BioMed Research International
Volume 2015 (2015), Article ID 719060, 12 pages
http://dx.doi.org/10.1155/2015/719060

Research Article

Biosorption of Pb(II) Ions by Klebsiella sp. 3S1 Isolated from a Wastewater Treatment Plant: Kinetics and Mechanisms Studies

Antonio Jesús Muñoz, Francisco Espínola, Manuel Moya, and Encarnación Ruiz

Department of Chemical, Environmental and Materials Engineering, University of Jaén, 23071 Jaén, Spain

Received 14 May 2015; Accepted 29 July 2015

Academic Editor: T. Komang Ralebitso-Senior

Copyright © 2015 Antonio Jesús Muñoz 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.

Lead biosorption by Klebsiella sp. 3S1 isolated from a wastewater treatment plant was investigated through a Rotatable Central Composite Experimental Design. The optimisation study indicated the following optimal values of operating variables: 0.4 g/L of biosorbent dosage, pH 5, and 34°C. According to the results of the kinetic studies, the biosorption process can be described by a two-step process, one rapid, almost instantaneous, and one slower, both contributing significantly to the overall biosorption; the model that best fits the experimental results was pseudo-second order. The equilibrium studies showed a maximum lead uptake value of 140.19 mg/g according to the Langmuir model. The mechanism study revealed that lead ions were bioaccumulated into the cytoplasm and adsorbed on the cell surface. The bacterium  Klebsiella sp. 3S1 has a good potential in the bioremoval of lead in an inexpensive and effective process.

1. Introduction

Biotechnology has a great potential to remove heavy metals using the ability of different bacteria and other microorganisms to capture metal ions, mainly through biosorption. This ability has a high potential for the development of effective and economic processes for heavy metal bioremoval, especially for dilute solutions (<100 mg/L) [1]. Low cost is the most important advantage of biosorption over conventional treatments because biosorbents are usually inexpensive and abundant materials, and biosorption also often offers the advantages of metal recuperation and biomass regeneration [2]. The main mechanisms involved can be cell-surface binding, intracellular bioaccumulation, and extracellular precipitation [3]. The binding of metal on the cell surface can occur with living microorganism or death biomass. Nevertheless, metal bioaccumulation takes place only in living cells.

Microorganisms and other biomass types have the advantage of having components as lipopolysaccharides, proteins, and phospholipids which have many functional groups. These groups confer a negative charge and thus offer the possibility of adding metal cations. This ability is present in all types of biomass, dead or alive. In the case of living microorganisms, other active cellular mechanisms are involved: synthesis of specific enzymes, action of cytoplasmic or membrane proteins, and so forth [4, 5].

In order to improve biosorption effectiveness, the identification of additional microbial strains with high metal uptake capacity and specificity is a key aspect. In this way, the isolation of autochthonous microorganisms from contaminated sites is an interesting option to obtain metal-resistant strains [6–8].

Lead is known for its high environmental impact and toxicity [9]. This metal, along with mercury and cadmium, is considered one of “the big three” heavy metals present in contaminated effluents [2]. The European Directive 2008/105/EC includes lead and its compounds in the list of priority substances in environmental quality standards, establishing a concentration of lead of 0.0072 mg/L as the maximum permissible in the case of surface water.

In this work, the biosorption characteristics of Klebsiella sp. 3S1 were investigated. This strain is a bacterium selected from a group of microorganisms isolated from wastewater treatment plants that showed high resistance to several heavy metals, namely, Pb, Zn, and Ag [10]. Kinetic studies were conducted to determine the optimal working time. A Rotatable Central Composite Design (RCCD) with six central points was employed to optimise the operational conditions: sorbent dosage, pH, and temperature. The interactions between the experimental factors were evaluated by Response Surface Methodology (RSM). This technique has proved its effectiveness in optimising the variables that influence the adsorption process and reducing both time and cost [11–13]. Finally, equilibrium studies were performed. Additionally, potential mechanisms of biosorption were studied by FTIR, SEM, and TEM techniques.

2. Materials and Methods

2.1. Preparation of Klebsiella sp. 3S1

Ten strains were selected and identified by molecular techniques in a previous study from wastewater treatment plants [10]. After preliminary biosorption tests, the bacterial strain Klebsiella sp. 3S1 was selected for kinetic and equilibrium studies. This isolate showed 98% homology with that of standard Klebsiella species based on its 16S-rDNA gene sequence (1476 bp) and was named Klebsiella sp. 3S1 (GenBank accession number HE975030).

For the biosorption experiments, the biomass was prepared by incubating the strain in tryptic soy broth (TSB, 30 g/L) medium at 30°C with stirring, after centrifugation at 6000 rpm and washing twice with electrolyte solution. The cells of Klebsiella sp. 3S1 used in kinetic studies and the adsorption isotherm were harvested by centrifugation from exponential phase cultures. Then, the cells were resuspended in the lead solution.

2.2. FTIR Spectroscopy

The infrared spectra of the biomass samples before and after metal uptake were recorded using a VERTEX 70 (Bruker Corporation) Fourier transform infrared spectrometer operating in the range of 4000–400 cm⁻¹. Measurements were performed with lyophilised samples. The samples were measured using Attenuated Total Reflection (ATR). FTIR characterisation was performed to identify characteristic chemical functional groups of the bacterium Klebsiella sp. that might be involved in the metal uptake procedure.

