The textural properties of all the samples were determined by nitrogen adsorption experiments at the temperature of liquid nitrogen (77 K) with a Quantachrom Autosorb1. The samples were all first degassed at 150˚C for 6 h under vacuum before the N2 adsorption/desorption tests. The surfaces were calculated by applying the BET equation (Brunauer-Emmet-Teller) to the first part of the isotherms. The total pore volume in each sample was evaluated from the amount of nitrogen adsorbed at the highest relative pressure examined. The results of the

texture study are given in Table 2. Surface micrographs of the samples before and after adsorption were taken using a JSM-840 model scanning electron microscope (SEM) for surface micro-analysis.

The method of Boehm [22] was used to determine the composition of active carbon in an acid or basic surface group. Concentration solutions of 0.1 N of strong bases of NaHCO₃, Na₂CO₃ and NaOH as well as strong acid of HCl were prepared. The number of sites of the various acid functions is calculated by considering that NaHCO₃ neutralizes the carboxylic groups, Na₂CO₃ neutralizes the carboxylic groups and the lactone groups and NaOH neutralizes the carboxylic, lactone and phenolic groups. The number of basic sites is calculated from the amount of HCl which has reacted with carbon.

The pH_ZPC was determined by the pH derivative method according to [23], using 100 mg of activated carbon and 50 mL of 0.01 M NaCl solutions with a pH varying from 2 to 12, pH adjusted by adding a 0.01 M HCl or NaOH solution. The suspensions are kept under constant stirring, at room temperature, for 48 h, in order to determine the final pH. The pH_ZPC is the point where the pH_final = f(pH_initial) curve intercepts the first bisector pH_final = f(pH_initial).

➢ The values of the yields from the production of active carbon are estimated by application of formula (1):

with:q_e and q_m: the adsorption capacities respectively at equilibrium and maximum (mg/g);C_e: residual concentration at equilibrium (mg/L);K_L, K_F, K_FG, K₁: Langmuir, adsorption-adsorbent constants, respectively Freundlich, Fowler-Guggenheim and Kiselev;K_n: Constant of complex formation between adsorbed molecules of Kiselev;W: Interaction energy between adsorbed molecules (kJ·mol⁻¹) from Fowler-Guggenheim.∆Q: Variation of the Temkin adsorption energy (kJ/mol).A_T: Temkin equilibrium constant (L·mg⁻¹); B = R T q m Δ Q (J·mol⁻¹): Constant linked to the heat of adsorption;R = 8.314 kJ·K⁻¹·mol⁻¹: Constant of ideal gases;T (K): Absolute temperature; q_mDR: Maximum adsorption capacity in micropores (mg/g) of Dubinin-Radushkevich;ε: Polanyi potential;β: Constant linked to the energy of adsorption (mol²·kJ⁻²) according to D-R. θ = q e / q m : Degree of overlap.

R ( % ) = mass   of   activated   carbon mass   of   the   precursor × 100 (1)

➢ The ash content of the carbon is determined according to the ASTM method (American Standards Technology Method) [24]. The carbon samples are calcined at 650˚C in a muffle furnace for 7 hours. The ash rate is given by the following relation (2):

C ( % ) = m 2 − m 0 m 1 − m 0 × 100 (2)

m₀: mass of the dry and empty crucible;

m₁: mass of the assembly (crucible and activated carbon);

m₂: crucible mass after cooling containing the ash.

