Synthesis of Quercetin Loaded Nanoparticles Based on Alginate for Pb(II) Adsorption in Aqueous Solution
© Qi et al. 2015
Received: 16 July 2015
Accepted: 12 October 2015
Published: 17 October 2015
Pb(II) is a representative heavy metal in industrial wastewater, which may frequently cause serious hazard to living organisms. In this study, comparative studies between alginate nanoparticles (AN) and quercetin-decorated alginate nanoparticles (Q-AN) were investigated for Pb(II) ion adsorption. Characterization of AN and Q-AN were analysed by transmission electron microscopy (TEM), Fourier transform infrared spectrometry (FT-IR), X-ray diffractometer (XRD), and thermogravimetric analysis (TG-DTG-DSC). The main operating conditions such as pH, initial concentration of Pb(II), and co-existing metal ions were also investigated using a batch experiment. AN and Q-AN, with a diameter of 95.06 and 58.23 nm, were constituted by many small primary nanoparticles. It revealed that when initial concentration of Pb(II) is between 250 and 1250 mg L−1, the adsorption rate and equilibrium adsorption were increased with the increase of pH from 2 to 7. The maximum adsorption capacities of 147.02 and 140.37 mg L−1 were achieved by AN and Q-AN, respectively, with 0.2 g adsorbents in 1000 mg L−1 Pb(II) at pH 7. The adsorption rate of Pb(II) was little influenced by the co-existing metal ions, such as Mn(II), Co(II), and Cd(II). Desorption experiments showed that Q-AN possessed a higher desorption rate than AN, which were 90.07 and 83.26 %, respectively. AN and Q-AN would probably be applied as adsorbents to remove Pb(II) and then recover it from wastewater for the advantages of simple preparation, high adsorption capacity, and recyclability.
KeywordsPb(II) Alginate Quercetin Nanoparticles Adsorption
The unique nature of lead (Pb), high malleability, low melting point, and strong resistance to corrosion, provides its widespread application in various industries . The major sources of anthropogenic Pb are the wastewaters from battery manufacturing, electroplating industry, mining activity, and combustion of automobile petrol [2, 3]. Pb(II) has access to human body through inhalation and ingestion in different ways such as contaminated air and water, soil, and food. Accumulation of lead produces damaging effects in peripheral and central nervous systems, kidneys, and blood pressure. If exposures exceed tolerable levels, lead is dangerous to individuals of any age, while fetuses and young children are the most vulnerable members. Based on the Substance Priority List of Agency for Toxic Substances and Disease Registry (ATSDR) 2013 Substance Priority List, Pb(II) is the top 2 hazardous material of environmental concern with high frequency, persistency, and toxicity [4, 5]. The methods have been applied for Pb(II) removal in contaminated water mainly including chemical precipitation, electrochemical reduction, ion-exchange, membrane separation, and sorption [6, 7]. Among these technologies, adsorption is one of the economic and efficient methods for removal of heavy metal from wastewaters. Nanomaterials have extremely small size and high surface area to volume ratio that provided immense scope and opportunities for water decontamination [8, 9].
Sodium alginate is a relatively economical biopolymer with compositions of α-1, 4-l-glucuronic acid (G units) and poly-β-1, 4-d-mannuronic acid (M units) which can provide rich ester groups (–COO−) for adsorbing cation [10–12]. Recently, nano alginate materials have attracted significant attentions in the area of heavy metal adsorption [13–15]. When exposed to aqueous calcium ion, sodium alginate will form a three-dimensional gel network, which is essential for adsorption .
Quercetin is a naturally-derived polyhydroxy (3, 3', 4', 5, 7-OH) compound, which can form complexes with many metal cations. It is presumed the hydroxyls on quercetin may enhance the adsorption capability of alginate. Besides, we have reported a microcapsule system based on alginate for Cr(VI) removal in our previous research . And the size of the microcapsule is about 200 μm. Considering that small particles (<1 μm) have a larger specific surface area and a higher mechanical strength, it is significant to prepare alginate particles in nanometer. An approach of alginate-in-water (W/O) nano-emulsions coupled with external gelation will be applied to prepare nanoparticles. The present work is aimed at the design of both uniformly sized alginate nanoparticles (AN) and quercetin-decorated alginate nanoparticles (Q-AN) for Pb(II) removal. Batch adsorption experiments were conducted to investigate the removal of Pb(II) from aqueous solution by both AN and Q-AN. The effect of parameters such as solution pH, initial Pb(II) concentration, and co-existing metal ions was studied.
