Advances in Physical Chemistry

Volume 2014 (2014), Article ID 935854, 12 pages

http://dx.doi.org/10.1155/2014/935854

Research Article

Sorption of Ammonium Ions onto Natural and Modified Egyptian Kaolinites: Kinetic and Equilibrium Studies

Ola I. El-Shafey, Nady A. Fathy, and Thoria A. El-Nabarawy

Physical Chemistry Department, Laboratory of Surface Chemistry and Catalysis, National Research Center, Dokki, Cairo 12622, Egypt

Received 26 December 2013; Revised 20 March 2014; Accepted 31 March 2014; Published 24 April 2014

Academic Editor: Taicheng An

Copyright © 2014 Ola I. El-Shafey et al. This is an open access article distributed under the Creative Commons Attribution License, which permits unrestricted use, distribution, and reproduction in any medium, provided the original work is properly cited.

Abstract.

Thermally activated, acid-activated, and acid-leached of thermally activated kaolinites were prepared from the Egyptian ore. The physical and chemical properties were studied using N₂ sorption at −196°C, FTIR, SEM, and the total surface acidity. The sorption of ions on the investigated sorbents was controlled with the solution pH, sorbent dosage, and initial concentration of solution. Kinetic and equilibrium sorption at 30°C were employed. Four kinetic models were applied to the kinetic sorption data; pseudo-second-order, Elovich, and intraparticle diffusion models fitted well the kinetic data whereas pseudo-first-order model was less applicable. Elovich parameters refer to physical sorption type of on nonuniform sites and the intraparticle diffusion controls the sorption of by kaolinites to a small extent. The equilibrium sorption data followed Langmuir and D-R models; the negative value of indicates a spontaneous sorption and the mean sorption energy obtained shows also physical sorption. The sorption capacities of nonactivated and activated Egyptian kaolinites towards sorption (10.87–45.45 mg·g⁻¹) were good sorbents as compared with those uptaken by other clays reported in the literature and proved to be more active besides being less expensive and highly available.

1. Introduction

Ammonium () is one of the most common nitrogenous pollutants in wastewater as well as in groundwater and agricultural water [1]. Also, ammonium is the inorganic ion form of nitrogen pollution contained in municipal sewage, industrial wastewater, and agricultural wastes or decomposed from organic nitrogen compounds in those wastewater and wastes. Where in the aqueous solution, ammoniac nitrogen can be classified into ammonium ion [] and free ammonia [NH₃(aq)] which are released from many industrial plants of coke, fertilizers, and metal finishing [2]. Higher concentration of ammonium will cause a sharp decrease of dissolved oxygen and obvious toxicity on aquatic organisms [3]. The amount of ammonium discharged to the environment is regulated strictly, where the maximum limit for drinking water according to the World Health Organization (WHO) is 10 mg/L of nitrate. Hence, it is of great importance to control nitrogen pollution due to the nitrification process resulting in the formation of nitrites and nitrates which lead to serious illness. Accordingly, the control of ammonia released into the environment is important in the protection of public health.

Several technologies have been employed, including precipitation [4], supercritical water oxidation [5], physicochemical [6], microwave radiation [7], ion exchange [8], and sorption [9]. Sorption of ammonium and some heavy metal ions using various types of natural and their modified clays has been studied and proved to be reliable, feasible, efficient, and less expensive as compared to the commercial activated carbon sorbents [10–15]. Of these clay sorbents investigated, the kaolinite clay gave the highest sorption capacity [14]. The layer structure and the high concentration of surface functional groups such as hydroxyl groups on kaolinite in particular stand behind its high sorption performance [15–17]. It has been reported that the sorption properties of kaolinite are related to the nature of its surface, edges, corners, porosity, and the existence of both Bronsted and Lewis acid sites which played an important role in enhancing the sorption capacity of kaolinite towards Ni and Cu (II) ions [15]. It has been pointed out that acid activation followed by thermal treatment increases the removal of phosphate to a good extent on activated kaolinite [16]. However, to our knowledge, the removal of ions onto calcined and/or acid-activated kaolinite has not been studied to date.

