The Brnsted-Lowry theory defines a substance that accepts protons. This acceptance is the defining characteristic of this type of compound or ion within this acid-base theory. For example, ammonia (NH3) readily accepts a proton (H+) to form ammonium (NH4+), thus acting as a proton acceptor.
Understanding proton acceptors is crucial in various chemical reactions and biological processes. This concept provides a broader definition of basicity compared to earlier theories, encompassing substances that do not necessarily contain hydroxide ions. This expanded view is beneficial for understanding reactions in non-aqueous solvents and explaining the behavior of many organic compounds. Historically, this definition revolutionized the study of acid-base chemistry by shifting the focus from hydroxide ions to proton transfer.
