Which of the following could be used to formulate 100 mls of a 0.10 M acetate buffer (pK=4.76) at pH 5 if you start with 64 mls of 0.10 M sodium acetate?

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The Henderson-Hasselbalch equation can be used to calculate the pH of a buffer solution:```pH = pKa + log([A-]/[HA])```where:* pH is the pH of the buffer solution* pKa is the acid dissociation constant of the weak acid* [A-] is the concentration of the conjugate base* [HA] is the concentration of the weak acidIn this case, we want to create a 100 mL buffer solution with a pH of 5.00. We are starting with 64 mL of 0.10 M sodium acetate, which is the conjugate base of acetic acid. We can use the Henderson-Hasselbalch equation to calculate the concentration of acetic acid that we need to add to the solution:```5.00 = 4.76 + log([A-]/[HA])``````log([A-]/[HA]) = 0.24``````[A-]/[HA] = 1.74```This means that we need to add enough acetic acid to the solution so that the ratio of [A-] to [HA] is 1.74. We can do this by adding 34 mL of 0.10 M acetic acid to the solution.

Which of the Following Could Be Used to Formulate 100