Which of the following best describes why magnesium hydroxide, found in milk of magnesia, is soluble in acidic solution? O According to Le Chatelier's principle, the acid will react with hydroxide ions in the solution, forming water and thereby decreasing the concentration of hydroxide ions in solution causing more magnesium hydroxide to dissolve. Magnesium hydroxide does not dissolve in acidic solutions. According to Le Chatelier's principle, the acid will react with magnesium ions in the solution, forming magnesium hydride and causing more magnesium hydroxide to dissolve. According to Le Chatelier's principle, the acid will react with water in the solution, forming hydroxide ions and thereby decreasing the concentration of magnesium ions in solution causing more magnesium hydroxide to dissolve. According to Le Chatelier's principle, the acid will react with hydroxide ions in the solution, forming a precipitate.
Which of the following best describes why magnesium hydroxide, found in milk of magnesia, is soluble in acidic solution? O According to Le Chatelier's principle, the acid will react with hydroxide ions in the solution, forming water and thereby decreasing the concentration of hydroxide ions in solution causing more magnesium hydroxide to dissolve. Magnesium hydroxide does not dissolve in acidic solutions. According to Le Chatelier's principle, the acid will react with magnesium ions in the solution, forming magnesium hydride and causing more magnesium hydroxide to dissolve. According to Le Chatelier's principle, the acid will react with water in the solution, forming hydroxide ions and thereby decreasing the concentration of magnesium ions in solution causing more magnesium hydroxide to dissolve. According to Le Chatelier's principle, the acid will react with hydroxide ions in the solution, forming a precipitate.
Chemistry & Chemical Reactivity
10th Edition
ISBN:9781337399074
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter21: The Chemistry Of The Main Group Elements
Section: Chapter Questions
Problem 118IL
Related questions
Concept explainers
Ionic Equilibrium
Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.
Arrhenius Acid
Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red.
Bronsted Lowry Base In Inorganic Chemistry
Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.
Question
Transcribed Image Text:Which of the following best describes why magnesium hydroxide, found in milk of magnesia, is soluble in
acidic solution?
O According to Le Chatelier's principle, the acid will react with hydroxide ions in the solution, forming
water and thereby decreasing the concentration of hydroxide ions in solution causing more
magnesium hydroxide to dissolve.
O Magnesium hydroxide does not dissolve in acidic solutions.
O According to Le Chatelier's principle, the acid will react with magnesium ions in the solution, forming
magnesium hydride and causing more magnesium hydroxide to dissolve.
O According to Le Chatelier's principle, the acid will react with water in the solution, forming hydroxide
ions and thereby decreasing the concentration of magnesium ions in solution causing more
magnesium hydroxide to dissolve.
O According to Le Chatelier's principle, the acid will react with hydroxide ions in the solution, forming a
precipitate.
Expert Solution
This question has been solved!
Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.
This is a popular solution!
Trending now
This is a popular solution!
Step by step
Solved in 2 steps with 1 images
Knowledge Booster
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 & Chemical Reactivity
Chemistry
ISBN:
9781337399074
Author:
John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:
Cengage Learning
Chemistry & Chemical Reactivity
Chemistry
ISBN:
9781133949640
Author:
John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:
Cengage Learning
Introductory Chemistry: A Foundation
Chemistry
ISBN:
9781337399425
Author:
Steven S. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry & Chemical Reactivity
Chemistry
ISBN:
9781337399074
Author:
John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:
Cengage Learning
Chemistry & Chemical Reactivity
Chemistry
ISBN:
9781133949640
Author:
John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:
Cengage Learning
Introductory Chemistry: A Foundation
Chemistry
ISBN:
9781337399425
Author:
Steven S. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry: The Molecular Science
Chemistry
ISBN:
9781285199047
Author:
John W. Moore, Conrad L. Stanitski
Publisher:
Cengage Learning
Chemistry: An Atoms First Approach
Chemistry
ISBN:
9781305079243
Author:
Steven S. Zumdahl, Susan A. Zumdahl
Publisher:
Cengage Learning
Chemistry: Principles and Practice
Chemistry
ISBN:
9780534420123
Author:
Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:
Cengage Learning