1. Double Displacement Reactions & Combustion

2. (c) McGraw Hill Ryerson 2007 When potassium chromate and silver nitrate react, they form a red precipitate, silver chromate, in a solution of potassium nitrate. K 2 CrO 4 (aq) + 2AgNO 3 (aq)  Ag 2 CrO 4 (s) + 2KNO 3 (aq) silver chromate Two solutions react to form a precipitate (solid) and another solution. Ionic solution + ionic solution  ionic solution + ionic solid. AB + CD  AD + CB DOUBLE REPLACEMENT: http://www.youtube.com/watch?v=opY3FLrPTa4

3. Total Ionic Equations  Once you write the molecular equation (synthesis, decomposition, etc.), you should check for reactants and products that are soluble or insoluble.  We usually assume the reaction is in water  We can use a solubility table to tell us what compounds dissolve in water.  If the compound is soluble (does dissolve in water), then splits the compound into its component ions  If the compound is insoluble (does NOT dissolve in water), then it remains as a compound

4. Solubility Table

5. Solubilities Not on the Table!  Gases only slightly dissolve in water  Strong acids and bases dissolve in water  Hydrochloric, Hydrobromic, Hydroiodic, Nitric, Sulfuric, Perchloric Acids  Group I hydroxides (should be on your chart anyway)  Water slightly dissolves in water! (H+ and OH-)  For the homework… SrSO 4 is insoluble; BeI 2 and the products are soluble  There are other tables and rules that cover more compounds than your table!

6. Total Ionic Equations Molecular Equation: K 2 CrO 4 + Pb(NO 3 ) 2  PbCrO 4 + 2 KNO 3 SolubleSolubleInsoluble Soluble Total Ionic Equation: 2 K + (aq) + CrO 4 2- (aq) + Pb 2+ (aq) + 2 NO 3 - (aq)  PbCrO 4 (s) + 2 K + (aq) + 2 NO 3 - (aq)

7. Net Ionic Equations These are the same as total ionic equations, but you should cancel out ions that appear on BOTH sides of the equation Total Ionic Equation: 2 K + + CrO 4 -2 + Pb +2 + 2 NO 3 -  PbCrO 4 (s) + 2 K + + 2 NO 3 - Net Ionic Equation: CrO 4 -2 + Pb +2  PbCrO 4 (s)

8. Net Ionic Equations Try this one! Write the ionic, total ionic, and net ionic equations for this reaction: Silver nitrate reacts with Lead (II) Chloride in hot water. Ionic Equation: Total Ionic: Net Ionic:

9. (c) McGraw Hill Ryerson 2007 Neutralization reactions occur when an acid (most compounds starting with H) and a base (most compounds ending in OH) react to form a salt and water. Acid + base  salt + water HOH HX + MOH  MX + H 2 O where X and M are elements HCl (aq) + NaOH (aq)  NaCl (aq) + H 2 O ( l ) See page 263

10. (c) McGraw Hill Ryerson 2007 1. Sulfuric acid is used to neutralize calcium hydroxide: H 2 SO 4 + Ca(OH) 2  CaSO 4 + 2H 2 O 2. Phosphoric acid helps to neutralize the compounds that cause rust, such as iron(II) hydroxide. H 3 PO 4 + 3Fe(OH) 2  Fe 3 (PO 4 ) 2 + 6H 2 O See page 263 NEUTRALIZATION: http://www.youtube.com/watch?v=_P5hGzA6Vb0

11. (c) McGraw Hill Ryerson 2007 After the double displacement reaction occurs, one of the products quickly decomposes into water and a gas If one of your products is carbonic acid (H 2 CO 3 (aq) ) it will decompose into CO 2 (g) and H 2 O ( l ) If one of your products is ammonium hydroxide (NH 4 OH (aq) ), it will decompose into NH 3 (g) and H 2 O (l) NaHCO 3 (aq) + HCH 3 COO (aq)  NaCH 3 COO + H 2 CO 3 H 2 CO 3 (aq)  CO 2 (g) + H 2 O ( l ) NH 4 Cl (aq) + NaOH (aq)  NH 4 OH (aq) + NaCl (aq) NH 4 OH (aq)  NH 3 (g) + H 2 O ( l ) See page 263

12. Practice Predict the products. Balance the equation 1.HCl (aq) + AgNO 3(aq)  2.CaCl 2(aq) + Na 3 PO 4(aq)  3.Pb(NO 3 ) 2(aq) + BaCl 2(aq)  4.FeCl 3(aq) + NaOH (aq)  5.H 2 SO 4(aq) + NaOH (aq)  6.KOH (aq) + CuSO 4(aq) 