In the previous experiment aluminium citrate was not destructed by oxidants (ammonium persulfate and hydrogen peroxide). No precipitate of aluminium hydroxide occurred.

Another possible way to destruct the complex and precipitate aluminium hydroxide is the addition of an alkali (ammonia or potassium hydroxide).

In the first experiment an excess of aqueous ammonia was added to the solution of aluminium citrate. No precipitate of aluminium hydroxide was formed.

In the second experiment the solution of aluminium citrate was added to an excess of a solution of potassium hydroxide. Also, the precipitate of aluminium hydroxide was not occurred.

(In case of the destruction of aluminium citrate the precipitate of Al(OH)₃ must occur, whereupon the precipitate will dissolve in KOH and not dissolve in NH₃).

Therefore, the alkalis did not destruct aluminium citrate in a solution. This proves that aluminium citrate is a strong complex. For example, EDTA forms such complexes with polyvalent cations.

Adding of hydrogen peroxide to the solutions of aluminium citrate with an excess of ammonia or potassium hydroxide did not lead to the precipitation of aluminium hydroxide also. (The combinations of an alkali and an oxidant did not work as well).

An aqueous solution containing 1:1 molar ratio of ethylenediammonium chloride (enH2Cl2) and copper chloride (CuCl2) was left to evaporate for 5 days. After 5 days the green solution was gone and flakes of golden yellow crystals were formed.

This compound is a rare case of the tetrachlorocuprate ion being able to be crystallized from aqueous solution
https://www.reddit.com/r/chemistry/comments/17j22se/platelike_crystals_of_ethylenediammonium/

Copper(II)-acetylacetonate made by the reaction of copper(II)-hydroxide with acetylacetone

Всё-таки надо так:
[Cu(NH3)4](OH)2 и т.д.