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Removal of Uranium-238, Thorium-232, and Potassium-40 from Wastewater via Adsorption on Multiwalled Carbon Nanotubes

The optimum conditions for the removal of uranium-238, thorium-232, and potassium-40 from wastewater and the discharge of nuclear facilities using multiwalled carbon nanotubes (CNTs) are described. The adsorption mechanism is mainly attributed to chemical interactions between the metal ions and surface functional groups of the CNTs. Batch adsorption experiments are carried out in order to study the effect of different parameters such as pH, contact time, initial metal ion concentration, adsorbent dose, and temperatures. Maximum metal removal (>98%) from solutions containing 20–120 Bq/L metal ions is achieved using a contact time of 15 min, a pH of 6.0, and 10 mg/L CNTs. The effect of temperature on the kinetics and equilibrium of adsorption on CNT particles is examined. Consistent with an exothermic reaction, an increase in the temperature resulted in an increase in the adsorption rate. Langmuir, Freundlich, and Dubinin–Radushkevich isotherms are applied to the data obtained at various temperatures. The Langmuir adsorption model is the best for data interpretations. The kinetics of adsorption reveals a pseudo-second-order mechanism. Thermodynamic parameters at 293 K (ΔG°, ΔH°, and ΔS°) for U-238, Th-232, and K-40 are −14590.7 kJ/mol, −6.66 kJ/mol, and 26.47 J/(mol K), −96,96.5 kJ/mol, −2.48 kJ/mol, and 14.17 J/(mol K), and −3922.09 kJ/mol, −1.32 kJ/mol, and 6.12 J/(mol K), respectively.


INTRODUCTION
"NORM" refers to a naturally occurring radioactive material that exposes individuals to radiation. 1 Human activities (e.g., burning coal, fertilizer industry, and oil and gas production operations), 2 frequently enhance NORM exposure. One of the main industries with an aqueous TENORM (technologically enhanced NORM) problem is the petroleum industry. 3 The radionuclides identified in oil and gas streams belong to the decay chains of uranium and thorium. 4 When the produced water is brought to the surface, it contains uranium-238, thorium-232, and potassium-40 together with an abundance of other cations, mainly alkaline earth cations. 5 The highly toxic nature of these radioactive metal ions renders the effective separation and removal of these radiotoxic substances from nontoxic compounds highly desirable. These hazardous contaminants are nonbiodegradable and highly toxic and tend to accumulate in living creatures. 6 The removal of radioactive nuclide ions from wastewater is a crucial step toward improving water quality and ensuring a safe water supply. 7 As a result, it is critical to remove these metal ions from the waste before releasing it into the environment. According to a study by the World Health Organization (WHO), uranium-238, thorium-232, and potassium-40 are some of the most hazardous elements that influence the environment. 8 Several studies have been carried out to identify a suitable and efficient sorbent for the removal of heavy metal ions and other contaminants. Natural inorganic materials, peat, peat moss, algae, yeast biomass, rice husk, nanomaterials, sawdust (SW), and others have been suggested. 9 Carbon multiwalled nanotubes showed promising adsorption efficiency due to their unique structure and properties, especially the large specific surface area and large pore volume. 10,11 The present work was undertaken to investigate the use of multiwalled carbon nanotubes (MWCNTs) for the removal of uranium-238, thorium-232, and potassium-40 from wastewater. The experimental conditions including the effect of pH, contact time, temperature, and initial concentrations of MWCNTs and the metal ions were optimized, and adsorption mechanisms, thermodynamics, and kinetic models are also discussed.

EXPERIMENTAL SECTION
2.1. Chemicals and Equipment. Deionized twice-distilled water was used throughout. All the chemicals are of the highest purity obtained from Sigma-Aldrich. Hydrochloric acid and sodium hydroxide are used for pH adjustment. MWCNTs were prepared via chemical vapor deposition (CVD). In CVD, a volatile precursor undergoes thermal decomposition at elevated temperatures to form a solid deposit on a substrate. The diameter of the tubes ranges between 110 and 170 nm, and the length is between 5 and 9 μm. The multiwalled nanotubes are stable in an inert atmosphere up to a temperature of 3697°C, according to Sigma-Aldrich production. A Dragon digital hotplate with a magnetic stirrer (MS-H-Pro) and a temperature sensor (PT 1000; IKA) was used. The pH of the test solutions was adjusted using a HANNA HI2211 Ph/ORP meter. A γ-ray spectrometer with a high-purity germanium (HPGe) detector/ORTEC was employed, and point sources of 137 Cs (661.6 keV) and 60 Co (1172 and 1332.3 keV) were used for the spectrometer energy calibration. Test samples containing NORMs were obtained from the local crude oil company (Suez governorate, Egypt). The half-life for the NORM isotopes is 4.468 × 10 9 years for uranium-238, 1.4 × 10 10 years for thorium-232, and 1.251 × 10 9 years for potassium-40.
