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A solution is prepared by dissolving 26.3 g of `CdSO_(4)`in 1000 g of water. The depression in freezing point of the solution was forund to be 0.284 K. Calculate Van't Hoff factor. The cryoscopic constant for water is 1.86 K kg `mol^(-1)`. (Given molar mass of `CdSO_(4)=208 g mol^(-1)`.)

Text Solution

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The correct Answer is:
1.21
`DeltaT_(f)=ixxK_(f)xxm=iK_(f)xxW_(B)/(M_(B)xxW_(A))`
`DeltaT_(f)=0.284 K, K_(f)=1.86" K kg mol"^(-1), W_(B)=26.3 g,`
`M_(B)=208.4" g mol"^(-1),W_(A)=1g.`
`i=(DeltaT_(f)xxM_(B)xxW_(B))/(K_(f)xxW_(B))=((0.28K)xx(208.4"g mol"^(-1))xx(1g))/((1.86" K kg mol"^(-1))xx(26.3g))=1.21.`
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