Question

If sodium sulphate is considered to be completely dissociated into cations and anions in aqueous solution, what is the change in freezing point of water(ΔTf),when 0.02mol of sodium sulphate is dissolved in 1kg of water,is (Kf=1.86Kkgmol−1)?

Answer 1

Answer:

What is the freezing point of a solution that contains 0.5 moles of Nal in 500g of water? (Kf = 1.86C/m; molar mass of water = 18g)

Explanation:

Explanation:

Your strategy here will be to

determine the van't Hoff factor for sodium iodide,

NaI

calculate the molality of the solution

calculate the freezing-point depression of the solution

The idea is that the freezing point of a solution is lower than the freezing point of the pure solvent, which for water is

0

∘

C

at normal pressure.

Now, the difference between the freezing point of the pure solvent and the freezing point of the solution is given by the freezing-point depression, which can be calculated

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