The interionic attraction depends on the interaction of:

$0.6 \, mL$ 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.

$A$ 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 $CaCl_2$)

Consider the following solutions at $25\,^oC$:
$(I)$ $0.01\, M$ aqueous solution of glucose
$(II)$ $0.01\, M$ aqueous solution of $KNO_3$
$(III)$ $0.01\, M$ solution of acetic acid in benzene
Select the correct statement.

The molal elevation constant of water is $0.51 \ K \ kg \ mol^{-1}$. The boiling point of a $0.1 \ m$ aqueous $NaCl$ solution is approximately ......... $^oC$.

Van't Hoff factor of $BaCl_2$ in its aqueous solution will be: ($BaCl_2$ is $60 \%$ ionized in the solution)