What is the balanced, net ionic equation for the reaction represented by this equat...
Check the final answer first, then review the worked steps.
Problem
What is the balanced, net ionic equation for the reaction represented by this equation?
Answer
\(H^{+}_{(aq)} + OH^{-}_{(aq)} \rightarrow H_2O_{(l)}\)
Step-by-step solution
1. Write the balanced molecular equation:
The given molecular equation is:
$$HCl_{(aq)} + NaOH_{(aq)} \rightarrow NaCl_{(aq)} + H_2O_{(l)}$$
This equation is already balanced.
2. Write the complete ionic equation:
Break down all soluble ionic compounds into their constituent ions. Strong acids and strong bases dissociate completely in water. Soluble salts also dissociate.
$$H^{+}_{(aq)} + Cl^{-}_{(aq)} + Na^{+}_{(aq)} + OH^{-}_{(aq)} \rightarrow Na^{+}_{(aq)} + Cl^{-}_{(aq)} + H_2O_{(l)}$$
Note that $H_2O$ is a liquid and does not dissociate into ions.
3. Identify and cancel out spectator ions:
Spectator ions are ions that appear on both sides of the equation unchanged. In this reaction, $Na^{+}_{(aq)}$ and $Cl^{-}_{(aq)}$ are spectator ions.
$$H^{+}_{(aq)} + \cancel{Cl^{-}_{(aq)}} + \cancel{Na^{+}_{(aq)}} + OH^{-}_{(aq)} \rightarrow \cancel{Na^{+}_{(aq)}} + \cancel{Cl^{-}_{(aq)}} + H_2O_{(l)}$$
4. Write the net ionic equation:
The net ionic equation includes only the species that participate in the reaction.
$$H^{+}_{(aq)} + OH^{-}_{(aq)} \rightarrow H_2O_{(l)}$$