We're being asked to calculate the volume of 0.500 M H_{2}SO_{4} is needed to react completely with 20.0 mL of 0.400 M LiOH.

The balanced reaction would be:** H _{2}SO**

Calculate the volume of H_{2}SO_{4}:

*molarity H _{2}SO_{4} (volume) → moles H_{2}SO_{4} (mole-to-mole comparison) → moles LiOH (molarity LiOH) → volume LiOH*

Given:

molarity H_{2}SO_{4} = 0.500 M

molarity LiOH = 0.400 M

volume LiOH solution = 25.00 mL → convert to L

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

What volume of 0.500 M H_{2}SO_{4} 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

Frequently Asked Questions

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Solution Stoichiometry concept. You can view video lessons to learn Solution Stoichiometry. Or if you need more Solution Stoichiometry practice, you can also practice Solution Stoichiometry practice problems.