The adsorption potential of raw pomegranate peel powder (PMPP) for lead (Pb) ions was investigated via batch mode at varying initial adsorbate concentration, contact time, and adsorbent concentration. The PMPP was extensively characterized using Fourier-transform infrared spectroscopy (FTIR), X-ray diffraction (XRD), Scanning electron microscopy (SEM), Energy-dispersion X-ray (EDX), thermogravimetry (TG), and differential scanning calorimetry (DSC) analyses. The instrumental characterization results confirmed the presence of important functional groups and surface texture/morphology that played key roles during the lead ion adsorption. Description of the experimental equilibrium data by nonlinear Langmuir, Freundlich, Dubinin–Radushkevich, and Temkin isotherm models was elaborately presented in the study. The experimental kinetic data were fitted to the Pseudo-first-order, Pseudo-second-order, Intra-particle diffusion, and Elovich models. The Temkin model satisfactorily predicted the isotherm data. Meanwhile, the intra-particle diffusion model was best at predicting the kinetic data at adsorbate concentration of 150 mg/L, while the Elovich model emerged as the best fit at 300 mg/L concentration. This study shows that lead ions could be efficiently removed using raw pomegranate peel powder.
Notes
Publisher's Note
Springer Nature remains neutral with regard to jurisdictional claims in published maps and institutional affiliations.
Introduction
Lead (Pb) is a household element with extensive application in lead pigments, smelting, battery production, etc. [1]. Due to their remarkably high tensile strength, pliability, and low melting point, they serve as raw materials for the production of domestic utensils and as antiknock in automobiles [2, 3]. However, reports have shown that acute lead poisoning (in humans) inhibits the enzymatic, cellular, and organ functionality, thus leading to kidney failure, nervous system breakdown, etc. [4]. To forestall such negative health impact, a maximum permissible limit was set at 10 mg of Pb/liter of drinking water by the World Health Organization [5].
As a simple and cost-effective approach, adsorption techniques using a wide range of organic and inorganic adsorbents have been effectively applied in the sequestration of aqueous heavy metals in general and lead pollutants in particular. Recently, renewable and cheaply available agro wastes are considered viable alternatives to conventional organic and inorganic adsorbents [6, 7]. Ashfaq, et al. [8] investigated the lead ion sorption capacity of a biosorbent synthesized from a mixture of banana and potato peels. The maximum lead uptake was recorded at pH 5.0 using 1.0 g of adsorbent at 2 h contact time and 10 ppm initial adsorbate concentration. The effectiveness of distinct low-cost adsorbents synthesized from casuarina fruit, sorghum stem, and banana stem was also investigated for the uptake of lead ions [9]. The authors concluded that these adsorbents had promising potentials for adsorbing lead ions from industrial wastewater, thus contributing to environmental protection and sustainability. Furthermore, biosorbents prepared from corn and rice husks were studied for the removal of aqueous lead ions [10]. According to the authors, these biosorbents indicated more than 90% lead ion removal efficiencies.
Advertisement
In the present study, an efficient lead ion adsorbent was obtained from pomegranate peels by subjecting them to three physical processing stages namely, drying, crushing, and sieving. Pomegranate peels are mostly sourced as one of the byproducts of the pomegranate juice industry. According to available records, about 669 kg of these byproducts (piths, rinds, and peels) are generated from the processing of a ton of pomegranate fruit [11]. Notably, the peels and the internal membrane constitute about 50% of the entire pomegranate fruit [12]. Asides from their ready availability, pomegranate peels have several inherent functional groups that play key roles during pollutant adsorption and also permit the occurrence of multiple mechanisms. For instance, the hydroxybenzoic (gallic and ellagic) acids, derivatives of flavones, and hydroxycinnamic acids are responsible for their superior heavy metal chelation properties [13]. The phenolic compounds and the anthocyanin derivatives contribute to the excellent surface adsorption of free metal ions [14]. In a previous phytochemical investigation of pomegranate peels, 10 phenolic compounds containing a common hexahydroxy diphenol moiety were isolated [15]. In pomegranate peels, the main phenolic compounds reported in the literature include flavonoids, tannins, and phenolic acids [16].
