>> >> I've never seen a reaction of ions with salt that amounted to much, if >> anything...maybe a slightly blue tinge in direct sunlight? >> Even adding both peroxide and salt to it doesn't make it go milky. > >Hold it under a bright light, and you should see a slight blue white tinge. It >should be comparable to adding several drops of milk to a glass of water.
## Did see a very slight blue tinge. Would have to compare that to adding salt to plain water. > >> >> >> No reaction with salt and peroxide mix. >> >> Mega reaction with salt, peroxide and dissolved silver oxide mix. >> Are you sure peroxide produces ions? ..or is it just that peroxide >> dissolves oxides into it where plain water doesn't. >> >> OK, another test. >> Batch run and evaporated to 6 oz at 86 uS, deep yellow brown, treated with >> 4 drops of peroxide to clear it...almost a month ago. Now colorless with >> extremely dense and fine textured TE, somewhat milky looking in direct >> light and tends to take on any color near it..especially bark brown making >> it look a bit black...looks clear when looking through it at a diffused light. >> This stuff is all over the place uS wise, Started at 86.6 uS before >> adding peroxide, the other day it was, what, 79 uS?..I posted it and forgot >> [lower, anyhow] and today its 111.2 uS. >> What the heck? >> >> Pull sample...Add a pinch of salt, stir to dissolve completely...no >> reaction. Before and after appear to be identical. >> > >That implies that all the silver is now silver particles. Is all the H2O2 gone? >If so, maybe the end point of the reversible reaction with silver favors the metal >as the peroxide level decreases to 0. ## There was a LOT of H2O2 Basic flaw in procedure is not measuring amounts of anything. But then , I was going for gross reactions, not nuances. > >Was it sitting in the light? If so then maybe after adding H2O2 you ended up with >a combination of silver particles and silver oxide, and then exposure to light >caused the silver oxide to photoexpose producing 100% silver metal. ## Now that's a funny thing. About an hour after I sent the post off, all but one container turned a dense bluish black ....including... the parent 86.6/111.2 uS batch that I had added nothing to. All I had done to that was pour some out into a beaker, dipped the PWT in and poured it back into the container. It's possible that traces of iron and calcium [and who knows what] were in the beaker and all the other containers, as water spots, from washing them. [I didn't "see" any water spots...but.] Since I as 'done', I didn't keep track of what container was what. It was all done near a window, but no direct sun. That batch had been stored in clear glass near a window, no direct sun, for almost a month. It had been exposed to direct sun early on, several times, for a few minutes though. I dumped peroxide into the parent batch..about 50/50.. to no avail. No change. Then I dumped it all into the flower bed. Ode > >Marshall > >> >> I don't have any currently colored CS to add salt to and very rarely wind >> up with any. Maybe I'll crank up the current, nix the stirrers and make >> some on purpose soon. >> >> Maybe strings of equations aren't including all the hidden factors, we >> don't really know what they all are...and they differ from person to person >> / generator to generator / process to process. >> >> Maybe the H2O2.com equation is correct [seems to me that it is] and we're >> watching something else entirely. >> >> That's about as far as the seat of my pants can figure. ["poot"] >> >> ode >> >> At 06:59 PM 8/24/2004 -0400, you wrote: >> >Re: CS>Adding peroxide to CS >> >From: Ode Coyote >> >Date: Tue, 24 Aug 2004 11:56:25 >> >http://escribe.com/health/thesilverlist/m72856.html >> > >> > > X-Sender: odecoyo...