posted by Chris on .
consider 1.0 L of a solution which is 0.55 M HF and 0.2 M NaF (Ka for HF = 7.2 x 10-4), Calculate the pH of this solution
Use the Henderson-Hasselbalch equation. F^- is the base; HF is the acid.
do i have to account for the NaF, when plugging in the concentration for F^-. The reason im confused is because they are both weak in respect to their acidity and base that wont allow them to dissociate and i don't really know where to go from there
never mind i understand where you were getting at thanks
OK but just to make sure let me point out that (NaF) = (F^-) = (base)