# Removal of Cadmium (II), Chromium (III), and Lead (II) Heavy Metal Ions from Water by Graft Copolymerization of Acrylonitrile onto Date Palm Fiber Using H2O2/Fe++ as an Initiator

Authors: Faraj Ahmad Abuilaiwi
Journal: International Journal of Polymer Science
 (2020)

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## Abstract

The study is aimed at assessing how the date palm wood fibers (DPWF) can be used for the removal of heavy metals from water. The study involved examination of the radical polymerization and graft polymerization parameters such as reaction period, reaction time, monomer volume, amount of the catalyst, and concentration of initiator to obtain the maximum yield of graft polymerization. Fiber and copolymer were characterized using SEM and FT-IR spectroscopy to ensure the completion of polymerization. Hydroxylamine hydrochloride was used for treating the grafted copolymers for the preparation of polyamidoxime chelating resin, which was then examined for removing the heavy metal ions. Different resin dosages, contact time, and initial concentrations were used, and the batch technique experiment was utilized. The study also applied the Langmuir and Freundlich isotherm model, and Langmuir was found to be better. The absorption ability was found to be better for polyamidoxime resin for metal ions of cadmium (II), chromium (III), and lead (II).


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## Body

## 1. Introduction

Discharge of heavy metals in the industrial effluents has increased the problem of water pollution [1]. Previous studies have revealed that nonbiodegradable heavy metals tend to accumulate in the bodies of living organisms and, for the same reason, they are more hazardous as compared to other water pollutants [2]. Copper, silver, zinc, selenium, cadmium, mercury, lead, nickel, chromium, tin, iron, arsenic, gold, molybdenum, cobalt, manganese, aluminum, etc. are some commonly found heavy metals [3], which are proved to be harmful for humans and other living organisms [1]. Fu and Wang [4] stated that regular deposition of heavy metal subsequently causes severe damage to the central nervous system, skin, kidneys, teeth, liver, or lungs and could also lead to death. Additionally, the removal of heavy metals is also challenging on account of their nonbiodegradability [5].In order to address this issue, researchers are focusing on the use of natural and bio-based materials [6]. Various kinds of biobased materials have been introduced, which may be based on cellular fibers, wood, or protein and help in reducing the harmful effects caused by nonbiodegradable elements [7]. Similarly, for the removal of heavy metals from aqueous solution, different methods, including precipitation and membrane processes: reverse osmosis, ion exchange, ultrafiltration, and more, are being used [8]. The use of precipitation after coagulation is limited on account of high sludge volume. Studies have identified membrane filtration as a cost-effective way of ensuring the removal of metal ions; however, its cost is a major impediment in its implementation [9, 10].Kanamarlapudi et al. [10] found absorption as an efficient, simple, and effective approach in the removal of heavy metals from the wastewater; however, its high cost is also major challenge in its implementation. These challenges instigated scholars and researchers to find or develop cost-effective, eco-friendly, and nonconventional absorbents [9]. Recently, the interest in the use of plant-based fiber has increased, which is commercially in the production of polymer composites [1]. These composites can be used for removing the heavy metal ions from water especially when conventional methods are proved ineffective [11]. In order to satisfy and solve the above-mentioned problems, some natural materials such as cellulose, chitosan, chitin, and their derivatives have been specified as good and inexpensive options because of their economic efficiency, absorbent properties, safety, and biodegradability.Ion exchange is a reaction in which free mobile ions of a solid are exchanged with different ions of identical charge in a solution. The exchanger contains an open network structure, either organic or inorganic, which carries the ions and let ions to pass through it. Ion exchangers may be organic or inorganic and are natural or synthetic materials such as synthetic resins which function as ion exchangers based on three-dimensional organic networks bearing charged or potentially charged groups [12]. Past research has shown increased interest in the use of date palm as a biodegradable material [13].Recently, many studies have focused on exploring an alternative metal adsorbent and grafted polymers. Grafting is the method in which functional monomers are covalently bonded to the backbone polymer chain [14–17]. Graft polymerization is significant as it permits implementing different functions of the grafted monomer on the parent polymer while retaining the mechanical features of the parent polymer. Radiation-induced grafting technique is dominant over all other approaches implemented to initiate graft copolymerization such as ultraviolet light, decomposition of chemical initiators, oxidation of polymers, plasma treatment, and ionizing radiation because of its extensive penetration into the polymer matrix and its rapid and homogeneous development of radicals [18, 19].Date palm (“Phoenix dactylifera”) is abundantly grown throughout Saudi Arabia, and its global production rate is 42%. It is an edible fruit with a papery skin and a single, long, narrow, hard seed. There are many uses of date palm wood; for instance, it is used as posts and rafters for huts because it is lighter than coconut. It is also used in the construction of aqueducts, bridges, and parts of boats and dhows. Moreover, the tree residues are used as fuel [20]. Date palm contains three major components: cellulose, lignin, hemicellulose, and other minor constituents such as protein and oil [21].The focus of this is on date palm on account of its abundance, cost-effectiveness, and renewability in the Kingdom of Saudi Arabia. Its fiber produces biodegradable materials when treated with certain monomers and can be obtained at low costs in comparison with the costly plastic materials which are commonly used for removing metal ions from water. The limitations associated with heavy metals have led to extensive researches for the production of cost-effective alternatives which should be excessively available as waste materials. In the current study, the effectiveness of date palm fibers as low-cost bioabsorbent of heavy metals has been studied, with a focus on the impacts of the different reaction parameters that influence the adsorption efficiency.


### 1.1. Modified Date Palm as Adsorbent of Heavy Metals

In 30 countries, approximately 120 million date palm trees are cultivated covering an area of 800,000 hectares [22, 23]. The investigation of the regional distribution shows that approximately 60 million date palm trees are located in Iran, Iraq, Oman, Pakistan, Saudi Arabia, Yemen, Bahrain, and Turkmenistan, and almost 32.5 million date palm trees are located in Africa. El-Hendawy [24] investigated the adsorption capacities of date pit-activated carbons with respect to Pb2+ and Cd2+. Data were compatible with the Langmuir model, which substantially contributed to the increase in adsorption capacity in comparison with raw date pits and subsequently led to the increase in the adsorption of lead. The consumption was higher than cadmium due to its suitable pH for complexation or deposition and lower solubility. el Nemr et al. [25] assessed the removal of toxic chromium (VI) from different aqueous solutions with the help of an adsorbent containing activated carbon obtained date palm seed. The optimum pH for absorption was 1.0, and the increase in pH decreased the adsorption percentage. 120.48 mg/g was the maximum adsorption capacity for chromium (VI), and the equilibrium was obtained in 180 min due to the fast adsorption process. Studies have shown that the use of date stone and palm tree waste increases the Cu2+ adsorption, where equilibrium was obtained within 120 min [26, 27]. Hilal et al. [28] stated that maximum absorption capacity of activated date pits was at a pH of 5.8±0.5, which was five times greater than that of the raw date pits.Abdulkarim and Al-Rub [29] studied the removal of lead (II) onto activated carbons, and 8-hydroxyquinoline modified activated carbons from date pits. The adsorption capacity was high in both the carbons; however, no significant improvement was found in adsorption after modification. Removal of Pb (II) ions using activated carbons was increased with an increase in pH. This process followed pseudo-second-order kinetics. The Langmuir and Freundlich models showed good agreement from the equilibrium data for the adsorption of lead (II) ions. Yadav et al. [30] showed that date palm fibers can remove 99.955 chromate anions (Cr6+) from a 100 mg L-1 solution with the use of a small absorbent dosage, i.e., 1.2 g L-1.Tunisian date stones activated via phosphoric acid were used for the removal of copper (II) from aqueous solutions. The best-activated carbon for the removal process was obtained with 60% phosphoric acid and an impregnation ratio of 1.75 at 450°C. Dubinin–Kaganer–Radushkevich and Langmuir adsorption isotherm models were enough to explain the adsorption of copper (II) onto activated carbon (q°) which was found to be 31.25 mg/g. Bouhamed et al. [26] suggested a chemisorption process from kinetic data that were compatible with the pseudo-second-order kinetic model.el-Shafey and al-Kindy [31] modified leaflets of date palm using the sulphuric acid method at 170°C. They suggested that the hot sulphuric acid dehydrates and induces reduction property in carbon. This carbon was used to remove copper and silver from aqueous solution using various parameters such as contact time, pH, temperature, and metal concentration. Adsorption of copper was greater as compared to the adsorption of silver as the equilibrium was reached within ∼2 h and ∼60 h, respectively. The adsorption of copper was carried out through the diffusion-controlled ion exchange process; however, the value of activation energy of silver indicated chemisorption of silver ions into carbon.The adsorption capacities of raw date pits and CO2 activated date pits were compared with respect to the adsorption of copper and zinc ions. Banat et al. [32] found adsorption of both copper and zinc onto raw date pits higher than adsorption onto activated date pit carbon. This attributed to the difference in the surface functional groups of date pits and activated date pits. The heating during the activation process may have destroyed the functional groups that facilitate binding of zinc and copper. The removal of copper was better in comparison with the removal of zinc with respect to both the materials on account of its small ionic radius that facilitates an easy movement into porous surface. The best result was obtained at pH=5 and temperature at 25°C.


