The concentration of Pb²⁺ in an aqueous solution is 5.5 × 10^-3 M.What concentration of SO₄^2- is required to begin precipitating PbSO₄? The K_sp of PbSO₄ is 2.5 × 10^-8. A) 1.4 × 10^-10 M B) 4.5 × 10^-6 M C) 1.6 × 10^-4 M D) 8.3 × 10^-4 M E) 2.9 × 10^-2 M

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Quizplus · Accepted Answer

The Ksp of PbSO4 is given as 2.5 × 10^-8. To find the concentration of SO4^2- required to begin precipitating PbSO4, we use the formula Ksp = [Pb^2+][SO4^2-]. Given [Pb^2+] = 5.5 × 10^-3 M, we rearrange the formula to find [SO4^2-] = Ksp / [Pb^2+] = (2.5 × 10^-8) / (5.5 × 10^-3) = 4.5 × 10^-6 M.

The Concentration of Pb2+ in an Aqueous Solution Is 5

The Concentration of Pb²⁺ in an Aqueous Solution Is 5