At 10:16 AM 1/24/2005 -0500, you wrote:
>
>Ode Coyote wrote:
>
>> A If you start with 1 oz of 10 ppm EIS, that will
>> >typically have about 9 ppm of silver hydroxide in it.
>
>>
>> ##  Might want to check and see how soluable silver hydroxide is. It's
>> listed as "insoluable".

@@@ Searched a bunch of sites a while back to include reagent
manufacturers...typically I ran across this below... [But no figures on
"how" insoluble]

http://www.ausetute.com.au/solrules.html
Rules for Learning the Solubility of Ionic Compounds in Water
###############
Hydroxide
OH-     +       alkali ions (Li+,Na+,K+,Rb+,Cs+,Fr+),
H+(aq),NH4+,Sr2+,Ba2+,Ra2+,Tl+  =       soluble         strontium hydroxide, 
Sr(OH)2,
is soluble + any other cation   =       low solubility (insoluble)      silver
hydroxide, AgOH, is insoluble (forms a precipitate)
########################### [An example of low solubility being 'called'
insolubility]

Chloride (Cl-), Bromide (Br-), Iodide (I-)      +       silver (Ag+), lead 
(Pb2+),
mercury (Hg2+), copper (Cu+), thallium (Tl+)    =       low solubility 
(insoluble)
        silver chloride, AgCl, forms a white precipitate (a white solid)
+       any other cation        =       soluble         potassium bromide, KBr, 
is soluble
>
>I have searched far and wide for information on silver hydroxide, and all I
>could ever find was that it tends to become silver oxide over time.  Where
>did you find this information?
 ##  UH, I didn't find it? [Wild supposition based on no mention of this
being a problem when handling AgOH powder after looking at many many
chemical suppliers websites]
 The apparent catalytic action of copper in EIS might be a clue to
something.  Drop a shiny piece into a strong batch of EIS and watch
conductivity, TE and deposits over a week or so. Check out copper and
deposits when still wet and dry.   Interesting.

Ode


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