Retention Factors for Trace Metal Elements in Solid Phase and Applicable Adsorption Models: Case of Moringa oleifera

Mariette Désirée Yehe^1,2*, Edwige Odoh³, Patrick Grah Atheba⁴, Joel Cyriaque Dadje¹, Gildas Komenan Gbassi^1,2

¹Département des Sciences Analytiques et Santé Publique, UFR Sciences Pharmaceutiques et Biologiques, Université Félix Houphouët Boigny, Abidjan, Côte d’Ivoire.
²Laboratoire National de la Santé Publique (LNSP), Service Contrôle des Aliments, Abidjan, Côte d’Ivoire.
³Département des Sciences du Médicament, UFR Sciences Pharmaceutiques et Biologiques, Université Félix Houphouët Boigny, Abidjan, Côte d’Ivoire.
⁴Laboratoire de Constitution et Réaction de la Matière, UFR Sciences des Structures de la Matière et Technologie, Université Félix Houphouët Boigny, Abidjan, Côte d’Ivoire.

DOI: 10.4236/ojpc.2021.113011                

Abstract

Moringa oleifera is an edible plant cultivated throughout the tropical belt. It belongs to the family Moringaceae and is one of its 14 known species. This paper presents a synthesis of the main factors responsible for the retention of trace metal elements (TMEs) by Moringa oleifera seed powder, a natural adsorbent. The five main factors studied are metal concentration, solution pH, adsorbent particle size, adsorbent dose and adsorbent/adsorbate contact time. Through these factors, we present the optimal conditions for removal of these TMEs, as well as adsorption isotherm models appropriate for the conditions of retention of these metal cations by the adsorbent. The times of 20 min (GD) and 50 min (GND) are the equilibrium times obtained in our study. An optimal adsorbent mass (GD and GND powders) of 4.5 g was found. 20% to 97% abatement is observed for average pH values between 6 and 8. The coefficients of determination (R2) obtained (0.972, 0.963, 0.991 and 0.799) during the isotherm experiments carried out at 20°C, 30°C, 40°C and 50°C are close to 1. Also, the separation factor (R_L), an essential characteristic of the Langmuir isotherm whose values are between 0 and 1, attest to the applicability of the Langmuir isotherm model to fit the experimental data of copper adsorption by Moringa powders. In this paper, we are particularly interested in the following TMEs (Mn, Ni, Cr, Cu, Cd, Co, Pb, Fe, Zn, Ag).

Keywords

Moringa oleifera, Adsorption, Trace Metal Elements (TMEs)

1. Introduction

The term “trace metal elements” (TMEs) is tending to replace the term “heavy metals”, which has no real scientific or legal definition that is unanimously recognized [1]. TMEs are naturally present in soils, some of which are essential for plants. They are found in run-off water from roads and commercial areas, metal foundries, plastic effluents, textiles, microelectronics, wood industries, agriculture (fertiliser and pesticide use) but are largely derived from industrial waste [2] [3].

TMEs can be removed from aqueous solutions by conventional methods (precipitation, redox, ion exchange, mechanical filtration, electrochemistry, reverse osmosis) [4]. However, the inefficiency and extremely high cost of these methods limit their use, and the environmental side effects have led to a growing interest in plant-derived adsorbents, such as Moringa oleifera (MO) [5]. The latter has several advantages over synthetic adsorbents.

In Ivory Coast, the most used natural adsorbents are made from coconut shell-activated carbon [6]. Faced with this observation, we wanted to valorize other (local natural adsorbents, other than activated carbons. Thus, we were particularly interested in powders from hulled and unhulled seeds of Moringa oleifera, a tree that has the advantage of being locally known and used. Indeed, a comparative study conducted in Abidjan by Tanauh [7] showed that Moringa occupied a knowledge level of 78.2% by the study population in Abidjan. It is known as a miracle tree, good for health and possessing several virtues. Also, the literature mentions studies using separately as natural adsorbent the powder from dehulled Moringa oleifera seeds [8] on the one hand and the hulls of Moringa oleifera seeds [9] on the other hand, but there are no previous studies using unhulled Moringa oleifera seed powder as a natural adsorbent for metal adsorption.

