Ionic Strength Effect on Green Malachite Adsorption onto Moroccan Montmorillonite Clay: Experimental Study and Theoretical Investigation

Abstract

The equilibrium adsorption process of Malachite Green (MG) from an aqueous solution using sodic Moroccan Montmorillonite Clay (Na-MMC) has been investigated under various experimental conditions. The effect of several inorganic salts (LiCl, NaCl, KCl, and CsCl) on green malachite adsorption at different ionic strength by sodic Montmorillonite as well as the pH effect were investigated through a number of batch adsorption experiments. The dye concentration in the solution before and after adsorption was measured spectrophotometrically. The experimental isotherm data show that the maximum removal of MG was observed at pH in the rang 8-10. The adsorbed amount increases with the concentration of the sodium or lithium, however it decrease with cesium or potassium salts. A theoretical explanation of GM adsorption and ionic strength effect was given based on data modeling developed by Nir and co. also. Geometry optimizations of GM molecule to get a better insight into structure geometry and reactivity were carried out by DFT calculations.

Introduction

The increasing use of organic dyes endangers the environment and poses health problems for humans and aquatic animals. Consequently, the risk of pollution increases if the depollution processes do not follow the rhythm of this evolution. Dyes are water-soluble and exhibit inherent chemical structure that is stable to photodegradation and biodegradation¹. A number ofphysicochemical and biological methods have been reported for removal of dyesfrom waste water ^{2, 3}. Adsorptionhas been widely recognized as effective and low-cost method to abet dye wastewater even at low concentration⁴. Various types of adsorbent materials areavailable: activated carbon, silica, natural polymericmaterials, sewage sludge, clays ^{5, 6}. However the quality of theadsorbent must meet the scientific and economic criteria, such as the quantityto be treated (high cationicexchange capacity), favourableconditions for the elimination, regeneration and above alla very low cost process ⁷. Recent studies show severalattempts to boost the adsorption performance of malachite green that is presentin effluent by its use as antifungal, anti-bacterial, and anti-parasitical andalso by its widely used as a direct dye for silk, wool, jute and leather ^{8, 9}.

The use of clays to remove this type of polluting molecules is one of the efficient and economical methods ¹⁰. In a wide variety of research, the bentonite (or montmorillonite) is the most used class^{2, 11, 12}. The montmorillonites clay is one of the minerals belongs to the smectite family, This type of phyllosilicates consists of two tetrahedral layers framing an octahedral layer (phyllosilicates 2: 1)¹³.

Montmorillonites surface promote a good physical properties for cations adsorption; the existence of negative charges on their surface gives them an adsorption capacity with cations and particularly with organic cations^{14, 15}.

Organic cations are adsorbed on montmorillonite surface by the cationic exchange with the hydrated exchangeable cation, which balance the negative intrinsic charge of surface. Other types of associations may also be present in the adsorption of organic molecules on the surface of montmorillonite, for example, van der Waals and hydrogen bonds ^16-18. Their importance also depends on such factors as the nature of organic molecule, its functional groups present, the nature of exchangeable cation, the temperature, the pH, the ionic strength and the nature of the ions present in the dispersion (Na⁺, K⁺, Cs⁺…)^{11, 12}. However, to date, the effect of ionic strength on this type of adsorption has been rarely studied; Giora Rytwo and his groups ^{15, 19-22} are the only ones who studied this effect experimentally and theoretically by developing a model applying a Gouy–Chapman–Stern (GCS) model for adsorption of organic cations ^{23, 24}.

The main concept of this model is developed in the theoretical part below.

With the development of density functional theory (DFT)²⁵,electronic properties of ground states can be calculated with good accuracy.Theoretical calculations (DFT) at B3LYP level have been carried out aiming toinvestigate the structure geometry of the MG dye, electronic properties andtheir dependences. We combined some theoretical descriptor reactivitycalculated with DFT with experimental results of MG-MMC interactions.

