Q31.The concentrated sulphuric acid that is peddled commercial is 95%H2SO4 by weight. If the density of this commercial acid is 1.834 g cmโ3 , the molarity of this solution is (1) 17.8M (2) 12.0M (3) 10.5M (4) 15.7M
What This Question Tests
This question tests the ability to calculate molarity of a solution given its percentage by weight and density, which requires interconverting different concentration units.
Concepts Tested
Formulas Used
Molarity = (weight % * density * 10) / molar mass
๐ NCERT Sections This Tests
1.4 โ Concentrated Nitric Acid Used In Laboratory Work Is 68% Nitric Acid By Mass In
Chemistry Class 11 ยท 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 mLโ1? 27 Solutions Reprint 2025-26
1.3 โ Define The Following Terms:
Chemistry Class 11 ยท Chapter 1
1.3 Define the following terms: (i) Mole fraction (ii) Molality (iii) Molarity (iv) Mass percentage.
1.28 โ Calculate The Mass Percentage Of Aspirin (C9H8O4) In Acetonitrile (Ch3Cn) When
Chemistry Class 11 ยท Chapter 1
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.
๐ Question Details
- Chapter
- Solutions
- Topic
- Molarity from percentage by weight and density
- Year
- 2012
- Shift
- 07 May Online
- Q Number
- Q31
- Type
- MCQ
- NCERT Ref
- Class 12 Chemistry Ch 2: Solutions
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