Answer :

Final answer:

The pH of a solution of 0.65 M acetic acid is approximately 0.19.

Explanation:

To calculate the pH of a solution of 0.65 M acetic acid, we need to consider its dissociation constant (Ka) and the initial concentration of the acid.

The dissociation constant (Ka) for acetic acid is approximately 1.8 x 10^-5.

Since acetic acid is a weak acid, it only partially dissociates in water. This means that not all of the acetic acid molecules will dissociate into hydrogen ions (H+) and acetate ions (CH3COO-).

To calculate the pH, we can use the equation:

pH = -log10[H+]

First, we need to calculate the concentration of hydrogen ions (H+) in the solution. Since acetic acid partially dissociates, we can assume that the concentration of hydrogen ions is equal to the concentration of the acid that dissociates.

Therefore, the concentration of hydrogen ions (H+) in the solution is 0.65 M.

Using the equation pH = -log10[H+], we can calculate the pH:

pH = -log10(0.65)

pH ≈ 0.19

Therefore, the pH of a solution of 0.65 M acetic acid is approximately 0.19.

Learn more about calculating the ph of a solution of acetic acid here:

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