Differential removal of tetracycline hydrochloride and quinolone antibiotics by calcined and uncalcined layered double hydroxides
Abstract
Antibiotics generally cause drug-resistant genes (ARGs) and drug-resistant bacteria (ARBs). With a complex class of antibiotics, it is very crucial to select specific adsorbents for different kinds of antibiotics. Zn-Al layered double hydroxide (LDH) and calcined layered double hydroxide (LDO) were prepared as absorbents for tetracycline hydrochloride (TCH) and ofloxacin (OFX), which were two antibiotics with different structures. According to the results of the adsorption experiments, LDO has the best adsorption capacity on TCH, reaching 322.58 mg/g. Acid-base titration, XRD, TEM, SEM, BET, and FI-TR analyses indicate that LDO has more active sites on the surface, the “memory effect”, and a larger specific surface area. In contrast, the removal rate of OFX by LDO is low because OFX has a more stable quinolone ring structure. Furthermore, after five adsorption-desorption cycles, the adsorption rate of TCH remains at 94.9%, demonstrating that LDO has good cyclic adsorption capacity for TCH. This study creatively combines acid-base buffering characteristics to study the mechanism of the adsorption of antibiotics by hydrotalcite, and proposes that LDO can be used as a special adsorbent for TCH.
Keywords
INTRODUCTION
More and more antibiotics are found in natural water bodies, and they always lead to an increase in drug-resistant genes (ARGs) and drug-resistant bacteria (ARB), which result in long-term persistent ecological toxicity[1]. According to survey data, in 2019, residual antibiotics caused more than 2.8 million infections and 35,000 fatalities in the United States[2]. Membrane separation[3], photocatalytic degradation[4], adsorption[5], electrochemical oxidation[6] and others are widely used for antibiotic wastewater treatment. Adsorption with low-cost adsorbents is considered to be the most suitable method[5]. Hu et al.[7] concluded that magnetic conjugated microporous polymer hollow spheres (CMP-HSs@Fe3O4) potentially adsorb antibiotic molecules effectively. However, not every kind of adsorbent is suitable for antibiotics including quinolones, aminoglycosides, macrolides, oxazolidinones, tetracyclines, etc. Therefore, it is particularly important to use specific adsorbents for various antibiotic wastewater.
Hydrotalcite-type clays belong to a member of layered structure clays, which are also known as layered double hydroxides. It was first discovered in schist deposits in 1,842 by Hochstetter[8], and its catalytic action on hydrogen addition attracted the attention of researchers. Nowadays, various types of layered double hydroxides (LDHs) have been synthesized, and their chemical formula is generally
The chemical properties of the solid surface play a decisive role in physical and chemical processes such as solid adsorption, desorption, and ion exchange[15]. The surface complexation models (SCMs) are mainly used to study the chemical reactions occurring at the solid-liquid interface. Hydroxy proton transfer occurs in the aqueous solution, some located on the surface of the metal are called Lewis acid, and others losing protons are called Lewis base, both of which react with ligands in the solution[16,17]. Protonation and deprotonation of surface functional groups on the material make a significant contribution to the acid-base buffering capacity. At present, acid-base buffering characteristics of materials are commonly used to reflect the surface chemical properties of solid materials[18].
tetracycline hydrochloride (TCH)[19] and ofloxacin (OFX)[20] are typical representatives of tetracyclines (TCs) and quinolone antibiotics, respectively, which are two common antibiotics. Therefore, in this study, a special adsorbent for the specific antibiotic will be proposed, and the acid-base buffering properties of the materials will be investigated to study the adsorption mechanism.
EXPERIMENTAL
Materials
Urea, Zn(NO3)2·6H2O, Al(NO3)3·9H2O, HNO3, HCl, NaNO3, NaOH, Na2CO3, potassium hydrogen phthalate, phenolphthalein indicator, bromocresol green, methyl- red and anhydrous ethanol were purchased from Sinopharm Chemical Reagent Co. (Shanghai, China) and were analytical grade. Deionized water (around 15 MΩ/cm) was used in experiments.
