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Advances in Materials Science and Engineering
Volume 2015, Article ID 897870, 8 pages
http://dx.doi.org/10.1155/2015/897870
Research Article

Adsorption of Atenolol on Kaolinite

1Beijing Key Laboratory of Materials Utilization of Nonmetallic Minerals and Solid Wastes, National Laboratory of Mineral Materials, School of Materials Science and Technology, China University of Geosciences, Beijing, 29 Xueyuan Road, Beijing 100083, China
2Geosciences Department, University of Wisconsin-Parkside, Kenosha, WI 53144, USA
3Department of Earth Science, National Cheng Kung University, Tainan 70101, Taiwan

Received 25 August 2014; Revised 12 December 2014; Accepted 13 December 2014

Academic Editor: Hanlie Hong

Copyright © 2015 Yingmo Hu 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

In this study the adsorption of atenolol (AT), a -blocker, on kaolinite, a clay mineral of low surface charge, was investigated under varying initial AT concentration, equilibrium time, solution pH, ionic strength, and temperature conditions. The results showed that the amounts of AT uptake by kaolinite were close to its cation exchange capacity value and the AT adsorption was almost instantaneous, suggesting a surface adsorption. The adsorption was exothermic and the free energy of adsorption was small negative, indicating physical adsorption. The increase in ionic strength of the solution drastically reduced AT uptake on kaolinite. A significant reduction in AT uptake was found at solution pH below 5 or above 10. The FTIR results showed band shifting and disappearance for NH bending vibration and benzene ring skeletal vibration at 3360 and 1515 cm−1 and band splitting at 1412 and 1240 cm−1 attributed to C–N valence vibration coupled with NH bending vibrations and alkyl aryl ether linkage, suggesting the participation of NH, –O–, and benzene ring for AT adsorption on kaolinite.

1. Introduction

Due to their widespread use and limited human metabolism β-blockers are widely detected in sewage effluents and surface waters [1]. In Phase I study of the risk assessment, the initial predicted environmental concentration of atenolol (AT), one of the commonly prescribed β-blockers, in surface water, was 500 ng/L, far exceeding the action limit of 10 ng/L [1]. Atenolol showed low potential for bioaccumulation as indicated by its low lipophilicity () and low affinity for sorption to the sediment [1]. However, transport of AT in sandy aquifer materials was strongly retarded despite its hydrophilic character [2]. The experimentally determined AT distribution coefficient ( value) was much higher in comparison to the other neutral compounds or carboxylic acids [3].

Common earth materials include clay minerals and zeolite, owing to their larger specific surface area (SSA) and inexpensive material costs, were studied extensively for drug uptake and release. Montmorillonite (MMT) was tested as a carrier for sustainable release of AT over a period of 24 hours in simulated gastric and intestinal fluids [4]. Extended release of AT was also tested using a multifunctional system of [SBA-15/Fe3O4/P(-iPAAm)] hybrids of interest for bioapplications [5]. Sorption of AT on fine ceramic pseudoboehmite resulted in no loss in its chemical stability [6]. Attapulgites modified by different reagents including hydrochloric acid, silane coupling agent, and chitosan showed extensive uptake of propranolol, another β-blocker medicine [7]. Adsorption of AT on a kaolinite, a bentonite, and a zeolite reached 20, 20, and 40 mmol/kg, respectively, while modification of the kaolinite and bentonite with an organic cation octadecyltrimethylammonium resulted in minimal influence on AT adsorption capacity but reduced affinity [8].

In addition to common Earth materials, removal of AT by activated carbon (AC) or granular activated carbon (GAC) was also conducted [9, 10]. Column experiments showed that AT breakthrough time decreased as its input concentration and flow rate increased and column length decreased [10, 11]. The amounts of AT uptake on AC or GAC were as high as 750 mmol/kg [10].

Even with this progress, conflict results were reported on interactions between AT and Earth materials. The strongest retardation and therefore the highest values were observed for the cationic compounds AT, diazepam, and trimethoprim [2]. On the contrary, AT showed a low affinity for the sediment and a rather low DT50 (dissipation time at which 50% of the substance is removed) of 3 d for the water compartment [1]. A similar low affinity for stream sediment was also found [12].

