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Solutions (NEET) — MCQs & Practice

Practice the Solutions chapter for NEET with solved MCQs, formula sheets, stepwise explanations and ChemNexa mock tests for quick revision.

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Solutions Revision Guide for NEET Chemistry

Solutions deals with concentration terms, vapour pressure and colligative properties. Many exam questions are short numericals where correct units and interpretation are more important than lengthy calculation.

For NEET Chemistry, revise mole fraction, molarity, molality, Raoult law, ideal and non-ideal behaviour, elevation of boiling point, depression of freezing point and osmotic pressure.

Important Topics

  • Concentration terms
  • Raoult law
  • Ideal and non-ideal solutions
  • Colligative properties
  • van’t Hoff factor
  • Osmotic pressure

Important Formulae & Relationships

  • Molarity M = moles of solute / volume of solution (L)
  • Molality m = moles of solute / mass of solvent (kg)
  • ΔTb = iKb m
  • ΔTf = iKf m
  • π = iCRT

Use formulas only after checking the required units, sign convention and assumptions for the question.

What to practise in Solutions

Concept Revision

Revise definitions, principles, equations, trends and core ideas from Solutions before attempting MCQs.

Exam-style MCQs

Use chapter-focused multiple-choice practice to improve accuracy, recall and application for NEET Chemistry.

Performance Practice

Attempt ChemNexa tests, review results and return to weak areas for another round of targeted revision.

Top 20 Solutions MCQs with Answers

These public questions are selected from the exact Solutions chapter, screened for topic relevance and deduplicated so repeated versions of the same MCQ are not shown publicly. Use them for quick revision, then sign in to attempt the complete test experience with more questions, results and performance review.

NEET Chemistry · Solutions · Very Hard

1. Raoult's law for a volatile component A is:

  • A. pA = pA°/xA
  • B. pA = xB pA°
  • C. pA = pA° − xA
  • D. pA = xA pA°
Answer: D
Explanation: The partial vapour pressure of component A equals its mole fraction in solution multiplied by vapour pressure of pure A.

NEET Chemistry · Solutions · Very Hard

2. Consider the statements: (I) Osmotic pressure is useful for determining molar masses of macromolecules. (II) Molality is temperature-independent. (III) Positive deviation means stronger A–B interactions. (IV) Colligative properties depend on particle number. Which are correct?

  • A. I, II, III and IV
  • B. I, II and IV only
  • C. I and III only
  • D. II and III only
Answer: B
Explanation: I, II and IV are correct. Positive deviation results from weaker, not stronger, A–B interactions.

NEET Chemistry · Solutions · Very Hard

3. The total vapour pressure of an ideal binary volatile solution is:

  • A. pA°pB°
  • B. xA pA° + xB pB°
  • C. pA° + pB°
  • D. xA + xB
Answer: B
Explanation: Dalton's law and Raoult's law give Ptotal = pA + pB = xA pA° + xB pB°.

NEET Chemistry · Solutions · Very Hard

4. A solution shows positive deviation from Raoult's law when:

  • A. A–B attractions are stronger
  • B. ΔHmix is highly negative
  • C. Vapour pressure is lower than ideal
  • D. A–B attractions are weaker than A–A and B–B attractions
Answer: D
Explanation: Weaker unlike interactions allow molecules to escape more readily, raising vapour pressure above the ideal value.

NEET Chemistry · Solutions · Very Hard

5. A solution showing negative deviation from Raoult's law generally has:

  • A. Higher vapour pressure than ideal
  • B. Stronger A–B interactions
  • C. Weaker A–B interactions
  • D. Positive ΔHmix only
Answer: B
Explanation: Stronger unlike interactions reduce escaping tendency, giving lower vapour pressure and negative deviation.

NEET Chemistry · Solutions · Very Hard

6. A minimum-boiling azeotrope is generally formed by solutions showing:

  • A. Only nonvolatile solutes
  • B. Positive deviation from Raoult's law
  • C. Negative deviation
  • D. No deviation
Answer: B
Explanation: Positive deviation raises vapour pressure and lowers boiling point, producing a minimum-boiling azeotrope.

NEET Chemistry · Solutions · Very Hard

7. A maximum-boiling azeotrope is generally formed by solutions showing:

  • A. Positive deviation
  • B. Ideal behaviour
  • C. Complete immiscibility
  • D. Negative deviation from Raoult's law
Answer: D
Explanation: Negative deviation lowers vapour pressure and raises boiling point, producing a maximum-boiling azeotrope.

NEET Chemistry · Solutions · Very Hard

8. Elevation in boiling point is given by:

  • A. ΔTb = Kf m
  • B. ΔTb = m/Kb
  • C. ΔTb = Kb/M
  • D. ΔTb = Kb m
Answer: D
Explanation: For dilute solutions, boiling-point elevation equals ebullioscopic constant times molality.

