A 4.00 10-2 M solution of unknown monoprotic weak base has a pH of 9.500. What is the value of Kb for the base?|||pOH = 14 - 9.500= 4.500
[OH-]= 10^-4.500 =3.16 x 10^-5 M
BOH %26lt;=%26gt; B+ + OH-
[B+]= [OH-]
Kb = [B+][OH-]/ 4.00 x 10^-2 - 3.16 x 10^-5 = 2.50 x 10^-7
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