Separation of Lead with a Novel Ion Separating Agent Prepared by Clothing a Chitin Whisker on a Potassium Tetratitanate Whisker.

Separation of Pb2+ from Cu2+-Pb2+ mixed solution by a newly-developed ion separating agent was examined, which was obtained by clothing chitin whiskers (ChW) on the surface of potassium tetratitanate whiskers (PTW). The separation capability and mechanism of the ion separating agent (ChW-PTW) was determined, based on the difference of the adsorption isotherm pattern and the adsorption kinetics model between ChW and PTW on Cu2+ and Pb2+, respectively. The results showed that the adsorption process of ChW could be described by Freundlish isotherm. The adsorption affinity of Cu2+ (kF = 0.085·g-1) on ChW was greater than Pb2+ (kF = 0.077 g-1). The adsorption pattern of PTW was inclined to the Langmuir isotherm, and Pb2+ (kL = 310.59 L·mmol-1) could be obviously more easily adsorbed on PTW than Cu2+ (kL = 25.85 L·mmol-1). The experimental data both fitted well with the pseudo-second order kinetics. The reaction rate of Pb2+ (k₂ = 4.442 for ChW and k₂ = 0.846 for PTW) was greater than that of Cu2+ on both ChW and PTW, while the diffusion rate of intra-particles of PTW was much higher than ChW. The adsorption model of ChW and PTW could illustrate well the separation mechanism of ChW-PTW and allowed for relevant results.

1. Introduction

Separation and recovery of heavy mental ions have always been a significant topic because they are non renewable. There have been some technologies for ions removal from wastewater, such as chemical precipitation, membrane filtration, electrochemistry, adsorption, and so on, in which adsorption has generally been used as an attractive method for industry wastewater treatment. Chen [1] prepared a kind of adsorbent based on copper hexacyanoferrate, which were chemically deposited on the electrode as a film. Metal ions could be adsorbed on the film under the electric power. Li [2] synthesized Cd(II) ion-imprinted polymer with imprinting technology by using allylthiourea as a functional monomer and cadmium chloride as the template. It has higher selectivity for the separation of Cd(II) ions from solutions. However, obvious disadvantages appeared with respect to these methods, such as larger energy consumption, complex processing, and giving rise to the transfer of metal ions into water in the process of preparation and use. Thus, it was necessary to develop a novel adsorbent which was low cost, environmental friendly, simple to prepare, and have good performance for separating metal ions.

Potassium tetratitanate whiskers (PTW) are a kind of crystal with a chainlike and open-stratified structure. It has attracted more attention because it is environmentally friendly, non-toxic, and has strong mechanical properties. The interlayer potassium ions can play an important role in ion exchange with other positive ions, such as Pb2+, Cr2+, Cu2+, and so on [3,4,5,6]. Additionally, PTW has powerful reactivity to be surface modified. Ce3+-imprinted functionalized PTW sorbent was prepared using surface imprinted technology [7] and the surface imprinted polymer composites (MIP/K2Ti4O9) were prepared using dibenzothiophene (DBT) as the template, 4-vinylpyridine as the functional monomer, and potassium tetratitanate whiskers as the carrier [8]; Ogawa et al. intercalated alkylmmonium cations into the layer of titanate [9,10,11,12]. These reports all illustrated that surface modification could promote the ion exchange properties of PTW.

