Conjugate acid

A conjugate acid is the species formed when a base accepts a proton. It differs from that base by one proton.

Brønsted–Lowry acid–base theory: An acid–base model in which acids donate protons and bases accept them. This theory defines a conjugate acid through the proton a base accepts.
Acid–base reaction: A chemical reaction involving transfer of protons or, in broader theories, electron pairs. Conjugate acids arise within acid–base reactions through proton transfer.
Buffer solution: A solution that resists changes in pH when small amounts of acid or base are added. A weak base and its conjugate acid can form a buffer pair.
Lewis acid: A species that accepts an electron pair to form a coordinate covalent bond. Lewis acidity does not require the proton transfer that defines conjugate acids here.
Protonation: The addition of a proton to an atom, molecule, or ion. Protonation is the process that turns a base into its conjugate acid.
Proton: A positively charged subatomic particle found in atomic nuclei; in chemistry, H⁺ denotes a proton. Accepting this particle is what distinguishes a base from its conjugate acid.
Henderson–Hasselbalch equation: An equation relating buffer pH to the pKa and concentrations of an acid and its conjugate base. Its acid–base pair can be expressed using a conjugate acid and base.
Arrhenius acid: A substance that increases hydrogen-ion concentration in aqueous solution. This narrower aqueous definition does not describe every conjugate-acid relationship.
Conjugate base: The species remaining after an acid donates a proton. It is the paired product formed when a conjugate acid donates its proton.
Acid dissociation constant: The equilibrium constant that quantifies an acid's dissociation in a specified solvent. It measures how readily a conjugate acid gives its proton back.

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