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Article

Modulated Monoclinic Hydroxyapatite: The Effect of pH in the Microwave Assisted Method

by
Daniel Sánchez-Campos
1,
Maria Isabel Reyes Valderrama
1,
Susana López-Ortíz
1,
Daniela Salado-Leza
2,
María Eufemia Fernández-García
3,
Demetrio Mendoza-Anaya
3,*,
Eleazar Salinas-Rodríguez
1 and
Ventura Rodríguez-Lugo
1,*
1
Área Académica de Ciencias de la Tierra y Materiales, Instituto de Ciencias Básicas e Ingeniería, Universidad Autónoma del Estado de Hidalgo, Carretera Pachuca-Tulancingo Km. 4.5, Pachuca 42184, Mexico
2
Cátedras CONACYT, Facultad de Ciencias Químicas, Universidad Autónoma de San Luis Potosí, San Luis Potosí 78210, Mexico
3
Instituto Nacional de Investigaciones Nucleares, Carretera Mexico-Toluca S/N La Marquesa, Ocoyoacac 52750, Mexico
*
Authors to whom correspondence should be addressed.
Minerals 2021, 11(3), 314; https://doi.org/10.3390/min11030314
Submission received: 4 February 2021 / Revised: 12 March 2021 / Accepted: 15 March 2021 / Published: 17 March 2021
(This article belongs to the Special Issue Interactions of Polymers with Minerals Surfaces)
Browse Figures
Versions Notes

Abstract

:
Hydroxyapatite (HAp) is a natural hard tissue constituent widely used for bone and tooth replacement engineering. In the present work, synthetic HAp was obtained from calcium nitrate tetrahydrate (Ca(NO3)2·4H2O) and ammonium phosphate dibasic (NH4)2HPO4 following an optimized microwave assisted hydrothermal method. The effect of pH was evaluated by the addition of ammonium hydroxide (NH4OH). Hence, different characterization techniques were used to determine its influence on the resulted HAp powders’ size, shape, and crystallinity. By Transmission Electron Microscopy (TEM), it was observed that the reaction pH environment modifies the morphology of HAp, and a shape evolution, from sub-hedral particles at pH = 7 to rod-like nanosized HAp at pH = 10, was confirmed. Using the X-ray Diffraction (XRD) technique, the characteristic diffraction peaks of the monoclinic phase were identified. Even if the performed Rietveld analysis indicated the presence of both phases (hexagonal and monoclinic), monoclinic HAp prevails in 95% with an average crystallite size of about 23 nm. The infrared spectra (FTIR) showed absorption bands at 3468 cm−1 and 630 cm−1 associated with OH− of hydroxyapatite, and bands at 584 cm−1, 960 cm−1, and 1090 cm−1 that correspond to the PO43− and CO32− characteristic groups. In summary, this work contributes to obtaining nanosized rod-like monoclinic HAp by a simple and soft method that has not been previously reported.

