Please use this identifier to cite or link to this item: http://hdl.handle.net/10553/49823
Title: Oxidation of nanomolar levels of Fe(II) with oxygen in natural waters
Authors: Santana-Casiano, J. Magdalena 
González-Dávila, Melchor 
Millero, Frank J.
UNESCO Clasification: 251002 Oceanografía química
230331 Química del agua
Keywords: Seawater
Oxidation
Kinetic modeling
Issue Date: 2005
Project: Efecto de Los Compuestos Catecolatos, Hidroxamatos y Porfirinas en El Comportamiento Qwuimico de Fe(Ii) en El Medio Marino. 
Journal: Environmental science & technology 
Abstract: The oxidation of Fe(II) by molecular oxygen at nanomolar levels has been studied using a UV−Vis spectrophotometric system equipped with a long liquid waveguide capillary flow cell. The effect of pH (6.5−8.2), NaHCO3 (0.1−9 mM), temperature (3−35 °C), and salinity (0−36) on the oxidation of Fe(II) are presented. The first-order oxidation rates at nanomolar Fe(II) are higher than the values at micromolar levels at a pH below 7.5 and lower than the values at a higher pH. A kinetic model has been developed to consider the mechanism of the Fe(II) oxidation and the speciation of Fe(II) in seawater, the interactions between the major ions, and the oxidation rates of the different Fe(II) species. The concentration of Fe(II) is largely controlled by oxidation with O2 and O2•- but is also affected by hydrogen peroxide that may be both initially present and formed from the oxidation of Fe(II) by superoxide. The model has been applied to describe the effect of pH, concentration of NaHCO3, temperature, and salinity on the kinetics of Fe(II) oxidation. At a pH over 7.2, Fe(OH)2 is the most important contributing species to the apparent oxidation rate. At high levels of CO32- and pH, the Fe(CO3)22- species become important. At pH values below 7, the oxidation rate is controlled by Fe2+. Using the model, log ki values for the most kinetically active species (Fe2+, Fe(OH)+, Fe(OH)2, Fe(CO3), and Fe(CO3)22-) are given that are valid over a wide range of temperature, salinity, and pH in natural waters. Model results show that when H2O2 concentrations approach the Fe(II) concentrations used in this study, the oxidation of Fe(II) with H2O2 also needs to be considered.
URI: http://hdl.handle.net/10553/49823
ISSN: 0013-936X
DOI: 10.1021/es049748y
Source: Environmental Science and Technology [ISSN 0013-936X], v. 39 (7), p. 2073-2079
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