Porous Methyltrimethoxysilane Coated Nanoscale-Hydroxyapatite for Removing Lead Ions from Aqueous Solutions

Ciobanu, C. S.; Iconaru, S. L.; Popa, C. L.; Costescu, A.; Motelica-Heino, M.; Predoi, D.

doi:https://doi.org/10.1155/2014/361061

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Nanomaterials and the Environment

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Volume 2014 | Article ID 361061 | https://doi.org/10.1155/2014/361061

Porous Methyltrimethoxysilane Coated Nanoscale-Hydroxyapatite for Removing Lead Ions from Aqueous Solutions

C. S. Ciobanu,¹S. L. Iconaru,^1,2C. L. Popa,^1,3A. Costescu,⁴M. Motelica-Heino,²and D. Predoi¹

Academic Editor: Arun Kumar

Received04 Apr 2014

Revised26 Jun 2014

Accepted30 Jun 2014

Published16 Jul 2014

Abstract

The aim of this study was to synthetize new porous nanoparticles based on methyltrimethoxysilane coated hydroxyapatite (MTHAp) for lead removal form aqueous solutions. The morphological and compositional analysis of MTHAp were investigated by X-ray diffraction (XRD), Fourier transform infrared spectroscopy (FTIR) and scanning electron microscopy (SEM) equipped with an energy dispersive X-ray spectrometer (EDS). Removal experiments of Pb²⁺ ions were carried out in aqueous solutions with controlled concentration of Pb²⁺ at a fixed pH value of 3 and 5 respectively. After the removal experiment of Pb²⁺ ions from solutions, porous hydroxyapatite nanoparticles were transformed into PbMTHAp_3 and PbMTHAp_5 via the adsorption of Pb²⁺ ions followed by a cation exchange reaction. The X-ray diffraction spectra of PbMTHAp_3 and PbMTHAp_5 revealed that the powders, after removal of the Pb²⁺ ions, were a mixture of Ca_2.5Pb_7.5(PO₄)₆(OH)₂, Pb₂Ca₄(PO₄)₂(SiO₄), and Ca₁₀(PO₄)₆(OH)₂. Our results demonstrate that the porous hydroxyapatite nanoparticles can be used as an adsorbent for removing Pb²⁺ ions from aqueous solutions.

1. Introduction

One of the major environmental problems is represented by the global contamination with potentially toxic trace elements (PTTE). Lead has been widely used in the industrial field, for lead-based batteries, ammunition, paints, and building materials [1–4]. Due to their nonbiodegradable behaviour and their incapacity of metabolization and decomposition, PTTE like Pb, Cu, Cd, Zn, and Hg are the main contaminants of soils and ground or surface waters. Their progressive accumulation in the human body can cause significant health problems, inducing chronic illness which, when untreated, can lead to a painful death.

Among a large variety of PTTE, one of the most dangerous is lead. Because of its unique properties, such as resistance to corrosion, malleability, and poor conductibility, it has been used since ancient times for many applications being found in pipes, pottery, or pigments [5]. Over time, it has become more and more clear that lead exposure for a long period of time may cause many health problems, affecting the human reproductive, nervous, gastrointestinal, immune, renal, cardiovascular, skeletal, muscular, and hematopoietic systems [5, 6]. Furthermore, it impairs the development process [5, 6]. Recently, The International Agency for Research on Cancer (IARC) has included lead in the list of possible human carcinogens (IARC, 1987) together with its inorganic compounds (IACR 2006) [5]. Therefore, researchers worldwide have focused on developing new and improved methods for removing PTTE from different environmental compartments such as soils and waters. Nowadays, different methods such as chemical precipitation [7, 8], nanofiltration [7–9], reverse osmosis [7–10], and adsorption [7, 11–14] are used for depollution of water.

