A 10.0-mL sample of sulfuric acid, H2SO4, from a battery of an old car is diluted to 100.0 mL, and a 10.00-mL aliquot (portion) of the diluted acid is then titrated with 0.2500 M NaOH solution. If the concentration of H2SO4 in the original battery was 3.25 M, how many milliliters (mL) of the NaOH solution is required to titrate the sulfuric acid present in the 10.0-mL portion of dilute acid solution

26.0 mL

Explanation:

The reaction that takes place is:

First we calculate the molar concentration of the diluted sulfuric acid solution, using the C₁V₁=C₂V₂ formula:

Now we calculate how many H₂SO₄ moles would there be in 10.00 mL of this diluted solution, using the definition of molarity:

Then we convert 3.25 mmoles of H₂SO₄ into mmoles of NaOH, using the stoichiometric coefficients of the balanced reaction:

Finally we calculate the required volume of the NaOH solution, using the definition of molarity:

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