The effective removal of Pb2+ by activated carbon fibers modified by l-cysteine: exploration of kinetics, thermodynamics and mechanism.

Herein, we developed a low-cost fabrication route to prepare chemically grafted activated carbon fibers, which effectively removed Pb2+ from solution. Multiple characteristic results indicated that l-cyst-ACF had abundant nitrogen-containing and sulfur-containing functional groups. Based on the XPS and EDS analyses, the capture of Pb2+ was attributed to the abundant adsorption sites on the fiber surface. According to the analysis of the pseudo-second-order kinetic model and the Langmuir isotherm model, the adsorption process could be interpreted as monolayer adsorption and chemisorption, and the equilibrium adsorption capacity was determined to be 136.80 mg g-1 by fitting the pseudo-second-order kinetic model. The maximum adsorption capacity of l-cyst-ACF for Pb2+ was calculated to be 179.53 mg g-1 using the Langmuir model. In addition, the adsorption reaction was endothermic and spontaneous, as evidenced by the thermodynamic parameters. The outcomes of this study provide a low-cost and feasible strategy for the remediation of Pb2+ pollution in the environment. This journal is © The Royal Society of Chemistry.

Introduction

The rapid development of modern industry has produced a large amount of wastewater polluted with heavy metals, which has caused great ecological and environmental harm, and finally poses a threat to human health through the food chain.[1,2] Heavy metal ions are non-biodegradable carcinogenic factors and tend to accumulate in organisms.[3,4] Heavy metals can enter the food chain through plants and pose a serious threat to human health.[5] Common heavy metal ions can cause acute and chronic diseases such as digestive inflammation, brain injury and cancers.[6] Therefore, the removal of heavy metal ions from industrial wastewater has become a major pro-environmental problem in recent years.

Various technologies to remove heavy metals from water are available, such as solvent extraction,[7] ion exchange,[8] precipitation[9,10] and adsorption.[11] Among them, adsorption has the advantages of simple operation, high efficiency, and strong flexibility. Many materials have been used to remove heavy metals such as activated carbon,[12,13] polymers,[14,15] and nanomaterials.[16] However, the practical application of adsorbents is hindered by their low adsorption efficiency for the target metal, the inconvenient process for their synthesis of and their unachievable recycling. Therefore, the development of advanced adsorbents with high adsorption capacity, recyclability and good chemical stability has become a vital research direction in the field of heavy metal remediation.

Activated carbon fibers (ACFs) are a new type of adsorbent developed in recent years to remove pollutants in aqueous solutions. Compared with the traditional activated carbon particles, activated carbon fibers have more suitable pore sizes, better adsorption effect and easy recycling.[17-19] Javier[20]et al. measured the effect of activated carbon fibers to adsorb both Pb2+-phenol and Cd2+-phenol simultaneously, proving that the selectivity of activated carbon fibers for Pb2+ ions was greater than Cd2+ ions. Deng[18]et al. found that a novel thiosemicarbazide-modified adsorbent exhibited a high performance towards Cd(ii) and Pb (ii). This result explained that sulfur-containing groups and nitrogen-containing groups could effectively adsorb metal ions in solution by chelation and coordination.

In the present study, activated carbon fiber adsorbents grafted with multiple functional groups with high adsorption properties were prepared via a simple amide reaction. The preparation fibers were characterization through multiple technologies such as Fourier transform infrared spectroscopy (FT-IR), X-ray photoelectron spectroscopy (XPS), scanning electron microscopy (SEM) and energy dispersive X-ray analysis (EDX). Meanwhile, the behavior and mechanism of Pb2+ adsorption were comprehensively explored via adsorption kinetics, isotherm models, and thermodynamic parameters. Then, the adsorption performance of l-cyst-ACF for Pb2+ was systematically discussed, which suggested that the adsorption process was spontaneous and endothermic.

Materials and methods

Materials

Activated carbon fibers were obtained from Jiangsu Sutong Carbon Fiber Co., Ltd (Suzhou, China). Thiourea (AR, 99%), N-(3-dimethylaminopropyl)-N′-ethyl-carbodiimide hydrochloride (EDC, AR, 99%), N-hydroxy-succinimide (NHS, AR, 99%), and NaHSO4 (AR, 99%) were purchased from Aladdin Regent Co. Ltd (Shanghai, China). Pb (NO3)2 (AR, 99%) was produced from Sinopharm Chemical Reagent Co, Ltd (Shanghai, China). Na2S (AR, 98%) was procured from Macklin Biochemical Technology Co., Ltd (Shanghai, China). Ethyl alcohol (AR, 99.9%) was bought from Jiangsu Qiangsheng Functional Chemistry Co., Ltd (Suzhou, China). Dichloromethane (AR, 99.5%) was produced from Hangzhou Shuanglin Chemical Reagent Co., Ltd (Hangzhou, China). HNO3 (AR 65%) and H2SO4 (AR 98%) were bought from Sinopharm Chemical Reagent Co, Ltd (Shanghai, China). l-Cysteine hydrochloride monohydrate (AR 99%), KH2PO4 (AR 99.5%), and Na2HPO4 (AR 99%) were all bought from Aladdin Regent Co. Ltd (Shanghai, China).

Preparation of l-Cysteine-modified activated carbon fiber

Activated carbon fibers were washed with deionized water several times and dried for 12 h at 80 °C until a constant weight. Then, the clean fibers were cut into small pieces and soaked in a HNO3/H2SO4 (3 : 1, v : v) solution for acidification. The fibers were washed several times and dried overnight. ACFs were put in an appropriate amount of KH2PO4/Na2HPO4 buffer solution with a pH of 8.5. EDC (1.8 g) and NHS (1.2 g) were added to the solution with constant stirring at room temperature, and then thiourea (1.52 g) was added. After 6 h, ACFs were washed and dried.

Firstly, 1.38 g of sodium bisulfate (NaHSO4) was added to 100 mL of 0.1 m L−1 dilute hydrochloric acid solution, and then 80 mL of ethanol was added. Subsequently, ACF and l-cysteine (1.7563 g) were added to the above mixture, and the system was heated at reflux at 95 °C for 6 h. The product was washed with ethanol and deionized water several times, and then dried at 80 °C in vacuo for 24 h. To reduce the oxidized sulfhydryl group (–SH), ACFs were added to an organic solvent (dichloromethane:ethyl alcohol, v : v = 1 : 2), Na2S was added to the mixture as a reducing agent, and then it was stirred at room temperature for a certain of time. Finally, ACFs were filtered and washed several times, and then stored after drying. The specific experimental steps are shown in Fig. 1.

Fig. 1

Process for the preparation of cysteine-modified activated carbon fibers.

Characterization of l-cyst-ACF

The properties of l-cyst-ACF were characterized via a series of performance tests. Fourier-transform infrared spectra (FTIR) were recorded in pressed KBr using a Vertex 70 spectrophotometer (Bruker) in the range of 500–4000 cm−1 at room temperature. The morphological characteristics of l-cyst-ACF were observed via SEM (Hitachi, SU8010). The elemental components of l-cyst-ACF before and after adsorption were identified by X-ray photoelectron spectroscopy (XPS, Thermo Fisher: ESCALAB 250Xi, single Al Kα as the light excitation source). An Oxford X-MaxN scanning electron microscope (SEM)/energy dispersive X-ray spectroscopy (EDS) was used to observe the surface morphology and element distribution of the fiber, respectively. Inductively coupled plasma atomic emission spectrometry (ICP-MS Agilent: 7800, China) was used to detect the Pb(ii) concentration.

Batch adsorption experiments

A sequence of batch adsorption experiments was conducted to investigate the performance of the synthesized adsorbents for the elimination of Pb2+ from aqueous solution. The adsorption experiments were performed in an SHA-B water bath oscillator (RongHua Instrument Manufacturing Co., Ltd, China) at a shaking speed of 120 rpm. Batch experiments were performed to investigate the kinetics, isothermal models, and thermodynamic parameters during the adsorption process. In this investigation, the initial metal ion concentration range was 0–500 mg L−1, adsorbent dose range was from 50 to 150 mg and the system temperatures were 303 K, 313 K and 323 K, respectively. The pH range of 2–6 was adopted in the experiment to investigate the influence of pH. All batch experimental solution concentrations were detected through inductively coupled plasma atomic emission spectrometry. Before the solution concentration test, the test liquids were filtered with a 0.22 μm filter to remove impurities.