2.2. Methods. Due of the small size of MWCNTs, a batch approach was utilized. These studies were carried out by swirling the MWCNTs with varying concentrations of uranium-238, thorium-232, and potassium-40, and the pH was adjusted to different values ranging from 2 to 8 using hydrochloric acid and/or sodium hydroxide solution. Adsorption experiments were conducted at various contact times (5, 10, and 15 min), temperatures (293, 303, and 313 K), and MWCNT dosages (0.004, 0.008, and 0.01 g). All figures representing the experimental data were based on the average of triplicate runs. The standard deviation did not exceed ±3%. The initial uranium-238, thorium-232, and potassium-40 ion concentrations were 27.9, 55.8, and 111.6 Bq/L for uranium-238, 5.91, 11.83, and 23.67 for thorium-232, and 19.3, 38.61, and 77.22 Bq/L for potassium-40 for MWCNT dosages of 0.004, 0.008, and 0.01 g, respectively. Aliquots of the test sample solutions were collected at regular intervals, filtered to remove particulates, and examined using a γ-ray spectrometer with an HPGe detector. The concentrations of the metal ions before and after adsorption were measured. The data were used to compute q e (mg/g), which is the difference between the initial and equilibrium metal concentrations, and q t (mg/ g), which is the difference between the initial and temporal variations (t) of metal concentrations (eqs 1 and 2, respectively) (1) Metal removal (%) was determined using eq 3 where C o (mg/L) is the initial metal concentration, C e (mg/L) is the equilibrium concentration of the metal ions, C t (mg/L) is the metal concentration in the solution after time t, m (g) is the used mass of the MWCNT dose, and V is the volume of the test solution represented by C t (mg/L).
2.3. Adsorption Kinetics Modeling. The kinetics of the metal removal was studied using a series of solutions having various initial concentrations of uranium-238, thorium-232, and potassium40 ions. Batch adsorption experiments were also conducted with various pH values, contact durations, dosages, metal concentrations, and temperature parameters. Applicability of pseudo-first-order, pseudo-second-order, and kinetic models was tested under the experimental conditions. Different aliquots of uranium-238, thorium-232, and potassium-40 ions were subjected to batch adsorption experiments using a stirring rate of 600 rpm and a 0.01 g MWCNT dosage at 293 K. The data were used to test the applicability of the adsorption isotherms of Langmuir, Freundlich, and Dubinin−Radushkevich (D−R).
2.4. Effect of Initial Metal Concentrations. A 0.01 g portion of the adsorbents (MWCNTs) was added to solutions containing 111.6, 23.67, and 77.2 Bq/L of uranium-238, thorium-232, and potassium-40, respectively. The mixtures were stirred using a magnetic stirrer for 15 min at 600 rpm. After different intervals of time (5, 10, and 15 min), the solutions were filtered off through Whatman no. 1 filter paper. The metal ions were quantified using the HPGe detector-based γ-ray spectrometer. The experiment was repeated using different doses of the adsorbent (MWCNTs).
2.5. Effect of pH of the Test Solutions. To 20 mL aliquots of uranium-238, thorium-232, and potassium-40 solutions, 0.01 g of the MWCNT adsorbents was added. The pH of the solutions was adjusted to 2, 4, 6, and 8 by adding 1.0 N HCl and/or NaOH. Using a 600 rpm mixer, the mixture was stirred, and the remaining concentrations were measured after 5, 10, and 15 min intervals using a HPGe detector-based γ-ray spectrometer.
2.6. Effect of Contact Time. Different portions (0.004, 0.008, and 0.01 g) of the MWCNT adsorbent were added to aqueous solutions containing uranium-238, thorium-232, and potassium-40. The solutions were stirred at 600 rpm, and the metal contents were measured at time intervals of 5, 10, and 15 min.
2.7. Effect of Temperature. Adsorbents (MWCNTs) were added to uranium-238, thorium-232, and potassium-40 test solutions with the concentrations of 27.9, 55.8, and 111.6, Bq/L for uranium-238, 5.91, 11.83, and 23.67 Bq/L for thorium-232, and 19.3, 38.61, and 77.2 Bq/L for potassium-40, respectively. The temperature of the solutions was adjusted to 293, 303, and 313 K, and the solution was stirred at a rate of 600 rpm. The solutions were filtered off, and the remaining metal ions were measured using the HPGe detector-based γray spectrometer at time intervals of 5, 10, and 15 min. The experiment was repeated at different temperatures T = 293, 303, and 313 K.

RESULTS AND DISCUSSION
Several factors affecting the reaction rate and influencing the removal of uranium-238, thorium-232, and potassium-40 nuclides from wastewater using MWCNTs have been investigated and optimized.
3.1. Effect of pH. The influence of pH on metal sorption was investigated because variation of solution acidity affects the ionization state of the sorbent functional groups. Equilibrium experiments were conducted with initial uranium-238, thorium-232, and potassium-40 test solutions with concentrations of 111.6, 23.67, and 77.22 Bq/L, respectively. The pH ranged from 2.0 to 8.0. To adjust the pH of the metal ions, a dilute NaOH and/or HCl solution was added to the test solution. Increasing the pH slightly increases metal sorption to reach a maximum adsorbing capacity at a pH of 6.0 and then decrease, as shown in Figures 1 and 2. While uranium-238 and thorium-232 ions are removed more efficiently at a pH of 2.0 than at a pH of 8.0, potassium-40 ions are not. Despite the fact that metal removal is more effective in acidic environments, a mild adsorption slightly occurs under some acidic circumstances. Under these conditions, the bulk of the functional component groups on the adsorbent are protonated, leaving a few ionizing groups free and available for the adsorption process. 12 This explains the weak metal ion adsorption in an acidic medium due to competition between protons and metal cation species. 13 The high adsorption at high pH values may be attributed to the presence of free lone pair of electrons on the adsorbate, suitable for coordination with the metal ions. The metal ions are generally solved and hydrolyzed in an aqueous solution. 14 It can be seen that increasing the pH up to 6 is associated to a slight increase of the adsorption effectiveness and the percentage removal of the metal ions due to the replacement of the hydrogen ions on the surface of carbon nanotubes by the metal ions. 15 3.2. Effect of Contact Time. Data from several measurements conducted at different contact times between the metal ions and MWCNTs were averaged, and the adsorption of metal ions was plotted as a function of time. A period of 15 min was sufficient to almost quantitatively remove all metal ions from the test solutions (Figures 4, 6, and 8). In order to determine the adsorption efficiency, three different initial metal concentrations and 0.01 g/L MWCNTs were used to measure the metal concentration change in the aqueous solutions before and after the adsorption equilibrium. Because the      adsorption capacity remained virtually constant for all quantities of metal and carbon nanotubes tested, it was deemed to represent the equilibrium state. There was a possibility that the initial speed was related to the surface adsorption, wherein the adsorbent surface is free. A higher rate of reaction occurred next, followed by the adsorbed metals penetrating and adhering to the porous adsorbents (intraparticle diffusion). 16 Both the sorption process and the adsorption equilibrium began to open up a large number of pores, as seen in Figures 3, 5, and 7. Uranium-238, thorium-232, and potassium-40 have different initial metal ion concentrations; with uranium-238 averaging 111.6 Bq/L and thorium-232 averaging 23.67 Bq/L. From these plots, it was clear that the amount of metal adsorption significantly increased with the increasing contact time at all initial metal concentrations, reaching a state of equilibrium within 15 min. 17 These results revealed a noticeable increase of q t (mg/g) with the increase of the initial metal ion concentration. In these set of kinetic experiments, uranium-238 and potassium-40 metal ions were rapidly adsorbed on the outer surface of MWCNTs, followed by a sluggish intraparticle diffusion in the interior adsorbent pores. Accordingly, these two-stage metal ion uptakes simultaneously occur on the binding sites of two distinct adsorbent particle types ( Figure 9). 18 3.3. Effect of the Adsorbent Dose. The dose of an adsorbent determines the capacity of an adsorbent for a certain initial concentration of the metal adsorbate. While maintaining other parameters constant (i.e., pH; stirring speed; temperature; initial uranium-238, thorium-232, and potassium-40 ion concentrations; and contact time), the dependence of uranium-238, thorium-232, and potassium-40 adsorption on different doses of the MWCNT adsorbent (0.004, 0.008, and 0.01 g) was examined. According to Figures 10−14, the removal % of uranium-238, thorium-232, and potassium-40 ions was increased by increasing the adsorbent dosage of MWCNTs from 0.004 to 0.01 g.

