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Molal depression constant for a solvent is $4.0 k g m o l^{- 1}$ The
depression in the freezing point of the solvent for $0.03 m o l k g^{- 1}$ solution of $K_{2} S O_{4}$ is
(Assume complete dissociation of the electrolyte)

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$0.12 K$

$0.36 K$

$0.18 K$

$0.24 K$

answer is B.

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Detailed Solution

$\begin{array}{l} K_{f} = 4 K - kg / mol \\ m = 0.03 mol / kg \\ i = 3 \\ Δ T_{f} = i K_{f} \times m \\ Δ T_{f} = 3 \times 4 \times 0.03 = 0.36 K . \end{array}$

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