Conjugate base

A conjugate base is the species formed when an acid donates a proton. It can accept a proton to regenerate that acid.

Brønsted–Lowry acid–base theory: A theory defining acids as proton donors and bases as proton acceptors. It defines conjugate bases through the proton donation that forms them.
Proton: A positively charged subatomic particle found in atomic nuclei; in chemistry, H⁺ denotes a hydrogen nucleus. The proton is the particle lost when a conjugate base forms.
Buffer solution: A solution that resists changes in pH when limited acid or base is added. A weak acid and its conjugate base jointly resist pH changes.
Base: A substance that accepts protons under Brønsted–Lowry theory or donates electron pairs under Lewis theory. A conjugate base is a specific base defined by the acid that produced it.
Proton transfer: The movement of a proton from one chemical species to another. An acid forms its conjugate base by transferring a proton away.
Chemical species: A distinct chemical entity, such as an atom, molecule, ion, or radical. A conjugate base is identified as a species with a particular composition and charge.
Acid dissociation constant: The equilibrium constant describing an acid's dissociation into a proton and its conjugate base. Its value quantifies how readily an acid forms its conjugate base.
Conjugate acid–base pair: Two species that differ by one proton and interconvert through proton transfer. The pair places a conjugate base alongside the acid from which it formed.
Conjugate acid: The species formed when a base accepts a proton. It is the paired species on the base side of a proton-transfer reaction.
Chemical equilibrium: A dynamic state in which forward and reverse reaction rates are equal. Acids and conjugate bases coexist at equilibrium in reversible proton-transfer reactions.

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