Bentonite was collected from Khulays bentonite deposit in Saudi Arabia. All reagents used were analytical grade and were not subjected to additional purification. Analytical grade Methylene Blue (MB) (C₁₆H₁₈ClN₃S), supplied from Fluka was used without further purification. Sodium tungstate Na₂WO₄, Ammonium vanadate(V) (NH₄VO₃) and sodium acetate (CH₃COONa) were all obtained from J.T. Baker. Distilled water was used to prepare all aqueous solutions in the study.

The adsorbent preparation was performed according to three steps. First Keggin-type polyoxometalates preparation was synthesized using the same procedure as in inorganic synthesis [10] . Then preparation of polyoxometalate Ionic liquid POM-IL by metathesis reaction, followed by impregnation of the Bentonite.

Sodium nonatungstate was synthesized using the same procedure as in inorganic synthesis [10] A mixture of 60 g (0.18 mol) of sodium tungstate dihydrate Na₂WO₄∙2H₂O and 75 ml of water is stirred in a 200 mL beaker with a magnetic stirring bar until the solid is completely dissolved. 2.4 mL (0.035 mol) of Phosphoric acid (85%) were added dropwise. After addition of the acid is complete, the measured pH is 8.9. 11.4 mL (0.19 mol) of glacial acetic acid is added dropwise with vigorous stirring. Large quantities of white precipitate form during the addition. The final pH of the solution is 7.6 ± 0.3. The solution is stirred for 1 h, and the precipitate is collected and dried by suction filtration on a medium frit.

In 250 mL beaker, 8.2 g (0.1 mol) of sodium acetate were dissolved in 100 mL of distilled water at Room Temperature (R.T). The pH of the solution was adjusted to 4.8 by adding approximately 3.5 mL (0.06 mol) of acetic acid. To this solution 2.9 g (0.024 mol) of NH₄VO₃ were added under vigorous stirring, then 20 g (0.0082 mol) of Na₉[A-PW₉O₃₄] were added and stirred for 48 h at R.T. The wine-red solution was filtered by suction frit porosity 4 to remove unreacted orange solid. Afterwards 13.4 g (0.024 mol) of tetraoctylammonium bromide in 50 mL of toluene were added to the solution. The reaction mixture was started to separate into two layers after addition of 50 mL of toluene. In the biphasic system the organic layer turned dark red after shaking in the separation funnel. The organic phase was separated, and the solvent removed under vacuum by rotary evaporator.

1.16 g of Q⁸PV₃W₉ (0.002 mol), was dissolved in 50 mL of acetone and then 4.5 g of Bentonite were added. The suspension was gently shaken for 30 min and the solvent was removed by rotary evaporator. 50 mL of acetone was added, and impregnation procedure was repeated four times. The final product Q⁸PV₃W₉@B was obtained as a solid, free flowing powder.

Information regarding the crystalline structures was obtained through X-ray diffraction (XRD) analysis using a powder PXRD diffractometer (Model Equinox 1000-INEL, France) with Co Kα radiation (λ = 1.7890 Å) at 30 kV and 30 mA. The polyoxometalates (POMs) were compared to the parent Keggin structure using reference data from the International Centre for Diffraction Data (ICDD) database. Sample morphology was examined using field emission scanning electron microscopy (FEG-SEM) with a Quanta FEG450 (FEI, Netherlands). This involved an ETD Everhart Thornley detector in High Vacuum mode, a solid-state backscattering electron detector (VCD), and an EDS detector (XFLASH6-30, Bruker) to determine the elemental composition of the samples. The dispersion and size of POM particles on the Bentonite support, as well as the layered structure of Bentonite and POM-IL@Bentonite, were confirmed using transmission electron microscopy (TEM) with a Tecnai G2 F20 Super Twin (FEI, Netherlands) equipped with a LaB6 source operating at 200 kV. The electron microscope also had an EDS detector for elemental analysis. Nanoprobe scanning transmission electron microscopy (STEM) imaging was conducted with a HADAF detector, and TEM images were captured using a Gatan camera at 200 kV with 2k × 2k resolution. Data from TEM, high-resolution TEM (HRTEM), STEM, and EDS were collected and processed using TIA software (Tecnai Imaging and Analysis version 1.9.162) and Gatan Micrograph Software version 2.3.

