What is formed when a proton (H⁺) is added to a Bronsted-Lowry base?

When a proton (H⁺) is added to a Brønsted-Lowry base, it results in the formation of a conjugate acid. According to Brønsted-Lowry theory, bases are defined as proton acceptors. When a base accepts a proton, it transforms into its conjugate acid.

For example, if we consider ammonia (NH₃), which acts as a Brønsted-Lowry base when it accepts a proton, it becomes ammonium (NH₄⁺), the conjugate acid. This is a fundamental concept in acid-base chemistry, where the relationship between acids and bases is based on the transfer of protons. Therefore, the addition of H⁺ to a base is the defining action that converts it to its conjugate acid, reinforcing the concept that every Brønsted-Lowry base has a corresponding conjugate acid.