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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

  • Chemistry -

    Use the Henderson-Hasselbalch equation. F^- is the base; HF is the acid.

  • Chemistry -

    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

  • Chemistry -

    never mind i understand where you were getting at thanks

  • Chemistry -

    OK but just to make sure let me point out that (NaF) = (F^-) = (base)

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