2.3. FE-SEM-EDX Analysis

Field emission scanning electron microscopy (MERLIN of Carl Zeiss) coupled with energy dispersive X-ray spectroscopy was carried out to characterise the Klebsiella sp. 3S1 surface before and after Pb(II) ion uptake. Samples were fixed with a 2.5% glutaraldehyde solution in PBS (pH 7.4), dehydrated with increasing solutions of acetone (50, 70, 90, and 100%), and, finally, dried by critical point drying and metalized with carbon.

2.4. HR-TEM-EDX Analysis

High-resolution transmission electron microscopy and energy dispersive X-ray analysis (Philips CM-20) were used to determine the location of the metal within the cell. The samples were fixed, dehydrated, and dried as in the previous case; these were then treated with resin and were finally polymerised.

2.5. Batch Biosorption

The test solutions of Pb(II) were prepared using Pb(NO₃)₂ and 0.1 M NaCl as an electrolyte. The initial pH was controlled with 0.1 M NaOH or 0.1 M HNO₃.

The preliminary biosorption tests were performed in Erlenmeyer flasks with the ten strains (Section 2.1). The biosorbents were suspended in 50 mL of Pb(II) solution (25 mg/L) to reach different cell concentrations. The cell/metal suspension was gently agitated (200 rpm) at 30°C in an orbital shaker (CERTOMAT IS, Sartorius). To prevent precipitation of the metal, the lead solution was adjusted to pH 5.0. After 24 h, the metal solution was filtered (pore size 0.22 μm). Finally, the sample was acidified with HNO₃ and analysed by absorption atomic spectrometry (AAS) using an AANALYST 800 (Perkin Elmer) to know the final metal concentration. The tests for each strain were performed in triplicate.

Isothermal and kinetic studies were conducted as described above. Two kinetics experiments were performed, with two different concentrations of biomass and metal: Experiment number 1: 50 mg/L of Pb(II) and 0.11 g/L of dry biomass and Experiment number 2: 25 mg/L of Pb(II) and 0.28 g/L of dry biomass. The adsorbent was separated from the solution by centrifugation at predetermined time intervals (5–3600 min), with two flasks at each time point. Then, the residual lead concentration was analysed by AAS. The biosorption isotherm was obtained for a constant biomass concentration (0.52 g/L) and different concentrations of metal at 25°C.

In all cases, the amount of metal ions biosorbed per unit mass of dry biosorbent (lead biosorption capacity) was determined according to the following equation:

where is the biosorption capacity (mg metal/g of the dry biosorbent); and are the initial and final metal concentrations, respectively; is the liquid volume (0.05 L); and is the amount of the biosorbent sample on a dry basis (g).

2.6. Experimental Design and Statistical Analysis

A Rotatable Central Composite Design (RCCD) with six central points was performed to evaluate the relationship between obtained results and experimental factors as well as optimise the working conditions. Biosorbent dosage (), pH, and temperature () were chosen as independent variables, and the equilibrium biosorption capacity () was chosen as the dependent output response variable. The lead concentration used in all cases was 100 mg/L.

According to the RCCD, the total number of experimental combinations is , where is the number of independent variables and is the number of repetitions of the experiments at the centre point. The independent variables (factors), experimental range, and levels for lead removal are given in Table 1. The experimental design incorporated 20 experimental points, including six replicates at the central point.

Table 1: Experimental design and response.

Run order
Factor
Response

: biosorbent dosage (mg/mL)
pH
: temperature (°C)
: biosorption capacity (mg/g)

12
0.55
5.50
25
104.02

6
0.80
4.30
34
118.51

13
0.55
4.75
10
80.97

11
0.55
4.00
25
87.42

1
0.30
4.30
16
67.27

15
0.55
4.75
25
105.02

18
0.55
4.75
25
105.75

4
0.80
5.20
16
86.16

10
1.00
4.75
25
94.99

19
0.55
4.75
25
108.65

5
0.30
4.30
34
127.21

9
0.10
4.75
25
122.13

3
0.30
5.20
16
76.36

7
0.30
5.20
34
138.52

16
0.55
4.75
25
105.31

2
0.80
4.30
16
79.17

20
0.55
4.75
25
106.18

8
0.80
5.20
34
119.79

14
0.55
4.75
40
163.53

17
0.55
4.75
25
106.18

The overall quadratic equation for biosorption capacity was

where is equilibrium biosorption capacity (mg metal/g of the dry biosorbent); is the biosorbent dosage; is the temperature (°C); β ₀ is the interception coefficient; , , and are the linear terms; , , and are the quadratic terms; and , , and are the interaction terms.

The response data were analysed by parameters obtained from the analysis of variance (ANOVA) using Design-Expert program, 8.0.7.1 version. The statistical significance was fixed at 5% probability level ( value = 0.05).

