Batch Adsorption, Kinetics and DFT study of Cd(II) Ion From Aqueous Solution By Low Cost Starch Based Activated Carbon

Cadmium(II) contamination in the environment is an emerging problem due to its acute toxicity and mobility, so it is very urgent to remove this specie from industrial wastewater before it is discharged into the environment. Thus, a starch-based activated carbon (AC) with a specific surface area of 1600 m2g-1 is used as an adsorbent for the capturing of toxic Cadmium(II) ion from synthetic solution. The sorbent is characterized by BET, SEM, TEM, XRD, FT-IR, TGA, and zeta potential. The maximum uptake (284 mg g-1) of Cadmium(II) ion is obtained at pH 6. The thermodynamics parameters like ∆G, ∆H, ΔS are found to be -17.42 kJmol-1, 6.49 kJ mol-1, and 55.66 Jmol-1K-1 respectively, revealing that the adsorption mechanism is endothermic, spontaneous, and feasible. The experimental data follows the D-R and Langmuir models well. The mass transfer is controlled by pseudo 2nd order kinetics. Furthermore, the density functional theory simulations demonstrates that the activated carbon strongly interacted with the Cd(II) ion through its various active sites. The adsorption energy noted for all interactive sites is highly negative (-0.45 eV to -10.03 eV), shows that the adsorption process is spontaneous and stable which are in agreement with the experimental thermodynamics analysis.


Introduction
Due to the rapid industrialization and urbanization the heavy metals concentration has increased enormously in water reservoirs. The rate of depletion of water reservoirs is alarming and is a serious environmental problem [1,2]. The clean water vitality cannot be compromised at any case. The large number of pollutants have been identified from industrial and domestic sources and are included of antibiotics, dyes phenols, insecticides and heavy metals constituents [3,4]. Due to the non-degradable and accumulative nature, heavy metals are extremely harmful for living organisms. Among heavy metals the non-nutritive cadmium (II) metal is classified as human teratogen, carcinogen, the most dangerous and priority water pollutant with biological half-life about 10-30 years [5].
The main sources of Cd(II) ion contamination are industrial wastewater, combustion of oil and coal and wastes incineration. The Cd(II) is extensively used in different industrial processes e.g., as a coloring pigment, anticorrosive agent, fabrication of batteries, in a nuclear power plants as an absorber of neutrons. It is been estimated that about 7000 tones /annum has been released on global level [6]. According to the world health organization (WHO), the permissible level of Cd(II) is less than 0.003 mg dm -3 for drinking water [6]. The Cd(II) has noxious effect on lungs, liver and kidney even in a very low concentration [7,8]. The inhaling of Cd(II) contaminated air can cause shortness of breath, damage of mucous membranes and lung edema. The intake of food contaminated with Cd(II) can cause diarrhoea and severe vomiting. Similarly, it can cause bone damage, infertility, prostate cancer and tumor [9,10]. So, it is pertinent for human health and environmental safety to ascertain the concentration of Cd(II) on regular basis and develop techniques for the capturing of Cd(II) ion, before it is discharged into water bodies.
Several techniques like reverse osmosis, ion exchange, chemical precipitation, electrolytic extraction, redox method, and electrodialysis have been designed and applied for the scavenging of heavy metals. However, these methods have their limitations e.g., long processing time, high energy consumption, and poor sequestration of heavy metals [11].
Chemical precipitation is one of the most widely used for heavy metal removal from inorganic effluent in industry due to its simple operation . These conventional chemical precipitation processes produce insoluble precipitates of heavy metals as hydroxide, sulfide, carbonate and phosphate [12].
Ion Exchange Ion exchange can attract soluble ions from the liquid phase to the solid phase, which is the most widely used method in water treatment industry. As a costeffective method, ion exchange process normally involves low-cost materials and convenient operations, and it has been proved to be very effective for removing heavy metals from aqueous solutions, particular for treating water with low concentration of heavy metals [13].
The adsorption technique is efficient as it is simple in operation, cost-effective, and environmentally friendly [1]. A variety of adsorbents like silica gel [14,15], clay [16,17] and bio sorbents [18] have already been reported for the sequestration of heavy metals from wastewater. The theoretical analysis is a complementary tool to know the mechanism of the absorption process [19][20][21]. The efficiency of ACs as adsorbents for diverse types of pollutants is well reported [22]. It is well known that activated carbon has been found much efficient for removing organic compounds than metals and other inorganic pollutants. Efforts are ongoing to substantially improve the potential of carbon surface by using different chemicals or suitable treatment methods which will enable AC to enhance its potential for the removal of specific contaminants from aqueous phase. The physical and chemical structure of carbon could be changed by various methods, i.e. activation conditions (different agents, temperature and time of the process), precursor, additives, etc.
Starch based activated carbon was prepared and characterized to remove Cd(II) ion from spiked water. For the determination of the adsorption mechanism the data were subjected to different adsorption models. The sorption obeys 2 nd order kinetics, Freundlich and Langmuir isotherms and was more favorable at pH 6. For the determination of thermodynamic parameters of the adsorption mechanism, the temperature study was carried out, which shows that the adsorption was spontaneous, feasible, and of endothermic nature. The DFT supported the experimental findings.

