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: 56


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In all cases except c, solubility as a function of Ksp is the same for both compounds, so the one with the higher Ksp is the more soluble; a) AgSCN, 1.0e-12 vs 5.4e-13 for AgBr b) SrSO4, 3.4e-7 vs 5.6e-10 for SrCO3 c) AgI: $Ksp=[Ag^+][I^-]\rightarrow Ksp=s^2\rightarrow s=9.22\dot{}10^{-9}\ M$ PbI2: $Ksp=[Pb^{2+}][I^-]^2\rightarrow Ksp=s\dot{}(2s)^2\rightarrow s=1.35\dot{}10^{-3}\ M$ PbI2 is more soluble. d) MgF2, 5.2e-11 vs 5.3e-11
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