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Solutions JENPAS MCQ & Practice Questions

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Solutions Revision Guide for JENPAS 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 JENPAS 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

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Top 20 Solutions MCQs with Answers

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JENPAS Chemistry · Solutions · Very Very Hard

1. Negative deviation from Raoult's law occurs when A-B attractions are:

  • A. Weaker
  • B. Absent
  • C. Always metallic
  • D. Stronger than A-A and B-B attractions
Answer: D
Explanation: Stronger unlike interactions reduce vapour pressure.

JENPAS Chemistry · Solutions · Very Very Hard

2. JENPAS advanced: Negative deviation from Raoult's law occurs when A-B attractions are:

  • A. Always metallic
  • B. Stronger than A-A and B-B attractions
  • C. Weaker
  • D. Absent
Answer: B
Explanation: Apply the underlying principle carefully. Stronger unlike interactions reduce vapour pressure.

JENPAS Chemistry · Solutions · Very Very Hard

3. Solution-chemistry reasoning: Negative deviation from Raoult's law occurs when A-B attractions are:

  • A. Weaker
  • B. Absent
  • C. Always metallic
  • D. Stronger than A-A and B-B attractions
Answer: D
Explanation: Use the relevant solution-law relationship. Stronger unlike interactions reduce vapour pressure.

JENPAS Chemistry · Solutions · Very Very Hard

4. Positive deviation from Raoult's law occurs when A-B attractions are:

  • A. Ionic only
  • B. Weaker than A-A and B-B attractions
  • C. Much stronger
  • D. Exactly identical always
Answer: B
Explanation: Weaker unlike interactions allow molecules to escape more readily.

JENPAS Chemistry · Solutions · Very Very Hard

5. A solution showing positive deviation has vapour pressure:

  • A. Higher than ideal prediction
  • B. Lower than ideal prediction
  • C. Always zero
  • D. Independent of composition
Answer: A
Explanation: Weaker A-B attraction increases escaping tendency.

JENPAS Chemistry · Solutions · Very Very Hard

6. Relative lowering of vapour pressure for a dilute nonvolatile solute is equal approximately to:

  • A. Mole fraction of solute
  • B. Mole fraction of solvent
  • C. Molarity
  • D. Molality squared
Answer: A
Explanation: Raoult's law gives (p°-p)/p°=xsolute for dilute solutions.

JENPAS Chemistry · Solutions · Very Very Hard

7. Consider: (I) molality is temperature independent; (II) positive deviation gives higher vapour pressure; (III) dissociation generally gives i>1; (IV) reverse osmosis needs pressure greater than osmotic pressure. Which are correct?

  • A. I, III and IV only
  • B. I, II, III and IV
  • C. I and II only
  • D. II and III only
Answer: B
Explanation: All four statements are correct.

JENPAS Chemistry · Solutions · Very Very Hard

8. JENPAS advanced: Positive deviation from Raoult's law occurs when A-B attractions are:

  • A. Much stronger
  • B. Exactly identical always
  • C. Ionic only
  • D. Weaker than A-A and B-B attractions
Answer: D
Explanation: Apply the underlying principle carefully. Weaker unlike interactions allow molecules to escape more readily.

JENPAS Chemistry · Solutions · Very Very Hard

9. JENPAS advanced: A solution showing positive deviation has vapour pressure:

  • A. Always zero
  • B. Independent of composition
  • C. Higher than ideal prediction
  • D. Lower than ideal prediction
Answer: C
Explanation: Apply the underlying principle carefully. Weaker A-B attraction increases escaping tendency.

JENPAS Chemistry · Solutions · Very Very Hard

10. JENPAS advanced: Relative lowering of vapour pressure for a dilute nonvolatile solute is equal approximately to:

  • A. Molarity
  • B. Molality squared
  • C. Mole fraction of solute
  • D. Mole fraction of solvent
Answer: C
Explanation: Apply the underlying principle carefully. Raoult's law gives (p°-p)/p°=xsolute for dilute solutions.

