Considering acetic acid dissociates in water, its dissociation constant is \(6.25\times {10}^{-5}\) . If \(5\mathrm{ml}\…

Considering acetic acid dissociates in water, its dissociation constant is \(6.25\times {10}^{-5}\) . If \(5\mathrm{ml}\) of acetic acid is dissolved in 1 litre water, the solution will freeze at \(-\mathrm{x}\times {10}^{-2}^\circ \mathrm{C}\), provided pure water freezes at \(0^\circ C\). \(x=\)________
Given: \({\left({K}_{f}\right)}_{\text{water }}=1.86Kkgmo{l}^{-1}\text{. }\)

Density of acetic acid is 1.2 g mL^–1.

molar mass of water = 18 g mol^–1.

molar mass of acetic acid = 60 g mol^–1.

density of water = 1 g cm^–3

Acetic acid dissociates as

\({\mathrm{CH}}_{3}\mathrm{COOH}⇌{\mathrm{CH}}_{3}{\mathrm{COO}}^{-}+{\mathrm{H}}^{+}\)