ATR–FTIR Spectroscopic Investigation on Phosphate Adsorption Mechanisms at the Ferrihydrite–Water Interface

Arai, Yuji; Sparks, Donald L.

doi:10.1006/jcis.2001.7773

Cited by 649 publications

(534 citation statements)

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“…Arai and Sparks investigated phosphate adsorption mechanisms at the ferrihydrite-water interface and found that the spectra under different adsorption conditions were an assemblage of well-resolved triplet splitting of the υ3 (P-O) vibration via Gaussian profile fitting analysis. They speculated from this result that bidentate binuclear (C2υ) and monodentate mononuclear phosphate complexes (C1) predominantly form at the ferrihydrite-H2O interface at pH g 7.5 and pH < 7.5, respectively (17). In this study, the triplet splitting of the υ3 vibration via Gaussian profile fitting analysis suggests the existence of C2ν or lower symmetry C1 point groups.…”

Section: Resultsmentioning

confidence: 57%

Arsenate Adsorption on an Fe−Ce Bimetal Oxide Adsorbent: Role of Surface Properties

Zhang

Yang

Dou

et al. 2005

Environ. Sci. Technol.

511

247

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An Fe-Ce bimetal adsorbent was investigated with X-ray powder diffraction (XRD), transmission electron micrograph (TEM), Fourier transform infrared spectra (FTIR), and X-ray photoelectron spectroscopy (XPS) methods for a better understanding of the effect of surface properties on arsenate (As(V)) adsorption. In the adsorption test, the bimetal oxide adsorbent showed a significantly higher As-(V) adsorption capacity than the referenced Ce and Fe oxides (CeO 2 and Fe 3 O 4 ) prepared by the same procedure and some other arsenate adsorbents reported recently. XRD measurement of the adsorbent demonstrated that the phase of magnetite (Fe 3 O 4 ) disappears gradually with the increasing dosage of Ce 4+ ions until reaching a molar ratio of Ce 4+ to Fe 3+ and Fe 2+ of 0.08:0.2:0.1 (Fe-Ce08 refers to the adsorbent prepared at this ratio), and the phase of CeO 2 begins to appear following a further increase of the Ce dose. Combined with the results of TEM observation, it was assumed that a solid solution of Fe-Ce is formed following the disappearance of the magnetite phase. Occurrence of a characteristic surface hydroxyl group (M-OH, metal surface hydroxyl, 1126 cm -1 ), which showed the highest band intensity in the solid solution state, was confirmed on the bimetal oxide adsorbent by FTIR. Quantificational calculation from the XPS narrow scan results of O(1s) spectra also indicated that the formation of the bimetal Fe-Ce08 was composed of more hydroxyl (30.8%) than was the formation of CeO 2 and Fe 3 O 4 (12.6% and 19.6%). The results of adsorption tests on Fe-Ce08 at different As(V) concentrations indicated that both the integral area of the As-O band at 836 cm -1 and the As(V) adsorption capacity increased almost linearly with the decrease of the integral area of M-OH bands at 1126 cm -1 , proving that the adsorption of As(V) by Fe-Ce08 is mainly realized through the mechanism of quantitative ligand exchange. The atomic ratio of Fe on Fe-Ce08 decreased from 20.1% to 7.7% with the increase of the As atom ratio from 0 to 16% after As(V) adsorption, suggesting that As(V) adsorption might be realized through the replacement of the M-OH group of Fe (Fe-OH) with arsenate. The well splitting of three υ 3 bands at As-O band (836 cm -1 ) of FTIR and the hydroxyl ratio (1.7) of Fe-Ce08 calculated from the XPS results suggested that the diprotonated monodentate complex (SOAsO(OH) 2 ) is possibly dominant on the surface of Fe-Ce08.

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Section: Resultsmentioning

confidence: 57%

Arsenate Adsorption on an Fe−Ce Bimetal Oxide Adsorbent: Role of Surface Properties

Zhang

Yang

Dou

et al. 2005

Environ. Sci. Technol.

