# Solutions Questions

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#### List of solutions Questions

Question NoQuestionsClass
1Henry’s law constant for the solubility of
( N_{2} ) gas in water at ( 298 mathrm{K} ) is ( 1.0 times 10^{5} )
atm. The mole fraction of ( N_{2} ) in air is 0.6
The number of moles of ( N_{2} ) from air
dissolved in 10 moles of water at ( 298 mathrm{K} )
and 5 atm pressure is:
A ( .3 .0 times 10^{-4} )
В. ( 4.0 times 10^{-4} )
c. ( 5.0 times 10^{-4} )
D. ( 4.0 times 10^{-5} )
12
2One litre hard water contains ( 1 mathrm{mg} )
( mathrm{CaCl}_{2} ) and ( 1 mathrm{mg} M mathrm{g} S mathrm{O}_{4} ). The hardness
of water is:
A . 1.743 ppm
в. 1.745 ppm
c. 1.734 ppm
D. none of the above
12
32.51 Assertion (A) Molarity of a solution in liquid state changes with
temperature.
Reason (R) The volume of a solution changes with change in temperature.
12
4( X, Y ) and ( Z ) in the given graph are?
A. ( X=p_{1}+p_{2}, Y=1, Z=0 )
B . ( X=p_{1}+p_{2}, Y=0, Z=0 )
C ( cdot X=p_{1} times p_{2}, Y=0, Z=0 )
D. ( X=p_{1}-p_{2}, Y=1, Z=0 )
12
5Among ( 0.1 ~ M ) solutions of
( N a C l, C a C l_{2} ) and ( A l_{2}(S O)_{3}, ) the one with highest vapour pressure is:
A ( . N a C l )
в. ( C a C l_{2} )
c. ( A l_{2}(S O)_{3} )
D. All have equal vapour pressure
12
6Vapour pressure of water at certain
temperature is ( 155 mathrm{mm} ) Hg and that of the another solvent ‘X’ is ‘p’ mm Hg. Molecular weight of ‘X’ is 128. An
aqueous solution of ‘X'(64% by wt) has
a vapour pressure of ( 145 mathrm{mm} ) Hg. What is ‘p’?
12
7Given below are few mixtures formed by mixing two components. Which of the following binary mixtures will have same composition in liquid and vapour phase?
(i) Ethanol ( + ) Chloroform
(ii) Nitric acid + Water
(iii) Benzene + Toluene
(iv) Ethyl chloride ( + ) Ethyl bromide
A. (i) and (iii)
B. (i) and (ii)
c. (i), (ii) and (iii)
D. (iii) and (iv)
12
8What is the molality of a solution containing ( 200 m g ) of urea (molar mass
( 60 g m o l^{-1} ) ) dissolved in ( 40 g ) of water?
A . 0.0833
B. 0.825
c. 0.498
D. 0.0013
12
9A mixture of volatile components ( A ) and B has total vapour pressure (in torr) as ( boldsymbol{P}=mathbf{2 5 4}-mathbf{1 1 9} chi_{A}, ) where ( chi_{A} ) is the
mole fraction of ( A ) in the mixture. Hence,
( P_{A}^{o} ) and ( P_{B}^{o} ) respectively are (in torr):
A. 254,119
в. 119,254
C. 135,254
D. 154, 119
12
10State True or False.
Lowering of vapour pressure is proportional to the mole fraction of the solute.
A. True
B. False
12
11Two liquids ( A ) and ( B ) form type II non ideal solution which shows a minimum
in its temperature-mole fraction plot ( T-chi text { diagram }) . ) Can the two liquids be
completely separated by fractional distillation?
12
12Q. 6 If the concentration of glucose (CGH206) in blood is 0.9 g L”, what will
be the molarity of glucose in blood?
(a) 5M
(b) 50 M
(c) 0.005 M (d) 0.5 M
12
13Van’t Hoff factor for ( boldsymbol{T} boldsymbol{H}left(boldsymbol{N} boldsymbol{O}_{3}right)_{4} ) in an
aqueous solution is :
12
14Illustration 2.66 Can we separate the components of
azeotropic mixture by distillation?
12
15Does a new substance form when a
solute dissolves in a solvent?
12
16Which of the following conditions are correct for real solutions showing negative deviation from Raoult’s law?
A ( cdot Delta H_{M i x}0 )
B. ( Delta H_{M i x}>0 ; Delta V_{M i x}>0 )
c. ( Delta H_{M i x}>0 ; Delta V_{M i x}<0 )
D. ( Delta H_{M i x}<0 ; Delta V_{M i x}<0 )
12
17An ideal aqueous solution containing liquid ( boldsymbol{A}(M cdot W boldsymbol{t}=mathbf{1 2 8}) mathbf{6 4 %} ) by weight
has a vapour pressure of ( 145 m m H g ). If
the vapour pressure of ( boldsymbol{A} ) is ( boldsymbol{x} ) mm of ( H g ) and that of water is ( 155 m m H g ) at the same temperature. Then find ( frac{x}{5} . ) The solutions is ideal.
12
18When mercuric iodide is added to an
aqueous solution of ( K I ) then:
A. boiling point increase
B. boiling point decrease
c. freezing point increase
D. osmotic pressure increase
12
19The vapour pressure of solution at 293
( mathrm{K} )
A .0 .0229
B. 0.4
( c .0 .6 )
D. 0.9
12
20( 0.124 g m ) of an organic compound containing phosphorus gave ( 0.222 g m )
of ( M g_{2} P_{2} O_{7} ) the usual analysis.
Calculate the percentage of phosphorous in the compound. ( (M g= )
( mathbf{2 4}, boldsymbol{P}=mathbf{3 1}) )
A .25
в. 15
( c .62 )
D. 50
12
21When a solution is diluted at constant
temperature, its vapour pressure:
A. increases
B. decreases
c. remains same
D. may increase or decrease
12
22At ( 100^{circ} mathrm{C} ), benzene ( & ) toluene have
vapour pressure of ( 1375 & 558 ) Torr
respectively. Assuming these two form an ideal binary solution, calculate the composition of Ithe solution that boils
at 1 atm ( & 100^{circ} mathrm{C} ). What is the
composition of vapour issuing at these conditions?
A . ( x_{b}=0.2472, Y_{b}=0.4473 )
B. ( x_{b}=0.4473, Y_{b}=0.2472 )
c. ( x_{b}=0.362, Y_{b}=0.321 )
D. None of these
12
23Calculate the mole fraction of glucose in an aqueous solution that contains 45 g of glucose in 45 g of water. Find out the weight of NaOH required to be disolved in 90 g of water in order to get a solution of the same mole fraction.
A ( cdot frac{1}{11}, 20 g )
в. ( frac{1}{11}, 10 g )
c. ( frac{1}{10}, 10 g )
D. ( frac{1}{10}, 20 g )
12
24is measured in moles per
litre.
A. Molality
B. Molar concentration
c. Number of moles
D. None of these
12
25Q. 30 van’t Hoff factor (i) is given by the expression
(a) – normal molar mass
(b); – abnormal molar mass
abnormal molar mass
normal molar mass
observed colligative property
(d) i =
calculated colligative property
calculated colligative property observed colligative property
(C)=
12
26Illustration 2.200 To 250 mL of water, x g of acetic acid is
added. If 11.5% of acetic acid is dissociated, the depression
in freezing point comes out 0.416. What will be the value of
x if K. (water) = 1.86 K kg- mol-1 and density of water is
0.997 g mL-1
12
27has the highest boiling
point.
A. ( 0.2 mathrm{m} mathrm{CaCl}_{2} )
B. 0.2 ( mathrm{m} ) NaCl
c. ( 0.1 mathrm{m} ) Al ( C l_{3} )
D. ( 0.2 mathrm{m} mathrm{CH}_{3} mathrm{OH} )
E. ( 0.2 mathrm{m} mathrm{NaC}_{2} mathrm{H}_{3} mathrm{O}_{2} )
12
28Write the formula to calculate the
molality.
12
29Which of the following solution in water will have the lowest vapour pressure?
A. ( 0.1 M, ) NaCI
B. ( 0.1 M, ) Sucrose
с. ( 0.1 M, )ВаС( I_{2} )
D. ( 0.1 M N a_{3} P O_{4} )
12
30The van’t Hoff factor of ( 0.005 M )
aqueous solution of ( K C l ) is ( 1.95 . ) The
degree of ionisation of ( K C l ) is:
A . 0.95
В. 0.97
( c .0 .94 )
D. 0.96
12
31The Henry’s law constant for the
solubility of ( mathbf{N}_{2} ) gas in water at ( mathbf{2 9 8 K} ) is
( 1.0 times 10^{5} ) atm. The mole fraction of ( mathbf{N}_{2} )
in air is ( 0.8 . ) The number of moles of ( mathbf{N}_{2} )
from air dissolved in 10 moles of water
at ( 298 mathrm{K} ) and 5 atm pressure is:
A ( cdot 4.0 times 10^{-4} )
В. ( 4.0 times 10^{-5} )
c. ( 5.0 times 10^{-4} )
D. ( 4.0 times 10^{-6} )
12
32Question 1. Calculate the mass percentage of benzene (CH) and
carbon tetrachloride (CC14) if 22 g of benzene is dissolved in 122 g carbon
tetrachloride.
(0) We have mass of CH6 and CCIA, so calculate the mass of solution by
(ii) Then, calculate the mass percentage from the formula,
Mass of one component 100
Mass %=
Mass of solution
12
33The density of ( 3 M ) solution of sodium
thiosulphate ( left(N a_{2} S_{2} O_{3}right) ) is ( 1.56 g / m L )
Calculate
(i) amount of ( N a_{2} S_{2} O_{3} ) in ( % ) w/w
(ii) mole fraction of ( N a_{2} S_{2} O_{3} )
(iii) Molality of ( N a^{+} ) and ( S_{2} O_{3}^{2-} ) ions
12
34Mustration 2.104 Define molal depression constant or
cryoscopic constant.
12
35For dilute solution, Raoult’s law states
that:
A. the relative lowering of vapour pressure is equal to mole fraction of solute
B. the vapor pressure of the solution is equal to mole fraction of the solvent
C. the relative lowering of vapour pressure is proportional to amount of solute
D. the lowering of vapor pressure is equal to the mole fraction of solute in solution
12
36A sample of ( boldsymbol{H}_{2} boldsymbol{O}_{2} ) solution labelled as
28 volume has density of 265 g/L. Mark the correct option(s) representing concentration of same solution in other
units.
This question has multiple correct options
A. Molarity of ( H_{2} O_{2}=2.5 )
B. Percentage ( w / v=17 )
C. Mole fraction of ( H_{2} O_{2}=0.2 )
D. Molality of ( H_{2} O_{2}=13.88 )
12
37Distinguish between the saturated and unsaturated solution using the data given below:
a) 16 g ( N a C l ) in 100 g water.
b) 36 g ( N a C l ) in 100 g water (Note – Solubility of ( N a C l ) is ( 36 g ) )
12
387. Increasing amount of solid Hgl, is added to 1 L of an
aqueous solution containing 0.1 mol KI. Which of the
following graphs do represent the variation of freezing
point of the resulting with the amount of Hgl, added?
a. If
b. If
0.05 0.10
Mol of Hgl2 →
0.05 0.10
Mol of Hgl2 →
c. Te
d. Tf
0.05 0.10
Mol of Hgl2 –>
0.05 0.10
Mol of Hgl2 ->
12
39Raoult’s law is obeyed by each
constituent of a binary liquid solution
when:
A. the forces of attractions between like molecules are greater than those between unlike molecules
B. the forces of attractions between like molecules are
smaller than those between unlike molecules
C. the forces of attractions between like molecules are identical with those between unlike molecules
D. the volume occupied by unlike molecules are different
12
40A plant cell shrinks when it is kept in a?
A. hypotonic solution
B. hypertonic solution
C. isotonic solution
D. pure water
12
41Which of the following solutions shows positive deviation from Raoult’s law?
A. Acetone + Aniline
B. Acetone + Ethanol
c. water + Nitric acid
D. Chloroform + Benzene
12
42How many grams of sucrose must be
added to ( 320 g ) of water to lower the
vapour pressure by ( 1.5 m m H g ) at ( 25^{circ} C )
( ? )
(Given: The vapour pressure of water at
( 25^{circ} mathrm{C} ) is ( 23.8 mathrm{mm} ) Hg and molar mass
of sucrose is ( 324.3 g / m o l ) )
A. ( 21.5 g )
в. ( 140 g )
c. ( 363.36 g )
D. ( 160.12 g )
12
43Which of the following aqueous solutions will have maximum freezing point. [Assume dilute solutions]
A. ( C_{6} H_{5} N H_{3} C I ) solution having ( 0.01 m )
B. ( C aleft(N O_{3}right)_{2} ) solution having ( 0.005 m )
C. ( A Ileft(N O_{3}right)_{3} ) solution having ( 0.004 m )
D. Glucose solution having ( 0.04 mathrm{m} )
12
44The freezing point of mercury is:
( A cdot 100 K )
в. 234.3 к
c. ( 123.5 mathrm{k} )
D. 450 K
12
45On increase of temperature, a saturated solution converts into
solution.
12
46Assertion
Aquatic species are more comfortable in warm waters than cold waters.
Reason
( boldsymbol{K}_{boldsymbol{H}} ) values for both ( boldsymbol{N}_{2} ) and ( boldsymbol{O}_{2} )
decrease with increase of temperature.
A. Both Assertion and Reason are correct and Reason is the correct explanation for Assertion
B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion
c. Assertion is correct but Reason is incorrect
D. Both Assertion and Reason are incorrect
12
47The fundamental cause of all colligative properties is:
A. higher entropy of the solution relative to that of pure solvent
B. lower entropy of the solution relative to that of pure solvent
c. higher enthalpy of the solution relative to that of pure solvent
D. lower enthalpy of the solution relative to that of pure solvent
12
48The vapour pressure of two liquids ‘P and ‘Q’ are 80 and 60 torr, respectively.
The total vapour pressure of solution obtained by mixing 3 mole of ( P ) and 2 mole of Q would be:
A. 68 torr
B. 140 torr
c. 72 torr
D. 20 torr
12
49Q. 6 Low concentration of oxygen in the blood and tissues of people living at
high altitude is due to …..
(a) low temperature
(b) low atmospheric pressure
(c) high atmospheric pressure
(d) Both low temperature and high atmospheric pressure
f
lo linat high altitudin
12
50Illustration 2.134 Given that the latent heat of fusion of
naphthalene is 19.0 kJ mol-1 and its melting point is 80.2°C.
Estimate the solubility of naphthalene in benzene at 76.2°C.
12
51Van’t Hoff factor of ( boldsymbol{H} boldsymbol{g}_{2} boldsymbol{C l}_{2} ) in its
aqueous solution will be ( left(H g_{2} C l_{2} ) is right. ( 80 % ) ionized in the solution):
A . 1.6
B . 2.
( c .3 .6 )
D. 4.6
12
52Hlustration 2.91 12.2 g of benzoic acid is dissolved in
(i) 1 kg acetone (K6 = 1.9 K kg mol-1) and (ii) 1 kg benzene
(K) = 2.6 K kg mol-1).
The elevations of boiling points are 0.19°C and 0.13°C,
respectively.
a. What are the molar masses of benzoic acid in the two
solutions?
b. What are the structures of benzoic acid in the two
solutions?
12
53Illustration 2.160 The osmotic pressure of decimolar
solution of urea at 27°C is
a. 2.49 bar b. 5 bar c. 3.4 bar d. 1.25 bar
12
54The ammonia evolved from the
treatment of ( 0.30 g ) of an organic compound for the estimation of nitrogen was passed in 100 m ( L ) of 0.1 ( M ) sulphuric acid. The excess of acid required ( 20 m L ) of 0.5 sodium hydroxide solution hydroxide solution for complete neutralization. The organic compound is:
A. acetamide
B. thiourea
c. urea
D. benzamide
12
55I. A ( 2 M ) solution of urea ( left(C H_{4} N_{2} Oright) )
can be prepared by dissolving 1 mole of
urea in ( 500 m L ) of water.
II. Urea is a non-polar molecular compound
A. Statement ( I ) is true, Statement ( I I ) is true
B. Statement I is true, Statement II is false
c. statement ( I ) is false, statement ( I I ) is true
D. Statement I is false, Statement II is false
12
56The vapour pressure of a mixture of
diethyl aniline and water is ( 1.013 times ) ( 10^{5} N m^{-2} ) at ( 99.4^{circ} C . ) The vapour
pressure of water at this temperature is
( 0.992 times 10^{5} N m^{-2} . ) The grams of steam
are necessary to distill over 100 g of diethylaniline are (write answer as nearest integer after dividing by 60 ).
12
57On diluting solution, its normality and molarity changes but molality remains
constant.
A. True
B. False
12
588. The vapour pressure of pure benzene C H at 50°C is 268
torr. How many moles of non-volatile solute per mole
of benzene are required to prepare a solution of benzene
having a vapour pressure of 167 torr at 50°C?
a. 0.377 b. 0.605 c. 0.623 d. 0.395
12
59Density of ( 2.03 M ) aqueous solution of
acetic acid is ( 1.017 g m L^{-1} ) molecular mass of acetic is ( 60 . ) Calculate the
molality of the solution.
A . 2.27
B. 1.27
c. 3.27
D. 4.27
12
60If the Vant Hoff factor for ( mathbf{0 . 1} mathbf{M} )
( B aleft(N O_{3}right)_{2} ) solution is 2.74 , the degree of dissociation is:
A . 0.87
в. 0.74
c. 0.91
D. 87
12
61Q. 8 Colligative properties depend on ……..
(a) the nature of the solute particles dissolved in solution
(b) the number of solute particles in solution
(C) the physical properties of the solute particles dissolved in solution
(d) the nature of solvent particles
12
62toppr
Assurite muldy unly A 2 anu ( cup cup 2 ) art
present
( A )
B.
( c )
( D )
12
63At ( 300 mathrm{K}, 36 mathrm{g} ) of glucose present per litre in its solution has an osmotic
pressure of 4.98 bar. If the osmotic
pressure of the solution is 1.58 bar at
the same temperature, what would be its concentration?
12
64A solution is made by dissolving 49 g of ( H_{2} S O_{4} ) in ( 250 mathrm{mL} ) of water. The molarity
of solution prepared is:
( A cdot 2 M )
в. 1
( c cdot 4 M )
D. 5 M
12
65The Henry’s law constant for the
solubility of ( N_{2} ) gas in water at ( 298 K ) is ( 1 times 10^{5} ) atm. The mole fraction of ( N_{2} ) in
air is ( 0.8 . ) Calculate the number of
moles of ( N_{2} ) dissolved in 10 moles of
water at ( 298 K ) and 5 atm.
A ( cdot 5 times 10^{-4} )
В. ( 3 times 10^{-5} )
c. ( 4 times 10^{-4} )
D. ( 4 times 10^{-5} )
12
66Mustration 2.51 Why is an increase in temperature
observed on mixing chloroform with acetone?
12
67If the molar concentration of ( boldsymbol{P b I}_{2} ) is
( 1.5 times 10^{-3} ) mol ( L^{-1}, ) then the
concentration of iodide ions of ( g ) ion ( L^{-1} )
is ?
A. ( 3.0 times 10^{-3} )
В. ( 6.0 times 10^{-3} )
c. ( 0.3 times 10^{-3} )
D. ( 0.6 times 10^{-6} )
12
68Ways of expressing the concentration of
a solution are:
( frac{text {Mass of solute}}{text {Mass of solution}} times 100 )
II) ( frac{text { Mass of solute }}{text {Volume of solution}} times 100 )
( A )
B. I
( c cdot 1,1 )
D. none of the above
12
69( 20 mathrm{ml} ) of ( 0.2 mathrm{M} A l_{2}left(S O_{4}right)_{3} ) is mixed with
( 20 mathrm{ml} ) of ( 6.6 mathrm{M} mathrm{BaCl}_{2} ), the concentration
of ( C l^{-} ) in solution is:
A. ( 0.2 mathrm{M} )
B. 6.6 ( M )
c. ( 0.02 mathrm{M} )
D. 0.06 м
12
70Which of the following aqueous solutions will exhibit the highest boiling point?
A . ( 0.01 M ) urea
в. ( 0.01 M ) К ( N O_{3} )
c. ( 0.01 M ) Na( _{2} ) SO ( _{4} ),
D. ( 0.015 M C_{6} H_{12} O_{6} )
12
71Which of the following units can be used to represent solubility?
( mathbf{A} cdot mathbf{g} )
B. mol
c. ( m o l / L )
( mathbf{D} cdot m L / s )
12
72Two liquids ( X ) and ( Y ) from an ideal
solution. At ( 300 K, ) a vapour pressure of
the solution containing 1 mol of ( X ) and
3 mol of ( Y ) is 550 mm ( H g . ) At the same
temperature, if 1 mol of ( Y ) is further
added to this solution, a vapour
pressure of the solution increased by 10
mm Hg. Vapour pressure ( in mmHg) of
( X ) and ( Y ) in their pure states will be
respectively:
A. 300 and 400
B. 400 and 600
c. 500 and 600
D. 200 and 300
12
73Which substance has a higher solubility in cold water and a lower
solubility in hot water?
A. Licl
( mathbf{B} cdot C a(O H)_{2} )
( c cdot C O_{2} )
D. ( C_{6} H_{12} O_{6} )
12
74A solution containing ( 30 g ) of a nonvolatile solute in exactly ( 90 g ) water has a vapour pressure of 21.85 mm ( H g ) at
( 25^{circ} mathrm{C} . ) Further 18 gm of water is then added to the solution. The resulting solution has a vapour pressure of 22.18 ( mathrm{mmHg} ) at ( 25^{circ} mathrm{C} ). Calculate
(a) molar mass of the solute, and (b) vapour
pressure of water at ( 25^{circ} mathrm{C} )
В. ( (a) 61.21 g ) тод( ^{-1} ),
(b) 23.99 ( mathrm{mm} ) Н ( g )
( (b) 28.87 mathrm{mm} mathrm{Hg} )
D. ( (a) 84.87 g ) mol ( ^{-1} ),
12
75Example 2.8 Two liquids A and B form an idea solution.
What will be the vapour pressure at 27°C of a solution having
1.5 mol of A and 4.5 mol of B? The vapour pressure of A and
B at 27°C is 0.116 atm and 0.140 atm, respectively.
12
76A Mixture of nitrogen and oxygen has a density of ( 1.00 g / 1 ) and the average
molecular weight ( left(M_{a y}right) ) of ( 31.2 g ) at
( 27^{circ} C ) and ( 600 mathrm{mm} ) Hg per mole pressure
What is the mole fraction of nitrogen? (Assume ideal gas behavior)
A . 0.8
B. 0.6
( c .0 .4 )
D. 0.2
12
77Determine the osmotic pressure of a solution prepared by dissolving ( 2.5 times ) ( 10^{-2} g ) of ( K_{2} S O_{4} ) in ( 2 L ) of water at 25
assuming that it is completely dissociated
( left(R=0.0821 L operatorname{atm} K^{-1} m o l^{-1}, ) Molar right.
( operatorname{mass} ) of ( K_{2} S O_{4}=174 mathrm{g} m o l^{-1} ) ).
12
78By dissolving 13.6 g of a substance in 20 ( g ) of water, the freezing point decreased
by ( 3.7^{circ} mathrm{C} ). Calculate the molecular mass
of the substance.
(Molal depression constant for water = ( 1.863 mathrm{K} mathrm{kg} mathrm{mol}^{-1} ) )
12
79The equation of the curve obtained by connecting all those points where the vapors of above mixture (all mixtures of
different composition are taken) just start forming will be
A ( cdot P=P_{C}^{o}+left(P_{B}^{o}-P_{C}^{o}right) X_{B}^{l} )
B . ( P=P_{B}^{o}+left(P_{B}^{o}-P_{C}^{o}right) X_{B}^{l} )
( ^{mathrm{c}} cdot p=frac{P_{B}^{o} P_{C}^{o}}{X_{B}^{o}left(P_{C}^{o}-P_{B}^{o}right)+P_{B}^{o}} )
D. ( P=frac{P_{B}^{o} P_{C}^{o}}{X_{B}^{l}left(P_{C}^{o}-P_{B}^{o}right)+P_{B}^{o}} )
12
80A sample of drinking was found to be severely contaminated with chloroform,
( C H C l_{3}, ) supposed to be a carcinogen
The level of contamination was 15 ppm
(by mass). Express this in percent by
mass.
A. ( 1.5 times 10^{-3} )
В. ( 4.0 times 10^{-3} )
c. ( 6 times 10^{-3} )
D. ( 0.75 times 10^{-3} )
12
81The solution showing positive deviation from ideal behaviour has
azeotrope.
A. negative
B. positive
c. neutral
D. ideal
12
82State true or false.
1 ppm is equal to 1 mg per ( mathrm{kg} )
A. True
B. False
12
83Define an ideal solution12
84The experiment value for the molar mass of a non-volatile solute is twice
the theoretic value. What is Vant Hoff
factor for the solute?
12
85Vapour Pressure of a mixture of
benzene and toluene is given by ( boldsymbol{P}= )
( mathbf{1 7 9 X}_{B}+mathbf{9 2}, ) Where ( boldsymbol{X}_{B} ) is mole
fraction of benzene.
If Vapours are removed and condensed
in to liquid then what will be the ratio of mole fraction of benzene and toluene in
first condensate:
A . 2.8
B. 1.5
c. 3.
D. 4.5
12
86A gas mixture contains ( 24 % ) nitrogen, ( 32 % ) oxygen and remaining is hydrogen by volumes at a given temperature and pressure then what is the mole fraction
of hydrogen? (assume there is no reaction between
the gases)
A .0 .44
B. 0.24
c. 0.91
D. 0.56
12
87How many ( N a^{+} ) ions are present in
( 100 m L ) of ( 0.25 M ) of ( N a C l ) solution?
A. ( 0.25 times 10^{23} )
В. ( 1.505 times 10^{22} )
C. ( 15 times 10^{22} )
D. ( 2.5 times 10^{23} )
12
88The vapour pressure of water at ( 20^{circ} mathrm{C} ) is
17.54 ( m m H g ). Then the vapour pressure
of the water in the apparatus is lowered, decreasing the volume of the gas above the liquid to one half of its initia
volume (temp. constant) is:
A. ( 5.77 mathrm{mmHg} )
в. ( 16 mathrm{mmHg} )
c. 35.08 mmHg
D. between 8.77 and ( 15.54 mathrm{mmHg} )
12
89Equal weights of mercury and ( l_{2} ) are allowed to react completely to form a mixture of mercurous and mercuric
iodide leaving none of the reactants. Calculate the ratio of the weights of
( H g_{2} l_{2} ) and ( H g l_{2} ) formed
A . 1: 0653
B . 0.732: 1
c. 1: 0.523
D. 0.532: 1
12
90The quantity of solute dissolved in a given mass or volume of the solution is called:
A. parameter of solution
B. concentration of solution
c. similarity of solution
D. massive mass
12
91At a particular temperature, the vapour pressures of two liquids ( A ) and ( B ) are respectively 120 and 180 mm of
mercury. If 2 moles of ( A ) and 3 moles of
Bare mixed to form an ideal solution,
the vapour pressure of the solution at the same temperature will be (in mm of
mercury) :
A . 156
в. 145
( c .150 )
D. 108
12
92Example 2.12 A solution containing 25.6 g of sulphur,
dissolved in 1000 g of naphthalene whose melting point is
80.1°C gave a freezing point lowering of 0.680°C. Calculate
the formula of sulphur (K, for naphthalene = 6.8 Km).
12
93( 0.2 mathrm{L} ) of aqueous solution of a protein contains ( 1.26 mathrm{g} ) of the protein. The osmotic pressure of such a solution at
( 300 mathrm{K} ) is found to be ( 2.57 times 10^{-3} ) bar.
Calculate the molar mass of the protein.
( left(boldsymbol{R}=mathbf{0 . 0 8 3} boldsymbol{L} text { bar } boldsymbol{m o l}^{-1} boldsymbol{K}^{-1}right) )
12
947. The concentration of fluoride, lead, nitrate and iron in a
water sample from an underground lake was found to be
1000 ppb, 40 ppb, 100 ppm and 0.2 ppm, respectively.
This water is unsuitable for drinking due to high
concentration of:
(JEE Main 2016)
(a) Iron
(b) Fluoride
(d) Nitrate
12
95Azeotropic mixtures can be seperated by distillation of solution. If true enter 1 , else enter 0 .12
96DHOKALA is a ( ——— ) type of solution.
A. solid-in-solid
B. solid-in-gas
c. solid-in-liquid
D. gas-in-solid
12
97( 10^{24} ) molecules of solute are dissolved
in ( 10^{25} ) molecules of solvent, the mole
fraction of solute in solution is :
A . 0.09
B. 0.08
c. 0.07
D. 0.9
12
98Illustration 2.99 Molal elevation constant (K) values of
following alcohols are in the order:
CH,CH,CH,CH,OH>(CH3),CH-CH,OH>(CH3),C-OH
Explain in brief.
12
99Calculate the molarity and molality of ( 20 % ) aqueous ethanol ( left(C_{2} H_{5} O Hright) )
solution by volume. (Density of solution ( =0.96 mathrm{g} / mathrm{mL}) )
A. Molarity ( =3.48 ), Molality ( =4.35 )
B. Molarity = 4.35, Molality = 3.48
C. Molarity ( =4.48 ), Molality ( =3.35 )
D. None of the above
12
100In an experiment, 18.0 g of mannitol was dissolved in 100 g of water. The vapour pressure of solution at ( 20^{circ} mathrm{C} ) was 17.226
mm of mercury. Calculate the molecular mass of mannitol. The vapour pressure
of water at ( 20^{circ} mathrm{C} ) is ( 17.535 mathrm{mm} ) of
mercury.
A. Molecular mass of mannitol = 171.02
B. Molecular mass of mannitol = 181.02
c. Molecular mass of mannitol = 161.02
D. Molecular mass of mannitol = 121.02
12
101When a gas is bubbled through water at ( 298 K, ) a very dilute solution of gas is
obtained. Henry’s law constant for the
gas is ( 100 k ) bar. If gas exerts a pressure
of 1 bar, number of moles of gas
dissolved in 1 litre of water is :
A. 0.555
В. ( 55.55 times 10^{-5} )
c. ( 55.55 times 10^{-3} )
D. ( 5.55 times 10^{-5} )
12
102Pure water can be obtained from sea
water by:
A . centrifugation
B. plasmolysis
c. reverse osmosis
D. sedimentation
12
103How solubility of a gas in liquid varies with i) Temperature ii) pressure?12
104Q. 18 The value of Henry’s constant, KH 1S…..
(a) greater for gases with higher solubility
(b) greater for gases with lower solubility
(c) constant for all gases
(d) not related to the solubility of gases
12
105Calculate the freezing point of a solution containing ( 60 g ) of glucose
(Molar mass ( =180 g ) mol ( ^{-1} ) ) in ( 250 g ) of
water
( left(K f text { of water }=1.86 K k g m o l^{-1}right) )
12
106The ( boldsymbol{K}_{s p}left(mathbf{2 5}^{o} boldsymbol{C}right) ) of sparingly salt
[
boldsymbol{X} boldsymbol{Y}_{2}(boldsymbol{s}) text { is } boldsymbol{3} . mathbf{5 6} times mathbf{1 0}^{-5}left(boldsymbol{m o l} quad boldsymbol{L}^{-1}right)^{3}
]
and at ( 30^{circ} mathrm{C} ),the vapour pressure of its saturated solution in water is ( 31.78 mathrm{mm} )
of Hg.Calculate the enthalpy change of the reaction.( write your answer to
nearest integer)
[
boldsymbol{X} boldsymbol{Y}_{2}(boldsymbol{s}) rightleftharpoons boldsymbol{X}^{2+}(boldsymbol{a} boldsymbol{q})+boldsymbol{2} boldsymbol{Y}^{ominus}(boldsymbol{a} boldsymbol{q})
]
Given : Vapour pressure of pure water ( =31.82 mathrm{mm} ) of ( mathrm{Hg} )
12
107Benzene and naphthalene form an ideal
solution at room temperature. For this process, the true statement(s) is(are):
This question has multiple correct options
A. ( Delta G ) is positive
B . ( Delta S_{text {system}} ) is positive
C. ( Delta S_{text {surroundings}}=0 )
D. ( Delta H=0 )
12
108A solution containing 4 g of a nonvolatile organic solute per ( 100 mathrm{mL} ) was found to have an osmotic pressure
equal to ( 500 mathrm{cm} ) of mercury at ( 27^{circ} mathrm{C.The} ) molecular weight of solute is:
A . 14.97
B. 149.7
c. 1697
D. 1.497
12
109Assertion
When methanol is added to water,
boiling point of water increases.
Reason
When a volatile solute is added to a
volatile solvent, elevation in boiling point is observed.
A. Both Assertion and Reason are correct and Reason is the correct explanation for Assertion
B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion
c. Assertion is correct but Reason is incorrect
D. Both Assertion and Reason are incorrect
12
110The density of a ( 3 mathrm{M} ) solution of NaCl is 1.25g/ml. Calculate the molality of the solution.12
111Sugar and Salt solutions
a re
12
112Units of parts per million (ppm) or parts per billion (ppb) are often used to describe the concentrations of solutes
in very dilute solutions. The units are
defined as the number of grams of solute per million or per billion grams of solvent. Bay of Bengal has 1.89 ppm of
lithium ions. The molality of ( L i^{+} ) in this water is (atomic number of ( L ) i ( =7 ) ):
A ( cdot 1.5 times 10^{-4} m )
В. ( 1.7 times 10^{-4} mathrm{m} )
c. ( 2.5 times 10^{-4} m )
D. ( 2.7 times 10^{-4} m )
12
113( 520 mathrm{gm} ) mixture of ( F e_{2} O_{3} ) and ( mathrm{Fe} 0 )
reacts completely with 158 gm ( K M n O_{4} ) in acidic medium. Calculate the mole ( % )
of ( F e_{2} O_{3} ) in mixture
12
114A solution of glucose ( left(mathbf{C}_{6} mathbf{H}_{mathbf{1 2}} mathbf{O}_{mathbf{6}}right) ) in
water is labelled as ( 10 % ) by weight. What would be the molality of the solution?
(Molar mass of glucose ( =180 mathrm{g} mathrm{mol}^{-1} ) )
A. 0.4
B. 0.6
( c .0 . )
D. 0.5
12
115A ( 5 % ) solution of cane sugar is isotonic with ( 0.877 % ) solution of ( X . ) Calculate
the molecular mass of ( X ), if the
molecular mass of cane sugar is 342 g/mol.
A ( .60 mathrm{g} / mathrm{mol} )
B. ( 120 mathrm{g} / mathrm{mol} )
c. 78 g/mol
D. 30 g/mol
12
116Illustration 2.135 If a solution containing 6 g of triphenyl
methane, (C H2) CH (molecular weight = 244), in 1000 g
of benzene is cooled to 0.22°C below the freezing point of
benzene, how much solvent will crystallize out and what will
be the molality of residual solution? (K. = 5.1 K m-1)
12
117A true solution (or simply a solution) is a homogeneous mixture, in which the solute and solvent molecules cannot be
distinguished even under a microscope.
A. True
B. False
12
118Example 2.24 A 0.1 M solution of glucose (molecular weight
180 g mol-l) and a 0.1 M solution of urea (molecular weight
= 60 g mol-l) are placed on the two sides of a semi-permeable
membrane to equal heights. In this context, which of the
following statements is correct?
a. Glucose will flow across the membrane into the urea
solution.
b. Urea will flow across the membrane into the glucose
solution.
c. Water will flow across the membrane from the urea
solution into the glucose solution.
d. There will be no net movement across the membrane.
sol
12
119( 0.4 g ) of ( mathrm{NaOH} ) is present in one litre of
the solution shows that ( boldsymbol{H}^{+} )
concentration of the solution is?
12
120Illustration 2.71 Calculate the vapour pressure of an
aqueous solution of 1.0 molal glucose solution at 100°C.
12
121Question 22. At 300 K, 36 g of glucose present in a litre of its solution
has an osmotic pressure of 4.98 bar. If the osmotic pressure of the solution
is 1.52 bar at the same temperature, what would be its concentration?
We
Apply a = CRT and C –
V
MB XV
12
122Five hundred milliliters of solution of 0.1
M Na Br has how many milligrams of bromine?
A. 200 ( mathrm{mg} )
B. 400 mg
c. ( 2,000 mathrm{mg} )
D. ( 4,000 mathrm{mg} )
E. 20,000 ( mathrm{mg} )
12
123Phenol associates in ( C_{6} H_{6} ) to double
molecules. A solution of 2 g of phenol in 100 g ( C_{2} H_{6} ) has its f.pt. lowered by 0.72
K. ( boldsymbol{K}_{f} ) for ( boldsymbol{C}_{boldsymbol{6}} boldsymbol{H}_{boldsymbol{6}} ) is ( mathbf{5 . 1 2} boldsymbol{K} boldsymbol{m o l}^{-1} boldsymbol{k} boldsymbol{g} )
Percentage degree of association of
phenol is (write the integer at tens place, e.g., if percentage degree of dissociation is ( x y % ) then answer would
be ( x ) )
12
124When ( 1.20 g ) of sulphur is melted with ( 15.00 g ) of naphthalene, the solution
freezes at ( 77.2^{circ} mathrm{C} ).. What is the molar
mass of this form of sulphur?
Data for Naphthalene:
Melting point, ( mathrm{M} . mathrm{P}=80^{circ} mathrm{C} )
Freezing point depression constant, ( k_{f}=6.80^{circ} mathrm{C} boldsymbol{m}^{-1} )
A . ( 180 g ) mol ( ^{-1} )
B. ( 194 g ) mol ( ^{-1} )
c. ( 260 g ) mol ( ^{-1} )
D. ( 450 mathrm{g} ) mol ( ^{-1} )
12
125Molecules of ethanoic acid dimerises in
benzene due to ( H- ) bonding if al molecules of ethanoic acid associated
in benzene then:
A. boiling boiling of ethanoic acid become half of norma value
B. freezing point of ethanoic acid become twice of normal value
c. molar mass become twice of normal value
D. vapour pressure of solution decreases due to dimerisation
12
126The molality of an aqueous dilute solution containing non-volatile solute is 0.1 m. What is the boiling
temperature (in ( ^{circ} boldsymbol{C} ) ) of solution?
(Boiling point elevation constant, ( boldsymbol{K}_{boldsymbol{b}}= ) ( 0.52 k g m o l^{-1} K ; ) boiling temperature
of water ( =100^{circ} mathrm{C} ) )
A. 100.0052
в. 100.052
c. 100.0
D. 100.52
12
127Which of the following relation is not correctly matched with the formula?
A ( cdot ln ) case of association, ( alpha=frac{i-1}{frac{1}{n}-1} )
B. ( _{text {In case of dissociation, } alpha}=frac{i-1}{n+1} )
( i frac{n_{B}}{n_{A}+n_{B}} )
Devation in boiling point, ( Delta T=K_{b} times frac{W_{B} times 1000}{M_{B} times W_{A}} )
12
128The molarity of ( C l^{-}(100 mathrm{ml}) ) ions in the
solution after 0.2 moles ( H C l ) are mixed
with 0.1 moles ( C a C l_{2} ) solution?
A. 0.8 m
B. 0.04 М
( c .0 .4 mathrm{M} )
D. 0.08 м
12
129Name the type of solution formed in the following cases:
i) ( 20 g ) of ( N a C l ) in ( 100 g ) of water.
ii) ( 36 g ) of ( N a C l ) in ( 100 g ) of water.
iii) ( 45 g ) of ( N a C l ) in ( 100 g ) of water at
( 80^{circ} mathrm{C} )
iv) Sulphur dissolved in ( C S_{2} )
v) Nitrogen in soil
12
Clapeyron equation describes this
relationship. The Clausius-Clapeyron equation is :
( ln left(P_{v a p o u r}right)=-frac{Delta H_{v a p o u r}}{R}left[frac{1}{T}right]+C )
According to the graph, at high temperatures, which substance has
the greatest vapour pressure?
( A cdot w )
B. ( x )
( c )
( D )
12
131The boiling point of a solution of 5 g sulphur in 100 g ( C S_{2} ) is ( 0.5^{circ} C ) above
pure solvent. If the ( K_{b} ) of ( C S_{2} ) is 2.56
( mathrm{K} / mathrm{m}, ) then find the atomicity of the sulphur in the solvent.
12
1321000 g aqueous solution of ( C a C O_{3} ) contains 10 g of calcium carbonate. ( mathbf{A} ) concentration of the solution is:
A. 10 ppm
B. 100 ppm
c. 1000 ppm
D. 10000 ppm
12
133A 3.4 g sample of ( H_{2} O_{2} ) solution containing ( boldsymbol{x} % boldsymbol{H}_{2} boldsymbol{O}_{2} ) by mass requires
( x ) mL of a ( K M n O_{4} ) solution for complete oixidation under acidic
condition.The molarity of ( boldsymbol{K} boldsymbol{M} boldsymbol{n} boldsymbol{O}_{4} )
solution is:
( A )
B. 0.5
( c cdot 0.4 )
D. 0.2
12
134Water is added to the solution M such
that the mole fraction of water in the
solution becomes 0.9. The boiling point of this solution is :
A . ( 380.4 mathrm{k} )
B . 376.35 К
c. 375.5 к
D. 354.7 к
12
135If 3.65 got ( mathrm{HCl} ) is dissolved in ( 16.2 mathrm{g} ) of water then the mole fraction of HCl in
the resulting solution is:
12
136Which of the following pairs of solutions is isotonic?
A. ( 6 % ) urea and ( 6 % ) glucose ( (w / v) )
B. ( 18 % ) urea and ( 18 % ) glucose ( (w / v) )
( c .6 % ) urea and ( 18 % ) fructose ( (w / v) )
D. ( 34.2 % ) sucrose and ( 60 % ) glucose ( (w / v) )
12
137Positive deviation from Raoult’s law is
shown by which of the following mixtures?
A. Benzene and toluene
B. ( C H C l_{3} ) and acetone
c. Ethanol and water
D. ( H C l ) and water
12
138The ratio of the actual value of a
colligative property to the value calculated, assuming the substance to be a nonelectrolyte, is referred to as
A. Henry’s law
B. vapor pressure lowering
c. the van’t Hoff factor
D. freezing point depression
E . osmotic pressure
12
139( 10^{-1} M ) HCl is diluted to 100 times. Its
pHis:
( A cdot 3 )
B. 8
( c cdot 6.98 )
D. 7.02
12
140The total vapour pressure of a mixture of 1 mol ( Aleft(P_{A}^{O}=150 text { tor } rright) ) and 2 mol ( B )
( left(P_{B}^{o}=240 text { tor } rright) ) is ( 200 mathrm{mm} . ) In this
case:
A. there is positive deviation from Raoult’s law
B. there is negative deviation from Raoult’s law.
c. there is no deviation from Raoult’s law
D. molecular masses of A and B are also required.
12
141Illustration 2.86 Two liquids A and B boil at 130°C and
160°C, respectively. Which of the them has higher vapour
pressure at 80°C.
12
142When no more of a solid can be
dissolved in a solvent ,it is called:
A. unsaturated solution
B. colloidal solution
c. saturated solution
D. none of the above
12
143Mole fraction =
A. ( frac{text { Number of moles of constituent }}{text { Number of moles of all constituents }} )
B. Number of molecule of constituent + Total number of
moles of all constituents
C. Both (A) and (B) above
D. None of the above
12
144Illustration 2.112 The freezing point of a solution containing
50 cm of ethylene glycol in 50 g of water is found to be -34°C.
Assuming ideal behaviour, calculate the density of ethylene
glycol (K, for water = 1.86 K kg mol-!).
12
145( 19.5 g ) of ( C H_{2} F C O O H ) is dissolved in ( mathbf{5 0 0} g ) of water. The depression in the freezing point of water observed is
( 1.00^{0} C . ) Calculate the van’t Hoff factor
and dissociation constant of
fluoroacetic acid.
12
146( 18.0 g ) of ( operatorname{glucose}left(C_{6} H_{12} O_{6}right) ) is added to
( 178.2 g ) of water. The vapour pressure of water for this aqueous solution at ( 100^{circ} mathrm{C} )
is :
A . ( 759 . .00 ) Torr
B. 7.60 Torr
c. 76.00 torr
D. 752.40 Torr
12
147Assertion: A 1 m NaCl(aq) solution will
freeze at a temperature below ( 273 K )
Reason: As a solute is added to a
Solvent, the boiling point increases
while the freezing point decreases.
A. Both Assertion and Reason are true and Reason is the correct explanation of Assertion.
B. Both Assertion and Reason are true but Reason is not the correct explanation of Assertion.
C. Assertion is true but Reason is false.
D. Assertion is false but Reason is true.
E. Both Asssertion and Reason are false
12
148Colligative molality ( = ) molality ( times )
Van’t Hoff factor
If true enter ( 1, ) if false enter 0
12
149( boldsymbol{P}_{boldsymbol{A}}=boldsymbol{X}_{boldsymbol{A}} boldsymbol{P}_{boldsymbol{A}} ) and ( boldsymbol{P}_{boldsymbol{B}}=boldsymbol{X}_{boldsymbol{B}} boldsymbol{P}_{boldsymbol{B}} )
( boldsymbol{P}_{boldsymbol{T}}=boldsymbol{X}_{boldsymbol{A}} boldsymbol{P}_{boldsymbol{A}}+boldsymbol{X}_{boldsymbol{B}} boldsymbol{P}_{boldsymbol{B}_{boldsymbol{B}}} )
Vapour pressure of mixtures of Benzene ( left(C_{6} H_{6}right) ) and toluene ( left(C_{7} H_{8}right) ) at ( 50^{circ} C ) are given by ( boldsymbol{P}_{M}=mathbf{1 7 9} boldsymbol{X}_{boldsymbol{B}}+mathbf{9 2} ) where
( X_{B} ) is mole fraction of ( C_{6} H_{6} )
What is the vapour pressure of pure liquids?
A ( cdot P_{B}=92 m m, P_{T}=179 m m )
B . ( P_{B}=271 mathrm{mm}, P_{T}=92 mathrm{mm} )
c. ( P_{B}=180 m m, P_{T}=91 m m )
D. None of these
12
150If the maximum concentration of ( boldsymbol{P b C l}_{2} )
in water is ( 0.01 M ) at ( 298 K ), Its
maximum concentration in
( mathbf{0 . 1} boldsymbol{M} boldsymbol{N} boldsymbol{a} boldsymbol{C l} ) will be:
A ( cdot 4 times 10^{-3} M )
В. ( 0.4 times 10^{-4} M )
( mathbf{c} cdot 4 times 10^{-2} M )
D. ( 4 times 10^{-4} M )
12
151The vapour pressure of a dilute aqueous
solution of glucose is ( 750 mathrm{mm} ) Hg at
( mathbf{3 7 3} mathbf{K} )
Calculate (i) molality, (ii) mole fraction of the solute.
в. 0.078,0.02
( c .0 .0729,0.0187 )
7
D. 0.0779,0.3
12
152For an ideal binary solution ( (A) ) and ( (B) )
( boldsymbol{y}_{A} ) is the mole fraction of ( boldsymbol{A} ) in vapor
phase. Which of the following plot should be linear?
A ( cdot P_{text {total }} ) vs ( y_{A} )
B. ( P_{text {total }} ) vs ( y_{B} )
( ^{c} frac{1}{P_{text {total}}} ) vs ( y_{A} )
D. ( frac{1}{P_{text {total }}} ) vs ( y_{B}+y_{A} )
12
153Mustration 2.101 Sodium chloride solution freezes at lower
temperature than water but boils at higher temperature than
water. Explain.
12
154To aqueous solution of Nal, increasing
amounts of solid ( H g I_{2} ) is added. The
vapor pressure of the solution-
A. Decreases to a constant value.
B. Increases to a constant value
c. Increases first and then decreases.
D. Remains constant because ( H g I_{2} ) is sparingly soluble in water.
12
155Density of ( H_{2} O ) is ( 1 g m L^{-1} . ) If we have
( 1 m L H_{2} O ) then:
This question has multiple correct options
A . It is 55.55 mol ( L^{-1} )
B . It has ( 3.33 times 10^{22} mathrm{H}_{2} mathrm{O} ) molecules
c. It has ( 3.33 times 10^{22} ) H-atoms
D. It has ( 6.66 times 10^{22} ) O-atoms
12
156The system that forms maximum boiling azeotrope is :
A. acetone-chloroform
B. ethanol- acetone
C. n-hexane- n- heptane
D. carbon disulphide – acetone
12
157A ( 10 % ) (mass/mass) solution of cane sugar undergoes partial conversion into glucose and fructose to show an inversion of cane sugar as:
Sucrose( + )Water( rightarrow )Glucose( + )
Fructose
The solution boils at ( 100.27^{circ} mathrm{C} ) at this
state. What fraction of the sugar has
inverted? ( left(text { Given } boldsymbol{K}_{boldsymbol{b}} text { for } boldsymbol{H}_{mathbf{2}} boldsymbol{O} ) is right.
( left.0.512 K m o l^{-1} k gright) )
Multiply answer with 10 and write the nearest integer value.
12
158A 0.5 molal solution of ethylene glycol in water is used as the coolant in a car. If
the freezing point constant of water is ( 1.86 mathrm{K} . mathrm{kg} / mathrm{mol} ), the mixture will freeze at:
( mathbf{A} cdot 0.93^{0} C )
B. ( -0.93^{0} C )
c. ( 1.86^{0} C )
D. ( -1.86^{0} C )
12
159Van’t Hoff factor is:
A. more than one in case of association
B. less than one in case of dissociation
C. ( frac{text { normal molecular mass }}{text { observed molecular mass }} )
D. ( frac{text { observed molecular mass }}{text { normal molecular mass }} )
12
160Q13. What is the effect of temperatures on the vapour pressure of a liquid?12
161Illustration 2.132 The freezing point of 0.02 mole fraction
acetic acid in benzene is 277.4 K. Acetic acid exists partly as
dimer. Calculate the equilibrium constant for dimerization.
The freezing point of benzene is 278.4 K and the heat of fusion
of benzene is 10.042 kJ mol-1. Assume molarity and molality
same.
12
162containing 8.19g
d from pure water
Illustration 2.201 A 250-ml water solution containing
of sodium chloride at 300 K is separated from pure
by means of a semi-permeable membrane. The pressure
must be applied above this solution in order to just prevent
osmosis is (R = 0.0821 L atm moll K-1)
a. 13.80 atm
b. 27.58 atm
c. 23.34 atm
d. 9.80 atm
12
163The cryoscopic constant for acid is ( 3.6 mathrm{K} ) kg/mol. A solution of 1 g of a hydrocarbon in 100 g of acetic acid
freezes at ( 16.60^{circ} mathrm{C} ). The hydrocarbon contains ( 92.3 % ) carbon.lf the molecular
formula is ( C_{x} H_{y} ). Find the value of ( x ) and
( y: )
A. ( x=2, y=4 )
В. ( x=3, y=8 )
c. ( x=4, y=10 )
D. ( x=6, y=6 )
12
164A mixture of 2 moles of ( N_{2} ) and 8 moles
of ( H_{2} ) are heated in a 2 lit vessel, till
equilibrium is established. At
equilibrium 0.4 moles of ( N_{2} ) was present. What will be the equilibrium
concentration of ( boldsymbol{H}_{2} ? )
( A cdot 2 ) mole/lit
B. 4 mole/lit
c. 1.6 mole/lit
D. 1 mole/lit
12
165Which of the following form is an ideal solution?
This question has multiple correct options
A. Ethyl bromide + Ethyl iodide
B. Ethyl alcohol + Water
c. chloroform + Benzene
D. Benzene + Toluene
12
166In a saturated solution:
A. dissolved solute ( >>> ) undissolved solute
B. dissolved solute ( <<< ) undissolved solute
C. dissolved solute and undissolved solutes are in equilibrium with each other
D. none of the above
12
167How are 0.50 mol ( N a_{2} C O_{3} ) and ( 0.50 mathrm{M} )
( N a_{2} C O_{3} ? )
12
168Which of the following choices will favor the melting of ice in a closed container
if all other parameters are kept constant?
A. Adding water with a temperature of ( 0^{circ} mathrm{C} )
B. Lowering the temperature below ( 0^{circ} mathrm{C} )
c. Lowering the pressure
D. Raising the pressure
E. Decreasing the amount of ice
12
169Which of the following is a true solution?
A. Copper in gold
B. Sulphur in water
c. мilk
D. water in sulphur dioxide
12
170What will be the mass of a ( 0.500 mathrm{m} )
solution of sodium acetate in water
containing ( 0.5 mathrm{Kg} ) sodium acetate?
12
171Question 8. How does sprinkling of salt help in clearing the snow
covered roads in hilly areas? Explain the phenomenon involved in the
process.
12
17275.2 ( g ) of ( C_{6} H_{5} O H ) (phenol) is dissolved
in a solvent of ( K_{f}=14 . ) If the depression in freezing point is ( 7 mathrm{K} ) then find the ( % ) of phenol that dimerises.
12
173The degree of dissociation of
( C aleft(N O_{3}right)_{2} ) in a dilute aqueous solution containing 7 gm of the salt per 100 gm
of water at ( 100^{circ} mathrm{C} ) is 70 per. If the vapour
pressure of water at ( 100^{circ} mathrm{C} ) is ( 760 mathrm{mm} )
Calculate the vapour pressure of the solution.
A. ( 373.12 mathrm{mm} / mathrm{Hg} )
в. ( 524.89 mathrm{mm} / mathrm{Hg} )
( mathbf{c} .746 .24 mathrm{mm} / mathrm{Hg} )
D. ( 1049.6 mathrm{mm} / mathrm{Hg} )
12
174(i) Prove that osmotic presser is a
colligative property
(ii) Calculate the molar concentration of
urea solution if it exerts an osmotic
pressure of 2.45 atmosphere at ( 300 mathrm{K} ) ( left[mathrm{R}=0.0821 mathrm{I} . text { atm. } operatorname{mol}^{1} boldsymbol{K}^{-1}right] )
12
175Which solution would have the most
altered boiling point?
A ( cdot 1 M L i_{2} S O_{4} )
в. ( 1 mathrm{M} mathrm{CuSO}_{4} )
( mathrm{c} cdot 1 mathrm{M} C_{6} mathrm{H}_{12} mathrm{O}_{6} )
D. 1 ( M ) NaCl
12
176Henry’s law constant for solubility of
methane in benzene is ( 4.27 times 10^{-5} )
( m m^{-1} H g m o l d m^{-3} ) at constant
temperature. Calculate solubility of
methane at 760 mm ( H g ) pressure at
same temperature
12
177The hardness of water due to ( H C O_{3}^{ominus} ) is
122 ppm. Select the correct statement(s).
This question has multiple correct options
A. The hardness of water in terms of ( C a C O_{3} ) is 200 ppm.
B. The hardness of water in terms of ( C a C O_{3} ) is 100 ppm.
C. The hardness of water in terms of ( C a C l_{2} ) is 222 ppm.
D. The hardness of water in terms of ( M g C l_{2} ) is 95 ppm.
12
178Q. 37 Explain why on addition of 1 mole of NaCl to 1 L of water, the boiling
point of water increases, while addition of 1 mole of methyl alcohol Lo
1 L of water decreases its boiling point.
12
17912.2 ( g ) of benzoic acid ( (M=122) ) in 100 g water has elevation in the boiling point of ( 0.27 mathrm{K} . K_{b}=0.54 mathrm{K} mathrm{kg} mathrm{mol}^{-1} . ) If there is
( 100 % ) polymerisation, the number of molecules of benzoic acid in the
associated state is:
A.
B. 2
( c cdot 3 )
( D )
12
180The relationship between osmotic pressure at ( 273 mathrm{K} ) when 10 g glucose
( left(P_{1}right), 10 ) g urea ( left(P_{2}right) ) and 10 g sucrose
( left(P_{3}right) ) are dissolved in ( 250 mathrm{mL} ) of water is
A ( . P_{1}>P_{2}>P_{3} )
в. ( P_{3}>P_{1}>P_{2} )
c. ( P_{2}>P_{1}>P_{3} )
D. ( P_{2}>P_{3}>P_{1} )
12
181The molarity of ( H_{2} S O_{4} ) is ( 18 M . ) Its
density is ( 1.8 g m L^{-1} . ) Hence, molality is :
( A cdot 36 m )
B. 200 ( mathrm{m} )
c. ( 500 mathrm{m} )
D. ( 18 mathrm{m} )
12
182A salt which in solution gives a bluish
white precipitate with ( N a O H ) solution
and a white precipitate with ( B a C l_{2} ) solution is:
A ( . C u S O_{4} )
в. ( F e S O_{4} )
c. ( F e_{2}left(S O_{4}right)_{3} )
D. ( C u C l_{2} )
12
183( 10 mathrm{L} ) of hard water required ( 0.56 mathrm{g} ) of lime ( (C a O) ) for removing hardness.
Hence, temporary hardness in ppm of ( boldsymbol{C a C O}_{3} ) is :
A . 100
в. 200
c. 10
D. 20
12
184Equal volumes of ( 0.1 M A g N O_{3} ) and
( 0.2 M N a C l ) are mixed. The
concentration of ( N O_{3}^{-} ) ions in the mixture will be:
( mathbf{A} cdot 0.1 M )
B. ( 0.05 M )
( c cdot 0.2 M )
D. ( 0.15 M )
12
185Benzene and toluene form an ideal
solution over the entire range of
composition. The vapour pressure of pure benzene and toluene at ( 300 K ) are
( 50.71 m m H g ) and ( 32.06 m m H g )
respectively. Calculate the mole fraction
of benzene in vapour phase if ( 80 g ) of
benzene is mixed with ( 100 g ) of toluene.
12
186( 100 mathrm{ml} ) of ( 2 mathrm{M} ) NaOH solution is diluted
by water and the final molarity becomes
0.5. The volume of water added to the
solution is:
A . ( 400 mathrm{ml} )
B. 300 m
c. ( 500 mathrm{ml} )
D. 200 m1
12
187Q. 33 Volume of a solution changes with change in temperature, then what
will the molality of the solution be affected by temperature? Give reason
12
188A ( 0.5 g ) sample of ( K H_{2} P O_{4} ) is titrated with ( 0.1 M ) NaOH.The volume of base
required to do this is ( 25.0 m l ) The
reaction is represented as:
( boldsymbol{H}_{2} boldsymbol{P} boldsymbol{O}_{4}^{-}+boldsymbol{O} boldsymbol{H}^{-} rightarrow boldsymbol{H} boldsymbol{P} boldsymbol{O}_{4}^{2-}+boldsymbol{H}_{2} boldsymbol{O} )
The percentage purity of ( K H_{2} P O_{4} ) is ( (boldsymbol{K}=mathbf{3 9}, boldsymbol{P}=mathbf{3 1}) )
A . ( 68 % )
B. 34%
c. ( 85 % )
D. 51%
12
189The phase diagram for solvent and solutions is shown in the figure. What
represents the normal boiling point of
the solution?
( A )
B.
( c cdot c )
( D )
12
190Which one of the following electrolytes has the same value of van’t Hoff’s factor
(i) as that of ( A l_{2}left(S O_{4}right)_{3} ) (if all are ( 100 % ) ionised)?
( mathbf{A} cdot A lleft(N O_{3}right)_{3} )
B . ( K_{4}left[F e(C N)_{6}right] )
( mathrm{c} cdot mathrm{K}_{2} mathrm{SO}_{4} )
D. ( K_{3}left[F e(C N)_{6}right] )
12
191An aqueous solution contains 0.53 g of
anhydrous ( N a_{2} C O_{3}(text { Mol. wt. } 106) ) dissolved in ( 100 mathrm{ml} ) of solution. The
molarity of the solution is:
( mathbf{A} cdot 0.1 M )
в. ( 0.05 M )
( mathbf{c} cdot 0.2 M )
D. ( 0.4 M )
12
192Illustration 2.38 An aqueous solution containing 28% by
weight of a liquid A (molecular mass = 140) has a vapour
pressure of 0.200 bar at 37°C. Calculate the vapour pressure
of pure liquid (vapour pressure of water at 37°C = 0.100 bar).
12
1933. 10.0 g of glucose (tt,), 10.0 g of urea (Tx), and 10.0 g of
sucrose (Ttz) are dissolved in 250.0 mL of water at 273
K (Tt = osmotic pressure of a solution). The relationship
between the osmotic pressure of the solutions is
a. Ty > T2 > Tz
b. nz > , > T2
C. Ty > Ty > Tz
d. Tey > Tz > TT,
12
194The osmotic pressure of a dilute solution is given by :
A. ( P=P_{0} times N_{1} )
B . ( pi V=n R T )
c. ( Delta P=P_{0} N_{2} )
D. ( frac{Delta P}{P^{o}}=frac{P^{o}-P_{S}}{P^{o}} )
12
195Cane sugar underoges the inversion as
follow:
( boldsymbol{C}_{12} boldsymbol{H}_{22} boldsymbol{O}_{11}+boldsymbol{H}_{2} boldsymbol{O} rightarrow boldsymbol{C}_{6} boldsymbol{H}_{12} boldsymbol{O}_{6}+ )
( boldsymbol{C}_{boldsymbol{6}} boldsymbol{H}_{mathbf{1 2}} boldsymbol{O}_{boldsymbol{6}} )
If solution of 0.025 moles of sugar in ( 200 mathrm{gm} ) of water show depression in
freezing point ( 0.372^{circ} mathrm{C}, ) then what ( % )
sucrose has inverted. ( left(boldsymbol{K}_{f}left(boldsymbol{H}_{2} boldsymbol{O}right)=right. )
1.86 ( left.K k g m o l^{1}right) )
12
196Maltose is converted to ‘A’ by Maltase. The mole fraction of ‘A’ in ( 10 % ) (w/w) aq solution is approximately.
( mathbf{A} cdot 0.989 )
B. 0.012
c. ( 0 . )
D. 0.017
12
197( 3 mathrm{g} ) of salt of molar mass 30 is dissolved in 250 g of water. The molality of a solution is ( x ) M. The value of ( 10 x ) is12
198Tritium, ( T ) (an isotope of ( H ) ) combines with fluorine to form weak acid TF,
which ionizes to give Tritium is radioactive and is ( alpha beta- )emitter.
freshly prepared aqueous solution of TF has pT (an equivalent of pH) of 1.5 and freezes at ( -0.372^{circ} mathrm{C} . ) If ( 600 mathrm{ml} ) of
freshly prepared solution were allowed to stand for 24.8 years. Calculate (i) ionization constant of TF. (ii)Number
of lbeta-particles emitted?(Given ( boldsymbol{K}_{f} ) forwater ( =mathbf{1 . 8 6 k g m o l} boldsymbol{K}^{-1}, boldsymbol{t}_{1 / 2} ) for
tritium ( =12.4 y ) ears
A ( cdot(i) K_{a}=7.3 times 10^{-3}(i i) 4.55 times 10^{22} )
B . (i)K ( _{a}=7.3 times 10^{-5}(i i) 4.55 times 10^{24} )
C . ( (i) K_{a}=14.3 times 10^{-3}(i i) 9.1 times 10^{22} )
D . (i) ( K_{a}=14.3 times 10^{-5}(i i) 9.1 times 10^{24} )
12
199Ilustration 2.169 At 300 K, 36 g of glucose present per
litre in its solution has an osmotic pressure of 4.98 bar. If
the osmotic pressure of the solution is 1.52 bar at the same
temperature, what would be its concentration?
12
200Which of the following aqueous solution will show maximum vapour pressure at
300K?
( mathbf{A} cdot 1 M N a C l )
в. ( 1 mathrm{M} mathrm{CaCl}_{2} )
c. ( 1 M A l C l_{3} )
D. ( 1 M C_{12} H_{22} O_{11} )
12
201An aqueous solution of a non-volatile
solute boils as ( 100.17^{circ} mathrm{C} ). What is the
depression in the freezing point for the
solution in ( ^{circ} mathrm{C} ) ?
( left[K_{b} text { and } K_{f} text { for water is } 0.512 ) and right.
( mathbf{1 . 8 6}^{circ} boldsymbol{C} / boldsymbol{m} ) respectively
A . 0.93
B. 0.11
( c cdot 0.62 )
D. 0.31
12
202Illustration 2.209 The freezing point of a solution
containing 0.3 g of acetic acid in 43 g of benzene reduces by
0.3°. Calculate the Van’t Hoff factor.
(K, for benzene = 5.12 K kg moll)
12
203Which of the following alkali metal ions has lowest ionic mobility in aqueous solutions?
( mathbf{A} cdot R b^{+} )
B. ( C s^{ } )
c. ( N a^{+} )
( mathbf{D} cdot L i^{+} )
12
204If the ionic product of ( M(O H)_{2} ) is ( 5 times ) ( 10^{-10}, ) then the molar solubility of
( M(O H)_{2} ) in ( 0.1 M N a O H ) is:
A ( .5 times 10^{-12} mathrm{M} )
В. ( 5 times 10^{-8} ) М
c. ( 5 times 10^{-10} M )
D. ( 5 times 10^{-9} M )
E ( .5 times 10^{-16} M )
12
205Calculate the vapour pressure of an
aqueous solution of 1.0 molal glucose solution at ( 100^{circ} mathrm{C} )
12
206Which of the following is not an air pollutant?
A. ( N_{2} )
в. ( N_{2} ),
c. ( N O )
D. ( C O )
12
207The freezing point of equimolal aqueous solution will be highest for:
A. ( C_{6} H_{5} N H_{3}^{+} C l^{-} )
в. ( quad C aleft(N O_{3}right)_{2} )
c. ( _{L a}left(N O_{3}right)_{2} )
D. ( C_{6} H_{12} O_{6} )
12
208| Illustration 2,90 The boiling point elevation constant for
benzene is 2.57°C/m. The boiling point of benzene is 81.0°C.
Determine the boiling point of a solution formed when 5 g
of C2H,, is dissolved in 15 g of benzene.
12
209A 0.001 molal solution of a complex
represented as ( P tleft(N H_{3}right)_{4} C l_{4} ) in water had freezing point depression of
( mathbf{0 . 0 0 5 3 ^ { circ }} mathbf{C .} ) Given, ( boldsymbol{K}_{f} ) for ( boldsymbol{H}_{2} boldsymbol{O}= )
1.86 Kmolality ( ^{-1} ). Assuming 100%
ionisation of the complex, write the ionisation nature and formula of
complex
A ( cdot P tleft[left(N H_{3}right)_{4} C l_{2}right] C l_{2} rightarrow P tleft[left(N H_{3}right)_{4} C l_{2}right]^{2+} 2 C l )
B . ( P tleft[left(N H_{3}right)_{4} C l_{2}right] C l_{2} rightarrow P tleft[left(N H_{3}right)_{4} C l_{2}right]^{+} C l )
c. ( P tleft[left(N H_{3}right)_{4} C l_{2}right] C l_{2} rightarrow 2 P tleft[left(N H_{3}right)_{4} C l_{2}right]^{+} C l )
D. ( P tleft[left(N H_{3}right)_{4} C l_{2}right] C l_{2} rightarrow P tleft[left(N H_{3}right)_{4} C l_{2}right]^{3+} 3 C l )
12
210A 0.2 molal solution of KCl freezes at
( -0.68^{circ} mathrm{C} . ) If ( K_{f} ) for ( H_{2} O ) is ( 1.86, ) the
degree of dissociation of ( boldsymbol{K} boldsymbol{C l} ) is:
A . ( 75 % )
B. ( 83 % )
( c .65 % )
D. ( 92 % )
12
2111 L sample of impure water containing sulphide ion is made ammonial and is
titrated with ( 300 mathrm{mL} ) of ( 0.1 M A g N O_{3} ) solution. Which of the following statements is/are correct about the
above reaction?
This question has multiple correct options
A. The strength of ( H_{2} S ) in water is ( 0.51 mathrm{g} / mathrm{L} )
B. The strength of ( H_{2} S ) in water is ( 5.1 mathrm{g} / mathrm{L} )
C. The concentration of ( H_{2} ) S in water in ppm is 510
D. The concentration of ( H_{2} S ) in water in ppm is 51
12
212A ( 5 % ) solution of cane sugar is isotonic with ( 0.877 % ) of ( X . ) The molecular weight of substance X is:
( mathbf{A} cdot 58.98 )
B. 119.96
( mathbf{c} .95 .58 )
D . 126.98
12
213Two liquids ( A ) and ( B ) form an ideal solution at temperature T. When the
total vapour pressure above the solution is 400 torr, the mole fraction of
( A ) in the vapour phase is 0.40 and in the liquid phase ( 0.75 . ) What are the vapour
pressure of pure ( A ) and pure ( B ) at
temperature T?
12
214Illustration 2.151 Addition of Hgl, to the aqueous solution
of KI shows an increase in the osmotic pressure, why?
12
215Question 2. Explain why on addition of 1 mole of NaCl to 1L of water,
the boiling point of water increases, while addition of 1 mole of methyl
alcohol to 1 L of water decreases its boiling point.
12
216Illustration 2.128 The molal freezing point depression
constant of benzene (CH) is 4.90 K kg mol-!. Selenium
exists as a polymer of the type Se. When 3.26 g of selenium
is dissolved in 226 g of benzene, the observed freezing point
is 0.112°C lower than pure benzene. Deduce the molecular
formula of selenium. (Atomic mass of Se = 78.8 g mol-‘)
12
217( 58.5 g m ) of ( N a C l ) and ( 180 g m ) of
glucose were separately dissolved in
1000 ( m l ) of water. Identify the correct
statement regarding the elevation of boiling point (b.p.) of the resulting solutions.
A. ( N a C l ) solution will show higher elevation of b.p.
B. Glucose solution will show higher elevation of b.p.
C. Both the solutions will show equal elevation of b.p.
D. The b.p. elevation will be shown by neither of the solutions
12
218( 250 m l ) of a sodium carbonate solution
contains 2.65 grams of ( N a_{2} C O_{3} .10 m l )
of this solution is added to ( ^{prime} x^{prime} m l ) of
water to obtain ( 0.001 M N a_{2} C O_{3} )
solution.
What is the value of ( ^{prime} x^{prime} ) in ( m l ) ?
[Molecular weight of ( left.boldsymbol{N} boldsymbol{a}_{2} boldsymbol{C O}_{3}=mathbf{1 0 6}right] )
A. 1000
в. 990
c. 9990
D. 90
12
219Two liquids ( A ) and ( B ) form an ideal
solution. What is the vapour pressure of solution containing 2 moles of ( A ) and 3
moles of ( B ) at ( 300 K ? )
[Given: At ( 300 K ), vapour pressure of
pure liquid ( boldsymbol{A}left(boldsymbol{P}_{A}^{circ}right)=mathbf{1 0 0} ) torr, Vapour
pressure of pure liquid ( Bleft(P_{B}^{circ}right)= ) ( 300 text { tor } r] )
A. 200 torr
B. 220 torr
c. 180 tor
D. None of these
12
220In an auto engine with no pollution
controls, about ( 5 % ) of the fuel ( left(C_{8} H_{18}right) )
is unburned. Molar ratio of ( C O ) and
( left(C_{8} H_{18}right), ) emitted in the exhaust gas is:
A . 100
B. 152
( c .50 )
D. 5
12
221lce begins to separate at ( -0.744^{circ} mathrm{C} ) from a solution containing 2.4 g of nonvolatile, non-electrolyte in 100 g water. Calculate the molar mass of solute, ( boldsymbol{K}_{boldsymbol{f}} )
for ( boldsymbol{H}_{2} boldsymbol{O} ) is ( 1.86 mathrm{K} ) mol( ^{-1} boldsymbol{k} boldsymbol{g} ). Assume
mass of solvent is equal to mass of solution. Answer in g/mol.(Enter the answer as ( frac{M a s s}{10} ) ).
12
222Illustration 2.92 The ebullioscopic constant for benzene
is 2.52 Km-1. A solution of an organic substance in benzene
boils at 0.125°C higher than benzene. Calculate the molality
of solution?
12
223For a solution of density, ( d ) in ( g / m ) containing solute of molecular weight ( W, ) the molarity ( M ) and molality ( m ) are
related by:
A ( cdot frac{d}{M}=frac{1}{m}+frac{W}{1000} )
в. ( frac{d}{m}=frac{1}{M}+frac{W}{1000} )
c. ( frac{W}{M}=frac{1}{m}+frac{d}{1000} )
D. ( frac{d}{m}=frac{W}{M}+frac{1}{1000} )
12
224The Vant Hoff factor (i) for a dilute
solution of ( boldsymbol{K}_{mathbf{3}}left[boldsymbol{F} boldsymbol{e}(boldsymbol{C} boldsymbol{N})_{boldsymbol{6}}right] ) is (Assuming
( 100 % text { ionsation }) )
A . 10
B. 4
c. 5
D. 0.25
12
225The concentration of ( mathrm{CO}_{2} ) in a soft drink
bottled with a partial pressure of ( mathrm{CO}_{2} ) of
4.0 atm over the liquid at ( 25^{circ} mathrm{C} ) is ( 1.2 times )
( 10^{-1} ) M. The Henry’s law constant for
( C O_{2} ) at this temperature is
A ( cdot 3.0 times 10^{-2} mathrm{mol} / mathrm{L}- ) atm
B . ( 4.5 times 10^{-3} ) mol ( / L- ) atm
c. ( 5.6 times 10^{-3} mathrm{mol} / mathrm{L}- ) atm
D. ( 2.3 times 10^{-2} mathrm{mol} / mathrm{L}- ) atm
12
226The increase in boiling point of a solution containing ( 0.6 g ) urea in ( 200 g )
water is ( 0.50^{circ} mathrm{C} ). Find the molal
elevation constant.
A ( cdot 10 K ) kg mol( ^{-1} )
в. ( 10 mathrm{K} ) g ( mathrm{mol}^{-1} )
c. ( 10 K ) kg moll ( l )
D. ( 1.0 K ) kg mol( ^{-1} )
12
227Illustration 2.72 The vapour pressure of pure benzene
at 50°C is 268 mm of Hg. How many moles of non-volatile
solute per mole of benzene are required to prepare a solution
of benzene having a vapour pressure of 160.0 mm of Hg at
50°C?
12
228Q13. Why ethyl alcohol is completely miscible with water?
Ang
Tu.
.
1
12
229Which of the following solutions is an example of negative deviation from
Raoult’s law?
A. Acetone + Ethanol
B. Carbon tetrachloride + Chloroform
c. Acetone + chloroform
D. water + Ethanol
12
230Molarity of a substance decreases with increase in temperature.
A. True
B. False
12
231Equal weights of methane and oxygen are mixed in an empty container at
( 25^{circ} mathrm{C} . ) The fraction of the total pressure
exerted by oxygen is:
A ( cdot frac{1}{3} )
B. ( frac{1}{2} )
( c cdot frac{2}{3} )
D.
12
232A solution containing 0.5 g of naphthalene in 50 g ( C C l_{4} ) yield a
boiling point elevation of ( 0.4 mathrm{K}, ) while a
solution of ( 0.6 mathrm{g} ) of an unknown solute in the same mass of the solvent gives a
boiling point elevation of 0.65 K. Find
the molar mass of the unknown solute.
12
233Statement 1: A supersaturated solution of glucose in boiling water crystallizes as it cools.

