url: http://escribe.com/health/thesilverlist/m60880.html Re: CS>Bob Beck Interview From: Mike Monett (view other messages by this author) Date: Tue, 1 Jul 2003 17:25:55
Well, maybe I figured it out. The OH(-) ion is the only thing around that can react with the Ag(+) silver ion. So I searched for AgOH. Sure enough, this is silver hydroxide. The equations are as follows: Water dissociates to H+ and OH- ions to a very small extent. This can be represented as: H2O <--> H(+) + OH(-) The concentration of hydrogen ions in aqueous solutions is pH: pH = -log[H+] = - logarithm in base 10 of [H+] A neutral solution has a pH of 7. During silver electrolysis, we apply current to the cell. At the anode: Ag(s) - e --> Ag(+) At the cathode: 2H(+) + 2e --> H2(g) The silver ions form an invisible cloud around both electrodes. In the ion cloud: Ag(+) + OH(-) --> AgOH (silver hydroxide) The silver hydroxide dissociates to form silver oxide particles: 2AgOH --> Ag2O + H2O (silver oxide) The silver ions leave the anode and drift towards the cathode. This means the ion density around the anode is less than the cathode. Since the ion cloud is most dense at the cathode, the mist forms there first, later followed by mist forming around the anode. This shows particle formation is a function of cloud density. The particles have less tendency to form when the ion cloud is less dense. This is a function of the voltage applied to the cell and the current density at the electrodes. This is why I can achieve much higher ion concentration at 87 uA/sq.in. than previously at 1.4 mA/sq.in. Best Regards, Mike Monett -- The silver-list is a moderated forum for discussion of colloidal silver. Instructions for unsubscribing may be found at: http://silverlist.org To post, address your message to: [email protected] Silver-list archive: http://escribe.com/health/thesilverlist/index.html List maintainer: Mike Devour <[email protected]>
