When equal volumes of the indicated aqueous solutions are mixed,precipitation should occur only for: A)2 × 10^-5 M Ag⁺ + 2 × 10^-5 M CO₃^2- B)2 × 10^-5 M Ca²⁺ + 2 × 10^-5 M CO₃^2- C)2 × 10^-4 M Ca²⁺ + 2 × 10^-2 M F^- D)2 × 10^-5 M Mg²⁺ + 2 × 10^-6 M F^- E)2 × 10^-3 M Ba²⁺ + 2 × 10^-3 M F^-

Question

Quizplus · Accepted Answer

In order for precipitation to occur, we need to identify the potential products of the reaction and determine if they are insoluble (i.e. will precipitate out of the solution).

For option A, mixing Ag+ and CO32- would result in the formation of insoluble Ag2CO3, which would precipitate out of solution.

For option B, mixing Ca2+ and CO32- would result in the formation of insoluble CaCO3, which would precipitate out of solution.

For option C, mixing Ca2+ and F- would not result in any precipitation, as CaF2 is soluble in water.

For option D, mixing Mg2+ and F- would not result in any precipitation, as MgF2 is also soluble in water.

For option E, mixing Ba2+ and F- would result in the formation of insoluble BaF2, which would precipitate out of solution.

Therefore, the only option where precipitation should occur is option C.

When Equal Volumes of the Indicated Aqueous Solutions Are Mixed,precipitation