A solution is 0.10 M Cl and 0.10 M I- . Silver nitrate is slowly added to precipitate the silver halide. Ksp(AgCl) = 1.77 x 10-10; Ksp(AgI) = 8.52 x 10-17
(A) Which solid will precipitate first?
(B) What will be the [Ag+ ] when the first solid begins to precipitate?
(C) What [Ag+ ] is required in order to precipitate AgCl?
(D) What will be the [I- ] when the AgCl starts to precipitate?
(E) What percentage of the iodide remains when the first AgCl precipitates?
A solution is 0.10 M Cl and 0.10 M I- . Silver nitrate is slowly added...
6). If a silver nitrate solution is slowly added to a solution where [Br-] = 0.05M and [Cl-] = 0.05M, at that [Ag+] will a precipitate begin to form and will the precipitate be AgBr or AgCl? Additional Info: Ksp(AgBr) = 5.0x10-13 and Ksp (AgCl) = 1.6x10-10
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