According to the Bronsted-Lowry and Lewis acid-base theories, which of the following species strictl — Ionic Equilibrium Chemistry Question

💡 Solution & Explanation

An amphiprotic species must be capable of both donating a proton and accepting a proton. $H_2PO_4^-$ 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 $H_2CO_3$. $HSO_4^-$ can donate $H^+$ to form $SO_4^{2-}$ or accept to form $H_2SO_4$. $O^{2-}$ is strictly a Bronsted base (can only accept $H^+$ to form $OH^-$) and cannot donate a proton.