Question:
Consider the reactions:

(a) H₃PO_2(aq) + 4 AgNO_3(aq) + 2 H₂O_(l) → H₃PO_4(aq) + 4Ag_(s)+ 4HNO_3(aq)

(b) H₃PO_2(aq) + 2CuSO_4(aq) + 2 H₂O_(l) → H₃PO_4(aq) + 2Cu_(s) + H₂SO_4(aq)

(c) C₆H₅CHO_(l) + 2 [Ag (NH₃)₂]⁺_(aq) + 3OH^-_(aq) → C₆H₅COO^-_(aq) + 2Ag_(s)+ 4NH_3(aq) + 2 H₂O_(l)

(d) C₆H₅CHO_(l) + 2Cu²⁺_(aq) + 5OH^-_(aq)→ No change observed.

What inference do you draw about the behaviour of Ag⁺and Cu²⁺from these reactions?

Answer:

Ag⁺and Cu²⁺ act as oxidising agents in reactions (a) and (b) respectively.

In reaction (c), Ag⁺ oxidises C₆H₅CHO to C₆H₅COO^-, but in reaction (d), Cu²⁺ cannot oxidise C₆H₅CHO.

Hence, we can say that Ag⁺ is a stronger oxidising agent than Cu²⁺.

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