Facile Fabrication of a Low-Cost Alginate-Polyacrylamide Composite Aerogel for the Highly Efficient Removal of Lead Ions

Abstract

In this study, we demonstrate a one-step method for fabricating a novel sodium alginate-polyacrylamide (Alg–PAM) composite aerogel, which exhibits a very high affinity and selectivity towards Pb²⁺. The as-prepared Alg–PAM composite aerogel can uptake 99.2% of Pb²⁺ from Pb²⁺-containing aqueous solution (0.1 mM) and the maximum adsorption capacity for Pb²⁺ reaches 252.2 mg/g, which is higher than most of the reported Pb²⁺ adsorbents. Most importantly, the prepared Alg–PAM adsorbent can be regenerated through a simple acid-washing process with only a little loss of the adsorption performance after five adsorption–desorption cycles. In addition, the influence of the experimental conditions, such as the solution pH, contact time, and temperature, on the adsorption performance of the Alg–PAM adsorbent was studied. It is clear that the low-cost raw materials, simple synthesis, regeneration ability, and highly efficient removal performance mean that the designed Alg–PAM aerogel has broad application potential in treating Pb²⁺-containing wastewater.

1. Introduction

Lead is widely used as a raw material in industrial production. Lead ions (Pb²⁺) are often found in lead storage batteries, lead ore smelting, and recycled lead industrial wastewater [1]. Pb²⁺ in wastewater can be absorbed and enriched by aquatic animals and plants and then enter the human body through the food chain, thereby posing serious damage to the nerves, digestive systems, kidneys, and endocrine systems of humans [2,3]. Children are more sensitive to Pb²⁺ than adults, and excessive Pb²⁺ can cause mental decline and behavioral abnormalities among children [4,5]. Therefore, new methods and materials for effectively and selectively removing Pb²⁺ from wastewater must be developed.

Previously, many synthesized materials, such as one-dimensional (1D) nanofibers [6,7], two-dimensional (2D) films or membranes [3,8,9], and three-dimensional (3D) scaffolds [10,11,12], have been utilized as effective absorbents for treating Pb²⁺-containing water systems. 1D and 2D nano-adsorbents have a high adsorption capacity and adsorption rate for Pb²⁺ due to their high specific surface area and chemical activity, but the preparation of these nanomaterials usually requires stringent conditions, such as a high temperature, high pressure, high purity reagents, etc. In addition, these nano-adsorbent materials are difficult to recollect because of their small size. Macroscopic 3D porous material can overcome the above shortcomings. It not only provides a high surface area, but also facilitates solid–liquid separation. To achieve an economical use of the synthesized absorbents, an important aspect is to find low-cost and source-rich natural materials for fabricating various functional nanomaterials [13,14].

Sodium alginate is a natural polysaccharide with an excellent biocompatibility and biodegradability. This molecule contains a large amount of carboxyl and hydroxyl functional groups that can complex metal ions [15]. Therefore, sodium alginate can also be used as a medical antidote for treating heavy metal ion poisoning [16]. However, alginate aerogels have poor mechanical properties. After repeated use, the aerogel structure can be easily destroyed, thereby resulting in an unstable adsorption capacity for heavy metal ions [17]. This kind of material shows improved mechanical properties given its special adhesion. In addition, the polyacrylamide molecule contains a large amount of amino groups that can chelate with metal ions, thereby adsorbing heavy metal ions in water [18,19].

In this work, to improve the mechanical properties of alginate-based aerogel, we modified polyacrylamide on alginate salt by applying a simple chemical grafting technique and then prepared a novel sodium alginate/polyacrylamide (Alg–PAM) composite aerogel by applying the vacuum freeze-drying technique. We then used this aerogel to remove Pb²⁺ from wastewater, characterized its morphology and chemical composition, and studied its adsorption effect on Pb²⁺ under different experimental conditions.

