In Bronsted-Lowry theory, what is a Bronsted-Lowry base?

A Bronsted-Lowry base is defined as a species that accepts protons (H⁺ ions) in a chemical reaction. This definition is part of the broader Bronsted-Lowry acid-base theory, which emphasizes the transfer of protons during chemical interactions. When a base encounters a proton donor (an acid), it will accept a proton, leading to the formation of a conjugate acid.

Understanding this concept is crucial because it highlights the dynamic nature of acids and bases, emphasizing their role in chemical reactions beyond just the presence of hydroxide ions or other traditional definitions. The focus here is on proton transfer, which underlies much of acid-base chemistry in various contexts.

In contrast, a proton donor aligns with the definition of an acid, while terms like conjugate acid and strong acid relate to specific behaviors of acids rather than the accepting property that defines bases. Thus, the characterization of a Bronsted-Lowry base revolves fundamentally around its capacity to accept protons in a reaction.