Solid Phase Extraction of Silicate by Sorption on Modified Magnetite Nanoparticles and Spectrophotometric Determination
1Department of Chemistry, Payame Noor University, Tehran, Iran
2Department of Chemistry & Nanoscience and Nanotechnology Research Laboratory (NNRL), Payame Noor University, Sirjan, Iran
3Department of Chemistry, Payame Noor University, Kerman, Iran
A new adsorbent of alumina-coated magnetite nanoparticles (ACMNPs) modified with cetyltrimethyl ammonium bromide (CTAB) was prepared for the separation/preconcentration of trace silicate from water samples and then determined by spectrophotometry method. Silicate was determined based on the molybdenum blue method, which monitored at λmax of 830 nm. MNPs and ACMNPs characterized by SEM and VSM. Under the optimal experimental conditions, the preconcentration factor, detection limit, linear range and relative standard deviation of silicate were 70 (for 350 mL of sample solution), 0.040 µg mL−1, 0.8-7.0 µg mL−1 and 2.2 % (for 5.0 µg mL-1, n=7), respectively. The method was applied to the separation/preconcentration and determination of silicate in tap water, river water and seawater samples with satisfactory results.
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Keywords: separation/preconcentration, silicate, modified alumina-coated magnetite nanoparticles (ACMNPs), molybdenum blue method
World Journal of Analytical Chemistry, 2013 1 (4),
Received June 23, 2013; Revised August 11, 2013; Accepted August 13, 2013Copyright: © 2013 Science and Education Publishing. All Rights Reserved.
Cite this article:
- Karimi, Mohammad Ali, et al. "Solid Phase Extraction of Silicate by Sorption on Modified Magnetite Nanoparticles and Spectrophotometric Determination." World Journal of Analytical Chemistry 1.4 (2013): 49-53.
- Karimi, M. A. , Hatefi-Mehrjardi, A. , Mohammadi, S. Z. , Mohadesi, A. , Yarahmadi, J. , Kabir, A. A. , Mahmoodian, H. , & Khorasani, S. N. (2013). Solid Phase Extraction of Silicate by Sorption on Modified Magnetite Nanoparticles and Spectrophotometric Determination. World Journal of Analytical Chemistry, 1(4), 49-53.
- Karimi, Mohammad Ali, Abdolhamid Hatefi-Mehrjardi, Sayed Zia Mohammadi, Alireza Mohadesi, Javad Yarahmadi, Asghar Askarpour Kabir, Havva Mahmoodian, and Shahla Nezhad Khorasani. "Solid Phase Extraction of Silicate by Sorption on Modified Magnetite Nanoparticles and Spectrophotometric Determination." World Journal of Analytical Chemistry 1, no. 4 (2013): 49-53.
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Analytical separation techniques play a central role in analytical chemistry. Among separation/preconcentration methods, solid phase extraction (SPE) is a separation/ preconcentration technique of rapidly growing importance in spectrometric determinations of various species . At present, nano-sized materials such as SiO2, Al2O3, TiO2 and carbon nanotubes are more important in SPE due to their special property i.e. high adsorption capacity [2, 3, 4, 5]. Among most of nanomaterials investigated, adsorbents made from magnetite nanoparticles (MNPs), proved to be useful in separation/preconcentration applications such as SPE [6, 7, 8]. A distinct advantage of these nanoparticles is that MNPs can be readily isolated from sample solutions by the application of an external magnetic field. The surface modification of MNPs is a challenged key for SPE application. The main advantage of the preparation of alumina-coated magnetite nanoparticles (ACMNPs) in comparison with MNPs is higher stability in acidic and basic solutions. Recently, we also reported the methods for separation and preconcentration of Pb(II), Ag(I), Pd(II), Rh(III) and Ni(II) using ACMNPs [9, 10, 11, 12].
It is well known that silicon is major component of various soils and natural minerals. Silicate has been used in different industries and important environmental contaminant. An increase in concentration of silicate ions in natural water lowers the dissolved oxygen concentration and cause the death of aquatic animals such as fishes due to the suffocation . Therefore, removal of the excessive silicate ions is important to improve the water quality. There are a relatively limited number of studies dealing with the separation/preconcentration of silicate ions in real samples such as water [14, 15, 16, 17]. To our knowledge, this is the ﬁrst report of using ACMNPs for the SPE and determination of silicate ions from real samples. In this study, ACMNPs were successfully synthesized and modified by a cationic surfactant i.e. cetyltrimethylammonium bromide (CTAB). The CTAB@ACMNPs sorbent has proved to be suitable for the extraction of silicate ions from different water samples prior to determination by spectrophotometric technique based on molybdenum blue method.
