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] }
Save your time - order a paper!
Get your paper written from scratch within the tight deadline. Our service is a reliable solution to all your troubles. Place an order on any task and we will take care of it. You won’t have to worry about the quality and deadlines
Order Paper Now= ?
[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*.)