Molal depression constant for a solvent is `4.0 K kg "mol"^(-1)` The depression in the freezing point of the solvent for `0.03 "mol kg^(-1)` solution of `K_(2)SO_(4)` is: (Assume complete dissociation of the electrolyte)

Answer

0.36

Explanation

Dissociation of potassium sulphate `(K_(2)SO_(4))`
`K_(2)SO_(4) to 2K^(+) + SO_(4)^(2-)`
i(Van.t hoff factor) =3
We know that, `DeltaT_(f) =iK_(f)m`
where, `K_(f)` is molal depression constant and m is molality .
`therefore DeltaT_(f) = 3 xx 4 xx 0.03 = 0.36 K`