1. Copper is above silver in the activity series. Thus Cu metal will displace Ag+ ions from
solution, forming Cu2+ ions and metallic Ag.
Observation: The reddish brown copper metal dissolves and silver metal precipitates out. The
colorless Ag+ solution turns blue due to Cu2+ ions formed.
2. Molecular equation:
Cu(s) + 2 AgNO3(aq) => 2 Ag(s) + Cu(NO3)2(aq)
3. Complete ionic equation (obtained by expanding soluble ions in molecular equation):
Cu(s) + 2 Ag+(aq) + 2 NO3-(aq) => 2 Ag(s) + Cu2+(aq) + 2 NO3-(aq)
4. Net ionic equation (obtained by cancelling common ions in complete ionic equation):
Cu(s) + 2 Ag+(aq) => 2 Ag(s) + Cu2+(aq)
Solution
1. Copper is above silver in the activity series. Thus Cu metal will displace Ag+ ions from
solution, forming Cu2+ ions and metallic Ag.
Observation: The reddish brown copper metal dissolves and silver metal precipitates out. The
colorless Ag+ solution turns blue due to Cu2+ ions formed.
2. Molecular equation:
Cu(s) + 2 AgNO3(aq) => 2 Ag(s) + Cu(NO3)2(aq)
3. Complete ionic equation (obtained by expanding soluble ions in molecular equation):
Cu(s) + 2 Ag+(aq) + 2 NO3-(aq) => 2 Ag(s) + Cu2+(aq) + 2 NO3-(aq)
4. Net ionic equation (obtained by cancelling common ions in complete ionic equation):
Cu(s) + 2 Ag+(aq) => 2 Ag(s) + Cu2+(aq).
1. Copper is above silver in the activity series. Thus Cu metal will.pdf
1. 1. Copper is above silver in the activity series. Thus Cu metal will displace Ag+ ions from
solution, forming Cu2+ ions and metallic Ag.
Observation: The reddish brown copper metal dissolves and silver metal precipitates out. The
colorless Ag+ solution turns blue due to Cu2+ ions formed.
2. Molecular equation:
Cu(s) + 2 AgNO3(aq) => 2 Ag(s) + Cu(NO3)2(aq)
3. Complete ionic equation (obtained by expanding soluble ions in molecular equation):
Cu(s) + 2 Ag+(aq) + 2 NO3-(aq) => 2 Ag(s) + Cu2+(aq) + 2 NO3-(aq)
4. Net ionic equation (obtained by cancelling common ions in complete ionic equation):
Cu(s) + 2 Ag+(aq) => 2 Ag(s) + Cu2+(aq)
Solution
1. Copper is above silver in the activity series. Thus Cu metal will displace Ag+ ions from
solution, forming Cu2+ ions and metallic Ag.
Observation: The reddish brown copper metal dissolves and silver metal precipitates out. The
colorless Ag+ solution turns blue due to Cu2+ ions formed.
2. Molecular equation:
Cu(s) + 2 AgNO3(aq) => 2 Ag(s) + Cu(NO3)2(aq)
3. Complete ionic equation (obtained by expanding soluble ions in molecular equation):
Cu(s) + 2 Ag+(aq) + 2 NO3-(aq) => 2 Ag(s) + Cu2+(aq) + 2 NO3-(aq)
4. Net ionic equation (obtained by cancelling common ions in complete ionic equation):
Cu(s) + 2 Ag+(aq) => 2 Ag(s) + Cu2+(aq)
