5.0 mL of 0.050 M Ba (NO3) 2 M and 100.0 mL of 0.10 M KIO3 are added together in a 250 mL erlenmeyer flask. In this problem, ignore ionic strength effects and neglect the possible presence of any complex ions in solution. a. Will Ba (IO3) 2 precipitate out of solution? Support your answer with appropriate calculations. b. What are the concentrations of Ba2 + and 103 in the solution? Report your answer using 2 significant figures.

The Ba (IO₃) ₂ will precipitate out in the solution.

Explanation:

The solubility of Ba (IO₃) ₂ is:

Ba (IO₃) ₂ (s) → Ba²⁺ (aq) + 2 IO₃⁻ (aq)

Where ksp, is defined as:

ksp = [Ba²⁺] [IO₃⁻]² = 1.5x10⁻⁹

If the multiplication of [Ba²⁺] [IO₃⁻] is higher than ksp, the reaction will produce Ba (IO₃) ₂, that means the solid will precipitate.

In solution, concentration of Ba²⁺ and IO₃⁻ are:

[Ba²⁺] = 0.050M * (5mL / 105mL) = 0.00238M

[IO₃⁻] = 0.10M * (100mL / 105mL) = 0.0952M

Replacing in ksp formula:

[0.00238] [0.0952]² = 2.16x10⁻⁵. As the result is higher than ksp, The Ba (IO₃) ₂ will precipitate out in the solution.