Re: CS>Adding peroxide to CS
From: Marshall Dudley
Date: Fri, 20 Aug 2004 21:08:25
http://escribe.com/health/thesilverlist/m72757.html
Hi Marshall,
I combined two posts to simplify things, and split the first para
into separate sentences to analyze. Hope it's ok..
> OK, I just ran a test.
> I started with 5 ppm EIS, approximately 80% ionic.
> I put equal amounts into to containers, and added a few drops of
> H2O2 to one of them.
> I could see no difference between, they were both crystal clear.
> I then added a pinch of salt to both.
> The one without H2O2 immediately formed AgCl and turned milky.
I'm surprised you got such a fast reaction adding NaCl to 5 ppm cs.
Normally, it takes several minutes at this concentration. You should
get a pale blue dispersion that is barely visible unless you hold it
in the light just the right way.
I really think you have a lot more that 5 ppm cs. Can you measure
the ppm with a Hanna? If so, 1 uS = 1 ppm. Are you using constant
current? If so, you can calculate the max ppm using the Faraday
equations in Mercury.
How do you know the cs was 80% ionic? It usually takes a very high
current density to get this much oxide. For example, 3 nines run to
the max like this:
http://www.utopiasilver.com/images/gen3.jpg
> The one that had had H2O2 added to it stayed crystal clear.
There is some very strange chemistry when NaCl is added to H2O2 and
high-ionic CS. Here is what happened when I tried it. I doubt I will
ever figure out how to write the equations that describe this:
"When H2O2 is added to the cs made with Godzilla, the salt test
does nothing for a few seconds. Then a huge cloud of bubbles
appears and the salt disappears. I have never seen this reaction
before."
"I repeat the same test over and over until I am almost out of
salt. The same thing happens. Then finally I get a strong
dispersion."
http://escribe.com/health/thesilverlist/m61977.html
Now, I was getting pretty high ppm with Godzilla, and the salt test
went haywire with H2O2. So this is another reason I think your
figure of 5 ppm is way too low.
> I can think of only 2 possibilities for this:
> 1. Silver ions were reduced to a colloid of silver atoms.
> 2. Silver ions became silver oxide, and it dissolved.
Marshall, there are a lot more possibilities, but please write the
balanced equations! This will tell you if something is possible or
not:)
Also note silver chloride dissolves in ammonia:
AgCl + 2 NH3 --> Ag(NH3)2+ + Cl-
This might be an additional diagnostic test if the H2O2 doesn't
interfere.
Re: CS>Adding peroxide to CS
From: Marshall Dudley
Date: Fri, 20 Aug 2004 21:19:31
http://escribe.com/health/thesilverlist/m72758.html
> OK, I have confirmed that converting silver chloride to silver
> oxide is exothermic, which means that the silver oxide is more
> stable.
Marshall, this is very interesting. If silver chloride does not
dissolve in the stomach, does this mean silver oxides are even more
inacessible to the body?
According to various web sites I came across, silver ions are from
hundreds to thousands of times more effective than silver chloride
in killing bacteria. I believe your information shows the oxides are
inert, and therefore have no effect in the body except perhaps to
contribute to argyria.
> Thus possibility 2 of the previous message is not eliminated as I
> had hoped it would be.
> See http://www.finishing.com/195/29.html
> This article also gives some extremely interesting information.
> Dextrose will reduce silver oxide to silver metal! Honey is about
> 50% dextrose (aka glucose), so that may be why some people feel
> that adding a drop of honey when making CS is a good idea, it
> converts any silver oxide formed to silver particles.
Fascinating - where do you dig up this information?
> So, according to this, one should be able to convert all the
> silver ions in EIS to silver atoms and silver particles by adding
> H2O2, and if that gives AgO, adding a little glucose, or honey.
How do we make a test that will show this? (And how do we write the
equations:)?
> Marshall
Best Wishes,
Mike Monett
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