The pH of a 0.10M solution of a weak base is 9.82. What is the value of Kb for this base?

pOH = 14 – 9.82 = 4.18::: [OH-] = 10^-4.18 = 6,7x10E-5

B + H2O = OH- + HB

Kb = [OH-][HB] / [B]: [OH-] = [HB] ::, = [6.7×10^-5]^2 / 0.10 = 4.5x10E-8

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