A buffer solution can be prepared from a mixture of — Ionic Equilibrium Chemistry Question

💡 Solution & Explanation

A buffer requires a mixture of a weak acid/base and its corresponding salt. (A) 2 moles of $\text{NH}_4\text{Cl}$ reacting with 1 mole of $\text{NaOH}$ forms 1 mole of $\text{NH}_4\text{OH}$ and leaves 1 mole of $\text{NH}_4\text{Cl}$, forming a basic buffer. (C) 2 moles of $\text{CH}_3\text{COONa}$ reacting with 1 mole of $\text{HCl}$ forms 1 mole of $\text{CH}_3\text{COOH}$ and leaves 1 mole of $\text{CH}_3\text{COONa}$, forming an acidic buffer. Mixtures (B) and (D) either fully convert to weak acid or leave excess strong acid, preventing buffer formation. Therefore, correct answer is A,C.