Summary
Summary Topic 5 - Acid-Base Equilibria
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These are the complete notes for the CCEA A2 1 specification and have been created through multiple sources. However, they are not endorsed by CCEA.
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ChemistryTopic 5: Acid-Base Equilibria
Recap
Acid + metal salt + hydrogen
Acid + base salt + water
Acid + alkali salt + water
Acid + carbonate salt + water + carbon dioxide
Brønsted-Lowry acid is a proton (H+), donor
Brønsted-Lowry base is a proton (H+), acceptor
HCl – monobasic
H2SO4 – Dibasic
H3PO4 – Tribasic
Conjugate acid-base pairs
An acid is related to its conjugate base by the fact that the acid has one more hydrogen ion than its
conjugate base.
A base is related to its conjugate acid H3O+ by the fact that the base has one hydrogen ion less than its
conjugate acid.
Example
H2O + HCl ⇌ H3O+ + Cl-
Acid -----> conjugate base
Base ----------> conjugate acid
Acid Conjugate base Base Conjugate acid
H2SO4 HSO4- NH3 NH4+
HNO3 NO3- H2O H3O+
H2O OH- HSO4- H2SO4-
CH3CO2H CH3CO2- SO42- HSO4-
An acid-base pair is a pair of two species that transform into each other by gain or loss of a proton.
The acidity of a solution depends on the concentration of [H + (aq)] and is measured on the pH scale.
pH = -log[H+(aq)]
The relationship between pH and [H+(aq)] has a ‘see-saw’ relationship – when one goes up, the other goes
down. A low pH means a high [H+(aq)] and vice versa.
Strong and weak acids
The strength of an acid HA is the extent of its dissociation of H + and A- ions.
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