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Answer:
0.034 M is the molarity of sodium acetate needed.
Explanation:
The pH of the buffer solution is calculated by the Henderson-Hasselbalch equation:
Where:
pK_a= Negative logarithm of the dissociation constant of a weak acid
= Concentration of the conjugate base
[HA] = Concentration of the weak acid
According to the question:
The desired pH of the buffer solution = pH = 5.27
The pKa of acetic acid = 4.74
The molarity of acetic acid solution = [HAc] = 0.01 M
The molarity of acetate ion =
Using Henderson-Hasselbalch equation:
Sodium acetate dissociates into sodium ions and acetate ions when dissolved in water.
0.034 M is the molarity of sodium acetate needed.