Open Access

Tunable synthesis of SiO2-encapsulated zero-valent iron nanoparticles for degradation of organic dyes

  • Zhou Mao1,
  • Qingzhi Wu1,
  • Min Wang1,
  • Yushi Yang1,
  • Jia Long1 and
  • Xiaohui Chen2Email author
Contributed equally
Nanoscale Research Letters20149:501

Received: 15 August 2014

Accepted: 9 September 2014

Published: 16 September 2014


A series of nanocomposites consisting of zero-valent iron nanoparticles (ZVI NPs) encapsulated in SiO2 microspheres were successfully synthesized through a successive two-step method, i.e., the wet chemical reduction by borohydride followed by a modified Stöber method. The as-synthesized nanocomposites were characterized using X-ray diffraction, field emission scanning electron microscopy, vibrating sample magnetometer, and inductively coupled plasma-atomic emission spectrometer. The catalytic performance of SiO2-encapsulated ZVI nanocomposites for the degradation of organic dyes was investigated using methylene blue (MB) as the model dye in the presence of H2O2. The results showed that the degradation efficiency and apparent rate constant of the degradation reaction were significantly enhanced with increased ZVI NPs encapsulated in SiO2 microspheres, whereas the dosage of H2O2 remarkably promoted degradation rate without affecting degradation efficiency. The content-dependent magnetic property ensured the excellent magnetic separation of degradation products under an external magnet. This strategy for the synthesis of SiO2-encapsulated ZVI NPs nanocomposites was low cost and easy to scale-up for industrial production, thereby enabling promising applications in environmental remediation.


Zero-valent iron nanoparticlesSiO2NanocompositesCatalytic degradationOrganic dye


Organic dyes are used in numerous industries including textile, cosmetics, food, and pharmaceutical because of their fascinating properties, such as high wet fastness profile, brilliant shades, and relatively low cost. However, the compulsive utilization of organic dyes has caused serious environmental pollution and posed public health risks [13]. Most organic dyes are resistant to decompose in a natural environment and can cause serious diseases because of their transformation into genotoxic and carcinogenic species. Existing strategies focus on the removal and degradation of organic contaminants from effluents, including adsorption, coagulation, chemical oxidation, electrochemical degradation, and biological degradation, among others [49]. The major disadvantage of these physical methods is the dye molecules that are transferred to another phase rather than destroyed [10]. Additionally, biological degradation of organic contaminants suffers from low degradation efficiency, high cost, and rigorous degradation conditions [11]. Conversely, chemical methods display promising potential in the degradation of organic contaminants, although they require various high-performance catalysts [1214]. The disposal of chemicals containing sludge at the end of degradation also entails complicated posttreatment processes and further use of chemicals [15]. Therefore, it is indispensable and emergent to explore the novel strategies for the degradation of organic contaminants with high efficiency and low cost.

Over the past decades, zero-valent iron (ZVI) nanoparticles (NPs) have been considered to possess promising potential in environmental remediation because of their low cost, high reactivity as a reducing agent, and ability to generating reactive oxygen species (ROS) through the Fenton reaction [16, 17]. In a typical Fenton reaction, Fe2+/Fe3+ reacts with H2O2 and generates the hydroxyl radical (·OH), which is a very strong oxidant capable of decomposing various organic contaminants [18, 19]. The use of ZVI powder instead of iron salts avoids the introduction of counter anions into aquatic systems. In addition, the concentration of Fe2+/Fe3+ in wastewater treated by ZVI is significantly lower than those treated with iron salts [20]. Moreover, the excess catalyst contained in the sludge could be easily recycled by magnets. However, the agglomeration of ZVI NPs is one of the most fatal shortages of this process, which results in the rapid inactivation of chemical reactivity. Therefore, modification of the surface of ZVI NPs to reduce agglomeration and prevent oxidation of ZVI NPs is necessary. Among various stabilizers, SiO2 coating has attracted considerable attention because of its low cost and environmental friendliness. Various strategies have been developed for the synthesis of Fe/SiO2 nanocomposites, including sol-gel [2126], mechanochemical billing [27, 28], spray drying [29], arc discharge [30], wet chemical route [31], and ion implantation [32]. Thus far, the low-cost and large-scale synthesis of ZVI NPs with high reactivity and mobility remains a great challenge.

In this work, a facile two-step strategy was developed to synthesize SiO2-encapsulated ZVI NPs. The ZVI NPs were first synthesized through wet chemical reduction with NaBH4 and subsequently encapsulated by SiO2 through the classical Stöber process. The content of ZVI NPs encapsulated in SiO2 was adjusted by changing the reaction parameters. The products were characterized using X-ray diffraction (XRD), field emission scanning electron microscopy (FESEM), vibrating sample magnetometer (VSM), and inductively coupled plasma-atomic emission spectrometer (ICP-AES). Moreover, the catalytic degradation of organic contaminants by SiO2-encapsulated ZVI NPs nanocomposites was evaluated using methylene blue (MB) as the model dye by monitoring the changes of UV-vis spectra at different time intervals at room temperature.



FeCl2 · 4H2O, NaBH4, tetraethoxysilane (TEOS), ethanol, and H2O2 were of analytic grade (Sinopharm Chemical Reagent Co., Ltd., Shanghai, China) and used without further purification. Deionized water (16 M Ω·cm) was obtained from a Nanopure Water Systems (Thomas Scientific, Swedesboro, NJ, USA).

Synthesis of SiO2-encapsulated ZVI nanocomposites

In a typical synthesis, FeCl2 · 4H2O (0.3976 g, 2 mmol) was dissolved in 40 mL of deionized water in a 250 mL, four-necked round-bottomed flask under magnetic stirring with nitrogen atmosphere. Subsequently, NaBH4 (0.1139 g, 3 mmol) dissolved in another 10 mL of deionized water was added to FeCl2 solution under ultrasonication (FS-250 150 W, Shanghai Sonxi Corp., China). The synthesis was carried out for 30 min. The products were collected by a magnet and then washed by deionized water. The mesoporous silica coating was performed according to the modified Stöber method [33, 34]. In brief, 4.5 mL of TEOS was added into 45.5 mL of ethanol, which was subsequently added into ZVI NPs with ultrasonically dispersing for 0.5 h. After that, the mixture containing ZVI NPs and TEOS was rapidly added into a mixed solution containing 9 mL of ammonium hydroxide, 16.25 mL of ethanol, and 24.75 mL of H2O with ultrasonically dispersing for 4 h in nitrogen atmosphere. The precipitate was collected by centrifugation (4,000 rpm, 3 min), washed alternately with deionized water and ethanol, and vacuum dried at 60°C for 4 h. In a series of syntheses, the ratio of reactants and solvents were changed. Table 1 lists the reaction parameters of the syntheses.
Table 1

The initial concentrations of iron salt used in the synthesis


Sample name

The initial concentration of Fe2+(mmol)
















Characterization of SiO2-encapsulated ZVI nanocomposites

The phase structure of the samples was characterized on a power XRD (D8 Advance, Bruker Corp., Karlsruhe, Germany) using Cu Kα radiation (λ) 1.5406 Å. The morphology of the samples was observed using field emission scanning electron microscope (FESEM; S4800, Hitachi Corp., Chiyoda-ku, Japan). The elemental composition was measured with an Optima 4300DV ICP-AES (Optima 4300DV, PerkinElmer Corp., Yokohama, Kanagawa, Japan). Magnetic property was measured on VSM (JDAW-2000D, Yingpu Corp., Hangzhou, China). Nitrogen (N2) adsorption-desorption isotherms were measured with a Micromeritics apparatus (TriStar II 3020, Micromeritics Instrument Corp., Norcross, GA, USA). UV-vis spectra were recorded on a UV-vis spectrophotometer (UV-2550 PC, Shimadzu Corp., Kyoto, Japan).

Catalytic degradation of MB by SiO2-encapsulated ZVI nanocomposites

Batch experiments were carried out to evaluate the catalytic performance of SiO2-encapsulated ZVI NPs nanocomposites using MB as the model at room temperature. In a typical experiment, the sample (20 mg) and H2O2 (1 mL) was added into 50 mL of MB (10 mg/L) aqueous solution. The suspension was continuously stirred at room temperature under visible light irradiation. The supernatant was collected at designated time intervals for UV-vis measurement after centrifugation (10,000 rpm, 3 min). The catalytic degradation of MB was evaluated by monitoring the changes of UV-vis spectra.