Chitin is a building block of the skeletons of crustaceans, insects, and diatoms. Chitin/chitosan-based materials have been widely applied as adsorbents for heavy metal ions or radioactive elements from wastewater [13,14,15,16]. The high adsorption property of chitin/chitosan-based materials could be attributed to: (i) high hydrophilicity due to the large number of hydroxyl groups of glucose units; (ii) the presence of a large number of functional groups; (iii) high chemical reactivity of these groups; and (iv) the flexible structure of the polymer chain [17]. Gomes [18] studied the interaction between metal cations and chitin/chitosan by means of density functional theory. For chitin, compounds with Cu2+ were more stable than others, and Cu2+ preferred to combine with the oxygen atom of the amide group than the nitrogen atom of the amide group. Wysokowski [19] proposed in their review that chitin-based inorganic-organic materials could be obtained under hydrothermal conditions, such as the formation of chitin/SiO2, chitin/ZrO2, and chitin/ZnO due to hydrogen bonds. Chitin whiskers (ChW) are widely applied as reinforcing agents because of its nontoxicity, biodegradability, and excellent mechanical behavior [20,21], can be obtained by removing the amorphous domains of chitin through acid hydrolysis [22,23,24,25]. Meanwhile, ChW has similar reactivity and adsorbability with chitin because they both have plenty of hydroxyl groups and acetyl amino groups [20,26,27,28,29]. For example, Kalaprasad [30] described the surface chemical modification of hydroxyl on ChW with various reagents to improve applied properties. ChW showed higher adsorption capability for crystal violet compared to other adsorbents [31]. Blending products of ChW and layered rectorite could enhance physicochemical properties of chitosan film due to cooperation effects. Moreover chitin hydrogel could be reinforced with TiO2 nanoparticles to enhance the adsorption of arsenic [32].

To sum up, it is feasible for ChW to combine with PTW as a novel composite material. According to the earlier experimental data, adsorption capacities of PTW for metal ions are much larger than that of ChW. When ChW film is attached to the surface of the PTW, ChW film outside will be like a barrier to block other impurity ions, and pure Pb2+ will enter inside and be adsorbed by PTW. There is almost no literature referring to ion separation by such an organic-inorganic compound adsorbent.

The purpose of the present study was to discuss the separation property and mechanism of the novel ion separating agent, named ChW-PTW, prepared by clothing ChW on the surface of PTW under heating treatment. Lead is one of the most toxic heavy metals and is used in industry widely. It is exhausted quickly with economic development. Thus, it was significant to choose Pb2+ as the subject. Firstly, a batch of adsorption experiments of ChW and PTW on Pb2+ and Cu2+ were conducted to determine the adsorption isotherm pattern and adsorption kinetics model, on which adsorption affinity, adsorption rate constant, and diffusion rate constant could be estimated. Then the separation capability and mechanism of ChW-PTW for Pb2+ from Cu2+-Pb2+ mixed solution was discussed based on the difference of adsorption processes between ChW and PTW on Cu2+ or Pb2+.

2. Experiments

2.1. Materials

Chitin whiskers (ChW) were prepared by a two-step acid-alkali process [13]. Potassium tetratitanate whiskers (PTW) were purchased from Shanghai Dian Yang Industry Co., Ltd. (Shanghai, China). Lead nitrate and cupric nitrate were obtained both from Tianjin Bodi Chemical Limited by Share Ltd. (Tianjing, China).

2.2. Preparation of ChW-PTW

2.2.1. Preparation of ChW

A certain amount of chitin powder was added into 3 N HCl with the material ratio of 1:30 (g:v). The sample was boiled and stirred for 1.5 h to hydrolyze chitin to obtain ChW. Then the mixture of ChW and residual chitin was centrifuged. The milky supernatant was collected and the pH adjusted with sodium hydroxide. Thus, colloidal ChW was obtained. The detailed preparation procedure was described in our previous paper [13].

2.2.2. Preparation of ChW-PTW

A certain amount of PTW was mixed with the emulsion of ChW by stirring under 500 r/min for 1 h. Then the free water in the sample was evaporated under stirring at 300 r/min at 100 °C. After cooling to ambient temperature, the sample was vacuum dried at −0.09 Mpa and 105 °C. The product was added to the emulsion of ChW again, and the above procedures were repeated seven times. The final product was obtained with ChW film clothing on the surface of PTW (ChW-PTW). The product was immersed in the cetyl sodium sulfate liquor with pH = 5–6 for a certain time to remove residual ChW. The product could be used after washing and drying.

2.3. Characterization

Scanning electron microscope (SEM) images were taken on a JEOL JSM-6700F SEM instrument (Japan Electron Optics Laboratory Co. Ltd., Tokyo, Japan), the testing voltage was 12 KV, and the magnification was 2000–50,000 times.

The concentration of Cu2+ and Pb2+ was determined by TAS-986 (Beijing Purkinje General Instrument Co., Ltd., Beijing, China) under room temperature.

