Utilization to Remove Pb (II) Ions from Aqueous Environments Using Waste Fish Bones by Ion Exchange

Kizilkaya, Bayram; Tekınay, A. Adem

doi:https://doi.org/10.1155/2014/739273

Journal of Chemistry

On this page

Abstract Introduction Materials and Methods Results and Discussion Conclusion Acknowledgments References Copyright Related Articles

Research Article | Open Access

Volume 2014 | Article ID 739273 | https://doi.org/10.1155/2014/739273

Utilization to Remove Pb (II) Ions from Aqueous Environments Using Waste Fish Bones by Ion Exchange

Bayram Kizilkaya¹and A. Adem Tekınay²

Academic Editor: Huu Hao Ngo

Received02 May 2013

Revised03 Mar 2014

Accepted17 Mar 2014

Published29 Apr 2014

Abstract

Removal of lead (II) from aqueous solutions was studied by using pretreated fish bones as natural, cost-effective, waste sorbents. The effect of pH, contact time, temperature, and metal concentration on the adsorption capacities of the adsorbent was investigated. The maximum adsorption capacity for Pb (II) was found to be 323 mg/g at optimum conditions. The experiments showed that when pH increased, an increase in the adsorbed amount of metal of the fish bones was observed. The kinetic results of adsorption obeyed a pseudo second-order model. Freundlich and Langmuir isotherm models were applied to experimental equilibrium data of Pb (II) adsorption and the value of for Pb (II) was found to be 0.906. The thermodynamic parameters related to the adsorption process such as , °, °, and ° were calculated and , °, and ° were found to be 7.06, 46.01 kJ mol⁻¹, and 0.141 kJ mol⁻¹K⁻¹ for Pb (III), respectively. ° values (46.01 kJmol⁻¹) showed that the adsorption mechanism was endothermic. Weber-Morris and Urano-Tachikawa diffusion models were also applied to the experimental equilibrium data. The fish bones were effectively used as sorbent for the removal of Pb (II) ions from aqueous solutions.

1. Introduction

The contamination with toxic metals is the most important problem facing all over the world. Lead is one of the most toxic metals for living species and people [1]. Many important industrial applications, such as storage battery, manufacturing, printing pigments, fuels, photographic materials, explosive manufacturing, metal plating, mining, painting, car manufacturing, smelters, and metal refineries [2, 3], are major sources of Pb (II) contamination [4]. Lead concentrations come near to 200–500 mg/L in many industrial wastewaters and it should be reduced to a range of 0.1–0.05 mg/L [5, 6]. Different removal methods such as chemical precipitation, ion exchange, membrane filtration, solvent extraction, phytoextraction, ultrafiltration, reverse osmosis, and adsorption have been used to remove heavy metals from water and wastewaters [7–10]. Many of these processes have some disadvantages such as deficient removal, high energy requirement, and new toxic sludge/waste products that need further treatment before disposal [6]. The adsorption procedure is a simple and low-cost method for metal removal [6]. Generally, cost-effective alternative sorbents for heavy metal removal from water resources can be obtained from materials which exist abundantly in nature or arise as byproducts and waste materials from various industries [8, 11]. Recently, researchers have reported that materials with biological and natural origins, such as agricultural, banana peel, peel waste, and animal waste, are effective and usable in the removal of metals [9, 12–16]. Some sorbents such as seaweed (Gymnogongrus Torulosus) [17], leaf powder (Ficus religiosa) [18], and bacteria (Tannery Effluents Contaminated Soil) [19] were used for metal removal. Bones are composed of 30% organic compounds and 70% inorganics by weight [20]. The inorganic phase consists mainly of hydroxyapatite Ca₁₀(PO₄)₆(OH)₂ (HAP) [11, 13]. HAP is an effective inorganic adsorption material because it has a high removal capacity for heavy metals by an ion exchange reaction with calcium ions on the bone surface. Animal bones, a source of biogenic apatite for heavy metal removal, have been used as a sorbent source due to their low cost, natural abundance, and efficiency [11, 12, 21, 22].

In this study, the removal of Pb (II) ions from aqueous environments was investigated using pretreated fish bones. The bogue (Boops boops, Linnaeus 1758) bones were selected as a model fish bone for adsorption. The removal efficiency of the adsorbent was investigated as a function of pH, contact time, initial metal concentration, and temperature. Langmuir and Freundlich models were used to find the adsorption isotherms with the best fit to the experimental data. Weber-Morris and Urano-Tachikawa diffusion models were also applied to experimental equilibrium data. Thermodynamic parameters such as , , , and were calculated to determine the feasibility of the adsorption mechanism. Desorption studies were also carried out to demonstrate reusability of the bone sorbent.

2. Materials and Methods

2.1. Preparation and Pretreatment of Bone Sorbents

The fish (Boops boops) were obtained from local fish-shops in Canakkale (TURKEY). Firstly, fish bones were separated from meat and washed with hot distilled water several times. The cleaning procedures are applied at solid to liquid ratio 1 : 50 for two hours and cleaned with 0.1 M NaOH solution at 60°C and stirring rate 150 rpm, denoted as B [20]. The fish bones were dried in an oven at 50°C and then milled to particle sizes between 50 and 200 μm with a mortar.

