# Sorption of Pyrene by Clay Minerals Coated with Dissolved Organic Matter (DOM) from Landfill Leachate

Authors: Pingxiao Wu; Yong Wen; Yun Xiang; Jianbing Zhou; Jianwei Du; Nengwu Zhu; Ping Li
Journal: Journal of Chemistry
 (2015)

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## Abstract

Interactions of dissolved organic matter (DOM) from landfill leachate with clays could affect significantly the fate of hydrophobic organic compounds (HOCs) in soils. The complexes of montmorillonite (MT) and kaolinite (KL) with DOM extracted from landfill leachate were prepared under controlled conditions, termed CMT and CKL, respectively. The bare clays and their complexes were characterized by powder X-ray diffraction (XRD), Fourier transform infrared (FTIR), thermogravimetry (TG), differential scanning calorimetry (DSC), and scanning electron microscopy (SEM). Batch experiments were designed to investigate the sorption behavior of pyrene onto the clays in the presence of DOM. The maximum sorption capacities of pyrene on MT, CMT, KL, and CKL were 22.18, 38.96, 42.00, and 44.99μg·g−1, respectively, at the initial concentration of 1000 ± 150 μg·L−1. The sorption isotherms of pyrene by the bare clays followed the Henry model well, whereas the Freundlich sorption isotherm provided a better fit to the equilibrium data of the sorption by the complexes. The role of montmorillonite and kaolinite complexes with DOM in the retention of pyrene in soils was different. This may be due to the different crystal structures between montmorillonite and kaolinite.


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## Body

## 1. Introduction

The contamination of soil and groundwater attributed to the migration of municipal solid waste (MSW) leachate from dilute-and-disperse landfills has aroused much concern [1–3]. High content of dissolved organic matter (DOM) is present in the landfill leachate, which significantly affects the sorption and transport of various pollutants in soils [4–7], and adsorption of DOM onto clay minerals in soils is an important process in the natural environment. After soils were contaminated by landfill leachate, certain functional groups of DOM could form complex with clay minerals owing to the fine particle size, favorable microspores, and high sorption capacity [8, 9]. Thus, interactions of DOM from landfill leachate with clays could affect significantly the fate and reactivity of organic pollutants in soils [9, 10], such as HOCs. Besides, one of the traditional liners is geosynthetic clay liners (GCLs), consisting primarily of nature clays or processed clays [11]. Thus, clay minerals also play an important role in the persistence of organic pollutants in the liner.Montmorillonite and kaolinite are important constituents of the soil in South China and are the chief available components of the geosynthetic clay liners in many landfills. Most of clays are composed of silica tetrahedral sheet(s) and alumina octahedral sheet(s). Montmorillonite, a kind of bentonite, has a 2 : 1 T–O–T layer structure, with the basic units consisting of two silica tetrahedral sheets and one alumina octahedral sheet in center. Interlayer swelling occurs when it is exposed to water and exchangeable cations. Kaolinite has a 1 : 1 T–O layer structure, which is composed of units made up of a tetrahedral sheet and an octahedral sheet. However, there is no exchangeable cation, and only water molecules in the Kaolinite’s interlayer. Indeed, the lack of dilatability in its interlayer results in the difficulty in exchanging reaction with substances into interlayer.Pyrene, one of common mutagenic polycyclic aromatic hydrocarbons (PAHs) in polluted soil [12–14], is difficult to be decomposed in the environment [15, 16] and has been listed as one of sixteen kinds of PAHs priority pollutants by the US EPA. In addition, pyrene is a powerful hydrophobic substance with the l
o
g
K
o
w value of 5.18, which represents HOCs in this study.The clay soil interactions with DOM and the mechanism of DOM-clay complexes influencing the transport of HOCs in the soil contaminated by landfill leachate are not fully understood. A major obstacle for understanding these problems is the complexity of clay soil components. Hence, montmorillonite and kaolinite, two main components of the soil in South China, were chosen to investigate the soil contaminated by landfill leachate, which provides better insight into the mechanism of the binding of DOM with clay soil and the influence of the association of DOM with clays on the sorption of HOCs.The major mechanisms of the interactions of DOM with mineral oxide surfaces are H-bonding, ligand exchange, van der Waals interactions, water bridging, cation bridging, and so on [17–20]. Yang et al. also suggested that humic acids adsorption by nano-Al2O3 could be basically explained with a ligand exchange mechanism because of the protonated O
H
2
+ groups on the Al2O3 surface [10]. Besides, many works about pyrene sorption studies have been reported. Wang et al. reported that metal oxides (Al2O3, ZnO, and TiO2) had linear isotherms for sorption of pyrene [21]. “Partitioning” like sorption is the main mechanism for the sorption of pyrene onto the bare clays. Because inorganic mineral surfaces are typically covered in aqueous solution by a layer of chemically adsorbed water molecules overlain by additional physically adsorbed water molecules, creating ice-like “vicinal” water [22]. Pyrene molecules would not be localized at specific sorption sites on oxide surfaces rather than being in the vicinal water [21, 22]. Laegdsmand et al. who studied pyrene sorption to water-dispersible colloids under the effect of solution chemistry and organic matter found that the sorption data were described well using Freundlich isotherms and had different sorption isotherms between manured soil and depleted soil [23]. Laor et al. found that phenanthrene sorption by mineral-associated humic acid was dependent on both solution chemistry and characteristics of clays [24]. Polubesova et al. discovered that sorption and fractionation of DOM fractions by montmorillonite saturated with transition metals was important to surface controlled reactions in the retention of DOM and transport of organic colloids in soils [17]. Yang and Xing reported phenanthrene sorption by both nano-TiO2 and nano-ZnO was enhanced by coated humic acids [25]. However, the sorption of HOCs onto montmorillonite and kaolinite in the presence of DOM from landfill leachate has not been examined.In this work, characterization of the bare clays and their complexes with DOM was analyzed by various techniques. Sorption experiments were performed under different contact time, initial concentrations of pyrene, and temperatures. Certain sorption kinetic models and isotherms models were applied to describe the quantitative sorption processes. These fundamental data are useful to have a better understanding of the geochemical behavior of HOCs in the soil contaminated by landfill leachate.


## 2. Materials and Methods

### 2.1. Materials and Reagents

The montmorillonite used in this study was obtained from a bentonite deposit in Heping (Guangdong, PRC) and the kaolinite was from a natural kaolinite mine in the Tarim Basin (Xinjiang, PRC).DOM was extracted from the leachate of a landfill in Guangzhou (PRC) and mainly consisted of organic amine, aromatic acids, fatty acid, alcohols, phenols, and so on, as revealed by Yang and Zhou [26]. The steps of preparing DOM solution were as follows: the leachate was centrifuged for 10 min at 4000 r·min−1, and the supernatant was filtered through a 0.45 um membrane, then the DOM solution was obtained and stored at 277 K before use. The total organic carbon (TOC) concentration of DOM solution was determined by a Shimadzu TOC-500 analyzer and its initial concentration was determined as 19.83 g·L−1 (almost 20000 ppm).Pyrene (>98% purity) was purchased from Aldrich Chemical Company, USA. The molecular weight is 178.23 g·mol−1 and the solubility in the mixture of water and methanol (3 : 2, v/v) water is 1.18 mg·L−1 at 298 K. Methanol is chromatogram grade and the other reagents are analytical grade. Deionized water was used in the most of sorption experiments.Pyrene was dissolved in methanol with a typical concentration of 1000 mg·L−1 as stock solution and then diluted into the designated concentration standards in mobile phase to construct a calibration curve. Synthetic solutions were prepared by proper dilution in deionized water. In the sorption experiments, 0.005 mol·L−1 CaCl2 and 100 mg·L−1 NaN3 of the background solution were used to prevent dissolution of sorbed organic matter and inhibit microbiological degradation of pyrene, respectively.


### 2.2. Preparation of the DOM-Clay Complexes

The preparation of the DOM-clay complex was as follows: First, 1.00 g clay was added in 100 mL diluted DOM solution (the ratio of solid/liquid is 1 : 100) under vigorous stirring for 15 h at 308 K. The suspension pH was adjusted with 1.0 mol·L−1 NaOH solution or 1.0 mol·L−1 HCl solution. Then the mixture was aged for 30 min and centrifuged for 30 min at 4000 r·min−1. The sediment was washed for 3 times with deionized water, dried at 318 K, grounded to 200-mush, and named as CMT or CKL.