Statement 2 : The solubility increases as the temperature increases.
A. Both Statement 1 and Statement 2 are correct and Statement 2 is the correct explanation of Statement 1
B. Both Statement 1 and Statement 2 are correct and Statement 2 is not the correct explanation of Statement 1
c. statement 1 is correct but statement 2 is not correct
D. Statement 1 is not correct but Statement 2 is correct
E. Both the Statement 1 and Statement 2 are not correct

12
234An ideal solution has two components
( A ) and ( B . A ) is more volatile than ( B ), i.e.
( boldsymbol{P}_{A}^{circ}>boldsymbol{P}_{B}^{circ} ) and also ( boldsymbol{P}_{A}^{circ}>boldsymbol{P}_{text {total}} . ) If ( boldsymbol{X}_{boldsymbol{A}} )
and ( Y_{A} ) are mole fractions of
components ( A ) in liquid and vapour
phases, then :
A. ( X_{A}=Y_{A} )
в. ( X_{A}>Y_{A} )
c. ( X_{A}<Y_{A} )
D. Data insufficient
12
235Q. 45 What is “semipermeable membrane”?12
236( Delta_{f} G^{o} ) at ( 500 K ) for substance ( S ) in liquid state and gaseous state are ( +100.7 k c a l m o l^{-1} ) and
( +103 k c a l ) mol( ^{-1} ) respectively. Vapour pressure of liquid ( S ) at ( 500 K ) is approximately equal to: ( (R= )
( left.2 operatorname{cal} K^{-1} m o l^{-1}right) )
A. 0.1 atm
B. 1 atm
c. 10 atm
D. 100 atm
12
237State Henry’s law.12
238For a dilute solution, Raoult’s law states
that:
A. The relative lowering of vapour pressure is equal to the mole fraction of solute
B. The relative lowering of vapour pressure is equal to the mole fraction of solvent
C. The relative lowering of vapour pressure is proportional to the amount of solute in solution
D. The vapour pressure of the solution is equal to the mole fraction of solvent
12
239If in a solvent, n simple molecules of solute combine to form an associated
molecule, ( alpha ) is the degree of association, the van’t Hoff’s factor is
equal to:
A. ( frac{1}{1-n alpha} )
B. ( 1-alpha+n alpha )
( c cdot_{1-alpha+frac{alpha}{n}} )
D. ( frac{alpha}{n}-1+alpha )
12
240Which of the following does not define
solubility?
A. The concentration of solute in a saturated solution
B. The moles of solute dissolved in a given volume of solution
C. The maximum mass of solute that can dissolve in a given volume of solution
D. The minimum moles of solute needed to produce one litre of a saturated solution
12
241At ( 25^{circ} mathrm{C} ) the saturated vapour pressure
of water is 3.165 kPa ( (23.75 mathrm{mm} mathrm{Hg}) ) Find the saturated vapour pressure of a ( 5 % ) aqueous solution of urea (carbamide) at the same temperature.
(Molar mass of urea ( =mathbf{6 0 . 0 5} ) g ( boldsymbol{m o l}^{-1} ) )
12
242The mole fraction of ( H N O_{3} ) in an
aqueous binary solution is ( 0.15> ) The
ratio of moles of ( H N O_{3} ) to ( H_{2} O ) in the
solution is nearly:
( mathbf{A} cdot 17: 3 )
B. 3: 17
c. 1: 1
D. 15: 100
12
243A water sample contains 81 ppm of
( boldsymbol{C a}left(boldsymbol{H} boldsymbol{C O}_{3}right)_{2}, 73 ) ppm of ( boldsymbol{M} boldsymbol{g}left(boldsymbol{H} boldsymbol{C O}_{3}right)_{2} )
68 ppm of ( C a S O_{4} ) and 60 ppm of
( M g S O_{4} . ) What is the hardness of the
Water sample? (Atomic weights of calcium, magnesium and sulphur are respectively 40,24 and 32 ).
A. 50 ppm
B. 100 ppm
c. 150 ppm
D. 200 ppm
12
244A liquid will boil when:
A. enough salt has been added to it
B. the vapor pressure of the liquid is equal to the atmospheric or surrounding pressure
C. the vapor pressure of the liquid reaches ( 760 mathrm{mmHg} )
D. conditions favor the liquids molecules to be closer together
E. it has been brought up to a higher elevation
12
245Assuming that concentration of ( C a^{2+} )
ions in solution is in equal equivalence ratio to chloride ions, the hardness of water is :
A ( .9 .180 times 10^{3} ) ppm
B . ( 6.180 times 10^{3} ) ppm
c. ( 12.180 times 10^{3} ) ppm
D. ( 4.180 times 10^{3} ) ppm
12
2460.6 ml of glacial acetic acid with density ( 1.06 g / m l ) is dissolved in ( 1 k g ) water and the solution froze at
( -0.0205^{circ} mathrm{C} . ) Calculate van’t Hoff factor:
( boldsymbol{K}_{f} ) for water is ( 1.86 boldsymbol{K} boldsymbol{k g} boldsymbol{m o l}^{-1} )
12
247Which of the following is weakly acidic?
В. ( 0.1 M ) NaCl
( mathrm{c} cdot 0.1 mathrm{M} quad mathrm{HC}_{2} mathrm{H}_{3} mathrm{O}_{2} )
D. ( 0.1 M quad C H_{3} O H )
E. ( 0.1 M ) KOH
12
248If ( 684 g ) of sucrose ( (M M=342 g) ) is
dissolved in ( 2000 g ) of ( H_{2} O ) (essentially
( 2 L), ) what will be the freezing point of this solution?
A . -0.51
B . -1.86
c. -3.72
D. – 6.58
12
249A mixture of ethyl alcohol and propyl alcohol has a vapour pressure of 290 ( mathrm{mm} ) at ( 300 mathrm{K} . ) The vapour pressure of propyl alcohol is ( 200 mathrm{mm} ). If the mole
fraction of ethyl alcohol is ( 0.6, ) its vapour pressure(in ( mathrm{mm} ) ) at the same temperature will be:
A . 350
в. 300
c. 700
D. 360
12
250Which of the following weak electrolytes would give aqueous solution having ( 3 C alpha ) anion concentration?
A ( . A_{3} B )
B. ( A_{3} B_{2} )
( mathrm{c} cdot A B_{3} )
D. ( A_{3} B_{4} )
12
251A closed vessel is maintained at a
constant temperature. It is first evacuated and then vapour is injected into it continuously. The pressure of the vapour in the vessel is:
A. increases continuously
B. first increases and then remains constant
c. first increases and then decreases
D. none of the above
12
252True or False.
The components of a mixture can never
be separated by physical methods.
12
253Calculate osmotic pressure of a solution (write only integer part) obtained on mixing ( 100 mathrm{mL} ) of ( 3.4 % ) (mass/vol) solution of urea (molar
mass 60 ) and ( 50 mathrm{mL} ) of ( 1.6 % ) (mass/vol)
solution of cane sugar (molar mass 342
( operatorname{at} 27^{circ} C )
12
254What type of deviation from Raoult’s law is exected?
(a) when equal volume of acetone and
ethanol is mixed?
(b) when equal volume of acetone and chloroform is mixed?
12
255Select incorrect statements.
A. ( N H_{3} ) is soluble in water due to hydrogen bonding as well as due to formation of ions.
B. Gases which can be liquefied easily are more soluble in water then the gases which cannot be liquefied.
C. The solute follows Henry law at all pressure of gas.
D. The solute follows Henry law at low pressure of gas.
12
2561 L of ( 0.15 M H C l ) and 1 L of ( 0.3 M )
( H C l ) is given. What is the maximum
volume of ( 0.2 M H C l ) which one can
make from these two solutions? No
( mathbf{A} cdot 1.2 L )
B. ( 1.5 L )
c. ( 1.3 L )
D. ( 1.4 L )
12
257Sea water is found to conatin
( mathbf{5 . 8 5 %} ) Nacl and ( mathbf{9 . 5 0 %} boldsymbol{M g C l}_{2} ) by
weight of solution. Calculate its normal
boiling point assuming ( 80 % ) ionisation for ( N a C l ) and ( 50 % ) ionisation of
( M g C l_{2} )
( left[boldsymbol{K}_{boldsymbol{b}}left(boldsymbol{H}_{2} boldsymbol{O}right)=mathbf{0 . 5 1} boldsymbol{k g} boldsymbol{m o l}^{-1} boldsymbol{K}right] )
A. ( T_{b}=51.15^{circ} mathrm{C} )
в. ( T_{b}=78.6^{circ} mathrm{C} )
c. ( T_{b}=102.3^{circ} mathrm{C} )
D. ( T_{b}=157.2^{circ} mathrm{C} )
12
258( H_{2} S, ) a toxic gas with rotten egg like smell, is used for the qualitative
analysis. If the solubility of ( H_{2} S ) in water at STP is ( 0.195 mathrm{m} ), Calculate Henry’s law constant.
A. 282.0 bar
B. 324.8 bar
c. 462.9 bar
D. 534.8 bar
12
259A certain liquid mixture of two liquids ( A ) and B (behaving ideally) has a vapour
pressure 70 torr ( (1 text { torr }=1 mathrm{mm}) ) at ( 25^{circ} mathrm{C} ) for a certain mole fraction ( X ) of ( A ). For the same mole fraction ( X ) for ( B ) in the
mixture, the vapour pressure of mixture
is 90 torr at ( 25^{circ} mathrm{C} . ) If ( boldsymbol{P}_{A}^{0}-boldsymbol{P}_{B}^{0}=mathbf{4 0} ) torr
calculate ( P_{A}^{0}, P_{B}^{0} ) and ( X )
A . 100 torr, 60 torr, 0.25
B. 120 torr, 80 torr, 0.25
c. 200 torr, 160 torr, 0.25
D. 220 torr, 180 torr, 0.25
12
260Henry’s law constant for oxygen
dissolved in water is ( 4.34 times 10^{4} ) atm at
( 25^{C} . ) If the partial pressure of oxygen in air is 0.4 atm. Calculate the
concentration (in moles per litre) of the dissolved oxygen in water in
equilibrium with air at ( 25^{circ} C )
( mathbf{A} cdot 5.11 times 10^{-4} )
В. ( 5.11 times 10^{-3} )
c. ( 9.2 times 10^{-6} )
D. ( 0.92 times 10^{-6} )
12
261Illustration 2.188 0.1 M aqueous solution of MgCl, at 300K
is 4.92 atm. What will be the percentage ionization of the salt?
a. 49% b. 59% c. 79% d. 69%
12
262( 56 mathrm{g} ) of nitrogen and ( 96 mathrm{g} ) of oxygen are mixed isothermally and at a total pressure of 10 atm. The partial pressures of oxygen and nitrogen (in atm) are ( _{text {- – }} ) -respectively
( A cdot 4,6 )
B. 5,5
c. 2,8
( D cdot 6,4 )
12
263When acetone and chloroform are
mixed, hydrogen bonding takes place between them. Such a liquid pair will
cause:
A. Positive deviation from Raoult’s law
B. Negative deviation from Raoult’s law
c. No deviation from Raoult’s law
D. cannot be predicted
12
264Find the freezing point of a solution containing 0.5 mole of glucose dissolved in 200 g of ( H_{2} ) O? (Given that ( boldsymbol{K}_{f} ) for water is ( 1.86 quad boldsymbol{K} boldsymbol{m}^{-1} )
A . -4.65
B . -2.65
c. -14.65
D. -8.65
12
265Example 2.28 0.5 g KCl was dissolved in 100 g water, and
the solution, originally at 20°C froze at -0.24°C. Calculate
the percentage ionization of salt. K. per 1000 g of water
= 1.86°C.
12
266Assuming each salt to be ( 90 % ) dissociated which of the followings will have highest osmotic pressure?
A. Decimolar ( A l_{2}left(S O_{4}right)_{3} )
B. Decimolar ( B a C l_{2} )
c. Decimolar ( N a_{2} S O_{4} )
D. A solution obtained by mixing equal volumes of ( (b) ) and (c) and filtering
12
267What is a mixture?
A. Substance with two or more different particles
B. Substance that is insoluble
c. substance with a single homogenous particle
D. None of above
12
268Which of the following aqueous solutions should have the highest boiling point?
A. ( 1.0 M ) NaOH
в. ( 1.0 M ) Na( _{2} ) SO ( _{4} ).
с. ( 1.0 M ) NH( _{4} N O_{3} )
12
2699. The molal boiling point constant for water is 0.513 Km-‘,
When 0.1 mole of sugar is dissolved in 200.0 g of water,
the solution boils under a pressure 1.0 atm at
a. 100.513°C
b. 100.0513°C
c. 100.256°C
d. 101.025°C
12
270To ( 500 c m^{3} ) of water ( 3.0 times 10^{-3} k g ) of
acetic acid is added. If ( 23 % ) of acetic
acid is dissociated, what will be the depression of freezing point? ( left[K_{f} ) and density of water are right. ( 1.86 K k g m o l^{-1} ) and ( 0.997 g c m^{-3} )
respectively
в. ( 0.33 K )
c. ( 0.98 K )
D. ( 0.68 K )
12
271Two elements ( A ) and ( B ) form
compounds having molecular formulae
( A B_{2} ) and ( A B_{4} . ) When dissolved in 20.0 g
of benzene, 1.0 g of ( A B_{2} ) lowers the freezing point by ( 2.3^{circ} mathrm{C} ), whereas ( 1.0 mathrm{g} )
of ( A B_{4} ) lowers the freezing point by
( 1.3^{circ} mathrm{C} . ) The molal depression constant for benzene in 1000 g is ( 5.1 . ) Calculate the atomic masses of ( A ) and ( B )
12
272The concentration of which of the
following solution has the highest
value?
A. Dilute solution
B. Concentration solution
c. saturated solution
D. Supersaturated solution
12
273We separate mixtures to:
A. remove unwanted components
B. to get pure substances
C. Both of the above
D. None of the above
12
274Hlustration 2.114 A solution of urea in water has boiling
point of 100.15°C. Calculate the freezing point of the same
solution if K, and K, for water are 1.87 K kg mol-1 and
0.52 K kg mol-, respectively.
12
275At temperature ( T_{1} ) and composition
Q,which of the following is true?
This question has multiple correct options
A. Vapour phase is richer in B while liquid phase is richer in ( A )
B. Distillation of composition Q gives only pure A
C. Distillation of composition ( Q ) gives pure ( A ) and pure ( B )
D. Distillation of composition Q gives higher percentage of B than A.
12
276Predict whether van’t HOff factor
( (i) ) is
less than one or greater than one in the
following:
(i) ( C H_{3} C O O H ) dissolved in water
(ii) ( C H_{3} C O O H ) dissolved in benzene
12
277A ( 5.8 % ) solution of ( N a C l ) has vapour
pressure closest to
A . ( 5.8 % ) solution of urea
B. 2 ( M ) solution of glucose
c. ( 1 M ) solution of urea
D. 5.8 % solution of glucose
12
278Which of the following substances will lose its solutbility with increase in temperature?
A . ( N a O H )
в. ( N a_{2} C O_{3} )
c. ( N a_{2} S O_{4} )
D. All
12
279Which one is not equal to zero for an
ideal solution?
A. ( Delta V_{operatorname{mix}} )
B. ( Delta P=P_{text {observed }}-P_{text {Rooult}} )
c. ( Delta H_{operatorname{mix}} )
D. ( Delta S_{text {mix }} )
12
280Dry air was drawn through bulbs containing a solution of 40 grams of
urea in 300 grams of water, then through bulbs containing pure water at the same temperature and finally through a tube in which pumice
moistened with strong ( H_{2} S O_{4} ) was kept. The water bulbs lost
( 0.0870 g r a m s ) and the sulphuric acid
tube gained 2.036 grams. Calculate the
molecular weight of urea.
D. ( M=93.6 )
12
281The vapour pressure of ethanol and methanol are 44.5 mm ( H g ) and 88.7 mm ( H g ) respectively. An ideal
solution is formed at the same
temperature by mixing ( 60 g ) of ethanol with ( 40 g ) of methanol. The total vapour pressure of the solution and the mole
fraction of methanol in the vapour are respectively:
A. ( 43.46 mathrm{mm} ) and 0.51
в. ( 66.13 mathrm{mm} ) and 0.657
c. ( 66.15 mathrm{mm} ) and 0.791
D. 70.59 ( m m ) and 0.657
12
282The vapour pressure of a dilute aqueous solution of glucose is ( 750 mathrm{mm} ) of ( mathrm{Hg} ) at
( 373 mathrm{K} ). Calculate molality.
12
2830.19 Consider the figure and mark the correct option.
Piston (AJ Piston (8)
SPM
Fresh water
(A)
Concentrated
sodium chloride
solution in
water (B)
(a) Water will move from side (A) to side (B) if a pressure lower osmotic pressure is
applied on piston (B)
(b) Water will move from side (B) to side (A) if a pressure greater than osmotic
pressure is applied on piston (B)
(c) Water will move from side (B) to side (A) if a pressure equal to osmotic pressure
is applied on piston (B)
(d) Water will move from side (A) to side (B) if pressure equal to osmotic pressure is
applied on piston (A)
12
284When acetone and chloroform are
mixed together, hydrogen bonds are formed between them. Which of the
following statements is correct about the solution made by mixing acetone and chloroform ?
A. on mixing acetone and chloroform will form an ideal solution
B. On mixing acetone and chloroform positive deviation is shown since the vapour pressure increases
c. on mixing acetone and chloroform negative deviation is shown since there is decrease in vapour pressure
D. At a specific composition, acetone and chloroform will form minimum boiling azeotrope
12
285Question 4. Concentrated nitric acid used in laboratory work is
68% nitric acid by aqueous solution. What should be the molarity of such
a sample of the acid if the density of the solution is 1.504 g L-lo
w () Since mass percentage i.e., mass of solute (HNO.) in 100 g solution is
given, find mass of HNO3; then calculate its molar mass and number
of moles.
(ii) From density, find the volume of solution
(iii) Calculate the molarity by applying the formula,
Moles of solute
Molarity = 7
Volume of solution (in )
12
286A non ideal solution was prepared by
mixing ( 30 mathrm{ml} ) chloroform and ( 50 mathrm{ml} ) acetone. The volume of mixture will be :
( A cdot>80 m l )
в. ( 80 m l )
12
287Some liquids on mixing form
‘azeotropes’. What are ‘azeotropes’?
12
288Out of 0.1 molal aqueous solution of
glucose and 0.1 molal aqueous solution of ( K C l, ) which one will have higher boiling point and why?
12
289Calculate the vapour pressure of solution having 3.42 g of canesugar in 180 g water at ( 40^{circ} C ) and ( 100^{circ} ) C. Given that, the boiling point of water is ( 100^{circ} mathrm{C} ) and heat of vaporisation is 10 kcal
( m o l^{-1} ) in the given temperature range. Also, calculate the lowering in vapour pressure of 0.2 molal cane-sugar at
( 40^{circ} C: )
( mathbf{A} .58 mathrm{mm} )
B. ( 13 mathrm{mm} )
c. ( 78 mathrm{mm} )
D. none of these
12
290Question 30. Calculate the amount of benzoic acid (CH-COOH)
required for preparing 250 mL of 0.15 M solution in methanol.
As molarity is given, apply the formula for molarity, to find the mass of
es benzoic acid.
12
291( 50 mathrm{mL} ) of sample of hard water gave good lather with ( 6 mathrm{mL} ) of standard soap solution (1 mL soap solutions = 1 mg ( mathrm{CaCO}_{3} ). If the hardness is only due to
( M gleft(H C O_{3}right)_{2}, ) the weight of milk of lime required to remove the hardness completely from ( 100 mathrm{kg} ) of that sample of water is:
A. ( 17.8 mathrm{g} )
в. ( 8.9 mathrm{g} )
c. ( 178 g )
D. 89 ( g )
12
292What is the molarity of ( H C l ) in a solution prepared by dissolving ( 5.5 mathrm{g} ) ( H C l ) in 200 g ethanol if the density of the solution is 0.79 g/ mL?
A . 0.58 M
B. 0.21
c. 0.93 M
D. 1.7 м
12
( mathbf{A} )
B.
( mathbf{C} )
( D )
12
294The decrease in the freezing point of an aqueous solution of a substance is
( 1.395 k ) and that in the
freezing point of benzene solution of
the same substance is ( 1.280 k . ) Explain
the difference in ( Delta T ).
The substance:
A. dissociates in the aqueous solutio as well as in the benzene solution
B. forms complex in solution
c. associates in the benzene solution
D. dissociates in the aqueous solution and not in the benzene solution
12
295For weak electrolytes, van’t Hoff factor ‘i
is a measure of the degree of
dissociation of weak electrolyte. If true enter 1 , if false enter 0 .
12
296Illustration 2.78 At 25°C, the vapour pressure of pure
water is 25.0 mm Hg and that of an aqueous dilute solution
of urea is 20 mm Hg. Calculate the molality of the solution.
12
297( mathbf{H}_{2} mathrm{O}_{2} ) is sold as a solution of
approximately ( 5.0 mathrm{g} mathrm{H}_{2} mathrm{O}_{2} ) per ( 100 mathrm{ml} ) of the solution the molecular mass of
( mathbf{H}_{2} mathbf{O}_{2} ) is ( mathbf{3 4} . ) The molarity of this solution is approximately:
A . ( 1.15 mathrm{M} )
в. 1.5 М.
c . ( 3.0 mathrm{M} )
D. 3.4M
12
298For a very dilute aqueous solution of
( boldsymbol{K}_{4}left[boldsymbol{F} boldsymbol{e}(boldsymbol{C} boldsymbol{N})_{6}right], ) van’t Hoff factor is :
( mathbf{A} cdot i=11 )
в. ( i=5 )
( c cdot_{i}=frac{1}{11} )
D. ( i=10 )
12
299The freezing point of a 0.05 molal solution of a non-electrolyte in water is:
( mathbf{A} cdot-0.093^{circ} mathrm{C} )
B . ( 1.86^{circ} mathrm{C} )
( mathbf{c} cdot 0.93^{circ} mathrm{C} )
D. ( 0.093^{circ} mathrm{C} )
12
300What is the amount of urea dissolved
per litre, if aqueous solution is isotonic with ( 10 % ) cane sugar solution: (mol. wt of urea ( =mathbf{6 0} ) )?
A ( .200 g / L )
в. ( 19.2 g / L )
c. ( 17.54 g / L )
D. ( 16.7 g / L )
12
301The osmotic pressure of solution increases if:
A. temperature is decreased
B. concentration is decreased
c. number of solute molecules are increased
D. volume is increased
12
302A solution containing ( 0.122 mathrm{kg} ) of
benzoic acid in ( 1 k g ) of benzene
(b.pt.353 K) boils at ( 354.5 K )
Determine the apparent molar mass of benzoic acid (which dimerizes) in
the solution and the degree of
dimerization
Given: ( Delta_{v a p} H_{1 m}(text {benzene})= )
( mathbf{3 9 4 . 5 7} boldsymbol{J} boldsymbol{g}^{-1} )
A. 0.214 kg ( mathrm{mol}^{-1}, 0.86 )
в. 0.257 kg ( m o l^{-1}, 0.932 )
c. ( 0.428 mathrm{kg} mathrm{mol}^{-1}, 0.956 )
D. ( 0.454 mathrm{kg} mathrm{mol}^{-1}, 0.986 )
12
303Mlustration 2.117 In a cold climate water gets frozen
causing damage to radiator of a car. Ethylene glycol is used
as an antifreezing agent. Calculate the amount of ethylene
glycol to be added to 4 kg of water to prevent it from freezing
at -6°C. (K for water = 1.85 K kg mol-!)
12
304Pick out the mixture from the following.
A. water
B. Oxygen
c. Carbon dioxide
D. Air
12
305The mass of ( N a_{2} C O_{3} ) required to
prepare ( 500 mathrm{ml} ) of ( 0.1 mathrm{M} ) solution is:
A . 10.6 g
B. ( 5.3 mathrm{g} )
c. ( 2.65 mathrm{g} )
D. 7.95
12
306A ( 5 % ) solution (w/v) of cane-sugar (Mol. weight ( =342 ) ) is isotonic with ( 0.877 % ) ( (w / v) ) of urea solution. Find molecular
weight of urea (round off to the nearest integer).
12
30718 g glucose ( left(C_{6} H_{12} O_{6}right) ) is added to
( 178.2 mathrm{g} ) of water. The vapour pressure of this aqueous solution at ( 100^{0} C ) in torr
is:
A . 7.60
B. 76.00
c. 752.40
D. 759.00
12
308( 14.2 mathrm{g} N a_{2} S O_{4} ) is present in ( 10^{2} mathrm{kg} )
water. Its concentration in ppm is:
A. 10 ppm
B. 100 ppm
c. 142 ppm
D. ( 14.2 mathrm{ppm} )
12
309The osmotic pressure of the solution obtained by mixing ( 200 mathrm{cm}^{3} ) of ( 2 % ) (mass-volume) solution of urea with
( 200 mathrm{cm}^{3} ) of ( 3.42 % ) solution of sucrose at
( mathbf{2 0} ) is?
A ( .421 P a )
в. ( 267 P a )
( c .5240 P a )
D. ( 153 P a )
12
310A student mixes ( 10.0 m L ) of
( 0.10 M A g N O_{3} ) with excess copper metal. The reaction should produce 0.107 gram of silver; however, the student obtains a mass of 150 grams of silver. Plausible explanations for this yield ( >100 % ) might include :
I. the student did not subtract the mass of the filter paper before recording
results.
II. the student did not thoroughly dry the sample before massing.
III. the copper metal did not react
completely.
A . I only
B. II only
c. I and II only
D. I and III only
E. I, II, and III
12
311An electrolyte ( A ) gives 3 ions and ( B ) is a non- electrolyte. If ( 0.1 ~ M ) solution of ( B )
produces an osmotic pressure ( P, ) then ( 0.05 M ) solution of ( A ) will produce an osmotic pressure, assuming that the electrolyte is completely ionised:
A . ( 1.5 P )
в. ( P )
( c .0 .5 P )
D. ( 0.75 P )
12
312What is a de-icing agent? How does it
work?
12
313The vapour pressure is a solvent decreased by ( 10 mathrm{mm} ) of mercuity when a non velocity was added to the solvent.
The mole traction of the solve in the
solution is ( 0.2 . ) What would be the mole
traction of the solvent.if decrease in the
vaspour pressure is t be ( 20 mathrm{mm} ) of mercurity?
A. 0.8
B. 0.6
( c cdot 0.4 )
( D cdot 0.2 )
12
314Molarity of the situation is depend on:
A. temperature
B. nature of solute dissolved
c. mass of solvent
D. pressure
12
315Wustration 2.136 A very small amount of a non-volatile
solute (that does not dissociate) is dissolved in 56.8 cm
of benzene (density 0.889 g cm-). At room temperature,
vapour pressure of this solution is 98.88 mm Hg while that of
benzene is 100 mm Hg. Find the molality of this solution. If
the freezing temperature of this solution is 0.73 degree lower
than that of benzene, what is the value of molal the freezing
point depression constant of benzene?
12
316Molality of a solution in aqueous medium is ( 0.8 . ) Calculate its mole
fraction and the percentage by mass of solute if molar mass of solute is 60 .
A. ( 0.014,4.8 % )
В. ( 0.014,5 % )
c. ( 0.1,4.8 % )
D. ( 0.4,8 % )
12
317When 100 g of a saturated solution is evaporated at ( 50^{circ} mathrm{C}, 50 mathrm{g} ) of solid is left over. Find the solubility of the
substance at ( 50^{circ} mathrm{C} )
A . 100
B. 50
c. 75
D. 28
12
318A 100 solution of ( N a_{2} C O_{3} ) is prepared
by dissolved 8.653 of the salt in water. The density of the solution is ( 1.0816 / ) What are the Molarity and Molality of the solution?
(Atomic mass of Na is 23 , e is 12 and of
O is 14 )
12
319Based on solute-solvent interactions,
arrange the following in order of increasing solubility in n-octane and explain.
Cyclohexane, ( boldsymbol{K} boldsymbol{C l}, boldsymbol{C H}_{3} boldsymbol{O H}, boldsymbol{C H}_{3} boldsymbol{C N} )
12
320An aqueous solution is 1 molal in ( K I )
Which change will cause the vapour pressure of the solution to increase?
A. Addition of ( N a C l )
B. Addition of ( N a_{2} S O_{4} )
c. Addition of 1 molal ( K I )
12
321State True or False.
A binary solution which has same composition in liquid, as well as vapour phase, is called azeotropic mixture.
A. True
B. False
12
3220.5 Faraday of electricity was passed to deposit all the copper present in ( 500 mathrm{m} ) of ( C u S O_{4} ) solution. What was the
molarity of this solution?
A. 1 м
B. 0.5 M
c. ( 0.25 mathrm{M} )
D. 2.5м
12
323Illustration 2.85 Define molal elevation constant or
ebullioscopic constant.
12
324Isotonic solutions have:
A. same boiling point
B. same vapour pressure
c. same melting point
D. same osmotic pressure
12
325Which of the following conditions is not correct for ideal solution
A. no change in volume on mixing
B. no change in enthalpy on mixing
c. it obeys Raoults law
D. lonisation of solute should occurs to a small extent
12
326( p H ) of a ( 0.1 mathrm{M} ) monobasic acid is
measured to be ( 2 . ) Its osmotic pressure
at a given temperature of ( boldsymbol{T} ) Kis:
A . 0.1 RT
в. 0.11 RТ
c. ( 1.1 mathrm{RT} )
D. 0.01 RT
12
327Question 2. Calculate the mole fraction of benzene in solution
containing 30% by mass in carbon tetrachloride.
( Concentration 30% by mass shows that 30 g C He is dissolved in 100 g
solution or 70 g CCI. So, calculate the moles of each by dividing their
mass with their molecular mass.
(1) Then calculate the mole fraction by using the formula,
Number of moles of the component
Mole fraction of a component = =
Total number of moles of all components
A NA+ no
12
328Solid ( B eleft(N O_{3}right)_{2} ) is gradually dissolved in a ( 1.0 times 10^{-4} M N a_{2} C O_{3} ) solution. At
what concentration of ( B a^{2+} ) will a
percipitate begin to form?
( left(K_{S P} text { for } B a C O_{3}=5 times 10^{-9}right) )
A. ( 8.1 times 10^{-8} M )
в. ( 8.1 times 10^{-7} M )
c. ( 4.1 times 10^{-5} M )
D. ( 5.1 times 10^{-5} M )
12
329The mole fraction of water in ( 20 % )
aqueous hydrogen peroxide solution is:
A . 0.2
B. 0.8
( mathbf{c} .0 .883 )
D. 0.117
12
330Assertion
Amalgam of mercury with sodium is an
example of solid solutions
Reason
Mercury is solvent and sodium is solute
in the solution
A. Both Assertion and Reason are correct and Reason is
the correct explanation for Assertion
B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion
C. Assertion is correct but Reason is incorrect
D. Both Assertion and Reason are incorrect
12
331. 46 Give an example of a material used for making semipermeable membrane
for carrying out reverse osmosis.
ble motorial is used
12
332In a saturated solution the relative
amount of solute when
compared to the unsaturated solution.
A. More
B. Less
c. Equal
D. ( C, D )
12
3331. Pressure of 0.210 bat ar 37°C. The vapour pressure of pure
liquid (vapour pressure of water at 37°C = 0.198 bar) in
bar is
a. 0.448
b. 44.8 c. 0.224 d. 2.24
12
334ollowing factor(s)affect the solubility of a gaseous solute
Q. 27 Which of the following factor(s)affect the
in the fixed volume of liquid solvent?
(i) Nature of solute
(ii) Temperature
(iii) Pressure
(a) (i) and (iii) at constant T
(b) (i) and (ii) at constant p
(c) (ii) and (iii)
(d) Only (iii)
12
335What is the sum of the mole fractions of
all the components in a three
component system?
( A )
B. 2
( c cdot 3 )
( D cdot 1 / 3 )
12
336Two liquids ( A ) and ( B ) form ideal
solutions. At ( 300 K ), the vapour
pressure of solution containing 1 mole
of ( A ) and 3 mole of ( B ) is 550 mm ( H g . A t )
the same temperature, if one more mole
of ( B ) is added to this solution, the
vapour pressure of the solution increases by 10 mm ( H g . ) Determine the vapour pressure of ( A ) and ( B ) in the pure
( operatorname{states}(operatorname{in} operatorname{mm} H g) )
A .400,600
B .500,500
( mathbf{c} .600,400 )
D. None of these
12
337NLERI
Q. 15 The values of van’t Hoff factors for KCL, N
s for KCl, NaCl and K SO, respectively are
(a) 2, 2 and 2
Ans. (h) Number
(b) 2. 2 and 3
(d) 1, 1 and 1
(c) 1, 1 and 2
(c) 1, 1 and 2
off factors (1)
12
338The solubility of solutions which are neither exothermic nor endothermic
increases with increase in temperature
A. True
B. False
12
339The molarity ( (M) ) of ( K M n O_{4} ) solution in basic medium is :
( mathbf{A} cdot 0.8 M )
в. ( 0.08 M )
c. ( 0.26 M )
D. ( 0.026 M )
12
340The mole percentage of oxygen in a
mixture of ( 7 g N_{2} ) and ( 8 g O_{2} ) is :
A . 25
B. 75
c. 50
D. 40
12
341Question 1. Define the term solution. How many types of solutions are
formed? Write briefly about each type with an example.
12
342For an ideal solution with ( boldsymbol{p}_{boldsymbol{A}}>boldsymbol{p}_{boldsymbol{B}} )
which of the following is true?
( mathbf{A} cdotleft(x_{A}right)_{l i q}=left(x_{B}right)_{v a p} )
B . ( left(x_{A}right)_{l i q}>left(x_{B}right)_{v a p} )
C . ( left(x_{A}right)_{l i q}<left(x_{B}right)_{v a p} )
D. ( left(x_{A}right) ) liqand ( left(x_{B}right)_{v a p} ) do not bear any ralationship with each other
12
343AT ( 25^{circ} C, ) a solution containing 0.2 g of polyisobutylene in ( 100 mathrm{mL} ) of benzene developed a rise of ( 2.4 mathrm{mm} ) at osmotic equilibrium. The molar mass of polyisobutylene if the density of the solution is ( 0.88 mathrm{g} / mathrm{mL} ) is :
A ( cdot 2.39 times 10^{5} g m o l^{-1} )
B . ( 7.36 times 10^{5} mathrm{g} ) mol ( ^{-1} )
c. ( 5.45 times 10^{5} g ) mol ( ^{-1} )
D. None of these
12
344Vapour pressure of a liquid increases with :
A. decrease in temperature
B. increase in temperature
c. increase in surface area
D. increase in volume
12
345Describes a solution containing solute particles of intermediate size that do
not settle but do scatter light
A. Miscible
B. Suspension
c. colloid
D. Saturated
E. Supersaturated
12
346Mustration 2.95 The boiling point of benzene is 353.22
K. When 1.80 g of a non-volatile solute was dissolved in 90,
benzene, the boiling point is raised to 354.11 K. Calculate the
molar mass of the solute. (K, for benzene is 2.53 K kg mol-1)
12
347Q. 7 Considering the formation, breaking and strength of hydrogen bond,
predict which of the following mixtures will show a positive deviation
from Raoult’s law?
(a) Methanol and acetone
(b) Chloroform and acetone
(c) Nitric acid and water
(d) Phenol and aniline
Ans. (a) In pure methanol molecules are hydrogen bonded. On adding acetone, its molecules
12
348The vapour pressure of the solution of
two liquids ( Aleft(P^{circ}=80 m mright) ) and
( Bleft(p^{circ}=120 m mright) ) is found to be
( 100 m m ) when ( x_{A}=0.4 . ) The result
shows that:
A. Solution exhibits ideal behaviour
B. Solution shows positive deviations
c. Solution shows negative deviations
D. Solution will show positive deviations for lower concentration and negative deviations for higher concentrations
12
349Take small amounts of salt and add it to
large amounts of water. ( X ) is formed.
The substance present in small amount
is called ( Y ) whereas the substance
present in large amounts is called ( Z )
and the salt solution formed is called ( A )
The solution in which more of the solute
can be dissolved at a given temperature
is called ( B ) solution. The solution which
cannot be dissolved any more of the solute at a given temperature is ( C ) solution.
What is ( B ) ?
A. Salt solution
B. Unsaturated
c. Saturated
D. Super saturated solution
12
350A solution is prepaired by mixing ( 8.5 g )
of ( C H_{2} C l_{2} ) and ( 11.95 g ) of ( C H C l_{3} ). If
vapour pressure of ( boldsymbol{C H}_{2} boldsymbol{C l}_{2} ) and
( C H C l_{3} ) at ( 4298 K ) are 415 and
( 200 m m H g ) respectively, the mole
fraction of ( boldsymbol{C H C l}_{3} ) in vapour form is :
(molar mass of ( left.boldsymbol{C l}=mathbf{3 5 . 5} boldsymbol{g} boldsymbol{m o l}^{-1}right) )
( mathbf{A} cdot 0.162 )
B. 0.675
c. 0.325
D. 0.486
12
351Example 2.27 The K. (25°C) of sparingly soluble salt
XY,(s) is 3.56 x 10-5 (mol L-1)3 and at 30°C, the vapour
pressure of its saturated solution in water is 31.78 mm of Ho
Calculate the enthalpy change of the reaction
XY,(s) =
X2+(aq) + 2Y (aq)
Given: Vapour pressure of pure water = 31.82 mm of Hg
12
352Illustration 2.45 Ethylene bromide C,H,Br2, and
1,2-dibromopropane, C H Br,, form a series of ideal solutions
over the whole range of composition. At 85°C, the vapour
pressure of these two pure liquids are 173 and 127 torr,
respectively.
a. If 10.0 g of ethylene bromide is dissolved in 80.0 g of
1,2-dibromopropane, calculate the partial pressure of
each component and the total pressure of the solution
at 85°C.
b. Calculate the mole fraction of ethylene bromide in the
vapour in equilibrium with the above solution.
c. What would be the mole fraction of ethylene bromide
in a solution at 85°C equilibrated with a 50 : 50 mole
mixture in the vapour?
12
353Define an ideal solution and write one of
its characteristics.
12
354Consider seperate solutions of
( mathbf{0 . 5 0 0} boldsymbol{M} boldsymbol{C}_{mathbf{2}} boldsymbol{H}_{mathbf{5}} boldsymbol{O H}(boldsymbol{a q}), mathbf{0 . 2 5 0} boldsymbol{M} boldsymbol{K} boldsymbol{B r} )
( mathbf{0 . 1 2 5} boldsymbol{M} boldsymbol{N a _ { 3 }} boldsymbol{P O}_{4}(boldsymbol{a q}) ) and
( mathbf{0 . 1} boldsymbol{M} boldsymbol{M} boldsymbol{g}_{3}left(boldsymbol{P} boldsymbol{O}_{4}right)_{2} ) at ( mathbf{2 5}^{circ} boldsymbol{C} )
Which statement is true about these
solutions, assuming all salts to be strong electrolytes?
A ( cdot 0.125 M N a_{3} P O_{4}(a q) ) has the highest osmotic
pressure
B. ( 0.500 M C_{2} H_{5} O H(a q) ) has the highest osmotic pressure.
C. They all have the same osmotic pressure.
D. ( 0.100 M M g_{3}left(P O_{4}right)_{2}(a q) ) has the highest osmotic pressure
12
355gulo yuu.
Question 12. State Henry’s law and mention some important
applications?
Henry’s law is, p x, State this in the form of statement and give its
applications, like dissolution of Co, in soda water, less oxygen intake at
high altitudes etc.
12
356What weight of the non-volatile solute
urea ( left(N H_{2}-C O-N H_{2}right) ) needs to be
dissolved in 100 g of water by ( 25 % ) ? (in ( g m) )
12
357The vapour pressure of a pure liquid ( mathbf{A} ) is ( 80 mathrm{mmHg} ) at ( 300 K . ) It forms an ideal solution with liquid B. When the mole fraction of ( mathrm{B} ) is ( 0.4, ) the total pressure
was to be ( 88 mathrm{mmHg} ). The vapour pressure of liquid B would be?
12
358How much ammonia 1 M solution of
ammonium hydroxide contains? (in g)
( A cdot 35 g )
B. 17 g
( c cdot 348 )
D. None of these
12
359Depression of freezing point of which of the following solutions does represent the cryoscopic constant of water?
A. ( 6 % ) by mass of urea in aqueous solution.
B. 100 g of aqueous solution containing 18 g of glucose.
c. 59 g of aqueous solution containing 9 g of glucose.
D. 1 M ( K C l ) solution in water.
12
360A solution at ( 20^{circ} mathrm{C} ) is composed of 1.5
mol of benzene and 3.5 mol of toluene. If
the vapour pressure of pure benzene of
pure benzene and pure toluene at this temperature are 74.7 torr and 22.3 torr. respectively, then the total vapour pressure of the solution and the benzene mole fraction in equilibrium with it will be, respectively.
A. 38.0 torr and 0.589
B. 30.5 torr and 0.389
c. 35.8 torr and 0.280
D. 35.0 torr and 0.480
12
361What is the molarity of ( 11.2 V ) of ( H_{2} O_{2} )
( ? )
( mathbf{A} cdot mathbf{1} )
B. 2
( c .5 .6 )
D. 11.2
12
362Molecular mass of a non-volatile solute
can be determined by which of the following method?
A. cryoscopic method
B. Victor-Meyer’s method
c. Graham’s method
D. Duma’s method
12
363The osmotic pressure of an aqueous solution of sucrose is 2.47 atm at ( 303 mathrm{K} )
and the molar volume of the water
present is ( 18.10 mathrm{cm}^{3} . ) Given ( Delta H_{v a p}= ) ( mathbf{5 4 0} ) cal / g. Assume the volume of
solvent equal to the volume of the
solution. The elevation in the boiling point of the solution is :
A ( .5 .145 times 10^{-2} )
B. ( 7.565 times 10^{-2} )
c. ( 6.355 times 10^{-2} )
D. None of these
12
364Calculate the mass in mole of ( C O_{2} ) that
will dissolve in enough water to form
( 900 m L ) of solution at ( 20^{circ} mathrm{C} ) if the
partial pressure of ( boldsymbol{C O}_{2} ) is 1 atm. ( boldsymbol{K}_{boldsymbol{H}} ) for ( C O_{2} ) is ( 2.3 times 10^{-2} ) mol ( / ) litre
( a t m )
A . 0.0401 mole
B. 0.0301 mole
c. 0.0217 mole
D. 0.0207 mole
12
365Q. 14 Which of the following statements is false?
(a) Two different solutions of sucrose of same molality prepared in
different solvents will have the same depression in freezing point.
(b) The osmotic pressure of a solution is given by the equation i = CRT (where, C is
the molarity of the solution)
(c) Decreasing order of osmotic pressure for 0.01 M aqueous solutions of barium
chloride, potassium chloride, acetic acid and sucrose is
BaCl, > KCI > CH,COOH > sucrose
(d) According to Raoult’s law, the vapour pressure exerted by a volatile component
of a solution is directly proportional to its mole fraction in the solution
12
366The solubility of solid in a liquid solution ( _{-1-} ) with a decrease in
pressure.
A . increases
B. decreases
c. remains same
D. none of these
12
367The van’t Hoff factor for a dilute solution
of ( boldsymbol{K}_{3}left[boldsymbol{F} boldsymbol{e}(boldsymbol{C} boldsymbol{N})_{6}right] ) is likely to be:
A . 10
B. 4
( c cdot frac{1}{4} )
D.
12
368Solubility of salt ( X ) in water is 32 at ( 30^{circ} )
C. Calculate the amount of solvent
present in 500 g of saturated solution of ( X )
A. ( 160 mathrm{g} )
в. 379 g
c. ( 460 mathrm{g} )
( D cdot 68 g )
12
369When a substance is dissolved in a
solvent, the vapour pressure of solvent decrease. It brings This question has multiple correct options
A. a decrcase in boilings point of solution
B. an increase in boiling point of the solution
c. a decrease in freezing point of the solution
D. an increase in freezeing point of the solution
12
370Which of the following changes decreases the vapour pressure of water kept in a sealed vessel?
A. Decreasing the quantity of water
B. Increasing the quantity of water
c. Decreasing the volume of vessel to one-half
D. Decreasing the temperature of water
12
37127 Calculate the mass per cent of calcium, phosphorus and oxygen in
calcium phosphate Caz(PO4)2.
12
372At ( 10^{circ} mathrm{C}, ) the osmotic pressure of urea
solution is 500 mm. The solution is
diluted and the temperature is raised to
( 25^{circ} C, ) when the osmotic pressure is
found to be 105.3 mm. Determine
extent of dilution?
A. Sol. ( left(V_{text {final}}=5 V_{text {original}}right) )
B. Sol. ( ( left.V_{text {final}}=7 V_{text {original}}right) )
c. sol. ( left(V_{text {final}}=3 V_{text {original}}right) )
D. None of the above
12
373A certain substance ‘A’ tetramerises in
water to the extent of ( 80 % ). A solution of
2.5 g of ( A ) in 100 g of water lowers the
freezing point by ( 0.3^{circ} mathrm{C} ). The molar mass of ( A ) is:
A .122
B. 31
c. 244
D. 62
12
374Two liquids ( A ) and ( B ) form ideal
solutions. At ( 300 K ), the vapour
pressure of a solution containing 1 mole of ( A ) and 3 moles of ( B ) is 550 mm
Hg. At the same temperature, if one
more mole of ( B ) is added to this
solution, the vapour pressure of the
solution increases by 10 mm ( H g ). The
vapour pressure of ( A ) and ( B ) in their
pure states are respectively:
A ( cdot p_{A}^{o}=600 mathrm{mm} mathrm{Hg} ) and ( p_{B}^{o}=400 mathrm{mm} mathrm{Hg} )
B . ( p_{A}^{o}=500 mathrm{mm} mathrm{Hg} ) and ( p_{B}^{o}=560 mathrm{mm} mathrm{Hg} )
C ( cdot p_{A}^{o}=450 mathrm{mm} mathrm{Hg} ) and ( p_{B}^{o}=650 mathrm{mm} mathrm{Hg} )
D . ( p_{A}^{o}=400 mathrm{mm} mathrm{Hg} ) and ( p_{B}^{o}=600 mathrm{mm} mathrm{Hg} )
12
375Which of the following statement is
correct?
A. Dilution increases the extent of deviation of ideality
B. Dilution has no effect on deviation
c. Dilution decreases the extent of deviation from ideality
D. More concentrated the solution is, lesser will be the deviation
12
376( 1 mathrm{kg} ) of ( mathrm{NaOH} ) solution contains ( 4 mathrm{g} ) of NaOH. The approximate concentration
of the solution is:
A. 0.1 molar
B. 0.1 molal
c. decinormal
12
377Elevation in boiling point of ( boldsymbol{C a}left(boldsymbol{N} boldsymbol{O}_{3}right)_{2} )
gives molar mass as ( 131.2 . ) The degree of
dissociation of ( boldsymbol{C a}left(boldsymbol{N} boldsymbol{O}_{3}right)_{2} ) is:
A. ( 100 % )
B. ( 75 % )
( c .50 % )
D. ( 12.5 % )
12
378Find the amount of sodium nitrate
dissolved in ( 200 g ) of solvent if the mass by mass percent of solute in solution is
( mathbf{2 0 %} )
A . ( 20 g )
в. ( 50 g )
c. ( 30 g )
D. ( 40 g )
12
3790.3 At equilibrium the rate of dissolution of a solid solute in a volatile liquid
solvent is
(a) less than the rate of crystallisation
(b) greater than the rate of crystallisation
(c) equal to the rate of crystallisation
(d) zero
12
380( 1.4 mathrm{g} ) of acetone dissolved in ( 100 mathrm{g} ) of benzene gave a solution which freezes
at ( 277.12 mathrm{K} . ) Pure benzene freezes at
( 278.4 mathrm{K} .2 .8 mathrm{g} ) of a solid
(A) dissolved in
( 100 mathrm{g} ) of benzene gave a solution which froze at ( 277.76 mathrm{K} ). Calculate the molar mass of ( (A) )
12
381Vapour pressure of a solvent containing nonvolatile solute is
A. more than the vapour pressure of a solvent
B. less than the vapour pressure of solvent
C. equal to the vapour pressure of solvent
D. none
12
382Q. 35 Colligative properties are observed when ……..
(a) a non-volatile solid is dissolved in a volatile liquid
(b) a non-volatile liquid is dissolved in another volatile liquid
(c) a gas is dissolved in non-volatile liquid
(d) a volatile liquid is dissolved in another volatile liquid
12
383The vapor pressure of water is
( 12.3 K P a ) at ( 300 K . ) Calculate the vapor
pressure of 1 molal solution of a non-
volatile solute in it.
12
account for this effect we define a
quantity called the Van’t Hoff factor
given by :
[
boldsymbol{i}=
]
Actual number of particles in solution Number of formula units initiall
( i=1 ) (for non-electrolytes)
( i>1 ) (for non-electrolytes, undergoing dissociation) ( i<1 ) (for solutes, undergoing dissociation)

A solution of benzoic acid is dissolved
in benzene such that it undergoes
molecular association and its molar
mass approaches 244. The benzoic molecules will exist as:
A . Dimer
B. Monomer
C. Tetramer
D. Trimer

12
385The van’t Hoff factor of the benzoic acid
solution in benzene is ( 0.5 . ) In this
solution, benzoic acid:
A. dissociates
B. forms dimer
c. remains unchanged
D. forms tetramer
12
386The osmotic pressure of ( 40 % )
(weight/volume) urea solution is 1.64 ( operatorname{atm} ) and that of ( 3.42 % ) (weight/volume) cane sugar is 2.46 atm. When equal volumes of the above two solutions are
mixed, the osmotic pressure of the resulting solution is:
A. 1.64 atm
B. 2.46 atm
c. 4.10 atm
D. 2.05 atm
12
387The Henry’s law constant for the
solubility of ( N_{2} ) gas in water at ( 298 mathrm{K} ) is
( 1 times 10^{5} ) atm. The mole fraction of ( N_{2} ) in
air is ( 0.8 . ) The number of moles of ( N_{2} )
from a dissolved in 100 moles of water
at ( 298 mathrm{K} ) and 5 atm pressure is?
A. ( 4 times 10^{-4} )
В. ( 4 times 10^{-5} )
c. ( 4 times 10^{-3} )
D. ( 5 times 10^{-4} )
12
3880.5 Maximum amount of a solid solute that can be dissolved in a specified
amount of a given liquid solvent does not depend upon ………
(a) temperature
(b) nature of solute
(c) pressure
(d) nature of solvent
unt of
given
12
389A current of ( 965 A ) is passed for 100 sec
between inert electrodes in ( 500 m L )
solution of ( 2 M C u S O_{4} . ) The molarity of solution after electrolysis would be:
(Assume no change in volume)
A ( .2 M )
в. ( 1 M )
c. ( 4 M )
D. ( 0.5 M )
12
390Consider following cases:
I. ( 2 mathrm{M} C H_{3} mathrm{COOH} ) solution in benzene at
( 27^{0} ) where there is dimer formation to
the extent of ( 100 % )
Il. ( 0.5 mathrm{M} ) KCl aq. solution at ( 27^{0}, ) which
ionises ( 100 % )
Which is lare true statements(s):
A. both are isotonic
B. I is hypertonic
c. I lis hypertonic
D. none is correct
12
391Two solutions of glucose have osmotic
pressures 1.5 and ( 2.5 a t m .1 L ) of first is
mixed with ( 2 L ) of second solution, the
osmotic pressure of the resultant solution is:
A . ( 2.5+1.5 a t m )
B. 2.5 – 1.5atm
c. ( frac{2.5+1.5}{2} ) at
D. ( 2.16 a t m )
12
392Which facts are true when we use van’t
Hoff equation ( P V=C S T ) for osmotic
pressure ( mathrm{P} ) of dilute solutions?
This question has multiple correct options
A. The equation is identical to that of ideal gas equation
B. The solute particles in solution are analogous to the gas molecules and the solvent is analogous to the empty space between the gas molecules
C. Solute molecules are dispersed in the solvent, the way the gas molecules are dispersed in empty space
D. The equation is not identical to that of ideal gas equation
12
393Illustration 2.214 Calculate the Van’t Hoff factor (i) for the
following if:
i. 100% ionization or association takes place
ü. 50% ionization or association takes place
a. S
b. Se с. Те
d. P
e. As f. Sb
g. B
h. AICI,
i. Hg, Cl, j. HgCl, k. Be2C 1. A1.Cz
m. CaC, n. Mg,C,
12
394Under what condition the van’t Hoff
factor is greater than one?
12
395The molarity of ( boldsymbol{H} boldsymbol{N} boldsymbol{O}_{3} ) in a sample
which has density ( 1.4 mathrm{g} / mathrm{mL} ) and mass percentage of ( 63 % ) is
[Molecular Weight of ( left.boldsymbol{H} boldsymbol{N} boldsymbol{O}_{3}=boldsymbol{6 3}right] )
12
396Solutions that have the same osmotic
pressure are called (isotonic/isometric) solutions
12
397Calculate the vapour pressure lowering caused by addition of 50 g of sucrose (molecular mass ( =342 ) ) to 500 g of water if the vapour pressure of pure
water at ( 25^{circ} mathrm{C} ) is ( 23.8 mathrm{mm} mathrm{Hg} )
12
398Super heating is minimized by stirring and indirect ( _{—} ) (heating/cooling)12
399Molar ratio of a mixture of water and
absolute alcohol is ( 0.2 . ) The mole
fraction ratio of alcohol and water is :
12
400Calculate the weight of ( C a O ) required to
remove the hardness of 1000000 litre of
water containing 1.62 g of ( C a C O_{3} ) per litre.
12
401Choose the correct statement from the
following.
This question has multiple correct options
A. Liquor ammonia and soda water are examples of liquid-gas type mixtures.
B. Mixture of coconut oil and water can be separated using separating funnel
C. A mixture of iodine and sulphur can be separated using magnetic separation.
D. A mixture of sand and sawdust can be separated using solvent extraction.
12
402In a glass of water, we cannot
dissolve sugar more than a certain
limit. At this stage, the solution is said
to be:
A. saturated
B. unsaturated
c. supersaturated
D. complete solution
12
403Question 1. Components of a binary mixture of
mponents of a binary mixture of two liquids A and B
were being separated by distillation. After some time separation of
components stopped and composition of vapour phase became same as
that of liquid phase. Both the components started coming in the distillate.
Explain why this happened.
the distillate and
12
404A solution of urea (mol. mass 56
( left.g m o l^{-1}right) ) boils at ( 100.18^{circ} C ) at the
atmospheric pressure. If ( boldsymbol{K}_{f} ) and ( boldsymbol{K}_{boldsymbol{b}} ) for
water are 1.86 and 0.52 Kkg.mol( ^{-1} )
respectively, the above solution will freeze at:
A. ( -6.54^{circ} )
B. ( 6.54^{circ} mathrm{C} )
( c cdot 0.654^{circ} C )
D. ( -0.654^{circ} mathrm{C} )
12
405Benzoic acid undergoes dimerisation
in benzene solution.The vant Hoff factor
is related to the degree of association
( alpha^{prime} ) of the acid as :
A ( . i=1-alpha )
B . ( i=1+alpha )
C ( i=1-frac{alpha}{2} )
D. ( i=1+frac{alpha}{2} )
12
406Which of the following cannot be dissolved in water?
A . Ice
B. Sugar
c. wood
D. salt
12
407Calculate the mole fraction of ( N_{2} ) gas in
a mixture of ( N_{2} ) and ( O_{2} ). If the partial
pressure of ( boldsymbol{O}_{2} ) is ( 63 mathrm{cm} ) of ( mathrm{Hg} ) and the
total pressure of the mixture is ( 90 mathrm{cm} ) of Hg.
12
408The incorrect statement is :
A. Vapour pressure of a liquid always increases by increasing temperature.
B. Vapour pressure onlydepends on temperature and not on the nature of substance.
C. Vapour pressure does not depend on the quantity of the liquid taken and the surface area of the liquid.
D. Vapour pressure is not a colligative property & is independent of the concentration of the liquid.
12
409An aqueous solutions of diabasic acid (molecular mass ( =118 ) ) containing
( 35.4 mathrm{g} ) of acid per litre of the solution has density ( 1.0077 g m L^{-1} ). Find the mole fraction of the solvent.
12
410The Molarity of ( 200 m l ) of ( H C l ) solution
which can neutralise ( 1.6 g ) of anhydrous
( N a_{2} C O_{3} ) is:
( mathbf{A} cdot 1 M )
B. ( 0.1 M )
c. ( 0.6 M )
D. ( 0.75 M )
12
411Example 2.9 A4% solution of sucrose C,H,O,, is isotonic
with 3% solution of an unknown organic substance. Calculate
the molecular mass of the unknown substance.
12
412Ratio of solubilities of gases ( N_{2} & O_{2} ) in water from air at ( 25^{circ} ) and 1 atm will
be if air is ( 20 % ) by volume of ( O_{2} ) and ( 80 % )
by volume of ( N_{2} ) is:
[
begin{array}{c}
text { Given }: boldsymbol{K}_{boldsymbol{H}}left(boldsymbol{N}_{mathbf{2}}right)=mathbf{2} times mathbf{1 0}^{mathbf{4}} boldsymbol{a} boldsymbol{t} boldsymbol{m} \
boldsymbol{K}_{boldsymbol{H}}left(boldsymbol{O}_{2}right)=mathbf{1 0}^{4} boldsymbol{a} boldsymbol{t} boldsymbol{m}
end{array}
]
( A cdot 8: 1 )
B. 1: 8
c. 2: 1
D. 1: 2
12
4138. Equimolal solutions KCl and compound X in water show
depression in freezing point in the ratio of 4:1. Assuming KCI
to be completely ionized, the compound X in solution must
a. Dissociate to the extent of 50%
b. Hydrolyze to the extent of 80%
c. Dimerize to the extent of 50%
d. Trimerize to the extent of 75%
12
414For a given value of the degree of dissociation ( (alpha), ) which of the following
have correct van’t Hoff factor?
This question has multiple correct options
A. ( N a C l ; i=2+alpha )
в. ( C aleft(N O_{3}right)_{2} ; i=1+2 alpha )
c. ( K_{4}left[left(F e(C N)_{6}right] ; i=1+4 alpharight. )
D. ( left(N H_{4}right)_{3} P O_{4} ; i=3+alpha )
12
415If the above process is repeated for all other compositions of mixture of ( mathrm{C} ) and
B. If all the points where vapours start converting into liquid are connected and all the points where vapours get
completely converted into liquid are connected then obtained graph will look
like
( A )
B. b-
( c cdot c )
( D cdot d )
12
416A 0.001 molal solution of
( left[boldsymbol{P t}left(boldsymbol{N} boldsymbol{H}_{3}right)_{4} boldsymbol{C l}_{4}right] ) in water has a freezing
point depression of ( 0.0054^{0} C . ) If ( K_{f} ) for water is ( 1.80, ) the correct formulation of
the above molecule is:
( mathbf{A} cdotleft[P tleft(N H_{3}right)_{4} C l_{3}right] C l )
B . ( left[P tleft(N H_{3}right)_{4} C l_{2}right] C l_{2} )
c. ( left[P tleft(N H_{3}right)_{4} C l_{2}right] C l_{3} )
D ( cdotleft[P tleft(N H_{3}right)_{4} C l_{4}right] )
12
4172.5 molar sulphuric acid contains:
This question has multiple correct options
A. ( 29.5 mathrm{g} ) of sulphuric acid per litre of solution.
B. ( 245.0 mathrm{g} ) of sulphuric acid per ( 1000 mathrm{ml} ) of solution.
C. ( 24.5 mathrm{g} ) of sulphuric acid per ( 100 mathrm{ml} ) of solution.
D. 59.0 g of sulphuric acid per litre of solution.
12
418mum boiling azeotrope at some specinc
(b)
2.28 IT two liquids A and B form minimum boiling azeotro
composition then
A B interactions are stronger than those between A-A or B
apour pressure of solution increases because more number on
liquids A and B can escape from the solution
(C) vapour pressure of solution decreases because less number of molecules
one of the liquids escape from the solution
(d) A-B interactions are weaker than those between A-A or B-B
because more number of molecules of
ses because less number of molecules of only
12
419Which choice is a gas which has a low
solubility in water?
A ( cdot N H_{3} )
в. ( C s H )
c. ( C H_{4} )
D. ( G a H_{3} )
12
4200.002 molar solution of NaCl having
degree of dissociation of ( 90 % ) at ( 27^{circ} C )
has osmotic pressure equal to
A. 0.94 bar
B. 9.4 bar
c. 0.0934 bar
D. ( 9.4 times 10^{-4} ) bar
12
421Illustration 2.111 1.4 g of acetone dissolved in 100 g of
benzene gave a solution which freezes at 277.12 K. Pure
benzene freezes at 278.4 K. 2.8 of solid (A) dissolved in 100 g
of benzene gave a solution which froze at 277.76 K. Calculate
the molecular mass of (A).
12
422The molar conductivity of acetic acid at
infinite dilution is 390.7 and for ( 0.1 mathrm{M} )
acetic acid solution is ( 5.2 mathrm{mhocm}^{2} ) mol
( -1 . ) The degree of dissociation of ( 0.1 mathrm{M} )
( mathrm{CH}_{3} mathrm{COOH} ) solution is:
A . ( 13.3 % )
B. 0.0133%
c. 1.33%
D. 133%
12
423The vapour pressure of pure benzene at
a certain temperature is 640 mm ( H g ). A
non-volatile solid weighing ( 2.715 g ) is
added to ( 39.0 g ) of benzene.

