If 5.6 g of KOH is present in
(a) 500 mL and
(b) 1 litre of solution 
Calculate the molarity of each of these solutions.

Describe how would you prepare the following solution from pure solute and solvent
(a) 1 L of aqueous solution of 1.5 M CoCl₂.
(b) 500 mL of 6.0% (V/V) aqueous methanol solution.

Vapour pressure of a pure liquid A is 10.0 torr at 27°C. The vapour pressure is lowered to 9.0 torr on dissolving one gram of B in 20 g of A. If the molar mass of A is 200 then calculate the molar mass of B.

An aqueous solution of 2% nonvolatile solute exerts a pressure of 1.004 bar at the boiling point of the solvent. What is the molar mass of the solute when P_A is 1.013 bar ?

Ethylene glycol (C₂H₆O₂) can be at used as an antifreeze in the radiator of a car. Calculate the temperature when ice will begin to separate from a mixture with 20 mass percent of glycol in water used in the car radiator. K_f for water = 1.86 K Kg mol^-1 and molar mass of ethylene glycol is 62 g mol^-1.

2g of a non electrolyte solute dissolved in 75 g of benzene lowered the freezing point of benzene by 0.20 K. The freezing point depression constant of benzene is 5.12 K Kg mol^-1. Find the molar mass of the solute.

What is the mass of glucose (C₆ H₁₂O₆) in it one litre solution which is isotonic with 6 g L^-1 of urea (NH₂ CO NH₂) ?

The depression in freezing point is 0.24K obtained by dissolving 1g NaCl in 200g water. Calculate van’t-Hoff factor. The molal depression constant is 1.86 K Kg mol^-1.

0.2 m aqueous solution of KCl freezes at -0.68ºC calculate van’t Hoff factor. k_f for water is 1.86 K kg mol^-1.

The observed depression in freezing point of water for a particular solution is 0.093^o C. Calculate the concentration of the solution in molality. Given that molal depression constant for water is 1.86 K Kg mol^-1.