Chemical kinetics of silver diammine fluoride in demineralization and remineralization solutions—an in vitro study
M. Kaur
P. Anderson
S. Shahid
F. S. L. Wong- Dental Physical Sciences Unit, Centre for Oral Bioengineering, Institute of Dentistry, Faculty of Medicine and Dentistry, Queen Mary University of London, London, United Kingdom
Introduction: Silver Diammine Fluoride (SDF) is a clinical minimal intervention to manage dentin caries. Its chemistry in demineralization conditions has been investigated widely, but far less in remineralization conditions. The aim was to investigate and compare the chemical reactions when SDF is added to remineralization and demineralization solutions.
Methods: 0.01 ml SDF (Riva Star) was added to deionized water (DW); demineralization (DS = pH4) and remineralization (RS = pH7.0) solutions. The time sequence of concentrations of NH4+, F−, and Ag+ were measured using ion selective electrodes (ISEs) every 2 min. The pH was also measured. Precipitates were characterized using x-ray Diffraction (XRD) and, 31P and 19F nuclear magnetic resonance spectroscopy (NMR).
Results: The concentrations of NH4+ and Ag+ showed decreasing trends in DW (−0.12 and −0.08 mM/h respectively), and in DS (−1.06 and −0.5 mM/h respectively); with corresponding increase in F− concentration (0.04 and 0.7 mM/h respectively). However, in RS, NH4+ concentration showed little change (0.001 mM/h), and Ag+ and F− concentrations were negligible. XRD results showed that precipitates (in RS only) contained AgCl, and metallic Ag. NMR showed that fluorapatite/carbonated fluorapatite (FAP/CFAP) were formed. The pH increased after SDF addition in all three solutions.
Discussion: SDF dissolved to release NH4+, F− and Ag + . In DW and DS, NH4+ combined with Ag+ to form diamminesilver, causing an increase of F− and pH. In RS, F− reacted with Ca2+ and (PO)43− to form FAP/CFAP, and Ag+ reacted with Cl− to form AgCl/Ag. These suggests why SDF is effective in managing dentin caries.
Introduction
Demineralization and remineralization studies serve as crucial tools in investigating the efficacy of therapeutic interventions on dental substrates such as hydroxyapatite (HA) discs, enamel, or dentin. These investigations simulate the cariogenic challenges encountered in the oral cavity and provide valuable insights into potential treatments for caries prevention and management.
While various models have been employed in cariology research to replicate the caries process, chemical models offer distinct advantages in terms of efficiency, cost-effectiveness, and reproducibility. Among these models, chemical approaches utilizing acid or acid buffers to mimic demineralization and remineralization mechanisms have gained prominence. Notably, Yu et al. (1) observed that 62% of mechanistic studies utilize simple mineralization models, while 38% employ pH cycling models.
Silver diammine fluoride (SDF) is a colorless liquid and is a promising agent for dentin caries management. Its application involves painting it onto carious lesions for a brief duration. Therefore, understanding the chemical interaction of SDF in both acidic and remineralization environments is important.
Ion-selective electrodes (ISEs) are an analytical tool for determining the concentration of specific free ions in solution. In dental research, ISEs have a proven efficacy in various studies. For example, Huang et al. (2) demonstrated that calcium ISEs is a reliable method for real-time quantification of mineral loss during demineralization using a hydroxyapatite model system.
While numerous investigations have explored the effect of SDF on HA during demineralization, but there are noticeably fewer investigating its impact during remineralization (3). The aim of this study was to compare the chemical kinetics of SDF following dissolution in water, demineralization solutions, and in remineralization solutions. The emphasis was to investigate the chemical reactions in real-time of following addition of SDF into de- and re-mineralization solutions rather than its reactions directly on tooth tissues.
