The Solutions chapter in Class 12 Chemistry is one of the most important and high-scoring units for CBSE Board as well as competitive exams like NEET and JEE. This chapter deals with different types of solutions, concentration terms such as molarity and molality, Raoult’s law, Henry’s law, colligative properties, and abnormal molar mass. Understanding these concepts is essential because many numerical and conceptual questions are directly based on them.
In competitive examinations, questions are frequently asked from topics like osmotic pressure, elevation in boiling point, depression in freezing point, and van’t Hoff factor. These concepts not only test theoretical understanding but also require strong problem-solving skills. Therefore, regular practice of multiple-choice questions (MCQs) helps students improve accuracy and speed.
In this post, we have provided 50 carefully selected MCQs from the Solutions chapter. These questions cover both basic concepts and higher-level applications, making them suitable for Board exams as well as NEET/JEE preparation. Practice all the questions and check the answers to strengthen your preparation and boost your confidence.
Class 12 Chemistry Solutions MCQs (Board + NEET Level)
1. The molarity of a solution depends on:
A. Temperature
B. Nature of solute
C. Pressure
D. Mass of solvent
Answer: A
2. Which concentration term is independent of temperature?
A. Molarity
B. Molality
C. Normality
D. Formality
Answer: B
3. A 1 molal solution contains:
A. 1 mole solute in 1 L solution
B. 1 mole solute in 1 kg solvent
C. 1 mole solute in 1 kg solution
D. 1 mole solute in 1000 mL solvent
Answer: B
4. According to Raoult’s law, vapor pressure of solution is:
A. Greater than pure solvent
B. Equal to pure solvent
C. Directly proportional to mole fraction of solvent
D. Independent of mole fraction
Answer: C
5. Which is a colligative property?
A. Density
B. Surface tension
C. Osmotic pressure
D. Viscosity
Answer: C
6. Osmosis occurs through:
A. Porous membrane
B. Filter paper
C. Semi-permeable membrane
D. Plastic sheet
Answer: C
7. The unit of osmotic pressure is:
A. Kelvin
B. atm
C. mol
D. kg
Answer: B
8. The relation for osmotic pressure is:
A. π = MRT
B. π = nRT
C. π = RT/M
D. π = M/RT
Answer: A
9. Elevation in boiling point depends on:
A. Molarity
B. Molality
C. Density
D. Volume
Answer: B
10. Depression in freezing point depends on:
A. Molality
B. Molarity
C. Normality
D. Volume
Answer: A
11. The van’t Hoff factor for NaCl is ideally:
A. 1
B. 2
C. 3
D. 4
Answer: B
12. The van’t Hoff factor is less than 1 in case of:
A. Dissociation
B. Association
C. Strong electrolyte
D. Complete ionization
Answer: B
13. Which solution shows positive deviation?
A. Benzene + Toluene
B. Acetone + Ethanol
C. NaCl + Water
D. Glucose + Water
Answer: B
14. Ideal solutions obey Raoult’s law at:
A. Low concentration only
B. High concentration only
C. All concentrations
D. Zero concentration
Answer: C
15. Cryoscopic constant is related to:
A. Boiling point
B. Freezing point
C. Osmotic pressure
D. Vapor pressure
Answer: B
16. Ebullioscopic constant is related to:
A. Freezing point
B. Boiling point
C. Osmosis
D. Density
Answer: B
17. Reverse osmosis is used in:
A. Distillation
B. Water purification
C. Sublimation
D. Chromatography
Answer: B
18. Solubility of gases increases with:
A. Increase in temperature
B. Decrease in pressure
C. Increase in pressure
D. No change
Answer: C
19. Henry’s law is applicable to:
A. Solid in liquid
B. Gas in liquid
C. Liquid in liquid
D. Solid in gas
Answer: B
20. Colligative properties depend on:
A. Nature of solute
B. Number of solute particles
C. Nature of solvent
D. Volume
Answer: B
21. Maximum boiling azeotrope shows:
