- Research article
- Open Access
Guar gum-grafted poly(acrylonitrile)-templated silica xerogel: nanoengineered material for lead ion removal
© The Author(s). 2016
- Received: 12 May 2016
- Accepted: 1 November 2016
- Published: 16 November 2016
Polysaccharides are renewable biodegradable natural materials and are accounted for to control the formation of hybrid silica nanocomposites by sol gel process.
The synthesis of templated silica xerogel essentially includes two critical steps of hydrolysis and polycondensation reaction that are started by catalyst and silica precursor solution. Aside from this Saponification guar-graft-polyacrylonitrile (s-GG-g-PAN) as a copolymer are included in the precursor solution for providing a novel templating environment for silica matrix formation. The s-GG-g-PAN acts as a template for the silica produced in the blended framework because of the hydrogen bonding between the hydroxyl groups at silanols and hydroxyl group and carbonyl groups at the copolymer surface. Connected silanol groups can further hydrolyze and after that take part in the condensation reaction. Accordingly, the s-GG-g-PAN template gets trapped inside the resulting silica system, which on calcining at 900 °C is lost, producing pores of shape and size of the template.
The surface area and pore volume of the developed templated silica xerogel have been determined. The surface area and pore volume of the template silica xerogel (H900) were observed to be (240 m2 g−1) and (0.286 ccg−1) respectively. The conditions for the adsorption by adsorbent had been enhanced, and kinetics and thermodynamic studies were performed. The best result in terms of lead adsorption was obtained with templated silica xerogel calcined at 900 °C. The % Pb2+ removal is observed to be 96% when H900 adsorbent was treated under ideal adsorption states of measurements 0.05g dose, 500mgL−1 Pb2+ concentration, time 2 h, pH 5 at 30 °C. The adsorption information fitted satisfactorily to Langmuir isotherms, showing unilayer adsorption. In view of the Langmuir model, Qmax was calculated to be 2000 mgg−1. Theadsorption demonstrated pseudo-second-order kinetics. The thermodynamic study revealed the endothermic and spontaneous nature of the adsorption. The adsorbent demonstrated good thermal stability and high reusability.
The present study highlights the possibility of silica xerogel derived from saponified guar gum-grafted poly (acrylonitrile) toward its potential application as superior adsorbent for removal of Pb2+ from aqueous solution.
- Guar gum
- Organic-inorganic nanocomposite
- Templated xerogel
- Environmental pollution
- Lead ion removal
Prolonged exposure to heavy metals such as cadmium, copper, lead, nickel, and zinc can cause deleterious health effects in humans (Harrison and Laxen 1981). Lead is one of the heavy metal that is non-essential and occurs naturally in the earth. Today, the potential sources of lead exposure in the drinking water are through leaching from lead-containing pipes, stockpiling batteries, lead purifying, tetraethyl lead assembling, mining, electroplating, ammunition, textiles, printing, painting, metal preparing, and the fired glass commercial enterprises (Schneegurt et al. 2001; Googerdchian et al. 2012). Lead poisoning is a type of metal poisoning caused by lead in the body. Exposure to lead can occur in contaminated air, water, dust, food, or consumer products. In any case, lead in drinking water can likewise bring about an assortment of antagonistic health impacts. The required Occupational Safety and Health Administration (OSHA) Permissible Exposure Limit (PEL) action level for lead in general industry and the construction industry is a time-weighted average (TWA) of 30 μg/m3 over 8-h. The US Environmental Protection Agency (EPA) final rule establishes an action level which is set at 15 μgL−1. Young children are particularly vulnerable to the toxic effects of lead and can suffer profound and permanent adverse health effects; particularly, it causes moderated development of the brain, learning issues, debilitated hearing, conduct issues (for example, hyperactivity), nerve and/or mind harm, extreme lethargies, and even demise. Lead can even create nephrotoxicity, neurotoxicity, circulatory strain, and unfriendly consequences for the hematological and cardiovascular systems in adult (Harrison and Laxen 1981; Hua et al. 2012).
