CBSE Class 12 Chemistry Solutions MCQs Set B

CBSE Class 12 Chemistry Solutions MCQs Set B with answers available in Pdf for free download. The MCQ Questions for Class 12 Chemistry with answers have been prepared as per the latest syllabus, NCERT books and examination pattern suggested in Standard 12 by CBSE, NCERT and KVS. Multiple Choice Questions are an important part of Term 1 and Term 2 exams for Grade 12 Chemistry and if practiced properly can help you to get higher marks. Refer to more Chapter-wise MCQs for NCERT Class 12 Chemistry and also download more latest study material for all subjects

Solutions Class 12 Chemistry MCQ

Class 12 Chemistry students should refer to the following multiple-choice questions with answers for Solutions in standard 12. These MCQ questions with answers for Grade 12 Chemistry will come in exams and help you to score good marks

Solutions MCQ Questions Class 12 Chemistry with Answers

Solutions

I. MCQ - Choose Appropriate Alternative

1. Molarity is the number of moles of a solute dissolved per __________. (dm3 of a solution, dm3 of solvent, Kg of solvent)

2. Molality is defined as the number of moles of solute dissolved per __________. (dm3 of solution, kg of solvent, kg of solute)

3. The solubility of a solute __________ with the increase of temperature. (increases, decreases, does not alter)

4. The loss of electron during a chemical reaction is known as __________. (Oxidation, Reduction, Neutralization)

5. The gain of electron during a chemical reaction is known as __________. (Oxidation, Reduction, Neutralization)

6. The ions, which are attracted towards the anode, are known as __________. (Anins, Cations, Positron).

7. The pH of a neutral solution is __________. (1.7, 7, 14)

8. A current of one ampere flowing for one minute is equal to __________. (One coulomb, 60 coulomb, one Faraday)

9. A substance, which does not allow electricity to pass through, is known as __________. (Insulator, Conductor, Electrolyte)

10. Such substances, which allow electricity to pass through them and are chemically decomposed, are called __________. (Electrolytes, Insulators, Metallic conductors)

11. __________ is an example of strong acid. (Acetic Acid, Carbonic Acid, Hydrochloric Acid)

12. __________ is an example of weak acid. (Hydrochloric Acid, Acetic Acid, Sulphuric Acid)

13. When NH4Cl is hydrolyzed, the solution will be __________. (Acidic, Basic, Neutral)

14. When Na2CO3 is hydrolyzed, the solution will be __________. (Acidic, Basic, Neutral)

15. When blue hydrated copper sulphate is heated __________. (It changes into white, it turns black, it remains blue)

16. Sulphur has the highest oxidation number in __________. (SO2, H2SO4, H2SO3)

17. The reaction between an acid and a base to form a salt and water is called __________. (Hydration, Hydrolysis, Neutralization)

18. __________ is opposite of Neutralization. (Hydration, Hydrolysis, Ionization)

19. The substance having pH value 7 is __________. (Basic, Acidic, Neutral)

20. An aqueous solution whose pH is zero is __________(Alkaline, Neutral, Strongly Acidic)

21. Solubility product of slightly soluble salt is denoted by __________. (Kc, Kp, Ksp)

22. The increase of oxidation number is known as __________. (Oxidation, Reduction, Hydrolysis)

23. The decrease of Oxidation number is known as __________. (Oxidation, Reduction, Electrolysis)

24. One molar solution of glucose contains __________ gms of glucose per dm3 of solution. (180, 100, 342)

25. The number of moles of solute present per dm3 of solution is called __________. (Molality, Molarity, Normality)

26. ‘M’ is the symbol used for representing __________.(Molality, Molarity, Normality)

27. 1 mole of H2SO4 is equal to __________.(98gms, 49gms, 180gms)

28. Buffer solution tends to __________ pH.

29. The logarithm of reciprocal of hydroxide ion is represented as __________.(pH, pOH, pOH)

30. In __________ water molecules surround solute particles.(Hydration, Hydrolysis, Neutralization)

 

