Hi Wolf:

The potential reactions between H2O2 and silver are complex. People
like to try to simplify it, but it really cannot be done.

Whenever you have larger silver particles or metallic silver, oxidation
becomes a significant factor in the reaction. Lack of tyndall CAN be
caused by the silver falling out of suspension. H2o2 is used to reclaim
silver from sludge water in industrial applications. If you talk to
these folks, who do this on a daily basis, they would tell you that the
silver will NOT remain in solution.

In a hydrosol, larger isolated silver particles are broken down into
smaller silver particles. This process can continue until the silver
particles are converted into ions. The process is different when adding
h2o2 to metallic silver, as apposed to an ionic silver solution with
colloidal particles. In this reaction, there is NO oxide coating that
occurs on the silver.

To meter your H2o2 with standard peroxide strips, you'll have to dilute
the H2o2 with distilled water further before adding it for your silver
experiments. You would see the effects via measurement, as an example,
if you diluted the H2O2 down to 75-100 PPM before adding it to any form
of silver.

You're not dealing with any dangerous gasses; with this reaction, mostly
oxygen, perhaps a very small amount of hydrogen.

Kind Regards,

Jason

wolftech711 wrote:
> Greetings,
>
> I have read about adding H202 to CS / EIS.
> The impression that I got from this process is that larger silver
> particals are being broken down into silver ions,
> while the H2O2 was broken down to hydrogen and oxygen.
>
> This led me to an experiment of dropping a silver coin into a quart
> of OTC 3% H2O2.
>
> Observations:
> Small bubbles appeard on the surface of the silver, growing in size
> and combining with others until released
> and raceing up to the surface.
> At times streams of very small bubbles would swirl around in the
> solution befor heading for the surface.
> Some bubbles accumulated on the tapered sides near the top of the
> Mason jar.
> The silver coin color turned to a drak gray with some small dark
> metallic blue patches.
> The solution remained clear with no TE throughout the process.
>
> After 6hrs the coin was removed and the jar sealed. (safety conserns
> as to what gases this reaction was producing)
> Somehow I expected it to reach a saturation point befor this.
> Next day the soultion remained clear with no TE.
> I took a sample, added a few grains of table salt, that produced a
> distinctive TE.
> PH test strip: tested about 7 Proxide test strip: still >100ppm.
>
> Maybe it's a good thing that I did'nt take chemistry in HS... I might
> have blown up the house or my car with my curiosity experiments. :)
> Ahh... The drive for knowledge can be oh so powerfull.
>
> At this point I will defer to those of greater chemistry knowledge
> and wisdom, as to what I just did.
>
> 1) Did this process produce a usable Ionic Silver soultion?
>
> 2) What are the gasses or by-products produced in this processes? And
> are they dangerous?
>
> 3) In general what will bring down a proxide content of a soultion?
>
> Thanks
> -Wolf-
>
>
>
>
>
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