Materials
All the chemicals like CdCl2, dithizone, NaOH, HCl, KOH, CH3COOH, CH3COONa, H3BO3, and NaOH of analytical grade were supplied by Sigma Aldrich Pakistan (Pvt.) Ltd. and were used without any further purification. The solutions of buffer 1-7 with the ionic strength of 10 mmol were prepared by taking the calculated amount of KCl and HCl for buffer 1-2, CH3COOH, and CH3COONa for buffer 3-6, and NaOH and H3BO3 for buffer 7. CdCl2 was mixed with dithizone in 2 M NaOH to get orange coloured Cd-dithizone complex (Figure 1) and its absorbance was studied at 549 nm wavelength as compared to the standard [23].
The concentration of Cadmium (II) ions was determined from its complex with dithizone in the presence of non-ionic surfactant e.g., CTAB. The molar absorptivity of complex becomes almost double as compare to the standard method and a very small amount of Cd +2 can be determined spectrometrically at wavelength of 549 nm. The increase in the molar absorptivity and rate constant are due to the micelle, which favours the formation of a Cd (II) ion and dithizone complex.

Reaction:
Cd

Synthesis of Adsorbent
The starch sample was sieved by 300 mesh size and mixed with potassium hydroxide in a 1:4 weight ratio and activated at 850 o C for 90 minutes with argon at 3 o C/minute rise. The obtained product was thoroughly washed again and again with 5 wt. % HCl followed by washing with double distilled water until the product was neutralized and dried at 120 o C overnight. The product thus obtained was named starch based activated carbon (AC) and characterized by BET, SEM, TEM, XRD, FT-IR, TGA, and zeta potential [24].

Adsorption experiment
Glass culture tubes with a given amount of adsorbent and a specific volume of sorbate with a known concentration were used in the batch mode experiments at room temperature or specified otherwise. The culture tubes were shaken on a wrist action shaker (Model Burrell 75, Burrell Scientific, USA). After shaking the concentration of Cd(II) was recorded by using a double beam UV-Visible spectrophotometer (Labmed. Inc UVD 2960). The adsorbed amount of Cd(II) and the distribution coefficient (Kd) were determined through the following equations.
where Ai is the initial Cd(II) concentration, Af is the equilibrium concentration, W represents the weight of sorbent and V is the volume of Cd(II) solution.
All the experiments were carried out in triplicate at room temperature or described otherwise. The linear regression of the data was carried out and was in the range of 1-0.997 for all analyses.

Material Characterization
The activated carbon derived from starch was used for the adsorption of Cd(II) ion from industrial wastewater. The material was characterized through the following techniques.

