Journal of Nanomaterials
Volume 2015 (2015), Article ID 498304, 13 pages
http://dx.doi.org/10.1155/2015/498304

Research Article

Adsorption of Organic Dyes by TiO₂@Yeast-Carbon Composite Microspheres and Their In Situ Regeneration Evaluation

Zheng Pei,¹ Zhang Kaiqiang,¹ Dang Yu,¹ Bai Bo,² Guan Weisheng,¹ and Suo Yourui²

¹College of Environmental Science and Engineering, Chang’an University, Xi’an 710054, China
²Northwest Plateau Institute of Biology, Chinese Academy of Sciences, Xining 810001, China

Received 21 July 2014; Revised 9 September 2014; Accepted 1 October 2014

Academic Editor: Jinmei He

Copyright © 2015 Zheng Pei et al. This is an open access article distributed under the Creative Commons Attribution License, which permits unrestricted use, distribution, and reproduction in any medium, provided the original work is properly cited.

Abstract.

TiO₂@yeast-carbon microspheres with raspberry-like morphology were fabricated based on the pyrolysis method. The obtained products were characterized by field emission scanning electron microscopy (FE-SEM), energy dispersive spectrometry (EDS), and X-ray diffraction (XRD). Effects of initial dye concentration and contact time on adsorption capacity of TiO₂@yeast-carbon for cationic dye methylene blue (MB) and anionic dye congo red (CR) were investigated. Experimental data were described by Langmuir, Freundlich, Temkin, and Koble-Corrigan isotherm models, respectively. It was found that the equilibrium data of MB adsorption were best represented by Koble-Corrigan, and CR adsorption was best described by both Freundlich and Koble-Corrigan isotherm models. The kinetic data of MB and CR adsorption fitted pseudo-second-order kinetic model well. The results demonstrated that TiO₂@yeast-carbon microspheres achieved favorable removal for the cationic MB in comparison with that for the anionic CR. In addition, regeneration experimental results showed that TiO₂@yeast-carbon exhibited good recycling stability, reusability, and in situ renewability, suggesting that the as-prepared TiO₂@yeast-carbon might be used as the potential low cost alternative for recalcitrant dye removal from industrial wastewater. One possible mechanism for regenerating dye-loaded TiO₂@yeast in situ was also proposed.

1. Introduction

Organic dyes are widely and frequently used in various industries as textile, printing, petroleum, paper, and rubber [1, 2]. During the manufacturing and dyeing process, a substantial amount of dyestuff is lost into water, which poses a great threat to the environment. Typically, the presence of these toxic organic compounds reduces light penetration into water, affects photosynthesis of aquatic lives, impedes the growth of microbes, creates toxicity to fish, accumulates in the food chain, and even travels long distance, causing harm not only to the place where they are produced and used but also globally [3]. Moreover, most of the organic dyes are recalcitrant and difficult to degrade because of their complex and stable aromatic molecular structure [4]. Hence, the removal or degradation of organic dyes from water bodies has become a major environmental problem. Till now, some physical or chemical strategies have been attempted to remove dye contaminants from water, including adsorption [5], advanced oxidation process (AOP) [6], membrane filtration [7], ozonation [8], and coagulation-flocculation [9]. Among the above-mentioned technologies, adsorption has been proven to be one of the most efficient and reliable methods for removing dyes from aqueous solution because of its flexibility, high efficiency, ease of operation, simplicity of design, and insensitivity to toxic pollutants [10]. A wide variety of low cost and easily available materials, such as bentonite [11], fly ash [12], clay [13], active carbon [14], and agriculture wastes [15, 16], have been exploited for the removal of dyes from aqueous solutions.

Yeast-carbon is a porous and amorphous solid carbon material, which is derived mainly from baker’s yeast. For example, Nacco and Aquarone [17] firstly reported the fabrication of yeast-carbon by carbonizing yeast cells in gas-heated muffle. The prepared yeast-carbon exhibited larger surface area. Guan et al. [18] synthesized amphiphilic porous hollow carbonaceous spheres via mild hydrothermal treatment of yeast cells and further pyrolyzing. The obtained carbon spheres displayed effective sorption of phenol from water. In comparison with the great successes in the yeast-carbon synthesis, the practical application of yeast-carbon as adsorbent in wastewater treatment has still been limited because the adsorbent could get saturated easily in the adsorption process, which requires extra regeneration or complete replacement [4]. More recently, TiO₂ has become a hot topic mainly for its excellent photocatalytic performance [19]. The integration of adsorption and TiO₂ photocatalysis seems to offer a good solution to overcome the shortcoming of extra regeneration or complete replacement from the traditional adsorption process. In such a synergetic process, the rich pore structure of adsorbents might promote the transfer and adsorption of organic dyes, while the TiO₂ could destroy dyes by photocatalytic oxidation, thus regenerating the adsorbent in situ [20].

