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Chemistry
Liquid Solutions
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1
An ideal solution was obtained by mixing methanol and ethanol. If the partial vapour pressure of methanol and ethanol are 2.619 kPa and 4.556 kPa respectively, the composition of vapour (in terms of mole fraction) will be -
A
0.635 MeOH, 0.365 EtOH
B
0.365 MeOH, 0.635 EtOH
C
0.574 MeOH, 0.326 EtOH
D
0.173 MeOH, 0.827 EtOH
2
The vapour pressure of pure liquid A is 10 torr and at the same temperature when 1 g of B solid is dissolved in 20 g of A, its vapour pressure is reduced to 9.0 torr. If the molecular mass of A is 200 amu, then the molecular mass of B is-
A
100 amu
B
90 amu
C
75 amu
D
120 amu
3
All of the water in a 0.20 M solution of NaCl was evaporated and 0.150 mol of NaCl was obtained. What was the original volume of the sample?
A
30 mL
B
333 mL
C
750 mL
D
1000 mL
4
Which one of the following salts would have the same value of the Vant Hoff factor (i) as that of K₃[Fe(CN)₆]-
A
NaCl
B
Na₂SO₄
C
Al₂(SO₄)₃
D
Al(NO₃)₃
5
At certain Hill-station pure water boils at 99.725°C. If Kb for water is 0.513°C kg mol⁻¹. The boiling point of 0.69 m solution of urea will be-
A
100.079°C
B
103°C
C
100.359°C
D
Unpredictable
6
If P0 and Ps are the vapour pressure of solvent and solution respectively and N1 and N2 are the mole of solute and solvent then:
A
(P0 – Ps)/P0 = N1/(N1 + N2)
B
(P0 – Ps)/Ps = N1/N2
C
Ps = P0 ⋅ N2/(N1 + N2)
D
All of the above
7
A complex of iron and cyanide ions is 100% ionised at 1 m (molal). If its elevation in b.p. is 2.08° (Kb = 0.52) then complex is-
A
K₃[Fe(CN)₆]
B
Fe(CN)₂
C
K₄[Fe(CN)₆]
D
Fe(CN)₄
8
The phase diagrams for a pure solvent (solid line) and a corresponding solution (containing a nonvolatile solute and represented by the dashed lines) are shown below. 
Choose the correct option.
A
A = ΔTb m and B = ΔTf m
B
A = ΔTf m and B = ΔTb m
C
A = ΔTf and B = ΔTb
D
A = ΔTb and B = ΔTf
9
Assertion : Reverse osmosis is used to purify sea water.
Reason : Solvent molecules pass from concentrate solution to pure solvent through semipermeable membrane if high pressure (> π) is applied on solution side
A
If both Assertion & Reason are True & the Reason is a correct explanation of the Assertion.
B
If both Assertion & Reason are True but Reason is not a correct explanation of the Assertion.
C
If Assertion is True but the Reason is False.
D
If both Assertion & Reason are false.
10
The osmotic pressure of urea solution is 3 atm and that of sugar solution is 8 atm. Osmotic pressure of solution formed by mixing above solutions in volume ratio 1 : 4 at same temperature will be-
A
2 atm
B
5 atm
C
7 atm
D
None
11
What is the freezing point of a solution containing 8.1 g HBr in 100 g water assuming the acid to be 90% ionised? (kf for wt. = 1.86 K mol–1)
A
0.85°C
B
– 3.53°C
C
+ 3.53°C
D
– 0.35°C
12
The molal elevation constant is the ratio of the elevation in BP to-
A
Molarity
B
Molality
C
Mole fraction of solute
D
Mole fraction of solvent
13
Mole fraction of solute in benzene is 0.2 then find molality of solute
A
3.2
B
2
C
4
D
3.6
14
A solution of urea (mol. mass 56) boils at 100.18°C at atmospheric pressure. If Kf and Kb for water are 1.86 and 0.512 K molality–1 respectively, the above solution will freeze at:
A
– 6.54°C
B
6.54°C
C
– 0.654°C
D
0.654°C
15
If pKa = −log Ka = 4, and Ka = Cα² then van't Hoff factor for weak monobasic acid when C = 0.01 M is -
A
0.01
B
1.02
C
1.10
D
1.20
16
5.85 g of NaCl are dissolved in 90 g of water. The mole fraction of NaCl is-
A
0.1
B
0.01
C
0.2
D
0.0196
17
The elevation of boiling point method is used for the determination of molecular weight of-
A
Non-volatile and soluble solute
B
Non-volatile and insoluble solute
C
Volatile and soluble solute
D
Volatile and insoluble solute
18
Assuming each salt to be completely dissociated which of the following will have highest osmotic pressure-
A
Decimolar Al₂(SO₄)₃
B
Decimolar BaCl₂
C
Decimolar Na₂SO₄
D
Decimolar NaCl
19
25 mL of an aqueous solution of KCl was found to require 20 mL of 1 M AgNO₃ solution when titrated using K₂CrO₄ as indicator. Depression in freezing point of KCl solution with 100% ionisation will be- (Kf = 2.0 K kg mol⁻¹ and molarity = molality)
A
5.0
B
3.2
C
1.6
D
0.8
20
A solution of benzoic acid dissolved in benzene will show a molecular mass closer to -
A
122
B
244
C
61
D
366
21
A 0.01 M solution of glucose in water freezes at −0.0186°C. A 0.01 M solution of KCl in water freezes at temperature-
A
higher than −0.0186°C
B
0°C
C
0.0186°C
D
lower than −0.0186°C
22
10 mL of concentrated H₂SO₄ (18 M) is diluted to one litre. The approximate strength of the dilute acid is-
A
18 M
B
180 M
C
0.18 M
D
1.8 M
23
The freezing point of 1 molal NaCl solution assuming NaCl to be 100% dissociated in water is-
A
−1.86°C
B
−3.72°C
C
+1.86°C
D
+3.72°C
24
Dissolution of a solute is an exothermic process if:
A
Hydration energy > lattice energy
B
Hydration energy < lattice energy
C
Hydration energy = lattice energy
D
None of the above
25
If 100 mL of 1.0 M NaOH solution is diluted to 1.0 L, the resulting solution contains-
A
1 mole of NaOH
B
0.1 mole of NaOH
C
10.0 mole of NaOH
D
0.05 mole of NaOH
26
Calculate the amount of CO₂ in moles that will dissolve in enough water to form 900 mL of solution at 20°C if partial pressure of CO₂ is 1 atm and kH for CO₂ is 2.3 × 10⁻² mol L⁻¹ atm⁻¹.
