Metal Oxide Nanostructures: Synthesis, Properties, and ApplicationsView this Special Issue
Research Article | Open Access
Comparing and Optimizing Nitrate Adsorption from Aqueous Solution Using Fe/Pt Bimetallic Nanoparticles and Anion Exchange Resins
This research work was carried out for the removal of nitrate from raw water for a drinking water supply. Nitrate is a widespread ground water contaminant. Methodology employed in this study included adsorption on metal based nanoparticles and ion exchange using anionic resins. Fe/Pt bimetallic nanoparticles were prepared in the laboratory, by the reduction of their respective salts using sodium borohydride. Scanning electron microscope, X-ray diffraction, energy dispersive spectrometry, and X-ray florescence techniques were utilized for characterization of bimetallic Fe/Pt nanoparticles. Optimum dose, pH, temperature, and contact time were determined for removal through batch tests, both for metal based nanoparticles and anionic exchange resin. Adsorption data fitted well the Langmuir isotherm and conformed to the pseudofirst-order kinetic model. Results indicated 97% reduction in nitrate by 0.25 mg/L of Fe/Pt nanoparticles at pH 7 and 83% reduction in nitrate was observed using 0.50 mg/L anionic exchange resins at pH 4 and contact time of one hour. Overall, Fe/Pt bimetallic nanoparticles demonstrated greater removal efficiency due to the small particle size, extremely large surface area (627 m2/g), and high adsorption capacity.
Nitrate is the most widely available contaminant in ground and surface waters . Excess of nitrate in drinking water results from anthropogenic sources, for example, overfertilization in agriculture, cattle shed discharge, untreated sewage, leakage from septic systems, infiltration of landfill leachate, and industrial waste water [2–5]. Out of these, synthetic fertilizers are the major contributors of nitrate pollution . Nitrate concentration above the maximum permissible limit in drinking water is injurious to human health. Nitrate exposure can also lead to several health issues such as blue baby syndrome, increased infant mortality, birth defects, abdominal pain, diarrhea, vomiting, diabetes, hypertension, respiratory tract infections, and changes in the immune system [7–11]. To limit the risk to human health from nitrate in drinking water, the Maximum Contaminant Level (MCL) is set to be 10 mg -N/L (45 mg /L) by USEPA, while the World Health Organization (WHO) and the European Community have set the MCL at 11.3 mg -N/L (50 mg /L) [12, 13]. Numerous technologies are available for removal of nitrate from water. These include reverse osmosis, electrodialysis, biological denitrification, and ion exchange methods. In case of reverse osmosis (RO) water passes through a semipermeable membrane, and nitrate and other ions are rejected because their size is greater than the membrane pore size [14, 15]. Biological denitrification is widely practiced for the treatment of municipal and industrial wastewater but is less commonly used in drinking water applications . Ion exchange is a process in which the target ion gets exchanged with a loosely adsorbed ion on a resin. Ion exchange is also like a reversible chemical process in which ions from an insoluble permanent solid medium (the ion exchanger is usually a resin) are exchanged for ions in a solution . This process is widely adopted for nitrate removal because of its simplicity, effectiveness, and relatively low cost [15–17]. Most of the on-going research has focused on nanosized zerovalent iron (NZVI) particles which typically have their size within the range of 1–100 nm [18, 19]. The nanosized iron have larger surface area, about ten to hundreds times larger than microscopic iron powder, which results in more exposure of particles surface leading to enhanced adsorption efficiency .
NZVI supplemented with the secondary metal is a new technique for nitrate removal, which enhances the catalytic reactivity through hydrogenation [21, 22]. Secondary metal also enhances reaction rate . In order to improve the nitrate removal, various bimetallic nanoparticles were tested in batch studies and the most efficient combination of metals, that is, (Fe/Pt) nanoparticles, was compared with commonly used, strong base anionic exchange resins (Amberlite IRA402 Cl). Langmuir and Freundlich isotherm models were used to study favorability of adsorption. To study kinetics of the chemical reactions pseudosecond-order kinetics model was applied.
