Silver compounds, particularly silver chloride (AgCl), exhibit low solubility due to the stability of their ionic bonds and the unique properties of silver ions. While silver nitrate is highly soluble, most silver salts, including chlorides and sulfates, are not. This trend is consistent across various anions, where silver compounds generally remain insoluble compared to other cations. However, exceptions exist, such as silver(I) fluoride and silver perchlorate, which demonstrate higher solubility due to differing ionic interactions.
PREREQUISITESChemistry students, researchers in inorganic chemistry, and professionals working with silver compounds in industrial applications will benefit from this discussion.
Then why silver (I) fluoride is so much water soluble than most other fluorides (excepting those of alcaline metals)?Char. Limit said:Yes, but silver nitrate is (close to) the only one. And if you check, just about anything nitrate is soluble. But silver isn't soluble where most other cations are. That is undeniable. Just look at silver chloride.
Sorry, but this is the only case on this forum so far where I am sure of my correctness. This and the concentration problem. A compound with silver, for the most part, is insoluble when the same anion with (almost) any other cation would be soluble.