The base hydrazine, N2H4, has a pKb equal to 5.90. Calculate the hydroxide concentration, the pH, and the % ionization for a 0.12 M solution. First, is pKb the same as the pOH? If so, pOH = -log[OH-] 5.90 = -log[OH-] log[OH-] = -5.90 =10^-5.90 [OH-]=1.26 x 10^-6 pH = 14.00 - pOH =14.00 - 5.90 =8.10 % ionized = [OH-]/0.12 M X 100% = 0.00105% ? Somehow I think I'm doing this problem wrong. Can anybody show me what the problem is?