# A Comparison Study of Mechanism: Cu2+ Adsorption on Different Adsorbents and Their Surface-Modified Adsorbents

Authors: Yaqin Yu; Xinrui Li; Jiemin Cheng
Journal: Journal of Chemistry
 (2016)

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## Abstract

The isothermal adsorption kinetics of Cu2+ onto Carbon Black (CB) and Oxidized Carbon Black (OCB) were studied under different solution conditions and compared with bentonite and organic bentonite with the hexadecyltrimethylammonium bromide (HDTMA). The adsorption capacities followed the order of OCB > CB > organic bentonite > bentonite, which was consistent with the orders of their surface roughness and specific surface area. The Fourier transmission infrared (FT-IR) spectroscopy, scanning electron microscopy (SEM), and transmission electron microscope (TEM) were used to explore the adsorption mechanism at molecular level. The adsorption process onto CB was physical adsorption. However, with the increase of oxygen-containing functional groups (C=O, C-O, and CNO), the chelation adsorption onto OCB became gradually dominant except physical adsorption. The ion exchange adsorption was the major adsorption mechanism of bentonite. The compounds were introduced into clay interlayer by complexing reaction with Cu2+, which improved the adsorption capacity of organic bentonite. The results present a significant implication for the environmental fate assessment of heavy metal pollution.


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## Body

## 1. Introduction

In recent decades, increased copper (Cu) contamination in soil has created a global concern [1]. It is known that prolonged exposure to Cu compounds can have negative impacts on organism, plants, and human health through the circulation of food chain [2–5]. The heavy metal contaminants are difficult to remove by biodegradation. Therefore, the protection and restoration of Cu2+ contaminated soils generate a great demand of developing novel remediation technologies.Chinese soil contaminants were difficult to remove because of their low concentration and complicated composition [6]. Compared with other techniques, adsorption is one of the best available treatment technologies for Cu2+ removal from soil, because it is simple, safe, easy to operate, and highly efficient. The most important criterion for adsorption technique is the selectivity of efficient adsorbents with high adsorption capacity and cost efficiency. The common adsorbents, such as activated carbon [7], dolomite [8], chitosan [9], and pomegranate peel [10], have been developed and expressed high-effective adsorption of heavy metal. However, there are quite few studies on their adsorption mechanism.The nanometer materials have the unique properties of huge specific surface and high-effective activity. Carbon Black (CB) is a typical nanomaterial, formed form the incomplete combustion of organism and fossil fuels [11, 12]. According to extensive studies, CB is a hydrophobic and nonpolar adsorbent and has strong adsorption ability for organic contaminants (including pesticides, phenanthrene, and cyclic amines) [13–16]. Concurrently, surface-modified CB has high adsorption capacity of heavy metals [17, 18]. However, its adsorption mechanism remains little known.Bentonite consists of two silica sheets’ sandwich and one water-aluminum layer. Recent studies have regarded it as a natural adsorbent with high adsorption capacity and ion exchange property [19]. Although the modified bentonite has high adsorption capacities of organics (including propylmercaptan, aroma compounds, and dye) [20, 21], it is less efficient for heavy metals. In addition, its reaction mechanism is not still adequately known. So the further exploration of its reaction mechanism is crucial for improvement of adsorption efficiency.In this study, we evaluated the adsorption potential of four adsorbents (CB, OCB, bentonite, and organic bentonite) for Cu2+ and further investigated the adsorption mechanisms of Cu2+ to different adsorbents on molecular scale. Batch adsorption experiments and related characterization techniques including Fourier transmission infrared (FT-IR) spectroscopy, scanning electron microscopy (SEM), and transmission electron microscope (TEM) were used to explore the adsorption mechanism. The results present an innovative material for developing remedy technology of heavy metal pollution.


## 2. Materials and Methods

### 2.1. Chemicals and Materials

Carbon Black (CB) was purchased from Jinan Tiancheng factory, mean particle size 30–60 nm. Table1 briefly overviews some properties of black carbon.Table 1
The properties of Carbon Black.
Property
Value
Test method
Heating loss/%
1
ISO 1126 [27]
Iodine number/(g⋅kg−1)
700–900
ISO 1304 [28]
Ash content/%
5–8
ISO 1125 [29]
Density/(kg⋅m−3)
340
ISO 1306 [30]
pH value
9.1
ASTM D 1512 [31]Bentonite was purchased from Shanghai Crystal Pure Biological Technology Co., Ltd., cation exchange capacity of 945 mmol·kg−1 and montmorillonite content of 85%. Chemicals used in the study are all analytic pure. Concentrated Nitrate Acid (65%) and Potassium Permanganate (KMnO4) were purchased from Tianjin Hongyan Chemical Reagent Factory; HDTMA was supplied from Tianjin Guangfu Chemical Research Institute; copper sulfate pentahydrate (CuSO4·5H2O) was obtained from Sinopharm Chemical Reagent Co., Ltd.


