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b(4.5) Preparation of Salts – Reactions with Acids:
Learn these General Equations and their Examples:
1. ACID + METAL –––––––> SALT + HYDROGEN Hydrochloric acid + Magnesium Magnesium Chloride + Hydrogen 2HCl(aq) + 2Mg(s) 2MgCl(aq) + H2(g) Sulphuric acid + Zinc Zinc Sulphate + Hydrogen H2SO4(aq) + Zn(s) ZnSO4(aq) + H2(g) Nitric acid + Aluminium Aluminium Nitrate + Hydrogen 2HNO3(aq) + 2Al(s) 2AlNO3(aq) + H2(g)

2. ACID + BASE –––––––> SALT + WATER
Hydrochloric acid + Copper II Oxide Copper II Chloride + Water
HCl(aq) + CuO(s) CuCl(aq) + H2O(l) Nitric acid + Aluminium Oxide Aluminium Nitrate + Water 6HNO3(aq) + Al2O3(aq) 2Al(NO3)3(aq) + 3H2O(l)

3. ACID + ALKALI –––––––> SALT + WATER Sulphuric acid + Sodium Hydroxide Sodium Sulphate + Water H2SO4(aq) + 2NaOH(aq) Na2SO4(aq) + 2H2O(l) Phosphoric acid + Potassium Hydroxide Potassium Phosphate + Water H3PO4(aq) + 3KOH(aq) K3PO4(aq) + 3H2O(l)

4. ACID + CARBONATE –––––––> SALT + WATER + CARBON DIOXIDE Sulphuric acid + Ammonium Carbonate Ammonium Sulphate + Water + Carbon Dioxide H2SO4(aq) + (NH4)2CO3(aq) (NH4)2SO4(aq) + H2O(l) + CO2(g) Nitric acid + Sodium Carbonate Sodium Nitrate + Water + Carbon Dioxide 2HNO3 (aq) +Na2CO3(aq) 2NaNO3(aq) + H2O(l) + CO2(g) Hydrochloric acid + Magnesium Carbonate Magnesium Chloride + Water + Carbon Dioxide 2HCl(aq)+ MgCO3(aq) MgCl2(aq) + H2O(l) + CO2(g)

(4.6) Solubility of Ionic Compounds – Learn the solubility patterns:

(2.11-2.12) Hydrogen Chloride / Hydrochloric Acid: The Fountain Experiment:
Hydrogen Chloride is a colourless gas, denser than air – collected by downward delivery
It is very highly soluble in water – a polar molecule – as it dissociates into H+ and Cl- ions – cannot be collected over water.
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