The following reaction occurs for hydrated aluminium ions. $[\text{Al(H}_2\text{O)}_6]^{3+}(aq) + \text{H}_2\text{O}(l) \rightleftharpoons [\text{Al(H}_2\text{O)}_5\text{OH}]^{2+}(aq) + \text{H}_3\text{O}^+(aq)$ Which statement is true about this reaction?
- A$\text{H}_2\text{O}(l)$ and $[\text{Al(H}_2\text{O)}_5\text{OH}]^{2+}(aq)$ are a conjugate acid-base pair.
- B$\text{H}_2\text{O}(l)$ is acting as an acid as it is donating $\text{H}^+$ ions.
- CIf $\text{OH}^-(aq)$ is added, the equilibrium will move to the right.
- D$K_c$ varies as the pH is varied.