The surface functional groups of POM-IL and Bentonite were analyzed using Fourier transform infrared spectroscopy (FTIR) with a Bruker Tensor II spectrometer. Nitrogen sorption analysis was performed to evaluate the specific surface area (using the BET method), specific pore volume, and pore diameter (using the BJH method) of both raw and POM-SIL modified bentonite, utilizing a NOVA (2200 e) high-speed surface area and pore size analyzer.

Analytical grade Methylene Blue (MB) and used without further purification. The chemical structure of MB is shown in Figure 1 . Stock solution of 1000 ppm, was prepared by dissolving a 1g of MB in 1 L of distilled water. The experimental solution was prepared by using distilled water for diluting the stock solution. The concentration of Methylene Blue dye before and after adsorption were determined using UV spectrophotometer, GENESYS 10S UV-VIS. As can see in Figure 1 , the absorption spectrum of the Methylene Blue is characterized by three main bands, one in the visible region (λ_max= 665 nm), and two in the UV region (λ_max = 292 nm and λ_max = 246 nm). In our case, the most important band is at 665 nm.

Adsorption test for the dye removal from aqueous solution was conducted using adsorption batch experiments to explore the adsorption properties and the factors influencing the adsorption. Batch experiments were performed by varying contact time, mass of adsorbents, concentration of dyes, pH and temperature. The following conditions were preserved for the different sets of experiments:

1) The effect of pH was conducted in the range from 2.0 to 12, 100 mg of Q⁸PV₃W₉@B and, 100 mL solution volume, 50 ppm MB concentration and T = 298 K. HCl (0.01 M) or NaOH (0.01 M) was added to set the desired pH value.

2) Effect of contact time was carried out through the time intervals (10, 20, 30, 40, 50, and 60 min), 100 mg of adsorbent, 100 mL solution, 50 ppm MB concentration, 298 K, initial non modified pH.

3) The effect of adsorbent mass was examined using different doses (20, 40, 60, 80 and 100 mg) of adsorbent, initial non modified pH, time 60 min, 50 ppm MB concentration, 100 mL solution volume, and temperature 298 K.

4) The effect of initial concentration was conducted using 40, 50, 60, 100, 200, 300, 400, 500 mg/L of MB, initial non modified pH, time 60 min, adsorbent mass 100 mg of Q⁸PV₃W₉@B and temperature 298 K.

5) The influence of temperature on the adsorption process was studied under different temperatures of 298, 303, 308, 313 and 318 K, initial non modified pH, time 60 min, 50 mg/L MB concentration, adsorbent mass 20 mg, solution volume 100 mL.

In each Experiment, the adsorbent is stirred at 300 rpm in the MB solution until the adsorption is reached. After that, the dye residual concentration is measured. After adsorption the dye was kept apart from the adsorbent by centrifugation with 3000 rpm speed and use UV-VIS spectrophotometric technique to determine the C based on Beer-lambert equation.

The amount of the dye adsorbed per unit mass; Q_t will be calculated using the equation

$Q_t=\frac{C_0-C_f}{m}\times V$(1)

And the Removal efficiency: (R%)

$R\%=\frac{C_0-C_f}{C_0}\times 100$ (2)

where C₀ and C_f (mg·L⁻¹) are the initial and final MB concentration, V (mL): the dye solution volume, m (mg): the adsorbent mass.

The reusability of the adsorbent makes it prominent adsorbent material for the adsorption and make it more economical. Adsorbents obtained after adsorption experiments were dried at (120˚C) and then shaken in 30 mL of ethanol for 15 min twice to remove the adsorbed dye. After that 400 mL of distilled water were added and the suspension was stirred under 80˚C in order to achieve desorption.

