Chapter 12: Acids and Bases

Arrhenius acid

substance that produces H+ ions when dissolved in water

Monobasic acid

molecule that releases one H+ ion in aqueous solution

Dibasic acid

molecule that releases two H+ ions in aqueous solution

Arrhenius strong acid

A substance that almost completely dissociates in water to give hydrogen ions

Arrhenius weak acid

A substance that only slightly dissociates in water to give hydrogen ions

Arrhenius base

Produces OH- ions when dissolved in water

Arrhenius strong base

A substance that almost completely dissociates in water to give hydroxide ions

Arrhenius weak base

A substance that only slightly dissociates in water to give hydroxide ions

Arrhenius theory faults

Definitions are restricted to aqueous solutions.

Solvents like ammonia and benzene are excluded from his definitions.

Fails to account for the presence of hydronium ions.

Bronsted-Lowry acid

proton donor

Bronsted-Lowry base

proton acceptor

Bronsted-Lowry strong acid

good proton donor

Bronsted-Lowry weak acid

poor proton donor

Bronsted-Lowry strong base

good proton acceptor

Bronsted-Lowry weak base

poor proton acceptor

amphiprotic

a substance that can act as either an acid or a base

conjugate acid

particle formed when a base gains a hydrogen ion

conjugate base

particle formed when an acid donates a proton

conjugate pair

Any pair consisting of an acid and a base that differ by one proton

a salt

substance formed when the hydrogen ion from an acid is replaced by a metal or an ammonium ion

neutralisation

A reaction of an acid with a base, forming a salt and water

neutralisation examples

Lime is added to acidic soil and Limestone neutralises acidity from acid rain in lakes