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Article

Removal of Malachite Green Dye from Aqueous Solution by Catalytic Wet Oxidation Technique Using Ni/Kaolin as Catalyst

by
Abdelhak Moumen
1,*,
Youghourta Belhocine
2,
Najoua Sbei
3,
Seyfeddine Rahali
4,
Fatima Adam Mohamed Ali
5,
Fedia Mechati
1,
Fouad Hamdaoui
1 and
Mahamadou Seydou
6,*
1
Department of Petrochemical, Faculty of Technology, 20 August 1955 University of Skikda, El Hadaik Road, Skikda 21000, Algeria
2
Laboratory of Catalysis, Bioprocess and Environment, Department of Process Engineering, Faculty of Technology, 20 August 1955 University of Skikda, El Hadaik Road, Skikda 21000, Algeria
3
Institute of Nanotechnology, Karlsruhe Institute of Technology, Eggenstein Leopoldshafen, 76344 Karlsruhe, Germany
4
Department of Chemistry, College of Science and Arts, Qassim University, Ar Rass, Saudi Arabia
5
Department of Chemistry, College of Science, Imam Mohammad Ibn Saud Islamic University (IMSIU), Riyadh 11432, Saudi Arabia
6
ITODYS, CNRS, UMR 7086, University de Paris, 15 rue J.A. de Baïf, 75013 Paris, France
*
Authors to whom correspondence should be addressed.
Molecules 2022, 27(21), 7528; https://doi.org/10.3390/molecules27217528
Submission received: 4 October 2022 / Revised: 21 October 2022 / Accepted: 25 October 2022 / Published: 3 November 2022
(This article belongs to the Special Issue Wastewater Treatment: Functional Materials and Advanced Technology)
Browse Figures
Versions Notes

Abstract

:
In this study, natural Algerian kaolin was used as a support and impregnated with nickel at different loading amounts (2 wt.%, 5 wt.%, and 7 wt.%) in order to prepare a supported catalyst. The wet impregnation technique was used in this preparation; nickel oxide (NiO) was the active phase precursor of the catalyst, and the catalysts were designated as follows: 2%, 5%, and 7% Ni/kaolin. These catalysts were put to the test in catalytic wet peroxide oxidation (CWPO) for degrading the organic contaminant malachite green dye (MG). Analytical techniques such as FTIR spectroscopy, X-ray diffraction, BET, and X-fluorescence were used to examine the structure, morphology, and chemical composition of the support and the produced catalysts. Several parameters, including temperature, catalytic dose, metal loading, hydrogen peroxide volume, and kinetic model were systematically investigated. The combination of improved parameters resulted in a significant increase in the catalytic activity, achieving a high removal rate of MG dye of 98.87%.

1. Introduction

Due to the high concentration of pollutants they contain, aqueous effluents polluted by organic matter such as dyes from a chemical activity are very few biodegradable [1]. Malachite green (MG) dye is a commonly used colorant in a variety of industries, including textiles, paper, and leather [2]. However, it has been demonstrated that MG is toxic to freshwater animals in both acute and chronic exposures [3], and it is particularly toxic to mammalian organs such as the liver, kidney, and skin [4,5]. As a result, it is critical to eliminate dyestuff wastewater from the environment [6]. To achieve this goal, many scientists explored different strategies for dye removal based on physical, chemical, and biological processes [7]. Filtration, precipitation, flocculation, adsorption, and ion exchange are only a few examples [8,9,10,11,12,13].
Because it is inexpensive, adaptable, and easy, the adsorption method [14,15] is one of the most preferred processes. This is in contrast to most other methods, which are ineffectual due to the cost or are ineffective at high and/or low contamination concentrations [14]. Adsorption has the advantage of being able to be used at extremely low concentrations, as well as the ability to regenerate and reuse the adsorbent [16]. To effectively remove pollutants, several types of advanced oxidation techniques have been used, such as the wet air oxidation process (WAO); this requires very high temperatures and pressures, resulting in high installation costs, and therefore the practical uses of this process are limited [17,18]. To avoid these disadvantages, research efforts in this field have primarily focused on cost-effective and environmentally friendly alternatives, such as catalytic wet peroxide oxidation (CWPO), where hydrogen peroxide is used as an oxidant. This process produces free hydroxyl radicals (OH•), powerful oxidants of organic pollutants [19,20] which are cost-effective in decomposing the most complex contaminants [21] to inorganic compounds such as CO2 and H2O. The most notable benefit of this technique is the widespread use of heterogeneous catalysts, such as supported catalysts for water treatment [16], to reduce the severity of the oxidation conditions [17,18].
Kaolin clay is a non–toxic material that has been the subject of substantial research in the field of clays and soils due to its potential use as catalyst support. Kaolin was used as a support in the manufacture of supported catalysts in numerous studies conducted all over the world [16,20,22,23,24,25]. These catalysts have been utilized in wastewater treatment to degrade organic pollutants [20,26].
Due to their availability, low cost, and chemical qualities, transition metals such as cobalt, manganese, iron, copper, nickel, etc., and metal oxides [27,28,29,30,31,32] are the most widely utilized in the fabrication of catalysts. However, transition metal ions are dangerous and difficult to recycle, and therefore their application in wastewater treatment systems is restricted [16,33]. On the other hand, because of its high specific capacity, inherent environmental friendliness, low cost, and high efficiency, nickel oxide (NiO) has gained a lot of attention among metal oxides [34]. Nickel oxide (NiO) particles are highly frequent in catalyst coatings due to their ease of accessibility.
In this work, we have developed a supported catalyst by impregnating nickel on local natural kaolin as support. The catalytic activity against the MG dye in water [35] was evaluated by considering experimental variables such as the temperature, the oxidant amount, and the catalyst mass.

