Hats Off and Thank You Marshall! For this illuminating article and all the other good information you and our other Experts share so generously with "us seekers"! In reading this I was transported back into time to 1940-43 to U of FL Pharcmacy and Chemistry Classes where I had many brilliant professors who labored to clarify similar problems. Thank You!
Sincerely, _______________________________________ Richard Harris, 57 Year FL Pharmacist 448 West Juniata Street Clermont, FL 34711 www.rharrisinc.com http://www.seasilver.com/reh http://healthandhealing.blogspot.com -----Original Message----- From: Marshall Dudley [mailto:[email protected]] Sent: Friday, January 21, 2005 11:58 AM To: [email protected] Subject: CS>Solubility of silver chloride in HCl and NaCl OK, I have just gotten the equation for silver chloride solubility in solutions containing chloride ions. It is in Forbes, Cole J. Am. Chem. Soc., 1921, 43, 2492. Sol, of AgCl = (2 x 10^-10)/[Cl] + b + 3.4 x 10^-5 x[Cl] b = 6.1 x 10^-7 for HCl and NaCl both. The units are in moles. I have worked through the solubility of silver chloride for blood plasma, stomach acid, and stomach juices. Contrary to the equation posted by Frank Key previously in his rebuttal, silver chloride does not obey the equation he proposed for solubility except at low Cl ion concentrations, which is a general equation for solubility of any substance. Silver chloride is different because it forms complexes when the Cl ion content becomes significant. Here are the needed constants if anyone wants to check my computations. molecular weight of salt = 58.5 molecular weight of HCl = 36.5 molecular weight of AgCl = 143.5 Stomach acid is about a pH of 2, which is a molar content of about .01 Salt in blood is .9%, which is a molar content of about .155 molarity of salt in the stomach is unknown, but probably stabilizes around .155 since it is continually replenished by salvia and surrounded by blood at that molarity level,, and if different, would stabilize through osmosis. Plugging into the above equation we get: Solubility of silver chloride in stomach acid will be about .139 ppm Solubility of silver chloride in blood will be about .8439 ppm Solubility of silver chloride in stomach juices assuming .155 molar of salt in it will be about .89 ppm (which is interestingly the same solubility that silver chloride has in pure water) This shows that it is not a problem for silver chloride to dissolve and make it into the blood after all from EIS. If you start with 1 oz of 10 ppm EIS, that will typically have about 9 ppm of silver hydroxide in it. When you drink that, it hits the stomach, and if we assume that the stomach has 3 oz of stomach acid plus .155 molar salt solution, then that will provide 4 oz of liquid to dissolve the AgCl. The EIS would reduce the Cl content to about .041 molar, and if we plug into the above equation, we find that it will dissolve .288 ppm of silver chloride. That means that just over 1 ppm of the 9 ppm of ionic silver will stay dissolved, and just under 8 ppm will precipitate out. Over time the dissolved silver chloride will diffuse through the stomach wall into the blood stream, and the silver chloride will slowly dissolve and enter the blood stream. Also the excess water will quickly diffuse into the blood stream returning the stomach acid and salt back to about .155 molar, which will dissolve about 4 ppm of the silver chloride. The remaining 5 ppm would have to wait for the silver chloride to diffuse through the stomach wall and redissolve, or if that takes too long, will end up going into the intestines. However if you take more EIS, like 10 oz, then the amount of silver chloride that will dissolve will be cut dramatically, and the amount of time for the rest to reach the blood will be significantly lower. This brings up the idea of mixing the EIS with solution of sodium or potassium chloride salts. If you do that then the silver chloride will be formed in the mixture, and if the salt content is high enough, say the same as blood level of .155 molar, then the silver chloride portion will dissolve at the rate of about .89 ppm. So, lets assume we are mixing 1 oz of 5 ppm EIS with 90% ionic content with 2 oz of solution that has about .2 molar of sodium plus potassium salts (IE Gatorade). The final result will be a solution with .133 molar of Cl. Plugging into the above equation we find that solubility of silver chloride in this is .737 ppm and with 3 times the volume, that will dissolve about 2.2 ppm of the 4.5 ppm silver chloride immediately. The remaining 2.3 ppm will form a suspended precipitate. Now, if we drink this, then assuming 3 oz of stomach juices with approximately the same chloride content as the blood, then this will not dilute the molar content of the stomach significantly, so now since we have 3 oz of solution being drunk, plus 3 oz of gastric juices, we now have 6 oz of juices with a molar content of about 1.45 of chloride ions. This will dissolve about .8 ppm of silver chloride if we substitute in the above equation, and since we have 6 oz of fluid with only 1 oz of EIS in it, that will dissolve an equivalent of 6 times as much, or .48 ppm of silver chloride. Since we only started with 4.5 ppm of silver chloride, that means that as soon as the solution hits the stomach 100% of the silver chloride will be dissolved, and will enter the blood stream very rapidly. So by theory then, if you mix and electrolyte, such as Gatorade, with EIS, the transfer speed of silver to the blood stream should increase dramatically. For Gatorade and 5 ppm of EIS, the proper ratio seems to be about 2 parts Gatorade to 1 part EIS. I believe that experimental evidence by Brookes Bailey has shown this to be the case. 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]>