2. Experimental2.1. Chemicals and Solutions
All reagents and standards were of analytical grade, and all dilutions were performed using triply distilled water. The stock standard solutions (1000 µg mL-1) of silicate were obtained by dissolving appropriate amounts of Na2SiO3.9H2O (Merck) in triple distilled water. Working standard solutions were prepared by appropriate dilution of the stock standard solution. Cethyltrimethyl ammonium bromide (CTAB), ferrous chloride (FeCl2.4H2O), ferric chloride (FeCl3.6H2O), aluminum isopropoxide, hydrochloric acid and ammonia were used without further purification processes. Stock solution of molybdate was prepared by dissolution of ammonium molybdate and potassium antimonyl tartarate in 60 mL of 9 mol L1 sulfuric acid and diluted by triple distilled water to a final volume of 100 mL in a volumetric flask and it was stable for one month. The pH adjustments of 410 were made by using buffer solutions of CH3COONa/CH3COOH, CH3COONH4/CH3COOH and NH3/NH4Cl.2.2. Apparatus
Magnetic properties of the particles were determined by vibrating sample magnetometer (VSM 7400 Model Lake-Shore). The surface morphology of the powders was observed by the scanning electron microscope (LEO 1455VP SEM). A GBC UV-Visible Cintra 6 Spectrophotometer model, attached to a Pentium (IV) computer, with 10-mm glass cells was used to measure the absorbance of silicate ion solution at 830 nm. For magnetic separations, a strong neodymium-iron-boron (Nd2Fe12B) magnet (1.2 T, 2.5 cm × 5 cm × 10 cm) was used.2.3. Preparation of ACMNPs Modified with CTAB
First, ACMNPs were synthesized by chemical coprecipitation procedure [9, 10, 11, 12]. Then, the obtained ACMNPs (100 mg) coated with admicelles of CTAB (40 mg). The pH of this suspension was adjusted to 7.5 by addition of 5 mL of CH3COONH4/CH3COOH buffer (0.1 mol L-1) solution. The mixed solution was shaken for 5 min and then CTAB@ACMNPs separated from the reaction medium under the magnetic field, and rinsed with 10 mL pure water. This product was used as sorbent for SiO32- ions.2.4. Extraction and Determination Procedure
The procedure for the magnetic extraction is demonstrated in Figure 1 and details are as follows: The extraction procedure was carried out in a batch process. A 5 mL SiO32- standard solution was added to CTAB@ACMNPs from above section. Subsequently the pH value adjusted to 7.5 with ammonium acetate/acetic acid buffer and the solution shaken for 2 min in a beaker to facilitate adsorption of the SiO32- ions onto the NPs. The beaker was placed on the magnet and nanoparticles were collected. After decanting the supernatant solution, the collected magnetite adsorbents washed with 5 mL of mixture solution of 0.25 mol L-1 H2SO4 and 0.15 mol L-1 HNO3 in order to desorb the adsorbed silicate ions by stirring for 3 min. Finally, SiO32- ions were determined at λmax of 830 nm using molybdenum blue method.
Samples of different waters were filtered through filter paper (Whatman, no. 4) to remove suspended particulate matters after collection and buffered to a pH of 7.5 with ammonium acetate/acetic acid buffer prior to storage in polyethylene container for use. The SPE procedure was carried out as described in general procedure.
3. Results and Discussion3.1. Characterization of ACMNPs
Magnetic nanoparticles may exhibit different magnetic properties due to their synthetic conditions . The hysteresis loops measured for the MNPs and ACMNPs are shown in Figure 2. Typical characteristics of superparamagnetic behavior can be observed. The saturation magnetization values from the magnetization curves in Figure 2a and Figure 2b for the uncoated MNPs and ACMNPs were found to be 56.8 and 9.4 emu g−1, respectively. The decrease of saturated magnetization was attributed to the formation of the alumina layer. However, the sorbent magnetization of ACMNPs is sufficient for magnetic separation with a normal magnet. SEM images conducted to characterize the surface of the MNPs and ACMNPs are shown in Figure 3. These images confirm highly porous morphology of adsorbent with uniform size distribution of the NPs.
In order to choose the optimum amount of ACMNPs required for quantitative recoveries of 50 mL solution containing 10.0 μg SiO32- ions, different quantities of pretreated ACMNPs ranging from 20 to 150 mg were examined. The recovery percentage was increased up to 80 mg. After this, the recovery remained constant. Therefore, 100 mg of ACMNPs was used in all subsequent experiments.
