Honor Chemistry
Name _________________________________
Chapter 8.1: Net Ionic Equations Worksheet I
Date _____/_____/_____
Period _____
Write a balance equation and label the states of the reactants and products for each in each reaction. After
writing the balanced equation, write the total ionic equation (TIE), list the driving force (DF) and spectator
ions (SI), and write the net ionic equation(s) (NET) below the balanced equation. If there is no driving force
for a reaction, write no reaction in place of the TIE, DF, SI, and NET.
1.
Hydrogen sulfide is bubbled through a solution of strontium hydroxide.
H2S(g)
+
Sr(OH)2(aq)

SrS(aq)
+
2 H(OH)()
TIE: H2S(g) + Sr+2(aq) + 2 (OH)-1(aq)  Sr+2(aq) + S-2(aq) + 2 H(OH)()
SI – Sr+2
DF – H(OH) ()
NET: H+1(aq)
2.

H(OH)()
Aluminum metal is added to a solution of copper (II) chloride.
2 Al(s)
+
3 CuCl2(aq)
TIE: 2 Al(s)
DF –

2 AlCl3(aq)
+
3 Cu(s)
3 Cu+2(aq) + 6 Cl-1(aq)  2 Al+3(aq) + 6 Cl-1(aq) + 3 Cu(s)
+
SI – Cl-1
Cu(s)
NET: Cu+2(aq)
3.
(OH)-1(aq)
+
+
2 e-1

Cu(s)
A manganese (II) nitrate solution is mixed with a sodium hydroxide solution.
Mn(NO3)2(aq)
+
2 NaOH(aq)

2 NaNO3(aq)
+
Mn(OH)2(s)
TIE: Mn+2(aq) + 2 (NO3)-1(aq) + 2 Na+1(aq) + 2 (OH)-1(aq)  2 Na+1(aq) + 2 (NO3)-1(aq) + Mn(OH)2(s)
DF –
Mn(OH)2(s)
NET: Mn+2(aq) + (OH)-1(aq) 
SI – Na+1(aq) , (NO3)-1(aq)
Mn(OH)2(s)
4.
Solutions of sodium carbonate and lead (II) nitrate are mixed.
Na2CO3(aq)
+

Pb(NO3)2(aq)
PbCO3(s)
+
2 NaNO3(aq)
TIE: 2 Na+1(aq) + (CO3)-2(aq) + Pb+2(aq) + 2 (NO3)-1(aq)  PbCO3(s)
DF –
5.
2 Na+1(aq) + 2 (NO3)-1(aq)
SI – Na+1(aq), (NO3)-1(aq)
PbCO3(s)
NET: Pb+2(aq)
+
+
(CO3)-2(aq)

PbCO3(s)
Aqueous solutions of sodium phosphate and barium chloride are mixed.
2 Na3PO4(aq)
+

3 BaCl2(aq)
Ba3(PO4)2(s)
+
6 NaCl(aq)
TIE: 6 Na+1(aq) + 2 (PO4)-3(aq) + 3 Ba+2(aq) + 6 Cl-1(aq)  Ba3(PO4)2(s) + 6 Na+1(aq) + 6 Cl-1(aq)
SI – Na+1(aq), Cl-1(aq)
DF – Ba3(PO4)2(s)
NET: Ba+2(aq)
6.
+
(PO4)-3(aq)

Ba3(PO4)2(s)
Hydrogen sulfide gas is added to a solution of cadmium (II) nitrate.
H2S(g)
+
Cd(NO3)2(aq)

CdS(s)
+
2 HNO3(aq)
TIE: H2S(g) + Cd+2(aq) + 2 (NO3)-1(aq)  CdS(s)
DF –
2 H+1(aq) + 2 (NO3)-1(aq)
SI – (NO3)-1
CdS(s)
NET: Cd+2(aq)
7.
+
+
S-2(aq)

CdS(s)
A solution of sulfuric acid is added to a solution of barium hydroxide.
H2SO4(aq)
+
Ba(OH)2(aq)

BaSO4(s)
+
2 H(OH)()
TIE: 2 H+1(aq) + (SO4)-2(aq) + Ba+2(aq) + 2 (OH)-1(aq)  BaSO4(s) + 2 H(OH)()
DF – H(OH)() , BaSO4(s)
NET: H+1(aq)
NET: Ba+2(aq)
(OH)-1(aq)

H(OH)()
+ (SO4)-2(aq)

BaSO4(s)
+
8.
Dilute sulfuric acid is added to a solution of calcium acetate.
H2SO4(aq)
+

