Linked from

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

• AmmoniaNarrower topic: Ammonia’s acceptance of a proton makes it a Brønsted–Lowry base.

• Acid dissociation constantNarrower topic: Ka applies the theory’s proton-donor definition to an equilibrium.

• 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.

• Conjugate acid–base pairNarrower topic: It supplies the proton-transfer definition that makes conjugate pairs possible.

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

• Hydrochloric acidNarrower topic: Hydrogen chloride acts as a proton donor when it dissolves in water.

• Acid–base equilibriumNarrower topic: Its proton-transfer definition supplies the framework for describing these equilibria.

• 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.

• Proton transferNarrower topic: Proton transfer is the defining event in a Brønsted–Lowry acid–base reaction.

• ProtonationNarrower topic: Protonation is the proton-accepting half of this model’s acid–base reactions.

• Svante ArrheniusCompared with: It applies beyond aqueous hydrogen- and hydroxide-ion definitions associated with Arrhenius.

• Conjugate acidNarrower topic: This theory defines a conjugate acid through the proton a base accepts.

• Conjugate baseNarrower topic: It defines conjugate bases through the proton donation that forms them.

• Elimination reactionNarrower topic: Many eliminations begin when a base removes a proton from the substrate.

• Lewis baseCompared with: It classifies bases by proton acceptance rather than electron-pair donation.

• Acid catalysisNarrower topic: Acid catalysis proceeds through transfer of the acid’s proton to a reactant.

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

• SuperacidNarrower topic: Superacid strength reflects exceptional ability to donate protons to weak bases.

• HydroniumNarrower topic: Water acts as a base when it accepts a proton to form hydronium.

• Strong acidNarrower topic: Strong-acid dissociation is proton donation to the surrounding solvent.

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

• Weak acidNarrower topic: It defines weak-acid behavior through reversible proton donation.

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

• Hammett acidity functionNarrower topic: H₀ quantifies how strongly a medium can protonate a base.

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

• DeprotonationNarrower topic: Deprotonation is the proton-donation half of a Brønsted–Lowry acid–base reaction.

• Gilbert N. LewisCompared with: Lewis’s electron-pair definition covers reactions that involve no proton transfer.

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

• Acid strengthNarrower topic: Acid strength compares how readily different Brønsted–Lowry acids donate protons.

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

• PhenolphthaleinNarrower topic: It describes the proton transfers that alter phenolphthalein's molecular forms.

• 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.

• Weak baseNarrower topic: It supplies the proton-acceptance definition used for weak bases.

• Carborane acidNarrower topic: Carborane acids exemplify proton donation with minimal interference from the conjugate base.

• EthylamineNarrower topic: Ethylamine acts as a base by accepting a proton from acids.

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

• Sodium amideNarrower topic: It describes sodium amide's proton-accepting behavior directly.

• Triflic acidNarrower topic: Triflic acid catalyzes reactions by donating protons to substrates.

• GuanidineNarrower topic: Guanidine acts as a base by accepting a proton from an acid.

• E1cB elimination reactionNarrower topic: The first step is proton transfer from the substrate to a base.

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

• Lewis acids and basesCompared with: It describes proton-transfer reactions, a narrower scope than Lewis electron-pair exchange.