Linear and Non Linear Recognition for the Sorption of 60Co and 152+154Eu Radionuclides onto Bio CuO Nanocomposite

A novel nanocomposite was prepared by hybridizing polyacrylic acid/maleic acid with nano copper oxide (PAACMA/CuO) for the sorption of 60Co (II) and 152+154Eu (III) radionuclides from an aqueous solution. Nano-CuO was biochemically produced by hydrolysing its salt in the presence of the Aspergillus terreus fungus. The PAACMA/CuO nanocomposite was characterized using a variety of analytical techniques. The optimum sorption conditions (pH  4.5 for 60Co and pH  3.53 for 152+154Eu, 24 h of equilibrium time at 20 oC) were applied. The kinetic mechanism of the sorption reaction was controlled by pseudo second order based on residual charts, coefficient of determination (R2), and corrected Akaike information Criterion (AICc). The sorption reaction mechanism was controlled by Langmuir model for linear regression using the coefficient of determination and the Dubinin-Radushkevich D-R model for the AICc and residual plots error functions. The reaction mechanism throughout non-linear regression was controlled by the D-R model due to the coefficient of determination, AICc, and residual charts. The PAACMA/CuO nanocomposite had a mono-layer adsorption capacity of 11.04 mg g− 1 for Co (II) and 21.54 mg g− 1 for Eu (III). According to desorption studies, Co (II) and Eu (III) could be recovered by 0.1 mol L− 1 EDTA with efficiencies 55.46% and 95.044%, respectively. According to thermodynamic studies, the sorption of Co (II) and Eu (III) on the prepared composite was endothermic and spontaneous.


Introduction
The global expansion of nuclear energy applications in fields such as agriculture, industry, nuclear medicine, nuclear weapons, nuclear research, and others has disrupted the environmental balance as radioactive residues for these applications have increased. Scientists [1][2][3][4] are working hard to find a solution to this growing problem. Radioactive isotopes like 60 Co and 152+154 Eu are hazardous to humans due to their prolonged half-lives of 5.3 and 8.8 years, respectively. They are polluters, and they cause significant harm to the environment and to human health [5]. 60 Co can cause skin burns, acute radiation sickness, and even death at extremely high doses. 152+154 Eu has been associated to cancers of the liver and/or bones [6]. A number of techniques for removing radionuclides from waste water have been developed such as coagulation, precipitation, sorption, ion exchange, membrane technique [7], and solvent extraction [8]. The most effective method determined by the waste treatment cost and methodology. Metal oxides, including iron oxide [9][10][11], activated aluminium oxide [12,13], titanium oxide [14,15], manganese oxide [16,17], and zirconium-magnesium binary oxide [18,19], have attracted a lot of attention as sorbents.
Yılmaz D et al. [20] found that nanomaterials offered a wide range of possibilities for producing the newest radioactive wastewater decontamination technology [21]. However, the toxicity features and expansive analysis requirements in addition to the need of skilled human resources hinder the actual/specific application of these nanomaterials [22]. The use of natural resource which named as green chemistry can solve most of these limitations [22].
Aspergillus terreus is a fungus that can produce extracellular or intracellular nanoparticles [23] through metabolic activity that bio-reduces or aggregates complex metal ions that do not dissolve into colloidal particles.
Dispersing nanoparticles in polymer matrices can enhance a variety of chemical properties, including thermal stability, electric conductivity, hydrophilicity, and the transition of chemical properties from "bulk" matrix-controlled criteria to interphase or "surface" dominated characteristics [24]. Maleic acid combined with polyacrylic acid (PAACMA) has superior adsorption capabilities for copper ions from wastewater. Its thermal stability could be improved from 40.3% to 99.84% after copper ions adsorption [25].
To the author's knowledge, the adsorption studies of 60 Co (II) and 152+154 Eu (III) radionuclide onto highly and low-cost adsorbent of dispersed nano copper oxide in polyacrylic/maleic acid have not yet been published. Accordingly, authors decided to study the effective conditions and mechanism of the sorption process.
Over the last few decades, the mechanism of the sorption reaction has been designed using linear regression [26]. Current findings, on the other hand, have revealed an increasing disparity (between predictions and experimental data) and model disability, resulting in model failure [27]. Recently, expanding nonlinear has been identified as a potentially powerful and efficient tool that could lead to further advances in adsorption science [28]. The use of error functions to generate a minimal distribution between experimental equilibrium data and predicted isotherms is common. Depending on how the applied error function is defined, the error distribution between the experimental equilibrium data and the predicted isotherms will be reduced either by minimising the error function or by obtaining maximum error functions. The most popular error function used to acquire the ideal distribution between experimental equilibrium data and isotherms is the coefficient of determination, or R 2 [29]. Recent studies have looked into additional error functions, such as average relative error (ARE), sum of absolute errors (EABS), and corrected Akaike information (AIC c ), to estimate the optimum isotherm [26,30]. To find the best isotherm fitting, it is advised to use more than one error function.
The purpose of this research was to prepare a novel nano copper oxide composite for the sorption of radionuclides 60 Co (II) and 152+154 Eu (III). Nano copper oxide biosynthesised with the assistance of the metabolic fungus Aspergillus terreus. The monomers of acrylic acid, maleic acid and biosynthesized nano copper oxide were then copolymerized with radiation from a 60 Co cell at a dose of 25 kGy. Calcined biosynthesized CuO nanoparticles (Nps) and PAACMA/ CuO were characterized. Batch sorption experiments were performed on the radionuclides 152+154 Eu (III) and 60 Co (II).
To optimise the sorption process, effective sorption factors such as pH, time, temperature, ionic strength, and concentration were investigated. Kinetic and equilibrium isotherms are used for determining the reaction mechanism. Fitting errors were minimised by using linear and nonlinear fitting techniques. Additionally, residual error plots, coefficient of determination (R 2 ), and corrected Akaike information Criterion (AIK c ) were used to examine the qualitative and quantitative aspects of the fitting results. To show the potential of using PAACMA/CuO nanocomposite as a radioactive waste sorbent, thermodynamic studies and the desorption process of 60 Co (II) and 152+154 Eu (III) were conducted.