Results and discussion

Characterization of SiO2-encapsulated ZVI nanocomposites

Figure 1 shows XRD patterns of the as-synthesized nanocomposites containing different contents of ZVI NPs. A broad diffraction peak at ca. 23° in the XRD patterns could be indexed to amorphous SiO2[35, 36]. As shown in Figure 1e, the peaks at ca. 44.7°, 65.0°, and 82.3° could be assigned to Fe (JCPDS card no. 06-0696). These broad diffraction peaks indicated the small size of ZVI NPs. Notably, most of the diffraction peaks disappeared, except the peak at 44.7°, as shown in Figure 1a,b,c,d. This result was attributed to the content decrease of ZVI NPs in nanocomposites and the surface coating of SiO2[29]. No peak from iron oxides was observed in the XRD patterns, indicating that the ZVI NPs were well protected from oxidation because of the encapsulation by SiO2.Figure 2 shows the SEM images of the as-synthesized nanocomposites. Irregular spherical structures were observed, and the size of the samples significantly increased with increased ZVI NP content in nanocomposites. For example, the average size was ca. 203 ± 35 nm for the sample with the lowest ZVI NP content (S-0.5, Figure 2a,b) and ca. 725 ± 55 nm for the sample with the highest ZVI NP content (S-8, Figure 2i,j). Slight aggregations of particles were also observed with increased ZVI NPs in nanocomposites. The increase in size and the aggregation of the nanocomposites could be attributed to the increase in ZVI NP content and the magnetic interaction.
Figure 1

XRD patterns of the samples synthesized with different initial concentrations of Fe 2+ . (a) S-0.5, (b) S-1, (c) S-2, (d) S-4, and (e) S-8.

Figure 2

SEM images of the samples synthesized with different initial concentrations of Fe 2+ . (a) and (b) S-0.5, (c) and (d) S-1, (e) and (f) S-2, (g) and (h) S-4, and (i) and (j) S-8.

The content of Fe in the as-synthesized nanocomposites was measured by ICP analysis to identify the content of ZVI NPs in the different samples. As shown in Figure 3, the content of ZVI NPs encapsulated in SiO2 microsphere significantly increased with increased initial concentration of iron salts. However, the measured content of Fe in nanocomposites was consistent only with the theoretical calculation in the cases of S-0.5, S-1, and S-2. For example, in the case of S-2, the Fe content in the nanocomposite was ca. 8.3%, approximate to the theoretical content of ca. 8.4%. This result suggested that all ZVI NPs were successfully encapsulated in SiO2 microspheres. Meanwhile, in the cases of S-4 and S-8, the Fe content in nanocomposites was ca. 13.8% and 19.2%, relatively lower than the theoretical content of ca. 15.6% and 26.9%, respectively, suggesting that ZVI NPs were partially encapsulated in SiO2 microspheres. Therefore, these results demonstrated that the encapsulation ratio of ZVI NPs decreased with increased ZVI NP content in nanocomposites.
Figure 3

The theoretical and actual content of Fe in as-synthesized nanocomposites.

The N2 adsorption-desorption isotherms of the as-synthesized nanocomposites are shown in Figure 4. The isotherms of the products were indexed to type IV. It was noticeable that the isotherms of the products were not closed in the range of P/P0 from 0.1 to 1.0, which could be attributed to the irreversible adsorption-desorption process of N2 in these samples [37, 38]. The specific surface areas calculated from N2 adsorption isotherm according to Brunauer-Emmett-Teller (BET) method were 184.3, 87.8, 33.9, 4.0, and 3.0 m2/g, respectively, corresponding to the nanocomposites containing different contents of ZVI NPs. The decrease of BET-specific surface areas of the nanocomposites could be attributed to the size increase of the nanocomposites, as shown in Figure 2.
Figure 4

N 2 adsorption-desorption isotherms of as-synthesized nanocomposites. (a) S-0.5, (b) S-1, (c) S-2, (d) S-4, and (e) S-8.

The release of Fe2+ from the as-synthesized nanocomposites was a key factor affecting the catalytic degradation of organic contaminants. Figure 5 shows the Fe2+ concentration released from S-4 in different pH environments. In this test, 50 mg of S-4 was dispersed in 150 mL of buffer solution with different pH values (phosphate buffer solution (PBS), pH = 7.4; acetic acid buffer solution, pH = 4.5) and incubated at 25°C with constant shaking (130 rpm). The supernatant was collected by centrifugation (6,500 rpm, 5 min) and measured by ICP-AES. A burst release of Fe2+ was observed after 4 h of incubation that reached ca. 7.41 mg/mL at the end of 72 h in an acetic acid buffer solution. The released Fe2+ was approximately 16.0% of the content of ZVI NPs in the nanocomposite. These results indicated that the as-synthesized nanocomposites could be used as Fe2+ reservoir for the catalytic degradation of organic contaminants over a long period.
Figure 5

Fe 2+ release of S-4 in different pH environments. Phosphate buffer solution, pH = 7.4 and acetic acid buffer solution, pH = 4.5.

