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

FREE Expert Solution

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

V=20.0 mL×10-3 L1 mL

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Problem Details

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

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