Effect of the Initial Metal Ion Concentration.
Metal ion adsorption was significantly influenced by its initial concentration in the test solutions. The removal % of uranium-238, thorium-232, and potassium-40 decreased from 100 to 99.5% with the increase of the initial metal ion concentrations from 27.9 to 111.6 Bq/L. At lower metal ion concentrations, the ratio of the initial concentration of uranium-238, thorium-232, and potassium-40 to the available adsorption sites was low; thus, complete adsorption occurred. However, at higher metal ion concentrations, the available adsorption sites decreased compared to the concentration of the metal ions present in the solution due to the lack of sufficient active sites on MWCNTs, and thus, the percentage sorption of metals decreased. 19 The amount of metal ions, q e (mg/g), increased with the increasing initial metal concentration, as shown in Figures 15−17. 3.5. Effect of Temperature. The temperature has a significant impact on the adsorption mechanism. Adsorption is increased when temperature is increased because it decreases viscosity and therefore speeds up the passage of adsorbed molecules through the adsorbent's exterior boundary layer. 20 Batch adsorption tests were conducted at temperatures of 293, 303, and 313 K, and the results are presented in Figures  18−20. Uranium-238 and potassium-40 ions become more mobile when the temperature increases because the retarding forces acting on them are reduced. As a result, the adsorbent's sorption capacity is increased, the chemical interaction between the adsorbate and adsorbent is also increased, and more surface active centers are generated. At higher temperatures, an increased rate of intraparticle diffusion of the metal      ions into the pores of the adsorbent may be considered. 21 These point to a possible exothermic adsorption process. 21,22 The temperature dependency of the adsorption technique is related to the changes of several thermodynamic factors. Using the obtained adsorption equilibrium data for various temperatures, significant thermodynamic characteristics such as standard Gibbs free energy (ΔG°), standard enthalpy change (ΔH°), and standard entropy change (ΔS°) are computed. These parameters were estimated using eqs 4−7 where q e is the equilibrium concentration of uranium-238, thorium-232, and potassium-40 ions adsorbed onto the MWCNT from the solution, C e is the equilibrium concentration of uranium-238, thorium-232, and potassium-40 in the solution, R is the gas constant, T is the absolute temperature, and K e is the adsorption equilibrium constant.
A van't Hoff plot of ln(K e ) against 1/T was constructed and used to determine ΔH°and ΔS°. The values of ΔG°, ΔH°, and ΔS°are presented in Table 1. A reduction in Gibbs free energy of uranium-238 and potassium-40 adsorption onto MWCNTs was found as the temperature increased, and its values were negative at all temperatures examined in the present work. Adsorption of uranium-238, thorium-232, and potassium-40 is an exothermic reaction, as confirmed by the negative Gibbs' free energy (ΔH°). Adsorption rates and capacities are high at high temperatures, enabling metal ions to be rapidly adsorbed. 23 When adsorption of radionuclide ions occurs, the enhanced unpredictability at the solid/liquid interface allows for randomness to prevail in the system, 24 as can be seen in Figure 14. Uranium-238 ions, thorium-232 ions, and potassium-40 ions are all adsorbed more easily as the temperature increases, suggesting an exothermic adsorption process, which may be ascribed to an increase in ion mobility. This increases the quantity of ions that interact with the active sites on adsorbent surfaces. In aqueous-phase adsorption, other studies have discovered similar patterns. This means that, as indicated in eq 1, the sign of ΔG°depends on the entropy term ΔS°(eq 6). It is important to note, as well, that the negative values of ΔG°are indicative of the spontaneous adsorption behavior. Temperature-dependent ΔG°values demonstrate that higher temperatures promote greater spontaneous reactions. As a result, the entire adsorption process of the tested radionuclides may be attributed to intraparticle diffusion ( Figure 21).

Adsorption Kinetics.
In order to understand the nature of adsorption processes, evaluation of the efficacy of adsorbents for the tested metal ions is undertaken by using kinetic models and choosing the optimal operating parameters for the full-scale batch process. This requires knowledge of the dynamics of uranium-238, thorium-232, and potassium-40 to   develop and simulate adsorption processes. This was achieved by examining the pseudo-first-order models, 25 as well as the pseudo-second-order models. Experimental findings and model-predicted values were compared using correlation coefficients (R 2 , values close or equal to the value 1, the relatively higher value is the more applicable model). Figures 3,5,and 7 show the removal of uranium-238, thorium-232, and potassium-40 via adsorption as a function of contact time.