Materials and Procedure
All precursors used during the study were of analytical grade and used without further purification. Acrylic acid (AA) with purity ≥ 99% got from Elf chem.co, France. Maleic acid (MA) of purity 99% obtained from Loba Chemie India. Copper sulphate (CuSO 4 .7H 2 O) 98% purchased from Merck, Egypt. Methylene bis-acrylamide (DAM) was supplied from (Merck, Germany). Extra pure cobalt (II) chloride (CoCl 2 .6H 2 O) was purchased from BDH (UK). Eu 2 O 3 salts got from Merck Co., Germany. The 60 Co and 152+154 Eu isotopes were produced by neutron irradiation of the corresponding salt in the Second Egyptian Research Reactor (ET-RR-2) at Inshas, Egyptian Atomic Energy Authority with initial activity 100 KBq/L. A 300 mg L − 1 stock solutions of Co (II) and Eu (III) prepared by dissolving a certain amount of Co (II) and Eu (III) salts in double distilled water then spiked with the 60 Co and 152+154 Eu radionuclides, respectively. These solutions kept as a stock radioactive solution for all experiments.

Preparation of CuO Nps and PAACMA/CuO Nanocomposite
Aspergillus terreus was cultivated in Czapek-Dox broth medium [23], and CuO Nps was synthesised by hydrolysis of CuSO 4 via the supernatant of the fungus [23]. The CuO Nps collected and washed with distilled water before drying for 24 h at 60 o C and calcined for 2 h at 600 o C (Fig. 1).
The calcined CuO Nps copolymerized with acrylic acid (AA) and maleic acid (MA) in the presence of the cross linker methylene bis-acrylamide (DAM). After mixing 80 mL of deoxygenated water with 18 mL of AA, 2 g MA, 0.5 g DAM, and 0.5-2 g of calcined CuO NPs, the mixture magnetically stirred for 2 h at room temperature. The mixture exposed to gamma radiation at a dose rate of 689.538 Gy/h using a cobalt-60 gamma cell 220. After polymerization, the materials were cut into small pieces and soaked in acetone for 2 h to remove water, unreacted polymer, and impurities before being dried for 24 h in a vacuum oven at 333 K and sieved to size (250 mm). The successful preparation of PAACMA/CuO nanocomposites with various molar compositions is shown in Table 1. A predicted polymerization mechanism is depicted in Fig. 2.

