The Basic Titration Methods section introduces the fundamental principles and practical applications of volumetric analysis, a core component of analytical chemistry and laboratory experiments. This module is designed for Class 11–12 students and undergraduate learners, with strong emphasis on conceptual understanding, calculation accuracy, and practical exam relevance.
In this section, you will study:
Principles of titration – equivalence point, end point, standard solutions, and indicators
Acid–base titrations – strong vs strong, strong vs weak systems, and indicator selection
Redox titrations – permanganometry, dichrometry, and iodometry (introductory level)
Precipitation titrations – Mohr’s and Volhard’s methods (basics)
Complexometric titrations – EDTA titration principles and applications
Titration curves and calculations – molarity, normality, equivalent weight, and stoichiometry
Experimental errors and precautions – indicator errors, endpoint detection, and accuracy improvement
NCERT- and UG-aligned theory, supported by diagrams, worked numericals, MCQs, viva questions, and practical exam tips
The content is structured to connect theory with laboratory practice, enhance quantitative problem-solving skills, and prepare students for school practicals, undergraduate labs, and written examinations.
Build a strong foundation in Basic Titration Methods to confidently perform volumetric analysis and analytical calculations in Chemistry.
Q. In a redox titration, what is being measured?
A.
The concentration of oxidizing or reducing agents
B.
The temperature of the solution
C.
The volume of gas produced
D.
The solubility of the reactants
Solution
In a redox titration, the concentration of oxidizing or reducing agents is measured by the amount of titrant required to reach the endpoint.
Correct Answer:
A
— The concentration of oxidizing or reducing agents
Q. In a titration curve, what does the steepest slope indicate?
A.
The equivalence point
B.
The endpoint
C.
The initial pH
D.
The final pH
Solution
The steepest slope in a titration curve indicates the equivalence point, where the amount of titrant added is stoichiometrically equivalent to the analyte.
Q. What is a common mistake when performing a titration?
A.
Not swirling the flask
B.
Using too much titrant
C.
Not recording the initial volume
D.
All of the above
Solution
Common mistakes in titration include not swirling the flask to ensure proper mixing, using too much titrant, and failing to record the initial volume accurately.
Q. What is the significance of the dilution factor in titration?
A.
It affects the endpoint
B.
It determines the concentration of the titrant
C.
It helps calculate the concentration of the analyte
D.
It has no significance
Solution
The dilution factor is significant as it helps in calculating the concentration of the analyte based on the volume and concentration of the titrant used.
Correct Answer:
C
— It helps calculate the concentration of the analyte
Q. What is the significance of the equivalence point in titration?
A.
It is when the titrant is first added
B.
It is when the amount of titrant equals the amount of analyte
C.
It is when the solution is neutral
D.
It is when the indicator changes color
Solution
The equivalence point is significant because it is the stage in the titration where the amount of titrant added is stoichiometrically equivalent to the amount of analyte present.
Correct Answer:
B
— It is when the amount of titrant equals the amount of analyte
Q. Which indicator is commonly used in acid-base titrations?
A.
Phenolphthalein
B.
Bromothymol blue
C.
Methyl orange
D.
All of the above
Solution
Phenolphthalein, Bromothymol blue, and Methyl orange are all indicators that can be used in acid-base titrations, depending on the pH range of the titration.
