What is the balanced, net ionic equation for the reaction represented by this equat...
Check the final answer first, then review the worked steps.
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.
$$H^{+}_{(aq)} + OH^{-}_{(aq)} \rightarrow H_2O_{(l)}$$