Kinetic study of copper complexation in hydrogenocarbonate solutions by electrochemical approaches
The determination of the complexing capacity of natural waters by amperometric copper (II) titrations must be made in pH-buffered solutions. Most if not all of classical buffers influence copper speciation through the formation of weak complexes. This paper deals with an attempt to use the naturally occurring hydrogenocarbonate buffet. A detailed study of copper (II) chemistry in synthetic solutions at controlled ionic strength and pH (0.02 mol.l-1 KNO3, 2.38 mol.l-1 NaHCO3, controlled Pco2) was carried out. In these solutions copper (Il) chemistry may involve precipitation of copper hydroxide Cu(OH)2, copper hydroxycarbonate Cu2(OH)2 CO3 (malachite) and formation of the soluble complexes CuCO30 and CuOH+. At low enough values of pH CuOH+ formation may be neglected. The three other reactions are studied using copper ionometry with a specific electrode and equilibrium constants determined in the 5.5 to 8.0 pH range. As CuCO30 is a major species in these solutions its lability is of major concern for the validity of the amperometric determination of the complexing capacity by copper (II) titration and bas been studied by several electrochemical approaches. AC polarography indicated a rapid reduction of copper (II) on the mercury electrode. Two waves were obtained for the deposition of copper (Il) by voltamperometry with a rotated platinum disk electrode (RDE) presenting the characteristics of a kinetic control. However the values of the forward (kf) and backward (kb) reaction rate constants for CuCO30 formation or dissociation seem too high for a precise determination.