    Question

# A concentrated solution of sulphuric acid is 98% H2SO4 by mass and has a density of 1.84 g/mL. What volume of this concentrated acid solution is required to make 6 L of a 6.13 M H2SO4 solution? (Molar mass of H2SO4=98 g/mol)

A
6.5 L
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B
3.2 L
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C
2 L
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D
4.4 L
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Solution

## The correct option is C 2 LLet the mass of the H2SO4 solution be 100 g. 98% by mass means 98 g of H2SO4 is present in 100 g of solution. Number of moles of H2SO4=given massmolar mass =9898=1 We know, Density=massvolume So, volume of the solution=1001.84 mL Molarity=number of moles of solutevolume of solution in mL×1000 Molarity=11001.84×1000=18.4 M Let the volume of 18.4 M acid be V L. So, conserving moles before and after dilution: M1V1=M2V2 where, M2 and V2 are the final concentration and volume, (18.4×V)=(6.13×6) V=2 L Volume of 18.4 M H2SO4 required is 2L.  Suggest Corrections  0      Similar questions  Explore more