## 1.1. Modified Date Palm as Adsorbent of Heavy Metals

In 30 countries, approximately 120 million date palm trees are cultivated covering an area of 800,000 hectares [22, 23]. The investigation of the regional distribution shows that approximately 60 million date palm trees are located in Iran, Iraq, Oman, Pakistan, Saudi Arabia, Yemen, Bahrain, and Turkmenistan, and almost 32.5 million date palm trees are located in Africa. El-Hendawy [24] investigated the adsorption capacities of date pit-activated carbons with respect to Pb2+ and Cd2+. Data were compatible with the Langmuir model, which substantially contributed to the increase in adsorption capacity in comparison with raw date pits and subsequently led to the increase in the adsorption of lead. The consumption was higher than cadmium due to its suitable pH for complexation or deposition and lower solubility. el Nemr et al. [25] assessed the removal of toxic chromium (VI) from different aqueous solutions with the help of an adsorbent containing activated carbon obtained date palm seed. The optimum pH for absorption was 1.0, and the increase in pH decreased the adsorption percentage. 120.48 mg/g was the maximum adsorption capacity for chromium (VI), and the equilibrium was obtained in 180 min due to the fast adsorption process. Studies have shown that the use of date stone and palm tree waste increases the Cu2+ adsorption, where equilibrium was obtained within 120 min [26, 27]. Hilal et al. [28] stated that maximum absorption capacity of activated date pits was at a pH of 5.8±0.5, which was five times greater than that of the raw date pits.Abdulkarim and Al-Rub [29] studied the removal of lead (II) onto activated carbons, and 8-hydroxyquinoline modified activated carbons from date pits. The adsorption capacity was high in both the carbons; however, no significant improvement was found in adsorption after modification. Removal of Pb (II) ions using activated carbons was increased with an increase in pH. This process followed pseudo-second-order kinetics. The Langmuir and Freundlich models showed good agreement from the equilibrium data for the adsorption of lead (II) ions. Yadav et al. [30] showed that date palm fibers can remove 99.955 chromate anions (Cr6+) from a 100 mg L-1 solution with the use of a small absorbent dosage, i.e., 1.2 g L-1.Tunisian date stones activated via phosphoric acid were used for the removal of copper (II) from aqueous solutions. The best-activated carbon for the removal process was obtained with 60% phosphoric acid and an impregnation ratio of 1.75 at 450°C. Dubinin–Kaganer–Radushkevich and Langmuir adsorption isotherm models were enough to explain the adsorption of copper (II) onto activated carbon (q°) which was found to be 31.25 mg/g. Bouhamed et al. [26] suggested a chemisorption process from kinetic data that were compatible with the pseudo-second-order kinetic model.el-Shafey and al-Kindy [31] modified leaflets of date palm using the sulphuric acid method at 170°C. They suggested that the hot sulphuric acid dehydrates and induces reduction property in carbon. This carbon was used to remove copper and silver from aqueous solution using various parameters such as contact time, pH, temperature, and metal concentration. Adsorption of copper was greater as compared to the adsorption of silver as the equilibrium was reached within ∼2 h and ∼60 h, respectively. The adsorption of copper was carried out through the diffusion-controlled ion exchange process; however, the value of activation energy of silver indicated chemisorption of silver ions into carbon.The adsorption capacities of raw date pits and CO2 activated date pits were compared with respect to the adsorption of copper and zinc ions. Banat et al. [32] found adsorption of both copper and zinc onto raw date pits higher than adsorption onto activated date pit carbon. This attributed to the difference in the surface functional groups of date pits and activated date pits. The heating during the activation process may have destroyed the functional groups that facilitate binding of zinc and copper. The removal of copper was better in comparison with the removal of zinc with respect to both the materials on account of its small ionic radius that facilitates an easy movement into porous surface. The best result was obtained at pH=5 and temperature at 25°C.


## 2. Methodology

### 2.1. Materials and Reagents

A nonwoven polyethylene fabric was used as a trunk polymer for graft polymerization; the material was obtained from Kurashiki MFG Co. Monomer acrylonitrile (BDH, England) was used for grafting onto a trunk polymer. Sodium carbonate, methanol, acetone, and sulphuric acid were obtained from Merck, Germany, and hydroxyl amine hydrochloride was obtained from Sigma-Aldrich, USA. Cadmium (II), lead (II) acetate trihydrate (Merck, Germany), and chromium (III) (Techno Pharmchem, India) were used for a metal adsorption study. Date palm fiber was obtained from a local market, and the size of the fiber was less than 200μm. The fiber was washed two times with hot distilled water and acetone. The acetone was removed by heating the fiber in an oven at 60°C.


### 2.2. FTIR Spectroscopy

Infrared (IR) spectra of the DPW, grafted DPW, and the poly (amidoxime) ion-exchange resin samples were recorded on a Fourier transform–IR spectrometer (Perkin–Elmer 1725, Norwalk, CT) using a KBr disk pellet.


### 2.3. Scanning Electron Microscopy (SEM)

The SEM photographs of the fiber surfaces of grafted PAN onto DPW and ungrafted DPW fiber were captured using a scanning electron microscope model SEM JEOL 6400 (JEOL, Peabody, MA).


### 2.4. Preparation of a Chelating Resin Containing Polyamidoxime Groups

Hydroxylamine hydrochloride (NH2OH.HCl) solution was prepared by dissolving 20 g (0.288 mol) of hydroxylamine hydrochloride in 300 ml of a methanolic aqueous solution (methanol/waterratio=80). The hydrochloride content of NH2OH.HCl was neutralized by the addition of NaOH solution, and the precipitated NaCl was removed by filtration. The grafted product was placed in a two-necked flask equipped with a condenser; the flask was placed in a thermostatic water bath, and the hydroxylamine solution was poured in it. The mixture was allowed to react at 70°C with continuous stirring for 180 min. After completion of the reaction, the resin was filtered and washed several times with the methanolic solution. The resin was neutralized by treating it with 0.1 M HCl solution for 15 min; afterwards, it was again filtered, washed several times with the methanolic solution, and then dried in an oven at a constant weight at 60°C.


### 2.5. Sorption of Lead Cadmium and Chromium Ions Using the Batch Technique

The lead, cadmium, and chromium ion adsorption capacities of the resin were measured over the pH range of 1–6. Thus, ca. 0.1 g of dried resin was placed in a series of 100 ml polyethylene bottles and equilibrated with 20 ml of distilled water. After adding 20 ml of 0.1 M sodium acetate buffer solution in each bottle, 10 ml of 0.1 M lead-ions solution was added. The resulting mixture was shaken for 24 h by a rotary shaker, and afterwards, 5 ml of the supernatant was collected for the determination of metal-ions. An AGBC-903 atomic absorption spectrometer was used to determine the initial and final amounts of metal ions present in the solutions.Blank experiments were performed, and the same experimental procedure was conducted for checking the adsorption level by the membrane filters and glass flasks for all adsorption tests. The kinetic samples were conducted in 1000 ml batch reactors at 20.0 in deionized water. The flasks were vigorously and magnetically stirred for 1.5 h for hydrating the beet pulp to naturally maintain the pH at 5.5.


### 2.6. Graft Copolymerization

To prepare the fiber/PAN copolymer, 1.00 g DPW fiber was placed in 250 ml three-necked flasks equipped with a stirrer and condenser and immersed into a thermostatic water bath. The DPW suspension was obtained by adding 100 ml distilled water and 0.1 g ferrous ammonium sulphate with continuous stirring. Nitrogen purged through the DPW fiber slurry to remove oxygen during the reaction. After 30 min, the required volume of 2.0 M H2O2 was added and the mixture was mixed for 5 min; afterwards, the required amounts of monomer (AN) were added into the mixture. The reaction mixture was stirred under nitrogen at the chosen temperature and for the predetermined reaction period. Immediately after the reaction, the reaction flask was cooled by placing it under running tap water, and the product was filtered. The crude product was washed thoroughly with distilled water and oven-dried at 60°C at a constant weight.


### 2.7. Removal of Polyacrylonitrile and Determination of Graft Level

The crude product was purified withN,N-dimethylformamide using a Soxhlet extractor for 48 h to remove the polyacrylonitrile (PAN). The pure grafted copolymers were then dried at 65°C at a constant weight. The following formula determined the percentage of grafting (Pg):
(1)Pg=W2−W1W1×100,where W1 is the weight of the original DPW fibers in grams and W2 is the weight of the grafted product after copolymerization and extraction [33].


