# A Study of Methylene Blue Dye Interaction and Adsorption by Monolayer Graphene Oxide

Authors: Jakub Ederer; Petra Ecorchard; Michaela Šrámová Slušná; Jakub Tolasz; Darina Smržová; Simona Lupínková; Pavel Janoš
Journal: Adsorption Science & Technology
 (2022)

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## Abstract

The graphene oxide (GO) interaction with methylene blue (MB) cationic dye was studied in an aqueous solution at different pH during MB adsorption. The mutual interaction of MB with GO surface was studied and evaluated by Fourier transform infrared spectroscopy (FTIR) and X-ray diffraction (XRD). Theπ-π and electrostatic interaction of MB with GO surface are the main types of interactions, and the XRD data show the monomeric arrangement of MB cation with GO. The GO surface functional groups and point of zero charge (PZC) were determined by acid-base titration. Suitability of zeta-potential measurement and acid-base titration method was briefly discussed. The quality of prepared GO was evaluated by Raman spectroscopy, XRD, and atomic force microscope (AFM). The experimental adsorption equilibrium data were analyzed using Langmuir, Langmuir-Freundlich, Freundlich, and Temkin isotherms. The GO maximum adsorption capacity increases with higher pH, that is ascribed to the facile interaction of negatively charged GO with positively charged MB structure.


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## Body

## 1. Introduction

The growth of the textile industry is responsible for the increasing pollution, mainly in the water environment. The textile industry commonly uses plenty of dyes, representing potential dangers for nature and health [1]. Moreover, many dyes are toxic and carcinogenic and can also consume dissolved oxygen and destroy aquatic life. In nature, dyes could undergo various types of reactions whose products could be more toxic and dangerous for living beings [2]. Therefore, it is important to look for efficient methods and materials for their removal. Many methods have been suggested for wastewater treatment and dyes removal, like adsorption [3, 4], biodegradation [5, 6], oxidation [7, 8], or photocatalytic degradation [7, 9–11]. Adsorption belongs to the simplest, noncomplicated, and low-cost method for removing various types of pollution, including dyes. Various types of adsorbents such as carbon-based materials [2, 12–16], chitosan [17], layered double hydroxides [3, 18, 19], cotton fibers [20], montmorillonite [21, 22], metal oxides, and metal oxide composites [23–25] have been studied for the adsorption of various dyes. Other materials that are often used to remove dyes include doped conducting polymers, like polyaniline doped by boron nitride [26], chitosan-grafted-polyaniline doped with Co3O4 [27], and polyaniline/Co3O4 nanocube composite [28], or polyaniline/SrTiO3 nanocubes [29], and those composites were successfully applied in adsorption or photocatalytic degradation methyl orange and MB dyes [26–29]. These materials are becoming more popular as they offer a wide range of applications such as sensors, adsorbents, photocatalysis, and batteries [26–29]. GO and its composites belong to the aforementioned popular adsorbents [30, 31]. GO belongs to the carbonaceous materials with an ideal two-dimensional structure with carbon atoms assembled to the honeycomb structure. The presence of various types of oxygen-containing surface functional groups (carboxyl, hydroxyl, epoxy, and carbonyl) belongs among the greatest GO benefits. These surface groups facilitate and contribute to the adsorption process via π-π stacking, hydrogen bonding, and electrostatic forces, such as van der Waals forces. They act as a weak acid cation exchange material, allow various GO modifications [32–36], and also complexation with positively charged molecules (dyes, pesticides, metal ions, etc.) [13, 14]. The information such as the GO surface hydroxyl group number and their effect on the adsorption process is limited in the scientific papers. GO-based materials with different degrees of oxidation were successfully applied in removing MB dyes with maximum adsorption capacity from 48.8 to 598.8 mg/g [37]. GO prepared by Hummer’s method or GO/calcium alginate was used in MB adsorption with a maximum adsorption capacity of 476.2 mg/g and 181.8 mg/g, respectively [38, 39]. According to Chen et al. [37] and Ramesha et al. [13], reduced GO can also be involved in removing the dye, with a relatively low adsorption capacity of 91 and 17.3 mg/g, respectively. MB (Figure 1) belongs to the widely used dying agents for coloring silks, cotton, paper, temporary hair color, wools, etc. [12, 16]. It is also used in medicine, analytical redox indicator, and aquaculture [2]. MB can have some negative effects on human health, including headache, confusion, high blood pressure, and vomiting [40, 41].Figure 1
Methylene blue structure (CAS 61-73-4).In this paper, we prepared monolayer GO by a simple ultrasound exfoliation process of natural graphite with subsequent oxidation, and we compared the adsorption ability of GO at various pHs for MB removal from an aqueous solution. In order to establish the GO removal capacity, different models of isotherms (Langmuir, Langmuir-Freundlich, Temkin, and Freundlich) were fitted to the experimental data. Besides, the MB adsorption kinetics were studied, and mathematical models for the pseudo-first order and pseudo-second order were applied for measured data. The Langmuir and Langmuir-Freundlich isotherms were used to obtain the maximum adsorption capacity, whereas the Temkin model was used to evaluate some indirect interaction of MB with GO. Raman spectroscopy, transmission electron microscopy (TEM), AFM, and zeta-potential were used for GO characterization, and the data combination from these methods was used to identify and characterize the mutual interactions of MB with GO structure. The GO surface functional groups (carboxylic and hydroxyl) were determined with simple and verified acid-base titration, and the effect of GO surface functional groups on MB adsorption was discussed. The suitability of zeta-potential measurement and acid-base titration method was discussed. The FTIR and XRD were used for GO characterization and analysis of the adsorbent before and after dye adsorption and for discussion of possible adsorption mechanisms. Based on FTIR and XRD data, specific interactions of surface groups with MB were shown and confirmed.


## 2. Experimental

### 2.1. Chemicals

All purchased chemicals were analytical reagent grade. MB (≥95%; calc. to the dried substance) was purchased from Sigma-Aldrich (Germany). The chemical reagents for preparation of Britton-Robinson buffer (BRB), i.e., CH3COOH, H3BO3, NaOH, and H3PO4 were purchased from Lach-Ner Ltd. The BRB solution was prepared according to the standard procedure published elsewhere [42]. Briefly, two solutions A and B were prepared. Solution A consists of a mixture of H3BO3, H3PO4, and CH3COOH with the concentration of each compound at 0.04 mol/L. Next, solution B was prepared by dissolving solid NaOH to obtain a solution with a concentration of 0.02 mol/L. By mixing solutions A and B, the solutions with the required pH (3.0, 7.0, and 11.0) were prepared. The stock solution of cationic MB dye (0.5 g/L) was prepared in BRB (pH=3.0, 7.0 and 11.0). KBr (FTIR grade, ≥99% trace metal basis) was used for FTIR measurements and was purchased from Sigma-Aldrich (Germany). Deionized water prepared by GORO Pharmpur reverse osmosis system (Goro, Czech Republic) was used for all the experiments. The chemical reagents for the synthesis of graphene oxide (GO), i.e., 96% H2SO4, 85% H3PO4, KMnO4, and H2O2, were obtained from commercial sources Penta, Ltd. and Lach-Ner, Ltd. (Czech Republic). The natural graphite was purchased from Koh-i-noor Grafite, Ltd. (Czech Republic).


### 2.2. Preparation of Sample

#### 2.2.1. Preparation of Graphene

Graphene sheets were prepared by exfoliation of natural graphite (1 g) in a bath ultrasound reactor UIP 2000hd (2 kHz, max. 2000 W, Hielscher Ultrasonics GmbH, Germany) under a high pressure of 5 bar in ethylene glycol (100 mL) [43]. The product was purified by dialysis with Spectra/Por 3 dialysis membrane in demineralized water to stable conductivity and constant pH.


#### 2.2.2. Preparation of Graphene Oxide

The dried exfoliated graphite (1 g) was mixed with H2SO4 (60 mL) and H3PO4 (10 mL) in a round-bottom flask. KMnO4 (3 g) was carefully added last. The reaction mixture was slowly heated to 40°C for 48 h. The additional KMnO4 (1.5 g) was added in smaller doses and stirred for 3 days at the same temperature. Thereafter, the mixture was left to cool down to laboratory temperature and slowly added to the ice mixture with H2O2 (200 mL) [44]. The resulting product was purified by dialysis with Spectra/Por 3 dialysis membrane in demineralized water to constant pH and stable conductivity.


### 2.3. Characterization of Samples

The FTIR spectra were recorded on a diffuse reflectance spectrophotometer Nicolet 6700 IR (Thermo Scientific, USA) in transmittance mode in the 4000−400 cm−1 wavenumber range at 100 scans per spectrum with 4 cm−1 resolution. Software OMNIC 7.3 was used for raw data processing. The GO sample for FTIR was firstly lyophilized (24 h) and subsequently grounded with KBr in a ratio from 1 : 100 to 1 : 400 in an agate mortar and then in a ball mill (5 min). A hydraulic press (80 kN, 5 min) was used to prepare KBr pellets of 13 mm in diameter.Raman spectra were collected using a DXR Raman microscope (Thermo Scientific, USA) the following way: 256 two-second scans were acquired with a 532 nm laser (0.5 mW), 25μm slit under a 10× objective Olympus microscope in full range with distinction of 2 cm−1. Crystal phase analysis was performed using Bruker D2 (Germany) with the LYNXEYE 1-dimensional detector (CuKα radiation, 30 kV, 10 mA). The primary divergence slit module width of 0.6 mm, Soler Module 2.5, Airscatter screen module of 2 mm, and Ni Kbeta-filter of 0.5 mm were used in the range of 5-90°, step of 0.00805°, and time per step of 1.0 s. The XRD sample patterns after interaction with MB were processed by the following procedure. First, the GO suspension (0.1 mL) was mixed with MB solution (2.1 mL, 0.2 g/L) in 4 mL vials and were shaken for 4 h. Further, the samples were centrifuged (30 min, 10 000 RPM), washed four times with deionized water, and followed by centrifugation (shorter time). Finally, the samples were transferred to a silicon wafer, dried and measured.Morphology of the samples deposited on microscopic copper grids covered by a transparent amorphous lacey carbon film was investigated using HRTEM FEI Talos F200X (Japan) at 120 kV. The obtained micrographs and SAED patterns (Selected area electron diffraction) were processed and evaluated by the TIA (TEM Imaging & Analysis software, FEI Company). AFM measurements were performed using Bruker Dimension Microscope (Germany) in ScanAsyst-air contact mode to determine lateral size and height profile of GO sheets. An aqueous suspension was pipetted onto mica support prior the measurement.