In this work, a Moroccan sodic Montmorillonite clay (obtained by the purification and treatment of raw clay extracted from the region of Nador) ²⁶, was characterized and tested as adsorbent for cationic MG dyes removal from aqueous solution. The evaluation of its potential as low cost adsorbents and the effect of ionic strength for adsorption of green malachite (MG) on sodic Montmorillonite (Na-MMC) will be shown. It is noteworthy that a variety of alkali metals (lithium, sodium, potassium and cesium) chlorides has been used .Interestingly, the effect of the concentration and the cation nature will be detailed on the equilibrium adsorption isotherm. The theoretical interpretation of the results is based on the modelling described at the top, using the coefficients of binding determined by Nir in 1986 ²⁷. This study is an extension of previous research related to bentonite (montmorillonite) deposits from Morocco and their possible applications in the removal of pollutants from wastewater.

Materials and methods

Materials

The Adsorbate

Malachite green (MG) used in this study was purchased from Merck (99% pure) and used without further purification. Its molecular structure and some of its characteristics are illustrated in Table 1. Dye stock solution (2mmol.L^-1) was prepared by dissolving accurately weighed quantity of the dye in double distilled water. Experimental dye solution of different concentrations was prepared by diluting the stock solution with suitable volume of double distilled water.

Table 1: Characteristics of Malachite Green (MG) ²⁸.

Dyestuff	Basic Green 4 (BG 4)
IUPAC	[4-[[4-(dimethylamino)phenyl]phenylmethylidene] cyclohexa-2,5-dien-1-ylidene] dimethylazanium;chloride
Commercial name	Malachite Green (MG)
C.I. number	42000
Empirical formula	C23H25N2Cl
Appearance	Green crystalline powder
Molecular weight	364.9g/moL
λmax	621 nm
Solubility at 25°C	40g/L
Molecular structure

The Adsorbent

The sodic Montmorillonite clay (Na-MMC) used in this work was prepared from crude bentonite extracted from a clay deposit in Nador region (northeast of Morocco). EL MIZ et al carried out purification; sodium activation and characterization ^{26, 29, 30}.The mineralogical and chemical compositions of the samples are typical of bentonites, mainly consisting of montmorillonite. Table 2 summarizes the physico-chemical characteristics of our Na-MMC and that of Wyoming Na-montmorillonite SWy obtained from the Source Clays Repository (Clay Minerals Society, Columbia, MO) ¹⁵ .

Table 2: Physico-chemical characteristics of selected clay

Characterization	Nador Na-Mont 26	Wyoming Na-montmorillonite SWy-1 31
CEC (meq/100g)	109	76.4
Stot (m2/g)	785	756

Methods

Theory

Gouy–Chapman–Stern (GCS) Adsorption Model

Rytwo et al developed the model presented here and based on the Gouy-Chapman-Stern theory ^{15, 23}. It is associatedwith the equations established by Nir and Margulies^{27, 31}. Two types of equations, modelled the interactionbetween the charged surface of montmorillonite and organic cations.

The interaction between a negative site P^– of clay and a cation X⁺:

The constant K_i of this reaction that translates the binding force (coefficient) for electrostatically associated is:

For the organic cations can have in addition, other interaction between these cations Xiand the neutral complex PX_i produced by first interaction:

With The binding coefficientḰ_iis :

In all equations, we have,

is the concentration of the cation at the surface and may be calculated upon knowing its concentration in the equilibrium solution

since the distribution of the cation as a function of its distance from the surface, depends on the electric potential.

For this, we may use Boltzmann’s equation:

With

Where: e is the elementary charge, Zi is the valence of the ion, being positive for a cation and negative for an anion, Ψ(0) is the surface potential, k_B is the Boltzmann constant, T is the absolute temperature, and

is the molar concentration of cation i in the solution heart, far from the surface. The potential value of the clay surface varies with the amount of adsorbed cations added. When the surface is negatively charged one has

if the amount of dye added is greater than the cationic exchange capacity (CEC) a charge reversal produced on the surface of the clay, consequently the electrostatic interactions repulsive causes the immigrations of the cations towards the core of solution or

