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A solution contains 0.040M Br - and 0.026M Cl - . The K sp of AgBr is 5.0x10 -13 . The K sp of AgCl is 1.8x10 -10 . Based on the the K values, which ion will precipitate first? Br - What concentration of Ag + ion will be present after 99% of the Br - has precipitated?

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  1. A solution contains 0.040M Br- and 0.026M Cl-. The Ksp of AgBr is 5.0x10-13. The Ksp of AgCl is 1.8x10-10. Based on the the K values, which ion will precipitate first? Br- What concentration of Ag+ ion will be present after 99% of the Br- has precipitated? [Ag+] = 1.2x10-9 M What concentration of Ag+ ion will be present after 99% of the Cl- has precipitated? [Ag+] = 6.9x10-7 M Can the Br- be 99% separated from the Cl- by precipitation with Ag+? Show your work. Yes, when 99% of the Br- has precipitated, none of the Cl- will have begun to precipitate. When [Ag+] = 1.2x10-9 M (1% of Br- left in solution), the Cl- concentration would have to be 0.15 M to create a solution saturated with AgCl.

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