Chapter 17 Principles of Chemical Reactivity: Other Aspects of Aqueous Equilibria - Study Questions - Page 677c: 58

See the answer below.

Pure water: $Ksp=[Ag^+][Br^-]=s^2$ $s=\sqrt{5.4\dot{}10^{-13}}=7.35\dot{}10^{-7}\ M$ With NaBr: $[NaBr]=(0.15\ g\div 102.89\ g/mol)/(22.5/1000\ L)=0.065\ M$ $Ksp=s\dot{}(0.065+s)$ $s=8.334\dot{}10^{-12}\ M$