Question

Write the balanced formula, complete ionic, and net ionic equations for each of the following acid-base reactions. a. \(\mathrm{HNO}_{3}(a q)+\mathrm{Al}(\mathrm{OH})_{3}(s) \rightarrow\) b. \(\mathrm{HC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}(a q)+\mathrm{KOH}(a q) \rightarrow\) c. \(\mathrm{Ca}(\mathrm{OH})_{2}(a q)+\mathrm{HCl}(a q) \rightarrow\)

Short answer

a. Balanced Formula: \(\mathrm{3HNO}_{3}(a q) + \mathrm{Al}(\mathrm{OH})_{3}(s) \rightarrow 3\mathrm{H}_{2}\mathrm{O}(l) + \mathrm{Al}(\mathrm{NO}_{3})_{3}(a q)\) Complete Ionic: \(3\mathrm{H}^{+}(a q) + 3\mathrm{NO}_{3}^{-}(a q) + \mathrm{Al}(\mathrm{OH})_{3}(s) \rightarrow 3\mathrm{H}_{2}\mathrm{O}(l) + \mathrm{Al}^{3+}(a q) + 3\mathrm{NO}_{3}^{-}(a q)\) Net Ionic: \(3\mathrm{H}^{+}(a q) + \mathrm{Al}(\mathrm{OH})_{3}(s) \rightarrow 3\mathrm{H}_{2}\mathrm{O}(l) + \mathrm{Al}^{3+}(a q)\) b. Balanced Formula: \(\mathrm{HC}_{2}\mathrm{H}_{3}\mathrm{O}_{2}(a q) + \mathrm{KOH}(a q) \rightarrow \mathrm{H}_{2}\mathrm{O}(l) + \mathrm{KC}_{2}\mathrm{H}_{3}\mathrm{O}_{2}(a q)\) Complete Ionic: \(\mathrm{H}^{+}(a q) + \mathrm{C}_{2}\mathrm{H}_{3}\mathrm{O}_{2}^{-}(a q) + \mathrm{K}^{+}(a q) + \mathrm{OH}^{-}(a q) \rightarrow \mathrm{H}_{2}\mathrm{O}(l) + \mathrm{K}^{+}(a q) + \mathrm{C}_{2}\mathrm{H}_{3}\mathrm{O}_{2}^{-}(a q)\) Net Ionic: \(\mathrm{H}^{+}(a q) + \mathrm{OH}^{-}(a q) \rightarrow \mathrm{H}_{2}\mathrm{O}(l)\) c. Balanced Formula: \(\mathrm{Ca}(\mathrm{OH})_{2}(a q) + 2\mathrm{HCl}(a q) \rightarrow 2\mathrm{H}_{2}\mathrm{O}(l) + \mathrm{CaCl}_{2}(a q)\) Complete Ionic: \(\mathrm{Ca}^{2+}(a q) + 2\mathrm{OH}^{-}(a q) + 2\mathrm{H}^{+}(a q) + 2\mathrm{Cl}^{-}(a q) \rightarrow 2\mathrm{H}_{2}\mathrm{O}(l) + \mathrm{Ca}^{2+}(a q) + 2\mathrm{Cl}^{-}(a q)\) Net Ionic: \(2\mathrm{H}^{+}(a q) + 2\mathrm{OH}^{-}(a q) \rightarrow 2\mathrm{H}_{2}\mathrm{O}(l)\)

Step-by-step solution

Write the balanced formula equation.

In this reaction, nitric acid \(\mathrm{HNO}_{3}\) reacts with aluminum hydroxide \(\mathrm{Al}(\mathrm{OH})_{3}\). The products of the reaction will be water and an aluminum nitrate salt. Therefore, we have: \(\mathrm{3HNO}_{3}(a q) + \mathrm{Al}(\mathrm{OH})_{3}(s) \rightarrow 3\mathrm{H}_{2}\mathrm{O}(l) + \mathrm{Al}(\mathrm{NO}_{3})_{3}(a q)\)

Write the complete ionic equation.

For the complete ionic equation, we separate the soluble ionic compounds into their respective ions. In this case, we have: \(3\mathrm{H}^{+}(a q) + 3\mathrm{NO}_{3}^{-}(a q) + \mathrm{Al}(\mathrm{OH})_{3}(s) \rightarrow 3\mathrm{H}_{2}\mathrm{O}(l) + \mathrm{Al}^{3+}(a q) + 3\mathrm{NO}_{3}^{-}(a q)\)

Write the net ionic equation.

For the net ionic equation, we cancel out ions that are present on both sides of the equation. In this case, we have: \(3\mathrm{H}^{+}(a q) + \mathrm{Al}(\mathrm{OH})_{3}(s) \rightarrow 3\mathrm{H}_{2}\mathrm{O}(l) + \mathrm{Al}^{3+}(a q)\) Reaction b: \(\mathrm{HC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}(a q)+\mathrm{KOH}(a q) \rightarrow\)

Write the balanced formula equation.

In this reaction, acetic acid \(\mathrm{HC}_{2}\mathrm{H}_{3}\mathrm{O}_{2}\) reacts with potassium hydroxide \(\mathrm{KOH}\). The products of the reaction will be water and a potassium acetate salt. Therefore, we have: \(\mathrm{HC}_{2}\mathrm{H}_{3}\mathrm{O}_{2}(a q) + \mathrm{KOH}(a q) \rightarrow \mathrm{H}_{2}\mathrm{O}(l) + \mathrm{KC}_{2}\mathrm{H}_{3}\mathrm{O}_{2}(a q)\)

Write the complete ionic equation.

For the complete ionic equation, we have: \(\mathrm{H}^{+}(a q) + \mathrm{C}_{2}\mathrm{H}_{3}\mathrm{O}_{2}^{-}(a q) + \mathrm{K}^{+}(a q) + \mathrm{OH}^{-}(a q) \rightarrow \mathrm{H}_{2}\mathrm{O}(l) + \mathrm{K}^{+}(a q) + \mathrm{C}_{2}\mathrm{H}_{3}\mathrm{O}_{2}^{-}(a q)\)

Write the net ionic equation.

For the net ionic equation, we have: \(\mathrm{H}^{+}(a q) + \mathrm{OH}^{-}(a q) \rightarrow \mathrm{H}_{2}\mathrm{O}(l)\) Reaction c: \(\mathrm{Ca}(\mathrm{OH})_{2}(a q)+\mathrm{HCl}(a q) \rightarrow\)

Write the balanced formula equation.

In this reaction, calcium hydroxide \(\mathrm{Ca}(\mathrm{OH})_{2}\) reacts with hydrochloric acid \(\mathrm{HCl}\). The products of the reaction will be water and a calcium chloride salt. Therefore, we have: \(\mathrm{Ca}(\mathrm{OH})_{2}(a q) + 2\mathrm{HCl}(a q) \rightarrow 2\mathrm{H}_{2}\mathrm{O}(l) + \mathrm{CaCl}_{2}(a q)\)

Write the complete ionic equation.

For the complete ionic equation, we have: \(\mathrm{Ca}^{2+}(a q) + 2\mathrm{OH}^{-}(a q) + 2\mathrm{H}^{+}(a q) + 2\mathrm{Cl}^{-}(a q) \rightarrow 2\mathrm{H}_{2}\mathrm{O}(l) + \mathrm{Ca}^{2+}(a q) + 2\mathrm{Cl}^{-}(a q)\)

Write the net ionic equation.

For the net ionic equation, we have: \(2\mathrm{H}^{+}(a q) + 2\mathrm{OH}^{-}(a q) \rightarrow 2\mathrm{H}_{2}\mathrm{O}(l)\)