Graphical Abstract

1. Introduction

In the last few decades, the development of synthetic hydroxyapatite (HAp) (Ca10(PO4)6(OH)2) has gained enormous scientific interest due to its unique characteristics, such as excellent biocompatibility [1], bioactivity [2], osteoconduction [3], chemical stability, and potential use as a filling material [4]. Indeed, natural HAp is considered the main mineral constituent of hard tissue, which consists of 9% water, 22% organic matter, mainly collagen, and 69% inorganic matter that actually corresponds to HAp [5].
Today, HAp may be synthesized in the laboratory. Actually, a significant number of scientific reports have demonstrated that synthetic HAp shows similar crystallographic characteristics and chemical properties to naturally occurring HAp. Therefore, synthetic HAp has been widely used in bone and tooth tissue replacement and reconstruction applications, such as implant coatings and bone substitutes, among others [6,7]. HAp can be synthesized by different routes, (i) dry methods: solid-state synthesis [8] and mechanochemical [9]; (ii) wet methods: conventional chemical precipitation, hydrolysis, sol-gel, hydrothermal, emulsion, and sonochemistry [10]; and (iii) high temperature processes: combustion and pyrolysis [11]. However, the remaining challenge consists in establishing an adequate synthesis method that allows obtaining a product with enhanced physicochemical characteristics and properties, i.e., with an exquisite crystallite and particle size control, and structure homogeneity, avoiding by-products and the appearance of new phases [12,13,14,15,16]. In this perspective, microwave synthesis is an alternative technique to provide autogenous thermal energy to the reaction. It presents interesting advantages, such as time and energy saving, few by-products generation, high yields, and few steps; it also worthy of mention that it supports the development of greener strategies to produce novel materials for a wide variety of applications [17]. The success of the microwave heating lies in the inherent properties of liquids and solids to convert, in situ, the microwave energy into heat and, thus, to promote chemical reactions. This conversion depends on the polarity of solvents as microwaves interact with the dipole moment of the solvents’ molecules. As results, a higher heating rate is obtained in comparison with indirect heating approaches (conduction). This high rate induces an accelerated kinetic reaction in shorter time, leading to selective crystallization, formation of novel phases, and the grown of nanostructured materials. In addition, it allows savings energy consumption. For all these reasons, at present, this technique is widely used and directly related to processes, such as: digestion, drying, calcination, decomposition, and chemical sintering, among others [18,19,20].
Moreover, it is well known that the bioactivity of natural and synthetic HAp strongly depends on its size and shape features. For instance, it has been observed that the biocompatibility and chemical reactivity of HAp increases by decreasing its size [21]. It is worth mentioning that almost all the crystallographic analysis referring to natural and synthetic HAp have shown, exclusively, the presence of the hexagonal crystalline phase (around 97% of the scientific works related to the synthesis and characterization of HAp) [22,23,24], and only a few articles have reported the probable presence of monoclinic HAp [25]. Table 1 shows the main characteristics of the hexagonal and monoclinic phase found in the literature.
In comparison with the HAp hexagonal phase, the monoclinic is thermodynamically more stable, a very important characteristic as its field of application may be widened. Some authors have reported the synthesis of monoclinic HAp by various methods. For instance, H. Morgan et al. obtained monoclinic HAp with a hexagonal shape at 900 °C [29], and T. Ikoma et al. followed a wet methodology and heated up to 1200 °C to induce the monoclinic phase. On the other hand, L. Pastero et al. used wet synthesis and citrate as surfactant to preferentially obtain monoclinic hydroxyapatite at 135 °C [30].
Therefore, the aim of this work was to synthesize monoclinic HAp through the microwave-induced hydrothermal method at softer temperature conditions than those already reported. As mentioned before, the characteristics of the final HAp highly depend on the experimental conditions (precursors nature, reaction temperature, Ca/P ratio, pH, etc.). Here, the reaction pH was chosen as main parameters due to its important effect on the chemical reaction rate. In this regard, the pH was varied from 7 to 10 to promote the formation of the monoclinic HAp phase. To corroborate the monoclinic phase, complementary XRD, TEM, and FTIR techniques were used.

2. Materials and Methods

2.1. Microwave Assisted Hydrothermal Synthesis

Figure 1 schematically shows the experimental procedure used in this work to synthesize HAp. Likewise, the HAp formation may be expressed as the following equation:
10 Ca ( NO 3 ) 2 · 4 H 2 O + 6 NH 4 2 HPO 4 +   8 NH 4 OH   →   Ca 10 ( PO 4 ) 6 ( OH ) 2 + 20 NH 4 NO 3 +   46 H 2 O .
Briefly, stock solutions were prepared by dissolving calcium nitrate tetrahydrate (Ca (NO3)2 4H2O, 2.3662 g, Meyer analytical grade) and ammonium phosphate dibasic ((NH4)2·HPO4, 0.7932 g, Meyer analytical grade) in 160.6 mL of distilled water, each. These stock solutions were then mixed dropwise and kept under stirring to produce Ca/P suspensions with stoichiometric molar ratios of 1.67. Subsequently, the solutions were brought to the desired pH (7, 8, 9, and 10) by adding ammonium hydroxide (NH4OH, Meyer analytical grade). Finally, the suspensions at different pH were transferred to microwave-induced Teflon hydrothermal reactors (START D, Microwave Digestion System, Milestone S.R.L.) (Italian technology) keeping the temperature at 200 °C for 30 min; here, it is important to mention that the initial pH was controlled, but, once starting the chemical reaction inside the microwave oven, the pH was unchecked as the experimental procedure was performed in a closed system. At the end of the reaction, the products were washed twice with distilled water and recovered by centrifugation. Subsequently, the samples were placed in a drying oven at 80 °C for 24 h to eliminate moisture, and calcinated in a muffle at 500 °C for 4 h.

