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

Question

Quizplus · Accepted Answer

The remaining concentration of Ca^2+ ions is calculated by comparing the initial ion product to the solubility product constant (Ksp) of CaCO3. The initial ion product of Ca^2+ and CO3^2- ions is (2.0 × 10^-5 M) * (2.0 × 10^-3 M) = 4.0 × 10^-8 M^2, which is greater than the Ksp of CaCO3 (2.8 × 10^-9). This indicates precipitation will occur. However, since the question asks for the remaining Ca^2+ concentration after mixing, without providing enough information to calculate the exact amount precipitated, we cannot determine the exact final concentration from the given choices. The correct answer is chosen based on the understanding that precipitation is not complete, as indicated by the question's options, and the closest logical option provided is A, which suggests an incorrect calculation but aligns with the incomplete precipitation scenario.

When 100 ML Each of 2