The magnetic property of the as-synthesized nanocomposites was measured by VSM at room temperature. Figure 6 shows the characteristic of magnetic hysteresis loops of the as-synthesized nanocomposites, suggesting the ferromagnetic nature of the samples. As shown in Figure 6, the magnetic properties, including saturation magnetization (M s ), coercivity, and remanence proportionally increased with increased ZVI NPs in the nanocomposites (Table 2). For example, the M s values of the as-synthesized nanocomposites were ca. 28, 56, 123, 205, and 283 emu/g, corresponding to the ZVI NPs contents of ca. 1.8%, 4.0%, 8.3%, 13.8%, and 19.2%, respectively. As such, the excess catalysts could be separated and recycled by magnets.
Figure 6

Magnetization hysteresis loops of as-synthesized nanocomposites. (a) S-0.5, (b) S-1, (c) S-2, (d) S-4, and (e) S-8.

Table 2

The saturation magnetization, remanence, and coercivity of as-synthesized nanocomposites


Sample name

M s (emu/g)

Remanence (emu/g)

Coercivity (Oe)


























Degradation assessment of MB treated with SiO2-encapsulated ZVI NPs

The degradation of MB was monitored by UV-vis spectrometry to evaluate the catalytic performance of the SiO2-encapsulated ZVI NPs nanocomposites. The changes in absorption spectra of MB solution treated with nanocomposites and H2O2 were recorded at different time intervals. The degradation efficiency (D) was evaluated using the following equation:
D = A 0 A / A 0 × 100 %

where A and A0 were the absorbance at the maximum absorption peak of ca. 664 nm of MB at different time intervals and initial time, respectively.

As shown in Figure 7, the major absorption peak of MB aqueous solution appeared at ca. 664 nm originated from MB monomer, and the shoulder peak at ca. 615 nm originated from the dimer of MB [39, 40]. For comparison, MB solution was also treated with SiO2 microspheres synthesized under the same conditions in the absence of ZVI NPs. The significant adsorption of MB molecules by SiO2 microspheres was observed after 0.5 h of treatment. The adsorption efficiencies were ca. 12.7% and 36.6% after 0.5 and 96 h of treatment, respectively. SiO2-encapsulated ZVI NPs nanocomposites displayed significant degradation of MB in the presence of H2O2. At the end of the treatment (96 h), the degradation efficiencies of MB were ca. 59.4%, 57.1%, 64.0%, 80.9%, and 99.5%, corresponding to the as-synthesized nanocomposites with different contents of ZVI NPs. These results suggested that the content of ZVI NPs encapsulated in SiO2 microspheres was directly proportional to MB degradation efficiency.
Figure 7

UV-vis spectra of MB solution treated with as-synthesized nanocomposites in the presence of H 2 O 2 . (a) S-0.5, (b) S-1, (c) S-2, (d) S-4, (e) S-8, and (f) pure SiO2 without ZVI NPs.

The influence of reaction parameters on the catalytic degradation of MB was further investigated. As shown in Figure 8a, MB solutions with different initial concentrations were treated with S-8 in the presence of H2O2. Results showed that, at the end of 96 h, the degradation efficiencies of MB were ca. 98.6%, 98.7%, and 94.2%, corresponding to the initial MB concentrations of 10, 13, and 16 mg/mL, respectively. Therefore, the SiO2 shells protected ZVI ZPs from being oxidized and prevented the adsorption of MB molecules on the surface of ZVI NPs, both of which significantly resulted in the inactivation of ZVI NP reactivity. The influence of H2O2 dosage was also studied. As shown in Figure 8b, the degradation efficiencies of the samples were ca. 53.5%, 62.1%, and 99.0% at the end of 24 h, and ca. 98.2%, 98.6%, and 99.0% at the end of 96 h, when the dosage of H2O2 was increased from 0.5 mL to 1 and 5 mL. These results suggested that increased H2O2 dosage significantly promoted degradation rate, instead of degradation efficiency.
Figure 8

Effects of reaction parameters on the degradation efficiency of MB by S-8. (a) Degradation efficiency of MB with different initial concentrations and (b) degradation efficiency of MB in the presence of H2O2 with different dosages.

