CameraIcon
CameraIcon
SearchIcon
MyQuestionIcon
MyQuestionIcon
1
You visited us 1 times! Enjoying our articles? Unlock Full Access!
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
No worries! We‘ve got your back. Try BYJU‘S free classes today!
B
3.2 L
No worries! We‘ve got your back. Try BYJU‘S free classes today!
C
2 L
Right on! Give the BNAT exam to get a 100% scholarship for BYJUS courses
D
4.4 L
No worries! We‘ve got your back. Try BYJU‘S free classes today!
Open in App
Solution

The correct option is C 2 L
Let 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.

flag
Suggest Corrections
thumbs-up
0
Join BYJU'S Learning Program
Join BYJU'S Learning Program
CrossIcon