Mechanochemical–hydrothermal synthesis of carbonated apatite powders at room temperature
Introduction
Hydroxyapatite (HAp) with the chemical formula corresponding to Ca10(PO4)6(OH)2, has been extensively used in medicine for implant fabrication and is one of the most biocompatible materials owing to its similarity with mineral constituents found in hard tissue (i.e. teeth and bones) [1], [2]. It is commonly the material of choice for fabrication of dense and porous HAp bioceramics [3]. Its general uses include biocompatible phase/reinforcement in composites [4], coatings on metal implants [1], [2], [3], and granular fill for direct incorporation into human tissues [1]. Among the variety of HAp-based ceramics, carbonated HAp (CO3HAp) appears to be an excellent material for bioresorbable bone substitutes [5]. Since the HAp phase present in natural bone, dentin, and enamel, respectively, contains approximately 7.4, 5.6, and 3.5 wt% of carbonate [6], CO3HAp materials have excellent biocompatibility and properties, which can be favorably compared with those of hard tissue.
Sintered CO3HAp ceramics can exhibit in vitro cell resorption rates similar to the resorption rate of natural bone minerals [5], which is higher than that of pure HAp ceramics [5], [7]. Cell appearance and proliferation does not differ on CO3HAp and pure HAp [7], [8]. Recent in vivo study using rats indicated that the dissolution rate of dense sintered CO3HAp ceramics implanted subcutaneously was intermediate between β-TCP and pure HAp [9]. In another in vivo study, it was found that the quantity of intermedullar bone formed around CO3HAp implants increased with carbonate concentration [10]. CO3HAp-forming injectable, moldable bone cement has been commercially available throughout Europe since 1997 and in the USA since 1998 [11]. The CO3HAp bone cements can be used as in situ-hardened bone fillers [12] or screw fixations [13]. Nanosized CO3HAp crystals were successfully applied to fabricate CO3HAp/collagen biodegradable composites [14]. When implanted in rabbits, these materials underwent resorption and promoted new bone formation.
The above studies indicate that CO3HAp ceramics should be superior to pure HAp for bioresorbable implants. Therefore, development of new synthesis techniques for CO3HAp powders with controlled morphology and chemical composition is of a great importance. CO3HAp powders with low crystallinity and nanometer particle size are suitable for the processing of bone-resembling materials [14]. In addition, controlling the level of carbonate substitution in HAp is a convenient way to change solubility [6] and morphology of the synthesized carbonated HAp crystals [6], which subsequently impact properties of the HAp-based biomaterials.
Multiple techniques have been used to prepare HAp and CO3HAp powders, with wet chemical methods [1], [3], [6], [15], [16] and solid-state reactions [1], [17] as the most popular. Depending upon the technique, powders with different morphologies, stoichiometries and levels of crystallinity can be obtained. Recently, several papers regarding mechanochemical and mechanochemical–hydrothermal synthesis of HAp and CO3HAp powders appeared in the literature [18], [19], [20], [21], [22], [23], [24], [25]. Mechanochemical powder synthesis is a solid-state synthesis method that takes advantage of the perturbation of surface-bonded species by pressure to enhance thermodynamic and kinetic reactions between solids [26]. In many cases, mechanochemistry can be used to prepare anhydrous multi-component oxides at room temperature in a single step. Pressure can be applied via conventional milling equipment ranging from low-energy ball mills to high-energy stirred mills (e.g. attrition, planetary, or vibratory mills). The main advantages of mechanochemical synthesis of ceramic powders are simplicity and low cost. A variety of chemical compounds have been prepared by this technique, such as CaSiO3 [27], PbTiO3 [28], and 0.9Pb(Mg1/3Nb2/3)O3-0.1PbTiO3 [29]. Since the mechanochemical synthesis involves only solid-state reaction, it should be clearly distinguished from the mechanochemical–hydrothermal synthesis (a.k.a., “wet” mechanochemical), which incorporates an aqueous phase in the system. An aqueous phase can actively participate in the mechanochemical reaction by accelerating kinetic processes that commonly rate limit a process, such as dissolution, diffusion, adsorption, reaction rate, and crystallization (nucleation and growth) [30]. The mechanochemical activation of slurries can generate local zones of high temperatures (up to 450–700°C) and high pressures due to friction effects and adiabatic heating of gas bubbles (if present in the slurry), while the overall temperature is close to the room temperature [31]. Thus, the mechanochemical–hydrothermal technique can be envisioned as being located at the intersection of hydrothermal [32] and mechanochemical [26] processing. The mechanochemical–hydrothermal route can produce large amounts of HAp powder. It also utilizes lower temperature, i.e. room temperature, as compared to 90–200°C for the hydrothermal process. Thus, for the mechanochemical–hydrothermal process, there is no need for a pressure vessel and external heating.
In an earlier study we have demonstrated that stoichiometric, crystalline HAp powder could be prepared at room temperature from heterogeneous reaction between Ca(OH)2 powder and (NH4)2HPO4 solution via the mechanochemical–hydrothermal route [25]. This process was advantageous when compared to prior reported mechanochemical HAp syntheses. Water actively participated in the reaction by both dissolving one of the reactant powders as well as serving as a reaction medium to produce a stoichiometric and highly crystalline product. In addition, the mechanochemical–hydrothermal route has been demonstrated to be applicable for reproducible and low-cost fabrication of high-quality HAp powders in large batch sizes [25]. In this paper, we will present a mechanochemical–hydrothermal method for preparation of nanocrystalline CO3HAp and NaCO3HAp powders with controlled carbonate substitution.
Section snippets
Mechanochemical–hydrothermal preparation of carbonated HAp powders
Calcium hydroxide powder (Ca(OH)2), calcium carbonate powder (CaCO3), and solid diammonium hydrogen phosphate ((NH4)2HPO4) (all analytical grade, Alfa Aesar, Ward Hill, MA) were used as reactants for synthesis of CO3-substituted HAp. For synthesis of HAp powders with coupled CO3- and Na-substitution, sodium carbonate (Na2CO3) (analytical grade, Alfa Aesar, Ward Hill, MA) was used instead of CaCO3. Purity of the reactants was confirmed by X-ray diffraction and thermogravimetry. Measured contents
CO3-substituted HAp powders
XRD patterns of the as-prepared CO3HAp powders are shown in Fig. 2. The XRD peaks are well defined and attributable only to apatite lattice planes for x=0 (i.e. nominal stoichiometric HAp) (Fig. 2a), x=1 (Fig. 2b), and x=2 (Fig. 2c). When a large excess of CaCO3, corresponding to the x value of 3, was used in the starting slurry, unreacted CaCO3 in the synthesis product was found (Fig. 2d). The sample containing apatite with the unreacted calcite (x=3) was excluded from any further evaluation.
Summary
Our work demonstrates the applicability of mechanochemical–hydrothermal synthesis for preparations of carbonated HAp powders. Crystalline CO3HAp and NaCO3HAp powders with carbonate concentration ranging between 0.8 and 12 wt% have been prepared by the mechanochemical–hydrothermal route at room temperature. The powders consisted of equiaxed crystals, ≈20 nm in diameter, which formed larger aggregates resulting in median particle size in the range of 350 nm–1.63 μm. This process is advantageous over
Acknowledgements
This research was supported by the Johnson & Johnson Corporate Biomaterials Center and the Center for Biomedical Devices at Rutgers University. The authors are greatly indebted to James Kim for experimental assistance, Chun-Wei Chen for obtaining TEM images, Eric Gulliver for FESEM images, and Charles Oakes for thermodynamic calculations.
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Present address: Rosemount Analytical Inc., 1201 North Main Street, P.O. Box 901, Orrville, Ohio 4467-0901, USA.
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Permanent address: Department of Geology, University of Mysore, P.B. No. 21, Mysore-570 006, India.