A 1.00 molar aqueous solution of trichloroacetic acid (CCl₃COOH) is heated to its boiling point. The solution has the boiling point of 100.18⁰C. Determine the van’t Hoff factor for trichloroacetic acid. (K_b for water = 0.512 kg mol^-1)

Define the following terms:

 (i) Mole fraction

(ii) Isotonic solutions

(iii) Van’t Hoff factor

 (iv) Ideal solution

Calculate the amount of KCl which must be added to 1 kg of water so that the freezing point is depressed by 2K. (K_f for water = 1.86 K kg mol^-1)

(a) Differentiate between molarity and molality for a solution. How does a change in temperature influence their values? 

(b) Calculate the freezing point of an aqueous solution containing 10.50 g of MgBr₂in 200 g of water. (Molar mass of MgBr₂ = 184 g) (K_f for water = 1.86 K kg mol^-1) 

(a) Define the terms osmosis and osmotic pressure. Is the osmotic pressure of a solution a colligative property? Explain. 

(b) Calculate the boiling point of a solution prepared by adding 15.00 g of NaCl to 250.0 g of water. (K_b for water = 0.512 K kg mol^-1), (Molar mass of NaCl = 58.44 g)

Why does a solution containing non-volatile solute have higher boiling point than the pure solvent? Why is elevation of boiling point a colligative property?

Calculate the freezing point of the solution when 31 g of ethylene glycol (C₂H₆O₂) is dissolved in 500 g of water. (K_f for water = 1.86 K kg mol^–1)

(a) State Raoult’s law for a solution containing volatile components.

How does Raoult’s law become a special case of Henry’s law?

(b) 1·00 g of a non-electrolyte solute dissolved in 50 g of benzene lowered the freezing point of benzene by 0·40 K. Find the molar mass of the solute. (K_f for benzene = 5·12 K kg mol^-1) 

(a) Define the following terms:

(i) Ideal solution

(ii) Azeotrope

(iii) Osmotic pressure

(b) A solution of glucose (C₆H₁₂O₆) in water is labeled as 10% by weight. What would be the molality of the solution?

(Molar mass of glucose = 180 g mol^-1)

a) Define the following terms:

(i) Mole fraction

(ii) Ideal solution

(b) 15.0 g of an unknown molecular material is dissolved in 450 g of water. The resulting solution freezes at - 0.34°C. What is the molar mass of the material? (K_f for water = 1.86 K kg mol^-1)