Ca(C2H3O2)2(aq)
CaSO4(s)
+
2 H(C2H3O2)2(aq)
TIE: 2 H+1(aq) + (SO4)-2(aq) + Ca+2(aq) + 2 (C2H3O2)-1(aq)  CaSO4(s) + 2 H+1(aq) + 2 (C2H3O2)-1(aq)
SI – H+1(aq), (C2H3O2)-1(aq)
DF – CaSO4(s)
NET: Ca+2(aq)
9.
(SO4)-2(aq)
+

CaSO4(s)
Ammonium chloride solution is added to a solution of sodium hydroxide.
NH4Cl(aq)
+
NaOH(aq)

NaCl(aq)
+
NH4OH(aq)
NO REACTION
10.
A precipitate is formed when solutions of sodium sulfite and calcium chloride are mixed.
Na2SO3(aq)
+
CaCl2(aq)

CaSO3(s)
+
2 NaCl(aq)
TIE: 2 H+1(aq) + (SO3)-2(aq) + Ca+2(aq) + 2 Cl-1(aq)  CaSO3(s) + 2 Na+1(aq) + 2 Cl-1(aq)
SI – Na+1(aq), Cl-1(aq)
DF – CaSO3(s)
NET: Ca+2(aq)
11.
SO3-2(aq)
+

CaSO3(s)
Solutions of silver nitrate and sodium sulfide are mixed.
2 AgNO3(aq)
+
Na2S(aq)

2 NaNO3(aq)
+
Ag2S(s)
TIE: 2 Ag+1(aq) + 2 (NO3)-1(aq) + 2 Na+1(aq) + S-2(aq)  2 Na+1(aq) + 2 (NO3)-1 (aq) + Ag2S(s)
SI – Na+1(aq), (NO3)-1(aq)
DF – Ag2S(s)
NET: Ag+1(aq) + S-2(aq)  Ag2S(s)
12.
Solutions of sodium fluoride and dilute hydrochloric acid are mixed.
NaF(aq)
+
HCl(aq)
NO REACTION

HF(aq)
+
NaCl(aq)
13.
A saturated solution of barium hydroxide is mixed with a solution of iron (III) sulfate.
3 Ba(OH)2(aq)
+

Fe2(SO4)3(aq)
2 Fe(OH)3(s)
+
3 BaSO4(s)
TIE: 3 Ba+2(aq) + 6 (OH)-1aq) + 2 Fe+2(aq) + 3 (SO4)-2(aq) 
DF –
14.
2 Fe(OH)3(s)
+
3 BaSO4(s)
Fe(OH)3(s), BaSO4(s)
NET: Fe+2(aq)
+
(OH)-1(aq)
NET: Ba+2(aq)
+
(SO4)-2(aq)

Fe(OH)3(s)

BaSO4(s)
A solution of ammonium sulfate is added to a potassium hydroxide solution.
(NH4)2SO4(aq)
+

2 KOH(aq)
K2SO4(aq)
+
2 (NH4)OH(aq)
NO REACTION
15.
A solution of ammonium sulfate is added to a saturated solution of barium hydroxide.
(NH4)2SO4(aq)
+

Ba(OH)2(aq)
BaSO4(s)
+
2 (NH4)OH(aq)
TIE: 2 (NH4) +1(aq) + (SO4)-2(aq) + Ba+2(aq) + (OH)-1(aq)  BaSO4(s) + 2 (NH4)+1(aq) + 2 (OH)-1(aq)
DF –
NET: Ba+2(aq)
16.
SI – (NH4)+1(aq), (OH)-1(aq)
BaSO4(s)
+
(SO4)-2(aq)

BaSO4(s)
Acetic acid solution is added to a solution of potassium hydroxide.
H(C2H3O2)(aq)
+
KOH(aq)
TIE: H+1(aq) + (C2H3O2)-1(aq)
DF –
+
+
K(C2H3O2)(aq)
+
H(OH)()
K+1(aq) + (OH)-1(aq)
SI – K+1(aq), (C2H3O2)-1(aq)
H(OH)()
NET: H+1(aq)

(OH)-1(aq)

H(OH)()

K+1(aq) + (C2H3O2) -1(aq)
+
H(OH)()
17.
Dilute sulfuric acid is added to solid calcium fluoride.
H2SO4(aq)
+
CaF2(s)

CaSO4(s)
+
TIE: 2 H+1(aq) + SO4-2(aq) + CaF2(s) 
CaSO4(s)
NET: Ca+2(aq)
2 H+1(aq) + 2 F-1(aq)
+
(SO4)-2(aq)

