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Article

Preparation and Characterization of Mono- and Biphasic Ca1−xAgxHPO4·nH2O Compounds for Biomedical Applications

by
Fahad Abdulaziz
1,
Khalil Issa
2,
Mohammed Alyami
3,
Satam Alotibi
3,
Abdulaziz A. Alanazi
4,
Taha Abdel Mohaymen Taha
5,6,
Asma M. E. Saad
3,
Gehan A. Hammouda
4,
Nagat Hamad
3 and
Mazen Alshaaer
3,7,*
1
Department of Chemistry, College of Science, University of Ha’il, Ha’il 81451, Saudi Arabia
2
Orthopedics Unit, Faculty of Medicine and Health Sciences, An-Najah National University, Nablus 00972, Palestine
3
Department of Physics, College of Science and Humanities in Al-Kharj, Prince Sattam bin Abdulaziz University, Al-Kharj 11942, Saudi Arabia
4
Department of Chemistry, College of Science and Humanities in Al-Kharj, Prince Sattam bin Abdulaziz University, Al-Kharj 11942, Saudi Arabia
5
Physics Department, College of Science, Jouf University, P.O. Box 2014, Sakaka 72388, Saudi Arabia
6
Physics and Engineering Mathematics Department, Faculty of Electronic Engineering, Menoufia University, Menouf 32952, Egypt
7
Department Mechanics of Materials and Constructions (MEMC), Vrije Universiteit Brussels (VUB), Pleinlaan 2, 1050 Brussels, Belgium
*
Author to whom correspondence should be addressed.
Biomimetics 2023, 8(7), 547; https://doi.org/10.3390/biomimetics8070547
Submission received: 10 October 2023 / Revised: 9 November 2023 / Accepted: 12 November 2023 / Published: 14 November 2023
(This article belongs to the Special Issue Advances in Biomaterials, Biocomposites and Biopolymers)
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Abstract

:
This study aimed to explore the effects of the full-scale replacement (up to 100%) of Ca2+ ions with Ag1+ ions in the structure of brushite (CaHPO4·2H2O). This substitution has potential benefits for producing monophasic and biphasic Ca1−xAgxHPO4·nH2O compounds. To prepare the starting solutions, (NH4)2HPO4, Ca(NO3)2·4H2O, and AgNO3 at different concentrations were used. The results showed that when the Ag/Ca molar ratio was below 0.25, partial substitution of Ca with Ag reduced the size of the unit cell of brushite. As the Ag/Ca molar ratio increased to 4, a compound with both monoclinic CaHPO4·2H2O and cubic nanostructured Ag3PO4 phases formed. There was a nearly linear relationship between the Ag ion ratio in the starting solutions and the wt% precipitation of the Ag3PO4 phase in the resulting compound. Moreover, when the Ag/Ca molar ratio exceeded 4, a single-phase Ag3PO4 compound formed. Hence, adjusting the Ag/Ca ratio in the starting solution allows the production of biomaterials with customized properties. In summary, this study introduces a novel synthesis method for the mono- and biphasic Ca1−xAgxHPO4·nH2O compounds brushite and silver phosphate. The preparation of these phases in a one-pot synthesis with controlled phase composition resulted in the enhancement of existing bone cement formulations by allowing better mixing of the starting ingredients.