Computational Method

The computations were performed utilizing the GAUSSIAN 09 program pack ³², GaussView program ³³ were used to visualisation. The ground state geometries were totally optimized using the hybrid B3LYP functional ^{34, 35} with the 6-31G (d) basis set. To account for the solvent effect, the single point calculation was carried out at the same theory level, with the aid of the integral equation formalism polarizable continuum model (IEFPCM) ³⁶

Batch Adsorption

To measure the dyes adsorption isotherms, a quantity 40mg of the Na-MMC was added to 50 ml solution of the prepared dye solution in 250 ml Erlenmeyer flasks. The final volume was brought to 100 mL by adding either the alkali chloride solution to study the effect of ionic strength, or a double distilled water to study the pH effect. The flasks were sealed and kept at 25 ± 1°C under continuous agitation (300 rpm) up to the equilibrium (for 12 hours). After the reaction period, the supernatant was separated by centrifugation at 9000 rpm for 15 min, the residual concentration in the supernatant was determined. The dye concentration in the raw and treated sample was determined by UV-Vis spectrophotometer (Shimadzu UV-1800 UV/Visible Scanning Spectrophotometer). The analyses were carried out at a wavelength of 619 nm. The amount of equilibrium adsorption, Qe (meq/100g), was calculated by Eq.7, and the percent of adsorption efficiency, (A %) was calculated as Eq.8 :

Where C₀ and Ce (mM) are the liquid-phase concentrations of dye at initial and equilibrium, respectively, V (L) is the volume of the solution and m(g) is the mass of dry prepared sorbent used.

X-Ray Diffraction

From the samples obtained after the centrifugal separation described above, 2 ml of suspension were deposited on glass microscope slides and dried. The basal spacing was measured using a PANalytical Diffractometer: XPERT-PRO, Copper Anticathode Ceramic X-ray Tube, Generator Power at RX: 40 mA, 45 kV. The angular scan was performed in discrete steps of 0.05° (2θ) with a counting time of 5 seconds per step.

Results and Discussion

Effect of the Solution pH

The pH of the aqueous solution has a major effect on the protonation and deprotonation of the functional groups of the Montmorillonite surface. The effect of pH on adsorption of MG on Na-MMC was examined through an agitation of 40mg of adsorbent with 100 mL of MG dye solution of 1,4mmoL/L concentration at different pH values from3 to 11. The solution pH was adjusted by HCl or NaOH solution.

Using Marvin Sketch³⁷, which is a software for structure property prediction and calculation, we have calculated the cationic MG charges at different pH, the results are shown on Figure 1. From the obtained results, we observe that the adsorption of MG increases with the initial pH values.

The adsorption of MG on the Na-MMC increases, from 176.7 to 249 meq/ 100g while the pH value increases from 4 to 8. The previous studies have shown that at high pH values, the cations are adsorbed due to the negatively charged surface sites of the Montmorillonite ^{2, 38-40}. In aqueous solution, the Montmorillonite surface hydroxyl site (M-OH), such as alumina, undergoes the protonation/deprotonation process ⁴¹. An alkaline environment gives rise to more negative charges on the Montmorillonite hydroxyl group’s ( Eq.10), which leads to an increase in the density of the negative charge on the external surface of the clay and consequently the MG adsorbed amount increase at higher pH value.

Compared to other adsorbates, the significant observed increase of the GM adsorption with the pH value can be explained by the deprotonation of GM at higher pH value (Figure 1) and, consequently, by the small positive charge density of MG at a higher pH. This promotes nonspecific adsorption (Eq.3) after surface charge reversal ³¹ and thereby increases the adsorbed amount at high pH. More, this modeling shows that the MG charge is stable (at the value 1) when the pH is greater than 7, it confirms the stability of the amount of MG adsorbed in this pH range (Figure 1). Because the surface charge of montmorillonite in the presence of sodium remains constant ⁴² when the pH> 7.

Effect of Initial Malachite Green Concentration

The effect of initial malachite green dye concentration was studied at different initial MG dye concentrations in the range of 25–400 meq dye/100g at 298 K with 0,04 g of Na-MMC at the solution pH. The results presented in Figure 2 showed that the equilibrium percent of adsorption efficiency A% slightly increases with increasing initial dye concentration.

