Chemistry · Acids, Bases and Salts

To determine the pH of a 10^-3 M H₂SO₄ solution, recognize that H₂SO₄ is a strong acid that completely dissociates into 2 H⁺ and SO₄^2-. Thus, the concentration of H⁺ ions is twice the initial concentration of H₂SO₄, which is 2 x 10^-3 M. The pH is calculated using the formula: pH = -log[H⁺]. Substituting the concentration, we get pH = -log(2 x 10^-3) = 3 - log(2) ≈ 2.7. Hence, the correct answer is 2.7. The other options result from incorrect calculations or misunderstandings of the relationship between H₂SO₄'s dissociation and pH.

This pH calculation doesn't account for the fact that each molecule of H₂SO₄ produces two H⁺ ions, doubling the concentration of H⁺ ions.

This is correct. After full dissociation, the concentration of H⁺ ions is 2 x 10^-3 M, leading to a pH = -log(2 x 10^-3) = 2.7.

This assumes incorrect initial concentration or incorrect ionization process, ignoring the logarithmic nature of pH calculation.

This value is too low and results from overestimating the concentration of H⁺ ions or misunderstanding the pH scale.