A. ( 7 times 10^{-4} ) mole /litre B. ( 7 times 10^{-5} g / )litre c. ( 1.316 times 10^{-2} g / )litre D. ( 1 times 10^{-3} ) mole ( / )litre |
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| 365 | Solubility of ( A s_{2} S_{3} ) in aqueous solution is ( operatorname{Smol} L^{-1} ). Its solubility product is ( 108 S^{n} . ) What will be the value of ( n ? ) |
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| 366 | Assertion Sodium bicarbonate is an acidic salt. Reason It gives basic solution in water. A. If both assertion and reason are correct and reason is the correct explaination of the assertion B. If both assertion and reason are correct, but reason is not the correct explanation of the assertion C. If assertion is correct, but reason is incorrect D. If assertion is incorrect, but reason is correct |
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| 367 | Nitric acid is a: A. diprotic acid B. strong acid C . organic acid D. both ( A ) and ( C ) |
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| 368 | ( N a C l ) is less soluble in ( D_{2} O ) than ( H_{2} O ) why? |
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| 369 | ( 0.001 M N H_{4} C l ) aqueous solution has ( mathbf{p H}: ) A . 6.127 B. 7.126 c. 2.167 D. 1.267 |
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| 370 | ( boldsymbol{K} boldsymbol{O} boldsymbol{H}(boldsymbol{a} boldsymbol{q}) rightleftharpoons ) A ( cdot K^{-}+O H^{+} ) B. ( K^{+}+O H^{+} ) ( mathbf{c} cdot K^{-}+O H^{-} ) ( mathbf{D} cdot K^{+}+O H^{-} ) |
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| 371 | A definite amount of solid ( N H_{4} H S ) is placed in a flask already containing gas at a certain temperature and 0.50 atm pressure. ( N H_{4} H S ) decomposes to give ( N H_{3} ) and ( H_{2} S ) and at equilibrium total pressure in flask is 0.84 atm. The equilibrium constant for the reaction is: A . 0.30 B. 0.18 c. 0.17 D. 0.11 |
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| 372 | 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% |
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| 373 | The graph (2) tells us that: A. The reaction is irreversible B. The reaction is reversible C. The reaction is exothermic D. The reaction is endothermic |
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| 374 | Which acid helps in the digestion of food without harming the stomach? A. ( H_{2} S O_{4} ) в. НС l c. ( C H_{3} ) СООН D. ( H_{3} P O_{4} ) |
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| 375 | Q.8 The ionisation constant of an acid, K, is the measure of strength of an acid. The K, values of acetic acid, hypochlorous acid and formic acid are 1.74 X 10″, 3.0 x 10-8 and 1.8 x 10-4 respectively. Which of the following orders of pH of 0 1 mol dm–solutions of these acids is correct? (a) Acetic acid > hypochlorous acid > formic acid (b) Hypochlorous acid > acetic acid > formic acid (c) Formic acid > hypochlorous acid > acetic acid (d) Formic acid > acetic acid > hypochlorous acid TL |
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| 376 | The values of ( boldsymbol{K}_{s p} ) of ( boldsymbol{C a C O}_{3} ) and ( mathrm{CaC}_{2} mathrm{O}_{4} ) are ( 4.7 times 10^{-9} ) and ( 1.3 times 10^{-9} ) respectively at ( 25^{circ} mathrm{C} ). If the mixture of these two is washed with water, what is the concentration of ( C a^{2+} ) ions in water? A ( cdot 7.746 times 10^{-5} M ) В. ( 5.831 times 10^{-5} M ) c. ( 6.856 times 10^{-5} M ) D. ( 3.606 times 10^{-5} M ) |
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| 377 | In the aqueous solution of sodium acetate the ion that undergoes hydrolysis is : A. ( C H_{3} C O O^{-} ) В. ( N a^{+} ) c. ( N a^{+} ) and ( C H_{3} C O O ) D. ( N a^{-} ) |
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| 378 | Equilibrium constant for the following reaction is ( 1 times 10^{-9} ) ( boldsymbol{C}_{5} boldsymbol{H}_{5} boldsymbol{N}(boldsymbol{a} boldsymbol{q} cdot)+boldsymbol{H}_{2} boldsymbol{O}(boldsymbol{l}) rightleftharpoons ) ( boldsymbol{C}_{5} boldsymbol{H}_{5} boldsymbol{N} boldsymbol{H}^{+}(boldsymbol{a} boldsymbol{q} cdot)+boldsymbol{O} boldsymbol{H}^{-}(boldsymbol{a} boldsymbol{q} cdot) ) Determine the mole of pyridinium chloride ( left(C_{5} H_{5} N . H C Iright) ) that should be added to ( 500 mathrm{mL} ) solution of ( 0.4 mathrm{M} ) pyridine ( left(C_{5} H_{5} Nright) ) to obtain a buffer solution of ( mathrm{pH}=5 ) A. 0.1 mole B. 0.2 mole c. 0.3 mole D. 0.4 mole |
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| 379 | Which of the following is not a characteristic of equilibrium? A. Rate is equal in both directions B. Measurable quantities are constant at equilibrium C . Equilibrium occurs in reversible condition D. Equilibrium occurs only in open vessel at constant temperature |
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| 380 | ( 20 % ) of ( N_{2} O_{4} ) molecule are dissociated in a sample of ( operatorname{gas} ) at 27 degree ( C ) and 760 torr mixture has the density at the equilibrium |
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| 381 | Select the anion which is the strongest bronsted base. A ( cdot C l O_{4}^{-} ) B. ( C l O_{3}^{-} ) ( mathrm{c} cdot mathrm{ClO}_{2}^{-} ) D. ( C l O^{-} ) |
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| 382 | The solubility of ( P b S O_{4} ) in water is ( 0.038 g L^{-1} ) at ( 25^{circ} C . ) Calculate its solubility at the same temperature. |
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| 383 | Common salt containing small amount of sodium iodide, is called iodised salt. A. True B. False |
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| 384 | A buffer solution is prepared by mixing ( 10 mathrm{ml} ) of ( 1.0 mathrm{M} ) acetic acid ( & 20 mathrm{ml} ) of 0.5 M sodium acetate and then diluted to ( 100 mathrm{ml} ) with distilled water. If the ( p K_{a} ) of ( C H_{3} C O O H ) is ( 4.76 . ) What is the pH of the buffer solution prepared? (1998) A . 3.84 B. 4.76 ( c cdot 4.34 ) D. 5.21 |
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| 385 | Calculate the pressure of ( C O_{2} ) gas at 700 K in heterogeneous equilibrium reaction ( boldsymbol{C a} boldsymbol{C O}_{3}(boldsymbol{g}) rightleftharpoons boldsymbol{C a O}(boldsymbol{s})+ ) ( C O_{2}(g) ) if ( Delta H ) for this reaction is ( 130.2 k J ) |
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| 386 | Plaster of paris should be stored in a moisture proof container because: A. it absorbs moisture from the atmosphere and becomes hard B. it cannot be stored in plastic c. it will change its colour D. it will become soft |
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| 387 | Which of the following give brisk effervescence with baking soda? A. methanoic acid B. propanoic acid c. ethanoic acid D. all of these |
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| 388 | The gaseous phase neutralisation reaction can be explained only on the basis of: A. Arrhenius theory B. Lowry -Bronsted theory c. Lewis theory D. Bohrs theory |
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| 389 | ( 25 m L ) of ( 0.107 M H_{3} P O_{4} ) was titrated with ( 0.115 M ) solution of ( N a O H ) to the end point identified by indicator bromocresol green. This required ( 23.1 m L ) The titration was repeated using phenolphthalein as indicator. This time ( 25 m L ) of ( 0.107 M H_{3} P O_{4} ) required ( 46.2 m L ) of the ( mathbf{0 . 1 1 5} M_{N a O H . text { What is the }} ) coefficient ( ^{prime} boldsymbol{n}^{prime} ) in the following reaction? ( boldsymbol{H}_{3} boldsymbol{P} boldsymbol{O}_{4}+boldsymbol{n} boldsymbol{O} boldsymbol{H}^{-} rightarrowleft[boldsymbol{H}_{3-n} boldsymbol{P} boldsymbol{O}_{4}right]^{n-}+ ) ( boldsymbol{n} boldsymbol{H}_{2} boldsymbol{O} ) |
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| 390 | Equilibrium constants for the following reaction at ( 1200 mathrm{K} ) are given ( 2 H_{2} O(g) leftrightharpoons 2 H_{2}(g)+O_{2}(g) ; K_{1}= ) ( 6.4 times 10^{-8} ) ( 2 C O_{2}(g) leftrightharpoons 2 C O(g)+O_{2}(g) ; K_{2}= ) ( mathbf{1 . 6} times mathbf{1 0}^{-mathbf{6}} ) The equilibrium constant for the reaction ( boldsymbol{H}_{2}(boldsymbol{g})+boldsymbol{C} boldsymbol{O}_{2}(boldsymbol{g}) leftrightharpoons boldsymbol{C} boldsymbol{O}(boldsymbol{g})+boldsymbol{H}_{2} boldsymbol{O}(boldsymbol{g}) ) at ( 1200 mathrm{K} ) will be: A. 0.05 в. 20 c. 0.2 D. 5.0 |
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| 391 | Calculate the equilibrium constants for the reactions with water of ( H_{2} P O_{4}^{ominus}, H P O_{4}^{2-} ) and ( P O_{4}^{3-} ) as base Comparing the relative values of two equilibrium constants of ( boldsymbol{H}_{2} boldsymbol{P} boldsymbol{O}_{4}^{ominus} ) with water, deduce whether solutions of this ion in water are acidic or bases. Deduce whether solutions of ( boldsymbol{H} boldsymbol{P} boldsymbol{O}_{4}^{2-} ) are acidic or bases. Given ( K_{1}, K_{2} ) and ( K_{3} ) for ( boldsymbol{H}_{3} boldsymbol{P} boldsymbol{O}_{4} ) are ( mathbf{7 . 1} times mathbf{1 0}^{-mathbf{3}}, mathbf{6 . 3} times mathbf{1 0}^{-mathbf{8}} ) and ( 4.5 times 10^{-13} ) respectively A ( .1 .4 times 10^{-12}, 1.6 times 10^{-7}, 2.2 times 10^{-2}, H_{2} P O_{4}^{circ} ) is acidic and ( H P O_{4}^{2-} ) is basic B . ( 2.2 times 10^{-12}, 1.6 times 10^{-7}, 1.4 times 10^{-2}, H_{2} P O_{4}^{ominus} ) is basic and ( H P O_{4}^{2-} ) is basic C ( .2 .2 times 10^{-12}, 1.6 times 10^{-7}, 1.4 times 10^{-2}, H_{2} P O_{4}^{circ} ) is acidic and ( H P O_{4}^{2-} ) is basic D. ( 1.4 times 10^{-12}, 1.6 times 10^{-7}, 2.2 times 10^{-2}, H_{2} P O_{4}^{circ} ) is basic and ( H P O_{4}^{2-} ) is acidic |
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| 392 | In a mixture of weak acid and its salt, the ratio of the concentration of salt to acid is increased tenfold.The pH of the solution would increase by: A. 0.5 B. ( c cdot 10 ) D. |
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| 393 | What do the letters I ( C ) and ( E ) stand for in a RICE table? A . Initial, Change, Equilibrium B. Initial, Concentration, Equilibrium c. Instant, Change Equilibrium D. Instant, Concentration, Equilibrium E. Initial, Change, Exact amounts |
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| 394 | When inert gas at constant pressure is added to the given reversible process then the equilibrium will: A. be unaffected B. shift in backward direction c. shift in forward direction D. cannot predicted |
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| 395 | Which of the following is/are ionization? This question has multiple correct options A ( cdot N a rightarrow N a^{+}+e^{-} ) B. ( C l+e^{-} rightarrow C l^{-} ) c. ( N a C l rightarrow N a^{+}+C l^{-} ) D. ( M g B r_{2} rightarrow M g^{2+}+2 B r ) |
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| 396 | Which of the following is correct for acid buffer? ( [text { salt }=H A, text { acid }=A] ) A ( cdot p^{K a}=p^{H}-log frac{[H A]}{|A|} ) B・ ( p^{H}=p^{K a}+log frac{[H A]}{|A|} ) c. ( p^{K a}=p^{H}-log frac{[A]}{[H A]} ) D・ ( p^{H}=p^{K a}+log frac{[A]}{[H A]} ) |
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| 397 | Which of the following is correct regarding buffer solution? A. It contains weak acid and its conjugate base. B. It shows low change in pH on adding small amount of acid or base. c. (A) and (B) both D. None of these |
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| 398 | Which of the following are Bronsted acids as well as Bronsted bases? ( N H_{3}, H S O_{4}^{-}, H_{2} S O_{4}, H C O_{3}^{-}, H_{3} O ) |
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| 399 | In the following strong acid and strong alkaine base is- (a) Acetic Acid or Hydrochloric Acid (b) Sodium hydroxide or calcium hydroxide |
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| 400 | A chemical which turns red litmus to blue is: A . acidic in nature B. basic in nature c. neutral in nature D. can be acidic or basic in nature |
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| 401 | Q2. The values of Ksp of two sparingly soluble salts Ni(OH), and AgCN are 2.0 * 10 6x 10-respectively. Which salt is more soluble? Explain. ana OT |
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| 402 | Given that ( boldsymbol{K}_{c}=mathbf{1 3 . 7} ) at ( mathbf{5 4 6 K} ) for ( boldsymbol{P C l}_{5}(boldsymbol{g}) rightleftharpoons boldsymbol{P C l}_{3}(boldsymbol{g})+boldsymbol{C l}_{2}(boldsymbol{g}) ) calculate what pressure will develop in a 10 litre box at equilibrium at ( 546 K ) when 1.00 mole of ( P C l_{5} ) is injected into the empty box? |
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| 403 | ( P C l_{2} rightleftharpoons P C l_{3}+C l_{2} ) in the reversible reaction the moles of ( boldsymbol{P C l}_{2}, boldsymbol{P C l}_{3} ) and ( C l_{2} ) are ( a, b ) and ( c ) respectively and total pressure is ( boldsymbol{P} ) then value of ( boldsymbol{K}_{boldsymbol{p}} ) is A ( cdot frac{b c}{a} R T ) в. ( frac{b}{(a+b+c)} P ) c. ( frac{b c P}{a(a+b+c)} ) D. ( frac{c}{(a+b+c)} P ) |
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| 404 | Addition of water to this solution will not change ( left[boldsymbol{H}_{3} boldsymbol{O}^{+}right] ) A. Chemical pH indicator B. Acid/base buffer c. Anhydrous solution D. Hypotonic solution |
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| 405 | What will be the pH of solution when ‘A’ and ‘C’ solutions are mixed completely? A. 9.5 B. 5 c. 10.15 D. 8.85 |
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| 406 | The pH of the solution obtained by mixing ( 100 mathrm{ml} ) of a solution of ( mathrm{pH}=3 ) with ( 400 mathrm{ml} ) of a solution of ( mathrm{pH}=4 ) is : A. ( 3-log 2.8 ) B. ( 7-log 2.8 ) c. ( 4-log 2.8 ) D. ( 5-log 2.8 ) |
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| 407 | Which of the following statement is correct about an aqueous solution of an acid and a base? (i) Higher the pH, stronger the acid. (ii) Higher the pH, weaker the acid. (iii) Lower the pH, stronger the base. (iv) lower the pH, weaker the base. ( A cdot ) (i) and (iii) B. (ii) and (iii) c. (i) and (iv) D. (ii) and (iv) |
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| 408 | The equation for the solubility product constant of ( boldsymbol{A} boldsymbol{g}_{2} boldsymbol{C r} boldsymbol{O}_{4} ) is: A ( cdot K_{s p}=left[A g^{2+}right] cdotleft[C r O^{2-}right] ) B . ( K_{s p}=left[A g^{+}right]^{2} cdotleft[C r^{6+}right] cdotleft[O_{4}^{8-}right] ) C ( cdot K_{s p}=left[A g^{+}right] cdotleft[C r^{6+}right] cdotleft[O_{4}^{8-}right. ) D. ( K_{s p}=left[A g^{+}right]^{2} cdotleft[C r O_{4}^{2-}right] ) |
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| 409 | Q16. What is the equilibrium concentration of each of the substances in the equilibrium when the initial concentration of ICI was 0.78 M? 2ICI(g) = 1,(8) + C1,(g); K = 0.14 11-1 |
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| 410 | What will happen if the pH of the solution of ( 0.001 mathrm{M} M gleft(N O_{3}right)_{2} ) solution is adjusted to ( boldsymbol{p} boldsymbol{H}=mathbf{9} ? ) ( left[text { Given that }: boldsymbol{K}_{s p} text { of } M g(boldsymbol{O} boldsymbol{H})_{2}=mathbf{8 . 9} timesright. ) ( mathbf{1 0}^{-12} ) ) A. ppt will take place B. ppt will not take place c. solution will be saturated D. none of the above |
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| 411 | An aqueous solution at room temperature is ( 0.1 M ) with respect to ammonium chloride and ( 0.1 M ) with respect to ( N H_{4} O Hleft(p K_{b}=5right), ) the ( p H ) of the solution is: A . 7.5 B. 6.8 c. 6.5 D. 9. |
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| 412 | The rate law for a reaction between the substances ( A ) and ( B ) is given by: Rate ( =boldsymbol{K}[boldsymbol{A}]^{n}[boldsymbol{B}]^{m} . ) On doubling the concentration of ( A ) and having concentration of ( B ) the ratio of new rate law to the earlier rate of the reaction will be as ( mathbf{A} cdot n-m ) B ( cdot 2^{(n-m)} ) c. ( frac{1}{2^{m+n}} ) D. ( m+n ) |
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| 413 | Assertion Osmotic pressure of ( 0.1 N ) urea solution is less than that of ( 0.1 M ) NaCl solution. Reason Osmotic pressure is not colligative property. 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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| 414 | Assertion On adding ( H_{2} S O_{4} ) to water, the resulting aqueous solution get corrosive. Reason Hydronium ions are responsible for corrosive action. 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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| 415 | ( boldsymbol{p} boldsymbol{K}_{boldsymbol{b}} ) of ( boldsymbol{N} boldsymbol{H}_{3} ) is ( boldsymbol{4} . boldsymbol{7} 4 ) and ( boldsymbol{p} boldsymbol{K}_{boldsymbol{b}} ) of ( boldsymbol{A}^{-}, boldsymbol{B}^{-} ) and ( C^{-} ) are 4,5 and 6 respectively. Aqueous solution of ( 0.01 M ) has ( p H ) in the increasing order. A ( . N H_{4} A<N H_{4} B<N H_{4} C ) B. ( N H_{4} C<N H_{4} B<N H_{4} A ) C . ( N H_{4} C<N H_{4} A<N H_{4} B ) D. All have equal ( p H ) |
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| 416 | Assertion: The solubility product of hydroxide of ( F e^{2+} ) is higher than that of ( boldsymbol{F} boldsymbol{e}^{boldsymbol{3}+} ) Reason: The lattice energy of ( boldsymbol{F e}(boldsymbol{O} boldsymbol{H})_{2} ) is lower than that of ( F e(O H)_{3} ) 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 Assertion and Reason are false |