The high lethality of Pb ions can bring about genuine biological harm; hence, there is a need to create procedures to wipe out or possibly to extraordinarily reduce the concentration in wastewater preceding discharge into the environment These days, various strategies have been proposed for productive heavy metal removal from wastewaters, including reverse osmosis, ion exchange, electrochemical, evaporation, chemical precipitation, flocculation, and chelation. Frequently, these strategies have high reagent necessities, create secondary pollutants, or are basically wasteful and especially oblige high cost in removing harmful metal ions in trace quantities from solutions (Fu and Wang 2011; Ghorai et al. 2012). Overall the different techniques, adsorption has been perceived as a standout amongst the most economical and effective systems for the removal of the lead from aqueous media because of adaptability in outline and operation, low upkeep expense, and high effectiveness (Mishra et al. 1996). Hence, the adsorption procedure has arrived at the cutting edge as one of the real systems for heavy metal removal from water/wastewater.
The human development has been grouped by paramount material on which the modern innovation is based on the Stone Age, the Iron Age, and now the Polymer Age. This age is properly called the polymer age because of broad utilization of polymers in all domains of life like sensors, water purification, antimicrobial activities, and catalysis (Pandey 2016; Pandey et al. 2013; Pandey et al. 2012; Pandey and Nanda 2016; Pandey and Nanda 2013; Pandey and Ramontja 2016c; Pandey and Ramontja 2016d; Pandey and Mishra 2014; Pandey and Mishra 2013; Pandey and Mishra 2011a, b, c; Singh et al. 2011a, 2011b; Singh et al. 2010a; Singh et al. 2007a; Singh et al. 2007b; Singh et al. 2006). Superparamagnetic nanocomposite of sodium alginate supported tetrasodium thiacalixarene tetrasulfonate (Fe3O4@TSTCAS-s-SA) (Lakouraj et al. 2014); biodegradable cyclodextrin-based gel (CAM) (Huang et al. 2013); Phanerochaete chryosporium immobilized in alginate gel beads (Arıca et al. 2003); magnetic chitosan hydrogel beads (m-CS/PVA/CCNFs) (Zhou et al. 2014); chitosan-g-poly(acrylic acid)/attapulgite/sodium humate (CTS-g-PAA/APT/SH) composite hydrogels (Zhang and Wang 2010); poly(acrylamide)-grafted iron(III) oxide (Pan et al. 2009); Sargassum sp., Ulva sp., and Padina sp., (Sheng et al. 2004); modified orange peel (Feng et al. 2011); palygorskite mud (Chen and Wang 2007); mesoporous silicates (Oshima et al. 2006); and Turkish lignite (Pehlivan and Arslan 2007) have been considered for the removal of the Pb2+ from aqueous solutions.
Commercial polysaccharides can be utilized as sorbents, yet their solvency in water restricts their applications as an adsorbent. Modification of humic acid with silica results in the adsorption of Pb2+, Cu2+, and Cd2+ (Siliva et al. 2008). Mesoporous organosilicas prepared by direct co-condensation of TEOS (tetraethyl orthosilicate) and other mixed organosilanes, namely, tris[3-(trimethoxysilyl)-propyl]isocyanurate, bis[3(triethoxysilyl)propyl]tetrasulfide, N-(3-triethoxysilylpropyl) 4,5-dihydroimidazole, and ureidopropyltrimethoxysilane, have great potential for Hg2+ adsorption (Olkhovyk and Jaroniec 2007). Consequently, the improvement of sol-gel inferred materials with custom-made porosity is an objective in the field of adsorbents and separation media (Pandey and Mishra 2011a).
