The pH of a mixture of 0.25 m acetic acid (CH3COOH) and 0.1 m sodium acetate (CH3COO- Na ) in a total volume of 1 l is 4.37.
The above situation represents a case of buffer solution.
Buffer solutions are those solutions that can resist change in their pH if any acid or base is added to them.
To calculate the pH of a buffer solution, the Henderson-Hasselbalch equation is used
pH = pKa + log [Salt]/[Acid]
Putting
pKa = 4.76
[Salt] = Concentration of sodium acetate = 0.1 M
[Acid] = Concentration of acetic acid = 0.25 M
pH = 4.76 + log [0.1]/[0.25]
pH = 4.76 + log[0.4]
pH = 4.76 - 0.39
pH = 4.37
Hence, the pH of a mixture of 0.25 m acetic acid (ch3cooh) and 0.1 m sodium acetate (ch3coo- na ) in a total volume of 1 l is 4.37.
To know more about "buffer solution", refer to the link given below:
https://brainly.com/question/24262133?referrer=searchResults
#SPJ4