The reported presence of elements (like sodium, Na; potassium, K; calcium, Ca; magnesium, Mg; nitrogen, N, etc.) and some complex polysaccharides could initiate the formation of important complexes during heavy metal adsorption [17]. Similarly, the electrically charged functional groups (such as the amino, hydroxyl, and carboxylic groups) on the peels provide strong binding sites for the aqueous heavy metal ions [18].
Within the last decade, several authors have investigated the heavy metal adsorption potentials of raw pomegranate peel powder (PMPP) [13, 14, 19‐28]. The novelty of the current study lies in the authors’ succinct discussion of the experimental results in comparison with findings from pertinent publications. Description of the experimental equilibrium data by nonlinear Langmuir, Freundlich, Dubinin–Radushkevich, and Temkin isotherm models was elaborately presented in the study. Non-linear regression analysis is preferable to determine isotherm and kinetic parameters. Previous investigations have shown that the nonlinear method is a better method than the linear method for fitting the kinetics of adsorption process [29, 30]. The nonlinear kinetic transformations to linear kinetic usually result in parameter estimation error and fit distortion. Furthermore, the PMPP was extensively characterized using Fourier-transform infrared (FT-IR) spectroscopy, X-ray Diffraction (XRD), Scanning electron microscopy (SEM), Energy diffraction X-ray (EDX), thermogravimetric analysis (TGA), and Differential scanning calorimetry (DSC) measurements. The effect of process variables was also investigated experimentally via a batch mode.
Materials and methods
Materials
Pomegranate peels were collected from fresh juice stores at a local market in Cairo, Egypt. The lead acetate (99%), sodium hydroxide pellets (97%), ethylene-diamine-tetra-acetic acid powder (98.5%), nitric acid (70%), sodium carbonate, acetone (99%), ethyl alcohol (95%), and all other reagents used in the study were laboratory-grade chemicals (Merck, Germany).
Advertisement
Preparation of pomegranate peel adsorbent
The collected pomegranate peels were cut into small pieces and washed with distilled water to remove inherent dust and dirt. The washed sample was soaked overnight in double distill water and afterward filtered off. This overnight soaking in water and filtration was repeated severally until all color and soluble materials were removed from the pomegranate peels. The decolored peels (PMPP) were oven-dried at 105 °C for 3 h, crushed to desired particle size (120 μm), and stored in an air-tight container for further use.
Batch adsorption studies
0.3 g of the PMPP was weighed into 125 mL Erlenmeyer flasks containing 100 mL of varying Pb(II) ion solution (100–600 mg/L). The pH of the initial solution was 7. The adsorption experiment was typically dynamic at 150 rpm, 30 °C, and a pre-defined period. After each adsorption experimental run (at a known initial adsorbate concentration), the spent PMPP was filtered off and the lead ion concentration in the supernatant was measured via the metal–ligand complexation titrations approach using a standard EDTA solution (0.0005 M). All experiments were repeated 3 times. The equilibrium adsorption capacity, qe (mg/g) of the PMPP sample is evaluated from Eq. (1).
where Co and Ce (mg/L) are the lead ion concentration at the onset of experiment and equilibrium, respectively, W (g) = mass of PMPP used, and V = volume of Pb(II) solution(0.1 L).