Templated mesoporous solids can promptly be arranged with organic functionalities coating the silicate structure by co-condensation of TEOS during synthesis and resulting removal of the template. Mesoporous silicates can be union by surfactant (Yang et al. 2008; Tao et al. 2003) or polymer templating routes (Wan and Zhao 2007; Feng et al. 2000). Aside from this, there are certain surfactants, which are known to be toxic to creatures, biological communities, and people, and can build the dispersion of other ecological contaminants. Nowadays, lion’s share of the polymers which are utilized for templating is petrochemical based and costly, and their removal from silica system is troublesome; also, they are not eco-friendly. Polysaccharides are renewable biodegradable natural materials (Goldstein et al. 1973) and are accounted for to control the formation of hybrid silica nanocomposites by the strategy for sol-gel (Shchipunov and Tat’yana 2004; Shchipunov et al. 2005; Shchipunov 2003), and their removal from the hybrid can be influenced under less drastic conditions when contrasted with the synthetic polymers. A few polysaccharides have been utilized for the synthesis of hybrid materials. But xerogel from the removal of the template from such hybrids and their act as adsorbent has not got much consideration yet. Couple of years back, we had reported novel nanocomposites of vinyl-modified guar gum and silica with amazing capacity to bind Zn2+ (Singh et al. 2008) and Cd2+ (Singh et al. 2009a), where saponified poly(acrylonitrile)-modified guar gum- and poly(acrylamide)-grafted guar were utilized as templates, respectively.
In the present article, we have performed the application of Pb2+ removal by s-GG-g-PAN-silica hybrids (templated silica xerogel). The xerogel obtained by the thermal curing of the templated silica xerogel will be assessed as an adsorbent in the removal of heavy metal ions, Pb2+ from aqueous solution. Near assessment of the s-GG-g-PAN-templated xerogel with blank xerogel (non-templated xerogel) synthesis under comparative conditions by dehydration condensation of TEOS in absence of the template has been undertaken.
Tetraethylorthosilicate Si(OC2H5)4 (98%) were purchased from Sigma-Aldrich. Ammonia solution (30%) NH4OH, guar gum (GG), acrylonitrile (CH2CHCN), ascorbic acid (C6H8O6), potassium persulfate (K2S2O8), N,N-dimethylformamide ((CH3)2NCH), sodium hydroxide (NaOH), hydrochloric acid (HCl), lead(II) nitrate (Pb(NO3)2), methanol (CH3OH), and ethanol (C2H5OH) solution were bought from Merck (South Africa) and utilized without further purification.
The powder X-ray diffraction patterns of biopolymer (guar gum) and templated xerogel (H900) nanocomposite samples were performed by using XRD (Rigaku Ultima IV, X-ray diffractometer, Japan) and were done by employing Cu Ka radiation of the wavelength of 1.5406 Å with visible lights at 45 kV/40 mA. The surface morphology of the templated xerogel (H900) nanocomposite and Pb2+-loaded templated xerogel (H900) nanocomposite was examined by a scanning electron microscopy (SEM) (TESCAN VEGA, Czech Republic) under a 20-kV electron acceleration voltage coupled with energy dispersive (EDS) for elemental examination. Powdering of the nanocomposite was performed by Fritsch Analysette 3 Spartan pulverisette 0 Vibratory Sieve Shaker/Mill (Germany). The concentrations of heavy metal (Pb2+) under study were determined by the atomic absorption technique type AA-6800, Shimadzu, Japan.
Preparation of the functionalized biopolymer by grafting
Guar gum-grafted poly(acrylonitrile) (GG-g-PAN) of 25% grafting can be achieved by following the method and parameter, where GG (2.0 g) was taken with acrylonitrile (8.8 × 10−2 M) and ascorbic acid (2.3 × 10−2 M) in 500 mL water in a 1-L flask and thermostated at (35 ± 0.2) °C. After 30 min, a known amount of potassium persulfate (20 × 10−3 M) was included. The total volume of the reaction mixture was kept constant to 500 mL, and grafting was allowed for 1 h. GG-g-PAN was separated from poly(acrylonitrile) by pouring the reaction mixture into a large quantity of DMF (Singh et al. 2008).