In the previous work, we fabricated the novel TiO₂@yeast-carbon microsphere with raspberry-like morphology based on the pyrolysis method [21]. In the present work, as a continual job, the prepared hybrid raspberry-like TiO₂@yeast-carbon microspheres were further used as adsorbents for removal of two typical organic dyes (Methylene blue and Congo red) from aqueous solution. The adsorption equilibrium isotherms and kinetics was fully conducted. Moreover, in situ regeneration of the adsorbents was investigated, and one possible mechanism for regenerating dye-loaded TiO₂@yeast in situ was also proposed.

2. Materials and Methods

2.1. Materials

The powdered yeast was provided by Angel Yeast Co. TiO₂ with the primary particle size at 20–30 nm was from Degussa and was used without further purification. Absolute ethanol and double-distilled water were used throughout all the experimental procedures. Methylene blue (MB) and Congo red (CR) were purchased from Xi’an Chemical Agent Company and were used as pollutants in the present work. Analytic grade sodium hydroxide (NaOH) and sulfuric acid (H₂SO₄) were purchased from Xi’an Chemical Agent Company.

2.2. Synthesis of TiO₂@Yeast-Carbon Microspheres

In a typical synthesis procedure, 0.1 g of TiO₂ was dissolved in 200 mL of distilled water, using ultrasonic vibration for 10 min, and the pH value was adjusted to approximately 9-10 by adding dropwise sodium hydroxide (1.0 mol/L). Then, the dispersion was stirred in magnetic stirrers for 30 min to facilitate particle deaggregation. In a separate vessel, 1.25 g yeast powder was washed with distilled water and absolute ethanol for three times, respectively. Subsequently, the yeast was dispersed in 200 mL of distilled water and magnetically stirred vigorously for 30 min, and the pH value was adjusted to approximately 3 with sulfuric acid (1.0 mol/L). After that, the above TiO₂ and yeast cells were gathered by centrifugation from their own suspensions and redispersed in 200 mL of distilled water, respectively. Thereafter, TiO₂ and yeast suspensions were slowly mixed with continuously magnetic stirring for 1.5 h at room temperature and left for 3.0 h without further stirring in order to ensure the formation of TiO₂@yeast particles. The mixture was collected by centrifugation, washed with distilled water and absolute ethanol for three times, and then desiccated at 353 K for 1.0 h. Finally, the dried TiO₂@yeast particles were calcined at 573 K in a nitrogen pipe furnace for 1.0 h and cooled to room temperature. After that, TiO₂@yeast-carbon hybrid microspheres were obtained. For comparison, the yeast-carbon was prepared by similar method without adding TiO₂.

2.3. Characterization

Surface structure and morphology of samples were observed by using Philip XL-30 field emission scanning electron microscope (FE-SEM). Detailed composition characterization was carried out with energy-dispersive spectroscopy (EDS) analysis. X-ray diffraction (XRD) patterns were conducted on X. Pert Pro diffractometer using Cu Kα radiation ( nm) at a scanning rate of 10°/min.

2.4. Dye Solution Preparation

Methylene blue and Congo red were cationic and anionic dyes, respectively, and were used as model pollutants to study the adsorption properties of TiO₂@yeast-carbon microspheres. The structures of both dyes are shown in Figure 1. Stock MB and CR solutions (1.0 g/L) were prepared by dissolving 1 g of MB or CR in 1 L of double distilled water, respectively. Experimental solutions of desired concentration were obtained by further dilution.

(a)

(b)

Figure 1: The structures of dyes: (a) MB and (b) CR.

2.5. Analysis of Organic Dyes

The samples were separated from the solution at set intervals with centrifugation at 3000 rpm for 5 min and were returned to the reaction system immediately after each analysis. The concentrations of MB and CR in the supernatant solution were determined using a double beam UV/visible spectrophotometer (UV-752, Shanghai) at 666.4 nm and 499.0 nm, respectively. Calibration curve was found to be very reproducible and linear over the concentration range used in this work.

2.6. Batch Adsorption Experiments

Adsorption studies were carried by adding 0.25 g TiO₂@yeast-carbon microspheres and 100 mL MB or CR solution of certain concentration into a set of flasks followed by stirring in magnetic stirrers at room temperature without adjusting the solution pH. The flasks were wrapped in aluminum foil to prevent photolysis. After desired adsorption time, 5 mL sample supernatant was taken out to analyze the residual concentration of MB or CR. In all sets of experiments, each test was conducted in duplicates, and the mean value was recorded. The amount of adsorbed dye per gram TiO₂@yeast-carbon hybrid microspheres at equilibrium (, mg/g) and at time (, mg/g) was calculated by the following equation:

where , , and (mg/g) are concentrations of dye at initial, equilibrium, and time , respectively. (L) is the volume of the dye solution, and (g) is the mass of adsorbent.

