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CBSE 12th Standard Chemistry Subject Solution Case Study Questions With Solution 2021

By QB365 on 21 May, 2021

QB365 Provides the updated CASE Study Questions for Class 12 , and also provide the detail solution for each and every case study questions . Case study questions are latest updated question pattern from NCERT, QB365 will helps to get  more marks in Exams

QB365 - Question Bank Software

12th Standard CBSE

Final Semester - June 2015

Read the passage given below and answer the following questions: The concentration of a solute is very important in studying chemical reactions because it determines how often molecules collide in solution and thus indirectly determine the rate of reactions and the conditions at equilibrium. There are several ways to express the amount of solute present in a solution. The concentration of a solution is a measure of the amount of solute that has been dissolved in a given amount of solvent or solution. Concentration can be expressed in terms of molarity, molality, parts per million, mass percentage, volume percentage, etc. The following questions are multiple choice questions. Choose the most appropriate answer: (i) The molarity (in mol L -1 ) of the given solution will be

(ii) Which of the following is correct relationship between mole fraction and molality?

(iii) Which of the following is temperature dependent?

(iv) Which of the following is true for an aqueous solution of the solute in terms of concentration?

Read the passage given below and answer the following questions: At 298 K, the vapour pressure of pure benzene, C 6 H 6 is 0.256 bar and the vapour pressure of pure toluene C 6 H 5 CH 3 is 0.0925 bar. Two mixtures were prepared as follows: (i) 7.8 g of C 6 H 6 + 9.2 g of toluene (ii) 3.9 g of C 6 H 6 + 13.8 g of toluene The following questions are multiple choice questions. Choose the most appropriate answer: (i) The total vapour pressure (bar) of solution 1 is

(ii) Which of the given solutions have higher vapour pressure?

(iii) Mole fraction of benzene in vapour phase in solution 1 is

(iv) Solution I is an example of a/an

Read the passage given below and answer the following questions: An ideal solution may be defined as the solution which obeys Raoult's law exactly over the entire range of concentration. The solutions for which vapour pressure is either higher or lower than that predicted by Raoult's law are called non-ideal solutions. Non-ideal solutions can show either positive or negative deviations from Raoult's law depending on whether the A-B interactions in solution are stronger or weaker than A - A and B - B interactions. The following questions are multiple choice questions. Choose the most appropriate answer: (i) Which of the following solutions is/are ideal solution(s)? (i) Bromoethane and iodoethane (ii) Acetone and chloroform (iii) Benzene and acetone (iv)n-heptane and n-hexane

(ii) Which of the following is not true for positive deviations?

(iii) For water and nitric acid mixture which of the given graph is correct?

(iv) Water- HCl mixture I. shows positive deviations  II. forms minimum boiling azeotrope III. shows negative deviations  IV. forms maximum boiling azeotrope

Read the passage given below and answer the following questions: The properties of the solutions which depend only on the number of solute particles but not on the nature of the solute are called colligative properties. Relative lowering in vapour pressure is also an example of colligative properties. For an experiment, sugar solution is prepared for which lowering in vapour pressure was found to be 0.061 mm of Hg. (Vapour pressure of water at 20°C is 17.5 mm of Hg.) The following questions are multiple choice questions. Choose the most appropriate answer: (i) Relative lowering of vapour pressure for the given solution is

(ii) The vapour pressure (mm of Hg) of solution will be

(iii) Mole fraction of sugar in the solution is

(iv) The vapour pressure (mm of Hg) of water at 293 K when 25 g of glucose is dissolved in 450 g of water is

Read the passage given below and answer the following questions: Few colligative properties are: (a) relative lowering of vapour pressure: depends only on molar concentration of solute (mole fraction) and independent of its nature. (b) depression in freezing point: it is proportional to the molal concentration of solution. (c) elevation of boiling point: it is proportional to the molal concentration of solute. (d) osmotic pressure: it is proportional to the molar concentration of solute. A solution of glucose is prepared with 0.052 g at glucose in 80.2 g of water. (K f = 1.86 K kg mol -1  and K b = 5.2 K kg mol -1 ) The following questions are multiple choice questions. Choose the most appropriate answer: (i) Molality of the given solution is

(ii) Boiling point for the solution will be

(iii) The depression in freezing point of solution will be

(iv) Mole fraction of glucose in the given solution is

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Cbse 12th standard chemistry subject solution case study questions with solution 2021 answer keys.

(i) (d) : Density of solution = 1.202 g/mL Volume of solution =  \(\frac{100 \mathrm{~g}}{1.202 \mathrm{~g} / \mathrm{mL}}=83.2 \mathrm{~mL}\) Molarity =  \(\frac{n_{\mathrm{KI}}}{\text { Volume of solution in } \mathrm{L}}\) \(=\frac{0.120 \mathrm{~mol}}{0.0832 \mathrm{~L}}=1.4423 \mathrm{~mol} \mathrm{~L}^{-1}\) (ii) (a):  \(x_{2}=\frac{n_{2}}{n_{1}+n_{2}} ; x_{1}=\frac{n_{1}}{n_{1}+n_{2}} ; \frac{x_{2}}{x_{1}}=\frac{n_{2}}{n_{1}}\) \(\frac{x_{2}}{x_{1}}=\frac{m_{2} / M_{2}}{m_{1} / M_{1}}=\frac{m_{2}}{m_{1}} \times \frac{M_{1}}{M_{2}}\)           ...(i) Molality =  \(\frac{n_{2}}{m_{1}}=\frac{m_{2}}{M_{2} \times m_{1}}\)               ...(ii) From(i) and (ii), m =  \(\frac{x_{2}}{x_{1}} \times \frac{1}{M_{1}} ; x_{1}=1-x_{2}\) Hence. x 2  =  \(\frac{m M_{1}}{1+m M_{1}}\) (iii) (a) : Mass does not depend on temperature while volume does. Hence, molarity depends on temperature. (iv) (b): 1M solution contains 1 mole of solute in less than 1000 g of the solvent whereas 1 m solution has 1 mole of the solute in 1000 g of the solvent.

(i) (b) : Moles of C 6 H 6  =  \(\frac{7.8}{78}=0.1\) Mole C 6 H 5 CH 3  =  \(\frac{9.2}{92}=0.1\) Mole fraction of C 6 H 6  =  \(\frac{0.1}{0.1+0.1}=0.5\) => Mole fraction of C 6 H 5 CH 3 = 0.5 Vapour pressure of toluene = Vapour pressure of pure toluene x mole fraction of toluene = 0.0925 x 0.5 = 0.04625 Vapour pressure of benzene = 0.256 x 0.5 = 0.128 Total vapour pressure of solution = 0.17425 (ii) (a) :  Moles of benzene in solution-II =  \(\frac{3.9}{78}=0.05\) Moles of toluene in solution-II =  \(\frac{13.8}{92}=0.15\) Vapour pressure of solution = 0.256 x 0.05 + 0.0925 x 0.15 = 0.0128 + 0.013875 = 0.026675 (iii) (c) : Mole fraction of benzene in vapour phase \(y_{\text {benzene }}=\frac{p_{\text {benzene }}}{P_{\text {total }}}=\frac{0.128}{0.17425}=0.734\) (iv) (a) : Benzene and toluene form an ideal solution.

(i) (d) : II represents negative deviations and III represents positive deviations. (ii) (b): For positive deviations  \(p_{A}>p_{A}^{\circ} x_{A} \text { and } p_{B}>p_{B}^{\circ} x_{B}\) (iii) (b) : Water and nitric acid mixture shows negative deviations from Raoult's law, hence  \(p_{A}<p_{A}^{\circ} x_{A} \text { and } p_{B}<p_{B}^{\circ} x_{B}\) (iv) (d): Water-HCl mixture shows negative deviations from Raoult's law and solutions showing negative deviations from ideal behaviour form maximum boiling azeotrope.

(i) (a) : Vapour pressure of water  \(\left(p_{A}^{\circ}\right)\)  = 17.5 mm of Hg Lowering of vapour pressure  \(\left(p_{A}^{\circ}-p_{A}\right)\) = 0.061 Relative lowering of vapour pressure   \(=\frac{p_{A}^{\circ}-p_{A}}{p_{A}^{\circ}}=\frac{0.061}{17.5}=0.00348\) (ii) (c): P = Vapour pressure of solvent - lowering in vapour pressure = 17.5 - 0.061 = 17.439 mm of Hg (iii) (a):  \(\frac{p_{A}^{\circ}-p_{A}}{p_{A}^{\circ}}=x_{B}=0.00348\) Hence, mole fraction of sugar = 0.00348 (iv) (b):  \(\frac{p_{A}^{\circ}-p_{A}}{p_{A}^{\circ}}=x_{B}=\frac{w_{B} \times M_{A}}{M_{B} \times w_{A}}\) \(\frac{17.5-p_{A}}{17.5}=\frac{25 \times 18}{450 \times 180}=5.56 \times 10^{-3}\) \(17.5-p_{A}=17.5 \times 5.56 \times 10^{-3}\) \(17.5-p_{A}=0.0973\) P = 17.40 mm Hg

(i) (b) : m  \(=\frac{0.052}{180} \times \frac{1000}{80.2}=0.0036\) (ii) (c):   \(\Delta T_{b}=K_{b} \times m=5.2 \times 0.0036=0.0187 \mathrm{~K}\) \(T_{b}=373+0.0187=373.0187 \mathrm{~K} \approx 373.02 \mathrm{~K}\) (iii) (d):  \(\Delta T_{f}=K_{f} \times m=1.86 \times 0.0036=0.067 \mathrm{~K}\) (iv) (a): Moles of glucose  \(=\frac{0.052}{180}=0.00028\) Moles 0f water =  \(\frac{80.2}{18}=4.455\) Mole fraction of glucose =  \(\frac{0.00028}{4.45+0.00028}=6.28 \times 10^{-5}\)

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Case Study Class 12 Chemistry With Questions Answers

In Coming Exams, CBSE will ask two Case Study Questions in the CBSE class 12 Chemistry questions paper. Each theme will have five questions and students will have a choice to attempt any four of them. Here are some example questions Based On Case Study Problems:

Question-1 Read the passage given below and answer any four out of the following questions: Ammonia is present in small quantities in air and soil where it is formed by the decay of nitrogenous organic matter e.g., urea. On a large scale, ammonia is manufactured by Haber’s process. In accordance with Le Chatelier’s principle, high pressure would favour the formation of ammonia. Ammonia is a colourless gas with a pungent odour. Its freezing and boiling points are 198.4 and 239.7 K respectively. In the solid and liquid states, it is associated with hydrogen bonds as in the case of water and that accounts for its higher melting and boiling points than expected on the basis of its molecular mass. Ammonia gas is highly soluble in water. Its aqueous solution is weakly basic due to the formation of OH– ions. The presence of a lone pair of electrons on the nitrogen atom of the ammonia molecule makes it a Lewis base.