Instrumental characterization procedures
The pre- and post-adsorption FTIR spectra of the PMPP were determined using Perkin–Elmer spectrophotometer from 4000 to 400 cm−1 using KBr disks containing ∼ 5–10 mg of sample in ∼ 300 mg of KBr. The XRD patterns were obtained on a PANalytical diffractometer (X’Pert PRO) in continuous scanning mode using a Cu tube (in the reading range of 2–80°). Solid samples are prepared for X-ray diffraction by grinding. The SEM micrograph of the PMPP was obtained (after overlaying the sample with a thin layer of gold using a diode sputter unit) on a scanning electron microscope (model JEOL-JSM-5600), at an accelerating voltage of 25.0 kV. Elemental analysis of the samples was obtained using an EDX spectrometer (Oxford Instruments 6587 EDX detector), attached to the JEOL-JSM-5600 unit used for SEM analysis. Thermogravimetric analysis (TGA) and differential scanning calorimetry (DSC) measurements were obtained using Themys thermal analyzer (SETARAM labsys TG-DSC-16). The samples were weighted to 13–15 mg in an aluminum crucible and introduced to the thermal analyzer with a measuring temperature range from room temperature up to700 °C with a heating rate of 10 °C/min under nitrogen atmosphere.
Results and discussion
Instrumental characterizations
Fourier-transform infrared (FTIR) spectroscopy
The FTIR spectra of the native and loaded PMPP are presented in Fig. 1. The native PMPP sample exhibited a broad absorption peak at 3291 cm−1, indicating the presence of bonded and free hydroxyl groups, due to the O–H groups' vibrations (carboxylic acid, phenol, or alcohols) of cellulose, lignin, hemicellulose, and adsorbed water [31]. The peak observed at 2917 cm−1 corresponds to the C–H stretching vibration in the methyl groups, while those at 1711 cm−1 represent C = O stretching of the carbonyl group of aldehydes and ketones. The band at 1602 cm−1 is assigned to the CH2 stretching of an aromatic ring from the hemicellulose. The strong stretching vibration of C–O at 1011 cm−1 is attributed to carboxylic acid, alcoholic, phenolic, ether, and ester groups of lignin and hemicelluloses components [19]. So far, the FTIR discussion has established the existence of five major absorption peaks on the native PMPP at 3291, 2917, 1711, 1602, and 1011 cm−1. Similar absorption peaks were reported by others during the FTIR investigation of the raw pomegranate peel powder. For instance, Ben-Ali, et al. [19] observed these main peaks at 3298.68, 2941, 1713, 1607.21, and 1029.18 cm−1, while Giri, et al.’s [13] findings coincided with 3402.05, 2926, 1735, 1619, and 1044 cm−1 peaks. Other weak peaks were recorded at 1320 and 1439 cm−1. The peaks at 1320 cm−1 (δsCH3) and 1439 cm−1 (δasCH3, δasCH2) are attributed to symmetric and asymmetric bending vibration of δCH3 and δCH2 scissoring in hemicelluloses (H3C–(C = O)–O–) and lignin (H3C–O–Ar), respectively [32]. The spectral line of loaded PMPP when compared to those of native PMPP shows a negligible change in the IR spectrum except the shrinking of the peak at 1711 cm−1 which corresponds to the carbonyl group stretching in aldehydes and ketones.
Fig. 1
FT-IR of Pomegranate Peel and Pb (II) loaded Pomegranate Peel
×
X-ray diffraction (XRD)
The X-ray diffraction pattern of the native PMPP (Fig. 2a) shows weak peaks at 17.14°, 22.11o, and 44.5°. Incidentally, these peaks were superimposed onto an amorphous diffraction spectrum, thus indicating the presence of a sublime crystalline cellulose Iβ structure [33]. The absence of the sharp diffraction peaks of the crystalline cellulose and the predominance of amorphous peaks in the XRD spectrum indicates that the non-cellulosic (hemicellulose and lignin) components are the main contents of the native PMPP. Figure 2b shows no observable change in the amorphous phase of the native PMPP after complexation with the aqueous lead ions. Hence, it is believed that the complexation of leads ions with the PMPP functional groups occurred at the same component phases. The present study on the application of raw pomegranate peel powder in heavy metal adsorption did not investigate the surface crystallinity of their respective adsorbent samples.
