Ammonia forms the complex [Cu(NH_3)_4]^{2+} w | vedclass

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(D) In an alkaline solution,the equilibrium is: $Cu^{2+}_{(aq)} + 4NH_3 \rightleftharpoons [Cu(NH_3)_4]^{2+}$.In an acidic solution,the $H^+$ ions rea

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In acidic solution protons are coordinated with ammonia molecules forming $NH_4^+$ ions

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(D) In an alkaline solution,the equilibrium is: $Cu^{2+}_{(aq)} + 4NH_3 \rightleftharpoons [Cu(NH_3)_4]^{2+}$.In an acidic solution,the $H^+$ ions react with the lone pair of $NH_3$ to form $NH_4^+$ ions: $NH_3 + H^+ \rightarrow NH_4^+$.Since $NH_4^+$ does not have a lone pair of electrons,it cannot act as a ligand to form a coordinate bond with the $Cu^{2+}$ ion. Therefore,no complex is formed in an acidic solution.

Ammonia forms the complex $[Cu(NH_3)_4]^{2+}$ with copper ions in alkaline solution but not in acidic solution. The reason for this is

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