In the last decades, a major attention has been given to a special material, hydroxyapatite (HAp) [Ca₁₀(PO₄)₆(OH)₂], due to its remarkable properties. Being the main inorganic constituent of bone and teeth and a natural source of phosphate, hydroxyapatite is widely used in the medical field for many orthopaedic, dental, and maxillofacial applications. On the other hand, hydroxyapatite has a high sorption capacity for actinides and divalent metals [15, 16]. Furthermore, previous studies have revealed a high capacity for removing divalent ions from aqueous solutions [17] and contaminated soils [15]. For the removal of PTTE from polluted media by synthetic HAp different mechanisms have been reported, like ion exchange [18] and substitution of Ca ions in HAp by metals ions [15, 18]. In order to improve the capacity of adsorption, it was shown that there are several factors that must be taken into account, among them the type of divalent metal, the physicochemical properties of HAp, the metal concentration, the solution pH, and so forth [19].

Thus, the aim of this study was to prepare methyltrimethoxysilane coated hydroxyapatite (MTHAp) composite powders at nanoscale and to investigate the removal of Pb²⁺ ions from aqueous solutions using MTHAp samples with different pH values of the solution.

2. Materials and Methods

The morphological and compositional analysis of MTHAp were investigated by X-ray diffraction (XRD), Fourier transform infrared spectroscopy (FTIR), and scanning electron microscopy (SEM) equipped with an energy dispersive X-ray spectrometer (EDS). Batch experiments at a fixed pH of 3 and 5 were conducted with the powders and solutions of lead.

2.1. Experimental Section

All the reagents for the HAp synthesis, including ammonium dihydrogen phosphate [(NH₄)₂HPO₄] (Alpha Aesar) and calcium nitrate [Ca(NO₃)₂·4H₂O] (Alpha Aesar), were purchased without further purification. Methyltrimethoxysilane (MTMS, H₃C–Si–(OCH₃)₃) was purchased from Merck (Darmstadt, Germany). Lead nitrate [Pb(NO₃)₂] and extra pure HCl solution acquired from Merck were used for adjusting the initial Pb²⁺ ion concentration and pH value in the aqueous solutions.

2.2. Preparation of Methyltrimethoxysilane Coated Hydroxyapatite (MTHAp)

Methyltrimethoxysilane coated hydroxyapatite (MTHAp) was synthesized using as precursors methyltrimethoxysilane and hydroxyapatite. The hydroxyapatite (Ca₁₀(PO₄)₆(OH)₂, HAp) was immobilized into a methyltrimethoxysilane foam using the technique reported in literature [20, 21]. In accord with [21], the atomic ratio Ca/P was set at 1.67 for obtaining pure HAp. The MTHAp was achieved by dropping the solution containing methyltrimethoxysilane (1 g HAp/10 mL) onto HAp powders after the last centrifugation. The mixture was then stirred vigorously for 1 h until homogeneity was achieved. The final MTHAp composites were dried in a vacuum oven at 80°C for 72 h. To obtain the powders, the MTHAp composite samples were ground after drying.

2.3. Removal Experiment of Pb²⁺ Ions in Aqueous Solution

Removal performance of Pb²⁺ ions by the MTHAp composite powders was investigated by batch experiments, monitoring the change of Pb²⁺ ion concentration in the aqueous solution. For these experiments, 5 g of MTHAp composite sample was added to 500 mL aqueous solution with various initial Pb²⁺ ion concentrations and pH values in accord with Jang et al. [17]. The initial Pb²⁺ ion concentrations of the aqueous solutions were controlled and the values were set in the range 0.1–0.9 g·L⁻¹ by dissolving lead nitrate [Pb(NO₃)₂] in deionized water. The pH values of aqueous solutions with a controlled initial Pb²⁺ ion concentration were adjusted from 5 to 3 by adding small amounts of 0.1 M HCl standard solution. For all experiments the solution was stirred constantly for 24 h by a mechanical stirrer at room temperature.

2.4. Characterization

The functional groups present in the prepared powders were identified by FTIR (Spectrum BX Spectrometer). For this, 1% of the powder was mixed and ground with 99% KBr. Pellets of 10 mm diameter for FTIR measurements were prepared by pressing the powder mixture at a load of 5 tons for 2 min and the spectrum was taken in the range of 400 to 4000 cm⁻¹ with a resolution of 4 and 128 times scanning. The X-ray diffraction spectra for the MTHAp samples were recorded using a Bruker D8 Advance diffractometer, with nickel filtered Cu (λ = 1.5405 Å) radiation. The diffraction patterns were collected in the 2θ range 20°–60°, with a step of 0.02° and 34 s measuring time per step. Scanning electron microscopy (SEM) study was performed on a HITACHI S2600N-type microscope equipped with an energy dispersive X-ray attachment (EDAX/2001 device). The concentration of Pb²⁺ ions remaining in the solution after the MTHAp reacted with the Pb²⁺ ion-containing solution was determined by flame atomic absorption spectroscopy (Hitachi Z-8100 spectrophotometer).