Fig. 2
XRD of Pomegranate Peel and Pb (II) loaded Pomegranate Peel
×
Scanning electron microscopy (SEM)
Figures 3 (a and b) shows the morphology of the surface of native and loaded PMPP. The SEM micrograph shows a soft amorphous and heterogeneous structure of typical non-cellulosic contents (lignin and hemicellulose). Also, the absence of orientation and fibrous structure of cellulose and porosity was observed. This finding coincides with the XRD and FTIR analyses result, thus confirming that the main components of the PMPP sample are non-cellulosic materials. Studies by Salam, et al. [14] and Giri, et al. [13] reported a coarse surface structure with hollow cavities and pore structure on the native/raw pomegranate peel. However, the coarse and rough surface structures metamorphized into a comparatively smoothened surface due to a possible occurrence of a redox reaction between the adsorbent active sites and adsorbed chromium ions. Conversely, Ghaneian, et al. [20] made a differing observation, as they reported a significant morphological modification in the pomegranate peel powder adsorbent from smooth (before adsorption) to rough morphology (after heavy metal biosorption).
Fig. 3
a SEM of Pomegranate Peel. b SEM of Pb (II) loaded Pomegranate Peel
×
The EDX spectrum demonstrated that the major elements of native PMPP were carbon (47.71%), oxygen (50.25%), and nitrogen (1.66%) [Fig. 4 (a and b)]. The presence of Pb (0.38%) on the surface of PMPP, clearly demonstrates that lead ions were successfully adsorbed. Other authors also reported the presence of carbon, oxygen, nitrogen, and hydrogen as the major constituents of PMPP [13, 19]. However, asides from the main constituents, traces of potassium, calcium, copper, zinc, manganese, iron were also observed by [13, 14].
Fig. 4
a EDX of Pomegranate Peel. b EDX of Pb (II) loaded Pomegranate Peel
×
Thermal analysis
The thermal behavior of the native PMPP was studied using thermogravimetry (TG), differential thermogravimetry (DTG), and differential scanning calorimetry (DSC) analyses under nitrogen atmosphere and heating rate of 10 °C min−1. Figure 5a shows TG and DTG curves for the native PMPP. The thermal weight loss of the sample proceeds in multi-steps with a total mass loss of 63wt% in a temperature range of 133–500 °C. The first step with a weight loss of 8% at 58–133 °C is attributed to the evolution of moisture. The multi-decomposition at 194–334 °C is attributed to the degradation of the hemicellulose, lignin, and cellulose [19, 34]. Furthermore, the multi-decomposition of the raw PMPP is associated in the DSC thermogram with an exothermic peak (91.96 j/g) at the initial main decomposition with a temperature range 136–218 °C and an endothermic peak (− 40. 48 j/g) at the end of the main decomposition peak with a temperature range 309–368 °C (Fig. 5b). The lignin has a wider degradation temperature range than cellulose and hemicellulose with a maximum weight loss at 240 and 334 °C due to its constituent functional groups, such as phenolic, hydroxyl, carboxyl, carbonyl, and methoxy groups [34]. The thermogravimetric data indicate that the native PMPP is thermally stable up to 143 °C.
Fig. 5
TGA and DSC of Pomegranate Peel
×
Effect of process variables
The effect of pH on adsorption capacity (mg/g) of Pb(II) onto pomegranate peel is shown in Fig. 6. With the increase in pH of solution pH (from pH 2.0 to 5.5), the amount of lead adsorbed significantly increased (from 0 to 335 mg/g). Adsorption decrease was observed at a pH greater than 6.0 as a result of Pb (II) ion precipitation as Pb(OH)2. The effect of adsorbent concentration on the lead uptake capacity as illustrated in Fig. 7(a) shows the highest lead uptake (335 mg/g) at 0.3 g/L adsorbent concentration and reaction conditions: Pb(II) ion con., 300 mg/L; pH, 5.5 and temp., 30 °C. The uptake values decreased progressively with a further increase in adsorbent concentration. It is well known that such improved heavy metal uptake at lower adsorbent concentration is related to the availability of more sorption sites [35]. Other authors who investigated the heavy metal sorption ability of raw pomegranate peel powder reported a similar improvement in the cation uptake (qe) at lower adsorbent concentration due to greater sorption site availability. Hence, 0.3 g/L was adopted as the optimum adsorbent concentration in the study.
