QUOTE (Juramike @ Aug 17 2011, 07:59 PM)
The rocks are sulfates, not carbonates...the acidity of water shouldn't affect dissolution of sulfates.
(Hmmm, maybe I need to think about this one a bit....).
Anyone?
Sulfates generally do not exhibit pH dependent solubilities because the sulfate anion is a very weak base. In other words, its very hard to protonate sulfate. Perchlorates, nitrates and halides are also very weak bases, but the solubilities of their metal salts are often high because they are monovalent anions. Sulfides, carbonates and phosphates are often pretty insoluble due to their high charge, but all are also good bases. For sulfides, carbonates and phosphates (for example) exposed to acidic water, a set of simultaneous equilibria involving protonation and dissolution steps are present. If the pH is specified, it's not horribly difficult to solve these simultaneous equilibria for the concentrations of each ionic species, even if multiprotic events occur.
Hoping this doesn't bring back bad memories of college chemistry!