Question

Write net ionic equations for the reactions of each of the following compounds with a strong acid. (a) \(\mathrm{CaF}_{2}\) (b) \(\mathrm{CuCO}_{3}\) (c) \(\mathrm{Ti}(\mathrm{OH})_{3}\) (d) \(\mathrm{Sn}(\mathrm{OH})_{6}^{2-}\) (e) \(\mathrm{Cd}\left(\mathrm{NH}_{3}\right)_{4}^{2+}\)

Short answer

Question: Write the net ionic equations for the reactions of the following compounds with a strong acid: a) \(\mathrm{CaF}_{2}\) b) \(\mathrm{CuCO}_{3}\) c) \(\mathrm{Ti}(\mathrm{OH})_{3}\) d) \(\mathrm{Sn}(\mathrm{OH})_{6}^{2-}\) e) \(\mathrm{Cd}\left(\mathrm{NH}_{3}\right)_{4}^{2+}\) Answer: a) \(\mathrm{CaF}_{2} + 2\mathrm{H}^{+} \to \mathrm{Ca}^{2+} + 2\mathrm{F}^{-}\) b) \(\mathrm{CuCO}_{3} + 2\mathrm{H}^{+} \to \mathrm{Cu}^{2+} + \mathrm{H}_{2}\mathrm{O} + \mathrm{CO}_{2}\) c) \(\mathrm{Ti}(\mathrm{OH})_{3} + 3\mathrm{H}^{+} \to \mathrm{Ti}^{3+} + 3\mathrm{H}_{2}\mathrm{O}\) d) \(\mathrm{Sn}(\mathrm{OH})_{6}^{2-} + 6\mathrm{H}^{+} \to \mathrm{Sn}^{4+} + 6\mathrm{H}_{2}\mathrm{O}\) e) \(\mathrm{Cd}\left(\mathrm{NH}_{3}\right)_{4}^{2+} + 4\mathrm{H}^{+} \to \mathrm{Cd}^{2+} + 4\mathrm{NH}_{4}^{+}\)

Step-by-step solution

Identify the reaction products

For each compound, we need to determine how it will react with a strong acid. Since strong acids donate protons (H\(^+\)) to the solution, we need to identify which component(s) of the compound will accept the protons, leading to the production of ions. (a) \(\mathrm{CaF}_{2}\) reacts with a strong acid to form \(\mathrm{Ca}^{2+}\) and \(2\mathrm{F}^{-}\) ions. (b) \(\mathrm{CuCO}_{3}\) reacts with a strong acid to form \(\mathrm{Cu}^{2+}\) and \(\mathrm{CO}_{2}\) gas. (c) \(\mathrm{Ti}(\mathrm{OH})_{3}\) reacts with a strong acid to form \(\mathrm{Ti}^{3+}\) and \(3\mathrm{OH}^{-}\) ions. (d) \(\mathrm{Sn}(\mathrm{OH})_{6}^{2-}\) reacts with a strong acid to form \(\mathrm{Sn}^{4+}\) and \(6\mathrm{OH}^{-}\) ions. (e) \(\mathrm{Cd}\left(\mathrm{NH}_{3}\right)_{4}^{2+}\) reacts with a strong acid to form \(\mathrm{Cd}^{2+}\) and \(4\mathrm{NH}_{4}^{+}\) ions.

Write balanced net ionic equations

Since the strong acid is completely dissociated in the solution, we only need to include the ions produced by the reaction of the compound with the protons. (a) \(\mathrm{CaF}_{2} + 2\mathrm{H}^{+} \to \mathrm{Ca}^{2+} + 2\mathrm{F}^{-}\) (b) \(\mathrm{CuCO}_{3} + 2\mathrm{H}^{+} \to \mathrm{Cu}^{2+} + \mathrm{H}_{2}\mathrm{O} + \mathrm{CO}_{2}\). Note that since \(\mathrm{CO}_{2}\) is a gas, we include it in the net ionic equation. (c) \(\mathrm{Ti}(\mathrm{OH})_{3} + 3\mathrm{H}^{+} \to \mathrm{Ti}^{3+} + 3\mathrm{H}_{2}\mathrm{O}\) (d) \(\mathrm{Sn}(\mathrm{OH})_{6}^{2-} + 6\mathrm{H}^{+} \to \mathrm{Sn}^{4+} + 6\mathrm{H}_{2}\mathrm{O}\) (e) \(\mathrm{Cd}\left(\mathrm{NH}_{3}\right)_{4}^{2+} + 4\mathrm{H}^{+} \to \mathrm{Cd}^{2+} + 4\mathrm{NH}_{4}^{+}\) These are the balanced net ionic equations for the reactions of each compound with a strong acid.