The vapour pressure of the solution is
( 600 m m H g . ) What is the molar mass of
the solid substance?

12
424Match the following:
List – List – II
1) Molality
A) unity
2) Relative
B) dilute solutions vapour lowering
3) Raoult’s law
C) independent of temperature
4) ( X_{text {solute}} X_{text {solvent}} )
D) Mole fraction of solute
( mathbf{A} cdot 1-C, 2-D, 3-B, 4-A )
B . ( 1-A, 2-C, 3-D, 4-B )
C ( .1-C, 2-B, 3-A, 4-D )
D . ( 1-D, 2-A, 3-B, 4-C )
12
425The solubility of gas in liquid is directly proportional to the pressure over the solutions at a given temperature.
A. True
B. False
12
426( mathbf{A} )
is a mixture of two or more
substances in a single phase.
A. Element
B. Compound
c. Solution
D. None of above
12
427Question 9. What is semipermeable membrane?12
428The boiling point of ( 95 % ) ethanol is higher than that of absolute ethanol.
A. True
B. False
12
429What is the mole fraction of the solution
in a ( 1.00 m ) aqueous solution?
A. 1.770
B. 0.0354
c. 0.0177
D. 0.177
12
430Which one is true for solutions showing
positive deviation from raoult’s law?
A. A-B interaction has nothing to do with positive deviations
B. A-B interactions are weaker than than those between
A-A and B-B
C. A-B interactions are stronger than those between A-A and B-B
D. A-B interactions are same as those between A-A and B-
( B )
12
431The value of Henry’s law constant for
some gases at ( 293 K ) is given below. Arrange the gases in the increasing order of their solubility. ( boldsymbol{H} boldsymbol{e}= )
( mathbf{1 4 4 . 9 7 k b a r} ; mathbf{H}_{mathbf{2}}=mathbf{6 9 . 1 6 k b a} )
( N_{2}=76.48 k b a r ; O_{2}=34.86 k b a r )
A. ( H e<N_{2}<H_{2}<O_{2} )
B. ( O_{2}<H_{2}<N_{2}<H e )
c. ( H_{2}<N_{2}<O_{2}<H e )
D. ( H e<O_{2}<N_{2}<H_{2} )
12
432Hlustration 2.44 A liquid mixture of benzene and toluene
is composed of 1 mol of benzene and 1 mol of toluene.
a. If the pressure over the mixture at 300 K is reduced,
at what pressure does the first vapour form?
b. What is the composition of the first trace of vapour
formed?
c. If the pressure is reduced further, at what pressure does
the last trace of liquid disappear?
d. What is the composition of the last trace of liquid?
e. What will be the pressure, the composition of the liquid,
and the composition of the vapour, when 1 mol of the
mixture is vapourized?
Given: Prº = 32.05 mm Hg, PR° = 103 mm Hg
12
433Assuming the compounds to be completely dissociated in aqueous solution, identify the pair of the solutions that can be expected to be isotonic at the same temperature.
A . ( 0.1 mathrm{M} ) Urea and ( 0.01 mathrm{M} ) Nac
B. 0.02 M NaCl and 0.01 M ( N a_{2} S O_{4} )
D. 0.01 M Sucrose and 0.02 M glucose
12
434Q. 14 Which of the following statements is false?
(a) Two different solutions of sucrose of same molality prepared in
different solvents will have the same depression in freezing point.
(b) The osmotic pressure of a solution is given by the equation t = CRT (where, C is
the molarity of the solution) |
(c) Decreasing order of osmotic pressure for 0.01 M aqueous solutions of barium
chloride, potassium chloride, acetic acid and sucrose is
BaCl, > KCI > CH2COOH > sucrose
(d) According to Raoult’s law, the vapour pressure exerted by a volatile component
of a solution is directly proportional to its mole fraction in the solution
CAFE
12
435Question 5. What is the significance of Henry’s law constant Ky?12
436The ratio of the value of any colligative property for ( N a C l ) solution of that of an
equimolal solution of sugar is nearly
( mathbf{2}: mathbf{1} )
A. True
B. False
12
437The molality of ( boldsymbol{H}_{2} boldsymbol{S} boldsymbol{O}_{4} ) solution is ( boldsymbol{9} ). The
weight of the solute in ( 1 mathrm{kg} H_{2} S O_{4} ) solution is:
A . ( 900.0 mathrm{g} )
в. ( 469 mathrm{g} )
c. ( 882.0 mathrm{g} )
D. ( 9.0 mathrm{g} )
12
438Which of the following is NOT soluble in
water?
A. Salt
B. Sugar
c. oxygen
D. None of these
12
439Which of the following solutions at the
same temperature will be isotonic?
A. ( 3.42 mathrm{g} ) of cane sugar in one litre water and ( 0.18 mathrm{g} ) of glucose in one litre water
B. 3.42 of cane sugar in one litre water and 0.18 g of glucose in 0.1 litre water
c. ( 3.42 mathrm{g} ) of cane sugar in one litre water and ( 0.585 mathrm{g} ) of NaCl in one litre water
D. 3.42 g of cane sugar in one litre water and 1.17 g of NaCl in one litre water
12
440For an ideal solution, ( Delta_{m i x} H ) is12
441Example 2.3 The vapour pressure of a 5% aqueous
solution of a non-volatile organic substance at 373 K is 745
mm. Calculate the molecular mass of the solute.
12
442A 3.4 g sample of ( mathrm{H}_{2} mathrm{O}_{2} ) solution containing ( x % mathrm{H}_{2} mathrm{O}_{2} ) by mass requires ( mathrm{x} )
( mathrm{ml} ) of a ( mathrm{KMnO}_{4} ) solution for complete oxidation under acidic condition. The
molarity of ( mathrm{KMnO}_{4} ) solution is :
( A )
B. 0.5
( c cdot 0.4 )
D. 0.2
12
443The osmotic pressure of ( 0.1 mathrm{M} ) aqueous
solution of ( M g C l_{2} ) at ( 300 mathrm{K} ) is ( 4.92 mathrm{atm} )
What will be the percentage ionization of the salt?
A . ( 49 % )
B. ( 29 % )
( c .39 % )
D. ( 69 % )
12
444Mixtures on separation can give
A. elements
B. compounds
c. both elements and compounds
D. impure substances
12
445The correct relationship between the boiling points of very dilute solutions of ( A l C l_{3}left(t_{1}right) ) and ( C a C l_{2}left(t_{2}right), ) having the same molar concentration, is :
A ( cdot t_{1}=t_{2} )
В. ( t_{1}>t_{2} )
c. ( t_{2}>t_{1} )
D. ( t_{2} geq t_{1} )
12
446Molarity is expressed as:
A. Gram/litre
B. Moles/litre
c. Litre/mole
D. Moles/1000 gms
12
447, (d) and L) both are correct.
Q. 28 Intermolecular forces between two benzene mo
strength as those between two toluene molecule
benzene and toluene, which of the following are not
(a) Amix H = zero
(b) Amix V = zero
(c) These will form minimum boiling azeotrope
(d) These will not form ideal solution
nzene molecules are nearly of same
lene molecules. For a mixture of
ng are not true?
12
448Illustration 2.123 How many grams of sucrose (molecular
weight 342) should be dissolved in 100 g water in order to
produce a solution with 105°C difference between the freezing
point and the boiling point? (K = 0.51°C m-1,K, = 1.86°C m-1)
12
449Calculate the mole fraction of benzene
in solution containing ( 30 % ) by mass in
( boldsymbol{C C l}_{4} ? )
12
450What are isotonic solutions? Give an
example.
12
451A mixture of two immiscible liquids at
a constant pressure of 1.0 atm boils at
temperature
A. Equal to the normal boiling point of more volatile liquid
B. Equal to the mean of the normal boiling points of two liquids.
C. Greater than normal boiling point of either of liquids.
D. Smaller than the normal boiling point of either of liquids.
12
452Relative decrease in vapor pressure is 0.4 for a solution containing 1 mole AB in 3 mol ( H_{2} O ), therefore ( A B ) is ionised at the
extent(percentage) of:
( mathbf{A} cdot 60 % )
B. ( 50 % )
( c cdot 100 % )
D. ( 40 % )
12
453One litre of ( C O_{2} ) ia passed through red hot coke. The volume become 1.4 litres
at same temperature and pressure The composition of product is
A. 0.8 litre of ( C O_{2} ) and 0.6 litre of ( C O )
B. 0.7 litre of ( C O_{2} ) and 0.7 litre of ( C O )
c. 0.6 litre of ( C O_{2} ) and 0.8 litre of ( C O )
D. 0.4 litre of ( C O_{2} ) and 1.0 litre of ( C O )
12
454In a mixture A and B components show
negative deviation as:
( mathbf{A} cdot Delta V_{m i x}=+v e )
B. ( Delta H_{text {mix}}=- )ve.
C. A-B interaction is weaker than A-A and B-B interaction.
D. None of the above reason is correct.
12
455Illustration 2.210 The freezing point of a 0.08 molal solution
of NaHSO, is -0.372°C. Calculate the dissociation constant
for the reaction.
HSO = H® + s0,2-
K, for water = 1.86 Km-1
12
456Molarity is defined as:
A. the number of moles of solute dissolved in one ( d m^{3} ) of
the solution.
B. the number of moles of solute dissolved in ( 1 mathrm{kg} ) of
solvent
C. the number of moles of solute dissolved in ( 1 d m^{3} ) of the
solvent.
D. the number of moles of solute dissolved in 100 ml of
the solvent.
12
457The vapour pressure of a solvent decreased by ( 10 mathrm{mm} ) of mercury when a non-volatile solute was added to the
solvent. The mole fraction of the solute
in the solution is 0.2. What should be the mole fraction of the solvent if the
decrease in the vapour pressure is to be ( 20 mathrm{mm} ) of mercury?
A. 0.4
B. 0.6
( c cdot 0.8 )
( D cdot 0.2 )
12
458Solute ( A ) is a ternary electrolyte and solute B is a non-electrolyte. If ( 0.1 mathrm{M} ) solution of solute B produces an
osmotic pressure of ( 2 P, ) then 0.05
M solution of ( A ) at the same
temperature will produce an osmotic
pressure equal to:
A . ( 1.5 P )
B. 2P
( c cdot 3 P )
D.
12
459Illustration 2.162 3% solution of glucose is isotonic with 1%
solution of non-volatile non-electrolyte solute. The molecular
mass of the solute would be
a. 180 b. 160
c. 120
d. 60
12
460The vapour pressure of a liquid
decreases by 10 tor ( r ) when a nonvolatile solute is dissolved. The mole
fraction of the solute in solution is 0.1
What would be the mole fraction of the
liquid if the decrease in vapour pressure is 20 tor ( r, ) the same solute
being dissolved?
A . 0.2
B. 0.9
( c .0 .8 )
D. 0.6
12
461Mass and percentage by weight do not change with temperature.
A. True
B. False
12
462The solubility of gases in water is
proportional to pressure
and ( _{-}—- ) proportional to
temperature.
A. directly
B. inversely
C . directly, inversely
D. inversely, directly
12
4634 A beaker contains a solution of substance ‘A’. Precipitation of substance A
takes place when small amount of ‘A’ is added to the solution. The solution
15
………
(a) saturated
(b) supersaturated
(c) unsaturated
(d) concentrated
Thinking Process
This problem includes concept of saturated unsaturated, supersaturated and
concentrated solution.
(b) When solute is added to the solution three
12
464Two samples of HCl of ( 1.0 mathrm{M} ) and ( 0.25 mathrm{M} )
are mixed. Find volumes of these
samples taken in order to prepare 0.75
M HCI solution. Assume no water is
(1) ( 20 mathrm{mL}, 10 mathrm{mL} )
(III) ( 100 mathrm{mL}, 50 mathrm{mL}(mathrm{III}) )
( 40 mathrm{mL}, 20 mathrm{mL}(mathrm{IV}) 50 mathrm{mL}, 25 mathrm{mL} )
A . ।, ॥।, IV
B. ।, ॥
c. ॥, ॥ा, । v
D. I, II, III, IV
12
465Higher is the (mass/volume) of
solute in a solution lower is its vapour
pressure.
12
466Illustration 2.35 100 g of water contains 1.0 g urea and
2.0 g sucrose at 298 K. The vapour pressure of water at
298 K is 0.3 atm. Calculate the vapour pressure of the
solution. (Molecular weight of urea = 60; Molecular weight
of sucrose = 342)
12
467Illustration 2.191 When cells of skeletal vacuoles of
a frog were placed in a series of NaCl solutions of
different concentration solution at 25°C, it was observed
microscopically that they remained unchanged in 0.7%
solution, shrank in a more concentrated and swelled in more
dilute solutions. Water freezes from the 0.7% salt solutions at
-0.406°C. What is the osmotic pressure of the cell cytoplasm
at 25°C.
(K= 1.86 kg mol-1 K)
12
4683 grams of salt of molecular weight 30
is dissolved in 250 g of water. Find the molality of the solution.(Multiply the answer by 10 )
12
469The azeotropic mixture of water (boiling
point ( =100^{circ} mathrm{C} ) ) and ( H C l ) (boiling point
( left.=85^{circ} mathrm{C}right) ) boils at about ( 110^{circ} mathrm{C} . ) During
distillation of this mixture, it is
possible to obtain:
A. pure ( H C l )
B. pure ( H_{2} O )
c. pure ( H C l ) as well as ( H_{2} O )
D. neither pure ( H_{2} O ) nor pure ( H C l )
12
470( 5 % ) solution of cane sugar is isotonic
with ( 0.877 % ) of ( X . ) The molecular weight
of substance ( boldsymbol{X} ) is:
A . 126.98
B. 119.96
c. 95.5
D. 59.98
12
471According to Henry’s law, the solubility of a gas in a given volume of liquid increases with increase in :
A. temperature
B. pressure
c. both A and B
D. none of the above
12
472The magnitude of colligative properties in all colloidal dispersions
is than solution.
A. lower
B. higher
c. Both
D. None of the above
12
4738. The vapour pressure of a solution containing 5.0 g of a non-
electrolyte in 100.0 g of water at a particular emperature is
2985 Nm-2. If the vapour pressure of pure water is 3000
N m-2, the molecular weight of the solute is
a. 60.0
b. 120.0
c. 180.0
d. 380.0
12
474The normal boiling of water is ( 373 K ) Vapour pressure of water at temperature ( boldsymbol{T} ) is ( 19 mathrm{mm} ) Hg. If enthalpy of evaporation is ( 40.67 k J / m o l, ) then
temperature ( boldsymbol{T} ) would be:
(Use ( log 2=mathbf{0 . 3}, boldsymbol{R}=mathbf{8 . 3} boldsymbol{J} boldsymbol{K}^{-1} mathbf{)} )
12
475The azeotropic solution of two miscible
liquids:
This question has multiple correct options
A. Can be seperated by simple distillation
B. May show positive or negative deviation from Raoult’s law
C . Are supersaturated
D. Behave like single pure component and boil at a fixed temperature
12
476When 45 gm of a solute is added to 900 ( mathrm{gm} ) of water, its vapour pressure decreased from ( 30 mathrm{mm} ) to ( 24 mathrm{mm} ). The
mole fraction of the solvent in the
solution is :
A . 0.2
B. 0.8
( c .0 . )
D. 0.9
12
477Assertion
Perfectly ideal solution is not possible with respect to binary solution of two liquids.
Reason
No two substances can have exactly the same nature of intermolecular forces
and also of the same magnitude.
A. Both Assertion and Reason are correct and Reason is the correct explanation for Assertion
B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion
c. Assertion is correct but Reason is incorrect
D. Assertion is incorrect but Reason is correct
12
478Pick out the correct statements
This question has multiple correct options
A. The ratio of vapour pressure over solution phase on mixing two immiscible liquids is equal to ratio of their moles in vapour phase
B. The ratio of vapour pressure over solution phase on mixing two miscible liquids is equal to ratio of their moles in liquid phase
C. The ratio of vapour pressure over solution phase on mixing two miscible liquids is equal to ratio of the product of their vapour pressure and their moles fraction in a liquid phase
D. The ratio of vapour pressure over solution phase on mixing two miscible liquids is equal to ratio of the product of their vapour pressure and their mole fraction in vapour phase
12
479toppr
are taken in ( A ) and ( B ). How many of the following statement(s) is/are correct?
( mathbf{P}_{X}^{0}=mathbf{2 0 0} ) tor ( r )
( mathbf{P}_{Y}^{0}=mathbf{5 0} ) tor ( r )
(i) If ( mathrm{NaCl} ) is added to vessel ( mathrm{B} ), the
lowering of vapour pressure takes place.
(ii) If glucose is added to vessel ( A, ) the boiling point of the solution increases.
(iii) If the valve connecting ( A ) and ( B ) is
opened, then ( mathbf{P}_{T} ) in both the vessel
becomes equal and is given by Raoult’s law.
(iv) After opening the valve, the level of liquid in both the container decreases (even a slight decrease is to be considered)
(v) After opening the valve, the final pressure in vessel B is more than 50
torr.
(vi) After opening the valve, the final pressure in vessel ( A ) is more than 200
torr
( A cdot 2 )
B. 3
( c )
( D )
12
480The melting points of most of the solid substances increase with an increase
of pressure acting on them. However, ice melts at a temperature lower than its usual melting point, when the pressure increases. This is because:
A. ice is less denser than water
B. pressure generates heat
C. the bounds break under pressure
D. ice is not a true solid
12
481A drop ( (0.05 mathrm{mL}) ) of ( 12.0 mathrm{M} ) HCl is
spread over a sheet of thin aluminium foil. Assuming that the acid dissolves
through the foil, the area is ( x times )
( 10^{-1} mathrm{cm}^{2} ) of the hole produced, then ( x )
is :
(Density of ( A l=2.70 g c m^{-3} )
thickness of the foil ( =0.10 mathrm{mm} )
12
482Calculate the amount of oxygen at 0.20 atm dissolved in 1 kg of water at 293 K. The Henry’s law constant for oxygen is
( 4.58 times 10^{4} ) atmosphere at ( 293 mathrm{K} )
( mathbf{A} cdot 7.07 times 10^{-6} mathrm{kg} )
В. ( 7.27 times 10^{-6} mathrm{kg} )
C ( .7 .57 times 10^{-6} mathrm{kg} )
D. ( 7.77 times 10^{-6} mathrm{kg} )
12
483What is saturated solution explain with one example?12
484A mixture of two immiscible liquids
nitrobenzene and water boiling at ( 99^{circ} C ) has a partial pressure of water ( 733 mathrm{mm} ) and of nitrobenzene ( 27 mathrm{mm} ). The ratio of
masses of water and nitrobenzene in
mixture is :
12
485Calculate the mass of compound (molar mass ( =256 g m o l^{-1} ) ) to be dissolved in
( 75 g ) of benzene to lower its freezing
point by ( 0.48 Kleft(K_{f}=5.12 K k g m o l^{-1}right) )
12
486Two glass bulbs of internal volume 0.5 and ( 0.2 L ) respectively are connected by a narrow tube of negligible volume. The
pressure of air in the vessel is ( 75 mathrm{cm} ) at
( 17^{circ} mathrm{C} . ) The smaller bulb is immersed in
melting ice and the larger bulb in boiling water. Calculate final pressure in the bulbs neglecting the expansion of glass.
12
487Azeotropic mixtures?
A. Boil at different temperatures
B. Are mixtures of solids
C . Are constant boiling mixtures
D. None of the above
12
4881 ( g ) of same non volatile solute is added
to ( 100 g ) o two different solvents ( A ) and ( B )
( boldsymbol{K}_{boldsymbol{b}} ) of ( boldsymbol{A}: boldsymbol{B}=mathbf{1}: mathbf{5} )
find out ( frac{left(Delta T_{b}right)_{A}}{left(Delta T_{b}right)_{B}} )
( mathbf{A} cdot 1: 10 )
B. 1: 5
c. 1: 20
D. 2: 5
12
489The depression in freezing point for ( 1 mathrm{M} ) urea, 1 M glucose and 1 M ( N a C l ) are in
the ratio:
A. 1: 2: 3
B. 3: 2: 2
( mathrm{c} cdot 1: 1: 2 )
D. 2: 3: 2
12
4902.82 ( mathrm{g} ) of glucose is dissolved in 30 g of water. The mole fraction of glucose in the solution is:
A . 0.01
B. 0.99
c. 0.52
D. 1.66
12
491A ( 5 % ) solution of cane sugar ( (text { mol. } boldsymbol{w} boldsymbol{t}= )
342) is isotonic with ( 1 % ) solution of
substance ( X . ) The molecular weight of
( boldsymbol{X} ) is:
A . 34.2
B. 171.2
( c .68 .4 )
D. 136.8
12
492Which of the following sequences lists the relative sizes of particles in a water mixture from smallest to largest?
A. Solutions, suspensions, colloids
B. Solutions, colloids, suspensions
c. colloids, solutions, suspensions
D. Colloids, suspensions, solutions
E. Suspensions, colloids, solutions
12
493The pair of boiling point and compound
are given as,
( boldsymbol{C}_{6} boldsymbol{H}_{6}, quad boldsymbol{C H}_{3} boldsymbol{O H} quad boldsymbol{C}_{6} boldsymbol{H}_{5} boldsymbol{N O}_{2} )
( boldsymbol{C}_{boldsymbol{6}} boldsymbol{H}_{boldsymbol{5}} boldsymbol{N} boldsymbol{H}_{boldsymbol{2}} )
( mathbf{8 0}^{circ} boldsymbol{C} quad mathbf{6 5}^{circ} boldsymbol{C} quad mathbf{2 1 2}^{boldsymbol{o}} boldsymbol{C} )
( 184^{circ} mathrm{C} )
(1)
( (|) )
(III)
Which will show lowest vapour pressure
at room temperature?
A. ( C_{6} H_{6} )
в. ( C H_{3} ) ОН
( mathbf{c} cdot C_{6} H_{5} N O_{2} )
D. ( C_{6} H_{5} N H_{2} )
12
494For an ideal binary liquid system:
This question has multiple correct options
A. the change in temperature ( (Delta H) ) is zero
B. Raoult’s law is obeyed
c. change in volume ( (Delta V) ) is zero
D. none of the above
12
495Van’t Hoff’s factor for ( 0.01 M ) aqueous
solution of acetic acid is ( 1.04, ) then ( p H: )
A . 3.4
B. 6.4
( c .9 .6 )
D. 10.6
12
4963.65 grams of HCl is dissolved in 16.2 grams of water. The mole fraction of HCI
in the resulting solution is:
A . 0.4
B. 0.3
( c .0 .2 )
D. ( 0 . )
12
497In an experiment, 18.04 g of mannitol were dissolved in 100 g of water. The vapour pressure of water was lowered by ( 0.309 mathrm{mm} ) Hg from ( 17.535 mathrm{mm} ) Hg.
Calculate the molar mass of manitol.
A. ( 150.0 mathrm{g} / mathrm{mol} )
в. ( 184.3 mathrm{g} / mathrm{mol} )
c. ( 140.4 mathrm{g} / mathrm{mol} )
D. 123.21 g/mol
12
498A solution contains 200 g ppm ( C a C O_{3} ) If there is ( frac{boldsymbol{x} times boldsymbol{N}_{boldsymbol{A}}}{mathbf{1 0}^{boldsymbol{6}}} boldsymbol{C a C} boldsymbol{O}_{3} ) molecules
per gram, what is the value of ( x ? )
12
499Illustration 2.73 Lowering of vapour pressure due to a
solute in 1 molal aqueous solution at 100°C is
a. 13.44 mm Hg
b. 14.12 mm Hg
c. 13.2 mm Hg
d. 35.2 mm Hg
12
500Carbon tetrachloride and benzene are:
A . immiscible in water
B. miscible in water
c. both ( A ) and ( B )
D. none of these
12
5010.38 Explain the solubility rule “like dissolves like” in terms of intermolecular
forces that exist in solutions.
12
502Vapour pressure of water at ( 293 K ) is
17.535 mm ( H g . ) Calculate the vapour
pressure of water at ( 293 K ) when ( 25 g ) of glucose is dissolved in ( 450 g ) of water.
12
503A solution contains ( 20 % ) solute by
weight at ( 60^{circ} ) C. When cooled to ( 30^{circ} mathrm{C} )
the solution contains ( 10 % ) solute by weight. When 45 g solution is cooled from ( 60^{circ} mathrm{C} ) to ( 30^{circ} mathrm{C} ), the mass of solute
deposited is :
A. ( 4.5 mathrm{g} )
B. 48
( c cdot 5 g )
D. ( 4.75 mathrm{g} )
12
504lute dissolved
of benzene by
Illustration 2.126 1.0 g of non-electrolyte solute diss
in 50.0 g of benzene lowered the freezing point of benzer
0.40 K. The freezing point depression constant of benzer
5.12 kg mol-1. Find the molecular mass of the solute.
12
505( 4.9 g ) of ( H_{2} S O_{4} ) is present in ( 100 m L ) of the solution. What is the molarity of the
solution? Calculate its normality also.
12
506A solution is prepared by urea and
water. If mole fraction of water is 0.8 in
the solution. Find the ratio of mass of
water and urea.
A ( cdot frac{5}{6} )
B. ( frac{6}{5} )
( c cdot frac{1}{4} )
D. ( frac{4}{1} )
12
507In an endothermic process, solubility increases with
temperature.
( A ). increase
B. decrease
c. no change in temperature
D. none of the above
12
508What are the conditions for an ideal
solution which obeys Raoult’s law over
the entire range of concentration?
A ( cdot Delta_{m i x} H=0, Delta_{m i x} V=0, P_{text {Total}}=p_{A}^{o} x_{A}+p_{B}^{o} x_{B} )
B. ( Delta_{operatorname{mix}} H=+v e, Delta_{operatorname{mix}} V=0, P_{text {Total}}=p_{A}^{o} x_{A}+p_{B}^{o} x_{B} )
C. ( Delta_{operatorname{mix}} H=0, Delta_{operatorname{mix}} V=+v e, P_{text {Total}}=p_{A}^{circ} x_{A}+p_{B}^{o} x_{B} )
D. ( Delta_{text {mix}} H=0, Delta_{text {mix}} V=0, P_{text {Total}}=p_{B}^{o} x_{B} )
12
509The volume of water required to make ( 0.20 mathrm{M} ) solution from ( 16 mathrm{ml} ) of ( 0.5 mathrm{M} ) solution is:
A . ( 40 mathrm{ml} )
B. 16 ( mathrm{ml} )
c. ( 50 mathrm{ml} )
D. 24 m
12
510Volume percentage decreases with increase in temperature.
A. True
B. False
12
511Question 23. Suggest the most important type of intermolec
attractive interaction in the following pairs.
(i) n-hexane and n-octane
(ii) I, and CCIA
(ii) NaCIO, and water
(iv) Methanol and acetone
(v) Acetonitrile (CH3CN) and acetone (CzH60)
Recall different types of intermolecular forces. London’s forces exist
between the non-polar molecules, ionic interactions are found in ionic
compound and dipole interactions are found in polar compounds.-OH,
-NH or HF bond if present, the molecule can form H-bond.
12
512The above experiment is done at ( N T P ) The stop cock is opened for certain time and then closed. After effusion, the bulb
( A ) contains ( 0.1 g m ) of ( D_{2} ). Find out the number of mole of ( H_{2} ) in bulb ( B ).
12
513A 0.15 molal solution of ( K_{4}left[F e(C N)_{6}right. )
in water freezes at ( -0.65^{circ} mathrm{C} ). What is
the apparent percentage of dissociation of this compound in this solution? ( left[boldsymbol{K}_{f} text { for water }=mathbf{1 . 8 6}^{circ} boldsymbol{C} boldsymbol{m o l}^{-1}right] )
A . 0.33
B. 0.52
( c .0 .63 )
D. 0.79
12
514The freezing point of benzene decrease
by ( 0.45^{circ} mathrm{C} ) when ( 0.2 g ) of acetic acid is added to ( 20 g ) of benzene. If acetic acid associates to form a dimer in benzene, percentage association of acetic acid in
benzene will be: ( left(K_{f} text { for benzene }=right. )
( left.mathbf{5 . 1 2} boldsymbol{K} boldsymbol{k g} boldsymbol{m o l}^{-1}right) )
A. ( 64.6 % )
B. ( 80.4 % )
c. ( 74.6 % )
D. ( 94.6 % )
12
515Illustration 2.155 Blood freezes at 272.44 K and a solution
of 3.0 g of urea in 250 g of water freezes at 272.63 K. Calculate
the osmotic pressure of blood at 300 K. (Assume density of
blood at 300 K to be 1 g cc-1)
12
516The freezing point of a solution containing 5.85 g of ( N a C l ) in ( 100 g ) of
water is ( -3.348^{circ} mathrm{C} . ) Calculate van’t Hoff
factor ‘i’ for this solution. What will be
the experimental molecular weight of NaCl?
( left(K_{f} text { for water }=1.86 K k g m o l^{-1}, ) at. wt. right. ( mathrm{Na}=23, mathrm{Cl}=35.5) )
12
517What will be the molarity of the solution in which 0.365 g of HCl gas is dissolved in ( 100 mathrm{mL} ) of solution?
A. 2 M
B. 0.2 ( M )
( c cdot 1 M )
D. 0.1 M
12
518A candle is burnt in a beaker until it
extinguishes itself. A sample of gaseous mixture in the beaker contains ( 6.08 times 10^{20} ) molecules of ( N_{2}, 0.76 times )
( 10^{20} ) molecules of ( O_{2}, ) and ( 0.50 times 10^{20} )
molecules of ( C O_{2} . ) The total pressure is
( 734 mathrm{mm} ) of Hg. The partial pressure of
( O_{2} ) would be:
A. ( 760.0 mathrm{mm} ) of ( mathrm{Hg} )
B. 76.0 mm of Hg
c. ( 7.6 mathrm{mm} ) of ( mathrm{Hg} )
D. ( 0.76 mathrm{mm} ) of ( mathrm{Hg} )
12
519POLIUNTV UOVICUT
Q.58 Why is it not possible to obtain pure ethanol by tras
What general name is given to binary mixtures whic
from Raoult’s law and whose components cannot
fractional distillation. How many types of such mixtures
e ethanol by fractional distillation?
y mixtures which show deviation
mponents cannot be separated by
es of such mixtures are there?
ac
12
520The Henry’s law constant for the
solubility of ( mathrm{N}_{2} ) gas in water at ( 298 mathrm{K} ) is
( 1.0 times 10^{5} ) atm. The mole fraction of ( mathrm{N}_{2} )
in air is ( 0.8 . ) The number of moles of ( mathrm{N}_{2} )
from air dissolved in 10 moles of water
at ( 298 mathrm{K} ) and 5 atm pressure is?
A ( cdot 4.0 times 10^{-4} )
B . ( 4.0 times 10^{-5} )
c. ( 5.0 times 10^{-4} )
D. ( 4.0 times 10^{-6} )
12
521The solubility of ( N_{2} ) in water is ( 2.2 times ) ( 10^{-4} g ) in ( 100 g ) of ( H_{2} O ) at ( 20^{circ} C ) when
the pressure of ( N_{2} ) over the solution is
1.2 atm.

Calculate the solubility at ( 20^{circ} mathrm{C} ) when
the pressure of ( N_{2} ) over the solution is
( mathbf{1 0} ) at ( boldsymbol{m} )
A ( cdot 1.25 times 10^{-3} g / 100 g mathrm{H}_{2} mathrm{O} )
B . ( 1.49 times 10^{-3} g / 100 g H_{2} O )
c. ( 2.56 times 10^{-3} g / 100 g H_{2} O )
D. ( 1.83 times 10^{-3} g / 100 g H_{2} O )

12
522Illustration 2.119 1.355 g of a substance dissolved in 55 g
of CH,COOH produced a depression in the freezing point
of 0.618°C. Calculate the molecular weight of the substance
(K. = 3.85)
12
523Illustration 2.164 The solution containing 10 g of an organic
compound per litre showed an osmotic pressure of 1.18 atm
at 0°C. Calculate the molecular mass of the compound (
0.0821 litre atm per degree per mol)
12
524Which of the following liquid pairs shows a positive deviation from Raoult’s law?
A. Acetone-chloroform
B. Benzene-methanol
c. water-nitric acid
D. water-hydrochloric acid
12
525What will be the solubility of the ( boldsymbol{C a}(boldsymbol{O H})_{2} ) solution when ( boldsymbol{N a O H} ) is
dissolved in it, compared with that in
pure water?
A. Unaffected
B. Increased
c. Decreased
D. None
12
526Define Raoult’s law for the elevation of
boiling point of a solution.
12
527The normality of a solution of a mixture containing ( boldsymbol{H} boldsymbol{C l} ) and ( boldsymbol{H}_{2} boldsymbol{S} boldsymbol{O}_{4} ) is ( boldsymbol{N} / mathbf{5} )
Twenty millilitres of this solution reacts
with an excess of ( A g N O_{3} ) solution to
give ( 0.287 g ) of silver chloride. The
percentage of ( H C l ) in the mixture by
mass, is ( (A g=108) )
A . ( 42.69 % )
B. ( 57.31 % )
c. ( 50 % )
D. 25%
12
528Question 10. Give an example of a material used for making
semipermeable membrane for carrying out reverse osmosis.
12
529For an ideal binary liquid solution with ( boldsymbol{p}_{boldsymbol{x}}^{0}>boldsymbol{p}_{boldsymbol{y}}^{0} ) in which relation between ( boldsymbol{X}_{boldsymbol{x}} )
(mole fraction of ( x ) in liquid phase) and
( Y_{x} ) (mole of fraction of ( x ) in vapour
phase) is correct where ( boldsymbol{X}_{boldsymbol{y}} ) and ( boldsymbol{Y}_{boldsymbol{y}} ) are mole fraction of ( y ) in liquid and vapour phase respectively.
A ( cdot X_{x}>Y_{x} )
в. ( X_{x}=Y_{x} )
с. ( frac{X_{x}}{X_{y}}<frac{Y_{x}}{Y_{y}} )
D. ( X_{x}, Y_{x}, X_{y} ) and ( Y_{y} ) cannot be correlated
12
530A very dilute saturated solution of a
sparingly soluble salt ( A_{3} B_{4} ) has a
vapour pressure of 20 mm of ( H g )
at temperature ( T, ) while pure water
exerts a pressure of 20.126 mm ( H g ) at
the same temperature

The solubility product constant of ( boldsymbol{A}_{3} boldsymbol{B}_{4} )
at the same temperature is ( 5.4 times 10^{-x} )
value of ( x ) is

12
53112. Substance used as an anti-
is :
(1) Methyl alcohol and H,O
(2) Methyl alcohol
(3) Ethyl alcohol
(4) Ethyl alcohol and H,O
12
5321 ( g ) of ( N a C l ) dissolved in ( 100 g ) of water to prepare a mixture. What is the mass percentage of sodium chloride?12
533Air contains ( O_{2} ) and ( N_{2} ) in the ratio of
1:4. Calculate the ratio of solubilities in
terms of mole fraction of ( boldsymbol{O}_{2} ) and ( boldsymbol{N}_{2} )
dissolved in water at atmospheric pressure and room temperature at
which Henry’s constant for ( boldsymbol{O}_{2} ) and ( boldsymbol{N}_{2} ) are ( 3.30 times 10^{7} ) torr and ( 6.60 times 10^{7} ) tor
respectively.
12
534Illustration 2.157 The osmotic pressure of a solution is
1.3 atm. The density of solution is 1.3 g cm . Calculate the
osmotic pressure rise. (1 atm = 76 cm Hg, dwg = 13.6 g cm-3)
12
535A chemist is preparing to analyse samples that will contain no more than ( 0.5 mathrm{g} ) of uranium. His procedure calls for
preparing the uranium as ( U^{4+} ) ion and
oxidizing it by ( M n O_{4}^{-} ) in acid solution:
( boldsymbol{U}^{4+}+boldsymbol{M} boldsymbol{n} boldsymbol{O}_{4}^{-}+boldsymbol{H}_{2} boldsymbol{O} rightarrow boldsymbol{U} boldsymbol{O}_{2}^{2+}+ )
( boldsymbol{M} boldsymbol{n}^{2+}+boldsymbol{H}_{3} boldsymbol{O}^{+} )
If he wants to react the total ( U^{4+} )
sample with a maximum of ( 50 mathrm{ml} ) of ( K M n O_{4} ) solution, what concentration does he choose? ( (mathrm{U}=238) )
A. 0.0336 M
B. 0.0168 М
c. 0.168 м
D. 0.0672 M
12
536At ( 80^{circ} mathrm{C}, ) the vapour pressure of pure
liquid ( A ) is 520 mmHg and that of pure liquid ( B ) is 1000 mmHg. If a mixture
solution of ( A ) and ( B ) boils at ( 80^{circ} ) and 1
atm pressure, the amount of ( A ) (mole
percent) in the mixture is:
A . ( 50 % )
B. 54%
c. ( 32 % )
D. 44%
12
537According to Henry’s law, the partial
pressure of ( operatorname{gas}left(mathrm{P}_{text {gas}}right) ) is directly
proportional to mole fraction of gas in
dissolved state, i.e., ( boldsymbol{P}_{text {gas}}=boldsymbol{K}_{boldsymbol{H}} cdot boldsymbol{X}_{boldsymbol{g a s}} )
where ( K_{H} ) is Henry’s constant. Now, choose the correct option(s). This question has multiple correct options
( mathbf{A} cdot K_{H} ) is characteristic constant for a given gas-solvent system.
B. Higher is the value of ( K_{H} ), lower is the solubility of gas for a given partial pressure of gas.
( mathbf{C} cdot K_{H} ) is temperature dependent
D. ( K_{H} ) increases with temperature.
12
538Illustration 2.187 0.002 molar solution of NaCl having
degree of dissociation of 90% at 27°C has osmotic pressure
equal to
a. 0.94 bar b. 9.4 bar c. 0.094 bar d.9.4 x 10-4 bar
12
539At ( 30^{circ} C, ) the solubility of
( A g_{2} C O_{3}left(K_{s p}=8 times 10^{-2}right) ) will be
maximum in:
A. 0.05 M ( mathrm{Na}_{2} mathrm{CO}_{3} )
B. ( 0.05 M A g N O_{3} )
c. Pure water
D. ( 0.05 N H_{3} )
12
540A solution containing ( 10 g d m^{-3} ) of urea
(molecular mass ( =60 g m o l^{-1} ) ) is
isotonic with a ( 5 % ) solution of a
nonvolatile solute. The molecular mass
of this is nonvolatile solute is:
A ( cdot 250 g m o l^{-1} )
в. 300 gmol-( ^{-1} )
c. 350 gmol-( ^{-1} )
D. ( 200 g ) mol ( ^{-1} )
12
541( A )
( 0.1(mathrm{M}) ) solution of an acid HA of density ( 1.01 mathrm{gm} / mathrm{ml} ) is taken in a beaker. The molec ular mass of HA is ( 300 mathrm{g} / mathrm{mol} ) The freezing point of solution is
( 0.2087^{circ} mathrm{C} . ) For ( mathrm{H}_{2} mathrm{O}, quad K_{f}=1.86 mathrm{K} / mathrm{m} )
What is the degree of dissociation of HA i
n its ( 0.1(mathrm{M}) ) aqueous solution (in percentage) ?
A . ( 10 % )
B. 20%
c. ( 25 % )
D. ( 55.56 % )
12
542An ideal gas is mixture of ( C_{2} H_{6} ) and
( C_{2} H_{4} ) occupies 281 at 1 atm 8273 k. The
mixture reacts completely with 128 g of ( O_{2} ) to produce ( C O_{2} ) pf water vapour
Mole fraction of ( C_{2} H_{6} ) in the mixture
will be:
A. 0.4
B. 0.6
( c cdot 0.2 )
D. 0.8
12
5430.24 4 L of 0.02 M aqueous solution of NaCl was diluted by adding 1 L of
water. The molality of the resultant solution is ……….
(a) 0.004 0 .008
0.012 (d) 0.016
Thinking Process
To calculate the strength of solution when it is diluted by adding solvent. Write all the
given values M.V.M and Then calculate required parameter using formula,
MY, MY,
where i volume of solution before dilution
= volume of solution after dilution
M = strength of solution before dilution
M = strength of solution after dilution
12
544Illustration 2.124 A liquid possessing which of the following
characteristics will be most suitable for determining the
molecular mass of a compound by cryoscopic meas!
a. That having low freezing point and small enthalpy Ol
fusion
b. That having high freezing point and small enthalpy
of fusion
c. That having high freezing point and small enthalpy
of vapourization
d. That having large surface tension
12
545The composition of the solution whose normal boiling point is ( T )
A ( cdot X_{A}=0.08, X_{B}=0.92 )
В. ( X_{A}=0.92, X_{B}=0.18 )
C ( . X_{A}=0.18, X_{B}=0.82 )
D. None of these
12
546( R H_{2} ) (ion exchange resin) can replace
( C a^{2+} ) in hard water:
[
boldsymbol{R} boldsymbol{H}_{2}+boldsymbol{C} boldsymbol{a}^{2+} rightarrow boldsymbol{R} boldsymbol{C} boldsymbol{a}+boldsymbol{2} boldsymbol{H}^{+}
]
( 1 L ) of hard water after passing through
( R H_{2} ) has ( p H=2 . ) Hence, hardness in
ppm of ( boldsymbol{C a}^{2+} ) is :
A . 200
в. 100
c. 50
D. 125
12
547Two liquids ( X ) and ( Y ) are perfectly
immiscible. If ( X ) and ( Y ) have molecular
masses in ration ( 1: 2, ) the total vapour pressure of a mixture of ( boldsymbol{X} ) and ( boldsymbol{Y} )
prepared in weight ratio 2: 3 should be:
( left(boldsymbol{P}_{X}^{0}=mathbf{4 0 0} text { torr }, boldsymbol{P}_{boldsymbol{Y}}^{0}=mathbf{2 0 0} text { torr }right) )
A. 314 torr
B. 466.7 torr
c. 600 torr
D. 700 torr
12
548Fill in the blanks with appropriate
words.

Azeotropic mixtures boil without change in their ( _{text {一一一一一一一. }} ) Azeotropic mixtures exist in solutions showing
or deviations.
solutions do not form
azeotropic. van’t Hoff factor for an
electrolyte is than 1
A. colour, positive, negative, non-ideal, greater
B. properties, positive, negative, ideal, smaller
c. boiling point, positive, negative, non-ideal, lesser
D. composition, positive, negative, ideal, greater

12
5490.17 Sulphuric acid reacts with sodium hydroxide as follows
H2SO4 + 2NaOH → Na2SO4 + 2H,0
When 1 of 0.1M sulphuric acid solution is allowed to react with 1L of
0.1M sodium hydroxide solution, the amount of sodium sulphate formed
and its molarity in the solution obtained is
(a) 0.1 mol L-1
(b) 7.10 g
(c) 0.025 mol L-
(d) 3.55 g
12
550At ( 300 mathrm{K} ), the vapour pressure of an ideal solution containing 3 mole of ( A ) and 2 mole of ( mathrm{B} ) is 600 torr. At the same
temperature, if 1.5 mole of ( A & 0.5 ) mole of ( mathrm{B} ) (non-volatile) are added to this solution the vapour pressure of solution increases by 30 torr. What is the value
of ( P_{B}^{circ} ? )
A . 150
в. 405
c. 90
D. none of these
12
551Ideal solution is formed when its
components:
A. have zero heat of mixing only
B. have zero volume change on mixing only
C. have zero heat of mixing and zero volume change
D. can be converted into gases
12
552Assuming the complete dissociation of HCl and lead salt, calculate how much
( mathrm{HCl} ) is added to ( 0.001 mathrm{m} ) lead salt
solution to just precipitate when
saturated with ( H_{2} S . ) The concentration
of ( boldsymbol{H}_{2} boldsymbol{S} ). The concentration of ( boldsymbol{H}_{2} boldsymbol{S} ) is ( boldsymbol{0 . 1} )
( mathbf{M} )
12
553A mixture of benzene and toluene forms
A. An ideal solution
B. Non-ideal solution
c. suspension
D. Emulsion
12
554A storage battery contains a solution of
( H_{2} S O_{4} 38 % ) by weight. What will be the
Vant Hoff factor if the ( Delta T_{f(e x p e r i m e n t)} ) in ( mathbf{2 9 . 0 8} .left[text {Given } boldsymbol{K}_{mathbf{1}}=mathbf{1 . 8 6 m o l}^{-mathbf{1}} mathbf{K} boldsymbol{g}right] )
12
555( p H ) of a ( 0.1 M ) monobasic acid is found to be ( 2 . ) Hence its osmotic pressure at a
given temp. ( boldsymbol{T} boldsymbol{K} ) is:
A. ( 0.1 R T )
( T )
в. ( 0.11 R T )
c. ( 1.1 R T )
D. ( 0.01 R T )
12
556If relative decrease in vapour pressure is 0.4 for a solution containing 1 mol
NaCl in 3 mol ( H_{2} ) O. NaCl is
( % ) ionised.
A . ( 60 % )
B. 50%
c. ( 100 % )
D. 40%
12
557For an ideal solution, the correct option
is :
A ( cdot Delta_{operatorname{mix}} S=0 ) at constant T and ( mathrm{P} )
B. ( Delta_{operatorname{mix}} V neq 0 ) at correct T and P
C. ( Delta_{operatorname{mix}} H=0 ) at constant ( mathrm{T} ) and ( mathrm{P} )
D. ( Delta_{text {mix}} G=0 ) at constant T and ( P )
12
558If the pH of ( 0.2 M ) dibasic acid ( left(H_{2} Aright) )
is ( 1.699, ) than its osmotic pressure at ( T ) K temperature will be?
в. ( 0.02 R T )
c. ( 0.4 R T )
D. ( 0.1 R T )
12
559g of sodium hydroxide is present in 1 litre of ( 1 mathrm{M} ) solution.
A . 20
B. 40
( c .30 )
D. 10
12
560Which is the condition, unrelated
to quantities, that indicates that the rate going into solution is equal to the rate coming out of solution?
A . Dilute
B. concentrated
c. Unsaturated
D. Saturated
E. Supersaturated
12
561Find mole fraction of ( N a O H ) in its ( 10 % )
aqueous solution.
12
5622.5 litre of ( 1 mathrm{M} ) NaOH solution mixed
with another 3 litre of ( 0.5 ~ M ) NaOH
solution. Then find out molarity of resultant solution.
в. ( 1.0 mathrm{M} )
c. 0.73 М
D. ( 0.50 M )
12
563Illustration 2.87 Match the following if the molar mass of
X, Y, and Z are same:
Solvent
T(°C)
K(kg K mol-1)
Х
127
0.73
27
0.53
253
0.98
12
564Addition of 0.643 g of a compound to 50 mL of benzene (density 0.879 glmL)
lowers the freezing point from ( 5.51^{circ} mathrm{C} ) to
( 5.03^{circ} mathrm{C} . ) If ( K_{f} ) for benzene is 5.12
calculate the molecular mass of the
compound.
A . 126
B. 166
( c cdot ) १५
D. 146
12
565Q.43 Why is the vapour pressure of an aqueous solution of glucos
that of water?
of water. When a
aqueous solution of glucose lower than
12
566For an ideal solution of two components
A and B, which of the following is true?
( mathbf{A} cdot Delta H_{m i x i n g}0(z text {ero}) )
C. ( A ) – ( B ) interaction is stronger than ( A-A ) and ( B-B ) interactions
D. ( A-A, B-B ) and ( A-B ) interactions are identical
12
567Which of the following solutions is more concentrated than the others?
A. ( 5.3 mathrm{gm} ) of ( mathrm{Na}_{2} mathrm{CO}_{3} ) in ( 500 mathrm{ml} ) solution
B. 5 gm of ( N a O H ) in 100 ml solution
c. 3.65 gm of ( H C l ) in 750 ml solution
D. 4.9 gm of ( H_{2} S O_{4} ) in ( 1000 mathrm{ml} ) solution
12
568Derive van’t Hoff general solution
equation.
12
569The mass of non-volatile, non-elctrolyte solute (molar mass ( 50 g ) mol ( ^{-1} ) ) needed
to be dissolved in ( 114 g ) octane to reduce
its vapour pressure to ( 75 % ), is
A . ( 150 g )
в. ( 75 g )
c. ( 37.5 g )
D. ( 50 g )
12
570The cryoscopic constant for acetic acid is ( 3.6 K k g / ) mol. A solution of ( 1 g ) of a hydrocarbon in ( 100 g ) of acetic acid
freezes at ( 16.14^{circ} mathrm{C} ) instead of the usual
( 16.60^{circ} mathrm{C} . ) The hydrocarbon contains ( 92.3 % ) carbon. If the molecular formula
is ( C_{6} H_{6} . ) Find the value of ( x ) and ( y )
A. ( x=2, y=4 )
В. ( x=3, y=5 )
c. ( x=4, y=4 )
D. ( x=6, y=6 )
12
571The van’t hoff factor for a very dilute
solution of ( boldsymbol{F e}_{2}left(boldsymbol{S O}_{4}right)_{3} ) is:
( mathbf{A} cdot mathbf{9} )
B. 5
( c cdot 24 )
D. 16
12
572When ( 25 g ) of ( N a_{2} S O_{4} ) is dissolved in
( 10^{3} k g ) of solution, its concentration will
be :
A . 2.5 ppm
в. 25 ррт
c. 250 ppm
D. 100 ppm
12
573Q. 14 Which of the following statements is false?
(a) Two different solutions of sucrose of same molality prepared in
different solvents will have the same depression in freezing point.
(b) The osmotic pressure of a solution is given by the equation it = CRT (where, C is
the molarity of the solution)
(c) Decreasing order of osmotic pressure for 0.01 M aqueous solutions of barium
chloride, potassium chloride, acetic acid and sucrose is
Bacl, > KCI > CH. COOH > sucrose
(d) According to Raoult’s law, the vapour pressure exerted by a volatile component
of a solution is directly proportional to its mole fraction in the solution
12
574Ideal solution is formed when its
components:
This question has multiple correct options
A. have zero heat of mixing
B. have zero volume change
c. obey Raoult’s law
D. can be converted into gases
12
575A solution having ( Delta boldsymbol{H}_{m i x}=+ ) ve will
exhibit deviation from
ideal behaviour
A. negative
B. positive
( c cdot ) no
D. depends upon the properties of the mixing components
12
576Ilustration 2.54 Why does a solution of ethanol and
cyclohexane show positive deviation from Raoult’s law?
12
577What amount of ( C a C l_{2}(i=2.47) ) is
dissolved in 2 litres of water so that its
osmotic pressure is 0.5 at ( m ) at ( 27^{circ} C )
A. ( 3.42 g )
B. ( 9.24 g )
c. ( 2.834 g )
D. ( 1.820 g )
12
578If ( alpha ) is the degree of dissociation of
( N a_{2} S O_{4}, ) the vant Hoff’s factor ( (i) ) used
for calculating the molecular mass is:
( mathbf{A} cdot 1+alpha )
B. ( 1-alpha )
( c cdot 1+2 alpha )
D. ( 1-2 alpha )
12
579Illustration 2.173 The osmotic pressure of a solution
containing 5 g of substance (molar mass = 100) in 308 ml
of solution was found to be 4.0 atm at 300 K. Calculate the
value of solution constant (R).
12
580A solution containing ( 25.6 g m ) of
sulphur dissolved in ( 1000 g ) of
naphthalene gave a freezing point lowering of 0.680 , then molecular formula of sulphur is:
( A cdot S_{2} )
в. ( S_{4} )
c. ( S_{6} )
D. ( S_{8} )
12
581In the azeotropic mixture of ( H C l ) and
water, the percentage of ( H C l ) is:
A . 20.2%
B . 11.1%
c. 44.4%
D. 10%
12
582Benzene and naphthalene form an ideal
solution at room temperature. For this process, the true statements are:
(i) ( Delta G ) is positive
(ii) ( Delta S_{s y s t e m} ) is positive
(iii) ( Delta S_{text {surroundings}}=0 )
(iv) ( Delta boldsymbol{H}=mathbf{0} )
A. (ii) and (iv) only
B. (i) and (iii) only
C. (ii), (iii) and (iv) only
D. all of these
12
583The volume of ( boldsymbol{H}_{2} boldsymbol{S} boldsymbol{O}_{4} ) acid ( (boldsymbol{9} boldsymbol{8} % ) by
mass, ( d=1.80 mathrm{g} / mathrm{mL} ) ) required to prepare
1 litre of ( 0.1 M H_{2} S O_{4} ) solution is:
A ( .16 .65 mathrm{mL} )
B . ( 22.20 mathrm{mL} )
( c .5 .55 mathrm{mL} )
D. ( 11.10 mathrm{mL} )
12
584Dimerization of benzoic acid occurs in
benzene solution, then the relation
between van’t Hoff factor ( i ) and amount
of association ( x ) is:
A ( cdot i=(1-x) )
B . ( i=(1+x) )
c. ( i=left(1-frac{x}{2}right) )
D. ( i=left(1+frac{x}{2}right) )
12
585mospheric pressure and osmotic pressure are the same
Q. 16 Which of the following statements is false
(a) Units of atmospheric pressure and osmotic pre
(b) In reverse Osmosis, solvent molecules move
membrane from a region of lower concen
concentration
(c) The value of molal depression constant depends on na
(a) Kelative lowering of vapour pressure is a dimensionless quantity
molecules move through a semipermeable
of lower concentration of solute to a region of higher
al depression constant depends on nature of solvent
lo membrane
12
586On mixing ( 10 mathrm{mL} ) of acetone with ( 40 mathrm{mL} ) of chloroform, the total volume of the solution is:
( A cdot 50 ( m ) L
( c_{c}=50 mathrm{mL} )
D. Can not be predicted
12
587Acetic acid dissolved in benzene shows
a molecular weight of
A . 60
B. 120
c. 180
D. 240
12
588Arrange the following aqueous solutions in the order of their increasing boiling points
( (mathrm{i}) 10^{-4} M N a C l )
(ii) ( 10^{-4} M ) Urea
( (text { iii }) 10^{-3} M M g C l_{2} )
(iv) ( 10^{-2} M N a C l )
A ( cdot(i)<(i i)<(i v)<(i i i) )
B. ( (i i)<(i)<(i i i)<(i v) )
c. ( (i i i)<(i)<(i i)<(i v) )
D. ( (i v)<(i i i)<(i)=(i i) )
12
589Lowering in vapour pressure is highest for:
A. ( 0.2 mathrm{m} ) urea
B. 0.1 m glucose
( mathrm{c} cdot 0.1 mathrm{m} mathrm{MgSO}_{4} )
D. ( 0.1 mathrm{m} ) BaCl ( _{2} )
12
590Caffeine has a molecular weight of 194 If it contains ( 28.9 % ) by mass of nitrogen, the number of atoms of nitrogen in one molecule of caffeine is:
( A cdot 4 )
B. 6
( c cdot 2 )
D.
12
591The molarity of ( boldsymbol{H} boldsymbol{C l} ) solution containing 0.4 moles in 200 ml of the
solution is:
A. 2 M
в. 1
( c cdot 3 M )
D. 4 M
12
592A mixture of ( C_{3} H_{8} ) and ( C H_{4} ) exerts a
pressure of ( 320 mathrm{mm} ) Hg at temperature ( boldsymbol{T}(boldsymbol{K}) ) in a ( boldsymbol{V} ) litre flask. On complete combustion, gaseous mixture contains
( C O_{2}, ) only and exerts a pressure of 448 ( mathrm{mm} ) Hg under identical condition.
Hence, mole fraction of ( C_{3} H_{8} ) in the mixture is :
A . 0.2
B. 0.8
c. 0.25
D. 0.75
12
593What concentration of ( boldsymbol{F}- )
( boldsymbol{C H}_{2} boldsymbol{C O O H},left(boldsymbol{K}_{a}=mathbf{2 . 6} times mathbf{1 0}^{-3}right) ) is
needed so that ( left[boldsymbol{H}^{+}right]=mathbf{2} times mathbf{1 0}^{-mathbf{3}} ) ?
в. ( 2.6 times 10^{-3} M )
c. ( 5.2 times 10^{-3} M )
D. ( 3.53 times 10^{-3} M )
12
594Illustration 2.64 What are minimum boiling azeotropes?
Give one example.
12
595Determine the amount of ( C a C l_{2}(i= ) 2.47) dissolved in 2.5 litre of water such
that its osmotic pressure is 0.75 atm at
( 27^{circ} C )
12
596Study the figures given below and mark
the correct statement
A. (i) Nitric acid + Water;
(i) Acetone + Ethyl alcohol
B. (i) Water + Ethyl alcohol
(ii) Acetone + Benzene
C. (i) Acetone + Ethyl alcohol;
(ii) Acetone + Chloroform
D. (i) Benzene + Chloroform
(ii) Acetone + Chloroform
12
597What is the effect of temperature on
solubility of a gas?
A. Solubility of a gas increase with rise in temperature
B. Solubility of a gas decreases with rise in temperature
c. No effect
D. Sometimes increases with increase in temperature sometimes decreases
12
598Find the volume of a 0.2 molar solution
of sodium hydroxide, which is used to neutralize 40 liters of a 0.3 molar
hydrochloric acid solution.
A. 10 liters
B. 20 liters
c. 40 liters
D. 60 liters
E. 120 liters
12
599Question 35. Henry’s law constant for the molality of methane in
benzene at 298 K is 4.27 x10 mm Hg Calculate the solubility of methane
in benzene at 298 K under 760 mm Hg.
Apply Henry’s law, p = Ky*
12
600Find out ( % ) strength of ( 11.2 V H_{2} O_{2} )
A . ( 34 % )
B. 3.4%
c. ( 1.7 % )
D . 13.8%
12
601Illustration 2.32 At a certain temperature, the vapour
pressure of pure ether is 640 mm and that of pure acetone is
280 mm. Calculate the mole fraction of each component in
the vapour state if the mole fraction of ether in the solution
is 0.50.
12
60210. The vapour pressure of a pure liquid A is 40 mm Hg at
310 K. The vapour pressure of this liquid in a solution
with liquid B is 32 mm Hg. The mole fraction of A in the
solution, if it obeys Raoult’s law, is:
a. 0.8
b. 0.5 c. 0.2
d. 0.4
12
603At STP, a container has 1 mole of ( A r, 2 )
moles of ( C O_{2}, 3 ) moles of ( O_{2} ) and 4
moles of ( N_{2} . ) Without changing the total
pressure of ( boldsymbol{O}_{2} ) is removed, the partial
pressure of ( boldsymbol{O}_{2} ) is:
A. changed by about ( 16 % )
B. halvedd
c. changed by ( 26 % )
D. unchanged.
12
604The vapour pressure of pure benzene at
( 88 C ) is ( 960 mathrm{mm} ) and that of toluene at
the same temperature is ( 380 mathrm{mm} ) of
benzene. At what mole fraction of
benzene. the mixture will boil at ( 88^{circ} mathrm{C} ) ?
A . 0.655
B. 0.345
( c cdot 0.05 )
D. 0.25
12
605Question 13. Why is the mass determined by measuring a colligative
property in case of some solutes abnormal? Discuss it with the help of
van’t Hoff factor.
oble molente
12
606An aqueous solution is 1.00 molal in ( mathrm{Kl} )
Which change will cause the vapour
pressure of the solution to increase?
B. Addition of ( mathrm{Na}_{2} mathrm{SO}_{4} )
c. Addition of 1.00 molal KI
12
607( 6 g ) urea and ( 11.8 g ) glucose are dissolved
in ( 100 m l H_{2} O . ) What is the osmotic
pressure at ( 300 K )
A. 27.06 atm
B. 30 atm
c. 45 atm
D. 13.07 atm
12
608Question 9. Vapour pressure of pure water at 298 K is 23.8 mm Hg. 50 g
urea (NH,CONH) is dissolved in 850 g of water. Calculate the vapour
pressure of water for this solution and its relative lowering.
Consider Raoult’s law and formula for relative lowering in vapour pressure,
PA – Ps – NB _WB MA
På NA MBWA
where, PA
Ps is called relative lowering in vapour pressure.
12
609Illustration 2.156 x g of non-electrolytic compound (molar
mass = 200) is dissolved in 1.0 L of 0.05 M NaCl solution. The
osmotic pressure of this solution is found to be 4.92 atm at
27°C. Calculate the value of x. Assume complete dissociation
of NaCl and ideal behaviour of this solution.
12
610Molecules of benzoic acid
( left(C_{6} H_{5} C O O Hright) ) dimerise in benzene. g of the acid dissolved in 30 g of benzene
shows a depression in freezing point
equal to ( 2 mathrm{K} ). If the percentage association of the acid to form a dimer
in the solution is ( 80, ) then ( w ) is:
(Given that ( boldsymbol{K}_{f}=mathbf{5} mathrm{K} ) kg ( boldsymbol{m o l}^{-1} ), Molar
mass of benzoic acid ( =122 ) g ( m o l^{-1} )
A . ( 1.8 g )
в. 2.4g
c. ( 1.0 g )
D. ( 1.5 mathrm{g} )
12
611The van’t Hoff’s factor for ( 0.1 mathrm{M} )
( B aleft(N O_{3}right)_{2} ) solution is ( 2.74 . ) The degree of dissociation is:
A . ( 91.3 % )
B. 87%
c. ( 100 % )
D. 74%
12
612( C H_{3} C O O H ) dimerizes in benzene
when ( 1.65 g ) of ( C H_{3} C O O H ) dissolved in
( 100 g ) of benzene the elevation of ( B p s ) of
the solution was found ( 0.36 K . ) If ( K_{b} ) for
benzene in 2.85 K.kgl mol. Then find
Vant Hoff factor and degree of
association of ( boldsymbol{C} boldsymbol{H}_{3} boldsymbol{C O O H} )
12
613The following substances were
all dissolved in 100 grams of water at ( 290 mathrm{K} ) to produce saturated solutions.lf the solution is
heated to ( 310 mathrm{K} ), which substance will have a decrease in its solubility:
( mathbf{A} cdot N a C I )
в. ( K I )
c. ( mathrm{CaCl}_{2} )
D. ( H C I )
E . ( K N O_{3} )
12
614Illustration 2.48 What is the composition of the vapour
which is in equilibrium at 30°C with a benzene-toluene
solution with a mole fraction of benzene of (a) 0.400 and
(b) 0.600?
Po° = 119 torr, p.° = 37.0 torr
12
615The Henry law constant for dissolution of a gas in an aqueous medium is ( 3 times ) ( 10^{2} ) atm. At what partial pressure of the
gas (in atm), the molality of gas in aqueous solution will be ( frac{5}{9} M ? )
A . 2.2 M
в. 9 м
( c .3 ) м
D. none
12
616At a given temperature, total vapour pressure (in torr) of a mixture of volatile
components ( A ) and ( B ) is given by ( P_{T o t a l}=120-75 X_{B} ) hence, the vapour
pressure of pure ( A ) and ( B ) respectively (in Torr) are:
A .120,75
в. 120,195
c. 120,45
D. 75,45
12
617( mathbf{3 0} boldsymbol{m} boldsymbol{L} ) of ( boldsymbol{C H}_{3} boldsymbol{O H}left(boldsymbol{d}=mathbf{0 . 8} boldsymbol{g} / boldsymbol{c m}^{3}right) ) is
mixed with ( 60 m L ) of ( C_{2} H_{5} O H(d= )
( left.0.92 g / c m^{3}right) ) at ( 25^{circ} C ) to form a solution
of density ( 0.88 g / c m^{3} . ) Select the
correct option. This question has multiple correct options
A. Molarity and molality of resulting solution are 6.33 and 13.59 respectively
B. The mole fraction of solute and molality are 0.385 and 13.59 respectively
c. Molarity and % change in volume are 13.59 and zero respectively
D. Mole fraction of solvent and molality are 0.615 and 13.59 respectively
12
618During dissolution when a solute is added to the solvent, some solute particles separate out from the solution as a result of crystallization. At the stage of equilibrium, the concentration of solute in the solution at a given
temperature and pressure:
A. increases
B. decreases
c. remains constant
D. keeps changing
12
619Which is least soluble?
A ( cdot N a_{2} S )
в. ( M g S )
c. ( M g C l_{2} )
D. ( N a C l )
12
620The vapour pressure of benzene C,H, at 298 K is 95
torr. After 10.00 g of benzene is injected into a 10.0 L
bulb at 298 K, how many grams of benzene remain as
liquid?
12
621What is Henry’s constant for neon
dissolved in water given ( C_{N e}= ) ( 23.5 m L / L ) solution and STP volume
( 22,414 mathrm{mL} / text { mole gas }) ) and pressure ( operatorname{atm}) ? )
A. 0.00105
5
В. 0.11004
begin{tabular}{l}
( c .0 .00115 ) \
hline
end{tabular}
D. 0.00015
12
622The boiling point of an azeotropic mixture of water and ethyl alcohol is
less than that of theoritical value of
water and alcohol mixture. Hence the
mixture shows:
A. that solution is saturated
B. positive deviation from Raolt’s law
c. negative deviation from Raoult’s law
D. that solution is super saturated
12
623How many moles of ( N a O H ) are required to neutralize 1.2 moles of
( boldsymbol{H}_{2} boldsymbol{S} boldsymbol{O}_{4} ? )
A. 0.6 mole
B. 1.2 mole
c. 2.4 mole
D. 3.6 mole
E . 4.8 mole
12
624The concentration of ( C aleft(H C O_{3}right)_{2} ) in a
sample of hard water is 486 ppm. The density of water sample is ( 1.0 mathrm{g} / mathrm{ml} ). The molarity of the solution is :
A . ( 3.0 times 10^{-3} M )
в. ( 5.0 times 10^{-3} M )
c. ( 2.0 times 10^{-3} M )
D. ( 6.0 times 10^{-3} M )
12
625Two components in the ratio of ( x: y )
form an azeotropic mixture. They are
mixed in the ratio of ( x: 2 y, ) how many
moles one of the pure component ( boldsymbol{y} ) will be evaporated before getting azeotropic
solution?
12
626At a particular temp, a solution that has dissolved as much solute as it is
capable of dissolving is said to be a :
A. saturated solution
B. unsaturated solution
c. both ( A ) and ( B )
D. none of the above
12
627Due to low concentration of oxygen in blood, climber become weak and unable to think clear –
(i) Write specific name of above condition?
(ii) Explain the reason of such
condition?
12
628When an electrolyte is dissociated in
solution, the van’t Hoff’s factor ( ( i ) ) is :
( A cdot>1 )
B. ( <1 )
( mathrm{c} cdot=0 )
( mathrm{D} cdot=1 )
12
629mole ( A_{X} B_{Y} ) when added to ( 1.08 mathrm{kg} ) of
water, lowers its vapour pressure by 35 torr to 700 torr. If further 1184 g of methanol is added, then the vapour
pressure increase by 37 torr. Consider
only few vapors are formed, and ( boldsymbol{A}_{boldsymbol{X}} boldsymbol{B}_{boldsymbol{Y}} )
is a non volatile solute. What is the
value of a if the vapour pressure of pure methanol is ( a times 10^{2} ) torr.
12
630llustration 2.146 What are isotonic solutions?12
631Example 2.10 Calculate the osmotic pressure of a solution
obtained by mixing 100 cm of 1.5% solution of urea (mol.
mass=60) and 100 cm of 3.42% solution by cane sugar (mol.
mass = 342) at 20°C. (R = 0.082 litre atm/deg/mole)
12
632Q. 10 The unit of ebullioscopic constant is
(a) K kg mol-‘or K(molality) (b) mol kg K-‘or K-‘ (molality)
(c) kg mol-‘K-‘ork-‘(molality)-! (d) K mol kg- or K (molality)
Thinking Process
Write the formula of ebullioscopic constant then put the values of their unit and then
calculate unit of ebullioscopic constant.
12
633For a dilute solution containing ( 2.5 g m ) of a non-volatile non-electrolyte solute in ( 100 g m ) of water, the elevation in boiling point at 1 atm pressure is ( 2^{circ} C ) Assuming concentration of solute is much lower than the concentration of
solvent, the vapour pressure (mm of ( boldsymbol{H} boldsymbol{g} )
of the solution is ( left(boldsymbol{K}_{boldsymbol{b}}=right. )
( left.0.76 K k g m o l^{-1}right) )
A .724
в. 740
( c .736 )
D. 718
12
634Vant Hoff factor (i) for dimerisation of benzoic acid insome solvent
assuming ( 30 % ) degree of association
A . 0.85
B. 0.95
( c .0 .90 )
D.
12
635Depression in f.pt. is more pronounced if camphor is used as a solvent in place of water for same mass of solute and
solvent.
If true enter ( 1, ) if false enter 0
12
636What is the difference between
lyophobic sol and lyophilic sol?
12
637If you mix 3 litres of 0.5M ( N a C l ) with 9 litres of ( 0.2777 mathrm{M} N a C l ) what will the
concentration of the final solution be
в. 0.39 м
c. ( 0.5777 mathrm{M} )
D. 0.6777 M
E. None of the above
12
638A current of ( 4.0 A ) is passed for 5 hours through ( 1 L ) of ( 2 M ) solution of nickel
nitrate using two nickel electrodes. The molarity of the solution at the end of the electrolysis will be:
( mathbf{A} cdot 1.6 M )
в. ( 1.2 M )
c. ( 2.5 M )
D. ( 2.0 M )
12
639In a very ideal imaginary condition, a sample of ice was taken, and its osmotic pressure was found to be 0.274 ( operatorname{atm} ) at ( 300 mathrm{K} ) (density ( =1 mathrm{g} / mathrm{mL} ) ). Thus, number of water units attached to one
water unit is
( A cdot 4 )
B. 3
( c cdot 6 )
( D .5 )
12
640Tlustration 2.185 A 1.17% solution of NaCl is isotonic with
7.2% solution of glucose. Calculate the Van’t Hoff factor of
NaCl.
12
641Why does solution of chloroform &
acetone show negative deviation from
Raoult’s law?

