1

Lakshya JEE 2.0 (2026)

Solution NPP-01
1. What weight of H2SO4 is required to prepare 0.1 M, 2 L 4. 149 gm of potassium chloride (KCl) is dissolved in 10
aqueous solution of H2SO4? L of an aqueous solution. Determine the molarity of
the solution (K = 39 Cl = 35.5)
2. 1 L solution of a solute X has molarity 3 M. If the
solution contains 180 g solute X in it, the solute might
be 5. Calculate the molarity of a solution containing 5 g of
(A) Glucose(60) (B) Ethanol(46) NaOH in 450 mL solution.
(C) Urea(60) (D) Sucrose(342)
6. Calculate the amount of benzoic acid (C6H5COOH)
3. Find the weight of urea in its 0.25 M aqueous solution. required for preparing 250 mL of 0.15 M solution in
(A) 7.5 g (B) 15 g
methanol.
(C) 30 g (D) 60 g

Answer Key
1. (19.6 gms) 4. (2 mole)
2. (C) 5. (5/18 M)
3. (B) 6. (4.575 gm)

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Solution NPP-02
1. 0.1 M, 400 mL NaCl is mixed with 'x' mL, 0.2 M NaCl 9. In a mixture 46 g C2H5OH (molar mass = 46) is
solution. The molarity of resulting mixture is 0.14 M dissolved in water to make 200 ml solution. The
Calculate 'x'? molarity of solution is
(A) 1M (B) 2M
2. Calculate the molarity of new solution when 250 mL (C) 3M (D) 5M
water is added in 350 mL of 0.1 M glucose solution.
10. 6.02 × 1021 molecules of HNO3 are dissolved in 100 ml
solution. Find the molarity of solution?
3. What volume of H₂O should be added to 500 mL, 4 M
(A) 0.01 M (B) 0.1 M
NaOH solution so that molarity is reduced to 0.8 M?
(C) 1 M (D) 10 M

4. 200 mL of 0.3 M sugar solution is diluted up to 500 mL.

11. 100 mL of Na3PO4 solution contains 3.45 g of sodium.
Calculate molarity of final solution.
The molarity of the solution is ____ × 10-2 mol L-1,
(Nearest Integer)
5. If 100 ml of 1.0 M NaOH solution is diluted to 1.0 the [Atomic Masses - Na: 23.0 u, 0: 16 u, P: 31.0 u]
resulting solution contains-
(A) 1 mole of NaOH 12. 0.1 M, 200 mL HCl is mixed with 800 mL, 0.2 M HCl
(B) 0.1 mole of NaOH solution. Calculate the molarity of resulting mixture?
(C) 10.0 mole of NaOH
13. Dissolving 120 g of urea (mol. Wt. 60) in 1000 g of
(D) 0.05 mole of NaOH
water gave a solution of density 1.15 g/mL. The
molarity of the solution is
6. What mass of NaOH is to be taken to prepare 0.2 M, (A) 1.78 M (B) 2.00 M
500 ml solution ? (C) 2.05 M (D) 2.22 M

7. If 80 g of copper sulphate CuSO4.5H2O is dissolved in 14. The amount of sugar (C12H22O11) required to prepare 2
deionised water to make 5 L of solution. The L of its 0.1 M aqueous solution is :
concentration of the copper sulphate solution is x × 10-3 (A) 136.8 g (B) 17.1 g
mol L-1. The value of x is ______. (C) 68.4 g (D) 34.2 g
[Atomic masses Cu: 63.54 u, S: 32 u, 0: 16 u, H: 1 u]
15. 5g of NaOH was dissolved in deionized water to
8. The molarity of the solution prepared by dissolving 6.3 prepare a 450mL stock solution. What volume (in mL)
g of oxalic acid (H2C2O4.2H2O) in 250 mL of water in of this solution would be required to prepare 500mL of
mol L–1 is x × 10-2. The value of x is Integer) (Nearest 0.1 M solution? Given: Molar Mass of Na, O and H is
23, 16 and 1 g mol–1 respectively
[Atomic mass: H: 1.0, C: 12.0, 0: 16.0]
 2

