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A salt of the type AB2 is only slightly soluble in water. If its molar solubility is 1.0 × 10−5 mol L−1, what is the value of its solubility product?

1. 4 × 10−10
2. 1 × 10−15
3. 1 × 10−10
4. 4 × 10−15

Correct answer: 4 × 10−15

Solution

The solubility product (Ksp) for a salt AB2 can be calculated using the formula Ksp = [A⁺][B^−]². Given the molar solubility of AB2 is 1.0 × 10−5 mol L−1, the concentration of A⁺ is 1.0 × 10−5 mol L−1 and the concentration of B^− is 2 × 1.0 × 10−5 mol L−1. Therefore, Ksp = (1.0 × 10−5)(2 × 1.0 × 10−5)² = 4 × 10−15.

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