A solution is prepared by dissolving `26.3` g of `CdSO_(4)` in `1000` g water. The depression in freezing point of solution was found to be `0.284` K. Calculate the Van't Hoff factor. The Cryoscopic constant of water is `1.86` K kg solvent `"mol"^(-1)-`solute.

Answer

1.21

Explanation

Molecular mass `CdSO_(4)=112.4+32+4xx16=208.4g//mol`
`"Molality "CdSO_(4)=("Mass " CdSO_(4))/("Molecular mass " CdSO_(4)xx"Mass solvent in kg"`
`=(26.3g)/((208.4g//mol)xx(1000/1000kg))=0.126m`
`Delta"T"_(f)=iK_(f)m " or " i=(Delta"T"_(f))/(K_(f)m)=(0.284K)/(1.86K//mxx0.126m)=1.21`