About 16 % of the acid in a 0.10 M solution of a weak acid dissociates to form ions. 1. What is the OH? concentration? Express your answer using two significant figures. 2.What is the pH of the solution? Express your answer using two decimal places. Solution Let the weak acid be HA It dissociates as: HA <—> H+  +  A- [H+] = 16 % of [A] = 16*0.10/100 = 0.016 M 1) use: [OH-] = Kw/[H+] Kw is dissociation constant of water whose value is 1.0*10^-14 at 25 oC [OH-] = (1.0*10^-14)/[H+] [OH-] = (1.0*10^-14)/(1.6*10^-2) [OH-] = 6.25*10^-13 M Answer: 6.25*10^-13 M 2) use: pH = -log [H+] = -log (1.6*10^-2) = 1.80 Answer: 1.80 .