The following questions are multiple-choice questions. Choose the most appropriate choice 1. On a small scale, ammonia is obtained from ammonium salts which decompose when treated with 1.caustic soda 2.calcium chloride 3.sodium hydroxide 4.sodium chloride

2.The optimum conditions for the production of ammonia are a pressure of 1. 200*105 Pa 2. 400*105 Pa 3. 100*105 Pa 4. 300*105 Pa

3. The catalyst which is used in the preparation of NH3 by Haber’s process 1. Mg2O3 + K2O 2. Al2O3 + K2O 3. NaO3 + K2O 4. None of these 4. The ammonium molecule has: 1. five bond pair and two lone pair 2. four lone pair and one bond pair 3. three bond pair and one lone pair 4. three bond pair and two lone pair 5. A compound reacts with ammonia to form deep colour solution, identify the compound 1. Au2+ 2. Cu2+ 3. Al3+

Questions-2 Read the passage and answer any four out of the following questions: Colloidal particles always carry an electric charge. The nature of this charge is the same on all the particles in a given colloidal solution and may be either positive or negative. The charge on the sol particles is due to one or more reasons, viz., due to electron capture by sol particles during electrodispersion of metals. When two or more ions are present in the dispersion medium, preferential adsorption of the ion common to the colloidal particle usually takes place. When silver nitrate solution is added to the potassium iodide solution, the precipitated silver iodide adsorbs iodide ions from the dispersion medium, and negatively charged colloidal solution results. acquired a positive or a negative charge by selective adsorption on the surface of a colloidal particle The combination of the two layers of opposite charges around the colloidal particle is called Helmholtz electrical double layer. The presence of equal and similar charges on colloidal particles is largely responsible for providing stability to the colloidal solution. In these questions, a statement of assertion followed by a statement of reason is given. Choose the correct answer out of the following choices.

1. Assertion and reason both are correct statements and reason is correct explanation for assertion 2. Assertion and reason both are correct statements but reason is not correct explanation for assertion 3. Assertion is correct statement and reason is wrong statement 4. Assertion is wrong statement but reason is correct statement

1. Assertion: The presence of equal and similar charges on colloidal particles is largely responsible in providing stability to the colloidal solution. Reason: The repulsive forces between charged particles having the same charge prevent them from aggregating and provide stability.

2. Assertion: The first layer is mobile in Helmholtz electrical double layer. Reason: The potential difference between the fixed layer and the diffused layer of opposite charges is called zeta potential.

3. Assertion: The sol particle in the colloid has a charge. Reason: The charge in sol is due to electron capture by sol particles during the electrodispersion of metals.

4. Assertion: Methylene blue sol is a negatively charged sol. Reason: When KI solution is added to AgNO3 solution, positively charged sol formed.

5. Assertion: If FeCl3 is added to an excess of hot water, a positively charged sol of hydrated ferric oxide is formed. Reason: When ferric chloride is added to NaOH a negatively charged sol is obtained with adsorption of OH- ions.

Question-3 .Read the passage and answer the following questions: The crystal field theory (CFT) is an electrostatic model which considers the metal-ligand bond to be ionically arising purely from electrostatic interactions between the metal ion and the ligand. Ligands are treated as point charges in case of anions or point dipoles in case of neutral molecules. The five d orbitals in an isolated gaseous metal atom/ion have the same energy, i.e., they are degenerate. In an octahedral coordination entity with six ligands surrounding the metal atom/ion, there will be repulsion between the electrons in metal d orbitals and the electrons (or negative charges) of the ligands. This splitting of the degenerate levels due to the presence of ligands in a definite geometry is termed crystal field splitting and the energy separation is denoted by Δ0. The colour in the coordination compounds can be readily explained in terms of the crystal field theory. In these questions, a statement of assertion followed by a statement of reason is given. Choose the correct answer out of the following choices. 1.Assertion and reason both are correct statements and reason is correct explanation for assertion. 2. Assertion and reason both are correct statements but reason is not correct explanation for assertion. 3. Assertion is correct statement but reason is wrong statement. 4. Assertion is wrong statement but reason is correct statement.

1. Assertion: The dx2-y2 and dz2 orbitals which point towards the axes along the direction of the ligand will experience more repulsion. Reason: The dxy, dyz and dxz orbitals which are directed between the axes will be lowered in energy.

2. Assertion: The complex [Ti(H2O)6]3+, which is red in colour. Reason: The crystal field theory attributes the colour of the coordination compounds to d-d transition of the electron.

3. Assertion: Ligands for which Δ0Δ0 < P are known as weak field ligands and form high spin complexes. Reason: If Δ0 > P, then the fourth electron enters one of the eg orbitals giving the configuration t2g3 eg1.

4. Assertion: In tetrahedral coordination entity formation, the d orbital splitting is inverted and is smaller as compared to the octahedral field splitting. Reason: Spectrochemical series is based on the absorption of light by complexes with different ligands.

5. Assertion: The crystal field model is successful in explaining the formation, structures, colour and magnetic properties of coordination compounds. Reason: The anionic ligands are found at the low end of the spectrochemical series.

Answer Key:

1. (b) Assertion and reason both are correct statements and reason is not correct explanation for assertion. 2. (c) Assertion is correct statement but reason is wrong statement. 3. (a) Assertion and reason both are correct statements and reason is correct explanation for assertion. 4. (a) Assertion and reason both are correct statements and reason is correct explanation for assertion. 5. (d) Assertion is wrong statement but reason is correct statement.

Question-4 Read the passage and answer any four out of the following question Alfred Werner (1866-1919), a Swiss chemist was the first to formulate his ideas about the structures of coordination compounds. Werner proposed the concept of a primary valence and a secondary valence for a metal. The coordination entity constitutes a central metal atom or ion bonded to a fixed number of ions or molecules. In a coordination entity, the atom/ion to which a fixed number of ions/groups are bound in a definite geometrical arrangement around it is called the central atom or ion. The ions or molecules bound to the central atom/ion in the coordination entity are called ligands. Ligands may be simple ions such as Cl-, small molecules such as H2O or NH3, larger molecules such as H2NCH2CH2NH2 or N(CH2CH2NH2)3 or even macromolecules, such as protein. Ligands are unidentate, bidentate and polydentate. The coordination number (CN) of a metal ion in a complex is the number of ligand donor atoms to which the metal is directly bonded.

In these questions, a statement of assertion followed by a statement of reason is given. Choose the correct answer out of the following choices.

1. Assertion and reason both are correct statements and reason is correct explanation for assertion 2. Assertion and reason both are correct statements but reason is not correct explanation for assertion 3. Assertion is correct statement but reason is wrong statement 4. Assertion is wrong statement but reason is correct statement

1. Assertion: Binary compounds such as CrCl3, have a primary valence of 3. Reason: Coordinate compound metals show only one type of linkage that is primary linkage.

2. Assertion: CoCl3(NH3)3 is a coordination entity in which the cobalt ion is surrounded by three ammonia molecules and three chloride ion. Reason: The central atom/ion in the coordination entities: [NiCl2(H2O)4] is Ni2+.

3. Assertion: H2NCH2CH2NH2 (ethane-1,2-diamine) ligand is said to be didentate. Reason: Didentate ligands are bind through two donor atoms.

4. Assertion: The complex ions, [PtCl6]2- the coordination number of Pt is 4. Reason: Ligand which can ligate through two different atoms is called ambidentate ligand.

5. Assertion: EDTA can bind through two nitrogen and four oxygen atoms to a central metal ion. Reason: The number of ligating groups attach to an atom is called the denticity of the ligand.

1. (c) Assertion is correct statement but reason is wrong statement 2. (b) Assertion and reason both are correct statements but reason is not correct explanation for assertion 3. (a) Assertion and reason both are correct statements and reason is correct explanation for assertion 4. (d) Assertion is wrong statement but reason is correct statement 5. (b) Assertion and reason both are correct statements but reason is not correct explanation for assertion

Question-5 Read the passage given below and answer any four out of the following questions: Nitrogen differs from the rest of the members of group 15 due to its smaller size, high electronegativity, high ionisation enthalpy, and non-availability of d orbitals. Nitrogen has a unique ability to form pπ-pπ multiple bonds with itself. Nitrogen exists as a diatomic molecule with a triple bond one s and two p between the two atoms. Phosphorus, arsenic and antimony from single bonds as P–P, As–As and Sb–Sb while bismuth forms metallic bonds in an elemental state. Dinitrogen is produced commercially by the liquefaction and fractional distillation of air. Liquid dinitrogen (b.p. 77.2 K) distils out first leaving behind liquid oxygen (b.p. 90 K). In the laboratory, dinitrogen is prepared by treating an aqueous solution of ammonium chloride with sodium nitrite. Dinitrogen is a colourless, odourless, tasteless and non-toxic gas. It has two stable isotopes 14N and 15N. It has very low solubility in water. The main use of dinitrogen is in the manufacture of ammonia and other industrial chemicals containing nitrogen.

The following questions are multiple-choice questions. choose the most appropriate answer

1. N–N bond is weaker than the single P–P bond because 1. high interelectronic repulsion of the bonding electrons 2. high interelectronic repulsion of the non-bonding electrons 3. no repulsion between bonding electrons 4. no repulsion between non-bonding electrons 2. Very pure nitrogen can be obtained by the 1. thermal decomposition of sodium 2. thermal decomposition of barium azide 3. thermal decomposition of ammonium dichromate 4. both (a) and (b) 3. Dinitrogen is rather inert at room temperature because of 1. low bond enthalpy of N≡≡N bond 2. high bond enthalpy of N≡≡N bond 3. low freezing point 4. low boiling point 4. Dinitrogen combines with dioxygen only at very high temperature (at about 2000 K) to form 1. nitric oxide 2. nitrate 3. nitrites 4. nitric acid 5. Liquid dinitrogen is used as a refrigerant to 1. preserve biological materials 2. preserve food items 3. in cryosurgery 4. all of these

1. (b) high interelectronic repulsion of the non-bonding electrons 2. (d) both (a) and (b) 3. (b) high bond enthalpy of N≡≡N bond 4. (a) nitric oxide 5. (d) all of these

Question-6 Read the following passage and answer any four out of the following questions: Transition metal oxides are generally formed by the reaction of metals with oxygen at high temperatures. The highest oxidation number in the oxides coincides with the group number. In vanadium, there is a gradual change from the basic V2O3 to less basic V2O4 and to amphoteric V2O5. V2O4 dissolves in acids to give VO2+ salts. Potassium dichromate is a very important chemical used in the leather industry and as an oxidant for the preparation of many azo compounds. Dichromates are generally prepared from chromate. Sodium dichromate is more soluble than potassium dichromate. The latter is, therefore, prepared by treating the solution of sodium dichromate with potassium chloride. Sodium and potassium dichromates are strong oxidising agents; sodium salt has a greater solubility in water and is extensively used as an oxidising agent in organic chemistry. Potassium dichromate is used as a primary standard in volumetric analysis.

