People have been taught in high school and college freshman chemistry that silver ions react with chloride ions to form water insoluble silver chloride. But in advanced courses in chemistry, one further learns that in the presence of large excesses of chloride ion, such as that found in stomach acid and/or blood, the silver exists as a water soluble complex ion containing 2 chloride ions per silver ion. Since this is water soluble it can be readily absorbed through the stomach if necessary. Now, while the strength of the complex ion formed by the reaction of silver with the two chloride ions is enough to prevent precipitation, it is also not enough to prevent the silver from its normal ability. There is no loss in effectiveness.