Answer Key
1. (266.67 ML) 9. (D)
2. (0.0583 M) 10. (B)
3. (2000 ML) 11. (50)
4. (0.12 M) 12. (0.18 M)
5. (B) 13. (C)
6. (4 GMS) 14. (C)
7. (64) 15. (180)
8. (20)

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Solution NPP-03
1. 8 gms of NaOH is added to 100 gm of water. Calculate 10. If sea water is assumed to contain 40g of salt per 200g
the molality of the solution? of sea water then percentage by mass of salt present is
(A) 15% (B) 40%
(C) 20% (D) 10%
2. 0.2 mol (Al2SO4)3 is dissolved in water to make 500 ml
solution. Find the molarity of each ion in the solution?
11. Calculate the mass percentage of benzene (C6H6) and
carbon tetrachloride (CCl4) if 22 g of benzene is
3. 0.2 mole of Na2CO3 is dissolved in water to make 100
dissolved in 122 g of carbon tetrachloride.
ml solution. Find the concentration of each ion
(A) 33% (B) 3.3%
assuming complete dissociation of salt in solution
(C) 96.77% (D) 16.67%

4. What mass of NaOH should be added to 500 gm of

12. 20 gram of NaOH dissolved in 100 ml of water solution
water to make a 3 molal solution. at 300K temperature. If the density of solution is
1.2g/ml than calculate mass percentage of NaOH.
5. 225 gm of an aqueous solution contains 5 gm of urea.
What is the concentration of the solution in terms of 13. 40 gram NaOH dissolve in 100 gram H2O. Select
molality (Mol. Wt. of urea = 60) correct statements for about solution.
(A) Mass % of NaOH is 28.57

6. Calculate molality of 2.5 g of ethanoic acid (B) Mass fraction of NaOH is 0.2857

(CH3COOH) in 75 g of benzene. (C) both A and B are correct

(D) None

7. Calculate the mass of urea (NH2CONH2) required in

making 2.5 kg of 0.25 molal aqueous solution. 14. 300 gram solution of 20% (w/w) NaOH mixed with 200
gram solution of 10% (w/w) NaOH solution, calculate
mass percentage of NaOH in resultant solution
8. Calculate the mole fraction of NaCl in a mixture
(A) 16% (B) 32%
containing 0.585 gm of NaCl in 30 gms of urea.
(C) 10% (D) 12%
(Assume mass of solution= mass of solvent)

9. 20 gms KCl is dissolved in 30 gms H2O. Calculate 15. 40 gms of NaOH is dissolved in 100 mL of H2O.
mass/mass percentage? Calculate Mass% of solution formed. Density-1 gm/mL.
 2

Answer Key
1. (2) 7. (37.5 GMS)
2. ( Al +3
= 0.8M ) 8. (1/51)
9. (40)
(SO −2
4 = 1.2M ) 10. (C)

3. ( Na +
= 4M ) 11. ((BENZENE= 15.28%)
CHLORIDE: 84.72%))
(CARBON TETRA-

( CO −2
3 = 2M ) 12. (D)

4. (60 GMS) 13. (C)

5. (25/66 m) 14. (A)

6. (0.55m) 15. (28.57%)

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Solution NPP-03
1. Calculate the molality of 1 M NaOH solution. Given: 9. Calculate the mole fraction of NaOH aqueous solution
Density of solution = 1.2 gm/mL. having 40%(mass/mass)?

2. Calculate the molality of an aqueous solution in which 10. 20% (W/W) solution of NaOH present in container.
the mole fraction of solute is 0.25? Calculate mole fraction of solute

3. Density of 20% (w/v) solution of NaOH is 1.2 g/ml 11. Mole fraction of NaOH in aq. Solution of NaOH is 0.4
calculate mole fraction of solute than calculate mass% of NaOH?

