Write euations to show how a buffer made up of equimolar amounts of acetic acid, CH3COOH, and acetate, CH3COO-, would behave when (a) HCl was added and (b) NaOH was added.
Is this right,If not what is the correct way?
CH3COOH + HCl ----> CH3COOHCl + OH
CH3COO + NaOH ----> CH3COOHNa + H2O
Not all right but the right idea.
When a strong base is added (such as NaOH) it reacts with the weak acid (CH3COOH) of the buffer.
CH3COOH + NaOH ==> CH3COONa + H2O
When an strong acid (such as HCl) is added, it reacts with the weak base of the buffer (CH3COO^-).
CH3COO^- + HCl ==> CH3COOH + Cl^-
No, the equations you provided are not correct. Here are the correct equations to show the behavior of the equimolar buffer solution when HCl and NaOH are added:
(a) When HCl is added:
CH3COOH + HCl -> CH3COOH2+ + Cl-
In this reaction, the acetic acid (CH3COOH) reacts with the HCl to form the hydronium ion (CH3COOH2+) and chloride ion (Cl-). The buffer system will help to minimize the change in pH by absorbing some of the added H+ (from HCl) through the formation of the hydronium ion.
(b) When NaOH is added:
CH3COO- + NaOH -> CH3COONa + H2O
In this reaction, the acetate ion (CH3COO-) reacts with the NaOH to form sodium acetate (CH3COONa) and water (H2O). The buffer system will help to minimize the change in pH by absorbing some of the added OH- (from NaOH) through the formation of water.
These equations describe the behavior of the equimolar buffer solution when HCl and NaOH are added.
The equations you have written are close, but there are a couple of errors. Let's correct them:
(a) When HCl is added to a buffer solution containing acetic acid (CH3COOH) and acetate (CH3COO-):
CH3COOH + HCl ----> CH3COOH2+ + Cl-
In this reaction, the acetic acid donates a proton (H+) to the chloride ion (Cl-), forming hydronium (H3O+) and chloride (Cl-) ions.
(b) When NaOH is added to a buffer solution containing acetic acid (CH3COOH) and acetate (CH3COO-):
CH3COO- + NaOH ----> CH3COONa + H2O
In this reaction, the acetate ion (CH3COO-) reacts with hydroxide ion (OH-) from sodium hydroxide (NaOH) to form sodium acetate (CH3COONa) and water (H2O).
It's important to note that in both cases, the acetic acid remains mostly undissociated and maintains the buffer's pH by reacting with the added acid or base and helping to resist changes in the overall pH of the solution.