Illustrate the deviation with the help of diagrams

12
642If observed vapour pressure is greater
than ideal vapour pressure then:
A. it is known as negative deviation from Raoult’s law
B. it is known as ideal solution
C. it is known as positive deviation from Raoult’s law
D. None of these
12
643A mixture of ethanol and water contains
( 54 % ) water by mass. Calculate the mole fraction of ethanol in this solution.
A. 0.25
B. 0.15
( c cdot 0.20 )
D. 0.30
12
644The boiling point of water at 735 torr is
( 99^{circ} mathrm{C} . ) The mass of ( mathrm{NaCl} ) added in 100
( operatorname{gmof} sin operatorname{tar}left(K_{b}=0.51 K k g m o l^{-3}right) ) to
make its boiling point at ( 100^{circ} mathrm{C} ) is:
A ( .10 .68 mathrm{g} )
B. ( 5.34 mathrm{g} )
c. 2.67 g
D. 26.7 g
12
645Statement – I: ( 1 mathrm{M} ) solution of NaCl has a
higher osmotic pressure than 1 M solution of glucose at the same temperature. Statement – II: The number of particles present in 1 M NaCl solution are more
than those present in 1 M glucose solution and osmotic pressure depends upon number of particles present in the
solution.
A. Statement-lis True, Statement – II is True; Statement I is a correct explanation for Statement –
B. Statement-lis True, Statement – /I is True; Statement I is NOT a correct explanation for Statement- –
c. Statement – – is True, Statement – II is False
D. Statement-lis False, Statement – II is True
12
646Flour, salt, sugar, eggs and baking powder are ingradients for baking a cake, when you mix these ingradients, you get batter. Is batter a mixture or a compound? The batter is put into an oven to bake into a cake. Is the cake a
mixture or a compound? Explain your
12
647The vapour pressure of pure benzene at
a certain temperature is 0.850 bar. ( A ) non-volatile, non-electrolyte solid weighing ( 0.5 g ) is added to ( 39.0 g ) of benzene (molar mass ( 78 g / )mol ). The vapour pressure of the solution then is
( mathbf{0 . 8 4 5} ) bar. What is the molecular mass
of the solid substance?
( mathbf{A} .58 )
в. 180
( c .170 )
D. 145
12
648The difference in height of the mercury column in two arms of U tube
manometer in the arrangement – lis ( boldsymbol{h}_{1}=mathbf{6 6 0} mathrm{mm} . ) In another arrangement –
Il at same temperature, 222 gm of
( mathrm{CaCl}_{2} ) is dissolved in ( 324 mathrm{gm} ) of water and difference in height of mercury
column in two arms is found to be ( h_{2}= )
( 680 mathrm{mm} . ) If the value of degree of
dissociation for ( C a C l_{2} ) in arrangement
-11 is ( alpha, ) then the value of ( 64 alpha ) is:
[Atmospheric pressure ( =1 ) atm]
A . 40
B. 38
c. 45
D. 50
12
649In case of an electrolyte which
dissociates in the solution, the van’t
hoff factor ( i ) is :
( A cdot>1 )
в. ( 1 ) or ( <1 )
12
650The solubility curve of ( boldsymbol{K} boldsymbol{N} boldsymbol{O}_{3} ) in water is shown below.

The amount of ( K N O_{3} ) that dissolves in
( 50 g ) of water at 40 is closest to:
A . 100 g
B. 150 g
c. ( 200 g )
D. ( 50 g )

12
651Assertion
The solubility of ammonium chloride increases with increase in temperature
Reason In case of substances whose solubility increases with increase in temperature is due to the dissolution process being endothermic.
A. Both Assertion and Reason are correct and Reason is the correct explanation for Assertion
B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion
c. Assertion is correct but Reason is incorrect
D. Both Assertion and Reason are incorrect
12
652What is meant by positive and negative
deviations from Raoult’s law and how is
the sign of ( Delta_{m i x} H ) related to positive
and negative deviations from Raoult’s law?
12
653( boldsymbol{H}_{2} boldsymbol{S} ) a toxic gas with rottenegg like smell is used for the qualetative
analysis, if the solubility of ( H_{2} S ) in
water,at STP is 0.195mole.kg ( ^{-1} ), the Henry’s law constant is:
A. 282 bar
B. 324.8 bar
c. 462.9 bar
D. 534.8 bar
12
654The standard reduction potential of the ( A g^{+} mid A g ) electrode at ( 298 mathrm{K} ) is ( 0.80 mathrm{V} )
The solubility product of ( A g l ) is ( 6.4 times ) ( 10^{-17} ) at ( 298 mathrm{K} .(2.303 mathrm{RT} / mathrm{F}=0.06) )
The potential of ( A g^{+} mid A g ) electrode in a saturated solution of Agl at ( 298 mathrm{K} ) is
( mathbf{A} cdot-0.314 V )
B . ( +0.314 V )
c. ( -0.172 V )
D. ( +0.172 mathrm{V} )
12
655The osmotic pressure of a solution in atm obtained on mixing each 50 mL of ( 1.2 % ) mass/volume urea solution and
( 2.4 % ) mass/volume glucose solution at ( mathbf{3 0 0} mathrm{K} ) is: ( (boldsymbol{R}=mathbf{0 . 0 8} ) litre atm
( left.boldsymbol{K}^{-1} boldsymbol{m o l}^{-1}right) )
12
656Two moles of ( O_{2} ) gas is collected over
water at ( 400 mathrm{K} ) temperature in 2
litre vessel. If the pressure of dry ( O_{2} ) gas is 32.20 bar then find the vapour pressure of water under the same
conditions.
12
657An aqueous solution of hydrochloric
acid
A. obeys Raoult’s law
B. shows negative deviation from Raoult’s law
C. shows positive deviation from Raoult’s law
D. obeys Henry’s law at all compositions
12
658If we add potassium nitrate to ice it will result in
(a) Increase in m.p. of ice.
(b) Decrease in m.p. ofice
(c) Neither (a) nor (b)
(d) Change in colour of ice
12
659Which of the following is true about a solution that has ( [boldsymbol{O H}]=mathbf{1 . 0} times mathbf{1 0}^{-mathbf{8}} )
M?
A. The pHis 8 and the solution is acidic
B. The ( left[H^{+}right]=1.0 times 10^{-8} mathrm{M} ) and the solution is basic
c. The pHis 6 and the solution is acidic
D. The ( left[H^{+}right]=1.0 times 10^{-6} mathrm{M} ) and the solution is basic
E . The ( left[H^{+}right]=1.0 times 10^{-14} mathrm{M} ) and the solution is neutral
12
6600.1 molal-equeous solution of an electrolyte ( mathrm{FeCl}_{2} ) is ( 80 % ) ionised. The
boiling point of the solution at 1 atm is:
( left[mathbf{K}_{mathbf{6}}left(mathbf{H}_{2} mathbf{O}right)=mathbf{0 . 5 2} mathbf{K} mathbf{k g} mathbf{m o l}^{-mathbf{1}}right] )
A. ( 273.17 K )
B . ( 273.19^{circ} mathrm{C} )
c. ( 373.19^{circ} mathrm{C} )
D. ( 100.17^{circ} mathrm{C} )
12
661(1) Define the following
(i) Henry’s law
(ii) Normality.
12
662. 32 The density of 3 molal solution of NaOH is 1.110 g mL . Calculate the
molarity of the solution.
12
663The Van’t Hoff factor of ( 0.1 mathrm{M} mathrm{Ba}left(mathrm{NO}_{3}right)_{2} )
solutions is ( 2.74 . ) The degree of dissociation will be
A . 91.3%
B. 87%
c. ( 100 % )
D. 74%
12
664Henry’s law constant for molality of methane in benzene at ( 298 K ) is ( 4.27 times )
( 10^{5} ) mm ( H g . ) The mole fraction of
methane in benzene at ( 298 K ) under
( 760 m m H g ) is:
A. ( 1.78 times 10^{-3} )
B. 17.43
c. 0.114
D. 2.814
12
665When ( 100 m l ) of ( 0.06 m mathrm{Fe}left(N O_{3}right)_{3}, 50 m l )
of ( 0.2 m l F e C l_{3} ) and ( 100 m l ) of
( 0.26 m m gleft(N O_{3}right)_{2} ) are mixed, then
calculate molarity of reaction in final solution.
12
666Sulphuric acid reacts with sodium hydroxide as follows
( H_{2} S O_{4}+2 N a O H rightarrow N a_{2} S O_{4}+2 H_{2} O )
When 1 L of 0.1 M sulphuric acid solution is allowed to react with 1 L of ( 0.1 mathrm{M} )
sodium hydroxide solution, the amount of sodium sulphate formed and its molarity in the solution obtained is ?
A. ( 0.1 mathrm{molL}^{-1} )
B. ( 7.10 g )
c. 0.025 mol ( L^{-1} )
D. ( 3.55 g )
12
667A ( 500 g ) tooth paste sample has ( 0.02 g m ) fluoride concentration. What is the
concentration of fluorine in terms of
ppm levels?
A .250
B. 40
c. 400
D. 1000
12
668The vapour pressure of two pure liquids ( A ) and ( B ) are 50 and 40 torr respectively. If 8 moles of ( A ) is mixed with ( x ) moles of
B, then vapour pressure of solution obtained is 48 torr. What is the value of
x?
12
669Which of the following dissolves more rapidly in blood haemoglobin than oxygen?
A. Ozone
B. Nitrous oxide
c. sulphur dioxide
D. Carbon monoxide
12
6701. What should be the boiling point of 1.0 molal aqueous
KCl solution (assuming complete dissociation of KCT)if|
K, HO is 0.52 K m-l?
a. 100.52°C
b. 101.04°C
c. 99.48°C
d. 98.96°C
12
671The normal boiling point of a liquid is that temperature at which vapour pressure of the liquid is equal to:
A. zero
B. 380 mm of Hg
c. ( 760 mathrm{mm} ) of ( mathrm{Hg} )
D. ( 100 mathrm{mm} ) of ( mathrm{Hg} )
12
672A ( 5.25 % ) solution of a substance is isotonic with a ( 1.5 % ) solution of urea
(molar mass ( =60 g ) mol ( ^{-1} ) ) in the same
solvent. If the densities of both the
solutions are assumed to be equal to
( 1.0 g c m^{-3}, ) molar mass of the substance will be:
в. ( 90.0 g ) mol( ^{-1} )
c. ( 115.0 g ) mol ( ^{-1} )
D. ( 105.0 g ) mol ( ^{-1} )
12
673How many grams of NaCl will be required to make a ( 100 . ) milliliters of ( 2 mathrm{M} )
solution?
A . 5.85
в. 11.7
c. 29.2
D. 58.5
E .117
12
674If 1 mole of ethyl alcohol in 1,000 grams of water depresses the freezing point by
( 1.86^{circ} mathrm{C}, ) what will be the freezing point
of a solution of 1 mole of ethyl alcohol in
( mathbf{5 0 0} ) grams of water?
A ( .-0.93^{circ} mathrm{C} )
В. ( -1.86^{circ} mathrm{C} )
( mathbf{c} cdot-2.79^{circ} mathrm{C} )
D. ( -3.72^{circ} mathrm{C} )
E . ( -5.58^{circ} mathrm{C} )
12
675The mole fraction of methanol in 4.5
molal aqueous solution is:
A. 0.250
B. 0.125
c. 0.100
D. 0.075
E. 0.055
12
676A solution is prepared by dissolving ( 5.64 mathrm{g} ) of glucose in ( 60 mathrm{g} ) of water. Calculate the molality of the
solution.
A. ( 0.281 mathrm{m} )
B. 1.21 ( mathrm{m} )
( c cdot 1.044 mathrm{m} )
D. 0.522 ( mathrm{m} )
12
677A ( 0.01 m ) aqueous solution of
( boldsymbol{K}_{3}left[boldsymbol{F} boldsymbol{e}(boldsymbol{C} boldsymbol{N})_{6}right] ) freezes ( mathbf{a t}-mathbf{0 . 0 6 2}^{circ} boldsymbol{C} )
What is the apparent percentage of
dissociation? ( left[boldsymbol{K}_{f} text { for water }=mathbf{1 . 8 6}right] )
[Note : write the value to the nearest integer
12
678What is the molarity of a solution that has 29.25 grams of NaCl dissolved to make ( 1.5 mathrm{L} ) of a solution?
A . 19.5 М
B. 3.0 М
c. 1.75 М
D. 0.33 м
E ( .1 .0 mathrm{M} )
12
679Van’t Hoff factor of a mixture of two
moles of KI with 1 mole ( H g I_{2} ) in a
solution of water is :
12
680An aqueous solution of glucose is ( 10 % ) (w/v). The volume in which 1 mole of glucose is dissolved, will be:
( mathbf{A} cdot 180 mathrm{L} )
B. 91 L
c. ( 0.91 mathrm{L} )
D. 1.8 L
12
681Vapour pressure of chloroform
( left(C H C l_{3}right) ) and dichloromethane
( left(C H_{2} C l_{2}right) ) at ( 298 K ) are ( 200 m m H g )
and 415 mm ( H g ) respectively.
(i) Calculate the vapour pressure of the solution prepared by mixing ( 25.5 g ) of
( boldsymbol{C H} boldsymbol{C l}_{3} ) and ( mathbf{4 0} boldsymbol{g} ) of ( boldsymbol{C H}_{2} boldsymbol{C l}_{2} ) at ( boldsymbol{2} boldsymbol{9 0} boldsymbol{K} )
and
(ii) Mole fraction of each component in solution.
12
682In the system ( : boldsymbol{F e}(boldsymbol{O H})_{3(s)} rightleftharpoons boldsymbol{F e}_{(a q)}^{3+}+ )
( 3 O H_{(a q)}^{-}, ) decreasing the conc. of ( O H^{-} ) ions ( frac{1}{3} ) times will cause the equilibrium
conc of ( F e^{3+} ) to increase
times.
( A cdot 3 )
B. 9
c. 18
D. 27
12
683In reverse osmosis the flow of solvent
molecules is from:
A. solution side to solvent side
B. solvent side to solution side
c. solvent molecules stay unmoving
D. none of these
12
684( 1 times 10^{-3} mathrm{kg} ) of urea is present in 400
cubic centimetre solution at ( 310 mathrm{K} )
Calculate the approximate osmotic pressure of the solution. ( left(boldsymbol{R}=mathbf{8 . 3 1 4} boldsymbol{J} boldsymbol{m o l}^{-1} boldsymbol{K}^{-1}, ) molecular right.
weight of urea ( =60 ) )
( A cdot 1 ) atm
B. 2 atm
( c cdot 4 a t m )
( D cdot 5 ) atm
12
685The potential of hydrogen electrode is
( -118.5 mathrm{mV} . ) The ( H^{+} ) concentration of
the solution is:
A . 0.01 M
в. 2 м
( c cdot 10^{-4} ) м
D. 1 M
12
686Hlustration 2.113 An aqueous solution of a non-volatile
solute boils at 100.17°C.At what temperature will the solution
freeze?
(Given: K = 0.512 and K. = 1.86)
12
687The Henry’s law constant for helium gas
in water at ( 30^{circ} mathrm{C} ) is ( 3.70 times 10^{-4} mathrm{M} / mathrm{atm} )
When the partial pressure of helium above a sample of water is 0.650 at ( mathrm{m} ) the concentration of helium in the water
is
M.
A. ( 5.69 times 10^{-4} )
В. ( 1.76 times 10^{3} )
c. 1.30
D. ( 2.41 times 10^{-4} )
E . ( 3.70 times 10^{-4} )
12
688The value of van’t Hoff factor for ( 0.1 mathrm{M} )
( B aleft(N O_{3}right)_{2} ) solution is ( 2.74 . ) The degree of dissociation is:
( mathbf{A} cdot 100 % )
B. ( 92 % )
c. ( 87 % )
D. ( 74 % )
12
689Which of the following forms ideal solution?

This question has multiple correct options
A ( cdot C_{6} H_{5} C l-C_{6} H_{5} B r )
в. ( C_{6} H_{6}-C_{6} H_{5} C H_{3} )
c. Hexane-heptane
D. none of these

12
690The freezing point depression of 0.1 molal solution of acetic acid in benzene
is ( 0.256 mathrm{K}, K_{f} ) for benzene is ( 5.12 K K g m o l^{-1} . ) What condition can
you draw about the molecular state of
acetic acid in benzene?
A. Acetic acid is doubly associated
B. Benzene is doubly associated
c. Both are equally associated
D. None of the above
12
691Henry’s Law constant for ( C O_{2} ) in water
is ( 1.67 times 10^{8} ) Pa at ( 298 mathrm{K} ). Calculate the
quantity in 1 L of soda water when packed under 2.5 atm pressure at 298 ( mathrm{K} )
12
692( F e C l_{3} ) on reaction with ( K_{4}left[F e(C N)_{6}right] ) in aqueous solution gives blue colour
These are separated by a
semipermeable membrane AB as
shown. Due to osmosis, there is:
A. Blue color formation in side ( x )
B. Blue color formation in side Y.
c. Blue colour formation in both of the sides ( x ) and
D. No blue colour formation
12
693Vapor pressure of pure water at ( 25^{circ} mathrm{C} ) is
( 20.0 mathrm{mm} ) of ( H g % . ) And the lowering of
vapor pressure of a sugar solution is
( 0.070 mathrm{mm} ) of ( H g . ) What will be the mole
fraction of water?
A . 0.9965
B. 0.0035
c. 0.0024
D. 0.7785
12
694An aqueous solution of a weak monobasic acid containing 0.1 g in 21.7 g of water freezes at ( 272.813 mathrm{K} ). If the value
of ( K_{f} ) for water is ( 1.86 mathrm{K} / mathrm{m}, ) what is the molecular mass of the monobasic acid.
12
695If the various terms in the below-given expressions have usual meanings, the van’t Hoff factor ( ( i ) ) cannot be calculated
by which of the following expression?
A ( . pi V=sqrt{i n R T} )
B. ( Delta T_{f}=i K_{f}-m )
c. ( Delta T_{b}=i K_{b}-m )
( frac{P_{text {solvent}}^{o}-P_{text {solution}}}{P_{text {solvent}}^{o}}=ileft(frac{n}{N+n}right) )
12
696Illustration 2.153 What is osmotic pressure and how is it
related with the molecular mass of a non-volatile substance?
What advantage the osmotic pressure method has over the
elevation of boiling point method for determining molecular
masses?
12
697If ( mathrm{SR}=100 ) torr and ( mathrm{PR}=350 ) torr, then
which of the following cannot be a mole
fraction of ( A ) in vapour phase and a mole
fraction of ( A ) in liquid phase
respectively?
This question has multiple correct options
A ( cdot frac{3}{10} ) and ( frac{2}{9} )
B. ( frac{7}{9} ) and ( frac{3}{10} )
c. ( frac{2}{9} ) and ( frac{7}{10} )
D. ( frac{2}{9} ) and ( frac{3}{10} )
12
698Illustration 2.180 A 0.5% aqueous solution of KCl was
found to freeze at -0.24°C. Calculate the Van’t Hoff factor
and degree of dissociation of the solute at this concentration.
(K, for water = 1.86 K kg mol-l)
12
699The solubility of ( N_{2} ) in water at ( 300 mathrm{K} ) and 500 torr, partial pressure is ( 0.01 mathrm{g} ) ( L^{-1} . ) The solubility ( left(operatorname{in} g L^{-1}right) ) at 750 torr partial pressure is:
A. 0.0075
B. 0.015
c. 0.02
D. 0.005
12
700The freezing point depression constant
for water is ( 1.86^{circ} mathrm{C} boldsymbol{m}^{-1} . ) If ( 5 mathrm{g} N a_{2} mathrm{SO}_{4} )
is dissolved in 45 g ( H_{2} O ), the freezing
point is changed by ( -3.82^{circ} mathrm{C} )
Calculate the van’t Hoff factor for
( N a_{2} S O_{4} )
A .0 .381
B . 2.05
( c .2 .63 )
D. 3.11
12
701Which one of the following is the ratio of the lowering of vapour pressure of ( 0.1 M ) aqueous solution of
( B a C l_{2}, N a C l ) and ( A l_{2}left(S O_{4}right)_{3} )
respectively?
A .3: 2: 5
B. 5: 2: 3
( mathrm{c} .5: 3: 2 )
D. 2: 3: 5
12
702If the concentration of ( O H^{-} ) ions in the
reaction ( boldsymbol{F e}(boldsymbol{O H})_{3}(boldsymbol{s}) rightleftharpoons boldsymbol{F} boldsymbol{e}^{+3}(boldsymbol{a q} cdot)+ )
( 3 O H^{-}(a q .) ) is decreased upto ( frac{1}{4} ) times
then equilibrium concentration of ( boldsymbol{F} boldsymbol{e}^{+} ) will increase upto:
A. 16 times
B. 64 times
c. 4 times
D. 8 times
12
703An azeotropic solution of two liquids has boiling point lower than either of them when it:
A. shows a negative deviation from Raoult’s law
B. shows no deviation from Raoult’s law
c. shows positive deviation from Raoult’s law
D. is saturated
12
704Ulustration 2.147 Outer hard shells of two eggs are
removed. One of the eggs is placed in pure water and the other
is placed in saturated solution of sodium chloride. What will
be observed and why?
12
705In a mixture of kerosene and water,
kerosene forms the:
A. Lower layer
B. Upper layer
c. It mixes with water and forms no layer
D. Data insufficient
12
706Vapour pressure of a pure liquid ( X ) is 2 ( operatorname{atm} ) at ( 300 mathrm{K} ). It is lowered to 1 atm on
dissolving 1 g of ( Y ) in ( 20 g ) of liquid ( X ). If
molar mass of ( X ) is 200 , what is the
molar mass of ( Y ? )
A . 20
B. 10
c. 100
D. 30
12
707Which of the following solution has the highest boiling point?
A. ( 1 % ) glucose
B . ( 1 % ) NaCl
c. ( 1 % ) sucrose
D. ( 1 % ) CaCl( _{2} ),
12
708Assertion: The rate at which sugar
dissolves in water increases with
stirring
Reason: Stirring exposes the surface of a solute crystal to a less concentrated
layer of solution.
A. Both Assertion and Reason are correct and Reason is the correct explanation of Assertion
B. Both Assertion and Reason are correct but Reason is the correct explanation of Assertion
c. Assertion is correct but Reason is not correct
D. Assertion is not correct but Reason is correct
E. Both Assertion and Reason are not correct
12
709( 2 S O_{3} rightleftharpoons 2 S O_{2}+O_{2} . ) If ( K_{c}=100, alpha=1 )
half of the reaction is completed, the
concentration of ( S O_{3} ) and ( S O_{2} ) are
equal, the concentration of ( O_{2} ) is ?
A. ( 0.001 M )
M
в. ( frac{1}{2} S O_{2} )
( mathrm{c} cdot 2 ) times of ( mathrm{SO}_{2} )
D. Data incomplete
12
710Why do gases always tend to be less
soluble in liquids as the temperature is raised?
12
711Van’t Hoffs factor for a solution is less
than one, what is the conclusion drawn
from it.
12
712Ethanol-Water mixture(95% by volume of ethanol) forms:
A. maximum boiling azeotrope
B. minimum boiling azeotrope
c. solution which shows negative deviation
D. ideal solutions
12
713Calculate the molarity of ( 9.8 % ) solution
of ( mathbf{H}_{2} mathbf{S O}_{4} ) if the density of the solution is
( 1.02 mathrm{gmL}^{-1} )
12
714( mathbf{A} )
(homogeneous/heterogeneous) mixture of solute and solvent is known as
solution.
12
715toppr
1.
of certain molarity was added gradually. The mass of precipitate produced (in g)
were measured and it was plotted
against volume of ( A g N O_{3} ) solution
added (in ml). Its known that ( A g I ) is
precipitated first. Precipitation of ( boldsymbol{B} boldsymbol{r} )
does not start until the already
precipitating ( boldsymbol{I}^{-} ) precipitates
completely. Find out the value of ( boldsymbol{A B} times )
CD where:
( A B= ) Atomic weight of metal ( M )
( C D= ) Mole percent of ( N a l ) in original
mixture.
( mathbf{A} cdot 4994 )
B . 2040
c. 3202
D. 3332
12
716Total vapour pressure of mixture of 1 mole of ( boldsymbol{A}left(boldsymbol{P}_{A}^{0}=mathbf{1 5 0 m m}right) ) and 2 mole of
B ( left(P_{B}^{0}=240 m mright) ) is ( 200 m m . ) In this
case:
A. There is a positive deviation from Raoult’s law
B. There is a negative deviation from Raoult’s law
c. There is no deviation from Raoult’s law
D. Molecular masses of A & B are also required for calculating deviation
12
717A salt is made by adding an excess of an insoluble metal oxide to an acid. How
is the excess metal oxide removed from
the mixture?
A. chromatography
B. crystallisation
c. distillation
D. filtration
12
718Concentration 1 microgram per gram is ( boldsymbol{x} ) ppm. Then, the value of ( boldsymbol{x} ) is :12
7192. The ratio of freezing point depression values of 0.01 M
solutions of urea, common salt, and Na SO4 are
a. 1:1:1 b. 1:2:1 c. 1:2:3 d. 2:2:3
12
720Select the correct statements.
(I) Increase in relative humidity decreases the density of air
(II) Increase in relative humidity decreases the rate of evaporation of
water
(III) Increase in relative humidity
decreases the velocity of sound
(IV) Increase in relative humidity increases the velocity of sound
A . ।, ॥, । v
в. ।, и, III
( c cdot 1,1 )
D. I, IV
12
721Mention the enthalpy of mixing
( left(triangle_{m i x} Hright) ) value to form an ideal
solution.
12
722Q. 13 At a given temperature, osmotic pressure of a concentrated solution of a
substance ……….
(a) is higher than that of a dilute solution
(b) is lower than that of a dilute solution
(c) is same as that of a dilute solution
(d) cannot be compared with osmotic pressure of dilute solution
12
723A solution prepared by dissolving a ( 2.50 g ) sample of an unknown compound dissolved in ( 34.0 g ) of benzene,
( C_{6} H_{6} ) boils at ( 1.38^{circ} C ) higher than pure benzene. Which expression gives the molar mass of the unknown compound
( ? )
Compound ( K_{b} )
( boldsymbol{C}_{6} boldsymbol{H}_{6} quad boldsymbol{2 . 5 3}^{circ} boldsymbol{C} cdot boldsymbol{m}^{-1} )
A ( cdot 2.53 times frac{2.50}{1.38} )
в. ( _{1.38} times frac{34.0}{2.53} times 2.50 )
c. ( 2.50 times 10^{3} times frac{2.53}{34.0} times frac{1}{1.38} )
D. ( 2.50 times 10^{3} times frac{1.38}{34.0} times 2.53 )
12
724When ( 1.88 g ) of ( operatorname{AgBr}(s) ) is added to a
( 10^{-3} M ) aqueous solution of ( K B r, ) the concentration of ( mathrm{Ag} ) is ( 5 times 10^{-10} mathrm{M} ). If the
same amount of ( A g B r(s) ) is added to a
( 10^{-2} ) M aqueous solution of ( A g N O_{F} )
the concentration of ( B r^{-} ) is:
A . ( 9.4 times 10^{-9} M )
В. ( 5 times 10^{-10} M )
c. ( 1 times 10^{-11} M )
D. ( 5 times 10^{-11} M )
12
725Example 2.15 A 10 g mixture of glucose and urea present
in 250 mL solution shows the osmotic pressure of 7.4 atm at
27°C. Calculate % composition of mixture.
12
726The sum of mole fractions of solute and
solvent of a solution is equal to:
A. number of moles of solute
B. number of moles of solvent
c. number of mole of solution
D. unity
12
727The plots of ( frac{1}{X_{A}} v s cdot frac{1}{Y_{A}}left(text { where }, X_{A} text { and } Y_{A}right. ) are the mole fraction of liquid ( A ) in liquid and vapour phase respectively) is linear with slope and intercepts respectively
( ^{mathbf{A}} cdot p_{A}^{0} / P_{B}^{0} ) and ( frac{left(P_{A}^{0}-P_{B}^{0}right)}{P_{B}^{0}} )
в. ( quad P_{A}^{0} / P_{B}^{0} ) and ( frac{left(P_{B}^{0}-P_{A}^{0}right)}{P_{B}^{0}} )
( ^{mathbf{c}} P_{B}^{0} / P_{A}^{0} ) and ( frac{left(P_{A}^{0}-P_{B}^{0}right)}{P_{B}^{0}} )
( P_{B}^{0} / P_{A}^{0} ) and ( frac{left(P_{B}^{0}-P_{A}^{0}right)}{P_{B}^{0}} )
12
728A solution contains ( 3.22 g ) of ( H C l O_{2} ) in
( 47.0 g ) of water. The freezing point of the
solution is ( 271.10 K )

Calculate the fraction of ( H C l O_{2} ) that
undergoes dissociation to ( boldsymbol{H}^{+} ) and
( C l O_{2}^{-} )
Given: ( boldsymbol{K}_{f}(boldsymbol{w} boldsymbol{a} boldsymbol{t e r})=mathbf{1 . 8 6} boldsymbol{K} boldsymbol{k g} boldsymbol{m o l}^{-1} )
B. ( alpha=0.204 )
C . ( alpha=0.30 )
D. ( alpha=0.60 )

12
7290.4 If 500 mL of a 5M solution is diluted to 1500 mL, what will be the
molarity of the solution obtained?
(a) 1.5 M
(b) 1.66 M (c) 0.017 M (d) 1.59 M
Thinking
12
730The van’s Hoff factor for 0.1 molar
( B aleft(N O_{3}right)_{2} ) solutions is ( 2.74 . ) Its degree of dissociation is:
A . 0.74
в. 0.87
c. 0.91
D. 1.0
12
731a. Which gas is dissolved in soft drinks?
What will you do to increase the solubility of this gas?
12
732Which of the following statment is
incorrect?
A. Greater the lowering of vapour pressure, greater is the boiling point of the solution
B. Greater the lowering of vapour pressure, greater is the freezing point of the solution
C. At the freezing point, the solute and the solvent have same vapour pressure
D. The units of molal depression constant are ( K m^{-1} )
12
733A tube of uniform cross-sectional area
( 1 c m^{2} ) is closed at one end with the
semipermeable membrane. a solution of 5 g glucose per 100 mL is placed inside the tube and is dipped in pure
water at ( 27^{circ} mathrm{C} ). When equilibrium is established the height developed in a vertical column in cm is ( 1000 x ). (Assume the density of final glucose solution ( 18 / mathrm{mL} )
Find the value of ( X )
12
734A solution containing 8 g of a substances in 100 g of diethyl ether
boils at ( 36.86^{circ} mathrm{C} ). Where as pure ether
boils at ( 35.60^{circ} mathrm{C} ). Determine the
molecular mass of the solute. (For ether,
( boldsymbol{K}_{boldsymbol{b}}=mathbf{2 . 0 2 mathrm { k }} mathrm{kh} boldsymbol{m o l}^{-1} mathbf{)} )
12
735Example 2.11 A solution containing 6 g of a solute dissolved
in 250 cm of water gave an osmotic pressure of 4.5 atm at
27°C. Calculate the boiling point of the solution. The molal
elevation constant for water is 0.52°C per 1000 g.
12
736Illustration 2.40 Two liquids A and B have vapo
pressures in the ratio of paº; PR° = 1: 2 at a certain
temperature. Suppose we have an ideal solution of A and B in
the mole fraction ratio A:B=1: 2. What would be the mole
fraction of A in the vapour in equilibrium with the solution
at a given temperature?
a. 0.25 b. 0.2
c. 0.5
d. 0.33
12
737. 34 For a binary ideal liquid solution, the variation in total vape
versus composition of solution is given by which of the curve
(C)
p
12-
12
738One mole of sugar is dissolved in two moles of water. The vapour pressure of the solution relative to that of pure
water is:
( A cdot 2 / 3 )
B. ( 1 / 3 )
c. ( 3 / 2 )
D. ( 1 / 2 )
12
739At a given temperature, total vapour pressure in Torr of a mixture volatile
components A and B is given by
( boldsymbol{P}_{text {Total}}=mathbf{1 2 0}-mathbf{7 5 X}_{boldsymbol{B}} )
Hence, vapour pressure of pure ( A ) and ( B ) respectively (in Torr) are?
A . 120,75
в. 120, 195
( c cdot 120,45 )
D. 75, 45
12
740Example 2.32 0.5 m solution of acetic acid (Mw = 60) in
benzene (Mw=78) boils at 80.80°C. The normal boiling point
of benzene is 80.10°C and Ava H=30.775 kJ mol-1. Calculate
the percent of association of acetic acid in benzene.
12
741A mixture of ( a ) mol of ( C_{3} H_{8} ) and ( b ) mol of
( C_{2} H_{4} ) was kept is a container of ( V ) L
which exerts a pressure of 4.93 atm at temperature T. Mixture was burnt in
presence of ( O_{2} ) to convert ( C_{3} H_{8} ) and
( C_{2} H_{4} ) into ( C O_{2} ) in the container at the
same temperature. The pressure of gases after the reaction and attaining the thermal equilibrium with atmosphere at temperature T was
found to be 11.08 atm.

The mole fraction of ( C_{3} H_{8} ) in the
mixture is :
A .0 .25
в. 0.75
( c cdot 0.45 )
D. 0.55