2.7. In Situ Regeneration of TiO₂@Yeast-Carbon Microspheres

In order to evaluate the reusability and renewability of the TiO₂@yeast-carbon, MB was chosen as the model pollutant. The procedure is as follows: an amount of 0.14 g of prepared TiO₂@yeast-carbon was suspended in a MB solution (100 mL) with an initial concentration of 2 mg/L in a beaker. The solution was magnetically stirred in dark for about 2.5 h to ensure the establishment of an adsorption-desorption equilibrium. Then, the mixed suspensions were irradiated under a UV lamp (Philips TL 8W/08F8T5/BLB; 0.0155 m bulb diameter, 0.26 m bulb length, and 1.2 W UVA output) located directly above the flasks at a distance of 6 cm from the surface of the solution. The aqueous samples were taken out at a regular interval time and analyzed until a second equilibrium was achieved, which meant that a cycle was over. At the end of each run, the dye-loaded TiO₂@yeast-carbon microspheres were collected by centrifugation, washed thoroughly, and dried to be reused in the next cycle. Another cycle of sorption-regeneration was repeated in the same manner as mentioned above. All of the experiments were performed in triplicate at room temperature. The removal rate of MB was calculated by the following equation:

3. Results and Discussion

3.1. Characterization

Figure 2(a) is the SEM images of yeast-carbon. It reveals that the yeast-carbon had smooth surface morphology and uniform size (length =  μm; width =  μm). Figure 2(b) depicts an image of the TiO₂@yeast which is the precursor of TiO₂@yeast-carbon. The size of TiO₂@yeast (length =  μm; width =  μm) increased compared with the yeast-carbon in Figure 2(a), which may be assigned to the attachment of TiO₂ particles. Figure 2(c) presents an overall image of the TiO₂@yeast-carbon hybrid microspheres. The micrograph in Figure 2(c) indicates that the particles inherited the general shape and good dispersity of the precursor in Figure 2(b). Figures 2(d) and 2(e) expresses the TiO₂@yeast-carbon spheres in different magnifications. The TiO₂@yeast-carbon in Figure 2(d) exhibits a typical raspberry-like structure since the TiO₂ nanoparticles were randomly decorated on the surface of carbon microspheres. Figure 2(f) displays the detailed information of the outer appearance of the TiO₂@yeast-carbon microspheres under a higher magnification. It can be clearly seen that the surfaces of the microspheres were coated with small TiO₂ particles, whereas some residual bare areas still remained. These residual bare regions were of great benefit to the adsorption of dye molecules in aqueous solution.

(a)

(b)

(c)

(d)

(e)

(f)

Figure 2: FE-SEM images of (a) the yeast-carbon, (b) general observation of the raspberry-like TiO₂@yeast precursor, (c) the overall view of the raspberry-like TiO₂@yeast-carbon microspheres, (d-e) the selected raspberry-like TiO₂@yeast-carbon microspheres, and (f) typical raspberry-like TiO₂@yeast-carbon microspheres observed under high magnifications.

Additionally, the unique raspberry-like structure of TiO₂@yeast-carbon is further confirmed from the EDS analysis. In the insert image in Figure 2(a), C, O, Zn, P, and Pt elements can be observed. C, O, and P result from the yeast cells, Zn element comes from the yeast cells activation agent ZnCl₂, and Pt is assumed to be due to the metal spraying before SEM studies. C, O, P, and Ti elements are observed in the insert image in Figure 2(d). C, O, and P elements also derive from the yeast, and the Ti element detected indicates that TiO₂ has been already successfully coated on the yeast carbon.

XRD patterns of TiO₂, yeast, yeast-carbon, and TiO₂@yeast-carbon are shown in Figure 3. Diffraction peaks at around 20° in Figures 3(a) and 3(b) indicate the formation of amorphous species. Figure 3(c) illustrates an XRD pattern of TiO₂@yeast-carbon. The broad peak at 20° is mainly caused by the amorphous structure of yeast-carbon. Moreover, the remaining diffraction peaks are in good agreement with TiO₂ in Figure 3(d) and no other diffraction peaks can be detected within the investigated range. Figure 3(d) exhibits the XRD pattern of the original components of TiO₂ nanoparticles (P25 TiO₂: 78% anatase-type TiO₂ and 22% rutile-type TiO₂). The observed sharper diffraction peaks at 25°, 37.9°, 48.2°, 54.8°, and 63.0° are consistent with diffraction peaks of anatase-type TiO₂ (JCPDS. number: 21-1272) [22], and the other diffraction peaks centering at 69.0°, 70.3°, and 75.0° correspond well with the reflections of rutile-type TiO₂ (JCPDS. number: 21-1276) [23].

Figure 3: XRD patterns for (a) the premier yeast; (b) the prepared yeast-carbon; (c) TiO₂@yeast-carbon; (d) the pure TiO₂.

