Explain why $H N O_{3}$ acts only as oxidising agent while $H N O_{2}$ can act both as a reducing agent and an oxidising agent?

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Solution

Nitrogen can have oxidation numbers from $- 3$ to $+ 5$ . The oxidation number fo nitrogen in $H N O_{3}$ is $+ 5$ . Thus, increase in oxidation number beyond $+ 5$ cannot occur. Hence, $H N O_{3}$ cannot act as reducing agent. The oxidation number of nitrogen in $H N O_{3}$ can only decrease; thus it acts as an oxidising agent. In $H N O_{2}$ , the oxidation number of nitrogen is $+ 3$ . Thus, it can increase or decrease within the range $- 3$ to $+ 5$ . Hence, it can act as an oxidising as well as a reducing agent.

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