1. Chapter 11 Chemical Reactions 11.3 Reactions in Aqueous Solution
11.1 Describing Chemical Reactions
11.2 Types of Chemical Reactions
11.3 Reactions in Aqueous Solution
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2. Classifying Reactions
Do Now:
__Ag + __Cu(NO3)2 → __Cu + __AgNO3
__Cl2 + __NaBr → __NaCl + __Br2
Balance the equations.
Identify the types of reaction.
Will the reactions proceed?
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3. Classifying Reactions
Predict the products and balance the following:
Mg + AlCl3 →
Br MgCl2 →
Fe CuCl2 →
Zn + HNO3 →
Will the reactions proceed?
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4. Classifying Reactions
Predict the products and balance the following:
AgNO KCl →
AgNO Na2CO3 →
AgNO KNO3 →
AgNO Na3PO4 →
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5. Classifying Reactions
Predict the products and balance the following:
Pb(NO3) K2CrO4 →
Cu(OH) H3PO4 →
Zn H2CO3 →
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6. Classifying Reactions
Do Now:
Predict the products
NaCl(aq) AgNO3(aq)
Cu(OH)2(aq) + H3PO4(aq) →
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7. Solubility Rules for Ionic Compounds
Interpret Data
Solubility Rules for Ionic Compounds
Compounds
Solubility
Exceptions
Salts of alkali metals and ammonia
Soluble
Some lithium compounds
Nitrate salts and chlorate salts
Few exceptions
Sulfate salts
Compounds of Pb, Ag, Hg, Ba, Sr, and Ca
Chloride salts
Compounds of Ag and some compounds of Hg and Pb
Carbonates, phosphates, chromates, sulfides, and hydroxides
Most are insoluble
Compounds of the alkali metals and of ammonia
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8. Predicting the Formation of a Precipitate
Use the solubility rules table to determine which compounds below are insoluble.
PbCl2
KOH
NaOH
SrSO4
Fe2S3
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9. Classifying Reactions
Do Now: Predict the products of the following reaction.
FeCl3 (aq) + 3KOH (aq) →
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10. Predict the products of the above reaction.
Do Now:
FeCl3 (aq) + 3KOH (aq) →
Predict the products of the above reaction.
Write a complete ionic equation.
Write the net ionic equation.
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11. Complete ionic equation
Net Ionic Equations
Complete ionic equation
shows dissolved ionic compounds as dissociated free ions.
Ag+(aq) + NO3–(aq) + Na+(aq) + Cl–(aq) → AgCl(s) + Na+(aq) + NO3–(aq)
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12. Net Ionic Equations
spectator ion - ion that appears on both sides of equation and is not involved in the reaction.
Ag+(aq) + NO3–(aq) + Na+(aq) + Cl–(aq) → AgCl(s) + Na+(aq) + NO3–(aq)
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13. Ag+(aq) + Cl–(aq) → AgCl(s) Make sure ionic charge is balanced!
Net Ionic Equations
net ionic equation – only shows particles directly involved in the chemical change.
Ag+(aq) + Cl–(aq) → AgCl(s)
Make sure ionic charge is balanced!
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14. MgCl2(aq) + 2 NaOH(aq) → Mg(OH)2(s) + 2 NaCl(aq)
Net Ionic Equations
Write the complete ionic equation and net ionic equation for:
MgCl2(aq) + 2 NaOH(aq) → Mg(OH)2(s) + 2 NaCl(aq)
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15. Writing and Balancing Net Ionic Equations
Sample Problem 11.8
Writing and Balancing Net Ionic Equations
Aqueous solutions of iron(III) chloride and potassium hydroxide are mixed. A precipitate of iron(III) hydroxide forms. Identify the spectator ions and write a balanced net ionic equation for the reaction.
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16. 1. Write a balanced equation.
Sample Problem 11.8
1. Write a balanced equation.
FeCl3 (aq) + 3KOH (aq) → Fe(OH)3(s) + 3KCl(aq)
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17. 2. Write the complete ionic equation.
Sample Problem 11.8
2. Write the complete ionic equation.
Fe3+(aq) + 3Cl–(aq) + 3K+(aq) + 3OH–(aq) →
Fe(OH)3(s) + 3K+(aq) + 3Cl–(aq)
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18. 3. Eliminate spectator ions.
Sample Problem 11.8
3. Eliminate spectator ions.
Fe3+(aq) + 3Cl–(aq) + 3K+(aq) + 3OH–(aq) →
Fe(OH)3(s) + 3K+(aq) + 3Cl–(aq)
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19. Fe3+(aq) + 3OH–(aq) → Fe(OH)3(s)
Sample Problem 11.8
4. Write the net ionic equation.
Fe3+(aq) + 3OH–(aq) → Fe(OH)3(s)
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20. Na2CO3(aq) + CaCl2(aq) → NaCl(aq) + CaCO3(s)
Net Ionic Equations
Do Now: Balance the reaction, then write the complete ionic equation and net ionic equation for:
Na2CO3(aq) + CaCl2(aq) → NaCl(aq) + CaCO3(s)
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21. Predicting the Formation of a Precipitate
Do Now: Write the complete ionic equation and net ionic equation for the reaction below:
K3PO4(aq) + Ba(OH)2(aq) →
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22. Sample Problem 11.9
Aqueous potassium carbonate reacts with aqueous strontium nitrate. Identify the precipitate formed and write the net ionic equation.
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23. Sample Problem 11.9
Aqueous potassium carbonate reacts with aqueous strontium nitrate. Identify the precipitate formed and write the net ionic equation.
CO32–(aq) + Sr2+(aq) → SrCO3(s)
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24. END OF 11.3
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