The amount of retained lead ion concentration was obtained using atomic absorption. The removal efficiency of lead ions was calculated using the following formula: where and are the initial and the equilibrium concentration of Pb²⁺ (g/L).

The adsorption isotherm was also obtained by mixing a solution with different initial concentrations of Pb²⁺ with a known amount of hydroxyapatite coated with methyltrimethoxysilane powder until the equilibrium was achieved. The sorption capacity representing the amount of metal retained on the unit mass of sorbent at the equilibrium was also estimated. The amount adsorbed at equilibrium, , was calculated with the following formula: where is initial concentration, (mg/L); is equilibrium concentration, (mg/L); is volume of solution, (L); is adsorbent quantity, (g).

3. Results and Discussions

The FTIR spectra of the methyltrimethoxysilane coated hydroxyapatite powder before (MTHAp) and after the removal experiment of Pb²⁺ ions at pH 5 (PbMTHAp_5) and pH 3 (PbMTHAp_3) are shown in Figure 1. The most noticeable feature in these spectra concerns the presence of the typical ν₄ and ν₃ bands [22, 23]. The bands present in the ranges 530–650 cm⁻¹ and 900–1200 cm⁻¹ correspond to IR vibrations of phosphate group belonging to apatite [24, 25].

(a)

(b)

(c)

The band at 475 cm⁻¹ can be attributed to the ν₂ vibrational mode. According to Gibson et al. [26] the incorporation of silicon in the HAp lattice affects the FTIR spectra of HAp, in particular the P–O vibrational bands. In previous studies realised by Karakassides et al. [27] and Bogya et al. [28] it was shown that the distortion is caused by the stretching vibrations assigned to the Si–O–Si bonds that should appear in the range of 950–1200 cm⁻¹. Due to the presence of the phosphate groups in the range of 950–1200 cm⁻¹, the peaks associated to Si–O–Si bonds cannot be observed [29, 30]. In addition, the band which appears at 631 cm⁻¹ is assigned to the vibrational stretching mode of OH in the apatite lattice. Moreover, the band at around 3435 cm⁻¹ is assigned to the water adsorbed on the surface. Another characteristic peak of the adsorbed water appears at 1640 cm⁻¹, due to O–H bending. According to Zhai et al. [31] the bands around 3400 cm⁻¹ are due to O–H stretching of water associated to crystallization.

Figure 2 presents the X-ray diffraction patterns of the methyltrimethoxysilane coated hydroxyapatite powder before (MTHAp) and after the removal experiment of Pb²⁺ ions at pH 5 (PbMTHAp_5) and pH 3 (PbMTHAp_3), respectively. All the diffraction peaks of MTHAp powders could be assigned to the standard characteristic peaks of hexagonal hydroxyapatite and no secondary phases were detected, indicating that the phase of the samples was of pure HAp [20]. The diffraction patterns support the fact that HAp nanoparticles were successfully coated with methyltrimethoxysilane without any structural changes. The hydroxyapatite coated with methyltrimethoxysilane composite was likely to be transformed into PbMTHAp via the adsorption of Pb²⁺ ions followed by the cation exchange reaction [32].

(a)

(b)

(c)

The spectra of PbMTHAp_5 and PbMTHAp_3 revealed that the powders after the removal of Pb²⁺ were a mixture of Ca_2.5Pb_7.5(PO₄)₆(OH)₂, Pb₂Ca₄(PO₄)₂(SiO₄) (represented by in the XRD spectra), and Ca₁₀(PO₄)₆(OH)₂. In previous studies on the removal of lead ions from aqueous solution by a phosphosilicate glass, Kim et al. [33] showed that, at pH 3 and 5, only Pb₁₀(PO₄)₆(OH)₂ crystals formed on the glass when the glass reacted with the solution containing Pb²⁺ ions. On the other hand, Zhang et al. [34], in their recently study on the efficient and selective immobilization of Pb²⁺ in a highly acidic wastewater using strontium hydroxyapatite nanorods, showed that the final solids were a mixture of SrHAp, PbHPO₄, and Pb₅(PO₄)₃(OH).

