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## Homework Statement

Ok, this is a lab related question. Given a diluted solution of approximately 1.25M H2SO4, determine the amount of solution needed to use for titration with the base you prepared and standardized. Do not use a volume of battery acid that will require more than 20mL of base to reach the equivalence point. Then determine the concentration of H2SO4 in the diluted solution you were given.

## Homework Equations

Balanced chemical equation: H2SO4 + 2NaOH --> 2H2O + Na2SO4

[NaOH] = 0.0939M

## The Attempt at a Solution

I determined the amount of diluted H2SO4 to be 18.9 mL (I used 18 mL)

20mL NaOH(1L/1000mL)(0.0939M NaOH)(1 mol H2SO4/2 mol NaOH) = 0.0945M H2SO4

(1.25M)(V1)=(0.0945M)(250mL); V1 = 18.9mL

It's at this point where I get stuck. I'm supposed to calculate the concentration of H2SO4 in the diluted acid solution then Find the original [H2SO4] in the undiluted battery acid (assume diluted 1:5). I know I'm supposed to use a titration calculation to find the concentration of the diluted acid but I'm not sure how to set it up and which numbers to use to end with mol/L H2SO4. I'm also not sure how to find the initial concentration. Any ideas?