What characterizes a Bronsted-Lowry base?

A Bronsted-Lowry base is characterized by its ability to accept protons (H⁺ ions) in a chemical reaction. This is fundamental to the Bronsted-Lowry theory of acids and bases, which defines acids as proton donors and bases as proton acceptors. When a base accepts a proton, it often results in the formation of a new species, sometimes referred to as a conjugate acid. For example, when ammonia (NH₃) acts as a Bronsted-Lowry base, it accepts a proton to form ammonium (NH₄⁺). Understanding this concept is crucial when predicting the behavior of substances in chemical reactions and acid-base equilibria.