Chemistry

posted by .

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.
Kb:1.7x10^-9

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

  • Chemistry -

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

  • Chemistry -

    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 -

    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.

Respond to this Question

First Name
School Subject
Your Answer

Similar Questions

  1. chemistry

    Captain Kirk, of the Starship Enterprise, has been told by his superiors that only a chemist can be trusted with the combination to the safe containing the dilithium crystals that power the ship. The combination is the pH of Solution …
  2. Chem

    Consider a solution that contains both C5H5N and C5H5NHNO3. (Kb for pyridine, C5H5N, is 4.0 x 10^-4) (a) Calculate the ratio of [C5H5N]/[C5H5NH+] if the solution has a pH of 4.50. (b) Calculate the ratio of [C5H5N]/[C5H5NH+] if the …
  3. chemistry

    A. Strong Base 1.) What is the concentration of a solution of KOH for which the pH is 11.89?
  4. Chemistry

    Use the Henderson-Hasselbalch equation to calculate the pH of each solution: a solution that contains 1.05% C2H5NH2 by mass and 1.10% C2H5NH2Br by mass
  5. Chemistry(Please check, thank you)

    For an experiment on the effect of a buffer solution, I need to calculate the expected pH of the buffer. I know that I have to make an amounts table and use the Hasselbalch equation to find the pH. For the first part, 0.10M HCl was …
  6. Chemistry

    Calculate the pH after 0.013 mole of gaseous HCl is added to 272.0 mL of each of the following buffered solutions. (Assume that all solutions are at 25°C.) (a) 0.080 M C5H5N and 0.19 M C5H5NHCl (b) 0.72 M C5H5N and 1.52 M C5H5NHCl
  7. Chemistry

    WOULD THE VOLUME OF A 0.10M NAOH SOLUTION NEEDED TO TITRATE25.0ML OF A 0.10M HNO2 ( A WEAK ACID)SOLUTION BE DIFFERENT FROMTHAT NEEDED TO TITRATE 25.0ML OF A 0.10M HCL (A STRONGACID)SOLUTION?
  8. chemistry

    use the Henderson-Hasselbalch equation to calculate the pH of a buffer solution prepared by mixing equal volumes of 0.20 M NaHCO3 and 0.10M Na2CO3.(Ka=5.6x10^-11). how would you prepare NaHCO3-Na2CO3 buffer solution that has the pH …
  9. Chemistry

    You have to prepare a pH 3.50 buffer, and you have the following 0.10M solutions available HCOOH, CH3COOH, H3PO4,CHOONa, CH3COONa, and NaH2PO4. a) What solutions would you use?
  10. chemistry

    What is the pH of a 0.2 M solution of pyridinium chloride (C5H5NHCl)?

More Similar Questions