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Original article
2021
:14;
202106
doi:
10.1016/j.arabjc.2021.103197

Efficient removal of Ni(II) ions from aqueous solutions using analcime modified with dimethylglyoxime composite

, , , , , , , , , , , , ,
a Department of Chemistry, Faculty of Applied Science, Umm Al-Qura University, Makkah 21955, Saudi Arabia
b Drug Exploration & Development Chair (DEDC), Department of Pharmaceutical Chemistry, College of Pharmacy, King Saud University, Riyadh 11451, Saudi Arabia
c Peptide Chemistry Department, Chemical Industries Research Division, National Research Centre, 12622-Dokki, Cairo, Egypt
d Department of Chemistry, Faculty of Science, King Saud University, Riyadh 11451, Saudi Arabia
e Department of Chemistry, University College in Al-Qunfudhah, Umm Al-Qura University, Saudi Arabia
f Department of Chemistry, College of Science, Princess Nourah Bint Abdulrahman University, Riyadh 11671, Saudi Arabia
g Department of Chemistry, College of Sciences and Arts-Alkamil, University of Jeddah, Jeddah 23218, Saudi Arabia
h Department of Chemistry, Faculty of Science, Al-Azhar University, Cairo 11651, Egypt
i Department of Chemistry, Rabigh College of Science and Arts, King Abdulaziz University, Rabigh 21911, Saudi Arabia
j Department of Chemistry, College of Science and Humanities in Al-Kharj, Prince Sattam bin Abdulaziz University, Al-Kharj 11942, Saudi Arabia
k Department of Chemistry, Faculty of Science, Mansoura University, Mansoura 35516, Egypt

⁎Corresponding author at: Drug Exploration & Development Chair (DEDC), Department of Pharmaceutical Chemistry, College of Pharmacy, King Saud University, Riyadh 11451, Saudi Arabia. anaglah@ksu.edu.sa (Ahmed M. Naglah)

Received: , Accepted: ,
© The Author(s) 2021
Disclaimer:
This article was originally published by Elsevier and was migrated to Scientific Scholar after the change of Publisher.

Abstract

In this work, the analcime/dimethylglyoxime composite was facilely fabricated as a novel adsorbent for the removal of Ni(II) ions from aqueous solutions. The fabricated adsorbent was characterized utilizing FT-IR, XRD, FE-SEM, and CHN analyses. Wide XRD peak and cotton-like structure FE-SEM image of the adsorbent confirmed that the crystal assembly of analcime combined or interfered over amorphous surroundings. The best analytical conditions for the uptake of Ni(II) ions are accomplished at time = 120 min, pH = 6.5, and temperature = 298 Kelvin. Removal of Ni(II) ions was well modeled by pseudo-second-order as a kinetic model and Langmuir as an equilibrium isotherm. The negative sign of ΔGo and ΔHo indicates a spontaneous and exothermic process. The value of ΔHo, which is more than 40 kJ/mole, indicates the chemical nature of the adsorption process. The maximum uptake capacity of the synthesized composite is 144.9 mg/g. 0.5 M EDTA disodium salt can recover the adsorbed Ni(II) ions for three adsorption/desorption cycles. Diverse ions such as Cd(II), Cu(II), Pb(II), and Zn(II) did not interfere during the extraction of Ni(II) ions.

Keywords

Adsorption
Analcime/dimethylglyoxime composite
Nanoparticles
Ni(II) ions
Selectivity
1

1 Introduction

Industrial wastewaters include several poisonous heavy metal ions such as Hg(II), Pb(II), Cr(III), Ni(II), Cu(II), Cd(II), and Zn(II). Serious water and soil pollution have been identified owing to discharging of these metals into the environment (Duan et al., 2020; Ajiboye et al., 2021; Senguttuvan et al., 2021). Small quantities of heavy metals are essential for our health whereas large quantities of them are generally toxic (Qiu and Zheng, 2009; Nosuhi and Nezamzadeh-Ejhieh, 2017; Pourshirband and Nezamzadeh-Ejhieh, 2020; Tamiji and Nezamzadeh-Ejhieh, 2018). These metals, in contrast to organic pollutants, are not degradable in the environment, resistant, unalterable, and causing severe pollution of groundwaters or agricultural products. They cause various health problems because of the accumulation of them in organisms (Shi et al., 2009). For example, nickel influences are fluctuating from the damage of the lungs or nervous system to skin irritation. Exposure to a high content of nickel for a long time decreases body weight and causes respiratory problems. Also, nickel can cause nervous system damage, reduction of cell growth, and lung cancer (Argun, 2008; Sobhanardakani, 2019). Consequently, the uptake of extra Ni(II) ions from wastewater is required to protect environmental and human health. According to the World Health Organization (WHO) recommendation, the maximum permissible limit of Ni(II) ions in drinking water is 0.10 mg/L (Hezarjaribi et al., 2020). Several techniques have been described for the uptake of Ni(II) ions from wastewater and water samples such as chemical precipitation, reverse osmosis, ultrafiltration membranes, complexation/ultrafiltration, membrane separation, microbial electrolysis, adsorption, electrocoagulation, electrodialysis/electrodeionization, ion exchange, and electroflocculation/filtration hybridization (Hezarjaribi et al., 2020; Meunier et al., 2006; Kandah and Meunier, 2007; Ren et al., 2011; Katsou et al., 2010; Vieira et al., 2010; Qin et al., 2012; Dermentzis, 2010; Graillot et al., 2013; De Mello Ferreira et al., 2013; Betancur et al., 2009; Sobhanardakani and Zandipak, 2017; Ipek, 2005; Chen et al., 2021; Sharma et al., 1990). A few of these techniques have drawbacks such as the requirement for special equipment, high cost, and low uptake capacity. The chemical precipitation procedure is operating for a high concentration of Ni(II) ions with low volume. Several electrochemical techniques such as electrochemical precipitation and electrocoagulation consume great electrical energy. Also, discharging of the coagulated products in the environment regards an environmental problem. Among these procedures, adsorption is considered to be cost-effective and simple if low-cost adsorbents are used such as modified zeolites, modified silica, and modified geopolymers (Khalifa et al., 2020; Abdelrahman and Hegazey, 2019; Abdelrahman and Subaihi, 2020; Tamiji and Nezamzadeh-Ejhieh, 2019; Derikvandi and Nezamzadeh-Ejhieh, 2017; Heidari-Chaleshtori and Nezamzadeh-Ejhieh, 2015). Soheil et al. synthesized Fe3O4/SiO2 core–shell nanoparticles modified with TiO2, utilizing a simple procedure for removal of Cd(II), Ni(II), and Hg(II) ions from aqueous solution. The maximum capacity was 670.90, 563.00, and 745.60 mg/g within 50 min, respectively (Sobhanardakani and Zandipak, 2017). Dhiwar et al. synthesized iron oxide/chitosan composite for the uptake of Ni(II) ions from aqueous media. The maximum capacity of the composite was 1.140 mg/g at pH 4.0 within 30 min (Dhiwar et al., 2013). Abdelrahman et al. synthesized graft copolymers of chitosan or maltodextrin with 2-acrylamido-2-methyl-1-propanesulfonic acid and abbreviated as M1 or M2, respectively. Furthermore, they synthesized homopolymer of 2-acrylamido-2-methyl-1-propanesulfonic acid and abbreviated as M3. The maximum capacity of M1, M2, and M3 was 32.74, 26.66, and 27.33 mg/g, respectively (Abdelrahman et al., 2019). Le et al. synthesized magnetic hydroxyapatite/chitosan composite for the uptake of Ni(II) ions from aqueous media. The maximum capacity was 112.36 mg/g at pH 6 within 60 min (Le et al., 2018). Zhao et al. synthesized Tannin-Based Dithiocarbamate composite for the uptake of Ni(II) ions from aqueous media. The maximum capacity of the composite was 112.49 mg/g at pH 6.0 within 45 min (Zhao et al., 2016). The main problem in the removal of a specific heavy metal using unselective adsorbents is the saturation of adsorbents by undesirable ions that lead to reducing adsorbent capacity for the removal of the preferred metal ion. Zeolites are regarded as effective solid supports to host several organic compounds on their surface for the uptake of numerous pollutants because of their distinctive properties such as size, thermal stability, surface area, and negative charge (Khalifa et al., 2020; Abdelrahman and Hegazey, 2019; Abdelrahman and Subaihi, 2020; Tamiji and Nezamzadeh-Ejhieh, 2019; Derikvandi and Nezamzadeh-Ejhieh, 2017; Heidari-Chaleshtori and Nezamzadeh-Ejhieh, 2015; Dhiwar et al., 2013; Abdelrahman et al., 2019; Le et al., 2018; Zhao et al., 2016). Several papers in the literature confirmed the successful modification of silica, clays, and zeolites as solid supports by many organic compounds such as amino acids, pentetic acid, chitosan, EDTA, and dibenzoylmethane for enhancing its selectivity and activity for the uptake of many heavy metals from aqueous solutions (Khalifa et al., 2020; Abdelrahman and Hegazey, 2019; Abdelrahman and Subaihi, 2020; Tamiji and Nezamzadeh-Ejhieh, 2019; Derikvandi and Nezamzadeh-Ejhieh, 2017; Heidari-Chaleshtori and Nezamzadeh-Ejhieh, 2015; Dhiwar et al., 2013; Abdelrahman et al., 2019; Le et al., 2018; Zhao et al., 2016; Shafiof and Nezamzadeh-Ejhieh, 2020; Eshraghi and Nezamzadeh-Ejhieh, 2018). There is a growing request for the fabrication of low-cost and effective adsorbents for the removal of toxic Ni(II) ions from aqueous media. So, in this paper, a novel composite was facilely fabricated by simple procedure via modifying analcime with dimethylglyoxime. The fabricated composite was utilized for the efficient removal of Ni(II) ions from aqueous media. The C⚌N functional group of the dimethylglyoxime, which is fixed on the analcime support, can form a chelate with Ni(II) ions. Also, the effect of several factors on the removal process, for example, pH, time, temperature, and concentration were studied. So, this work reports novel, new, and innovative results in the environmental field.

