Preparation and application of oyster shell supported zero valent nano scale iron for removal of natural organic matter from aqueous solutions
© Alipour et al.; licensee BioMed Central. 2014
Received: 4 August 2014
Accepted: 6 December 2014
Published: 19 December 2014
In this Research, oyster shell supported zero valent iron nanoparticles were prepared and applied for the removal of natural organic matters (NOMs) from aqueous solutions under different experimental conditions.
The nanoadsorbents prepared by wet impregnation method, then characterized using Scanning Electron Microscopy, Energy Dispersive Spectroscopy, X-Ray Fluorescence and BET analysis. Adsorption test was done in a batch reactor and the effects of different parameters such as initial adsorbate concentration, adsorbent dose, adsorption kinetic, pH, and temperature on removal of NOMs (humic acid as the indicator) were studied.
Results showed that particle size of nanoadsorbent was in the range of 60-83 nm, and surface area and micropore volume as 16.85 m2/g and 0.021 m3/g, respectively; the main elements of adsorbent were Ca, O, Fe and Na and lime, as high as about 94.25% was the main structural component of the total weight. Produced nanoadsorbent was not soluble in water. It was also shown that by increasing the nanoadsorbent dose from 0.5 to 5 g/100 ml, the removal of humic acid increased from 62.3% to 97.4%. An inverse relationship was found between initial concentration and adsorption capacity, so that a decreasing rate of 33% for humic acid removal was observed by increasing pH from 5 to 10. Temperature increase from 25°C to 40°C, resulted in an increase in humic acid removal from 76.8% to 91.4% and its adsorption on the adsorbent could be better described by Freundlich isotherm (n = 0.016, Kf = 0.013 and R2 = 0.74). The most fitted adsorption kinetic model was pseudo-second order model.
The chemical structure of nanoadsorbent was proper and free from harmful substances. Despite the relative good condition of the effective surface, due to the large size of the shell, the overall micropore volume was low. Hence the qualitative characteristics the adsorbent caused the absorption capacity of humic acid to be low (0.96 mg/g).
Although surface water is an important natural resource used for many purposes, especially drinking, this resource generally contain natural organic matters (NOMs) so many scientific references have pointed out that more than 1500 different organic compounds are suspected to be present in drinking waters ,. Naturally organic materials, a nonhomogeneous mixture of complex organic compounds, including; humic acids (HA), lipids, proteins, hydrophilic acids, carboxylic acids, amino acids, polysaccharides, and hydrocarbons are invariably present in surface and ground water resources, in dissolved or colloidal forms . Various environmental and health problems have been reported that may be related to the presence of NOMs in natural waters, including; (a) the potential of NOMs have to cause undesirable color and taste ; (b) NOMs contributing the reactions with heavy metals and biocides to yield high concentrations of these substances and enhance their transportation in water ; (c) NOMs role in increasing coagulant and disinfectant dose requirements that lead to more sludge amounts; (d) in treatment plants, NOMs react with chlorine to form harmful organic compounds ; (e) NOMs are important factors in fouling which affect various applications of membrane processes ; and (f) their tendency to compete with low-molecular weight synthetic organic chemicals and inorganic pollutants, reducing their adsorption rates and equilibrium capacities ,.
Considering harmful effects of NOMs on human health, these compounds should be eliminated from water before the chlorination process in drinking water treatment plants and it is important for the public health and drinking water industry to find reliable methods to remove a wide range of organic contaminants from water . During the recent years, a large number of researches have been carried out on the NOMs removal from water in order to minimize its impacts on water quality ,-. Based on these researches, the most conventional options for NOM removal include membrane filtration and ion exchange ,, ozonation , biodegradation , ultrasound waves , adsorption, and coagulation . Among the methods, membrane separation and adsorption were the most effective and available processes for removing NOMs from water . High removal efficiency and no harmful by-products production are the main advantages for adsorption process and many kinds of adsorbents have been developed for the removal of humic acid from water.
During the past few years, nanoparticles have been proposed as a removal method for a wide range of pollutants from waters . Some important nanoparticles in water treatment include metal-containing nanoparticles, carbonaceous nanomaterials, zeolites, and dendrimers . As nanoscale zero-valent iron (NZVI) particles have unique reactive and sorption characteristics, they have received high attention for the treatment of contaminated waters ,.