12
742Which of the following graph shows the best relationship of the number of
grams of a solid that are soluble in 100
( operatorname{grams} ) of ( H_{2} O ) at varying temperature if
the solubility begins at a small quality and increases at a slow, steady pace as the temperature is increased?
( A cdot A )
B. B
( c cdot c )
D.
E.
12
743There is ( 50 % ) dimer formation of benzoic
( operatorname{acid}left(C_{6} H_{5} C O O Hright) ) in benzene
solution.
( 2 C_{6} H_{5} C O O H rightleftharpoonsleft(C_{6} H_{5} C O O Hright)_{2} )
Hence the abnormal molecular weight of benzoic acid ( theoretical value ( =122 )
( left.g m o l^{-1}right) ) is:
A. ( 61 mathrm{g} ) mol ( ^{-1} )
B. 244 g mol-
c. ( 163 mathrm{g} ) mol ( ^{-1} )
D. 81 g ( m o l^{-1} )
12
744( 2 mathrm{g} ) benzoic acid ( left(C_{6} H_{5} C O O Hright) )
dissolved in 25 g of benzene shoes a depression in freezing point equal to 1.62 K. Molal depression constant for benzene is ( 4.9 mathrm{K} mathrm{kg} ) mol( ^{-1} . ) What is the percentage association of acid if it
forms dimer in solution?
12
745If quantities ( Delta T_{f}, Delta T_{b}, Delta p ) and ( pi ) without subscript refer to the electrolyte solution and these with subscript refer to non-electrolyte solution then which one is wrong?
( ^{mathbf{A}} cdot_{i}=frac{Delta T_{f}}{left(Delta T_{f}right)_{0}} )
в. ( _{i}=frac{Delta T_{b}}{left(Delta T_{b}right)_{0}} )
c. ( _{i}=frac{Delta P}{left(P^{0}right)_{0}} )
D. ( _{i}=frac{pi}{(pi)_{0}} )
12
746If ( 6.022 times 10^{23} ) molecules of urea are
present in 100 ml of its solution, then
calculate the concentration of the
solution (Molecular mass of urea ( =mathbf{6 0} ) )
12
7470.56 Using Raoult’s law explain how the total vapour pressure over the solution
is related to mole fraction of components in the following solutions.
(a) CHCL3 (L) and CH,CL, (l) (b) NaCl(s) and H20 (1)
12
748A ( 500 mathrm{mL} ) solution is prepared by dissolving 20 g sodium hydroxide in water. This is mixed in another ( 200 mathrm{mL} )
solution of ( N a O H ) having molarity 0.2
M. The molarity of resulting solution is:
A. 0.66 M
в. 0.77 М
c. ( 1.80 mathrm{M} )
D. 1.97 М
12
749Illustration 2.88 The boiling point of a solution made by
dissolving 12.0 g of glucose in 100 g of water is 100.34°C.
Calculate the molecular weight of glucose; K, for water
= 0.52°C/m.
12
750Which of the following may be dissolved
in water?
A. Alcohol
B. Ether
c. Amine
D. all of these
12
751Unsaturated solvents are
filled with solutes.
A. completely
B. not completely
c. Both a and
D. None of the above
12
752A solution of a substance containing 1.05 g per 100 mL was found to be isotonic with ( 3 % ) glucose solution. The molecular mass of the substance is:
A . 31.5
B. 6.3
( c .630 )
D. 63
12
753Two liquids ( A ) and ( B ) have vapour
pressures in the ratio ( P_{A}^{0}: P_{B}^{0}=2: 3 ) at
a certain temperature. Assuming that ( mathbf{A} ) and ( mathrm{B} ) form an ideal solution and ratio of
mole fractions of ( A ) and ( B ) in the vapour
phase is ( 1: 3, ) then the mole fraction of ( mathbf{A} ) in the solution at the same temperature
is :
A ( cdot frac{1}{3} )
B. ( frac{2}{3} )
c. ( frac{1}{4} )
D. ( frac{3}{4} )
12
754A mixture of ethanol and ( C C l_{4} ) has ( 30 % )
( C C l_{4} ) by weight, what is mole fraction of
( boldsymbol{C C l}_{4} ) in the mixture?
A . 0.11
B. 0.89
c. 0.25
D. 0.67
12
755Which one is correct for a solution?
A. Saturated and dilute
B. Supersaturated and saturated
C. Saturated and unsaturated
D. Dilute and concentrated
12
756An ideal gas, of volume ( 189 m L ), is collected over water. The temperature is
( 27^{circ} mathrm{C}, ) and the barometric pressure is
( 756 m m H g . A t 27^{circ} C, ) the vapor
pressure of water is 27 mm ( H g )
Which of the following CORRECTLY gives the mole fraction of water vapor in the
collection vessel?
A ( cdot frac{27}{756} )
в. ( frac{27}{729} )
c. ( frac{729}{756} )
D. ( frac{729}{27} )
12
757Which of the following correctly
represent solubility of ( N_{2} ) in water (in
terms of mmole/litre) if ( N_{2} ) is bubbled
through water at ( 293 K ) at a pressure of
0.768 bar and Henry’s constant is
( mathbf{7 6 . 8} K ) at ( mathbf{2 9 3} mathbf{K} ? )
A ( cdot 10^{-5} )
5
В. ( 5.56 times 10^{-4} )
( c cdot 10^{-2} )
D. ( 4.3 times 10^{-4} )
12
758Assertion
Decrease in the vapour pressure of
water by adding 1 mol of sucrose to one jg of water is higher to that produced by
adding 1 mol of urea to the same quantity of water at the same temperature.
Reason
Molecular mass of sugar is less than
that of urea.
A. Both Assertion and Reason are correct and Reason is the correct explanation for Assertion
B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion
C. Assertion is correct but Reason is incorrect
D. Both Assertion and Reason are incorrect
12
759ml were taken. One of these beakers,
h 400 mL water whereas the beaker labelled
2. 22 Two beakers of capacity 500 mL were taken. One
labelled as “A”, was filled with 400 mL water whereas the
“B’ was filled with 400 mL of 2M solution o
h 400 mL of 2M solution of NaCl. At the same
temperature both the beakers were placed in closed
ne beakers were placed in closed containers of same
material and same capacity as shown in figure.
Water
NaCl solution
At a given temperature, which of the following statement is correct
about the vapour pressure of pure water and that of NaCl solution?
(a) Vapour pressure in container (A) is more than that in container (B)
(b) Vapour pressure in container (A) is less than that in container (B)
(c) Vapour pressure is equal in both the containers
(d) Vapour pressure in container (B) is twice the vapour pressure in container (A)
Com
12
760The amount of the solute present in the saturated solution at a particular
temperature is called its:
A. solubility
B. saturation
c. solvent concentration
D. none of the above
12
761Mlustration 2.81 2 g each of two solutes A and B (molar
mass of A is greater than that of B) are dissolved separately
in 50 g each of the same solvent. Which will show greater
elevation in the boiling point?
12
762Illustration 2.75 Calculate the vapour pressure of an
aqueous solution which contains 5 mass per per cent of urea.
The vapour pressure of pure water is 23.5 mm Hg. The molar
mass of urea is 60.
12
763Which option is inconsistent for
Raoult’s Jaw?
A. The change in heat of dilution for solution ( =0 )
B. Volume of liquid solvent + volume of liquid solute = volume of solution
C. Solute does not undergo association in solution
D. Solute undergoes dissociation in solution
12
764Illustration 2.67 What mass of non-volatile solute (urea)
needs to be dissolved in 100 g of water in order to decrease the
vapour pressure of water by 30%. What will be the molality
of solution?
12
765Example 2.19 Calculate osmotic pressure of a solution
obtained by mixing 100 mL of 3.4% solution (weight/volume)
of urea (molecular weight 60) and 100 mL of 1.6% solution
(weight/volume) of cane sugar (molecular weight 342) at
20°C.
12
766Assertion
Acetone-Carbon disulphide solution shows positive deviation from Raoult’s
law.
Reason
Acetone ( + ) Aniline solution shows
positive deviation from Raoult’s law.
A. Both Assertion and Reason are correct and Reason is the correct explanation for Assertion
B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion
c. Assertion is correct but Reason is incorrect
D. Both Assertion and Reason are incorrect
12
767( boldsymbol{F} boldsymbol{e} boldsymbol{C l}_{3} ) on reaction with ( boldsymbol{K}_{boldsymbol{4}}left[boldsymbol{F} boldsymbol{e}(boldsymbol{C} boldsymbol{N})_{boldsymbol{6}}right] )
in aqueous solution gives blue colour. These are separated by a
semipermeable membrane ( A B ) as
shown. Due to osmosis there is:
A. blue colour formation in side ( X )
B. blue colour formation in side ( Y ).
c. blue colour formation in both of the sides ( X ) and ( Y ).
D. no blue colour formation
12
768Vapour is injected at a uniform rate in a closed vessel which was initially evacuated. The pressure in the vessel
A. Increases continuously
B. Decreases continuously
c. First increases and then decreases
D. First increases and then becomes cosntant
12
769A solution containing 3.3 g of a substance in 125 g of benzene (b.pt. ( = ) ( 80^{circ} mathrm{C} ) ) boils at ( 80.66^{circ} mathrm{C} ). If ( mathrm{K}_{b} ) for
benzene is ( 3.28 mathrm{K} mathrm{kg} ) mol( ^{-1} ) the
molecular mass of the substance will
be:
A . 130.20
B. 129.20
c. 132.20
D. 131.20
12
770Ilustration 2.192 A saturated solution of Mg(OH), has
a vapour pressure of 759.5 mm at 373 K. Calculate the
solubility and Kp of Mg(OH)2. (Assume molarity equals
molality)
12
771Define mole fraction. A solution of
sucrose in water is labelled as ( 20 % ) w/w.
What would be the mole fraction of each
component in the solution?
12
772For electrolytic solution, the Van’t Hoff
factor (i) is always equals to unity.
A. True
B. False
12
773With increase in pressure
This question has multiple correct options
A. solubility of solids in liquids is unaffected
B. solubility of solids decreases
C . solubility of gases decreases in liquids
D. solubility of gases in liquids increases
12
774The ratio of the molar amounts of ( boldsymbol{H}_{2} boldsymbol{S} )
needed to precipitate the metal ions
from ( 20 mathrm{ml} ) each of ( 1 mathrm{M} C dleft(N O_{3}right)_{2} ) and
( mathbf{0 . 5} boldsymbol{M} boldsymbol{C u} boldsymbol{S O}_{4} ) is:
A . 1:
B. 2:1
( c cdot 1: 2 )
D. indefinite
12
775Two elements ( A ) and ( B ) form ideal
compounds of formula ( A B_{2} ) and ( A B_{4} ) When dissolved in ( 20.0 g ) of benzene 1.0 ( g ) of ( A B_{2} ) lowers freezing point by ( 2.3^{0} C ) whereas ( 1.0 g ) of ( A B_{4} ) lowers
freezing point by ( 1.3^{0} mathrm{C} ). The ( K_{f} ) for
benzene is ( 5.4 . ) The atomic masses of ( A )
and ( B ) are:
A .27,45
в. 42,25
c. 52,48
D. 48,52
12
776( mathrm{CoCl}_{3} cdot 3 mathrm{NH}_{3} ) does not form any
precipitate with excess ( A g N O_{3} ) solution, whereas 1 mole of
( mathrm{CoCl}_{3} cdot 5 mathrm{NH}_{3} ) gives two moles of ( mathrm{AgCl} )
with excess ( A g N O_{3} . ) The van’t Hoff factor for both the compounds
respectively are:
A. 0 and 2
B. O and 3
( c cdot 1 ) and 3
D. 1 and 2
12
777For one mole of a pure substance free energy is identical with:12
778Azeotropic mixture:
A. Boil at different temperature
B. Are mixture of solids
C. Are constant boiling mixture
D. Gaseous mixture
12
779A mixture of ethanol and propanol has
vapor pressure ( 279 mathrm{mm} ) of ( mathrm{Hg} ) at ( 300 mathrm{K} ) The mol fraction of ethanol in the
solution is 0.6 and vapour pressure of pure propanol is ( 210 mathrm{mm} ) of Hg. Vapour pressure of pure ethanol will be:
( mathbf{A} cdot 336.6 mathrm{mm} )
B . ( 325 mathrm{mm} )
c. ( 375 mathrm{mm} )
D. ( 415 mathrm{mm} )
12
780Illustration 2.195 A 0.025 m solution of monobasic acids
has a freezing point of -0.060°C. What are K, and pk of the
acid? (K. = 1.86°C)
12
781At ( 80^{0} mathrm{C}, ) the vapour pressure of pure liquid ( A ) is ( 250 m m ) of ( H g ) and that of pure liquid B is ( 1000 mathrm{mm} ) of Hg. If a
solution of ( A ) and ( B ) boils at ( 80^{circ} mathrm{C} ) and 1
atm pressure, the amount of A in the
mixture is : ( (1 a t m=760 m m H g) )
A . 50 mole percent
B. 52 mole percent
c. 32 mole percent
D. 48 mole percent
12
782Pick out the liquid-in-gas type of mixture from the following.
A. Dissolved carbon dioxide in water
B. Droplets of water in air
C. Oxygen dissolved in water
D. All of the above
12
783The values of van’t Hoff factors for
( K C l, N a C l ) and ( K_{2} S O_{4} ) respectively
are:
A. 1,1,2
B. 1,1,1
c. 2,2,3
D. 2,3,2
12
784( mathbf{0 . 1} boldsymbol{M} boldsymbol{K}_{mathbf{4}}left[boldsymbol{F} e(boldsymbol{C} boldsymbol{N})_{mathbf{6}}right] ) is 60% ionized.
What will be its van’t Hoff factor?
A . 1.4
B. 2.4
c. 3.4
D. 4.4
12
785How much ( B a C l_{2} ) would be needed to
make 250 ml of a solution having the
same concentration of ( C l^{-} ) as one
containing ( 3.78 g N a C l ) per 100 ml?
( (B a=137) )
A. ( 22.4 g )
в. ( 16.8 g )
c. ( 67.2 g )
D. 33.6 ( g )
12
786Heptane and octane form an ideal
solution. At ( 373 K ), the vapour
pressures of the two liquid components are ( 105.2 k P a ) and ( 46.8 k P a )
respectively. What will be the vapour pressure of a mixture of ( 26.0 mathrm{g} ) of
heptane and ( 35 g ) of octane?
12
787Q. 9 What is the mass per cent of carbon in carbon dioxide?
(a) 0.034% (b) 27.27% (c) 3.4%
(d) 28.7%
12
788At ( 80^{circ} mathrm{C}, ) the vapour pressure of pure
liquid ( mathbf{A}^{prime} ) is ( mathbf{5} mathbf{2 0} mathbf{m m} mathbf{H} boldsymbol{g} ) and that of
pure liquid B’ is 1000 mm ( H g ). If a
mixture solution of ( mathbf{A}^{prime} ) and ( mathbf{B}^{prime} ) boils at
( 80^{circ} mathrm{C} ) and 1 atm pressure, the amount of A’ in the mixture is:
( [1 a t m=760 m m H g] )
A. 48 mol%
B . 50 mol%
c. 52 mol%
D. 34 mol%
12
789The correct relation between elevation
of boiling point and molar mass of
solute is:
A ( ldots_{M_{2}}=frac{K_{b} times W_{2}}{Delta T_{b} times W_{1}} )
В. ( M_{2}=frac{K_{b} times W_{1}}{Delta T_{b} times W_{2}} )
( ^{mathrm{C}} cdot_{M_{2}}=frac{Delta T_{b} times K_{b}}{W_{1} times W_{2}} )
D. ( M_{2}=frac{Delta T_{b} times W_{1}}{K_{b} times W_{2}} )
12
790Q. 3 What will be the molarity of a solution, which contains 5.85 g of NaCl(s
per 500 mL?
(a) 4 mol L-1 (b) 20 mol L-1 (c) 0.2 mol L-1 (d) 2 mol L-1
12
791Compute the molar solubility of water
that is saturated with air.
( left[text { Given: } k=0.00105 mathrm{M} / mathrm{atm}, P_{N e} text { in air }=right. )
( 0.0341 mathrm{atm}] )
A ( .2 .56 times 10^{-2} M )
в. ( 3.58 times 10^{-5} M )
c. ( 4.44 times 10^{-6} M )
D. ( 2.78 times 10^{-4} M )
12
792State True or False.
For a non-ideal solution, ( Delta_{m i x} V ) and
( Delta_{m i x} H ) are zero.
A . True
B. False
12
793Estimate the lowering of vapour pressure due to the solute (glucose) in
a ( 1.0 mathrm{M} ) aqueous solution at ( 100^{circ} mathrm{C} )
A . 10 torr
B. 18 torr
c. 13.45 torr
D. 24 torr
12
794At ( 400^{circ} mathrm{C}, ) the vapour pressure of water
is 55.3 mm ( H g ). Calculate the vapour
pressure at the same temperature over
( 10 % ) aqueous solution of urea
( left[boldsymbol{C O}left(boldsymbol{N} boldsymbol{H}_{2}right)_{2}right] ? )
12
795When 3 L of ( 0.5 ~ M ) NaCl is mixed with
( 9 mathrm{L} ) of ( 0.2777 M N a C l, ) determine the
concentration of the final solution, assuming that volumes are additive?
A. 0.33 M .
В. 0.39 М
c. ( 0.5777 M )
D. ( 0.7777 M )
E. None of the above
12
796When an azeotropic mixture is distilled,
its composition remains unchanged If true enter ( 1, ) if false enter 0
12
797Question 41. Determine the osmotic pressure of a solution prepared by
dissolving 25 mg of K2SO4 in 2 L of water at 25°C, assuming that it is
completely dissociated.
Apply van’t Hoff equation, n = iCRT, where, i = Number of ions produced
by K2SO4).
12
798Increase of temperature of an aqueous
solution will cause:
A. decrease in molality of the solution
B. decrease in molarity of the solution
c. decrease in mole fraction of the solution
D. decrease in percentage (w/w) of the solution
12
7993. From a measurement of the freezing point depression of
benzene, the molecular weight of acetic acid in a benzene
solution was determined to be 100. The percentage
association of acetic acid is
a. 79% b. 93% c. 80%
d. 100%
12
800Illustration 2.59 Two liquids A and B on mixing produce
a warm solution. Which type of deviation from Raoult’s law
does it show?
12
801Positive deviation from ideal behaviour
takes place because of :
A . molecular interaction between atoms and ( frac{P V}{n R T}>1 )
B. molecular interaction between atoms and ( frac{P V}{n R T}1 )
D tinite size of atoms and ( frac{P V}{n R T}<1 )
12
802Dilute ( 20.8 mathrm{mL} ) of ( 6.0 mathrm{M} mathrm{H}_{2} mathrm{SO}_{4} ) to a
volume of 1 L. The concentration of the
resultant ( boldsymbol{H}_{2} boldsymbol{S} boldsymbol{O}_{4} ) solution is ( boldsymbol{2 5} boldsymbol{y} times )
( 10^{-3} M, ) then ( y ) is
12
803( 1.5 mathrm{g} ) of a monobasic acid, when dissolved in 150 g of water, lowers the freezing point by ( 0.165^{circ} mathrm{C} .0 .5 mathrm{g} ) of the same acid when titrated, after
dissolution in water, requires ( 37.5 mathrm{ml} ) of N/10 alkali. Calculate the degree of
dissociation of the acid ( ?left(K_{f} text { for water }=right. ) ( left.1.86^{circ} mathrm{C} mathrm{mol}^{-1}right) )
A . ( 11.34 % )
в. ( 34.64 % )
c. ( 65.36 % )
D. ( 89.64 % )
12
804How many grams of ( N a O H ) are needed
to make ( 100 g ) of a ( 5 % ) solution?
( A cdot 2 )
B. 5
c. 20
D. 40
E . 95
12
805Illustration 2.49 Two liquids A and B form an ideal
solution at temperature T. When the total vapour pressure
above the solution is 600 torr, the amount fraction of A in the
vapour phase is 0.40 and in the liquid phase is 0.60. What are
the vapour pressures of pure A and pure B at temperature T?
11
12
806The azeotropic mixture of water and HCl
boils at ( 108.5^{circ} mathrm{C} ). When this mixture is
distilled, it is possible to obtain
A. pure ( H C l )
B. pure water
c. neither pure HCI nor pure water
D. both pure HCl and pure water
12
807Ilustration 2.120 What mass of sugar C, H,0,(M,=342)
must be dissolved in 4.0 kg of 1,0 to yield a solution that
will freeze at -3.72°C. (Take Kg = 1.86°C m-1)
12
808e. 17 Value of Henry’s constant KH ………..
(a) increases with increase in temperature
(b) decreases with increase in temperature
(c) remains constant
(d) first increases then decreases
12
809The relationship between the values of osmotic pressure of ( 0.1 mathrm{M} ) solutions of ( boldsymbol{K} boldsymbol{N} boldsymbol{O}_{3}left(boldsymbol{P}_{1}right) ) and ( boldsymbol{C} boldsymbol{H}_{3} boldsymbol{C O O H}left(boldsymbol{P}_{2}right) ) is:
A ( cdot P_{1}>P_{2} )
в. ( P_{2}>P_{1} )
( mathrm{c} cdot P_{1}=P_{2} )
D. ( frac{P_{1}}{P_{1}+P_{2}}=frac{P_{2}}{P_{1}+2 P_{2}} )
12
810What is Raoult’s Law?
Derive Raoult’s Law for solution which
contain non-volatile solute.
12
811Illustration 2.186 Calculate the amount of NaCl which must
be added to 100 g water so that the freezing point, depressed
by 2 K. For water K = 1.86 K kg mol-1.
12
812( mathbf{A} )
1.00 molal aqueous solution of trichloroacetic acid ( left(C C l_{3} C O O Hright) ) is heated to its boiling point. The solution
has the boiling point of ( 100.18^{circ} mathrm{C} ) Determine the van’t Hoff factor for
trichloroacetic acid. ( left(K_{b} text { for water }=right. )
( 0.512 mathrm{K} mathrm{kg} mathrm{mol}^{-1} ) )
12
813Osmotic pressure of a solution is:
This question has multiple correct options
A. directly proportional to the molar concentration of the solution
B. inversely proportional to the molecular weight of the solute
C. inversely proportional to the temperature
D. directly proportional to the volume of the solution
12
814What concentration of nitrogen should
be present in a glass of water at room
temperature? Assume a temperature of
( 25^{circ} mathrm{C}, ) a total pressure of 1 atmosphere
and mole fraction of nitrogen in air of ( 0.78 .left(K_{H} text { for nitrogen }=8.42 times 10^{-7}right. )
( mathrm{M} / mathrm{mm} mathrm{Hg} )
12
815Illustration 2.208 The vapour pressure of benzene at 30°C is
164.88 mm of Hg. In 3 mol of benzene, when 6 g of acetic acid
was dissolved, the vapour pressure of the solution became
162.04 mm of Hg. Calculate
a. Van’t Hoff factor
b. The degree of association of acetic acid in benzene at
30°C
12
816The percentage of ( F e(I I I) ) present in
iron ore ( F e_{0} .9301 .00 ) is ( (F e=56) )
A . 94
B. 6
c. 21.5
D. 15
12
817When ( H g I_{2} ) is added to aqueous
solution of ( mathrm{KI} ), why there is an increase
in vapour pressure of solution?
12
818Explain with a suitable diagram and
appropriate examples why some nonideal solutions show positive deviation from ideal behaviour.
12
8194. 0.6 g of a solute is dissolved in 0.1 L of a solvent which
develops an osmotic pressure of 1.23 atm at 27°C. The
molecular weight of the solute is
a. 149.5 g mol-
b. 120.0 g mol-1
c. 430.0 g mol-1
d. None of these
12
820Which one will have highest boiling
point, if 1 mole of each of the following substances was discovered in 1,000
grams of water?
A. Nacı
в. кс।
c. ( C a C l_{2} )
D. ( C_{6} H_{10} O_{5} )
E ( cdot C_{12} H_{22} O_{11} )
12
821What will be the vapour pressure of a
solution containing 5 moles of sucrose
( left(C_{12} H_{22} O_{11}right) ) in ( 1 k g ) of water, if the vapour pressure of pure water is ( 4.57 m m ) of ( H g ?[C=12, H=1, O= )
( mathbf{1 6}] )
12
822If liquids ( A ) and ( B ) form an ideal solution,
then :
A. the entropy of mixing will be zero
B. the Gibbs free energy of mixing will be zero
C. the Gibbs free energy as well as the entropy of mixing both will be zero
D. the enthalpy of mixing will be zero
12
823Pressure over ideal binary liquid
mixture containing 10 moles each of liquid ( A ) and ( B ) is gradually decreased
isothermally. If ( P_{A}^{circ}=200 m m H g ) and
( P_{B}^{circ}=100 m m H g, ) the pressure at
which half of the liquid is converted into
vapour is:
A. ( 150 mathrm{mm} ) Hg
в. ( 166.5 mathrm{mm} ) ну
c. ( 133 mathrm{mm} ) нg
D. 141.4 mm нg
12
8245. The Van’t Hoff factor for a 0.1 MALL(SO2)2 solution is
4.20. The degree of dissociation is
a. 80% b. 90% c. 78% d. 83%
12
825A solution containing ( 62 g ) ethyl glycol
in ( 250 g ) water is cooled to ( -10^{circ} mathrm{C} ). If ( K_{f} )
for water is ( 1.86 K k g m o l^{-1}, ) the
amount of water ( (text { in } g ) ) separated as ice is:
A . 32
B. 48
( c cdot 16 )
D. 64
12
826Assertion
The solubility of Ammonium chloride increases with increase in temperature
Reason In case of substances whose solubility increases with increase in temperature is due to the dissolution process being endothermic.
A. Both Assertion and Reason are correct and Reason is the correct explanation for Assertion
B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion
c. Assertion is correct but Reason is incorrect
D. Both Assertion and Reason are incorrect
12
827Assertion
Salt dissolved in water lowers the
freezing point.
Reason
The change in freezing point is given by:
( Delta boldsymbol{T}_{boldsymbol{f}}=boldsymbol{i} boldsymbol{K}_{boldsymbol{f}} boldsymbol{m} )
A. Both Assertion and Reason are correct and Reason is
the correct explanation for Assertion
B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion
C. Assertion is correct but Reason is incorrect
D. Both Assertion and Reason are incorrect
12
828Illustration 2.190 A certain substance A tetramerizes in
water to the extent of 80%. A solution of 2.5 g of A in 100 g
of water lowers the freezing point by 0.3°C. The molar mass
of A is
a. 120 b. 61 c. 60
d. 62
12
829Calculate the amount of ( C a C l_{2} ) (van’t
Hoff factor ( i=2.47 ) ) dissolved in ( 2.5 L )
solution so that its osmotic pressure at
( 300 K ) is 0.75 atmosphere
Given: Molar mass of ( C a C l_{2} ) is
( 111 g cdot m o l^{-1} )
( boldsymbol{R}=mathbf{0 . 0 8 2} boldsymbol{L} . boldsymbol{a t m} . boldsymbol{K}^{-1} boldsymbol{m o l}^{-1} )
12
830Van’t Hoff factor, when benzoic acid is
dissolved in benzene, will be:
A . 2
B.
( c .0 .5 )
D. 1.5
12
831State True or False.
( C_{2} H_{5} O H ) and cyclohexane mixture shows positive deviation from Raoult’s law.
A. True
B. False
12
832The vapour pressure of two pure liquids ( A ) and ( B ) which from an ideal solution
are 500 and 800 torr respectively at
( 300 K . ) A liquid solution ( A ) and ( B ) for
which the mole fraction of ( A ) is 0.60 is
contained in a cylinder closed by a piston on which the pressure can be
varied. What will be the pressure when 1 mol of the mixture has been vaporized?
12
833Question 17. The vapour pressure of water is 12.3 kPa at 300 K.
Calculate vapour pressure of 1 molal solution of a non-volatile solute in it.
(1) In order to calculate vapour pressure, mole fraction is required but
we have molality. So, convert molality into mole fraction by using
following steps.
(a) Find the moles of solute and mass of solvent from molality.
(b) Find of moles of solvent, i.e., water by dividing its mass by molar mass.
(c) Find mole fraction of solute, Xo = —
o At no
(ii) Find mole fraction of solvent xa as XA + X8 = 1
(iii) Finally calculate the vapour pressure by using Raolut’s law, p = pºx.
12
834Aquatic species are more comfortable
in cold water because of:
A. as the temperature decreases, the solubility of dissolved oxygen increases
B. as the temperature increases, the solubility of dissolved oxygen increases.
c. as the temperature increases, the solubility of dissolved oxygen decreases
D. none of the above
12
835Concentrated hydrochloric acid is ( 36.5 % ) by weight. What is the molality of the
solution?
A . 1.575 molal
B. 15.75 molall
c. 157.5 molal
D. 1575 molal
12
836A liquid mixture of benzene ( (B) ) and
toluene ( (T) ) contains 1 mole each of ( B )
and ( T )
( boldsymbol{P}_{boldsymbol{T}}^{boldsymbol{o}}=mathbf{4 . 2 7 4} boldsymbol{k} boldsymbol{N} boldsymbol{m}^{-2} ) and ( boldsymbol{P}_{boldsymbol{B}}^{boldsymbol{o}}= )
( mathbf{1 3 . 7 3 4} mathbf{k} mathbf{N m}^{-mathbf{2}} )
If the pressure is reduced further, pressure ( left(text { in } k N m^{-2}right) ) (write only integer part) at which the last trace of liquid does disappear
is
12
837The ratio of the value of any colligative
property for ( B a C l_{2} ) solution to that for
urea solution under similar condition
is:
A .2
B. 3
( c )
( D )
12
838What is the density (in ( g m / )lit ) of wet air with ( 75 % ) relative humidity at 1 at
and ( 300 K ? ) Given : vapour pressure of
( H_{2} O ) is 30 torr and average molar
mass of air is ( 29 g / ) mol.
Write as the nearest integer:
12
839The melting point of ice is
(a) 273K
c) 300K
(b) 373K
(d) 298 K
12
840toppr
acids pictured, which of the following
would be the LEAST soluble in water?
A. Histidine
B. Lysine
C. Alanine
D. Cysteine
12
841Derive the relation between elevation of
boiling point and molar mass of solute.
12
842Elevation in boiling point was ( 0.52^{circ} mathrm{C} ) when 6 g of a compound ( X ) was dissolved in 100 g of water. Molecular mass of the compound M in ( g ) mol ( ^{-1} ) is:
( K_{b} ) for water is ( 0.52 mathrm{Km}^{-1} ).)
A . 120
B. 60
( c cdot 600 )
D. 180
12
843A ( 10 % ) solution (by mass) of sucrose in water has a freezing point of ( 269.15 K )
Calculate the freezing point of ( 10 % ) glucose in water if the freezing point of
pure water is ( 273.15 K )
(Given : molar mass of sucrose ( = )
( 342 g ) mol ( ^{-} ?, ) Molar mass of glucose ( = )
( left.180 g m o l^{-1}right) )
A. 275. 53 K
B. 265. 53 K
c. २७१. 32 ( mathrm{K} )
D. 282.43 K
12
844When the concentration of ( boldsymbol{K}^{+} ) across a
cell membrane drops from ( 0.01 M ) to
( 0.001 M, ) the potential difference across the membrane is:
A . ( 0.0 V )
B. ( 0.0059 V )
c. ( 0.059 V )
D. ( 0.59 V )
12
845Illustration 2.143 What is reverse osmosis?12
84618g glucose and 6 g urea are dissolved
in 1 litre aqueous solution at ( 27^{circ} C . ) The
osmotic pressure of the solution will be
( mathbf{A} cdot 3.826 mathrm{atm} )
B. 4.926 atm
c. 2.92 atm
D. 9.42 atm
12
847If benzoic acid (mol. mass = 122) is associated into double molecules when
dissolved in benzene and the osmotic
pressure of a solution of 5 g of benzoic acid in ( 100 mathrm{mL} ) benzene is 5.73 atm at
( 10^{circ} mathrm{C}, ) what is the percentage
association of benzoic acid?
( mathbf{A} cdot 60 % )
B. ( 70 % )
( c .80 % )
D. ( 85 % )
12
848The molal lowering of vapour pressure( in cm to nearest integer) for ( boldsymbol{H}_{2} boldsymbol{O} ) at
( 100^{circ} mathrm{C} ) is
12
849If the concentration of water vapour in
the air is ( 1 % ) and the total atmospheric pressure equals 1 atm, then the partial
pressure of water vapour is?
A. ( 0.1 mathrm{atm} )
В. ( 1 mathrm{mm} ) нв
( mathbf{c} .7 .6 mathrm{mm} mathrm{Hg} )
D. 100 atm
12
850Assertion
The molecules of the dissolved gas
present in a liquid gain kinetic energy as temperature is raised.
Reason
Gases tends to be more soluble in
liquids as the temperature is raised.
A. Both Assertion and Reason are correct and Reason is the correct explanation for Assertion
B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion
c. Assertion is correct but Reason is incorrect
D. Assertion is incorrect but Reason is correct
12
851If relative decrease in ( mathrm{V} . mathrm{P} ) is 0.4 for ( mathrm{a} )
solution containing 1 mol ( N a C l ) in 3
mol of ( mathrm{H}_{2} mathrm{O} ). Calculate ( % ) ionization of
NaCl.
A . 100
B. 95
c. 90
D. 85
12
8523. At 27°C. the vapour pressure of an ideal solution
containing 1 mole of A and 1 mole of B is 500 mm of Hg.
At the same temperature, if 2 mol of B is added to this
solution the vapour pressure of solution increases by 50
mm of Hg. The vapour pressure of A and B in their pure
states is respectively,
a. 600 mm, 400 mm b. 400 mm, 600 mm
c. 300 mm, 700 mm
d. 200 mm, 800 mm
12
853A volume of ( 6 L H_{2} O ) is placed in a
closed evacuated room of volume ( 827 L )
at the temperature ( 300 mathrm{K} ). The density of liquid water at ( 300 mathrm{K} ) is ( 1.0 mathrm{g} / mathrm{ml} ). The
vapour pressure of water at ( 300 mathrm{K} ) is
( 22.8 mathrm{mm} ) Hg. Neglect the change in volume of liquid water by vaporization.
12
854For a non-volatile solute:
A. vapour pressure of solution is more than vapour pressure of solvent
B. vapour pressure of solvent is zero
C. vapour pressure of solute is zero
D. all of the above
12
855Ilustration 2.89 A solution containing 0.2563 g of
naphthalene (molecular mass = 128) in 50 g of carbon
tetrachloride yields a boiling point elevation of 0.201°C while
a solution of 0.6216 g of an unknown solute in the same mass
of the solvent gives a boiling point elevation of 0.647°С. Find
the molecular mass of unknown solute.
12
856For a dilute solution, mole fraction of solute is given as ( (n= ) no. of moles of solute and ( N=text { no. of moles of solvent }) )
A ( cdot frac{n}{N} )
в. ( frac{N}{n} )
c. ( frac{N}{n+N} )
D. Both B and C
12
857Illustration 2.167 A 5% solution of cane sugar is isotonic
with 0.877% solution of urea. Calculate the molecular mass
of urea if the molecular mass of cane sugar is 342.
12
858In the solvation of ( N a C l ) in water, which
of the following occur?
A. Hydrogen atom interacts with ( C l^{-} ) atom
B. Oxygen atom interacts with ( N a^{+} ) atom
c. Both ( A ) and ( B )
D. None of these
12
859Ulustration 2.176 What will be the osmotic pressure of
0.1 M monobasic acid its pH is 2 at 25°C?
12
860Illustration 2.193 The freezing point of an aqueous solution
of KCN containing 0.1892 mol kg-1 was found to be -0.704°C.
On adding 0.095 mol of Hg(CN), the freezing point of the
solution was found to be -0.530°C. If the complex formation
takes place according to the following equation:
Hg(CN)2 + nKCN K,[Hg(CN)n+2]
What is the formula of the complex? [K, (H2O) is 1.86 K
kg mol-1
12
861The relationship between the value of
Osmotic pressure ( (pi) ) of the solution
obtained by dissolving ( 6 g . mathrm{L}^{-1} ) of acetic
( operatorname{acid}left(pi_{1}right) ) and 7.45 g.L ( ^{-1} ) of ( mathrm{KCl}left(pi_{2}right) ) is :
A ( cdot pi_{1}pi_{2} )
( mathbf{c} cdot pi_{1}=pi_{2} )
D. ( frac{pi_{1}}{pi_{1}+pi_{2}}=frac{pi_{2}}{pi_{1}+pi_{2}} )
12
862i. ( 0.1 M ) ethanol
ii. ( mathbf{0 . 1} boldsymbol{M} boldsymbol{B} boldsymbol{a}_{3}left(boldsymbol{P} boldsymbol{O}_{4}right)_{3} )
¡¡ii.0.1 ( M N a_{2} S O_{4} )
Increasing order of freezing point
A ( cdot(i i)<(i i i)<(i) )
B. ( (i i i)<(i i)<(i) )
c. ( (i)<(i i)<(i i i) )
D. ( (i i)<(i)<(i i i) )
12
863The azeotropic mixture of water and
( H C l ) boils at ( 108.5^{0} C . ) This solution is:
A . ideal
B. non-ideal with positive deviation
c. non-ideal with negative deviation
D. cannot be predicated
12
864( 252 mathrm{gm} ) of oxalic acid with molecular
formula ( C_{2} H_{2} O_{4} cdot 2 H_{2} O ) dissolve in
water to form ( 250 mathrm{ml} ). of the solution. Its
molarity will be:
A . 16 м
B. 8 M
c. 32 м
D. 24 M
12
865The maximum amount of solute that will
saturate ( 100 mathrm{g} ) of solvent at that temperature is known as:
A. solubility
B. soluble
c. solution
D. none of the above
12
866A storage battery contains a solution of
( H_{2} S O_{4}, 38 % ) by mass. At this
concentration, van’t Hoff factor is 2.50
The temperature at which battery contents freeze will be:
( left(boldsymbol{K}_{f}=mathbf{1 . 8 6} boldsymbol{K} boldsymbol{m o l}^{-1} boldsymbol{k g}right) )
A ( .-29.08^{circ} mathrm{C} )
B . ( -25.18^{circ} mathrm{C} )
c. ( -17.25^{circ} mathrm{C} )
D. none of these
12
867If ( 200 mathrm{ml} ) solution of ( 0.5 mathrm{M} ) NaOH is
diluted to ( 800 mathrm{ml} ) then find molarity of
resultant solution.
A. 0.250 М
в. 0.125 м
c. 0.225 м
D. ( 0.4 mathrm{M} )
12
868A solution is prepared by dissolving ( 5.64 mathrm{g} ) of glucose in ( 60 mathrm{g} ) of water. Calculate the molality of the solution.
A. ( 0.2611 mathrm{m} )
B. 1.21 ( mathrm{m} )
( c cdot 1.044 mathrm{m} )
D. 0.522 ( mathrm{m} )
12
869Calculate the mole fraction of Benzene
( left(C_{6} H_{6}right) ) in a solution containing ( 30 % ) by ( operatorname{mass} operatorname{in} H C l .(C l=35.5) )
12
870toppr
solution?
( A )
3
( c )
( D )
12
871Benzoic acid (molecular weight ( =122 ) g
mol ( ^{-1} ) ) associates to form dimer when
dissolved in benzene and the osmotic
pressure of a solution of 5 g of benzoic acid in ( 100 mathrm{ml} ) benzene is 5.73 atm at
( 10^{circ} mathrm{C} . ) What is the percentage
association of benzoic acid?
A . ( 8 % )
B. ( 80 % )
c. ( 40 % )
D. ( 20 % )
12
872Calculate the concentration of nitric
acid in moles per litre in a sample which has a density, ( 1.41 g m L^{-1} ) and
the mass per cent of nitric acid in it
being ( 69 % )
12
873Negative deviation from Raoult’s law is observed in which one of the following binary liquid mixtures?
A. Ethanol and acetone
B. Benzene and toluene
c. Acetone and chloroform
D. Chloroethane and bromoethane
12
874When a solution of ( C H C l_{3} ) and acetone is formed, the solution is non-ideal with
deviation from Raoult’s
law.The vapour pressure of such a solution will be
corresponding ideal solution.
A. Positive, more
B. Negative, more
c. Negative ,less
D. Positive , less
12
875Vapour pressure of water is ( 360 mathrm{mm} mathrm{Hg} ) how much urea should be added to 200
mL water to reduce its vapour pressure by ( 0.5 % ?(text { Molecular wt. of urea }=60) )
A . ( 2.52 g )
в. 3.33 g
c. ( 3.96 g )
D. None of these
12
876Determine the degree of association (polymerisation) for the reaction in
aqueous solution ( 6 H C H O rightleftharpoons )
( boldsymbol{C}_{boldsymbol{6}} boldsymbol{H}_{mathbf{1 2}} boldsymbol{O}_{boldsymbol{6}} )
If observed(mean) molar mass of
( H C H O ) and ( C_{6} H_{12} O_{6} ) is 150
A . 0.50
B. 0.833
c. 0.90
D. 0.96
12
877( 10 mathrm{L} ) of hard water required ( 0.56 mathrm{g} ) of lime (CaO) for removing hardness. Hence, the temporary hardness in ppm
(part per million) of ( C a C O_{3} ) is :
A. 100
в. 200
c. 10
D. 20
12
878Molarity of a liquid ( H_{2} S O_{4} ) with density ( 1.2 g / c c ) is
A . 36.
B. 12.24
c. 1.224
D. 5.0
12
879What should be the density of an aqueous solution of urea
( (text {molarmass}=mathbf{6 0} boldsymbol{g} / text { mol}) ) such that
the molarity and molarity of the solution become equal?
A. ( 16.0 g / m l )
в. ( 1.6 g / m l )
c. ( 1.06 g / m l )
D. ( 1.16 g / m l )
12
880Solutions distilled without change in
composition at a temperature are called
A. Amorphous
B. Azeotropic mixture
c. Ideal solution
D. Super saturated solution
12
881What is the composition of last droplet of liquid remaining in equilibrium with
vapour?
A ( . x_{A}=0.6 ; x_{B}=0.4 )
B . ( x_{A}=0.5 ; x_{B}=0.5 )
c. ( x_{A}=0.7 ; x_{B}=0.3 )
D. ( x_{A}=0.3 ; x_{B}=0.7 )
12
882An aqueous solution of methanol in
water has vapour pressure:
A. less than that of water
B. equal to that of water
c. more than that of water
D. equal to that of methano
12
883The mole fraction of ( A ) in ( 10 %(w / w) ) aq. solution of glucose is:
A . 0.18
B. 0.011
( c .0 . )
D. 0.017
12
884Ethylene glycol is used as an antifreeze in a cold climate. Mass of ethylene
glycol which should be added to 4 kg of water to prevent it from freezing at
( -6^{o} C ) will be :
( left(K_{f} text { for water }=1.86 mathrm{K} mathrm{kg} / mathrm{mol} ) and molar right. mass of ethylene glycol ( =62 ) g mol ( ^{-1} ) )
A . ( 304.6 mathrm{g} )
в. ( 800 mathrm{g} )
c. 204.3 g
D. ( 400.00 mathrm{g} )
12
885The boiling point ( T_{b}^{*} ) of a solvent becomes ( T_{b} ) on addition of ( X_{1} ) mole
fraction of solute. Heat of vaporisation
of solvent is ( Delta boldsymbol{H}_{boldsymbol{v} boldsymbol{a} boldsymbol{p}} . ) The relation
between elevation in b.pt. ( Delta T_{b}left(=T_{b}-right. )
( left.T_{B}^{*}right) ) can be given by:
( frac{Delta T_{b}}{T_{b} times T_{b}^{*}}=-frac{R I n X_{1}}{Delta H_{v a p}} )
A graph plotted between ( log _{10} X_{1} ) vs. ( frac{1}{T_{b}} ) gives:
A.
[
text { straight line with slope } frac{R}{Delta H_{v a p}} text { and intercept } T_{b}^{*}
]
B. a straight line with slope ( frac{2.303 R}{Delta H_{v a p}} ) and intercept ( frac{1}{T_{b}} )
c. a straight line with slope ( frac{Delta H_{v a p}}{2.303 R} ) and intercept ( frac{1}{T_{b}^{*} times 2.303} )
D. a straight line with slope ( frac{Delta H_{v a p}}{2.303 R} ) and intercept ( -frac{Delta H_{v a p}}{2.303 R T_{b}^{*}} )
12
886For a gas in equilibrium with a liquid, the ratio of the concentration of the gas
in the solution phase to that in the gaseous phase is constant at constant
temperature, only if molecules undergo:
A. ionisation
B. dissociation
c. isolation
D. reaction with solvent
12
887A 1.00 molal aqueous solution of
trichloroacetic acid ( left(C C l_{3} C O O Hright) ) is
heated to its boiling point. The solution
has the boiling point of ( 100.8^{circ} mathrm{C} ).
Determine the van ‘t Hoff factor for
trichloroacetic acid. ( left(K_{b} text { for water } 0.512 mathrm{K}right. )
( left.operatorname{kg} M o l^{-1}right) )
Define the following terms:
(i) Mole fraction
(ii) Isotonic solutions
(iii) Van ‘t Hoff factor
(iv) Ideal solution
12
888The difference in height of the mercury column in two arms of a U tube
manometer in arrangement-lis ( boldsymbol{h}_{mathbf{1}}= )
( 660 mathrm{mm} . ) In another arrangement -II at the same temperature, 222 gm of
( mathrm{CaCl}_{2} ) is dissolved in ( 324 mathrm{gm} ) of water and the difference in height of mercury
column in two arms is found to be ( h_{2}= )
( 680 mathrm{mm} . ) If the value of degree of
dissociation for ( C a C l_{2} ) in arrangement
-II is ( alpha, ) then the value of ( 64 alpha ) is:
[Atmospheric pressure ( =1 text { atm }] )
( : mathbb{1} )
12
889Mole fraction of ethanol ( left(C_{2} H_{5} O Hright) ) in
ethanol-water system is ( 0.25 . ) Thus, it has:
This question has multiple correct options
A. ( 25 % ) ethanol by weight of solution
B. ( 75 % ) water by weight of solution
c. ( 46 % ) ethanol by weight of solution
D. 54% water by weight of solution
12
890Which of the following plots represents an ideal binary mixture?
( mathbf{A} cdot ) Plot of ( P_{text {total}} v / s 1 / X ) is linear ( left(X_{B}= ) mole fraction of right. ‘B’ in liquid phase).
B. Plot of ( P_{text {total}} v / s Y_{A} ) is linear ( left(Y_{B}= ) mole fraction of ‘A’ right. in vapour phase)
C ef of ( frac{1}{P_{text {total}}} v / s Y_{A} ) is linear
D. plot of ( frac{1}{P_{text {total}}} v / s Y_{B} ) is non linear
12
891Statement – I: The mixing of two completely miscible liquid. A and B showing positive deviation from Raoult’s law is followed by an
absorption of heat Statement – ll: The A- B molecular
interaction forces are stronger than the
A-A or B-B molecular interaction forces.
A. Statement-lis true, Statement- – 2 is true; Statement 2 is a correct explanation for Statement- –
B. Statement-1 is true, Statement – 2 is true; Statement 2 is not a correct explanation for Statement – –
c. statement-lis true, Statement- – 2 is false
D. Statement-lis false, Statement- – 2 is true
12
892room temperature solution feels cool to
Q. 2 On dissolving sugar in water at room temperature solutio
touch. Under which of the following cases dissolution of sugar
most rapid?
(a) Sugar crystals in cold water
(b) Sugar crystals in hot water
(c) Powdered sugar in cold water (d) Powdered sugar in hot water
Thinking Process
Use the concept of solubility and effect of temperature on solubility to answer this
question
12
893Two liquids ( H N O_{3}(A) ) and water ( (B) )
form a maximum boiling azeotrope
when mixed in the ratio of ( 68 % ) and ( 32 % )
respectively. It means:
A. A-B interactions are stronger than ( A ) -A and B-B interactions
B. A-B interactions are weaker than A-A and B-B interactions
c. vapour pressure of solution is more than the pure components
D. vapour pressure of solution is less since only one component vaporises
12
894r at
Question 39. The air is a mixture of a number of gase
air is a mixture of a number of gases. The major
components are oxygen and nitrogen with a
are oxygen and nitrogen with approximate proportion of
20% is to 79% by volume at 298 K. The water is in equilibrium
a pressure of 10 atm. At 298 K if the Henry’s law constants for oxygen
and nitrogen at 298 K are 3.30 x107 mm and 6.51 x10 mm respecuve,
calculate the composition of these gases in water.
First find the partial pressure of oxygen and nitrogen from Henry’s law,
p= K X and the find their mole fraction (again applying the
Henry’s law).
12
895Hlustration 2.212 Under what conditions Van’t Hoff factor
(i) is
(a) equal to unity, (b) less than 1, and (c) greater than 1.
12
896In amalgam of mercury with sodium, solvent is;
A. mercury
B. sodium
c. amalgam
D. none of these
12
897A solution of ( 50 % ) of ( A ) and ( 50 % ) of ( B ) on
distillation results into
A. Seperation of an azeotropic mixture and pure ( A )
B. Seperation of an azeotropic mixture and pure B.
C. Seperation of both pure ( A ) and pure ( B )
D. None.
12
898A solution is prepared by dissolving 9.8
( g ) of ( H_{2} S O_{4} ) in 54 g of water. What is the
mole fraction of ( boldsymbol{H}_{2} boldsymbol{S O}_{4} ? )
A. 0.03
B. 0.04
c. 0.01
D. 0.02
12
899The Van’t Hoff factor of ( N a C l ) assuming ( 100 % ) dissociation is :
A . ( 1 / 2 )
B . 2
c. 1
D. 3
12
900If equal volume of ( B a C l_{2} ) and ( N a F ) solutions are mixed, which of these
combination will give a precipitate? ( boldsymbol{K}_{s p} ) of ( boldsymbol{B a} boldsymbol{F}_{2}=mathbf{1 . 7} times mathbf{1 0}^{-mathbf{7}} )
12
901Calculate Vant Hoff factor for ( 0.2 m )
aqueous solution of KCl which freezes
at ( -mathbf{0 . 6 8 0}^{circ} mathbf{C} .left(boldsymbol{K}_{boldsymbol{f}}=mathbf{1 . 8 6} mathbf{K} mathbf{k g} boldsymbol{m o l}^{-mathbf{1}} mathbf{)}right. )
A . 3.72
в. 1.83
( c .6 .8 )
D. 1.86
12
902What is the relative lowering in vapour pressure of ( 10 % ) aqueous solution of glucose :
A ( .1 / 10 )
B. 1/90
c. ( 1 / 20 )
D. 1/30
12
903VLASOV UUTUUUUUUUUUU
Illustration 2.60
. . .
What type of liquids form ideal solutions?
1 colonitione
12
904Fizziness appears on opening a bottle of
cold drink.
12
905A mixture has 18 g water and 414 g ethanol. The mole fraction of water in
mixture is (assume ideal behaviour of
the mixture):
A . ( 0 . )
B. 0.4
( c . ) о.
D. 0.9
12
906A solution containing
0.1 mole of naphthalene and 0.9 mole of benzene is cooled out until some benzene freezes
out. The solution is then decanted off
from the solid and warmed up to ( 353 mathrm{K} ) where its vapour pressure was found to
be 670 torr. The freezing point and boiling point of benzene are ( 278.5 mathrm{K} ) and
( 353 mathrm{K} ) respectively and its enthalpy of fusion is ( 10.67 mathrm{kJ} ) mol ( ^{-1} ). Calculate the
depression in freezing point for original solution to the nearest integer. Assume ideal behaviour
12
907( 0.6 mathrm{g} ) of an organic compound when dissolved in 21.7 g water freezes at 272.187 K. The molar mass of the
organic compound is close to:
( left(K_{f} text { of water is } 1.86 ) deg/molality; right. freezing point is ( 273 mathrm{K} ) )
A. ( 61 mathrm{g} ) mol ( ^{-1} )
B. ( 63 mathrm{g} ) mol ( ^{-1} )
( mathbf{c} cdot 65 mathrm{g} m o l^{-1} )
D. ( 67 mathrm{g} ) mol ( ^{-1} )
12
908The solubility of gases in liquids is not affected by the pressure because the vapor pressure of a substance is not a function of external pressure.
A . True
B. False
12
909Illustration 2.82 Distinguish between the boiling point of
a liquid and the normal boiling point of a liquid.
12
910An aqueous solution of methanol in
water has vapour pressure:
A. equal to that of water
B. equal to that of methanol
c. more than that of water
D. less than that of water
12
911Explain with suitable diagram and appropriate examples why some nonideal solution show positive deviation from ideal behavior:12
912A solution containing ( 4 g ) of a non-
volatile organic solute per ( 100 m L ) was found to have an osmotic pressure
equal to ( 500 mathrm{cm} ) of mercury at ( 27^{circ} mathrm{C} ) The molecular weight of solute is:
A .14 .97
B. 149.7
( c .1697 )
D. 1.497
12
913When a non volatile solute is added to a
pure solvent, the:
A. vapour pressure of the solution becomes lower then that of the pure solvent
B. rate of evaporation of the pure solvent is reduced
C. solute does not effect the rate of condensation
D. rate of the evaporation of the solution is equal to the rate of condensation of the solution at a lower vapour pressure than that in the case of the pure solvent
12
914When ( 1.04 g ) of ( B a C l_{2} ) is present in ( 10^{5} g )
of solution, the concentration of
solution is:
A. 0.104 ppm
в. 10.4 ррт
c. 0.0104 ppm
D. 104 ppm
12
915A ( 0.0020 M ) aqueous solution of an
ionic compound ( boldsymbol{C} boldsymbol{o}left(boldsymbol{N} boldsymbol{H}_{3}right)_{5}left(boldsymbol{N} boldsymbol{O}_{2}right) boldsymbol{C l} )
freezes at ( -0.00732^{circ} mathrm{C} . ) Number of
moles of ions which 1 mole of ionic
compound produces on being dissolved in water will be:
( left[k_{f}=1.86^{circ} C / mright] )
A . 1
B. 2
( c .3 )
D. 4
12
916A ( 5 % ) solution of glucose is isotonic
with ( 1.1 % ) solution of ( mathrm{KCl} ) at ( 30^{circ} mathrm{C} )
Calculate the degree of ionisation of KCI.
A . ( 90 % )
в. ( 88 % )
c. ( 78 % )
D. ( 80 % )
12
9171. An aqueous solution freezes at -2.55°C. What is its boiling
point (K 4,0 = 0.52 K m-!; KH20 = 1.86 Km-!)?
a. 107.0°C b. 100.6°C c.100.1°C d. 100.7°C
12
918Illustration 2.139 A 10 m solution of urea is cooled to
-13.02°C. What amount of urea will separate out if the mass
of solution taken is 100 g? [K, (water) = 1.86 K kg mol-‘) S
12
919Henry law constant for the solubility of methane in benzene at ( 298 mathrm{K} ) is ( 4.27 times )
( 10^{5} mathrm{mm} ) Hg then the solubility of
methane in benzene at ( 298 mathrm{K} ) under
760mm Hg is:
A ( cdot 7.8 times 10^{-2} ) mole ( / mathrm{kg} )
B . ( 7.8 times 10^{-3} ) mole / kg
c. ( 7.8 times 10^{-4} ) mole ( / mathrm{kg} )
D. ( 1.78 times 10^{-3} ) mole ( / mathrm{kg} )
12
920yuuuu 10 OUVOU
Q. 44 How does sprinkling of salt help in clearing the snow co
hilly areas? Explain the phenomenon involved in the process
Anchon polt
from the surface
lp in clearing the snow covered roads in
12
921What is the concentration of a solution
of 2,000 grams of water in which 684
grams of sucrose, ( C_{12} H_{22} O_{11} ) is
dissolved?
A. 25 molar
B. 0.5 molal
c. 1 molal
D. 5 molar
E. 1 molar
12
922The vapour pressure of pure liquid is 70
Torr at ( 27^{circ} mathrm{C} ). The vapour pressure of a
solution of this liquid and another liquid (mole fraction 0.2) is 84 Torr at
( 27^{circ} mathrm{C} . ) The vapour pressure of pure
liquid ( B ) at ( 27^{circ} C ) is?
A. 140 Torr
B. 280 Torr
c. 160 Torr
D. 200 Torr
12
923Which of the following liquid pairs shows a positive deviation from
Raoult’s law?
A. Water – hydrochloric acid
B. Benzene – methanol
c. water – nitric acid
D. Acetone – chloroform
12
924The density of 3 M solution of NaCl is 1.2 ( mathrm{g} m L^{-1} . ) The molality of the solution is?
A. 2.79 ( mathrm{m} )
B. 1.79 ( m )
c. ( 3.5 mathrm{m} )
D. 5.58 m
12
9250.53 Assertion (A) When NaCl is added to water a depression in freezing
point is observed.
Reason (R) The lowering of vapour pressure of a solution causes
depression in the freezing point.
12
926To determine whether a water solution
of ( N a_{2} S_{2} O_{3} ) at room temperature is
supersaturated, one can :
A. heat the solution to its boiling point
B. add water to the solution
c. add a crystal of ( N a_{2} S_{2} O_{3} ) to the solution
D. acidify the solution
E. cool the solution to its freezing point
12
927Teleases WIL HUILast Ulumpur
Assertion : During extreme winter season the roads get
blocked in Jammu and Kashmir due to snowfall and to remove
ice on roads some salt water is sprinkled on ice.
Reason: The addition of any soluble impurity results in
decrease in melting point.
12
928Write the formula to calculate the mole
fraction?
12
929The vapour pressure of a certain liquid is given by the equation:
( log _{10} P=3.54595-frac{313.7}{T}+ )
( mathbf{1} . mathbf{4 0 6 5 5} log _{mathbf{1 0}} boldsymbol{T} )
where ( P ) is the vapour pressure in ( mathrm{mm} ) and ( T=K ) elvin temperature. Determine
the molar latent heat of vaporisation at
( boldsymbol{T}=mathbf{8 0} boldsymbol{K} )
12
930If an excess of ( A g N O_{3} ) solution is added to ( 100 mathrm{ml} ) of ( 0.024 mathrm{M} ) solution of dichlorobis (ethylene diamine) cobalt
(III) chloride, how many moles of ( A g C l ) will be precipitated?
A . 0.0012
B. 0.0016
c. 0.0024
D. 0.0048
12
931An azeotropic mixture of two liquids
boils at a lower temperature than either of them when :
A . it is saturated
B. it does not deviate from Raoult’s law
c. it shows negative deviation from Raoult’s law
D. it shows positive deviation from Raoult’s law
12
932Which substance does NOT dissolve
well in water?
A ( cdot N H_{3} )
B. ( C_{4} H_{10} )
c. ( C_{12} H_{22} O_{11} )
D. ( H_{2} S O_{4} )
12
933The vapour pressure of a pure liquid ( boldsymbol{A} )
is 70 torr at ( 27^{circ} mathrm{C} ). It forms an ideal
solution with another liquid ( B ). The mole
fraction of ( B ) is 0.2 and total vapour
pressure of the solution is 84 torr at
( 27^{circ} mathrm{C} . ) The vapour pressure of pure
liquid ( B ) at ( 27^{circ} mathrm{C} ) is:
A . 14
B. 56
( c .140 )
D. 70
12
934If the elevation in boiling point of a solution of non-volatile, non-electrolytic and non-associating solute in a solvent ( left(K_{b}=x K k g m o l^{-1}right) ) is ( y K, ) then the depression in freezing point of solution of same concentration would be:
( left[boldsymbol{K}_{f} text { of the solvent }=boldsymbol{z} boldsymbol{K} boldsymbol{k} boldsymbol{g} boldsymbol{m o l}^{-1}right] )
A ( cdot frac{2 x z}{y} )
в. ( frac{y z}{x} )
c. ( frac{x z}{y} )
D. ( frac{y z}{2 x} )
E ( cdot frac{x z}{2 y} )
12
935Equal volumes of ( 1 mathrm{M} K_{2} S O_{4} ) and ( 1 mathrm{M} )
( A l_{2}left(S O_{4}right)_{3} ) solutions are mixed. Which
of the following is incorrect?
A. The concentration of ( K^{+} ) is 1 M
B. The concentration of ( A l^{3+} ) is 1M
C. The concentration of ( S O_{4}^{2-} ) is 2 M
D. The concentration of all the three ions is 1 M
12
936Illustration 2.97 On dissolving 3.24 g of sulphur in 40 g
of benzene, the boiling point of the solution was higher than
that of benzene by 0.81 K. What is the molecular formula of
sulphur? (K, for benzene = 2.53 K kg mol-, atomic mass of
sulphur = 32 g mol-?).
12
937Which of the following condition is not followed for an ideal solution?
A ( cdot Delta H_{text {mixing}}=0 )
B. ( Delta S_{text {mixing}}=0 )
C. ( Delta v_{text {mixing}}=0 )
D. All A, B, and C are followed
12
938Addition of ethylene glycol (non-volatile) to water lowers the freezing point of water and hence it is used as antifreeze.
Addition of any substance to water
lowers its freezings point of water.
A. Statement-1 is true, statement-2 is true and statement-2 is correct explanation for statement-
B. Statement-1 is true, statement-2 is true and statement-2 is NOT the correct explanation for statement-1
C. Statement-1 is true, statement-2 is false
D. Statement-1 is false, statement-2 is true
12
939Question 5. A solution of glucose in water is labelled as 10% w/w. What
should be the molality and mole fraction of each component in the
solution? If the density of solution is 12 g mL, then what shall be the
molarity of the solution?
0 As percentage by weight is given find weight of solute (Wa) and
solvent (WA) from it and calculate molar mass of solute (glucose), MB
by adding atomic masses of different elements,
(ii) Calculate molality by using, m =
WA
(iii) In order to calculate mole fraction, calculate the number of moles of
solute and solvent.
(iii) Calculate the volume by the formula of density and then molarity by
using moles of solute and volume of solution.
12
940( 20 mathrm{ml} ) of ( 1 mathrm{M} mathrm{BaCl}_{2} ) solution and ( 25 mathrm{m} )
of ( 0.1 mathrm{M} mathrm{Na}_{2} mathrm{SO}_{4} ) are mixed to form
( B a S O_{4} . ) The amount of ( B a S O_{4} )
precipitated are:
A . 2.5 g
B. 2.5 moles
c. 2.5 millimoles
D. 0.05 millimoles
12
941A ( 5 % ) solution (w/W) of cane sugar
(molar mass ( =342 g ) mol ( ^{-1} ) ) has
freezing point ( 271 K . ) What will be the freezing point of ( 5 % ) glucose (molar mass ( =18 g ) mol ( ^{-1} ) ) in water if freezing
point of pure water is ( 273.15 K ? )
( mathbf{A} cdot 273.07 K )
в. ( 269.07 K )
c. ( 273.15 K )
D. ( 260.09 K )
12
942Clothes do not protect us from
A. heat
B. cold
c. blood pressure
D. dust and germs
12
943Q. 42 (a) Explain the following phenomena with the help of Henry’s law.
(i) Painful condition known as bends.
(ii) Feeling of weakness and discomfort in breathing at high altitude.
(b) Why soda water bottle kept at room temperature fizzes on opening?
12
944Illustration 2.34 The vapour pressure of acetone at 298 K
is 40 mm of Hg. Its mole fraction in a solution with alcohol
is 0.80. What is its vapour pressure in solution if the mixture
obey Raoult’s law?
12
945An example of solid in non-aqueous solvent is :
A. sugar in Ethanol
B. blood
c. starch
D. sugar sol
12
946Solutions ( A, B, C ) and ( D ) are
respectively ( 0.1 M ) glucose,
( mathbf{0 . 0 5} M N a C l, 0.05 M B a C l_{2} ) and
( 0.1 M A l C l_{3} . ) Which one of the following
pairs is isotonic?
A. ( A ) and ( B )
B. ( B ) and ( C )
c. ( A ) and ( D )
D. ( A ) and ( C )
12
947On mixing equal volumes of acetone and ethanol, what type of deviation from Raoult’s law is expected?12
948The binary mixture of a particular composition in both liquid and vapour state is known as a/an azeotropic mixture.
If true enter 1 , if false enter 0 .
12
949Ratio of solubilities of ( operatorname{gases} N_{2} & O_{2} )
in water from air at ( 25^{circ} & 1 ) atm will be
if air is ( 20 % ) by volume of ( O_{2} ) and ( 80 % ) by
volume of ( boldsymbol{N}_{2} )
[
begin{aligned}
operatorname{Given} &: boldsymbol{K}_{boldsymbol{H}}left(boldsymbol{N}_{2}right)=boldsymbol{2} times mathbf{1 0}^{4} boldsymbol{a t m} \
boldsymbol{K}_{boldsymbol{H}}left(boldsymbol{O}_{2}right) &=mathbf{1 0}^{4} boldsymbol{a t m}
end{aligned}
]
A . 8: 1
B. 1: 8
( c cdot 1: 2 )
D. 2: 1
12
950To determine the solubility of a solute in water, a solution must be prepared that is
A. saturated
B. unsaturated
c. concentrated
D. supersaturated
12
951The van’t Hoff factor for a very dilute
aqueous solution of ( boldsymbol{K}left[boldsymbol{A} boldsymbol{g}(boldsymbol{C} boldsymbol{N})_{2}right] ) is:
A . 4
B. 3
c. 2
D. 5
12
952Calculate the freezing temperature of
an aqueous solution having its boiling
temperature ( 100.1^{circ} mathrm{C} ). The mola
ebullioscopic constant and the molal cryoscopic constant are 0.513 deg and 1.86 deg, respectively. The answer is
( -0 . m n ) then ( m+n= )
12
953When ( 12.044 times 10^{23} ) molecule of
( H_{2} S O_{4} ) is dissolve in ( 195 mathrm{cm}^{3} ) solution.
What is mass percent ( boldsymbol{H}_{2} boldsymbol{S} boldsymbol{O}_{4} ) in the solution. If the density of the solution is ( 1.25 g c m^{-3} )
12
954A solution of glucose ( left(C_{8} H_{12} O_{6}right) ) is
isotonic with ( 5 g ) of urea
( left(N H_{2} C O N H_{2}right) ) per litre of solution
The concentration of glucose is:
A. ( 48 / L )
B. 8 g/L
c. 12 g/L
D. ( 15 mathrm{g} / mathrm{L} )
12
Question 25. Among the following compounds, identify which are
insoluble, partially soluble and highly soluble in water?
(1) Phenol
(ii) Toluene
(ii) Formic acid
(iv) Ethylene glycol
(v) Chloroform
(vi) Pentanol
Consider different types of molecular forces.
12
956An aqueous solution of a substance molar mass 240 has osmotic pressure
( 0.2 mathrm{atm} ) at ( 300 mathrm{K} ). The density of solution ( operatorname{in} g cdot d m^{3} ) is: ( (R= )
( left.0.08 text { litre atm } K^{-1} m o l^{-1}right) )
12
957g mixture of glucose and urea present in ( 250 mathrm{mL} ) aqueous solution shows the
osmotic pressure of 0.74 atm at ( 27^{circ} C )
Assuming solution to be diluted, which
are correct?
1. Percentage of urea in the mixture is
17.6
2. Relative lowering of the vapour
pressure of this solution is ( 5.41 times 10^{-4} )
3. The solution will boil at ( 100.015^{circ} C ), if
( K_{b} ) of water is ( 0.5 mathrm{K} ) molality ( ^{-1} )
4. If glucose is replaced by the same amount of sucrose, the solution will
show higher osmotic pressure at ( 27^{circ} C )
5. If glucose is replaced by the same amount of ( N a C l ), the solution will show
lower osmotic pressure at ( 27^{circ} mathrm{C} )
A. 1,2,3
в. 1,2,3,5
c. 2,4,5
D. 1,4,5
12
958A substance is completely trimerized on dissolution in a solvent. The Van’t
Hoff factor ( (i) ) for such change is:
A . 1
B . 2
( c .3 )
D. ( 1 / 3 )
12
959Molarity of ( 4 % ) (w/v) solution of ( N a O H )
is:
A . ( 0 . )
B. 0.5
c. 0.001
D. 1.0
12
9600.5 Maximum amount of a solid solute that can be dissolved in a specified
amount of a given liquid solvent does not depend upon ……..
(a) temperature
(b) nature of solute
(c) pressure
(d) nature of solvent
12
961Tlustration 2.115 By dissolving 13.6 g of a substance in 20g
of water, the freezing point decreased by 3.7°C. Calculate the
molecular mass of the substance. (Molal depression constant
for water = 1.863 K kg mol-l)
12
962( 10^{-3} ) mol of ( C u S O_{4} cdot 5 H_{2} O ) is
introduced in a ( 1.9 L ) vessel maintained
at a constant temperature of ( 27^{circ} mathrm{C} ) containing moist air at relative
humidity of ( 12.5 % . ) What is the final molar composition of solid mixture?
For ( boldsymbol{C u} boldsymbol{S O}_{4} cdot boldsymbol{5} boldsymbol{H}_{2} boldsymbol{O}(boldsymbol{s}) rightleftharpoons boldsymbol{C u} boldsymbol{S} boldsymbol{O}_{4}(boldsymbol{s})+ )
( mathbf{5} H_{2} O(boldsymbol{g}), boldsymbol{K}_{p}(boldsymbol{a} boldsymbol{t m})=mathbf{1 0}^{-10} . ) Take vapor
pressure of water at ( 27^{circ} mathrm{C} ) as 28 torrs.
12
963A solution is obtained by mixing ( 200 g ) of ( 30 % ) and ( 300 g ) of ( 20 % ) solution by weight What is the percentage of solute in the
final solution?
A . ( 50 % )
B . 28%
c. ( 64 % )
D. 24%
12
964The vapour pressure of a deliquescent
substance is:
A. equal to the atmospheric pressure
B. equal to that of the water vapour in air
C . greater than that of the water vapour in air
D. less than that of the water vapour in air
12
965( 0.24 mathrm{g} ) of a volatile gas upon vaporization gives 45 mL vapour at ( mathrm{NTP} ) What will be the vapour density of the
substances? (density of ( boldsymbol{H}_{2}=mathbf{1} ) )
(a) 95.39
(b) 5.973
(c) 95.93
(d) 59.73
12
966What is a vitreous state?12
967Example 2.22 At 17°C, the osmotic pressure of sugar
solution is 580 torr. The solution is diluted and the
temperature is raised to 57°C, when the osmotic pressure is
found to be 165 torr. The extent of dilution is
a. 2 times b. 3 times c. 4 times d. 5 times
12
968Question 5. Calculate (a) molality (b) molarity and (c) mole fraction of
KI if the density of 20% (mass/mass) aqueous KI is 1.202 g mL-.
(0) As density and % by mass is given, so find the mass of solute and
solvent (as x % solution contains xg solute in (100 – x)g solvent).
(ii) Find volume of the solution, by using,
Volume = Mass
on Density
(iii) Recall the formulae of molality, molarity and mole fraction, to
calculate them.
12
969A solution of 0.2 mole ( mathrm{Kl}(alpha=100 %) ) in
1000 g water freezes at ( T_{1}^{circ} ) C. Now to
this solution 0.1 mole ( H g I_{2} ) is added
and the resulting solution freezes at
( T_{2}^{circ} mathrm{C} . ) Which of the following is correct?
A ( cdot T_{1}=T_{2} )
в. ( T_{1}>T_{2} )
c. ( T_{1}<T_{2} )
D. can't be prediced
12
970so Components of a binary mixture of two liquids A and B were being
separated by distillation. After some time separation of components
stopped and composition of vapour phase became same as that o ur
phase. Both the components started coming in the distillate. Explam
why this happened?
12
971Question 3. Explain the solubility rule ‘like dissolves like’ in terms of
intermolecular forces that exist in solutions.
12
972The expression relating mole fraction of
solute ( left(chi_{2}right) ) and molarity ( (mathrm{M}) ) of the
solution is (where dis the density of the
solution in ( g L^{-1} ) and ( M w_{1} ) and ( M w_{2} )
are the molar masses of solvent and
solute, respectively
A ( cdot x_{2}=frac{M times M w_{1}}{Mleft(M w_{1}-M w_{2}right)+1000 d} )
B. ( x_{2}=frac{M times M w_{1}}{Mleft(M w_{1}-M w_{2}right)+d} )
c. ( _{x_{2}}=frac{M times M w_{1}}{Mleft(M w_{1}-M w_{2}right)-1000 d} )
D. ( _{x_{2}}=frac{M times M w_{1}}{Mleft(M w_{1}-M w_{2}right)-d} )
12
973Which of the following azeotropes is not
correctly matched?
( mathbf{A} cdot H N O_{3}(68 %)+H_{2} O(32 backslash %): ) Maximum boiling
azerotrope, boiling point ( =393.5 K )
B ( cdot H_{2} O(43 %)+H I(57 %): ) Minimum boiling azeotrope, boiling point ( =290 K )
C ( cdot C_{2} H_{5}(95.5 %)+H_{2} O(4.5 %): ) Minimum boiling azerotrope, boiling point ( =351.15 K )
D. Chloroform (93.2%) ( +C_{2} H_{5} O H ) (6.8%): Minimum boiling azeotrope, boiling point ( =332.3 K ) )
12
974Illustration 2.76 The relative lowering of the vapour
pressure of an aqueous solution containing a non-volatile
solute is 0.0125. The molality of the solution is
a. 0.80 b. 0.50
c. 0.70
d. 0.40
12
975If mole fraction of urea in 11.11 mola
aqueous solution?
A . 0.1
B. 0.17
( c .0 .2 )
D. 0.37
12
976Illustration 2.184. A solution of non-volatile solute in water
freezes at -0.80°C. The vapour pressure of pure water at
298 K is 23.51 mm Hg and K, for water is 1.86 degree per
molal. Calculate the vapour pressure of this solution at
298 K.
12
977A solution containing 500 g of a protein per liter is isotonic with a solution
containing 3.42 g of sucrose per liter. The molecular mass of protein is:
( A cdot 58 )
B. ( 146 mathrm{g} )
c. ( 34200 mathrm{g} )
D. 50000 ( g )
12
978If you dilute ( 25.0 mathrm{mL} ) of ( 1.5 mathrm{M} H C l ) to ( 500 mathrm{mL}, ) then the molar concentration of
each ions becomes ( boldsymbol{Y} times mathbf{1 0}^{-mathbf{3}} boldsymbol{M} . ) Here ( boldsymbol{Y} )
is:
12
979The substance ( A ), when dissolved in
solvent ( mathrm{B} ), shows the molecular mass
corresponding to ( A_{3} . ) The Vant Hoff’s factor will be:
A . 1
B. 2
( c cdot 3 )
D. ( 1 / 3 )
12
980A solution of 1.25 g of ( mathrm{P} ) in 50 g of water lowers freezing point by 0.3. Molar mass of ‘Pis 94. ( boldsymbol{K}_{f(text {water})}=mathbf{1 . 8 6} mathrm{K} mathrm{kg} mathrm{mol}^{-1} )
The degree of association of P in water is:
A . ( 60 % )
B. 75%
c. ( 80 % )
D. 65%
12
981On mixing, heptane and octane form an
ideal solution. At ( 373 mathrm{K} ), the vapour pressures of the two liquid components (heptane and octane) are 105 kPa and
45 kPa respectively. Vapour pressure of the solution obtained by mixing 25.0 gm of heptane and 35 gm of octane will be:(molar mass of heptane ( = )
( 100 mathrm{gmo} 1^{-1} ) and of octane ( = )
( left.114 operatorname{gmol}^{-1}right) )
( mathbf{A} cdot 72.0 mathrm{kPa} )
B . ( 36.1 mathrm{kPa} )
c. ( 96.2 mathrm{kPa} )
D. ( 144.5 mathrm{kPa} )
12
982Illustration 2.121 Calculate the freezing point depression
and boiling point elevation of a solution of 10.0 g of urea
(MR = 60) in 50.0 g of water at 1 atm. pressure. K and K, for
water 0.52°C m-1 and 1.86°C m-1 respectively.
12
983A volume of 50 lof dry ( N_{2} ) is passed
through ( 36 g ) of water at 300 K. After
passage of gas, there is a loss of 1.20 g in water. The vapour pressure of water at ( 300 mathrm{K} ) is?
в. ( 24.96 mathrm{mm} ) Н ( mathrm{g} )
c. ( 16.05 mathrm{mm} ) нв
D. ( 38.73 mathrm{mm} ) Hg
12
984When 1 mole of a substance is present
in 1 L of the solution, it is known as:
A. normal solution
B. molar solution
c. molal solution
D. None of the above
12
985What is the concentration of a cobalt (II)
nitrate solution whose absorbance was
measured at 0.55 in a ( 1.1 mathrm{cm} ) cuvette
with a molar extinction coefficient of
( mathbf{1 . 5} / boldsymbol{M} mathbf{c m} ? )
в. ( 0.60 M )
c. ( 0.90 M )
D. ( 1.2 M )
12
986Hardness in water is expressed in
terms of ppm of ( C a C O_{3} . ) If hardness is
200 ppm ( C a C O_{3}, ) then in terms of molarity, it is:
A. ( 0.004 mathrm{M} )
B. ( 0.002 M )
c. ( 0.001 M )
D. ( 0.0005 M )
12
987What do you mean by the
“concentration” of a substance?
A. It is the measure of undissolved substances
B. It refers to the impurities
C. Concentration refers to the amount of substance per defined space
D. It means total mass of the un dissolved gases
12
988What is the equivalent mass ( I O_{4}^{-} ) when
it is converted into ( I_{2} ) in acid medium?
A. M/6
в. м/7
c. м/5
D. M/4
12
989An ideal gaseous mixture of ethane and ethene occupy ( 28 L ) as STP. The mixture
required ( 128 g O_{2} ) combustion, mole fraction of ethene in the mixture is:
A . 0.4
B. 0.5
c. 0.6
D. 0.8
12
990Define molarity.12
991If the formula weight of ( boldsymbol{H}_{2} boldsymbol{S} boldsymbol{O}_{4} ) is 98 then the amount of acid present in 400 ( mathrm{ml} ) of 0.1 molar solution of acid will be:
A. ( 2.45 g )
B . ( 3.92 g )
c. ( 4.90 g )
D. ( 9.80 g )
12
992A mixture of ( N a_{2} C_{2} O_{4}(A) ) and
( K H_{2} C_{2} O_{4} cdot 2 H_{2} O(B) ) required equal
volumes of ( 0.1 mathrm{M} K M n O_{4} ) and ( 0.1 mathrm{M} )
NaOH separately. Molar ratio of ( A ) and
( B ) in the mixture is :
A . 1: 1
B. 1: 5.5
c. 5.5: 1
D. 3.1 : 1
12
993Find out the correct statement
regarding a saturated solution of salt in
water?
A. All dissolving has stopped
B. Crystals begin to grow
C. An equilibrium has been established
D. Crystals of the solute will visibly continue to dissolve
E. The solute is exceeding its solubility
12
994Illustration 2.31 Assuming ideal behaviour, calculate the
pressure of 1.0 molal solution of a non-volatile molecular
solute in water at 50°C. The vapour pressure of water at 50° C
is 0.222 atm.
12
995The mole fraction of ( N_{2} O ) In a mixture of ( N_{2} O ) and ( N O ) is ( frac{1}{3} . ) The mole fraction
of ( N O ) in a mixture of ( N O ) and ( N O_{2} ) is
3. The two mixtures are mixed in 3: 4
( overline{mathbf{4}} )
molar ratio. the mole fraction of ( N O_{2} ) in
the resulting mixture is:
12
996At ( 10^{0} C, ) the osmotic pressure of urea solution is ( 500 mathrm{mm} ). The solution is
diluted and the temperature is raised to
( 25^{0} C, ) so that the osmotic pressure became ( 105.3 mathrm{mm} . ) The number of times,
the solution diluted is:
A . 6
B. 5
( c cdot 4 )
D. 3
12
997The main reason for the extremely low solubility of carbon dioxide in benzene
( left(C_{6} H_{6}right) ) at room temperature is due to which of the following?
A. The increased disorder due to mixing of the solute and solvent
B. The relatively low strength of the intermolecular forces between carbon dioxide and benzene
c. The strong hydrogen bonding in benzene
D. The weak solvation of carbon and oxygen ions by benzene
12
998Find the degree of association when 1.0 gram benzoic acid, dissolved in 25
gram benzene is having depression in
freezing point ( 0.81 k . ) The mola
depression constant for solvent is ( 4.9 K ) kg mole ( ^{-1} )
12
999Which of the following is a mixture?
A. water
B. Oxygen
c. Carbon dioxide
D. Air
12
1000Molal elevation constant and molal
depression constant of water
respectively ( left(text { in } quad K m^{-1}right) ) are:
A. 0.52,1.86
В. 1.86,0.52
c. 1.52,0.86
D. 0.86,1.52
12
1001The total pressure or a mixture of
oxygen and hydrogen is 1.0 atm. The mixture is ignited and the water is removed. The remaining gas is pure hydrogen and exerts a pressure of 0.40 when measured at the same values of ( T )
and ( mathrm{V} ) as the original mixture. What was
the composition of the original mixture in mole per cent?
A ( cdot x_{O_{2}}=0.2 ; x_{H_{2}}=0.8 )
в. ( x_{0}_{0}=0.4 ; x_{H_{2}}=0.6 )
c. ( x_{o_{2}}=0.6 ; x_{H_{2}}=0.4 )
D. ( x_{O_{2}}=0.8 ; x_{H_{2}}=0.2 )
12
1002Volume (in litres) of ( 0.1 mathrm{M} boldsymbol{H}_{2} boldsymbol{S O}_{4} )
required to completely neutralize 1 litres of ( 0.5 mathrm{M} ) NaOH is:
( mathbf{A} cdot mathbf{5} )
в. 2.
c. 0.5
D. 10
12
1003Example 2.7 In a study of aqueous solution of thorium
nitrate, the freezing point depression of 0.0703 °C is observed
for a 9.6 mmol kg of the solution. How many ions are present
in one thorium nitrate unit? (K, for H,0 = 1.86 Km !)
12
1004If molality of the dilute solution is doubled, the value of molal depression
constant ( left(boldsymbol{K}_{boldsymbol{f}}right) ) will be :
A. unchanged
B. doubled
c. halved
D. tripled
12
1005Illustration 2.110 If the boiling point of an aqueous solution
containing a non-volatile solute is 100.15°C. What is its
freezing point? Given latent heat of fusion and vapourization
of water 80 cal g1 and 540 cal g, respectively.
12
1006The above laboratory setup can be used
to prepare:
A. gas lighter than air and soluble in water
B. gas heavier than air and soluble in water
c. gas soluble in water that reacts with water
D. gas insoluble in water
E. gas that reacts with water
12
1007Which characteristic the weak
intermolecular forces of attraction in a
liquid?
A. High boiling point
B. High vapour pressure
c. High critical temperature
D. High heat of vaporization
12
1008A solution containing 5 g acetic acid in 100 g ( boldsymbol{H}_{2} boldsymbol{O}left(boldsymbol{O}_{boldsymbol{H}_{2}}^{0} boldsymbol{O}=mathbf{2} boldsymbol{3} . mathbf{7} mathbf{5} boldsymbol{6} boldsymbol{m} boldsymbol{m} text { at } mathbf{2} mathbf{5}^{boldsymbol{o}} boldsymbol{C}right. )
shows a vapour pressure of ( 23.40 mathrm{mm} ) whereas same mass of acetic acid in
( 100 mathrm{g} C_{6} H_{6}left(P_{C_{6} H_{6}}^{0}=72.5 m m text { at } 25^{circ} Cright) )
shows a vapour pressure of ( 70.0 mathrm{mm} ) Assuming non-volatile nature of ( C H_{3} C O O H, ) discuss the data given to discuss hydrogen bonding:
A. acetic acid exists as a monomer
B. acetic acid exists as a dimer
c. acetic acid is dissociated
D. acetic acid exists as an anhydride
12
1009Tlustration 2.171 A solution was prepared by dissolving
6.0 g an organic compound in 100 g of water. Calculate the
osmotic pressure of this solution at 298 K, when the boiling
point of the Solution is 100.2°C. (K, for water = 0.52 K m-,
R = 0.082 L atm K-1 mol1)
12
1010An unknown composition of a mixture of carbon disulphide and hydrogen sulphide was burnt in sufficient
amount of oxygen. The resulting gases found to exert a pressure of 1.97 atm in a 20 I vessel at 400 K. The gaseous
mixture required 2.8 M iodine solution and ( 250 mathrm{ml} ) of it was required to reach
the end point, forming ( boldsymbol{I}^{-} ). Calculate the
mole fraction of ( boldsymbol{C} boldsymbol{S}_{2} ) in the original
mixture.
A. 0.2
B. 0.4
c. 0.6
D. 0.8
12
1011Van’t Hoff’s factor of aq. ( K_{2} S O_{4} ) at infinite dilution has value equal to:
( mathbf{A} cdot mathbf{1} )
B. 2
( c .3 )
D. Between 2 and 3
12
1012Q.59 When kept in water, raisin swells in size. Name
phenomenon involved with the help of a diagrami.
applications of the phenomenon.
un incide the raisin and
swells in size. Name and explain the
the help of a diagram. Give three
12
1013The osmotic pressure of a solution containing 40 g of solute (molecular mass 246 ) per litre at ( 27^{circ} C ) is:
( left[boldsymbol{R}=mathbf{0 . 0 8 2 2} boldsymbol{operatorname { a t m }} boldsymbol{L} boldsymbol{m o l}^{-mathbf{1}}right] )
A. 3.0 atm
B. 4.0 atm
c. 2.0 atm
D. 1.0 atm
12
1014Which has the highest boiling point?
A. ( 0.1 mathrm{M} mathrm{Na}_{2} mathrm{SO}_{4} )
В. ( 0.1 M C_{6} H_{12} O_{6} )
c. ( 0.1 mathrm{M} ) М ( g ) Са( _{2} )
D. ( 0.1 mathrm{M} ) Аl ( left(mathrm{NO}_{3}right)_{3} )
12
1015The solution with the highest boiling point temperature is:
в. ( 0.1 mathrm{M} ) НС ( mathrm{CO}_{4} )
c. ( 0.1 mathrm{M} mathrm{NH}_{4} mathrm{OH} )
D. 0.1 М КОН
E. ( 0.1 mathrm{M} ) LiNO ( _{3} )
12
1016The vapour pressure in ( mathrm{mm} ) of ( boldsymbol{H} boldsymbol{g} ), of an aqueous solution obtained by adding 18 g of glucose ( left(C_{6} H_{12} O_{6}right) ) to 180 gof water at ( left(100^{circ} mathrm{C}right) ) is:
A . 7.60
B. 76.0
c. 759
D. 752.4
12
10170.39 Concentration terms such as mass percentage, ppm, mole fraction and
molality are independent of temperature, however molarity is a function
of temperature. Explain.
Thinking Process
To solve this problem notice the role of temperature in component of concentration
term such as volume, mass, number of moles etc.
H
ali
12
1018For an ideal solution with ( boldsymbol{p}_{boldsymbol{A}}^{boldsymbol{o}}>boldsymbol{p}_{boldsymbol{B}}^{boldsymbol{o}} )
which of the following is true?
A ( cdotleft(x_{A}right)_{text {liquid}}=left(x_{A}right)_{text {vapour}} )
В . ( left(x_{A}right)_{text {liquid }}>left(x_{A}right)_{text {vapour }} )
C ( cdotleft(x_{A}right)_{text {liquid}}<left(x_{A}right)_{text {vapour}} )
D cdot ( left(x_{A}right)_{text {liquid }} ) and ( left(x_{A}right)_{text {vapour }} ) cannot be correlated with each other
12
1019Which substance would dissolve
fastest in water?
A ( .1 g ) granulated sugar
B. ( 1 ~ g ) powdered sugar
C. ( 1 ~ g ) sugar cube
D. ( 1 g ) piece of crystallized sugar
12
32
elone
37. Vapour pressures of pure acetone and chloroform at
are 141.8 mm Hg and 632.8 mm Hg respectively. Assuming that
they form ideal solution over the entire range of composition, P. total
Pchloroform and Pacetone as function of Xane. The experimental data
observed for different compositions of mixture is :
0 11.8 23.4 36.0 50.8 58.2 645 721
Pacetone/ mm Hg 0 54.9 110.1 202.4 322.7 405.9 4541 521.1
Pchloroform/mm Hg 632.8 548.1 469.4 359,7 257.7 193.6 161.2 120.7
Plot this data also on the same graph paper. Indicate whether it has
positive deviation or negative deviation from the ideal solution.
100 x acetone
Find Ptotal and x acetone and then plot the graph.
12
1021If we take ( 44 mathrm{g} ) of ( C O_{2} ) and ( 14 mathrm{g} ) of ( N_{2} )
what will be the mole fraction of ( C O_{2} ) in
the mixture?
A . ( 1 / 5 )
в. ( 1 / 3 )
c. ( 2 / 3 )
D. ( 1 / 4 )
12
1022Concentration terms like mass
percentage, ppm, mole fraction and
molality do not depend on temperature.
However, molarity is a function of
temperature because:
A. volume depends on temperature and molarity involves volume
B. molarity involves non-volatile solute while all other terms involve volatile solute
C. number of moles of solute change with change in temperature
D. molarity is used for polar solvents only
12
1023A solution of sugar in which some more sugar could be dissolved without
changing its temperature is called a/an
A. unsaturated solution
B. saturated solution
c. solid solution
D. true solution
12
1024The solubility of the gas in a liquid solution with an increase in
temperature.
A . decreases
B. increases
c. remains same
D. none of these
12
1025The density of ( 85 % ) Phosphoric acid is ( 1.70 g c m^{-3} . ) What is the volume of a
solution that contains ( 17 g m ) Phosphoric acid?
12
1026How many kg (nearest integer value) of wet ( N a O H ) containing ( 12 % ) water is
required to prepare 60 L of ( 0.50 M )
Na ( O H ) solution? If the answer is ( x ) then
the nearest integral value of ( 1000 x )
12
1027Number of moles of ( S_{2} O_{3}^{2-} ) present in
the sample is:
A . 0.0005
B. 0.01
c. 0.0025
D. 0.02
12
1028Which among the following has lowest
vapour pressure?
A ( .0 .5 M A l_{2}left(S O_{4}right)_{3} )
B. ( 12 % ) Urea solution
c. ( 1 M ) NaCl ( (a q) )
D. ( 18 % ) Glucose solution
12
1029The molarity of a NaOH solution by dissolving ( 4 g ) of it on ( 250 m L ) water is:
A ( .0 .4 M )
B. ( 0.8 M )
c. ( 0.2 M )
D. ( 0.1 M )
12
10309. The vapour pressure of pure liquid solvent A is 0.80 atm.
When a non-volatile substance B is added to the solvent,
its vapour pressure drops to 0.60 atm; the mole fraction
of component B in the solution is
b. 0.25 c. 2.0
d. 3.0
a. 0
12
1031The vapour pressure of three liquids
( P, Q ) and ( R, ) of nearly equal molecular
masses is shown as a function of
temperature
The correct statement is:
A. The normal boiling points follow the order ( P>Q>R )
B. The variation of pressure with respect to temperature for each liquid is given by ( frac{d P}{d T}=frac{K}{T^{2}}, ) where ( K ) is a
constant
c. The strength of intermolecular interactions follows the order ( P>Q>R )
D. The normal boiling point of ( Q ) is close to ( 65^{circ} mathrm{C} )
12
1. Derive the mathematical expression
between molar mass of a non-volatile
solute and elevation of boiling point
2. State and explain van’t Hoff-
12
1033What is the total pressure of the dry gas collected if the vapor pressure due to
water at ( 25^{circ} C ) is 24 mm Hg( ? )
A. ( 24 mathrm{mm} mathrm{Hg} )
в. ( 240 mathrm{mm} mathrm{Hg} )
( mathbf{c} .736 mathrm{mm} mathrm{Hg} )
D. ( 760 mathrm{mm} mathrm{Hg} )
12
1034Illustration 2.206 Van’t Hoff factors of aqueous solutions
of X, Y, and Z are 2.8, 1.8, and 3.5, respectively. Which of the
following statement(s) is(are) correct?
a. BP: X<Y<Z
b. FP: Z<X<Y
c. Osmotic pressure: X=Y= Z
d. VP: Y<3 <3
12
1035What is the concentration of nitrate
ions if equal volumes of ( 0.1 M A g N O_{3} )
and ( 0.1 M ) NaCl are mixed together?
( mathbf{A} cdot 0.1 mathrm{M} )
B. 0.2 М
c. 0.05 M
D. 0.25 м
12
1036At high altitudes, the boiling of water
takes place below ( 100^{circ} mathrm{C} ) because :
A. the atmospheric pressure is low
B. the temperature is low
c. the atmospheric pressure is high
D. none of the above
12
1037A mixture contains 1 mole of volatile
liquid ( Aleft(P_{A}^{circ}=100 m m H gright) ) and 3
moles of volatile liquid ( boldsymbol{B}left(boldsymbol{P}_{boldsymbol{B}}^{circ}=right. )
( 80 m m H g) . ) If solution behaves ideally
the total vapour pressure of the distillate is :
A. ( 85 mathrm{mm} ) Hg
B. ( 85.88 mathrm{mm} ) Н
( mathbf{c} .90 mathrm{mm} mathrm{Hg} )
D. ( 92 mathrm{mm} ) Hg
12
1038What is the molarity of ( 2.00 g ) of ( N a O H ) dissolved in a total solution volume of
( 250 m L ? )
( mathbf{A} cdot 0.2 M )
в. ( 0.5 mathrm{M} )
c. ( 0.008 M )
D. 252 М
12
1039Formation of a solution from two
components can be considered as:
(i) Pure solvent ( rightarrow ) separated solvent
molecules, ( Delta boldsymbol{H}_{mathbf{1}} )
(ii) Pure solvent ( rightarrow ) separated solute
molecules, ( Delta boldsymbol{H}_{2} )
(ii) Separated solvent and solute
molecules ( rightarrow ) solution, ( Delta boldsymbol{H}_{3} )

Solution so formed will be ideal if
( mathbf{A} cdot Delta H_{s o l n .}=Delta H_{1}+Delta H_{2}+Delta H_{3} )
B. ( Delta H_{text {soln.}}=Delta H_{1}+Delta H_{2}-Delta H_{3} )
C ( . Delta H_{text {soln.}}=Delta H_{1}-Delta H_{2}-Delta H_{3} )
D. ( Delta H_{text {soln.}}=Delta H_{3}-Delta H_{1}-Delta H_{2} )

