# Cr(VI) Removal from Aqueous by Adsorption on Amine-Functionalized Mesoporous Silica Prepared from Silica Fume

Authors: Xitong Li; Caiyun Han; Wenjie Zhu; Wenhui Ma; Yongming Luo; Yang Zhou; Jie Yu; Kuixian Wei
Journal: Journal of Chemistry
 (2014)

---

## Abstract

Amino-functionalized mesoporous silica MCM-41 materials have been prepared to develop efficient adsorbents of Cr(VI) in wastewater, using silica fume as silica source. Functionalization with amino groups has been carried out by using grafting method. The materials have been characterized by means of X-ray diffraction (XRD), nitrogen (N2) adsorption-desorption, Fourier transform infrared (FTIR) spectroscopy, scanning electron microscopy (SEM), transmission electron microscopy (TEM), and X-ray photoelectron spectroscopy (XPS). Adsorption potential of the material for Cr(VI) removal from aqueous solution was investigated by varying experimental conditions such as pH, initial metal concentration, and contact time. The equilibrium data were analyzed using the Langmuir and Freundlich isotherm by linear regression analysis, and the results show that the adsorption equilibrium data obeyed the Langmuir model. In addition, the kinetics analysis revealed that the overall adsorption process was successfully fitted with the pseudo-second-order kinetic model.


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## Body

## 1. Introduction

The release of heavy metals from industrial entities into the natural environmental has led to serious pollution problem. Presence of heavy metals in water bodies is of great concern. Elevated levels of heavy metals may have adverse impacts on the environment and pose serious human health risks. Chromium is commonly found in the waste effluents from electroplating, metallurgical, tannery, and textile industry [1, 2]. In the natural environment Cr occurs in different oxidation states ranging from II to VI, with Cr(III) and Cr(VI) as the most abundant species. Cr(III) is a required nutrient, whereas Cr(VI) has toxic effects [3]. Cr(VI) (i.e., Cr
O
4
2
- and Cr
2
O
7
2
-) is very toxic and is a strictly regulated pollutant. Accidental chromium ingestion causes stomach upsets, ulcers, kidney and liver damages, and even death. Moreover, Cr(VI) is also mutagenic, carcinogenic, and teratogenic and has been recognized as a priority pollutant [4, 5].A wide variety of techniques to remove heavy metals from water is available such as ion exchange, reverse osmosis and nanofiltration, precipitation, coagulation/coprecipitation, and adsorption [6–8]. This last technique is very popular due to simplicity and low cost. The MCM-41 solids exhibit high specific surface areas, high crystallinity, high thermal stability, uniformity of hexagonal cylindrical pores, narrow pore distribution, and regulated pore diameter from 15 to 100 Å. Then, those materials with various chelating agents are increasingly utilized as adsorbents because of the high selectivity of the agents for metal ions adsorption. These characteristics render these solids as ideal heavy metal adsorbents [9, 10]. For instance, the maximum adsorption capacity of modified MCM-41 for Ni(II), Cd(II), and Pb(II) was found to be 12.36, 18.25, and 57.74 mg/g, respectively [11]. It was larger than the capacity of activated carbon. Unfortunately, the main disadvantage of mesoporous material is the lack of popular prices in the process of synthesis, because the price of silica resource is very expensive.Silica fume is formed as a byproduct during the production of alusil alloy or metallurgy grade silicon. As an industrial solid waste, SF is normally utilized as a substitute for fine aggregates in cement and concrete, in bricks and ceramic tiles and a filler in plastics and paints [12–14]. However, it has pozzolanic properties and phase minerals comprising major silica components (95.1%) in the amorphous form, with traces of alumina, alkaline metal oxides, and transition metal oxides [15, 16]. Hence, SF has the capability to become a kind of useful silica resources in the synthesis of mesoporous materials. With the addition of an external silicon source (silica fume) to the synthesis mixture which allows controlling the final Si/Al ratio Habib et al. synthesized the ZSM-5 successfully [17]. Recently, with the industrial silica fume as silica source, the MCM-41 and MCM-48 were synthesized [15, 18]. They proved that the possibility of the mesoporous material can be synthesized by using silica fume as silica source. However, the adsorption capacities of this material are rare for scholar to mention.This work describes Cr(VI) removal from aqueous by adsorption on amine-functionalized mesoporous silica prepared from silica fume. The NH2-MCM-41 grafted with aminopropyls was selected. The Cr
2
O
7
2
- is expected to adsorb on NH2-MCM-41 at low pH. The adsorption kinetics and equilibrium studies were then conducted to evaluate their adsorption behaviors. The effect of solution pH was investigated. This study is to provide a better understanding on the adsorption mechanisms of metal ions by NH2-MCM-41 and a way of mesoporous material synthesis in a popular price.


## 2. Experimental

### 2.1. Chemicals

Silica fumes (SF) were collected from a local metallurgy-grade silicon factory using an electro-precipitator, and it was used as silica source (Table1). Surfactant cetyltrimethylammonium bromide (CTAB) was employed as structure directing agent. The organoalkoxysilanes selected for the functionalization process was 3-aminopropyl trimethoxysilane (MPTS, Alfa Aesar). Source of metal for sorption experiments was potassium dichromate and sodium hydroxide (NaOH) was obtained from Shanghai Chemical Co. All chemical reagents and solvents were analytical grade and used without further purification.Table 1
The contents of silica fume.
Sample
SiO2
CO2
K2O
MgO
P2O5
CaO
Al2O3
MnO
Na2O
Fe2O3
(%)
92.4850
2.3249
2.5057
1.0010
0.2852
0.3287
0.1033
0.0685
0.0903
0.0593


### 2.2. Adsorbents Synthesis

In a typical synthesis procedure, mesoporous silica materials were synthesized by using cetyltrimethylammonium bromide (CTAB) as the template and silica fume (SF) as the silica source with the molar ratio of 1.0 SiO2 : 0.3 NaOH : 0.15 CTAB : 168 H2O. Exactly 1.33 g of silica fume and 1.21 g of CTAB were dissolved at room temperature and stirred for 2 h. The mixtures were then transferred into a flask and heated to 363 K for 48 h for hydrothermal reaction. The gray powders were recovered by filtration and extensively washed with deionized water. The samples were dried at 373 K for 12 h and then calcined at 823 K for 5 h to yield the mesoporous silica materials (MCM-41).The MCM-41 adsorbent containing aminopropyls, NH2-MCM-41, was prepared by refluxing of 2.5 g MCM-41 powder in 250 mL dry toluene (>99.5%, Mallinckrodt) containing 0.4 M 3-aminopropyltrimethoxysilane (97%, Aldrich) for 18 h. The NH2-MCM-41 powder was filtered, washed with toluene, and dried in an oven at 383 K overnight (toluene purified). The dried adsorbent was ground and sieved to obtain a free flowing powder.