A
0.02
B
0.04
C
0.09
D
1.0
27
The correct relationship between the boiling points of very dilute solutions of AlCl₃ (t₁) and CaCl₂ (t₂), having the same molar concentration is-
A
t₁ = t₂
B
t₁ > t₂
C
t₂ > t₁
D
t₂ ≥ t₁
28
The vapour pressures of pure A and B at given temperature are 108 and 36 bar respectively. What is the mole fraction of B in the vapour phase of the solution containing equimolar mixture of A and B-
A
0.25
B
0.5
C
0.75
D
0.66
29
A solution containing 1.8 g of a compound (empirical formula CH2O) in 40 g of water is observed to freeze at –0.465°C. The molecular formula of the compound is (Kf of water – =1.86 kg K mol–1)
A
C2H4O2
B
C3H6O3
C
C4H8O4
D
C6H12O6
30
The molarity of a glucose solution containing 36 g of glucose per 400 mL of the solution is-
A
1.0
B
0.5
C
2.0
D
0.05
31
The relative lowering in vapour pressure is-
A
∝ Xsolute
B
∝ 1/Xsolute
C
= Xsolute
D
∝ m
32
An aqueous solution of urea containing 18 g urea in 1500 cm³ of solution has a density of 1.052 g cm⁻³. If the molecular weight of urea is 60, then molality of solution is-
A
0.2
B
0.192
C
0.064
D
1.2
33
A solution containing 12.5g of non-electrolyte substance in 175g of water gave boiling point elevation of 0.70K. Calculate the molar mass of the substance. Molal elevation constant (Kb) for water 0.52K kg mol−1
A
53
B
65
C
84
D
79
34
Van’t hoff factor of Ca(NO3)2 is:
A
One
B
Two
C
Three
D
Four
35
Equal volume of 1 M urea and 1 M glucose are mixed. The mixture will have-
A
Same osmotic pressure
B
Lower osmotic pressure
C
Higher osmotic pressure
D
None of these
36
2.56 g of sulphur in 100 g of CS₂ has depression in f.p. of 0.010°, Kf = 0.1° (molal)⁻¹. Hence, atomicity of sulphur is -
A
2
B
4
C
6
D
8
37
The values of observed and theoretical molecular masses of certain electrolyte XY are 65.4 and 114.45 respectively. The electrolyte XY in the solution has dissociation to the extent of-
A
75%
B
80%
C
50%
D
90%
38
Two solutions have different osmotic pressures. The solution of higher osmotic pressure is called-
A
Isotonic solution
B
Hypotonic solution
C
Isotopic solution
D
Hypertonic solution
39
Which of the following is correct for a solution showing positive deviations from Raoult's law?
A
ΔV = +ve, ΔH = +ve
B
ΔV = −ve, ΔH = −ve
C
ΔV = +ve, ΔH = −ve
D
ΔV = −ve, ΔH = +ve
40
Given at 350 K , p°A = 300 torr and p°B = 800 torr, the composition of the mixture having a boiling point of 350 K is -
A
XA = 0.08
B
XA = 0.06
C
XA = 0.04
D
XA = 0.02
41
The vapour pressure of benzene at a certain temperature is 640 mm of Hg. A non-volatile and nonelectrolyte solid weighing 2.175 g is added to 39.08 g of benzene. If the xapour pressure of the solution is 600 mm of Hg, what is the molecular weight of solid substance?
A
49.50
B
59.60
C
69.60
D
79.82
42
Solutions A, B, C and D are respectively 0.1M glucose, 0.05 M NaCl, 0.05 M BaCl2 and 0.1 M AlCl3. Which one of the following pairs is isotonic?
A
A and B
B
B and C
C
A and D
D
A and C
43
How many grams of glucose should be dissolved to make one litre solution of 10% (w/v) glucose-
A
10 g
B
180 g
C
100 g
D
1.8 g
44
In which of the following, the Vant Hoff factor (i) is equal to one-
A
NaCl
B
KNO₃
C
Urea
D
All
45
A property which depends primarily on the number of molecules of a system and not on their nature is known to be-
A
Constitutive
B
Additive
C
Colligative
D
None of the above
46
The mole fraction of NaCl in a solution containing 1 mole of NaCl in 1000 g of water is-
A
0.0177
B
0.001
C
0.5
D
0.244
47
Vapour pressure of a solvent containing nonvolatile solute is -
A
More than the vapour pressure of a solvent
B
Less than the vapour pressure of solvent
C
Equal to the vapour pressure of solvent
D
None of these
48
Which of the following is a colligative property-
A
Change in free energy
B
Dipole moment
C
Heat of vaporisation
D
Osmotic pressure
49
Two solutions A and B are separated by a semipermeable membrane. As a result of osmosis, the level of solution A is found to rise. It implies that-
A
Solution A is more concentrated than solution B
B
Solution B is more concentrated than solution A
C
The solute molecules of A are smaller than those of B
D
The solute molecules of B are smaller than those of A
50
The Vant Hoff factor (i) for a dilute aqueous solution of glucose is-
A
zero
B
1.0
C
1.5
D
2.0
51
If the observed and theoretical molecular mass of NaCl is found to be 31.80 and 58.50, then the degree of dissociation of NaCl is-
A
83.96%
B
8.39%
C
90%
D
100%
52
Which of the following shows maximum depression in freezing point?
