$A^{2+}$,$B^{2+}$ and $C^{-}$ form an ionic complex like $A_{x-2}[B(C)_x]_2$. If the complex is $75 \%$ dissociated in a solvent with $i=4$,the coordination number of $B$ is:

Which of the following $0.05 \ M$ aqueous solution will have the lowest freezing point?

The elevation in the boiling point of an aqueous solution of $NaCl$ is $0.01^{\circ}C$. If its van't Hoff factor is $1.92$,the molality of the $NaCl$ solution is: $(K_{b} \text{ for water} = 0.52 \ K \ kg \ mol^{-1})$ (in $m$)

$A$ solution of $CaCl_2$ is prepared by dissolving $0.0112 \ g$ of $CaCl_2$ in $1 \ kg$ of distilled water. If the molal freezing point depression constant $(K_f)$ of water is $2 \ K \ kg \ mol^{-1}$,what is the depression in the freezing point of the solution? (Assume $100\%$ ionization of $CaCl_2$)

Calculate the van't Hoff factor $(i)$ of a centimolar solution of potassium ferrocyanide $(K_4[Fe(CN)_6])$ if it is $60\%$ dissociated at $300\text{ K}$.

The freezing point of an equimolal aqueous solution will be highest for: