Printer Friendly

Adsorptive Removal of Iron Using Si[O.sub.2] Nanoparticles Extracted from Rice Husk Ash.

1. Introduction

In the past few decades, absorptive materials have been developed for removal of heavy metal ions including [Hg.sup.2+], [Cu.sup.2+], [Pb.sup.2+], [Zn.sup.2+], [Cd.sup.2+], and [Fe.sup.2+] from the environmental and biological system due to their toxicity [1-5]. Among all of the heavy metals mentioned, [Fe.sup.2+] ions widely existed in underground water and they are commonly used for household activity in the South of Viet Nam. Long-term drinking water containing high level of [Fe.sup.2+] ions may cause kidney disease, cancer, and anemia along with metabolism disorders [6-12]. Until now, a great deal of effort has been developed for [Fe.sup.2+] ion collection using various techniques, for instance, membrane technology, chemical precipitation coagulation, ion exchange, and electrolytic reduction [13-21]. However, it was known that these methods have several drawbacks such as long time for operation, low capacity for removal, and low thermal and mechanical stability [17, 19, 21]. Among these methods, the adsorption-based technique is a promising technique for removal of [Fe.sup.2+] ions due to its high efficiency, easy operation, cost-effectiveness, and environmental-friendly method. Therefore, several adsorptive materials for removal of [Fe.sup.2+] ions have been widely investigated such as rice husk, activated carbon, fly ash, zeolites, and agricultural by-products [22-27]. It is worth to mention that silica dioxide (Si[O.sub.2]) is a promising adsorptive material due to peculiar properties such as porous structure and large surface area. In addition, there are several methods to prepare silica nanoparticles (SNPs) from different agents such as synthesis of nanosilica via the precipitation method with the SNP size of around 50 nm [28, 29] and synthesis of SNPs based on the sol-gel method using rice husk with SNP size of 15 to 90 nm [30-33]. In Viet Nam, the average rice husk produced was around 42 billion tons per year. After burning at high temperature, it became rice husk ash (RHA), which contained a very high amount of silica (approximately 90%). Note that the presence of silica in rice husk had been known since 1938 [34].

In this work, we presented the SNPs efficiency in [Fe.sup.2+] ion adsorption, with SNPs extracted from RHA in brick-kiln industry. We used the sol-gel method for extraction of SNPs under certain controlled conditions such as acid, base, pH, and stirring speed. The physicochemical properties of SNPs were studied for applications of removal of [Fe.sup.2+] ions. The SNPs synthesized could find potential applications including environment for removal of heavy metals and biomedicine for drug delivery.

2. Materials and Methods

2.1. Agents. Rice husk ash (RHA) was taken from brick-kiln industry. Hydrochloric acid (HCl), nitric acid (HN[O.sub.3]), sulfuric acid ([H.sub.2]S[O.sub.4]), sodium hydroxide (NaOH), iron(II) sulfate, heptahydrate (FeS[O.sub.4]-7[H.sub.2]O), hydroxylamide ([H.sub.2]NO), and 1,10 phenanthroline ([C.sub.12][H.sub.8][N.sub.2]) were purchased from Sigma-Aldrich. All agents were diluted in distilled water (DI water).

2.2. Methods

2.2.1. Extraction of Si[O.sub.2] Nanoparticles. SNPs were extracted from RHA based on the sol-gel method. Figure 1 illustrates the procedure for extraction of Si[O.sub.2] nanoparticles. The extraction process could be briefly described: Firstly, RHA of 2 g was collected from brick-kiln industry and then washed with DI water for removal of dirt. Secondly, RHA was soaked in the sodium hydroxide solvent under stirring at the speed of 400 rpm to generate sodium silicate. The RHA-induced sodium silicate was filtered to remove the nonreactive impurities. Finally, the sodium silicate solution obtained was cooled at room temperature and added to acid under vigorous stirring in order to initiate the hydrolysis-condensation reaction at pH~7. The gel obtained was then dispersed in ethanol, washed with DI water (three times), and dried at 110[degrees]C for 2h to remove remaining surfactants. The SNPs synthesized were stored in a desiccator for further characterizations. In this work, the effect of acids, NaOH concentration, dissolved time, and temperature was studied.

