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Cited by 131Arsenic contamination and mitigationIron oxide chemistry and applicationsAdsorption and biosorption for pollutant removal

The DOI matches its Crossref record; 50 of the 50 references it cites were found in a registry or an index.

Coprecipitation of Arsenate with Metal Oxides. 2. Nature, Mineralogy, and Reactivity of Iron(III) Precipitates

Violante, Antonio, Gaudio, Stefania Del, Pigna, Massimo, Ricciardella, Mariarosaria, Banerjee, Dipanjan·2007·Environmental Science & Technology
DOI 10.1021/es070382+
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Abstract

Coprecipitation involving arsenic with aluminum or iron has been studied because this technique is considered particularly efficient for removal of this toxic element from polluted waters. Coprecipitation of arsenic with mixed iron-aluminum solutions has received scant attention. In this work we studied (i)the mineralogy, surface properties, and chemical composition of mixed iron-aluminum oxides formed at initial Fe/Al molar ratio of 1.0 in the absence or presence of arsenate [As/ Fe+Al molar ratio (R) of 0, 0.01, or 0.1] and at pH 4.0, 7.0, and 10.0 and aged for 30 and 210 days at 50 degrees C and (ii) the removal of arsenate from the coprecipitates after addition of phosphate. The amounts of short-range ordered precipitates (ferrihydrite, aluminous ferrihydrite and/or poorly crystalline boehmite) were greater than those found in iron and aluminum systems (studied in previous works), due to the capacity of both aluminum and arsenate to retard or inhibitthe transformation of the initially formed precipitates into well-crystallized oxides (gibbsite, bayerite, and hematite). As a consequence, the surface areas of the iron-aluminum oxides formed in the absence or presence of arsenate were usually much larger than those of aluminum or iron oxides formed under the same conditions. Arsenate was found to be associated mainly into short-range ordered materials. Chemical composition of all samples was affected by pH, initial R, and aging. Phosphate sorption was facilitated by the presence of short-range ordered materials, mainly those richer in aluminum, but was inhibited by arsenate present in the samples. The quantities of arsenate replaced by phosphate, expressed as percentages of its total amount present in the samples, were particularly low, ranging from 10% to 26%. A comparison of the desorption of arsenate by phosphate from aluminum-arsenate and iron-arsenate (studied in previous works) and iron-aluminum-arsenate coprecipitates evidenced that phosphate has a greater capacity to desorb arsenate from aluminum than iron sites.

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  • Phosphate desorbed more arsenate from aluminum-arsenate and iron-aluminum-arsenate coprecipitates than from iron-arsenate coprecipitates, because arsenate forms stronger complexes with Fe than with Al.

    “A comparison of the desorption of arsenate by phosphate from aluminum -arsenate, iron -arsenate, and iron -aluminum -arsenate coprecipitates evidenced that phosphate desorbed more arsenate from aluminum -arsenate, iron -aluminum -arsenate than iron -arsenate coprecipitates (in the order listed), because arsenate forms stronger complexes with Fe than with Al.”

    From Chemical Processes Affecting the Mobility of Heavy Metals and Metalloids in Soil Environments (2016) · cites this paper as [55]

  • Low amounts of arsenate coprecipitated with aluminum and/or iron oxides at pH 7.0 were removed by phosphate (5-25%), attributed to the formation of strong inner-sphere complexes, metal-arsenate precipitates, and partial occlusion of arsenate into the coprecipitates.

    “Low amounts of arsenate coprecipitated with aluminum and/or iron oxides at pH 7.0 were removed by phosphate (5 -25 %), attributed to the formation of strong inner-sphere complexes, metal -arsenate precipitates, and partial occlusion of arsenate into the coprecipitates.”

    From Chemical Processes Affecting the Mobility of Heavy Metals and Metalloids in Soil Environments (2016) · cites this paper as [55]

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Research works printed but not linked: 2

  1. Viraraghavan T., 1999, Water Sci. Technol., 40, 69, 10.2166/wst.1999.0088 · DOI
  2. Cornell R. M., 1996, The iron oxides. Structure, properties, reactions and uses

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Metadata

Authors
Violante, A., Gaudio, S. D., Pigna, M., Ricciardella, M., & Banerjee, D.
Affiliations
University of Naples Federico II (IT)
Corresponding author
Violante, Antonio
Venue
Environmental Science & Technology
Publisher
American Chemical Society (ACS)
Published
2007-11-13
Volume
41
Issue
24
Pages
8275-8280
ISSN
  • 0013-936X (ISSN-L)
  • 1520-5851
DOI
10.1021/es070382+
OpenAlex
W2138316873
Cited by
131
References
50
Citations by year
2026: 2 · 2025: 2 · 2024: 2 · 2023: 2 · 2022: 5 · 2021: 4 · 2020: 2 · 2019: 3 · 2018: 14 · 2017: 4 · 2016: 10 · 2015: 9 · 2014: 11 · 2013: 12 · 2012: 10
FWCI
7.40
Type
journal article
Language
en
Open access
closed
Locations
  • Environmental Science & Technology (publishedVersion)
  • PubMed (publishedVersion)
Topics
  • Physical Sciences › Environmental Science › Environmental Chemistry › Arsenic contamination and mitigation
  • Physical Sciences › Materials Science › Materials Chemistry › Iron oxide chemistry and applications
  • Physical Sciences › Environmental Science › Water Science and Technology › Adsorption and biosorption for pollutant removal
Keywords
iron(III) oxide, ferrihydrite, boehmite, phosphate adsorption, arsenic removal from water, pH effect, surface area
MeSH terms
Arsenates, Ferric Compounds, Kinetics, Oxides, Chemical Precipitation, X-Ray Diffraction

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