Next Article in Journal
A Quick Method for Predicting Reflectance Spectra of Nanophotonic Devices via Artificial Neural Network
Next Article in Special Issue
Alginate Microbeads Containing Halloysite and Layered Double Hydroxide as Efficient Carriers of Natural Antimicrobials
Previous Article in Journal
Improved Breakdown Strength and Restrained Leakage Current of Sandwich Structure Ferroelectric Polymers Utilizing Ultra-Thin Al2O3 Nanosheets
Previous Article in Special Issue
Advances in Nanomaterials Based on Cashew Nut Shell Liquid
 
 
Search for Articles:
Title / Keyword
Author / Affiliation / Email
Journal
Article Type
 
 
Advanced Search
 
Section
Special Issue
Volume
Issue
Number
Page
 
Journals
Nanomaterials
Volume 13
Issue 21
10.3390/nano13212838
nanomaterials-logo
Submit to this Journal Review for this Journal Propose a Special Issue
► Article Menu

Article Menu

share Share announcement Help format_quote Cite question_answer Discuss in SciProfiles
first_page
settings
Order Article Reprints
Font Type:
Arial Georgia Verdana
Font Size:
Aa Aa Aa
Line Spacing:
Column Width:
Background:
Article

Efficient Fluoride Wastewater Treatment Using Eco-Friendly Synthesized AlOOH

by
Wan-Tae Kim
,
Joo-Won Lee
,
Hong-Eun An
,
So-Hye Cho
and
Sohee Jeong
*
Materials Architecturing Research Center, Korea Institute of Science and Technology, Seoul 02792, Republic of Korea
*
Author to whom correspondence should be addressed.
Nanomaterials 2023, 13(21), 2838; https://doi.org/10.3390/nano13212838
Submission received: 6 October 2023 / Revised: 22 October 2023 / Accepted: 24 October 2023 / Published: 26 October 2023
(This article belongs to the Special Issue Recent Advances in Green Nanomaterials: Design and Applications)
Browse Figures
Versions Notes

Abstract

:
Fluoride ion is essential for health in small amounts, but excessive intake can be toxic. Meeting safety regulations for managing fluoride ion emissions from industrial facilities with both cost-effective and eco-friendly approaches is challenging. This study presents a solution through a chemical-free process, producing a boehmite (AlOOH) adsorbent on aluminum sheets. Utilizing cost-effective Al foil and DI water, rather than typical precursors, yields a substantial cost advantage. The optimized AlOOH adsorbent demonstrated a high fluoride ion removal rate of 91.0% in simulated wastewater with fluoride ion concentrations below 20 ppm and displayed a similar performance in industrial wastewater. Furthermore, the AlOOH adsorbent exhibited excellent reusability through a simple regeneration process and maintained stable performance across a wide pH range of 4 to 11, demonstrating its capability to adsorb fluoride ions under diverse conditions. The efficiency of the AlOOH adsorbent was validated by a high fluoride ion removal efficiency of 90.9% in a semi-batch mode flow cell, highlighting its potential applicability in engineered water treatment systems. Overall, the AlOOH adsorbent developed in this study offers a cost-effective, eco-friendly, and sustainable solution for effectively removing fluoride ion from surface waters and industrial wastewaters.

Graphical Abstract

1. Introduction

Fluoride is a common element found in various minerals and widely used in various industries [1,2,3]. It has numerous benefits for human beings, such as reducing enamel erosion and preventing osteoporosis at low concentrations. However, prolonged exposure to high levels of fluoride ions can lead to dental and skeletal fluorosis and other related diseases [4,5,6]. To ensure safe exposure to fluoride ions, the World Health Organization (WHO) has recommended a limit of 1.5 ppm or less of fluoride ions in drinking water [4,7]. Additionally, some jurisdictions recommend a limit of 2.0 ppm or less of fluoride ions in wastewater [8]. Wastewater contaminated with fluoride ions is increasingly being discharged from various industrial processes such as semiconductor manufacturing and fertilizer industries [9,10]. In order to comply with safety regulations and restrict imprudent fluoride ion emissions from industrial facilities, fluoride ions have been captured and precipitated in the form of CaF2 using Ca(OH)2 as a coagulant aid. However, even after fluoride ion removal via precipitation, water can still contain fluoride ion levels of about 20 ppm that exceed the effluent quality standard [11], which requires additional post treatments.
To meet the requirements for drinking water and wastewater, various methods including chemical precipitation [12], ion exchange [13], electrochemical processes [14], and adsorption techniques [15,16,17] have been developed to remove excess fluoride ions [7]. Adsorption is one of the most attractive options due to its low cost and simplicity of operation. Various materials have been examined as adsorbents for fluoride ion removal, such as activated carbon, metal oxides, and Al-based materials. Although activated carbon and metal oxides are cost-effective options for large-scale treatment systems, their effectiveness in fluoride ion removal is limited [18]. In contrast, Al-based fluoride ion adsorbents have been extensively studied due to their strong affinity to fluoride ion and their cost-effectiveness in large-scale operations. This preference for Al-based fluoride ion adsorbents can be explained by Pearson’s Hard Soft Acids Bases (HSAB) theory, which states that the Al ion (a hard Lewis acid) has a strong affinity for fluoride ions, as the fluoride ion is the hardest Lewis base with the highest electronegativity and a small ionic radius [19,20,21].
Boehmite (AlOOH) is a prominent representative Al-based mineral that is not only cost-effective and abundantly available but also easy to synthesize. Notably, AlOOH has a relatively strong adsorption ability for fluoride ions compared to other Al-based materials, such as gibbsite (Al(OH)3) and activated Al2O3 [3,4,22]. The hydroxyl ions (OH−) on the surface play a crucial role in achieving high fluoride ion removal efficiency by facilitating the exchange of hydroxyl ions for fluoride ions. Consequently, boehmite and gibbsite, which have a relatively large amount of Al-OH bonds, exhibit a higher fluoride ion removal capacity compared to activated Al2O3. Despite the higher concentration of Al-OH bonds in Al(OH)3, AlOOH has a better fluoride ion removal performance due to its higher stability in response to pH changes in water [23,24]. Ensuring high performance across a wide range of pH levels is crucial, as these levels can vary depending on the environment of various wastewaters.
The type of sorbents plays a pivotal role in designing a fluoride ion removal process that is both cost-effective and high-performing. Sorbents can be categorized into powder or granular forms, with powder adsorbents being the most widely employed for fluoride ion removal from wastewater. However, this method presents economic drawbacks due to its limited recyclability and substantial space requirements. Additionally, after fluoride ion removal, the powder adsorbents must undergo filtration prior to discharge, resulting in the generation of significant amounts of sludge. The proper disposal of the sludge can be difficult and expensive [5,25]. Moreover, the improper collection of the sludge during water treatments can lead to the release of the powder adsorbents into the environment, posing a significant threat to human health [7,26,27]. To address these concerns associated with the release of adsorbent powders, researchers have explored the utilization of various substrates, such as polyacrylonitrile nanofibers [28], polyaniline nanofibers [29,30], and cellulose nanofibers [31], to create composite adsorbents—where powder adsorbents are fixed on a substrate. However, the fabrication of these composite adsorbents often involves metal precursors, organic solvents, and other chemicals, such as anionic metal salts, acetone, hydrochloric acid, and ammonia solution, which can have adverse environmental effects. Therefore, it is crucial to develop a cost-effective and recyclable adsorbent that can be produced through environmentally friendly processes.
Herein, an efficient adsorption of fluoride ions is presented using a 2D-shaped AlOOH-based adsorbent grown on aluminum (Al) foil. Our fabrication method is simple, cost-effective, and environmentally friendly, involving only the reaction solely between the Al foil and boiled DI water (Scheme 1). By controlling the immersion time of Al in boiling DI water, the fabrication process is optimized to achieve an adsorbent with a high fluoride ion removal rate. The fluoride ion adsorption properties of the optimized AlOOH are evaluated using the pseudo-first-order and Langmuir isotherm model. The effectiveness of the adsorbent in removing fluoride ions at low concentrations ranging from 5 to 20 ppm and a wide range of pH levels (4, 5, 7, 9, and 11) is demonstrated. To evaluate the reusability of the optimized AlOOH, cycling experiments are carried out that illustrate its sustained fluoride ion removal capacity through a regeneration process. Additionally, two distinct experiments are performed to emulate practical wastewater treatment systems. First, the fluoride ion removal rates of AlOOH are tested using actual industrial wastewater. Second, the fluoride ion removal performance is verified by operating a continuous flow cell in a semi-batch mode with the AlOOH fabricated Al mesh, achieving a high fluoride ion removal efficiency of 90.9%.

