Answer:
The behaviour is linked with the
oxidation state of phosphorus atom in the two acids. In phosphorus acid \[({{H}_{3}}P{{O}_{3}})\]
the oxidation state of P is + 3. It is in a position to increase its oxidation
state (acts as reducing agent) as well as decrease it (acts as oxidising
agent). The oxidation state of phosphorus in phosphoric acid \[({{H}_{3}}P{{O}_{3}})\]
is + 5. Since it cannot increase it beyond 5, it cannot act as a reducing
agent. However, it can behave as oxidising agent by decreasing its oxidation
state.
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