When $4.5 \ g$ of a non-electrolyte solute is dissolved in $100 \ g$ of water,the freezing point of the solution is lowered by $0.465^o C$. The molar mass of the solute is ....... $g/mol$. (Given $K_f = 1.86 \ K \ kg \ mol^{-1}$)

$A$ solution containing $8.0 \, g$ of nicotine in $92 \, g$ of water freezes $0.925 \, ^{\circ}C$ below the normal freezing point of water. If the molal freezing point depression constant,$k_f = 1.85 \, ^{\circ}C \, kg \, mol^{-1}$,then the molar mass of nicotine is $...$

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 the correct relation between depression in freezing point and the freezing point of a pure solvent.

Bromoform has a normal freezing point of $7.734^{\circ} C$ and its $K_{f} = 14.4^{\circ} C / m$. $A$ solution of $2.60 \ g$ of an unknown substance in $100 \ g$ of bromoform freezes at $5.43^{\circ} C$. What is the molecular weight of the unknown substance?

Calculate $\Delta T_f$ of $0.15 \ m$ solution of nonvolatile solute $\left[K_f = 1.5 \ K \ kg \ mol^{-1}\right]$ (in $K$)