Honors Chemistry Name__________________________________
Net Ionic Equation Worksheet
READ THIS: When two solutions of ionic compounds are mixed, a solid may form. This type of reaction is called a
precipitation reaction, and the solid produced in the reaction is known as the precipitate. You can predict whether a
precipitate will form using a list of solubility rules such as those found in the table below. When a combination of ions is
described as insoluble, a precipitate forms. There are three types of equations that are commonly written to describe a
precipitation reaction. The molecular equation shows each of the substances in the reaction as compounds with
physical states written next to the chemical formulas. The complete ionic equation shows each of the aqueous
compounds as separate ions. Insoluble substances are not separated and these have the symbol (s) written next to
them. Water is also not separated and it has a (l) written next to it. Notice that there are ions that are present on both
sides of the reaction arrow –> that is, they do not react. These ions are known as spectator ions and they are eliminated
from complete ionic equation by crossing them out. The remaining equation is known as the net ionic equation.
For example: The reaction of potassium chloride and lead II nitrate
Molecular Equation: 2KCl (aq) + Pb(NO
3
)
2
(aq) -> 2KNO
3
(aq) + PbCl
2
(s)
Complete Ionic Equation: 2K
+
(aq) + 2Cl
-
(aq) + Pb
2+
(aq) + 2NO
3–
(aq) -> 2K
+
(aq) + 2NO3
–
(aq) + PbCl
2
(s)
Net Ionic Equation: 2Cl
-
(aq) + Pb
2+
(aq) -> PbCl
2
(s)
Directions: Write balanced molecular, ionic, and net ionic equations for each of the following reactions. Assume all
reactions occur in aqueous solution. Include states of matter in your balanced equation.
1. Sodium chloride and lead II nitrate
Molecular Equation:
Complete Ionic Equation:
Net Ionic Equation:
2. Sodium carbonate and Iron II chloride
Molecular Equation:
Complete Ionic Equation:
Net Ionic Equation:
3. Magnesium hydroxide and hydrochloric acid
Molecular Equation:
Complete Ionic Equation:
Net Ionic Equation:
4. Potassium chromate and calcium chloride
Molecular Equation:
Complete Ionic Equation:
Net Ionic Equation:
5. Ammonium phosphate and zinc nitrate
Molecular Equation:
Complete Ionic Equation:
Net Ionic Equation:
6. Lithium hydroxide and barium chloride
Molecular Equation:
Complete Ionic Equation:
Net Ionic Equation:
7. Sodium carbonate and hydrochloric acid produces sodium chloride, carbon dioxide and water
