All chemicals were analytical grade, purchased and used as received without further purification: Potassium Permanganate KMnO₄; Sigma-Aldrich, Manganese Chloride MnCl₂∙4H₂O; Merk, Activated Carbon (AC) commercial-grade provided by El-Gomhoria company for trade service (Cairo), ⁹⁹Tc radionuclide (activity 257.4 CPM/ml) was extracted from residual ^99mTc columns from the technetium generator used in nuclear medicine centers, Ultima Gold^TM (AB LSC-cocktail) from Packard bioscience company, concentrated acids of A.R HNO₃, HCl and NaOH were used throughout the investigations as required and freshly bi-distilled water was used through all experiments.

A variety of sorbents were prepared for T 99 cO 4 − removal from the aqueous waste. Sorbent material includes 1) Nanosized manganese oxide (NMO) by co-precipitation method, at which the prepared 0.2 M KMnO₄ stirred with a magnetic stirrer, the pH was adjusted between pH 8 - 9 using 2 M NaOH then dropwise 0.3 M MnCl₂. The suspension is stirred for 60 min then the precipitate is left overnight to settle. The solution is decanted to the extent possible, and the remaining suspension is centrifuged. The sample washed with bi-distilled water, dried under vacuum for two days and finally heated at 90˚C till constant weight [21]. 2) Activated carbon (AC) was soaked overnight in three different HNO₃ concentrations (4 M, 6 M and 8 M) followed by heating at 80˚C - 90˚C for 6 hours with refluxing. The treated samples washed with bi-distilled water. The treated AC samples were dried under vacuum for two days and finally, heated at 900˚C till constant weight, grinding and homogenized. 3) Mix the sorbents to evaluate the synergistic effects of modified activated carbon and NMO.

­ The first composite prepared by mixed sorbent between NMO and modified activated carbon with 4 M HNO₃ with ratio (1:1) code (NMO/4 M AC).

­ The second mixed sorbent between NMO and modified activated carbon with 6 M HNO₃ with ratio (1:1) code (NMO/6 M AC).

­ The third mixed sorbent between NMO and modified activated carbon with 8 M HNO₃ with ratio (1:1) code (NMO/8 M AC).

These mixed sorbents were studied because of their low cost and expected high capacity to adsorb T 99 cO 4 − from low-level radioactive liquid waste.

The batch experiments were performed by 0.05 gm of sorbent which added to 5 ml of radioactive waste solutions into a polypropylene centrifuge tube. The suspensions were placed on a slow-moving shaker rotates at 200 rpm for 2 hours. Each suspension was passed through a 0.45 µm cellulose membrane filter with a diameter (25 mm). The effect of initial pH, contact time, initial concentration of adsorbate (⁹⁹Tc), ionic strength and temperature were investigated. The pH of the solution adjusted at the desired value by adding 0.1 M NaOH or HCl. The radionuclide concentrations of the filtrates were analyzed by a liquid scintillation counter (LSC) where 5 ml of the filtrate was added to 5 ml Packard Ultima Gold^TM AB LSC-cocktail for effective beta discrimination LSC, for measuring the activity the LSC model Packard TRI CARB 2770 was used. The adsorption capacity of ⁹⁹Tc q_t (CPM/g) calculated by Equation (1).

Where: C₀ (CPM/L) is the initial concentration of ⁹⁹Tc, C_t (CPM/L) is the concentration of ⁹⁹Tc at time t, V (L) is the volume of ⁹⁹Tc solution, and m (g) the mass of sorbent.

q t = ( C 0 − C t ) × V m (1)

The percent uptake or the removal efficiency (R%) was calculated by Equation (2).

R % = C 0 − C t C 0 × 100 (2)

The equilibrium adsorption capacity of adsorbent, q_e (CPM/g) can be determined by Equation (3).

q e = ( C 0 − C e ) × V m (3)

where: C_e (CPM/g) is the ⁹⁹Tc concentration at equilibrium in the supernatant after separation of the adsorbent and V, m, and C₀ have the same meaning as in Equations (1) & (2) [22].

­ X-Ray diffraction

X-ray diffraction (XRD) analysis was employed to study the phase composition of the synthesized composites, using a diffractometer (Bruker; D8 advance) with monochromator Cu-Kα target wavelength 1.54178 , 40 kV, and 40 mA Germany.