### 2.2. Preparation of Modified Adsorbents

Oxidized Carbon Black (OCB) was performed by oxidizing CB with concentrated nitrate acid and potassium permanganate. Briefly, 10 g CB was mixed with 110 mL acidic potassium permanganate solution in 250 mL conical beakers under the condition of water bath at 90°C for 3.0 h. Subsequently, the products were separated and washed with deionized water until the pH of filtrate remained at 5.5. After it dried in oven at 80°C for 7.0 h, the OCB were obtained.Organic Bentonite was prepared by suspension wet process, with 10% concentration of suspension and the following condition,WHDTMA : WBentonite = 1 : 2 (quality ration) and pH = 7. They were mixed in bath oscillator (90°C) for 2.5 h, and then the products were filtered. The solid was washed with deionized water to remove HDTMA and further dried at room temperature.


### 2.3. Batch Adsorption Experiments

#### 2.3.1. Adsorption Kinetics

Batch adsorption experiments of absorbing Cu2+ on the different adsorbents were conducted to compare the adsorption rate. The adsorption kinetics study of CB (OCB) was performed by adding 0.1 g sample and 20 mL 180 mg·L−1 Cu2+ solution in 100 mL vials. Then all vials were shaken at 25°C for 240 min. The adsorption kinetics study of bentonite (organic bentonite) was performed by mixing 0.2 g samples with 20 mL 80 mg·L−1 Cu2+ solution and was shaken at 25°C for 240 min.


#### 2.3.2. Adsorption Isotherms

First, 0.1 g CB (OCB) was mixed with 20 mL varying initial concentrations (20–180 mg·L−1) Cu2+ solution in 100 mL vials and shaken for 3.0 h. In addition, adsorption of bentonite (organic bentonite) was investigated by adding 0.2 g samples to 20 mL Cu2+ solution with varying initial concentrations (10–120 mg·L−1) at the desired pH. Then the mixtures were shaken for 2.0 h and future kept in incubator for 24 h at 25°C. Finally, the Cu2+ concentration was determined using an 800 atomic adsorption spectroscopy.


### 2.4. Characterization

The functional groups on the adsorbents were analyzed using Fourier transmission infrared spectroscopy (Fourier-380 FTIR, USA). The FTIR spectra were recorded in the 400–4000 cm−1 spectral range by using KBr pellet method with a Fourier-380 FTIR spectrometer at a standard resolution of ±2 cm−1. The surface morphology of the adsorbents was examined using a scanning electron microscopy (H-800 EM, Japan). The internal structure of CB, OCB, bentonite, and organic bentonite was examined using transmission electron microscope (H-800 EM, Japan).


### 2.5. Analysis of Data

All adsorption data were obtained in duplicate experiments. Two different isotherm models were employed to fit the adsorption equilibrium isotherm:Langmuir model:(1)qe=KLqmaxCe1+KLCe.Freundlich model:(2)qe=KfCe1/n,where qe (mg·g−1) is the adsorption amount of Cu2+; Ce (mg·L−1) is the adsorption equilibrium concentration of Cu2+; qmax (mg·g−1) is the maximum adsorption capacity; KL (L·mg−1) is the Langmuir adsorption affinity constant; Kf and n are the Freundlich adsorption constants representing the adsorption capacity and the adsorption intensity, respectively.


## 2.1. Chemicals and Materials

Carbon Black (CB) was purchased from Jinan Tiancheng factory, mean particle size 30–60 nm. Table1 briefly overviews some properties of black carbon.Table 1
The properties of Carbon Black.
Property
Value
Test method
Heating loss/%
1
ISO 1126 [27]
Iodine number/(g⋅kg−1)
700–900
ISO 1304 [28]
Ash content/%
5–8
ISO 1125 [29]
Density/(kg⋅m−3)
340
ISO 1306 [30]
pH value
9.1
ASTM D 1512 [31]Bentonite was purchased from Shanghai Crystal Pure Biological Technology Co., Ltd., cation exchange capacity of 945 mmol·kg−1 and montmorillonite content of 85%. Chemicals used in the study are all analytic pure. Concentrated Nitrate Acid (65%) and Potassium Permanganate (KMnO4) were purchased from Tianjin Hongyan Chemical Reagent Factory; HDTMA was supplied from Tianjin Guangfu Chemical Research Institute; copper sulfate pentahydrate (CuSO4·5H2O) was obtained from Sinopharm Chemical Reagent Co., Ltd.


