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The solubility of CaCO(3) is 7mg//L. Cal...

The solubility of `CaCO_(3)` is `7mg//L`. Calculate the `K_(sp)` of `BaCO_(3)` when `Na_(2)CO_(3)` is added slowly a solution containing equimolar concentration of `Ca^(2+)` and `Ba^(2+)` and no precipitate is formed until `90%` of `Ba^(2+)` has been precipitated as `BaCO_(3)`.

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To solve the problem, we need to calculate the solubility product constant (Ksp) of BaCO₃ given the solubility of CaCO₃ and the conditions of the problem. Here’s a step-by-step breakdown of the solution: ### Step 1: Convert the solubility of CaCO₃ from mg/L to moles/L The solubility of CaCO₃ is given as 7 mg/L. We need to convert this to grams per liter and then to moles per liter. - **Convert mg to grams:** \[ 7 \, \text{mg/L} = 7 \times 10^{-3} \, \text{g/L} ...
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