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 $K _ { \mathrm { a } 2 } = 6.3 \times 10 ^{- 8}$ A)1.02 B)1.06 C)1.82 D)2.04

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The correct answer is A because the pH of a 0.60 mol L^-1 H₂SO₃ solution that has the stepwise dissociation constants K_a1 = 1.5 × 10^-2 and $K _ { \mathrm { a } 2 } = 6.3 \times 10 ^{- 8}$ is 1.02.

Calculate the PH of a 0 Ka2=6.3×10−8K _ { \mathrm { a } 2 } = 6.3 \times 10 ^{- 8}Ka2​=6.3×10−8

Calculate the PH of a 0 $K _ { \mathrm { a } 2 } = 6.3 \times 10 ^{- 8}$