2.4. Difference of Adsorption Property between ChW and PTW

The difference of the equilibrium adsorption isotherm and adsorption kinetics between ChW and PTW was studied to analyze the separation mechanism of ChW-PTW for Pb2+ from Cu2+-Pb2+ mixed solution. The absorption process can be expressed by formulas, as follows: 2Chi- + M K where Chi- are activated adsorption sites on the surface of ChW; M2+ represents metal ions.

2.4.1. Adsorption Isotherm

The equilibrium adsorption isotherm tests were conducted by transferring 0.10 g adsorbents and 20 mL Cu2+ or Pb2+ solution (0.15–2.5 mmol/L) to triangular flasks in a temperature-controlled orbital shaker (150 rpm). Experiments were performed at 25 °C for 48 h.

Langmuir, Freundlish, and Temkin equations (Equations (3)–(5), respectively) were used to estimate the isotherm parameters for ChW/PTW on Cu2+ or Pb2+. where q and q are the equilibrium and maximum monolayer adsorption capacities (mmol/g), respectively; C is the equilibrium concentration of mental ions in the solution (mmol/L); b is the Langmuir adsorption equilibrium constant that is related to the binding energy (L/mg); K is the Freundlich constant that is related to the adsorption capacity (mmol/g); and n is the adsorption intensity parameter.

2.4.2. Adsorption Kinetics

Adsorption kinetics experiments were carried out by blending 0.10 g adsorbent with 20 mL Cu2+ or Pb2+ solution (0.94 mmol/L). The samples were shaken at 25 °C for 10 min, 20 min, 40 min, 60 min, 90 min, 180 min, and 360 min, respectively.

Pseudo-first-order (Equation (6)) and pseudo-second-order (Equation (7)) equations were used to discuss the adsorption rate constant of Cu2+ or Pb2+ on ChW/PTW. Webber-Morris model (Equation (8)) was used to study intra-particle diffusion model, as follows: where q is the adsorption quantity at time t (mmol/g); t is the contact time (min); k1, k2 are reaction rate constant of pseudo-first-order model (min−1) and pseudo-second-order model (g/mg·min), respectively; k is intra-particle diffusion rate constant (mmol/g·min0.5); and C is the constant related to the thickness of the boundary layer (mmol/g).

2.5. Separation of Double-Ions-Mixed Solution

2.5.1. Ionic Adsorption

The separation experiments were operated by immersed 0.10 g ChW-PTW into 20 mL of the mixed solution with 1.888 mmol/L of Cu2+ and 0.944 mmol/L of Pb2+, respectively. Then the samples were oscillated under 25 °C for a certain time. Monitoring the concentration of Cu2+ and Pb2+ in the supernatant to estimate the adsorption quantity of ChW-PTW.

2.5.2. Determination of Separation Capability

ChW-PTW, which had adsorbed the mixed ions in the adsorption process, was collected and dried at 80 °C, then transferred into HNO3 (pH = 1) and vibrated at 25 °C for 12 h to peel off ChW from the surface of PTW. ChW would enter into the supernatant to form an emulsion while PTW settled to the bottom. The emulsion and the sediment were separated, purified, and dried to obtain ChW and PTW, respectively. ChW and PTW were immersed into 5 mol/L HNO3 alone for 24 h to desorb Cu2+ and Pb2+. The concentration of Cu2+and Pb2+ in both solutions was detected to assess the adsorption quantity of the ChW film and PTW layer, and then the separation ability of the sorbent was estimated.

3. Results and Discussions

3.1. Morphological and Structural Characteristics

The morphology of ChW, PTW, and ChW-PTW are shown in the Figure 1. It can be revealed in Figure 1a that the length of the ChW is about 80 nm to 300 nm. It is well distributed and takes on a membrane shape. It can be seen from the Figure 1b that PTW has a smoother and larger surface than ChW, and it presents stiff rod-like. In the Figure 1c, it shows the morphology of ChW-PTW from an overall perspective and a partially enlarged view. Obvious coalescence between ChW and PTW occurs. ChW is even-distributed on the surface of PTW and clads PTW as a film.

