Calculate the pH of a 0. 60 mol L^-1 H₂SO₃ solution that has the stepwise dissociation constants K_a1 = 1.5 × 10^-2 and K_a2=6.3 x 10-8 A) 1.02 B) 1.06 C) 1.82 D) 2.04

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Quizplus · Accepted Answer

H₂SO₃ is a weak diprotic acid. The first dissociation constant (K_a1) is much larger than the second dissociation constant (K_a2), so we can assume that the first dissociation is complete before the second dissociation begins. Therefore, we can use the following equation to calculate the pH of the solution:pH = -log[H⁺] = -log(K_a1[H₂SO₃]) = -log(1.5 × 10^-2 × 0.60) = 1.02

Calculate the PH of a 0