The following questions are multiple-choice questions. Choose the most appropriate answer.

1. All transition metal reacts with oxygen to form MO oxide except 1. scandium 2. vanadium 3. cupper 4. zinc 2. As the oxidation number of a metal increases, ionic character 1. increases 2. decreases 3. remain the same 4. none of these 3. The shape of chromate ion is 1. tetrahedral 2. pyramidal 3. square planer 4. triangular 4. Dichromates are generally prepared from chromate, which in turn are obtained by the fusion of 1. FeCr2O 2. FeCr2O 4 3. Na2CrO 4 4. Na2Cr2O 7 5. The oxo cations stabilise VIV 1. VO 2. VO 4+ 3. VO 2+ 4. all of these

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CBSE Class 12 Chemistry Case Study Questions PDF

Case studies play a pivotal role in CBSE Class 12 Chemistry, as they enable students to apply theoretical knowledge to real-life scenarios. CBSE Class 12 Chemistry Case Study Questions PDF section introduces the significance of case studies in enhancing analytical skills and understanding complex chemical reactions.

Case studies challenge students to think critically, analyze experimental data, and devise problem-solving strategies. They provide a deeper understanding of chemical principles and their practical applications, fostering a holistic learning experience. Familiarize yourself with the structure of case study questions to streamline your preparation. Each case study presents a unique chemical problem, encouraging students to identify relevant concepts and devise accurate solutions.

Table of Contents

Class 12 Chemistry Case Study Questions

CBSE Class 12 Chemistry question paper will have case study questions too. These case-based questions will be objective type in nature. So, Class 12 Chemistry students must prepare themselves for such questions. First of all, you should study NCERT Textbooks line by line, and then you should practice as many questions as possible.

Chapter-wise Solved Case Study Questions for Class 12 Chemistry

Class 12 students should go through important Case Study problems for Chemistry before the exams. This will help them to understand the type of Case Study questions that can be asked in Grade 12 Chemistry examinations. Our expert faculty for standard 12 Chemistry have designed these questions based on the trend of questions that have been asked in last year’s exams. The solutions have been designed in a manner to help the grade 12 students understand the concepts and also easy-to-learn solutions.

Tips to Excel in CBSE Class 12 Chemistry Examinations

Excel in your Chemistry exams with these practical tips.

A. Regular Practice with Case Studies

Consistent practice with case study questions enhances your ability to tackle complex problems. Dedicate time to solving various case studies to build confidence.

B. Understanding Analytical Skills

Develop strong analytical skills to approach case studies logically. Break down complex problems into simpler components and analyze them step-by-step.

C. Time Management Strategies

Allocate sufficient time for each case study during the exam. Practice time management in mock tests to complete the paper within the stipulated time.

Best Books for Class 12 Chemistry

Strictly as per the new term-wise syllabus for Board Examinations to be held in the academic session 2024 for class 12 Multiple Choice Questions based on new typologies introduced by the board- Stand-Alone MCQs, MCQs based on Assertion-Reason Case-based MCQs. Include Questions from CBSE official Question Bank released in April 2024 Answer key with Explanations What are the updates in the book: Strictly as per the Term wise syllabus for Board Examinations to be held in the academic session 2024. Chapter-wise -Topic-wise Multiple choice questions based on the special scheme of assessment for Board Examination for Class 12th Chemistry.

Mastering CBSE Class 12 Chemistry case study questions is crucial for excelling in the exams. Embrace case studies as a valuable learning tool, and with practice, you’ll ace your Chemistry exams with confidence.

Benefits of Utilizing the CBSE Class 12 Chemistry Case Study PDF

• Enhanced Learning Experience : The case study PDF offers practical examples and scenarios, making the learning process engaging and relatable for students.
• Application of Theoretical Concepts : It enables students to apply theoretical knowledge to practical situations, honing their problem-solving and analytical skills.
• Real-World Relevance : By connecting classroom learning to real-life applications, students can grasp the practical significance of chemistry in various industries.
• Critical Thinking Development : Analyzing case studies encourages students to think critically and make informed decisions based on chemical principles.
• Exam Preparation : Exposure to case studies aids in better preparation for chemistry examinations by providing a comprehensive understanding of the subject.

The CBSE Class 12 Chemistry case study PDF brings a refreshing perspective to the world of education. By intertwining theoretical knowledge with practical applications, it equips students to face real-world challenges with confidence. The diverse case studies provide invaluable insights, encouraging students to explore chemistry beyond the classroom and make a positive impact on society.

What is the CBSE Class 12 Chemistry case study PDF?

The CBSE Class 12 Chemistry case study PDF is a curated document by CBSE, presenting real-life applications of chemistry concepts for students to understand the subject’s practical relevance.

How does the case study PDF benefit students?

The case study PDF enhances the learning experience, fosters critical thinking, promotes application-based learning, and prepares students for examinations.

Are the case studies diverse in content?

Yes, the case studies cover various branches of chemistry, including organic, inorganic, physical, environmental, and analytical chemistry.

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CBSE Class 12 Chemistry Case Study Based Important Questions with Solutions, Download PDF Here

Cbse class 12 chemistry case study based questions: for the cbse class 12 chemistry exam that is scheduled for february 27, 2024, important case study-based questions in chemistry are provided in this article. also, get information related to the chemistry exam pattern and marking scheme in the article..

CBSE Class 12 Chemistry Paper Pattern

Important case study based questions for class 12th chemistry with solutions.

The following questions are case-based questions. Each question has an internal choice and carries 4 marks each. Read the passage carefully and answer the questions that follow.

Q.1. Many people believe that James Watson and Francis Crick discovered DNA in the 1950s. In reality, this is not the case. Rather, DNA was first identified in the late 1860s by Swiss chemist Friedrich Miescher. Then, in the decades following Miescher's discovery, other scientists--notably, Phoebus Levene and Erwin Chargaff--carried out a series of research efforts that revealed additional details about the DNA molecule, including its primary chemical components and the ways in which they joined with one another. Without the scientific foundation provided by these pioneers, Watson and Crick may never have reached their groundbreaking conclusion of 1953: that the DNA molecule exists in the form of a three-dimensional double helix. Chargaff, an Austrian biochemist, as his first step in this DNA research, set out to see whether there were any differences in DNA among different species. After developing a new paper chromatography method for separating and identifying small amounts of organic material, Chargaff reached two major conclusions: (i) the nucleotide composition of DNA varies among species. (ii) Almost all DNA, no matter what organism or tissue type it comes from maintains certain properties, even as its composition varies. In particular, the amount of adenine (A) is similar to the amount of thymine (T), and the amount of guanine (G) approximates the amount of cytosine (C). In other words, the total amount of purines (A + G) and the total amount of pyrimidines (C + T) are usually nearly equal. This conclusion is now known as "Chargaff's rule." Chargaff’s rule is not obeyed in some viruses. These either have single- stranded DNA or RNA as their genetic material. Answer the following questions: a. A segment of DNA has 100 adenine and 150 cytosine bases. 

a. What is the total number of nucleotides present in this segment of DNA? 

Ans. A = 100 so T = 100

C=150 so  G = 150

Total nucleotides = 100+100+150+150 =500 

b. A sample of hair and blood was found at two sites. Scientists claim that the samples belong to the same species. How did the scientists arrive at this conclusion? 

Ans. They studied the nucleotide composition of DNA. It was the same so they concluded that the samples belong to the same species. 

c. The sample of a virus was tested and it was found to contain 20% adenine, 20% thymine, 20 % guanine and the rest cytosine. Is the genetic material of this virus (a) DNA- double helix (b) DNA-single helix (c) RNA? What do you infer from this data? 

Ans.  A = T = 20%

But G is not equal to C so double helix is ruled out. 

 The bases pairs are ATGC and not AUGC so it is not RNA.

 The virus is a single helix DNA virus.

Importance of Solving Case Study Questions for Class 12 Chemistry

• Case study-based questions in Class 12 are pivotal for good scores. Practicing these questions equips students to tackle these types of questions effectively.
• Solving case study-based questions helps students develop an efficient time management strategy.
• Excelling in Case study-based questions cultivates a holistic subject comprehension essential for future pursuits.

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Case Study Questions Class 12 Chemistry

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CBSE will ask Case Study Questions class 12 Chemistry in session 2020-21. These will be the first two questions in the board exam question paper. The first question will have 5 MCQs out of which students will attempt any 4 questions. The second question will carry 5 Assertion & Reason type questions with the choice to attempt any four.

Case Study Questions

As you know, CBSE will hold exams in May-June this year. There is already a reduction of 30% in the syllabus. Now, the case study questions have been added. So, this year the question paper is going to be a bit easier. Although it is easy yet these case study questions need special attention and regular practice.

We have added around 10 sample questions based on the latest pattern in myCBSEguide App. These all questions include two case study questions.

Class 12 Chemistry Question Bank

If you go through the previous year question papers, you will analyze that many questions are repeated word by word and many others are almost similar. So, it is always recommended to check all questions asked in previous years. This will not only help you to get an idea about the question pattern but also help you to understand the difficulty level of the questions.

myCBSEguide App has the previous year’s question bank. These questions are arranged chapter-wise. If you are preparing a particular chapter, you will get all questions asked from that chapter in the last 10 years.

Case Study Questions Examples

Here are two examples of case study questions. To get more such questions download the myCBSEguide App and browse Sample Papers there.

Read the passage given below and answer any four out of the following questions: Ammonia is present in small quantities in air and soil where it is formed by the decay of nitrogenous organic matter e.g., urea. On a large scale, ammonia is manufactured by Haber’s process. In accordance with Le Chatelier’s principle, high pressure would favour the formation of ammonia. Ammonia is a colourless gas with a pungent odour. Its freezing and boiling points are 198.4 and 239.7 K respectively. In the solid and liquid states, it is associated through hydrogen bonds as in the case of water and that accounts for its higher melting and boiling points than expected on the basis of its molecular mass. Ammonia gas is highly soluble in water. Its aqueous solution is weakly basic due to the formation of OH– ions. The presence of a lone pair of electrons on the nitrogen atom of the ammonia molecule makes it a Lewis base.