The adsorption amount qe (mg g−1) of Pb2+ in adsorption equilibrium was calculated using eqn (1):

The removal efficiency of Pb2+ at equilibrium was calculated using eqn (2):where C0 and Ce are the initial concentration and equilibrium concentration (mg L−1), respectively. V (L) is the volume of the solution and M (g) is the weight of the absorbent.

Results and discussion

Characterization of ACF and l-cyst-ACF

The FT-IR spectra of ACF and l-cyst-ACF are shown in Fig. 2. In the spectrum of the activated carbon fibers, the band at 3442 cm−1 is ascribed to the –OH stretching vibration[21] and that at 1654 cm−1 is ascribed to the CO stretching.[22] The peaks at 1541 cm−1 and 1388 cm−1 correspond to the C–C and C–O bonds, respectively.[23] Similarly, the peak at 3446 cm−1 in the spectrum of l-cyst-ACF represents the –OH stretching vibration, and the two peaks at 1527 cm−1 and 1386 cm−1 can be ascribed to the C–C and C–O groups, respectively.[24] The peaks at 2813 cm−1 and 2933 cm−1 are attributed to the stretching vibrations of –CH2 and –CH3, respectively. The sharp peak at 3471 cm−1 and the broad band at around 3100–3300 cm−1 are attributed to the –NH2 vibration.[25] Obviously, the sharp peak at 1655 cm−1 can be assigned to the carbonyl stretch of the –NHCO– group, not just the carbonyl group (CO).[24] Meanwhile, a weak peak located at 2401 cm−1 was observed, which can be attributed to the –SH bending vibration.[18,26] The small peak at 1267 cm−1 is ascribed to the CS bond.[12] The band at 1000 cm−1 may be caused by the C–N stretching.[27] In addition, the peaks at 740 cm−1 and 632 cm−1 correspond to the bending vibration of –NH2 and vibrational C–S bonds, respectively.[28]

Fig. 2

FT-IR spectra of activated carbon fibers and l-cysteine-modified activated carbon fibers.

Characterization of ACF-SH

The SEM images of ACF and l-cyst-ACF are shown in Fig. 3. The SEM image of ACF (Fig. 3a) displays a regular smooth surface; meanwhile, that of l-cyst-ACF (Fig. 3b) shows an irregular rough surface after modification, which illustrates that organo-functional groups were successfully grafted. Alternatively, a larger specific surface area is also conducive to an improvement in adsorption capability. The changes on the surface of the modified ACF after adsorption are showed in Fig. 3(c and d). It can be observed that some irregular tiny particles covered the surface of the fibers after adsorption, demonstrating the further improved effective adsorption ability of l-cyst-ACF to remove Pb2+ ions.

Fig. 3

SEM images of ACF and l-cyst-ACF (a) original ACF, (b) l-cyst-ACF (c and d) after Pb2+ adsorbed on l-cyst-ACF.

The energy dispersive X-ray spectroscopy mapping of l-cyst-ACF is displayed in Fig. 4, which authenticated the presence of elements including carbon (C), oxygen (O), sulfur (S) and nitrogen (N) related to the presence of l-cysteine modified on ACF. As shown as Fig. 4(B–F), the successful grafting reaction of functional groups occurred on ACF. According to the data, it can be concluded that O and N are not co-localized with Pb. Fig. 4E and F show strong S and Pb signals, respectively, which are co-localized, suggesting that the primary adsorbent for Pb is S and that N and O did not significantly contribute to the adsorption.

Fig. 4

(A) SEM image of l-cyst-m-ACF after adsorption (B)–(F) EDS mapping of l-cyst-m-ACF of C, O, S, N, and Pb elements after the adsorption of Pb2+.

Fig. 5A reveals the chemical composition changes in the modified activated carbon fibers compared with the original fiber according to the XPS analysis. The presence of amine groups confirmed that the grafting reaction occurred. Additionally, the ratio of different elements illustrates that the organic functional groups were successfully grafted, as shown in Fig. 5B. EDS mapping, FT-IR, and XPS analyses were employed to confirm the adsorption of Pb2+ on l-cyst-ACF.

Fig. 5

(a) XPS spectra of base ACF, l-cyst-ACF and l-cyst-ACF-Pb. (b) Composition of fiber samples determined by XPS analysis.

