The freezing point of nitrobenzene is 278.8 K. A 0.25 molal solution of a substance (MM. 120) in nitrobenzene have freezing points 276.8 K. Calculate the molal depression constant of nitrobenzene.

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Solution

$Δ T_{f} = K_{f} \times m o l a l i t y = K_{f} \times 0.25 Δ T_{f} = 278.8 K - 276.8 K = 2.0 K Δ T_{f} = K_{f} \times 0.25 K_{f} = \frac{Δ T_{f}}{0.25} = \frac{2.0}{0.25} = 8 K k g {m o l}^{- 1}$

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