### 2.8. Graft Copolymerization

Date palm wood fiber (DPWF) was treated with a mixed solution of hydrogen peroxide and ferrous ammonium sulfate to initiate a free radical in the backbone of the fiber and provide cellulose macroradical. Graft copolymerization occurred after adding acrylonitrile (AN) monomer to the mixture during which the cellulose macroradical broke the double bond in AN and a covalent bond between monomer and cellulose was formed, the chain initiated with continues creation of free radical on the AN. Chain grafting onto the cellulose was possible by adding AN monomer subsequently. The reaction was ultimately terminated either by the formation of a copolymer on account of the reaction of two macroradical or formation of poly(methacrylate) by the reaction of two monomer radicals. Figure1 explains the whole process [34, 35].Figure 1
Mechanism of graft copolymerization of acrylonitrile onto DPWF.


### 2.9. Optimization of Grafted Polymerization Parameters

Effects of various parameters on the yield of grafted copolymerization were studied. These parameters included temperature, reaction time, monomer volume, cocatalyst amount, and concentration of initiator. All these parameters were studied separately to investigate the best conditions and to obtain the best yield.


#### 2.9.1. Effect of Temperature

A wide range of temperatures was used to obtain the best yield of the grafted copolymer. Figure2 illustrates the effect of temperature that increase in temperature from 30°C up to 75°C increases the % yield of grafting. This increase could be attributed to the increase of monomer diffusion into the active sites on the backbone of the substrate. If temperature goes above 75°C, the monomer starts to evaporate, and hydrogen peroxide decomposes. This condition leads to creation of a huge number of free radicals, the yield of a homopolymer will increase, and % of the grafted copolymer in pg will decrease [36, 37].Figure 2
Effect of reaction temperature on the % of grafting in pg. Reaction time: 60 min, AN: 8 ml, H2O2: 0.03 M, Fe+2: 0.3 mmol, and (∆): % of grafting.


#### 2.9.2. Effect of the Concentration of Initiator

The yield of grafted polymer is clearly affected by the concentration of the initiator. As shown in Figure3, the % of grafting increased with the increase in the concentration of the hydrogen peroxide as it increases the production of free radicals in the active sites of the fiber. At 0.03 M concentration, 81% grafting was obtained. However, the grafting percentage decreased with further increase in the percentage of hydrogen peroxide because of the reaction between cellulose radicals before addition of monomers, and this reaction is the termination step. Moreover, at higher concentrations, the yield of homopolymer increases [34].Figure 3
Effect of the amount of initiator H2O2 on the % of grafting. Reaction time: 60 min, AN: 8 ml, temperature: 75°C, Fe+2: 0.3 mmol, and (∆): % of grafting.


#### 2.9.3. Effect of the Amount of Monomer

The percentage of grafting increased with the increasing volume of the (AN) monomer on account of the availability of a large number of monomer molecules reaching the active sites in the backbone of the fiber. However, as shown in Figure4, increase in volume over 8 ml decreased the percentage of grafting on account of the increased possibility of homopolymerization [37, 38].Figure 4
Effect of the amount of monomer (AN) on the % of grafting. Reaction time: 60 min, H2O2: 0.03 M, temperature: 75°C, Fe+2: 0.3 mmol, and (∆): % of grafting.


#### 2.9.4. Effect of Reaction Period

The percentage of grafting was found directly proportional to the increase in the reaction time, and it increases the time available to all monomer molecules to reach the active sites on the backbone; however, the maximum grafting yield was obtained with the reaction time of 60 minutes. Afterwards, all active sites were covered, and the concentration of all reaction species decreased and this accounted for the low yield of grafting which almost remains constant with increasing time [39]. This explanation is in line with the results shown in Figure 5.Figure 5
Effect of reaction period on the % of grafting and efficiency. AN: 8 ml, H2O2: 0.03 M, temperature: 75°C, Fe+2: 0.3 mmol, and (∆): % of grafting.


#### 2.9.5. Effect of the Amount of Catalyst

Small amount of ammonium ferrous sulphate [(NH4)2SO4·FeSO4·6H2O] was found to be enough for the best yield of a product (Figure 6), where 0.306 mmol of catalyst gave 81% of grafting product. This yield decreased with the increase in the amount of the catalyst on account of a large number of radicals produced by the decomposition of hydrogen per oxide. The reaction finally terminates due to the reaction between radicals and yield will decrease [33, 40].Figure 6
Effect of the amount of catalyst Fe+2on the % of grafting. AN: 8 ml, H2O2: 0.03 M, temperature: 75°C, time: 60 min, and (∆): % of grafting.


### 2.10. Preparation of Polyamidoxime Resin

The AN-DPWF grafted copolymer containing nitrile group was treated with hydroxylamine hydrochloride at pH 11 to change the nitrile group into amidoxime. This reaction was performed for 3 hours at 75°C, and the ratio between grafted copolymer and hydroxylamine in methanolic solution was 1 : 1. The mechanism of this conversion is shown in Figure7.Figure 7
Reaction mechanism of preparation of polyamidoxime resin.


### 2.11. Characterization of AN-DPWF Grafted Copolymer and Resin

FT-IR spectra were obtained for DPWF, grafted copolymer, and amidoxime resin to confirm the completion of polymerization and conversion of grafted copolymer into the chelating resin. In Figure8, the same characteristic adsorption bands for DPWF, such as broad absorption band between 3000 and 3500 cm-1 were assigned to O-H stretching vibration and bands that appeared at 2900 and 1020 cm-1 for C-H stretching and bending modes, respectively. The characteristic adsorption at 2240 cm-1 for C≡N stretching modes confirms the presence of acrylonitrile onto the backbone of DPWF and grafting reaction completely [41].Figure 8
FTIR DPWF fiber (─), AN-g-DPWF fiber (- -), and resin containing amidoxime groups (···).This band disappeared completely after conversion to amidoxime resin, and new adsorption band formed at 1650 cm-1 associated with C=N vibration of the amidoxime group. Another adsorption band observed at 941 cm–1 may be assigned to the N–O bond of the oxime group [42]. Scanning electron microscope (SEM) images were taken for DPWF before and after polymerization to investigate the changes in the morphology of the fiber surface. Figures 9 and 10 show the surface of the fiber before and after grafted polymerization, respectively. As can be seen in Figure 10, all pours on the DPWF surface were covered with polyacrylonitrile (PAN) via the chemical bond and this covering yielded a homogeneous surface with less porosity.Figure 9
Scanning electron micrographs of DPWF before grafting, SEM MAG (1.36 KX).Figure 10
Scanning electron micrographs of DPWF after grafting, SEM MAG (1.47 KX).


### 2.12. Effect of Initial pH

The pH solution is a substantial parameter used in the study of the removal of heavy metal ions from aqueous solution or water on account of many reasons such as its effects on the concentration of counter ions placed in adsorbent functional clusters, the level of ionization of the adsorbate during the reaction, and the solubility of metal ions. Batch technique was conducted to find out the optimum pH level required for the removal of heavy metals using amidoxime chelating resin. The concentration of the counter ions on the resin, ability of ionization, and solubility of adsorbates depend on pH [43]. A wide range of pH (1.0 to 6.0) was investigated to get the optimum pH for a fixed concentration of metals and dosage of resin at 25°C. The adsorption of lead (II), Cr (III), and Cd (II) was maximum at the pH=5.0 as shown in Figure 11. At low pH (<3.0), the competition between H+ ions for the resin sites increased and the resin’s chelating ability was greatly reduced. At pH 5, the competition of H+ ions for the resin sites decreases and the chelating ability of the metal ion increases [44]. Equation (2) is used to calculate the percentage of the removal of metal ions using this resin [39, 45, 46].
(2)%ofremoval=C0−CeC0×100.Figure 11
Effect of pH on the adsorption of (Pb+2), (Cr+3), and (Cd+2) ions; dosage of chelating resin: 1 g; ion concentration: 50 mg/L; time: 60 min; and temperature: 25°C.


### 2.13. Effect of Contact Time and Initial Concentration

The contact time is one of the important parameters to study as it affects the adsorption of heavy metals onto chelating resin. From Figure12, it can be observed that the adsorption of heavy metals increases with the increase in the contact time. Also, the adsorption was fast in the beginning until it reaches equilibrium at 35 min, and afterwards, the value of qt (mg/g) remains constant. This can be attributed to the availability of active sites on the surface of chelating resin in the beginning of reaction [47]. Initial concentration of metals under study: lead (II), Cr (III), and Cd (II), influenced the removal of these metals. The amount of metal ions, qt (milligrams per gram) adsorbed, is calculated by increasing the initial concentrations. The following equation is used to calculate metal ion adsorption at certain time, t (qt mg/g):
(3)qt=c0−ct×νm.Figure 12
Effect of contact time on (a) lead (II), (b) Cr (III), and (c) Cd (II) adsorption at different initial feed concentration; solution: pH 5; and temperature: 25°C.
(a)(b)(c)This can be illustrated by the ratio between available surface and initial metal ion concentration. On higher concentration, this ratio was low and it increased with the lower concentration and the initial concentration also affects the removal of heavy metals [48].


