SAMBHAWANA- 2026
DAV (KHALARI)
DPP-01 TOPIC:- SOLUTION
📘 Class 12 Chemistry – Important Questions
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📍 Chapter: Solutions
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Topics Covered:
● Introduction to Solutions
● Concentration of Solutions
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● Solubility
● Henry’s Law
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● Raoult’s Law
🟠 1 Mark Questions (Very Short Answer Type)
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1. Define an ideal solution. Give an example. (CBSE PYQ)
2. What is the mass percentage?
3. Write the mathematical expression for Henry’s Law.
4. State one difference between ideal and non-ideal solutions.
5. Why does solubility of a gas in a liquid decrease with rise in
temperature?
🟡 2 Mark Questions (Short Answer Type-I)
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6. Differentiate between molarity and molality. Which of them is
temperature independent? (CBSE PYQ)
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7. Why are carbonated beverages bottled under high pressure
according to Henry’s law?
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8. How does the solubility of NaCl and KNO₃ in water vary with
temperature?
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9. How is concentration of a solution expressed in terms of (i) mass %
and (ii) mole fraction?
10. Define Raoult’s law. How does it apply to ideal solutions?
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🔵 3 Mark Questions (Short Answer Type-II)
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11. State Henry’s law and explain its application in carbonated drinks
and scuba diving. (CBSE PYQ 2020)
12. Calculate the molality of a 0.5 M NaCl solution with a density of 1.2
g/mL.
13. Explain the difference between ideal and non-ideal solutions in
terms of intermolecular interactions. Give examples.
14. State Raoult’s law and explain vapour pressure of a binary liquid
solution using a graph.
15. Two partially miscible liquids are mixed. What type of behaviour
and observations would you expect?
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🔴 5 Mark Questions (Long Answer Type)
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16. Explain vapour pressure of an ideal solution using Raoult’s law.
Distinguish between ideal and non-ideal solutions with diagrams and
examples. (CBSE PYQ 2019)
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17. State Henry’s law. What is the effect of pressure and temperature
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on the solubility of a gas? Explain with examples. (CBSE PYQ)
18. Write the steps for preparing a 2 m (molal) solution of glucose in
water.
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19. Show graphically how total vapour pressure of a liquid-liquid
mixture varies with mole fraction of the component using Raoult’s law.
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20. What is the significance of deviations from Raoult’s law? Explain
positive and negative deviations with examples.
1. A binary liquid solution forms an azeotrope. This means:
a) It behaves ideally
b) It has constant boiling point
c) It has zero vapour pressure
d) It forms immiscible liquids
2. Which of the following will form an ideal solution?
a) Benzene + Toluene
b) Acetone + Chloroform
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c) HCl + H2O
d) Ethanol + Water
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3. A mixture of ethanol and water shows:
a) Positive deviation from Raoult's law
b) Negative deviation from Raoult's law
c) No deviation
d) Forms solid solution
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4. For a binary solution with components A and B showing positive
deviation, the A-B interaction is:
a) Stronger than A-A and B-B
b) Weaker than A-A and B-B
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c) Equal to A-A and B-B
d) Cannot be determined
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5. Which type of solution exhibits minimum boiling azeotrope?
a) Positive deviation from Raoult’s law
b) Negative deviation
c) Ideal
d) Solid solution
6. In an ideal solution:
a) ΔHmix = 0
b) ΔVmix = 0
c) Raoult’s law is obeyed over entire composition range
d) All of the above
7. If a binary solution is non-ideal with negative deviation, its total
vapour pressure is:
a) Greater than predicted
b) Equal to ideal solution
c) Less than predicted
d) Can’t say
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8. Vapour pressure of pure benzene is 100 mmHg and that of pure
toluene is 50 mmHg. In a solution containing 0.5 mole fraction of
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each, the total pressure is:
a) 75 mmHg
b) 60 mmHg
c) 50 mmHg
d) 100 mmHg R
9. A system showing ΔHmix ≠ 0 and ΔVmix ≠ 0 behaves:
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a) Ideally
b) Non-ideally
c) Cannot be determined
d) Like a gas
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10. Which of the following pairs is most likely to show ideal solution
behaviour?
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a) Acetone and Chloroform
b) HCl and Water
c) n-Hexane and n-Heptane
d) Water and Glycerol
11. A solution is formed by mixing 2 moles of ethanol with 1 mole of
methanol. Identify the solvent:
a) Ethanol
b) Methanol
c) Both
d) None
12. Which parameter is not affected in ideal solution formation?
a) Enthalpy
b) Entropy
c) Volume
d) Pressure
13. For an ideal solution, the graph of total vapour pressure vs mole
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fraction is:
a) Linear
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b) Parabolic
c) Exponential
d) No relation
a) Nature of solute
b) Nature of solvent
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14. In solutions, colligative properties depend on:
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c) Number of solute particles
d) Temperature only
15. Which statement is false?
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a) Solutions can be solid, liquid or gas
b) Solute is always in lesser quantity
c) Solvent determines the phase of the solution
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d) All binary solutions obey Raoult's law
16. Which of the following pairs shows maximum deviation from
ideality?