1. Introduction

Currently, there is a strong demand for improved bone substitutes and implants to treat various bone defects in the body [1,2] stemming from causes like osteoporosis, surgeries, and fractures. Traditionally, autografts are the common solution for bone replacement [2]. However, conventional bone implants and substitutes pose challenges, such as a high infection risk, limited graft materials, and complications [3,4]. Moreover, bone marrow treatment faces limitations due to donor shortages and safety concerns [5,6]. Implant-related infections are a significant issue with serious clinical and socioeconomic consequences [7,8]. Bacterial biofilm formation on inert surfaces and nearby tissues is a major problem, reducing susceptibility to host defenses and antimicrobial treatments [9]. Current remedies involve surgery, antibiotics, and even implant removal, leading to more surgeries, extended hospital stays, and increased mortality [10]. To address these challenges, synthetic bone materials have emerged as a safer alternative to autografts, offering reduced infection risks and complications. There is also a rising need for clinically viable implants that can naturally degrade in the body.
Biodegradable materials are promising as bone substitutes because they can be absorbed and replaced by natural bone tissue over time, eliminating the need for additional surgeries. These materials possess osteogenic, osteoinductive, and osteoconductive properties. However, a significant obstacle in using biodegradable materials for bone regeneration is their integration and vascularization within the body [11,12]. Calcium phosphate (CaP) plays a crucial role in various fields, including medicine, biology, engineering, and environmental science, due to its structural characteristics [13]. CaPs are advantageous for medical applications because they are biocompatible, low in toxicity, highly bioactive, and similar to natural mineral phases in bone tissue [1,6]. Currently, CaPs are used in advanced biocements and bioceramics for dental and medical interventions [11,14].
In supersaturated solutions, various CaP phases can form, such as amorphous calcium phosphate (ACP) or hydroxyapatite (HA), brushite (DCPD), monetite (DCPA), β-tricalcium phosphate (β-TCP), and octacalcium phosphate (OCP) [13,14,15,16,17,18]. These phases vary in solubility and crystalline structures. Calcium phosphate phases can spontaneously form in aqueous supersaturated solutions or with substrate assistance through seeded crystal growth [13]. Dicalcium phosphate dihydrate (DCPD, CaHPO4·2H2O), known as brushite, is crucial, serving as a precursor for bioceramics, bone cement, and hydroxyapatite (HA) [12,19]. It remains stable at pH levels of 4.0–6.5 and low temperatures [20] and can be reabsorbed by the body, supporting bone tissue remodeling, as it is typically metastable at a pH of around 7.4 [21].
Brushite has been utilized as a precursor for other CaP phases, such as HA and OCP. This mineral (phase) crystallizes in a monoclinic structure (space group Ia) with lattice parameters a = 5.81, b = 15.18, c = 6.24, and β = 116.42° [3]. It exhibits a layered structure, with corrugated sheets of CaHPO4 and two water molecules alternating along the [010] direction. The octahedral is represented by every Ca2+ ion being surrounded by six phosphate oxygen molecules from four phosphoryl groups (HPO4)2− and two oxygen molecules from two water molecules [6]. The monoclinic structure of these calcium ions allows protons to migrate toward the electrode–electrolyte interface through their interaction with the oxygen atom of the phosphate group and water molecules. Moreover, the characteristic features of brushite, like high porosity, good biocompatibility, and high adsorption capacity, make it a suitable candidate material for biomedical applications.
Unfortunately, bone implants can be vulnerable to bacterial colonization in environments with reduced blood supply and local immunodeficiency, leading to postoperative infections that may require implant removal [22,23]. Metal ions, including Ag+, Cu2+, and Zn2+, are recognized as antimicrobial agents in CaPs [24,25,26]. Ag+ is particularly known for its antibacterial properties against various microorganisms, including antibiotic-resistant strains [27], demonstrating high antimicrobial activity with relatively low cytotoxicity [28,29]. Dissolved Ag ions in the human body exhibit antibacterial effects through multiple mechanisms, including deactivation of electron donor groups, membrane interaction, and the generation of reactive oxygen species (ROS) and DNA damage within bacterial cells [30,31]. Consequently, the addition of Ag to CaPs has been explored in several studies [32]. However, high Ag ion concentrations in body fluids can be toxic to certain tissues [33], prompting the establishment of a recommended exposure limit (REL) for soluble Ag compounds and Ag metal dust by the National Institute for Occupational Safety and Health (NIOSH) [34].
In previous [35,36,37,38,39] studies, CaPs like HA and TCP have been utilized to synthesize biomaterials that have antibacterial properties and no cytotoxicity. It was found that Ag-containing CaPs are safe and can prevent infection for long-term in vivo applications. The production of silver phosphate and calcium phosphates was carried out separately with the use of a precipitation method [36]. Subsequently, the two phases were incorporated into a resin in mass fractions below 30% for antibacterial and biomedical purposes. One of the advanced applications of silver phosphate/CaP compounds is silver-loaded calcium phosphate bone cement with CaP phases such as brushite, HA, and TCP [37]. The molar ratio of Ag/Ca used to prepare those cements was 5%. In addition to CaPs, pure Ag3PO4 powder was introduced as a precursor of bone cement in that study. Silver phosphate showed significant effects on the morphology, setting time, and phase composition of the final cements. Loaded silver ions extended the final setting time of the bone cement by approximately 25%. The XRD indicated a change in the cement’s crystalline composition, with peaks of whitlockite visible in samples loaded with silver. According to FTIR spectroscopy, the phase of pyrophosphate was present. It has also been observed that implant-associated infections can be eliminated effectively with silver-loaded calcium phosphate bone cement [38]. The antibacterial capability and biomechanical properties of end products can be enhanced by adding silver ions to calcium phosphate bone cement, as shown in previous studies [37,38]. In summary, silver-loaded calcium phosphate bone cements are characterized by high cytocompatibility, good injectability, and good interdigitating in spongy bone, with sustainable antibacterial effects. Therefore, these cements bear great potential for the treatment of bone infections or implant-associated infections.
Both brushite (CaHPO4·2H2O) and silver phosphate (Ag3PO4) play significant roles in biomedical applications and complement each other. Nonetheless, careful consideration of the Ag content in these compounds is crucial to avoid adverse effects. Therefore, when developing bone substitutes and implants, it is vital to balance factors like biocompatibility, bioactivity, osteogenic properties, and potential antimicrobial effects. Calcium phosphate (CaP) materials, particularly dicalcium phosphate dihydrate (DCPD or brushite), hold promise in bone regeneration due to their biocompatibility and resemblance to natural bone tissue. Introducing antimicrobial agents like silver ions (Ag+) into CaP materials can help prevent implant-related infections. Nevertheless, it is imperative to carefully control the concentration of silver ions to avoid detrimental effects.
According to the above, there has not yet been a full study of the effects of gradual full-scale (up to 100%) silver replacement for calcium in brushite, with only the effect of doping brushite with a lower percentage of silver ions, less than 5%, having been investigated. In addition, no compound containing both silver phosphate and calcium phosphate has ever been synthesized in specific ratios, despite the importance of combining both phases in biomedical applications. However, both phases have been prepared separately [37] and then mixed. Therefore, this research work’s novelty lies in its study of the effect of full-scale substitution and replacement (up to 100%) of Ca ions in brushite with Ag ions. At each level of ion replacement, the phase composition, thermal properties, and crystal morphology of the produced powders were investigated. The findings of this research fill an important research gap and may prove valuable for mineral synthesis to derive novel (Ag and Ca) phosphate-based precursors of biomaterials with unique bioactive and antibacterial characteristics. Synthesized products and minerals have great potential in bone cement and bioceramic synthesis, as well as have a variety of applications in the bone tissue engineering and pharmaceutical industries.

2. Materials and Methods

2.1. Materials

This study used chemicals obtained from different suppliers. Diammonium hydrogen phosphate ((NH4)2HPO4) was sourced from Techno Pharmchem in Delhi, India. Calcium nitrate tetrahydrate (Ca(NO3)2·4H2O) and silver nitrate hexahydrate (AgNO3·6H2O) were purchased from LOBA Chemie in Mumbai, India. To ensure their purity, we prepared distilled water with a low conductivity of 0.055 µS/cm using the PURELAB option-Q purification system from ELGA in the UK. To ensure precise measurements, we used an EX324N digital analytical balance from OHAUS in Parsippany, NJ, USA, and an ISOTEMP magnetic stirrer from Fisher Scientific in China, as needed.

2.2. Synthesis of Ca1−xAgxHPO4·nH2O Compounds

Seven different compounds of Ca1−xAgxHPO4·nH2O were synthesized at room temperature (RT) using solutions of (NH4)2HPO4, Ca(NO3)2·4H2O, and AgNO3 with specific molar proportions, as shown in Table 1, and Figure 1.
To prepare pure brushite (referred to as BAg0 in Table 1), 100 mL of the Ca(NO3)2·4H2O solution was mixed with the (NH4)2HPO4 solution at a controlled flow rate of approximately 2 mL/min. This mixing process was conducted using a glass funnel equipped with a stopcock while maintaining a stirring speed of 450 rpm until achieving a 1 Ca/P molar ratio, which took approximately one hour. The resulting solution was stirred at RT for 60 min to ensure thorough mixing. Ammonia (~15 moL/L, Labochemie, Mumbai, India) was added to maintain the pH level within the range of 6–6.5. The resulting white precipitate was separated using a Büchner funnel and qualitative filter paper (45 µm, Ø 12 cm, Double Rings, China). The filter cake underwent three washes with deionized water and ethanol to prevent clumping [40,41,42]. Finally, the sample was dried in an oven (set at 40 °C) for 7 days on a watch glass (ED53/E2, Binder, Tuttlingen, Germany) [18].
For compounds BAg2, BAg4, BAg5, BAg6, and BAg10, we combined the Ca(NO3)2·4H2O and AgNO3 solutions in the molar ratios outlined in Table 1. Following a procedure similar to the one described earlier, 100 mL of the resulting solution was introduced into 100 mL of the (NH4)2HPO4 solution at a controlled flow rate of approximately 2 mL/min. The same approach was used to prepare BAg10 but using a mixture of (NH4)2HPO4 and AgNO3.