➢ To determine the iodine value, we used a method which is an adaptation of the CEFIC 1989 method and the AWWA B600-76 standard applied by Ousmaila et al. [25]. Thus, a mass m = 0.2 g of activated carbon is placed in a 100 ml beaker. 20 mL of a 0.02 N solution of I₂ are added to the pipette, and then stirred for 4 to 5 min. After filtering the mixture on filter paper, 10 mL of the filtrate are removed and dosed with a 0.1 N sodium thiosulfate solution in the presence of two drops of starch paste until the solution is completely discoloured and iodine index ( Q I 2 ) is determined from the following Formula (3):

Q I 2 = [ C 0 − C n ⋅ V n 2 V I 2 ] ∗ M I 2 ∗ V a b s m A C (3)

V_n: volume of sodium thiosulfate poured at the equivalence (mL);

C_n: concentration of sodium thiosulfate (mol/L);

C₀: initial concentration of I₂;

V I 2 : Volume of I₂ dosed;

M I 2 Molar mass of iodine (253.81 g/mol);

V_abs: adsorption volume (20 mL);

M_AC: mass of activated carbon (g).

Activated carbon with the best physicochemical properties has been used for the removal of metal ions (Pb²⁺) in aqueous solution.

Lead nitrate II Pb(NO₃)₂ with a molar mass of 331.2 g/mol produced in the form of a white powder used in this study is characterized by a purity of 99.5% (Merck product). It was bought with a chemical sales company in Abidjan. All the series of lead(II) solution of well-defined concentration (10 mg/L - 500 mg/L) are obtained by dilution with distilled water of the mother solution of 1000 mg/L in lead element (i.e. 4.036 g Pb(NO₃)₂ in 1000 mL of distilled water). The nitrate ions are chosen for their low capacity complexing with respect to many cations. The solutions of the metal cation of various experiments carried out are prepared with 65% nitric acid in order to allow good solubility.

All the adsorption tests were carried out in batch mode by putting 50 mL of lead(II) solution in 250 mL Erlenmeyer flasks. These suspensions are placed under constant stirring of 350 rpm at room temperature of the room (27˚C). After the time considered, the suspensions are filtered on whatman 44 filter paper. The residual concentration of lead(II) element in the filtered solution is determined using a Varian SpectrAA 110 brand Atomic Absorption Spectrometer at length. 261.42 nm wave.

The effects of the contact time, the dose of activated carbon, the pH of the solution, the concentration of Pb²⁺ ion and the temperature (27˚C - 75˚C) were studied by adsorption of Pb²⁺; then:

· to study the effect of the mass of carbon, the lead(II) solution at 100 mg/L is brought into contact for 120 min, with different masses of carbon (0.1; 0.25; 0.5; 1 and 2 g);

· with regard to the adsorption kinetics and the effect of the initial concentration of the solution, the kinetic tests were carried out for 5 min to 180 min, by mixing volumes of 50 mL of lead(II) solution with different concentrations (50, 100, 300 and 500 mg/L) with 0.5 g of activated carbon;

· in order to examine the influence of the pH of the solution on the adsorption capacity, 0.5 g of carbon is stirred with 50 mL of lead(II) solution at 300 mg/L. The pH of the solutions was adjusted to the following values (2, 4, 5, 6, 7, 9 and 11) at the start of the experiment with solutions of sulfuric acid or sodium hydroxide (0.1N). The evolution of the adsorption being controlled as a function of the equilibrium time;

· To study the effect of temperature on the adsorption of lead(II) ions, the experiments were carried out by adding the mass of 0.5 g of carbon to 50 mL of the metallic solution of lead(II) at different concentrations. Initials, at temperatures varying between 27˚C and 75˚C;

· For the adsorption isotherm, 0.5 g of carbon is added to various lead(II) solutions at different concentrations (20, 40, 60, 80, 100, 200 and 300 mg/L) and stirred for the time of balance.

In all cases, the adsorption capacity q_t (mg/g) or q_e and the elimination rate TA (%) of the lead element (II) are calculated respectively by the relations (4) and (5):

q t = ( C 0 − C r ) ⋅ V m (4)

T A ( % ) = C 0 − C r C 0 ⋅ 100 (5)

with:

V = volume of lead solution (L);

C₀= initial concentration of the solution (mg/L);

C_r = residual concentration of the solution (mg/L);

m = mass of activated carbon used (g).

