Final answer:
To reach the second equivalence point in a titration of 58.0 mL of 0.350 M H2SO4 with 0.600 M Ba(OH)2, the volume of Ba(OH)2 required is closest to 34.0 mL. This is based on the stoichiometry of the balanced equation and the concept of molarity in titrations.
Step-by-step explanation:
The question asks how many milliliters of 0.600 M Ba(OH)2 are required to reach the second equivalence point in a titration with 58.0 mL of a 0.350 M solution of diprotic acid H2SO4. To reach the second equivalence point, both hydrogen ions in H2SO4 must be neutralized by Ba(OH)2.
The balanced chemical equation for the reaction is:
H2SO4 (aq) + Ba(OH)2 (aq) → BaSO4 (s) + 2H2O (l)
Since sulfuric acid is diprotic, it can donate two protons, and the ratio of Ba(OH)2 to H2SO4 is 1:1. To find out the volume of Ba(OH)2 needed, we can use the molarity of the acid and bases titration relation:
- Moles of H2SO4 = 0.350 moles/L × 0.058 L = 0.0203 moles
- Moles of Ba(OH)2 needed = 0.0203 moles (since the ratio is 1:1 for the second equivalence point)
- Volume of Ba(OH)2 = moles of Ba(OH)2 / molarity of Ba(OH)2 = 0.0203 moles / 0.600 moles/L = 0.03383 L
- Convert liters to milliliters: 0.03383 L × 1000 mL/L = 33.83 mL
Since the answer must be one of the options provided, we'll choose the closest one, which is option b) 34.0 mL (rounding from 33.83 mL to the nearest whole number).