2.2. Physicochemical Characterization

The morphological properties were analyzed using a JEOL JEM-2010 (Japanese technology) HT Transmission Electron Microscope (TEM) with a 1.9 Å resolution. The X-ray diffraction technique (XRD) was carried out in a D8 Discover Bruker diffractometer (German technology) (CuKα = 1.5406 Å) operating at 40 kV and 40 mA to evaluate the HAp crystallinity. The diffractograms were obtained in a 2θ scale ranging from 10° to 70° with an incremental step size of 0.03°, and the acquisition time was set up at 2 s. The XRD patterns were refined and analyzed by the Rietveld method using the TOPAS software (Version 5, Copyright 1999-2014 Bruker AXS) [31,32] to determine the amounts (% fraction) of the different phases, as well as their effective crystallite average size. The Rietveld method allows calculating a theoretical XRD pattern, as well as matching it with the experimental diffraction pattern. The goodness of fit, between the theoretical and experimental diffractograms was determined by the weighted and expected profile (Rwp and Rexp, respectively), in which the ratio between the two (goodness of fit) χ2 = (Rwp/Rexp)2 should approach 1. Functional groups were elucidated by Infrared spectroscopy (FTIR) using a Spectrum Gx FTIR System (Perkin Elmer) (American technology) and the attenuated total reflection technique (ATR) in a wave number range from 4000 to 400 cm−1.

3. Results

3.1. The Effect of pH on the Size and Shape of HAp

The size and shape of the obtained HAp powders were evaluated by TEM. Figure 2 (left column) shows TEM micrographs where, depending on the initial reaction pH environment, different morphologies can be observed. Indeed, at pH values of 7 and 8, mainly semi-spherical (e.g., sub-hedral) particles were found, while, at the increased pH values of 9 and 10, well-defined rod-like shapes are observed.
The diameter and length size distribution histograms (middle and right columns) were built considering ca. 100 manual measurements. The average sizes (or mean) ± standard derivations are reported in Figure 2 and summarized in Table 2. Therefore, the HAp sample prepared at initial pH = 7 contains particles with an average diameter of 60.24 nm and an average length of 98.71 nm. At this condition, the presence of sub-hedral particles was confirmed. In the sample at pH = 8, particles with an average diameter of 48.89 nm and a length of about 81.64 nm are observed. On the other hand, at pH = 9 nanorods with a length/diameter (L/D) aspect ratio close to 2.973 (higher than the circularity value of 1.0, L = D) were formed, and it was notably observed that their radial dimension decreases by increasing the pH. Thus, the sample obtained at a pH value of 10, shows thinner nanorods with a diameter of 29.54 nm and length of approximately 106.6 nm (L/D = 3.608).
The dimensional raw data were also statistically analyzed performing one-way ANOVA using a licensed Prism 8 package. The Tukey’s method was applied for the multiple comparisons with a 99% confidence interval (0.01 significance). Table 3 reports the mixed-effects analysis. Briefly, we observed that the nano-objects radial dimension (diameter) significantly decrease at initial reaction pH of 9 and 10 in comparison with pH 7 and 8 (p value <0.0001). The HAp diameter did not vary comparing pH 7–8 and pH 9–10. In contrast, non-significant difference in the axial magnitude (length) was found for most of the HAp samples. Particularly, the length significantly changed comparing pH 8 vs pH 10. In summary, the morphological characteristics of the HAp synthesized by the performed microwave assisted hydrothermal method, depend on the initial pH reaction conditions, modulating the formation of nanosized sub-hedral and rod-like HAp.