511

247

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“…Similar conclusions were drawn by Antelo et al (2010), whereas Luengo et al (2006) proposed protonated bidentate phosphate surface complexes at lower pH condition using attenuated total reflection-infrared (ATR-IR) spectroscopic measurements. On the other hand the presence of non-protonted bidentate complexes at pH 7.5 was confirmed by Arai and Sparks (2002). Nevertheless, the majority of previous studies did not rule out the presence of unidentified surface species at various pHs.…”

mentioning

confidence: 85%

“…Nevertheless, the majority of previous studies did not rule out the presence of unidentified surface species at various pHs. It was also suggested that conclusions drawn regarding surface complexes of HFO are generally taken based on goethite as a proxy mineral and therefore HFO surface characterisation still lacks accuracy (Antelo et al, 2010;Kare et al, 2011;Arai and Sparks, 2002).…”

mentioning

confidence: 99%

Surface-complexation modelling for describing adsorption of phosphate on hydrous ferric oxide surface

Mengistu

Tessema

Demlie

et al. 2015

WSA

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Adsorption of dissolved phosphate onto synthetic hydrous ferric oxide (HFO) was measured in the laboratory as a function of pH, ionic strength, and phosphate relative concentration. Experimental data were used to constrain optimal values of surface complexation reactions using a geochemical modeling code JCHESS according to the diffuse layer model. The results provide a consistent set of model equilibrium constant (log K) values at 25° C and 100 KPa for the following reactions: These results differ significantly from previously-published estimates of log K 2 int and log K 3 int [1][2][3], and provide a more accurate fit to experimental measurements over a broad range of pH (3-12), ionic strength (0.001-0.1 mol/ℓ) and total relative phosphate concentration (12-500 µmol phosphate/g HFO). The results provide a close fit to the experimental data within a wide range of conditions, and should be adopted in modelling the chemical speciation of phosphate in natural systems containing HFO as a predominant adsorbing material.

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“…Bidentate complexes require more activation energy to break the bond than do monodentate complexes, so it can be more difficult for P desorption to take place in environments where the bidentate complexes predominate between phosphate and the soil surface. In spite of precise investigations using infrared spectroscopy (Parfitt & Atkinson, 1976) and X-ray photoelectron spectroscopy (Martin & Smart, 1987), assigning peaks among possible complexation types remains controversial (Arai & Sparks, 2001;Kreller et al, 2002). Clarification of the effects of pH and P surface coverage on the formation of different surface-complex types may help to resolve these issues.…”

Section: Soil Ph Effect On P Desorptionmentioning

confidence: 99%

Influence of soil pH on inorganic phosphorus sorption and desorption in a humid brazilian Ultisol

Sato

Comerford²

2005

Rev. Bras. Ciênc. Solo

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SUMMARYLiming is a common practice to raise soil pH and increase phosphorus (P) bioavailability in tropical regions. However, reports on the effect of liming on P sorption and bioavailability are controversial. The process of phosphorus desorption is more important than P sorption for defining P bioavailability. However few studies on the relationship between soil pH and P desorption are available, and even fewer in the tropical soils. The effects of soil pH on P sorption and desorption in an Ultisol from Bahia, Brazil, were investigated in this study. Phosphorus sorption decreased by up to 21 and 34 % with pH increases from 4.7 to 5.9 and 7.0, respectively. Decreasing Langmuir K parameter and decreasing partition coefficients (K d ) with increasing pH supported this trend. Phosphorus desorption was positively affected by increased soil pH by both the total amount of P desorbed and the ratio of desorbed P to initially sorbed P. A decreased K parameter and increased K d value, particularly at the highest pH value and highest P-addition level, endorsed this phenomenon. Liming the soil had the double effect of reducing P sorption (up to 4.5 kg ha -1 of remaining P in solution) and enhancing P desorption (up to 2.7 kg ha -1 of additionally released P into solution).Index terms: liming, phosphorus bioavailability, Langmuir, partition coefficients, and Atlantic Forest.(

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ATR–FTIR Spectroscopic Investigation on Phosphate Adsorption Mechanisms at the Ferrihydrite–Water Interface

Cited by 649 publications

References 46 publications

Arsenate Adsorption on an Fe−Ce Bimetal Oxide Adsorbent: Role of Surface Properties

Arsenate Adsorption on an Fe−Ce Bimetal Oxide Adsorbent: Role of Surface Properties

Surface-complexation modelling for describing adsorption of phosphate on hydrous ferric oxide surface

Influence of soil pH on inorganic phosphorus sorption and desorption in a humid brazilian Ultisol

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