2.2.2. [Fe.sup.2+] Ion Adsorption Study. The adsorption of [Fe.sup.2+] metal ions from aqueous solution was studied at room temperature. The influence of pH, adsorption time, and mass of adsorbed material was investigated. Consequently, the pH was changed from 3 to 7; adsorption time was set up from 5 to 25 min with increment of 5 min; and mass of Si[O.sub.2] varied between 0.1, 0.5, 1.0, 1.5, and 2.0 g.

For [Fe.sup.2+] ion adsorption measurement, a standard curve was plotted using the concentrations of [Fe.sup.2+] solution in the range of 0.2, 0.4, 0.6, 0.8, and 1.0 ppm. The standard [Fe.sup.2+] solution was generated by mixing FeS[O.sub.4] x 7[H.sub.2]O with 1 ml hydroxylamine hydrochloride, 5 ml phenanthroline, and acetate buffer solution (pH = 3.5). The standard solution generated was kept for 15 min and measured by using a UV-V is spectrum analyzer. The adsorption capacity ([C.sub.cap]) and the adsorption efficiency ([E.sub.eff] were estimated using the following equation, respectively:

[C.sub.cap] = [[C.sub.in] - [C.sub.fin] / m] V, [E.sub.eff] = [[C.sub.in] - [C.sub.fin] / [C.sub.in]] x 100%, (1)

where [C.sub.in] and [C.sub.fin] are the initial concentration and concentration of equilibrium of [Fe.sup.2+] ions in solution, respectively, m is the mass of the adsorbent used, and V is the volume of solution.

2.2.3. Physicochemical and Morphological Characterization. Five analytical techniques were used for physicochemical characterization of Si[O.sub.2] extracted and adsorption of [Fe.sup.2+] ions: energy dispersive X-ray spectroscopy (EDS) for the elemental composition of Si[O.sub.2] extracted, transmission electron microscopy (TEM) for ultrastructural analysis; Fourier transform infrared spectroscopy (FT-IR) for characterization of functional groups in the range 4000-500 [cm.sup.-1], ultraviolet-visible spectroscopy (UV-Vis) for determination concentration of solution, surface area measurement by the BET method, and pore size distribution by BJH (Micrometrics ASAP 2010).

3. Results and Discussion

In this work, we used 2 g of RHA for synthesis of nanosilica particles. To optimize the conditions for nanosilica synthesis, the effect of dissolved temperature, concentration of sodium hydroxide, concentration of acids, and dissolved time was investigated. The stirring speed of 400 rpm was kept during all the process. Note that each square point in Figures 2 and 3 represents the average value of the three repeated experimental results.

3.1. Effect of Acids. The efficiency of Si[O.sub.2] extracted using different acids for neutralization is presented in Figure 2(a). We used three different acids including sulfuric acid, nitric acid, and hydrochloric acid with the same concentration of 3 M for precipitation. The results obtained showed that the extracted efficiency was 58%, 75%, and 76%, respectively. It should be noted that no significant difference was observed using HCl and HN[O.sup.3] for precipitation. The results were better than those of [H.sub.2]S[O.sub.4], caused by slow gelation process of silica when sodium silicate reacted with [H.sub.2]S[O.sub.4]. Thus, HCl was chosen for further study. Herein, concentration of NaOH, temperature, stirring speed, and dissolved time was 3.5 M, 70[degrees]C, 400 rpm, and 120 min, respectively. Then, the effect of concentration of HCl was studied in the range from 1 to 5 M. The results showed the highest efficiency of 82%, due to increase in concentration of acids. In addition, the efficiency also depended on the amount of silicate in RHA. So, the optimizing concentration of HCl used was 4 M.

3.2. Effect of NaOH. In order to optimize the condition for nanosilica synthesis, an effect of NaOH concentration was investigated. The experiments were performed with NaOH concentration series of 2.0, 2.5, 3.0, 3.5, and 4M; the dissolved time, concentration of HCl, temperature, and stirring speed were fixed at 120 min, 4 M, 70[degrees]C, and 400 rpm, respectively. The results showed that the concentration of NaOH was directly proportional to the efficiency. And, the efficiency of silica synthesized was obtained around 81% at NaOH concentration of 3.5 M as seen in Figure 2(b). This led us believe that the efficiency can be enhanced by controlling the other factors.

3.3. Effect of Dissolved Time. Based on the above results, the concentration of NaOH chosen was 3.5 M for further investigating dissolved time. Dissolved time of RHA in NaOH solution was set as a series of 60, 90, 120, 150, and 180 min. Figure 2(c) shows that the amount of Si[O.sub.2] extracted was gradually increased. Efficiency increased from 70, 82, and 83% for the first, second, and third hours, respectively. The results showed that the amount of Si[O.sub.2] extracted was saturated at 120 min. This was because of the restricted amount of silicate on RHA under burning conditions in brick-kiln industry.

3.4. Effect of Temperature. The influence of temperature on the extraction of Si[O.sub.2] from RHA was illustrated in Figure 2(d). This study had been performed using the temperature range from 60[degrees]C to 100[degrees]C with an interval increment of 10[degrees]C. The amount of Si[O.sub.2] extracted had increased with temperature and presented a maximum around 90[degrees]C and remained until 100[degrees]C. The maximum of extraction mass of Si[O.sub.2] was 1.66 g Si[O.sub.2] in this experiment, corresponding to 83% of efficiency. The efficiency was not higher than that of the other work, due to impurity of RHA in brick-kiln industry under variant conditions in comparison with RHA produced at laboratory with standard conditions [35].

The FT-IR spectrum showed strong adsorption bands at 1069 and 794 [cm.sup.-1] that corresponded to the symmetric and asymmetric Si-O-Si vibration as seen in Figure 4(a), respectively. After extraction of Si[O.sub.2], it was clear that the spectrum differs from the RHA, showing a deeper signal between 1069 and 794 [cm.sup.-1] due to increase in amount of Si[O.sub.2] extracted. In addition, an adsorption peak at 3450 [cm.sup.-1] was associated with the O-H bonds of the silanol groups. Moreover, the main elements consisted of Si, O, and Na with weight concentrations of 23, 75, and 2%, respectively. The small remaining Na was due to unperfect washing. The surface analysis of TEM showed that Si[O.sub.2] had a spherical shape with the diameter of around 50 nm. In addition, BET and BJH analyses of Si[O.sub.2] showed the specific surface area of 78 [m.sup.2]/g with a pore size of 2.7 nm. This led us to believe that the extracted Si[O.sub.2] could be used for removal of heavy metal applications.

The adsorption of [Fe.sup.2+] ions by the synthesized Si[O.sub.2] was analyzed. Figure 3(b) shows the relation of the loading capacity (mg-[g.sup.-1]) and adsorption efficiency as a function of pH. At pH < 4, Figure 3(b) presents a low adsorption capacity due to competition between [H.sup.+] ions and [Fe.sup.2+] ions. For pH > 4, concentration of [H.sup.+] decreased, offering the adsorption of [Fe.sup.2+] ions. The adsorption phenomena could be explained by the charge of Si[O.sub.2] dependent on the pH of the surrounding medium. When the pH of the surrounding medium increased, negative charges on the surface of Si[O.sub.2] increased, leading to enhanced electrostatic interaction capacity between Si[O.sub.2] and [Fe.sup.2+] ions as follows:

