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Mind Map by Rhea Hogben, updated more than 1 year ago
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Created by Bee Brittain
about 8 years ago
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Copied by Rhea Hogben
about 7 years ago
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4.1 Acids, Bases and Neutralisation
- Acids
- All contain hydrogen in their
formulae
- When dissolved in water, release hydrogen ions as protons H+ into the
solution
- Hydrogen chloride gas releases H+ ions as is dossolves in
water
- HCl (g) + aq --> H+ (aq) + Cl-
(aq)
- HCl (g) + aq --> H+ (aq) + Cl-
(aq)
- All contain hydrogen in their
formulae
- Strong and Weak
Acids
- Strong Acid
- Releases all its hydrogen atoms into solution as H+
ions
- Fully
Dissociates
- E.g/ Hydrochloric Acid
(HCl)
- Releases all its hydrogen atoms into solution as H+
ions
- Weak
Acid
- E.g/ Ethanoic Acid
(CH3COOH)
- Releases only a small proportion of its
available hydrogen atoms into solution as H+
ions
- Partially
Dissociates
- E.g/ Ethanoic Acid
(CH3COOH)
- Strong Acid
- Bases and Alkalis
- Bases
- Metal Oxides
- Metal Hydroxides
- Metal Carbonates
- Ammonia (NH3)
- A base neutralises an acid to form a
salt
- Metal Oxides
- Alkalis
- An alkali is a base that dissolves in water releasing
hydroxide ions (OH-) into the solution
- Sodium Hydroxide releasing hydroxide ions as it dissolves in
water
- NaOH (s) + aq --> Na+ (aq) + OH-
(aq)
- NaOH (s) + aq --> Na+ (aq) + OH-
(aq)
- An alkali is a base that dissolves in water releasing
hydroxide ions (OH-) into the solution
- Bases
- Neutralisation
- In neutralisation of an acid, H+ ions react with a base to form a salt and neutral water
- H+ ions from the acid are replaced by metal or ammonium ions from the base
- H+ ions from the acid are replaced by metal or ammonium ions from the base
- Neutralisation of Acids with Metal Oxides and Hydroxides
- Acid + Metal Oxide --> Salt + Water
- Acid + Metal Hydroxide --> Salt + Water
- Neutralisation of sulphuric acid and hydrochloric acid by Copper(II) oxide
to form a salt and water only
- CuO (s) + H2SO4 (aq) --> CuSO4 (aq) + H2O (l)
- CuO (s) + 2HCl (aq) --> CuCl2 (aq) + H2O (l)
- CuO (s) + H2SO4 (aq) --> CuSO4 (aq) + H2O (l)
- Acid + Metal Oxide --> Salt + Water
- Alkalis
- Reactants in solution
- Acid + Alkali --> Salt + Water
- Ionic Equation
- H+ (aq) + OH- (aq) --> H2O (l)
- H+ (aq) + OH- (aq) --> H2O (l)
- Reactants in solution
- Neutralisation of acids with Carbonates
- Acid + Metal Carbonate --> Salt + Water + Carbon Dioxide
- Neutralisation of two carbonates by sulphuric acid and hydrochloric acid
- ZnCO3 (s) + H2SO4 --> ZnSO4 + H2O + CO2
- MgCO3 + 2HCl (aq) --> MgCl2 (aq) + H2O (l) + CO2 (g)
- ZnCO3 (s) + H2SO4 --> ZnSO4 + H2O + CO2
- Acid + Metal Carbonate --> Salt + Water + Carbon Dioxide
- In neutralisation of an acid, H+ ions react with a base to form a salt and neutral water
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