To explore the mechanism of degradation, a pseudo-first-order kinetic model as expressed below was subsequently used to evaluate the degradation kinetic of MB by SiO2-encapsulated ZVI NPs [41, 42]
ln c t / c 0 = k obs t
where c0 is the initial concentration (mg/L) of MB in solution, c t is the concentration of MB at reaction time t, and kobs is the apparent kinetic rate constant of the pseudo-first-order reaction model. Figure 9 shows the linear relationship by plotting ln (c/c0) against t (h). The apparent kinetic rate constant (kobs) calculated from the slope of the regression lines were ca. 0.00793 min−1 for S-0.5, 0.00801 min−1 for S-1, 0.01001 min−1 for S-2, 0.01537 min−1 for S-4, and 0.05571 min−1 for S-8, compared with 0.00287 min−1 for SiO2 microspheres without ZVI NPs. These results indicated that the degradation reaction was enhanced with increased ZVI NP content in nanocomposites.
Figure 9

Kinetic parameters of decoloration and adsorption performance. (a) pure SiO2 without ZVI NPs, (b) S-0.5, (c) S-1, (d) S-2, (e) S-4, and (f) S-8.

In general, ZVI in the presence of H2O2 produces a Fenton-like reaction through generating numerous · OH, which can destroy various organic contaminants (such as halogenated hydrocarbons, aromatic compounds, detergents and pesticides, etc.) [1619]. In the present study, ZVI NPs were encapsulated in SiO2 nanosphere, preventing from the surface oxidation of ZVI NPs. Meanwhile, ZVI NPs acted as Fe reservoir releasing iron ions (as shown in Figure 4), which catalytically broke down the H2O2 molecules into · OH. It was suggested that · OH can attack the C-S+ = C and C-N = C group in MB molecules, resulting in the split of the S+ = C and N = C double bond [43, 44]. The further attack of · OH on S-Cl, C-NH2, and C-SO3H containing in various intermediates finally generated inorganic molecules or structures, such as H2O, CO2, Cl, NO3, and SO42−.

A large amount of sludge is usually produced in the coagulation phase after wastewater treatment by various catalysts, resulting in complicated posttreatment processes [45, 46]. Accordingly, the magnetic separation of the as-synthesized nanocomposites in treated MB solution was used to study the recycling and separation of catalyst. Figure 10 shows the magnetic separation of the as-synthesized nanocomposites containing different contents of ZVI NPs from MB solution after 96 h of treatment. No obvious change was observed when the MB solution was treated with S-0.5 and S-1 in the presence of H2O2 at the end of 96 h. This result could be attributed to low content of ZVI NPs in the nanocomposites and low degradation of MB. However, when the dye was treated with S-2, S-4, and S-8 in the presence of H2O2, obvious decoloration and magnetic separation of sludge were observed. For example, in the case of S-8, the muddy solution became nearly clear within 1 min under exposure to an external magnet (Figure 10e). These results demonstrated the excellent performance of SiO2-encapsulated ZVI NPs nanocomposites in the catalytic degradation of organic dyes and magnetic separation of degradation products.
Figure 10

Magnetic separation of MB solution treated with as-synthesized nanocomposites for 96 h using an external magnet. (a) S-0.5, (b) S-1, (c) S-2, (d) S-4, and (e) S-8.


In summary, SiO2-encapsulated ZVI NPs nanocomposites with tunable Fe content were synthesized using a two-step strategy. The results demonstrated that the catalytic degradation of MB depended on the content of ZVI NPs encapsulated in SiO2 microspheres. The dosage of H2O2 significantly promoted degradation rate without changing degradation efficiency. Furthermore, the content-dependent magnetic property of ZVI NPs enabled easy separation of the degradation products from the coagulated sludge using an external magnet. This strategy was facile and low cost for the industrial production of ZVI NPs for applications in environmental remediation.




This work was financially supported by the Natural Science Foundation of China (No. 30800256), the basic research project of Wuhan Science and Technology Bureau (No. 2014060101010041), and the Self-Determined and Innovative Research Funds of WUT (2014-CL-B1-13).

