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Titration of acetic acid

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Titration of Acetic Acid with NaOH and HCL

  1. In the titration of acetic acid with NaOH why does the pH not change very much from 4-6 drops of added NaOH?
  2. In the titration of acetic acid with NaOH why does a buffer plus 10 drops of 1.0 M HCL not change the pH very much? (Also write an equation to explain).
  3. In the titration of acetic acid with NaOH why does the pH not change very much after adding 10 extra drops of 1.0 M NaOH?

Calculated Data on Acid Unknown

Weight of acid unknown = 1.623 g

NaOH sol'n molarity = 0.1986 M

Voluume used to titrate acid unknown = 24.9 mL

pH of original acid solution = 2.05 pH

pH of half neutralized solution (buffer) = 3.85 pH

1. Calculate molecular weight of acid unknown.

2. Calculate pKa and Ka of acid unknown.

3. Using the Ka and [H+] of original acid solution, calculate the molarity of the original acid solution (assume a monoprotic acid; correct for disassociation).

4. Using the volume of NaOH needed to neutralize 25 mL of the original solution, again calculate its molarity.

Reference no: EM131109250

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