Recently, we have been reported the method for separation and preconcentration of palladium and rhodium using magnetite nanoparticles . This method is based on the solid-phase extraction (SPE) of trace amounts of Pd(II) and Rh(III) using MNPs without addition of a chelating agent and modification of NPs. In this paper, we investigate the application of CTAB immobilized on ACMNPs (CTAB@ACMNPs) for the separation/ preconcentration of SiO32- ions. Positively charged CTAB surfactant, can be strongly adsorb on negatively charged surfaces of ACMNPs in basic solutions (Figure 4). Influence of various amounts of 10, 20, 30, 40, 45, 50, 60 and 80 mg CTAB (below its critical micellar concentration, 1 × 10−3 mol L−1) on the adsorption of SiO32- ions through the ACMNPs substrate was investigated. The results showed that maximum adsorption was obtained when 40 mg of CTAB per 100 mg of ACMNPs used for SiO32- ions. Thus, this amount was selected as the optimum concentration of CTAB for further studies.3.3. Effect of pH
The pH value plays a key role in the SPE procedure. In order to investigate the effect of pH on the SPE of SiO32- ions, the pH of aqueous samples was varied from 4 to 10 using buffer solutions of CH3COONa/CH3COOH, CH3COONH4/CH3COOH and NH3/NH4Cl. Negatively charged ACMNPs surfaces effectively adsorb positively charged CTAB at upper pH values. Therefore, retention of SiO32- ions on CTAB@ACMNPs occurs. It was found that the maximum removal of SiO32- ions on the CTAB@ACMNPs as adsorbent observed at pH range of 7.0 to 8.0 (Figure 5). At the pH values higher than 8.0 and lower than 7.0, the recovery decreased, due to competition of OH- ions with SiO32- ions and the formation of negative charges of ACMNPs surfaces (reduction of CTAB adsorption), respectively. Therefore, the pH 7.5 ± 0.5 was selected for the all subsequent works. The pH 7.5 was made by adding an appropriate amount of dilute CH3COOH to CH3COONH4 solution.
In order to realize complete extraction, the effect of standing time on the adsorption and desorption was investigated. Experimental results showed that 5 min is sufficient for achieving satisfactory adsorption and 1 min for desorption. Meanwhile, in the experiment, CTAB@ACMNPs possessed superparamagnetic properties and large saturation magnetization, which enabled them to be completely isolated in a short amount of time (less than 1 min) by a strong magnet. In a word, analysis time is shortened greatly compared with the traditional column-passing SPE.
Various desorbing eluents were used to find the best desorbing solution for the adsorbed SiO32- ions. Among different solutions (such as HNO3, H2SO4, HCl, ethanol and acetonitrile) a mixed solution 0.25 mol L-1 H2SO4 and 0.15 mol L-1 were used as eluent, HNO3 provided higher recovery. In addition, the effect of elution volume for quantitative elution of the studied SiO32- ions was investigated. The minimum volume of a mixed solution of 0.25 mol L-1 H2SO4 and 0.15 mol L-1 HNO3 required for a quantitative elution of the retained analytes was found 5.0 mL.3.5. Study of Sample Volume Effect, Adsorption Capacity and Sorbent Regeneration
In order to obtain higher preconcentration factors, a larger volume of sample solution is required. The effect of sample solution volume on the extraction of SiO32- ions was studied by using different volumes (50–450 mL) of aqueous solution spiked with a fixed 5 μg SiO32- ions in the optimal conditions. Quantitative recoveries of studied SiO32- ions (>95%) were obtained when sample volume was less than 350 mL. Hence, sample volume of 350 mL was selected for subsequent experiments. Therefore, a preconcentration factor of 70 could be achieved by this method.
The capacity of the adsorbent is an important factor because it determines how much adsorbent is required to remove a specific amount of SiO32- ions from the solutions, quantitatively. In order to determinate the adsorption capacity, 100 mg of CTAB@ACMNPs and 50 mL of solution containing 5.0 mg of SiO32- ions at pH 7.5 was equilibrated for 30 min. In order to reach the “saturation”, the initial SiO32- ions’ concentration was increased till the plateau value (adsorption capacity value) obtained. The maximum adsorption capacity of CTAB@ACMNPs has been found to be 8.6 mg g−1 for SiO32- ions.