A
K2SO4
B
NaCl
C
Urea
D
glucose
53
When 36 g of a solute having empirical formula CH₂O is dissolved in 1.20 kg of water the solution freezes at −0.93°C. Molecular formula will be- (Kf(H₂O)=1.86°C kg mol⁻¹)
A
C₂H₄O
B
C₂H₂O₂
C
C₂H₄O₃
D
C₂H₄O₂
54
0.01 molal solution of Pt(NH₃)₄Cl₄ in water had a freezing point depression of 0.054°C. If Kf of water is 1.8, the correct formula for above molecule is-
A
[Pt(NH₃)₄Cl₃]Cl
B
[Pt(NH₃)₄Cl₂]Cl₂
C
[Pt(NH₃)₄Cl₂]Cl
D
[Pt(NH₃)₄Cl₄]
55
Which of the following mixture does not show positive deviation from the Raoult's law?
A
Benzene + acetone
B
Acetone + ethanol
C
Acetone + chloroform
D
Water + ethanol
56
In certain solvent, phenol dimerizes to the extent of 60%. Its observed molecular mass in that solvent should be-
A
> 94
B
= 94
C
< 94
D
Unpredictable
57
Which is not a colligative property in the following?
A
pH ofa buffer solution
B
Boiling point elevation
C
Freezing point depression
D
Relative vapour pressure lowering
58
The substance A when dissolved in solvent B shows the molecular mass corresponding to A₃. The van't Hoff factor will be (assuming 100% association)-
A
1
B
2
C
3
D
1/3
59
Binary liquid mixtures which exhibit positive deviations from Raoult's law boil at ..... temperature than the expected b.pt -
A
Lower
B
Higher
C
Same
D
Can’t be said
60
A complex containing K+, Pt(IV) and Cl− is 100% ionised giving i = 3. Thus, complex is -
A
K2[PtCl4]
B
K2[PtCl6]
C
K3[PtCl5]
D
K[PtCl3]
61
When two liquids A and B are mixed then their boiling points becomes greater than both of them. What is the nature of this solution?
A
Ideal solution
B
Normal solution
C
Negative deviation with non-ideal solution
D
Positive deviation with non-ideal solution
62
For dilute solution Raoult's law states that-
A
The lowering of vapour pressure is equal to the mole fraction of the solute
B
The relative lowering of vapour pressure is equal to the mole fraction of the solute
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 the solvent
63
Pure water will boil at 101.5°C at which of the following pressure -
A
76 cm of Hg
B
76 mm of Hg
C
> 76 cm of Hg
D
< 76 cm of Hg
64
Two liquids A and B form an ideal solution. At 300 K the vapour pressure of a solution of 1 mole of A and x moles of B is 550 mm. If the vapour pressures of pure A and B are 400 mm and 600 mm respectively, then x is -
A
1
B
2
C
3
D
4
65
1000 g aqueous solution of CaCO₃ contains 10 g of calcium carbonate. Concentration of solution is-
A
10 ppm
B
100 ppm
C
1000 ppm
D
10000 ppm
66
The vapour pressure of benzene at 80°C is lowered by 10 mm by dissolving 2g of a non-volatile substance in 78 g of benzene. The vapour pressure of pure benzene at 80°C is 750 mm. The molecular weight of the substance will be:
A
15
B
150
C
1500
D
148
67
The relationship between osmotic pressure at 273 K when 10 g glucose (p1), 10 g urea (p2) and 10 g sucrose (p3) are dissolved in 250 mL of water is:
A
p1 > p2 > p3
B
p3 > p2 > p1
C
p2 > p1 > p3
D
p2 > p3 > p1
68
In case of electrolyte which dissociates in solution the Vant Hoff's Factor-
A
> unity
B
< unity
C
= Unity
D
can be > or < 1
69
At high altitude the boiling of water occurs at low temp. because:
A
Atmospheric pressure is low
B
Temperature is low
C
Atmospheric pressure is high
D
None of the above
70
Which statement is correct for the boiling point of solvent containing a dissolved solid substance-
A
Boiling point of the liquid is depressed
B
Boiling point of the liquid is elevated
C
There is no effect on the boiling point
D
The change depends upon the polarity of the liquid
71
An ideal solution is that which-
A
Shows positive deviation from Raoult's law
B
Shows negative deviation from Raoult's law
C
Has no connection with Raoult's law
D
Obeys Raoult's law
72
In the case of osmosis, solvent molecules move from-
A
Higher vapour pressure to lower vapour pressure
B
Higher concentration to lower concentration
C
Lower vapour pressure to higher vapour pressure
D
Higher osmotic pressure to lower osmotic pressure
73
The osmotic pressure of 0.2molar solution of urea at 27°C (R = 0.082 L atm mol–1 K–1) is
A
4.92 atm
B
1 atm
C
0.2 atm
D
27 atm
74
Y g of non-volatile organic substance of molecular mass M is dissolved in 250 g benzene. Molal elevation constant of benzene of Kb. Elevation in its boiling point is given by:
A
KbY/M
B
4KbY/M
C
KbY/4M
D
KYb/M
75
Ratio of (ΔTb/Kb) of 10 g of AB₂ and 14 g of A₂B in 100 g solvent in their respective solutions (AB₂ & A₂B both are non-electrolytes) is 1 mol kg⁻¹ in both cases. Hence atomic wt. of A and B respectively-
A
100, 40
B
60, 20
C
20, 60
D
None of these
76
The osmatic pressure of a 5% (wt./vol) solution of cane sugar at 150°C is:
A
3.078 atm
B
4.078 atm
C
5.078 atm
D
2.45 atm
77
Saturated solution of NaCl on heating becomes:
A
Super saturated
B
Unsaturated
C
Remains saturated
D
None of these
78
Which aqueous solution has minimum freezing point -
A
0.01 M NaCl
B
0.005 M C₂H₅OH
C
0.005 M MgI₂
D
0.005 M MgSO₄
79
The vapour pressures of ethanol and methanol are 42.0 mm and 88.5 mm Hg respectively. An ideal solution is formed at the same temperature by mixing 46.0 g of ethanol with 16.0 g of methanol. The mole fraction of methanol in the vapour is-
A
0.467
B
0.502
C
0.513
D
0.556
80
Which one of the following aqueous solutions will exhibit highest boiling point?
