•0.336 moles of a weak, monoproticacid added to a final volume of 2.00 L exhibits 2.14% ionization. What is the pOH of the solution? 11.56 is the answer please explain steps Solution The equation for the dissociation of HA is: HAc H+ + A¯ Molarity = 0.336/2 = 0.168 M 1) Find [H+] using the concentration and the percent dissociation: (0.0214) (0.168) = 3.595 x 10¯3 M 2) pH = -log [H+] = -log (3.595 x 10¯3) = 2.44 3) pH + pOH = 14 pOH = 14 -2.44 = 11.56.