Class 11 Chemistry Chapter 1 Some Basic Concepts of Chemistry MCQ Questions with Answers

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Some Basic Concepts of Chemistry Class 11 MCQ

Class 11 Chemistry MCQ with answers are given here to Chapter 1 Some Basic Concepts of Chemistry. These MCQs are based on the latest CBSE board syllabus and relate to the latest Class 11 Chemistry syllabus. By Solving these Class 11 MCQs, you will be able to analyze all of the concepts quickly in the chapter and get ready for the Class 11 Annual exam.

Learn Class 11 Some Basic Concepts of Chemistry MCQs with answers pdf free download according to the latest CBSE and NCERT syllabus. Students should prepare for the examination by solving CBSE Class 11 Chemistry Some Basic Concepts of Chemistry MCQ with answers given below

Question 1. The oxide of an element contains 67.67% oxygen and the vapour density of its volatile chloride is 79. Equivalent weight of the element is:
(a) 2.46
(b) 3.82
(c) 4.36
(d) 4.96

Question 2. 60 gm of an organic compound on analysis is found to have C = 24 g, H = 4 g and O = 32 g. The empirical formula of compound is:
(a) CH₂O
(b) CHO
(c) C₂H₂O
(d) C₂H₂O₂

Question 3. The molar concentration of 20 g of NaOH present in 5 litre of solution is :
(a) 0.1 moles/litre
(b) 0.2 moles/litre
(c) 1.0 moles/litre
(d) 2.0 moles/litre

Question 4. The weight of a single atom of oxygen is :
(a) 1.057 × 10²³ g
(b) 3.556 × 10²³ g
(c) 2.656 × 10^–23 g
(d) 4.538 × 10^–23 g

Question 5. Temperature does not affect :
(a) Molality
(b) Formality
(c) Molarity
(d) Normality

Question 6. Volume of a gas at NTP is 1.12×10−7 cc. The number of molecule in it is :
(a) 3.01×10¹²
(b) 3.01×10¹⁸
(b) 3.01×10²⁴
(d) 3.01×10³⁰

Question 7. The normality of solution obtained by mixing 10 ml of N/5 HCI and 30 ml of N/10 HCl is :
(a) N /15
(b) N /5
(c) N /7.5
(d N /8

Question 8. The weight of NaCl decomposed by 4.9g of H₂SO₄, if 6 g of sodium hydrogen sulphate and 1.825 g of HCl, were produced in the reaction is:
(a) 6.921 g
(b) 4.65 g
(c) 2.925 g
(d) 1.4 g

Question 9. 0.4 moles of HCl and 0.2 moles of CaCl₂ were dissolved in water to have 500 mL of solution, the molarity of Cl– ion is:
(a) 0.8 M
(b) 1.6 M
(c) 1.2 M
(d) 10.0 M

Question 10. 1021 molecules are removed from 200 mg of CO₂. The moles of CO₂ left are :
(a) 2.88 ×10×⁻³
(b) 28.8×10×⁻³
(c) 288×10×⁻³
(d) 28.8×10³

Question 11. The empirical formula of a compound is CH₂O. Its molecular weight is 180. The molecular formula of compound is :
(a) C₄HO₄
(b) C₃H₆O₆
(c) C₆H₁₂O₆
(d) C₅H₁₀O₅

Question 12. Which of the following pairs of solutions are expected to be isotonic, temperature being the same?
(a) 0.1 M glucose and 0.1M C₆H₅N+H₃Cl–
(b) 0.1 M NaCl and 0.05 M BaCl₂
(c) 0.1 M Na₂SO₄ and 0.1 M KNO₃
(d) 0.1 M BaCl₂ and 0.075 M FeCl₃

Question 13. For preparing 0.1 N solution of a compound from its impure sample of which the percentage purity is known, the weight of the substance required will be
(a) less than the theoretical weight
(b) more than the theoretical weight
(c) same as the theoretical weight
(d) none of these

Question 14. The normality of orthophosphoric acid having purity of 70 % by weight and specific gravity 1.54 is :
(a) 11 N
(b) 22 N
(c) 33 N
(d) 44 N

