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As per your syllabus, what is the molar SOLUBILITY S of barium sulphate at 298 K, given Ksp(BaSO₄) = 1.1 × 10⁻¹⁰?
A1.1 × 10⁻¹⁰ M
B1.1 × 10⁻⁵ M
C3.3 × 10⁻⁵ M
D1.05 × 10⁻⁵ M
Answer & Solution
Correct answer: D. 1.05 × 10⁻⁵ M
Your syllabus: BaSO₄ → Ba²⁺ + SO₄²⁻, Ksp = S² ⇒ S = √(1.1×10⁻¹⁰) = 1.05 × 10⁻⁵ M.
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