CLASS: XII CHAPTER: SOLUTION WORKSHEET No: 01
Q.1 Increasing the temperature of an aqueous solution will cause:
(a) decrease in molality (b) decrease in molarity
(c) decrease in mole fraction (d) decrease in % (w/w)
Q.2 The value of Henry’s constant KH 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
Q.3 Which of the following condition is not satisfied by an ideal solution?
(a) ΔHmixing = 0 (b) ΔVmixing = 0
(c) Raoult’s Law is obeyed (d) Formation of an azeotropic
mixture
Q.4 If 2 gm of NaOH is present is 200 ml of its solution, its molarity will be_
(a) 0.25 mol /L (b) 0.5 mol/ L (c) 5 mol /L (d) 1.0 mol/ L
Q.5 If two liquids A and B form minimum boiling azeotrope at some specific
composition then _____.
(a) A–B interactions are stronger than those between A–A or B–B.
(b) vapour pressure of solution increases because a greater number of molecules of
liquids A and B can
escape from the solution.
(c) vapour pressure of solution decreases because a smaller number of molecules
of only one of the
liquids escape from the solution.
(d) A–B interactions are weaker than those between A–A or B–B
Given below are two statements labelled as Assertion (A) and Reason (R)
Select the most appropriate answer from the options given below:
(a) Both A and R are true and R is the correct explanation of A
(b) Both A and R are true but R is not the correct explanation of A
(c) A is true but R is false
(d) A is false but R is true
Q.6 Assertion (A): Azeotropic mixtures are formed only by non-ideal solutions and
they may have boiling points either greater than both the components or less than
both the components.
Reason (R): The composition of the vapour phase is same as that of the liquid phase
of an azeotropic mixture.
Q.7 Assertion (A): Soda bottles are sealed under high pressure.
Reason (R): High pressure increases the solubility of carbon dioxide gas
Answer the questions in short
Q.1 (a) Define Mole fraction: (b) Azeotropes
Q.2 State the law co-relating the pressure & solubility of a gas in a liquid. State an application of this law.
Q.3 What type of deviation is shown by mixture of ethanol and acetone? Give reason.
Q.04 Write two differences between the solutions showing positive & negative deviation from Raoult’s law.
Q.05 On mixing liquid X and liquid Y , the volume of the resulting solution increases _
(a) What type of deviation from Raoult’s law is shown by the resulting solution?
(b) What change in temperature would you observe after mixing liquids X and Y?
Q.06 A solution of glucose (C6H12O6) in water is labelled as 10% by weight. What would be the molality of the
solution? (Molar mass of glucose = 180 g /mol)
Q.7 Give reason for followings
(a) Why are aquatic species more comfortable in cold water than in warm water?
(b) Deep sea divers are advised not to come to surface immediately from deep waters. Why?
(c) Cooking is faster in pressure cooker than in cooking pan
o o
(d) Two liquids A and B boil at 120 C and 160 C respectively. Which of them has
o
higher vapour pressure at 70 C?
(e) Name the substances which are used by deep sea divers to neutralize the toxic
effects of nitrogen
dissolved in the blood.
MULTIPLE CHOICE QUESTIONS:
1. The molality of 98% H2SO4 (density = 1.8 g/mL) by weight is:
(a) 6 m (b) 18 m (c) 10 m (d) 4 m
2. Which of the following does not show positive deviation from Raoult's law?
(a) benzone + chloroform (b) benzene + acetone
(c) benzene + ethanol (d) benzene + CCl4
3. Which solution will have least vapour pressure?
(a) 0.1 M BaCl2 (b) 0.1 M Urea (c) 0.1 M Na2SO4 (d) 0.1 M Na3PO4
4. Which condition is not satisfied by an ideal solution?
(a) ΔHmix = 0 (b) ΔVmix = 0 (c) ΔPmix = 0 (d) ΔSmix = 0
5. Azeotrope mixture are:
(a) mixture of two solids (b) those will boil at different temperature
(c) those which can be fractionally distilled (d) constant boiling mixtures
6. If Kf value of H2O is 1.86. The value of ΔTf for 0.1 m solution of non-volatile solute is
(a) 18.6 (b) 0.186 (c) 1.86 (d) 0.0186
7. Solute when dissolve in water
(a) increases the vapour pressure of water (b) decreases the boiling point of water
(c) decrease the freezing point of water (d) All of the above
8. The plant cell will shrink when placed in:
(a) water (b) A hypotonic solution (c) a hypertonic solution (d) an siotonic solution
9. The freezing point of 11% aquous solution of calcium nitrate will be:
(a) 0°C (b) above 0°C (c) 1°C (d) below 0°C
10. The Van’t Hoff factor for 0.1 M Ba(NO3)2 solution is 2.74. The degree of dissociation is:
(a) 91.3% (b) 87% (c) 100% (d) 74%
11. Which of the following solutions would have the highest osmotic pressure:
a) M/10NaCl (b) M/10 Urea c )M/10 BaCl2 d)M/10 Glucose
12. 0.5 M aquous solution of Glucose is isotonic with:
(a) 0.5 M KCl solution (b) 0.5 M CaCl2 solution
(c) 0.5 M Urea solution (d) 1 M solution of sucrose
13. Which of the following is true for Henry's constant
(a) It decreases with temperature (b) It increases with temperature
(c) Independent on temperature (d) It do not depend on nature of gases.
