1. Predicting Ionic Solubility Precipitation Formation

2. Predicting Ionic Solubility Most Ionic compounds (Salts) are soluble in water, but the degree of solubility is different for different salts. Salts can be described in one of the following categories: Soluble Partly (or Sparingly) Soluble Insoluble

3. Predicting Ionic Solubility A soluble salt can be defined in 2 ways:  Qualitatively: Soluble salts tend to dissolve in aqueous solution in almost unlimited amounts.  Quantitatively : More than 1 g of the salt dissolves in 100 mL of solution. or More than 0.1 mole of the salt will dissolve in 1 L of solution.

4. Predicting Ionic Solubility A partly soluble salt can be defined in 2 ways:  Qualitatively: Partly soluble salts tend to dissolve in aqueous solution but in limited amounts.  Quantitatively : Between 1 g and 0.1g of the salt dissolves in 100 mL of solution. Between 0.1mole and 0.01 mole of the salt will dissolve in 1 L of solution.

5. Predicting Ionic Solubility An insoluble salt can be defined in 2 ways:  Qualitatively: Insoluble salts do not dissolve in aqueous solution in any amount.  Quantitatively : Less than 0.1g of the salt dissolves in 100 mL of solution. Less than 0.01 mole of the salt will dissolve in 1 L of solution.

6. Predicting Solubility - Using the Solubility Chart Using the Solubility Chart, a guided example. Example: Is Calcium carbonate soluble or insoluble? 1.Determine the ions present in this compound: - Ca 2+ and CO 3 2- 2. Look up the anion on the Solubility chart. (in this case CO 3 2- ) 3.Look for the cation (in this case Ca 2+ ) in the two lists:  if the combination of Ca 2+ and CO 3 2- forms a precipitate, the chart will indicate it is insoluble or has low solubility.  if the combination of Ca 2+ and CO 3 2- doesn’t form a precipitate, the chart will indicate it is soluble.

7. Predicting Solubility - Using the Solubility Chart Using the Solubility Chart, a guided example. Example: Is Calcium carbonate soluble or insoluble? 1.Determine the ions present in this compound: 2. Look up the anion on the Solubility chart. (in this case CO 3 2- ) 3.Look for the cation (in this case Ca 2+ ) in the two lists:  if the combination of Ca 2+ and CO 3 2- forms a precipitate, the chart will indicate it is insoluble or has low solubility.  if the combination of Ca 2+ and CO 3 2- doesn’t form a precipitate, the chart will indicate it is soluble.

8. Predicting Solubility - Using the Solubility Chart Using the Solubility Chart, a guided example. Example: Is Calcium carbonate soluble or insoluble? 1.Determine the ions present in this compound: - Ca 2+ and CO 3 2- 2. Look up the anion on the Solubility chart. (in this case CO 3 2- ) 3.Look for the cation (in this case Ca 2+ ) in the two lists:  if the combination of Ca 2+ and CO 3 2- forms a precipitate, the chart will indicate it is insoluble or has low solubility.  if the combination of Ca 2+ and CO 3 2- doesn’t form a precipitate, the chart will indicate it is soluble.

9. Predicting Solubility - Using the Solubility Chart Using the Solubility Chart, a guided example. Example: Is Calcium carbonate soluble or insoluble? 1.Determine the ions present in this compound: - Ca 2+ and CO 3 2- 2. Look up the anion on the Solubility chart. (in this case CO 3 2- ) 3.Look for the cation (in this case Ca 2+ ) in the two lists:  if the combination of Ca 2+ and CO 3 2- forms a precipitate, the chart will indicate it is insoluble or has low solubility.  if the combination of Ca 2+ and CO 3 2- doesn’t form a precipitate, the chart will indicate it is soluble.