4. A bottle of commercial sulphuric acid (density 1.787 g 12. A solution is obtained by mixing 300g of 25% solution
–1
ml ) is labeled as 85% by weight. What is the molarity and 400g of 40% solution by mass. Calculate the mass
of acid ? percentage of the resulting solution.

5. Calculate the molality of 1.0 L solution of 93% 13. Calculate the mole fraction of benzene in solution
H2SO4(weight/ volume). The density of the solution is containing 30% by mass in carbon tetrachloride.
1.84g/ mL.
14. Concentrated nitric acid used in laboratory work is 68%

6. gm of oxygen is dissolved in water to form 104 gm of nitric acid by mass in aqueous solution. What should be
solution. Find the concentration of oxygen in ppm. the molarity of such a sample of the acid if the density
of the solution is 1.504g mL–1?

7. Calculate the mass % of 10 PPM aqueous solution of

CaCO3? 15. A sample of drinking water was found to be severely

8. Glucose forms 3 different solution with water contaminated with chloroform (CHCl3) supposed to be

Solution-A 10% (w/w) ac carcinogen. The level of contamination was 15 ppm

Solution-B 10 ppm (by mass) :

Solution-C 10 ppb (i) express this percent by mass

Select the correct option? (ii) Determine the molality of chloroform in the water

(A) Maximum Mass of Glucose is present in A sample.

(B) Maximum Mass of Glucose is present in B

16. What is molarity of 10% CaCO3 solution
(C) Maximum Mass of Glucose is present in C
(mass/volume) ? Molar mass = 100
(D) Same Mass of Glucose is present in A,B and C
 2

17. What is the molality of 10% CaCO3 solution

(mass/mass)% ? 23. A commercially sold conc. HCl is 35% HCl by mass. If
the density of this commercial acid is 146g / mL, the
18. What is the molality of 0.1 Molar solution (density = molarity of this solution is :
1.1g / ml) of CaCO3 ? (Atomic mass: Cl = 35.5 amu, H = 1amu)
(A) 10.2 M
19. 100 ppm CaCO3 (aq. Solution). What is the molality of (B) 12.5 M
the solution ? (C) 14.0 M
(D) 18.2 M
20. What is mole fraction of solute in aqueous solution
whose molality is 2 ? 24. 29.2 % (w/W) HCl stock solution has density of
1.25g mL–1. The molecular weight of HCl is 36.5g
21. A 6.50 molal solution of KOH (aq) has a density of 1.89 mol–1. The volume of (mL) of stock solution required
g cm–3. The molarity of the solution is _____mol dm–3 to prepare a 200 mL solution 0.4 M HCl is

(Round off to the nearest integer).

[Atomic masses : K = 39.0u, O = 16.0u, H = 1.0u]
25. The density of NaOH solution is 1.2 gm cm–3. The
molality of this solution is________m.
22. The mole fraction of a solute in a 100 molal aqueous (Round off the Nearest Integer)
solution is _______×10–2 [Use : Atomic masses : Na 23.0u O : 16. 0u H: 1.0 u
(Round off the Nearest Integer). Density of H2O : 1.0 gm cm–3]
[Given : Atomic masses : H: 1.0 u, O : 16.0 u]

Answer Key
 3

1. (0.86) 14. (16.2)

2. (18.51) 15. (1.) (1.5×10–3%)
3. (0.081) (2.) (1.3×10–4m)
4. (15.68) 16. (1 M)
5. (10.42) 17. (1.11 m)
6. (200) 18. (1/119 m)
7. (.001) 19. (10–3 m)
8. (D) 20. (0.035)
9. (10/13) 21. (9)
10. (0.1) 22. (64)
11. (59.7%) 23. (C)
12. (33.6%) 24. (8 mL)
13. (0.46) 25. (5)

