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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![**Problem Statement:**
Determine the [OH⁻] concentration in 0.191 M M(OH)₂ solution, where M is a metal and M(OH)₂ is a soluble compound.
**Explanation:**
This problem requires us to calculate the concentration of hydroxide ions [OH⁻] in a given solution of a soluble metal hydroxide M(OH)₂. This type of question is helpful for understanding concepts related to chemical equilibrium, solubility, and stoichiometry.
For a soluble metal hydroxide like M(OH)₂, which dissolves completely in water, the dissociation can be represented as follows:
\[ \text{M(OH)}_2 \rightarrow \text{M}^{2+} + 2\text{OH}^- \]
Given that the initial concentration of M(OH)₂ is 0.191 M, we can use the stoichiometry of the dissociation reaction to determine that the concentration of hydroxide ions [OH⁻] will be twice the concentration of M(OH)₂, because each formula unit produces two OH⁻ ions upon dissociation.
Thus, the [OH⁻] concentration will be:
\[ [OH^-] = 2 \times 0.191 \text{ M} \]
\[ [OH^-] = 0.382 \text{ M} \]
Therefore, the hydroxide ion concentration [OH⁻] in the 0.191 M M(OH)₂ solution is 0.382 M.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fdabc7e8b-d42d-4c7a-8b8c-eac102cb510a%2F67fd0dfc-cace-4587-ac09-227c491d34d3%2F9qzxntq_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Problem Statement:**
Determine the [OH⁻] concentration in 0.191 M M(OH)₂ solution, where M is a metal and M(OH)₂ is a soluble compound.
**Explanation:**
This problem requires us to calculate the concentration of hydroxide ions [OH⁻] in a given solution of a soluble metal hydroxide M(OH)₂. This type of question is helpful for understanding concepts related to chemical equilibrium, solubility, and stoichiometry.
For a soluble metal hydroxide like M(OH)₂, which dissolves completely in water, the dissociation can be represented as follows:
\[ \text{M(OH)}_2 \rightarrow \text{M}^{2+} + 2\text{OH}^- \]
Given that the initial concentration of M(OH)₂ is 0.191 M, we can use the stoichiometry of the dissociation reaction to determine that the concentration of hydroxide ions [OH⁻] will be twice the concentration of M(OH)₂, because each formula unit produces two OH⁻ ions upon dissociation.
Thus, the [OH⁻] concentration will be:
\[ [OH^-] = 2 \times 0.191 \text{ M} \]
\[ [OH^-] = 0.382 \text{ M} \]
Therefore, the hydroxide ion concentration [OH⁻] in the 0.191 M M(OH)₂ solution is 0.382 M.
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