A solution of 49.0% H2SO4 by mass has a density of 1.39 g cm−3 at 293 K. A 22.6 cm3 sample of this solution is mixed with enough water to increase the volume of the solution to 88.5 cm3 . Find the molarity of sulfuric acid in this solution.

The molarity of the sulfuric acid in the solution is 1.77 M.

Explanation:

The molarity of the sulfuric acid in the solution can be found using the following equation:

Where:

: is the initial concentration of the acid

: is the initial volume of the solution = 22.6 cm³

: is the final volume of the solution = 88.5 cm³

The initial concentration of the H₂SO₄ is:

Where:

n: is the number of moles

m: is the mass

M: is the molar mass = 98.079 g/mol

d: is the density of the acid = 1.39 g/cm³

%: is the percent by mass = 49.0 %

Finally, the final concentration of H₂SO₄ after the dilution is:

Therefore, the molarity of the sulfuric acid in the solution is 1.77 M.

I hope it helps you!

it takes on an electronical energy