A
0.01 M Na2SO4
B
0.01 M KNO3
C
0.015 M urea
D
0.015 M glucose
81
The vapour pressure (VP) of a dilute solution of non-volatile solute is P and the VP of pure solvent is P0, the lowering of the VP is:
A
+ ye
B
– ye
C
P/P0
D
P0/P
82
A molal solution is one that contains one mole of a solute in-
A
1000 g of the solution
B
1000 cc of the solution
C
1000 cc of the solvent
D
1000 g of the solvent
83
The solubility order for the following gases is:
A
NH3 > CO2 > O2 > H2
B
H2 > O2 > NH3 > CO2
C
CO2 > NH3 > O2 > N2
D
O2 > H2 > NH3 > CO2
84
Which of the following is correct-
A
mole = molarity × V(in L) = wt./mol.wt.
B
millimole = molarity × V(in mL) = (wt./mol.wt.) × 1000
C
Moles and millimoles react according to stoichiometric ratio of balanced chemical equation
D
All
85
The osmotic pressure of 0.2 molar solution of urea at 300 K (R = 0.082 litre atm mol⁻¹ K⁻¹) is-
A
4.92 atm
B
1 atm
C
0.25 atm
D
27 atm
86
Which of the following statement is true?
A
The relative lowering of vapour pressure of a solution is equal to the mole fraction of the solute present in the solution.
B
Passage of solute molecules towards solution side through semipermeable membrane is osmosis.
C
The boiling point of solution is always lower than the solvent.
D
The boiling point of a liquid is the temperature at which its vapour pressure becomes equal to 260 mm.
87
100 mL of liquid A and 25 mL of liquid B is mixed to give a solution which does not obey Raoult's law. The volume of the solution-
A
will be 125 mL
B
can be > or < than 125 mL
C
can be greater than, equal to or less than 125 mL
D
will be less than 125 mL
88
Colligative properties of a solution depends upon
A
Nature of both solvent and solute
B
Nature of solute only
C
Number of solvent particles
D
The number of solute particles
89
The normality of 0.3 M phosphorous acid (H3PO3) is -
A
0.1
B
0.9
C
0.3
D
0.6
90
Van't Hoff factors of aqueous solutions of X, Y, Z are 1.8, 0.8 and 2.5. Hence their -
A
b.p. : Y < Z < X
B
f.p. : Z < X < Y
C
osmotic pressure : X = Y = Z
D
v.p. : Y < X < Z
91
The osmotic pressure of a solution of benzoic acid dissolved in benzene is less than expected because-
A
Benzoic acid is an organic solute
B
Benzene is a non-polar solvent
C
Benzoic acid dissociates in benzene
D
Benzoic acid gets associated in benzene
92
A solution of sulphuric acid in water exhibits -
A
Negative deviations from Raoult’s law
B
Positive deviations from Raoult’s law
C
Ideal properties
D
The applicability of Henry’s law
93
Molality of the solution is-
A
The number of moles of the solute dissolved per kilogram of solvent
B
The number of gram mole of the solute dissolved per mL of solution
C
The number of grams of the solute dissolved per kilogram of solvent
D
The number of moles of the solute dissolved per litre of the solution
94
Blood cells retain their normal shapes in solutions which are-
A
isotonic to blood
B
hypotonic to blood
C
hypertonic to blood
D
all of these
95
Boiling point of water is defined as the temperature at which –
A
Vapour pressure of water becomes equal to that of atmospheric pressure
B
Bubbles are formed
C
Steam comes out
D
None of the above
96
A solution X contains 30 mole % of A and is in equilibrium with its vapour that contains 40 mole % of B. The ratio of vapour pressures of pure A and B will be-
A
2 : 7
B
7 : 2
C
3 : 4
D
4 : 3
97
At a given temperature, total vapour pressure in Torr of a mixture of volatile components A and B is given by
P = 120 − 75 XB
Hence, vapour pressure of pure A and B respectively (in Torr) are -
A
120, 75
B
120, 195
C
120, 45
D
75, 45
98
For a solution containing non-volatile solute, the relative lowering of vapour pressure is 0.2. If the solution contains 5 moles in all, which of the following are true?
I. Mole fraction of solute = 0.2
II. Number of moles of solute = 0.2
III. Number of moles of solvent = 4
IV. Mole fraction of solvent = 0.2
A
I, IV
B
II, III
C
I, III
D
II, IV
99
The solution having same osmotic pressure at constant (given) temperature are called-
A
Equivalent solutions
B
Ideal solutions
C
Equimolar solutions
D
Isotonic solutions
100
Which of the following concentration term is/are independent of temperature?
