If the $O.P.$ (Osmotic Pressure) of $1 \ M$ solutions of the following compounds in water can be measured,which one will show the maximum $O.P.$?

Calculate the approximate $\Delta T_b$ (in $K$) for $0.001 \ m$ $KCl$ solution, if its van't-Hoff factor is $1.98$ [$K_b$ of water is $0.52 \ K \ kg \ mol^{-1}$].

Considering acetic acid dissociates in water,its dissociation constant is $6.25 \times 10^{-5}$. If $5 \ mL$ of acetic acid is dissolved in $1 \ L$ water,the solution will freeze at $-x \times 10^{-2} \ {}^{\circ}C$,provided pure water freezes at $0 \ {}^{\circ}C$.
$x = . . . . . . . . .$ (Nearest integer)
Given: $(K_{f})_{\text{water}} = 1.86 \ K \ kg \ mol^{-1}$.
Density of acetic acid is $1.2 \ g \ mL^{-1}$.
Molar mass of water $= 18 \ g \ mol^{-1}$.
Molar mass of acetic acid $= 60 \ g \ mol^{-1}$.
Density of water $= 1 \ g \ cm^{-3}$.
Acetic acid dissociates as:
$CH_3COOH \rightleftharpoons CH_3COO^{-} + H^{+}$

$A$ $0.5 \ m$ 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 ....... $K$.

The $\Delta T_{b}$ value for $0.01 \ m$ $KCl$ solution is $0.01 \ K$. What is the Van't Hoff factor? $(K_{b}$ for water $= 0.52 \ K \ kg \ mol^{-1})$

Which one of the following $0.10 \ M$ aqueous solutions will exhibit the largest freezing point depression?