If the solubility product of AB2 is 3.20 × 10–11 M3, then the solubility of AB2 in pure water is________ × 10–4 mol L–1 [Assuming that neither kind of ion reacts with water]

AB2 ⇌ A2+(s) + 2B-(2s) Ksp = 4s3 = 3.20 × 10–11 So solubility = 2 × 10–4 mol L–1

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If the solubility product of AB2 is 3.20 × 10^–11 M3, then the solubility of AB2 in pure water is________ × 10^–4 mol L^–1

Chemistry

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21/09/2020 12:22 pm

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Shaneylee18

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If the solubility product of AB₂ is 3.20 × 10^–11 M³, then the solubility of AB₂ in pure water is________ × 10^–4 mol L^–1

[Assuming that neither kind of ion reacts with water]

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21/09/2020 12:26 pm

Freddie12

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AB₂⇌ A²⁺(s) + 2B^-(2s)

K_sp = 4s³ = 3.20 × 10^–11

So solubility = 2 × 10^–4 mol L^–1

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