Copper and copper alloys suffers rapid attack by concentrated solution of ammonium hydroxide to form a soluble complex of copper-ammonium compound. In some cases, the corrosion of copper exposed to dilute solution of ammonium hydroxide is low. Copper specimen submerged at room temperature for one week in 0.01N ammonium hydroxide solution suffered a weight loss of 3.5mil/yr.
The rates of dissolution of polycrystalline metallic copper in aqueous ammonium hydroxide solutions have been determined under various experimental conditions. Over a considerable range of conditions the dissolution has been found to be autocatalytic. An empirical equation is presented which represents the autocatalytic rate data with an average deviation of $\ce{\pm4\%}$. The rate equation is discussed in terms of a mechanism which assumes that the rate controlling process is the removal of cuprous ion species from the copper solution interface by diffusion. Data are also given for an essentially zero-order rate of dissolution observed when the dissolving medium was concentrated with respect to oxygen or very dilute with respect to cupric ion species. The autocatalytic dissolution is well represented by a half-order rate equation.
Copper and copper alloys suffers rapid attack by concentrated solution of ammonium hydroxide to form a soluble complex of copper-ammonium compound. In some cases, the corrosion of copper exposed to dilute solution of ammonium hydroxide is low. Copper specimen submerged at room temperature for one week in 0.01N ammonium hydroxide solution suffered a weight loss of 3.5mil/yr.
The rates of dissolution of polycrystalline metallic copper in aqueous ammonium hydroxide solutions have been determined under various experimental conditions. Over a considerable range of conditions the dissolution has been found to be autocatalytic. An empirical equation is presented which represents the autocatalytic rate data with an average deviation of $\ce{\pm4\%}$. The rate equation is discussed in terms of a mechanism which assumes that the rate controlling process is the removal of cuprous ion species from the copper solution interface by diffusion. Data are also given for an essentially zero-order rate of dissolution observed when the dissolving medium was concentrated with respect to oxygen or very dilute with respect to cupric ion species. The autocatalytic dissolution is well represented by a half-order rate equation.
No, I believe that copper(II) hydroxide will not form rather a soluble copper-ammonium complex will be formed.
This handbook discuss the corrosion of copper in ammonium hydroxide solution:
Also, this paper discuss the rates of Copper Dissolution in Aqueous Ammonium Hydroxide Solutions:
No, I believe that copper(II) hydroxide will not form rather a soluble copper-ammonium complex will be formed.
This handbook discuss the corrosion of copper in ammonium hydroxide solution:
Also, this paper discuss the rates of Copper Dissolution in Aqueous Ammonium Hydroxide Solutions:
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