• caustic soda
• calcium chloride
• sodium hydroxide
• sodium chloride
• ​200 10 5 Pa
• 400 10 5 Pa
• 100 10 5 Pa
• 300 10 5 Pa
• Mg 2 O 3  + K 2 O
• Al 2 O 3  + K 2 O
• NaO 3  + K 2 O
• None of these
• five bond pair and two lone pair
• four lone pair and one bond pair
• three bond pair and one lone pair
• three bond pair and two lone pair

Read the passage and answer any four out of the following questions: Colloidal particles always carry an electric charge. The nature of this charge is the same on all the particles in a given colloidal solution and may be either positive or negative. The charge on the sol particles is due to one or more reasons, viz., due to electron capture by sol particles during electrodispersion of metals. When two or more ions are present in the dispersion medium, preferential adsorption of the ion common to the colloidal particle usually takes place. When silver nitrate solution is added to the potassium iodide solution, the precipitated silver iodide adsorbs iodide ions from the dispersion medium, and negatively charged colloidal solution results. acquired a positive or a negative charge by selective adsorption on the surface of a colloidal particle The combination of the two layers of opposite charges around the colloidal particle is called Helmholtz electrical double layer. The presence of equal and similar charges on colloidal particles is largely responsible for providing stability to the colloidal solution.

In these questions, a statement of assertion followed by a statement of reason is given. Choose the correct answer out of the following choices. 

• Assertion and reason both are correct statements and reason is correct explanation for assertion
• Assertion and reason both are correct statements but reason is not correct explanation for assertion
• Assertion is correct statement and reason is wrong statement
• Assertion is wrong statement but reason is correct statement
• Assertion:  The presence of equal and similar charges on colloidal particles is largely responsible in providing stability to the colloidal solution. Reason:  The repulsive forces between charged particles having the same charge prevent them from aggregating and provide stability.
• Assertion: The first layer is mobile in Helmholtz electrical double layer. Reason:  The potential difference between the fixed layer and the diffused layer of opposite charges is called zeta potential.
• Assertion: The sol particle in colloid has a charge. Reason:  The charge in sol is due to electron capture by sol particles during the electrodispersion of metals.
• Assertion:  Methylene blue sol is a negatively charged sol. Reason: When KI solution is added to AgNO 3 solution, positively charged sol formed.
• Assertion:  If FeCl3 is added to an excess of hot water, a positively charged sol of hydrated ferric oxide is formed. Reason: When ferric chloride is added to NaOH a negatively charged sol is obtained with adsorption of OH- ions.

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CBSE Class 12 Chemistry Case study Questions & Answers For Chapter 1, 2, 4, 6, 7, 8, 9, 10, 11, 12, 13, 14, 15, 16

Understudies can discover the chapter astute vital questions for course 12th Chemistry within the table underneath. These imperative questions incorporate questions that are regularly inquired in a long time. Moreover, arrangements are to give for these questions, with extraordinary accentuation on ease-of-study. Tap on the joins underneath to begin investigating.

Below we posted all the Case Study Questions & Answers for Class 12 Chemistry all Chapters –

CBSE Class 12 Case Study Question for Chemistry

Case study 1.

(1) Read the passage given below and answer the questions that follow.

 Are there nuclear reactions going on in our bodies?

There are nuclear reactions constantly occurring in our bodies, but there are very few of them compared to the chemical reactions, and they do not affect our bodies much. All of the physical processes that take place to keep a human body running are chemical processes. Nuclear reactions can lead to chemical damage, which the body may notice and try to fix. The nuclear reaction occurring in our bodies is radioactive decay. This is the change of a less stable nucleus to a more stable nucleus. Every atom has either a stable nucleus or an unstable nucleus, depending on how big it is and on the ratio of protons to neutrons. The ratio of neutrons to protons in a stable nucleus is thus around 1:1 for small nuclei (Z < 20). Nuclei with too many neutrons, too few neutrons, or that are simply too big are unstable. They eventually transform to a stable form through radioactive decay. Wherever there are atoms with unstable nuclei (radioactive atoms), there are nuclear reactions occurring naturally. The interesting thing is that there are small amounts of radioactive atoms everywhere: in your chair, in the ground, in the food you eat, and yes, in your body.

The most common natural radioactive isotopes in humans are carbon-14 and potassium-40. Chemically, these isotopes behave exactly like stable carbon and potassium. For this reason, the body uses carbon-14 and potassium-40 just like it does normal carbon and potassium; building them into the different parts of the cells, without knowing that they are radioactive. In time, carbon-14 atoms decay to stable nitrogen atoms and potassium-40 atoms decay to stable calcium atoms. Chemicals in the body that relied on having a carbon-14 atom or potassium-40 atom in a certain spot will suddenly have a nitrogen or calcium atom. Such a change damages the chemical. Normally, such changes are so rare, that the body can repair the damage or filter away the damaged chemicals. The natural occurrence of carbon-14 decay in the body is the core principle behind carbon dating. As long as a person is alive and still eating, every carbon-14 atom that decays into a nitrogen atom is replaced on average with a new carbon-14 atom. But once a person dies, he stops replacing the decaying carbon-14 atoms. Slowly the carbon-14 atoms decay to nitrogen without being replaced, so that there is less and less carbon-14 in a dead body. The rate at which carbon-14 decays is constant and follows first order kinetics. It has a half – life of nearly 6000 years, so by measuring the relative amount of carbon-14 in a bone, archeologists can calculate when the person died. All living organisms consume carbon, so carbon dating can be used to date any living organism, and any object made from a living organism. Bones, wood, leather, and even paper can be accurately dated, as long as they first existed within the last 60,000 years. This is all because of the fact that nuclear reactions naturally occur in living organisms. (source: The textbook Chemistry: The Practical Science by Paul B. Kelter, Michael D. Mosher and Andrew Scott states)

(a)  Why is Carbon -14 radioactive while Carbon -12 not? (Atomic number of Carbon: 6)

Ans: Ratio of neutrons to protons is 2.3: 1 which is not the stable ratio of 1:1

(b) Researchers have uncovered the youngest known dinosaur bone, dating around 65 million years ago. How was the age of this fossil estimated?

Ans: Age of fossils can be estimated by C-14 decay. All living organisms have C-14 which decays without being replaced back once the organism dies.

(c)  Which are the two most common radioactive decays happening in human body?

Ans: carbon-14 atoms decay to stable nitrogen atoms and potassium-40 atoms decay to stable calcium.

(d) Suppose an organism has 20 g of Carbon -14 at its time of death. Approximately how much Carbon -14 remains after 10,320 years? (Given antilog 0.517 = 3.289)

Ans: t = 2.303/ k log (Co/Ct)

Co = 20 g Ct = ?

t = 10320 years k = 0.693/6000 (half-life given in passage)

substituting in equation:

10320 = 2.303 / (0.693/6000) log 20/ Ct

0.517 = log 20 / Ct anlilog (0.517) = 20/Ct

3.289 = 20/Ct

Ct = 6.17 g

(d) Approximately how old is a fossil with 12 g of Carbon -14 if it initially possessed 32 g of Carbon -14? (Given log 2.667 = 0.4260)

Co = 32 g Ct = 12

t = ? k = 0.693/6000 (half life given in passage) substituting in equation:

t = 2.303 / (0.693/6000) log 32/ 12

t = 2.303 x 60000 /0.693 log 2.667

t = 2.303x6000x0.4260 /0.693

= 8494 years

Key questions for 12th review Biology are outlined agreeing to the CBSE NCERT program. All address sorts are accessible within the PDF, from one-word to one-line answers, brief reply sorts to five point long reply sorts. Hence, understudies can plan for exams and indeed clarify their concepts through them. On the off chance that they refer to these questions, it’ll get ready their minds to pick up a competitive advantage. Understudies will gotten to be commonplace with question patterns and the sorts of questions that will show up on exams.

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Case Study Questions for Class 12 Chemistry Chapter 3 Electrochemistry

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There is Case Study Questions in class 12 Chemistry in session 2020-21. For the first time, the board has introduced the case study questions in the board exam. The first two questions in the board exam question paper will be based on Case Study and Assertion & Reason. The first question will have 5 MCQs out of which students will have to attempt any 4 questions. The second question will carry 5 Assertion & Reason type questions with the choice to attempt any four. Here are the questions based on case study.

Case Study Question 1:

Read the passage given below and answer the following questions:

All chemical reactions involve interaction of atoms and molecules. A large number of atoms/molecules are present in a few gram of any chemical compound varying with their atomic/molecular masses. To handle such large number conveniently, the mole concept was introduced. All electrochemical cell reactions are also based on mole concept. For example, a 4.0 molar aqueous solution of NaCl is prepared and 500 mL of this solution is electrolysed. This leads to the evolution of chlorine gas at one of the electrode. The amount of products formed can be calculated by using mole concept.

The following questions are multiple choice questions. Choose the most appropriate answer:

(i) The total number of moles of chlorine gas evolved is (a) 0.5 (b) 1.0 (c) 1.5 (d) 1.9

(ii) If cathode is a Hg electrode, then the maximum weight of amalgam formed from this solution is (a) 300g (b) 446 g (c) 396 g (d) 256 g

The total charge (coulomb) required for complete electrolysis is (a) 186000 (b) 24125 (c) 48296 (d) 193000

(iii) In the electrolytes, the number of moles of electrons involved are (a) 2 (b) 1 (c) 3 (d) 4

(iv) In electrolysis of aqueous NaCl solution when Pt electrode is taken, then which gas is liberated at cathode? (a) H 2 gas (b) Cl 2 gas (c) O 2 gas (d) None of these

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ScoreMore Case Study Chapter-wise Practice Questions Chemistry Class-12 is curated with 800+ Chapter-wise MCQs related to Case study/ Passage based and Assertion & Reason with hints and explanations based on latest pattern of CBSE (2020-2021).

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MTG ScoreMore Case Study Based Sample Questions Chemistry Class 12 is specially designed to help students get familiar with solving these new patterns of questions. The book covers 800 + sample questions for practice with detailed explanations to each question. Practising these questions will definitely help students to get an edge in their CBSE preparations.

For the academic year 2020-21 CBSE has incorporated more Objective type/MCQ based questions which will focus on measuring critical thinking ability of students.

The new pattern of questions includes Case study based questions, Passage based questions, Assertion and Reason type questions. In Case study based/ Passage based questions, students will be expected to answer questions after reading a given paragraph or a passage. Assertion and Reason type question is just another way of checking the clarity of one’s concept.

