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This is similar to how Cu reacts with NH3.When NH3(aq) is added to a green solution containing Ni2+(aq) ions, a grey-green precipitate is formed. This precipitate dissolves in an excess of NH3(aq) to give a blueviolet solution. Suggest an explanation for these observations, showing your reasoning and including equations for the reactions you describe.
The green ppt. is Ni(OH)2. How are we supposed to get that ?
On adding drops of NH3, it ionizes:
NH3 + H2O <---> NH4+ + OH-
The Ni2+ (aq) is in fact [Ni(H2O)6]2+ (aq). A ligand exchange reaction occurs upon addition of OH-:
[Ni(H2O)6]2+ (aq) + 2OH-(aq) <----> Ni(H2O)4(OH)2 (s) + 2H2O
The solid produced is the ppt. Sometimes we ignore the water ligands and simply write Ni(OH)2. Same thing applies for copper. Only the color differs.
When excess ammonia is added, more ligands are replaced, this time by molecular NH3:
Ni(H2O)4(OH)2 (s) + 4NH3(aq) ------> [Ni(NH3)4(H2O)2]2+ (aq) + 2H2O + 2OH- (aq)