Regeneration is one of the key factors for evaluating the performance of the adsorption material. In this work, it was found that the ACMNPs can be re-used up to three times without loss of analytical performance.3.6. Interference Study
The effects of interferences from coexisting ions on the preconcentration /separation and determination of SiO32- ions were examined under the optimum conditions described above. The solutions containing 0.05 μg mL−1 SiO32- ions and other ions were prepared and the developed procedure applied in order to determine the selectivity of the sorbent. The following excesses of ions did not interfere (i.e., caused a relative error of less than 5%): less than a 1000-fold (largest amount tested) amount of Na+, K+, Ag+, NO3¯, F¯, Cl¯, Br¯; a 500-fold amount of NH4+, Ba2+, Co2+, Zn2+, Co2+; a 200-fold amount of Ni2+, Zn2+, Cu2+, Fe2+, Mn2+, Cd2+, Fe3+, Al3+; a 50-fold amount of Ca2+, Mg2+, Pb2+, Hg2+; and a 1fold amount of AsO43- and PO43-. The results showed that most of the investigated ions do not interfere in the adsorption–desorption and determination of traces of SiO32- ions in real samples. Only AsO43- and PO43- ions appeared to interfere with SiO32- ions for molybdenum blue method, that these interferences can be eliminated by reduction with thiosulfate in an acidic medium and masking by La3+ or Ca2+, respectively [19, 20].3.7. Analytical Performance
The calibration curve for the preconcentration of silicate by the optimized method was found to be linear over the concentration range of 0.8-7.0 µg mL−1. The regression equation was A=0.0369Csilicate+0.1744 (n =7), where A is the absorbance and Csilicate is the concentration of SiO32- ions in µg mL−1. Detection limit (DL) for the target SiO32- ions based on 3Sb/m definition (where m is the slope of the calibration curve and Sb is the standard deviation for seven blank measurements) was found 0.040 µg mL−1. The relative standard deviation (RSD) of 7 replicates was found to be less than ±2.5% at 5.0 µg mL-1of SiO32- ions.3.8. Application of the Method
To test the applicability of the optimized method to real water samples, it was applied to the determination of SiO32- ions in different water samples. The analytical results are shown in Table 1. The accuracy of the method was verified by the analysis of the samples spiked with known amounts of the silicate analyte. As could be seen, recoveries for the target analyte ranged from 94 to 108 %. The results show that the proposed method could be successfully applied to the determination of silicate ions.
In this study, the synthesized ACMNPs were successfully applied as a new sorbent in solid phase extraction for convenient, fast and efficient enrichment of trace SiO32- ions from environmental water samples. This new adsorbent was prepared easily and low costly, utilized conveniently and harmless to environment. Magnetic separation in the method shortened analysis times greatly. The results showed that the proposed method is very suitable for the rapid SPE of SiO32- ions from large volume of water samples.
The authors would like to express their appreciations to Professor Afsaneh Safavi for her valuable discussion and useful suggestions. This research was supported by the Nanoscience and Nanotechnology Research Laboratory (NNRL) of Payame Noor University of Sirjan.
|||Buszewski, B., and Szultka, M., “Past, present, future of solid phase extraction: A review”, Crit. Rev. Anal. Chem., 42, 198-213, 2012.|
|||Zhang, L., Zhai, Y., Chang, X., He, Q., Huang, X., and Hu, Z., “Determination of trace metals in natural samples by ICP-OES after preconcentration on modified silica gel and on modified silica nanoparticles”, Microchim. Acta, 165, 319-327, 2009.|
|||Liang, P., Qin, Y., Hu, B., Peng, T., and Jiang, Z., “Nanometer-size titanium dioxide microcolumn on-line preconcentration of trace metals and their determination by inductively coupled plasma atomic emission spectrometry in water”, Anal. Chim. Acta, 440, 207-213, 2001.|
|||Taghizadeh, T., Shemirani, F., Karimi, M.A., Abdi, K., and Ezoddin, M., “Modified nanoalumina sorbent for sensitive trace cobalt determination in environmental and food samples by flame atomic absorption spectrometry”, Int. J. Environ. Anal. Chem., 92, 1264-1273, 2012.|
