Colligative Properties of Solutions
Chemistry ⇒ Solutions and Colloids
Colligative Properties of Solutions starts at 11 and continues till grade 12.
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A 0.1 molal solution of a non-electrolyte in benzene lowers the freezing point by 0.512 K. If Kf for benzene is 5.12 K kg mol-1, calculate the molar mass of the solute if 1 g is dissolved in 100 g benzene.
A 0.2 molal solution of a non-electrolyte in water has a freezing point depression of 0.372°C. If Kf for water is 1.86 K kg mol-1, calculate the expected freezing point of the solution.
A 0.2 molal solution of K2SO4 is prepared. Assuming complete dissociation, what is the van't Hoff factor (i)?
A solution containing 0.1 mol of NaCl in 1 kg of water freezes at -0.372°C. Calculate the van't Hoff factor (Kf for water = 1.86 K kg mol-1).
A solution containing 0.5 mol of a non-volatile solute in 1 kg of water has a boiling point elevation of 0.26°C. If Kb for water is 0.52 K kg mol-1, calculate the van't Hoff factor.
A solution is prepared by dissolving 10 g of urea (molar mass = 60 g/mol) in 250 g of water. Calculate the molality of the solution.
A solution is prepared by dissolving 2 g of a non-volatile solute in 100 g of water. The vapour pressure of the solution is 23.5 mm Hg at 25°C. If the vapour pressure of pure water at 25°C is 23.8 mm Hg, calculate the mole fraction of the solute.
A solution of 5 g of a non-volatile solute in 100 g of water lowers the vapour pressure of water by 0.5 mm Hg at 25°C. If the vapour pressure of pure water at 25°C is 23.8 mm Hg, calculate the mole fraction of the solute.
Define the term 'colligative property'.
Describe the effect of association and dissociation of solute particles on colligative properties.
Describe the effect of temperature on the magnitude of colligative properties.
Explain the term 'hypertonic solution' in the context of osmosis.
Explain the term 'hypotonic solution' in the context of osmosis.
Explain the term 'isotonic solutions'.
Explain why electrolytes have a greater effect on colligative properties than non-electrolytes at the same concentration.
Explain why the freezing point of a solution is lower than that of the pure solvent.
State Raoult's Law.
The boiling point elevation constant (Kb) of water is 0.52 K kg mol-1. What is the boiling point of a 1 molal NaCl solution (assume complete dissociation)?
The freezing point depression constant (Kf) of water is 1.86 K kg mol-1. What is the freezing point of a solution containing 0.5 molal NaCl (assume complete dissociation)?
Which property is used in the desalination of seawater by reverse osmosis?
