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Posted by on Monday, April 1, 2013 at 8:36pm.

use the Hendeson-Hasselbalch equatio. To calculator the pH of a solution at is
A) 0.15 M on C5H5N and 0.10M in C5H5NHCl.

B) 15.0 g of HF and 25.0g of NaFin 125 ml of a solution.
Ka 3.5x10^-4

  • Chemistry - , Monday, April 1, 2013 at 9:37pm

    What's the problem. Just plug and chug.
    pH = pKa + log (base)/(acid)

  • Chemistry - , Monday, April 1, 2013 at 10:12pm

    I guess I am still stuck on problem a. I know I have to calculate Ka from Kb in order to calculate pH. When I do that, I get a pH over 14 which cannot be. What am I doing wrong?

  • Chemistry - , Monday, April 1, 2013 at 11:59pm

    Here is what I would do. Convert Kb to pKb. That is pKb = -logKb = -log 1.7E-9 = 8.77, then
    pKa + pKb = pKw. You know pKw and pKb, solve for pKa.

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