Antimicrobial activities of the Q⁸PV₃W₉ and Q⁸PV₃W₉@B were performed against two different pathogenic bacteria gram-positive bacteria: S. aureus ATCCBAA977 and gram negative bacteria E. coli ATCC25922. The bacterial inoculum concentration (6 × 10⁶ CFU/ml) uniformly spread using a sterile cotton swab on a sterile Petri dish containing Muller–Hinton agar medium [11] [12] . For this, the discs were placed on Petri plates containing bacterial culture was poured in pores 0.1 ml Q⁸PV₃W₉ and Q⁸PV₃W₉@B (9 mm in diameter) in Muller–Hinton agar medium. The plates incubated for 24 h at 37˚C ± 1˚C, under aerobic conditions. After incubation, confluent bacterial growth was observed. Inhibition of bacterial growth was measured in mm.

The FTIR spectra of raw Bentonite, Q⁸PV₃W₉@B in the range of 4000 - 400 cm⁻¹ were shown in Figure 2 . FT-IR spectrum of the Q⁸PV₃W₉@B showed that in the low frequency region, the modified and unmodified Bentonites are largely comparable indicating that the clay mineral has not changed upon addition of Q⁸PV₃W₉ to Bentonite. Besides, no peak shift was observed during the modification which indicates the retention of the structure of Bentonite.

The absorbance peaks at 524 cm⁻¹, 914 cm⁻¹ and 468 cm⁻¹ ascribed respectively to δ(Al-O-Si), δ(Al-Al-OH), δ(Si-O-Si) which confirm the presence of montmorillonite.

The very strong characteristic peak observed at 1032 cm⁻¹ was ascribed to asymmetric stretching vibrations of Si-O-Si bonds. The broad band in the 3430 - 3623 cm⁻¹ region can be ascribed to the symmetric stretching of (Si-OH, Al-OH) structural hydroxyl groups OH and of the physically adsorbed water OH. The shoulder at 3694 cm⁻¹ and the weak band at 695 cm⁻¹ suggest the presence of kaolinite. The absorption band at 1639 cm⁻¹ is attributed to the angular vibration of the OH group and related to the adsorbed water and the hydration water present in the clay.

The presence of tetraalkylammonium cation is confirmed by the presence of peaks at 1379 and 1460 cm⁻¹ which are assigned to C-H scissoring vibrations of CH₂-N⁺ and peaks at 2855 and 2956 cm⁻¹ assigned to the symmetric and asymmetric stretching modes of -CH₂ of organic cation [14] .

The characteristic bands for POM are not observed in low frequency, they overlaped with the characteristic band of Bentonite.

The SEM results for the raw Bentonite sample presented in Figure 3(A) . As can be seen, raw Bentonite has a rough surface with large number of pores distinguished as dark areas. SEM images in Figure 3(B) for modified Bentonite by POM-IL samples show that chemical modification by Q⁸PV₃W₉ lead to a change of the surface morphology of raw Bentonite and presents rose-like agglomerates on the surface.

After loading with MB dye molecules, the morphology has changed and becomes cloudy, the layered-stacking structure is no more observed. This change is due to the occupation of MB molecules into the heterogeneous pores of Q⁸PV₃W₉ @B as shown in Figure 3(C) [15] .

EDS analysis in Table 2 showed that natural Saudi bentonite is mainly composed of silicon dioxide, Aluminum oxide, iron oxide, sodium oxide, in addition to calcium, magnesium, titanium and potassium oxides. Figure 4 revealed appearance of new peaks of P, W, V relative to PV₃W₉ polyoxometalate with the correct V/W ratio (3:9); this result confirms that PV₃W₉ is present in the prepared adsorbent and retain its keggin structure.

The X-ray patterns of raw Bentonite, Q⁸PV₃W₉@B. are illustrated in Figure 5 .

The XRD pattern of raw Bentonite in Figure 5 shows the presence of montmorillonite (6.26˚, 24.30˚, 42.67˚, 46.12˚, 49.57˚, 53.54˚, 58.88˚) as major phase. The results show that the characteristic peaks of the Bentonite support are not affected during the POM impregnation with Bentonite.

The X-ray diffractometer recorded in a range of small angle (2θ) ranging from 0˚ to 10˚ shows the presence of a characteristic diffraction peak located at 2θ = 6˚ from which the interlayer distance was found to be 14.08 Å. This peak is associated with the (001) diffraction (d001) of the montmorillonite phase [16] .