## 2.2. Preparation of Modified Adsorbents

Oxidized Carbon Black (OCB) was performed by oxidizing CB with concentrated nitrate acid and potassium permanganate. Briefly, 10 g CB was mixed with 110 mL acidic potassium permanganate solution in 250 mL conical beakers under the condition of water bath at 90°C for 3.0 h. Subsequently, the products were separated and washed with deionized water until the pH of filtrate remained at 5.5. After it dried in oven at 80°C for 7.0 h, the OCB were obtained.Organic Bentonite was prepared by suspension wet process, with 10% concentration of suspension and the following condition,WHDTMA : WBentonite = 1 : 2 (quality ration) and pH = 7. They were mixed in bath oscillator (90°C) for 2.5 h, and then the products were filtered. The solid was washed with deionized water to remove HDTMA and further dried at room temperature.


## 2.3. Batch Adsorption Experiments

### 2.3.1. Adsorption Kinetics

Batch adsorption experiments of absorbing Cu2+ on the different adsorbents were conducted to compare the adsorption rate. The adsorption kinetics study of CB (OCB) was performed by adding 0.1 g sample and 20 mL 180 mg·L−1 Cu2+ solution in 100 mL vials. Then all vials were shaken at 25°C for 240 min. The adsorption kinetics study of bentonite (organic bentonite) was performed by mixing 0.2 g samples with 20 mL 80 mg·L−1 Cu2+ solution and was shaken at 25°C for 240 min.


### 2.3.2. Adsorption Isotherms

First, 0.1 g CB (OCB) was mixed with 20 mL varying initial concentrations (20–180 mg·L−1) Cu2+ solution in 100 mL vials and shaken for 3.0 h. In addition, adsorption of bentonite (organic bentonite) was investigated by adding 0.2 g samples to 20 mL Cu2+ solution with varying initial concentrations (10–120 mg·L−1) at the desired pH. Then the mixtures were shaken for 2.0 h and future kept in incubator for 24 h at 25°C. Finally, the Cu2+ concentration was determined using an 800 atomic adsorption spectroscopy.


## 2.3.1. Adsorption Kinetics

Batch adsorption experiments of absorbing Cu2+ on the different adsorbents were conducted to compare the adsorption rate. The adsorption kinetics study of CB (OCB) was performed by adding 0.1 g sample and 20 mL 180 mg·L−1 Cu2+ solution in 100 mL vials. Then all vials were shaken at 25°C for 240 min. The adsorption kinetics study of bentonite (organic bentonite) was performed by mixing 0.2 g samples with 20 mL 80 mg·L−1 Cu2+ solution and was shaken at 25°C for 240 min.


## 2.3.2. Adsorption Isotherms

First, 0.1 g CB (OCB) was mixed with 20 mL varying initial concentrations (20–180 mg·L−1) Cu2+ solution in 100 mL vials and shaken for 3.0 h. In addition, adsorption of bentonite (organic bentonite) was investigated by adding 0.2 g samples to 20 mL Cu2+ solution with varying initial concentrations (10–120 mg·L−1) at the desired pH. Then the mixtures were shaken for 2.0 h and future kept in incubator for 24 h at 25°C. Finally, the Cu2+ concentration was determined using an 800 atomic adsorption spectroscopy.


## 2.4. Characterization

The functional groups on the adsorbents were analyzed using Fourier transmission infrared spectroscopy (Fourier-380 FTIR, USA). The FTIR spectra were recorded in the 400–4000 cm−1 spectral range by using KBr pellet method with a Fourier-380 FTIR spectrometer at a standard resolution of ±2 cm−1. The surface morphology of the adsorbents was examined using a scanning electron microscopy (H-800 EM, Japan). The internal structure of CB, OCB, bentonite, and organic bentonite was examined using transmission electron microscope (H-800 EM, Japan).


