This is a comprehensive package of acids and bases examined in the final IEB school exams at the end of grade 12. It includes all the basic principles learnt in grade 11 but focuses on the necessary theory for matric chemistry. Each document is typed in a column format to help simplify the work, an...
Acids and Bases
Acids Bases
Sour taste. Bitter taste & feel soapy.
Influence colour of indictors. Influence colour of indictors.
Increases concentration of H+ -ions / Increase concentration of hydroxide
H3O+ -ions in sol. ions (OH−) in sol / decreases
Conduct electricity in aqueous sols (= hydronium ion (H3O+) concentration in
electrolyte in solution). sol.
React w/ water 2 prod hydronium ions: An alkali conducts electricity in
H+ + H2O → H3O+ aqueous solutions (is an electrolyte in
Acid + Metal → Salt + H2 solutions) due 2 ions moving freely in
Acid + Carbonate → Salt +H2O+CO2(g) sol.
Acid + Base → A base that dissolves in H2O = alkali.
Salt + H2O (Neutralisation) Some bases such as CuO & CaCO3 =
insoluble in water.
Must Know
Must Know
Hydrochloric acid HCℓ
• Strong Sodium carbonate/washing soda
• Na2CO3
Stomach acid,
• • Weak, Production of glass
swimming pool acid,
• Soldering Sodium bicarbonate/baking
Nitric acid 𝑯𝑵𝑶𝟑 soda NaHCO3
• Strong • Weak, Causes dough 2 rise
• Fertilisers, Sodium hydroxide/caustic soda
• Explosives NaOH
Sulphuric acid 𝑯𝟐𝑺𝑶𝟒 • Strong
• Strong • Production of soap, Drain cleaner
• Used in industries, Ammonia NH3
• Gold extraction, • Weak, Cleaning agents
• Dehydrating agent Potassium hydroxide/ caustic
Phosphoric acid 𝑯𝟑𝑷𝑶𝟒 potash KOH
• Strong • Strong
• Adds taste 2 gaseous cold drinks, • Production of soap, Electrolytes in
• Dental cement cells, Production of biodiesel
Carbonic acid 𝑯𝟐𝑪𝑶𝟑 Calcium carbonate CaCO3
• Weak • Weak,
• Gaseous cold drinks • Production of cement
Ethanoic acid 𝑪𝑯𝟑𝑪𝑶𝑶𝑯 Calcium hydroxide Ca(OH)2
• Weak • Strong
• Vinegar • Neutralises acidic soil
Oxalic acid (COOH)2 Magnesium hydroxide Mg(OH)2
• Weak • Strong
• Bleaching agents • Antacids
, Ionization of Acids Acid-Base Models
Acids ionize in water. Arrhenius Theory
Bcz = molecular compound does not An Arrhenius acid releases H+ -ions in
contain ions. aqueous solutions.
When dissolves in water, water HCℓ → H+ + Cℓ−
molecule remove proton thereby An Arrhenius base releases OH− -ions
creating ionic substance. in aqueous solutions.
Hydrochloric acid in water: NaOH → Na+ + OH−
HCℓ(g) + H2O(ℓ) ⇋ H3O+(aq) + Cℓ−(aq)
Sulphuric acid in water:
Brønsted-Lowry Theory
H2SO4(g) + 2H2O(ℓ) ⇋ 2H3O+(aq) + SO42−(aq) A Brønsted-Lowry acid = proton
Dissociation of Bases donor.
Most bases dissociate= breaks up in2 HCℓ → H+ + Cℓ−
ions w/e dissolved in water. NH4+ → H+ + NH3
The ions = already present b4 sub A Brønsted-Lowry base = proton
added 2 water & merely separate from acceptor.
e/o. OH− + H+ → H2O
Sodium hydroxide in water: Conjugate Acid-Base Pairs
NaOH(s) → Na+(aq) + OH−(aq) An acid-base reaction = reaction in
*Exception is NH3. Because it is which there = transfer of proton (H+)
molecular it will ionize in water* from acid to base & = called protolytic
Ammonia in water: reaction.
NH3(g) + H2O(ℓ) ⇋ NH4+(aq) + OH−(aq) Conjugated Bases
(Ionisation)
W/e acid donates proton (H+), a
Mono and Polyprotic Acids conjugated base is produced.
Some acids = only 1 proton (H+) 2 Acid ⇌ Conjugated Base + H+
donate while oths have more. Strong acid always produces weak
Acids = classified acc 2 # protons (H+) conjugate base.
can donate. HCℓ ⇌ H+ + Cℓ−
Monoprotic Acids Strong acid weak conjugated base
Can only donate 1 proton (H+) per H2CO3 ⇌ H+ + HCO3-
Weak acid strong conjugated base
formula unit.
Conjugated Acids
HCℓ, HNO3, CH3COOH
W/e base receives proton (H+), a
Polyprotic Acids
conjugated acid = produced.
Can donate more than 1 proton (H+)
Base + H+ ⇌ Conjugated Acid
per formula unit.
The strong base always produces a
• Diprotic acids weak conjugated acid
Can donate 2 protons (H+) per formula OH− + H+ ⇌ H2O
unit. H2SO4, H2CO3 Strong base Weak conjugated acid
• Triprotic acids HSO4 − + H+ ⇌ H2SO4
Can donate 3 protons (H+) per formula Weak base Strong conjugated acid
unit. H3PO4
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