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Methylamine, CH3NH4, is a weak base. A 0.504 M solution of methylamine has equilibrium concentrations of...

Methylamine, CH3NH4, is a weak base. A 0.504 M solution of methylamine has equilibrium concentrations of both CH3NH3^+ and OH^- equal to 0.0150 M. What is the Kb of the base?
CH3NH2(aq) + H2O(l) <> CH3NH3^+(aq) + OH^-(aq)
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Answer #1

----- CH3NH2(aq) + H2O(l) <> CH3NH3^+(aq) + OH^-(aq)

I ----- 0.504 --------------------------- 0 ------------- 0

C ----- -0.015 ----------------------- +0.015 ------- +0.015

E ------ 0.489------------------------- +0.015 ----- + 0.015

      Kb    =   [CH3NH3^+][OH^-]/[{CH3NH2]

                  = 0.015*0.015/0.489

                     = 4.6*10^-4

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