2 (-Si[O.sup.-]) + [Fe.sup.2+] [right arrow] [(-SiO).sub.2] Fe (2)

The adsorption of [Fe.sup.2+] ions on Si[O.sub.2] was found between pH 4 and 5. At pH > 5, the small change in adsorption of [Fe.sup.2+] ions resulted from the precipitation of [Fe.sup.2+] and small volume of the pore on Si[O.sub.2] surface. Furthermore, the removal of [Fe.sup.2+] ions was also associated with contact time as seen in Figure 3(c). Results showed that the maximum adsorption efficiency occurred within 20 min with 0.5 g loading mass of Si[O.sub.2] and the maximum adsorption capacity was around 9 mg/g (efficiency of 99%). This result was better than other works using other adsorbents as depicted in Table 1 [36-38]. Note that the higher adsorption capacity would be caused by an increase in the number of active -OH sites on the SNPs surface as presented in Figure 4(a) as well as the surface area and the pore volume of the synthesized Si[O.sub.2].

We fitted the exponential shape curves of the form of q = [q.sub.o] + a/[1 + exp((b - x)/c)] to the measurement data in Figures 3(b)-3(d) to confirm the characteristic exponential shape of adsorption capacity with variable parameters including pH, time, and mass during adsorption process. Unlike the Langmuir and Freundlich isothermal model, this fitting equation could be used to estimate minimum possible adsorption capacity ([q.sub.o]) of the adsorbent. As shown in Table 2, the minimum possible adsorption capacity was 7.7, 7.8, and 0.5 mg/g for the case of time change (Figure 3(c)), mass change (Figure 3(c)), and pH change (Figure 3(b)), respectively. We saw that there was large difference in minimum possible adsorption capacity between pH with the other ones. This was due to the fact that there was competitive adsorption occurring between [Fe.sup.2+] ions and [H.sup.+] ions into SNPs at low pH as we already discussed based on equation (2). Moreover, the correlation coefficients (R2) were both higher than 0.95 indicating that the exponential adsorption data fit well into the model.

The use of the synthesized silica nanoparticles may offer several benefits for drug delivery and adsorption of heavy metals in environment, as mentioned below. Firstly, silica nanoparticles can eliminate the toxicity in comparison with the other particles linked with magnetic nanoparticles or silver nanoparticles when they are introduced into human body for treatment. Secondly, the synthesis process of silica nanoparticles can also be applied for generation of an insulating layer to control electron tunneling between particles, which may be important in charge transfer or magneto-optics. Thirdly, surface modification via functional group immobilization is being pursued with great interest since it can provide unique opportunities to engineer the interfacial of solid substrates while retaining particles' basic geometry. Moreover, the extracted Si[O.sub.2] can be conjugated with various functional groups for specific target detection such as heavy metal ions ([Pb.sup.2+], [Cu.sup.2+], and [Cr.sup.6+]) for environmental applications. Finally, the surface area of synthesized Si[O.sub.2] can be increased by using cetyltrimethyl ammonium bromide (CTAB) to enhance capability for drug delivery and heavy metal adsorption.

4. Conclusion

We presented the extraction process of SNPs from RHA under different conditions like types of acids, NaOH concentration, dissolved time, and temperature. The results showed that the extraction efficiency was around 83% with purity of 98% and surface area of 78 [m.sup.2]/g. Moreover, the [Fe.sup.2+] ion adsorption capacity of the Si[O.sub.2] extracted from RHA was studied under different conditions including pH, contact time, and adsorbent mass. We obtained a maximum loading adsorption capacity of 9 mg [Fe.sup.2+]/g Si[O.sub.2] at pH 5 with 20 min of contact time. The adsorption efficiency can be enhanced by modification of Si[O.sub.2] with functional groups. In addition, the synthesized Si[O.sub.2] with the size of around 50 nm can be used for biomedical applications such as drug delivery.

https://doi.org/10.1155/2019/6210240

Data Availability

The data used to support the findings of this study are available from the corresponding author upon request.

