Years ago, we became interested in the properties of properly made ionic silver dispersions. The initial samples we received effectively eradicated the mould, reduced odours in clothes and shoes, and, in general, eliminated microbes. However, we quickly observed that the results varied significantly between samples produced using various production methods.
We were curious to learn which parameters were important in determining the effectiveness of the ionic silver dispersion and how the production process methodology affected the quality and consequent effectiveness of the end product. As a starting point, we had numerous internet resources at our disposal. It fast became evident that a lot of presented data is contradictory and even self-conflicting.
We performed several experiments to determine which statements are factual and which are just conjectures. We aimed to determine which production methods end up with usable dispersion and which do not. After much experimenting, we understood which parameters are essential for producing very high concentrations of silver ion cations (Ag+) and which are only marginally relevant. As it turns out, the purity and temperature of the water, the shape, surface and size of electrodes and the geometry of fluid flow are all important contributing factors in the production of saturated ionic silver, containing a high content of silver ions.
Additionally, appropriate laboratory and measurement equipment must be used to employ a proper electrical signal and maintain precise control of the dispersion production process to prevent contamination of dispersion or its agglomeration. When sufficiently exact measurements of several physical parameters are made continuously, the dispersion saturation curve in the time domain can be observed. It is then possible to dynamically adjust the processing rate and eventually stop it just before the agglomeration point. Reaching high concentration values of up to 20 ppm of silver particles (mostly Ag+) is achievable even with some conventional equipment if appropriate production methodology is observed. However, in most cases of standard ionic silver production equipment, making such saturated dispersions comes at the expense of significantly longer processing time.
It soon became apparent that appropriate methodology and hardware would have to be developed to produce high-quality ionic silver dispersion in time as short as possible. Preliminary results during our ongoing research and development in that direction yielded dispersions with an extremely high concentration of silver particles of up to 20 ppm.
Even considering inaccuracies and non-linearity of the measuring process and equipment, some of the observed physical properties of saturated dispersion provide circumstantial evidence that such high saturation is possible. For example, it can be observed that high-concentration dispersions are sometimes so saturated that although they appear stable, sometimes all it takes is some external stimulus to destabilise them to the point of agglomeration. For example, brief exposure of such saturated ionic silver dispersions to sunlight or a change in temperature of just 2-3 °C often causes sudden agglomeration. Agglomeration usually happens momentarily, and the very moment it happens, it renders produced dispersion inadequate for any practical medicinal purposes.
By carefully observing all relevant parameters and with the developed methodology, we could reliably produce stable, saturated ionic silver dispersions. Based on gained experience, we are considering the development of manufacturing equipment capable of comparatively faster production of high-quality, saturated ionic silver dispersions with a high content of silver cations (Ag+).
Many simple experiments we performed with different yeasts and moulds confirmed that, indeed almost linear relationship exists between saturation level of dispersion and observed bioactive effects (death of yeast and mould samples). Saturated ionic silver dispersion virtually always yielded better results than less saturated dispersions.
It also became apparent that saturated dispersions are more light-sensitive than low-saturation dispersions. Storing them in dark glass containers is best to postpone eventual agglomeration and prolong shelf-life. Saturated ionic silver dispersions are also increasingly unstable and tend to agglomerate with rising temperatures, so storing them in cool places is recommended. Given the fact that the density of water is at its maximum at ~4°C, one could assume that as the storage temperature nears the region of highest density, the potential for agglomeration of the dispersion would rise. If such an assumption is verified with further experimental observations, it would mean that saturated ionic silver dispersions have to be stored at temperatures higher than 10 °C because, at that point, the density of water starts to drop, thus reducing the probability of agglomeration significantly. That puts the best storage temperature in the 10 – 20 °C range. Another solution for storage in an unfavourable temperature environment would be to adjust the saturation of the dispersion to account for the storage temperature range with the consequent reduction in therapeutic effectiveness.