Commercially available sulphuric acid contains 93%acid by mass and has density of 1.84g/cm3.What volume of concentrated acid is required to prepare 2.5/0.5m sulphuric acid?
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Answer:
% of the sulfuric acid in the solution = 93 %
This means that 93 g of the sulphuric acid is present in the 100 g of the solution.
Molar Mass = 98 g/mole.
∵ No. of moles = Mass/Molar mass
∴ No. of moles = 93/98
= 0.949 moles.
Also, Density of the solution = 1.84 g/cm³.
∵ Density = Mass/Volume.
∴ Volume = 100/1.84
= 54.35 cm³
= 0.543 L.
Now, Using the Formula,
Molarity = No. of moles of solute/Volume of the solutions in liter.
= 0.95/0.0543
= 17.5 M.
Hence, the molarity of the solution is 17.5 M.
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