## It's doubtful that there are many, if any 'free' ions in ionic CS
after several hours.
There may be some surviving the stabilization period if they oriented
themselves with the oxygen component of water but most will have found
their anions and formed silver oxide and silver hydroxide which allows ions
to be dissolved in water and stay stable.
Please correct me if I'm off base here....[not a chemist]
I don't think these are metallic "salts" [Certainly not a metallic halide
salt like silver chloride]
I'm not sure of the effectiveness of silver oxides but there are several
different configurations possible each having different solubility limits
and apparently silver tetroxide is an effective agent.
Silver hydroxide is very unstable and will release metallic silver,
highly reactive free ions or oxidize when its environment changes depending
on how the environment changed.
There is certainly some sort of threshold reached at around 25-30 uS
conductivity and electrical properties start to drift 'off line' a little
past that point, but it is possible to exceed 30 uS and have stable CS/EIS.
I've gone as high as 79 uS and produced colorless batches that stayed
colorless and so have others.
[Very dense TE], but contaminate that just a little and all sorts of
changes happen. [Murky purple or red]
Perhaps past that 25-30 uS solubility limit other configurations of oxides
start forming??? [Silver Peroxides and Tetroxides maybe?]
Ode
At 10:18 AM 12/14/2005 -0700, you wrote:
Why do the silver ions in a dissolved salt have the possibility of causing
Argyria and the free ions in a mixture of colloidal and ionic silver not
do that?
Jim
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