### 2.14. Effect of Adsorbent Dosage

The efficiency of the amidoxime chelating resin dosage was investigated on the basis of its initial concentrations. Adsorption of lead (II), Cr (III), and Cd (II) was studied with different dosages of resin and 50 mg/l as the initial concentration of metals at 25°C andpH=5. According to Figure 13, when the resin dosage was increased from 0.05 g/l to 2 g/l, the percentage of removal from 61.1% to 87.84% for lead (II), from 49.94 to 71.50% for chromium (III), and from 50.26 to 67.48 for cadmium (II) was observed. This increase in the removal percentage can be attributed to the availability of huge surface area and number of active sites on account of increase in the dosage of resin at constant concentration of metal ions.Figure 13
Effect of adsorbent dosage on adsorption of lead (II), Cr (III), and Cd (II); initial concentrations: 50 mg/L; time: 60 min; solution: pH 5; and temperature: 25°C.


### 2.15. Adsorption Kinetics

To investigate the adsorption mechanism and reaction pathways, some adsorption kinetic studies were conducted. Various kinetic models were applied to analyse the adsorption process of lead (II), Cr (III), and Cd (II) onto chelating resin. These models include pseudo-first-order, pseudo-second-order, and intraparticle diffusion. Models with high correlation coefficients (R2) may describe the adsorption of metal onto chelating resin.


#### 2.15.1. The Pseudo-First-Order Model

The pseudo-first-order kinetic model illustrates the adsorption mechanisms in solid-liquid systems, which is generally expressed as(4)Logqe−qt=Logqe−k1t2.303,where k1 is the rate constant of pseudo-first-order adsorption (per minute) and qt and qe are the quantities of metal ions adsorbed (milligrams per gram) at time t and equilibrium, respectively [39, 49]. The plots of log (qe−qt) versus t demonstrated in Figure 14 give the value rate constant k1 and adsorption density qe from the slope and intercept, respectively. Bad linearity was obtained for this model, and it was clear from the values of correlation coefficients (R2) which was low for different concentrations. Moreover, no agreement was observed between the experimentally observed equilibrium adsorption (qe, exp) and that derived theoretically (qe, cal), which means that the adsorption of metal ions onto chelating resin kinetic data was not compatible with the pseudo-first-order kinetic model.Figure 14
Lagergren first-order plot for adsorption of (a) Pb (II), (b) Cr (III), and (c) Cd (II) on amidoxime chelating resin for different initial feed concentrations at pH 5 and temperature at 25°C.
(a)(b)(c)


#### 2.15.2. The Pseudo-Second-Order Equation

The pseudo-second-order adsorption kinetic rate is expressed as(5)dqtdt=k2qe−qt2,where k2 is the rate constant of the pseudo-second-order sorption (g/mg·min), qe and qt are the sorption capacities at equilibrium and time t (mg/g), respectively. For the boundary conditions t=0 to t=t and qt=0 to qt=qt, the integrated form of Equation (5) will be as
(6)1qe−qt=1qe+k2t.Equation (6) can be expressed as
(7)tqt=1k2qe2+tqe.The initial adsorption rate,h (milligrams per gram per minute), is given as
(8)h=k2qe2.Equation (7) also can be written as
(9)tqt=1h+tqe.The plots oft/qt versus t from Equation (9) at different concentrations of lead (II), Cr (III), and Cd (II) are shown in Figure 15. From slope and intercept, adsorption parameters qe (Cal.) and k2 were calculated, respectively (Table 1). The high linearity of the plots was indicated by values of correlation coefficients (R2) (≥0.99), which means that the adsorption kinetics between amidoxime chelating resin and heavy metals can be described using a pseudo-second-order adsorption kinetic model. Moreover, the good agreement between (qe, Cal.) and (qe, Exp.) gives evidence for the compatibility of the adsorption data. This shows that the adsorption of heavy metals onto amidoxime chelating resin occurs through the chemical interaction between the adsorbent and adsorbate [50–52].Figure 15
Pseudo-second-order kinetic plot for adsorption of (a) Pb (II), (b) Cr (III), and (c) Cd (II) on amidoxime chelating resin for different initial feed concentrations at pH 5 and temperature at 25°C.
(a)(b)(c)Table 1
Kinetic constant parameters obtained for heavy metal adsorption on polyamidoxime resin.
MetalPseudo-first orderPseudo-second orderIntraparticle diffusion modelCi (mg/L)qe exp (mg/g)K1 (10-3) (min-1)qe cal (mg/g)R2K2 (10-2) (g/mg·min)qe cal (mg/g)h (g/min)R2Kid (mg/g·min)C (mg/g)R2Lead (II)7022.4041.22518.80.9760.3017.950.970.9962.2625.3970.9925023.9032.7226.010.9760.4027.032.910.9921.73310.5210.9903013.8153.19363.090.9810.2427.851.820.9901.5672.1120.979Chromium (III)7019.5862.871659.70.8800.0832.790.8980.9742.9291.6310.9655016.3933.85111.880.9940.9317.642.890.9950.8569.6450.9863010.7229.4843.580.9740.3114.470.640.9701.2591.080.988Cadmium (II)7016.2445.14832.60.9370.39936.490.530.9472.7453.9990.9835015.5453.1919.130.9211.116.863.140.9980.8089.540.977308.9251.8272.310.9240.50311.480.660.9860.9771.6620.967


#### 2.15.3. The Intraparticle Diffusion Model

Adsorption mechanism and intraparticle diffusion rate determined steps of lead (II). Cr (III) and Cd (II) onto chelating resin were identified using the Weber and Morris model. The rate constant for intraparticle (kid) can be expressed as
(10)qt=kidt1/2+C.Figure16 shows the plots of qt versus t1/2. It is clear that all lines for different concentrations do not pass through the point of origin indicating the difficulty of predicting the mechanism of the overall process, and it seems to be very complex [46, 53].Figure 16
Intraparticle diffusion kinetic plot for adsorption of (a) Pb (II), (b) Cr (III), and (c) Cd (II) on amidoxime chelating resin for different initial feed concentrations at pH 5 and temperature at 25°C.
(a)(b)(c)


### 2.16. Adsorption Isotherm Models

The adsorption efficiency of polyamidoxime chelating resin towards heavy metals was tested using some isotherm models. It describes the partition of adsorbate molecules between liquid and solid phases at equilibrium. Langmuir and Freundlich adsorption isotherm models were used to determine the adsorption capacity of amidoxime chelating resin towards lead (II), Cr (III), and Cd (II).


#### 2.16.1. The Langmuir Isotherm Model

The Langmuir model assumes that the monolayer adsorption process takes place between the adsorbate and adsorbent, and the surface is homogenous with a finite number of active sites when sites are filled with adsorbate molecules. There is no chance of further adsorption on this site, and the saturation point is accomplished [54]. The linear equation is expressed as
(11)Ceqe=1KLqm+Ceqm,where Ce is the equilibrium concentration (mg/l) of metals in solution; qe is the amount of metal ions adsorbed (mg/g) at equilibrium; KL is the Langmuir equilibrium constant (l/mg), and it is related to the affinity of adsorption sites; and qm gives the maximum theoretical monolayer adsorption capacity (mg/g). The values of qm and KL (Table 2) were obtained from the slope and intercept, respectively, of plots of Ce/qe versus Ce, which are shown in Figure 17. The linearity and high values of correlation coefficients (R2) indicate that the Langmuir model describes the adsorption process very well, confirming the formation of monolayer. Weber and Chakravorti [55] defined the separation factor (RL) as a characteristic dimensionless equilibrium parameter for the Langmuir model, and it is expressed as
(12)RL=11+KLCo.Table 2
Langmuir and Freundlich isotherm constants for lead (II), Cr (III), and Cd (II) adsorption on amidoxime chelating resin.
CompoundsT (k)Langmuir isotherm constantsFreundlich isotherm constantsqm (mg/g)KL (L/mg)RLR21/nnKFR2Lead (II)298.1643.869.120.0020.9990.0423.1548.620.8638Chromium (III)298.1642.745.320.0040.9990.0615.4349.740.9701Cadmium (II)298.1632.471.540.0120.9930.1010.0448.070.7647Figure 17
Langmuir adsorption isotherms for adsorption of (a) Pb (II), (b) Cr (III), and (c) Cd (II) on amidoxime chelating resin, pH 5, and temperature at 25°C.
(a)(b)(c)The values ofRL for each initial concentration was less than unity and greater than zero indicating the favourable adsorption of lead (II), Cr (III), and Cd (II) on polyamidoxime chelating resin [53].


