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The freezing point of nitrobenezene is 2...

The freezing point of nitrobenezene is 278.82K. A 0.15 molal solution of nitrobenzene caues freezing point depression of 1.2K. Calculate the value of `K_(f)` for nitrobenzene.

Text Solution

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Molality of solution =0.15m. Depression of freezing point, `Delta T_(f)= K_(f).m`
`1.2K=K_(f)xx 0.15m`
Therefore, molal depression constant, `K_(f)= (1.2K)/(0.15m)=8Km^(-1)`
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