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

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

Step-by-step 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.)`