$50 \ g$ of antifreeze (ethylene glycol) is added to $200 \ g$ of water. What amount of ice will separate out at $-9.3 \ ^oC$? $(K_f = 1.86 \ K \ kg \ mol^{-1})$

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 $= 3.9 \ K \ kg \ mol^{-1}$)

$A$ solution of $5 \ g$ nonvolatile solute in $50 \ g$ water decreases its freezing point by $0.2 \ K$. Calculate the molar mass of solute if $K_{f}$ of water is $1.86 \ K \ kg \ mol^{-1}$.

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

The amount of urea to be dissolved in $500 \ mL$ of water $(K_f = 18.6 \ K \ kg \ mol^{-1})$ to produce a depression of $0.186 \ ^oC$ in freezing point is $....... \ g$. (Assume density of water = $1 \ g/mL$)

The normal freezing point $(f.p.)$ of nitrobenzene is $278.82 \ K$. If a non-volatile solute is dissolved in it and a solution of $0.25 \ molality$ is prepared,the observed freezing point of the solution is $276.82 \ K$. Evaluate the cryoscopic constant $(K_f)$ of nitrobenzene in $K \ kg \ mol^{-1}$.