Lessee here... "dissolved" or ionic components are
invisible [correct?]....so all this has to do with that portion that's 26
PPM and under.
Metallic silver isn't dissolved, but 2 molecule sized particles would also
be invisible.
So, these would be reactions that we can't actually "see" happening [??]
And if all of the OH anions were being used up by Ag ions> dissolved
Hydroxides wouldn't the PH be neutral ?
Ahh.. the question of why the drop in conductivity over time.
All that which contributes to TE or color isn't dissolved [is
colloidal...or bottom sludge]
AgOH is tan to white.
AgO and Ag2O would be yellow to brown to black.
While one of these Oxides is destroyed by H2O2 into metallic silver, the
other can be created by H2O2 action on metallic silver.
Concerning the particle arc that can be seen when not stirring and
current is not limited, one electrode will emit a golden stream, the other
a white stream of particles and between where the two meet...nothing
visible. [ Ag Ions?] ..a transitional area?
But if that arc intersects the glass bottom of the container. under the
golden stream will be a black spot that H2O2 won't touch, a silver mirror
in the middle and a whitish spot that H2O2 won't touch under the white stream.
On the black electrode H2O2 will destroy that form of Oxide, but not where
it collects on the glass under it.
Premis: The glass contributes electrons that collect on its surface like a
capacitor and changes the chemistry at that surface.
Key question: Do the electrodes produce monatomic Oxygen and/or Hydrogen
in the diffusion layers where many reactions take place?
LOL..care to bend your considerable brain around those *not dissolved*
[colloidal and droput] products?
And delve into why the addition of H2O2 produces 2 different visible
reactions if done early, [ flash white/ flash brown...and murky ] but not
when done later on after conductivity stops dropping?...except for clearing
up a yellow batch, color presumably from suspended Oxides that H2O2 will
convert.
It seems like the various actions of H2O2 will be the decoder of what
happens where and when.
WAY over MY head.
Here's an opportunity to "write the book" [E-gads!].....for some idgit to
shoot holes in. [wink]
Ode
At 10:49 AM 3/12/2010 -0500, you wrote:
Actually Ag2O converts back and forth with AgOH without anything added
(just a water molecule taking part in it):
Ag2O + H2O <=> 2 AgOH
A saturated solution in balance has equal molar part of each, because once
you reach around 13 ppm, the silver oxide precipitates limiting the amount
of it, but the silver hydroxide is much more soluble, so with the
switching back and forth the hydroxide is also limited to 13 ppm giving an
upper level of ionic silver to be around 26 ppm.
When you add H2O2 things get interesting, as it is a redox agent.
It reduces the silver oxide and silver hydroxide to silver particles:
Ag2O + H2O2 -> Ag2 + H2O + O2
2AgOH + H2O2 -> 2Ag + 2H2O
and oxidizes silver metal to silver oxide:
2Ag + 2H2O2 -> Ag2O + 2H2O
The AgO that you have below is NOT silver oxide, but actually silver
peroxide, and is actually believed to be Ag2O2. If you add hydrogen
peroxide to it you may get:
Ag2O2 + 2H2O2 -> 2Ag + 2H2O + 2O2
However silver peroxide is 100% insoluble, so unless you have a
precipitate, there is none there, and without being in solution it might
not react with dilute amounts of H2O2 significantly.
Marshall
--
The Silver List is a moderated forum for discussing Colloidal Silver.
Rules and Instructions: http://www.silverlist.org
Unsubscribe:
<mailto:[email protected]?subject=unsubscribe>
Archives:
http://www.mail-archive.com/[email protected]/maillist.html
Off-Topic discussions: <mailto:[email protected]>
List Owner: Mike Devour <mailto:[email protected]>
