The van't Hoff factor $(i)$ is .....

Determination of the molar mass of acetic acid in benzene using freezing point depression is affected by

The observed osmotic pressure of a solution of benzoic acid in benzene is less than its expected value because:

When benzoic acid dissolves in benzene,the observed molecular mass is

The depression in freezing point observed for a formic acid solution of concentration $0.5 \, mL \, L^{-1}$ is $0.0405^{\circ} \, C$. The density of formic acid is $1.05 \, g \, mL^{-1}$. The Van't Hoff factor of the formic acid solution is nearly: (Given for water $K_{f} = 1.86 \, K \, kg \, mol^{-1}$)

When $2.44 \ g$ of benzoic acid $(C_6H_5COOH)$ is dissolved in $25 \ g$ of benzene,it shows a depression of freezing point equal to $2.2 \ K$. The molal depression constant of benzene is $5.0 \ K \ kg \ mol^{-1}$. What is the percentage association of the acid,if it forms a dimer in the solution (in $\%$)?