Adsorption and desorption characteristics of arsenic onto ceria nanoparticles
© Feng et al; licensee Springer. 2012
Received: 8 August 2011
Accepted: 23 January 2012
Published: 23 January 2012
The rapid increase in the use of engineered nanoparticles [ENPs] has resulted in an increasing concern over the potential impacts of ENPs on the environmental and human health. ENPs tend to adsorb a large variety of toxic chemicals when they are emitted into the environment, which may enhance the toxicity of ENPs and/or adsorbed chemicals. The study was aimed to investigate the adsorption and desorption behaviors of arsenic on ceria NPs in aqueous solution using batch technique. Results show that the adsorption behavior of arsenic on ceria NPs was strongly dependent on pH and independent of ionic strength, indicating that the electrostatic effect on the adsorption of these elements was relatively not important compared to surface chemical reactions. The adsorption isotherms fitted very well to both the Langmuir and Freundlich models. The thermodynamic parameters (ΔH 0 , ΔS 0 , and ΔG 0 ) for the adsorption of arsenic were determined at three different temperatures of 283, 303, and 323 K. The adsorption reaction was endothermic, and the process of adsorption was favored at high temperature. The desorption data showed that desorption hysteresis occurred at the initial concentration studied. High adsorption capacity of arsenic on ceria NPs suggests that the synergistic effects of ceria NPs and arsenic on the environmental systems may exist when they are released into the environment.
Keywordsceria nanoparticles arsenic adsorption desorption.
With the large-scale production and widespread application, the potential environmental risks of engineered nanoparticles [NPs] have consequently attracted much attention since NPs will be unavoidably released to the environment after their production, use, and disposal. To date, the potential environmental effects of NPs, in any quantity, are largely unknown [1–3]; therefore, an understanding of the transport, transfer, and fate of NPs in the environment is an important issue for evaluating their environmental and health impacts.
NPs usually exhibit remarkable physical properties, rapid chemical reactivity, and high sorption capacity for inorganic and organic compounds. Studies of the fate and transport of NPs are largely concerned with how their properties and behavior change over time, whether they will interact with toxic contaminants after being released into the environment or they will change the anticipated impact of NPs themselves and the toxic contaminants when they interact with one another. For example, recent studies showed that phenanthrene could be adsorbed by iron and copper NPs through hydrophobic effect and dipole interactions between NPs' charged surface and phenanthrene . Carbon nanotubes [CNTs] tend to adsorb toxic chemicals of atrazine, and CNTs with adsorbed atrazine exhibited the toxicities of both the toxic chemicals and CNTs themselves when interacting with living organisms . Therefore, the potential environmental risks of NPs are exerted not only from the NPs themselves, but also from the toxic contaminants adsorbed by them [4, 5]. Hence, knowledge of toxic compound adsorption onto NPs is critical and helpful for their risk assessment, and it is also useful for understanding the effect of nanomaterials on the fate of toxic compounds in the environment [4, 5]. Unfortunately, to the best of our knowledge, these studies are limited within zerovalent metal NPs, CNTs, and related materials [4, 5]; there are no studies that have examined the adsorption and desorption behaviors of toxic contaminants onto metal oxide NPs.
Ceria NPs are considered to be a representative member of an industrially important class of metal oxide NPs [6, 7]; they can be used as automotive catalytic converters , UV-blocking agents , and single, nanowire-based gas sensors . Indeed, ceria NPs are on the OECD list of priority nanomaterials for immediate testing. However, at present, little ecotoxicity data are available. Previous studies have demonstrated that ceria NPs have toxic effects on cells [11, 12], aquatic organisms [13, 14], and plants ; however, other reports show that ceria NPs are able to rescue HT22 cells from oxidative stress-induced cell death  and protect against the progression of cardiac dysfunction . These contradictory results suggest the complex behaviors of ceria NPs in the environment.
Arsenic is one of the most toxic elements and is found virtually in all environmental systems as a result of both geological processes and anthropogenic activities [18, 19]; the USEPA has set a maximum contaminant level for arsenic at 10 μg L-1 in drinking water . Adsorption with metal oxides has been widely used to remove these contaminants because of its effectiveness and simplicity for point-of-use applications. However, since the environmental release of ceria NPs from various applications, the NPs' solid surface interactions with organic contaminants, such as arsenic, have become increasingly important, and the subsequent behavior and effects of the released NPs must be considered an urgent need.