2. Materials and Methods

Commercial Al foil (household Al foil) is used in order to fabricate AlOOH, as it is immersed in boiling DI water for various durations ranging from 10 s to 4.0 h. The surface morphology, chemical compositions, and crystal structure were investigated via a field emission scanning electron microscope (FE-SEM, Inspect F, FEI Company Co., Ltd., Hillsboro, OR, USA), energy-dispersive spectroscopy (EDS), a transmission electron microscope (TEM, Titan, FEI Company Co., Ltd.), and Fourier transform infrared spectroscopy (FT-IR, Nicolet iS10, Thermo Fisher Scientific Co., Ltd., Boston, MA, USA). The cross-sectional view of AlOOH fabricated on Al foil was observed via FE-SEM and TEM after the preparation of the sample using ion milling and a focused ion beam (FIB). The chemical composition of AlOOH adsorbent was measured via X-ray photoelectron spectroscopy (XPS, Nexsa, Thermo Fisher Scientific Co., Ltd.) with Al Kα X-ray radiation as the X-ray source for excitation and FT-IR with diamond attenuated total reflection (ATR).
The concentration of fluoride ions in simulated wastewater was adjusted with hydrofluoric acid (HF, 40%, Alfa Aesar Co., Ltd., Boston, MA, USA). Fluoride ion removal rates of AlOOH were confirmed using sodium 2-(parasulfophenylazo)-1,8-dihydroxy-3,6-naphthalene disulfonate (SPADNS) and zirconium oxychloride, along with a colorimeter (HI-739, HANNA instruments Co., Ltd., Seoul, Republic of Korea). Its maximum fluoride ion adsorption capacity was evaluated using a pseudo-first order and Langmuir isotherm model.
The pH of each solution was adjusted with small drops of aqueous solutions containing nitric acid and sodium hydroxide. For the reusability test the fluoride ion adsorbed sample was repeatedly immersed in boiling DI water (5 times). Furthermore, the fluoride ion removal rates in diluted semiconductor wastewater were assessed, which was initially at a concentration of 5000 ppm and then diluted with DI water to a concentration of 20 ppm. For the evaluation, AlOOH was fabricated on the surface of a porous Al mesh (2.0 mm × 2.0 mm mesh, 0.24 mm diameter) and the fluoride ion removal rate of the AlOOH fabricated sample was then evaluated within the flow cell using 1.00 g of the sample in 25 mL of diluted semiconductor wastewater. The flow cell consists of a sample container (with an inner diameter of 4 cm), a peristaltic pump, simulated wastewater, and tubing. Two sample containers were connected to accommodate the loading of Al mesh samples.

3. Results and Discussions

3.1. Synthesis and Characterization of AlOOH Adsorbents on Al Substrate

The sheet-type AlOOH adsorbent was synthesized via eco-friendly and cost-effective methods using Al foil and DI water. The significant cost advantage of this method is emphasized by the fact that aluminum foil is up to 90 times less expensive than a typical aluminum precursor and it eliminates the need for any organic solvents (see Table S1). The foil was immersed in boiling DI water, resulting in the formation of AlOOH on the surface, which was used for the fluoride ion removal test without any rinsing and activation of adsorption sites. AlOOH is generated when Al on the surface of the foil reacts with water molecules during boiling, resulting in the deposition of AlOOH on the Al surface and the concurrent generation of hydrogen gases as a by-product (Scheme 1) [32,33,34]. The resulting samples were designated as AlOOH-10s, AlOOH-30s, AlOOH-1m, AlOOH-5m, AlOOH-0.5, AlOOH-1, AlOOH-2, and AlOOH-4 corresponding to the immersion time of 10 s, 30 s, 1 min, 5 min, 0.5 h, 1.0 h, 2.0 h, and 4.0 h, respectively. The color of the foil transitioned from shiny silver to matte silver mixed with white, indicating the growth of AlOOH on the Al foil (see Figure S1a,c,e,g) [35].
The FE-SEM images show the morphology of as-synthesized AlOOH on the Al surface. Two-dimensional (2D)-shaped Al-O compounds were grown more densely on the Al surface with the increase in immersion time from 10 s to 1 min, as shown in Figure S2a–c [35,36]. Moreover, the thickness of AlOOH increases with longer immersion times in boiling DI water, measured to be about 21 nm, 27 nm, 30 nm, and 59 nm for AlOOH-0.5, AlOOH-1, AlOOH-2, and AlOOH-4 (the AlOOH series), respectively (as shown in Figure S2d and Figure 1b–e). This increase was even more pronounced in AlOOH-4, leading to a substantially thicker AlOOH which entirely covered the surface (see Figure 1e). In order to accurately measure the height of the AlOOH film on the Al foil, a side view of samples prepared via ion milling was observed via FE-SEM. As a result, the height of the AlOOH film increased with longer immersion times, measured to be about 483 nm, 501 nm, 504 nm, and 602 nm (Figure S1b,d,f,h), respectively. Overall, AlOOH shows superior growth in a direction parallel to the lateral direction, resulting in a high aspect ratio of lateral size to thickness.
The elemental composition in both the top view and the cross-sectional view was determined via EDS analysis (Figure 1f and Figure S3, Tables S1 and S2). The O/Al ratios for the AlOOH series were determined to be 1.90, 1.89, 1.96, and 1.97, respectively. These values were calculated based on the analysis from a cross-sectional view, where solely AlOOH was detected, unlike the top view. These ratios are consistent with the theoretical O/Al ratio for AlOOH, confirming the formation of AlOOH on the surface (Table S2). The trend in O/Al ratios in the AlOOH series is also observed as show via the top view, where both AlOOH and Al foil are detected. The O/Al ratio exhibits a rapid increase within the first 5 min of the reaction, followed via a slower rate of increase with a gentler slope by top-view EDS analysis. This suggests that Al-O clusters rapidly form within a few minutes, leading to a sudden increase in oxygen concentration [37]. Subsequently, as these Al-O clusters transform into AlOOH, there seems to be a decrease in the increment of the O/Al ratio.
TEM analysis was performed to observe the more detailed morphology and crystal structure of AlOOH on the surface of Al. The observation revealed the presence of 2D-shaped AlOOH structures with a lateral size of less than 600 nm on the Al surface (Figure 2b,c). A schematic illustration of AlOOH on the Al surface is provided in Figure 2a, corroborating the finding via the cross-sectional view obtained from FE-SEM. In Figure 2d, the fast Fourier transform (FFT) pattern of AlOOH-2 showed the presence of (0 −2 1), (0 1 2), and (0 3 1) planes of AlOOH [38], indicating that AlOOH was successfully fabricated on the Al surface.
FT-IR data also provide evidence for the formation of AlOOH on the surface of Al (Figure 3). Compared to Al foil, the FT-IR spectra of the AlOOH series exhibited two distinct bands at 3301 and 3096 cm−1 which are attributed to O-H bonds from the physically adsorbed water [3] in hydrophilic AlOOH. In addition, the bands corresponding to Al-O-H and Al–O bonds of AlOOH are observed at 1063 cm−1 and 594 cm−1, respectively [37,39,40].

