Final answer:
The pH at the equivalence point for the titration of sodium hydroxide (NaOH) with sulfuric acid (H₂SO₄), both strong electrolytes, is expected to be approximately 7.00, indicating a neutral solution resulting from complete neutralization.
Step-by-step explanation:
The pH at the equivalence point of a titration between sodium hydroxide (NaOH) and sulfuric acid (H₂SO₄) is dependent on the nature of the salt formed and the dissociation of water. In this titration, the products are a salt (Na₂SO₄) and water. Since sulfuric acid is a strong acid and sodium hydroxide is a strong base, the resulting solution of the salt and water at the equivalence point will be neutral, and thus the pH should be approximately 7.00.
This is because the salt formed does not undergo any hydrolysis that would affect the pH of the solution. If the reaction had involved a weak acid or a weak base, the pH at the equivalence point would have been different. However, in the reaction of a strong acid with a strong base, such as the reaction of NaOH with H₂SO₄, neutralization occurs and the pH is expected to be neutral at the equivalence point.