1.

A solution of an organic compound is prepared by dissolving 34.2 g in 500 g of water. Calculate the molar mass of the compound and freezing point of the solution. Given that K_(b) for water ="0.52 K mol"^(-1) B.pt of solution =100.104^(@)C.K_(f) for water =1.87"K mol"^(-1).

Answer»


Solution :`DeltaT_(b)=0.104^(@),w_(2)=34.2g, w_(1)=500 g, K_(b)=0.52Kmol"^(-1)`
`therefore""M_(2)=(1000K_(b)w_(2))/(w_(1)xxDeltaT_(b))=(1000xx0.52xx34.2)/(500xx0.104)="342 g mol"^(-1)`
`DeltaT_(F)=K_(f)xxm=(1.87)XX((34.2)/(342)xx(1)/(500)xx1000)=0.374""therefore"F.pt "=-0.374^(@)C`.


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