How does adding acids (H+ ions) to limited soluble salts help it further dissolve?

For example, adding $\ce{HCl}$ to the very insoluble $\ce{CaF2}$ will help it further dissolve. How?


I believe the concept deals with equilibrium and Le Chatelier's Principle:


$$ \ce{ CaF2 <=> Ca^2+ + 2F^-} $$


Does adding $\ce{H+}$ react with the $\ce{F-}$, which shifts the equilibrium to the right-hand side and therefore further dissolve the salt?




In general, the solubility of a sparingly soluble salt having a basic anion will increase with the addition of a strong acid. Given: 


$$\ce{X+A- <--> X+ + A-}$$ 


where $K\_{sp}$ is small and A- is a weak base, the addition of a strong acid will form HA, driving the reaction to the right and increasing $K\_{sp}$. 


In the specific case of 


$$\ce{CaF2 <--> Ca^2+ + 2F−}$$ 


the addition of $\ce{HCl}$ gives 


$$\ce{CaF2 + 2HCl <--> Ca^2+ + 2Cl- +2HF}$$ 


driving the reaction to the right, thus increasing the solubility of $\ce{CaF2}$. Note that $\ce{HF}$ itself is a weak acid, having a pKa of $3.17$, and will be in equilibrium with $\ce{H+}$ and $\ce{F-}$.


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