Synthesize of Poly (acrylamide-co-itaconic/TiO2) Nanocomposite for Ce(III) Sorption from Monazite Leachate

In this study, Acrylamide (AAM), Itaconic acid (IA) and nano TiO2 were copolymerized using gamma irradiation with 60Co γ-rays at a dose of 25 KGy to form poly (acrylamide-co-Itaconic acid/TiO2) (P(AAM-co-IA/TiO2)). Different compositions of P(AAM-co-IA/TiO2) nanocomposites are prepared and examined for Ce(III) sorption. The optimum composition is C6P(AAM-co-IA/TiO2); 61.54 AAM: 30.77 IA: 2.56 TiO2: 5.13 DAM with sorption efficiency at 298 K, pH 6 after 60 min is 80% for initial Ce(III) concentration 200 mgL–1. C6P(AAM-co-IA/TiO2) is characterized by different physicochemical techniques. The optimum pH for the sorption process at 298 K is 6 and the equilibrium attained after 60 min. Different kinetics and isothermal models is applied. The monolayer adsorption capacity is 76.04 mg g–1 at 298 K. The sorption reaction follows a pseudo - 2nd - order kinetic mechanism. The change of Gibbs free energy is – 4.78 kJ/mol at 298 K and change in enthalpy is 60.874 kJ/mole, i.e., the process is spontaneous and endothermic.

Among these techniques, ion exchange is the simple and effective technique, but the various ion exchange suffers from some major drawbacks which limits their applicability. As inorganic synthetic ion exchangers are non-reproducible, expensive and are incompetent to treat large volume of waste [13] in comparison to adsorption technique.
Various soils [14], montmorillonite nanoclay [15], HKUST-1 framework [16] and chert rocks [17] were used as sorbents for Ce(III) from aqueous solutions. However, there is a still requirement for an efficient sorbent of low cost, selective, high sorption and desorption rates, better thermal stability and mechanical strength, easily regenerated which is the aim of this study.
Organic polymers as poly acrylic acid, poly malic acid, poly acrylamide and poly itaconic acid are well known for their uniformity and chemical stability. However, these materials have some drawbacks such as non-adequate mechanical strength, radiation stability [13] and flexibility. Introduction of nano inorganic material as metal oxides [18] to organic monomers to develop polymeric-inorganic nanocomposite greatly enhances its mechanical strength, toughness, glass transition temperature, optical and tensile strength, their multifunctionality, selectivity and specificity, etc. [13,[19][20][21]. The adsorption capacity as well as mechanical properties and the durability of single polymers has been improved by copolymerization process [22].
Because of the chemical inertness, non-toxicity, high refractive index, and the excellent surface properties of TiO 2 [23], it could be used as a component in a variety of nanocomposite materials with unique properties. In general, TiO 2 enhance the mechanical strength of polymer composite [24].
Our study aims to prepare a novel nanocomposite for Ce(III) sorption from monazite leachate. Poly(acrylamideco-Itaconic/TiO 2 ) nanocomposite prepared using gamma irradiation with 60 Co γ-rays at a dose of 25 KGy. Characterization of P(AAM-co-IA/TiO 2 performed by using FT-IR, DTA-TGA, SEM, XRD, particle size analysis, TEM and pore size distribution. Optimization of the parameters affecting sorption process like; pH, contact time, metal ion concentration and sorbent weight carried out. The mechanism of the sorption reaction is proposed by applying different kinetic models and isotherm models. Finally, the prepared nanocomposite used as sorbent with optimum parameters for Ce(III) from monazite leachate.

Reagents
All of the reagents utilized in this study were analytical grade and were not purified further. Acrylamide (AM) was supplied by Fuchen Chemical Co., Ltd., Tianjin, China. Ethylene bis-acrylamide (DAM) and itaconic acid (IA) was used as polymeric monomers (Merck, Germany). Cerium(III) chloride heptahydrate (CeCl 3 ⋅7H 2 O) was purchased from Sigma Aldrich.