Figure 2 shows the XRD patterns of the produced NMO, NMO/(4 M, 6 M, 8 M) AC and AC. Figure 2(a) shows a broad diffraction pattern for NMO, which characteristic of pyrolusite tetragonal phase of β-MnO₂ at 2θ = 28.877 and 2θ = 37.984 indexed to (JCPDS 01-0799) [23] and hausmannite tetragonal phase of Mn₃O₄ at 2θ = 24.907 and 2θ = 26.464 related to (JCPDS 75-1560) [24] [25] meanwhile Figure 2(b) shows NMO/(4M AC) which fitted to pyrolusite tetragonal phase of β-MnO₂ at 2θ = 26.531 corresponding to (JCPDS 01-0799), hausmannite phase Mn₃O₄ at 2θ = 22.485, 2θ = 25.209 indexed to (JCPDS 75-1560) and carbon at 2θ = 37.113, 2θ = 28.632 related to (JCPDS 26-1077) [26] Figure 2(c) employed of NMO/(6M AC) the tetragonal crystalline phase pyrolusite β-MnO₂ at 2θ = 28.875 corresponding to (JCPDS 01-0799), monoclinic manganese oxide Mn₅O₈ at 2θ = 18.212, 2θ = 56.659 indexed to (JCPDS 39-1218) [27] and carbon at 2θ = 37.514 related to (JCPDS 46-0944) [28]. Figure 2(d) apply NMO/(8 M AC) presence of a diffraction peaks of pyrolusite tetragonal phase of β-MnO₂ at 2θ = 29.11 corresponding to (JCPDS 01-0799), manganese oxide monoclinic phase Mn₅O₈ at 2θ = 17.824, 2θ = 58.064 indexed to (JCPDS 39-1218), Ramsdellite orthorhombic phase γ-MnO₂ at 2θ = 22.253 (JCPDS 44-0142) [29] [30] and carbon at 2θ = 37.594 related to (JCPDS 26-1076) [31]. It was obvious that sharp diffraction beaks for carbon at 2θ = 26.726 indexed to (JCPDS 26-1077) in their diffraction patterns as depicted in Figure 2(e). The subsequent phase transition into different valences of manganese oxide possibly owing to the oxidative atmosphere used at the beginning of the synthesis provides a pathway to oxidize some Mn²⁺ present in Mn(OH)₂ to Mn³⁺ and Mn⁴⁺ during the drying step, the reducing reaction with these carbon matrix or the acidic treatment of carbon, then it seems that a partial amount of Mn³⁺ can be oxidized leading to Mn₅O₈ monoclinic phase, which stabilizes the divalent Mn ions inherited from Mn₃O₄. Digestion time and acid concentration could explain this discrepancy [25] [32]. The calculated average crystallite size of the prepared NMO, NMO/(4 M AC), NMO/(6 M AC), NMO/(8 M AC) and AC are 11.6 nm, 16.9 nm, 9.6 nm, 14.3 nm and 21.4 nm respectively which calculated by Dedye-Scherer Equation (4) [33].

D = 0.9 λ β cos θ B (4)

where, λ (nm) is the X-ray radiation wavelength, β is the diffraction peak full width at half maximum (FWHM), and θ_B is the Bragg diffraction angle.

­ FT-IR analysis

Fourier Transform Infra-Red spectroscopy (FTIR) model (BRUKER; VERTEX 70v) was used at room temperature in Egyptian Nuclear and Radiological Regulatory Authority for obtaining information about the functional groups in the structure. The FTIR spectra of samples NMO, NMO/(4M AC), NMO/(6M AC), NMO/(8M AC) and AC are depicted in Figure 3 and the bands illustrated as follows. In 400 - 4000 cm⁻¹, the bands at 414 - 592 cm⁻¹ should be ascribed to the Mn−O vibrations, and the bands at 750 - 1640 cm⁻¹ are usually attributed to the –OH bending vibration with Mn atoms [34] [35],meanwhile, bands can be observed at 3400 - 3678 cm⁻¹ which attributed to the O−H stretching vibration [36] [37]. The bands 1500 - 1900 cm⁻¹ due to C = O stretching [37] [38],where the bands at 2846, 2912 cm⁻¹ correspond to C–H symmetric and asymmetric respectively [37] [39]. It was found that bands at 3700 - 3899 cm⁻¹

attributed to hydrogen bonds (H₂O…H…H₂O)⁺, which were formed between water and protons of acidic groups [40]. Finally, the wave number at bond 2356 cm⁻¹ may be due to forming a new functional group NC = O which can be turned into an electron structure [39].