2

2 Experimental

2.1

2.1 Chemicals

L-alanine (C3H7NO2), hydrochloric acid (HCl), dimethylglyoxime (C4H8N2O2), aluminum chloride hexahydrate (AlCl3·6H2O), ethanol (C2H6O), fumed silica (SiO2), nitric acid (HNO3), sodium hydroxide (NaOH), and nickel(II) chloride hexahydrate (NiCl2·6H2O) were obtained from Sigma Aldrich Company. All the previous chemicals were of analytical grade and used as received without additional purification.

2.2

2.2 Synthesis of analcime/dimethylglyoxime composite

Firstly, the analcime was synthesized as reported by Hameed et al (Hameed et al., 2020). Briefly, 2.88 g of fumed silica (as a silicon source) was dissolved in 90 mL of 2.25 M sodium hydroxide solution. Besides, 2.88 g of aluminum chloride hexahydrate (as an aluminum source) was dissolved in 30 mL of distilled water. 1.00 g of L-alanine (as a template source) was dissolved in 20 mL of 1.25 M sodium hydroxide solution. The previous solutions were mixed then hydrothermally treated using Teflon lined autoclave at 120 °C for one day. For the synthesis of the composite, 3 g of dimethylglyoxime was dissolved in 200 mL of water/ethanol solvent. Besides, 3 g of analcime was added to the previous solution then the mixture was agitated at room temperature for one day. Moreover, the product was separated using a centrifuge with a speed of 2800 rpm, washed several times using hot distilled water, and dried at room temperature.

2.3

2.3 Characterization of the analcime/dimethylglyoxime composite

The X-ray diffraction (XRD) pattern of the analcime/dimethylglyoxime composite was obtained utilizing a Bruker diffractometer (D8 Advance) with Kα Cu radiations have wavelength (λ) equals 0.15 nm. The Fourier transform (FT-IR) spectra of the analcime/dimethylglyoxime composite, on KBr pellets, was recorded at room temperature using a Nicolet single beam spectrometer in the range from 400 to 4000 cm−1. The surface morphology of the analcime/dimethylglyoxime composite was studied using JSM5410 JEOL scanning electron microscopy (SEM) and 2100 JEOL transmission electron microscopy (TEM). Furthermore, CHN analysis of the analcime/dimethylglyoxime composite was estimated utilizing CHN Elemental Analyzer (2400 Perkin Elmer. BET surface area, average pore radius, and total pore volume of the analcime/dimethylglyoxime composite were determined from nitrogen isotherms at −196 °C using Quantachrome (NOVA touch LX4).

2.4

2.4 Uptake of Ni(II) ions from aqueous solutions

Typical batch experiments for the uptake of Ni(II) ions from aqueous media by the analcime/dimethylglyoxime composite were accomplished as the following: 0.1 g of the analcime/dimethylglyoxime adsorbent was added to 50 mL of 350 mg/L of Ni(II) aqueous solution which was adjusted at the wanted pH value using 0.1 M NaOH and HCl. Then, the mixture was agitated using a magnetic stirrer at 450 rpm for several times (15–180 min) and temperatures (298–328 Kelvin). Also, the effect of concentration was studied as previously described but in the range 250–450 mg/L. Besides, the suspensions were centrifuged then the concentration of Ni(II) ions which exists in the filtrate was determined using inductively coupled plasma optical emission spectrometry (ICP-OES).

The mass of the adsorbed Ni(II) ions per gram of the analcime/dimethylglyoxime composite (A, mg/g) was determined using Eq. (1).

(1)
A = B o - B e C D

The % removal (% E) of Ni(II) ions using the analcime/dimethylglyoxime composite was calculated using Eq. (2).

(2)
% E = B o - B e 100 B o where Bo (mg/L) is the initial concentration of Ni(II) ions whereas Be (mg/L) is the equilibrium concentration of Ni(II) ions. Besides, C (L) is the volume of Ni(II) aqueous solution whereas D (g) is the utilized amount of the analcime/dimethylglyoxime composite.

Influence of desorption and reusability was studied as follows; 0.1 g of analcime/dimethylglyoxime adsorbent was stirred with 50 mL of 350 mg/L Ni(II) solution at pH 6.5 for 120 min at 298 Kelvin. Then, the solid phase was filtered and washed several times with distilled water to eliminate the non-adsorbed Ni(II) ions. The loaded composite was then stirred for 30 min with 50 mL of 0.5 M of some desorbing agents (HNO3, HCl, EDTA disodium salt, and thiourea) for three cycles of adsorption/desorption.

