In a Bronsted-Lowry acid-base reaction, what happens to a proton?

In a Bronsted-Lowry acid-base reaction, the concept revolves around the transfer of protons (H⁺ ions). According to this theory, an acid is defined as a substance that donates a proton, while a base is defined as a substance that accepts a proton.

When the correct answer states that the proton is transferred from acid to base, it emphasizes this fundamental process: the acid donates a proton to the base, resulting in the formation of a conjugate base from the acid and a conjugate acid from the base. This transfer is crucial to understanding acid-base reactions because it highlights how substances interact during the reaction, effectively changing their identity in the process.

This understanding is key in various chemical contexts, including equilibrium, reaction mechanisms, and the behavior of different substances in solution. By recognizing the transfer of the proton, one can better predict the outcomes of reactions and analyze the strength and behavior of acids and bases in different environments.