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Precipitation of Halides: Analyzing AgBr and AgCl Ion Concentrations

This analysis explores the precipitation of AgBr and AgCl based on their solubility product constants (Ksp). Given initial concentrations of bromide (Br-) at 0.040 M and chloride (Cl-) at 0.026 M, it determines which ion will precipitate first and calculates the remaining concentrations of Ag+ after 99% of each halide has precipitated. The critical findings reveal that Br- precipitates first, with final Ag+ concentrations of 1.2 x 10^-9 M after Br- precipitation and 6.9 x 10^-7 M after Cl- precipitation. It concludes that 99% of Br- can be separated from Cl- through selective precipitation.

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Precipitation of Halides: Analyzing AgBr and AgCl Ion Concentrations

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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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