#### 2.16.2. The Freundlich Isotherm Model

The Freundlich model is always used to describe the adsorption on heterogeneous surface of adsorbent [56]. Different initial concentrations of heavy metals were used with fixed dosage of amidoxime resin to obtain the equilibrium data. The Freundlich isotherm model is expressed as follows:
(13)lnqe=lnkf+1nlnCe,where Kf (mg/g) and n (g/L) are the Freundlich adsorption constants. The plots of lnqe against lnCe shown in Figure 18 give straight lines. From the slope and intercept of those lines, the values of n and Kf can be calculated. Bad linearity and low values of correlation coefficient (R2) indicate disagreement between equilibrium data and this model. Values of n more than the unit mean favourable adsorption condition, and lead (II), Cr (III), and Cd (II) are favourably adsorbed via amidoxime resin [53].Figure 18
Freundlich adsorption isotherms for adsorption of (a) Pb (II), (b) Cr (III), and (c) Cd (II) on amidoxime chelating resin, pH 5, and temperature at 25°C.
(a)(b)(c)


## 2.1. Materials and Reagents

A nonwoven polyethylene fabric was used as a trunk polymer for graft polymerization; the material was obtained from Kurashiki MFG Co. Monomer acrylonitrile (BDH, England) was used for grafting onto a trunk polymer. Sodium carbonate, methanol, acetone, and sulphuric acid were obtained from Merck, Germany, and hydroxyl amine hydrochloride was obtained from Sigma-Aldrich, USA. Cadmium (II), lead (II) acetate trihydrate (Merck, Germany), and chromium (III) (Techno Pharmchem, India) were used for a metal adsorption study. Date palm fiber was obtained from a local market, and the size of the fiber was less than 200μm. The fiber was washed two times with hot distilled water and acetone. The acetone was removed by heating the fiber in an oven at 60°C.


## 2.2. FTIR Spectroscopy

Infrared (IR) spectra of the DPW, grafted DPW, and the poly (amidoxime) ion-exchange resin samples were recorded on a Fourier transform–IR spectrometer (Perkin–Elmer 1725, Norwalk, CT) using a KBr disk pellet.


## 2.3. Scanning Electron Microscopy (SEM)

The SEM photographs of the fiber surfaces of grafted PAN onto DPW and ungrafted DPW fiber were captured using a scanning electron microscope model SEM JEOL 6400 (JEOL, Peabody, MA).


## 2.4. Preparation of a Chelating Resin Containing Polyamidoxime Groups

Hydroxylamine hydrochloride (NH2OH.HCl) solution was prepared by dissolving 20 g (0.288 mol) of hydroxylamine hydrochloride in 300 ml of a methanolic aqueous solution (methanol/waterratio=80). The hydrochloride content of NH2OH.HCl was neutralized by the addition of NaOH solution, and the precipitated NaCl was removed by filtration. The grafted product was placed in a two-necked flask equipped with a condenser; the flask was placed in a thermostatic water bath, and the hydroxylamine solution was poured in it. The mixture was allowed to react at 70°C with continuous stirring for 180 min. After completion of the reaction, the resin was filtered and washed several times with the methanolic solution. The resin was neutralized by treating it with 0.1 M HCl solution for 15 min; afterwards, it was again filtered, washed several times with the methanolic solution, and then dried in an oven at a constant weight at 60°C.


## 2.5. Sorption of Lead Cadmium and Chromium Ions Using the Batch Technique

The lead, cadmium, and chromium ion adsorption capacities of the resin were measured over the pH range of 1–6. Thus, ca. 0.1 g of dried resin was placed in a series of 100 ml polyethylene bottles and equilibrated with 20 ml of distilled water. After adding 20 ml of 0.1 M sodium acetate buffer solution in each bottle, 10 ml of 0.1 M lead-ions solution was added. The resulting mixture was shaken for 24 h by a rotary shaker, and afterwards, 5 ml of the supernatant was collected for the determination of metal-ions. An AGBC-903 atomic absorption spectrometer was used to determine the initial and final amounts of metal ions present in the solutions.Blank experiments were performed, and the same experimental procedure was conducted for checking the adsorption level by the membrane filters and glass flasks for all adsorption tests. The kinetic samples were conducted in 1000 ml batch reactors at 20.0 in deionized water. The flasks were vigorously and magnetically stirred for 1.5 h for hydrating the beet pulp to naturally maintain the pH at 5.5.


## 2.6. Graft Copolymerization

To prepare the fiber/PAN copolymer, 1.00 g DPW fiber was placed in 250 ml three-necked flasks equipped with a stirrer and condenser and immersed into a thermostatic water bath. The DPW suspension was obtained by adding 100 ml distilled water and 0.1 g ferrous ammonium sulphate with continuous stirring. Nitrogen purged through the DPW fiber slurry to remove oxygen during the reaction. After 30 min, the required volume of 2.0 M H2O2 was added and the mixture was mixed for 5 min; afterwards, the required amounts of monomer (AN) were added into the mixture. The reaction mixture was stirred under nitrogen at the chosen temperature and for the predetermined reaction period. Immediately after the reaction, the reaction flask was cooled by placing it under running tap water, and the product was filtered. The crude product was washed thoroughly with distilled water and oven-dried at 60°C at a constant weight.


## 2.7. Removal of Polyacrylonitrile and Determination of Graft Level

The crude product was purified withN,N-dimethylformamide using a Soxhlet extractor for 48 h to remove the polyacrylonitrile (PAN). The pure grafted copolymers were then dried at 65°C at a constant weight. The following formula determined the percentage of grafting (Pg):
(1)Pg=W2−W1W1×100,where W1 is the weight of the original DPW fibers in grams and W2 is the weight of the grafted product after copolymerization and extraction [33].


## 2.8. Graft Copolymerization

Date palm wood fiber (DPWF) was treated with a mixed solution of hydrogen peroxide and ferrous ammonium sulfate to initiate a free radical in the backbone of the fiber and provide cellulose macroradical. Graft copolymerization occurred after adding acrylonitrile (AN) monomer to the mixture during which the cellulose macroradical broke the double bond in AN and a covalent bond between monomer and cellulose was formed, the chain initiated with continues creation of free radical on the AN. Chain grafting onto the cellulose was possible by adding AN monomer subsequently. The reaction was ultimately terminated either by the formation of a copolymer on account of the reaction of two macroradical or formation of poly(methacrylate) by the reaction of two monomer radicals. Figure1 explains the whole process [34, 35].Figure 1
Mechanism of graft copolymerization of acrylonitrile onto DPWF.


## 2.9. Optimization of Grafted Polymerization Parameters

Effects of various parameters on the yield of grafted copolymerization were studied. These parameters included temperature, reaction time, monomer volume, cocatalyst amount, and concentration of initiator. All these parameters were studied separately to investigate the best conditions and to obtain the best yield.


### 2.9.1. Effect of Temperature

A wide range of temperatures was used to obtain the best yield of the grafted copolymer. Figure2 illustrates the effect of temperature that increase in temperature from 30°C up to 75°C increases the % yield of grafting. This increase could be attributed to the increase of monomer diffusion into the active sites on the backbone of the substrate. If temperature goes above 75°C, the monomer starts to evaporate, and hydrogen peroxide decomposes. This condition leads to creation of a huge number of free radicals, the yield of a homopolymer will increase, and % of the grafted copolymer in pg will decrease [36, 37].Figure 2
Effect of reaction temperature on the % of grafting in pg. Reaction time: 60 min, AN: 8 ml, H2O2: 0.03 M, Fe+2: 0.3 mmol, and (∆): % of grafting.


### 2.9.2. Effect of the Concentration of Initiator

The yield of grafted polymer is clearly affected by the concentration of the initiator. As shown in Figure3, the % of grafting increased with the increase in the concentration of the hydrogen peroxide as it increases the production of free radicals in the active sites of the fiber. At 0.03 M concentration, 81% grafting was obtained. However, the grafting percentage decreased with further increase in the percentage of hydrogen peroxide because of the reaction between cellulose radicals before addition of monomers, and this reaction is the termination step. Moreover, at higher concentrations, the yield of homopolymer increases [34].Figure 3
Effect of the amount of initiator H2O2 on the % of grafting. Reaction time: 60 min, AN: 8 ml, temperature: 75°C, Fe+2: 0.3 mmol, and (∆): % of grafting.


### 2.9.3. Effect of the Amount of Monomer

The percentage of grafting increased with the increasing volume of the (AN) monomer on account of the availability of a large number of monomer molecules reaching the active sites in the backbone of the fiber. However, as shown in Figure4, increase in volume over 8 ml decreased the percentage of grafting on account of the increased possibility of homopolymerization [37, 38].Figure 4
Effect of the amount of monomer (AN) on the % of grafting. Reaction time: 60 min, H2O2: 0.03 M, temperature: 75°C, Fe+2: 0.3 mmol, and (∆): % of grafting.


### 2.9.4. Effect of Reaction Period

The percentage of grafting was found directly proportional to the increase in the reaction time, and it increases the time available to all monomer molecules to reach the active sites on the backbone; however, the maximum grafting yield was obtained with the reaction time of 60 minutes. Afterwards, all active sites were covered, and the concentration of all reaction species decreased and this accounted for the low yield of grafting which almost remains constant with increasing time [39]. This explanation is in line with the results shown in Figure 5.Figure 5
Effect of reaction period on the % of grafting and efficiency. AN: 8 ml, H2O2: 0.03 M, temperature: 75°C, Fe+2: 0.3 mmol, and (∆): % of grafting.


