As stated above the indirect potentiometry follows the change of pH with

As stated above the indirect potentiometry follows

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the determination of an end point, or in this case, the equivalence point. As stated above, the indirect potentiometry follows the change of pH with respect to the volume of titrant added in the solution, thus making it possible to plot the titration curve and easily determining the equivalence point of the solution. The endpoint in potentiometry is indicated at the largest potential breaks, therefore the value of the exact potential is unnecessary and only the change of the cell potentials is needed. The approximate equivalence point may be determined when the pH had undergone a radical change and this may indicate that the solution is near to its endpoint. In the experiment, the pH meter’s electrode is immersed in the solution while it is being titrated with NaOH solution. A magnetic stir bar was used to stir the solution constantly to distribute the titrant evenly throughout the solution containing the KHP analyte. In trial 1, the titrant is added with one mL increments.

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0.00E+00 5.00E+00 1.00E+01 1.50E+01 2.00E+01 2.50E+01 5 6 7 8 9 10 11 12 8.06 Trial 1: Titration Curve Volume of NaOH, mL pH value Figure 1: Titration Curve of Trial 1 With this graph, the approximate equivalence point is determined at the corresponding volume in which a radical change of pH has occurred, in this case, at 20mL. Now, for trial 2, the increments of the added titrant in the analyte solution decrease as it approaches the approximate equivalence point, thus, giving the graph shown below.
• Fall '17
• pH, KHP, Potentiometry

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