The `pH` of `0.1 M` solution of cyanic acid `(HCNO)` is `2.34`. Calculate the ionization constant of the acid and its degree of ionisation in the solution.

Explanation

`HCNO + H_(2)O to H_(3)O^(+) + CNO^(-)`
pH=2.34`implies[H^(+)]=[H_(3)O^(+)]=4.57xx10^(-3)M`
Degree of ionization,`alpha= (4.57xx10^(-3))/0.1 = 4.57xx10^(-2)`
Ionization constant,`K_(a)=([H_(3)O^(+)] [CNO^(-)])/([HCNO])`=`(4.57xx10^(-3)xx4.57xx10^(-3))/0.1 = 2.089xx10^(-4)`