Question

A piece of solid Zn metal is put into an aqueous solution of SnSO4. Write the net ionic equation for any single-replacement redox reaction that may be predicted.

Answer 1

Answer:

$Zn (s) + SnSO_4 (aq)\longrightarrow ZnSO_4 (aq) + Sn (s)$

Explanation:

Hi, when adding Zn to the solution because of its high reactivity it will displace the Sn. This process is a redox reaction.

First step is to identify the compound that oxidates and the  compound that reduces. The Zn has a high oxidation potencial so it will oxidate:

Oxidation hemireaction: $Zn (s) \longrightarrow Zn^+^2 (aq) + 2e^-$

The reduction reaction will be performed by the Sn:

Reduction hemireaction: $Sn^+^2 (aq) + 2e^- \longrightarrow Sn (s)$

Writting the net redox equation:

$Zn (s) + Sn^+^2 (aq) + 2e^-\longrightarrow Zn^+^2 (aq) + 2e^- + Sn (s)$

$Zn (s) + SnSO_4 (aq)\longrightarrow ZnSO_4 (aq) + Sn (s)$

Answer 2

Not complete the sure, but I think it’s

Zn(s) + SnSO4(aq) —> ZnSO4(aq) + Sn(s)