MP Board Class 12 Chemistry Important Questions, Practice Now

Chemistry is an important subject for MP Board Class 12 students, especially for those preparing for competitive exams or pursuing science-related careers. The subject includes physical chemistry, organic chemistry, and inorganic chemistry, which require both conceptual clarity and memorization of reactions, formulas, and mechanisms.

MP Board Class 12 Chemistry Important Questions are extremely helpful for exam preparation. These questions are selected based on previous exam patterns, frequently asked topics, and important concepts from the syllabus.

By practicing these important questions chapter-wise, students can identify high-weightage topics, revise key reactions and formulas, and gain confidence in answering both theoretical and numerical questions during the exam.

MP Board Class 12 Chemistry Important Questions

MP Board Class 12 Chemistry Important Questions are given here chapter-wise. It helps students prepare each unit systematically. These questions focus on key concepts, chemical reactions, derivations, and numerical problems that are commonly asked in the MPBSE Class 12 Chemistry examination.

Practicing important questions from each chapter helps students revise major topics efficiently and understand the type of questions that may appear in the exam. It also makes last-minute revision easier and more organized.

SECTION-A

Question 1 to 6 are MCQ Based questions carrying 1 mark each

Q1. Identify the phase of solute and solvent among the options are given below, for a solution as amalgam of mercury with sodium.

Answer: (C) Solute - Liquid, Solvent - Solid.

Q2. Maximum amount of a solid solute that can be dissolved in a specified amount of a given liquid solvent does not depend upon 

(A) Temperature
(B) Nature of solute
(C) Pressure
(D) Nature of solvent

Answer: (C) Pressure. Pressure does not have any significant effect on the solubility of solids in liquids because solids and liquids are highly incompressible.

Q3. Which is not true for a standard hydrogen electrode?
(A) The hydrogen ion concentration is 1 M
(B) Temperature is 25°C
(C) Pressure of hydrogen is 1 atmosphere
(D) It contains a metallic conductor which does not adsorb hydrogen

Answer: 

Q4. In an electrochemical cell:
(A) potential energy changes into kinetic energy.
(B) kinetic energy changes into potential energy.
(C) chemical energy changes into electrical energy.
(D) electrical energy changes into chemical energy.

Answer: (C) chemical energy changes into electrical energy. In a galvanic cell, a redox reaction occurs spontaneously and released chemical energy is converted to electrical energy.

Q5. Chemical kinetics deals with:
(A) rate of reaction
(B) factors affecting rate of reaction
(C) mechanism of the reaction
(D) All of these

Answer: (D) All of these. Chemical kinetics deals with the rate, factors affecting the rate, and the mechanism.

Q6. Rate law can be determined from balanced chemical equation if
(A) reverse reaction is involved
(B) it is an elementary reaction
(C) it is a sequence of elementary reactions
(D) any of the reactants is in excess

Answer: (B) it is an elementary reaction. In elementary reactions, the rate law is directly based on the stoichiometric coefficients of the reactants.

Q7. Fill in the blanks. (1*6 = 6)

(i). The unit of molarity is ___.
(ii). Raoult's law states that the relative lowering of vapour pressure is equal to the mole fraction of the ___.
(iii). The standard electrode potential of hydrogen electrode is assigned a value of ___.
(iv). In a galvanic cell, the cathode is the electrode where ___ takes place.
(v). The unit of rate constant for a first order reaction is ____.
(vi). The half-life of a first order reaction is given by the expression ____. 

Ans: (i). mol L⁻¹
(ii). solute
(iii). 0.00 volt
(iv). reduction
(v). s⁻¹
(vi). 0.693/k

Q8. Write True / False (1*6= 6)

I. In an ideal solution, the enthalpy of mixing is zero.
II. In a galvanic cell, oxidation takes place at the cathode.
III. For a first order reaction, the half-life is independent of the initial concentration.
IV. The unit of molality is mol L⁻¹.
V. Benzene reacts with chlorine in the presence of FeCl3 to give chlorobenzene.
VI. A catalyst increases the rate of a reaction by increasing activation energy.

Ans: I. (True)
II. (False)
III. (True)
IV. (False)
V. (True)
VI. (False)

Q9. Match the correct pair and write (1* 5 = 5)

Answers:

1 – a

2 – b

3 – c

4 – d

5 – e

Q10. Write the answer in one word (1* 5 = 5)

I. The process of separating solute particles from solvent through a semipermeable membrane:
II. The unit of cell constant:
III. The order of a reaction whose rate does not depend on reactant concentration:
IV. The law relating relative lowering of vapour pressure to mole fraction of solute:
V. The effect of temperature on rate constant is given by which equation? 

