Titration 1.

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Presentation transcript:

Titration 1

2 Titrations Titration: the process of analyzing composition by measuring the volume of one solution needed to completely react with another solution. Usually the reaction of an acid with a base.

3 Titrations Analyte: the solution of unknown concentration but known volume. Titrant: the solution of known concentration. Analyte + Titrant → Products

4 Titrations Equivalence Point: the point at which exactly the right volume of titrant has been added to complete the reaction. Indicator: substance that changes color when an excess of titrant has been added (phenolphthalein).

5 Solution Stoichiometry Solution Stoichiometry uses molarity as a conversion factor between volume and moles of a substance in a solution.

6 Titrations Titration Calculations: 1. Find the number of moles of titrant added to reach the endpoint. 2. Determine the moles of analyte that must have been present (use stoichiometric coefficients). 3. Determine the concentration of analyte that must have been present in the flask (use the volume of analyte). 4. Calculate the concentration of analyte in the original sample.

7 Titrations Example #1: mL of an HCl solution of unknown concentration is titrated with standard NaOH solution. At the equivalence point, 25.0 mL of the M NaOH has been added. Calculate the concentration of the HCl solution. NaOH + HCl → NaCl + H 2 O Titrant = ?Analyte = ?