Nuetralization Reaction involving a weak acid and weak base

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The discussion centers on the reaction between acetic acid (CH3OOH) and ammonia (NH3), questioning whether it qualifies as a neutralization reaction involving a weak acid and weak base. It is noted that if "neutralization" is defined by achieving a pH of 7, the resulting ammonium acetate would approximate this pH. However, if equimolar acid/base pairs are the criteria, a reaction with sodium bicarbonate would be more appropriate. Concerns are raised about ammonia being a gas, which could lead to improper neutralization. Additionally, the resulting ammonium ion (NH4+) is recognized as a significant acid, suggesting that the reaction could function as a buffer solution rather than a classic neutralization.
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CH3OOH (aq) + NH3 (aq) ‹———› NH4+ (aq) + CH3COO- (aq)

Would the above reaction, involving acetic acid and ammonia qualify as a proper neurtalization reaction involving a weak acid and weak base? Or, would a reaction involving acetic acid and sodium bicarbonate be better?

Regards
 
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It depends on what you understand from "neutralization". If you mean pH=7 point for it, then ammonium acetate will almost just give pH=7 level. If you mean equimolar acid/base pair, then the second one will fit better.

Ammonia is okay, but it is a gas and there is a probablity of improper neutralization.

By the way, welcome to the forum.
 
Probably not. The salt formed through such a reaction will contribute to the pH, NH4 is a significant acid.
 
The above could be treated as a buffer solution, right?
 

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