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

When mercuric iodide $(HgI_2)$ is added to an aqueous solution of potassium iodide $(KI)$,the

$17.4\% \text{ (mass/volume) } K_2SO_4$ solution at $27^\circ C$ is isotonic to $5.85\% \text{ (mass/volume) } NaCl$ solution at $27^\circ C$. If $NaCl$ is $100\%$ ionized,what is the $\%$ ionization of $K_2SO_4$ in aqueous solution? [Atomic weights: $K = 39, Na = 23, S = 32, O = 16, Cl = 35.5$]

Which of the following compounds has a Van't Hoff factor $i$ equal to $2$ for a dilute solution?

Which of the following will have the highest depression in freezing point when their concentration is $0.1 \ M$?

The freezing point of equimolal aqueous solution will be highest for