In addition to adsorption, degradation of β-blockers was also experienced in extensive study, though with conflict results. One study found that AT was not readily ultimately biodegradable [1]. In another study, elevated biodegradability in the surface water-sediment systems with 90% disappearance (DT90) for AT was observed in 10 days [12]. Abiotic processes, most likely sorption of the positively charged AT to clay minerals, dominated the first 5–10 d of the AT removal experiment under nitrate reducing conditions, yielding removal of about 14% [13]. In the presence of hydroxyl radical six atenolol decomposition products at detectable levels were revealed by LC-MS at multiple irradiation doses; however, the fraction of hydroxyl radical available to degrade the atenolol was only 0.19% [14]. Under 240 min UVA irradiation in the absence of catalyst, the extent of photolytic conversion of AT was only 12%, but the conversion increased to 85% in the presence of TiO2 as the photocatalyst [15]. In addition, the data on AT removal were very inconsistent and the removal rates varied from less than 10% up to 95% depending on the treatment [16].

As the presence of solid would strongly affect the distribution of pharmaceutical compounds between the solid and liquid phases, which would ultimately affect the performance of their biotic or abiotic degradation, it is necessary to assess the degrees of uptake of pharmaceutical compounds on solid under different physic-chemical conditions. Because of the lack of ecotoxicological data, low metabolism, wide use, and frequent detection in sewage effluents and receiving waters [1], AT was chosen in this study for its interactions with low charge clay minerals, using kaolinite as an example.

2. Materials and Methods

The material used was KGa-2, a poorly crystalized kaolinite obtained from the Clay Mineral Repository in Purdue University. It had a cation exchange capacity (CEC) value of 37 mmol/kg [17], with Na+, Ca2+, and Mg2+ as the major exchangeable cations. It has an SSA of 21.7 m2/g [18]. It was used without further pretreatment.

The atenolol (CAS number: 29122-68-7) with a purity of >98% was purchased from Tokyo Chemical Industry Co., Ltd. (Figure 1). It has a formula mass of 266.336 g/mol and a value of 9.6 [1, 1921]. Its solubility in pure water was 9.34 g/L [22]. An experimental and predicted solubility of and −1.94, corresponding to 13 and 3 g/L, was also reported [23, 24]. At 37°C its solubility increased to 37 g/L [15]. A value of 0.1 [1, 13] and a of 44 L/kg for sludge [1] were also reported. Stable concentrations of AT were observed in the control samples with Milli-Q water [3].

Figure 1: Molecular structure of atenolol. It could be a racemic mixture and the chiral center is at the C marked with an arrow. The red is O, the blue is N, and the dark gray is C, while the white is H.

For the AT adsorption isotherm study, 1.0 g of kaolinite and 10 mL of AT at concentrations of 0.0, 0.6, 1.2, 1.8, 2.4, 3.0, 3.6, and 4.0 mmol/L were combined in 50 mL centrifuge tubes. For all other studies, the initial AT concentration was fixed at 2.0 or 4.0 mmol/L. For AT adsorption kinetics, the equilibrium time was 0.25, 0.5, 1, 2, 4, 8, 16, and 24 h. The equilibrium solution pH was maintained at 2–11 with an increment of 1 for the pH-dependent study, while the ionic strength was adjusted to reach NaCl concentrations of 0.001, 0.01, 0.1, and 1.0 M. The temperature study was conducted at 22, 32, and 42°C. The mixtures were shaken at 150 rpm for 24 h, except the kinetic study, and were then centrifuged at 3500 rpm for 10 min, and the supernatants passed through 0.45 μm syringe filters before being analyzed for the equilibrium AT concentrations using an UV-Vis method.

The AT concentration was measured by an UV-Vis method at a wavelength of 274 nm [25, 26]. The absorbance value at this wavelength was stable at pH 1–11 ranges [4]. In this study, the absorbance was determined at a wavelength of 236 nm. At this wavelength, the absorbance value was also pH-independent at pH 1–11 ranges [4]. Meanwhile, the absorbance value at this wavelength is large, making it more sensitive for AT analyses.

The FTIR analysis was conducted using a Jasco FT/IR-4100 spectrometer equipped with a ZnSe crystal and attenuated total reflection (ATR) accessory. The spectra were obtained from 600 to 4000 cm−1 by accumulating 256 scans at a resolution 4 cm−1. Powder XRD analyses of AT-adsorbed kaolinite were carried out with CuKα radiation at 40 kV and 40 mA on a D8 ADVANCE diffractometer (Bruker Corp.). Unoriented samples were scanned from 2 to 22° 2θ with a scanning speed of 0.01°/s. The desorption of exchangeable cations was determined using an ion chromatography (IC).

