If 8 g of a non-electrolyte solute is dissolved in 114 g of n-octane to reduce its vapor pressure to 80 %, the molar mass (in g mol^–1) of the solute is:

[Molar mass of n-octane is 114 g mol^–1]

1.	40	2.	60
3.	80	4.	20

Isotonic solutions have the same:

1. Vapour pressure

2. Freezing temperature

3. Osmotic pressure

4. Boiling temperature

A 0.1 molal aqueous solution of a weak acid (HA) is 30 % ionized. If K_f for water is 1.86 °C/m, the freezing point of the solution will be:

200 mL of an aqueous solution contains 1.26 g of protein. The osmotic pressure of this solution at 300 K is found to be 2.57 × 10^–3 bar. The molar mass of protein will be:

(R = 0.083 L bar mol^–1 K^–1):

The positive deviations from Raoult’s law mean the vapour pressure is:

1. Higher than expected.
2. Lower than expected.
3. As expected.
4. None of the above

The type of inter-molecular interactions present in:

Henry’s law constant for the solution of methane in benzene at 298 K is 4.27 × 10⁵ mm Hg. The mole fraction of methane in benzene at 298 K under 760 mm Hg will be:

1. 1.85 × 10^–5

2. 192 × 10^–4

3. 178 × 10^–5

4. 18.7 × 10^–5

A solution that has the highest boiling point among the following is:

1. 1.0 M NaOH

2. 1.0 M Na₂SO₄ 

3. 1.0 M NH₄NO₃

4. 1.0 M KNO₃

Colligative properties are dependent on which of the following factors?

On dissolving sugar in water at room temperature solution feels cool to touch. Dissolution of sugar will be most rapid under the following case is:

1.  Sugar crystals in cold water
2.  Sugar crystals in hot water
3.  Powdered sugar in cold water
4.  Powdered sugar in hot water