Water is universally recognized as an amphoteric solvent capable of auto-protolysis. Which of the fo — Hydrogen Chemistry Question

💡 Solution & Explanation

As a Bronsted acid, water donates a proton (e.g., to $NH_3$, forming $OH^-$ and $NH_4^+$). As a Bronsted base, water accepts a proton (e.g., from $H_2S$, forming $H_3O^+$ and $HS^-$). Redox reactions (like with Na) or extensive hydrolysis (like $CaC_2$) are not direct proofs of simple Bronsted acid-base duality.