Questions About Colligative Properties
Multiple-Choice Questions — Colligative Properties
1. What are colligative properties dependent upon?
A) Chemical nature of the solute
B) Volume of solvent
C) Number of solute particles
D) Color of solute
E) Pressure of the atmosphere
2. Which of the following is not a colligative property?
A) Boiling point elevation
B) Freezing point depression
C) Vapor pressure lowering
D) Density of the solution
E) Osmotic pressure
3. Colligative properties are influenced by:
A) Shape of solute particles
B) Molecular weight of solvent
C) Number of solute particles in solution
D) Type of container
E) Color of the solution
4. Which of the following best defines a colligative property?
A) Depends on type of solute
B) Depends on amount (number) of solute particles
C) Only occurs in non-aqueous solutions
D) Requires electrolytes
E) Is influenced by temperature only
5. The addition of a non-volatile solute to a solvent results in:
A) Increase in vapor pressure
B) Increase in freezing point
C) Increase in boiling point
D) Decrease in solute concentration
E) No change in properties
6. Vapor pressure lowering occurs because:
A) Solute particles increase temperature
B) Solute particles reduce solvent molecules at the surface
C) Solute increases evaporation
D) Solute adds pressure
E) Solvent density increases
7. Boiling point elevation means:
A) The solvent boils at a lower temperature
B) The vapor pressure decreases to zero
C) The boiling point increases due to solute addition
D) The solute evaporates first
E) The solution freezes faster
8. Freezing point depression occurs because:
A) Solute heats the solution
B) Solute particles block ice formation
C) Solvent becomes more viscous
D) Vapor pressure increases
E) Solute reduces atmospheric pressure
9. What is osmotic pressure?
A) The pressure that prevents freezing
B) Pressure applied to evaporate solvent
C) Pressure needed to stop osmosis across a semipermeable membrane
D) Pressure that increases boiling point
E) Pressure due to gas molecules
10. The unit for osmotic pressure is typically:
A) °C
B) atm
C) mol
D) m³
E) kg/mol
11. Which solution will exhibit the greatest colligative effect?
A) 1 m NaCl
B) 1 m glucose
C) 1 m urea
D) 1 m MgCl₂
E) 1 m CH₃OH
12. Which of the following properties will increase when a solute is added to a solvent?
A) Freezing point
B) Vapor pressure
C) Boiling point
D) Solvent volume
E) None of the above
13. Colligative properties depend on:
A) Solute mass
B) Solute molarity
C) Number of dissolved particles (ions or molecules)
D) Solvent polarity
E) Molecular structure
14. Which solution would have the lowest vapor pressure?
A) Pure water
B) 0.1 m NaCl
C) 0.1 m glucose
D) 0.2 m glucose
E) 0.1 m ethanol
15. The freezing point depression constant (Kf) depends on:
A) The solute
B) The solvent
C) The container
D) The gas pressure
E) None of the above
16. A solution that contains a solute that dissociates will have:
A) No effect on colligative properties
B) The same freezing point as the pure solvent
C) Greater colligative effects than a non-electrolyte at the same concentration
D) No boiling point change
E) Lower osmotic pressure
17. Colligative properties are useful in determining:
A) Solvent polarity
B) Molar mass of solutes
C) Solute color
D) Reaction rate
E) Specific heat
18. Which solution would cause the greatest boiling point elevation?
A) 0.1 m NaCl
B) 0.1 m glucose
C) 0.1 m MgCl₂
D) 0.1 m CH₃OH
E) 0.1 m sucrose
19. Which colligative property is most useful for studying cell membranes?
A) Freezing point depression
B) Vapor pressure lowering
C) Osmotic pressure
D) Boiling point elevation
E) Refractive index
20. Colligative properties apply only when:
A) Solute is volatile
B) Solution is saturated
C) Solute is non-volatile and dissolved
D) Temperature is below 0°C
E) Gases are involved
Answer Key with Explanations
1. C – Colligative properties depend on the number of solute particles, not their identity.
2. D – Density is a physical property but not a colligative one.
3. C – Number of solute particles influences colligative effects.
4. B – They depend solely on quantity, not type, of solute particles.
5. C – Boiling point increases because solute lowers vapor pressure.
6. B – Solute particles occupy space at the surface, reducing evaporation.
7. C – The boiling point is raised when solute is added to a solvent.
8. B – Solute disrupts solid lattice formation needed for freezing.
9. C – Osmotic pressure is the pressure needed to stop osmosis.
10. B – It’s usually measured in atmospheres (atm).
11. D – MgCl₂ dissociates into 3 ions, giving stronger effect.
12. C – Only boiling point increases; others decrease.
13. C – The total number of particles (ions or molecules) is what matters.
14. D – 0.2 m glucose has more particles than the other options.
15. B – Kf is a constant for the solvent, not solute.
16. C – Ionic compounds like NaCl dissociate, increasing particle count.
17. B – Used to determine molar mass by freezing point depression.
18. C – MgCl₂ dissociates into 3 particles, increasing boiling point more.
19. C – Osmotic pressure is crucial in understanding cell membrane transport.
20. C – Must be non-volatile solute and properly dissolved in solvent.
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