Which pair is a Brønsted-Lowry conjugate acid-base pair?

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Motivational context for this question centers on identifying Brønsted-Lowry conjugate acid–base pairs. 
Option 1: NH4+/NH3. Here, NH3 acts as a base that can accept a proton to become NH4+, its conjugate acid. Conversely, NH4+ can donate a proton to revert to NH3. This pair exactly fits the Brønsted-Lowry relationship of conjugate acid–base partners.
Option 2: H3O+/OH–. While these species are related through the autoionization of water, they are not a conjugate acid–base pair of one another. H3O+ is the conjugate acid of H2O, and OH– is the conjugate base of H2O; the pair H3O+ and OH– do not arise from a single conjugate pair transformation between two species, so this is not a Brønsted-Lowry conjugate pair.
Option 3: ClO4–/ClO3–. These anions differ by oxidation state and structure rather than by proton transfer. There is no Brønsted-Lowry acid–base interconversion between them, so they do not form a conjugate pair.
Option 4: HCl/HBr. Both substances are strong Brønsted-Lowry acids, but the pair does not consist of an acid and its conjugate base. Their conjugate bases would be Cl– and Br–, respectively, not each other’s partners. Therefore this set is not a conjugate acid–base pair.

Chem 1C General Chemis... Self Assessment Quiz 11

Which pair is a Brønsted-Lowry conjugate acid-base pair?

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