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Solution NPP-05
1. The molarity of a 70% (mass/mass) aqueous solution of 9. The molarity of 1L orthophosphoric acid (H3PO4)
a monobasic acid (X) is ________ × 10-1 M (Nearest having 70% purity by weight (specific gravity 1.54 g
integer) cm³) is M.(Molar mass of H3PO4 = 98 g mol–1)
[Given: Density of aqueous isolation of (X) is 1.25 g
mL–1 Molar mass of the acid is 70 g mol–1] 10. The Molarity (M) of an aqueous solution containing
5.85 g of NaCl in 500 mL water is:
2. Concentrated nitric acid is labelled as 75% by mass. The
volume in mL of the solution which contains 30 g of (Given: Molar Mass Na: 23 and Cl: 35.5 g mol–1)
nitric acid is_______. (A) 20
Given: Density of nitric acid solution is 1.25 g/mL. (B) 0.2
(A) 45 (B) 55 (C) 2
(C) 32 (D) 40
(D) 4
3. The quantity which changes with temperature is:
11. The density of 'x' M solution ('x' molar) of NaOH is
(A) Molarity
(B) Mass percentage 1.12 g mL–1. while in molality, the concentration of the
solution is 3 m (3 molal). Then x is (Given: Molar mass
(C) Molality
of NaOH is 40 g/mol)
(D) Mole fraction (A) 3.5
(B) 3.0
4. Volume of 3M NaOH (formula weight 40 g mol–1)
which can be prepared from 84 g of NaOH is_______ (C) 3.8
× 10–1 dm3. (D) 2.8

5. A solution of H2SO4 is 31.4% H2SO4 by mass and has a 12. Molality (m) of 3M aqueous solution of NaCl is:
density of 1.25 g/mL. The molarity of the H2SO4
(Given: Density of solution = 1.25 g mL–1, Molar mass
solution is M (nearest integer) [Given molar mass of
H2SO4 = 98 g mol–1] is g mol–1 - Na-23, Cl-35.5)
(A) 2.90 m
6. Molality of 0.8 M H2SO4 solution (density 1.06 g cm ) 3 (B) 2.79 m
is _______ × 10-3 m. (C) 1.90 m
(D) 3.85 m
7. The mass of sodium acetate (CH3COONa) required to
prepare 250 mL of 0.35 M aqueous solution is g.(Molar
13. Molarity of an aqueous solution of urea is 4.44 M. Mole
mass of CH3COONa is 82.02 g mol–1)
fraction of urea in solution is x × 10-3. Value of x is
8. If a substance 'A' dissolves in solution of a mixture of (integer answer)
'B' and 'C' with their respective number of moles as nA,
nB and nC, mole fraction of C in the solution is: 14. A solution is prepared by adding 1 mole ethyl alcohol
nC nC in 9 mole water. The mass percent of solute in the
(A) (B)
nA − nB − nC nA − nB − nC solution is _______ (Integer Answer)
nC nB (Given: Molar mass in g mol–1 Ethyl alcohol: 46, water:
(C) (D) 18)
nA + nB + nC nA + nB
 2

15. Molarity (M) of an aqueous solution containing x g of 17. The density of 3 M aqueous solution of NaCl is 1.0 g
anhyd. CuSO4 in 500 mL solution at 32°C is 2 × 10-1 M. mL–1. Molarity of the solution is _______× 10-2 m.
Its molality will be ______ × 10-3 m. (Nearest integer). (Nearest Integer)
(Given density of the solution = 1.25 g/mL) Given: Molar masses of Na and Cl is 23 and 35.5 g
mol–1 respectively.
16. Given below are two statements: one is labelled as
Assertion (A) and the other is labelled as Reason (R). 18. The molarity of a 10%(V/V) solution of di-bromine
Assertion (A): 3.1500g of hydrated oxalic acid solution in CCl4 (carbon tetrachloride) is: x. x =
dissolved in water to make 250.0 mL solution will result _______ × 10-2 M. (Nearest Integer)
in 0.1 M oxalic acid. [Given: Molar mass of Br2 = 160 g mol–1,
Reason (R): Molar mass of hydrated oxalic acid is 126 atomic mass of C = 12g mol-1
g mol-1. atomic mass of Cl = 35.5g mol-1
In the light of the above statements, choose the correct density of dibromine = 3.2 g cm-3,
answer from the options given below: density of CCl4 = 1.6 g cm³]
(A) Both (A) and (R) are true but (R) is NOT the
correct explanation of (A). 19. 74.5 g of a metallic chloride contains 35.5 g of chlorine.
(B) (A) is false but (R) is true. Find the equivalent mass of metal.
(C) (A) is true but (R) is false.
20. If the equivalent mass of S in SO2 is 8, then equivalent
(D) Both (A) and (R) are true and (R) is the correct
weight of S in SO3 is:
explanation of (A).
 3