The selective extraction of Ni(II) ions by the current method was studied in a 50 mL binary aqueous media containing the Ni(II) ions (5 mg/L) in addition to a potentially interfering ion such as K(I), Na(I), Ca(II), Ba(II), Mg(II), Cu(II), Cd(II), Pb(II), Hg(II), Zn(II), Al(III), Fe(III), Fe(II), Cl−, NO3−, HCO3−, and SO42−. The pH of the Ni(II) solution was adjusted to 6.5. Then, the solution mixed with 0.1 g of the analcime/dimethylglyoxime composite and stirred at 298 Kelvin for 120 min.

The point of zero charge (pHPZC) of the analcime⁄dimethylglyoxime composite was determined as follows: 0.15 g of the fabricated composite was added to 60 mL of 0.01 M potassium chloride solutions. The initial pH value (pHinitial) of potassium chloride solution was studied in the range 2–12. After that, the mixtures were agitated using a magnetic stirrer at 450 rpm for 6 h. Besides, the suspensions were centrifuged then the final pH values (pHfinal) of the filtrates were measured. Additionally, pHfinal values were plotted versus pHinitial values. The pHpzc is the pHfinal level where a typical plateau was obtained (Khalifa et al., 2020).

3

3 Results and discussion

3.1

3.1 Characterization of the analcime/dimethylglyoxime composite

The space group, chemical formula, and crystal structure of analcime are Ia-3d, Na (AlSi2O6) (H2O), and Cubic, respectively as clearly clarified using JCPDS No. 70–1575 (Hameed et al., 2020). The percentages of silicon, aluminum, sodium, and oxygen of analcime were 30.85, 15.26, 8.26, and 45.63%, respectively. So, the Si/Al of analcime is 2.02.

Fig. 1 shows the XRD pattern of the analcime/dimethylglyoxime composite. The typical XRD peaks of the analcime appeared at 2θ equals about 69°, 66°, 58°, 54°, 53°, 52°, 49°, 48°, 40°, 37°, 36°, 33°, 32°, 31°, 26°, 24°, 18°, and 16° (Hameed et al., 2020). In the analcime/dimethylglyoxime composite, these peaks disappeared and a wide peak appeared at 2θ equals 24°. Consequently, this confirmed that the crystal assembly of analcime combined or interfered over amorphous surroundings (Khalifa et al., 2020; Kenawy et al., 2018).

The XRD pattern of the analcime/dimethylglyoxime composite.
Fig. 1
The XRD pattern of the analcime/dimethylglyoxime composite.

Fig. 2 shows the FT-IR spectra of the analcime/dimethylglyoxime composite. The peaks, which were detected at 476 and 606 cm−1, are owing to bending and symmetrical vibration of F-O-F (F = Al and/or Si), respectively (De Mello Ferreira et al., 2013; Khalifa et al., 2020; Kenawy et al., 2018). The peaks, which were detected at 708 and 905 cm−1, are owing to bending vibration of CNO and skeleton deformation of dimethylglyoxime molecule, respectively (Panja et al., 1991; Szabó and Kovács, 2003). The peak, which was detected at 1070 cm−1, is attributed to the asymmetric vibration of F-O-F (F = Al and/or Si) (De Mello Ferreira et al., 2013; Khalifa et al., 2020; Kenawy et al., 2018). The peaks, which were detected at 1365 and 1445 cm−1, are owing to symmetrical and asymmetrical vibration of CH3, respectively. The peaks, which were detected at 1639 and 3444 cm−1, are owing to bending and stretching vibration of OH, respectively (Panja et al., 1991; Szabó and Kovács, 2003; Haghshenas and Nezamzadeh-Ejhieh, 2017).

The FT-IR spectra of the analcime/dimethylglyoxime composite before (A) and after (A) the nickel adsorption.
Fig. 2
The FT-IR spectra of the analcime/dimethylglyoxime composite before (A) and after (A) the nickel adsorption.

Elemental analysis of the analcime/dimethylglyoxime composite clarified that the % carbon, % hydrogen, and % nitrogen are 14.23, 3.50, and 1.14%, respectively.

Fig. 3A-B shows the FE-SEM and HR-TEM images of the analcime/dimethylglyoxime composite. The FE-SEM image clarified that the analcime/dimethylglyoxime composite has a cotton-like structure.

The FE-SEM (A) and HR-TEM (B) images of the analcime/dimethylglyoxime composite.
Fig. 3
The FE-SEM (A) and HR-TEM (B) images of the analcime/dimethylglyoxime composite.

Also, the HR-TEM image clarified that the analcime/dimethylglyoxime composite has irregular shapes. Hence, the aforementioned analyses confirmed that the crystal assembly of analcime combined or interfered over amorphous surroundings (Khalifa et al., 2020; Kenawy et al., 2018).

BET surface area (m2/g), average pore radius (Ao), and total pore volume (cc/g) of the analcime equal 12.76, 22.32, and 1.50E-2, respectively. BET surface area (m2/g), average pore radius (Ao), and total pore volume (cc/g) of the analcime/dimethylglyoxime composite equal 1.87, 40.30, and 3.54E-3, respectively. The BET surface area and total pore volume of the analcime/dimethylglyoxime composite were decreased because the dimethylglyoxime molecules blocking the pores of analcime. These analyses confirmed the success of the modification process of analcime with the dimethylglyoxime as clarified in Scheme 1.

The Proposed structure of the analcime/dimethylglyoxime composite.
Scheme 1
The Proposed structure of the analcime/dimethylglyoxime composite.

3.2

3.2 Analytical parameters affecting the uptake of Ni(II) ions from aqueous solutions

3.2.1

3.2.1 Influence of pH

Fig. 4A displays the plot of the percentage of removal of Ni(II) ions (% E) versus pH of Ni(II) solution. Besides, Fig. 4B displays the plot of the adsorption capacity of the analcime/dimethylglyoxime composite (A) toward Ni(II) ions versus pH of Ni(II) solution. The % E is 11.4, 25.7, 54.3, 65.7, 71.4, 72.9, and 73.4% at pH values equal 2.5, 3.5, 4.5, 5.5, 6.5, 7.5, and 8.5, respectively. Besides, A is 20, 45, 95, 115, 125, 127.5, and 128.5 mg/g at pH values equal 2.5, 3.5, 4.5, 5.5, 6.5, 7.5, and 8.5, respectively. The results confirmed that there is a slight unnoticeable change in the value of both A and % E in the pH range from 6.5 to 8.5. So, the optimum pH value, which will be taken in further impacts, is 6.5. The point of zero charge of the fabricated composite was 5.8 as clarified in Fig. 4C. If the pH of the Ni(II) solution is less than 5.8, the surface of the fabricated composite is surrounded by positive hydrogen ions (H+). Consequently, % E decreases due to competition between positive hydrogen ions and Ni(II) ions to reach the composite. On the contrary, if the pH of the Ni(II) solution is higher than 5.8, the surface of the fabricated composite is surrounded by negative hydroxide ions (OH−) that facilitate the approach of the Ni(II) ions to the composite and hence % E increases (Khalifa et al., 2020; Anari-Anaraki and Nezamzadeh-Ejhieh, 2015; Shirzadi and Nezamzadeh-Ejhieh, 2017; Fakari and Nezamzadeh-Ejhieh, 2017; Naghash and Nezamzadeh-Ejhieh, 2015; Borandegi and Nezamzadeh-Ejhieh, 2015; Nasiri-Ardali and Nezamzadeh-Ejhieh, 2020; Mehrali-Afjani and Nezamzadeh-Ejhieh, 2020; Nezamzadeh-Ejhieh and Afshari, 2012; Shafiof and Nezamzadeh-Ejhieh, 2020; Nezamzadeh-Ejhieh and Kabiri-Samani, 2013; Şimşek et al., 2017; Şenol et al., 2019; Şenol et al., 2019).