Afterwards, the adsorption capacity marks a sudden decrease with further increasing in the initial concentration of MG. Theoretically and according to the Boltzmann’s law, the decrease of the adsorption percent with the increase in the initial dye concentration is attributed to the reduction of sites charged on the surface of the clay. This has been experimentally analyzed by using X-Ray diffraction (XRD). Tracking the 001 peak position by DRX has shown a displacement of this peak Figure 3, after adsorption, the basal distance increases, which indicates that the exchange process between sodium and GM was carried out.

The measurement of the interlayer space distance or the basal spacing of the montmorillonite after adsorption, for each initial concentration of MG showed that this distance has a simulated variation by comparison with the percentage of the adsorption as shown in Figure 4.

In the range 0-100 meq/100g, where the adsorbed quantity is lower than the CEC, the increase in the basal space is explained by the replacement of the hydrated sodium cations by MG organic cations. However, a quantity of sodium ions compensates negative charges on the surface of the clay since the amount of dye is lower than CEC.

The measurement of the interlayer space distance or the basal spacing of the montmorillonite after adsorption, for each initial concentration of MG showed that this distance has a simulated variation by comparison with the percentage of the adsorption (Figure 4). In the range 0-100 meq/100g, where the adsorbed quantity is lower than the CEC, the increase in the basal space is explained by the replacement of the hydrated sodium cations by MG organic cations. However, a quantity of sodium ions compensates negative charges on the surface of the clay since the amount of dye is lower than CEC. According to the bibliographic literature, in an excess of water, the sodium ions in the interfoliair space of montmorillonite are bi or tri-hydrated ^43-47 and since the radius of the sphere of hydration varies from 14,5 Å to 19 Å (Table 4). The geometric optimization of the GM molecule in water as a solvent by the method described above, assigns a non-plane structure Figure 10 (a) and a strong positive electron density around the atoms of nitrogen Figure 10(c).

Theoretical calculations, estimates the thickness of the non-plane molecule MG at 5Å. The spacing of the aluminosilicate layer is 9.5 Å ¹⁵, when the amount of dye is less than 50 meq/100g The basal spacing is 14,6 Å, hence the value of the interlayer spacing is 5,1Å. This value confirms the non-planar structure geometrical of the molecule, a situation corresponding to the presence of two MG molecules between the clay plates along the axis C (Figure 5(a)). When the amount of added MG increases and tends towards CEC, the presence of a small amount of sodium give rise to MG molecules a take inclined orientations with respect to the platelets of the clay (Figure 5(b)). Which explains the increase in the basal distance to 22 Å. At dye concentrations greater than the CEC of the clay, the amount of sodium adsorbed is nil (negligible). In this case, an order of orientation of the GM molecules parallel to the platelet increases the basal spacing of montmorillonite see Figure 5(c).

Adsorption Isotherms

The relationship between the amounts adsorbed Qad for MG per 100g mass of Na-MMC as a function of total dye concentration in the solution is plotted in Figure 6. The pH was measured and found to be between 3.5 and 5.75 for all samples.

The amount of adsorption increases with the increase of the MG concentration according to a linear law Qad = C₀up to the value of 110meq/100 g, the latter corresponds to the CEC value of thesodic Montmorilloniteused, as it is mentioned in theoretical model (Eq.1). At amounts less than the CEC of theclay, all the dye was essentially adsorbed, indicating a very large affinity ofthe dyes to Montmorillonite, ashas been previously reported. The saturation level were 177 meq/100g of Montmorillonite (close to 163% of the CEC). Thisgreat affinity after CEC has been demonstrated for triphenylmethane organicdyes. Other studies on the adsorption ofsimilar dyes on the even support (the Nador Na-MMC),have shown this great affinity for the crystal violet (CV), that has a closestructure to the malachite green with amaximum adsorbed quantity greater than180 meq/100g clay ³⁹. For the Crystal Violet, G. Rytwo and als, have determinedby using the model GCS the values of the binding coefficients K and K’ (Table3), the coefficient binding value of the K’ is greater than K, which is attributedto the strong attraction between the dye and the neutral complex (Eq.3)via others bonds ⁴¹.