### 2.4. Titration of GO Sample

According to our procedure published in our previous work [44], acid-base titration was used to determine the number of surface functional groups, i.e., carboxylic and hydroxyl. Titration of GO sample was realized by automatic titrator 794 Basic Titrino (Metrohm, Switzerland) with potentiometric endpoint determination. GO water suspension containing 4 mg of solid in the initial volume (4 mL) was titrated with sodium hydroxide solution (0.1 mol/L) under continuous stirring and a nitrogen atmosphere. Equivalence points were evaluated from titration curves transformed in the 1st derivation curves.


### 2.5. Sorption Experiments

Free MB dye in an aqueous solution was evaluated and measured by the double-beam UV/VIS spectrophotometer Cintra 2020 (GBC Scientific Equipment, Australia) controlled by Cintral software vs. 2.6. All adsorption experiments were realized in the Eppendorf vials (2 mL) at25±1°C. Briefly, 100 μL of GO sample (cGO=23.5mg/mL) and the calculated volume of MB stock solution in BRB buffer (MB concentration range 0.05–0.475 g/L) were pipetted into the vials, and vials were filled with BRB to a total volume 2 mL. To reach equilibrium, the Eppendorf vials were shaken for 3 hours (at 25±1°C) and subsequently centrifuged for 30 min at 14 000 RPM. Immediately, the absorbance of free MB dye was measured by UV/VIS spectroscopy at 658 nm. The concentration of free MB dye was calculated from the measured absorbance and previously obtained calibration curves. The amount of MB dye adsorbed by GO samples at equilibrium qE (mg/g) was calculated by
(1)qE=c0−cE∙Vm.Thec0andcE (mg/L) are the initial and equilibrium dye concentration, V (L) is the volume of solution, and m (g) is the mass of the sample in the solution.


### 2.6. Kinetic Study Experiment

The batch adsorption experiments in a beaker (50 mL) were used to study the adsorption kinetics. MB stock solutions in BRB (0.5 g/L, 32 mL), BRB (6 mL), and GO suspension (2 mL) were pipetted into the beaker. The initial MB concentration for the kinetic study was 400 mg/L. The beaker was placed on the magnetic stirrer. At selected times, aliquots were taken into the Eppendorf vials (2 mL). The Eppendorf vials were centrifuged for 30 min at 14 000 RPM and immediately the absorbance of free MB dye was measured by UV/VIS spectroscopy at 658 nm. The previously obtained calibration curves were used to calculate the concentration of free MB dye in the solution.


### 2.7. Zeta Potential Measurements

Zeta potential of prepared particles was monitored by electrophoretic light scattering (ELS) measurement performed on Lizesizer™ 500 (Anton Paar, Austria) coupled to a Metrohm automatic titrator with an 867 pH module and an 846 dosing interface controlled by the software Kalliope™. The temperature was 25°C, the initial pH was 11, and the final pH was 2, with a step of 0.5 modified with 0.5 M of HCl or NaOH with stabilization time of 5 min per step. The Smoluchowski approximation method was used.


## 2.1. Chemicals

All purchased chemicals were analytical reagent grade. MB (≥95%; calc. to the dried substance) was purchased from Sigma-Aldrich (Germany). The chemical reagents for preparation of Britton-Robinson buffer (BRB), i.e., CH3COOH, H3BO3, NaOH, and H3PO4 were purchased from Lach-Ner Ltd. The BRB solution was prepared according to the standard procedure published elsewhere [42]. Briefly, two solutions A and B were prepared. Solution A consists of a mixture of H3BO3, H3PO4, and CH3COOH with the concentration of each compound at 0.04 mol/L. Next, solution B was prepared by dissolving solid NaOH to obtain a solution with a concentration of 0.02 mol/L. By mixing solutions A and B, the solutions with the required pH (3.0, 7.0, and 11.0) were prepared. The stock solution of cationic MB dye (0.5 g/L) was prepared in BRB (pH=3.0, 7.0 and 11.0). KBr (FTIR grade, ≥99% trace metal basis) was used for FTIR measurements and was purchased from Sigma-Aldrich (Germany). Deionized water prepared by GORO Pharmpur reverse osmosis system (Goro, Czech Republic) was used for all the experiments. The chemical reagents for the synthesis of graphene oxide (GO), i.e., 96% H2SO4, 85% H3PO4, KMnO4, and H2O2, were obtained from commercial sources Penta, Ltd. and Lach-Ner, Ltd. (Czech Republic). The natural graphite was purchased from Koh-i-noor Grafite, Ltd. (Czech Republic).


## 2.2. Preparation of Sample

### 2.2.1. Preparation of Graphene

Graphene sheets were prepared by exfoliation of natural graphite (1 g) in a bath ultrasound reactor UIP 2000hd (2 kHz, max. 2000 W, Hielscher Ultrasonics GmbH, Germany) under a high pressure of 5 bar in ethylene glycol (100 mL) [43]. The product was purified by dialysis with Spectra/Por 3 dialysis membrane in demineralized water to stable conductivity and constant pH.


### 2.2.2. Preparation of Graphene Oxide

The dried exfoliated graphite (1 g) was mixed with H2SO4 (60 mL) and H3PO4 (10 mL) in a round-bottom flask. KMnO4 (3 g) was carefully added last. The reaction mixture was slowly heated to 40°C for 48 h. The additional KMnO4 (1.5 g) was added in smaller doses and stirred for 3 days at the same temperature. Thereafter, the mixture was left to cool down to laboratory temperature and slowly added to the ice mixture with H2O2 (200 mL) [44]. The resulting product was purified by dialysis with Spectra/Por 3 dialysis membrane in demineralized water to constant pH and stable conductivity.


## 2.2.1. Preparation of Graphene

Graphene sheets were prepared by exfoliation of natural graphite (1 g) in a bath ultrasound reactor UIP 2000hd (2 kHz, max. 2000 W, Hielscher Ultrasonics GmbH, Germany) under a high pressure of 5 bar in ethylene glycol (100 mL) [43]. The product was purified by dialysis with Spectra/Por 3 dialysis membrane in demineralized water to stable conductivity and constant pH.


## 2.2.2. Preparation of Graphene Oxide

The dried exfoliated graphite (1 g) was mixed with H2SO4 (60 mL) and H3PO4 (10 mL) in a round-bottom flask. KMnO4 (3 g) was carefully added last. The reaction mixture was slowly heated to 40°C for 48 h. The additional KMnO4 (1.5 g) was added in smaller doses and stirred for 3 days at the same temperature. Thereafter, the mixture was left to cool down to laboratory temperature and slowly added to the ice mixture with H2O2 (200 mL) [44]. The resulting product was purified by dialysis with Spectra/Por 3 dialysis membrane in demineralized water to constant pH and stable conductivity.


## 2.3. Characterization of Samples

The FTIR spectra were recorded on a diffuse reflectance spectrophotometer Nicolet 6700 IR (Thermo Scientific, USA) in transmittance mode in the 4000−400 cm−1 wavenumber range at 100 scans per spectrum with 4 cm−1 resolution. Software OMNIC 7.3 was used for raw data processing. The GO sample for FTIR was firstly lyophilized (24 h) and subsequently grounded with KBr in a ratio from 1 : 100 to 1 : 400 in an agate mortar and then in a ball mill (5 min). A hydraulic press (80 kN, 5 min) was used to prepare KBr pellets of 13 mm in diameter.Raman spectra were collected using a DXR Raman microscope (Thermo Scientific, USA) the following way: 256 two-second scans were acquired with a 532 nm laser (0.5 mW), 25μm slit under a 10× objective Olympus microscope in full range with distinction of 2 cm−1. Crystal phase analysis was performed using Bruker D2 (Germany) with the LYNXEYE 1-dimensional detector (CuKα radiation, 30 kV, 10 mA). The primary divergence slit module width of 0.6 mm, Soler Module 2.5, Airscatter screen module of 2 mm, and Ni Kbeta-filter of 0.5 mm were used in the range of 5-90°, step of 0.00805°, and time per step of 1.0 s. The XRD sample patterns after interaction with MB were processed by the following procedure. First, the GO suspension (0.1 mL) was mixed with MB solution (2.1 mL, 0.2 g/L) in 4 mL vials and were shaken for 4 h. Further, the samples were centrifuged (30 min, 10 000 RPM), washed four times with deionized water, and followed by centrifugation (shorter time). Finally, the samples were transferred to a silicon wafer, dried and measured.Morphology of the samples deposited on microscopic copper grids covered by a transparent amorphous lacey carbon film was investigated using HRTEM FEI Talos F200X (Japan) at 120 kV. The obtained micrographs and SAED patterns (Selected area electron diffraction) were processed and evaluated by the TIA (TEM Imaging & Analysis software, FEI Company). AFM measurements were performed using Bruker Dimension Microscope (Germany) in ScanAsyst-air contact mode to determine lateral size and height profile of GO sheets. An aqueous suspension was pipetted onto mica support prior the measurement.


## 2.4. Titration of GO Sample

According to our procedure published in our previous work [44], acid-base titration was used to determine the number of surface functional groups, i.e., carboxylic and hydroxyl. Titration of GO sample was realized by automatic titrator 794 Basic Titrino (Metrohm, Switzerland) with potentiometric endpoint determination. GO water suspension containing 4 mg of solid in the initial volume (4 mL) was titrated with sodium hydroxide solution (0.1 mol/L) under continuous stirring and a nitrogen atmosphere. Equivalence points were evaluated from titration curves transformed in the 1st derivation curves.