Figure 1

The SEM of (a) ChW; (b) PTW; and (c) ChW-PTW.

ChW has enough activity binding sites, such as hydroxyl, acetyl, and amidogen, and there is powerful electronegativity on the surface of PTW due to Ti-O. When PTW was mixed with ChW emulsion completely and operated by heating treatment, a new composite material was obtained by hydrogen bonding between ChW and PTW.

3.2. The Adsorption Property of ChW and PTW

The optimal adsorption conditions were determined, when 0.1 g of adsorbent was added into 20 mL solution with a concentration of 1.0 mmol/L, optimal pH of the solution was 5–6, the suitable temperature was 25 °C, and the time needed to reach equilibrium was 2–3 h. At this time, the adsorption capacities and comparison with other adsorbents were listed in Table 1.

Table 1

The adsorption capacities of ChW, PTW, and a comparison with other adsorbents.

Samples	Adsorption Capacities mmol/g	Reference
ChW-Cu	0.080	-
ChW-Pb	0.075	-
PTW-Cu	0.362	-
PTW-Pb	0.296	-
Mg2Al–LS–LDH composite-Cu	1.000	[33]
Mg2Al–LS–LDH composite-Pb	0.594	[33]
Peat-Pb	0.398	[34]
Lignin/inorganic oxide system-Cu	1.312	[35]

It can be seen from Table 1 that adsorption capacities of PTW for Cu2+ and Pb2+ are both much larger than that of ChW. This difference will contribute to the ion separation. To analyze the separation process of the composite, it is necessary to research each removal and diffusion pattern of ChW and PTW.

Compared with other adsorbents, the adsorption capacities are lower, possibly because that: (1) adsorbability of ChW itself is weaker than chitin; (2) before preparing of the composite material, ChW and PTW were both unground. The composite material was also unground, because the structure of the composite was very important to assure the separation degree. As contrast samples, ChW and PTW were unground when batch of experiments were carried out for isotherm and kinetics.

The symbols used in adsorption isotherm and kinetics were listed in Table 2.

Table 2

Symbol descriptions.

Symbol	Description	Unit
kL	The adsorption affinity	L·mmol−1
kF	Characterization of adsorption capacity	g−1
At	The maximum adsorption equilibrium constant	L·mmol−1
qe	Adsorption capacity	mmol·g−1
k1	Reaction rate constant for pseudo-first-order kinetic	min−1
k2	Reaction rate constant for pseudo-second-order kinetic	g·min·mmol−1
R2	Correlation coefficient transformation	-
E2	The estimate of the error variance	-

3.2.1. Adsorption Isotherm

The adsorption isotherm curves of Langmuir, Freundlich and Temkin for ChW and PTW are revealed in Figure 2. Figure 2a,b correspond to the adsorption process of ChW on Cu2+ and Pb2+, respectively. According to the parameters in Table 3, the correlation coefficient (R2) of the Freundlich model for ChW is 0.998 for Cu2+ and 0.999 for Pb2+, which is slightly larger than that of Langmuir and Temkin, indicating that the absorption pattern of ChW for Cu2+ and Pb2+ is more inclined to the Freundlich adsorption model. In this case, kF was 0.085 g−1 for Cu2+ and 0.077 g−1 for Pb2+, that is to say, binding activity of Cu2+ on ChW is stronger than that of Pb2+.

Figure 2

The adsorption isotherm of ChW and PTW. (a) ChW-Cu2+; (b) ChW-Pb2+; (c) PTW-Cu2+; and (d) PTW-Pb2+.

Table 3

The parameter of the adsorption isotherm.