Preparation
Compared with other preparation methods, the urea synthesis method achieves a larger yield and higher crystallinity[21]. 250 mL deionized water, 0.525 mol urea, 0.15 mol Zn (NO3)2·6H2O, and 0.075 mol Al
Characterizations
The crystal structures of materials were characterized with XRD (D8, Brucker, Germany). The microstructures of the materials were characterized by TEM (Talos F200S, Thermo Scientific, America) and SEM (JSM 7100F, Jeol, Japan). The specific surface areas were determined by BET (ASAP2020, Micromeritics, America). FT-IR spectrometer (Vector-22, Bruker, Germany) was used to study the adsorption mechanism.
Acid-base titration
The automated potentiometric titrator (907 Titrano, Metrohm Corporation, Switzerland) was used to determine the titration data. The material was exposed to 0.1 mo1/L NaNO3 solution in a water bath at
Batch adsorption experiments
HCl and NaOH were utilized to regulate the pH of the solutions for the batch adsorption experiments. The effects of original pH (TCH: 2.5, 4.5, 6.5, 8.5, 10.5; OFX:3, 5, 7, 9, 11) on the adsorption abilities of LDH and LDO were studied, respectively. Different dosages of materials ranging from 0.02 g to 0.12 g were added to the antibiotic solutions to investigate the effects of adsorbent dosages on the adsorption effect. Samples were exposed to a range of antibiotic concentrations (TCH: 5-500 mg/L; OFX: 5-120 mg/L) for the kinetics experiments. The isotherm experiments were carried out at 293.15 K. The adsorption ability (qe) and adsorption rate (R) are calculated as Equations (1) and (2).
where C0 (mg/L) and C1 (mg/L) are the concentration of antibiotics before and after adsorption; m (g) and V (L) are the mass of adsorbent and the volume of antibiotic, respectively.
In order to study the cyclic adsorption performance, LDO after adsorption of TCH was calcined at 450 °C for 4 h for desorption. Considering the material loss during operation, TCH-LDO liquid-solid ratio was fixed at 0.25 g/L during the five-cyclic adsorption experiment[25].
RESULT AND DISCUSSION
Microstructural characterization LDH and LDO
XRD analysis
According to Figure 1A, LDH was synthesized with high crystallinity (JCPDS 48-1021). After calcination, characteristic peaks such as (003), (006), and (009) disappear and are replaced by low strength and scattered diffraction peaks, indicating that LDO lost its lamellar structure to form Zn oxide and Zn-Al composite oxides[26].
Figure 1. XRD patterns of (A) LDH, LDO; (B) before and after adsorption of LDH on TCH and OFX; (C) LDH, before and after adsorption of LDO on TCH and OFX; (D) LDH, LDO, before and after adsorption of LDO on TCH at the fourth and fifth times. LDH: Layered double hydroxide; LDO: layered double hydroxide; OFX: ofloxacin; TCH: tetracycline hydrochloride.
TEM analysis
The morphologies of LDH and LDO are shown in Figure 2. The obvious layered structure of LDH can be seen in Figure 2A. The crystal plane spacings of d1 = 7.6200 nm and d2 = 3.8100 nm correspond to (003) and (006) of LDH as in Figure 2C (JCPDS 48-1021), which also indicates that LDH was successfully prepared. Some lamellar structures are still observed in the TEM images of LDO [Figure 2B] due to “the memory effect” under the influence of ethanol during TEM measurement[27]. In Figure 2D, d1 = 2.4759 nm and d2 = 2.6033 nm correspond to (101) and (002) of ZnO (JCPDS 36-1451), d3=2.442 nm corresponded to (311) of ZnAl2O4 (JCPDS 74-1138). The results are consistent with XRD characterization results.
Figure 2. TEM images of (A) LDH at bar = 200 nm; (B) LDO at bar = 5 nm; (C) LDH at bar = 5 nm; (D) LDO at bar = 5 nm.
SEM
LDH shows a distinct lamellar structure [Figure 3A], but LDO loses its lamellar structure and instead appears as a collapsed state with many micropores [Figure 3B]. The alteration of the structure of LDO may potentially enhance the adsorption capability.
Figure 3. SEM images of (A) LDH; (B) LHO.