2.2. Apparatus and Chemicals

FT-IR (Perkin Elmer FT-IR-Spectrum One, using ATR technique, 4000–550 cm⁻¹), SEM-EDX (Phillips XL-30S FEG, analyzed IYTE-Material Research Central/IZMIR), Carbon-Sulfur analyzer (LECO SC-144DR), ICP-AES (Varian Liberty II Series, Sequential Series-Axial, Australia), and Micromeritics-Gemini V for BET surface area were used for the characterization of bone sorbents. ICP-AES was used for the determination of the elements (Ca, Cr, K, Mg, Na, and P) and controlled with Intel Pentium IV PC and Liberty ICP-Expert Sequential (version: v.30) software. Each measurement was repeated three times and then standard errors of the means were calculated. The pH values of the metal solutions were measured with Consort-C864 (Belgium) multi-pH-meter. Ion chromatography (Shimadzu, Japan) was used to define within the metal solutions. The equipment was calibrated using Shimadzu anion (P/N 228-33603-93) standard solution prepared at different concentrations.

Pb(NO₃)₂ (Acros, ≥98.0%) were used for preparing the metal solutions. The pH of the metal solutions was adjusted with 0.1 M HNO₃ and 0.01 M NaOH. HNO₃ (Merck, 65%), NaOH (Merck, ≥97.0%), and NaCl (Merck, ≥99.5%) were used for the experiments.

2.3. Adsorption Experiments

Adsorption studies were performed in 100 mL Erlenmeyer flasks containing 0.4 g bone sorbent and 100 mL aqueous Pb (II) solutions, solid to liquid ratio 1 : 250, at a fixed temperature and a stirring rate of 200 rpm for 30 hours. The temperature was controlled by a water bath consisting of a glass beaker in a magnetic stirrer heater. Dried fish bones (B) were exposed to aqueous metal ions in order to determine their adsorption capacity values. The amount of Pb (II) (final metal concentration) was determined in the remaining metal solutions after filtration through a 0.45 μm Whatman filter by ICP-AES. All adsorption experiments were repeated three times () and the standard errors of the means were calculated. B was used in the adsorption experiments of Pb (II). The effect of the initial concentration of the metal ions, pH, contact time, and temperature on the adsorption of Pb (II) onto B was investigated.

The adsorption capacities of fish bone as milligram per gram of bone (mg/g fish bone) were calculated with as follows [23]: where is the initial concentration of metal ions (mg/L) and is the metal ion concentration after adsorption time (mg/L). is the volume of metal ion solutions (mL) and is the weight of bone (g). and are the experimental and calculated adsorption capacities (mg/g).

3. Results and Discussion

3.1. Characterization of Sorbents

The elemental composition of B and B-Pb was determined by Carbon-Sulfur analyzer, ICP-AES, XRD, and SEM-EDX. The carbon, calcium, phosphorus, sodium, magnesium, and sulphur amounts (wt %) of B were found to be 10.65%, 28.72%, 13.58%, 0.93%, 0.51%, and 0.04% by ICP-AES and Carbon-Sulfur analyzer, respectively. Ca/P mole ratio of B was calculated as 1.63 according to the results of previous study [20]. Figure 1 shows the XRD analysis spectrum of B. XRD patterns of bone sorbent prepared in the present study agreed with the reference patterns of calcium phosphate (Ca₂P₂O₇, Ref. Code, 00-003-0605). Table 1 gives some physical results of surface analysis of B as surface area (m²/g), pore volume (cm³/g), and average pore width . The analysis of surface area is useful in determining the surface details of the sorbent. The specific surface area of B was determined with the BET method by using nitrogen. Single point surface area of B was found to be 27.72 m²/g. BJH pore volume, BET, and BJH pore widthwere determined as , 26.58, and 43.58 , respectively.

The FT-IR analysis of B and B-Pb is given in Figure 2. The bands at 3300 cm⁻¹ are assigned to stretching. The peaks at 1020 cm⁻¹, 963 cm⁻¹, 600 cm⁻¹, and 558 cm⁻¹ are assigned to vibrations of groups. The stretching and bending modes of groups were attributed to peaks at 1413 cm⁻¹ and 872 cm⁻¹. The and band intensities of B at 1413 cm⁻¹ and 1020 cm⁻¹ reduced when the Pb (II) was adsorbed onto its surface (Figure 2). It could be said that the adsorption of Pb ions from aqueous solutions the surfaces of bone sorbents were changed to vibrations of and groups.

The adsorption of Pb²⁺ ions on to the fish bone surfaces can be explained with two different mechanisms. In the first adsorption mechanism, an ion exchange reaction occurred between metal ions in solution and Ca²⁺ ions of HAP on the bone surface [20, 24, 25]. This main removal mechanism is as the following reaction :

On the other hand, the second adsorption mechanism took place between metal ions and Na⁺ ions of HAP which was formed to HAP-(ONa) due to the alkali cleaning procedure (with NaOH solution) of the bone surface [20]. These reactions and are given below:

The initial concentration of ions in the solutions was not changed by the ion exchange reaction between metal ions and Ca²⁺ ions on the bone surface.

Table 2 and Figure 3 show the SEM-EDX analysis of B and B-Pb. The calcium percentages for B and B-Pb were found to be 36.44% and 14.63% and the Ca/P mole ratios of B and B-Pb were calculated as 1.60 and 1.06, respectively. The results in Figure 3 and Table 1 verified the Pb (II) adsorption on the bone surface by ion-exchange with calcium. Scanning electron microscope (SEM) images are useful in determining the surface and adsorption details of the bone sorbent during the adsorption [20]. The SEM images (Figure 4) show that the surfaces of B are slick and smooth. The surfaces of B-Pb exhibited roughness compared to the surfaces of B_BBB. SEM images of B-Pb clearly show that the bone surfaces with adsorbed Pb (II) are rough compared with surfaces of B. After the adsorption of metal ions from the aqueous solutions the surfaces of bone sorbents were changed. The change in the surfaces could be explained by the reaction . Based on this reaction, it could be said that very small HAP particles (<1 μm) were attached to the surfaces of bone sorbents by ion exchange between trivalent Pb metal ions and –ONa of HAP [20].