### 2.3. Characterization

The contents of silica fume were quantified by XRF spectrometer (Rigaku ZSX100). The X-ray powder diffraction spectra were recorded by XRD diffractometer (Rigaku D/MAX-3B) equipped with a liquid nitrogen-cooled germanium solid-state detector using Cu-Kα radiation over a range of 0.5–8° with a voltage of 40 kV. Nitrogen adsorption-desorption isotherms were measured at −196°C using a surface area and pore size analyzer (Quantachrome Instruments NOVA 2200e) in order to determine the textural properties. Approximately 0.1 g of all samples was degassed at 100°C for 3 h under argon gas flow before analysis. The specific surface area was evaluated using the Brunauer-Emmett-Teller (BET) method, and the pore size distribution was calculated from desorption branches of nitrogen isotherms applying the Barrett-Joyner-Halenda (BJH) method. Fourier transform infrared spectra (FTIR) were recorded (Varian 640-IR FTIR) in the range of 400–4000 cm−1 with a resolution of 4 cm−1. The morphology of the mesoporous materials was obtained by electron scanning microscopy (Philips XL-30ESEM-TMP) and transmission electron microcopy (JEOL JEM-2100). The XPS spectra were recorded with a monochromatized Mg (Kα) source of 1253.6 eV energy. The binding energy scale for final calibration was corrected by the C1 s peak of 284.6 eV (PHI 5500). Concentrations of Cr(VI) ions were analyzed by a Flame Atomic Absorption Spectrophotometer (AAS, Hitachi Z200).


### 2.4. Adsorption Experiments

The adsorption experiments were carried out under ambient conditions (25°C). Analytical grade lead nitrate was used to prepare a stock solution Cr(VI) of 1000 mg/L, which was further diluted with deionized water to different concentrations for the adsorption experiments. In the adsorption kinetics experiments, NH2-MCM-41 were mixed with 40 mg/L of Cr(VI) in 100 mL solution and stirred with a magnetic stirrer at 200 rpm. The kinetic sorption data (discussed in Section 3.2) suggested that 24 h were sufficient to reach the state of equilibrium. The adsorption isotherm studies were conducted with initial Cr(VI) concentrations ranging from 5 to 200 mg/L together with 20 mg NH2-MCM-41 in 100 mL solution. The initial solution was adjusted by using HNO3 or NaOH to reach the desired pH values. For the purpose of analytical characterizations, the NH2-MCM-41 samples were recovered by centrifugation, followed by drying.


## 2.1. Chemicals

Silica fumes (SF) were collected from a local metallurgy-grade silicon factory using an electro-precipitator, and it was used as silica source (Table1). Surfactant cetyltrimethylammonium bromide (CTAB) was employed as structure directing agent. The organoalkoxysilanes selected for the functionalization process was 3-aminopropyl trimethoxysilane (MPTS, Alfa Aesar). Source of metal for sorption experiments was potassium dichromate and sodium hydroxide (NaOH) was obtained from Shanghai Chemical Co. All chemical reagents and solvents were analytical grade and used without further purification.Table 1
The contents of silica fume.
Sample
SiO2
CO2
K2O
MgO
P2O5
CaO
Al2O3
MnO
Na2O
Fe2O3
(%)
92.4850
2.3249
2.5057
1.0010
0.2852
0.3287
0.1033
0.0685
0.0903
0.0593


## 2.2. Adsorbents Synthesis

In a typical synthesis procedure, mesoporous silica materials were synthesized by using cetyltrimethylammonium bromide (CTAB) as the template and silica fume (SF) as the silica source with the molar ratio of 1.0 SiO2 : 0.3 NaOH : 0.15 CTAB : 168 H2O. Exactly 1.33 g of silica fume and 1.21 g of CTAB were dissolved at room temperature and stirred for 2 h. The mixtures were then transferred into a flask and heated to 363 K for 48 h for hydrothermal reaction. The gray powders were recovered by filtration and extensively washed with deionized water. The samples were dried at 373 K for 12 h and then calcined at 823 K for 5 h to yield the mesoporous silica materials (MCM-41).The MCM-41 adsorbent containing aminopropyls, NH2-MCM-41, was prepared by refluxing of 2.5 g MCM-41 powder in 250 mL dry toluene (>99.5%, Mallinckrodt) containing 0.4 M 3-aminopropyltrimethoxysilane (97%, Aldrich) for 18 h. The NH2-MCM-41 powder was filtered, washed with toluene, and dried in an oven at 383 K overnight (toluene purified). The dried adsorbent was ground and sieved to obtain a free flowing powder.


## 2.3. Characterization

The contents of silica fume were quantified by XRF spectrometer (Rigaku ZSX100). The X-ray powder diffraction spectra were recorded by XRD diffractometer (Rigaku D/MAX-3B) equipped with a liquid nitrogen-cooled germanium solid-state detector using Cu-Kα radiation over a range of 0.5–8° with a voltage of 40 kV. Nitrogen adsorption-desorption isotherms were measured at −196°C using a surface area and pore size analyzer (Quantachrome Instruments NOVA 2200e) in order to determine the textural properties. Approximately 0.1 g of all samples was degassed at 100°C for 3 h under argon gas flow before analysis. The specific surface area was evaluated using the Brunauer-Emmett-Teller (BET) method, and the pore size distribution was calculated from desorption branches of nitrogen isotherms applying the Barrett-Joyner-Halenda (BJH) method. Fourier transform infrared spectra (FTIR) were recorded (Varian 640-IR FTIR) in the range of 400–4000 cm−1 with a resolution of 4 cm−1. The morphology of the mesoporous materials was obtained by electron scanning microscopy (Philips XL-30ESEM-TMP) and transmission electron microcopy (JEOL JEM-2100). The XPS spectra were recorded with a monochromatized Mg (Kα) source of 1253.6 eV energy. The binding energy scale for final calibration was corrected by the C1 s peak of 284.6 eV (PHI 5500). Concentrations of Cr(VI) ions were analyzed by a Flame Atomic Absorption Spectrophotometer (AAS, Hitachi Z200).


## 2.4. Adsorption Experiments

The adsorption experiments were carried out under ambient conditions (25°C). Analytical grade lead nitrate was used to prepare a stock solution Cr(VI) of 1000 mg/L, which was further diluted with deionized water to different concentrations for the adsorption experiments. In the adsorption kinetics experiments, NH2-MCM-41 were mixed with 40 mg/L of Cr(VI) in 100 mL solution and stirred with a magnetic stirrer at 200 rpm. The kinetic sorption data (discussed in Section 3.2) suggested that 24 h were sufficient to reach the state of equilibrium. The adsorption isotherm studies were conducted with initial Cr(VI) concentrations ranging from 5 to 200 mg/L together with 20 mg NH2-MCM-41 in 100 mL solution. The initial solution was adjusted by using HNO3 or NaOH to reach the desired pH values. For the purpose of analytical characterizations, the NH2-MCM-41 samples were recovered by centrifugation, followed by drying.