Saponification of the guar-grafted poly(acrylonitrile) (s-GG-g-PAN)
GG-g-PAN sample with 25% G was saponified in aqueous alkali for making silica composites. Grafted samples (2 g) were homogeneously dissolved in 1% NaOH at 100 °C for 1.5 h. After hydrolysis, the samples (s-GG-g-PAN) were precipitated in 600 mL methanol. Finally, s-GG-g-PAN was washed with methanol (CH3OH) and ethanol (C2H5OH) solution two to three times and then dried and weighed (Singh et al. 2008). The partial basic hydrolysis of 1.5 h is performed in order to increase the functionality such as –CONH2 and –COOH in the copolymer.
Synthesis of composites: s-GG-g-PAN-silica hybrids (templated silica xerogel)
The synthesis and characterization of s-GG-g-PAN-silica hybrids (templated silica xerogel) had already been published before by our group (Singh et al. 2008). The s-GG-g-PAN (1.0 g) was dissolved in 10 mL of distilled water. Independently, TEOS (2.5 mL) was likewise dissolved in ethanol (2.5 mL). A third solution incorporating 1.75 mL of 12 N ammonium hydroxide was prepared independently. A short time later, all the three solutions were emptied together into a reaction glass flask and kept under tender blending for more than 18 h at room temperature to develop monodisperse SiO2 particles inside of the biopolymer/modified biopolymer medium. The following blend was then dissipated in air at 40 °C (3 h), 60 °C (4 h), 70 °C (2 h), and 80 °C for 2 h until a dry material s-GG-g-PAN-silica hybrids (templated silica xerogel) was acquired (H1). H1 was further calcinated in air at 250, 500, and 900 °C (for 3 h at every temperature inside a muffle furnace) to obtained templated silica xerogel H250, H500, and H900, respectively.
Preparation of silica (non-templated silica xerogel)
The method for the synthesis of non-templated silica xerogel is similar to templated silica xerogel, but non-templated silica xerogel is prepared in absence of template (s-GG-g-PAN) and designated as S80. The synthesis S80 was also calcinated in air at 250, 500, and 900 °C (for 3 h at each temperature inside a muffle furnace) to obtain non-templated silica xerogel S250, S500, and S900, respectively.
Metal ion removal experiments
Pb2+ sorption investigations were performed by the batch method. Stock solutions of 1000 mgL−1 of standardized Pb2+ were prepared from lead salt in DI (deionized) water. Adsorption examinations were carried out using the templated silica xerogel (H900) as adsorbent on a temperature controlled incubator shaker set at 120 rpm (revolutions per minute) kept up at 30 °C for 2 h. Here, known measure of adsorbent was completely mixed with 50 mL of individual Pb2+ solutions, whose concentrations and pHs were beforehand known. As we realize that pH assumes a vital part in metal ion binding, thus, pH of the reaction mixture was initially adjusted using either HCl or NaOH (1 M). The pH measurements were made with OHAUS starter 2100 (USA). After the flask was shaken for the desired time, the suspensions were filtered through Whatman 0.45 mm filter paper and the filtrates after suitable dilutions were analyzed for Pb2+ concentration utilizing using atomic absorption spectrophotometer (AAS) at 217 nm utilizing a slit width of 1 nm. Control tests demonstrated that no sorption occurred on either glass or filtration frameworks. All the adsorption examination was performed in triplicate, and there average was reported. For enhancing the adsorption, one parameter was change at a time, keeping all the other parameters constant.
Thirty milliliters of the various background electrolytes (KCl, KNO3, K2SO4) in three concentrations of 0.1, 0.01, and 0.001 mol L−1 containing 500 mg L−1 Pb2+ were separately added to 0.05 g of adsorbent. The pH of these solutions was not adjusted to avoid negating the pH effects of the electrolytes. These solutions were agitated in an orbital shaker for 2 h, 120 rpm, and at 30 °C. The supernatants collected were analyzed for Pb2+.