The plot of pH of the Ni(II) solution versus % E (A) and A (B). The point of zero charge (C). Experimental conditions: [Concentration of nickel solution = 350 mg/L, volume of nickel solution = 50 mL, temperature = 298 Kelvin, amount of composite = 0.1 g, and time = 200 min].
Fig. 4
The plot of pH of the Ni(II) solution versus % E (A) and A (B). The point of zero charge (C). Experimental conditions: [Concentration of nickel solution = 350 mg/L, volume of nickel solution = 50 mL, temperature = 298 Kelvin, amount of composite = 0.1 g, and time = 200 min].

3.2.2

3.2.2 Influence of time

Fig. 5A displays the plot of the percentage of removal of Ni(II) ions (% E) versus time. Also, Fig. 5B displays the plot of the adsorption capacity of the analcime/dimethylglyoxime composite (A) toward Ni(II) ions versus time. The % E is 14.6, 23.1, 34.3, 42.9, 70, 69.7, and 70.3% at time values equal 15, 30, 60, 90, 120, 150, and 180 min, respectively. Also, A is 25.5, 40.5, 60, 75, 122.5, 122, and 123 mg/g at time values equal 15, 30, 60, 90, 120, 150, and 180 min, respectively. The results confirmed that there is a slight unnoticeable change in the value of both A and % E in the time range from 120 to 180 min. So, the optimum time value, which will be taken in further impacts, is 120 min.

The plot of time versus % E (A) and A (B). Experimental conditions: [Concentration of nickel solution = 350 mg/L, volume of nickel solution = 50 mL, temperature = 298 Kelvin, pH = 6.5, and amount of composite = 0.1 g].
Fig. 5
The plot of time versus % E (A) and A (B). Experimental conditions: [Concentration of nickel solution = 350 mg/L, volume of nickel solution = 50 mL, temperature = 298 Kelvin, pH = 6.5, and amount of composite = 0.1 g].

The experimental results of time were analyzed using the pseudo-first-order which is described using Eq. (3). Also, the experimental results of time were analyzed using the pseudo-second-order which is described using Eq. (4) (Abdelrahman, 2018; Abdelrahman and Hegazey, 2019; Abdelrahman et al., 2020; Abdelrahman et al., 2019; Subaihi et al., 2020; Abdelrahman et al., 2020; Youssef et al., 2020; Abdelrahman et al., 2021; Abdelbaset et al., 2020; Mahmoud et al., 2021; Abdelrahman et al., 2021). Besides, the experimental results of time were analyzed using the intra-particle diffusion which is described using Eq. (5) (Khalifa et al., 2020).

(3)
log A e - A t = l o g A e - L 1 t 2.303
(4)
t A t = 1 L 2 A e 2 + 1 A e t
(5)
A t = L 3 t 0.5 + F where Ae (mg/g) is the uptake capacity of the analcime/dimethylglyoxime composite toward Ni(II) ions at the equilibrium. At (mg/g) is the uptake capacity of the analcime/dimethylglyoxime composite at the time t. L3 (mg/g min0.5), L2 (g/mg.min) and L1 (1/min) are the rate constants of the intra-particle diffusion, pseudo-second-order and pseudo-first-order models, respectively. F (mg/g) is the thickness of the boundary layer. Fig. 6A-B displays the plot of log (Ae-At) and t/At versus time, respectively. The results showed that the rate constant (L2) and correlation coefficient (R2) of the pseudo-second-order model are larger than those of the pseudo-first-order model as clarified in Table 1. Also, Ae, which was obtained from the pseudo-second-order model, is very close to the experimental adsorption capacity more than that of the pseudo-first-order model. Hence, the pseudo-second-order model described the results better than the pseudo-first-order model. A straight line with a high correlation coefficient was produced when plotting At versus t0.5 as clarified in Fig. 6C. The straight-line does not go through the origin and hence this confirms that the intra-particle diffusion model is not the only pathway that controls the uptake of Ni(II) ions (Khalifa et al., 2020). The obtained constants of applied equations are listed in Table 1.
The plot of time versus log (Ae-At) (A) and t/At (B). The plot of t0.5 versus At (C).
Fig. 6
The plot of time versus log (Ae-At) (A) and t/At (B). The plot of t0.5 versus At (C).
Table 1 Constants of the kinetic models.
Pseudo first order Pseudo second order Intra-particle diffusion
Ae (mg/g) L1 (1/min) R2 Ae (mg/g) L2 (g/mg.min) R2 L3 (mg/g min0.5) F (mg/g) R2
110.31 0.0094 0.993 122.85 0.0001 0.998 8.78 8.13 0.999

3.2.3

3.2.3 Influence of temperature

Fig. 7A displays the plot of the percentage of removal of Ni(II) ions (% E) versus the temperature of the Ni(II) solution. Besides, Fig. 7B displays the plot of the adsorption capacity of the analcime/dimethylglyoxime composite (A) versus the temperature of the Ni(II) solution. The % E is 70, 58.6, 45.7, and 28.6% at temperature values equal to 298, 308, 318, and 328 Kelvin, respectively. Besides, A is 122.5, 102.5, 80, and 50 mg/g at temperature values equal to 298, 308, 318, and 328 Kelvin, respectively. The observable decrease of the value of both A and % E with the increase in the temperature shows that the highest removal efficiency is gotten at temperature equals 298 Kelvin. So, the optimum temperature value, which will be taken in further impacts, is 298 Kelvin.

The plot of temperature versus % E (A) and A (B). The plot of ln Ld versus 1/T (C). Experimental conditions: [Concentration of nickel solution = 350 mg/L, volume of nickel solution = 50 mL, time = 120 min, pH = 6.5, and amount of composite = 0.1 g].
Fig. 7
The plot of temperature versus % E (A) and A (B). The plot of ln Ld versus 1/T (C). Experimental conditions: [Concentration of nickel solution = 350 mg/L, volume of nickel solution = 50 mL, time = 120 min, pH = 6.5, and amount of composite = 0.1 g].

The thermodynamic parameters such as a change in free energy (ΔGo), change in the entropy (ΔSo), and change in enthalpy (ΔHo) were calculated utilizing Eqs. (6) and (7) (Abdelrahman, 2018; Abdelrahman and Hegazey, 2019; Abdelrahman et al., 2020; Abdelrahman et al., 2019; Subaihi et al., 2020; Abdelrahman et al., 2020; Youssef et al., 2020; Abdelrahman et al., 2021; Abdelbaset et al., 2020; Mahmoud et al., 2021; Abdelrahman et al., 2021).

(6)
ln L d = Δ S O R - Δ H O RT
(7)
Δ G O = Δ H O - T Δ S O where T (Kelvin), Ld (L/g), and R (kJ/mol K) are the temperature, distribution constant, and gas constant, respectively. The distribution constant (Ld) was calculated utilizing Eq. (8).
(8)
L d = A e B e

Fig. 7C displays the plot of lnLd versus 1/T. The thermodynamic parameters are listed in Table 2. The data illuminated that the uptake of Ni(II) ions is chemical due to negative sign of ΔHo. The analcime/dimethylglyoxime composite can form chelates with Ni(II) ions as shown in Scheme 2.