2. Retention Factors for TMEs

A number of works mention the use of MO to remove TMEs from aqueous solutions. This work reviews different parameters studied during the removal of TMEs by MO, as well as the adsorption isotherm models applicable to this adsorbent. The TMEs studied in this work are found in water in cationic form, i.e. Mn²⁺, Ni²⁺, Cr³⁺, Cu²⁺, Co²⁺, Fe²⁺, Zn²⁺, Cd²⁺, Ag²⁺, Pb²⁺.

The preparation method of Moringa seed powders and the physicochemical, structural and morphological parameters have been previously described in our article published in June 2019 [10].

2.1. Effect of Metal Concentration

Farrokhzadeh et al. [11] worked on the removal of TMEs (Mn²⁺, Ni²⁺, Cr³⁺, Cu²⁺, Fe²⁺, and Zn²⁺) by deshelled MO seed powders in aqueous solution. They reported an initial metal concentration of 50, 100 and 200 mg∙L⁻¹, with an adsorption percentage of 35% at the minimum concentration of 50 mg∙L⁻¹. An increase in the initial concentration decreased the adsorption percentage.

Bhatti et al. [3] in their study on Zn²⁺ removal by MO pod biomass also reported an initial metal concentration of 50, 100 and 200 mg∙L⁻¹, with an adsorption percentage of 74.76% at the minimum concentration of 50 mg∙L⁻¹. An increase in the initial concentration also decreased the adsorption percentage.

Sharma et al. [7], in their study on the removal of cadmium (Cd²⁺) by dehulled MO seed powders, observed that for an initial metal concentration ranging from 10 - 100 mg∙L⁻¹, the adsorption percentage increased reaching a constant level of 85% at 25 mg∙L⁻¹.

Kalavathy and Miranda [2] studied the adsorption of Cu²⁺, Ni²⁺ and Zn²⁺ in the aqueous phase by activated carbon from MO wood. They reported initial concentrations ranging from 10 - 50 mg∙L⁻¹. The amount of metal adsorbed per unit weight increased with the initial metal concentration. The maximum adsorption capacity is 10.08 mg∙g⁻¹; 17.48 mg∙g⁻¹ and 14.16 mg∙g⁻¹ for Cu²⁺, Ni²⁺ and Zn²⁺ respectively.

The authors asserted that the lower the initial metal concentration, the greater the removal of this metal. This observation may be due to the saturation of the binding site of the adsorbent with the metal or to the fact that the rate of adsorption is a function of the initial adsorbate concentration.

2.2. Effect of Solution pH

Farrokhzadeh et al. [11] reported three pH values: pH 3, pH 5 and pH 7 in their study on the removal of metals (Mn²⁺, Ni²⁺, Cr³⁺, Cu²⁺, Fe²⁺ and Zn²⁺) by MO seed powders in aqueous solution. They asserted that the adsorption percentage was higher (30%) at pH 7. The removal of Fe²⁺ and Cu²⁺ increased with increasing pH of the solutions, which was in compliance with previous studies [11] [12]. However, the minimum removal efficiency of Ni²⁺, Cr³⁺ and Zn²⁺ (25%) was obtained at pH 5. On the other hand, Mn²⁺ had the highest removal efficiency at pH 5. Bhatti et al. [3] also showed that the adsorption of Zn²⁺ increased with increasing pH.

Sharma et al. [8], in their study on Cd²⁺ removal by MO seed powder, observed that the percentage adsorption of Cd²⁺ by plant biomass increased as the pH of the solution increased from 4.5 to 8.5. The adsorption profile of Cd²⁺ by MO powder shows that the adsorption is pH dependent, with a maximum adsorption of 84% at pH 6.5. Ajmal et al. [9] showed an increase in Cd²⁺ adsorption up to pH 8.5.