Isotherm Type	Parameter	ChW		PTW
		Cu2+	Pb2+	Cu2+	Pb2+
Langmuir	kL	16.725	1.574	25.851	310.59
	R2	0.994	0.943	0.997	0.999
	E2	4.65 × 10−4	1.93	6.90 × 10−3	3.00 × 10−3
Freundlich	kF	0.085	0.077	0.364	0.363
	n	6.011	1.676	16.484	5.141
	R2	0.998	0.999	0.926	0.744
	E2	2.00 × 10−4	2.00 × 10−4	1.10 × 10−3	0.61
Temkin	BT	2.91 × 105	1.08 × 105	1.43 × 105	1.03 × 105
	R2	0.988	0.92	0.878	0.907
	E2	1.00 × 10−4	1.00 × 10−4	8.00 × 10−4	1.50 × 10−3
	At	1.99 × 104	32.73	1.0 × 109	2.64 × 105

The absorption pattern of PTW on Cu2+ and Pb2+ fits well to the Langmuir model, as shown in the Figure 2c,d and Table 3. At this time, the kL was 25.85 L·mmol−1 for Cu2+ and 310.59 L·mmol−1 for Pb2+, indicating that Pb2+ can be captured by PTW much more firmly than Cu2+.

The adsorption pattern of ChW on Cu2+ and Pb2+ is in accordance with the Freundlich isotherm, and Cu2+ will be adsorbed more easily than Pb2+. The adsorption pattern of PTW on Cu2+ and Pb2+ can be represented by the Langmuir isotherm, and the adsorption of Pb2+ was much stronger than that of Cu2+.

3.2.2. Adsorption Kinetics

Figure 3 shows the adsorption kinetics curves of ChW or PTW on Cu2+ and Pb2+. Relevant parameters for pseudo-first-order and types 1–4 of pseudo-second-order were shown in the Table 4. All of the models fit the experiment data very well. However considering the conformity of data and the calculated values expressed by the correlation coefficient (R2), the pseudo-second-order kinetics are more suitable for describing the adsorption behaviors of both ChW and PTW. The results illustrate that ions can combine with active sites on ChW or PTW by covalent chemical bonds [2].

Figure 3

The kinetics curves of ChW and PTW. (a) ChW-Cu2+; (b) ChW-Pb2+; (c) PTW-Cu2+; and (d) PTW-Pb2+.

Table 4

The parameters for pseudo-first-order and types 1–4 of pseudo-second-order.

Kinetics Type		Parameter	ChW		PTW
			Cu2+	Pb2+	Cu2+	Pb2+
		qe, exp	0.080	0.046	0.137	0.145
Pseudo-first-order		qe, cal	0.068	0.1016	0.068	0.067
		k1	0.075	0.046	0.075	0.136
		R2	0.878	0.927	0.878	0.877
Pseudo-second-order	Type 1	qe, cal	0.083	0.047	0.141	0.149
		k2	1.152	6.518	0.750	0.772
		R2	0.999	0.999	0.999	0.999
		h	0.008	0.014	0.015	0.015
	Type 2	qe, cal	0.083	0.049	0.139	0.144
		k2	1.162	3.553	0.825	0.846
		R2	0.995	0.988	0.988	0.934
		h	0.008	0.008	0.016	0.018
	Type 3	qe, cal	10.500	5.878	8.873	8.957
		k2	1.153	3.495	0.810	0.763
		R2	0.995	0.988	0.988	0.934
		h	127.127	120.729	63.778	61.195
	Type 4	qe, cal	−0.028	−0.039	−0.036	3.602
		k2	5.351	7.569	3.740	3.602
		R2	0.982	0.979	0.954	0.890
		E2	0.004	0.011	0.015	0.005

Note: 1. The bold values are related with the parameters of the pseudo-second order kinetic model of type 1 which preferably describes the realized process of adsorption as compared to bold experimental data. 2. h is the initial adsorption rate, h = k2q2.

As for the pseudo-second-order kinetics, k2 and q can be calculated from the plots for the linear forms of pseudo-second-order kinetics models of types 1–4 [34] given in Table 5. The values of k2, q, h, and qe, cal obtained from the four linear forms of pseudo-second-order equations were found to be different. Giving consideration to both correlation coefficients and differences between the experimental (qe, exp) and calculated sorption capacities (qe, cal), the adsorption of ChW based on Cu2+ and Pb2+ better fits type 1, while adsorption of PTW can be described by type 2. Pseudo-second-order models of types 3–4, although the high values of their correlation coefficients, cannot be taken into consideration because of the larger differences between the experimental and calculated sorption capacities.

