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Synthesis of Manganese Chloride Activated Carbon Deriving from Wheat Straw and its Adsorption Mechanism for Arsenic and Chromium | OMICS International
ISSN: 2380-2391
Journal of Environmental Analytical Chemistry
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Synthesis of Manganese Chloride Activated Carbon Deriving from Wheat Straw and its Adsorption Mechanism for Arsenic and Chromium

Ningyuan Zhu1,2, Tingmei Yan1*, Jun Qiao1 and Honglei Cao1,2

1Institute of Soil Science, Chinese Academy of Sciences, No. 71 East Beijing Road, Nanjing 210008, China

2Graduate School of the Chinese Academy of Sciences, Beijing 100039, China

*Corresponding Author:
Tingmei Yan
Institute of Soil Science
Chinese Academy of Sciences
No. 71 East Beijing Road
Nanjing 210008, China
Tel: 8602586881308
E-mail: [email protected]

Received Date: March 01, 2016; Accepted Date: March 03, 2016; Published Date: March 10, 2016

Citation: Zhu N, Yan T, Qiao J, Cao H (2016) Synthesis of Manganese Chloride Activated Carbon Deriving from Wheat Straw and its Adsorption Mechanism for Arsenic and Chromium. J Environ Anal Chem 3:172. doi:10.4172/2380-2391.1000172

Copyright: © 2016 Zhu N, et al. This is an open-access article distributed under the terms of the Creative Commons Attribution License, which permits unrestricted use, distribution, and reproduction in any medium, provided the original author and source are credited.

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Abstract

Manganese impregnated biochar deriving from wheat straw were synthesized to treat heavy metal contamination. Nitrogen adsorption-desorption isotherms, scanning electron microscopy-energy dispersive X-Ray spectroscopy (SEM-EDS), and X-ray diffraction (XRD) were used to determine the characteristics of adsorbents. Batch adsorption experiments demonstrated a fit Langmuir model with the maximum adsorption capacity of 0.216 mmol g-1 for As (III) and a suitable Freundlich model for Cr (VI) respectively. Fourier transform infrared spectroscopy (FTIR) and X-ray photoelectron spectroscopy (XPS) were measured to explore probable adsorption mechanisms involving As and Cr adsorption, which indicated that the Lewis acid-base interactions play a more important role in arsenic adsorption while electrostatic interaction along with the reduction Cr (VI) to Cr (III) contribute primarily to chromium adsorption.

Keywords

Wheat straw; Manganese chloride; Activated carbon; Adsorption mechanism

Introduction

In the past few decades, discharging thousands of organic, inorganic, and biological pollutants into environment has severely deteriorated water quality especially the heavy metals pollution which could be concentrated in organisms and, thus, harmful to most plants and animals not only at a high dose but also in relatively low concentration [1]. The continuous existence of heavy metal contaminant in the water environment, such as the high toxic arsenic and chromium, has been threaten seriously to water resource. Many studies have applied various methods such as ion exchange, solvent extraction, chemical precipitation and adsorption to reduce the concentration of these kinds of metal ions [2,3]. Among these methods, adsorption has been proved to be the most commonly used technique due to its simplicity of design, high efficiency, ease of operation and heavy metal adsorbents like polymeric hybrid sorbent, manganese oxide modified biochar and akaganeite nanoparticles have been well investigated [4-6]. Pacheco et al. [7] prepared alumina silica nanoparticles with hydroxyl, alkoxy, and oxy groups, which could remove cadmium efficiently by cationic exchange from wastewater samples. Banerjee and Chen [8] modified magnetic Fe3O4 nanoparticles with gum arabic which could adsorb copper metal ion rapidly from aqueous solution due to carboxylic groups of gum arabic, complexation of the amine group of gum arabic and surface hydroxyl groups of iron oxide.

