In an ammoniacal solution,copper ions form th | vedclass

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(B) The formation of the complex $[Cu(NH_3)_4]^{2+}$ requires free $NH_3$ molecules to act as ligands.In an acidic solution,the concentration of $H^+$

Vedclass · Accepted Answer

In an acidic solution,protons combine with ammonia to form $NH_4^+$ ions,leaving no free ammonia molecules available for complexation.

Vedclass · Answer

(B) The formation of the complex $[Cu(NH_3)_4]^{2+}$ requires free $NH_3$ molecules to act as ligands.In an acidic solution,the concentration of $H^+$ ions is high.These $H^+$ ions react with $NH_3$ (a base) to form ammonium ions: $NH_3 + H^+ \rightarrow NH_4^+$.Because the $NH_3$ is consumed to form $NH_4^+$,there are no free $NH_3$ molecules available to coordinate with the $Cu^{2+}$ ions to form the complex.

In an ammoniacal solution,copper ions form the complex ion $[Cu(NH_3)_4]^{2+}$,but this does not occur in an acidic solution. The reason for this is:

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