2.3. Characterization Techniques

Qualitative mineralogical analysis was conducted on the BAg0–BAg10 samples using a Shimadzu XRD diffractometer-6000 from Kyoto, Japan. The analysis involved using a cobalt tube and scanning in the 2-theta range of 10–60° at a scan rate of 2°/min. For phase and crystal analysis, Match! software (version 3.15, Crystal Impact, Bonn, Germany) was used to process powder XRD diffraction data.
To obtain a comprehensive view of the product morphology, scanning electron microscopy with an Inspect F50 instrument was used (FEI Company, Eindhoven, The Netherlands). Surface chemistry and in-depth sample analysis were evaluated using an XPS system, specifically the Thermo K Alpha spectrometer from the USA, which conducted elemental X-ray photoelectron spectroscopy.
Additionally, a thermogravimetric (TG) analyzer (Netzsch, Waldkraiburg, Germany, TG 209 F1 Libra) was used to measure the mass loss (approximately 100 mg) of each product as they were heated from 40 to 750 °C, in increments of 5 °C/min, under a helium atmosphere.
To determine the silver (Ag) content of the synthesized compounds, inductively coupled plasma optical emission spectrometry (ICP-OES) using the Thermo Fisher Scientific iCAP 7000 series instrument was used.

3. Results and Discussion

3.1. Mineralogical and Microstructural Analysis

In Figure 2, we present XRD scan analyses of various samples, including pure Ca-HPO4·2H2O (Ag0) and pure Ag3PO4 (Ag10). The qualitative mineralogical analysis confirmed the formation of pure brushite (BAg0) by combining solutions of Ca(NO3)2·4H2O and (NH4)2HPO4 with a Ca to P molar ratio of 1:1, as detailed in Table 1. The crystals showed expansion in three primary crystallographic planes with Miller indices of (020), (12 1 - ), and (14 1 - ), indicating a monoclinic structure [43]. Importantly, the XRD peak at 2-theta of 11.7° indicated significant crystal growth along the (020) plane [43].
As the Ag/Ca molar ratios increased from 0.25 to 4, biphasic compounds of CaHPO4·2H2O and Ag3PO4 formed, as evidenced by the patterns of BAg2, BAg4, BAg5, BAg6, and BAg8. The prominent planes corresponding to the new phase (Ag3PO4) included (110), (200), (210), (211), (220), (310), (333), (320), and (321) [39]. When the complete replacement of Ca with Ag ions occurred in the initial solutions, a monophasic compound of Ag3PO4 (Ag10) was formed. Residual salts of ammonium phosphate were observed between 10° and 30° in the XRD pattern (Figure 2).
To delve deeper into the phase composition and unit cell parameters of the compounds, we conducted XRD scans and used Rietveld refinement and MATCH! software analysis, with the results reported in Table 2. The increase in Ag ions in the initial solutions (Table 1) corresponded to an increase in the proportion of Ag3PO4 at the expense of CaHPO4·2H2O. The weight percentage of CaHPO4·2H2O decreased while the weight percentage of Ag3PO4 increased, exhibiting an almost linear relationship (Figure 3). The crystal structures, lattice parameters, and unit cell volumes of both phases matched their respective standards [18,44,45]. The unit cell volume of CaHPO4·2H2O decreased with an increasing Ag/Ca molar ratio up to 0.67 but remained relatively stable thereafter. These variations in unit cell volume indicate that the Ag ions not only participated in Ag3PO4 precipitation but also became integrated into the CaHPO4·2H2O lattice as dopants or substitutes. A monophasic phase of Ag3PO4 (BAg10) was formed when the Ag/Ca ratio exceeded 4.
In Figure 4, the SEM images reveal monophasic CaHPO4·2H2O (BAg0) and Ag3PO4 (Ag10), as well as biphasic compounds (BAg2, BAg4, BAg5, BAg6, and BAg8), with varying Ag/Ca molar ratios. Monoclinic crystals of brushite (BAg0) with dimensions of 0.5 × 5 × 10 µm3 were observed, consistent with prior studies [46,47]. As the Ag/Ca molar ratio increased, nanosized cubic crystals of Ag3PO4 appeared alongside monoclinic CaHPO4·2H2O, as evident in the SEM images. The Ag3PO4 content increased with higher Ag/Ca molar ratios. Notably, BAg10 exhibited larger cubic crystals of Ag3PO4 compared with the other compounds.
The SEM analysis corroborated the XRD findings, confirming the presence of Ag3PO4 in the resulting compounds. The elemental analysis revealed an incremental trend in Ag content. These results established a clear relationship between the proportions of Ag3PO4 and the Ag content in the initial solutions (Figure 3 and Figure 4), confirming the involvement of Ag in various stages of the reactions

3.2. FTIR Spectrum of the Ca1−xAgxHPO4·nH2O Compounds

In Figure 5, we present the infrared spectra (FTIR) of the compounds CaHPO4·2H2O and Ag3PO4. These FTIR results align with the XRD analysis findings. The spectrum of CaHPO4·2H2O (Ag0) displays distinct absorption bands that are characteristic of this phase [48,49]. Notably, the broad absorption peak spanning from 2400 to 3600 cm–1 in BAg0, BAg2, BAg4, BAg5, BAg6, and BAg8 is attributed to the O–H stretching vibration within CaHPO4·2H2O [50]. The presence of P–O–P asymmetric stretching vibrations is evidenced by the band at 983 cm–1, P=O stretching, while the bands at 654 and 569 cm–1 may be attributed to (H–O–)P=O in acid phosphates [51]. Additionally, the peak at 1643 cm–1 indicates the presence of water, with its intensity diminishing as the CaHPO4·2H2O content decreased in the samples (BAg2, BAg4, BAg5, BAg6, BAg8, and BAg10).
As the Ag content in the initial solutions increased from BAg2 to BAg10, new peaks emerged at 960 and 548 cm–1, corresponding to P–O bending vibrations in Ag3PO4. The presence of ammonium cations in the BCo10 compound was confirmed with infrared spectroscopy, revealing bands at 2840 and 1440 cm–1 [29,30].