3.2. Adsorption Capacity of MB and CR on TiO₂@Yeast-Carbon

Figure 4 describes the measured isotherms for MB and CR on the TiO₂@yeast-carbon samples at the same initial dye concentration. From Figure 4, for MB and CR increased dramatically during the initial time. Then, MB and CR adsorption reached equilibrium at the time of about 80 and 130 min, respectively, which was similar to observations of Hameed et al. [24]. As shown in Figure 4, two adsorption stages existed obviously: a very rapid initial adsorption over a few minutes, followed by a longer period of much slower uptake. The rapid uptake at the initial contact time could be ascribed to the fact that there were plenty of available adsorption active sites on the surface of TiO₂@yeast-carbon, while the slow rate of dye adsorption was probably due to the repulsive forces between the dye molecules in the solution and on the surface of the TiO₂@yeast-carbon [25]. It can also be seen from Figure 4 that the adsorption capacity of cationic dye MB by TiO₂@yeast-carbon was significantly higher than that of anionic dye CR, as manifested by the approximately 3-fold higher adsorption capacity of the CR, which could be assigned to the negatively charged surface of the adsorbent [21, 26]. Moreover, because the CR possesses more polar atoms (N and S), the interaction between CR and TiO₂@yeast-carbon may be stronger than that between MB and TiO₂@yeast-carbon. This may induce a collapse in the pore structure of TiO₂@yeast-carbon and then create a sharp decrease in the adsorption capacity. It is noteworthy that the adsorption capacity of MB on TiO₂@yeast-carbon is similar to that of Basic Green 5 measured by Juang et al. [27]. According to the adsorption results above, it is experimentally demonstrated that TiO₂@yeast-carbon may be a good adsorbent for the removal of MB even if no chemical modification is taken.

Figure 4: Adsorption isotherms for MB: (a) and CR: (b) on TiO₂@yeast-carbon.

The favorable removal of cationic MB in comparison with the anionic CR by TiO₂@yeast-carbon adsorbent can be further verified by changing of initial dye concentration. Figure 5 illustrates the influence of dye concentration on adsorption capacity of TiO₂@yeast-carbon nanocomposite for MB and CR. As shown in Figure 5, the adsorption capacity for MB and CR augmented with the increase of dye concentration, which could be explained by the elevated concentration gradient between the bulk solution and the surface of the TiO₂@yeast-carbon [25]. As presented in Figure 5, the adsorption of MB on TiO₂@yeast-carbon showed higher capacity than CR within the investigated concentration. However, the adsorption capacity for MB or CR is sure to reach a constant if the dye concentration exceeds continuously because a certain amount of TiO₂@yeast-carbon could only provide limited active adsorption sites.

Figure 5: Influence of adsorbate concentration on adsorption capacity of TiO₂@yeast-carbon nanocomposite for MB and CR.

3.3. Adsorption Isotherms

Adsorption isotherm models are important to investigate how adsorbates interact with adsorbents [28] and are widely used to describe the adsorption progress [10]. Langmuir, Freundlich, Temkin, and Koble-Corrigan isotherm models were used to fit the equilibrium data obtained from the study of MB and CR adsorption onto TiO₂@yeast-carbon at initial concentrations of 1.0~5.0 mg/L and 3.0~11.0 mg/L, respectively.

Langmuir isotherm assumes monolayer adsorption onto a surface containing a finite number of adsorption sites of uniform strategies of adsorption with no transmigration of the adsorbate in the plane of surface [10, 29]. The nonlinear Langmuir equation is given as

where is the amount of dye adsorbed per unit mass of the hybrid microspheres at equilibrium (mg/g), is the equilibrium concentration of the adsorbate (mg/L), is the theoretical maximum adsorption capacity (mg/g), and is the Langmuir adsorption constant reflecting the tendency of adsorption (L/mg).

To predict whether the adsorption process is favorable or unfavorable, equilibrium parameter , a dimensionless constant separation factor, is defined by Weber and Chakravorti as the following equation [30]:

where is the highest initial dye concentration (mg/L); the value of indicates the type of isotherm to be either favorable (), unfavorable (), irreversible (), or linear ().

The Freundlich model is an empirical theory based on adsorption on heterogeneous surface with nonuniform distribution of adsorption energy and affinities through a multilayer adsorption [31]. The nonlinear Freundlich equation is expressed as follows [32]:

where is the Freundlich isotherm constant related to the sorption capacity and represents the strength of the adsorptive bond (mg·g⁻¹ (L·mg⁻¹)1/n). The constant gives an indication of how favorable the adsorption process is, and a value between 0.1 and 1.0 represents a favorable adsorption [33].

Moreover, Temkin isotherm takes the adsorbate-adsorbent interactions into account based on the assumptions that the heat of adsorption of all the molecules in the layer decreases linearly with coverage due to adsorbent-adsorbate interactions and that the adsorption is characterized by a uniform distribution of binding energies, up to some maximum binding energy [34, 35]. The Temkin isotherm has generally been applied as

where and is J/mol, (K) is the absolute temperature, (8.314 J/mol·K) is the universal gas constant, and (L/mol) is the equilibrium binding constant corresponding to the maximum binding energy, respectively.

Koble-Corrigen (K-C) isotherm model is an empirical three-parameter model which combines both Langmuir and Freundlich isotherm models for representing equilibrium adsorption data and is given by (7) as follows [36]:

where , , and are Koble-Corrigen isotherm constants. When , the equation reduces to Langmuir equation; if , the equation becomes Freundlich equation. If , the adsorbate quantity per unit weight of adsorbent at equilibrium remains to be a constant of [37].

A comparison of the adsorption experimental isotherms of MB onto the TiO₂@yeast-carbon and theoretical plots of the Langmuir, Freundlich, Temkin, and Koble-Corrigan isotherm models was shown in Figure 6. Correlation coefficients and constants of the models were given in Table 1.