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| 417 | . 44 Assertion (A) Increasing order or acidity of hydrogen halides is HF < HCI < HBr < HI. Reason (R) While comparing acids formed by the elements belonging to the same group of periodic table, H-A bond strength is a more important factor in determining acidity of an acid than the polar nature of the bond. (a) Both A and R are true R is the correct explanation of A (b) Both A and Rare true but is not the correct explanation of A (c) A is true but R is false (d) Both A and Rare false |
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| 418 | Species acting as Bronsted acid and base is: A. ( H S O_{4}^{-} ) в. ( N a_{2} C O_{3} ) c. ( N H_{3} ) D. ( O H^{-} ) |
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| 419 | State which of the following solutions contain both molecules and ions? A. ( C H_{3} ) СООН в. ( N a_{2} C O_{3} ) c. oxalic acid D. All of these |
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| 420 | For the reaction, ( boldsymbol{H}_{2}(boldsymbol{g})+boldsymbol{I}_{2}(boldsymbol{g}) rightleftharpoons ) ( 2 H I(g), ) the equilibrium constant ( K_{p} ) changes with: A. total pressure B. catalyst C. the amounts of ( H_{2} ) and ( I_{2} ) present D. temperature |
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| 421 | The pH of blood stream is maintained by a proper balance of ( boldsymbol{H}_{2} boldsymbol{C O}_{3} ) and ( N a H C O_{3} ) concentration. What volume of ( 5 M N a H C O_{3} ) solution should be mixed with a ( 10 mathrm{mL} ) sample of blood which is ( 2 M ) in ( H_{2} C O_{3} ) in order to maintain its pH? ( mathbf{A} cdot 40 mathrm{mL} ) B . ( 38 mathrm{mL} ) c. ( 50 mathrm{mL} ) D. ( 78 mathrm{mL} ) |
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| 422 | ( C H_{3} C H_{2} O H ) on reaction with bleaching powder forms: A ( . C H C l_{3} ) в. ( C C l C H O ) c. ( C H_{2} ) ClCHO D. ( C C l_{4} ) |
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| 423 | Match the items in column-I with those in column – II begin{tabular}{lllll} & Column I & & Column II \ & & & \ 1. & Electric Fuse & A & Chemical Effect \ hline 2. & Relay & B & Electric Discharge \ 3. & CFL & C & Magnetic effect \ 4. & Button Cell & D & Heating Effect end{tabular} Which of the following shows the correct matching? ( A cdot 1-C, 2-B, 3-A, 4-D ) B. ( 1-B, 2-A, 3-C, 4-D ) c. ( 1- ) D, ( 2-c, 3-B, 4-A ) D. ( 1- ) D, ( 2-B, 3-C, 4-A ) |
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| 424 | Show that for reaction ( A B(g) rightleftharpoons A(g)+ ) ( mathrm{B}(mathrm{g}), ) the total pressure at which ( mathrm{AB} ) is ( 50 % ) dissociated is numerically equal to three times of ( boldsymbol{K}_{boldsymbol{p}} ) |
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| 425 | The ( p H ) of ( 0.001 M C H_{3} C O O H ) is: ( A cdot 3 ) B. 1 c. ( 3-7 ) D. |
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| 426 | Q66. Calculate the pH of the resultant mixtures (a) 10 mL of 0.2 M Ca (OH), + 25 mL of 0.1 M HCI (b) 10 mL of 0.01 M H,SO, + 10 mL of 0.01 M Ca (OH), (c) 10 mL of 0.1 MH,50, + 10 mL of 0.1 M KOH 10 :11: |
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| 427 | A buffer solution, ( 0.080 M ) in ( N a_{2} P O_{4} ) and ( 0.020 M ) in ( N a_{3} P O_{4} ) is prepared. The electrolytic oxidation of 1.0 mmol of the organic compound ( R N H O H ) is carried out in ( 100 mathrm{m} L ) of the buffer. The reaction is as follows: ( boldsymbol{R} boldsymbol{N} boldsymbol{H} boldsymbol{O} boldsymbol{H}+boldsymbol{H}_{2} boldsymbol{O} longrightarrow boldsymbol{R} boldsymbol{N} boldsymbol{O}_{2}+ ) ( 4 H^{+}+4 e ) Calculate the approximate ( p H ) of the solution after the oxidation is complete. A . 6.19 B. 7.81 c. 10.34 D. 12.45 |
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| 428 | Q13. SO,2-is Bronsted base or acid and why? | 11 |
| 429 | Then equilibrium constant for the reaction is: For the following reactions, equilibrium constants are indicated on the arrow [ begin{array}{l} mathrm{H}_{3} mathrm{PO}_{4} stackrel{K_{1}}{Leftrightarrow} mathrm{H}^{+}+mathrm{H}_{2} mathrm{PO}_{4} \ mathrm{H}_{2} mathrm{PO}_{4}^{*} Leftrightarrow mathrm{H}^{*}+mathrm{HPO}_{4}^{-2} \ mathrm{HPO}_{4}^{-2} stackrel{K_{3}}{Leftrightarrow} mathrm{H}^{+}+mathrm{PO}_{4}^{-3} end{array} ] Then equilibrium constant for the reaction [ mathrm{H}_{3} mathrm{PO}_{4} Leftrightarrow quad 3 mathrm{H}^{+}+mathrm{PO}_{4}^{3} text { will be } ] ( mathbf{A} cdot K_{1}+K_{2}+K_{3} ) B . ( sqrt{K_{1} K_{2} K_{3}} ) ( mathbf{c} cdot K_{1} times K_{2} times K_{3} ) D. ( frac{1}{K_{1} K_{2} K_{3}} ) |
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| 430 | The chemical formula of king of chemicals, sulphuric acid is : A ( cdot H_{2} S_{2} O_{3} ) в. ( H_{2} S O_{3} ) c. ( H S O_{4} ) D. ( H_{2} S O_{4} ) |
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| 431 | Ammonia is a weak base that reacts with water according to the equation: ( N H_{3}(a q)+2 H_{2} O(l) quad rightleftharpoons ) ( N H_{4}^{+}(a q)+O H^{-}(a q) ) Which of the following conditions will decrease the moles of ammonium in water? This question has multiple correct options A. Addition of ( H C l ) B. Addition of ( N a O H ) c. Addtion of ( N H_{4} C l ) D. Addition of ( H_{2} O ) |
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| 432 | For ( boldsymbol{C r}_{2} boldsymbol{O}_{mathbf{7}}^{-2}+mathbf{1 4} boldsymbol{H}^{+}+boldsymbol{6} boldsymbol{e}^{-} rightarrow ) ( mathbf{2} boldsymbol{C r}^{+mathbf{3}}+mathbf{7 H}_{mathbf{2}} boldsymbol{O} ; quad boldsymbol{E}^{boldsymbol{o}}=mathbf{1 . 3 3} boldsymbol{V} ) At ( left[boldsymbol{C r}_{2} boldsymbol{O}_{7}^{-2}right]=mathbf{4 . 5} ) millimole, ( left[boldsymbol{C r}^{+3}right]= ) 15 millimole, ( boldsymbol{E} ) is 1.067 V. The pH of the solution is nearly equal to : A . 3 B. 4 ( c cdot 2 ) D. 5 |
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| 433 | The conjugate acid of ( boldsymbol{O}^{-2} ) ion is: A ( . O H^{-} ) B. ( O H^{+} ) c. ( H_{2} O ) D. ( H O_{2}^{-} ) |
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| 434 | For the reaction ( boldsymbol{P C l}_{3}(boldsymbol{g})+boldsymbol{C l}_{2}(boldsymbol{g}) rightleftharpoons ) ( boldsymbol{P C l}_{5}(boldsymbol{g}) ) the value of ( boldsymbol{K}_{c} ) at ( 250^{circ} boldsymbol{C} ) is 26 The value of ( boldsymbol{K}_{boldsymbol{p}} ) at this temperature will be: A . 0.61 B. 0.57 c. 0.83 D. 0.46 |
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| 435 | The pH of a solution of hydrochloric acid is ( 4 . ) The molar concentration of this solution is: A . 4.0 B. 0.4 c. 0.000 D. 0.04 |
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| 436 | Two weak acids ( H A ) and ( H B ) have same ( p H ) when their concentration ratio is ( 3: 1 . ) The ratio of the dissociation constants of ( H B ) and ( H A ) is |
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| 437 | An equimolar solution of ( N a N O_{2} ) and ( H N O_{2} ) can act as a: A. strong reductant B. strong oxidant c. buffer solution D. none of these |
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| 438 | In the reaction, ( C(s)+C O_{2}(g) leftrightharpoons ) ( 2 C O(g), ) the equilibrium pressure is 12 atm. If ( 50 % ) of ( C O_{2} ) reacts, calculate ( K_{p} ) A. 1.6 atm B. 0.16 atm ( c cdot 16 operatorname{atm} ) D. 160 atm |
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| 439 | Which of the following will not change the concentration of ammonia in the equilibrium? ( N_{2}(g)+3 H_{2}(g) rightleftharpoons 2 N H_{3}(g) ; Delta H= ) ( -boldsymbol{x} boldsymbol{k} boldsymbol{J} ) A. increase of pressure B. increase of temperature c. decrease of volume D. addition of catalyst |
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| 440 | For the reaction ( N_{2} O_{4}(g) rightleftharpoons 2 N O_{2}(g) ) if percentage dissociation of ( N_{2} O_{4} ) and ( 20 %, 45 %, 65 % ) and ( 80 % ) then the sequence of observed vapour densities will be: A ( cdot d_{20}>d_{45}>d_{65}>d_{80} ) В. ( d_{80}>d_{65}>d_{45}>d_{20} ) C ( . d_{20}=d_{45}=d_{65}=d_{80} ) D ( cdotleft(d_{20}=d_{45}right)>left(d_{65}=d_{80}right) ) |
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| 441 | Of the following solutions, the one that is acidic is: A ( cdot Z n S O_{4}(a q .) ) в. ( operatorname{NaAl}(O H)_{4}(text {аq.}) ) ( mathbf{c} cdot operatorname{NaH} C O_{3}(a q) ) D ( cdot K N O_{3}(a q .) ) |
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| 442 | Which change in the system will drive equilibrium to the left in the following reaction? ( N_{2} O_{5}(g)=N O_{2}(g)+N O_{3}(g) ) A. Increase the volume B. Increase the pressure c. Decrease the amount of ( N O_{3} ) D. Increase the amount of ( N_{2} O_{5} ) |
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| 443 | The ( p H ) of a buffer solution is ( 5 . p K a ) of the acid present in it is 4. What is the ratio of acid and salt present in the solution? A . 1: B. 1:10 ( c cdot 10: ) D. 1: 2 |
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| 444 | Which has the highest pH? A. ( C H_{3} ) СООК в. ( N a_{2} C O_{3} ) c. ( N H_{4} C l ) D. ( operatorname{NaNO}_{3} ) |
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| 445 | ( N_{2(g)}+3 H_{2(g)} leftrightarrow 2 N H_{3(g)} ) If some ( H C l ) gas is passed into the reaction mixture at the equilibrium of this reaction,then: A. Equilibrium position shifts towards left B. Equilibrium position shifts towards right c. concentration of ( H_{2} ) increases D. The equilibrium position is not affected |
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| 446 | Which of the following acids is a weak electrolyte? A. ( H_{2} C O_{3} ) в. ( C H_{3} ) СООН c. Both A and B D. None of the above |
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| 447 | ( boldsymbol{K}_{s p} ) of ( M boldsymbol{g}(boldsymbol{O} boldsymbol{H})_{2} ) is ( 1 times ) ( mathbf{1 0}^{-mathbf{1 2}}, mathbf{0 . 0 1} boldsymbol{M} mathbf{M g} mathbf{C l}_{mathbf{2}} ) will be precipitating at the limiting pH: ( A cdot 8 ) B. 9 ( c cdot 10 ) D. 12 |
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| 448 | For the equilibrium, ( boldsymbol{H}_{2} boldsymbol{O}(boldsymbol{s}) Leftrightarrow boldsymbol{H}_{2} boldsymbol{O}(boldsymbol{l}) ) which of the following is true? A. The pressure changes do not affect the equilibrium. B. The amount of ice that melts is more, if the pressure on the system is increased c. The amount of liquid that freezes is more, if the pressure on the system is increased. D. At low pressure, the nature of equilibrium changes to forward direction |
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| 449 | What is the partial pressure (atm) of HI in the equilibrium mixture? A . 6.385 в. 12.77 c. 40.768 D. 646.58 |
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| 450 | Which of the following acids, listed with their ionization constant at ( 25^{circ} C ), is the strongest? A . Nitrous acid ( left(H N O_{2}right) K_{i}=4.5 times 10^{-4} ) B. Formic acid ( left(H C H O_{2}right) K_{i}=1.8 times 10^{-4} ) C . Benzoic acid ( left(H C_{7} H_{5} O_{2}right) K_{i}=6.3 times 10^{-5} ) D. Acetic acid ( left(H C_{2} H_{3} O_{2}right) K_{i}=1.8 times 10^{-5} ) E . Hydrocyanic acid (H ( C N ) ) ( K_{i}=4.0 times 10^{-10} ) |
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| 451 | ( K_{h} ) values for ( boldsymbol{A} boldsymbol{r}(boldsymbol{g}), boldsymbol{C} boldsymbol{O}_{2}(boldsymbol{g}), boldsymbol{H} boldsymbol{C} boldsymbol{H} boldsymbol{O}_{(boldsymbol{g})} ) and ( boldsymbol{C} boldsymbol{H}_{4}(boldsymbol{g}) ) are ( 40.39,1.67,1.83 times 10^{-5} ) and 0.413 respectively. The order of their increasing solubility is: A. ( H C H O<C H_{4}<C O_{2}<A r ) в. ( H C H O<C O_{2}<C H_{4}<A r ) c. ( A r<C O_{2}<C H_{4}<H C H O ) D. ( A r<C H_{4}<C O_{2}<H C H O ) |
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| 452 | Q11. State Ostwald’s dilution law. | 11 |
| 453 | For the reaction ( boldsymbol{P} boldsymbol{C l}_{5}_{5} rightleftharpoons boldsymbol{p} boldsymbol{C l}_{3(g)}+ ) ( C l_{2(g)}, ) the forward reaction at constant temperature is favoured by: A. introducing an inert gas at constant volume B . introducing ( C l_{2} ) at constant volume C . introducing ( P C l_{5} ) at constant volume D. reducing the volume of the container |
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| 454 | What is the ( H^{+} ) ion concentration in ammonium acetate solution? ( left(boldsymbol{K}_{boldsymbol{a}}=mathbf{1 . 8} times mathbf{1 0}^{-mathbf{5}}, boldsymbol{K}_{boldsymbol{b}}=mathbf{1 . 8} times mathbf{1 0}^{-mathbf{5}}, boldsymbol{K}_{boldsymbol{v}}right. ) |
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| 455 | What ( left(H_{3} O^{+}right) ) must be maintained in a saturated ( H_{2} S ) solution to precipitate ( P b^{2+}, ) but not ( Z n^{2+} ) from a solution in which each ion is present at a concentration of ( 0.01 M ? ) ( left(K_{s p} H_{2} S=1.1 times 10^{-22} ) and right. ( boldsymbol{K}_{s p} Z boldsymbol{n} boldsymbol{S}=mathbf{1 . 0} times mathbf{1 0}^{-mathbf{2 1}} mathbf{)} ) |
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| 456 | ( 0.16 g ) of ( N_{2} H_{4} ) are dissolved in water and the total volume made up to 500 ( m L ). Calculate the percentage of ( N_{2} H_{4} ) that has reached with water at this dilution. The ( K_{b} ) for ( N_{2} H_{4} ) is ( 4.0 times ) ( mathbf{1 0}^{-6} boldsymbol{M} ) |
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| 457 | Degree of ionisation does not depend on: A. nature of the solvent B. nature of the electrolyte c. dilution D. molecular mass of the electrolyte |
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| 458 | The ( p K_{a} ) of acetylsalicylic acid (aspirin) is 3.5 The pH of gastric juice in human stomach is about ( 2-3 ) and the pH in the same intestine is about ( 8 . ) Aspirin will be A. Unionised in the small intestine and in the stomach B. Completely ionised in the small intestine and in the stomach c. lonised in the stomach and almost unionised in the samılı intestine D. lonised in small intestine and almost unionised in the stomach |
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| 459 | Which of the following will function as buffer? This question has multiple correct options A. ( N a C l+N a O H ) в. Borax + Boric acid c. ( N a H_{2} P O_{4}+N a_{2} H P O_{4} ) D. ( N H_{4} C l+N H_{4} O H ) |
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| 460 | According to Lewis concept, acid is: A. proton donor B. electron pair donor C . electron pair acceptor D. proton acceptor |
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| 461 | To which type of reaction, Le Chatelier’s principle can always be applied? A . Reversible B. Elementary c. synthesis D. Decomposition E. Double Replacement |
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| 462 | A mixture of ( boldsymbol{H}_{2} boldsymbol{O} ) and solid ( boldsymbol{A} boldsymbol{g} boldsymbol{C l} ) shaken to obtain saturated solution. The solid is filtered and to ( 100 m L ) filtrate, ( 100 m L ) of ( 0.03 M N a B r ) is added, will a precipitate formed? ( boldsymbol{K}_{s p} boldsymbol{A} boldsymbol{g} boldsymbol{C l}=mathbf{1 0}^{-10}, boldsymbol{K}_{s p} boldsymbol{A} boldsymbol{g} boldsymbol{B r}=mathbf{5} times ) ( mathbf{1 0}^{-13} ) |
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| 463 | The equilibrium constant for the reaction ( 3 A+2 B rightleftharpoons C ) will be: A ( cdot frac{[3 A][2 B]}{[C]} ) ( ^{mathbf{B}} cdot frac{[A]^{3}[B]}{[C]} ) c. ( frac{[C]}{[A]^{3}[B]^{2}} ) D. ( frac{[C]}{[3 A][2 B]} ) |
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| 464 | State whether the given statement is true or false: Bleaching powder contains about 50 % available chlorine. |
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| 465 | ( Z n S rightarrow ) solubility in water ( =0.97 g K ) we mixed 2 moles of ( Z nleft(N O_{3}right)_{2} ) is ( 5 L ) solution. Find new solubility of Zn? |
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| 466 | Q2. State the law of mass action? | 11 |
| 467 | A gaseous hypothetical chemical equation ( 2 A rightleftharpoons 4 B+C ) is carried out in a closed vessel. The concentration of ( B ) is found to be increase by ( 5 x ) ( 10^{3} ) mol. ( L^{-1} . ) in 10 seconds. The rate of appearance of ( B ) is: A ( cdot 5 times 10^{2} mathrm{molL}^{-1} mathrm{sec}^{-1} ) B. ( 5 times 10^{5} mathrm{mol} mathrm{L}^{-1} mathrm{sec}^{-1} ) c. ( 6 times 10^{-5} mathrm{mol} mathrm{L}^{-1} mathrm{sec}^{-1} ) D. ( 4 times 10^{-4} mathrm{mol} mathrm{L}^{-1} mathrm{sec}^{-1} ) |
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| 468 | ( X e F_{6}+H_{2} O rightleftharpoons X e O F_{4}+2 H F ) constant ( =k_{1}, X e O_{4}+X e F_{6} rightleftharpoons ) ( X e O F_{4}+X e O_{3} F_{2} ) constant ( =K_{2} ) Then equilibrium constant for the following reaction will be: ( boldsymbol{X} boldsymbol{e} boldsymbol{O}_{4}+boldsymbol{2} boldsymbol{H} boldsymbol{F} rightleftharpoons boldsymbol{X} boldsymbol{e} boldsymbol{O}_{3} boldsymbol{F}_{2}+boldsymbol{H}_{2} boldsymbol{O} ) A ( cdot frac{K_{2}}{K_{1}} ) в. ( K_{1}+K_{2} ) c. ( frac{K_{1}}{K_{2}} ) D. ( frac{K_{1}}{left(K_{2}right)^{2}} ) |
