$A$ solution of $CaCl_2$ is prepared by dissolving $0.0112 \ g$ of $CaCl_2$ in $1 \ kg$ of distilled water. If the molal freezing point depression constant $(K_f)$ of water is $2 \ K \ kg \ mol^{-1}$,what is the depression in the freezing point of the solution? (Assume $100\%$ ionization of $CaCl_2$)

$A$ $0.5 \ m$ aqueous solution of a weak acid $(HX)$ is $20\%$ ionized. If $K_f$ for the solvent is $1.86 \ K \ kg \ mol^{-1}$,the depression in freezing point of the solution is ..... $K$.

Which solution has the maximum boiling point?

$19.5 \text{ g}$ of fluoroacetic acid (molar mass = $78 \text{ g mol}^{-1}$) is dissolved in $500 \text{ g}$ of water at $298 \text{ K}$. The depression in the freezing point of water was $1^\circ\text{C}$. What is $K_a$ of fluoroacetic acid? (For water, $K_f = 1.86 \text{ K kg mol}^{-1}$). Assume molarity and molality to have same values.

The freezing point of a $0.2 \ m$ aqueous solution of a weak acid $(HX)$ which is $20\%$ ionized is ......... $^oC$. (Given: $K_f = 1.86 \ ^oC/m$ for water)

Which of the following has the minimum freezing point?