Several studies have been conducted using various materials such as mesoporous silica beads , carbon and titanium dioxide , chitosan beads , ceramic membranes , kaolin , and betonite  as a bases for nanoparticles. In southern coasts of Iran, there is a considerable amount of oyster shells which may have the potential to be used for a perfect bases for nanoadsorbents, and so far no study and information are achieved on the use of the shell as adsorbent. Considering the possibility of successful production of air-stable ZVI nanoparticles with a high gravimetric ratio, good stability and no harmful matters, that in this research, it was studied as a bases for NZVI.
This study focused on the oyster shell supported NZVI application for the removal of NOMs under different experimental conditions, in order to remove taste and odor-causing agents from surface water resources.
In this study, HA was used as NOMs representative and stock solution of HA was prepared using 1 g of HA powder dissolved in 1 L of deionized water, followed by filtering the solution through a 0.45 μ membrane filter (cellulose acetate). The solution was further diluted to the required concentrations and were stored at 4°C before application.
Preparation of nano-supported shell
The formation of the oyster shell supported iron nanoadsorbent was carried out by wet impregnation technique -. Shells collected from the coast of the Persian Gulf were transported to research lab and after physically cleaning (removal of mud, rinsing for 10 min and washing by deionized water), were crushed, dried in 100°C oven and then sieved with a mesh of 100. To prepare the NZVI coated shell, the shell beads were placed in the reactor during the synthesis of NZVI, by using the reduction of dissolved iron method, which comprised of four stages; mixing, separating, washing and drying ,.
Afterwards, the contents of the flask were discharged to a funnel containing a millipore filter, under the suction force, leading to dewatering. The shell beads coated with NZVI were washed by ethanol, and then dried at 50°C and then kept in desiccators.
Characterization of nanoadsorbent
Laboratory synthesized nanoadsorbent was analyzed using Scanning Electron Microscopy (SEM) of TESCAN, Energy Dispersive Spectroscopy (EDS) and X-Ray Fluorescence (XRF). The specific surface area of nanoadsorbent was analyzed using BET-N2 adsorption method.
Batch reactor adsorption system and experiments
Adsorption of HA onto produced adsorbent was carried out by a batch reactor and effect of different parameters such as initial HA concentration, adsorbent dose, pH, and temperature were studied.
Different doses of nanoadsorbent (0.5gr, 1gr, 3gr and 5gr) were added to the reaction flask containing 100 mL of 5 mg/L HA solution with the initial pH of 7 and temperature of 25°C. The containers were sampled: firstly at intervals of 5 and 10 min and then at a frequency of every 15 min to reach equilibrium time. After shaking and settling for 5 min, the samples supernatant were centrifuged followed by membrane filter (0.45 μm, cellulose acetate), absorbance values of solutions remaining without adsorption were measured by using UV–Vis spectrophotometer at wavelength of 254 nm. In the next step, adsorption equilibrium data were correlated with two well-known empirical isotherm models; Freundlich and Langmuir.
The kinetic of HA adsorption
After determining the adsorption isotherm, using collected data and models related to the absorption kinetics, modeling kinetic of HA adsorption study on the nanoadsorbent was determined.
The effect of initial HA concentration
The effect of initial HA concentration on the adsorption rate was studied by contacting 0.5 g of adsorbent at room temperature of 25°C and pH = 7 using four initial concentrations of HA solution (0.5, 2, 5 and 10 mg/L) in 100 mL of samples at time = 0 and at selected time intervals (up to a maximum of 180 min), sample concentration was determined by UV–Vis spectrophotometer.
The effect of pH
In order to survey the pH effect on HA adsorption, pH of the solution was changed in the range of 5.0 and 10.0 at four intervals (5, 7, 8 and 10) using either 0.1 mol/L NaOH or 0.1 mol/L HCl. pH values were determined using a Elmetron CP-501 pH meter, fitted with a combined glass-reference electrode.
The effect of temperature
In order to assess the effect of temperature on the equilibrium adsorption capacity of HA, 0.5gr of the nanoadsorbent was used at different temperatures (25, 30 and 40°C), with 5 mg/L HA solutions, optimum pH = 5 and in equilibrium contact time.