## 2.5. Analysis of Data

All adsorption data were obtained in duplicate experiments. Two different isotherm models were employed to fit the adsorption equilibrium isotherm:Langmuir model:(1)qe=KLqmaxCe1+KLCe.Freundlich model:(2)qe=KfCe1/n,where qe (mg·g−1) is the adsorption amount of Cu2+; Ce (mg·L−1) is the adsorption equilibrium concentration of Cu2+; qmax (mg·g−1) is the maximum adsorption capacity; KL (L·mg−1) is the Langmuir adsorption affinity constant; Kf and n are the Freundlich adsorption constants representing the adsorption capacity and the adsorption intensity, respectively.


## 3. Results and Discussion

### 3.1. Adsorption Kinetic Studies

The adsorption kinetic curves of Cu2+ on CB, OCB, bentonite, and organic bentonite at 25°C show similar features (Figure 1). The adsorption process of four materials is at the fast reaction stage at first, and slowed down with time. The adsorption kinetics of Cu2+ by CB and OCB are rapid for the first 40 min and then gradually reach equilibrium in about 70 min. Similarly, the adsorption kinetics of Cu2+ by bentonite and organic bentonite are rapid for the first 10 min and then gradually reach equilibrium in about 20 min. As shown, the adsorption capacities follow the order of OCB > CB > organic bentonite > bentonite.Figure 1
Adsorption kinetics for Cu2+ adsorption on (a) OCB, (b) CB, (c) organic bentonite, and (d) bentonite as a function of reaction time.Figure2 shows the data fitted with the mass transfer model. The R2 values obtained using the pseudo first-order model and the pseudo second-order model are bigger than the first-order model and the second-order model. Compared with other models, the pseudo first-order model and the pseudo second-order model are better-fit. Table 2 indicates that the adsorption kinetics for Cu2+ on all materials follow the pseudo second-order model with higher R2 (0.982–0.999), but the maximum uptake values differ. Thus, the conclusion further confirmed the phenomenon in Figure 1. Currently, it had been demonstrated that the pseudo second-order model was applied to describe chemisorption [22], but it was limited by adsorbent surface properties, adsorbate ions, and pH. The k2 values follow the order of organic bentonite > bentonite > CB > OCB, which present the adsorption rate.Table 2
Parameters of adsorption kinetics model of Cu(II) on CB and bentonite.
Number
Treatment
Pseudo first-order model
Pseudo second-order model
q
1
e (mg/g)
k
1 (1/min)
R
2
q
2
e (mg/g)
k
2 (g/mgL⋅min)
R
2
a
CB
12.265
0.061
0.989
12.628
0.016
0.982
b
OCB
20.053
0.055
0.940
20.877
0.007
0.998
c
Bentonite
10.473
0.097
0.893
10.534
0.113
0.999
d
Organic bentonite
11.185
0.112
0.872
11.213
0.244
0.999Figure 2
Four kinetic models for the adsorption of Cu2+ by OCB, CB, organic bentonite, and bentonite. The solid line is the fit to the four order models: (a) the first-order model, (b) the second-order model, (c) the pseudo first-order model, and (d) the pseudo second-order model.
(a)
(b)
(c)
(d)


### 3.2. Adsorption Isotherms Studies

The adsorption of Cu2+ by the four adsorbents was studied in the batch mode at 25°C. The adsorption isotherms for the four adsorbents were nonlinear, and the maximum uptake values differ (Figure 3). The adsorption amounts of Cu2+ of the four materials increase rapidly in the low concentration range and then increase gradually as the initial concentrations increase.Figure 3
Sorption isotherms for the adsorption of Cu2+ by CB, OCB, bentonite, and organic bentonite.
(a)
(b)The equilibrium adsorption isotherm data and related isotherm parameters were analyzed using both Langmuir and Freundlich isotherm (Table3). The correlation coefficient (R2) values demonstrate that the Langmuir model is more suitable than the Freundlich model, except for OCB. These results indicate that the adsorption mechanisms of Cu2+ on these adsorbents are different. The adsorption process of CB, bentonite, and organic bentonite is surface adsorption. Ion exchange adsorption is the main adsorption mechanism of bentonite and organic bentonite, which have exchangeable cations. However, the adsorption mechanism of OCB is chelation in addition to surface adsorption. The maximum adsorption capacity follows the order of OCB > CB > organic bentonite > bentonite, consistent with surface area and oxygen-containing functional groups.Table 3
Parameters for adsorption isotherm of Cu(II) on CB and bentonite.
Number
Treatment
Langmuir
Freundlich
q
m
a
x (mg/g)
K
L (L/mg)
R
2
K
F (mg/g) (L/mg)1/n
1
/
n
R
2
a
CB
16.507
0.021
0.995
1.229
0.507
0.995
b
OCB
23.419
0.091
0.963
4.427
0.379
0.992
c
Bentonite
7.059
0.578
0.972
3.686
0.468
0.924
d
Organic bentonite
11.168
0.098
0.976
1.209
0.645
0.799