BET
Based on the IUPAC classification[28], the N2 adsorption and desorption isotherms curves of the materials are categorized as type IV, as demonstrated in Figure 4. Compared with LDH, LDO exhibits superior performance attributed to its larger surface area and pore volume, as outlined in Table 1. The result explains the SEM images and indicates that LDO has a superior adsorption capacity than LDH[29].
Figure 4. N2 adsorption/desorption isotherms of LDH and LDO. LDH: Layered double hydroxide; LDO: layered double hydroxide.
Specific surface area (BET), capillary diameter, and volume capillaries of LDH and LDO
| Materials | Surface area BET (m2/g) | Porous diameter (nm) | Porous volume (cm3/g) |
| LDH | 21.11 | 26.10 | 0.14 |
| LDO | 96.15 | 7.77 | 0.19 |
Batch adsorption experiments
Effects of pH and adsorbent dosage on adsorption
According to Figure 5A and B, pH has little effect on the stability of TCH and OFX but has significant effects on the adsorption abilities of the adsorbents. The performances of adsorbents for TCH and OFX reach the maximum at pH 8.5 and pH 7, respectively. Compared with the acidic condition, an alkaline environment has a more negative influence on the removal rate.
Figure 5. Effects of pH on absorption of (A) TCH (30 mg/L) and (B) OFX (20 mg/L) by LDH and LDO; effects of LDH and LDO dosage on the absorption of (C) TCH and (D) OFX. CK: Blank control group; LDH: layered double hydroxide; LDO: layered double hydroxide.
The adsorbent dosage also plays an important role in the adsorption process [Figure 3C and D]. Overall, the adsorption performance of LDO is better than that of LDH. When the dosages of LDH and LDO reach 0.1 g and 0.06 g, respectively, the removal rates of TCH and OFX tend to be steady.
Adsorption kinetics
The pseudo-first-order model and the pseudo-second-order model are applied to explore the adsorption kinetic behavior and provide a basis for the adsorption mechanism[30].
For the pseudo-first-order model[31]
For the pseudo-second-order model[32]
where qe and qt are the abilities of the material adsorbing antibiotics at equilibrium and at time t (min). K1 and K2 separately are the constants of the two dynamics.
As shown in Figure 6 and Table 2, the correlation coefficients of the pseudo-second-order model are greater than those of the pseudo-first-order model. It demonstrates that the adsorptions are primarily chemical processes, in which the concentration of adsorbents and antibiotics jointly control the adsorption rates. In other words, the sharing and transferring of electrons between the absorbents and the antibiotics are most likely the main factors[33].
Figure 6. (A) Adsorption kinetics of LDH and LDO absorbing TCH/OFX. (A) The pseudo-first-order model; (B)the pseudo-second-order model. LDH: Layered double hydroxide; LDO: layered double hydroxide; OFX: ofloxacin; TCH: tetracycline hydrochloride.
The kinetic parameters of antibiotics on LDH and LDO
| Pseudo-first-order model | Pseudo-second-order model | |||||
| Materials | qe (mg/g) | K1 | R2 | qe (mg/g) | K2 | R2 |
| LDH-TCH | 4.86 | 0.013 | 0.886 | 8.028 | 0.125 | 0.982 |
| LDH-OFX | 12.12 | 0.025 | 0.868 | 10.018 | 0.100 | 0.990 |
| LDO-TCH | 5.67 | 0.055 | 0.927 | 11.132 | 0.090 | 0.989 |
| LDO-OFX | 8.10 | 0.019 | 0.970 | 8.774 | 0.114 | 0.983 |
Adsorption isotherms
Adsorption isotherms are used to describe the relationship between adsorption capacity and adsorption equilibrium concentration[30]. Langmuir model and Freundlich model are commonly adsorption isotherm models, which are represented as follows.
For Langmuir model[22]:
where Ce (mg/L), Qe (mg/g), QM (mg/g) represent equilibrium concentration, equilibrium adsorption capacity, and maximum adsorption capacity, respectively.
Meanwhile, based on the Langmuir adsorption isotherm, the dimensionless factor RL can be used to characterize the difficult degree of adsorption. When RL is in the range of 0-1, it indicates that the adsorption is easy to carry out[34].
where KL is Langmuir constant and C0 (mg/L) is the initial concentration.