+
2 H+1(aq) + 2 F-1(aq)
CaSO4(s)
Dilute sulfuric acid is added to solid calcium fluoride.
H2SO4(aq)
+
CaF2(s)

CaSO4(s)
+
TIE: 2 H+1(aq) + SO4-2(aq) + CaF2(s) 
2 HF(aq)
CaSO4(s)
SI – H+1(aq)
DF – CaSO4(s)
NET: Ca+2(aq)
18.
+
SI – H+1(aq)
DF – CaSO4(s)
17.
2 HF(aq)
+
(SO4)-2(aq)

CaSO4(s)
Dilute hydrochloric acid is added to a dilute solution of mercury (I) nitrate.
HCl(aq)
+
HgNO3(aq)

HgCl(aq)
+
HNO3(aq)
NO REACTION
19.
Dilute sulfuric acid is added to a solution of lithium chlorate.
H2SO4(aq)
+

2 LiClO3(aq)
Li2SO4(aq)
+
2 HClO3(aq)
NO REACTION
20.
Dilute zinc chloride is added to a solution of potassium sulfite.
K2SO3(aq)

2 KCl(aq)
TIE: Zn+2(aq) + 2 Cl-1(aq)
+
2 K+1(aq) + (SO3)-2(aq)
ZnCl2(aq)
+
ZnSO3(s)

SI – K+1(aq), Cl-1(aq)
DF – ZnSO3(s)
NET: Zn+2(aq)
+
+
(SO3)-2(aq)

ZnSO3(s)
2 K+1(aq) + 2 Cl-1(aq)
+
ZnSO3(s)
21.
A solution of sodium sulfide is added to a solution of cobalt (III) nitrate.
3 Na2S(aq)
+

2 Co(NO3)3(aq)
Co2S3 (s)
+
6 NaNO3(aq)
TIE: 6 Na+1(aq) + 3 S-2(aq) + 2 Co+3(aq) + 6 (NO3)-1(aq) 
+
6 Na+1(aq) + 6 (NO3)-1(aq)
SI – Na+1(aq), (NO3)-1(aq)
DF – Co2S3(s)
NET: Co+3(aq)
22.
Co2S3(s)
S-2(aq)
+

Co2S3(s)
A solution of sodium hydroxide is added to a solution of ammonium chloride.
NaOH(aq)
+

NH4Cl(aq)
NH4OH(aq)
+
NaCl(aq)
NO REACTION
23.
A solution of ammonium oxide is added to a solution of lead (IV) acetate.
2 (NH4)2O(aq)
+
Pb(C2H3O2)4(aq)

PbO2(s)
+
4 NH4(C2H3O2)(aq)
TIE: 4 (NH4)+1(aq) + 2 O-2(aq) + Pb+4(aq) + 4 (C2H3O2)-1(aq)  PbO2(s) + 4 (NH4)+1(aq) + 4 (C2H3O2)-1(aq)
SI – (NH4)+1(aq), (C2H3O2)-1(aq)
DF – PbO2(s)
NET: Pb+4(aq)
24.
O-2(aq)
+

PbO2(s)
Dilute sulfuric acid is added to a solution of barium chloride.
H2SO4(aq)
+
BaCl2(aq)

BaSO4(s)
+
2 HCl(aq)
TIE: 2 H+1(aq) + (SO4)-2(aq) + Ba+2(aq) + 2 Cl-1(aq)  BaSO4(s)
25.
2 H+1(aq) + 2 Cl-1(aq)
SI – H+1(aq), Cl-1(aq)
DF – BaSO4(s)
NET: Ba+2(aq)
+
(SO4)-2(aq)
+

BaSO4(s)
Solutions of zinc sulfate and sodium phosphate are mixed.
3 ZnSO4(aq)
+
2 Na3PO4(aq)

3 Na2SO4(aq)
+
Zn3(PO4)2(s)
TIE: 3 Zn+2(aq) + 3 (SO4)-2(aq) + 6 Na+1(aq) + 2 (PO4)-3(aq)  6 Na+1(aq) + 3 (SO4)-2(aq) + Zn3(PO4)2(s)
SI – Na+1(aq), (SO4)-2(aq)
DF – Zn3(PO4)2(s)
Zn+2(aq)
+
(PO4)-3(aq)

Zn3(PO4)2(s)
26.
Solutions of silver nitrate and lithium bromide are mixed.
AgNO3(aq)
+
LiBr(aq)

