10.1007/s40089-014-0124-5

Magnetic solid phase adsorption, preconcentration and determination of methyl orange in water samples using silica coated magnetic nanoparticles and central composite design

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  • Masoud Shariati-Rad*1,
  • Mohsen Irandoust1,
  • Somayyeh Amri1,
  • Mostafa Feyzi2,
  • Fattaneh Ja’fari2,
  1. Department of Analytical Chemistry, Faculty of Chemistry, Razi University, Kermanshah, 6714967346, IR
  2. Department of Physical Chemistry, Faculty of Chemistry, Razi University, Kermanshah, 6714967346, IR
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Published in Issue 2014-10-07

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Shariati-Rad, M., Irandoust, M., Amri, S., Feyzi, M., & Ja’fari, F. (2014). Magnetic solid phase adsorption, preconcentration and determination of methyl orange in water samples using silica coated magnetic nanoparticles and central composite design. International Nano Letters, 4(4 (December 2014). https://doi.org/10.1007/s40089-014-0124-5
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Abstract

Abstract This work evaluates the efficiency of SiO 2 -coated Fe 3 O 4 magnetic nanoparticles (SMNPs) for adsorption of methyl orange (MO). Adsorption of MO on the studied nanoparticle was developed for removal, preconcentration and spectrophotometric determination of trace amounts of it. To find the optimum adsorption conditions, the influence of pH, dosage of the adsorbent and contact time was explored by central composite design. In pH 2.66, with 10.0 mg of the SMNPs and time of 30.0 min, the maximum adsorption of MO was obtained. The experimental adsorption data were analyzed by the Langmuir and Freundlich adsorption isotherms. Both models were fitted to the equilibrium data and the maximum monolayer capacity q max of 53.19 mg g −1 was obtained for MO. Moreover, the sorption kinetics was fitted well to the pseudo-second-order rate equation model. The results showed that desorption efficiencies higher than 99 % can be achieved in a short contact time and in one step elution by 2.0 mL of 0.1 mol L −1 NaOH. The SMNPs were washed with deionized water and reused for two successive removal processes with removal efficiencies more than 90 %. The calibration curve was linear in the range of 10.0–120.0 ng mL −1 for MO. A preconcentration factor of about 45 % was achieved by the method.

Keywords

  • Magnetic nanoparticles,
  • Methyl orange,
  • Preconcentration,
  • Central composite design,
  • Isotherm
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References

