Nicotinic acid `(K_(a) = 1.4 xx 10^(-5))` si represented by the formula `HNiC`. Calculate its percent dissociation in a solution which contains `0.10` moles of nictinic acid per `2.0L` of solution.

Explanation

Given, `{:(HNiC,hArr,H^(o+),+,NiC^(Θ)),(1,,0,,0),(1-alpha,,alpha,,alpha):}`
Also
`C = 0.1//2 = 5 xx 10^(-2) mol L^(-1), K_(a) = 1.4 xx 10^(-5)`
`:. K_(a) = (C alpha^(2))/((1-alpha)) = Calpha^(2)`
`alpha = sqrt(K_(a)//C) = sqrt(1.4 xx 10^(-5))/(5xx10^(-2)) = 1.67 xx10^(-2) or 1.67%`