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Chemistry

Grade 12: Acids and Bases

TermDefinition
Arrhenius theory Acids produce hydrogen ions (H+/H3O+/hydronium ions) in aqueous solution. Bases produce hydroxide ions (OH-) in aqueous solution.
Lowry-Brønsted theory An acid is a proton (H+ ion) donor. A base is a proton (H+ ion) acceptor.
Strong acids Ionise completely in water to form a high concentration of H3O+ ions.
Weak acids Ionise incompletely in water to form a low concentration of H3O+ ions.
Strong bases Dissociate completely in water to form a high concentration of OH- ions.
Weak bases Dissociate/ionise incompletely in water to form a low concentration of OH- ions.
Concentrated acids/bases Contain a large amount (number of moles) of acid/base in proportion to the volume of water.
Dilute acids/bases Contain a small amount (number of moles) of acid/base in proportion to the volume of water.
Ampholyte Substance that can act as either acid or base.
Hydrolysis The reaction of a salt with water.
Equivalence point of a titration The point at which the acid/base has completely reacted with the base/acid.
Endpoint of a titration The point where the indicator changes colour.
Kw The equilibrium constant for the ionisation of water or the ion product of water or the ionisation constant of water.
Created by: StiKManLabs
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