Table 1: Isotherm constants for the adsorption of MB and CR onto TiO₂@yeast-carbon.

Adsorption isotherm models
Constants
MB
CR

Langmuir isotherm
(mg/g)
2.20
1.62

(l/mg)
0.65
0.57

0.6745
0.9128

0.2346
0.2597

Freundlich isotherm
1/n
0.630
0.655

[(mg/g)]
0.840
0.033

0.5832
0.9920

Temkin isotherm
A
0.607
0.500

B
4.314
0.510

0.7517
0.9134

Koble-Corrigan isotherm

8.63
0.03

7.08
5.22

β
4.20
1.54

0.9745
0.9883

Figure 6: Comparison of Langmuir, Freundlich, Temkin, and Koble-Corrigan isotherm models for MB adsorption onto TiO₂@yeast-carbon composites (adsorbent = 0.014 g; solution volume = 100 mL; pH = 6; contact time = 1.5 h; temperature = 298 K; and concentration of MB = 1.0, 2.0, 3.0, 4.0, and 5.0 mg/L, resp.).

As can be seen from Figure 6, Koble-Corrigan isotherm plot was very close to the experimental data plot. Besides, it was observed in Table 1 that the value of of Koble-Corrigan model () was higher than those of Temkin, Langmuir, and Freundlich isotherm models, showing that Koble-Corrigan model was most suitable for the MB adsorption than the other models. This indicated that a combination of heterogeneous and homogeneous uptakes occurred in MB uptake by the synthesized TiO₂@yeast-carbon. Meanwhile, comparing the coefficients of determination of the Langmuir and Freundlich models, we could infer that homogeneous uptake was the main mechanism of the MB adsorption process [38]. Moreover, the value of from the Langmuir isotherm was between 0 and 1, the Freundlich constant was smaller than 1, and the value in Koble-Corrigan model is over 1, indicating that the adsorption of MB onto TiO₂@yeast-carbon was a favorable adsorption process.

Figure 7 typically showed the adsorption isotherms of CR onto the TiO₂@yeast-carbon. The parameters of the isotherm equations were summarized in Table 1. It was shown in Figure 7 that both Koble-Corrigan and Freundlich models are suitable for CR adsorption process. From Figure 7, the low deviation between the calculated behavior and experimental plot had been observed. This fitting result can be explained by the presence of competition between adsorbate molecules for the adsorption sites on the surface [36]. The higher value of in Table 1 from Freundlich model than Koble-Corrigan model implied that Freundlich model fitted the most exactly. In contrast, the value obtained from the Langmuir model, the Freundlich constant (), and the value from Koble-Corrigan model exhibited the same tendency as those for MB adsorption above, representing that the adsorption of CR on the TiO₂@yeast-carbon was favorable.

Figure 7: Comparison of Langmuir, Freundlich, Temkin, and K-C isotherm models for CR adsorption onto TiO₂@yeast-carbon composites (adsorbent = 0.014 g; solution volume = 100 mL; pH = 6; contact time = 1.5 h; temperature = 298 K; and concentration of CR = 3.0, 5.0, 7.0, 9.0, and 11.0 mg/L, resp.).

The above analyses showed that the Koble-Corrigan model yields a better fit of MB than the other models. CR adsorption on the TiO₂@yeast-carbon microspheres conforms well to Freundlich and Koble-Corrigan models. Namely, the Koble-Corrigan model fitted both MB and CR adsorption well. In addition, constants of and from Koble-Corrigan model are indicators of adsorption capacity and affinity of the adsorbent [36]. The values of Kolbe-Corrigan constant were 8.63 and 0.03 and those of were 7.08 and 5.22 for MB and CR, respectively. The greater and values for MB indicated higher MB adsorption capacity, affinity, and intensity compared to CR adsorption onto TiO₂@yeast-carbon microspheres. This phenomenon was in accordance with the result illustrated in Figure 4, which may be attributed to the different active functional groups in MB and CR molecules [39], revealing that the TiO₂@yeast-carbon microspheres can be served as a promising adsorptive material for MB.

Since adsorption isotherm is basically important to describe how adsorbates interact with adsorbents, some researchers had also investigated the best fitted isotherm models for the adsorption of MB and CR onto several adsorbents in aqueous solutions [2, 24, 33, 34, 40–45]. The results were listed in Table 2, and the TiO₂@yeast-carbon studied in this work represented different adsorption behaviors.

Table 2: Isotherm models for adsorption of MB and CR on various adsorbents.