Text Solution:

l. Answer: Osmosis
ll. Answer: m 1
lll. Answer: Zero
lV. Answer: Raoult’s law
V. Answer: Arrhenius equation

SECTION-B

Question 11-17 carry 2 marks each. Word limit is 75 words approx.

Q11. Write the integrated rate equation for a first order reaction. 

Answer: For a first order reaction:

Q12. Define half-life period of a reaction.
Answer:

Q13. How does a catalyst increase the rate of reaction? 

Answer: A catalyst provides an alternative reaction pathway with lower activation energy, allowing more reactant molecules to have sufficient energy to react.

Q14. State Faraday's first law of electrolysis. 

Answer: 

Q15. What is the effect of temperature on the rate constant of a reaction? 

Answer: Rate constant increases with temperature because higher temperature increases the kinetic energy of molecules, leading to more effective collisions. This is given by the Arrhenius equation: 

Q16. What is van't Hoff factor (i)? 

Answer: It is the ratio of the observed value of a colligative property to its calculated value assuming no association/dissociation.

Q17. What is a salt bridge? State its two functions. 

Answer: A salt bridge is a U-shaped tube filled with concentrated inert electrolyte in agar or gel. Functions: 1. Maintains electrical neutrality by allowing ion flow. 2. Prevents mixing of solutions in the two half-cells.

SECTION-C

Question from 18-21 carry 3 marks each. Word limit is approximately 75 words.

Q18.

Ans: 

Q19. Explain the effect of dilution on molar conductivity for strong and weak electrolytes.

Answer: * Strong electrolytes: Molar conductivity increases slowly with dilution because ions are already fully dissociated; the increase is due to decrease in inter-ionic attraction.

• Weak electrolytes: Molar conductivity increases sharply with dilution because ionisation increases as per Ostwald's dilution law.

Q20. Derive the half-life expression for a first order reaction. 

Answer: 

Q21. Differentiate between ideal and non-ideal solutions with one example each.

Answer:

• Non-ideal solution: Deviates from Raoult’s law; shows positive or negative deviation. Example: ethanol + acetone (positive deviation).

SECTION-D

Question 22-25 carry 4 marks each. Word limit is 120 words approximately.

Q22. Explain the colligative property of depression in freezing point and derive its expression.

Answer: 

Derivation: Solute lowers the vapour pressure, so freezing occurs at a lower temperature. From Clausius–Clapeyron equation and molality definition, the above relationship is obtained. This property depends only on the number of solute particles, not their nature.

Q23. Discuss the working of a lead storage battery with reactions at electrodes. 

Answer: 

Q24. Describe the effect of temperature and catalyst on the rate of reaction. 

Ans:

Q25. Define solubility of a solid in a liquid. Discuss factors affecting it. 

Answer: Solubility is the maximum amount of solute that can dissolve in a given quantity of solvent at a specified temperature and pressure. 

Factors:

1. Nature of solute & solvent: "Like dissolves like".

2. Temperature: Generally increases with temperature if dissolution is endothermic.

3. Pressure: Has negligible effect on solids in liquids.

4. Particle size: Smaller particles dissolve faster due to larger surface area.

MP Board Class 12 Hindi Important Questions PDF

Students often prefer preparing with Chemistry H2 Important Questions PDFs because they make revision more structured and convenient. Solving these questions helps students focus on key concepts, understand common reaction mechanisms, and become familiar with the pattern of exam questions.

How to Use MP Board Class 12 Chemistry Important Questions for Exam Preparation?

Using MP Board Class 12 Chemistry Important Questions effectively can help students improve their exam preparation and boost their confidence before the board exam.

• Students should begin by revising the theory, important formulas, and chemical reactions from each chapter. 

• After understanding the concepts, they should solve the important questions to test their knowledge and identify weak areas.

• It is also helpful to practice writing structured answers for theoretical questions and step-by-step solutions for numerical problems. 

• Revising key reactions regularly and solving questions from previous year papers can further strengthen preparation.

By consistently practicing these important questions along with regular revision, students can improve their conceptual clarity, reduce mistakes, and perform better in the MP Board Class 12 Chemistry exam.