MWCNTs display good removal % over the first 15 min. There was no increase in adsorption when the contact period exceeded 15 min. According to these observations, the metal ion adsorption to the adsorbent occurred quite quickly. As part of the investigation of the process of adsorption and its probable rate-controlling measures, which entail mass movement and chemical reaction prowess, two kinetic models are employed to evaluate the experimental results. Kinetic data are well-correlated to describe how metal ions are adsorbed in the solid phase. A summary of kinetic parameters is shown in Table 2. For each model, the R 2 values are compared in order to assess the model validity. The data displayed in Table 2 agree fairly well with the pseudo-second order model.

Kinetic Model (Pseudo-First-Order).
The oldest known equation for the adsorption rate as a function of the adsorption capacity is Lagergren's pseudo-first-order model (eq 8) where k 1 , q e (mg/g), and q t (mg/g) are the metal quantities adsorbed per unit mass at the equilibrium at any time. Figures  22−24 and Table 2 display the values of k 1 and q e . The true test of the validity of eq 8 is a comparison of the empirically measured q e values with those derived from plots of ln(q e − q t ) versus t. 25,26 The correlation coefficients for the pseudo-firstorder kinetic model are low, and a difference in the equilibrium adsorption capacity (q e ) between the experimental data and the calculated data was observed, indicating a poor pseudofirst-order fit to the experimental data. 3.8. Kinetic Model (Pseudo-Second-Order). The kinetic data are based on the assumption that the adsorption process follows a pseudo-second-order model (eq 9).
where k 2 is the pseudo-second-order rate constant for adsorption (mg g −1 min −1 ). As shown in Figures 18 and 19, the slope and intercept may be used to obtain q e (q e = 1/ intercept) and K 2 [k 2 = (slope) 2 /intercept] values from the linear plots given in Figures 25−27. For each of the aforementioned two models, presented in the figures, a linear plot was employed to test their applicability. In order to assess the applicability of each model, the correlation coefficient, R 2 , was computed from these plots. Table 1 shows that the kinetic rate constants obtained from the firstand second-order pseudo-kinetic models. The pseudo-second-order adsorption model's correlation coefficient, R 2 , is relatively high (>0.9979), and the adsorption capacities calculated by the model are also close to those determined from the experiments. The R 2 values for the pseudo-first-order model, on the other hand, are not satisfactory. 27 As a result, the pseudo-second-order adsorption model was found to be more suitable for describing uranium-238, thorium-232, and potassium-40 adsorption kinetics on MWCNTs.
In general, the adsorption process proceeds in three steps: (i) the adsorbate moves from the bulk solution to an adsorbent surface via diffusion; (ii) the adsorbate migrates into adsorbent pores; and (iii) the adsorbate interacts with the accessible sites on the inner surface of pores. 28 3.9. Equilibrium Adsorption Study. Adsorption process design and optimization necessitate the establishment of an adequate isotherm model. Some of the established isotherm models for estimating the equilibrium adsorption of chemicals from solutions are known; these are Langmuir, Freundlich, Redlich−Peterson, D−R, Sips, and Temkin. Because the Langmuir, Freundlich, and D−R equations are the most often employed to analyze the adsorption isotherm, the experimental data of this work were fit using these three models. Equilibrium adsorption isotherms are useful for assessing metal ion adsorption capacity as well as identifying the type of adsorption on MWCNTs. 28,29 3.10. Langmuir Model. The theoretical Langmuir sorption isotherm 28 (10) In this equation, q e is equal to the equilibrium metal ion concentration of the adsorbent in milligrams per gram, C e is equal to the equilibrium metal ion concentration of the solution, q max is equal to the monolayer adsorption saturation capacity of the adsorbent, and b is equal to the Langmuir constant. Using a regression equation, the Langmuir isotherm parameters were calculated, as shown in Figure 28, and the results are summarized in Table 3. In order to determine b and q max, the slope and intercept of the plots were employed. Langmuir's adsorption model performs exceptionally well with metal ions, as seen by high R 2 values.
