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)

Options

A. 0.12K
B. 0.36K
C. 0.18K
D. 0.24K

Answer

B

Explanation

`Delta T_(f) = I k_(f) m`
`K_(2) SO_(4) hArr 2K^(+) + SO_(4)^(2-)`
` i= 3`
`Delta T_(f) = 3 xx 4.0 xx 0.03 = 0.36 K`