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| 469 | R. 35 Calculate the volume of water required to dissolve 0.1 g lead (11) chloride to get a saturated solution. (Ksp of PbCl2 = 3.2x 10-8, atomic mass of Pb= 207u) |
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| 470 | Chemical equilibrium is dynamic because: A. the equilibrium attained quickly B. the concentration of the reactants and products become same at equilibrium c. the concentration of reactants and products are constant but different D. both forward and backward reactions occur at all time with the same speedd |
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| 471 | ( 40 % ) of ( P C l_{s} ) is not dissociated at ( 300^{0} C . ) The reaction is carried out in a flask of 1 litre capacity. The value of ( boldsymbol{K}_{boldsymbol{c}} ) would be: A. 3.2 B. 1.6 ( c .2 .8 ) D. 0.9 |
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| 472 | The equilibrium constant ( K ) for the reaction ( : 2 H I(g) rightleftharpoons H_{2}(g)+I_{2}(g) ) at room temperature is 2.85 and that at ( 698 K ) is ( 1.4 times ! 0^{-2} . ) This implies that the forward reaction is: A. exothermic B. endothermic c. slow D. unpredictable |
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| 473 | toppr LoGIN vow 5 Q Type your question acid or base is added to it. Buffer solutions have wide applications. ( 20.0 m L ) of ( 0.10 M ) of 1 -aminopropane is titrated with ( 0.10 M ) of ( H C l . ) The ( p H ) at the equivalence point is ( p simeq 6 ) and the appropriate acid-base indicator. is Methyl red. (4.2-6.2) wright the right answer Table 1. Table 1: List of acid/base indicators Common name ( quad ) Transition range, ( p boldsymbol{H} quad ) color change ser red- orange Methyl orange Methyl red ( 4.2^{-6.2} ) red- yellow Phenol red ( 6.8-8.2 ) yellow- red ( y ) ( r ) Phenolphthalein ( quad 8.0-9.8 quad ) colorlessThymolphthalein ( quad 9.3-10.5 quad begin{array}{l}text { colorless- } \ text { blue }end{array} ) |
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| 474 | In the reaction ( C_{(g)}+C O_{2(g)} rightleftharpoons 2 C O_{(g)} ) the equilibrium pressure is 12 atm. IF ( 50 % ) of ( C O_{2} ) reacts, ( K_{p} ) for the change is: A . 12 atm B. 32 atm ( c .64 a t m ) D. 16 atm |
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| 475 | Which solution has the greatest percent ionization? ( mathbf{A} cdot 0.10 mathrm{M} N H_{3}left(K_{b}=1.8 times 10^{-5}right) ) B. 0.25 M ( H N O_{2}left(K_{1}=4.5 times 10^{-4}right) ) C . 1.000 M HCOOH ( left(K_{a}=1.7 times 10^{-4}right) ) D . ( 2.000 mathrm{M} C H_{3} N H_{2}left(K_{b}=4.4 times 10^{-4}right) ) |
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| 476 | ( boldsymbol{B} boldsymbol{a} boldsymbol{S} boldsymbol{O}_{4}(boldsymbol{s}) rightleftharpoons boldsymbol{B} boldsymbol{a}^{2+}(boldsymbol{a} boldsymbol{q})+boldsymbol{S} boldsymbol{O}_{4}^{2-}(boldsymbol{a} boldsymbol{q}) ) Whai is ( K_{s p} ) for above reaction? ( mathbf{A} cdotleft[B a^{2+}right]left[S O_{4}^{2-}right] ) ( ^{mathbf{B} cdot} frac{left[B a^{2+}right]left[S O_{4}^{2-}right]}{B a S O_{4}} ) ( ^{mathrm{c}} cdot frac{left[B a^{2+}right]left[S O_{4}^{2-}right]}{left[B a S O_{4}right]} ) D. None |
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| 477 | The ( p H ) of a solution which is ( 0.1 M ) sodium acetate and ( 0.01 M ) acetic acid ( left(p K_{a}=4.74right) ) would be: A . 4.2 B. 5.1 ( c .5 .74 ) D. None of these |
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| 478 | The solubility product of lead iodide is ( 1.4 times 10^{-8} . ) Calculate its molar solubility in ( 0.1 M K I ) solution. |
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| 479 | The equilibrium constant ( boldsymbol{K}_{boldsymbol{p}} ) for the reaction ( N_{2} O_{4}(g) rightleftharpoons 2 N O_{2}(g) ) is 4.5 What would be the average molar mass (in g/mol) of an equilibrium mixture of ( N_{2} O_{4} ) and ( N O_{2} ) formed by the dissociation of pure ( N_{2} O_{4} ) at a total pressure of 2 atm? ( mathbf{A} cdot 69 ) в. 57.5 ( c .80 .5 ) D. 85.5 |
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| 480 | ( boldsymbol{H}_{3} boldsymbol{P} boldsymbol{O}_{4} rightleftharpoons boldsymbol{H}^{oplus}+boldsymbol{H}_{2} boldsymbol{P} boldsymbol{O}_{4}^{ominus} ; boldsymbol{K}_{a_{1}} ) ( boldsymbol{H}_{3} boldsymbol{P} boldsymbol{O}_{4}^{ominus} rightleftharpoons boldsymbol{H}^{oplus}+boldsymbol{H} boldsymbol{P} boldsymbol{O}_{4}^{2-} ; boldsymbol{K}_{a_{2}} ) ( boldsymbol{H} boldsymbol{P} boldsymbol{O}_{4}^{2-} rightleftharpoons boldsymbol{H}^{oplus}+boldsymbol{P} boldsymbol{O}_{4}^{3-} ; boldsymbol{K}_{a_{3}} ) Mark out the incorrect statements This question has multiple correct options ( mathbf{A} cdot K_{a_{1}}>K_{a_{2}}>K_{a_{3}} ) B. ( _{p Hleft(H_{2} P O_{4}^{circ}right)=frac{p K_{a_{1}}+p K_{a_{2}}}{2}} ) C. Both ( H_{3} P O_{4} ) and ( H_{2} P O_{4}^{odot} ) are more acidic than ( H P O_{4}^{2} ) D. only ( H P O_{4}^{2-} ) is amphiprotic anion in the solution |
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| 481 | How many of the following reactions goes almost all the way to completion? ( N_{2}(g)+O_{2}(g) rightleftharpoons 2 N O(g) ; K_{c}=2.7 times ) ( mathbf{1 0}^{-18} ) ( mathbf{2} boldsymbol{N} boldsymbol{O}(boldsymbol{g})+boldsymbol{O}_{2}(boldsymbol{g}) rightleftharpoons mathbf{2} boldsymbol{N} boldsymbol{O}_{2}(boldsymbol{g}) ) |
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| 482 | At ( 1200^{circ} C, ) the following equilibrium is established between chlorine atoms & molecule. ( boldsymbol{C l}_{2}(boldsymbol{g}) rightleftharpoons mathbf{2} boldsymbol{C l}(boldsymbol{g}) ) The composition of the equilibrium mixture may be determined by measuring the rate of effusion of the mixture through a pinhole. It is found that at ( 1200^{circ} ) Cand 1 atm pressure the mixture effuses 1.16 times as fast as krypton effuses under the same condition. Calculate the equilibrium constant ( boldsymbol{K}_{c} ) A ( .3 .1 times 10^{5} ) В . ( 6.3 times 10^{4} ) c. ( 12.6 times 10^{5} ) D. None of these |
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| 483 | If one-third of ( H I ) decomposes at a particular temperature, ( boldsymbol{K}_{c} ) for the equilibrium is: ( boldsymbol{H} boldsymbol{I} rightleftharpoons boldsymbol{H}_{2}+boldsymbol{I}_{2} ) A . ( 1 / 16 ) B. ( 1 / 4 ) ( c cdot 1 / 6 ) D. ( 1 / 2 ) |
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| 484 | The standard Gibbs energy change at ( 300 K ) for the reaction ( 2 A rightleftharpoons B+C ) is ( 2494.2 J . ) At a given time, the composition of the reaction mixture is ( [boldsymbol{A}]=frac{1}{2},[boldsymbol{B}]=mathbf{2},[boldsymbol{C}]=frac{1}{2} . ) The reaction proceeds in the: ( [boldsymbol{R}=mathbf{8 . 3 1 4} boldsymbol{J} / boldsymbol{K} / boldsymbol{m o l}, boldsymbol{e}=mathbf{2 . 7 1 8}] ) A. Reverse direction because ( QK_{c} ) c. Reverse direction because ( Q>K_{c} ) D. Forward direction because ( Q<K_{c} ) |
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| 485 | The thermal dissociation equilibrium of ( boldsymbol{C a C O}_{3}(s) ) is studied under different conditions. [ begin{array}{r} boldsymbol{C a C O}_{3}(boldsymbol{s}) rightleftharpoons boldsymbol{C a O}(boldsymbol{s})+ \ boldsymbol{C O}_{2}(boldsymbol{g}) end{array} ] For this equilibrium, the correct statement(s) is (are): A. ( Delta H ) is dependent on ( T ) B. ( K ) is independent of the initial amount of ( C a C O_{3} ) C. ( K ) is dependent on the pressure of ( C O_{2} ) at a given ( T ) D. ( Delta H ) is independent of the catalyst, if any |
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| 486 | In the graph ( (1), A, B ) and ( C ) respectively are: ( A cdot S O_{3}, S O_{2} ) and ( O_{2} ) B. ( S O_{3}, O_{2} ) and ( S O_{2} ) ( c cdot S O_{2}, O_{2} ) and ( S O_{3} ) D. ( O_{2}, S O_{2} ) and ( S O_{3} ) |
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| 487 | The molar solubility of ( mathrm{PbCl}_{2} ) in ( 0.20 mathrm{M} ) ( mathrm{Pb}left(mathrm{NO}_{3}right)_{2} ) solution is: ( left(boldsymbol{K}_{boldsymbol{s} p} text { for } boldsymbol{P b C l}_{2}=mathbf{1 . 6} times mathbf{1 0}^{-mathbf{5}}right) ) A . ( 1.7 times 10^{-4} M ) В. ( 9.2 times 10^{-3} M ) c. ( 1.7 times 10^{-5} M ) D. ( 4.6 times 10^{-3} M ) E . ( 8.5 times 10^{-5} M ) |
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| 488 | One litre of water contains ( 1.0 times 10^{-7} ) moles of ( boldsymbol{H}^{+} ) ions. The degree of ionization of water is: A ( cdot 1.8 times 10^{-9} % ) В. ( 0.8 times 10^{-9} % ) c. ( 3.6 times 10^{-9} % ) D. ( 3.6 times 10^{-7} % ) |
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| 489 | An acid ( H A ) ionises as ( boldsymbol{H} boldsymbol{A} rightleftharpoons boldsymbol{H}^{+}+boldsymbol{A}^{-} ) The pH of ( 1.0 mathrm{M} ) solution is ( 5 . ) Its dissociation constant would be: |
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| 490 | Assertion According to Bronsted Lowry theory ( B F_{3} ) is an acid. Reason ( B F_{3} ) is an electron deficient compound. 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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| 491 | Q73. The concentration of sulphide ion in 0.1 M HCl solution saturated with hydrogen sulphide is 1.0 10-19 M. IF 10 mL of this solution is added to 5 mL of 0.04 M solution of FeSO,, MnCI, ZnCl, and Cdci, in which of these solutions precipitation will take place? Given K for Fes = 6.3 x 10-18, MnS = 2.5 x 10-13, ZnS = 1.6 x 10-24 and CAS = 8.0 x 10-27 1 |
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| 492 | Which of the following is an example of weak electrolyte? A ( cdot C H_{3} C O O H rightarrow C H_{3} C O O^{-}+H^{+} ) в. ( K O H rightarrow K^{+}+O H^{-} ) ( mathrm{c} cdot A g N O_{3} rightarrow A g^{+}+N O_{3} ) D. all of the above |
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| 493 | Which of the following is not a Lewis acid? A. Aluminum chloride B. Ammonia c. sulphur trioxide D. cupric ion |
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| 494 | The equilibrium constants for the reactions are: [ begin{array}{l} boldsymbol{H}_{3} boldsymbol{P} boldsymbol{O}_{4} stackrel{boldsymbol{K}_{1}}{rightleftharpoons} boldsymbol{H}^{+}+boldsymbol{H}_{2} boldsymbol{P} boldsymbol{O}_{4}^{-} ; boldsymbol{K}_{mathbf{1}} \ boldsymbol{H}_{2} boldsymbol{P} boldsymbol{O}_{4}^{-} frac{boldsymbol{K}_{2}}{rightleftharpoons} boldsymbol{H}^{+}+boldsymbol{H} boldsymbol{P} boldsymbol{O}_{4}^{2-} ; boldsymbol{K}_{2} \ boldsymbol{H} boldsymbol{P} boldsymbol{O}_{4}^{2-} stackrel{boldsymbol{K}_{3}}{rightleftharpoons} boldsymbol{H}^{+}+boldsymbol{P} boldsymbol{O}_{4}^{3-} ; boldsymbol{K}_{3} end{array} ] The equilibrium constant for [ boldsymbol{H}_{3} boldsymbol{P} boldsymbol{O}_{4} rightleftharpoons mathbf{3} boldsymbol{H}^{+}+boldsymbol{P} boldsymbol{O}_{4}^{3-} text { will be: } ] ( A ) [ frac{K_{1}}{K_{2} times K_{3}} ] В. ( K_{1} times K_{2} times K_{3} ) ( c ) [ frac{K_{2}}{K_{1} times K_{3}} ] D. ( K_{1}+K_{2}+K_{3} ) |
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| 495 | ( boldsymbol{K}_{boldsymbol{a}_{1}}, boldsymbol{K}_{boldsymbol{a}_{2}}, boldsymbol{K}_{boldsymbol{a}_{3}} ) values for ( boldsymbol{H}_{3} boldsymbol{P} boldsymbol{O}_{4} ) are ( 10^{-3}, 10^{-8}, 10^{-12} ) respectively. If ( boldsymbol{K}_{boldsymbol{w}}left(boldsymbol{H}_{2} boldsymbol{O}right)=mathbf{1 0}^{-14}, ) then (i) What is dissociation constant of ( H P O_{4}^{2-} ? ) (ii) What is ( K_{b} ) of ( H P O_{4}^{2-} ) (iii) What is ( K_{b} ) of ( H_{2} P O_{4}^{2-} ) ? (iv) What order of ( boldsymbol{K}_{boldsymbol{b}} ) of ( boldsymbol{P O}_{4}^{3-}left(boldsymbol{K}_{b_{3}}right), boldsymbol{H} boldsymbol{P} boldsymbol{O}_{4}^{2-}left(boldsymbol{K}_{b_{2}}right) ) and ( boldsymbol{H}_{2} boldsymbol{P} boldsymbol{O}_{4}^{-}left(boldsymbol{K}_{b_{1}}right) ? ) |
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| 496 | ( 9.2 mathrm{gm} ) of ( N_{2} O_{4}(g) ) is taken in a closed one-litre vessel and heated till the following equilibrium is reached ( N_{2} O_{4}(g) rightleftharpoons 2 N O_{2}(g) ) At equilibrium ( 50 % ) of ( N_{2} O_{4}(g) ) is dissociated. What is the equilibrium constant? [in mole lit ( ^{-1} ) ] [M.wt. of ( N_{2} O_{4} ) is 92] A. ( 0 . ) в. 0.2 ( c cdot 0.4 ) D. 2 |
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| 497 | Sodium bicarbonate is also known as: A. washing soda B. baking soda c. glauber’s salt D. lime soda |
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| 498 | Ammonia is basic in nature hence it turns: A . red litmus to blue B. blue litmus to red c. white litmus to red D. white litmus to blue |
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| 499 | Consider the following statements (a) The ( p H ) of a mixture containing ( 400 m L ) of ( 0.1 M H_{2} S O_{4} ) and ( 400 m L ) of ( 0.1 M N a O H ) will be approximately 1.3 (b) lonic product of water is temperature dependent (c) A monobasic acid with ( boldsymbol{K}_{boldsymbol{a}}=mathbf{1 0}^{-5} ) has a ( p H=5 . ) The degree of dissociation of this acid is ( 50 % ) (d) The Le Chatelier’s principle is not applicable to common-ion effect. The correct statement are : A ( cdot(a),(b) ) and ( (d) ) B. (a), (b) and (c) c. (a) and (b) D. (b) and (c) |
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| 500 | ( 2 S O_{2}(g)+O_{2}(g) leftrightharpoons 2 S O_{3}(g) ) Given that the equilirbium constant for the reaction above has a value of 278 at a particular temperature, what is the value of equilibrium constant for the following reaction at same temperature? ( boldsymbol{S O}_{3}(boldsymbol{g}) rightleftharpoons boldsymbol{S} boldsymbol{O}_{2}(boldsymbol{g})+frac{1}{2} boldsymbol{O}_{2}(boldsymbol{g}) ) A ( cdot 1.3 times 10^{-5} ) B . ( 1.8 times 10^{-3} ) c. ( 3.6 times 10^{-3} ) D. ( 6 times 10^{-2} ) |
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| 501 | The gas released when baking soda is mixed with vinegar, is: A. ( C O ) в. ( C O_{2} ) c. ( C H_{4} ) D. ( O_{2} ) |
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| 502 | If the salts ( M_{2} X, Q Y_{2} ) and ( P Z_{3} ) have the same solubilities,their ( boldsymbol{K}_{s p} ) values are related as ( -(S<1) ) A ( cdot K_{s p}left(M_{2} Xright)=K_{s p}left(Q Y_{2}right)K_{s p}left(Q Y_{2}right)=K_{s p}left(P Z_{3}right) ) C. ( K_{s p}left(M_{2} Xright)=K_{s p}left(Q Y_{2}right)>K_{s p}left(P Z_{3}right) ) D. ( K_{s p}left(M_{2} Xright)>K_{s p}left(Q Y_{2}right)>K_{s p}left(P Z_{3}right. ) |
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| 503 | The equilibrium constant ( boldsymbol{K}_{boldsymbol{p}} ) for the following reaction at ( 191^{circ} mathrm{C} ) is 1.24 What is ( boldsymbol{K}_{c} ) ? ( B(s)+frac{3}{2} F_{2}(g) rightleftharpoons B F_{3}(g) ) A . 6.7 B. 0.61 c. 8.30 D. 7.6 |
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| 504 | Fill in the blanks: ¡. ( quad ) taste is a characteristic property of all acids in aqueous solution. ii. Acids react with some metals to produce iii. Because aqueous acid solutions conduct electricity, they are identified as iv. Acids react with bases to produce a and water. v. Acids turn different colours. |
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| 505 | The ( p H ) of the solution cantaining ( mathbf{0 . 1} boldsymbol{M} boldsymbol{H} boldsymbol{N} boldsymbol{O}_{3} & mathbf{0 . 1} boldsymbol{M} boldsymbol{H} boldsymbol{C O O H} mathbf{~ i s : ~} ) ( left[boldsymbol{K}_{s} text { of } boldsymbol{H} boldsymbol{C O O H} text { is } mathbf{1 . 8} times mathbf{1 0}^{-mathbf{1 4}}right] ) A . ( 0 . ) B. ( c cdot 2 ) D. 0.2 |
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| 506 | Which of the following has a very high ( boldsymbol{K}_{boldsymbol{a}} ? ) A. Bronsted acid B. Bronsted base c. Strong acid D. weak base |
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| 507 | For the reaction ( boldsymbol{A}+mathbf{2} boldsymbol{B} rightleftharpoons mathbf{2} boldsymbol{C} ) at equilibrium ( [boldsymbol{C}]=mathbf{1 . 4} boldsymbol{M} cdot[boldsymbol{A}]_{o}= ) ( mathbf{1} boldsymbol{M},[boldsymbol{B}]_{o}=mathbf{2} boldsymbol{M},[boldsymbol{C}]_{o}=mathbf{3} M . ) The value of ( K_{c} ) is: (Given: volume =1 litre, [ ] ( _{o} ) is initial concentration) A .0 .084 B. 8.4 ( c cdot 48 ) D. None of these. |
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| 508 | If the pH of pure water is ( 7, ) then the hydrogen ion concentration, ( left[boldsymbol{H}^{+}right] ) in mol ( mathbf{L}^{-1} ) will be: A ( cdot 10^{-7} ) 7 B. 0 ( c cdot 7 ) D. ( 10^{+7} ) |
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| 509 | Q42. The pH of a sample of vinegar is 3.76. Calculate the concentration of hydrogen ion in it. | 11 |
| 510 | lonisation constant of ( C H_{3} C O O H ) is ( 1.7 times 10^{-5} ) and concentration of ( H^{+} ) ions is ( 3.4 times 10^{-4} . ) Then find out initia concentration of ( boldsymbol{C H}_{3} ) COOH molecules: A ( .3 .4 times 10^{-4} ) B . ( 3.4 times 10^{-3} ) c. ( 6.8 times 10^{-4} ) D. ( 6.8 times 10^{-3} ) |
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| 511 | Q4. (a) In the reaction A + B +C+D, what will happen to the equilibrium if concentration of A is increased? (b) The equilibrium constant for a reaction is 2 x 10-23 at 25°C and 2 x 10-2 at 50°C. Is the reaction endothermic or exothermic? (c) Mention at least three ways by which the concentration of so, can be increased in the following reaction in a state of equilibrium. . |