Table 2 Thermodynamic constants.
ΔGo (kJ/mol) ΔSo (kJ/molK) ΔHo (kJ/mol)
Temperature (Kelvin)
298 308 318 328
−94.07 −95.64 −97.20 −98.77 0.1569 −47.31
The proposed mechanism of the nickel adsorption.
Scheme 2
The proposed mechanism of the nickel adsorption.

Fig. 2B shows the FT-IR spectra of the analcime/dimethylglyoxime composite after the adsorption of Ni(II) ions. The increased intensity of FT-IR peaks after adsorption of Ni(II) ions and the shift in their wavelengths were considered as good evidence of nickel entering the composite.

The uptake of Ni(II) ions is exothermic because ΔHo is −47.31 kJ/mol. Moreover, the uptake of Ni(II) ions is spontaneous because of the negative sign of ΔGo as presented in Table 2. The uptake of Ni(II) ions takes place in a disordered way at the solution boundary/composite owing to the positive sign of ΔSo as presented in Table 2.

3.2.4

3.2.4 Influence of concentration

Fig. 8A displays the plot of the percentage of removal of Ni(II) ions (% E) versus initial nickel ion solution concentration. Besides, Fig. 8B displays the plot of the adsorption capacity of the analcime/dimethylglyoxime composite (A) versus initial nickel ion solution concentration. The % E is 86, 76.4, 70, 64.9, and 59.9% at concentration values equal 250, 300, 350, 400, and 450 mg/L, respectively. Also, A is 107.5, 114.6, 122.5, 129.8, and 134.8 mg/g at concentration values equal 250, 300, 350, 400, and 450 mg/L, respectively. The data proved the increase of A and decrease of % E with the rise in the concentration (Khalifa et al., 2020; Abdelrahman, 2018; Abdelrahman and Hegazey, 2019; Abdelrahman et al., 2020; Abdelrahman et al., 2019; Subaihi et al., 2020; Abdelrahman et al., 2020; Youssef et al., 2020; Abdelrahman et al., 2021; Abdelbaset et al., 2020; Mahmoud et al., 2021; Abdelrahman et al., 2021).

The plot of concentration versus % E (A) and A (B). Experimental conditions: [Volume of nickel solution = 50 mL, time = 120 min, temperature = 298 Kelvin, pH = 6.5, time = 120 min, and amount of composite = 0.1 g].
Fig. 8
The plot of concentration versus % E (A) and A (B). Experimental conditions: [Volume of nickel solution = 50 mL, time = 120 min, temperature = 298 Kelvin, pH = 6.5, time = 120 min, and amount of composite = 0.1 g].

The experimental results of concentration were analyzed using the Langmuir isotherm which is described using Eq. (9). Also, the experimental results of concentration were analyzed using the Freundlich isotherm which is described using Eq. (10) (Abdelrahman, 2018; Abdelrahman and Hegazey, 2019; Abdelrahman et al., 2020; Abdelrahman et al., 2019; Subaihi et al., 2020; Abdelrahman et al., 2020; Youssef et al., 2020; Abdelrahman et al., 2021; Abdelbaset et al., 2020; Mahmoud et al., 2021; Abdelrahman et al., 2021).

(9)
B e A e = 1 L 3 A max + B e A max
(10)
ln A e = l n L 4 + 1 n l n B e where Amax (mg/g) is the maximum uptake capacity of the analcime/dimethylglyoxime composite. L3 (L/mg) and L4 (mg/g)(L/mg)1/n) are the Langmuir and Freundlich constants, respectively. 1/n is the heterogeneity constant. The Amax for Freundlich isotherm was determined utilizing the formula which is described using Eq. (11) (Abdelrahman, 2018; Abdelrahman and Hegazey, 2019; Abdelrahman et al., 2020; Abdelrahman et al., 2019; Subaihi et al., 2020; Abdelrahman et al., 2020; Youssef et al., 2020; Abdelrahman et al., 2021; Abdelbaset et al., 2020; Mahmoud et al., 2021; Abdelrahman et al., 2021).
(11)
A max = L 4 B O 1 / n

Fig. 9A-B displays the Langmuir (The plot of Be/Ae versus Be) and Freundlich (The plot of ln Ae versus ln Be) isotherms, respectively. The results showed that the correlation coefficient value (R2) of the Langmuir isotherm is larger than that of the Freundlich isotherm. Hence, the Langmuir isotherm described the results better than the Freundlich isotherm. The obtained constants of applied equations are listed in Table 3. The calculated maximum adsorption capacity of analcime/dimethylglyoxime composite is 144.9 mg/g while 134.8 mg/g is the experimental one. Also, the maximum adsorption capacity of analcime was 24.2 mg/g. Hence, the analcime/dimethylglyoxime composite has higher efficiency than analcime.

The plot of Be/Ae versus Be (A). The plot of ln Ae versus ln Be (B). The plot of Ae versus ln Be (C). The plot of ln Ae versus ξ 2 (D).
Fig. 9
The plot of Be/Ae versus Be (A). The plot of ln Ae versus ln Be (B). The plot of Ae versus ln Be (C). The plot of ln Ae versus ξ 2 (D).
Table 3 Constants of the equilibrium isotherms.
Langmuir Freundlich D-R Temkin
Amax (mg/g) L3 (L/mg) R2 Amax (mg/g) L4 (mg/g)(L/mg)1/n R2 Amax (mg/g) L5 (mol2/KJ2) R2 H (J/mol) L6 (L/g) R2
144.9 0.063 0.997 146.6 64.23 0.974 86.21 0.003 0.984 0.057 2.9E18 0.952

Also, the experimental results of concentration were analyzed using the Dubinin-Radushkevich (D-R) (which is described using Eq. (12)) and Temkin isotherms (which is described using Eq. (13)) (Mahmoud et al., 2021; Abdelrahman et al., 2021).

(12)
ln A e = l n A max - L 5 ξ 2
(13)
A e = H l n L 6 + H l n B e where L6 (L/g) is the Temkin constant whereas H(J/mol) is constant related to heat of sorption. L5 (mol2/KJ2) is D-R constant whereas ε is the Polanyi potential which is described using Eq. (14).
(14)
ξ = R T l n 1 1 + B e

Eg is the mean energy of sorption which is described using Eq. (15).

(15)
E g = 1 / 2 L 5

Fig. 9C-D displays the Temkin (The plot of Ae versus ln Be) and D-R (The plot of ln Ae versus ξ 2) isotherms, respectively. The results refer that the Temkin isotherms and D-R isotherms is also suitable models to describe Ni(II) adsorption onto the fabricated composite. Also, Eg equals 13.76 kJ/mol and this confirms that the adsorption process is chemical (Abdelrahman et al., 2021).

The adsorption performance of the analcime/dimethylglyoxime composite was evaluated by comparing its adsorption capacity (Amax) with that of other adsorbent materials in the literature as clarified in Table 4. Obviously, the analcime/dimethylglyoxime composite outperformed most of the materials because it has the highest adsorption capacity value (Dhiwar et al., 2013; Sobhanardakani and Zandipak, 2015; Talebzadeh et al., 2016; Sobhanardakani et al., 2016).