SEM and TEM analysis
The SEM images of the AC derived from starch at different resolutions illustrate the sheet type morphology that ranges from nanometer to several micrometers (Figure 2 a and b), whereas the TEM images at low and high magnification further confirm the multilayer nature of the individual sheet for the obtained activated carbon (Figure 2 c and d) [25].

AFM analysis
AFM technique was performed further to investigate the average and maximum height of the AC Figure 3 (a-d) shows the 2-dimensional (2D) and 3-dimensional (3D) patterns of starch-based AC with particle height that varied from 5 to 50 nm [26]. Thus, through the AFM technique, we could guess the maximum height (50 nm) of the multilayer AC sheets, which make it an attractive choice for toxic Cd(II) ion adsorption [23].

FT-IR analysis
FTIR analysis is used to confirm different groups on the surface of AC (Figure 4). The broader peak at 3480 cm -1 in corresponds to the hydroxyl group [27]. The absorption peaks at 2920 is due to -CH3 and peak at 1720 cm -1 is due to -C=O vibration [28]. The peaks on 1550 and 1115 cm -1 representing -NO2 and -SO3H groups respectively [29]. The spectra indicates that starch-based AC contains aromatic rings [30].

XRD analysis
The structure and crystallinity of activated carbon was investigated by using XRD technique Figure 5 represents the XRD patterns of virgin starch-based AC. In the XRD patterns, the peaks at 2θ= 25° and 2θ= 43.460° originates from its graphite-like nature and can be assigned to the (002) and (100) plane of graphitic carbon, respectively [31,32].

TGA Study
The thermal stability of the starch-based AC was studied at temperature up to 1000 o C, from TGA analysis it can be concluded that the starch-based AC was stable at a very high temperature (Figure 6). The starch-based AC converted into CO and CO2 [33] and some other compounds at various temperatures [34]. At the end only 11% loss was observed from the total mass of starch-based AC. 3.1.5. Zeta potential and zeta sizer analysis The particle size distribution is a useful parameter to elucidate the arrangement of particle size in the adsorbents while its zeta potential determines its surface charge required for dispersion. Figure 7 shows the size distribution and zeta potential plots of the AC, which reveals that the average particle size was 575 nm and polydispersity index (PDI) of 0.635, representing sufficient variation in sizes. Its surface charge was -16.9 mV, which is sufficient to remain suspended [35].

BET and BJH analysis
The surface .area was found to .be 1600 m 2 g -1 of starch-derived AC as determined from BET isotherm, with porous structure (Figure 8). The BJH analysis shows that AC has microspores and mesopores on its surface (inset of Fig. 8a). While the BET isotherm Figure 8 b shows the Cd(II) ions loaded AC ,s surface area, which remained only 13.35 m 2 g -1 , reflecting that most of the surface has been covered by the metal.

Effect of pH on sorption
The sorption capacity is greatly influenced by the medium [2]. The effect of pH on the adsorption of Cd(II) was investigated at pH 1.0 -9.0. The concentration of sorbate of 100 mg L -1 , sorbent amount of 30 mg, and shaking time of 120 minutes were chosen arbitrarily. The equilibrium uptake of Cd(II) increased notably up to pH 6 and then decreased continuously (Figure 9a). The maximum uptake (98.58%) was observed at pH 6 and was selected for further experiments. At acidic pH, the electrostatic repulsion is created between protonated surface of AC and Cd(II) metal ion. These observations have also been reported by other researchers [5,36]. Beyond pH 6 the adsorption capacity has decreased due the formation of Cd(OH)2 (cadmium hydroxide) [37].
Based on equilibrium constants, a speciation diagram was constructed and is depicted in Figure 9e. The diagram shows that at pH below 6, the Cd 2+ ion predominates and at pH values just below 7, cadmium begins to precipitate out as Cd(OH)2. At pH of 6 the species distribution is approximately 90% Cd 2+ and 10% Cd(OH) + . This means that all the species occurring at pH values of 6 and below carry a positive charge either as Cd 2+ or Cd(OH) + . Depending on the pH of the solution, the Cd 2+ in aqueous solution can form various species or hydro complexes. [38]

