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So Ka would be calculated for a compound by studying its equilibrium concentrations as if it were an acid, and Kb would be calculated for the conjugate base of that acid and its reaction is what I'm getting. Like the example with NH3 and NH4+ we did in lecture.
KB and KA are calculated the same way. From what I gathered from the lecture, KB has to do with the equilibrium constant of bases and has [OH-] as a product. Conversely, KA has to do with the equilibrium constant of acids and has [H3O+] as a product. That's the extent to how much they differ.
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