Sorbent Manufactured
Synthesized of Nano TiO 2 TiO 2 nanoparticles are synthesized by the sol-gel hydrolysis technique of titanium alkoxide [25]. The hydrolyzed product gel is dried at 60 °C/48 h and used for the nanocomposite preparation.
Synthesized of P(AAM-co-IA/TiO 2 ) Nanocomposites To synthesize the P(AAM-co-IA/TiO 2 ) nanocomposites, different molar ratios of AAM and IA were copolymerized with nano TiO 2 as shown in Table 1 in the presence of methylene bisacrylamide (DAM) as a cross-linker.
Acrylamide (AAM) is mixed with Itaconic acid (IA) and TiO 2 nanoparticles in the presence of methylene bisacrylamide (DAM) in 50 ml deoxygenated water. The mixture is stirred for 2 h and ultrasonically treated for 10 min. The details of the monomer compositions taken are given in Table 1. The mixture was subjected to gamma irradiation dose from a 60 Co unit at a dose 25 KGy. The materials were cut into small pieces and soaked in acetone for 2 h to eradicate water and contaminants before being dried in a vacuum oven at 333 K for 24 h and sieved to size (< 300 µm).

Mechanism of Polymerization and Sorption Reaction
Possible mechanism reactions for the co-polymerization of C 6 P(AAM-co-IA/TiO 2 ) nanocomposite in the presence of DAM as cross linker can be predicted as shown in Fig. 1.

Instruments
The morphology of the particles investigated by scanning electron microscope combined with energy-dispersive X-ray spectroscopy and electron backscatter diffraction (SEM, Philips XL 30 ESEM (25-30 keV accelerating voltage, 1-2 mm beam diameter and 60-120 s counting time). The existence functional groups achieved by Fourier transform infrared spectra (FT-IR) (KBr pellet technique on a Perkin Elmer 1600 FTIR Spectrophotometer in wave number range 600-4000 cm −1 ). The thermal stability of the composite determined by DTA-TGA analyses (Shimadzu DT-60,

Sorption Studies
Sorption of Ce(III) onto the highest sorption efficiency C 6 P(AAM-co-IA/TiO 2 ) nanocomposite studied by batch method [26]. 0.05 g of C 6 P(AAM-co-IA/TiO 2 ) nanocomposite is contacted with 20 mL of the Ce(III) solution till sorption equilibrium attained. The optimum conditions for the sorption process maintained by studying the variation of the reaction parameters. i.e., pH (2-7), contact time (15-120 min), initial concentration (50-500 mgL −1 ) and sorbent weight (m). After sorption time; samples were filtered and thus separated from the solution. The Sorption efficiency of Ce(III) ions at each interval of time is given by Eq. (1) [27]. sorbed amount q (mg g −1 ) is calculated using Eq. (2): where C o , C f and C e is the initial, final and equilibrium concentrations of the Ce(III) ions, respectively. m is the mass of the C 6 P(AAM-co-IA/TiO 2 ) (g) and V volume of solution (L for q and ml for K d ).

Kinetic Modeling
Pseudo 1st order, pseudo 2nd order and Elovich model are applied through this work to arrive to a proposal for the mechanism of the sorption reaction.
where q e and q t are the sorbed amounts of Ce (III) ions; (mg g −1 ) at equilibrium time and at any time t, respectively; k 1 (min -1 ) is the pseudo 1st rate constant. The pseudo 2nd order is described by the equation (5) [30].
where k 2 (g mg -1 min -1 ) is the pseudo 2nd order rate constant.
The surface coverage and activation energy are indicated in Elovich equation (6) [31].
where α and β are the constants of Elovich. α (mg g -1 min -1 ) is the rate of chemisorption at zero coverage, whereas β (g mg -1 ) is the extent of surface coverage and chemisorption activation energy.

Isotherm Modeling
Langmuir [32], Freundlich [33] and Temkin isotherm [34] are applied through this work. Langmuir isothermes model applied by Eq. (7): where Q is the monolayer sorption capacity (mg g -1 ), b sorption free energy constant (b α e -ΔG/RT ) and C e is the metal ion concentration at equilibrium. The free energy, ΔG o , was used to quantify the spontaneity of the sorption process. Negative ΔG o values indicate that the sorption process is occurring spontaneously. Using the following Eq. (8), ΔG o may be computed:

Desorption Studies
The cost of the sorbent, sorption efficiency, and desorption ability are used to determine the success of the sorption process. The desorption behavior of C 6 P(AAM-co-IA/ TiO 2 ) was investigated using three different concentrations of HCl, HNO 3 , and acetic acid; 0.002 mol L -1 , 0.2mol L -1 , and 2 mol L -1 at 298 K for 24 h. The mixture was filtered to separate the solid from the liquid phase, and the concentration of Ce(III) was then measured by atomic absorption spectrophotometer. The desorption percent percentage was calculated using Eq. (12): where C aq (mg L -1 ) is the concentration of Ce(III) in the aqueous phase and Cs (mg L -1 ) is the concentration of Ce(III) in the solid-phase.