Fig. 6
Effect of pH on adsorption capacity of Pb(II) onto Pomegranate Peel; Reaction conditions: Pb(II) ion conc., 300 mg/l; Adsorbent conc., 0.3 g/l; temp., 30 °C; contact time, 2 h
Fig. 7
The graphical representation of the effect of a adsorbent concentration, Pb(II) ion con., 300 mg/L, b contact time and initial adsorbate concentration on the adsorption capacity; Reaction conditions: Pb(II) ion con., 150 mg/L and 300 mg/L; Adsorbent conc., 0.3 g/L; pH, 5.5; temp., 30 °C
×
×
The combined effect of contact time and adsorbate concentration as presented in Fig. 7(b) shows a consistent increase in the amount of lead ion adsorbed as the adsorption time extends. Notably, the qe (mg/g) value appreciated significantly within the first 60 min at 150 mg/L and 300 mg/L Pb(II) ion concentration.
The observed variation in the qe (mg/g) value at varying initial concentrations is attributed to changes in concentration gradient within the bulk adsorbate phase [36]. At 300 mg/L adsorbate concentration, increased sorption driving force predominates due to the existence of a larger concentration gradient. This development ensures the complete saturation of the available PMPP active sites by the lead ions, thus resulting in higher adsorptive uptake per gram of adsorbent [37]. Similarly, the progressive increase in the qe (mg/g) value with the rise in contact time is attributed to improvement in surface area and porosity, as well as minimal pore diffusion resistance within the PMPP matrix sequel to their swelling in the adsorbate solution.
Adsorption isotherm modeling
Adsorption isotherms provide insight into the nature of adsorbate–adsorbent interaction within an adsorption system at equilibrium (dynamic balance in adsorbate and adsorbent concentration). The nature of these interactions is often informed from the associated isotherm model constants [38]. In this study, the experimental equilibrium data were fitted to four widely used isotherm models namely, Langmuir, Freundlich, Dubinin–Radushkevich, and Temkin as shown in Fig. 8. The equations of the adsorption isotherm models are presented Table 1. The error distribution between the data of the predicted isotherm models and the experimental data was minimized using error functions to determine the most accurate model of the obtained isothermal data. The variance between predicted isotherm data and experimental data was optimized using the solver add-in of Microsoft Excel. The common error functions used for optimization of the isotherm parameters are (Table 2): average percentage error (APE%), average relative error (ARE), a determinant of the quality of the fit (χ2), hybrid fractional error function (HYBRID), and normalized standard deviation (Δq%).
Fig. 8
Comparison between two-parameter isotherm models and experimental data (exp) obtained for adsorption on Pb(II) ions onto Pomegranate Peel at 30 °C; Reaction conditions: pH,5.5; adsorbent conc., 0.3 g/L; temp., 30 °C; time, 2 h
Table 1
Equations of two-parameter isotherm and adsorption kinetic models
The best adsorption isotherm was predicted by normalizing the error functions and finding the sum of normalized error (SNE). This procedure involves the division of all the error values obtained for the different error function models with the lowest error value and their subsequent summation to generate the minimum normalization error, SNE. Judging from the magnitude of the sum of normalized error values (SNE), all the studied models provided a good description of the experimental equilibrium data (Table 3). Detailed interpretation of the data fittings of the respective isotherm model in comparison with published literature is presented in subsequent subheadings.