Information on the interaction of free and aggregated NPs with adsorbed chemicals is lacking from the literature, although studies suggest that the adsorption of phenanthrene on nanosized zerovalent iron and copper significantly decreases with the increase in pH, that naphthalene exerted significant competition adsorption with phenanthrene , and that Th(IV) adsorption onto oxidized MWCNTs is endothermic . The present work investigated the adsorption and desorption behaviors of arsenic onto ceria NPs. The objectives include (1) to quantify and predict the adsorption behavior of arsenic on ceria NPs under different pH and ionic strength, (2) to determine adsorption isotherms and analyze regressively experimental data with Langmuir and Freundlich models, (3) to study the adsorption of arsenic at different temperatures and measure the adsorption thermodynamic parameters (i.e., ΔH 0 , ΔS 0 , ΔG 0 ), and (4) to investigate the desorption behavior of arsenic at the ceria NPs' surface using batch adsorption experiments.
Materials and methods
All chemicals used were of analytical reagent grade. Milli-Q water (18.2 MΩ cm, Millipore, Beijing, China) was used for all solution preparation. Stock solutions of arsenic were purchased from the National Institute of Metrology (Beijing, China). These stock solutions were kept at 4°C in darkness. Working solutions of arsenic (0.4 to 40.0 μg L-1) were prepared daily by dilution of the stock solution with HCl. Working solutions of 20% (w/v) potassium tetrahydroborate were prepared daily by dilution of the KBH4 stock solution in 5% NaOH. Pre-reducing solutions containing 10% (w/v) thiourea (Beijing Chemical Works, Beijing, China) and 10% (w/v) ascorbic acid (Sigma, Sigma-Aldrich Corporation, St. Louis, MO, USA) were prepared fresh daily in water. Glassware used for the determination of arsenic was soaked in a 10% (v/v) nitric acid solution and rinsed with Milli-Q water.
Preparation and characterization of ceria NPs
Ceria NPs used in the experiments were synthesized using a precipitation method as described in our former reports [16, 22, 23].The resulting ceria NPs were characterized with a Tecnai G2 20 S-Twin transmission electron microscope (FEI Company, Tokyo, Japan) operated at 200 keV and with dynamic light scattering, using a Coulter Nicomp™ 380 ZLS Particle Size Analyzer (Santa Barbara, CA, USA). The surface area was characterized by nitrogen adsorption/desorption analysis of Brunauer-Emmett-Teller (Autosorb-1, Quantachrome Instruments, Boynton Beach, FL, USA).
The X-ray diffraction [XRD] patterns for ceria NPs were recorded on an X' Pert PRO (PANalytical B.V., Almelo, The Netherlands) with monochromatized Cu Kα radiation. The particle size of CeO2 was calculated from the Scherrer formula using the (220) diffraction peak of the respective cerium oxide .
Adsorption isotherms by batch studies were conducted in 7-mL capped centrifuge tubes. Each tube containing 5-mL varying concentrations of arsenic was mechanically shaken on a horizontal motion shaker for 24 h (preliminary experiments had shown that all solid-solution mixtures reached apparent equilibrium within 2 h) at room temperature (25°C). Thermodynamic parameters associated with the adsorption processes were carried out in temperatures of 283, 303, and 323 K. After centrifugation (10,000 rpm for 10 min), the supernatant was sampled and analyzed. The concentration of ceria NPs used for the adsorption experiments was 5 g L-1. Initial concentrations of arsenic were ranged from 0.4 to 40.0 μg L-1. All experiments were conducted in triplicate.
The solution pH plays a critical role in the adsorption of metalloid ions onto various adsorbents. To optimize the pH for maximum removal efficiency, a sorption experiment was conducted in the initial pH range from 1.0 to 13.0, adjusted using HCl or NaOH.
For ionic strength effect tests, the desired initial sodium nitrate was from 1 × 10-8 to 1.0 mol L-1, arsenic was added, and the batch equilibration was initiated immediately. The effect of H2SiO3 colloid and Fe(OH)3 colloid on As(III) and As(V) adsorptions was examined with the concentration from 2 × 10-6 to 0.1 mmol L-1 and from 1 × 10-7 to 0.05 mmol L-1 for H2SiO3 colloid and Fe(OH)3 colloid, respectively.
Desorption experiments of arsenic were carried out in sequential decant-refill steps immediately following the completion of the sorption experiments. The supernatant (4.0 mL) was removed and immediately replaced by the same volume of background solution (0.01 M NaNO3), and the vials were resealed and shaken. After 24 h of equilibration, the vials were centrifuged, arsenic in the supernatant was determined, and the amount of arsenic desorbed was calculated from mass differences. The above process was repeated for four complete cycles. All samples were performed at least in triplicate.
