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12 Acids & Bases

Acids and Bases

TermDefinition
Properties of acids: -sour or tart -conduct electricity in solutions -react with metals to produce hydrogen gas
Properties of bases: -taste bitter and feel slippery -conduct electricity in solutions -react with fats, oils, and waxes
Acidic solutions contain: more H+ than OH-
Basic solutions contain: more OH- than H+
Acids are hydrogen + ion/Proton donors
Bases are hydrogen + ion/Proton accepters
Conjugate acid: an acid that forms when a base gains an H+
Conjugate base: a base that forms when an acid loses an H+
Strong acid: an acid that ionizes completely in a solvent (like HCl)
Examples of strong acids: HCL, H2SO4, HNO3, HCLO4,
Weak acid: an acid that does not completely ionize in a solvent eg CH3COOH
Strong base: a base that completely ionizes in H2O
Weak base: a base that does not completely ionize in H2O
Arrhenius Acid A substance that dissociates in water to produce H+ ions.
Arrhenius Base A substance that dissociates in water to produce OH- ions.
Hydroxonium ion H3O+
Shortcomings of Arrhenius Theory 1.H3O+ ion actually forms not just H+ ion in solution 2. Only applies to aqueous solutions 3. Not all acid base reactions require water eg NH3 + HCl → NH4Cl
Neutralisation is the formation of a salt from an acid and a base
conjugate acid/base pair an acid & base that differ by a proton (H+)
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