### 2.3. Sorption-Desorption Experiments

Batch sorption experiments were carried out in 50 mL Erlenmeyer flasks by mixing together the sample (MT, CMT, KL, and CKL) with the aqueous solution of pyrene. The flasks were agitated at 170 r·min−1 by a table concentrator, and constant temperature (25
±
1°C) was kept with the water bath for a known time interval (30 min). The mixture was then centrifuged at 4000 r·min−1 for 10 min and the concentration of pyrene remaining in the supernatant was determined by high performance liquid chromatography (HPLC). All batch sorption experiments were replicated.The desorption experiment was conducted as follows: After the sorption of pyrene, the suspension was centrifuged, and the solid was mixed with distilled water and agitated in the table concentrator [27]. The final suspension was centrifuged again (10 min) and the concentration of pyrene in the supernatant was determined by HPLC. In order to avoid the photodegradation of pyrene, the whole sorption-desorption experiments were conducted in the dark. Through preliminary experiments, the volatilization and photodegradation of pyrene were negligible.The equilibrium sorption quantityq
e (μg·g−1) and the desorption percentage D (%) were determined by the following expressions:(1)
q
e
=
V
o
C
o
-
C
e
1000
W
s
,
D
%
=
C
o
C
t
q
e
1000
W
s
×
100
%
,where V
o (mL) is the volume of pyrene solution and C
o and C
e (μg·g−1) are the initial concentration and equilibrium concentration, respectively. W
s (g) denotes the mass of clay and C
t denotes the concentration of pyrene after addition of distilled water with contact time.


### 2.4. Analytical Procedure

#### 2.4.1. Characterization of the Materials

The X-ray diffraction (XRD) patterns of the bare clays and the DOM-clay complexes were measured with a Rigaku D/MAX-IIIA X-ray diffractometer equipped with Cu Kα radiation.The dried DOM powder and the complexes spectra were recorded by the KBr pellet technique on a PerkinElmer 1725X Fourier transform infrared spectrometer.Thermogravimetry (TG) and differential scanning calorimetry (DSC) curves were obtained on a German NETZSCH TG209 and German NETZSCH DSC204C, respectively.The microstructure at external surface of samples was observed by a Hitachi S-4500 scanning electron microscopy (SEM).


#### 2.4.2. Reaction Solution Analysis

Pyrene was determined by high performance liquid chromatography (HPLC, Hitachi, L-2000) which consisted of a UV/vis detector at 254 nm and a reversed-phase column of Luna 5u C18. The methanol-ultrapure water mixture (90 : 10) was used at mobile flow rate of 1.0 mL·min−1 under isocratic conditions at 308 K. Samples of 20 μL were injected into the column by automatic sample handling system. The relative standard deviation for HPLC analysis was controlled within 2%.


## 2.1. Materials and Reagents

The montmorillonite used in this study was obtained from a bentonite deposit in Heping (Guangdong, PRC) and the kaolinite was from a natural kaolinite mine in the Tarim Basin (Xinjiang, PRC).DOM was extracted from the leachate of a landfill in Guangzhou (PRC) and mainly consisted of organic amine, aromatic acids, fatty acid, alcohols, phenols, and so on, as revealed by Yang and Zhou [26]. The steps of preparing DOM solution were as follows: the leachate was centrifuged for 10 min at 4000 r·min−1, and the supernatant was filtered through a 0.45 um membrane, then the DOM solution was obtained and stored at 277 K before use. The total organic carbon (TOC) concentration of DOM solution was determined by a Shimadzu TOC-500 analyzer and its initial concentration was determined as 19.83 g·L−1 (almost 20000 ppm).Pyrene (>98% purity) was purchased from Aldrich Chemical Company, USA. The molecular weight is 178.23 g·mol−1 and the solubility in the mixture of water and methanol (3 : 2, v/v) water is 1.18 mg·L−1 at 298 K. Methanol is chromatogram grade and the other reagents are analytical grade. Deionized water was used in the most of sorption experiments.Pyrene was dissolved in methanol with a typical concentration of 1000 mg·L−1 as stock solution and then diluted into the designated concentration standards in mobile phase to construct a calibration curve. Synthetic solutions were prepared by proper dilution in deionized water. In the sorption experiments, 0.005 mol·L−1 CaCl2 and 100 mg·L−1 NaN3 of the background solution were used to prevent dissolution of sorbed organic matter and inhibit microbiological degradation of pyrene, respectively.


## 2.2. Preparation of the DOM-Clay Complexes

The preparation of the DOM-clay complex was as follows: First, 1.00 g clay was added in 100 mL diluted DOM solution (the ratio of solid/liquid is 1 : 100) under vigorous stirring for 15 h at 308 K. The suspension pH was adjusted with 1.0 mol·L−1 NaOH solution or 1.0 mol·L−1 HCl solution. Then the mixture was aged for 30 min and centrifuged for 30 min at 4000 r·min−1. The sediment was washed for 3 times with deionized water, dried at 318 K, grounded to 200-mush, and named as CMT or CKL.


## 2.3. Sorption-Desorption Experiments

Batch sorption experiments were carried out in 50 mL Erlenmeyer flasks by mixing together the sample (MT, CMT, KL, and CKL) with the aqueous solution of pyrene. The flasks were agitated at 170 r·min−1 by a table concentrator, and constant temperature (25
±
1°C) was kept with the water bath for a known time interval (30 min). The mixture was then centrifuged at 4000 r·min−1 for 10 min and the concentration of pyrene remaining in the supernatant was determined by high performance liquid chromatography (HPLC). All batch sorption experiments were replicated.The desorption experiment was conducted as follows: After the sorption of pyrene, the suspension was centrifuged, and the solid was mixed with distilled water and agitated in the table concentrator [27]. The final suspension was centrifuged again (10 min) and the concentration of pyrene in the supernatant was determined by HPLC. In order to avoid the photodegradation of pyrene, the whole sorption-desorption experiments were conducted in the dark. Through preliminary experiments, the volatilization and photodegradation of pyrene were negligible.The equilibrium sorption quantityq
e (μg·g−1) and the desorption percentage D (%) were determined by the following expressions:(1)
q
e
=
V
o
C
o
-
C
e
1000
W
s
,
D
%
=
C
o
C
t
q
e
1000
W
s
×
100
%
,where V
o (mL) is the volume of pyrene solution and C
o and C
e (μg·g−1) are the initial concentration and equilibrium concentration, respectively. W
s (g) denotes the mass of clay and C
t denotes the concentration of pyrene after addition of distilled water with contact time.


## 2.4. Analytical Procedure

### 2.4.1. Characterization of the Materials

The X-ray diffraction (XRD) patterns of the bare clays and the DOM-clay complexes were measured with a Rigaku D/MAX-IIIA X-ray diffractometer equipped with Cu Kα radiation.The dried DOM powder and the complexes spectra were recorded by the KBr pellet technique on a PerkinElmer 1725X Fourier transform infrared spectrometer.Thermogravimetry (TG) and differential scanning calorimetry (DSC) curves were obtained on a German NETZSCH TG209 and German NETZSCH DSC204C, respectively.The microstructure at external surface of samples was observed by a Hitachi S-4500 scanning electron microscopy (SEM).


### 2.4.2. Reaction Solution Analysis

Pyrene was determined by high performance liquid chromatography (HPLC, Hitachi, L-2000) which consisted of a UV/vis detector at 254 nm and a reversed-phase column of Luna 5u C18. The methanol-ultrapure water mixture (90 : 10) was used at mobile flow rate of 1.0 mL·min−1 under isocratic conditions at 308 K. Samples of 20 μL were injected into the column by automatic sample handling system. The relative standard deviation for HPLC analysis was controlled within 2%.


## 2.4.1. Characterization of the Materials

The X-ray diffraction (XRD) patterns of the bare clays and the DOM-clay complexes were measured with a Rigaku D/MAX-IIIA X-ray diffractometer equipped with Cu Kα radiation.The dried DOM powder and the complexes spectra were recorded by the KBr pellet technique on a PerkinElmer 1725X Fourier transform infrared spectrometer.Thermogravimetry (TG) and differential scanning calorimetry (DSC) curves were obtained on a German NETZSCH TG209 and German NETZSCH DSC204C, respectively.The microstructure at external surface of samples was observed by a Hitachi S-4500 scanning electron microscopy (SEM).


