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

$1.2 \, mL$ of acetic acid is dissolved in water to make $2.0 \, L$ of solution. The depression in freezing point observed for this strength of acid is $0.0198^{\circ} C$. The percentage of dissociation of the acid is $....$ (Nearest integer)
[Given : Density of acetic acid is $1.02 \, g \, mL^{-1}$
Molar mass of acetic acid is $60 \, g \, mol^{-1}$
$K_{f}(H_{2}O) = 1.85 \, K \, kg \, mol^{-1}$]

In a solvent,$50\,\%$ of an acid $HA$ dimerizes and the rest dissociates. The van't Hoff factor of the acid is $.....\times 10^{-2}$. (Round off to the nearest integer)

When $1.0 \ g$ of $KCl$ is dissolved in $200 \ g$ water,the decrease in freezing point of such solution is $0.24 \ K$,calculate Van't Hoff factor $(i)$ for such solution. $K_f$ of water $=$ $1.86 \ K \ kg \ mol^{-1}$.

Acetic acid dissolved in benzene shows a molecular weight of

$20 \ g$ of a binary electrolyte (molar mass = $100 \ g \ mol^{-1}$) is dissolved in $500 \ g$ of water. The freezing point of the solution is $-0.74 \ ^oC$. Given $K_f = 1.86 \ K \ kg \ mol^{-1}$,the degree of dissociation of the electrolyte is ......... $\%$.