Instruments
The morphology of the particles analysed using a scanning electron microscope (SEM, Philips XL 30 ESEM), which combined with energy-dispersive X-ray spectroscopy and electron backscatter diffraction (25-30 keV accelerating voltage, 1-2 mm beam diameter and 60-120 s counting time). CuO nanoparticles investigated using a transmission electron microscope (TEM), model JEM2100, manufactured by Jeol.s.b (Japan). Fourier transform infrared (FT-IR) spectra revealed the presence of functional groups (KBr pellet technique on a Perkin Elmer 1600 FTIR Spectrophotometer in wave number range 400-4000 cm − 1 ). The all characterization was performed at 20 o C.

Sorption Studies
The sorption of 60 Co (II) and 152+154 Eu (III) onto CuO Nps and PAACMA/CuO nanocomposite was studied. Reaction parameters such as pH (1-7), contact time (5 min − 48 h), metal ion concentration (50-300 mg L − 1 ) and ionic strength   were investigated in order to achieve optimal sorption conditions. After contacting 0.1 g of the sorbent with 10 mL of the 60 Co (II) and 152+154 Eu (III) solutions, samples were filtered and separated from the solution. The sorption efficiency of 60 Co (II) and 152+154 Eu (III) radionuclides was calculated using Eq. (1): The sorbed amount q (mg g − 1 ) was calculated using Eq. (2).
Where A o and A e represent the initial and equilibrium concentrations of the radionuclides 60 Co (II) and 152+154 Eu (III), m represents the mass of the nanocomposite (g), and V represents the volume of solution (L). Equation (3) was used to calculate the distribution coefficient K d (mL g − 1 ).

Kinetic Modelling
The pseudo first order, pseudo second order, and Elovich models were used to propose a mechanism for the sorption (1) Where q e and q t are the sorbed amounts of radionuclides (mg g − 1 ) at equilibrium time and at any time t, respectively; k 1 (min − 1 ) is the pesudo first rate constant, k 2 (g mg − 1 min − 1 ) is the pseudo second order rate constant, α, β are the Elovich constants. α (mg g − 1 min − 1 ) represents the rate of chemisorptions at zero coverage, whereas β (g mg − 1 ) represents the extent of surface coverage and chemisorption activation energy.

Adsorption Isotherm Modelling
Langmuir, Freundlich, Dubinin-Radushkevich, and Temkin isotherms were used in this work. Table 3 depicts the linear and non-linear adsorption isotherm modelling forms.

Thermodynamic Parameters
The thermodynamic parameters such as standard Gibbs free energy (∆G o ), enthalpy (∆H o ), and entropy (∆S o ) were used to determine the spontaneity, nature, and adsorbent suitability of the adsorption process [41]. Equations (20,21,22) were used to calculate thermodynamic parameters using temperature-dependent adsorption isotherms.
where K d is the distribution coefficient, mL g − 1 ; R represents the general gas constant (8.314 JK − 1 mol − 1 ), T is the absolute temperature (K). ∆H o and ∆S o are obtained from the slope and intercept of the ln K d against 1/T graph, respectively.

Desorption Studies
The 60 Co (II) and 152+154 Eu (III) solutions were replaced with 10 mL of 0.1 M desorbing agents, including FeCl 3 , AlCl 3 , EDTA, HCl, and NaOH, following the sorption experiments. The concentrations of 60 Co (II) and 152+154 Eu (III) were then determined as previously mentioned, and the desorption efficiency was calculated using Eq. (23). This was followed by 24 h of shaking.