3.2. Fluoride Ion Removal Capacity of AlOOH Adsorbents on Al Substrate

With successfully fabricated AlOOH adsorbents, the fluoride ion adsorption capacity is initially evaluated using the simulated wastewater with 25 mL of 20 ppm HF solution. The choice of 20 ppm of fluoride ion as the initial concentration is made because conventional adsorbents often struggle to reduce fluoride ion levels below this point. For example, at concentrations lower than 20 ppm, the efficiency of the method utilizing Ca(OH)2 as a coagulant aid for adsorbing fluoride ions tends to decrease because of the dissolution of the adsorbed form of F ions (CaF2) back into the solution [11,41]. To find the most effective adsorbent among AlOOH-0.5, AlOOH-1, AlOOH-2, and AlOOH-4, the fluoride removal rate was measured using a colorimeter (Figure 4a). The rate of AlOOH-2 and AlOOH-4 reached steady states within 1.0 h, with removal rates of approximately 91.0% and 89.5%, respectively. The AlOOH-2 sample shows a decrease in fluoride concentration from 20 ppm to 1.8 ppm, showing compliance with the regulatory standards (2.0 ppm) [8]. Unlike AlOOH-2, for AlOOH-0.5 and AlOOH-1, the fluoride ion removal rate did not reach a steady state until 4.0 h, with fluoride ion removal rates of 73.0% and 77.5%, respectively. Among the samples, AlOOH-2 exhibited the highest adsorption performance. Therefore, AlOOH-2 was chosen as an efficient adsorbent for the fluoride ion adsorption tests at concentrations below 20 ppm (Figure 4b). To better discern efficiency differences under these low concentration conditions, the weight of the adsorbent was reduced in the test. After 4.0 h, the fluoride ion removal rates were 91.0%, 77.0%, 66.5%, and 59.5% at 5 ppm, 10 ppm, 15 ppm, and 20 ppm, respectively. These results indicate that AlOOH-2 is an effective adsorbent even at low fluoride ion concentrations (below 20 ppm).
To further understand the maximum capacity of AlOOH-2 for fluoride ion adsorption, kinetic studies are conducted as shown in Figure 5a and Table S3. For the fluoride ion removal adsorption tests, 0.25 g of the sample is soaked in 25 mL of HF solution. Measurement of the rate of fluoride ion adsorption was carried out using varying initial concentrations (ranging from 20 to 200 ppm) in a simulated wastewater environment. At an initial fluoride ion concentration of 20 ppm, the fluoride ion adsorption rate reached a plateau of 0.30 mg/g. For higher initial concentrations (40 ppm, 60 ppm, 80 ppm, and 100 ppm), the adsorption rates reached steady states after 2.0 h, measuring 0.56 mg/g, 0.74 mg/g, 0.97 mg/g, and 1.10 mg/g, respectively. In the case of 200 ppm of simulated wastewater, the adsorption rate took a longer time to reach a steady state, stabilizing after 4.0 h at 1.40 mg/g. Consequently, the total fluoride ion removal rates increased as the initial fluoride ion concentration decreased (Figure 5a and Figure S4), indicating once again that our absorbent is more effective at lower fluoride ion concentrations in wastewater. Figure 5b shows the Langmuir adsorption isotherm fitting of AlOOH on Al foil with different initial fluoride ion concentrations and adsorption times, illustrating the process of fluoride adsorption. Utilizing the pseudo-first order model and the Langmuir isotherm model, the maximum fluoride ion adsorption capacity (qmax) of AlOOH-2 is calculated to be 1.98 mg/g based on the total sample mass (Al and AlOOH), with additional details provided in text of the Supplementary Materials and Tables S3 and S4 [22,42]. It is important to note that AlOOH, which solely undertakes the role of an adsorbent, only exists on the surface of the Al foil which is an inactive or dead adsorbent. AlOOH comprises 6.15 vol% (the volumetric ratio, calculated from the height of the AlOOH film, as shown in Figure S1) and 7.58 wt% (calculated from the volumetric ratio and molar mass of Al and AlOOH, assuming that the AlOOH layer consists of dense layers) of the total sample (Al and AlOOH). The fluoride ion adsorption isotherms of AlOOH-2 are normalized using the weight percent of AlOOH in the total sample (Figure S5). Consequently, the maximum adsorption capacity of fluoride ions can be normalized to 26.12 mg/g based on the weight of AlOOH in the sample. This capacity is comparable to values reported in previous studies, even though AlOOH-2 shows lower total weight-based capacities compared to other Al-based materials (Figure S6).

3.3. Fluoride Adsorption Mechanism of AlOOH Adsorbents on an Al Substrate

To understand the mechanism of fluoride ion adsorption, the reaction process is investigated by analyzing the XPS and FT-IR spectra of the AlOOH-2 before and after fluoride ion adsorption. To maximize the fluoride ion adsorption, AlOOH-2 (mass = 1.00 g) was immersed in a 25 mL 200 ppm HF solution for 4.0 h. After fluoride ion adsorption, new peaks corresponding to adsorbed fluoride species were observed at 684.9 eV in the F 1s spectrum and 75.3 eV, in the Al 2p spectrum, confirming the presence of fluoride ions on the surface of AlOOH-2 (Figure 6a,b) [3,43,44]. Additionally, the content of Al-OH, located at 74.1 eV decreased from 68.36 to 56.87% after fluoride ion adsorption (Table 1). In the O 1s spectra, the peak at 532.0 eV, which corresponds to Al-OH, also showed a decreasing trend from 68.03 to 63.04% (Table 1) [3]. The decrease in Al-OH bonding in AlOOH-2 and the formation of Al-F bonding indicated that the hydroxyl ions on the surface serve as active sites for fluoride ion adsorption and facilitate the exchange between hydroxyl ions and fluoride ions (Equation (1) and Figure 7) [3,45,46]. Also, the involvement of hydroxyl ions in the fluoride ion adsorption process was confirmed via FT-IR analysis of the AlOOH-2 before and after fluoride ion removal (details are shown in the text of the Supplementary Materials and Figure S6).
F− + Al-OH → Al-F + OH−