3.3. Elemental Analysis of CaHPO4·2H2O and Ag3PO4

XPS analysis was conducted to examine the chemical states of Ag, Ca, and P in the prepared CaHPO4·2H2O and Ag3PO4 compounds, shedding light on their surface chemistry, as depicted in Figure 6. The phase composition of these compounds was notably influenced by the Ag/Ca molar ratio in the initial solution. The XPS spectra of compounds ranging from Bag2 to Bag10 revealed distinct peaks associated with the Ag 3d and Ag 3p orbitals. These peaks’ concentrations gradually increased, reaching their peak intensity at Bag10, while the intensity of the Ca 2p and Ca 2s peaks exhibited a proportional decrease with the escalating Ag/Ca ratio. Conversely, the intensity of the P 2s peak remained relatively stable, indicating that the concentrations of the P, Ca, and Ag peaks were contingent on the extent of Ca substitution with Ag and the quantities of precipitated compounds, particularly at higher Ag/Ca molar ratios.
The influence of the Ag/Ca ratio on the binding energies of Ag 3d, Ca 2s, and P 2s, along with the corresponding peaks, is evident in Figure 7A–C, respectively. Notably, for the Ag/Ca 0.25 (BAg2) molar ratio, the binding energies of the P 2s and Ca 2s peaks exhibited an increase from 438 to 442 eV and from 190 to 193 eV, respectively [3]. Furthermore, the Ca 2s and Ca 2p peaks disappeared in the BAg10 compound because no Ca ions were added to the starting solutions (see Table 1). The binding energy attributed to Ag 3d was observed at 371 eV for biphasic compounds with Ag3PO4 contents ranging from BAg2 to BAg8 [52].
Further evidence of the Ag/Ca ratio’s influence can be observed in the assessments of P 2s, as presented in Figure 7C. The appearance of Ca 2s peaks in BAg2 to BAg8 signifies the co-precipitation of CaHPO4·2H2O alongside Ag3PO4. However, these peaks vanished at higher Ag/Ca molar ratios (BAg10) due to the formation of pure Ag3PO4. In summary, the XPS findings firmly establish that an increase in the Ag/Ca molar ratio in the initial solution (BAg2–BAg8) led to the formation of a biphasic phosphate compound composed of CaHPO4·2H2O and Ag3PO4. Conversely, altering the crystal structure of the CaHPO4·2H2O and Ag3PO4 compounds necessitated raising the binding energies of the Ca 2s and P 2s peaks. As the Ag intensity rose and the Ca concentration decreased, the degree of supersaturation concerning CaHPO4·2H2O diminished. Consequently, a pure Ag3PO4 compound was obtained when the Ca availability was low (below 20%), as observed in the BAg10 compound.
The XPS results corroborate the presence of Ag in compounds ranging from BAg2 to BAg10. Notably, despite setting the Ag/Ca molar ratio to 4 in the starting solutions, no Ca ions were detected in BAg10, aligning with the XRD analysis presented in Figure 2. Lastly, the shifts in the peaks of Ca and P to higher positions, resulting from the addition of Ag in the starting solutions (BAg2–BAg10), signify alterations in the surroundings of these elements induced by the precipitation of the new phase (Ag3PO4).

3.4. Thermogravimetric Analysis (TGA)

The TGA analysis results for the investigated materials (BAg0–BAg10) are presented, shedding light on the arrangement of Ca ions with six PO4 ions and two oxygen atoms belonging to the structural water in brushite [53]. Additionally, the presence of Ca-HPO4·2H2O was confirmed with the observation of two distinct peaks indicating mass loss during the temperature increase from 80 to 220 °C. These peaks are indicative of the release of the structural water molecules within the lattice and the adsorbed water molecules on the surface [42,54].
Based on the available evidence, it is suggested that a portion of the chemically attached water was released during the conversion of brushite to monetite (CaHPO4) at around 220 °C, with further conversion to calcium pyrophosphate (Ca2P2O7) occurring as the temperature rose to approximately 400 °C [55]. In the current study, heating pure CaHPO4·2H2O (BAg0) to 750 °C resulted in a mass loss of approximately 24.8 wt%, consistent with the expected hypothetical mass loss of 20.93 wt% [56]. In contrast, the BAg2–BAg10 samples, with increasing Ag/Ca ratios, experienced lower mass losses ranging from 5.4% to 20.1% (Figure 8).
The dehydration reaction of brushite is represented by Equation (1), while the formation of calcium pyrophosphate can be explained by Equation (2).
C a H P O 4 · 2 H 2 O → C a H P O 4 + 2 H 2 O
2 C a H P O 4 → C a 2 P 2 O 7 + H 2 O
Figure 9 illustrates the mass loss rate of the compounds as a function of temperature. Previous research [42] displayed clear dehydration peaks below 200 °C, attributed to the two structural water molecules of CaHPO4·2H2O (BAg0), as shown in Figure 9A–F. The thermal stability of the monophase Ag3PO4 compound (BAg10) was also studied, as depicted in Figure 9. Weight loss below 150 °C is attributed to the release of weakly adsorbed water, while a second weight loss between 150 and 260 °C corresponds to the dehydration of pristine Ag3PO4 [57]. The gradual decrease in weight loss associated with CaHPO4 in the range of 470–410 °C strongly indicates the increased presence of Ag3PO4 at the expense of CaHPO4·2H2O in the resulting compounds, from BAg0 to BAg10. These findings align with the previous XRD analysis results presented in Figure 3.

4. Conclusions

This research work highlighted the effect of full-scale gradual replacement of Ca ions with Ag ions in CaHPO4·2H2O. This process was thoroughly examined using a series of analyses, including XRD, SEM, XPS, FTIR, and TG, focusing on various Ca1−xAgxHPO4·nH2O compounds. This research achieved two main goals, as the first goal was to study the effect of the gradual full-scale replacement of Ag ions with Ca ions in brushite. Changes in crystal morphology, phase composition, and thermal properties were studied at each step of the replacement. The second goal was to synthesize a biphasic compound from silver phosphate and brushite for antibacterial and biomedical applications.
The results of Ca ion replacement with silver ions showed that when the Ag/Ca molar ratio in the initial solution fell below 0.25, Ag could partially substitute for Ca. With a gradual increase in the Ag/Ca molar ratio up to 4, biphasic compounds comprising CaHPO4·2H2O and Ag3PO4 appeared. The Ag3PO4 phase, characterized by a cubic crystal structure, was precipitated at an Ag/Ca molar ratio of 0.25. As the Ag/Ca molar ratio continued to rise, reaching higher supersaturation levels concerning Ag, a biphasic compound featuring monoclinic brushite and cubic Ag3PO4 was obtained. When the molar ratio of silver to calcium exceeded 4, a monophasic nanostructured Ag3PO4 precipitated. There was a nearly linear relationship between the Ag ion ratio in the starting solutions and the wt% precipitation of the Ag3PO4 phase in the resulting compound.
These findings hold significant implications for the future production of biomaterials, enabling the synthesis of materials with precise phase compositions, distinct structural characteristics, and tailored properties. This underscores the potential to achieve specific combinations of material components and geometries by controlling the Ag/Ca ratio in the initial solution.

