Final answer:
To prepare 600.0 mL of 0.10 M H₂SO₄ from a 13.2 M solution, 4.545 mL of the concentrated acid is required, which rounds to option (a) 4.55 mL. This calculation is based on the dilution equation M1V1 = M2V2.
Step-by-step explanation:
To find out how many milliliters of 13.2 M H₂SO₄ are required to prepare 600.0 mL of 0.10 M H₂SO₄, we can use the dilution equation M₁V₁ = M₂V₂, where M₁ and V₁ are the molarity and volume of the concentrated solution, and M₂ and V₂ are the molarity and volume of the diluted solution.
Let's solve for V₁:
M₁V₁ = M₂V₂
V₁ = (M₂V₂) / M₁
V₁ = (0.10 M × 600.0 mL) / 13.2 M
V₁ = 60.0 mmol / 13.2 M
V₁ = 4.5454... mL
So, 4.545 mL (rounded to three significant figures) of the 13.2 M H₂SO₄ solution are needed to prepare 600.0 mL of a 0.10 M H₂SO₄ solution, which corresponds to option (a) 4.55 mL.