## 2.4.2. Reaction Solution Analysis

Pyrene was determined by high performance liquid chromatography (HPLC, Hitachi, L-2000) which consisted of a UV/vis detector at 254 nm and a reversed-phase column of Luna 5u C18. The methanol-ultrapure water mixture (90 : 10) was used at mobile flow rate of 1.0 mL·min−1 under isocratic conditions at 308 K. Samples of 20 μL were injected into the column by automatic sample handling system. The relative standard deviation for HPLC analysis was controlled within 2%.


## 3. Results and Discussion

### 3.1. Sample Characterization

#### 3.1.1. X-Ray Diffraction and FTIR Spectra of Samples

The XRD results of the bare clays and their complexes are shown in Figure1. The d
001 reflection is the main source applied to identify clays. The d
001 reflection of MT was 1.55 nm, which represented a kind of Ca-montmorillonite [27]. The basal spacing of CMT increased slightly to 1.57 nm, indicating that some molecules of DOM are possibly intercalated into the interlayer. Further, the intensity was a bitweakened under the influence of DOM, which demonstrated the crystallinity decreased in the presence of DOM. A similar phenomenon was obtained by He et al. [28].Figure 1
XRD patterns of MT, CMT, KL, and CKL.However, the XRD patterns of kaolinite in the absence and the presence of DOM were different from that of montmorillonite cases. In the XRD patterns, thed
001 reflection of CKL was sharper and a higher order harmonics appeared. This suggested that the kaolinite in the presence of DOM could be in favor of a better crystallization. In addition, the d
001 basal spacing remained basically unchanged after the introduction of DOM. No DOM molecules but water can be intercalated into the interlayer since kaolinite is the least reactive clay and lack of dilatability in its interlayer. The lack of dilatability in the interlayer of kaolinite is closely related with its structure (1 : 1). The two sides (oxygen and hydroxyl) of the interlayer are linked tightly by hydrogen bond, which limitsthe dilatability.Figure2 shows the FTIR spectra of the bare clays and their complexes. In the presence of DOM, the CMT sample exhibited an OH stretching which shifted from 3427 cm−1 to 3441 cm−1 and showed a lower band near 3441 cm−1. It suggested some DOM molecules were bonding with the Ca-montmorillonite through water bridging [17], not mechanical superposition. In comparison to MT, the CMT sample showed a lower and broader band near 1644 cm−1, which demonstrated a diminution of water in the interlayer. As shown in Figure 2, a vibration mode at 1463 cm−1, attributed to the –CH2– or –CH3 bending mode, was observed in the spectrum of DOM, while it showed a new vibration mode at 1402 cm−1 in the spectrum of CMT. It could be inferred that some aliphatic hydrocarbon molecules from DOM were intercalated into the interlayer of montmorillonite. Similarly, Sutton and Sposito found that the DOM-montmorillonite complex featured significantly direct hydrophobic and H-bonding interactions between organic and mineral components using molecule simulation [29]. In contrast to the montmorillonite system, kaolinite is a nonexpanding clay mineral. FTIR signals of KL were identical to that of CKL, which indicated that no significant structural changes of kaolinite occurred in the absence and the presence of DOM. The result presented here agreed with those reported by Sachs and Bernhard [30], who studied the humic-kaolinite associate. In fact, the result of FTIR spectra was in accordance with the result of XRD patterns.Figure 2
FTIR spectra of the bare clays, their complexes, and the dried DOM powder.


#### 3.1.2. Morphology and Properties of Samples

Thermogravimetry (TG) is an important method for analyzing the thermal stability of sorbent and environments of the inserting molecules [31]. Generally, the decomposition of bare clays or organoclays consists of several steps including the following: adsorbed water and interlayer water desorption, dehydroxylation, surfactant desorption, and decomposition of clay structure [32–36]. The thermogravimetry and the differential scanning calorimetry (DSC) curves are shown in Figure 3. The MT sample showed two low-temperature decalescence peaks from 100 to 200°C, which is mostly due to the loss of adsorbed water and interlayer water [32] and the lost weight was 15.2% (Table 1). In comparison with MT, the DSC curve of CMT became smooth and slightly straight, without sharp decalescence peaks below 200°C. It was possible that the intercalation of DOM into the interlayer contributed to the reduction of interlayer water. This phenomenon was in agreement with the experiments performed by He et al. [37]. In the cases of kaolinite, there was no significant difference in TG curves in the absence and the presence of DOM. It is no more than 1% mass-loss which was assigned to the loss of humidity below 250°C. This was related to the moisture content of kaolinite samples. The dehydroxylation of KL sample was observed at 525.7°C and that of CKL shifted a little to 529.1°C [38]. An exothermic valley centered at 409°C attributed to the loss of organic matter from the kaolinite host [39].Table 1
TG results of samples (MT, CMT, KL, and CKL).
Samples
Temperature (°C)
Mass loss (%)
Reasons
CMT
179.0
2.7
Loss of humidity
MT
172.9
15.2
Loss of humidity
CKL
525.7
12.9
Dehydroxylation and loss of organic matter
KL
529.1
11.3
DehydroxylationFigure 3
TG (a) and DSC (b) curves of MT, CMT, KL, and CKL.
(a)
(b)SEM is applied to observe the changes in morphology of the bare clays compared to the organoclays, and the results are shown in Figure4. It was clear that MT sample had a tight and compact surface. Nevertheless, CMT sample appeared to be looser and changed into flocculent structure in the presence of DOM. The size of CMT colloids became smaller than the size of bare montmorillonite, which could significantly enhance the sorption capacity [40]. These two images (Figures 4(a) and 4(b)) present features which were similar to those previously reported for montmorillonite modified by petroleum organic compounds [39]. As shown in Figures 4(c) and 4(d), it revealed that the bare kaolin particles are clearly ball-like, and the matrix is filled with amorphous fuzzy materials [40]. However, few or no “ball” could be seen by the image of CMT sample, and the DOM-kaolinite complex transformed into network shape (Figure 4(d)). Meanwhile, this indicated a number of DOM molecules had adsorbed onto the surface of kaolinite sample. A similar phenomenon was observed for fulvic acid fractions on kaolinite [40].Figure 4
SEM images of MT (a), CMT (b), KL (c), and CKL (d).
(a)
(b)
(c)
(d)A possible reaction mechanism of the interfacial interactions between DOM and clays is shown in Figure5. In the case of montmorillonite, on one hand, a small amount of DOM molecules may be distributed in the interlayer field. Certain positively charged DOM groups could be intercalated into its interlayer through cation exchange, forming organic pillared montmorillonite, which could improve the sorption capacity. On the other hand, it was confirmed that there was an exchange of negatively charged DOM groups occurring on surface hydroxyl groups of montmorillonite silica surfaces [17], but the contribution of ligand exchange to sorption of DOM on the 2 : 1 layer type silicate was relatively small [41]. In contrast to the montmorillonite system, the DOM molecules were difficult to be intercalated into the interlayer field of kaolinite because the framework of interlayer is closed and no layer change is available. Thus, no DOM molecules could be intercalated into its interlayer. Nevertheless, there is an alumina octahedral sheet by exposure, which is full of hydroxyl on the surface, so carboxylate groups of DOM could interact with the alumina surface hydroxyl groups of kaolinite undergo ligand exchange [41]. Besides, the hydrophobic DOM-DOM interactions contributed to multiple adsorption of DOM on clays surfaces and went against the Langmuir model.Figure 5
Schematic representation of the interfacial interactions between clays and DOM.


