Question

explain why HNO2 behaves both as oxidising as well as reducing agent?

Answer 1

in HNO2 oxidizing number of nitrogen is +3 and can either lose or gain electrons and hence as both .
as oxidizing agent :
2HNO2 + 2HI -------> 2H2O + 2NO2 + I2

as reducing agent :
HNO2 + Br2 + H2O --------> 2HNO3 + 2HBr

Answer 2

Answer:

In $HNO_2$, the oxidation number of nitrogen is +3. As a result, it can easily change its oxidation state by increasing from -3 to +5. Hence it acts as an oxidizing as well as a reducing agent

Explanation:

• Oxidation values for nitrogen range from -3 to +5.
• In $HNO_2$, the oxidation number of nitrogen is +3. As a result, it can increase or decrease within the range of -3 to 5.
• As a result, it functions as both an oxidizing and a reducing agent.
• For example, $HNO_2$ can be reduced to $NH_3$, which has a -3 oxidation state, or it can be oxidized to $HNO_3$, which has a +5 oxidation state.
• While in  $HNO_3$, the nitrogen oxidation number is +5. As a result, this can't go higher than +5.
• As a result, it functions as an oxidizer.