Ode Coyote wrote: > ## It's doubtful that there are many, if any 'free' ions in ionic CS > after several hours.
It is actually instanteous, you cannot have a cation without a cation. So as soon as you have an Ag+, it will associate with an OH forming dissolved silver hydroxide. Over time 50% of this will convert to silver oxide. > > 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] The only salt would be some silver carbonate formed from any dissolved CO2 in the water, or any formed from trace amounts of other acids that may be in the distilled water. > 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. Well half the ionic silver in EIS is silver oxide, and there is a good bit of evidence that it is pretty effective against pathogens. > > 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. Silver hydroxide is very unstable when you dry it, releasing silver metal as you indicate. When in solution it is unstable as well, spontaneouly converting to silver oxide. However in solution silver oxide is unstable as well spontaneously converting to silver hydroxide, so although silver oxide and silver hydroxide are both unstable alone, since they convert to each other, the two taken together are fairly stable when in solution. > > > There is certainly some sort of threshold reached at around 25-30 uS > conductivity and electrical properties start to drift 'off line' a little Since the solubility limit of silver oxide and silver hydroxide are both 13 ppm, the two together have a limit of 26 ppm. > > 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] Most likely much of these batches have a high silver carbonate. Silver carbonate is highly unstable and thus very prone to change from any outside influences. > > > Perhaps past that 25-30 uS solubility limit other configurations of oxides > start forming??? [Silver Peroxides and Tetroxides maybe?] That is another possibility that I have not previously considered. Marshall > > > 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 > > > > > >No virus found in this incoming message. > >Checked by AVG Anti-Virus. > >Version: 7.1.371 / Virus Database: 267.13.13 - Release Date: 12/13/2005 > > -- > No virus found in this outgoing message. > Checked by AVG Anti-Virus. > Version: 7.1.371 / Virus Database: 267.13.13 - Release Date: 12/14/2005 > > -- > The Silver List is a moderated forum for discussing Colloidal Silver. > > Instructions for unsubscribing are posted at: http://silverlist.org > > To post, address your message to: [email protected] > > Address Off-Topic messages to: [email protected] > > The Silver List and Off Topic List archives are currently down... > > List maintainer: Mike Devour <[email protected]> >
