In a message dated 3/23/01 8:14:37 AM EST, [email protected] writes: << Subj: Re: CS>Re: saturated solution Date: 3/23/01 8:14:37 AM EST From: [email protected] (Ivan Anderson) Reply-to: [email protected] To: [email protected] ----- Original Message ----- From: <[email protected]> > Ivan: You said, "Of course for every silver ion liberated at the anode there > is a corresponding anion formed at the cathode (or the reduction of a cation) > so the solution remains electrically neutral." Would you please provide some > examples of the anions formes at the cathode. 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. 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? 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 -- 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]>