10. Predicting Solubility - Using the Solubility Chart Using the Solubility Chart, a guided example. Example: Is Calcium carbonate soluble or insoluble? 1.Determine the ions present in this compound: - Ca 2+ and CO 3 2- 2. Look up the anion on the Solubility chart. (in this case CO 3 2- ) 3.Look for the cation (in this case Ca 2+ ) in the two lists:  if the combination of Ca 2+ and CO 3 2- forms a precipitate, the chart will indicate it is insoluble or has low solubility.  if the combination of Ca 2+ and CO 3 2- doesn’t form a precipitate, the chart will indicate it is soluble.

11. Predicting Solubility - Using the Solubility Chart Using the Solubility Chart, a guided example. Example: Is Calcium carbonate soluble or insoluble? 1.Determine the ions present in this compound: - Ca 2+ and CO 3 2- 2. Look up the anion on the Solubility chart. (in this case CO 3 2- ) 3.Look for the cation (in this case Ca 2+ ) in the two lists: is the combination of Ca 2+ and CO 3 2- in the soluble group? is the combination of Ca 2+ and CO 3 2- in the insoluble group?  if the combination of Ca 2+ and CO 3 2- doesn’t form a precipitate, the chart will indicate it is soluble.

12. Predicting Solubility - Using the Solubility Chart Using the Solubility Chart, a guided example. Example: Is Calcium carbonate soluble or insoluble? 1.Determine the ions present in this compound: - Ca 2+ and CO 3 2- 2. Look up the anion on the Solubility chart. (in this case CO 3 2- ) 3.Look for the cation (in this case Ca 2+ ) in the two lists: is the combination of Ca 2+ and CO 3 2- in the soluble group? NO is the combination of Ca 2+ and CO 3 2- in the insoluble group?  if the combination of Ca 2+ and CO 3 2- doesn’t form a precipitate, the chart will indicate it is soluble.

13. Predicting Solubility - Using the Solubility Chart Using the Solubility Chart, a guided example. Example: Is Calcium carbonate soluble or insoluble? 1.Determine the ions present in this compound: - Ca 2+ and CO 3 2- 2. Look up the anion on the Solubility chart. (in this case CO 3 2- ) 3.Look for the cation (in this case Ca 2+ ) in the two lists: is the combination of Ca 2+ and CO 3 2- in the soluble group? is the combination of Ca 2+ and CO 3 2- in the insoluble group?  if the combination of Ca 2+ and CO 3 2- doesn’t form a precipitate, the chart will indicate it is soluble.

14. Predicting Solubility - Using the Solubility Chart Using the Solubility Chart, a guided example. Example: Is Calcium carbonate soluble or insoluble? 1.Determine the ions present in this compound: - Ca 2+ and CO 3 2- 2. Look up the anion on the Solubility chart. (in this case CO 3 2- ) 3.Look for the cation (in this case Ca 2+ ) in the two lists: is the combination of Ca 2+ and CO 3 2- in the soluble group? is the combination of Ca 2+ and CO 3 2- in the insoluble group? YES  if the combination of Ca 2+ and CO 3 2- doesn’t form a precipitate, the chart will indicate it is soluble.

15. Predicting Solubility - Using the Solubility Chart Using the Solubility Chart, a guided example. Example: Is Calcium carbonate soluble or insoluble? 1.Determine the ions present in this compound: - Ca 2+ and CO 3 2- 2. Look up the anion on the Solubility chart. (in this case CO 3 2- ) 3.Look for the cation (in this case Ca 2+ ) in the two lists: is the combination of Ca 2+ and CO 3 2- in the soluble group? is the combination of Ca 2+ and CO 3 2- in the insoluble group?  The combination of Ca 2+ and CO 3 2- forms a precipitate, the chart indicates it has Low Solubility

16. Predicting Ionic Solubility Use a solubility chart to predict the solubility of the following compounds in water. State whether they are soluble or insoluble in water. Ca(NO 3 ) 2 CuCl 2 KBr(NH 4 ) 2 CO 3 Fe(NO 3 ) 3 Ca(OH) 2 NH 4 CH 3 COOPb(NO 3 ) 4 Ca 3 (PO 4 ) 2 CuCl KCH 3 COOPbCO 3 BaSO 4 AgOH Ag 2 SO 4 Cr(OH) 3

