Q43.The density (in g mL−1 ) of a 3.60 M sulphuric acid solution that is 29% H2SO4 (Molar mass = 98 g mol−1 ) by mass will be (1) 1.64 (2) 1.88 (3) 1.22 (4) 1.45
What This Question Tests
This question requires interconverting between molarity and mass percentage for a solution, using the definition of density to find the final answer.
Concepts Tested
Formulas Used
Molarity = (moles of solute) / (volume of solution in L)
Mass % = (mass of solute / mass of solution) * 100
Density = mass of solution / volume of solution
📚 NCERT Sections This Tests
1.4 — Concentrated Nitric Acid Used In Laboratory Work Is 68% Nitric Acid By Mass In
Chemistry Class 11 · Chapter 1
1.4 Concentrated nitric acid used in laboratory work is 68% nitric acid by mass in aqueous solution. What should be the molarity of such a sample of the acid if the density of the solution is 1.504 g mL–1? 27 Solutions Reprint 2025-26
1.3 — Define The Following Terms:
Chemistry Class 11 · Chapter 1
1.3 Define the following terms: (i) Mole fraction (ii) Molality (iii) Molarity (iv) Mass percentage.
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1.28 Calculate the mass percentage of aspirin (C9H8O4) in acetonitrile (CH3CN) when 6.5 g of C9H8O4 is dissolved in 450 g of CH3CN.
📋 Question Details
- Chapter
- Solutions
- Topic
- Concentration terms
- Year
- 2007
- Shift
- Unknown
- Q Number
- Q43
- Type
- MCQ
- NCERT Ref
- Class 12 Chemistry Ch 2: Solutions
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