b and c **89. Use the given molar solubilities in pure water to calculate \(K_{sp}\) for each compound.***Missed this? Read Section 18.5*a. \( \text{MX; molar solubility} = 3.27 \times 10^{-11} \, \text{M} \)b. \( \text{PbF}_2; \text{molar solubility} = 5.63 \times 10^{-3} \, \text{M} \)c. \( \text{MgF}_2; \text{molar solubility} = 2.65 \times 10^{-4} \, \text{M} \)

Calculate Ksp of the given solubility --

Answered: 5.63 × 10¯3 M b. PbF2; molar solubility…

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5.63 × 10¯3 M b. PbF2; molar solubility c. MgF2; molar solubility 2.65 × 10-4 M

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Question

b and c

**89. Use the given molar solubilities in pure water to calculate \(K_{sp}\) for each compound.**

*Missed this? Read Section 18.5*

a. \( \text{MX; molar solubility} = 3.27 \times 10^{-11} \, \text{M} \)

b. \( \text{PbF}_2; \text{molar solubility} = 5.63 \times 10^{-3} \, \text{M} \)

c. \( \text{MgF}_2; \text{molar solubility} = 2.65 \times 10^{-4} \, \text{M} \)

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