## 3. Results and Discussion

### 3.1. Characterization of the MCM-41 and NH2-MCM-41

Nitrogen adsorption-desorption isotherms obtained at 77 K of pure. The nitrogen adsorption-desorption isotherms and pore size distributions of the MCM-41 sample are plotted in Figure1(a). The BJH pore size distribution of MCM-41 shows a relatively narrow distribution with a pronounced peak that corresponds to pores with diameter 2–4 nm. The figure shows the isotherm which is a typical type-IV isotherm with a well-defined hysteresis loop indicating the presence of mesopores. This is an expected result, reflecting that the MCM-41 surface was indeed.(a) Nitrogen adsorption isotherm of MCM-41. (b) TEM image of the MCM-41. (c) XRD patterns of the MCM-41 and NH2-MCM-41. (d) SEM image of NH2-MCM-4.
(a)
(b)
(c)
(d)XRD patterns of two samples are presented in Figure1(c). An intense peak (100) could be observed for all samples and two well-resolved small peaks (110) and (200) could be observed for MCM-41, being indicative of well-ordered hexagonal mesoporous structures [19]. This result indicates that the mesoporous structure was not destroyed during the surface amino-functionalization process.Figure1(b) shows the photographs of MCM-41 taken with the TEM images. The hexagonal structure can be seen at the sample, indicating that the MCM-41 was successfully synthesized. To better understand the structural and morphological differences between MCM-41 and NH2-MCM-41, SEM analysis showed that the NH2-MCM-41 clearly displays the hexagonal structure. Figure 1(d) shows the representative SEM images of NH2-MCM-41. At the same time, this hexagonal structure did not disappear with small group of ion from silica fume added to MCM-41. The SEM and TEM images are in accordance with the XRD results in explaining the hexagonal structure in NH2-MCM-41.The inner assembly details of MCM-41 and NH2-MCM-41 were illustrated by FTIR spectroscopy. Figure 2 showed the FTIR spectra of unmodified MCM-41 and NH2-MCM-41. The typical vibration modes of MCM-41 (OH, 3432 cm−1; Si–O–Si, 1090 and 798 cm−1; Si–OH, 972 cm−1; and Si–O, 468 cm−1) were presented. Comparing the intensity of the unmodified MCM-41, the intensity of the Si–OH vibration at 972 cm−1 in NH2-MCM-41 decreased, which indicated that most of the Si–OH bonds on the inner surface of MCM-41 had been occupied due to the modification. In addition, the bands at 3432 and 1547 cm−1 in the spectrum implied the existence of the N–H stretching and bending vibrations after the modification. Both symmetric and asymmetric CH2 (tas(CH2) = 2927 cm−1, ts(CH2) = 2856 cm−1) groups [20] were identified. As a result, it indicated that aminopropyl groups had been grafted onto the inner surface of MCM-41 via reactions between APTES and OH groups on the channel wall. From the characterizations we can infer that the interaction mechanism between the silanol groups and the APTES was as follows:
(1)
Si–OH
+
H
2
NC
H
2
C
H
2
C
H
2
Si
(
O
C
2
H
5
)
3
⟶
Si–O–Si
(
O
C
2
H
5
)
2
C
H
2
C
H
2
C
H
2
N
H
2Figure 2
FTIR spectra of MCM-41 and NH2-MCM-41.This was also the reason why the two well-resolved small peaks (110) and (200) were absent in amino-functionalised MCM-41 (Figure1(c)).As has been reported, in supported Cr/SiO2 materials chromium ions exist in different oxidation states, which are responsible of their catalytic behavior. XPS is an useful technique to determine the surface of materials. Figure 3(a) shows the XPS spectra of NH2-MCM-41. The N 1s spectrum was assigned to peak corresponding to the binding energies of 398.5 and 400.66 eV. The C 1s peak appears at the binding energies corresponding to 208.06 eV. The result indicated that amino groups had been grafted onto the inner surface of MCM-41. Figure 3(b) shows that the –
N
H
3
+ and –NH2 XPS spectra suggest that amino groups exit in the MCM-41 and the groups of amino had been changed. As is shown in Figure 2(a), the protonation had occurred on the grafted amino groups. It indicated that the capacity of NH2-MCM-41 combination with Cr
2
O
7
2
- in the adsorption process is easier.XPS spectra of NH2-MCM-41 and Cr–NH2-MCM-41. (a) Over all spectra of NH2-MCM-41; (b) N 1s spectra of NH2-MCM-41 before adsorption; (c) overall spectra of Cr–NH2-MCM-41; (d) Cr 2p spectra of Cr–NH2-MCM-41; (e) N 1s spectra of NH2-MCM-41 after adsorption.
(a)
(b)
(c)
(d)
(e)Figure3(c) shows the XPS spectra of NH2-MCM-41 after adsorption. Figure 3(d) illustrates the Cr 2p XPS spectra of the difference in sample. The spectra were deconvoluted using Gaussian functions in order to fit them with the experimental spectra in the 570–595 eV range of binding energy. The significant binding energies at 577.96 eV and 587.66 eV could be attributed to Cr(III) corresponding to 2p3/2 and 2p1/2 orbitals, respectively. The Cr 2p core region corresponds to the blinding 577.96 and 587.66 eV and the chrome content was 1.94% indicated that the absorbent had a good adsorb capacity of Cr(VI). It is known that XPS detections limited by the mean photoelectron escape depth to about 2 nm. Consequently, high mesoporous materials only exhibit a very low surface to the XPS beam [21]. So the low intensity of Cr 2p signal observed in Figure 3(c) suggests that most of the chromium is on the inner surface hidden into the pores and not detected for the XPS technique.Figure3(e) illustrates the N 1s spectra of NH2-MCM-41 after adsorption. The intensity of –
N
H
3
+ decreased and the peak to the binding energies of 398.5 disappeared. In addition, the peak at 398.8 eV and 401.4 eV before adsorption for NH2-MCM-41 was different from the peak at 399 eV and 400.7 eV after adsorption, indicating that the structure of –
N
H
3
+ was changed. The similar phenomenon was observed in the image of Cr(VI). The result indicated that –
N
H
3
+ and Cr
2
O
7
2
- in the process of adsorption are held together by their mutual electrostatic attraction. But the mechanism cannot be described by only one pattern. Another mechanism can be described by another way. Due to the less electron of Cr(VI) in C
r
2
O
7
2
- and the didymous electron of –
N
H
3
+, Cr(VI) reached electron from the –
N
H
3
+. By sharing a pair of electrons they formed a kind of coordinate bond. But in this research the second mechanism was the dominant.


### 3.2. Cr(VI) Adsorption onto NH2-MCM-41

#### 3.2.1. Effect of Initial pH on the Adsorption of Cr(VI)

The pH value of the system controls the adsorption capacity due to its influence on the charge density of the adsorbent and the ionic forms of the chrome ions in solutions. Hence, the pH value is one of the most important parameters while assessing the adsorption capacity of an adsorbent for metal ions sequestering from aqueous solution. In the present work, adsorption of Cr(VI) on the as-prepared NH2-MCM-41 sample was studied over the initial Cr(VI) concentration used in the solution which was 40 mg/L. Figure 4 shows the effect of pH on the adsorption of Cr(VI) ions where the adsorption capacity of Cr(VI) decreases with the increasing pH value in the solution and the maximum adsorption capacity of Cr(VI) was reached at a pH value of around 2.0 (more than 20 mg/g). When the pH value around 6-7 the adsorption capacity of Cr(VI) was almost zero. In such a system, active sites are becoming protonated to the virtual appeal to metal binding on the NH2-MCM-41 surface. This means that at lower pH the NH2-MCM-41 surface becomes more positively charged thus producing the attraction between the surface and Cr
2
O
7
2
-. At pH = 2, there are many species of chromium ions in solution such as Cr
O
4
2
-, HCr
O
4
-, and H2Cr2O7. But the predominant species is HCr
O
4
-. However, the adsorption capacity decreased at pH < 1, which was related to the formation of nonionic H2Cr2O7 [22]. As the pH value increases, less positively charged surface becomes available thus controlling greater metal uptake. Therefore, the pH value of 2.0 was selected to be the optimum pH value for further studies. In order to maintain the pH, the initial solution was adjusted by using HNO3 or NaOH to reach the pH values.Figure 4
Effect of initial pH on the adsorption of Cr(VI).