Speciation and analysis of arsenic by hydride generation-atomic fluorescence spectrometry
The AFS-9800 atomic fluorescence spectrometer (Beijing Kechuang Haiguang Instrument Co., Ltd, Beijing, China) was used for arsenic determination. The arsine was generated by adding precise, known volumes of the sample, a reducing solution of potassium tetrahydroborate solution (20%) and hydrochloric acid (10%) using an autosampler. Also, a pre-reducing solution (thiourea 10% and ascorbic acid 10%) was used to pre-reduce arsenic(V) to arsenic(III) when the task was to speciate arsenic(III) and arsenic(V). Arsenic(V) was determined by the difference between total inorganic arsenic and arsenic(III).
Results and discussion
Characterization of ceria NPs
The results of XRD in Figure 1b showed that ceria NPs were a single-phase, cubic, calcium fluoride-type structure with space group Fm3m, and no evidence was found for the existence of impurities in the products which was consistent with other reports .
The adsorption capacity qmax and adsorption constant KL can be determined from the slope and intercept of a linearized plot of Ce/qe against Ce.
where Kf and n are the Freundlich constants: n gives an indication of how favorable the adsorption is, and Kf (mg/g (L/mg)1/n) is the adsorption capacity of the adsorbent. If the value of 1/n is lower than 1, it indicates a normal Freundlich isotherm; otherwise, it is indicative of cooperative adsorption. The Freundlich constants can be obtained from the plot of log qe versus log Ce.
Isotherm model constants of three isotherm models for arsenic adsorption onto ceria NPs
qmax (mg g-1)
KL (L mg-1)
Kf (mg g-1) (L mg-1)1/n
Thermodynamic parameters associated with the adsorption processes
Thermodynamic parameters for arsenic adsorption onto ceria NPs
Δ G0 (kJ mol-1)
Δ H0 (kJ mol-1)
Δ S0 (J mol-1 K-1)
Adsorption and desorption
Hysteresis is referred to as irreversible adsorption which is reproducible and originates from a shift in the equilibrium point when a reaction approaches equilibrium from desorption direction rather than sorption [4, 26, 27]. Similar result was reported by Shirvani et al. that the quantity of Cd desorbed from the minerals after five cycles of desorption was depending on the initial load of Cd on the minerals . Recent studies supported irreversible deformation as the cause of hysteresis in flexible solids, such as natural organic matter and organoclays [5, 27]. During the adsorption-desorption cycle, pore deformation may result in some of adsorbent transferred to sites in the solid where free exchange with molecules in the bulk fluid phase is no longer possible.
Desorption of inorganic and organic contaminants from the adsorbent is rapidly gaining recognition owing to its importance to the fate, toxicity, and transport of these contaminants in the environmental system. If the contaminants would be released from the adsorbent in significant concentrations, either in the environmental or biotic mediums, they would be a risk for living organisms. In this work, high adsorption capacity and reversible adsorption of arsenic on ceria NPs suggest that ceria NPs may influence the fate and behavior of arsenic in the environment. Thus, ceria NPs with arsenic may exhibit synergistic effects when interacting with living organisms.
Adsorption characteristics of arsenic(III) and arsenic(V) in different environmental conditions
Inorganic arsenic has four oxidation states: +5, +3, 0, and -3. In the soil/water environment, it is mainly present in the +3 and +5 oxidation states. In reduced environments, arsenious acid is a common arsenic(III) aqueous species, whereas oxidized environments contain more arsenic(V) aqueous species. These two aqueous species may adsorb onto inorganic and organic components and precipitate in a variety of forms. The environmental fate of arsenic in subsurface environments is highly dependent on the arsenic speciation, pH, ionic strength, and the presence of adsorbents such as metal oxides. Furthermore, there are many kinds of colloidal solutions with different charges in water, for example, in general, H2SiO3 colloid surface has a negative charge and Fe(OH)3 colloid surface has a positive charge, which may affect the adsorption of arsenic on ceria NPs. However, little investigation had been conducted on the adsorption of arsenic by ceria NPs in different colloidal solutions. The experiments below were carried out to investigate the adsorption characteristic of arsenic onto ceria NPs in different environmental conditions.