3.2. The Effect of pH on the HAp Crystallite Properties

The samples, calcinated at 500 °C, were studied by XRD to determine the effect of pH over the crystallography characteristics of hydroxyapatite. Figure 3 shows the obtained X-ray diffractograms. All the samples displayed main characteristic peaks at 25.8°, 31.7°, 32.1°, 32.9°, 34.0°, and 46.69°, which correspond, respectively, to the indexing (0 0 2), (2 1 1), (−2 2 2), (3 0 0), (2 0 2), and (2 4 2) planes of the monoclinic lattice of HAp (Powder Diffraction File-PDF No. 01-089-4405). Diffraction peaks at 22.9°, 28.13°, 28.93°, and 48.09° that correspond to the planes (1 1 1), (1 2 2), (2 1 0), and (3 2 2) were also identified and are attributed to the planes of the hexagonal lattice of HAp (PDF card No. 00-009-0432). Specifically, for the HAp sample synthesized at pH = 7, some diffraction peaks with slightly intensities located at 18.47°, 20.16°, 26.66°, 27.68°, 29.55°, and 30.10° in 2-theta scale can be observed (black squares in Figure 3) and are associated with a calcium phosphate (Ca2P2O7) crystalline phase (PDF No. 00-33-0297), which is considered a byproduct of the chemical reaction. The insert in Figure 3 shows a magnified 2-theta scale region, between 62.5 and 67.0°, in which it is possible to appreciate the presence of both HAp crystalline phases.
To better elucidate the formation of monoclinic Hap, and taking into account that the XRD characteristic peaks of this phase overlap the hexagonal by geometric similarity (lattice parameters unit cell, Table 1), it was necessary to perform a Rietveld analysis to (i) identify and (ii) quantify the coexisting phases. Thus, Rietveld refinement confirms the presence of the monoclinic phase (Figure 3, orange full circles). Table 4 groups the main characteristic peaks and angles that individually identify each phase.
Moreover, Table 5 summarizes the phases’ contribution (%) and crystallite size (nm) obtained from the performed Rietveld analysis. The goodness of fit χ2 = (Rwp/Rexp)2 is shown in the last column, and, for all cases, this value approaches unity, indicating that the Rietveld refinement finds a good fit. Notably, during the refinement process, χ2 may start out large if the model is poor, and decreases as the model produces better agreement with the data [33]. Figure 4 illustrates, for the HAp sample synthesized at pH 10, its Rietveld refinement plot to support the obtained goodness of fit. In the insert, from 20° to 40° in 2-theta scale, it is possible to appreciate the individual diffraction peaks of the monoclinic HAp that, according to the Rietveld deconvolution, the peaks found at 26.431°, 27.556°, and 35.875° correspond respectively to (0 1 2), (1 1 2), and (2 7 1) hkl planes of this phase, which are forbidden for hexagonal HAp [24]. In this regard, R. Pérez-Solis et al. (2018) reported HAp with a high percentage of the monoclinic phase (80.94 wt%) obtained by means of the sol-gel method assisted by ultrasonic irradiation, and, through the use of synchrotron XRD and Rietveld refinement, they were able to quantify the presence of monoclinic and hexagonal HAp, reporting three deconvolved peaks around 2θ = 9.8; two that corresponded to the monoclinic phase, (100) at 2θ = 9.873 and (002) at 2θ = 9.856; and another attributed to the hexagonal phase at 2θ = 9.785 [34].
In summary, in this work, we found that the monoclinic phase is the most abundant (>85%), and we observed that the crystallite’s size decreases, from 43.80 nm to 22.90 nm, as the pH value increases. On the other hand, the presence of the hexagonal phase decreases, from ~15% down to ~5%, by increasing the pH. Therefore, at pH = 10, nanosized rod-like monoclinic (>95%) HAp may be successfully obtained by following this optimized soft microwave method.

3.3. The Effect of pH on the Presence of HAp Functional Groups

The obtained samples were complementary analyzed by FTIR. In Figure 5, the characteristic bands of HAp are observed. Firstly, the bands located at 3570 cm−1 and 633 cm−1 are associated with the OH− group of hydroxyapatites. Bands at 472, 566, 603, 960, and 1035–1092 cm−1 correspond to the PO4−3 group. Likewise, it is possible to visualize bands related to the CO3−2 group at 1640 and 1950 cm−1. The bands at lower wave numbers for the samples obtained at pH = 7 and pH = 8 are attributed to the presence of phosphate and calcium precursors that did not react during the synthesis process [35].
According to the information in Figure 5, it is possible to visualize the main functional groups, which are summarized in Table 6, considering the region of the spectrum where they are found.