Table 3
Isotherm model parameters
Langmuir
Freundlich
Temkin
D–R
qmax = 707.424
1/nF = 0.41
KT = 73.95
qD = 554.53
KL = 7.55
KF = 49.16
bT = 43.24
βD = 1.2E-04
RL = 0.011
R2 = 0.994
R2 = 0.940
R2 = 0.895
R2 = 0.999
SNE = 1.026
SNE = 1.013
E = 64.55
SNE = 1.059
SNE = 1.014
Bold indicates Sum of Normalized Error [SNE] value
Langmuir model
From the model-generated constants presented in Table 3, the Langmuir model depicted a reasonably low sum of normalized error (SNE) value, thus indicating a good model fit. A maximum adsorption capacity (qmax, mg/g) value of 600 mg/g was obtained at ambient temperature. This value is quite high and depicts a strong affinity between the lead ions and the PMPP due to the strong metal–ligand interaction with Pb(II) ion in aqueous solutions compared with divalent cations in addition to the presence of functional groups on the peels and small size of lead ion, which could favor for the accessibility of Pb(II) intercalation and diffusion more easily to the PMPP surface. Literature survey on the heavy metal adsorption application of raw pomegranate peel powder shows a relatively lower adsorption capacity (Table 4). Similarly, the KL(L/mg) constant which is related to the energy of adsorption was found to be 7.55 in this study. This value is synonymous with high associated adsorption energy (a likely chemisorption process). Comparatively, the KL values reported in the aforementioned pertinent literature were less than unity, except for the KL = 2.76 reported by Giri, et al. [13]. The dimensionless separation factor, RL, which is used to evaluate the feasibility and applicability of the process was found to be less than unity in the current study, as well as in the result presented by Salam, et al. [14] and Ben-Ali, et al. [19]. This finding is an indication of a favorable adsorption (since 0 < RL < 1).
Table 4
Maximum adsorption capacity reported in pertinent studies using raw Pomegranate peel powder
The Freundlich model depicted a good description of the experimental data judging from the low SNE value shown in Table 3. Also, the models’ dimensionless constant “n” quantifies the adsorbent–adsorbate bond energy. If 0 < 1/nF < 1, then a favorable adsorption process is postulated. Table 3 shows 1/nF-value that is less than unity. This result is in line with the 1/nF value of 0.30 [14], 0.40 [19], and 0.80 [21] reported during the adsorption removal of heavy metal using raw pomegranate peel powder. Similarly, the KF value, which quantifies the bond strength, was relatively high (KF = 49.16) and is in line with the value of 74.68 reported by Salam, et al. [14] during aqueous Cr(VI) adsorption onto pomegranate peel powder. Using similar adsorbents for heavy metal adsorption, Ben-Ali, et al. [19], and Mohammed, et al. [21] reported minimal bond strengths as expressed in much lower KF-values of 3.98 and 3.15, respectively.
Temkin model
From the model-generated constants presented in Table 3, the Temkin model satisfactorily predicted the isotherm data. The nature of the adsorption process in terms of heat energy distribution is captured in the sign convention of the model’s bT value. A positive value indicates an exothermic process, while a negative one is typical of an endothermic adsorption operation. From Table 2, a positive bT value was recorded in the study. Hence, the lead ions were adsorbed onto the PMPP sites, with the liberation of some latent adsorption energy (exothermic process). Thus, lead binding onto PMPP is a low-temperature operation. Salam, et al. [14] and Ben-Ali, et al. [19] reported lower but positive bT-values of 56.88 and 5.624 J mol−1 during the adsorption of Cr(VI) and Cu(II), respectively onto raw pomegranate peels powder.