2. Materials and Methods
Chemicals used in this research work included NaBH4 (Sigma-Aldrich), FeCl3·6H2O (Merck), FeSO4·7H2O (Merck), PtCl4 (Merck), PEG-4000 (Merck), and CuSO4·6H2O (Merck). For solution preparation, known quantities of the compounds were dissolved in deionized water (EC < 0.7 μS/cm, Labconco Waterpro PS). KNO3 was used for the nitrate solutions. For ion exchange experiments, strong base anion exchange resins (Amberlite IRA402 Cl) were purchased from Sigma-Aldrich. 0.1 M. Hydrochloric acid (HCl) and sodium hydroxide (NaOH) were used to adjust pH of the nitrate solutions. 10% NaCl was used for regeneration of anionic exchange resins.
2.2.1. Synthesis of Pt/Fe Bimetallic Nanoparticles
Fe/Pt bimetallic nanoparticles were synthesized in the laboratory in a Vacuum Glove Box (model: CV-1000 SAMPLATEC Corp., Japan) in an inert atmosphere. To synthesize Fe/Pt nanoparticles, NaBH4 (0.2 M, 99% Aldrich) solution was prepared in DI water/ethanol in 4 : 1 (v/v) and added slowly at the rate of 2 mL/min to FeCl3·6H2O (0.05 M, 99% Merck) and PtCl4 (0.05 M, 99% Merck) aqueous solution at 400 rpm in nitrogen atmosphere in glove box. The solution was filtered using 0.45 μm membrane filter in inert atmosphere to avoid contact of nanoparticles with air, prior to titration against HNO3. The resulting nanoparticles were washed thrice with distilled water and ethanol and stored in the dark.
2.2.2. Characterization of Fe/Pt Bimetallic Nanoparticles
Bimetallic nanoparticles were analyzed through X-ray diffraction (XRD, JEOL JDX-II, Japan). X-ray fluorescence analysis was performed using XRF-JEOL (Model JSX-3202M, Japan). The scanning electron microscope (JSM-6460, JEOL Ltd., Japan) attached with energy dispersive spectrometer (EDS, JSM-6460, JEOL Ltd., Japan) was used to find out surface morphology and composition of nanoparticles. The porous texture characterization of the samples was recorded by N2 adsorption data at −196°C (Autosorb-6B apparatus from Quantachrome ) the specific BET surface area () was determined by applying using Brunauer-Emmett-Teller (BET) equation.
2.2.3. Batch Experiments Using Fe/Pt Bimetallic Nanoparticles
Batch experiments were carried out in 250 mL glass beaker covered with aluminum foil. All of the apparatus was covered, during experimentation, to restrict photocatalytic activity of nanoparticles and, moreover, to study adsorption efficiency of nanoparticles only. All experimental conditions optimization experiments were performed with 100 mg/L nitrate solutions. For dosage optimization, test solutions containing different concentrations of Fe/Pt bimetallic nanoparticles (0.1, 0.25, 0.50, 0.75, and 1 g) were placed at an orbital shaker at 200 rpm for one hour at room temperature. After dosage optimization, test solution with optimized dosage was tested at 200 rpm for one hour, at three different pH levels (4, 7, and 10). Subsequent to dose and pH optimization, test solutions with optimized dosage were tested for different contact times (5, 10, 15, 20, 30, 45, 60, 90, and 120 min), with optimized dosage and optimized pH. Finally, effect of temperature on removal efficiencies was studied at 15, 25, and 40°C, with all other optimized conditions.
2.2.4. Batch Experiments Using Anionic Exchange Resins
Slurry based anionic exchange experiments were performed at different temperatures (i.e., 25, 45, and 60°C), in 250 mL beaker containing nitrate solution added with varying quantities of anionic resin. Mixing was maintained by orbital shaker. After providing specific mixing time, the sample was filtered and tested. Parameters such as pH (4, 7, and 10), effect of initial nitrate concentrations (10, 25, 50, 100, 200, 300, 400, and 500 mg/L) on removal efficiencies, and reaction times (5, 10, 15, 30, 45, 60, 90, and 120 min) were investigated using spectrophotometer.
