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. 2018 Dec 28;12(1):96.
doi: 10.3390/ma12010096.

Adsorption Analyses of Phenol from Aqueous Solutions Using Magadiite Modified with Organo-Functional Groups: Kinetic and Equilibrium Studies

Mingliang Ge  1 , Xubin Wang  2 , Mingyi Du  3 , Guodong Liang  4 , Guoqing Hu  5 , Jahangir Alam S M  6   7   8
Affiliations

Adsorption Analyses of Phenol from Aqueous Solutions Using Magadiite Modified with Organo-Functional Groups: Kinetic and Equilibrium Studies

Mingliang Ge et al. Materials (Basel). .

Abstract

Organically-modified magadiite (MAG⁻CTAB⁻KH550) was synthesized via ion-exchange method and condensation reaction in the presence of pure magadiite (MAG), cetyltrimethylammonium bromide (CTAB) and γ-aminopropyltriethoxysilane (KH550) in aqueous solution in this research. This new adsorbent material was studied using scanning electron microscope (SEM), X-ray diffraction (XRD), Fourier transforms infrared spectroscopy (FTIR), and N₂ adsorption/desorption isotherms process. It was found that the MAG⁻CTAB⁻KH550 has high Brunaur-Emmet-Teller (BET) specific surface area and mesoporous pore size distribution which enhanced its ability to remove phenol in aqueous solution; and, the value of pH has a relatively large impact on the adsorption behavior of the sorbent. Finally, the adsorptive behavior of the mesoporous material on phenol was followed pseudo-second-order kinetic adsorption model. In contrast, the adsorption equilibrium isotherm was better performed Langmuir isotherm model than the Freundlich isotherm model; in addition, the results also showed that the MAG⁻CTAB⁻KH550 had a better adsorption capacity and removal efficiency than MAG.

Keywords: adsorption; adsorption isotherms; adsorption kinetics; magadiite; phenol.

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Conflict of interest statement

The authors declare no conflict of interest.

Figures

Figure 1
Figure 1
Procedure of MAG–CTAB–KH550 preparation.
Figure 2
Figure 2
SEM images of (a) MAG; (b) MAG–CTAB and (c) MAG–CTAB–KH550.
Figure 3
Figure 3
(a) XRD patterns of MAG, MAG–CTAB, and MAG–CTAB–KH550; (b) Infrared spectrum of MAG, MAG–CTAB, and MAG–CTAB–KH550.
Figure 4
Figure 4
N2 adsorption/desorption (a) curve and pore size distribution and (b) of MAG and MAG–CTAB–KH550 (at 10 s of equilibration interval, and −196 °C of analysis bath temperature).
Figure 5
Figure 5
(a) Effects of adsorbent dosage of MAG and MAG–CTAB–KH550 on removal efficiency and adsorption capacity of phenol (in the conditions of pH = 10, and the adsorption time for 60 min); (b) Effects of initial concentration of phenol on the removal efficiency and adsorption capacity under the conditions of sorbents dosage of 1 g/L and adsorption equilibrium time for 60 min, and pH value of 10; (c) Effects of adsorption time on adsorption capacity of phenol under the conditions of initial concentration of phenol at 50 mg/L, pH of 10, and the sorbents dosage of 1 g/L; and (d) Effects of pH values of the solution on adsorption capacity of phenol under the conditions of initial concentration of phenol at 50 mg/L, sorbents dosage of 1 g/L, and adsorption equilibrium time of 60 min.
Figure 6
Figure 6
Kinetic curves of the sorption of phenol for pristine MAG and MAG–CTAB–KH550 in the conditions of initial phenol concentration at 50 mg/L, the pH value at 10, and sorbents dosage at 1 g/L for: (a) Pseudo-first-order kinetic model; (b) Pseudo-second-order kinetic model.
Figure 7
Figure 7
Equilibrium isotherms of adsorption of MAG, and MAG–CTAB–KH550 for phenol.
Figure 8
Figure 8
Adsorption isotherm models (a) Langmuir model and (b) Freundlich model.
See this image and copyright information in PMC

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