Effect of Cd(II) ion solution concentration
The effect of Cd(II) ions solution concentration was studied at 20-220 mg/L (  Figure 3.63b). The rate of removal of adsobate was maximum at 80 mg/L and then it remained constant [39,40], thus 80 mg/L was taken as standard for further experiments.
The Langmuir equation was used in the following form: where Qmax. is the amount adsorbed, KL , qe and Ce were calculated from slope and intercept of the graph, (Figure 9d) and their magnitudes are listed in Table  1. The adsorbate affinity (RL) is represented as below: The RL (0.0072) indicating favourable adsorption [41]..
The Freundlich equation was used in the following form [42].

log
log log e F e q K C n =+ (5) where the adsorption capacity (KF mmol.g -1 ) and 1/n represented the surface heterogeneity and can be calculated from the slope and intercept of the graph (Figure 9c). The Freundlich parameters are tabulated in Table 1 [43,44].

Influence of the AC dose
The influence of the dose of the AC on the adsorption of Cd(II) ion was teste at AC dose ranges 0.01-0.035 g Figure 10a. The rate of adsorption increased at the AC dose up to 0.025 g and then it remained constant. Thus, 0.025 g was taken as standard for further experiments.

Influence of shaking time
The influence of shaking time on Cd(II) ion removal was investigated between 0-50 minutes. The equilibrium was attained within 40 minutes and was selected for further investigations (Figure 10b). The "adsorption rate of Cd(II) ion was high initially, as abundant vacant sites were available and after that, the movement of the ions was intraparticle which was relatively a slow process The mass transfer during the process in the rate determining step can be determined by using kinetic models [2,45,46]. The pseudo 2 nd order equation applied in the following linear form was the best fitted. t e e t t q k q q = + (6) where" k2 rate constant and qe can be determined from the slope Fig. 10c and their magnitudes are calculated and are listed in Table 2. The experimental and theoretical values of qe are in close agreement with each other, indicating the applicability of the model.
The Reichenberg equation were used in the following form in order to further explore the mechanism [47].
Where F is the ratio of qt and qe and BT is a constant (Fig. 10d), showing that both film diffusion and intraparticle diffusion are involved in the mechanism.

The thermodynamic study
The effect of temperature on sorption was investigated in the temperature ranges of 283-313K. It was observed that the adsorption increased with the increases in temperature Figure 6e, which reveals that the process may be chemisorption reverse may be true for physiosorption. This increase in the rate of adsorption with temperature may be due to the efficient flow of sorbate molecules against the concentration gradient or transport of sorbate through the energy barrier. This may also create some new sites on the surface of the sorbent [48]. The thermodynamic parameters like Gibbs free energy change (ΔG), enthalpy (ΔH), and entropy (ΔS) were determined by using the relations below [49].

ΔG = −RTlnk
The calculated value of ΔG was -15.75 kJ/mole, revealing that the adsorption of the Cd(II) ion on to AC is feasible and spontaneous [50]. The magnitude of ΔH was 6.49 kJ mol −1 , showing that the sorption mechanism is endothermic [51]. The ΔS as determined from the intercept of the graph of lnk against 1/T was 55.66 J/mol. (Figure 11a) reflecting the sorbate/sorbent complex stability [52]. The thermodynamic results are summarized in Table 3.