2.2.5. Adsorption and Kinetic Isotherm Experiments
In order to evaluate the surface properties and nanoparticles adsorption capacity, the experimental data were applied to the Langmuir equation. Isotherm experiments were performed with different initial nitrate concentration solution (10–500 mg/L), and the contact time of 1 hour, pH values of , and temperature of 25°C were chosen as the experimental conditions to determine the adsorption isotherm of nitrate ions. For kinetic studies similar reaction conditions were used and reaction time was extended, till 2.5 hours, and samples were taken from time to time for final nitrate concentration analysis.
3. Results and Discussion
3.1. Characterization of Fe/Pt Bimetallic Nanoparticles
Characterization of Fe/Pt bimetallic nanoparticles is represented in Figure 1. The Pt is loaded at the surface of Fe nanoparticles, giving it a kind of bimetallic alloy nature. SEM images confirmed the presence of uniform spheroid, macroporous, sponge-like structure of high roughness and complexity. Such structure indicated the high surface area (627 m2/g) which has been proven to be efficient for photocatalytic degradation purposes. XRF analysis confirmed that nanoparticles were composed of Fe and Pt metals in equimolar ratio. All of the samples show the superlattice reflections (001) and (110) as well as some splitting of the (200)/(002) peak which signifies a tetragonality, as shown in Figure 1. EDS pattern revealed that the Fe/Pt nanoparticles were composed of almost 50% of each metal. X-ray diffraction was used to investigate the crystal phase composition bimetallic nanoparticles. XRD patterns showed that the nanoparticles contained pure anatase phase with the average crystallite sizes of 19 to 42 nm.
3.2. Experiment Conditions Optimization
3.2.1. Effect of Adsorbent Dose
To study the removal efficiencies of adsorbent doses, 200 mg/L of the initial nitrate solution was used. Dosages for both anion exchange resin and Fe/Pt bimetallic nanoparticles were varied among 100 mg/L to 1000 mg/L, at pH 7 within the contact time of 60 min for both adsorbents. It is clear from Figure 2 that removal is directly proportional to the absorbent dose till 500 mg/L. Doses higher than 500 mg/L for resins and 250 mg/L for nanoparticles did not show significant NO3, so it would not be economical. The higher removal of nitrate was because of greater surface area of Fe/Pt nanoparticles requiring smaller dose as compared to anionic exchange resins.
3.2.2. Effect of pH
The effect of pH on nitrate removal using Fe/Pt bimetallic nanoparticles and anionic exchange resins was studied at three different pH values (4, 7, and 10) with the optimized dosage (0.50 mg/L resins, 0.25 mg/L nanoparticles) against 200 mg/L nitrate solution, within the contact time of one hour. Nitrate removal by Fe/Pt bimetallic nanoparticles and anionic exchange resins as a function of pH is shown in Figure 3. Results showed that, for anionic resin, nitrate was removed at all pH levels to a varying degree, at a contact time of 60 minutes. A maximum of 82.5% removal was achieved, using resin at 4 pH. Nitrate reduction efficiency by resins decreased notably with raising pH of the solution. The removal efficiency of nanoparticles, after contact time of 60 min and pH value of 4–10, varied between 92 and 83%. Rate of nitrate removal at pH 7 was distinctively higher than for pH 4 or 10.
3.2.3. Effect of Contact Time
Effect of adsorption of nitrate on Fe/Pt nanoparticles and anionic exchange resins as a function of contact time of absorbents is shown in Figure 4. A pH 7 was maintained for nanoparticles and pH 4 for anionic exchange resins. Optimized dose of each adsorbent was used for initial 200 mg/L nitrate solution. As reflected from the results, with increasing reaction time, the nitrate removal efficiency increased, for both adsorbents.