Adsorbent
Dyes
Adsorption isotherm
Reference

Activated carbon/cobalt ferrite/alginate
MB
Langmuir, Freundlich
Ai et al. [40]

Bamboo-based activated carbon
MB
Langmuir
Hameed et al. [24]

TiO₂@yeast
MB
Langmuir
Chen and Bai [33]

Graphene
MB
Langmuir
Liu et al. [41]

Perlite
MB
Langmuir
Doğan et al. [42]

Garlic peel
MB
Freundlich
Hameed and Ahmad [43]

TiO₂@yeast-carbon
MB
Koble-Corrigan
This study

Bagasse fly ash and activated carbon
CR
Redlich-Peterson
Mall et al. [34]

Kaolin
CR
Langmuir
Vimonses et al. [2]

Bentonite zeolite
CR
Freundlich
Vimonses et al. [2]

Activated carbon prepared from coir pith
CR
Langmuir, Freundlich
Namasivayam and Kavitha [44]

Chitosan/montmorillonite nanocomposite
CR
Langmuir
L. Wang and A. Wang [45]

TiO₂@yeast-carbon
CR
Freundlich, Koble-Corrigan
This study

3.4. Adsorption Kinetics

To investigate the adsorption mechanism, such as mass transfer and chemical reaction, the MB and CR adsorption data were analyzed using the pseudo-first-order and pseudo-second-order models, respectively. The pseudo-first-order kinetic model was described by Lagergren and the pseudo-second-order kinetic model was based on the assumption that the rate limiting step of the adsorption process was chemical sorption [25]. The pseudo-first-order equation can be expressed as [46]

where (mg/g) and (mg/g) are the amounts of dye adsorbed onto the composites at equilibrium and at time , respectively. The rate constant (min⁻¹) of the pseudo-first-order model was calculated from the plots of versus .

The pseudo-second-order equation can be described in the following equation [28]:

where (g·mg⁻¹·min⁻¹) is the adsorption rate constant of the pseudo-second-order equation and can be obtained from the linear plots of against .

Besides, the applicability of both kinetic models was tested through the sum of error squares , which was given as follows [47]:

where is the number of data points. The higher the correlation coefficient () and the lower the values of , the better the goodness of fit will be. Table 3 also listed the calculated SSE results for MB and CR adsorption onto TiO₂@yeast-carbon at different initial concentrations.

Table 3: Kinetic adsorption parameters of different initial concentration of MB and CR.

(mg/L)
(mg/g)
Pseudo-first-order
Pseudo-second-order

(min⁻¹)
(mg/g)

SSE (%)
(g/mg⋅min)
(mg/g)

SSE (%)

MB

1.0
0.43
3.4 × 10⁻³
2.16
0.868
0.87
0.426
0.39
0.961
0.10

2.0
0.60
4.9 × 10⁻³
1.65
0.912
1.01
0.404
0.63
0.989
0.08

3.0
0.81
1.0 × 10⁻²
1.82
0.683
0.42
0.260
1.01
0.994
0.02

4.0
1.06
2.4 × 10⁻²
1.79
0.953
0.38
0.055
1.16
0.976
0.24

5.0
2.15
2.0 × 10⁻²
1.84
0.767
0.18
0.049
2.14
0.936
0.32

CR

3.0
0.29
9.6 × 10⁻²
1.67
0.960
0.69
0.270
0.30
0.981
0.04

9.0
0.62
8.5 × 10⁻²
1.25
0.903
0.32
0.052
0.64
0.989
0.11

11.0
1.24
11.0 × 10⁻²
3.75
0.941
1.25
0.040
1.33
0.994
0.01

Figure 8 exhibits the plots of the pseudo-first-order and pseudo-second-order kinetics of MB adsorption on TiO₂@yeast-carbon at different initial concentrations. The adsorption rate constants, correlation coefficient, and values were calculated and summarized in Table 2. It was observed from Table 2 that the experimental values () did not agree with the calculated ones () although the correlation coefficient values for the pseudo-first-order at some concentrations were higher than 0.85. As a result, the sorption of MB on the TiO₂@yeast-carbon did not follow pseudo-first-order in all cases. It was also obvious that the correlation coefficient was found to range from 0.936 to 0.994 for the pseudo-second-order kinetic model, which were higher than those for the pseudo-second-order model, and the experimental values () were closer with the theoretical calculated values () compared to the pseudo-first-order model. Furthermore, SSE values for the pseudo-second-order model were lower than those for the pseudo-second-order model. All the illustrations mentioned above indicated that the adsorption of MB onto TiO₂@yeast-carbon followed the pseudo-second-order kinetic model, and the chemical sorption might be involved in the adsorption process. Moreover, the rate constant () decreased with the increase of the initial MB concentrations, which was due to the striking hindrance of higher concentrations of MB [40].

(a)

(b)

Figure 8: Pseudo-first-order (a) and pseudo-second-order (b) adsorption kinetics for adsorption of MB onto TiO₂@yeast-carbon at different initial concentrations (TiO₂@yeast-carbon dosage = 0.14 g/L; pH = 6.0; temperature = 298 K; and concentration of MB = 1.0, 2.0, 3.0, 4.0, and 5.0 mg/L, resp.).

Figure 9 presents the plots of the pseudo-first-order and pseudo-second-order kinetics of CR adsorption on TiO₂@yeast-carbon at different initial concentrations. The adsorption rate constants, correlation coefficient, and values are also given in Table 3. The results presented an ideal fit to the pseudo-second-order kinetics for all concentrations with the higher correlation coefficient () and lower values. A good agreement with this model was confirmed by the similar values of calculated adsorption capacity at equilibrium () and experimental ones () for all concentrations. The best fit to the pseudo-second-order kinetics model indicates that the adsorption mechanism depends on the adsorbate and adsorbent, and the rate controlling step might be chemical sorption involving valence forces through exchange or sharing of electrons [2]. The rate constant () also decreased with the increase of the initial CR concentrations, owing to that the higher probability of collisions among CR molecules would decrease the sorption rate [28]. Similar kinetic results have also been reported for the CR adsorption onto bagasse fly ash [34], activated carbon from coir [44], and chitosan/montmorillonite [45].

