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Question

# Which of the following can act as oxidising as well as reducing agent ?

A
H2O2
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B
SO3
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C
H2SO4
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D
HNO3
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Solution

## The correct option is C H2O2A species can act as oxidizing as well as reducing species, if it can get reduced and oxidized further, respectively.A. H2O2:oxidation number of O is: 2×1+2x=0x=−1Since O can have oxidation number as -2 and 0 when reduced and oxidized respectively as shown below in the reaction.Reduction of peroxide: -1 -2H2O2+2H++2e−→2H2OOxidation of peroxide: -1 0H2O2→O2+2H++2e−B. SO3: oxidation number of S is:x+3×(−2)=0x=+6maximum oxidation state of S is +6 and can not be reduced further, thus can act as only reducing agent and not as oxidizing agent.C. H2SO4: oxidation number of S is:2×1+x+4×(−2)=0x=+6maximum oxidation state of S is +6 and can not be reduced further, thus can act as only reducing agent and not as oxidizing agent.D. HNO3: oxidation number of N is:1+x+3×(−2)=0x=+5maximum oxidation state of N is +5 and can not be reduced further, thus can act as only reducing agent and not as oxidizing agent.therefore H2O2 can act as oxidising as well as reducing agent.

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