The distinct slopes in Fe/Pt nanoparticles curve showed that overall adsorption characteristics of nanoparticles changed with contact time over 45 min and continuously yielding slope reflected that extension in contact time would not have any dramatic effect on NO3 removal. The ion exchange resin however smoothly exhausted at about 70 min. This also confirmed that minimum contact time of 60 minutes used in this experiment would be logical. For the contact time of 60 min, nitrate removal efficiency was 91% vis-à-vis 83% under all other optimized conditions and the same contact time.
3.2.4. Effect of Temperature
The effect of temperature on nitrate was studied using optimized dosage, pH, and contact time, against 200 mg/L nitrate solution at three different temperatures, that is, 15, 25, and 35°C. Figure 5 shows the results. The effect of temperature on nitrate removal via anionic exchange resins indicated that nitrate removal increased, by increasing temperature. For Fe/Pt nanoparticles, during contact time of 60 min and at temperature 25°C, about 87–90% of nitrate was removed. For resin rise in temperature up to 35°C helps improving NO3 removal. For Fe/Pt bimetallic nanoparticles, rise in temperature lowers NO3 removal efficiency.
3.2.5. Effect of Initial Nitrate Concentration
In the batch experimentation using anionic resin, the adsorption efficiency of resins under all other optimized conditions decreased from 83% to 48%, when the initial nitrate concentration increased from 10 to 400 mg/L as shown in Figure 6. For similar changes in initial concentration of nitrate, with Fe/Pt nanoparticles and nitrate adsorption efficiency gradually reduced from 98% to 51%.
It seems to be an ion exchange resin support ion exchange phenomenon, till the concentration rises beyond its exchange capacity. There is however a smooth reduction in Fe/Pt nanoparticle effectiveness with increase in initial concentration of NO3.
3.3. Adsorption and Kinetic Isotherms
3.3.1. Langmuir Isotherm
Capacity of the adsorbent can be estimated by adsorption studies. In order to evaluate the surface properties and resins adsorbent or exchange capacity the experimental data of varying initial nitrate concentrations was applied to the Langmuir equations. The linear Langmuir adsorption isotherms of nitrate ions are illustrated in Figure 7. The Langmuir parameters, and , are calculated from the slope and intercept of the graphs and are given in Table 1. The linear fitting of models was examined by calculation of correlation factors (). The correlation values are also given in Table 1. These values for Langmuir constants are higher in case of Fe/Pt bimetallic nanoparticles indicating that Langmuir isotherm better fits adsorption data of nanoparticles, compared to the resin. Data clearly suggests that the adsorption of nitrates ions is monolayer-type in both cases; moreover, it agrees with the observation that the adsorption from an aqueous solution usually forms a layer on the adsorbent surface. The higher values of Langmuir constant shows the enhanced affinity of binding sites and suggests that a chemical interaction between adsorbent and adsorbate occurs much better in case of nanoparticles. The values (see Table 1) are all found to be within 0 and 1 indicating a highly favorable adsorption of nitrate ions onto ion exchange resins.
The Langmuir model assumes that adsorption occurs in monolayer or that adsorption may only occur at fixed number of localized sites on the surface with all adsorption sites identical and energetically equivalent.
3.3.2. Kinetic Isotherms
Adsorption kinetics determines the efficiency of adsorption; therefore, pseudosecond-order kinetic model was applied on the adsorption data. The correlation coefficients values indicate that the experimental data fits the kinetic model as shown in Figure 8.
Results explicitly explain that nitrate adsorption on nanoparticles and resins is a function of time and pH 4. For a 200 ppm initial nitrate concentration and reins dose of 0.5 mg/L, 12% of the total nitrate was removed after the first 5 min; this value promptly increased to about 53% after 20 min. After 120 min, the maximum removal was 97%. Nitrate adsorption on bimetallic nanoparticles is also a function of contact time and dose at pH 7 as removal efficiency increased with the increase of contact time. For a 200 ppm initial nitrate concentration and bimetallic nanoparticles dose of 0.25 mg/L, after the first 5 min, 15.5% of the total nitrate was removed and removal percentage drastically increased to about 68% after 20 min. After 120 min the maximum removal was 83.5%. Parameters for kinetic isotherm for both adsorbents are represented in Table 2, and all values are higher in case of nanoparticles, compared to resins. It is clear from the results that adsorption using nanoparticles gives much better removal efficiency.