Materials and methods
Commercially available SDF (Ag(NH4)2F) (Riva Star, SDI, Australia) was used which has a concentration of 3.16M. Demineralization solutions of buffered 0.1M acetic acid at pH4.0 were prepared. Remineralization solutions comprising of 0.222 g/L CaCl2, 0.163 g/L KH2PO4, 8.7 g/L NaCl at pH7 were also prepared (4). 0.01 ml of SDF was added to 50 ml of: deionized water, demineralization solution, and remineralization solutions, thus resulting in a concentration of 0.632 mM of SDF in each. ISEs (Nico2000, UK) were used to measure initial, and also to continually monitor NH4+, Ag+ and F− concentrations at intervals of 2 min (2) for a period of 2 h. All the experiments were carried out at 37 °C (repeated three times). The pH of the solution was measured before addition of SDF, and at the end of the experiment using a calibrated pH meter (Mettler Toledo portable pH meter).
Any precipitates were collected and dried in an incubator and characterized using x-ray diffraction (XRD), and 31P and 19F solid state Magic Angle Spinning nuclear magnetic resonance (MAS-NMR) spectroscopy. XRD spectra were collected using a x-ray powder diffractometer (PANalytical CubiX3, UK). The theta-2theta scan measurements were carried out in standard reflection mode, using Cu K radiation, with sample holders spinning on the stage during the scan. 31P MAS-NMR was conducted using a 14.1 Tesla spectrometer (600 MHz Bruker, UK) at a Larmor frequency of 242.94 MHz. 19F MAS NMR analysis was conducted using a 14.1 Tesla spectrometer at a Larmor frequency of 564.658 MHz. All spectra were obtained with a 2.5 mm probe under spinning conditions of 20 kHz.
Results
The ISE results of the real-time changes of free NH4+, F− and Ag+ in the water, demineralization and remineralization solutions are shown in Figure 1. The trends after initial values were similar in deionized water and the demineralization solutions, i.e., decreasing concentration with time for NH4+, and Ag+, but increasing for F−. Whereas, for remineralization solution, after initial solubilization, following addition of SDF, the trend was no change in NH4+ and very low with virtually no change in Ag+ and F− concentrations.
Figure 1. Changes in concentration of (A) NH4+, (B) F− and (C) Ag+ ions on addition of 0.01 ml SDF (3.16 M) to 50 ml deionized water, demineralization solution at pH4, and remineralization solution at pH7 in a time series. *Please note that the concentration of Ag+ ions in the remineralization solution was below the lowest detection limit of ISE as a result of immediate precipitation.
Ammonium ions
Following addition of SDF into deionized water, the initial NH4+ concentration increased immediately to 1.2 mM, and then subsequently decreased linearly by 0.12 mM/h. Following addition of SDF into demineralization solution the NH4+ concentration increased rapidly to 9.0 mM, and then subsequently decreased linearly by 1.06 mM/h. However, following addition of SDF into remineralization solution, the initial NH4+ concentration increased to 1.0 mM but subsequently did not change much over time.
Fluoride ions
The initial F− concentration in deionized water was 0.6 mM on addition of SDF, and then increased by 0.04 mM/h. The initial F− in demineralizing solution was 6 mM on addition of SDF, and then increased by 0.7 mM/h. In the remineralization solution, the F− concentration was between 0.025 and 0.045 mM on addition of SDF, and did not change subsequently.
Silver ions
The initial Ag+ concentration in deionized water was 0.6 mM on addition SDF, and then decreased by 0.08 mM/h. Following addition of SDF in demineralization solution, the concentration of Ag+ was 4.5 mM, and then decreased by 0.5 mM/h. Whereas, following addition of SDF to the remineralization solution, the Ag+ concentration did not rise above the minimum detection limit of the ISE electrode.
Precipitation of solids
No precipitate was seen when SDF was added to either deionized water or demineralization solution. However, when SDF was added to remineralization solution, there was a rapid change in color from clear to white and a white precipitate was formed. XRD pattern of the precipitate (Figure 2) showed peaks at 27.9°, 32.3°, 46.3°, 54.9° and 57.6° that could be assigned to silver chloride (AgCl, Reference code-04-007-3906). The small peaks at 38.3°, 44.3° and 64.4° are consistent with the formation of metallic silver (Reference code: 04-006-1881). The 19F MAS-NMR spectrum (Figure 3A) shows a peak at −102 ppm suggesting the formation of fluorapatite (FAP); and the peak at −88 ppm suggesting the formation of carbonated fluorapatite (CFAP) (5, 6). The 31P MAS-NMR spectrum peak at 2.7 ppm indicates the presence of calcium hydroxyapatite (Figure 3B).
