TY - JOUR
T1 - Oxidative dissolution of UO2 in a simulated groundwater containing synthetic nanocrystalline mackinawite
AU - Bi, Yuqiang
AU - Hyun, Sung Pil
AU - Kukkadapu, Ravi
AU - Hayes, Kim F.
N1 - Funding Information:
We thank Tom Yavaraski for his technical assistance in the laboratory. We are also grateful to Dr. Edward Burton for helpful discussion in our analysis. We thank Drs. Juan S. Lezama Pacheco and John Bargar for assistance with XAS collection at Stanford Synchrotron Radiation Lightsource (SSRL).Y.B. thanks Julian Carpenter and Tara Clancy for their help in XAS data collection and numerous discussions throughout the study. This research was supported by the U.S. Department of Energy, Office of Science, Office of Biological and Environmental Research (BER), Subsurface Biogeochemical Research (SBR) program (DE-FG02-09ER64803). Part of this research was carried out at SSRL, a Directorate of SLAC National Accelerator Laboratory and an Office of Science User Facility operated for the U.S. DOE by Stanford University. A portion of the research was performed using Environmental and Molecular Sciences Laboratory (EMSL), a national scientific user facility sponsored by the Department of Energy’s Office of Biological and Environmental Research and located at Pacific Northwest National Laboratory, Richland, WA.
PY - 2013/2/1
Y1 - 2013/2/1
N2 - The long-term success of in situ reductive immobilization of uranium (U) depends on the stability of U(IV) precipitates (e.g., uraninite) in the presence of natural oxidants, such as oxygen, Fe(III) hydroxides, or nitrite. Field and laboratory studies have implicated iron sulfide minerals as redox buffers or oxidant scavengers that may slow oxidation of reduced U(VI) solid phases. Yet, the inhibition mechanism(s) and reaction rates of uraninite (UO2) oxidative dissolution by oxic species such as oxygen in FeS-bearing systems remain largely unresolved. To address this knowledge gap, abiotic batch experiments were conducted with synthetic UO2 in the presence and absence of synthetic mackinawite (FeS) under simulated groundwater conditions of pH=7, PO2=0.02atm, and PCO2=0.05atm. The kinetic profiles of dissolved uranium indicate that FeS inhibited UO2 dissolution for about 51h by effectively scavenging oxygen and keeping dissolved oxygen (DO) low. During this time period, oxidation of structural Fe(II) and S(-II) of FeS were found to control the DO levels, leading to the formation of iron oxyhydroxides and elemental sulfur, respectively, as verified by X-ray diffraction (XRD), Mössbauer and X-ray absorption spectroscopy (XAS). After FeS was depleted due to oxidation, DO levels increased and UO2 oxidative dissolution occurred at an initial rate of rm=1.2±0.4×10-8molg-1s-1, higher than rm=5.4±0.3×10-9molg-1s-1 in the control experiment where FeS was absent. XAS analysis confirmed that soluble U(VI)-carbonato complexes were adsorbed by iron oxyhydroxides (i.e., nanogoethite and lepidocrocite) formed from FeS oxidation, which provided a sink for U(VI) retention. This work reveals that both the oxygen scavenging by FeS and the adsorption of U(VI) to FeS oxidation products may be important in U reductive immobilization systems subject to redox cycling events.
AB - The long-term success of in situ reductive immobilization of uranium (U) depends on the stability of U(IV) precipitates (e.g., uraninite) in the presence of natural oxidants, such as oxygen, Fe(III) hydroxides, or nitrite. Field and laboratory studies have implicated iron sulfide minerals as redox buffers or oxidant scavengers that may slow oxidation of reduced U(VI) solid phases. Yet, the inhibition mechanism(s) and reaction rates of uraninite (UO2) oxidative dissolution by oxic species such as oxygen in FeS-bearing systems remain largely unresolved. To address this knowledge gap, abiotic batch experiments were conducted with synthetic UO2 in the presence and absence of synthetic mackinawite (FeS) under simulated groundwater conditions of pH=7, PO2=0.02atm, and PCO2=0.05atm. The kinetic profiles of dissolved uranium indicate that FeS inhibited UO2 dissolution for about 51h by effectively scavenging oxygen and keeping dissolved oxygen (DO) low. During this time period, oxidation of structural Fe(II) and S(-II) of FeS were found to control the DO levels, leading to the formation of iron oxyhydroxides and elemental sulfur, respectively, as verified by X-ray diffraction (XRD), Mössbauer and X-ray absorption spectroscopy (XAS). After FeS was depleted due to oxidation, DO levels increased and UO2 oxidative dissolution occurred at an initial rate of rm=1.2±0.4×10-8molg-1s-1, higher than rm=5.4±0.3×10-9molg-1s-1 in the control experiment where FeS was absent. XAS analysis confirmed that soluble U(VI)-carbonato complexes were adsorbed by iron oxyhydroxides (i.e., nanogoethite and lepidocrocite) formed from FeS oxidation, which provided a sink for U(VI) retention. This work reveals that both the oxygen scavenging by FeS and the adsorption of U(VI) to FeS oxidation products may be important in U reductive immobilization systems subject to redox cycling events.
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U2 - 10.1016/j.gca.2012.10.032
DO - 10.1016/j.gca.2012.10.032
M3 - Article
AN - SCOPUS:84870534486
SN - 0016-7037
VL - 102
SP - 175
EP - 190
JO - Geochimica et Cosmochimica Acta
JF - Geochimica et Cosmochimica Acta
ER -