Author Contributions

Conceptualization, M.A. (Mazen Alshaaer), K.I. and A.M.E.S.; methodology, M.A. (Mazen Alshaaer), N.H. and F.A.; software, M.A. (Mazen Alshaaer); validation, M.A. (Mazen Alshaaer) and F.A.; formal analysis, M.A. (Mazen Alshaaer), G.A.H. and A.M.E.S.; investigation, M.A. (Mazen Alshaaer) and A.A.A.; resources, M.A. (Mazen Alshaaer), T.A.M.T. and A.A.A.; data curation, M.A. (Mazen Alshaaer), F.A., T.A.M.T., N.H. and A.A.A.; writing—original draft preparation, M.A. (Mazen Alshaaer), M.A. (Mohammed Alyami) and K.I.; writing—review and editing, M.A. (Mazen Alshaaer), G.A.H. and M.A. (Mohammed Alyami); visualization, M.A. (Mazen Alshaaer); supervision, M.A. (Mazen Alshaaer) and M.A. (Mohammed Alyami); project administration, M.A. (Mazen Alshaaer), M.A. (Mohammed Alyami) and S.A.; funding acquisition, M.A. (Mazen Alshaaer), M.A. (Mohammed Alyami) and S.A. All authors have read and agreed to the published version of the manuscript.

Funding

This study was supported by funding from Prince Sattam bin Abdulaziz University (project number PSAU/2023/R/1444).

Institutional Review Board Statement

Not applicable.

Data Availability Statement

The data that support the findings of this study are available from the corresponding author (M. Alshaaer) upon reasonable request.

Conflicts of Interest

The authors declare no conflict of interest.