  1. Malik et al. (2007) Adsorption of malachite green on ground nutshell waste based powdered activated carbon (pp. 1129-1138) https://doi.org/10.1016/j.wasman.2006.06.009
  2. Mittal et al. (2007) Studies on the adsorption kinetics and isotherms for the removal and recovery of methyl orange from wastewaters using waste materials (pp. 229-240) https://doi.org/10.1016/j.jhazmat.2007.02.028
  3. Juang et al. (2002) Characterization and use of activated carbons prepared from bagasse for liquid-phase adsorption (pp. 191-199) https://doi.org/10.1016/S0927-7757(01)01004-4
  4. Teng and Lin (2006) Removal of methyl orange dye from water onto raw and acid-activated montmorillonite in fixed beds (pp. 71-81) https://doi.org/10.1016/j.desal.2006.03.521
  5. Chena et al. (2011) Characterization of anionic-cationic surfactants modified montmorillonite and its application for removal of methyl orange (pp. 1150-1158) https://doi.org/10.1016/j.cej.2011.05.013
  6. Liu et al. (2011) Rapid modification of montmorillonite with novel cationic Gemini surfactants and its adsorption for methyl orange (pp. 1220-1226) https://doi.org/10.1016/j.matchemphys.2011.08.064
  7. Kan et al. (2011) Removal of methyl orange from aqueous solutions using a bentonite modified with a new gemini surfactant (pp. 184-187) https://doi.org/10.1016/j.clay.2011.07.009
  8. Leodopoulos et al. (2012) Single and simultaneous adsorption of methyl orange and humic acid onto bentonite (pp. 84-90) https://doi.org/10.1016/j.clay.2012.08.005
  9. Tang et al. (2012) Enhanced adsorption of methyl orange by vermiculite modified by cetyltrimethylammonium bromide (CTMAB) (pp. 2179-2187) https://doi.org/10.1016/j.proenv.2012.01.207
  10. Zhu et al. (2010) Preparation, characterization, adsorption kinetics and thermodynamics of novel magnetic chitosan enwrapping nanosized γ-Fe2O3 and multi-walled carbon nanotubes with enhanced adsorption properties for methyl orange (pp. 5063-5069) https://doi.org/10.1016/j.biortech.2010.01.107
  11. Rakhshaee et al. (2011) Removal of methyl orange from aqueous solution by Azolla filicoloides: synthesis of Fe3O4 nano-particles and its surface modification by the extracted pectin of Azolla (pp. 501-504) https://doi.org/10.1016/j.cclet.2010.10.041
  12. Deligeer et al. (2011) Adsorption of methyl orange on mesoporous-Fe2O3/SiO2 nanocomposites (pp. 3524-3528) https://doi.org/10.1016/j.apsusc.2010.11.067
  13. Chen et al. (2011) Isotherm, thermodynamic, kinetics and adsorption mechanism studies of methyl orange by surfactant modified silkworm exuviae (pp. 246-254)
  14. Elizalde-Gonzalez et al. (2008) Chemically modified maize cobs waste with enhanced adsorption properties upon methyl orange and arsenic (pp. 5134-5139) https://doi.org/10.1016/j.biortech.2007.09.023
  15. Li et al. (2012) Removal of methyl orange from aqueous solution by calcium alginate/multi-walled carbon nanotubes composite fibers (pp. 863-868) https://doi.org/10.1016/j.egypro.2012.01.138
  16. Mittal et al. (2007) Studies on the adsorption kinetics and isotherms for the removal and recovery of methyl orange from wastewaters using waste materials (pp. 229-240) https://doi.org/10.1016/j.jhazmat.2007.02.028
  17. Jalil et al. (2010) Adsorption of methyl orange from aqueous solution onto calcined Lapindo volcanic mud (pp. 755-762) https://doi.org/10.1016/j.jhazmat.2010.05.078
  18. Haque et al. (2010) Adsorptive removal of methyl orange from aqueous solution with metal-organic frameworks, porous chromium-benzenedicarboxylates (pp. 535-542) https://doi.org/10.1016/j.jhazmat.2010.05.047
  19. Haque et al. (2011) Adsorptive removal of methyl orange and methylene blue from aqueous solution with a metal-organic framework material, iron terephthalate (MOF-235) (pp. 507-511) https://doi.org/10.1016/j.jhazmat.2010.09.035
  20. Afkhami et al. (2010) Modified maghemite nanoparticles as an efficient adsorbent for removing some cationic dyes from aqueous solution (pp. 240-248) https://doi.org/10.1016/j.desal.2010.06.065
  21. Ngomsik et al. (2005) Magnetic nano- and microparticles for metal removal and environmental applications: a review (pp. 963-970) https://doi.org/10.1016/j.crci.2005.01.001
  22. Afkhami and Norooz-Asl (2009) Removal, preconcentration and determination of Mo (VI) from water and wastewater samples using maghemite nanoparticles (pp. 52-57) https://doi.org/10.1016/j.colsurfa.2009.05.024
  23. Qadri et al. (2009) Removal and recovery of acridine orange from solutions by use of magnetic nanoparticle (pp. 318-323) https://doi.org/10.1016/j.jhazmat.2009.03.103