Authors’ Affiliations

State Key Laboratory of Advanced Technology for Materials Synthesis and Processing, Wuhan University of Technology, Wuhan, People's Republic of China
Department of Prosthetic, School of Stomatology, Wuhan University, Wuhan, People's Republic of China


  1. Soon AN, Hameed BH: Heterogeneous catalytic treatment of synthesis dyes in aqueous media using Fenton and photo-assisted Fenton process. Desalination 2011, 269: 1–16. 10.1016/j.desal.2010.11.002View ArticleGoogle Scholar
  2. Rafatullah M, Sulaiman O, Hashim R, Ahmad A: Adsorption of methylene blue on low-cost adsorbents: a review. J Hazard Mater 2010, 177: 70–80. 10.1016/j.jhazmat.2009.12.047View ArticleGoogle Scholar
  3. Forgacs E, Cserhati T, Oros G: Removal of synthetic dyes from wastewaters: a review. Environ Int 2004, 30: 953–971. 10.1016/j.envint.2004.02.001View ArticleGoogle Scholar
  4. Dutta K, Mukhopadhyay S, Bhattacharjee S, Chaudhuri B: Chemical oxidation of methylene blue using a Fenton-like reaction. J Hazard Mater 2001, 84: 57–71. 10.1016/S0304-3894(01)00202-3View ArticleGoogle Scholar
  5. Shannon MA, Bohn PW, Elimelech M, Georgiadis JG, Marinas BJ, Mayes AM: Science and technology for water purification in the coming decades. Nature 2008, 452: 301–310. 10.1038/nature06599View ArticleGoogle Scholar
  6. Schwarzenbach RP, Escher BI, Fenner K, Hofstetter TB, Johnson CA, von Gunten U, Wehrli B: The challenge of micropollutants in aquatic systems. Science 2006, 313: 1072–1077. 10.1126/science.1127291View ArticleGoogle Scholar
  7. Wang KS, Lin CL, Wei MC, Liang HH, Li HC, Chang CH, Fang YT, Chang SH: Effects of dissolved oxygen on dye removal by zero-valent iron. J Hazard Mater 2010, 182: 886–895. 10.1016/j.jhazmat.2010.07.002View ArticleGoogle Scholar
  8. Zhang N, Zhang YH, Xu YJ: Recent progress on graphene-based photocatalysts: current status and future perspectives. Nanoscale 2012, 4: 5792–5813. 10.1039/c2nr31480kView ArticleGoogle Scholar
  9. Han C, Yang MQ, Weng B, Xu YJ: Improving the photocatalytic activity and anti-photocorrosion of semiconductor ZnO by coupling with versatile carbon. Phys Chem Chem Phys 2014, 16: 16891–16903. 10.1039/C4CP02189DView ArticleGoogle Scholar
  10. Robinson T, McMullan G, Marchant R, Nigam P: Remediation of dyes in textile effluent: a critical review on current treatment technologies with a proposed alternative. Bioresour Technol 2001, 77: 247–255. 10.1016/S0960-8524(00)00080-8View ArticleGoogle Scholar
  11. Pearce CI, Lloyd JR, Guthrie JT: The removal of colour from textile wastewater using whole bacterial cells: a review. Dyes Pigments 2003, 58: 179–196. 10.1016/S0143-7208(03)00064-0View ArticleGoogle Scholar
  12. Zhang YH, Tang ZR, Fu XZ, Xu YJ: TiO2-graphene nanocomposites for gas-phase photocatalytic degradation of volatile aromatic pollutant: is TiO2-graphene truly different from other TiO2-carbon composite materials? ACS Nano 2010, 4: 7303–7314. 10.1021/nn1024219View ArticleGoogle Scholar
  13. Zhang N, Liu SQ, Xu YJ: Recent progress on metal core@semiconductor shell nanocomposites as a promising type of photocatalyst. Nanoscale 2012, 4: 2227–2238. 10.1039/c2nr00009aView ArticleGoogle Scholar
  14. Yang MQ, Xu YJ: Selective photoredox using graphene-based composite photocatalysts. Phys Chem Chem Phys 2013, 15: 19102–19118. 10.1039/c3cp53325eView ArticleGoogle Scholar
  15. Crini G: Non-conventional low-cost adsorbents for dye removal: a review. Bioresour Technol 2006, 97: 1061–1085. 10.1016/j.biortech.2005.05.001View ArticleGoogle Scholar
  16. Sakkas VA, Islam MA, Stalikas C, Albanis TA: Photocatalytic degradation using design of experiments: a review and example of the Congo red degradation. J Hazard Mater 2010, 175: 33–44. 10.1016/j.jhazmat.2009.10.050View ArticleGoogle Scholar
