Chemistry and Chemical Reactivity (9th Edition)

Published by Cengage Learning
ISBN 10: 1133949649
ISBN 13: 978-1-13394-964-0

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


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Work Step by Step

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