In addition, many authors have used natural Akadama clay, modified chitosan and activated carbon for removal chromium [9-11] and sorbents derived from iron and aluminium such as granular ferric hydroxide, Fe-loaded sponge and gibbsite for arsenic reduction [3,12-14]. Still, there are no low-cost and high effective methods and materials, even based on adsorption methods, for arsenic and chromium treatment, which predominantly exist in the inorganic anion forms of AsO2-(III), AsO43-(V), and Cr2O72- (VI) [11,15]. Unfortunately, Cr (VI) is about one hundred to five hundred times more toxic than Cr (III) and toxicity of Cr (VI) can seriously destroy people’s health including skin irritation, nausea, severe diarrhea, as well as lung, liver, and kidney damage because of its teratogenicity, mutagenicity, and carcinogenicity in biological systems [16,17]. Still, there are few researches had reported a cost-effective and eco-friendly material for lower of chromium and arsenic which are main existed as the anion forms and, thus, more difficult to be reduced [16,18]. Besides, the inorganic species arsenate (As (V) at high redox potential value) and arsenite (As (III) at low redox potential value) were the predominant forms of as in aquatic  environment. The trivalent Cr (III) and hexavalent forms Cr (VI) are the primarily form for chromium in natural water, which depends on the oxidative properties and pH level. Heavy metals, especially the chromium and arsenic, are more problematic and threatening to ecological environment and human beings because of their high toxicity, non-biodegradation and accumulation through food chain. Thus, the World Health Organization recommended the maximum permissible limit for arsenic is 10 μg L-1 while the maximum limit for chromium is 0.05 mg L-1 in drinking water [15,17,19].

As (III), that can take up 67-99% of total arsenic in groundwater, is more problematic than As (V) because As (III) is more toxic and difficult to remove from water [3,15]. Since arsenic and chromium are highly toxic and carcinogenic, the maximum permissible limit for arsenic is 10 μg/L in drinking water according to the World Health Organization and the maximum contaminant level of chromium (VI) is 50 μg/L for potable water according to the United States Environment Protection Agency, respectively [10,12]. Therefore, it is very imperative to consider innovative and effective treatment options to meet the stringent arsenic and chromium standard.

Herein, to enhance their sorption capacity, the manganese chloride and wheat straw, which was one of the most abundant straw resources in China [20], were explored to prepare a low cost but high efficiency material for heavy metal treatment and straw utilization. The specific objectives of this work were to: (1) prepare and characterize MnCl2 impregnated biochar composites, (2) test its sorption capacities for As (III) and Cr (VI), and (3) investigate the possible mechanisms involved in the As (III) and Cr (VI) sorption.

Materials and Methods

Preparation of manganese activated carbon

Stock solutions of 0.2 M manganese chloride (Mn-solution) was prepared in a volumetric flask. 7.692 mmol L-1 sodium arsenite and 3.401 mmol L-1 potassium dichromate were prepared and diluted to the required concentrations with 0.01 M NaCl. MnCl2.4H2O, sodium arsenite, potassium dichromate, sodium chloride and other reagents used in this work were all analytical grade.

Wheat straw was obtained from Wuxi city, Jiangsu province, China. Manganese activated carbon (MnBCs) were produced as follow: 100 ml Mn-solution was mixed with wheat straw milled and sized to diameters <0.80 mm, stirred vigorously at 80°C for 3 h, sonicated for 1 h and then dried at 105°C. The biochar precursors were continuously heated to a target temperature (300, 400, 500,600, 700 and 800°C) and finally maintained for 60 min in a furnace with the heating rate of 10°C min-1 under 100 ml min-1 nitrogen flow. Activated carbons were labelled as MnBC300, MnBC400, MnBC500, MnBC600, MnBC700 and MnBC800. The control biochar was also prepared by the same pyrolyzation process as manganese activated carbon under 500°C and labelled as CBC500.

Sorption experiments

Effect of pH on arsenic and chromium removal was investigated in a 100 ml digestion vessels containing 0.1 gram adsorbent and 50 ml of 0.385 mmol L-1 sodium arsenite or 0.170 mmol L-1 potassium dichromate solution at room temperature. The pH level was adjusted at the range of 2-12 with hydrochloric acid and sodium hydroxide.

Adsorption isotherm experiments were conducted by mixing 0.1 g adsorbent with 50 ml sodium arsenite with the concentration ranging from 0.038-1.538 mmol L-1 or potassium dichromate solutions with the concentration ranging from 0.017-0.680 mmol L-1 under the optimum pH level in a vessel. All the vessels above were shaken at 150 rpm in the oscillator for 2 h and then placed in the water bath under constant temperature (25°C) for 24 h to reach equilibrium. Inductive coupled plasma emission spectrometry (ICP) and Inductive coupled plasma emission spectrometry- mass spectrum (ICP-MS) were used to detect the concentration of arsenic and chromium.

