0.6 ml of acetic acid $\left(C{H}_{3}COOH\right)$ having density 1.06 g/ml is dissolved in 1 litre of water. The depression in freezing point observed for this strength of acid was $0.0205{}^{0}C.$ Calculate the Van't Hoff factor and the dissociation constant of acid.

0.6 ml of acetic acid $\left(C{H}_{3}COOH\right)$ having density 1.06 g/ml is dissolved in 1 litre of water. The depression in freezing point observed for this strength of acid was $0.0205{}^{0}C.$ Calculate the Van't Hoff factor and the dissociation constant of acid.

$0.6$mL of acetic acid having density $1.06gm{l}^{-1}$, is dissolved in $1$ litre of water. The depression of freezing point observed for the strength of acid was ${0.0205}^o$C. The dissociation constant of acid is:

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

$0.6ml$ of glacial acetic acid with density $1.06g/ml$ is dissolved in $1kg$ water and the solution froze at $-{0.0205}^{\circ }C$. Calculate van't Hoff factor:

$19.5g$ of $C{H}_{2}FCOOH$ is dissolved in $500g$ of water .The depression in the freezing point of water observed is ${1.0}^{o}C.$ Calculate the van't Hoff factor and dissociation constant of fluoroacetic acid.