Molecular Equation:
Complete Ionic Equation:
Net Ionic Equation:
8. Magnesium nitrate and sodium chromate
Molecular Equation:
Complete Ionic Equation:
Net Ionic Equation:
9. Iron III chloride and magnesium metal
Molecular Equation:
Complete Ionic Equation:
Net Ionic Equation:
10. Barium Bromide and sodium sulfate
Molecular Equation:
Complete Ionic Equation:
Net Ionic Equation:
11. Silver nitrate and magnesium iodide
Molecular Equation:
Complete Ionic Equation:
Net Ionic Equation:
12. Ammonium chromate and aluminum perchlorate
Molecular Equation:
Complete Ionic Equation:
Net Ionic Equation:
13. Nickel nitrate and sodium hydroxide
Molecular Equation:
Complete Ionic Equation:
Net Ionic Equation:
14. Hydrobromic acid and lead II perchlorate
Molecular Equation:
Complete Ionic Equation:
Net Ionic Equation:
15. Potassium fluoride and magnesium nitrate
Molecular Equation:
Complete Ionic Equation:
Net Ionic Equation:
16. Sodium phosphate and nickel II perchlorate
Molecular Equation:
Complete Ionic Equation:
Net Ionic Equation:
17. Copper II chloride and silver acetate
Molecular Equation:
Complete Ionic Equation:
Net Ionic Equation:
Net Ionic Equation Worksheet - answers
1. 2NaCl(aq) + Pb(NO
3
)
2
(aq) → PbCl
2
(s) + 2NaNO
3
(aq)
Ionic Equation: 2Na
+
(aq) + 2Cl
-
(aq) + Pb
2+
(aq) + 2NO
3
-
(aq) → PbCl
2
(s) +
2Na
+
(aq) + 2NO
3
-
(aq)
NIE: 2Cl
-
(aq) + Pb
2+
(aq) → PbCl
2
(s)
2. Na
2
CO
3
(aq) + FeCl
2
(aq) → FeCO
3
(s) + 2NaCl(aq)
Ionic Equation: 2Na
+
(aq) + CO
3
2-
(aq) + Fe
2+
(aq) + 2Cl
-
(aq) → FeCO
3
(s) +
2Na
+
(aq) + 2Cl
-
(aq)
NIE: CO
3
2-
(aq) + Fe
2+
(aq) → FeCO
3
(s)
3. Mg(OH)
2
(aq) + 2HCl(aq) → MgCl
2
(aq) + 2H
2
O(l)
Ionic Equation: Mg
2+
(aq) + 2OH
-
(aq) + 2H
+
(aq) + 2Cl
-
(aq) → Mg
2+
(aq) +
2Cl
-
(aq) + 2H
2
O(l)
NIE: 2OH
-
(aq) + 2H
+
(aq) → 2H
2
O(l)
(your final answer would be: OH
-
(aq) + H
+
(aq) → H
2
O(l))
4. K
2
(C
r
O
4
)(aq) + CaCl
2
(aq) → 2KCl(aq) + Ca(C
r
O
4
)(aq)
Ionic Equation: 2K
+
(aq) + C
2
O
4
2-
(aq) + Ca
2+
(aq) + 2Cl
-
(aq) → 2K
+
(aq) + 2Cl
-
(aq) +
Ca
2+
+ C
2
O
4
2-
NIE: NA all spectator ions
5. 2(NH
4
)
3
PO
4
(aq) + 3Zn(NO
3
)
2
(aq) → 6NH
4
NO
3
(aq) + Zn
3
(PO
4
)
2
(s)
Ionic Equation: 6NH
4
+
(aq) + 2PO
4
3-
(aq) + 3Zn
2+
(aq) + 6NO
3
-
(aq) → 6NH
4
+
(aq) + 6NO
3
-
(aq) + Zn
3
(PO
4
)
2
(s)
NIE: 2PO
4
3-
(aq) + 3Zn
2+
(aq) → Zn
3
(PO
4
)
2
(s)
6. 2LiOH(aq) + BaCl
2
(aq) → 2LiCl(aq) + Ba(OH)
2
(aq)
Ionic Equation: 2Li
+
(aq) + 2OH
-
(aq) + Ba
2+
(aq) + 2Cl
-
(aq) → 2Li
+
(aq) + 2Cl
-
(aq)
+ Ba
2+
+ 2 OH
-
NIE: Na all spectator ions
