1. Unit 9 Part II Precipitation

2. Formation of a solid: AgCl AgNO 3 (aq) + KCl(aq)  KNO 3 (aq) + AgCl(s)

3. Solubility Rules 1. Most nitrates are soluble. 2. Most salts containing Group I ion and ammonium ion, NH 4 +, are soluble. 3. Most chloride, bromide, and iodide salts are soluble, except Ag +, Pb 2+ and Hg 2 2+. Ohn-Sabatello, Morlan, Knoespel, Fast Track to a 5 Preparing for the AP Chemistry Examination 2006, page 91 4. Most sulfate salts are soluble, except BaSO 4, PbSO 4, Hg 2 SO 4, and CaSO 4. 5. Most hydroxides except Group 1 and Ba(OH) 2, Sr(OH) 2, and Ca(OH) 2 are only slightly soluble. 6. Most sulfides, carbonates, chromates, and phosphates are only slightly soluble.

4. Copyright © 2007 Pearson Benjamin Cummings. All rights reserved. PbI 2 K 1+ Pb 2+ lead (II) chloride + potassium iodide Cl 2 I Pb 2+ Pb K 1+ K Cl 1- I 1- Cl 1- I 1- KCl potassium chloride lead (II) iodide + (aq) (ppt) + +

5. Copyright © 2007 Pearson Benjamin Cummings. All rights reserved. PbI 2 K 1+ Pb 2+ lead (II) chloride + potassium iodide Cl 2 I Pb 2+ Pb K 1+ K Cl 1- I 1- Cl 1- I 1- KCl potassium chloride lead (II) iodide + (aq) (ppt) + +

6. FeCO 3 Na 1+ Fe 2+ iron (II) chloride + sodium carbonate Cl 2 Using a SOLUBILITY TABLE: sodium chloride is soluble iron (II) carbonate is insoluble CO 3 Fe 2+ Fe Na 1+ Na 2 Cl 1- CO 3 2- Cl 1- CO 3 2- NaCl sodium chloride iron (II) carbonate + (aq) (ppt) 2 FeCl 2 Na 2 CO 3 NaCl FeCO 3 (aq) (ppt) ++ Predict if a reaction will occur when you combine aqueous solutions of iron (II) chloride with aqueous sodium carbonate solution. If the reaction does occur, write a balanced chemical equation showing it. (be sure to include phase notation) (aq) Balanced chemical equation Complete Ionic Equation Fe 2+ (aq) + 2Cl 1- (aq) + 2Na 1+ (aq) + CO 3 2- (aq) 2Na 1+ (aq) + 2Cl 1- (aq) + FeCO 3 (s)