Molecular simulation was performed using the module Forcite of Materials Studio 6.0 software to investigate the sorption sites of AT on kaolinite. The kaolinite model was constructed and the atomic coordinates were derived from the space group of C1 with  Å,  Å,  Å, °, °, and °. The supercell of the model was made of 12 kaolinite unit cells at . The established model was optimized geometrically. The temperature was set at 298 K and time was 1 ns with a time step of 1 fs. Universal force field was used during the simulation. The Ewald summation method was used to calculate the electrostatic interaction. After the system reached equilibrium at about 500 ps, the NVT kinetic simulation was performed under the same time constant and temperature conditions. The data were collected at the last 500 ps for later analyses.

3. Results and Discussion

3.1. AT Adsorption Isotherm

Adsorption of AT on kaolinite followed the Langmuir adsorption isotherm (Figure 2): where is the amount of AT adsorbed at equilibrium (mmol/kg), the apparent sorption capacity (mmol/kg), the equilibrium AT concentration (mmol/L), and the Langmuir coefficient (L/mmol). Equation (1) can be rearranged to a linear form: so that and can be determined by linear regression. The adsorption capacity of AT on kaolinite was 40 mmol/kg and the was 1.25 L/mmol. The values are comparable to AT adsorption at 20, 20, and 40 mmol/kg on kaolinite, bentonite, and zeolite, respectively [8].

Figure 2: Adsorption of atenolol on kaolinite. The line is the Langmuir fit to the observed data.

The equilibrium uptake of AT on an MMT also followed the Langmuir model with an AT adsorption capacity of 86 mg/g or 320 mmol/kg [4]. Multilayer adsorption of AT on natural kaolin was indicated by slight increase of AT adsorption values in the last part of the isotherm [8]. A linear adsorption of AT on some river sediments or silt loam soil was reported with values ranging from 1.3 for the river sediments to 110 L/kg for the silt loam soil due to its higher CEC value [3]. Adsorption of AT on GAC reached a capacity of 750 mmol/kg in comparison to the measured basicity of 802 mmolc/kg [10].

3.2. AT Adsorption Kinetics

AT adsorption on kaolinite was very fast, especially when the initial AT concentration was low (Figure 3). The equilibrium could be reached in less than half an hour. This quick sorption may indicate a surface process; thus diffusion may not play a significant role. The data of AT adsorption were fitted to several kinetic models and the pseudo-second-order model fitted the experimental data well [27]: where and are amounts of AT adsorbed at equilibrium and at time (mmol/kg) and is the pseudo-second-order rate constant (kg/mmol-h). Equation (3) can be rearranged to a linear form so that and can be determined by linear regression. The rate constants thus obtained were 0.1 and 1.9 kg/mmol-h, and the initial rates were 68 and 476 mmol/kg-h, for AT adsorption on kaolinite from initial concentrations of 4 and 2 mmol/L.

Figure 3: Kinetics of AT adsorption on kaolinite from initial concentrations of 2 and 4 mmol/L. The lines are pseudo-second-order fits to the observed data. Inset is the plot based on  (4).

A rate constant of 0.082 g/mg-min or 1.2 kg/mmol-h was reported for AT adsorption on MMT [4]. The values were 25 and 16 mmol/kg, agreeing well with the isotherm study. Sorption of AT on AC reached equilibrium in less than 2 h [9] or less than 8 h [10]. The quick AT adsorption on kaolinite confirmed that surface adsorption is the dominant process and diffusion may not play a significant role.

3.3. Solution Ionic Strength Effect

The amount of AT adsorbed decreased from 16 mmol/kg at very low ionic strength to almost zero at a background NaCl concentration of 1 mol/L (Figure 4). In addition, the free energy of adsorption can be calculated from the by where is the gas constant and is the reaction temperature in . A systematic increase in was found as the solution ionic strength increases, reflecting strong completing effect of background salt NaCl against AT adsorption. Previous results showed that, with the increase of Na+, more and more sorbed propranolol molecules desorbed into the aqueous phase [7].

Figure 4: Influence of solution ionic strength on AT adsorption on kaolinite from 2 mmol/L solution and changes in free energies associated with AT adsorption.
3.4. pH Effect

Solution pH had a significant effect on AT uptake by kaolinite (Figure 5). When solution pH was below 5 or above 10, the uptake of AT on kaolinite was drastically reduced (Figure 5). Similarly, aqueous phase pH showed significant influence on AT adsorption onto AC with the highest AT adsorption at pH 7 [9]. The solubility of AT was higher than 1 mol/L when solution pH was below 7 and increased with decreasing solution pH [23]. Even at pH 11, the solubility of AT was still much greater than the initial concentration of 2 mmol/L [23]. Thus, precipitation would not be a factor for the reduced AT adsorption under low and high pH conditions. The decreased AT uptake under low solution pH conditions could be attributed to competition between H+ and ATH+ for sorption sites. Meanwhile, as the solution pH was higher than the of AT, the significant reduction in AT uptake could be attributed to the loss of electrostatic interactions between neutral AT molecule and negatively charged kaolinite surfaces. In contrast, relatively stable adsorption of propranolol on attapulgites or modified attapulgites was found in initial pH 3–11 range [7]. The AT retardation factor in a sandy aquifer material decreased from 23.3 to 15.8 as the pH increased from 4 to 8 [2].

