1. Precipitation Reactions ● A reaction in which two solutions are mixed an insoluble solid (precipitate) is formed – Double replacement – ions switch partners ● Remember: always positive- negative combo ● Potassium iodide and lead(II)nitrate

2. Solubility Rules ● Not in reference tables – you need to know just the basics, not all the exceptions (p.121) ● 1. nitrate salts are soluble (NO 3 - ) ● 2. group 1, acetates and ammonium (NH 4 + ) salts are soluble ● 3. most sulfate salts are soluble – Except: Ba 2+, Pb 2+, Hg 1+ and Ca 2+ ● 4. Hydroxide salts are only slightly soluble – NaOH and KOH are soluble (Group I, Sr 2+ and Ba 2+ ) ● 5. sulfide (S 2- ), carbonate (CO 3 2- ), chromate (CrO 4 2- ), phosphate (PO 4 3- ) only slightly soluble

3. Net Ionic Equations ● Write the complete equation, balance, determine solubility ● Write complete ionic equation, separating all aqueous compounds ● Cross out spectator ions, then write what is left, the net ionic equation ● Sodium phosphate and silver nitrate

4. Net Ionic Practice ● Pick any two soluble salts (use rules)