Results and discussion
Characterization of nanoadsorbent
Physical properties of the nanoadsorbent
BET surface area
Solubility @ (20°C)
Chemical composition of the nanoadsorbent
Chemical composition of the nanoadsorbent
As shown in the Figure 1, most of the sheet structure has been changed to irregular small particles and depicts the synthesized nanoadsorbent with an approximately 60–85 nm diameter. The main elements of the adsorbent were Ca, O, Fe and Na and as it can be found from Table 3, the highest component of the adsorbents was lime (CaCO3 and CaO), whit about 94.25% of the total weight.
The effect of the adsorbent dose
Kinetic of HA adsorption
Based on results of Figure 4, the pseudo second order model generates better fit to the experimental data of the investigated adsorption of HA on nanoadsorbent (R2 = 0.997). The degree of the reaction is determined by sharing or exchange of electrons between adsorbent positive (nzvi) and negative groups (HA).
The effect of initial HA concentration
As can be seen from Figure 5 when an increase occurs in the initial concentrations, the adsorption capacity of HA would enhance. Driving force is one of the most important factors in the adsorption process so the adsorption capacity of HA is a function of HA initial concentration, as it is important to overcome the mass transfer resistance of the HA between the adsorbate and the adsorbent. In other words, the increase in the mass driving force allows more HA molecules to pass from the solution to the adsorbent surface. Therefore there is an inverse relationship between initial concentration and adsorption capacity . This finding were in accordance with Moussavi et al  who investigated adsorption characteristics of HA onto single-walled carbon nanotubes and reported that the amount of adsorbed HA was higher at lower initial concentrations of HA.
The effect of pH
The effect of temperature
The obtained results revealed that surface area and pore volume of nanoadsorbent were 16.85 (m2/g) and 0.021 m3/g, respectively; the main elements of the adsorbent were Ca, O, Fe and Na and most of the adsorbent component was composed of lime (CaCO3 and CaO about 94.25% of the total weight). The produced nanoadsorbent was not soluble in water. HA Adsorption onto the nanoadsorbent increased by increasing of adsorbent dose and temperature and decreased by increasing HA concentration and pH. The r-shaped adsorption isotherm indicated a high affinity of contact time with adsorption rate. In optimal conditions provided in the study (HA = 5 mg/L, nanoadsorbent dose = 0.5 g/100 mL, pH = 5 and temperature = 40°C), maximum HA removal efficiency reached to 94.6%, within 90-120 min at the experimental conditions in all cases is Pseudo-second order and Freundlich isotherm models were fitted to the adsorption kinetic and isotherm, respectively.
The authors are grateful to the Dr Elham Boushehri and Mrs. Afsoon Pirouzan, Hormozgan University of Medical Sciences, as well as all laboratory staffs of the Departments of Environmental Health Engineering in both Hormozgan University of Medical Sciences and Tehran University of Medical Sciences.