• 1. The Solid State
• 2. Solutions
• 3. Electrochemistry
• 4. Chemical Kinetics
• 5. Surface Chemistry
• 6. General Principles and Processes of Isolation of Elements*
• 7. The p-Block Elements
• 8. The d- and f-Block Elements
• 9. Coordination Compounds
• 10. Haloalkanes and Haloarenes
• 11. Alcohols, Phenols and Ethers
• 12. Aldehydes, Ketones and Carboxylic Acids
• 14. Biomolecules
• 15. Polymers*
• 16. Chemistry in Everyday Life*
• *This chapter is not a part of the Board Examination 2020-21 syllabus

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Class 12 Chemistry Case Study Questions Chapter 10 Haloalkanes and Haloarenes

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In Class 12 Boards there will be Case studies and Passage Based Questions will be asked, So practice these types of questions. Study Rate is always there to help you. Free PDF Download of CBSE Class 12 Chemistry Chapter 10 Haloalkanes and Haloarenes Case Study and Passage Based Questions with Answers were Prepared Based on Latest Exam Pattern. Students can solve NCERT Class 12 Chemistry Case Study Questions Haloalkanes and Haloarenes  to know their preparation level.

Join our Telegram Channel, there you will get various e-books for CBSE 2024 Boards exams for Class 9th, 10th, 11th, and 12th.

In CBSE Class 12 Chemistry Paper, There will be a few questions based on case studies and passage-based as well. In that, a paragraph will be given, and then the MCQ questions based on it will be asked.

Haloalkanes and Haloarenes Case Study Questions With Answers

Here, we have provided case-based/passage-based questions for Class 12 Chemistry  Chapter 10 Haloalkanes and Haloarenes

Case Study/Passage-Based Questions

Case Study 1: A chlorocompound (A) on reduction with Zn-Cu and ethanol gives the hydrocarbon (B) with five carbon atoms. When (A) is dissolved in dry ether and treated with sodium metal it gave 2,2,5,5 tetramethylhexane. The treatment of (A) with alcoholic KCN gives compound (C).

(i) The compound (A) is

Answer: (a) 1-chloro- 2, 2-dimethylpropane.

(ii) The reaction of (C) with Na, C 2 H 5 OH gives

Answer: (c) (CH)3C CH2CH2NH2

(iii) The reaction of (C) with Na, C 2 H 5 OH is called

Answer: (b) Mendius reaction

(iv) Compound (B) is

Answer: (b) 2, 2-dimethylpropane

Case Study 2: Nucleophilic substitution reactions are of two types; substitution nucleophilic bimolecular (SN2) and substitution nucleophilic unimolecular (SN1) depending on molecules taking part in determining the rate of reaction. The reactivity of alkyl halide towards SN1 and SN2 reactions depends on various factors such as steric hindrance, stability of intermediate or transition state and polarity of solvent. SN2 reaction mechanism is favored mostly by primary alkyl halide or transition state and polarity of the solvent, SN2 reaction mechanism is favored mostly by primary alkyl halide then secondary and then tertiary. This order is reversed in the case of SN1 reactions.

(i) Which of the following is most reactive towards nucleophilic substitution reaction? (a) C 6 H 5 Cl (b) CH 2 =CHCl (c) ClCH 2 CH=CH 2 (d) CH 3 CH=CHCl

Answer: (c) ClCH2CH=CH2

(ii) Isopropyl chloride undergoes hydrolysis by (a) S N 1 mechanism (b) S N 2 mechanism (c) S N 1 and S N 2 mechanism (d) neither S N 1 nor S N 2 mechanism

Answer: (c) SN1 and SN2 mechanism

(iii) The most reactive nucleophile among the following is (a) CH 3 O- (b) C 6 H 5 O- (c) (CH 3 ) 2 CHO- (d) (CH 3 ) 3 CO-

Answer: (a) CH3O-

Which of the following is the correct order of decreasing S N 2 reactivity? (a) RCH 2 X > R 2 CHX > R 3 CX (b) R 3 CX > R 2 CHX >RCH 2 X (c) R 2 CHX >R 3 CX > RCH 2 X (d) RCH 2 X >R 3 CX >R 2 CHX

Answer: (a) RCH2X > R2CHX > R3CX

Case Study 3: A primary alkyl halide (A) C 4 H 9 Br reacted with alcoholic KOH to give compound (B). Compound (B) is reacted with HBr to give compound (C) which is an isomer of (A). When (A) reacted with sodium metal, it gave a compound (D) C 8 H 18  that is different than the compound obtained when n-butyl bromide reacted with sodium metal

(i) Which type of isomerism is present in compounds (A) and (C)?

Answer: (c) Chain

(ii) IUPAC name of compound (D) is

Answer: (c) 2-methyl heptane

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Case Study Question 1 on Solutions – Chapter 2 CBSE Class 12 Chemistry

• May 14, 2022
• Chemistry , CBSE , Class 12

Case-based Questions

Read the given passages and answer the questions that follow :

The spontaneous flow of the solvent through a semipermeable membrane from a pure solvent to a solution or from a dilute solution to a concentrated solution is called osmosis. The phenomenon of osmosis can be demonstrated by taking two eggs of the same size. In an egg, the membrane below the shell and around the egg material is semi- permeable. The outer hard shell can be removed by putting the egg in dilute hydrochloric acid. After removing the hard shell, one egg is placed in distilled water and the other in a saturated salt solution. After some time, the egg placed in distilled water swells-up while the egg placed in salt solution shrinks.

The external pressure applied to stop the osmosis is termed as osmotic pressure (a Colligative property). Reverse osmosis takes place when the applied external pressure becomes larger than the osmotic pressure.

1.      What do you expect to happen when red blood corpuscles (RBC’s) are placed in 0.5% NaCl solution?

Ans.   RBC’s are isotonic with 0.9% NaCl solution, so they will swell and may even burst when placed in 0.5% NaCl solution.

2.      Which one of the following will have higher osmotic pressure in 1 M KCl or 1 M urea solution?

Ans. 1 M KCl will have higher osmotic pressure because its dissociates to give K + and Cl – ions while urea does not dissociate into ions in the solution.

3. Name one SPM which can be used in the process of reverse osmosis.

Ans. Cellulose acetate placed on a suitable support.

4.      What are isotonic solutions?

Ans. Solutions having equal osmotic pressure are called isotonic solutions.

5.      Write van’t Hoff equation for dilute solution.

Ans. p V = nRT ,

Where, p = Osmotic pressure, n = Number of moles, V = Volume of solution in litre, R = Gas constant ,

T = Temperature

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• Important Questions
• Class 12 - Chemistry
• Chapter 2: Solutions

Important Questions for Class 12 Chemistry Chapter 2 - Solutions

Class 12 chemistry important questions with answers are provided here for chapter 2 Solutions. These important questions are based on the CBSE board curriculum and correspond to the most recent Class 12 chemistry syllabus. By practising these Class 12 important questions, students will be able to quickly review all of the ideas covered in the chapter and prepare for the Class 12 Annual examinations as well as other entrance exams such as NEET and JEE.

Download Class 12 Chemistry Chapter 2 – Solutions Important Questions with Answers PDF by clicking on the button below.

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Class 12 Solutions Important Questions with Answers

Short answer type questions.

1. Components of a binary mixture of two liquids A and B were separated by distillation. After some time separation of components stopped and the composition of the vapour phase became the same as that of the liquid phase. Both the components started coming in the distillate. Explain why this happened.

Solution: When the composition of a binary mixture of two liquids A and B in the liquid state and in the vapour phase is the same, the mixture is known as an azeotropic mixture. In any azeotropic mixture, liquids are boils at the same temperature without undergoing any change in composition.

2. Explain why on the addition of 1 mol of NaCl to 1 litre of water, the boiling point of water increases, while the addition of 1 mol of methyl alcohol to one litre of water decreases its boiling point.

Solution: Sodium chloride (NaCl) is a non-volatile solute. When added to water taken in a beaker, the solute occupies some surface area. As a result, the vapour pressure decreases and the boiling point of the solution increases. On the other hand, methyl alcohol is more volatile than water. The addition of methyl alcohol to water increases the total vapour pressure of the solution. The boiling point of the solution decreases.

3. Explain the solubility rule “like dissolves like” in terms of intermolecular forces that exist in solutions.

Solution: The solubility, in general, is guided by the principle that “Like dissolve Like”. This means that a solute will dissolve in a particular solvent if both have the same nature. The ionic and polar solutes generally dissolve in polar solvents while the non-polar solutes are soluble in non-polar solvents. These are mostly organic in nature i.e benzene, carbon tetrachloride, carbon disulphide etc. However, there are many exceptions also. For example, non-polar solutes like sugar, glucose etc. dissolve in water mainly because of hydrogen bonding.

4. Concentration terms such as mass percentage, ppm, mole fraction and molality are independent of temperature, however molarity is a function of temperature. Explain.

Solution:By definition, molarity takes into account the volume of the solution which changes with a change in temperature. All other terms, such as mass percentage, ppm, mole fraction and molality for expressing the concentration of a solution involve the mass of the solvent which is not influenced by the temperature.

5. What is the significance of Henry’s Law constant K H ?

Solution: Henry’s Law constant (K H ) helps in comparing the relative solubilities of different gases in the same solvent (e.g. water). In general, the lesser the value of K H , the more the solubility of a gas.

6. Why are aquatic species more comfortable in cold water in comparison to warm water?

Solution: The aquatic species are more comfortable in cold water than in warm water. This is because the solubility of any gas in water decreases with the rise in temperature. The solubility of oxygen in water is more in cold water than in warm or hot water. Since oxygen is essential for breathing, aquatic species can breathe more comfortably in cold water than in warm water due to the higher percentage of oxygen present in cold water. Hence, they feel more comfortable in cold water than in warm water.

7. (a) Explain the following phenomena with the help of Henry’s law.

(i) Painful condition known as bends.

(ii) Feeling of weakness and discomfort in breathing at high altitude.

(b) Why does soda water bottle kept at room temperature fizzes on opening?

(i) When scuba divers go deep in the sea, the solubility of atmospheric gases increases in blood. When the divers come up, there is the release of dissolved gases and it leads to the formation of bubbles of nitrogen in our blood capillaries, hence there is a painful sensation called bends. To avoid bends; the tanks of scuba divers are filled with He,N₂ and oxygen.

(ii) At high altitude, partial pressure of oxygen is low, it leads to a low concentration of oxygen in the blood of people living there. A low concentration of oxygen develops anoxia, i.e., unable to think and act properly.

(b) In order to increase the solubility of CO₂ gas in soft drinks and soda water, the bottles are normally sealed under high pressure. An increase in pressure increases the solubility of a gas in a solvent according to Henry’s Law. If the bottle is opened by removing the stopper or seal, the pressure on the surface of the gas will suddenly decrease. This will cause a decrease in the solubility of the gas in the liquid. As a result, it will rush out of the bottle producing a hissing noise or with a fiz.