Lead adsorption

Contact time

The exploration of the adsorption equilibrium time is a crucial part of measuring the performance of an adsorbent and it is significance for subsequent research.[29] The change in the adsorption of the material with contact time is presented in Fig. 6. It shows that the adsorption capacity of Pb2+ increased rapidly within the first hour, which can be ascribed to the effective complexation of organic groups with Pb2+.[30,31] Then, it remained at approximately 125 mg g−1 for Pb2+ after 6 h, indicating that adsorption equilibrium had been achieved.

Fig. 6

Effect of contact time on the adsorption capacity of Pb2+ (pH = 5.5, temperature = 303 K, C0 = 100 mg L−1, and V = 100 mL).

Different adsorbent dosages

The removal efficiency of Pb2+ with different adsorbent dosages was also investigated. As shown in Fig. 7, the removal rate of Pb2+ increased significantly as the dosage increased. When the dosage increased from 0.25 g L−1 to 0.5 g L−1, the removal of Pb2+ increased from 23.78% to 51.55%. Simultaneously, the degradation rate of Pb2+ did not increase significantly with an increase in the adsorption dosage. However, the removal efficiency of l-cyst-ACF was limited when the adsorption dosage was greater than 0.5 g L−1, indicating that a larger adsorption dosage had a greater impact on the further removal of Pb2+. Thus, we chose the dosage of l-cyst-ACF to be 0.5 g L−1 for the subsequent removal process.

Fig. 7

Effect of different adsorbent dosages on the adsorption capacity and removal efficiency of Pb2+ (C0 = 100 mg L−1, V = 100 mL, contact time = 6 h, and temperature = 303 K).

Initial pH

Research has shown that the surface charge of the absorbent material, the degree of ion migration and the state of the adsorbed substance are affected by the pH of the solution during the adsorption process.[32]Fig. 8a shows that the amount of adsorption observably increased with an increase in pH. This phenomenon demonstrated that the existence of a large amount of H+ ions competed with Pb2+ ions for the adsorption sites in the material in an acidic environment.[31] It is generally believed that lead ions exist as cations in aqueous solutions.[33,34] However, Pb2+ ions easily form Pb(OH)2 (precipitation) with OH− when the pH is greater than 6.[35] Thus, zeta potential (ζ) measurements at different pH were performed to explore the surface charge of the absorbent, as shown in Fig. 8b. Fig. 8b shows that the surface of the material exhibited a negative charge state as the pH increased. Because the functional groups such as –NH2 and –SH on the material surface lost H− ions as the OH− gradually increased in the solution, and they became the active state.[36] This active state was conducive to the adsorption of Pb2+ ions by the material. On the contrary, the hydroxyl, carboxyl, amine and sulfhydryl groups on the surface of l-cyst-ACF tended to be protonated, and they were positively charged when the pH value was low, which led to electrostatic repulsion between the binding site and Pb2+ ions.[15,37,38] Therefore, the pH of the solution and the surface charge of the material were the key factors that affected its adsorption capacity.

Fig. 8

Effect of initial pH on Pb2+ adsorption and zeta potential of l-cyst-ACF during removal process at different pH.

Adsorption kinetics

To quickly and accurately interpret the adsorption behavior of materials, four types of kinetic models were adopted in this investigation. The linear types of models are expressed as eqn (3)–(6).[39,40]where qe and q are the adsorption capacity at equilibrium and time t (mg g−1).[36]K1 (min−1) and K2 [g·(mg min)−1] are the rate constant. K is the rate constant of diffusion particles.[41]α [mg (g min)−1] and β (g mg−1) represent the initial constant adsorption and desorption constants, respectively.[42]

According to the fitting results in Fig. 9 and Table 1, it can be seen that the R2 values of the pseudo-second-order and intra-particle-diffusion kinetic models were better than that of the pseudo-first-order kinetic models and Elovich model, indicating that the possible mechanism of adsorption is chemisorption and the adsorbent surface corresponds to a heterogeneous system. Furthermore, this result reveals that the adsorption is related to the electron exchange between the surface functional groups and Pb2+ ions. The experimental equilibrium adsorption capacity, qe (136.80 mg g−1), obtained by fitting the pseudo-second-order kinetic equation maintained high consistency with the actual test value (∼125 mg g−1).

