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CBSE Class 11 Chemistry MCQs: Redox in Titrations and Reactions – NCERT Practice Test
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Introduction Paragraph
The concept of Redox in Titrations and Reactions is one of the most crucial topics in Chapter 8: Redox Reactions of CBSE Class 11 Chemistry (Part B: Inorganic Chemistry). Redox titrations are based on oxidation and reduction processes, where electron transfer occurs between oxidizing and reducing agents. These titrations are essential for determining the concentration of analytes and are widely used in analytical chemistry, especially in permanganate, dichromate, and iodometric titrations.
This online MCQ practice test has been prepared according to the NCERT Class 11 Chemistry syllabus and follows the CBSE exam pattern. It includes questions covering titration principles, indicators, stoichiometry, and the role of oxidation-reduction agents. Each question is accompanied by an answer and explanation to help students understand concepts thoroughly.
These NCERT-based Chemistry MCQs are ideal for CBSE board exam preparation, school tests, and competitive exams like JEE and NEET, enhancing conceptual clarity and problem-solving speed.
Sample MCQs (with Answers and Explanations)
Q1. In a titration of Fe²⁺ with KMnO₄ in acidic medium, the end-point color appears due to:
A) Formation of blue complex B) Appearance of pink color C) Disappearance of brown color D) Gas evolution
Answer: B) Appearance of pink color
Explanation: In acidic solution, MnO₄⁻ is reduced to Mn²⁺ (colorless). A faint pink color appears when KMnO₄ is in excess, indicating the end point.
Q2. Which indicator is used in iodometric titration?
A) Phenolphthalein B) Methyl orange C) Starch D) Bromothymol blue
Answer: C) Starch
Explanation: Starch forms a blue-colored complex with iodine, making it a sensitive indicator for end-point detection in iodometric titrations.
Q3. In dichromate titration, K₂Cr₂O₇ acts as a/an:
A) Reducing agent B) Oxidizing agent C) Acid D) Base
Answer: B) Oxidizing agent
Explanation: Potassium dichromate oxidizes Fe²⁺ to Fe³⁺ in acidic medium and itself gets reduced to Cr³⁺, serving as a strong oxidizing agent.
Q4. In the titration of H₂O₂ with KMnO₄, the stoichiometric ratio of MnO₄⁻ : H₂O₂ in acidic medium is:
A) 1:1 B) 1:2 C) 1:5 D) 2:3
Answer: C) 1:5
Explanation: The balanced redox reaction shows 2MnO₄⁻ + 5H₂O₂ + 6H⁺ → 2Mn²⁺ + 5O₂ + 8H₂O; hence, the ratio is 1:5.
Q5. Why is heating necessary in permanganate titration of oxalic acid?
A) To accelerate reaction rate B) To dissolve oxalate crystals C) To evaporate solvent D) To reduce MnO₄⁻ directly
Answer: A) To accelerate reaction rate
Explanation: The redox reaction between MnO₄⁻ and oxalic acid proceeds slowly at room temperature; heating speeds up the process for a clear end point.
✅ Highlight:
These MCQs on Redox in Titrations and Reactions are created strictly following the NCERT syllabus, making them perfect for CBSE Class 11 Chemistry exam preparation and competitive practice.