7. Na
2
CO
3
(aq) + 2HCl(aq) → 2NaCl(aq) + CO
2
(g) + H
2
O(l)
Ionic Equation: 2Na
+
(aq) + CO
3
2-
(aq) + 2H
+
(aq) + 2Cl
-
(aq) → 2Na
+
(aq) + 2Cl
-
(aq) +
CO
2
(g) + H
2
O(l)
NIE: CO
3
2-
(aq) + 2H
+
(aq) → CO
2
(g) + H
2
O(l)
8. Mg(NO
3
)
2
(aq) + Na
2
CrO
4
(aq) → 2NaNO
3
(aq) + MgCrO
4
(s)
Ionic Equation: Mg
2+
(aq) + 2NO
3
-
(aq) + 2Na
+
(aq) + CrO
4
2-
(aq) → 2Na
+
(aq) + 2NO
3
-
(aq) + MgCrO
4
(s)
NIE: Mg
2+
(aq) + CrO
4
2-
(aq) → MgCrO
4
(s)
9. 2FeCl
3
(aq) + 3Mg(s) → 3MgCl
2
(aq) + 2Fe(s)
Ionic Equation: 2Fe
3+
(aq) + 6Cl
-
(aq) + 3Mg(s) → 3Mg
2+
(aq) + 6Cl
-
(aq) + 2Fe(s)
NIE: 2Fe
3+
(aq) + 3Mg(s) → 3Mg
2+
(aq) + 2Fe(s)
10. BaBr
2
(aq) + Na
2
SO
4
(aq) → BaSO
4
(s) + 2NaBr(aq)
Ionic Equation: Ba
2+
(aq) + 2Br
-
(aq) + 2Na
+
(aq) + SO
4
2-
(aq) → BaSO
4
(s)
+ 2Na
+
(aq) + 2Br
-
(aq)
NIE: Ba
2+
(aq) + SO
4
2-
(aq) → BaSO
4
(s)
11. 2AgNO
3
(aq) + MgI
2
(aq) → 2AgI(s) + Mg(NO
3
)
2
(aq)
Ionic Equation: 2Ag
+
(aq) + 2NO
3
-
(aq) + Mg
2+
(aq) + 2I
-
(aq) → 2AgI(s) +
Mg
2+
(aq) + 2NO
3
-
(aq)
NIE: 2Ag
+
(aq) + 2I
-
(aq) → 2AgI(s)
(your final answer would be: Ag
+
(aq) + I
-
(aq) → AgI(s))
12. 3(NH
4
)
2
C
r
O
4
(aq) + 2Al(ClO
4
)
3
(aq) → Al
2
(C
r
O
4
)
3
(s) + 6NH
4
ClO
4
(aq)
Ionic Equation: 6NH
4
+
(aq) + 3C
r
O
4
2-
(aq) + 2Al
3+
(aq) + 6ClO
4
-
(aq) → 6NH
4
+
(aq) + 6ClO
4
-
(aq)
+ Al
2
(C
r
O
4
)
3
(s)
NIE: 3C
2
O
4
2-
(aq) + 2Al
3+
(aq) → Al
2
(C
r
O
4
)
3
(s)
13. Ni(NO
3
)
2
(aq) + 2NaOH(aq) → Ni(OH)
2
(s) + 2NaNO
3
(aq)
Ionic Equation: Ni
2+
(aq) + 2NO
3
-
(aq) + 2Na
+
(aq) + 2OH
-
(aq) → Ni(OH)
2
(s) +
2Na
+
(aq) + 2NO
3
-
(aq)
NIE: Ni
2+
(aq) + 2OH
-
(aq) → Ni(OH)
2
(s)
14. 2HBr(aq) + Pb(ClO
4
)
2
(aq) → 2HClO
4
(aq) + PbBr
2
(s)
Ionic Equation: 2H
+
(aq) + 2Br
-
(aq) + Pb
2+
(aq) + 2ClO
4
-
(aq) → 2H
+
(aq)
+ 2ClO
4
-
(aq) + PbBr
2
(s)
NIE: 2Br
-
(aq) + Pb
2+
(aq) → PbBr
2
(s)
15. 2KF(aq) + Mg(NO
3
)
2
(aq) → 2KNO
3
(aq) + MgF
2
(s)
Ionic Equation: 2K
+
(aq) + 2F
-
(aq) + Mg
2+
(aq) + 2NO
3
-
(aq) → 2K
+
(aq) + 2NO
3
-
(aq) + MgF
2
(s)
NIE: 2F
-
(aq) + Mg
2+
(aq) → MgF
2
(s)
16. 2Na
3
PO
4
(aq) + 3Ni(ClO
4
)
2
(aq) → 6NaClO
4
(aq) + Ni
3
(PO
4
)
2
(s)
Ionic Equation: 6Na
+
(aq) 2PO
4
3-
(aq) + 3Ni
2+
(aq) + 6ClO
4
-
(aq) → 6Na
+
(aq) +
6ClO
4
-
(aq) + Ni
3
(PO
4
)
2
(s)
NIE 2PO
4
3-
(aq) + 3Ni
2+
(aq) → Ni
3
(PO
4
)
2
(s)
17. CuCl
2
(aq) + 2AgC
2
H
3
O
2
(aq) → Cu(C
2
H
3
O
2
)
2
(aq) + 2AgCl(s)
Ionic Equation: Cu
2+
(aq) + 2Cl
-
(aq) + 2Ag
+
(aq) + 2C
2
H
3
O
2
-
(aq) → Cu
2+
(aq) +
2C
2
H
3
O
2
-
(aq) + 2AgCl(s)
NIE: Cl
-
(aq) + Ag
+
(aq) → AgCl(s)
