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Solutions and Solubility

Solutions and Solubility. 7.3 Reactions in Solution. Predicting Ionic Solubility. m ost 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: s oluble

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Solutions and Solubility

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  1. Solutions and Solubility 7.3 Reactions in Solution

  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. REVIEW: Predicting IONIC SOLUBILITY • In a chemical reaction between two Ionic solutions, a precipitatemay form. • If a precipitate forms, one of the products of the reaction is the precipitate, in other words, it is insoluble and it is asolid. • We can predict which product forms the precipitate if we have a solubility chart handy.

  4. Solubility Table (pg. 324)

  5. Predicting Ionic Solubility – warm-up • Use a solubility chart to predict the solubility of the following compounds in water. State whether they are soluble or insoluble in water.

  6. 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.

  7. 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.

  8. 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.

  9. 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.

  10. 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.

  11. 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.

  12. 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.

  13. 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.

  14. 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.

  15. 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.

  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.

  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.

  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.

  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.

  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.

  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.

  22. General Solubility Rules (Time savers) • Nitrates (NO31-) • soluble with all cations. • Ammonium (NH41+) • soluble with all anions. • Alkali Metals (Li1+, Na1+, K1+,…) • soluble with all anions.

  23. 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(NO3)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)

  24. Predicting the Precipitate that Forms in a Chemical Reaction • First Step: Write out the Balanced Chemical Equation: 2KI (aq) + 1Pb(NO3)2(aq) 2KNO3(?) + 1PbI2(?) • Second step: Determine which product is insoluble:

  25. Predicting the Precipitate that Forms in a Chemical Reaction • First Step: Write out the Balanced Reaction Equation: 2KI (aq) + 1Pb(NO3)2(aq) 2KNO3(?) + 1PbI2(?) • Second step: Determine which product is insoluble:

  26. Predicting the Precipitate that Forms in a Chemical Reaction • First Step: Write out the Balanced Reaction Equation: 2KI (aq) + 1Pb(NO3)2(aq) 2KNO3(?) + 1PbI2(?) • Second step: Determine which product is insoluble:

  27. Predicting the Precipitate that Forms in a Chemical Reaction • First Step: Write out the Balanced Reaction Equation: 2KI (aq) + 1Pb(NO3)2(aq) 2KNO3(?) + 1PbI2(?) • Second step: Determine which product is insoluble:

  28. WRITING TOTAL IONIC EQUATIONS • 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). 2K1+(aq) + 2I1-(aq)

  29. WRITING TOTAL IONIC EQUATIONS • 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). 2K1+(aq) + 2I1-(aq) + 1Pb2+(aq) + 2NO31-(aq)

  30. WRITING TOTAL IONIC EQUATIONS • 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). 2K1+(aq) + 2I1-(aq) + 1Pb2+(aq) + 2NO31-(aq) 2K1+(aq) + 2NO31-(aq)

  31. WRITING TOTAL IONIC EQUATIONS • 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). 2K1+(aq) + 2I1-(aq) + 1Pb2+(aq) + 2NO31-(aq) 2K1+(aq) + 2NO31-(aq) + 1PbI2(s)

  32. WRITING NET IONIC EQUATIONS • 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.) 2K1+(aq) + 2I1-(aq) + 1Pb2+(aq) + 2NO31-(aq) 2K1+(aq) + 2NO31-(aq) + 1PbI2(s)

  33. WRITING NET IONIC EQUATIONS • 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.) 2K1+(aq) + 2I1-(aq) + 1Pb2+(aq) + 2NO31-(aq) 2K1+(aq)+ 2NO31-(aq) + 1PbI2(s)

  34. WRITING NET IONIC EQUATIONS • 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.) 2K1+(aq)+ 2I1-(aq) + 1Pb2+(aq)+ 2NO31-(aq) 2K1+(aq)+ 2NO31-(aq) + 1PbI2(s)

  35. WRITING NET IONIC EQUATIONS • 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 thatdo 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: 1Pb2+(aq) + 2I1-(aq) 1PbI2(s)

  36. 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.

  37. Homework • Read pg. 331 – 336 • Do #1 – 3 (Section Questions) on pg. 336 – 337 • Worksheet: Net Ionic Equations

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