Table 3: Binding coefficients of the some cations

Cation	Binding coefficient for neutral complex Κi [M– 1] 15, 27	Binding coefficient for charged complex Ḱi [M– 1] 15
Lithium (Li+)	0,6	–
Sodium (Na+)	1	–
Potassium (K+)	2	–
Cesium (Cs+)	200	–
Crystal violet (CV)	106	8.109

It is thus deduced that the specific absorption (Eq.1) requires that the surface of the clay have high affinity to the Triphenylmethane organic dyes such as crystal violet ^{15, 39} and GM in our work. From theprevious results, we can conclude that montmorillonite from Nador (North eastof Morocco) show superior properties for the adsorption of our dye MG comparedto other clays such as montmorillonite Wyoming SWy-1 ^{11, 15, 31}.

Effect of Various Alkali Chloride Salts on Equilibrium MG Adsorption

The effect of various metals alkali chloride salts on Malachite green removal by Na-MMC has been systematically investigated and the results are presented in Figure7. When a maximum quantity (C₀ = 350 meq/100g) of dye was added. It has be found that the type of cations has a significant effect on malachite green removal. The removal rate of malachite green decreases with the introduction of cesium and potassium inorganic cations while it slightly increases in the presence of lithium chloride salt and sodium chloride. This can be explained by the competence of inorganic cations to be adsorbed onto negative sites of montmorillonite. That may decrease the amount of organic molecules MG adsorbed from the first layer to the clay surface when the initial dye concentration is below the CEC (specific adsorption Eq.1). The results have been analyzed in the framework of the model GCS (Nir 1984, 1986) ^{27, 48, 49}, that has been already employed for the study of specific adsorption to Montmorillonite of Li⁺, Na⁺, K⁺, Cs⁺and of the hydration sphere for each of the inorganic cations. Table 4 shows that the decrease of the GM adsorption in the presence of cesium or potassium is related to their values of binding coefficient K (Table 3). Lithic and sodium montmorillonites show similarities in the relative abundances of different hydration states ^{43, 50}. This can be explained in particular by the ionic radiation sizes and hydration energies, which are close enough for the two cations. Although they have not determined the basal distance, Berend and als demonstrated that the tri-hydrated state is likely to form in lithic montmorillonites for very high water contents (aqueous solution) ⁴³, this strong hydration decreases the attraction force to the clay surface and consequently increases the amount of GM adsorbed.

The results found in the literature show that the stable state for cesium montmorillonite is the mono-hydrated state ⁴³, hence the bindingforce between the clay and the cesium ions is very large compared to othercations K = 200 M^-1(Table3), this strong interaction decreases theamount of GM adsorbed which explains the experimental results obtained in thiswork.

Potassium has an ionic radius and an intermediate hydration energy (Table 4) between those of lithium and sodium on the one hand, and those of cesium on the other hand. This certainly justifies why the tri-hydrated state is not observed experimentally in the montmorillonites potassic. In addition, the bi-hydrated and the mono-hydrated states exist only for very high water contents ^{43, 50, 51}. This explains the value of binding coefficient K = 2M^-1, which has been determined by Nir et als. and also the weak interactions with respect to cesium at the surface of the clay. Therefore, the presence of potassium reduces the amount of GM adsorbed because a small amount of potassium adsorbs onto the surface of the clay.