  24. Santhi et al. (2010) Removal of methyl red from aqueous solution by activated carbon prepared from the Annona squmosa seed by adsorption (pp. 11-18) https://doi.org/10.3329/cerb.v14i1.3767
  25. Chin and Yaacob (2007) Synthesis and characterization of magnetic iron oxide nanoparticles via w/o microemulsion and Massart’s procedure (pp. 235-237) https://doi.org/10.1016/j.jmatprotec.2007.03.011
  26. Albornoz and Jacobo (2006) Preparation of a biocompatible magnetic film from an aqueous ferrofluid (pp. 12-15) https://doi.org/10.1016/j.jmmm.2005.11.021
  27. Kim et al. (2005) Synthesis of ferrofluid with magnetic nanoparticles by sonochemical method for MRI contrast agent (pp. 328-330) https://doi.org/10.1016/j.jmmm.2004.11.093
  28. Kimata et al. (2003) Preparation of monodisperse magnetic particles by hydrolysis of iron alkoxide (pp. 112-118) https://doi.org/10.1016/S0032-5910(03)00046-9
  29. Alvarez et al. (2006) Novel flow injection synthesis of iron oxide nanoparticles with narrow size distribution (pp. 4625-4633) https://doi.org/10.1016/j.ces.2006.02.032
  30. Basak et al. (2007) Electrospray of ionic precursor solutions to synthesize iron oxide nanoparticles: Modified scaling law (pp. 1263-1268) https://doi.org/10.1016/j.ces.2006.11.029
  31. Feyzi et al. (2013) Catalytic performance of Fe–Mn/SiO2 nanocatalyst for CO hydrogenation (pp. 1-10) https://doi.org/10.1155/2013/973160
  32. Alizadeh et al. (2012) Biguanide-functionalized Fe3O4/SiO2 magnetic nanoparticles: an efficient heterogeneous organosuperbase catalyst for various organic transformations in aqueous media (pp. 2546-2552) https://doi.org/10.5012/bkcs.2012.33.8.2546
  33. Simkiene et al. (2011) Multifunctional iron and iron oxide nanoparticles in silica (pp. 1026-1032) https://doi.org/10.1016/j.matchemphys.2011.08.025
  34. Klug and Alexander (1974) Wiley
  35. Predoi et al. (2007) Iron oxide in a silica matrix prepared by the sol–gel method (pp. 6319-6323) https://doi.org/10.1016/j.tsf.2006.11.148
  36. Bruni et al. (1999) IR and NMR study of nanoparticle-support interactions in a Fe2O3–SiO2 nanocomposite prepared by a sol–gel method (pp. 573-586) https://doi.org/10.1016/S0965-9773(99)00335-9
  37. Bordiga et al. (1996) Structure and reactivity of framework and extraframework iron in Fe–silicalite as investigated by spectroscopic and physicochemical methods (pp. 486-501) https://doi.org/10.1006/jcat.1996.0048
  38. Fabrizioli et al. (2002) Synthesis, structural and chemical properties of iron oxide–silica aerogels (pp. 619-630) https://doi.org/10.1039/b108120a
  39. Qing et al. (2011) Modification of Fe–SiO2 interaction with zirconia for iron-based Fischer–Tropsch catalysts (pp. 111-122) https://doi.org/10.1016/j.jcat.2011.01.005
  40. Gunaraj and Murugan (1999) Application of response surface methodology for predicting weld bead quality in submerged arc welding of pipes (pp. 266-275) https://doi.org/10.1016/S0924-0136(98)00405-1
  41. Box and Hunter (1957) Multi-factor experimental designs for exploring response surfaces (pp. 195-241) https://doi.org/10.1214/aoms/1177707047
  42. Brereton, R.G.: Chemometrics: Data Analysis for the Laboratory and Chemical Plant. Wiley, New York, pp. 76–84 (2003)
  43. Afkhami and Moosavi (2010) Adsorptive removal of Cango red, a carcinogenic textile dye, from aqueous solutions by maghemite nanoparticles (pp. 398-403) https://doi.org/10.1016/j.jhazmat.2009.09.066
  44. Chien and Clayton (1980) Application of Elovich equation to the kinetics of phosphate release and sorption on soils (pp. 265-268) https://doi.org/10.2136/sssaj1980.03615995004400020013x
  45. Shariati et al. (2011) Fe3O4 magnetic nanoparticles modified with sodium dodecyl sulfate for removal of safranin O dye from aqueous solutions (pp. 160-165) https://doi.org/10.1016/j.desal.2010.11.040
  46. Langmuir (1918) The adsorption of gases on plane surfaces of glass, mica and platinum (pp. 1361-1403) https://doi.org/10.1021/ja02242a004
  47. Chatterjee et al. (2009) Enhanced adsorption of Congo red from aqueous solutions by chitosan hydrogel beads impregnated with cetyl trimethyl ammonium bromide (pp. 2803-2809) https://doi.org/10.1016/j.biortech.2008.12.035
  48. Belessi et al. (2009) Removal of reactive red 195 from aqueous solutions by adsorption on the surface of TiO2 nanoparticles (pp. 836-844) https://doi.org/10.1016/j.jhazmat.2009.05.045
  49. Miller, JN, Miller, JC (Eds.): Statistics and Chemometrics for Analytical Chemistry. Fifth ed., Pearson Education Limited, London, p. 114 (2005)