Dubinin–Radushkevich (DR) model
This model is an important one due to its temperature dependence and the mean free energy, E (kJ/mol) term of the model. According to Aniagor, et al. [39], E (kJ/mol) defines the change in adsorption energy occurring when a mole of adsorbate migrates from the bulk fluid phase and attaches to the adsorbent surface. Consequently, the physical (physisorption) and the chemical (chemisorption) nature of an adsorption process is distinguished when E < 8 kJ/mol and E > 8 kJ/mol, respectively [40]. The E (kJ/mol) value obtained in this study (Table 2) suggests the existence of chemisorption. This conclusion was made earlier as informed from the Langmuir isotherm model analysis. Using similar raw pomegranate peel powder for Cr(VI) adsorption, Salam, et al. [14] reported an E (kJ/mol) value of less than 8.0 kJ/mol, thus a probable physi-sorption process. The study also noted an increase in the E (kJ/mol) values from 1.17 to 4.46 kJ/mol as the operating temperature appreciated from 303 to 323 K. Similarly, Ben-Ali, et al. [19] obtained E (kJ/mol) values in the range of 32.596 kJ/mol to 40.572 kJ/mol during the adsorption of Cu(II) onto raw pomegranate peel powder. Thus, a chemisorption interaction between the adsorbate and adsorbent was postulated.
Adsorption kinetics modeling
For the kinetics studies, four nonlinear models were utilized as shown in Fig. 9. The nonlinear equations of the adsorption kinetics models are presented in Table 1. Judging from the low SNE values depicted in Table 5, all the studied models provided a good description of the experimental kinetics data. The intra-particle diffusion model was best at predicting the kinetic data at adsorbate concentration of 150 mg/L, while the Elovich model emerged as the best fit at 300 mg/L concentration.
Fig. 9
Comparison between kinetic models and experimental data (exp) obtained for adsorption on Pb(II) ions onto Pomegranate Peel; Reaction conditions: Pb(II) ion con., 300 mg/L; Adsorbent conc., 0.3 g/L; pH, 5.5; temp., 30 °C
Table 5
Kinetic model parameters
Pseudo-first-order
Pseudo-second-order
Elovich
Intra-particle diffusion
Co = 150 mg/L
qe = 94.50
qe = 104.66
α = 32.696
Kid = 11.870
k1 = 0.039
k2 = 2.0E-04
β = 0.020
c = 83.658
R2 = 0.995
R2 = 0.996
R2 = 0.995
R2 = 0.974
SNE = 1.058
SNE = 1.095
SNE = 1.090
SNE = 1.056
Co = 300 mg/L
qe = 151.86
qe = 166.77
α = 30.048
Kid = 18.371
k1 = 0.040
k2 = 1.18E-04
β = 9.7E-03
c = 134.883
R2 = 0.998
R2 = 0.995
R2 = 0.990
R2 = 0.956
SNE = 1.111
SNE = 1.068
SNE = 1.029
SNE = 1.038
Bold indicates Sum of Normalized Error [SNE] value
qe.exp @ 150 mg/L = 129.60 mg/g
qe.exp @ 300 mg/L = 144.65
×
The Pseudo-first-order (PFO) model-generated constants, as presented in Table 5, shows a slight variation in the first-order rate constant (k1) with an increase in the initial adsorbate concentration. The same could not be said about the calculated adsorption capacity (qecal), as the value significantly increased as the initial concentration. A similar observation was made by Ben-Ali, et al. [19] and Ghaneian, et al. [20] during the application of raw pomegranate peel powder in heavy metal sorption, as they reported a slight and inconsistent variation in the k1 values with the increase in initial adsorbate concentration. The authors did not explain the observed data inconsistency. Similarly, the increment in the qe cal value (from the aforementioned studies) as a function of initial concentration increase was also irregular. Giri, et al. [13] reported a negative k1-value which is indicative of the poor fitting of the Pseudo-first-order model to the experimental kinetic data.
The Pseudo-second-order rate constant (PSO), k2 at 150 mg/L initial adsorbate concentration was found to be higher than the one recorded at 300 mg/L initial adsorbate concentration. Hence, the k2-value decreased with increasing adsorbate concentration. This could be due to the presence of adsorbent sites that is large enough to absorb all the available adsorbate molecules within the 150 mg/L adsorbate concentration system. With an increase in the initial adsorbate concentration, the adsorption rate constant value dropped slightly due to limited adsorption sites (since there was no corresponding increase in the adsorbent concentration). Studies by Ghaneian, et al. [20], and Salam, et al. [14] reported a consistent decrease in the k2 values with an increase in the initial adsorbate concentration, while Ben-Ali, et al. [19] observed inconsistency in the k2 values. The qe cal value obtained in this study was further found to consistently increase as the initial adsorbate concentration. This finding is in line with the variation in qe cal values reported by Ghaneian, et al. [20].
