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OpenStudy (anonymous):
A certain weak base has a Kb of 8.50 × 10-7. What concentration of this base will produce a pH of 10.38?
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OpenStudy (mstv1112):
pH = 10.05 pOH = 3.95 [OH-] = 10^-pOH = 10^-3.95 = 0.00011220 M B + H2O <==> HB+ + OH- Kb = ([HB+] [OH-]) / [B] 8.50 x 10^-7 = [(1.122 x 10^-4) (1.122 x 10^-4)] / x x = 0.0148 M I found this on Answers.com
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