Acids Bases Neutralisation

Acids
1. All contain hydrogen in their formulae
2. When dissolved in water, release hydrogen ions as protons H+ into the solution
3. Hydrogen chloride gas releases H+ ions as is dossolves in water
  1. HCl (g) + aq --> H+ (aq) + Cl- (aq)
Strong and Weak Acids
1. Strong Acid
  1. Releases all its hydrogen atoms into solution as H+ ions
  2. E.g/ Hydrochloric Acid (HCl)
2. Weak Acid
  1. E.g/ Ethanoic Acid (CH3COOH)
  2. Releases only a small proportion of its available hydrogen atoms into solution as H+ ions
Bases and Alkalis
1. Bases
  1. Metal Oxides
  2. Metal Hydroxides
  3. Metal Carbonates
  4. Ammonia (NH3)
  5. A base neutralises an acid to form a salt
2. Alkalis
  1. An alkali is a base that dissolves in water releasing hydroxide ions (OH-) into the solution
  2. Sodium Hydroxide releasing hydroxide ions as it dissolves in water
    1. NaOH (s) + aq --> Na+ (aq) + OH- (aq)
Neutralisation
1. In neutralisation of an acid, H+ ions react with a base to form a salt and neutral water
  1. H+ ions from the acid are replaced by metal or ammonium ions from the base
2. Neutralisation of Acids with Metal Oxides and Hydroxides
  1. Acid + Metal Oxide --> Salt + Water
  2. Acid + Metal Hydroxide --> Salt + Water
  3. Neutralisation of sulphuric acid and hydrochloric acid by Copper(II) oxide to form a salt and water only
    1. CuO (s) + H2SO4 (aq) --> CuSO4 (aq) + H2O (l)
    2. CuO (s) + 2HCl (aq) --> CuCl2 (aq) + H2O (l)
3. Alkalis
  1. Reactants in solution
  2. Acid + Alkali --> Salt + Water
  3. Ionic Equation
    1. H+ (aq) + OH- (aq) --> H2O (l)
4. Neutralisation of acids with Carbonates
  1. Acid + Metal Carbonate --> Salt + Water + Carbon Dioxide
  2. Neutralisation of two carbonates by sulphuric acid and hydrochloric acid
    1. ZnCO3 (s) + H2SO4 --> ZnSO4 + H2O + CO2
    2. MgCO3 + 2HCl (aq) --> MgCl2 (aq) + H2O (l) + CO2 (g)

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Acids Bases Neutralisation

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	Created by Bee Brittain over 8 years ago

	Copied by Jack Ball about 5 years ago