Sodium alginate (low viscosity, 4–12 cP), Span 80, and Tween 80 were provided by Sigma-Aldrich Co. (St. Louis, USA). Quercetin was supplied by Sangon Biotech, Co., Ltd. (Shanghai, China). Lead nitrate (Pb(NO3)2), manganous nitrate (Mn(NO3)2), cobaltous nitrate (Co(NO3)2), and cadmium(II) nitrate (Cd(NO3)2) were purchased from Aladdin Industrial Corporation (Shanghai, China). All remaining chemicals used in this study were analytical grade or ACS grade. All solutions were prepared with ultrapure water.
Preparation of AN and Q-AN
Preparation of AN
The AN in aqueous phase of W/O nano-emulsions were prepared by following procedure. (1) 1.05 mL Span 80 and 0.45 mL Tween 80 were added into 150 mL liquid paraffin (HLB = 7.5) in a 500-mL three-necked flask while stirring with a mechanical stirring speed of 500 rpm at a constant temperature of 40 °C for 30 min. (2) To obtain small-sized alginate nanoparticles, the stirring speed was increased to 1000 rpm. 45 mL of 0.50 % (v/w) alginate was dropped into above liquid paraffin at a rate of 1 mL 6 min−1. The solution was then stirred at the same temperature for 60 min. (3) CaCl2 (0.10 %) (v/w) prepared with 60 % (v/v) ethanol was dropped into the above mixture at a rate of 1 mL 6 min−1. Keep stirring for another 60 min. Then, the alginate nano-emulsions was transferred into Eppendorf tubes, centrifuged at 3800 r min−1 for 10 min, and then left for equilibration at 25 °C. The upper phase (oil of surfactant or reverse micelles) of the phase-separated samples was discarded, whereas the lower phase containing alginate nanoparticles was collected . (4) An equal volume of ethyl ether was added into alginate nanoparticles and vibrated gently. And the upper phase (solution of ethyl ether and residual liquid paraffin) was removed. Purge lower phase with nitrogen gas to replace ethyl ether. The obtained alginate nanoparticles were filtrated with a 0.22-μm membrane filter and lyophilized or kept in a refrigerator until further investigation.
Preparation of Q-AN
The procedure of Q-AN preparation was similar to that of AN except an addition of 0.0675 g quercetin into 45 mL of 0.50 %(v/w) alginate.
Samples for the transmission electron microscopy (TEM; JEOL JEM-2100F, Japan) observation were dispersed in ultrapure water, and two drops were placed on a carbon-coated copper mesh grid. The experiment was carried out after the evaporation of water.
Particle Size Determination and Zeta Potential Measurement
The particle size and zeta potential of the samples were estimated by phase angle light scattering (PALS) using Zetasizer Nano-Series (NanoZS, Malvern, UK), controlled by the Dispersion Technology Software (DTS 5.03, Malvern, UK). Samples were diluted with ultrapure water before measurement. In each case, the experiment was carried out three times.
Quantification of Alginate and Quercetin
The quercetin in the Q-AN was assessed by measuring the quercetin released from Q-AN in the methanol solution. The yield of alginate and quercetin was calculated as the percent of alginate and quercetin in obtained nanoparticles, which was compared to the initial amount of alginate and quercetin used in the prepared process, respectively.
Thermogravimetric data (TG-DTG-DSC) for samples were obtained using thermogravimetry and differential scanning calorimetry (TG-DSC; STA449F3, Netzsch, Germany). All tests were conducted with sample mass of 2–5 mg at 10 °C min−1 over a range of 50–800 °C. The measurements were carried out in Ar atmosphere
FT-IR spectra of samples were recorded on a FT-IR spectrometer (Tensor 27, Bruker, Germany). The spectra were collected in the range of 4000–400 cm−1 with a resolution of 2 cm−1 at 16 scans per spectrum.