Error Functions
The suitability of a model equation for experimental results was typically evaluated using an error function. The difference between theoretically predicted and actual experimental data values was computed by error functions. It is possible to examine error functions using quantitative or qualitative criteria [42]. It is frequently preferable to use both qualitative and quantitative criteria. The coefficient of determination (R 2 ) [29] and corrected Information about Akaike (AIC c ) [30] error functions were used for quantitative criteria, while residual error plots were used for qualitative evaluation of the kinetic and adsorption isotherm modelling.
Where q exp (mg g -1 ) is the number of sorbed radionuclides obtained from Eq. (2), q calc (mg g -1 ) is the number of sorbed radionuclides obtained from the model, n is the number of experimental data points, and p is the number of modelling parameters. The model with the highest R 2 and the lowest value of AIK C was the best fit.

Zero Point Charge
The pH of the zero point charge (pH ZPC ) used as a base point for determining the type of sorbent because the surface charge is zero at a certain pH level. The sorbent surface charge is positive before the pH ZPC , indicating that it works as an anionic exchanger, and negative after pH ZPC , indicating that it works as a cationic exchanger. The efficiency of the sorbents was determined by the value pH ZPC over a wide pH range. The zero point charge was determined by mixing 0.1 g of P 4 AACMA/CuO nanocomposite at 20 o C with 10 mL of 0.1 M NaCl and shaking the solution for 24 h at 20 o C in pH intervals ranging from 1 to 11. Finally, after shaking, the pH was measured, and the zero point charge was calculated by graphing the initial pH against the pH difference (pH f -pH i ). The plot intersected the x-axis (pH i ) at the zero point charge [43]. According to Fig. 3, the pH ZPC was 2.9, implying that the P 4 AACMA/CuO nanocomposite can be AIC c = (n ln (SER∕n)) + (2(p + 1)) + (2(p + 1)(p + 2)∕n − p − 2)

FT-IR Analysis
FT-IR spectrum of biosynthesized nano CuO are represented in Fig. 4. A small broad peak was observed at 3480 cm − 1 assigned to the O-H group stretching vibration for hydrogen bonding of physically adsorbed water or moisture content [44]. Furthermore, the band was observed at 1630 cm − 1 assigned to the bending vibration of O-H group combined with copper atoms [45]. In the lower wavenumber region (< 600 cm − 1 ), two peaks are shown in spectrum. These are the characteristics peaks of Cu-O bond vibrations, confirming the synthesis of CuO nanoparticles [46]. The spectrum of the P 4 AACMA/CuO nanocomposite at 20 o C had a broad band at 3421 cm − 1 , which corresponds to OH stretching for the COOH group. The band at 2927 cm − 1 represented C-H asymmetric vibration, while the band at 1736 cm − 1 represented the C=O group. The 1457 cm − 1 band represented the deformation of C-H bending vibration [47]. The C-O group is represented by the band at 1249 cm − 1 . The presence of CuO in the polymeric matrix was confirmed by the bands at 1106, 876, 507, and 469 cm − 1 [46]. Figure 5 shows the TEM micrographs of CuO NPs to investigate the nano character of CuO particles. The crystalline nanoparticles were well dispersed and had a size of less than 50 nm with spherical and porous structure. The SEM micrograph of CuO NPs clearly showed rough agglomeration of nanostructural homogeneities with spherical morphologies of CuO nanoparticles. The SEM micrograph of P 4 AACMA/CuO nanocomposite show variation in morphological features and appeared rough and entangled structure and agglomeration with intergranular micropores and spherical morphologies of CuO nanoparticles are distributed randomly between the polymeric matrix. Incorporation of CuO Nps into the polymeric matrix caused cavities and roughness of the P 4 AACMA/CuO nanocomposite resulting in a heterogeneous framework of the synthesised nanocomposite [23].