Conflicts of Interest

The authors declare that there are no conflicts of interest.

Acknowledgments

This research was supported by Tra Vinh University under Basic Science Research Fund No. 181/H[??].H[??]CN-[??]HTV.

References

[1] D. L. Gutnick and H. Bach, "Engineering bacterial biopolymers for the biosorption of heavy metals; new products and novel formulations," Applied Microbiology and Biotechnology, vol. 54, no. 4, pp. 451-460, 2000.

[2] G. Renard, M. Mureseanu, A. Galarneau, D. A. Lerner, and D. Brunel, "Immobilisation of a biological chelate in porous mesostructured silica for selective metal removal from wastewater and its recovery," New Journal of Chemistry, vol. 29, no. 7, pp. 912-918, 2005.

[3] M. Mureseanu, N. Cioatera, I. Trandafir, I. Georgescu, F. Fajula, and A. Galarneau, "Selective [Cu.sup.2+] adsorption and recovery from contaminated water using mesoporous hybrid silica bio-adsorbents," Microporous and Mesoporous Materials, vol. 146, no. 1-3, pp. 141-150, 2011.

[4] F. Ge, M.-M. Li, H. Ye, and B.-X. Zhao, "Effective removal of heavy metal ions [Cd.sup.2+], [Zn.sup.2+], [Pb.sup.2+], [Cu.sup.2+] from aqueous solution by polymer-modified magnetic nanoparticles," Journal of Hazardous Materials, vol. 211-212, pp. 366-372, 2012.

[5] F. Ke, L.-G. Qiu, Y.-P. Yuan et al., "Thiol-functionalization of metal-organic framework by a facile coordination-based postsynthetic strategy and enhanced removal of [Hg.sup.2+] from water," Journal of Hazardous Materials, vol. 196, pp. 36-43, 2011.

[6] B. Halliwel, "Antioxidants in human health and disease," Annual Review of Nutrition, vol. 16, no. 1, pp. 33-50, 1996.

[7] B. Halliwell and J. M. C. Gutteridge, "Oxygen toxicity, oxygen radicals, transition metals and disease," Biochemical Journal, vol. 219, no. 1, pp. 1-14, 1984.

[8] B. Halliwell, "Reactive oxygen species in living systems: source, biochemistry, and role in human disease," The American Journal of Medicine, vol. 91, no. 3, pp. S14-S22, 1991.

[9] B. Halliwell, "Free radicals and antioxidants: a personal view," Nutrition Reviews, vol. 52, no. 8, pp. 253-265, 1994.

[10] S. L. Simpson and G. E. Batley, "Disturbances to metal partitioning during toxicity testing of iron(II)-rich estuarine pore waters and whole sediments," Environmental Toxicology and Chemistry, vol. 22, no. 2, pp. 424-432, 2003.

[11] I. I. Somers and J. W. Shive, "The iron-manganese relation in plant metabolism," Plant Physiology, vol. 17, no. 4, pp. 582-602, 1942.

[12] L. H. A. Rahman, R. M. E. Khatib, L. A. E. Nasr, and A. M. Abu-Dief, "Synthesis, physicochemical studies, embryos toxicity and DNA interaction of some new Iron (II) Schiff base acid complexes," Journal of Molecular Structure, vol. 1040, pp. 9-18, 2013.

[13] V. A. Elrod, K. S. Johnson, and K. H. Coale, "Determination of subnanomolar levels of iron(II) and total dissolved iron in seawater by flow injection and analysis with chemiluminescence detection," Analytical Chemistry, vol. 63, no. 9, pp. 893-898, 1991.

[14] F. Jaouen, S. Marcotte, J. P. Dodelet, and G. Lindbergh, "Oxygen reduction catalysts for polymer electrolyte fuel cells from the pyrolysis of iron acetate adsorbed on various carbon supports," Journal of Physical Chemistry B, vol. 107, no. 6, pp. 1376-1386, 2003.

