A buffer solution is prepared by mixing 1.00 L of 0.050 M pentafluorobenzoic acid (C6F5COOH) and 1.00 L of 0.060 M sodium pentafluorobenzoate (NaC6F5COO). The Ka of this weak acid is 0.033. Determine the pH of the buffer solution.

pH = 1.401

Explanation:

Using The Henderson-Hasselbalch Equation

pH = pKa + log [base] / [acid]

Ka = 0.033

pKa = -log Ka

pKa = -log 0.033

pKa = 1.48

[base] = concentration of congugate base = 0.060 M

[acid] = concentration of Acid = 0.050 M

pH = pKa + log([base] / [acid])

pH = 1.48 + log (0.050 / 0.060)

pH = 1.48 + log 0.83

pH = 1.48 - 0.079

pH = 1.401

the pH of the buffer solution is 1.401

i would say b

explanation:

but i think i would need more information than that

the correct answer is b. a strong acid completely dissociates to its ions when dissolved in water. completely dissociates to and ions. a is incorrect because does not fully ionize to and ions and some remain as the compound . c and d are incorrect because, and do not fall into the category of bronsted lowry acids. a bronsted lowry acid is a proton donor and since both molecules do not have a proton to donate they are not bronsted lowry acids. likewise,   if we use the lewis acid definition, they cannot be acids. a lewis acid is an electron pair acceptor. both and have a complete octet so can not accept any electrons which disqualifies them as acids.