The introduction of POM to the Bentonite does not affect the d001 diffraction peak which appears at 14.75 Å for Q⁸PV₃W₉@B ( Figure 6 ). This finding confirmed that the structure of Bentonite is retained after impregnation by Q⁸PV₃W₉@B.

Moreover, the presence of POM in the prepared adsorbent is confirmed by the presence of structural characteristic peaks in the ranges of 2θ (5˚ - 10˚, 17˚ - 22˚, 25˚ - 30˚, and 31˚ - 37˚) in agreement with the Keggin structure [17] [18] .

TEM characterization carried out on the POM modified Bentonite are presented in Figure 7 . TEM analysis confirmed the XRD results and revealed the existence of layers at basal space d₀₀₁ = 14.08 A for Bentonite and d₀₀₁ = 14.75 A for POM modified Bentonite. There is no significant expansion of interlayer space θd (4.38 A and 5.05 A).

Nitrogen sorption was used to investigate the specific surface area (BET method), specific pore volume and pore diameter (BJH method) of the Raw Bentonite and Q⁸PV₃W₉@B to establish the consequences of POM-IL adsorption on the Bentonite pore structure. The data in Table 3 show that an overall reduction in pore diameter, specific pore volume and specific surface area is observed, with respect to the raw bentonite reference, indicating that the Q⁸PV₃W₉ coats the exterior surface and some of the internal pore structure.

The effect of contact time on Methylene Blue removal by Q⁸PV₃W₉@B is shown in Figure 8 . It could be seen that the percentage removal increase with increasing the contact time, and occurred in two stages: first fast stage and equilibrium stage. The uptake is rapid for the first stage (5 min) with 48.2% removal. This fast kinetic is due to the presence of high number of available vacant sites. The equilibrium was reached within almost 20 min with total removal. Futher increase in contact time will no longer improve the percentage removal.

The percentage removal of dye is directly proportional to the adsorbent mass. As seen clearly from Figure 9 Q⁸PV₃W₉@B the adsorbent mass used, ranged from (20 - 100 mg). As expected, the results followed the general trend with adsorbent mass. In fact, The findings revealed that the percentage of adsorption of Methylene Blue dye increased with increasing amount of the modified Bentonite from 37.2% (20 mg) to 100% (100 mg); this might have been ascribed to an enhanced surface area of the adsorbent and the availability of additional adsorption sites.

Methylene blue dye solution of different concentration ranging from 50 - 500 mg/L were prepared by dilution from the 1000 ppm stock solution. The effect of initial concentration on the removal of methylene blue on Q⁸PV₃W₉@B is shown in Figure 10 .

The results show that the % removal of MB increased initially and reached more than 95% with concentration of (50 - 200 mg/L) at constant adsorbent amount (100 mg). Adding more methylene blue above the saturation level (200 mg/L) did not find available vacant sites resulting on the formation of accumulation of methylene blue molecule on the surface of adsorbent and the percentage removal decrease.

The adsorption capacity (Q_e) increased gradually with the increase in concentration Figure 10(A) . However, at lower dye concentrations, the adsorption is independent of initial concentration since the ratio of the number of MB cations to the number of available adsorption sites is small.

The pH experiments were performed at pH ranging from 2 to 12. According to reported studies on the adsorption of dye, the effect of pH on the solute adsorption capacity and removal by c can be slightly or moderately significant.

For MB dye used in this study, the result related to the pH dependence are apparently surprising.

As shown in Figure 11 there is no significant effect on the adsorption of methylene blue while changing the pH solutions values, Q⁸PV₃W₉@B is stable adsorbent over a wide pH range [19] [20] .

Independent of the origin of this insignificant effect of the pH, this finding is quite meaningful in the adsorption process application since it makes pH adjustment of the effluent before treatment unnecessary. Since pH control is complicated and difficult to realize.

As a result, pH will not be adjusted during adsorption experiment to simulate real treatment condition of industrial effluents.

The experimental results are shown in Figure 12 . The influence of temperature on the adsorption of MB onto Q⁸PV₃W₉@B was carried out at 5 different temperatures ranging from 298 to 318K. Figure 12 shows that the removal percentage of MB increased with the increase in temperature; indicating that the adsorption process of methylene blue dye is endothermic in nature. The increase of adsorption is due to the absorbed heat used as activation energy.