8. Why is the vapour pressure of an aqueous solution of glucose lower than that of water?

Solution: Evaporation of liquid is a surface phenomenon. The more the surface area available, the more the evaporation of the liquid. Now glucose is a non-volatile solute. It occupies a certain surface area of water. This means evaporation of water from the surface gets reduced and its vapour presence also gets lowered.

9. How does sprinkling of salt help in clearing the snow-covered roads in hilly areas? Explain the phenomenon involved in the process.

Solution: The phenomenon involved in the melting of snow on snow-covered roads is the depression in the freezing point which is caused by the addition of non-volatile impurities to a liquid. The addition of salt (sodium chloride) lowers the freezing point temperature of the water and thus, helps in the melting of snow.

10. What is a “semi-permeable membrane”?

Solution: The membranes which allow only the movement of the solvent molecules through them is called semi-permeable membrane. The membranes appear to be continuous sheets or films. here only the molecules of the solvent can pass while those of the solute which are of bigger size, are not in a position to pass through.

11. Give an example of a material used for making semipermeable membrane for carrying out reverse osmosis.

Solution: Polymer cellulose acetate is used for making semipermeable membrane for carrying out reverse osmosis.

Matching Type Questions

Note: In the following questions match the items given in Column I and Column II.

1. Match the items given in Column I and Column II.

Solution: (a)-(iv); (b)-(iii); (c)-(i); (d)-(ii); (e)-(vi); (f)- (v)

2. Match the items given in Column I with the type of solutions given in Column II.

Solution: (a)-(v); (b)-(iii); (c)-(iv); (d)-(ii); (e)-(i)

3. Match the laws given in Column I with expressions given in Column II.

Solution: (a)-(iii); (b)-(v); (c)-(iv); (d)-(i); (e)-(ii)

4. Match the terms given in Column I with expressions given in Column II.

Solution: (a)-(iv); (b)-(iii); (c)-(ii); (d)-(v); (e)-(i)

Assertion and Reason Type Questions

Note:  In the following questions a statement of assertion followed by a statement of reason is given. Choose the correct answer out of the following choices.

(i) Assertion and reason both are correct statements and reason is the correct explanation for assertion.

(ii) Assertion and reason both are correct statements but the reason is not a correct explanation for assertion.

(iii) Assertion is a correct statement but the reason is the wrong statement.

(iv) Assertion and reason both are incorrect statements.

(v) Assertion is a wrong statement but the reason is a correct statement.

1. Assertion: The molarity of a solution in liquid state changes with temperature.

Reason: The volume of a solution changes with a change in temperature.

Solution: (i) Both are correct statements and reason is the correct explanation for assertion.

2. Assertion: When methyl alcohol is added to water, the boiling point of water increases.

Reason: When a volatile solute is added to a volatile solvent elevation in boiling point is observed.

Solution: (iv) Assertion and reason both are incorrect statements.

3. Assertion: When NaCl is added to water a depression in the freezing point is observed.

Reason: The lowering of the vapour pressure of a solution causes depression at the freezing point.

4. Assertion: When a solution is separated from the pure solvent by a semi-permeable membrane, the solvent molecules pass through it from the pure solvent side to the solution side.

Reason: Diffusion of solvent occurs from a region of high concentration solution to a region of low concentration solution.

Solution: (ii) Assertion and reason both are correct statements but the reason is not a correct explanation for assertion.

Long Answer Type Questions

1. Define the following modes of expressing the concentration of a solution. Which of these modes are independent of temperature and why?

(i) w/w (mass percentage)

(ii) V/V (volume percentage)

(iii) w/V (mass by volume percentage)

(iv) ppm. (parts per million)

(v) x (mole fraction)

(vi) M (Molarity)

(vii) m (Molality)

(i) w/w (mass percentage) : It is defined as the amount of solute in grams present in 100 gram of the solution.

Mass percentage of solute = (mass of solute/ Mass of solution) x 100

= {mass of solute/ (mass of solvent + mass of solute)} x 100

(ii) V/V (volume percentage): It is defined as the volume of solute in mL present in 100 mL solution.

Percentage of solute by volume = (volume of solute/ volume of solution) x 100

(iii) w/V (mass by volume percentage): It is defined as the mass of solute present in 100 mL of solution.

Percent of solute mass by volume = (mass of solute/ volume of solution) x 100

(iv) ppm. (parts per million): It is defined as the quantity of solute in grams present in 10 6 grams of the solution.

ppm = (Mass of solute/ Mass of solution) x 10 6

(v) x (mole fraction): It is defined as the ratio of the number of moles of one component to the total number of moles of the solution.

(vi) M (Molarity): It is defined as the number of moles of the solute present per litre or per dm 3 of the solution.

Molarity = number of moles of solute / Number of litres of the solution

(vii) m (Molality): It is defined as the number of moles of solute present in 1kg of the solvent.

Molality (m) = number of moles of solute / Number of kilograms of solvent

The volume of the solution changes with change in temperature while the mass of the solution is independent of temperature.

Hence w/w (mass percentage), ppm. (parts per million), x (mole fraction) and m (Molality) are independent of temperature as the mass does not depend on temperature.

2.Using Raoult’s law, explain how the total vapour pressure over the solution is related to the mole fraction of components in the following solutions.

(i) CHCl 3 ( l ) and CH₂Cl₂( l ) (ii) NaCl(s) and H₂O ( l )

(i) In this case, CHCl 3 ( l ) and CH₂Cl₂( l ) both the components are volatile liquids.

According to Raoult’s law,

P A = P A 0 χ A ; P B = P B 0 χ B

P = P A + P B

P = P A 0 χ A + P B 0 χ B = P A 0 χ A + P B 0 (1-χ A )

Here, A and B are volatile components

P A and P B are the partial pressures while P is the total vapour pressure.

χ A and χ B are the mole fractions of the components in the binary solution.

(ii) In this case, NaCl(s) is non-volatile and Raoult’s law is applicable only to water which is of volatile nature

P = P A 0 χ A

Here the total vapour pressure of the solution is dependent on the mole fraction of solvent only.

3. Explain the terms ideal and non-ideal solutions in the light of forces of interactions operating between molecules in liquid solutions.

In the case of ideal solution:

(i) The forces of interaction of the components in the solution are the same as in pure components i.e. A….. B interactions are the same as A….. A and B….B. interactions.

(ii) There is no change in volume on mixing the components i.e. ΔV mixing = 0.

(iii) There is no change in ΔH upon mixing the components i.e. ΔH mixing = 0.

(iv) Components obey Raoult’s Law at all temperatures and concentrations i.e.

In case of non-ideal solution:

(i) The forces of interaction of the components in the solution different from those present in pure components i.e. A….B interactions are different from A….. A and B…. B interactions.

(ii) There is a change in volume on mixing the components i.e. ΔV mixing ≠ 0

(iii) There is a change in ΔH on mixing the components i.e. ΔH mixing ≠ 0.

(iv) Components deviate from Raoult’s Law i.e.

P A ≠ P A 0 χ A ; P B ≠ P B 0 χ B

4. Why is it not possible to obtain pure ethanol by fractional distillation? What general name is given to binary mixtures which show deviation from Raoult’s law and whose components cannot be separated by fractional distillation?How many types of such mixtures are there?

• A mixture of ethanol and water is generally obtained when we prepare it commercially with the help of alcoholic fermentation.
• The two liquids are completely miscible with each other. Their boiling points are 351 K and 373K respectively. Since the two liquids differ in their boiling points by more than 20°, they should be easily separated by a fractional distillation process.
• However, during the operation, a stage is reached when we get a liquid mixture containing 95 percent ethanol and 5 percent water. This constitutes an azeotropic mixture also called a constant boiling mixture. Both alcohol and water start boiling together at a temperature which is close to the boiling point temperature of alcohol.

The azeotropic mixture shows a positive deviation from Raoult’s Law. In fact there are two types of azeotropic mixtures.

(a) Azeotropic mixture which shows positive deviation from Raoult’s Law (Minimum boiling azeotrope)

(b) Azeotropic mixture which shows negative deviation from Raoult’s Law (Maximum boiling azeotrope)

5. When kept in water, raisins swell in size. Name and explain the phenomenon involved. Give three applications of the phenomenon.

This happens due to a phenomenon known as osmosis. When the reisin is kept in water, it swells in size. Actually water is a hypotonic solution while the liquid or fluid inside the raisin is of hypertonic nature. The outer wall of the raisin acts as a semipermeable membrane. There is an osmosis of water molecules inside the raisin through this membrane and the raisin slowly swells in size.

Applications of osmosis:

• In animals circulation of water to all parts of the body takes place due to osmosis.
• Osmosis helps in plant growth and germination of seeds.
• When the dried fruits and vegetables are placed in water, they slowly swell because of osmosis.

6. Discuss the biological and industrial importance of osmosis.

Biological importance of osmosis

(i) Osmosis plays a significant role in the absorption of water by plant roots from the soil and its movement to different parts of the plant body.

(ii) When placed in water containing less than 0.9% (mass/volume) salt, blood cells collapse due to loss of water by osmosis.

(iii) In animals circulation of water to all parts of the body takes place due to osmosis.

(iv) Osmosis helps in plant growth and germination of seeds.

The industrial importance of osmosis

(i) The phenomenon of osmosis is also useful in some industrial processes. It is employed commercially for the desalination of seawater so that it may become useful for drinking purposes.(reverse osmosis)

(ii) The Reverse Osmosis process is very popular for the purification of drinking water in households.

7. How can you remove the hard calcium carbonate layer of the egg without damaging its semipermeable membrane? Can this egg be inserted into a bottle with a narrow neck without distorting its shape? Explain the process involved.

The hard layer of egg white in colour, consists of calcium carbonate. It can be removed by placing the egg in dilute hydrochloric acid for some time. It dissolves calcium carbonate, leaving behind the egg without damaging its soft semipermeable membrane.

The size of the egg can be reduced or it shrinks by placing it in saline water (contains NaCl) for some time. The fluid from the egg slowly escapes and passes into saline water which is at higher osmotic pressure (hypertonic in nature). Now, the egg with reduced size can be inserted in a bottle with a narrow neck. If the bottle contains water, the egg will regain its original shape and size due to the osmosis of water (hypotonic) through the semipermeable membrane.

8. Why is the mass determined by measuring a colligative property in case of some solutes are abnormal? Discuss it with the help of the Van’t Hoff factor.

Certain solutes do not behave normally in solution in the sense that they may either undergo dissociation or association. As a result, the number of solute particles in the solution changes.

Since the colligative properties are linked with the number of particles, they show abnormal results. In the same way, the molecular masses of these solutes also show abnormal results.

The exact behaviour of the solute in a solution and the extent of association or dissociation can be expressed in terms of Van’t Hoff factor (i).

i = Normal/ calculated molecular mass/ Observed molecular mass.

or i = Observed colligative properties/ Normal colligative properties.

