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OpenStudy (anonymous):
enough of a monoprotic acid is dissolved in water to produce a 0.0111M solution. The pH of the resulting solution is 2.62. Calculate Ka for the acid.
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OpenStudy (aaronq):
Henderson-Hasselbach equation! pH=pKa-log[A-]/[HA]
OpenStudy (aaronq):
sorry it's +log
OpenStudy (anonymous):
I'm sorry, can you please show me the step with the numbers? I'm not quite used to doing these kind of equation...
OpenStudy (aaronq):
dude i haven't done these in a while, would you mind if i just sent you a vid and you can figure it out?
OpenStudy (anonymous):
sure, anything would do, thanks!
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OpenStudy (aaronq):
sorry you don't even need that equation, here you go though http://www.youtube.com/watch?v=OA-f_8F5iNU
OpenStudy (anonymous):
thanks!
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