In the present investigation, the sorption at 30°C was conducted on natural kaolinite and thermally and acid-activated kaolinites. Activation was made either by thermal treatment, acid treatment, or acid treatment of prethermally treated kaolinite. Characterization of the sorbents was determined by XRD, FTIR, SEM, and N₂ sorption techniques. The factors controlling sorption including the solution pH, amount of sorbent dose, and initial concentration in the solution were considered. The kinetics of sorption were determined by applying pseudo-first-order, pseudo-second-order, Elovich, and intraparticle diffusion models. The equilibrium sorption data were analyzed using Freundlich, Langmuir, and Dubinin-Radushkevich equations.

2. Materials and Methods

2.1. Materials

In this work, Egyptian kaolinite clay (K) from El-Tih plateau, Egypt (kindly provided by Sinai Manganese Co.), was used as the starting material. The mineralogy of kaolinite raw was determined by means of a XRF Phillips Powder Spectrometer Model (PW 1170) using Co   radiations as published in [18]. It was found that the K contained 95% kaolinite with 5% anatase (TiO₂). The chemical analysis data are listed in Table 2. The principle aim of this work was to activate natural kaolinite by either acid, heat, or acid leaching thermally pretreated kaolinite, thereby increasing its surface area and changing its physicochemical characteristics. For this purpose, advantage was taken of the methods described by Hassan and El-Shall [18].

For the chemical activation the starting kaolinite (K) was soaked in 50% (v/v) sulphuric acid (98% assay, H₂SO₄) for 24 h at room temperature (30°C) and then activated in a muffle furnace at 886°C for 2 h. Thermal activation was accomplished by calcining kaolinite at the same temperature for 2 hours in a muffle furnace to produce metakaolinite. For the acid leaching process, the resulting metakaolinite sample was leached with 50% (v/v) H₂SO₄ for 1 h at 30°C and then raised the temperature up to 100°C for another 1 h. The treated clays were washed thoroughly with distilled water several times until they are free from and the pH of the rinsed solution reaches 6. The washed samples were centrifuged and then dried overnight at 100°C in an air oven until constant weight was attained. These samples were designated as AHK, HK, and HAK, respectively, where A stands for acid, H for heat, and K for kaolinite according to the sequence in preparation procedures.

Ammonium chloride stock (1000 mg·L⁻¹) was prepared by dissolving in deionized water. Synthetic aqueous solutions were employed by adding appropriate amount of NH₄Cl stock solution to deionized water to obtain NH₄Cl concentrations in the range of 100–1000 mg·L⁻¹.

2.2. Kaolinite Characterization

Nitrogen sorption isotherms at −196°C were constructed using a Quantachrome Nova Automated Gas Sorption instrument, where the tested samples outgas at 200°C for 2 h. Specific surface areas were calculated by the Brunauer-Emmett-Teller (BET) method. The total pore volume was obtained from the maximum amount of nitrogen gas adsorbed at a relative pressure .

The different types of functional groups were identified by a Fourier transform infrared spectrum (FTIR-6100 JASCO) in the range of 4000–400 cm⁻¹.

The total surface acidity of each sample was determined employing the method proposed by Boehm [19]. Thus, 0.1 g of each investigated samples was taken and 50 mL of 0.1 M NaOH was added to determine the acidity. The mixture was kept at a constant temperature of 30°C with constant stirring overnight. Subsequently, a 10 mL aliquot of each of the solutions in contact with the kaolinite samples was titrated employing corresponding 0.1 M standard solution of HCl.

Surface morphologies of the prepared sorbents were identified using a scanning electron microscope (SEM-JEOL, JXA-840A electron probe microanalyzer, Japan). Before scanning, the selected samples were coated with gold (Au) using a quick autocoater (JFC-1500, JEOL). X-ray diffraction (XRD) measurements of kaolinite sorbents were carried out using Phillips analytical X-ray spectrometer (PW1710) employing Cu-Kα  radiations. This technique was used to determine the structural changes that occurred in the kaolinite clay during thermal and acid treatment processes.

