Out of the following, which species are amphiprotic in an aqueous medium? — Ionic Equilibrium Chemistry Question

💡 Solution & Explanation

An amphiprotic species can act as both a Bronsted acid (donate $H^+$) and a Bronsted base (accept $H^+$). $H_2PO_4^-$ can donate $H^+$ to form $HPO_4^{2-}$ or accept $H^+$ to form $H_3PO_4$. $HCO_3^-$ can donate $H^+$ to form $CO_3^{2-}$ or accept $H^+$ to form $H_2CO_3$. $H_2PO_2^-$ is derived from hypophosphorous acid which is monoprotic; it has no more ionizable protons. $OH^-$ cannot act as an acid in water (forming $O^{2-}$ is not feasible in aqueous medium).