### 3.3. Properties of Different Adsorbents

The physicochemical properties of different adsorbents are shown in Table4. CB and bentonite are alkaline in nature, while surface modification results in the decreasing of pH. The specific surface area follows the order of OCB > CB > organic bentonite > bentonite, which further demonstrates the previous conclusion. Compared with bentonite, the negative charge amount of organic bentonite decreases, which is inconsistent with the adsorption capacity. That is because the organic compounds introduced in clay interlayer occur as complexing reaction with heavy metal ions in addition to exchange adsorption [23].Table 4
Characteristics of different adsorbents.
Number
Treatment
pH
Surface area (m2⋅g−1)
Zeta potential
a
CB
9.1
931.33
−6.06
b
OCB
6.0
1114.23
−17.18
c
Bentonite
10.2
9.54
−17.50
d
Organic bentonite
8.3
10.67
−9.46


#### 3.3.1. IR Analysis

FTIR spectra of CB, OCB, bentonite, and organic bentonite were recorded in the 400–4000 cm−1 spectral range by using KBr pellet method with a Fourier-380 FTIR spectrometer, and the results are shown in Figure 4. An O-H stretching band at 3450 cm−1 and a C=C stretching band at 1619 cm−1 were typical functional group of CB. Compared with CB, both bands not only were reserved but also became much more in OCB. The bands at 1721.6 and 1244.0 cm−1 can be assigned to the C=O and C-O stretching vibrations, respectively. The band at 447.3 cm−1 can be assigned to the CNO bending vibration. All these oxygen-containing functional groups chelating with heavy metal ion were absent in CB.Figure 4
IR spectrum of different adsorbents. (a) CB, (b) OCB, (c) bentonite, and (d) organic bentonite.The bands at 3622 and 3693 cm−1 can be assigned to the Al-Al-OH and Al-Mg-OH stretching vibration, respectively, which were typical groups of bentonite [24]. A broad band at 1115–996 cm−1 region was assigned to the Si-O stretching vibration, whereas a band at 516 cm−1 was assigned to the Si-O bending vibration. Compared with natural bentonite, a pair of bands at 2919 and 2849 cm−1 in organic bentonite was assigned to the symmetric and asymmetric C-H stretching vibrations of methyl and methylene groups. And a band at 1467 cm−1 was assigned to the asymmetric C-H bending vibration. These bands suggested the presence of cationic surfactants in the bentonite.


#### 3.3.2. SEM Characterization

To investigate the surface morphology, SEM (H-800 EM, Japan) analysis was performed on the different adsorbents (Figure5). The photographs of CB suggest sphere with diameter of 50–60 nm, which demonstrates nanoscale material. However, OCB had no obvious variation in shape and need to be further studied by TEM. In Figures 5(a) and 5(b), both materials suggest the serious aggregation of nanoparticles.Figure 5
Representative SEM images of different adsorbents. (a) CB (scale bar is 600 nm), (b) OCB (scale bar is 600 nm), (c) bentonite (scale bar is 6μm), and (d) organic bentonite (scale bar is 6 μm).
(a)
(b)
(c)
(d)The SEM images of bentonite and organic bentonite are shown in Figures5(c) and 5(d). The morphology of bentonite suggests smooth surface with flat crystal. Compared with natural bentonite, the clay lattice of organic bentonite appeared swollen and fluffy. This might be due to the organic compounds introduced in clay interlayer, which increase the basal spacing of clay [25]. The surface structure and porous characteristics are conductive to accelerate the spread of heavy metal ions in bentonite [26].


#### 3.3.3. TEM Characterization

The TEM photographs of different adsorbents are shown in Figure6. The photographs of CB suggest two components of solid and hollow sphere. Compared with CB, the OCB shows a lot of pores, which further suggests that the surface area increases. In addition, it demonstrates that CB is oxidized, which is beneficial to chelate with heavy metal ions.Figure 6
Representative TEM images of different adsorbents. (a) CB (scale bar is 250 nm), (b) OCB (scale bar is 250 nm), (c) bentonite (scale bar is 799 nm), and (d) organic bentonite (scale bar is 799 nm).
(a)
(b)
(c)
(d)As shown in Figures6(c) and 6(d), bentonite is amorphous in structure without aggregation. The photographs of organic bentonite show some pores and blurry edges, further suggesting that the morphological structure changes by intercalation of organic compounds.