The hydroxyapatite coated with methyltrimethoxysilane before and after the reaction with the Pb²⁺ ion-containing solution with pH 3 and 5 for 24 h was investigated by SEM and the results are presented in Figure 3. The SEM investigations suggest that the solid reaction products of aqueous Pb with the MTHAp were dependent on the pH value. Distinct differences between the sample morphologies were observed in the SEM micrographs. The presence of Ca_2.5Pb_7.5(PO₄)₆(OH)₂ and Pb₂Ca₄(PO₄)₂(SiO₄) crystals was identified by crystal clusters with needle or rod-like shapes. The quantity of Ca_2.5Pb_7.5(PO₄)₆(OH)₂ and Pb₂Ca₄(PO₄)₂(SiO₄) crystals is more substantial for the solution with pH 3 consistent with the XRD analysis. These results are in good agreement with preliminary studies [34].

(a)

(b)

(c)

In order to investigate the Pb absorption by the MTHAp samples, the EDAX mapping technique was used. In Figure 4 the EDAX spectrum and elemental mapping of hydroxyapatite coated with methyltrimethoxysilane after the reaction with a solution containing 950 mg of Pb/L at pH 3 are presented.

The presence of Si, O, P, Ca, and Pb in the sample after the reaction with a solution containing 950 mg of Pb/L at pH 3 was revealed.

The impact of the lead concentration in the aqueous solution was studied by absorption experiments performed at 25°C. For this purpose MTHAp concentration in the range of 0.1– 0.9 g·L⁻¹ at pH 5 was used. The measurements were performed on 500 mL solution (pH 5) with an initial Pb²⁺ ion concentration of 63 mg·L⁻¹. Figure 5 presents the adsorption efficiency of Pb²⁺ ions as a function of the Pb concentration in the solution. It was noticed that the removal efficiency increased proportionally with the Pb concentration. When a Pb concentration of 0.1 g·L⁻¹ was used, the removal efficiency reached 98.4%, showing that the adsorbent composite, MTHAp, had a strong affinity to Pb²⁺ ions. At Pb concentration from 0.5 g·L⁻¹ to 1.5 g·L⁻¹, the removal efficiency was nearly 100%. In this case, the Pb²⁺ ions in the solution were completely removed. For the studies on the effect of the solution pH, the lead concentration of 0.9 g·L⁻¹ was chosen.

A solution containing 563 mg·L⁻¹ of Pb²⁺ ions was prepared from 0.9 g of Pb(NO₃)₂ in 1 L of distilled water. Figure 6 shows the measured Pb²⁺ ions concentration in the solution after the reaction with MTHAp has taken place.

At pH 3, a removal efficiency of 100% was achieved. At pH 6, the removal efficiency of Pb²⁺ ions was 82%. For intermediate pH values, the removal efficiency of Pb²⁺ ions was 95% and 91% for pH 4 and pH 5, respectively.

As shown before, the influence of pH on the adsorption efficiency of lead is small. These results are in good agreement with the outcome of XRD and SEM analysis.

The theoretical Langmuir isotherm is often used to describe adsorption of a solute from a liquid solution as follows [35, 36]: where and are the Langmuir constants, which represent the maximum adsorption capacity for the solid phase loading and the energy constant related to the heat of adsorption, respectively. The two constants from the Langmuir isotherm can be determined by plotting () versus ().

The experimental data and the Langmuir theoretical model are shown in Figure 7. The graph of Pb²⁺ adsorbed per unit mass of MTHAp, , against the concentration of Pb²⁺ remaining in the solution, , is shown. The coefficient of Langmuir isotherm at room temperature is . In agreement with previous studies [37, 38] there was no problem with the transformation of nonlinear isotherm equation to linear form, by using nonlinear method.