In order to determine the reusability of the templated silica xerogel (H900) adsorbent, Pb2+ was stripped off from the used adsorbent using H2SO4 and reused. To optimize the concentration of the acid required for the quantitative stripping of the loaded Pb2+, experiments were carried out with varying concentrations of H2SO4 ranging from 0.001 to 1 M, where efficient desorption could be achieved using 0.01 N H2SO4 in 2 h. Templated silica xerogel (H900) adsorbent (50 mg) was placed in the 25 mL of 0.01 N H2SO4, stirred at 100 rpm for 2 h at 30 °C, centrifuged, and dried.
To examine the impact of calcination, H1 was calcinated in air at 250, 500, and 900 °C (for 3 h at every temperature inside a muffle furnace) to obtained templated silica xerogel H250, H500, and H900, separately, and they were tested for Pb2+ removal (Additional file 1: Table S1). Additional file 1: Table S1 demonstrates that the adsorption of Pb2+ takes after the order: H900 > H500 > H250 > H80 > S900. The H900 having most extreme binding is indicated to have the high surface area (240 m2g−1) and the pore volume (0.286 ccg−1) supporting its sorption capacity. The binding additionally relies on the extraordinary shapes of this mesopore, which are dictated by packing mode and by the size distribution of the constituent particles (Yang et al. 2007). The porosity present in the adsorbent has all the earmarks of being basically in charge of the adsorption, where the pore size is confined by the copolymer template like perception in Zn2+ removal. It was likewise delineated from the outcome that the calcining of xerogel at different temperature results in a critical impact on the physical attributes and thus on the adsorption properties of the composites.
Surface parameters of the templated silica xerogel (H80, H900) and non-templated silica xerogel (S80, S900)
BET surface area (m2 g−1)
BJH pore volume (cm3 g−1)
Templated silica xerogel (H80)
Templated silica xerogel (H900)
Silica xerogel (S80)
Silica xerogel (S900)
Optimization of Pb2+ removal
Since the greatest Pb2+ binding was observed for templated silica xerogel (H900), adsorption was further upgraded with templated silica xerogel (H900) by varying one adsorption parameter at a time keeping all the others fixed.
Effect of pH on Pb2+ adsorption
In aqueous solutions of pH under 6, Pb2+ ions exist as either Pb2+ or Pb(OH)+ or both. However, the formation of Pb2+ hydrolysis products begins to happen at pH values somewhere around 6 and 7, and this achieves insoluble precipitation of Pb(OH)2, Pb(OH)3 −, and Pb(OH)4 2−. Possibly, templated silica xerogel (H900) may carry on as negatively charged surface. These are in charge of improved adsorption of positively charged Pb2+ and Pb(OH)+ through electrostatic interaction and surface complexation model at higher pH (Pretorius and Linder 2001).
The equilibrium pH (pHe) values were marginally higher than initial pH at pH = 1–5 (Additional file 1: Table S3). This is an aftereffect of competition between Pb2+ ions and H3O+ for binding sites. So in templated silica xerogel, negatively charge surface-bound hydroxyl groups get to be accessible to heavy metal ions for coordination. Low pH of solution expands H3O+ concentration and strengthens the competition between H3O+ and heavy metal ions for complexation sites. Be that as it may, at pH ≥6.0, the q e estimations of Pb2+ diminished with an increment of pH, inferable from the interaction between OH− and Pb2+ ions in the solution to form Pb(OH)2. This reveals that adsorption of heavy metals on templated silica xerogel was complexation, in particular non-stoichiometric, as opposed to ion-exchange adsorption mode. Thus, adsorption mechanisms of heavy metals by templated silica xerogel are may be possibly because of complexation between heavy metal ions and templated silica xerogel fundamentally at pH = 1–5 and hydrolysis adsorption and surface micro-precipitation at pH = 6–7 as per literature. It was clearly affirmed from researchers (Escudero et al. 2013), who have reported the quantitative chemical examination of Pb (dissolved and precipitated). The author has depicted the Pb broke down and Pb accelerated are 97.3 and 2.7% separately at pH 5, 1.9 and 98.1% at pH 8, and 0 and 100% at pH 11 from 40 mgL−1 of lead solution. Therefore, it affirms there is irrelevant or no precipitation at pH 5.