(a)

(b)

Figure 9: Pseudo-first-order (a) and pseudo-second-order (b) adsorption kinetics for adsorption of CR onto TiO₂@yeast-carbon at different initial concentrations (TiO₂@yeast-carbon dosage = 0.14 g/L; pH = 6.0; temperature = 298 K; and concentration of MB = 3.0, 9.0, and 11.0 mg/L, resp.).

3.5. Regeneration of Dye Loaded TiO₂@Yeast-Carbon Microspheres

No matter if adsorption is carried out in statical or dynamical forms, it will gradually reach equilibrium if more contaminated water was treated or more adsorption cycles were conducted without regeneration [48]. So the removal of adsorbed pollutants and the regeneration study of saturated composite were completely necessary. Hence, experiments were performed to evaluate the lifetime and reusing efficiency of prepared composite in removing MB (Figure 10).

Figure 10: The circulation experiment of TiO₂@yeast-carbon composite microspheres.

For the dark adsorption section in the first cycle, near absorption-desorption equilibrium was established during the 3.0 h dark phase before the irradiation of the dyes solutions. It can also be seen from Figure 10 that strengthening trend occurs for the adsorption capacities of TiO₂@yeast-carbon microsphere when TiO₂ nanoparticles were attached onto the yeast-carbon. This enhanced effect of absorption might be ascribed to the integration of yeast-carbon and TiO₂ nanoparticles, which creates more adsorption sites for MB. The dark adsorption results show that TiO₂@yeast-carbon microsphere have faster adsorption kinetics due to their larger vacant surface area compared to the naked yeast-carbon. This phenomenon can be further affirmed by the pseudo-first-order kinetic data in Table 4. As can be seen, the kinetic rate constant in dark () for TiO₂@yeast-carbon is 5.5 × 10⁻³, which is almost 4.2 times of that for the yeast-carbon. The higher gave clear evidence that TiO₂@yeast-carbon exhibited higher adsorption rate than yeast-carbon. Thereafter, the experiments for the removal of MB compound from aqueous solution were continued for about 3 h under UV light irradiation. Figure 10 shows that in the first cycle approximately 30% of MB was removed from the aqueous solution by adsorption on the naked yeast-carbon. In the presence of the raspberry-like TiO₂@yeast-carbon microspheres and under UV irradiation, nearly 85% of MB molecule disappearance was accomplished.

Table 4: Kinetic constant (g/mg⋅min) (in dark), (light on), and Adj. -Square for removing MB.

Cycle 1
Cycle 2
Cycle 3

Yeast-carbon
TiO₂@yeast-carbon
Yeast-carbon
TiO₂@yeast-carbon
yeast-carbon
TiO₂@yeast-carbon

1.3 × 10⁻³
5.5 × 10⁻³
2.8 × 10⁻⁴
4.2 × 10⁻³
8.9 × 10⁻⁵
9.0 × 10⁻⁴

0.980
0.838
0.834
0.870
0.866
0.904

1.22 × 10⁻³
6.03 × 10⁻³
5.7 × 10⁻⁴
5.57 × 10⁻³
1.7 × 10⁻⁵
5.44 × 10⁻³

0.992
0.917
0.946
0.968
0.894
0.946

These results suggest that the prepared TiO₂@yeast-carbon composites are effective for the removal of MB from aqueous solutions. The integration of adsorption by the yeast-carbon with photocatalysis by the TiO₂ nanoparticles attached on the yeast-carbon surface showed a combined function in the removal of the MB molecule. Specifically, yeast-carbon can increase the photodegradation rate by progressively allowing an increased concentration of MB to come in contact with the TiO₂ nanoparticles through means of adsorption. TiO₂ nanoparticles on the surface of yeast-carbon can be activated to generate hydroxyl free radicals, which can decompose most of the MB molecules and keep the adsorption sites unsaturated. In return, the simultaneous adsorption of the MB molecules onto the renewed areas of the yeast-carbon provides a continuous supply of substrate to the TiO₂ nanoparticles [49]. Thus, the adsorption performance of the yeast-carbon and the photocatalytic property of the attached TiO₂ have been integrated as a novel property for the raspberry-like TiO₂@yeast-carbon composites.

It was also observed in Figure 10 that, after three times reuses, the MB removal by yeast-carbon apparently dropped from 30.6% to 7.0%. It could be attributed to the fact that the removal of MB in aqueous solution by yeast-carbon mostly relied on adsorption, which fully depended on the absorption sites. Hereby, the bare active sites on yeast-carbon were covered by MB molecules adsorbed in the last cycle, which gave explanation for the rapid loss of MB removal. However, the TiO₂@yeast-carbon still achieved desired removal efficiency for MB with slight decrease from 84.4% to 59.3% even though it had been reused for three times; that is, after 3 successive cycles under UV light irradiation, the removal rate of MB by TiO₂@yeast-carbon was still 70% of that for the first cycling run. These phenomena give evidence that TiO₂@yeast-carbon nanocomposites exhibited excellent photocatalytic stability and regeneration efficiency.