Answer Key
1. (125) 11. (B)

2. (C) 12. (B)

3. (A) 13. (74)

4. (7) 14. (22)

5. (4) 15. ()

6. (815) 16. (D)

7. (7) 17. (364)

8. (B) 18. (139)

9. (11) 19. (39)

10. (B) 20. (16/3)

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Solution NPP-06

1. On increasing the altitude at constant temperature, 8. The vapour pressure of pure benzene at a certain
vapour pressure of a liquid temperature is 640 mm Hg. A non-volatile solid
(A) increases weighing 2.175gm is added to 39.0gm of benzene. The
(B) decreases V.P. of the solution is 600 mmHg. What is the
(C) remains the same molecular mass of the solid substance?
(D) depends upon climate
9. At 40°C the vapour pressure of mix of methyl alcohol
2. The vapour pressure of water at 300 K in a closed ethyl alcohol is represented by P = 199x + 135
container is 0.4 atm. If the volume of the container is where x is mol fraction of methyl alcohol. What is the
doubled, its vapour pressure at 300 K will be
pressure of pure ethyl alcohol at 40°C?
(A) 0.8 atm (B) 0.2 atm
(C) 0.4 atm (D) 0.6 atm
10. The vapour pressure of two volatile liquids A and B at
3. The vapour pressure of a given liquid will decrease if : 25°C are 50 Torr and 100 Torr, respectively. If the
(A) surface area of liquid is decreased liquid mixture contains 0.3 mole fraction of A, then the
(B) the volume of liquid in the container is decreased x
mole fraction of liquid B in the vapour phase is The
(C) the volume of the vapour phase is increased 17
(D) the temperature is decreased value of x is

4. Vapour pressure of the liquid 11. Liquids A and B form an ideal solution in the entire
(A) increases with increase in temperature. composition range. At 350 K, the vapour pressures of
(B) decreases with increase in temperature. pure A and pure B are 7 × 103 Pa and 12 × 103 Pa,
(C) is independent of temperature. respectively. The composition of the vapour in
(D) either increases or decreases with the increase in equilibrium with a solution containing 40 mole percent
temperature, depending on the nature of liquid. of A at this temperature is
(A) xA = 0.76 xB = 0.24
5. The boiling points of C6H6, CH3OH, C6H5NH2 and
(B) xA = 0.28 xB = 0.72
C6H5NO2 are 80°C, 65°C, 184°C and 212°C,
(C) xA = 0.4 xB = 0.6
respectively. Which of the following will have the
highest vapour pressure at the room temperature? (D) xA = 0.37 xB = 0.63
(A) C6H6 (B) CH3OH
(C) C6H5NH2 (D) CH3NO2 12. Calculate the mole fraction of toluene in the vapour
phase which is in equilibrium with a solution of benzene
6. Which of the following is not a characteristic property and toluene having a mole fraction of toluene 0.50. The
of the polar liquids? vapour pressure of pure benzene is 119 torr; that of
(A) They have high boiling points. toluene is 37 torr at the same temperature.
(B) They have high heat of vaporization (A) 0.327
(C) They have low viscosity. (B) 0.237
(D) They have low vapour pressure. (C) 0.732
(D) 0.456
7. A mixture of ethyl alcohol and propyl alcohol has a
vapour pressure of 290 mm at 300 K. The vapour 13. What weight of the non-volatile solution urea (NH2–
pressure of propyl alcohol is 200 mm. If the mole CO–NH2) needs to be dissolved in 100 g of water, in
fraction of ethyl alcohol is 0.6, its vapour pressure (in order to decrease the vapour pressure of water by 25%?
mm) at the same temperature will be ____.
 2

