# “determine how many ml of solution a (acetic acid-indicator solution)

“determine how many ml of solution a (acetic acid-indicator solution).

“Determine how many mL of solution A (acetic acid-indicator solution) must be added to solution B (sodium acetate-indicator solution) to obtain a buffer solution that is equimolar in acetate and acetic acid. You ill need to refer to the Experimental Procedure, particularly the section on calculations, to answer this question.

Solution A:

10.0 mL 3.0e-4M bromescol green solution

25.0mL 1.60M acetic acid (HAc)

10.0mL .200M KCl solution

Solution B: 10.0mL 3.0e-4M bromescol green solution

10.0mL of .160M sodiuma cetate solution

a.Calculate moles Ac- in solution B

b. Calculate the molarity of HAc in solution A.

c. Calculate the volume of solution A needed when the moles of Ac- equals moles of HAc

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K HAc is approximately 2e-5 under your experimental conditions. Use pK HAc = pH + log(N HAc/ N Ac-)

a. Calculate pKa

b. calculate moles HAc in 5mL solution A added to solution B

c.Calculate moles Ac- in solution B

d. Rearrange equation to solve for pH”

“determine how many ml of solution a (acetic acid-indicator solution)