## 2.5. Sorption Experiments

Free MB dye in an aqueous solution was evaluated and measured by the double-beam UV/VIS spectrophotometer Cintra 2020 (GBC Scientific Equipment, Australia) controlled by Cintral software vs. 2.6. All adsorption experiments were realized in the Eppendorf vials (2 mL) at25±1°C. Briefly, 100 μL of GO sample (cGO=23.5mg/mL) and the calculated volume of MB stock solution in BRB buffer (MB concentration range 0.05–0.475 g/L) were pipetted into the vials, and vials were filled with BRB to a total volume 2 mL. To reach equilibrium, the Eppendorf vials were shaken for 3 hours (at 25±1°C) and subsequently centrifuged for 30 min at 14 000 RPM. Immediately, the absorbance of free MB dye was measured by UV/VIS spectroscopy at 658 nm. The concentration of free MB dye was calculated from the measured absorbance and previously obtained calibration curves. The amount of MB dye adsorbed by GO samples at equilibrium qE (mg/g) was calculated by
(1)qE=c0−cE∙Vm.Thec0andcE (mg/L) are the initial and equilibrium dye concentration, V (L) is the volume of solution, and m (g) is the mass of the sample in the solution.


## 2.6. Kinetic Study Experiment

The batch adsorption experiments in a beaker (50 mL) were used to study the adsorption kinetics. MB stock solutions in BRB (0.5 g/L, 32 mL), BRB (6 mL), and GO suspension (2 mL) were pipetted into the beaker. The initial MB concentration for the kinetic study was 400 mg/L. The beaker was placed on the magnetic stirrer. At selected times, aliquots were taken into the Eppendorf vials (2 mL). The Eppendorf vials were centrifuged for 30 min at 14 000 RPM and immediately the absorbance of free MB dye was measured by UV/VIS spectroscopy at 658 nm. The previously obtained calibration curves were used to calculate the concentration of free MB dye in the solution.


## 2.7. Zeta Potential Measurements

Zeta potential of prepared particles was monitored by electrophoretic light scattering (ELS) measurement performed on Lizesizer™ 500 (Anton Paar, Austria) coupled to a Metrohm automatic titrator with an 867 pH module and an 846 dosing interface controlled by the software Kalliope™. The temperature was 25°C, the initial pH was 11, and the final pH was 2, with a step of 0.5 modified with 0.5 M of HCl or NaOH with stabilization time of 5 min per step. The Smoluchowski approximation method was used.


## 3. Results and Discussion

### 3.1. Sample Characterization

The Raman spectrum (Figure2(a)) shows typical GO bands G (~1591 cm–1) and G′ bands (~2700 cm–1) for E2g vibrational modes, which are associated with in-plane vibration of sp2 carbon framework. The spectrum also contains D band (~1356 cm–1) describing the deformations and breathing of aromatic rings of carbon lattice [45–47]. The presence of D bands proves the presence of defects connected with oxygen-containing groups such as hydroxyl, carbonyl, carboxyl, and epoxy [48]. The distance between defects in GO structure and the number of GO layers were evaluated from ID/IG ratio, and for GO, it is standardly about 1 (532 nm laser excitation). According to ID/IG ratio, the distance between the defects varies from 1 to 3 nm [49]. The I2D/IG ratio is 0.25 (ID/IG=0.94), and it generally corresponds to the multilayer GO structure (more than 5 layers) [50]. The lower ID intensity suggests a low number of defects in the GO structure, whereas the higher IG intensity supports the unbroken sp2 carbon framework. The G bands at 1591 cm–1 indicate significant disorders in GO structure due to the rough oxidation process [51]. The G and 2D bands usually located at 1581 and 2679 cm–1 correspond to the single graphene sheets, whereas for multilayer GO sheets, the G and 2D bands shift to higher wavenumbers (1591 and 2718 cm–1). The 2D band at 2718 cm–1 serves as an indicator of graphene layer number [33, 52]. The S3 band at ~2944 cm–1 corresponds to the second-order peak derived from the combination of the D-G peak [52, 53]. The 2G band (~3174 cm–1) can be attributed to the overtone of the G band [53].Figure 2
Raman (a) and XRD pattern (b) of prepared GO sample.
(a)(b)XRD patterns of prepared graphene oxide (GO) are shown in Figure2(b). A broad and very strong peak localized at 11.7° is characteristic for interplanar d002 spacing in GO and confirmed successful synthesis of GO sheets. The d-spacing parameter 0.79 nm indicates the presence of oxygen functionality in the interlayer spacing of the graphite skeleton [54, 55]. Typically, the interlayer distance between GO sheets ranges from 0.5 to 0.9 nm and depends on the amount and the type of intercalated groups (hydroxyl, carboxyl, carbonyl, epoxy, and H2O molecules) [55].HRTEM image of the prepared GO shows monolayered sheets (Figure3(a)). In Figure 3(b), the fast Fourier transform (FFT) is shown where the points in the GO hexagonal honeycomb structure are present; i.e., it confirms that the plate is a monolayer. Figure 3(c) shows the TEM image with SEAD analysis of GO (inlet) which revealed a spot pattern, which proves single-layered GO. From the TEM image (Figure 3(c)), the presence of the monolayer is not clearly visible; therefore, the data from the AFM are present. GO AFM image shows large differences in the lateral size of GO sheets with a height profile of 1 nm in all measured cases (Figure 3(d)).Figure 3
HRTEM image (a), FFT analysis (b), TEM image with SAED patterns (c), and AFM image with height profile (d) of GO sample.
(a)(b)(c)(d)


### 3.2. Evaluation of Surface Hydroxyl Groups

The potentiometric titration was used to evaluate surface functional groups. The measured titration curve with the 1st derivation is shown in Figure4(a). Two equivalence points (EP1 and EP2) were present on the titration curve. According to our previous research, the EP1 corresponds to the NaOH consumed to neutralize the carboxylic groups type (q1). In contrast, the difference between (EP2–EP1) and the NaOH consumed for the neutralization of hydroxyl type groups (q2) [44]. The determined number of carboxylic group type (q1) was 1.10±0.04mmol/g, and that of hydroxyl group type (q2) was 0.96±0.02mmol/g, respectively. A slightly higher number of carboxylic functional groups were observed in comparison with the hydroxyl groups.Figure 4
(a) Titration curve with the 1st derivative curve of the prepared GO sample with two distinct equivalent points (EP1 and EP2). (b) Curve corresponding to the total concentration of protons consumed in the titration process (TOTH). The inset plot present pH corresponds to the point of zero charge (PZC).
(a)(b)The measured titration curve was transformed into the curve corresponding to the total concentration of protons consumed in the titration process (TOTH, see Figure4(b)) and can be calculated by [14, 56]
(2)TOTH=−VNaOH−VEP1∙cNaOHmGO.In Equation (2), cNaOHandVNaOH represent the analytical concentration of NaOH and the volume of NaOH added at different titration points, respectively. VEP1 corresponds to the volume of the first equivalent point, and mGO is the weight of GO used in the titration.The amphoteric behavior of GO surface groups provides the ability of the GO material to become positively or negatively charged depending on solution pH. The hydroxyl and carboxyl groups exhibit amphoteric behavior. The TOTH curve in Figure4(b) shows the ability to release or associate protons per solid weight into or from the solution. The positive TOTH values represent proton association and can be described by Equation (3). In contrast, negative values represent the opposite process (Equation (4)). The GO surface becomes positively charged at low pH values due to the proton association (TOTH positive values). In contrast, the GO surface becomes negatively charged at high pH values due to the proton release (TOTH negative values) [57, 58].
(3)GO−COOH+H+⇆GO−COOH2+GO−OH+H+⇆GO−OH2+(4)GO−COOH⇆GO−COO−+H+GO−OH⇆GO−OH−+H+The TOTH curve (Figure4(b)) shows that the GO surface was positively charged below pH<4.3, and at pH>4.3, the GO surface was negatively charged. The TOTH curve analysis provided that the PZC corresponds to pHPZC=4.3, as demonstrated [14, 56, 59].The high degree stability of GO nanosheets was confirmed by zeta potential measurements (ζ=−36.7mV). Standardly, the nanosheets with high degrees of stability have zeta potential values greater than ±30 mV [60]. Figure 5 represents the GO zeta potential change with pH and the values are negative at all pH values studied. The data in Figure 5 suggest that the GO oxygen species are deprotonated in the whole pH range studied and the data agree with other GOs and carbon-based materials [37, 61–63]. The negative zeta potential values in acid pH showed that GO forms stable colloids due to the ionized oxygen functional groups (-COOH) electrostatic repulsion [37, 62], which helps the adsorption of positively charged MB dye. The discrepancies in pH(PZC) evaluated from TOTH curves and zeta potential measurement can be ascribed to the (a) differences in the evaluation methods used and (b) GO ageing process. The GO ageing is followed by a spontaneous chemical reaction, especially in epoxy groups deprivation and hydroxyl group enrichment [64]. Besides, the GO degradation pathway leads to humic acid-like structures and mainly occurs in the water environment [65, 66].Figure 5
GO zeta potential change with pH.The isoelectric point values (IEP) represent external surface charges of nanosheets in solution, at which the zeta potential of the surface or molecule is equal to zero. The IEP value indicates the pH at which the GO nanosheets do not move in an electric field [67]. Conversely, pH(PZC) is connected to GO nanosheets’ total net surface charge distributions (internal and external). The pH(PZC) values are defined as the negative logarithm of the activity of the potential determining ions at which the net surface charge distribution is equal σOH2+=σOH−, as well as the surface concentrations MO−=MOH2+ [68–70]. The pH(IEP) and pH(PZC) values are commonly identical if no other reaction or adsorption process occurs [69]. The discrepancies in IEP and pH(PZC) indicate some specific absorption of the bulk electrolyte. The shift to lower or higher IEP values would be caused mainly by some specific adsorption of cations or anions from the background electrolyte used in zeta potential measurement [71, 72]. On the other hand, the acid-base titration is based on the transfer of OH− and H3O+ ions between the GO ionizable surface groups, which is the primary process involved in acid-base titration. In contrast, zeta potential (electrophoretic mobility) corresponds to the external surface charge potential. According to Corapcioglu and Huang [73], high pH(PZC) values obtained by acid-base titration are characteristic of reduced surfaces. Conversely, the low pH(PZC) values obtained by zeta potential are typical of oxidized surfaces. In addition, Corapcioglu and Huang [73] mentioned that zeta potential measurements provide false information and acid-base titration provides better quantitative information about the surface acidity of carbon-based materials. The differences in pH(PZC) and IEP indicate higher heterogeneity of carbon-based materials and can be connected with the GO oxidation process and the degree of oxidation [67, 74].According to Menéndez et al. [67], the relatively low value of pH(PZC) showed the high acidity of GO material and, thus, an increased number of oxygen-containing surface groups with an acidic character. Acid-base titration as well as the zeta potential methods belong to the powerful techniques for GO surface characterization.