NEET Chemistry · Solutions · Very Hard

9. Depression in freezing point is given by:

  • A. ΔTf = m/Kf
  • B. ΔTf = Kf m
  • C. ΔTf = Kb m
  • D. ΔTf = Kf/M
Answer: B
Explanation: For dilute solutions, freezing-point depression equals cryoscopic constant times molality.

NEET Chemistry · Solutions · Very Hard

10. Reverse osmosis occurs when external pressure applied on the solution side is:

  • A. Zero
  • B. Greater than osmotic pressure
  • C. Less than osmotic pressure
  • D. Equal to vapour pressure only
Answer: B
Explanation: Applying pressure greater than osmotic pressure forces solvent from solution through the semipermeable membrane toward pure solvent.

NEET Chemistry · Solutions · Very Hard

11. A solution contains 0.5 mol solute and 2.0 kg solvent. Its molality is:

  • A. 1.0 m
  • B. 2.5 m
  • C. 4.0 m
  • D. 0.25 m
Answer: D
Explanation: Molality = moles of solute / kilograms of solvent = 0.5/2.0 = 0.25 m.

NEET Chemistry · Solutions · Very Hard

12. The mole fraction of a component in a binary solution is:

  • A. Mass divided by solution volume
  • B. Moles of that component divided by total moles
  • C. Mass of that component divided by total mass
  • D. Moles divided by solvent mass in kg
Answer: B
Explanation: Mole fraction is defined as the ratio of moles of one component to total moles of all components.

NEET Chemistry · Solutions · Very Hard

13. For an ideal solution, the enthalpy of mixing is:

  • A. Positive
  • B. Negative
  • C. Infinite
  • D. Zero
Answer: D
Explanation: In an ideal solution, A–B interactions are comparable to A–A and B–B interactions, so ΔHmix = 0.

NEET Chemistry · Solutions · Very Hard

14. For an ideal solution, the volume change on mixing is:

  • A. Equal to molar volume
  • B. Zero
  • C. Positive
  • D. Negative
Answer: B
Explanation: Ideal solutions obey ΔVmix = 0 because intermolecular packing is not significantly altered on mixing.

NEET Chemistry · Solutions · Very Hard

15. Henry's law is commonly written as:

  • A. p = x + KH
  • B. p = KH x
  • C. p = x/KH
  • D. p = KH/x
Answer: B
Explanation: Henry's law states that the partial pressure of a gas is proportional to its mole fraction in solution: p = KHx.

NEET Chemistry · Solutions · Very Hard

16. The relative lowering of vapour pressure for a dilute solution of a nonvolatile solute equals approximately:

  • A. Molarity
  • B. Mole fraction of solute
  • C. Mole fraction of solvent
  • D. Molality
Answer: B
Explanation: For dilute solutions, (p°−p)/p° = xsolute.

NEET Chemistry · Solutions · Very Hard

17. The osmotic pressure of a dilute solution is:

  • A. π = C/RT
  • B. π = RT/C
  • C. π = Kf m
  • D. π = CRT
Answer: D
Explanation: The van't Hoff equation for dilute solutions is π = CRT.

NEET Chemistry · Solutions · Very Hard

18. The van't Hoff factor i is greater than one when the solute:

  • A. Associates
  • B. Does not change particle count
  • C. Is nonvolatile only
  • D. Dissociates
Answer: D
Explanation: Dissociation increases the number of solute particles, so observed colligative effect and i exceed one.

NEET Chemistry · Solutions · Very Hard

19. For complete dissociation of CaCl2 in a very dilute solution, the ideal van't Hoff factor is:

  • A. 2
  • B. 1
  • C. 4
  • D. 3
Answer: D
Explanation: CaCl2 gives one Ca2+ and two Cl− ions, producing three particles per formula unit.

NEET Chemistry · Solutions · Very Hard

20. Which concentration term is independent of temperature?

  • A. Volume percentage
  • B. Molality
  • C. Molarity
  • D. Normality
Answer: B
Explanation: Molality depends on moles of solute per kilogram of solvent, both mass-based quantities, so it is independent of temperature.

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Solutions Practice Tests

Solutions Frequently Asked Questions

Which concentration unit is temperature independent?

Molality is based on mass of solvent and therefore does not change with temperature, unlike molarity which depends on solution volume.

Why is the van’t Hoff factor used?

It accounts for association or dissociation of solute particles so that observed colligative properties can be related to the effective number of dissolved particles.

How can I improve accuracy in Solutions numericals?

Convert masses, volumes and molecular masses carefully, write the chosen concentration unit explicitly and check whether association or dissociation affects the particle count.

Continue with another chapter to build connected concepts and strengthen your overall Chemistry preparation.

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