Chemistry Ksp Solution: Consider a beaker containing a saturated solution ...

Solution: Consider a beaker containing a saturated solution of CaF2 in equilibrium with undissolved CaF2(s). Solid CaCl2 is then added to the solution.Will the concentration of Ca2+ ions in solution increase or decrease?

Problem

Consider a beaker containing a saturated solution of CaF2 in equilibrium with undissolved CaF2(s). Solid CaCl2 is then added to the solution.

Will the concentration of Ca2+ ions in solution increase or decrease?

Solution

We’re being asked what would happen to the concentration of Ca2+ ions when solid CaCl2 is added to CaF2 solution upon reaching equilibrium.


The common ion effect states that the solubility of a salt is lower in the presence of a common ion


For CaF2: The chloride ion, Cl, has a charge of –1. Calcium is in Group 2A then has a charge of +2:

CaF2(s)  Ca2+(aq) + 2 Cl(aq)


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