Which term is designated for the transfer of protons in acid-base chemistry?

In acid-base chemistry, the transfer of protons is specifically defined by the Bronsted-Lowry Theory. This theory posits that an acid is a substance that donates a proton (H⁺) to another substance, while a base is a substance that accepts a proton. This concept is critical in understanding how acids and bases interact in various chemical reactions.

The focus on proton transfer distinguishes the Bronsted-Lowry Theory from other theories. For instance, the Arrhenius Theory defines acids as substances that increase the concentration of hydrogen ions in solution and bases as substances that increase the concentration of hydroxide ions, but it does not encompass proton transfer in a broader sense. Similarly, the Lewis Theory is centered around the donation and acceptance of electron pairs rather than protons. The Kinetic Theory is not applicable here, as it deals with the behavior of gases rather than acid-base reactions.

Therefore, the Bronsted-Lowry Theory is the correct term for describing proton transfer in acid-base chemistry, as it specifically identifies the roles of acids and bases based on their ability to donate or accept protons.