net ionic equations an application of double replacement reactions
TRANSCRIPT
Net Ionic EquationsAn Application of Double Replacement
Reactions
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.”
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
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
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
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
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
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
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
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
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
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
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
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
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
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
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
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
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
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
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
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
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
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
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
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
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
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
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
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
To write the complete ionic equation -
separate all aqueous ionic compounds into their aqueous ions
keep all solids, insoluble gases, and water together
Summary
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
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