#### 3.2.2. Adsorption Kinetics

Adsorption kinetics was one of the most important characters which represented the adsorption efficiency. The effect of different contact time intervals ranging from 0 to 720 min on the adsorption of Cr(VI) by NH2-MCM-41 was shown in Figure 5. It could be observed that in the process of the absorption of Cr(VI) by NH2-MCM-41 within 240 min was fast, relatively. The absorption of Cr(VI) by NH2-MCM-41 approached an adsorption equilibrium within 600 min with the removal rate and adsorption capacity reaching 91.8% and 45.89 mg/g. The high initial removal rate and the equilibration time demonstrated that the surface of the modified MCM-41 had density of active sites. The possible reasons were that postgrafting could not break the mesoporous structure and functional groups were distributed in the pipe, and the adsorption of Cr(VI) onto the NH2-MCM-41 support proceeded with the intended Cr–NH2-MCM-41 chelate format [23].Figure 5
The Cr(VI) adsorption capacity and removal efficiency as functions with contact time (solution volume 100 mL, adsorbent 20 mg, 200 rpm, 25°C, initial Cr(VI) concentration 40 mg/L).The kinetics on the NH2-MCM-41 is described by the pseudo-first-order and pseudo-second-order models and the intraparticle diffusion model. The pseudo-first-order model is generally expressed as follows:
(2)
ln
⁡
⁡
(
q
e
-
q
)
=
ln
⁡
⁡
q
e
-
k
1
t
,
where q
e and q are the sorption capacities at equilibrium and time, respectively (mg/g). k
1 represents the rate constant of the pseudo-first-order kinetic model (min−1). The pseudo-second-order model equation is given as follows:
(3)
t
q
=
t
q
e
+
1
k
2
q
e
2
,
where k
2 is the rate constant of the pseudo-second-order kinetic model (g/mg min). The intraparticle diffusion model equation is given as
(4)
q
t
=
k
ip
t
1
/
2
+
C
,
where k
ip is the rate constant of the intraparticle diffusion (mg·g−1·min−1/2) [24].The adsorption kinetics of Cr(VI) by NH2-MCM-41 was investigated at pH = 2. The good accessibility of the chelating sites grafted on the NH2–MCM-41 mesoporous silica matrix is reflected by the kinetics of the interaction between immobilized ligand and the metal ion. The sorption kinetic data were examined by using pseudo-first-order, pseudo-second-order, and intraparticle diffusion kinetic models (Figure 6). It can be seen from the values of R
2 that the adsorption process follows the intraparticle diffusion model. Therefore, surface sorption contributes less to the rate limiting step than intraparticle diffusion. Surface, pore, and intraparticle diffusion could be the plausible means that could characterize the adsorption of Cr(VI) onto the amino-group grafted MCM-41 adsorbent surface. Analysis of the experimental data with the pseudo-second-order and pseudo-first-order kinetic models both showed agreement of the sets of data (Table 2). The results could be reasonably described by pseudo-second-order kinetic model with a high correlation coefficient (Table 2), suggesting an adsorption process of rate limiting step. Additionally, the calculated values of q
e
.
cal obtained from pseudo-second-order models showed good agreement with the experimental values. It can be inferred that the process was limited by the chemical adsorption [25]. The possible process of adsorption was Cr(VI) which could combine with the amino structure. In the beginning of the adsorption process Cr(VI) combined with –NH2 which is outside the MCM-41. With the adsorption process, the –NH2 outside of the MCM-41 was less and then the rate of adsorption was slow. With the process of intraparticle diffusion, more Cr(VI) into the MCM-41 and then Cr(VI) combined with the –NH2 which is inside the MCM-41.Table 2
Kinetic model parameters for Cr(VI).
Model
q
e
.
exp
⁡ (mg/g)
k
q
e
.
cal (mg/g) or C
R
2
Pseudo-first-order
47.27
0.059
26.87
0.957
Pseudo-second-order
0.04
50.00
0.998
Intraparticle diffusion
5.133
29.95
0.982(a) Pseudo-first-order model fit for the adsorption of Cr(VI) by NH2-MCM-41. (b) Pseudo-second-order model fit for the adsorption of Cr(VI) by NH2-MCM-41. (c) Intraparticle diffusion model fit for the adsorption of Cr(VI) by NH2-MCM-41.
(a)
(b)
(c)


#### 3.2.3. Adsorption Isotherms

The adsorption capacity of NH2-MCM-41, q
e (mg/g) was plotted as a function of the equilibrium concentrations of Cr(VI). In order to investigate the adsorption mechanism, the adsorption data were analyzed by using Langmuir and Freundlich adsorption isotherms. The Langmuir and Freundlich equations are the most common models employed to describe the adsorption process in heterogeneous systems. The Langmuir model assumes monolayer adsorption on the solid surface, while Freundlich model is empirical in nature. The Langmuir equation was expressed as
(5)
C
e
q
e
=
C
e
q
m
+
1
q
m
K
L
,
where q
e (mg/g) is the equilibrated adsorption amount, C
e (mg/L) is the equilibrated concentration of metal ions, q
m (mg/g) is the saturated adsorption capacity of the adsorbent, and K
L is the Langmuir constant related to the free energy of adsorption [26]. While the Freundlich isotherm is an empirical equation described multilayer adsorptions and assuming the adsorption surface was heterogeneous, the equation was written as
(6)
log
⁡
⁡
q
e
=
log
⁡
⁡
K
F
+
1
n
log
⁡
⁡
C
e
,
where K
F   (L/mg) is the Freundlich constant related to the adsorption capacity of the adsorbent and n is the heterogeneity factor indicating the adsorption intensity of the adsorbent [27]. All of the isotherm constants and correlation coefficients computed by nonlinear curve fitting are given in Table 3. Each value in these tables is the mean of three determinations with an accepted relative standard deviation of ±3%.Table 3
Langmuir and Frenudlich isotherm parameters for Cr(VI) adsorption on NH2-MCM-41 in different temperature.
Model
Langmuir
Frenudlich
q
m
b
R
2
n
f
k
f
R
2
25°C
60.91
0.069
0.994
1.927
7.463
0.910
35°C
80.06
0.262
0.980
2.674
14.04
0.921
45°C
82.05
0.443
0.971
3.115
19.47
0.874The results show that the adsorption equilibrium data obeyed the Langmuir model, and the Langmuir model should better describe the adsorption system on NH2-MCM-41 than the Freundlich model. These results suggested that the adsorption of Cr(VI) onto NH2-MCM-41 was monolayer, and NH2-MCM-41 surface was homogeneous. Calculation of the isotherm parameters using these plots provided the data presented in Table 3. When the aqueous metal concentration increased, the saturation constant value was reached. Figure 7 shows the adsorption isotherms at 25°C, 35°C, and 45°C. The adsorption capacity of NH2-MCM-41 was compared with different temperature. The maximum Cr(VI) adsorption capacity of NH2-MCM-41 in 25°C amounted to 60.9 mg/g. Whereas the maximum Cr(VI) adsorption capacity of NH2-MCM-41 in 35°C amounted to 80.06 mg/g. On the other hand, the values of n were all greater than 1 for the different temperature, indicative of high adsorption intensity.Figure 7
Adsorption isotherms at 25°C, 35°C, and 45°C of Cr(VI) on NH2-MCM-41.Gibbs free energy change (Δ
G), entropy change (Δ
S), equilibrium constant (K
eq), and enthalpy change (Δ
H) were estimated from the following:
(7)
Δ
G
=
-
R
T
ln
⁡
⁡
b
,
ln
⁡
⁡
b
=
-
Δ
H
(
R
T
)
+
Δ
S
R
,
Δ
S
=
(
Δ
H
-
Δ
G
)
T
,
b
=
C
0
C
e
,
where b is the initial concentration of Cr(VI) removed from NH2-MCM-41 per volume of solution used for this study (
C
0
), C
e is the concentration of Cr(VI) solution at equilibrium, T is the temperature of solution measured in Kelvin, and R is the universal gas constant (8.314 J/(mol·K)) [28].Table4 shows the estimated value of thermodynamic parameters for NH2-MCM-41. The sign of the Gibbs free energy change value shows that the adsorption process was faster with the increase of temperature, and the sign of the entropy change value also shows that the process follows the increase of entropy. Additionally, the sign of enthalpy change value confirmed the endothermic disposition of the adsorption process.Table 4
Thermodynamic parameter for adsorption of Cr(VI) at different temperatures on NH2-MCM-41.
T
(
K
)
ΔG (kJ/mol)
ΔH (kJ/mol)
ΔS [J/(mol·K)]
298
-
1.506
2.024
39.876
308
-
1.665
318
-
1.843


