The Van't Hoff factor will be highest for

Calculate the freezing point (in ${}^{\circ}C$) of a solution obtained by dissolving $0.1 \ g$ of potassium ferricyanide (molecular weight $= 329$) in $100 \ g$ of water. Given that $K_f$ for water is $1.86 \ K \ kg \ mol^{-1}$.

The freezing point of a $2\%$ aqueous solution of $[Ag(CH_3NH_2)_2]Cl$ is:

The addition of a polar solvent to a solid electrolyte results in:

The boiling point of $0.001 \ M$ aqueous solutions of $NaCl$,$Na_{2}SO_{4}$,$K_{3}PO_{4}$ and $CH_{3}COOH$ should follow the order.

$MX_{2}$ dissociates into $M^{2+}$ and $X^{-}$ ions in an aqueous solution,with a degree of dissociation $(\alpha)$ of $0.5$. The ratio of the observed depression of freezing point of the aqueous solution to the value of the depression of freezing point in the absence of ionic dissociation is