Final answer:
In the net ionic equation F⁻ + HSO₃⁻ ⇌ HF, F⁻ functions as a Brønsted-Lowry base and HSO₃⁻ functions as a Brønsted-Lowry acid.
Step-by-step explanation:
In the net ionic equation F⁻ + HSO₃⁻ ⇌ HF, F⁻ functions as a Brønsted-Lowry base and HSO₃⁻ functions as a Brønsted-Lowry acid.
A Brønsted-Lowry acid is a compound that donates a proton (H+) to another compound, while a Brønsted-Lowry base is a compound that accepts a proton. In this equation, F⁻ accepts a proton from HSO₃⁻, therefore acting as a base, while HSO₃⁻ donates a proton to F⁻, acting as an acid.
This reaction involves the transfer of protons between the reactants, resulting in the formation of the conjugate acid of the base and the conjugate base of the acid.
Learn more about Brønsted-Lowry Acids and Bases