Ionic liquid-modified magnetic graphene oxide nanocomposite as a powerful adsorbent for the removal of lead ions and brilliant blue dye

Ionic liquid-modified magnetic graphene oxide nanocomposite as a powerful adsorbent for the removal of lead ions and brilliant blue dye | Research Square window.SnipcartSettings = { analytics: { enabled: false } }; (function() { var accessVector = localStorage.getItem('access_vector') || ''; window.dataLayer = window.dataLayer || []; if (accessVector) { window.dataLayer.push({ user: { profile: { profileInfo: { snid: accessVector } } } }); } })(); (function(w,d,s,l,i){w[l]=w[l]||[];w[l].push({'gtm.start':new Date().getTime(),event:'gtm.js'});var f=d.getElementsByTagName(s)[0],j=d.createElement(s),dl=l!='dataLayer'?'&l='+l:'';j.async=true;j.src='https://www.googletagmanager.com/gtm.js?id='+i+dl;f.parentNode.insertBefore(j,f);})(window,document,'script','dataLayer','GTM-K279D39R'); Browse Preprints In Review Journals COVID-19 Preprints AJE Video Bytes Research Tools Research Promotion AJE Professional Editing AJE Rubriq About Preprint Platform In Review Editorial Policies Our Team Advisory Board Help Center Sign In Submit a Preprint Cite Share Download PDF Article Ionic liquid-modified magnetic graphene oxide nanocomposite as a powerful adsorbent for the removal of lead ions and brilliant blue dye Farkhondeh Dadvar, Dawood Elhamifar This is a preprint; it has not been peer reviewed by a journal. https://doi.org/ 10.21203/rs.3.rs-4986593/v1 This work is licensed under a CC BY 4.0 License Status: Posted Version 1 posted You are reading this latest preprint version Abstract In this research, a magnetic graphene oxide modified with ionic liquid has been synthesized and used as a powerful nanocomposite for the removal of lead (Pb 2+ ) ions and brilliant blue (BB) dye from a water sample. This nanocomposite was characterized by using EDS, FTIR, SEM, and VSM techniques, which confirmed the successful formation of the desired nanocomposite and good immobilization of the ionic liquid. The ultraviolet-visible (UV-Vis) and atomic absorption (AA) spectroscopy techniques were employed to quantify the extent of removal of Pb 2+ ions and BB dye. The removal percentages of Pb 2+ ions and BB dye by the prepared nanocomposite were 94% and 96%, respectively, demonstrating its excellent performance. According to the Langmuir isotherm, the maximum adsorption capacities of the nanocomposite toward Pb 2+ ions and BB dye were achieved to be 83.34 and 84.76 mg g − 1 , respectively. Also, this nanocomposite was recoverable and reusable at least three times. Earth and environmental sciences/Environmental sciences Physical sciences/Chemistry Magnetic graphene oxide Ionic liquid Adsorbent Lead ions Brilliant blue dye Figures Figure 1 Figure 2 Figure 3 Figure 4 Figure 5 Figure 6 Figure 7 Figure 8 Figure 9 Figure 10 Figure 11 Figure 12 Figure 13 1. Introduction Water, the most abundant molecule on earth, plays an important role in supporting the survival of a wide range of living organisms. Its absence would jeopardize a multitude of essential functions that are vital for life. Water pollution, which stems from the discharge of chemical, mineral, biological, and research materials from industrial plants, factories, and hospitals, is a significant environmental challenge for chemists 1 – 8 . Contaminated water poses serious threats and inflicts detrimental effects on the health of humans, animals, ecosystems, and plants 9 – 11 . These types of water pollution contain pollutants such as heavy metals, dyes, and organic and inorganic substances soluble in water, as well as pathogens. Numerous sources contribute to heavy metal and dye pollution, including mining activities, smelting, battery production, leather tanning, oil refining, dye production, pesticide application, pigment manufacturing, and printing and photography industries. Pollutants containing toxic metals like Cd, Hg, Ag, and Pb, as well as anionic and cationic dyes, pose significant health risks, including brain damage, kidney diseases, cancer, and systemic disorders 2 , 12 – 16 . To remove pollutants such as metals and toxic dyes, a variety of methods are employed, including absorption, flocculation, ultrafiltration, biodegradation, reverse osmosis, sedimentation, ion exchange, electrodes, membrane separation, and photocatalysis. Among these, is a highly effective method for removing pollutants from water and air, offering numerous advantages of simplicity, cost-effectiveness, environmental compatibility, and lack of harmful byproducts. Pollutants are removed from air or water by adhering to the surface of a solid material through physical and chemical interactions 12 , 13 , 17 – 19 . Activated carbon, zeolites, alumina oxides, silica gels, and other materials are employed as adsorbents in the surface adsorption method 20 – 23 . A suitable adsorbent should possess characteristics of non-toxicity, biodegradability, economic viability, and high efficiency, making carbon compounds and allotropes excellent candidates for this purpose 24 – 27 . Among the most significant and versatile allotropes of carbon is graphene oxide (two-dimensional), where carbon atoms exhibit sp 2 (honeycomb) hybridization, and its surface is replete with hydroxy, carboxylic acid, and epoxy functional groups. The remarkable properties of graphene oxide include exceptional strength, superior electrical and thermal conductivity, remarkable heat capacity, an extensive surface-to-volume ratio, extraordinary catalytic potential, and exceptional flexibility. Graphene oxide finds application in diverse fields, including water treatment, pharmaceutical carriers, hydrogen storage, high-performance filters, coating medical devices, biosensors, reinforcing structures and composites, catalysts, and adsorbents 28 – 31 . Given the remarkable properties discussed above, graphene oxide emerges as a promising adsorbent for removing dyes, paints, and heavy metals, offering an environmentally friendly solution for pollutant treatment. However, one of the challenges associated with utilizing graphene oxide as an adsorbent is the difficulty in separating it from the operating environment. This issue can be effectively addressed by introducing magnetic to the adsorbent’s surface 32 – 35 . Iron oxide is one of the most important magnetic oxides that finds extensive use due to its abundance, exceptional surface-to-volume ratio, minimal toxicity, and convenient separation using external magnets 36 – 39 . Furthermore, to enhance the adsorption capacity of magnetic graphene oxide, their surface can be modified by novel green materials such as ionic liquids. Ionic liquids are environmentally friendly compounds composed of two anions and cations, where the cation is organic or inorganic. These Ionic compounds are well-suited for applications as solvents, adsorbing, and catalysts due to their inherent low vapor pressure and exceptional chemical and thermal stability 40 – 45 . In view of the above here, and novel ionic liquid converter magnetic graphene oxide nanocomposite (GO@Fe 3 O 4 @SiO 2 -NH 2 / IL) prepared, characterized, and applied as an efficiency and green nanocomposite for the adsorption and removal of Pb 2+ ion and also BB dye from wastewater. 2. Experimental 2.1. Production of GO@Fe 3 O 4 @SiO 2 -NH 2 The GO@Fe 3 O 4 @SiO 2 -NH 2 nanocomposite was prepared through the following steps. First, 0.6 g of GO was thoroughly dispersed in 25 mL of distilled water for approximately 20 min. Next, 0.3 g of Fe 3 O 4 @SiO 2 -NH 2 was added and the obtained combination was stirred vigorously at 70°C for 2.5 h. Ultimately, by using a magnet the product was separated, washed with EtOH and H 2 O, dried at 65°C for 7 h, and called GO@Fe 3 O 4 @SiO 2 -NH 2 46 . 2.2. Production of GO@Fe 3 O 4 @SiO 2 -NH 2 / IL To synthesize GO@Fe 3 O 4 @SiO 2 -NH 2 /IL, 0.5 g of GO@Fe 3 O 4 @SiO 2 -NH 2 was first dispersed in dry toluene (30 mL). Subsequently, 0.2 mmol of IL was added to the reaction vessel and this was refluxed for 24 h. By using a magnet, the product was separated, washed with EtOH, dried at 65°C for 7 h, and called GO@Fe 3 O 4 @SiO 2 -NH 2 /IL 47 . 2.3. Batch adsorption experiments The absorption test was carried out in glass vials containing synthesized adsorbents (0.005, 0.01, 0.015, and 0.02 g) and pollutant concentration (Pb 2+ ion and BB dye) in the range of 5 mg/L to 30 mg/L. The vials were continuously stirred using a stirrer for 15 to 45 minutes at different temperatures of 25°C, 45°C, and 70°C. HCl and NaOH were used to adjust the pH of the solution. Moreover, different amounts of adsorbent were added to 50 mL of BB dye and 30 mL of Pb(NO 3 ) 2 solution to achieve the desired concentrations. By dissolving 0.016 g Pb(NO 3 ) 2 in 100 mL of distilled water, the corresponding standard solution was obtained. Also, by dissolving 0.01 g BB in distilled water (100 mL), the standard solution of BB was prepared. After the desired time for pollutant absorption by the designed GO@Fe 3 O 4 @SiO 2 -NH 2 /IL nanocatalyst, this adsorbent was removed by using a magnet. The filtered solution was then analyzed using atomic absorption spectroscopy (AAS) and UV-Vis spectroscopy to determine the concentration of the remaining pollutants. The removal percentage of Pb 2+ ion and BB dye was calculated using the following formula: Pb 2+ or BB dye removal percentage = [(C 0 - C t )/C 0 ] × 100 where C 0 (mg L − 1 ) is the primary concentration of pollutants (Pb 2+ ions and BB dye) in an aqueous solution and C t (mg L − 1 ) is the residual concentration of them at time t . 3. Results and discussion 3.1. Preparation and characterization of the GO@Fe 3 O 4 @SiO 2 -NH 2 /IL adsorbent For the preparation of this nanocomposite, firstly, Fe 3 O 4 @SiO 2 -NH 2 was prepared according to our previous procedure 47 . Then, GO was composted with Fe 3 O 4 @SiO ₂ -NH 2 to give GO@Fe 3 O 4 @SiO 2 -NH 2 . Next, the latter magnetic material was chemically modified with ionic liquid (IL) to deliver the GO@Fe 3 O 4 @SiO 2 -NH 2 /IL nanocomposite (Fig. 1 ). This composite was characterized by using FT-IR, SEM, VSM, EDS mapping, and EDS elemental analyses. FT-IR of prepared composites are shown in Fig. 2 . For all materials, the sharp peaks in the region of 3400–3425 cm − 1 are due to O-H and N-H bonds ( Figure. 