When 19.5 g of fluoroacetic acid (CH₂FCOOH) is dissolved in 500 g of water, the observed depression in the freezing point was found to be 1.00 K. The Van’t Hoff factor and the dissociation constant of the fluoroacetic acid, respectively are: (Given: \(K_f\) for water = 1.86 K kg mol⁻¹, Molar mass of CH₂FCOOH = 78 g mol⁻¹)

1.	20.75 , 4.77 × 10–3	2.	1.075 ,  4.77 × 10–2
3.	2.073 , 3.07 × 10–4	4.	1.075 , 3.07 × 10–3

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

100 g of liquid A (molar mass 140 g mol^–1) was dissolved in 1000 g of liquid B (molar mass 180 g mol^–1). The vapour pressure of pure liquid B was found to be 500 torr. If the total vapour pressure of the solution is 475 torr, the vapour pressure of pure liquid A will be:

Air consists primarily of nitrogen, which occupies approximately 79% by volume at 298 K under normal conditions. Water is in equilibrium with air at a total pressure of 10 atm and a temperature 298 K. The Henry's law constant for nitrogen in water at 298 K is given as 6.51 × 10⁷ mm Hg.

Determine the mole fraction of dissolved nitrogen in the water under these conditions:

The amount of CaCl₂ (i = 2.47) dissolved in 2.5 litre of water such that its osmotic pressure is 0.75 atm at 27 °C is:

Match the following type of intermolecular interactions present in the pair of compounds given:

The solubility of gases in liquids generally decreases as temperature increases.
The primary reason for this behavior is:

Which law is applied when deep-sea divers use a breathing mixture of oxygen and less soluble helium to minimise the painful effects caused by the increased dissolution of gases in blood at high pressure?

An example of a gas in a solid-type solution is:
1. Solution of hydrogen in palladium
2. Ethanol dissolved in water
3. Camphor vapours in N₂ gas
4. Amalgams