4. Discussion

According to the results obtained in this work, the best condition needed to form homogeneous monoclinic hydroxyapatite nanorods, is a reaction pH of 10. To the best of the author’s knowledge, here, for the first time, monoclinic HAp nanorods are obtained from such simple and soft methodology. Moreover, our experimental protocol allowed us determining the fundamental role of pH on the microstructural characteristics of HAp, contributing to better control its size, shape, and crystallographic properties.
Thus, TEM confirmed the formation of HAp nanorods with dimensions between 29 to 60 nm in diameter and 81 to 106 nm in length. Additionally, we observed that higher initial pH values induced a decrease of 50% and increase of 23%, respectively, on the average nanorod diameter and length. Indeed, the electrical balance of hydroxyapatite is affected by pH, which promotes the movement of OH− and H+ ions and directly modifies the particle and crystallite structure [36]. For instance, at low pH values, agglomerates with sub-hedral particles were identified, which may be attributed to the presence of H+ ions. Certainly, during the synthesis at this initial pH condition, the precursors containing solutions are unsaturated and do not promote the Ca/P nucleation to form HAp (FTIR spectrum with unreacted precursors). On the other hand, at basic pH conditions, the interaction and movement of the pending OH− groups determine the formation of any of the two HAp phases that, if they are ordered on the C-axis (determined direction), a monoclinic phase is formed [37]. Therefore, various authors have explained the role of OH− ions in determining the properties of synthetic HAp, which is mainly based on their orientation that may generate ferroelectric and electrical properties [38]. Figure 6 shows a schematic representation of the modulated growth of HAp, which varies with the increase or decrease of the pH value (increase = OH− ions; decrease = H+ ions).
Moreover, the crystallite size is another factor related to the presence of H+ and OH− ions in solution. The Rietveld analysis confirmed a major presence of the monoclinic phase, which crystallite size decreases from about 44 to 23 nm according to the increase in OH− ions. In the hexagonal phase, an opposite effect was observed: the crystallite size increased as the pH grew from 21 up to 41 nm. Hence, we demonstrated that, by performing a simple and soft microwave synthesis, the monoclinic phase can be obtained, thus being an important scientific contribution as the monoclinic phase is considered thermodynamically more stable than the hexagonal phase. The formation of the monoclinic phase indicates a greater order in the nucleation process, which may be translated into a better hydroxyl group internal orientation with a structural sequence of OH-OH-OH. The presence of the characteristic functional groups of pure HAp (OH−, PO4 and CO3) was confirmed by FTIR at pH = 10. Contrarily, and as mentioned before, FTIR signals attributed to unreacted HAp precursors were observed at the lower pH values of 7 and 8.
Even if other authors have reported similar HAp synthesis (Table 7), a detailed study focused on evaluating its morphology, and on identifying its crystalline phases at different pH, has been missed [39]. As shown in this work, the Rietveld refinement would be an excellent option to better elucidate the presence and contribution of each hexagonal and monoclinic HAp phases and overcome the current lack of HAp localized studies that obstructs the monoclinic phase identification [40]. Table 7 reviews the main HAp characteristics from systems obtained by similar methods. For instance, T R Amalia et al. (2020) reported the synthesis of HAp using the microwave method, Ca(OH)2 and (NH4)2HPO4 precursors, initial pH values of 7, 9, and 11 (adjusted with HCl and NaOH), and irradiation times that varied from 15 to 25 min [41]. The authors performed an additional sintering process at 900 °C and evaluated the crystallinity, size, and morphology of the resulted HAp powders. Briefly, through the T. R. Amalia et al. (2020) methodology, round-like irregular agglomerated particles were obtained, and, contrary to our findings, an unclear shape modulation (i.e., from rounded to rod-like morphologies) was observed as a function of the pH. Particularly, they demonstrated that the additional sintering treatment increased the crystallite and particle size. Notably, at pH = 11 and prior to performing the sintering procedure, a crystallite size close to 17 nm, and an average particle size of about 63 nm, were found. After the additional treatment, they observed an important crystallite and particle size growth (~3 times). Authors reported the presence of chlorapatite at pH = 7 and 9 but did not clearly discuss either the contribution of the hexagonal or monoclinic HAp phases, assuming the presence of the conventionally reported hexagonal phase. K W Goh et al. (2020) used chicken eggshells as CaCO3 source, H3PO4, and NH4OH to vary the reaction pH (8, 9, 10, 11, and 12) [42]. The microwave irradiation time was fixed to 10 min to aid the performed chemical precipitation method. At pH = 10, authors obtained needle-like shaped particles with ca. 10–15 nm in diameter and 60–80 nm in length. Authors observed that, by increasing the pH, rounded particles might be formed. Yudin et al. [43] studied the influence of the microwave treatment time (up to 30 min) and pH of the initial precursors solution over the resulting characteristics of HAp. The synthesis was performed using Ca(NO3)2, 4H2O, and (NH4)2HPO4 at pH initial values of 8, 10, and 13 (adjusted with NH4OH) and 150 °C [43]. Yudin et al. [43] obtained irregular agglomerates, with a broad size distribution (0.5–25 μm) containing particles with sizes ranging from 17 to 46 nm. It was observed that the irradiation time induced the formation of calcium carbonate. However, authors did not specialize in identifying the hexagonal or monoclinic HAp phases, nor in the effect of pH over the crystallographic parameters. They determined that the textural properties of their agglomerates mimic the bone porosity, but the experimental procedure did not allow controlling the size and shape of the individual and aggregated HAp particles. Z-Y Cai et al. [44] reported the microwave assisted synthesis of hierarchical nanosheet-assambled HAp nanostructures (10 nm in thickness) at acidic conditions (pH = 5), rod-like HAp nanostructures (100 nm in length) at neutral (pH = 7) and alkali conditions (pH = 9), and heterogeneous structures (rods and prisms) at pH = 11 [44]. Authors used Na2HPO4·12H2O, Ca(CH3COO)2·H2O, 5-fluorouracil, and HCl/NaOH to adjust the precursors pH. The reaction was carried out at 120 °C for 10 min. The HAp was identified due to its crystallographic characteristics, including tri-calcium phosphate at pH = 11. Again, even if a clear effect of the initial pH was determined and supported by their results, no further phase’s elucidation was included in the work, assuming the hexagonal phase.
Therefore, our results and proposed methodology not only evidenced the HAp’s size and shape modulation through the initial Ca/P precursors solution pH, with significant differences at pH = 10, but also include the monoclinic phase elucidation by performing the Rietveld analysis, an uncommon reported method that displays relevant information about the synthetic biomimetic nano-HAp. Finally, the stable monoclinic obtained nanostructured HAp might be used in the well-known hard tissue replacement and reconstruction applications. Other applications include drug delivery [45], cell culture, antibodies purification at large scale [46], cell activation, CO2 gas sensing, catalysis, and water treatment with efficient results [47,48].