Table 5

Linear forms of the pseudo-second-order kinetics model.

Type of Kinetics Pseudo-Second-Order	Linear Form	Plots
Type 1	tq_t=1k_2qe2+tq_e	tq_t vs. t
Type 2	1q_t=(1k_2qe2)1t+1q_e	1q_t vs. 1t
Type 3	1t=k_2qe2q_t−k_2qe2q_e	1t vs. 1q_t
Type 4	q_tt=k_2qe2−k_2qe2q_e	q_tt vs. q_t

The reaction rate constant (k2) of ChW on Cu2+ is 1.152, much lower than that of Pb2+ (6.518), while k2 of PTW on Cu2+ is 0.825, slightly smaller than that of Pb2+ (0.846). Demonstrating that Pb2+ can be more rapidly captured on both available adsorption sites of ChW and PTW than the adsorption of Cu2+.

Weber-Morris model is applied to determine the rate-limiting step in this adsorption system, which represents the time dependent intra-particle diffusion of the solvend. If the Weber-Morris curve of q (mmol/g) against t0.5 (min0.5) gives a straight line, the adsorption process is diffusion controlled. If the plot is multi-linear and the lines do not pass through the origin, then a combination of two or more processes influence the adsorption [36].

Multi-linear relationships that have three different linear regions with different slopes are shown in Figure 4. The intra-particle diffusion rate constants (kind1, kind2, kind3) correspond with the diffusion rates which can be calculated from the slopes of the linear curves and changes in different adsorption stages. The diffusion rate constants are presented in Table 6, along with the correlation coefficients. The initial region (0–10 min) is the sharpest and corresponds to the external adsorbate diffusion in the boundary layer. That is, ions could quickly diffuse to exposed adsorption sites on the surface, and kind1 of Pb2+ towards PTW is significantly higher than that of Pb2+ towards ChW. The second region (20–90 min) relates to the gradual adsorption stage in which the intra-particle diffusion is potentially the rate-limiting step. When the external surface is nearly saturated, the ions gradually pass through the surface pores and will be retained in the micropores of the particles. At this stage, the diffusion resistance increases and the diffusion rate decreases. kind2 of ChW-Pb2+ decreases from 0.0106 mmol/g·min0.5 to 0.0016 mmol/g·min0.5, reduces to about 15%. In contrast, kind2 of PTW-Pb2+ decreases from 0.0247 mmol/g·min0.5 to 0.0114 mmol/g·min0.5, reduces to about 46%, illustrating that after 20 min, the diffusion resistance of Pb2+ on ChW will be far greater than on PTW. The third region (>90 min) is a plateau that represents the final equilibrium stage, kind3 especially of the adsorption ChW reduce to nearly zero. By contrast, PTW can absorb ions continuously at this stage (kind3 was 0.001 mmol/g·min0.5 for both Cu2+ and Pb2+).

Figure 4

The kinetics curves of ChW and PTW based on the Weber-Morris pattern. (A) ChW-Cu2+; (B) ChW-Pb2+; (C) PTW-Cu2+; and (D) PTW-Pb2+.

Table 6

The intra-particle diffusion for ChW and PTW on Pb2+and Cu2+.

Samples	kind1	C1	R12	kind2	C1	R22	kind3	C3	R32
ChW-Cu2+	0.012	−0.002	0.9169	0.003	0.042	0.9643	0	0.077	1
ChW-Pb2+	0.011	−0.001	0.9495	0.002	0.032	0.9013	0	0.047	1
PTW-Cu2+	0.022	−0.004	0.9104	0.009	0.051	0.9911	0.001	0.118	0.8976
PTW-Pb2+	0.025	−0.003	0.9509	0.011	0.042	0.9863	0.001	0.126	0.7363

3.3. The Separation Effect of Double-Ion-Mixed Solution

The separating capability of ChW-PTW on Pb2+ from Cu2+-Pb2+ mixed solution is discussed in Figure 5. As shown in the Figure 5a, the overall adsorption rate of ChW-PTW on Pb2+ is quicker than that of Cu2+. When the time reaches 160 min, the adsorbance of Pb2+ can be up to 0.046 mmol/g, more than that of Cu2+. This outcome can be explained by the test data of adsorption kinetics, as the adsorption rate constant of Pb2+ on ChW or PTW is both larger than that of Cu2+.

