The freezing point of a $0.05 \ molal$ solution of a non-electrolyte in water is $.......... \ ^oC$. $(K_f = 1.86 \ K \ kg \ mol^{-1})$

Give the formula which shows the relation between the freezing point and the fusion enthalpy of a solvent.

The freezing point of a $1\% \, Ca(NO_3)_2$ solution is ......

The freezing point of a $0.05 \ molal$ solution of a non-electrolyte in water is $(K_f = 1.86 \ K \ kg \ mol^{-1})$:

When $36 \ g$ of a non-volatile,non-electrolytic solute having the empirical formula $CH_2O$ is dissolved in $1.2 \ kg$ of water,the solution freezes at $-0.93 \ ^\circ C$. The molecular formula of the solute is ($K_f$ of water $= 1.86 \ K \ kg \ mol^{-1}$)

What is the freezing point depression constant of a solvent,$50 \ g$ of which contains $1 \ g$ of a non-volatile solute (molar mass $256 \ g \ mol^{-1}$) and the decrease in freezing point is $0.40 \ K$?