2b and 2c). The peak appearing at 2945 cm − 1 is for aliphatic C-H bonds ( Figures. 2b and 2c) 48 , 49 . The observed peaks at 1750, 1626, and 1540 cm − 1 are respectively related to the carboxyl (C = O) groups of GO, the C = N and C = C bonds of ionic liquid ( Figures. 2a-2c). The peak at 1100 cm − 1 corresponds to the epoxy C-O and alkoxy C-O bonds of GO ( Figures. 2a-2c) 50 . The peak at 550 cm − 1 is assigned to the Fe-O bond. Also, the signals at 870 and 1110 cm − 1 are due to the Si-O-Si bonds of the silica shell ( Figures. 2b and 2c) 51 , 52 . These results confirm the high stability and successful immobilization of silica and ionic liquid species onto the material surface. The SEM image of the GO@Fe 3 O 4 @SiO 2 -NH 2 /IL nanocomposite provides a clear view of the dispersed spherical iron oxide nanoparticles on the folded graphene oxide layer Fig. 3 . Vibrating sample magnetometer (VSM) analysis of the Fe 3 O 4 and GO@Fe 3 O 4 @SiO 2 -NH 2 /IL nanocomposites was also performed and the result is shown in Fig. 4 . According to this analysis, the magnetization of the Fe 3 O 4 and GO@Fe 3 O 4 @SiO 2 -NH 2 /IL nanocomposites were, respectively, found to be 63 and 21 emu/g which confirms the successful chemical stabilization of GO moieties on Fe 3 O 4 . The TGA curve of GO@Fe 3 O 4 @SiO 2 -NH 2 /IL cleared two weight losses. At temperatures in the range of 25 to 130°C, a weight loss of about 0.64% is assigned to the removal of water and organic solvents. The main weight loss at 210–580°C (about 31%) corresponds to the elimination of grafted IL moieties confirming the high stability and well immobilization of IL species on the material surface Fig. 5 . The PXRD of GO@Fe 3 O 4 @SiO 2 -NH 2 /IL showed a pattern with six reflection peaks at 2θ of 32, 38, 42, 58, 63 and 68 degrees, corresponding to the Miller indices values ( hkl ) of 440, 511, 422, 400, 311 and 220, respectively, proving that the crystalline structure of the magnetite NPs is maintained during the adsorbent preparation steps Fig. 6 53 . The EDS and EDS mapping analyses showed the presence and well distribution of C, N, Si, Fe, and O elements onto/into the nanocomposite framework and also confirmed the successful immobilization of the ionic liquids on the surface of the nanocomposite Figs. 7 and 8 . 3.2. Adsorption studies 3.2.1. Effect of pH In the adsorption of Pb 2+ and BB dye by GO@Fe 3 O 4 @SiO 2 -NH 2 /IL nanocomposite, the pH effect was investigated. For this content, the pH was changed from 4 to 10, while other effective parameters including temperature (25°C), sonication time (20 min), initial concentration (Pb 2+ and BB) (10 mgL − 1 ), and the adsorbent dose (0.01 g) were kept constant. According to the results of Fig. 9 a, pH = 7 was found to be the optimal pH for the removal of both Pb 2+ and BB. The decrease in removal percentage under acidic conditions can be attributed to the overabundance of H + ions, which can compete with BB dye and Pb 2+ ions 3 . In addition, under acidic conditions, the adsorbent surface receives a positive charge, causing a strong electrostatic repulsion between the adsorbent and Pb 2+ ions, thereby reducing the removal percentage. Furthermore, at alkaline pH (pH > 7), Pb 2+ ions precipitate, which reduces their removal. At alkaline pH (pH > 7), the adsorbent surface becomes negatively charged creating a strong electrostatic repulsion with the BB dye. 3.2.2. Temperature effect The temperature effect (25, 30, 45, and 70°C) on the adsorption of Pb 2+ ions and BB dye molecules was evaluated at the fixed values of other parameters (0.01 g of the adsorbent, initial concentration of Pb 2+ and BB (10 mg L − 1 ), pH 7 and sonication time of 20 minutes). This showed that with increasing the temperature, the adsorption of both BB and Pb 2+ is increased. As shown in Fig. 9 b, the highest adsorption of BB (97%) is achieved at 45°C., while in comparison, the highest adsorption of Pb 2+ (95%) is obtained at 70°C. 3.2.3. Contact time effect The contact time effect (15–45 minutes) on the removal of Pb 2+ ions and BB dye by GO@Fe 3 O 4 @SiO 2 -NH 2 /IL nanocomposite was investigated. The other parameters, including temperature (70°C for Pb 2+ ions, 45°C for BB dye, pH = 7, initial concentration of Pb 2+ (10 mg L − 1 ), initial concentration of BB dye (10 mg L − 1 ) and adsorbent amount (0.01 g) were kept constant. As can be seen from Fig. 9 c, with increasing the contact time, the removal percentage of both Pb 2+ ions and BB dye molecules is increased. This is because the increase in the contact time increases the interactions between pollutants and the adsorbent and, subsequently, enhances the removal percentage. The maximum removal of Pb 2+ ions and BB dye molecules was achieved in a contact time of 35 minutes. After 35 minutes, the removal efficiency was decreased, which may be attributed to the desorption of Pb 2+ ions and BB dye molecules under ultrasonic irradiation. 3.2.4. Adsorbent dose effect To evaluate the adsorbent amount effect on the removal of Pb 2+ ions and BB dye molecules by GO@Fe 3 O 4 @SiO 2 -NH 2 /IL nanocomposite, different doses of adsorbent (0.005, 0.01, 0.015, and 0.02 g) were evaluated under the optimum values of the other parameters. The values of other parameters were: contact time (35 minutes), temperature of 45°C for BB molecules and 70°C for Pb 2+ ions, initial concentration of 10 mg L − 1 for Pb 2+ and BB molecules, and pH = 7. According to the data presented in Fig. 9 d, by increasing the adsorbent amount from 0.005 g to 0.015 g, the removal percentage was increased. This is because increasing the adsorbent amount increases the interaction sites for adsorbing pollutants. As shown, the maximum adsorption of Pb 2+ ions and BB molecules is achieved using only 0.015 g of the nanocomposite. 3.2.5. Effect of the initial concentrations of Pb 2+ ions and BB dye molecules The effect of the initial concentrations of Pb 2+ ions and BB dye molecules (5–30 mg. L − 1 ) on the removal process by the GO@Fe 3 O 4 @SiO 2 -NH 2 /IL nanocomposite was also examined. The values of the other parameters were: adsorbent dose of (0.015 g), temperature (45°C for BB and 70°C for Pb 2+ ), sonication time (25–35 minutes), and pH = 7. According to the findings of Fig. 9 e, the removal percentage of BB dye and Pb 2+ ions was decreased by increasing their initial concentrations. At lower concentrations of Pb 2+ and BB, the GO@Fe 3 O 4 @SiO 2 -NH 2 /IL nanocomposite sites have more opportunities to interact with Pb 2+ ions and BB dye molecules. By increasing concentrations of Pb 2+ and BB, the adsorption sites of the nanocomposite are saturated, and then the removal percentage is decremented. Next, the EDS analysis was carried out to evaluate the efficiency of the GO@Fe 3 O 4 @SiO 2 -NH 2 /IL adsorbent for the removal of Pb ion and BB dye. After adsorption process, the new signals of Pb and S have been observed in the EDS spectra (Figs. 10 and 11 ), confirming the successful removal of both Pb ions and BB dye on the designed GO@Fe 3 O 4 @SiO 2 -NH 2 /IL adsorbent. 3.3. Adsorption isotherms To properly understand the adsorption mechanism, as well as the maximum adsorption of BB and Pb + 2 by GO@Fe 3 O4@SiO 2 -NH 2 /IL, different isotherm models, including Langmuir, Freundlich, and Temkin, were assessed 47 – 50 , 54 , 55 . The results are presented in Table 1 . Table 1 Adsorption isotherm models parameters for the adsorption of Pb + 2 and BB using GO@Fe 3 O 4 @SiO 2 -NH 2 /IL BB Pb Adsorbent dosage (g) 0.01 0.015 Isotherm Parameters Value of parameters Langmuir Q m (mg g _1 ) K a (L mg _1 ) R 2 84.76 68 0.952 83.34 98 0.939 Freundlich 1/n K F (L mg _1 ) R 2 0.245 2.25 0.940 0.340 4.23 0.937 Temkin B1 K T (L mg _1 ) R 2 16.91 5.84 0.950 12.83 8.73 0.909 The equations of the isotherms are as follows: Langmuir \(\frac{\varvec{C}}{\varvec{q}}\varvec{=}\frac{\varvec{1}}{{\varvec{K}{\varvec{q}_\varvec{m}}}}\varvec{+}\frac{\varvec{C}}{{{\varvec{q}_\varvec{m}}}}\) : In this relation, C (mg L − 1 ) represents the concentration of equilibrium of the species (the remaining concentration of the species in the solution that the adsorbent could not absorb), q (mg g − 1 ) is the amount of species absorbed on the surface of the adsorbent, K (L mg − 1 ) is Langmuir's equilibrium constant, and q m (mg. g − 1 ) is the maximum amount of species that can be absorbed by a certain amount of adsorbent 51 , 52 . Freundlich: \(\varvec{Ln}{\varvec{q}_\varvec{e}}\varvec{=Ln}{\varvec{K}_\varvec{f}}\varvec{+}\frac{\varvec{1}}{\varvec{n}}\varvec{Ln}{\varvec{C}_\varvec{e}}\) where q e (mg/g) is the amount of substance absorbed per adsorbent mass, and C e (mg/L) is the concentration of the equilibrium in the solution. Freundlich's constants, n and K f , are the adsorption intensity and relative adsorption capacity of the adsorbent, respectively. When K f increases, the adsorption capacity of the adsorbent increases to absorb the adsorbed substance 52 , 56 . Temkin: \({\varvec{q}_\varvec{e}}\varvec{=}{\varvec{B}_\varvec{1}}\varvec{Ln}{\varvec{K}_\varvec{t}}\varvec{+}{\varvec{B}_\varvec{1}}\varvec{Ln}{\varvec{C}_\varvec{e}}\) B 1 and K t are the parameters of the model, which are calculated by using the chart that B = RT/b and K t are the temperature constants of Temkin, which are proportional to the heat of surface adsorption and the bond constant associated with the maximum bond energy. The adsorption isotherm diagrams of BB and Pb + 2 (Langmuir, Freundlich, and Temkin), are shown in Table 1 . According to the results of Table 1 , the removal process was followed by the Langmuir and Freundlich models, which was due to their higher R 2 compared to the Temkin. The Langmuir model undertakes that the process of adsorption is monolayer and the surface of the adsorbent is homogenous. While the Freundlich model undertakes that this process is multilayer and the surface of the adsorbent is heterogeneous. The maximum adsorption according to the Langmuir model for BB dye molecules and Pb + 2 ions were 84.76 and 83.34 mg g − 1 , respectively. The n values of the Freundlich model were greater than 1, which represents a promising adsorption condition. The n values between 2–10 in the model of Freundlich show an easy adsorption. Moreover, the n = 1–2 and n < 1 illustrate moderate and difficult adsorption, respectively. 