References

  1. Khalifehzadeh, R.; Arami, H. Biodegradable calcium phosphate nanoparticles for cancer therapy. Adv. Colloid Interface Sci. 2020, 279, 102157. [Google Scholar] [CrossRef] [PubMed]
  2. Wu, F.; Wei, J.; Guo, H.; Chen, F.; Hong, H.; Liu, C. Self-setting bioactive calcium-magnesium phosphate cement with high strength and degradability for bone regeneration. Acta Biomater. 2008, 4, 1873–1884. [Google Scholar] [CrossRef] [PubMed]
  3. Alshaaer, M.; Al-Kafawein, J.; Afify, A.; Hamad, N.; Saffarini, G.; Issa, K. Effect of Ca2+ Replacement with Cu2+ Ions in Brushite on the Phase Composition and Crystal Structure. Minerals 2021, 11, 1028. [Google Scholar] [CrossRef]
  4. Mouriño, V.; Cattalini, J.; Boccaccini, A. Metallic ions as therapeutic agents in tissue engineering scaffolds: An overview of their biological applications and strategies for new developments. J. R. Soc. Interface 2011, 9, 401–419. [Google Scholar] [CrossRef]
  5. Alshaaer, M.; Kailani, M.H.; Jafar, H.; Ababneh, N.; Awidi, A. Physicochemical and Microstructural Characterization of Injectable Load-Bearing Calcium Phosphate Scaffold. Adv. Mater. Sci. Eng. 2013, 2013, 149261. [Google Scholar] [CrossRef]
  6. Mert, I.; Mandel, S.; Tas, A.C. Do cell culture solutions transform brushite (CaHPO4 2H2O) to octacalium phosphate (Ca8(HPO4)2(PO4)4 5H2O)? In Advances in Bioceramics and Porous Ceramics IV; Narayan, R., Colombo, P., Eds.; John Wiley & Sons, Inc.: Hoboken, NJ, USA, 2011; pp. 79–94. [Google Scholar]
  7. Vallet-Regí, M. Our contributions to applications of mesoporous silica nanoparticles. Acta Biomater. 2022, 137, 44–52. [Google Scholar] [CrossRef]
  8. Sánchez-Salcedo, S.; García, A.; González-Jiménez, A.; Vallet-Regí, M. Antibacterial effect of 3D printed mesoporous bioactive glass scaffolds doped with metallic silver nanoparticles. Acta Biomater. 2023, 155, 654–666. [Google Scholar] [CrossRef] [PubMed]
  9. Donlan, R.; Costerton, J. Biofilms: Survival mechanisms of clinically relevant microorganisms. Clin. Microbiol. Rev. 2002, 15, 1671–1693. [Google Scholar] [CrossRef]
  10. Rosas, S.; Ong, A.; Buller, L.; Sabeh, K.; Law, T.; Roche, M.; Hernández, V. Season of the year influences infection rates following total hip arthroplasty. World J. Orthop. 2017, 8, 895–901. [Google Scholar] [CrossRef]
  11. Wei, S.; Ma, J.; Xu, L.; Gu, X.-S.; Ma, X.-L. Biodegradable materials for bone defect repair. Mil. Med. Res. 2020, 7, 1–25. [Google Scholar] [CrossRef] [PubMed]
  12. Alshaaer, M.; Kailani, M.H.; Ababneh, N.; Abu Mallouh, S.A.; Sweileh, B.; Awidi, A. Fabrication of porous bioceramics for bone tissue applications using luffa cylindrical fibres (LCF) as template. Process. Appl. Ceram. 2017, 11, 13–20. [Google Scholar] [CrossRef]
  13. Nosrati, H.; Quang Svend Le, D.; Zolfaghari Emameh, R.; Perez, M.C.; Bünger, C.E. Nucleation and growth of brushite crystals on the graphene sheets applicable in bone cement. Boletín Española Cerámica Vidr. 2020, 61, 27–34. [Google Scholar] [CrossRef]
  14. Tamimi, F.; Le Nihouannen, D.; Eimar, H.; Sheikh, Z.; Komarova, S.; Barralet, J. The effect of autoclaving on the physical and biological properties of dicalcium phosphate dihydrate bioceramics: Brushite vs. monetite. Acta Biomater. 2012, 8, 3161–3169. [Google Scholar] [CrossRef] [PubMed]
  15. Hurle, K.; Oliveira, J.; Reis, R.; Pina, S.; Goetz-Neunhoeffer, F. Ion-doped Brushite Cements for Bone Regeneration. Acta Biomater. 2021, 123, 51–71. [Google Scholar] [CrossRef] [PubMed]
  16. Dosen, A.; Giese, R.F. Thermal decomposition of brushite; CaHPO4·2H2O to monetite CaHPO4 and the formation of an amorphous phase. Am. Mineral. 2011, 96, 368–373. [Google Scholar] [CrossRef]
  17. Radwan, N.H.; Nasr, M.; Ishak, R.A.; Abdeltawa, N.F.; Awad, G.A. Chitosan-calcium phosphate composite scaffolds for control of postoperative osteomyelitis: Fabrication, characterization, and in vitro–in vivo evaluation. Carbohydr. Polym. 2020, 244, 116482. [Google Scholar] [CrossRef]
  18. Alshaaer, M.; Afify, A.; Moustapha, M.; Hamad, N.; Hammouda, G.; Rocha, F. Effects of the full-scale substitution of strontium for calcium on the microstructure of brushite: (CaxSr1–x)HPO4·nH2O system. Clay Miner. 2020, 55, 366–374. [Google Scholar] [CrossRef]
  19. Xue, Z.; Wang, Z.; Sun, A.; Huang, J.; Wu, W.; Chen, M.; Hao, X.; Huang, Z.; Lin, X.; Weng, S. Rapid construction of polyetheretherketone (PEEK) biological implants incorporated with brushite (CaHPO4·2H2O) and antibiotics for anti-infection and enhanced osseointegration. Mater. Sci. Eng. C 2020, 111, 110782. [Google Scholar] [CrossRef]
  20. Lu, B.Q.; Willhammar, T.; Sun, B.B.; Hedin, N.; Gale, J.D.; Gebauer, D. Introducing the crystalline phase of dicalcium phosphate monohydrate. Nat. Commun. 2020, 11, 1546. [Google Scholar] [CrossRef]
  21. Luo, J.; Engqvist, H.; Persson, C. A ready-to-use acidic, brushite-forming calcium phosphate cement. Acta Biomater. 2018, 81, 304–314. [Google Scholar] [CrossRef]
  22. Campoccia, D.; Montanaro, L.; Arciola, C. The significance of infection related to orthopedic devices and issues of antibiotic resistance. Biomaterials 2006, 27, 2331–2339. [Google Scholar] [CrossRef] [PubMed]
  23. Kilgus, D.; Howe, D.; Strang, A. Results of periprosthetic hip and knee infections caused by resistant bacteria. Clin. Orthop. Relat. Res. 2002, 404, 116–124. [Google Scholar] [CrossRef] [PubMed]
  24. Alanazi, A.A.; Abdulaziz, F.; Alyami, M.; Alotibi, S.; Sakka, S.; Mallouh, S.A.; Abu-Zurayk, R.; Alshaaer, M. The Effect of Full-Scale Exchange of Ca2+ with Zn2+ Ions on the Crystal Structure of Brushite and Its Phase Composition. Biomimetics 2023, 8, 333. [Google Scholar] [CrossRef] [PubMed]
  25. Laskus-Zakrzewska, A.; Zgadzaj, A.; Kolmas, J. Synthesis and physicochemical characterization of Zn-doped brushite. Ceram. Int. 2021, 47, 7798–7804. [Google Scholar] [CrossRef]
  26. Lowry, N.; Brolly, M.; Han, Y.; McKillop, S.; Meenan, B.; Boyd, A. Synthesis and characterisation of nanophase hydroxyapatite co-substituted with strontium and zinc. Ceram. Int. 2018, 44, 7761–7770. [Google Scholar] [CrossRef]
  27. Honda, M.; Kawanobe, Y.; Nagata, K.; Ishii, K.; Matsumoto, M.; Aizawa, M. Bactericidal and Bioresorbable Calcium Phosphate Cements Fabricated by Silver-Containing Tricalcium Phosphate Microspheres. Int. J. Mol. Sci. 2020, 21, 3745. [Google Scholar] [CrossRef]
