Which of the following chemical equations best represents the ionization of a strong electrolyte in water?

• A. H_2O(l) ⇌ H^+(aq) + OH^-(aq)
• B. NaCl(s) → Na^+(aq) + Cl^-(aq)
• C. NH_3(aq) + H_2O(l) ⇌ NH_4^+(aq) + OH^-(aq)
• D. CH_3COOH(aq) ⇌ CH_3COO^-(aq) + H^+(aq)

Answer: (B)

Verified step by step guidance

1. Step 1: Understand what a strong electrolyte is. A strong electrolyte is a substance that completely dissociates into its ions when dissolved in water, meaning the ionization reaction goes to completion and does not establish an equilibrium.
2. Step 2: Examine each given chemical equation to determine if it represents complete ionization (strong electrolyte) or partial ionization (weak electrolyte or water autoionization).
3. Step 3: The equation \(\mathrm{H_2O(l) \rightleftharpoons H^+(aq) + OH^-(aq)}\) represents the autoionization of water, which is a very weak ionization and is an equilibrium process, so it is not a strong electrolyte ionization.
4. Step 4: The equation \(\mathrm{NH_3(aq) + H_2O(l) \rightleftharpoons NH_4^+(aq) + OH^-(aq)}\) shows ammonia acting as a weak base, partially ionizing in water, so it is not a strong electrolyte.
5. Step 5: The equation \(\mathrm{CH_3COOH(aq) \rightleftharpoons CH_3COO^-(aq) + H^+(aq)}\) represents acetic acid, a weak acid that partially ionizes in water, so it is not a strong electrolyte. The equation \(\mathrm{NaCl(s) \rightarrow Na^+(aq) + Cl^-(aq)}\) shows complete dissociation of sodium chloride, a strong electrolyte, into its ions without equilibrium, which best represents the ionization of a strong electrolyte.