Net Ionic Equations Meghan Daniel Emily Spellmire Mandy Radulea.
Net Ionic Equations
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Transcript of Net Ionic Equations
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Net Ionic EquationsAn Application of Double Replacement
Reactions
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IntroductionWe know that double replacement reactions
result in the formation of either -
a precipitate, or
an insoluble gas, or
water
Pb(NO3)2(aq) + 2 KI(aq) → PbI2(s) + 2 KNO3(aq)
“An aqueous solution of lead(II) nitrate is mixed with an aqueous solution of potassium iodide and results in the formation of solid lead(II) iodide and an aqueous solution of potassium nitrate.”
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Ions in SolutionPb(NO3)2(aq) + 2 KI(aq) → PbI2(s) + 2 KNO3(aq)
Let’s look at what happens when we make the two starting solutions -
Pb(NO3)2(s) → Pb2+(aq) + 2 NO3−(aq)
KI(s) → K+(aq) + I−(aq)
•Our solutions are actually composed of the ions in solution.
• When we write “Pb(NO3)2(aq)” we really mean “Pb2+(aq) + 2 NO3
−(aq)”
H2O
H2O
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Ions in SolutionPb(NO3)2(aq) + 2 KI(aq) → PbI2(s) + 2 KNO3(aq)
Now, we can write the equation as a mixture of solvated ions –
Pb2+(aq) + 2 NO3−(aq) + 2 K+(aq) + 2 I−(aq) → PbI2(s) + 2 KNO3(aq)
•The PbI2(s) is a solid and is not in solution -
• we don’t have separated ions
•The KNO3(aq) is in solution and represents solvated ions –
KNO3(aq) → K+(aq) + NO3−(aq)
H2O
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Pb(NO3)2(aq) + 2 KI(aq) → PbI2(s) + 2 KNO3(aq)
Now, we can write the equation as a mixture of solvated ions -
Pb2+(aq) + 2 NO3−(aq) + 2 K+(aq) + 2 I−(aq) → PbI2(s) + 2 K+(aq) + 2 NO3
−
(aq)
Ionic Equations
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Pb(NO3)2(aq) + 2 KI(aq) → PbI2(s) + 2 KNO3(aq)
Now, we can write the equation as a mixture of solvated ions -
Pb2+(aq) + 2 NO3−(aq) + 2 K+(aq) + 2 I−(aq) → PbI2(s) + 2 K+(aq) + 2 NO3
−
(aq)
•This is called the “complete ionic equation”
• We have all the ionic species on both sides of the arrow
Ionic Equations
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Pb(NO3)2(aq) + 2 KI(aq) → PbI2(s) + 2 KNO3(aq)
Now, we can write the equation as a mixture of solvated ions -
Pb2+(aq) + 2 NO3−(aq) + 2 K+(aq) + 2 I−(aq) → PbI2(s) + 2 K+(aq) + 2 NO3
−
(aq)
•This is called the “complete ionic equation”
•If we look carefully at the equation, we will see compounds that are the same on both sides
Ionic Equations
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Pb(NO3)2(aq) + 2 KI(aq) → PbI2(s) + 2 KNO3(aq)
Now, we can write the equation as a mixture of solvated ions -
Pb2+(aq) + 2 NO3−(aq) + 2 K+(aq) + 2 I−(aq) → PbI2(s) + 2 K+(aq) + 2 NO3
−
(aq)
•This is called the “complete ionic equation”
•If we look carefully at the equation, we will see compounds that are the same on both sides
• 2 NO3−(aq)
Ionic Equations
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Pb(NO3)2(aq) + 2 KI(aq) → PbI2(s) + 2 KNO3(aq)
Now, we can write the equation as a mixture of solvated ions -