## 3.1. Characterization of the MCM-41 and NH2-MCM-41

Nitrogen adsorption-desorption isotherms obtained at 77 K of pure. The nitrogen adsorption-desorption isotherms and pore size distributions of the MCM-41 sample are plotted in Figure1(a). The BJH pore size distribution of MCM-41 shows a relatively narrow distribution with a pronounced peak that corresponds to pores with diameter 2–4 nm. The figure shows the isotherm which is a typical type-IV isotherm with a well-defined hysteresis loop indicating the presence of mesopores. This is an expected result, reflecting that the MCM-41 surface was indeed.(a) Nitrogen adsorption isotherm of MCM-41. (b) TEM image of the MCM-41. (c) XRD patterns of the MCM-41 and NH2-MCM-41. (d) SEM image of NH2-MCM-4.
(a)
(b)
(c)
(d)XRD patterns of two samples are presented in Figure1(c). An intense peak (100) could be observed for all samples and two well-resolved small peaks (110) and (200) could be observed for MCM-41, being indicative of well-ordered hexagonal mesoporous structures [19]. This result indicates that the mesoporous structure was not destroyed during the surface amino-functionalization process.Figure1(b) shows the photographs of MCM-41 taken with the TEM images. The hexagonal structure can be seen at the sample, indicating that the MCM-41 was successfully synthesized. To better understand the structural and morphological differences between MCM-41 and NH2-MCM-41, SEM analysis showed that the NH2-MCM-41 clearly displays the hexagonal structure. Figure 1(d) shows the representative SEM images of NH2-MCM-41. At the same time, this hexagonal structure did not disappear with small group of ion from silica fume added to MCM-41. The SEM and TEM images are in accordance with the XRD results in explaining the hexagonal structure in NH2-MCM-41.The inner assembly details of MCM-41 and NH2-MCM-41 were illustrated by FTIR spectroscopy. Figure 2 showed the FTIR spectra of unmodified MCM-41 and NH2-MCM-41. The typical vibration modes of MCM-41 (OH, 3432 cm−1; Si–O–Si, 1090 and 798 cm−1; Si–OH, 972 cm−1; and Si–O, 468 cm−1) were presented. Comparing the intensity of the unmodified MCM-41, the intensity of the Si–OH vibration at 972 cm−1 in NH2-MCM-41 decreased, which indicated that most of the Si–OH bonds on the inner surface of MCM-41 had been occupied due to the modification. In addition, the bands at 3432 and 1547 cm−1 in the spectrum implied the existence of the N–H stretching and bending vibrations after the modification. Both symmetric and asymmetric CH2 (tas(CH2) = 2927 cm−1, ts(CH2) = 2856 cm−1) groups [20] were identified. As a result, it indicated that aminopropyl groups had been grafted onto the inner surface of MCM-41 via reactions between APTES and OH groups on the channel wall. From the characterizations we can infer that the interaction mechanism between the silanol groups and the APTES was as follows:
(1)
Si–OH
+
H
2
NC
H
2
C
H
2
C
H
2
Si
(
O
C
2
H
5
)
3
⟶
Si–O–Si
(
O
C
2
H
5
)
2
C
H
2
C
H
2
C
H
2
N
H
2Figure 2
FTIR spectra of MCM-41 and NH2-MCM-41.This was also the reason why the two well-resolved small peaks (110) and (200) were absent in amino-functionalised MCM-41 (Figure1(c)).As has been reported, in supported Cr/SiO2 materials chromium ions exist in different oxidation states, which are responsible of their catalytic behavior. XPS is an useful technique to determine the surface of materials. Figure 3(a) shows the XPS spectra of NH2-MCM-41. The N 1s spectrum was assigned to peak corresponding to the binding energies of 398.5 and 400.66 eV. The C 1s peak appears at the binding energies corresponding to 208.06 eV. The result indicated that amino groups had been grafted onto the inner surface of MCM-41. Figure 3(b) shows that the –
N
H
3
+ and –NH2 XPS spectra suggest that amino groups exit in the MCM-41 and the groups of amino had been changed. As is shown in Figure 2(a), the protonation had occurred on the grafted amino groups. It indicated that the capacity of NH2-MCM-41 combination with Cr
2
O
7
2
- in the adsorption process is easier.XPS spectra of NH2-MCM-41 and Cr–NH2-MCM-41. (a) Over all spectra of NH2-MCM-41; (b) N 1s spectra of NH2-MCM-41 before adsorption; (c) overall spectra of Cr–NH2-MCM-41; (d) Cr 2p spectra of Cr–NH2-MCM-41; (e) N 1s spectra of NH2-MCM-41 after adsorption.
(a)
(b)
(c)
(d)
(e)Figure3(c) shows the XPS spectra of NH2-MCM-41 after adsorption. Figure 3(d) illustrates the Cr 2p XPS spectra of the difference in sample. The spectra were deconvoluted using Gaussian functions in order to fit them with the experimental spectra in the 570–595 eV range of binding energy. The significant binding energies at 577.96 eV and 587.66 eV could be attributed to Cr(III) corresponding to 2p3/2 and 2p1/2 orbitals, respectively. The Cr 2p core region corresponds to the blinding 577.96 and 587.66 eV and the chrome content was 1.94% indicated that the absorbent had a good adsorb capacity of Cr(VI). It is known that XPS detections limited by the mean photoelectron escape depth to about 2 nm. Consequently, high mesoporous materials only exhibit a very low surface to the XPS beam [21]. So the low intensity of Cr 2p signal observed in Figure 3(c) suggests that most of the chromium is on the inner surface hidden into the pores and not detected for the XPS technique.Figure3(e) illustrates the N 1s spectra of NH2-MCM-41 after adsorption. The intensity of –
N
H
3
+ decreased and the peak to the binding energies of 398.5 disappeared. In addition, the peak at 398.8 eV and 401.4 eV before adsorption for NH2-MCM-41 was different from the peak at 399 eV and 400.7 eV after adsorption, indicating that the structure of –
N
H
3
+ was changed. The similar phenomenon was observed in the image of Cr(VI). The result indicated that –
N
H
3
+ and Cr
2
O
7
2
- in the process of adsorption are held together by their mutual electrostatic attraction. But the mechanism cannot be described by only one pattern. Another mechanism can be described by another way. Due to the less electron of Cr(VI) in C
r
2
O
7
2
- and the didymous electron of –
N
H
3
+, Cr(VI) reached electron from the –
N
H
3
+. By sharing a pair of electrons they formed a kind of coordinate bond. But in this research the second mechanism was the dominant.