The application of adsorption isotherms is very useful for describing the interaction between the adsorbent and the adsorbent. There are several models for analyzing experimental adsorption equilibrium data. In this study, six two-para- meter models (Langmuir, Freundlich, Temkin, Dubinin-Radushkevich (D-R), Kiselev and Fowler-Guggenheim models) were applie Kinetic models such as pseudo-first order, pseudo-second order, intraparticle, Boyd and Elovich diffusion models [26] [27] were used to understand the kinetics of adsorption. Table 2 and Table 3 present the equations and parameters of these adsorption isotherms and these kinetic models. The experimental results were evaluated by simple plots of the linear forms of the two-parameter equations, with which it is possible to calculate the values of the adsorption parameters. For our study, the correlation coefficient R² was used to assess the validity of the theoretical isotherms. Indeed, the correlation coefficient of the straight line of a model close to unity reflects the applicability of this model to the adsorption of the adsorbate on the adsorbent.

The thermodynamics of lead(II) adsorption on CAA carbon is studied through the calculation of thermodynamic parameters such as standard free enthalpy (ΔG°), standard enthalpy (ΔH°) and standard entropy (ΔS°) of the experiment using the following Equations (6) and (7):

Δ G ° = Δ H ° − T Δ S ° (6)

Δ G ° = − R T ln K L (7)

By replacing ΔG° of relation (6) in (7) we obtain Equation (8):

with: q_eandq_t: The adsorption capacities respectively at equilibrium and at time t; k₁andk₂: respectively the speed constants of the pseudo-first order and the pseudo-second order; α: the initial adsorption rate; β: Constant linked to the extent of surface coverage; k_di: The intraparticle diffusion rate; C: Constant indicating the thickness of the boundary layer; F = q t / q e fraction of the solute adsorbed at time t.

ln K L = ( Δ S ° R ) − ( Δ H ° R ) ⋅ 1 T (8)

The plotting of the lnK_L curve as a function of 1 T allows the estimation of

the thermodynamic parameters.

Adsorption tests on activated carbon of the lead element contained in the industrial effluent are carried out. Among the experimental conditions retained: the quantities of activated carbon used are: 0.5 g; 1 g; 1.5 g and 2 g for 50 mL of polluted water solution. The contact times are 120 min and 1440 min (24 h). The samples are adjusted to the pH level to have the optimum adsorption pH of the metallic element. The tests are carried out in batch mode on the effluent in the presence of activated carbon and the concentrations before and after treatment are measured by an atomic absorption spectrometer in order to determine the residual concentration and the rate of reduction.

As shown in Figure 1, the increase in CAA significantly affects the removal of the Pb²⁺ cation. In other words, the amount of Pb²⁺ adsorbed increases with the amount of CAA. With the increase in the dose of adsorbent from 0.1 to 2 g (i.e. 2 to 40 g/L), the percentage of removal of Pb²⁺ increased from 70% to 80%. Furthermore, the maximum retention is already obtained for a mass of 0.5 g of activated carbon (10 g/L). Beyond this mass, there is stability in the rate of reduction which could be explained by the saturation of the carbon. This quantity of mass necessary to fix the maximum of metal ions Pb²⁺, which will be retained for the rest of our work as optimal mass. This improvement in the retention rate of metal ions in the mass of activated carbon increases is mainly due to an increase in the number of active adsorption sites within the CAA. In fact, if the mass of activated carbon in the solution is large, the number of sites will also be. Consequently, the probability of interaction (solute-site) also increases. This same trend has been reported by Bendaho et al. [28].