From Figure 3, it could also be found that arsenite is commonly more strongly adsorbed on ceria NPs than arsenate especially when pH was above 9. Theoretically, arsenate is commonly more strongly adsorbed on ceria NPs than arsenite since arsenate presents as H2AsO4- and HAsO42- when pH is from 2 to 8, while arsenite presents as As(OH)30 species. Some reports showed that at all pH values, arsenic(V) was more strongly bound than arsenic(III) [28–30]. Thus, further experiments in our future study should be carried out to study the adsorption mechanism.
The ionic strength can influence the double-layer thickness and interface potential; thereby, it can affect the binding of the sorbed species [36, 37]. The specific and nonspecific adsorptions can be distinguished by evaluating the effect of ionic strength on anion partitioning . It was reported that the specific adsorption is unaffected by the change in ionic strength, whereas the nonspecific adsorption is likely to be influenced greatly by the change of ionic strength because of the competitive adsorption with counteractions. The insignificant impact of ionic strength indicated that the specific adsorption was found on the adsorption of arsenic(V) and arsenic(III) by ceria NPs which resulted from an inner sphere complex formation between arsenic and the surface of ceria NPs. The strong pH dependence and ionic strength independence further indicate that the adsorption mechanism is mainly surface complexation rather than ion exchange.
The high adsorption capacity and reversible adsorption of arsenic on ceria NPs clearly confirm that ceria NPs can interact with arsenic when they are released into the environment, which may influence the fate and behavior of arsenic and may enhance the toxicity of ENPs and/or arsenic. Taken together, the results indicate that studies dealing with the potential ecotoxicological effects of NPs for the environment have to be designed carefully in order to have the defined understanding between the NPs and the adsorbed chemicals in the environment.
This work is financially supported by the Ministry of Science and Technology of China (grant no. 2011CB933400), the Ministry of Environmental Protection of China (grant no. 201209012), the National Natural Science Foundation of China (grant nos. 10875136 and 10905062), and the China Postdoctoral Science Foundation (grant nos. 20090460520 and 201003155).
- Stephen JK, Pedro JJ, Graeme EB, Teresa FF, Richard DH, Delina YL, Shaily M, Michael JM, Jamie RL: Nanomaterials in the environment: behavior, fate, bioavailability, and effects. Environ Toxicol Chem 2008, 27: 1825–2851. 10.1897/08-090.1View Article
- Grazyna B, Jerzy G, Pawel LU: Nanoparticles: their potential toxicity, waste and environmental management. Waste Manage 2009, 29: 2587–2595. 10.1016/j.wasman.2009.04.001View Article
- Moore MN: Do nanoparticles present ecotoxicological risks for the health of the aquatic environment? Environ Int 2006, 32: 967–976. 10.1016/j.envint.2006.06.014View Article
- Fang J, Shan XQ, Wen B, Lin JM, Lu XC, Liu XD, Owens G: Sorption and desorption of phenanthrene onto iron, copper, and silicon dioxide nanoparticles. Langmuir 2008, 24: 10929–10935. 10.1021/la801459sView Article
- Yan XM, Shi BY, Lu JJ, Feng CH, Wang DS, Tang HX: Adsorption and desorption of atrazine on carbon nanotubes. J Colloid Interf Sci 2008, 321: 30–38. 10.1016/j.jcis.2008.01.047View Article
- Birbaum K, Brogioli R, Schellenberg M, Martinoia E, Stark WJ, Günther D, Limbach LK: No evidence for cerium dioxide nanoparticle translocation in maize plants. Environ Sci Technol 2010, 44: 8718–8723. 10.1021/es101685fView Article
- Ludwig KL, Robert B, Elisabeth M, Rolf K, René G, Wendelin JS: Removal of oxide nanoparticles in a model wastewater treatment plant: influence of agglomeration and surfactants on clearing efficiency. Environ Sci Technol 2008, 42: 5828–5833. 10.1021/es800091fView Article
- Chen JP, Patil S, Seal S, Mcginnis JF: Rare earth nanoparticles prevent retinal degeneration induced by intracellular peroxides, nature nanotechnology. Nature Nanotechnology 2006, 1: 142–150. 10.1038/nnano.2006.91View Article