The Scanning Electron Microscope (SEM) with a microscope (JEOL JSM-6510LA) was used to study the surface morphology and the particle diameter of NMO, NMO/(4 M AC), NMO/(6 M AC),NMO/(8 M AC) and AC investigated by field emission Figure 4 indicate the different morphology between the used adsorbents. Figure 4(a) showed that NMO is foamy, spongy and agglomerated. The size of agglomerates is about 50 µm. Figure 4(b) show NMO/(4 M AC) like sea wave with void or pores and the agglomerates is 50 µm. Figure 4(c) illustrate the morphology of NMO/(6 M AC) like aquatic plant, a narrow holes in wall with aggregates 50 µm. Figure 4(d) for the composite NMO/(8 M AC) is composed of small single spheres, bulk agglomerates of sphere with average size 50 µm. Figure 4(e) the SEM micrograph showed that the obtained nanoparticle has a flower, mushrooms and agglomerated, with an average size of agglomerates about 50 µm.

­ Effect of solution pH

The pH of the solution is an important parameter that controlling the surface charge of the adsorbent and it has a significant change in the behavior of TcO 4 − ions. HNO₃ or HCl and NaOH were used to adjust the pH and reduction of Tc is favored at low pH and alkaline media oxidizes [41]. The results of the adsorbed pertechnetate TcO 4 − ion in pH range 2.3 to 7.04 shown in Figure 5.

It is observed that the percent uptake for the adsorbents NMO/(4 M, 6 M, 8 M) AC is higher than that of AC and NMO. The optimum pH value in case of using NMO/(4 M, 6 M, 8 M AC) as adsorbents is 2.33 whereas, in case AC alone and NMO are 3.02.

The obtained maximum removal percentages for sorbents (NMO/4 M AC, NMO/6 M AC, NMO/8 M AC, NMO, AC) were 93.57%, 90.3%, 90.3%, 41%, 38.9% respectively.

It was found that the adsorption decreased as the pH increased from 2.33 to 7.04 for all the investigated samples Figure 5. This behavior could be explained by the surface charge of the sorbent at lower pH values covered by protons (H⁺) forming positively charged particles and the pertechnetate T 99 cO 4 − is negative which increases the electrostatic interaction between negative T 99 cO 4 − ions and the positive surface of the sorbents. While, at higher pH value there is a notable decrease in TcO 4 − removal this may be attributed to electrostatic repulsion between T 99 cO 4 − and the negatively charged surface of the sorbents. it claimed that anion exchange sites (AC^{+ −}NO₃) were formed at pH value ~2 in nitrate solutions and at a higher pH value, there was a competition between pertechnetate ion and OH⁻ [12] [42].

­ Effect of contact time

The influence of contact time on the adsorption efficiency of T 99 cO 4 − anions by a prepared composite were studied using 0.05 g of NMO/(4 M, 6 M, 8 M) AC at room temperature and initial activity concentration of 709 CPM/vial (141.8 CPM/ml) for T 99 cO 4 − . The sorption of the investigated isotope T 99 cO 4 − increases with time to reach a saturation level for one-hour prolonged adsorption 24 hours did not a significant change of the equilibrium capacity for any of the investigated sorbents. Figure 6 shows that there was no significant difference between the removal of T 99 cO 4 − by samples NMO/6 M AC and NMO/8 M AC whereas slight difference in the using NMO/4 M AC. Moreover, NMO and AC have lower efficient than the other composites.

The significant increase in the adsorption capacity for the anionic type of adsorbates could be attributed to the interaction of the Nano-manganese oxide loaded into the AC by 4 M, 6 M and 8 M [43]. This variation may be due to the initial large number of vacant sites on the adsorbent surface is available for adsorption and high gradient of solute concentration [44] [45]. The slow rate of adsorption may be due to decreasing in the number of vacant surface sites of adsorbent and remaining vacant surface sites are difficult to be occupied due to repulsive force between the solute molecules on the solid and bulk phases [46].

­ Effect of temperature

The temperature of the reaction has a significant effect on the rate of the adsorption process. The adsorption process was carried out at different temperatures (25˚C, 30˚C, 40˚C and 50˚C) for T 99 cO 4 − ions using 0.05 gm of

adsorbents (NMO/4 M AC, NMO/6 M AC and NMO/8 M AC), T 99 cO 4 − activity concentration 709 CPM/vial (5 ml) with stirring and contact time 60 min. Figure 7 shows that the removal uptake decreased gradually with increasing the temperature of the solution which indicates the process may be exothermic reaction during the adsorption of T 99 cO 4 − .

­ Effect of competing ion concentration

The effect of competing ion concentration on the adsorption of T 99 cO 4 − on NMO/4 M AC, NMO/6 M AC, and NMO/8 M AC was studied by using KCl salt at a different concentration from 5 to 100 ppm. The result depicts in Figure 8 illustrated that the solution ionic strength has a relatively very small effect on the removal percentage of T 99 cO 4 − ions.

