Ka vs Kb
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Ka vs Kb
Going off of Dr. Lavelle's example in the review lecture this week, how do you determine whether the reaction you are observing has a Ka or Kb value?
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Re: Ka vs Kb
You can just look at the species that is disassociating! If the species that is disassociating is an acid like in the example (ie. produces hydronium ions), then it has a Ka value (which can be calculated using its conjugate base's Kb value). Likewise, if the species that is disassociating is a base (ie. produces hydroxide ions), then it has a Kb value (that can be calculated using its conjugate acid's Ka value). Hope this helps!
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Re: Ka vs Kb
Usually Ka is associated with acids and Kb with bases. If you need to convert between the two, just use the equation Ka x Kb = Kw = 1x10^-14
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Re: Ka vs Kb
Adding on, I believe if the equilibrium expression written has [H3O+] or [H+] in the numerator, its a ka expression since its generating H+ in solution, and if it has an [OH-] its a kb expression since its generating OH- in solution.
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