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Properties of Goethite and Jarosite Precipitated from Acidic Groundwater, Dalarna, Sweden

Published online by Cambridge University Press:  28 February 2024

Roger B. Herbert Jr.*
Affiliation:
Institute of Earth Sciences, Uppsala University, Norbyvägen 18B, 75236 Uppsala, Sweden
*
Email address: Roger.Herbert@geo.uu.se

Abstract

This study characterizes various chemical and mineralogical properties of goethite and jarosite from a mine drainage environment using chemical extraction techniques, X-ray diffractometry (XRD), 57Fe Mössbauer spectroscopy and scanning electron microscopy (SEM). Goethite and jarosite precipitates were collected from leachate-contaminated soils and from groundwater samples that were stored for up to 3 y. The results indicate that the soil goethites have primarily microcrystalline morphologies with moderately large mean crystallite dimensions (MCD110 ∼ 40 nm), and are superparamagnetic at room temperature and magnetically ordered at 77 K. The substitution of Al for Fe in the goethites is less than 0.03 mol/mol, and there is consequently no measured contraction in the goethite unit cell volume. The jarosite unit cell dimensions, Mössbauer parameters and chemical compositions indicate that the precipitates are primarily well-crystallized K-Na-H3O solid solutions, although the presence of poorly crystalline H3O-rich jarosite is also identified in one sample.