JENPAS Chemistry · Solutions · Very Very Hard

11. JENPAS advanced: Consider: (I) molality is temperature independent; (II) positive deviation gives higher vapour pressure; (III) dissociation generally gives i>1; (IV) reverse osmosis needs pressure greater than osmotic pressure. Which are correct?

  • A. I and II only
  • B. II and III only
  • C. I, III and IV only
  • D. I, II, III and IV
Answer: D
Explanation: Apply the underlying principle carefully. All four statements are correct.

JENPAS Chemistry · Solutions · Very Very Hard

12. Solution-chemistry reasoning: Raoult's law for a volatile component states:

  • A. pi=xi/ pi°
  • B. pi=xi+pi°
  • C. pi=xi pi°
  • D. pi=pi°/xi
Answer: C
Explanation: Use the relevant solution-law relationship. Partial vapour pressure equals liquid mole fraction times pure-component vapour pressure.

JENPAS Chemistry · Solutions · Very Very Hard

13. Solution-chemistry reasoning: Positive deviation from Raoult's law occurs when A-B attractions are:

  • A. Ionic only
  • B. Weaker than A-A and B-B attractions
  • C. Much stronger
  • D. Exactly identical always
Answer: B
Explanation: Use the relevant solution-law relationship. Weaker unlike interactions allow molecules to escape more readily.

JENPAS Chemistry · Solutions · Very Very Hard

14. Solution-chemistry reasoning: A solution showing positive deviation has vapour pressure:

  • A. Higher than ideal prediction
  • B. Lower than ideal prediction
  • C. Always zero
  • D. Independent of composition
Answer: A
Explanation: Use the relevant solution-law relationship. Weaker A-B attraction increases escaping tendency.

JENPAS Chemistry · Solutions · Very Very Hard

15. Raoult's law for a volatile component states:

  • A. pi=xi/ pi°
  • B. pi=xi+pi°
  • C. pi=xi pi°
  • D. pi=pi°/xi
Answer: C
Explanation: Partial vapour pressure equals liquid mole fraction times pure-component vapour pressure.

JENPAS Chemistry · Solutions · Very Very Hard

16. For an ideal binary volatile solution, total vapour pressure equals:

  • A. pA/pB
  • B. pA+pB
  • C. pA-pB
  • D. pA pB
Answer: B
Explanation: Dalton's law gives total pressure as the sum of partial pressures.

JENPAS Chemistry · Solutions · Very Very Hard

17. An ideal solution obeys Raoult's law:

  • A. Over the entire composition range
  • B. Only at infinite dilution
  • C. Only at boiling point
  • D. Never
Answer: A
Explanation: Ideal solutions obey Raoult's law at all compositions.

JENPAS Chemistry · Solutions · Very Very Hard

18. For molar-mass determination of proteins, the most suitable colligative method is often:

  • A. Freezing-point depression only
  • B. Vapour density
  • C. Osmotic pressure
  • D. Boiling-point elevation
Answer: C
Explanation: Osmotic pressure is measurable at room temperature even for very dilute macromolecular solutions.

JENPAS Chemistry · Solutions · Very Very Hard

19. Adding a nonvolatile solute to a solvent generally causes its boiling point to:

  • A. Decrease
  • B. Remain unchanged
  • C. Become zero
  • D. Increase
Answer: D
Explanation: Lower vapour pressure requires a higher temperature to reach atmospheric pressure.

JENPAS Chemistry · Solutions · Very Very Hard

20. JENPAS advanced: Raoult's law for a volatile component states:

  • A. pi=xi pi°
  • B. pi=pi°/xi
  • C. pi=xi/ pi°
  • D. pi=xi+pi°
Answer: A
Explanation: Apply the underlying principle carefully. Partial vapour pressure equals liquid mole fraction times pure-component vapour pressure.

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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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