# Solid NaBr is slowly added to a solution that is 0.010 M inCu+ and 0.010 M in Ag+. (a) Which compoundwill begin to precipitate first? (b) Calculate [A

Solid NaBr is slowly added to a solution that is 0.010 M inCu+ and 0.010 M in Ag+. (a) Which compoundwill begin to precipitate first? (b) Calculate [Ag+] when CuBr justbegins to precipitate. (c) What percent of Ag+ remains in solutionat this point?
a) AgBr: $\left(0.010+s\right)s=4.2\cdot {10}^{-8}$ $s=4.2\cdot {10}^{-9}MBr$ needed form PPT
CuBr: $\left(0.010+s\right)s=7.7\cdot \left(0.010+s\right)s=7.7\cdot {10}^{-13}$ Ag+=$1.8\cdot {10}^{-7}$
b) $4.2\cdot {10}^{-6}\left[Ag+\right]=7.7\cdot {10}^{-13}$ [Ag+]$=1.8\cdot {10}^{-7}$
c) $\frac{1.8\cdot {10}^{-7}}{0.010M}\cdot 100\mathrm{%}=0.18\mathrm{%}$
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Yes ur correct.i a and b part
c ) 0.0018% not 0.18%