Fig. 9

(a) Plots of pseudo-first-order kinetic model for the adsorption of Pb2+, (b) pseudo-second-order kinetic model for the adsorption of Pb2+, (c) intra-particle-diffusion kinetic model for the adsorption of Pb2+, (d) Elovich kinetic model for the adsorption of Pb2+. Conditions: T = 303 K [adsorbent] = 0.5 g L−1 [metal] = 100 mg L−1, pH = 5.5, and contact time = 6 h.

The parameters of four types of kinetic models

Kinetic model	Parameter	Value
Pseudo-first-order model	q e (mg g−1)	99.01
	K1 (min−1)	0.0106
	R 2	0.9211
Pseudo-second-order model	q e (mg g−1)	136.80
	K2 [g·(mg min)−1]	0.0073
	R 2	0.9743
Intraparticle diffusion model	K 1 [mg·(g·min1/2)−1]	7.2388
	K 2 [mg·(g·min1/2)−1]	14.9328
	K 3 [mg·(g·min1/2)−1]	3.7675
Elovich model	α [mg·(g min)−1]	6.5584
	β (g mg−1)	0.0342
	R 2	0.9551

To investigate the internal diffusion mechanism during the adsorption process, the intra-particle diffusion model proposed by Weber and Morris[43] was used to discuss the rate-controlling step. Multi-linearity was observed, as shown in Fig. 9c, and the crucial information obtained is presented in Table 1. As shown in Fig. 9c, the Pb2+ adsorption process involved three steps. The initial linear part was the result of adsorption on the external surface, namely, the attachment of Pb2+ to the surface of l-cyst-ACF.[44] The second linear part represents the progressive internal diffusion of particles.[12] In the third part, the decreased diffusion rate is due to the reduction in Pb2+ concentration and the enhanced electrostatic repulsion on the material surface.[45] The intra-particle diffusion and complex or ion exchange may play a certain role in the adsorption process given that none of the three linear curves passed through the origin of the coordinate.[23] Combined with the characterization test and mechanism investigation, we realized that the relatively rough surface on the fiber surface and the partially oxidized thiol functional groups generated sulfonic acid groups, which reduced contact probability between the Pb2+ in solution and active sites on the material surface, affecting the transfer rate of Pb2+ in the surface liquid layer. Comparatively, the ion transport rate in the pore was larger. The α and β constants also indicated that the material had a low adsorption rate and a non-homogeneous surface structure.

Adsorption isotherms

Two common isothermal models were used to evaluate the adsorption behavior between Pb2+ and l-cyst-ACF. The linear form of the Langmuir isotherm is represented by the following equation:[46]where qe and qmax represent the equilibrium adsorption capacity and monolayer maximum adsorption capacity (mg g−1), respectively.[18] The constant KL describes the affinity between the adsorbent and the target substance.[12]

The Freundlich model is described by the following equation:[46,47]where KF and 1/n are empirical constants expressed the adsorption intensity and .[48]

The experimental results obtained by fitting the Langmuir and Freundlich models are shown in Fig. 10. The affinity and adsorption capacity of l-cyst-ACF for Pb2+ at different temperatures were evaluated. The constants for the two models are summarized in Table 2. The Langmuir model is normally used to evaluate the monolayer adsorption characteristics and energy level of a homogeneous material surface.[49] The R2 value from the Langmuir model was higher than that from the Freundlich model, which indicates the adsorption of Pb2+ was primarily homogeneous and monolayer adsorption. The low KL value suggests a relatively strong interaction between Pb2+ and l-cyst-ACF. Compared with the results in other works, as shown in Table 3, that herein exhibited a higher adsorption effect. The Freundlich model generally describes the multi-layer adsorption of the adsorbent on a heterogeneous surface and that the energy level of the adsorption site is not constant.[43] Meanwhile, the poor fitting data showed that the adsorption was not physical adsorption or multilayer adsorption. Furthermore, the value of 1/n in the three ranges of 0 < 1/n < 1, 1/n = 0 and 1/n > 1 implies favorable, unfavorable and irreversible adsorption, respectively.[50] Thus, it can be predicted that the adsorption behavior was favorable and spontaneous according to the fitting results.

Fig. 10

Adsorption isotherms from (a) Langmuir and (b) Freundlich isotherm models for the adsorption of Pb2+ on the l-cyst-ACF composite. Conditions: [adsorbent] = 0.5 g L−1 [metal] = 100 mg L−1, contact time = 6 h, and pH = 5.5.