Table 4: Basal distance of montmorillonite in the presence of a single type of alkaline cation in the interlamellar space

Alkaline cations	Ionic radius (A) 52, 53	Hydration enthalpies (KJ/moL) 54	Basal distance of montmorillonite in the presence of a single type alkaline cation (Å)
			Monohydrate 45, 46 50, 55 43, 44	Dihydrate 45, 55,43, 50	Trihydrate 56,55, 57
Li+	0,76	-520	—	—	22,5
Na+	1,02	-406	12,20 – 12,58	14,5 – 15,6	18,10 – 19
K+	1,38	-320	12,40 – 12,65	15,55 – 16,0	—
Cs+	1,67	-264	12,6 – 12,3	—	—

Ionic Strength Effect over the Adsorption Isotherm of GM onto Na-MMC

According to the previous results, the experimental study of the effect of the ionic strength is concentrated on the small and the large cation (lithium and cesium). The ionic strength was adjusted with 0M, 0.02 M, 0.2 M and 1 M saline to the target values. The amount of MG removed as a function of initial dye concentrations for each ionic strength of salt (lithium chloride or cesium chloride) was measured and the results are displayed in Figure 8 and Figure 9.

To simplify the analysis of the adsorption isotherms obtained based on the GCS model detailed above, the curves are decomposed in two parts, before and after CEC = 109meq/100g of clay.

For initial dye concentrations below the CEC value (adsorption modeled by Equation 1), the ionic strength of lithium chloride has no effect on the adsorption isotherm (Figure 8). The interpretation of this result is reported (Rytwo et als) by the very low value of the lithium (Table 3) binding constant K (Eq.1 and 2) with respect to the same dye value ²², the closest reason is the strong hydration of the lithium ion ^{43, 53}. Interestingly, we observe a significant decrease for GM adsorbed when the ionic strength of cesium chloride increases (Figure 9), compared to lithium. Two important factors accounting for this decrease, (1) the highest value of the ion binding constant K_Cs> 400K_Li (Table 1) and (2) his low hydration (monohydrate) ^{43, 44, 53}. The first leaves a quantity of cesium ions adsorbed on negative charges in interlamellar space. In general the clay minerals have a high affinity with the large inorganic cations ^{58, 59}, studies show that the adsorption of cesium on montmorillonite is favored compared to other alkaline ions^{27, 60}. The second factor complicates the adsorption of the GM molecules in this space, because the radius of the hydration sphere of cesium ion is smaller than the size of the GM molecule. If the amount of dye added is greater than the cation exchange capacity (CEC), a charge reversal occurs at the surface of the clay; therefore, the cations diffuse to the core of the solution by electrostatic repulsions according to the equations Eq.5 and Eq.6.

The increase of the ionic strength in lithium chloride favors the adsorption of the GM cations, because the increase of the concentration of lithium ions in the core of the solution (far from the positive surface), increases that of the MG at the surface of the clay. According to Table 3, the binding coefficients of the monovalent organic dyes being very important ²², therefore the improvement of the GM adsorption is due to the strong interactions between the complex over face and the organic dyes (Eq.3).

DFT Investigations

The full geometry optimization of MG dye were performed to investigate the structure geometry in the gas phase applying DFT/B3LYP. As illustrated in Figure 10 (a), the optimized structure are not planar. We notice that the three fragments (1 unsubstituted and 2 substituted phenyl) of the molecule take an arrangement to reduce steric hindrance and obtaining a stable geometry.

Density Functional Theory (DFT) has become a successful tool to acquire a better understanding of chemical reactivity and stability about molecules, the examination of the frontier molecular orbitals is an important key to get insights into reactivity and studying electron excitation from the highest occupied molecular orbital (HOMO) to the lowest unoccupied molecular orbital (LUMO). The LUMO corresponds to the ability of the molecule to capture an electron, the HOMO represents the ability to donate an electron. The HOMO-LUMO energy gap refers to the difference between the HOMO and the LUMO energy values, which indicates the charge transfer interaction taking place within the molecule.

In general, molecules with a small energy gap are attributed to a high chemical reactivity, low kinetic stability and are also defined as soft molecules, those with large energy gap have higher stability and are considered as hard molecules for the reason that they resist charge transfer and changes in their electron density and distribution ^61-64.