Optimization of the Sorption Parameters
Effect of pH Figure 6a showed the results of an investigation into how pH affects the sorption efficiencies of the P 4 AACMA/CuO nanocomposite towards the 60 Co (II) and 152+154 Eu (III  Fig. 6b, showed that a significant precipitated quantity of Co (II) began to appear after pH 4.5 and of Eu (III) after pH 4. Figure 6c and d depicted the speciation diagrams of Co (II) and Eu (III) at various pH values as determined by the Hydra/Medusa chemical equilibrium software [49]. Co (II) is the most dominant species in the charts up to pH 4.5, then Co (OH) 2 species appears after pH 4.5 and becomes dominant at pH 6. The trivalent species   [50]. Figure 7 depicted the effect of contact time on the sorption of Co (II) and Eu (III) onto P 4 AACMA/CuO nanocomposite from 5 min to 48 h. The equilibrium state was appointed after contacting time 24 h, as the results indicated no further change in the sorbed amounts for both elements. The sorbed amounts of the two studied elements increased substantially because the number of available active sites on the surface of P 4 AACMA/CuO nanocomposite was initially large enough to overcome the resistance to transfer of Co (II) and Eu (III) from aqueous phase to P 4 AACMA/CuO nanocomposite surface [50]. The increase in sorbed amount slowed gradually from 30 min to the saturation state at 24 h as an equilibrium time. This is due to a decrease in the number of active  1 3 sites of the caused by metal ion occupancy, so there were no more available active sites on the P 4 AACMA/CuO nanocomposite surface after the equilibrium time. At the equilibrium state, the sorbed amounts of Co (II) and Eu (III) onto P 4 AACMA/CuO nanocomposite were 5.1505 and 8.705 mg g − 1 , respectively. Figure 8 depicted the amount of metal ion sorbed as a function of initial concentration, which ranges from 50 to 300 mg L − 1 and labelled with the appropriate radioactivity of 60 Co (II) and 152+154 Eu (III). There is a relationship between metal ion concentration and sorbed amount on composite, which means that increasing the concentration of Co (II) and Eu (III) in the solution increased the sorbed amount of metal ions. The driving force of Co (II) and Eu (III) at the surface interface has increased as the number of effective interactions or collisions between initial metal ions and active sites on the surface of the P 4 AACMA/CuO nanocomposite has increased. Because Eu (III) has a higher charge density than Co (II), Eu (III) had higher sorption efficiency than Co (II). The sorbed amount of Co (II) increased from 4.176 to 11.939 mg g − 1 at 300 mg L − 1 , while it increased from 4.55 to 18.16 mg g − 1 over the same initial metal ion concentration range for Eu (III).

Ionic Strength
The impact of ionic strength on the sorption reaction was studied by incorporating 0.1 g of the nanocomposite with 10 mL of the sorbents at pH 4.5 for 60 Co (II) and 3.53 for 152+154 Eu (III) and ranging the concentration of NaCl from 0.02 to 0.2 mol L − 1 . Ionic strength had a significant effect on the sorption reaction of 60 Co (II) and 152+154 Eu (III) ions onto P 4 AACMA/CuO nanocomposite, as shown in Fig. 9.
The sorbed amounts of 60 Co (II) and 152+154 Eu (III) ions decreased from 5.1505 to 8.704 mg g − 1 to 4.06 and 5.99 mg g − 1 , respectively, in the presence of 0.02 mol L − 1 NaCl. The sorbed amounts of the radionuclides 60 Co (II) and 152+154 Eu (III) decreased to 0.442 mg g − 1 and 3.485 mg g − 1 , respectively, at the concentration of 0.2 mol L − 1 NaCl. The competition between Na (I) and 60 Co (II) or 152+154 Eu (III) ions in the solution, as well as the electrostatic stability of 60 Co (II) and 152+154 Eu (III) in the solution by Cl − anions, could be contributed to this trend. These aspects reduced the rate at which these radionuclides diffuse onto the surface of the nanocomposite. This implies that the predicted physical adsorption or ion exchange chemisorption occurred, as well as an outer-sphere interaction between the radionuclides 60 Co (II) or 152+154 Eu (III) and the P 4 AACMA/CuO nanocomposite surface [51,52] existed. Figure 10 depicted the study of the effect of temperature on the sorption reaction over a temperature range of 20 to 50 o C. The sorption of 60 Co (II) and 152+154 Eu (III) radionuclides were affected by temperature, suggesting a chemical mechanism for the reaction [45]. The findings demonstrated that increasing temperature accelerated the rate of the sorption reaction due to an increase in radionuclide kinetic energy, which led to an increase in radionuclide diffusion at the surface of the nanocomposite, thereby enhanced the sorption process. Increased sorption on the surface of the nanocomposite and promoted deprotonation of the active group were additional effects of increased temperature [53].

