a. What is the pH of an aqueous solution of 100.0 mL with 1.00 mmol Ca(OH)2 (74.1 mg) dissolved in it? b. Selective precipitation can be used to clear brines of carbonates of calcium and magnesium during the manufacturing of salts for foods and pharmaceuticals. Will a precipitate form if a solution of 0.10 L of 8.0 x 103 M Ca(OH)2 is added to a solution of 0.40 L of 5.0 x 103 M Na2CO3? (Ksp for the insoluble salt is 3.36 x 10°) When considering an equilibrium of a dilute solution of Ca(OH)2 shown below, determine which way the equilibrium will shift given the following manipulations: c. Ca(OH)2(aq) = Ca²*(aq) + 20H'(aq) Removing Ca?+ Left No change Right Increasing Pressure Left No change Right Adding water Left No change Right

a. What is the pH of an aqueous solution of 100.0 mL with 1.00 mmol Ca(OH)2 (74.1 mg) dissolved in it? b. Selective precipitation can be used to clear brines of carbonates of calcium and magnesium during the manufacturing of salts for foods and pharmaceuticals. Will a precipitate form if a solution of 0.10 L of 8.0 x 103 M Ca(OH)2 is added to a solution of 0.40 L of 5.0 x 103 M Na2CO3? (Ksp for the insoluble salt is 3.36 x 10°) When considering an equilibrium of a dilute solution of Ca(OH)2 shown below, determine which way the equilibrium will shift given the following manipulations: c. Ca(OH)2(aq) = Ca²*(aq) + 20H'(aq) Removing Ca?+ Left No change Right Increasing Pressure Left No change Right Adding water Left No change Right

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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