@mail.alltel.net (Unverified) >> > > X-Mailer: QUALCOMM Windows Eudora Pro Version 3.0.3 (32) >> > > Date: Tue, 24 Aug 2004 13:50:34 -0400 >> > > To: odecoy...@alltel.net >> > > From: odecoyote <odecoyo...@alltel.net> >> > > Subject: Re: H2O2.com - Email Us Form >> > >> > >>Reply-To: "Kristin Mills" <mills...@bellsouth.net> >> > >>From: "Kristin Mills" <mills...@bellsouth.net> >> > >>To: "Kenneth Steckenrider" <odecoyo...@alltel.net> >> > >>Subject: Re: H2O2.com - Email Us Form >> > >>Date: Mon, 23 Aug 2004 11:54:14 -0400 >> > >>X-MSMail-Priority: Normal >> > >>X-Mailer: Microsoft Outlook Express 6.00.2800.1409 >> > >>X-MimeOLE: Produced By Microsoft MimeOLE V6.00.2800.1409 >> > >> > >>Mr. Steckenrider, >> > >> > [...snip contents of letter to Ode] >> > >> > Hi Ken >> > >> > I also wrote h2o2.com a year ago and asked the same question. I see >> > they haven't changed:) >> > >> > http://escribe.com/health/thesilverlist/m60792.html >> > >> > Could you do a little test to help settle the question of how H2O2 >> > reacts with silver ions? >> > >> > 1. Take several ounces of high-ppm ionic cs made with your >> > Silverpuppy. (I wouldn't try it with low ppm cs made with HVAC, >> > since Marshall's description of the salt test is a bit strange, and >> > I don't know what else is going on with his stuff.) >> > >> > 2. Carefully heat the to 120F to 140F until all the liquid >> > evaporates. Let it cool. You should have black stuff in the bottom >> > of the glass. Here are the equations: >> > >> > When the cs evaporates, the silver ions combine with the hydroxyl >> > ions to form silver oxide. There are at least two paths. >> > >> > Path #1: >> > >> > One silver ion combines with one hydroxyl ion to form silver >> > hydroxide: >> > >> > Ag(+) + OH(-) --> AgOH (silver hydroxide) >> > >> > The silver hydroxide dissociates to form silver oxide particles: >> > >> > 2AgOH --> Ag2O + H2O (silver oxide) >> > >> > Path #2: >> > >> > Two silver ions combine with two hydroxyl ions to form silver oxide: >> > >> > 2Ag(+) + 2OH(-) --> Ag2O + H2O >> > >> > 3. Add 1/8 inch H2O2 and swirl it around. You should see plenty of >> > bubbles and fizzing as the black stuff dissolves. Here is one >> > possible reaction: >> > >> > 2Ag2O + H2O2 --> 4Ag(+) + O2(g) + H2O2 >> > >> > 4. When everything settles down, add several shakes of salt. You >> > should see the heaviest white dispersion you will ever see, and the >> > silver chloride particles ahould be so large they are visible with >> > the naked eye. Here are the equations: >> > >> > From the dissociation of salt in water: >> > >> > NaCl(s) + H2O --> Na(+)(aq) + Cl(-)(aq) >> > >> > A silver ion reacts with a chlorine ion to form silver chloride: >> > >> > Ag(+)(aq) + Cl(-)(aq) --> AgCl(s) >> > >> > The silver chloride is insoluble in water and precipitates out as a >> > white solid. >> > >> > This shows that H2O2 reacts with silver oxide to form silver ions. >> > >> > If H2O2 reacted with silver ions to form oxide, there would be no >> > white dispersion in step 4. I posted this experiment over a year >> > ago: >> > >> > http://escribe.com/health/thesilverlist/m62791.html >> > >> > The hardest part of this experiment is evaporating the cs:) >> > >> > I'd sure appreciate hearing from anyone else who might like to try! >> > >> >Best Wishes, >> > >> >Mike Monett >> > >> > >> >-- >> >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: silver-list@eskimo.com >> >Silver List archive: http://escribe.com/health/thesilverlist/index.html >> > >> >Address Off-Topic messages to: silver-off-topic-l...@eskimo.com >> >OT Archive: http://escribe.com/health/silverofftopiclist/index.html >> > >> >List maintainer: Mike Devour <mdev...@eskimo.com> >> > >> > > >
