Brønsted–Lowry acid–base theory

A theory that defines acids as proton donors and bases as proton acceptors. An acid–base reaction transfers a proton from an acid to a base.

Proton transfer: The movement of a proton from one chemical species to another. It is the defining event in a Brønsted–Lowry acid–base reaction.
Proton: A positively charged subatomic particle found in atomic nuclei and present as a hydrogen ion in many acid–base reactions. The theory’s acid–base role is defined by donation or acceptance of this particle.
pH: A logarithmic measure related to hydrogen-ion activity in a solution. It tracks acidity in water, where acids transfer protons to solvent molecules.
Svante Arrhenius: A Swedish physical chemist who defined acids and bases through their production of hydrogen and hydroxide ions in water. His aqueous definitions were the framework Brønsted and Lowry generalized.
Conjugate acid–base pair: Two species that differ by one proton and act as an acid and its corresponding base. Each proton donation creates the donor’s conjugate base and the acceptor’s conjugate acid.
Hydronium: The H₃O⁺ ion formed when a water molecule accepts a proton. It is the usual representation of the protonated water species in aqueous reactions.
Neutralization: A reaction in which acidic and basic species react, often producing water and a salt. It is a practical outcome of proton transfer between an acid and a base.
Johannes Nicolaus Brønsted: A Danish chemist who independently proposed a proton-transfer definition of acids and bases in 1923. His formulation gives the theory its first name.
Amphoteric substance: A substance that can act as either an acid or a base, depending on its reaction partner. Water demonstrates that proton donation and acceptance depend on the reaction partner.
Hydroxide: The OH⁻ ion, which can accept a proton to form water. It acts as a Brønsted base in many aqueous neutralization reactions.

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