Marshall wrote: > Although this is correct, I feel it is irrelevant. Silver chloride will not > remain silver chloride in the blood stream. Trace amounts of ammonia which are > present in the blood should quickly combine with silver ions of the silver > nitrate to produce a complex ion called the diamminesilver(I) ion, [Ag(NH3)2]+. > I would expect this to end up being diamminesilver chloride. >
Since the concentration of ammonia in blood serum is 0.17 - 0.80 ppm and the chloride concentration is about 3500 ppm, it would seem to me that the ammonia concentration is too weak with such a high chloride concentration to make much difference. (Values from the Merck Manual, see: http://www.silver-colloids.com/Tables/LabValues.PDF ) I have asked Dr. Maass for his opinion on this issue and will post his answer when it is available. Regarding the comments on stomach acid, below is a comment from Dr. Maass. frank key The Chemical Handbook lists the solubility of AgCl to be 0.000089g/100 ml of pure water. This corresponds to 0.89 ppm, a small enough number for every analytical book in the world to list AgCl as insoluble. If one calculates the solubility from the well-known solubility product constant Ksp = [Ag+] [Cl-] = 1.8 x 10-10 , one would get approximately the same answer, around 1 ppm. In a chloride environment, however, the solubility of AgCl would be less than it would be foe pure water, a result which would be expected from Le Chatelier's Principle. For the equilibrium Ag+ + Cl- à AgCl (s) Le Chatelier's Principle would state that the addition of chloride would drive the equilibrium to the right, towards the insoluble AgCl side. In a chloride environment, however, according to the Merck index, the amount of Cl- in the bloodstream is about 3500 ppm, which translates to approximately 0.1 M. Substituting this value into the above solubility product equation, one calculates that the amount of ionic silver in the blood cannot exceed 1.94 x 10-4 ppm. The common method of dissolving AgCl is not to use more acid, but to use a base, such as ammonium hydroxide, to form a soluble complex, i.e., AgCl (s) + 2NH4OH à Ag(NH3)2+(aq) + 2H2O While there is some evidence that an acid chloride complex can be formed to re-dissolve the AgCl precipitate, e.g., AgCl (s) + 2HCL à AgCl2-(aq) + 2H+ , this complex is of questionable stability and only exists in very high concentrations of acid, around 12 M, or over 100 times stronger than stomach acid. -- 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]>