(a)

(b)

The DTA/TG analysis of B and B-Pb is shown in Table 3. The DTA/TGA analysis shows that B and B-Pb have 69.88% and 74.55% inorganic residue amount (RA) with mono weight losses at 800°C, respectively. The weight losses of 10% for B and B-Pb were found to be 328°C and 336°C, respectively. The maximum degradation temperatures (D₂) of B and B-Pb were calculated as 352°C and 354°C, respectively.

3.2. Effect of pH

The effect of pH on the adsorption of Pb (II) on the pretreated fish bones B was studied in the pH range of 3 and 5.5 at 780 mg/L of initial metal concentration. The initial pH values were adjusted by adding diluted HNO₃ and NaOH solutions. The results are shown in Figure 5 and Table 4. Since HAP, the main constituent of the fish bones, starts to dissolve at pH lower than 3, the initial pH was chosen to be 3 [11]. The pH values higher than 5.5 were not studied because the precipitation of lead ions as lead hydroxides occurs at high concentrations [26]. In this study, a number of kinetic, temperature, pH, and time experiments were carried out on high lead concentrations (like 2000 mg/L lead (II) solutions) and therefore, the selected pH value of 5 was chosen in order to prevent the formation of lead hydroxides and to get comparable results at standard pH. pH 5 was selected instead of pH 3, because this pH is close to natural water.

Figure 5 demonstrates that the adsorption capacity for Pb (II) increased with increasing pH. The highest adsorption capacity was found to be 118.7 mg/g at pH 5.5 and the results of lead removal capacities at different pH values are given in Table 4. The effect of pH plays an important role in the phosphate and hydroxyl groups of HAP during the cation-exchange reaction on the bone surface. At lower pH, HAP is dissolved and protons compete with metal ions for a binding site. The concentration of protons at lower pH is higher; thus, more groups are bound with protons and therefore fewer groups are available for metal ions to bind with [27].

3.3. Kinetic Study

The modeling of the kinetics of adsorption of Pb (II) using B_BBB was investigated by using two common models: pseudo-first and second-order kinetic equations. The Lagergren equation was used for the pseudo-first-order equation (2) [28, 29]: where is the rate constant of pseudo-first-order sorption and and are the amounts of metal adsorbed per gram of fish bone (mg/g bone) at equilibrium and any time, respectively. The plot of versus for pseudo-first-order kinetics showed a linear relationship. The slope and intercept of versus were used to calculate the pseudo-first-order rate constant and , shown in Table 5. Equation (3) was used for the pseudo-second-order kinetic model [30, 31]: where (g bone/mg hour) is the rate constant for pseudo-second-order adsorption. The constants and values were calculated from the slopes and intercepts of versus plots. value was calculated using rate constant obtained from pseudo-second-order kinetic data and expressed as where the value of is the initial metal adsorption rate (mg/g bone hour) [32]. The constants , , and were calculated from the intercept and slope of the line obtained by plotting against and are shown in Table 5.

The kinetic data obtained from Pb (II) adsorption experiments were analyzed using the pseudo-first-order kinetic model according to (2) and the results are given in Table 5. Maximum rate constants were determined at a temperature of 30°C. The calculated adsorption values () are not supported by the experimental data (). The highest values at different temperatures and concentrations were found to be and at 50°C and 417 mg/L, respectively. The effect of time on the adsorption capacity for Pb (II) at different temperatures is given in Figure 6.

According to Table 5, the correlation coefficients of the pseudo-second-order kinetic model for the linear plots are higher than 0.99 for all the temperatures and concentrations. On the other hand, when values of the pseudo-second-order kinetic model are calculated from the values, it is clearly shown that values for all the temperatures and concentrations are higher than 0.9999 and at the same time are higher than the values of the pseudo-first-order kinetic model. The calculated () adsorption amount for the pseudo second-order kinetic model is close to the experimental data (), but for the pseudo-first-order kinetic model are generally not supported by . The correlation coefficients of the pseudo-second-order kinetic model for the linear plots are higher than 0.99 for all the temperatures and concentrations. According to the correlation coefficient constant and the experimental adsorption amount (), it could be said that the experimental data exhibit a good compliance with the pseudo second-order equation for Pb (II) removal. Similar kinetic applications were also determined for Co (II) removal with animal bone [11], in which the adsorption rate of Co (II) ions on the animal bones was described by a second-order rate expression; the pseudo-second-order model correlates well with the experimental data on the sorption of divalent and trivalent metal cations by synthetic HAP [33].

3.4. Diffusion Parameters

The intraparticle diffusion model (IPD) of Weber and Morris has been widely applied to the analysis of adsorption kinetics [34]. Weber-Morris and Urano-Tachikawa modeling were used to model the diffusion of Pb (II) from aqueous solution using B_BBB.

The Weber and Morris diffusion model is expressed as [15, 35, 36] In this equation, is the Weber and Morris intraparticle diffusion rate constant and is a value of intercept constant of the plot that provide information about thickness of the boundary layer (mg/g). The value of (the amount of adsorption at any time) is plotted against (the square root of time) to get a straight line. The intraparticle diffusion constant was calculated from the slopes of versus plots.

The intraparticle diffusion coefficient () was calculated using [37, 38] where is the diffusion coefficient in the solid and (m) is the mean particle diameter.

The following equation (7) was used for the intraparticle diffusion model of Urano and Tachikawa [37, 39]: where was calculated from the slopes of versus plots.

