A solution containing CaCl₂ is mixed with a solution of Li₂C₂O₄ to form a solution that is 3.5 × 10^-4 mol L^-1 in calcium ion and 2.33 × 10^-4mol L^-1 in oxalate ion. What will happen once these solutions are mixed? K_sp (CaC₂O₄) = 2.3 × 10^-9. A) Nothing will happen since both calcium chloride and lithium oxalate are soluble compounds. B) Nothing will happen because K_sp Q for all possible precipitates. C) A precipitate will form as calcium oxalate is not soluble to any extent. D) A precipitate will form since Q K_sp for calcium oxalate. E) Nothing will happen because Q = K_sp.

Question

A solution containing CaCl₂ is mixed with a solution of Li₂C₂O₄ to form a solution that is 3.5 × 10^-4 mol L^-1 in calcium ion and 2.33 × 10^-4mol L^-1 in oxalate ion. What will happen once these solutions are mixed? K_sp (CaC₂O₄) = 2.3 × 10^-9. A) Nothing will happen since both calcium chloride and lithium oxalate are soluble compounds. B) Nothing will happen because K_sp > Q for all possible precipitates. C) A precipitate will form as calcium oxalate is not soluble to any extent. D) A precipitate will form since Q > K_sp for calcium oxalate. E) Nothing will happen because Q = K_sp.

Quizplus · Accepted Answer

The problem provides the concentration of both calcium and oxalate ions in the mixed solution, which enables us to calculate the ion product, Q. Since Q is greater than the solubility product constant, KS, for calcium oxalate, a precipitate will form. Therefore, the correct choice is D.

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A Solution Containing CaCl₂ Is Mixed with a Solution of Li₂C₂O₄