### 2.9.5. Effect of the Amount of Catalyst

Small amount of ammonium ferrous sulphate [(NH4)2SO4·FeSO4·6H2O] was found to be enough for the best yield of a product (Figure 6), where 0.306 mmol of catalyst gave 81% of grafting product. This yield decreased with the increase in the amount of the catalyst on account of a large number of radicals produced by the decomposition of hydrogen per oxide. The reaction finally terminates due to the reaction between radicals and yield will decrease [33, 40].Figure 6
Effect of the amount of catalyst Fe+2on the % of grafting. AN: 8 ml, H2O2: 0.03 M, temperature: 75°C, time: 60 min, and (∆): % of grafting.


## 2.9.1. Effect of Temperature

A wide range of temperatures was used to obtain the best yield of the grafted copolymer. Figure2 illustrates the effect of temperature that increase in temperature from 30°C up to 75°C increases the % yield of grafting. This increase could be attributed to the increase of monomer diffusion into the active sites on the backbone of the substrate. If temperature goes above 75°C, the monomer starts to evaporate, and hydrogen peroxide decomposes. This condition leads to creation of a huge number of free radicals, the yield of a homopolymer will increase, and % of the grafted copolymer in pg will decrease [36, 37].Figure 2
Effect of reaction temperature on the % of grafting in pg. Reaction time: 60 min, AN: 8 ml, H2O2: 0.03 M, Fe+2: 0.3 mmol, and (∆): % of grafting.


## 2.9.2. Effect of the Concentration of Initiator

The yield of grafted polymer is clearly affected by the concentration of the initiator. As shown in Figure3, the % of grafting increased with the increase in the concentration of the hydrogen peroxide as it increases the production of free radicals in the active sites of the fiber. At 0.03 M concentration, 81% grafting was obtained. However, the grafting percentage decreased with further increase in the percentage of hydrogen peroxide because of the reaction between cellulose radicals before addition of monomers, and this reaction is the termination step. Moreover, at higher concentrations, the yield of homopolymer increases [34].Figure 3
Effect of the amount of initiator H2O2 on the % of grafting. Reaction time: 60 min, AN: 8 ml, temperature: 75°C, Fe+2: 0.3 mmol, and (∆): % of grafting.


## 2.9.3. Effect of the Amount of Monomer

The percentage of grafting increased with the increasing volume of the (AN) monomer on account of the availability of a large number of monomer molecules reaching the active sites in the backbone of the fiber. However, as shown in Figure4, increase in volume over 8 ml decreased the percentage of grafting on account of the increased possibility of homopolymerization [37, 38].Figure 4
Effect of the amount of monomer (AN) on the % of grafting. Reaction time: 60 min, H2O2: 0.03 M, temperature: 75°C, Fe+2: 0.3 mmol, and (∆): % of grafting.


## 2.9.4. Effect of Reaction Period

The percentage of grafting was found directly proportional to the increase in the reaction time, and it increases the time available to all monomer molecules to reach the active sites on the backbone; however, the maximum grafting yield was obtained with the reaction time of 60 minutes. Afterwards, all active sites were covered, and the concentration of all reaction species decreased and this accounted for the low yield of grafting which almost remains constant with increasing time [39]. This explanation is in line with the results shown in Figure 5.Figure 5
Effect of reaction period on the % of grafting and efficiency. AN: 8 ml, H2O2: 0.03 M, temperature: 75°C, Fe+2: 0.3 mmol, and (∆): % of grafting.


## 2.9.5. Effect of the Amount of Catalyst

Small amount of ammonium ferrous sulphate [(NH4)2SO4·FeSO4·6H2O] was found to be enough for the best yield of a product (Figure 6), where 0.306 mmol of catalyst gave 81% of grafting product. This yield decreased with the increase in the amount of the catalyst on account of a large number of radicals produced by the decomposition of hydrogen per oxide. The reaction finally terminates due to the reaction between radicals and yield will decrease [33, 40].Figure 6
Effect of the amount of catalyst Fe+2on the % of grafting. AN: 8 ml, H2O2: 0.03 M, temperature: 75°C, time: 60 min, and (∆): % of grafting.


## 2.10. Preparation of Polyamidoxime Resin

The AN-DPWF grafted copolymer containing nitrile group was treated with hydroxylamine hydrochloride at pH 11 to change the nitrile group into amidoxime. This reaction was performed for 3 hours at 75°C, and the ratio between grafted copolymer and hydroxylamine in methanolic solution was 1 : 1. The mechanism of this conversion is shown in Figure7.Figure 7
Reaction mechanism of preparation of polyamidoxime resin.


## 2.11. Characterization of AN-DPWF Grafted Copolymer and Resin

FT-IR spectra were obtained for DPWF, grafted copolymer, and amidoxime resin to confirm the completion of polymerization and conversion of grafted copolymer into the chelating resin. In Figure8, the same characteristic adsorption bands for DPWF, such as broad absorption band between 3000 and 3500 cm-1 were assigned to O-H stretching vibration and bands that appeared at 2900 and 1020 cm-1 for C-H stretching and bending modes, respectively. The characteristic adsorption at 2240 cm-1 for C≡N stretching modes confirms the presence of acrylonitrile onto the backbone of DPWF and grafting reaction completely [41].Figure 8
FTIR DPWF fiber (─), AN-g-DPWF fiber (- -), and resin containing amidoxime groups (···).This band disappeared completely after conversion to amidoxime resin, and new adsorption band formed at 1650 cm-1 associated with C=N vibration of the amidoxime group. Another adsorption band observed at 941 cm–1 may be assigned to the N–O bond of the oxime group [42]. Scanning electron microscope (SEM) images were taken for DPWF before and after polymerization to investigate the changes in the morphology of the fiber surface. Figures 9 and 10 show the surface of the fiber before and after grafted polymerization, respectively. As can be seen in Figure 10, all pours on the DPWF surface were covered with polyacrylonitrile (PAN) via the chemical bond and this covering yielded a homogeneous surface with less porosity.Figure 9
Scanning electron micrographs of DPWF before grafting, SEM MAG (1.36 KX).Figure 10
Scanning electron micrographs of DPWF after grafting, SEM MAG (1.47 KX).


## 2.12. Effect of Initial pH

The pH solution is a substantial parameter used in the study of the removal of heavy metal ions from aqueous solution or water on account of many reasons such as its effects on the concentration of counter ions placed in adsorbent functional clusters, the level of ionization of the adsorbate during the reaction, and the solubility of metal ions. Batch technique was conducted to find out the optimum pH level required for the removal of heavy metals using amidoxime chelating resin. The concentration of the counter ions on the resin, ability of ionization, and solubility of adsorbates depend on pH [43]. A wide range of pH (1.0 to 6.0) was investigated to get the optimum pH for a fixed concentration of metals and dosage of resin at 25°C. The adsorption of lead (II), Cr (III), and Cd (II) was maximum at the pH=5.0 as shown in Figure 11. At low pH (<3.0), the competition between H+ ions for the resin sites increased and the resin’s chelating ability was greatly reduced. At pH 5, the competition of H+ ions for the resin sites decreases and the chelating ability of the metal ion increases [44]. Equation (2) is used to calculate the percentage of the removal of metal ions using this resin [39, 45, 46].
(2)%ofremoval=C0−CeC0×100.Figure 11
Effect of pH on the adsorption of (Pb+2), (Cr+3), and (Cd+2) ions; dosage of chelating resin: 1 g; ion concentration: 50 mg/L; time: 60 min; and temperature: 25°C.


## 2.13. Effect of Contact Time and Initial Concentration

The contact time is one of the important parameters to study as it affects the adsorption of heavy metals onto chelating resin. From Figure12, it can be observed that the adsorption of heavy metals increases with the increase in the contact time. Also, the adsorption was fast in the beginning until it reaches equilibrium at 35 min, and afterwards, the value of qt (mg/g) remains constant. This can be attributed to the availability of active sites on the surface of chelating resin in the beginning of reaction [47]. Initial concentration of metals under study: lead (II), Cr (III), and Cd (II), influenced the removal of these metals. The amount of metal ions, qt (milligrams per gram) adsorbed, is calculated by increasing the initial concentrations. The following equation is used to calculate metal ion adsorption at certain time, t (qt mg/g):
(3)qt=c0−ct×νm.Figure 12
Effect of contact time on (a) lead (II), (b) Cr (III), and (c) Cd (II) adsorption at different initial feed concentration; solution: pH 5; and temperature: 25°C.
(a)(b)(c)This can be illustrated by the ratio between available surface and initial metal ion concentration. On higher concentration, this ratio was low and it increased with the lower concentration and the initial concentration also affects the removal of heavy metals [48].


## 2.14. Effect of Adsorbent Dosage

The efficiency of the amidoxime chelating resin dosage was investigated on the basis of its initial concentrations. Adsorption of lead (II), Cr (III), and Cd (II) was studied with different dosages of resin and 50 mg/l as the initial concentration of metals at 25°C andpH=5. According to Figure 13, when the resin dosage was increased from 0.05 g/l to 2 g/l, the percentage of removal from 61.1% to 87.84% for lead (II), from 49.94 to 71.50% for chromium (III), and from 50.26 to 67.48 for cadmium (II) was observed. This increase in the removal percentage can be attributed to the availability of huge surface area and number of active sites on account of increase in the dosage of resin at constant concentration of metal ions.Figure 13
Effect of adsorbent dosage on adsorption of lead (II), Cr (III), and Cd (II); initial concentrations: 50 mg/L; time: 60 min; solution: pH 5; and temperature: 25°C.


