Chapter 4: Worksheet #2b: Molecular, Net Ionic Equations, Solubility Rules, & Redox
1.
Write the net ionic equations for each of the following unbalanced molecular equations.
Na3PO4(aq)
+
3 AgNO3(aq)
3 Ag+(aq)
+
PO43–(aq)
Ag3PO4(s)
K2SO4(aq)
+
BaCl2(aq)
BaSO4(s)
Ba2+(aq)
SO42–(aq)
+
Hg2(NO3)2(aq)
+
+
+
Ag3PO4(s)
2 KCl(aq)
BaSO4(s)
CaCl2(aq)
Hg22+(aq) + 2 Cl–(aq)
2.
3 NaNO3(aq)
Ca(NO3)2(aq)
+
Hg2Cl2(s)
Hg2Cl2(s)
Using the solubility rules, predict the products, balance the equation, and write the
complete ionic and net ionic equations for each of the following reactions.
Pb(NO3)2(aq)
+
Pb2+(aq)
SO42–(aq)
+
AgClO3(aq)
+
KCl(aq)
Ag+(aq) + Cl–(aq)
3 KOH(aq)
Fe3+(aq)
ZnCl2(aq)
Zn2+(aq)
3 OH–(aq)
+
S2–(aq)
+
2 Na3PO4(aq)
3 Ca2+(aq)
H2S(aq)
+
+
3 CaCl2(aq)
2 PO43–(aq)
+
2 NaNO3(aq)
PbSO4(s)
AgCl(s)
+
KClO3(aq)
AgCl(s)
Fe(OH)3(s)
Fe(NO3)3(aq)
+
+
PbSO4(s)
Na2SO4(aq)
+
3 KNO3(aq)
Fe(OH)3(s)
ZnS(s)
+
2 HCl(aq)
ZnS(s)
Ca3(PO4)2(s)
Ca3(PO4)2(s)
+
6 NaCl(aq)
3.
Balance each of the following molecular equations and classify each as precipiation,
acid-base or oxidaion-reduction. If the reaction can be classified as oxidation/reduction,
label the element that is being reduced and the element being oxidized.
Na3PO4(aq)
+
3 AgNO3(aq)
3 NaNO3(aq)
+
Ag3PO4(s)
precipitation
2 HCl(aq)
+
Ca(OH)2(aq)
2 H2O(l)
+
CaCl2(aq)
acid-base
2 Na(s)
+
Na2S(s)
S(s)
oxidation-reduction; Na oxidized, S reduced
2 C2H6(g)
+ 7 O2(g)
4 CO2(g)
+
6 H2O(l)
+
H2(g)
oxidation-reduction; C oxidized, O reduced
2 Li(s)
+
2 H2O(l)
2 LiOH(s)
oxidation-reduction; Li oxidized, H reduced
K2SO4(aq)
+
BaCl2(aq)
BaSO4(s)
+
2 KCl(aq)
precipitation
Mg(s)
+
CuCl2(aq)
MgCl2(aq)
oxidation-reduction; Mg oxidized, Cu reduced
2 Hg(l)
2 HgO(s)
+
O2(g)
oxidation-reduction; O oxidized, Hg reduced
4 FeO(s)
+
O2(g)
2 Fe2O3(s)
oxidation-reduction; Fe oxidized, O reduced
2 Fe(s)
+
3 Br2(l)
2 FeBr3(s)
oxidation-reduction; Fe oxidized, Br reduced
+
Cu(s)