Effect of adsorbent dose
The removal of Pb2+ increases from 170 to 482 mgL−1 by expanding the adsorbent dose from 15 to 75 mg in 50 mL of 500 mgL−1 initial Pb2+ concentration at 30 °C, rpm 120, contact time 2 h, and pH 5. This increase is because at the higher dose of adsorbent, more binding sites are available due to increased surface area (Fig. 5b).
Effect of Pb2+ concentration
Effect of Pb2+ concentration studies were carried out by taking concentration in the range 500 to 2300 mg L−1 at temperature 30 °C (Fig. 5c). It was observed that increase in the adsorption is sharp initially followed by slow increase leading to saturation. Initially due to more availability of Pb2+, adsorption increases which later on after the saturation of the adsorption sites at the adsorbent, adsorption gradually decreases.
Effect of ionic nature and strength on Pb2+ adsorption
The vicinity of salts may meddle with the lead adsorption. The effect of inorganic anion on the adsorption of Pb2+ onto templated silica xerogel (H900) was studied. It was observed that more Pb was adsorbed in the presence of SO4 2− whereas NO3 − and Cl− gave almost equal Pb adsorption. Notwithstanding, the Pb adsorption rate of H900 was diminished in the presence of Cl− and NO3 − compared to SO4 2−. There was a stronger attraction between Pb2+ and the adsorbent in the vicinity of SO4 2− than alternate anions which indicate almost equal attraction. Increasing the ionic strength of the anions (from 0.001 to 0.1 mol L−1) influenced the adsorption of lead. In the vicinity of SO4 2−, Pb adsorption increased with increasing ionic strength but the reverse was the case in the presence of Cl− and NO3 −. In the vicinity of anions, the distribution coefficient (Kd) values decreased with increase in ionic strength aside from SO4 2−. At ionic strength of 0.001 mol L−1, SO4 2−, Cl−, and NO3 − were 487.5, 480, and 477.5 mgL−1 in H900 adsorbent, respectively, while at 0.01 mol L−1, SO4 2−, Cl−, and NO3 − were 493.5, 445, and 442 mgL−1 in H900 adsorbent, respectively (Fig. 2d), and at 0.1 mol L−1, SO4 2−, Cl−, and NO3 − were 495, 397.5, and 395 mgL−1 in H900 adsorbent, respectively (Fig. 5d). Thus, we can say that in the % adsorption of Pb2+ at 0.1 mol L−1, SO4 2−, Cl−, and NO3 − were 99, 79.5, and 79% in templated silica xerogel (H900) adsorbent, respectively. It demonstrated that increasing the ionic strength of SO4 2− increased the affinity of Pb2+ for H900 adsorbent, while increased the affinity of Cl− and NO3 − decreased the affinity of Pb2+ for templated silica xerogel (H900) adsorbent.
