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On the right, acid is being added to base. In both cases, the equivalence point is at pH 7. Titration curves can also be generated in the case of a weak acid-strong base titration or a strong base-weak acid titration. The general shape of the titration curve is the same, but the pH at the equivalence point is different. In a weak acid-strong base titration, the pH is greater than 7 at the equivalence point.
In a strong acid-weak base titration, the pH is less than 7 at the equivalence point. Watch the video at the link below and answer the following questions:. Read the material at the link below and answer the following questions:.
Skip to main content. Acids and Bases. Search for:. Titration Learning Objectives Define equivalence point. Describe how to perform a titration experiment. Perform calculations to determine concentration of unknown acid or base.
Describe titration curves of acid-base neutralization reactions. Figure 1. Phenolphthalein in basic solution. How is soap made? Sample Problem: Titration In a titration of sulfuric acid against sodium hydroxide, Figure 3. Titration curve of weak acid and strong base. Summary Definitions are given for equivalence point, titration and indicator.
The process for carrying out a titration is described. The process of calculating concentration from titration data is described and illustrated. Acid-base titration curves are described. Practice Titration Experiment Watch the video at the link below and answer the following questions: What is the indicator used?
What color is it in acid solution? Measure ad performance. Select basic ads. Create a personalised ads profile. Select personalised ads.
Apply market research to generate audience insights. Measure content performance. Develop and improve products. List of Partners vendors. Share Flipboard Email. Todd Helmenstine. Todd Helmenstine is a science writer and illustrator who has taught physics and math at the college level. He holds bachelor's degrees in both physics and mathematics. Updated January 24, For example, a 0. Figure 1 Setup for a Typical Titration In a typical titration, the titrant in the buret is added to the solution in the Erlenmeyer flask until the indicator changes color to show that the reaction is complete.
An indicator is added to the solution being titrated. The indicator is a substance that changes color when the reaction is complete. Phenolphthalein has two chemical forms. In acidic conditions, it is in the acid form, which is colorless. The titrant is slowly added to the solution being titrated until the indicator changes color, showing that the reaction is complete. This stage in the procedure is called the endpoint. In our example, the NaOH solution is slowly added from the buret until the mixture in the Erlenmeyer flask changes from colorless to red.
These react with the phenolphthalein molecules, changing them from the acid form to the base form. Because the base form is red, the solution turns red, telling us that the reaction is complete or just slightly beyond complete.
The volume of titrant added from the buret is measured.
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