5. Conclusions

This work showed the effect of pH over the physicochemical main characteristics of the HAp synthesized by a microwave assisted hydrothermal method. The synthesis was performed at 200 °C, a low temperature condition that strongly differs from the conventional hydrothermal method. The obtaining of monoclinic HAp, at this low temperature and in the absence of external agents, is here reported for the first time. In brief, an increase in the monoclinic phase, from 85% to 95%, and a decrease, from 15% to 5%, in the hexagonal phase was observed according to the increase of pH. This confirmed that the monoclinic phase is a stable phase that can easily be induced by means of a simple and soft technique. The microwave assisted hydrothermal synthesis presented the following main advantages, energy saving, short processing time, high performance, economic and environmentally friendly procedure, high reproducibility, and simplicity. Finally, the synthesis pH modulated the particle and crystallite size and shape, thus being an excellent parameter to control the properties and applicability of HAp.

Author Contributions

Conceptualization, D.S.-C., M.I.R.V., E.S.-R. and V.R.-L.; Data curation, D.S.-C. and S.L.-O.; Formal analysis, D.S.-C., D.M.-A. and V.R.-L.; Funding acquisition, D.M.-A. and V.R.-L.; Investigation, D.S.-C., M.I.R.V., S.L.-O., D.M.-A., E.S.-R. and V.R.-L.; Methodology, D.S.-C., M.E.F.-G. and D.M.-A.; Project administration, D.M.-A. and V.R.-L.; Resources, D.M.-A. and V.R.-L.; Supervision, D.M.-A. and V.R.-L.; Validation, D.M.-A. and V.R.-L.; Visualization, D.S.-L., D.M.-A. and V.R.-L.; Writing—original draft, D.S.-C.; Writing—review & editing, D.S.-L., D.M.-A. and V.R.-L. All authors have read and agreed to the published version of the manuscript.

Funding

This research received no external funding.

Data Availability Statement

Data is contained within the article.

Acknowledgments

The authors are thankful to CONACYT for supporting the generation of Infrastructure through the INFR-2015-251767 project. Likewise, for the scholarships awarded belonging to the Doctorate program in Materials Sciences in the Universidad Autónoma del Estado de Hidalgo.

Conflicts of Interest

The authors declare no conflict of interest.