The values of , , , and C are given in Table 6. The highest values for the Urano and Tachikawa model were found to be 5.00 m²h⁻¹ at 30°C. The maximum values according to the Weber and Morris model were found to be 75.7 mg g⁻¹h^−0.5 at 50°C. The constant increased with the increase in temperature from 20°C to 50°C and likewise increased with the increase in concentration. The value of the intercepts of the plot of versus and the constant from (5) provide information about the boundary layer effect for the Weber and Morris model. An increase in the value of constant indicates the abundance of solute adsorbed by the boundary effect [36]. Our results were similar to the research of Bilgili [40], who reported that values decreased and values increased with increasing temperatures. was found to decrease from to with an increase in temperature from 20°C to 50°C except for at 30°C, respectively. On the other hand, was found to increase from to with an increase in concentration from 50 mg/L to 1667 mg/L except for at 417 mg/L, respectively. According to Greluk and Hubicki [36], if the intraparticle diffusion is involved in the adsorption process, then the plot of versus would result in a linear graph and the process of intraparticle diffusion would be the controlling step if this line passed through the origin. When the data exhibit multilinear plots which do not pass through the origin, this is indicative of some degree of boundary layer control and further shows that intraparticle diffusion is not the only rate-controlling factor, but that other processes may control the rate of sorption [36].

The values of and are different from each other and the Weber and Morris model gives lower diffusion coefficients than the Urano and Tachikawa model. Generally, Table 6 shows that values and intraparticle diffusion of the Urano and Tachikawa model were better than those of the Weber and Morris model. Thus, it can be concluded that the experimental data for the intraparticle diffusion model of Pb (II) on the bone sorbents fit the Urano and Tachikawa model.

3.5. Temperatures and Thermodynamic Parameters

The activation energy () for the adsorption of Pb (II) was determined using the Arrhenius equation and is expressed as [29] where is the rate constant (pseudo-second-order) which was obtained from Table 3, (kJ mol⁻¹), T(K), R (kJ mol^-1K⁻¹), and are the Arrhenius activation energy, temperature of the adsorption medium, the gas constant and the Arrhenius factor, respectively. The activation energy was calculated from the slope of the line obtained by plotting against and is shown in Table 4.

The thermodynamic parameters known as Gibbs free energy , enthalpy , and entropy were determined by using the following equations [32, 41–43]: where and are the amount of metal ions (mg) adsorbed on the adsorbent per liter of the solution at equilibrium time and the equilibrium concentration (mg/L) of metal ions in the solution, respectively. The value is used in (11) to determine the thermodynamic parameters of adsorption. and are the solution temperature and gas constant, respectively. The constants of and were calculated from the slope and intercept of van’t Hoff plots of versus . The free energy () was calculated from (10) using and . The results are shown in Table 4. The Gibbs free energy indicates the fundamental of spontaneity of the adsorption process. When is a negative quantity, the adsorption process occurs spontaneously and higher negative values reflect a more energetically favorable adsorption [42].

The values of , , and were found to be 7.06, , and for Pb (III), respectively (Table 7). The values of for the temperatures of 20°C, 30°C, 40°C, and 50°C were found to be , , , and , respectively. According to Şeker et al. [30], if the value of is between and , the adsorption is said to be chemical type and the rate constant changes with temperature according to the activation energy in the Arrhenius equation (8). The positive values of at temperatures lower than 55°C (328 K) show that the adsorption of Pb (II) ions onto the fish bonesis nonspontaneous; in other words the adsorption process requires higher temperatures to occur. It could be explained that the ion exchange amounts of metal ions with calcium at the solid/liquid interface at low temperatures are lower than those at higher temperatures during the sorbates and sorbents interaction. When the temperature increased beyond 328 K (55°C), the values turned to negative. For example, the for 328 K (55°C) is calculated as . According to Lazarević et al. [44], this state points the presence of an energy barrier for the sorption process. The positive values of Gibbs free energy () indicate that the adsorption process requires a small amount of energy with increasing temperature [44]. On the other hand, according to Zhou et al. [23], the decrease in with increasing temperature implies a greater driving force and more spontaneous adsorption at high temperature. Similar calculations of thermodynamic parameters were also determined for Ni (II) removal with Sepiolite by Lazarević et al. [44]. According to Lazarević et al. [44], enthalpy () and entropy () for Ni (II) removal with sepiolite were found to be 27.93 kJ/mol and 0.0767 kJ/mol K, respectively, and the Gibbs free energy () was found to decrease from 5.05 kJ/mol at 25°C to 1.98 kJ/mol at 65°C. For the positive , Lazarević et al. [44] have explained that “Considering the positive values of , it has been suggested that this is quite common for the sorption of metal ions by the ion exchange mechanism, because an activated complex of a metal ion is formed with the sorbent in the excited state.” On the other hand, the values of and in the study of Gupta et al. [45] were found to be 4.519 kJ/mol, 0.0491 kJ/mol K and 4.519 519 kJ/mol, respectively. In the studies of Guan et al. [46] and Bhaumik et al. [47] show that all values of , , and were determined as positive. The positive values of enthalpy () show that the adsorption and removal of metal ions using bone sorbents are the endothermic case and the positive Gibbs’ free energy () values confirm that the adsorption process for Pb (II) ions requires heat to proceed. Entropy has been defined as the degree of randomness of systems and for Pb was found to be a positive value in our study. The positive values of entropy may be a result of some structural changes in the bone sorbent which result in increased electronegativity and decreased atomic volume (for Pb) during the adsorption process between the metal and Ca²⁺ ions. The adsorption capacities at different temperatures are given in Table 7. The highest removal was found to be 323.2 mg/g at 50°C.

3.6. Adsorption Isotherms

Adsorption isotherms are widely used as important criteria in optimizing the use of adsorbents because they describe the nature ofthe interaction between adsorbate and adsorbent [17]. Two isotherms were used to describe the experimental results for the adsorption process of Pb (II) ions on fish bone, namely, the Langmuir and the Freundlich adsorption isotherms.