Characterization of adsorbents

N2 (0.162 nm2) adsorption-desorption experimental, scanning electron microscopy - energy spectrum analysis (SEM-EDS) and X-ray diffraction were used to detective the surface characteristic of materials. Fourier transform infrared spectroscopy (FTIR) and X-ray photoelectron spectroscopy (XPS) were measured to explore probable adsorption mechanisms involving as and Cr adsorption.

Results and Discussion

Characteristics of activated carbon

N2 adsorption-desorption isotherms: In order to investigate the porosity of the MnCl2 activated carbon, nitrogen adsorption, a standard procedure for determination of the porosity of porous adsorbents, was used for determining its surface area and porous structure [21]. Figure 1 shown a reversible Type II isotherm which obtained with a non-porous or macropore adsorbent and represented unrestricted monolayer-multilayer adsorption. A type II isotherm contained a Point B, the beginning of the almost linear middle section of the isotherm, indicating the end stage of monolayer coverage and the initiate of multilayer adsorption. The Point B was positioned very far forward on those line suggesting MnBCs possessed few tiny micropore structure.

environmental-analytical-chemistry-adsorption–desorption

Figure 1: N2 adsorption–desorption isotherms of various activated carbons.

Surface area and pore volume: Most of the pore size distributions of the activated carbons are between 20 Å and 200 Å, which indicates that the carbons are mainly mesopore (Figure 2). Table 1 displayed the significant effect of carbonization temperature and manganese chloride on pore development and specific surface area. Specific surface area and pore volume increased with temperature escalating from 300 to 500°C, decreased dramatically at 600°C and then enlarged again as temperature rising from 600 to 800°C. The average pore diameter showed the opposite changing rule as the surface area and pore volume. Unexpectedly, the average pore diameter under a high carbonization temperature displayed a different variation trend from former investigation: the pore diameter did not increased, they decreased instead. In general, pore size distribution of activated carbon is dependent on activation temperature, raw material and retention time. Increasing the carbonization temperature within a certain temperature range increases the evolution of volatile matters from the precursor, making the benefit of pore development, and creating new pores. The pyrolyzation effect, when out of the range, will cause the collapse of micropore and wide a significant amount of micropore to mesopore, quality just drop [22,23]. The abnormal variation trend under high pyrolyzation temperature indicated that the activating agent must make a difference in biochars pore structure and specific surface area.

environmental-analytical-chemistry-Pore-distribution

Figure 2: Pore distribution of MnBCs.

Sample SBET (m2/g) SExternal (m2/g) Dp (nm) VTotal (cm3/g)
MnBC300 17.27 9.239 16.01 0.027
MnBC400 19.35 6.352 16.51 0.030
MnBC500 19.47 8.009 10.99 0.035
MnBC600 6.732 3.765 12.3 0.012
MnBC700 8.88 2.998 10.15 0.011
MnBC800 9.126 5.944 8.39 0.014

Table 1: Surface areas and pore volumes of activated carbons.

SEM-EDS and XRD: Surface morphology and the main element of the activated carbon were investigated by scanning electron microscope (SEM) and energy spectrum analysis (EDS). The pore structure was observed obviously for the MnBC300, MnBC400 and MnBC500. The surface of MnBC600, however, was smooth and evidently absence of porosity. The pore structure appeared again for MnBC700 and became distinctly for MnBC800 (Figure 3). EDS results shown that the MnBCs were mainly contained carbon, oxygen, manganese and chloride (EDS was unable to detect the hydrogen element) (Table 2). The amount of chloride atom was almost as twice as the manganese atom may indicating that a considerable number MnCl2, not the manganese oxide, still existed on the surface of those activated carbons. The X-ray diffraction could prove that hypothesis. The diffraction peaks were almost same for MnBC400, MnBC500, MnBC600, MnBC700 and MnBC800 (Figure 4). Diffraction peaks at 2θ=15.729, 20.165 and 31.879 which were corresponding to 110, 020 and 021 planes respectively, for MnCl2 (H2O)4 structure. The diffraction peaks for MnBC300 was obviously different from other MnBCs, which represented MnCl2 (H2O)2. It is known that melting point of MnCl2 was almost 650°C. Thus, we hypothesis that activating agent (melted liquid MnCl2) may inhibit the collapse of the micropore and even created new pore structure within the carbon matrix at 700 and 800°C.

environmental-analytical-chemistry-SEM-MnBCs

Figure 3: SEM of MnBCs: a, MnBC300; b, MnBC400; c, MnBC500; d, MnBC600; e, MnBC700 and f, MnBC800.

environmental-analytical-chemistry-XRD-pattern

Figure 4: XRD pattern of MnBCs.