### 3.3. Adsorption Isotherm Data

The adsorption isotherms describe the relationship between the adsorbent and adsorbate in the equilibrium state. The relationship between the solution dye concentration and equilibrium state has been described by the most widely used Langmuir, Freundlich, Langmuir-Freundlich, and Temkin isotherms [4, 75, 76]. The experimental data for MB adsorption in an aqueous solution (25±1°C) were evaluated using all these four types of isotherms. In Equations (5), (6), (7), and (8), cE is the equilibrium dye concentration (mg/L), qE is the equilibrium amount of cationic dye adsorbed per unit weight of adsorbent (mg/g), qM is the maximum adsorption capacity (mg/g), KL is the Langmuir adsorption constant (L/g), KF is the Freundlich isotherm constant (L/g), nF is the adsorption intensity, KLF the equilibrium constant for heterogeneous solid (L/g), and nLF is the heterogeneity parameter [77]. In the Temkin isotherm model (Equation (8)), AT is Temkin parameter related to the equilibrium binding constant (L/g); BT is the Temkin constant related to the adsorption heat (J/mol), and it is defined by the expression BT=RT/bT, where R is the universal gas constant (8.314 J/K mol), T is the thermodynamic temperature (K), and bT is the Temkin constant [15, 76, 78].Monolayer adsorption on a homogeneous surface can be described by the Langmuir (L) adsorption isotherm. The Langmuir isotherm assumes the surface with a finite number of definite localized places which are identical and equivalent [13, 79]. The Langmuir adsorption isotherm in non-linear form can be expressed by
(5)qE=qM∙KL∙cE1+KL∙cE.The Freundlich (F) adsorption isotherm is frequently used to describe the non-ideal and reversible adsorption at heterogeneous surfaces and to describe the adsorption process of organic compounds on carbon-based materials or molecular sieves [79, 80]. The formation of a monolayer is not limiting for this isotherm. The Freundlich isotherm can be expressed in non-linear form by
(6)qE=KF∙cE1/nF.The Langmuir-Freundlich (LF) isotherm is a useful and flexible mathematical model, combining the advantages and behaviour of Freundlich and Langmuir isotherm [81]. The main advantage of LF isotherm is that, at low adsorbate concentration, it reduces to Freundlich isotherm. In contrast, at high adsorbate concentrations, it behaves as the Langmuir isotherm with monolayer adsorption capacity [79, 82]. The Langmuir-Freundlich isotherm can be expressed in a nonlinear form by
(7)qE=qM∙KLF∙cE1/nLF1+KLF∙cE1/nLF.In addition, for the evaluation of some indirect GO-MB interactions, the Temkin isotherm was used. This model suggested that the adsorption heat of all the molecules in the layer linearly decreases with coverage [78]. The Temkin isotherm in a nonlinear form can be expressed by
(8)qE=BT∙lnAT∙cE.MB sorption experiments were performed in acidic, neutral, and basic pH values (3.0; 7.0; 11.0). The pH effect on the MB sorption process and adsorption isotherm data are shown in Figure6, and isotherm parameters are presented in Table 1.Figure 6
Fits of the Freundlich, Langmuir, Langmuir-Freundlich, and Temkin isotherms for the adsorption of MB on GO sample atpH=3.0a,pH=7.0bandpH=11.0c. 2.35 mg of GO; i.e., 100 μL of GO suspension, MB initial concentration range: 0.05–0.475 g/L at 298 K.
(a)(b)(c)Table 1
Freundlich, Langmuir, Langmuir-Freundlich, and Temkin model constants and correlation coefficients for the adsorption of MB by GO sample.
pHFreundlichLangmuirLangmuir-FreundlichTemkinKF (L/mg)nFR2KL (L/mg)qM (mg/g)R2KLF (L/mg)qM (mg/g)nLFR2AT (L/mg)BTR2bT (J/mol)3.00.1541.490.97700.476487.70.99900.560440.50.9400.99945.9592.30.991826.97.00.1342.580.92110.389445.90.99000.500a391.10.7730.98583.9194.10.980926.311.00.0791.130.94150.0332441.10.95300.050a803.70.5600.98420.83280.10.97658.85aFixed parameters.In comparison with the other experiments on GO carried out by Li et al. [12] (2 times) and Ramesha et al. [13] (30 times) at pH=3.0andpH=7.0, our prepared GO sample has shown higher MB sorption capacity. In contrast, at pH=11.0, the qM is 10 times and 140 times higher, respectively. The higher sorption capacity could probably be ascribed to the different GO synthesis procedures and the number of surface functional groups. However, GO oxidation degree strongly affects adsorption capacity to MB dye [37, 83], heavy metals (Co2+) [84], or metalloid (AsO33-) [85]. According to Yan et al. [37], the GO samples in low oxidation degree exhibit 10 times lower qM values for MB than highly oxidized samples. Table 2 presents an adsorption capacity comparison between GO, other adsorbents, and GO/composite materials towards MB dye. The table shows the experimental conditions, maximum adsorption capacity, and mathematical model used for data fitting.Table 2
Comparison of GO adsorption capacity towards MB with other values from the literature.
AdsorbentqM (mg/g)Mathematical model∗pHTemperature (K)Refs.GO440.5LF3.0298This workGO445.9L7.0298This workGO803.7LF11.0298This workGO476.2LNA293[38]GO144.9L5.4298[39]GO243.9L6.0298[12]GO (various oxidation degrees)40.6 – 570.4L7.0298[37]Active carbon270.3L6.0298[12]GO/calcium alginate181.8L5.4298[39]GO17.3LNANA[13]GO/polyaniline6.7LNA298[86]GO/magnetic cellulose composite70.0LNA298[87]Magnetic multi/wall carbon nanotube11.86L7.0298[88]Activated carbon375L4 - 5298[89]Modified expanded graphite powder0.0077L7.0293[90]∗LF: Langmuir-Freundlich mathematical model; L: Langmuir mathematical model.The data summarized in Table2 show significant differences in qM values and comparison of laboratory conditions for various GOs, active carbons, carbon nanotubes, and GO/composites from the literature. Nevertheless, our GO sample under various experimental conditions showed the highest adsorption capacity towards MB dye. The GO/composite materials did not show such high qM values as may be expected. However, the lower absorption capacity of composites does not mean that they are inefficient materials if these composites show, e.g., photocatalytic activity, as demonstrated by Shahabuddin et al. [26, 27, 29]. The MB removal efficiency and lower qM should probably be connected with another synthesis procedure (Hummer’s, Brodie’s), the number of surface hydroxyl groups, pH(PZC), defects in GO honeycomb structure, and GO oxidation degree [37, 48, 56, 91]. Similar qM values were found for GO by Chia et al. [38]; compared to other GO materials [12, 13, 39] and GO/composites [39, 86, 87], our GO material showed at least two times higher, however, even fifty times higher qM values. Comparable qM values can be found for the various activated carbons [12, 16, 89] and GO [37, 38] that exhibit a relatively large surface area as well as the activation/synthesis procedure, which may play a crucial role in MB removal.The sorption process is describable at different pH values by various mathematical models. It shows the variability of the GO behavior and its ability to eliminate MB dye from aqueous solutions at different pH values. The calculated parameters (Table1) have shown differences in MB sorption depending on solution pH. In acidic (pH=3.0) and basic (pH=11.0) environment, the sorption process can be described by the Langmuir-Freundlich mathematical model (R2=0.9994;R2=0.9842) with maximum adsorption capacity of 440.5 mg/g (pH=3.0) and 803.7 mg/g (pH=11.0), respectively. Conversely, in neutral pH (pH=7.0), the behavior can be described by Langmuir mathematical model (R2=0.9900) with a maximum adsorption capacity of 445.9 mg/g.The Langmuir, Langmuir-Freundlich, and Temkin models appear to be the most suitable for the description of the MB sorption by GO under our conditions. The mathematical models (L and LF) suggested the creation of MB monolayer with GO active sites, which are identical and homogeneously distributed on the GO surface [16, 87]. Conversely, the Temkin mathematical model was used to evaluate the indirect MB-GO interaction. According to R2 values, the Temkin model can be evidently also used to describe MB on GO. The data obtained by a nonlinear fitting (Temkin model) suggested the presence of various indirect MB interactions with GO surface. Those indirect interactions probably come from the MB interactions with functional groups and GO carbon honeycomb structure (see Figure 7). The Temkin equilibrium binding constant AT decreases with increasing pH to the lowest value of 0.83 L/mg at pH 11.0. The Temkin constant bT related to the sorption heat decreased with increasing pH to the lowest value of 8.85 J/mol at pH 11.0 (Table 1). The positive Temkin constant bT values (for all pH) indicate that the MB adsorption onto GO is an exothermic reaction. With the increasing pH, the adsorption reaction is less exothermic.Figure 7
Potential interactions of MB dye with GO surface.In contrast, the Freundlich mathematical model is not suitable for the description of MB adsorption concerningR2. According to the calculated Langmuir constant, the affinity of MB sorption decreases at higher pH values.The higher sorption ability of the GO sample is dependent on the pH. It can be most likely explained by the deprotonation of the GO surface functional groups, which support MB interaction with negatively charged GO surface [2, 92]. According to data published elsewhere, the GO materials with rich oxygen-containing functional groups showed and played an essential role in the increased adsorption capacity to radioactive iodine [93], arsenic(III) [85], cadmium [94], and MB [48, 91]. Oxygen-containing functional groups enable the formation of covalent bonding, electrostatic attraction, and cation exchange with MB dye. The MB adsorption mechanism can be attributed to (a) electrostatic/ionic interactions of positively charged MB structure with negatively charged –OH, carboxyl, carbonyl, and epoxy groups on the basal plane and edges of GO and (b) π-π interaction and conjugation based on the electron donor-acceptor interaction with honeycomb GO structure (see Figure 7). The adsorption mechanism involves mainly the interaction of π electrons in C=C bond in MB structure with the π electrons in the GO honeycomb structure [48, 91, 95].Maximum adsorption capacity (L and LF) supports the above-mentioned effect of surface groups. The pH value greatly affects MB sorption, as demonstrated [2, 13], but contradicts the results of Liu et al. [92]. Adsorption efficiency for MB removal (at measured pH) achieved 98.2% (pH=3.0), 99.2% (pH=7.0), and 99.0% (pH=11.0) for initial MB concentration of 400 mg/L. The adsorption efficiencies are similar for carbon nanotubes (<98.8%) [88], activated carbon (90%) [16], and cellulose/GO composite (96.7%) [87], but not so high for GO/calcium alginate composite (83.7%) [39] and carbon nanotubes (≈ 75%) [12] in comparison with data published elsewhere.A heterogeneity parameter (nF>1) shows that MB sorption is the physical process at all pH values. The value (1/nF) suggested the standard MB sorption process. According to our results (data not shown), calculated values (nF>1;1/nF<1) show that the Freundlich model is suitable for the description of MB sorption onto GO sample (at measured pH values) [79], despite the correlation coefficient.Besides that, we calculated the separation factor (RL, Equation (9)) from Langmuir isotherm (data not shown). The RL value was used for evaluation and confirmation, whether the sorption is unfavorable (RL>1), linear (RL=1), or favorable (0<RL<1).
(9)RL=11+KL∙cE.Calculated values (0.05–0.475 g/L MB concentration range) have shown a favorable MB sorption process onto the GO sample under our experimental conditions. As shown in Figure8, RL value decreases with increasing initial concentration (c0) (at measured pH values), suggesting the MB sorption is more favorable at a higher MB concentration [16]. At pH 3.0 and 7.0, the dependence RL on c0 has shown a similar trend. Conversely, at pH 11.0, the decline is not so steep; it is evident that the MB adsorption process also becomes more favorable at a relatively high MB concentration.Figure 8
Separation factor value (RL) depending on the MB initial concentration (c0). MB initial concentration range of 0.05–0.475 g/L at 298 K.