In addition, the Langmuir isotherm can be expressed in terms of a dimensionless constant separation factor (R L ), which is defined in eq 11 where C o is the initial concentration of the metal ion and the values of R L indicate the type of isotherm to be either unfavorable (R L > 1), linear (R L = 1), favorable (0 < R L < 1), or irreversible (R L = 0). The present study shows R L values in the range of 0.66−0.88, 0.06−0.88, and 0.68−0.88 for uranium-238, thorium-232, and potassium-40, respectively. These data indicate that the adsorption process is more favorable. 29,30 3.11. Freundlich Model. According to the Freundlich isotherm model, which is commonly used in the case of      adsorption on heterogeneous surfaces, the adsorbent sorption energy drops exponentially when adsorbent sorption sites are saturated. In the linear form, this isotherm is an empirical equation (eq1 12) that can be used to explain heterogeneous systems. 31 The adsorption capacity and intensity are represented by the Freundlich constants K F and 1/n, respectively. Table 3 presents the values of constants 1/n and K F , which are determined from the slope and intercept, respectively. The plot of log q e versus log C e is shown in the results. A value of 1/n smaller than 1 indicates good adsorption and validates the heterogeneity of the adsorbent (Figure 29). It also implies that radioactive nuclide ions and MWCNTs have a strong connection ( Figure 30). 31 3.12. D−R Model. Using the D−R isotherm model, which is semi-empirical in nature, the adsorption process is controlled by the pore filling mechanism, assuming multilayer adsorption, van der Waals forces, and physical adsorption processes. 30,31 The linear form of the D−R isotherm model is represented as eq 13 where q s is the theoretical isotherm saturation capacity (mg/g), K ad is the D−R isotherm constant (mol 2 /J 2 ), and ε is the Polanyi potential, which is equal to RT ln(1 + 1/C e ), where R (J/mol K) is the gas constant and T(K) is the absolute temperature. Figure 31 shows a linear relation between ln q e and ε 2 . The slope of the plot gives K ad (mol 2 /J 2 ), and the intercept yields the sorption capacity q s (mg/g) ( Table 3). The constant K ad gives an idea about the mean free energy E (kJ/ mol) for adsorption per molecule of the adsorbate when it is transferred to the surface of the solid from infinity in the  This value reveals whether chemical ion exchange or physical interaction is the mechanism of metal removal. When E is between 8 and 16 kJ/mol, the adsorption process is referred to as chemical ion exchange, whereas when E is less than 8 kJ/mol, the adsorption process is referred to as physical contact. The adsorption of the mean free energy in uranium-238 is 100 kJ/mol and in thorium-232 is 235 kJ/mol, which corresponds to a physical process. 32 Finally, when the R 2 values in Table 3 are compared, all of the isotherm models fit quite well.
4. X-RAY DIFFRACTION X-ray diffraction (XRD) spectrometry was conducted in order to clarify whether there is a change in the crystal structure of MWCNTs before and after adsorption. Figure 31 shows that XRD patterns of all MWCNTs before and after adsorption of radionuclides have almost the same first-order diffraction peak at a 2θ of 25.1, which corresponds to a d-spacing of 0.43 nm according to Bragg's equation. 33 This means that adsorption of uranium-238, thorium-232, and potassium-40 leads to no significant change in the crystalline structure of MWCNTs. The main difference in the XRD patterns of MWCNTs is the intensity of the first-order diffraction peak. This difference is probably due to the different adsorption coefficients of the elements present on MWCNTs or due to the transformation of amorphous carbon, leading to an increase of the graphitization degree after adsorption of the radionuclide ions on MWCNTs. 34

CONCLUSIONS
In this study, MWCNTs have been used for the removal of uranium-238, thorium-232, and potassium-40 ions from aqueous solutions. Batch experiments of metal adsorption were carried out to study the effect of pH, contact time, initial metal ion concentration, adsorbent dose, and temperature. Under optimized conditions (contact time = 15 min, pH = 6, and MWCNT concentration = 0.01 mg/L), >98% of uranium-238, thorium-232, and potassium-40 were removed. A pseudosecond-order adsorption model was found to be more suitable for describing the adsorption kinetics. The Langmuir adsorption model displayed the best R L values for adsorption of uranium-238, thorium-232, and potassium-40 ions in the ranges of 0.66−0.88, 0.06−0.88, and 0.686−0.89, respectively. The Freundlich value of 1/n was less than 1, indicating fa avorable adsorption process and confirming the adsorbent's heterogeneity. The thermodynamic data (ΔG, ΔH, and ΔS) reveal an exothermic reaction. No change in the crystal structure of the adsorbate due to the metal adsorption was confirmed via XRD.