3.4. pH Variance, Reusability, and Industrial Wastewater Evaluation

The pH of the solution is one of the crucial factors in determining the adsorption capacity of the adsorbent. In the semiconductor industry, wastewater can have an acidic pH of about 4 to 5 or an alkaline pH of 11, depending on the specific process involved [47,48]. Therefore, achieving a high fluoride ion removal performance across different pH levels is essential. AlOOH-2’s removal rate of fluoride ions was studied at various pH levels ranging from 4 to 11 (Figure 8). AlOOH-2 exhibited fluoride ion removal rates of 72.6%, 84.1%, 90.0%, 88.4%, and 80.1% at pH 4, pH 5, pH 7, pH 9, and pH 11, respectively. It was observed that the fluoride ion adsorption performance slightly decreased under basic conditions. This behavior aligns with previous studies, which reports that the surface of AlOOH becomes negatively charged at pH levels higher than the point of zero charge (8.5–9.5) of AlOOH determined via zeta potential measurement [3]. This change of charge results in the repulsion of fluoride ions and subsequently reduces adsorption efficiency. On the other hand, the decrease in fluoride ion adsorption performance under acidic conditions appears to be due to the dissolution of the Al-F complex into the solution [49]. Interestingly, AlOOH-2 exhibits relatively consistent performance over a broad pH range, showing a slight decrease of 1.6% from pH 7 to pH 9. This decline is smaller compared to the values (12.0%) reported in a previous study [43]. Also, to evaluate the stability of AlOOH-2 in different pH conditions, dissolved Al concentrations in the simulated wastewater were measured via inductively coupled plasma optical emission spectroscopy (ICP-OES) after the removal of fluoride ions. After this evaluation, it was observed that, in relation to the initial sample dosing amount, only a very small amount of Al was dissolved back into the solution (Table S7).
Furthermore, the reusability of AlOOH-2 for fluoride ion removal is tested. Initially, AlOOH-2 was tested for its fluoride ion removal rate by soaking it in 25 ml of 20 ppm HF solution for 1.0 h. After fluoride ion removal, the adsorbent was regenerated through immersion of the fluoride ion-adsorbed adsorbent in boiling DI water for 0.5 h. Then, the regenerated AlOOH-2 was tested for its fluoride ion removal rate under the same conditions as the initial test. This regeneration was repeated five times. The results showed that the adsorbent maintained over 80.0% of its removal rate up to the fourth cycle with regeneration, and exhibited around 77.5% of its fluoride ion removal rate in the fifth cycle (Figure 9). It is proposed that the regeneration mechanism involves the exchange of fluoride ions for hydroxyl ions once again during the re-immersion process. This is supported by the decrease in the Al-F peak observed in the XPS analysis following the regeneration process. Furthermore, the concentration ratio of Al-OH/Al-O in the Al 2p spectra exhibited an increase from 1.86 to 2.80. Similarly, in the O 1s spectra, the Al-OH/Al-O-Al ratio showed an increase from 1.70 to 3.59 (refer to Figure S7 and Table S8, in comparison to Figure 6 and Table 1).
The adsorbent developed in this study shows excellent performance in wastewater treatment systems. The fluoride removal rate of AlOOH-2 is specifically evaluated using actual wastewater discharged from the semiconductor manufacturing process (20 ppm). The adsorbent exhibited a rapid removal rate of 72.0% within 10 min, and the rates further increased to 89.5% within 4.0 h (Figure 10), which is a similar performance to that in simulated wastewater (Figure 4a).
Additionally, to examine the possibility of using the AlOOH adsorbent for an actual fluoride ion treatment system, the continuous flow cell operated in a semi-batch mode is adopted, simulating an industrial wastewater treatment module (Figure 11a). To enhance the water flow, Al mesh is utilized instead of Al foil. The AlOOH-fabricated mesh was produced using the same method as for the growth of AlOOH on Al foil (Figure 11b). The fluoride ion removal rate of the AlOOH-fabricated mesh was evaluated in a flow cell using 500 mL of a 20 ppm HF solution at a flow rate of 1 L/min, using 87.56 g of the sample over 5.0 h. Within the initial 10 min, 81.0% of fluoride ions were rapidly removed, and after 5.0 h, a removal rate of 90.9% was achieved (Figure 11c).

4. Conclusions

In this work, a cost-effective and eco-friendly synthetic method for producing an AlOOH-based sheet-type fluoride ion adsorbent is successfully demonstrated. The economic advantage is highlighted by the significant cost difference between the utilized aluminum foil and other common Al precursors. The synthesis process is optimized and a high fluoride ion removal rate is achieved by varying the immersion time in boiling water. As a result, AlOOH-2 is obtained, which exhibited an efficient fluoride ion removal rate of 91.0% for fluoride ion concentrations below 20 ppm. Additionally, the cycle performance of the adsorbent is assessed, and its excellent reusability is confirmed through a simple regeneration method involving a re-immersion process in boiling DI water. Importantly, our adsorbent exhibited an efficient fluoride ion removal capability in diverse conditions, including actual semiconductor wastewater and various pH levels. Furthermore, its practical applicability was demonstrated through the use of a continuous flow cell operating in a semi-batch mode. These results highlight the versatility and potential of our adsorbent for various industrial water treatment applications with highly scalable production in the near future.

Supplementary Materials

The following supporting information can be downloaded at: https://www.mdpi.com/article/10.3390/nano13212838/s1, Figure S1: photographs and cross-sectional view FE-SEM images of AlOOH on Al foil, which were fabricated by immersing Al foil in boiling DI water with different immersing times; Figure S2: FE-SEM images of AlOOH on Al foil, synthesized by immersing in boiling DI water for 10 s, 30 s, 1 min, and 5 min; Figure S3: atomic ratio of Al and O of AlOOH on Al foil with different immersing times in boiling DI water, from EDS analysis; Figure S4: fluoride ion removal rates of AlOOH-2 with different adsorption times and initial fluoride ion concentration; Figure S5: fluoride ions adsorbed by AlOOH-2 with different adsorption time and initial fluoride ion concentrations; Figure S6: FT-IR spectra of AlOOH-2; Figure S7: XPS survey spectra and XPS spectra of F 1s, Al 2p, and O 1s of regenerated AlOOH-2; Table S1: comparison of the costs of common Al salts and Al foil used as precursors for Al-based adsorbent synthesis; Table S2: atomic percent of Al and O of AlOOH on Al foil with different immersing times in boiling DI water via EDS analysis; Table S3: atomic percent of Al and O of AlOOH-0.5, AlOOH-1, AlOOH-2, and AlOOH-4 via spot EDS analysis from a cross-sectional view; Table S4: kinetic model parameters of AlOOH-2 for pseudo-first-order model obtained from sorption experiments with different initial fluoride ion concentrations; Table S5: calculated parameters for Langmuir isotherm models obtained from equilibrium sorption experiments; Table S6: adsorption capacities of various Al-based adsorbents for fluoride ions [3,22,45,46,50,51,52,53,54,55,56,57,58,59]; Table S7: concentrations of dissolved Al in the simulated wastewater with different pH conditions measured using inductively coupled plasma optical emission spectroscopy (ICP-OES) after removal of fluoride ions.; Table S8: Al 2p and O 1s peak parameters for the regenerated AlOOH-2.