- Yue Z, Economy J: Nanoparticle and nanoporous carbon adsorbents for removal of trace organic contaminants from water. J Nanoparticle Res 2005, 7: 477–487. 10.1007/s11051-005-4719-7View ArticleGoogle Scholar
- Mahvi AH, Alipour V, Rezaei L: Atmospheric moisture condensation to water recovery by home air conditioners. Am J Appl Sci 2013, 10(8):917–923. 10.3844/ajassp.2013.917.923View ArticleGoogle Scholar
- Moussavi G, Talebi S, Farrokhi M, Mojtabaee Sabouti R: The investigation of mechanism, kinetic and isotherm of ammonia and humic acid co-adsorption onto natural zeolite. Chem Eng J 2013, 171: 1159–1169. 10.1016/j.cej.2011.05.016View ArticleGoogle Scholar
- Bai R, Zhang X: Polypyrrole-coated granules for humic acid removal. J Colloid Interface Sci 2001, 243: 52–60. 10.1006/jcis.2001.7843View ArticleGoogle Scholar
- Schmitt D, Saravia F, Frimmel FH, Schuessler W: NOM facilitated transport of metal ions in aquifers: importance of complex-dissociation kinetics and colloid formation. Water Res 2003, 37: 3541–3550. 10.1016/S0043-1354(01)00525-5View ArticleGoogle Scholar
- Yuan W, Zydney AL: Humic acid fouling during ultrafiltration. Environ Sci Technol 2000, 34: 5043–5050. 10.1021/es0012366View ArticleGoogle Scholar
- Klausen J, Vikesland PJ, Kohn T, Burris DR, Ball WP, Roberts AL: Longevity of granular iron in groundwater treatment processes: solution composition effects on reduction of organohalides and nitroaromatic compounds. Environ Sci Technol 2003, 37: 1208–1218. 10.1021/es025965sView ArticleGoogle Scholar
- Tratnyek PG, Scherer MM, Deng B, Hu S: Effects of natural organic matter, anthropogenic surfactants, and model quinones on the reduction of contaminants by zero- valent iron. Water Res 2001, 35: 4435–4443. 10.1016/S0043-1354(01)00165-8View ArticleGoogle Scholar
- Bansal RC, Goyal M: Activated carbon adsorption. Taylor & Francis Group, New York; 2005.View ArticleGoogle Scholar
- Jonglertjunya W, Lertchutimakul T: Equilibrium and kinetic studies on the adsorption of humic acid by activated sludge and Bacillus subtilis. Songklanakarin J Sci Technol 2012, 34(6):669–677.Google Scholar
- Giasuddin AM, Kanel S, Choi HC: Adsorption of Humic Acid onto Nanoscale Zerovalent Iron and Its Effect on Arsenic Removal. Environ Sci Technol 2007, 41: 2022–2027. 10.1021/es0616534View ArticleGoogle Scholar
- Harman BI, Koseoglu H, Yigit NO, Beyhan M, Kitis M: The use of iron oxide-coated ceramic membranes in removing natural organic matter and phenol from waters. Desalination 2010, 261: 27–33. 10.1016/j.desal.2010.05.052View ArticleGoogle Scholar
- Doulia D, Leodopoulos C, Gimouhopoulos K, Rigas F: Adsorption of humic acid on acid-activated Greek bentonite. J Colloid Interface Sci 2009, 340: 131–141. 10.1016/j.jcis.2009.07.028View ArticleGoogle Scholar
- Kabsch-Korbutowicz M: Effect of Al coagulant type on natural organic matter removal efficiency in coagulation/ultrafiltration process. Desalination 2005, 185(1–3):327–333. 10.1016/j.desal.2005.02.083View ArticleGoogle Scholar
- Bolto B, Dixon D, Eldridge R, King S, Linge K: Removal of natural organic matter by ion exchange. Water Res 2002, 36(20):5057–5065. 10.1016/S0043-1354(02)00231-2View ArticleGoogle Scholar
- Zazouli MA, Nasseri S, Mahvi AH, Gholami M, Mesdaghinia AR, Younesian M: Retention of humic acid from water by nanofiltration membrane and influence of solution chemistry on membrane performance. Iran J Environ Health Sci Eng 2008, 5(1):11–18.Google Scholar
- Selcuk H, Rizzo L, Nikolaou AN, Meric S, Belgiorno V, Bekbolet M: DBPs formation and toxicity monitoring in different origin water treated by ozone and alum/PAC coagulation. Desalination 2007, 210(1–3):31–43. 10.1016/j.desal.2006.05.030View ArticleGoogle Scholar
- Leiknes T, Lazarova M, Odegaard H: Development of a hybrid ozonation biofilm-membrane filtration process for the production of drinking water. Water Sci Technol 2005, 51(6–7):241–248.Google Scholar
