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The freezing point of a solution contain...

The freezing point of a solution containing of `0.2g` of acetic acid in `20.0g` of benzene is lowered `0.45^(@)C`. Calculate.
(i) the molar mass of acetic acid from this data
(ii) Van't Hoff factor
[For benzene, `K_(f)=5.12K kg "mol"^(-1)`]
What conclusion can you draw from the value of Van't Hoff factor obtained ?

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