3.4. Possible mechanism of absorption The adsorption mechanism of Pb + 2 and BB by GO@Fe 3 O 4 @SiO 2 -NH 2 /IL nanocomposite was investigated. Since the GO@Fe 3 O 4 @SiO 2 -NH 2 /IL nanocomposite contains the ionic liquid ion pairs, therefore, the adsorption of both BB cationic dye and Pb 2+ ions may be performed via their electrostatic interaction with the ionic liquid moieties Fig. 12 . The recyclability and reusability of GO@Fe 3 O 4 @SiO 2 -NH 2 /IL nanocomposite were also studied in the adsorption of both Pb + 2 and BB under optimal conditions. For this purpose, after the completion of the adsorption process for each sample, the absorbent was magnetically separated and washed completely with water and ethanol. Then, it was reused under the same conditions as the first run. It was found that the designed adsorbent could be recovered and reapplied at least three times with no significant loss of efficiency Fig. 13 . These results confirm the high performance and excellent stability of the designed adsorbent in practical conditions. 4. Conclusion In this research, a novel magnetic nanocomposite (GO@Fe 3 O 4 @SiO 2 -NH 2 /IL) was developed to remove Pb 2+ ions and BB dye from aqueous solutions. This nanocomposite was characterized by using FT-IR, EDX, SEM, TG, and VSM analyses. The effects of initial concentration, pH value, initial concentration of pollutant (Pb 2+ ions or BB dye), time, and adsorbent amount on the adsorption of Pb 2+ ions and BB dye by GO@Fe 3 O 4 @SiO 2 -NH 2 /IL were studied to determine the optimal conditions. The findings revealed that the optimal conditions were achieved at pH 7, 0.01 g of adsorbent, 5 min of contact time, and initial pollutant concentrations of 5 mg L − 1 and temperatures of 45°C for BB dye and at 70°C for Pb 2+ ions. The ease of separation of the nanocomposite using an external magnet, rapid adsorption rate, ability to recycle up to four times with minimal waste, superior adsorption capacity for heavy metals and dye pollutants, and environmentally friendly nature of the adsorbent stand out as its unique and superior characteristics compared to other previously developed adsorbents. Declarations Competing interests The authors declare no competing interests. Author Contribution F. D.: Investigation, Writing—original draft, Formal analysis, Resources. D. E.: Conceptualization, Writing – review& editing, Visualization, Supervision. Acknowledgements The authors thank Yasouj University and Iran National Science Foundation (INSF) for supporting this work. Data Availability All the research date is include in the manuscript. References F.S. Abdulraheem, Z.S. Al-Khafaji, K.S. Hashim, M. Muradov, P. Kot, A.A. 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Surface tensions of imidazolium based ionic liquids: Anion, cation, temperature and water effect. J.A. Coutinho, J. Colloid Interface Sci 314 , 621-630 (2007). Othman, N. H., Alias, N. H., Shahruddin, M. Z., Bakar, N. F. A., Him, N. R. N., & Lau, W. J. Adsorption kinetics of methylene blue dyes onto magnetic graphene oxide. J. Environ. Chem. Eng 6, 2803-2811 (2018). Dadvar, F., & Elhamifar, D. Magnetic silica/graphene oxide nanocomposite supported ionic liquid–manganese complex as a powerful catalyst for the synthesis of tetrahydrobenzopyrans. Sci. Rep 13 , 19354 (2023). Singh, N., Riyajuddin, S., Ghosh, K., Mehta, S. K., & Dan, A. Chitosan-graphene oxide hydrogels with embedded magnetic iron oxide nanoparticles for dye removal. ACS Appl. Nano Mater 2 , 7379-7392 (2019). Arslan, M., & Günay, K. Application of 4-VP-g-PET fibers and its N-oxide derivative as an adsorbent for removal of cationic dye. Polym. Bull 76 , 953-965 (2019). Vahidhabanu, S., Adeogun, A. I., & Babu, B. R. Biopolymer-grafted, magnetically tuned halloysite nanotubes as efficient and recyclable spongelike adsorbents for anionic azo dye removal. ACS omega 4, 2425-2436 (2019). Mittal, H., Babu, R., Dabbawala, A. A., Stephen, S., & Alhassan, S. M. Zeolite-Y incorporated karaya gum hydrogel composites for highly effective removal of cationic dyes. Colloids Surf. A: Physicochem. Eng. Asp 586 , 124161 (2020). Umpleby, R. J., Baxter, S. C., Chen, Y., Shah, R. N., & Shimizu, K. D. Characterization of molecularly imprinted polymers with the Langmuir− Freundlich isotherm. Anal. Chem , 4584-4591 (2001). Jeppu, G. P., & Clement, T. P. A modified Langmuir-Freundlich isotherm model for simulating pH-dependent adsorption effects. J. Contam. Hydrol 129 , 46-53 (2012). Norouzi, M., & Elhamifar, D. Magnetic yolk-shell structured methylene and propylamine based mesoporous organosilica nanocomposite: A highly recoverable and durable nanocatalyst with improved efficiency. Colloids Surf. A: Physicochem. Eng. 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Cite Share Download PDF Status: Posted Version 1 posted You are reading this latest preprint version Research Square lets you share your work early, gain feedback from the community, and start making changes to your manuscript prior to peer review in a journal. As a division of Research Square Company, we’re committed to making research communication faster, fairer, and more useful. We do this by developing innovative software and high quality services for the global research community. Our growing team is made up of researchers and industry professionals working together to solve the most critical problems facing scientific publishing. Also discoverable on Platform About Our Team In Review Editorial Policies Advisory Board Help Center Resources Author Services Accessibility API Access RSS feed Manage Cookie Preferences © Research Square 2026 | ISSN 2693-5015 (online) Privacy Policy Terms of Service Do Not Sell My Personal Information {"props":{"pageProps":{"initialData":{"identity":"rs-4986593","acceptedTermsAndConditions":true,"allowDirectSubmit":true,"archivedVersions":[],"articleType":"Article","associatedPublications":[],"authors":[{"id":358920375,"identity":"1609d133-0a06-4f68-a578-ffbab53d7797","order_by":0,"name":"Farkhondeh Dadvar","email":"","orcid":"","institution":"Yasouj University","correspondingAuthor":false,"submittingAuthor":false,"prefix":"","firstName":"Farkhondeh","middleName":"","lastName":"Dadvar","suffix":""},{"id":358920376,"identity":"b77935de-c89c-4a40-9e9e-a74dd5f05c89","order_by":1,"name":"Dawood Elhamifar","email":"data:image/png;base64,iVBORw0KGgoAAAANSUhEUgAAAZAAAAAyAQMAAABI0h/eAAAABlBMVEX///8AAABVwtN+AAAACXBIWXMAAA7EAAAOxAGVKw4bAAAA40lEQVRIie3OsQrCMBCA4YuBuFzt2oLgK8TFSemrKEJdBcFFh0Khbrp28CGcnAMHOukLdFGETg6dxEmMuujS2k0w/5Jw5CMHYDL9YgoY6QOrAbDDa8SCIgJPggq4LEVAE+F8tVdNcUXD6bqO1V06sSJo2AGPsjziKtGleJMg4qCVaNKMFQvjPCIVSkKRoAe+eBC2AhbmLiaVnRHe9C92KkaaeF8QBLIiTRxfcE16hcQlIcmaP0jK3eXe6cdUQGrb8HjCS+Kh7bPsPG53FrPZKZcAf7tXEJzPSWHsWua1yWQy/U13y0lDyuSn3DgAAAAASUVORK5CYII=","orcid":"","institution":"Yasouj University","correspondingAuthor":true,"submittingAuthor":false,"prefix":"","firstName":"Dawood","middleName":"","lastName":"Elhamifar","suffix":""}],"badges":[],"createdAt":"2024-08-27 19:44:12","currentVersionCode":1,"declarations":"","doi":"10.21203/rs.3.rs-4986593/v1","doiUrl":"https://doi.org/10.21203/rs.3.rs-4986593/v1","draftVersion":[],"editorialEvents":[],"editorialNote":"","failedWorkflow":false,"files":[{"id":65439087,"identity":"09629caa-d198-48f8-9e1b-eda48700491b","added_by":"auto","created_at":"2024-09-27 12:28:03","extension":"png","order_by":1,"title":"Figure 1","display":"","copyAsset":false,"role":"figure","size":138720,"visible":true,"origin":"","legend":"\u003cp\u003eSynthesis of GO@Fe\u003csub\u003e3\u003c/sub\u003eO\u003csub\u003e4\u003c/sub\u003e@SiO\u003csub\u003e2\u003c/sub\u003e-NH\u003csub\u003e2\u003c/sub\u003e/IL\u003c/p\u003e","description":"","filename":"image1.png","url":"https://assets-eu.researchsquare.com/files/rs-4986593/v1/77319416197f69922d8ab84d.png"},{"id":65439081,"identity":"ede09e61-b82b-4861-8875-0ac7e3eab0d5","added_by":"auto","created_at":"2024-09-27 12:28:03","extension":"png","order_by":2,"title":"Figure 2","display":"","copyAsset":false,"role":"figure","size":132203,"visible":true,"origin":"","legend":"\u003cp\u003eFT-IR of (a) GO, (b) Fe\u003csub\u003e3\u003c/sub\u003eO\u003csub\u003e4\u003c/sub\u003e@SiO\u003csub\u003e2\u003c/sub\u003e-NH\u003csub\u003e2\u003c/sub\u003e, and (c) GO@Fe\u003csub\u003e3\u003c/sub\u003eO\u003csub\u003e4\u003c/sub\u003e@SiO\u003csub\u003e2\u003c/sub\u003e-NH\u003csub\u003e2\u003c/sub\u003e/IL\u003c/p\u003e","description":"","filename":"image2.png","url":"https://assets-eu.researchsquare.com/files/rs-4986593/v1/f9043a5afd30b5e3013026bb.png"},{"id":65439317,"identity":"d3f22093-e025-4d13-8046-ac20824394f7","added_by":"auto","created_at":"2024-09-27 12:36:03","extension":"png","order_by":3,"title":"Figure 3","display":"","copyAsset":false,"role":"figure","size":763148,"visible":true,"origin":"","legend":"\u003cp\u003eSEM of GO@Fe\u003csub\u003e3\u003c/sub\u003eO\u003csub\u003e4\u003c/sub\u003e@SiO\u003csub\u003e2\u003c/sub\u003e-NH\u003csub\u003e2\u003c/sub\u003e/IL\u003c/p\u003e","description":"","filename":"image3.png","url":"https://assets-eu.researchsquare.com/files/rs-4986593/v1/510b7bb59d76022d87967fe2.png"},{"id":65440135,"identity":"30f19baf-740d-48ab-940b-1f9d77501bd3","added_by":"auto","created_at":"2024-09-27 12:44:03","extension":"png","order_by":4,"title":"Figure 4","display":"","copyAsset":false,"role":"figure","size":19086,"visible":true,"origin":"","legend":"\u003cp\u003eVSM of (a) Fe\u003csub\u003e3\u003c/sub\u003eO\u003csub\u003e4\u003c/sub\u003e and, (b) GO@Fe\u003csub\u003e3\u003c/sub\u003eO\u003csub\u003e4\u003c/sub\u003e@SiO\u003csub\u003e2\u003c/sub\u003e-NH\u003csub\u003e2\u003c/sub\u003e/IL.