Answer
Right.
Work Step by Step
$K=[Cl^-]/[I^-]=Ksp(AgCl)/Ksp(AgI)$
$K=1.77\times10^{-10}/(8.52\times10^{-17})=2.08\times10^8$
Since $K>1$, the equilibrium lie predominantly to the right.
Chemistry and Chemical Reactivity (9th Edition)
by Kotz, John C.; Treichel, Paul M.; Townsend, John R.; Treichel, David A.
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 677e: 91
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