Figure 5: AT adsorption on kaolinite as affected by equilibrium solution pH.
3.5. Temperature Effect

As the temperature increased, the decreased, reflecting a slightly exothermic reaction for AT adsorption on kaolinite (Figure 6). Also, the changes in enthalpy after AT adsorption from 2 to 4 mmol/L solution were −25 and −14 kJ/mol, confirming the exothermic reaction. Moreover, the values were in the range from −7 to −9 kJ/mol (Table 1), much less than the changes affected by solution ionic strength. In comparison, adsorption of AT on AC showed endothermic feature, too, with , , and values of −2–−5 kJ/mol, 29 kJ/mol, and 0.09 kJ/mol/K, respectively [9]. The lower negative values of for AT adsorption on kaolinite may indicate physical adsorption such as cation exchange processes as observed in the case of ciprofloxacin adsorption on the same kaolinite [28].

Table 1: Thermodynamic parameters of AT adsorption on kaolinite.
Figure 6: Change in distribution coefficient as affected by temperature for AT adsorption on kaolinite.
3.6. FTIR Analysis

The FTIR spectra of kaolinite adsorbed with different amounts of AT displayed both bands of raw kaolinite and AT (Figure 7(a)). Their characteristic band locations and assignments were listed in Table 2. The IR spectrum of the pure AT displayed characteristic peaks at 3362 cm−1, 3172 cm−1, and 1636 cm−1 due to O–H, N–H, and C=O groups, respectively [6, 29, 30]. Other bands observed were at 1245, 1510, 1184, 805, and 820 cm−1 [6]. For pure AT the strong band at 1638 cm−1, originating from C=O valence vibrations (amide band I), decreased significantly and shifted to 1668 cm−1, after inclusion into the cavity of 2-hydroxypropyl-β-cyclodextrin owing to the restriction of this vibration [29]. After the interaction with pseudoboehmite it shifted to 1650 cm−1 [6]. In this study, similar observation was found, and the band shifted from 1633 to 1654 cm−1 with a significant decrease in its intensity (Figure 7(b)).

Table 2: FTIR bands for AT and AT adsorbed on KGa-2.
Figure 7: FTIR spectra of crystalline AT, and kaolinite with different amounts of AT adsorption in the ranges of 600–4000cm−1 (a) and 1100–1700 cm−1 (b). The values indicate initial AT concentrations in mmol/L.

The peak of 2972 cm−1 was due to C–H stretching [4]. It remained in the same location after AT adsorption on kaolinite (Table 2). A small band at 3350 cm−1 and 1506 cm−1 corresponding to NH bending vibration and benzene ring skeletal vibration, respectively, from AT also appeared in MMT-AT complex and was attributed to the presence of organic cations AT in the interlayer region of the MMT layers [4]. In this study, the 3350 cm−1 band that occurred at 3360 cm−1 shifted to 3410 cm−1 after adsorption on kaolinite, while the benzene ring skeletal vibration was at 1515 cm−1 and also disappeared after AT adsorption on kaolinite. Similarly, the band at 1515 cm−1 disappeared after forming MMT-AT complex [29].

The peak at 1240 cm−1 was due to alkyl aryl ether linkage [4]. In this study, there is a single sharp peak located at 1237 cm−1 for crystalline AT. However, this peak split into two peaks, located at 1230 and 1252 cm−1, respectively, after being adsorbed onto the surface of kaolinite (Figure 7(b)). The amide band III, originating from the C–N valence vibration coupled with NH bending vibrations, occurred at 1417 cm−1 for crystalline AT but was absent when forming a complex with MMT [29]. Similarly, this band was split into two bands also (Figure 7(b)). The band at 3180 cm−1 originating from the NH valence vibrations was present in the spectrum of crystalline AT but was absent after being uptaken on MMT [29]. This band occurred at 3158 cm−1 but was absent after being adsorbed on kaolinite (Table 2). New peaks at wavenumbers 2300 cm−1 and 1719 cm−1 (NC=N–, NC=C, C=O stretch) were noticed on AC after AT adsorption and were attributed to chemical type of adsorption reaction [9]. In this study, these two new peaks were never observed.

