What is the percentage of dissociation of a $0.011 \ m$ aqueous solution of $K_3[Fe(CN)_6]$ having a freezing point of $-0.063 \ ^oC$? (Given: $K_f = 1.86 \ K \ kg \ mol^{-1}$ for water)

Carnallite in solution in $H_2O$,shows the properties of

The freezing points of equimolar solutions of glucose,$KNO_3$ and $AlCl_3$ are in the order of:

Calculate the depression in the freezing point of water when $10 \ g$ of $CH_3CH_2CHClCOOH$ is added to $250 \ g$ of water. $K_a = 1.4 \times 10^{-3}$,$K_f = 1.86 \ K \ kg \ mol^{-1}$

Calculate the molality of an aqueous solution of an electrolyte that freezes at $-0.93 \text{ }^\circ\text{C}$. Given that $K_f$ for water is $1.86 \text{ K kg mol}^{-1}$ and the van't Hoff factor $(i)$ is $1.25$. (Freezing point of pure water $= 0 \text{ }^\circ\text{C}$) (in $\text{ m}$)

Which one of the following electrolytes has the same value of van't Hoff factor $(i)$ as that of $Al_2(SO_4)_3$ (if all are $100 \%$ ionised)?