Table 4 Comparison of adsorption capacity of synthesized composite with different adsorbents in the literature.
Adsorbent Adsorption capacity (mg/g) Ref
Iron oxide/chitosan composite 1.140 (Khalifa et al., 2020)
Graft copolymer of chitosan with 2-acrylamido-2-methyl-1-propanesulfonic acid 32.74 (Abdelrahman and Hegazey, 2019)
Graft copolymer of maltodextrin with 2-acrylamido-2-methyl-1-propanesulfonic acid 26.66 (Abdelrahman and Hegazey, 2019)
Magnetic hydroxyapatite/chitosan composite 112.36 (Abdelrahman and Subaihi, 2020)
Tannin-Based Dithiocarbamate composite 112.49 (Dhiwar et al., 2013)
Multi-carboxyl-functionalized silica gel 31.92 (Sobhanardakani and Zandipak, 2015)
Magnetite nanorods 95.42 (Sobhanardakani and Zandipak, 2015)
Chelating resin 62.79 (Sobhanardakani and Zandipak, 2015)
Activated carbon from scrap tire 19.53 (Sobhanardakani and Zandipak, 2015)
Thiol modified Fe3O4@SiO2 148.8 (Talebzadeh et al., 2016)
Amino functionalized magnetic graphenes 22.07 (Sobhanardakani et al., 2016)
Analcime/dimethylglyoxime composite 144.93 This study

3.2.5

3.2.5 Influence of desorption and reusability

An appropriate desorbing agent is required for the recovery of the adsorbed Ni(II) ions on the analcime/dimethylglyoxime composite. Some desorbing agents such as HNO3, HCl, EDTA disodium salt, and thiourea was utilized for three cycles of adsorption/desorption. The desorption fraction (% G) was calculated using Eq. (16) (Khalifa et al., 2020).

(16)
% G = 100 B H C H ( B O - B e ) C where CH (L) is the volume of desorbing agent whereas BH (mg/L) is the concentration of Ni(II) ions that exist in the desorbing agent. As can be seen from Table 5, the use of 0.5 M EDTA disodium salt can recover the adsorbed Ni(II) ions.
Table 5 Effect of several agents on desorption of Ni(II) ions.
Desorbing agent %G
First cycle Second cycle Third cycle
HCl 85.68 82.25 77.45
HNO3 88.37 86.48 81.26
Thiourea 96.58 95.87 95.16
EDTA disodium salt 99.97 99.84 99.25

3.2.6

3.2.6 Influence of selectivity

The matrix ions (K(I), Na(I), Ca(II), Ba(II), Mg(II), Cu(II), Cd(II), Pb(II), Hg(II), Zn(II), Al(III), Fe(III), Fe(II), Cl−, NO3−, HCO3−, and SO42−) are common in the real samples. So, these ions can noticeably affect the uptake of Ni(II) ions because of the formation of stable products with the target Ni(II) ions and/or competition binding to active sites. The tolerance limit was estimated as the maximum amount of the adverse ion that causes an error ≤ 5% in the uptake of Ni(II) ions by the procedure. As clarified in Table 6, all of the studied ions did not interfere during the uptake of Ni(II) ions by the presented procedure.

Table 6 Removal of Ni(II) ions from binary solutions in the presence of different diverse ions.
Diverse ion Tolerance limit (mg/L) % E of Ni(II) ions
Na(I) 1200 99.58
K(I) 1200 99.46
Ca(II) 150 99.28
Mg(II) 150 97.93
Ba(II) 100 98.57
Cu(II) 100 98.50
Cd(II) 100 97.48
Pb(II) 100 97.78
Hg(II) 100 96.94
Ni(II) 100 99.54
Zn(II) 120 98.62
Al(III) 120 99.41
Fe(III) 120 98.29
Fe(II) 120 98.89
Cl− 1200 99.57
NO3− 1200 99.35
HCO3− 1200 99.58
SO42− 1200 99.18

4

4 Conclusions

A novel composite was fabricated by modifying analcime with dimethylglyoxime. The fabricated composite was characterized using several tools such as XRD, FT-IR, FE-SEM, and CHN elemental analysis. XRD and FE-SEM revealed that the composite has a wide peak at 2θ = 24° and cotton-like structure, respectively. Hence, the crystal assembly of analcime combined or interfered over amorphous surroundings. The fabricated composite was operated as an efficient and novel adsorbent for the removal of Ni(II) ions from aqueous media. The effect of several factors on the removal process, for example, pH, time, temperature, and concentration were studied. The % removal (% E) equals 11.4, 25.7, 54.3, 65.7, 71.4, 72.9, and 73.4% at pH values equal 2.5, 3.5, 4.5, 5.5, 6.5, 7.5, and 8.5, respectively. The % E equals 14.6, 23.1, 34.3, 42.9, 70, 69.7, and 70.3% at time values equal 15, 30, 60, 90, 120, 150, and 180 min, respectively. The % E equals 70, 58.6, 45.7, and 28.6% at temperature values equal 298, 308, 318, and 328 Kelvin, respectively. The maximum adsorption capacity of the fabricated composite is 144.9 mg/g. The removal of Ni(II) ions is exothermic, chemical, spontaneous, and well explained by the pseudo-second-order as a kinetic model and Langmuir as an equilibrium isotherm. The efficiency of the extraction of nickel ions was not affected by the presence of many ions in the solution such as Cu(II), Cd(II), Hg(II), Pb(II), and Zn(II). 0.5 M EDTA disodium salt can recover more than 99% of the adsorbed Ni(II) ions on the composite.

Acknowledgments

The authors are grateful to the Deanship of Scientific Research, King Saud University for funding through Vice Deanship of Scientific Research Chairs.

Declaration of Competing Interest

The authors declare that they have no known competing financial interests or personal relationships that could have appeared to influence the work reported in this paper.