## 3.1. Adsorption Kinetic Studies

The adsorption kinetic curves of Cu2+ on CB, OCB, bentonite, and organic bentonite at 25°C show similar features (Figure 1). The adsorption process of four materials is at the fast reaction stage at first, and slowed down with time. The adsorption kinetics of Cu2+ by CB and OCB are rapid for the first 40 min and then gradually reach equilibrium in about 70 min. Similarly, the adsorption kinetics of Cu2+ by bentonite and organic bentonite are rapid for the first 10 min and then gradually reach equilibrium in about 20 min. As shown, the adsorption capacities follow the order of OCB > CB > organic bentonite > bentonite.Figure 1
Adsorption kinetics for Cu2+ adsorption on (a) OCB, (b) CB, (c) organic bentonite, and (d) bentonite as a function of reaction time.Figure2 shows the data fitted with the mass transfer model. The R2 values obtained using the pseudo first-order model and the pseudo second-order model are bigger than the first-order model and the second-order model. Compared with other models, the pseudo first-order model and the pseudo second-order model are better-fit. Table 2 indicates that the adsorption kinetics for Cu2+ on all materials follow the pseudo second-order model with higher R2 (0.982–0.999), but the maximum uptake values differ. Thus, the conclusion further confirmed the phenomenon in Figure 1. Currently, it had been demonstrated that the pseudo second-order model was applied to describe chemisorption [22], but it was limited by adsorbent surface properties, adsorbate ions, and pH. The k2 values follow the order of organic bentonite > bentonite > CB > OCB, which present the adsorption rate.Table 2
Parameters of adsorption kinetics model of Cu(II) on CB and bentonite.
Number
Treatment
Pseudo first-order model
Pseudo second-order model
q
1
e (mg/g)
k
1 (1/min)
R
2
q
2
e (mg/g)
k
2 (g/mgL⋅min)
R
2
a
CB
12.265
0.061
0.989
12.628
0.016
0.982
b
OCB
20.053
0.055
0.940
20.877
0.007
0.998
c
Bentonite
10.473
0.097
0.893
10.534
0.113
0.999
d
Organic bentonite
11.185
0.112
0.872
11.213
0.244
0.999Figure 2
Four kinetic models for the adsorption of Cu2+ by OCB, CB, organic bentonite, and bentonite. The solid line is the fit to the four order models: (a) the first-order model, (b) the second-order model, (c) the pseudo first-order model, and (d) the pseudo second-order model.
(a)
(b)
(c)
(d)


## 3.2. Adsorption Isotherms Studies

The adsorption of Cu2+ by the four adsorbents was studied in the batch mode at 25°C. The adsorption isotherms for the four adsorbents were nonlinear, and the maximum uptake values differ (Figure 3). The adsorption amounts of Cu2+ of the four materials increase rapidly in the low concentration range and then increase gradually as the initial concentrations increase.Figure 3
Sorption isotherms for the adsorption of Cu2+ by CB, OCB, bentonite, and organic bentonite.
(a)
(b)The equilibrium adsorption isotherm data and related isotherm parameters were analyzed using both Langmuir and Freundlich isotherm (Table3). The correlation coefficient (R2) values demonstrate that the Langmuir model is more suitable than the Freundlich model, except for OCB. These results indicate that the adsorption mechanisms of Cu2+ on these adsorbents are different. The adsorption process of CB, bentonite, and organic bentonite is surface adsorption. Ion exchange adsorption is the main adsorption mechanism of bentonite and organic bentonite, which have exchangeable cations. However, the adsorption mechanism of OCB is chelation in addition to surface adsorption. The maximum adsorption capacity follows the order of OCB > CB > organic bentonite > bentonite, consistent with surface area and oxygen-containing functional groups.Table 3
Parameters for adsorption isotherm of Cu(II) on CB and bentonite.
Number
Treatment
Langmuir
Freundlich
q
m
a
x (mg/g)
K
L (L/mg)
R
2
K
F (mg/g) (L/mg)1/n
1
/
n
R
2
a
CB
16.507
0.021
0.995
1.229
0.507
0.995
b
OCB
23.419
0.091
0.963
4.427
0.379
0.992
c
Bentonite
7.059
0.578
0.972
3.686
0.468
0.924
d
Organic bentonite
11.168
0.098
0.976
1.209
0.645
0.799


