(a) Explain the following:

(i) Henry’s law about the dissolution of a gas in a liquid.

(ii) Boiling point elevation constant for a solvent.

(b) A solution of glycerol (C₃H₈O₃) in water was prepared by dissolving some glycerol in 500 g of water. This solution has a boiling point of 100.42°C. What mass if glycerol was dissolved to make this solution? (K_b for water = 0.512 K kg mol^-1)

a) Calculate the freezing point of the solution when 1.9 g of MgCl₂ (M = 95 g mol⁻¹) was dissolved in 50 g of water, assuming MgCl₂ undergoes complete ionization.
 (K_f for water = 1.86 K kg mol−1)

(b)
(i) Out of 1 M glucose and 2 M glucose, which one has a higher boiling point and why?
(ii) What happens when the external pressure applied becomes more than the osmotic pressure of solution?

OR

(a)When 2.56 g of sulphur was dissolved in 100 g of CS₂, the freezing point lowered by 0.383 K. Calculate the formula of sulphur (Sx).
 
(K_f for CS2 = 3.83 K kg mol−1, Atomic mass of sulphur = 32 g mol⁻¹]

(b)Blood cells are isotonic with 0.9% sodium chloride solution. What happens if we place blood cells in a solution containing
(i)1.2% sodium chloride solution?
(ii)0.4% sodium chloride solution?

(i) Gas (A) is more soluble in water than Gas (B) at the same temperature which one of two gases will the higher value of K_H (Henry's constant) and why ?

(ii)In non-ideal solution, what type of deviation shows the formation of maximum boiling azeotropes?

Calculate the boiling point of the solution when 4g of MgSO₄ (M =120 g mol^-1) was dissolved in 100g of water,assuming MgSO₄ undergoes complete ionization.

(K_b for water =0.52 K kg mol^-1)

What is meant by ‘reverse osmosis’?

Differentiate between molarity and molality values for a solution. What is the effect of change in temperature on molarity and molality values?

267.

A solution prepared by dissolving 8.95 mg of a gene fragment in 35.0 mL of water has an osmotic pressure of 0.335 torr at 25°C.

Assuming that the gene fragment is a non-electrolyte, calculate its molar mass.

(a) Define the following terms :
(i) Molarity
(ii) Molal elevation constant (K_b)

(b) A solution containing 15 g urea (molar mass = 60 g mol^–1) per litre of the solution in water has the same osmotic pressure (isotonic) as a solution of glucose (molar mass = 180 g mol^–1) in water. Calculate the mass of glucose present in one litre of its solution.

OR

(a) What type of deviation is shown by a mixture of ethanol and acetone? Give reason.

(b) A solution of glucose (molar mass = 180 g mol^–1) in water is labelled as 10% (by mass). What would be the molality and molarity of the solution?
(Density of solution = 1.2 g mL^–1)

Define the following terms:
Colligative properties

Define the following terms:
Molality (m)