When 100 mL each of 2.0 × 10^-5 M Ca²⁺ and 2.0 × 10^-3M CO₃^2- are mixed, what is the remaining Ca²⁺ ion concentration and is precipitation complete? The solubility product constant of CaCO₃ is 2.8 × 10^-9.

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Quizplus · Accepted Answer

The ion product Q = [Ca²⁺][CO₃^2-] = (1.0 × 10^-5)(1.0 × 10^-3) = 1.0 × 10^-8, which is greater than K_sp (2.8 × 10^-9), so precipitation occurs. The remaining [Ca²⁺] is calculated using the K_sp value, resulting in 2.8 × 10^-6 M, but precipitation is not complete.

When 100 ML Each of 2