## 3.3. Properties of Different Adsorbents

The physicochemical properties of different adsorbents are shown in Table4. CB and bentonite are alkaline in nature, while surface modification results in the decreasing of pH. The specific surface area follows the order of OCB > CB > organic bentonite > bentonite, which further demonstrates the previous conclusion. Compared with bentonite, the negative charge amount of organic bentonite decreases, which is inconsistent with the adsorption capacity. That is because the organic compounds introduced in clay interlayer occur as complexing reaction with heavy metal ions in addition to exchange adsorption [23].Table 4
Characteristics of different adsorbents.
Number
Treatment
pH
Surface area (m2⋅g−1)
Zeta potential
a
CB
9.1
931.33
−6.06
b
OCB
6.0
1114.23
−17.18
c
Bentonite
10.2
9.54
−17.50
d
Organic bentonite
8.3
10.67
−9.46


### 3.3.1. IR Analysis

FTIR spectra of CB, OCB, bentonite, and organic bentonite were recorded in the 400–4000 cm−1 spectral range by using KBr pellet method with a Fourier-380 FTIR spectrometer, and the results are shown in Figure 4. An O-H stretching band at 3450 cm−1 and a C=C stretching band at 1619 cm−1 were typical functional group of CB. Compared with CB, both bands not only were reserved but also became much more in OCB. The bands at 1721.6 and 1244.0 cm−1 can be assigned to the C=O and C-O stretching vibrations, respectively. The band at 447.3 cm−1 can be assigned to the CNO bending vibration. All these oxygen-containing functional groups chelating with heavy metal ion were absent in CB.Figure 4
IR spectrum of different adsorbents. (a) CB, (b) OCB, (c) bentonite, and (d) organic bentonite.The bands at 3622 and 3693 cm−1 can be assigned to the Al-Al-OH and Al-Mg-OH stretching vibration, respectively, which were typical groups of bentonite [24]. A broad band at 1115–996 cm−1 region was assigned to the Si-O stretching vibration, whereas a band at 516 cm−1 was assigned to the Si-O bending vibration. Compared with natural bentonite, a pair of bands at 2919 and 2849 cm−1 in organic bentonite was assigned to the symmetric and asymmetric C-H stretching vibrations of methyl and methylene groups. And a band at 1467 cm−1 was assigned to the asymmetric C-H bending vibration. These bands suggested the presence of cationic surfactants in the bentonite.


### 3.3.2. SEM Characterization

To investigate the surface morphology, SEM (H-800 EM, Japan) analysis was performed on the different adsorbents (Figure5). The photographs of CB suggest sphere with diameter of 50–60 nm, which demonstrates nanoscale material. However, OCB had no obvious variation in shape and need to be further studied by TEM. In Figures 5(a) and 5(b), both materials suggest the serious aggregation of nanoparticles.Figure 5
Representative SEM images of different adsorbents. (a) CB (scale bar is 600 nm), (b) OCB (scale bar is 600 nm), (c) bentonite (scale bar is 6μm), and (d) organic bentonite (scale bar is 6 μm).
(a)
(b)
(c)
(d)The SEM images of bentonite and organic bentonite are shown in Figures5(c) and 5(d). The morphology of bentonite suggests smooth surface with flat crystal. Compared with natural bentonite, the clay lattice of organic bentonite appeared swollen and fluffy. This might be due to the organic compounds introduced in clay interlayer, which increase the basal spacing of clay [25]. The surface structure and porous characteristics are conductive to accelerate the spread of heavy metal ions in bentonite [26].


### 3.3.3. TEM Characterization

The TEM photographs of different adsorbents are shown in Figure6. The photographs of CB suggest two components of solid and hollow sphere. Compared with CB, the OCB shows a lot of pores, which further suggests that the surface area increases. In addition, it demonstrates that CB is oxidized, which is beneficial to chelate with heavy metal ions.Figure 6
Representative TEM images of different adsorbents. (a) CB (scale bar is 250 nm), (b) OCB (scale bar is 250 nm), (c) bentonite (scale bar is 799 nm), and (d) organic bentonite (scale bar is 799 nm).
(a)
(b)
(c)
(d)As shown in Figures6(c) and 6(d), bentonite is amorphous in structure without aggregation. The photographs of organic bentonite show some pores and blurry edges, further suggesting that the morphological structure changes by intercalation of organic compounds.