\u003c/p\u003e","description":"","filename":"image4.png","url":"https://assets-eu.researchsquare.com/files/rs-4986593/v1/6f6b1acd808fb52ae4394772.png"},{"id":65439089,"identity":"ca353516-9679-415f-a154-a591c351c31b","added_by":"auto","created_at":"2024-09-27 12:28:03","extension":"png","order_by":5,"title":"Figure 5","display":"","copyAsset":false,"role":"figure","size":36901,"visible":true,"origin":"","legend":"\u003cp\u003eTGA of GO@Fe\u003csub\u003e3\u003c/sub\u003eO\u003csub\u003e4\u003c/sub\u003e@SiO\u003csub\u003e2\u003c/sub\u003e-NH\u003csub\u003e2\u003c/sub\u003e/IL\u003c/p\u003e","description":"","filename":"image5.png","url":"https://assets-eu.researchsquare.com/files/rs-4986593/v1/d35a23a18ace9d3e0be162f3.png"},{"id":65439083,"identity":"ec105fcd-b2cd-4391-b2a1-e51135b1a972","added_by":"auto","created_at":"2024-09-27 12:28:03","extension":"png","order_by":6,"title":"Figure 6","display":"","copyAsset":false,"role":"figure","size":161404,"visible":true,"origin":"","legend":"\u003cp\u003ePXRD of \u003cstrong\u003eGO@Fe\u003c/strong\u003e\u003csub\u003e\u003cstrong\u003e3\u003c/strong\u003e\u003c/sub\u003e\u003cstrong\u003eO\u003c/strong\u003e\u003csub\u003e\u003cstrong\u003e4\u003c/strong\u003e\u003c/sub\u003e\u003cstrong\u003e@SiO\u003c/strong\u003e\u003csub\u003e\u003cstrong\u003e2\u003c/strong\u003e\u003c/sub\u003e\u003cstrong\u003e-NH\u003c/strong\u003e\u003csub\u003e\u003cstrong\u003e2\u003c/strong\u003e\u003c/sub\u003e\u003cstrong\u003e/IL\u003c/strong\u003e\u003c/p\u003e","description":"","filename":"image6.png","url":"https://assets-eu.researchsquare.com/files/rs-4986593/v1/e97767e98672b26d34a298da.png"},{"id":65439085,"identity":"8f4b3f8f-bd67-4d39-9423-d6e12fe25342","added_by":"auto","created_at":"2024-09-27 12:28:03","extension":"png","order_by":7,"title":"Figure 7","display":"","copyAsset":false,"role":"figure","size":56231,"visible":true,"origin":"","legend":"\u003cp\u003eEDS of\u003cstrong\u003e GO@Fe\u003c/strong\u003e\u003csub\u003e\u003cstrong\u003e3\u003c/strong\u003e\u003c/sub\u003e\u003cstrong\u003eO\u003c/strong\u003e\u003csub\u003e\u003cstrong\u003e4\u003c/strong\u003e\u003c/sub\u003e\u003cstrong\u003e@SiO\u003c/strong\u003e\u003csub\u003e\u003cstrong\u003e2\u003c/strong\u003e\u003c/sub\u003e\u003cstrong\u003e-NH\u003c/strong\u003e\u003csub\u003e\u003cstrong\u003e2\u003c/strong\u003e\u003c/sub\u003e\u003cstrong\u003e/IL\u003c/strong\u003e\u003c/p\u003e","description":"","filename":"image7.png","url":"https://assets-eu.researchsquare.com/files/rs-4986593/v1/5e8b4e00a96c109e4342117f.png"},{"id":65439316,"identity":"2d5092dc-da8f-4e81-86e9-ad14992acb15","added_by":"auto","created_at":"2024-09-27 12:36:03","extension":"png","order_by":8,"title":"Figure 8","display":"","copyAsset":false,"role":"figure","size":438585,"visible":true,"origin":"","legend":"\u003cp\u003eEDS mapping of \u003cstrong\u003eGO@Fe\u003c/strong\u003e\u003csub\u003e\u003cstrong\u003e3\u003c/strong\u003e\u003c/sub\u003e\u003cstrong\u003eO\u003c/strong\u003e\u003csub\u003e\u003cstrong\u003e4\u003c/strong\u003e\u003c/sub\u003e\u003cstrong\u003e@SiO\u003c/strong\u003e\u003csub\u003e\u003cstrong\u003e2\u003c/strong\u003e\u003c/sub\u003e\u003cstrong\u003e-NH\u003c/strong\u003e\u003csub\u003e\u003cstrong\u003e2\u003c/strong\u003e\u003c/sub\u003e\u003cstrong\u003e/IL\u003c/strong\u003e\u003c/p\u003e","description":"","filename":"image8.png","url":"https://assets-eu.researchsquare.com/files/rs-4986593/v1/78d2a1677ed026b1e0927c1d.png"},{"id":65439091,"identity":"789042e9-3685-4c3d-a6a2-acf506789d6e","added_by":"auto","created_at":"2024-09-27 12:28:03","extension":"png","order_by":9,"title":"Figure 9","display":"","copyAsset":false,"role":"figure","size":135991,"visible":true,"origin":"","legend":"\u003cp\u003eInfluence of (a) pH, (b) temperature, (c) sonication time (d) GO@Fe\u003csub\u003e3\u003c/sub\u003eO\u003csub\u003e4\u003c/sub\u003e@SiO\u003csub\u003e2\u003c/sub\u003e-NH\u003csub\u003e2\u003c/sub\u003e/IL dose and (e) initial concentrations of Pb\u003csup\u003e+2\u003c/sup\u003e and BB\u003c/p\u003e","description":"","filename":"image9.png","url":"https://assets-eu.researchsquare.com/files/rs-4986593/v1/db7517c2f3f43ba43892e39f.png"},{"id":65439319,"identity":"5729bdf7-08d9-464a-ba38-a6dc5cdb739d","added_by":"auto","created_at":"2024-09-27 12:36:03","extension":"png","order_by":10,"title":"Figure 10","display":"","copyAsset":false,"role":"figure","size":11142,"visible":true,"origin":"","legend":"\u003cp\u003eEDS spectrum of GO@Fe\u003csub\u003e3\u003c/sub\u003eO\u003csub\u003e4\u003c/sub\u003e@SiO\u003csub\u003e2\u003c/sub\u003e-NH\u003csub\u003e2\u003c/sub\u003e/IL after absorption of Pb\u003csup\u003e+2\u003c/sup\u003e\u003c/p\u003e","description":"","filename":"image10.png","url":"https://assets-eu.researchsquare.com/files/rs-4986593/v1/1fed75e2c1c713716c3b4e5b.png"},{"id":65439093,"identity":"85aed538-cdb6-426d-a7db-499e40ec47bb","added_by":"auto","created_at":"2024-09-27 12:28:03","extension":"png","order_by":11,"title":"Figure 11","display":"","copyAsset":false,"role":"figure","size":80135,"visible":true,"origin":"","legend":"\u003cp\u003eEDS spectrum of GO@Fe\u003csub\u003e3\u003c/sub\u003eO\u003csub\u003e4\u003c/sub\u003e@SiO\u003csub\u003e2\u003c/sub\u003e-NH\u003csub\u003e2\u003c/sub\u003e/IL after absorption of BB\u003c/p\u003e","description":"","filename":"image11.png","url":"https://assets-eu.researchsquare.com/files/rs-4986593/v1/4999613f7de05ed365df4e1f.png"},{"id":65440498,"identity":"5caa188b-49c1-45c7-94f3-2e67d7a01438","added_by":"auto","created_at":"2024-09-27 12:52:03","extension":"png","order_by":12,"title":"Figure 12","display":"","copyAsset":false,"role":"figure","size":113148,"visible":true,"origin":"","legend":"\u003cp\u003eThe absorption mechanism of Pb\u003csup\u003e+2\u003c/sup\u003e and BB using GO@Fe\u003csub\u003e3\u003c/sub\u003eO\u003csub\u003e4\u003c/sub\u003e@SiO\u003csub\u003e2\u003c/sub\u003e-NH\u003csub\u003e2\u003c/sub\u003e/IL\u003c/p\u003e","description":"","filename":"image12.png","url":"https://assets-eu.researchsquare.com/files/rs-4986593/v1/618757b1069e8781eea28f44.png"},{"id":65439321,"identity":"a08d8625-906c-484a-861b-7308499253f5","added_by":"auto","created_at":"2024-09-27 12:36:03","extension":"png","order_by":13,"title":"Figure 13","display":"","copyAsset":false,"role":"figure","size":28086,"visible":true,"origin":"","legend":"\u003cp\u003eRecoverability and reusability of GO@Fe\u003csub\u003e3\u003c/sub\u003eO\u003csub\u003e4\u003c/sub\u003e@SiO\u003csub\u003e2\u003c/sub\u003e-NH\u003csub\u003e2\u003c/sub\u003e/IL in the adsorption of Pb ions and BB dye\u003c/p\u003e","description":"","filename":"image13.png","url":"https://assets-eu.researchsquare.com/files/rs-4986593/v1/eb383490104a6cc34f000bf0.png"},{"id":71100051,"identity":"972c2437-ca89-47c5-b52b-7d30d3377226","added_by":"auto","created_at":"2024-12-11 06:38:59","extension":"pdf","order_by":0,"title":"","display":"","copyAsset":false,"role":"manuscript-pdf","size":2667089,"visible":true,"origin":"","legend":"","description":"","filename":"manuscript.pdf","url":"https://assets-eu.researchsquare.com/files/rs-4986593/v1/61a61cf1-0509-474f-980d-a7c9e8952763.pdf"}],"financialInterests":"No competing interests reported.","formattedTitle":"Ionic liquid-modified magnetic graphene oxide nanocomposite as a powerful adsorbent for the removal of lead ions and brilliant blue dye","fulltext":[{"header":"1. Introduction","content":"\u003cp\u003eWater, the most abundant molecule on earth, plays an important role in supporting the survival of a wide range of living organisms. Its absence would jeopardize a multitude of essential functions that are vital for life. Water pollution, which stems from the discharge of chemical, mineral, biological, and research materials from industrial plants, factories, and hospitals, is a significant environmental challenge for chemists \u003csup\u003e\u003cspan additionalcitationids=\"CR2 CR3 CR4 CR5 CR6 CR7\" citationid=\"CR1\" class=\"CitationRef\"\u003e1\u003c/span\u003e\u0026ndash;\u003cspan citationid=\"CR8\" class=\"CitationRef\"\u003e8\u003c/span\u003e\u003c/sup\u003e. Contaminated water poses serious threats and inflicts detrimental effects on the health of humans, animals, ecosystems, and plants \u003csup\u003e\u003cspan additionalcitationids=\"CR10\" citationid=\"CR9\" class=\"CitationRef\"\u003e9\u003c/span\u003e\u0026ndash;\u003cspan citationid=\"CR11\" class=\"CitationRef\"\u003e11\u003c/span\u003e\u003c/sup\u003e. These types of water pollution contain pollutants such as heavy metals, dyes, and organic and inorganic substances soluble in water, as well as pathogens. Numerous sources contribute to heavy metal and dye pollution, including mining activities, smelting, battery production, leather tanning, oil refining, dye production, pesticide application, pigment manufacturing, and printing and photography industries. Pollutants containing toxic metals like Cd, Hg, Ag, and Pb, as well as anionic and cationic dyes, pose significant health risks, including brain damage, kidney diseases, cancer, and systemic disorders \u003csup\u003e\u003cspan citationid=\"CR2\" class=\"CitationRef\"\u003e2\u003c/span\u003e, \u003cspan additionalcitationids=\"CR13 CR14 CR15\" citationid=\"CR12\" class=\"CitationRef\"\u003e12\u003c/span\u003e\u0026ndash;\u003cspan citationid=\"CR16\" class=\"CitationRef\"\u003e16\u003c/span\u003e\u003c/sup\u003e. To remove pollutants such as metals and toxic dyes, a variety of methods are employed, including absorption, flocculation, ultrafiltration, biodegradation, reverse osmosis, sedimentation, ion exchange, electrodes, membrane separation, and photocatalysis. Among these, is a highly effective method for removing pollutants from water and air, offering numerous advantages of simplicity, cost-effectiveness, environmental compatibility, and lack of harmful byproducts. Pollutants are removed from air or water by adhering to the surface of a solid material through physical and chemical interactions \u003csup\u003e\u003cspan citationid=\"CR12\" class=\"CitationRef\"\u003e12\u003c/span\u003e, \u003cspan citationid=\"CR13\" class=\"CitationRef\"\u003e13\u003c/span\u003e, \u003cspan additionalcitationids=\"CR18\" citationid=\"CR17\" class=\"CitationRef\"\u003e17\u003c/span\u003e\u0026ndash;\u003cspan citationid=\"CR19\" class=\"CitationRef\"\u003e19\u003c/span\u003e\u003c/sup\u003e. Activated