Elizabeth Tram Experiment Two

Elizabeth Tram Experiment Two - Elizabeth Tram FRI...

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Elizabeth Tram FRI – Supramolecular Sensors Experiment 2: Acid-Base Equilibria Purpose Necessary solutions will be prepared by the dilution of liquid solutes in order to be measured with a pH probe or meter. With the pH probe, the Logger Pro program will be used to create a titration curve for the purpose of observing the equilibria for a weak acid and strong base combination, which will be used to determine the ionization constant of acetic acid. A comparison of measured pH and calculated pH for various unbuffered and buffered solutions will also be made. Data and Observations Standardized concentration of NaOH used for titrations: 0.097267 ± 0.000451 M Average equivalent point values of titrant volume: pH of 10.52 at 20.65 mL Average half-equivalence point values of titrant volume: pH of 4.69 at 10.32 mL Average pK a from titration curves: ≈ 4.67 There was an error after the first titration was completed, and the second titration was in process. The computer was accidentally shut down, and the pH probe had to be recalibrated. The setup was redone for the second titration, and the original second titration was removed from the experimental data. Table 1: pH readings for acetic acid Solution pH 1.6 M acetic acid (10 mL) 2.44 1.6 M sodium acetate (25 mL) & 1.6 M acetic acid (10 mL) 5.36 1.6 M sodium acetate (15 mL) & 1.6 M acetic acid (20 mL) 4.76 Average pH: 4.19 Results Table 2: Determination of the ionization constant of acetic acid, titrating using a pH meter Titration Curve Equivalence Point Half-Equivalence Point pH K a 1 19.94 9.97 4.62 2.40 x 10 -5 2 22.0 11.0 4.47 3.39 x 10 -5 3 20.0 10.0 4.93 1.17 x 10 -5 Table 3: Determination of the ionization constant of acetic acid, from pH readings Solution pH K
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This note was uploaded on 11/10/2011 for the course HDF 304 taught by Professor Gray during the Spring '08 term at University of Texas at Austin.

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Elizabeth Tram Experiment Two - Elizabeth Tram FRI...

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