2.3. Sorption of Ions

Batch sorption experiments were conducted by mixing 0.1 g of sorbent with 50 mL of solutions at the desired concentration (0.01–0.2 mg·L⁻¹) in a 100 mL sealed conical flask using a shaking thermostat machine at a speed of 120 rpm/min for an equilibrium time of 2 h at 30°C. The effect of solution pH value on the equilibrium sorption of the was investigated by mixing 0.1 g of sorbent with 50 mL of solution between pH values of (5 to ). The effect of sorbent dose on the equilibrium sorption of is an important parameter since it determines the capacity of sorbate at a given initial concentration of the latter. The effect of the investigated samples dosage on the sorption of ions was studied employing 0.05, 0.1, 0.3, 0.5, and 1 g of samples K, AHK, HK, and HAK in 50 mL of solution ( 262 mg·L⁻¹).

To follow the sorption kinetics, a sample of dried sorbent (0.5 g) was added to 100 mL of the aqueous sorbate solution at an initial pH 7. Different initial sorbate concentrations ( 100, 200, and 500 mg·L⁻¹) were used for sorbate. The uptake of the sorbate per unit mass of the sorbent was followed by withdrawing a 2 mL of supernatant at fixed time intervals (min) to determine the concentration at each time, . The values of both and were measured spectrophotometrically at a wavelength 427 nm (UV-Vis spectrophotometer, Shimadzu model-PC-2401).

Also, equilibrium sorption measurements were carried out at 30°C at the optimum pH 7. Different initial concentrations of the sorbate were used and these solutions were shaken in a thermostat for 24 h to ensure equilibrium conditions. 2 mL samples were withdrawn from each sorption flask to determine the equilibrium concentrations. The amount adsorbed at equilibrium, (mg/g), was determined from the corresponding initial concentration using

where and are the initial and equilibrium liquid phase concentrations of solution (mg·L⁻¹), respectively, the volume of the solution (), and is the weight of the dry investigated sample used (g).

3. Results and Discussions

3.1. Physicochemical Features of the Kaolinite Sorbents

The textural properties (surface area and porosity) of a sorbent are important parameters [20, 21] in determining its sorption capacity as well as its sorption performance. The nitrogen sorption isotherms thus obtained (not illustrated) were analyzed using the conventional BET equation. Table 3 lists the surface area, total pore volume, mean pore diameter, and total acidity of natural and activated kaolinite samples. In Table 3, the results reveal that (i) activation with sulphuric acid (50% v/v) brought about a 100% increase in specific surface area, a 2.44-fold increase in total pore volume, a 17% increase in pore diameter, and about a 10% decrease in the total acidity; (ii) calcination of K at 886°C for 2 h was associated with a 27% decrease in the specific surface area, 21% decrease in the total pore volume, 9% increase in pore diameter, and about 20% decrease in the total acidity; (iii) concerning calcination followed by leaching with H₂SO₄, the changes were determined to be a 2.94-fold increase in specific surface area, a 2.5-fold increase in the total pore volume, a 26% decrease in the mean pore diameter, and a 41% decrease in the total acidity. It may be concluded that leaching process involves partial dissolution and reprecipitation of amorphous Si and Al materials besides the removal of other metallic oxides leaving pores within the structure and thus leading to a remarkable increase in both specific surface area and total pore volume as well as a decrease in average pore diameter (cf. Table 3). This observation was confirmed by FTIR spectra.

