Question

the following reaction takes place in aqueous solution. hcl (aq) + koh(aq) → kcl(aq) + h₂o(l) write the balanced net ionic equation for this reaction. be sure to include the proper phases for all species within the reaction.

Explanation:

Step1: Write the complete ionic equation

HCl is a strong acid and dissociates completely in water: $HCl(aq)
ightarrow H^{+}(aq)+Cl^{-}(aq)$. KOH is a strong base and dissociates completely: $KOH(aq)
ightarrow K^{+}(aq)+OH^{-}(aq)$. KCl is a soluble salt and dissociates: $KCl(aq)
ightarrow K^{+}(aq)+Cl^{-}(aq)$. The complete ionic equation is $H^{+}(aq)+Cl^{-}(aq)+K^{+}(aq)+OH^{-}(aq)
ightarrow K^{+}(aq)+Cl^{-}(aq)+H_{2}O(l)$.

Step2: Identify and cancel out spectator ions

Spectator ions are ions that appear on both sides of the equation. Here, $K^{+}(aq)$ and $Cl^{-}(aq)$ are spectator ions. After canceling them out, we get the net - ionic equation.

Answer:

$H^{+}(aq)+OH^{-}(aq)
ightarrow H_{2}O(l)$