a) Acetone-chloroform
b) Benzene-toluene
c) Water-ethanol
d) HCl-water
17. In an ideal binary solution, the component with lower vapour
pressure will:
a) Evaporate more
b) Have lower partial pressure
c) Have greater mole fraction in vapour phase
d) Show negative deviation
18. What is the effect of temperature on the ideality of a solution?
a) Always ideal at high T
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b) Always non-ideal at low T
c) No effect
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d) Depends on components
19. A maximum boiling azeotrope occurs due to:
a) Strong intermolecular forces
b) Weak interactions
c) Equal vapour pressure
d) No boiling point
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20. The enthalpy change (ΔHmix) for an ideal solution is:
a) Zero
b) Positive
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c) Negative
d) Variable
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21. Which of the following expressions does not represent a valid
concentration unit?
a) mol/L
b) mol/kg
c) g/mole
d) g/L
22. Molarity of a solution depends on:
a) Temperature
b) Mass
c) Volume
d) Both a and c
23. Which unit is independent of temperature?
a) Molarity
b) Molality
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c) Normality
d) Volume percent
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24. A solution contains 2 moles of solute in 500 mL of solution. What
is its molarity?
a) 0.25 M
b) 1 M
c) 2 M
d) 4 M
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25. If 0.5 mole of NaCl is dissolved in 100 g of water, the molality is:
a) 5 m
b) 0.5 m
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c) 50 m
d) 2 m
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26. Which of the following is a colligative property?
a) Osmotic pressure
b) Molarity
c) Density
d) Conductivity
27. If 5.85 g of NaCl is dissolved in 1 L of water, what is the molarity?
(Na = 23, Cl = 35.5)
a) 0.5 M
b) 1 M
c) 0.1 M
d) 2 M
28. The mole fraction of a solute in a solution is 0.2. What is the mole
fraction of solvent?
a) 0.2
b) 0.8
c) 1
d) Cannot be determined
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29. Which statement about molality is true?
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a) Depends on volume
b) Changes with temperature
c) Independent of temperature
d) Always less than molarity
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30. For a dilute aqueous solution, molality and molarity are:
a) Always equal
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b) Approximately equal
c) Molarity > Molality
d) Molality > Molarity
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31. A 1 molal solution means:
a) 1 mol solute/1 L solvent
b) 1 mol solute/1 kg solvent
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c) 1 mol solute/1 L solution
d) 1 mol solute/100 g solvent
32. What is the normality of a 1 M H2SO4 solution?
a) 1 N
b) 2 N
c) 0.5 N
d) 0.1 N
33. Which of the following is a dimensionless quantity?
a) Molarity
b) Molality
c) Mole fraction
d) Normality
34. A solution has mole fraction of ethanol 0.4. What is the mole
fraction of water?
a) 0.6
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b) 0.4
c) 1.0
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d) 0.2
35. A 10% (w/v) solution of NaOH contains:
a) 10 g in 100 mL solution
b) 10 g in 1 L solution
c) 10 mL in 100 g solution
d) 10 mol in 1 L solution
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36. Density of a solution is 1.2 g/mL and its molarity is 2 M. The
molality is approximately:
a) 1.5 m
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b) 2.5 m
c) 3 m
d) 1.67 m
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37. What is the concentration of a solution with 0.2 moles of solute in 2
L of solution?
a) 0.1 M
b) 0.2 M
c) 2 M
d) 0.05 M
38. If 1 mole of KCl is dissolved in 1 kg of water, molality is:
a) 1 m
b) 2 m
c) 0.5 m
d) 4 m
39. Molarity and molality become equal when:
a) Density = 1 and solution is dilute
b) Temperature = 25°C
c) At high concentrations
d) Always equal
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40. Which of the following gives maximum concentration for the same
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solute?
a) Molarity
b) Molality
c) Mole fraction
d) Normality R
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41. Solubility of gases in liquids decreases with:
a) Increase in pressure
b) Decrease in temperature
c) Increase in temperature
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d) Increase in solute size
42. Which of the following solids is most likely to be more soluble in
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hot water?
a) NaCl
b) AgCl
c) KNO₃
d) PbS
43. Which does not affect solubility of a solid in a liquid?
a) Temperature
b) Pressure
c) Nature of solute
d) Nature of solvent
44. For most gases, solubility in water increases with:
a) Increasing volume
b) Decreasing temperature
c) Increasing temperature
d) Decreasing pressure
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45. Which of the following statements is false?
a) Solubility of NaCl in water is due to ion-dipole interaction
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b) Solubility of gases is governed by Henry’s law
c) Solubility of organic compounds always increases with pressure
d) Solubility of solids may increase or decrease with temperature
proportions?
