Homework Help is Here – Start Your Trial Now!
Science
Chemistry
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
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...
See similar textbooks
icon
Related questions
icon
Concept explainers
Question
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.
Expert Solution
steps

Step by step

Solved in 2 steps with 2 images

SEE SOLUTIONCheck out a sample Q&A here
Blurred answer
Knowledge Booster
Ionic Equilibrium
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.
Recommended textbooks for you
Chemistry
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Organic Chemistry
Organic Chemistry
Chemistry
ISBN:
9780078021558
Author:
Janice Gorzynski Smith Dr.
Publisher:
McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
Elementary Principles of Chemical Processes, Bind…
Elementary Principles of Chemical Processes, Bind…
Chemistry
ISBN:
9781118431221
Author:
Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:
WILEY
SEE MORE TEXTBOOKS