Answer Key
1. (C) 8. (69.6)

2. (C) 9. (135)

3. (D) 10. (14)

4. (A) 11. (13)

5. (B) 12. (B)

6. (D) 13. (111.11 gm)

7. (A)

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Solution NPP-07

1. Water and chlorobenzene are immiscible liquids. 5. A gaseous mixture of two substances A and B, under a
Their mixture boils at 89°C under a reduced total pressure of 0.8 atm is in equilibrium with an ideal
pressure of 7.7 × 104 Pa. The vapour pressure of liquid solution. The mole fraction of substance A is 0.5
pure water at 89°C is 7 × 104 Pa. Weight per ccent in the vapour phase and 0.2 in the liquid phase. The
of chlorobenzene in the distillate is vapour pressure of pure liquid A is atm. (Nearest
Integer)
2. The vapour pressure of pure benzene and methyl
benzene at 27°C is given as 80 Torr and 24 Torr, 6. Liquid A and B form an ideal solution. The vapour
respectively. The mole fraction of methyl benzene in pressures of pure liquids A and B are 350 and 750 mm
vapour phase, in equilibrium with an equimolar mixture Hg respectively at the same temperature. If XA and XB
of those two liquids (ideal solution) at the same are the mole fraction of A and B in solution while yA
temperature is ________× 10-2 (nearest integer)
and yB are the mole fraction of A and B in vapour phase
then:
3. Mass of Urea (NH2CONH2) required to be dissolved in
x A yA
1000 g of water to reduce the vapour pressure of water (A) 
x B yB
by 25% is g.(Nearest Integer)
Given: Molar mass of N, C, O and H are 14, 12, 16 and x A yA
(B) =
1g mol–1 respectively x B yB
x A yA
(C) 
4. The Total pressure observed by mixing two liquid A x B yB
and B is 350 mm Hg when their mole fractions are 0.7
(D) ( x A − yA )  ( x B − yB )
and 0.3 respectively. The Total pressure becomes 410
mm Hg if the mole fractions are changed to 0.2 and 0.8
respectively for A and B. The vapour pressure of pure
A is mmHg. (Nearest Integer) Consider the liquids and
solutions behave ideally.
 2

Answer Key
1. (38.46) 4. (314)

2. (23) 5. (2)

3. (1111) 6. (C)

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Solution NPP-11

1. The amount of (urea) to be dissolved in 500cc of 3. A solution of urea in water has boiling point of
water (Kf = 1.86) to produce a depression of 100.15°C. Calculate the freezing point of the same
0.186°C in the freezing point. solution. If Kr and Kb for water are 1.87 K Kg mol-1 and
0.52 K kg mol–1 respectively.
2. What should be the freezing point of aqueous solution
containing 17gm of C2H5OH is 100gm of water.
(Kf for water = 1.86)

Answer Key
1. (3gms) 3. (–0.54)

2. (–6.87)

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Solution NPP-12

1. 1.46 g of a biopolymer dissolved in a 100 mL water at 6. Which of the following have maximum freezing point?
300 K exerted an osmotic pressure of 2.42 × 10-3 bar. (A) 10 M urea
The molar mass of the biopolymer is ______ × 104 g (B) 2 M Al2(SO4)3
mol-1. (Round off to the Nearest Integer) (C) 4 M KCl
[Use: R = 0.083 L bar mol-1 K-1]
(D) All same

