Dissolved state of chromium in seawater

Nakayama, Eiichiro; Tokoro, Hiroyuki; Kuwamoto, Tooru; Fujinaga, Taitiro

doi:10.1038/290768a0

Cited by 90 publications

(32 citation statements)

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“…Following reduction of Cr(VI), Cr(III) may be immobilised in sparingly soluble hydroxide precipitates and in solid solution with Cr(OH) 3 at circumneutral or higher pH (Zachara et al, 2004), or may remain mobile as dissolved Cr(III) species. Numerous investigators have provided evidence for the existence of Cr(III)-organic complexes under environmental conditions (Harris, 1977;Nakayama et al, 1981;Ahern et al, 1985;Davis et al, 1994;Kaczynskl et al, 1994;Fukushima et al, 1995;Zhitkovich et al, 1995Zhitkovich et al, , 1996Mattuck and Nikolaidis, 1996;Sule and Ingle, 1996;Walsh and O'Halloran, 1996;Quievryn et al, 2002;Howe and Loeppe, 2003;Puzon et al, 1997Puzon et al, , 2005Puzon et al, , 2008. Organo -Cr(III) species increase the mobilisation of chromium and play a relevant role either in phyto-remediation strategies by increasing Cr uptake by plants (Erenoglu et al, 2007) or in microbial bioremediation of Cr(VI) contaminated sites by increasing the risk of Cr(III) migration in groundwater (Puzon et al, 2005).…”

Section: Introductionmentioning

confidence: 99%

“…According to Puzon et al (2005), organic-Cr(III) complexes are converted to inorganic Cr(III) species such as Cr(OH) 3 or Cr 2 O 3 through ligand exchange reactions or via biologically mediated processes. Nakayama et al (1981) suggested that organic-Cr(III) complexes might be quite stable and resistant to oxidation. Tzou et al (2002) have recently investigated the influence of organic compounds on Cr(III) oxidation by Mnoxides and found that the ligands they studied reduced the oxidation rates.…”

Section: Introductionmentioning

confidence: 99%

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Kinetics of oxidation of Cr(III)-organic complexes by H₂O₂

Luo

Chatterjee

2010

Chemical Speciation & Bioavailability

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Section: Introductionmentioning

confidence: 99%

Section: Introductionmentioning

confidence: 99%

Kinetics of oxidation of Cr(III)-organic complexes by H₂O₂

Luo

Chatterjee

2010

Chemical Speciation & Bioavailability

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“…Chromium (Cr) exists in two most common stable oxidation states, Cr(III) and Cr(VI), in the natural water system [1,2]. Cr(VI) is more labile and 10-100 times more toxic than Cr(III), and carcinogenic even at low concentrations of 50 ppb [3,4].…”

Section: Introductionmentioning

confidence: 99%

The controlling effect of pH on oxidation of Cr(III) by manganese oxide minerals

Feng

Zhai

Tan

et al. 2006

Journal of Colloid and Interface Science

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Oxidation of Cr(III) by three types of manganese oxide minerals (birnessite I, birnessite II, and todorokite) and effects of pH were investigated by chemical analysis, equilibrium redox, X-ray diffraction (XRD), and transmission electron microscopy. The effects of pH in the reaction systems on the oxidation of Cr(III) were similar among the three manganese oxide minerals. As pH increased from pH 2.0, the amount of Cr(III) oxidized by the tested manganese oxide minerals first increased, and then peaked at pH 3.0-3.5. While pH continually increased from 3.0 to 3.5, the amount of Cr(III) oxidized by the manganese oxide minerals sharply decreased. Until pH was higher than 5.0-5.5, the Cr(III) oxidation amounts changed to a small extent or kept stable. pH influenced the oxidation of Cr(III) mainly by altering the redox potential in the system, i.e., the concentration of H + , the species of Cr(III), and their distributions in the system. However, the surface charge of the manganese oxide minerals, subjected to the pH in the system, was not found to greatly influence the extent of the oxidation. When pH was below 5.0, oxidation of Cr(III) by the manganese oxide minerals was (or tended to be) an equilibrium reaction and was controlled thermodynamically. When pH was above 5.0-5.5, Cr(OH) 3 precipitate was produced in the system and pH had little effect on the oxidation content of Cr(III).

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“…Although the metastable nitrate--nitrite redox couple comes much closer in this respect, this does not imply that the Cr(VI)/ Cr(III) ratio is controlled by the complicated microbiologically induced nitrogen cycle in seawater. Recently Nakayama et al (1981a) reported the presence of dissolved organic Cr(III)-species in the Pacific Ocean and in the Japan Sea. These species constituted about half of the dissolved chromium in their samples.…”

Section: Stability Of Cr (Iii)-and Cr (Vi)-species In Seawatermentioning

confidence: 99%

Chromium(III) — chromium(VI) interconversions in seawater

Weijden

Reith

1982

Marine Chemistry

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Van der Weijden, C.H. and Reith, M. 1982. Chromium(III)--chromium(VI) interconversions in seawater. Mar. Chem., 11: 565--572.The stable form of dissolved chromium in oxygenated seawater is Cr(VI). But Cr(III)-species are also present at an analytically significant level. It is shown that Cr(III) is oxidized only slowly by dissolved oxygen, and that manganese oxide is a strong catalyst for such oxidation. However, the low oceanic concentration of suspended MnO2 impedes the conclusion that the former process is quantitatively less important than the latter one. The distribution of dissolved chromium among Cr(VI)-and Cr(III)-species is probably kinetically controlled.

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Dissolved state of chromium in seawater

Cited by 90 publications

References 8 publications

Kinetics of oxidation of Cr(III)-organic complexes by H₂O₂

Kinetics of oxidation of Cr(III)-organic complexes by H₂O₂

The controlling effect of pH on oxidation of Cr(III) by manganese oxide minerals

Chromium(III) — chromium(VI) interconversions in seawater

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Dissolved state of chromium in seawater

Cited by 90 publications

References 8 publications

Kinetics of oxidation of Cr(III)-organic complexes by H2O2

Kinetics of oxidation of Cr(III)-organic complexes by H2O2

The controlling effect of pH on oxidation of Cr(III) by manganese oxide minerals

Chromium(III) — chromium(VI) interconversions in seawater

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Kinetics of oxidation of Cr(III)-organic complexes by H₂O₂

Kinetics of oxidation of Cr(III)-organic complexes by H₂O₂