Quantitative Analysis: Principle of Volumetric (Titrimetric) Analysis
Introduces quantitative analysis and defines volumetric (titrimetric) analysis as determining an unknown concentration from the volume of a standard solution needed for complete reaction. Covers the equivalence and end points, the M1V1 = M2V2 relationship, the four requirements for a titration, the four titration types and common applications. Includes a labelled titration diagram explaining the burette, stopcock, pipette, conical flask, indicator and white tile, followed by the working steps.
Inside: 10 sections · 1 labelled picture · 1 formula · 15 flashcards · 4 min
Topic 20 of 47 in the MU Pleven syllabus for Chemistry (Medicine, Year 1). The free AceMed note covers it in 10 sections, about 494 words (4 min of reading), with 15 flashcards.
In this note
Quantitative Analysis: Principle of Volumetric (Titrimetric) Analysis
Definition
Principle
Requirements of Volumetric Analysis
Types of Volumetric Titrations
Applications
Labeled Titration Diagram – Explanation
Diagram Description and Functions of Parts
Working Principle Shown by the Diagram
Conclusion
Quantitative Analysis: Principle of Volumetric (Titrimetric) Analysis
Quantitative analysis is the branch of analytical chemistry that deals with the determination of the amount or concentration of a substance present in a sample. One of the most commonly used quantitative methods is volumetric analysis, also known as titrimetric analysis.
Definition
Volumetric analysis is a method in which the concentration of an unknown solution is determined by measuring the volume of a standard solution required to react completely with it.
Principle
The principle of volumetric analysis is based on a chemical reaction of known stoichiometry between a standard solution and an unknown solution. During titration, the standard solution (titrant) is added gradually to the analyte until the reaction is complete.
The point at which the reaction is chemically complete is called the equivalence point. The completion of the reaction is detected by a suitable indicator, which shows a visible color change at the end point.
At the equivalence point:
Number of equivalents (or moles) of titrant = number of equivalents (or moles) of analyte
Where M_1, V_1 = molarity and volume of standard solution
M_2, V_2 = molarity and volume of unknown solution
Using this relationship, the concentration of the unknown solution is calculated.
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