2. A solution containing 4.0 g of PVC in 2 litre of dioxane

7. If 5.85 gm of NaCl is present in 100 gm of water and %
(industrial solvent) was found to have an osmotic
dissociation for NaCl is 80%. Calculate the boiling
pressure 3 × 10-4 atm at 27°C. The molar mass of the
point of this solution.
polymer (g/mol) will be:
(A) 1.6 × 104 (B) 1.6 × 105
8. The number of pairs of the solutions having the same
(C) 1.6 × 103 (D) 1.6 × 102
value of the osmotic pressure from the following is
______ (Assume 100% ionization)
3. A solution is prepared by dissolving 0.6 g of urea (molar 1. 0.500M C2H5OH(aq) and 0.25M KBr(aq)
mass = 60 g mol-1) and 1.8 g of glucose (molar mass =
180 g mol-1) in 100 mL of water at 27°C. The osmotic 2. 0.100M K  Fe(CN)6  (aq) and
pressure of the solution is (R = 0.08206 L atm K K–1 0.100M FeSO 4 ( NH 4 )2 SO 4 (aq)
mol-1)
3. 0.05M K 4  Fe(CN)6  (aq) and
(A) 8.2 atm (B) 2.46 atm
0.25M NaCl(aq)
(C) 4.92 atm (D) 1.64 atm
4. 0.15M NaCl(aq) and 0.1M BaCl2 (aq)

4. An aqueous solution of sucrose (C12H22O11) having a 5. 0.02M KCl.MgCl2  6H2O(aq) and

concentration of 34.2 gram/litre has an osmotic pressure 0.05M KCl(aq)
of 2.38 atmospheres at 17°C. For an aqueous solution
of glucose (C6H12O6) to be isotonic with this solution, 9. A 0.5 percent solution of potassium chloride was found
its concentration should be: to freeze at -0.24°C. The percentage dissociation of
(A) 34.2 gram per litre potassium chloride is _______.
(B) 17.1 gram per litre (Nearest integer)
(C) 18.0 gram per litre (Molal depression constant for water is 1.80 K kg mol-1
and molar mass of KCl is 74.6 g mol-1)
(D) 36.0 gram per litre

10. Of the following four aqueous solutions, total number

5. Which of the following pair of solutions can be
of those solutions whose freezing point is lower than
expected to be isotonic at the same temperature?
that of 0.10 M C2H5OH is ______(Integer answer)
(A) 0.1 M urea and 0.1 NaCl
(A) 0.10 M Ba3(PO4)2
(B) 0.1 M NaCl and 0.1 M Na2SO4
(B) 0.10 M Na₂SO₄
(C) 0.1 M Ca(NO3)2 and 0.1 M Na2SO4
(C) 0.10 M KCI
(D) 0.1 M glucose and 0.2 M MgCl2
(D) 0.10 M Li3PO4
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11. In a solvent 50% of an acid HA dimerizes and the rest 14. How much amount of NaCl should be added to 600
dissociates. The van't Hoff factor of the acid is ______ g of water (p = 1.00 g/mL) to decrease the freezing
× 10–2.
point of water to -0.2°C ______. (The freezing point
12. A solute A dimerizes in water. The boiling point of a 2 depression constant for water = 2 k kg mol–1)
molal solution of A is 100.52°C. The percentage
association of A is ______.
(Round off to the Nearest Integer). 15. A 1.2% solution (wt/vol) of NaCl is isotonic with 7.2%
[Use: Kb for water = 0.52 K kg mol-1 Boiling point of solution (wt/vol) of glucose. Calculate the degree of
water = 100°C] ionisation & Van't Hoff factor of NaCl ?

13. Which one of the following 0.06 M aqueous solutions

has lowest freezing point? 16. Calculate observed Molar Mass of NaCl when it is 80%
(A) Al2(SO4)3 (B) C6H12O6 ionised?
(C) Kl (D) K2SO4
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Answer Key
1. (15) 9. (98)
2. (B) 10. (4)
3. (C) 11. (125)
4. (C) 12. (100%)
5. (C) 13. (A)
6. (C) 14. (1.755 gms)
7. (100.936) 15. (i = 1.95 and 0.95)
8. (4) 16. (32.5 gm)

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