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

H_{2} O_{2}

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S O_{3}

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H_{2} S O_{4}

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H N O_{3}

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Solution

The correct option is C $H_{2} O_{2}$
A species can act as oxidizing as well as reducing species, if it can get reduced and oxidized further, respectively.
A. $H_{2} O_{2}$ :
oxidation number of $O$ is: $2 \times 1 + 2 x = 0$
$x = - 1$
Since $O$ can have oxidation number as -2 and 0 when reduced and oxidized respectively as shown below in the reaction.
Reduction of peroxide:
-1 -2
$H_{2} O_{2} + 2 H^{+} + 2 e^{-} \to 2 H_{2} O$
Oxidation of peroxide:

-1 0
$H_{2} O_{2} \to O_{2} + 2 H^{+} + 2 e^{-}$
B. $S O_{3}$ : oxidation number of $S$ is:
$x + 3 \times (- 2) = 0$
$x = + 6$
maximum 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. $H_{2} S O_{4}$ : oxidation number of $S$ is:
$2 \times 1 + x + 4 \times (- 2) = 0$
$x = + 6$
maximum 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. $H N O_{3}$ : oxidation number of $N$ is:
$1 + x + 3 \times (- 2) = 0$
$x = + 5$
maximum 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 $H_{2} O_{2}$ can act as oxidising as well as reducing agent.

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