  28. Ewald, A.; Hösel, D.; Patel, S.; Grover, L.B.J.; Gbureck, U. Silver-doped calcium phosphate cements with antimicrobial activity. Acta Biomater. 2011, 7, 4064–4070. [Google Scholar] [CrossRef]
  29. Fadeeva, I.; Gafurov, M.; Kiiaeva, I.; Orlinskii, S.B.; Kuznetsova, L.M.; Filippov, Y.Y.; Fomin, A.S.; Davydova, G.A.; Selezneva, I.I.; Barinov, S.M. Tricalcium Phosphate Ceramics Doped with Silver, Copper, Zinc, and Iron (III) Ions in Concentrations of Less Than 0.5 wt.% for Bone Tissue Regeneration. BioNanoScience 2017, 7, 434–438. [Google Scholar] [CrossRef]
  30. Schierholz, J.; Lucas, L.; Rump, A.; Pulverer, G. Efficacy of silver-coated medical devices. J. Hosp. Infect. 1998, 40, 257–262. [Google Scholar] [CrossRef]
  31. Feng, Q.; Wu, J.; Chen, G.; Cui, F.; Kim, T.; Kim, J. A mechanistic study of the antibacterial effect of silver ions on Escherichia coli and Staphylococcus aureus. J. Biomed. Mater. Res. 2000, 52, 662–668. [Google Scholar] [CrossRef]
  32. Deyneko, D.V.; Zheng, Y.; Barbaro, K.; Lebedev, V.n.; Aksenov, S.M.; Borovikova, E.Y.; Gafurov, M.R.; Fadeeva, I.V.; Lazoryak, B.I.; Giacomo, G.D.; et al. Dependence of antimicrobial properties on site-selective arrangement and concentration of bioactive Cu2+ ions in tricalcium phosphate. Ceram. Int. 2023, 49, 21308–21323. [Google Scholar] [CrossRef]
  33. Singh, B.; Dubey, A.; Kumar, S.; Saha, N.; Basu, B.; Gupta, R. In vitro biocompatibility and antimicrobial activity of wet chemically prepared Ca10−xAgx(PO4)6(OH)2 (0.0 ≤ x ≤ 0.5) hydroxyapatites. Mater. Sci. Eng. C 2011, 31, 1320–1329. [Google Scholar] [CrossRef]
  34. Drake, P.; Hazelwood, K. Exposure-related health effects of silver and silver compounds: A review. Ann. Occup. Hyg. 2005, 49, 575–585. [Google Scholar] [PubMed]
  35. Patil, S.B.; Jena, A.; Bhargava, P. Influence of Ethanol Amount During Washing on Deagglomeration of Co-Precipitated Calcined Nanocrystalline 3YSZ Powders. Int. J. Appl. Ceram. Technol. 2012, 10, E247–E257. [Google Scholar] [CrossRef]
  36. Gokcekaya, O.; Ueda, K.; Ogasawara, K.; Kanetaka, H.; Narushima, T. In vitro evaluation of Ag-containing calcium phosphates: Effectiveness of Ag-incorporated β-tricalcium phosphate. Mater. Sci. Eng. C 2017, 75, 926–933. [Google Scholar] [CrossRef] [PubMed]
  37. Natale, L.C.; Alania, Y.; Rodrigues, M.C.; Simões, A.; de Souza, D.n.; de Lima, E.; Arana-Chavez, V.E.; Hewer, T.L.R.; Hiers, R.; Esteban-Florez, F.L.; et al. Synthesis and characterization of silver phosphate/calcium phosphate mixed particles capable of silver nanoparticle formation by photoreduction. Mater. Sci. Eng. C 2017, 76, 464–471. [Google Scholar] [CrossRef]
  38. Fathi, M.; El Yacoubi, A.; El Youbi, M.; El Idrissi, B.C. New silver loaded calcium phosphate bone cement: Characterization and phase composition. Phosphorus Sulfur Silicon Relat. Elem. 2022, 197, 758–765. [Google Scholar] [CrossRef]
  39. Liu, H.; Li, P.; Tang, Z.; Liu, H.; Zhang, R.; Ge, J.; Yang, H.; Ni, X.; Lin, X.; Yang, L. Study on injectable silver-incorporated calcium phosphate composite with enhanced antibacterial and biomechanical properties for fighting bone cement-associated infections. Colloids Surf. B Biointerfaces 2023, 227, 113382. [Google Scholar] [CrossRef]
  40. Qureshi, F.; Nawaz, M.; Ansari, M.A.; Khan, F.A.; Berekaa, M.M.; Abubshait, S.A.; Al-Mutairi, R.; Paul, A.K.; Nissapatorn, V.; de Lourdes Pereira, M.; et al. Synthesis of M-Ag3PO4, (M = Se, Ag, Ta) Nanoparticles and Their Antibacterial and Cytotoxicity Study. Int. J. Mol. Sci. 2022, 23, 11403. [Google Scholar] [CrossRef]
  41. Piva, R.H.; Piva, D.H.; Pierri, J.; Montedo, O.R.K.; Morelli, M.R. Azeotropic distillation, ethanol washing, and freeze drying on coprecipitated gels for production of high surface area 3Y–TZP and 8YSZ powders: A comparative study. Ceram. Int. 2015, 41, 14148–14156. [Google Scholar] [CrossRef]
  42. Tortet, L.; Gavarri, J.R.; Nihoul, G. Study of Protonic Mobility in CaHPO4 · 2H2O (Brushite) and CaHPO4 (Monetite) by Infrared Spectroscopy and Neutron Scattering. J. Solid. State Chem. 1997, 132, 6–16. [Google Scholar] [CrossRef]
  43. Madsen, H.E.L. Influence of foreign metal ions on crystal growth and morphology of brushite (CaHPO4, 2H2O) and its transformation to octacalcium phosphate and apatite. J. Cryst. Growth 2008, 310, 2602–2612. [Google Scholar] [CrossRef]
  44. Batvandi, M.; Haghighatzadeh, A.; Mazinani, B. Synthesis of Ag3PO4 microstructures with morphology-dependent optical and photocatalytic behaviors. Appl. Phys. A 2020, 126, 571. [Google Scholar] [CrossRef]
  45. Botelho, G.; Sczancoski, J.; Andres, J.; Gracia, L.; Longo, E. Experimental and theoretical study on the structure, optical properties, and growth of metallic silver nanostructures in Ag3PO4. J. Phys. Chem. C 2015, 119, 6293–6306. [Google Scholar] [CrossRef]
  46. Alshaaer, M. Microstructural characteristics and long-term stability of wollastonite-based chemically bonded phosphate ceramics. Int. J. Appl. Ceram. Technol. 2020, 18, 319–331. [Google Scholar] [CrossRef]
  47. Alkhraisat, M.H.; Rueda, C.; Cabarcos, E.L. Strontium Ions Substitution in Brushite Crystals: The Role of Strontium Chloride. J. Funct. Biomater. 2011, 2, 31–38. [Google Scholar] [CrossRef]
  48. Alshaaer, M.; Issa, K.; Alanazi, A.; Mallouh, S.A.; Afify, A.S.; Moustapha, M.E.; Komnitsas, K. Gradual Replacement of Ca2+ with Mg2+ Ions in Brushite for the Production of Ca1−xMgxHPO4·nH2O Materials. Minerals 2021, 11, 284. [Google Scholar] [CrossRef]
  49. Hirsch, A.; Azuri, I.; Addadi, L.; Weiner, S.; Yang, K.; Curtarolo, S.; Kronik, L. Infrared Absorption Spectrum of Brushite from First Principles. Chem. Mater. 2014, 26, 2934–2942. [Google Scholar] [CrossRef]
  50. Alotibi, S.S.; Alshaaer, M. The Effect of Full-Scale Exchange of Ca2+ with Co2+ Ions on the Crystal Structure and Phase Composition of CaHPO4·2H2O. Crystals 2023, 13, 941. [Google Scholar] [CrossRef]
  51. Rajendran, K.K.C. Growth and Characterization of Calcium Hydrogen Phosphate Dihydrate Crystals from Single Dif-fusion Gel Technique. Cryst. Res. Technol. 2010, 45, 939–945. [Google Scholar] [CrossRef]
  52. Promnopas, S.; Promnopas, W.; Maisang, W.; Wannapop, S.; Thongtem, T.; Thongtem, S.; Wiranwetchayan, O. Synthesis of Ag3PO4/Ag4P2O7 by microwave-hydrothermal method for enhanced UV–visible photocatalytic performance. Sci. Rep. 2023, 13, 4742. [Google Scholar] [CrossRef] [PubMed]
