Magnesium hydroxide is only very slightly soluble in water. The reaction by which it goes into solution is: Mg(O H)2(s) = Mg²+(a q) + 2 O H minus (a q)
Magnesium hydroxide is only very slightly soluble in water. The reaction by which it goes into solution is: Mg(O H)2(s) = Mg²+(a q) + 2 O H minus (a q)
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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![### Solubility of Magnesium Hydroxide and the Effect of Adding Hydroxide Ions
Magnesium hydroxide (Mg(OH)₂) is only very slightly soluble in water. The reaction by which it goes into solution is as follows:
\[ \text{Mg(OH)}_2(\text{s}) \leftrightarrow \text{Mg}^{2+}(\text{aq}) + 2 \text{OH}^- (\text{aq}) \]
When hydroxide ions (OH⁻) are added to the solution, it affects the equilibrium of this reaction according to Le Chatelier's principle.
**Question:**
What will happen if OH⁻ is added to the solution and why?
1. Solid dissolves. OH⁻ concentration decreases. Reaction moves to the left.
2. **Solid remains. OH⁻ concentration decreases. Reaction moves to the left.** (Correct answer)
3. Solid remains. OH⁻ concentration decreases. Reaction moves to the right.
4. Solid dissolves. OH⁻ concentration increases. Reaction moves to the right.
5. Solid dissolves. OH⁻ concentration decreases. Reaction moves to the right.
6. Solid remains. OH⁻ concentration increases. Reaction moves to the right.
7. Solid remains. OH⁻ concentration increases. Reaction moves to the left.
**Explanation:**
When additional OH⁻ ions are introduced into the solution, the equilibrium will shift to counteract this change (Le Chatelier's Principle). The reaction will move left to decrease the concentration of OH⁻ ions by precipitating more \( \text{Mg(OH)}_2 \) as a solid. Therefore, the solid remains and the concentration of OH⁻ decreases as the system strives to reach a new equilibrium.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F4e4f8662-3b3d-4e1d-95ea-59793f6a3296%2F58effc3e-800e-4607-a4a7-1e9350fd1a5c%2F7ywafd_reoriented.jpeg&w=3840&q=75)
Transcribed Image Text:### Solubility of Magnesium Hydroxide and the Effect of Adding Hydroxide Ions
Magnesium hydroxide (Mg(OH)₂) is only very slightly soluble in water. The reaction by which it goes into solution is as follows:
\[ \text{Mg(OH)}_2(\text{s}) \leftrightarrow \text{Mg}^{2+}(\text{aq}) + 2 \text{OH}^- (\text{aq}) \]
When hydroxide ions (OH⁻) are added to the solution, it affects the equilibrium of this reaction according to Le Chatelier's principle.
**Question:**
What will happen if OH⁻ is added to the solution and why?
1. Solid dissolves. OH⁻ concentration decreases. Reaction moves to the left.
2. **Solid remains. OH⁻ concentration decreases. Reaction moves to the left.** (Correct answer)
3. Solid remains. OH⁻ concentration decreases. Reaction moves to the right.
4. Solid dissolves. OH⁻ concentration increases. Reaction moves to the right.
5. Solid dissolves. OH⁻ concentration decreases. Reaction moves to the right.
6. Solid remains. OH⁻ concentration increases. Reaction moves to the right.
7. Solid remains. OH⁻ concentration increases. Reaction moves to the left.
**Explanation:**
When additional OH⁻ ions are introduced into the solution, the equilibrium will shift to counteract this change (Le Chatelier's Principle). The reaction will move left to decrease the concentration of OH⁻ ions by precipitating more \( \text{Mg(OH)}_2 \) as a solid. Therefore, the solid remains and the concentration of OH⁻ decreases as the system strives to reach a new equilibrium.
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