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Posted by on Friday, March 22, 2013 at 9:45pm.

Calculate the pH of a solution that is 2.00M HF, 1.00M NaOH, and 0.393M NaG (Ka=7.2 x10^-4).

The answer I got was 4.76 ..

  • Chemistry - , Friday, March 22, 2013 at 10:24pm

    What in the world is NaG? Could that be NaF? If so, did you use Henderson-Hasselbalch equation and adjust it for the 1.00 M NaOH? And how much NaOH was added.

  • Chemistry - , Friday, March 22, 2013 at 10:30pm

    Sorry typo..it's NaF and it doesn't say how much was added that's the question given

  • Chemistry - , Friday, March 22, 2013 at 11:03pm

    I would do this.
    2.00M HF = 1.00M NaOH gives 1.00M NaF and leaves 1.00 M HF.
    1.00N NaF + 0.393M = 1.393M
    pH = pKa + log(base)/(acid)
    I get something like 3.28.

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