An acid is a chemical compound which when dissolved in water gives a pH reading of under 7. This is due to the hydrogen ions which are part of the compound. This means that acids are defined as proton donors.
The Brønsted - Lowry theory of Acids and BasesEdit
This states that acids are proton donors, while bases are proton acceptors which accept a proton (or hydrogen ion) from an acid. It had previously been thought that it was the oxygen in an acid that made it an acid.
Acid + MetalEdit
Acids react with a metal to form hydrogen gas and a salt. Bubbles will be given off - the hydrogen.
- Ionic Equation: 2H+ + 2e- --> 2H2. Note that the 2 electrons come from the metal.
- Overall Equation: Acid + Metal --> Hydrogen + Salt
- Example: hydrochloric acid + magnesium --> hydrogen + magnesium chloride
- Symbol Equation: 2HCl (aq) + Mg (s) --> H2 (g) + MgCl2 (aq)
Acid + CarbonateEdit
Acids react with metal carbonates, forming carbon dioxide, water and a salt. Bubbling is seen (this is the carbon dioxide).
- Ionic Equation: 2H+ + CO3 --> CO2 + H2O.
- Overall Equation: Acid + Metal Carbonate --> Water + Carbon Dioxide + Salt
- Example: hydrochloric acid + magnesium carbonate --> water + magnesium chloride + carbon dioxide
- Symbol Equation: 2HCl + MgCO3 --> H2O + MgCl2 + CO2
Acid + BaseEdit
Acids react with bases to form a salt and water. This reaction is exothermic.
- Ionic Equation: H+ + OH- --> H2O
- Overall Equation: Acid + Base --> Water + Salt
- Example: hydrochloric acid + magnesium hydroxide --> water + magnesium chloride
- Symbol Equation: 2HCl + Mg(OH)2 --> 2H2O + MgCl2
Strong and weak acidsEdit
The 'strength' of an acid is whether it completely dissociates (or ionises) when dissolved in water. Acids which totally dissociate are called strong acids, while ones where some molecules remain un-ionised are called weak acids.
Strong acids include hydrochloric acid, sulphuric acid and nitric acid. A weak acid is ethanoic acid.