Considering acetic acid dissociates in water, its dissociation constant is $$6.25 \times 10^{-5}$$. If $$5$$ mL of acetic acid is dissolved in 1 litre water, the solution will freeze at $$-x \times 10^{-2} °C$$, provided pure water freezes at $$0°C$$. $$x =$$ ______ . (Nearest integer) Given : $$(K_f)_{water} = 1.86 \text{ K kg mol}^{-1}$$, density of acetic acid is $$1.2 \text{ g mL}^{-1}$$, molar mass of water $$= 18 \text{ g mol}^{-1}$$, molar mass of acetic acid $$= 60 \text{ g mol}^{-1}$$, density of water $$= 1 \text{ g cm}^{-3}$$. Acetic acid dissociates as $$CH_3COOH \rightleftharpoons CH_3COO^- + H^+$$