2. Experimental

2.1. Materials and Methods

Materials

The kaolin used in this work is collected in the region of Tamazert (North-East of Algeria) and procured from the sanitary ceramic company of El-Milia, Algeria.
All the chemicals employed in the present study were of analytical reagent grade. Hydrogen peroxide (H2O2), caustic soda (NaOH), nickel (II) nitrate hexahydrate Ni(NO3)2∙6H2O, and malachite green (MG) were purchased from Merck Chemical Company (Darmstadt, Germany). The chemical structure of the MG dye is displayed in Figure 1.

2.2. Synthesis of the Supported Catalysts

The supported catalysts were synthesized according to the following experimental protocol: the wet impregnation method was used to produce tailored catalysts with good dispersion of the active phase. To prepare a sufficient amount of catalyst, we started with a known mass of catalyst; from this, we calculated the mass of the kaolin support, which had been prepared beforehand, and the mass of metal impregnated with the desired loading amounts (2%, 5%, and 7%). The support (kaolin) was previously washed in distilled water and dried at 100 °C. A known concentration of the aqueous solution of precursor Ni(NO3)2∙6H2O was prepared. After that, this was added to the support (kaolin), which was first wetted in a volume of water. Complete nitrate precipitation was ensured by gradually adding NaOH until a pH of 10 was reached. Then, the mixture was put under magnetic stirring at room temperature for 3 h; at the end of stirring, the mixture underwent several treatments. To evaporate the solvents existing in the mixture, we used a sand bath at a constant temperature for 5 h.
At the end, after filtration, we used two heat treatments: drying and calcination. The solid obtained was dried in the oven for 24 h at a temperature of 80 °C, then brayed and calcined at 400 °C for 3 h. The same process was used for all of the samples (2% Ni/kaolin, 5% Ni/kaolin, and 7% Ni/kaolin).

2.2.1. Apparatus

The mineral and elemental composition of the kaolin sample was performed by X-Ray Fluorescence (XRF) analysis using a Siemens-type apparatus (SRS 3000, Munich, Germany). The crystalline structure of the samples was identified by X-Ray diffraction (XRD) analysis using PANalyticalX’Pert PRO diffractometer (Malvern, UK) with Cu/Kα radiation (λ = 0.1540 nm) and scanning over the 2θ range from 10 to 90°. The infrared spectra were recorded on a Thermo Scientific Nicolet iS10 Fourier transform spectrometer in the spectral range between 4000 and 400 cm−1. BET analysis was performed using nitrogen gas adsorption/desorption isotherms obtained at 77 K with a Micromeritics Accusorb 2100E (Norcross, GA, USA) model surface area analyzer. The porosity of the kaolin was also examined. A UV-vis spectrometer (OPTIZEN 3220UV, Warsawa, Poland) was used to measure the concentration of MG in the sample at 617 nm.