Pb2+(aq) + 2 NO3−(aq) + 2 K+(aq) + 2 I−(aq) → PbI2(s) + 2 K+(aq) + 2 NO3
−
(aq)
•This is called the “complete ionic equation”
•If we look carefully at the equation, we will see compounds that are the same on both sides
• 2 NO3−(aq)
Ionic Equations
![Page 10: Net Ionic Equations](https://reader038.fdocuments.us/reader038/viewer/2022110102/56813486550346895d9b6754/html5/thumbnails/10.jpg)
Pb(NO3)2(aq) + 2 KI(aq) → PbI2(s) + 2 KNO3(aq)
Now, we can write the equation as a mixture of solvated ions -
Pb2+(aq) + 2 NO3−(aq) + 2 K+(aq) + 2 I−(aq) → PbI2(s) + 2 K+(aq) + 2 NO3
−
(aq)
•This is called the “complete ionic equation”
•If we look carefully at the equation, we will see compounds that are the same on both sides
• 2 NO3−(aq) and 2 K+(aq)
Ionic Equations
![Page 11: Net Ionic Equations](https://reader038.fdocuments.us/reader038/viewer/2022110102/56813486550346895d9b6754/html5/thumbnails/11.jpg)
Pb(NO3)2(aq) + 2 KI(aq) → PbI2(s) + 2 KNO3(aq)
Now, we can write the equation as a mixture of solvated ions -
Pb2+(aq) + 2 NO3−(aq) + 2 K+(aq) + 2 I−(aq) → PbI2(s) + 2 K+(aq) + 2 NO3
−
(aq)
•This is called the “complete ionic equation”
•If we look carefully at the equation, we will see compounds that are the same on both sides
• 2 NO3−(aq) and 2 K+(aq)
Ionic Equations
![Page 12: Net Ionic Equations](https://reader038.fdocuments.us/reader038/viewer/2022110102/56813486550346895d9b6754/html5/thumbnails/12.jpg)
Pb(NO3)2(aq) + 2 KI(aq) → PbI2(s) + 2 KNO3(aq)
Now, we can write the equation as a mixture of solvated ions -
Pb2+(aq) + 2 NO3−(aq) + 2 K+(aq) + 2 I−(aq) → PbI2(s) + 2 K+(aq) + 2 NO3
−
(aq)
•This is called the “complete ionic equation”
•If we look carefully at the equation, we will see compounds that are the same on both sides
• 2 NO3−(aq) and 2 K+(aq)
• These are called “spectator ions”
Ionic Equations
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Pb(NO3)2(aq) + 2 KI(aq) → PbI2(s) + 2 KNO3(aq)
Now, we can write the equation as a mixture of solvated ions -
Pb2+(aq) + 2 NO3−(aq) + 2 K+(aq) + 2 I−(aq) → PbI2(s) + 2 K+(aq) + 2 NO3
−
(aq)
•This is called the “complete ionic equation”
•Spectator ions don’t participate in the reaction
• They hang around and watch
Ionic Equations
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Pb(NO3)2(aq) + 2 KI(aq) → PbI2(s) + 2 KNO3(aq)
Now, we can write the equation as a mixture of solvated ions -
Pb2+(aq) + 2 NO3−(aq) + 2 K+(aq) + 2 I−(aq) → PbI2(s) + 2 K+(aq) + 2 NO3
−
(aq)
•If we remove the spectator ions from the equation ...
Ionic Equations
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Pb(NO3)2(aq) + 2 KI(aq) → PbI2(s) + 2 KNO3(aq)
Now, we can write the equation as a mixture of solvated ions -
Pb2+(aq) + 2 I−(aq) → PbI2(s)
•If we remove the spectator ions from the equation ...
Ionic Equations
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Pb(NO3)2(aq) + 2 KI(aq) → PbI2(s) + 2 KNO3(aq)
Now, we can write the equation as a mixture of solvated ions -
Pb2+(aq) + 2 I−(aq) → PbI2(s)
•If we remove the spectator ions from the equation, we end up with an equation that has only the reacting species.