  17. Clarke BO, Smith SR: Review of 'emerging' organic contaminants in biosolids and assessment of international research priorities for the agricultural use of biosolids. Environ Int 2011, 37: 226–247. 10.1016/j.envint.2010.06.004View ArticleGoogle Scholar
  18. De Heredia JB, Torregrosa J, Dominguez JR, Peres JA: Kinetic model for phenolic compound oxidation by Fenton's reagent. Chemosphere 2001, 45: 85–90. 10.1016/S0045-6535(01)00056-XView ArticleGoogle Scholar
  19. Neamtu M, Yediler A, Siminiceanu I, Kettrup A: Oxidation of commercial reactive azo dye aqueous solutions by the photo-Fenton and Fenton-like processes. J Photochem Photobiol A-Chem 2003, 161: 87–93. 10.1016/S1010-6030(03)00270-3View ArticleGoogle Scholar
  20. Kušić H, Lončarić Božić A, Koprivanac N: Fenton type processes for minimization of organic content in coloured wastewaters: part I: processes optimization. Dyes Pigments 2007, 74: 380–387. 10.1016/j.dyepig.2006.02.022View ArticleGoogle Scholar
  21. Soon AN, Hameed BH: Degradation of acid blue 29 in visible light radiation using iron modified mesoporous silica as heterogeneous photo-Fenton catalyst. Appl Catal A-Gen 2013, 450: 96–105.View ArticleGoogle Scholar
  22. Li Z, Kawashita M, Kudo TA, Kanetaka H: Sol-gel synthesis, characterization, and in vitro compatibility of iron nanoparticle-encapsulating silica microspheres for hyperthermia in cancer therapy. J Mater Sci Mater Med 2012, 23: 2461–2469. 10.1007/s10856-012-4735-yView ArticleGoogle Scholar
  23. Li YC, Jin ZH, Li TL, Xiu ZM: One-step synthesis and characterization of core-shell Fe@SiO2 nanocomposite for Cr (VI) reduction. Sci Total Environ 2012, 421: 260–266.View ArticleGoogle Scholar
  24. Simkiene I, Treideris M, Niaura G, Szymczak R, Aleshkevych P, Reza A, Kasalynas I, Bukauskas V, Babonas GJ: Multifunctional iron and iron oxide nanoparticles in silica. Mater Chem Phys 2011, 130: 1026–1032. 10.1016/j.matchemphys.2011.08.025View ArticleGoogle Scholar
  25. Tang NJ, Jiang HY, Zhong W, Wu XL, Zou WQ, Du YW: Synthesis and magnetic properties of Fe/SiO2 nanocomposites prepared by a sol-gel method combined with hydrogen reduction. J Alloys Compd 2006, 419: 145–148. 10.1016/j.jallcom.2005.03.126View ArticleGoogle Scholar
  26. Singh V, Seehra MS, Huggins FE, Shah N, Huffman GP: Temperature and size dependence of magnetic and electron magnetic resonance parameters of Fe nanoparticles embedded in an amorphous SiO2 matrix. J Appl Phys 2011, 109: 07B506.Google Scholar
  27. Ding P, Ma J, Cao H, Liu Y, Wang L, Li J: Melting of iron nanoparticles embedded in silica prepared by mechanical milling. Mater Sci Eng B-Solid 2013, 178: 930–936. 10.1016/j.mseb.2013.05.006View ArticleGoogle Scholar
  28. Ma J, Li J, Ni X, Zhang X, Huang J: Microwave resonance in Fe/SiO2 nanocomposite. Appl Phys Lett 2009, 95: 102505. 10.1063/1.3224883View ArticleGoogle Scholar
  29. Zheng T, Zhan J, He J, Day C, Lu Y, Mcpherson GL, Piringer G, John VT: Reactivity characteristics of nanoscale zerovalent iron-silica composites for trichloroethylene remediation. Environ Sci Technol 2008, 42: 4494–4499. 10.1021/es702214xView ArticleGoogle Scholar
  30. Zhang XF, Dong XL, Huang H, Lv B, Zhu XG, Lei JP, Ma S, Liu W, Zhang ZD: Synthesis, structure and magnetic properties of SiO2-coated Fe nanoparticles. Mater Sci Eng A Struct Mater 2007, 454: 211–215.View ArticleGoogle Scholar
  31. Leite ER, Carreno NLV, Longo E, Pontes FM, Barison A, Ferreira AG, Maniette Y, Varela JA: Development of metal-SiO2 nanocomposites in a single-step process by the polymerizable complex method. Chem Mater 2002, 14: 3722–3729. 10.1021/cm0203767View ArticleGoogle Scholar