## 2.15. Adsorption Kinetics

To investigate the adsorption mechanism and reaction pathways, some adsorption kinetic studies were conducted. Various kinetic models were applied to analyse the adsorption process of lead (II), Cr (III), and Cd (II) onto chelating resin. These models include pseudo-first-order, pseudo-second-order, and intraparticle diffusion. Models with high correlation coefficients (R2) may describe the adsorption of metal onto chelating resin.


### 2.15.1. The Pseudo-First-Order Model

The pseudo-first-order kinetic model illustrates the adsorption mechanisms in solid-liquid systems, which is generally expressed as(4)Logqe−qt=Logqe−k1t2.303,where k1 is the rate constant of pseudo-first-order adsorption (per minute) and qt and qe are the quantities of metal ions adsorbed (milligrams per gram) at time t and equilibrium, respectively [39, 49]. The plots of log (qe−qt) versus t demonstrated in Figure 14 give the value rate constant k1 and adsorption density qe from the slope and intercept, respectively. Bad linearity was obtained for this model, and it was clear from the values of correlation coefficients (R2) which was low for different concentrations. Moreover, no agreement was observed between the experimentally observed equilibrium adsorption (qe, exp) and that derived theoretically (qe, cal), which means that the adsorption of metal ions onto chelating resin kinetic data was not compatible with the pseudo-first-order kinetic model.Figure 14
Lagergren first-order plot for adsorption of (a) Pb (II), (b) Cr (III), and (c) Cd (II) on amidoxime chelating resin for different initial feed concentrations at pH 5 and temperature at 25°C.
(a)(b)(c)


### 2.15.2. The Pseudo-Second-Order Equation

The pseudo-second-order adsorption kinetic rate is expressed as(5)dqtdt=k2qe−qt2,where k2 is the rate constant of the pseudo-second-order sorption (g/mg·min), qe and qt are the sorption capacities at equilibrium and time t (mg/g), respectively. For the boundary conditions t=0 to t=t and qt=0 to qt=qt, the integrated form of Equation (5) will be as
(6)1qe−qt=1qe+k2t.Equation (6) can be expressed as
(7)tqt=1k2qe2+tqe.The initial adsorption rate,h (milligrams per gram per minute), is given as
(8)h=k2qe2.Equation (7) also can be written as
(9)tqt=1h+tqe.The plots oft/qt versus t from Equation (9) at different concentrations of lead (II), Cr (III), and Cd (II) are shown in Figure 15. From slope and intercept, adsorption parameters qe (Cal.) and k2 were calculated, respectively (Table 1). The high linearity of the plots was indicated by values of correlation coefficients (R2) (≥0.99), which means that the adsorption kinetics between amidoxime chelating resin and heavy metals can be described using a pseudo-second-order adsorption kinetic model. Moreover, the good agreement between (qe, Cal.) and (qe, Exp.) gives evidence for the compatibility of the adsorption data. This shows that the adsorption of heavy metals onto amidoxime chelating resin occurs through the chemical interaction between the adsorbent and adsorbate [50–52].Figure 15
Pseudo-second-order kinetic plot for adsorption of (a) Pb (II), (b) Cr (III), and (c) Cd (II) on amidoxime chelating resin for different initial feed concentrations at pH 5 and temperature at 25°C.
(a)(b)(c)Table 1
Kinetic constant parameters obtained for heavy metal adsorption on polyamidoxime resin.
MetalPseudo-first orderPseudo-second orderIntraparticle diffusion modelCi (mg/L)qe exp (mg/g)K1 (10-3) (min-1)qe cal (mg/g)R2K2 (10-2) (g/mg·min)qe cal (mg/g)h (g/min)R2Kid (mg/g·min)C (mg/g)R2Lead (II)7022.4041.22518.80.9760.3017.950.970.9962.2625.3970.9925023.9032.7226.010.9760.4027.032.910.9921.73310.5210.9903013.8153.19363.090.9810.2427.851.820.9901.5672.1120.979Chromium (III)7019.5862.871659.70.8800.0832.790.8980.9742.9291.6310.9655016.3933.85111.880.9940.9317.642.890.9950.8569.6450.9863010.7229.4843.580.9740.3114.470.640.9701.2591.080.988Cadmium (II)7016.2445.14832.60.9370.39936.490.530.9472.7453.9990.9835015.5453.1919.130.9211.116.863.140.9980.8089.540.977308.9251.8272.310.9240.50311.480.660.9860.9771.6620.967


### 2.15.3. The Intraparticle Diffusion Model

Adsorption mechanism and intraparticle diffusion rate determined steps of lead (II). Cr (III) and Cd (II) onto chelating resin were identified using the Weber and Morris model. The rate constant for intraparticle (kid) can be expressed as
(10)qt=kidt1/2+C.Figure16 shows the plots of qt versus t1/2. It is clear that all lines for different concentrations do not pass through the point of origin indicating the difficulty of predicting the mechanism of the overall process, and it seems to be very complex [46, 53].Figure 16
Intraparticle diffusion kinetic plot for adsorption of (a) Pb (II), (b) Cr (III), and (c) Cd (II) on amidoxime chelating resin for different initial feed concentrations at pH 5 and temperature at 25°C.
(a)(b)(c)


## 2.15.1. The Pseudo-First-Order Model

The pseudo-first-order kinetic model illustrates the adsorption mechanisms in solid-liquid systems, which is generally expressed as(4)Logqe−qt=Logqe−k1t2.303,where k1 is the rate constant of pseudo-first-order adsorption (per minute) and qt and qe are the quantities of metal ions adsorbed (milligrams per gram) at time t and equilibrium, respectively [39, 49]. The plots of log (qe−qt) versus t demonstrated in Figure 14 give the value rate constant k1 and adsorption density qe from the slope and intercept, respectively. Bad linearity was obtained for this model, and it was clear from the values of correlation coefficients (R2) which was low for different concentrations. Moreover, no agreement was observed between the experimentally observed equilibrium adsorption (qe, exp) and that derived theoretically (qe, cal), which means that the adsorption of metal ions onto chelating resin kinetic data was not compatible with the pseudo-first-order kinetic model.Figure 14
Lagergren first-order plot for adsorption of (a) Pb (II), (b) Cr (III), and (c) Cd (II) on amidoxime chelating resin for different initial feed concentrations at pH 5 and temperature at 25°C.
(a)(b)(c)


## 2.15.2. The Pseudo-Second-Order Equation

The pseudo-second-order adsorption kinetic rate is expressed as(5)dqtdt=k2qe−qt2,where k2 is the rate constant of the pseudo-second-order sorption (g/mg·min), qe and qt are the sorption capacities at equilibrium and time t (mg/g), respectively. For the boundary conditions t=0 to t=t and qt=0 to qt=qt, the integrated form of Equation (5) will be as
(6)1qe−qt=1qe+k2t.Equation (6) can be expressed as
(7)tqt=1k2qe2+tqe.The initial adsorption rate,h (milligrams per gram per minute), is given as
(8)h=k2qe2.Equation (7) also can be written as
(9)tqt=1h+tqe.The plots oft/qt versus t from Equation (9) at different concentrations of lead (II), Cr (III), and Cd (II) are shown in Figure 15. From slope and intercept, adsorption parameters qe (Cal.) and k2 were calculated, respectively (Table 1). The high linearity of the plots was indicated by values of correlation coefficients (R2) (≥0.99), which means that the adsorption kinetics between amidoxime chelating resin and heavy metals can be described using a pseudo-second-order adsorption kinetic model. Moreover, the good agreement between (qe, Cal.) and (qe, Exp.) gives evidence for the compatibility of the adsorption data. This shows that the adsorption of heavy metals onto amidoxime chelating resin occurs through the chemical interaction between the adsorbent and adsorbate [50–52].Figure 15
Pseudo-second-order kinetic plot for adsorption of (a) Pb (II), (b) Cr (III), and (c) Cd (II) on amidoxime chelating resin for different initial feed concentrations at pH 5 and temperature at 25°C.
(a)(b)(c)Table 1
Kinetic constant parameters obtained for heavy metal adsorption on polyamidoxime resin.
MetalPseudo-first orderPseudo-second orderIntraparticle diffusion modelCi (mg/L)qe exp (mg/g)K1 (10-3) (min-1)qe cal (mg/g)R2K2 (10-2) (g/mg·min)qe cal (mg/g)h (g/min)R2Kid (mg/g·min)C (mg/g)R2Lead (II)7022.4041.22518.80.9760.3017.950.970.9962.2625.3970.9925023.9032.7226.010.9760.4027.032.910.9921.73310.5210.9903013.8153.19363.090.9810.2427.851.820.9901.5672.1120.979Chromium (III)7019.5862.871659.70.8800.0832.790.8980.9742.9291.6310.9655016.3933.85111.880.9940.9317.642.890.9950.8569.6450.9863010.7229.4843.580.9740.3114.470.640.9701.2591.080.988Cadmium (II)7016.2445.14832.60.9370.39936.490.530.9472.7453.9990.9835015.5453.1919.130.9211.116.863.140.9980.8089.540.977308.9251.8272.310.9240.50311.480.660.9860.9771.6620.967


