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Bronsted-Lowry theory is a fundamental concept in chemistry that describes the behavior of acids and bases. It was developed independently by Johannes Nicolaus Bronsted and Thomas Martin Lowry in the early 20th century. The theory proposes that acids and bases react by transferring protons (H+ ions) between them. This proton transfer leads to the formation of a conjugate acid-base pair.

In the Bronsted-Lowry theory, an acid is defined as a substance that donates a proton (H+), while a base is defined as a substance that accepts a proton. For example, in the reaction between hydrochloric acid (HCl) and water (H2O), HCl donates a proton to H2O, forming the conjugate base Cl- and the conjugate acid H3O+. Conversely, H2O acts as a base by accepting the proton.

The Bronsted-Lowry theory provides a more comprehensive understanding of acid-base reactions compared to the earlier Arrhenius theory, which only considered aqueous solutions and specific types of acids and bases. It applies to a broader range of chemical environments, including non-aqueous solutions and gases. The theory also introduces the concept of conjugate acid-base pairs, which are pairs of substances that differ by a single proton. This concept is crucial for understanding the behavior of acids and bases in various chemical reactions.