Author Contributions

Conceptualization, S.J.; methodology, W.-T.K.; validation, W.-T.K., J.-W.L. and H.-E.A.; formal analysis, W.-T.K.; investigation, W.-T.K.; resources, S.-H.C. and S.J.; data curation, W.-T.K.; writing—original draft preparation, W.-T.K.; writing—review and editing, S.J.; visualization, W.-T.K. and J.-W.L.; supervision, S.J.; project administration, S.J.; funding acquisition, S.-H.C. and S.J. All authors have read and agreed to the published version of the manuscript.

Funding

This research was supported by the National R&D Program (2020M3H4A3106354) through the National Research Foundation of Korea (NRF) funded by the Ministry of Science and ICT and the Future Key Technology Program (Project No. 2E32511) funded by the Korea Institute of Science and Technology.

Data Availability Statement

Not applicable.

Acknowledgments

We acknowledge the sustainability team at the Korea Advanced Nano Fab Center for supplying the wastewater from their semiconductor fabrication laboratory.

Conflicts of Interest

The authors declare no conflict of interest.

References

  1. Wan, K.; Huang, L.; Yan, J.; Ma, B.; Huang, X.; Luo, Z.; Zhang, H.; Xiao, T. Removal of fluoride from industrial wastewater by using different adsorbents: A review. Sci. Total Environ. 2021, 773, 145535. [Google Scholar] [CrossRef] [PubMed]
  2. Choubisa, S.L.; Choubisa, D. Status of industrial fluoride pollution and its diverse adverse health effects in man and domestic animals in India. Environ. Sci. Pollut. Res. 2016, 23, 7244–7254. [Google Scholar] [CrossRef] [PubMed]
  3. Gai, W.Z.; Zhang, S.H.; Yang, Y.; Zhang, X.; Deng, Z.Y. Separation of Excess Fluoride from Water Using Amorphous and Crystalline AlOOH Adsorbents. ACS Omega 2021, 6, 16488–16497. [Google Scholar] [CrossRef] [PubMed]
  4. Sun, R.; Zhang, H.-B.; Qu, J.; Yao, H.; Yao, J.; Yu, Z.-Z. Supercritical carbon dioxide fluid assisted synthesis of hierarchical AlOOH@reduced graphene oxide hybrids for efficient removal of fluoride ions. Chem. Eng. J. 2016, 292, 174–182. [Google Scholar] [CrossRef]
  5. Meenakshi; Maheshwari, R.C. Fluoride in drinking water and its removal. J. Hazard. Mater. 2006, 137, 456–463. [Google Scholar] [CrossRef] [PubMed]
  6. Kumar, E.; Bhatnagar, A.; Hogland, W.; Marques, M.; Sillanpää, M. Interaction of anionic pollutants with Al-based adsorbents in aqueous media—A review. Chem. Eng. J. 2014, 241, 443–456. [Google Scholar] [CrossRef]
  7. WHO. Guidelines for Drinking-Water Quality; World Health Organization: Geneva, Switzerland, 2004; Volume 1. [Google Scholar]
  8. Saltworks Technologies Inc. Fluoride Removal from Industrial Wastewater Using Advanced Chemical Precipitation and Filtration; Saltworks Technologies Inc.: Richmond, BC, Canada, 2019. [Google Scholar]
  9. Bagastyo, A.Y.; Anggrainy, A.D.; Nindita, C.S.; Warmadewanthi. Electrodialytic removal of fluoride and calcium ions to recover phosphate from fertilizer industry wastewater. Sustain. Environ. Res. 2017, 27, 230–237. [Google Scholar] [CrossRef]
  10. Chen, J.; Yang, R.; Zhang, Z.; Wu, D. Removal of fluoride from water using aluminum hydroxide-loaded zeolite synthesized from coal fly ash. J. Hazard. Mater. 2022, 421, 126817. [Google Scholar] [CrossRef]
  11. Wambu, E.; Frau, F.; Machunda, R.; Pasape, L.; Barasa, S.; Ghiglieri, G. Water Defluoridation Methods Applied in Rural Areas over the World. 2022. Available online: https://dspace.nm-aist.ac.tz/handle/20.500.12479/1483 (accessed on 5 October 2023).
  12. Reardon, E.J.; Wang, Y. A Limestone Reactor for Fluoride Removal from Wastewaters. Environ. Sci. Technol. 2000, 34, 3247–3253. [Google Scholar] [CrossRef]
  13. Meenakshi, S.; Viswanathan, N. Identification of selective ion-exchange resin for fluoride sorption. J. Colloid Interface Sci. 2007, 308, 438–450. [Google Scholar] [CrossRef]
  14. Amor, Z.; Bariou, B.; Mameri, N.; Taky, M.; Nicolas, S.; Elmidaoui, A. Fluoride removal from brackish water by electrodialysis. Desalination 2001, 133, 215–223. [Google Scholar] [CrossRef]
  15. Li, W.; Cao, C.Y.; Wu, L.Y.; Ge, M.F.; Song, W.G. Superb fluoride and arsenic removal performance of highly ordered mesoporous aluminas. J. Hazard. Mater. 2011, 198, 143–150. [Google Scholar] [CrossRef] [PubMed]
  16. Gebremariam, A.M.; Asgedom, A.G.; Mekonnen, K.N.; Ashebir, M.E.; Gebremikael, Z.H.; Mesfin, K.A. Defluoridation of Water Using Aluminum Hydroxide Activated Carbon Biosorbents. Adv. Mater. Sci. Eng. 2022, 2022, 4038444. [Google Scholar] [CrossRef]
  17. Kuang, L.; Liu, Y.; Fu, D.; Zhao, Y. FeOOH-graphene oxide nanocomposites for fluoride removal from water: Acetate mediated nano FeOOH growth and adsorption mechanism. J. Colloid Interface Sci. 2017, 490, 259–269. [Google Scholar] [CrossRef] [PubMed]
  18. Chiavola, A.; D’Amato, E.; Di Marcantonio, C. Comparison of Adsorptive Removal of Fluoride from Water by Different Adsorbents under Laboratory and Real Conditions. Water 2022, 14, 1423. [Google Scholar] [CrossRef]
  19. Salifu, A. Fluoride Removal from Groundwater by Adsorption Technology; CRC Press: Boca Raton, FL, USA, 2017. [Google Scholar]
  20. Hu, H.; Yang, L.; Lin, Z.; Zhao, Y.; Jiang, X.; Hou, L. A low-cost and environment friendly chitosan/aluminum hydroxide bead adsorbent for fluoride removal from aqueous solutions. Iran. Polym. J. 2018, 27, 253–261. [Google Scholar] [CrossRef]
  21. Burton, D.J.; Briney, G.C. Disproportionation of 3, 3-difluorotetrachloropropene. Application of the hard and soft acids and bases principle to organic halogen compounds. J. Org. Chem. 1970, 35, 3036–3045. [Google Scholar] [CrossRef]
  22. Wang, S.-G.; Ma, Y.; Shi, Y.-J.; Gong, W.-X. Defluoridation performance and mechanism of nano-scale aluminum oxide hydroxide in aqueous solution. J. Chem. Technol. Biotechnol. 2009, 84, 1043–1050. [Google Scholar] [CrossRef]
  23. Gai, W.-Z.; Zhang, S.-H.; Yang, Y.; Sun, K.; Jia, H.; Deng, Z.-Y. Defluoridation performance comparison of aluminum hydroxides with different crystalline phases. Water Supply 2022, 22, 3673–3684. [Google Scholar] [CrossRef]
  24. Huang, L.; Yang, Z.; He, Y.; Chai, L.; Yang, W.; Deng, H.; Wang, H.; Chen, Y.; Crittenden, J. Adsorption mechanism for removing different species of fluoride by designing of core-shell boehmite. J. Hazard. Mater. 2020, 394, 122555. [Google Scholar] [CrossRef]
  25. Onyango, M.S.; Matsuda, H. Fluoride removal from water using adsorption technique. Adv. Fluor. Sci. 2006, 2, 1–48. [Google Scholar] [CrossRef]
  26. Krasovskiĭ, G.; Vasukovich, L.; Chariev, O. Experimental study of biological effects of leads and aluminum following oral administration. Environ. Health Persp. 1979, 30, 47–51. [Google Scholar] [CrossRef]
  27. Nieboer, E.; Gibson, B.L.; Oxman, A.D.; Kramer, J.R. Health effects of aluminum: A critical review with emphasis on aluminum in drinking water. Environ. Rev. 1995, 3, 29–81. [Google Scholar] [CrossRef]
  28. Wang, X.; Pan, S.; Zhang, M.; Qi, J.; Sun, X.; Gu, C.; Wang, L.; Li, J. Modified hydrous zirconium oxide/PAN nanofibers for efficient defluoridation from groundwater. Sci. Total Environ. 2019, 685, 401–409. [Google Scholar] [CrossRef] [PubMed]
