$0.8 \mathrm{~mL}$ of acetic acid of density $1.06 \mathrm{~g} \mathrm{~mL}^{-1}$ when dissolved in $1…
$0.8 \mathrm{~mL}$ of acetic acid of density $1.06 \mathrm{~g} \mathrm{~mL}^{-1}$ when dissolved in $1 \mathrm{~kg}$ of water causes a depression in freezing point by $0.0325^{\circ} \mathrm{C}$. The Van't Hoff factor is:
$\left(\mathrm{K}_{\mathrm{f}} \text { of } \mathrm{H}_2 \mathrm{O}=1.86 \mathrm{~K} \mathrm{~kg} \mathrm{~mol}^{-1}\right)$