MnBCs C O N Cl Mn
Element (wt%)
MnBC300 43.64 14.02 1.68 23.88 16.78
MnBC400 46.5 7.6 0.82 23.01 22.07
MnBC500 51 5.54 0.31 21.59 21.56
MnBC600 44.6 4.72 0.62 24.47 25.59
MnBC700 53.85 5 0.53 19.9 20.72
MnBC800 45.42 6.22 0.88 23.4 24.08

Table 2: ED’s results of the main elements content of MnBCs.

Adsorption study

Effect of pH and sorbent dosage: MnBC500 was chosen for adsorption study because of its highest specific surface area and pore volume. Prior to sorption study, the manganese chloride modified carbon was washed thoroughly to get rid of manganese chloride. The effect of initial solution pH level for adsorption of arsenic and chromium were studied firstly. The raw biochar (CBC500) removed few chromium and negligible arsenic. The removal efficiency of arsenic for MnBC500 went up gradually and then decreased with increasing the initial solution pH level (Figure 5). The maximum adsorption ability of As (III) was obtained at pH 9.5, which was coincident with the first dissociation constant of H3AsO3 (pK1=9.23). Chromium adsorption was also affected dramatically by the initial solution pH value. Removal efficiency decreased with increasing initial pH value ranging from 2 to 12.

environmental-analytical-chemistry-chromium-adsorption

Figure 5: The effect of pH value on arsenic and chromium adsorption.

Adsorption isotherm: Three widely used isotherm models, namely the Langmuir, Freundlich isotherm and Temkin models, were applied to fitted adsorption experimental data [24]. The Langmuir model (i.e., L model) assumed the repulsive interaction was inexistent among adsorbate particles and adsorption heat was homogeneous; Freundlich model (i.e., F model) was based on a multilayer adsorption condition with an inhomogeneous distribution of adsorption heat; Temkin isotherm (i.e., T model) assumed that the heat of adsorption decreased linearly. These equations could be expressed in the following form:

Equation                                                          (1)

Equation                                              (2)

Equation                                        (3)

Where Ce (mmol L-1) was the equilibrium concentration, and qe (mmol g-1) was the amount of adsorption capacity at equilibrium, respectively. Q0 (mmol g-1) and b (L mmoL-1) were Langmuir constants. Kf (mmol g-1) and n were Freundlich constants. A (L mmoL-1) and bT (J moL-1) were Temkin constants. T was absolute temperature and R was universal gas constant 8.314 J moL-1 K-1. Results shown the L model was mostly suitable the equilibrium data of arsenic adsorption (r2L>r2T> r2F) assuming a monolayer adsorption process for As (Figure 6). The maximum adsorption capacity was 0.216 mmol g-1 for As (III) which was more excellent than other commonly used adsorbents reported in the literature. A dimensionless equilibrium parameter (RL) can further analysis of the Langmuir equation. The lower RL value means the more favorable adsorption provided at the range between 0 and 1. The value of RL was 0.025-0.507 for MnBC500 in the C0 range of this study, implying a favorable arsenic adsorption process. The Temkin plots also had good linearity indicating the strong chemical interaction between adsorbate and adsorbent. These results illustrated the homogenous distribution of active sites over sorbent surface. Generally, the Langmuir model was suitable for the uniformly distributed metal salts, namely, the active sorption site to some certain contaminants on the surface of activated carbon. The Freundlich model, however, best fitted to the chromium sorption data ( r2F> r2L> r2T) suggesting a multilayer sorption process for chromium. This result may also indicated that those active adsorption sites were inoperative to chromium. The maximum Cr (VI) adsorption capacity was detected as 0.442 mmol g-1 in our study (Table 3).

environmental-analytical-chemistry-adsorption-isotherm

Figure 6: Three adsorption isotherm modes for arsenic and chromium adsorption.

Temperature
(K)
Langmuir parameters Thermodynamics
Q0
(mmol/g)
b R2 ΔG°
(kJ mol−1)
ΔH°
(kJ mol−1)
ΔS°
(kJ mol−1)
283 0.183 10.75 0.992 -33.2    
298 0.216 25.24 0.999 -35.13 0.15 9.55
318 0.268 28.22 0.999 -37.45 � �

Table 3: Parameters of Langmuir isotherms and thermodynamics of As (III) adsorption.

