"Mike Monett" <[email protected]> wrote:

  [...]

  > Let's face  the issue. You have a pathogen that if  you  allow it,
  > will cause you great harm or kill you.

  > This does  not lend itself to diplomacy or  negotiation.  There is
  > only one correct response, and that is utter, complete destruction
  > and total obliteration of the pathogen. In many cases, silver ions
  > are invaluable  depending  on the threat. In  other  cases, copper
  > ions may be the best answer.

  > My designs incorporate both. But are there other answers we should
  > be looking for? If so, how do we find them?

  To give  an  example,  silver   and   copper  ions  are  fairly well
  understood in  the  literature,  and  they  are  extremely effective
  against pathogens.

  But what about other metals, such as zinc? It is  readily available,
  performs exceptionally well in electrolysis, and should be deadly to
  pathogens.

  Like copper,  the chloride is very soluble (4320  g/L  (25C)), where
  silver chloride  has very limited solubility (ppb or sub-ppb  in the
  absence of ammonia.)

  Where silver  has  a  problem with  sulfur  making  insoluble silver
  tarnish (Ag2S),  copper  has a problem with  oxygen,  making  CuO or
  Cu2O. These form contamination products when you try to use  them in
  electrolysis, and they destroy the process.

  But zinc  doesn't  seem to be bothered by either. Just  look  at any
  carbon-zinc battery. The outside is pure zinc. It never seems  to be
  bothered by  unwanted oxides or sulfides. The only  problem  is when
  the electrolyte breaks through the shell, then everything  gets real
  messy. But we don't have to deal with that.

  When you  put  zinc  in electrolysis, it  behaves  beautifully  - it
  immediately migrates to the cathode, where it plates out.  There are
  no hydroxide  problems  to deal with,  and  no  unexpected responses
  anywhere. It just goes and does its thing.

  Is this the metal we need to explore?

  So many questions. So little time...

  Thanks,

  Mike


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