The freezing point of a solution prepared from $1.25 \ g$ of a non-electrolyte and $20 \ g$ of water is $271.9 \ K$. If the molar depression constant is $1.86 \ K \ kg \ mol^{-1}$,then the molar mass of the solute will be:

Calculate the molal depression constant of a solvent, which freezes at $15^{\circ}C$. The latent heat of fusion is $180.7 \ Jg^{-1}$.

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

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

Lead storage battery contains $38\%$ by weight solution of $H_2SO_4$. The van't Hoff factor is $2.67$ at this concentration. The temperature in Kelvin at which the solution in the battery will freeze is $..........$ (Nearest integer). Given $K_f = 1.8 \, K \, kg \, mol^{-1}$.

The mass of ascorbic acid $(C_6H_8O_6)$ to be dissolved in $100 \ g$ of acetic acid to lower its freezing point by $1.5^{\circ}C$ in $g$ is: (Given: $K_f$ for acetic acid $= 3.9 \ K \ kg \ mol^{-1}$)