A chemical equation that lists those species only which are participating in the reaction is said to be a net-ionic equation. It is commonly used in double-displacement reactions, acid-base neutralization reactions, and redox reactions.
In order to write the net ionic equation:
The molecular equation between perchloric acid, [tex]HClO_4[/tex] in water, [tex]H_2O[/tex] is:
[tex]HClO_4(aq) + H_2O(l)\rightarrow H_3O^{+}(aq) + ClO_{4}^{-}(aq)[/tex]
Breaking the strong electrolytes in their respective ions:
[tex]H^{+}(aq) + ClO_4^{-} (aq) + H_2O(l)\rightarrow H_3O^{+}(aq) + ClO_{4}^{-}(aq)[/tex]
Cancelling the common ion, [tex]ClO_{4}^{-}(aq)[/tex] from both the sides:
[tex]H^{+}(aq) + H_2O(l)\rightarrow H_3O^{+}(aq)[/tex]
Hence, the net ionic equation between perchloric acid, [tex]HClO_4[/tex] in water, [tex]H_2O[/tex] is:
[tex]H^{+}(aq) + H_2O(l)\rightarrow H_3O^{+}(aq)[/tex]
Since, the production of [tex]H_3O^{+}[/tex] takes place so, the perchloric acid, [tex]HClO_4[/tex] acts as an acid by donating proton, [tex]H^{+}[/tex] ion to water.