• If i = 1 , solute behave normally in the solution
• If i > 1 , solute undergo dissociation in solution
• If i < 1 , solute undergo association in solution

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Case Study Questions Haloalkanes and Haloarenes Class 12 Chemistry

        Case Study Questions Haloalkanes and Haloarenes Class 12 Chemistry

1. Read the passage given below and answer the following questions: Nucleophilic substitution reactions are of two types; substitution nucleophilic bimolecular (S N 2) and substitution nucleophilic unimolecular (S N 1) depending on molecules taking part in determining the rate of reaction. The reactivity of alkyl halide towards S N 1 and S N 2 reactions depends on various factors such as steric hindrance, stability of intermediate or transition state, and polarity of the solvent. S N 2 reaction mechanism is favoured mostly by primary alkyl halide or transition state and polarity of the solvent, S N 2 reaction mechanism is favoured mostly by primary alkyl halide then secondary and then tertiary. This order is reversed in the case of S N 1 reactions. (i) Which of the following is most reactive towards nucleophilic substitution reaction? (a) C 6 H 5 Cl (b) CH 2 = CHCl (c) ClCH 2 CH = CH 2 (d) CH 3 CH = CHCl

(ii) Isopropyl chloride undergoes hydrolysis by (a) S N 1 mechanism (b) S N 2 mechanism (c) S N 1 and S N 2 mechanism (d) Neither S N 1 nor S N 2 mechanism

(iii) Tertiary alkyl halides are practically inert to substitution by S N 2 mechanism because of (a) Insolubility (b) Instability (c) Inductive effect (d) Steric Hindrance

(iv) Which of the following is the correct order of decreasing S N 2 reactivity? (a) RCH 2 X > R 2 CHX > R 3 CX (b) R 3 CX > R 2 CHX >RCH 2 X (c) R 2 CHX > R 3 CX > RCH 2 X (d) RCH 2 X > R 3 CX > R 2 CHX

(v) An organic molecule necessarily shows optical activity if it- a) Contains asymmetric carbon atoms b) Is non-polar c) Is non-superimposable on its mirror image d) Is superimposable on its mirror image.

2. Read the passage given below and answer the following questions: The replacement of hydrogen atom in a hydrocarbon, aliphatic or aromatic results in the formation of haloalkanes and haloarenes respectively. Haloalkanes contain a halogen atom attached to sp 3 hybridized carbon atom of an alkyl group whereas haloarenes contain a halogen atom attached to sp 2 hybridized carbon atom of an aryl group. Haloalkanes and haloarenes may be classified on the basis of the number of halogen atoms in their structures as mono, di, or poly halogen compounds and also on the basis of the state of hybridization of the carbon atom to which the halogen atom is bonded. (i) Which of the following halide is 2°? (a) Isopropyl chloride (b) Isobutyl chloride (c) n-propyl chloride (d) n-butyl chloride

(ii) Which of the following is a Gem-dibromide is: (a) CH 3 CH(Br)CH 2 (Br) (b) CH 3 CBr 2 CH 3 (c) CH 2 (Br)CH 2 CH 2 (d) CH 2 BrCH 2 Br

(iii) IUPAC name of (CH 3 ) 3 CCl is: (a) 3-Chlorobutane (b) 2-Chloro-2-methylpropane (c) t-butyl chloride (d) n-butyl chloride

(iv) Which of the following is a primary halide? (a) Isopropyl iodide (b) Secondary butyl iodide (c) Tertiarybutyl bromide (d) Neohexyl chloride

(v) Which one of the following is not an allylic halide? (a) 4-Bromopent-2-ene (b) 3-Bromo-2-methylbut-1-ene (c) 1-Bromobut-2-ene (d) 4-Bromobut-1-ene

3. Read the passage given below and answer the following questions: Alkyl halides are prepared by the free radical halogenation of alkanes, addition of halogen acids to alkenes, replacement of -OH group of alcohols with halogens using phosphorus halides, thionyl chloride, or halogen acids. Aryl halides are prepared by electrophilic substitution to arene. Fluorine and iodides are best prepared by the halogen exchange method. These compounds find wide applications in industry as well as in day-to-day life. These compounds are generally used as solvents and as starting materials for the synthesis of a large number of organic compounds. (i) The best method for the conversion of an alcohol into an alkyl chloride is by treating the alcohol with (a) PCl 5 (b) Dry HCl in the presence of anhydrous ZnCl 2 (c) SOCl 2 in presence of pyridine (d) None of these

(ii) The catalyst used in the preparation of an alkyl chloride by the action of dry HCl on alcohol is (a) anhydrous AlCl 3 (b) FeCl 3 (c) anhydrous ZnCl 2 (d) Cu

(iii) An alkyl halide reacts with metallic sodium in dry ether. The reaction is known as: (a) Frankland’s reaction (b) Sandmeyer’s reaction (c) Wurtz reaction (d) Kolbe’s reaction

(iv) Fluorobenzene (C 6 H 5 F) can be synthesized in the laboratory (a) By direct fluorination of benzene with F 2 gas (b) By reacting bromobenzene with NaF solution (c) By heating phenol with HF and KF (d) From aniline by diazotization followed by heating the diazonium salt with HBF 4

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Get here all the Important questions for Class 12 Chemistry chapter wise as free PDF download. Here you will get Extra Important Questions with answers, Numericals and Multiple Choice Questions (MCQ's) chapter wise in Printable format. Solving Chapter wise questions is one of the best ways to prepare for the examination. Students are advised to understand the concepts and theories of Chemistry properly before the exam. You can easily find 1 Mark, 2 marks, 3 marks, and 5 marks questions from each chapter of Class 12 Chemistry and prepare for exam more effectively. These preparation material for Class 12 Chemistry , shared by teachers, parents and students, are as per latest NCERT and CBSE Pattern syllabus and assure great success in achieving high score in Final CBSE Board Examinations.

Latest MCQ's and Important Questions for CBSE Class 12 Chemistry

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Total Papers :

CBSE Class 12 Chemistry Syllabus

• Solid State
• Electrochemistry
• Chemical Kinetics
• Surface Chemistry
• General Principles and Processes of Isolation of Elements
• p-Block Elements
• d- and f-Block Elements
• Coordination Compounds
• Haloalkanes and Haloarenes.
• Alcohols, Phenols and Ethers
• Aldehydes, Ketones and Carboxylic Acids
• Organic compounds containing Nitrogen
• Biomolecules
• Chemistry in Everyday life

Unit II: Solutions 15 Periods

Types of solutions, expression of concentration of solutions of solids in liquids, solubility of gases in liquids, solid solutions, Raoult's law, colligative properties - relative lowering of vapour pressure, elevation of boiling point, depression of freezing point, osmotic pressure, determination of molecular masses using colligative properties, abnormal molecular mass, Van't Hoff factor.

Unit III: Electrochemistry 18 Periods

Redox reactions, EMF of a cell, standard electrode potential, Nernst equation and its application to chemical cells, Relation between Gibbs energy change and EMF of a cell, conductance in electrolytic solutions, specific and molar conductivity, variations of conductivity with concentration, Kohlrausch's Law, electrolysis and law of electrolysis (elementary idea), dry cell-electrolytic cells and Galvanic cells, lead accumulator, fuel cells, corrosion.

Unit IV: Chemical Kinetics 15 Periods

Rate of a reaction (Average and instantaneous), factors affecting rate of reaction: concentration, temperature, catalyst; order and molecularity of a reaction, rate law and specific rate constant, integrated rate equations and half-life (only for zero and first order reactions), concept of collision theory (elementary idea, no mathematical treatment), activation energy, Arrhenius equation.

Unit VIII: d and f Block Elements 18 Periods

General introduction, electronic configuration, occurrence and characteristics of transition metals, general trends in properties of the first-row transition metals – metallic character, ionization enthalpy, oxidation states, ionic radii, colour, catalytic property, magnetic properties, interstitial compounds, alloy formation, preparation and properties of K2Cr2O7 and KMnO4.

Lanthanoids – Electronic configuration, oxidation states, chemical reactivity and lanthanoid contraction and its consequences.

Actinoids - Electronic configuration, oxidation states and comparison with lanthanoids.

Unit IX: Coordination Compounds 18 Periods

Coordination compounds - Introduction, ligands, coordination number, colour, magnetic properties and shapes, IUPAC nomenclature of mononuclear coordination compounds. Bonding, Werner's theory, VBT, and CFT; structure and stereoisomerism, the importance of coordination compounds (in qualitative analysis, extraction of metals and biological system).

Unit X: Haloalkanes and Haloarenes. 15 Periods Haloalkanes: Nomenclature, nature of C–X bond, physical and chemical properties, optical rotation mechanism of substitution reactions.

Haloarenes: Nature of C–X bond, substitution reactions (Directive influence of halogen in monosubstituted compounds only). Uses and environmental effects of - dichloromethane, trichloromethane, tetrachloromethane, iodoform, freons, DDT.

Unit XI: Alcohols, Phenols and Ethers 14 Periods

Alcohols: Nomenclature, methods of preparation, physical and chemical properties (of primary alcohols only), identification of primary, secondary and tertiary alcohols, mechanism of dehydration, uses with special reference to methanol and ethanol.

Phenols: Nomenclature, methods of preparation, physical and chemical properties, acidic nature of phenol, electrophilic substitution reactions, uses of phenols.

Ethers: Nomenclature, methods of preparation, physical and chemical properties, uses.

Unit XII: Aldehydes, Ketones and Carboxylic Acids 15 Periods

Aldehydes and Ketones: Nomenclature, nature of carbonyl group, methods of preparation, physical and chemical properties, mechanism of nucleophilic addition, reactivity of alpha hydrogen in aldehydes, uses.

Carboxylic Acids: Nomenclature, acidic nature, methods of preparation, physical and chemical properties; uses.

Unit XIII: Amines 14 Periods

Amines: Nomenclature, classification, structure, methods of preparation, physical and chemical properties, uses, identification of primary, secondary and tertiary amines.

Diazonium salts: Preparation, chemical reactions and importance in synthetic organic chemistry.

Unit XIV: Biomolecules 18 Periods

Carbohydrates - Classification (aldoses and ketoses), monosaccharides (glucose and fructose), D-L configuration oligosaccharides (sucrose, lactose, maltose), polysaccharides (starch, cellulose, glycogen); Importance of carbohydrates.

Proteins - Elementary idea of - amino acids, peptide bond, polypeptides, proteins, structure of proteins - primary, secondary, tertiary structure and quaternary structures (qualitative idea only), denaturation of proteins; enzymes. Hormones - Elementary idea excluding structure.

