${\mathrm{H}}_2{\mathrm{SO}}_4$ is labelled as 9.8% by weight. Specific gravity of ${\mathrm{H}}_2{\mathrm{SO}}_4$ is 1.8. The volume of the acid to be taken to prepare 1000 ml of 0.18M solution is

Step 1: Calculate the amount of H₂SO₄ in grams per mL in the given solution

The specific gravity means 1 mL of the solution weighs 1.8 g. Since the solution is 9.8% by weight, the amount of H₂SO₄ in 1 mL is:

Mass of H₂SO₄ per mL = 1.8 × (9.8/100) = 0.1764 g/mL

Step 2: Calculate the moles of H₂SO₄ per mL in the given solution

The number of moles of H₂SO₄ in 1 mL is:

Moles per mL = Mass per mL / Molar mass = 0.1764 / 98 = 0.0018 mol/mL

Step 3: Calculate the total moles required for 1000 mL of 0.18 M solution

The total moles of H₂SO₄ required are:

Total moles = Molarity × Volume in liters = 0.18 × 1 = 0.18 mol

Step 4: Calculate the volume of the given solution required

The volume (V) in mL of the given solution required is:

V = Total moles / Moles per mL = 0.18 / 0.0018 = 100 mL

Final Answer:

The volume of the H₂SO₄ solution required is 100 mL.