A 1500 mL solution contains 0.100 M K₂ CrO and 0.100 M Na₂SO. A concentrated Ba(NO3), is slowly added to the solution. What is the barium ion concentration at the point when a = 2.3x10-8) precipitate just starts to form? (K BaCrO = 8.5x10-¹1 and K BaSO = M
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![A 1500 mL solution contains 0.100 M K₂CrO₄ and 0.100 M Na₂SO₄. A concentrated Ba(NO₃)₂ is slowly added to the solution. What is the barium ion concentration at the point when a precipitate just starts to form? (Kₛₚ BaCrO₄ = 8.5×10⁻¹¹ and Kₛₚ BaSO₄ = 2.3×10⁻⁸)
[Textbox for answer] M](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F43c41e7b-d1fd-4f8b-969d-dea9b3b3fd4e%2F308524d1-1e51-45f5-99e5-2ec3a67cd0c1%2Fub3s2mo_processed.jpeg&w=3840&q=75)
Concentration of CrO4–2 = 0.100 M
Concentration of SO4–2 = 0.100 M
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