----- Original Message ----- From: <[email protected]>
> Roger, > There can only one anion formed at the cathode, given we only have water > and silver, and that is OH-. > > Ivan: Then perhaps you can explain the following: Brewing a typical LVDC for > 30-45 minutes will generate a 'net' CS of 5-10 PPM and the 'solution' will be > neutral to slightly acidic. So please explain how electrical neutrality was > maintained when, > > 1) The generation of OH- would have created a basic pH and/or > 2) The complete reduction of ALL Ag+ at the cathode would have resulted in NO > ionic silver present, at situation that Frank (and probably you too) asserts > is virtually impossible. Yes. > It seems to me that the evidence is pretty strong that there is an electrical > IMBALANCE, and THAT imbalance is precisely what maintains particle > separation. What think thee Ivan? Well, as a whole, the solution contains no more charge than it did before electrolysis, it is just that the charges have been separated into positive and negative ions. It is just like a battery, when fresh, one side is positive and one side is negative, and when consumed both sides are neutral, but the same amount of electrons and protons exist in both states. The pH of the solution is determined by the amount of H+ ions (H3O) but as hydrogen is reduced at the cathode it leaves the cell as H2 gas, but it leaves as a neutral species and so does not effect the net electrical state. > > b Both silver and H2 have a similar reduction > potential, silver slightly lower. So silver ions will be reduced > preferentially to hydrogen, once they make the journey from the anode... > hydrogen will be reduced until then. But even when silver ions are there > in quantity there reduction will cause a lowering in concentration in > the immediate cathode area which will allow hydrogen to be reduced > again, untill the concentration is restored, and so on. > > > Ivan: Even allowing for prolonged contact with air, I wonder how > readily Ag+ > > will react with dissolced CO2 [CO3=] to form Ag2CO3? My guess is that > they > > don't readily react. Likewise for Ag+ & OH- forming AgOH. What sayeth > the > > literature? > > http://www.chee.iit.edu/~anderson/courses/enve501/sol11.pdf > Here is a worked example of Ag+ ions added to a sloution containing OH-, > CO3- and Cl- . > > At the concentrations of colloidal silver (10-5M) there will be no > precipitates of AgCO3 or AgOH I shouldn't think, as the concentrations > of these molecules will be very low given the neutral or acidic pH of > the solution. Both OH- and CO3- are bases. > > Ivan: Are you simply saying that in an acidic to neutral pH, the solubility > of these species is too high to cause them to precipitate? Roger Yes, the concentration of OH- and CO3(2-) will be very low and so they exist as free ions. Ivan. --- Outgoing mail is certified Virus Free. Checked by AVG anti-virus system (http://www.grisoft.com). Version: 6.0.237 / Virus Database: 115 - Release Date: 08/03/2001 -- The silver-list is a moderated forum for discussion of colloidal silver. To join or quit silver-list or silver-digest send an e-mail message to: [email protected] -or- [email protected] with the word subscribe or unsubscribe in the SUBJECT line. To post, address your message to: [email protected] Silver-list archive: http://escribe.com/health/thesilverlist/index.html List maintainer: Mike Devour <[email protected]>
