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Based on the given value of the Kp. calculate the ratio of solubility of Mg(OH)2 dissolved in pure H20 to Mg(OH)2 dissolved in a 0.190 M NAOH solution. Express your answer numerically to three significant figures.

Based on the given value of the Kp. calculate the ratio of solubility of Mg(OH)2 dissolved in pure H20 to Mg(OH)2 dissolved in a 0.190 M NAOH solution. Express your answer numerically to three significant figures.

Chemistry: The Molecular Science
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter15: Additional Aqueous Equilibria
Section: Chapter Questions
Problem 15.BCP
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The common-ion effect is an application of Le Châtelier's principle, which states that an equilibrium system that is stressed will work to alleviate that stress and reestablish equilibrium. Part C- Calculate how many times more soluble Mg(OH)2 is in pure water Based on the given value of the Kp, calculate the ratio solubility of Mg(OH)2 dissolved in pure H20 to Mg(OH)2 dissolved in a 0.190 MNaOH solution. Express your answer numerically to three significant figures. > View Available Hint(s) να ΑΣφ solubility Mg(OH), in pure water ratio solubility Mg(OH), in NAOH solution = 1.72 • 10-5 You have already submitted this answer. Enter a new answer. No credit lost. Try again. Submit Previous Answers The common-ion effect and buffer systems A buffer is a mixed solution of a weak acid or base, combined with its conjugate. Note that this can be understood essentially as a common-ion problem: The conjugate is a common ion added to an equilibrium system of a weak acid or base. The addition of the conjugate shifts the equilibrium of the system to relieve the stress of the added concentration of the common ion. In a solution consisting of a weak acid or base, the equilibrium shift also results in a pH shift of the system. It is the presence of the common ion in the system that results in buffering behavior, because both added H' or OH ions can be neutralized.
Transcribed Image Text:The common-ion effect is an application of Le Châtelier's principle, which states that an equilibrium system that is stressed will work to alleviate that stress and reestablish equilibrium. Part C- Calculate how many times more soluble Mg(OH)2 is in pure water Based on the given value of the Kp, calculate the ratio solubility of Mg(OH)2 dissolved in pure H20 to Mg(OH)2 dissolved in a 0.190 MNaOH solution. Express your answer numerically to three significant figures. > View Available Hint(s) να ΑΣφ solubility Mg(OH), in pure water ratio solubility Mg(OH), in NAOH solution = 1.72 • 10-5 You have already submitted this answer. Enter a new answer. No credit lost. Try again. Submit Previous Answers The common-ion effect and buffer systems A buffer is a mixed solution of a weak acid or base, combined with its conjugate. Note that this can be understood essentially as a common-ion problem: The conjugate is a common ion added to an equilibrium system of a weak acid or base. The addition of the conjugate shifts the equilibrium of the system to relieve the stress of the added concentration of the common ion. In a solution consisting of a weak acid or base, the equilibrium shift also results in a pH shift of the system. It is the presence of the common ion in the system that results in buffering behavior, because both added H' or OH ions can be neutralized.
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