The chemistry of the surface, in particular, that of the surface functional groups, plays an important role in determining the sorption capacities of the investigated kaolinites for . FTIR spectra were recorded over the spectral region 4000–400 cm⁻¹ for all the kaolinites prepared. The FTIR plots (not illustrated) were used to identify the surface functional groups and results can be broadly described as follows. (i) The FTIR spectrum of natural kaolinite (K) shows bands located at 3695, 3651, and 3620 cm⁻¹ which ascribed to disordered poorly crystalline kaolinite clay. (ii) After thermal and acid treatments, the bands at wavenumber higher than 3600 cm⁻¹ disappeared in cases of HK, HAK, and AHK samples. (iii) Acid treatment of kaolinite led to appearance of a new band at 936–905 cm⁻¹ assigned to the Si-O stretching vibration of Si-OH group [22]. It is then recognized that acid treatment transforms Si-O bands to Si-OH bands [23]. (iv) The presence of a band at 795–803 cm⁻¹ is generally considered as evidence for a three-dimensional amorphous silica [18, 24, 25], suggesting the formation of a porous silica with a three-dimensional of cross-linked structure in AHK sample. These findings are in agreement with the results reported earlier by Hassan and El-Shall [18].

The scanning electron micrographs are shown in Figure 1. The micrograph of natural kaolinite (K) shows developed micropores and small particle size of the solid. The micrograph of the thermally treated kaolinite (HK) shows less micropore volume but larger particle size compared with K; this may be ascribed to a sintering process leading to agglomeration of the particles and meanwhile a decrease in the surface area associated with some increase in pore diameter. The micrograph of H₂SO₄-activated kaolinite (AHK) depicts a considerable area of black color which may be attributed to the dissolution of relatively large amount of soluble components that may form a dark film leading in turn to masking a fraction of porosity within kaolinite particles. The micrograph of HAK shows more porosity and pore grain particles compared with HK.

(a)

(b)

(c)

(d)

Figure 1: SEM photographs of the natural and modified kaolinite clays.

Furthermore, X-ray diffraction patterns (XRD) for kaolinite and its activated samples were determined (not shown here). For kaolinite, XRD profile showed well-defined reflections at values of 12.41° and 24.89° corresponding to -space values of 7.13 and 3.58 Å, respectively, which are typically characteristic peaks of kaolinite 1A [Al₂Si₂O₅ (OH)₄]. Also some quartz (SiO₂) and anatase (TiO₂) minerals were determined at values of 26.64° and 25.35°, respectively, which remained in all samples, thereby demonstrating their stability among the thermal or acid treatment. It was shown that a wide band at range 20–25° was recorded in the XRD patterns of metakaolinite sample (HK) which ascribed to amorphous silica with a three-dimensional cross-linked structure [17] as confirmed by FTIR.

3.2. Sorption of Ions

3.2.1. Effect of pH

The effect of pH on the sorption of ions from aqueous solution onto investigated samples was studied at pH 5–9 (Figure 2). For all sorbents, the maximum uptake occurred at pH 7. However, as pH increased to alkaline values, the sorption capacity decreased slightly. Solution pH affected equilibrium between the soluble ions and dissolved molecular ammonia (NH₃) in water [26]. In an acidic environment, ammonium was present as [13]. The solution H⁺ competed with to absorb on the kaolinites, so that the sorption of ions on sorbents decreased. When the pH increased to alkaline values, the nonvolatile ion paired with in the solution, which led to the formation of molecular ammonia. As the number of exchangeable ions in the interlayer increased, the removal of ammonium increased. Thus the sorption was most favorable at neutral pH; for this reason, subsequent experiments were conducted on solutions with an initial pH 7.

Figure 2: Influence of pH on the amount of adsorbed onto all investigated sorbents ( 262 mg/L; sorbent dose = 0.1 g; temperature = 30°C; contact time = 2 h).

3.2.2. Effect of Sorbent Dosage

The sorbent dosage is an important parameter, since it determines the capacity of a sorbate at a given initial concentration of the latter. The effect of K, HK, HAK, and AHK dosage (0.05, 0.1, 0.3, 0.5, and 1 g) on the sorption of ions was studied employing at 50 mL of solutions (262 mg·L⁻¹). The sorption was found to decrease as the amount of employed sorbent increased above 0.1 g as shown in Figure 3. The maximum sorption of occurred for suspension densities of 0.1 g per 50 mL of solution by K, HK, HAK, and AHK which were found to be 5.21, 12.61, 10.91, and 11.75 mg, respectively. For this reason, the optimum sorbent dosage was maintained at 0.1 g for further experiments.

