For J. 9., when do we separate H+ from the acid?

[Tiffany Chao 2H]

J. 9. says: Identify the salt that is produced from the acid–base neutralization reaction between (a) potassium hydroxide and acetic acid,
CH 3 COOH; (b) ammonia and phosphoric acid; (c) calcium
hydroxide and bromous acid; (d) sodium hydroxide and hydrosulfuric acid, H2S (both H atoms react). Write the complete ionic
equation for each reaction.

I've noticed in the answer key, the ionic equation sometimes separates H+ from the acid on the reactant side and sometimes it leaves the acid as it is. Is there a reason why?

[Robin Cadd 1D]

I don't have the textbook on me at the moment, but I'd assume it probably has something to do with the strength of the acid.

[Ariel Davydov 1C]

If an acid or base is strong, it will entirely ionize in solution. Thus, if the problem has a strong acid or base as a part of the equation, it must be written out in dissociated form (ex: HBr would be written as H+ and Br-). If the acid is weak (ex: CH3COOH, acetic acid), it does not entirely ionize in solution, so it must be written as unionized.