0.6 mL of acetic acid ($CH_3COOH$) having a density of 1.06 g $mL^{−1}$ is dissolved in 1 litre of water. The depression in freezing point observed for this strength of the acid was 0.0205$^{\large\circ}$C. Calculate the van’t Hoff factor and the dissociation constant of the acid. $K_f$ for water = 1.86 K kg $mol^{−1}$.

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