HardChemistryHigh School (11–12)Atoms and Molecules › Stoichiometry and Concentration Atoms and Molecules › The Mole ConceptNumerical

Concentrated sulphuric acid is 98% H₂SO₄ by mass, and its density is 1.84 g mL⁻¹.

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Concentrated sulphuric acid is $98\%$ $\text{H}_2\text{SO}_4$ by mass, and its density is $1.84\ \text{g mL}^{-1}$ . What is its molarity? $\text{H}_2\text{SO}_4$ is $98\ \text{g mol}^{-1}$ .

Need a reminder? The key ideaShow

Mass percent $= \dfrac{\text{mass of solute}}{\text{mass of solution}} \times 100$ . Mole fraction $x_A = \dfrac{n_A}{n_A + n_B}$ . Molarity $= \dfrac{\text{mol of solute}}{\text{L of solution}}$ . Molality $= \dfrac{\text{mol of solute}}{\text{kg of solvent}}$ , which does not change with temperature. A mass percent becomes a molarity through the density: find the mass of one litre, then the mass of solute in it.

The worked solution

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← A bottle is labelled sodium hydroxide, 3.0 M, density 1.11 g mL⁻¹.Calcium (40.08 u), strontium (87.62 u) and barium (137.33 u) behave alike. →

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Concentrated sulphuric acid is 98% H₂SO₄ by mass, and its density is 1.84 g mL⁻¹.

The worked solution

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