17. Predicting Ionic Solubility Use a solubility chart to predict the solubility of the following compounds in water. State whether they are soluble or insoluble in water. Ca(NO 3 ) 2 soluble CuCl 2 KBr(NH 4 ) 2 CO 3 Fe(NO 3 ) 3 Ca(OH) 2 NH 4 CH 3 COOPb(NO 3 ) 4 Ca 3 (PO 4 ) 2 CuCl KCH 3 COOPbCO 3 BaSO 4 AgOH Ag 2 SO 4 Cr(OH) 3

18. Predicting Ionic Solubility Use a solubility chart to predict the solubility of the following compounds in water. State whether they are soluble or insoluble in water. Ca(NO 3 ) 2 soluble CuCl 2 KBr soluble (NH 4 ) 2 CO 3 Fe(NO 3 ) 3 Ca(OH) 2 NH 4 CH 3 COOPb(NO 3 ) 4 Ca 3 (PO 4 ) 2 CuCl KCH 3 COOPbCO 3 BaSO 4 AgOH Ag 2 SO 4 Cr(OH) 3

19. Predicting Ionic Solubility Use a solubility chart to predict the solubility of the following compounds in water. State whether they are soluble or insoluble in water. Ca(NO 3 ) 2 soluble CuCl 2 KBr soluble (NH 4 ) 2 CO 3 Fe(NO 3 ) 3 soluble Ca(OH) 2 NH 4 CH 3 COOPb(NO 3 ) 4 Ca 3 (PO 4 ) 2 CuCl KCH 3 COOPbCO 3 BaSO 4 AgOH Ag 2 SO 4 Cr(OH) 3

20. Predicting Ionic Solubility Use a solubility chart to predict the solubility of the following compounds in water. State whether they are soluble or insoluble in water. Ca(NO 3 ) 2 soluble CuCl 2 KBr soluble (NH 4 ) 2 CO 3 Fe(NO 3 ) 3 soluble Ca(OH) 2 NH 4 CH 3 COO soluble Pb(NO 3 ) 4 Ca 3 (PO 4 ) 2 CuCl KCH 3 COOPbCO 3 BaSO 4 AgOH Ag 2 SO 4 Cr(OH) 3

21. Predicting Ionic Solubility Use a solubility chart to predict the solubility of the following compounds in water. State whether they are soluble or insoluble in water. Ca(NO 3 ) 2 soluble CuCl 2 KBr soluble (NH 4 ) 2 CO 3 Fe(NO 3 ) 3 soluble Ca(OH) 2 NH 4 CH 3 COO soluble Pb(NO 3 ) 4 Ca 3 (PO 4 ) 2 insoluble CuCl KCH 3 COOPbCO 3 BaSO 4 AgOH Ag 2 SO 4 Cr(OH) 3

22. Predicting Ionic Solubility Use a solubility chart to predict the solubility of the following compounds in water. State whether they are soluble or insoluble in water. Ca(NO 3 ) 2 soluble CuCl 2 KBr soluble (NH 4 ) 2 CO 3 Fe(NO 3 ) 3 soluble Ca(OH) 2 NH 4 CH 3 COO soluble Pb(NO 3 ) 4 Ca 3 (PO 4 ) 2 insoluble CuCl KCH 3 COO soluble PbCO 3 BaSO 4 AgOH Ag 2 SO 4 Cr(OH) 3

23. Predicting Ionic Solubility Use a solubility chart to predict the solubility of the following compounds in water. State whether they are soluble or insoluble in water. Ca(NO 3 ) 2 soluble CuCl 2 KBr soluble (NH 4 ) 2 CO 3 Fe(NO 3 ) 3 soluble Ca(OH) 2 NH 4 CH 3 COO soluble Pb(NO 3 ) 4 Ca 3 (PO 4 ) 2 insoluble CuCl KCH 3 COO soluble PbCO 3 BaSO 4 insoluble AgOH Ag 2 SO 4 Cr(OH) 3