A
Molarity
B
Molarity and mole fraction
C
Mole fraction and molality
D
Molality and normality
101
An azeotropic solution of two liquids has boiling point lower than either when it -
A
shows a negative deviation from Raoult's law
B
shows a positive deviation from Raoult's law
C
shows no deviation from Raoult's law
D
is saturated
102
When one mole of non-volatile solute is dissolved in three moles of solvent, the vapour pressure of the solution relative to the vapour pressure of the pure solvent is -
A
1/3
B
1/4
C
3/4
D
1
103
The hardness of water is usually expressed in-
A
ppm
B
g/litre
C
mol/litre
D
None
104
If mole fraction of the solvent in a solution decreases then-
A
Vapour pressure of solution increases
B
b.pt decreases
C
Osmotic pressure increases
D
All are correct
105
Which of the following conditions is not correct for ideal solution-
A
no change in volume on mixing
B
no change in enthalpy on mixing
C
it obey's Raoult's law
D
Ionisation of solute should occurs to a small extent
106
0.2 molal acid HX is 20% ionised in solution Kf = 1.86 K molality–1. The freezing point of the solution is
A
-0.45
B
-0.90
C
-0.30
D
-0.53
107
The amount of H₂SO₄ present in 400 mL of 0.1 M solution of the acid is -
A
2.45 g
B
3.92 g
C
9.80 g
D
4.9 g
108
Choose the correct statement. When concentration of a salt solution is increased
A
Boiling point increases while vapour pressure decreases.
B
Boiling point decreases while vapour pressure increases.
C
Freezing point decreases while vapour pressure increases.
D
Freezing point increases while vapour pressure decreases.
109
Which characterises 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
110
Decimolar solution of potassium ferricyanide, K3[Fe(CN)6], has osmotic pressure 3.94 atm at 27°C. Hence percent ionisation of the solute is -
A
10%
B
20%
C
30%
D
40%
111
The amount of ice that will separate out on cooling a solution containing 50 g ethylene glycol in 200 g water to −9.3°C is (Kf = 1.86 K kg mol⁻¹)-
A
38.71 g
B
38.71 mg
C
42 g
D
42 mg
112
The molar freezing point constant for water is 1.86°C/mole. If 342 g of cane sugar (C₁₂H₂₂O₁₁) is dissolved in 1000 g of water, the solution will freeze at-
A
−1.86°C
B
1.86°C
C
−3.92°C
D
2.42°C
113
The relative lowering of vapour pressure of an aqueous solution containing non-volatile solute is 0.0125. The molality of the solution is:
A
0.70
B
0.50
C
0.60
D
0.80
114
The relationship between osmotic pressure at 273 K when 10 g glucose (P₁), 10 g urea (P₂) and 10 g sucrose (P₃) are dissolved in 250 mL of water is -
A
P₁ > P₂ > P₃
B
P₃ > P₁ > P₂
C
P₂ > P₁ > P₃
D
P₂ > P₃ > P₁
115
Consider following solutions -
I : 1 M aq. glucose
II : 1 M aq. sodium chloride
III : 1 M benzoic acid in benzene
IV : 1 M ammonium phosphate
Select incorrect statement -
A
all are isotonic solutions
B
III is hypotonic of I, II, IV
C
I, II, IV are hypertonic of III
D
IV is hypertonic of I, II, III
116
In which case van't Hoff factor is maximum?
A
KCl, 50% ionised
B
K₂SO₄, 40% ionised
C
FeCl₃, 30% ionised
D
SnCl₄, 20% ionised
117
Molarity of a solution relates the-
A
Moles of solute and solvent
B
Moles of solute and mass of solution
C
Volume of solute and volume of solvent
D
Volume of solution and moles of solute
118
A solution contains one mole of alcohol and four moles of water. What are the mole fractions of water and alcohol-
A
1/4, 4/1
B
4/1, 1/4
C
4/5, 1/5
D
1/5, 4/5
119
When a substance is dissolved in a solvent, the vapour pressure of solvent decreases. This brings -
A
An increase in b.pt of the solution
B
A decrease in b.pt of a solution
C
An increase in f.pt of the solvent
D
none
120
The osmotic pressure of a dilute solution is given by-
A
P = P₀X
B
πV = nRT
C
ΔP = P₀N₂
D
ΔP/P₀ = (P₀ − P)/P₀
121
Which statement is incorrect about osmotic pressure (π), volume (V) and temperature (T)-
A
π ∝ 1/V if T is constant
B
π ∝ T if V is constant
C
π ∝ V if T is constant
D
πV is constant if T is constant
122
3.0 molal NaOH solution has a density of 1.110 g/mL. The molarity of the solution is-
A
2.9732
B
3.05
C
3.64
D
3.0504
123
All form ideal solutions except-
A
C₂H₅Br and C₂H₅I
B
C₆H₅Cl and C₆H₅Br
C
C₆H₆ and C₆H₅CH₃
D
C₂H₅I and C₂H₅OH
124
The osmotic pressure of equimolar solutions of urea, BaCl₂ and AlCl₃ will be in the order-
A
AlCl₃ > BaCl₂ > Urea
B
BaCl₂ > AlCl₃ > Urea
C
Urea > BaCl₂ > AlCl₃
D
BaCl₂ > Urea > AlCl₃
125
Aqueous solutions of 0.004 M Na2SO4 and 0.01 M Glucose are isotonic. The degree of dissociation of Na2SO4 is
A
25%
B
60%
C
75%
D
85%
126
Total vapour pressure of mixture of 1 mol volatile component A (p°A = 100 mmHg) and 3 mol volatile component B (p°B = 60 mmHg) is 75 mmHg. For such case -
A
there is positive deviation from Raoult's law
B
boiling point has been lowered
C
force of attraction between A and B is smaller than that between A and A or between B and B
D
