Answer:
This solution acts as an efficient buffer
Explanation:
the pH of a buffer solution can be described like this: [tex]pH=pKa+log\frac{[base]}{[acid]}[/tex]
[acid]=[acetic acid]=[tex]1mL.\frac{12mol}{1000mL} . \frac{1}{1L} = 0.012M[/tex]
[base]=[sodium acetate]=[tex]0.82g.\frac{1mol}{82g} .\frac{1}{1l} = 0.01M[/tex]
replacing, [tex]pH=4.76+log\frac{0.01M}{0.012M} =4.84[/tex]
If we add an acid, pH will decrease a little bit and if we add a base, pH wil increase a little bit.
lets supose that we change the rate by increasing [base] to 0.1, then
[tex]pH=4,76+log\frac{0.1}{0.012} = 5.68[/tex]
and now lets supose that we increase [acid] to 0.1 [tex]pH=4.76+log\frac{0.01}{0.1} = 3.76[/tex]
Big changes in concentration of base or acid doesn´t produce big changes in pH, in that way the mix of sodium acetate with acetic acid is a good buffer solution.
