At a certain temperature, the ionisation of two weak acids, HA and HB are `K_(a_(1)) and K_(a_(2))`, respectively. If `K_(a_(1)) gt K_(a_(2))` and the concentration of the aqueous solutions of both the acids be 0.1(M), then which solution will have a higher pH?

Explanation

As the ionisation constant of HA is higher than that of HB, the degree of ionisation of HA in its 0.1 M solution. As a result, the molar concentration of `H_(3)O^(+)` ions in 0.1(M) HA solution will be more than that in 0.1(M) HB solution. Therefore, pH of HB solution will be greater than that of HA solution.