2. Materials and Methods

2.1. Chemicals and Materials

Sodium alginate (low viscosity), polyacrylamide, nitric acid (HNO₃), sodium hydroxide (NaOH), metal salts, 1-Ethyl-3-(3-dimethyllaminopropyl)carbodiimide hydrochloride, and N-hydroxysuccinimide were purchased from the Shanghai Aladdin Reagent Company (Shanghai, China). All metal salt solutions were prepared by using ultrapure water. The pH value of the solution was adjusted with 1.0 M HNO₃ or NaOH. Lake water was taken from the Anqing Lianhu Lake (Anqing, China), whereas river water was collected from the Anqing section of the Yangtze River (Anqing, China).

2.2. Apparatus

Macroscopic and microscopic images of the materials were taken using a D600 Canon digital camera and Quanta 250FEG scanning electron microscopes (SEM, FEI Company, Hillsboro, Oregon, USA), respectively. The chemical composition of the adsorbent and the functional groups contained therein were determined using an Avatar 360 infrared spectrometer (Thermo Nicolet Corporation, Waltham, Massachusetts, USA) and Axis Ultra DLD X-ray photoelectron spectrometer (XPS, Shimadzu Corporation, Tokyo, Japan). A JJ-1 electric agitator (Changzhou Guohua Company, Changzhou, China) and MS7-H550-Pro agitator (Dragon Laboratory Instruments Limited, Beijing, China) were used for mechanical and magnetic stirring, respectively. A PHS-3E acidity meter (Shanghai Leici Company, Shanghai, China) was used to determine the pH value of the solution. Each adsorption/desorption experiment was conducted three times in parallel, and the concentration of each metal ion in the solution was measured by an Optima 8000 inductively coupled plasma optical emission spectrometer (ICP–OES, PerkinElmer Instrument Co., Ltd, Waltham, MA, USA).

2.3. Preparation of the Sodium Alginate-polyacrylamide (Alg–PAM) Composite Aerogel

First, 2.0 g of sodium alginate was weighed and dissolved in 98.0 mL of ultrapure water. Second, 0.15 g of 1-Ethyl-3-(3-dimethyllaminopropyl)carbodiimide hydrochloride and 0.12 g of N-hydroxysuccinimide were added to the solution and mechanically stirred for 3 hours. Third, 2.0 g of polyacrylamide was added to the mixture, and stirring was continued for 12 hours at room temperature. Fourth, under magnetic stirring, the mixture was dropped into a calcium nitrate solution (when the mixture was in contact with the Ca²⁺ solution (0.5 M), an oval hydrogel was immediately formed), and the hydrogels were then collected by filtration and washed thrice with ultrapure water. Fifth, the hydrogels were immersed in ultrapure water, placed in a vacuum freeze-drying apparatus, frozen for 4 hours, and vacuum dried for 20 hours to obtain the sodium alginate-polyacrylamide (Alg–PAM) composite aerogel.

2.4. Adsorption and Desorption Tests

In an adsorption experiment, about 100 mg of Alg–PAM was weighed and added to 40 mL of the 0.1 mM Pb²⁺ (or other metal ions) solution, stirred at room temperature for 24 hours, and eventually filtered through filter paper and a funnel at atmospheric pressure. The amount of Pb²⁺ remaining in the filtrate was measured using the ICP–OES.

In a desorption experiment, Pb²⁺-loaded Alg–PAM was immersed in 40 mL of the 0.05 M HNO₃ solution for 30 minutes, filtered, and washed thrice with ultrapure water, and the amount of Pb²⁺ in the eluate was then determined using ICP–OES.

3. Results and Discussion

3.1. Material Characterization

In order to determine the components and functional groups contained in the prepared Alg–PAM, we characterized the raw sodium alginate, polyacrylamide, and Alg–PAM composite aerogel by infrared spectroscopy. As shown in Figure 1, in the three spectra, the absorption peaks around 2925 cm⁻¹ are aliphatic C–H stretching vibrations. In the spectrum of sodium alginate, the broad absorption peak near 3400 cm⁻¹ is –OH stretching vibration, and the absorption peak at 1412 cm⁻¹ belongs to the –COO^– group [20]. In the spectrum of polyacrylamide, the absorption peak at 1650 cm⁻¹ can be assigned to the amide bond [21]. Compared with the spectrum of sodium alginate, a new peak of the amide bond is observed near 1650 cm⁻¹ in Alg–PAM, thereby suggesting that polyacrylamide was successfully modified on the calcium alginate aerogel [20]. Furthermore, we also characterized the XPS spectra of Alg–PAM before and after Pb²⁺ adsorption. As shown in Figure 2, after adsorption, new Pb 4f peaks could be observed on the Alg–PAM adsorbent, thereby indicating that Pb²⁺ ions were successfully loaded onto the Alg–PAM adsorbent [22].

