The experimental molecular weight of an electrolyte will always be less than its calculated value because the value of Van't Hoff factor $i$ is

Which of the following aqueous solutions has the highest boiling point,under identical conditions having a concentration of $0.03 \ m$?

The van't Hoff factor $(i)$ for the reaction of $HNO_3$ with $H_2SO_4$ 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.

Write the value of the van't Hoff factor $(i)$ for $K_{2}SO_{4}$ and $K_{4}[Fe(CN)_{6}]$.

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.