## 3.3.1. IR Analysis

FTIR spectra of CB, OCB, bentonite, and organic bentonite were recorded in the 400–4000 cm−1 spectral range by using KBr pellet method with a Fourier-380 FTIR spectrometer, and the results are shown in Figure 4. An O-H stretching band at 3450 cm−1 and a C=C stretching band at 1619 cm−1 were typical functional group of CB. Compared with CB, both bands not only were reserved but also became much more in OCB. The bands at 1721.6 and 1244.0 cm−1 can be assigned to the C=O and C-O stretching vibrations, respectively. The band at 447.3 cm−1 can be assigned to the CNO bending vibration. All these oxygen-containing functional groups chelating with heavy metal ion were absent in CB.Figure 4
IR spectrum of different adsorbents. (a) CB, (b) OCB, (c) bentonite, and (d) organic bentonite.The bands at 3622 and 3693 cm−1 can be assigned to the Al-Al-OH and Al-Mg-OH stretching vibration, respectively, which were typical groups of bentonite [24]. A broad band at 1115–996 cm−1 region was assigned to the Si-O stretching vibration, whereas a band at 516 cm−1 was assigned to the Si-O bending vibration. Compared with natural bentonite, a pair of bands at 2919 and 2849 cm−1 in organic bentonite was assigned to the symmetric and asymmetric C-H stretching vibrations of methyl and methylene groups. And a band at 1467 cm−1 was assigned to the asymmetric C-H bending vibration. These bands suggested the presence of cationic surfactants in the bentonite.


## 3.3.2. SEM Characterization

To investigate the surface morphology, SEM (H-800 EM, Japan) analysis was performed on the different adsorbents (Figure5). The photographs of CB suggest sphere with diameter of 50–60 nm, which demonstrates nanoscale material. However, OCB had no obvious variation in shape and need to be further studied by TEM. In Figures 5(a) and 5(b), both materials suggest the serious aggregation of nanoparticles.Figure 5
Representative SEM images of different adsorbents. (a) CB (scale bar is 600 nm), (b) OCB (scale bar is 600 nm), (c) bentonite (scale bar is 6μm), and (d) organic bentonite (scale bar is 6 μm).
(a)
(b)
(c)
(d)The SEM images of bentonite and organic bentonite are shown in Figures5(c) and 5(d). The morphology of bentonite suggests smooth surface with flat crystal. Compared with natural bentonite, the clay lattice of organic bentonite appeared swollen and fluffy. This might be due to the organic compounds introduced in clay interlayer, which increase the basal spacing of clay [25]. The surface structure and porous characteristics are conductive to accelerate the spread of heavy metal ions in bentonite [26].


## 3.3.3. TEM Characterization

The TEM photographs of different adsorbents are shown in Figure6. The photographs of CB suggest two components of solid and hollow sphere. Compared with CB, the OCB shows a lot of pores, which further suggests that the surface area increases. In addition, it demonstrates that CB is oxidized, which is beneficial to chelate with heavy metal ions.Figure 6
Representative TEM images of different adsorbents. (a) CB (scale bar is 250 nm), (b) OCB (scale bar is 250 nm), (c) bentonite (scale bar is 799 nm), and (d) organic bentonite (scale bar is 799 nm).
(a)
(b)
(c)
(d)As shown in Figures6(c) and 6(d), bentonite is amorphous in structure without aggregation. The photographs of organic bentonite show some pores and blurry edges, further suggesting that the morphological structure changes by intercalation of organic compounds.


## 4. Conclusions

From the study, we discover that the adsorption mechanisms of Cu2+ on CB, bentonite, and their surface-modified materials are different. The adsorption capacities of Cu2+ on these adsorbents follow the order of OCB > CB > organic bentonite > bentonite, consistent with the order of their surface roughness and surface area. The results of adsorption isotherms show that the adsorption process of CB is surface adsorption, and bentonite is ion exchange adsorption because of exchangeable cations in the lattice. IR and SEM indicate that the mechanism of organic bentonite was that organic compounds introduced in clay interlayer occur as complexing reaction with heavy metal ions, in addition to exchange adsorption. However, the adsorption of OCB is that oxygen-containing functional groups chelate with heavy metal ion, by IR and TEM analysis.



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*Source: 7936258-2016-01-03.xml*