Acids and Bases

Acids and Bases

Arrhenius' theory of acids and bases
1. Acid- A substance that dissociates in water to form H+ ions
2. Base-A substance that dissociates in water to form OH- ions
3. Limitations of the Arrhenius Definitions
  1. 1. Acid-Base reactions are considered only in aqueous solutions.
  2. 2. The OH- ion is singled out as a source of the basicity and therefore certain insoluble oxides cannot be classed as Arrhenius bases E.g. CuO
  3. 3. The action of amphoteric species can't be explained
Strong and Weak Acids
1. H2SO4 and HCl are strong acids. A strong acid is one that dissociates (break up) fully in aqueous solution.
2. A weak acid is one that does not dissociate fully in aqueous solution. Examples include Ethanoic Acid and Methanoic acid (Formic acid).
Neutralisation
1. Neutralisation is the reaction between an acid and base to form salt and water.
2. Acid + Base = Salt + Water
  1. HCl + NaOH = NaCl + H2O
3. A salt is a substance formed when the Hydrogen of an acid is replaced by a metal or an ammonium ion
4. Everyday Examples of Neutralisation
  1. Wasp stings are basic They can be neutralised with vinegar or lemon juice
  2. Nettle, bee and ant stings are acidic They can be neutralised with baking soda
Definitions
1. Conjugate acid
  1. An acid changes into a conjugate base when it donates a proton.
2. Conjugate base
  1. A base changes into a conjugate acid when it accepts a proton.
3. Conjugate pair
  1. A conjugate acid-base pair is any pair consisting of an acid and a base which differs by one proton
4. Bronsted Acid
  1. An acid is a proton donor
5. Bronsted Base
  1. A base is a proton acceptor.
6. Amphoteric
  1. A substance that can act as an acid or a base is said to be amphoteric.

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