### 3.2. Sorption-Desorption Experiments

#### 3.2.1. Sorption Kinetics

To test the rate of the sorption process and investigate the potential rate-controlling step, a series of sorption experiments at constant temperature was performed, the adsorptive capacity (q
t) was monitored, and several kinetic models were investigated.The sorption kinetics was tested by the following famous models, processed by nonlinear least squares fitting [42, 43] (NLSF) using data analysis and graphing software Origin Pro 8 (OriginLab Corporation, USA).(a)
Elovish equation [44, 45] is(2)
q
t
=
1
b
l
n
a
b
+
1
b
l
n
t
,
wheret is sorption time, q
t is the amounts sorbed per unit mass with time t, and a and b are sorption constant.
(b)
Pseudo-first-order model [46, 47] is (3)
q
t
=
q
e
1
-
e
x
p
-
k
1
t
,
whereq
e is the amounts sorbed per unit mass at equilibrium time and k
1 is the pseudo-first-order sorption rate constant.
(c)
Pseudo-second-order model [46, 47] is (4)
q
t
=
q
e
2
k
2
t
1
+
q
e
k
2
t
,
wherek
2 is the pseudo-first-order sorption rate constant. q
e
2
k
2 is described as the initial sorption rate as t to 0. This model is in agreement with chemical sorption being the rate-controlling step [48].The amount of pyrene sorbed on unit mass of samples (q
t) for various contact times at the initial concentration of 1000 ± 150 μg·L−1 are shown in Figure 6. The initial pH before sorption was 7.3. A little change of pH was observed after equilibrium in the preliminary experiment. At the beginning, the sorption of pyrene proceeded at a rapid rate as a large number of sorption sites were available. As the sorption sites were filled up gradually, sorption proceeded slowly and the kinetics became more dependent on the rate at which the sorption was transferred from the bulk phase to the actual sorption sites [49]. The efficiency of sorption was high with 20 min enough to nearly reach equilibrium and equilibrium was achieved after 30 min. Indeed, the sorption rate by MT was a bit slower than others in the first 20 min. The sorption capacity of CMT was nearly twice higher than MT, suggesting that DOM-montmorillonite complex was favorable toward promoting the sorption of pyrene. The fact that the sorption capacity of KL was obviously higher than MT may be related to the difference in hydrophobic nature of sorbents. There is substitution of Al3+ by Mg2+ in the octahedral sheet and of Si4+ by Al3+ in the tetrahedral sheet, which results in negative net charge in the interlayer of montmorillonite. However, there is no substitution in the layer of kaolinite, indicating that the net layer charge of kaolinite is zero. Therefore, the silica surface of bare kaolinite has stronger hydrophobic nature than that of bare montmorillonite. In the case of kaolinite, although many potential sorption sites on the bare kaolinite surface were reduced by the DOM coating, new sorption sites would be produced subsequently. As shown in Figure 6, there was minimal difference concerning sorption capacity between CKL and KL, indicating that the contribution of the new sorption sites for sorption capacity was nearly equivalent to the hydrophobicity of bare kaolinite.Figure 6
Effect of time on the sorption of pyrene by the bare clays and their complexes at 298 K.The fitting results of kinetics models, including the experimental and calculatedq
e values, rate constants (k), and coefficient of correlation coefficients (R
2), are given in Table 1. Obviously, the correlation coefficients for the Elovich model obtained by CMT, CKL, and KL were very low. It suggested that the sorption of pyrene did not follow Elovich model.The pseudo-first-order mode had correlation coefficients (R
2) in the range of 0.97 to 0.99 and the calculated q
e values agree well with the experimental q
e (Table 2). The pseudo-first-order sorption rate (k
1) lies between 0.61 and 1.32 min−1. K
f values were in the order of CMT > KL > CKL > MT. The kinetic data were also tested with respect to the pseudo-second-order model, as high value of the correlation coefficients and the calculated q
e values agreed well with the experimental q
e. Therefore, both models (pseudo-first-order and second-order) provided a good description of the sorption process; thus, the sorption can be described as a chemical-reaction-based process. A similar result was obtained by Valderrama et al. [50].Table 2
The coefficients of the kinetic models for sorption of pyrene at 298 K.
Sample
Elovich
Pseudo-first-order
Pseudo-second-order
Experimental
R
2
q
e
k
1
R
2
q
e
k
2  ×  103
R
2
q
e
CMT
0.152
38.63
1.32
0.98
38.69
4.18
0.99
38.96
MT
0.929
21.76
0.61
0.97
22.01
25.97
0.98
22.18
CKL
0.792
44.56
0.85
0.99
44.72
7.04
0.99
44.99
KL
0.774
41.95
1.01
0.98
42.01
4.86
0.99
42.00
Note. The units of k
1 and k
2 are, respectively, min−1 and g·μg−1min−1.


#### 3.2.2. Sorption Isotherms

Sorption isotherms are used to indicate the partition of adsorbate between solution and adsorbent at equilibrium [47]. Sorption isotherms were studied by operating a set of sorption experiments at constant temperature with different equilibrium concentrations of the adsorbate. The sorption isotherm was tested by the following models using NLSF.(i)
Henry isotherm, is usually used to describe the linear sorption process and its formula is(5)
q
e
=
K
D
C
e
,
whereC
e and q
e are the equilibrium concentrations of the adsorbate in the liquid and the solid phases, respectively; the K
D is the sorption distribution coefficient.
(ii)
Freundlich isotherm, is usually used to describe nonhomogeneous surface sorption process (an empirical sorption model) and its formula is(6)
q
e
=
K
f
C
e
n
,
whereK
f is Freundlich sorption coefficient, relating to the capacity and the intensity of sorption and n is Freundlich sorption index.For a series of initial concentrations of pyrene from 100μg·L−1 to 1000 μg·L−1, the q
e versus C
e isotherms for pyrene-samples interactions with a fixed adsorbent amount 20 g·L−1 at 298 K are shown in Figure 7. It was observed that the sorption isotherms of CKL and CMT had a similar feature. Obviously, CMT, CKL, and KL reached the equilibrium amount in solid phase at much lower equilibrium concentration in liquid phase than that of MT. In addition, the CMT, CKL, and KL had much higher uptake of pyrene compared to that of MT. Accordingly, saturation of sorption sites on MT had been attained with a much lower concentration of pyrene and the others with a much higher concentration of pyrene [51].Figure 7
Isothermal sorption plot of pyrene by the bare clays and their complexes at 298 K.The sorption data were analyzed by Henry and Freundlich models. The correlation coefficients (R
2) and other parameters are summarized in Table 3. Both the Henry isotherm and the Freundlich isotherm showed good fits to the isotherms data. Indeed, the sorption isotherms by the bare clays showed a relatively high value of R
2 for Henry model, whereas Freundlich model provided a better fit to the equilibrium data of sorption onto the complexes. Furthermore, the sorption intensity given by the Freundlich sorption index,n, approached 1.0 in the cases of bare clays, which further indicated the process of the sorption onto the bare clays well followed the linear model. The DOM molecules adsorbed onto clays contributed to the mineral surfaces covered by a layer of hydrophobic substance which contained aromatic content. The sorption of pyrene was likely related to this aromatic content on the complexes’ surfaces [52]. Besides, the role of the retention of pyrene on the complexes surfaces is not only dispersion, but also important of π-π interactions [50].Table 3
Parameters of Henry isotherm and Freundlich isotherm at 298 K.
Sorbents
Henry
Freundlich
K
D
R
2
K
f  ×  103
n
R
2
CMT
0.28
0.90
1.69
2.13
0.94
MT
0.16
0.98
30.67
1.33
0.96
CKL
0.26
0.88
0.16
2.61
0.92
KL
0.18
0.95
15.93
1.49
0.90
Note. The units of K
D and K
f are, respectively, L·g−1 and μg(
1
-
1
/
n
)·L1
/
n·g−1.


#### 3.2.3. Effect of the Different Temperatures

The temperature of the aqueous solution is a fundamental parameter in the sorption process. Figure8 represents the effect of temperature on the equilibrium amount of pyrene sorbed on unit mass of sorbents (q
e). The reaction temperature had a significant effect on the sorption, especially when sorbents were the complexes. Importantly, this figure revealed that the amount of pyrene sorbed onto the sorbents per unit mass of sorbents decreased as the temperature of the process increased from 298 to 318 K. Accordingly, pyrene sorbed onto CMT, MT, CKL, and KL was an exothermal process in the range from 298 K to 318 K.Figure 8
Effect of temperature on sorption capacity.


#### 3.2.4. Desorption of Pyrene

In order to test the stability of sorbents after sorption, desorption experiment was conducted after sorption experiment at 298 K. Figure9 shows the trend in desorption percentage of pyrene with different contact time. Desorption percentage was obtained by determining the rate of the amount of pyrene stripping from unit mass of samples to equilibrium sorption quantity (q
e). Desorption results showed that very little amounts of pyrene were desorbed from CMT, which indicated the binding of pyrene with the DOM-montmorillonite complex were strong [27]. Nevertheless, almost the same percentage of pyrene desorbed from KL and CKL, suggesting DOM had little effect on the binding of pyrene with kaolinite.Figure 9
Desorption plot of pyrene from the bare clays and their complexes at 298 K.


