Problem: What volume of 0.500 M H2SO4 is needed to react completely with 20.0 mL of 0.400 M LiOH?A. 12.5 mL B. 32.0 mL C. 8.00 mL D. 16.0 mL E. 4.00 mL

We're being asked to calculate the volume of 0.500 M H₂SO₄ is needed to react completely with 20.0 mL of 0.400 M LiOH.

The balanced reaction would be: H₂SO₄(aq) + 2 LiOH(aq) → Li₂SO₄(aq) + 2 H₂O(l)

Calculate the volume of H₂SO₄:

molarity H₂SO₄ (volume) → moles H₂SO₄ (mole-to-mole comparison) → moles LiOH (molarity LiOH) → volume LiOH

Given:

molarity H₂SO₄ = 0.500 M
molarity LiOH = 0.400 M
volume LiOH solution = 25.00 mL → convert to L

$\mathbf{V}\mathbf{=}\mathbf{20}\mathbf{.}\mathbf{0}\mathbf{ }\cancel{\mathbf{mL}}\mathbf{\times }\frac{{\mathbf{10}}^{\mathbf{-}\mathbf{3}}\mathbf{ }\mathbf{L}}{\mathbf{1}\mathbf{ }\cancel{\mathbf{mL}}}$