2.7. Modelling of Uptake Kinetics

To know the biosorption mechanisms and speed of the process, it is important to study the mass transfer and chemical reactions. To do this, the experimental data have been adjusted to several kinetic models. In most cases, it is assumed that adsorption is controlled by chemical reaction and not by diffusion, which contributes to the mechanical agitation. However, we have tested three kinetic models of chemical reaction control and one of intraparticle diffusion. The kinetic models tested are shown in Table 2. To adjust the experimental data to the kinetic models, we used the IBM SPSS Statistics software, 19 version (SPSS Inc. and IBM Company).

Table 2: Kinetic models tested.

Model
Equation

Pseudo-first order or Lagergren [14]

Pseudo-second order [15]

Elovich [16]

Intraparticle diffusion or Weber and Morris [14]

: biosorption capacity (mg/g) at time , according to (1).

: biosorption capacity (mg/g) at equilibrium.

: pseudo-first-order kinetic rate constant (min⁻¹).

: pseudo-second-order kinetic rate constant (g·mg⁻¹·min⁻¹).

: Elovich constant (mg·g⁻¹·min⁻¹).

: Elovich constant (g·mg⁻¹).

: intraparticle diffusion rate constant in the bacterium (mg·g⁻¹·min−1/2).

2.8. Modelling of the Biosorption Isotherm

Several adsorption isotherms have been tested to fit experimental data. The most widely used among them are the Langmuir and Freundlich models; other well-known models are the Sips and Redlich-Peterson equations (Table 3). Adsorption isotherms originally used for gas phase adsorption can be readily adapted to correlate adsorption equilibrium in heavy metals biosorption. The Langmuir model establishes a relationship between the amount of gas adsorbed on a surface and the pressure of gas and assumes monolayer coverage of the adsorbate over a homogeneous adsorbent surface. The Freundlich model is an empirical equation, which assumes that as the adsorbate concentration in solution increases it also increases on the adsorbent surface. This model can be applied to nonideal sorption on heterogeneous surfaces as well as to multilayer sorption. The Sips model is also called the Langmuir-Freundlich isotherm; this isotherm model incorporates features of both the Langmuir and Freundlich isotherms and may be used to represent adsorption equilibrium over a wide concentration range. The Redlich-Peterson model is another empirical equation that can represent adsorption equilibrium over a wide concentration range. When β = 1, it effectively reduces to a Langmuir isotherm, and when β = 0, it obeys Henry’s law. To adjust the experimental data to kinetic models, IBM SPSS Statistics software described above was employed.

Table 3: Isotherm models used to represent the biosorption equilibrium.

Model
Equation

Langmuir [17]

Freundlich [18]

Sips [19]

Redlich-Peterson [20]

: biosorption capacity (mg/g) at equilibrium.

: maximum biosorption capacity (mg/g).

: Langmuir biosorption equilibrium constant (L/mg).

: equilibrium concentrations of metal (mg/L).

: characteristic constant related to the biosorption capacity.

: characteristic constant related to the biosorption intensity.

and : Sips isotherm parameters.

, , and β: Redlich-Peterson parameters; and β varies between 0 and 1.

3. Results and Discussion

3.1. Preliminary Biosorption Tests

Ten strains isolated from wastewater treatment plants showed resistance to lead in our previous study [10]. Preliminary biosorption tests were performed on these strains to select the most appropriate one. Table 4 shows the results obtained, which range from 45 to 104 mg/g for fungi, 22 to 38 mg/g for yeast, and 78 to 90 mg/g for bacteria. The best results are obtained with the fungus Trichosporon sp. 1L1 and the bacterium Klebsiella sp. 3S1.

Table 4: Lead biosorption capacity from preliminary tests.

Isolates
(mg/g)

Fungi

    Galactomyces geotrichum 5L2
66.00

    Penicillium sp. 8L2
44.74

    Pseudallescheria boydii 3S3
85.17

    Trichosporon sp. 1L1
104.53

Yeasts

    Trichosporon sp. 4L2
22.29

    Trichosporon sp. 4S3
35.72

    Rhodotorula mucilaginosa 1S1
23.95

    Rhodotorula mucilaginosa 2S4
37.59

Bacteria

    Klebsiella sp. 3S1
90.48

    Enterobacter sp. 2E2
78.10

To choose the most suitable strain for heavy metals biosorption, other aspects of interest should be taken into account. It is very interesting to support microbial biomass in low cost inert solids. Therefore, microorganisms with greater ability to form biofilms are always the most appropriate [31]. This was the reason why that Klebsiella sp. 3S1 was chosen.

3.2. FTIR Spectroscopic Study

FTIR analysis was performed to identify the main functional groups and to study their evolution during biosorption process. This technique has proved effective in obtaining structural information on metal-microbe bonds [32]. The results for Klebsiella sp. 3S1 showed the presence of the following functional groups: amino, carbonyl, carboxylic, hydroxyl, and phosphate. Table 5 shows band assignments and the typical functional groups present in this bacterium before and after Pb(II) uptake [33–35]. The IR spectra of metal-free and metal-loaded biomass showed differences in the functional groups (Figure 1). After contact with the metal solution, the spectra obtained show a shift of the frequency band and the appearance of new peaks [36]; furthermore, a decrease in band intensity was observed. These changes indicate that the functional groups are involved in the process of adsorption. Moreover, it is important to note the appearance of a peak at 1038 cm⁻¹; this peak occurs after contact with the metal solution, and this shift is typical of the complexation of phosphate or carboxyl groups by coordination with metal ions [37, 38]. Finally, two new peaks were observed in the region with low wave numbers (under 800 cm⁻¹); these peaks (571 and 539 cm⁻¹) could be attributed to the interaction between the metal ions and N-containing bioligands [39, 40].

