A 1.25 M solution of the weak acid HA is 9.2% dissociated. What is the pH of the solution?
HA
H+ + A-
concentration of weak acid is 1.25 M, and it dissociates 9.2%, then
9.2% of the starting acid is now in the form of H+ and A-. Further,
the concentrations of H+ and A- are equal to [1.25M X 0.092] =
0.115 M.
pH = -log[H+]
pH = -log(0.115)
= 0.94
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