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Solid barium nitrate, Ba(NO3)2, is added slowly to a 1.0 × 10⁻⁴ M sodium carbonate solution. At what Ba2+ concentration will BaCO3 just start to precipitate? (Ksp of BaCO3 = 5.1 × 10⁻⁹)
- 5.1 × 10⁻⁵ M
- 8.1 × 10⁻⁸ M
- 8.1 × 10⁻⁷ M
- 4.1 × 10⁻⁵ M
Correct answer: 5.1 × 10⁻⁵ M
Solution
The correct option is right because the solubility product constant (Ksp) for BaCO3 indicates that the product of the concentrations of Ba2+ and CO3²- ions must equal 5.1 × 10⁻⁹ at equilibrium. Given the carbonate concentration of 1.0 × 10⁻⁴ M, the concentration of Ba2+ that leads to precipitation can be calculated using the Ksp expression, resulting in 5.1 × 10⁻⁵ M.
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