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"Acid-base" redirects here. For chemicals that can behave as acids or bases, see Amphoterism.
Acids and bases
Diagrammatic representation of the dissociation of acetic acid in aqueous solution to acetate and hydronium ions.
AcidAcid–base reactionAcid–base homeostasisAcid strengthAcidity functionAmphoterismBaseBuffer solutionsDissociation constantEquilibrium chemistryExtractionHammett acidity functionpHProton affinitySelf-ionization of waterTitrationLewis acid catalysisFrustrated Lewis pairChiral Lewis acid
Acid types
Brønsted–LowryLewisAcceptorMineralOrganicOxideStrongSuperacidsWeakSolid
Base types
Brønsted–LowryLewisDonorOrganicOxideStrongSuperbasesNon-nucleophilicWeak
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An acid–base reaction is a chemical reaction that occurs between an acid and a base. It can be used to determine pH. Several theoretical frameworks provide alternative conceptions of the reaction mechanisms and their application in solving related problems; these are called the acid–base theories, for example, Brønsted–Lowry acid–base theory.
Their importance becomes apparent in analyzing acid–base reactions for gaseous or liquid species, or when acid or base character may be somewhat less apparent. The first of these concepts was provided by the French chemist Antoine Lavoisier, around 1776.[1]
Lewis, Brønsted-Lowery, Arrhenius ways of thinking of Acids and Bases
Acid Base Reaction Theories as superset and subset models.
It is important to think of the acid-base reaction models as theories that complement each other.[2] For example, the current Lewis model has the broadest definition of what an acid and base are, with the Brønsted-Lowry theory being a subset of what acids and bases are, and the Arrhenius theory being the most restrictive.
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