Figure 5

The adsorption capacity of ChW-PTW among Cu2+ and Pb2+ in a double-ion-mixed solution. (a) Adsorbing capacity of ChW-PTW with time; (b) the percentages of Cu2+ and Pb2+ in ChW film; and (c) the percentages of Cu2+ and Pb2+ in the PTW layer.

The relative percentage quantity of Cu2+ and Pb2+ in the ChW film on the surface of PTW is shown in Figure 5b. The relative mass percent of Cu2+ gradually reduces as time progresses, while that of Pb2+ gradually increases. Figure 5c shows the relative percentage quantity of Cu2+ and Pb2+ in the inner PTW layer. When adsorbed within 90 min, the mass percent of Pb2+ was 100%, but when the time was prolonged to 120 min, Cu2+ could pass through the ChW film and permeate into the PTW layer.

In summary, Pb2+ can be adsorbed more quickly on ChW-PTW than Cu2+ and is more inclined to be combined on the PTW layer. When adsorbing within 90 min, ions on the PTW are pure Pb2+. Thus, ChW-PTW will be a promising ion separating agent, and can play an important role to purify Pb2+.

3.4. The Possible Separation Mechanism of ChW-PTW

Based on the isotherm patten and kinetics model of ChW and PTW, (1) the reaction rate of Pb2+ is greater than that of Cu2+ on both ChW and PTW; (2) the adsorption affinity between Cu2+ and ChW is much larger than that of PTW; (3) PTW has greater advantage to adsorb Pb2+; (4) the diffusion resistance of Pb2+ in the intra-particle of PTW is much smaller than ChW in the second stage; and (5) the third stage begins after adsorbing 90–120 min. At this time, adsorption of Cu2+ on ChW is over, and Cu2+ can pass through the ChW film and permeate into the PTW layer.

When Cu2+ and Pb2+ contacted with the composite material ChW-PTW, the ChW film could catch Cu2+ firmly and block Cu2+ from entering into the PTW layer. Most of the chelation sites of ChW could be occupied by Cu2+. On the other hand, Pb2+ would adsorb on the ChW layer prior to Cu2+, but the adsorption capability (kF) and diffusion rate (kind2) of Pb2+ on ChW was less than Cu2+, moreover, the diffusion rate (kind2) of Pb2+ on PTW was much larger than on ChW. Then partial Pb2+ chelated on the residual active sites of external ChW film quickly, other Pb2+ would continuously transfer into the interior-ChW-PTW and adsorbed on the PTW layer by ion exchange. The possible separation process and mechanism of the double-ion-mixed solution is revealed in the Figure 6.

Figure 6

The separation process and mechanism of the double-ion-mixed solution.

4. Conclusions

A newly-developed ion-separating agent was prepared by clothing ChW on the surface of PTW. The microstructure of the product (ChW-PTW) was observed by scanning electron microscope (SEM). The separation capability and mechanism of ChW-PTW on Pb2+ from mixed solution was discussed on the foundation of the difference of the adsorption isotherm pattern and adsorption kinetics model between ChW and PTW on Cu2+ and Pb2+, respectively.

The results show that: (1) ChW can form a kind of compact film, and is well-distributed on the surface of PTW; (2) the reaction rate of Pb2+ is greater than that of Cu2+ on both ChW and PTW, while the binding affinity between Cu2+ and ChW is larger, and PTW has greater advantage to adsorb Pb2+; (3) the different reaction rate and binding affinity could explain the separation mechanism perfectly; (4) the intra-particle diffusion resistance of Pb2+ on PTW is much smaller than on ChW; and (5) the ion separating agent prepared by ChW and PTW was promising to remove Pb2+ from Cu2+-Pb2+ mixed solutions. There were pure Pb2+ on the inner PTW layer when adsorbed within 90 min. This material could successful employed in water pollution control or in purifying of Pb2+ ions from industry wastewater.