Kinetic Modelling
The rate and pathways of radionuclide adsorption on the nanocomposite were determined using kinetic modelling. Three kinetic models were used to determine the correct mechanism for the sorption reaction: pseudo first order, pseudo second order, and the Elvoich model. Figure 11 depicted a linear plot examination. In addition to the coefficients of determination (R 2 ) and AIC c values, the more fitted model can be identified by comparing the calculated q t to the experimental q t . The Elvoich model's coefficients and can be used to distinguish between physisorption and chemisorption reactions by comparing their coefficients α and β.
The results in Table 5 showed that the pseudo second order model had good fitting results, such as higher coefficients of determination, lower AIC c values, and consistency with the equilibrium sorbed amount (q texp ). The residual error plots were examined, and the pseudo second order employed the lowest residual error possible, as shown in Fig. 11e, f. This refers to the chemisorption nature of the reaction, which occurs via electrostatic attraction of the 60 Co (II) and 152+154 Eu (III) radionuclides and negatively charged surface of the P 4 AACMA/CuO nanocomposite, which was consistent with the pH ZPC results. Furthermore, the Elvoich model expressed the initial adsorption rate and the desorption constant. The highest and lowest parameter values for 60 Co (II) and 152+154 Eu (III) confirmed the sorption reaction's chemisorption nature.

Isotherm Modelling
The isotherm model was used to determine the interaction of 60 Co (II) and 152+154 Eu (III) with the surface of P 4 AACMA/ CuO nanocomposite. Figure 12 depicted the residual error plots of the investigated models with linear and non-linear regression plots of Langmuir, Freundlich, Temkin, and Dubinin-Radushkevich (D-R) isotherm modelling. The linear and non-linear regression results were listed in Table 6. For both linear and nonlinear regression, the residual error plots had the lowest D-R values. The highest R 2 , in linear regression revealed that the sorption mechanism was regulated by the Langmuir isotherm and D-R model regulated the sorption reaction in non-linear regression. Thus, linear regression indicated that monolayer coverage of Co (II) and Eu (III) causes sorption onto P 4 AACMA/CuO nanocomposites. Chemisorption was responsible for the sorption of Co (II) and Eu (III) ions onto P 4 AACMA/CuO nanocomposites, as E values were greater than 8 kJ mol − 1 in non-linear regression [54]. The D-R mechanism outperformed the Langmuir isotherm because it did not consider a homogeneous surface or constant adsorption potential. The sorption mechanism was controlled by the D-R mechanism in terms of AIC c for both linear and nonlinear regression because D-R fitting had the lowest AIC c values. Non-linear regression was found to be more accurate in determining the best isotherm [55].