Effect of temperature
The effect of temperature on the adsorption was studied in the range 10–70 °C at the initial concentration of Pb2+ 500 mgL−1, rpm 120, contact time 2 h, and pH 5. It was observed that initial increment in the adsorption with the increment in the temperature from 10 to 30 °C demonstrates that adsorption is endothermic nature (Fig. 5e). However, at the temperature more noteworthy than 30 °C, a slight decrease in adsorption was observed from 40 to 70 °C. The adsorption decreases from 96 to 88.4% with an increase in temperature from 30 to 70 °C. As we know that the physical adsorption decreases with increasing temperature, and chemical adsorption increases as the temperature increases, in solution, the molecule or adsorbate is not free like in the gas phase; it is surrounded by solvent molecules. Such molecules to be adsorbed on a surface or in a cage (silica) should break its interaction with solvent molecules; it requires energy (endothermic process). In such a case, there is the possibility that the energy required to break interactions with the solvent be higher than the energy released during its adsorption on the surface. In such a case, adsorption is favored with temperature and the whole process be endothermic (favored with temperature). While the possible reason for the decrease in adsorption at certain temperature may be because if temperatures are high and are capable of initiating a back reaction from the chemisorbed state, chemisorption will as well drop by increasing temperature. This is the case if your chemisorption process involves a covalent-reversible reaction. Basically, the elevated temperature makes the chemisorption (in a whole) a physisorption process.
Adsorption isotherm studies
Adsorption isotherms are helpful to advance the attempt of templated silica xerogel (H900) as an adsorbent. Therefore, exact comparisons are important for adsorption information understanding and expectations. The accompanying articulations of a straight line were utilized and found by method for scientific transformation of isotherms.
For Langmuir isotherm
For Freundlich isotherm
For Temkin isotherm
The equilibrium information best fitted to Langmuir model than Freundlich and Temkin models demonstrating surface homogeneity of the adsorbent and unilayer adsorption. Similar results have been observed in the adsorption of Cd2+ on Cassia Grandis seed gum-grafted poly(acrylamide)-silica hybrid (Singh et al. 2015), activated Eskom fly ash/chitosan composite (Pandey and Tiwari 2015), starch/silica nanocomposite (Singh et al. 2011a, 2011b) and adsorption of Cr6+ onto guar gum-grafted poly(methylacrylate) (Singh et al. 2009b).
Langmuir, Freundlich, and Temkin constants at 30 and 15 °C
Adsorption isotherm model
A T (Lg−1)
While Temkin plotted at two diverse temperature 15 and 30 °C as demonstrated in (Fig. 6e, f), the accompanying values were evaluated: A T = 7.134 Lg−1 and B = 395 Jmol−1 and A T = 3.9439 Lg−1 and B = 347 Jmol−1 at 15 and 30 °C separately, which is a sign of the heat of sorption showing a physical adsorption process.
Linear plots of log(q e − q t ) versus t, t/qt versus t, and 1/(q e − q t ) versus t were indicated in Fig. 7a–c. The K L , K′, and K 2 values from the slopes and intercepts are 1.543 × 10−2/min (R 2 = 0.962), 2.85 × 10−4gmg−1 min−1 (R 2 = 0.999), and 3.8 × 10−4 gmg−1min−1 (R 2 = 0.962), respectively, at 500 mgL−1 Pb2+. The pseudo-second-order reaction rate model demonstrates satisfactorily the depicted kinetics of sorption of lead with high correlation coefficient (R 2 = 0.999). Similar results have been observed in the adsorption of metal ions (Pandey and Ramontja 2016a) and dyes (Pandey and Ramontja 2016b) on different adsorbents.
Kinetics was performed at three diverse Pb2+ concentrations and the R 2 values and the rate constants for all the three models are recorded in Additional file 1: Table S4, showing that rate of adsorption was higher at 500 mgL−1 Pb2+ concentration.