X-ray Diffraction Analysis
The crystal structures of samples were identified using X-ray diffractometer (XRD, D/max-2500, Rigaku, Japan) operated at 50.0 kV and 180.0 mA with Cu Kα radiation, and in the range of 10°–50° with a scanning rate of 0.2° min−1.
X-ray Photoelectron Spectrometer
The valence state of Pb absorbed on Q-AN was determined by X-ray photoelectron spectrometer (PHI 1600, PerkinElmer, USA). Experiments of Q-AN and adsorption of Pb(II) in this characterization was conducted in nitrogen atmosphere to avoid interference of oxygen in air. Measurement was carried out with an AlK (hλ = 1667.0 eV) X-ray source at 250.0 W and pass energy of 29.35 eV for high-resolution analyses. Vacuum in analysis chamber was kept below 3 × 10−6 Pa during measurement. Binding energy of spectra was calibrated with aliphatic carbons C1s (284.6 eV).
Batch adsorption experiments for Pb(II) removal in aqueous solution were performed in polypropylene bottles with a reaction volume of 45 mL at room temperature (25 ± 1 °C). Nanoparticles (0.2 g) were sealed in dialysis bags (MW 12,000) and then immersed in the above Pb(II) aqueous solution. Equilibrium adsorption was achieved by a shaker incubator at 120 rpm for 4 h. Effects of several parameters, such as initial pH (2, 3, 4, 5, 6, 7), initial Pb(II) concentration (250, 500, 750, 1000, 1250 mg L−1), and co-existing heavy metal ions (Mn, Co, Cd), on removal of Pb(II) in aqueous solution were studied. The solution pH was adjusted with 0.1 M HCl and 0.1 M NaOH. The adsorption capability of AN and Q-AN was conducted in 1000 mg L−1 Pb(II) aqueous solution at pH 7. Experiments of Pb(II) desorption were carried out in 1 M HCl solution. And the AN and Q-AN used in desorption experiment reached the equilibrium adsorption in 500 mg L−1 Pb(II) aqueous solution at pH 7. The residual Pb(II) aqueous solution was filtrated with 0.22 μm membrane filter, and then, Pb(II) concentration was quantified with an inductively coupled plasma atomic emission spectroscopy (SPECTRO ARCOS EOP, Spectro Analytical Instruments GmbH, USA).
Results and Discussion
Characterization of AN and Q-AN
Related information about AN and Q-AN
Loading rate (%)
Encapsulation efficiency (%)
Adsorption Capability (mg/g)
Desorption rate (%)
95.06 ± 9.97
0.34 ± 0.11
147.02 ± 3.91
83.26 ± 7.46
58.23 ± 2.34
0.15 ± 0.03
0.36 ± 0.03
10.67 ± 0.89
140.37 ± 5.04
90.07 ± 3.39
The DSC curve of alginate presented one exothermic peak at 265.9 °C corresponding to the thermal decomposition. As to quercetin, the endothermic peak at 133.5 °C was related to the water loss and the second one at 323.4 °C to its melting point. The difference between DSC curve of sodium alginate and AN was mainly caused by gel formation. Two exothermic peaks at 238.5 and 370.9 °C were respectively attributed to the decomposition of gel and residual substances mentioned in DTG analysis. However, no obvious melting point appeared in the DSC curve of Q-AN though the typical crystal structure of quercetin. Besides, the very weak exothermic peak at 408.4 °C might be due to the decomposition of quercetin, and this decomposition temperature is higher than it in the DSC curve of pure quercetin. Thus, it confirmed the interactive force between alginate gel and quercetin.
For quercetin (Fig. 3b), the major peaks were as follows: a strong-broad band at 3422.82 cm−1 (O–H stretching), a medium-sharp peak at 1668.93 cm−1 and a strong-sharp 1610.88 cm−1 (C = O stretching), a strong-sharp peak at 1523.81 cm−1 (aromatic group), a medium-sharp peak at 1316.49 cm−1 and a medium-sharp peak at 1163.08 cm−1 (C–O–C stretching), and a weak-sharp peak at 930.89 cm−1 (aromatic group C–H stretching).