Figure 2. X-ray diffraction results obtained from the precipitate formed as a result of interaction of SDF with remineralization solution. The sharp diffraction lines and the pattern seen above indicate AgCl crystal (Reference Code: 04-007-3906) and small amount of metallic silver (Reference code: 04-006-1881).
Figure 3. (A) 19F MAS-NMR, and (B) 31P MAS-NMR spectra of the precipitate formed as a result of interaction of SDF with remineralisation solution. The Asterix denote the sidebands. (A) The peak at −102.4 ppm indicates the formation of fluorapatite and at −88.1 ppm, carbonated complex. (B) The peak at 2.67 ppm signifies formation of apatite.
pH
The change of pH in the solutions is presented in Table 1. The pH increased after the addition of SDF in all solutions. The greatest increase in pH was in deionized water and the least was in demineralization solution.
Table 1. Change of pH in solutions on interaction with SDF before and after experimental period.
Discussion
The complete dissolution of SDF in any of the solutions would result in concentrations of 1.2 mM NH4+, 0.6 mM F−, and 0.6 mM Ag+ calculated from the stoichiometry and concentration and volumes of SDF used, and assuming complete dissociation. SDF is known to be soluble in water (7). The ISE results in deionized water showed that it completely dissociated to give rise to around 1.2 mM NH4+, and 0.6 mM Ag+ and F− ions after adding 0.01 ml of 3.16 mM SDF in 50 ml of water. The subsequent small decrease of NH4+ and Ag+ in the following 2 h indicated that an aqueous ammonia-silver ion complex, likely to be diamminesilver [Ag(NH)3)2+] (8, 9), leading to a corresponding increase in F− in the solution, which might be the cause for the pH increase.
This situation was similar for SDF dissolved in demineralization solution as the gradients of the decrease of NH4+ and Ag+ concentrations, and the corresponding gradient of increase for F−, were similar to that in deionized water. As Ag(NH)3)2+ is a stable aqueous species, and its ammonia-silver covalent bonds prevent the photo-reduction of silver, no precipitate was formed and the solution remained clear.
However, when SDF was dissolved in remineralization solution, the NH4+ concentration remained constant at about the stoichiometric value, but the concentrations of F− and Ag+ were both very low. This indicated that these ions were taken up immediately to form the precipitate. The XRD and NMR analyses (Figures 2, 3) showed that these precipitates contained a mixture of AgCl, metallic silver, and fluorapatites, which are all insoluble compounds. As the remineralization solution contained CaCl2, KH2PO4, and NaCl, this suggests that the dissociated Ag+ reacted rapidly with the Cl− to form AgCl as a white precipitate, thus reducing the Ag+ concentration in the solution to a negligible amount. Subsequently, when the AgCl precipitate was exposed to light, a small amount was then photo-reduced to metallic silver, which was also seen in the XRD analysis. The F− would react immediately with Ca2+ to form CaF2 (10, 11), another white precipitate, which in the presence of phosphate, would form insoluble fluorapatite, (and therefore was not seen in the NMR spectra). Thus, the F− concentration was also very little (Figure 1C).
This in vitro study, investigating the kinetics of the chemical reactions of SDF in demineralization and remineralization conditions can be used to predict the effects of SDF in the oral environment. As saliva contains Ca2+, (PO4)3− and Cl−, these ions would also react with SDF to form insoluble FAP/CFAP and AgCl. These precipitates would then be retained for example in exposed dentinal tubules and not be washed away. The formation of the FAP would render the dentin to be less susceptible to acid demineralization (12–14). AgCl is photo-reduced to metallic Ag (giving the black appearance seen when SDF is used in dentin treatments) which will hinder bacterial growth and degradation of dentin collagen (15, 16). As the components of SDF also increase the pH in the oral environment, this will further reduce the damage caused by acid challenges. Furthermore, as the AgCl and FAP/CFAP precipitate within the dental tubules, these precipitated compounds may occlude the tubular lumens and minimize pain by reducing direct communication of the pulp with external stimuli. However, in enamel, these precipitates could only be retained in demineralized porous lesions, and not on sound smooth surface. Therefore, clinically, the SDF protective benefit against acidic challenge for enamel (17) is reduced compared to dentin (13). Other studies [e.g., (14)] also demonstrated that the use of SDF/NaF had a remineralizing effect on a dentin surface under acid challenge.
