When copper is introduced into a silver-ion solution, the equilibrium below is set up. $\text{Cu}(s) + 2\text{Ag}^+(aq) \rightleftharpoons \text{Cu}^{2+}(aq) + 2\text{Ag}(s) \quad K_c = 1.0 \times 10^5$ What is the equilibrium concentration of silver ions when $[\text{Cu}^{2+}] = 0.10\,\text{mol dm}^{-3}$?
- A$5.0 \times 10^{-7}\,\text{mol dm}^{-3}$
- B$5.0 \times 10^{-4}\,\text{mol dm}^{-3}$
- C$1.0 \times 10^{-3}\,\text{mol dm}^{-3}$
- D$1.0 \times 10^{2}\,\text{mol dm}^{-3}$