3.7. X-Ray Diffraction Analysis

The characteristic peaks of AT are located at 2θ at 3.2, 6.4, and 9.6°, corresponding to (200), (400), and (600) diffractions [31]. These peaks were present in the mixture of AT and kaolinite at the level of 25 mmol/kg (Figure 8). However, these peaks were absent after being adsorbed on kaolinite surfaces, suggesting that the removal of AT from solution was via sorption instead of precipitation. In addition, the (001) peak of kaolinite did not change at all (Figure 8), indicating that AT sorption sites were on the external surface or edges, instead of interlayer. Similar results were observed in the XRD patterns of physical mixture of AT and hydrophilic swellable polymers, indicating that AT was completely dispersed in the solid substrate [32].

Figure 8: X-ray diffraction patterns of kaolinite adsorbed with different amounts of AT. The values are initial AT concentrations.
3.8. Discussion on AT Adsorption Mechanism

Although several studies were reported on the uptake and adsorption of AT by AC, sediments, and some clay minerals, mixed results often lead to contradicting results. Cation exchange was attributed to the dominating role for the retardation of AT in different sediments [2, 3]. However, similar AT adsorption capacities on both kaolinite and bentonite were obtained, even though the CEC of kaolinite was much lower than that of bentonite, which seemed that the uptake of TA on these minerals was not strongly related to the cation exchange processes [8]. Moreover, the contribution of electrostatic interactions to overall adsorption of AT on sediments and sludge was thought rather small, as significant shifting of AT from solution into the sediment was not observed [1]. In one study, adsorption onto organic carbon was considered as the relevant adsorption process for AT uptake onto sediments [1]. On the contrary, the influence of organic matter on the adsorption of AT and metoprolol on aquifer sediments was much less important [33].

In this study, the AT adsorption capacity on kaolinite was 40 mmol/kg, while the CEC of the kaolinite was 37 mmolc/kg [17]. Thus, to the first degree, the AT adsorption capacities matched the CEC values of these minerals well. In addition, the reduced AT uptake at low pH and high ionic strength conditions also suggested that cation exchange mechanism or electrostatic interactions played important roles on AT uptake by kaolinite. However, IC results showed nondetectable Na+, K+, Mg2+, and Ca2+ in the supernatants, suggesting no release of exchangeable cations after AT uptake (data not shown). In contrast, stoichiometric release of exchangeable cations was observed after ciprofloxacin adsorption on the same kaolinite [28].

A newly proposed cation exchange model that defined the adsorption of organic cations to soil as a summed contribution of adsorption to organic matter (OM) and adsorption to phyllosilicate clay minerals showed good agreement between the observed and predicted values within a factor of 3 [34]. The equation used was where was the faction of organic carbon and and were the ion-exchange-based adsorption coefficients for NOM and clay. However, due to the fact that AT adsorption on kaolinite did not follow the linear adsorption isotherm and the value for the pure kaolinite was essentially zero, the value in this study varied with the equilibrium AT concentration. Thus, for pure clay minerals, this equation may not be applicable.

One important piece of information from the FTIR study was the breakup of the bands at 1412 and 1240 cm−1, each into two. These bands were attributed to NH bending vibrations [29] and alkyl aryl ether linkage [4]. Thus, it is more likely that the adsorption of AT on low charge kaolinite was via electrostatic interaction between the amine group of AT and the negatively charged mineral surface and/or hydrogen bonding between the hydroxyl group of the kaolinite and the alkyl aryl ether linkage, as confirmed by molecular simulation of AT adsorption on the (100) and (010) surfaces of kaolinite (Figure 9).

Figure 9: Interactions between AT and kaolinite on (100) (a) and (010) (b). Dashed lines indicate hydrogen bonding.

4. Conclusions

Strong interactions between AT and kaolinite were revealed in this study. The AT adsorption capacity on kaolinite was close to its cation exchange capacity value and the AT adsorption was almost instantaneous, suggesting surface adsorption instead of intercalation, as confirmed by X-ray diffraction analyses. Both solution pH and ionic strength had significant effect on AT adsorption on kaolinite. An increase in ionic strength of the solution drastically reduced AT adsorption and at solution pH below 5 or above 10 AT adsorption was significantly reduced, too. The FTIR results showed band shifting and disappearance for NH bending vibration and benzene ring skeletal vibration at 3360 and 1515 cm−1 and band splitting at 1412 and 1240 cm−1 attributed to C–N valence vibration coupled with NH bending vibrations and alkyl aryl ether linkage, suggesting the participation of NH, –O–, and benzene ring for AT adsorption on kaolinite. Molecular simulation results confirmed the FTIR observations.

Conflict of Interests

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

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