## 3.1. Sample Characterization

### 3.1.1. X-Ray Diffraction and FTIR Spectra of Samples

The XRD results of the bare clays and their complexes are shown in Figure1. The d
001 reflection is the main source applied to identify clays. The d
001 reflection of MT was 1.55 nm, which represented a kind of Ca-montmorillonite [27]. The basal spacing of CMT increased slightly to 1.57 nm, indicating that some molecules of DOM are possibly intercalated into the interlayer. Further, the intensity was a bitweakened under the influence of DOM, which demonstrated the crystallinity decreased in the presence of DOM. A similar phenomenon was obtained by He et al. [28].Figure 1
XRD patterns of MT, CMT, KL, and CKL.However, the XRD patterns of kaolinite in the absence and the presence of DOM were different from that of montmorillonite cases. In the XRD patterns, thed
001 reflection of CKL was sharper and a higher order harmonics appeared. This suggested that the kaolinite in the presence of DOM could be in favor of a better crystallization. In addition, the d
001 basal spacing remained basically unchanged after the introduction of DOM. No DOM molecules but water can be intercalated into the interlayer since kaolinite is the least reactive clay and lack of dilatability in its interlayer. The lack of dilatability in the interlayer of kaolinite is closely related with its structure (1 : 1). The two sides (oxygen and hydroxyl) of the interlayer are linked tightly by hydrogen bond, which limitsthe dilatability.Figure2 shows the FTIR spectra of the bare clays and their complexes. In the presence of DOM, the CMT sample exhibited an OH stretching which shifted from 3427 cm−1 to 3441 cm−1 and showed a lower band near 3441 cm−1. It suggested some DOM molecules were bonding with the Ca-montmorillonite through water bridging [17], not mechanical superposition. In comparison to MT, the CMT sample showed a lower and broader band near 1644 cm−1, which demonstrated a diminution of water in the interlayer. As shown in Figure 2, a vibration mode at 1463 cm−1, attributed to the –CH2– or –CH3 bending mode, was observed in the spectrum of DOM, while it showed a new vibration mode at 1402 cm−1 in the spectrum of CMT. It could be inferred that some aliphatic hydrocarbon molecules from DOM were intercalated into the interlayer of montmorillonite. Similarly, Sutton and Sposito found that the DOM-montmorillonite complex featured significantly direct hydrophobic and H-bonding interactions between organic and mineral components using molecule simulation [29]. In contrast to the montmorillonite system, kaolinite is a nonexpanding clay mineral. FTIR signals of KL were identical to that of CKL, which indicated that no significant structural changes of kaolinite occurred in the absence and the presence of DOM. The result presented here agreed with those reported by Sachs and Bernhard [30], who studied the humic-kaolinite associate. In fact, the result of FTIR spectra was in accordance with the result of XRD patterns.Figure 2
FTIR spectra of the bare clays, their complexes, and the dried DOM powder.


### 3.1.2. Morphology and Properties of Samples

Thermogravimetry (TG) is an important method for analyzing the thermal stability of sorbent and environments of the inserting molecules [31]. Generally, the decomposition of bare clays or organoclays consists of several steps including the following: adsorbed water and interlayer water desorption, dehydroxylation, surfactant desorption, and decomposition of clay structure [32–36]. The thermogravimetry and the differential scanning calorimetry (DSC) curves are shown in Figure 3. The MT sample showed two low-temperature decalescence peaks from 100 to 200°C, which is mostly due to the loss of adsorbed water and interlayer water [32] and the lost weight was 15.2% (Table 1). In comparison with MT, the DSC curve of CMT became smooth and slightly straight, without sharp decalescence peaks below 200°C. It was possible that the intercalation of DOM into the interlayer contributed to the reduction of interlayer water. This phenomenon was in agreement with the experiments performed by He et al. [37]. In the cases of kaolinite, there was no significant difference in TG curves in the absence and the presence of DOM. It is no more than 1% mass-loss which was assigned to the loss of humidity below 250°C. This was related to the moisture content of kaolinite samples. The dehydroxylation of KL sample was observed at 525.7°C and that of CKL shifted a little to 529.1°C [38]. An exothermic valley centered at 409°C attributed to the loss of organic matter from the kaolinite host [39].Table 1
TG results of samples (MT, CMT, KL, and CKL).
Samples
Temperature (°C)
Mass loss (%)
Reasons
CMT
179.0
2.7
Loss of humidity
MT
172.9
15.2
Loss of humidity
CKL
525.7
12.9
Dehydroxylation and loss of organic matter
KL
529.1
11.3
DehydroxylationFigure 3
TG (a) and DSC (b) curves of MT, CMT, KL, and CKL.
(a)
(b)SEM is applied to observe the changes in morphology of the bare clays compared to the organoclays, and the results are shown in Figure4. It was clear that MT sample had a tight and compact surface. Nevertheless, CMT sample appeared to be looser and changed into flocculent structure in the presence of DOM. The size of CMT colloids became smaller than the size of bare montmorillonite, which could significantly enhance the sorption capacity [40]. These two images (Figures 4(a) and 4(b)) present features which were similar to those previously reported for montmorillonite modified by petroleum organic compounds [39]. As shown in Figures 4(c) and 4(d), it revealed that the bare kaolin particles are clearly ball-like, and the matrix is filled with amorphous fuzzy materials [40]. However, few or no “ball” could be seen by the image of CMT sample, and the DOM-kaolinite complex transformed into network shape (Figure 4(d)). Meanwhile, this indicated a number of DOM molecules had adsorbed onto the surface of kaolinite sample. A similar phenomenon was observed for fulvic acid fractions on kaolinite [40].Figure 4
SEM images of MT (a), CMT (b), KL (c), and CKL (d).
(a)
(b)
(c)
(d)A possible reaction mechanism of the interfacial interactions between DOM and clays is shown in Figure5. In the case of montmorillonite, on one hand, a small amount of DOM molecules may be distributed in the interlayer field. Certain positively charged DOM groups could be intercalated into its interlayer through cation exchange, forming organic pillared montmorillonite, which could improve the sorption capacity. On the other hand, it was confirmed that there was an exchange of negatively charged DOM groups occurring on surface hydroxyl groups of montmorillonite silica surfaces [17], but the contribution of ligand exchange to sorption of DOM on the 2 : 1 layer type silicate was relatively small [41]. In contrast to the montmorillonite system, the DOM molecules were difficult to be intercalated into the interlayer field of kaolinite because the framework of interlayer is closed and no layer change is available. Thus, no DOM molecules could be intercalated into its interlayer. Nevertheless, there is an alumina octahedral sheet by exposure, which is full of hydroxyl on the surface, so carboxylate groups of DOM could interact with the alumina surface hydroxyl groups of kaolinite undergo ligand exchange [41]. Besides, the hydrophobic DOM-DOM interactions contributed to multiple adsorption of DOM on clays surfaces and went against the Langmuir model.Figure 5
Schematic representation of the interfacial interactions between clays and DOM.


