Solid, soluble silver nitrate is added slowly to a solution forwhich the initial concentrations of Cl^-1 andCrO4^-2 were [Cl^-1 ]₀ = 0.10 molL^-1 and [CrO₄^2- ]0 = 0.025 molL-¹.

(a) Calculate [Ag+] when a precipitate first appears andidentify the precipitate. The K_sp values for AgCl(s) andAg₂CrO₄(s) are 1.8x10^-10 and1.1x10^-12, respectively.

(b) Calculate [Cl^-1] and[CrO₄^2-] just before the second precipitateis formed. What is the % efficiency of the separation? (i.e. If Xrepresents the anion that precipitates first, then what fraction ofX was precipitated from the solution at the instant the secondprecipitate starts to form?)

Question

Solid, soluble silver nitrate is added slowly to a solution forwhich the initial concentrations of Cl^-1 andCrO4^-2 were [Cl^-1 ]₀ = 0.10 molL^-1 and [CrO₄^2- ]0 = 0.025 molL-¹.

(a) Calculate [Ag+] when a precipitate first appears andidentify the precipitate. The K_sp values for AgCl(s) andAg₂CrO₄(s) are 1.8x10^-10 and1.1x10^-12, respectively.

(b) Calculate [Cl^-1] and[CrO₄^2-] just before the second precipitateis formed. What is the % efficiency of the separation? (i.e. If Xrepresents the anion that precipitates first, then what fraction ofX was precipitated from the solution at the instant the secondprecipitate starts to form?)

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