SaitechAI – Solutions MCQ Quiz (30 Questions)

Test Timings:
Start Time: –
End Time: –
Duration: – minutes

Marking Scheme: 30 questions, 4 options each.
Correct answer: +1 mark | Wrong answer: −0.25 mark | Not attempted: 0 mark.

MCQ – Solutions

Q1. Moles of solute per kilogram of solvent is called:

Molarity Molality Mole fraction Normality

Q2. Which concentration unit is temperature independent?

Molarity Normality Molality Volume percentage

Q3. Mole fraction of component A (X_A) in a binary solution is defined as:

n_A / (n_A + n_B) n_B / (n_A + n_B) n_A / n_B n_B / n_A

Q4. Which of the following is an example of an ideal solution?

Ethanol + water Acetone + chloroform Benzene + toluene HCl + water

Q5. Henry’s law relates:

Vapour pressure and temperature Vapour pressure and mole fraction of solvent Partial pressure of gas and its mole fraction in solution Boiling point and pressure

Q6. In an ideal solution, ΔH_mix and ΔV_mix are respectively:

Zero and zero Positive and positive Negative and zero Positive and negative

Q7. The vapour pressure of each component in an ideal binary solution obeys:

Henry’s law Raoult’s law Dalton’s law Boyle’s law

Q8. For a non-volatile solute, the relative lowering of vapour pressure Δp/p° equals:

Mole fraction of solvent Mole fraction of solute Molality of solution Molarity of solution

Q9. A positive deviation from Raoult’s law is shown when:

A–B interactions are stronger than A–A and B–B A–B interactions are weaker than A–A and B–B Solution forms a maximum boiling azeotrope ΔH_mix = 0

Q10. A solution showing negative deviation from Raoult’s law usually has:

Higher vapour pressure than ideal Lower boiling point than ideal Strong solute–solvent interactions No solute–solvent interactions

Q11. Azeotropes are mixtures which:

Can be separated by simple distillation Boil at constant temperature and composition Show no vapour pressure Always obey Henry’s law

Q12. Which one is a minimum-boiling azeotrope?

HCl–water Ethanol–water Nitric acid–water None of these

Q13. Colligative properties depend on:

Nature of solute only Nature of solvent only Number of solute particles present Volume of solvent only

Q14. Which of the following is not a colligative property?

Relative lowering of vapour pressure Elevation in boiling point Heat of vaporisation Depression in freezing point

Q15. Elevation in boiling point ΔT_b is directly proportional to:

Molarity Mole fraction of solute Molality Density

Q16. The relation for depression in freezing point is:

ΔT_f = K_f · M ΔT_f = K_f · m ΔT_f = K_b · m ΔT_f = K_b · M

Q17. Osmotic pressure Π of a dilute solution is given by:

Π = CRT Π = C/RT Π = RT/C Π = kT/C

Q18. The unit of osmotic pressure, when C is in mol L⁻¹ and R in L atm K⁻¹ mol⁻¹, is:

kPa J mol⁻¹ atm K

Q19. van’t Hoff factor (i) is defined as the ratio of:

Calculated colligative property to observed Observed colligative property to calculated Observed vapour pressure to ideal vapour pressure Calculated vapour pressure to observed

Q20. For NaCl in water (complete dissociation), theoretical van’t Hoff factor is:

1 2 3 4

Q21. Depression in freezing point of 0.1 m glucose is 0.186 K. For 0.1 m KCl (complete dissociation), ΔT_f will be approximately:

0.093 K 0.186 K 0.372 K 0.558 K

Q22. A 0.1 M solution of a non-electrolyte has osmotic pressure 2.46 atm at 300 K. A 0.1 M electrolyte solution (same T) shows 4.92 atm. van’t Hoff factor is:

0.5 1.0 2.0 4.0

Q23. A solution whose vapour pressure is greater than that predicted by Raoult’s law will form:

Minimum-boiling azeotrope Maximum-boiling azeotrope No azeotrope Ideal solution

Q24. For gas solubility in a liquid, increase in temperature generally:

Increases solubility Decreases solubility Has no effect First increases then decreases

Q25. Solubility of a gas in a liquid at constant temperature is directly proportional to:

Square of pressure Reciprocal of pressure Pressure (for dilute solutions) Temperature

Q26. Freezing point of pure water is 273 K. If ΔT_f = 0.372 K, the freezing point of solution is:

272.628 K 273.372 K 272.000 K 274.000 K

Q27. Which colligative property is most suitable for determining molar mass of macromolecules (polymers, proteins)?

Relative lowering of vapour pressure Elevation in boiling point Depression in freezing point Osmotic pressure

Q28. When a solute associates in solution to form dimers, the van’t Hoff factor will be:

Greater than 1 Equal to 1 Less than 1 Infinite

Q29. If a solution has higher boiling point than pure solvent, then:

Vapour pressure is higher than pure solvent Vapour pressure is lower than pure solvent Vapour pressure is same as pure solvent No conclusion about vapour pressure

Q30. The main reason for adding ethylene glycol to car radiators is:

To increase vapour pressure of water To decrease boiling point of water To lower freezing point and raise boiling point of coolant To increase colour intensity of water

Result Summary
Total Questions: 30
Correct Answers: 0
Wrong Answers: 0
Unattempted: 0
Final Score: 0 / 30
Time Taken: 0 minutes
Marks per Minute: 0

SaitechAI – 30 MCQ Quiz
Chapter: Solutions (Class 12)

Student Details

MCQ – Solutions

SaitechAI – 30 MCQ QuizChapter: Solutions (Class 12)

Student Details

MCQ – Solutions

SaitechAI – 30 MCQ Quiz
Chapter: Solutions (Class 12)