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(D) substance can act as both an oxidising and a reducing agent if the central atom is in an intermediate oxidation state.$1$. In $H_2O_2$,the oxidati

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$H_3PO_4$

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(D) substance can act as both an oxidising and a reducing agent if the central atom is in an intermediate oxidation state.$1$. In $H_2O_2$,the oxidation state of $O$ is $-1$,which can increase to $0$ (reducing) or decrease to $-2$ (oxidising).$2$. In $H_2SO_3$,the oxidation state of $S$ is $+4$,which can increase to $+6$ (reducing) or decrease to lower values (oxidising).$3$. In $HNO_2$,the oxidation state of $N$ is $+3$,which can increase to $+5$ (reducing) or decrease to lower values (oxidising).$4$. In $H_3PO_4$,the oxidation state of $P$ is $+5$,which is its maximum oxidation state. Therefore,it can only act as an oxidising agent and cannot be further oxidised to act as a reducing agent.

The compound that cannot act both as an oxidising and reducing agent is:

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