Definition: Titration is a laboratory technique used to determine the concentration of an unknown solution by reacting it with a solution of known concentration.
Basic Components of Titration
Analyte: The solution of unknown concentration.
Titrant: The solution of known concentration used to titrate the analyte.
Indicator: A substance that changes color at (or near) the equivalence point.
Burette: A glass tube with precise volume markings used to deliver the titrant.
Process of Titration
Preparation: The analyte is placed in a flask. The titrant is filled in the burette.
Addition of Indicator: An indicator is added to the analyte.
Titration: The titrant is slowly added to the analyte until the endpoint is reached, indicated by a color change.
Volume Measurement: The volume of titrant used to reach the endpoint is measured.
Types of Titration
Acid-Base Titration: Determines the concentration of an acid or a base using a base or acid as the titrant.
Redox Titration: Involves a reduction-oxidation reaction between the analyte and titrant.
Precipitation Titration: Based on the formation of a precipitate during the reaction.
Equivalence Point vs. Endpoint
Equivalence Point: The point at which the amount of titrant added is chemically equivalent to the amount of analyte in the solution.
Endpoint: The point where the indicator changes color, signifying the completion of the reaction.
Calculations in Titration
Formula:MA×VA=MT×VT
MA: Molarity of the analyte.
VA: Volume of the analyte.
MT: Molarity of the titrant.
VT: Volume of the titrant used.
Determining Concentration: The concentration of the analyte is calculated using the known concentration of the titrant and the volume of titrant used.
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