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| 512 | A 0.02 M solution of pyridinium hydrochloride has ( p H=3.44 . ) Calculate the ionization constant of pyridine. |
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| 513 | m illoride ced in terms of bult hent(s) about buffe 13. Effectiveness of a buffer is measured in capacity (). Select correct statement capacity d[Base] (a) B = | d[pH] d[Base] (6) B= -d[AH] (c) B is maximum for an acidic buffer at pH = pk (d) If pH = pK, +1, then it is most effective range for a buffer |
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| 514 | Which of the following salts has the greatest molar solubility in pure water? A ( cdot C a C O_{3} ; K_{s p}=8.7 times 10^{-9} ) B. ( C u S ; K_{s p}=8.5 times 10^{-45} ) C ( cdot A g_{2} C O_{3} ; K_{s p}=6.2 times 10^{-12} ) D. ( P bleft(I O_{3}right)_{2} ; K_{s p}=2.6 times 10^{-13} ) |
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| 515 | Will ( C a F_{2} ) be precipitated? A. Yes B. No c. Data insufficient D. None of these |
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| 516 | The correct order of pH is A. Lemon juice < water water> Milk of Magnesia C. Water > lemon juice > milk of Magnesia D. Milk of Magnesia > lemon juice > water |
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| 517 | Calculate the pH of a ( 0.033 M ) ammonia solution, if ( 0.033 M N H_{4} C l ) is introduced in this solution at the same temperature. ( left(k_{b} text { for } N H_{3}=right. ) ( left.1.77 times 10^{-5}right) ) |
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| 518 | ( 20 m L ) of ( 0.1 N ) acetic acid is mixed with ( 10 m L ) of ( 0.1 N ) solution of ( N a O H ) The ( p H ) of the resulting solution is : ( left[text { Given }: p K_{a} text { of acetic acid is } 4.74right] ) A . 3.74 в. 4.74 ( c .5 .74 ) D. 6.74 |
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| 519 | For the reaction, ( boldsymbol{A B}(boldsymbol{g}) rightleftharpoons boldsymbol{A}(boldsymbol{g})+boldsymbol{B}(boldsymbol{g}), boldsymbol{A B} ) is ( boldsymbol{3} boldsymbol{3} % ) dissociated at a total pressure of ( boldsymbol{P} ) Therefore, ( P ) is related to ( K_{p} ) by one of the following option: A ( cdot P=K_{p} ) В. ( P=3 K_{p} ) ( mathbf{c} cdot P=4 K_{p} ) D. ( P=8 K_{p} ) |
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| 520 | The process in which metal surface is made inactive is called: A. passivation B. galvanizing c. corrosion D. pickling |
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| 521 | A solution contains ( 0.1 M C l^{-} ) and ( mathbf{0 . 0 0 1} boldsymbol{M} boldsymbol{C r} boldsymbol{O}_{4}^{2-} . ) If solid ( boldsymbol{A} boldsymbol{g} boldsymbol{N} boldsymbol{O}_{3} ) is gradually added to this solution, which will precipitate first, ( A g C l ) or ( A g_{2} C r O_{4} ) ? Assume that the addition causes no change in volume. Given ( boldsymbol{K}_{s p} boldsymbol{A} boldsymbol{g} boldsymbol{C l}=mathbf{1 . 7} times mathbf{1 0}^{-mathbf{1 0}} boldsymbol{M}^{mathbf{2}} ) ( boldsymbol{K}_{s p} boldsymbol{A} boldsymbol{g}_{2} boldsymbol{C r} boldsymbol{O}_{4}=mathbf{1 . 7 9} times mathbf{1 0}^{-mathbf{1 2}} boldsymbol{M}^{mathbf{3}} ) What percent of ( C l^{-} ) remains in the solution when ( C r O_{4}^{2-} ) starts precipitating? |
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| 522 | In the reaction ( boldsymbol{F e}(boldsymbol{O} boldsymbol{H})_{3}, boldsymbol{F} boldsymbol{e}_{boldsymbol{a} boldsymbol{q}}^{3+}+ ) ( 3 O H_{a q}^{-}, ) if the concentration of ( O H^{-} ) is decreased by ( frac{1}{4} ) times then the equilibrium concentration of ( boldsymbol{F} boldsymbol{e}^{mathbf{3}+} ) increased by how many times?? |
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| 523 | 0.23 The aqueous solution of sugar does not conduct electricity. However when sodium chloride is added to water, it conducts electricity. How will you explain this statement on the basis of ionisation and how is it affected by concentration of sodium chloride? |
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| 524 | The equilibrium constant for the following reaction is ( 64 . H_{2} O(l)+ ) ( boldsymbol{C O}(boldsymbol{g}) leftrightharpoons boldsymbol{H}_{2}(boldsymbol{g})+boldsymbol{C} boldsymbol{O}_{2}(boldsymbol{g}) . ) If the rate constant for the forward reaction is 160 the rate constant for the backward reaction is: A . 0.4 B . 2. c. 6.2 D. 10.24 |
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| 525 | Which of the following is not a conjugate acid-base pair? ( mathbf{A} cdot H P O_{3}^{2-}, P O_{3}^{3-} ) B . ( H_{2} P O_{4}^{-}, H P O_{4}^{2-} ) c. ( H_{2} P O_{4}^{-}, H_{3} P O_{4} ) D. ( H_{2} P O_{4}^{-}, P O_{3}^{3-} ) |
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| 526 | If two gases ( A B_{2} ) and ( B_{2} C ) are mixed the following equilibria are readily established ( boldsymbol{A B}_{2}(boldsymbol{g})+boldsymbol{B}_{2} boldsymbol{C}(boldsymbol{g}) rightarrow boldsymbol{A} boldsymbol{B}_{3}(boldsymbol{g})+boldsymbol{B C}(boldsymbol{g}) ) ( boldsymbol{B C}(boldsymbol{g})+boldsymbol{B}_{2} boldsymbol{C}(boldsymbol{g}) rightarrow boldsymbol{B}_{3} boldsymbol{C}_{2}(boldsymbol{g}) ) If the reaction is started only with ( A B_{2} ) with ( B_{2} C, ) then which of the following is necessarily true at equilibrium: This question has multiple correct options ( mathbf{A} cdotleft[A B_{3}right]_{e q}=[B C]_{e q} ) ( mathbf{B} cdotleft[A B_{2}right]_{e q}=left[B_{2} Cright]_{e q} ) ( mathbf{c} cdotleft[A B_{3}right]_{e q}>left[B_{3} C_{2}right]_{e q} ) ( mathbf{D} cdotleft[A B_{3}right]_{e q}>[B C]_{e q} ) |
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| 527 | ( H_{3} P O_{4} ) is a tribasic acid with ( boldsymbol{p} boldsymbol{K}_{a_{1}}, boldsymbol{p} boldsymbol{K}_{a_{2}} ) and ( boldsymbol{p} boldsymbol{K}_{a_{3}} boldsymbol{2} .12, boldsymbol{7} .21 ) and ( 12.32, ) respectively. It is used in fertiliser productions and its various salts are used in food, detergent, toothpaste, and in metal treatment. Small quantities of ( boldsymbol{H}_{3} boldsymbol{P} boldsymbol{O}_{4} ) are used in imparting the sour or tart taste to soft drinkes, such as Coca Cola, and beers in which ( H_{3} P O_{4} ) is present ( 0.05 % ) by weight (density ( left.=1.0 g m L^{-1}right) ) ( mathbf{1 0}^{-3} boldsymbol{M} boldsymbol{H}_{3} boldsymbol{P} boldsymbol{O}_{4}(boldsymbol{p} boldsymbol{H}=mathbf{7}) ) is used in fertilisers as an aqueous soil digesting. Plants can absorb zinc in water soluble form only. Zinc phosphate is the source of zinc and ( P O_{2}^{3-} ) ions in the soil. ( K_{s p} ) of zonic phosphate ( =9.1 times 10^{-33}left[Z n^{2+}right] ) ion in the soil is: A ( .2 .9 times 10^{-11} mathrm{M} ) В. ( 4.0 times 10^{-10} M ) c. ( 3.0 times 10^{-6} M ) D. ( 9.1 times 10^{-5} M ) |
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| 528 | A buffer solution of ( p H=9 ) can be prepared by mixing: A. ( C H_{3} C O O N a ) and ( C H_{3} C O O O H ) B. ( N a C l ) and ( N a O H ) c. ( N H_{4} C l ) and ( N H_{4} O H ) D. ( K H_{2} P O_{4} ) and ( K_{2} H P O_{4} ) |
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| 529 | The pH of a solution of ( B(O H)_{2} ) is 10.6 Calculate the solubility and solubility product of hydroxide. |
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| 530 | For the equilibrium reaction ( boldsymbol{C a} boldsymbol{C O}_{3}(boldsymbol{s}) rightleftharpoons boldsymbol{C a O}(boldsymbol{s})+boldsymbol{C O}_{2}(boldsymbol{g}) . ) The addition of more ( C a C O_{3}(s) ) causes? A. The decrease in the concentration of ( C O_{2}(g) ) B. The increase in the concentration of ( C O_{2}(g) ) C. No change in the concentration of ( C O_{2}(g) ) D. Increase in the concentration of ( C a O(s) ) |
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| 531 | ( boldsymbol{C O}_{2}+boldsymbol{N} boldsymbol{H}_{3}+boldsymbol{H}_{2} boldsymbol{O} rightarrow boldsymbol{X} ) ( boldsymbol{X}+boldsymbol{N} boldsymbol{a} boldsymbol{C l} rightarrow boldsymbol{Y}+boldsymbol{N} boldsymbol{H}_{4} boldsymbol{C l} ) ‘Y’ in the above reaction is: ( mathbf{A} cdot N a_{2} C O_{3} ) в. ( left(N H_{4}right)_{2} C O_{3} ) c. ( N H_{4} H C O_{3} ) D. ( N a H C O_{3} ) |
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| 532 | Assertion At ( 25^{circ} C ), the pH of ( 10^{-8} M ) HClis 8 Reason pH of acidic solution is always below 7 ( operatorname{at} 25^{circ} C ) 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 the Reason is correct |
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| 533 | The equilibrium state can be attained from both sides of the chemical reaction. A. True B. False |
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| 534 | In an experiment starting with 1 mole of ethyl of alcohol, 1 mole of acetic acid and 1 mole of water at ( 100^{circ} mathrm{C} ), the equilibrium mixture on analysis shows that ( 54.3 % ) of the acid is esterified. Calculate the equilibrium constant of this reaction. |
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| 535 | In the reaction, ( boldsymbol{H}_{2}(boldsymbol{g})+boldsymbol{I}_{2}(boldsymbol{g}) rightleftharpoons ) ( 2 H I(g) ) the concentration of ( H_{2}, I_{2} ) and ( H I ) at equilibrium are 8.0,3.0 and 28 moles per litre respectively. What will be the equilibrium constant? ( A cdot 30.61 ) B. 32.66 c. 29.40 D. 20.90 |
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| 536 | The percentage hydrolysis in ( 0.003 M ) aqueous solution of ( N a O C Nleft(K_{a} ) for right. ( left.boldsymbol{H} boldsymbol{O} boldsymbol{C} boldsymbol{N} text { is } boldsymbol{3} boldsymbol{3} boldsymbol{3} times mathbf{1 0}^{-4} boldsymbol{M}right) ) is: A . ( 0.1 % ) B. ( 0.01 % ) ( c .0 .5 % ) D. ( 0.8 % ) |
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| 537 | Bleaching powder gives smell of chlorine because it: A . is unstable B. gives chlorine on exposure to atmosphere c. is a mixture of chlorine and slaked lime D. contains excess of chlorine |
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| 538 | Q8. Write conjugate acid and conjugate base of H,O? Ana Caninote :: In |
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| 539 | Q1. What is meant by equilibrium? 11 |
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| 540 | Calculate the ratio of pH of a solution containing 1 mol. of ( C H_{3} C O O N a+ ) 1 mol of HCl per litre and of other solution containing 1 mol of ( boldsymbol{C H}_{3} boldsymbol{C O O N a +} mathbf{1 m o l} ) of ( boldsymbol{C H}_{3} boldsymbol{C O O H} ) per litre. |
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| 541 | What would be the pH of an aqueous solution of ( 1 N ) tribasic acid? A. 3 B. ( c cdot 0 ) D. 1.5 |
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| 542 | Consider the two gaseous equilibria involving ( S O_{2} ) and the corresponding equilibrium constants at ( 298 mathrm{K} ) ( boldsymbol{S O}_{2}(boldsymbol{g})+frac{1}{2} boldsymbol{O}_{2}(boldsymbol{g}) Leftrightarrow boldsymbol{S} boldsymbol{O}_{3}(boldsymbol{g}) ; boldsymbol{K}_{1} ) ( 2 S O_{3}(g) Leftrightarrow 2 S O_{2}(g)+O_{2}(g) ; K_{2} ) The values of the equilibrium constants are related by: A ( cdot K_{1}=K_{2} ) в. ( K_{2}=K_{1}^{2} ) c. ( _{K_{2}=frac{1}{K_{1}^{2}}} ) D. ( _{K_{2}}=frac{1}{K_{1}} ) |
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| 543 | A reaction system in equilibrium according to reaction ( 2 S O_{2}(g)+ ) ( O_{2}(g) rightarrow 2 S O_{3}(g)(k=5) ) in one litre vessel at a given temperature was found to be 0.12 mole each of ( S O_{2} ) and ( boldsymbol{S} boldsymbol{O}_{3} ) and 5 mole of of ( boldsymbol{O}_{2} ) must be added to this vessel to order that at equilibrium ( 20 % ) of ( S O_{2} ) is oxidized to ( S O_{3} . ) Find out the mass of oxygen formed? A. ( 0.41245 mathrm{g} ) B. ( 11.6 g ) c. ( 1.6 g ) D. None of these. |
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| 544 | ( N_{2}(g)+3 H_{2}(g) rightleftharpoons 2 N H_{3}(g)+ ) heat For the reaction above, what is the effect on the equilibrium position when the pressure is decreased? A. Increased production of products B. Increased production of reactants c. Fluctuations in the amounts of reactants and products D. No impact on the equilibrium E. Cannot be determined |
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| 545 | ( A l F_{3} ) is soluble in ( H F ) only in presence of ( K F ). It is due to the formation of : A. ( A l H_{3} ) B . ( Kleft[A l F_{3} Hright] ) c. ( K_{3}left[A l F_{3} H_{3}right] ) D. ( K_{3}left[A l F_{6}right] ) |
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| 546 | If the ( p H ) of a solution is ( 8, ) its ( left[H^{+}right] ) is: A ( cdot log 10^{-8} ) B . ( 10^{6} ) ( c cdot 10^{-8} ) D. 8 |
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| 547 | For a gaseous phase reaction ( boldsymbol{A}+ ) ( mathbf{2} boldsymbol{B} rightleftharpoons boldsymbol{A} boldsymbol{B}_{2}, boldsymbol{K}_{C}=mathbf{0 . 3 4 7 5} boldsymbol{L}^{2} boldsymbol{m o l} boldsymbol{e}^{-mathbf{2}} mathbf{a} ) ( 200^{circ} mathrm{C} ). When 2 moles of ( B ) are mixed with one mole of ( A ), what total pressure is required to convert ( 60 % ) of ( A ) in ( A B_{2} ) ? A ( . P=1.8 a t m ) B. ( P=63 ) atm c. ( P=181.5 ) atm ( D . P=34 a t m ) |
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| 548 | For a reversible chemical reaction where the forward process is exothermic, which of the following statements is correct? A. The backward reaction has higher activation energy than the forward reaction B. The backward and the forward processes have the same activation energy C. The backward reaction has lower activation energy D. No activation energy is required at all since energy is liberated in the process |
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| 549 | If equal concentrations of products and reactants are mixed, then which of the following reactions will proceed to the right and which will proceed to the left? ( (A) H_{2} S O_{4}(a q)+N H_{3}(a q) rightleftharpoons ) ( N H_{4}^{+}(a q)+H S O_{4}^{-}(a q) ) (B) ( boldsymbol{H} boldsymbol{C O}_{3}^{-}(boldsymbol{a q})+boldsymbol{S O}_{4}^{2-}(boldsymbol{a q}) rightleftharpoons ) ( boldsymbol{H} boldsymbol{S} boldsymbol{O}_{4}^{-}(boldsymbol{a} boldsymbol{q})+boldsymbol{C} boldsymbol{O}_{3}^{2-}(boldsymbol{a} boldsymbol{q}) ) |
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| 550 | Given ( 2 N O_{(g)}+O_{2(g)} rightarrow 2 N O_{2(g)} ; ) rate ( =mathbf{k}[boldsymbol{N} boldsymbol{O}]^{2}left[boldsymbol{O}_{2}right]^{1} . ) By how many times does the rate of the reaction change when the volume of the reaction vessel is reduced to ( 1 / 3 ) rd of its original volume? Will there be any change in the order of the reaction? |
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| 551 | LUL CICLO LO TOLLIC PIULUICIDE Q19. A sample of pure PCI was introduced into an evacuated vessel at 473 K. After equilibrium was reached, the concentration of PCI, was found to be 0.5 x 10-1 mol L-1. If K is 8.3 x 10″, what are the concentrations of PCI, and Cl, at equilibrium? |
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| 552 | f pressure increases then its effect on given equilibrium ( boldsymbol{C}(s)+boldsymbol{H}_{2} boldsymbol{O}(boldsymbol{g}) rightleftharpoons boldsymbol{C} boldsymbol{O}(boldsymbol{g})+boldsymbol{H}_{2}(boldsymbol{g}) ) It is shifted in: A. forward direction B. backward direction c. no effect D. none of these |
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| 553 | A buffer solution is made up of acetic acid ( left[boldsymbol{p} boldsymbol{K}_{boldsymbol{a}}=mathbf{5}right] ) having conc. ( =mathbf{1 . 5} boldsymbol{M} ) and sodium acetate having conc. ( = ) ( 0.15 M . ) What is the number of ( O H^{-} ) ions present in 1 litre solution? В. ( 10^{-4} M ) ( mathrm{c} cdot 10^{-3} M ) D. ( 10^{-6} M ) |
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| 554 | Addition of water to ( boldsymbol{X} ) solution will not change concentration of ( boldsymbol{H}_{3} boldsymbol{O}^{+} . boldsymbol{X} ) is: A. chemical pH indicator B. acid/base buffer c. anhydrous solution D. hypotonic solution E. supersaturated solution |
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| 555 | Assertion: Addition of ( N H_{4} O H ) to an aqueous solution of ( B a C l_{2} ) in the presence of excess ( N H_{4} C l ) precipitates ( boldsymbol{B} boldsymbol{a}(boldsymbol{O} boldsymbol{H})_{2} ) Reason: ( boldsymbol{B a}(boldsymbol{O H})_{2} ) is soluble in water. |
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| 556 | Which of the following statements relationships is correct? ( mathbf{A} cdot K_{P}=K_{C} ) for ( N_{2}+O_{2} rightleftharpoons 2 N O ) B. ( Q_{P}>K_{C} ) corresponds to backward reaction C ( . K_{P} ) is not defined for ( C H_{3} C O O C H_{3}+H_{2} O rightleftharpoons ) ( C H_{3} C O O H+C H_{3} O H ) D. ( K_{s p}=4 s^{-1} ) (for salt like ( C a F_{2} ) ) is applicable even in an ( H F ) solution |
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| 557 | Assertion ( boldsymbol{I}_{2}+boldsymbol{I}^{-} longrightarrow boldsymbol{I}_{boldsymbol{3}} ) In above reaction, ( boldsymbol{I}_{2} ) is Lewis base. Reason Electron pair acceptor is Lewis base. |