[15] S. O. Pehkonen, Y. Erel, and M. R. Hoffmann, "Simultaneous spectrophotometric measurement of iron(II) and iron(III) in atmospheric water," Environmental Science & Technology, vol. 26, no. 9, pp. 1731-1736, 1992.

[16] S. Kagaya, Y. Araki, N. Hirai, and K. Hasegawa, "Coprecipitation with yttrium phosphate as a separation technique for iron(III), lead, and bismuth from cobalt, nickel, and copper matrices," Talanta, vol. 67, no. 1, pp. 90-97, 2005.

[17] L. C. Roberts, S. J. Hug, T. Ruettimann, M. M. BIllah, A. W. Khan, and M. T. Rahman, "Arsenic removal with iron(II) and iron(III) in waters with high silicate and phosphate concentrations," Environmental Science & Technology, vol. 38, no. 1, pp. 307-315, 2004.

[18] S. P. Burke and S. A. Banwart, "A geochemical model for removal of iron(II)(aq) from mine water discharges," Applied Geochemistry, vol. 17, no. 4, pp. 431-443, 2002.

[19] G. Muniz, V. Fierro, A. Celzard, G. Furdin, G. Gonzalez-Sanchez, and M. L. Ballinas, "Synthesis, characterization and performance in arsenic removal of iron-doped activated carbons prepared by impregnation with Fe(III) and Fe(II)," Journal of Hazardous Materials, vol. 165, no. 1-3, pp. 893-902, 2009.

[20] W. Chen, R. Parette, J. Zou, F. S. Cannon, and B. A. Dempsey, "Arsenic removal by iron-modified activated carbon," Water Research, vol. 41, no. 9, pp. 1851-1858, 2007.

[21] T. L. Theis and P. C. Singer, "Complexation of iron(II) by organic matter and its effect on iron(II) oxygenation," Environmental Science & Technology, vol. 8, no. 6, pp. 569-573, 1974.

[22] S. Cetin and E. Pehlivan, "The use of fly ash as a low cost, environmentally friendly alternative to activated carbon for the removal of heavy metals from aqueous solutions," Colloids and Surfaces A: Physicochemical and Engineering Aspects, vol. 298, no. 1-2, pp. 83-87, 2007.

[23] C. Quintelas, Z. Rocha, B. Silva, B. Fonseca, H. Figueiredo, and T. Tavares, "Biosorptive performance of an Escherichia coli biofilm supported on zeolite NaY for the removal of Cr(VI), Cd(II), Fe(III) and Ni(II)," Chemical Engineering Journal, vol. 152, no. 1, pp. 110-115, 2009.

[24] F. Fu and Q. Wang, "Removal of heavy metal ions from wastewaters: a review," Journal of Environmental Management, vol. 92, no. 3, pp. 407-418, 2011.

[25] M. Hua, S. Zhang, B. Pan, W. Zhang, L. Lv, and Q. Zhang, "Heavy metal removal from water/wastewater by nanosized metal oxides: a review," Journal of Hazardous Materials, vol. 211-212, pp. 317-331, 2012.

[26] T. G. Chuah, A. Jumasiah, I. Azni, S. Katayon, and S. Y. Thomas Choong, "Rice husk as a potentially low-cost biosorbent for heavy metal and dye removal: an overview," Desalination, vol. 175, no. 3, pp. 305-316, 2005.

[27] A. B. Jusoh, W. H. Cheng, W. M. Low, A. Nora'aini, and M. J. M. M. Noor, "Study on the removal of iron and manganese in groundwater by granular activated carbon," Desalination, vol. 182, no. 1-3, pp. 347-353, 2005.

[28] N. Thuadaij and A. Nuntiya, "Synthesis and characterization of nanosilica from rice husk ash prepared by precipitation method," Nanotechnology, vol. 7, no. 1, 2008.

