Yes, I was speaking in terms of unassociated silver ions made by the electro CS process where they come in contact with unassociated pure oxygen created by the same process. Wham! Near Instant oxides. [And some unstable hydroxides?]
Fortunately, there are many more silver ions made than oxygen anions. ode At 10:27 AM 11/18/2003 -0500, you wrote: >Ode Coyote wrote: > >> Ionic silver reacts with oxygen quite readily. >> Silver ions have a + charge and oxygen has a - charge >> That's why one electrode turns black. > >Yes and no. Ionic silver that has no anion associated with it is much more >active than other forms of silver, and will quickly oxidize as you point out. >But silver ions that are part of a compound disolved in water, do not react with >oxygen easily. For instance if you bubble air through silver nitrate, it will >remain silver nitrate, it will not become silver oxide. > >> >> And it happens so fast, so close to that electrode, that most of the >> oxides never leave the electrode. >> If you up the current, oxygen and ions can be produced so fast that the >> reaction time is overcome and the oxides form in the water resulting in >> grey to blackish CS which clears up as the heavy and larger particles of >> oxides drop out. >> >> Now, If I have this right, silver is strange in that it will pick up >> oxygen when it is heated to almost vaporization and release that oxygen >> again when it cools. > >I am not aware of that. I do know it will release it when exposed to certain >wavelengths of light, once again part of the photographic process. > >Marshall > >> >> >> Ode >> >> At 02:18 PM 11/17/2003 -0500, you wrote: >> >Reid Harvey wrote: >> > >> >> Marshall, >> >> I've gotten to thinking: if silver chloride disolves little by little, >> >> tiny amounts getting into the filtrate, isn't it likely that the same >> >> would be true for the silver oxides? After all, aren't the oxides of >> >> silver even more soluble than is the chloride. >> > >> >Silver oxide has a solubility of 0.0013 g/100 cc in cold water and 0.0053 >> >g/100cc in hot water. >> > >> >Silver peroxide is totally insoluble. >> > >> >> >> >> >> >> I'm asking because the current, widely used practice is to satrurate >> >> ceramic purifiers with concentrated CS, which then goes through >> >> reactions in drying, ending up with the oxides. >> > >> >I would be surprised if it ends up as an oxide, it is usually rather hard to >> >get silver to react with oxygen. It should stay a metal if not exposed to >> >sulfur compounds, or nitrates. >> > >> >> I guess what I'm asking >> >> is: how could this be a problem for silver chloride and not for silver >> >> oxides? And if a 'precendent' of sorts has been set, by allowing the >> >> oxides, why not the chloride? Or is my chemistry off the mark? >> >> >> > >> >I think you are off the mark. But I did have a thought over the weekend. >> >Can you obtain copper power (or dust) very fine, like a flour, and mix that >> >in when you make them? If so the you could run silver nitrate through >> >filter that has copper particles in it, and the silver will plate the >> >copper, as long as the copper does not become oxidized.. So you would end up >> >with copper particles, with a silver coating a few atoms thick on the >> >outside. That would give you a lot of silver surface area, but with very >> >little silver being required overall. >> > >> >Marshall >> > >> >> Reid >> >> >> >> -- >> >> The silver-list is a moderated forum for discussion of colloidal silver. >> >> >> >> Instructions for unsubscribing may be found at: http://silverlist.org >> >> >> >> To post, address your message to: [email protected] >> >> >> >> Silver-list archive: http://escribe.com/health/thesilverlist/index.html >> >> >> >> List maintainer: Mike Devour <[email protected]> >> > >> > > >
