Water exhibits an amphoteric nature, capable of acting as both a Bronsted acid and a Bronsted base. — Hydrogen Chemistry Question

💡 Solution & Explanation

In reaction A, water donates a proton to $NH_3$ (acts as an acid). In reaction B, water accepts a proton from $H_2S$ (acts as a base). Reaction D is auto-protolysis, proving dual nature. Reaction C is a *redox* reaction where water is reduced, not a Bronsted acid-base proton transfer.