In the case of the Elovich model, minimal numerical differences were observed between the initial adsorption rate (α) and desorption constant (β) values at varying initial adsorbate concentrations. Incidentally, both constants decreased with increasing initial adsorbate concentration. The aforementioned explanation regarding adsorbent site depletion at higher adsorbate concentration (paragraph 2 of this section) still explains the decrease in the α value, with concentration increase from 150 mg/L to 300 mg/L. Also, the desorption rate expressed as the β values reduced due to initial concentration increase, as reflected in the improved adsorption capacity recorded at higher concentration in the case of Pseudo-first-order (PFO)and Pseudo-second-order (PSO) models. The Elovich model constants obtained by Ghaneian, et al. [20] followed the same trend as those reported in this study. The α- and β-values reported by other authors [19] varied inconsistently as the initial adsorbate concentration.
Regarding the intra-particle diffusion model, Table 5 shows an increase in the viscous drag occurring within the system with an increase in the initial adsorbate concentration. This is expressed in the magnitude of the boundary layer thickness (c values). Accordingly, the lower the c value, the weaker the viscous drag and vice versa. Hence, the c-value which increased from 83.66 (at 150 mg/L initial adsorbate concentration) to 134.88 (at 300 mg/L initial adsorbate concentration) implies an increase in the viscous drag. Despite the perceived drag, the intra-particle diffusion-controlled sorption rate (kid) was still more at 300 mg/L adsorbate concentration and also explains the higher adsorption capacity recorded in the case of Pseudo-first-order (PFO) and Pseudo-second-order (PSO) models at higher initial adsorbate concentrations.
Conclusion
Based on the conducted literature survey, only a few authors reported the lead adsorptive application of raw pomegranate peel powder (PMPP). Hence, this present research investigated the adsorptive potentials of raw pomegranate peel powder for the adsorption of aqueous lead pollutants. Experimental findings show the dependence of PMPP adsorption capacity on adsorbent concentration, contact time, and initial lead ion concentration. The adsorption process was studied over an extended 3 h period. However, the maximum lead ion uptake was attained within the first 60 min. Pomegranate peel powder showed a high affinity to adsorb lead ions. The experimental equilibrium data correlated well with the nonlinear forms of Langmuir, Freundlich, Temkin, and Dubinin–Radushkevich isotherms models. The Temkin model satisfactorily predicted the isotherm data. Similarly, effective kinetics data modeling and description were achieved using the Pseudo-first-order, Pseudo-second-order, Intra-particle diffusion, and Elovich models. The intra-particle diffusion model was best at predicting the kinetic data at adsorbate concentration of 150 mg/L, while the Elovich model emerged as the best fit at 300 mg/L concentration.
Declarations
Conflict of interests
The authors declare that they have no known competing financial interests or personal relationships that could have appeared to influence the work reported in this paper.
Ethical approval
“Not applicable”.
Open AccessThis article is licensed under a Creative Commons Attribution 4.0 International License, which permits use, sharing, adaptation, distribution and reproduction in any medium or format, as long as you give appropriate credit to the original author(s) and the source, provide a link to the Creative Commons licence, and indicate if changes were made. The images or other third party material in this article are included in the article's Creative Commons licence, unless indicated otherwise in a credit line to the material. If material is not included in the article's Creative Commons licence and your intended use is not permitted by statutory regulation or exceeds the permitted use, you will need to obtain permission directly from the copyright holder. To view a copy of this licence, visit http://creativecommons.org/licenses/by/4.0/.
Publisher's Note
Springer Nature remains neutral with regard to jurisdictional claims in published maps and institutional affiliations.
