Consider the reactions:

(a) $$H_{ 3 }PO_{ 2 \; (aq) } \; + \; 4 \; AgNO_{ 3 \; (aq) } \; + \; 2 \; H_{ 2 }O_{ (l) } \;$$

$$\rightarrow \; H_{ 3 }PO_{ 4 \; (aq) } \; + \; 4 \; Ag_{ (s) } \; + \; 4 \; HNO_{ 3 \; (aq) }$$

(b) $$H_{ 3 }PO_{ 2 \; (aq) } \; + \; 2 \; CuSO_{ 4 \; (aq) } \; + \; 2 \; H_{ 2 }O_{ (l) } \;$$

$$\rightarrow \; H_{ 3 }PO_{ 4 \; (aq) } \; + \; 2 \; Cu_{ (s) } \; + \; H_{ 2 }SO_{ 4 \; (aq) }$$

(c) $$C_{ 6 }H_{ 5 }CHO_{ (l) } \; + \; 2 \; [Ag(NH_{ 3 })_{ 2 }]^{ + }_{ (aq) } \; + \; 3 \; OH^{ – }_{ (aq) } \;$$

$$\rightarrow \; C_{ 6 }H_{ 5 }COO^{ – }_{(aq)} \; + \; 2\; Ag_{ (s) } \; + \; 4 \; NH_{ 3 \; (aq)} \; + \; 2 \; H_{ 2 }O_{ (l) }$$

(d) $$C_{ 6 }H_{ 5 }CHO_{ (l) } \; + \; 2 \; Cu^{ 2+ }_{ (aq) } \; + \; 5 \; OH^{ – }_{ (aq) } \; \rightarrow$$No change is observed

What inference do you draw about the behavior of $$Ag^{ + }$$ and $$Cu^{ 2+ }$$ from these reactions?

Asked by Pragya Singh | 1 year ago |  54

##### Solution :-

Ag+ and $$Cu^{ 2+ }$$ behaves as oxidizing agent in reactions (i) and (ii) respectively.

In reaction (iii), $$Ag^{ + }$$ oxidizes $$C_{ 6 }H_{ 5 }CHO$$ to $$C_{ 6 }H_{ 5 }COO^{ – }$$

In reaction (iv), $$Cu^{ 2+ }$$ cannot oxidize $$C_{ 6 }H_{ 5 }CHO$$

Therefore, $$Ag^{ + }$$is a stronger oxidizing agent compared to $$Cu^{ 2+ }$$.

Answered by Abhisek | 1 year ago

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