The student Louise continued the analysis of acetic acid using half - neutralization technique. She titrates this acetic acid solution using 0.984 M NaOH titrant solution. When volume of NaOH reaches 14.34 mL, she stopped titration. The averaged pH value is measured to be 4.75. Determine the acid dissociation constant Ka.
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The student Louise continued the analysis of acetic acid using half - neutralization technique. She titrates this acetic acid solution using 0.984 M NaOH titrant solution. When volume of NaOH reaches 14.34 mL, she stopped titration. The averaged pH value is measured to be 4.75.
Determine the acid dissociation constant Ka.
The reaction between acetic acid and NaOH is
NaOH + CH3COOH --------> CH3COONa + H2O
Since the titration is done till half neutralisation point.
Hence it means only half of the acid has reacted.
Hence concentration of salt CH3COONa formed = initial concentration of CH3COOH taken / 2 ( i.e half of acid)
And concentration of CH3COOH remaining = initial concentration of CH3COOH / 2 ( i.e half of initial)
Hence at half neutralisation point, also known as half equivalence point,
the concentration of CH3COOH i.e acid remaining = the concentration of CH3COONa i.e conjugate base salt of acid
Since the solution has both acid and its conjugate base. Hence it will act as a buffer solution.
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