Araujo et al. [13] worked on the characterization and use of MO seeds as a biosorbent to remove ions (Cd²⁺, Pb²⁺, Co²⁺, Cu²⁺, Ag⁺) from aqueous effluents. They reported an optimum pH value of 6.5 for a pH range initially between 2 and 8. Furthermore, Alves et al. [14] noted that above pH 6.5, the surface of the adsorbent is negatively charged and adsorbs positively charged species. The percentage removal of metal ions can be explained, according to Araujo et al. by the difference in the size of the ionic radius of the chemical species. Among TMEs studied, Pb²⁺ had a larger ionic radius and therefore a higher adsorption capacity, while Co²⁺ had a lower adsorption capacity [15].

Bhatti et al. [3] worked over a pH range from 3 to 11. They observed a negligible adsorption at pH 3, indicating the possibility of using this pH for TME elution and biomass regeneration. Their results clearly indicated that Zn²⁺ adsorption increased from pH 3 to pH 7 but decreased from pH 7 to pH 11. This increase in Zn²⁺ removal with increasing pH up to 7 was also demonstrated by Matos et al. [16] using fungal biomass.

Kumar et al. [14] worked on the adsorption of Ni²⁺ in the aqueous phase by the bark of MO. Under very acidic conditions (pH 2), the amount of Ni²⁺ removed was very low (20%), whereas adsorption was high (35% to 97%) from pH 3 to 6 and then decreased (97% to 78%) when pH increased from 6 to 8.

Kalavathy and Miranda [2] worked at different pH values ranging from 2 to 10 for the adsorption of Cu²⁺, Ni²⁺ and Zn²⁺ in the aqueous phase by activated carbon from MO wood. They observed a very low adsorption in the pH range from 2 to 4 (0.2% to 0.8%). By increasing the pH above 6, the adsorption capacity increased rapidly from 1% to 1.5%. An optimal pH of 6 was chosen because metal hydroxide precipitation was observed at pH above 6. These data were in agreement with the results obtained by Kalavathy et al. [17].

All these authors having studied the effect of the pH of the metal solution, made a general observation that the pH is one of the most important parameters for any adsorption process.

The relationship between pH and TME removal could be related to the functional groups of the adsorbent used as well as to the nature of the mineral species in solution. Due to their ability to interact with metal ions, these functional groups are likely to increase the adsorption of metal ions [17]. From pH 2.5 to 5, a high number of hydrogen and hydronium ions compete with metal ions for the metal binding sites on the adsorbent, resulting in poor adsorption of the latter. At pH values between 5 and 7, there is little competition due to a lower number of hydrogen ions [18].

2.3. Effect of Moringa oleifera Particle Size

The effect of Moringa oleifera particle size has been discussed by several authors (Table 1).

Farrokhzadeh et al. [11] worked with MO seed powder particles that were prepared in three categories A, B and C (A < 0.125 mm; 0.125 mm < B < 0.420 mm and 0.420 mm < C < 1.180 mm). For these authors, the larger the particle size is, the greater the efficiency of metal removal is. However, some studies reported very small particles of adsorbent [3] [8].

Araujo et al. [10] worked with MO seed powder particles ranging in size from 0.075 mm to 0.500 mm, which is smaller than those used by Farrokhzadeh et al. [11]. However, particles with a size close to 0.500 mm gave better metal removal (Ag⁺, 2.31%).

Bhatti et al. [3] worked with MO particles whose size varied from 0.250 mm to 0.500 mm. According to these authors, the efficiency of the removal of Zn²⁺ decreased with increasing particle size (from 0.250 mm to 0.500 mm). Total surface area provides more adsorption sites for the metal ions.

Sharma et al. [8] worked on three different particle sizes of MO seed powders (0.105 mm, 0.210 mm and 0.420 mm). The removal efficiency of Cd²⁺ was 85.10%, 70.04% and 52.20% for particle sizes of 0.105 mm, 0.210 mm and 0.420 mm respectively.

Kalavathy and Miranda [2] used 0.074 mm particles. They obtained an average removal efficiency of 58.7% for Zn²⁺, Cu²⁺ and Ni²⁺.

The effect of MO particle size has been a much debated parameter in all previous works. For some authors, the larger the particle size is, the higher the metal removal efficiency is [11] [13] while other authors have reported the opposite effect [3] [8].

2.4. Effect of Adsorbent Dose

Table 2 shows the results in relation to the effect of adsorbent dose discussed by

Table 1. Effect of adsorbent particle size.

