Question

Write a net ionic equation to show that perchloric acid, hclo4, behaves as an acid in water.

Answer 1

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 is written first.
• The strong electrolytes are break into their respective ions with correct formula and number of ions.
• The common ions on both the sides that is on reactant and product side are cancelled out.
• The resulting equation is a net-ionic equation

The molecular equation between perchloric acid, $HClO_4$ in water, $H_2O$ is:

$HClO_4(aq) + H_2O(l)\rightarrow H_3O^{+}(aq) + ClO_{4}^{-}(aq)$

Breaking the strong electrolytes in their respective ions:

$H^{+}(aq) + ClO_4^{-} (aq) + H_2O(l)\rightarrow H_3O^{+}(aq) + ClO_{4}^{-}(aq)$

Cancelling the common ion, $ClO_{4}^{-}(aq)$ from both the sides:

$H^{+}(aq) + H_2O(l)\rightarrow H_3O^{+}(aq)$

Hence, the net ionic equation between perchloric acid, $HClO_4$ in water, $H_2O$ is:

$H^{+}(aq) + H_2O(l)\rightarrow H_3O^{+}(aq)$

Since, the production of $H_3O^{+}$ takes place so, the perchloric acid, $HClO_4$ acts as an acid by donating proton, $H^{+}$ ion to water.

Answer 2

Answer: 1) Molecular equation: HClO(aq) + H2O(l) → H3O+(aq) + ClO- (aq) 2) ionic equation: H+(aq) + ClO-(aq) + H2O(l) → H3O+(aq) + ClO-(aq) 3) Net Ionic Equation: H+(aq) + H2O(aq) → H3O+(aq) Because the H3O+ ion is produced, HClO acts as an acid in water. Note that ClO- is a spectator ion.