1.

3.9 g of benzoic acid dissoved in 49 g of benzene shows a depression in freezing point of 1.62 K. Calculate Van't Hoff factor and predict the nature of solute (associated or dissociated) . (Given. Molar mass of benzoic acid = 122 g mol^(-1) , K_(f) for benzene = 4.9 K kg mol^(-1)).

Answer»


Solution :`i=(DeltaT_(f))/(K_(f)xxm)DeltaT_(f)=1.62 K, K_(f)=4.9" K kg mol"^(-1), M=((3.9g)//(122" g mol"^(-1)))/((0.049 kg))`
`i=(1.62Kxx(0.049" kg")XX(122" g mol"^(-1)))/((4.9"K kg mol"^(-1))xx(3.9g))=0.506`
SCINCE Van't Hoff factor is LESS than 1, SOLUTE has UNDERGONE has undergone associated in benzene solvent.


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