What concentrations of acetic acid (pKa = 4.76) and acetate would be required to

Question

What concentrations of acetic acid (pKa = 4.76) and acetate would be required to prepare a 0.15 M buffer solution at pH 4.5? Rearrange the Henderson-Hasselbalch equation to solve for the ratio of base (acetate) to add (acetic acid), [A^-1]/[HA]. Use the mole fraction of acetate to calculate the concentration of acetate. Calculate the concentration of acetic acid. Step 1: Rearrange the Henderson Hasselbalch equation to solve for [A^-]/[HA] The Henderson-Hasselbalch equation is pH = p k_a + log [A^-]/[HA] if the solution is at pH 4.5.

Explanation / Answer

pKa for acetic acid = 4.75

4.5 = 4.75 + log [A-/HA]

log [A-/HA] = 4.5 / 4.75

log [A-/HA] = 0.9474

[A-/HA] = 100.9474 = 8.858

[A-/HA] = 8.86

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