­ Effect of initial T 9 9 c O 4 − activity concentration

The adsorption process was carried out at a different initial concentration of T 99 cO 4 − at (102, 200, 368, 763 and 1287 CPM), pH 2.3 for 1 h contact time and at room temperature. From Figure 9 the adsorption capacity increased with increasing the initial activity concentration of pertechnetate ions. The obtained results agree with other investigators Dowlen et al., in 1996 [13]. The increase in the amount of adsorption was according to an increase in the electrostatic interaction between the pertechnetate ions and the adsorbent active sites due to the

fact that more adsorption sites were being covered as the pertechnetate ions concentration increased [47].

An adsorption isotherm is a curve describing the phenomenon governing the retention or mobility of a substance from the aqueous porous media or aquatic environments to a solid-phase at a constant temperature and pH [48] [49]. Adsorption equilibrium (the ratio between the adsorbed amount with the remaining in the solution) is established when an adsorbate containing phase has been contacted with the adsorbent for sufficient time, with its adsorbate concentration in the bulk solution is in a dynamic balance with the interface concentration [50] [51] was determined the adsorption capacity of T 99 cO 4 − onto NMO/4 M AC, NMO/6 M AC and NMO/8 M AC in the light of Langmuir and Freundlich adsorption isotherm models.

­ Langmuir isotherm model

This empirical model assumes monolayer adsorption (the adsorbed layer is one molecule in thickness), adsorption can only occur at a finite (fixed) number of definite localized sites, that are identical and equivalent, with no lateral interaction and steric hindrance between the adsorbed molecules, even on adjacent sites [52]. In its derivation, Langmuir isotherm refers to homogeneous adsorption, in which each molecule possesses constant enthalpies and sorption activation energy (all sites possess an equal affinity for the adsorbate) [53],with no transmigration of the adsorbate in the plane of the surface [54]. Graphically, it is characterized by a plateau, an equilibrium saturation points where once a molecule occupies a site, no further adsorption can take place [49] [55]. The linear form of Langmuir isotherm equation is given as in Equation (5).

C e q e = 1 Q m ⋅ K L + C e Q m (5)

where: C_e (CPM/L) is the equilibrium concentration of the adsorbate, q_e (CPM/g) is the amount of adsorbate adsorbed per unit mass of adsorbent, K_L and Q_m are Langmuir constants and the adsorption capacity in (CPM/g) respectively. C_e/q_e is plotted against C_e, a straight line with slope (1/Q_m) and intercept (1/Q_mK_L) is obtained. The essential characteristics of Langmuir isotherm can be expressed by a dimensionless constant called separation factor or equilibrium parameter, R_L, defined by Weber and Chakkravorti Equation (6) [56].

R L = 1 1 + K L C 0 (6)

Lower in R_L value reflects that adsorption is more favorable. In explanation, R_L value indicates the adsorption nature to be either unfavorable if (R_L > 1), linear (R_L = 1), favorable (0 < R_L < 1) or irreversible (R_L = 0). Table 1 illustrates R_L values near to zero, which indicate irreversible adsorption process.

­ Freundlich isotherm model

Freundlich isotherm model assumes that the adsorption takes place on a heterogeneous surface of the adsorbent and the linearized form of this model can be given by Equation (7) [57] [58].

ln q e = ln K F + ( 1 n ) ln C e (7)

where: K_f is the Freundlich constant (CPM/g) which represents the relative adsorption capacity of the adsorbent. (1/n) is the heterogeneity factor and it is a function of the strength of adsorption in the adsorption process and (n) has various values depending on the heterogeneity of the sorbent. if (n) lies between one and ten, this indicates a favorable sorption process [25]. (1/n) and lnK_f values were calculated from the slope and intercept of the linear plots of lnq_e versus lnC_e which shows Freundlich isotherm as in Figure 10 and Table 1.

The plot of lnq_e versus lnC_e gave a straight line with a slope of (1/n) and intercept of lnK_F (Equation (7)). The slope ranges between 0 and 1 is a measure of adsorption intensity or surface heterogeneity, becoming more heterogeneous as its value gets closer to zero. Whereas, a value below unity implies chemisorption’s process where (1/n) above one is indicative of cooperative adsorption [59].

According to the results presented in Table 1 the calculated correlation coefficients (R²) for Freundlich Model were closer to unity so, this model may be the more appropriate than Langmuir Model. Moreover, the values of (1/n) obtained

from Freundlich Isotherm, equal 1.935, 1.6514 and 1.6513 for NMO/4 M AC, NMO/6 M AC and NMO/8 M AC respectively, (1/n) above unity indicate bi-mechanism and cooperative adsorption [60].