The effect of the contact time on the adsorption of Pb²⁺ on the CAA was carried out at 27˚C at different initial concentrations of Pb²⁺ (Figure 2). Adsorption is shown to increase rapidly and is followed by a step without significant variation in adsorption. The rapid adsorption at the initial stage may be due to the occupation of active centers of CAA, thus providing many active sites easily accessible to Pb²⁺ ions. By increasing the time and the concentration, the availability of the remaining active sites decreases, thus leading to a long time to reach equilibrium [29]. This is explained by the fact that most of the vacant sites will be quickly occupied by Pb²⁺ cations, but the few remaining sites will be gradually occupied due to the high concentration of Pb²⁺ and the overflow of available sites. In solution, at low concentration of Pb²⁺ 50 - 100 mg/L, equilibrium is obtained after 30 min, while at high concentration (300 - 500 mg/L), a longer equilibrium time of 90 min. In addition, the overall retention is comparable for the four concentrations with a yield which increases when the concentration increases with orders of magnitude of 48%, 61%, 81% respectively for the concentrations of 50, 100, and 300 mg/L excepted when the initial concentration is 500 mg/L corresponding to a yield of 64%. Furthermore, the increase in the initial concentration of Pb²⁺ leads to an increase in the adsorption capacity, which suggests that the increase in the concentration of lead(II) ions promotes mass transfer from the aqueous phase to the phase solid. Similar observations were made by Murat et al. [30]. Thus, the adsorption at equilibrium increased from 2.4 to 32 mg·g⁻¹ with an increase in the initial concentration from 50 to 500 mg/L. For our study, 81% is the maximum retention rate, corresponding to an equilibrium time of 90 min and an initial concentration of 300 mg/L. This 90 min duration could have been used as equilibrium time, but 120 min duration was used to allow maximum adsorption of the carbon for the study of the adsorption isotherms.

The initial pH of the aqueous solution remains one of the most important factors in determining the adsorption properties of the absorbent. The removal of metal ions by adsorption depends greatly on the pH of the solution [31] [32]. Thus, the effect of the pH of the starting solution on the adsorption of Pb²⁺ was studied between 2 and 11 at room temperature (27˚C), a contact time of 120 minutes and a Pb²⁺ concentration of 300 mg·L⁻¹. Figure 3 shows the initial effect of the pH of the adsorption of Pb²⁺ by the CAA. It shows that the initial concentration of Pb²⁺ increases to 146.06 mg/L (pH = 2) to 43.19 mg/L (pH = 5) and then rises to 130.60 mg/L (pH = 11). Thus, the percentage of adsorption increases (43.19% to 85.90%) with the increase in pH from 2 to 5 and decreases (85.90% to 56.46%) when the pH drops from 5 to 11. In Indeed, according to Table 2, the pH_PZC value of CAA is approximately 4.8. This indicates that when the pH of the solution is above 4.8; the surface of CAA will have a net negative charge therefore will tend to attract more Pb²⁺ ions., while at a pH lower than 4.8, the surface of CAA will have a positive charge therefore will tend to repel Pb²⁺ ions [33].

The low abatement rates observed between 2 ≤ pH < 4.8 could also be explained by the competitive effect between the H⁺ and Pb²⁺ cations which compete for the negative adsorption sites existing on the carbon surface. The surface of the adsorbent being positively charged due to the H⁺ already adsorbed will tend to repel Pb²⁺ ions. On the other hand, a remarkable capacity for eliminating Pb²⁺ was observed when the pH was increased from 5 to 11. This decrease in adsorption in the basic medium could be explained by a change of phase of the ion lead(II) by the formation of lead complexes such as Pb(OH)₂ and insoluble forms since the pH of the addition of NaOH controlled the medium, thus increasing the concentration of OH⁻ in the medium [34]. The decrease in the adsorption of Pb²⁺ at alkaline pH could be due to the neutralization of the acid sites present in the activated carbon by hydroxyl ions OH⁻. A similar trend has been reported by Madhava et al. [35] when removing Pb and Zn on activated carbon. In total, the removal of lead(II) could therefore be done either by electrostatic interactions,

by complexation or by ion exchange. Since the alkaline conditions accelerate the formation of hydroxyl complexes resulting in poor adsorption of Pb²⁺ by CAA, the pH = 5 seems to be the best for the adsorption of Pb²⁺ by CAA in the context of our study.

