Name three oxoacids of nitrogen. Write the disproportionation reaction of that oxoacid of nitrogen in which nitrogen is in +3 oxidation state.

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Solution

Oxoacids of Nitrogen

Three oxoacids of nitrogen are:
(1) Nitric acid $(H N O_{3})$
(2) Nitrous acid $(H N O_{2})$
(3) Hyponitrous acid $(H_{2} N_{2} O_{2})$

The oxidation state of nitrogen in the given oxoacids are:
(1) $H N O_{3}$ - oxidation state of N = +5
(2) $(H N O_{2})$ -oxidation state of N = +3
(3) $(H_{2} N_{2} O_{2})$ -oxidation state of N = +1

Disproportionation reaction of oxoacids of nitrogen

In Nitrous acid $(H N O_{2})$ nitrogen has +3 oxidation state.
Thus disproportionation reaction of $H N O_{2}$ is given as:
$H N O_{2} \to H N O_{3} + 2 N O + H_{2} O$

Oxidation state:
N = +3 N = +5 N = +2

Thus, in the above reaction $H N O_{2}$ is getting reduced to NO and it is getting oxidized to $H N O_{3}$ simultaneously.

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