## 3.1.1. X-Ray Diffraction and FTIR Spectra of Samples

The XRD results of the bare clays and their complexes are shown in Figure1. The d
001 reflection is the main source applied to identify clays. The d
001 reflection of MT was 1.55 nm, which represented a kind of Ca-montmorillonite [27]. The basal spacing of CMT increased slightly to 1.57 nm, indicating that some molecules of DOM are possibly intercalated into the interlayer. Further, the intensity was a bitweakened under the influence of DOM, which demonstrated the crystallinity decreased in the presence of DOM. A similar phenomenon was obtained by He et al. [28].Figure 1
XRD patterns of MT, CMT, KL, and CKL.However, the XRD patterns of kaolinite in the absence and the presence of DOM were different from that of montmorillonite cases. In the XRD patterns, thed
001 reflection of CKL was sharper and a higher order harmonics appeared. This suggested that the kaolinite in the presence of DOM could be in favor of a better crystallization. In addition, the d
001 basal spacing remained basically unchanged after the introduction of DOM. No DOM molecules but water can be intercalated into the interlayer since kaolinite is the least reactive clay and lack of dilatability in its interlayer. The lack of dilatability in the interlayer of kaolinite is closely related with its structure (1 : 1). The two sides (oxygen and hydroxyl) of the interlayer are linked tightly by hydrogen bond, which limitsthe dilatability.Figure2 shows the FTIR spectra of the bare clays and their complexes. In the presence of DOM, the CMT sample exhibited an OH stretching which shifted from 3427 cm−1 to 3441 cm−1 and showed a lower band near 3441 cm−1. It suggested some DOM molecules were bonding with the Ca-montmorillonite through water bridging [17], not mechanical superposition. In comparison to MT, the CMT sample showed a lower and broader band near 1644 cm−1, which demonstrated a diminution of water in the interlayer. As shown in Figure 2, a vibration mode at 1463 cm−1, attributed to the –CH2– or –CH3 bending mode, was observed in the spectrum of DOM, while it showed a new vibration mode at 1402 cm−1 in the spectrum of CMT. It could be inferred that some aliphatic hydrocarbon molecules from DOM were intercalated into the interlayer of montmorillonite. Similarly, Sutton and Sposito found that the DOM-montmorillonite complex featured significantly direct hydrophobic and H-bonding interactions between organic and mineral components using molecule simulation [29]. In contrast to the montmorillonite system, kaolinite is a nonexpanding clay mineral. FTIR signals of KL were identical to that of CKL, which indicated that no significant structural changes of kaolinite occurred in the absence and the presence of DOM. The result presented here agreed with those reported by Sachs and Bernhard [30], who studied the humic-kaolinite associate. In fact, the result of FTIR spectra was in accordance with the result of XRD patterns.Figure 2
FTIR spectra of the bare clays, their complexes, and the dried DOM powder.


## 3.1.2. Morphology and Properties of Samples

Thermogravimetry (TG) is an important method for analyzing the thermal stability of sorbent and environments of the inserting molecules [31]. Generally, the decomposition of bare clays or organoclays consists of several steps including the following: adsorbed water and interlayer water desorption, dehydroxylation, surfactant desorption, and decomposition of clay structure [32–36]. The thermogravimetry and the differential scanning calorimetry (DSC) curves are shown in Figure 3. The MT sample showed two low-temperature decalescence peaks from 100 to 200°C, which is mostly due to the loss of adsorbed water and interlayer water [32] and the lost weight was 15.2% (Table 1). In comparison with MT, the DSC curve of CMT became smooth and slightly straight, without sharp decalescence peaks below 200°C. It was possible that the intercalation of DOM into the interlayer contributed to the reduction of interlayer water. This phenomenon was in agreement with the experiments performed by He et al. [37]. In the cases of kaolinite, there was no significant difference in TG curves in the absence and the presence of DOM. It is no more than 1% mass-loss which was assigned to the loss of humidity below 250°C. This was related to the moisture content of kaolinite samples. The dehydroxylation of KL sample was observed at 525.7°C and that of CKL shifted a little to 529.1°C [38]. An exothermic valley centered at 409°C attributed to the loss of organic matter from the kaolinite host [39].Table 1
TG results of samples (MT, CMT, KL, and CKL).
Samples
Temperature (°C)
Mass loss (%)
Reasons
CMT
179.0
2.7
Loss of humidity
MT
172.9
15.2
Loss of humidity
CKL
525.7
12.9
Dehydroxylation and loss of organic matter
KL
529.1
11.3
DehydroxylationFigure 3
TG (a) and DSC (b) curves of MT, CMT, KL, and CKL.
(a)
(b)SEM is applied to observe the changes in morphology of the bare clays compared to the organoclays, and the results are shown in Figure4. It was clear that MT sample had a tight and compact surface. Nevertheless, CMT sample appeared to be looser and changed into flocculent structure in the presence of DOM. The size of CMT colloids became smaller than the size of bare montmorillonite, which could significantly enhance the sorption capacity [40]. These two images (Figures 4(a) and 4(b)) present features which were similar to those previously reported for montmorillonite modified by petroleum organic compounds [39]. As shown in Figures 4(c) and 4(d), it revealed that the bare kaolin particles are clearly ball-like, and the matrix is filled with amorphous fuzzy materials [40]. However, few or no “ball” could be seen by the image of CMT sample, and the DOM-kaolinite complex transformed into network shape (Figure 4(d)). Meanwhile, this indicated a number of DOM molecules had adsorbed onto the surface of kaolinite sample. A similar phenomenon was observed for fulvic acid fractions on kaolinite [40].Figure 4
SEM images of MT (a), CMT (b), KL (c), and CKL (d).
(a)
(b)
(c)
(d)A possible reaction mechanism of the interfacial interactions between DOM and clays is shown in Figure5. In the case of montmorillonite, on one hand, a small amount of DOM molecules may be distributed in the interlayer field. Certain positively charged DOM groups could be intercalated into its interlayer through cation exchange, forming organic pillared montmorillonite, which could improve the sorption capacity. On the other hand, it was confirmed that there was an exchange of negatively charged DOM groups occurring on surface hydroxyl groups of montmorillonite silica surfaces [17], but the contribution of ligand exchange to sorption of DOM on the 2 : 1 layer type silicate was relatively small [41]. In contrast to the montmorillonite system, the DOM molecules were difficult to be intercalated into the interlayer field of kaolinite because the framework of interlayer is closed and no layer change is available. Thus, no DOM molecules could be intercalated into its interlayer. Nevertheless, there is an alumina octahedral sheet by exposure, which is full of hydroxyl on the surface, so carboxylate groups of DOM could interact with the alumina surface hydroxyl groups of kaolinite undergo ligand exchange [41]. Besides, the hydrophobic DOM-DOM interactions contributed to multiple adsorption of DOM on clays surfaces and went against the Langmuir model.Figure 5
Schematic representation of the interfacial interactions between clays and DOM.


## 3.2. Sorption-Desorption Experiments

### 3.2.1. Sorption Kinetics

To test the rate of the sorption process and investigate the potential rate-controlling step, a series of sorption experiments at constant temperature was performed, the adsorptive capacity (q
t) was monitored, and several kinetic models were investigated.The sorption kinetics was tested by the following famous models, processed by nonlinear least squares fitting [42, 43] (NLSF) using data analysis and graphing software Origin Pro 8 (OriginLab Corporation, USA).(a)
Elovish equation [44, 45] is(2)
q
t
=
1
b
l
n
a
b
+
1
b
l
n
t
,
wheret is sorption time, q
t is the amounts sorbed per unit mass with time t, and a and b are sorption constant.
(b)
Pseudo-first-order model [46, 47] is (3)
q
t
=
q
e
1
-
e
x
p
-
k
1
t
,
whereq
e is the amounts sorbed per unit mass at equilibrium time and k
1 is the pseudo-first-order sorption rate constant.
(c)
Pseudo-second-order model [46, 47] is (4)
q
t
=
q
e
2
k
2
t
1
+
q
e
k
2
t
,
wherek
2 is the pseudo-first-order sorption rate constant. q
e
2
k
2 is described as the initial sorption rate as t to 0. This model is in agreement with chemical sorption being the rate-controlling step [48].The amount of pyrene sorbed on unit mass of samples (q
t) for various contact times at the initial concentration of 1000 ± 150 μg·L−1 are shown in Figure 6. The initial pH before sorption was 7.3. A little change of pH was observed after equilibrium in the preliminary experiment. At the beginning, the sorption of pyrene proceeded at a rapid rate as a large number of sorption sites were available. As the sorption sites were filled up gradually, sorption proceeded slowly and the kinetics became more dependent on the rate at which the sorption was transferred from the bulk phase to the actual sorption sites [49]. The efficiency of sorption was high with 20 min enough to nearly reach equilibrium and equilibrium was achieved after 30 min. Indeed, the sorption rate by MT was a bit slower than others in the first 20 min. The sorption capacity of CMT was nearly twice higher than MT, suggesting that DOM-montmorillonite complex was favorable toward promoting the sorption of pyrene. The fact that the sorption capacity of KL was obviously higher than MT may be related to the difference in hydrophobic nature of sorbents. There is substitution of Al3+ by Mg2+ in the octahedral sheet and of Si4+ by Al3+ in the tetrahedral sheet, which results in negative net charge in the interlayer of montmorillonite. However, there is no substitution in the layer of kaolinite, indicating that the net layer charge of kaolinite is zero. Therefore, the silica surface of bare kaolinite has stronger hydrophobic nature than that of bare montmorillonite. In the case of kaolinite, although many potential sorption sites on the bare kaolinite surface were reduced by the DOM coating, new sorption sites would be produced subsequently. As shown in Figure 6, there was minimal difference concerning sorption capacity between CKL and KL, indicating that the contribution of the new sorption sites for sorption capacity was nearly equivalent to the hydrophobicity of bare kaolinite.Figure 6
Effect of time on the sorption of pyrene by the bare clays and their complexes at 298 K.The fitting results of kinetics models, including the experimental and calculatedq
e values, rate constants (k), and coefficient of correlation coefficients (R
2), are given in Table 1. Obviously, the correlation coefficients for the Elovich model obtained by CMT, CKL, and KL were very low. It suggested that the sorption of pyrene did not follow Elovich model.The pseudo-first-order mode had correlation coefficients (R
2) in the range of 0.97 to 0.99 and the calculated q
e values agree well with the experimental q
e (Table 2). The pseudo-first-order sorption rate (k
1) lies between 0.61 and 1.32 min−1. K
f values were in the order of CMT > KL > CKL > MT. The kinetic data were also tested with respect to the pseudo-second-order model, as high value of the correlation coefficients and the calculated q
e values agreed well with the experimental q
e. Therefore, both models (pseudo-first-order and second-order) provided a good description of the sorption process; thus, the sorption can be described as a chemical-reaction-based process. A similar result was obtained by Valderrama et al. [50].Table 2
The coefficients of the kinetic models for sorption of pyrene at 298 K.
Sample
Elovich
Pseudo-first-order
Pseudo-second-order
Experimental
R
2
q
e
k
1
R
2
q
e
k
2  ×  103
R
2
q
e
CMT
0.152
38.63
1.32
0.98
38.69
4.18
0.99
38.96
MT
0.929
21.76
0.61
0.97
22.01
25.97
0.98
22.18
CKL
0.792
44.56
0.85
0.99
44.72
7.04
0.99
44.99
KL
0.774
41.95
1.01
0.98
42.01
4.86
0.99
42.00
Note. The units of k
1 and k
2 are, respectively, min−1 and g·μg−1min−1.


