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CBSE

Class 11

Chemistry Practicals

Class 11 Chemistry Practical

An Overview of Class 11 Chemistry Practical

The world of chemistry comes alive when you get to do real experiments in the lab. In Class 11 Chemistry Practical, you'll learn how to handle laboratory equipment, carry out exciting chemical reactions, test for salts, and see the science from your textbooks happening right before your eyes. It's a fun way to understand how chemistry works in real life.

Table of Content

If experiments or viva questions make you feel nervous, don't worry! Practicing these important practical questions and preparing step-by-step can make everything much simpler. You’ll boost your confidence for the exam, avoid common mistakes, and get ready to answer those tricky viva questions with ease. For more details about the overall topics you'll cover, check the updated Class 11 Chemistry Syllabus on Vedantu.

You can also easily download Vedantu’s free PDF of Class 11 Chemistry Practical important questions to help you prep for your practicals and score better. Find more at Class 11 Chemistry Important Questions.

Class 11 Chemistry Experiments Objectives

To grasp fundamental concepts in chemistry through hands-on experience and observation.
Understanding the importance of accurate measurements and the use of appropriate units (SI units, molarity, etc.) in experiments.
Recognizing types of chemical reactions (combination, decomposition, displacement, redox) and predicting products based on reactants.
Applying stoichiometric calculations to determine the relationships between reactants and products in a chemical reaction.
Understanding the concepts of pH, acidity, and basicity, and using indicators to measure the pH of different solutions.
Calculating molarity and understanding the concept of concentration in solutions, including dilution calculations.
Exploring the behaviour of gases under various conditions, including Boyle's law and Charles's law, and conducting experiments to demonstrate these principles.
Investigating energy changes during chemical reactions, including exothermic and endothermic processes, and measuring heat changes.
Understanding factors affecting solubility and conducting experiments to observe the solubility of different substances in solvents.
Learning methods for qualitative analysis to identify the presence of specific ions or compounds in a mixture.

Latest Practical Evaluation Scheme

Evaluation Scheme for Examination	Marks
Volumetric Analysis	8
Salt Analysis	8
Content-Based Experiment	6
Project Work	4
Class record and viva	4
Total	30

Below are the List of Experiments for Class 11 Chemistry

A. Basic Laboratory Techniques

1. Cutting glass tube and glass rod

2. Bending a glass tube

3. Drawing out a glass jet

4. Boring a cork

B. Characterization and Purification of Chemical Substances

1. Determination of the melting point of an organic compound.

2. Determination of the boiling point of an organic compound.

3. Crystallization of impure sample of any one of the following: Alum, Copper Sulphate, Benzoic Acid.

C. Experiments based on pH

a) Any one of the following experiments:

Determination of pH of some solutions obtained from fruit juices, solution of known and varied concentrations of acids, bases, and salts using pH paper or universal indicator.
Comparing the pH of solutions of strong and weak acids of the same concentration.

Study the pH change in the titration of a strong base using a universal indicator.

b) Study the pH change by common-ion in case of weak acids and weak bases.

D. Chemical Equilibrium

One of the following experiments:

a) Study the shift in equilibrium between ferric ions and thiocyanate ions by increasing/decreasing the concentration of either of the ions.

b) Study the shift in equilibrium between [Co(H2O)6] 2+ and chloride ions by changing the concentration of either of the ions.

E. Quantitative Estimation

i. Using a mechanical balance/electronic balance.

ii. Preparation of standard solution of Oxalic acid.

iii. Determination of strength of a given solution of Sodium hydroxide by titrating it against standard solution of Oxalic acid.

iv. Preparation of standard solution of Sodium carbonate.

v. Determination of strength of a given solution of hydrochloric acid by titrating it against standard Sodium Carbonate solution.

F. Qualitative Analysis a) Determination of one anion and one cation in a given salt Cations- Pb2+, Cu2+, As3+, Al3+, Fe3+, Mn2+, Ni2+, Zn2+, Co2+, Ca2+, Sr2+, Ba2+, Mg2+, NH4 + Anions – CO3 2--, S 2-, NO2 -, SO3 2- -, SO4 2-, NO3 -, Cl-, Br-, I-, PO4 3- , CH3COO-

(Note: Insoluble salts excluded)

b) Detection of -Nitrogen, Sulphur, and Chlorine in organic compounds.

Benefits Class 11 Chemistry Practical Experiments

Builds curiosity and encourages scientific thinking.
Emphasizing the importance of safety measures and proper disposal methods in the chemistry laboratory.
To enhance practical skills such as measurement, observation, and data analysis.
To apply theoretical knowledge to practical situations, reinforcing learning through experimentation.
To instil a sense of safety and responsibility in handling chemicals and laboratory equipment.
To promote scientific inquiry and critical thinking by encouraging students to formulate hypotheses and draw conclusions based on their observations.
To encourage collaboration and teamwork during experiments, enhancing communication skills among peers.
To improve skills in documenting and presenting experimental procedures and results accurately.

Preparation Tips to Get your Expertise in Chemistry Concepts

Start with basic experiments to build a strong foundation before advancing to complex ones.
Ensure you have all the required materials ready before starting each experiment.
Follow the instructions carefully and take notes on your observations to help with understanding.
Perform the experiments under proper guidance to avoid any risks or mistakes.
Revise the scientific concepts behind each experiment to connect theory with practical application.