2.2.2. Catalytic Activity Test

The catalytic activity of the Ni/kaolin catalyst was tested in the catalytic oxidation of malachite green dye using H2O2 (30%) as an oxidant reagent at the flow rate. All the samples were prepared and distributed in 250 mL glass breakers, into which 200 mL of the solution of MG with C = 20 mg/L and 0.2 g of the catalyst for different amounts (2 wt.%, 5 wt.%, and 7 wt.%) were added. The reaction was kept going for 3 h with constant stirring at 320 rpm. Samples were collected every 15 min and analyzed by UV-Vis spectroscopy.
The percentage removal of dye was calculated using the following equation:
D y e   r e m o v a l   ( % ) = C 0 − C t   C 0 × 100
where C0 and Ct are the concentrations of dye in solution (mg/L) at reaction times 0 and t, respectively. The experimental data are fit using a pseudo-first-order kinetics model defined by the Matthews–Weber equation, where k (min−1) is the reaction rate constant.
ln C t C 0 = − k t
The effect of catalyst dose, oxidant volume, and the temperature was investigated.

3. Results and Discussion

3.1. Support and Catalyst Characterization

3.1.1. The Chemical Composition of Support (Natural Kaolin)

The chemical analysis of the kaolin is shown in Table 1; the kaolin is relatively rich in silica (43.82%) and alumina (36.66%), and it also contains a low quantity of oxides. The loss on ignition of pure kaolin can be estimated theoretically from the molecular mass of kaolinite. The loss of a mass of pure kaolin is evaluated at 16.36%.

3.1.2. Specific Surface Area (SBET) and Pore Size

The pore size, specific surface area (SBET), and micropore volume are considered key parameters in evaluating the adsorption capacity of materials. The SBET of the kaolin was studied using the nitrogen gas adsorption and desorption isotherms, as shown in Figure 2.
The obtained results show that the BET curve fits the type IV isotherm according to the classification of the IPUAC, with an H3 hysteresis loop ranging between 0.50 and 0.90 relative pressure (P/P0), indicating that this support has a typical mesoporous structure enhanced by the presence of meso and macroporous morphologies on its surface. The specific surface area of Tamazert kaolin was found to be 31.2 m2 g−1, and the pore size distribution was reported to be in the range of 5–15 nm, as shown in Figure 2.

3.1.3. FT-IR Spectroscopic Analysis

FT-IR spectra for 2%, 5%, and 7% Ni/kaolin are represented in Figure 3.
Two intense absorption bands are located at 3600 and 3690 cm−1, which are generally assigned to hydroxyl groups (OH−). The band at 1620 cm−1 corresponds to the vibration of water molecules. Si–O stretching vibrations appeared at 1119 cm−1, while the asymmetrical Si–O–Si stretching vibrations occurred around 1032 cm−1. Absorption bands at 475 cm−1 can be attributed to the stretching vibration of the Ni–O bond [24].

3.1.4. XRD Analysis

Structural modifications occurring in the treated kaolin were studied using the X-ray diffraction technique. The XRD patterns were recorded in the range of 10–90°. Figure 4 shows the XRD profiles of catalysts (2%, 5%, and 7% Ni/kaolin).
The raw kaolin exhibits narrow peaks, indicating the existence of crystalline quartz phases (2θ = 12, 20, 22, 25, and 56°). In the supported catalysts, the presence of peaks at 2θ = 37.3, 43.3, 62.8, and 75.3° could indicate the presence of NiO at the surface of the kaolin according to JCPDS 47-1049 [36]. As shown in Figure 4, the main peaks have low intensity due to low Ni loading. Jiang et al. [37] obtained similar results. The good crystallinity of the catalyst is confirmed by the narrowness of the peaks.

4. Effect of the Experimental Parameters

The examination of the catalytic characteristics of the prepared catalysts in the presence of hydrogen peroxide was performed using different parameters such as the catalyst dose, the amount of H2O2, the metal loading of the catalyst and the temperature.

4.1. Effect of Metal Loading

To elucidate the effect of metal loading on the catalytic performance of the prepared catalysts, different amounts of Ni/kaolin (2 wt.%, 5 wt.%, and 7 wt.%) were loaded at varied time intervals in order for the dye to reach its removal percentage by keeping a constant weight of the catalyst (0.2 g), while progressively increasing the contact time. Every 15 min, a small sample of the reaction mixture was centrifuged for 10 min before the absorbance was measured with a UV-Vis spectrophotometer. The influence of the percentage of nickel loading on dye removal is shown in Figure 5.
The results revealed that nickel loading has an impact on the degradation of MG. Indeed, when the amount of nickel in the solution was increased from 2 to 7 wt.%, the decolorization of malachite green gradually increased until it reached its maximum value, leading to an increase in the generation of (OH•) radicals in the system. A rate of 77.78% was achieved for 7 wt.% of Ni/kaolin loading within 180 min; therefore, this optimal percentage (7 wt.% of Ni/kaolin) was used as a reference in the subsequent investigations.

