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Suppose: B- is symbol for any (soluble) base.

Equilibrium of a base when diluted in water:

B- + H2O <==> HB + OH-

Equilibrium constant:

Keq = [HB] * [OH-] / [B-] * [H2O]

The base dissociation contant is defined by:

KB = [HB]*[OH-]/[B-]

So, KB = Keq*[H2O] = Keq*55.6 mol/L

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What is the base dissociation constant for a weak base at equilibrium B H2O BH OH?

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