In the laboratory, a general chemistry student measured the pH of a 0.314 M aqueous solution of phenol (a weak acid), C6H5OH to be 5.269. Use the information she obtained to determine the Ka for this acid.

Ka = 9.0974 E-12

Explanation:

∴ Ka =([H3O+]*[C6H5O-])/[C6H5OH]

∴ C C6H5OH = 0.314 M

∴ pH = 5.269 = - Log [H3O+]

⇒ [H3O+] = 5.3827 E-6 M

mass balanced:

⇒ C C6H5OH = 0.314 M = [C6H5O-] + [C6H5OH](1)

charge balanced:

⇒ [H3O+] = [C6H5O-] + [OH-][OH-] is neglected, it comes from the water

⇒ [H3O+] = [C6H5O-](2)

(2) in (1):

⇒ 0.314 M - [H3O+] = [C6H5OH]

⇒ [C6H5OH] = 0.314 M - 5.3827 E-6 M

⇒ [C6H5OH] = 0.31399 M

replacing in Ka:

⇒ Ka = ((5.3827 E-6)*(5.3827 E-6))/(0.31399) = 9.0974 E-12

the answer is c

tell me if wrong