Thermodynamic Studies
The plot of lnK d versus 1/T for the sorption of 60 Co (II) and 152+154 Eu (III) onto P 4 AACMA/CuO nanocomposite shown in Fig. 13. Table 7 showed the results of ∆G o , ∆H o and ∆S o . The free energy change ∆G o obtained during the sorption reaction at 293, 303, 313, and 323 K was all negative, indicating that the sorption process was spontaneous and favourable. Furthermore, an increase in negative ∆G o values by increase in temperature indicated a greater driving force for metal ion binding. The presence of a positive value for ∆H o indicated that the sorption process was endothermic. The increased randomness at the 60 Co (II) and 152+154 Eu (III) molecules onto the P 4 AACMA/CuO nanocomposite interface during the sorption process was indicated by a positive value of ∆S o . Figure 14 depicted the results of desorption of 60 Co (II) and 152+154 Eu (III) using a different desorbing reagents. The results indicated that 55.53% and 95.04% of 60 Co (II) and 152+154 Eu (III), respectively were quantitatively desorbed from the loaded P 4 AACMA/CuO nanocomposite with 0.1 mol L − 1 EDTA solution. 0.1 mol L − 1 NaOH had poor desorbing percentage due to the deprotonation of the surface [56]. Hence, 60 Co (II) and 152+154 Eu (III) find it was difficult to be detached from the adsorbent. However, HCl had the ability to cover loaded P 4 AACMA/CuO nanocomposite surface with [H + ] and hence, 60 Co (II) and 152+154 Eu (III) detached easily [44]. However, EDTA had higher desorption efficiency than HCl due to the strong complexation of EDTA. For AlCl 3 and FeCl 3 used as desorbing agents by ion exchange but the difference in ionic size among [H + ], Al(III) and Fe(III) caused the difference in desorption efficiencies. The order of desorbing efficiencies was EDTA > HCl > AlCl 3 > FeCl 3 > NaOH. Table 8 summarized the adsorbent materials [33,38,44,[57][58][59][60][61][62] to that of the P 4 AACMA/CuO nanocomposite for the adsorption of 60 Co (II) and 152+154 Eu (III) radionuclides. As a result, P 4 AACMA/CuO nanocomposite can be considered as a prospective low-cost adsorbent for 60 Co (II) and 152+154 Eu (III) radionuclides from radioactive waste solution.

Conclusion
A nanocomposite of polyacrylic acid/maleic acid with nano copper oxide (PAACMA/CuO) was successfully prepared and well characterized. The prepared PAACMA/CuO nanocomposite was used for sorption of 60 Co (II) and 152+154 Eu (III) radionuclides from aqueous solutions. CuO was synthesised in nano-size less than 50 nm by hydrolysis of its salt in the presence of the fungus Aspergillus terreus and then cross linked with acrylic acid and maleic acid via free radical polymerization. P 4 AACMA/CuO nanocomposite with acrylic acid (80%), maleic acid (8.89%), CuO (8.88%), and 2.23% cross linker (DAM) was chosen for batch testing. The best sorption conditions (pH 4.5 for 60 Co and pH 3.53 for 152+154 Eu, 24 hours equilibrium time at 20 o C) were used. The reaction kinetic was controlled by pseudo second order based on residual plots, (R 2 ), and (AIC c ). Due to R 2 , the sorption reaction mechanism was regulated with D-R model for non-linear regression, and with Langmuir model for linear regression. While the D-R model was used to control the sorption reaction mechanism based on residual error plots and AIC c results for linear and non-linear regression. The P 4 AACMA/CuO nanocomposite had a monolayer adsorption capacity of 11.04 mg g -1 for Co (II) and 21.54 mg g -1 for Eu (III). According to desorption studies, EDTA at 0.1 mol L -1 concentration could recover 55.46% and 95.044% of the sorbed radionuclides 60 Co (II) and 152+154 Eu (III), respectively. Thermodynamically, the sorption process was endothermic in nature and took place spontaneously. Finally, the results indicate that the P 4 AACMA/CuO nanocomposite has great potential to be used as an economic and effective sorbent for preconcentration and recovery of 60 Co (II) and 152+154 Eu (III) from aqueous solutions. It was recommended to use more than one error function as a deciding factor when selecting the best isotherm. For superior advancements in the field of adsorption science, non-linear regression was preferred over linear regression. 1.687 K f (mmol n −1 g −1 .L −n ) 2.802 (mg n −1 g −1 .L −n ) 0.077 (mmol n −1 g −1 .L −n ) 2.681 (mg n −1 g −1 .L −n ) 0.00784 (mmol n −1 g −1 .L −n )