If 22.15mL of 0.100M sulfuric acid is required to neutralize 10.0mL of lithium hydroxide solution, what is the molar concentration of the base? How would I approach this problem?

When it comes to neutralization reactions, your approach is to use the balanced chemical equation to figure out how many moles of each reactant need to be in solution for total neutralization to occur.

The balanced chemical equation in your situation looks like this.

The molarity and volume of the sulfuric acid solution are now provided by the problem, which is one method of determining the number of moles of sulfuric acid because

Using the previously mentioned mole ratio, you can calculate how many moles of lithium hydroxide would be required to ensure that every mole of acid is neutralized if you know how many moles of sulfuric acid were in the original solution.

Thus, the amount of sulfuric acid in moles will be

Thus, you would require

All that's left to do is calculate the solution's molarity using its volume.

Thus, keep in mind that mole ratios are the foundation of chemical reactions. In terms of solutions, begin by concentrating on moles; you can then use molarity and volume to help you find what you need.

You would use the equation: ( \text{M}_1V_1 = \text{M}_2V_2 ) where M1 is the molar concentration of sulfuric acid, V1 is the volume of sulfuric acid used, M2 is the molar concentration of lithium hydroxide, and V2 is the volume of lithium hydroxide used. Rearrange the equation to solve for M2, the molar concentration of lithium hydroxide. Then plug in the given values and solve for M2.