The normal freezing point of a pure liquid is the temperature at which the vapour pressure of the solid is equal to the vapour pressure of the liquid at atmospheric pressure. That is at the freezing point of a solvent the solid and the liquid are in equilibrium. When a solution freezes, it is not the solution that solidifies but the pure solvent that freezes out from the solution. Thus the freezing point of a solution is the temperature at which the vapour pressure of the solvent in the solid state and the vapour pressure of the solution in the liquid state are equal. Since the vapour pressure of a solution is lower than that of the pure liquid solvent the solution and the solid solvent can be in equilibrium only if the vapour pressure of the solid solvent becomes lower.
1. WHich one of the following gases has the lowest value of Henry’s law constant?
2. If 10ml of 0.1M aqueous solution of NaCl is divided into 1000 drops of equal volume. What will be the concentration of one drop?
3. A 0.5 molal solution of ethylene glycol in water is used as coolant in a car. If the freezing point constant of water be 1.86oC per mole, the mixture shall freeze at
4. Which statement is true for a solution of 0.020M H2SO3?
- 2 litre of the solution contains 0.020 mole of SO42-
- 2 litre of the solution contains 0.080 mole of H3O+
- 1 litre of the solution contains 0.020 mole of H3O+
- None of these
5. A 500g toothpaste sample has 0.2g fluoride concentration. What is the concentration of F in terms of ppm level?
6. If at certain temperature the vapour pressure of pure water is 25mm Hg and that of a very dilute aqueous urea solution is 24.5mm Hg, the molality of the solution is
7. WHich of the following 0.10m aqueous solutions will have the lowest freezing point?
8. The amount of urea to be dissolved in 500cc of water (K = 1.86oC mol-1) to produce a depression of 0.186oC in the freezing point is
9. The empirical formula of a nonelectrolyte is CH2O. A solution containing 6g of the compound exerts the same osmotic pressure as that of 0.05M glucose solution at the same temperature, The molecular formula of the compound is
10. The molar mass of the solute sodium hydroxide obtained from the measurement of the osmotic pressure of its aqueous solution at 27oC is 25gmol-1. Therefore its ionization solution at 27oC is 25g mol-1. Therefore its ionization percentage in this solution is