This is called the “net ionic equation”
Ionic Equations
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Example 1:
Write the complete ionic equation, the net ionic equation, and determine the spectator ions for the following equation:
BaCl2(aq) + Na2SO4(aq) → BaSO4(s) + 2 NaCl(aq)
Applications
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Example 1:
Write the complete ionic equation, the net ionic equation, and determine the spectator ions for the following equation:
BaCl2(aq) + Na2SO4(aq) → BaSO4(s) + 2 NaCl(aq)
Ions in solution:•Ba2+(aq) + 2 Cl−(aq) + 2 Na+(aq) + SO4
2−(aq)
Applications
![Page 19: Net Ionic Equations](https://reader038.fdocuments.us/reader038/viewer/2022110102/56813486550346895d9b6754/html5/thumbnails/19.jpg)
Example 1:
Write the complete ionic equation, the net ionic equation, and determine the spectator ions for the following equation:
BaCl2(aq) + Na2SO4(aq) → BaSO4(s) + 2 NaCl(aq)
Ions in solution:•Ba2+(aq) + 2 Cl−(aq) + 2 Na+(aq) + SO4
2−(aq)•Ions on both sides of the arrow:
2 Cl−(aq) + 2 Na+(aq)
Applications
![Page 20: Net Ionic Equations](https://reader038.fdocuments.us/reader038/viewer/2022110102/56813486550346895d9b6754/html5/thumbnails/20.jpg)
Example 1:
Write the complete ionic equation, the net ionic equation, and determine the spectator ions for the following equation:
BaCl2(aq) + Na2SO4(aq) → BaSO4(s) + 2 NaCl(aq)
Ions in solution:•Ba2+(aq) + 2 Cl−(aq) + 2 Na+(aq) + SO4
2−(aq)•Ions on both sides of the arrow:
2 Cl−(aq) + 2 Na+(aq)
Applications
These are the spectator ions
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Example 1:
Write the complete ionic equation, the net ionic equation, and determine the spectator ions for the following equation:
BaCl2(aq) + Na2SO4(aq) → BaSO4(s) + 2 NaCl(aq)
Complete Ionic Equation:Ba2+(aq) + 2 Cl−(aq) + 2 Na+(aq) + SO4
2−(aq) → BaSO4(s) + 2 Na+(aq) +2 Cl−(aq)
Applications
![Page 22: Net Ionic Equations](https://reader038.fdocuments.us/reader038/viewer/2022110102/56813486550346895d9b6754/html5/thumbnails/22.jpg)
Example 1:
Write the complete ionic equation, the net ionic equation, and determine the spectator ions for the following equation:
BaCl2(aq) + Na2SO4(aq) → BaSO4(s) + 2 NaCl(aq)
Complete Ionic Equation:Ba2+(aq) + 2 Cl−(aq) + 2 Na+(aq) + SO4
2−(aq) → BaSO4(s) + 2 Na+(aq) +2 Cl−(aq)
•Net Ionic Equation:•Ba2+(aq) + SO4
2−(aq) → BaSO4(s)
Applications
![Page 23: Net Ionic Equations](https://reader038.fdocuments.us/reader038/viewer/2022110102/56813486550346895d9b6754/html5/thumbnails/23.jpg)
Example 1:
Write the complete ionic equation, the net ionic equation, and determine the spectator ions for the following equation:
BaCl2(aq) + Na2SO4(aq) → BaSO4(s) + 2 NaCl(aq)
Complete Ionic Equation:Ba2+(aq) + 2 Cl−(aq) + 2 Na+(aq) + SO4
2−(aq) → BaSO4(s) + 2 Na+(aq) +2 Cl−(aq)
•Net Ionic Equation:•Ba2+(aq) + SO4
2−(aq) → BaSO4(s)
•Spectator Ions:•Na+(aq) and Cl−(aq)
Applications
![Page 24: Net Ionic Equations](https://reader038.fdocuments.us/reader038/viewer/2022110102/56813486550346895d9b6754/html5/thumbnails/24.jpg)
Example 2:
Write the complete ionic equation, the net ionic equation, and determine the spectator ions for the following equation:
AgClO4(aq) + NaCl(aq) → AgCl(s) + NaClO4(aq)
Applications
![Page 25: Net Ionic Equations](https://reader038.fdocuments.us/reader038/viewer/2022110102/56813486550346895d9b6754/html5/thumbnails/25.jpg)
Example 2:
Write the complete ionic equation, the net ionic equation, and determine the spectator ions for the following equation:
AgClO4(aq) + NaCl(aq) → AgCl(s) + NaClO4(aq)
