“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
————————————————————
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)

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