Table 5: IR absorption bands: changes and possible assignment.

FTIR peak
Original biomass wavenumbers (cm⁻¹)
Pb(II) loaded biomass wavenumbers (cm⁻¹)
Displacement (cm⁻¹)
Functional groups
Assignment

1
3282
3280
2
–OH, –NH
Stretching vibrations of amino and hydroxyl groups

2
2958
2957
1
–CH₃
–CH₃ asymmetric stretching

3
4
2925
2875
2924
2875
1
0
–CH₂
–CH₃
–CH₂ asymmetric stretching vibrations
–CH₃ symmetric stretching vibrations

5
2854
2853
1
–CH₂
–CH3 asymmetric stretching vibrations

6
1638
1639
1
–CO, C–N
C=O and C–N stretching in amide I group

7
1531
1534
3
–CN, –NH
C–N stretching in amide II group and N–H bending

8
1453
1453
0
–CH₂, –CO
–CH₂ bending, symmetric C=O

9
1396
1398
2
–COO⁻
–COO⁻ symmetric stretching of carboxyl groups

10
1233
1236
3
, –CO
P=O asymmetric stretching of phosphate groups, deformation vibration of C=O carboxylic acids

11
12
1063

1058
1038
5
1038
, –OH
–CO,
P=O symmetric stretching of phosphate groups, –OH of polysaccharides
C–O stretching of alcoholic groups, symmetric stretching of phosphate groups

13

993
993
–C–O, –CH₂
C–O–C, C–O–P, and –CH₂ stretching vibrations of polysaccharides

14
967
969
2

N-containing bioligands

15
914
915
1

N-containing bioligands

16
860
861
1

S=O stretching

17
796
796
0

N-containing bioligands

18
780
780
0

N-containing bioligands

19

571
571

N-containing bioligands

20
515
539
24

N-containing bioligands

Figure 1: FTIR spectra of Klebsiella sp. 3S1 before and after Pb(II) biosorption.

3.3. Chemical and SEM Analysis

Figure 2 shows micrographs and EDX spectra obtained after and before the biosorption process. These micrographs show changes in the cell morphology of Klebsiella sp. 3S1; there is also a large presence of bright particles on the surface of the bacteria treated with lead. EDX analysis supported this observation, confirming that the metal remained adsorbed by the entire cell surface. Other authors have obtained similar results with different microorganisms [39, 41].

Figure 2: SEM-EDX analysis of Klebsiella sp. 3S1 before (a) and after Pb(II) biosorption (b).

3.4. Chemical and TEM Analysis

The location of the metal within the cell was evaluated using HR-TEM-EDX technique. The micrographs obtained together with the corresponding EDX microanalysis (Figure 3) show that the metal is largely fixed at the cell surface. However, in some cases, lead accumulation also appears within the cytoplasm, which could indicate the presence of a bioaccumulation mechanism; some authors have identified this capacity in different microorganisms [42]. Perdrial et al. [43] localised lead accumulations associated with polyphosphate bodies in bacteria isolated from the environment.

Figure 3: Transmission electron micrographs of a thin section of Klebsiella sp. 3S1 and the location of fixed lead (a). Energy dispersive X-ray spectra of the intracellular accumulation of lead (b) acquired from the region indicated by arrow 1 in (a) and the surface biosorption (c) acquired from the region indicated by arrow 1 in (a).

3.5. Uptake Kinetics

Sorption kinetics is important because it describes the solute uptake, which also controls the residence time of the metal ions at the solid-solution interface. Figure 4 shows the results of two biosorption experiments. The observed values ​​are the average of two replicates. From the figure, it can be observed that the biosorption occurs in two phases: first a very fast initial rate within the first 5 min and then a slow attainment of equilibrium within 1 to 2 days, both of which contribute to the total metal biosorption. This finding suggests that adsorption of lead may occur by two mechanisms: cell-surface binding and intracellular accumulation. To contemplate both mechanisms, we used different boundary conditions. Ho et al. [44] considered an imaginary negative time when the rate of sorption is infinity, in the same case.

Figure 4: Experimental data and curves corresponding to the model that best fits the experimental results, pseudo-second order with boundary conditions: at and at .

Kinetic behavior during adsorption has been studied by numerous models [45]. They have attempted to quantitatively describe the process. However, they present limitations that can be solved with theoretical assumptions and specific experimental conditions. The models that best fit our experimental data were pseudo-first and second order. To fit models to data, we used linear and nonlinear regression (always getting the best results from nonlinear regressions) and used different boundary conditions; namely, at and at , where corresponds to a quick, practically instantaneous biosorption at the beginning of the experiment. The use of the latter boundary conditions is a major difference from what is found in the literature, as the typical boundary condition is at .