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| 558 | On increasing temperature, the equilibrium constant of exothermic and endothermic reactions and ( ——- ) respectively: A. increases and decreases B. decreases and increases c. increases and increases D. decreases and decreases |
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| 559 | Q59. The ionization constant of propanoic acid is 1.32 x 10-6. Calculate the degree of ionization of the acid in its 0.05 M solution and also its pH. What will be its degree of ionization if the solution is 0.01 M HCl also? Be the formula |
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| 560 | A weak mono acidic base is ( 5 % ) ionized in ( 0.01 M ) solution. The hydroxide ion concentration in the solution is: A. ( 5 times 10^{-2} ) В. ( 5 times 10^{-4} ) c. ( 5 times 10^{-10} ) D. ( 2 times 10^{-11} ) |
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| 561 | For a given exothermic reaction ( boldsymbol{K}_{boldsymbol{p}} ) and ( K_{p}^{prime} ) are the equilibrium constants at temperature ( T_{1} ) and ( T_{2} ) respectively. Assuming that heat of reaction is constant in temperature range between 183. ( T_{1} ) and ( T_{2} ) it is readily observed that: ( mathbf{A} cdot K_{p}=K_{p}^{prime} ) B . ( K_{p}=1 / K_{p}^{prime} ) ( mathbf{c} cdot K_{p}>K_{p}^{prime} ) D. ( K_{p}<K_{p}^{prime} ) |
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| 562 | Which of the following solution cannot act as a buffer? A. ( N a H_{2} P O_{4}+H_{3} P O_{4} ) в. ( C H_{3} ) СООН ( +C H_{3} ) СОО Na c. ( H C l+N H_{4} C l ) D. ( H_{3} P O_{4}+N a_{2} H P O_{4} ) |
11 |
| 563 | Which of the following is an organic acid? A. Sulphurous acid B. Nitric acid c. Hydrochloric acid D. Formic acid |
11 |
| 564 | For the reaction [ boldsymbol{P C l}_{3(g)}+boldsymbol{C l}_{2(g)} rightleftharpoons boldsymbol{P} boldsymbol{C l}_{5(g)} ] the value of ( boldsymbol{K}_{c} ) at ( 250^{circ} mathrm{C} ) is ( 26 . ) The value of ( K_{p} ) a this temperature will be A . 0.61 B. 0.57 c. 0.83 D. 0.46 |
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| 565 | When sulphur in the form of ( S_{8} ) is heated at ( 900 K ) and constant volume, the initial pressure of 1 atm increases by ( 27 % ) at equilibrium. This is because of conversion of some ( S_{8} ) to ( S_{2} ). Find the value of the equilibrium constant for this reaction. |
11 |
| 566 | Le Chatelier’s principle is applicable to what equilibrium. A. Physical equilibrium. B. Chemical equilibrium. c. Both equilibrium. D. None of these |
11 |
| 567 | Match List-I with List-II. | 11 |
| 568 | If the pressure of ( N_{2} / H_{2} ) mixture in a closed apparatus is 100 atm and ( 20 % ) of the mixture reacts,then the pressure at same temperature would be: A. 100 B. 90 ( c cdot 85 ) ( D cdot 80 ) |
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| 569 | Ethylene dibromide ( left(C_{2} H_{4} B r_{2}right) ) and 1, 2 – dibromopropane ( left(C_{3} H_{6} B r_{2}right) ) forms a series of ideal solution over the whole range of composition. At ( 85^{circ} C ) the vapour pressure of these pure liquids are are ( 183 mathrm{mmHg} ) and 127 mm ( H g ) respectively. 10gm of ethylene dibromide is dissolved in ( 80 g m ) of ( 1,2- ) dibromo – propane. Calculate the partial pressures of each components and the total pressure of the solution at ( 85^{circ} C ) Calculate the composition of vapour in equilibrium with the above and express as mole fraction of ethylene dibromide. |
11 |
| 570 | ( boldsymbol{C a} boldsymbol{C O}_{3}(boldsymbol{s}) rightleftharpoons boldsymbol{C a O}(boldsymbol{s})+boldsymbol{C O}_{2}(boldsymbol{g}), boldsymbol{K}= ) ( 10^{-9} ) at ( 300 K . ) The value of ( p_{c o_{2}} ) is ( 10^{-x} ) ( x ) is |
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| 571 | Assertion A substance that can either act as an acid or a base is called ampholyte. Reason Bisulphide ion ( left(boldsymbol{H} boldsymbol{S}^{-}right) ) and bicarbonate ion ( left(H C O_{3}^{-}right) ) are ampholytes. 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 |
11 |
| 572 | Which of the following is a weak acid? A. Acetic acid B. Formic acid c. Carbonic acid D. All of the above |
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| 573 | Which of the following is true about the reaction quotient? A. It relates the ratio of the concentrations of products to reactants once the reaction has reached chemical equilibrium. B. It is always equal to the equilibrium constant. C. It can never be equal to the equilibrium constant. D. It relates the concentrations of products to reactants at any point in time. E. None of these answers are correct |
11 |
| 574 | The correct relationship between free energy change in a reaction and the corresponding equilibrium constant ( boldsymbol{K} ) is: A ( .-Delta G^{circ}= ) RTin ( K ) в. ( Delta G= ) RT in ( K ) c. ( -Delta G=R T ) in ( K ) D. ( Delta G^{circ}=R T ) in ( K ) |
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| 575 | Starting with sodium chloride how would you proceed to prepare (i) sodium metal, (ii) sodium hydroxide, (iii) sodium peroxide, (iv) sodium carbonate? |
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| 576 | In a vessel containing ( S O_{3}, S O_{2} ) and ( O_{2} ) at equilibrium, some helium gas is introduced so that total pressure increases while temperature and volume remain the same. According to Le Chatelier’s principle the dissociation of ( boldsymbol{S O}_{3} ) A. increases B. decreases c. remains unaltered D. changes unpredictably |
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| 577 | ( mathrm{HX} ) is a weak acid ( left(boldsymbol{K}_{boldsymbol{a}}=mathbf{1 0}^{-mathbf{5}}right) . ) It forms a salt ( mathrm{NaX}(0.1 mathrm{M}) ) on reacting with caustic soda. The degree of hydrolysis of NaX is: A . 0.01 % B. 0.0001 % c. ( 0.1 % ) D. 0.5 % |
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| 578 | Compare the concentrations of each of the species ( N a^{+}, H^{+} ) and ( C N ) in the solution. A ( cdot N a^{+}>O H^{-}>C N^{-} ) В. ( C N^{-}>O H^{-}>N a^{+} ) c. ( N a^{+}>C N^{-}>O H^{-} ) D. ( O H^{-}>C N^{-}>N a^{+} ) |
11 |
| 579 | Q7. How does common ion affect the solubility of electrolyte? | 11 |
| 580 | Which of the following reactions proceed at low pressure ( mathbf{A} cdot N_{2}+3 H_{2} rightleftharpoons 2 N H_{3} ) ( mathbf{B} cdot H_{2}+I_{2} rightleftharpoons 2 H I ) ( mathbf{c} cdot P C l_{5} rightleftharpoons P C l_{3}+C l_{2} ) D. ( N_{2}+O_{2} rightleftharpoons 2 N O ) |
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| 581 | For a gaseous phase reaction, ( boldsymbol{A}+ ) ( mathbf{2} boldsymbol{B} rightleftharpoons boldsymbol{A} boldsymbol{B}_{2} boldsymbol{K}_{C}=mathbf{0 . 3 4 7 5} ) litre ( ^{2} boldsymbol{m o l}^{-2} ) at ( 200^{circ} mathrm{C} ). When 2 mole of ( B ) are mixed with one mole of ( A ). What total pressure is required to convert ( 60 % ) of ( A ) in ( A B_{2} ) ? |
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| 582 | Which of the following statement is correct regarding container B? Container ( (mathbf{A}) ) Container |
11 |
| 583 | What is the ( p H ) of dil.HCl solution with concentration ( 10^{-8} ) mol ( / L ) ? ( A cdot 7 ) B. 8 c. 6.98 D. 10 |
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| 584 | 0.6 mole of ( N H_{3} ) in a reaction vessel of ( 2 d m^{3} ) capacity was brought to equilibrium. The vessel was then found to contain 0.15 mole of ( H_{2} ) formed by the reaction ( mathbf{2} N boldsymbol{H}_{3}(boldsymbol{g}) rightleftharpoons boldsymbol{N}_{2}(boldsymbol{g})+mathbf{3} boldsymbol{H}_{2}(boldsymbol{g}) ) Which of the following statements is true? A. 0.15 mole of the original ( N H_{3} ) had dissociated at equilibrium B. 0.55 mole of ammonia is left in the vessel C . At equilibrium the vessel contained 0.45 mole of ( N_{2} ) D. The concentration of ( N H_{3} ) at equilibrium is 0.25 mole per ( d m^{3} ) |
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| 585 | ( boldsymbol{A}_{boldsymbol{3}(boldsymbol{g})} rightleftharpoons mathbf{3} boldsymbol{A}_{(boldsymbol{g})} ) In the above reaction, the initial moles of ( A_{3} ) is “a”. If ( alpha ) is degree of dissociation of ( A_{3} ). The total number of moles at equilibrium will be: A ( cdot a-frac{a alpha}{3} ) B. ( frac{a}{3}-alpha ) c. ( left(frac{a-a alpha}{2}right) ) D. None of these |
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| 586 | ( 100 mathrm{mL} ) of a solution contains ( 2 mathrm{g} ) of acetic acid and 3 g of sodium acetate providing ( K_{a}=1.8 times 10^{-5} . ) Choose the correct option. A. This solution is basic in nature B. This solution is acidic in nature c. This solution is amphoteric in nature D. This solution is neutral in nature |
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| 587 | The reaction ( boldsymbol{C H}_{3} boldsymbol{C O O H}+ ) ( C_{2} H_{5} O H leftrightharpoons C H_{3} C O O C_{2} H_{5}+H_{2} O ) can be made to proceed in the forward direction by: A. increasing the temperature B. sudden cooling of the reaction mixture c. conducting the reaction in the presence of a small quantity of ( N a O H ) D. taking excess of ( C_{2} H_{5} O H ) and ( C H_{3} C O O H ) |
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| 588 | Strength of an acid solution or a basic solution can be determined by knowing the hydrogen ion concentrations in them, using a pH scale. (i) Neutral solution has pH 7. (ii) Acidic solution has pH less than 7 . (iii) Basic solution has pH more than 7 . The pH of a solution is inversely proportional to hydrogen(H+) ion concentration in it. Teacher told three students Renuka, Bhawna and Seema to test their saliva with pH paper before and after having their lunch. Identify the correct observation from the following. A. Bhawna observed that pH paper turned red and recorded pH value of ( 2.3-2.5 ) after having lunch B. Seema observed that pH paper turned yellow and recorded pH value of ( 5.6-5.8 ) before having lunch c. Renuka observed that pH paper turned green and recorded pH value of 7.4-7.9 before having lunch D. observations made by both Renuka and Seema were correct |
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| 589 | The solubility of ( P b F_{2} ) in water at ( 25^{circ} C ) is ( sim 10^{-3} M . ) What is its solubility in ( mathbf{0 . 0 5} boldsymbol{M} boldsymbol{N} boldsymbol{a} boldsymbol{F} ) solution? Assume the latter to be fully ionised. A . ( 1.6 times 10^{-6} M ) В. ( 1.2 times 10^{-6} M ) c. ( 1.2 times 10^{-5} M ) D. ( 1.6 times 10^{-4} M ) |
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| 590 | What is the maximum ( p H ) of ( 0.10 M ) solution in ( M g^{2+} ) from which ( M g(O H)_{2} ) will not precipitate. Given : ( boldsymbol{K}_{s p}left(boldsymbol{M} boldsymbol{g}(boldsymbol{O} boldsymbol{H})_{2}right)=mathbf{1 . 2} times mathbf{1 0}^{-11} ) |
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| 591 | Assertion ( boldsymbol{K}_{boldsymbol{p}}=boldsymbol{K}_{c} ) for all reactions. BECAUSE Reason ( boldsymbol{K}_{boldsymbol{p}} ) and ( boldsymbol{K}_{boldsymbol{c}} ) are interrelated by the equation ( boldsymbol{K}_{boldsymbol{p}}=boldsymbol{K}_{c}(boldsymbol{R} boldsymbol{T})^{boldsymbol{Delta} boldsymbol{n}} ) 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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| 592 | For the reaction ( A+B rightleftharpoons 3 C ) at ( 25^{0} C ) A 3 Lvessel contains ( 1,2, ) and 4 moles of A, ( B, ) and ( C ) respectively. Predict the direction of reaction if: a) ( K_{C} ) for the reaction is 10 b) ( K_{C} ) for the reaction is 15 c) ( K_{C} ) for the reaction is 10.66 A. a) Backward direction b) Forward direction ( c ) ) At equilibrium B. a) Forward direction b) Backward direction c) Forward direction c. a) Backward direction b) Forward direction c) Back direction D. a) Backward direction b) Backrward direction c) At equilibrium |
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| 593 | If the concentration of ( mathrm{H}^{+}(mathrm{aq}) ) ions increases in a solution, the acidity: A . increases B. decreases C. remains same D. None of the above |
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| 594 | Which of the following represents a bronsted acid-base reaction? ( mathbf{A} cdot 3 O_{2}(g) rightleftharpoons 2 O_{3}(g) ) B. ( O H^{-}+H_{3} O^{+} rightleftharpoons 2 H_{2} O ) ( mathbf{c} cdot B a C l_{2} cdot 2 H_{2} O(s) triangleq B a C l_{2}(s)+2 H_{2} O(g) ) ( mathbf{D} cdot C a^{2+}+C O_{3}^{2-} rightarrow C a C O_{3}(s) ) ( mathbf{E} cdot F e+C u^{2+} rightleftharpoons F e^{2+}+C u ) |
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| 595 | What is the equation for the equilibrium constant ( left(K_{c}right) ) for the following equilibrium reaction? ( frac{1}{2} A(g)+frac{1}{3} B(g) rightleftharpoons frac{3}{2} C(g) ) ( ^{mathbf{A}} cdot_{K_{C}}=frac{[A]^{frac{1}{2}}[B]^{frac{1}{3}}}{[C]^{frac{3}{2}}} ) ( ^{mathrm{B}} K_{C}=frac{[C]^{frac{3}{2}}}{[A]^{2}[B]^{2}} ) ( ^{mathbf{c}}_{K_{C}}=frac{[C]^{frac{3}{2}}}{[A]^{frac{1}{2}}[B]^{frac{1}{5}}} ) ( ^{mathrm{D}} K_{C}=frac{[C]^{frac{3}{2}}}{[A]^{frac{1}{2}}+[B]^{frac{1}{3}}} ) |
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| 596 | Fresh milk has a pH of 6. On changing into curd, its pH becomes: A. more than 6 B. less than 6 c. does not change ( D ) |
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| 597 | Calculate pH of solution obtained by mixing ( 500 mathrm{ml} ) of ( 0.4 mathrm{M}, M_{1} O H ) and 1500ml of ( frac{mathbf{0 . 8}}{mathbf{3}} ) molar ( boldsymbol{N}_{mathbf{2}} boldsymbol{O} boldsymbol{H} . boldsymbol{K}_{boldsymbol{b}_{1}}= ) ( mathbf{1 0}^{-mathbf{7}} boldsymbol{K}_{boldsymbol{b}_{2}}=mathbf{4} times mathbf{1 0}^{-mathbf{7}} ) |
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| 598 | The value of ( boldsymbol{K}_{s p} ) is ( boldsymbol{H} boldsymbol{g} boldsymbol{C l}_{2} ) at room temperture is ( 4.0 times 10^{-15} ). The concentration of ( C l^{ominus} ) ion in its aqueous solution at saturation point is: A ( cdot 1 times 10^{-5} ) В. ( 2 times 10^{-5} ) c. ( 2 times 10^{-15} ) D. ( 8 times 10^{-15} ) |
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| 599 | Consider the reaction, ( boldsymbol{F} boldsymbol{e}^{boldsymbol{3}+}(boldsymbol{a} boldsymbol{q})+boldsymbol{S} boldsymbol{C} boldsymbol{N}^{-}(boldsymbol{a} boldsymbol{q}) rightleftharpoons ) ( boldsymbol{F} boldsymbol{e} boldsymbol{S} boldsymbol{C} boldsymbol{N}^{2-}(boldsymbol{a} boldsymbol{q}) ) How will the equilibrium position shift if ( A g N O_{3}(a q) ) is added? ( (A g S C N ) is insoluble) |
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| 600 | You have two solutions A and B. The pH of solution ( A ) is 6 and ( p H ) of solution ( B ) is 8. Which solution has more hydrogen ion concentration? Which of this is acidic and which one is basic? |
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| 601 | Discuss the relation between ( boldsymbol{K}_{boldsymbol{p}} ) and ( K_{c} ) for this equilibrium: ( mathbf{2} boldsymbol{H}_{2} boldsymbol{O}(boldsymbol{g})+mathbf{2} boldsymbol{C} boldsymbol{l}_{2(boldsymbol{g})} rightleftharpoons boldsymbol{4} boldsymbol{H} boldsymbol{C l}_{(boldsymbol{g})}+ ) ( boldsymbol{O}_{2(boldsymbol{g})} ) A. ( K_{p}=K_{c} ) ( mathbf{B} cdot K_{p}>K_{c} ) c. ( K_{p}<K_{c} ) ( ^{mathrm{D}} K_{p}=frac{1}{K_{c}} ) |
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| 602 | What is ( p H ) Scale? Explain that ( p H ) change of the mouth is the cause of tooth decay |
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| 603 | Sodium carbonate exists as(in): A ( cdot N a_{2} C O_{3} cdot 10 H_{2} O(s) ) B . ( N a_{2} C O_{3} cdot H_{2} O(s) ) c. ( N a_{2} C O_{3} ) D. All of the above |
11 |
| 604 | un 9. The process depicted by the equation H2O (s) — H2O (1) AH = +1.43 kcal represents (a) fusion (b) melting (c) evaporation (d) boiling |
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| 605 | Introduction of inert gas at constant volume to a gaseous reaction at equilibrium, results in formation of : A. same amount of product B. more quantity of product c. less quantity of product D. no product |
11 |
| 606 | Which of the following metal sulphides has maximum solubility in water? ( mathbf{A} cdot C d Sleft(K_{s p}=36 times 10^{-30}right) ) B ( cdot operatorname{Fe} Sleft(K_{s p}=11 times 10^{-20}right) ) ( mathbf{c} cdot H g Sleft(K_{s p}=32 times 10^{-54}right) ) D. ( Z n Sleft(K_{s p}=11 times 10^{-22}right) ) |
11 |
| 607 | Which of the following will give a neutral pH solution when dissolved in water? A. ( N a O H ) B. ( C s C l ) ( mathbf{c} cdot H B r ) D. ( C H_{3} ) СООН E. ( O_{2} ) |
11 |
| 608 | Which of the following is not Lewis base? A. ( A g^{+} ) в. ( H_{2} ) о c. ( C N^{-} ) D. ( R N H_{2} ) |
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| 609 | 4. Calculate the oxalate concentration necessary to precipitate CaC,0, in a saturated solution of calcium carbonate. Kcac,0. = 2.6 10-9; Kcaco, = 8.7 x 10-9. (a) 2.6 x 10-9M (b) 2.8 x 10-5 M (c) 9.3 x 10-5 M (d) 3.4 x 10-3 M |
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| 610 | The hydrogen, ion concentration of a solution is 0.001 M. What is the ( p H ) of the solution? |
11 |
| 611 | Which buffer solution comprising of the following has its ( p H ) value greater than ( 7 ? ) A ( cdot C H_{3} C O O H+C H_{3} C O O N a ) в. ( H C O O H+H C O O K ) c. ( C H_{3} C O O N H_{4} ) D. ( N H_{4} O H+N H_{4} C l ) |