TIE: Ag+1(aq) + (NO3)-1(aq)
LiNO3(aq)
AgBr(s)
Li+1(aq) + Br-1(aq)
+

NET: Ag+1(aq)
+
AgBr(s)
+
Br-1(aq)

AgBr(s)
Solutions of sodium iodide and lead (II) nitrate are mixed.
2 NaI(aq)
+

Pb(NO3)2(aq)
PbI2(s)
+
2 NaNO3(aq)
TIE: 2 Na+1(aq) + 2 I-1(aq) + Pb+2(aq) + 2 (NO3)-1(aq)

PbI2(s)
+
2 Na+1(aq) + 2 (NO3)-1(aq)
SI – Na+1(aq), (NO3)-1(aq)
DF – PbI2(s)
NET: Pb+2(aq)
28.
Li+1(aq) + (NO3)-1(aq)
SI – Li+1(aq), (NO3)-1(aq)
DF – AgBr(s)
27.
+
+
I-1(aq)

PbI2(s)
Solutions of copper (I) nitrate and cesium hydroxide are mixed.
CuNO3(aq)
+

CsOH(aq)
CsNO3(aq)
+
CuOH(s)
TIE: Cu+1(aq) + (NO3)-1(aq) + Cs+1(aq) + (OH)-1(aq)  CsNO3(aq) + CuOH(s)
SI – Cs+1(aq), (NO3)-1(aq)
DF – CuOH(s)
NET: Cu+1(aq)
29.
+
(OH)-1(aq)

CuOH(s)
Sulfuric acid and potassium hydroxide are mixed.
H2SO4(aq)
+
2 KOH(aq)

K2SO4(aq)
+
2 H(OH)()
TIE: 2 H+1(aq) + (SO4)-2(aq) + 2 K+1(aq) + 2 (OH)-1(aq)  2 K+1(aq) + (SO4)-2(aq) + 2 H(OH)()
DF –
SI – K+1(aq), (SO4)-2(aq)
H(OH)()
NET: H+1(aq)
+
(OH)-1(aq)

H(OH)()
30.
A solution of copper (II) sulfate is added to a solution of barium hydroxide.
CuSO4(aq)
+
TIE: Cu+2(aq) + (SO4)-2(aq)
DF –
31.

Ba(OH)2(aq)
BaSO4(s)
+
+
BaSO4(s)
+
Cu(OH)2(s)
Ba+2(aq) + (OH)-1(aq)

BaSO4(s)
+
Cu(OH)2(s)
Cu(OH)2(s)
NET: Ba+2(aq)
+
(SO4)-2(aq)

BaSO4(s)
NET: Cu+2(aq)
+
(OH)-1(aq)

Cu(OH)2(s)
An excess of sodium hydroxide solution is added to a solution of magnesium nitrate.
2 NaOH(aq)
+

Mg(NO3)2(aq)
Mg(OH)2(s)
+
2 NaNO3(aq)
TIE: 2 Na+1(aq) + 2 (OH)-1(aq) + Mg+2(aq) + 2 (NO3)-1(aq)  Mg(OH)2(s) + 2 Na+1(aq) + 2 (NO3)-1(aq)
DF –
NET: Mg+2(aq)
32.
SI – Na+1(aq), (NO3)-1(aq)
Mg(OH)2(s)
+
(OH)-1(aq)
Mg(OH)2(s)
Solid ammonium carbonate is added to a saturated solution of barium acetate.
(NH4)2CO3(s)
+
Ba(C2H3O2)2(aq)
TIE: (NH4)2CO3(s)
+
NET: Ba+2(aq)

BaCO3(s)
Ba+2(aq) + 2 (C2H3O2)-1(aq)
+

2 NH4C2H3O2(aq)
BaCO3(s)
+
2 NH4(aq) + 2 (C2H3O2)-1(aq)
SI – (C2H3O2)-1(aq)
DF – BaCO3(s)
33.

+
(CO3)-2(aq)

BaCO3(s)
A solution of nickel (III) chloride is added to a solution of sodium sulfide.
2 NiCl3(aq)
+
3 Na2S(aq)

6 NaCl(aq)
+
Ni2S3(s)
TIE: 2 Ni+3(aq) + 6 Cl-1(aq) + 6 Na+1(aq) + 3 S-2(aq)  6 Na+1(aq) + 6 Cl-1(aq) + Ni2S3(s)
SI – Na+1(aq), Cl-1(aq)
DF – Ni2S3(s)
NET: Ni+3(aq)
+
S-2(aq)

Ni2S3(s)