12
1040Example 2.4 At 298 K, the vapour pressure of water
is 23.75 mm Hg. Calculate the vapour pressure at the
same temperature over 5% aqueous solution of urea.
– [CO (NH2)2).
12
1041Which of the following plot is correct for an ideal binary solution of liquids ( A ) and
B with ( boldsymbol{P}_{A}^{o}>boldsymbol{P}_{B}^{o} )
( A )
в.
( c )
D.
12
1042Which of the following solution contains approximately equal hydrogen ion concentration?
This question has multiple correct options
A. ( 100 mathrm{mL} ) of ( 0.1 mathrm{M} mathrm{HCl}+50 mathrm{mL} mathrm{H}_{2} mathrm{O} )
B. ( 75 mathrm{mL} ) of ( 0.1 mathrm{M} mathrm{HCl}+75 mathrm{mL} mathrm{H}_{2} mathrm{O} )
c. ( 50 mathrm{mL} ) of ( 0.1 mathrm{M} mathrm{H}_{2} mathrm{SO}_{4}+100 mathrm{mL} mathrm{H}_{2} mathrm{O} )
D. ( 100 mathrm{mL} ) of ( 0.1 mathrm{N} mathrm{H}_{2} mathrm{SO}_{4}+50 mathrm{mL} mathrm{H}_{2} mathrm{O} )
12
1043A sample of wustite ( F e_{x} O ) contains one ( boldsymbol{F} e(boldsymbol{I} boldsymbol{I} boldsymbol{I}) ) for every three ( boldsymbol{F} boldsymbol{e}(boldsymbol{I} boldsymbol{I}) . ) The
value of ( x ) is:
( mathbf{A} cdot 9 / 8 )
в. ( 8 / 9 )
c. ( 3 / 4 )
D. ( 4 / 3 )
12
1044Illustration 2.137 Calculate the amount of ice that will
separate out on cooling containing 50 g of ethylene glycol in
200 g of water to -9.3°C. (K, for water = 1.86 K mol-1 kg)
12
1045Example 2.2 The vapour pressure of water at 293 K is
17.51 mm. The lowering of vapour pressure of sugar is
0.0614 mm. Calculate:
a. The relative lowering of vapour pressure
b. The vapour pressure of the solution
c. The mole fraction of water
12
1046A solution with negative deviation among the following is:
A. ethanol- acetone
B. chlorobenzene-bromobenzene
c. chloroform-acetone
D. benzene-toluene
12
1047The vapour pressure of a dilute solution
of a solute is not influenced by:
A. temperature of solution
B. melting point of solute
c. mole fraction of solute
D. degree of dissociation of solute
12
1048At ( 90^{circ} mathrm{C} ), the vapour pressure of toluene is 400 torr and that of ( sigma-x y ) lene is
150 torr. What is the composition of the
liquid mixture the boils at ( 90^{circ} mathrm{C}, ) when
the pressure is 0.50 atm? What is the composition of vapour produced?
A. Toluene 8 mol%, Toluene=3.2 mol%
B. Toluene 15mol%, Toluene=36 mol%
c. Toluene 85 mol%, Toluene=64 mol%
D. Toluene 92 mol%, Toluene ( =96.8 mathrm{mol%} )
12
1049Each pair forms ideal solution except :
A. ( C_{2} H_{5} B r ) and ( C_{2} H_{5} I )
в. ( C_{6} H_{5} C l ) and ( C_{6} H_{5} B r )
c. ( C_{6} H_{6} ) and ( C_{6} H_{5} C H_{3} )
D. ( C_{2} H_{6} I ) and ( C_{2} H_{5} O H )
12
1050The vapour pressure of a mixture of two
volatile liquids is expressed as ( boldsymbol{P}_{boldsymbol{m}}= )
( 6.0+1.5 X_{B}, ) where, ( X_{B} ) is mole
fraction of ( boldsymbol{B} ) is a mixture. The vapour
pressure of ( boldsymbol{A} ) at the same temperature is:
12
1051Ilustration 2.125 45 g of ethylene glycol C,H,O, is mixed
with 600 g of water. Calculate (a) the freezing point depression
and (b) the freezing point of the solution.
Given K= 1.86 K kg moll (NCERT Example 2.9)
12
1053At ( 25^{circ} mathrm{C}, 1 ) mol of ( A ) having a vapour
pressure of 100 torr and 1 mol of ( B ) having a
vapour pressure of 300 torr were
mixed.
The vapour at equilibrium is removed, condensed and the condensate is
heated back to ( 25^{circ} C )

The vapour now formed are again removed, recondensed and analyzed.If the mole fraction of ( A ) in this
condensate is ( 1 times 10^{-x} ), then what is the
value of ( mathbf{x} ? )

12
1054A solution contains ( 75 mathrm{mg} ) of ( mathrm{NaCl} ) per mL. To what extent must it be diluted to
give a solution of concentration ( 15 mathrm{mg} )
of ( N a C l ) per mL of solution?
12
1055Question 9. A sample of drinking water was found to be several
contaminated with chloroform (CHCIZ) supposed to a carcinogen.
level of contamination was 15 ppm (by mass):
(i) Express this in per cent by mass.
(ü) Determine the molality of chloroform in the water sample.
ppm= parts per million = 10 units
Determine mass % and molality as in previous problems.
12
1056In an expression of the equilibrium constant, units for concentrations are:
A. mol/mL
B. mol/L
( c cdot g / L )
D. gram-equivalents/L
12
1057An Unsaturated solution can be
converted into saturated solution
A. by adding more solute to the solvent
B. by removing solute from the solvent
c. by increasing temperature
D. Both b and c
12
1058Two glucose solutions are mixed of ( 1 M )
and ( 2 M ) respectively in equal volume ratio then the new molarity will be:
( mathbf{A} cdot 1.4 M )
в. ( 1.25 M )
c. ( 1.5 M )
D. ( 1.27 M )
12
1059At ( 80 C, ) the vapour pressure of pure benzene is ( 753 mathrm{mm} ) Hg and of pure toluene ( 290 mathrm{mm} ) Hg. Calculate the composition of a liquid in mole per cent which at ( 80 C ) is in equilibrium with the vapour containing 30 mole per cent of
benzene.
12
1060The sum of mole fractions of solute and
solvent of a solution is equal to:
A. number of moles of solute
B. number of moles of solvent
c. number of moles of solution
D. unity
12
1061Percentage of ( K_{2} S O_{4} ) in the sample is:
A . ( 65.75 % )
в. 72 %
( c .60 .35 % )
D. 78.74 %
12
1062The molarity of a glucose solution containing 36 g of glucose per ( 400 mathrm{mL} ) of the solution is:
A . 1.0
B. 0.5
c. ( 2 . )
D. 0.05
12
1063What is the vapour pressure of the solution containing ( 34.2 mathrm{g} ) of sucrose per 100 g of water at ( 25^{circ} mathrm{C} ) ? The vapour
pressure of water at ( 25^{circ} mathrm{C} ) is ( 23.75 mathrm{mm} )
( A cdot 20.3 mathrm{mm} )
B. 23.10 mm
c. Unpredictable
D. 23.33 mm
12
1064For a given value of degree of dissociation,which of the following have correct Van’t Hoff factor?
This question has multiple correct options
A. ( N a C l, i=2+alpha )
в. ( C aleft(N O_{3}right)_{2}, i=1+2 alpha )
C . ( K_{4}left[F e_{3}(C N)_{6}right], i=1+4 alpha )
D. ( left(N H_{3}right)_{3} P O_{4}, i=3+alpha )
12
1065( Y ) molal solution of a compound in benzene has mole fraction of solute
equal to ( 0.2 . ) The value of ( ? )
A . 14
B. 3.
c. 1.4
D. 2
12
1066Illustration 2.148 When dehydrated fruits and vegetables
form. Why? Would a temperature increase accelerate the
process? Explain.
12
1067Illustration 2.105 What is an antifreeze?12
1068The vapour pressure of pure water at
( 26^{circ} mathrm{C} ) is 25.21 torr. The vapour pressure
of a solution which contains 20.0 g glucose, ( C_{6} H_{12} O_{6}, ) in 70 g water is :
A .22 .5 torr
B . 23.4 torr
c. 24.4 torr
D. 24.5 torr
12
1069A solution is prepared by dissolving ( 5.64 mathrm{g} ) of glucose in ( 60 mathrm{g} ) of water. Calculate the mole fraction of
each of glucose and water respectively.
B. 0.009, 0.991
c. 1.12,0.08
D. 0.789, 0.211
12
1070The vapour pressure of two miscible
liquids ( (A) ) and ( (B) ) are 300 and
( 500 m m ) of ( H g ) respectively. In a flask 10 mole of ( (A) ) is mixed with 12 mole
of ( (B) . ) However, as soon as ( (B) ) is added, ( (A) ) starts polymerising into a completely insoluble solid. The polymerisation follows first-order kinetics. After 100 minute, 0.525 mole of a solute is dissolved which arrests
the polymerisation completely. The final vapour pressure of the solution is
400 mm of ( H g . ) Estimate the rate
constant of the polymerisation reaction. Assume negligible volume change on mixing and polymerisation and ideal behaviour for the final solution.
A . ( 1.3 times 10^{-2} )
B . ( 15 times 10^{-3} )
c. ( 2.0 times 10^{-4} )
D. ( 1.0 times 10^{-4} )
12
1071The vapour pressure of water at ( 293 mathrm{k} ) is 2438 Pa and the vapour pressure of an aqueous solution is 2395.8 Pa. If
solution density is ( 1080 mathrm{kg} / mathrm{m}^{3} ) at ( 313 mathrm{K} )
Calculate the osmotic pressure at 313
K. The molecular weight of solute =60.
A .24 .54 Pa
B . ( 24.54 times 10^{5} ) Pa
c. 0.955 Pa
D. None of these
12
1072The b.p. of a solution of ( 5 g ) of sulphur in
100g of carbon disulphide is ( 0.476^{circ} )
above that of pure solvent. Determine
the moles of sulphur in this solvent. The
b.p. of pure carbon disulphide is
( 46.30^{circ} mathrm{C} ) and its heat of vaporation is
84.1 calories per gram.
12
1073Illustration 2.122 1 g of monobasic acid in 100 g of
water lowers the freezing point by 0.168º. If 0.2 g of same
acid requires 15.1 mL mol-l of N/10 alkali for complete
neutralization, calculate the degree of dissociation of acid.
K for H,O is 1.86 K mol-1 kg.
12
1074| Example 2.16 A tube of uniform cross-sectional area 1
cm2 is closed at one end with semi-permeable membrane. A
solution of 5 g glucose per 100 mL is placed inside the tube
and is dipped in pure water at 27°C. When equilibrium is
established, calculate:
a. The osmotic pressure of solution.
b. The height developed in vertical column.
Assume the density of final glucose solution 1 g mL-1
12
1075A solution contains ( 20 % ) solute by
weight at ( 60^{circ} mathrm{C} ). Whencooled to ( 30^{circ} mathrm{C} )
the solution contains ( 10 % ) solute by
weight. When ( 45 g ) solution is cooled
from ( 60^{circ} mathrm{C} ) to ( 30^{circ} mathrm{C} ), the mass of solute
deposited is:
12
1076Question 11. Why do gases always tend to be less soluble in liquids as
the temperature is raised?
Consider the heat exchange during dissolution of gases in liquids and
give answer on the basis of Le-Chatelier’s principle.
12
1077The moles of ( B aleft(N O_{3}right)_{2} ) which on
dissolving in 12 moles of water lowers the vapour pressure of water to ( 80 % ) are
12
1078A mixture of hydrogen and oxygen contains ( 20 % ) by mass of hydrogen. What is the total number of molecules
present per gram of the mixture?
12
1079Which of the following aqueous solutions has the highest boiling point?
A ( .0 .1 mathrm{M} ) К ( mathrm{NO}_{3} )
В. ( 0.1 mathrm{M} ) Na ( _{3} mathrm{PO}_{4} )
c. ( 0.1 mathrm{M} ) ВаСг
D. ( 0.1 mathrm{M} mathrm{K}_{2} mathrm{SO}_{4} )
12
1080A solution of ( X Y(100 % ) ionised has osmotic pressure equal to four times
the osmotic pressure of ( 0.01 mathrm{MBaCl}_{2} ) 100% ionised ). Find the molarity of ( boldsymbol{X} boldsymbol{Y} )
A ( cdot 6 times 10^{-2} M )
В. ( 3 times 10^{-2} M )
c. ( 4 times 10^{-2} M )
D. ( 12 times 10^{-2} M )
12
1081The depressions in freezing point for ( 1 mathrm{m} ) urea, ( 1 mathrm{m} ) glucose and ( 1 mathrm{m} ) NaCl are in
the ratio:
A .1: 2: 3
B. 3:2:2
c. 1: 1: 2
D. None of these
12
1082(Molarity/Molality) is the number of moles of solute dissolved
per kg of solvent.
12
1083For an ideal solution containing a nonvolatile solute, which of the followig expressions represents the vapour
pressure of the solution? ( left(x_{1} rightarrowright. ) mole fraction of solvent
A ( . p=x_{2} p_{2} )
В . ( p=x_{1} p_{2}^{*} )
c. ( p=x_{1} p_{1}^{*} )
D. ( p_{1}^{*}-p=x_{2} )
12
1084Ilustration 2.84 What happens to the vapour pressure of
water if a table spoon of sugar is added to it?
12
1085A solution containing 7 g of a solute (molar mass 210 g ( m o l^{-1} ) ) in 350 g of acetone raised the boiling point of
acetone from ( 56^{circ} mathrm{C} ) to ( 56.3^{circ} mathrm{C} ). The value
of ebullioscopic constant of acetone in ( mathrm{K} mathrm{kg} operatorname{mol}^{-1} ) is :
A . 2.66
B. 3.15
c. 4.12
D. 2.86
12
1086A student slowly mixes salt into ( 25 mathrm{m} )
of water until no more salt dissolves in
it. The student could make more salt
dissolve in the solution by:
A. cooling it
B. evaporating it
c. heating it
D. stirring it
12
1087( R H_{2} ) (ion exchange resin) can replace
( C a^{2+} ) ions in hard water as: ( R H_{2}+ )
( C a^{2+} rightarrow R C a+2 H^{+} )
If ( 1 L ) of hard water after passing through
( R H_{2} ) has ( p H=3, ) then hardness in parts
per million of ( C a^{2+} ) is:
A. 80
B. 10
( c cdot 40 )
D. 100
12
1088A mixture of ( N a O H ) and ( M g(O H)_{2} )
weights 2.325 g. It requires 3 g of ( H_{2} S O_{4} ) for its neutralization. What is
the percentage composition of mixture?
12
1089Van’t Hoff factor of ( 0.01 M B a C l_{2} ) is
1.98, percentage dissociation of ( B a C l_{2} )
on this concentration will be:
( mathbf{A} cdot 69 )
в. 100
c. 49
D. 98
12
1090Vapour pressures of pure acetone and
chloroform at ( 328 K ) are 741.8 mm ( H g )
and 632.8 mm ( H g ) respectively. Assuming that they form ideal solution over the entire range of composition,
plot ( boldsymbol{p}_{text {total}}, boldsymbol{p}_{text {chloroform}}, ) and ( boldsymbol{p}_{text {acetone}} ) as a
function of ( x_{text {acetone}} . ) The experimental
data observed for different
compositions of mixture is:
100x ( x_{text {acetone }} ) What is and
( P_{text {actone}} / m m H g ) 54
( P_{text {chloro}} ) of or ( / m m ) ( H g ) 632.8 548.1
Plot this data also on the same graph paper. Indicate whether it has positive
deviation or negative deviation from the
ideal solution.
12
1091Osmotic pressure of the solution obtained by dissolving ( 100 g m ) of an organic compound in 1 litre solution is ( 2.414 times 10^{5} frac{N}{m^{2}} ) at ( 298 K . ) The organic compound can be:
A. glucose
B. urea
c. maltose
D. Nacl
12
1092Q. 26 What is the difference between molality and molarity?12
1093( 200 mathrm{mL} ) of an aqueous solution of a protein contains its 1.26 g. The osmotic pressure of this solution at ( 300 mathrm{K} ) is
found to be ( 2.57 times 10^{-3} ) bar. The molar
mass of protein will be:
( left(boldsymbol{R}=mathbf{0 . 0 8 3} boldsymbol{L} boldsymbol{b a r} boldsymbol{m o l}^{-1} boldsymbol{K}^{-1}right) )
( A cdot 61038 ) g mol ( ^{-1} )
B. 51022 g mol-1
C. ( 122044 mathrm{g} mathrm{mol}^{-1} )
D. 31011 g mol-
12
1094A binary liquid solution is prepared by mixing n-heptane and ethanol. Which one of the following statement is correct regarding the behavior of the solution?
A. The solution formed is an ideal solution
B. The solution is non-ideal, showing +ve deviation from Raoults Law
c. The solution is non-ideal, showing ve deviation from Raoults Law
D. n-heptane shows +ve deviation while ethanol shows ve deviation from Raoults Law
12
1095The ( boldsymbol{K}_{s p} ) for ( boldsymbol{C r}(boldsymbol{O H})_{3} ) is ( 1.6 times 10^{-30} )
The solubility of this compound in water
is:
( mathbf{A} cdot 4 sqrt{1.6 times 10^{-30}} )
в. ( 4 sqrt{1.6 times 10^{-30} / 27} )
c. ( 1.6 times 10^{-9} )
D. ( 2 sqrt{1.6 times 10^{-30}} )
12
1096A complex is represented as ( C o C l_{3} )
( X N H_{3} . ) Its 0.1 molal solution in water
shows ( Delta T_{f}=0.558^{circ} C . K_{f} ) of ( H_{2} O ) is
( 1.86 mathrm{K} / mathrm{m} . ) Assuming ( 100 % ) ionisation,
the number of ( N H_{3} ) molecules
associated with Co is:
12
1097A china dish weighs 25 g when empty. When a saturated solution of
potassium chloride is poured into it at ( 40^{circ} mathrm{C}, ) the weight of the dish is 63 g. When the solution is totally evaporated, the chine dish along with the crystals weighs 40 g. Find the solubility of potassium chloride at ( 40^{0} mathrm{C} )
A . 35
B. 65.2
c. 39.5
D. 7.5
12
1098Calculate the concentration of solution
which contains 5 g of salt dissolved in 100 g water
A . 5.26
B. 9.52
( c cdot 4.54 )
D. 4.76
12
1099For the two compounds, the vapour
pressure of (2) at a particular temperature is expected to be:-
( (i) )
(ii)
A. Higher than (i)
B. Lower than that of (i)
c. Same as that of (i)
D. Can be ‘higher or lower depending upon the size of the vessel
12
1100A decimolar solution of potassium ferrocyanide is ( 50 % ) dissociated at 300
K. Calculate the osmotic pressure of the
solution.
12
1101The density of lake water is 1.3 g/cc. and
it contains 69 g of ( N a^{+} ) ions per kg of
water. What is molality of ( N a^{+} ) ion in the lake?
( A cdot 1 m )
B. 3 ( m )
( c cdot 2 m )
D. ( 4 mathrm{m} )
12
1102The mole fraction of benzene in a
solution containing ( 39 % ) by mass in an organic solvent of molecular mass 122
is :
A . 0.5
B. 0.6
( c .0 .4 )
D. 0.35
12
1103The largest value of Henry’s law
constant for the liquid solvent ( mathrm{H}_{2} mathrm{O} ) will
be obtained with …………… gas as the solute
and a temperature of ( ldots )
A. ( C_{2} H_{4}, 45 )
B. ( A r, 11 )
с. ( H C l, 49 )
D. ( C O_{2}, 32 )
12
1104What is the degree of hardness of a
sample of water containing 24 mg of
( M g S O_{4}(text { mol. mass } 120) ) per kg of water?
A . 10 pp
в. 15 ррт
c. 20 ppm
D. 25 ppm
12
1105Example 2.6 A certain solution of 1 m benzoic acid in
benzene has a freezing point of 3.1°C and a normal boiling
point of 82.6°C. The freezing point of benzene is 5.5°C and
its boiling point is 80.1°C. Analyze the state of the solute
(benzoic acid) at two temperatures and comment.
12
1106A current of dry air was passed through a series of bulbs containing 1.25 g of a solute ( A_{2} B ) in 50 g of water and then through pure water. The loss in mass of the former series of bulbs was 0.98 g and in the later series 0.01 g. If the molar
mass of ( A_{2} B ) is ( 80, ) the degree of
dissociation of ( A_{2} B ) is (divide answer by ( 10): )
12
1107A maxima or minima obtained in the
temperature composition curve of a mixture of two liquids indicates:
A. an azeotropic mixture
B. an eutectic formation
c. that the liquids are immiscible with one another
D. that the liquids are partially miscible at the maximumm or minimum
12
1108Addition of which of the following material to water does not make it
hard?
( mathbf{A} cdot M g_{3}left(P O_{4}right)_{2} )
B. ( operatorname{Fe}left(mathrm{NO}_{3}right)_{3} )
c. ( Vleft(N O_{3}right)_{3} )
D. ( T ileft(C l O_{4}right)_{4} )
12
1109The mole fraction of water in ( 98 % ) (w/w)
( H_{2} S O_{4} ) solution is :
A . ( 0 . )
B. 0.9
( c cdot 0.8 )
D. 0.02
12
1110Ice skating can be used to demonstrate that when ice is under pressure, its:
A. Melting point remains unchanged
B. Melting point is raised
c. Melting point is lowered
D. coefficient of friction with metal is reduced
12
1111The osmotic pressure of equimolar
solutions of urea, ( B a C l_{2} ) and ( A l C l_{3} ) will
be in the order of:
A ( cdot A l C l_{3}>U r e a>B a C l_{2} )
в. Urea( >B a C l_{2}> )АlСl( _{3} )
c. ( A l C l_{3}>B a C l_{2}>U r e a )
D. ( B a C l_{2}>A l C l_{3}>U r e a )
12
1112The Van’t Hoff’s factor ( ^{prime} boldsymbol{i}^{prime} ) accounts for:
A. extent of dissolution of solute
B. extent of mobility of solute
c. extent of solubility of solute
D. extent of dissociation of solute
12
1113Assertion
The solubility of a solid in a liquid increases with increase of pressure.
Reason

Solubility of gas in a liquid is directly proportional to the pressure of the gas.
A. Both Assertion and Reason are correct and Reason is the correct explanation for Assertion
B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion
c. Assertion is correct but Reason is incorrect
D. Both Assertion and Reason are incorrect

12
1114Which of the following equimolar solution have highest vapour pressure?
A. Glucose
B. ( N a C l )
c. ( K_{2} S O_{4} )
D. ( K_{4} ) Fe ( (C N)_{6} )
12
1115Example 2.31 Calculate the Van’t Hoff factor when 0.1 mol
NH,Cl is dissolved in 1 L of water. The degree of dissociation
of NH 1,Cl is 0.8 and its degree of hydrolysis is 0.1.
12
1116Example 2.18 2.5 g of a substance is present in 200 mL of
solution showing the osmotic pressure of 60 cm Hg at 15°C.
Calculate the molecular weight of substance. What will be
the osmotic pressure if temperature is raised to 25°C?
12
1117The vapour pressure of a solvent
decreased by ( 10 mathrm{mm} ) of mercury when a
non-volatile solute was added to the
solvent. The mole fraction of the solute
in the solution is ( 0.2 . ) What should be the mole fraction of the solvent, if the
decrease in the vapour pressure is to be
20 mm of mercury?
A . 0.8
B. 0.6
( c .0 .4 )
D. 0.2
12
1118Dissolving 120 gm of a compound of (mol.wt. 60 ) in 1000 g of water gave a solution of density ( 1.5 mathrm{g} / mathrm{mL} ). The molarity of the solution is:
A ( .1 .00 M )
в. ( 1.78 M )
( c .2 .50 M )
D. ( 4.00 M )
12
1119A solution in which, still more number of solute can be dissolved, is known as:
A. unsaturated
B. super saturated
c. saturated
D. dilute
E. concentrated
12
1120Which one of the following statements regarding Henry’s law is not correct?
A. The value of ( K_{H} ) increases with the function of the nature of the gas
B. Higher the value of ( K_{H} ) at a given pressure, higher is the solubility of the gas in the liquids
C. The partial of the gas in vapour phase is proportional to the mole fraction of the gas in the solution
D. Different gases have different ( K_{H} ) (Henry’s law constant) values at the same temperature
12
1121Water and chlorobenzene are
immiscible liquids. Their mixture boils
at ( 89^{circ} mathrm{C} ) under a reduced pressure of
( 7.7 times 10^{4} ) Pa. The vapour pressure of
pure water at ( 89^{circ} mathrm{C} ) is ( 7 times 10^{4} mathrm{Pa} )
Weight percent of chlorobenzene in the distillate is:
A . 50
B. 60
c. 79
D. 38.46
12
1122The Henry’s law constant for the
solubility of ( N_{2} ) gas in water at ( 298 K ) is
( 1.0 times 105 ) atm. The mole fraction of ( N_{2} )
in air is ( 0.8 . ) The number of moles of ( N_{2} )
from air dissolved in 10 moles of water
at ( 298 K ) and 5 atm pressure is
A ( cdot 4 times 10^{-4} )
B . ( 4 times 10^{-5} )
( mathbf{c} cdot 5 times 10^{-4} )
D. ( 4 times 10^{-6} )
12
1123Equimolal solutions ( A ) and ( B ) show depression in freezing point in the ratio
2:1. A remains in the normal state in
solution B will be :
A. Normal in solution
B. Dissociated in solution
C. Associated in solution
D. Hydrolysed in solution
12
1124Match the mixture given in column with the corresponding type of solutions given in column II12
1125A solution containing 0.2563 g of naphthalene (molecular mass = 128) in ( 50 mathrm{g} ) of carbon tetrachloride yields a boiling point elevation of ( 0.201^{circ} mathrm{C} ) while a solution of 0.6216 g of an unknown solute in the same mass of the solvent
gives a boiling point elevation of
( 0.647^{circ} mathrm{C} . ) Find the molecular mass of
the unknown solute.
12
1126State True or False.
For two solutions to be isotonic, ( boldsymbol{C}_{mathbf{1}}= )
( C_{2} ) in all the cases.
A. True
B. False
12
1127Illustration 2.198 1575.2 g of C,H,OH (phenol) is dissolved
in 960 g of a solvent of K. = 14 K kg mol-1. If the depression
in freezing point is 7 K, then find the percentage of phenol
that dimerizes.
12
1128When ethanol mixes in cyclohexane, the intermolecular forces
reduces between ethanol molecule. In
this, liquid pair shows:
A. positive deviation from Raoult’s law
B. negative deviation from Raoult’s law
c. no deviation from Raoult’s law
D. decrease in volume
12
1129Which condition is not satisified by an
ideal solution?
A ( cdot Delta H_{operatorname{mixing}}=0 )
B. ( Delta V_{text {mixing}}=0 )
C. ( Delta S_{text {mixing}}=0 )
D. obeyance of Raoult’s law
12
1130To what temperature should water be
heated so that its vapor pressure
equals the vapor pressure chloroform at
( 40^{circ} mathrm{C} ? )
( mathbf{A} cdot 40^{circ} C )
( mathbf{B} cdot 50^{circ} C )
( mathbf{c} cdot 60^{circ} C )
D. ( 70^{circ} mathrm{C} )
( E cdot 80^{circ} C )
12
1131Illustration 2.63 What are maximum boiling azeotropes?
Give one example.
12
1132In an ideal solution of non-volatile
solute ( mathrm{B} ) in solvent ( mathrm{A} ) in 2: 5 molar ratio
has vapour pressure ( 250 mathrm{mm} ). If another solution in ratio 3: 4 prepared then vapour pressure above this solution is:
( A cdot 200 mathrm{mm} )
B. 250 mm
c. 350 ( mathrm{mm} )
D. ( 400 mathrm{mm} )
12
1133( 0.2 g ) of fine animal charcoal is mixed
with half litre of acetic acid ( (2 M) )
solution and shaken for 30 minutes?
A. Concentration remains same
B. Concentration increases
c. concentration of the solution decreases
D. None of above
12
1134The vapour pressure of water is ( 12.3 k P a ) at ( 300 K . ) Calculate the vapour
pressure 1 molal solution of a non-
volatile solute in it
( mathbf{A} cdot 12.08 k P a )
B. 1.208 Ppa
( mathrm{c} .2 .4 mathrm{kPa} )
D. ( 0.4 k P a )
12
1135Which of the following pairs of solutions are expected to be isotonic, temperature being the same?
A ( cdot 0.1 mathrm{M} ) glucose and ( 0.1 mathrm{M} mathrm{C}_{6} mathrm{H}_{5} mathrm{N}^{+} mathrm{H}_{3} mathrm{Cl} )
B. ( 0.1 mathrm{M} ) NaCl and ( 0.05 mathrm{M} ) BaCl ,
c. ( 0.1 mathrm{M} mathrm{Na}_{2} mathrm{SO}_{4} ) and ( 0.1 mathrm{M} mathrm{KNO} )
D. ( 0.1 mathrm{M} ) BaCl( _{2} ) and ( 0.075 mathrm{M} ) FeCl( _{3} ),
12
1136Two liquids ( A ) and ( B ) form a non ideal
solution which obey the equation:
( boldsymbol{P}_{boldsymbol{T}}+boldsymbol{P}_{boldsymbol{A}}^{boldsymbol{o}}+boldsymbol{3}left(boldsymbol{P}_{boldsymbol{B}}^{boldsymbol{o}}-boldsymbol{P}_{boldsymbol{A}}^{boldsymbol{o}}right) boldsymbol{X}_{boldsymbol{B}}+boldsymbol{2}left(boldsymbol{P}_{boldsymbol{A}}^{boldsymbol{o}}-right. )
( left.P_{B}^{o}right) X_{B}^{2} )
When an equimolar mixture of ( A ) and ( B ) is distilled, find the composition (by mole) when this mixture will have a
single boiling point.
( left(P_{B}^{o}>P_{A}^{o}right) ) where ( P_{A}^{o} ) and ( P_{B}^{o} ) are vapour
pressure of pure ( A ) and ( B ) respectively
and ( X_{B}= ) is the mole fraction of ( B ) in
the liquid phase.
A. 3:
B. 2:3
c. 1: 2
D. 1: 3
12
11373 moles of ( boldsymbol{P} ) and 2 moles of ( boldsymbol{Q} ) are
mixed, what will be their total vapour pressure in the solution if their partial
vapour pressures are 80 and 60 torr respectively?
A. 80 torr
B. 140 torr
c. 72 torr
D. 70 torr
12
1138The ppm strength of ( C O_{2}(g) ) volume by
volume ( left(mathrm{mL} text { of } C mathrm{O}_{2} text { per } 10^{6} mathrm{mL} ) of air) is: right.
A .224
в. 2240
c. 100
D. 1000
12
1139( mathbf{A} mathbf{5} . mathbf{8 5} %(mathbf{w} mathbf{t} / mathbf{v} text { ol }) mathbf{N} boldsymbol{a} boldsymbol{C l} ) solution will
exert an osmotic pressure closet to which one of the following.
A. ( 5.85 % ) (wt/vol) sucrose solution
B. ( 5.85 % ) (wt/vol) glucose solution
c. 2 m sucrose solution
D. ( 1 mathrm{m} ) glucose solution
12
1140( 16.0 mathrm{g} ) of NaOH is present in ( 100 mathrm{ml} ) of an aqueous solution. Its density is 1.06 g/ml. Mole fraction of the solute is approximately:
( mathbf{A} cdot 25 / 27 )
B. 2 /27
c. ( 1 / 27 )
D. ( 26 / 27 )
12
1141A solution of acetone is ethanol:
A. shows a negative deviation from Raoult’s law
B. shows a positive deviation from Raoult’s law
C. behaves like a near ideal solution
D. obeys Raoult’s law
12
1142Illustration 2.175 A solution of an organic compound is
prepared by dissolving 30 g in 100 g water. Calculate the
molecular mass of compound and the osmotic pressure of
solution at 300 K, when the elevation in boiling point is 0.52
and K, for water is 0.52 K m-1.
12
1143The molality ( (mathrm{m}) ) of each ion ( left(mathrm{N} boldsymbol{H}_{4}^{+} ) and right.
( left.C l^{-}right), ) respectively, present in the
aqueous solution of ( 2 M N H_{4} C l )
assuming ( 100 % ) dissociation according to given reaction is,
( N H_{4} C l(a q) rightarrow N H_{4}^{+}(a q)+C l^{-}(a q) )
Given that density of solution ( =3.107 )
( mathrm{g} / mathrm{ml} )
A ( .0 .45 mathrm{m}, 0.67 mathrm{m} )
в. ( 0.67 mathrm{m}, 0.45 mathrm{m} )
( c .0 .67 m, 0.67 m )
( m )
D. ( 0.45 mathrm{m}, 0.45 mathrm{m} )
12
1144( mathbf{A} )
0.1 molar solution of ( N a C l ) is found
to be isotonic with ( 1 % ) urea solution.
Calculate
(a) Van’t Hoff factor
(b)Degree of dissociation of sodium
chloride.

Assume density of ( 1 % ) urea equal to
( 1 g c m^{-3} )
( begin{array}{ll}text { A. }(a) & 1.667, text { (b) } 0.667end{array} )
В. (а) ( 1.82, ) (b) 0.69

12
1145The azeotropic solutions of two
miscible liquids:
A. can be separated by simple distillation
B. are supersaturated solutions
C. behave like a single component and boil at a constant temperature
D. none of the above
12
1146The total pressure when this drop formed in torr is12
1147The osmotic pressure of equimolar
solutions of ( mathrm{BaCl}_{2}, ) NaCl and glucose will
be in the order:
A ( . ) glucose ( >N a C l>B a C l_{2} )
в. ( B a C l_{2}>N a C l> ) glucose
c. ( N a C l>B a C l_{2}>g l u operatorname{cose} )
D. ( N a C l>g l u c o s e>B a C l_{2} )
12
1148Which of the following combinations of ( 0.20 M ) aqueous solutions will form a precipitate on mixing?
I. ( A g N O_{2} ) and ( H C l )
Il. ( B a C_{2} H_{2} O_{2} ) and ( M g S O_{4} )
III. ( boldsymbol{K} boldsymbol{I} ) and ( boldsymbol{P b}left(boldsymbol{N} boldsymbol{O}_{3}right)_{2} )
A. I only
B. I and II only
c. I and III only
D. II and III only
E . ।, II, and III
12
1149Saturated solution of NaCl on heating:
A. becomes supersaturated
B. becomes unsaturated
c. remains saturated
D. vaporises
12
1150Calculate the molality of 1 litre solution
containing ( 93 % H_{2} S O_{4}(W / V) ) if the
density of the solution is ( 1.84 g m L^{-1} )
12
1151The elevation in boiling point of a
solution of 13.44 g of ( C u C l_{2} ) (Molar mass 134.4 ) in ( 1 mathrm{kg} ) water is:
( left[boldsymbol{K}_{boldsymbol{b}}=mathbf{0 . 5 2} mathrm{K} text { molality }^{-1}right] )
A . 0.16
B. 0.05
c. ( 0 . )
D. 0.2
12
1152The weight (in-grams) of ( A g N O_{3} ) present in ( 100 mathrm{ml} ) of ( 0.25 mathrm{M} ) solution:
A . 4.25
B. 2
c. 17
D. 1.
12
1153( 33.6 mathrm{L} ) of water vapour at STP are condensed to liquid state. The volume occupied by it is approximately:
A . ( 1 mathrm{mL} )
B. 18 mL
c. 27 ( mathrm{mL} )
D. 127 mL
12
1154The vapour pressure of pure benzene is
( 639.7 mathrm{mm} mathrm{Hg} ) and the vapour pressure of a solution of a solute in benzene at the
temperature is ( 631.9 mathrm{mm} ) Hg. If the
molality of the solution is ( 156 times 10^{-x} )
then what is the value of ( x ? )
12
1155To cool a liquid just below its f.pt. is
called super cooling.
If true enter 1 , if false enter 0 .
12
1156A ( 10 % ) solution of ( N a C l ) means that in
( 100 g ) of solution there is:
A. ( 5.85 g ) NaCl
в. ( 58.5 g ) NaCl
c. ( 10 g ) NaCl
D. ( 94 g ) NaCl
12
1157Illustration 2.37 At 20°C, the vapour pressure of pure
liquid A is 22 mm Hg and that of pure liquid B is 75 mm
Hg. What is the composition of the solution of these two
components that has vapour pressure of 48.5 mm Hg at this
temperature?
12
1158Hlustration 2.127 Addition of 0.40 g of a compound to
45.5 mL of benzene (density 0.879 g mL-1) lowers the freezing
point from 5.51°C to 4.998°C. If K, for benzene is 5.12 K kg
mol-1, calculate the molar mass of the compound.
12
1159The vapour pressure of water at ( 23^{circ} C ) is ( 19.8 mathrm{mm} .0 .1 mathrm{mole} ) glucose is dissolved in ( 178.2 mathrm{g} ) water. What is the vapour pressure (in ( mathrm{mm} ) ) of the resultant solution?
( A cdot 19 )
B. 19.602
c. 19.402
D. 19.202
12
1160Match the following
Column – I Column – II
a) A nearly ideal solution
p) ( H_{2} O+ )
[
C_{2} H_{5} O H
]
b) A solution
q) ( C_{6} H_{6}+ ) showing positive deviation ( quad C_{6} H_{5} C H_{3} )
c) A solution
r) ( C_{6} H_{6}+C H C l_{3} )
showing negative deviation
s) ( C H_{3} C O C H_{3}+ )
d) An azeotropic mixture
[
C_{2} H_{5} O H
]
( t )
( Delta H ) and ( Delta V ) are
positive
and ( Delta V )
( Delta H )
u) are negative
( mathbf{A} cdot mathrm{A}-mathrm{q} ; mathrm{B}-mathrm{s}, mathrm{t} ; mathrm{C}-mathrm{r}, mathrm{u} ; mathrm{D}-mathrm{p} )
B. ( A-s ; B-s, t ; C-r ; D-q, p )
( mathbf{C} cdot A-q ; B-s ; C-r ; D-p, t )
D. ( A-r ; B-p ; C-s, t ; D-q )
12
1161The density of ( 3 M ) solution of ( N a C l ) is
( 1.25 g m l^{-1} . ) The molality of the solution
is:
A ( .2 .79 mathrm{m} )
В. 1.79 m
c. ( 3.5 mathrm{m} )
D. 5.58 m
12
1162What is molal elevation constant? Drive
its equation and give its unit.
12
1163Solutions which distill without change in composition or temperature are called:
A. amorphous
B. azeotropic mixture
c. ideal
D. super saturated
12
1164The van’t Hoff factor for ( 0.1 M ) barium
nitrate is ( 2.74 . ) The percentage of dissociation of barium nitrate is:
A . ( 91.3 % )
B. ( 87 % )
c. ( 100 % )
D. ( 74 % )
12
1165Assertion
The molecular weight of acetic acid determined by depression in freezing point method in benzene and water was found to be different.
Reason
Water is polar and benzene is non-polar.
A. Both Assertion and Reason are correct and Reason is the correct explanation for Assertion
B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion
c. Assertion is correct but Reason is incorrect
D. Assertion is incorrect but Reason is correct
12
1166Dissolving ( 120 g ) of urea in ( 1000 g ) of water gave a solution of density ( mathbf{1 . 1 5} g / boldsymbol{m} boldsymbol{L} . ) The molarity of the solution is:
A ( .1 .79 M )
в. ( 2 M )
( c .2 .05 M )
D. 2.22 ( M )
12
1167Relative lowering of vapour pressure is maximum for:
A. ( 0.1 mathrm{m} ) urea
B. 0.1m Nacı
( mathbf{c} cdot 0.1 m quad M g C I_{2} )
D. ( 0.1 m quad A I_{2}left(S O_{4}right)_{3} )
12
1168Calculate the molarity of each of the following solutions:
(a) ( 30 g ) of ( C oleft(N O_{3}right)_{2} cdot 6 H_{2} O ) in ( 4.3 mathrm{L} ) of
solution
(b) ( 30 mathrm{mL} ) of ( 0.5 mathrm{M} H_{2} S O_{4} ) diluted to 500
mL.
12
1169When 5.0 gram of ( B a C l_{2} ) is dissolved in
water to have ( 10^{6} ) gram of solution. The concentration of a solution is:
A . 2.5 ppm
в. 5 ррт
( c .5 M )
D. ( 5 g L^{-1} )
12
1170Question 7. A solution is obtained by mixing 300 g of 25% solution and
400 g of 40% solution by mass. Calculate the mass percentage of the
resulting solution.
(i) Calculate the masses of solute in both the solutions separately.
(ii) Find the mass of solute and solution after mixing.
(iii) And then mass % of solute and solvent in the resulting solution.
25
12
1171Calculate the molality of 1 L solution of
( 93 % H_{2} S O_{4} ) (weight/volume). The
density of the solution is 1.84 g. (If the answer is ( x, text { then find }[x]) )
12
1172The elevation in boiling point of a
solution ( d T_{b} ) is related with molality of
solution ( (mathrm{m}) ) by the relation:
( boldsymbol{d} boldsymbol{T}_{boldsymbol{b}}=left[frac{boldsymbol{R} boldsymbol{T}_{boldsymbol{b}}^{2}}{boldsymbol{Delta} boldsymbol{H}_{boldsymbol{v a p}}}right]left[frac{boldsymbol{M}_{mathbf{1}}}{mathbf{1}+boldsymbol{m} boldsymbol{M}_{mathbf{1}}}right], ) where
( M_{1} ) is molar mass of solvent and ( Delta boldsymbol{H}_{boldsymbol{v} boldsymbol{a} boldsymbol{p}} )
is heat of vaporisation of solvent. For a dilute solution, the relation ( left(frac{partial T_{b}}{partial m}right)_{m rightarrow 0} )
gives:
A. molal ebullioscopic constant
B. elevation in boiling point
C. elevation in boiling point ( partial T_{b} ) becomes more predominant
D. boiling point of solvent
12
1173The solution which has the highest boiling point temperature is:
( begin{array}{lll}text { A. } 0.1 & M & M g C l_{2}end{array} )
( begin{array}{lll}text { В. } 0.1 & M & H C l O_{4}end{array} )
( begin{array}{llll}text { c. } 0.1 & M & N H_{4} O Hend{array} )
( begin{array}{lll}text { D. } 0.1 & M & text { KOH }end{array} )
( begin{array}{lll}text { E. } 0.1 & M & L i N O_{3}end{array} )
12
117401 M solution of glucose, the depression is
freezing point of a 0.01 M MgCl2 solution is
(a) the same
Thinking Process
Calculate value of van’t Hoff factor then correlate it with colla
solution
e it with colligative property of given
12
1175What will be the molality of the solution containing 18.25 g of ( H C l ) gas in 500 g of water?
( mathbf{A} cdot 0.1 mathrm{m} )
B. ( 1 mathrm{m} )
c. ( 0.5 mathrm{m} )
D. 2 ( m )
12
1176The vapour pressure of water is ( 92 mathrm{mm} ) at ( 323 mathrm{K} .18 .1 mathrm{g} ) of urea are dissolved in 100g of water. The vapour pressure is
reduced by ( 5 mathrm{mm} ). Calculate the molar
mass of urea.
12
1177If in the fermentation of sugar in an
enzymatic solution that is ( 0.2 M ), the
concentration of the sugar is reduced to ( 0.06 M ) in ( 10 h ) to ( 0.03 M ) in ( 20 h, ) what
is the order of the reacation:
A . 1
B. 2
( c .3 )
D.
12
1178Van’t-Hoff factor(i) for this reaction is:
A .2
B.
( c )
( D )
12
1179Lowering in vapour pressure is highest
for:
A. ( 0.2 m ) urea
B. ( 0.1 m ) glucose
c. ( 0.1 m ) M ( g S O_{4} )
D. ( 0.1 m B a C l_{2} )
12
1180( mathbf{A} )
42 molal solution of sodium chloride
in water causes an elevation in the
boiling point of water by ( 1.88 mathrm{K} ). What is
the value of Van’t Hoff factor? What does
it signify? ( left[boldsymbol{K}_{boldsymbol{b}}=mathbf{0 . 5 2} boldsymbol{K} mathbf{k g} boldsymbol{m o l}^{-mathbf{1}}right] )
12
1181Enough ( N a_{2} S O_{4} ) is dissolved in water
at ( 40^{circ} C ) to saturated the solution. When
this occurs heat is given off. All of the following statements are true EXCEPT:
A. The enthalpy change of this process is negative
B. The boiling point of the solution is higher than that of pure water
C. The freezing point of the solution is lower than that of pure water
D. If the temperature of the water is lowered, then the solubility of ( N a_{2} S O_{4} ) decreases
12
1182By dissolving 0.35 mole of sodium
chloride in water, ( 1.30 l ) of salt solution
is obtained. The molarity of the resulting solution should be reported
as:
A . 0.3
B. 0.269
c. 0.27
D. 0.2692
12
1183When ( 400 g ) of a ( 20 % ) Solution was
cooled ( 50 g ) of the solute precipitated. What is the percent concentration of the
remaining solution.
12
1184The number of moles of ( C O_{2} ) that can be
dissolved in a liter of water increases
when the
(1) pressure of the ( C O_{2} ) is increased
(2) temperature of the water is increased
(3) liquid is stirred
A. If 1,2 and 3 are correct
B. If only 1 and 2 are correct
c. If only 2 and 3 are correct
D. If only 1 is correct
E. If only 3 is correct
12
1185The concentration of a solution is ( 8 % )
( (w / w) ) and ( 10 %(w / v) . ) Calculate density ( (text { in } g / m l) ) of solution.
12
1186If for a sucrose,elevation in boiling point
is ( 1.0^{circ} mathrm{C} ),then what will be the boiling
point of ( N a C l ) solution for same molal concentration?
( mathbf{A} cdot 1.0^{circ} mathrm{C} )
B . ( 2.0^{circ} mathrm{C} )
( mathbf{c} cdot 3.0^{circ} mathrm{C} )
D. ( 4.0^{circ} mathrm{C} )
12
1187Calculate the concentration of nitric
acid in moles per litre in a sample
which has a density. 1.41 g ( m L^{-1} ) and the mass per cent of nitric acid in it being ( 69 % )
12
1188Average osmotic pressure of human
blood is 7.4 at ( m ) at ( 27^{circ} C, ) then total
concentration of various solutes is:
( mathbf{A} cdot 0.1 mathrm{molL}^{-1} )
B. 0.2 molL( ^{-1} )
c. 0.3 molL ( ^{-1} )
D. 0.4 molL( ^{-1} )
12
1189( D 5 W ) refers to one of the solution used
as an intravenous fluid. It is a ( 5 % ) by
mass solution of dextrose, ( C_{6} H_{12} O_{6} ) in
water. The density of ( D 5 W ) is ( 1.08 g / m l ) The molarity of the solution is
( mathbf{A} cdot 0.3 M )
в. ( 0.6 M )
c. ( 0.28 M )
D. ( 0.26 ~ M )
12
1190Which of the following pair will form an ideal solution?
A. Chlorobenzen, chloro ethane
B. Benzene, Toluene
c. Acetone, chloroform
D. water, HCl
12
1191Molarity and molality of a solution of a liquid (mol wt=50) in aqueous solution
is 9 and 10 respectively. What is the density of solution?
( mathbf{A} cdot 1 g / c c )
в. ( 0.95 g / c c )
c. ( 1.05 g / c c )
D. ( 1.35 g / c c )
12
1192In an endothermic process, solubility increases with
temperature.
( A ). increase
B. decrease
c. remains same
D. none of the above
12
1193Solubility of ( K B r ) shows slow rise in
solubility with increase in temperature
A. True
B. False
12
1194The osmotic pressure of urea solution
at ( 10^{circ} mathrm{C} ) is ( 200 mathrm{mm} ) becomes ( 105.3 mathrm{mm} )
when it is diluted and the temperature
raised to ( 25^{circ} mathrm{C} ). The extent of dilution is:
A. 8 times
B. 5 times
c. 4 times
D. 2 times
12
1195A solution contains ( 15 % ) glucose
( left[boldsymbol{C}_{6} boldsymbol{H}_{12} boldsymbol{O}_{6}right] ) in water and has density ( mathbf{1 . 5} )
( mathrm{g} / mathrm{ml} . ) Find the molarity and molality of this solution ( [boldsymbol{C}=mathbf{1 2}, boldsymbol{H}=mathbf{1}, boldsymbol{O}=mathbf{1 6}] )
12
1196Two liquids ( A ) and ( B ) form an ideal
solution at temperature ( T . ) When the
total vapour pressure above the
solution if 600 torr, the amount
fraction of ( A ) in the vapour phase is 0.40
and in the liquid phase is ( 0.6 . ) What are the vapour pressure of pure ( A ) and ( B ) at
temperature ( T ? )
12
1197Solubility of which among the following substances in water increases slightly with rise in temperature?
A. Potassium bromide
B. Potassium chlorid
c. Potassium nitrate
D. Sodium nitrate
12
119818 g glucose ( left(C_{6} H_{12} O_{6}right) ) is added to 178.2 ( g ) water. The vapor pressure of water (in torr) for this aqueous solution
is:
A . 76.0
B. 752.4
c. 759.0
D. 7.6
12
1199State True or False.
( C H C l_{3} ) and acetone mixture shows
negative deviation from Raoult’s law.
A. True
B. False
12
1200From the table given below, furnish your points of inference.
begin{tabular}{ll}
Substance & Solubility at ( 25^{circ} mathrm{C} ) \
( mathrm{NaCl} ) & ( 36 mathrm{g} ) \
( mathrm{NaBr} ) & ( 95 mathrm{g} ) \
( mathrm{Nal} ) & ( 184 mathrm{g} ) \
hline
end{tabular}
12
1201One litre of a sample of hard water ( (d=1 )
( g / m L ) contains 136 mg of ( C a S O_{4} ) and
( 190 mathrm{mg} ) of ( M g C l_{2} . ) What is the total
hardness of water in terms of ( C a C O_{3} ? )
A. 100 ppm
B. 200 ppm
c. 300 ppm
D. None of the above
12
1202Illustration 2.202 Calculate the osmotic pressure of a
solution containing 0.02 mol of NaCl and 0.03 mol of glucose
in 500 mL at 27°C.
12
1203How many milli moles of sucrose should
be dissolved in 500 gms of water so that the difference between the boiling point and freezing point of the solution
becomes ( 103.57^{circ} mathrm{C} ?left(K_{f}=right. )
( mathbf{1} . mathbf{8 6}^{circ} boldsymbol{C} / boldsymbol{m}, boldsymbol{K}_{boldsymbol{b}}=mathbf{0 . 5} mathbf{2}^{boldsymbol{o}} boldsymbol{C} / boldsymbol{m} )
A. 500 moles
B. 90 mmoles
c. 1330 mmoles
D. 1330 moles
12
1204The depression in freezing point for
( 0.01 m ) aqueous solution of
( boldsymbol{K}_{boldsymbol{x}}left[boldsymbol{F} boldsymbol{e}(boldsymbol{C} boldsymbol{N})_{boldsymbol{6}}right] ) is ( boldsymbol{0 . 0 7 4 4} boldsymbol{K} . ) The motal
depression constant for solvent is
( 1.86 K k g ) mol( ^{-1} . ) If the solute
undergoes complete dissociation, what is the correct molecular formula for the
solute?
( A cdot_{K_{2}left[F e(C N)_{6}right]} )
B ( cdot_{K_{3}}left[F e(C N)_{6}right] )
c. ( left._{Kleft[F e(C N)_{6}right.}right] )
D ( quad K_{4}left[F e(C N)_{6}right] )
12
1205The freezing point ( left(text { in }^{circ} Cright) ) of a solution
containing 0.1 g of ( K_{3}left[F e(C N)_{6}right] ) (molar ( operatorname{mass} 329) ) in 100 g of water ( left(boldsymbol{K}_{boldsymbol{f}}=right. )
1.86 ( K . k g . m o l^{-1} ) ) is :
A. ( -2.3 times 10^{-2} ) о ( C )
В. ( -5.7 times 10^{-2} ) о ( C )
c. ( -5.7 times 10^{-3} ) о ( C )
D. ( -1.2 times 10^{-2} ) о ( C )
12
1206The vapour pressure of a solvent at 293
K is 100 mm Hg. Then the vapour pressure of a solution containing 1 mole of a strong electrolyte ( left(A B_{2}right) ) in 99 moles of the solvent at ( 293 mathrm{K} ) is:
(Assume complete dissociation of solute)
A. ( 103 mathrm{mm} ) Hg
в. ( 99 mathrm{mm} ) Нв
( mathbf{c} .97 mathrm{mm} mathrm{Hg} )
D. ( 101 mathrm{mm} ) Н
12
1207Q. 47 Match the items given in Column I and Column II.
Column 1
Column II
A. Saturated solution 1 Solution having same osmotic pressure at a
given temperature as that of given solution
B. Binary solution 2. A solution whose osmotic pressure is less than
that of another
C Isotonic solution 3 Solution with two components
D. Hypotonic solution 4. A solution which contains maximum amount of
solute that can be dissolved in a given amount
of solvent at a given temperature.
E Solid solution 5. A solution whose osmotic pressure is more
than that of another.
F. Hypertonic solution 6. A solution in solid phase,
12
12080.48 Match the items given in Column I with the type of solutions given in
Column II.
Column 1
Column II
A Soda water
1. A solution of gas in solid
B. Sugar solution
2. A solution of gas in gas
C German silver
3. A solution of solld in liquid
D. Air
4. A solution of solid in solid
E Hydrogen gas in palladium 5. A solution of gas in liquid
6. A solution of liquid in solid
12
1209State Raoult’s law for the solution
containing volatile components. What is the similarity between Raoult’s law
and Henry’s law?
12
1210When ( 100 g ) of saturated solution is
evaporated at ( 50^{circ} mathrm{C}, 50 mathrm{g} ) of solid is left over. Find the solubility of the
substance at ( 50^{circ} mathrm{C} )
A . 100
B. 50
c. 75
D. 25
12
1211Illustration 2.57 Cutting onions taken from the fridge
is more comfortable than cutting those lying at room
temperature. Explain why.
12
1212A 0.004 M solution of ( N a_{2} S O_{4} ) is
isotonic with a ( 0.010 mathrm{M} ) solution of
glucose at same temperature. The apparent degree of dissociation of
( N a_{2} S O_{4} ) is:
A . ( 25 % )
B. ( 50 % )
c. ( 75 % )
D. ( 85 % )
12
1213Explain homogenous and heterogenous
conditions with an example.
12
1214The correct value for the relative
lowering of vapour pressure of a
very dilute solution is equal to:
This question has multiple correct options
A. mole fraction of solute
B. mole fraction of solvent
C. ratio of moles of solute to moles of solvent
D. ratio of moles of solvent to moles of solute
12
1215Which of the following is a type of mixture in which constituent elements
are not uniformly distributed?
A. Blood
B. Salt and water
c. Bronze
D. None of the above
12
1216Amount in g of simple containing ( 80 % ) NaOH required to prepare 60 litre of 0.5 M solution is :
A . 1000
B. 1200
( c cdot 1500 )
D. 1600
12
1217A 0.1 molal solution of a monobasic
acid is ( 45 % ) ionized. Calculate the
depression in freezing point:
(Molecular weight of the acid ( =300 )
( left.mathrm{g} / mathrm{mol}, boldsymbol{K}_{f}=mathbf{1 . 8 6} boldsymbol{K} boldsymbol{m o l}^{-1} boldsymbol{k g}right) )
A ( .–0.199^{circ} mathrm{C} )
B . ( 2.00^{circ} mathrm{C} )
( mathrm{c} cdot 0^{circ} mathrm{C} )
D. ( 0.269^{circ} mathrm{C} )
12
1218The concentration of a solution can be
expressed in molarity, normality, formality and molality. Among them, which mode of expression is the most accurate for the all conditions?
A. Molarity
B. Formality
c. Normality
D. Molality
12
1219An aqueous solution of ( 2 % ) non-volatile
solute exerts a pressure of 1.004 bar at the normal boiling point of the solvent.
What is the molecular mass of the
solute?
A ( .23 .4 mathrm{gmol}^{-1} )
B . ( 41.35 mathrm{gmol}^{-1} )
c. ( 10 mathrm{gmol}^{-1} )
D. 20.8 gmol-
12
1220Q. 60 Discuss biological and industrial applications of osmosis.12
1221Two solvent ( A ) and ( B ) have ( K_{f} ) values 1.86
and ( 2.79 mathrm{K} ) mol( ^{-1} ) kg respectively.
given amount of substance when
dissolved in 500 g of ( A, ) it completely dimerizes and when same mass of
substance is dissolved in 500 g of ( mathrm{B} ), the solute undergoes trimerization.
The ratio of observed lowering of freezing points in two cases is ( 1:(?) )
12
1222Q. 32 Which of the following binary mixtures will have same composition in
liquid and vapour phase?
(a) Benzene-toluene
(b) Water-nitric acid
(c) Water-ethanol
(d) n-hexane-n-heptane
12
1223Vapour pressure of pure benzene at any
temperature is 640 mm ( H g . ) A non volatile, non-electrolyte solid whose
weight is ( 2.75 g m, ) is added to ( 39.0 g m ) of benzene. Vapour pressure of solution is 600 mm ( H g ). Calculate the molecular weight of the solid?
12
1224Illustration 2.177 100 mL of 1.0 g sample of a drug having
compound C,H,O,N as drug is coated with sugar lactose
(mol. wt. 342) exerts the osmotic pressure of 0.70 atm at 27°C.
What is the drug percentage in sample?
12
1225If a mixture of ( O_{2} ) and ( O_{3} ) is having
( V_{r m s}=12.92 m / s ) at ( 300 K . ) Calculate
mole percentage of ( O_{2} ) in the mixture.
A. 35 %
B. 20%
c. ( 66.67 % ) %
D. none of these
12
1226Mustration 2.58
Define an ideal solution.
12
1227117 grams of ( N a C l ) are dissolved
in water to make ( 500 m L ) of
solution. Water is then added to this
solution to make a total of one liter
of solution. The final molarity of
the solution is :
( A cdot 4 M )
в. 2 М
( c cdot 1 M )
D. ( 0.5 ~ M )
E . 0.585 М
12
1228The vapour pressure of an aqueous solution is found to be 750 torrs at
certain temperature ‘T’. If ‘T’ is the temperature at which pure water boils under atmospheric pressure and same solution show elevation in the boiling
point ( Delta T_{b}=1.04 K, ) find the
atmospheric pressure?
( left[boldsymbol{K}_{boldsymbol{b}}=mathbf{0 . 5 2} boldsymbol{K} boldsymbol{k g m o l}-mathbf{1}right] )
A . 77
в. 779
( c .782 )
D. 746
12
1229( 4.6 mathrm{cm}^{3} ) of methyl alcohol is dissolved in ( 25.2 mathrm{g} ) of water. Calculate mole fraction of methyl alcohol and water. (Given density of methyl alcohol = ( mathbf{0 . 7 9 5 2 g c m}^{-mathbf{3}} ) and ( boldsymbol{C}=mathbf{1 2}, boldsymbol{H}=mathbf{1}, boldsymbol{O}= )
( mathbf{1 6}) )
12
1230Assuming ideal behaviour, the enthalpy and volume of mixing of two liquids, respectively, are:
A. zero and zero
B. +ve and zero
c. -ve and zero
D. -ve and -ve
12
1231The relative decrease in VP of an aqueous glucose dilute
solution is found to be 0.018. Hence, the elevation in
boiling point is (it is given 1 molal aqueous urea solution
boils at 100.54°C at 1 atm pressure)
a. 0.018° b. 0.18° c.0.54° d. 0.030
12
1232Illustration 2.205 A 0.1 M solution of potassium sulphate
K,SO, is dissolved to the extent of 80%. What would be its
osmotic pressure at 27°C?
12
1233What is the density of wet air with ( 75 % ) relative humidity at 1 atm and ( 300 mathrm{K} ) ?
Given : vapour pressure of ( H_{2} O ) is 30 torr
and average molar mass of air is
( 29 g / m o l )
A. ( 1.614 g / L )
в. ( 0.96 g / L )
c. ( 1.06 g / L )
D. ( 1.164 g / L )
12
1234Example 2.25 If the radiator of an automobile contains
12 L of water, how much would the freezing point be lowered
by the addition of 5 kg of prestone (glycol C,H,OH)2). How
many kg of Zeron (methyl alcohol) would be required to
produce the same result?
12
1235The degree of dissociation of
( boldsymbol{C a}left(boldsymbol{N} boldsymbol{O}_{3}right)_{2} ) in a dilute aqueous solution
containing 7 g of salt per 100 g of water at ( 100^{circ} mathrm{C} ) is ( 75 % ). The vapour pressure of solution in ( mathrm{mm} ) is ( x, ) then find the
value of ( x / 150 ) to the nearest integer.
12
1236If ‘ ( alpha ) ‘ is degree of dimerisation of
( C H_{3} C O O H ) in benzene, then van’t Hoff factor ‘i’ for circulation of colligative
properties is:
( mathbf{A} cdot 1+alpha )
B ( cdot 1-frac{alpha}{2} )
( c cdot 1+frac{alpha}{2} )
D. ( 1+2 alpha )
12
1237Which one of the following mixture is non-ideal solution?
A. Chloroform and acetone
B. Benzene and toulene
c. Chlorobenzene and bromobenzene
D. Bromoethane and chloroethane
12
12387.
A solution of common salt is prepared and freezed by Raj.
(a) It occurs by evolution of heat
(b) Freezing point of solvent is higher than solution.
(C) No heat change occurs in this process
(d) Kinetic energy of Liquid molecule increases.
12
123910 g of cane sugar (molecular mass =
342) in ( 1 times 10^{-3} m^{3} ) of solution
produces an osmotic pressure of ( 6.68 times 10^{4} N m^{-2} ) at ( 273 mathrm{K} . ) Calculate
the value of ( mathrm{R} ) in SI units.
A. ( 8.3684 J K^{-1} mathrm{mol}^{-1} )
B . ( 9.3684 J K^{-1} ) mol ( ^{-1} )
c. ( 7.3684 J K^{-1} ) mol ( ^{-1} )
D. ( 5.3684 J K^{-1} ) mol ( ^{-1} )
12
1240What type of deviation is shown by a mixture of ethanol and acetone? What
type of azeotrope is formed by mixing
ethanol and acetone?
12
1241How much AgBr could dissolve in 1.0L of
( 0.40 mathrm{M} N H_{3} ? ) Assume that ( A gleft(N H_{3}right)_{2}^{-} )
is the only complex formed.
( left[boldsymbol{K}_{f}left(boldsymbol{A} boldsymbol{g}left(boldsymbol{N} boldsymbol{H}_{3}right)_{2}^{+}right)=mathbf{1} times mathbf{1 0}^{8}right. )
( left.boldsymbol{K}_{s p}(boldsymbol{A} boldsymbol{g} boldsymbol{B r})=mathbf{5} times mathbf{1 0}^{-mathbf{1 3}}right] )
( [sqrt{mathbf{5 0}}=mathbf{7}] )
12
1242( 0.1 M ) solution of urea would be
with ( 0.1 ~ M ) solution of ( N a C l )
A. hypotonic
B. hypertonic
c. isotonic
D. none of these
12
1243Assuming the formation of an ideal
solution, the boiling point of a mixture
containing 1560 g benzene (molar mass =78) and 1125 g chlorobenzene (molar” mass ( =112.5)^{prime} ) using the given vapour
pressure vs. temperature diagram against anexternal pressure of 1000
torr, is :
( mathbf{A} cdot 90^{circ} C )
B. ( 100^{circ} mathrm{C} )
( mathbf{c} cdot 110^{circ} C )
D. ( 120^{circ} mathrm{C} )
12
1244How many grams of concentrated sulphuric acid ( (80 % w / w) ) should be
used to prepare ( 100 m L ) of one molar
( boldsymbol{H}_{2} boldsymbol{S} boldsymbol{O}_{4} ? )
A . ( 10 g )
в. 12.25 g
c. ( 15 g )
D. ( 17.5 g )
12
1245Equal volumes of ( 0.1 M A g N O_{3} ) and
( 0.2 M N a C l ) are mixed. The
concentration of ( N O_{3}^{-} ) ion in the mixture will be:
A . ( 0.1 M )
B. ( 0.05 M )
c. ( 0.2 M )
D. 0.15 М
12
1246g of a substance when dissolved in
Illustration 2.30 4.375 g of a substance when diss
36.0 g of water, lowered its vapour pressure by 0.5 mm a
a given temperature. The vapour pressure of wat
temperature is 25.0 mm. Calculate the molecular weight 01
solute.
12
1247To from a super saturated solution of salt one must:
A. cool slowly
B. cool rapidly
c. add some salt to cold solution
D. use a clear vesse
12
1248The molecular weight of benzoic acid in benzene as determined by depression in the freezing point method corresponds
to:
A. ionization of benzoic acid
B. dimerization of benzoic acid
c. trimerization of benzoic acid
D. solvation of benzoic acid
12
1249Equal volumes of M/20 urea solution
and M/20 glucose solution are mixed. The mixture will have osmotic pressure:
A. equal to either of the solution
B. less than either of the solution
c. higher than either of the solution
D. zero
12
1250When acetone and chloroform are
mixed together, which of the following
observations is correct?
( (mathbf{A}) )
A. A-A and B-B interactions are stronger than A-B interactions
B. A-A and B-B interactions are weaker than A-B
interactions
C. A-A and B-B interactions are equal
D. The liquid form separate layers and are immiscible
12
1251Valli took some common salt,
naphthalene balls, camphor, baking
soda and washing soda. She attempted
to dissolve these substances either in
water or in acetone.