carbon, zeolites, alumina oxides, silica gels, and other materials are employed as adsorbents in the surface adsorption method \u003csup\u003e\u003cspan additionalcitationids=\"CR21 CR22\" citationid=\"CR20\" class=\"CitationRef\"\u003e20\u003c/span\u003e\u0026ndash;\u003cspan citationid=\"CR23\" class=\"CitationRef\"\u003e23\u003c/span\u003e\u003c/sup\u003e. A suitable adsorbent should possess characteristics of non-toxicity, biodegradability, economic viability, and high efficiency, making carbon compounds and allotropes excellent candidates for this purpose \u003csup\u003e\u003cspan additionalcitationids=\"CR25 CR26\" citationid=\"CR24\" class=\"CitationRef\"\u003e24\u003c/span\u003e\u0026ndash;\u003cspan citationid=\"CR27\" class=\"CitationRef\"\u003e27\u003c/span\u003e\u003c/sup\u003e. Among the most significant and versatile allotropes of carbon is graphene oxide (two-dimensional), where carbon atoms exhibit sp\u003csup\u003e\u003cspan citationid=\"CR2\" class=\"CitationRef\"\u003e2\u003c/span\u003e\u003c/sup\u003e (honeycomb) hybridization, and its surface is replete with hydroxy, carboxylic acid, and epoxy functional groups. The remarkable properties of graphene oxide include exceptional strength, superior electrical and thermal conductivity, remarkable heat capacity, an extensive surface-to-volume ratio, extraordinary catalytic potential, and exceptional flexibility. Graphene oxide finds application in diverse fields, including water treatment, pharmaceutical carriers, hydrogen storage, high-performance filters, coating medical devices, biosensors, reinforcing structures and composites, catalysts, and adsorbents \u003csup\u003e\u003cspan additionalcitationids=\"CR29 CR30\" citationid=\"CR28\" class=\"CitationRef\"\u003e28\u003c/span\u003e\u0026ndash;\u003cspan citationid=\"CR31\" class=\"CitationRef\"\u003e31\u003c/span\u003e\u003c/sup\u003e. Given the remarkable properties discussed above, graphene oxide emerges as a promising adsorbent for removing dyes, paints, and heavy metals, offering an environmentally friendly solution for pollutant treatment. However, one of the challenges associated with utilizing graphene oxide as an adsorbent is the difficulty in separating it from the operating environment. This issue can be effectively addressed by introducing magnetic to the adsorbent\u0026rsquo;s surface \u003csup\u003e\u003cspan additionalcitationids=\"CR33 CR34\" citationid=\"CR32\" class=\"CitationRef\"\u003e32\u003c/span\u003e\u0026ndash;\u003cspan citationid=\"CR35\" class=\"CitationRef\"\u003e35\u003c/span\u003e\u003c/sup\u003e. Iron oxide is one of the most important magnetic oxides that finds extensive use due to its abundance, exceptional surface-to-volume ratio, minimal toxicity, and convenient separation using external magnets \u003csup\u003e\u003cspan additionalcitationids=\"CR37 CR38\" citationid=\"CR36\" class=\"CitationRef\"\u003e36\u003c/span\u003e\u0026ndash;\u003cspan citationid=\"CR39\" class=\"CitationRef\"\u003e39\u003c/span\u003e\u003c/sup\u003e. Furthermore, to enhance the adsorption capacity of magnetic graphene oxide, their surface can be modified by novel green materials such as ionic liquids. Ionic liquids are environmentally friendly compounds composed of two anions and cations, where the cation is organic or inorganic. These Ionic compounds are well-suited for applications as solvents, adsorbing, and catalysts due to their inherent low vapor pressure and exceptional chemical and thermal stability \u003csup\u003e\u003cspan additionalcitationids=\"CR41 CR42 CR43 CR44\" citationid=\"CR40\" class=\"CitationRef\"\u003e40\u003c/span\u003e\u0026ndash;\u003cspan citationid=\"CR45\" class=\"CitationRef\"\u003e45\u003c/span\u003e\u003c/sup\u003e. In view of the above here, and novel ionic liquid converter magnetic graphene oxide nanocomposite (GO@Fe\u003csub\u003e3\u003c/sub\u003eO\u003csub\u003e4\u003c/sub\u003e@SiO\u003csub\u003e2\u003c/sub\u003e-NH\u003csub\u003e2\u003c/sub\u003e\u003cb\u003e/\u003c/b\u003eIL) prepared, characterized, and applied as an efficiency and green nanocomposite for the adsorption and removal of Pb\u003csup\u003e2+\u003c/sup\u003e ion and also BB dye from wastewater.\u003c/p\u003e"},{"header":"2. Experimental","content":"\u003cdiv id=\"Sec3\" class=\"Section2\"\u003e \u003ch2\u003e2.1. Production of GO@Fe\u003csub\u003e3\u003c/sub\u003eO\u003csub\u003e4\u003c/sub\u003e@SiO\u003csub\u003e2\u003c/sub\u003e-NH\u003csub\u003e2\u003c/sub\u003e\u003c/h2\u003e \u003cp\u003eThe GO@Fe\u003csub\u003e3\u003c/sub\u003eO\u003csub\u003e4\u003c/sub\u003e@SiO\u003csub\u003e2\u003c/sub\u003e-NH\u003csub\u003e2\u003c/sub\u003e nanocomposite was prepared through the following steps. First, 0.6 g of GO was thoroughly dispersed in 25 mL of distilled water for approximately 20 min. Next, 0.3 g of Fe\u003csub\u003e3\u003c/sub\u003eO\u003csub\u003e4\u003c/sub\u003e@SiO\u003csub\u003e2\u003c/sub\u003e-NH\u003csub\u003e2\u003c/sub\u003e was added and the obtained combination was stirred vigorously at 70\u0026deg;C for 2.5 h. Ultimately, by using a magnet the product was separated, washed with EtOH and H\u003csub\u003e2\u003c/sub\u003eO, dried at 65\u0026deg;C for 7 h, and called GO@Fe\u003csub\u003e3\u003c/sub\u003eO\u003csub\u003e4\u003c/sub\u003e@SiO\u003csub\u003e2\u003c/sub\u003e-NH\u003csub\u003e2\u003c/sub\u003e \u003csup\u003e46\u003c/sup\u003e.\u003c/p\u003e \u003c/div\u003e \u003cdiv id=\"Sec4\" class=\"Section2\"\u003e \u003ch2\u003e\u003cb\u003e2.2. Production of GO@Fe\u003c/b\u003e\u003csub\u003e\u003cb\u003e3\u003c/b\u003e\u003c/sub\u003e\u003cb\u003eO\u003c/b\u003e\u003csub\u003e\u003cb\u003e4\u003c/b\u003e\u003c/sub\u003e\u003cb\u003e@SiO\u003c/b\u003e\u003csub\u003e\u003cb\u003e2\u003c/b\u003e\u003c/sub\u003e\u003cb\u003e-NH\u003c/b\u003e\u003csub\u003e\u003cb\u003e2\u003c/b\u003e\u003c/sub\u003e/\u003cb\u003eIL\u003c/b\u003e\u003c/h2\u003e \u003cp\u003eTo synthesize GO@Fe\u003csub\u003e3\u003c/sub\u003eO\u003csub\u003e4\u003c/sub\u003e@SiO\u003csub\u003e2\u003c/sub\u003e-NH\u003csub\u003e2\u003c/sub\u003e/IL, 0.5 g of GO@Fe\u003csub\u003e3\u003c/sub\u003eO\u003csub\u003e4\u003c/sub\u003e@SiO\u003csub\u003e2\u003c/sub\u003e-NH\u003csub\u003e2\u003c/sub\u003e was first dispersed in dry toluene (30 mL). Subsequently, 0.2 mmol of IL was added to the reaction vessel and this was refluxed for 24 h. By using a magnet, the product was separated, washed with EtOH, dried at 65\u0026deg;C for 7 h, and called GO@Fe\u003csub\u003e3\u003c/sub\u003eO\u003csub\u003e4\u003c/sub\u003e@SiO\u003csub\u003e2\u003c/sub\u003e-NH\u003csub\u003e2\u003c/sub\u003e/IL\u003csup\u003e47\u003c/sup\u003e.\u003c/p\u003e \u003c/div\u003e \u003cdiv id=\"Sec5\" class=\"Section2\"\u003e \u003ch2\u003e2.3. Batch adsorption experiments\u003c/h2\u003e \u003cp\u003eThe absorption test was carried out in glass vials containing synthesized adsorbents (0.005, 0.01, 0.015, and 0.02 g) and pollutant concentration (Pb\u003csup\u003e2+\u003c/sup\u003e ion and BB dye) in the range of 5 mg/L to 30 mg/L. The vials were continuously stirred using a stirrer for 15 to 45 minutes at different temperatures of 25\u0026deg;C, 45\u0026deg;C, and 70\u0026deg;C. HCl and NaOH were used to adjust the pH of the solution. Moreover, different amounts of adsorbent were added to 50 mL of BB dye and 30 mL of Pb(NO\u003csub\u003e3\u003c/sub\u003e)\u003csub\u003e2\u003c/sub\u003e solution to achieve the desired concentrations. By dissolving 0.016 g Pb(NO\u003csub\u003e3\u003c/sub\u003e)\u003csub\u003e2\u003c/sub\u003e in 100 mL of distilled water, the corresponding standard solution was obtained. Also, by dissolving 0.01 g BB in distilled water (100 mL), the standard solution of BB was prepared.\u003c/p\u003e \u003cp\u003eAfter the desired time for pollutant absorption by the designed GO@Fe\u003csub\u003e3\u003c/sub\u003eO\u003csub\u003e4\u003c/sub\u003e@SiO\u003csub\u003e2\u003c/sub\u003e-NH\u003csub\u003e2\u003c/sub\u003e/IL nanocatalyst, this adsorbent was removed by using a magnet. The filtered solution was then analyzed using atomic absorption spectroscopy (AAS) and UV-Vis spectroscopy to determine the concentration of the remaining pollutants. The removal percentage of Pb\u003csup\u003e2+\u003c/sup\u003e ion and BB dye was calculated using the following formula:\u003c/p\u003e \u003cp\u003ePb\u003csup\u003e2+\u003c/sup\u003e or BB dye removal percentage = [(C\u003csub\u003e0\u003c/sub\u003e - C\u003csub\u003et\u003c/sub\u003e)/C\u003csub\u003e0\u003c/sub\u003e] \u0026times; 100\u003c/p\u003e \u003cp\u003ewhere C\u003csub\u003e0\u003c/sub\u003e (mg L\u003csup\u003e\u0026minus;\u0026thinsp;1\u003c/sup\u003e) is the primary concentration of pollutants (Pb\u003csup\u003e2+\u003c/sup\u003e ions and BB dye) in an aqueous solution and C\u003csub\u003et\u003c/sub\u003e (mg L\u003csup\u003e\u0026minus;\u0026thinsp;1\u003c/sup\u003e) is the residual concentration of them at time \u003cem\u003et\u003c/em\u003e.\u003c/p\u003e \u003c/div\u003e"},{"header":"3. Results and discussion","content":"\u003cdiv id=\"Sec7\" class=\"Section2\"\u003e\n\u003ch2\u003e3.1. Preparation and characterization of the GO@Fe\u003csub\u003e3\u003c/sub\u003eO\u003csub\u003e4\u003c/sub\u003e@SiO\u003csub\u003e2\u003c/sub\u003e-NH\u003csub\u003e2\u003c/sub\u003e/IL adsorbent\u003c/h2\u003e\n\u003cp\u003eFor the preparation of this nanocomposite, firstly, Fe\u003csub\u003e3\u003c/sub\u003eO\u003csub\u003e4\u003c/sub\u003e@SiO\u003csub\u003e2\u003c/sub\u003e-NH\u003csub\u003e2\u003c/sub\u003e was prepared according to our previous procedure \u003csup\u003e\u003cspan class=\"CitationRef\"\u003e47\u003c/span\u003e\u003c/sup\u003e. Then, GO was composted with Fe\u003csub\u003e3\u003c/sub\u003eO\u003csub\u003e4\u003c/sub\u003e@SiO\u003csub\u003e₂\u003c/sub\u003e-NH\u003csub\u003e2\u003c/sub\u003e to give GO@Fe\u003csub\u003e3\u003c/sub\u003eO\u003csub\u003e4\u003c/sub\u003e@SiO\u003csub\u003e2\u003c/sub\u003e-NH\u003csub\u003e2\u003c/sub\u003e. Next, the latter magnetic material was chemically modified with ionic liquid (IL) to deliver the GO@Fe\u003csub\u003e3\u003c/sub\u003eO\u003csub\u003e4\u003c/sub\u003e@SiO\u003csub\u003e2\u003c/sub\u003e-NH\u003csub\u003e2\u003c/sub\u003e/IL nanocomposite (Fig.