6.03 Calorimetry Lab
Figure 1: Titration curve of 0.160 grams of an unknown diprotic acid that was dissociated in distilled water. Shown is the pH versus the volume in milliliters of 0.1 M NaOH, a strong base, added to the solution.
The initial pH reading of the solution was a pH of 2.60. Although the pH of the ½ equivalence point was unknown, it could be estimated by halving the volume of NaOH used at the first equivalence point. At the first equivalence point, 13.63 milliliters of NaOH had been added to the unknown acid solution. Once divided by two, that value ended up being 6.815 milliliters of NaOH added at the ½ equivalence point pH. In order to estimate the pH at that volume of NaOH being added, two data points around the volume of 6.815 milliliters were
The initial pH reading of the solution was a pH of 2.60. Although the pH of the ½ equivalence point was unknown, it could be estimated by halving the volume of NaOH used at the first equivalence point. At the first equivalence point, 13.63 milliliters of NaOH had been added to the unknown acid solution. Once divided by two, that value ended up being 6.815 milliliters of NaOH added at the ½ equivalence point pH. In order to estimate the pH at that volume of NaOH being added, two data points around the volume of 6.815 milliliters were