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Solutions and Solubility

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Presentation on theme: "Solutions and Solubility"— Presentation transcript:

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 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.

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. Ca(NO3)2 CuCl2 KBr (NH4)2CO3 Fe(NO3)3 Ca(OH)2 NH4CH3COO Pb(NO3)4 Ca3(PO4)2 CuCl KCH3COO PbCO3 BaSO4 AgOH Ag2SO4 Cr(OH)3

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. Ca(NO3)2 soluble CuCl2 KBr (NH4)2CO3 Fe(NO3)3 Ca(OH)2 NH4CH3COO Pb(NO3)4 Ca3(PO4)2 CuCl KCH3COO PbCO3 BaSO4 AgOH Ag2SO4 Cr(OH)3

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. Ca(NO3)2 soluble CuCl2 KBr (NH4)2CO3 Fe(NO3)3 Ca(OH)2 NH4CH3COO Pb(NO3)4 Ca3(PO4)2 CuCl KCH3COO PbCO3 BaSO4 AgOH Ag2SO4 Cr(OH)3

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. Ca(NO3)2 soluble CuCl2 KBr (NH4)2CO3 Fe(NO3)3 Ca(OH)2 NH4CH3COO Pb(NO3)4 Ca3(PO4)2 CuCl KCH3COO PbCO3 BaSO4 AgOH Ag2SO4 Cr(OH)3

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. Ca(NO3)2 soluble CuCl2 KBr (NH4)2CO3 Fe(NO3)3 Ca(OH)2 NH4CH3COO Pb(NO3)4 Ca3(PO4)2 CuCl KCH3COO PbCO3 BaSO4 AgOH Ag2SO4 Cr(OH)3

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. Ca(NO3)2 soluble CuCl2 KBr (NH4)2CO3 Fe(NO3)3 Ca(OH)2 NH4CH3COO Pb(NO3)4 Ca3(PO4)2 insoluble CuCl KCH3COO PbCO3 BaSO4 AgOH Ag2SO4 Cr(OH)3

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. Ca(NO3)2 soluble CuCl2 KBr (NH4)2CO3 Fe(NO3)3 Ca(OH)2 NH4CH3COO Pb(NO3)4 Ca3(PO4)2 insoluble CuCl KCH3COO PbCO3 BaSO4 AgOH Ag2SO4 Cr(OH)3

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. Ca(NO3)2 soluble CuCl2 KBr (NH4)2CO3 Fe(NO3)3 Ca(OH)2 NH4CH3COO Pb(NO3)4 Ca3(PO4)2 insoluble CuCl KCH3COO PbCO3 BaSO4 AgOH Ag2SO4 Cr(OH)3

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. Ca(NO3)2 soluble CuCl2 KBr (NH4)2CO3 Fe(NO3)3 Ca(OH)2 NH4CH3COO Pb(NO3)4 Ca3(PO4)2 insoluble CuCl KCH3COO PbCO3 BaSO4 AgOH Ag2SO4 Cr(OH)3

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. Ca(NO3)2 soluble CuCl2 KBr (NH4)2CO3 Fe(NO3)3 Ca(OH)2 NH4CH3COO Pb(NO3)4 Ca3(PO4)2 insoluble CuCl KCH3COO PbCO3 BaSO4 AgOH Ag2SO4 Cr(OH)3

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. Ca(NO3)2 soluble CuCl2 KBr (NH4)2CO3 Fe(NO3)3 Ca(OH)2 NH4CH3COO Pb(NO3)4 Ca3(PO4)2 insoluble CuCl KCH3COO PbCO3 BaSO4 AgOH Ag2SO4 Cr(OH)3

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(NO3)2 soluble CuCl2 KBr (NH4)2CO3 Fe(NO3)3 Ca(OH)2 insoluble NH4CH3COO Pb(NO3)4 Ca3(PO4)2 CuCl KCH3COO PbCO3 BaSO4 AgOH Ag2SO4 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(NO3)2 soluble CuCl2 KBr (NH4)2CO3 Fe(NO3)3 Ca(OH)2 insoluble NH4CH3COO Pb(NO3)4 Ca3(PO4)2 CuCl KCH3COO PbCO3 BaSO4 AgOH Ag2SO4 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(NO3)2 soluble CuCl2 KBr (NH4)2CO3 Fe(NO3)3 Ca(OH)2 insoluble NH4CH3COO Pb(NO3)4 Ca3(PO4)2 CuCl KCH3COO PbCO3 BaSO4 AgOH Ag2SO4 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(NO3)2 soluble CuCl2 KBr (NH4)2CO3 Fe(NO3)3 Ca(OH)2 insoluble NH4CH3COO Pb(NO3)4 Ca3(PO4)2 CuCl KCH3COO PbCO3 BaSO4 AgOH Ag2SO4 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(NO3)2 soluble CuCl2 KBr (NH4)2CO3 Fe(NO3)3 Ca(OH)2 insoluble NH4CH3COO Pb(NO3)4 Ca3(PO4)2 CuCl KCH3COO PbCO3 BaSO4 AgOH Ag2SO4 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(NO3)2 soluble CuCl2 KBr (NH4)2CO3 Fe(NO3)3 Ca(OH)2 insoluble NH4CH3COO Pb(NO3)4 Ca3(PO4)2 CuCl KCH3COO PbCO3 BaSO4 AgOH Ag2SO4 Cr(OH)3

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

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: Name of product Formula Solubility Potassium nitrate Lead (II) iodide

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: Name of product Formula Solubility Potassium nitrate KNO3 Lead (II) iodide PbI2

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: Name of product Formula Solubility Potassium nitrate KNO3 Soluble - ie (aq) Lead (II) iodide PbI2

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: Name of product Formula Solubility Potassium nitrate KNO3 Soluble - ie (aq) Lead (II) iodide PbI2 Insoluble - ie (s)

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 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: 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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