Table 6 shows the values ​​of the parameters that best fit the models provided. The higher correlation coefficients confirm that pseudo-second-order kinetics is the most suitable to represent the biosorption data. This fact also supports the assumption of the model, namely, that adsorption is due to chemisorption. Our results are similar to those obtained by other authors with different microorganisms [14, 21]. Figure 4 also shows the curves corresponding to the model that best fits the experimental results so that the experimental data can easily be compared with the model predictions.

Table 6: Integrated equations, boundary conditions, and kinetic parameters of the biosorption by Klebsiella sp. 3S1.

Exp. number 1
Exp. number 2

Pseudo-first order

at and at  

103.2
78.15

0.00775
0.00607

0.437
0.627

5826
2781

at and at  

115.7
85.43

49.43
30.21

0.0013
0.0018

0.992
0.983

81.65
124.5

Pseudo-second order

at and at  

107.5
82.64

0.629
0.774

3836
1686

at and at  

130.9
96.56

47.57
28.84

0.996
0.974

45.26
197.4

Elovich

at and at  

26.55
7.176

0.07855
0.08845

0.922
0.923

811.1
570.1

at and at  

1.832
1.516

0.04807
0.06404

45.76
26.39

0.992
0.962

78.03
286.7

Intraparticle diffusion

2.488
1.971

—
0.241

11718
5652

1.305
1.146

48.84
31.50

0.957
0.903

439.8
719.0

Exp. number 1: 50 mg/L of Pb(II) and 0.11 g/L of dry biomass. Exp. number 2: 25 mg/L of Pb(II) and 0.28 g/L of dry biomass. is the correlation coefficient, and is the sum of the errors squared.

3.6. Response Surface Modelling and Optimum Biosorption Conditions

A Rotatable Central Composite Design was performed. Table 1 shows the values of the operating variables, that is, biosorbent dosage (), pH and temperature (), and the biosorption capacity () response. The results were fit to a quadratic equation for biosorption capacity, (2), by using the Design-Expert statistical package. The final equation in terms of actual factors is shown below:

Analysis of variance (ANOVA) was performed to determine the influence of the significant factors involved in the biosorption capacity. Table 7 shows the variability of the factors and their interactions. The effect of a factor can be defined as the response variation produced by a change in the factor level, where only terms found to be statistically significant were included. In this case, seven effects showed values below 0.05. This indicates that they are significantly different from zero with a 95% confidence level and one required to support hierarchy.

Table 7: ANOVA for the response surface reduced quadratic model.

Source
Sum of squares
DF
Mean square
-value
value

Model
9588.53
8
1198.57
437.66
<0.0001

    : biosorbent dosage
4.10
1
4.10
1.50
0.2520

    pH
234.13
1
234.13
85.49
<0.0001

    : temperature
8164.13
1
8164.13
2981.14
<0.0001

    pH
18.39
1
18.39
6.72
0.0291

301.72
1
301.72
110.17
<0.0001

161.57
1
161.57
59.00
<0.0001

    pH²
164.17
1
164.17
59.95
<0.0001

387.29
1
387.29
141.42
<0.0001

Residual
24.65
9
2.74

    Lack of fit
16.26
4
4.06
2.42
0.1790

    Pure error
8.39
5
1.68

Cor total
9613.18
17

CV %
1.58

-Squared
0.9974

Adj. -Squared
0.9952

Pred. -Squared
0.9837

The model is significant (-value = 437.66) and the lack of fit is not significant (-value = 2.42). Therefore, it can be stated that the model can predict biosorption capacity as an equation of the three studied factors. The -Squared suggests that the model explains 99.74% of the variability in the response.

The perturbation plots were obtained to study the effects of several factors. These plots showed that temperature has the greatest influence on Pb(II) removal efficiency, and the biosorbent dosage exerts less influence. This is shown in Figure 5, with the response surface corresponding to pH 4.75. Moreover, this figure also shows that increases with biosorbent dosage for low values ​​of temperature, whereas if the temperature values ​​are high, the biosorbent dosage influence is negative; this is justified by the interaction between the biosorbent dosage and temperature.

Figure 5: Response surface plot for biosorption of Pb(II) by Klebsiella sp. 3S1 showing the interactive effect of temperature () and biosorbent dosage () (pH, 4.75, and initial lead concentration, 100 mg/L).

The empirical model given as (3) was also optimised: the maximum , 139.96 mg/g, was mathematically located at 34°C, pH 5.05, and biosorbent dosage 0.40 mg/mL. However, the adjusted model also allows different operational conditions, for example, a temperature of 25°C, which is closer to room temperature (Figure 6).

Figure 6: Response surface plot for biosorption of Pb(II) by Klebsiella sp. 3S1 showing the interactive effect of biosorbent dosage () and pH (temperature, 25°C, and initial lead concentration, 100 mg/L).

3.7. Biosorption Equilibrium

Equilibrium data were obtained experimentally using different initial concentrations of Pb(II) between 50 and 320 mg/L and a constant biomass concentration (0.52 g/L), at 25°C and pH 5 (Figure 7). These are the optimum conditions according to the obtained model, (3), given a temperature of 25°C, which was chosen because it is more like environmental conditions.

