PLEASE HELP!!! The Kb of pyridine, C5H5N, is 1.5 x 10-9. Calculate the pH of a solution of 0.157 M pyridine.?

3 Answers

• C5H5N in water --> C5H5NH+ & OH-

  Kb = [C5H5NH+] [OH-] / [C5H5N]

  1.5e-9 = [x] [x] / [0.157]

  X2 = 2.355e-10

  x = = [OH-] = 1.53e-5 molar

  pOH = 4.81

  14 - pOH = pH

  your answer = 9.19

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  PLEASE HELP!!! The Kb of pyridine, C5H5N, is 1.5 x 10-9. Calculate the pH of a solution of 0.157 M pyridine.?

  The Kb of pyridine, C5H5N, is 1.5 x 10-9. Calculate the pH of a solution of 0.157 M pyridine.

  Work Plz.

  THANKS!

• Kb Of Pyridine