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Question

Balance the following in basic medium:

AsO3+3+MnO4AsO34+MnO2

A
3AsO3+3+2MnO4+H2O3AsO34+2MnO2+2OH
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B
3AsO3+3+2MnO4+4H2O3AsO34+3MnO2+2OH
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C
3AsO3+3+4MnO4+3H2O3AsO34+2MnO2+4OH
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D
None of these
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Solution

The correct option is A 3AsO3+3+2MnO4+H2O3AsO34+2MnO2+2OH
The unbalanced redox equation is as follows:
AsO33+MnO4AsO34+MnO2+H2O
All atoms other than H and O are balanced.
The oxidation number of As changes from +3 to +5. The change in the oxidation number of As is +2.
The oxidation number of Mn changes from +7 to +4. The change in the oxidation number of Mn is 3.
The increase in the oxidation number is balanced with decrease in the oxidation number by multiplying
AsO33 and AsO34 with 3 and multiplying MnO4 and MnO2 with 2.
3AsO33+2MnO43AsO34+2MnO2+H2O
O atoms are balanced.
3AsO33+2MnO43AsO34+2MnO2+H2O
Hydrogen atoms are balanced by adding 2 H+ atoms on the LHS.
3AsO33+2MnO4+2H+3AsO34+2MnO2+H2O
Since the reaction occurs in basic medium, add 2 hydroxide ions on both sides of the equation.
3AsO33+2MnO4+2H++2OH3AsO34+2MnO2+H2O+2OH
On LHS, 2 H+ ions combine with 2 OH ions to form 2 water molecules out of which, one water molecule cancels with one water molecule on RHS..
3AsO33+2MnO4+H2O3AsO34+2MnO2+2OH
This is the balanced chemical equation.

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