The parameters of the isotherm models

Isotherm models	Parameters	303 K	313 K	323 K
Langmuir model	q max (mg g−1)	161.03	167.78	179.53
	K L (L mg−1)	0.1021	0.1342	0.0481
	R 2	0.992	0.991	0.991
Freundlich model	K F (L mg−1)	51.9481	57.4619	38.4964
	1/n	0.2201	0.196	0.2644
	R 2	0.967	0.883	0.857

The comparison of the effect of different adsorption materials

Adsorbent	Fitting model	q max mg g−1	Ref.
Sulfur-ferromagnetic nanoparticles	Langmuir	66.45	51
Chitosan-gelatin aerogels	Langmuir	11.1	52
Agro waste biochar	Freundlich	119.8	53
Microwave-assisted rice straw activated carbon	Langmuir	152.39	54
Nonwoven polyethylene-coated polypropylene fiber	Langmuir	63.36	55
Activated carbon nanofiber	Freundlich	120.3	56
Nitrogen-doped carbon nanofibers	Langmuir	88	57
l-Cysteine-modified activated carbon fiber	Langmuir	179.53	This study

Adsorption thermodynamics

The standard Gibbs free energy change (ΔGθ), entropy change (ΔSθ) and enthalpy change (ΔHθ) were calculated using eqn (9) and (10) to recognize the energetics and spontaneity involved in the procedure for the combination of Pb2+ and the adsorbent.where Kθ represents the constant associated with the thermodynamic equilibrium, which is replaced by KL from the Langmuir fitting.[43]R and T are the universal gas constant [8.314 J (mol−1 K−1)] and the temperature, respectively.[13]

The thermodynamic parameters of adsorption provide an effective method for in-depth understanding of the nature of the adsorption process. The changes on Gibbs free energy (ΔG), enthalpy (ΔH), and entropy (ΔS) values during Pb2+ adsorption was given in Table 4. Accordingly, the calculated adsorption enthalpy and entropy for of Pb2+ adsorption were positive, which indicated that the affinity between metal ions and the material surface was sufficient to make it adhere, and the randomness of the solid-liquid interface increased during this process. Otherwise, negative ΔG value showed the feasibility and spontaneity of the adsorption process, indicating endothermic process which was also predicted before. The endothermic nature of adsorption could be attributed to the increasing temperature that accelerated the diffusion of Pb2+ and the increase of system disorder, which lead to the positive progress of adsorption.

Thermodynamic parameters for the adsorption of Pb2+

Parameter	298 K	308 K	318 K
ΔGθ (kJ mol−1)	−5.75	−5.23	−8.15
ΔHθ (kJ·mol−1)		18.83
ΔSθ (J mol−1 K−1)		43.56

Adsorption mechanism

The adsorption of metal ions on the surface of carbon materials is primarily related to their pore structure and surface groups. According to Fig. 11, the XPS spectra of l-cyst-ACF before and after adsorbing were recorded to gain insight into the mechanism of action between Pb2+ and l-cyst-ACF. The peak positions of Pb 4f 7/2 and Pb 4f 5/2 were detected at 143.78 and 139.03 eV, respectively, which indicate the successful adsorption of Pb2+.[58] As shown in Fig. 11c, the binding energies of C 1s appeared at 284.74, 286.02 and 287.16 eV, which are ascribed to the C–C, C–O, and CO bonds, respectively.[59] Subsequently, the peaks located at 284.63 and 285.35 eV are assigned to C–C and C–O, respectively, suggesting that both bonds almost did not play a role in the adsorption process. Notably, the peak position at 287.16 eV shifted to a higher position at 288.33 eV, which illustrates that the adsorption depends on the CO bond.

Fig. 11

XPS spectra of (a) full survey (b) Pb 4f and (c and d) C 1s (e and f) O 1s (g and h) N 1s and (i and j) S 2p before and after adsorption, respectively.

