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3.41 is the pH value of a sample that has ten times fewer hydronium ions than an equal volume of a vinegar sample with a pH value of 2.4.
Explanation:
pH of the first sample of acetic acid = 2.4
to know the [H+] concentration in the acetic acid solution, the equation used is:
pH = -log [H+]
[H+] =
[H+] =
[H+] = 3.98 X M
The concentration of H+ ion in first case is 3.98 X M, the second sample has ten times less hydronium ion so concentration of first case is divided by 10.
3.98 x M
Now pH of the sample having 10 times fewer ions of acetic acid:
pH = -log [H+]
putting the values in the above equation:
pH = -log [3.98 x M]
pH = 3.41
If solution has ten times less hydronium ion the pH will change to 3.41.