For a dilute aqueous solution of glucose,the van't Hoff factor $(i)$ is:

We have three aqueous solutions of $NaCl$ labelled as $A$,$B$ and $C$ with concentrations $0.1 \ M$,$0.01 \ M$ and $0.001 \ M$,respectively. The value of van 't Hoff factor $(i)$ for these solutions will be in the order:

$A$ 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 $CaCl_2$)

Identify the compound amongst the following whose $0.1 \ M$ aqueous solution has the highest boiling point.

$A^{2+}$,$B^{2+}$ 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:

$0.6 \, mL$ of acetic acid $(CH_{3}COOH)$,having density $1.06 \, g \, mL^{-1}$,is dissolved in $1 \, L$ of water. The depression in freezing point observed for this strength of acid was $0.0205^{\circ} \, C$. Calculate the van't Hoff factor and the dissociation constant of acid.