- Zholobak NM, Ivanov VK, Shcherbakov AB, Shaporev AS, Polezhaeva OS, Baranchikov AY, Spivak NY, Tretyakov YD: UV-shielding property, photocatalytic activity and photocytotoxicity of ceria colloid solutions. J Photoch Photobio B 2010, 102: 32–38.View Article
- Yuan Q, Duan HH, Li LL, Sun LD, Zhang YW, Yan CH: Controlled synthesis and assembly of ceria-based nanomaterials. J Colloid Interf Sci 2009, 335: 151–167. 10.1016/j.jcis.2009.04.007View Article
- Thill A, Zeyons O, Spalla O, Chauvat F, Rose J, Auffan M, Flank AM: Cytotoxicity of CeO2 nanoparticles for Escherichia coli . Physico-chemical insight of the cytotoxicity mechanism. Environ Sci Technol 2006, 40: 6151–6156. 10.1021/es060999bView Article
- Safi M, Sarrouj H, Sandre O, Mignet N, Berret JF: Interactions between sub-10-nm iron and cerium oxide nanoparticles and 3T3 fibroblasts: the role of the coating and aggregation state. Nanotechnology 2010, 21: 145103. 10.1088/0957-4484/21/14/145103View Article
- Hoecke KV, Quik JT, Mankiewicz-Boczek J, Schamphelaere KA, Elsaesser A, Meeren PV, Barnes C, McKerr G, Howard VC, Meent DV, Rydzyński K, Dawson KA, Salvati A, Lesniak A, Lynch I, Silversmit G, Samber BD, Vincze L, Janssen CR: Fate and effects of CeO2nanoparticles in aquatic ecotoxicity tests. Environ Sci Technol 2009, 43: 4537–4546. 10.1021/es9002444View Article
- Johnston BD, Scown TM, Moger J, Cumberland SA, Baalousha M, Linge K, Aerle R, Jarvis K, Lead JR, Tyler CR: Bioavailability of nanoscale metal oxides TiO2, CeO2, and ZnO to fish. Environ Sci Technol 2010, 44: 1144–1151. 10.1021/es901971aView Article
- López-Moreno ML, Rosa G, Hernández-Viezcas J, Castillo-Michel H, Botez CE, Peralta-Videa JR, Gardea-Torresdey JL: Evidence of the differential biotransformation and genotoxicity of ZnO and CeO2nanoparticles on soybean ( Glycine max ) plants. Environ Sci Technol 2010, 44: 7315–7320. 10.1021/es903891gView Article
- Lu K, Zhang ZY, He X, Ma YH, Zhou KB, Zhang HF, Bai W, Ding YY, Wu ZQ, Zhao YL, Chai ZF: Bioavailability and distribution of ceria nanoparticles in simulated aquatic ecosystems, quantification with a radiotracer technique. J Nanosci Nanotechno 2010, 10: 8658–8662. 10.1166/jnn.2010.2494View Article
- Niu JL, Asim A, Linda MR, Wang XH, Pappachan EK: Cardioprotective effects of cerium oxide nanoparticles in a transgenic murine model of cardiomyopathy. Cardiovasc Res 2007, 73: 549–559. 10.1016/j.cardiores.2006.11.031View Article
- Huang JH, Ilgen G, Vogel D, Michalzik B, Hantsch S, Tennhardt L, Bilitewski B: Emissions of inorganic and organic arsenic compounds via the leachate pathway from pretreated municipal waste materials: a landfill reactor study. Environ Sci Technol 2009, 43: 7092–7097. 10.1021/es901605qView Article
- Williams PN, Lei M, Sun GX, Huang Q, Lu Y, Deacon C, Meharg AA, Zhu YG: Occurrence and partitioning of cadmium, arsenic and lead in mine impacted paddy rice: Hunan, China. Environ Sci Technol 2009, 43: 637–642. 10.1021/es802412rView Article
- Arai Y, Lanzirotti A, Sutton S, Davis JA, Sparks DL: Arsenic speciation and reactivity in poultry litter. Environ Sci Technol 2003, 37: 4083–4090. 10.1021/es0340580View Article
- Chen CL, Li XL, Zhao DL, Tan XL, Wang XK: Adsorption kinetic, thermodynamic and desorption studies of Th(IV) on oxidized multi-wall carbon nanotubes. Colloids Surface A 2007, 302: 449–454. 10.1016/j.colsurfa.2007.03.007View Article
- Zhang F, Jin Q, Chan SW: Ceria nanoparticles: size, size distribution, and shape. J Appl Phys 2004, 95: 4319–4325. 10.1063/1.1667251View Article
- Ma YH, Kuang LL, He X, Bai W, Ding YY, Zhang ZY, Zhao YL, Chai ZF: Effects of rare earth oxide nanoparticles on root elongation of plants. Chemosphere 2010, 78: 273–279. 10.1016/j.chemosphere.2009.10.050View Article
- Zhang J, Ju X, Wu ZY, Liu T, Hu TD, Xie YN: Structural characteristics of cerium oxide nanocrystals prepared by the microemulsion method. Chem Mater 2001, 13: 4192–4197. 10.1021/cm010235pView Article
- Rane N, Zou H, Buelna G, Lin JYS: Sol-gel synthesis and properties of unsupported and supported mesoporous ceria membranes. J Membrane Sci 2005, 256: 89–97.
