Problem 50 - Chemistry: An Atoms-Focused Approach

Question

Write the net ionic equation for the neutralization of a strong acid by a strong base.

Step-by-Step Solution

Answer

Answer: H⁺(aq) + OH⁻(aq) -> H2O(l)

Step 1: Write the balanced molecular equation

For the neutralization of a strong acid and a strong base, we can use hydrogen chloride (HCl) as the strong acid and sodium hydroxide (NaOH) as the strong base. The balanced molecular equation is: HCl + NaOH -> NaCl + H2O

Step 2: Write the complete ionic equation

Since strong acids and strong bases ionize in water, the complete ionic equation involves representing each ionized species in aqueous solutions: HCl -> H^{+}(aq) + Cl^{-}(aq) NaOH -> Na^{+}(aq) + OH^{-}(aq) Replace these species in the balanced molecular equation, resulting in: H^{+}(aq) + Cl^{-}(aq) + Na^{+}(aq) + OH^{-}(aq) -> Na^{+}(aq) + Cl^{-}(aq) + H2O(l)

Step 3: Identify and cancel spectator ions

Spectator ions are ions that appear on both sides of the equation and do not participate in the reaction. In this case, Na^{+}(aq) and Cl^{-}(aq) are spectator ions. Cancel out the spectator ions to obtain the net ionic equation: H^{+}(aq) + OH^{-}(aq) -> H2O(l)

Step 4: Write the final net ionic equation

Our final net ionic equation for the neutralization of a strong acid by a strong base is: H^{+}(aq) + OH^{-}(aq) -> H2O(l)