Table 2. Effect of adsorbent dose.

AAS: Atomic Absorption Spectrometry.

the authors.

Farrokhzadeh et al. [11] observed a positive relation between the removal efficiency of TMEs and the adsorbent concentration. In the case of Cu²⁺, the removal efficiency decreased (70% to 9%) when the MO dose was increased from 5 - 10 g/L and then increased (9% to 70%) when the dose was increased from 10 - 20 g∙L⁻¹. Also, they noted a lower removal of Cr³⁺ and Mn²⁺ (70% to 22%) than that of Zn²⁺, Cu²⁺ and Fe²⁺ (70% to 40%).

This effect was also reported by Bhatti et al. [3] and Sharma et al. [8] in their respective work on the removal of Zn²⁺ and Cd²⁺.

Araujo et al. [13] worked with adsorbent concentrations ranging from 0.1 - 4 g∙L⁻¹ and the maximum removal efficiency (2.31%) was obtained with a mass of 2 g.

Bhatti et al. [3] worked with an adsorbent concentration of 0.5 g∙L⁻¹ while Sharma et al. [8] used 2 - 6 g/L.

Kumar et al. [19] used 0.1 - 0.8 g∙L⁻¹ and observed a maximum adsorption of 92% with 0.4 g∙L⁻¹.

Kalavathy and Miranda [2] used concentrations from 0.5 - 7 g∙L⁻¹. The dose of 0.5 g∙L⁻¹ was the optimum dose in their study for removal of copper, nickel and zinc.

2.5. Effect of Adsorbent-Metal Contact Time

The results in relation to the effect of adsorbent metal contact time are presented in Table 3.

Bhatti et al. [3] used a time between 10 min and 640 min. The optimum adsorption time was 50 minutes.

Sharma et al. [8] studied for a time between 10 min and 60 min. The percentage of adsorption increased gradually from 10 min to 30 min to reach the optimum value at 40 min. Once equilibrium was reached, the percentage adsorption did not change with time.

Araujo et al. [13] worked between 5 - 50 min and equilibrium was reached in 20 min. Kumar et al. [19] worked between 5 - 100 min and equilibrium was reached in 60 min. Kalavathy and Miranda [2] worked with a time range from 0 - 300

Table 3. Effect of adsorbent/adsorbate contact time.

AAS: Atomic Absorption Spectrometry.

min with a maximum adsoprtion in 240 min for copper, 60 min for nickel and 180 min for zinc. There was no significant change in equilibrium concentration after 240, 60 and 180. Contact times and equilibrium times differ from one metal to anothers

3. Adsorption Isotherm Models for Moringa Powder

Studying isotherm models of metal adsorption by MO seed powders are mainly based on these three models (Langmuir, Freundlich, Temkin) and the choice of the best adsorption model for each TME is indicated in Table 4.

3.1. Langmuir Isotherm Model

The first fundamental theory of gas adsorption on solids was proposed by Langmuir in 1918 and remains one of the most widely used models in the literature for liquid phase adsorption phenomena [21]. This model is based on the following assumptions:

· Adsorption is localized and only results in the formation of a monolayer;

· All sites are equivalent: the surface is uniform;

· There is no interaction between the adsorbed molecules;

· The reaction is reversible (i.e. there is an equilibrium between adsorption and desorption).

Table 4. Adsorption isotherms.

The Langmuir isotherm is represented mathematically by the equation:

$q_e=q_m\left[\left(K_L{C}_e\right)/\left(1+K_L{C}_e\right)\right]$ (1)

q_e (mg∙g⁻¹): the quantity of adsorbed species per gram of solid at equilibrium;

q_m (mg∙g⁻¹): the quantity of adsorbed species per gram of solid necessary to cover the surface of the solid with a monolayer; C_e (mg∙L⁻¹): the residual concentration of liquid at equilibrium; K_L (L∙mg⁻¹): the Langmuir thermodynamic constant linked to the adsorbate-adsorbent system (specific adsorption constant of the adsorbate on the adsorbent).