All the above statements are correct
127
The freezing point of a 0.05 molal solution of a non-electrolyte in water is- (Kf = 1.86°C/mol)
A
−1.86°C
B
−0.93°C
C
−0.093°C
D
0.93°C
128
Vant Hoff factor (i)-
A
Is less than one in case of dissociation
B
Is more than one in case of association
C
i = normal molecular mass / observed molecular mass
D
i = observed molecular mass / normal molecular mass
129
The molality of 15% (wt./vol.) solution of H₂SO₄ of density 1.1 g/cm³ is approximately-
A
1.2
B
1.4
C
1.8
D
1.6
130
0.2 mole of HCl and 0.1 mole of CaCl₂ were dissolved in water to have 500 mL of solution, the molarity of Cl− ions is-
A
0.04 M
B
0.8 M
C
0.4 M
D
0.08 M
131
The number of moles present in 2 litre of 0.5 M NaOH is-
A
2
B
1
C
0.1
D
0.5
132
The molecular weight of NaCl determined by studying freezing point depression of its 0.5% aqueous solution is 30. The apparent degree of dissociation of NaCl is -
A
95%
B
85%
C
75%
D
None
133
According to Boyle-Vant Hoff law for solutions, the osmotic pressure of a dilute solution is-
A
Inversely proportional to its volume
B
Directly proportional to its volume
C
Equal to its volume
D
None of the above
134
Density of water is 1 g/mL. The concentration of water in mol/litre is-
A
1000
B
18
C
0.018
D
55.5
135
The degree of dissociation (α) of a weak electrolyte, AxBy is related to van’t Hoff factor (i) by the expression
A
(i–1)/(x+y–1)
B
(i–1)/(x+y+1)
C
(x+y–1)/(i–1)
D
(x+y+1)/(i–1)
136
During osmosis, flow of water through a semipermeable membrane is:
A
From both sides of semipermeable membrane with unequal flow rates
B
From solution having lower concentration of solvent only
C
From solution having higher concentration of solvent only
D
From both sides of semipermeable membrane with equal flow rates
137
Which of the following 0.1 M aqueous solutions will have the lowest freezing point-
A
Potassium sulphate
B
Sodium chloride
C
Urea
D
Glucose
138
How many grams of NaOH will be needed to prepare 250 mL of 0.1 M solution-
A
1 g
B
10 g
C
4 g
D
6 g
139
The freezing point of solvent is depressed by 0.37°C in a 0.01 mol NaCl solution. The freezing point of 0.02 molal solution of urea is depressed by:
A
0.37°C
B
0.74°C
C
0.185°C
D
0°C
140
A and B ideal gases. The molecular weights of A and B are in the ratio of 1:4. The pressure of a gas mixture containing equal weight of A and B is p atm. What is the partial pressure (in atm) of B in the mixture?
A
p/5
B
p/2
C
p/2.5
D
3/4 p
141
Select correct statement -
A
b.p. of 1 molal NaCl solution is twice that of 1 molal sucrose solution
B
b.p. elevation of 1 molal glucose solution is half of the 1 molal KCl solution
C
b.p. is a colligative property
D
All of the above
142
Which solution will show maximum elevation in b.pt-
A
0.1 M KCl
B
0.1 M BaCl₂
C
0.1 M FeCl₃
D
0.1 M Fe₂(SO₄)₃
143
A binary solution of ethanol and n-heptane is an example of-
A
Ideal solution
B
Non ideal solution with +ve deviation
C
Non ideal solution with −ve deviation
D
Unpredictable behaviour
144
25 mL of 3.0 M HNO₃ are mixed with 75 mL of 4.0 M HNO₃. If the volumes are additive, the molarity of the final mixture would be-
A
3.25 M
B
4.0 M
C
3.75 M
D
3.50 M
145
10 gram of glucose are dissolved in 150 gram of water. The mass % of glucose is-
A
5%
B
6.25%
C
93.75%
D
15%
146
Solute when dissolved in water -
A
Increases the vapour pressure of water
B
Decreases the boiling point of water
C
Decreases the freezing point of water
D
All of the above
147
The vapour pressure of two liquids X and Y are 80 and 60 Torr respectively. The total vapour pressure of the ideal solution obtained by mixing 3 moles of X and 2 moles of Y would be:
A
68 Torr
B
140 Torr
C
48 Torr
D
72 Torr
148
Which among the following solutions will exhibit positive deviation from Raoult's law?
A
n-hexane and n-heptane
B
HNO₃ and water
C
Acetone and chloroform
D
Ethanol and acetone
149
When mango is placed in dilute aqueous solution of hydrochloric acid, it-
A
Shrinks
B
Swells
C
Bursts
D
Nothing happens
150
The unit of molality is:
A
mol–1
B
mol kg–1
C
mol–1 L–1
D
mol L
151
For an ideal binary liquid solution with P°A > P°B which relation between XA (mole fraction of A in liquid phase) & YA (mole fraction of A in vapour phase) is correct. XB & YB are mole fractions of B in liquid & vapour phase respectively-
A
XA = YA
B
XA > YA
C
XA/XB < YA/YB
D
XA, YA, XB, YB cannot be correlated
152
The hard shell of an egg is dissolved in acetic acid and then egg was subsequently placed in saturated solution of NaCl
A
The egg will shrink
B
The egg will become harder
C
The egg will swell
D
No change in the size of egg
153
In order to prepare 100 cm³ of 0.250 M barium chloride solution the amount of BaCl₂·2H₂O required will be (Ba = 137) -
A
0.250 moles
B
0.0025 moles
C
2.5 moles
D
6.1 gram of BaCl₂·2H₂O
154
Which of the following associated with isotonic solutions is not correct?
