Nicotinic acid `(K_(a)=1.4xx10^(-5))` is repersented by the formula HNiC. Calculate its per cent dissociation in a solution, which contains `0.10` mole of nicotinic acid per `2.0` litre of solution.

Explanation

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