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Question

Balance the following reaction.
S+OHS2+S2O23

A
6OH+4S2S2+S2O23+3H2O
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B
6OH+5S2S2+3S2O23+2H2O
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C
6OH+S2S2+2S2O23+H2O
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D
None of these
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Solution

The correct option is A 6OH+4S2S2+S2O23+3H2O
The unbalanced redox equation is
S+OHS2+S2O23
Balance all atoms other than H and O.
3S+OHS2+S2O23
The oxidation number of S changes from 0 to -2. The change in the oxidation number of S is 2.
The oxidation number of S changes from 0 to 4. The change in the oxidation number of S is 4.
The increase in the oxidation number is balanced with decrease in the oxidation number by multiplying
S and S2 with 2.
4S+OH2S2+S2O23
O atoms are balanced by adding 2 water molecules on LHS.
4S+OH+2H2O2S2+S2O23
Hydrogen atoms are balanced by adding 5 H+ atoms on RHS
4S+OH+2H2O2S2+S2O23+5H+.
Since the reaction occurs in basic medium, 5 hydroxide ions are added on the either side
4S+OH+2H2O+5OH2S2+S2O23+5H++5OH.
On RHS five protons and five hydroxide ions forms five water molecules out of which two cancels out with two water molecule on RHS.
6OH+4S2S2+S2O23+3H2O
This is the balanced chemical equation.

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