The Langmuir adsorption model assumes that the adsorbent surface has a saturated monolayer of molecules and finite number of identical sites which shows homogeneous surfaces [48]. The Langmuir equation is given by [49, 50] where (mg/L) and (mg/g) are the residual metal concentration in solution and the amount of the metal adsorbed on the sorbent at equilibrium, respectively. (mg/g) is the maximum amount of the metal ions per unit weight of sorbent and is the Langmuir adsorption equilibrium constant related to the affinity between the sorbent and metal ions. For the calculation of the Langmuir adsorption equilibrium constant, the plot of versus showed a linear relationship. The constants and were calculated from the slope and intercept of the curve of versus and the obtained results are shown in Table 8.

To determine whether the adsorption process was favourable or unfavourable for the Langmuir adsorption, was used, given in [23, 51, 52] where (mg/L) and (L/mg) are initial metal concentration and Langmuir constant, respectively. The value of indicates the shape of the isotherm to be unfavorable , linear , favorable , or irreversible . The values between 0 and 1 indicate favorable adsorption [35].

The Freundlich equation is applicable to heterogeneous surfaces and multilayer adsorption [48]. The linear form of the Freundlich equation is given by following equation [53, 54]: where and are the adsorption capacity of the sorbent and adsorption intensity, respectively. For calculation of Freundlich adsorption equilibrium constants, the plot of versus shows a linear relationship. The values of and are calculated from the intercept and slope of the plot of versus and the results are given in Table 8.

The adsorption amounts depending on concentrations are shown in Figure 7. The constants , , and obtained from the Freundlich isotherm were found to be 26.5, 3.9, and 0.806, respectively. Based on the calculated correlation coefficients () for the Langmuir and Freundlich isotherms, it can be suggested that the experimental data for the adsorption of Pb (II) on the bones fit the Langmuir isotherm model. The value of was found to be 0.906 (Table 8). The calculated value indicated that the adsorption of Pb (II) ions on the fish bones was favorable Pb (II) concentration. The adsorption capacities at different concentrations are given in Table 8. The highest removal was found to be 155.6 at 2036 mg/L. The lead removal capacities of various adsorbents given in the literature are summarized in Table 9. Table 9 clearly shows that pretreated fish bones appear to be very useful sorbent.

4. Conclusion

Fish bones, one of the most abundant fish-processing industry waste products, were investigated for lead removal. With many specific advantages such as low cost, easy availability, natural origin, and high adsorption capacity, fish waste products can be used as sorbents to remove heavy metal. In this study, fish bones which exhibited high sorption capacity were used as a natural sorbent to remove lead.

The highest removal capacity for Pb (II) was found to be 323 mg/g at 50°C. The experiments showed that when pH increased, an increase in the adsorption capacity of the fish bones was observed. The correlation coefficients showed that the experimental data for the adsorption of Pb fitted well to the Langmuir isotherm model and the value of for Pb (II) was found to be 0.906. The kinetic data fitted a pseudo-second-order kinetic model. The enthalpy of lead was calculated as and the adsorption mechanism was endothermic. The activation energy, of adsorption of Pb (II), was determined as 7.06 kJ/mol. The experimental results showed that the correlation coefficients of intraparticle diffusion of the Urano and Tachikawa model were better than those of the Weber and Morris model. Desorption/leaching experiments showed that desorption of the Pb on the bone surface exhibited very low ratios. Fish bones can be used as adsorbent with simple processing. Therefore, the utilization of pretreated fish bones could be low cost and effective and might contribute to the protection of the environment.

Conflict of Interests

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

Acknowledgments

The authors acknowledge the Scientific Research Project Commission of Canakkale Onsekiz Mart University (Project no: 2010/16) for financial support. The authors wish to thank the Central Laboratory of Canakkale Onsekiz Mart University.

