Final answer:
The question involves calculating the initial concentration of sulfuric acid in a titration with barium hydroxide. By applying the molarity concept and using stoichiometry from the balanced chemical equation, we determine that the initial concentration of sulfuric acid is 0.25M.
Step-by-step explanation:
The student is asking about a quantitative chemical analysis problem involving a titration between barium hydroxide (Ba(OH)2) and sulfuric acid (H2SO4). To solve this, we can use the concept of molarity and the stoichiometry of the balanced chemical reaction.
The balanced equation for the reaction between barium hydroxide and sulfuric acid is:
Ba(OH)2 (aq) + H2SO4 (aq) → BaSO4 (s) + 2H2O (l)
From the equation, we see that one mole of sulfuric acid requires one mole of barium hydroxide to neutralize it. The titration data tells us that 50 mL of 0.5 M Ba(OH)2 are required to fully titrate 100 mL of the H2SO4 solution. Using the molarity equation Molarity (M) = moles of solute / volume of solution in liters (L), we find:
So, the correct answer is c. 0.25M. This is the initial concentration of the sulfuric acid solution.