Figure 7: Biosorption equilibrium data and Freundlich isotherm for Klebsiella sp. 3S1.

Four isotherm equations have been examined in the present study. All parameters were adjusted by nonlinear regression. Table 8 shows the results obtained. The biosorption isotherms for Pb(II) ion uptake by Klebsiella sp. 3S1 were found to be appropriate for all predictions. Only the correlation coefficient of the Langmuir curve was lower. This fact suggests that heterogeneous surface conditions predominate, but monolayer biosorption may coexist. Accordingly, the biosorption process on the bacteria is complex, involving several mechanisms.

Table 8: Biosorption equilibrium parameters of the isotherm models by Klebsiella sp. 3S1.

Langmuir

140.19

0.075353

0.9395

60.955

Freundlich

65.266

7.4312

0.9901

15.920

Sips

66.223

0.019748

7.1713

0.9901

15.915

Redlich-Peterson

20850.6

319.3393

0.86949

0.9901

15.923

is the correlation coefficient.

is the sum of the errors squared.

The maximum biosorption capacity () was obtained with the Langmuir model (140.18 mg/g), which is comparable to other types of biomass studied (Table 9). A direct comparison between different biosorbents is difficult because of the varying experimental conditions employed. However, it can be seen as Klebsiella sp. 3S1 exhibits good biosorption efficiency, among the highest that have been reported for lead ions.

Table 9: Maximum lead biosorption capacity of different microorganisms.

Biosorbent
(mg/g)
Reference

Penicillium sp.
60.77
[21]

R. arrhizus
48.79
[22]

Ceratophyllum demersum
44.80
[23]

Bacillus cereus
70.42
[24]

Aspergillus niger
34.92
[25]

Dried activated sludge
131.60
[26]

Caulerpa lentillifera
28.99
[27]

Cladophora fascicularis
227.70
[28]

Immobilised Saccharomyces cerevisiae
30.04
[29]

Recombinant Escherichia coli
108.99
[30]

Klebsiella sp. 3S1
140.19
In this study

4. Conclusions

This work concluded that the isolate Klebsiella sp. 3S1 may be employed to be used as an inexpensive biosorbent, highly efficient for Pb(II) uptake. Maximum biosorption capacity (140.19 mg/g dry cell) was obtained at 25°C and an initial pH of 5. As a result of TEM-EDX analysis, both cell-surface binding and bioaccumulation could be involved in Pb removal. The biosorption process was found to be dependent on experimental factors such as the biosorbent dosage, initial metal ion concentration, pH, temperature, and contact time. Biosorption equilibrium data fit better to the Freundlich model, which implies heterogeneous surface conditions. This result is in accordance with the kinetic studies, which show that the sorption process is slow and that biosorption is performed in two phases: a very fast initial rate within the first 5 min, followed by slow attainment of equilibrium within 1 to 2 days, both of which contribute to the total metal biosorption. FTIR and SEM-EDX techniques confirmed the interactions between lead ions and functional groups on the wall surface of Klebsiella sp. 3S1. Moreover, TEM-EDX analysis showed the presence of metal in the cytoplasm.

Future research should be carried out to develop a robust immobilisation method for wastewater treatment, including continuous biosorption with reuse and recycling.

Conflict of Interests

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

Acknowledgment

The support of the Spanish Agency for International Development Cooperation (Project Reference A/018600/08) is greatly acknowledged.

References

S. O. Lesmana, N. Febriana, F. E. Soetaredjo, J. Sunarso, and S. Ismadji, “Studies on potential applications of biomass for the separation of heavy metals from water and wastewater,” Biochemical Engineering Journal, vol. 44, no. 1, pp. 19–41, 2009.

B. Volesky, “Biosorption and me,” Water Research, vol. 41, no. 18, pp. 4017–4029, 2007.

B. Volesky and Z. R. Holan, “Biosorption of heavy-metals,” Biotechnology Progress, vol. 11, no. 3, pp. 235–250, 1995.

S. A. Kumar, M. K. Abyaneh, S. W. Gosavi et al., “Nitrate reductase-mediated synthesis of silver nanoparticles from AgNO₃,” Biotechnology Letters, vol. 29, no. 3, pp. 439–445, 2007.

C. Cervantes, A. E. Espino-Saldaña, F. Acevedo-Aguilar et al., “Interacciones microbianas con metales pesados,” Revista Latinoamericana de Microbiología, vol. 48, pp. 203–210, 2006.

R. A. Amer, F. Mapelli, H. M. El Gendi et al., “Bacterial diversity and bioremediation potential of the highly contaminated marine sediments at el max district (Egypt, mediterranean sea),” BioMed Research International, vol. 2015, 17 pages, 2015.

M. L. Merroun, M. Nedelkova, J. J. Ojeda et al., “Bio-precipitation of uranium by two bacterial isolates recovered from extreme environments as estimated by potentiometric titration, TEM and X-ray absorption spectroscopic analyses,” Journal of Hazardous Materials, vol. 197, pp. 1–10, 2011.

