In terms of acid-base chemistry, what defines a Bronsted-Lowry acid?

A Bronsted-Lowry acid is defined specifically as a substance that donates a proton (H⁺) to another substance in a chemical reaction. This definition is fundamental to understanding acid-base chemistry under the Bronsted-Lowry theory, which focuses on the transfer of protons during reactions.

In a Bronsted-Lowry reaction, when an acid donates a proton, it generates a conjugate base, which is the species that remains after the proton donation. This concept is critical because it allows for the identification of acids and bases not only in aqueous solutions but also in other solvents.

For instance, in the reaction between hydrochloric acid (HCl) and water, HCl donates a proton to the water molecule, forming hydronium (H₃O⁺) and chloride ions (Cl⁻). Here, HCl acts as the Bronsted-Lowry acid because it donates a proton.

Understanding this definition helps in predicting the behavior of various substances in acid-base reactions, assisting in calculations related to pH, determination of equilibria in reactions, and assessing the strength of acids and bases. This core principle is foundational in the study of chemistry and plays a vital role in various applications across chemical research