The molal depression constant for water is $1.86 \, ^\circ C \, kg \, mol^{-1}$. The freezing point of a $0.05 \, m$ solution of a non-electrolyte in water is:

The freezing point depression constant $(K_{f})$ of benzene is $5.12 \ K \ kg \ mol^{-1}$. The freezing point depression for the solution of molality $0.078 \ m$ containing a non-electrolyte solute in benzene is..........$K$ (rounded off up to two decimal places).

$CaCl_2$ is preferred over $NaCl$ for clearing ice on roads,particularly in very cold countries. This is because:

If the $K_f$ value of $H_2O$ is $1.86 \ K \ kg \ mol^{-1}$,the value of $\Delta T_f$ for a $0.1 \ m$ solution of a non-volatile solute is:

Calculate the molality of a solution if its depression in freezing point is $0.18 \ K$. $[K_f = 1.6 \ K \ kg \ mol^{-1}]$ (in $m$)

Calculate the mass of ascorbic acid $(\text{C}_6\text{H}_8\text{O}_6)$ to be dissolved in $75 \text{ g}$ of acetic acid to lower its melting point by $1.5^\circ\text{C}$. $[K_f = 3.9 \text{ K kg mol}^{-1}, \text{H} = 1, \text{C} = 12, \text{O} = 16 \text{ amu}]$ (in $\text{ g}$)