Linked from

The 47 pages that link to Brønsted–Lowry acid–base theory, each with the reason it gives.

• Acid–base reactionRelated: It describes reactions as proton transfers between an acid and a base.

• EsterificationRelated: Proton transfers activate the carbonyl and alcohol during acid-catalyzed esterification.

• Carbonic acidRelated: It explains why carbonic acid is classified as an acid when it donates protons.

• AmineRelated: Amines act as bases by accepting protons at the nitrogen lone pair.

• AcidRelated: It defines acids through proton transfer between reacting partners.

• HydroxideRelated: Hydroxide acts as a proton acceptor, forming water.

• NeutralizationRelated: Proton transfer explains neutralization for acids and bases that do not produce hydroxide ions directly.

• AmmoniumRelated: It describes ammonia accepting a proton to become ammonium.

• Strong baseRelated: It describes hydroxide formation when a base accepts a proton from water.

• AmphoterismRelated: It explains amphoterism through a substance’s ability to donate or accept a proton.

• Acid–base chemistryRelated: It supplies the proton-transfer definition used to describe most reactions in this field.

• OxyanionRelated: Adding or removing protons interconverts many oxyanions and their conjugate acids.

• Amino groupRelated: The amino nitrogen acts as a Brønsted–Lowry base when its lone pair accepts a proton.

• Universal indicatorRelated: Proton transfer between indicator forms underlies their pH-dependent colors.

• Aluminium hydroxideRelated: In the stomach, aluminium hydroxide consumes protons as it neutralizes gastric acid.

• Mineral acidRelated: It describes proton donation by mineral acids in aqueous reactions.

• HydronRelated: Its central reaction is the transfer of a hydron between chemical species.