What is the ratio of acetic acid to acetate ion in solutions at ph 4, 6, 9 if the pka of acetate is 4.8?

At pH = 4, [Acetic acid]/[Acetate ion] = 6.3096

At pH = 6, [Acetic acid]/[Acetate ion] = 0.0631

At pH = 9, [Acetic acid]/[Acetate ion] = 6.3096×10⁻⁵

Explanation:

The pH of a buffer solution is calculated using Henderson Hasselbalch equation. The expression for the equation is:

For, Acetic acid (pKa = 4.8), Acetate will be its conjugate base.

To calculate the ratio of acetic acid and acetate ion in the solution.

Using the property of log that:

log(a/b) = -log(b/a)

The equation can be written as:

For pH =4 :

Thus, Taking anti log and solving as:

[Acetic acid]/[Acetate ion] = 6.3096

For pH =6 :

Thus, Taking anti log and solving as:

[Acetic acid]/[Acetate ion] = 0.0631

For pH =9 :

Thus, Taking anti log and solving as:

[Acetic acid]/[Acetate ion] = 6.3096×10⁻⁵

bcde is the incorrect answer it is a