DFT study
To gain deeper insights into the interactions of Cd(II) ion with the activated carbon, density functional theory (DFT) simulations are performed which are recently frequently utilized combine with experimental studies to understand the mechanism of adsorption process [32,53,54]. The DFT simulations were performed by DMol3 code [55,56], using the spin unrestricted density functional theory along with Perdew Burke Ernzerhof (PBE) in combination with double numerical basis set involving polarization functions (DNP). The Hirshfeld charge density method was used for the population analysis. The adsorption energies were calculated using the formula; (12) where, Ecomplex is the total electronic energy of complex system (Cd(II) ion adsorbed over activated carbon), EAC and ECd(II) are the energies of activated carbon and Cd(II) ion separately.
The optimized geometries are represented in Figure 12 and values of adsorption energies, intermolecular distances and charge transfer are collected in Table 4. Four different adsorption modes of Cd(II) ion onto activated carbon (AC) are simulated which are named as CMP-1, CMP-2, CMP-3 and CMP-4 as illustrated in Figure 12. In CMP-1 the Cd(II) ion interacted with the O atom of C=O bond present on the surface of AC. The geometry optimization reveals that the Cd(II) ion formed in intermolecular bond of bond distance of 2.39 Å, while the adsorption energy (Ead) shows that the Ead value for this complex is -9.20 eV, which shows the stronger interaction. The Hirshfeld charge analysis depicts that there is larger charge transfer (0.59 e) occurred from the Cd(II) ion to the O atom of the surface which resulted stronger intermolecular bond. In CMP-2 the Cd(II) ion interacted with the O atoms of the NO2 group and O atom of C=O group at the edge of the AC. The optimization shows that the Cd(II) ion formed intermolecular bonds with one O atom of NO2 group and with O atom of C=O group. The bond distances noticed for this interaction is 2.25 and 2.41 Å, respectively. The Ead energy and Hisrhfeld charge transfer value obtained for this complex is -10.03 eV and 0.70 e. This larger Ead value and higher charger transfer value demonstrate that the formation of this complex is highly thermodynamically stable. In CMP-3 the Cd(II) ion interacted with the SO3H group at the edge of AC. The intermolecular bond distances values calculated for this complex are 2.98 and 2.92 Å, respectively. The Ead and charge transfer values noticed for this complex is -9.54 eV and 0.59 e. While in CMP-4 the Cd(II) ion placed over the top of hexagonal ring of the AC. The geometry optimization reveals that the Cd(II) ion form weak intermolecular bonds in this complex having binding distances upto 3.45 Å. Smaller Ead and charge transfer values obtained for this complex which is -0.45 eV and 0.23 e. In summary, the DFT simulations shows that the AC has higher affinity for the adsorption of Cd(II) ions due to the presence of higher negative active sites i.e. N, O and S atom. The Cd formed stronger bonds with these active sites which resulted stronger adsorption. The larger negative values depicts that the adsorption process is spontaneous and thermodynamically stable.

Conclusions
The Cd 2+ was adsorbed onto activated carbon and the experimental data were adjusted to the Langmuir isotherm. Temperature and pH of the solutions were shown to influence significantly the adsorption isotherm. At initial pH of 2 or lower. Cd 2+ did not adsorb to the activated carbon. However at pH greater than 3 Cd 2+ began to adsorb achieving its maximum adsorption capacity at an initial pH of 6. Based on results obtained it can be (concluded, confirmed, stated) that starch-based activated carbon can be used as an efficient and economical sorbent for the sequestration of Cd(II) from wastewater. The adsorption phenomena were dependent upon several factors including pH and the optimum pH for maximum sorption was found to be 6.0. The adsorption results obey Langmuir, Freundlich isotherms well. The adsorption capacity and other parameters have been computed from different isotherm constants. The pseudo 2 nd order adequately describes the kinetic data. The pseudo 2 nd order kinetics shows a high kinetics correlation with experimental data. Moreover, the DFT study shows that the AC has stronger affinity for the adsorption of Cd(II) ions due to presence of highly active sites. The shorter bond distances in CMP-1, CMP-2 and CMP-2 evince that the Cd(II) strongly interacted with various active sites of the AC, which resulted stronger adsorption. Therefore, the Ead values are highly negative which ranges from -0.45 eV to -10.03 eV, indicates that the adsorption process is spontaneous and thermodynamically feasible. The larger charge transfer (0.23 e to 0.70 e) give roots to the presence of stronger intermolecular bond between the Cd(II) ions and AC.