References

H. Kalavathy, B. Karthik, and L. R. Miranda, “Removal and recovery of Ni and Zn from aqueous solution using activated carbon from Hevea brasiliensis: batch and column studies,” Colloids and Surfaces B: Biointerfaces, vol. 78, no. 2, pp. 291–302, 2010.
View at: Publisher Site | Google Scholar
P. H. Kansanen and J. Venetvaara, “Comparison of biological collectors of airborne heavy metals near ferrochrome and steel works,” Water, Air, and Soil Pollution, vol. 60, no. 3-4, pp. 337–359, 1991.
View at: Google Scholar
E. Pip, “Cadmium, copper, and lead in soils and garden produce near a metal smelter at Flin Flon, Manitoba,” Bulletin of Environmental Contamination and Toxicology, vol. 46, no. 5, pp. 790–796, 1991.
View at: Google Scholar
H. Huang, G. Cheng, L. Chen, X. Zhu, and H. Xu, “Lead (II) removal from aqueous solution by spent agaricus bisporus: determination of optimum process condition using Taguchi method,” Water, Air, and Soil Pollution, vol. 203, no. 1–4, pp. 53–63, 2009.
View at: Publisher Site | Google Scholar
A. S. Özcan, Ö. Gök, and A. Özcan, “Adsorption of lead(II) ions onto 8-hydroxy quinoline-immobilized bentonite,” Journal of Hazardous Materials, vol. 161, no. 1, pp. 499–509, 2009.
View at: Publisher Site | Google Scholar
H. Ghassabzadeh, M. Torab-Mostaedi, A. Mohaddespour, M. G. Maragheh, S. J. Ahmadi, and P. Zaheri, “Characterizations of Co (II) and Pb (II) removal process from aqueous solutions using expanded perlite,” Desalination, vol. 261, no. 1-2, pp. 73–79, 2010.
View at: Publisher Site | Google Scholar
R. Donat, A. Akdogan, E. Erdem, and H. Cetisli, “Thermodynamics of Pb²⁺ and Ni²⁺ adsorption onto natural bentonite from aqueous solutions,” Journal of Colloid and Interface Science, vol. 286, no. 1, pp. 43–52, 2005.
View at: Publisher Site | Google Scholar
S. E. Bailey, T. J. Olin, R. M. Bricka, and D. D. Adrian, “A review of potentially low-cost sorbents for heavy metals,” Water Research, vol. 33, no. 11, pp. 2469–2479, 1999.
View at: Publisher Site | Google Scholar
A. Bhatnagar and A. K. Minocha, “Biosorption optimization of nickel removal from water using Punica granatum peel waste,” Colloids and Surfaces B: Biointerfaces, vol. 76, no. 2, pp. 544–548, 2010.
View at: Publisher Site | Google Scholar
X.-F. Sun, C. Liu, Y. Ma, S.-G. Wang, B.-Y. Gao, and X.-M. Li, “Enhanced Cu(II) and Cr(VI) biosorption capacity on poly(ethylenimine) grafted aerobic granular sludge,” Colloids and Surfaces B: Biointerfaces, vol. 82, no. 2, pp. 456–462, 2011.
View at: Publisher Site | Google Scholar
S. Dimovic, I. Smiciklas, I. Plećaš, D. Antonovic, and M. Mitric, “Comparative study of differently treated animal bones for Co²⁺ removal,” Journal of Hazardous Materials, vol. 164, no. 1, pp. 279–287, 2009.
View at: Publisher Site | Google Scholar
F. Banat, S. Al-Asheh, and F. Mohai, “Batch zinc removal from aqueous solution using dried animal bones,” Separation and Purification Technology, vol. 21, no. 1-2, pp. 155–164, 2000.
View at: Publisher Site | Google Scholar
Y. Zhang, Y. Liu, X. Ji, C. E. Banks, and J. Song, “Flower-like agglomerates of hydroxyapatite crystals formed on an egg-shell membrane,” Colloids and Surfaces B: Biointerfaces, vol. 82, no. 2, pp. 490–496, 2011.
View at: Publisher Site | Google Scholar
S. S. Baral, S. N. Das, G. R. Chaudhury, and P. Rath, “Adsorption of Cr (VI) by treated weed Salvinia cucullata: kinetics and mechanism,” Adsorption, vol. 14, no. 1, pp. 111–121, 2008.
View at: Publisher Site | Google Scholar
A. El-Sikaily, A. El Nemr, A. Khaled, and O. Abdelwehab, “Removal of toxic chromium from wastewater using green alga Ulva lactuca and its activated carbon,” Journal of Hazardous Materials, vol. 148, no. 1-2, pp. 216–228, 2007.
View at: Publisher Site | Google Scholar
J. R. Memon, S. Q. Memon, M. I. Bhanger, A. El-Turki, K. R. Hallam, and G. C. Allen, “Banana peel: a green and economical sorbent for the selective removal of Cr(VI) from industrial wastewater,” Colloids and Surfaces B: Biointerfaces, vol. 70, no. 2, pp. 232–237, 2009.
View at: Publisher Site | Google Scholar
M. M. Areco and M. D. S. Afonso, “Copper, zinc, cadmium and lead biosorption by Gymnogongrus torulosus. Thermodynamics and kinetics studies,” Colloids and Surfaces B: Biointerfaces, vol. 81, no. 2, pp. 620–628, 2010.
View at: Publisher Site | Google Scholar
K. S. Rao, S. Anand, and P. Venkateswarlu, “Adsorption of cadmium from aqueous solution by Ficus religiosa leaf powder and characterization of loaded biosorbent,” CLEAN—Soil, Air, Water, vol. 39, no. 4, pp. 384–391, 2011.
View at: Publisher Site | Google Scholar
M. Z. Alam and S. Ahmad, “Chromium removal through biosorption and bioaccumulation by bacteria from tannery effluents contaminated soil,” CLEAN—Soil, Air, Water, vol. 39, no. 3, pp. 226–237, 2011.
View at: Publisher Site | Google Scholar
B. Kizilkaya, A. A. Tekinay, and Y. Dilgin, “Adsorption and removal of Cu (II) ions from aqueous solution using pretreated fish bones,” Desalination, vol. 264, no. 1-2, pp. 37–47, 2010.
View at: Publisher Site | Google Scholar