The high-resolution XPS spectra of O 1s and N 1s before and after the adsorption of Pb2+ are showed in Fig. 11e–h. According to Fig. 11e, three peaks appeared at 531.17, 532.82, and 535.29 eV, which are attributed to the C–O, OC–NH–, and OC–O bonds, respectively.[60] Then, it was clearly demonstrated that the bonding energy positions at 531.94 and 532.93 eV did not change, which suggests that the covalent bonds of C–O and OC–NH– are not involved in the adsorption process. The peak at 535.29 eV shifted to 534.07 eV, which illustrates that the carboxyl group (OC–O–) played a key role during the adsorption process. According to reports, a variety of carbonyl-containing oxygen functional groups, carboxylate and epoxide groups in the adsorbent structure act as electron donors, which lead to surface complexation with metal ions, contributing to the uptake of Pb2+.[15,37,61]

There are three main binding energy positions at 398.63, 399.94, and 401.28 eV in Fig. 11g, which correspond to –NH, C–N, and OC–NH–, respectively.[62] Obviously, these binding energy positions did not exhibit a visible change, as shown in Fig. 11h, which indicates that nitrogen-containing functional groups did not participate in the adsorption process. There are many chemical environments of S in the modified fiber material,[26] such as S–S, C–S, –SH, CS, and SO32−, which were accurately found at 163.74, 164.61, 167.53, 169.05, and 169.95 eV in Fig. 11i, respectively.[26,27] As shown in Fig. 11j, the spectra of S–S and C–S could be fitted with two peaks at 163.45 and 164.31 eV, which represent that these two bonds did not participate in the adsorption of Pb2+. Surprisingly, the binding energy positions at 167.53, 169.05, and 169.95 shifted to lower positions, as shown in Fig. 11j (∼165.57 eV, ∼167.85 eV, and ∼169.08 eV), revealing that –SH, CS, and SO32−, respectively, produced coordinated chelation and electrostatic attraction toward Pb2+. According to the hard soft acid base (HSAB) theory,[63] a metal–ligand complex can be formed between Pb2+ (soft acid with empty track) and surface functional groups, such as –SH, OC–O–, and CS (soft base with free electrons) via covalent bonding. Therefore, the formation of metal–organic complexes greatly improved the adsorption properties of the material.

Reusability and cycling performance

It was very important to evaluate the cycling performance of l-cyst-ACF considering the cost of adsorbents used in practical production. Therefore, adsorption–desorption cycle experiments were carried out on l-cyst-ACF herein, focusing on the reusability and removal efficiency changes. EDTA-2Na salt solution with a concentration of 0.5 mol L−1 was used to desorb l-cyst-ACF saturated with adsorbed species in this study. The changes in the adsorption capacity and adsorption efficiency of the material after 5 adsorption–desorption cycles are summarized in Fig. 12. With an increase in the number of regeneration cycles, the adsorption of lead ions decreased from about 130 mg g−1 to only 80 mg g−1, indicating that the adsorption capacity of l-cyst-ACF for Pb2+ decreased after the fiber underwent multiple elution cycles. We speculated that the functional groups on the fiber surface were lost and some were oxidized and failed during repeated experimental operations. In general, l-cyst-ACF exhibited ideal reusability and has certain prospects in the treatment of lead pollution.

Fig. 12

Reusability performance of l-cyst-ACF-adsorbed Pb2+.

Conclusion

An activated carbon fiber material grafted with l-cysteine was prepared via an amide reaction and the batch adsorption experiments showed that l-cyst-ACF was effective for the removal of Pb2+ from aqueous solution. Adsorption experiments were carried out to investigate different factors such as initial concentration, pH, adsorbent dosage, contact time, and temperature. The experimental results showed that the adsorption effect was better when the pH of the solution was between 5 and 6; a higher temperature was conducive to the adsorption process; the adsorption efficiency was the best when the dosage of adsorbent was 0.5 g L; the adsorption reached equilibrium within 6 h, and qe was 136.80 mg g−1. In addition, l-cyst-ACF had a certain cycling performance after multiple regeneration treatments.

Compared with the pseudo-first-order kinetic equation, it was concluded that the fitting of the pseudo-second-order kinetic equation was more suitable in the adsorption process, implying that the adsorption process was chemisorption. The data from the isothermal models showed that the Langmuir model fitted well, which indicated that the material adsorption process was monolayer adsorption. The thermodynamic analysis showed that ΔG was negative at all temperatures, which indicated that the adsorption process was endothermic and spontaneous. The positive ΔS indicated that the system disorder gradually increased during the adsorption process. Finally, the XPS analysis illustrated that abundant –SH, –COOH, and CS groups on the fiber surface were the crucial factor for the significant improvement in the adsorption capacity.

Conflicts of interest

The authors declare no competing financial interest.