### 3.2.2. Sorption Isotherms

Sorption isotherms are used to indicate the partition of adsorbate between solution and adsorbent at equilibrium [47]. Sorption isotherms were studied by operating a set of sorption experiments at constant temperature with different equilibrium concentrations of the adsorbate. The sorption isotherm was tested by the following models using NLSF.(i)
Henry isotherm, is usually used to describe the linear sorption process and its formula is(5)
q
e
=
K
D
C
e
,
whereC
e and q
e are the equilibrium concentrations of the adsorbate in the liquid and the solid phases, respectively; the K
D is the sorption distribution coefficient.
(ii)
Freundlich isotherm, is usually used to describe nonhomogeneous surface sorption process (an empirical sorption model) and its formula is(6)
q
e
=
K
f
C
e
n
,
whereK
f is Freundlich sorption coefficient, relating to the capacity and the intensity of sorption and n is Freundlich sorption index.For a series of initial concentrations of pyrene from 100μg·L−1 to 1000 μg·L−1, the q
e versus C
e isotherms for pyrene-samples interactions with a fixed adsorbent amount 20 g·L−1 at 298 K are shown in Figure 7. It was observed that the sorption isotherms of CKL and CMT had a similar feature. Obviously, CMT, CKL, and KL reached the equilibrium amount in solid phase at much lower equilibrium concentration in liquid phase than that of MT. In addition, the CMT, CKL, and KL had much higher uptake of pyrene compared to that of MT. Accordingly, saturation of sorption sites on MT had been attained with a much lower concentration of pyrene and the others with a much higher concentration of pyrene [51].Figure 7
Isothermal sorption plot of pyrene by the bare clays and their complexes at 298 K.The sorption data were analyzed by Henry and Freundlich models. The correlation coefficients (R
2) and other parameters are summarized in Table 3. Both the Henry isotherm and the Freundlich isotherm showed good fits to the isotherms data. Indeed, the sorption isotherms by the bare clays showed a relatively high value of R
2 for Henry model, whereas Freundlich model provided a better fit to the equilibrium data of sorption onto the complexes. Furthermore, the sorption intensity given by the Freundlich sorption index,n, approached 1.0 in the cases of bare clays, which further indicated the process of the sorption onto the bare clays well followed the linear model. The DOM molecules adsorbed onto clays contributed to the mineral surfaces covered by a layer of hydrophobic substance which contained aromatic content. The sorption of pyrene was likely related to this aromatic content on the complexes’ surfaces [52]. Besides, the role of the retention of pyrene on the complexes surfaces is not only dispersion, but also important of π-π interactions [50].Table 3
Parameters of Henry isotherm and Freundlich isotherm at 298 K.
Sorbents
Henry
Freundlich
K
D
R
2
K
f  ×  103
n
R
2
CMT
0.28
0.90
1.69
2.13
0.94
MT
0.16
0.98
30.67
1.33
0.96
CKL
0.26
0.88
0.16
2.61
0.92
KL
0.18
0.95
15.93
1.49
0.90
Note. The units of K
D and K
f are, respectively, L·g−1 and μg(
1
-
1
/
n
)·L1
/
n·g−1.


### 3.2.3. Effect of the Different Temperatures

The temperature of the aqueous solution is a fundamental parameter in the sorption process. Figure8 represents the effect of temperature on the equilibrium amount of pyrene sorbed on unit mass of sorbents (q
e). The reaction temperature had a significant effect on the sorption, especially when sorbents were the complexes. Importantly, this figure revealed that the amount of pyrene sorbed onto the sorbents per unit mass of sorbents decreased as the temperature of the process increased from 298 to 318 K. Accordingly, pyrene sorbed onto CMT, MT, CKL, and KL was an exothermal process in the range from 298 K to 318 K.Figure 8
Effect of temperature on sorption capacity.


### 3.2.4. Desorption of Pyrene

In order to test the stability of sorbents after sorption, desorption experiment was conducted after sorption experiment at 298 K. Figure9 shows the trend in desorption percentage of pyrene with different contact time. Desorption percentage was obtained by determining the rate of the amount of pyrene stripping from unit mass of samples to equilibrium sorption quantity (q
e). Desorption results showed that very little amounts of pyrene were desorbed from CMT, which indicated the binding of pyrene with the DOM-montmorillonite complex were strong [27]. Nevertheless, almost the same percentage of pyrene desorbed from KL and CKL, suggesting DOM had little effect on the binding of pyrene with kaolinite.Figure 9
Desorption plot of pyrene from the bare clays and their complexes at 298 K.


