# 8.8 While sulphur dioxide and hydrogen peroxide can act as oxidising as well as reducing agents in their reactions, ozone and nitric acid act only as oxidants. Why?

• sulphur dioxide $(SO_{2})$ here oxidation state of sulphur is +4  and the range of oxidation number of S is from -2 to +6. It means it can accept an electron and lose as well, therefore, it can behave as oxidant and reductant both.
• In case of hydrogen peroxide $(H_{2}O_{2})$ oxidation state is -1 and the oxidation state of O can vary from 0 to -2. So it shows both oxidizing and reducing properties.
• For $HNO_{3}$ , Nitrogen has +5 oxidation state and it varies from +5 to -3. So it only accepts electrons. The oxidation state of N only decreases. Hence it acts as only oxidants.
• And in case of $O_{3}$ , the oxidation state of O is zero(0) and the range of oxidtion number of O is 0 to -2. It only decreases in this case also so therefore it acts as only oxidants.

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