Brønsted–Lowry acids and bases
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Question
What is a Brønsted–Lowry acid?
Answer
A **proton (H⁺) donor**.
Question
What is a Brønsted–Lowry base?
Answer
A **proton (H⁺) acceptor**.
Question
What is a proton in acid–base chemistry?
Answer
A **hydrogen ion, H⁺** — a hydrogen atom that has lost its electron.
Question
What is a conjugate acid–base pair?
Answer
Two species that differ by **exactly one H⁺** (an acid and the base left after it donates).
Question
How do you get a conjugate base?
Answer
**Remove** one H⁺ from the acid (e.g. HCl → Cl⁻).
Question
How do you get a conjugate acid?
Answer
**Add** one H⁺ to the base (e.g. NH_{3} → NH_{4}^{+}).
Question
What is an amphiprotic species?
Answer
A species that can **both donate and accept** a proton (e.g. H_{2}O, HCO_{3}⁻).
Question
Conjugate base of H_{2}SO_{4}?
Answer
**HSO_{4}⁻** (remove one H⁺ — not SO_{4}^{2-}, which is two H⁺ away).
Question
Conjugate acid of H_{2}O?
Answer
**H_{3}O^{+}** (the oxonium / hydronium ion).
Question
Two amphiprotic examples?
Answer
**H_{2}O** and **HCO_{3}⁻** — both can donate or accept a proton.
Question
In HCl + H_{2}O → H_{3}O^{+} + Cl⁻, which is the acid?
Answer
**HCl** — it donates the proton; water is the base.
Question
Why does an acid need a base present?
Answer
An acid can only **donate** H⁺ if a base is there to **accept** it — every proton transfer has both.
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Full study notes for Brønsted–Lowry acids and bases
Topic 6.1 hub
Proton transfer reactions
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