# Can dissolved salts (or any soluble chemicals, for that matter) 'bump' each other out of solubility?

Will a more soluble substance dissociate, causing a less soluble substance to precipitate out?

in equation:

AB(s)+ C(aq)+ D(aq)--> A(aq)+ B(aq)+ CD(s)

Does that equation go through, under the assumptions that AB, as a whole, is more soluble than CD, and saturation point is achieved with both substances?

Thanks in advance! This question has been bothering me for a while...

$\ce{AgCl(s) + Cl- (aq) -> AgCl2- (aq)}$
• I don't think the OP was asking about the common ion effect. More like $$\ce{KNO3_{(s)} + Ag^+_{(aq)} + Cl^{-}_{(aq)} -> K^+{(aq)} + NO3^{-}_{(aq)} + AgCl_{(s)}}$$ which I think would have the opposite effect. I'd expect $\ce{AgCl}$ to be more soluble in a $\ce{KNO3}$ solution. – MaxW Dec 2 '15 at 1:18