JEE Main - Colligative properties boiling point elevation freezing point depression osmotic pressure One Line Questions & Answers

1. For a non-electrolyte solute like glucose, the Van't Hoff factor (i) is: — 1

2. If a solution boils at 100.52 °C and the Kb for water is 0.52 K kg mol⁻¹, what is the molality of the non-volatile, non-electrolyte solute? — 0.1 mol kg⁻¹

3. A solution of urea in water freezes at -0.186 °C. If Kf for water is 1.86 K kg mol⁻¹, what is the molality of the solution? — 0.1 mol kg⁻¹

4. What is the osmotic pressure of a 0.1 M NaCl solution at 27°C? (R = 0.0821 L atm mol⁻¹ K⁻¹) — 0.492 atm

5. For a strong electrolyte that dissociates into two ions (e.g., NaCl), the theoretical Van't Hoff factor (i) is: — 2

6. For a strong electrolyte that dissociates into three ions (e.g., CaCl2), the theoretical Van't Hoff factor (i) is: — 3

7. What is a semipermeable membrane? — A membrane that allows only solvent molecules to pass through, but not solute molecules.

8. What is the primary definition of a colligative property? — A property that depends on the concentration of solute particles, irrespective of their identity.

9. A 0.1 molal aqueous solution of a salt that dissociates into three ions will have a freezing point depression: — Approximately three times that of a 0.1 molal glucose solution.

10. Which of the following is NOT a colligative property? — Surface tension

11. Which colligative property is most sensitive to concentration and therefore useful for determining molar masses of very dilute solutions? — Osmotic pressure

12. Which colligative property is typically measured in terms of pressure difference across a semipermeable membrane? — Osmotic pressure

13. Isotonic solutions have: — The same osmotic pressure at the same temperature.

14. The process of solvent molecules moving from a region of higher solvent concentration to a region of lower solvent concentration through a semipermeable membrane is called: — Osmosis

15. In the context of colligative properties, 'non-volatile' means that the solute: — Does not exert a significant vapor pressure at the boiling point of the solvent.

16. The molal boiling point elevation constant (Kb) is also known as: —

17. The molal freezing point depression constant (Kf) is also known as: — Cryoscopic constant

18. The depression in freezing point of a solvent on dissolving a non-volatile solute is called: — Cryoscopy

19. When a solution is placed in contact with pure solvent through a semipermeable membrane, osmosis will occur: — From the solvent to the solution.

20. Which of the following substances is a strong electrolyte? — Hydrochloric acid (HCl)

21. Pure water freezes at 0°C. If a solution of a non-volatile solute is prepared, its freezing point will be: — Lower than 0°C

22. If a solute undergoes association in solution, its observed colligative property will be: — Lower than expected, and 'i' will be less than 1.

23. If a solute undergoes dissociation in solution, its observed colligative property will be: — Higher than expected, and 'i' will be greater than 1.

24. Adding a non-volatile solute to a solvent will generally: — Increase the boiling point and decrease the freezing point

25. Reverse osmosis is a process used for: — Purifying water.

26. Which of the following units is commonly used for Kb? — K kg mol⁻¹

27. Which of the following units is commonly used for Kf? — K kg mol⁻¹

28. A solution with a higher concentration of solute particles will have a: — Higher boiling point and higher osmotic pressure.

29. The elevation in boiling point of a solvent on dissolving a non-volatile solute is called: — Ebullioscopy

30. The formula for boiling point elevation is ΔTb = Kb * m. What does 'm' represent? — Molality of the solution

31. The formula for freezing point depression is ΔTf = Kf * m. What does 'm' represent? — Molality of the solution

32. Which factor directly influences the boiling point elevation of a solution? — Concentration of solute particles

33. Which of the following is an example of a semipermeable membrane? — Cellophane

34. Which of the following substances is a non-electrolyte? — Urea (CO(NH2)2)

35. When 1 mole of NaCl is dissolved in 1 kg of water, the boiling point elevation would be approximately double that of dissolving 1 mole of glucose in 1 kg of water, assuming ideal behavior. This is due to: — The dissociation of NaCl into two ions.

36. For a non-volatile, non-electrolyte solute, the boiling point elevation is directly proportional to: — The molality of the solution

37. For a non-volatile, non-electrolyte solute, the freezing point depression is directly proportional to: — The molality of the solution

38. Osmotic pressure is defined as: — The minimum pressure required to prevent the passage of solvent into the solution through a semipermeable membrane.

39. Osmotic pressure is a colligative property because it depends on: — The concentration of solute particles.

40. The molar mass of a non-volatile solute can be determined using the freezing point depression method if: — The solvent has a high Kf value.

41. The Van't Hoff factor (i) accounts for: — The effect of solute association or dissociation on colligative properties.

42. Which of the following statements about colligative properties is FALSE? — They are independent of the nature of the solvent.

43. What is the relationship between vapor pressure lowering and other colligative properties? — Vapor pressure lowering is directly proportional to boiling point elevation.

44. Which solvent has the highest Kf value, making it suitable for determining molar masses of solutes? — Acetic acid

45. Which of the following solvents is often used to determine the molar mass of organic compounds due to its high Kf value? — Benzene

46. The modified formula for boiling point elevation considering Van't Hoff factor is: — ΔTb = i * Kb * m

47. The modified formula for freezing point depression considering Van't Hoff factor is: — ΔTf = i * Kf * m

48. The modified formula for osmotic pressure considering Van't Hoff factor is: — π = i * M R T

49. The relationship between osmotic pressure (π), molarity (M), gas constant (R), and absolute temperature (T) is given by: — π = M R T

Colligative properties boiling point elevation freezing point depression osmotic pressure - One Line Questions