The Kb for an amine is 3.513×10−5. What percentage of the amine is protonated if the pH of a solution of the amine is 9.872 ? Assume that all OH− came from the reaction of B with H2O.
I've been able to figure out how to find the pH and [OH-], but not sure where to go from here. I know that Kb is equal to [BH+][OH-]/[B], but I keep getting the wrong answer when I go to find the % protonated. Any help is appreciated! :)
achieve week 2 question 5
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Charmaine Ho 2G
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