Experiment 9 AcidBase Equilibria: Determination of Acid Ionization Constants
In part 1 of the lab, we determined the Dissociation Constant Ka of Acetic Acid
by Measuring the Titration Curve using a pH meter.
In adding the Sodium Hydroxide to
the acetic acid, the pH was titrated all the way to 11.5 to give us a range of where the
equivalence point may occur.
We found the volume of NaOH at the equivalence point to
be 26.25 mL and half the equivalence point was approximately 13.2 mL.
The
equivalence point was where the spike occurred.
From that point, we took the x value on
the graph of the half equivalence point which was 13.2 mL and the corresponding y value
on the graph gave us the pH which had a value of 4.7.
We took 10 to the power of 4.7
and that in turn gave us our Dissociation Constant, which is our Ka value of 2 x 10^5.
In part 2 of the lab, we determined the Dissociation Constant of Acetic Acid, we
measured the pH of 10 mL of a 1.0 M HA solution.
The pH was observed as 2.3 and the
Hydrogen Ion Concentration determined from 10 to the power of 2.3 was found to be .
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 Fall '06
 NEUMAN
 pH, 10 mL, 1.0 M, 2 ml, 10.0 mL, 13.2 mL

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