The adsorption isotherm indicates that the adsorbate molecules are shared between the adsorbent and the liquid phase at equilibrium as a function of the adsorbate concentration. In this study, the equilibrium data obtained for the adsorption of lead(II) ions on the CAA were analyzed by considering the isothermal model of Langmuir, Freundlich, Temkin, Dubinin-Radushkevich, Fowler- Guggenheim and Kiselev. The linear forms of the different isotherms are described by the equations in Table 2.

· Langmuir isotherm

The linear form of the Langmuir isotherm equation is given in Table 2. The

two parameters K_L and q_m are determined from a graph 1 q e as a function of 1 C e (Figure 4(a)). The Langmuir isotherm is frequently evaluated by a separation factor, R_L, which is defined by: R L = 1 1 + K L C 0 where C₀ is the initial solute

concentration. Depending on the R_L value, the adsorption is said to be: favorable if 0 < R_L < 1; unfavorable if R_L > 1; linear if R_L= 1 and irreversible if R_L = 0. [36]. According to the data calculated and presented in Table 5, R_L is greater than 0 but less than 1, which indicates that the Langmuir isotherm is favorable. Based on this research, the maximum single-layer coverage capacity (Q_m) of the Langmuir model was established at 74.07 mg/g, K_L at 0.0356 L/mg, R_L (separation factor) at 0.412, which indicates that the sorption equilibrium is favorable and the value of R² is equal to 0.96, which proves that the sorption data correspond well to the Langmuir model.

In addition, the value of the adsorption capacity from this acacia wood obtained in the context of our study is high compared to other adsorbent raw materials found in the literature (Table 6), thus showing that our CAA carbon is effective in removing Lead(II) ions from water.

According to Langmuir’s model, adsorption is carried out on a homogeneous energy surface by the formation of monolayer without any interaction between the adsorbed species. However it gives no information on the heterogeneity of the adsorbent. Let’s check through Freundlich model if adsorption also occurs on heterogeneous surfaces.

· Freundlich isotherm

This isotherm is commonly used to describe the adsorption characteristics of the heterogeneous surface [50]. These data often correspond to the empirical equation proposed by Freundlich in Table 2 with n_F, an indicator of adsorption intensity. The Freundlich isotherm is obtained by plotting the linearized equation

ln ( q e ) = f ( ln C e ) (Figure 4(b)). The linearly transformed equation was applied to correlate the sorption data where 1/n is a heterogeneity parameter, the smaller 1/n, the greater the expected heterogeneity. This expression is reduced to a linear adsorption isotherm when 1/n = 1. If n is between one and ten, this indicates a favourable sorption process [51]. According to the data in Table 5, this value of 1/n = 0.7456 while n = 1.33 indicates that the sorption of Pb²⁺ on CAA is

favourable and that the value of R² is 0.99. The Langmuir and Freundlich isotherms do not consider the energy aspect during adsorption, the Temkin model is used to obtain information on the variation of the adsorption energy.

· Temkin isotherm

The Temkin isotherm considers the fact that the heat of adsorption of all the molecules of the cover layer decreases linearly with the cover due to the decrease in adsorbent-adsorbate interactions. Adsorption is characterized by a uniform distribution of the binding energies at the surface. The linear form of the Temkin isothermal model is given by the equation of Table 2. The plot of q e = f ( ln C e )

(Figure 4(c)) allows to determine B T = q m R T Δ Q , then by introducing a value of

q_m (for example from the Langmuir application) calculates the variation in adsorption energy ΔQ. In Table 5, the correlation coefficient (R²) obtained is close

to 1; thus, showing that the Temkin model is applicable. The variation of the adsorption energy ΔQ resulting from the linearization of the Temkin model is positive (20.394 kJ/mol) which implies that the adsorption reaction is exothermic. Similar values of the adsorption energy have been reported by Oualid et al. [52] during the copper (II) adsorption study. The Temkin isotherm does not determine the nature of the adsorption, so the Dubinin and Radushkevich isotherm is used.