|||Ozcan, S.G., Satiroglu, N., and Soylak, M., “Column solid phase extraction of iron (III), copper (II), manganese (II) and lead (II) ions food and water samples on multi-walled carbon nanotubes”, Food Chem. Toxicol., 48, 2401-2406, 2010.|
|In article||CrossRef PubMed|
|||Parham, H., and Rahbar, N., “Solid phase extraction–spectrophotometric determination of fluoride in water samples using magnetic iron oxide nanoparticles”, Talanta, 80, 664-669, 2009.|
|In article||CrossRef PubMed|
|||Faraji, M., Yamini, Y., Saleh, A., Rezaee, M., Ghambarian, M., aHassani, R., “A nanoparticle-based solid-phase extraction procedure followed by flow injection inductively coupled plasma-optical emission spectrometry to determine some heavy metal ions in water samples”, Anal. Chim. Acta, 659, 172-177, 2010.|
|In article||CrossRef PubMed|
|||Zhu, L., Pan, D., Ding, L., Tang, F., Zhang, Q., Liu, Q., and Yao, S., “Mixed hemimicelles SPE based on CTAB-coated Fe3O4/SiO2 NPs for the determination of herbal bioactive constituents from biological samples”, Talanta, 80,1873-1880, 2010.|
|In article||CrossRef PubMed|
|||Karimi, M.A., Hatefi-Mehrjardi, A., Mohammadi, S.Z., Hormozi Nezhad, M.R., Askarpour Kabir, A., Mazloum-Ardakani, M., and Mohadesi, A., “Solid phase extraction of lead(II) trace amounts in opium, heroin, lipstick, plants and water samples using modified magnetite nanoparticles prior to atomic absorption spectrometric determination”, J. Iran. Chem. Soc., 9, 171-180, 2012.|
|||Karimi, M.A., Hatefi-Mehrjardi, A. Mohammadi, S.Z., Mohadesi, A., Mazloum-Ardakani, M., Askarpour Kabir, A., Kazemipour, M., and Afsahi, N., “Solid phase extraction of trace amounts of silver(I) using dithizone-immobilized alumina-coated magnetite nanoparticles prior to determination by flame atomic absorption spectrometry”, Int. J. Environ. Anal. Chem., 92, 1325-1340, 2012.|
|||Mohammadi, S.Z., Karimi, M.A., Hamidian, H., Baghelani, Y.M., and Karimizadeh, L., “Determination of trace amounts of Pd(II) and Rh(III) ions in Pt–Ir alloy and road dust samples by flame atomic absorption spectrometry after simultaneous separation and preconcentration on non-modified magnetic nanoparticles”, Scientia Iranica,,18, 1636-1642, 2011.|
|||Karimi, M.A., and Kafi, M., “Removal, preconcentration and determination of Ni(II) from different environmental samples using modified magnetite nanoparticles prior to flame atomic absorption spectrometry,” Arabian J. Chem., In Press.|
|||Randall, C.W., Barnard, L.J., and Stensel, H.D., “Design and retrofit of wastewater treatment plants for biological neutrient removal,” Technomic Publishing, USA, 1992.|
|||Bazzi, A., and Boltz, D.F., “The preconcentration, separation and spectrophotometric determination of trace silicate,” Microchim. J., 20, 462-467, 1975.|
|||Zaporozhets, O.A., Bas, J.P., Kachan, I.A., Zinko, L.S., and Daadov, V.I., “Solid-phase spectrophotometric and test determination of silicate in natural water,” Talanta, 90, 85-90, 2012.|
|In article||CrossRef PubMed|
|||Yokoyama, Y., Danno, T., Haginoya, M., Yaso, Y., and Sato, H., “Simultaneous determination of silicate and phosphate in environmental waters using pre-column derivatization ion-pair liquid chromatography,” Talanta, 79, 308-313, 2009.|
|In article||CrossRef PubMed|
|||Nakatani, N., Kozaki, D., Masuda, W., Nakagoshi, N., Hasebe, K., Mori, M., and Tanaka, K., “Simultaneous spectrophotometric determination of phosphate and silicate ions in river water by using ion-exchange chromatographic separation and post-column derivatization,” Anal. Chim. Acta, 619, 110-114, 2008.|
|In article||CrossRef PubMed|
|||Gupta, A.K., and Gupta,M., “Synthesis and surface engineering of iron oxide nanoparticles for biomedical applications,” Biomaterials, 26, 3995-4021, 2005.|
|In article||CrossRef PubMed|
|||Goulden, P.D., and Brooksbank, P., “Automated phosphate analysis in the presence of arsenic,” Limnol. Oceanogr., 19, 705-707, 1974.|
|||Galhardo, C.X., and Masini, J.C., “Spectrophotometric determination of phosphate silicate by sequential injection using molybdenum blue chemistry,” Anal. Chim. Acta, 417, 191-200, 2000.|