What will be the freezing point of a $1\%$ aqueous solution of $Ca(NO_3)_2$?

Calculate the freezing point of a $0.05 \ m$ aqueous solution of a non-electrolyte. (in $K$)

Calculate the molal depression constant of a solvent which has freezing point $16.6\,^oC$ and latent heat of fusion $180.75\,J\,g^{-1}$.

$6 \ g$ of a non-volatile,non-electrolyte $X$ dissolved in $100 \ g$ of water freezes at $-0.93^{\circ} C$. The molar mass of $X$ in $g \ mol^{-1}$ is ($K_f$ of $H_2O = 1.86 \ K \ kg \ mol^{-1}$)

When $1.25 \ g$ of a non-volatile solute is dissolved in $20 \ g$ of water,the freezing point of the solution is found to be $271.9 \ K$. If the molal depression constant $(K_f)$ is $1.86 \ K \ kg \ mol^{-1}$,what is the molar mass of the solute?

During the depression in freezing point experiment, an equilibrium is established between the molecules of