  29. Parashar, K.; Ballav, N.; Debnath, S.; Pillay, K.; Maity, A. Hydrous ZrO2 decorated polyaniline nanofibres: Synthesis, characterization and application as an efficient adsorbent for water defluoridation. J. Colloid Interface Sci. 2017, 508, 342–358. [Google Scholar] [CrossRef] [PubMed]
  30. Chigondo, M.; Kamdem Paumo, H.; Bhaumik, M.; Pillay, K.; Maity, A. Hydrous CeO2-Fe3O4 decorated polyaniline fibers nanocomposite for effective defluoridation of drinking water. J. Colloid Interface Sci. 2018, 532, 500–516. [Google Scholar] [CrossRef] [PubMed]
  31. Sankararamakrishnan, N.; Srivastava, I.; Mishra, S. Studies on novel nano-bimetal doped cellulose nanofibers derived from agrowaste towards deflouridation. Int. J. Biol. Macromol. 2019, 128, 556–565. [Google Scholar] [CrossRef]
  32. Wang, X.Y.; Li, G.; Eckhoff, R.K. Kinetics study of hydration reaction between aluminum powder and water based on an improved multi-stage shrinking core model. Int. J. Hydrogen Energy 2021, 46, 33635–33655. [Google Scholar] [CrossRef]
  33. Kumar, D.; Muthukumar, K. An overview on activation of aluminium-water reaction for enhanced hydrogen production. J. Alloys Compd. 2020, 835, 155189. [Google Scholar] [CrossRef]
  34. Etminanbakhsh, M.; Allahkaram, S.R. Reaction of aluminum particles with superheated steam to generate hydrogen gas as a readily usable clean fuel. Fuel 2023, 332, 126011. [Google Scholar] [CrossRef]
  35. Wang, Z.; Du, H.; Gong, J.; Yang, S.; Ma, J.; Xu, J. Facile synthesis of hierarchical flower-like γ-AlOOH films via hydrothermal route on quartz surface. Colloids Surf. A 2014, 450, 76–82. [Google Scholar] [CrossRef]
  36. Han, D.; Lee, D. Morphology Controlled Synthesis of gamma-Al(2)O(3) Nano-Crystallites in Al@Al(2)O(3) Core-Shell Micro-Architectures by Interfacial Hydrothermal Reactions of Al Metal Substrates. Nanomaterials 2021, 11, 310. [Google Scholar] [CrossRef] [PubMed]
  37. Strålin, A.; Hjertberg, T. Influence of surface composition on initial hydration of aluminium in boiling water. Appl. Surf. Sci. 1994, 74, 263–275. [Google Scholar] [CrossRef]
  38. Christensen, A.N.; Lehmann, M.; Convert, P. Deuteration of crystalline hydroxides. Hydrogen bonds of g-AlOO (H, D) and g-FeOO (H, D). Acta Chem. Scand. 1982, 36, 303–308. [Google Scholar] [CrossRef]
  39. Scott, J.R.; Groenewold, G.S.; Gianotto, A.K.; Benson, M.T.; Wright, J.B. Experimental and Computational Study of Hydration Reactions of Aluminum Oxide Anion Clusters. J. Phys. Chem. A 2000, 104, 7079–7090. [Google Scholar] [CrossRef]
  40. Alwitt, R.S. The Growth of Hydrous Oxide Films on Aluminum. J. Electrochem. Soc. 1974, 121, 1322. [Google Scholar] [CrossRef]
  41. Clayton, G.D.; Clayton, F.E. Patty’s Industrial Hygiene and Toxicology. Vol. 2A. Toxicology; John Wiley & Sons, Inc.: Chichester, UK, 1981. [Google Scholar]
  42. Mohapatra, M.; Anand, S.; Mishra, B.K.; Giles, D.E.; Singh, P. Review of fluoride removal from drinking water. J. Environ. Manag. 2009, 91, 67–77. [Google Scholar] [CrossRef] [PubMed]
  43. Adeno, F.; Mulugeta, E.; Zewge, F.; Chebude, Y. Adsorptive removal of fluoride from water using nanoscale aluminium oxide hydroxide (AlOOH). Bull. Chem. Soc. Ethiop. 2014, 28, 215–227. [Google Scholar] [CrossRef]
  44. Tao, W.; Zhong, H.; Pan, X.; Wang, P.; Wang, H.; Huang, L. Removal of fluoride from wastewater solution using Ce-AlOOH with oxalic acid as modification. J. Hazard. Mater. 2020, 384, 121373. [Google Scholar] [CrossRef]
  45. Barathi, M.; Kumar, A.S.K.; Rajesh, N. Aluminium hydroxide impregnated macroreticular aromatic polymeric resin as a sustainable option for defluoridation. J. Environ. Chem. Eng. 2015, 3, 630–641. [Google Scholar] [CrossRef]
  46. Barathi, M.; Kumar, A.S.K.; Kodali, J.; Mittal, S.; Samhith, G.D.; Rajesh, N. Probing the Interaction between Fluoride and the Polysaccharides in Al (III)-and Zr (IV)-Modified Tea Waste by Using Diverse Analytical Characterization Techniques. ChemistrySelect 2017, 2, 10123–10135. [Google Scholar] [CrossRef]
  47. Pommerenk, P.; Schafran, G.C. Adsorption of inorganic and organic ligands onto hydrous aluminum oxide: Evaluation of surface charge and the impacts on particle and NOM removal during water treatment. Environ. Sci. Technol. 2005, 39, 6429–6434. [Google Scholar] [CrossRef] [PubMed]
  48. Omar, F.M.; Rahman, N.N.N.A.; Ahmad, A. COD reduction in semiconductor wastewater by natural and commercialized coagulants using response surface methodology. Water Air Soil Pollut. 2008, 195, 345–352. [Google Scholar] [CrossRef]
  49. He, Z.; Liu, R.; Xu, J.; Liu, H.; Qu, J. Defluoridation by Al-based coagulation and adsorption: Species transformation of aluminum and fluoride. Sep. Purif. Technol. 2015, 148, 68–75. [Google Scholar] [CrossRef]
  50. García-Sánchez, J.; Solache-Ríos, M.; Martínez-Gutiérrez, J.; Arteaga-Larios, N.; Ojeda-Escamilla, M.; Rodríguez-Torres, I. Modified natural magnetite with Al and La ions for the adsorption of fluoride ions from aqueous solutions. J. Fluor. Chem. 2016, 186, 115–124. [Google Scholar] [CrossRef]
  51. Cai, H.-m.; Chen, G.-j.; Peng, C.-y.; Zhang, Z.-z.; Dong, Y.-y.; Shang, G.-z.; Zhu, X.-h.; Gao, H.-j.; Wan, X.-c. Removal of fluoride from drinking water using tea waste loaded with Al/Fe oxides: A novel, safe and efficient biosorbent. Appl. Surf. Sci. 2015, 328, 34–44. [Google Scholar] [CrossRef]
  52. Jin, H.; Ji, Z.; Yuan, J.; Li, J.; Liu, M.; Xu, C.; Dong, J.; Hou, P.; Hou, S. Research on removal of fluoride in aqueous solution by alumina-modified expanded graphite composite. J. Alloys Compd. 2015, 620, 361–367. [Google Scholar] [CrossRef]
  53. Wan, Z.; Chen, W.; Liu, C.; Liu, Y.; Dong, C. Preparation and characterization of γ-AlOOH@ CS magnetic nanoparticle as a novel adsorbent for removing fluoride from drinking water. J. Colloid Interface Sci. 2015, 443, 115–124. [Google Scholar] [CrossRef]
  54. Zhao, X.; Zhang, L.; Xiong, P.; Ma, W.; Qian, N.; Lu, W. A novel method for synthesis of Co–Al layered double hydroxides and their conversions to mesoporous CoAl2O4 nanostructures for applications in adsorption removal of fluoride ions. Microporous Mesoporous Mater. 2015, 201, 91–98. [Google Scholar] [CrossRef]
  55. Tangsir, S.; Hafshejani, L.D.; Lähde, A.; Maljanen, M.; Hooshmand, A.; Naseri, A.A.; Moazed, H.; Jokiniemi, J.; Bhatnagar, A. Water defluoridation using Al2O3 nanoparticles synthesized by flame spray pyrolysis (FSP) method. Chem. Eng. J. 2016, 288, 198–206. [Google Scholar] [CrossRef]
  56. Dayananda, D.; Sarva, V.R.; Prasad, S.V.; Arunachalam, J.; Parameswaran, P.; Ghosh, N.N. Synthesis of MgO nanoparticle loaded mesoporous Al2O3 and its defluoridation study. Appl. Surf. Sci. 2015, 329, 1–10. [Google Scholar] [CrossRef]
  57. Jia, Y.; Zhu, B.-S.; Jin, Z.; Sun, B.; Luo, T.; Yu, X.-Y.; Kong, L.-T.; Liu, J.-H. Fluoride removal mechanism of bayerite/boehmite nanocomposites: Roles of the surface hydroxyl groups and the nitrate anions. J. Colloid Interface Sci. 2015, 440, 60–67. [Google Scholar] [CrossRef]