## 3.2.1. Sorption Kinetics

To test the rate of the sorption process and investigate the potential rate-controlling step, a series of sorption experiments at constant temperature was performed, the adsorptive capacity (q
t) was monitored, and several kinetic models were investigated.The sorption kinetics was tested by the following famous models, processed by nonlinear least squares fitting [42, 43] (NLSF) using data analysis and graphing software Origin Pro 8 (OriginLab Corporation, USA).(a)
Elovish equation [44, 45] is(2)
q
t
=
1
b
l
n
a
b
+
1
b
l
n
t
,
wheret is sorption time, q
t is the amounts sorbed per unit mass with time t, and a and b are sorption constant.
(b)
Pseudo-first-order model [46, 47] is (3)
q
t
=
q
e
1
-
e
x
p
-
k
1
t
,
whereq
e is the amounts sorbed per unit mass at equilibrium time and k
1 is the pseudo-first-order sorption rate constant.
(c)
Pseudo-second-order model [46, 47] is (4)
q
t
=
q
e
2
k
2
t
1
+
q
e
k
2
t
,
wherek
2 is the pseudo-first-order sorption rate constant. q
e
2
k
2 is described as the initial sorption rate as t to 0. This model is in agreement with chemical sorption being the rate-controlling step [48].The amount of pyrene sorbed on unit mass of samples (q
t) for various contact times at the initial concentration of 1000 ± 150 μg·L−1 are shown in Figure 6. The initial pH before sorption was 7.3. A little change of pH was observed after equilibrium in the preliminary experiment. At the beginning, the sorption of pyrene proceeded at a rapid rate as a large number of sorption sites were available. As the sorption sites were filled up gradually, sorption proceeded slowly and the kinetics became more dependent on the rate at which the sorption was transferred from the bulk phase to the actual sorption sites [49]. The efficiency of sorption was high with 20 min enough to nearly reach equilibrium and equilibrium was achieved after 30 min. Indeed, the sorption rate by MT was a bit slower than others in the first 20 min. The sorption capacity of CMT was nearly twice higher than MT, suggesting that DOM-montmorillonite complex was favorable toward promoting the sorption of pyrene. The fact that the sorption capacity of KL was obviously higher than MT may be related to the difference in hydrophobic nature of sorbents. There is substitution of Al3+ by Mg2+ in the octahedral sheet and of Si4+ by Al3+ in the tetrahedral sheet, which results in negative net charge in the interlayer of montmorillonite. However, there is no substitution in the layer of kaolinite, indicating that the net layer charge of kaolinite is zero. Therefore, the silica surface of bare kaolinite has stronger hydrophobic nature than that of bare montmorillonite. In the case of kaolinite, although many potential sorption sites on the bare kaolinite surface were reduced by the DOM coating, new sorption sites would be produced subsequently. As shown in Figure 6, there was minimal difference concerning sorption capacity between CKL and KL, indicating that the contribution of the new sorption sites for sorption capacity was nearly equivalent to the hydrophobicity of bare kaolinite.Figure 6
Effect of time on the sorption of pyrene by the bare clays and their complexes at 298 K.The fitting results of kinetics models, including the experimental and calculatedq
e values, rate constants (k), and coefficient of correlation coefficients (R
2), are given in Table 1. Obviously, the correlation coefficients for the Elovich model obtained by CMT, CKL, and KL were very low. It suggested that the sorption of pyrene did not follow Elovich model.The pseudo-first-order mode had correlation coefficients (R
2) in the range of 0.97 to 0.99 and the calculated q
e values agree well with the experimental q
e (Table 2). The pseudo-first-order sorption rate (k
1) lies between 0.61 and 1.32 min−1. K
f values were in the order of CMT > KL > CKL > MT. The kinetic data were also tested with respect to the pseudo-second-order model, as high value of the correlation coefficients and the calculated q
e values agreed well with the experimental q
e. Therefore, both models (pseudo-first-order and second-order) provided a good description of the sorption process; thus, the sorption can be described as a chemical-reaction-based process. A similar result was obtained by Valderrama et al. [50].Table 2
The coefficients of the kinetic models for sorption of pyrene at 298 K.
Sample
Elovich
Pseudo-first-order
Pseudo-second-order
Experimental
R
2
q
e
k
1
R
2
q
e
k
2  ×  103
R
2
q
e
CMT
0.152
38.63
1.32
0.98
38.69
4.18
0.99
38.96
MT
0.929
21.76
0.61
0.97
22.01
25.97
0.98
22.18
CKL
0.792
44.56
0.85
0.99
44.72
7.04
0.99
44.99
KL
0.774
41.95
1.01
0.98
42.01
4.86
0.99
42.00
Note. The units of k
1 and k
2 are, respectively, min−1 and g·μg−1min−1.


## 3.2.2. Sorption Isotherms

Sorption isotherms are used to indicate the partition of adsorbate between solution and adsorbent at equilibrium [47]. Sorption isotherms were studied by operating a set of sorption experiments at constant temperature with different equilibrium concentrations of the adsorbate. The sorption isotherm was tested by the following models using NLSF.(i)
Henry isotherm, is usually used to describe the linear sorption process and its formula is(5)
q
e
=
K
D
C
e
,
whereC
e and q
e are the equilibrium concentrations of the adsorbate in the liquid and the solid phases, respectively; the K
D is the sorption distribution coefficient.
(ii)
Freundlich isotherm, is usually used to describe nonhomogeneous surface sorption process (an empirical sorption model) and its formula is(6)
q
e
=
K
f
C
e
n
,
whereK
f is Freundlich sorption coefficient, relating to the capacity and the intensity of sorption and n is Freundlich sorption index.For a series of initial concentrations of pyrene from 100μg·L−1 to 1000 μg·L−1, the q
e versus C
e isotherms for pyrene-samples interactions with a fixed adsorbent amount 20 g·L−1 at 298 K are shown in Figure 7. It was observed that the sorption isotherms of CKL and CMT had a similar feature. Obviously, CMT, CKL, and KL reached the equilibrium amount in solid phase at much lower equilibrium concentration in liquid phase than that of MT. In addition, the CMT, CKL, and KL had much higher uptake of pyrene compared to that of MT. Accordingly, saturation of sorption sites on MT had been attained with a much lower concentration of pyrene and the others with a much higher concentration of pyrene [51].Figure 7
Isothermal sorption plot of pyrene by the bare clays and their complexes at 298 K.The sorption data were analyzed by Henry and Freundlich models. The correlation coefficients (R
2) and other parameters are summarized in Table 3. Both the Henry isotherm and the Freundlich isotherm showed good fits to the isotherms data. Indeed, the sorption isotherms by the bare clays showed a relatively high value of R
2 for Henry model, whereas Freundlich model provided a better fit to the equilibrium data of sorption onto the complexes. Furthermore, the sorption intensity given by the Freundlich sorption index,n, approached 1.0 in the cases of bare clays, which further indicated the process of the sorption onto the bare clays well followed the linear model. The DOM molecules adsorbed onto clays contributed to the mineral surfaces covered by a layer of hydrophobic substance which contained aromatic content. The sorption of pyrene was likely related to this aromatic content on the complexes’ surfaces [52]. Besides, the role of the retention of pyrene on the complexes surfaces is not only dispersion, but also important of π-π interactions [50].Table 3
Parameters of Henry isotherm and Freundlich isotherm at 298 K.
Sorbents
Henry
Freundlich
K
D
R
2
K
f  ×  103
n
R
2
CMT
0.28
0.90
1.69
2.13
0.94
MT
0.16
0.98
30.67
1.33
0.96
CKL
0.26
0.88
0.16
2.61
0.92
KL
0.18
0.95
15.93
1.49
0.90
Note. The units of K
D and K
f are, respectively, L·g−1 and μg(
1
-
1
/
n
)·L1
/
n·g−1.


## 3.2.3. Effect of the Different Temperatures

The temperature of the aqueous solution is a fundamental parameter in the sorption process. Figure8 represents the effect of temperature on the equilibrium amount of pyrene sorbed on unit mass of sorbents (q
e). The reaction temperature had a significant effect on the sorption, especially when sorbents were the complexes. Importantly, this figure revealed that the amount of pyrene sorbed onto the sorbents per unit mass of sorbents decreased as the temperature of the process increased from 298 to 318 K. Accordingly, pyrene sorbed onto CMT, MT, CKL, and KL was an exothermal process in the range from 298 K to 318 K.Figure 8
Effect of temperature on sorption capacity.


## 3.2.4. Desorption of Pyrene

In order to test the stability of sorbents after sorption, desorption experiment was conducted after sorption experiment at 298 K. Figure9 shows the trend in desorption percentage of pyrene with different contact time. Desorption percentage was obtained by determining the rate of the amount of pyrene stripping from unit mass of samples to equilibrium sorption quantity (q
e). Desorption results showed that very little amounts of pyrene were desorbed from CMT, which indicated the binding of pyrene with the DOM-montmorillonite complex were strong [27]. Nevertheless, almost the same percentage of pyrene desorbed from KL and CKL, suggesting DOM had little effect on the binding of pyrene with kaolinite.Figure 9
Desorption plot of pyrene from the bare clays and their complexes at 298 K.


## 4. Conclusion

In this study, the interactions of DOM from landfill leachate with the clays were discussed and the sorption of pyrene onto the clays in the presence of DOM was investigated. The results of characterization indicated that the adsorption of DOM mainly occurred on the flat exposed planes of the silica and alumina sheets. A small amount of DOM molecules may be intercalated into the interlayer of montmorillonite, but no DOM molecules were intercalated into the interlayer of kaolinite. The changes in morphology of the clays surfaces were strongly affected by DOM, and especially the morphology of kaolinite particles transformed into network shape.The results of sorption-desorption experiments indicated the sorption isotherms of pyrene by the bare clays followed the Henry model well, whereas the isotherms by their complexes with DOM were well described by the Freundlich model. Association of DOM with montmorillonite would remarkably reduce the mobility of HOCs in the soil contaminated by landfill leachate than the bare ones. However, association of DOM with kaolinite did not affect significantly the retention of pyrene in comparison to the bare kaolinite. Therefore, montmorillonite played a more dominant role in the persistence of HOCs in the soil contaminated by landfill leachate than kaolinite.



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*Source: 734610-2015-08-12.xml*