Considering acetic acid dissociates in water, its dissociation constant is 6.25 × 10^-5. If 5 mL of acetic acid is dissolved in 1 litre water, the…

Considering acetic acid dissociates in water, its dissociation constant is $\displaystyle 6.25 \times 10^{-5}$. If $\displaystyle 5$ mL of acetic acid is dissolved in $\displaystyle 1$ litre water, the solution will freeze at $\displaystyle -x \times 10^{-2}{ }^{\circ} \mathrm{C}$, provided pure water freezes at $\displaystyle 0{ }^{\circ} \mathrm{C}$. $\displaystyle x=$ $\displaystyle \_\_\_\_$. (Nearest integer) Given: $\displaystyle \left(\mathrm{K}_f\right)_{\text {water }}=1.86 \mathrm{~K} \mathrm{~kg} \mathrm{~mol}^{-1}$. density of acetic acid is $\displaystyle 1.2 \mathrm{~g} \mathrm{~mol}^{-1}$. molar mass of water $\displaystyle =18 \mathrm{~g} \mathrm{~mol}^{-1}$. molar mass of acetic acid $\displaystyle =60 \mathrm{~g} \mathrm{~mol}^{-1}$. density of water $\displaystyle =1 \mathrm{~g} \mathrm{~cm}^{-3}$ Acetic acid dissociates as $\displaystyle \mathrm{CH}_3 \mathrm{COOH} \rightleftharpoons \mathrm{CH}_3 \mathrm{COO}^{\ominus}+\mathrm{H}^{\oplus}$