Type
Research Article
Copyright
Copyright © 1997, The Clay Minerals Society

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References

Alpers, C.N., Nordstrom, D.K. and Ball, J.W.. 1989. Solubility of jarosite solid solutions precipitated from acid mine waters, Iron Mountain, California, USA. Sci Géol Bull 42: 281298.Google Scholar
Alpers, C.N., Rye, R.O., Nordstrom, D.K., White, L.D. and King, B.-S.. 1992. Chemical, crystallographic, and stable isotopic properties of alunite and jarosite from acid-hypersaline Australian lakes. Chem Geol 96: 203226.CrossRefGoogle Scholar
Bigham, J.M.. 1994. Mineralogy of ochre deposits formed by sulfide oxidation. In: Jambor, J., Blowes, D., editors. Handbook on environmental geochemistry of sulfide mine-wastes. Mineral Assoc Can 22: 103132.Google Scholar
Bigham, J.M., Carlson, L. and Murad, E.. 1994. Schwertmannite, a new iron oxyhydroxy-sulphate from Pyhäsalmi, Finland, and other localities. Mineral Mag 58: 641648.CrossRefGoogle Scholar
Bigham, J.M., Schwertmann, U., Carlson, L. and Murad, E.. 1990. A poorly crystalline oxyhydroxysulfate of iron formed by bacterial oxidation of Fe(II) in acid mine water. Geochim Cosmochim Acta 54: 27432758.CrossRefGoogle Scholar
Blowes, D.W. and Jambor, J.L.. 1990. The pore-water chemistry and the mineralogy of the vadose zone of sulfide tailings, Waite Amulet, Quebec, Canada. Appl Geochem 5: 327346.CrossRefGoogle Scholar
Brady, K.S., Bigham, J.M., Jaynes, W.F. and Logan, T.J.. 1986. Influence of sulfate on Fe-oxide formation: Comparisons with a stream receiving acid mine drainage. Clays Clay Miner 34: 266274.CrossRefGoogle Scholar
Brindley, G.W.. 1980. Order-disorder in clay mineral structures. In: Brindley, G.W., Brown, G., editors. Crystal structures of clay minerals and their X-ray identification. London: Mineral Soc. p 125195.CrossRefGoogle Scholar
Brophy, G.P., Scott, E.S. and Snellgrove, R.A.. 1962. Sulphate studies II. Solid solution between jarosite and alunite. Am Mineral 47: 112126.Google Scholar
Brophy, G.P. and Sheridan, F.S.. 1965. Sulphate studies IV: The jarosite-narojarosite-hydronium jarosite solid solution series. Am Mineral 50: 15951607.Google Scholar
Campbell, A.S. and Schwertmann, U.. 1984. Iron oxide mineralogy of placic horizons. J Soil Sci 35: 569582.CrossRefGoogle Scholar
Carlson, L. and Schwertmann, U.. 1990. The effect of CO2 and oxidation rate on the formation of goethite versus lepidocrocite from an Fe(II) system at pH 6 and 7. Clay Miner 25: 6571.CrossRefGoogle Scholar
Chapman, B.M., Jones, D.R. and Jung, R.F.. 1983. Processes controlling metal ion attenuation in acid mine drainage streams. Geochim Cosmochim Acta 47: 19571973.CrossRefGoogle Scholar
Dutrizac, J.E. and Kaiman, S.. 1976. Synthesis and properties of jarosite-type compounds. Can Mineral 14: 151158.Google Scholar
Ficklin, W.H., Love, A.H. and Papp, C.S.E.. 1991. Solid-phase variations in an aquifer as the aqueous solution changes, Globe, Arizona. In: Mallard, G.E., Aronson, D.A., editors. USGS toxic substances hydrology program, Proc Tech Meet. Water-resources investigations report 91-4034. p 475480.Google Scholar
Filipek, L.H., Nordstrom, D.K. and Ficklin, W.H.. 1987. Interaction of acid mine drainage with waters and sediments of West Squaw Creek in the West Shasta Mining district, California. Environ Sci Technol 21: 388396.CrossRefGoogle ScholarPubMed
Goldman, D.S.. 1979. A reevaluation of the Mössbauer spectroscopy of calcic amphiboles. Am Mineral 64: 109118.Google Scholar
Herbert, R.B.. 1994. Metal transport in groundwater contaminated by acid mine drainage. Nordic Hydrol 25: 193212.CrossRefGoogle Scholar
Herbert, R.B.. 1995a. Precipitation of Fe oxydroxides and jarosite from acidic groundwater. GFF 117: 8185.CrossRefGoogle Scholar
Herbert, R.B.. 1995b. The geochemistry of groundwater and soils contaminated by acid mine leachate: A field study from Rudolfsgruvan, Dalarna, Sweden [Ph.D. thesis]. Uppsala, Sweden: Institution of Earth Sciences, Uppsala Univ. 133 p.Google Scholar
Herbert, R.B.. 1996. Metal retention by iron oxide precipitation from acid ground water in Dalarna, Sweden. Applied Geochem 11: 229236.CrossRefGoogle Scholar
Jambor, J.L.. 1994. Mineralogy of sulfide-rich tailings and their oxidation products. In: Jambor, J., Blowes, D., editors. Handbook on environmental geochemistry of sulfide mine-wastes. Mineral Assoc Can 22: 59102.Google Scholar
JCPDS, Joint Committee on Powder Diffraction Standards. 1972. Selected powder diffraction data for minerals. Publication DBM-1-23. Swarthmore, PA: JCPDS.Google Scholar