### 3.4. Kinetics Studies

To evaluate the effectiveness of the pH solution on the MB adsorption, the plot in Figure9 shows the amount of MB adsorbed qT at time t. The initial adsorption stage is rapid for pH 7.0 and 11.0, which could be ascribed to partly and fully deprotonated GO surface groups. Conversely, the initial adsorption stage at pH 3.0 was relatively slow, and the maximum was achieved after 180 min. The slow initial adsorption stage at pH 3.0 (Figure 9) can be attributed to the complicated adsorption process, which could be connected to the mutual competition of MB dye and other ions, mainly with protons, in solution with positively charged GO surface groups. The π-π interactions of MB with the GO honeycomb structure are probably the primary type of MB interaction with the GO structure [2, 12]. GO sheets at lower pH values aggregated together and could play a role in the lower adsorption capacity and slow adsorption process. Negatively charged GO sheets and the electrostatic repulsion between sheets with increasing solution pH could be helpful for MB adsorption [86, 96], as is evident from our measured data.Figure 9
The adsorption kinetics of MB atpH=3.0 (■), pH=7.0 (●), and pH=11.0 (▲). Initial MB concentration of 0.5 g/L and 2 mL of GO suspension, i.e., 47 mg of GO at 298 K.To investigate the adsorption kinetics of MB dye on the GO, the pseudosecond-order kinetics model (10) and pseudofirst-order model (11) were tested. The pseudosecond-order and pseudofirst-order kinetics model in a nonlinear form can be expressed by [12, 97]
(10)qt=qE2∙k2∙tqE∙k2∙t+1,(11)qt=qE∙1−e−k1∙t,where qEandqt are the adsorption capacity (mg/g) at equilibrium and at time t (min), respectively, and k2 (min g/mg) and k1 (min–1) are the rate adsorption constants. The parameters of pseudo-second order can be calculated from the plot of (t/qt) vs. t (plot not shown). The results are presented in Table 3. The results showed that the pseudo-second-order model was better than the pseudo-first-order model for MB adsorption on the GO, which is in agreement with other literatures [92, 98]. Conversely, the pseudofirst order is partly suitable for the description of MB adsorption only in acidic pH, but unsuitable at neutral and basic pH, as evident from the correlation coefficient. Moreover, the rate constant of the adsorption increases with increasing pH, suggesting faster kinetic of MB adsorption at the higher pH solution.Table 3
The adsorption kinetics parameters for MB adsorption on the GO.
pHPseudosecond orderPseudofirst orderqE (mg/g)k2 (min g/mg)R2qE (mg/g)k1 (min–1)R23.0336.40.0801.0000336.21.100.80347.0336.90.1011.0000337.13.9×104−0.142911.0336.20.1061.0000336.31.3×106−0.1667The mutual correlation of measured and calculated parameters is complicated. Thus, we tried a correlation between the maximum adsorption capacity (qM), a model solution pH, and the adsorption rate constant (k2) (see Figure 10). The main effect of increasing pH is evident in the adsorption rate constant (pH=3 vs. pH=11), and the change in maximum adsorption capacity (pH=3 and pH=7 vs. pH=11) is significant, as shown in Figure 10. Basic solution pH values mainly affect qM values, and the increase in adsorption rate constant is insignificant. The k2 value variates from 0.08 to 0.106 min g/min for pH=3andpH=11, respectively.Figure 10
Mutual correlation of maximum adsorption capacityqM vs. model solution pH (●) and adsorption rate constant k2vs.qM (■) for MB removal by GO.


### 3.5. Characterization of Samples before and after Sorption of MB by FTIR

The FTIR spectra of prepared GO sample are shown in Figure11. The most intensive bands are localized in the 3800–3000 cm–1 region, corresponding to the stretching vibration of O—H bonds in hydroxyl from carboxyl groups and residual water intercalated in the GO sheets. The further bands were localized in the 2000–1000 cm–1 fingerprint region. The vibration band found at 1732 cm–1 is the characteristic of stretching vibration of C=O bonds in carboxylic groups [99–101]. The C=C stretching vibration (for carbon with sp2 hybridization) in GO was localized at 1625 cm–1 [56, 100, 101]. The bands corresponding to the bending and stretching vibration of alkoxide (C—O) and epoxides (C—O—C) functional groups were found at 1226 and 1078 cm–1 [99–101].Figure 11
(a) FTIR spectra of prepared GO sample, MB cationic dye, and GO with adsorbed MB dye, details of the fingerprint region on (b).
(a)(b)The FTIR spectra of MB dye are shown in Figure11. The fundamental bands are localized in the 1800–600 cm–1 region. The stretching vibration bands corresponding to the Chet=N+(CH3)2 bonds were found at 1648 cm–1. The intensive stretching vibration of C=C and C=N bonds is localized at 1600 cm–1. The stretching vibration of C—N and C—C bond of heterocycle was found at 1540 and 1225 cm–1 and the deformation vibration of C—N bond of heterocycle at 1143 cm–1. The C=S+ stretching vibration of MB heterocycle is seen at 1491 and 1355 cm–1. The next bands localized at 1446 and 1398 cm–1 can be ascribed to asymmetric and symmetric deformation vibration of C—H bond in N(CH3)2. The stretching vibration of C—N in N—CH3 is found at 1340 cm–1 and deformation and bending out-of-plane vibration of C—H at 1251, 1225, and 1189 cm–1. Finally, the C—S—C bond vibration of MB heterocycle is located at 1069 cm–1. All these vibrations correspond with the literature [102–104].The FTIR spectra shown in Figure11 correspond to the GO after sorption of MB dye. It should be mentioned that the intensity of characteristic GO bands decreased, particularly the intensity of the characteristic stretching vibration of (O—H) bonds in 3800–3000 cm–1 region. The vibration band at 1730 cm–1 corresponding to C=O bonds in carboxylic groups nearly disappeared, the band at 1625 cm–1 slightly shifted to 1638 cm–1, and the intensity also decreased for C=C stretching vibration. The most intensive bands of MB were also found in the sample of GO after MB adsorption as 1491, 1398, 1355, and 1340 cm–1. Only two vibration bands were slightly shifted at 1143 and 1069 cm–1 to 1149 and 1074 cm–1, corresponding to deformation vibration of C—N and stretching vibration of C—S—C of heterocycle of MB (Figure 11). The attenuation of the GO bands could be ascribed to covering of GO sheets by MB and just slight shifting tends to the suggestion that most probably π-π interaction coming from aromatic rings of MB and GO is present [16, 87].


### 3.6. Characterization of Samples before and after Sorption of MB by Powder XRD

The mechanism of MB adsorption was studied by Bujdák et al. [105], where orientations of MB cation were compared with experimental data. The calculated height of the MB cation is 0.77 nm. The arrangements of MB cation as intercalated dimer and monomer were determined and compared with the results obtained by Bujdák et al. [105]. The interlayer space was found to be at the range 7.2°–7.7° 2Θ corresponding to ~1.15-1.25 nm and monomeric arrangement of MB cations for all samples after sorption of MB at pH 3, 7, and 11 (Figure 12). The zones with no occupancy by MB cation were confirmed by the presence of large diffraction line at the range 10.9°–13.5° 2Θ (~0.81-0.66 nm). So, the interlayer space decreases significantly by the absence of MB cation.Figure 12
XRD patterns of GO before and after sorption MB at pH 3, pH 7, and pH 11.