The energy of HOMO is directly connected to the ionization potential (IP = -E_HOMO) and the energy of LUMO concern the electron affinity (EA = -E_LUMO) ⁶⁵. Additionally and by utilizing these values, attractive properties such as chemical hardness (η), electrophilicity index (ω) and electronic chemical potential (μ) can be obtained. The chemical hardness is an indication of how molecule are polarizable and how much is the distortion of electron cloud in an electric field. The hardness and softness were reported in literature ^{61, 62}. Chemical potential indicates the affinity of an electron to fleeing and present the first derivative of the total energy with respect to the number of electrons in a molecule ⁶⁶. Electrophilicity index concern the aptitude to accept electrons and it provide a quantification of the electrophilic power in a molecule ⁶⁷. Table 5 present the calculated parameters values and certain properties of MG(in this work) and CV ³⁹ dyes in order to compare with each other .

Table 5: Calculated quantum chemical parameters (eV) using B3LYP/6-31G(d).

Dye	EHOMO	ELUMO	HOMO-LUMO gap	η	μ	ω
MG	-8.203	-5.620	2.583	1.291	-6.911	18.495
CV	-7.859	-5.163	2.696	1.348	-6.511	15.724

From the reported results, the HOMO_LUMO gap, chemical hardness (η) and electronic chemical potential (μ) of MG is comparable to thus of CV, which indicate a similar electronic reactivity of the Triphenylmethane organic dyes. Furthermore, the higher electrophilicity index (18.495 eV) indicate the good ability of MG to accept negative charges. This suggests that the interactions between MG and the surface sites are strong and more important than those of CV .

As it is shown in Figure 10 (b), the HOMO are mainly localized on the two substituted phenyl, the LUMO get their contribution from the whole molecule. These results suggest that the primary interaction (Eq.1) with the charged surface is assured by the totality of MG molecule; however, the secondary type of binding (Eq.3) comes from the two-amine arm parts.

MEP mapping is a very useful technique for predicting favorable sites for electrophilic and nucleophilic reactions or for revealing preferred sites for non-covalent electrostatic interactions. An isosurface of electron density mapped with electrostatic surface potential represents the size, shape, charge density, the electrophilic sites, nucleophiles, hydrogen bonds and coordination sites in the molecule. The mapped electrostatic potential (MEP) are normally represented by different colors and the increasing order of their magnitude is: red0, while regions with MEP<0 are repulsive. In our case, the MG molecule is an organic cation, which possess a large conjugated system with an electrostatic potential which is totally positive, and a possible electrostatic interactions is highly favorable particularly on negative charged surfaces like our clay.

When the amount of GM is less than CEC, the charged surface of MMC interact with MG molecule electrostatically and the nature of MEP (Figure 10(c)) surface suggest a good primary binding coefficient K (Eq.2), also the LUMO confirm that interactions can be made with the majority of MG molecule surface. After CEC, a charge reversal of clay occurs, in this case, HOMO-MG can give electron density by the two substituted and linked sides (amine and Pi system). The interaction are concentrated and localized on only one side, in fact, the binding K’ (Eq.4) becomes more important (K’>K).

Conclusion

In this study, a Moroccan sodic Montmorillonite was tested for its adsorption capacity to remove green malachite from aqueous solutions in the presence of various inorganic salts, ionic strength and pH solution. The experiments indicated that Na-MMC possesses excellent adsorption capacity for GM removal from aqueous solution at pH 10. The results also indicate that the presence of lithium or sodium salts at solution pH improves the maximum amount adsorbed. However, the removal rate of MG has very affected by the increase in the ionic strength of cesium chloride; at equilibrium, there is a serious decrease in the adsorbed amount. The theoretical investigation using the GCS model and the reported data was in a great agreement with experimental results, it allow us to propose the structure of the interfoliar space after the adsorption. The calculated quantum parameters explained electronically the type of interaction, which are taking place before and after CEC. MEP and molecular orbitals frontiers (HOMO-LUMO) suggest the electrostatic binding with MNC.

This study demonstrated that crude bentonite extracted from a clay deposit in the Nador region (northeast of Morocco) purified and active by sodium is a promising adsorbent for environmental pollutants, even if in the presence of some inorganic salts

Acknowledgment

The authors are sincerely thankful to MESRSFC and CNRST –Morocco for financial support of Project PPR 15-17.

Conflict of Interests

The authors declare that there is no conflict of interests regarding the publication of this paper.