## 3.2. Cr(VI) Adsorption onto NH2-MCM-41

### 3.2.1. Effect of Initial pH on the Adsorption of Cr(VI)

The pH value of the system controls the adsorption capacity due to its influence on the charge density of the adsorbent and the ionic forms of the chrome ions in solutions. Hence, the pH value is one of the most important parameters while assessing the adsorption capacity of an adsorbent for metal ions sequestering from aqueous solution. In the present work, adsorption of Cr(VI) on the as-prepared NH2-MCM-41 sample was studied over the initial Cr(VI) concentration used in the solution which was 40 mg/L. Figure 4 shows the effect of pH on the adsorption of Cr(VI) ions where the adsorption capacity of Cr(VI) decreases with the increasing pH value in the solution and the maximum adsorption capacity of Cr(VI) was reached at a pH value of around 2.0 (more than 20 mg/g). When the pH value around 6-7 the adsorption capacity of Cr(VI) was almost zero. In such a system, active sites are becoming protonated to the virtual appeal to metal binding on the NH2-MCM-41 surface. This means that at lower pH the NH2-MCM-41 surface becomes more positively charged thus producing the attraction between the surface and Cr
2
O
7
2
-. At pH = 2, there are many species of chromium ions in solution such as Cr
O
4
2
-, HCr
O
4
-, and H2Cr2O7. But the predominant species is HCr
O
4
-. However, the adsorption capacity decreased at pH < 1, which was related to the formation of nonionic H2Cr2O7 [22]. As the pH value increases, less positively charged surface becomes available thus controlling greater metal uptake. Therefore, the pH value of 2.0 was selected to be the optimum pH value for further studies. In order to maintain the pH, the initial solution was adjusted by using HNO3 or NaOH to reach the pH values.Figure 4
Effect of initial pH on the adsorption of Cr(VI).


### 3.2.2. Adsorption Kinetics

Adsorption kinetics was one of the most important characters which represented the adsorption efficiency. The effect of different contact time intervals ranging from 0 to 720 min on the adsorption of Cr(VI) by NH2-MCM-41 was shown in Figure 5. It could be observed that in the process of the absorption of Cr(VI) by NH2-MCM-41 within 240 min was fast, relatively. The absorption of Cr(VI) by NH2-MCM-41 approached an adsorption equilibrium within 600 min with the removal rate and adsorption capacity reaching 91.8% and 45.89 mg/g. The high initial removal rate and the equilibration time demonstrated that the surface of the modified MCM-41 had density of active sites. The possible reasons were that postgrafting could not break the mesoporous structure and functional groups were distributed in the pipe, and the adsorption of Cr(VI) onto the NH2-MCM-41 support proceeded with the intended Cr–NH2-MCM-41 chelate format [23].Figure 5
The Cr(VI) adsorption capacity and removal efficiency as functions with contact time (solution volume 100 mL, adsorbent 20 mg, 200 rpm, 25°C, initial Cr(VI) concentration 40 mg/L).The kinetics on the NH2-MCM-41 is described by the pseudo-first-order and pseudo-second-order models and the intraparticle diffusion model. The pseudo-first-order model is generally expressed as follows:
(2)
ln
⁡
⁡
(
q
e
-
q
)
=
ln
⁡
⁡
q
e
-
k
1
t
,
where q
e and q are the sorption capacities at equilibrium and time, respectively (mg/g). k
1 represents the rate constant of the pseudo-first-order kinetic model (min−1). The pseudo-second-order model equation is given as follows:
(3)
t
q
=
t
q
e
+
1
k
2
q
e
2
,
where k
2 is the rate constant of the pseudo-second-order kinetic model (g/mg min). The intraparticle diffusion model equation is given as
(4)
q
t
=
k
ip
t
1
/
2
+
C
,
where k
ip is the rate constant of the intraparticle diffusion (mg·g−1·min−1/2) [24].The adsorption kinetics of Cr(VI) by NH2-MCM-41 was investigated at pH = 2. The good accessibility of the chelating sites grafted on the NH2–MCM-41 mesoporous silica matrix is reflected by the kinetics of the interaction between immobilized ligand and the metal ion. The sorption kinetic data were examined by using pseudo-first-order, pseudo-second-order, and intraparticle diffusion kinetic models (Figure 6). It can be seen from the values of R
2 that the adsorption process follows the intraparticle diffusion model. Therefore, surface sorption contributes less to the rate limiting step than intraparticle diffusion. Surface, pore, and intraparticle diffusion could be the plausible means that could characterize the adsorption of Cr(VI) onto the amino-group grafted MCM-41 adsorbent surface. Analysis of the experimental data with the pseudo-second-order and pseudo-first-order kinetic models both showed agreement of the sets of data (Table 2). The results could be reasonably described by pseudo-second-order kinetic model with a high correlation coefficient (Table 2), suggesting an adsorption process of rate limiting step. Additionally, the calculated values of q
e
.
cal obtained from pseudo-second-order models showed good agreement with the experimental values. It can be inferred that the process was limited by the chemical adsorption [25]. The possible process of adsorption was Cr(VI) which could combine with the amino structure. In the beginning of the adsorption process Cr(VI) combined with –NH2 which is outside the MCM-41. With the adsorption process, the –NH2 outside of the MCM-41 was less and then the rate of adsorption was slow. With the process of intraparticle diffusion, more Cr(VI) into the MCM-41 and then Cr(VI) combined with the –NH2 which is inside the MCM-41.Table 2
Kinetic model parameters for Cr(VI).
Model
q
e
.
exp
⁡ (mg/g)
k
q
e
.
cal (mg/g) or C
R
2
Pseudo-first-order
47.27
0.059
26.87
0.957
Pseudo-second-order
0.04
50.00
0.998
Intraparticle diffusion
5.133
29.95
0.982(a) Pseudo-first-order model fit for the adsorption of Cr(VI) by NH2-MCM-41. (b) Pseudo-second-order model fit for the adsorption of Cr(VI) by NH2-MCM-41. (c) Intraparticle diffusion model fit for the adsorption of Cr(VI) by NH2-MCM-41.
(a)
(b)
(c)