  53. Alshaaer, M.; Cuypers, H.; Rahier, H.; Wastiels, j. Production of monetite-based Inorganic Phosphate Cement (M-IPC) using hydrothermal post curing (HTPC). Cem. Concr. Res. 2011, 41, 30–37. [Google Scholar] [CrossRef]
  54. Gashti, M.P.; Stir, M.; Jurg, H. Growth of strontium hydrogen phosphate/gelatin composites: A biomimetic approach. New J. Chem. 2016, 40, 5495–5500. [Google Scholar] [CrossRef]
  55. Alshaaer, M.; Cuypers, H.; Mosselmans, G.; Rahier, H.; Wastiels, J. Evaluation of a low temperature hardening Inorganic Phosphate Cement for high-temperature applications. Cem. Concr. Res. 2011, 41, 38–45. [Google Scholar] [CrossRef]
  56. Frost, R.L.; Palmer, S.J. Thermal stability of the ‘cave’ mineral brushite CaHPO4·2H2O—Mechanism of formation and decomposition. Thermochim. Acta 2011, 521, 14–17. [Google Scholar] [CrossRef]
  57. Martín-Gómez, A.; Navío, J.; Jaramillo-Páez, C.; Sánchez-Cid, P.; Hidalgo, M. Hybrid ZnO/Ag3PO4 photocatalysts, with low and high phosphate molar percentages. J. Photochem. Photobiol. A Chem. 2020, 388, 112196. [Google Scholar] [CrossRef]
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Figure 1. Experimental procedure for the synthesis of the Ca1−xAgxHPO4·nH2O compounds.
Figure 1. Experimental procedure for the synthesis of the Ca1−xAgxHPO4·nH2O compounds.
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Figure 2. X-ray diffraction patterns of the Ca1−xAgxHPO4·nH2O compounds produced under the conditions shown in Table 1 and Figure 1.
Figure 2. X-ray diffraction patterns of the Ca1−xAgxHPO4·nH2O compounds produced under the conditions shown in Table 1 and Figure 1.
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Figure 3. Phase composition of the produced compounds compared with the Ag molar fraction in the starting solutions.
Figure 3. Phase composition of the produced compounds compared with the Ag molar fraction in the starting solutions.
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Figure 4. SEM images of the Ca1−xAgxHPO4·nH2O compounds (labeled using the compound names shown in Table 1): (A) BAg0, (B) BAg4, (C) BAg5, (D) BAg6, (E) BAg8, and (F) BAg10. Point 1, CaHPO4·2H2O crystals; point 2, AgPO4 crystals.
Figure 4. SEM images of the Ca1−xAgxHPO4·nH2O compounds (labeled using the compound names shown in Table 1): (A) BAg0, (B) BAg4, (C) BAg5, (D) BAg6, (E) BAg8, and (F) BAg10. Point 1, CaHPO4·2H2O crystals; point 2, AgPO4 crystals.
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Figure 5. FTIR spectrum of the CaHPO4·2H2O and Ag3PO4 compounds.
Figure 5. FTIR spectrum of the CaHPO4·2H2O and Ag3PO4 compounds.
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Figure 6. XPS spectra of the CaHPO4·2H2O and Ag3PO4 compounds.
Figure 6. XPS spectra of the CaHPO4·2H2O and Ag3PO4 compounds.
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Figure 7. XPS analysis of the chemical state of the (A) Ca 2s, (B) P 2s, and (C) Ag 2p orbitals in the Ca1−xAgxHPO4·nH2O compounds.
Figure 7. XPS analysis of the chemical state of the (A) Ca 2s, (B) P 2s, and (C) Ag 2p orbitals in the Ca1−xAgxHPO4·nH2O compounds.
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Figure 8. TG curves of the CaHPO4·2H2O and Ag3PO4 compounds (product names BAg0–BAg10).
Figure 8. TG curves of the CaHPO4·2H2O and Ag3PO4 compounds (product names BAg0–BAg10).
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Figure 9. Differential TGA of the Ca1−xAgxHPO4·nH2O compounds: (A) BAg0, (B) BAg2, (C) BAg4, (D) BAg5, (E) BAg6, (F) BAg8, and (G) BAg10.
Figure 9. Differential TGA of the Ca1−xAgxHPO4·nH2O compounds: (A) BAg0, (B) BAg2, (C) BAg4, (D) BAg5, (E) BAg6, (F) BAg8, and (G) BAg10.
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Table 1. Molar proportions of (NH4)2HPO4, Ca(NO3)2·4H2O, and AgNO3, in addition to the Ag/Ca molar ratios applied for the synthesis of Ca1−xAgxHPO4·nH2O compounds.
Table 1. Molar proportions of (NH4)2HPO4, Ca(NO3)2·4H2O, and AgNO3, in addition to the Ag/Ca molar ratios applied for the synthesis of Ca1−xAgxHPO4·nH2O compounds.
ID(NH4)2HPO4Ca(NO3)2·4H2OAgNO3·6H2OAg/Ca Molar Ratio
BAg01100
BAg210.80.20.25
BAg410.60.40.67
BAg510.50.51.0
BAg610.40.61.5
BAg810.20.84
BAg10101-
Table 2. The phase composition and parameters of the Ca1−xAgxHPO4·nH2O unit cell, as determined by XRD scanning (Rietveld refinement, MATCH! software analysis). * Scherrer equation.
Table 2. The phase composition and parameters of the Ca1−xAgxHPO4·nH2O unit cell, as determined by XRD scanning (Rietveld refinement, MATCH! software analysis). * Scherrer equation.
Phase
Composition		% wt.Crystal
Structure		a (Å)b
(Å)		c (Å)ß°Unit Cell Volume (Å3)Crystallite Size (Å) *
BAg0CaHPO4·2H2O100Monoclinic5.8215.226.27116.41496.6553
BAg2CaHPO4·2H2O87.1Monoclinic5.8115.196.24116.41493.4350
Ag3PO412.9Cubic6.006.006.0090216.4321
BAg4CaHPO4·2H2O80.9Monoclinic5.8115.186.24116.43492.9165
Ag3PO419.1Cubic6.016.016.016.01217.0333
BAg5CaHPO4·2H2O67Monoclinic5.8115.216.26116.41495.6556
Ag3PO433Cubic6.016.016.016.01217.0334
BAg6CaHPO4·2H2O54.9Monoclinic5.8115.216.26116.41495.6570
Ag3PO445.1Cubic6.006.006.0090216.0030
BAg8CaHPO4·2H2O36.3Monoclinic5.8215.226.27116.41496.65130
Ag3PO463.7Cubic6.006.006.0090216.0018
BAg10Ag3PO4100Cubic6.006.006.006.00216.0040
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Abdulaziz, F.; Issa, K.; Alyami, M.; Alotibi, S.; Alanazi, A.A.; Taha, T.A.M.; Saad, A.M.E.; Hammouda, G.A.; Hamad, N.; Alshaaer, M. Preparation and Characterization of Mono- and Biphasic Ca1−xAgxHPO4·nH2O Compounds for Biomedical Applications. Biomimetics 2023, 8, 547. https://doi.org/10.3390/biomimetics8070547

AMA Style

Abdulaziz F, Issa K, Alyami M, Alotibi S, Alanazi AA, Taha TAM, Saad AME, Hammouda GA, Hamad N, Alshaaer M. Preparation and Characterization of Mono- and Biphasic Ca1−xAgxHPO4·nH2O Compounds for Biomedical Applications. Biomimetics. 2023; 8(7):547. https://doi.org/10.3390/biomimetics8070547

Chicago/Turabian Style

Abdulaziz, Fahad, Khalil Issa, Mohammed Alyami, Satam Alotibi, Abdulaziz A. Alanazi, Taha Abdel Mohaymen Taha, Asma M. E. Saad, Gehan A. Hammouda, Nagat Hamad, and Mazen Alshaaer. 2023. "Preparation and Characterization of Mono- and Biphasic Ca1−xAgxHPO4·nH2O Compounds for Biomedical Applications" Biomimetics 8, no. 7: 547. https://doi.org/10.3390/biomimetics8070547

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