II. Fill in the Blank

1. A mixture of two or more substances, which are homogeneously mixed, is called a __________. 
2. __________ is defined as the amount of solute dissolved in a given amount of solvent. 
3. A solution is composed of two components __________ and __________. 
4. A solution containing one mole of solute per dm3 of solution is called one __________ solution.
5. Molarity is denoted by __________. 
6. 1M solution of NaOH contains __________ gms of it dissolved per dm3 of solution.
7. A solution containing one mole of solute dissolved by per kg of solvent is called __________ solution.
8. Molality is denoted by __________.
9. 1M solution of H2SO4 contains __________ gms of it per kg of solvent.
10. The process in which ions are surrounded by water molecules is called __________.
11. The water molecules attached with the hydrated substance are called __________.
12. Hydrated copper sulphate evolves __________ water molecules on heating.
13. The interaction between salt and water to produce acids and bases is called __________.
14. The products of ionic concentration in a saturated solution at a certain temperature are called the __________.
15. Solubility product constant expressed as __________.
16. The suppression of ionization by adding a common ion is called __________.
17. The process of dissociation of an electrolyte into ions is known as __________.
18. The chemical decomposition of a compound in a solution or in fused state brought about by a flow of electric current is known as __________.
19. Electrolysis is performed in an electrolytic cell, which is known as __________.
20. The positive electrode of a voltmeter is called __________ and negative as __________.
21. A solution, which tends to resist changes in pH is called a __________ solution.
22. A mixture of acetic acid and sodium acetate acts as a __________.
23. According to Sorenson __________ is defined as negative logarithm of the hydrogen ion concentration.
24. pH is mathematically expressed as __________.
25. The pH of a neutral solution is __________.
26. __________ substances have pH values lower than 7.
27. __________ solutions have pH values more than 7.
28. Oxidation is __________ of electron.
29. Reduction is the __________ of electron.
30. Such chemical reactions in which the oxidation number of atoms or ions is changed are called __________ reactions.
31. Oxidation number of a free element is __________.
32. Oxidation number of Oxygen in a compound is __________.
33. The sum of oxidation number of any formula of a compound is __________.
34. The oxidation number of any ion is equal to the __________ on the ion.
35. __________ is the reaction in which an acid reacts with a base to form salt and water.
36. __________ are organic compounds which change colour in accordance with the pH of the medium.
37. An indicator that changes from colourless to pink in the presence of an alkaline solution is called __________.
38. An indicator that changes from red to yellow in the presence of an alkaline solution is called __________.
39. Dissociation constant is denoted by __________.
40. According to Bronsted-Lowry Concept, __________ is the donor of proton and __________ is the acceptor of proton.
41. According to Arrhenius, acid is substance that produces __________ ions when dissolved in water.
42. According to Arrhenius, base is a substance that produces __________ ions when dissolved in water.
43. When ionic product is less than ksp, the solution will __________.
44. When ionic product is greater than ksp, the solution will __________.
45. The electrode at which oxidation takes place is called __________.
46. The electrode at which reduction takes place is called __________.
47. H3O+ ion is called __________ ion.
48. The logarithm of reciprocal of hydroxyl ion (OH)- is called __________.
49. Aqueous solution of NH4Cl is __________ while that of NaHCO3 is __________.
50. The ionic product of [H+] and [OH-] of pure water is __________.
51. An increase in the oxidation number of an element or ion during a chemical change is called __________.
52. A decrease in the oxidation number of an element or ion during a chemical change is called __________.
53. The degree of dissociation __________ with the increase in temperature.
54. The degree of dissociation __________ with the dilution of electrolytic solution.
55. A __________ consists of an electrode immersed in solution of its ion.
56. The potential difference between the electrode and the solution of its salt at equilibrium position is called __________ potential.
57. If the pH of a solution is 14, the solution is __________.
58. If the pH of a solution is 4, the solution is __________.
59. The oxidation number of Mn in KMnO4 is __________.
60. The oxidation number of Fe in FeCl3 is __________.

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