Answer:
Net ionic: [tex]NH_{4}^{+}(aq.)+H_{2}O(l)\rightarrow NH_{3}(aq.)+H_{3}O^{+}(aq.)[/tex]
Explanation:
Ammonium perchlorate consists of [tex]NH_{4}^{+}[/tex] and [tex]ClO_{4}^{-}[/tex] ions. [tex]NH_{4}^{+}[/tex] is a strong conjugate acid of weak base [tex]NH_{3}[/tex]. [tex]ClO_{4}^{-}[/tex] is an weak conjugate base of strong acid [tex]HClO_{4}[/tex].
So, in case of hydrolysis of [tex]NH_{4}ClO_{4}[/tex], [tex]NH_{4}^{+}[/tex] is only being hydrolyzed to produce [tex]NH_{3}[/tex] and [tex]H_{3}O^{+}[/tex].
Molecular equation: [tex]NH_{4}ClO_{4}(aq.)+H_{2}O(l)\rightarrow NH_{3}(aq.)+H_{3}OClO_{4}(aq.)[/tex]
Total ionic: [tex]NH_{4}^{+}(aq.)+ClO_{4}^{-}(aq.)+H_{2}O(l)\rightarrow NH_{3}(aq.)+H_{3}O^{+}(aq.)+ClO_{4}^{-}(aq.)[/tex]
Net ionic: [tex]NH_{4}^{+}(aq.)+H_{2}O(l)\rightarrow NH_{3}(aq.)+H_{3}O^{+}(aq.)[/tex]