- Shirvani M, Kalbasi M, Shariatmadari H, Nourbakhsh F, Najafi B: Sorption-desorption of cadmium in aqueous palygorskite, sepiolite, and calcite suspensions: isotherm hysteresis. Chemosphere 2006, 65: 2178–2184. 10.1016/j.chemosphere.2006.06.002View Article
- Sander M, Lu YF, Pignatello JJ: A thermodynamically based method to quantify true sorption hysteresis. J Environ Qual 2005, 34: 1063–1072. 10.2134/jeq2004.0301View Article
- Goldberg S: Competitive adsorption of arsenate and arsenite on oxides and clay minerals sabine goldberg. Soil Sci Soc Am J 2002, 66: 413–421. 10.2136/sssaj2002.0413View Article
- Chakraborty S, Wolthers M, Chatterjee D, Charlet L: Adsorption of arsenite and arsenate onto muscovite and biotite mica. J Colloid Interf Sci 2007, 309: 392–401. 10.1016/j.jcis.2006.10.014View Article
- Buschmann J, Kappeler A, Lindauer U, Kistler D, Berg M, Sigg L: Arsenite and arsenate binding to dissolved humic acids: influence of pH, type of humic acid, and aluminum. Environ Sci Technol 2006, 40: 6015–6020. 10.1021/es061057+View Article
- Antelo J, Avena M, Fiol S, López R, Arce F: Effects of pH and ionic strength on the adsorption of phosphate and arsenate at the goethite-water interface. J Colloid Interf Sci 2005, 285: 476–486. 10.1016/j.jcis.2004.12.032View Article
- Vithanage M, Chandrajith R, Bandara A, Weerasooriya R: Mechanistic modeling of arsenic retention on natural red earth in simulated environmental systems. J Colloid Interf Sci 2006, 294: 265–272. 10.1016/j.jcis.2005.07.026View Article
- Arai Y, Elzinga EJ, Sparks DL: X-ray absorption spectroscopic investigation of arsenite and arsenate adsorption at the aluminum oxide-water interface. J Colloid Interf Sci 2001, 235: 80–88. 10.1006/jcis.2000.7249View Article
- Catalano JG, Zhang Z, Fenter P, Bedzyk MJ: Inner-sphere adsorption geometry of Se(IV) at the hematite (100)-water interface. J Colloid Interf Sci 2006, 297: 665–671. 10.1016/j.jcis.2005.11.026View Article
- Su TZ, Guan XH, Gu GW, Wang JM: Adsorption characteristics of As(V), Se(IV), and V(V) onto activated alumina: effects of pH, surface loading, and ionic strength. J Colloid Interf Sci 2008, 326: 347–353. 10.1016/j.jcis.2008.07.026View Article
- Chen CL, Wang XK: Sorption of Th (IV) to silica as a function of pH, humic/fulvic acid, ionic strength, electrolyte type. Appl Radiat Isotopes 2007, 65: 155–163. 10.1016/j.apradiso.2006.07.003View Article
- Xu RK, Wang Y, Tiwari D, Wang HY: Effect of ionic strength on adsorption of As(III) and As(V) on variable charge soils. J Environ Sci 2009, 21: 927–932. 10.1016/S1001-0742(08)62363-3View Article
- Altundoğan HS, Altundoğan S, Tümen F, Bildik M: Arsenic adsorption from aqueous solutions by activated red mud. Waste Manage 2002, 22: 357–363. 10.1016/S0956-053X(01)00041-1View Article
- Raven K, Jain A, Loeppert R: Arsenite and arsenate adsorption on ferrihydrite: kinetics, equilibrium, and adsorption envelopes. Environ Sci Technol 1998, 32: 344–349. 10.1021/es970421pView Article
- Wang YH, Morin G, Ona-Nguema G, Juillot F, Guyot F, Calas G, Brown GE: Evidence for different surface speciation of arsenite and arsenate on green rust: an EXAFS and XANES Study. Environ Sci Technol 2010, 44: 109–115. 10.1021/es901627eView Article
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