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You have 275 mL of an 0.13 M acetic acid solution. What volume (V) of 2.30...

You have 275 mL of an 0.13 M acetic acid solution. What volume (V) of 2.30 M NaOH solution must you add in order to prepare an acetate buffer of pH = 4.84? (The pKa of acetic acid is 4.76.)

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Answer #1

Here we use Henderson hasselbalch equation to solve this problem.

We are given volume and molarity of acetic acid and molarity of NaOH.

Concentration = mol solute / volume of solution in L .

This buffere is formed from weak acid CH3COOH and NaOH

Conjujgate base is CH3COO- which is formed from CH3COONa

Since CH3COONa dissociates complete and so conjugate base has same concentration as that of CH3COONa.

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