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| 612 | The ionization constant of dimethylamine is ( 5.4 times 10^{-4} ). Calculate its degree of ionization in its ( 0.02 mathrm{M} ) solution. What percentage of dimethylamine is ionized if the solution is also 0.1M in NaOH? |
11 |
| 613 | ( 100 mathrm{ml} ) of ( 0.1 mathrm{M} C mathrm{H}_{3} mathrm{COOH} ) is mixed with ( 50 mathrm{ml} ) of ( 0.1 mathrm{M} ) NaOH solution and pH of the resulting solution is 5. The change in pH if ( 100 mathrm{ml} ) of ( 0.05 mathrm{M} ) NaOH is added in the above solution is: A . 1.30 B. 4.74 ( c cdot 5 ) D. 3.8 |
11 |
| 614 | Two moles of ( P C l_{5} ) are heated in a closed vessel of 2 litre capacity. When the equilibrium is attained ( 40 % ) of it has been found to be dissociated. What is the value of ( K_{c} ) in ( m o l / d m^{3} ? ) A. 0.532 B. 0.266 c. 0.133 D. 0.174 E . 0.25 |
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| 615 | Which compound is used for bleaching cloths in laundry? A. Bleaching powder B. Washing powder c. Baking powder D. Plaster of Paris |
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| 616 | The equilibrium constant for the reaction ( N_{2}(g)+O_{2}(g) leftrightharpoons 2 N O(g) ) is ( 4 times 10^{-4} ) at ( 2000 mathrm{K} . ) In the presence of a catalyst, the equilibrium is attained three times faster. The equilibrium constant in the presence of the catalyst at ( 2000 mathrm{K} ) is: A. ( 40 times 10^{-4} ) B. ( 4 times 10^{-4} ) c. ( 4 times 10^{-3} ) D. ( 4 times 10^{-8} ) |
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| 617 | The ( p H ) of ( 10^{-4} M K O H ) solution will be: ( A cdot 4 ) B. 1 ( c cdot 10.5 ) D. 10 |
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| 618 | pH of saturated solution of ( C a(O H)_{2} ) is 9. the solubility product ( left(K_{s p}right) ) of ( boldsymbol{C a}(boldsymbol{O H})_{2} ) is: A ( .0 .5 times 10^{-15} ) В. ( 0.25 times 10^{-10} ) ( c cdot 0.125 times 10^{-15} ) 5 D. ( 0.5 times 10^{10} ) |
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| 619 | The conductivity of a saturated solution of ( A g_{3} P O_{4} ) is ( 9 times 10^{-6} S m^{-1} ) and its equivalent conductivity is ( 1.50 times ) ( 10^{-4} S m^{2} ) equivalent ( ^{-1} . ) The ( K_{s p} ) of ( A g_{3} P O_{4} ) is: A ( cdot 4.32 times 10^{-18} ) B. ( 1.8 times 10^{-9} ) c. ( 8.64 times 10^{-13} ) D. None of these |
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| 620 | On long standing, bleaching powder undergoes auto oxidation. A. True B. False |
11 |
| 621 | The ( p H ) of ( 0.1 mathrm{M} ) acetic acid is ( 3, ) the dissociation constant of acid will be: A ( cdot 1.0 times 10^{-4} ) В. ( 1.0 times 10^{-5} ) c. ( 1.0 times 10^{-3} ) D. ( 1.0 times 10^{-8} ) |
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| 622 | Choose the correct combination among thefollowing A) A mixture of weak acid and its salt of strong base acts as acidic buffer. B) As number of moles of acid or base required to change the ( p^{H} ) of the buffer by one unit increases, the quality of buffer increases. C) Buffer action is maximum at ( boldsymbol{p}^{boldsymbol{H}}= ) ( P^{K a} ) in case of acidic buffer. A. All are correct B. A only correct c. B only correct D. A only false |
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| 623 | In which of the following cases, does the reaction go furthest to completion? A ( cdot K=10^{3} ) B. ( K=10^{-2} ) c. ( K=10^{5} ) D. ( K=1 ) |
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| 624 | In which of the following ( K_{p} ) is less than ( boldsymbol{K}_{c} ? ) A ( cdot N_{2} O_{4}(g) rightleftharpoons 2 N O_{2}(g) ) B . ( 2 H I(g) rightleftharpoons H_{2}(g)+I_{2}(g) ) c. ( 2 S O_{2}(g)+O_{2}(g) rightleftharpoons 2 S O_{3}(g) ) D. ( P C l_{5}(g) rightleftharpoons P C l_{3}(g)+C l_{2}(g) ) |
11 |
| 625 | Calculate the ( mathrm{pH} ) of ( 10^{-8} mathrm{M} mathrm{HCl} ) ( A cdot 8 ) B. 6 ( c cdot 7 ) D. 6.98 |
11 |
| 626 | Equilibrium constant for the reaction ( mathbf{2} N boldsymbol{O}(boldsymbol{g})+boldsymbol{C l}_{2}(boldsymbol{g}) rightleftharpoons 2 boldsymbol{N} boldsymbol{O} boldsymbol{C l}(boldsymbol{g}) ) is correctly given by the expression: ( ^{mathbf{A}} cdot_{K}=frac{[2 N O C l]}{[2 N O]left[C l_{2}right]} ) в. ( _{K}=frac{[N O C l]^{2}}{[N O]^{2}left[C l_{2}right]} ) ( ^{mathbf{c}}_{K}=frac{[N O]^{2}[C l]^{2}}{[N O]^{2}+left[C l_{2}right]} ) ( K=frac{[N O]^{2}+[C l]^{2}}{[N O C l]} ) |
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| 627 | The following reaction is at equilibrium, ( boldsymbol{F} boldsymbol{e}_{(a q)}^{3+}+boldsymbol{S C} boldsymbol{N}_{(a q)}^{-} rightleftharpoons ) ( left[boldsymbol{F e}(boldsymbol{S C N})_{(a q)}^{2+} ; boldsymbol{K}_{c}=frac{[boldsymbol{F e}(boldsymbol{S C N})]^{2+}}{left[boldsymbol{F e}^{3+}right]left[boldsymbol{S C N}^{-}right]}right. ) In the above reaction, color intensity of red colour can be increased by: A. addition of KSCN B. addition of oxalic acid which reacts with ( F e^{3+} ) ions C. addition of ( H g^{2+} ) ions which reacts with ( S C N^{-} ) ions D. red colour intensity cannot be changed. |
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| 628 | ( boldsymbol{K}_{s p} ) of ( boldsymbol{C u} boldsymbol{S}, boldsymbol{A} boldsymbol{g}_{2} boldsymbol{S} ) and ( boldsymbol{H} boldsymbol{g} boldsymbol{S} ) are ( 10^{-31}, 10^{-44} ) and ( 10^{-54} ) mol ( ^{2} ) litre ( ^{-2} ) respectively. Select the correct order for their solubility in water ( mathbf{A} cdot A g_{2} S>H g S>C u S ) B. ( H g S>C u S>A g_{2} S ) c. ( H g S>A g_{2} S>C u S ) D. ( A g_{2} S>C u S>H g S ) |
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| 629 | The equilibrium constant ( left(boldsymbol{K}_{c}right) ) for the reaction ( boldsymbol{H} boldsymbol{A}+boldsymbol{B} rightleftharpoons boldsymbol{B} boldsymbol{H}^{+}+boldsymbol{A}^{-} ) is ( mathbf{1 0 0} ) If the rate constant for the forward reaction is ( 10^{5} ), then rate constant for the backward reaction is A ( cdot 10^{7} ) B . ( 10^{3} ) ( mathbf{c} cdot 10^{-3} ) D. ( 10^{-5} ) |
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| 630 | Sulphide ions in alkaline solution react with solid sulphur to form polyvalent sulphide ions. The equilibrium constant for the formation of ( S_{2}^{2-} ) and ( S_{3}^{2-} ) from. ( S ) and ( S^{2-} ) ions are 1.7 and 5.3 respectively. Calculate equuilibrium constant for the formation of ( S_{3}^{2-} ) from ( S_{2}^{2-} ) and ( S ) A . 0.31 в. 3.11 c. 31.3 D. 0.0313 |
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| 631 | A buffer of ( mathrm{pH} 8.50 ) is prepared from 0.02 mole of ( K C N . ) The desired volume of buffer solution is to be 1 litre. How will you make this buffer using ( boldsymbol{H} boldsymbol{C l} ) ? What is the change after addition of ( 0.5 times 10^{-4} ) mole ( H C l ) to ( 100 c m^{3} ) and same amount of ( N a O H ) in ( 100 c m^{3} ) of buffer? ( left(boldsymbol{K}_{boldsymbol{a}} boldsymbol{H} boldsymbol{C} boldsymbol{N}=boldsymbol{6} . boldsymbol{2} times mathbf{1 0}^{-10}right) ) |
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| 632 | Which of the following compounds will be dissociated into its constituent ions? This question has multiple correct options A. Solid ( N a C l ) B. Molten NaCl c. solid ( C a C l_{2} ) D. Molten ( C a C l ) |
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| 633 | In a buffer solution consisting of a weak acid and its salt, the ratio of the concentration of salt to acid is increased tenfold, then the ( p H ) of the solution will: A. Increase by one B. Increase tenfold c. Decrease by one D. Decrease tenfold |
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| 634 | The solubility of all solids in water increase with increase in temperature. A. True B. False |
11 |
| 635 | For an equilibrium reaction involving gases, the forward reaction is first order while the reverse reaction is second order. The units of ( boldsymbol{K}_{boldsymbol{p}} ) for forward equilibrium is: A . atm B ( . a t m^{2} ) c. ( a t m^{-1} ) D. ( a t m^{-2} ) |
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| 636 | ( p K_{a_{1}} ) of carbonic acid in blood at body temperature ( left(37^{circ} Cright) ) is ( 6.1 . ) Hence, ratio ( left[boldsymbol{H} boldsymbol{C O}_{3}^{-}right] /left[boldsymbol{H}_{2} boldsymbol{C O}_{3}right] ) is approximately: A . 1.3: B. 1: 1.3 ( c cdot 20: ) D. 1: 20 |
11 |
| 637 | Q47. It has been found that the pH of a 0.01 M solution of an organic acid is 4.15. Calculate the concentration of the anion, the ionization constant of the acid and its pk |
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| 638 | For the equilibrium ( N_{2}+3 H_{2} rightleftharpoons ) ( 2 N H_{3}, K_{c} ) at ( 1000 K ) is ( 2.37 times 10^{-3} . ) If at equilibrium ( left[boldsymbol{N}_{2}right]=mathbf{2} boldsymbol{M},left[boldsymbol{H}_{2}right]=boldsymbol{3} boldsymbol{M} ) the concentration of ( boldsymbol{N} boldsymbol{H}_{3} ) is: A . ( 0.00358 M ) B. ( 0.0358 M ) c. ( 0.358 M ) D. 3.58 М |
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| 639 | The ( p H ) of ( 0.1 ~ M ) solution of the following salts increases in the order A. ( N a C l<N H_{4} C l<N a C N<H C l ) в. ( operatorname{NaCN}<N H_{4} C l<N a C l<H C l ) c. ( H C l<N a C l<N a C N<N H_{4} C l ) D. ( H C l<N H_{4} C l<N a C l<N a C N ) |
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| 640 | ( boldsymbol{p} boldsymbol{K}_{a} ) of Quinoline base is ( 4.88 . ) What will be the ( p K_{a} ) of ( 0.01 mathrm{M} ) solution of it? A . 4.88 B. 0.01 c. 9.12 D. 14 |
11 |
| 641 | 1.6 mole of ( boldsymbol{P C l}_{5}(boldsymbol{g}) ) is placed in ( boldsymbol{4} boldsymbol{d} boldsymbol{m}^{3} ) closed vessel. When the temperature is raised to ( 500 K ), it decomposes and at equilibrium 1.2 mole of ( P C l_{5}(g) ) remains.What is the ( K_{c} ) value for the decomposition of ( boldsymbol{P} boldsymbol{C l}_{mathbf{5}}(boldsymbol{g}) ) to ( boldsymbol{P} boldsymbol{C l}_{3}(boldsymbol{g}) ) and ( C l_{2}(g) ) at ( 500 K ? ) ( mathbf{A} cdot 0.013 ) B. 0.050 c. 0.033 D. 0.067 |
11 |
| 642 | Q61. The ionization constant of nitrous acid is 4.5 x 10-4. Calculate the pH of 0.04 M sodium nitrite solution and also its degree of hydrolysis. |
11 |
| 643 | The solubility product of ( boldsymbol{H} boldsymbol{g}_{2} mathbf{1}_{2} ) is equal to ( mathbf{A} cdotleft[H g_{2}^{2+}right]left[I^{-}right] ) B ( cdotleft[H g^{2+}right]left[I^{-}right] ) c. ( left[H g_{2}^{2+}right]left[I^{-}right]^{2} ) D ( cdotleft[H g^{2+}right]left[I^{-}right]^{2} ) |
11 |
| 644 | Which of the following is not Lewis acid? A. ( B F_{3} ) в. ( A l C l_{3} ) c. ( F e C l_{3} ) D. ( P H_{3} ) |
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| 645 | A reaction in equilibrium is represented by the following equation: ( mathbf{2 A}(s)+mathbf{3 B}(boldsymbol{g}) rightleftharpoons mathbf{3} boldsymbol{C}(boldsymbol{g})+boldsymbol{D}(boldsymbol{g})+boldsymbol{O}_{2} ) if the pressure on the system is reduced to half of its original value then A. The amounts of ( C ) and ( D ) increases B. The amounts of ( C ) and ( D ) decreases c. The amounts of ( B ) and ( D ) decreases D. All the amounts remain constant |
11 |
| 646 | Which of the following salts is a strong electrolyte? A . ( N a C l ) в. ( K C l ) c. ( M g C l_{2} ) D. All of the above |
11 |
| 647 | For the given reaction the equilibrium expression ( mathbf{2} boldsymbol{A}_{(boldsymbol{g})}+boldsymbol{B}_{(boldsymbol{g})} Leftrightarrow mathbf{3} boldsymbol{C}_{(boldsymbol{g})}+boldsymbol{D}_{(boldsymbol{g})} ) ( mathbf{A} cdot[A]^{2}[B][D] ) В. ( frac{[C]^{3}[D]}{left.[A]^{2}[] Bright]} ) c. ( frac{[2 C][D]}{[2 A][B]} ) D. ( frac{[D]}{[A]^{2}[B]} ) E ( cdot frac{[A]^{2}[B]}{[C]^{3}[D]} ) |
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| 648 | Table salt is contaminated with ( N a H C O_{3} ) due to presence of ( M g C l_{2} ) as impurity (from sea). If true enter 1 , else enter 0 . |
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| 649 | Solid Ammonium carbamate dissociates as: ( N H_{2} C O O N H_{4}(s) rightleftharpoons 2 N H_{3}(g)+ ) ( boldsymbol{C O}_{2}(boldsymbol{g}) ) In a closed vessel, solid ammonium carbonate is in equilibrium with its dissociation products. At equilibrium, ammonia is added such that the partial pressure of ( N H_{3} ) at new equilibrium now equals the original total pressure. Calculate the ratio of total pressure at new equilibrium to that of original total pressure. A ( cdot frac{31}{27} ) в. ( frac{17}{7} ) c. ( frac{49}{29} ) D. None of these |
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| 650 | Q12. A mixture of 1.57 mol of N, 1.92 mol of H, and 8.13 mol of NH, is introduced into a 20L reaction vessel at 500 K. At this temperature, the equilibrium constant K for the reaction N. (g) + 3H, (g) + 2NH, () is 1.7 x 10-2. Is this reaction at equilibrium? If not, what is the direction of net reaction? |
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| 651 | At same temperature and under a pressure of ( 4 a t m, P C l_{5} ) is ( 10 % ) dissociation. Calculate the pressure at which ( P C l_{5} ) will be ( 20 % ) dissociated temperature remaining same. |
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| 652 | Solid rightleftharpoons liquid equilibrium can be achieved only at the melting point of the substance. A. True B. False |
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| 653 | ( Z n(O H)_{2} ) is an amphoteric hydroxide which is involved in the following two equilibria existing simultaneously in aqueous solution. ( boldsymbol{Z n}(boldsymbol{O} boldsymbol{H})_{2}(boldsymbol{s}) rightleftharpoons boldsymbol{Z} boldsymbol{n}^{2+}(boldsymbol{a} boldsymbol{q})+ ) ( mathbf{2 O H}^{-}(boldsymbol{a q}) ; boldsymbol{K}_{s p}=mathbf{1 . 2} times mathbf{1 0}^{-mathbf{1 7}} ) ( operatorname{Zn}(O H)_{2}(s)+2 O H^{-}(a q) rightleftharpoons ) ( left[Z n(O H)_{4}right]^{2-}(a q) ; K_{c}=0.12 ) At what ( p H ) the solubility of ( Z n(O H)_{2} ) will be minimum? A. ( p H=4.11 ) в. ( p H=6.32 ) c. ( p H=7.68 ) D. ( p H=9.99 ) |
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| 654 | The decrease in % in ( left[boldsymbol{H}^{+}right] ) when ( boldsymbol{p} boldsymbol{H} ) increases by 0.1 will be: A . 10 B. 30 c. 50 D. 20 |
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| 655 | Assertion pH of 10 M H Cl aqueous solution is less than 1. Reason pH is negative logarithm of ( boldsymbol{H}^{+} ) concentration. 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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| 656 | The value of ( k_{c} ) for the reaction ( mathbf{2} boldsymbol{A} rightleftharpoons boldsymbol{B}+boldsymbol{C} ) is ( 2 times 10^{-3} ) At a given time the composition of reaction mixture is ( [A]=[B]=[C]=3 x ) ( 10^{-4} ) M. In which direction the reaction will proceed? A. From left to right B. From right to left c. The reaction is at equilibrium D. First to the right than left |
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| 657 | The experimental curve obtained when the rate of a reaction is plotted against time, appeared parallel to the time axis some time after the reaction started. This indicates that: A. the reaction has stopped B. the equilibrium is established c. the concentration of the reactants is negligible D. the reaction is complex |
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| 658 | At ( 1400 K, K_{c}=2.5 times 10^{-3} ) for reaction ( boldsymbol{C H}_{4}(boldsymbol{g})+mathbf{2} boldsymbol{H}_{2} boldsymbol{S}(boldsymbol{g}) rightleftharpoons boldsymbol{C} boldsymbol{S}_{2}(boldsymbol{g})+ ) ( 4 H_{2}(g) . ) At ( 10.0 L ) reaction vessel at ( 1400 mathrm{K} ) contains 2.00 mole of ( mathrm{CH}_{4}, 3.0 ) mol of ( mathrm{CS}_{2}, 3.0 ) mole of ( mathrm{H}_{2} ) and 4.0 mole of ( mathrm{H}_{2} mathrm{S} ). Then A. this reaction is at equilibrium with above concentrations B. the reaction will proceed in forward direction to reach equilibrium c. the reaction will proceed in backward direction to each equilibrium D. the information is insufficient to decide the direction of progress of reaction |
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| 659 | Which of the following cannot decompose on heating to give ( C O_{2} ? ) A ( cdot L i_{2} C O_{3} ) в. ( N a_{2} C O_{3} ) ( mathbf{c} cdot K H C O_{3} ) D. ( B a C O_{3} ) |
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| 660 | ( boldsymbol{K}_{boldsymbol{w}} ) of pure water is ( mathbf{1 0}^{-12} ) at ( mathbf{6 0}^{circ} boldsymbol{C} ). The ( p H ) of pure water at ( 60^{circ} mathrm{C} ) is: |
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| 661 | Which has highest ( p H ? ) A. ( C H_{3} ) СООК в. ( N a_{2} C O_{3} ) c. ( N H_{4} C l ) D. ( N a N O_{3} ) |
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| 662 | The solubility of a substance is 40 to 50 C such that at same temperature its solution contains 5 g of it in 10 gof water A . True B. False c. Nither D. Either |
11 |
| 663 | Which of the following compounds is known as baking soda? A. Sodium carbonate B. Calcium carbonate c. Sodium bicarbonate D. Calcium bicarbonate |
11 |
| 664 | The degree of dissociation ( (alpha) ) of a weak electrolyte, ( A_{x} B_{y} ) is related to van’t Hoff factor (i) by the expression: A ( cdot alpha=frac{i-1}{(x+y-1)} ) B. ( alpha=frac{i-1}{x+y+1} ) c. ( alpha=frac{x+y-1}{i-1} ) D. ( alpha=frac{x+y+1}{i-1} ) |