Zero Point Charge
Zero point charge is defined as the pH pzc at which the charge on the surface is zero. The surface has a positive charge when the pH of the solution is less than pH pzc , and a negative charge when the pH of the solution is more than pH pzc . A small value of pH pzc is considered a sign of a good sorbent since it allows for a wide range of pH in its application for cation sorption. pH pzc of C 6 P(AAM-co-IA/TiO 2 ) nanocomposite was determined practically by modifying pH for a series of 50 ml flasks, each of which contained 0.1 g of sorbent and 10 ml of 0.01 mol L -1 (NaCl), and pH was varied from 1.0 to 12. (pH initial ). After shaking the mixture for 24 h, the pH of the solutions was determined (pH final ). The pH pzc is then calculated by graphing pH initial against ∆pH (pH final -pH initial ).
As shown in Fig. 2, the pH pzc of C 6 P(AAM-co-IA/ TiO 2 ) nanocomposite is 3.2. Cations sorption onto C 6 P(AAM-co-IA/TiO 2 ) nanocomposite requires a pH greater than 3.2. At pH greater than 3.2, the carboxylic groups deprotonate, allowing negatively charged carboxylate ligands (-COO -) to bind Ce (III) ions. This suggests an ion exchange mechanism between negatively charged nanocomposite and positively charged nanocomposites.

Measurements of Particle Size
The particle size of nano TiO 2 particles are distributed in the range from 39 to 412 nm in Fig. 3a. More than 90% of TiO 2 particles have nanocharacter. The incorporation of nanoparticles into a polymer can lead to a considerable improvement of mechanical properties [35]. However, the particles size of the composite increased in the range between 220 and 340 nm in Fig. 3b due to agglomeration of TiO 2 nanoparticles and particle growth in the nanocomposite [36].

SEM and TEM Analysis
SEM of C 6 P(AAM-co-IA/TiO 2 ) nanocomposite shown in Fig. 4a clarified the rough surface of the nanocomposite. This is due to the incorporation of the agglomerated TiO 2 nanoparticles at the surface of the nanocomposite. The agglomeration of TiO 2 nanoparticles is depicted in the TEM in Fig. 4b where the particle size of the nanoparticles is smaller than 50 nm. This result seems to be less than that obtained by particle size measurements due to agglomeration of the particles [37]. The agglomeration of TiO 2 increases at the surface of the polymers leading to an increase in the particle size and this result confirmed by particle size measurements of C 6 P(AAM-co-IA/TiO 2 ) nanocomposite (Fig. 4c).

X-ray Diffraction
The amorphous nature of the nanocomposite is depicted from Fig. 5 [38]. The amorphous character is due to the huge amounts of water content C 6 P(AAM-co-IA/TiO 2 ) nanocomposite as a result of -COOH presence from Itaconic acid. broad band from 3000 to 3600 cm -1 referred to O-H stretching vibration band overlapping with N-H bending [39].

FT-IR Analysis
The absorption bands at 2934, 1608 and 1412 cm -1 assigned to -CH 2 stretching band, O-H and -COO symmetric vibration band, respectively. The stretching vibration of carbonyl group -C=O represented by the absorption band at 1666 cm -1 .
The amide group at C 6 P(AAM-co-IA/TiO 2 ) nanocomposite is identified by the vibration stretching band C-N at 1450 cm -1 and 1191 cm -1 for -NH 2 bending vibration band [40]. The interaction between TiO 2 Nanoparticles and AAM, IA is confirmed by the Ti-O-C deformation structure at 1120 cm -1 absorption band [41]. The bands at 775 cm -1 and 524 cm -1 was as a result of the Ti-O bond stretching mode of the TiO 2 [40].  However, after sorption of Ce 3+ onto C 6 P(AAM-co-IA/ TiO 2 ) nanocomposite Fig. 6c, The intensity of all characteristic functional groups peaks confirming the prediction of sorption mechanism performance by ion exchange as in Eq. 13 and/or by electrostatic attraction as in Eqs. 14, 15.  Fig. 6e shows the vibration bands at corresponding to TiO 2 NPs nanoparticles, A broad peak observed at 460 cm −1 owing to the vibration of the Ti-O bond. The band at 3397 cm -1 suggest the presence of OH group due to hygroscopic water and structure H 2 O.

