Answer
The amount of solid $CaF_2$ in the beaker will increase.
Work Step by Step
1. This is the solubility equilibrium:
$CaF_2(s) \lt -- \gt Ca^{2+}(aq) + F^-(aq)$
2. When we add a common ion ($Ca^{2+}$ from $CaCl_2$), the equilibrium will move.
According to the Le Chatelier's principle, the equilibrium will move to the $CaF_2(s)$ side. This occurs because the equilibrium will try to consume the $Ca^{2+}$, since we added more to the solution.