· Isotherm of Dubinin-Radushkevich

The Dubinin-Radushkevich isotherm (D-R) is applied to determine the nature of the adsorption mechanism based on the theory of potential assuming that the surface of the adsorbent is heterogeneous. The isotherm of D-R is given by the equa-

tion of Table 2 with: the Polanyi potential given by the relation ε = ln ( 1 + 1 C e ) .

The linear form makes it possible to trace the curve ln q e = f ( ε 2 ) (Figure 4(d)) and to determine β then calculate the average energy of adsorption E (kJ·mol⁻¹) by using the equation:

E = 1 2 β

E < 8 kJ·mol⁻¹: physisorption dominates the sorption mechanism;

8 <E < 16 kJ·mol⁻¹: ion exchange is the dominant factor;

E > 16 kJ·mol⁻¹: sorption is dominated by intra-particle scattering.

In Table 5 the value found of the free energy E to estimate the type of Pb²⁺ adsorption process is 0.707 kJ·mol⁻¹. This value belongs to the energy interval when physisorption dominates (E < 8 kJ·mol⁻¹). However, the regression coefficient is far from unity (0.883) so this model is not applicable. In order to assess the interaction energies between adsorbed molecules, the Fowler-Guggenheim isotherm was applied.

· Fowler-Guggenheim isotherm

The Fowler-Guggenheim model is based on statistical thermodynamics and takes into account the interactions between adsorbed molecules. The molecules adsorbed on the nearest neighboring sites have an interaction energy equal to 2W/Z with Z the number of lateral coordinates, that is to say the number of nearest neighbours.

If W > 0, the adsorbed molecules repel each other.

If W < 0, the adsorbed molecules attract each other.

By representing the curve ln [ C e ( q m − q e ) q e ] = f ( q e q m ) , the slope leads to

2W/RT and the intercept at –lnK_FG. The experimental results of the Pb²⁺ adsorption isotherms modelled by the Fowler-Guggenheim equation are represented by Figure 4(e) and the parameters recorded in Table 5. The interaction energy valueW = 1.217 kJ·mol⁻¹ > 0 stipulates that the adsorbed Pb²⁺ cations repel each other. However, this result cannot be taken into account because the regression coefficient is low: 0.409. This model is limited to the interactions taking place between the adsorbed molecules but does not provide information on the formation of a possible complex between the adsorbed molecules. Let’s check if there is complex formation through the Kiselev model.

· Kiselev isotherm

The Kiselev model leads to the determination of a complex formation constant which supposes adsorption in a monomolecular layer according to the equation in Table 2. The graphic representation of the linear form

q m ( q m − q e ) C e = f ( q m q e ) , allows to deduce K and K_n. The experimental results of

the isothermal adsorption equilibria of the Pb²⁺ cation on the CAA modelled by the Kiselev equation are grouped in Figure 4(f) and in Table 5. This model applies fairly well to the adsorption of the Pb²⁺ cation about correlation coefficients equal 0.955. This implies that there is formation of complexes between the cations adsorbed on the surface of the activated carbon. These results confirm once again the high rate of metal cation abatement in alkaline media when studying the effect of pH on adsorption. By way of illustration, the formation of Pb complex is moreover observable on the surface of the CAA charcoal through the SEM pictures of Figure 5.

