Write the balanced net ionic equations for the reaction of a) added H+ and B) added OH- with the components of the acetic acid/sodium acetate buffer solution:
H^+ reacts with the acetate ion to form CH3COOH (acetic acid).
OH^- reacts with the acetic acid to form H2O and acetate ion.
To write the balanced net ionic equations for the reaction of H+ and OH- with the components of the acetic acid/sodium acetate buffer solution, we first need to understand the components involved in the buffer solution and their properties.
The acetic acid/sodium acetate buffer solution consists of acetic acid (CH3COOH) and its conjugate base, acetate (CH3COO-), in the presence of water. Acetic acid can donate a proton (H+) to form its conjugate base, acetate ion (CH3COO-). In an aqueous solution, acetic acid partially dissociates into H+ and CH3COO-. On the other hand, sodium acetate dissociates completely into sodium ions (Na+) and acetate ions (CH3COO-) in the solution.
Now, let's look at the reactions when H+ (added acid) is introduced and when OH- (added base) is introduced:
A) Reaction with H+ (added acid):
When H+ is added to the buffer solution, it reacts with the acetate ions to form acetic acid. The balanced net ionic equation for this reaction is:
CH3COO- (aq) + H+ (aq) → CH3COOH (aq)
B) Reaction with OH- (added base):
When OH- is added to the buffer solution, it reacts with the acetic acid to form water. The balanced net ionic equation for this reaction is:
CH3COOH (aq) + OH- (aq) → H2O (l) + CH3COO- (aq)
In both cases, the acetate ion (CH3COO-) acts as a conjugate base and reacts to neutralize the added acid (H+) or base (OH-), maintaining the pH of the buffer solution.
Remember, these balanced net ionic equations are written by considering only the species that are involved in the reaction and omitting the spectator ions (ions that do not directly participate in the reaction).