Common-Ion Effect Practice Test

A saturated solution of $\text{CaF}_2(s)$ is at equilibrium: $\text{CaF}_2(s) \rightleftharpoons \text{Ca}^{2+}(aq)+2\text{F}^-(aq)$. A soluble fluoride salt is added, increasing $\text{F}^-$. At constant temperature, what happens to the amount of $\text{CaF}_2(s)$ that can dissolve?​

The equilibrium $\text{HNO}_2(aq) \rightleftharpoons \text{H}^+(aq)+\text{NO}_2^-(aq)$ is established in solution. A small amount of $\text{KNO}_2(aq)$ is added. Qualitatively, how is the concentration of $\text{H}^+$ affected after the system reestablishes equilibrium?​