Question

A 1.25 M solution of the weak acid HA is 9.2% dissociated. What is the pH...

A 1.25 M solution of the weak acid HA is 9.2% dissociated. What is the pH of the solution?

Homework Answers

Answer #1

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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