A. Positive deviation
B. Negative deviation
C. Ideal behavior
D. No deviation
Answer: B
22. Minimum boiling azeotrope shows:
A. Negative deviation
B. Positive deviation
C. Ideal solution
D. Immiscible solution
Answer: B
23. Mole fraction lies between:
A. 0 to 10
B. 1 to 10
C. 0 to 1
D. 1 to 100
Answer: C
24. Unit of molarity is:
A. mol/kg
B. mol/L
C. g/L
D. kg/mol
Answer: B
25. Unit of molality is:
A. mol/L
B. mol/kg
C. g/kg
D. kg/mol
Answer: B
26. If i = 1, the solute is:
A. Strong electrolyte
B. Weak electrolyte
C. Non-electrolyte
D. Strong acid
Answer: C
27. Osmotic pressure increases with:
A. Temperature
B. Concentration
C. Both A and B
D. None
Answer: C
28. Freezing point of solution is:
A. Increased
B. Decreased
C. Same
D. Doubled
Answer: B
29. Boiling point of solution is:
A. Decreased
B. Increased
C. Same
D. Zero
Answer: B
30. Ideal solution has:
A. ΔHmix ≠ 0
B. ΔVmix ≠ 0
C. ΔHmix = 0 and ΔVmix = 0
D. High boiling point
Answer: C
31. The expression for lowering of vapor pressure is:
A. ΔP = P°
B. ΔP = P° × X₂
C. ΔP = P° × X₁
D. ΔP = X₁ / P°
Answer: B
32. If the relative lowering of vapor pressure is 0.02, the mole fraction of solute is:
A. 0.98
B. 0.02
C. 1.02
D. 0.50
Answer: B
33. Which of the following is not a colligative property?
A. Osmotic pressure
B. Elevation in boiling point
C. Depression in freezing point
D. Surface tension
Answer: D
34. The freezing point depression is given by:
A. ΔTf = Kb m
B. ΔTf = Kf m
C. ΔTf = MRT
D. ΔTf = kH x
Answer: B
35. Elevation in boiling point is given by:
A. ΔTb = Kf m
B. ΔTb = Kb m
C. ΔTb = MRT
D. ΔTb = P°x
Answer: B
36. The van’t Hoff factor (i) is defined as:
A. Normal molar mass / Observed molar mass
B. Observed molar mass / Normal molar mass
C. Moles of solvent / Moles of solute
D. Molality × Temperature
Answer: A
37. If a solute dissociates into 3 ions, the value of i will be:
A. Less than 1
B. Equal to 1
C. Greater than 1
D. Zero
Answer: C
38. Which of the following will have highest freezing point?
A. 0.1 m NaCl
B. 0.1 m CaCl₂
C. 0.1 m Glucose
D. 0.1 m KCl
Answer: C
39. Henry’s law is expressed as:
A. p = kH x
B. π = MRT
C. ΔTb = Kb m
D. ΔTf = Kf m
Answer: A
40. Solubility of gas decreases with:
A. Increase in pressure
B. Decrease in temperature
C. Increase in temperature
D. Increase in mole fraction
Answer: C
41. An ideal solution has:
A. Strong A–B interactions
B. Weak A–B interactions
C. A–A = B–B = A–B interactions
D. Only A–A interactions
Answer: C
42. Osmotic pressure of a dilute solution is proportional to:
A. Mass of solute
B. Volume of solvent
C. Molar concentration
D. Density
Answer: C
43. If two solutions have same osmotic pressure, they are:
A. Hypertonic
B. Hypotonic
C. Isotonic
D. Ideal
Answer: C
44. A solution that causes plant cells to shrink is:
A. Hypotonic
B. Isotonic
C. Hypertonic
D. Ideal
Answer: C
45. For association of molecules, observed molar mass is:
A. Greater than normal
B. Less than normal
C. Equal to normal
D. Zero
Answer: A
46. For dissociation of molecules, observed molar mass is:
A. Greater than normal
B. Less than normal
C. Equal to normal
D. Infinite
Answer: B
47. The unit of Henry’s law constant (kH) is:
A. atm
B. mol/kg
C. Kelvin
D. Joule
Answer: A
48. The main application of osmotic pressure measurement is:
A. Determination of molar mass of macromolecules
B. Measuring density
C. Finding boiling point
D. Measuring viscosity
Answer: A
49. Which solution will show no deviation from Raoult’s law?
A. Ethanol + Water
B. Benzene + Toluene
C. Acetone + Chloroform
D. HCl + Water
Answer: B
50. The boiling point elevation constant (Kb) depends on:
A. Nature of solute
B. Nature of solvent
C. Concentration
D. Temperature only
Answer: B