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Question:

The solubility of BaSO4 in water is 2.42 × 10⁻³ g/L at 298 K. The value of its solubility product (Ksp) will be: (Given molar mass of BaSO4 = 233 g/mol)

1.08 × 10⁻⁴ mol²L⁻²

1.08 × 10⁻¹⁰ mol²L⁻²

1.08 × 10⁻¹² mol²L⁻²

1.08 × 10⁻⁸ mol²L⁻²

Solution:

The solubility S = 2.42 × 10⁻³ g/L
233 g/mol = 1.04 × 10⁻⁵ mol/L
Ksp = [Ba²⁺][SO₄²⁻]
Ksp = S × S
Ksp = 1.04 × 10⁻⁵ mol/L × 1.04 × 10⁻⁵ mol/L = 1.08 × 10⁻¹⁰ mol²L⁻²