Complete the following acid-base reactions with balanced molecular, total ionic, and net ionic equations:
A) Cesium hydroxide (aq) + nitric acid (aq)
The Correct Answer and Explanation is :
To complete the acid-base reaction between cesium hydroxide (CsOH) and nitric acid (HNO₃), we will go through the steps of writing the balanced molecular equation, the total ionic equation, and the net ionic equation.
1. Balanced Molecular Equation
The balanced molecular equation represents the reactants and products in their molecular forms.
[ \text{CsOH (aq) + HNO}_3 \text{ (aq) } \rightarrow \text{ CsNO}_3 \text{ (aq) + H}_2\text{O (l)} ]
2. Total Ionic Equation
In the total ionic equation, we separate the strong electrolytes into their constituent ions. Both cesium hydroxide and nitric acid are strong electrolytes and dissociate completely in water.
Total Ionic Equation:
[
\text{Cs}^+ \text{(aq) + OH}^- \text{(aq) + H}^+ \text{(aq) + NO}_3^- \text{(aq)} \rightarrow \text{Cs}^+ \text{(aq) + NO}_3^- \text{(aq) + H}_2\text{O (l)}
]
3. Net Ionic Equation
The net ionic equation removes the spectator ions, which do not participate in the actual chemical reaction. In this case, cesium ions ((\text{Cs}^+)) and nitrate ions ((\text{NO}_3^-)) are spectator ions.
Net Ionic Equation:
[
\text{OH}^- \text{(aq) + H}^+ \text{(aq)} \rightarrow \text{H}_2\text{O (l)}
]
Explanation
In this reaction, cesium hydroxide (a strong base) reacts with nitric acid (a strong acid) to form cesium nitrate and water. This is a classic acid-base neutralization reaction, where the hydroxide ion ((\text{OH}^-)) from the base combines with the hydrogen ion ((\text{H}^+)) from the acid to form water ((\text{H}_2\text{O})). The other product, cesium nitrate, remains in aqueous solution as ions.
The balanced molecular equation shows the overall stoichiometry of the reaction, while the total ionic equation emphasizes the ionic nature of the reactants and products. The net ionic equation is particularly important as it highlights the core reaction between the hydroxide and hydrogen ions, effectively demonstrating the essential change occurring during the neutralization process. Understanding these equations is crucial for grasping the concepts of acid-base chemistry, reaction mechanisms, and the behavior of strong electrolytes in solution.