Figure 3: Influence of sorbent dose on the sorption of ions ( 262 mg/L; pH = 7; temperature = 30°C; contact time = 2 h).

3.2.3. Kinetics of Sorption

The kinetics of sorption process are largely dependent on the physical and/or chemical characteristics of both the sorbent and sorbate [26–29]. The controlling mechanism in the sorption of the ions with three different initial concentrations at 30°C was examined using various kinetic models such as pseudo-first-order equation (2), pseudo-second-order equation (3), Elovich model equation (4), and intraparticle diffusion model equation (5) to determine whether processes such as mass transfer and/or chemical reaction were evolved:

where and are the amounts of solute adsorbed at equilibrium and at a time mg/g, respectively, is the pseudo-first-order sorption rate constant (min⁻¹), and is the pseudo-second-order sorption rate constant (g·mg−1 min⁻¹).

In a further attempt to study the nature of sorption, another equation, namely, Elovich equation, normally applicable to chemisorption on energetically heterogeneous solid surface, is given by [28]

where and , respectively, are the initial sorption rate (mg·g−1 min⁻¹) and the desorption coefficient (g·mg⁻¹), respectively. These can be computed from plots of versus .

If intraparticle diffusion is assumed to be the rate-limiting step in the sorption process, the Weber and Morris equation [29] is as follows:

where is the intraparticle diffusion constant (g·mg−1 min−0.5) and and have been previously identified, while is the intercept at stage .

The kinetic sorption curves at 30°C for ions were obtained with three different initial concentrations ( 100, 200, and 500 mg·L⁻¹). Figure 4 shows the influence of the time on the sorption of ions onto K, HK, HAK, and AHK. Figure 4 depicts the following. (i) Generally, the amount adsorbed increased typically with the increase of the initial concentration. (ii) All the kinetic data show a tendency to exhibit a plateau. (iii) With the exception of natural kaolinite (K), the other modified kaolinites exhibited their plateau within 10 to 20 min. Initial sorption took place on the most active sites and accordingly the earlier attainment of the kinetic plateau should be expected with sorbents rich in high activated sites for the sorbate under investigation. This may be taken as evidence that thermal treatment and/or leaching with H₂SO₄ increased the concentration of highly activated sorption sites for ions.

(a)

(b)

Figure 4: Influence of contact time on the sorption of onto all investigated sorbents (sorbent dose = 0.1 g; pH = 7; temperature = 30°C; contact time = 2 h).

All kinetic parameters arising from the application of the four kinetic models to the sorption onto K, HK, HAK, and AHK sorbents as well as the correlation coefficient values () are listed in Table 4. The pseudo-first-order kinetic equation was applied by plotting versus (not shown). No satisfactory straight lines were obtained, indicating that the sorption of ions onto the investigated samples does not follow the pseudo-first-order kinetic. On the other hand, the application of pseudo-second-order rate equation was found to be satisfactorily applicable to the sorption data in Figure 5, giving straight lines with high values of ranging between 0.9947 and 0.9980. The linear plots of this kinetic model are linear without scatter of points. Another evidence for the reliability of this model is the agreement of the calculated () and the corresponding experimental values (), indicating the dependence of the sorption rate on both the sorbent and sorbate concentrations.

(a)

(b)

Figure 5: Pseudo-second-order kinetic plots for the sorption of onto all investigated sorbents at different initial concentrations (sorbent dose = 0.1 g; pH = 7; temperature= 30°C; contact time = 2 h).