The effect of temperature on the adsorption of Pb²⁺ was carried out at temperatures ranging from 27˚C to 75˚C in 50 mL of Pb²⁺ solutions of different concentrations from 40 to 300 mg·L⁻¹. The equilibrium contact time for adsorption is fixed at 120 minutes. It is observed that the amount of Pb²⁺ adsorbed decreases by increasing the temperature from 27˚C to 75˚C (Figure 6), indicating that the reaction is exothermic. The thermodynamic parameters ΔG°, ΔH° and ΔS° are determined from Equations (5), (6) and (7) and the plot of lnK_Las a function of 1/T (Figure 7) Where, K_L is the constant of Langmuir equilibrium (L·mg⁻¹) at each temperature multiplied by the density of water (10⁶ mg·L⁻¹) according to Dos Santos et al. [53] and T the absolute temperature. The values of the parameters ΔG° (kJ·mol⁻¹), ΔS° (kJ·mol⁻¹·K⁻¹) and ΔH° (kJ·mol⁻¹) are summarized in Table 7. The negative value of ΔG°, suggests that the process of adsorption of Pb²⁺ by CAA is spontaneous. The negative value of ΔH° indicates the exothermic nature of the adsorption process according to Chouchane et al. [54] and Emna et al. [55] and shows that the transfer of Pb²⁺ ions from the aqueous phase to the solid phase releases energy. Retention is ordered at the solid/liquid interface during adsorption due to the negative value of ΔS°. Furthermore, the standard enthalpy value (of the order of −51 kJ·mol⁻¹ less than −40 kJ·mol⁻¹) during the adsorption of the Pb²⁺ ion indicates that chemisorption is involved in this adsorption process according to Kumaret al. [23].

The kinetic study of the experimental data allows a description of the fixing mechanisms and provides information relating to the mode of transfer of solutes from the liquid phase to the solid phase. Like the adsorption equilibria, the adsorption kinetics of a material can also be modelled. For this purpose, the literature reports a certain number of models which are quite used, among which appear the models of pseudo-first order and pseudo-second order, the model of Elovich, the model of intraparticle diffusion and the model of Boyd [56]. In order to understand the nature of the Pb²⁺ adsorption phenomenon on CAA in the framework of our study, the mathematical equations describing the kinetic

models (Table 3) were used to adjust the experimental data. Figure 8 presents the linear plot of the intraparticle diffusion and pseudo-first order, pseudo-second order, Elovich and Boyd equations. The calculated kinetic constants of all the applied models are indicated in Table 8. On the one hand, about the values of the correlation coefficient, it is clear that the adsorption of Pb²⁺ on the CAA follows the pseudo-second-order model. This adsorption reaction therefore depends on the concentrations of the adsorbent and the adsorbate. On the other hand, the study reveals that the intraparticle diffusion model is involved in the adsorption process. However it does not correspond alone to the limiting stage of the reaction of adsorption of Pb(II) by CAA. It is also limited by extra-particulate transport because the straight lines obtained during the plot of B_t as a function of time for different initial concentrations of lead(II) illustrated in Figure 8(e) do not pass through the origin.

The tests are aimed at determining the mass of activated carbon and the contact time required to remove a maximum amount of Pb²⁺ ions in real wastewater. The results are shown in Figure 9. The residual concentration of Pb²⁺ ions decreases with increasing mass of activated carbon regardless of the contact time. For a contact time of 120 min, the residual concentration decreases from 4.40 to 2.61 mg/L, i.e. a maximum reduction rate of 40.52%. As for the contact time of 1440 min (24 h), the residual concentration fluctuates when the mass of coal increases and the maximum reduction rate recorded is 29.20%. These results show that the amount of lead eliminated, although it depends on the amount of AC involved, also depends on the contact time. The more the mass of AC increases

and the shorter the contact time, the more important the elimination of lead by AC becomes. The maximum value of the rate of elimination of the Pb²⁺ cation recorded in the industrial effluent (40.52%) is moderately significant to judge the efficiency of our coal about the reduction rate reaching around 86% in the case of synthetic solutions. This difference could be justified by a possible competition between several pollutants contained in real wastewater. Among these pollutants could be found several other metal cations, nitrites, nitrates, phosphates, sulphates, and certain organic materials. In addition, the difference in the maximum elimination rate observed between the case of the contact time of 120 min and that of 1440 min, could be explained by desorption when the contact time becomes too long.