Complete the table with the expected results.
MEDIUM IN SUBSTANCE WHICH ITIS SOLUBLE
a. Common salt
( b )
Naphthalene balls
c. Camphor
d. Baking soda
e. Washing soda

12
1252( 5 mathrm{g} ) of a polymer of molar mass ( 50 k g m o l^{-1} ) is dissolved in ( 1 d m^{3} )
solution. The height of solution ( (m m) ) that will represent its osmotic pressure if density of solution at
equilibrium is ( 0.96 mathrm{kg} mathrm{dm}^{-3} ) is (divide
answer by 5 and write nearest integer value).
12
1253Which is the descriptive term that indicates there is a large quantity of solute, compared with the amount of solvent, in a solution?
A . Dilute
B. concentrated
c. Unsaturated
D. Saturated
E. Supersaturated
12
1254The correct statement among the
following is:
A. smoke is carbon dispersed in air
B. butter is water dispersed in fat
C . greater is the valency of ion more will be its coagulating power
D. more is the gold number of a lyophobic sot, more is protecting power
12
1255Explain the following giving example Saturated solution, Pure
substance, colliod.
12
1256For which of the following solutes the
van’t Hoff factor is not greater than one?
A. ( N a N O_{3} )
в. ( B a C l_{2} )
( mathbf{c} cdot_{K_{4}}left[F e(C N)_{6}right] )
D. ( N H_{2} C O N H_{2} )
12
1257Illustration 2.149 Why is great care taken in intravenous
injections to have comparable concentration of solutions to
be injected to that of blood plasma?
12
1258The mole fraction of water in a
sulphuric acid solution is 0.85 Calculate the molality of the solution:
12
1259The vapour prerssure of pure liquids ( A ) and B are 400 and ( 600 m m H g ) respectively at ( 298 K . ) On mixing the two liquids, the sum of their initial volumes is equal to the volume of the final mixture. The mole fraction of liquids B
is 0.5 in the mixture. The vapour pressure of the final solution,the mole fraction of components ( A ) and ( B ) in
vapour phase, respectively are:
A. ( 500 mathrm{mmHg}, 0.5,0.5 )
в. 450 ттН ( g, 0.4,0.6 )
c. 450 mmHg ( , 0.5,0.5 )
D. ( 500 mathrm{mmHg}, 0.4,0.6 )
12
1260State True or False.
Mixture of ( H N O_{3} ) and ( H C l ) is an
example of maximum boiling point
azeotrope
A. True
B. False
12
1261Illustration 2.130 In a cold climate water gets frozen
causing damages to the radiator of a car. Ethylene glycol
is used as an antifreezing agent. Calculate the amount of
ethylene glycol the added to 2 kg of water to prevent it from
freezing at -8°C. (K, for water = 1.8 K m-!)
12
1262Washing soda ( left(N a_{2} C O_{3} .10 H_{2} Oright) ) is widely used in softening of hard water. If 1 L of hard water requires 0.0286 g of
washing soda, the hardness of ( C a C O_{3} ) in ppm is :
A . 10
B. 5
c. 8
D. 6
12
1263The mole fraction of solute in ( 10 % ) (w/w)
aqueous NaOH solution is:
A . 0.1
B. 0.05
c. 0.0476
D. 0.075
12
1264The van’t Hoff factor indicates the
number of solute particles produced per formula unit that dissolves.
If true enter 1 , if false enter 0 .
12
1265( 4.6 mathrm{cm}^{3} ) of methyl alcohol is dissolved in
( 25.2 mathrm{g} ) of water. Calculate mole fraction of methyl alcohol.
A. 0.1232
B. 0.0759
c. 0.0932
D. 0.0562
12
12665. Negative deviations from Raoult’s law are exhibited by
binary mixtures
a. in which the molecules tend to attract each other and
hence their escape into the vapour phase is retarded.
b. in which the molecules tend to repel each other and
hence their escape into the vapour phase is retarded.
c. in which the molecules tend to attract each other and
hence their escape into the vapour phase is speeded up.
d. in which the molecules tend to repel each other and
hence their escape into the vapour phase is speeded up.
12
1267One millimole ( O_{2} ) gas is dissolved in
( mathbf{5 4 0 0} mathrm{ml} ) water at ( 25^{circ} mathrm{C} ). Calculate the
Henry’s law constant ( boldsymbol{K}_{boldsymbol{H}} ) for this
solution. ( p_{O_{2}}=2 times 10^{-8} ) bar.
12
1268When mango is placed in dilute aqueous solution of hydrochloric acid, it
A. shrinks
B. swells
c. bursts
D. nothing happens
12
1269Justify the following statements with an explanation:
¡) Solubility of calcium oxide decreases with increase in temperature.
ii) What happens to the solubility in exothermic process with regard to temperature?
iii) In endothermic process, solubility increases with increase in temperature.
iv) At a given temperature, increase in pressure increases the solubility of the
gas
12
1270Which of the following substance(s) dissolves in water?
This question has multiple correct options
A. Vinegar
B. Groundnut Oi
c. Lemon Juice
D. Kerosene
12
1271If in solvent, n simple molecules of solute combine to form an associated
molecule, ( x ) is degree of association the
Van’t Hoff’s factor ( ^{prime} boldsymbol{i}^{prime} ) is equal to:
A ( cdot frac{1}{1-n x} )
в. ( frac{1-x+n x}{1} )
c. ( frac{1-x+frac{x}{n}}{1} )
D. ( frac{x}{frac{n}{1}-1+x} )
12
1272Example 2.13. A mixture which contains 0.550 g of
camphor and 0.090 g of an organic solute melts at 161°C.
The solute contains 93.75% C and 6.25% H by weight. What
is the molecular formula of compound? K, for camphor is
37.5°C mol-1 kg. The melting point of camphor is 209°C.
12
1273( 100 mathrm{ml} ) of liquid ( mathrm{A} ) and ( 50 mathrm{ml} ) of liquid ( mathrm{B} ) are mixed to form ( 138 mathrm{ml} ) of solution. It
is :
A. Ideal solution
B. High boiling azeotrope
c. Low boiling azeotrope
D. None of these
12
1274What will be the value of Van’t Hoff
factor for ethanoic acid in benzene?
12
1275An aqueous solution of a salt ( M X_{2} ) at
certain temperature has a van’t Hoff
factor of ( 2 . ) The degree of dissociation for this solution of the salt is:
A . 0.50
B. 0.33
c. 0.67
D. 0.80
12
1276What are the materials which contain
at least two pure substances and show
the properties of their constituents called?
A. A compound
B. An element
c. A mixture
D. A solution
12
1277A solution is ( 25 % ) water, ( 25 % ) ethanol
and ( 50 % ) acetic acid by mass. Calculate the mole fraction of each component.
12
1278Identify the solute ( & ) the solvent in the following solutions:
(a) Sugar solution
(b) Air
(c) Grains (d)
Aerated drinks.
12
1279Illustration 2.80 Consider the following vapour pressure
composition graph. SP is equal to:
a. PQ + RS
b. PQ + QR
c. SR + SQ
d. PQ + QR + RS
Total vapour pressure
P — PB
ok
APB
P
0
X –
S
1
12
1280Match the items of Column-I with its
proportional term in the items of
Column-II:
Column-I
(a) Kinetic energy
(p) Mole fraction
(b) Partial pressure of a
(q) Density
gas
(c) Rate of diffusion
(r) Molar mass
(d) Vapour pressure of a
(s) Absolute liquid ( quad ) temperature
12
1281The simplest way to describe the concentration of solution is :
I) mass by mass
Il) mass by volume
III) volume by pressure
A . ।, ॥
в. ॥, III
( c cdot ) ।, ॥
D. I, II, III
12
1282What will be the value of van’t Hoff
factor
(i) of benzoic acid if it demerises
in aqueous solution? How will the
experimental molecular weight vary as compared to the normal molecular
weight?
12
1283• 29 Relative lowering of vapour pressure is a colligative property
pour pressure is a colligative property because
(a) it depends on the concentration of a non-electrolyte solute in solution and does
not depend on the nature of the solute molecules
(b) it depends on number of particles of electrolyte solute in solution and does not
depend on the nature of the solute particles
(c) it depends on the concentration of a non-electrolyte solute in solution as well as
on the nature of the solute molecules
(d) it depends on the concentration of an electrolyte or non-electrolyte solute in
solution as well as on the nature of solute molecules
(
ahl
12
1284The molal elevation constant is the ratio
of the elevation in boiling point to:
A. molarity
B. molality
c. mole fraction of solute
D. mole fraction of solvent
12
1285The solubility of a solid solute in a liquid solvent increases with increase
in temperature
A. True
B. False
12
1286Which pair(s) of liquids on mixing is/are expected to show no net volume
change and no heat effect? This question has multiple correct options
A. Acetone and ethanol.
B. Chlorobenzene and bromobenzene
c. chloroform and benzene
D. n-Butyl chloride and n-butyl bromide
12
1287Q. 7 What will be the molality of the solution containing 18.25 g of HCL gas in
500 g of water?
(a) 0.1 m
(b) 1 M
(c) 0.5 m
(d) 1 m
12
1288The weight in grams of a non-volatile
solute ( (M . w t: 60) ) to be dissolved in
( 90 g ) of water to produce a relative
lowering of the vapour pressure of 0.02 is:
A . 4
B. 8
( c .6 )
D. 10
12
1289A ( 6.90 M ) KOH solution in water has
( 30 % ) by weight of ( K O H . ) The density of
KOH solution is:
A. ( 1.288 g / m L )
в. ( 12.88 g / m L )
c. ( 0.1288 g / m L )
D. none of these
12
1290The solubility of gases in water
with rise in
temperature
A . increases
B. decreases
c. no change
D. None of the above
12
1291The vapour pressure of ( 2.1 % ) of an aqueous solution of a non-electrolyte at
( 373 K ) is ( 755 mathrm{mm} ). Calculate the molar
mass of solution ( left(M_{2}right) )
A . ( 46.1 mathrm{gm} / mathrm{mol} ) le
B. ( 57.456 mathrm{gm} / mathrm{mole} )
c. ( 10 mathrm{gm} / mathrm{mole} )
D. ( 87.12 mathrm{gm} / mathrm{mole} )
12
1292‘The extent to which a solute is
dissociated or associated can be
expressed by Van ‘t Hoff factor’. Substantiate the statement.
12
1293Vant Hoff factor for a dilute solution
of glucose is:
A . 0
B.
c. 1.5
( D )
12
1294The vapour pressure of a solution containing 2 g of an electrolyte BA in 100 g water which dissociates in one
( B^{+} ) and one ( A^{-} ) ion in water is ( 751 mathrm{mm} )
at ( 100^{circ} mathrm{C} . ) Percentage degree of
ionisation of BA if its molar mass is 56
g ( m o l^{-1} ) (write answer after dividing
degree of dissociation by 80 to the nearest integer) is
12
1295What will be density ( left(operatorname{in} g m L^{-1}right) ) of 3.60 molar sulphuric acid having ( 29 % ) by mass? ( left(text {Molar mass}=mathbf{9 8 g m L}^{-1}right) )
A . 1.88
B. 1.22
( c cdot 1.45 )
D. 1.64
12
1296Illustration 2.145 State how does osmotic pressure vary
with temperature?
12
thermodynamic properties during the formation of 1 mol of an ideal binary solution.
( A )
( (mathbf{A}) )
B.
( (mathbf{A}) )
( c )
( (mathbf{A}) )
( D )
(A)
12
1298I. Agitation and stirring will increase
the rate at which salt dissolves in water
( I I . ) Increased movement of water
molecules allow sodium ions and
chloride ions to be pulled apart as
shells of hydration are formed.
A. Statement I is true, Statement ( I I ) is true and is a correct explanation of the phenomena described in ( I )
B. Statement I is true, Statement II is false
c. statement ( I ) is false, statement ( I I ) is true
D. Statement I is false, Statement II is false
12
1299A solution contains 2.80 moles of
acetone ( left(C H_{3} C O C H_{3}right) ) and 8.20 moles
of ( C H C l_{3} ). Calculate the mole fraction
of acetone.(give answer in ( 110 X) )
12
13000.21 On the basis of information given below mark the correct option.
Information
(i) In bromoethane and chloroethane mixture intermolecular interactions
of A-A and B-B type are nearly same as A-B type interactions.
(ii) In ethanol and acetone mixture –A or B-B type intermolecular
interactions are stronger than A-B type interactions.
(iii) In chloroform and acetone mixture A-A or B-B type intermolecular
interactions are weaker than A-B type interactions.
(a) Solution (ii) and (iii) will follow Raoult’s law
(b) Solution (i) will follow Raoult’s law
(c) Solution (ii) will show negative deviation from Raoult’s law
(d) Solution (iii) will show positive deviation from Raoult’s law
12
13011 kg of water under a nitrogen pressure of 1 atmosphere dissolves 0.02 gm of nitrogen at ( 293 mathrm{K} ) Calculate Henry’s law constant.
A ( cdot 7.2 times 10^{-4} ) atm
B . ( 7.5 times 10^{4} ) atm
( c cdot 7.4 times 10^{4} operatorname{atm} )
D. ( 7.2 times 10^{4} ) atm
12
1302The freezing point of one molal ( N a C l )
solution assuming ( N a C l ) to be ( 100 % ) dissociated in water is:
[Molal depression constant is ( 1.86] )
A ( .-2.72^{2} C )
В. ( -3.72^{2} C )
c. ( 2.72^{2} C )
D. ( 3.72^{2} C )
12
1303Illustration 2.158 Two solutions of glucose have osmotic
pressure 1.5 and 2.5 atm, respectively. 1 L of first solution is
mixed with 2 L of second solution. The osmotic pressure of
the resultant solution will be
12
1304How many grams of ( N a O H ) should be
added to water to prepare ( 250 mathrm{ml} ) solution of 2 M NaOH ?
A ( cdot 9.6 times 10^{3} )
В. ( 2.4 times 10^{3} )
c. 20
D . 24
12
1305Question 12. Calculate the osmotic pressure in pascals exerted by a
solution prepared by dissolving 10 g of polymer of molar mass 185000 in
450 mL of water at 37° C.
Use the formula for osmotic pressure (T) = CRT, and C and na
MB
12
1306( mathbf{A} )
( 3 mathrm{M} )
3L solution of NaOH is mixed with
another ( 3 mathrm{M} ) 5L solution of ( mathrm{NaOH} ). How
much should the mixture be diluted so
that the final molarity of the solution becomes 1M?
12
1307The value of Henry’s constant ( boldsymbol{K}_{boldsymbol{H}} ) is :
A. greater for gases with higher solubility
B. greater for gases with lower solubility
c. constant for all gases
D. not related to the solubility of gases
12
1308The osmotic pressure at ( 293 mathrm{K} )
( A cdot 2 )
B. 3
( c cdot 4 )
D. 4.805
12
1309A solution containing 10 g per ( mathrm{dm}^{3} ) of urea (m.w. = 60) is isotonic with a 5%
solution of a non-volatile solute. The
molecular mass of this non-volatile
solute is:
A . ( 250 mathrm{g} mathrm{mol}^{-1} )
B . 300 g mol-
c. ( 350 mathrm{g} ) mol ( ^{-1} )
D. ( 200 mathrm{g} mathrm{mol}^{-1} )
12
1310us solution is
Example 2.26 If the boiling point of an aqueous solutie
100.1°C, what is its freezing point? Givenly = 80,1, = 540 cal
g’ respectively, of H20.
12
1311The answer to this question is a single digit integer, ranging from 0 to 9
The van’t Hoff factor for aqueous
solution of ( C u S O_{4} cdot 5 H_{2} O ) will be
12
1312Which of the liquids in each of the following pairs has a higher vapour pressure?
A. Alcohol, glycerine
B. Mercury, water
c. petrol, kerosene
D. None of these
12
1313Example 2.5 Liquids A and B form an ideal mixture, in
which the mole fraction of A is 0.25. At temperature T, a
small quantity of the vapour in equilibrium with the liquid
is collected and condensed. This process is repeated for a
second time with the first condensate. The second condensate
now contains 0.645 mole fraction of A. Calculate the ratio
(
P P ). What will be the mole fraction of B in the third
condensate?
12
1314The molecular weight of an organic compound is 58.0 g/mol. Compute the boiling point of a solution containing ( 24.0 mathrm{g} ) of the solute and ( 600 mathrm{g} ) of water when the barometric pressure is such that pure water boils at
( 99.725^{circ} mathrm{C} .left(K_{6} text { forwater } 0.513^{circ} mathrm{C} / mathrm{m}right) )
( mathbf{A} cdot 50^{circ} C )
B . ( 100.08^{circ} mathrm{C} )
( c cdot 150.1^{circ} C )
D. ( 180.34^{circ} mathrm{C} )
12
1315is soluble in water, ethanol
and methanol.
A . ( N a O H )
в. ( N a H )
( c . N a O )
D. None of these
12
13166. Mole fraction of component A in vapour phase is X1
and mole fraction of component A in liquid mixture is
X2(PA°= vapour pressure of pure A), then the total vapour
pressure of the liquid mixture is
2 PAX2 h. PAXI s. PBRI d. PB 22
Xi
X2
22
12
1317Blood is isotonic with.
A. ( 0.16 M ) NaCl
( l )
B. Conc.NaCl
c . ( 30 % ) NaCl ( l )
D. ( 50 % ) NaCl
12
1318What is the number of mole of benzene
( left(P_{B}^{0}=150 text { torrs }right) ) per mole of toluene
( left(P_{T}^{0}=50 text { tor } r sright) ) in vapour phase if the
given solution has a vapour pressure of 120 torrs in equilibrium with its vapour?
( A cdot 7 )
B. 8
c. 9
D. 10
12
1319What would be the freezing point of a
solution that has 684 grams of sucrose
( (1 mathrm{mol}=342 mathrm{g}) ) dissolved in 2,000
grams of water (1 mole= 18 grams)?
B. ( -0.93^{circ} mathrm{C} ) or ( 272.07 mathrm{K} )
( mathbf{c} .-1.39^{circ} mathrm{C} ) or ( 271.61 mathrm{K} )
D. ( -2.48^{circ} mathrm{C} ) or ( 270.52 mathrm{K} )
E. ( -3.72^{circ} mathrm{C} ) or ( 269.28 mathrm{S} )
12
1320Identify the solute ( & ) the solvent in the following solution:
a) sugar solution
b) Air
c) Rain water
d) Aerated drinks
12
1321Question 28cm Casa, the remaining of emotion de
em
Question 28. Calculate the mass percentage of aspirin (C9Hg04) in
acetonitrile (CH3CN) when 6.5 g of C,H,O, is dissolved in 450 g of
CH3CN.
Mass of solute
We know that mass %=
2 x 100
Mass of solution
and mass of solution = mass of solute + mass of solvent.
So, calculate mass of solution and then mass percentage.
12
1322Acetic acid undergoes dimerisation, when dissolved in benzene (as shown in
figure) Molecular mass of acetic acid is found
to be 120 .

Which among the following relation is correct?
(where, ( alpha= ) degree of association,
( d= ) observed vapour density, ( D= ) Theoretical vapour density
[
2 mathrm{CH}_{3}-mathrm{cooH} rightleftharpoons mathrm{cH}_{3}-mathrm{c} underbrace{mathscr{J}}_{mathrm{oH} ldots mathrm{o}}^{mathrm{o} ldots mathrm{OH}}_{mathscr{J}}^{mathrm{c}-mathrm{cH}_{3}}
]
( A )
[
alpha=2left(frac{D-d}{d}right)
]
в.
[
alpha=2left(frac{D-d}{D}right)
]
c.
[
alpha=2left(frac{d-D}{d}right)
]
D.
[
alpha=frac{2 d}{D-d}
]

12
1323A sample of water has a hardness
expressed as 77.5 ppm ( C a^{2+} . ) This sample is passed through an ion
exchange column and ( C a^{2+} ) is replaced
by ( boldsymbol{H}^{+} . ) Select correct statement(s).
This question has multiple correct options
A. pH of the water after it has been so treated is 2.4
B. Every ( C a^{2+} ) ion is replaced by one ( H^{+} ) ion.
C . Every ( C a^{2+} ) ion is replaced by two ( H^{+} ) ions.
D. pH of the solution remains unchanged.
12
1324The exact mathematical expression of Raoult’s law is:
( ^{text {A }} cdot frac{P_{0}-P_{s}}{P_{0}}=frac{n}{N} )
в. ( frac{P_{0}-P_{s}}{P_{0}}=frac{N}{n} )
c. ( frac{P_{0}-P_{s}}{P_{s}}=frac{n}{N} )
D. ( frac{P_{0}-P_{s}}{P_{0}}=n times N )
12
1325If the observed and theoretical
molecular mass of NaCl is found to be
31.80 and ( 58.50, ) then the degree of dissociation of NaCl is:
A . 83.96%
B . 8.39%
c. ( 90 % )
D. 100%
12
1326Define solubility and write the factors which influence the solubility.12
1327State True or False.
Elevation in boiling point is directly proportional to the molality of the solution.
A. True
B. False
12
1328A solution is prepared by dissolving
( 11 g ) glucose in ( 250 c m^{3} ) water at ( 30^{circ} C )
what is mass percent glucose in
solution. The density of water at ( 30^{circ} ) is ( mathbf{0 . 9 9 6} boldsymbol{g} / boldsymbol{c m}^{mathbf{3}} )
12
1329( p H ) of a dilute solution of ( H C l ) is 6.95
Calculate molarity of ( H C l ) solution. ( left[begin{array}{c}10^{-6.95}=11.22 times 10^{-8} \ 10^{-7.05}=8.90 times 10^{-8}end{array}right] )
12
1330A solution contain ( 36 % ) water and ( 64 % )
acetaldehyde ( left(C H_{2} C H Oright) ) by mass. The mole fraction of acetaldehyde is:
A . 0.42
B. 0.2
c. 4.2
D. 2.1
12
1331A sample of air is saturated with benzene (vapour pressure =100 mm Hg at ( 298 mathrm{K} ) ) at ( 298 mathrm{K}, 750 mathrm{mm} ) Hg pressure. If it is isothermally compressed to one third of its initial volume, the final
pressure of the system is:
A. 2250 torr
B . 2150 torr
c. 2050 torr
D. 1950 torr
12
1332The normality of ( 10 % ) ( weight / volume) acetic acid is:
( A cdot 1 N )
B. 10 N
c. ( 1.67 mathrm{N} )
D. 0.83
12
1333Pure water boils at ( 99.725^{circ} C ) at shimla.
If ( K_{b} ) for water is ( 0.51 K m o l^{-1} k g, ) the
boiling point of 0.69 molal urea solution will be:
A . 100.35
B. 100.08
c .99 .37
D. None of these
12
1334A solution of sucrose (molar mass ( =342 )
( left.g m o l^{-1}right) ) has been prepared by dissolving 68.5 g of sucrose in 1000 g of water. The freezing point of the solution obtained will be:
( left[mathrm{K}_{f} text { for water }=1.86 mathrm{K} mathrm{kg} mathrm{mol}^{-1}right] )
A . – ( 0.372 mathrm{c} )
B. 0.520C
c. ( +0.372 c )
D. 0.570C
12
1335Question 3. Calculate the molarity of each of the following solutions :
(a) 30 g of Co(NO3)2.6H 0 in 4.3 L of solution.
(b) 30 mL of 0.5 M H2SO, diluted to 500 mL.
12
1336111.1g of the non-volatile solute, urea needs to be dissolved in 100 g of water, in order to decrease the vapour pressure of water by ( 25 % ). The molarity of the solution will be:
A. 18.52 м
в. 18.92
c. 19.52 м
D. None of the above
12
1337Hlustration 2.161 The osmotic pressure of a solution at 0°C
is 4 atm. What will be its osmotic pressure at 546 K under
similar conditions?
a. 4 atm b. 9 atm c. 8 atm d. 6 atm
12
1338Ferrous sulphate heptahydrate is used to fortify foods with iron. The amount (in grams) of the salt required to achieve 10 ppm of iron in 100 kg of wheat is
[Atomic weight ( : mathrm{Fe}=mathbf{5 5 . 8 5} mathrm{S}=mathbf{3 2 . 0 0} mathrm{O} )
( =mathbf{1 6 . 0 0}] )
12
13391 mol benzene ( left(P_{text {benzene }}^{o}=42 mathrm{mm}right) ) and 2 mol toluene ( left(P_{text {toluene}}^{o}=36 mathrm{mm}right) ) will have
This question has multiple correct options
A. total pressure of 38 mm.
B. mole fraction of vapour of benzene above liquid mixture is ( 7 / 19 )
c. positive deviation from Raoult’s law
D. negative deviation from Raoult’s law
12
1340The freezing point depression constant
for water is ( -1.86^{0} mathrm{Cm}^{-1} . ) If ( 5.00 mathrm{g} )
( N a_{2} S O_{4} ) is dissolved in 45.0 g ( H_{2} O, ) the
freezing point is changed by ( 3.82^{0} C )
Calculate the vant Hoff factor for
( N a_{2} S O_{4} )
A . 2.05
B . 2.63
c. 3.11
D. 0.381
12
1341Two liquids ( A ) and ( B ) form an ideal solution. At ( 300 mathrm{K} ), the vapour pressure of a solution containing 1 mole of A and 3 mole of ( mathrm{B} ) is ( 550 mathrm{mm} ) of Hg. At the
same temperature, if one more mole of ( mathrm{B} ) is added to this solution, the vapour pressure of the solution increases by 10 ( mathrm{mm} ) of Hg. Determine the vapour pressure of ( A ) and ( B ) in their pure states.
12
1342If the density of methanol is ( 0.793 mathrm{kg} L^{-1}, ) what is its volume
needed for making 2.5 L of its 0.25 M
solution?
12
1343A solution of ( N a_{2} S_{2} O_{3} ) is saturated iodometrically against 0.334 g of pure ( K B r O_{3}left(text { converted to } B r^{-}right) ) requiring 40
( mathrm{ml} . mathrm{Na}_{2} mathrm{S}_{2} mathrm{O}_{3} ) solution. What is the
molarity of ( N a S_{2} O_{3} ) solution? (Molar
mass of ( boldsymbol{K} boldsymbol{B} boldsymbol{r} boldsymbol{O}_{3}=mathbf{1 6 7} ) g ( boldsymbol{m o l}^{-1} ) )
12
1344If the mass ratio of non-reacting gases
( O_{2} ) and ( N_{2} ) in a vessel is ( 2: 7, ) then the
ratio of their molecules will be:
A ( cdot 1: 2 )
B. 3:5
c. 2: 7
D. 1: 4
12
1345( 380 mathrm{mL} ) of a gas at ( 27^{0} mathrm{C}, 800 mathrm{mm} ) of ( mathrm{Hg} )
weight
( 0.455 mathrm{g} . ) the mol.wt.of gas is:
A .27
B . 28
c. 29
D. 30
12
1346Illustration 2.174 The osmotic pressure of a solution was
found to be 8 atm when 8 mol of a non-volatile solute was
dissolved in V L of solution at 300 K. Calculate the volume
of solution (R = 0.0821 L-atm K-1 mol-1)
12
1347The freezing point of a 0.05 molal solution of non-electrolyte in water is:
( left[boldsymbol{K}_{f}=mathbf{1 . 8 6} boldsymbol{K} boldsymbol{m}^{-1}right] )
( mathbf{A} cdot-1.86^{circ} mathrm{C} )
B. ( -0.93^{circ} mathrm{C} )
с. ( -0.093^{circ} mathrm{C} )
и. ( -0.093^{circ} ).
D. ( 0.093^{circ} mathrm{C} )
12
1348Illustration 2.140 The melting point of phenol is 40°C.
A solution containing 0.172 g acetanilide (C,H,OH) in 12.54 g
phenol freezes at 39.25°C. Calculate the freezing point
constant and the latent heat of fusion of phenol.
12
1349In a solvent ( 50 % ) of benzoic acid
dimerises while rest ionises,
determines molar mass of acid which is
observed and also its van’t Hoff factor.
12
1350h expressions given in Column II.
Q.49 Match the laws given in Column I with expressions giv
Column
Column Il
A Raoult’s law
1. AT, = Km
B. Henry’s law
2. T = CRT
C. Elevation of boiling point
3 p=xp; + X,
D. Depression in freezing point 4. AT,
E. Osmotic pressure
15. DEK, X
12
1351The vapour pressure of pure water at
( 25^{circ} mathrm{C} ) is 23.76 torr. The vapour pressure of a solution containing 5.40 g of a nonvolatile substance in 90.0 g water is 23.32 torr. The molecular weight of the solute is:
A. ( 97.24 mathrm{g} / mathrm{mol} )
B. 24.29 g/mol
c. ( 50.44 mathrm{g} / mathrm{mol} )
D. ( 57.24 mathrm{g} / mathrm{mol} )
12
1352The unit of ebullioscopic constant is?
A . ( K ) kg mol ( ^{-1} ) or ( K(text { molality })^{-1} )
B . mol kg ( K^{-1} ) or ( K^{-1} ) (molality)
c. ( k g ) mol ( ^{-1} K^{-1} ) or ( K^{-1} ) (molality) ( ^{-1} )
D. ( K ) mol ( k g^{-1} ) or ( K(text { molality }) )
12
1353( 6.02 times 10^{20} ) molecules of urea are
present in ( 100 mathrm{mL} ) of its solution. The
molarity of urea solution is :
A . ( 0 . )
B. 0.01
c. 0.02
D. 0.001
12
1354A solution of benzene and toluene is an
example of solution.
A. Ideal
B. non ideal
c. azeotrope
D. none
12
1355Define the term : isotonic solution12
13560.40 What is the significance of Henry’s law constant Kh?
Ans According to Henry’s law
n
12
1357The vapour pressure of o-nitrophenol at any given temperature is predicted to be:
A. Higher than that of p-nitrophenol
B. Lower than that of p-nitropheno
c. Same as that of p-nitrophenol
D. Higher or lower depending upon the size of the vesse
12
1358Define azeotropes.What type of azeotrope is formed by a positive deviation from Raoult’s law? Give an
example
12
1359( mathbf{0 . 1} boldsymbol{M} boldsymbol{K}_{4}left[boldsymbol{F} e(boldsymbol{C} boldsymbol{N})_{6}right] ) is ( 60 % ) ionized
What will be its Van’t Hoff factor?
A . 1.4
в. 3.4
c. 2.4
D. 4.
12
1360Benzoic acid undergoes dimerization in benzene solution. The Van’t Hoff factor ( i )
is related to the degree of assoication ( alpha )
of the acid as :
B. ( i=1+(alpha / 3) )
c. ( i=1-(alpha / 2) )
D. ( i=1+(alpha / 2) )
12
1361An aqueous solution freezes at ( 272.4 K )
while pure water freezes at ( 273.0 K )
while pure water freezes at ( 273.0 K ) Determine
(a) the molality of the solution
(ii) boiling point of the solution
(iii) lowering of vapour pressure of water at ( 298 K )
(Given, ( boldsymbol{K}_{boldsymbol{f}}=mathbf{1 . 8 6 K} boldsymbol{k g} boldsymbol{m o l}^{-1}, boldsymbol{K}_{boldsymbol{b}}= )
( 0.512 K k g ) mol( ^{-1} ) and vapour pressure
of water at ( 298 K=22.756) )
12
1362A mixture from which some of the
solute particles will settle on standing:
A. Miscible
B. Suspension
c. colloid
D. Saturated
E. Supersaturated
12
1363Hustration 2.163 300 cm? of an aqueous solution contains
1.26 g a polymer. The osmotic pressure of such solution at
300 K is found to be 1.26 x 10-3 bar. Calculate the molar mass
of the polymer.
12
1364The vapour pressure of water at room temperature is ( 23.8 mathrm{mm} ) Hg. The vapour
pressure of an aqueous solution of sucrose with mole fraction 0.1 is equal
to:
( mathbf{A} cdot 23.9 mathrm{mm} mathrm{Hg} )
B. ( 24.2 mathrm{mm} ) Hg
c. ( 21.42 mathrm{mm} ) Hg
D. ( 31.44 mathrm{mm} ) нв
12
1365Determine the osmotic pressure of a solution a solution prepared by
dissolving ( 2.5 times 10^{-2} g ) of ( K_{2} S O_{4} ) in ( 2 L )
of water at ( 25^{0} C ), assuming that it is completely dissociated ( left(R=0.0821 L text { at } m K^{-1} m o l^{-1}, ) Molar right.
mass of ( K_{2} S O_{4}=174 g m o l^{-1} )
12
1366One mole of non volatile solute is
dissolved in two moles of water. The
vapour pressure of the solution relative to that of water is:
A ( cdot frac{2}{3} )
в. ( frac{1}{3} )
( c cdot frac{1}{2} )
D. ( frac{3}{1} )
12
1367Which one of the following statements
is false?
A. Raoult’s law states that the vapour pressure of a component over a solution is proportional to its mole fraction
B. The osmotic pressure ( ( pi ) ) of a solution is given by the equation ( pi=M R T ), where, ( M ) is the molarity of the
solution
C. The correct order of osmotic pressure for ( 0.01 mathrm{M} )
aqueous solution of each compound is ( B a C l_{2}> ) ( K C l>C H_{3} C O O H> )sucrose
D. Two sucrose solutions of same molality prepared in different solvents will have the same freezing point depression
12
1368The vapour pressure of water depends
upon:
A. surface area of container
B. volume of container
c. temperature
D. all of the above
12
1369Question 8. The vapour pressure of pure liquids A and B are 450 and
700 mm Hg respectively, at 350 K. Find out the composition of the liquid
mixture if total vapour pressure is 600 mm Hg. Also find the composition
of the vapour phase.
Apply Raoult’s law Pa = PÅ XA + P8XB = PÅ XA+ P8 (1 – Xa) to calculate
mole fraction of A(XA) and B (XB).
In vapour phase, partial pressures are used instead of number of moles.
12
1370Illustration 2.154 Why a person suffering from high blood
pressure is advised to take minimum quantity of common
salt?
12
1371Which has the highest freezing point?
A ( cdot operatorname{lm} K_{4}left[F e(C N)_{6}right] quad ) solution
B. ( 1 m C_{6} H_{12} O_{6} ) solution
c. ( 1 m K C l ) solution
D. ( 1 m ) rock salt solution
12
1372For a non-ideal solution exhibiting positive deviation from Raoult’s law,
( Delta_{m i x} H ) has a
(nonzero)
A. positive
B. negative
c. zero
D. none
12
1373Two liquids ( X ) and ( Y ) form an ideal
solution at ( 300 K ), the vapour pressure
of the solution containing 1 mole of ( X )
and 3 moles of ( Y ) is 550 mm Hg. At the
same temperature, if 1 mole of ( Y ) is further added to this solution, the
vapour pressure of the solution
increases by 10 mm ( H g . ) Vapour
pressure (in ( mathrm{mm} ) Hg ) of ( boldsymbol{X} ) and ( boldsymbol{Y} ) in
their pure states will be respectively:
A . 200 and 300
B. 300 and 400
c. 400 and 600
D. 500 and 600
12
1374In the reaction; ( boldsymbol{A}+mathbf{2} boldsymbol{B} rightarrow mathbf{3} boldsymbol{C}+boldsymbol{D} )
which of the following expression does not describe changes in the concentration of various species as a function of time?
A ( cdot{d[C] / d t}=-{3 d[A] / d t} )
B . ( {3 d[D] / d t}={d[C] / d t} )
c. ( {3 d[B] / d t}=-{2 d[C] / d t} )
D . ( {2 d[B] / d t}=-{d[A] / d t} )
12
1375Assertion
For rubber and water, ( V(I)<V(s) )
Reason
The density of both rubber and water is
more in liquid state.
A. Both Assertion and Reason are correct and Reason is
the correct explanation for Assertion
B. Both Assertion and Reason are correct but Reason is
not the correct explanation for Assertion
C. Assertion is correct but Reason is incorrect
D. Assertion is incorrect but Reason is correct
12
1376The vapour pressure of two miscible liquids ( A ) and ( B ) are 300 and 500 mm of
Hg respectively. In a flask, 10 moles of ( A )
is mixed with 12 moles of ( B ). However,
as soon as ( B ) is added, ( A ) starts
polymerizing into a completely insoluble solid. After 100 minutes,
0.525 moles of a non-volatile solute is
dissolved which arrests the polymerization completely. The final vapour pressure of the solution is 400 mm of Hg. Assume negligible volume
change on mixing, polymerization and ideal behaviour for the final solution.
If a number of moles of ( boldsymbol{A} ) polymerized
in 100 minutes are expressed as ( x, ) then
a value of ( 10 x ) is:
( mathbf{A} cdot mathbf{1} )
B . 2
( c .3 )
D. 4
12
1377( 100 mathrm{ml} ) of ( 0.1 mathrm{M} ) solution of a weak acid
( H A ) has molar conductivity
( 5 S c m^{2} m o l^{-1} . ) The osmotic pressure of
the resulting solution obtained after
dilution of original solution upto 1 litre at ( 500 mathrm{K}, ) assuming ideal solution is:
( left(G i v e n: lambda_{m}^{infty}left(H^{+}right)=right. )
( 450 S c m^{2} m o l^{-1}, lambda_{m}^{infty}left(A^{-}right)= )
( mathbf{5 0} boldsymbol{S c m}^{2} boldsymbol{m o l}^{-1}, boldsymbol{R}= )
( left.0.08 L text { atm } operatorname{mole}^{-1} K^{-1}, sqrt{10}=3.2right) )
A. 0.3128 atm
B. 0.4128 atm
c. 0.5128 atm
D. 0.6128 atm
12
1378( 2.0 mathrm{g} ) of bensoic acid dissolved in ( 25.0 mathrm{g} ) of benzene shows a depression in freezing point to 1.62K. Mollal
depression constant ( left(K_{f} ) of bezene is right.
4.9 K.kg. ( m o l^{-1} . ) What is the percentage association of the acid?
A. ( (alpha)=90.8 % )
B. ( (alpha)=99.2 % )
c. ( (alpha)=9.8 % )
D. ( (alpha)=49.6 % )
12
1379Which aqueous solution has minimum
freezing point?
в. 0.005 М ( C_{2} ) Н ( _{5} ) ОН
c. 0.005 М ( M g I_{2} )
D. ( 0.005 mathrm{M} mathrm{MgSO}_{4} )
12
1380pH of a ( 0.1 mathrm{M} ) monobasic acid is found to
be ( 2 . ) Hence, its osmotic pressure at a given temperature T K is :
( mathbf{A} cdot 0.1 mathrm{RT} )
B. 0.11RT
c. ( 1.1 mathrm{RT} )
D. 0.01RT
12
1381Which salt shows maximum osmotic
pressure in its ( 1 mathrm{m} ) solution.
A ( . A g N O_{3} )
в. ( N a_{2} S O_{4} )
( mathrm{c} cdotleft(N H_{4}right)_{3} P O_{4} )
D. ( M g C l_{2} )
12
1382Question 10. Boiling point of water 750 mm Hg is 99.63°C. How much
sucrose is to be added to 500 g of water such that it boils at 100° C.
[K, for water is 0.52 K kg mol-‘).
12
1383Pure water can be obtain from sea
water by:
A. Centrifugation
B. Plasmolysis
c. Reverse osmosis
D. Sedimentation
12
1384If the vapour pressure of solutions of two liquids are less than those expected from ideal solution they are said to have:
A. negative deviation from ideal behaviour
B. positive deviations from ideal behaviour
c. ideal behaviour
D. positive deviation for lower concentration and negative deviations for higher concentration
12
1385Which of the following are dilution dependent but temperature independent? This question has multiple correct options
A. Formality
B. Molality
c. Mole fraction
D. Molarity
12
1386An azeotropic mixture of HCl and water
has:
A . ( 84 % ) of ( mathrm{HCl} )
в. 22.2% НС।
c. 63% of HCI
D. 20.2% HCI
12
1387Considering the formation, breaking and strength of hydrogen bond, predict which of the following mixtures will show a positive deviation from
Raout’s law?
A. Methanol and acetone
B. Chloroform and acetone
c. Nitric acid and water
D. Phenol and aniline
12
1388Maximum depression in freezing point is caused by:
A. potassium chloride
B. sodium sulphate
c. magnesium sulphate
D. magneisum carbonate
12
1389A solution that is at equilibrium and contains the maximum amount of
solute for a given amount of solvent at constant temperature and pressure. What type of solution is it?
A. Miscible
B. Suspension
c. colloid
D. Saturated
12
1390( 4 g ) of hydrogen and ( 128 g ) of hydrogen iodide are present in a 2 litre flask. What are their active masses?12
1391Out of ( 1 M B a C l_{2} ) and ( 1 M A l C l_{3}, ) which
one has higher freezing point and why?
12
13926. What mass of urea be dissolved in 171 g of water so as
to decrease the vapour pressure of water by 5%?
a. 15 g b. 20 g c. 25 g d. 30 g
12
1393Illustration 2.168 200 cm of an aqueous solution of a
protein contains 1.26 g of the protein. The osmotic pressure
of such a solution at 300 K is found to be 2.57 x 10-3 bar.
Calculate the molar mass of the protein.
12
1394If molality of ethyl alcohol in aqueous
solution is 4.45 then the mole fraction of
ethyl alcohol in the solution is
12
1395Illustration 2.178 At 10°C, the osmotic pressure of
urea solution is 500 mm. The solution is diluted and the
temperature is raised to 25°C, when the osmotic pressure is
found to be 105.3 mm. Determine the extent of dilution.
12
1396Assertion
The solubility of a substance changes
with temperature.
Reason
Heat is required to break the bonds
holding molecules together so solubility is dependent on temperature.in dissolution, energy, in the form of heat, is required to break the bonds joining
the molecules in the solid together.
A. Both Assertion and Reason are correct and Reason is the correct explanation for Assertion
B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion
C. Assertion is correct but Reason is incorrect
D. Both Assertion and Reason are incorrect
12
1397Generally solubility of gases in liquids is decreases as increasing temperature. Give reason12
1398( mathbf{0 . 0 0 1} ) molal solution of ( left[boldsymbol{P t}left(boldsymbol{N} boldsymbol{H}_{3}right)_{4} boldsymbol{C l}_{4}right] )
in water had a freezing point depression
of ( 0.0054 quad^{o} C . ) If ( K_{f} ) for water is 1.80 the correct formula of the compound is :
( mathbf{A} cdotleft[P tleft(N H_{3}right)_{4} C l_{3}right] C l )
( ^{mathbf{B}} cdotleft[P tleft(N H_{3}right)_{4} C l_{4}right] )
c. ( left[P tleft(N H_{3}right)_{4} C l_{2}right] C l_{2} )
D. ( left[P tleft(N H_{3}right)_{4} C lright] C l_{3} )
12
1399( 25.6 mathrm{g} ) of sulphur in 100 g benzene shows depression in freezing point of
( 5.12^{circ} mathrm{C} . K_{f} ) for benzene is
( 5.12^{circ} mathrm{Ckg} ) mol( ^{-1} . ) The molecular
formula of sulphur in benzene is:
( A cdot S_{2} )
в. ( S_{6} )
( mathrm{c} cdot S_{8} )
D. ( S_{12} )
12
14002.21 Which of the following terms are unitless?
(a) Molality (b) Molarity (c) Mole fraction
(d) Mass per cent
12
1401Vapour pressure of ( C C l_{4} ) at ( 25^{circ} C ) is 143 mm ( H g ). If ( 0.5 g m ) of non-volatile solute (mol. mass 65 ) is dissolved in
( 100 m l C C l_{4}, ) then the vapour pressure
of the solution at ( 25^{circ} mathrm{C} ) is:
[Given: density of ( left.C C l_{4}=1.58 g / c m^{3}right] )
( mathbf{A} cdot 141.93 m m )
B . ( 94.39 mathrm{mm} )
c. ( 199.34 mathrm{mm} )
D. ( 143.99 mathrm{mm} )
12
1402Why do soaps not work in hard water?12
1403The van’t Hoff factor of
( 0.1 M L aleft(N O_{3}right)_{3} ) solution is found to
be 2.74 , the percentage dissociation of the salt is:
A. ( 85 % )
в. ( 58 % )
c. ( 65.8 % )
D. ( 56.8 % )
12
1404The freezing point of equimolal solution will be highest for:
A ( cdot C_{6} H_{5} N H_{3} C l )
в. ( A g N O_{3} )
( mathbf{c} cdot C aleft(N O_{3}right)_{2} )
( mathbf{D} cdot L aleft(N O_{3}right) )
E. ( D- ) fructose
12
1405A solution is prepared by dissolving ( 5.64 mathrm{g} ) of glucose in ( 60 mathrm{g} ) of water. Calculate the mole fraction of
each of glucose and water respectively.
B. 0.01,0.99
c. 0.92,0.08
D. 0.789, 0.211
12
1406The ratio of lowering of vapour pressure of ( 0.1 ~ M ) aqueous solutions of ( K C l )
( boldsymbol{C u} boldsymbol{S O}_{4} & boldsymbol{N a}_{2} boldsymbol{S O}_{4} ) is:
A. 1: 2: 3
B. 2: 2: 3
( mathrm{c} cdot 1: 1: 1 )
D. 3: 2: 1
12
1407The solubility of a gas in a liquid is directly proportional to the pressure of the gas. This statement is:
A. Raoult’s law
B. Henry’s law
c. van’t Hoff’s law
D. None of these
12
1408Example 2.23 Among the following, the solution which
shows the lowest osmotic pressure is
a. 0.10 M NaCI b. 0.05 M CaCl,
c. 0.04 M K [Fe(CN)] d. 0.03 M FeCl2
12
1409Illustration 2.165 Calculate the osmotic pressure of 5%
solution of cane sugar (sucrose) at 300 K.
12
1410Dissolution of a non-volatile solute into
A. Decrease of entropy.
B. Increase in tendency of the liquid to freeze
c. Increase in tendency to pass into the vapour phase.
D. Decrease in tendency of the liquid to freeze
12
1411When a non-volatile solute is dissolved
in a solvent, the relative lowering of vapour pressure is equal to :
A. mole fraction of solvent
B. mole fraction of solute
c. molarity of solution
D. molality of solution
12
1412Write two differences between ideal
solutions and non-ideal solutions.
12
1413The freezing point of equimolal aqueous solution will be highest for :
A. ( C_{6} H_{5} N H_{3} C l )
в. ( C aleft(N O_{3}right)_{2} )
c. ( L aleft(N O_{3}right)_{3} )
D. ( C_{6} H_{12} O_{6} )
12
1414Hlustration 2.170 The osmotic pressure of blood is 8.21
atm at 310 K. How much glucose should be used per L for
an intravenous injection that is isotopic with blood?
12
1415A well stirred ( (1 L) ) solution of
( 0.1 M C u S O_{4} ) is electrolysed at ( 25^{circ} C )
using copper electrodes with a current of 25 m ( A ) for 6 hours. If current
efficiency is ( 50 % ). At the end of the duration what would be the
concentration of copper ions in the solution?
A ( .0 .0856 M )
В. ( 0.092 mathrm{M} )
c. ( 0.0986 M )
D. ( 0.1 M )
12
1416Which of the following 0.1 M aqueous solutions will have the lowest freezing point?
A. Potassium sulphate
B. Sodium chloride
c. urea
D. Glucose
12
1417( 0.3500 g ) of potassium oxalate is titrated with ( 37.40 m L ) of sodium
permaganate to reach a pink end point in the following reaction:
( mathbf{5} C_{2} O_{4(a q)}+2 M n O_{4(a q)}^{-}+16 H_{(a q)}^{+} rightarrow )
( mathbf{2} M boldsymbol{n} boldsymbol{S} boldsymbol{O}_{4(a q)}+boldsymbol{6} boldsymbol{S} boldsymbol{O}_{4(a q)}^{2-}+mathbf{1 0} boldsymbol{C} boldsymbol{O}_{2(boldsymbol{g})}+ )
( mathbf{8} boldsymbol{H}_{2} boldsymbol{O}_{(l)} )
What was the concentration of the
sodium permanganate?
12
1418Choose the correct statement with
respect to the vapour pressure of a liquid among the following.
A. Increases linearly with increasing temperature.
B. Increases non-linearly with increasing temperature.
c. Decreases linearly with increasing temperature
D. Decreases non-linearly with increasing temperature.
12
1419Match column I with column II.12
1420Which of the following will form an ideal
solution?
A ( cdot C_{2} H_{5} O H ) and water
B. ( H N O_{3} ) and water
c. ( C H C l_{3} ) and ( C H_{3} C O C H_{3} )
D. ( C_{6} H_{6} ) and ( C_{6} H_{5} C H_{3} )
12
1421We define p value of a term (say ( x ) ) as
( boldsymbol{p}_{boldsymbol{x}}=-log boldsymbol{x} )
Calculate the value of ( 1000 p ) for ( N O_{3} ) in a solution that is ( 4.78 times 10^{-2} mathrm{M} ) in
( boldsymbol{C u}left(boldsymbol{N} boldsymbol{O}_{3}right)_{2} ) and ( boldsymbol{0 . 1 0 4} boldsymbol{M} ) in ( boldsymbol{Z} boldsymbol{n}left(boldsymbol{N} boldsymbol{O}_{3}right)_{2} )
12
1422( 100 mathrm{ml} ) of ( 10 mathrm{V} mathrm{H}_{2} mathrm{O}_{2} ) solution is heated.
The evolved gas is completely reacted with Ca to form CaO. The aqueous solution of Cao is neutralised by ( 50 mathrm{m} )
of ( boldsymbol{H}_{2} boldsymbol{S} boldsymbol{O}_{4} ) solution. The molarity of
( boldsymbol{H}_{2} boldsymbol{S O} mathbf{4} ) is:
A. 2.43 M
B. 1.78 M
c. ( 1.55 mathrm{M} )
D. 2.78 м
12
1423A molal solution is one that contains
one mole of a solute in :
A. 1000 g of the solvent
B. 1000 ( mathrm{mL} ) of the solution
c. 1 litre of the solvent
D. 1000 g of the solution
12
1424The density ( left(operatorname{in} g m l^{-1}right) ) of a 3.60 M
sulphuric acid solution that is ( 29 % )
( H_{2} S O_{4}left(text { Molar mass }=98 mathrm{g} mathrm{mol}^{-1}right) mathrm{by} )
mass will be:
A .1 .64
B. 1.88
c. 1.22
D. 1.45
12
1425Calculate the amount of ( C a C l_{2} ) (molar
mass ( =111 g ) mol ( ^{-1} ) ) which must be
added to ( 500 g ) of water to lower its
freezing point by ( 2 K, ) assuming ( C a C l_{2} )
is completely dissociated. ( left(K_{f} ) for right. water ( =1.86 K k g m o l^{-1} ) )
12
1426The vapour pressure of pure benzene
and toluene at a particular temperature are ( 100 m m ) and 50 mm respectively. Then the mole fraction of benzene in
vapour phase in contact with equimolar solution of benzene and toluene is :
A . 0.67
B. 0.75
c. 0.33
D. 0.50
E . 0.20
12
1427Illustration 2.41 A certain ideal solution of two liquids A
and B has mole fraction of 0.3 and 0.5 for the vapour phase
and liquid phase, respectively. What would be the mole
fraction of B in the vapour phase, when the mole fraction of
A in the liquid is 0.25?
12
1428ustration 2.181 Two grams of benzoic acid (CH-COOH)
dissolved in 25.0 g of benzene shows a depression in freezing
point equal to 1.62 K. Molal depression constant for benzene
is 4.9 K kg-moll. What is the percentage association of acid
if it forms dimer in solution? (NCERT Example 2.12)
12
1429An ammonia solution has a density of
( 0.910 mathrm{g} mathrm{cm}^{-3} ) and is ( 25.0 % mathrm{NH}_{3} ) by mass.
What is the molarity of the solution?
A . ( 12.1 mathrm{M} )
B. 13.4 M
c. ( 14.5 mathrm{M} )
D. 15.5 M
12
1430The boiling point of 0.1molal
( boldsymbol{K}_{4}left[boldsymbol{F} boldsymbol{e}(boldsymbol{C} boldsymbol{N})_{6}right] ) solution will be :
( left(text {Given } boldsymbol{K}_{boldsymbol{b}} text {for water}=mathbf{0 . 5 2 K k g} mathbf{m o l}right. )
A ( cdot 100.52^{0} C )
В. ( 100.104^{0} C )
c. ( 100.26^{circ} mathrm{C} )
D. ( 102.6^{circ} mathrm{C} )
12
1431( frac{pi}{4} )12
1432The quantity of ( C O_{2} ) in ( 500 mathrm{ml} ) of soda
water when packed under 2.5 atm ( C O_{2} )
pressure at ( 298 mathrm{K} ) is gm ( Henry’s law constant ( 1.67 times 10^{8} ) pa at ( 298 mathrm{K} ) )
A . 0.64
B. 1.86
( c cdot 6.4 )
D. 18.6
12
1433Number of moles of solute in solution is
represented by :
A. ( M times V(L) )
в. ( M times V(m l) )
c. ( m times V(L) )
D. ( N times V(m l) )
12
1434Two liquids ( A ) and ( B ) are miscible over the whole range of composition and may be treated as ideal (obeying Raoult’s Law). At ( 350 mathrm{K} ) the vapour pressure of pure ( A ) is ( 24.0 mathrm{kPa} ) and of pure B is 12.0 kPa. A mixture of 60% A
and ( 40 % mathrm{B} ) is distilled at this
temperature; what is the pressure in a closed distillation apparatus from which air is excluded? in KPa
12
1435The composition of a sample of Wustite
is ( F e_{0.93} ) O. What is the percentage of
iron present as ( F e^{3+} ) in total iron?
A . ( 15.05 % )
B. 25%
( c .35 % )
D. ( 45 % )
12
1436Vapour pressure of ( C C l_{4} ) at ( 25^{circ} mathrm{C} ) is 143
( mathrm{mm} ) of Hg. ( 0.5 mathrm{g} ) of a non-volatile solute (mol. Mass ( =mathbf{6 5} ) ) is dissolved in ( 100 mathrm{mL} )
( boldsymbol{C C l}_{4} . ) Find the vapour pressure of the
solution: (Density of ( boldsymbol{C} boldsymbol{C l}_{4}= )
( 1.58 g / c m^{3} )
( mathbf{A} cdot 141.93 mathrm{mm} )
B. ( 94.39 mathrm{mm} )
c. ( 199.34 mathrm{mm} )
D. ( 143.99 mathrm{mm} )
12
1437Illustration 2.108 What do you understand by the term
that K, for water is 1.86 K kg mol-l?
12
1438What mass of an organic compound
( left(M w_{0}=156right) ) must be dissolved in 50
( mathrm{mL} ) of an organic solvent ( left(boldsymbol{d}=mathbf{0 . 9 g c c}^{-1}right) )
water to lower the freezing point by ( 0.48^{circ} mathrm{C} . K_{f} ) of benzene ( =5.12 )
12
1439Solubility of a gas in a liquid increases
on:
A. increasing temperature.
B. decreasing pressure.
C. increasing pressure.
D. increasing temperature and pressure
12
1440Illustration 2.194 One mole of triphenyl methanol lowers
the freezing point of 1000 g of 100% sulphuric acid twice as
much as one mole of methanol. Why?
12
1441Question 40. Determine the amount of CaCl, (i=2.47) dissolved in
2.5 L of water such that its osmotic pressure is 0.75 atm at 27°C.
First calculate the moles of CaCl, by applying van’t Hoff equation,
T = iCRT and C = MB
Then calculate amount of CaCl, by multiplying the moles with molar
mass.
12
1442Which of the following statements is true for a solution containing
components ( A ) and ( B ) and following
Raoult’s law:
A. ( A-B ) attraction force is greater than ( A-A ) and ( B- ) ( B )
B. ( A-B ) attraction force is less than ( A-A ) and ( B-B )
c. ( A-B ) attraction force remains same as ( A-A ) and ( B-B )
D. Volume of solution is different from sum of volume of solute and solvent
12
1443The volume vs. temperature graph of
mole of an ideal gas is given below.
The pressure of the gas (in atm) at
( X, Y ) and ( Z, ) respectively, are:
A. 0.328,0.820,0.820
0
B. 3.28,8.20,3.28
c. 0.238,0.280,0.280
D. 32.8,0.280,82.0
12
1444For a dilute solution containing 2.5 g of a non-volatile non-electrolyte solute in ( 100 g ) of water, the elevation in boiling point at 1 atm pressure is 2 ?. Assuming
that the concentration of solute is much
lower than the concentration of solvent,
the vapour pressure (in ( mathrm{mm} ) of ( mathrm{Hg} ) ) of the
solution is:
[Take ( : K_{b}=0.76 K k g ) mol ( ^{-1} ) ]
12
1445In which of the following solvent, the solubility of ( N a C l ) is maximum?
A. Methanol
B. water
c. Formic acid
D. Formamide
12
1446The vapour if an aqueous solution of glucose is ( 750 m m ) of ( mathrm{Hg} ) at ( 373 mathrm{K} ) Calculate molality of the solution?
A. 0.523 mol/kg
в. 0.617 mol / ( / k g )
c. 0.731 mol ( / mathrm{kg} )
D. 0.836 mol / ( / k g )
12
1447a) A solution containing ( 18 g ) of nonvolatile non-electrolyte solute is dissolved in 200 g of water freezes at 272.07 K. Calculate the molecular mass
of the solute.
Given ( : boldsymbol{K}_{boldsymbol{f}}=mathbf{1 . 8 6} mathrm{K} mathrm{kg} / mathrm{mol} )
The freezing point of water ( =273 mathrm{K} )
b) Define the isotonic solution. What
happens when the blood cell is dipped in a solution containing more than normal saline concentration?
12
1448In case a solute associates in solution,
the van’t Hoff factor is :
A ( . i>1 )
в. ( i=1 )
( c cdot i<1 )
D. None of these
12
1449Determine the pH value of ( 0.001 M )
acetic acid solution if it is ( 2 % ) ionised at
this concentration. How can the degree
of dissociation of this acetic acid
solution be increased?
12
1450Mustration 2.129 Two elements A and B form compounds
having molecular formula AB, and AB, When dissolved
in 20 g of benzene, 1 g of AB, lowers the freezing point by
2.3 K, whereas 1.0 g of AB, lowers it by 1.3 K. The molar
depression constant for benzene is 5.1 K kg mol-1. Calculate
the atomic mass of A and B.
12
1451Aqueous ( N a O H ) solution is labelled as
( 10 % ) by weight mole fraction of the
solute in it is:
A . 0.05
B. 0.0476
c. 0.052
D. 0.52
12
1452The osmotic pressure of a decimolar
solution of glucose at ( 30^{circ} mathrm{C} ) is :
( mathbf{A} cdot 24.88 mathrm{atm} )
B. 2.488 atm
( mathbf{c} .0 .248 mathrm{atm} )
D. ( 189.09 mathrm{cm} )
12
1453The mass percentage of nitrogen in
histamine is
12
1454Hlustration 2.102 Why is camphor preferred as a solvent
for measuring the molecular mass of naphthalene by Rast
method?
12
1455The vapour pressure of water at ( 20^{circ} mathrm{C} ) is 17 mm Hg. Calculate the vapour pressure of a solution containing 2.8 g
of urea ( left(N H_{2} C O N H_{2}right) ) in 50 g of water
( mathrm{N}=14, mathrm{C}=12,0=16, mathrm{H}=1(16.71 mathrm{mm} mathrm{Hg}) )
12
1456The partial pressure of ( boldsymbol{O}_{2} ) in air is 0.21 at ( m ) at sea level. If aquatic life
requires a concentration of ( boldsymbol{O}_{2} ) at least
4.16 ( m g / ) litre, will the aquatic life
sustain in sea level lake. ( boldsymbol{K}_{boldsymbol{H}} ) for ( boldsymbol{O}_{2} ) is ( 1.3 times 10^{-3} ) mol / litre – atm.
A. 0.82 mg/litre
в. ( 0.87 mathrm{mg} / ) litre
c. 0.95 mg/litre
D. ( 0.9 mathrm{mg} / ) litre
12
1457The plot of ( frac{1}{X_{A}} ) vs ( frac{1}{Y_{A}} ) (where ( X_{A} ) and
( boldsymbol{Y}_{A} ) are the mole fractions of liquid ( mathrm{A} ) in liquid and vapour phase, respectively) is linear. The slope and intercept of this plot are respectively:
( ^{mathrm{A}} cdot frac{P_{d}^{0}}{P_{B}^{0}} ) and ( frac{P_{A}^{0}-P_{B}^{0}}{P_{B}^{0}} )
в. ( frac{P_{d}^{0}}{P_{B}^{0}} ) and ( frac{P_{B}^{0}-P_{A}^{0}}{P_{B}^{0}} )
c. ( frac{P_{B}^{0}}{P_{A}^{0}} ) and ( frac{P_{A}^{0}-P_{B}^{0}}{P_{B}^{0}} )
D. ( frac{P_{B}^{0}}{P_{A}^{0}} ) and ( frac{P_{B}^{0}-P_{A}^{0}}{P_{B}^{0}} )
12
145818 g glucose is added to 178.2 g of water the vapour pressure of water for this
aqueous solution at ( 100^{0} C ) is:
A. 704 torr
B. 759 torr
c. 7.6 torr
D. None of these
12
1459The correct relationship between
enthalpy (in cal mol-1) of vaporisation
of liquid and its boiling points is?
12
1460A metal ( M ) of molar mass 96 g ( m o l^{-1} ) reacts with fluorine to form a salt that
can be represented as ( M F_{x} ). In order to determine ( x .9 .18 mathrm{g} ) of the sample of the salt is dissolved in 100 g of water and its boiling point was determined to be
( 374.38 mathrm{K} ). What is the value of ( x ) ?
Given: ( boldsymbol{K}_{boldsymbol{b}}(boldsymbol{w} boldsymbol{a} boldsymbol{t e r})=mathbf{0 . 5 1 2} boldsymbol{K} boldsymbol{k g m o l}^{-1} )
Assume complete dissociation of salt
A . ( x=2 )
в. ( x=4 )
c. ( x=5 )
D. ( x=7 )
12
1461Pure benzene freezes at ( 5.3^{circ} mathrm{C} ). A
solution of 0.223 g of phenyl acetic acid ( left(C_{6} H_{5} C H_{2} C O O Hright) ) in 4.4 g of benzene ( left(K_{f} 5.12 mathrm{K} mathrm{kg} mathrm{mol}^{-1}right) ) freezes at ( 4.47^{circ} mathrm{C} )
From the observation one can conclude
that:
A. phenyl acetic acid exists as such in benzene
B. phenyl acetic acid undergoes partial ionization in benzene
c. phenyl acetic acid undergoes complete ionization in benzene
D. phenyl acetic acid dimerizes in benzene
12
1462At ( 300 K ), two pure liquids ( A ) and ( B )
have vapour pressures ( 150 mathrm{mm} mathrm{Hg} )
and 100 mm ( H g ) respectively. In an equimolar liquid mixture of ( boldsymbol{A} ) and ( boldsymbol{B} ) the mole fraction of ( B ) in the vapour
mixture at this temperature is:
A . 0.6
B. 0.5
c. 0.8
D. 0.4
12
1463Henry’s law constant for the molality of methane in benzene at ( 298 mathrm{K} ) is ( 4.27 times )
105 mm ( H g ). Calculate the solubility of
methane in benzene at ( 298 K ) under
( 760 m m H g )
12
1464What is the molarity of ( 11.2 ~ V ) of ( H_{2} O_{2} ? )
( A cdot 1 M )
в. ( 2 M )
c. ( 5.6 M )
D. ( 11.2 M )
12
1465A mixture of two miscible liquids ( A ) and B is distilled under equilibrium
conditions at 1 atm pressure. The mole fraction of ( A ) in solution and vapour
phase are 0.30 and 0.60 respectively. Assuming ideal behaviour of the
solution and the vapour. Calculate the
ratio of the vapour pressure of pure ( A ) to that of pure ( B )
12
1466Hlustration 2.36 Benzene and toluene form nearly ideal
solution. At 298 K, the vapour pressure of pure benzene is
150 torr and of pure toluene is 50 torr. Calculate the vapour
pressure of the solution, containing equal weights of two
substances at this temperature?
12
14670.62 Why is the mass determined by measuring a colligative property in case
of some solutes abnormal? Discuss it with the help of van’t Hoff factor.
12
1468tion 2.42 Solution of two volatile liquids x and y
by Raoult’s law. At a certain temperature it is found that
when the total pressure above a given solution is 400 mm of
Ho the mole fraction of x in the vapour is 0.45 and in the
liquid is 0.65. What are the vapour pressures of two pure
liquids at the given temperature?
12
1469The Van’t Hoff factor (i) for ( K_{2} S O_{4} ) is
( A )
B. 2
( c cdot 0 )
D. 3
12
1470Vapour pressure of water is ( 360 mathrm{mm} mathrm{Hg} ) how much urea should be added to 200
ml. water to reduce its vapour pressure by ( 0.5 % ?(text { Molecular weight of urea }=60) )
12
1471Illustration 2.141 How much ethyl alcohol must be added
to 1.00 L of water so that the solution will not freeze at
-4°F ?
12
1472The molarity of ( 98 % )
( mathbf{H}_{2} mathbf{S O}_{4}(boldsymbol{d}=mathbf{1} . mathbf{8} boldsymbol{g} / boldsymbol{m} boldsymbol{L}) ) by weight is:
A. 6 .
B. 18M
c. 10 м
D. 4 M
12
1473DULULUI CUI Valen.
Ouestion 7. Why is vapour pressure of an aqueous solution of glucose
lower than that of water?
12
1474The unit of concentration may be given
by :
A. gram per millilitre (g/mı)
B. kilogram per litre (kg/I)
c. gram per litre (g/I)
D. all of the above
12
1475On the basis of composition of matter, milk is considered to be:
A . a pure substance
B. an impure substance
c. an element
D. a compound
12
1476Assertion
Van’t Hoff factor for solute showing
dissociation is always greater than for solute showing association.
Reason
number of particles whereas,
association leads to a decrease in
number of particles.
A. Both Assertion and Reason are correct and Reason is the correct explanation for Assertion
B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion
C. Assertion is correct but Reason is incorrect
D. Assertion is incorrect but Reason is correct
12
1477I to ice
2. When potassium nitrate is added to ice, it
(a) increases the melting point of ice
(b) decreases the melting point of ice
(c) does not effect the melting point of ice
(d) None of the above is correct
12
1478( 4 L ) of ( 0.02 M ) aqueous solution of ( N a C l )
was diluted by adding ( 1 L ) of water. The
molarity of the resultant solution is:
( mathbf{A} cdot 0.004 )
B. 0.008
c. 0.012
D. 0.016
12
1479What will be the molarity of ( 30 m L ) of
( 0.5 M H_{2} S O_{4} ) solution diluted to
( 500 m L ? )
( mathbf{A} cdot 0.3 M )
в. ( 0.03 M )
( c .3 M )
D. ( 0.103 M )
12
1480One litre of a sample of hard water
contains ( 55.5 mathrm{mg} ) of ( mathrm{CaCl}_{2} ) and ( 4.75 mathrm{mg} )
of ( M g C l_{2} . ) The total hardness in terms
of ppm of ( C a C O_{3} ) is :
A. 5 ppm
в. ( 10 mathrm{ppm} )
c. 20 ppm
D. none of the above
12
1481Two liquids ( A ) and ( B ) form an ideal solution. The vapour pressure of pure ( mathbf{A} ) and pure B are 66mm of Hg and 88mm of Hg, respectively. Calculate the composition of vapour ( A ) in the solution which is equilibrium and whose molar volume is ( 36 % )
A. 0.43
B. 0.70
c. 0.30
D. 0.50
12
1482Addition of which solute in 1.0 molar ( K I )
solution will not cause a change in
vapour pressure:
A ( cdot I_{2} )
B. water
c. ( H g I_{2} )
D. addition of ( N a_{2} S O_{4} )
12
1483How many grams of potassium chloride ( (K C l) ) must be added to make ( 500 mathrm{mL} )
of ( 1.00 mathrm{M} K C l ) solution?
A ( .1 .00 mathrm{g} )
B. 18.6 ( g )
c. ( 37.3 mathrm{g} )
D. 74.5 g
E. ( 149 mathrm{g} )
12
1484Assertion
Helium shows only positive deviation from ideal behaviour at room
temperature.
Reason
Helium is an inert gas.
A. Both Assertion and Reason are correct and Reason is the correct explanation for Assertion
B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion
c. Assertion is correct but Reason is incorrect
D. Both Assertion and Reason are incorrect
12
1485The Henry’s law constant for the solubility of oxygen in water is ( 3.3 times )
( 10^{-4} ) M ( / ) atm at ( 12^{circ} mathrm{C} ). Air is ( 21 mathrm{mol} % )
oxygen. How many grams of oxygen can be dissolved in one litre of a trout
stream at ( 12^{circ} mathrm{C} ) at an air pressure of 1.00
atm?
A. 0.222 g
gg ( . . .222 )
В. 0.11222 g
c. 0.333 g
D. 0.422 g
12
1486Illustration 2.196 A 0.2 molal solution of KCl freezes at
-0.68°C. If K, for H,O is 1.86, the degree of dissociation of
KCl is
a. 85%
b. 83% c. 65% d. 90%
12
1487The Van’t Hoff factor for a dilute
aqueous solution of glucose is :
A. Zero
в. 1.0
c. 1.5
D. 2.0
12
1488The substance ( A ), when dissolved in
solvent ( mathrm{B} ), shows the molecular mass
corresponding to ( A_{3} . ) The van”t Hoffs factor will be:
A.
B. 2
( c cdot 3 )
( D cdot 1 / 3 )
12
1489The vapour pressure of a pure liquid ( mathbf{A} ) is ( 40 mathrm{mm} ) of ( mathrm{Hg} ) at ( 310 mathrm{K} ). The vapour pressure of this liquid in a solution with liquid B is 32 mm of Hg. The mole fraction of ( A ) in the solution, if it obey’s Raoult’s law, is?
A . 0.8
B. 0.5
( c cdot 0.2 )
D. 0.4
12
1490Illustration 2.50 The vapour pressure of chloroform
(CHCI), and dichloromethane (CH,C1,) at 298 K is 200 mm
Hg and 415 mm Hg, respectively. Calculate
a. The vapour pressure of the solution prepared by mixing
25.5 g of CHCI, and 40 g of CH,Cl, at 298 K.
b. Mole fractions of each component in vapour phase.
(NCERT Example 2.5)
12
1491In a mixture, ( ^{prime} A^{prime} ) and ‘ ( B^{prime} ) components
show the negative deviations as:
( mathbf{A} cdot triangle V_{operatorname{mix}}>0 )
( mathbf{B} cdot triangle V_{operatorname{mix}}<0 )
C. ( A ) – ( B ) interaction is weaker than ( A-A ) and ( B-B )
interactions
D. None of the above reasons is correct
12
1492Define Henry’s law.12
1493What is vapour pressure?12
1494To make ( 50 mathrm{mL} ) solution of ( K C l ) of ( 1 mathrm{M} )
how many grams of ( K C l ) are required to add to this solution?
A ( .1 .00 mathrm{g} )
В. ( 1.86 mathrm{g} )
c. ( 3.73 mathrm{g} )
D. 7.45 g
E . ( 1.49 mathrm{g} )
12
1495In the following equilibrium ( N_{2} O_{4(g)} rightleftharpoons ) ( mathbf{2} N boldsymbol{O}_{2(boldsymbol{g})} boldsymbol{N} boldsymbol{O}_{2(g)} ) is ( mathbf{5 0 1 %} ) of the total
volume. hence degree of dissociation and vant hoff factor (i) respectively are:
A. 0.5,1.5
B. 0.25,1.25
c. 0.33,1.33
D. 0.66,1.66
12
1496Solution (by mass) of cane sugar in water has
ulate freezing point of 5% glucose in water if
Question 20. A 5% solution (by mass) of cane
freezing point 271 K. Calculate freezing point of 5% 810
freezing point of pure water is 273.15 K.
Freezing point of pure water is 273 15 K (0°C) and that of given solution is
271 K, i.e., we have depression in freezing point.
So.
0 Apply the formula of depression in freezing point for cane sugar and
make it eq (0)
(ii) Similarly, find the depression in freezing point for glucose and make it
eq (1)
(iii) Compare the two equations to find the freezing point of glucose.
12
1497( 40 % ) by weight solution will contain how much mass of the solute in 1 L solution?
Density of the solution is ( 1.2 mathrm{g} / mathrm{mL} )
A. ( 480 g )
B. ( 48 g )
( c cdot 38 g )
D. ( 380 g )
12
1498Determine the osmotic pressure of a solution prepared by dissolving 2.5
( times 10^{-2} ) of ( K_{2} S O_{4} ) in ( 2 L ) of water at
( 25^{circ} mathrm{C}, ) assuming that it is completely dissociated
( left(R=0.0821 mathrm{L} operatorname{atm} K^{-1} m o l e^{-1}, ) Molar right.
( operatorname{mass} K_{2} S O_{4}=174 mathrm{g} operatorname{mol} e^{-1} )
12
1499For a dilute solution containing 2.5 g of a non-volatile non-electrolyte solute in ( 100 mathrm{g} ) of water, the elevation in boiling
point at 1 atm pressure is ( 2^{circ} C ) Assuming concentration of solute is much lower than the concentration of
solvent, the vapour pressure (mm of Hg) of the solution is:
( left[boldsymbol{K}_{boldsymbol{b}}=mathbf{0 . 7 6} boldsymbol{K} boldsymbol{K} boldsymbol{g} boldsymbol{m o l}^{-1}right] )
A . 724
в. 740
( c cdot 736 )
D. 718
12
1500A solution of 10 g of a nonvolatile binary electrolyte (mat. wt. ( =100 ) ) in 500 g of
water freezes at ( -0.74^{circ} mathrm{C} ). What is the
degree of ionisation? ( left[k_{f} text { of water }=1.85 K text { molality }^{-1}right] )
A . 50%
B. 75%
c. ( 100 % )
D. 0%
12
1501Mole fraction of solute present in an aqueous solution having molality equal to 2 is:
A . 0.9653
B. 0.347
c. 0.653
D. 0.0347
12
1502f at a particular temperature, the density of ( 18 ~ M ~ H_{2} S O_{4} ) is ( 1.8 ~ g c m^{-3} )
then calculate the molality of the
solution:
12
1503How many moles of glucose ( left(C_{6} H_{12} O_{6}right) ) should be dissolved into a solution with
a total volume of ( 0.500 L ) to produce a
1 ( M ) glucose solution?
( mathbf{A} cdot 1 mathrm{mol} )
B. 24mol
( c .0 .5 mathrm{mol} )
D. 0.25 mol
12
1504How much water, in liters, must be added to 0.5 L of 6 M HCl to make it 2 M?
A . 0.33
B. 0.5
( c cdot 1 )
D. 1.5
( E cdot 2 )
12
1505Which of the following statements is correct, if the intermolecular force of
attraction between the particles in liquid ( A, B, C ) is in the order ( A<B<C ? ) This question has multiple correct options
A. All the three evaporate at the same rate
B. B evaporates faster than A
c. B evaporates more readily than ( c )
D. A evaporates more readily than
12
1506Q. 52 Assertion (A) When methyl alcohol is added to water, boiling point of
water increases.
Reason (R) When a volatile solute is added to a volatile solvent
elevation in boiling point is observed.
12
1507A sugar syrup of weight ( 214.2 mathrm{g} )
contains 34.2 g of sugar ( left(C_{12} H_{22} O_{11}right) ) Calculate. the molal concentration
(Write your answer as ( 18 X ), where, ( X= ) molality)
12
1508In which of the following pairs of solutions will the values of the Van’t
Hoff factor be the same?
A ( cdot_{0.05} ) M ( K_{4}left[text { Fe }(C N)_{6}right] ) and 0.10 M FeSO( _{4} )
B. 0.20 М NaCl and 0.10 М Ва С( l_{2} ),
c. ( _{0.05} ) M FeSO( _{4}left(N H_{4}right)_{2} ) SO( _{4} ). ( 6 H_{2} ) O and 0.02 M
КСl.М ( g C l_{2} .6 H_{2} O )
D. All have same value
12
1509The degree of dissociation of
( boldsymbol{C a}left(boldsymbol{N O}_{3}right)_{2} ) in a dilute aqueous
solution containing ( 7 g ) of the salt per ( 100 g ) of water at ( 100^{circ} C ) is ( 70 % ). If the vapour pressure of water at ( 100^{circ} mathrm{C} ) is
( mathbf{7 6 0} boldsymbol{m m}, ) calculate the vapour pressure of the solution.
( mathbf{A} .378 .5 mathrm{mm} )
В. ( 492.8 mathrm{mm} )
c. ( 746.10 m m )
D. ( 985.6 mathrm{mm} )
12
1510The values of the Henry’s law constant
of ( A r, C O_{2}, C H_{4} ) and ( O_{2} ) in water at
( 25^{0} C ) are 40.30,1.67,0.41 and
( 34.86 k b a r, ) respectively. The order of
their solubility in water at the same
temperature and pressure is:
A. ( A r>O_{2}>C O_{2}>C H_{4} )
в. ( C H_{4}>C O_{2}>A r>O_{2} )
c. ( C H_{4}>C O_{2}>O_{2}>A r )
D. ( A r>C H_{4}>O_{2}>C O_{2} )
12
1511Which of the following statements is
false?
A. Two different solutions of sucrose of same molality prepared in different solvents will have the same depression in freezing point.
B. The osmotic pressure of a solution is given by the equation ( pi=C R T ) (where ( C ) is the molarity of the
solution)
C. Decreasing order of osmotic pressure for ( 0.01 M ) aqueous solutions of barium chloride, potassium chloride, acetic acid and sucrose is ( B a C l_{2}>K C l> )
( C H_{3} C O O H> ) sucrose
D. According to Raout’s law the vapour pressure exerted by a volatile component of a solution is directly proportional to its mole fraction in the solution
12
1512Van’t Hoff factor, (i), of a ( 0.5 % ) (w/W)
aqueous solution of ( K C l ) which freezes
at ( -0.24^{circ} mathrm{C} ) is:
( left(K_{f} text { of water }=1.86 mathrm{K} mathrm{kg} text { mol}^{-1}right. )
molecular weight of ( K C l=74.5 ) )
A . 1.52
B. 2.32
c. 1.92
D. 1.32
12
1513A compound ( M X_{2} ) has observed
and normal molar masses 65.6 and 164
respectively. The apparent degree of
ionization of ( M X_{2} ) is:
A . ( 75 % )
B. ( 85 % )
c. ( 65 % )
D. ( 25 % )
12
1514An ideal binary solution is prepared by
two liquids ( A ) and ( B, ) with ( p_{A}^{o}>p_{B}^{o} . ) Then :
A. A-B interactions are stronger than A-A and B-B
B. A and B have same molecular masses
c. A-B interactions are similar to A-A and B-B interactions
D. Both A and B are non-polar substances
12
1515Illustration 2.74 Calculate the vapour pressure lowering
caused by the addition of 68.4 g of sucrose (molecular mass
= 342) to 500 g of water if the vapour pressure of pure water
at 25°C is 20.0 mm Hg.
12
1516( 68 % H N O_{3} ) and ( 32 % H_{2} O ) by mass forms:
A. Maximum boiling azeotrope
B. Minimum boiling azeotrope
C. mixture which shows positive deviation
D. Ideal solution
12
1517Each pair forms ideal solution except :
A ( cdot C_{2} H_{5} B r ) and ( C_{2} H_{5} )
B . ( C_{6} H_{5} C l ) and ( C_{6} H_{5} B r )
c. ( C_{6} H_{6} ) and ( C_{6} H_{5} cdot C H_{3} )
D. ( C_{2} H_{5} I ) and ( C_{2} H_{5} O H )
12
1518The vapor pressure of water at ( 80^{circ} mathrm{C} ) is
355 torr. ( A ) 100 ( m l ) vessel contained
water-saturated oxygen at ( 80^{circ} mathrm{C} ) the
total gas pressure being 760 torr. The contents of the vessel were pumped into a ( 50.0 mathrm{ml} ), vessel at the same
temperature, What were the partial pressure of oxygen and of water vapor
what was the total pressure in the final equilibrated state? Neglect the volume of any water which might condense.
12
1519Derive the relationship between relative lowering of vapour pressure and molar mass of non-volatile solute.12
1520A concentrated solution of lead nitrate
in water can be stored in
A. an iron vessel
B. a copper vessel
c. a zinc vessel
D. a magnesium vessel
12
1521( 25 mathrm{cm}^{3} ) of oxalic acid completely
neutralised ( 0.064 g ) of sodium
hydroxide. Molarity of the oxalic acid solution is :
в. 0.032 м
c. 0.064 м
D. 0.015 М
12
1522Hlustration 2.197 A mixture of 0.1 mol of Na, and 0.1 mol
of BaO is dissolved in 1000 g of H,O. Calculate the vapour
pressure of solution at 373 K.
12
1523Illustration 2.96 Calculate the molar mass of a substance
1g of which when dissolved in 100 g of water gave a solution
boiling at 100.1°C at a pressure of 1 atm (Kfor water
= 0.52 K kg mol-l)
12
1524In a 0.2 molal aqueous solution of a weak acid HX, the degree of ionization
is ( 0.3 . ) taking ( K_{f} ) for water as ( 1.85, ) the freezing point of the solution will be
nearest to:
A. -0.360
B. -0.260
c. +0.480
D. -0.481
12
1525Solute when dissolved in water:
A. increases the vapour pressure of water
B. decreases the boiling point of water
C . decreases the freezing point of water
D. all of the above
12
1526State True or False.
In association of solute, the Van’t Hoff
factor is greater than unity.
A. True
B. False
12
1527What would be the change in
the freezing point of ( H_{2} O ) in a solution
of ( 1 m N a C l(a q) ? )
( mathbf{A} cdot-1.86^{circ} mathrm{C} )
B. ( -0.52^{circ} mathrm{C} )
c. ( -3.72^{circ} mathrm{C} )
D. ( 1.86^{circ} mathrm{C} )
E ( .3 .72^{circ} mathrm{C} )
12
1528( K_{2} H g I_{4} ) is ( 40 % ) ionised in aqueous solution. The value of its van’t Hoff
factor (i) is:
A. 1.8
B. 2.
c. 2.0
D. 1.
12
1529For a very dilute solution of ( boldsymbol{H}_{3} boldsymbol{P} boldsymbol{O}_{3} )
Van’t Hoff factor is:
( mathbf{A} cdot i=7 )
B. ( i=3 )
( c cdot i=4 )
( mathbf{D} cdot i=5 )
12
15305. A 5% solution of cane sugar (molecular weight = 342) is
isotonic with a 1% solution of substance X. The molecular
weight of X is
a. 342 b. 171.12 c. 65.6
d. 136.8
12
1531The conductivity of 0.001 mol ( L^{-1} ) acetic
acid is ( 5 times 10^{-5} s c m^{-1} ). Calculate it’s
dissociation constant if ( lambda_{m}^{o} ) m for acetic
( operatorname{acid} ) is ( 250 operatorname{scm}^{2} m o l^{-1} ? )
12
1532Illustration 2.131 Two aqueous solution containing,
respectively, 7 g urea (molar mass = 60 g) and 42 g of
substance X in 100 g of water freeze at the same temperature.
Calculate the molecular weight of X.
12
1533The addition of 0.643 g of a compound to ( 50 mathrm{mL} ) of benzene (density ( 0.879 g m L^{-1} ) ) lowers the freezing point
from 5.51 to ( 5.03^{circ} mathrm{C} . ) If ( K_{f} ) for benzene is
( mathbf{5 . 1 2} boldsymbol{K} / boldsymbol{m}, ) calculate the molecular
weight of the compound.
12
1534The strength of 11.2 volume solution of
( H_{2} O_{2} ) is: ( [ ) Given that molar mass of
( boldsymbol{H}=mathbf{1} boldsymbol{g} boldsymbol{m o l}^{-1} ) and ( boldsymbol{O}=mathbf{1 6} boldsymbol{g} boldsymbol{m o l}^{-1} mathbf{j} )
A . ( 13.6 % )
в. ( 3.4 % )
( c .34 % )
D. ( 1.7 % )
12
1535The degree of dissociation of an electrolyte is ( alpha ) and its van’t Hoff factor
is ( i ). The number of ions obtained by complete dissociation of 1 molecule of the electrolyte is:
A. ( frac{i+alpha-1}{alpha} )
B. ( i-alpha-1 )
c. ( frac{i-1}{alpha} )
D. ( frac{i+alpha+1}{1-alpha} )
12
1536State Henry’s law and mention some
important applications?
12
153734. Vapour pressure of water at 293 K is 17.535 mm Hg.
alculate the vapour pressure of water at 293 K when 25 g of glucose is
dissolved in 450 g of water.
As vapour pressure is changing, Apply Raoult’s law, for the relative
l owering of vapour pressure to calculate vapour pressure of water.
F
12
1538( 100 mathrm{ml} ) of liquid ( mathrm{A} ) and ( 25 mathrm{ml} ) of liquid ( mathrm{B} ) is mixed to give a solution which does not obey Raoult’s law. The volume of the
solution:
A. will be 125 ( mathrm{m} ) ।
B. can be > or < than 125 ( mathrm{m} )
c. can be greater than, equal to or less than ( 125 mathrm{m} )
D. will be less than 125 ( mathrm{m} ) ।
12
1539A 0.5 m solution could be prepared by dissolving 20 g NaOH in:
A . 0.5 L water
B. 0.5 kg water
c. 1 L water
D. 1 kg water
E. 2 L water
12
1540A monoprotic acid in a ( 0.1 mathrm{M} ) solution
ionizes to ( 0.001 % ). Its ionization
constant is:
A ( cdot 1.0 times 10^{-3} )
В. ( 1.0 times 10^{-6} )
c. ( 1.0 times 10^{-8} )
D. ( 1.0 times 10^{-1} )
12
1541How many mL of a solution of
concentration ( 100 mathrm{mg} ) Co( ^{2+} ) per mL is
needed to prepare ( 10 mathrm{mL} ) of a solution of
concentration ( 20 mathrm{mg} mathrm{Co}^{2+} ) per ( mathrm{mL} ) ?
12
1542( 10 % ) of urea is isotonic with ( 6 % ) solution
of a non-volatile solute ( X . ) What is the
molecular mass of solute ( boldsymbol{X} ) ?
A ( cdot 6 g ) mol ( ^{-1} )
B. ( 60 g ) mol ( ^{-1} )
c. ( 36 g ) mol ( ^{-1} )
D. ( 32 g ) mol ( ^{-1} )
12
1543If ( N_{2} ) gas is bubbled through water at
( 293 K ), Calculate solubility of ( N_{2} ) gas?
Assume that ( N_{2} ) exerts a partial pressure of 0.987 bar. Given that
Henry’s law constant for ( N_{2} ) at ( 293 K ) is ( mathbf{7 6 . 4 8} frac{boldsymbol{k} text { bar }}{text { mole } / text { litre }} )
A ( cdot 1.29 times 10^{-5} ) litree
В. ( _{1.29} times 10^{-4} frac{text { тоде }}{text { litre }} )
с. ( _{2.9} times 10^{-3} ) mole
D. ( 2.9 times 10^{-5} ) mole
12
1544Assertion
Azeotropic mixtures are formed only by non-ideal solutions and they may have boiling points either greater than both the components or lesser than both the
components.
Reason
The composition of the vapour phase is same as that of the liquid phase of an azeotropic mixture.
A. Both Assertion and Reason are correct and Reason is the correct explanation for Assertion
B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion
C. Assertion is correct but Reason is incorrect
D. Both Assertion and Reason are incorrect
12
1545What osmotic pressure would the 1.25 molal sucrose solution exhibit at ( 25^{circ} mathrm{C} ) ?
(The density of this solution is 1.34 ( g / m L )
( mathbf{A} cdot 28.70 mathrm{atm} )
B. 30.22 atm
c. 21.72 atm
D. 24.55 atm
12
1546A super saturated solution is a meta
stable state of solution in which solute
concentration:
A. is equal to the solubility of that substance in water
B. is more than its solubility
c. is less than its solubility
D. continuously changes
12
1547( 1.525 g ) of an organic compound was kjeblahlised and the ammonia so produced was passed through ( 30 m l ) of 1 ( N ) HCl.The remaining ( H C l ) was
further neutralised by 120 ml of ( frac{N}{10} N a O H ) solution. Calculate the ( % ) nitrogen in the compound.
12
1548The concentration of ( K^{+} ) ion in ( 0.1 mathrm{M} )
( K_{2} C r_{2} O_{7} ) solution is ( x ) M. The value of
( 10 x ) is
12
1549The boiling point of a solution containing ( 68.4 mathrm{g} ) of sucrose (molar
( left.operatorname{mass}=342 g operatorname{mol}^{-1}right) operatorname{in} 100 ) g of water
is:
( left[K_{b} text { for water }=0.512 mathrm{K} mathrm{kg} text { mol}^{-1}right] )
A ( cdot 101.02^{circ} mathrm{C} )
B . ( 100.512^{circ} mathrm{C} )
c. ( 100.02^{circ} mathrm{c} )
D. ( 98.98^{circ} mathrm{C} )
12
1550Which of the following is most soluble?
A ( cdot B i_{2} S_{3}left(K_{s p}=1 times 10^{-17}right) )
B . ( operatorname{MnS}left(K_{s p}=7 times 10^{-16}right) )
c. ( C u Sleft(K_{s p}=8 times 10^{-37}right) )
D. ( A g_{2} Sleft(K_{s p}=6 times 10^{-51}right) )
12
1551Illustration 2.109 Calculate the molal depression constant
of a solvent which has
a. Freezing point 16.6°C and latent heat of fusion
180.75 J g-1.
b. Freezing point 20.0°C and latent heat of fusion
200.00 Jg-1
12
1552If the mole fraction of a solute is
changed from ( frac{1}{4} ) to ( frac{1}{2} ) by adding some
solute in 800 g of ( H_{2} O ) solvent, then the ratio of molarity of two solutions will be:
A . 1: 3
B. 1: 4
( c cdot 2: 3 )
D. 1: 2
12
1553State True or False.
On hills, water boils quickly.
A. True
B. False
12
1554If air is taken as a binary solution, the
solvent is:
( A cdot N_{2} )
B. ( 0_{2} )
( c cdot c O_{2} )
D. Ar
12
1555Q. 41 Why are aquatic species more comfortable in cold water in comparision
to warm water?
12
1556The Henr’s law constant for ( mathrm{N}_{2}, mathrm{O}_{2} ) and
( mathrm{CO}_{2} ) in water are 1600,780 and 29 atm
M-1, respectively. Which of these gases has the highest concentration in a
sample of water at 25 degrees ( C ) when
the gas pressure over the water is 1.0 atm?
( A cdot N_{2} )
B. 0,2
( c cdot c O_{2} )
12
1557Solubility is the amount of the present in the saturated solution at a
particular temperature
A. solute
B. solvent
c. dispersed phase
D. dispersed medium
12
1558What will be the abnormal molecular
( operatorname{mass} ) of ( mathrm{K}_{3}left[mathrm{Fe}(mathrm{CN})_{6}right] . ) If in a aqueous
solution it is ( 40 % ) dissociated? (Given, normal molecular weight of
( left.mathbf{K}_{3}left[mathbf{F e}(mathbf{C N})_{6}right] text { is } 329right) )
A . 149.54
B. 723.8
c. 82.25
D. 329.0
12
1559Which of the following solutions has the more capacity dissolve the solute in the
solvent?
A. Saturated solution
B. Unsaturated solution
c. super saturated solution
D. None of the above
12
1560Which gas is more soluble in water, ( boldsymbol{O}_{2} )
or ( N_{2} ? )
12
1561When ( C u S O_{4} ) is added to a solution of
ammonia?
A. Freezing point is lowered
B. Freezing point is raised
c. Boiling point is raised
D. Both (1) and (2)
12
1562Question 4. Concentration terms such as mass percentage, ppm, mole
fraction and molality are independent of temperature. However, molarity
is a function of temperature. Explain.
12
1563Calculate the osmotic pressure at ( 25^{circ} mathrm{C} ) of a solution containing 1 g of glucose and 1 g of sucrose in 1 litre of solution. If it were not known that the solute was
a mixture of glucose and sucrose, what would be the molecular weight of solute corresponding to the calculated osmotic pressure?
12
1564How many grams of carbon dioxide gas is dissolved in a 1 L bottle of carbonated
water if the manufacturer uses a
pressure of 2.4 atm in the bottling
process at ( 25^{circ} mathrm{C} ? )

