Question

Write the net ionic equation for the acid-base hydrolysis equilibrium that is established when ammonium perchlorate is dissolved in water. (Use H3O instead of H .)

Answer 1

Answer:

Net ionic: $NH_{4}^{+}(aq.)+H_{2}O(l)\rightarrow NH_{3}(aq.)+H_{3}O^{+}(aq.)$

Explanation:

Ammonium perchlorate consists of $NH_{4}^{+}$ and $ClO_{4}^{-}$ ions.  $NH_{4}^{+}$ is a strong conjugate acid of weak base $NH_{3}$. $ClO_{4}^{-}$ is an weak conjugate base of strong acid $HClO_{4}$.

So, in case of hydrolysis of $NH_{4}ClO_{4}$,  $NH_{4}^{+}$ is only being hydrolyzed to produce $NH_{3}$ and $H_{3}O^{+}$.

Molecular equation: $NH_{4}ClO_{4}(aq.)+H_{2}O(l)\rightarrow NH_{3}(aq.)+H_{3}OClO_{4}(aq.)$

Total ionic: $NH_{4}^{+}(aq.)+ClO_{4}^{-}(aq.)+H_{2}O(l)\rightarrow NH_{3}(aq.)+H_{3}O^{+}(aq.)+ClO_{4}^{-}(aq.)$

Net ionic: $NH_{4}^{+}(aq.)+H_{2}O(l)\rightarrow NH_{3}(aq.)+H_{3}O^{+}(aq.)$