4.2. Effect of the Catalyst Mass

The amount of MG degraded at room temperature under the influence of the catalyst mass is shown in Figure 6. The mass of the catalyst (7% Ni/kaolin) varied from 0.2 to 0.8 g, and the initial concentration of the pollutant was set at 20 mg/L.
The results from Figure 6 show that the degradation of MG is proportional to the dose of the catalyst. An increase in catalyst dose leads to an improvement in the number of active sites responsible for the catalytic activity, therefore increasing the percentage degradation of the dye. The optimum dye degradation rate (82.20%) was achieved at a catalyst mass of 0.8 g.

4.3. Effect of Oxidant Amount

The effect of H2O2 dosage on MG degradation was assessed by adding several H2O2 volumes (3 mL, 6 mL, and 10 mL) under the following conditions: the amount of catalyst was set at 0.8 g and the dye concentration at 20 mg/L; the pH of the solutions was set at 7 and the temperature at 25 °C. The results are presented in Figure 7.
It was found that the degradation rate of the dye was significantly increased with the increase in the amount of hydrogen peroxide. The optimum degradation rate (82.20%) was obtained for an oxidant amount of 10 mL after 180 min. The excess of H2O2 and the presence of a catalyst promote the formation of large numbers of (OH•) radicals, which are responsible for the degradation of the dye due to their potential to convert the molecules of MG into intermediate products.

4.4. Effect of Temperature

The influence of the temperature was studied in the temperature range of 25–50 °C and under the following operating conditions: a mass of catalyst of 0.8 g; a dye concentration of 20 mg/L; and 10 mL of H2O2. To keep the temperature at the target value, a stirring plate and a thermometer were used.
Figure 8 shows the percentage increase in the degradation of MG with the evolution of the temperature. We notice that the optimal degradation rate (98.87%) was obtained at 50 °C after 180 min. On the other hand, as the temperature increases, exothermic adsorption of the reactants becomes less desirable due to a decrease in the apparent activation energy. Additionally, the increase in temperature leads to an increase in the rate of reaction between H2O2 and the catalyst, and thus increases the rate of generation of oxidizing species, such as hydroxyl free radicals that are efficient to degrade the dye [38]. The same conclusions regarding the temperature effect were drawn in previous studies [39,40,41,42,43].

5. Kinetic Study of MG Removal during the Oxidation Process

The kinetic investigation of the degradation of MG is essential to evaluate the catalytic performance of the catalyst Ni/kaolin in the presence of H2O2. The straightline plot of Figure 9 showed that the degradation of the MG undergoes a first-order pseudo-reaction. The rate constant value (k) was determined from the slope of the plot.
The coefficient of determination R2 and apparent rate constants kapp at different temperatures are presented in Table 2. It should be noted that the observed deviation of the last two data points from the linear trend for the plot of ln(C/C0) vs. T (35 °C) can be attributed to the interaction of the intermediate products of the degradation with the remaining MG dye.
Based on the Arrhenius formula, the activation energy of the degradation of MG by the catalyst Ni/kaolin in the presence of hydrogen peroxide was calculated according to Equation (3):
ln k a p p = ln k 0 − E a R T
where k0 is the pre-exponential factor, and Ea denotes the apparent activation energy kJ/mol.
The value of the activation energy was calculated from the regression slope (line of lnkapp as a function of 1/T), as illustrated in Figure 10.
The apparent activation energy of the catalytic oxidation of the dye is 27.51 kJ/mol. Furthermore, the typical activation energy Ea ranges between 60 and 250 kJ/mol [44,45]. The reported value is quite similar to that of organic pollutants degraded by hydroxyl radicals (≈30 kJ/mol) [46]. The low value of the activation energy suggests that the degradation of MG is limited by a diffusion step, and the apparent constant rate reflects the rate at which the MG molecules migrate from the solution to the catalyst surface where the reaction takes place. A similar result was obtained by Behnajady et al. [47]. On the other hand, any increase in temperature can provide more energy for the reactive molecules to dominate the activation energy of the reaction [38]. This result indicates that Ni/kaolin catalyst faces a low energy barrier and can be activated easily in the presence of H2O2 [48].

6. Comparative Investigation of MG Removal on Different Catalysts

Due to the different experimental conditions used in prior investigations, a direct comparison of the adsorption capabilities investigated in this work with those previously published in the literature is challenging. However, an examination of Table 3 shows that Ni/kaolin catalyst used in this study exhibits a better MG removal rate than other catalysts [49,50,51,52], as listed in Table 3.