24. Predicting Ionic Solubility Use a solubility chart to predict the solubility of the following compounds in water. State whether they are soluble or insoluble in water. Ca(NO 3 ) 2 soluble CuCl 2 KBr soluble (NH 4 ) 2 CO 3 Fe(NO 3 ) 3 soluble Ca(OH) 2 NH 4 CH 3 COO soluble Pb(NO 3 ) 4 Ca 3 (PO 4 ) 2 insoluble CuCl KCH 3 COO soluble PbCO 3 BaSO 4 insoluble AgOH Ag 2 SO 4 insoluble Cr(OH) 3

25. Predicting Ionic Solubility Use a solubility chart to predict the solubility of the following compounds in water. State whether they are soluble or insoluble in water. Ca(NO 3 ) 2 soluble CuCl 2 soluble KBr soluble (NH 4 ) 2 CO 3 Fe(NO 3 ) 3 soluble Ca(OH) 2 NH 4 CH 3 COO soluble Pb(NO 3 ) 4 Ca 3 (PO 4 ) 2 insoluble CuCl KCH 3 COO soluble PbCO 3 BaSO 4 insoluble AgOH Ag 2 SO 4 insoluble Cr(OH) 3

26. Predicting Ionic Solubility Use a solubility chart to predict the solubility of the following compounds in water. State whether they are soluble or insoluble in water. Ca(NO 3 ) 2 soluble CuCl 2 soluble KBr soluble (NH 4 ) 2 CO 3 soluble Fe(NO 3 ) 3 soluble Ca(OH) 2 NH 4 CH 3 COO soluble Pb(NO 3 ) 4 Ca 3 (PO 4 ) 2 insoluble CuCl KCH 3 COO soluble PbCO 3 BaSO 4 insoluble AgOH Ag 2 SO 4 insoluble Cr(OH) 3

27. Predicting Ionic Solubility Use a solubility chart to predict the solubility of the following compounds in water. State whether they are soluble or insoluble in water. Ca(NO 3 ) 2 soluble CuCl 2 soluble KBr soluble (NH 4 ) 2 CO 3 soluble Fe(NO 3 ) 3 soluble Ca(OH) 2 insoluble NH 4 CH 3 COO soluble Pb(NO 3 ) 4 Ca 3 (PO 4 ) 2 insoluble CuCl KCH 3 COO soluble PbCO 3 BaSO 4 insoluble AgOH Ag 2 SO 4 insoluble Cr(OH) 3

28. Predicting Ionic Solubility Use a solubility chart to predict the solubility of the following compounds in water. State whether they are soluble or insoluble in water. Ca(NO 3 ) 2 soluble CuCl 2 soluble KBr soluble (NH 4 ) 2 CO 3 soluble Fe(NO 3 ) 3 soluble Ca(OH) 2 insoluble NH 4 CH 3 COO soluble Pb(NO 3 ) 4 soluble Ca 3 (PO 4 ) 2 insoluble CuCl KCH 3 COO soluble PbCO 3 BaSO 4 insoluble AgOH Ag 2 SO 4 insoluble Cr(OH) 3

29. Predicting Ionic Solubility Use a solubility chart to predict the solubility of the following compounds in water. State whether they are soluble or insoluble in water. Ca(NO 3 ) 2 soluble CuCl 2 soluble KBr soluble (NH 4 ) 2 CO 3 soluble Fe(NO 3 ) 3 soluble Ca(OH) 2 insoluble NH 4 CH 3 COO soluble Pb(NO 3 ) 4 soluble Ca 3 (PO 4 ) 2 insoluble CuCl insoluble KCH 3 COO soluble PbCO 3 BaSO 4 insoluble AgOH Ag 2 SO 4 insoluble Cr(OH) 3

30. Predicting Ionic Solubility Use a solubility chart to predict the solubility of the following compounds in water. State whether they are soluble or insoluble in water. Ca(NO 3 ) 2 soluble CuCl 2 soluble KBr soluble (NH 4 ) 2 CO 3 soluble Fe(NO 3 ) 3 soluble Ca(OH) 2 insoluble NH 4 CH 3 COO soluble Pb(NO 3 ) 4 soluble Ca 3 (PO 4 ) 2 insoluble CuCl insoluble KCH 3 COO soluble PbCO 3 insoluble BaSO 4 insoluble AgOH Ag 2 SO 4 insoluble Cr(OH) 3

