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Question

Given: E0(Sn2+/Sn4+)=0.15 V,E0(Hg2+2/Hg2+)=0.92 V and E0(Pb2+/PbO2)=1.45 V.
Based on this data, which of the following statements is incorrect?

A
Sn4+ is a stronger oxidizing agent than Pb4+
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B
Sn2+ is a stronger reducing agent than Hg2+2
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C
Hg2+ is a stronger oxidizing agent than Pb4+
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D
Pb2+ is a stronger reducing agent than Sn2+
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Solution

The correct option is B Sn2+ is a stronger reducing agent than Hg2+2
The oxidising agent is reduced and reducing agent is oxidised in the process. So a better oxidising agent is the one having more tendency to get reduced i.e. its reduction potential is high.
So, higher reduction potential means better oxidising agent.
Similalry, lower reduction potential means better reducing agent. The given data is of oxidation potential but reduction potential = - oxidation potential. So, reduction potential follows the order:
Pb4+<Hg2+<Sn4+
As Sn4+ to Sn2+ has a reduction potential of 0.15 V whereas Pb4+ to Pb2+ has a reduction potential of 1.45 V which is lesser than 0.15 V. So, Sn4+ is stronger oxidizing agent than Pb2+.

Similarly we can check the statements in options (c) and (d) and verify that these statements are correct.
For option (b), Sn2+ is not a better reducing agent than
Hg2+2 because a better reducing agent needs higher value of oxidation potential but Sn2+ has smaller oxidation potential(0.15 V) than Hg2+2(0.92 V).
Hence, (b) is the incorrect statement.

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