## 2.15.3. The Intraparticle Diffusion Model

Adsorption mechanism and intraparticle diffusion rate determined steps of lead (II). Cr (III) and Cd (II) onto chelating resin were identified using the Weber and Morris model. The rate constant for intraparticle (kid) can be expressed as
(10)qt=kidt1/2+C.Figure16 shows the plots of qt versus t1/2. It is clear that all lines for different concentrations do not pass through the point of origin indicating the difficulty of predicting the mechanism of the overall process, and it seems to be very complex [46, 53].Figure 16
Intraparticle diffusion kinetic plot for adsorption of (a) Pb (II), (b) Cr (III), and (c) Cd (II) on amidoxime chelating resin for different initial feed concentrations at pH 5 and temperature at 25°C.
(a)(b)(c)


## 2.16. Adsorption Isotherm Models

The adsorption efficiency of polyamidoxime chelating resin towards heavy metals was tested using some isotherm models. It describes the partition of adsorbate molecules between liquid and solid phases at equilibrium. Langmuir and Freundlich adsorption isotherm models were used to determine the adsorption capacity of amidoxime chelating resin towards lead (II), Cr (III), and Cd (II).


### 2.16.1. The Langmuir Isotherm Model

The Langmuir model assumes that the monolayer adsorption process takes place between the adsorbate and adsorbent, and the surface is homogenous with a finite number of active sites when sites are filled with adsorbate molecules. There is no chance of further adsorption on this site, and the saturation point is accomplished [54]. The linear equation is expressed as
(11)Ceqe=1KLqm+Ceqm,where Ce is the equilibrium concentration (mg/l) of metals in solution; qe is the amount of metal ions adsorbed (mg/g) at equilibrium; KL is the Langmuir equilibrium constant (l/mg), and it is related to the affinity of adsorption sites; and qm gives the maximum theoretical monolayer adsorption capacity (mg/g). The values of qm and KL (Table 2) were obtained from the slope and intercept, respectively, of plots of Ce/qe versus Ce, which are shown in Figure 17. The linearity and high values of correlation coefficients (R2) indicate that the Langmuir model describes the adsorption process very well, confirming the formation of monolayer. Weber and Chakravorti [55] defined the separation factor (RL) as a characteristic dimensionless equilibrium parameter for the Langmuir model, and it is expressed as
(12)RL=11+KLCo.Table 2
Langmuir and Freundlich isotherm constants for lead (II), Cr (III), and Cd (II) adsorption on amidoxime chelating resin.
CompoundsT (k)Langmuir isotherm constantsFreundlich isotherm constantsqm (mg/g)KL (L/mg)RLR21/nnKFR2Lead (II)298.1643.869.120.0020.9990.0423.1548.620.8638Chromium (III)298.1642.745.320.0040.9990.0615.4349.740.9701Cadmium (II)298.1632.471.540.0120.9930.1010.0448.070.7647Figure 17
Langmuir adsorption isotherms for adsorption of (a) Pb (II), (b) Cr (III), and (c) Cd (II) on amidoxime chelating resin, pH 5, and temperature at 25°C.
(a)(b)(c)The values ofRL for each initial concentration was less than unity and greater than zero indicating the favourable adsorption of lead (II), Cr (III), and Cd (II) on polyamidoxime chelating resin [53].


### 2.16.2. The Freundlich Isotherm Model

The Freundlich model is always used to describe the adsorption on heterogeneous surface of adsorbent [56]. Different initial concentrations of heavy metals were used with fixed dosage of amidoxime resin to obtain the equilibrium data. The Freundlich isotherm model is expressed as follows:
(13)lnqe=lnkf+1nlnCe,where Kf (mg/g) and n (g/L) are the Freundlich adsorption constants. The plots of lnqe against lnCe shown in Figure 18 give straight lines. From the slope and intercept of those lines, the values of n and Kf can be calculated. Bad linearity and low values of correlation coefficient (R2) indicate disagreement between equilibrium data and this model. Values of n more than the unit mean favourable adsorption condition, and lead (II), Cr (III), and Cd (II) are favourably adsorbed via amidoxime resin [53].Figure 18
Freundlich adsorption isotherms for adsorption of (a) Pb (II), (b) Cr (III), and (c) Cd (II) on amidoxime chelating resin, pH 5, and temperature at 25°C.
(a)(b)(c)


## 2.16.1. The Langmuir Isotherm Model

The Langmuir model assumes that the monolayer adsorption process takes place between the adsorbate and adsorbent, and the surface is homogenous with a finite number of active sites when sites are filled with adsorbate molecules. There is no chance of further adsorption on this site, and the saturation point is accomplished [54]. The linear equation is expressed as
(11)Ceqe=1KLqm+Ceqm,where Ce is the equilibrium concentration (mg/l) of metals in solution; qe is the amount of metal ions adsorbed (mg/g) at equilibrium; KL is the Langmuir equilibrium constant (l/mg), and it is related to the affinity of adsorption sites; and qm gives the maximum theoretical monolayer adsorption capacity (mg/g). The values of qm and KL (Table 2) were obtained from the slope and intercept, respectively, of plots of Ce/qe versus Ce, which are shown in Figure 17. The linearity and high values of correlation coefficients (R2) indicate that the Langmuir model describes the adsorption process very well, confirming the formation of monolayer. Weber and Chakravorti [55] defined the separation factor (RL) as a characteristic dimensionless equilibrium parameter for the Langmuir model, and it is expressed as
(12)RL=11+KLCo.Table 2
Langmuir and Freundlich isotherm constants for lead (II), Cr (III), and Cd (II) adsorption on amidoxime chelating resin.
CompoundsT (k)Langmuir isotherm constantsFreundlich isotherm constantsqm (mg/g)KL (L/mg)RLR21/nnKFR2Lead (II)298.1643.869.120.0020.9990.0423.1548.620.8638Chromium (III)298.1642.745.320.0040.9990.0615.4349.740.9701Cadmium (II)298.1632.471.540.0120.9930.1010.0448.070.7647Figure 17
Langmuir adsorption isotherms for adsorption of (a) Pb (II), (b) Cr (III), and (c) Cd (II) on amidoxime chelating resin, pH 5, and temperature at 25°C.
(a)(b)(c)The values ofRL for each initial concentration was less than unity and greater than zero indicating the favourable adsorption of lead (II), Cr (III), and Cd (II) on polyamidoxime chelating resin [53].


## 2.16.2. The Freundlich Isotherm Model

The Freundlich model is always used to describe the adsorption on heterogeneous surface of adsorbent [56]. Different initial concentrations of heavy metals were used with fixed dosage of amidoxime resin to obtain the equilibrium data. The Freundlich isotherm model is expressed as follows:
(13)lnqe=lnkf+1nlnCe,where Kf (mg/g) and n (g/L) are the Freundlich adsorption constants. The plots of lnqe against lnCe shown in Figure 18 give straight lines. From the slope and intercept of those lines, the values of n and Kf can be calculated. Bad linearity and low values of correlation coefficient (R2) indicate disagreement between equilibrium data and this model. Values of n more than the unit mean favourable adsorption condition, and lead (II), Cr (III), and Cd (II) are favourably adsorbed via amidoxime resin [53].Figure 18
Freundlich adsorption isotherms for adsorption of (a) Pb (II), (b) Cr (III), and (c) Cd (II) on amidoxime chelating resin, pH 5, and temperature at 25°C.
(a)(b)(c)


## 3. Conclusion

This study used the grafted copolymerization of date palm wood fiber using hydrogen peroxide as an initiator and ammonium ferrous sulphate as a catalyst. It studied the grafting parameters for obtaining the best grafting percentage. The grafting percentage depends upon the parameters such as the reaction period, reaction temperature, amount of the catalyst, concentration of the initiator, and monomer volume. The best grafting percent was obtained using acrylonitrile monomer under following conditions: 8 ml monomer, 0.03 M solution of hydrogen peroxide, and 0.306 mmol concentration of the catalyst. The reaction completed in 60 min at 75°C.FTIR and STEM techniques were used for grafting products. Hydroxylamine was used for treating an AN-grafted copolymer for producing polyamidoxime chelating resins. The conversion process was confirmed using the FT-IR technique. Also, the batch template was used for examining the absorption capacity for heavy metal ions. The absorption pH value was found to range between 5 and 6. The better absorption behavior was observed for cadmium (II), chromium (III), and lead (II). The Langmuir isotherm found the correlation coefficient for resin to be 0.99, which was better than Freundlich isotherms.



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