14. Which one is the best colligative property for determination of molecular mass of polymer?
(a) osmotic pressure (b) elevation in boiling point
(c) depression in freezing point (d) osmosis
15. Which of the following do not depend on temperature?
(a) % W/V (weight/volume) (b) molality (c) molarity (d) normality
16. Henry's law constant K of CO2 in water at 25°C is 3 × 10–2 mol/L atm–1. Calculation the mass of CO2 present
in 100 L of soft drink bottled with apartial pressure of CO2 of 4 atm at the same temperature.
(a) 5.28 g (b) 12.0 g (c) 428 g (d) 528 g
17. Mixing of HNO3 and HCl is reaction:
(a) endothermic reaction (b) exothermic reaction
(c) both exothermic and endothermic (d) depend on entropy of reaction
18. The most likely on ideal solution is:
(a) NaCl—H2O (b) C2H5OH—C6H6 (c) C7H16—H2O (d) C7H16—C8H18
19. Van't Hoff factor for a dilute solution of a K2[HgI4] is:
(a) 2 (b) 1 (c) 3 (d) zero
20. Benzoic acid dissolved in benzene shows a molecular weight of:
(a) 122 (b) 61 (c) 244 (d) 366
21. 6% (W/V) solution of urea will be isotonic with:
(a) 18% (W/V) solution of glucose (b) 0.5 M solution of NaCl
(c) 1 M solution of CH3COOH (d) 6% (W/V) solution of sucrose.
22. Solution showing (+) ve deviation from Raoult’s law include:
(a) acetone + CS2 (b) acetone + C2H5OH (c) acetone + Benzene (d) acetone + aniline
23. The property which depends on number of particles of solute is called .............
24. Azeotrope mixture cannot be separate by .............
25. Match the column and choose correct option
Vant'Hoff factor Behaviour of compound
(A) i = 1 P. Impossible
(B) i > 1 Q. Association is the solution
(C) i < 1 R. Dissociation in the solution
(D) i = 0 S. No dissociation or association
(a) A–S, B–R, C–P, D–Q (b) A–R, B–S, C–Q, D–P
(c) A–S, B–P, C–R, D–Q (d) A–S, B–R, C–Q, D–P
Assertion Reason Type
26. Statement 1: Azeotropemixture are formed by only non-ideal solution
Statement 2: Azeotrope mixture can't be separated by fractional distillation.
VERY SHORT ANSWER TYPE QUESTIONS (1 Mark)
Q. 1. What is Van’t Hoff factor ?
Q. 2. What is the Van’t Hoff factor in K4[Fe(CN)6] and BaCl2 ?
Q. 3. Why the molecular mass becomes abnormal ?
Q. 4. What role does the molecular interaction play in the solution of alcohol and water ?
Q. 5. What is van’t Hoff factor ? How is it related with :
(a) degree of dissociation (b) degree of association
Q. 6. Why NaCl or CaCl2 is used to clear snow from roads ?.
Q. 7. Why the boiling point of solution is higher than pure liquid ?.
Q. 8. Henry law constant for two gases are 21.5 and 49.5 atm, which gas is more soluble ?
Q.9. Define azeotrope. Give an example of maximum boiling azeotrope.
Q.10. Calculate the volume of 75% of H2SO4 by weight (d = 1.8 gm/ml) required to prepare 1 L of 0.2 M solution.
Q.11. Why water cannot be completely separated from aqueous solution of ethyl alcohol ?
Q.12. What is the effect on boiling and freezing point of a solution on addition of NaCl ?.
Q.13. Why osmotic pressure is considered as colligative property ?
Q.14. Liquid A and B on mixing produce a warm solution. Which type of deviation does this solution show ?
Q.15. Give an example of a compound in which hydrogen bonding results in the formation of a dimer.
SHORT ANSWER TYPE QUESTIONS (2 Marks)
Q. 1. Out of the following three solutions, which has the highest freezing point and why ?
(a) 0.1 M urea (b) 0.1M BaCl2 (c) 0.1M Na2SO4
Q. 2. Which of the following solutions have highest boiling point and why ?
(a) 1M glucose (b) 1M KCl (c) 1M aluminium nitrate
Q. 3. Equal moles of liquid P and Q are mixed. What is the ratio of their moles in the vapour phase ? Given that
Given that PP = 2 ⋅ PQ
Q. 4. On mixing liquid X and Y, volume of the resulting solution decreases. What type of deviation from Raoult’s law
is shown by the resulting solution ? What change in temperature would you observe after mixing liquids X and Y ?
Q 5.Why is it advised to add ethylene glycol to water in a car radiator in hill station ?.
Q.6. The dissolution of ammonium chloride in water is endothermic process. What is the effect of temperature on its
solubility ?
Q.7. Two liquids A and B boil at 145ºC and 190ºC respectively. Which of them has higher vapour pressure at 80ºC ?
Q.8. Why is liquid ammonia bottle first cooled in ice before opening it ?
Q.9. Which colligative property is preferred for the molar mass determination of macromolecules ?
Q 10. 18 g of glucose (C6 H12O6 ) (molar mass = 180 g mol-1 ) is dissolved in 1 kg of water in a sauce pan. At what
temperature will this solution boil ? (Kb for water = 0.52 K kg mol-1 ,