Thermal Analysis
The thermal stability of the prepared nanocomposite indicated in Fig. 7. A total 66% of the total weight of the nanocomposite lost up to 600 °C. Two endothermic peaks at 96.38 °C and 233.4 °C with weight loss percentage 6.9% due to evaporation of physically adsorbed water and structural water, respectively. Three exothermic peaks at 409.8 °C, 459 °C and 524 °C due to degradation of C 6 P(AAM-co-IA/ TiO 2 ) nanocomposite and combustion of organic materials.

Surface Measurements
The porous material reveals its efficiency for sorption process. However, only open pores take a part in sorption process as active sites. The difference between apparent density and bulk density express the extent of open pores in the sample. C 6 P(AAM-co-IA/TiO 2 ) nanocomposite has ~ 27% porosity as shown in Table 2. The average pore diameter is 88 nm indicate macropores structure expecting an increase in sorption and desorption efficiency.

Sorption Study
The sorption efficiency (%) and distribution coefficients of TiO 2 NPs, P(AAM-co-IA), and P(AAM-co-IA/TiO 2 ) nanocomposites towards Ce(III) are given in Table 3. The order of sorption efficiency of the samples was P(AAM-co-IA/ TiO 2 ) > P (AAM-co-IA) > TiO 2 NPs. Sorption efficiency of Ce 3+ onto nanocomposite enhanced by TiO 2 NPs This due to doping of Ce 3+ to TiO 2 NPs crystal lattice leads to formation of coordinate band between lone pair of the Ti-O and Ce 3+ cations. As a result for charge balance, a negative charged surface is formed due to the electron trap and a net result increase in the electrostatic attraction of cations [42]. It is observed that sorption efficiencies (%) and distribution coefficient of C 6 P(AAM-co-IA/TiO 2 ) composition show high sorption efficiency compared with the other compositions of the prepared samples. Thus, sample C 6 P(AAM-Co-IA/TiO 2 ) selected for the aim of the study.

Effect of pH
Hydrogen ion concentration considers as an important parameter effecting the sorption reaction. In Fig. 8a, the influence of pH on Ce(III) sorption onto C 6 P(AAM-co-IA/TiO 2 ) nanocomposite is investigated in the range 2-7. It is indicated that the amount sorbed of Ce(III) is increased by increasing pH levels. When the pH is more than 6, the sorption efficiency increases from 80.11 to 85% but Ce(III) precipitate, making it impossible to distinguish between the amount of Ce(III) sorbed onto the nanocomposite and the precipitated amount [43]. Therefore, the optimum pH value was maintained at pH = 6. As value of pH is less than 6, the hydronium ion [H 3 O] + compete Ce(III) for occupying the active sites on C 6 P(AAM-co-IA/TiO 2 ) nanocomposite surface and so the sorption of Ce(III) is decreased. Increasing pH value,  , led to a decrease in the competition and so the sorption of Ce(III) onto the C 6 (PAAM-co-IA)/TiO 2 nanocomposite is increased. Figure 8b shows the Ce(III) speciation diagram in aqueous solution at various pH levels. It demonstrates that Ce(III) ions are provided at the optimal pH of 6, indicating that Ce(III) ions are trivalent sorbed. Hydroxides began to form at pH levels greater than 6 [44].
The distribution coefficient of Ce(III) at 298 K onto C6P(AAM-co-IA/TiO 2 ) (Fig. 8c) increases as the pH increase at V/m ratio 400. This is due to the increase of the electrostatic attraction between the cerium ions and the surface of the composite.

Impact of Contact Time
The impact of contact time on sorption process studied at range (10-240 min) and represented in Fig. 9. The sorbed amount increases gradually till the equilibrium time of the sorption process which reached attained nearly at 60 min. The high sorption efficiency at the initial stage of the process owing to the great number of vacant active sites on the

