Final answer:
To determine the molarity of sulfuric acid in a titration with a known volume and molarity of sodium hydroxide, we calculate the moles of NaOH used, adjust for the stoichiometry of the reaction, and divide by the volume of the acid. The molarity of the sulfuric acid is found to be 0.25 M.
Step-by-step explanation:
To calculate the molarity of the sulfuric acid (H2SO4), we can use the titration method provided in the question. First, we need to determine the number of moles of sodium hydroxide (NaOH) used in the titration. Since the concentration of NaOH is 0.200 M and the volume used is 25.0 mL (or 0.025 L), the number of moles can be found by the formula:
moles of NaOH = Molarity × Volume = 0.200 M × 0.025 L = 0.005 moles.
The balanced chemical equation given is: H2SO4 + 2NaOH → Na2SO4 + 2H2O, indicating that it takes 2 moles of NaOH to neutralize 1 mole of H2SO4. Therefore, we can find the number of moles of H2SO4 by dividing the moles of NaOH by 2.
moles of H2SO4 = 0.005 moles NaOH ÷ 2 = 0.0025 moles.
To find the molarity of the H2SO4, we divide the moles of H2SO4 by the volume in liters of the H2SO4 sample. As the volume of H2SO4 used is 10.0 mL (or 0.010 L), the calculation will be:
Molarity of H2SO4 = 0.0025 moles / 0.010 L = 0.25 M.