2007-01-28 10:08:36 · 1 answers · asked by mn1998 2 in Science & Mathematics ➔ Chemistry
First of all it depends on the acid.
If you use the conjugate acid of the anion eg HCl for AgCl then you have a common ion effect and thus you will be reducing the solubility.
If you use an acid like HNO3, which doesn't have a common ion, doesn't form a different precipitate with Ag+, or a complex ion with Ag+, then the solubility of AgCl should not be affected as HCl is also a stong acid and thus in solution you will have the Ag+, Cl-, H+ and NO3- ions.
On the other hand, the solubility of Ag2CO3 will increase since H2CO3 is a weak acid, so some of the CO3^-2 ions will now become HCO3^-1 and if you acidify a lot then you will have some H2CO3 forming which will decompose in H2O and gas CO2 and a lot of the CO2 will leave the solution. Since the CO3^-2 decreases, according to Le Chatelier's principle the equilibrium Ag2CO3(s) <=> 2Ag+(aq) + CO3^-2 (aq) will shift to the right and more solid Ag2CO3 will be dissolved
2007-01-28 23:25:28 · answer #1 · answered by bellerophon 6 · 0⤊ 0⤋