Effect of Sorbent Weight
Effect of C 6 P(AAM-co-IA/TiO 2 ) nanocomposite dose was studied in the range (0.01-0.1 g) and represented in Fig. 10. The sorbed amount of Ce(III) onto C 6 P(AAM-co-IA/TiO 2 ) nanocomposite found to increase from 35.58 to 71.84 mg g -1 by increasing the weight of C 6 P(AAM-co-IA/ TiO 2 ) nanocomposite from 0.01 to 0.07 g at an initial concentration of Ce(III) 200 mg L -1 . This is due to the fact that the sorption capacity influenced by surface activity. The increase in the amount of C 6 P(AAM-co-IA/TiO 2 ) nanocomposite weight will increase specific surface area which increases the number of sorption sites available for Ce(III) surface interactions as well as increase in diffusion path length [45,46]. Any increase after 0.07 weight of C 6 P(AAM-co-IA/TiO 2 ) nanocomposite, the sorption process become steady and no further significant increase in sorption efficiency was observed due to keeping constant the Ce(III) [45].

Effect of Metal Ion Concentration and Temperature
The sorption reaction is influenced by Ce (III) concentration. A series of concentration 50-500 mg L -1 of Ce(III) were studied and depicted in Fig. 11a. Even the sorbed amount increases, the sorption efficiency of C 6 P(AAM-co-IA/TiO 2 ) nanocomposite decreases in percentage from 92.07 to 35.5% with raising original Ce (III) ion concentration from 50 to 500 mg L -1 . This is owing to the active sites on the sorbent becoming available at low Ce(III) concentration. If the concentration of Ce(III) increase, C 6 P(AAM-co-IA/TiO 2 ) nanocomposite has a fixed number of sorption sites and so inability to adsorb more Ce(III) [46,47].
From the results shown in Fig. 11b for the sorbed amount of Ce(III) onto C 6 P(AAM-co-IA/TiO 2 ) nanocomposite at different temperatures at 298, 308, and 318 K, it is obvious that the sorbed amount increases by raising the temperature due to acceleration of some originally slow sorption steps or due to the enhanced mobility of Ce(III) ions from the solution to the functionalized C 6 P(AAM-co-IA/TiO 2 ) surface [48]. Figure 12a, b shows the pseudo 1st order and pseudo 2nd order fitting plots. Table 4 contains the kinetic parameters. The identity value of q e (cal.) with the value of the experimental data q e (exp.) and the high R 2 for pseudo 2nd order for Ce(III) elucidate that the sorption of Ce(III) onto C 6 P(AAM-co-IA/TiO 2 ) nanocomposite controlled by pseudo 2nd order mechanism. The pseudo 2nd order reaction mechanism of C 6 P(AAM-co-IA/TiO 2 ) nanocomposite are synchronized with chemisorption reaction and valence electrons sharing or ion exchange between Ce (III) and H + [49,50]. Figure 12c shows the interpretation of Elvoich Eq. (6). The linear relation with correlation coefficient R 2 = 0.96 accumulates for the agreement of the reaction mechanism with Elvoich and a good correlation for C 6 P(AAM-co-IA/ TiO 2 ) heterogeneous surface [51]. α and β parameters listed in Table 4.  Figure 13a shows the linear plot of C e /q e versus C e illustrating the sorption process fitted with Langmuir model with high correlation coefficient, R 2 = 0.99. The values of the monolayer capacity (Q) at different temperatures were estimated from the slope and represented in Table 5. The sorption capacity of Ce(III) at 298 K onto C 6 P(AAM-co-IA/ TiO 2 ) nanocomposite is 76.04 mgg -1 . The sorption capacity increased with the temperature. The process is favorable because 0 < R L < 1. By graphing log qe versus log Ce, (Fig. 13b), straight lines were produced at different temperatures. The values of Freundlich constants, 1/n and k, are determined from the slope and intercept, respectively, and given in Table 5.

Isotherm Modeling
The numerical of n > 1 suggested that C 6 P(AAM-co-IA/ TiO 2 ) bind with a highest strength multiple binding sites of sorbent and the sorption capacities were only slightly inhibited in relative low equilibrium concentration. The  Table 4 Calculated parameters of the studied kinetic models for sorption of Ce(III) onto C 6 P(AAM-co-IA/TiO 2 ) nanocomposite at pH = 6, v/m = 0.4 L g -1 and 298 K Pseudo 1st order kinetic parameters q e(exp) (mg g -1 ) Pseudo 2nd order kinetic parameters Elvoich kinetic parameters k 1 (min -1 ) q e (cal.) (mg g -1 ) The constants of A T and b T for Temkin fitting determined from the slope and intercept of the plot of q e against ln C e in Fig. 13c and represented in Table 5. These constants correlated to the sorption capacity and intensity of sorption. R 2 , correlation coefficient value is close to unity indicating the sorption mechanism which is governed by chemisorption process confirming pseudo 2nd order and Elvoich model.