## 3.1. Sample Characterization

The Raman spectrum (Figure2(a)) shows typical GO bands G (~1591 cm–1) and G′ bands (~2700 cm–1) for E2g vibrational modes, which are associated with in-plane vibration of sp2 carbon framework. The spectrum also contains D band (~1356 cm–1) describing the deformations and breathing of aromatic rings of carbon lattice [45–47]. The presence of D bands proves the presence of defects connected with oxygen-containing groups such as hydroxyl, carbonyl, carboxyl, and epoxy [48]. The distance between defects in GO structure and the number of GO layers were evaluated from ID/IG ratio, and for GO, it is standardly about 1 (532 nm laser excitation). According to ID/IG ratio, the distance between the defects varies from 1 to 3 nm [49]. The I2D/IG ratio is 0.25 (ID/IG=0.94), and it generally corresponds to the multilayer GO structure (more than 5 layers) [50]. The lower ID intensity suggests a low number of defects in the GO structure, whereas the higher IG intensity supports the unbroken sp2 carbon framework. The G bands at 1591 cm–1 indicate significant disorders in GO structure due to the rough oxidation process [51]. The G and 2D bands usually located at 1581 and 2679 cm–1 correspond to the single graphene sheets, whereas for multilayer GO sheets, the G and 2D bands shift to higher wavenumbers (1591 and 2718 cm–1). The 2D band at 2718 cm–1 serves as an indicator of graphene layer number [33, 52]. The S3 band at ~2944 cm–1 corresponds to the second-order peak derived from the combination of the D-G peak [52, 53]. The 2G band (~3174 cm–1) can be attributed to the overtone of the G band [53].Figure 2
Raman (a) and XRD pattern (b) of prepared GO sample.
(a)(b)XRD patterns of prepared graphene oxide (GO) are shown in Figure2(b). A broad and very strong peak localized at 11.7° is characteristic for interplanar d002 spacing in GO and confirmed successful synthesis of GO sheets. The d-spacing parameter 0.79 nm indicates the presence of oxygen functionality in the interlayer spacing of the graphite skeleton [54, 55]. Typically, the interlayer distance between GO sheets ranges from 0.5 to 0.9 nm and depends on the amount and the type of intercalated groups (hydroxyl, carboxyl, carbonyl, epoxy, and H2O molecules) [55].HRTEM image of the prepared GO shows monolayered sheets (Figure3(a)). In Figure 3(b), the fast Fourier transform (FFT) is shown where the points in the GO hexagonal honeycomb structure are present; i.e., it confirms that the plate is a monolayer. Figure 3(c) shows the TEM image with SEAD analysis of GO (inlet) which revealed a spot pattern, which proves single-layered GO. From the TEM image (Figure 3(c)), the presence of the monolayer is not clearly visible; therefore, the data from the AFM are present. GO AFM image shows large differences in the lateral size of GO sheets with a height profile of 1 nm in all measured cases (Figure 3(d)).Figure 3
HRTEM image (a), FFT analysis (b), TEM image with SAED patterns (c), and AFM image with height profile (d) of GO sample.
(a)(b)(c)(d)


## 3.2. Evaluation of Surface Hydroxyl Groups

The potentiometric titration was used to evaluate surface functional groups. The measured titration curve with the 1st derivation is shown in Figure4(a). Two equivalence points (EP1 and EP2) were present on the titration curve. According to our previous research, the EP1 corresponds to the NaOH consumed to neutralize the carboxylic groups type (q1). In contrast, the difference between (EP2–EP1) and the NaOH consumed for the neutralization of hydroxyl type groups (q2) [44]. The determined number of carboxylic group type (q1) was 1.10±0.04mmol/g, and that of hydroxyl group type (q2) was 0.96±0.02mmol/g, respectively. A slightly higher number of carboxylic functional groups were observed in comparison with the hydroxyl groups.Figure 4
(a) Titration curve with the 1st derivative curve of the prepared GO sample with two distinct equivalent points (EP1 and EP2). (b) Curve corresponding to the total concentration of protons consumed in the titration process (TOTH). The inset plot present pH corresponds to the point of zero charge (PZC).
(a)(b)The measured titration curve was transformed into the curve corresponding to the total concentration of protons consumed in the titration process (TOTH, see Figure4(b)) and can be calculated by [14, 56]
(2)TOTH=−VNaOH−VEP1∙cNaOHmGO.In Equation (2), cNaOHandVNaOH represent the analytical concentration of NaOH and the volume of NaOH added at different titration points, respectively. VEP1 corresponds to the volume of the first equivalent point, and mGO is the weight of GO used in the titration.The amphoteric behavior of GO surface groups provides the ability of the GO material to become positively or negatively charged depending on solution pH. The hydroxyl and carboxyl groups exhibit amphoteric behavior. The TOTH curve in Figure4(b) shows the ability to release or associate protons per solid weight into or from the solution. The positive TOTH values represent proton association and can be described by Equation (3). In contrast, negative values represent the opposite process (Equation (4)). The GO surface becomes positively charged at low pH values due to the proton association (TOTH positive values). In contrast, the GO surface becomes negatively charged at high pH values due to the proton release (TOTH negative values) [57, 58].
(3)GO−COOH+H+⇆GO−COOH2+GO−OH+H+⇆GO−OH2+(4)GO−COOH⇆GO−COO−+H+GO−OH⇆GO−OH−+H+The TOTH curve (Figure4(b)) shows that the GO surface was positively charged below pH<4.3, and at pH>4.3, the GO surface was negatively charged. The TOTH curve analysis provided that the PZC corresponds to pHPZC=4.3, as demonstrated [14, 56, 59].The high degree stability of GO nanosheets was confirmed by zeta potential measurements (ζ=−36.7mV). Standardly, the nanosheets with high degrees of stability have zeta potential values greater than ±30 mV [60]. Figure 5 represents the GO zeta potential change with pH and the values are negative at all pH values studied. The data in Figure 5 suggest that the GO oxygen species are deprotonated in the whole pH range studied and the data agree with other GOs and carbon-based materials [37, 61–63]. The negative zeta potential values in acid pH showed that GO forms stable colloids due to the ionized oxygen functional groups (-COOH) electrostatic repulsion [37, 62], which helps the adsorption of positively charged MB dye. The discrepancies in pH(PZC) evaluated from TOTH curves and zeta potential measurement can be ascribed to the (a) differences in the evaluation methods used and (b) GO ageing process. The GO ageing is followed by a spontaneous chemical reaction, especially in epoxy groups deprivation and hydroxyl group enrichment [64]. Besides, the GO degradation pathway leads to humic acid-like structures and mainly occurs in the water environment [65, 66].Figure 5
GO zeta potential change with pH.The isoelectric point values (IEP) represent external surface charges of nanosheets in solution, at which the zeta potential of the surface or molecule is equal to zero. The IEP value indicates the pH at which the GO nanosheets do not move in an electric field [67]. Conversely, pH(PZC) is connected to GO nanosheets’ total net surface charge distributions (internal and external). The pH(PZC) values are defined as the negative logarithm of the activity of the potential determining ions at which the net surface charge distribution is equal σOH2+=σOH−, as well as the surface concentrations MO−=MOH2+ [68–70]. The pH(IEP) and pH(PZC) values are commonly identical if no other reaction or adsorption process occurs [69]. The discrepancies in IEP and pH(PZC) indicate some specific absorption of the bulk electrolyte. The shift to lower or higher IEP values would be caused mainly by some specific adsorption of cations or anions from the background electrolyte used in zeta potential measurement [71, 72]. On the other hand, the acid-base titration is based on the transfer of OH− and H3O+ ions between the GO ionizable surface groups, which is the primary process involved in acid-base titration. In contrast, zeta potential (electrophoretic mobility) corresponds to the external surface charge potential. According to Corapcioglu and Huang [73], high pH(PZC) values obtained by acid-base titration are characteristic of reduced surfaces. Conversely, the low pH(PZC) values obtained by zeta potential are typical of oxidized surfaces. In addition, Corapcioglu and Huang [73] mentioned that zeta potential measurements provide false information and acid-base titration provides better quantitative information about the surface acidity of carbon-based materials. The differences in pH(PZC) and IEP indicate higher heterogeneity of carbon-based materials and can be connected with the GO oxidation process and the degree of oxidation [67, 74].According to Menéndez et al. [67], the relatively low value of pH(PZC) showed the high acidity of GO material and, thus, an increased number of oxygen-containing surface groups with an acidic character. Acid-base titration as well as the zeta potential methods belong to the powerful techniques for GO surface characterization.