Given: ( K_{H} ) of ( C O_{2} ) in water ( =29.76 )
( operatorname{atm} /(operatorname{mol} / L) ) at ( 25^{circ} mathrm{C} )
A. ( 3.88 mathrm{g} )
B. 4.90 g
c. ( 5.33 mathrm{g} )
D. 3.52 g

12
1565Illustration 2.43 Liquids X and Y form an ideal solution.
The vapour pressure of X and Y at 100°C are 300 and 100
mm of Hg, respectively. Suppose that a solution composed of
1 mol of X and 1 mol of Y at 100°C is collected and condensed.
This condensate is then heated at 100°C and vapour is again
condensed to form a liquid A. What is the mole fraction of
X in A?
12
1566(a) Give two differences between Ideal
and non-Ideal solutions.
(b) Find out osmotic pressure of Glucose solutions of ( 5 % ) solution at
( 25^{circ} mathrm{C} ) temperature while molecular
mass of Glucose 180 and ( R=0.0821 )
Litre Atmosphere.
12
1567Define the following terms:
(i) Molality (m)
(ii) Abnormal molar mass
12
1568A mixture of ethyl alcohol and propyl
alcohol has vapour pressure of ( 290 m m ) at ( 300 K . ) The vapour pressure of propyl alcohol is 200 mm. If mole fraction of
ethyl alcohol is 0.6 its vapour presssure at same temperature will be:-
A . 360
в. 350
( c .300 )
D. 700
12
1569The mole fraction of ( C_{2} H_{4} ) in the mixture is :
A . 0.25
в. 0.75
( c .0 .45 )
D. 0.55
12
1570A solution of known concentration is
known as:
A. molar solution
B. normal solution
C. mole solution
D. standard solution
12
1571For strong electrolytes, van’t Hoff factor i’ equals to total number of
(ions/atoms) in the formula unit
12
1572A solution made by dissolving 0.32 g of a new compound in 25 g of water has freezing point ( -2.201^{circ} mathrm{C} . ) Calculate the molecular mass of the new compound.
A . 218.4
в. ( 118 . )
c. 318.4
D. 10.81
12
1573If two liquids ( A ) and ( B ) form minimum
boiling azeotrope at some specific
composition then:
A. ( A ) -B interactions are stronger than those between ( A-A ) or B-B
B. vapour pressure of solution increases because more number of molecules of liquids ( A ) and ( B ) can escape from the solution
C. vapour pressure of solution decreases because less number of molecules of liquids ( A ) and ( B ) can escape from the solution
D. show a large positive deviation from Raoult’s law
12
1574Column II gives method to separate phases mentioned in column I. Match
them and select the correct answer
from the codes given below.
Column Column I
(a) Miscible liquids
(p) Distillation
( (q) )
(b) Immiscible liquids ( quad ) Crystallization
(c) Pure copper sulphate from
( (r) )
an impure sample Sublimation
(s) Separating
(d) Salt and ammonium chloride funnel
( A cdot(a)-(q),(b)-(s),(c)-(p),(d)-(r) )
B. ( (a)-(p),(b)-(s),(c)-(q),(d)-(r) )
( c cdot(a)-(r),(b)-(s),(c)-(p),(d)-(q) )
D. (a) – (r), (b) – (s), (c) – (q), (d) – (p)
12
1575A solution that obeys Raoult’s law is:
A. non-ideal
B. colliod
( c . ) ideal
D. saturate
12
1576For an ideal liquid solution, which of the
following is unity?
A. Activity coefficient
B. Fugacity coefficient
c. Fugacity
D. Activity
12
1577Tlustration 2.116 On dissolving 0.25 g of a non-volatile
substance in 30 mL benzene (density 0.8 g mL-‘), its freezing
point decreases by 0.25°C. Calculate the molecular mass of
non-volatile substance (K, = 5.1 K kg mol-?).
12
1578( 5 g ) of ( N a C l ) can be dissolved in ( 50 g ) water
Then the solubility of ( N a C l ) is:
( mathbf{A} cdot 10 g )
B. ( 5 g )
c. ( 20 g )
D. none of the above
12
1579What is the quantity of NaOH present in ( 250 mathrm{cc} ) of the solution, so that it gives a
( mathrm{pH}=13 ? )
A ( cdot 10^{-13} mathrm{g} )
B . ( 10^{-1} mathrm{g} )
( c .1 .0 mathrm{g} )
D. ( 4.0 mathrm{g} )
12
1580In 1 L saturated solution of
( A g C lleft[K_{s p}(A g C l)=1.6 times 10^{10}right], 0.1 mathrm{mol} )
of ( boldsymbol{C u} boldsymbol{C l}left[boldsymbol{K}_{s p}(boldsymbol{C u} boldsymbol{C l})=mathbf{1 . 0} times mathbf{1 0}^{-mathbf{6}}right] ) is
( A g^{+} ) in the solution is ( 1.6 times 10^{-x} ). The
value of ( x ) is:
12
1581A ( 10 % ) (w/w) solution of cane sugar has
undergone partial inversion according
to the reaction:
sucrose ( + ) water ( rightarrow ) glucose ( + ) fructose The boiling point of the solution is
( 100.7^{circ} mathrm{C} . ) What fraction of sugar has
inverted? ( left[boldsymbol{K}_{boldsymbol{b}}left(boldsymbol{H}_{mathbf{2}} boldsymbol{O}right)=mathbf{1 . 8} boldsymbol{K} boldsymbol{g} boldsymbol{K} boldsymbol{m o l}^{-1}right] )
A. 0.5
B. 0.2
( c cdot 0.3 )
D. 0.4
12
1582For an infinitely dilute aqueous solution, molality will be equal to:
A. formality
B. molarity
c. mole fraction
D. ppm
12
1583Illustration 2.152 What will happen if pressure greater than
the osmotic pressure is applied on the solution separated by
a semi-permeable membrane from the solvent?
12
1584When ( C a(O H)_{2} ) attains solubility equilibrium, the:
A. solution is saturated
B. ( p H ) will be less than 7
C . trial ( K_{s p} ) is less than the ( K_{s p} )
D. concentrations of the ions are equal
12
1585The osmotic pressure of a ( 5 % ) solution of cane sugar (molecular mass 342 ) at
( 15^{circ} C ) is:
( A cdot 3.46 ) atm
B. 3.64 atm
c. 4.0 atm
D. 2.45 atm
12
1586The latent heat of fusion of ice is 80
calories per gram at ( 0^{circ} ) C. What is the
freezing point of a solution of KCl in water containing 7.45 grams of solute 500 grams of water, assuming that the salt is dissociated to the extent of ( 95 % ? )
( mathbf{A} cdot T_{f}=-0.73^{circ} mathrm{C} )
B. ( T_{f}=-0.92^{circ} mathrm{C} )
c. ( T_{f}=-1.46^{circ} mathrm{C} )
( mathbf{D} cdot T_{f}=-1.84^{circ} mathrm{C} )
12
1587Some substances completely disappear
or dissolve in water. We say that these substances are in water.
A . immiscible
B. soluble
c. insoluble
D. none of the above
12
1588The volume of ( 1.5 mathrm{M} mathrm{H}_{2} mathrm{SO}_{4} ) required to
completely neutralize ( 150 mathrm{mL} ) of ( 2 mathrm{M} ) NaOH solution is
A . 150 ( mathrm{mL} )
B. 200 mL
( c .100 mathrm{mL} )
D. 250 mL
12
1589The mole fraction of a solute in a
solution is ( 0.1 . ) At ( 298 mathrm{K} ), molarity of this solution is the same as its molality Density of this solution at ( 298 K ) is
( 2.0 g mathrm{cm}^{-3} . ) The ratio of the molecular
weights of the solute and solvent, ( left(frac{M W_{text {solute}}}{M W_{text {solvent}}}right) ) is:
12
1590The molarity of 600 g ( H_{2} ) O is ?
A. 50
B. 55.5 M
c. 33.10
D. Cannot be calculated
12
15910.61 How can you remove the hard calcium carbonate layer of the egg
without damaging its semipermeable membrane? Can this egg be
inserted into a bottle with a narrow neck without distorting its shape?
Explain the process involved.
Thinking Process
The question can be answered using the concept of solubility, osmosis, reverse-osmosis,
hypertonic solution and hypotonic solution
12
1592The vapour pressure of ethanol and methanol are ( 44.5 mathrm{mm} ) and ( 88.7 mathrm{mm} mathrm{Hg} ) respectively. An ideal solution is
prepared at the same temperature by mixing 60 g of ethanol with 40 gof methanol. The total vapour pressure of the solution is:
A. ( 67.13 mathrm{mm} ) Hg
B. 66.13 ( mathrm{mm} ) Нв
c. ( 76.13 mathrm{mm} ) нв
D. None of the above
12
1593( 5.5 m g ) of nitrogen gas dissolves in ( 180 g ) of water at ( 273 K ) and one atm
pressure due to nitrogen gas. The mole fraction of nitrogen in ( 180 g ) of water at
5 atm nitrogen pressure is approximately:
A ( cdot 1 times 10^{-5} )
B. ( 1 times 10^{-4} )
c. ( 1 times 10^{-6} )
D. ( 1 times 10^{-3} )
12
1594Find the correct statement about the
solubility of a solution?
A. Gases decrease in solubility with an increase in temperature
B. ( N a C l ) is insoluble in water
( mathbf{C} cdot P b l_{2} ) is soluble in water
D. All nitrates are insoluble in water
E. Solubility depends solely upon the amount of solvent used
12
1595(i) What is meant by positive deviations from Raoult’s Law ? Give an example.
(ii) What is the sign of ( Delta_{m i x} H ) for positive derivation?
12
1596At ( 25^{circ} C, ) the total pressure of an ideal solution obtained by mixing 3 mole of ( A ) and 2 mole of ( mathrm{B} ), is 184 torr. What is the
vapour pressure (in torr) of pure ( mathrm{B} ) at the same temperature (Vapour pressure of
pure ( A ) at ( 25^{circ} C ) is 200 torr.)?
A . 180
B. 160
( c cdot 16 )
D. 100
12
1597For an ideal binary liquid solution with
( P_{A}^{circ}>P_{B}^{circ}, ) which relation between ( X_{A} )
(mole fraction of ( A ) in liquid phase) and
( Y_{A}(text { mole fraction of } A text { in vapour phase }) )
is correct?
( mathbf{A} cdot Y_{A}X_{B} )
c. ( frac{Y_{A}}{Y_{B}}>frac{X_{A}}{X_{B}} )
D. ( frac{T_{A}}{Y_{B}}<frac{X_{A}}{X_{B}} )
12
1598At ( 25^{circ} C, ) the vapour pressure of methyl alcohol is 96.0 torr. The mole fraction of
( C H_{3} O H ) in solution in which the
(partial) vapor pressure of ( boldsymbol{C} boldsymbol{H}_{3} boldsymbol{O H} ) is 23.0 torr at ( 25^{circ} C ) is ( frac{x}{y} . ) Find ( y-x )
12
1599A 0.4 molal aqueous solution of ( boldsymbol{M}_{boldsymbol{x}} boldsymbol{A} )
has freezing point ( 3.72^{circ} mathrm{C} ). The ( K_{f} ) of
( H_{2} O ) is ( 1.86 K m o l a l i t y^{-1} . ) The value of ( x ) is :
12
1600Calculate the concentration of ( C O_{2} ) in a
soft drink that is bottled with a partial
pressure of 4 atm over the liquid at
( 25^{circ} mathrm{C} . ) The Henry’s law constant for ( C O_{2} )
in water at ( 25^{circ} mathrm{C} ) is ( 3.1 times )
( 10^{-2} ) atm / mole ( – ) litre.
A. 0.129 mol/litre
в. 129.03 mol/litre
c. 0.224 mol / litre
D. 224.3 mol/litre
12
1601Q. 26 Kh value for Ar(g), CO2 (g), HCHO (g) and CH. (g) are 40.39, 1.67,
1.83 x 10-5 and 0.413 respectively.
Arrange these gases in the order of their increasing solubility.
(a) HCHO < CH, <CO, < Ar (b) HCHO < CO, < CH, < AT
(c) A < CO,< CH < HCHO (d) AC – CH = CO2 < HCHO
Thinking Process
Higher the value of Ky at a given pressure, the lower is the solubility of the gas in the
liquid
12
1602The vapour pressure of a solution
having ( 2.0 g ) of solute ( X ) (gram atomic
( left.operatorname{mass}=32 g operatorname{mol}^{-1}right) operatorname{in} 100 g ) of ( C S_{2} )
(vapour pressure ( =854 text { torr }) ) is 848.9 torr. The molecular formula of the solute
is:
( mathbf{A} cdot X )
в. ( X_{2} )
( c cdot X_{4} )
D. ( X_{8} )
12
1603Illustration 2.159 18 g glucose and 6 g urea are dissolved
in 1 L aqueous solution at 27°C. The osmotic pressure of the
solution will be
a. 8.826 atm
b. 4.926 atm
c. 2.92 atm
d. 4.42 atm
12
1604I. ( 2 M n^{2+}(a q)+4 O H^{-}(a q)+ )
( O_{2}(g) rightarrow 2 M n O_{2}(s)+2 H_{2} O(l) )
II. ( M n O_{2}(s)+2 I^{-}(a q)+ )
( 4 H^{+}(a q) rightarrow M n^{2+}(a q)+I_{2}(a q)+ )
( 2 H_{2} O(l) )
III. ( 2 S_{2} O_{3}^{2-}(a q)+I_{2}(a q) rightarrow )
( boldsymbol{S}_{4} boldsymbol{O}_{mathbf{6}}^{2-}(boldsymbol{a} boldsymbol{q})+boldsymbol{2} boldsymbol{I}^{-}(boldsymbol{a} boldsymbol{q}) )
Dissolved oxygen in water is determined by using the given redox reactions.When ( 3 times 10^{3} ) moles ( O_{2} ) is
dissolved per litre of water, then
what will be the molarity of ( I^{-} ) produced
in the given reaction?
A ( cdot 3 times 10^{-3} ) М
В. ( 4 times 3 times 10^{-3} mathrm{M} )
c. ( 2 times 3 times 10^{-3} ) М
D. ( frac{1}{2} times 3 times 10^{-3} mathrm{M} )
12
1605What will be the molality of a solution of glucose in water which is ( 10 % boldsymbol{w} / W ? )
( mathbf{A} cdot 0.01 m )
в. 0.617 т
( c .0 .668 m )
D. 1.623 m
12
1606If a solute under goes dimerization and trimerization, the minimum values
of the vant Hoff factors are:
A. 0.50 and 1.50
B. 1.50 and 1.33
( c .0 .50 ) and 0.33
D. 0.25 and 0.67
12
1607A soluction contains ( 7 g ) of solute (molar ( operatorname{mass} 210 g operatorname{mol}^{-1} ) ) in ( 350 g ) of acetone
raised the boiling point of acetone from
( 56^{circ} C ) to ( 56.3^{circ} C )
The value of ebullioscopic constant of acetone in ( K . K g m o l^{-1} ) is:
A . 2.66
в. 3.15
c. 4.12
D. 2.86
12
1608Number of moles of the solute per
kilogram of the solvent is:
A. mole fraction
B. molality
c. molarity
D. molar mass
12
1609Two closed vessels of an equal volume
containing air at pressure ( P_{1} ) and
temperature ( T_{1} ) are connected to each
other through a narrow tube. If the temperature in one of the vessels is now
maintained at ( T_{1} ) and that in the other
at ( T_{2}, ) what will be the pressure in the
vessels?
A ( cdot frac{2 P_{1} T_{1}}{T_{1}+T_{2}} )
в. ( frac{T_{1}}{2 P_{1} T_{2}} )
c. ( frac{2 P_{1} T_{2}}{T_{1}+T_{2}} )
D. ( frac{2 P_{1}}{T_{1}+T_{2}} )
12
16107. The vapour pressure at a given temperature of an ideal
solution containing 0.2 mol of non-volatile solute and 0.8
mol of a solvent is 60 mm of Hg. The vapour pressure of
the pure solvent at the same temperature will be
a. 120 mm Hg
b. 150 mm Hg
c. 60 mm Hg
d. 75 mm Hg
12
1611Which of the following liquid pairs shows a positive deviation from Raoults law?
A. Water hydrochloric acid
B. Acetone chloroform
c. water nitric acid
D. Benzene methanol
12
1612Sulphuric acid is ( 95.8 % ) by mass.
Calculate mole fraction of ( boldsymbol{H}_{2} boldsymbol{S} boldsymbol{O}_{4} ) of
density ( 1.91 mathrm{cm}^{-3} .(H=1, S= )
( mathbf{3 2}, boldsymbol{O}=mathbf{1 6}) )
A . 0.8950
B. 0.2982
c. 0.2056
D. 0.8075
12
1613Hlustration 2.33 The vapour pressure of methyl alcohol
at 298 K is 0.158 bar. The vapour pressure of this liquid in
solution with liquid B is 0.095 bar. Calculate the mole fraction
of methyl alcohol in the solution if the mixture obeys Raoult’s
law.
12
1614( 4.28 mathrm{g} ) of ( mathrm{NaOH} ) is dissolved in water and the solution is made to 250 cc. What
will be the molarity of the solution?
A . 0.615 mol ( L^{-1} )
B. 0.428 mol ( L^{-1} )
c. 0.99 mol ( L^{-1} )
D. 0.301 mol ( L^{-1} )
12
1615Deliquescent substances absorb moisture from the air ( & ) changes into a solution.
A. True
B. False
12
1616The equilibrium constant for the
reaction: ( N_{2(g)}+3 H_{2(g)} rightleftharpoons 2 N H_{3(g)} ) at
( mathbf{7} 15 K, ) is ( 6.0 times 10^{-2} . ) If, in a particular
reaction, there are 0.25 mol ( L^{-1} ) of ( H_{2} )
and ( 0.06 m o l L^{-1} ) of ( N H_{3} ) present
calculate the concentration of ( N_{2} ) at
equilibrium.
12
1617Illustration 2.53 Two liquids X and Y boil at 110°C and
130°C, respectively. Which one of them has higher vapour
pressure at 50°C?
12
1618Illustration 2.207 Acetic acid associates in benzene to
form a dimer. 1.65 g of acetic acid when dissolved in 100 g
of benzene raised the boiling point by 0.36°C. Calculate the
Van’t Hoff factor and degree of association of acetic acid.
(K, for benzene = 2.57°C m-1)
12
1619The depression in freezing point is maximum if the solvent used is:
A. Camphor
B. Naphthalene
c. Benzene
D. water
12
1620Can a solution be heterogeneous?12
1621The initial pressure inside the flask is:
A. near zero (vacuum)
В. 27 тт Н( g )
c. 760 mm ( H g )
D. ( (760-27) ) mm ( H g )
12
1622Which of the following will show a negative deviation from Raoult’s law?
A. Acetone-benzene
B. Acetone-ethanol
c. Benzene-methanol
D. Acetone-chloroform
12
1623Mass of glucose in ( g ) must be present in
0.5 litre of a solution for its osmotic
pressure be same as that of 8 g glucose in 1 litre is :
12
1624Example 2.1 Calculate the mole fraction of solute in a
dilute aqueous solution from which ice begins to separate
out at -0.46°C. (K, of H,0 = 1.86 Km-l)
12
1625Illustration 2.47 Calculate the vapour pressure lowering
of a 0.1 m aqueous solution of non-electrolyte at 75°C.
AH = 9.720 kcal mol-1, P, = 742.96 torr
12
1626At ( 20^{circ} C ) the vapour pressure of
( C H_{3} O H ) and ( C_{2} H_{5} O H ) is ( 94 mathrm{mm} ) and
( 44 mathrm{mm}, ) respectively.

If 20 g of ( C H_{3} O H ) is mixed with 100 g
of ( C_{2} H_{5} O H, ) determine the total
pressure of the solution (in ( mathrm{mm} ) )

12
1627A solution of sulphuric acid in water exhibits:
A. negative deviations from Raoult’s law
B. positive deviations from Raoult’s law
c. ideal properties
D. the applicability of Henry’s law
12
1628The boiling point of liquid ( A, B, C ) and ( D ) ( operatorname{are} 80^{circ} C, 60^{circ} C, 90^{circ} C ) and ( 100^{circ} C )
respectively. Which will show highest vapour pressure at room temperature?
( A cdot A )
B. B
( c cdot c )
( D . ) D
12
1629( M X_{2} ) dissociates in ( M^{2+} ) and ( X^{-} ) ions
in an aqueous solution with a degree of dissociation ( 0.5(alpha) . ) The ratio of the observed depression of the freezing point of the aqueous solution to the value of the depression of freezing point in the absence of ionic dissociation
is
12
1630Calculate mole fraction of solute if
molarity of solution is ( 20 %left(frac{W %}{W}right) ) aqueous solution of NaOH.
A. 0.2
B. 0.15
c. ( 0 . )
D. none of these
12
1631Which of the following are correct about
mixture of two miscible liquids forming
azeotopes?
This question has multiple correct options
A. Has the lowest temperature at which the two liquids can exist in the liquid state
B. Has the lowest temperature attainable at which two liquids forms eutectic mixture
C. Eutectic point has found application to attain low melting point solids which are eutectic mixture
D. Composition of azeotrope and their b.pt. vary with the external pressure
12
1632Why doesn’t sea water freeze so easily?12
1633Statement ( 1: A ) salt dissolved in an
organic solvent will be a good electrical conductor.
Statement 2: Salts will not dissolve
appreciably in an organic solvent.
A. Statement 1 and Statement 2 are correct and Statement 2 is the correct explanation of Statement 1
B. Both the Statement 1 and Statement 2 are correct, but Statement 2 is not the correct explanation of Statement 1.
c. statement 1 is correct, but statement 2 is not correct
D. Statement 1 is not correct, but Statement 2 is correct
12
1634If ( N_{2} ) gas bubbled through water at
( 293 K ) how many millimoles of ( N_{2} ) gas
would dissolve in 1 litre of water?

Assume that exerts a partial pressure
of ( 0.987 b a r )
Given that Henry’s law constant for ( N_{2} )
at ( 293 K ) is ( 76.48 K b a r )
A. 0.716
B. 0.62
c. 0.93
D. 0.54

12
1635illustration 2.133 The freezing point of 0.08 molal NaHSO4
is -0.345°C. Calculate the percentage of HSO, ions that
transfers a proton to water. Assume 100% ionization of
NaHSO, and K, for H,0 = 1.86 K molality:
12
1636. 19 Which of the following solutions have the same concentration?
(a) 20 g of NaOH in 200 mL of solution (b) 0.5 mol of KCl in 200 mL of solution
(C) 40 g of NaOH in 100 mL of solution (d) 20 g of KOH in 200 mL of solution
12
1637Which of the following shows positive deviation from Raoult’s law?
A. ( C_{6} H_{6} ) and ( C_{6} H_{5} C H_{3} )
B . ( C_{6} H_{6} ) and ( C C l_{4} )
c. ( C H C l_{3} ) and ( C_{2} H_{5} O H )
D. ( C H C_{3} ) and ( C H_{3} C O C H_{3} )
12
1638The vapour pressure is least for?
A. pure water
B. ( 0.1 mathrm{m} ) aqueous urea
c. ( 0.2 mathrm{m} ) aqueous urea
D. 0.3m aqueous urea
12
16391 Which of the following units is useful in relating concentration of solution
with its vapour pressure?
(a) Mole fraction
(b) Parts per million
(c) Mass percentage
(d) Molality
An
ution in oronortional to the
12
1640On mixing, heptane and octane form an ideal solution. At ( 373 mathrm{K} ), the vapour pressure of the two liquid components (heptane and octane) are ( 105 mathrm{kPa} ) and
45 kPa respectively. Vapour pressure of the solution obtained by mixing 25 g of heptane and 35 g of octane will be :
(molar mass of heptane ( =100 ) g ( m o l^{-2} ) and of octane ( =114 ) g ( m o l^{-1} )
A ( .96 .2 k P a )
в. ( 144.5 k P a )
c. ( 72 k P a )
D. ( 36.1 k P a )
12
1641Which one has same Van’t Hoff factor ( ‘ i^{prime} )
as that of ( boldsymbol{H} boldsymbol{g}_{2} boldsymbol{C l}_{2} ) ?
A . ( N a C l )
в. ( N a_{2} S O_{4} )
c. ( A lleft(N O_{3}right)_{3} )
D. ( A l_{2}left(S O_{4}right)_{3} )
12
1642Excess of ( K l ) was added to
( 100 m l H_{2} O_{2} ) solution of unknown
strength along with sufficient ( boldsymbol{H}_{2} boldsymbol{S} boldsymbol{O}_{4} ) lodine liberated was titrated against
( 40 m l ) of ( 0.1 M ) hypo solution. The
concentration of ( boldsymbol{H}_{2} boldsymbol{O}_{2} ) solution is:
A ( .0 .04 mathrm{N} )
в. 0.04 М
c. ( 0.68 g m / L )
D. ( 0.02 mathrm{M} )
12
16430.2 molal acid ( H X ) is ( 20 % ) ionised in
solution. ( boldsymbol{K}_{boldsymbol{f}}=mathbf{1 . 8 6 K} ) molality ( ^{-1} ). The
freezing point of the solution is:
A. ( -0.45^{circ} mathrm{C} )
B . ( -0.90^{circ} mathrm{C} )
c. ( -0.31^{circ} mathrm{C} )
D. ( -0.53^{circ} mathrm{C} )
12
1644For which among the following equimolar aqueous solutions Van’t Hoff factor has the lowest value?
A. Aluminium Chloride
B. Potassium Sulphate
c. Ammonium chloride
D. urea
12
1645Illustration 2.142 Define osmotic pressure.12
1646A solution ( X ) is prepared by dissolving three moles of glucose in one litre of water and a solution Y is prepared by dissolving 1.5 moles of sodium chloride in one litre of water. Will the osmotic
pressure of ( mathrm{X} ) be higher, lower or equal to that of Y? Give a reason for your
12
16470.1 normal solution of ( N a C l ) is found to
be isotonic with ( 1.1 % ) solution of Urea.
Calculate the apparent degree of
ionisation of ( N a C l )
( mathbf{A} cdot 0.083 )
B. 8.3
c. 0.83
D. 0.42
12
1648Illustration 2.166 A solution is prepared by dissolving 1.08 g
of human serum albumin, a protein obtained from blood
plasma, in 50 cm of aqueous solution. The solution has an
osmotic pressure of 5.85 mm Hg at 298 K.
a. What is the molar mass of albumin?
b. What is the height of water column placed in
solution?
d99,0) = 1 g cm-3
12
1649Loss of a beta particle is equivalent to:
A. increase of one neutron only
B. decrease of one neutron only
( c . ) both 1 and 2
D. none of these
12
1650The freezing point of aqueous solution that contains ( 3 % ) urea, ( 7.45 % K C l ) and
( 9 % ) of glucose is: ( left(operatorname{given} K_{1} text { of water }=right. )
1.86 and assume molarity ( = ) molality
).
A . ( 290 K )
в. 285.5 К
c. ( 267.42 K )
D. 250 K
12
1651Prachi makes a saturated solution of
potassium chloride in water at ( 353 mathrm{K} ) and leaves the solution to cool at room
temperature. What would she observe as the solution cools? Explain.
12
1652The freezing point of a solution containing 0.2 g of acetic acid in 20.0 g benzene is lowered by ( 0.45^{circ} mathrm{C} ). The degree of association of acetic acid in benzene is:
[Assume acetic acid dimerizes in
benzene and ( K_{f} ) for benzene ( =mathbf{5 . 1 2} mathbf{K} )
( left.mathrm{kg} mathrm{mol}^{-1}right] )
A. ( 94.5 % )
B . ( 54.9 % )
c. ( 78.2 % )
D. 100%
12
1653The osmotic pressure of a solution of benzoic acid dissolved in benzene is
less than expected because
A. benzoic acid is an organic solute
B. benzene is a non-polar solvent
c. benzoic acid dissociates in benzene
D. benzoic acid gets associated in benzene
12
1654Illustration 2.199 Following are equimolal aqueous
solutions:
a. 1 m urea
b. 1 m KCI
c. 1 m MgCl2
d. 1 m Na,PO4
Arrange them in increasing
i. Boiling point
Ïi. Freezing point
ü. Osmotic pressure iv. Vapour pressure
12
1655Which of the following units could be used to describe solubility?
( A cdot g / s )
в. ( g / l )
( c cdot k g / s )
D. mol/s
12
1656i). State Raoult’s Law.
ii). The vapour pressure of pure benzene at a certain temperature is 0.850 bar. ( A ) non-volatile non-electrolyte solid weighing 0.5 g when added to 39.0 gof benzene (molar mass 78 g ( m o l^{-1} ) ). Vapour pressure of the solution, then is
0.845 bar. What is the molar mass of
the solid substance?
12
1657By adding a non-volatile salute into a solution vapour pressure is reduces.12
1658The vapour pressures of two liquids ( A )
and B in their pure states are in the ratio of ( 1: 2 . ) A binary solution of ( A ) and ( B )
contains ( A ) and ( B ) in the mole proportion of ( 1: 2 . ) The mole fraction of ( A ) in the
vapour phase of the solution will be:
A . 0.33
B. 0.2
c. 0.25
D. 0.52
12
1659For the standardization of ( B a(O H)_{2} ) solution, 0.204 g of potassium acid phthalate was weighed which was then
titrated with ( B a(O H)_{2} ) solution. The titration indicated equivalence at 25.0
( mathrm{ml} ) of ( B a(O H)_{2} ) solution. The reaction involved is:
( boldsymbol{K} boldsymbol{H} boldsymbol{C}_{8} boldsymbol{H}_{4} boldsymbol{O}_{4}+boldsymbol{B} boldsymbol{a}(boldsymbol{O} boldsymbol{H})_{2} rightarrow boldsymbol{H}_{2} boldsymbol{O}+ )
( boldsymbol{K}^{+}+boldsymbol{B} boldsymbol{a}^{2+}+boldsymbol{C}_{8} boldsymbol{H}_{4} boldsymbol{O}_{4}^{2-} )
The molarity of the base solution is ( (K= )
39)
A. ( 0.04 mathrm{M} )
в. о.озм
c. о.о२м
D. 0.01M
12
1660At ( 20^{circ} mathrm{C} ) and a pressure of 1 atm each gas, 1 litre of water dissolves 0.043 g of pure ( O_{2} ) or 0.019 g of pure ( N_{2} . ) Assuming that dry air is composed of ( 20 % mathrm{O}_{2} ) and
( 80 % N_{2} ) (by volume) determine the
masses of ( boldsymbol{O}_{2} ) and ( boldsymbol{N}_{2} ) dissolved by 1 litre
of water at ( 20^{circ} mathrm{C} ) exposed to air at a
total pressure of 1 atm. Assume ( V . P . ) of
( H_{2} ) at ( 20^{circ} C ) be ‘b’ atm
A ( cdot O_{2}=4.3 times 10^{-3} g / L, N H 2=0.75 times 10^{-2} g / L )
B. ( O_{2}=5.25 times 10^{-4} g / L, N H 2=1.7 times 10^{-3} g / L )
C ( cdot O_{2}=8.6 times 10^{-3} g / L, N H 2=1.5 times 10^{-2} g / L )
D. ( O_{2}=10.5 times 10^{-4} g / L, N H 2=3.4 times 10^{-3} g / L )
12
1661Mass ( % ) of carbon in ethanol is:
A . 52
B. 13
c. 34
D. 90
E . 80
12
1662A complex is represented as ( mathrm{CoCl}_{3} cdot x N H_{3} ) its 0.1 molal solution in
aq. solution shows ( Delta T_{f}=0.558^{0} C . K_{f} )
for ( boldsymbol{H}_{2} boldsymbol{O} ) is ( 1.86 boldsymbol{K} boldsymbol{m o l}^{-1} boldsymbol{k g} . ) Assuming
( 100 % ) ionisation of complex and
coordination no. of ( C o ) is six, calculate
formula of complex.
12
1663Give an example of a solid solution in which the solute is a gas.12
1664Which solutions have a concentratoin of
( 1.0 mathrm{M} ? )
i. 74 grams of calcium hydroxide dissolved to make 1 liter of
Solution
ii. 74.5 grams of potassium chloride dissolved to maek 1 liter of
Solution
iii. 87 grams of lithium bromide
dissolved to make 1 liter of solution
A. i only
B. iii only
c. i and iii only
D. ii and iii only
E. i, ii and iii
12
1665The phenol-water system has a upper critical solution temperature.
A. True
B. False
12
1666wustration 2.79 Equal amounts of a solute are dissol
in equal amounts of two solvents A and B. The lowering of
vapour pressure for solution A has twice the lowering of
vapour pressure for solution B. If MwA and Mws are the
molecular weights of solvents A and B, respectively, then
a. Mwa = MWB
b. Mwa = Mwg/2
c. Mw = 4Mw
d. Mw = 2MWB
And D
12
1667( boldsymbol{C u} boldsymbol{S O}_{4} cdot boldsymbol{5} boldsymbol{H}_{2} boldsymbol{O}(s) rightleftharpoons boldsymbol{C u S O}_{4} cdot boldsymbol{3} boldsymbol{H}_{2} boldsymbol{O}(boldsymbol{s}) )
( +2 H_{2} O(g) ; K_{p}=4 times 10^{-4} a t m^{2} ) if the
vapour pressure of water is 38 torr then percentage of relative humidity is:
Assume all data at constant
temperature)
( mathbf{A} cdot mathbf{4} )
B. 10
c. 40
D. none of these
12
1668A mixture of chlorobenzene and wate
(immiscible) boils at ( 90.3^{circ} mathrm{C} ) at an
external pressure of ( 740.2 mathrm{mm} . ) The vapour pressure of pure water at
( 90.3^{circ} mathrm{C} ) is ( 530.1 mathrm{mm} ). Calculate the ( % )
composition of distillate:
A. ( H_{2} O=35 % )
в. ( H_{2} O= ) 22%
c. ( H_{2} O= ) २९% ( %= )
D. ( H_{2} O=71 % )
12
1669Calculate the molarity of each of the following: (a) ( 30 g ) of ( C oleft(N O_{3}right)_{2} .6 H_{2} O )
in ( 4.3 L ) of solution
(b) ( 30 m L ) of 0.5
( M H_{2} S O_{4} ) diluted to ( 500 m L )
12
1670Total vapour pressure of mixture of
mol of ( Aleft(P_{A}^{0}=150 text { tor } rright) ) and 2 mol of ( B )
( left(P_{B}^{0}=240 text { tor } rright) ) is 200 torr. In this case
A. there is positive deviation from Raoult’s law
B. there is negative deviation from Raoult’s law
c. there is no deviation from Raoult’s law
D. molecular masses of A and B are also required for calculating the deviation
12
1671Which of the following would show the LARGEST increase in solubility with increasing pressure based on intermolecular force knowledge?
( A ). Ammonia
B. Calcium oxide
c. Potassium bromide
D. Sodium hydroxide
12
1672Which characteristics the weak inter
molecular forces of attraction in a
liquid?
A. High boiling point
B. High vapour pressure
c. High critical temperature
D. High heat of vapourisation
12
1673A storage battery contains a solution of
( H_{2} S O_{4} 38 % ) by weight. What will be the
Van’t Hoff factor if the
( boldsymbol{Delta} boldsymbol{T}_{f text {experiment}} ) is ( mathbf{2 9 . 0 8} .left[text { Given } boldsymbol{K}_{f}=mathbf{1}right. )
B . ( i=2.5 )
c. ( i=3 )
D. ( i=3.5 )
12
1674(a) Explain the following
(i) Henry’s law about a dissolution of a gas in a liquid.
(ii) Boiling paint elevation constant for a solvent.
(b) A solution of glycerol ( left(C_{3} H_{8} O_{3}right) ) in
water was prepared by dissolving some glycerol in 500 g of water. This solution
has a boiling point of ( 100.42^{circ} mathrm{C} ). What
mass of glycerol was dissolved to make
this solution? ( left(K_{b} text { for water }=0.512 mathrm{K} mathrm{kg}right. )
( left.operatorname{mol}^{-1}right) )
12
1675The mole fraction of water in ( 20 % ) (wt. ( / )
wt.) aqueous solution of ( boldsymbol{H}_{2} boldsymbol{O}_{2} ) is:
A ( cdot frac{77}{68} )
в. ( frac{68}{77} )
c. ( frac{20}{80} )
D. ( frac{80}{20} )
12
1676Example 2.14 A solution containing 0.1 mol of naphthalene
and 0.9 mol of benzene is cooled out until some benzene
freezes out. The solution is then decanted off from the solid
and warmed upto 353 K where its vapour pressure was found
to be 670 mm. The freezing point and boiling point of benzene
are 278.5 K and 353 K respectively, and its enthalpy of fusion
is 10.67 kJ mol-1. Calculate the temperature to which the
solution was cooled originally and the amount of benzene
that must have frozen out. Assume ideal behaviour.
12
1677How much water must be added to 0.50
litre of ( 6.0 mathrm{M} ) H ( C l ) to make the solution
A . 0.33
B. 0.50
c. ( 1 . )
D. 1.5
E . 2.0
12
1678Define cryoscopic constant.12
1679For a solution of a non-electrolyte in water, the Van’t Hoff factor is :
A. Always equal to 0
в. ( leq 1 )
c. Always equal to
D. ( >1 ) but ( <2 )
12
1680The osmotic pressure of ( 400 mathrm{ml} ) urea and ( 600 mathrm{ml} ) glucose solutions are respectively 0.3 atm and 0.4 atm. The osmotic pressure of the solution obtained by mixing them will be?
A. 0.24 atm
B. 0.36 atm
c. 0.48 atm
D. 0.52 atm
12
16813 moles of ( boldsymbol{P} ) and 2 moles of ( boldsymbol{Q} ) are
mixed, what will be their total vapour pressure in the solution if their partial
vapour pressures are 80 and 60 respectively.
A. 80 torr
B. 140 torr
( c .720 ) torr
D. 70 torr
12
1682Arrange the following compounds in increasing order of solubility in water:
( boldsymbol{C}_{6} boldsymbol{H}_{5} boldsymbol{N} boldsymbol{H}_{2},left(boldsymbol{C}_{2} boldsymbol{H}_{5}right)_{2} boldsymbol{N} boldsymbol{H}, boldsymbol{C}_{2} boldsymbol{H}_{5} boldsymbol{N} boldsymbol{H}_{2} )
12
1683We define p value of a term (say ( x ) ) as
( boldsymbol{p}_{boldsymbol{x}}=-log boldsymbol{x} )
Calculate ( boldsymbol{p}_{left(C l^{-}right)} ) value as ( boldsymbol{x} times mathbf{1 0}^{-1} ) in a
solution that is ( 2.00 times 10^{-3} mathrm{Min} ) NaCl
and ( 5.4 times 10^{-4} ) M ( H C l )
12
1684Deep sea divers use ( left(O_{2}+H eright) ) mixture
as preference to ( left(O_{2}+N_{2}right) ) mixture.
This is because:
A. helium is lighter than nitrogen
B. helium is less soluble in blood than nitrogen
c. helium is more soluble in blood.
D. helium provides a better inert atmosphere than nitrogen.
12
1685( 1000 mathrm{g} ) aqueous solution of ( mathrm{CaCO}_{3} ) contain ( 10 g ) of calcium carbonate
concentration of the solution is?
A. 10 ppm
B. 100 ppm
c. 1000 ppm
D. 10,000 ppm
12
1686Assertion
The sum of mole fractions of all the
components of a solution is unity.
Reason
Mole fraction is a temperature
dependent mode of concentration.
Choose the correct option.
A. Both Assertion and Reason are correct and Reason is the correct explanation for Assertion
B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion
C. Assertion is correct but Reason is incorrect
D. Assertion is incorrect but Reason is correct
12
1687The vapour density of undecomposed
( N_{2} O_{4} ) is ( 46 . ) When heated, vapour density decreases to 24.5 due to its
dissociation to ( N O_{2} . ) The percentage
dissociation of ( N_{2} O_{4} ) at the final
temperature is:
( mathbf{A} cdot 88 )
B. 60
c. 40
D. 70
12
1688Which will have the lowest freezing
point?
A. A 0.01-molar solution of HNO
B. A 0.01-molar solution of ( mathrm{HC}_{2} mathrm{H}_{3} mathrm{O}_{2} )
C. A 0.01-molar solution of Cu(NO ( _{3} ) )
D. A 0.01-molar solution of NaNO
12
1689The volume of ethyl alcohol (density ( 1.15 g / c c) ) that has to be added to
prepare ( 100 mathrm{cc} ) of ( 0.5 mathrm{M} ) ethyl alcohol
solution in water is :
A . ( 1.15 c c )
B. ( 2 c c )
c. ( 2.15 c c )
D. 2.30 ( c c )
12
1690Dry ( N_{2} ) was passed successively
through a solution of solute ( A_{2} B ) in
water at ( 27^{circ} C ) and then through pure
water. The loss in mass of solution was
( 2.5 mathrm{g} ) and that of pure water was ( 0.04 mathrm{g} ) Find the degree of dissociation of salt
( A_{2} B ) when solution of ( A_{2} B ) has same concentration as ( 1.86 % ) (mass/vol)
solution of urea at ( 27^{circ} C . ) Assume
molarity is equal to molality. Divide answer by 10 and write the nearest integer.
12
1691( H_{2} S ) a toxic gas with rotten egg like smell, is used for the qualitative
analysis. If the solubility of ( H_{2} S ) in water at ( S T P ) is 0.195 m, calculate
Henry’s law constant.
12
1692Assertion
( 1 M ) solution of ( K C l ) has greater
osmotic pressure than ( 1 M ) solution of
glucose at the same temperature.
Reason
In solution ( K C l ) dissociates to produce more number of particles.
A. Both Assertion and Reason are correct and Reason is the correct explanation for Assertion
B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion
c. Assertion is correct but Reason is incorrect
D. Both Assertion and Reason are incorrect
12
1693Select the one which describe the best
among all the given options. To determine whether a water solution of
( N a_{2} S_{2} O_{3} ) at room temperature is
supersaturated, one can:
A. heat the solution to its boiling point
B. add water to the solution
c. add a crystal of ( N a_{2} S_{2} O_{3} ) to the solution
D. acidify the solution
E. cool the solution to its freezing point
12
1694Which of the following is an example of
gaseous solution?
A. Camphor in nitrogen gas
B. Solution of hydrogen in palladium
c. chloroform mixed with nitrogen gas
D. Both (A) and (C)
12

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