References

  1. , , , , . Utilisation of wastes for low-cost synthesis of chitosan composites with nanosized sodium aluminium silicate hydrate and geopolymer/zeolite A for the removal of Hg(II) and Pb(II) ions from aqueous media. Int. J. Environ. Anal. Chem. 2020
    [CrossRef] [Google Scholar]
  2. , . Synthesis of zeolite nanostructures from waste aluminum cans for efficient removal of malachite green dye from aqueous media. J. Mol. Liq.. 2018;253:72-82.
    [Google Scholar]
  3. , , , , . Facile synthesis of graft copolymers of maltodextrin and chitosan with 2-acrylamido-2-methyl-1-propanesulfonic acid for efficient removal of Ni(II), Fe(III), and Cd(II) ions from aqueous media. J. Polym. Res.. 2019;26:251-256.
    [Google Scholar]
  4. , , . Application of geopolymers modified with chitosan as novel composites for efficient removal of Hg(II), Cd(II), and Pb(II) ions from aqueous media. J. Inorg. Organomet. Polym. Mater.. 2020;30:2440-2463.
    [Google Scholar]
  5. , , , . Efficient removal of methylene blue dye from aqueous media using Fe/Si, Cr/Si, Ni/Si, and Zn/Si amorphous novel adsorbents. J. Mater. Res. Technol.. 2019;8:5301-5313.
    [Google Scholar]
  6. , , , , , , , . Facile fabrication of novel analcime/sodium aluminum silicate hydrate and zeolite Y/faujasite mesoporous nanocomposites for efficient removal of Cu(II) and Pb(II) ions from aqueous media. J. Mater. Res. Technol.. 2020;9:7900-7914.
    [Google Scholar]
  7. , , . Utilization of waste aluminum cans in the fabrication of hydroxysodalite nanoparticles and their chitosan biopolymer composites for the removal of Ni(II) and Pb(II) ions from aqueous solutions: kinetic, equilibrium, and reusability studies. Microchem. J.. 2019;145:18-25.
    [Google Scholar]
  8. , , , . Facile synthesis of mordenite nanoparticles for efficient removal of Pb(II) ions from aqueous media. J. Inorg. Organomet. Polym. Mater.. 2020;30:1369-1383.
    [Google Scholar]
  9. , , , , , . Utilization of rice husk and waste aluminum cans for the synthesis of some nanosized zeolite, zeolite/zeolite, and geopolymer/zeolite products for the efficient removal of Co(II), Cu(II), and Zn(II) ions from aqueous media. J. Hazard. Mater.. 2021;401:123813
    [Google Scholar]
  10. , , , , , . Utilization of rice husk and waste aluminum cans for the synthesis of some nanosized zeolite, zeolite/zeolite, and geopolymer/zeolite products for the efficient removal of Co(II), Cu(II), and Zn(II) ions from aqueous media. J. Hazard. Mater.. 2021;401:123813
    [Google Scholar]
  11. , , . Exploitation of Egyptian insecticide cans in the fabrication of Si/Fe nanostructures and their chitosan polymer composites for the removal of Ni(II), Cu(II), and Zn(II) ions from aqueous solutions. Compos. Part B Eng.. 2019;166:382-400.
    [Google Scholar]
  12. , , , . Simultaneous removal of organics and heavy metals from industrial wastewater: a review. Chemosphere.. 2021;262:128379
    [Google Scholar]
  13. , , . Modification of an Iranian clinoptilolite nano-particles by hexadecyltrimethyl ammonium cationic surfactant and dithizone for removal of Pb(II) from aqueous solution. J. Colloid Interface Sci.. 2015;440:272-281.
    [Google Scholar]
  14. , . Use of clinoptilolite for the removal of nickel ions from water: kinetics and thermodynamics. J. Hazard. Mater.. 2008;150:587-595.
    [Google Scholar]
  15. , , , , . Potentiality of lignin from the Kraft pulping process for removal of trace nickel from wastewater: effect of demineralisation. Bioresour. Technol.. 2009;100:1130-1137.
    [Google Scholar]
  16. , , . Enhanced removal efficiency of clinoptilolite nano-particles toward Co(II) from aqueous solution by modification with glutamic acid. Colloids Surfaces A Physicochem. Eng. Asp.. 2015;479:35-45.
    [Google Scholar]
  17. , , , , , , , , , . Enhanced removal of Co(II) and Ni(II) from high-salinity aqueous solution using reductive self-assembly of three-dimensional magnetic fungal hyphal/graphene oxide nanofibers. Sci. Total Environ.. 2021;756:143871
    [Google Scholar]
  18. , , , . Removal of copper, zinc and nickel present in natural water containing Ca2+ and HCO3 ions by electrocoagulation. Sep. Purif. Technol.. 2013;107:109-117.
    [Google Scholar]
  19. , , . Increased photocatalytic activity of NiO and ZnO in photodegradation of a model drug aqueous solution: effect of coupling, supporting, particles size and calcination temperature. J. Hazard. Mater.. 2017;321:629-638.
    [Google Scholar]
  20. , . Removal of nickel from electroplating rinse waters using electrostatic shielding electrodialysis/electrodeionization. J. Hazard. Mater.. 2010;173:647-652.
    [Google Scholar]
  21. , , , . Nano-iron oxide-encapsulated chitosan microspheres as novel adsorbent for removal of Ni (II) ions from aqueous solution. Res. Chem. Intermed.. 2013;39:2989-3009.
    [Google Scholar]
  22. , , , , . Removal of heavy metals from aqueous solution using carbon-based adsorbents: a review. J. Water Process Eng.. 2020;37:101339
    [Google Scholar]
  23. , , . EDTA-functionalized clinoptilolite nanoparticles as an effective adsorbent for Pb(II) removal. Environ. Sci. Pollut. Res.. 2018;25:14043-14056.
    [Google Scholar]
  24. , , . Synergistic effects of ion exchange and complexation processes in cysteine-modified clinoptilolite nanoparticles for removal of Cu(II) from aqueous solutions in batch and continuous flow systems. New J. Chem.. 2017;41:3811-3820.
    [Google Scholar]
  25. , , , , , . Removal of nickel ions from aqueous solution by low energy-consuming sorption process involving thermosensitive copolymers with phosphonic acid groups. J. Hazard. Mater.. 2013;244–245:507-515.
    [Google Scholar]
  26. , , . Clinoptilolite nanoparticles modified with dimethyl glyoxime as a sensitive modifier for a carbon paste electrode in the voltammetric determination of Ni(II): experimental design by response surface methodology. New J. Chem.. 2017;41:13355-13364.
    [Google Scholar]
  27. , , , , , , , , . Facile Hydrothermal fabrication of analcime and zeolite X for efficient removal of Cd(II) ions from aqueous media and polluted water. J. Inorg. Organomet. Polym. Mater. 2020
    [CrossRef] [Google Scholar]
  28. , , . Clinoptilolite nano-particles modified with aspartic acid for removal of Cu(ii) from aqueous solutions: isotherms and kinetic aspects. New J. Chem.. 2015;39:9396-9406.
    [Google Scholar]
  29. , , , , , . Novel adsorptive membrane through embedding thiol-functionalized hydrous manganese oxide into PVC electrospun nanofiber for dynamic removal of Cu(II) and Ni(II) ions from aqueous solution. J. Water Process Eng.. 2020;37:101401
    [Google Scholar]
  30. , . Removal of Ni(II) and Zn(II) from an aqueous solution by reverse osmosis. Desalination. 2005;174:161-169.
    [Google Scholar]
  31. , , . Removal of nickel ions from water by multi-walled carbon nanotubes. J. Hazard. Mater.. 2007;146:283-288.
    [Google Scholar]
  32. , , , , . Use of ultrafiltration membranes and aluminosilicate minerals for nickel removal from industrial wastewater. J. Memb. Sci.. 2010;360:234-249.
    [Google Scholar]
  33. , , , , , . Use of microwave irradiation for modification of mesoporous silica nanoparticles by thioglycolic acid for removal of cadmium and mercury. Microporous Mesoporous Mater.. 2018;258:217-227.
    [Google Scholar]
