On 9/24/2011 5:19 PM, David AuBuchon wrote:
1. So in EIS, Ag+ combines with OH- and gets AgOH. Some of this
turns into Ag2O. Then some of both of these may get stuck together
and form particles. Some free Ag+ and OH- also exist. Yes?
Depends on concentration. Each of them have a solubility of about 13
ppm, so up to around 26 ppm of ionic, they will both be completely
dissolved. If the concentration exceeds that then they do indeed clump
together to some extent, and precipitate out of solution.
2. When we say that AgOH or Ag2O is "dissolved" does that mean:
a) they are disassociated into ions most of the time. They
occasionally recombine but quickly separate again.
b) They are still in compounds, and occasionally disassociate into
ions for a short time, then quickly tend to recombine.
c) none of the above.
If they are in solution, then they will be ions.
3. When we measure conductivity of EIS, since AgOH, Ag2O, and
particles of the former do not contribute, this is an actual
indication of free silver ions, right?
Conductivity will be a measure of free ions. Silver ions will be
approximately half of the conductivity. The OH and O-- ions will be the
other half.
4. If we took silverchloride and just dissolved it in water and kept
it under a reasonable PPM, how would this be any different than what
we are making by electrolysis?
It would have a chloride ion, and be quite stable. For instance if you
add H2O2 to ionic silver, it reacts producing particles, but there is no
reaction with silver chloride.
Marshall
Sorry if I have asked these several times already, but my Lyme brain
is not the best.
~David
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