[29] U. Kalapathy, A. Proctor, and J. Shultz, "An improved method for production of silica from rice hull ash," Bioresource Technology, vol. 85, no. 3, pp. 285-289, 2002.

[30] Y. Qu, Y. Tian, B. Zou et al., "A novel mesoporous lignin/silica hybrid from rice husk produced by a sol-gel method," Bioresource Technology, vol. 101, no. 21, pp. 8402-8405, 2010.

[31] U. Kalapathy, A. Proctor, and J. Shultz, "A simple method for production of pure silica from rice hull ash," Bioresource Technology, vol. 73, no. 3, pp. 257-262, 2000.

[32] J. P. Nayak, S. Kumar, and J. Bera, "Sol-gel synthesis of bioglass-ceramics using rice husk ash as a source for silica and its characterization," Journal of Non-Crystalline Solids, vol. 356, no. 28-30, pp. 1447-1451, 2010.

[33] T. Witoon, M. Chareonpanich, and J. Limtrakul, "Synthesis of bimodal porous silica from rice husk ash via sol-gel process using chitosan as template," Materials Letters, vol. 62, no. 1011, pp. 1476-1479, 2008.

[34] J. I. Martin, "The desilification of rice hull and a study of the products obtained," M.S. thesis, Lousiana State University, Baton Rouge, LA, USA, 1938.

[35] D. Z. Zhao, S. B. Jing, J. N. Xu et al., "Recycle adsorption of [Cu.sup.2+] on amine-functionalized mesoporous silica monolithic," Chemical Research in Chinese Universities, vol. 29, no. 4, pp. 793-797, 2013.

[36] S. R. Shukla, R. S. Pai, and A. D. Shendarkar, "Adsorption of Ni(II), Zn(II) and Fe(II) on modified coir fibres," Separation and Purification Technology, vol. 47, no. 3, pp. 141-147, 2006.

[37] B. Acemioglu, "Removal of Fe(II) ions from aqueous solution by Calabrian pine bark wastes," Bioresource Technology, vol. 93, no. 1, pp. 99-102, 2004.

[38] W. S. W. Ngah, S. Ab Ghani, and A. Kamari, "Adsorption behaviour of Fe(II) and Fe(III) ions in aqueous solution on chitosan and cross-linked chitosan beads," Bioresource Technology, vol. 96, no. 4, pp. 443-450, 2005.

Tan Tai Nguyen [ID], (1) Hoa Thai Ma, (2) Pramod Avti [ID], (3) Mohammed J. K. Bashir [ID], (4) Choon Aun Ng, (4) Ling Yong Wong, (4) Hieng Kiat Jun, (5) Quang Minh Ngo, (6,7,8) and Ngoc Quyen Tran [ID] (9,10)

(1) Department of Materials Science, School of Applied Chemistry, Tra Vinh University, Tra Vinh City 87000, Vietnam

(2) Department of Active Polymers and Nanomaterials Applications, School of Applied Chemistry, Tra Vinh University, Tra Vinh City 87000, Vietnam

(3) Department of Biophysics, Postgraduate Institute of Medical Education and Research (PGIMER), Sector-12, Chandigarh 160012, India

(4) Faculty of Engineering and Green Technology (FEGT), Universiti Tunku Abdul Rahman, Jalan Universiti, Bandar Barat, 31900 Kampar, Perak, Malaysia

(5) Department of Mechanical and Material Engineering, Lee Kong Chian Faculty of Engineering and Science, Universiti Tunku Abdul Rahman, Sungai Long Campus, Bandar Sg. Long, 43000 Kajang, Malaysia

(6) Institute of Materials Science, Vietnam Academy of Science and Technology, 18 Hoang Quoc Viet, Cau Giay, Hanoi, Vietnam

(7) Graduate University of Science and Technology, Vietnam Academy of Science and Technology, 18 Hoang Quoc Viet, Cau Giay, Hanoi, Vietnam

