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

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Tiffany Chao 2H
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Joined: Fri Aug 09, 2019 12:17 am

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

Postby Tiffany Chao 2H » Sun Dec 01, 2019 8:33 pm

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
Posts: 113
Joined: Thu Jul 11, 2019 12:16 am

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

Postby Robin Cadd 1D » Mon Dec 02, 2019 9:06 am

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

Postby Ariel Davydov 1C » Mon Dec 02, 2019 9:48 am

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.


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