The characteristics of the Langmuir isotherm can be expressed by a dimensionless term, called the equilibrium parameter R_L [22], which is widely used in the field of chemical engineering for the dimensioning of industrial adsorbers and whose usefulness is the knowledge of the type of equilibrium (favourable or unfavourable for adsorption). This parameter is defined by the relation:

$R_L=1/\left(1+K_L{C}_0\right)$ (2)

C₀: Initial concentration (mg∙L⁻¹); K_L: Langmuir constant (L∙mg⁻¹).

The equilibrium is said to be:

· Favourable if R_L < 1;

· Unfavourable if R_L > 1;

· Linear if R_L = 1;

· Irreversible if R_L = 0.

Table 5 summarises the results of the equilibrium data for the adsorption of TMEs by MO seed powders that were described by the Langmuir isotherm model.

3.2. Freundlich Isotherm Model

In 1926, Freundlich proposed another model to describe adsorption in gaseous or liquid media [24]. This model is based on the distribution of pollutants between the surface of the adsorbent and the liquid phase at equilibrium and takes into account the heterogeneity of the adsorbent surface. It is based on the following assumptions:

· Existence of adsorbed multilayers;

· Absence of saturation phenomenon;

· Possibility of interaction between the adsorbed species;

· Heterogeneous distribution of adsorption energies.

The Freundlich isotherm model is represented by a two parameter equation (K_F and n) given by the following relation.

$q_e=K_F{C}_e^{1/n}$ (3)

where K_F (mg∙g⁻¹) and 1/n represent the Freundlich constant and the adsorption intensity respectively.

K_F and 1/n are the Freundlich constants to be assessed for each solution and for each temperature. The feasibility of the adsorption process depends on the value of 1/n:

Table 5. Adsorption of TMEs by MO seed powders described by the Langmuir isotherm model.

· 1/n < 1 implies a favourable adsorption;

· 1/n > 1 implies an unfavourable adsorption.

Table 6 summarises the results of the equilibrium data for adsorption of TMEs by OM seed powder that were described by the Freundlich isotherm model.

3.3. Temkin Isotherm Model

The Temkin isotherm is used in several adsorption processes. This model considers a non-uniform surface, a preferential occupation of the most adsorptive sites and an interaction between the adsorbate molecules and the adsorbent material. Temkin’s model is based on the assumption that, during gas phase adsorption, the heat of adsorption due to interactions with the adsorbate decreases linearly with the recovery rate θ. Dipu et al. [25] propose to use this model in the liquid phase by plotting q_e or θ as a function of ln(C_e) given by the following relationship.

Table 6. Adsorption of TMEs by MO seed powders described by the Freundlich isotherm model.

$q_e/q_m=RT\left(A_T{C}_e\right)/\Delta Q_L$ (4)

The linear form of the Temkin isotherm is given by the following équation:

$q_e=B\ln A_T+B\ln C_e$ (5)

where B = RT/b_T (J∙mol⁻¹) is related to the heat of adsorption; R the perfect gas constant (8.314 J∙K⁻¹∙mol⁻¹); T (K) the absolute temperature; b_T the Temkin isotherm constant; ΔQ the change in adsorption energy (J∙mol⁻¹) and A_T (L∙g⁻¹) the equilibrium binding constant corresponding to the maximum binding energy.

In Table 7, the results of the equilibrium adsorption data of TMEs by MO were described by the Temkin isotherm model.

Farrokhzadeh et al. [11] showed in their study on the removal of TMEs (Mn²⁺, Ni²⁺, Cr³⁺, Cu²⁺, Fe²⁺ and Zn²⁺) by deshelled M. oleifera seed powders in aqueous solution that the appropriate isotherm model for Zn²⁺ adsorption was the Langmuir model. The graphical representation of this model [1/q_e =f(1/C_e)] gave a straight line with a coefficient of determination R² = 0.99, R_L values between 0 and 1 (0.045; 0.023; 0.087) with a maximum adsorption capacity of 2.09 mg∙g⁻¹.