The Elovich equation was also applied to suggest the type of sorption [28]. Two representative Elovich plots of sorption are shown in Figure 6. The values of and and the corresponding are listed in Table 4. Evidently the Elovich plots are linear with high values of . The initial rate of sorption generally increases with the increase in concentration. Thus, for example, the value of at initial concentration of (100 mg·L⁻¹) adsorbed on HK was 196.4, the increase to 200 mg·L⁻¹ brought about a tremendous increase in to 17.3 × 10⁴, and the increase of concentration to 500 mg·L⁻¹ was associated again with further increase in to 30.3 × 10⁵. On the other hand, the corresponding desorption rate coefficient values are moderate and decrease with the increase in concentration. This indicates that ions were held at energetically nonuniform sites, and perhaps at chemically different sites.

Figure 6: Elovich kinetic plots for the sorption of by HK and HAK sorbents ( = 50 mg·L⁻¹; sorbent dose = 0.1 g; pH = 7; temperature = 30°C; contact time = 2 h).

The uptake of sorbate species by sorbents is usually limited by intraparticle diffusion. To determine if intraparticle diffusion was the rate-determining step for sorption, the data in Figure 4 for HK and HAK samples were replotted against the square root of time as suggested by Weber and Morris [29]. Plots of as a function of at different concentrations of solution are shown in Figure 7.

(a)

(b)

Figure 7: Intraparticle diffusion plots for the sorption of by HK and HAK sorbents (sorbent dose = 0.1 g; pH = 7; temperature = 30°C; contact time = 2 h).

The plots exhibit two linear ranges, which indicate that the sorption rate is controlled by two processes. The first step is related to the diffusion of towards the sorbent and is the fastest step where the majority of the ions can be sorbed. This is followed by the second step, which consists of intraparticle diffusion [30]. From the linear corresponding to the second step of data presented in Figure 7, the obtained values increase with increasing solution concentration, which indicates that the contribution of intraparticle diffusion to the sorption process is less significant as the amount of ions available for sorption increases. These results obtained indicate the applicability of the pseudo-second-order, Elovich equation, and intraparticle diffusion to the present sorption system.

3.2.4. Sorption Isotherm Models

The Langmuir, Freundlich, and Dubinin-Radushkevich (D-R) isotherm models were employed for fitting the experimental data [31–33]. The Langmuir model employs the assumption that the surface of the sorbent is totally homogeneous, whereas the Freundlich isotherm is suitable for a highly heterogeneous surface. The D-R isotherm, on the other hand, is based on the potential theory of sorption which assumes that the surface is energetically nonuniform and that the dominant sorption interaction involves dispersion forces. The linear form of the Langmuir isotherms is given as

where is the maximum amount adsorbed which is assumed to be the monolayer sorption capacity, both expressed in (mg·g⁻¹), and is the Langmuir constant (mg·L⁻¹) related to the free energy of sorption as expressed in (). Thus the free energy of sorption (kJ·mol⁻¹) can also be evaluated from the parameter according to the expression .

The linear form of the Freundlich equation is given as

where is the Freundlich constant related to the sorption capacity, in which is a constant related to the sorption strength, that is, the sorbent-sorbate interaction.

Another independent model was also applied to the equilibrium sorption data of ions onto the investigated samples. This model is adopted by Dubinin-Radushkevich where it assumes that only a small fraction of the surface is uniform in structure and energetically homogeneous. The D-R equation is given as

where is the monolayer sorption capacity (mg·g⁻¹), is the constant related to the mean sorption energy (g²·J⁻²), and is the Polanyi potential energy of the surface (J²·g⁻²) which equal , where is the universal gas constant (8.314 kJ·mol²²¹²¹·K⁻¹) and is the absolute temperature (K).

The linear form of D-R equation can be written as

A plot of versus    values gave a straight line. The values of and were obtained from the intercept and slope, respectively. The sorption energy (kJ·mol–1) can be obtained from the relationship:

The equilibrium sorption isotherms of ions at 30°C onto all investigated samples are shown in Figure 8. A contact time of 24 h was allowed to ensure equilibrium condition. The sorption isotherms of ions onto kaolinites exhibit very initial steep portion followed by a plateau covering a wide range of equilibrium concentrations. These isotherms are typical type isotherms according to the classification reported by Ho [34].