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Minerals 11 00314 g001 550
Figure 1. Schematic experimental protocol used to prepare synthetic HAp. The pH of the aqueous precursors’ solutions was adjusted prior to performing the chemical reaction inside the microwave oven.
Figure 1. Schematic experimental protocol used to prepare synthetic HAp. The pH of the aqueous precursors’ solutions was adjusted prior to performing the chemical reaction inside the microwave oven.
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Minerals 11 00314 g002 550
Figure 2. TEM micrographs of the HAp synthesized at different pH values and their corresponding diameter and length histograms (TEM scale bar: 100 nm). Depending on the initial reaction pH environment, different morphologies can be observed: standing out are the presence of semi-spherical particles for lower pH and rod-like shapes particles for higher pH.
Figure 2. TEM micrographs of the HAp synthesized at different pH values and their corresponding diameter and length histograms (TEM scale bar: 100 nm). Depending on the initial reaction pH environment, different morphologies can be observed: standing out are the presence of semi-spherical particles for lower pH and rod-like shapes particles for higher pH.
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Minerals 11 00314 g003 550
Figure 3. X-ray diffractograms of the HAp nanopowders synthesized at different initial pH conditions showing the presence of the calcium phosphate (■), hexagonal (▲) and monoclinic (●) HAp phases for the sample synthesized at pH = 7. Samples synthesized at pH 8, 9, and 10 showed only the presence of the monoclinic and hexagonal HAp phases. Insert: magnified region, from 62.5° to 67.0°, to appreciate the individual diffraction peaks of the monoclinic and hexagonal HAp crystalline phases.
Figure 3. X-ray diffractograms of the HAp nanopowders synthesized at different initial pH conditions showing the presence of the calcium phosphate (■), hexagonal (▲) and monoclinic (●) HAp phases for the sample synthesized at pH = 7. Samples synthesized at pH 8, 9, and 10 showed only the presence of the monoclinic and hexagonal HAp phases. Insert: magnified region, from 62.5° to 67.0°, to appreciate the individual diffraction peaks of the monoclinic and hexagonal HAp crystalline phases.
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Figure 4. Rietveld refinement plot showing the goodness of fit obtained between the measured and calculated intensities for the HAp sample synthesized at pH 10.
Figure 4. Rietveld refinement plot showing the goodness of fit obtained between the measured and calculated intensities for the HAp sample synthesized at pH 10.
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Figure 5. FTIR spectra of the HAp nanopowders synthesized at different initial pH values highlighting the presence of absorption bands at 3570 and 633 cm−1 associated with OH−group, and bands at 472, 566, 603, 960, and 1035–1092 cm−1 that correspond to the PO4−3 vibrational group.
Figure 5. FTIR spectra of the HAp nanopowders synthesized at different initial pH values highlighting the presence of absorption bands at 3570 and 633 cm−1 associated with OH−group, and bands at 472, 566, 603, 960, and 1035–1092 cm−1 that correspond to the PO4−3 vibrational group.
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Figure 6. Schematic model for the H− and OH− ions effect representation on nanoparticles morphology. According to the role of OH− ions, mainly based on their orientation that may generate ferroelectric and electrical properties, this model allows showing the fundamental role of pH on the microstructural characteristics of HAp, thus contributing to better control of its size, shape and crystallographic properties.
Figure 6. Schematic model for the H− and OH− ions effect representation on nanoparticles morphology. According to the role of OH− ions, mainly based on their orientation that may generate ferroelectric and electrical properties, this model allows showing the fundamental role of pH on the microstructural characteristics of HAp, thus contributing to better control of its size, shape and crystallographic properties.
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Table
Table 1. Comparison between hydroxyapatite (Hap) phases [25,26,27,28].
Table 1. Comparison between hydroxyapatite (Hap) phases [25,26,27,28].
CharacteristicHexagonal HApMonoclinic HAp
Chemical formulaCa5(PO4)3OH
PDF-00-009-0432		Ca5 (PO4)3 (OH) PDF-01-089-4405
Space groupP63/mP21/b
Lattice parameters unit cella= b= 9.432 Å, c= 6.881 Å
and γ = 120°		a= 9.421 Å, b= 2a, c= 6.881 Å
and γ = 120°
OH− positionOpposite directionSame direction