a) Water and ethanol
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46. Which of the following pairs is completely miscible in all
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b) Water and chloroform
c) Water and benzene
d) Acetone and oil
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47. The term ‘saturated solution’ means:
a) A solution with no solute
b) A solution where no more solute can be added at given conditions
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c) A supersaturated solution
d) A dilute solution
48. What happens to the solubility of a gas if the pressure is halved?
a) Doubles
b) Halves
c) Becomes zero
d) No effect
49. Which gas is least soluble in water at room temperature?
a) O₂
b) CO₂
c) NH₃
d) H₂
50. At equilibrium, in a saturated solution of a salt:
a) All salt is undissolved
b) Solute and solvent are in different phases
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c) Rate of dissolution = rate of crystallisation
d) Solubility = 0
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51. Which one is likely to decrease solubility of a salt?
a) Increase in temperature (for endothermic dissolution)
b) Common ion effect
c) Use of hot solvent
d) Agitation
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52. A solute is sparingly soluble in water. Which technique can
improve solubility?
a) Adding inert gas
b) Increasing pressure
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c) Adding common ion
d) Removing water
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53. Solubility product (Ksp) is applicable to:
a) Soluble salts
b) Saturated solutions of sparingly soluble salts
c) Super-saturated solutions
d) All ionic compounds
54. Which compound will precipitate first from a saturated solution?
a) Compound with highest Ksp
b) Compound with lowest Ksp
c) Compound with highest molar mass
d) Compound with highest solubility
55. Solubility of a solid increases with temperature when dissolution is:
a) Endothermic
b) Exothermic
c) Non-spontaneous
d) Reversible
56. Which of the following increases solubility of a solid solute?
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a) High pressure
b) Lower temperature
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c) Greater surface area of solute
d) All of these
57. The solubility of CO₂ in soft drinks is due to:
a) High temperature
b) High pressure
c) pH of solution
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d) Addition of sugar
58. Which substance has maximum solubility in water?
a) NaCl
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b) KCl
c) BaSO₄
d) AgCl
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59. Which of the following forms an unsaturated solution when added
to water?
a) Excess NaCl
b) 2 g of sugar in 1 L water
c) Saturated salt solution
d) 5 g of PbCl₂
60. The van’t Hoff factor for a solute undergoing complete dissociation
is:
a) 1
b) 0
c) >1
61. According to Henry’s law, the solubility of a gas in a liquid is
directly proportional to:
a) Temperature
b) Pressure of the gas
c) Volume of the liquid
d) Mass of the solvent
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62. Henry’s constant for a gas is high. This implies:
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a) Gas is highly soluble
b) Gas is less soluble
c) Gas is very reactive
d) None of these
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63. Which of the following does not affect gas solubility according to
Henry’s law?
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a) Pressure
b) Temperature
c) Nature of solute
d) Henry’s constant
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64. Henry’s law is used in soft drink packaging to:
a) Reduce calories
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b) Increase taste
c) Maintain high CO₂ concentration
d) Enhance sweetness
65. Which gas shows minimum solubility in water?
a) NH₃
b) CO₂
c) O₂
d) H₂
66. Which statement is incorrect regarding Henry’s law?
a) It is valid for ideal solutions only
b) Solubility ∝ partial pressure
c) Solubility increases with temperature
d) It is applicable for gases in liquids
67. The best condition for high gas solubility is:
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a) High temperature, high pressure
b) Low temperature, high pressure
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c) High temperature, low pressure
d) Low temperature, low pressure
68. Which of the following is not an application of Henry’s law?
a) Carbonated beverages
b) Scuba diving
c) Airplane cabin pressure
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d) Acid-base titration
69. Solubility of O₂ in blood increases under high pressure. This is
used in:
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a) Oxygen therapy
b) Hyperbaric treatment
c) Soda preparation
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d) Combustion process
70. Which factor is not considered in Henry’s law equation?
a) Gas solubility
b) Temperature
c) Pressure
d) Volume of solvent
71. When a sealed bottle of soda is opened, bubbles appear because:
a) Temperature increases suddenly
b) Henry’s constant changes
c) Pressure is suddenly decreased
d) Liquid volume decreases
72. In scuba diving, excessive dissolved nitrogen can cause:
a) Carbon poisoning
b) Oxygen toxicity
c) Decompression sickness
d) Hypoxia
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73. The units of Henry’s constant for gas solubility are:
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a) atm
b) mol/L·atm
c) atm/mol·L
d) None of these
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74. Which gas does not obey Henry’s law well?
a) H₂
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b) NH₃
c) CO₂
d) N₂
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75. The pressure required to dissolve 0.5 mol of gas in 1 L of solution
with KH=0.25 extmol/L⋅atmK_H = 0.25 \, ext{mol/L·atm} is:
a) 1.25 atm
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b) 2 atm
c) 0.5 atm
d) 0.25 atm
76. Henry’s law constant for oxygen increases with:
a) Increase in solubility
b) Decrease in pressure
c) Increase in temperature
d) Decrease in temperature
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