  34. , , , , . Application of mesoporous silica nanoparticles modified with dibenzoylmethane as a novel composite for efficient removal of Cd(II), Hg(II), and Cu(II) ions from aqueous media. J. Inorg. Organomet. Polym. Mater.. 2020;30:2182-2196.
    [Google Scholar]
  35. , , , , , , , . A novel cross-linked magnetic hydroxyapatite/chitosan composite: preparation, characterization, and application for Ni(II) ion removal from aqueous solution. Water. Air. Soil Pollut.. 2018;229:101-111.
    [Google Scholar]
  36. , , , . Manganese dioxide nanoparticles decorated with chitosan for effective removal of lead and lanthanum ions from water by microwave sorption technique. Mater. Sci. Eng. B Solid-State Mater. Adv. Technol.. 2021;267:115091
    [Google Scholar]
  37. , , . Efficient solid amino acid–clinoptilolite nanoparticles adsorbent for Mn(II) removal: a comprehensive study on designing the experiments, thermodynamic and kinetic aspects. Solid State Sci.. 2020;101:106124
    [Google Scholar]
  38. , , , , , , . Comparison between electrocoagulation and chemical precipitation for metals removal from acidic soil leachate. J. Hazard. Mater.. 2006;137:581-590.
    [Google Scholar]
  39. , , . Comparison of the efficiency of modified clinoptilolite with HDTMA and HDP surfactants for the removal of phosphate in aqueous solutions. J. Ind. Eng. Chem.. 2015;31:185-191.
    [Google Scholar]
  40. , , . A comprehensive study on the kinetics and thermodynamic aspects of batch and column removal of Pb(II) by the clinoptilolite–glycine adsorbent. Mater. Chem. Phys.. 2020;240:122142
    [Google Scholar]
  41. , , . Modification of a PVC-membrane electrode by surfactant modified clinoptilolite zeolite towards potentiometric determination of sulfide. Microporous Mesoporous Mater.. 2012;153:267-274.
    [Google Scholar]
  42. , , . Effective removal of Ni(II) from aqueous solutions by modification of nano particles of clinoptilolite with dimethylglyoxime. J. Hazard. Mater.. 2013;260:339-349.
    [Google Scholar]
  43. , , . High catalytic activity of Fe(II)-clinoptilolite nanoparticales for indirect voltammetric determination of dichromate: experimental design by response surface methodology (RSM) Electrochim. Acta.. 2017;223:47-62.
    [Google Scholar]
  44. , , , , . Infrared spectroscopic studies of dimethylglyoxime chelates of nickel, cobalt, copper, palladium and platinum. J. Mol. Struct.. 1991;249:277-283.
    [Google Scholar]
  45. , , . Experimental design on determination of Sn(II) by the modified carbon paste electrode with Fe(II)-exchanged clinoptilolite nanoparticles. Solid State Sci.. 2020;99:106082
    [Google Scholar]
  46. , , , , , , , . Nickel ion removal from wastewater using the microbial electrolysis cell. Bioresour. Technol.. 2012;121:458-461.
    [Google Scholar]
  47. , , . Removal of lead, copper, nickel, cobalt, and zinc from water by a cancrinite-type zeolite synthesized from fly ash. Chem. Eng. J.. 2009;145:483-488.
    [Google Scholar]
  48. , , , , , , , . Graphene/δ-MnO2 composite as adsorbent for the removal of nickel ions from wastewater. Chem. Eng. J.. 2011;175:1-7.
    [Google Scholar]
  49. , , , , . Significance of conducting polyaniline based composites for the removal of dyes and heavy metals from aqueous solution and wastewaters-A review. Chemosphere.. 2021;267:129201
    [Google Scholar]
  50. , , , . Assessment of Pb2+ removal capacity of lichen (Evernia prunastri): application of adsorption kinetic, isotherm models, and thermodynamics. Environ. Sci. Pollut. Res.. 2019;26:27002-27013.
    [Google Scholar]
  51. , , , . Preparation and characterization of a novel diatomite-based composite and investigation of its adsorption properties for uranyl ions. J. Radioanal. Nucl. Chem.. 2019;321:791-803.
    [Google Scholar]
  52. , , . A comprehensive study on the removal of Cd(II) from aqueous solution on a novel pentetic acid-clinoptilolite nanoparticles adsorbent: experimental design, kinetic and thermodynamic aspects. Solid State Sci.. 2020;99:106071.
    [Google Scholar]
  53. , , . A comprehensive study on the removal of Cd(II) from aqueous solution on a novel pentetic acid-clinoptilolite nanoparticles adsorbent: experimental design, kinetic and thermodynamic aspects. Solid State Sci.. 2020;99:106071.
    [Google Scholar]
  54. , , , , . Use of wollastonite in the removal of ni(ii) from aqueous solutions. Water Air Soil Pollut.. 1990;49:69-79.
    [Google Scholar]
  55. , , , , , . Progress in the remediation of hazardous heavy metal-polluted soils by natural zeolite. J. Hazard. Mater.. 2009;170:1-6.
    [Google Scholar]
  56. , , . An efficient modified zeolite for simultaneous removal of Pb(II) and Hg(II) from aqueous solution. J. Mol. Liq.. 2017;230:221-229.
    [Google Scholar]
  57. , , , . Synthesis and characterization of a composite polymeric material including chelating agent for adsorption of uranyl ions. J. Hazard. Mater.. 2017;338:437-446.
    [Google Scholar]
  58. , . Ecological and human health risk assessment of heavy metal content of atmospheric dry deposition, a case study: Kermanshah, Iran. Biol. Trace Elem. Res.. 2019;187:602-610.
    [Google Scholar]
  59. , , . 2,4-Dinitrophenylhydrazine functionalized sodium dodecyl sulfate-coated magnetite nanoparticles for effective removal of Cd(II) and Ni(II) ions from water samples. Environ. Monit. Assess.. 2015;187:412-424.
    [Google Scholar]
  60. , , , . Removal of Ni(II) and Zn(II) from aqueous solutions using chitosan. Arch. Hyg. Sci.. 2016;5:47-55.
    [Google Scholar]
  61. , , . Synthesis and application of TiO2/SiO2/Fe3O4 nanoparticles as novel adsorbent for removal of Cd(II), Hg(II) and Ni(II) ions from water samples. Clean Technol. Environ. Policy.. 2017;19:1913-1925.
    [Google Scholar]
  62. , , , , , , , , . Studying some analytical parameters affecting the removal of Mn(II) ions from aqueous media using facilely synthesised analcime. Int. J. Environ. Anal. Chem. 2020
    [CrossRef] [Google Scholar]
  63. , , . Vibrational analysis of the bis(dimethylglyoximato)nickel(II) complex. J. Mol. Struct.. 2003;651–653:547-553.
    [Google Scholar]
  64. , , , . CeO2 nanoparticles supported on CuFe2O4 nanofibers as novel adsorbent for removal of Pb(II), Ni(II), and V(V) ions from petrochemical wastewater. Desalin. Water Treat.. 2016;57:28363-28377.
    [Google Scholar]
  65. , , . A comprehensive study on the kinetic aspects and experimental design for the voltammetric response of a Sn(IV)-clinoptilolite carbon paste electrode towards Hg(II) J. Electroanal. Chem.. 2018;829:95-105.
    [Google Scholar]
  66. , , . Sensitive voltammetric determination of bromate by using ion-exchange property of a Sn(II)-clinoptilolite-modified carbon paste electrode. J. Solid State Electrochem.. 2019;23:143-157.
    [Google Scholar]
  67. , , , , . Sorption kinetics and equilibrium for the removal of nickel ions from aqueous phase on calcined Bofe bentonite clay. J. Hazard. Mater.. 2010;177:362-371.
    [Google Scholar]
  68. , , , , , , , , , , . Facile hydrothermal procedure for the synthesis of sodium aluminum silicate hydrate/analcime and analcime for effective removal of manganese(II) ions from aqueous solutions. J. Inorg. Organomet. Polym. Mater. 2020
    [CrossRef] [Google Scholar]
  69. , , , , , , , . Fabrication of tannin-based dithiocarbamate biosorbent and its application for Ni(II) ion removal. Water. Air. Soil Pollut.. 2016;228:409-412.
    [Google Scholar]

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