\u0026nbsp;\u003cspan class=\"InternalRef\"\u003e1\u003c/span\u003e).\u003c/p\u003e\n\u003cp\u003eThis composite was characterized by using FT-IR, SEM, VSM, EDS mapping, and EDS elemental analyses. FT-IR of prepared composites are shown in Fig.\u0026nbsp;\u003cspan class=\"InternalRef\"\u003e2\u003c/span\u003e. For all materials, the sharp peaks in the region of 3400\u0026ndash;3425 cm\u003csup\u003e\u0026minus;\u0026thinsp;1\u003c/sup\u003e are due to O-H and N-H bonds \u003cstrong\u003e(\u003c/strong\u003eFigure. 2b and 2c). The peak appearing at 2945 cm\u003csup\u003e\u0026minus;\u0026thinsp;1\u003c/sup\u003e is for aliphatic C-H bonds \u003cstrong\u003e(\u003c/strong\u003eFigures. 2b and 2c) \u003csup\u003e\u003cspan class=\"CitationRef\"\u003e48\u003c/span\u003e, \u003cspan class=\"CitationRef\"\u003e49\u003c/span\u003e\u003c/sup\u003e. The observed peaks at 1750, 1626, and 1540 cm\u003csup\u003e\u0026minus;\u0026thinsp;1\u003c/sup\u003e are respectively related to the carboxyl (C\u0026thinsp;=\u0026thinsp;O) groups of GO, the C\u0026thinsp;=\u0026thinsp;N and C\u0026thinsp;=\u0026thinsp;C bonds of ionic liquid \u003cstrong\u003e(\u003c/strong\u003eFigures. 2a-2c). The peak at 1100 cm\u003csup\u003e\u0026minus;\u0026thinsp;1\u003c/sup\u003e corresponds to the epoxy C-O and alkoxy C-O bonds of GO \u003cstrong\u003e(\u003c/strong\u003eFigures. 2a-2c) \u003csup\u003e\u003cspan class=\"CitationRef\"\u003e50\u003c/span\u003e\u003c/sup\u003e. The peak at 550 cm\u003csup\u003e\u0026minus;\u0026thinsp;1\u003c/sup\u003e is assigned to the Fe-O bond. Also, the signals at 870 and 1110 cm\u003csup\u003e\u0026minus;\u0026thinsp;1\u003c/sup\u003e are due to the Si-O-Si bonds of the silica shell \u003cstrong\u003e(\u003c/strong\u003eFigures. 2b and 2c) \u003csup\u003e\u003cspan class=\"CitationRef\"\u003e51\u003c/span\u003e, \u003cspan class=\"CitationRef\"\u003e52\u003c/span\u003e\u003c/sup\u003e. These results confirm the high stability and successful immobilization of silica and ionic liquid species onto the material surface.\u003c/p\u003e\n\u003cp\u003eThe SEM image of the GO@Fe\u003csub\u003e3\u003c/sub\u003eO\u003csub\u003e4\u003c/sub\u003e@SiO\u003csub\u003e2\u003c/sub\u003e-NH\u003csub\u003e2\u003c/sub\u003e/IL nanocomposite provides a clear view of the dispersed spherical iron oxide nanoparticles on the folded graphene oxide layer Fig.\u0026nbsp;\u003cspan class=\"InternalRef\"\u003e3\u003c/span\u003e.\u003c/p\u003e\n\u003cp\u003eVibrating sample magnetometer (VSM) analysis of the Fe\u003csub\u003e3\u003c/sub\u003eO\u003csub\u003e4\u003c/sub\u003e and GO@Fe\u003csub\u003e3\u003c/sub\u003eO\u003csub\u003e4\u003c/sub\u003e@SiO\u003csub\u003e2\u003c/sub\u003e-NH\u003csub\u003e2\u003c/sub\u003e/IL nanocomposites was also performed and the result is shown in Fig.\u0026nbsp;\u003cspan class=\"InternalRef\"\u003e4\u003c/span\u003e. According to this analysis, the magnetization of the Fe\u003csub\u003e3\u003c/sub\u003eO\u003csub\u003e4\u003c/sub\u003e and GO@Fe\u003csub\u003e3\u003c/sub\u003eO\u003csub\u003e4\u003c/sub\u003e@SiO\u003csub\u003e2\u003c/sub\u003e-NH\u003csub\u003e2\u003c/sub\u003e/IL nanocomposites were, respectively, found to be 63 and 21 emu/g which confirms the successful chemical stabilization of GO moieties on Fe\u003csub\u003e3\u003c/sub\u003eO\u003csub\u003e4\u003c/sub\u003e.\u003c/p\u003e\n\u003cp\u003eThe TGA curve of GO@Fe\u003csub\u003e3\u003c/sub\u003eO\u003csub\u003e4\u003c/sub\u003e@SiO\u003csub\u003e2\u003c/sub\u003e-NH\u003csub\u003e2\u003c/sub\u003e/IL cleared two weight losses. At temperatures in the range of 25 to 130\u0026deg;C, a weight loss of about 0.64% is assigned to the removal of water and organic solvents. The main weight loss at 210\u0026ndash;580\u0026deg;C (about 31%) corresponds to the elimination of grafted IL moieties confirming the high stability and well immobilization of IL species on the material surface Fig.\u0026nbsp;\u003cspan class=\"InternalRef\"\u003e5\u003c/span\u003e.\u003c/p\u003e\n\u003cp\u003eThe PXRD of GO@Fe\u003csub\u003e3\u003c/sub\u003eO\u003csub\u003e4\u003c/sub\u003e@SiO\u003csub\u003e2\u003c/sub\u003e-NH\u003csub\u003e2\u003c/sub\u003e/IL showed a pattern with six reflection peaks at 2\u0026theta; of 32, 38, 42, 58, 63 and 68 degrees, corresponding to the Miller indices values (\u003cem\u003ehkl\u003c/em\u003e) of 440, 511, 422, 400, 311 and 220, respectively, proving that the crystalline structure of the magnetite NPs is maintained during the adsorbent preparation steps Fig.\u0026nbsp;6 \u003csup\u003e53\u003c/sup\u003e.\u003c/p\u003e\n\u003cp\u003eThe EDS and EDS mapping analyses showed the presence and well distribution of C, N, Si, Fe, and O elements onto/into the nanocomposite framework and also confirmed the successful immobilization of the ionic liquids on the surface of the nanocomposite Figs.\u0026nbsp;\u003cspan class=\"InternalRef\"\u003e7\u003c/span\u003e and \u003cspan class=\"InternalRef\"\u003e8\u003c/span\u003e.\u003c/p\u003e\n\u003c/div\u003e\n\u003cdiv id=\"Sec8\" class=\"Section2\"\u003e\n\u003ch2\u003e3.2. Adsorption studies\u003c/h2\u003e\n\u003cdiv id=\"Sec9\" class=\"Section3\"\u003e\n\u003ch2\u003e3.2.1. Effect of pH\u003c/h2\u003e\n\u003cp\u003eIn the adsorption of Pb\u003csup\u003e2+\u003c/sup\u003e and BB dye by GO@Fe\u003csub\u003e3\u003c/sub\u003eO\u003csub\u003e4\u003c/sub\u003e@SiO\u003csub\u003e2\u003c/sub\u003e-NH\u003csub\u003e2\u003c/sub\u003e/IL nanocomposite, the pH effect was investigated. For this content, the pH was changed from 4 to 10, while other effective parameters including temperature (25\u0026deg;C), sonication time (20 min), initial concentration (Pb\u003csup\u003e2+\u003c/sup\u003e and BB) (10 mgL\u003csup\u003e\u0026minus;\u0026thinsp;1\u003c/sup\u003e), and the adsorbent dose (0.01 g) were kept constant. According to the results of Fig.\u0026nbsp;\u003cspan class=\"InternalRef\"\u003e9\u003c/span\u003ea, pH\u0026thinsp;=\u0026thinsp;7 was found to be the optimal pH for the removal of both Pb\u003csup\u003e2+\u003c/sup\u003e and BB. The decrease in removal percentage under acidic conditions can be attributed to the overabundance of H\u003csup\u003e+\u003c/sup\u003e ions, which can compete with BB dye and Pb\u003csup\u003e2+\u003c/sup\u003e ions \u003csup\u003e\u003cspan class=\"CitationRef\"\u003e3\u003c/span\u003e\u003c/sup\u003e. In addition, under acidic conditions, the adsorbent surface receives a positive charge, causing a strong electrostatic repulsion between the adsorbent and Pb\u003csup\u003e2+\u003c/sup\u003e ions, thereby reducing the removal percentage. Furthermore, at alkaline pH (pH\u0026thinsp;\u0026gt;\u0026thinsp;7), Pb\u003csup\u003e2+\u003c/sup\u003e ions precipitate, which reduces their removal. At alkaline pH (pH\u0026thinsp;\u0026gt;\u0026thinsp;7), the adsorbent surface becomes negatively charged creating a strong electrostatic repulsion with the BB dye.\u003c/p\u003e\n\u003c/div\u003e\n\u003cdiv id=\"Sec10\" class=\"Section3\"\u003e\n\u003ch2\u003e3.2.2. Temperature effect\u003c/h2\u003e\n\u003cp\u003eThe temperature effect (25, 30, 45, and 70\u0026deg;C) on the adsorption of Pb\u003csup\u003e2+\u003c/sup\u003e ions and BB dye molecules was evaluated at the fixed values of other parameters (0.01 g of the adsorbent, initial concentration of Pb\u003csup\u003e2+\u003c/sup\u003e and BB (10 mg L\u003csup\u003e\u0026minus;\u0026thinsp;1\u003c/sup\u003e), pH 7 and sonication time of 20 minutes). This showed that with increasing the temperature, the adsorption of both BB and Pb\u003csup\u003e2+\u003c/sup\u003e is increased. As shown in Fig.\u0026nbsp;\u003cspan class=\"InternalRef\"\u003e9\u003c/span\u003eb, the highest adsorption of BB (97%) is achieved at 45\u0026deg;C., while in comparison, the highest adsorption of Pb\u003csup\u003e2+\u003c/sup\u003e (95%) is obtained at 70\u0026deg;C.\u003c/p\u003e\n\u003c/div\u003e\n\u003cdiv id=\"Sec11\" class=\"Section3\"\u003e\n\u003ch2\u003e3.2.3. Contact time effect\u003c/h2\u003e\n\u003cp\u003eThe contact time effect (15\u0026ndash;45 minutes) on the removal of Pb\u003csup\u003e2+\u003c/sup\u003e ions and BB dye by GO@Fe\u003csub\u003e3\u003c/sub\u003eO\u003csub\u003e4\u003c/sub\u003e@SiO\u003csub\u003e2\u003c/sub\u003e-NH\u003csub\u003e2\u003c/sub\u003e/IL nanocomposite was investigated. The other parameters, including temperature (70\u0026deg;C for Pb\u003csup\u003e2+\u003c/sup\u003e ions, 45\u0026deg;C for BB dye, pH\u0026thinsp;=\u0026thinsp;7, initial concentration of Pb\u003csup\u003e2+\u003c/sup\u003e (10 mg L\u003csup\u003e\u0026minus;\u0026thinsp;1\u003c/sup\u003e), initial concentration of BB dye (10 mg L\u003csup\u003e\u0026minus;\u0026thinsp;1\u003c/sup\u003e) and adsorbent amount (0.01 g) were kept constant. As can be seen from Fig.\u0026nbsp;\u003cspan class=\"InternalRef\"\u003e9\u003c/span\u003ec, with increasing the contact time, the removal percentage of both Pb\u003csup\u003e2+\u003c/sup\u003e ions and BB dye molecules is increased. This is because the increase in the contact time increases the interactions between pollutants and the adsorbent and, subsequently, enhances the removal percentage. The maximum removal of Pb\u003csup\u003e2+\u003c/sup\u003e ions and BB dye molecules was achieved in a contact time of 35 minutes. After 35 minutes, the removal efficiency was decreased, which may be attributed to the desorption of Pb\u003csup\u003e2+\u003c/sup\u003e ions and BB dye molecules under ultrasonic irradiation.\u003c/p\u003e\n\u003c/div\u003e\n\u003cdiv id=\"Sec12\" class=\"Section3\"\u003e\n\u003ch2\u003e\u003cstrong\u003e3.2.4. Adsorbent dose effect\u003c/strong\u003e\u003c/h2\u003e\n\u003cp\u003eTo evaluate the adsorbent amount effect on the removal of Pb\u003csup\u003e2+\u003c/sup\u003e ions and BB dye molecules by GO@Fe\u003csub\u003e3\u003c/sub\u003eO\u003csub\u003e4\u003c/sub\u003e@SiO\u003csub\u003e2\u003c/sub\u003e-NH\u003csub\u003e2\u003c/sub\u003e/IL nanocomposite, different doses of adsorbent (0.005, 0.01, 0.015, and 0.02 g) were evaluated under the optimum values of the other parameters. The values of other parameters were: contact time (35 minutes), temperature of 45\u0026deg;C for BB molecules and 70\u0026deg;C for Pb\u003csup\u003e2+\u003c/sup\u003e ions, initial concentration of 10 mg L\u003csup\u003e\u0026minus;\u0026thinsp;1\u003c/sup\u003e for Pb\u003csup\u003e2+\u003c/sup\u003e and BB molecules, and pH\u0026thinsp;=\u0026thinsp;7. According to the data presented in Fig.