The Van't Hoff factor of $Ca(NO_3)_2$ is

$A$ $0.2 \ m$ solution of acid $HX$ is $20\%$ ionized in the solution. Given $K_f = 1.86 \ K \ kg \ mol^{-1}$,the freezing point of the solution is ........... $^oC$.

The Van't Hoff factor of the compound $K_3[Fe(CN)_6]$ is

$12.25 \ g$ of $CH_3CH_2CHClCOOH$ is added to $250 \ g$ of water to make a solution. If the dissociation constant of the above acid is $1.44 \times 10^{-3}$,the depression in the freezing point of water in $^{\circ}C$ is ($K_f$ for water is $1.86 \ K \ kg \ mol^{-1}$)

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

Two solutions of $KNO_3$ and $CH_3COOH$ are prepared separately. Molarity of both is $0.1 \ M$ and osmotic pressures are $P_1$ and $P_2$ respectively. The correct relationship between the osmotic pressures is :-