Question 15. The molarity of H₂SO₄ solution, which has a density 1.84 g/cc. at 35° C and contains 98% by weight, is :
(a) 1.84 M
(b) 18.4 M
(c) 20.6 M
(d) 24.5 M

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Question 16. A solution is prepared by dissolving 24.5 g of sodium hydroxide in distilled water to give 1 L solution. The molarity of NaOH in the solution is
(a) 0.2450 M
(b) 0.6125 M
(c) 0.9800 M
(d) 1.6326 M
(Given that molar mass of NaOH = 40.0 g mol–1)

Question 17. In a hydrocarbon, mass ratio of hydrogen and carbon is 1:3, the empirical formula of hydrocarbon is
(a) CH₄
(b) CH₂
(c) C₂H
(d) CH₃

Question 18. The reaction of calcium with water is represented by the equation Ca + 2H₂O → Ca(OH)₂ + H₂ What volume of H₂ at STP would be liberated when 8 gm of calcium completely eacts with water?
(a) 0.2 cm³
(b) 0.4 cm³
(c) 2240 cm³
(d) 4480 cm³

Question 19. The vapour density of a mixture containing NO₂ and N₂O4 is 27.6. Mole fraction of NO₂ in the mixture is
(a) 0.8
(b) 0.6
(c) 0.4
(d) 0.2

Question 20. Arrange the following in the order of increasing mass (atomic mass: O = 16, Cu = 63, N = 14)
I. one atom of oxygen
II. one atom of nitrogen
III. 1 × 10^–10 mole of oxygen
IV. 1 × 10^–10 mole of copper
(a) II < I < III < IV
(b) I < II < III < IV
(c) III < II < IV < I
(d) IV < II < III < I

Question 21. Which has the maximum number of molecules among the following ?
(a) 44 g CO₂
(b) 48 g O₃
(c) 8 g H₂
(d) 64 g SO₂

Question 22. The weight of one molecule of a compound of molecular formula C₆0H₁₂₂ is
(a) 1.2 × 10^–20 g
(b) 5.025 × 10²³ g
(c) 1.4 × 10^–21 g
(d) 6.023 × 10^–20 g

Question 23. During electrolysis of water the volume of O₂ liberated is 2.24 dm³. The volume of hydrogen liberated, under same conditions will be
(a) 2.24 dm³
(b) 1.12 dm³
(c) 4.48 dm³
(d) 0.56 dm³

Question 24. An aqueous solution of 6.3 g of oxalic acid dihydrate is made up to 250 ml. The volume of 0.1 N NaOH required to completely neutralise 10 ml of this solution is
(a) 20 ml
(b) 40 ml
(c) 10 ml
(d) 4 ml

Question 25. 4 g of a hydrated crystal of formula A.xH₂O has 0.8 g of water. If the molar mass of the anhydrous crystal (A) is 144 g mol–1, The value of x is
(a) 4
(b) 1
(c) 2
(d) 3

Question 26. A solution of 20.2 g of 1,2-dibromopropane in MeOH upon heating with excess Zn produces 3.58 g of an unsaturated compound X. The yield (%) of X is closest to [Atomic weight of r is 80]
(a) 18
(b) 85
(c) 89
(d) 30

Question 27. Sulphur forms the chlorides S₂Cl₂ and SCl₂. The equivalent mass of sulphur in SCl₂ is
(a) 8 g/mol
(b) 16 g/mol
(c) 64.8 g/mol
(d) 32 g/mol

Question 28. 5.0 g of a certain element X forms 10.0 g of its oxide having the formula X4O6. The atomic mass of X is
(a) 12.0 amu
(b) 24.0 amu
(c) 30.0 amu
(d) 32.0 amu

Question 29. Calculate the normality of 10 volume H₂O₂ ?
(a) 1.7 N
(b) 12 N 
(c) 30.3 N
(d) 0.0303 N

Question 30. Volume of water needed to mix with 10 mL 10N HNO₃ to get 0.1 N HNO₃ is :
(a) 1000 mL
(b) 990 mL
(c) 1010 mL
(d) 10 mL

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