  58. Ku, Y.; Chiou, H.-M. The adsorption of fluoride ion from aqueous solution by activated alumina. Water Air Soil Pollut. 2002, 133, 349–361. [Google Scholar] [CrossRef]
  59. Maliyekkal, S.M.; Sharma, A.K.; Philip, L. Manganese-oxide-coated alumina: A promising sorbent for defluoridation of water. Water Res. 2006, 40, 3497–3506. [Google Scholar] [CrossRef]
Nanomaterials 13 02838 sch001
Scheme 1. A cost-effective, eco-friendly, and simple method for AlOOH fabrication on the surface of Al foil using boiling DI water. The 2D-shaped AlOOH nanostructures within the AlOOH film show a high ratio of lateral size (d) to thickness (T).
Scheme 1. A cost-effective, eco-friendly, and simple method for AlOOH fabrication on the surface of Al foil using boiling DI water. The 2D-shaped AlOOH nanostructures within the AlOOH film show a high ratio of lateral size (d) to thickness (T).
Nanomaterials 13 02838 sch001
Nanomaterials 13 02838 g001
Figure 1. FE-SEM images of Al foil (a) before and (b–e) after immersion in boiling DI water with different immersion times ((b): 0.5 h, (c): 1.0 h, (d): 2.0 h, and (e): 4.0 h, refer to AlOOH-0.5, AlOOH-1, AlOOH-2, and AlOOH-4, respectively; white scale bar is 500 nm), and (f) Al and O atomic ratio of (a–e), which was analyzed via EDS analysis.
Figure 1. FE-SEM images of Al foil (a) before and (b–e) after immersion in boiling DI water with different immersion times ((b): 0.5 h, (c): 1.0 h, (d): 2.0 h, and (e): 4.0 h, refer to AlOOH-0.5, AlOOH-1, AlOOH-2, and AlOOH-4, respectively; white scale bar is 500 nm), and (f) Al and O atomic ratio of (a–e), which was analyzed via EDS analysis.
Nanomaterials 13 02838 g001
Nanomaterials 13 02838 g002
Figure 2. (a) Illustration of AlOOH-2 on Al foil and TEM images of AlOOH-2: (b–d) cross-sectional TEM image of AlOOH on the Al surface (inset showing the FFT pattern of the white square box region).
Figure 2. (a) Illustration of AlOOH-2 on Al foil and TEM images of AlOOH-2: (b–d) cross-sectional TEM image of AlOOH on the Al surface (inset showing the FFT pattern of the white square box region).
Nanomaterials 13 02838 g002
Nanomaterials 13 02838 g003
Figure 3. FT-IR spectra of Al foil, AlOOH-0.5, AlOOH-1, AlOOH-2, and AlOOH-4.
Figure 3. FT-IR spectra of Al foil, AlOOH-0.5, AlOOH-1, AlOOH-2, and AlOOH-4.
Nanomaterials 13 02838 g003
Nanomaterials 13 02838 g004
Figure 4. Fluoride ion removal rate with (a) different immersion times in boiling water (Al foil, AlOOH-0.5, AlOOH-1, AlOOH-2, and AlOOH-4, initial fluoride ion concentration: 20 ppm, sample loading: 1.00 g, and adsorption time: 4.0 h) and (b) different initial fluoride ion concentrations ranging from 5 to 20 ppm of AlOOH-2 (sample loading: 0.25 g, and adsorption time: 4.0 h).
Figure 4. Fluoride ion removal rate with (a) different immersion times in boiling water (Al foil, AlOOH-0.5, AlOOH-1, AlOOH-2, and AlOOH-4, initial fluoride ion concentration: 20 ppm, sample loading: 1.00 g, and adsorption time: 4.0 h) and (b) different initial fluoride ion concentrations ranging from 5 to 20 ppm of AlOOH-2 (sample loading: 0.25 g, and adsorption time: 4.0 h).
Nanomaterials 13 02838 g004
Nanomaterials 13 02838 g005
Figure 5. (a) Fluoride ion adsorption kinetics of AlOOH-2 with different initial fluoride ion concentrations (dashed line shows the result of fitting a pseudo-first-order model with each initial concentration of fluoride ions) and (b) isotherm of fluoride ion adsorption of (a) with linear form Langmuir isotherm model. (Initial fluoride ion concentration: 20 to 200 ppm, sample loading: 0.25 g, and adsorption time: 4.0 h.).
Figure 5. (a) Fluoride ion adsorption kinetics of AlOOH-2 with different initial fluoride ion concentrations (dashed line shows the result of fitting a pseudo-first-order model with each initial concentration of fluoride ions) and (b) isotherm of fluoride ion adsorption of (a) with linear form Langmuir isotherm model. (Initial fluoride ion concentration: 20 to 200 ppm, sample loading: 0.25 g, and adsorption time: 4.0 h.).
Nanomaterials 13 02838 g005
Nanomaterials 13 02838 g006
Figure 6. (a) XPS survey spectra and XPS spectra of (b) F 1s, (c) Al 2p and (d) O 1s of AlOOH-2, before and after fluoride ion removal (green: background, black: experimental data).
Figure 6. (a) XPS survey spectra and XPS spectra of (b) F 1s, (c) Al 2p and (d) O 1s of AlOOH-2, before and after fluoride ion removal (green: background, black: experimental data).
Nanomaterials 13 02838 g006
Nanomaterials 13 02838 g007
Figure 7. Schematic illustration of fluoride ion adsorption on AlOOH-2.
Figure 7. Schematic illustration of fluoride ion adsorption on AlOOH-2.
Nanomaterials 13 02838 g007
Nanomaterials 13 02838 g008
Figure 8. Fluoride ion removal rate of AlOOH-2 under pHs ranging from 4 to 11 (initial fluoride ion concentration: 20 ppm, sample loading: 1.00 g, and adsorption time: 4.0 h).
Figure 8. Fluoride ion removal rate of AlOOH-2 under pHs ranging from 4 to 11 (initial fluoride ion concentration: 20 ppm, sample loading: 1.00 g, and adsorption time: 4.0 h).
Nanomaterials 13 02838 g008
Nanomaterials 13 02838 g009
Figure 9. Reusability test for fluoride ion removal of AlOOH-2 through the regeneration process (initial fluoride ion concentration: 20 ppm, sample loading: 1.00 g, and adsorption time: 1.0 h).
Figure 9. Reusability test for fluoride ion removal of AlOOH-2 through the regeneration process (initial fluoride ion concentration: 20 ppm, sample loading: 1.00 g, and adsorption time: 1.0 h).
Nanomaterials 13 02838 g009
Nanomaterials 13 02838 g010
Figure 10. Fluoride ion removal rates of AlOOH-2 in industrial semiconductor wastewater (initial fluoride ion concentration: 20 ppm, sample loading: 1.00 g, and adsorption time: 4.0 h).
Figure 10. Fluoride ion removal rates of AlOOH-2 in industrial semiconductor wastewater (initial fluoride ion concentration: 20 ppm, sample loading: 1.00 g, and adsorption time: 4.0 h).
Nanomaterials 13 02838 g010
Nanomaterials 13 02838 g011
Figure 11. (a) Schematic diagram of the flow cell for fluoride ion removal test, (b) FE-SEM image of AlOOH on Al mesh, (c) fluoride ion removal rates of the AlOOH fabricated Al mesh in HF solution with the flow cell.
Figure 11. (a) Schematic diagram of the flow cell for fluoride ion removal test, (b) FE-SEM image of AlOOH on Al mesh, (c) fluoride ion removal rates of the AlOOH fabricated Al mesh in HF solution with the flow cell.
Nanomaterials 13 02838 g011
Table 1. Al 2p and O 1s peak parameters for the AlOOH-2 before and after fluoride ion removal.
Table 1. Al 2p and O 1s peak parameters for the AlOOH-2 before and after fluoride ion removal.
ElectronsPeakBinding Energy
(eV)		Before AdsorptionAfter Adsorption
Concentration
(Atomic %)
Al 2pAl-O73.531.6430.53
Al-OH74.168.3656.87
Al-F75.3-12.61
O 1sAl-O-Al530.631.9736.96
Al-OH532.068.0363.04
Disclaimer/Publisher’s Note: The statements, opinions and data contained in all publications are solely those of the individual author(s) and contributor(s) and not of MDPI and/or the editor(s). MDPI and/or the editor(s) disclaim responsibility for any injury to people or property resulting from any ideas, methods, instructions or products referred to in the content.