Figure 8: Sorption isotherms for ions by all investigated sorbents (sorbent dose = 0.1 g; pH = 7; temperature = 30°C; contact time =24 h).

The essential characteristics of the Langmuir isotherm can be expressed in terms of a dimensionless constant separation factor of equilibrium parameters , which describes the type of isotherm and is defined by the following relationship: . The parameter gives an indication of the isotherm type. Here, the magnitude of is a reflection of the isotherm shape, according to Table 1.

Table 1

Value of
Type of isotherm

Unfavorable

Linear

Favorable

Irreversible

Table 2: Chemical analysis of kaolinite clay as given in literature [18].

Oxide
Content (wt%)

Evaluated
Theoretical

SiO₂
51.51
46.3

Al₂O₃
31.43
39.8

Fe₂O₃
0.35
0–0.2

TiO₂
2.14
0–0.3

K₂O
0.01
—

CaO
1.51
—

NaO
0.50
—

SO₃
0.036
—

LOI
13.0
13.9

Table 3: Surface properties of natural and modified kaolinites.

Samples

(m²·g⁻¹)
Total pore volume

(cm³·g⁻¹)
Average pore diameter

(nm)
Total acidity

(m·equiv·g⁻¹)

K
19.1
0.0075
15.65
5.1

AHK
39.9
0.0183
18.36
5.3

HK
13.9
0.0059
16.97
4.9

HAK
56.09
0.0171
12.23
3.0

Table 4: Kinetic constants and correlation coefficients for sorption of ammonium using natural and modified kaolinite sorbents at different initial concentrations.

Sorbents
, (mg·L⁻¹)
(mg·g⁻¹)
Pseudo-first-order
Pseudo-second-order
Intraparticle diffusion
Elovich kinetic model

(mg·g⁻¹)

(mg·g⁻¹)

K
100
2.65

6.33
0.9145

2.82
0.9947
2.09
2.48
2.77
0.171
0.9811

200
7.88

10.22
0.8632

8.47
0.9987
4.55
29.30
26.49
0.071
0.9598

500
18.58

21.22
0.9335

18.87
0.9971
12.77
39.24
33.25
0.028
0.9824

AHK
100
4.44
0.0104
18.17
0.9342

4.52
0.9979
1.64
27.38
47.64
0.149
0.9554

200
10.23
0.0239
20.33
0.9424

10.70
0.9997
1.94
80.21
100.08
0.144
0.9514

500
25.65
0.0214
35.56
0.9219

24.56
0.9997
0.676
84.44
234.29
0.138
0.9538

HK
100
4.89

24.17
0.8888

5.04
0.9999
1.49
35.05
196.37
0.160
0.9645

200
9.93

25.10
0.9205

9.52
0.9997
0.407
96.45
172.18
0.142
09656

500
22.76
0.0198
44.8
0.9389

22.98
0.9995
4.58
198.96
302.19
0.069
0.9654

HAK
100
4.75
0.0161
15.1
0.8971

4.87
0.9997
1.80
30.02
65.97
0.161
0.9755

200
9.55
0.0103
14.0
0.8935

9.71
0.9998
2.37
73.69
75.01
0.135
0.9887

500
23.16

64.8
0.8773

23.25
0.9992
3.04
197.28
221.18
0.061
0.9745

The values of for the sorption isotherms of ions at 30°C were calculated. All the values are greater than 0 and less than 1, indicating the favorability of the sorption of the investigated pollutant by the investigated sorbents.