M. A. Kumar, A. Vijayalakshmi, E. A. R. Lincy et al., “Biotransformation of reactive black HEBL into 3 nitroso-3-azabicyclo (3.2.2) nonane by an acclimated mixed culture,” International Journal of ChemTech Research, vol. 6, no. 9, pp. 4172–4179, 2014.

L. H. Mason, J. P. Harp, and D. Y. Han, “Pb neurotoxicity: neuropsychological effects of lead toxicity,” BioMed Research International, vol. 2014, Article ID 840547, 8 pages, 2014.

A. J. Muñoz, E. Ruiz, H. Abriouel et al., “Heavy metal tolerance of microorganisms isolated from wastewaters. Identification and evaluation of its potential for biosorption,” Chemical Engineering Journal, vol. 210, pp. 325–332, 2012.

Y. G. Bermúdez, I. L. R. Rico, E. Guibal, M. C. de Hoces, and M. Á. Martín-Lara, “Biosorption of hexavalent chromium from aqueous solution by Sargassum muticum brown alga. Application of statistical design for process optimization,” Chemical Engineering Journal, vol. 183, pp. 68–76, 2012.

M. Seenuvasan, K. S. Kumar, S. Abinandan et al., “Statistical analysis on stress induced lipid accumulation along with the major cell components of Chlorella sp,” International Journal of ChemTech Research, vol. 6, no. 9, pp. 4186–4192, 2014.

T. Vidhyadevi, A. Murugesan, S. S. Kalaivani et al., “Optimization of the process parameters for the removal of reactive yellow dye by the low cost Setaria verticillata carbon using response surface methodology: thermodynamic, kinetic, and equilibrium studies,” Environmental Progress & Sustainable Energy, vol. 33, no. 3, pp. 855–865, 2014.

J. Febrianto, A. N. Kosasih, J. Sunarso, Y.-H. Ju, N. Indraswati, and S. Ismadji, “Equilibrium and kinetic studies in adsorption of heavy metals using biosorbent: a summary of recent studies,” Journal of Hazardous Materials, vol. 162, no. 2-3, pp. 616–645, 2009.

Y. S. Ho, D. A. J. Wase, and C. F. Forster, “Kinetic studies of competitive heavy metal adsorption by sphagnum moss peat,” Environmental Technology, vol. 17, no. 1, pp. 71–77, 1996.

C. W. Cheung, J. F. Porter, and G. Mckay, “Sorption kinetic analysis for the removal of cadmium ions from effluents using bone char,” Water Research, vol. 35, no. 3, pp. 605–612, 2001.

I. Langmuir, “The adsorption of gases on plane surfaces of glass, mica and platinum,” The Journal of the American Chemical Society, vol. 40, no. 9, pp. 1361–1403, 1918.

H. Freundlich, “Adsorption in solutions,” Physical Chemistry, vol. 57, pp. 384–410, 1906.

R. Sips, “Combined form of Langmuir and Freundlich equations,” The Journal of Chemical Physics, vol. 16, pp. 490–495, 1948.

O. Redlich and D. L. Peterson, “A useful adsorption isotherm,” The Journal of Physical Chemistry, vol. 63, no. 6, pp. 1024–1039, 1959.

L. Ezzouhri, E. Ruiz, E. Castro et al., “Mechanisms of lead uptake by fungal biomass isolated from heavy metals habitats,” Afinidad, vol. 67, no. 545, pp. 39–44, 2010.

Y. Sag, A. Yalçuk, and T. Kutsal, “Mono and multi-component biosorption of heavy metal ions on Rhizopus arrhizus in a CFST,” Process Biochemistry, vol. 35, no. 8, pp. 787–799, 2000.

O. Keskinkan, M. Z. L. Goksu, M. Basibuyuk, and C. F. Forster, “Heavy metal adsorption properties of a submerged aquatic plant (Ceratophyllum demersum),” Bioresource Technology, vol. 92, no. 2, pp. 197–200, 2004.

L. Ray, S. Paul, D. Bera, and P. Chattopadhyay, “Bioaccumulation of Pb (II) from aqueous solutions by Bacillus cereus ,” Journal for Hazardous Substance Research, vol. 5, pp. 1–21, 2006.

A. Y. Dursun, “A comparative study on determination of the equilibrium, kinetic and thermodynamic parameters of biosorption of copper(II) and lead(II) ions onto pretreated Aspergillus niger,” Biochemical Engineering Journal, vol. 28, no. 2, pp. 187–195, 2006.

X.-J. Wang, S.-Q. Xia, L. Cwen, J.-F. Zhao, J.-M. Chovelon, and J.-R. Nicole, “Biosorption of cadmium(II) and lead(II) ions from aqueous solutions onto dried activated sludge,” Journal of Environmental Sciences, vol. 18, no. 5, pp. 840–844, 2006.

P. Pavasant, R. Apiratikul, V. Sungkhum, P. Suthiparinyanont, S. Wattanachira, and T. F. Marhaba, “Biosorption of Cu²⁺, Cd²⁺, Pb²⁺, and Zn²⁺ using dried marine green macroalga Caulerpa lentillifera,” Bioresource Technology, vol. 97, no. 18, pp. 2321–2329, 2006.