Moreover, we also characterized the morphology of Alg–PAM. As shown in Figure 3, the as-prepared Alg–PAM takes the form of white aerogel balls in the shape of water droplets. When amplified locally, many wrinkles can be seen on the Alg–PAM surface. This wrinkled surface can increase the contact area between the adsorbent and adsorbate, thereby increasing the adsorption capacity of Alg–PAM to the target metal ions.

3.2. Effect of Solution pH

In order to investigate the effect of solution acidity on the adsorption performance of Alg–PAM, ~100 mg of Alg–PAM adsorbent was added to 40 mL pH = 1, 2, 3, 4, 5, or 6 of Pb²⁺ (0.1 mM) solution. After stirring for 24 hours and filtration, the concentration of Pb²⁺ in the filtrate was measured by ICP–OES. The experimental results are shown in Figure 4. When the pH value of the solution is 1, Alg–PAM can only remove 17.7% of Pb²⁺ in wastewater, which may be ascribed to the fact that the carboxyl and amino groups on Alg–PAM are protonated in the strongly acidic environment, thereby reducing the functional groups bound to Pb²⁺ [23]. When the pH value of the solution is within the range of 3 to 6, Alg–PAM can remove more than 99.0% of Pb²⁺ in wastewater. When the pH value of the solution exceeds 6, according to the solubility product rule, the Pb²⁺ in the solution begins to form a Pb(OH)₂ precipitate. Therefore, the optimum pH value of the adsorbed solution ranges between 3 and 6. Within this range, neither the amino group nor the carboxyl group is protonated, and the Pb²⁺ in the solution does not form a Pb(OH)₂ precipitate.

3.3. Effect of Adsorption Time

Approximately 100 mg of Alg–PAM was weighed and added to 40 mL of the 0.1 mM Pb²⁺ solution; stirred for 0.5, 1, 2, 3, 6, 12, 20, 24, 30, or 36 hours; and then filtered. The amount of Pb²⁺ remaining in the filtrate was determined by ICP–OES. As can be seen in Figure 5, as the contact time increases, the amount of Pb²⁺ adsorbed by Alg–PAM initially increases, followed by a gradual increase, and eventually reaches stability. When the adsorption time is 12 hours, Alg–PAM can remove 97.6% of Pb²⁺ in the solution. When the adsorption time is 24 hours, Alg–PAM can remove 99.2% of Pb²⁺ in the solution. When the adsorption time is longer than 24 hours, the Pb²⁺ removal efficiency of Alg–PAM remains stable. Therefore, the adsorption time we selected in this study was 24 hours, which is close to the reported values in the literature [24,25].

3.4. Influence of Temperature

We also studied the removal efficiency of Alg–PAM for Pb²⁺ at different ambient temperatures. About 100 mg of Alg–PAM was weighed and added to 40 mL of the 0.1 mM Pb²⁺ solution, placed at 0, 5, 15, 20, 30, 40, or 50 °C for 24 hours, and filtered, and the amount of Pb²⁺ remaining in the filtrate was then measured by ICP–OES. Figure 6 shows that the Pb²⁺ removal efficiency of Alg–PAM gradually increases along with ambient temperature. When the ambient temperature is 15 °C, the adsorption efficiency of Pb²⁺ by Alg–PAM is 94.9%. When the temperature increases to 40 °C, the removal efficiency reaches 99.3%. These experimental results are similar to the reported literature and indicate that the process by which Alg–PAM binds to Pb²⁺ is endothermic [26,27].