Lagergren’s first order, Ho’s second order kinetic and the intraparticle diffusion model are applied in this study to determine the rate of adsorption at different time intervals.

Lagergren [21] , proposed the first order kinetics and improved and was given by

$\ln \left(q_e-q_t\right)=\ln q_e-K_{1}t$ (3)

where q_e and q_t are amounts of dye adsorbed (mg/g) per unit mass at equilibrium and at any time t (min), K₁ is the first order constant.

The pseudo second-order rate equation by Ho [22] , can be expressed as follows:

$\frac{t}{q_t}=\frac{1}{K_2{q}_e^2}+\frac{1}{q_e}t$ (4)

where q_e and q_t are amounts of dye adsorbed (mg/g) at time t (min) at equilibrium and at any time t respectively, K₂ is the second order constant.

The kinetics of MB dye adsorption onto Q⁸PV₃W₉@B were analyzed using pseudo-first-order PFO model (Equation (3)) and pseudo-second order PSO model (Equation (4)).

It was found that pseudo-first-order kinetic model did not well fit. Plot of $\ln \left(q_e-q_t\right)$ vs. t is not linear.

On other hand, the plot of t/q_t vs. t for pseudo-second-order model ( Figure 13 ) is applicable over the whole range of contact time with excellent linearity.

The kinetic parameter for pseudo-first-order and pseudo-second order were calculated and tabulated in Table 4 .

The real test for the validity of the kinetic model arises from the comparison between the experimentally determined (q_e,exp) and the calculated (q_e,cal) [21] [22] .

It can be noticed that in the pseudo-second-order kinetic model, the calculated q_e (51.5 mg/g) is very close to the experimental q_e (49.9 mg/g). In addition, the correlation coefficient R² for the pseudo-second-order (R² = 0.9935) is higher than that obtained for pseudo-first-order (R² = 0.5231).

Therefore, it is reasonable to conclude that the pseudo-second-order model is the obeyed model.

The adsorption isotherm is important for the description of how the adsorbate will interact with the adsorbent and give an idea about the adsorption capacity of the adsorbent. In this study Langmuir, Freundlich isotherm models were used to evaluate the equilibrium experimental data.

Langmuir isotherm predicts the formation of adsorbed solute monolayer and is based on the assumption that dye molecules are adsorbed on a fixed number of well-defined sites, each site con hold a unique molecule [23] . The general equation for Langmuir is:

$q_e=\frac{q_{\max }{K}_L{C}_e}{1+K_L{C}_e}$ (5)

where, q_e is the dye adsorbed amount at equilibrium (mg/g). q_max is the maximum adsorption capacity (mg/g). K_L is the constant for Langmuir. C_e is dye concentration at equilibrium.

Langmuir model can be mathematically expressed as:

$\frac{C_e}{q_e}=\frac{1}{q_{\max }{K}_L}+\frac{C_e}{q_{\max }}$ (6)

The value of (1/q_max) and K_L can be obtained from linear curve of (C_e/q_e) versus C_e, R_L provide information about the affinity between adsorbate and adsorbent which can be calculated using the following equation:

$R_L=\frac{1}{1+K_L{C}_o}$ (7)

where K_L is the Langmuir constant. C_o (mg/L) is the initial concentration of dye.

The R_L separation factor values ( Table 5 ) indicate the nature of the adsorption to be:

The Freundlich equation is empirical and represent the equilibrium on heterogeneous surfaces.

The Freundlich model in its linear form is express as:

$q_e=K_f{\left(C_e\right)}^{1/n}$ (8)

where C_e is the equilibrium dye concentration (mg/L), q_e is the dye adsorbed amount at equilibrium (mg/g). K_f are the Freundlich constants and n indicative of the extent of the adsorption and the degree of nonlinearity between solution concentration and adsorption intensity.