7. Degradation Mechanism of MG Dye

The mechanism for the decomposition of H2O2 molecules and the production of reactive species in the NiO/kaolin/H2O2 system is proposed in this article. The OH• radicals are produced by heterogenous reactions that occur in the solid phase between the adsorption of H2O2 molecules and the actives sites of the catalyst, according to Equation (4), leading to the generation of OH• (ads). It has to be noted that the adsorption of the dye (Equation (5)) and H2O2 molecules on the catalyst surface facilitates the reaction between the oxidant and the active sites to produce free radicals in the solid phase [22]. Finally, the OH• (ads) radicals directly attack the dye molecule (MG) to obtain degraded products (Equation (6)).
Catalyst + H2O2 → catalyst (OH•)ads (adsorption of H2O2 on the surface of catalyst)
Dye + catalyst → catalyst (dye)ads (adsorption of the dye on the surface of catalyst
OH• + organic toxic dye (MG) → degraded products

8. Conclusions

In this study, the catalytic activity of the supported catalyst, which was prepared by the impregnation technique (kaolin impregnated by nickel) on the degradation of the malachite green dye in the presence of hydrogen peroxide H2O2, was investigated. The experimental tests carried out allowed us to determine the optimal reaction conditions for the degradation of MG, which are the percentage of nickel 7%, the reaction temperature of 50 °C, the mass of catalyst 0.8 g, the volume of H2O2 10 mL, and the pH = 7. Under these conditions, the removal rate of malachite green dye reached a maximum of 98.87% after 3 h. The increase in Ni content in the catalyst increases and improves the degradation efficiency of the malachite green. The kinetic study showed that the degradation reaction of the malachite green follows the pseudo-first-order. The results of this study evidenced the feasibility and the effectiveness of supported catalysts prepared by the wet impregnation method as potential and cost-effective adsorbents for the removal of pollutant dyes.

Author Contributions

Conceptualization, A.M.; methodology, A.M., Y.B. and S.R.; software, F.H. and F.M.; validation, Y.B., M.S. and F.A.M.A.; formal analysis, N.S., F.M. and F.H.; investigation, A.M., S.R. and Y.B.; resources, F.A.M.A., F.H. and F.M.; data curation, F.H.; writing—original draft preparation, A.M. and Y.B.; writing—review and editing, S.R., N.S. and M.S.; supervision, Y.B. and M.S.; project administration, A.M., S.R. and Y.B. All authors have read and agreed to the published version of the manuscript.

Funding

This research received no external funding.

Institutional Review Board Statement

Not applicable.

Informed Consent Statement

Not applicable.

Data Availability Statement

The data presented in this study are available on reasonable request from the corresponding author.

Conflicts of Interest

The authors declare no conflict of interest.