Clearly, this in vitro study is limited if compared to the complexity of the in vivo oral environment, where there are a multitude of other charged species (ions and proteins) in saliva, all of which may partially interact with the ionic constituents of SDF. In the oral environment both demineralization and remineralization occur within the complex biological fluid that is saliva (18). Enamel biodemineralization (19, 20) has been proposed as the process by which tooth mineral is lost within a chemically interacting environment. Nevertheless, this in vitro study does demonstrate that complexes are formed when SDF is dissolved, especially when other ions including Cl− are present, which is a major component of saliva.
Conclusion
In remineralizing solutions which contain chloride ions (and therefore likely to be the case in saliva), SDF reacts rapidly with calcium, phosphate, and chloride ions, leading to the formation of fluorapatite, carbonated fluorapatite, and silver chloride precipitates. The silver chloride precipitate will undergo photo-reduction, resulting in black discoloration. These precipitates, which would be retained inside dentinal tubes, with the increases of pH, suggests why SDF is beneficial in clinical treatments for dentin caries.
Data availability statement
The original contributions presented in the study are included in the article/Supplementary Material, further inquiries can be directed to the corresponding author.
Author contributions
MK: Conceptualization, Data curation, Methodology, Writing – original draft, Writing – review & editing. PA: Conceptualization, Formal Analysis, Investigation, Methodology, Project administration, Writing – review & editing. SS: Conceptualization, Methodology, Supervision, Writing – review & editing. FW: Conceptualization, Data curation, Investigation, Methodology, Supervision, Writing – original draft, Writing – review & editing.
Funding
The author(s) declare that no financial support was received for the research, authorship, and/or publication of this article.
Acknowledgment
We wish to thank Dr. Harold Toms and Dr. Nasima Kanwal, both the facility managers of cross faculty NMR Centre, and Dr. Natalia Karpukhina for her help in NMR analysis and interpretation, at Queen Mary University of London.
Conflict of interest
The authors declare that the research was conducted in the absence of any commercial or financial relationships that could be construed as a potential conflict of interest.
Publisher's note
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Keywords: SDF, demineralization, remineralization, XRD, NMR, AgCl
Citation: Kaur M, Anderson P, Shahid S and Wong FSL (2024) Chemical kinetics of silver diammine fluoride in demineralization and remineralization solutions—an in vitro study. Front. Oral. Health 5:1374333. doi: 10.3389/froh.2024.1374333
Received: 21 January 2024; Accepted: 8 April 2024;
Published: 19 April 2024.
Edited by:
Raman Bedi, King's College London, United KingdomReviewed by:
Sonia Groisman, State University of Rio de Janeiro, BrazilAshwin Jawdekar, Bharati Vidyapeeth Deemed to be University Dental College and Hospital, India
© 2024 Kaur, Anderson, Shahid and Wong. This is an open-access article distributed under the terms of the Creative Commons Attribution License (CC BY). The use, distribution or reproduction in other forums is permitted, provided the original author(s) and the copyright owner(s) are credited and that the original publication in this journal is cited, in accordance with accepted academic practice. No use, distribution or reproduction is permitted which does not comply with these terms.
*Correspondence: F. S. L. Wong f.s.l.wong@qmul.ac.uk
Abbreviations Ag+, silver ion; AgCl, silver chloride; Ca2+, calcium ion; CaF2, calcium fluoride; Cl−, chloride ion; DS, demineralizing solution; DW, de-ionized water; F−, fluoride ion; FAP, fluorapatite; g, gram; h, hour; HAp, hydroxyapatite; ISE, ion-selective electrodes; kHz, kilo hertz; L, litre; mM, millimolar; M, Mol; MAS-NMR, magic angle spinning nuclear magnetic resonance spectroscopy; ml, milli litre; mm, millimetre; MHz, mega hertz; NH4+, ammonium ion; RM, remineralizing solution; XRD, x-ray diffraction.