L. Deng, Y. Su, H. Su, X. Wang, and X. Zhu, “Sorption and desorption of lead (II) from wastewater by green algae Cladophora fascicularis,” Journal of Hazardous Materials, vol. 143, no. 1-2, pp. 220–225, 2007.

A. Çabuk, T. Akar, S. Tunali, and S. Gedikli, “Biosorption of Pb(II) by industrial strain of Saccharomyces cerevisiae immobilized on the biomatrix of cone biomass of Pinus nigra: equilibrium and mechanism analysis,” Chemical Engineering Journal, vol. 131, no. 1–3, pp. 293–300, 2007.

T. T. L. Nguyen, H. R. Lee, S. H. Hong, J.-R. Jang, W.-S. Choe, and I.-K. Yoo, “Selective lead adsorption by recombinant Escherichia coli Displaying a Lead-Binding Peptide,” Applied Biochemistry and Biotechnology, vol. 169, no. 4, pp. 1188–1196, 2013.

N. K. Srivastava and C. B. Majumder, “Novel biofiltration methods for the treatment of heavy metals from industrial wastewater,” Journal of Hazardous Materials, vol. 151, no. 1, pp. 1–8, 2008.

K. Aftab, K. Akhtar, A. Jabbar, I. H. Bukhari, and R. Noreen, “Physico-chemical study for zinc removal and recovery onto native/chemically modified Aspergillus flavus NA9 from industrial effluent,” Water Research, vol. 47, no. 13, pp. 4238–4246, 2013.

M. Kiliç, M. E. Keskin, S. Mazlum, and N. Mazlum, “Hg(II) and Pb(II) adsorption on activated sludge biomass: effective biosorption mechanism,” International Journal of Mineral Processing, vol. 87, no. 1-2, pp. 1–8, 2008.

X. Wei, L. Fang, P. Cai et al., “Influence of extracellular polymeric substances (EPS) on Cd adsorption by bacteria,” Environmental Pollution, vol. 159, no. 5, pp. 1369–1374, 2011.

Y. Wang, Q. Zhou, B. Li et al., “Differentiation in MALDI-TOF MS and FTIR spectra between two closely related species Acidovorax oryzae and Acidovorax citrulli,” BMC Microbiology, vol. 12, article 182, 2012.

G. Blázquez, M. A. Martín-Lara, G. Tenorio, and M. Calero, “Batch biosorption of lead(II) from aqueous solutions by olive tree pruning waste, equilibrium, kinetics and thermodynamic study,” Chemical Engineering Journal, vol. 168, no. 1, pp. 170–177, 2011.

R. Aravindhan, B. Madhan, J. R. Rao, and B. U. Nair, “Recovery and reuse of chromium from tannery wastewaters using Turbinaria ornata seaweed,” Journal of Chemical Technology and Biotechnology, vol. 79, no. 11, pp. 1251–1258, 2004.

R. Nadeem, T. M. Ansari, and A. M. Khalid, “Fourier transform infrared spectroscopic characterization and optimization of Pb(II) biosorption by fish (Labeo rohita) scales,” Journal of Hazardous Materials, vol. 156, no. 1–3, pp. 64–73, 2008.

T. Akar, S. Tunali, and I. Kiran, “Botrytis cinerea as a new fungal biosorbent for removal of Pb(II) from aqueous solutions,” Biochemical Engineering Journal, vol. 25, no. 3, pp. 227–235, 2005.

S. T. Akar, A. Gorgulu, B. Anilan, Z. Kaynak, and T. Akar, “Investigation of the biosorption characteristics of lead(II) ions onto Symphoricarpus albus: batch and dynamic flow studies,” Journal of Hazardous Materials, vol. 165, no. 1–3, pp. 126–133, 2009.

W.-B. Lu, J.-J. Shi, C.-H. Wang, and J.-S. Chang, “Biosorption of lead, copper and cadmium by an indigenous isolate Enterobacter sp. J1 possessing high heavy-metal resistance,” Journal of Hazardous Materials, vol. 134, no. 1–3, pp. 80–86, 2006.

J. Maldonado, A. Solé, Z. M. Puyen, and I. Esteve, “Selection of bioindicators to detect lead pollution in Ebro delta microbial mats, using high-resolution microscopic techniques,” Aquatic Toxicology, vol. 104, no. 1-2, pp. 135–144, 2011.

N. Perdrial, N. Liewig, J.-E. Delphin, and F. Elsass, “TEM evidence for intracellular accumulation of lead by bacteria in subsurface environments,” Chemical Geology, vol. 253, no. 3-4, pp. 196–204, 2008.

Y. S. Ho, J. C. Y. Ng, and G. McKay, “Removal of lead(II) from effluents by sorption on peat using second-order kinetics,” Separation Science and Technology, vol. 36, no. 2, pp. 241–261, 2001.

K. Vijayaraghavan and Y.-S. Yun, “Bacterial biosorbents and biosorption,” Biotechnology Advances, vol. 26, no. 3, pp. 266–291, 2008.