3.5. Adsorption Performance of Alg–PAM for Metal Ions

The adsorption abilities of Alg–PAM for different metal ions (such as Pb²⁺, Cu²⁺, Cr³⁺, Cd²⁺, Zn²⁺, and Co²⁺) are shown in Table 1. It can be seen from Table 1 that Alg–PAM has a high affinity for Pb²⁺, Cu²⁺, and Cd²⁺, and can remove more than 90% of the corresponding metal ions in the solution, which may be attributed to the carboxyl, hydroxyl, and amino groups on Alg–PAM that bind the metal ions via a coordination effect. In addition, despite the coexistence of Cu²⁺, Cr³⁺, Cd²⁺, Zn²⁺, or Co²⁺, Alg–PAM can still remove more than 95% of Pb²⁺ in the mixed solution, and the relative selectivity coefficients (k) are all over 8. This indicates that the prepared Alg–PAM has a higher selectivity for Pb²⁺, and can selectively remove Pb²⁺ in the presence of other ions.

In order to confirm the maximum adsorption capacity of the Alg–PAM adsorbent for Pb²⁺, we added ~100 mg of Alg–PAM to 40 mL of different concentrations of Pb²⁺ solution, stirred for 24 hours, filtered, and then measured the amount of Pb²⁺ remaining in the filtrate. It can be seen from Figure 7 that as the solution concentration increases, the adsorption capacity of Alg–PAM for Pb²⁺ gradually increases. When the Pb²⁺ concentration increases from 0.1 to 50 mM, the adsorption capacity of Alg–PAM for Pb²⁺ rapidly increases from 8.2 to 252.2 mg/g. However, when the concentration of Pb²⁺ exceeds 50 mM, the adsorption capacity of Alg–PAM remains stable and shows no further increase. Therefore, the maximum adsorption capacity of Alg–PAM for Pb²⁺ is 252.2 mg/g, which is higher than that of most of the reported Pb²⁺ sorbents (Table 2) [28,29,30,31,32,33,34,35,36,37,38,39,40,41].

3.6. Regeneration of Alg–PAM

Under acidic conditions, H protons can displace Pb²⁺ ions that are attached to the carboxyl, hydroxyl, and amino groups of the Alg–PAM [42]. To avoid introducing other impurity ions, we used HNO₃ as an eluent to regenerate the adsorbent in this study. In the adsorbent regeneration experiment, the Pb²⁺-loaded Alg–PAM was immersed in 40 mL of the 0.05 M HNO₃ solution for 30 minutes and filtered, and the adsorbent was washed successively with ultrapure water, saturated Ca(OH)₂ solution, and ultrapure water. The adsorbent was then dried in an oven at 40 ℃ for 4 hours to obtain the regenerated Alg–PAM. It can be seen from Figure 8 that the regenerated Alg–PAM adsorbent has stable chemical properties, and its removal efficiency for Pb²⁺ is in the range of 97 ± 3%. In addition, the physical morphology of Alg–PAM also remains stable after five adsorption–desorption cycles.

4. Conclusions

We successfully prepared a novel sodium alginate-polyacrylamide composite aerogel (Alg–PAM) by using a simple one-step synthesis method. The prepared Alg–PAM is a macroscopic adsorbent that can be easily applied for solid–liquid separation. Alg–PAM also exhibits a high affinity and selectivity for Pb²⁺ due to the carboxyl, hydroxyl, and amide groups and can remove 99.2% of Pb²⁺ from wastewater with a maximum adsorption capacity up to 252.2 mg/g. This adsorbent can be regenerated by simple acid washing, and its adsorption performance remains stable after repeated use. Given its use of low-cost and green raw materials, its simple preparation process, and its high efficiency removal performance, Alg–PAM has broad application potential in treating heavy metal ions in wastewater.

Author Contributions

Z.W. conceived and designed the experiments; Q.Y. performed the experiments; Q.Y. and X.Z. analyzed the data; Z.W. and G.W. wrote the paper; G.W. revised the manuscript.

Funding

This research was funded by the Anhui Department of Education, grant number gxyZD2019045.

Conflicts of Interest

The authors declare no conflicts of interest.

