• A Brønsted–Lowry acid is a proton/H+ donor and a Brønsted–Lowry base is a proton/H+ acceptor.

• Amphiprotic species can act as both Brønsted–Lowry acids and bases.

• A pair of species differing by a single proton is called a conjugate acid-base pair.

• Deduction of the Brønsted–Lowry acid and base in a chemical reaction.

• Deduction of the conjugate acid or conjugate base in a chemical reaction.

• Lewis theory is not required here.

• The location of the proton transferred should be clearly indicated. For example, CH3COOH/CH3COO– rather than C2H4O2/C2H3O2–.

• Students should know the representation of a proton in aqueous solution as both H+ (aq) and H3O+ (aq).

• The difference between the terms amphoteric and amphiprotic should be covered.