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Molecules 27 07528 g001 550
Figure 1. Chemical structure of MG dye.
Figure 1. Chemical structure of MG dye.
Molecules 27 07528 g001
Molecules 27 07528 g002 550
Figure 2. Size distribution analysis, BET adsorption, and desorption isotherms of Tamazert kaolin.
Figure 2. Size distribution analysis, BET adsorption, and desorption isotherms of Tamazert kaolin.
Molecules 27 07528 g002
Molecules 27 07528 g003 550
Figure 3. FT-IR spectra of supported catalysts (2%, 5%, and 7% Ni/kaolin).
Figure 3. FT-IR spectra of supported catalysts (2%, 5%, and 7% Ni/kaolin).
Molecules 27 07528 g003
Molecules 27 07528 g004 550
Figure 4. X-ray diffractograms of supported catalysts (2%, 5%, and 7% of Ni/kaolin).
Figure 4. X-ray diffractograms of supported catalysts (2%, 5%, and 7% of Ni/kaolin).
Molecules 27 07528 g004
Molecules 27 07528 g005 550
Figure 5. Effect of nickel loading on MG removal in terms of time. (Reaction conditions: C0 = 20 mg/L, m = 0.2 g, VH2O2 = 10 mL, pH = 7 and T = 25 °C).
Figure 5. Effect of nickel loading on MG removal in terms of time. (Reaction conditions: C0 = 20 mg/L, m = 0.2 g, VH2O2 = 10 mL, pH = 7 and T = 25 °C).
Molecules 27 07528 g005
Molecules 27 07528 g006 550
Figure 6. Effect of catalyst loading on MG removal. Reaction conditions: C0 = 20 mg/L, VH2O2 = 10 mL, pH = 7 and T = 25 °C.
Figure 6. Effect of catalyst loading on MG removal. Reaction conditions: C0 = 20 mg/L, VH2O2 = 10 mL, pH = 7 and T = 25 °C.
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Molecules 27 07528 g007 550
Figure 7. Effect of oxidant volume on MG removal. Reaction conditions: C0 = 20 mg/L, m = 0.8 g, pH = 7 and T = 25 °C.
Figure 7. Effect of oxidant volume on MG removal. Reaction conditions: C0 = 20 mg/L, m = 0.8 g, pH = 7 and T = 25 °C.
Molecules 27 07528 g007
Molecules 27 07528 g008 550
Figure 8. Effect of temperature on MG removal. Reaction conditions: C0 = 20 mg/L, VH2O2 = 10 mL, pH = 7 and m = 0.8 g.
Figure 8. Effect of temperature on MG removal. Reaction conditions: C0 = 20 mg/L, VH2O2 = 10 mL, pH = 7 and m = 0.8 g.
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Molecules 27 07528 g009 550
Figure 9. ln(C/C0) as a function of time t (min) (Reaction conditions: C0 = 20 mg/L, catalyst mass = 0.8 g, and pH = 7).
Figure 9. ln(C/C0) as a function of time t (min) (Reaction conditions: C0 = 20 mg/L, catalyst mass = 0.8 g, and pH = 7).
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Molecules 27 07528 g010 550
Figure 10. The plot of lnkapp versus 1/T at different temperatures.
Figure 10. The plot of lnkapp versus 1/T at different temperatures.
Molecules 27 07528 g010
Table
Table 1. The chemical composition (wt.%) of natural kaolin (derived from XRF analysis).
Table 1. The chemical composition (wt.%) of natural kaolin (derived from XRF analysis).
OxidesSiO2Fe2O3Al2O3CaCO3CaOMgOMnOPAF
(wt.%)43.820.5536.661.351.050.050.116.36
Table
Table 2. The coefficient of determination R2 and apparent rate constants kapp.
Table 2. The coefficient of determination R2 and apparent rate constants kapp.
TemperaturekappR2σ (Standard Deviation)
T = 298 K0.00780.9650.495
T = 308 K0.01020.9360.683
T = 323 K0.01820.9621.297
Table
Table 3. Comparison of the percentage degradation of MG dye by supported catalysts reported in the literature.
Table 3. Comparison of the percentage degradation of MG dye by supported catalysts reported in the literature.
CatalystDegradation %References
Ag/ZnCo-ZIF98%[49]
NiO/Al2O382%[50]
Chitosan/ZnO54%[51]
Chitosan/Ce-ZnO87%[51]
Mn-ZnO/CNT95%[52]
Ni/kaolin98.87%This work
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Moumen, A.; Belhocine, Y.; Sbei, N.; Rahali, S.; Ali, F.A.M.; Mechati, F.; Hamdaoui, F.; Seydou, M. Removal of Malachite Green Dye from Aqueous Solution by Catalytic Wet Oxidation Technique Using Ni/Kaolin as Catalyst. Molecules 2022, 27, 7528. https://doi.org/10.3390/molecules27217528

AMA Style

Moumen A, Belhocine Y, Sbei N, Rahali S, Ali FAM, Mechati F, Hamdaoui F, Seydou M. Removal of Malachite Green Dye from Aqueous Solution by Catalytic Wet Oxidation Technique Using Ni/Kaolin as Catalyst. Molecules. 2022; 27(21):7528. https://doi.org/10.3390/molecules27217528

Chicago/Turabian Style

Moumen, Abdelhak, Youghourta Belhocine, Najoua Sbei, Seyfeddine Rahali, Fatima Adam Mohamed Ali, Fedia Mechati, Fouad Hamdaoui, and Mahamadou Seydou. 2022. "Removal of Malachite Green Dye from Aqueous Solution by Catalytic Wet Oxidation Technique Using Ni/Kaolin as Catalyst" Molecules 27, no. 21: 7528. https://doi.org/10.3390/molecules27217528

APA Style

Moumen, A., Belhocine, Y., Sbei, N., Rahali, S., Ali, F. A. M., Mechati, F., Hamdaoui, F., & Seydou, M. (2022). Removal of Malachite Green Dye from Aqueous Solution by Catalytic Wet Oxidation Technique Using Ni/Kaolin as Catalyst. Molecules, 27(21), 7528. https://doi.org/10.3390/molecules27217528

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