1.00 g of a non-electrolyte solute dissolved in 50g of benzene lowered the freezing point of benzene by 0.40 K. The freezing point depression constant of benzene is 5.12 K kg `mol^(-1)`. Find the molar mass of the solute.

Explanation

Substituting the values of various terms involved in equation (2.36) we get,
` M_(2) = (5.12 "kg mol"^(-1) xx 1.00 g xx 1000 " g kg"^(-1))/(0.46 xx50 g ) = 256 " g mol"^(-1)`
Thus, molar mass of the solute = `256" g mol"^(-1)`