The overall results indicate that Fe/Pt nanoparticles having a large surface area (627 m2/g) are potentially more efficient than the commercially used anionic resins for nitrate removal from water. Literature review demonstrates that, in bimetallic system, Fe is considered reductant for water to generate hydrogen, and the second metal, that is, Pt, which has a high ability to dissociate H2 acts as catalyst . For hydrochlorination of halogenated compounds, the coating of secondary metal not only enhances the reactivity but also lowered the accumulation of toxic byproducts. Presence of Pt dramatically increased the reactivity of Fe nanoparticles for nitrate reduction.
During the catalytic reduction process of nitrate, nitrite was tested as intermediate product with the trend of first rising and then decreasing; no nitrite existed in solution at the end of reaction. This indicates that nitrate reduction with Fe/Pt nanoparticles undergoes two steps: firstly, nitrate is adsorbed to nanoparticles surface and afterward is reduced to nitrite; as a result of strong affinity of particles surface to nitrite, only a little nitrite was detected in the solution during the reaction. Finally adsorbed nitrite reduced to ammonium followed by desorption of ammonium due to the weak affinity between Fe/Pt bimetallic particles surface and ammonium .
Adsorption of nitrate was determined to be a pseudofirst-order reaction, with rates influenced by the initial concentration of the nitrate; furthermore, adsorption rate using nanoparticles were maximum at 7 pH and 25°C with an optimized nanoparticles dose of 0.25 mg/L. While adsorption results generated for both adsorbents fitted well the Langmuir isotherm, all Langmuir constants showed higher values in case of nanoparticles. Using optimized adsorption conditions resins showed maximum 83% removal; however, nanoparticles gave 97% nitrate removal for an initial nitrate solution of 200 mg/L in water. Experiments are currently underway (at IESE, NUST) in attempt to test and to study adsorption and photocatalytic effect of Pt/Fe bimetallic nanoparticles on other ions present in waste water, through rapid small scale filter column tests.
Conflict of Interests
The authors declare that there is no conflict of interests regarding the publication of this paper.
The authors gratefully acknowledge financial support from the National University of Science and Technology, Islamabad, Pakistan.
- A. Liu, J. Ming, and R. O. Ankumah, “Nitrate contamination in private wells in rural Alabama, United States,” Science of the Total Environment, vol. 346, no. 1–3, pp. 112–120, 2005.
- A. Nuhoglu, T. Pekdemir, E. Yildiz, B. Keskinler, and G. Akay, “Drinking water denitrification by a membrane bio-reactor,” Water Research, vol. 36, no. 5, pp. 1155–1166, 2002.
- F. Hell, J. Lahnsteiner, H. Frischherz, and G. Baumgartner, “Experience with full-scale electrodialysis for nitrate and hardness removal,” Desalination, vol. 117, no. 1–3, pp. 173–180, 1998.
- S. Samatya, N. Kabay, Ü. Yüksel, M. Arda, and M. Yüksel, “Removal of nitrate from aqueous solution by nitrate selective ion exchange resins,” Reactive and Functional Polymers, vol. 66, no. 11, pp. 1206–1214, 2006.
- S. K. Nataraj, K. M. Hosamani, and T. M. Aminabhavi, “Electrodialytic removal of nitrates and hardness from simulated mixtures using ion-exchange membranes,” Journal of Applied Polymer Science, vol. 99, no. 4, pp. 1788–1794, 2006.
- M. G. Rupert, “Decadal-scale changes of nitrate in ground water of the United States, 1988–2004,” Journal of Environmental Quality, vol. 37, no. 5, pp. S240–S248, 2008.
- D. Majumdar and N. Gupta, “Nitrate pollution of groundwater and associated human health disorders,” Indian Journal of Environmental Health, vol. 42, no. 1, pp. 28–39, 2000.