The outstanding regeneration ability of TiO₂@yeast-carbon in comparison with the yeast-carbon could be further affirmed by contrasting the pseudo-first-order kinetic rate constants (in dark) and (light on) in Table 4. As can be seen, the for TiO₂@yeast-carbon during three cycle times are 5.5 × 10⁻³, 4.2 × 10⁻³, and 9.0 × 10⁻³, respectively, which were almost 4.2, 15.0, and 10.1 times those for the yeast-carbon. The higher means that TiO₂@yeast-carbon regenerated by UV light illumination exhibited higher adsorption rate than yeast-carbon. Besides, irradiation of yeast-carbon after dark adsorption equilibrium had resulted in smaller (1.22 × 10⁻³, 5.7 × 10⁻⁴, and 1.7 × 10⁻⁵) compared to TiO₂@yeast-carbon under UV light, showing that the attachment of TiO₂ nanoparticles on the surface of yeast-carbon had a great significant influence on the removal rate of MB and implied that in situ regeneration of the MB-loaded TiO₂@yeast-carbon had already occurred.

3.6. In Situ Regenerating Mechanism for TiO₂@Yeast-Carbon

Based on the results above, a synergistic effect might be one possible mechanism for in situ regenerating dye-loaded TiO₂@yeast-carbon. The synergistic effect works by integrating the adsorption of the yeast-carbon with the photocatalysis of the TiO₂ nanoparticles attached on the yeast-carbon surface. More specifically, based on the bare areas on the surface of yeast-carbon and TiO₂, dye molecules were adsorbed onto the TiO₂@yeast-carbon through means of adsorption. Then, the adsorption sites are keeping unsaturated by illuminating the whole system. Because the irradiation of TiO₂ particles on the yeast-carbon with photons of energy () equal to or higher than those of band gap results in the excitation of electrons from the valence band () to the conduction band () of the particle, which can produce the electrons () in the conduction band and the holes () at the valence band edge of the TiO₂ (11) [50]. The electrons and holes can migrate to the particle surface of TiO₂, where the can react with the adsorbed O₂, surrounded water molecules, and surface hydroxide group, respectively, to generate the highly reactive hydroxyl radicals () ((12) and (13)) and superoxide ions (14). The resulted and are known to be very powerful and indiscriminately oxidizing agents and can oxidize the organic compounds adsorbed onto or very close to the TiO₂ surface during the photocatalytic process, resulting in degradation of dye into small units like carbon dioxide and water (15):

Simultaneously, the renewed adsorption sites provide a durative supply of MB molecule for TiO₂ particle. Then, the activity of TiO₂@yeast-carbon was successfully recovered after in situ regeneration. The recovered adsorbent could be used for the next adsorption and catalytic reaction cycle. All in all, the combination of both adsorption and heterogeneous catalysis could be regarded as cleaner, greener, favored, and promising technology for removing dye from water. An optimal amount of TiO₂ coverage should exist since the coverage rate of the attached TiO₂ nanoparticles onto the yeast-carbon surface in the TiO₂@yeast-carbon composite is an important factor for the control of removing dyes. This aspect is currently under investigation.

4. Conclusions

In conclusion, TiO₂@yeast-carbon with raspberry-like structure was successfully prepared based on pyrolysis method and was characterized by FE-SEM, EDS, and XRD. The synthetic TiO₂@yeast-carbon was used as adsorbent to remove MB and CR from aqueous solutions, respectively. FE-SEM images displayed that TiO₂@yeast-carbon microspheres have rough surface morphology and uniform diameter with good dispersity. EDS showed that TiO₂ has been already successfully coated on the yeast carbon. The adsorption results showed that TiO₂@yeast-carbon microspheres achieved favorable removal of cationic MB in comparison with the anionic CR. Equilibrium data for MB adsorption were best described by the Koble-Corrigan isotherm model. The adsorption of CR onto TiO₂@yeast-carbon showed best agreement with both Freundlich and Koble-Corrigan models. Kinetic data indicated that the adsorption of both MB and CR onto TiO₂@yeast-carbon microspheres obeyed pseudo-second-order kinetic model well. Moreover, regeneration experiments showed that TiO₂@yeast-carbon composites exhibited excellent recycling stability, reusability, and renewable ability. One possible mechanism for regenerating dye-loaded TiO₂@yeast in situ was also proposed. This paper may be useful for further research and practical applications of the novel TiO₂@yeast composite in dye wastewater treatment.

Conflict of Interests

The authors declare that there is no conflict of interests regarding the publication of this paper.

Acknowledgments

This work was financially supported by the National Natural Science Foundation of China (no. 21176031), Fundamental Research Funds for the Central Universities (no. 2013G2291015), and National Undergraduate Training Programs for Innovation and Entrepreneurship of Chang’an University (no. 201410710059).

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