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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

General Chemistry - Standalone book (MindTap Course List)
General Chemistry - Standalone book (MindTap Course List)
11th Edition
ISBN:9781305580343
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Publisher:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Chapter16: Acid-base Equilibria
Section: Chapter Questions
Problem 16.125QP: A solution made up of 1.0 M NH3 and 0.50 M (NH4)2SO4 has a pH of 9.26. a Write the net ionic...
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15. I've got my ion you. Calcium hydroxide has many uses in the pharmaceutical industry as well as USDA-certified food production. 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 0.40L of 5.0 x 103 M Na2CO3? (Ksp for the insoluble salt is 3.36 x 10) c. 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: Ca(OH)2(aq) = Ca²*(aq) + 20H (ag) Removing Ca?+ Left No change Right Increasing Pressure Left No change Right Adding water Left No change Right
Transcribed Image Text:15. I've got my ion you. Calcium hydroxide has many uses in the pharmaceutical industry as well as USDA-certified food production. 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 0.40L of 5.0 x 103 M Na2CO3? (Ksp for the insoluble salt is 3.36 x 10) c. 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: Ca(OH)2(aq) = Ca²*(aq) + 20H (ag) Removing Ca?+ Left No change Right Increasing Pressure Left No change Right Adding water Left No change Right
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