M. Ozawa, K. Satake, and R. Suzuki, “Removal of aqueous chromium by fish bone waste originated hydroxyapatite,” Journal of Materials Science Letters, vol. 22, no. 7, pp. 513–514, 2003.
View at: Publisher Site | Google Scholar
I. Smičiklas, S. Dimović, I. Plećaš, and M. Mitrić, “Removal of Co²⁺ from aqueous solutions by hydroxyapatite,” Water Research, vol. 40, no. 12, pp. 2267–2274, 2006.
View at: Publisher Site | Google Scholar
Y.-T. Zhou, C. Branford-White, H.-L. Nie, and L.-M. Zhu, “Adsorption mechanism of Cu²⁺ from aqueous solution by chitosan-coated magnetic nanoparticles modified with α-ketoglutaric acid,” Colloids and Surfaces B: Biointerfaces, vol. 74, no. 1, pp. 244–252, 2009.
View at: Publisher Site | Google Scholar
S. H. Jang, B. G. Min, Y. G. Jeong, W. S. Lyoo, and S. C. Lee, “Removal of lead ions in aqueous solution by hydroxyapatite/polyurethane composite foams,” Journal of Hazardous Materials, vol. 152, no. 3, pp. 1285–1292, 2008.
View at: Publisher Site | Google Scholar
C. Stötzel, F. A. Müller, F. Reinert, F. Niederdraenk, J. E. Barralet, and U. Gbureck, “Ion adsorption behaviour of hydroxyapatite with different crystallinities,” Colloids and Surfaces B: Biointerfaces, vol. 74, no. 1, pp. 91–95, 2009.
View at: Publisher Site | Google Scholar
I. Chaari, E. Fakhfakh, S. Chakroun et al., “Lead removal from aqueous solutions by a Tunisian smectitic clay,” Journal of Hazardous Materials, vol. 156, no. 1–3, pp. 545–551, 2008.
View at: Publisher Site | Google Scholar
K. Chojnacka, “Biosorption of Cr(III) ions by eggshells,” Journal of Hazardous Materials, vol. 121, no. 1–3, pp. 167–173, 2005.
View at: Publisher Site | Google Scholar
S. Chowdhury and P. Saha, “Adsorption kinetic modeling of safranin onto rice husk biomatrix using pseudo-first- and pseudo-second-order kinetic models: comparison of linear and non-linear methods,” CLEAN—Soil, Air, Water, vol. 39, no. 3, pp. 274–282, 2011.
View at: Publisher Site | Google Scholar
Ç. Doğar, A. Gürses, M. Açıkyildiz, and E. Özkan, “Thermodynamics and kinetic studies of biosorption of a basic dye from aqueous solution using green algae Ulothrix sp.,” Colloids and Surfaces B: Biointerfaces, vol. 76, no. 1, pp. 279–285, 2010.
View at: Publisher Site | Google Scholar
A. Şeker, T. Shahwan, A. E. Eroğlu, S. Yılmaz, Z. Demirel, and M. C. Dalay, “Equilibrium, thermodynamic and kinetic studies for the biosorption of aqueous lead(II), cadmium(II) and nickel(II) ions on Spirulina platensis,” Journal of Hazardous Materials, vol. 154, no. 1–3, pp. 973–980, 2008.
View at: Publisher Site | Google Scholar
F. Granados-Correa, J. Vilchis-Granados, M. Jiménez-Reyes, and L. A. Quiroz-Granados, “Adsorption behaviour of La(III) and Eu(III) ions from aqueous solutions by hydroxyapatite: kinetic, isotherm, and thermodynamic studies,” Journal of Chemistry, vol. 2013, Article ID 751696, 9 pages, 2013.
View at: Publisher Site | Google Scholar
M. S. Chiou and H. Y. Li, “Adsorption behavior of reactive dye in aqueous solution on chemical cross-linked chitosan beads,” Chemosphere, vol. 50, no. 8, pp. 1095–1105, 2003.
View at: Publisher Site | Google Scholar
I. Smičiklas, A. Onjia, S. Raičević, Đ. Janaćković, and M. Mitrić, “Factors influencing the removal of divalent cations by hydroxyapatite,” Journal of Hazardous Materials, vol. 152, no. 2, pp. 876–884, 2008.
View at: Publisher Site | Google Scholar
F.-C. Wu, R.-L. Tseng, and R.-S. Juang, “Initial behavior of intraparticle diffusion model used in the description of adsorption kinetics,” Chemical Engineering Journal, vol. 153, no. 1–3, pp. 1–8, 2009.
View at: Publisher Site | Google Scholar
B. H. Hameed, J. M. Salman, and A. L. Ahmad, “Adsorption isotherm and kinetic modeling of 2,4-D pesticide on activated carbon derived from date stones,” Journal of Hazardous Materials, vol. 163, no. 1, pp. 121–126, 2009.
View at: Publisher Site | Google Scholar
M. Greluk and Z. Hubicki, “Sorption of SPADNS azo dye on polystyrene anion exchangers: equilibrium and kinetic studies,” Journal of Hazardous Materials, vol. 172, no. 1, pp. 289–297, 2009.
View at: Publisher Site | Google Scholar
O. M. M. Freitas, R. J. E. Martins, C. M. Delerue-Matos, and R. A. R. Boaventura, “Removal of Cd(II), Zn(II) and Pb(II) from aqueous solutions by brown marine macro algae: kinetic modelling,” Journal of Hazardous Materials, vol. 153, no. 1-2, pp. 493–501, 2008.
View at: Publisher Site | Google Scholar
A. Selatnia, M. Z. Bakhti, A. Madani, L. Kertous, and Y. Mansouri, “Biosorption of Cd²⁺ from aqueous solution by a NaOH-treated bacterial dead Streptomyces rimosus biomass,” Hydrometallurgy, vol. 75, no. 1–4, pp. 11–24, 2004.
View at: Publisher Site | Google Scholar
K. Urano and H. Tachikawa, “Process development for removal and recovery of phosphorus from wastewater by a new adsorbent. II. Adsorption rates and breakthrough curves,” Industrial & Engineering Chemistry Research, vol. 30, no. 8, pp. 1897–1899, 1991.
View at: Publisher Site | Google Scholar
M. S. Bilgili, “Adsorption of 4-chlorophenol from aqueous solutions by xad-4 resin: isotherm, kinetic, and thermodynamic analysis,” Journal of Hazardous Materials, vol. 137, no. 1, pp. 157–164, 2006.
View at: Publisher Site | Google Scholar