Therefore, T 99 cO 4 − adsorption to NMO/4 M AC, NMO/6 M AC and NMO/8 M AC could be believed to be complex. The adsorption sites were most likely heterogeneous while the adsorption was not limited to be monolayer formation.

To predict the adsorption kinetic model for adsorption T 99 cO 4 − from its radioactive liquid waste onto composites MnO₂/AC (4, 6, 8 M). The kinetics models: pseudo-first and second order models were applied to the experimental data. The best fit model was selected based on the linear regression correlation coefficient (R²), which is a measure of how the predicted values from a forecast model match with the experimental data.

­ Pseudo-first order model

It assumes that the rate of change of the solute uptake with time is directly proportional to the difference in the saturation concentration and the amount of solid uptake with the time, i.e. the rate of occupation sites is directly proportional to the number of unoccupied sites. Probably the earliest known and one of the most widely used kinetic equations so far for the adsorption of a solute from a liquid solution is the Lagergren equation or the pseudo-first order equation [61]. The pseudo-first order kinetics is calculated by Equation (8).

log ( q e − q t ) = log q e − ( K 1 / 2.303 ) t (8)

where: K₁ is the rate constant of pseudo-first-order adsorption (min⁻¹), and q_e and q_t denote the amounts of adsorbed T 99 cO 4 − anions at equilibrium and at time t (Bq∙g⁻¹) respectively. Plot of log ( q e − q t ) versus t should give a straight line to confirm the applicability of the kinetic model, logq_e should be equal to the intercept and K₁ the slope as disputed in Figure 11 and Table 2.

­ Pseudo-second order model

It assumes that the rate of occupation of adsorption sites is proportional to the square of the number of unoccupied sites. Where the rate limiting step may be chemical sorption involving valence forces through sharing or exchange of electrons between TcO 4 − and sorbent [62]. The pseudo-second order equation is applied in the given form Equation (9).

t / q t = 1 / ( k 2 q e 2 ) + ( 1 / q e ) t (9)

where: k₂ (CPM∙g⁻¹∙min⁻¹) is the rate constant of the pseudo-second order adsorption. Additionally, the initial adsorption rate h (CPM∙g⁻¹∙min⁻¹) can be determined using Equation (10) [63].

h = K 2 ⋅ q e 2 (10)

Plot of t/q_t versus t should give a straight line, 1/q_t equal the intercept and 1 / K 2 q e 2 the slope as shown in Figure 12. Table 2 illustrate the value of the

correlation coefficient (R²) is unity comparing with that obtained from the pseudo-first order. Moreover, the value of the calculated equilibrium adsorption capacity q_e(Cal) according to the pseudo-second order model is much closer to the experimentally obtained q_e(exp) on comparing to the calculated from the pseudo-first order model. It could be stated that the adsorption of T 99 cO 4 − onto NMO/4 M AC, NMO/6 M AC and NMO/8 M AC obeyed the pseudo-second order kinetics model.

The concept of thermodynamic assumes that in an isolated system where the energy cannot be gained or lost, the entropy change is the driving force [64].

Van’t hoff Equation (11) was used to calculate the thermodynamic parameters such as change in enthalpy (∆H˚), a change in entropy (∆S˚) and change in Gibbs free energy (∆G˚). Adsorption of T 99 cO 4 − on the investigated materials, at different temperatures was determined by using Equations (12) & (13) and illustrated in Figure 13.

ln K d = Δ S ˚ R − Δ H ˚ R T (11)

where: R (8.314 J/mol K) is the universal gas constant, T (K) the absolute solution temperature and K_d is the equilibrium constant which can be calculated as:

K d = C A e C e (12)

C_Ae (CPM/L) is the activity concentration of T 99 cO 4 − adsorbed on solid at equilibrium and C_e (CPM/L) is the equilibrium concentration of T 99 cO 4 − in the solution. The values of ∆H˚ and ∆S˚ were calculated from the slope and intercept of plot between lnK_d versus 1/T Figure 13. ∆G˚ can be calculated using the Equation (13) [65] [66]:

Δ G ˚   = Δ H ˚   − T Δ S ˚ (13)

The obtained values of thermodynamic parameters, (∆H˚, ∆S˚ and ∆G˚), are presented in Table 3, the negative value of ∆H˚ indicates the exothermic nature of Nanosized MnO₂/AC (4 M, 6 M & 8 M). The negative value of ∆G˚ confirmed the feasibility of the process and the spontaneous nature of the sorption with a high preference for T 99 cO 4 − .