31. Predicting Ionic Solubility Use a solubility chart to predict the solubility of the following compounds in water. State whether they are soluble or insoluble in water. Ca(NO 3 ) 2 soluble CuCl 2 soluble KBr soluble (NH 4 ) 2 CO 3 soluble Fe(NO 3 ) 3 soluble Ca(OH) 2 insoluble NH 4 CH 3 COO soluble Pb(NO 3 ) 4 soluble Ca 3 (PO 4 ) 2 insoluble CuCl insoluble KCH 3 COO soluble PbCO 3 insoluble BaSO 4 insoluble AgOH insoluble Ag 2 SO 4 insoluble Cr(OH) 3

32. Predicting Ionic Solubility Use a solubility chart to predict the solubility of the following compounds in water. State whether they are soluble or insoluble in water. Ca(NO 3 ) 2 soluble CuCl 2 soluble KBr soluble (NH 4 ) 2 CO 3 soluble Fe(NO 3 ) 3 soluble Ca(OH) 2 insoluble NH 4 CH 3 COO soluble Pb(NO 3 ) 4 soluble Ca 3 (PO 4 ) 2 insoluble CuCl insoluble KCH 3 COO soluble PbCO 3 insoluble BaSO 4 insoluble AgOH insoluble Ag 2 SO 4 insoluble Cr(OH) 3 insoluble

33. General Solubility Rules (Time savers) Nitrates (NO 3 1- ) soluble with all cations. Ammonium (NH 4 1+ ) soluble with all anions. Alkali Metals (Li 1+, Na 1+, K 1+,…) soluble with all anions.

34. Predicting the Precipitate that Forms in a Chemical Reaction In a chemical reaction between two Ionic solutions, a precipitate may form. If a precipitate forms, one of the products of the reaction is the precipitate, in other words, it is insoluble and it is a solid. We can predict which product forms the precipitate if we have a solubility chart handy.

35. Predicting the Precipitate that Forms in a Chemical Reaction For example, When a solution of Potassium iodide [KI (aq) ] reacts with a solution of Lead (II) nitrate [Pb(NO 3 ) 2 (aq) ], a yellow precipitate forms. This reaction can be described in words: Potassium iodide solution reacts with Lead (II) nitrate solution to form Potassium nitrate with Lead (II) iodide. One of the products is insoluble (the yellow precipitate)

36. Predicting the Precipitate that Forms in a Chemical Reaction First Step: Write out the Balanced Reaction Equation: 2KI (aq) + 1Pb(NO 3 ) 2(aq)  2KNO 3(?) + 1PbI 2(?) Second step: Determine which product is insoluble: Name of productFormulaSolubility Potassium nitrate Lead (II) iodide

37. Predicting the Precipitate that Forms in a Chemical Reaction First Step: Write out the Balanced Reaction Equation: 2KI (aq) + 1Pb(NO 3 ) 2(aq)  2KNO 3(?) + 1PbI 2(?) Second step: Determine which product is insoluble: Name of productFormulaSolubility Potassium nitrate KNO 3 Lead (II) iodide PbI 2

38. Predicting the Precipitate that Forms in a Chemical Reaction First Step: Write out the Balanced Reaction Equation: 2KI (aq) + 1Pb(NO 3 ) 2(aq)  2KNO 3(?) + 1PbI 2(?) Second step: Determine which product is insoluble: Name of productFormulaSolubility Potassium nitrate KNO 3 Soluble - ie (aq) Lead (II) iodide PbI 2

39. Predicting the Precipitate that Forms in a Chemical Reaction First Step: Write out the Balanced Reaction Equation: 2KI (aq) + 1Pb(NO 3 ) 2(aq)  2KNO 3(?) + 1PbI 2(?) Second step: Determine which product is insoluble: Name of productFormulaSolubility Potassium nitrate KNO 3 Soluble - ie (aq) Lead (II) iodide PbI 2 Insoluble - ie (s)