\u0026nbsp;\u003cspan class=\"InternalRef\"\u003e9\u003c/span\u003ed, by increasing the adsorbent amount from 0.005 g to 0.015 g, the removal percentage was increased. This is because increasing the adsorbent amount increases the interaction sites for adsorbing pollutants. As shown, the maximum adsorption of Pb\u003csup\u003e2+\u003c/sup\u003e ions and BB molecules is achieved using only 0.015 g of the nanocomposite.\u003c/p\u003e\n\u003c/div\u003e\n\u003cdiv id=\"Sec13\" class=\"Section3\"\u003e\n\u003ch2\u003e3.2.5. Effect of the initial concentrations of Pb\u003csup\u003e2+\u003c/sup\u003e ions and BB dye molecules\u003c/h2\u003e\n\u003cp\u003eThe effect of the initial concentrations of Pb\u003csup\u003e2+\u003c/sup\u003e ions and BB dye molecules (5\u0026ndash;30 mg. L\u003csup\u003e\u0026minus;\u0026thinsp;1\u003c/sup\u003e) on the removal process by the GO@Fe\u003csub\u003e3\u003c/sub\u003eO\u003csub\u003e4\u003c/sub\u003e@SiO\u003csub\u003e2\u003c/sub\u003e-NH\u003csub\u003e2\u003c/sub\u003e/IL nanocomposite was also examined. The values of the other parameters were: adsorbent dose of (0.015 g), temperature (45\u0026deg;C for BB and 70\u0026deg;C for Pb\u003csup\u003e2+\u003c/sup\u003e), sonication time (25\u0026ndash;35 minutes), and pH\u0026thinsp;=\u0026thinsp;7. According to the findings of Fig.\u0026nbsp;\u003cspan class=\"InternalRef\"\u003e9\u003c/span\u003ee, the removal percentage of BB dye and Pb\u003csup\u003e2+\u003c/sup\u003e ions was decreased by increasing their initial concentrations. At lower concentrations of Pb\u003csup\u003e2+\u003c/sup\u003e and BB, the GO@Fe\u003csub\u003e3\u003c/sub\u003eO\u003csub\u003e4\u003c/sub\u003e@SiO\u003csub\u003e2\u003c/sub\u003e-NH\u003csub\u003e2\u003c/sub\u003e/IL nanocomposite sites have more opportunities to interact with Pb\u003csup\u003e2+\u003c/sup\u003e ions and BB dye molecules. By increasing concentrations of Pb\u003csup\u003e2+\u003c/sup\u003e and BB, the adsorption sites of the nanocomposite are saturated, and then the removal percentage is decremented.\u003c/p\u003e\n\u003cp\u003eNext, the EDS analysis was carried out to evaluate the efficiency of the GO@Fe\u003csub\u003e3\u003c/sub\u003eO\u003csub\u003e4\u003c/sub\u003e@SiO\u003csub\u003e2\u003c/sub\u003e-NH\u003csub\u003e2\u003c/sub\u003e/IL adsorbent for the removal of Pb ion and BB dye. After adsorption process, the new signals of Pb and S have been observed in the EDS spectra (Figs.\u0026nbsp;\u003cspan class=\"InternalRef\"\u003e10\u003c/span\u003e and \u003cspan class=\"InternalRef\"\u003e11\u003c/span\u003e), confirming the successful removal of both Pb ions and BB dye on the designed GO@Fe\u003csub\u003e3\u003c/sub\u003eO\u003csub\u003e4\u003c/sub\u003e@SiO\u003csub\u003e2\u003c/sub\u003e-NH\u003csub\u003e2\u003c/sub\u003e/IL adsorbent.\u003c/p\u003e\n\u003c/div\u003e\n\u003c/div\u003e\n\u003cdiv id=\"Sec14\" class=\"Section2\"\u003e\n\u003ch2\u003e3.3. Adsorption isotherms\u003c/h2\u003e\n\u003cp\u003eTo properly understand the adsorption mechanism, as well as the maximum adsorption of BB and Pb\u003csup\u003e+\u0026thinsp;2\u003c/sup\u003e by GO@Fe\u003csub\u003e3\u003c/sub\u003eO4@SiO\u003csub\u003e2\u003c/sub\u003e-NH\u003csub\u003e2\u003c/sub\u003e/IL, different isotherm models, including Langmuir, Freundlich, and Temkin, were assessed \u003csup\u003e\u003cspan class=\"CitationRef\"\u003e47\u003c/span\u003e\u0026ndash;\u003cspan class=\"CitationRef\"\u003e50\u003c/span\u003e, \u003cspan class=\"CitationRef\"\u003e54\u003c/span\u003e, \u003cspan class=\"CitationRef\"\u003e55\u003c/span\u003e\u003c/sup\u003e. The results are presented in Table\u0026nbsp;\u003cspan class=\"InternalRef\"\u003e1\u003c/span\u003e.\u003c/p\u003e\n\u003cdiv class=\"gridtable\"\u003e\n\u003cdiv class=\"colspec\" align=\"left\"\u003e\u0026nbsp;\u003c/div\u003e\n\u003ctable id=\"Tab1\" border=\"1\"\u003e\u003ccaption\u003e\n\u003cdiv class=\"CaptionNumber\"\u003eTable 1\u003c/div\u003e\n\u003cdiv class=\"CaptionContent\"\u003e\n\u003cp\u003eAdsorption isotherm models parameters for the adsorption of Pb\u003csup\u003e+\u0026thinsp;2\u003c/sup\u003e and BB using GO@Fe\u003csub\u003e3\u003c/sub\u003eO\u003csub\u003e4\u003c/sub\u003e@SiO\u003csub\u003e2\u003c/sub\u003e-NH\u003csub\u003e2\u003c/sub\u003e/IL\u003c/p\u003e\n\u003c/div\u003e\n\u003c/caption\u003e\n\u003cthead\u003e\n\u003ctr\u003e\n\u003cth colspan=\"4\" align=\"left\"\u003e\n\u003cp\u003eBB Pb\u003c/p\u003e\n\u003cp\u003eAdsorbent dosage (g) 0.01 0.015\u003c/p\u003e\n\u003c/th\u003e\n\u003c/tr\u003e\n\u003c/thead\u003e\n\u003ctbody\u003e\n\u003ctr\u003e\n\u003ctd colspan=\"4\" align=\"left\"\u003e\n\u003cp\u003eIsotherm Parameters Value of parameters\u003c/p\u003e\n\u003c/td\u003e\n\u003c/tr\u003e\n\u003ctr\u003e\n\u003ctd align=\"left\"\u003e\n\u003cp\u003eLangmuir\u003c/p\u003e\n\u003c/td\u003e\n\u003ctd align=\"left\"\u003e\n\u003cp\u003eQ\u003csub\u003em\u003c/sub\u003e (mg g\u003csup\u003e_1\u003c/sup\u003e)\u003c/p\u003e\n\u003cp\u003eK\u003csub\u003ea\u003c/sub\u003e (L mg\u003csup\u003e_1\u003c/sup\u003e)\u003c/p\u003e\n\u003cp\u003eR\u003csup\u003e2\u003c/sup\u003e\u003c/p\u003e\n\u003c/td\u003e\n\u003ctd align=\"left\"\u003e\n\u003cp\u003e84.76\u003c/p\u003e\n\u003cp\u003e68\u003c/p\u003e\n\u003cp\u003e0.952\u003c/p\u003e\n\u003c/td\u003e\n\u003ctd align=\"left\"\u003e\n\u003cp\u003e83.34\u003c/p\u003e\n\u003cp\u003e98\u003c/p\u003e\n\u003cp\u003e0.939\u003c/p\u003e\n\u003c/td\u003e\n\u003c/tr\u003e\n\u003ctr\u003e\n\u003ctd align=\"left\"\u003e\n\u003cp\u003eFreundlich\u003c/p\u003e\n\u003c/td\u003e\n\u003ctd align=\"left\"\u003e\n\u003cp\u003e1/n\u003c/p\u003e\n\u003cp\u003eK\u003csub\u003eF\u003c/sub\u003e (L mg\u003csup\u003e_1\u003c/sup\u003e)\u003c/p\u003e\n\u003cp\u003eR\u003csup\u003e2\u003c/sup\u003e\u003c/p\u003e\n\u003c/td\u003e\n\u003ctd align=\"left\"\u003e\n\u003cp\u003e0.245\u003c/p\u003e\n\u003cp\u003e2.25\u003c/p\u003e\n\u003cp\u003e0.940\u003c/p\u003e\n\u003c/td\u003e\n\u003ctd align=\"left\"\u003e\n\u003cp\u003e0.340\u003c/p\u003e\n\u003cp\u003e4.23\u003c/p\u003e\n\u003cp\u003e0.937\u003c/p\u003e\n\u003c/td\u003e\n\u003c/tr\u003e\n\u003ctr\u003e\n\u003ctd align=\"left\"\u003e\n\u003cp\u003eTemkin\u003c/p\u003e\n\u003c/td\u003e\n\u003ctd align=\"left\"\u003e\n\u003cp\u003eB1\u003c/p\u003e\n\u003cp\u003eK\u003csub\u003eT\u003c/sub\u003e(L mg\u003csup\u003e_1\u003c/sup\u003e)\u003c/p\u003e\n\u003cp\u003eR\u003csup\u003e2\u003c/sup\u003e\u003c/p\u003e\n\u003c/td\u003e\n\u003ctd align=\"left\"\u003e\n\u003cp\u003e16.91\u003c/p\u003e\n\u003cp\u003e5.84\u003c/p\u003e\n\u003cp\u003e0.950\u003c/p\u003e\n\u003c/td\u003e\n\u003ctd align=\"left\"\u003e\n\u003cp\u003e12.83\u003c/p\u003e\n\u003cp\u003e8.73\u003c/p\u003e\n\u003cp\u003e0.909\u003c/p\u003e\n\u003c/td\u003e\n\u003c/tr\u003e\n\u003c/tbody\u003e\n\u003c/table\u003e\n\u003c/div\u003e\n\u003cp\u003eThe equations of the isotherms are as follows:\u003c/p\u003e\n\u003cp\u003eLangmuir\u003cspan class=\"InlineEquation\"\u003e\u003cspan class=\"mathinline\"\u003e\\(\\frac{\\varvec{C}}{\\varvec{q}}\\varvec{=}\\frac{\\varvec{1}}{{\\varvec{K}{\\varvec{q}_\\varvec{m}}}}\\varvec{+}\\frac{\\varvec{C}}{{{\\varvec{q}_\\varvec{m}}}}\\)\u003c/span\u003e\u003c/span\u003e:\u003c/p\u003e\n\u003cp\u003eIn this relation, C (mg L\u003csup\u003e\u0026minus;\u0026thinsp;1\u003c/sup\u003e) represents the concentration of equilibrium of the species (the remaining concentration of the species in the solution that the adsorbent could not absorb), q (mg g \u003csup\u003e\u0026minus;\u0026thinsp;1\u003c/sup\u003e) is the amount of species absorbed on the surface of the adsorbent, K (L mg \u003csup\u003e\u0026minus;\u0026thinsp;1\u003c/sup\u003e) is Langmuir's equilibrium constant, and q\u003csub\u003em\u003c/sub\u003e (mg. g \u003csup\u003e\u0026minus;\u0026thinsp;1\u003c/sup\u003e) is the maximum amount of species that can be absorbed by a certain amount of adsorbent \u003csup\u003e\u003cspan class=\"CitationRef\"\u003e51\u003c/span\u003e, \u003cspan class=\"CitationRef\"\u003e52\u003c/span\u003e\u003c/sup\u003e.\u003c/p\u003e\n\u003cp\u003eFreundlich:\u003c/p\u003e\n\u003cp\u003e\u003cspan class=\"InlineEquation\"\u003e \u003cspan class=\"mathinline\"\u003e\\(\\varvec{Ln}{\\varvec{q}_\\varvec{e}}\\varvec{=Ln}{\\varvec{K}_\\varvec{f}}\\varvec{+}\\frac{\\varvec{1}}{\\varvec{n}}\\varvec{Ln}{\\varvec{C}_\\varvec{e}}\\)\u003c/span\u003e\u0026nbsp;\u003c/span\u003e\u003c/p\u003e\n\u003cp\u003ewhere q\u003csub\u003ee\u003c/sub\u003e (mg/g) is the amount of substance absorbed per adsorbent mass, and C\u003csub\u003ee\u003c/sub\u003e (mg/L) is the concentration of the equilibrium in the solution. Freundlich's constants, n and K\u003csub\u003ef\u003c/sub\u003e, are the adsorption intensity and relative adsorption capacity of the adsorbent, respectively. When K\u003csub\u003ef\u003c/sub\u003e increases, the adsorption capacity of the adsorbent increases to absorb the adsorbed substance \u003csup\u003e\u003cspan class=\"CitationRef\"\u003e52\u003c/span\u003e, \u003cspan class=\"CitationRef\"\u003e56\u003c/span\u003e\u003c/sup\u003e.