### 3.2.3. Adsorption Isotherms

The adsorption capacity of NH2-MCM-41, q
e (mg/g) was plotted as a function of the equilibrium concentrations of Cr(VI). In order to investigate the adsorption mechanism, the adsorption data were analyzed by using Langmuir and Freundlich adsorption isotherms. The Langmuir and Freundlich equations are the most common models employed to describe the adsorption process in heterogeneous systems. The Langmuir model assumes monolayer adsorption on the solid surface, while Freundlich model is empirical in nature. The Langmuir equation was expressed as
(5)
C
e
q
e
=
C
e
q
m
+
1
q
m
K
L
,
where q
e (mg/g) is the equilibrated adsorption amount, C
e (mg/L) is the equilibrated concentration of metal ions, q
m (mg/g) is the saturated adsorption capacity of the adsorbent, and K
L is the Langmuir constant related to the free energy of adsorption [26]. While the Freundlich isotherm is an empirical equation described multilayer adsorptions and assuming the adsorption surface was heterogeneous, the equation was written as
(6)
log
⁡
⁡
q
e
=
log
⁡
⁡
K
F
+
1
n
log
⁡
⁡
C
e
,
where K
F   (L/mg) is the Freundlich constant related to the adsorption capacity of the adsorbent and n is the heterogeneity factor indicating the adsorption intensity of the adsorbent [27]. All of the isotherm constants and correlation coefficients computed by nonlinear curve fitting are given in Table 3. Each value in these tables is the mean of three determinations with an accepted relative standard deviation of ±3%.Table 3
Langmuir and Frenudlich isotherm parameters for Cr(VI) adsorption on NH2-MCM-41 in different temperature.
Model
Langmuir
Frenudlich
q
m
b
R
2
n
f
k
f
R
2
25°C
60.91
0.069
0.994
1.927
7.463
0.910
35°C
80.06
0.262
0.980
2.674
14.04
0.921
45°C
82.05
0.443
0.971
3.115
19.47
0.874The results show that the adsorption equilibrium data obeyed the Langmuir model, and the Langmuir model should better describe the adsorption system on NH2-MCM-41 than the Freundlich model. These results suggested that the adsorption of Cr(VI) onto NH2-MCM-41 was monolayer, and NH2-MCM-41 surface was homogeneous. Calculation of the isotherm parameters using these plots provided the data presented in Table 3. When the aqueous metal concentration increased, the saturation constant value was reached. Figure 7 shows the adsorption isotherms at 25°C, 35°C, and 45°C. The adsorption capacity of NH2-MCM-41 was compared with different temperature. The maximum Cr(VI) adsorption capacity of NH2-MCM-41 in 25°C amounted to 60.9 mg/g. Whereas the maximum Cr(VI) adsorption capacity of NH2-MCM-41 in 35°C amounted to 80.06 mg/g. On the other hand, the values of n were all greater than 1 for the different temperature, indicative of high adsorption intensity.Figure 7
Adsorption isotherms at 25°C, 35°C, and 45°C of Cr(VI) on NH2-MCM-41.Gibbs free energy change (Δ
G), entropy change (Δ
S), equilibrium constant (K
eq), and enthalpy change (Δ
H) were estimated from the following:
(7)
Δ
G
=
-
R
T
ln
⁡
⁡
b
,
ln
⁡
⁡
b
=
-
Δ
H
(
R
T
)
+
Δ
S
R
,
Δ
S
=
(
Δ
H
-
Δ
G
)
T
,
b
=
C
0
C
e
,
where b is the initial concentration of Cr(VI) removed from NH2-MCM-41 per volume of solution used for this study (
C
0
), C
e is the concentration of Cr(VI) solution at equilibrium, T is the temperature of solution measured in Kelvin, and R is the universal gas constant (8.314 J/(mol·K)) [28].Table4 shows the estimated value of thermodynamic parameters for NH2-MCM-41. The sign of the Gibbs free energy change value shows that the adsorption process was faster with the increase of temperature, and the sign of the entropy change value also shows that the process follows the increase of entropy. Additionally, the sign of enthalpy change value confirmed the endothermic disposition of the adsorption process.Table 4
Thermodynamic parameter for adsorption of Cr(VI) at different temperatures on NH2-MCM-41.
T
(
K
)
ΔG (kJ/mol)
ΔH (kJ/mol)
ΔS [J/(mol·K)]
298
-
1.506
2.024
39.876
308
-
1.665
318
-
1.843


## 3.2.1. Effect of Initial pH on the Adsorption of Cr(VI)

The pH value of the system controls the adsorption capacity due to its influence on the charge density of the adsorbent and the ionic forms of the chrome ions in solutions. Hence, the pH value is one of the most important parameters while assessing the adsorption capacity of an adsorbent for metal ions sequestering from aqueous solution. In the present work, adsorption of Cr(VI) on the as-prepared NH2-MCM-41 sample was studied over the initial Cr(VI) concentration used in the solution which was 40 mg/L. Figure 4 shows the effect of pH on the adsorption of Cr(VI) ions where the adsorption capacity of Cr(VI) decreases with the increasing pH value in the solution and the maximum adsorption capacity of Cr(VI) was reached at a pH value of around 2.0 (more than 20 mg/g). When the pH value around 6-7 the adsorption capacity of Cr(VI) was almost zero. In such a system, active sites are becoming protonated to the virtual appeal to metal binding on the NH2-MCM-41 surface. This means that at lower pH the NH2-MCM-41 surface becomes more positively charged thus producing the attraction between the surface and Cr
2
O
7
2
-. At pH = 2, there are many species of chromium ions in solution such as Cr
O
4
2
-, HCr
O
4
-, and H2Cr2O7. But the predominant species is HCr
O
4
-. However, the adsorption capacity decreased at pH < 1, which was related to the formation of nonionic H2Cr2O7 [22]. As the pH value increases, less positively charged surface becomes available thus controlling greater metal uptake. Therefore, the pH value of 2.0 was selected to be the optimum pH value for further studies. In order to maintain the pH, the initial solution was adjusted by using HNO3 or NaOH to reach the pH values.Figure 4
Effect of initial pH on the adsorption of Cr(VI).


