The Acid Base Titrations And Indicator Titrations Introduction-

1003 Words Apr 11th, 2016 null Page
Title- Experiment #9- Acid Base Titrations II: Potentiometric and Indicator Titrations Introduction- In this experiment, the reactions of three different acids with a strong base are studied by observing how the pH of the solution changes as the titrant is added. A plot of pH versus amount of titrant added will be constructed. Such a curve is called a pH titration curve. The equivalence point of the reaction will be determined from an analysis of the pH titration curve, and by the use of acid-base indicators. The pH measures the solution whether it is acidic and basic. The pH of the solution could be determined by using the following equation, pH= -log[H+]. It could also be determined by finding the pOH= -log[OH-] and then subtracting by using the formula pH= 14-pOH. The lower the pH, the more acidic the solution is. The higher the pH is, the more basic (less acidic) the solution is. However, by titrating a weak acid with a strong base, the pH of the solution would be depending on how low or high the concentration and ionization are. A strong acid dissociates completely in a solution, meanwhile a weak acid will ionize partially. The equivalence point is an important factor because it can help determine the pH of a solution where the amount of acid equals the amount of base. Also, each indicator has its own pH range. For example, there are indicators that only change color when pH is equivalent to a specific pH that belong within that range.
Procedure-
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