- Mahvi AH, Maleki A, Rezaee R, Safari M: Reduction of humic substances in water by application of ultrasound waves and ultraviolet irradiation. Iran J Environ Health Sci Eng 2009, 6(4):233–240.Google Scholar
- Ho L, Newcombe G: Effect of NOM, turbidity and floc size on the PAC adsorption of MIB during alum coagulation. Water Res 2005, 39(15):3668–3674. 10.1016/j.watres.2005.06.028View ArticleGoogle Scholar
- Li Q, Mahendra S, Lyon DY, Brunet L, Liga MV, Li D, Alvarez PJ: Antimicrobial nanomaterials for water disinfection and microbial control: Potential applications and implications. Water Res 2008, 4(18):4591–4602. 10.1016/j.watres.2008.08.015View ArticleGoogle Scholar
- Savage N, Diallo MS: Nanomaterials and water purification: Opportunities and challenges. J Nanoparticle Res 2005, 7(4–5):331–342. 10.1007/s11051-005-7523-5View ArticleGoogle Scholar
- Bezbaruah AN, Shanbhogue SS, Simsek S, Khan E: Encapsulation of iron nanoparticles in alginate biopolymer for trichloroethylene remediation. J Nanoparticle Res 2011, 13: 6673–6681. 10.1007/s11051-011-0574-xView ArticleGoogle Scholar
- Dickinson M, Scott TB: The application of zero valent iron nanoparticles for the remediation of a uranium-contaminated waste effluent. J Hazard Mater 2010, 178: 171–179. 10.1016/j.jhazmat.2010.01.060View ArticleGoogle Scholar
- Park H, Yeon KH, Park YM, Lee SJ, Lee SH, Choi YS, Chung Y: Reduction of nitrate by nanoscale zero-valent iron supported on mesoporous silica beads. J Water Environ Technol 2008, 6(1):35–42. 10.2965/jwet.2008.35View ArticleGoogle Scholar
- Petala E, Baikousi M, Dimos K, Filip J, Pechousek J, Tucek J, Safarova K, Douvalis A, Bakas T, Karakassides ZM, Zboril R: Zero valent iron nanoparticles supported on porous matrices: enhanced efficiency and application for water treatment. J Hazard Mater 2013, 261: 295–306. 10.1016/j.jhazmat.2013.07.046View ArticleGoogle Scholar
- Liu T, Zhao L, Sun D, Tan X: Entrapment of nanoscale zero-valent iron in chitosan beads for hexavalent chromium removal from wastewater. J Hazard Mater 2010, 184(1–3):724–730. 10.1016/j.jhazmat.2010.08.099View ArticleGoogle Scholar
- Zhang X, Lin S, Lu XQ, Chen ZI: Removal of Pb (II) from water using synthesized kaolin supported nanoscale zero-valent iron. Chem Eng J 2010, 163: 243–248. 10.1016/j.cej.2010.07.056View ArticleGoogle Scholar
- WZW Yaacob, Kamaruzaman N, Samsudin AR: Development of nano-zero valent iron for the remediation of contaminated water. Chemical engineering transactions 2012, 28: 25–30.Google Scholar
- Pan BC, Chen BJ, Meng XQ, Pan XT, Li MW, Zhang X, Zhang JL, Chen AB, Zhang XQ, Sun Y: Application of an effective method in predicting breakthrough curves of ?xed bed adsorption onto resin adsorbent. J Hazard Mater 2005, B,124: 74–80. 10.1016/j.jhazmat.2005.03.052View ArticleGoogle Scholar
- Wan Ngah WS, Kamari A, Koay YJ: Equilibrium and kinetic studies of adsorption of copper (II) on chitosan and chitosan/PVA beads. Int J Biol Macromol 2004, 3: 155–161. 10.1016/j.ijbiomac.2004.03.001View ArticleGoogle Scholar
- Perez-Aguilar NV, Diaz-Flores PE, Rangel-Mendez JR: The adsorption kinetics of cadmium by three different types of carbon nanotubes. J Colloid Interface Sci 2011, 364: 279. 10.1016/j.jcis.2011.08.024View ArticleGoogle Scholar
- Bringle CD, Shibi IG, Vinod VD, Anirudhan TS: Sorption of humic acid from aqueos solutions by lanthana alumina oxide pillared bentonite. J Sci Ind Res 2005, 46: 782–788.Google Scholar
- Zulfikar MA: Effect of Temperature on Adsorption of Humic Acid from Peat Water onto Pyrophyllite. International Journal of Chemical, Environmental & Biological Sciences, 2013, 1(1):88–90.Google Scholar
- Zeinali F, Ghoreyshi A, Najafpour DD: Adsorption of dichloromethane from aqueous phase using granular activated carbon; Isotherm and breakthrough curve measurements. Middle East J Sci Res 2010, 5(4):191–198.Google Scholar
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