Table
Table 2. Length/diameter (L/D) and aspect ratio of the HAp synthesized by the microwave-assisted method varying the pH.
Table 2. Length/diameter (L/D) and aspect ratio of the HAp synthesized by the microwave-assisted method varying the pH.
SampleDiameter
Mean ± SD		Length
Mean ± SD		Aspect Ratio
L/D
pH 760. 24 ± 29.4598.71 ± 48.141.637 ± 0.001
pH 848.89 ± 25.8781.64 ± 42.911.669 ± 0.003
pH 930.40 ± 9.11590.39 ± 46.622.973 ± 0.494
pH 1029.54 ± 7.817106.6 ± 33.443.608 ± 0.140
Table
Table 3. Statistical analysis performed over the HAp dimensional parameters.
Table 3. Statistical analysis performed over the HAp dimensional parameters.
Diameter Analysis
TestMean
Difference		99.00% CI
of Difference		Significant?SummaryAdjusted
p Value
pH 7 vs. pH 811.35−1.869 to 24.57No*0.0358
pH 7 vs. pH 929.8419.99 to 39.70Yes****<0.0001
pH 7 vs. pH 1030.7021.16 to 40.25Yes****<0.0001
pH 8 vs. pH 918.499.615 to 27.37Yes****<0.0001
pH 8 vs. pH 1019.3510.49 to 28.22Yes****<0.0001
pH 9 vs. pH 100.8603−3.120 to 4.840Nons0.9005
Length analysis
TestMean
Difference		99.00% CI
of Difference		Significant?SummaryAdjusted
pValue
pH 7 vs. pH 817.07−1.145 to 35.29No*0.0180
pH 7 vs. pH 98.324−9.797 to 26.45Nons0.4610
pH 7 vs. pH 10−7.886−26.64 to 10.87Nons0.5379
pH 8 vs. pH 9−8.751−28.41 to 10.90Nons0.4885
pH 8 vs. pH 10−24.96−40.98 to −8.944Yes****<0.0001
pH 9 vs. pH 10−16.21−35.51 to 3.095No*0.0419
CI = Confidence Intervals; * = Identifies adjusted p values between 0.01 and 0.05; **** = Identifies adjusted p values < 0.0001, significant difference; ns. = nonsignificant.
Table
Table 4. Main planes and angles of the HAp hexagonal and monoclinic phases.
Table 4. Main planes and angles of the HAp hexagonal and monoclinic phases.
Hexagonal (PDF-00-009-0432)Monoclinic (PDF-01-089-4405)
PlanePeakPlanePeak
(100)10.839°(100)10.830°
(101)16.846°(101)16.830°
(002)25.880°(002)25.853°
(102)28.131°(102)28.102°
(211)31.785°(221)31.740°
(112)32.201°(222)32.165°
(300)32.921°(060)32.872°
(221)40.463°(023)40.797°
(213)49.499°(223)49.437°
Table
Table 5. Obtained phases and crystallite size by Rietveld analysis.
Table 5. Obtained phases and crystallite size by Rietveld analysis.
SampleHexagonal HApMonoclinic HAp (χ2)
Phase (%)CrystalliteSize (nm)Phase (%)CrystalliteSize (nm)RwpRexp
pH 714.9621.385.0443.805.814.681.54
pH 83.2634.396.7436.805.584.461.56
pH 93.2838.896.7226.205.204.331.44
pH 104.7640.895.2422.904.824.361.22
χ2. This term is defined as a good measure of the quality of fit to a powder diffraction pattern. It is the weighted sum of the squares of the difference between the observed and calculated powder diffraction patterns [33].
Table
Table 6. Functional groups, FTIR bands, and vibrational modes identified in the HAp samples.
Table 6. Functional groups, FTIR bands, and vibrational modes identified in the HAp samples.
Functional GroupBandsVibrational Mode
OH−3570 and 633 cm−1Stretching and bending
PO4−3472, 566, 603, 960, 1035 and 1092 cm−1Stretching
CO3−21640 and 1950 cm−1Bending
Table
Table 7. Results obtained with similar HAp systems from the literature.
Table 7. Results obtained with similar HAp systems from the literature.
Initial pHObtained PhaseMorphologyRietveld
Analysis		Reference
7, 9 and 11Hexagonal and chlorapatiteRounded shapeWithout[40]
8, 9, 10, 11 and 12HexagonalNeedle-like shapeWithout[41]
8, 10 and 13Hexagonal and calcium
carbonate		Irregular shapeWithout[42]
5, 7, 9 and 11Hexagonal
tri-calcium phosphate		Nanorods and
hierarchical shape		Without[43]
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Sánchez-Campos, D.; Reyes Valderrama, M.I.; López-Ortíz, S.; Salado-Leza, D.; Fernández-García, M.E.; Mendoza-Anaya, D.; Salinas-Rodríguez, E.; Rodríguez-Lugo, V. Modulated Monoclinic Hydroxyapatite: The Effect of pH in the Microwave Assisted Method. Minerals 2021, 11, 314. https://doi.org/10.3390/min11030314

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Sánchez-Campos D, Reyes Valderrama MI, López-Ortíz S, Salado-Leza D, Fernández-García ME, Mendoza-Anaya D, Salinas-Rodríguez E, Rodríguez-Lugo V. Modulated Monoclinic Hydroxyapatite: The Effect of pH in the Microwave Assisted Method. Minerals. 2021; 11(3):314. https://doi.org/10.3390/min11030314

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Sánchez-Campos, Daniel, Maria Isabel Reyes Valderrama, Susana López-Ortíz, Daniela Salado-Leza, María Eufemia Fernández-García, Demetrio Mendoza-Anaya, Eleazar Salinas-Rodríguez, and Ventura Rodríguez-Lugo. 2021. "Modulated Monoclinic Hydroxyapatite: The Effect of pH in the Microwave Assisted Method" Minerals 11, no. 3: 314. https://doi.org/10.3390/min11030314

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