Identify the stronger base in each of the following pairs.
Explain your reasoning.
(a) ClO₂^- or ClO₃^-
(b) HSO₄^- or HSeO₄^-

Acid-base theory explains the behavior of acids and bases in chemical reactions. According to the Brønsted-Lowry theory, acids are proton donors and bases are proton acceptors. Understanding this concept is crucial for determining the strength of a base, as stronger bases are more effective at accepting protons.

Conjugate acid-base pairs consist of two species that differ by the presence or absence of a proton (H+). When a base accepts a proton, it forms its conjugate acid. Analyzing the conjugate pairs helps in understanding which base is stronger, as the strength of a base is inversely related to the strength of its conjugate acid.

Electronegativity refers to the tendency of an atom to attract electrons in a bond. In the context of oxyanions like ClO2- and ClO3-, the stability of the resulting conjugate acids (HClO2 and HClO3) is influenced by the electronegativity of the central atom and the number of oxygen atoms. A more stable conjugate acid indicates a weaker base, thus helping to identify the stronger base in the pair.