R. Aravindhan, J. R. Rao, and B. U. Nair, “Removal of basic yellow dye from aqueous solution by sorption on green alga Caulerpa scalpelliformis,” Journal of Hazardous Materials, vol. 142, no. 1-2, pp. 68–76, 2007.
View at: Publisher Site | Google Scholar
Z. Aksu, “Determination of the equilibrium, kinetic and thermodynamic parameters of the batch biosorption of nickel(II) ions onto Chlorella vulgaris,” Process Biochemistry, vol. 38, no. 1, pp. 89–99, 2002.
View at: Publisher Site | Google Scholar
A. Babarinde, J. O. Babalola, J. Adegoke et al., “Biosorption of Ni(II), Cr(III), and Co(II) from solutions using Acalypha hispida leaf: kinetics, equilibrium, and thermodynamics,” Journal of Chemistry, vol. 2013, Article ID 460635, 8 pages, 2013.
View at: Publisher Site | Google Scholar
S. Lazarević, I. Janković-Častvan, V. Djokić, Z. Radovanović, D. Janaćković, and R. Petrović, “Iron-modified sepiolite for Ni²⁺ sorption from aqueous solution: an equilibrium, kinetic, and thermodynamic study,” Journal of Chemical & Engineering Data, vol. 55, no. 12, pp. 5681–5689, 2010.
View at: Publisher Site | Google Scholar
V. K. Gupta, R. Jain, T. A. Saleh, A. Nayak, S. Malathi, and S. Agarwal, “Equilibrium and thermodynamic studies on the removal and recovery of Safranine-T dye from industrial effluents,” Separation Science and Technology, vol. 46, no. 5, pp. 839–846, 2011.
View at: Publisher Site | Google Scholar
W. Guan, J. Pan, H. Ou et al., “Removal of strontium(II) ions by potassium tetratitanate whisker and sodium trititanate whisker from aqueous solution: equilibrium, kinetics and thermodynamics,” Chemical Engineering Journal, vol. 167, no. 1, pp. 215–222, 2011.
View at: Publisher Site | Google Scholar
M. Bhaumik, T. Y. Leswifi, A. Maity, V. V. Srinivasu, and M. S. Onyango, “Removal of fluoride from aqueous solution by polypyrrole/F₃O₄ magnetic nanocomposite,” Journal of Hazardous Materials, vol. 186, no. 1, pp. 150–159, 2011.
View at: Publisher Site | Google Scholar
M. Chiban, A. Soudani, F. Sinan, and M. Persin, “Single, binary and multi-component adsorption of some anions and heavy metals on environmentally friendly Carpobrotus edulis plant,” Colloids and Surfaces B: Biointerfaces, vol. 82, no. 2, pp. 267–276, 2011.
View at: Publisher Site | Google Scholar
I. Langmuir, “The adsorption of gases on plane surfaces of glass, mica and platinum,” Journal of the American Chemical Society, vol. 40, no. 9, pp. 1361–1403, 1918.
View at: Google Scholar
Ü. Geçgel, G. Özcan, and G. Ç. Gürpınar, “Removal of methylene blue from aqueous solution by activated carbon prepared from pea shells (Pisum sativum),” Journal of Chemistry, vol. 2013, Article ID 614083, 9 pages, 2013.
View at: Publisher Site | Google Scholar
A. Rafique, M. A. Awan, A. Wasti, I. A. Qazi, and M. Arshad, “Removal of fluoride from drinking water using modified immobilized activated alumina,” Journal of Chemistry, vol. 2013, Article ID 386476, 7 pages, 2013.
View at: Publisher Site | Google Scholar
S. S. Majumdar, S. K. Das, R. Chakravarty, T. Saha, T. S. Bandyopadhyay, and A. K. Guha, “A study on lead adsorption by Mucor rouxii biomass,” Desalination, vol. 251, no. 1–3, pp. 96–102, 2010.
View at: Publisher Site | Google Scholar
N. Y. Mezenner, A. Hamadi, S. Kaddour, Z. Bensaadi, and A. Bensmaili, “Biosorption behavior of basic red 46 and violet 3 by dead Pleurotus mutilus from single- and multicomponent systems,” Journal of Chemistry, vol. 2013, Article ID 965041, 12 pages, 2013.
View at: Publisher Site | Google Scholar
T. Shanthi and V. M. Selvarajan, “Removal of Cr(VI) and Cu(II) ions from aqueous solution by carbon prepared from Henna leaves,” Journal of Chemistry, vol. 2013, Article ID 304970, 6 pages, 2013.
View at: Publisher Site | Google Scholar
R. Zein, R. Suhaili, F. Earnestly, I. Indrawati, and E. Munaf, “Removal of Pb(II), Cd(II) and Co(II) from aqueous solution using Garcinia mangostana L. fruit shell,” Journal of Hazardous Materials, vol. 181, no. 1–3, pp. 52–56, 2010.
View at: Publisher Site | Google Scholar
C. Mahamadi and T. Nharingo, “Utilization of water hyacinth weed (Eichhornia crassipes) for the removal of Pb(II), Cd(II) and Zn(II) from aquatic environments: an adsorption isotherm study,” Environmental Technology, vol. 31, no. 11, pp. 1221–1228, 2010.
View at: Publisher Site | Google Scholar
J. Anwar, U. Shafique, Waheed-uz-Zaman, M. Salman, A. Dar, and S. Anwar, “Removal of Pb(II) and Cd(II) from water by adsorption on peels of banana,” Bioresource Technology, vol. 101, no. 6, pp. 1752–1755, 2010.
View at: Publisher Site | Google Scholar
M. Ghaedi, G. R. Ghezelbash, F. Marahel, S. Ehsanipour, A. Najibi, and M. Soylak, “Equilibrium, thermodynamic, and kinetic studies on lead (II) biosorption from aqueous solution by Saccharomyces cerevisiae biomass,” CLEAN—Soil, Air, Water, vol. 38, no. 9, pp. 877–885, 2010.
View at: Publisher Site | Google Scholar

Copyright

Copyright © 2014 Bayram Kizilkaya and A. Adem Tekınay. 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.

PDF Download Citation

Download other formats

Order printed copies

Views

2697

Downloads

1345

Citations