The Langmuir, Freundlich, and D-R isotherm parameters evaluated from the corresponding isotherms with their correlation coefficients are listed in Table 5. Inspection of Table 5 indicates that (i) comparing the correlation coefficient value of the linear plot of the Langmuir, Freundlich, and D-R isotherms indicated that the Langmuir model gave a better statistical fit, (ii) from Langmuir isotherm model, the calculated sorption monolayer capacity (, mg·g⁻¹) of all investigated samples for ions at 30°C decreased in the following order: AHK > HAK > HK > K, (iii) the negative value of indicates the feasibility and spontaneous nature of the sorption of ions onto the investigated samples. The fact that the Δ values were larger than −22 kJ·mol⁻¹ also shows that the sorption was a physical process [35], and (iv) for D-R sorption isotherm model, the sorption energies of the investigated samples were between 1.183 and 1.357 kJ·mol⁻¹. The sorption energy values provide information about the sorption mechanism, that is, whether it involves ion exchange or physical sorption. Thus, if the value of sorption energy is between 8 and 16 kJ·mol⁻¹, the sorption process corresponds to ion exchange process. The sorption energy values obtained in the present study were less than those expected for a typical ion exchange process, thereby suggesting that the sorption mechanism may be a combination of electrostatic and physical sorption. At the start of the sorption process (i.e., during the formation of a monolayer), ion exchange and van der Waals interactions are predominantly responsible for the process.

Table 5: Langmuir, Freundlich, and D-R isotherm parameters for sorption of ions onto natural and modified kaolinites.

Isotherm parameters
K
AHK
HK
HAK

Langmuir isotherm

     (mg·g⁻¹)
10.87
45.45
38.46
43.48

     (L·g⁻¹)
0.7022
0.3107
0.2962
0.2949

0.1246
0.2435
0.2524
0.2532

    ΔG (kJ·mol⁻¹)
−24.7
−22.7
−22.5
−22.5

0.9749
0.9750
0.9595
0.9622

Freundlich isotherm

     (mg/g)·
1.851
8.367
3.823
6.005

    1/
0.5959
0.5982
0.5550
0.8171

0.9367
0.9548
0.9499
0.9595

D-R isotherm

     (mg·g⁻¹)
7.81
18.05
16.85
17.61

     (mol²·kJ⁻²)
−2.266
−1.723
−1.064
−1.817

     (kJ·mol⁻¹)
1.183
1.357
1.221
1.321

0.9353
0.8909
0.7178
0.7878

The maximum sorption capacities (, mg·g⁻¹) for ions by the present kaolinites were compared with those by other clay sorbents reported in the literature. It was found that the prepared kaolinite showed higher sorption of than that adsorbed by other clays as follows: 10.87–45.45 mg·g⁻¹ in this study, 8.61 mg·g⁻¹—zeolite 13X [10], 9.21 mg·g⁻¹—natural clynoptilolite [11], 17.3 mg·g⁻¹—NaCl modified zeolite [13], and 30.1 mg·g⁻¹—natural Turkish bentonite [14]. Thus, the physical, chemical, and acid-leached of thermal treatments caused a remarkable increase in the sorption capacity of kaolinite clay confirming the amenability of treatment in removing ammonium from wastewater.

4. Conclusion

The sorption studies of onto the ore kaolinite and its activated samples may be considered to be a spontaneous and exothermic process, as indicated by negative values obtained for . FTIR analysis showed that the surface of the resulting sorbents was occupied by –OH functional groups. The sorption isotherms of ions onto investigated kaolinites exhibit very initial steep portion followed by a plateau covering a wide range of equilibrium concentrations. The initial interactions might be with the surface sites, but then the ammonium ions slowly enter into the pores, slowing down the entire process. The pseudo-second-kinetic-order and Langmuir isotherm models best describe the sorption of ions. Elovich and Dubinin-Radushkevich parameters refer to physical sorption. The activation of kaolinite clay thermally or chemically increases its capacity almost fourfold toward as shown in the subsequent order: K > HK > HAK > AHK. Thus the modification of natural kaolinite brings remarkable surface properties and sorption capacities. Therefore, obtained results showed that given treatment process enhanced the ability of ore kaolinite for removal from the aqueous solution.

Conflict of Interests

The authors declare that there is no conflict of interests regarding the publication of this paper.

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