1. Precipitation Reactions

2. Precipitation When two aqueous solutions combine to form an insoluble or only slightly soluble salt

3. Solubility Rules Memorize: sodium, potassium, ammonium and nitrate always soluble

4. Is Each Soluble? AgNO 3 KCl K 2 CrO 4 AgCl Ba(OH) 2 CaS NaOH

5. Double Replacement Reactions Ions trade places AX + BY  AY + BX

6. What Will Occur In Each? If a precipitate forms underline KNO 3 + BaCl 2 Na 2 SO 4 + Pb(NO 3 ) 2 KOH + Fe(NO 3 ) 3

7. Net Ionic Equations Strong electrolytes are represented as ions in aqueous solution Spectator ions (not part of the reaction) cancel out What is left behind is called the net ionic equation

8. For each below write the molecular equation, complete ionic equation, and net ionic equation Aqueous potassium chloride is added to aqueous silver nitrate Aqueous potassium hydroxide is mixed with aqueous iron (III) nitrate

9. Net Ionic also applies to Single Replacement Sodium metal is dropped into cold water Lithium metal is dropped into a solution of zinc nitrate

10. Stoichiometry Calculate the mass of NaCl that must be added to 1.50L of a.100M AgNO 3 solution to precipitate all of the Ag + ions

11. Calculate the mass of precipitate formed when 1.25L of a.0500M lead nitrate solution is mixed with 2.00L of a.0250M sodium sulfate solution