Experiment #1

Experiment #1 - Discussion: This experiment had two main...

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Discussion: This experiment had two main purposes. First, was to determine the dissociation constant, Ka, of acetic acid by measuring the pH of solutions containing acetic acid and through titration. The second objective was to compare the capacity of a buffer solution to resist pH change to that of water. CH 3 COOH (aq) H + (aq) + CH 3 COO - (aq) CH 3 COOH (aq) + NaOH (aq) NaCH 3 COO (aq) + H 2 O (l) HA (aq) + H 2 O (l) H 3 O + (aq) + A - (aq) OH - (aq) + HA (aq) A - (aq) + H 2 O (l) In the first part of the experiment acetic acid was titrated with the base NaOH. The results were then graphed on the computer, which was used to view the equivalence point (where moles of H + disassociated equaled the initial moles of NaOH) and the half equivalence point. Using pH= pKa + log ([A-]/[HA]), and [A-] = [HA] at half of the equivalence point, pH = pKa, a Ka of 3.98*10 -5 was found. While the result was on the same magnitude as the standardized value of Ka for acetic acid (1.76*10 -5 ) it had a 77%
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This note was uploaded on 03/14/2012 for the course CHEM 1B 1BL taught by Professor Nielsen during the Winter '12 term at UCSB.

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Experiment #1 - Discussion: This experiment had two main...

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