40. Predicting the Precipitate that Forms in a Chemical Reaction The Total Ionic Equation shows all of the ions present in the two solutions, and which ones form the precipitate. When writing this equation, you must balance the atoms and the charges, you must also indicate which species are (aq) and which, if any forms the precipitate (s). 2K 1+ (aq) + 2I 1- (aq)

41. Predicting the Precipitate that Forms in a Chemical Reaction The Total Ionic Equation shows all of the ions present in the two solutions, and which ones form the precipitate. When writing this equation, you must balance the atoms and the charges, you must also indicate which species are (aq) and which, if any forms the precipitate (s). 2K 1+ (aq) + 2I 1- (aq) + 1Pb 2+ (aq) + 2NO 3 1- (aq) 

42. Predicting the Precipitate that Forms in a Chemical Reaction The Total Ionic Equation shows all of the ions present in the two solutions, and which ones form the precipitate. When writing this equation, you must balance the atoms and the charges, you must also indicate which species are (aq) and which, if any forms the precipitate (s). 2K 1+ (aq) + 2I 1- (aq) + 1Pb 2+ (aq) + 2NO 3 1- (aq)  2K 1+ (aq) + 2NO 3 1- (aq)

43. Predicting the Precipitate that Forms in a Chemical Reaction The Total Ionic Equation shows all of the ions present in the two solutions, and which ones form the precipitate. When writing this equation, you must balance the atoms and the charges, you must also indicate which species are (aq) and which, if any forms the precipitate (s). 2K 1+ (aq) + 2I 1- (aq) + 1Pb 2+ (aq) + 2NO 3 1- (aq)  2K 1+ (aq) + 2NO 3 1- (aq) + 1PbI 2(s)

44. Predicting the Precipitate that Forms in a Chemical Reaction The Net Ionic Equation demonstrates only the ions that form the precipitate. To show the Net Ionic Equation, you get rid of Spectator Ions – ions that do not take part in the reaction (ie., they appear the same on the reactant side as they do on the product side.) 2K 1+ (aq) + 2I 1- (aq) + 1Pb 2+ (aq) + 2NO 3 1- (aq)  2K 1+ (aq) + 2NO 3 1- (aq) + 1PbI 2(s)

45. Predicting the Precipitate that Forms in a Chemical Reaction The Net Ionic Equation demonstrates only the ions that form the precipitate. To show the Net Ionic Equation, you get rid of Spectator Ions – ions that do not take part in the reaction (ie., they appear the same on the reactant side as they do on the product side.) 2K 1+ (aq) + 2I 1- (aq) + 1Pb 2+ (aq) + 2NO 3 1- (aq)  2K 1+ (aq) + 2NO 3 1- (aq) + 1PbI 2(s)

46. Predicting the Precipitate that Forms in a Chemical Reaction The Net Ionic Equation demonstrates only the ions that form the precipitate. To show the Net Ionic Equation, you get rid of Spectator Ions – ions that do not take part in the reaction (ie., they appear the same on the reactant side as they do on the product side.) 2K 1+ (aq) + 2I 1- (aq) + 1Pb 2+ (aq) + 2NO 3 1- (aq)  2K 1+ (aq) + 2NO 3 1- (aq) + 1PbI 2(s)

47. Predicting the Precipitate that Forms in a Chemical Reaction The Net Ionic Equation demonstrates only the ions that form the precipitate. To show the Net Ionic Equation, you get rid of Spectator Ions – ions that do not take part in the reaction (ie., they appear the same on the reactant side as they do on the product side.) Simplified and rearranged: 1Pb 2+ (aq) + 2I 1- (aq)  1PbI 2(s)

48. Summary - Big Ideas Some double displacement reactions form precipitates. Precipitates form in double displacement reactions between two ionic solutions. Precipitates are insoluble ionic compounds, and do not dissolve. A net ionic equation demonstrates only the ions that react.

49. Any Questions?