Chemistry

posted by .

What is the pH of a solution that is .060M in potassium propionic and .085M in propionic acid?
Ka=1.3E-5 for the acid.

The answer is +4.73 but I don't know how to go about the problem. I thought that the potassium propionic was reacting with the acid to form their conjugate acid and base but I wa told that the acid would be reacting with water and dissociate forming the ions of the acid. I'm not sure how this works.

  • Chemistry -

    Use the Henderson-Hasselbalch equation. That's what you use for buffers.
    pH = pKa + log (base)/(acid)
    The base is the K salt and the acid is propionic acid.

Respond to this Question

First Name
School Subject
Your Answer

Similar Questions

  1. Chemistry

    What is the pH of a buffer solution that is 0.15 M propionic acid and 0.20M sodium propionate?
  2. Chemistry

    Calculate the pH of a solution that is 0.060 M in potassium propionate(C2H5COOK or KC3H5O2) and 0.085 M in propionic acid (C2H5COOH or HC3H5O2)
  3. chemistry

    A 625mL sample of an aqueous solution containing 0.275 mol propionic acid (CH3CH2CO2H),has [H30+]= 0.00239M. What is the value of Ka for propionic acid?
  4. chemistry

    1. if 15.0mL of 4.5 M NaOH are diluted with water to a volume of 500mL, what is the molarity of the resulting solution?
  5. Chemistry

    calculate the pH and the propionate ion concentration [c3h502-] of a solution that is .06M in potassium propionate [kc3h502] and .085M in propionic acid [hc3h502]
  6. Chemistry

    Calculate the pH at the equivalence point when 50 mL of 0.098 M propionic acid is titrated with 0.340 M NaOH. I tried solving for the volume of NaOH and them using the total volume and then plugging it in to [H+][A-]/[HA] and used …
  7. chemistry

    Propionic acid has a ka of 1.3x10^(-5), 50.0ml of a buffer solution having a pH of 4.65 is to be prepared using a 0.20 M solutions of propionic acid and sodium propionate. How many ml of each of these solutions must be mixed?
  8. Chemistry

    I am trying to solve a buffer problem. I know I need to use the Henderson-Hasselblach equation but I am not getting the correct answer. The problem is: Propionic acid is a weak monoprotic acid with Ka = 1.3×10-5 M. NaOH(s) was gradually …
  9. Cara-Chem

    I made a bobo, which may lead to some confusion. Here is my post revised: You don't need it. Just calculate the new molarity of the acid after addition of NaOH, and then determine the molarity of the acid in solution. How many moles …
  10. Bio chem

    How many mL of 0.80 molar NaOH must be added to 20 ml of 0.40 of molar propionic acid, in order to produce a solution with a pH of 4.89?

More Similar Questions