a) AgBr:

CuBr:

b)

c)

Mylo O'Moore
2021-02-23
Answered

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:$(0.010+s)s=4.2\cdot {10}^{-8}$ $s=4.2\cdot {10}^{-9}MBr$ needed form PPT

CuBr:$(0.010+s)s=7.7\cdot (0.010+s)s=7.7\cdot {10}^{-13}$ Ag+=$1.8\cdot {10}^{-7}$

b)$4.2\cdot {10}^{-6}[Ag+]=7.7\cdot {10}^{-13}$ [Ag+]$=1.8\cdot {10}^{-7}$

c)$\frac{1.8\cdot {10}^{-7}}{0.010M}\cdot 100\mathrm{\%}=0.18\mathrm{\%}$

a) AgBr:

CuBr:

b)

c)

You can still ask an expert for help

ottcomn

Answered 2021-02-25
Author has **97** answers

Yes ur correct.i a and b part

c ) 0.0018% not 0.18%

c ) 0.0018% not 0.18%

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