The Langmuir and Freundlich isotherms were appropriate for Cr³⁺. The Temkin isotherm was the best model for the adsorption of Fe²⁺, Cu²⁺and Mn²⁺. In the

Table 7. Adsorption of TMEs by MO seed powders described by the Temkin isotherm model.

case of Ni²⁺, the adsorption reaction could not be associated with the isotherms studied.

Bhatti et al. [3] studied Langmuir and Freundlich isotherms for the metal ion Zn²⁺. These authors show that the coefficients of determination (R²) of the two models are 0.994 and 0.995 respectively. This indicates that both models correctly describe the experimental data of these Zn²⁺ metal adsorption experiments.

Sharma et al. [8] analysed the Cd²⁺ adsorption data using the Freundlich isotherm which accurately described the adsorption behaviour of this ion.

Kumar et al. [19] applied the experimental data to the Langmuir, Freundlich, and Temkin isotherm models. In addition to determining the coefficient of determination (R²), the chi-square test (χ²) was performed to determine the best isotherm model. These authors observed from the values of the coefficient of determination R² (0.997) and the chi-square test χ² (1.413) that the Langmuir model best described the Ni²⁺ adsorption phenomenon. This was followed by the models of Temkin (0.967), Freundlich (0.945).

The previous four models were also studied by Kalavathy and Miranda [2] to describe the equilibrium data for Cu²⁺, Ni²⁺and Zn²⁺ adsorption. These authors observed R² values of 0.990, 0.970 and 0.980 respectively for the Langmuir, Freundlich and Temkin models for Cu²⁺ adsorption. However, the R² values were higher in the Langmuir model for Ni²⁺ (0.997) and in the Freundlich model for Zn²⁺ (0.995). The Temkin isotherm had a higher R² for all metal ions (0.98).

The analysis of the monolayer adsorption capacity with temperature by these authors indicates that adsorption is an endothermic process for Cu²⁺ and exothermic for Ni²⁺ and Zn²⁺. The values of the Freundlich isotherm constant (n) are between 2.17 and 2.92, which indicates a favourable adsorption process. Kalavathy and Miranda observed that the monolayer adsorption capacity (Langmuir isotherm) is maximum in the case of Ni²⁺ (19.08 mg∙g⁻¹), followed by Zn²⁺ (17.67 mg∙g⁻¹) and Cu²⁺ (11.53 mg∙g⁻¹).

Sahabi et al. [20] observed, based on the (R²) values, that the Freundlich model best described the adsorption process of Pb²⁺ and Cd²⁺ ions. The fit of the Cd²⁺ equilibrium data to the Freundlich isotherm model is in agreement with the study of. Sharma et al. [8], who had already revealed that the adsorption of cadmium by MO seed powder was consistent with this model. On the other hand, the fitting of Pb²⁺ equilibrium data to the Freundlich and Langmuir models did not agree with the findings of Adelaja et al. [26], who revealed that Pb²⁺ adsorption by MO seed powder was not consistent with these two isotherm models.

The authors generally noted that the values of (R²) and the parameters related to each isotherm (R_L, 1/n and B_T) are important factors in the interpretation of the experimental data of the TMEs adsorption process. The choice of the adsorption isotherm depends on the type of surface of the adsorbent (monolayer, heterogeneous surface...), but also on the temperature (endothermic or exothermic process). The Langmuir model assumes that adsorption is limited to a monolayer, whereas the Freundlich model is an empirical analysis describing the adsorption of solutes from a liquid on the surface of a solid, thus assuming a heterogeneous adsorption surface. The Temkin isotherm assumes that the heat of adsorption of all molecules in the layer decreases linearly with coverage due to adsorbent-adsorbate interactions.

4. Conclusions

In this article, we have presented different factors responsible for TMEs retention by MO as well as different models of adsorption isotherms that best approximate the retention capacities.

The optimal conditions for the removal of TMEs differ from one metal to another. Overall, it can be said that the different parameters (initial metal concentration, pH, particle size, adsorbent dose, contact time and adsorption isotherms) impacted the removal capacity of the TMEs present in the aqueous solutions.

However, an optimisation of these parameters must be performed, which is essential for a better performance of the adsorption process.

Conflicts of Interest

The authors declare no conflicts of interest regarding the publication of this paper.

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