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Date: 21-5-2019
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Date: 21-5-2019
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Date: 21-5-2019
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Sometimes it is inconvenient to use the concentration units during a reaction a species’ concentration may change by many orders of magnitude. If we want to display the reaction’s progress graphically we might plot the reactant’s concentration as a function of time or as a function of the volume of a reagent being added to the reaction. Such is the case in Figure 1.1 for the titration of HCl with NaOH.
Figure 1.1: Graph showing the progress for the titration of 50.0 mL of 0.10 M HCl with 0.10 M NaOH. The [H+] is shown on the left y-axis and the pH on the right y-axis.
The y-axis on the left-side of the figure displays the [H+] as a function of the volume of NaOH. The initial [H+] is 0.10 M and its concentration after adding 80 mL of NaOH is 4.3 × 10-13 M. We can easily follow the change in [H+] for the first 14 additions of NaOH. For the remaining additions of NaOH, however, the change in [H+] is too small to see.
When working with concentrations spanning many orders of magnitude, it is often more convenient to express concentration using a p-function. The p-function of X is written as pX and is defined as
The pH of a solution that is 0.10 M H+ is
and the pH of 4.3 × 10-13 M H+ is
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