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Calculating the expected pH of the buffer solution: Given that the pKa for Acetic Acid is 4.
Calculating the expected pH of the buffer solution:
Given that the pKa for Acetic Acid is 4.77, calculate the expected pH of the buffer solutions using the Henderson-Hasselbalch equation and the concentrations of Acetic Acid and Acetate added to the 250 ml Erlenmeyer flask:
pH = pKa + log { [base] / [acid] }
= ?
[CH3COOH]=[CH3COO-]
Ph= pKa + log ( base/ acid)
Ph = pKa + log ([CH3COO-]/[CH3COOH]
Ph = 4.77+ log 1
pH = 4.77 for both acetate and acetic acid
Hints:
moles of base = mass of NaC2H3O2 / GMW of NaC2H3O2
(GMW available from Chemicals dialog box under Info)
moles of acid = volume of C2H4O2 in litres x molarity of C2H4O2
Preparation the buffer solution:
initial pH of buffer solution: ____
Titration of a weak acid with a strong base:
initial pH of weak acid: ____
final pH of weak acid: ____
Amount of NaOH added: ____
Titration Curve for Weak Acid with a Strong Base
(Paste curve here*.)
Titration of buffer with a strong base:
pH of buffer solution: ____
Amount of NaOH added: ____
Titration Curve for Buffer with a Strong Base
(Paste curve here*.)
Titration of the buffer with a strong acid:
pH of buffer solution: ____
Amount of HCl added: ____
Titration Curve for Buffer with a Strong Acid
(Paste curve here*.)
