Answer :
The pH of a 0.100M solution of HF is approximately 2.17.
The pH of a solution can be determined using the equation pH = -log[H+], where [H+] represents the concentration of hydrogen ions in the solution.
To find the pH of a 0.100M solution of HF, we need to calculate the concentration of hydrogen ions using the given Ka value.
Since HF is a weak acid, it partially dissociates in water, so we can assume that the concentration of [H+] is equal to the concentration of HF that dissociates.
Applying the formula for weak acids, we can solve for [H+]:
Ka = [H+][F-] / [HF]
Substituting the known values, we have:
6.8x10^-4 = [H+] x [0.100] / [0.100]
Simplifying the equation gives us:
[H+] = 6.8x10^-4 M
Finally, we can calculate the pH using the equation:
pH = -log(6.8x10^-4)
Using a calculator, we find that the pH is approximately 2.17.
Therefore, none of the given options (1.78, 1.69, 2.08, 5.26) are correct.
Learn more about the topic of pH here: https://brainly.com/question/2288405
#SPJ11