The Freundlich equation can also be linearized in logarithmic form as shown below:

$\log q_e=\log K_f+\frac{1}{n}\log C_e$ (9)

where C_e is the equilibrium concentration (mg/L). q_e is the adsorbed amount at equilibrium (mg/g). K_f and n are Freundlich coefficients, related respectively to adsorption capacity and adsorption intensity of the solid adsorbent.

The slope and the intercept of the plot $\log q_e$ Vs $\log C_e$ correspond to (1/n) and $\log K_f$, respectively.

Figure 14 and Table 6 summarize the calculated coefficients of determination (R²) and model parameters of the Langmuir and Freundlich isotherms. The results show clearly that the experimental data fit better to the Langmuir isotherm model (R² = 0.9495) than Freundlich (R² = 0.7251) which indicates homogeneous and monolayer coverage of MB cations at the surface of the Q⁸PV₃W₉@B. The maximum adsorption capacity for MB onto Q⁸PV₃W₉@B was 270 mg/g. Moreover, the adsorption is considered favorable when the separation factor R_L equation (7) range between 0 and 1 as shown in Table 5 [24] .

The R_L values for MB for each initial concentration was greater than zero and less than unity which indicates favorable adsorption.

Moreover, it is observed that R_L values are decreasing with increasing initial concentration which implies that the adsorption of MB becomes more favorable.

In order to evaluate the effect of temperature on the adsorption process and the thermodynamic function. ∆G˚ The standard Gibbs free energy, the standard ∆H˚ enthalpy, were calculated using the below Equations:

$\Delta G°=-RT\ln K_{dc}$ (10)

$\ln K_{dc}=-\frac{\Delta H°}{RT}+\frac{\Delta S°}{R}$ (11)

$K_{dc}=\frac{q_t}{C_t}$ (12)

The standard entropy values (J/mol·K), ∆S˚, were calculated by use Gibbs–Helmholtz equation as follows:

$\Delta S^0=\frac{\Delta H^0-\Delta G^0}{T}$(13)

where K_dc (Lg⁻¹) is Distribution coefficient, T (K): temperature expressed in Kelvin.

R is Gas constant (8.314 J·mol⁻¹·K⁻¹).

Thermodynamic parameters of the MB dye on Q⁸PV₃W₉@B are summarized in Table 7 . It is obvious that at higher temperatures the adsorption of MB onto Q₆⁸PV3@B was favorable. The ∆G˚ values are negative at all temperatures become more negative with increasing temperatures indicating the adsorption process is spontaneous. Mainly owing to chemisorption rather than physisorption [25] . The value of standard enthalpy change was positive (∆H˚ > 0), showing that adsorption is of MB an endothermic process. The positive values of ∆S˚ indicate that the MB dye adsorption process increase the randomness at the solid-liquid interface during the adsorption process and suggest a strong affinity between MB and Q₆⁸PV₃@B [26] .

The ability of the adsorbents to be reused is a crucial factor. Reusability of the adsorbent is usually carried out in order to avoid the cost of a new acquisition and minimizing the amount of waste. In order to evaluate the reusability of adsorbents, ethanol was selected as elution solvent. The recycled adsorbent indicated reasonable efficiency (100%) after eleven consecutive cycles as shown in Figure 15 . These results revealed that the Q⁸PV₃ W₉@B have a good potential as cost-effective adsorbent for removal.

Antibacterial activity is considered as an important criterion for the evaluation of adsorbent features in water decontamination. The antibacterial activity of Free Bentonie and Q⁸PV₃W₉@B against different bacterial isolates was tested and showed a higher score in the case of gram negative than gram positive pathogenic bacteria. The antibacterial of free Bentonite and Q⁸PV₃W₉@B is shown in Figure 16 , against pathogenic E. coli ATCC25922 and S. aureus ATCCBAA977. Free Bentonie showed minor bacterial activity as illustrated in Figure 16(C) , Figure 16(D) , the bacteria

was grown with no significant inhibitory zone. While, in case of Q⁸PV₃W₉@B, the inhibtory zone was strong around the disc free of bacteria, showing an important antibacterial activity.

The incorpration of Q⁸PV₃W₉ enhanced the antibacterial activity to the adsorbent. Similar result were reported in the case of Q^x₈[α-SiW₁₁O₃₉] x = 6, 7 supported on silica [27] .