Nuetralization Reaction involving a weak acid and weak base

In summary, the conversation discusses a neutralization reaction involving acetic acid and ammonia. It is debated whether this qualifies as a proper neutralization reaction, with one participant mentioning the possibility of improper neutralization due to the gaseous nature of ammonia. Another participant suggests that the resulting salt, ammonium acetate, may contribute to the pH and could be treated as a buffer solution.
  • #1
JM_BC
1
0
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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  • #2
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.
 
  • #3
Probably not. The salt formed through such a reaction will contribute to the pH, NH4 is a significant acid.
 
  • #4
The above could be treated as a buffer solution, right?
 
H2What is a neutralization reaction involving a weak acid and weak base?

A neutralization reaction involving a weak acid and weak base is a chemical reaction in which an acid and a base react with each other to form a salt and water. In this type of reaction, the acid and base are both weak, meaning they do not completely dissociate into ions in solution.

H2What are some examples of weak acids and weak bases?

Examples of weak acids include acetic acid (vinegar), citric acid (found in citrus fruits), and carbonic acid (found in carbonated drinks). Some examples of weak bases include ammonia, baking soda, and antacids.

H2How is the strength of a weak acid or base determined?

The strength of a weak acid or base can be determined by its acid dissociation constant (Ka) or base dissociation constant (Kb). These values represent the extent to which the acid or base dissociates into ions in solution. A larger Ka or Kb value indicates a stronger acid or base, while a smaller value indicates a weaker acid or base.

H2What factors can affect the strength of a neutralization reaction involving a weak acid and weak base?

The strength of a neutralization reaction can be affected by the concentration of the acid and base, the temperature of the reaction, and the presence of any catalysts or inhibitors. Additionally, the strength of the weak acid and weak base themselves can impact the strength of the reaction.

H2What is the pH of the resulting solution after a neutralization reaction involving a weak acid and weak base?

The pH of the resulting solution after a neutralization reaction involving a weak acid and weak base will depend on the strength of the acid and base, as well as the initial concentrations of each. If the acid and base are equally strong, the resulting solution will have a neutral pH of 7. If one is stronger than the other, the resulting solution may be slightly acidic or basic.

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