1. Acid-Base reactions CH 3 CO 2 H(aq) + NaOH(aq)  1. CH 3 CO 2 H 2 + (aq) + NaO(aq) 2. CH 3 CO 2 - (aq) + H 2 O(l) + Na + (aq) 3. CH 4 (g) + CO 2 (g) + H2O(l)

2. Acid-Base reactions HCN(aq) + NH 3 (aq)  1. NH 4 + (aq) + CN - (aq) 2. H 2 CN + (aq) + NH 2 - (aq) 3. C 2 N 2 (s) + 3 H 2 (g)

3. Acid-Base Reactions: Find the hidden bases Thing to know: Anions of weak acids are bases. Example: CH 3 COOH = weak acid CH 3 COO - therefore = weak base HCN = weak acid CN - = weak base H 3 PO 4 = weak acid PO 4 3- = weak base

4. Return to Acid-Base Reactions: Find the hidden bases HCl + NaCN  ? HCl + AlPO 4  ? HCl + CaC 2 O 4  ?

6. Precipitation Reactions Solubility of Ionic Compounds dissolving

7. To Determine Solubility: 1. identify the two ions 2. soluble ions with no “exceptions” never form precipitates 3. use listing under soluble/insoluble, but check to see if it’s an exception

8. Examples Soluble or Insoluble? 1.NaNO 3 2.FeCl 3 3.Fe(OH) 3 4.BaSO 4 5.AgNO 3 6.AgCl

9. More Examples Soluble or Insoluble? 1.K 3 PO 4 2.Fe 3 (PO 4 ) 2 3.PbCl 2 4.FeSO 4 5.(NH 4 ) 2 S 6.PbS

10. PRS Example 1 Which of the following is soluble? 1.AlPO 4 2.PbBr 2 3.Al(OH) 3 4.FeSO 4

11. PRS Example 2 Which of the following is insoluble? 1.Al(NO 3 ) 3 2.PbC 2 O 4 3.NaOH 4.FeF 3

12. Precipitation Reactions Net Ionic Equations Pb(NO 3 ) 2 + K 2 CrO 4  ? Pb(NO 3 ) 2 + KI  ? BaCl 2 + KNO 3 

14. Gas Forming Reactions 2 H + + CO 3 2-  CO 2 (g) + H 2 O(l) 2 H + + SO 3 2-  SO 2 (g) + H 2 O(l) 2 H + + M  H 2 (g) + M 2+ (aq) M = metal, like Mg or Fe