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

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

Chemistry
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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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. \( \text{MgF}_2; \text{molar solubility} = 2.65 \times 10^{-4} \, \text{M} \)
Transcribed Image Text:**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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