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| 665 | Solubility product of ( C a C O_{3} ) is ( 5 times 10^{-9} . ) Find its solubility. |
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| 666 | Concentration of ( boldsymbol{N} boldsymbol{H}_{4} boldsymbol{C l} ) and ( boldsymbol{N} boldsymbol{H}_{4} boldsymbol{O} boldsymbol{H} ) in a buffer solution are in the ratio of ( 1: 10, mathrm{Kb} ) for ( N H_{4} O H ) is ( 10^{-10} . ) The pH of the buffer is: (BHU, 1994) A .4 B. 5 ( c cdot 9 ) D. 1 |
11 |
| 667 | Which of the following statement is correct: A. Sodium hydroxide turns blue litmus red. B. Nitric acid turns red litmus blue. C. Sodium hydroxide turns red litmus blue D. tooth decay is caused by the presence of a base |
11 |
| 668 | When strong base ( (N a O H) ) is added to the weak acid (acetic acid, ( left.C H_{3} C O O Hright), ) then dissociation of acetic acid increases; this effect is known as: A. Common ion effect B. Reverse ion effect c. Saltation effect D. Solubility effect |
11 |
| 669 | If very small amount of phenolphthalein is added to 0.15 mol litre ( ^{-1} ) solution of sodium benzoate, what fraction of the indicator will exist in the coloured form? State any assumption that you make. ( K_{a}(text { Benzoic acid })=6.2 times ) ( mathbf{1 0}^{-mathbf{5}}, boldsymbol{K}_{boldsymbol{w}}left(boldsymbol{H}_{mathbf{2}} boldsymbol{O}right)=mathbf{1} times mathbf{1 0}^{-mathbf{1 4}} ) ( boldsymbol{K}_{l n} ) (Phenolphthalein) ( mathbf{3} . mathbf{1 6} times mathbf{1 0}^{-mathbf{1 0}} ) |
11 |
| 670 | In the system, ( C a F_{2}(s) rightleftharpoons ) ( C a^{+2}(a q)+2 F^{-} ) increasing the concentration of ( C a^{2+} ) ions four times will cause the equilibrium concentration of ( boldsymbol{F}^{-} ) ions to change to times the initial value. A . 4 B. ( frac{1}{2} ) ( c cdot 2 ) D. |
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| 671 | A reversible reaction ( A rightleftharpoons C ) takes place in two steps ( boldsymbol{A} rightleftharpoons boldsymbol{B} ; boldsymbol{B} rightleftharpoons boldsymbol{C} ) which are also equilibrium steps. If the equilibrium constants of the two steps are ( K_{1} ) and ( K_{2} ) respectively, the overall equilibrium constant ( boldsymbol{K} ) is equal to: ( ^{text {A }} cdot frac{K_{1}}{K_{2}} ) в. ( frac{K_{2}}{K_{1}} ) ( mathbf{c} cdot K_{1} times K_{2} ) D. ( K_{1}-K_{2} ) |
11 |
| 672 | For an equilibrium ( boldsymbol{H}_{2} boldsymbol{O}(boldsymbol{s}) rightleftharpoons boldsymbol{H}_{2} boldsymbol{O}(ell) ) which of the following statement is true? A. The pressure changes do not affect the equilibrium B. More of ice melts if pressure on the system is increased c. More of liquid freezes if pressure on the system is increase D. The pressure changes may increase or decrease the degree of advancement of the reaction depending upon the temperature of the system. |
11 |
| 673 | ( boldsymbol{C C l}_{4} rightleftharpoons boldsymbol{C}+mathbf{2 C l}_{2} ) The equilibrium constant ( p K ) for the given reaction at ( 700^{0} C ) is 0.76 atm. The initial pressure of carbon tetrachloride that will produce a total equilibrium pressure of 1.20 atm at ( mathbf{7} mathbf{0 0}^{mathbf{o}} mathbf{C} ) is: A. 0.22 atm B. 0.44 atm c. 0.84 atm D. 0.11 atm |
11 |
| 674 | The real bleaching agent present in bleaching powder is: A. chlorine B. oxygen c. сао D. None of the above |
11 |
| 675 | The ( K_{s p} ) for a sparingly soluble ( A g_{2} C r O_{4} ) is ( 4 times 10^{-12} . ) The molar solubility of the salt is: ( begin{array}{lll}text { A } cdot 2.0 times 10^{-6} & text {mol } & L^{-1}end{array} ) ( begin{array}{lll}text { В. } 1.0 times 10^{-4} & text {тод } L^{-1}end{array} ) ( begin{array}{lll}text { C. } 2.0 times 10^{-12} & text {mol } & L^{-1}end{array} ) D. ( 1.0 times 10^{-15} ) mol ( L^{-1} ) |
11 |
| 676 | List 1 and List 2 contains four entries each. Entries of List 1 are to be matched with some entries of List 2. One or more than one entries of List 1 may have the matching with the same entries of List 2 |
11 |
| 677 | The equilibrium constant for the reaction, ( N_{2}(g)+O_{2}(g)=2 N O(g) ) is ( 4 times 10^{-4} ) at ( 2000 mathrm{k} . ) In the presence of a catalyst, the equilibrium is attained ten times faster. Therefore, the equilibrium constant in the presence of the catalyst of ( 2000 mathrm{k} ) is: A. ( 4 times 10^{-2} ) B. ( 40 times 10^{-4} ) c. ( 4 times 10^{-4} ) D. ( 4 times 10^{-1} ) |
11 |
| 678 | Assume that the decomposition of ( H N O_{3} ) can be represented by the following equation ( 4 H N O_{3}(g) rightleftharpoons 4 N O_{2}(g)+ ) ( mathbf{2} boldsymbol{H}_{mathbf{2}} boldsymbol{O}(boldsymbol{g})+boldsymbol{O}_{2}(boldsymbol{g}) ) The reaction approaches equilibrium at ( 400 K ) temperature and 30 atm pressure. At equilibrium partial pressure of ( boldsymbol{H} boldsymbol{N} boldsymbol{O}_{3} ) is ( boldsymbol{2} ) atm. Calculate ( boldsymbol{K}_{c} ) in ( (boldsymbol{m} boldsymbol{o l} / boldsymbol{L})^{3} ) at ( boldsymbol{4} boldsymbol{0} boldsymbol{0} boldsymbol{K} ) ( (text { Use }: boldsymbol{R}=mathbf{0 . 0 8 a t m}-boldsymbol{L} / boldsymbol{m o l}-boldsymbol{K}) ) ( A cdot 4 ) B. 8 ( c cdot 16 ) D. 32 |
11 |
| 679 | The following reaction is known to occur in the human body: ( boldsymbol{C O}_{2}+boldsymbol{H}_{2} boldsymbol{O} rightleftharpoons boldsymbol{H}_{2} boldsymbol{C O}_{3} rightleftharpoons boldsymbol{H}^{+}+ ) ( boldsymbol{H} boldsymbol{C O}_{mathbf{3}}^{-} ) If ( C O_{2} ) escapes from the system A . pH will decrease B. ( H^{+} ) ion concentration will decrease c. ( H_{2} C O_{3} ) concentration will be unaltered D. The forward reaction will be promoted |
11 |
| 680 | In reversible reactions concentration of: A. reactants decreases with time at equilibrium B. products increases with time at equilibrium C. reactants decreases and then increases with time at equilibrium D. reactants and products are constant at equilibrium |
11 |
| 681 | ( 0.5 mathrm{ml} ) of ( H_{2} ) and 0.5 mole of ( I_{2} ) react in 10 litre flask at ( 448^{circ} mathrm{C} ). The equilibrium constant ( boldsymbol{K}_{c} ) is ( mathbf{5 0} ) for ( boldsymbol{H}_{2}(boldsymbol{g})+boldsymbol{I}_{2}(boldsymbol{g}) rightleftharpoons ) ( 2 H I(g) ) What is the value of ( boldsymbol{K}_{boldsymbol{p}} ) ? A . 50 B. 20 c. 10 D. 40 |
11 |
| 682 | Molten NaCl conducts electricity due to the presence of : ( mathbf{A} cdot ) free molecules B. free ions c. free electrons D. free atoms |
11 |
| 683 | A buffer solution is formed by mixing ( 100 mathrm{mL} 0.01 mathrm{M} C mathrm{H}_{3} mathrm{COOH} ) with ( 200 mathrm{mL} ) ( 0.02 mathrm{M} C H_{3} C O O N a . ) If this buffer solution is made to 1 lit by adding 700 mL of water, ( boldsymbol{p} boldsymbol{H} ) will change by a factor of: |
11 |
| 684 | For the following reaction at ( 250^{circ} mathrm{C} ), the value of ( K_{c} ) is ( 26, ) then the value of ( K_{p} ) at the same temperature will be: ( boldsymbol{P C l}_{3}(boldsymbol{g})+boldsymbol{C l}_{2}(boldsymbol{g}) rightleftharpoons boldsymbol{P} boldsymbol{C l}_{5}(boldsymbol{g}) ) A . 0.57 B. 0.61 c. 0.83 D. 0.91 |
11 |
| 685 | The ( p H ) at which a ( 0.01 mathrm{M} A l^{+3} ) solution is ( 99.99 % ) precipitated is: ( left(boldsymbol{K}_{s p} boldsymbol{A l}(boldsymbol{O H})_{3}=mathbf{1} times mathbf{1 0}^{-18} boldsymbol{a t} quad mathbf{2 5}right) ) A . 6.67 B. 7.67 c. 8.67 D. 9.617 |
11 |
| 686 | At a certain temperature 2 moles of carbonmonoxide and 3 moles of chlorinw were allowed to reach equilibrium according to the reaction ( boldsymbol{C O}_{(g)}+boldsymbol{C l}_{2} leftrightharpoons boldsymbol{C O C l}_{2} ) in a 5 lit vessel. At equilibrium if one mole of ( C O ) is present then equilibrium constant for the reaction is |
11 |
| 687 | State which of the following solutions contains only ions? A ( cdot d i l . H N O_{3} ) B. Kerosene c. ( C H_{3} ) СООН D. Oxalic acid |
11 |
| 688 | In a 20 litre vessel initially ( 1-1 ) mole ( C O, H_{2} O, C O_{2} ) is present, then for the equilibrium of ( boldsymbol{C O}+boldsymbol{H}_{2} boldsymbol{O} rightleftharpoons boldsymbol{C} boldsymbol{O}_{2}+ ) ( boldsymbol{H}_{2} ) following is true? A. ( H_{2}, ) more than 1 mole B. ( C O, H_{2} O, H_{2} ) less then 1 mole c. ( C O_{2} & H_{2} O ) both more than 1 mole D. All of these |
11 |
| 689 | Le Chatelier’s principle is applicable to both homogeneous and heterogeneous equilibria. If true enter 1 , if false enter 0 . |
11 |
| 690 | A ( 20 L ) box contains ( O_{3} ) and ( O_{2} ) at ( t ) equilibrium at ( 202 K . K_{p}=2 times 10^{14} ) for ( 2 O_{3} rightleftharpoons 3 O_{2} . ) Assume that ( p_{O_{3}}>> ) ( p_{O_{2}} ) and total pressure is 8 at ( m ), then the partial pressure of ( boldsymbol{O}_{3} ) is: A . exactly ( 1.6 times 10^{-6} ) at ( m ) B. sufficiently less than ( 1.6 times 10^{-6} ) atm C. slightly more than ( 1.6 times 10^{-6} ) atm D. very slightly less than ( 1.6 times 10^{-6} ) atm |
11 |
| 691 | In the third group of qualitative analysis, the precipatitating reagent is ( N H_{4} C l / N H_{4} O H . ) The function of ( N H_{4} C l ) is to A. increase the ionisation of ( N H_{4} O H ) B. supress the ionisation of ( N H_{4} O H ) C. convert the ions of group third into their respective chlorides D. stabilise the hydroxides of group III cations |
11 |
| 692 | The equilibrium constant for a reaction is ( K, ) and the reaction quotient is ( Q ). For a reaction mixture, the ratio ( frac{K}{Q} ) is 0.33 This means that: A. the reaction mixture will equilibrium to form more reactant species B. the reaction mixture will equilibrium to form more product species c. the equilibrium ratio of reactant to product concentrations will be 3 D. the equilibrium ratio of reactant to product concentrations will be 0.33 |
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| 693 | What is the ( K_{b} ) for ( N H_{2} ) group in glycine? ( mathbf{A} cdot 4 times 10^{-3} ) в. ( 1.6 times 10^{-10} ) c. ( 6.25 times 10^{-5} ) D. ( 2.5 times 10^{-12} ) |
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| 694 | Assertion Solubility of sparingly soluble salt decreases due to common ion effect Reason Solubility product constant does not |
11 |
| 695 | Two systems, ( boldsymbol{P C l}_{5(g)} rightleftharpoons boldsymbol{P C l}_{3(g)}+ ) ( boldsymbol{C l}_{2(boldsymbol{g})} ) and ( boldsymbol{C O C l}_{2(boldsymbol{g})} rightleftharpoons boldsymbol{C O}_{(g)}+boldsymbol{C l}_{2(boldsymbol{g})} ) are simultaneously in equilibrium in a vessel at constant volume. If some ( C O ) is introduced into the vessel then at the new equilibrium, the concentration of : A . ( P C l_{5} ) is increased B. ( P C l_{3} ) remains unchanged c. ( P C l_{5} ) is decreased D. ( C l_{2} ) is increased |
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| 696 | 0.01 mol of ( A g N O_{3} ) is added to 1 L of a solution which is ( 0.1 M N a_{2} C r O_{4} ) and ( 0.005 M ) in ( N a I O_{3} . ) Calculate ( left[boldsymbol{A} boldsymbol{g}^{oplus}right],left[boldsymbol{I} boldsymbol{O}_{3}^{ominus}right] ) and ( left[boldsymbol{C r} boldsymbol{O}_{4}^{2-}right] ) ( K_{s p} A g_{2} C r O_{4} ) and ( A g I O_{3} ) are ( 10^{-8} ) and ( 10^{-13} ) respectively ( mathbf{A} cdotleft[A g^{oplus}right]=0.316 times 10^{-4} M,left[I O_{3}^{ominus}right]=0.31 times ) ( 10^{-10} M,left[C r O_{2}^{2-}right]=0.0975 M ) B ( cdotleft[A g^{oplus}right]=3.16 times 10^{-4} M,left[I O_{3}^{ominus}right]=3.1 times ) ( 10^{-10} M,left[C r O_{2}^{2-}right]=0.975 M ) C ( cdotleft[A g^{oplus}right]=31.6 times 10^{-4} M,left[I O_{3}^{odot}right]=31 times ) ( 10^{-10} M,left[C r O_{2}^{2-}right]=9.75 M ) D. None of these |
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| 697 | Given the reaction ( boldsymbol{A} rightarrow boldsymbol{B}+boldsymbol{C}, ) when ( triangle boldsymbol{H}_{text {reaction}} ) is negative, what effect would increase in temperature (at constant pressure) have on the system at equilibrium? A. No change B. Cannot be determined c. Shift to the right D. Shift to left for ( K1 ) E. Shift to the left |
11 |
| 698 | The equilibrium constant for the reaction ( boldsymbol{P C l}_{5(g)} rightleftharpoons boldsymbol{P} C l_{3(g)}+boldsymbol{C l}_{2(g)} ) is ( 2.4 times ) ( 10^{-3} . ) Determine the equilibrium constant for the reverse reaction at same temperature |
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| 699 | Q3. Ata certain temperature and total pressure of 10° Pa, iodine vapours contain 40% by volume of iodine atoms in the equilibrium I.(g) = 21 (g). Calculate K, for the equilibrium. |
11 |
| 700 | The acid present in tea is: A . citric B. tannic c. formic D. lactic |
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| 701 | Gaseous ( N_{2} O_{4} ) dissociates into gaseous ( N O_{2} ) according to the reaction ( N_{2} O_{4}(g) rightleftharpoons 2 N O_{2}(g) ) at ( 300 mathrm{K} ) and 1 atm pressure, the degree of dissociation of ( N_{2} O_{4} ) is ( 0.2 . ) If one mole of ( N_{2} O_{4} ) gas is contained in a vessel then the density of the equilibrium mixture is : A. ( 3.11 mathrm{g} / mathrm{L} ) B. 4.56 g/L c. ( 1.56 g / L ) D. ( 6.22 mathrm{g} / mathrm{L} ) |
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| 702 | Calculate the equilibrium concentration ratio of ( boldsymbol{C} ) to ( boldsymbol{A} ) if equimolar ratio of ( A ) and ( B ) were allowed to come to equilibrium at ( 300 K ) ( boldsymbol{A}(boldsymbol{g})+boldsymbol{B}(boldsymbol{g}) leftrightharpoons boldsymbol{C}(boldsymbol{g})+ ) ( boldsymbol{D}(boldsymbol{g}) ; quad boldsymbol{Delta} boldsymbol{G}^{o}=-boldsymbol{8} boldsymbol{3} boldsymbol{0} boldsymbol{c a l} ) |
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| 703 | The ( left[boldsymbol{H}_{3} boldsymbol{O}^{+}right] ) in a solution having ( left[boldsymbol{O H}^{-}right]=mathbf{5} times mathbf{1 0}^{-mathbf{3}} boldsymbol{M} ) is: A ( cdot 2 times 10^{-3} ) B. ( 2 times 10^{-12} ) c. ( 5 times 10^{-3} ) D. none of these |
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| 704 | LV- 5101 – Q68. The solubility product constants of Ag, Cro, and AgBr are 1.1 X 10and 5.0 * 10 respectively. Calculate the ratio of molarities of their saturated solutions. |
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| 705 | Concentrated strong acid is added to a solid mixture of 0.015 mole samples of ( F e(O H)_{2} ) and ( C a(O H)_{2} ) placed in one litre of water. At what value of ( mathrm{pH} ) will the dissolution of each hydroxide be complete? (Assume negligible volume change) ( boldsymbol{K}_{s p}left[boldsymbol{F e}(boldsymbol{O H})_{2}right]=mathbf{7 . 9} times mathbf{1 0}^{-15} ) and ( boldsymbol{K}_{s p}left[boldsymbol{C u}(boldsymbol{O} boldsymbol{H})_{2}right]=mathbf{1 . 6} times mathbf{1 0}^{-19} ) A . 6.67 в. 7.86 ( c .8 .86 ) D. 7.26 |
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| 706 | The ( K_{a} ) value of ammonium ion ( left(N H_{4}+right) ) is ( 5.6 times 10^{-10}, ) the ( K_{b} ) value of ( operatorname{ammonia} N H_{3}=1.8 times 10^{-5}, ) then A. Ammonia is more strongly basic than ammonium is acidic B. Ammonia is weaker basic than ammonium is acidic c. Both a and ( b ) D. Data insufficient |
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| 707 | Q. 13 What will be the value of pH of 0.01 mol dm-3 CH,COOH (Ka = 1.74 x 10-5)? (a) 3.4 ond (6) 3.6 ton (c) 3.9 holland (d) 3.0 -5 |
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| 708 | 16. A buffer solution of pH = 9.00 is made by dissolving ammonium chloride and ammonia in water. How many moles of ammonium chloride must be added to 1.0 L of 0.25 M ammonia to prepare this buffer? NH,(aq) + H2O NH(aq) + OH-(aq); K, = 1.8 x 10-5 (a) 0.25 mol (b) 0.45 mol (c) 0.65 mol (d) 2.2 mol |
11 |
| 709 | Which of the following cations is not hydrolyzed in aqueous solution? (i) ( M g^{2+} ) ( (text { ii }) C a^{2+} ) ( (text { iii }) N a^{+} ) ( (text { iv }) boldsymbol{K}^{+} ) A. (i), (ii) B. (iii), (iv) c. (i), (ii), (iii), (iv) D. (i), (ii), (iii) |
11 |
| 710 | The characteristic properties of an acid is due to the presence of A. hydride ions B. hydroxyl ions c. hydronium ions D. oxide ions |
11 |
| 711 | Equilibrium constant for the given reaction is ( K=10^{20} ) at temperature ( mathbf{3 0 0} boldsymbol{K} ) ( boldsymbol{A}(s)+mathbf{2} boldsymbol{B}(boldsymbol{a} boldsymbol{q} .) rightleftharpoons mathbf{2} boldsymbol{C}(boldsymbol{s})+boldsymbol{D}(boldsymbol{a} boldsymbol{q} .) ) ( boldsymbol{K}=mathbf{1} mathbf{0}^{mathbf{2 0}} ) The equilibrium concentration of B starting with a mixture of 1 mol ( / ) lit of A and ( 1 / 3 m o l / l i t ) of ( B ) at ( 300 K ) is в. ( 2 times 10^{-1} ) c. ( 2 times 10^{-11} ) D. ( 10^{-10} ) |
11 |
| 712 | Find the correct graph regarding equilibrium state: ( A ) B. ( c ) D. All of these |
11 |
| 713 | When ( N O ) and ( N O_{2} ) are mixed, the following equilibrium are readily obtained, ( 2 N O_{2} rightleftharpoons N_{2} O_{4}, K_{p}= ) ( 6.8 a t m^{-1} ) and ( N O+N O_{2} rightleftharpoons N_{2} O_{3} . ) In an experiment when ( N O ) and ( N O_{2} ) are mixed in the ratio of ( 1: 2, ) the final total pressure was 5.05 at ( m ) and the partial pressure of ( N_{2} O_{4} ) was ( 1.7 a t m ) Calculate (a) the equilibrium partial pressure of ( N O,(b) K_{p} ) for: ( N O+ ) ( N O_{2} rightleftharpoons N_{2} O_{3} ) A ( .3 .43 a t m^{-1} ) B. ( 5.63 a t m^{-1} ) c. ( 7.43 a t m^{-1} ) D. None of these |
11 |
