According to Bronsted-Lowry theory, what is the definition of a Bronsted-Lowry acid?

In the Bronsted-Lowry theory of acids and bases, a Bronsted-Lowry acid is defined as a substance that donates a proton (H+) to another substance. This theory expands on the classical definition of acids and bases by focusing on the transfer of protons in chemical reactions.

When a substance donates a proton, it increases the concentration of H+ ions in the solution, thus allowing for the existence of various acid-base reactions that involve the exchange of protons. For instance, in the reaction of hydrochloric acid (HCl) with water, HCl donates a proton to water, forming hydronium ions (H3O+) and chloride ions (Cl-). This characteristic of proton donation is fundamental to the Bronsted-Lowry concept, making it clear that an acid in this context is specifically recognized by its ability to lose H+, distinguishing it from bases, which are defined as proton acceptors.

Other definitions provided do not correctly encapsulate the concept of Bronsted-Lowry acids. A proton acceptor refers to Bronsted-Lowry bases, and neutral substances or electron pair donors relate to other theories of acids and bases, such as Lewis theory. Therefore, understanding the role of proton