Vitamins - Classification and functions. Nucleic Acids: DNA and RNA.

Structure of CBSE Chemistry Sample Paper for Class 12 Science is

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Question Bank of Other Subjects of Class 12

Importance of Question Bank for Exam Preparation?

There are many ways to ascertain whether a student has understood the important points and topics of a particular chapter and is he or she well prepared for exams and tests of that particular chapter. Apart from reference books and notes, Question Banks are very effective study materials for exam preparation. When a student tries to attempt and solve all the important questions of any particular subject , it becomes very easy to gauge how much well the topics have been understood and what kind of questions are asked in exams related to that chapter.. Some of the other advantaging factors of Question Banks are as follows

• Since Important questions included in question bank are collections of questions that were asked in previous exams and tests thus when a student tries to attempt them they get a complete idea about what type of questions are usually asked and whether they have learned the topics well enough. This gives them an edge to prepare well for the exam.Students get the clear idea whether the questions framed from any particular chapter are mostly either short or long answer type questions or multiple choice based and also marks weightage of any particular chapter in final exams.
• CBSE Question Banks are great tools to help in analysis for Exams. As it has a collection of important questions that were asked previously in exams thereby it covers every question from most of the important topics. Thus solving questions from the question bank helps students in analysing their preparation levels for the exam. However the practice should be done in a way that first the set of questions on any particular chapter are solved and then solutions should be consulted to get an analysis of their strong and weak points. This ensures that they are more clear about what to answer and what can be avoided on the day of the exam.
• Solving a lot of different types of important questions gives students a clear idea of what are the main important topics of any particular chapter that needs to focussed on from examination perspective and should be emphasised on for revision before attempting the final paper. So attempting most frequently asked questions and important questions helps students to prepare well for almost everything in that subject.
• Although students cover up all the chapters included in the course syllabus by the end of the session, sometimes revision becomes a time consuming and difficult process. Thus, practicing important questions from Question Bank allows students to check the preparation status of each and every small topic in a chapter. Doing that ensures quick and easy insight into all the important questions and topics in each and every individual. Solving the important questions also acts as the revision process.

Question Bank of Other Classes

To Prepare better for CBSE paperclass; ?> " title="Download Free CBSE Papers">Ribblu.com brings to you all the previous years papers & worksheets of subject; ?//> for CBSE paperclass; ?>. This CBSE paper and worksheet can be instrumental in students achieving maximum marks in their exams. These Papers and worksheets help students gain confidence and make them ready to face their school examinations. These Papers and worksheets school wise, covers important concepts from an examination perspective. Students and parents can download all the available papers & worksheets directly in the form of PDF. One can use these papers and worksheets to get extensive practice and familiarise themselves with the format of the question paper.

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PSEB Class 12 Chemistry Paper Analysis 2024: Difficulty Level, Question Paper PDF and Answer Key

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PSEB Class 12 Chemistry Exam Analysis 2024: The Punjab School Education Board (PSEB) is successfully conducting the intermediate board examinations for the 2023-24 session. The board started conducting the PSEB 12th exams on February 13, 2024, in pen and paper format. Today, it was the Chemistry paper for class 12 students which was held for 3 hours and 15 minutes. The exam started at 11:00 AM and ended at 2:15 PM. As the exam concludes, it’s important to discuss the pattern and difficulty level of the questions included to evaluate the overall performance of students. Here’s the detailed analysis of the PSEB Class 12 Chemistry Paper 2024 which is based on the the experts’ review and the reactions of students who appeared for the exam. In addition to this, the PSEB Class 12 Chemistry Question Paper 2024 can also be downloaded here along with its answer key. The answer key includes answers and solutions to all objective and short answer type questions.

PSEB Class 12 Chemistry  Exam 2024   Highlights

Pattern of pseb class 12 chemistry  paper   2024.

The PSEB Class 12 Chemistry question paper was for 70 marks and had a total of 17 questions. The questions were distributed as follows:

• Question No. 1 had 28 parts carrying 1 mark each (MCQs & True/False)
• Question No. 2 to 11 were for 2 marks each.
• Question No. 12 to 15 were for 3 marks each.
• Question No. 16and 17 were for 5 marks each

 All questions were compulsory, however, internal choices were provided in some questions.

PSEB  Class 12 Chemistry  Paper Analysis 2024: Student Reactions

Students who appeared for the Chemistry exam found the paper simple and well-balanced. “All the questions were direct and numerical calculations were simple” expressed a student of a government school in Chandigarh region. Some of the common reviews are as follows:

• The paper was entirely based on the prescribed s 
• MCQs were direct and easy.
• 3 and 5 Mark questions were balanced.
• Averagely, students are expecting 60-70 marks out 80.

PSEB Class 12 Chemistry  Paper Analysis 2024: Expert Review

The expert analysis includes comments and reviews from the subject teachers. The PSEB Chemistry Exam has been reviewed as moderate and balanced. “The question paper followed the pattern provided in the PSEB model paper and was a perfect blend of easy and challenging questions,” mentioned a Chemistry PGT, Khalsa School, Chandigarh.  

PSEB Class 12 Chemistry Question Paper 2024

Below is a preview of the PSEB Class 12 Chemistry Question Paper for Board Exam 2024:

Answers will be updated soon!

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Chemistry Case Study for Class 12 (Download Free PDF)

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Chemistry Case Study for Class 12

While preparing for the board exams, students are being judged on different levels of skills, such as writing, reading, etc. Chemistry Case Study for Class 12 questions are one of them that helps in assessing critical thinking.

The Central Board of Secondary Education will be asking the case study questions in the Class 12 board examination. Therefore, here on this page, we have provided the Chemistry Case Study for Class 12 at free of cost. Our subject matter experts have prepared Case Study questions so that Apart from the basic standard questions, students can have a variety of problems to solve. 

Just like MCQs, and other written types questions Chemistry Case Study for Class 12 questions will impact the overall performance of a student. Therefore for the convenience of the students we have provided the download links here, so that they can easily access the Class 12 Case Study.

Download Chapter Wise Chemistry Case Study for Class 12 Question and Answers PDF 

There are lots of chapters in class 12 Chemistry from which Class 12 Case Study Questions can be framed. Going through such types of questions help the students to assess their understanding level in the topics discussed in NCERT Class 12 Chemistry Books. By practicing the Class 12 Case Study Questions for Chemistry students will be very confident to ace the board exam. Also the Chemistry case study will be very useful for the NEET exam preparation.

Doing a regular practice of Class 12 Chemistry Case Study questions is a great way to score higher marks in the board exams as it will help students to develop a grip on the concepts. 

Here our subject experts have crafted the Chapter Wise Case Study For Class 12. Download Chapter Wise CBSE Case Study Class 12 Question and Answers PDF from the below given links.

Case Study Questions Class 12 Chapter 1 The Solid State

Case Study Questions Class 12 Chapter 2 Solutions

Case Study Questions Class 12 Chapter 3 Electrochemistry

Case Study Questions Class 12 Chapter 4 Chemical Kinetics

Case Study Questions Class 12 Chapter 5 Surface Chemistry  

Case Study Questions Class 12 Chapter 7 The p-Block Elements

Case Study Questions Class 12 Chapter 8 The d- and f-Block Elements

Case Study Questions Class 12 Chapter 9 Coordination Compounds

Case Study Questions Class 12 Chapter 10 Haloalkanes And Haloarenes

Case Study Questions Class 12 Chapter 11 Alcohols, Phenols And Ethers

Case Study Questions Class 12 Chapter 12 Aldehydes. Ketones & Carboxylic Acids

Case Study Questions Class 12 Chapter 13 Amines

Case Study Questions Class 12 Chapter 14 Biomolecules

Case study types of questions are generally descriptive that helps to gather more information easily so, it is kinda easy to answer. However, our subject matter experts have given the solutions of all the Chemistry Case Study for Class 12 Chemistry questions.

Passage Based Class 12 Chemistry Case Study Questions in PDF

CBSE Class 12 Case studies are known as Passage Based Questions. These types of problems usually contain a short/long paragraph with 4 to 5 questions. 

Students can easily solve Passage Based Class 12 Case Study Questions by reading those passages. By reading the passage students will get the exact idea of what should be the answers. Because the passage already contains some vital information or data. However a better understanding of the basic concepts that can be learned from the NCERT Class 12 Textbooks will aid in solving the Case based questions or passage based questions.

How to Download CBSE Case Study of Class 12 Chemistry ?

Follow the below given simple steps to know how to download CBSE Case Study of Class 12 Chemistry:-

• Open Selfstudys website in your browser
• Go to the navigation menu that look like this
• Now, click on CBSE and then Case Study respectively
• A new page will open, where you have to click on “Class 12”
• Now, you are ready to select the subject for which you want to download the case study questions.

How to Solve Chemistry Case Study Based Questions of Class 12?

There are very simple methods that a student should keep in mind while solving Chemistry Case Study for Class 12:

• Read each line of paragraph carefully and pay attention to the given data/numbers. Often questions are framed according to the highlighted data of the passage.
• Since case study questions are often framed in Multiple choice questions, students should have the knowledge of elimination methods in MCQs.
• Having a good understanding of the topics that are discussed in CBSE Class 12 Books are ideal to Solve Case Study Based Questions of Class 12.

Features Of Class 12 Chemistry Case Study Questions And Answers PDF

The three most noticeable features of Class 12 Chemistry Case Study Questions And Answers Pdf are -

• It Is Free To Use:  Keeping in mind the need of students and to help them in doing Self Study, our team has made all the PDF of Chemistry Case Study for Class 12 free of cost.
• Answers Are Given:  Not only the PDFs are free provided but answers are given for all the questions of Chemistry Case Study for Class 12. 
• PDF Can Be Downloaded Or Viewed Online:  Many students don’t like to download the PDFs on their device due to the shortage of storage. Therefore, CBSE Class 12 Case Study questions are made available here in online format, so that students can view them online. However, through the Selfstudys app, a learner can download the PDFs too.

Benefits of Using CBSE Class 12 Chemistry Case Study Questions and Answers

The CBSE Class 12 Chemistry Case Study Questions and Answers can help a student in several ways:

• In Exam Preparation:  Those who go through the Chemistry Case Study for Class 12 will find support during the exam preparation as case based questions are also asked in the CBSE Class 12 Board examination. 
• Help in brushing up the previous learnings:  No matter how brilliant you are, you have to revise the studied topics time and again to keep them refreshed. And in this task, the CBSE Class 12 Case Study Questions and Answers can help a lot.
• To develop the critical thinking:  Able to analyse information and make an objective judgement is a skill that is known as critical thinking. A student of class 12 can use Chemistry Case Study for Class 12 with answers to develop critical thinking so that they can make better decisions in their life and in the board examination.

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