Adsorption mechanism

FTIR: FTIR spectra of CBC500, MnBC500, MnAsBC500 and MnCrBC500 were presented in Figure 4 to identify some important functional groups and the roles they played in adsorption process. The peaks at 3436, 2976, 1634, 1384, and 1045 cm-1 were related groups of biochar, which assigned in Table 4. The new peak at 617 cm-1 demonstrated the Mn2+–O lattice vibration band [25]. The vibration on 1634 cm-1 shift to 1604 cm-1 for MnBC500 suggesting the activation agent enhanced the formation of aromatic ring structure which possession the conjugated π bond decreasing the vibrational force constant of C=C. These aromatic compounds are easy to take place nucleophilic substitution and nucleophilic addition (Figure 7b). It was reported that the characteristic absorption bands of adsorbed arsenate was 650-950 cm-1 for As-OH or As–O stretching vibration [26]. Peak at 793 cm-1 represented a weak As -O bond suggesting As (III) surface complex was non-protonated [27,28] while peak at 876 cm-1 may implying the As-OH vibration. Only a new peak at 880 cm-1 was observed after Cr adsorption. However, this peak has no relation with Cr-O.

environmental-analytical-chemistry-FTIR-spectra

Figure 7: FTIR spectra for biochars: a, CBC500; b, MnBC500; c, MnCrBC500; d, MnAsBC500.

Wave number (cm−1) Characteristic vibrations
3446 O-H stretching of H-bonded hydroxyl
2976 C-H stretching vibration
1634 C=C stretching of aromatic ring
1384 C-H bending of CH3 (symmetric) groups
1045 C-O stretching of C-OH groups

Table 4: Assignment of the main characteristic vibrations of biochar’s FT-IR spectrum.

XPS investigation: XPS was used to further investigate the mechanism of arsenic sorption on the manganese modified biochars as well as chromium adsorption mechanism (Figure 8). A manganese peaks corresponding to Mn2p was found in the surface of Mnimpregnated biochar both before and after as interaction. The binding energy 641.7 eV represented the existence of MnO structure while the binding energy 653.7 eV suggested a higher valency of manganese (III) [29,30]. The higher valency of manganese like Mn(IV) and Mn(III) had the ability to oxide As (III) to As (V) which was more easier to adsorbed by manganese oxide [31]. However, there was no obvious decrease of Mn (III) content or increase of Mn (II) after arsenic adsorption. Prominent peak corresponding to As3d was observed in the surface of MnAsBC500 and the binding energy was 48.75 suggesting As (III) oxidation was not happen. The former researches has demonstrated As (V) could be adsorbed through the electrostatic force as well as ligand exchange reactions while the As (III) adsorption was mainly involved ligand exchange reaction [13]. Thus, the main adsorption mechanism could be attributed to the ligand reaction between the manganese and arsenite. If we can control the oxygen content to form a high valency manganese oxide, the arsenic adsorption capacity may be further enhanced. Nevertheless, the definite structure of Mn-As complexes needs to be further studied. That is our ongoing research work.

environmental-analytical-chemistry-High-resolution-XPS

Figure 8: High-resolution XPS spectra for Mn2p, As3d and Cr2p regions of MnBC500, MnAsBC500 and MnCrBC500.

Meanwhile, during the chromium sorption process, the 72% of manganese (II) atoms are oxidized to Mn (III) and Mn (IV), which was illustrated in Figure 8. Consequently, the adsorbed Cr (VI) could be reduced to Cr (III) via reaction with the Mn (II) (Figure 8). This results suggested that chromium adsorption mechanism was related to the reduction Cr (VI) to Cr (III) along with the electrostatic phenomenon.

Conclusion

Based on experimental results, manganese chloride activated carbons derived from wheat straw were synthesized and shown high sorption ability to arsenic and chromium. Bach sorption experiments shown a fitted Langmuir model for arsenic adsorption while a suitable Freundlich model for chromium adsorption. Ligand exchange contributed mainly to arsenic removal while electrostatic phenomenon with the chromium reduction played an important role in chromium sorption. This work demonstrated that manganese modified biochar provides an innovative and effective way to utilize straw resources by preparing low-cost adsorbents for heavy metal pollutants treatment.

Acknowledgements

This study was funded by the National Natural Science Foundation of China (41171236), the National Key Technology R&D Program of China (2012BAD15B03) and the National S&T Major Project of China (2012ZX07204-003).

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