Consider the reactions-a H 3 PO 2 aq -4 AgNO 3 aq -2 H 2 O l - H 3 PO 4 aq -4 Ag s -4 HNO 3 aq b H 3 PO 2 aq -2 CuSO 4 aq -2 H 2 O l - H 3 PO 4 aq -2 Cu s - H 2 SO 4 aq c C 6 H 5 CHO l -2- Ag NH 32- aq -3 OH - aq - C 6 H 5 COO - aq -2 Ag s -4 NH 3 aq -2 H 2 O l d C 6 H 5 CHO l -2 Cu 2- aq -5 OH - aq - No change observed-What inference do you draw about the behaviour of Ag -and Cu 2- from these reactions-

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Byju's Answer

Standard XII

Chemistry

Types of Redox Reactions

Consider the ...

Question

Consider the reactions:

(a) H₃PO₂(aq) + 4 AgNO₃(aq) + 2 H₂O(l) → H₃PO₄(aq) + 4Ag(s) + 4HNO₃(aq)

(b) H₃PO₂(aq) + 2CuSO₄(aq) + 2 H₂O(l) → H₃PO₄(aq) + 2Cu(s) + H₂SO₄(aq)

(c) C₆H₅CHO(l) + 2[Ag (NH₃)₂]⁺(aq) + 3OH^–(aq) → C₆H₅COO^–(aq) + 2Ag(s) + 4NH₃ (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?

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Solution

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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