For Freundlich model[31]:
where KF expresses the Freundlich constant; 1/n represents adsorption intensity[35].
According to Figure 7 and Table 3, the Langmuir model is more suitable for the adsorption process than the Freundlich model. The saturated adsorption capacities of materials on TCH and OFX are 112.87, 55.04, 324.68, and 72.89 mg/g, respectively. Moreover, the dimensionless factors RL of adsorbents adsorbing TCH and OFX calculated by Equation (6) are 0.42, 0.73, 0.259, and 0.09 mg/g, which are in the range of 0-1. It demonstrates the effective adsorption of materials and antibiotics.
Figure 7. Adsorption isotherms of adsorbents absorbing TCH and OFX (A) Langmuir model; (B) Freundlich model. LDH: Layered double hydroxide; LDO: layered double hydroxide; OFX: ofloxacin; TCH: tetracycline hydrochloride.
The isotherm parameters of antibiotics on LDH and LDO
| Langmuir | Freundlich | |||||
| Materials | QM (mg/g) | KL | R2 | 1/n | KF | R2 |
| LDH-TCH | 112.87 | 0.046 | 0.961 | 0.334 | 15.782 | 0.927 |
| LDH-OFX | 55.04 | 0.019 | 0.974 | 0.434 | 13.000 | 0.892 |
| LDO-TCH | 324.68 | 0.096 | 0.928 | 0.323 | 58.545 | 0.902 |
| LDO-OFX | 72.89 | 0.526 | 0.949 | 0.262 | 27.424 | 0.809 |
Cyclic adsorption experiment
According to Figure 8, LDO has a good adsorption effect on TCH during five adsorption cycles. At the fourth adsorption, the adsorption rate begins to slow down, and the adsorption equilibrium time is extended from 50 min to 100 min. At the fifth adsorption, the removal rate decreases from 95.19% to 94.89%. Therefore, the LDO4 finishing the fourth adsorption, and the LHO5 finishing the fifth adsorption are characterized by XRD [Figure 1D].
Figure 8. Cyclic adsorption experiment of TCH absorption by LDO.
LDO4 as well as LDO5 recover lamellar structures with the unique “memory effect”[36]. Compared with LDH, the diffraction peak intensity of LDO4 and LDO5 decreased significantly. Moreover, the characteristic peaks of Zn oxide and Zn-Al composite oxides appeared at 31.79° and 36.24°, which show that multiple high-temperature desorptions weaken its reconstruction performance. It explains why the fourth and fifth adsorption rates in the cyclic adsorption process have a lower adsorption rate and an extended equilibrium time. However, its obvious diffraction peaks are still observed, and the removal rate of TCH remains at 94.9%, indicating that LDO can achieve multiple cyclic adsorptions. Meanwhile, a new peak is generated at 37.29°, indicating that new substances are produced during the adsorption of TCH.
Adsorption mechanisms
FT-IR
After absorbing the antibiotics [Figure 9A], the peak at 3,447 cm-1 is blue-shifted, which indicates that hydrogen bonds formed between the adsorbents and the electronegative atoms of the two antibiotics. After the adsorption of TCH and OFX, the characteristic amino group peaks at 3,064 cm-1, 3,060 cm-1, and
Figure 9. FT-IR spectrum comparison of (A) LDH and (B) LDO adsorbed antibiotics. LDH: Layered double hydroxide; LDO: layered double hydroxide; OFX: ofloxacin; TCH: tetracycline hydrochloride.
XRD
After the adsorption of antibiotics, the characteristic diffraction peaks intensities of LDH, particularly TCH-LDH, clearly decrease in Figure 1B. And new peaks appear, and measurements of the crystal plane spacings (d1 = 2.4172 nm and d2 = 2.0631 nm) confirm the complexation reaction between LDH and TCH. As shown in Figure 1C, the unique “memory effect” allows LDO to recover the layered structure during the adsorption of antibiotics. The fact that the distinctive peak of Zn/Al spinel is still present at 36.70° shows that LDO has not completely reverted. At the same time, new peaks also appear at 37.39° (d = 2.3989 nm) and 44.15° (d = 2.0482 nm), which indicate that antibiotics were absorbed by LDO due to “memory effect” and coordination reaction[39].