- B. C. Kross, A. D. Ayebo, and L. J. Fuortes, “Methemoglobinemia: nitrate toxicity in rural America,” American Family Physician, vol. 46, no. 1, pp. 183–188, 1992.
- L. Fewtrell, “Drinking-water nitrate, methemoglobinemia, and global burden of disease: a discussion,” Environmental Health Perspectives, vol. 14, no. 112, pp. 1371–1374, 2004.
- F. R. Greer and M. Shannon, “Infant methemoglobinemia: the role of dietary nitrate in food and water,” Pediatrics, vol. 116, no. 3, pp. 784–786, 2005.
- M. H. Ward, T. M. deKok, P. Levallois et al., “Workgroup report: drinking-water nitrate and health—recent findings and research needs,” Environmental Health Perspectives, vol. 113, no. 11, pp. 1607–1614, 2005.
- P. J. Squillace, J. C. Scott, M. J. Moran, B. T. Nolan, and D. W. Kolpin, “VOCs, pesticides, nitrate, and their mixtures in groundwater used for drinking water in the United States,” Environmental Science and Technology, vol. 36, no. 9, pp. 1923–1930, 2002.
- World Health Organization, Revisions of the WHO Guidelines for Drinking Water Quality Report on a WHO Consultation, WHO Regional Office for Europe, Medmenham, UK, 1992.
- J. M. Symons, L. C. Bradley Jr., and T. C. Cleveland, The Drinking Water Dictionary, AWWA, McGraw-Hill, New York, NY, USA, 2001.
- MWH, Water Treatment Principles and Design, John Wiley & Sons, Hoboken, NJ, USA, 2005.
- A. Kapoor and T. Viraraghavan, “Nitrate removal from drinking water review,” Journal of Environmental Engineering, vol. 123, no. 4, pp. 371–380, 1997.
- A. Darbi, T. Viraraghavan, R. Butler, and D. Corkal, “Pilot-scale evaluation of select nitrate removal technologies,” Journal of Environmental Science and Health, vol. 38, no. 9, pp. 1703–1715, 2003.
- M. I. M. Soares, “Biological denitrification of groundwater,” Water, Air, and Soil Pollution, vol. 123, no. 1–4, pp. 183–193, 2000.
- I. F. Cheng, R. Muftikian, Q. Fernando, and N. Korte, “Reduction of nitrate to ammonia by zero-valent iron,” Chemosphere, vol. 35, no. 11, pp. 2689–2695, 1997.
- G. Yang and H. Lee, “Chemical reduction of nitrate by nanosized iron: kinetics and pathways,” Water Research, vol. 39, no. 5, pp. 884–894, 2005.
- M. Kumar and S. Chakraborty, “Chemical denitrification of water by zero-valent magnesium powder,” Journal of Hazardous Materials, vol. 135, no. 1–3, pp. 112–121, 2006.
- F. He and D. Y. Zhao, “Preparation and characterization of a new class of starch-stabilized bimetallic nanoparticles for degradation of chlorinated hydrocarbons in water,” Environmental Science and Technology, vol. 39, no. 9, pp. 3314–3320, 2005.
- B. Schrick, J. L. Blough, A. D. Jones, and T. E. Mallouk, “Hydrodechlorination of trichloroethylene to hydrocarbons using bimetallic nickel-iron nanoparticles,” Chemistry of Materials, vol. 14, no. 12, pp. 5140–5147, 2002.
- F. He and D. Zhao, “Preparation and characterization of a new class of starch-stabilized bimetallic nanoparticles for degradation of chlorinated hydrocarbons in water,” Environmental Science and Technology, vol. 39, no. 9, pp. 3314–3320, 2005.
- S. Anders, M. F. Toney, T. Thomson et al., “X-ray absorption and diffraction studies of thin polymer/FePt nanoparticle assemblies,” Journal of Applied Physics, vol. 93, no. 10, p. 6299, 2003.
Copyright © 2015 Muhammad Daud et al. This is an open access article distributed under the Creative Commons Attribution License, which permits unrestricted use, distribution, and reproduction in any medium, provided the original work is properly cited.