\u003c/p\u003e\n\u003cp\u003eTemkin:\u003c/p\u003e\n\u003cp\u003e\u003cspan class=\"InlineEquation\"\u003e \u003cspan class=\"mathinline\"\u003e\\({\\varvec{q}_\\varvec{e}}\\varvec{=}{\\varvec{B}_\\varvec{1}}\\varvec{Ln}{\\varvec{K}_\\varvec{t}}\\varvec{+}{\\varvec{B}_\\varvec{1}}\\varvec{Ln}{\\varvec{C}_\\varvec{e}}\\)\u003c/span\u003e \u003c/span\u003e\u003c/p\u003e\n\u003cp\u003eB\u003csub\u003e1\u003c/sub\u003e and K\u003csub\u003et\u003c/sub\u003e are the parameters of the model, which are calculated by using the chart that B\u0026thinsp;=\u0026thinsp;RT/b and K\u003csub\u003et\u003c/sub\u003e are the temperature constants of Temkin, which are proportional to the heat of surface adsorption and the bond constant associated with the maximum bond energy. The adsorption isotherm diagrams of BB and Pb\u003csup\u003e+\u0026thinsp;2\u003c/sup\u003e (Langmuir, Freundlich, and Temkin), are shown in Table\u0026nbsp;\u003cspan class=\"InternalRef\"\u003e1\u003c/span\u003e. According to the results of Table\u0026nbsp;\u003cspan class=\"InternalRef\"\u003e1\u003c/span\u003e, the removal process was followed by the Langmuir and Freundlich models, which was due to their higher R\u003csup\u003e\u003cspan class=\"CitationRef\"\u003e2\u003c/span\u003e\u003c/sup\u003e compared to the Temkin. The Langmuir model undertakes that the process of adsorption is monolayer and the surface of the adsorbent is homogenous. While the Freundlich model undertakes that this process is multilayer and the surface of the adsorbent is heterogeneous. The maximum adsorption according to the Langmuir model for BB dye molecules and Pb\u003csup\u003e+\u0026thinsp;2\u003c/sup\u003e ions were 84.76 and 83.34 mg g\u003csup\u003e\u0026minus;\u0026thinsp;1\u003c/sup\u003e, respectively. The n values of the Freundlich model were greater than 1, which represents a promising adsorption condition. The n values between 2\u0026ndash;10 in the model of Freundlich show an easy adsorption. Moreover, the n\u0026thinsp;=\u0026thinsp;1\u0026ndash;2 and n\u0026thinsp;\u0026lt;\u0026thinsp;1 illustrate moderate and difficult adsorption, respectively.\u003c/p\u003e\n\u003c/div\u003e\n\u003cdiv id=\"Sec15\" class=\"Section2\"\u003e\n\u003ch2\u003e3.4. Possible mechanism of absorption\u003c/h2\u003e\n\u003cp\u003eThe adsorption mechanism of Pb\u003csup\u003e+\u0026thinsp;2\u003c/sup\u003e and BB by GO@Fe\u003csub\u003e3\u003c/sub\u003eO\u003csub\u003e4\u003c/sub\u003e@SiO\u003csub\u003e2\u003c/sub\u003e-NH\u003csub\u003e2\u003c/sub\u003e/IL nanocomposite was investigated. Since the GO@Fe\u003csub\u003e3\u003c/sub\u003eO\u003csub\u003e4\u003c/sub\u003e@SiO\u003csub\u003e2\u003c/sub\u003e-NH\u003csub\u003e2\u003c/sub\u003e/IL nanocomposite contains the ionic liquid ion pairs, therefore, the adsorption of both BB cationic dye and Pb\u003csup\u003e2+\u003c/sup\u003e ions may be performed \u003cem\u003evia\u003c/em\u003e their electrostatic interaction with the ionic liquid moieties Fig.\u0026nbsp;\u003cspan class=\"InternalRef\"\u003e12\u003c/span\u003e.\u003c/p\u003e\n\u003cp\u003eThe recyclability and reusability of GO@Fe\u003csub\u003e3\u003c/sub\u003eO\u003csub\u003e4\u003c/sub\u003e@SiO\u003csub\u003e2\u003c/sub\u003e-NH\u003csub\u003e2\u003c/sub\u003e/IL nanocomposite were also studied in the adsorption of both Pb\u003csup\u003e+\u0026thinsp;2\u003c/sup\u003e and BB under optimal conditions. For this purpose, after the completion of the adsorption process for each sample, the absorbent was magnetically separated and washed completely with water and ethanol. Then, it was reused under the same conditions as the first run. It was found that the designed adsorbent could be recovered and reapplied at least three times with no significant loss of efficiency Fig.\u0026nbsp;\u003cspan class=\"InternalRef\"\u003e13\u003c/span\u003e. These results confirm the high performance and excellent stability of the designed adsorbent in practical conditions.\u003c/p\u003e\n\u003cp\u003e\u0026nbsp;\u003c/p\u003e\n\u003c/div\u003e"},{"header":"4. Conclusion","content":"\u003cp\u003eIn this research, a novel magnetic nanocomposite (GO@Fe\u003csub\u003e3\u003c/sub\u003eO\u003csub\u003e4\u003c/sub\u003e@SiO\u003csub\u003e2\u003c/sub\u003e-NH\u003csub\u003e2\u003c/sub\u003e/IL) was developed to remove Pb\u003csup\u003e2+\u003c/sup\u003e ions and BB dye from aqueous solutions. This nanocomposite was characterized by using FT-IR, EDX, SEM, TG, and VSM analyses. The effects of initial concentration, pH value, initial concentration of pollutant (Pb\u003csup\u003e2+\u003c/sup\u003e ions or BB dye), time, and adsorbent amount on the adsorption of Pb\u003csup\u003e2+\u003c/sup\u003e ions and BB dye by GO@Fe\u003csub\u003e3\u003c/sub\u003eO\u003csub\u003e4\u003c/sub\u003e@SiO\u003csub\u003e2\u003c/sub\u003e-NH\u003csub\u003e2\u003c/sub\u003e/IL were studied to determine the optimal conditions. The findings revealed that the optimal conditions were achieved at pH 7, 0.01 g of adsorbent, 5 min of contact time, and initial pollutant concentrations of 5 mg L\u003csup\u003e\u0026minus;\u0026thinsp;1\u003c/sup\u003e and temperatures of 45\u0026deg;C for BB dye and at 70\u0026deg;C for Pb\u003csup\u003e2+\u003c/sup\u003e ions. The ease of separation of the nanocomposite using an external magnet, rapid adsorption rate, ability to recycle up to four times with minimal waste, superior adsorption capacity for heavy metals and dye pollutants, and environmentally friendly nature of the adsorbent stand out as its unique and superior characteristics compared to other previously developed adsorbents.\u003c/p\u003e"},{"header":"Declarations","content":"\u003cp\u003e \u003ch2\u003eCompeting interests\u003c/h2\u003e \u003cp\u003eThe authors declare no competing interests.\u003c/p\u003e \u003c/p\u003e\u003ch2\u003eAuthor Contribution\u003c/h2\u003e\u003cp\u003eF. D.: Investigation, Writing\u0026mdash;original draft, Formal analysis, Resources. D. E.: Conceptualization, Writing \u0026ndash; review\u0026amp; editing, Visualization, Supervision.\u003c/p\u003e\u003ch2\u003eAcknowledgements\u003c/h2\u003e \u003cp\u003eThe authors thank Yasouj University and Iran National Science Foundation (INSF) for supporting this work.\u003c/p\u003e\u003ch2\u003eData Availability\u003c/h2\u003e\u003cp\u003eAll the research date is include in the manuscript.\u003c/p\u003e"},{"header":"References","content":"\u003col\u003e\n\u003cli\u003eF.S. Abdulraheem, Z.S. Al-Khafaji, K.S. Hashim, M. Muradov, P. Kot, A.A. Shubbar, in Natural filtration unit for removal of heavy metals from water, p. 012034, IOP Publishing, Abdulraheem, F. S., Al-Khafaji, Z. S., Hashim, K. S., Muradov, M., Kot, P., \u0026amp; Shubbar, A. A. Natural filtration unit for removal of heavy metals from water. Mater. Sci. Eng. 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Thermodyn \u003cstrong\u003e2013,\u003c/strong\u003e\u0026nbsp; 375830 (2013).\u003c/li\u003e\n\u003c/ol\u003e"}],"fulltextSource":"","fullText":"","funders":[],"hasAdminPriorityOnWorkflow":false,"hasManuscriptDocX":true,"hasOptedInToPreprint":true,"hasPassedJournalQc":"","hasAnyPriority":false,"hideJournal":true,"highlight":"","institution":"","isAcceptedByJournal":false,"isAuthorSuppliedPdf":false,"isDeskRejected":"","isHiddenFromSearch":false,"isInQc":false,"isInWorkflow":false,"isPdf":false,"isPdfUpToDate":true,"isWithdrawnOrRetracted":false,"journal":{"display":true,"email":"[email protected]","identity":"researchsquare","isNatureJournal":false,"hasQc":true,"allowDirectSubmit":true,"externalIdentity":"","sideBox":"","snPcode":"","submissionUrl":"/submission","title":"Research Square","twitterHandle":"researchsquare","acdcEnabled":true,"dfaEnabled":false,"editorialSystem":"","reportingPortfolio":"","inReviewEnabled":false,"inReviewRevisionsEnabled":true},"keywords":"Magnetic graphene oxide, Ionic liquid, Adsorbent, Lead ions, Brilliant blue dye","lastPublishedDoi":"10.21203/rs.3.rs-4986593/v1","lastPublishedDoiUrl":"https://doi.org/10.21203/rs.3.rs-4986593/v1","license":{"name":"CC BY 4.0","url":"https://creativecommons.org/licenses/by/4.0/"},"manuscriptAbstract":"\u003cp\u003eIn this research, a magnetic graphene oxide modified with ionic liquid has been synthesized and used as a powerful nanocomposite for the removal of lead (Pb\u003csup\u003e2+\u003c/sup\u003e) ions and brilliant blue (BB) dye from a water sample. This nanocomposite was characterized by using EDS, FTIR, SEM, and VSM techniques, which confirmed the successful formation of the desired nanocomposite and good immobilization of the ionic liquid. The ultraviolet-visible (UV-Vis) and atomic absorption (AA) spectroscopy techniques were employed to quantify the extent of removal of Pb\u003csup\u003e2+\u003c/sup\u003e ions and BB dye. The removal percentages of Pb\u003csup\u003e2+\u003c/sup\u003e ions and BB dye by the prepared nanocomposite were 94% and 96%, respectively, demonstrating its excellent performance. According to the Langmuir isotherm, the maximum adsorption capacities of the nanocomposite toward Pb\u003csup\u003e2+\u003c/sup\u003e ions and BB dye were achieved to be 83.34 and 84.76 mg g\u003csup\u003e\u0026minus;\u0026thinsp;1\u003c/sup\u003e, respectively. Also, this nanocomposite was recoverable and reusable at least three times.\u003c/p\u003e","manuscriptTitle":"Ionic liquid-modified magnetic graphene oxide nanocomposite as a powerful adsorbent for the removal of lead ions and brilliant blue dye","msid":"","msnumber":"","nonDraftVersions":[{"code":1,"date":"2024-09-27 12:27:58","doi":"10.21203/rs.3.rs-4986593/v1","editorialEvents":[{"type":"communityComments","content":0}],"status":"published","journal":{"display":true,"email":"[email protected]","identity":"researchsquare","isNatureJournal":false,"hasQc":true,"allowDirectSubmit":true,"externalIdentity":"","sideBox":"","snPcode":"","submissionUrl":"/submission","title":"Research Square","twitterHandle":"researchsquare","acdcEnabled":true,"dfaEnabled":false,"editorialSystem":"","reportingPortfolio":"","inReviewEnabled":false,"inReviewRevisionsEnabled":true}}],"origin":"","ownerIdentity":"0c61a223-4fcb-42d0-9e65-09cd71c87c2c","owner":[],"postedDate":"September 27th, 2024","published":true,"recentEditorialEvents":[],"rejectedJournal":[],"revision":"","amendment":"","status":"posted","subjectAreas":[{"id":38188201,"name":"Earth and environmental sciences/Environmental sciences"},{"id":38188202,"name":"Physical sciences/Chemistry"}],"tags":[],"updatedAt":"2024-12-11T06:38:18+00:00","versionOfRecord":[],"versionCreatedAt":"2024-09-27 12:27:58","video":"","vorDoi":"","vorDoiUrl":"","workflowStages":[]},"version":"v1","identity":"rs-4986593","journalConfig":"researchsquare"},"__N_SSP":true},"page":"/article/[identity]/[[...version]]","query":{"redirect":"/article/rs-4986593","identity":"rs-4986593","version":["v1"]},"buildId":"7rjqhiLT3MXkJMwkYKINL","isFallback":false,"isExperimentalCompile":false,"dynamicIds":[84888],"gssp":true,"scriptLoader":[]}