## 3.2.2. Adsorption Kinetics

Adsorption kinetics was one of the most important characters which represented the adsorption efficiency. The effect of different contact time intervals ranging from 0 to 720 min on the adsorption of Cr(VI) by NH2-MCM-41 was shown in Figure 5. It could be observed that in the process of the absorption of Cr(VI) by NH2-MCM-41 within 240 min was fast, relatively. The absorption of Cr(VI) by NH2-MCM-41 approached an adsorption equilibrium within 600 min with the removal rate and adsorption capacity reaching 91.8% and 45.89 mg/g. The high initial removal rate and the equilibration time demonstrated that the surface of the modified MCM-41 had density of active sites. The possible reasons were that postgrafting could not break the mesoporous structure and functional groups were distributed in the pipe, and the adsorption of Cr(VI) onto the NH2-MCM-41 support proceeded with the intended Cr–NH2-MCM-41 chelate format [23].Figure 5
The Cr(VI) adsorption capacity and removal efficiency as functions with contact time (solution volume 100 mL, adsorbent 20 mg, 200 rpm, 25°C, initial Cr(VI) concentration 40 mg/L).The kinetics on the NH2-MCM-41 is described by the pseudo-first-order and pseudo-second-order models and the intraparticle diffusion model. The pseudo-first-order model is generally expressed as follows:
(2)
ln
⁡
⁡
(
q
e
-
q
)
=
ln
⁡
⁡
q
e
-
k
1
t
,
where q
e and q are the sorption capacities at equilibrium and time, respectively (mg/g). k
1 represents the rate constant of the pseudo-first-order kinetic model (min−1). The pseudo-second-order model equation is given as follows:
(3)
t
q
=
t
q
e
+
1
k
2
q
e
2
,
where k
2 is the rate constant of the pseudo-second-order kinetic model (g/mg min). The intraparticle diffusion model equation is given as
(4)
q
t
=
k
ip
t
1
/
2
+
C
,
where k
ip is the rate constant of the intraparticle diffusion (mg·g−1·min−1/2) [24].The adsorption kinetics of Cr(VI) by NH2-MCM-41 was investigated at pH = 2. The good accessibility of the chelating sites grafted on the NH2–MCM-41 mesoporous silica matrix is reflected by the kinetics of the interaction between immobilized ligand and the metal ion. The sorption kinetic data were examined by using pseudo-first-order, pseudo-second-order, and intraparticle diffusion kinetic models (Figure 6). It can be seen from the values of R
2 that the adsorption process follows the intraparticle diffusion model. Therefore, surface sorption contributes less to the rate limiting step than intraparticle diffusion. Surface, pore, and intraparticle diffusion could be the plausible means that could characterize the adsorption of Cr(VI) onto the amino-group grafted MCM-41 adsorbent surface. Analysis of the experimental data with the pseudo-second-order and pseudo-first-order kinetic models both showed agreement of the sets of data (Table 2). The results could be reasonably described by pseudo-second-order kinetic model with a high correlation coefficient (Table 2), suggesting an adsorption process of rate limiting step. Additionally, the calculated values of q
e
.
cal obtained from pseudo-second-order models showed good agreement with the experimental values. It can be inferred that the process was limited by the chemical adsorption [25]. The possible process of adsorption was Cr(VI) which could combine with the amino structure. In the beginning of the adsorption process Cr(VI) combined with –NH2 which is outside the MCM-41. With the adsorption process, the –NH2 outside of the MCM-41 was less and then the rate of adsorption was slow. With the process of intraparticle diffusion, more Cr(VI) into the MCM-41 and then Cr(VI) combined with the –NH2 which is inside the MCM-41.Table 2
Kinetic model parameters for Cr(VI).
Model
q
e
.
exp
⁡ (mg/g)
k
q
e
.
cal (mg/g) or C
R
2
Pseudo-first-order
47.27
0.059
26.87
0.957
Pseudo-second-order
0.04
50.00
0.998
Intraparticle diffusion
5.133
29.95
0.982(a) Pseudo-first-order model fit for the adsorption of Cr(VI) by NH2-MCM-41. (b) Pseudo-second-order model fit for the adsorption of Cr(VI) by NH2-MCM-41. (c) Intraparticle diffusion model fit for the adsorption of Cr(VI) by NH2-MCM-41.
(a)
(b)
(c)


## 3.2.3. Adsorption Isotherms

The adsorption capacity of NH2-MCM-41, q
e (mg/g) was plotted as a function of the equilibrium concentrations of Cr(VI). In order to investigate the adsorption mechanism, the adsorption data were analyzed by using Langmuir and Freundlich adsorption isotherms. The Langmuir and Freundlich equations are the most common models employed to describe the adsorption process in heterogeneous systems. The Langmuir model assumes monolayer adsorption on the solid surface, while Freundlich model is empirical in nature. The Langmuir equation was expressed as
(5)
C
e
q
e
=
C
e
q
m
+
1
q
m
K
L
,
where q
e (mg/g) is the equilibrated adsorption amount, C
e (mg/L) is the equilibrated concentration of metal ions, q
m (mg/g) is the saturated adsorption capacity of the adsorbent, and K
L is the Langmuir constant related to the free energy of adsorption [26]. While the Freundlich isotherm is an empirical equation described multilayer adsorptions and assuming the adsorption surface was heterogeneous, the equation was written as
(6)
log
⁡
⁡
q
e
=
log
⁡
⁡
K
F
+
1
n
log
⁡
⁡
C
e
,
where K
F   (L/mg) is the Freundlich constant related to the adsorption capacity of the adsorbent and n is the heterogeneity factor indicating the adsorption intensity of the adsorbent [27]. All of the isotherm constants and correlation coefficients computed by nonlinear curve fitting are given in Table 3. Each value in these tables is the mean of three determinations with an accepted relative standard deviation of ±3%.Table 3
Langmuir and Frenudlich isotherm parameters for Cr(VI) adsorption on NH2-MCM-41 in different temperature.
Model
Langmuir
Frenudlich
q
m
b
R
2
n
f
k
f
R
2
25°C
60.91
0.069
0.994
1.927
7.463
0.910
35°C
80.06
0.262
0.980
2.674
14.04
0.921
45°C
82.05
0.443
0.971
3.115
19.47
0.874The results show that the adsorption equilibrium data obeyed the Langmuir model, and the Langmuir model should better describe the adsorption system on NH2-MCM-41 than the Freundlich model. These results suggested that the adsorption of Cr(VI) onto NH2-MCM-41 was monolayer, and NH2-MCM-41 surface was homogeneous. Calculation of the isotherm parameters using these plots provided the data presented in Table 3. When the aqueous metal concentration increased, the saturation constant value was reached. Figure 7 shows the adsorption isotherms at 25°C, 35°C, and 45°C. The adsorption capacity of NH2-MCM-41 was compared with different temperature. The maximum Cr(VI) adsorption capacity of NH2-MCM-41 in 25°C amounted to 60.9 mg/g. Whereas the maximum Cr(VI) adsorption capacity of NH2-MCM-41 in 35°C amounted to 80.06 mg/g. On the other hand, the values of n were all greater than 1 for the different temperature, indicative of high adsorption intensity.Figure 7
Adsorption isotherms at 25°C, 35°C, and 45°C of Cr(VI) on NH2-MCM-41.Gibbs free energy change (Δ
G), entropy change (Δ
S), equilibrium constant (K
eq), and enthalpy change (Δ
H) were estimated from the following:
(7)
Δ
G
=
-
R
T
ln
⁡
⁡
b
,
ln
⁡
⁡
b
=
-
Δ
H
(
R
T
)
+
Δ
S
R
,
Δ
S
=
(
Δ
H
-
Δ
G
)
T
,
b
=
C
0
C
e
,
where b is the initial concentration of Cr(VI) removed from NH2-MCM-41 per volume of solution used for this study (
C
0
), C
e is the concentration of Cr(VI) solution at equilibrium, T is the temperature of solution measured in Kelvin, and R is the universal gas constant (8.314 J/(mol·K)) [28].Table4 shows the estimated value of thermodynamic parameters for NH2-MCM-41. The sign of the Gibbs free energy change value shows that the adsorption process was faster with the increase of temperature, and the sign of the entropy change value also shows that the process follows the increase of entropy. Additionally, the sign of enthalpy change value confirmed the endothermic disposition of the adsorption process.Table 4
Thermodynamic parameter for adsorption of Cr(VI) at different temperatures on NH2-MCM-41.
T
(
K
)
ΔG (kJ/mol)
ΔH (kJ/mol)
ΔS [J/(mol·K)]
298
-
1.506
2.024
39.876
308
-
1.665
318
-
1.843


## 4. Conclusion

Result of characterization of the MCM-41 show that the MCM-41 was successfully synthesized with silica fume (SF) as the silica source. The maximum removal of Cr(VI) was reached at a pH value of around 2.0, when the NH2-MCM-41 is the absorbent. In addition, the kinetics analysis revealed that the overall adsorption process was successfully fitted with the pseudo-second-order kinetic model. The adsorption data for Cr(VI) had a good fit with Langmuir isotherm and the maximum adsorption capacity of Cr(VI) was 82.05 mg/g at 45°C. The intensity of –
N
H
3
+ in XPS spectra decreased and the peak to the binding energies of 398.5 disappeared indicating that –
N
H
3
+ and Cr
2
O
7
2
- in the process of adsorption are held together by their mutual electrostatic attraction.



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*Source: 765856-2014-08-28.xml*