Regeneration of saturated adsorbents
For pragmatic application, the reusing and recovery of the adsorbent is essential. As a result of their insoluble nature of xerogel, the collection of Pb2+-adsorbed templated silica xerogel (H900) was simple and quick. We treated it with 0.01 N H2SO4 solution which analyzed the concentration of Pb2+ ions desorbed to the solution by AAS. To make the sorbent economically competitive, the readied adsorbent ought to be reused for number of cycles. Ninety-six percent of the Pb2+ was uprooted in the first cycle. Adsorbed Pb2+ could be stripped by the presentation of protons that contended with metal ions for binding site. The utilized composite was treated with 0.01 N H2SO4 which brought about to 93.6% stripping of Pb2+. The adsorption capacity was totally continued after the recovery of acid-treated sorbent. In the second cycle, the material could now remove 95.4% Pb2+ that could be desorbed up to 94%. In the third cycle, 96.4% adsorption and 92.6% desorption were conceivable (Fig. 7d). The removal decreases ostensibly per cycle up to the seventh cycle recommending high proficiency of the adsorbent. In the last cycle, 77% adsorption was achievable.
It is fascinating to find that the structure of mesoporous templated silica xerogel (H900) could keep well amid the reuse tests with no change, even under persistent mechanical disturbance with mechanical agitation of 120 rpm and mixing time of 21 h. This affirms the stability of our adsorbent.
Thermodynamic parameters of the adsorption by templated silica xerogel (H900)
ΔG 0 (kJmol−1)
ΔH 0 (kJmol−1)
ΔS 0 (Jmol−1)
Comparative list of the maximum sorption capacity (Q max) for Pb2+ sorption of templated silica xerogel (H900) by different adsorbent reported in the literature
Conc. range (mgL−1)
Pb2+ Qmax (mgg−1)
Sodium alginate supported tetrasodium thiacalixarene tetrasulfonate (TSTCAS-s-SA) nanogel
(Lakouraj et al. 2014).
Superparamagnetic nanocomposite of sodium alginate (Fe3O4@TSTCAS-s-SA)
Biodegradable cyclodextrin-based gel (CAM)
(Huang et al. 2013).
Phanerochaete chryosporium immobilized in alginate gel beads live
(Arıca et al. 2003).
Immobilized spore containing alginate beads (heat inactivated fungus)
(Chen and Wang 2007)
(Pandey and Mishra 2012)
Magnetic chitosan hydrogel beads (m-CS/PVA/CCNFs)
(Zhou et al. 2014).
Chitosan entrapped in poly(acrylamide)
(Akkaya and Ulusoy 2008)
Chitosan-g-poly(acrylic acid)/attapulgite/sodium humate (CTS-g-PAA/APT/SH) composite hydrogels
(Zhang and Wang 2010)
Poly(acrylic acid) crosslinked by N,N′-methylenebisacrylamide/montmorillonite
(Bulut et al. 2009)
Templated silica xerogel (H900)
s-GG-g-PAN templating produces novel groups of intriguing porous solids displaying a regular mesostructure alongside high-specific surface areas, thermal and mechanical stability, exceptionally uniform pore distribution, and tunable pore size. Pb2+-binding capacity of the templated silica xerogel could be controlled by calcinations in air. The kinetics of the adsorption procedure was obtained by a pseudo-second-order model. The adsorption isotherm information fit better to the Langmuir adsorption isotherm, and the most extreme monolayer capacity of the adsorbent was observed to be 2000 mgg−1 at 30 °C. The particular surface area and pore volume of the templated silica xerogel (H900) were observed to be (240 m2 g−1) and (0.286 ccg−1), respectively. The % Pb2+ removal is observed to be 96% when H900 adsorbent was treated under ideal adsorption states of measurements 0.05 g dose, 500 mgL−1 Pb2+ concentration, time 2 h, and pH 5 at 30 °C. The 77% adsorption was achievable in the seventh cycle which shows the good recyclability of adsorbent.
The corresponding author is grateful to National Research foundation (NRF), South Africa (Grant No. 91399) for its liberal financial support. The authors also acknowledge University of Johannesburg (UJ) (South Africa) for the Lab and instrumentation facilities and UJ Online Library Services.
SP contributed to the experimental design, experimental work, analysis results, and writing. Both SP and JR contributed to the discussion and proofing and approved the final manuscript.
The authors declare that they have no competing interests.
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