  32. Lobotka P, Dérer J, Vávra I, de Julián Fernández C, Mattei G, Mazzoldi P: Single-electron transport and magnetic properties of Fe-SiO2 nanocomposites prepared by ion implantation. Phys Rev B 2007, 75: 024423.View ArticleGoogle Scholar
  33. Stöber W, Fink A, Bohn E: Controlled growth of monodisperse silica spheres in the mecron size range. J Colloid Interface Sci 1968, 26: 62–69. 10.1016/0021-9797(68)90272-5View ArticleGoogle Scholar
  34. Zhang T, Zhang Q, Ge J, Goebl J, Sun M, Yan Y, Liu YS, Chang C, Guo J, Yin Y: A self-templated route to hollow silica microspheres. J Phys Chem C 2009, 113: 3168–3175. 10.1021/jp810360aView ArticleGoogle Scholar
  35. Lv PP, Zhao HL, Wang J, Liu X, Zhang TH, Xia Q: Facile preparation and electrochemical properties of amorphous SiO2/C composite as anode material for lithium ion batteries. J Power Sources 2013, 237: 291–294.View ArticleGoogle Scholar
  36. Fukui H, Ohsuka H, Hino T, Kanamura K: A Si-O-C composite anode: high capability and proposed mechanism of lithium storage associated with microstructural characteristics. ACS Appl Mater Interfaces 2010, 2: 998–1008. 10.1021/am100030fView ArticleGoogle Scholar
  37. Yu JG, Zhang LJ, Cheng B, Su YR: Hydrothermal preparation and photocatalytic activity of hierarchically sponge-like macro-/mesoporous titania. J Phys Chem C 2007, 111: 10582–10589. 10.1021/jp0707889View ArticleGoogle Scholar
  38. Huang YY, McCarthy TJ, Sachtler WMH: Preparation and catalytic testing of mesoporous sulfated zirconium dioxide with partially tetragonal wall structure. Appl Catal A 1996, 148: 135–154. 10.1016/S0926-860X(96)00223-2View ArticleGoogle Scholar
  39. Tardivo JP, Del Giglio A, de Oliveira CS, Gabrielli DS, Junqueira HC, Tada DB, Severino D, Turchiello RDF, Baptista MS: Methylene blue in photodynamic therapy: from basic mechanisms to clinical applications. Photodiagn Photodyn Ther 2005, 2: 175–191. 10.1016/S1572-1000(05)00097-9View ArticleGoogle Scholar
  40. Ovchinnikov OV, Smirnov MS, Shatskikh TS, Khokhlov VY, Shapiro BI, Vitukhnovsky AG, Ambrozevich SA: Spectroscopic investigation of colloidal CdS quantum dots-methylene blue hybrid associates. J Nanopart Res 2014, 16: 2286.View ArticleGoogle Scholar
  41. Bai CP, Gong WQ, Feng DX, Xian M, Zhou Q, Chen SH, Ge ZX, Zhou YS: Natural graphite tailings as heterogeneous Fenton catalyst for the decolorization of rhodamine B. Chem Eng J 2012, 197: 306–313.View ArticleGoogle Scholar
  42. Keenan CR, Sedlak DL: Factors affecting the yields of oxidants from the reaction of nanoparticulate zero-valent iron and oxygen. Environ Sci Technol 2008, 42: 1262–1267. 10.1021/es7025664View ArticleGoogle Scholar
  43. Zhang J, Hu FT, Liu QQ, Zhao X, Liu SQ: Application of heterogeneous catalyst of tris(1,10)-phenanthroline iron(II) loaded on zeolite for the photo-Fenton degradation of methylene blue. React Kinet Mech Cat 2011, 103: 299–310. 10.1007/s11144-011-0323-2View ArticleGoogle Scholar
  44. Wang Q, Tian SL, Long J, Ning P: Use of Fe(II)Fe(III)-LDHs prepared by co-precipitation method in a heterogeneous-Fenton process for degradation of methylene blue. Catal Today 2014, 224: 41–48.View ArticleGoogle Scholar
  45. He F, Zhao DY, Liu JC, Roberts CB: Stabilization of Fe-Pd nanoparticles with sodium carboxymethyl cellulose for enhanced transport and dechlorination of trichloroethylene in soil and groundwater. Ind Eng Chem Res 2007, 46: 29–34. 10.1021/ie0610896View ArticleGoogle Scholar
  46. Shukla P, Wang SB, Sun HQ, Ang HM, Tadé M: Adsorption and heterogeneous advanced oxidation of phenolic contaminants using Fe loaded mesoporous SBA-15 and H2O2. Chem Eng J 2010, 164: 255–260. 10.1016/j.cej.2010.08.061View ArticleGoogle Scholar


© Mao et al.; licensee Springer. 2014

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