A
They will have the same osmotic pressure
B
They will have the same vapour pressure
C
They have same weight concentrations
D
Osmosis does not take place when the solutions is separated by a semipermeable membrane
155
A molar solution represents a solution of molarity equal to-
A
1
B
2
C
3
D
None
156
The boiling point of C₆H₆, CH₃OH, C₆H₅NH₂ and C₆H₅NO₂ are 80°C, 65°C, 184°C and 212°C respectively. Which will show highest vapour pressure at room temperature-
A
C₆H₆
B
CH₃OH
C
C₆H₅NH₂
D
C₆H₅NO₂
157
In cold countries, ethylene glycol is added to water in the radiators of cars during winters. It results in-
A
Lowering in boiling point
B
Reducing viscosity
C
Reducing specific heat
D
Lowering in freezing point
158
Binary liquid solutions which exhibit negative deviations from Raoult's law boil at temperature .... than the expected value:
A
Lower
B
Higher
C
Same
D
Cannot be said
159
The units of mole fraction of a compound in solution are-
A
mol kg⁻¹
B
mol litre⁻¹
C
g litre⁻¹
D
None of these
160
In a mixture of A and B, components show negative deviation when
A
A-B interaction is stronger than A-A and B-B interaction
B
A-B interaction is weaker than A-A and B-B interaction
C
ΔVmix > 0, ΔSmix > 0
D
ΔVmix = 0, ΔSmix > 0
161
The statement, “The mass of a gas dissolved in a given mass of a solvent at any temperature is proportional to the pressure of the gas above the solvent” is
A
Henry’s law
B
Law of mass action
C
Dalton’s law
D
None of these
162
Freezing point of an aqueous solution is –0.186°C. Elevation of boiling point of same solution would be: (Kb = 0.512 and Kf = 1.86 K molality–1)
A
0.186°C
B
0.0512°C
C
0.092°C
D
0.237°C
163
A 5% solution of cane sugar is isotonic with 0.877% of X. The molecular weight of substance X is-
A
58.98
B
119.96
C
95.58
D
126.98
164
One among the following is an incorrect statement-
A
Molality of a solution is dependent on the temperature
B
Molarity of a solution is dependent on the temperature
C
Normality of 0.5 M aqueous solution of H₂C₂O₄·2H₂O is 1 N
D
Molality of a solution relates moles of solute and mass of solvent
165
When 5.0 gram of BaCl₂ is dissolved in water to have 10⁶ gram of solution. The concentration of solution is-
A
2.5 ppm
B
5 ppm
C
5 M
D
5 g L⁻¹
166
25 mL of 3 M HCl were added to 75 mL of 0.05 M HCl. The molarity of HCl in the resulting solution is approximately-
A
0.055 M
B
0.35 M
C
0.787 M
D
3.05 M
167
Which of the following is not a colligative property -
A
ΔTf
B
π
C
ΔTb
D
Kb
168
If α is the degree of dissociation of Na2SO4 the van’t Hoff factor (i) used for calculating the molecular mass is:
A
1 – 2 α
B
1 + 2 α
C
1 – α
D
1 + α
169
Match List-I with List-II
The correct option is
A
a(i), b(ii), c(iv), d(iii)
B
a(i), b(iii), c(ii), d(iv)
C
a(iii), b(ii), c(i), d(iv)
D
a(iii), b(i), c(iv), d(ii)
170
0.5 M solution of urea is isotonic with-
A
0.5 M NaCl solution
B
0.5 M sugar solution
C
0.5 M BaCl₂ solution
D
0.5 M solution benzoic acid in benzene
171
The osmotic pressure of solution increases if-
A
Temperature is decreased
B
Solution constant is increased
C
Number of solute molecules are increased
D
Volume is increased
172
The vapour pressure of two pure liquid (A) and (B) are 100 torr and 80 torr respectively. The total pressure of solution obtained by mixing 2 mole of (A) and 3 mole of (B) would be:
A
120 torr
B
36 torr
C
88 torr
D
180 torr
173
Pure benzene freezes at 5.45°C at a certain place but a 0.374 m solution of tetra chloroethane in benzene freezes at 3.55°C. The Kf for benzene is-
A
5.08 K kg mol⁻¹
B
508 K kg mol⁻¹
C
0.508 K kg mol⁻¹
D
50.8°C kg mol⁻¹
174
In the aqueous solution of sulphuric acid the mole fraction of water is 0.85. The molality of the solution is-
A
8.9 m
B
0.19 m
C
9.8 m
D
15 m
175
The vant's Hoff factor for 0.1 Mba (NO3)2 solution is 2.74. The degree of dissociation is:
A
91.3%
B
87%
C
100%
D
74%
176
H₂O₂ solution used for hair bleaching is sold as a solution of approximately 5.0 g H₂O₂ per 100 mL of the solution. The molecular weight of H₂O₂ is 34. The molarity of this solution is approximately-
A
3.0
B
1.5
C
0.15
D
4.0
177
The V.P. curve of same solute in the same solvent are shown. The curves are parallel to each other and do not intersect. The concentration of solutions are in order of-
A
I < II < III
B
I = II = III
C
I > II > III
D
I > III > II
178
An example of colligative property is-
A
Freezing point
B
Boiling point
C
Vapour pressure
D
Osmotic pressure
179
The osmotic pressure of a solution is given by the relation-
A
π = RT/C
B
π = CT/R
C
π = RC/T
D
π/C = RT
180
Azeotropic mixture of water and HCl boils at 381.5 K. By distilling the mixture it is possible to obtain-
A
Pure HCl only
B
Pure water only
C
Neither HCl nor water
D
Both water and HCl in pure state
181
If 18 gram of glucose (C₆H₁₂O₆) is present in 1000 gram of an aqueous solution of glucose it is said to be-
A
39.2 gram
B
1.1 molal
C
0.5 molal
D
0.1 molal
182
Y gm of non-volatile solute of molar mass M is dissolved in 250 g of benzene. If Kb is molal elevation constant, the value of ΔT is given by-
A
.