Johnson, C.A.. 1986. The regulation of trace element concentrations in river and estuarine waters contaminated with acid mine drainage: The adsorption of Cu and Zn on amorphous Fe oxyhydroxides. Geochim Cosmochim Acta 50: 24332438.CrossRefGoogle Scholar
Karlsson, S., Allard, B. and Håkansson, K.. 1988. Chemical characterization of stream-bed sediments receiving high loadings of acid mine effluents. Chem Geol 67: 115.CrossRefGoogle Scholar
Klug, H.P. and Alexander, L.E.. 1974. X-ray diffraction procedures for polycrystalline and amorphous materials. New York: J Wiley. 966 p.Google Scholar
Langmuir, D. and Whittemore, D.O.. 1971. Variations in the stability of precipitated ferric oxyhydroxides. In: Gould, R.F., editor. Nonequilibrium systems in natural water chemistry. Adv Chem Ser 106: 209234.CrossRefGoogle Scholar
Leclerc, A.. 1980. Room temperature Mössbauer analysis of jarosite-type compounds. Phys Chem Miner 6: 327334.CrossRefGoogle Scholar
Murad, E.. 1982. The characterization of goethite by Mössbauer spectroscopy. Am Mineral 67: 10071011.Google Scholar
Murad, E.. 1988. Properties and behavior of iron oxides as determined by Mössbauer spectroscopy. In: Stucki, J.W., Goodman, B.A., Schwertmann, U., editors. Iron in soils and clay minerals. Dordrecht: D. Reidel. p 309350.CrossRefGoogle Scholar
Murad, E., Bigham, J.M., Bowen, L.H. and Schwertmann, U.. 1990. Magnetic properties of iron oxides produced by bacterial oxidation of Fe2+ under acid conditions. Hyperfine Interact 58: 23732376.CrossRefGoogle Scholar
Murad, E. and Schwertmann, U.. 1980. The Mössbauer spectrum of ferrihydrite and its relations to those of other iron oxides. Am Mineral 65: 10441049.Google Scholar
Nordstrom, D.K.. 1982. Aqueous pyrite oxidation and the consequent formation of secondary iron minerals. In: Hossner, L.R., editor. Acid sulfate weathering. SSSA publication 10. Madison: Soil Sci Soc Am. p 95108.Google Scholar
Postma, D.. 1993. The reactivity of iron oxides in sediments: A kinetic approach. Geochim Cosmochim Acta 57: 50275034.CrossRefGoogle Scholar
Ripmeester, J.A., Ratcliffe, C.I., Dutrizac, J.E. and Jambor, J.L.. 1986. Hydronium ion in the alunite-jarosite group. Can Mineral 24: 435447.Google Scholar
Schulze, D.G.. 1981. Identification of soil iron oxide minerals by differential X-ray diffraction. Soil Sci Soc Am J 45: 437440.CrossRefGoogle Scholar
Schulze, D.G.. 1984. The influence of aluminum on iron oxides. VIII. Unit-cell dimensions of Al-substituted goethites and estimation of Al from them. Clays Clay Miner 32: 3644.CrossRefGoogle Scholar
Schulze, D.G. and Schwertmann, U.. 1984. The influence of aluminum on iron oxides. X. Properties of Al-substituted goethites. Clay Miner 19: 521539.CrossRefGoogle Scholar
Schwertmann, U.. 1964. Differenzierung der Eisenoxides des Bodens durch photochemische Extraktion mit saurer Ammoniumoxalat-Lösung. Z Pflanzenernähr Bodenkd 105: 194202.CrossRefGoogle Scholar
Schwertmann, U.. 1973. Use of oxalate for Fe extraction from soils. Can J Soil Sci 53: 244246.CrossRefGoogle Scholar
Schwertmann, U.. 1985. The effect of pedogenic environments on iron oxide minerals. Adv Soil Sci 1: 172200.Google Scholar
Schwertmann, U., Cambier, P. and Murad, E.. 1985. Properties of goethites of varying crystallinity. Clays Clay Miner 33: 369378.CrossRefGoogle Scholar
Schwertmann, U. and Carlson, L.. 1994. Aluminum influence on iron oxides: XVII. Unit-cell parameters and aluminum substitution on natural goethites. Soil Sci Soc Am J 58: 256261.CrossRefGoogle Scholar
Schwertmann, U., Carlson, L. and Murad, E.. 1987. Properties of iron oxides in two Finnish lakes in relation to the environment of their formation. Clays Clay Miner 35: 297304.CrossRefGoogle Scholar
Schwertmann, U. and Cornell, R.M.. 1991. Iron oxides in the laboratory: Preparation and characterization. Weinheim: VCH Verlagsgesellschaft mbH. 137 p.Google Scholar
Schwertmann, U. and Taylor, R.M.. 1989. Iron oxides. In: Dixon, J.B., Weed, S.B., editors. Minerals in soil environments, 2nd ed. Madison, WI: Soil Sci Soc Am. p 379438.Google Scholar
Stollenwerk, K.. 1994. Geochemical interactions between constituents in acidic groundwater and alluvium in an aquifer near Globe, Arizona. Applied Geochem 9: 353369.CrossRefGoogle Scholar
Ribet, I., Ptacek, C.J., Blowes, D.W. and Jambor, J.L.. 1995. The potential for metal release by reductive dissolution of weathered mine tailings. J Contam Hydrol 17: 239273.CrossRefGoogle Scholar
WaveMetrics. 1994. Igor Pro user's manual 2.00. Lake Oswego, OR: WaveMetrics Inc. 1080 p.Google Scholar