(8) University of Science and Technology of Hanoi, Vietnam Academy of Science and Technology, 18 Hoang Quoc Viet, Cau Giay, Hanoi, Vietnam

(9) Graduate University of Science and Technology, Vietnam Academy of Science and Technology, HCM City 70000, Vietnam

(10) Institute of Applied Materials Science, Vietnam Academy of Science and Technology, HCM City 70000, Vietnam

Correspondence should be addressed to Tan Tai Nguyen; nttai60@tvu.edu.vn

Received 13 December 2018; Revised 18 March 2019; Accepted 15 April 2019; Published 2 June 2019

Academic Editor: Jaroon Jakmunee

Caption: Figure 1: Extraction process of Si[O.sub.2] from rice husk ash. (a) Rice husk ash from brick industry. (b) Rice husk ash diluted in sodium hydroxide after filtering. (c) Rice husk ash solution after precipitation by acid. (d) Extracted Si[O.sub.2] after drying.

Caption: Figure 2: Experimental results of Si[O.sub.2] nanoparticles extraction process. Effect of (a) acids, (b) sodium hydroxide, (c) dissolved time, and (d) temperature.

Caption: Figure 3: Experimental results of [Fe.sup.2+] adsorption capacity and [Fe.sup.2+] removal efficiency by the Si[O.sub.2] nanoparticles extracted. (a) UV-Vis calibration curve for [Fe.sup.2+] ion adsorption and effect of (b) pH, (c) contact time, and (d) Si[O.sub.2] mass.

Caption: Figure 4: Characterization of Si[O.sub.2] extracted. (a) FT-IR spectrum of the RHA and extracted Si[O.sub.2]. (b) TEM image of Si[O.sub.2] nanoparticles. (c) EDS elemental composition analysis of Si[O.sub.2] nanoparticles. (d) Si[O.sub.2] nanoparticles extracted from RHA.
Table 1: Comparison of iron adsorption capacity of Si[O.sub.2] extracted
from RHA with adsorbent materials in the references.

                                            Iron
Adsorbent                Concentration   adsorption   References
                             range        capacity
                                           (mg/g)

SiO2                       0.1-1 ppm        9.0       This study
Coir fibers modifying     73-444 mg/L       7.5          [36]
  hydrogen peroxide
Coir fibers               73-444 mg/L       2.8          [36]
Pine bark waste           55-111 mg/L       2.0          [37]
Cross-linked                3-9 ppm         64.1         [38]
  chitosan

Table 2: Kinetic coefficients in iron adsorption.

       Minimum adsorption     Fitting coefficients   [R.sup.2]
       capacity, [q.sub.0]
             (mg/g)            a       b       c

Time           7.7            0.9    12.3     1.6      0.98
Mass           7.8            1.3     1.9     0.1      0.96
pH             0.5            7.9     4.2     0.2      0.99
COPYRIGHT 2019 Hindawi Limited
No portion of this article can be reproduced without the express written permission from the copyright holder.
Copyright 2019 Gale, Cengage Learning. All rights reserved.

Article Details
Printer friendly Cite/link Email Feedback
Title Annotation:Research Article
Author:Nguyen, Tan Tai; Ma, Hoa Thai; Avti, Pramod; Bashir, Mohammed J.K.; Ng, Choon Aun; Wong, Ling Yong;
Publication:Journal of Analytical Methods in Chemistry
Geographic Code:9VIET
Date:Jun 1, 2019
Words:4631
Previous Article:Development of a Sensitive Chemiluminescence Immunoassay for the Quantification of Folic Acid in Human Serum.
Next Article:Highly Selective Fluorescent Probe for the Detection of Copper (II) and Its Application in Live Cell Imaging.
Topics:

Terms of use | Privacy policy | Copyright © 2020 Farlex, Inc. | Feedback | For webmasters