## 3.3. Adsorption Isotherm Data

The adsorption isotherms describe the relationship between the adsorbent and adsorbate in the equilibrium state. The relationship between the solution dye concentration and equilibrium state has been described by the most widely used Langmuir, Freundlich, Langmuir-Freundlich, and Temkin isotherms [4, 75, 76]. The experimental data for MB adsorption in an aqueous solution (25±1°C) were evaluated using all these four types of isotherms. In Equations (5), (6), (7), and (8), cE is the equilibrium dye concentration (mg/L), qE is the equilibrium amount of cationic dye adsorbed per unit weight of adsorbent (mg/g), qM is the maximum adsorption capacity (mg/g), KL is the Langmuir adsorption constant (L/g), KF is the Freundlich isotherm constant (L/g), nF is the adsorption intensity, KLF the equilibrium constant for heterogeneous solid (L/g), and nLF is the heterogeneity parameter [77]. In the Temkin isotherm model (Equation (8)), AT is Temkin parameter related to the equilibrium binding constant (L/g); BT is the Temkin constant related to the adsorption heat (J/mol), and it is defined by the expression BT=RT/bT, where R is the universal gas constant (8.314 J/K mol), T is the thermodynamic temperature (K), and bT is the Temkin constant [15, 76, 78].Monolayer adsorption on a homogeneous surface can be described by the Langmuir (L) adsorption isotherm. The Langmuir isotherm assumes the surface with a finite number of definite localized places which are identical and equivalent [13, 79]. The Langmuir adsorption isotherm in non-linear form can be expressed by
(5)qE=qM∙KL∙cE1+KL∙cE.The Freundlich (F) adsorption isotherm is frequently used to describe the non-ideal and reversible adsorption at heterogeneous surfaces and to describe the adsorption process of organic compounds on carbon-based materials or molecular sieves [79, 80]. The formation of a monolayer is not limiting for this isotherm. The Freundlich isotherm can be expressed in non-linear form by
(6)qE=KF∙cE1/nF.The Langmuir-Freundlich (LF) isotherm is a useful and flexible mathematical model, combining the advantages and behaviour of Freundlich and Langmuir isotherm [81]. The main advantage of LF isotherm is that, at low adsorbate concentration, it reduces to Freundlich isotherm. In contrast, at high adsorbate concentrations, it behaves as the Langmuir isotherm with monolayer adsorption capacity [79, 82]. The Langmuir-Freundlich isotherm can be expressed in a nonlinear form by
(7)qE=qM∙KLF∙cE1/nLF1+KLF∙cE1/nLF.In addition, for the evaluation of some indirect GO-MB interactions, the Temkin isotherm was used. This model suggested that the adsorption heat of all the molecules in the layer linearly decreases with coverage [78]. The Temkin isotherm in a nonlinear form can be expressed by
(8)qE=BT∙lnAT∙cE.MB sorption experiments were performed in acidic, neutral, and basic pH values (3.0; 7.0; 11.0). The pH effect on the MB sorption process and adsorption isotherm data are shown in Figure6, and isotherm parameters are presented in Table 1.Figure 6
Fits of the Freundlich, Langmuir, Langmuir-Freundlich, and Temkin isotherms for the adsorption of MB on GO sample atpH=3.0a,pH=7.0bandpH=11.0c. 2.35 mg of GO; i.e., 100 μL of GO suspension, MB initial concentration range: 0.05–0.475 g/L at 298 K.
(a)(b)(c)Table 1
Freundlich, Langmuir, Langmuir-Freundlich, and Temkin model constants and correlation coefficients for the adsorption of MB by GO sample.
pHFreundlichLangmuirLangmuir-FreundlichTemkinKF (L/mg)nFR2KL (L/mg)qM (mg/g)R2KLF (L/mg)qM (mg/g)nLFR2AT (L/mg)BTR2bT (J/mol)3.00.1541.490.97700.476487.70.99900.560440.50.9400.99945.9592.30.991826.97.00.1342.580.92110.389445.90.99000.500a391.10.7730.98583.9194.10.980926.311.00.0791.130.94150.0332441.10.95300.050a803.70.5600.98420.83280.10.97658.85aFixed parameters.In comparison with the other experiments on GO carried out by Li et al. [12] (2 times) and Ramesha et al. [13] (30 times) at pH=3.0andpH=7.0, our prepared GO sample has shown higher MB sorption capacity. In contrast, at pH=11.0, the qM is 10 times and 140 times higher, respectively. The higher sorption capacity could probably be ascribed to the different GO synthesis procedures and the number of surface functional groups. However, GO oxidation degree strongly affects adsorption capacity to MB dye [37, 83], heavy metals (Co2+) [84], or metalloid (AsO33-) [85]. According to Yan et al. [37], the GO samples in low oxidation degree exhibit 10 times lower qM values for MB than highly oxidized samples. Table 2 presents an adsorption capacity comparison between GO, other adsorbents, and GO/composite materials towards MB dye. The table shows the experimental conditions, maximum adsorption capacity, and mathematical model used for data fitting.Table 2
Comparison of GO adsorption capacity towards MB with other values from the literature.
AdsorbentqM (mg/g)Mathematical model∗pHTemperature (K)Refs.GO440.5LF3.0298This workGO445.9L7.0298This workGO803.7LF11.0298This workGO476.2LNA293[38]GO144.9L5.4298[39]GO243.9L6.0298[12]GO (various oxidation degrees)40.6 – 570.4L7.0298[37]Active carbon270.3L6.0298[12]GO/calcium alginate181.8L5.4298[39]GO17.3LNANA[13]GO/polyaniline6.7LNA298[86]GO/magnetic cellulose composite70.0LNA298[87]Magnetic multi/wall carbon nanotube11.86L7.0298[88]Activated carbon375L4 - 5298[89]Modified expanded graphite powder0.0077L7.0293[90]∗LF: Langmuir-Freundlich mathematical model; L: Langmuir mathematical model.The data summarized in Table2 show significant differences in qM values and comparison of laboratory conditions for various GOs, active carbons, carbon nanotubes, and GO/composites from the literature. Nevertheless, our GO sample under various experimental conditions showed the highest adsorption capacity towards MB dye. The GO/composite materials did not show such high qM values as may be expected. However, the lower absorption capacity of composites does not mean that they are inefficient materials if these composites show, e.g., photocatalytic activity, as demonstrated by Shahabuddin et al. [26, 27, 29]. The MB removal efficiency and lower qM should probably be connected with another synthesis procedure (Hummer’s, Brodie’s), the number of surface hydroxyl groups, pH(PZC), defects in GO honeycomb structure, and GO oxidation degree [37, 48, 56, 91]. Similar qM values were found for GO by Chia et al. [38]; compared to other GO materials [12, 13, 39] and GO/composites [39, 86, 87], our GO material showed at least two times higher, however, even fifty times higher qM values. Comparable qM values can be found for the various activated carbons [12, 16, 89] and GO [37, 38] that exhibit a relatively large surface area as well as the activation/synthesis procedure, which may play a crucial role in MB removal.The sorption process is describable at different pH values by various mathematical models. It shows the variability of the GO behavior and its ability to eliminate MB dye from aqueous solutions at different pH values. The calculated parameters (Table1) have shown differences in MB sorption depending on solution pH. In acidic (pH=3.0) and basic (pH=11.0) environment, the sorption process can be described by the Langmuir-Freundlich mathematical model (R2=0.9994;R2=0.9842) with maximum adsorption capacity of 440.5 mg/g (pH=3.0) and 803.7 mg/g (pH=11.0), respectively. Conversely, in neutral pH (pH=7.0), the behavior can be described by Langmuir mathematical model (R2=0.9900) with a maximum adsorption capacity of 445.9 mg/g.The Langmuir, Langmuir-Freundlich, and Temkin models appear to be the most suitable for the description of the MB sorption by GO under our conditions. The mathematical models (L and LF) suggested the creation of MB monolayer with GO active sites, which are identical and homogeneously distributed on the GO surface [16, 87]. Conversely, the Temkin mathematical model was used to evaluate the indirect MB-GO interaction. According to R2 values, the Temkin model can be evidently also used to describe MB on GO. The data obtained by a nonlinear fitting (Temkin model) suggested the presence of various indirect MB interactions with GO surface. Those indirect interactions probably come from the MB interactions with functional groups and GO carbon honeycomb structure (see Figure 7). The Temkin equilibrium binding constant AT decreases with increasing pH to the lowest value of 0.83 L/mg at pH 11.0. The Temkin constant bT related to the sorption heat decreased with increasing pH to the lowest value of 8.85 J/mol at pH 11.0 (Table 1). The positive Temkin constant bT values (for all pH) indicate that the MB adsorption onto GO is an exothermic reaction. With the increasing pH, the adsorption reaction is less exothermic.Figure 7
Potential interactions of MB dye with GO surface.In contrast, the Freundlich mathematical model is not suitable for the description of MB adsorption concerningR2. According to the calculated Langmuir constant, the affinity of MB sorption decreases at higher pH values.The higher sorption ability of the GO sample is dependent on the pH. It can be most likely explained by the deprotonation of the GO surface functional groups, which support MB interaction with negatively charged GO surface [2, 92]. According to data published elsewhere, the GO materials with rich oxygen-containing functional groups showed and played an essential role in the increased adsorption capacity to radioactive iodine [93], arsenic(III) [85], cadmium [94], and MB [48, 91]. Oxygen-containing functional groups enable the formation of covalent bonding, electrostatic attraction, and cation exchange with MB dye. The MB adsorption mechanism can be attributed to (a) electrostatic/ionic interactions of positively charged MB structure with negatively charged –OH, carboxyl, carbonyl, and epoxy groups on the basal plane and edges of GO and (b) π-π interaction and conjugation based on the electron donor-acceptor interaction with honeycomb GO structure (see Figure 7). The adsorption mechanism involves mainly the interaction of π electrons in C=C bond in MB structure with the π electrons in the GO honeycomb structure [48, 91, 95].Maximum adsorption capacity (L and LF) supports the above-mentioned effect of surface groups. The pH value greatly affects MB sorption, as demonstrated [2, 13], but contradicts the results of Liu et al. [92]. Adsorption efficiency for MB removal (at measured pH) achieved 98.2% (pH=3.0), 99.2% (pH=7.0), and 99.0% (pH=11.0) for initial MB concentration of 400 mg/L. The adsorption efficiencies are similar for carbon nanotubes (<98.8%) [88], activated carbon (90%) [16], and cellulose/GO composite (96.7%) [87], but not so high for GO/calcium alginate composite (83.7%) [39] and carbon nanotubes (≈ 75%) [12] in comparison with data published elsewhere.A heterogeneity parameter (nF>1) shows that MB sorption is the physical process at all pH values. The value (1/nF) suggested the standard MB sorption process. According to our results (data not shown), calculated values (nF>1;1/nF<1) show that the Freundlich model is suitable for the description of MB sorption onto GO sample (at measured pH values) [79], despite the correlation coefficient.Besides that, we calculated the separation factor (RL, Equation (9)) from Langmuir isotherm (data not shown). The RL value was used for evaluation and confirmation, whether the sorption is unfavorable (RL>1), linear (RL=1), or favorable (0<RL<1).
(9)RL=11+KL∙cE.Calculated values (0.05–0.475 g/L MB concentration range) have shown a favorable MB sorption process onto the GO sample under our experimental conditions. As shown in Figure8, RL value decreases with increasing initial concentration (c0) (at measured pH values), suggesting the MB sorption is more favorable at a higher MB concentration [16]. At pH 3.0 and 7.0, the dependence RL on c0 has shown a similar trend. Conversely, at pH 11.0, the decline is not so steep; it is evident that the MB adsorption process also becomes more favorable at a relatively high MB concentration.Figure 8
Separation factor value (RL) depending on the MB initial concentration (c0). MB initial concentration range of 0.05–0.475 g/L at 298 K.