Share and Cite

MDPI and ACS Style

Kim, W.-T.; Lee, J.-W.; An, H.-E.; Cho, S.-H.; Jeong, S. Efficient Fluoride Wastewater Treatment Using Eco-Friendly Synthesized AlOOH. Nanomaterials 2023, 13, 2838. https://doi.org/10.3390/nano13212838

AMA Style

Kim W-T, Lee J-W, An H-E, Cho S-H, Jeong S. Efficient Fluoride Wastewater Treatment Using Eco-Friendly Synthesized AlOOH. Nanomaterials. 2023; 13(21):2838. https://doi.org/10.3390/nano13212838

Chicago/Turabian Style

Kim, Wan-Tae, Joo-Won Lee, Hong-Eun An, So-Hye Cho, and Sohee Jeong. 2023. "Efficient Fluoride Wastewater Treatment Using Eco-Friendly Synthesized AlOOH" Nanomaterials 13, no. 21: 2838. https://doi.org/10.3390/nano13212838

APA Style

Kim, W.-T., Lee, J.-W., An, H.-E., Cho, S.-H., & Jeong, S. (2023). Efficient Fluoride Wastewater Treatment Using Eco-Friendly Synthesized AlOOH. Nanomaterials, 13(21), 2838. https://doi.org/10.3390/nano13212838

Note that from the first issue of 2016, this journal uses article numbers instead of page numbers. See further details here.

Article Metrics

Back to TopTop