When the alginate nanogel was formed in the presence of Ca2+, several shifts of absorbance peaks were observed compared with the FT-IR spectra of alginate. The change was observed for C–O–C stretching peak at 1109.22 cm−1 (sodium alginate) to 1101.10 cm−1 (AN). A very slight shift of COO– asymmetric stretch peak at 1623.60 cm−1 (sodium alginate) to 1627.58 cm−1 (AN) was also observed. However, the COO– symmetric stretch peak at 1419.73 cm−1 (sodium alginate) was distinctly transferred to 1463.04 cm−1 (AN). Peak shifts mentioned above provided the evidence that the Na+ ions in the sodium alginate were replaced by Ca2+, thus forming a regular three-dimensional net structure bound by Ca2+ . The FT-IR spectra of Q-AN (Fig. 3d) indicated that it kept the major absorption peaks of AN, namely C–O–C stretching peak and COO– asymmetric and symmetric stretch peaks. However, peaks of quercetin were concealed. The reason might be that the trace of quercetin was involved in the interaction with alginate molecule in the preparation process.
X-ray diffraction was performed to study the crystallinity of samples. The characteristic peaks of sodium alginate (Fig. 3b) rose at 13.56 °, 20.74 °, 21.64 °, 24.06 °, 28.96 °, 36.64 °, and 38.40 ° (2θ), demonstrating its semi-crystalline nature . The crystalline nature of quercetin was confirmed by distinct peaks at 10.70 °, 12.32 °, 13.36 °, 16.02 °, 17.76 °, 23.76 °, 27.36 °, 38.6 °, and 40.84 ° [24, 25]. However, the AN and Q-AN exhibited no distinct peaks but broad ones. Similar phenomena of microcrystallites observation in amorphous structure were also reported by some research [26–28]. One of the reasons for this is that the gelation processes changed the spatial structure of sodium alginate. And another reason accounted for the intermolecular interaction occurring between quercetin and sodium alginate. Similar phenomena that oridonin and quercetin transformed from crystal form to amorphous form when loaded in nanoparticles have also been observed by al [29, 30]. And this is accordance with the results obtained in TG-DTG-DSC and FT-IR analysis.
Batch adsorption of Pb(II)
Effect of pH
Effect of Initial Pb(II) Concentration
Effect of Other Co-existing Metal
Adsorption Capability and Desorption Rate
Maximum adsorption capacity of sodium alginate related nano-adsorbents for Pb(II) removal from aqueous media
Sodium alginate-related nano-adsorbents
Maximum adsorption capacity (mg/g)
Silica nanopowders/alginate composite
TSTC  AS-s-SA nanogel
Superparamagnetic Fe3O4@TSTC  AS-s-SA nanocomposite
Magnetic alginate beads based on maghemite nanoparticles
Polyaniline nanofibers assembled on alginate microsphere
In this study, AN and Q-AN were prepared with the technique of nano-emulsions coupled with external gelation. These nanoparticles turned out to be effective for the removal of Pb(II) from aqueous solutions. Compared with the diameter of AN, that of Q-AN underwent an obvious decrease from 95.06 to 58.23 nm. The removal of Pb(II) is found to be highly pH-dependent, and the optimal pH value was 7 among examined pHs. Under the conditions of 1000 mg L−1 Pb(II) at pH 7, the adsorption capability of AN and Q-AN were similar, which were 147.02 ± 3.91 mg g−1 and 140.37 ± 5.04 mg g−1, respectively. The Pb(II) desorption rate of AN and Q-AN were 83.26 ± 7.46 % and 90.07 ± 3.39 %, respectively. Generally, Q-AN got a slightly higher quality for Pb(II) removal than AN. Though further research is required to illustrate the mechanism of marked nanoparticle diameter decrease after the decoration of quercetin, the satisfactory Pb(II) removal rate illustrated that AN and Q-AN are promising adsorbents, which are probably to obtain wide application.
The authors gratefully acknowledge the financial support from the National Natural Science Foundation of China (51108310) and State Scholarship Fund from China Scholarship Council (201406255066).
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