Solution: How many milliliters of a 9.0 M H 2SO4 solution are needed to make 0.45 L of a 3.5 M solution?

We are being asked to find how many milliliters of 9.0 M H₂SO₄ is needed to make a 0.45 L of 3.5 M solution.

When we are adding water (or solvent) to a solution to decrease its concentration, we are diluting the solution. 

When dealing with dilution we will use the following equation:

$\boxed{{\mathbf{M}}_{\mathbf{1}}{\mathbf{V}}_{\mathbf{1}}\mathbf{=}{\mathbf{M}}_{\mathbf{2}}{\mathbf{V}}_{\mathbf{2}}}$

M₁ = initial concentration
V₁ = initial volume
M₂ = final concentration
V₂ = final volume

Calculate the initial volume (milliliters needed) of the H₂SO₄ solution.