Chemistry - Ionic Equilibrium Question with Solution | TestHub

$\text{H}\text{P}{\text{O}}_4^{2-}+{\text{H}}_2\text{O}\rightleftharpoons {\text{H}}_2\text{P}{\text{O}}_4^{-}+\text{O}{\text{H}}^{-}$

$\text{H}\text{P}{\text{O}}_4^{2-}+{\text{H}}_2\text{O}\rightleftharpoons \text{P}{\text{O}}_4^{3-}+{\text{H}}_3{\text{O}}^{+}$

${\text{H}}_2\text{P}{\text{O}}_2^{-}$is a conjugate base of${\text{H}}_3\text{P}{\text{O}}_2$(a monobasic acid) and does not give${\text{H}}^{+},\text{H}\text{P}{\mathrm{O}}_3{}^{2-}$is a conjugate base of${\text{H}}_2\text{P}{\text{O}}_3^{-}$and does not ionise further. Since,${\text{H}}_2\text{P}{\text{O}}_3^{}$is a dibasic acid,$\text{H}\text{P}{\text{O}}_4^{2-}$can both accept or donate a proton.