The following rule will help you to predict if ionic precipitation reactions will take place when two solutions are mixed:
- all nitrates are soluble in water
- all chlorides are soluble in water except AgCl and PbCl2
- all sulfates are soluble in water except BaSO4, PbSO4 and SrSO4,
- all sodium, potassium and ammonium salts are soluble in water
- all carbonates are insoluble in water except (NH4)2CO3 and those of group 1 elements.
Neutralisation reactions can also be summariesd using ionic equations. When an acid and alkali react, a covalent compound is formed - in this case water. When hydrochloric acid reacts with sodium hydroxide the ions involves, and the products are:
H+(aq) + Cl-(aq) + Na+(aq) + OH-(aq) -> H20 (l) + Na+(aq) + Cl-(aq)
When the spectator ions have been removed, the ionic equation is:
H+(aq) + OH-(aq) --> H2O(l)
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