Chemistry Experiments for Class 11 provide an engaging way to learn key scientific concepts through hands-on experience. These experiments help students solidify their understanding of the CBSE syllabus while developing a passion for chemistry. With clear instructions and easy access to resources, students can explore the exciting chemistry experiments and excel in their studies.

S. No	Related Study Materials for Class 11 Chemistry
1.	CBSE Class 11 Chemistry NCERT Book
2.	CBSE Class 11 Chemistry Notes
3.	CBSE Class 11 Chemistry Sample Papers
4.	CBSE Class 11 Chemistry Formulas
5.	CBSE Class 11 Chemistry Important Questions
6.	CBSE Class 11 Chemistry Exemplar Solutions
7.	CBSE Class 11 Chemistry NCERT Solutions

FAQs on Class 11 Chemistry Practical

1. What is the typical marks distribution for the CBSE Class 11 Chemistry Practical Exam for the 2025-26 session?

For the 2025-26 session, the CBSE Class 11 Chemistry Practical exam is worth 30 marks. A common distribution of marks, which can vary slightly between schools, is as follows:

Volumetric Analysis: 8 Marks
Salt Analysis (Qualitative Analysis): 8 Marks
Content-Based Experiment: 6 Marks
Project Work and Viva: 4 Marks
Class Record and Viva: 4 Marks

Students must score passing marks in both the theory and practical examinations separately.

2. What are some expected questions from the salt analysis (qualitative analysis) experiment?

In salt analysis, you are expected to identify one anion and one cation from an unknown salt. Important questions revolve around the systematic procedure. Be prepared to:

Identify the colour and solubility of the salt during the preliminary tests.
Explain the logic behind the sequence of group reagents for cation analysis.
Write the chemical equations for confirmatory tests, for example, the ring test for nitrate ions or the flame test for Ba²⁺ or Sr²⁺ ions.
Justify why certain tests are performed (e.g., why the original solution is prepared in a specific acid).

3. Why is it critically important to heat the oxalic acid solution to 60-70°C before titrating against KMnO₄?

This is a crucial step and a common viva question. The reaction between potassium permanganate (KMnO₄) and oxalic acid is very slow at room temperature. Heating the oxalic acid solution to 60-70°C acts as a catalyst, increasing the rate of reaction. However, heating above 70°C is avoided because it can cause the oxalic acid to decompose into carbon dioxide and water, which would lead to an inaccurate, lower titre value.

4. Which important viva questions should a student prepare for the Class 11 Chemistry practical exam?

The viva voce tests your fundamental understanding. Besides questions about your specific experiment, prepare for these important areas:

Apparatus: The use and principle of burettes, pipettes, and standard flasks.
Reagents: The role of each chemical used, e.g., the function of dilute H₂SO₄ in the KMnO₄ titration.
Indicators: Why a specific indicator is used, or why KMnO₄ acts as a self-indicator.
Formulas and Units: The formula for molarity and normality, and the chemical formulas of common salts like Mohr's salt.
Sources of Error: Potential errors in your experiment, such as parallax error in reading the burette or improper washing of apparatus.

5. How does the choice of indicator affect the result of an acid-base titration, and why is phenolphthalein a common choice?

The choice of indicator is vital for accuracy. An ideal indicator must change colour at the pH of the equivalence point of the reaction. Using the wrong indicator, one that changes colour significantly before or after the equivalence point, will result in an incorrect endpoint and an inaccurate calculation of concentration. Phenolphthalein is a common choice for titrations between a strong acid and a strong base, or a weak acid and a strong base, because its pH range for colour change (approx. 8.2-10) falls within the sharp pH jump at the equivalence point of these reactions.

6. Beyond just safety, how do precautions taken in the lab contribute to marks in the practical exam?

Examiners observe your technique and adherence to safety protocols as an indicator of your practical skill. While direct marks for safety are not specified, poor practices can lead to marks deduction. For example:

Incorrect Handling of Apparatus: Improperly using a pipette (e.g., blowing out the last drop) leads to volume errors and lower marks in volumetric analysis.
Contamination: Not washing the test tubes properly can lead to incorrect results in salt analysis, resulting in zero marks for identification.
Technique: The way you control the stopcock of the burette to release drop-by-drop solution near the endpoint demonstrates proficiency and is often noted by the examiner.

7. What is the importance of a well-maintained practical record for the CBSE Class 11 Chemistry exam?

A well-maintained practical record is crucial and carries specific marks (typically 4-5 marks, combined with viva). Its importance is twofold:

Proof of Work: It serves as documented evidence of the experiments you have performed throughout the year as per the CBSE 2025-26 syllabus.
Assessment Tool: The examiner assesses your record for completeness, neatness, correct recording of observations, and accurate calculations. An organised and accurate record reflects a student's diligence and understanding, often influencing the viva assessment positively.

8. What are the most common sources of error in determining the melting point of an organic compound, and how do they affect the result?

Determining the melting point is a key content-based experiment. Common errors include:

Rapid Heating: Heating the capillary tube too quickly does not allow for thermal equilibrium between the substance, thermometer, and heating bath. This almost always results in a higher and broader melting point range.
Impure Sample: The presence of impurities disrupts the crystal lattice structure of the compound. This typically causes the melting point to be lower and occur over a wide range rather than a sharp point.
Incorrect Packing: Packing too much sample into the capillary tube can also lead to a wider melting range due to uneven heat distribution.