## 3.4. Kinetics Studies

To evaluate the effectiveness of the pH solution on the MB adsorption, the plot in Figure9 shows the amount of MB adsorbed qT at time t. The initial adsorption stage is rapid for pH 7.0 and 11.0, which could be ascribed to partly and fully deprotonated GO surface groups. Conversely, the initial adsorption stage at pH 3.0 was relatively slow, and the maximum was achieved after 180 min. The slow initial adsorption stage at pH 3.0 (Figure 9) can be attributed to the complicated adsorption process, which could be connected to the mutual competition of MB dye and other ions, mainly with protons, in solution with positively charged GO surface groups. The π-π interactions of MB with the GO honeycomb structure are probably the primary type of MB interaction with the GO structure [2, 12]. GO sheets at lower pH values aggregated together and could play a role in the lower adsorption capacity and slow adsorption process. Negatively charged GO sheets and the electrostatic repulsion between sheets with increasing solution pH could be helpful for MB adsorption [86, 96], as is evident from our measured data.Figure 9
The adsorption kinetics of MB atpH=3.0 (■), pH=7.0 (●), and pH=11.0 (▲). Initial MB concentration of 0.5 g/L and 2 mL of GO suspension, i.e., 47 mg of GO at 298 K.To investigate the adsorption kinetics of MB dye on the GO, the pseudosecond-order kinetics model (10) and pseudofirst-order model (11) were tested. The pseudosecond-order and pseudofirst-order kinetics model in a nonlinear form can be expressed by [12, 97]
(10)qt=qE2∙k2∙tqE∙k2∙t+1,(11)qt=qE∙1−e−k1∙t,where qEandqt are the adsorption capacity (mg/g) at equilibrium and at time t (min), respectively, and k2 (min g/mg) and k1 (min–1) are the rate adsorption constants. The parameters of pseudo-second order can be calculated from the plot of (t/qt) vs. t (plot not shown). The results are presented in Table 3. The results showed that the pseudo-second-order model was better than the pseudo-first-order model for MB adsorption on the GO, which is in agreement with other literatures [92, 98]. Conversely, the pseudofirst order is partly suitable for the description of MB adsorption only in acidic pH, but unsuitable at neutral and basic pH, as evident from the correlation coefficient. Moreover, the rate constant of the adsorption increases with increasing pH, suggesting faster kinetic of MB adsorption at the higher pH solution.Table 3
The adsorption kinetics parameters for MB adsorption on the GO.
pHPseudosecond orderPseudofirst orderqE (mg/g)k2 (min g/mg)R2qE (mg/g)k1 (min–1)R23.0336.40.0801.0000336.21.100.80347.0336.90.1011.0000337.13.9×104−0.142911.0336.20.1061.0000336.31.3×106−0.1667The mutual correlation of measured and calculated parameters is complicated. Thus, we tried a correlation between the maximum adsorption capacity (qM), a model solution pH, and the adsorption rate constant (k2) (see Figure 10). The main effect of increasing pH is evident in the adsorption rate constant (pH=3 vs. pH=11), and the change in maximum adsorption capacity (pH=3 and pH=7 vs. pH=11) is significant, as shown in Figure 10. Basic solution pH values mainly affect qM values, and the increase in adsorption rate constant is insignificant. The k2 value variates from 0.08 to 0.106 min g/min for pH=3andpH=11, respectively.Figure 10
Mutual correlation of maximum adsorption capacityqM vs. model solution pH (●) and adsorption rate constant k2vs.qM (■) for MB removal by GO.


## 3.5. Characterization of Samples before and after Sorption of MB by FTIR

The FTIR spectra of prepared GO sample are shown in Figure11. The most intensive bands are localized in the 3800–3000 cm–1 region, corresponding to the stretching vibration of O—H bonds in hydroxyl from carboxyl groups and residual water intercalated in the GO sheets. The further bands were localized in the 2000–1000 cm–1 fingerprint region. The vibration band found at 1732 cm–1 is the characteristic of stretching vibration of C=O bonds in carboxylic groups [99–101]. The C=C stretching vibration (for carbon with sp2 hybridization) in GO was localized at 1625 cm–1 [56, 100, 101]. The bands corresponding to the bending and stretching vibration of alkoxide (C—O) and epoxides (C—O—C) functional groups were found at 1226 and 1078 cm–1 [99–101].Figure 11
(a) FTIR spectra of prepared GO sample, MB cationic dye, and GO with adsorbed MB dye, details of the fingerprint region on (b).
(a)(b)The FTIR spectra of MB dye are shown in Figure11. The fundamental bands are localized in the 1800–600 cm–1 region. The stretching vibration bands corresponding to the Chet=N+(CH3)2 bonds were found at 1648 cm–1. The intensive stretching vibration of C=C and C=N bonds is localized at 1600 cm–1. The stretching vibration of C—N and C—C bond of heterocycle was found at 1540 and 1225 cm–1 and the deformation vibration of C—N bond of heterocycle at 1143 cm–1. The C=S+ stretching vibration of MB heterocycle is seen at 1491 and 1355 cm–1. The next bands localized at 1446 and 1398 cm–1 can be ascribed to asymmetric and symmetric deformation vibration of C—H bond in N(CH3)2. The stretching vibration of C—N in N—CH3 is found at 1340 cm–1 and deformation and bending out-of-plane vibration of C—H at 1251, 1225, and 1189 cm–1. Finally, the C—S—C bond vibration of MB heterocycle is located at 1069 cm–1. All these vibrations correspond with the literature [102–104].The FTIR spectra shown in Figure11 correspond to the GO after sorption of MB dye. It should be mentioned that the intensity of characteristic GO bands decreased, particularly the intensity of the characteristic stretching vibration of (O—H) bonds in 3800–3000 cm–1 region. The vibration band at 1730 cm–1 corresponding to C=O bonds in carboxylic groups nearly disappeared, the band at 1625 cm–1 slightly shifted to 1638 cm–1, and the intensity also decreased for C=C stretching vibration. The most intensive bands of MB were also found in the sample of GO after MB adsorption as 1491, 1398, 1355, and 1340 cm–1. Only two vibration bands were slightly shifted at 1143 and 1069 cm–1 to 1149 and 1074 cm–1, corresponding to deformation vibration of C—N and stretching vibration of C—S—C of heterocycle of MB (Figure 11). The attenuation of the GO bands could be ascribed to covering of GO sheets by MB and just slight shifting tends to the suggestion that most probably π-π interaction coming from aromatic rings of MB and GO is present [16, 87].


## 3.6. Characterization of Samples before and after Sorption of MB by Powder XRD

The mechanism of MB adsorption was studied by Bujdák et al. [105], where orientations of MB cation were compared with experimental data. The calculated height of the MB cation is 0.77 nm. The arrangements of MB cation as intercalated dimer and monomer were determined and compared with the results obtained by Bujdák et al. [105]. The interlayer space was found to be at the range 7.2°–7.7° 2Θ corresponding to ~1.15-1.25 nm and monomeric arrangement of MB cations for all samples after sorption of MB at pH 3, 7, and 11 (Figure 12). The zones with no occupancy by MB cation were confirmed by the presence of large diffraction line at the range 10.9°–13.5° 2Θ (~0.81-0.66 nm). So, the interlayer space decreases significantly by the absence of MB cation.Figure 12
XRD patterns of GO before and after sorption MB at pH 3, pH 7, and pH 11.


## 4. Conclusions

Graphene oxide prepared by a simple and low-cost verified synthesis process can serve as an effective sorbent for removing dyes in effluents or other contaminated waters. We have shown a higher GO adsorption capacity for MB removal in the whole pH range compared to other works [12, 13, 37, 38, 83] and GO-based composites. Solution pH plays a crucial role in the MB removal by GO and also affects the dissociation degree of surface functional groups, i.e., hydroxyl and carboxyl. The number of surface groups was determined by acid-base titration, and IEP was evaluated by zeta potential measurement. Negatively charged oxygen-containing groups in the whole studied pH range were confirmed. According to MB kinetic adsorption studies at pH=3.0, MB adsorption is complicated and slower due to the competition of MB with protons and positively charged functional groups on the GO surface. The increase of pH solution facilitated the MB adsorption via negatively charged GO surface and electrostatic repulsion. The purity of the prepared GO samples was proved by Raman spectroscopy and XRD; the good quality of the sheets was confirmed by TEM and AFM. The FTIR spectroscopy confirmed that the MB covering of GO sheet made the vibration spectrum of GO generally less intensive. Just slight shifting was found for C=C stretching vibration of GO and deformation vibration of C—N and stretching vibration of C—S—C of heterocycle of MB. Therefore, only electrostatic interaction, π-π interaction of aromatic rings of MB, and GO could be present. The higher sorption capacity of GO to MB dye and the other dyes belongs to the benefits of our prepared material, as we have shown in our previous paper [106]. The MB adsorption process can be described by the Langmuir-Freundlich mathematical model in acidic and alkaline pH, whereas by the Langmuir model in neutral pH. The Temkin model suggested various indirect MB interactions with the GO surface and the adsorption as an exothermic process. The applied mathematical models indicated that the MB adsorption on the GO is a chemisorption process based on the ionic bonds and weak chemical interaction formed between MB and GO.



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