Figures and Tables

Figure 1. Infrared spectra of (a) raw sodium alginate, (b) alginate/polyacrylamide composite aerogel (Alg–PAM), and (c) raw polyacrylamide.

Figure 2. X-ray photoelectron spectrometer (XPS) spectra of sodium alginate-polyacrylamide (Alg–PAM) (a) before and (b) after Pb2+ adsorption.

Figure 3. (A) Digital photograph of Alg–PAM; (B) Scanning electron microscope (SEM) Image of Alg–PAM; and (C) partial enlargement of (B).

Figure 4. Influence of the solution acidity on the Pb2+ removal efficiency of Alg–PAM.

Figure 5. Effect of the contact time on the removal efficiency of Alg–PAM for Pb2+.

Figure 6. Removal efficiency of Alg–PAM for Pb2+ at different ambient temperatures.

Figure 7. Maximum adsorption capacity of the Alg–PAM for Pb2+.

Figure 8. Removal efficiency of Pb2+ by Alg–PAM in five adsorption–desorption cycles.

Table 1

Adsorption ability of the sodium alginate-polyacrylamide (Alg–PAM) for different metal ions.

Alg–PAM	Initial Solution (mM)		Removal Efficiency (%)		Adsorption Capacity (mg/g)		Kd		k
In ultrapure water	0.1 (Pb2+)	-	99.2	-	8.2	-	49.6	-	-
	0.1 (Cu2+)	-	91.6	-	2.3	-	4.4	-	-
	0.1 (Cr3+)	-	92.4	-	1.9	-	4.9	-	-
	0.1 (Cd2+)	-	90.2	-	4.1	-	3.7	-	-
	0.1 (Zn2+)	-	76.9	-	2.0	-	1.3	-	-
	0.1 (Co2+)	-	69.5	-	1.6	-	0.9	-	-
	0.1 (Pb2+)	0.1 (Cu2+)	95.3	71.8	7.9	1.8	8.1	1.0	8.0
	0.1 (Pb2+)	0.1 (Cr3+)	96.5	67.7	8.0	1.4	11.0	0.8	13.2
	0.1 (Pb2+)	0.1 (Cd2+)	96.7	66.0	8.0	3.0	11.7	0.8	15.1
	0.1 (Pb2+)	0.1 (Zn2+)	97.8	61.9	8.1	1.6	17.8	0.6	27.3
	0.1 (Pb2+)	0.1 (Co2+)	97.1	43.2	8.0	1.0	13.4	0.3	44.0
In lake water	0.1 (Pb2+)	-	88.4	-	7.3	-	3.1	-	-
In river water	0.1 (Pb2+)	-	94.3	-	7.8	-	6.6	-	-

Table 2

Adsorption capacities of the reported adsorbents for Pb²⁺.

Adsorbents	Adsorbate	Maximum Adsorption Capacity (mg/g)	References
Polyampholyte hydrogel	Pb2+, Cd2+	216.1(Pb2+), 153.8(Cd2+)	[28]
Nanohydroxyapatite	Pb2+	200.0	[29]
GO 1	Pb2+	178.5	[30]
GO/chitosan/FeOOH	Pb2+	111.1	[31]
Thiol-functionalized GO	Pb2+	200.0	[32]
Dithiocarbamate-functionalized GO	Pb2+	132.0	[33]
Xanthate-modified thiourea chitosan sponge	Pb2+	188.1	[34]
Biochar	Pb2+, Cd2+, Cu2+	153.1(Pb2+), 28.1(Cd2+), 34.2(Cu2+)	[35]
Amino-functionalized wood flour	Pb2+	189.9	[36]
GO	Pb2+	125.0	[37]
Chitosan-poly(acrylic acid) composite beads	Pb2+	138.9	[38]
Titanium-Tin oxide nanocomposite	Pb2+	70.0	[39]
Nitrogen-doped carbon nanospheroids	Pb2+	99.8	[40]
Cysteine-functionalized lignin	Pb2+, Cu2+	55.5(Pb2+), 68.7(Cu2+)	[41]
Alg–PAM 2	Pb2+	252.2	Our work

¹ GO: graphene oxide. ² Alg–PAM: sodium alginate-polyacrylamide.