FRANK CUNS-RIAL wrote: > Marshall, I suspect that the peroxide would oxidize the ionic silver from > one free reactive electron to two, reacting simultaneously and stripping an > oxygen from the peroxide and releasing water. > Ag+1 + H2O2=AgO +H2O > This reaction is stoichiometrically balanced and chemically viable.
Well, first it is not actually AgO, but will always take the form of Ag2O2. That is usually called silver peroxide, what we normally find formed is silver oxide Ag2O. Ag2O2 is TOTALLY insoluble, so it cannot be in any of the ionic silver. However you may have found a key to what may be happening when insufficient H2O2 is added, and the solution will become milky until a little more H2O2 is added. Not sure how you would test for that. > It may > help in the form of catalysis, heat, etc. (I have not checked the > electropotentials of each entity) > Whether it happens only experiementation would tell. > I also suspect it'd be rather difficult for the peroxide (even 35%) to react > with the free metal, other than a surface oxidation. We have done the experiments, and 3% H2O2 will react with silver metal. It forms the oxide, as expected, and the oxide dissolves until the solubility limit is reached, then it forms an oxide layer on the metal. Also tyndall will form indicating that the silver oxide also gets changed to a colloid at the same time. Marshall -- The Silver List is a moderated forum for discussing Colloidal Silver. Instructions for unsubscribing are posted at: http://silverlist.org To post, address your message to: [email protected] Silver List archive: http://escribe.com/health/thesilverlist/index.html Address Off-Topic messages to: [email protected] OT Archive: http://escribe.com/health/silverofftopiclist/index.html List maintainer: Mike Devour <[email protected]>