Acid-base buffer capacity
An automatic potentiometric titration instrument is used to perform the acid-base titration experiments on the adsorbents before and after adsorbing antibiotics, and the total acid concentration (Ht) is calculated. The Ht-pH diagrams are made by taking the Ht value as the X-axis and the pH measured at each drip point as the Y-axis to present the acid-base buffering performance of materials[18]. Ht (mo1/L) is calculated as Equation (8)
where Ca, Cb (mo1/L) separately are concentrations of HNO3 and NaOH; V0, Va, and Vb (mL) are the volume of solutions before titration, the volume of consumed acid, and the volume of consumed base.
Compared with the blank control group, the suspensions of adsorbents show a stronger buffering ability to acids and bases. However, LDO performs better at acid-base buffering than LDH [Figure 10A], particularly alkaline environment, which may be related to the existence of metal oxides in LDO. The greater acid-base buffering capacity indicates more active sites on the LDO surface than LDH[18,40].
Figure 10. Ht-pH function of (A) LDH, LDO, CK; (B) CK, before and after LDH adsorbing antibiotics; (C) CK, before and after LDO adsorbing antibiotics. CK: Blank control group; LDH: layered double hydroxide; LDO: layered double hydroxide; OFX: ofloxacin; TCH: tetracycline hydrochloride.
After absorbing antibiotics, the buffering abilities of LDH and LDO are significantly weakened
CONCLUSIONS
LDH was prepared by the urea method, and LDO was obtained by calcining LDH at 450 °C. According to the adsorption experiments of TCH and OFX, the maximum adsorption capacities of LDH and LDO for TCH are 116.28 mg/g and 322.58 mg/g at pH 8.5, and for OFX were 25.06 mg/g and 43.37 mg/g at pH 7, respectively. XRD, TEM, SEM, FI-TR, BET, and especially acid-base titration experiments indicate that the adsorption performance of LOD on the two antibiotics is better than that of LDH, which is due to more active sites on the surface, “memory effect” and bigger specific surface area. Due to the more stable quinolone ring structure of OFX, the adsorption capacity of materials to OFX is weaker than TCH. Furthermore, after five cycles of adsorption and desorption, the adsorption rate of LDO to TCH remains at 94.9%. Thus, LDO can be employed as a special adsorbent for TCH.
DECLARATIONS
Authors’ contributionsWriting, formal analysis, editing: Zhang C
Review: Li Y
Validation: García-Meza JV
Availability of data and materialsNot applicable.
Ethical approval and consent to participateNot applicable.
Consent for publicationNot applicable.
Financial support and sponsorshipThis work was financially supported by Innovation Ability Improvement Project of Science and Technology smes in Shandong Province, China (Grant No.2022TSGC2501). Also, Cui Zhang would like to thank CONACyT for granting her scholarship (No. 813509) during her Ph.D. study.
Conflicts of interestAll authors declared that there are no conflicts of interest.
Copyright© The Author(s) 2023.
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Zhang C, García-Meza JV, Li Y. Differential removal of tetracycline hydrochloride and quinolone antibiotics by calcined and uncalcined layered double hydroxides. Miner Miner Mater 2023;2:3. http://dx.doi.org/10.20517/mmm.2022.10
AMA Style
Zhang C, García-Meza JV, Li Y. Differential removal of tetracycline hydrochloride and quinolone antibiotics by calcined and uncalcined layered double hydroxides. Minerals and Mineral Materials. 2023; 2(1): 3. http://dx.doi.org/10.20517/mmm.2022.10
Chicago/Turabian Style
Zhang, Cui, J. Viridiana García-Meza, Yinta Li. 2023. "Differential removal of tetracycline hydrochloride and quinolone antibiotics by calcined and uncalcined layered double hydroxides" Minerals and Mineral Materials. 2, no.1: 3. http://dx.doi.org/10.20517/mmm.2022.10
ACS Style
Zhang, C.; García-Meza JV.; Li Y. Differential removal of tetracycline hydrochloride and quinolone antibiotics by calcined and uncalcined layered double hydroxides. Miner. Miner. Mater. 2023, 2, 3. http://dx.doi.org/10.20517/mmm.2022.10
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