A solution is prepared by dissolving 17.75 g sulfuric acid,H₂SO₄,in enough water to make 100.0 mL of solution.If the density of the solution is 1.1094 g/mL,what is the mole fraction H₂SO₄ in the solution? A)0.0181 B)0.0338 C)0.0350 D)19.0

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Quizplus · Accepted Answer

The mole fraction of sulfuric acid in the solution can be calculated by first determining the moles of sulfuric acid and the total moles in the solution. The molar mass of sulfuric acid (H₂SO₄) is approximately 98.08 g/mol. Thus, the moles of sulfuric acid are 17.75 g / 98.08 g/mol = 0.1809 mol. The mass of the solution is the volume multiplied by the density, which is 100.0 mL * 1.1094 g/mL = 110.94 g. The mass of water in the solution is the total mass minus the mass of sulfuric acid, which is 110.94 g - 17.75 g = 93.19 g. The moles of water are 93.19 g / 18.015 g/mol (molar mass of water) = 5.172 mol. The total moles in the solution are the moles of sulfuric acid plus the moles of water, which is 0.1809 mol + 5.172 mol = 5.353 mol. The mole fraction of sulfuric acid is then the moles of sulfuric acid divided by the total moles, which is 0.1809 mol / 5.353 mol = 0.0338.

A Solution Is Prepared by Dissolving 17