Ab2 has a molar solubility of 3.72×10−4 m. what is the value of the solubility product constant for ab2? express your answer numerically.

Answer is: Ksp for AB₂ is 2.06·10⁻¹⁰.
Chemical reaction: AB₂(s) → Aˣ⁺(aq) + 2Bⁿ⁻(aq).

s(AB₂) = 3,72·10⁻⁴ M.
s(AB₂) = s(Aˣ⁺).

s(Bⁿ⁻) = 2s(AB₂).

Ksp(AB₂) = s(Aˣ⁺) · (s(Bⁿ⁻))².
Ksp(AB₂) = 3,72·10⁻⁴ · (7,44·10⁻⁴)².

Ksp(AB₂)= 2,06·10⁻¹⁰.

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