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Solubility of BaSO₄ = 2.42 × 10⁻³ g L⁻¹. s = 2.42 × 10⁻³ / 233 = 1.038 × 10⁻⁵ mol L⁻¹.

1. Ksp = s² = (1.038 × 10⁻⁵)² = 1.08 × 10⁻¹⁰ mol² L⁻²
2. Ksp = s² = (1.038 × 10⁻⁵)² = 1.08 × 10⁻⁹ mol² L⁻²
3. Ksp = s² = (1.038 × 10⁻⁵)² = 1.08 × 10⁻⁸ mol² L⁻²
4. Ksp = s² = (1.038 × 10⁻⁵)² = 1.08 × 10⁻⁷ mol² L⁻²

Correct answer: Ksp = s² = (1.038 × 10⁻⁵)² = 1.08 × 10⁻⁹ mol² L⁻²

Solution

The solubility product (Ksp) is calculated as s². Substituting s = 1.038 × 10⁻⁵ mol L⁻¹, we get Ksp = (1.038 × 10⁻⁵)² = 1.08 × 10⁻¹⁰ mol² L⁻². Thus, option A is correct.

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