B
.
C
.
D
.
183
The osmotic pressure of the solution having concentration 0.05 M.
A
Increases with increase in temperature
B
Does not change with change in temperature
C
Decreases with increase in temperature
D
Initially decreases and then increases with rise in temperature
184
Molal elevation constant of a liquid is:
A
The elevent in b.p. which would be produced by dissolving one mole of solute in 100 g of solvent
B
The elevation of b.p. which would be produced by dissolving 1 mole solute in 10 g of solvent.
C
Elevation in b.p. which would be produced by dissolving 1 mole of solute in 1000 g of solvent
D
None of the above
185
During depression of freezing point in a solution, the following are in equilibrium:
A
liquid solvent, solid solvent
B
liquid solvent, solid solute
C
liquid solute, solid solute
D
liquid solute, solid solvent
186
Cryoscopic constant of a liquid is-
A
Decrease in freezing point when 1 gram of solute is dissolved per kg of the solvent
B
Decrease in the freezing point when 1 mole of solute is dissolved per kg of the solvent
C
Is the elevation for 1 molar solution
D
Is a factor used for calculation of elevation in boiling point
187
If the vapour pressure of solutions of two liquids are less than those expected from ideal solution they are said to have-
A
Negative deviation from ideal behaviour
B
Positive deviations from ideal behaviour
C
Ideal behaviour
D
Positive deviation for lower conc. and negative deviations for higher concentration
188
The normality of 2.3 MH2SO4 solution is:
A
4.6 N
B
5.6 N
C
6.6 N
D
7.6 N
189
Which one of the following pairs of solution can we expect to be isotonic at the same temperature-
A
0.1 M urea and 0.1 M NaCl
B
0.1 M urea and 0.2 M MgCl₂
C
0.1 M NaCl and 0.1 M Na₂SO₄
D
0.1 M Ca(NO₃)₂ and 0.1 M Na₂SO₄
190
Which salt may show the same value of Vant Hoff factor (i) as that of K₄Fe(CN)₆ in very dilute solution state -
A
Al₂(SO₄)₃
B
NaCl
C
Al(NO₃)₃
D
Na₂SO₄
191
10 gram of solute with molecular mass 100 g mol⁻¹ is dissolved in 100 gram solvent to show 0.3°C elevation in boiling point. The value of molal ebullioscopic constant will be-
A
10
B
3
C
0.3
D
Unpredictable
192
Which of the following is not correct for ideal solution -
A
Raoult's law is obeyed for entire concentration range and temperatures
B
ΔSmix = 0
C
ΔVmix = 0
D
ΔHmix = 0
193
The passing of solvent particles through semipermeable membrane is called-
A
Osmosis
B
Electrodialysis
C
Electrophoresis
D
Electroplating
194
H₂O and perchloric acid (b.p. 383 K) form constant boiling mixture at 71.6% of perchloric acid. The boiling point of the solution at this composition is-
A
> 373 K but < 383 K
B
< 373 K
C
> 383 K
D
= 373 K
195
The vapour pressure of pure liquid A is 0.80 atm. When a non-volatile B is added to A its vapour pressure drops to 0.60 atm. The mole fraction of B in the solution is:
A
0.125
B
0.25
C
0.5
D
0.75
196
An azeotropic solution of two liquids has boiling point lower than either when it
A
Shows a negative deviation from Raoult’s law
B
Shows a positive deviation from Raoult’s law
C
Shows no deviation from Raoult’s law
D
Is saturated
197
Consider following vapour pressure composition graph. Hence-
A
V.P. of A = SZ
B
V.P. of B = ZY
C
V.P. of B = SY
D
V.P. of solution at X = SZ + SY
198
Solutions distilled without change in composition at a temperature are called-
A
Amorphous
B
Azeotropic mixture
C
Ideal solution
D
Super saturated solution
199
A solution of sucrose (molar mass 342 g mol–1) has been produced by dissolving 68.5 g sucrose in 1000 g water. The freezing point of the solution obtained will be: (Kf for H2O = 1.86 K kg mol–1)
A
–0.372°C
B
0.520°C
C
+ 0.372°C
D
0.570°C
200
The osmotic pressure of 10%(w/v) aqueous solution of urea (π₁) is related to that of 10%(w/v) aqueous solution of glucose (π₂) as -
A
π₁ = π₂
B
π₁ > π₂
C
π₁ < π₂
D
π₁ = 1 − π₂
201
The molal elevation/depression constant depends upon -
A
Nature of solvent
B
Nature of solute
C
Temperature
D
ΔH solution
202
pH of 1 M HA (weak acid) is 2. Hence van't Hoff factor is -
A
1.2
B
1.02
C
1.1
D
1.01
203
Henry's law is valid for which of the following gases in water-
A
CO₂
B
HCl
C
SO₂
D
N₂
204
When 10 g of a non-volatile solute is dissolved in 100 g of benzene, it raises boiling point by 1°C then molecular mass of the solute is (kb for C6 H6 = 2.53 kg–mol–1)
A
223 g
B
233 g
C
243 g
D
253 g
205
Which pair shows a contraction in volume on mixing along with evolution of heat-
A
CHCl₃ + C₆H₆
B
H₂O + HCl
C
H₂O + HNO₃
D
All
206
Which of the following is incorrect?
A
Relative lowering of vapour pressure is dependent on solute mole
B
Vapour pressure of a solution is lower than the vapour pressure of the solvent
C
The vapour pressure is a colligative property
D
The relative lowering of vapour pressure is directly proportional to the mole fraction solute
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