Therefore, by plotting () versus (), the two constants from the Langmuir isotherm were determined. Figure 8 shows the plots of the Langmuir isotherm model. It can be seen that the isotherm data fits the Langmuir equation with the highest value of the regression coefficients . On the other hand, the maximum adsorption capacity for the solid phase () is 105.485 mg(Pb)/g(MTHAp). The Langmuir constant was found to be 9.856 L/mg.

Following these results, it can be emphasized that MTHAp can effectively remove Pb²⁺ ions from aqueous solutions. Because the pH of the groundwater and surface waters varies in the range of 5–7, the pH value in the aqueous solution used for the removal of Pb²⁺ ions is an important parameter that must be considered [39]. Along with previous studies, such as [39], our study suggests that the solid reaction products of aqueous Pb with the apatite are pH-dependent. In order to describe the uptake of different metals from aqueous solutions by synthetic hydroxyapatite [40–43] various processes have been proposed, such as cation exchange, metal complexation on the HAp surface, and apatite dissolution followed by a new metal phase precipitation. Suzuki et al., in their previous study [44], suggested the formation of a more stable lead apatite, such as Ca_(10−x)Pb_x(PO₄)₆(OH)₂ via an ion exchange mechanism where Pb²⁺ present in the solution replaces Ca²⁺ ions from the hydroxyapatite lattice.

According to [45], Pb_(10−x)Ca_x(PO₄)₆(OH)₂ crystals with higher content of calcium are unstable. As a consequence, the HAp would be subject to a continuous process of dissolution and precipitation leading to more stable structures with a higher lead content.

After the reaction of lead uptaken by MTHAp, dissolution of Ca₁₀ (PO₄)₆(OH)₂ was involved, followed by the precipitation of solid solution of Pb and Ca as Ca_2.5Pb_7.5(PO₄)₆(OH)₂ and Pb₂Ca₄(PO₄)₂(SiO₄). In agreement with previous studies [3], the formation of the new crystals was identified. Distinct morphologies were observed in the SEM micrographs. Scattered needle- or rod-shaped crystals were observed in the sample obtained from the reaction performed at low pH. Ma et al. [46] reported similar crystals in previous studies. In agreement with former experiments [3, 18, 45, 46], the differences were detected under SEM between the unreacted apatite and those reacted under conditions of low pH.

4. Conclusions

The objective of this study was to synthesize a new porous nanocomposite material based on methyltrimethoxysilane coated hydroxyapatite. Its ability to remove Pb²⁺ ions from aqueous solutions with a variety of initial Pb²⁺ ion concentrations and pH values from 3 to 5 was investigated. When MTHAp reacted with the solution containing Pb²⁺ ions, the lead ions were completely removed from the solution. The dissolution of Ca₁₀(PO₄)₆(OH)₂ occurred, forming Ca_2.5Pb_7.5(PO₄)₆(OH)₂ and Pb₂Ca₄(PO₄)₂(SiO₄). The MTHAp composite material exhibited the higher removal efficiency of Pb²⁺ ions at low pH. Its removal capacity was the highest at pH 3 and the removal capacity of lead decreased slowly when the pH increased. After 24 h, most of the Pb²⁺ ions were eliminated from the aqueous solution at various pH values and for an initial Pb concentration of 563 mg·L⁻¹. This research showed that the MTHAp nanocomposite material is a promising adsorbent for Pb²⁺ ions from aqueous solution at various pH values and could be used as a purifier for wastewaters.

Conflict of Interests

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

Acknowledgment

The financial support and encouragement were provided by the Ministry of Education of Romania under the Project IFA-CEA C2-06.

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Copyright © 2014 C. S. Ciobanu 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.

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Journal of Nanomaterials

Nanomaterials and the Environment

Porous Methyltrimethoxysilane Coated Nanoscale-Hydroxyapatite for Removing Lead Ions from Aqueous Solutions

Abstract

1. Introduction

2. Materials and Methods

2.1. Experimental Section

2.2. Preparation of Methyltrimethoxysilane Coated Hydroxyapatite (MTHAp)

2.3. Removal Experiment of Pb2+ Ions in Aqueous Solution

2.4. Characterization

3. Results and Discussions

4. Conclusions

Conflict of Interests

Acknowledgment

References

Copyright

2.3. Removal Experiment of Pb²⁺ Ions in Aqueous Solution