Final answer:
At the equivalence point of titrating 0.20M sulfuric acid with 0.4M NaOH, the resulting solution will contain the salt Na2SO4 and water and will have a neutral pH of 7.00 at 25°C, because both reactants are strong.
Step-by-step explanation:
In the context of this titration problem, when titrating 0.20M sulfuric acid, H2SO4, with 0.4M NaOH, the equivalence point occurs when the amount of NaOH added is stoichiometrically equivalent to the amount of H2SO4 present. Because H2SO4 is a strong acid and NaOH is a strong base, the resulting solution at the equivalence point will consist of the salt Na2SO4 and water and will have a neutral pH of 7.00 at 25°C. This is because the neutralization reaction between a strong acid and a strong base produces salt and water, which do not have any acidic or basic properties.