| 714 | The plot of ( log _{10} K_{p} ) against ( 1 / T ) for the reaction: [ boldsymbol{S O}_{2}(boldsymbol{g})+frac{1}{2} boldsymbol{O}_{2}(boldsymbol{g}) rightleftharpoons boldsymbol{S} boldsymbol{O}_{3}(boldsymbol{g}) ] is a straight line with slope ( =4.95 times ) ( 10^{3} . ) If the ( K_{p} ) at 25 if standard entropies for ( boldsymbol{S O}_{2}(boldsymbol{g}), boldsymbol{O}_{2}(boldsymbol{g}) ) and [ boldsymbol{S O}_{3}(boldsymbol{g}) text { are } mathbf{2 4 8 . 2}, mathbf{2 0 5 . 1} text { and } ] ( 256.8 J K^{-1} m o l^{-1} ) at 25 respectively is [ boldsymbol{K}_{boldsymbol{p}}=boldsymbol{X} times mathbf{1 0}^{11} text { then } mathbf{1 0} boldsymbol{X} ] is |
11 |
| 715 | Q5. (i) Define Le Chatelier’s principle. (ii) Following reactions occur in a Blast furnace. Fe,O3(s) + 3CO(g) 2Fe(s) + 3C02(8) use Le chatelier’s principle to predict the direction of reaction when equilibrium mixture is disturbed by (a) adding Fe,0, (b) removing CO, (c) removing Co. TAY . . |
11 |
| 716 | The equilibrium constant for the given reaction: ( boldsymbol{S O}_{3}(boldsymbol{g}) rightleftharpoons boldsymbol{S} boldsymbol{O}_{2}(boldsymbol{g})+ ) ( frac{1}{2} O_{2}(g) ; K_{c}=4.9 times ) ( 10^{-2} m o l^{1 / 2} l i t r e^{-1 / 2} ) What is the value of ( K_{c} ) for the reaction: ( 2 S O_{2}(g)+O_{2}(g) rightleftharpoons 2 S O_{3}(g) ? ) A. 416 litre ( m o l^{-1} ) B . ( 2.40 times 10^{-3} ) litre ( mathrm{mol}^{-1} ) c. ( 9.8 times 10^{-2} ) litre mole( ^{-1} ) D. ( 4.9 times 10^{-2} ) litre ( m o l^{-1} ) |
11 |
| 717 | When ( 0.2 M ) acetic acid is neutralised with ( 0.1 M ) NaOH in 0.5 litre of water the resulting solution is slightly alkaline. Calculate the pH of the resulting solution. ( boldsymbol{K}_{boldsymbol{a}} ) for ( boldsymbol{C H}_{3} boldsymbol{C O O H}=mathbf{1 . 8} times mathbf{1 0}^{-mathbf{5}} ) |
11 |
| 718 | The solubility curve of ( mathrm{KNO}_{3} ) as a function of temperature is given above The amount of ( mathrm{KNO}_{3} ) that will crystallize when a saturated solution of ( mathrm{KNO}_{3} ) in ( 100 mathrm{ml} ) of water is cooled from ( 90^{circ} mathrm{C} ) to ( 30^{circ} mathrm{C}, ) is ( A cdot 16 g ) B. 100 g ( c cdot 56 g ) D. 160 g |
11 |
| 719 | Which acid is present in the stinging hair of nettle leafs? | 11 |
| 720 | The ionisation constants of formic acid and ammonium hydroxide are ( 2 times 10^{-4} ) and ( 2 times 10^{-5} ) respectively. The pH of aqueous solution of ammonium formate is : ( A cdot 7 ) B. 6. c. 11.5 D. 8 |
11 |
| 721 | 1. Given that K, for HClO and HCN are 3.0 x 10-8 and 4.8 x 10-10, respectively, the equilibrium constant for the reaction HCIO(aq) + CN-(aq) C10 (aq) + HCN(aq), is (a) 6.3 x 101 (C) 1.6 x 1012 (6) 1.6 x 10-2 (d) 1.4 x 10-17 |
11 |
| 722 | Which of the following is the most acidic compound? A. ( C H_{2}=C H_{2} ) в. ( C H equiv C H ) c. D. |
11 |
| 723 | ( 0.25 mathrm{M} ) solution of pyridine chloride ( C_{5} H_{6} N^{+} C l^{-} ) was found to have a pH of 2.699. What is ( boldsymbol{K}_{boldsymbol{b}} ) for pyridine, ( boldsymbol{C}_{boldsymbol{5}} boldsymbol{H}_{boldsymbol{5}} boldsymbol{N} ) ? ( (log 2=0.3010) ) |
11 |
| 724 | The reactions ( boldsymbol{P C l}_{5}(boldsymbol{g}) rightleftharpoons boldsymbol{P C l}_{3}(boldsymbol{g})+ ) ( C l_{2}(g) ) and ( C O C l_{2}(g) rightleftharpoons C O(g)+ ) ( C l_{2}(g) ) are simultaneously in equilibrium in an equilibrium box at constant volume. A few moles of ( C O(g) ) are later introduced into the vessel. After some time, the new equilibrium concentration of A. ( P C l_{5} ) will remain unchanged B. ( C l_{2} ) will be greater c. ( P C l_{5} ) will become less D. ( P C l_{5} ) will become greater |
11 |
| 725 | Which of the following is a Lewis acid? A ( . H_{2} O ) в. ( C l^{circ} ) ( mathrm{c} cdot B F_{3} ) D. ( N H_{3} ) |
11 |
| 726 | For the reaction ( C O(g)+2 H_{2}(g) leftrightharpoons ) ( boldsymbol{C H}_{2} boldsymbol{O H}(boldsymbol{g}) . ) If active mass of ( boldsymbol{C O} ) is kept constant and active mass of ( boldsymbol{H}_{2} ) is tripled, the rate of forward reaction will become: A. three times B. six times c. eight times D. nine times |
11 |
| 727 | Which among following is electron pair acceptor? A. Arrhenius acid B. Arrhenius base c. Lewis acid D. Lewis base E. Bronsted-Lowry acid |
11 |
| 728 | Assertion ( K_{p} ) can be equal to or less than or even greater than the value of ( boldsymbol{K}_{c} ) Reason ( boldsymbol{K}_{boldsymbol{p}}=boldsymbol{K}_{boldsymbol{c}}(boldsymbol{R} boldsymbol{T})^{boldsymbol{Delta} boldsymbol{n}} ) the relation between ( boldsymbol{K}_{boldsymbol{p}} ) and ( boldsymbol{K}_{boldsymbol{c}} ) depends on the change in the number of moles of gaseous reactants and products. 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 |
11 |
| 729 | Find the ( p H ) of the resulting solution and then mark the option in which ( p H ) exists between color transition range of an indicator. ( 100 mathrm{ml} ) of ( 0.8 mathrm{M} mathrm{HCO}_{3}^{-}+100 mathrm{ml} ) of ( 0.4 mathrm{M} ) ( boldsymbol{C O}_{3}^{2-} ) [For ( boldsymbol{H}_{2} boldsymbol{C O}_{3}: boldsymbol{K}_{boldsymbol{a}_{1}}=boldsymbol{4} times mathbf{1 0}^{-boldsymbol{7}} boldsymbol{&} boldsymbol{K}_{boldsymbol{a}_{2}}= ) ( left.4 times 10^{-11}right] ) A. phenol red ( (6.8 text { to } 8.4) ) B. propyl red ( (4.6 text { to } 6.4) ) c. phenolphthalein ( (8.3 text { to } 10.1) ) D. Malachite green (11.4 to 13) |
11 |
| 730 | Oxidation number of ( C l ) in ( C a O C l_{2} ) (bleaching powder) is: A . zero, since it contains ( C l_{2} ) B. -1 , since it contains ( C l^{-} ) c. ( -1, ) since it contains ( C l O^{-} ) D. +1 and -1 since it contains ( C l O^{-} ) and ( C l^{-} ) |
11 |
| 731 | Simultaneous solubility of ( boldsymbol{A} boldsymbol{g} boldsymbol{C} boldsymbol{N} boldsymbol{S}(boldsymbol{a}) ) and ( A g B r(b) ) in a solution of water will be ( boldsymbol{K}_{s p_{(A g B r)}}=mathbf{5} times mathbf{1 0}^{-13} ) and ( boldsymbol{K}_{s p_{(A g C N S)}}= ) ( 10^{-12} ) A ( cdot a=4.08 times 10^{-7} ) mol litre ( ^{-1} ; b=8.16 times 10^{-7} ) mollitre ( ^{-1} ) В . ( a=4.08 times 10^{-7} ) mol litre ( ^{-1} ; b=4.08 times 10^{-7} ) mollitre ( ^{-1} ) ( mathbf{c} cdot a=8.16 times 10^{-7} )mollitre( ^{-1} ; b=4.08 times 10^{-7} )mollitre( ^{-1} ) D. None of these |
11 |
| 732 | Q4. PC15, PCl, and Cl, are at equilibrium at 500 K and having concentration 1.59M PCI, 1.59M Cl, and 1.41M PCI. Calculate Kc for the reaction PCI, = PC1, + Cl2 |
11 |
| 733 | Assertion: A mixture of ( C H_{3} ) COOH and ( C H_{3} C O O N H_{4} ) is not a buffer solution. Reason: An acidic buffer contains |
11 |
| 734 | What would be the ionisation constant ( left(boldsymbol{K}_{boldsymbol{a}}right) ) of ( boldsymbol{C H}_{3} boldsymbol{C O O H} ? ) A ( cdot 2 times 10^{-5} ) B ( cdot 10^{-5} ) C ( .2 times 10^{-6} ) D. ( 5 times 10^{-6} ) |
11 |
| 735 | A closed vessel contains helium and ozone at a pressure of ( mathrm{P} ) atm. The ratio of He and oxygen atoms is 1: 1 . If helium is removed from the vessel, the pressure of the sytem will reduced to: ( A cdot 0.5 P ) atm B. 0.75 P atm c. ( 0.25 mathrm{P} ) atm D. 0.33 P atm |
11 |
| 736 | The solubility product of a sparingly soluble salt ( A X_{2} ) is ( 3.2 times 10^{11} ). Its solubility (moles/litre) is: A ( .3 .1 times 10^{-4} ) B. ( 2 times 10^{3} ) c. ( 4 times 10^{-4} ) D. ( 5.6 times 10^{-6} ) |
11 |
| 737 | ( 0.02 M ) solution of ( N H_{4} O H ) is ( 3 % ) dissociated. Calculate the dissociation constant of ( boldsymbol{N} boldsymbol{H}_{mathbf{4}} boldsymbol{O} boldsymbol{H} ) |
11 |
| 738 | The precipitate of ( boldsymbol{C a} boldsymbol{F}_{2}left(boldsymbol{K}_{s p}=mathbf{1 . 7} timesright. ) ( left.10^{-10}right) ) is obtained when equal volumes of the following are mixed ( mathbf{A} cdot 10^{-4} M C a^{2+}+10^{-4} M F^{-} ) B. ( 10^{-2} M C a^{2+}+10^{-3} M F^{-} ) c. Both A and B D. None of these |
11 |
| 739 | Useful buffer range of weak acid ( boldsymbol{H} boldsymbol{A}left(boldsymbol{K}_{a}=mathbf{1 0}^{-5}right) ) is: ( mathbf{A} cdot 5 ) to 7 B. 4 to 6 c. 3 to 5 D. none of these |
11 |
| 740 | The function of ‘buffer solution’ is: A. to increase the pH value in chemical reaction B. to decrease the pH value on chemical reaction C. to increase or decrease the pH value of according the need D. to keep the pH value constante in chemical reaction |
11 |
| 741 | Which of the following is not a mineral acid? A. Hydrochloric acid B. Citric acid c. Sulphuric acid D. Nitric acid |
11 |
| 742 | ( 30 g m ) of ethanoic acid present in 100 ( g m ) of water, determine molality of ethanoic acid in water? | 11 |
| 743 | The element which is not common between the compounds called baking soda and soda ash is: A. nitrogen B. hydrogen c. oxygen D. sulphur |
11 |
| 744 | What concentration of ( boldsymbol{F}- ) ( boldsymbol{C H}_{2} boldsymbol{C O O H},left(boldsymbol{K}_{boldsymbol{a}}=boldsymbol{2} boldsymbol{6} times mathbf{1 0}^{-boldsymbol{3}}right) ) is needed so that ( left[boldsymbol{H}^{+}right]=mathbf{2} times mathbf{1 0}^{-mathbf{3}} ) ? A ( cdot 1.53 times 10^{-3} M ) В. ( 2.6 times 10^{-3} M ) c. ( 5.2 times 10^{-3} M ) D. ( 3.53 times 10^{-3} ) М |
11 |
| 745 | Bleaching powder is used: This question has multiple correct options A. for bleaching cotton, wood pulp B. as a disinfectant and germicide C. for the manufacture of chloroform D. as a reducing agent in industries |
11 |
| 746 | From the give options, which of the following compound will make best buffer solution? A. ( H_{2} O, 1 M ) NaOH, 1 M ( H_{2} ) SO ( _{4} ), в. ( H_{2} O, ) 1 ( M C H_{3} C O O H, 1 M N a^{+} C H_{3} C O O^{-} ) c. ( H_{2} O, 1 M C H_{3} C O O H, 6 M N a^{+} C H_{3} C O O^{-} ) D. ( H_{2} O, 1 M C H_{3} C O O H, 1 M N a O H ) |
11 |
| 747 | ( boldsymbol{K}_{boldsymbol{p}} ) for the reaction ( boldsymbol{N}_{mathbf{2}}(boldsymbol{g})+mathbf{3} boldsymbol{H}_{2}(boldsymbol{g}) rightleftharpoons ) ( 2 N H_{3}(g), ) at ( 298 K ) is ( 5.2 times 10^{-5} . ) What is the value of ( K_{c} ) at ( 298 K ), for the reaction ( frac{1}{2} N_{2}(g)+frac{3}{2} H_{2}(g) rightleftharpoons N H_{3}(g) ) |
11 |
| 748 | LLLLLLLLL LLCCC Q22. Bromine monochloride (BrCl) decomposes into bromine and chlorine and reaches the equilibrium: 2BrCl(3) – Br.(g) + C1,(g) The value of K is 32 at 500 K. If initially pure BrCl is present at a concentration of 3.3 10 mol L”, what is its molar concentration in the mixture at equilibrium? – 1 |
11 |
| 749 | Two equilibria, ( A B rightleftharpoons A^{+}+B^{-} . ) are simultaneously maintained in a solution with equilibrium constants, ( K_{1} ) and ( K_{2} ) respectively. The ratio of ( left[boldsymbol{A}^{+}right] ) to ( left[boldsymbol{A B}_{2}^{-}right] ) in the solution is: A. directly proportional to ( left[B^{-}right] ) B . inversely proportional to [ ( B^{-} ) C. directly proportional to the square of ( left[B^{-}right] ) D. inversely proportional to the square of ( left[B^{-}right] ) E. independent of ( left[B^{-}right] ) |
11 |
| 750 | 14. AGº for the reaction X+Y- Z is – 4.606 kcal. The equilibrium constant for the reaction at 227°C is: (a) 100 (b) 10 (c) 2 (d) 0.01 |
11 |
| 751 | The following equilibrium exists in aqueous solution: ( boldsymbol{C H}_{3} boldsymbol{C O O H} rightleftharpoons boldsymbol{H}^{+}+boldsymbol{C H}_{3} boldsymbol{C O O} ) If dilute ( H C l ) is added: A. The equilibrium constant will increase B. The equilibrium constant will decrease c. Acetate ion concentration will increase D. Acetate ion concentration will decrease |
11 |
| 752 | ( ln ) a reaction ( boldsymbol{A}+boldsymbol{B} rightleftharpoons boldsymbol{C}+boldsymbol{D}, ) the rate constant of forward reaction and backward reaction is ( K_{1} ) and ( K_{2}, ) then the equilibrium constant (K) for reaction is expressed as ( ^{mathrm{A}} cdot_{K_{c}}=frac{K_{2}}{K_{1}} ) в. ( K_{c}=frac{K_{1}}{K_{2}} ) ( mathbf{c} cdot K_{c}=K_{1} times K_{2} ) D. ( K_{c}=K_{1}+K_{2} ) |
11 |
| 753 | Which of the following substances has the lowest pH-value? A. Tomato B. Vinegar c. washing soda D. Human blood |
11 |
| 754 | For the following three reactions ( a, b, c ) equilibrium constants are given: 1. ( boldsymbol{C O}(mathbf{g})+mathbf{H}_{2} mathbf{O}(mathbf{g}) rightleftharpoons mathbf{C} mathbf{O}_{2}(mathbf{g})+mathbf{H}_{2}(mathbf{g}) ) ( ; mathbf{K}_{mathbf{1}} ) 2. ( mathbf{C H}_{4}(mathbf{g})+mathbf{H}_{2} mathbf{O}(mathbf{g}) rightleftharpoons mathbf{C O}(mathbf{g})+ ) ( mathbf{3} mathbf{H}_{mathbf{2}}(mathbf{g}) ; mathbf{K}_{mathbf{2}} ) 3. ( mathbf{C H}_{4}(mathbf{g})+mathbf{2} mathbf{H}_{mathbf{2}} mathbf{O}(mathbf{g}) rightleftharpoons mathbf{C} mathbf{O}_{mathbf{2}}(mathbf{g})+ ) ( mathbf{4} mathbf{H}_{mathbf{2}}(mathbf{g}) ; mathbf{K}_{mathbf{3}} ) Which of the following relations is correct? A ( cdot mathrm{K}_{3}=mathrm{K}_{1} mathrm{K}_{2} ) в. ( mathrm{K}_{3} cdot mathrm{K}_{2}^{3}=mathrm{K}_{1}^{2} ) c. ( mathrm{K}_{1} sqrt{mathrm{K}_{2}}=mathrm{K}_{3} ) D. ( mathrm{K}_{2} mathrm{K}_{3}=mathrm{K}_{1} ) |
11 |
| 755 | When HCl gas is passed through a saturated solution of common salt, pure NaCl is precipitated because A. HCl is highly ionised in solution B. HCl is highly soluble in water C. The solubility product of NaCl is lowered by HC D. The ionic product of ( left[N a^{+}right]left[C l^{-}right] ) exceeds the solubility product of NaCl |
11 |
| 756 | The rate constant for the forward reaction ( boldsymbol{A}(boldsymbol{g}) rightleftharpoons 2 boldsymbol{B}(boldsymbol{g}) ) is ( 1.5 times ) ( 10^{-3} s^{-1} ) at ( 100 mathrm{K} ). If ( 10^{-5} ) moles of ( mathrm{A} ) and 100 moles of ( mathrm{B} ) are present in a 10 litre vessel at equilibrium then rate constant for the backward reaction at this temperature is: ( begin{array}{ll}text { A } cdot 1.50 times 10^{4} L & text { mol- }^{-1} s^{-1}end{array} ) В. ( 1.5 times 10^{11} L quad ) mol ( ^{-1} s^{-1} ) C. ( 1.5 times 10^{10} L quad ) mol ( ^{-1} s^{-1} ) D. ( 1.5 times 10^{-11} L quad ) mol ( ^{-1} s^{-1} ) |
11 |
| 757 | For the system ( 3 A+2 B rightarrow 2 C ), the expression for equilibrium constant ( boldsymbol{K} ) is: A ( cdot frac{[3 A] times[2 B]}{[C]} ) B. ( frac{[A]^{3} times[B]}{[C]} ) c. ( frac{[C]^{2}}{[A]^{3} times[B]^{2}} ) D. ( frac{[C]}{[3 A] times[2 B]} ) |
11 |
| 758 | If ( S_{0}, S_{1}, S_{2} ) and ( S_{3} ) are the solubilities in water of ( boldsymbol{A} boldsymbol{g} boldsymbol{C l} ) ( mathbf{0 . 0 1} boldsymbol{M} boldsymbol{C a C l}_{2}, mathbf{0 . 0 1} boldsymbol{M} boldsymbol{N a C l} ) and ( mathbf{0 . 5} boldsymbol{M} boldsymbol{A} boldsymbol{g} boldsymbol{N} boldsymbol{O}_{3} ) solutions, respectively then which of the following is true? A ( . S_{0}>S_{2}>S_{1}>S_{3} ) B. ( S_{0}=S_{2}=S_{1}>S_{3} ) c. ( S_{3}>S_{1}>S_{2}>S_{0} ) D. none of these |
11 |
| 759 | The pH of solution containing ( 0.10 M ) sodium acetate and ( 0.03 M ) acetic acid is: ( left(p K_{a} text { for } C H_{3} C O O H=4.57right) ) A . 4.09 B. 6.09 c. 5.09 D. 7.09 |
11 |
| 760 | In the following reaction: ( 2 S O_{2}(g)+O_{2}(g) rightleftharpoons 2 S O_{3}(g) ) the equilibrium is not attained. The rate of forward reaction is greater than that of backward reaction. Thus, which of the following is the correct relation between ( boldsymbol{K}_{boldsymbol{p}} ) and ( boldsymbol{Q}_{boldsymbol{p}} ? ) ( mathbf{A} cdot K_{p}=Q_{p} ) B ( cdot Q_{p}>K_{p} ) ( mathbf{c} cdot Q_{p}<K_{p} ) D. ( K_{p}=Q_{p}=1 ) |
11 |
| 761 | The concentration of ( left[boldsymbol{H}^{+}right] ) and ( [boldsymbol{O H}]^{-} ) in a 0.1 M aqueous solution of ( 2 % ) ionised weak monobasic acid is ( left[text { ionicproducto fwater }=1 times 10^{-14}right] ) A ( cdot 0.02 times 10^{-3} ) M and ( 5 times 10^{-11} ) M B. ( 1 times 10^{-3} ) M and ( 3 times 10^{-11} ) M C . ( 2 times 10^{-3} ) M and ( 5 times 10^{-12} ) M D. ( 3 times 10^{-2} ) M and ( 4 times 10^{-13} ) M |
11 |
| 762 | The solubility product of ferric hydroxide in aqueous solution is ( 6 times ) ( 10^{-38} ) at ( 298 K . ) The solubility of ( F e^{3+} ) ion will increase when the: ( mathbf{A} cdot p H ) is increased B. ( p H ) is 7.0 c. ( p H ) is decreased D. saturated solution is exposed to the atmosphere |
11 |
| 763 | For the reaction ( 2 S O_{2}+O_{2} rightleftharpoons 2 S O_{3} ) the unit of ( boldsymbol{K}_{c} ) A. litre/mole B. mol/litre c. ( left(text {mol litre}^{-1} text {) }^{-1}right. ) D cdot (litre mole ( ^{-1} ) ) ( ^{2} ) |
11 |
| 764 | Assume that the decomposition of ( H N O_{3} ) can be represented by the following equation: ( 4 boldsymbol{H} boldsymbol{N} boldsymbol{O}_{boldsymbol{3}}(boldsymbol{g}) rightleftharpoons ) ( 4 N O_{2}(g)+2 H_{2} O(g)+O_{2}(g) ) The reaction approaches equilibrium at ( 400 mathrm{K} ) temperature and ( 30 mathrm{atm} ) pressure. At equilibrium, the partial pressure of ( H N O_{3} ) is 2 atm. The value of ( boldsymbol{K}_{c}left((boldsymbol{m o l} / boldsymbol{L})^{3}right) ) at ( 400 mathrm{K} ) is: (Use ( : boldsymbol{R}=.08 a t boldsymbol{m}-boldsymbol{L} / boldsymbol{m} boldsymbol{o l} boldsymbol{e}-boldsymbol{K}) ) |
11 |
| 765 | A sample of ( A g C l ) was treated with ( 5 m L ) of ( 1.5 M N a_{2} C O_{3} ) solution to ( operatorname{give} A g_{2} C O_{3} . ) The remaining solution contained ( 0.0026 g C l^{-} ) per litre Calculate the solubility product of ( A g C l ) ( left(boldsymbol{K}_{s p}left(boldsymbol{A} boldsymbol{g}_{2} boldsymbol{C O}_{3}right)=boldsymbol{8} cdot boldsymbol{2} times mathbf{1 0}^{-12}right) ) |
11 |
| 766 | Q. 14 K, for CH2COOH is 1.8 x 10-5 and K, for NH,OH is 1.8 x 10-5. The pH of ammon |