Why is copper hydroxide soluble in excess of ammonia solution and not soluble in excess of caustic potash?

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Solution

1. When the concentration of ammonia solutions is very high, divalent copper ions inpresenceof dioxygen, catalyze ammonia oxidation, giving rise to copper ammine nitrites: $C u (N O_{2})_{2} (N H_{3}) n$ .
2. Copper hydroxide acts as a weak base in aqueous solution.

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Q. A salt giving a white precipitate with sodium hydroxide and soluble in excess of ammonia is:

The hydroxide of which metal ion is soluble in excess of sodium hydroxide solution.

Q. Name
(a) a metallic hydroxide soluble in excess of NH₄OH.
(b) a metallic oxide soluble in excess of caustic soda solution.
(c) a strong alkali
(d) a weak alkali
(e) two coloured metal ions.
(f) two bases which are not alkalis but dissolve in strong alkalis.
(g) a coloured metallic oxide which dissolves in alkalis to yield colourless solutions.

Ammonia forms the complex ion $[C u (N H_{3})_{4}]^{+ 2}$ with copper ions in alkaline solutions but not in acidic solutions. What is the reason for it?

___ is insoluble in cold water but soluble in excess of ammonia solution.

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Why is copper hydroxide soluble in excess of ammonia solution and not soluble in excess of caustic potash?

1. When the concentration of ammonia solutions is very high, divalent copper ions inpresenceof dioxygen, catalyze ammonia oxidation, giving rise to copper ammine nitrites: Cu(NO2)2(NH3)n. 2. Copper hydroxide acts as a weak base in aqueous solution.

1. When the concentration of ammonia solutions is very high, divalent copper ions inpresenceof dioxygen, catalyze ammonia oxidation, giving rise to copper ammine nitrites: $C u (N O_{2})_{2} (N H_{3}) n$ .
2. Copper hydroxide acts as a weak base in aqueous solution.