> -----Original Message----- > From: Marshall Dudley [mailto:[email protected]] > > Ivan Anderson wrote: > > > > -----Original Message----- > > > From: Marshall Dudley [mailto:[email protected]] > > > > > If a silver atom loses an electron something else has to gain it. > > > From what I > > > can gather it is an OH radical under these circumstances. > > > > > > Marshall > > > > No, the power supply gains the electron removed from the silver atom. In > > doing so the power supply supplies an electron at the other > electrode which > > is used to create hydrogen gas. > > It is impossible for a power supply to gain or lose any > electrons. Most are > completely isolated from ground, and if they did then the entire > liquid would > become more positive, which it does not. Initially an electron > is removed from > the silver atom on the anode side, and an electron is added to an > OH radical on > the cathode side, which releases an atom of H which combines with > another H > atom and creates hydrogen gas.
That is what I said...the silver donates an electron to the power supply at one electrode and in doing so an electron is supplied to the other electrode. Water is then electrolysed releasing hydrogen gas. Hydroxyl ions are created as a result. There are no hydroxyl radicals involved. Besides which, a power supply has two components, an electron sink, and an electron donor, grounded or not...otherwise it does nothing. > Thus for each Ag+ we have a corresponding OH- generated. The > liquid remains > neutral as a whole. Yes. > > > > The fact that free silver ions are found in solutions undergoing such a > > process is indisputable. > > No one ever said they were not free. Just that they were > associated with OH > radicals. The silver ions are solvated and are not associated with anything. >Just like sodium is free when you dissolve lye in > water. The Na and > OH disassociate, but are still there, and are still considered a compound. A compound is associated by a covalent or ionic bond, that is not the case here. > What is the difference between Na+ and OH- in water and Ag+ and > OH- in water as > far as definitions are concerned? And to test the theory, if you > add any acid > to ionic silver, you would expect the OH- to combine with the > acid, and the Ag > to aggregated and precipitate out, which I have found to be true > any time I > have done it. Precipitate out as what? Did you titrate the addition or just add some acid. What strength was the acid? What was the acid you used? One would expect the H+ of the acid to combine with the OH- in solution thereby lowering pH and leaving the conjugated base. Whether this reacts with the silver or not depends upon what it is, and how much you put in. > Marshall Ivan. -- 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]>
