Bob wrote: > > When one has a solution that contains positive ions they try desperately to > avoid each other, mutual repulsion. On occasion several individual ions will > agglomerate into a larger one and the PPM as measured by a spectrophotometer > will show a reduction, even though the total amount of silver is in > solution. > How have you determined the occurrence of "On occasion several individual ions will agglomerate into a larger one ".
At the sub-nanometer size of ions, the repulsive force of the ions is over one hundred thousand G-forces which virtually assures that the ions will never get close to each other. The closer they get, the higher the repulsive force becomes. What do you think would overcome mutual repulsion to allow ions to come together? "... and the PPM as measured by a spectrophotometer will show a reduction, even though the total amount of silver is in solution." If your only means of determining the silver concentration is the spectrophotometer how have you determined that the total silver in solution is the same when the "spectrophotometer will show a reduction"? frank key -- 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]>