Ions in solution:•Ag+(aq) + ClO4
−(aq) + Na+(aq) + Cl−(aq)
Applications
![Page 26: Net Ionic Equations](https://reader038.fdocuments.us/reader038/viewer/2022110102/56813486550346895d9b6754/html5/thumbnails/26.jpg)
Example 2:
Write the complete ionic equation, the net ionic equation, and determine the spectator ions for the following equation:
AgClO4(aq) + NaCl(aq) → AgCl(s) + NaClO4(aq)
Ions in solution:•Ag+(aq) + ClO4
−(aq) + Na+(aq) + Cl−(aq)•Ions on both sides of the arrow:
ClO4−(aq) + Na+(aq)
Applications
![Page 27: Net Ionic Equations](https://reader038.fdocuments.us/reader038/viewer/2022110102/56813486550346895d9b6754/html5/thumbnails/27.jpg)
Example 2:
Write the complete ionic equation, the net ionic equation, and determine the spectator ions for the following equation:
AgClO4(aq) + NaCl(aq) → AgCl(s) + NaClO4(aq)
Ions in solution:•Ag+(aq) + ClO4
−(aq) + Na+(aq) + Cl−(aq)•Ions on both sides of the arrow:
ClO4−(aq) + Na+(aq)
Applications
These are the spectator ions
![Page 28: Net Ionic Equations](https://reader038.fdocuments.us/reader038/viewer/2022110102/56813486550346895d9b6754/html5/thumbnails/28.jpg)
Example 2:
Write the complete ionic equation, the net ionic equation, and determine the spectator ions for the following equation:
AgClO4(aq) + NaCl(aq) → AgCl(s) + NaClO4(aq)
Complete Ionic Equation:•Ag+(aq) + ClO4
−(aq) + Na+(aq) + Cl−(aq) → AgCl(s) + Na+(aq) + ClO4−(aq)
Applications
![Page 29: Net Ionic Equations](https://reader038.fdocuments.us/reader038/viewer/2022110102/56813486550346895d9b6754/html5/thumbnails/29.jpg)
Example 2:
Write the complete ionic equation, the net ionic equation, and determine the spectator ions for the following equation:
AgClO4(aq) + NaCl(aq) → AgCl(s) + NaClO4(aq)
Complete Ionic Equation:•Ag+(aq) + ClO4
−(aq) + Na+(aq) + Cl−(aq) → AgCl(s) + Na+(aq) + ClO4−(aq)
Net Ionic Equation:•Ag+(aq) + Cl−(aq) → AgCl(s)
Applications
![Page 30: Net Ionic Equations](https://reader038.fdocuments.us/reader038/viewer/2022110102/56813486550346895d9b6754/html5/thumbnails/30.jpg)
Example 2:
Write the complete ionic equation, the net ionic equation, and determine the spectator ions for the following equation:
AgClO4(aq) + NaCl(aq) → AgCl(s) + NaClO4(aq)
Complete Ionic Equation:•Ag+(aq) + ClO4
−(aq) + Na+(aq) + Cl−(aq) → AgCl(s) + Na+(aq) + ClO4−(aq)
Net Ionic Equation:•Ag+(aq) + Cl−(aq) → AgCl(s)
•Spectator Ions:•Na+(aq) and ClO4
−(aq)
Applications
![Page 31: Net Ionic Equations](https://reader038.fdocuments.us/reader038/viewer/2022110102/56813486550346895d9b6754/html5/thumbnails/31.jpg)
To write the complete ionic equation -
separate all aqueous ionic compounds into their aqueous ions
keep all solids, insoluble gases, and water together
Summary
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To write the complete ionic equation -
separate all aqueous ionic compounds into their aqueous ions
keep all solids, insoluble gases, and water together
To find the spectator ions -
find the aqueous ions that are the same on both sides of the arrow
Summary
![Page 33: Net Ionic Equations](https://reader038.fdocuments.us/reader038/viewer/2022110102/56813486550346895d9b6754/html5/thumbnails/33.jpg)
To write the complete ionic equation -
separate all aqueous ionic compounds into their aqueous ions
keep all solids, insoluble gases, and water together
To find the spectator ions -
find the aqueous ions that are the same on both sides of the arrow
To write the net ionic equation -
remove the spectator ions from the complete ionic equation
Summary