Abstract
A copper(II) ion-selective-electrode potentiometric method was used to determine the first and second hydrolysis constants of Cu2+. Special techniques prevented copper(II) hydroxide precipitation, and copper(II) carbonate and cipper(II) organic complexation during the titration of the experimental solution over the pH range 6.8–8.4. The large change in the total copper concentration during the titration due to adsorption of copper onto the vessel walls was accounted for by measuring the total copper concentration at each pH by atomic absorption spectrophotometry. The two hydrolysis constants were determined at 25°C in 0.7 and 0.05m NaClO4 media. The measured stability constants are independent of the copper concentration and yield similar zero ionic strength values. Also, the stepwise equilibrium constants decrease as the ligand number increases.
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Paulson, A.J., Kester, D.R. Copper(II) ion hydrolysis in aqueous solution. J Solution Chem 9, 269–277 (1980). https://doi.org/10.1007/BF00644552
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DOI: https://doi.org/10.1007/BF00644552