Dissolution of $1.5 \ g$ of a non-volatile solute (mol. wt. $= 60$) in $250 \ g$ of a solvent reduces its freezing point by $0.01 \ ^{\circ}C$. Find the molal depression constant of the solvent.

The depression in freezing point of a solution of molality $0.01 \ mol \ kg^{-1}$ is highest with respect to which of the following solvents? (The $K_f$ value is given in brackets)

Identify $(i)$,$(ii)$ and $(iii)$ in the following diagram representing the depression in freezing point:

When glycerine is added to a litre of water,which of the following behaviors is observed?

$A$ solution of a nonvolatile solute is obtained by dissolving $15 \ g$ in $200 \ mL$ of water,which has a depression in freezing point of $0.75 \ K$. Calculate the molar mass of the solute if the cryoscopic constant of water is $1.86 \ K \ kg \ mol^{-1}$.

Calculate the molality of a nonvolatile solution if the solution freezes at $-0.95^{\circ}C$ $[K_f \text{ for water} = 1.86 \ K \ kg \ mol^{-1}, \text{ freezing point of water} = 0^{\circ}C]$.