Thermodynamic Studies
The slope and intercept of the plot of Fig. 14, according to Eqs. (8,9), can be used to derive the values of ΔH° and ΔS°, respectively, represented in Table 6. The endothermic character of the sorption process is indicated by the positive value of ΔH°, and the increase in randomness at the     nanocomposite/solution interface is indicated by the positive value of ΔS°. The negative value ΔG° indicates the sorption process is spontaneous. The increase in negative Gibbs free energy with increasing temperature indicates that the process is becoming more spontaneous. Furthermore, positive values of ΔS° suggest that Ce (III) exchanges with mobile ions exist on C 6 P(AAM-co-IA/TiO 2 ) nanocomposite, resulting in an increase in entropy value via the sorption process. Figure 15 represents the variation of accessible desorption efficiency with the different concentration of acids. The percentage of desorption increased as the concentration of the acids increased. The order of desorption efficiency is HCl > HNO 3 > acetic acid and 2 mol L -1 HCl is the most prober fluent for Ce(III) with 70.7% desorption efficiency.

Sorption of Ce(III) from Monazite Leachate
Sorption of Ce(III) and some rare earth ions (RE 3+ ) onto C 6 P (AAM-co-IA/TiO 2 ) nanocomposite is measured using inductive coupled plasma optical emission spectrometer. 0.14 g of C 6 P(AAM-co-IA/TiO 2 ) contacting with 40 mL of the monazite leachate solution at 298 K and pH 6. The results for energy dispersive X-ray spectra of loaded C 6 P(AAM-co-IA/ TiO 2 ) is shown in Fig. 16. The spectrum shows La, Ce, Eu… bands besides C, O, N, and Na consistent with the elemental formula of monazite [57] and nanocomposite. The roughness of the surface of C 6 P(AAM-co-IA/TiO 2 ) at the end of the sorption processes as depicted in Fig. 16. Furthermore, the mapping images of loaded C 6 P(AAM-co-IA/ TiO 2 ) nanocomposite with REEs indicate that REEs ions are adequately adsorbed at the surface of the nanocomposite and they are distributed uniformly. La, Ce and Eu are taken as examples of REEs to confirm sorption process. Table 8 includes the sorption efficiency and desorption percentage of light rare earth ions (LRE 3+ ) and heavy rare earth ions (HRE 3+ ) onto C 6 P(AAM-co-IA/TiO 2 ) nanocomposite. The results show a sorption selectivity for C 6 P(AAM-co-IA/ TiO 2 ) nanocomposite towards HRE 3+ where the sorption efficiency is 70.94% compared to 54.09% for LRE 3+ . Thus, C 6 P(AAM-co-IA/TiO 2 ) nanocomposite could be used for  for Ce(III) decreased in single component system than in multicomponent system in case of monazite leachate solution these is due to selectivity of C 6 P(AAM-co-IA/TiO 2 ) nanocomposite towards HRE 3+ possessing low ionic radii [58].

Conclusions
Poly(acrylamide-co-Itaconic acid/TiO 2 ) (P(AAM-co-IA/ TiO 2 )) nanocomposite with composition 61.54 AAM: 30.77 IA: 2.56 TiO 2 : 5.13 DAM at 298 K, pH 6 could be used as a sorbent for Ce(III) with sorption efficiency 80% after 60 min and initial Ce(III) concentration 200 mg L -1 . The sorption process has endothermic nature; the results indicated that, the sorption reaction is regulated by pseudo-2nd order mechanism and Langmuir isotherm. The monolayer capacity of Ce (III) onto C 6 P(AAM-co-IA/TiO 2 )) at 298 K, pH = 6 is 76.04 mg g -1 . Using C 6 P(AAM-co-IA/TiO 2 ) nanocomposite as a sorbent for Ce(III) in multicomponent system of monazite leachate shows sorption efficiency 61.62% for initial concentration is 577.652 mg L -1 . Therefore, the prepared C 6 P(AAM-co-IA/TiO 2 ) nanocomposite can be considered as a promising material for the sorption of Ce(III).
Author Contributions GD, RMM, EES and KA contributed to the study conception and design, Material preparation, data collection and analysis. All authors read and approved the final manuscript.

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