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Reduction of Copper(II) by Iron(II)

Department of Agronomy, University of Kentucky, N-122 Agricultural Science Center-North, Lexington, KY 40546-0091

View larger version (30K): [in a new window]   Fig. 1. Dissolved Cu and Fe concentrations over time under anoxic conditions with initial metal concentrations of 1.0 mM and (a) 2 mM [Cl–], (b) 4 mM [Cl–], and (c) 0.1 M [Cl–]. Reactions contained 0.1 M pH 5.5 MES buffer.

View larger version (24K): [in a new window]   Fig. 2. Dissolved Cu and Fe concentrations over time under anoxic conditions with initial metal concentrations of 9.1 mM and (a) 0.04 M [Cl–] and (b) 0.1 M [Cl–]. Experiments were performed in water and an automatic titrator was used to maintain a pH of 5.2 ± 0.2.

View larger version (29K): [in a new window]   Fig. 3. (a) X-ray diffraction patterns of the solid-phase precipitates collected after 60 min of reaction time for 0.04 M and 0.10 M [Cl–] treatments, and (b) corresponding plots of base added during the precipitation reactions. Reactions contained 9.1 mM Cu(II) and Fe(II) and were performed at pH 5.2 ± 0.2 in water.

View larger version (26K): [in a new window]   Fig. 4. Fourier transform infrared (FTIR) spectra of the solid-phase precipitates collected after 60 min of reaction time for 0.04 M and 0.10 M [Cl–] treatments. Reactions contained 9.1 mM Cu(II) and Fe(II) and were performed at pH 5.2 ± 0.2 in water.

View larger version (48K): [in a new window]   Fig. 5. Representative scanning electron microscope image of precipitates after 60 min of reaction time for the 0.1 M [Cl–] treatment and corresponding energy dispersive X-ray spectra shown below. Reactions contained 9.1 mM Cu(II) and Fe(II) and were performed at pH 5.2 ± 0.2 in water. Scale bar equals 2 µm.