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...




Yes, this effect is termed [*salting out*](https://en.wikipedia.org/wiki/Salting_out) for non-ionic compounds and [*the common ion effect*](https://en.wikipedia.org/wiki/Common-ion_effect) for ionic ones.


Note that in specific cases, the *converse* may hold true. For example, "the solubility of silver chloride in water is reduced if a solution of sodium chloride is added to a suspension of silver chloride in water (op cit)." However, *adding more chloride re-dissolves the precipitate* [due to the formation of complex ions](http://chemwiki.ucdavis.edu/Inorganic_Chemistry/Descriptive_Chemistry/Elements_Organized_by_Block/3_d-Block_Elements/Group_11%3A_Transition_Metals/Chemistry_of_Silver/Silver_Chloride):


$\ce{AgCl(s) + Cl- (aq) -> AgCl2- (aq)}$


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