There is a constant, but small reaction, at the silver metal/water interface: Ag + e <----> Ag+. Thermal currents and diffusion will dilute the concentration near this interface, so that in order to maintain an equilibrium more silver will dissolve.
http://www.burnsurgery.org/Betaweb/Modules/silver/section3.htm (well worth reading, if you are into silver ions) 'This unique physical structure, in combination with the oxygen atoms/molecules that are trapped in the crystal lattice, contribute to the enhanced solubility of the films which continue to release silver until the concentration in solution reached 66 mg/L a level that is 50 to 100 times higher than is expected from typical bulk pieces of silver metal. Handbook of Chemistry and Physics, 55th ed., CRC Press, Cleveland, 1974, pp B-134.' This passage would seem to suggest one can expect a concentration of 0.66 - 1.32mg/L to be eventually reached in solution. Ivan. ----- Original Message ----- From: "Frank Key" <[email protected]> To: <[email protected]> Sent: Thursday, 22 March 2001 08:35 Subject: Re: CS>Fwd: Dr. Jon's Special Silver FAQ's 3-19-01 > Dean wrote: > > > I see. So what is it that increases the conductivity of the water > > after a few days when a silver ingot has been added? > > If you believe that silver is dissolving in water, then try a simple test; > > 1. Using a lab balance that reads to 5 places in grams, determine the weight > (mass) of a small pure silver object. > > 2. Place this object in pure DI water for a period of time (hours, days, etc). > > 3. Remove the object and again weigh it. > > This will tell you if you are dissolving silver in water. > > > If silver particles don't change the conductivity, then the silver > > must be going into the water as ionic silver. > > Since silver is not water soluble, then silver ions are not being added to the > water. The change in conductivity is probably the result of the addition of > absorbed gasses. > > To test this theory, draw some pure DI water and measure its conductivity. > Place part in an open container, and part in an evacuated container (vacuum or > filled with an inert gas such as argon). > Let both containers sit for about a few days, then measure the conductivity. > > The increased conductivity of the open container demonstrates the absorption > of gases. > > > I admit that my chem classes in college were some time ago, but I have > > been under the (probably erroneous) impression that "to dissolve" > > meant to "make ions" of whatever's being dissolved. > > Indeed, dissolving does cause ions to be added to the solution. The problem lies in the fact that silver is not water soluble. > > The only way to dissolve silver in water is to pass an electric current through > it. This forces the removal of an orbital electron from an atom of silver changing it to a silver ion which is water soluble. > > frank key --- Outgoing mail is certified Virus Free. Checked by AVG anti-virus system (http://www.grisoft.com). Version: 6.0.237 / Virus Database: 115 - Release Date: 08/03/2001 -- 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]>
