객관식
Which of the following pairs of compounds are both electrolytes?
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6. Chemical Quantities & Aqueous Reactions
Electrolytes
객관식
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)
검증된 단계별 안내1
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.
Step 2: Examine each given chemical equation to determine if it represents complete ionization (strong electrolyte) or partial ionization (weak electrolyte or water autoionization).
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.
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.
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.
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