Final answer:
To dilute 30 mL of a 10.0 M H2SO4 solution to a 0.170 M H2SO4 solution, you should dilute the concentrated solution to approximately 1765 mL.
Step-by-step explanation:
Diluting a Concentrated Solution
To determine to what volume you should dilute 30 mL of a 10.0 M H₂SO₄ solution to obtain a 0.170 M H₂SO₄ solution, you 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 respectively.
Using the given values:
M₁ = 10.0 M (concentrated solution molarity)
V₁ = 0.030 L (30 mL converted to liters)
M₂ = 0.170 M (desired molarity of diluted solution)
Substitute these values into the dilution equation and solve for V₂:
(10.0 M)(0.030 L) = (0.170 M)V₂
Now, calculate for V₂:
V₂ = (10.0 M × 0.030 L) / 0.170 M
V₂ ≈ 1.765 L (or 1765 mL)
Therefore, you should dilute the solution to approximately 1765 mL to achieve the desired concentration of 0.170 M H₂SO₄.