HCHO2 + H2O E--→CHO,1 + H3O* when the [CHO2'] increases then which of the following will occur? a) [H2O] inc. b) [HCHO2] dec. c) [H3O*] inc. d) they all increase T
HCHO2 + H2O E--→CHO,1 + H3O* when the [CHO2'] increases then which of the following will occur? a) [H2O] inc. b) [HCHO2] dec. c) [H3O*] inc. d) they all increase T
Introduction to General, Organic and Biochemistry
11th Edition
ISBN:9781285869759
Author:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar Torres
Publisher:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar Torres
Chapter7: Reaction Rates And Chemical Equilibrium
Section: Chapter Questions
Problem 7.75P
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![### Equilibrium and Reaction Dynamics
Consider the following chemical reaction at equilibrium:
\[ \text{HCHO}_2 + \text{H}_2\text{O} \leftrightarrow \text{CHO}_2^- + \text{H}_3\text{O}^+ \]
The question concerns the changes in reactant and product concentrations when the concentration of the formate ion (\(\text{CHO}_2^-\)) is increased.
#### Question
If the concentration of \([\text{CHO}_2^-]\) is increased, which of the following will occur?
a) \([\text{H}_2\text{O}]\) increases.
b) \([\text{HCHO}_2]\) decreases.
c) \([\text{H}_3\text{O}^+]\) increases.
d) They all increase.
### Explanation
Based on Le Chatelier's Principle, increasing the concentration of one of the products of a reaction at equilibrium will shift the equilibrium position to the left, favoring the formation of reactants. Consequently, the relevant changes can be inferred:
- \(\text{HCHO}_2\) concentration (\([\text{HCHO}_2]\)) is likely to increase as the system shifts to produce more reactants.
- \(\text{H}_2\text{O}\) concentration (\([\text{H}_2\text{O}]\)), assuming it's in large excess as a solvent, will likely remain relatively unchanged or increase slightly.
- \(\text{H}_3\text{O}^+\) concentration (\([\text{H}_3\text{O}^+]\)) will decrease as the system shifts to the left, consuming \(\text{H}_3\text{O}^+\) to form more \(\text{HCHO}_2\) and \(\text{H}_2\text{O}\).
Therefore, the correct answer is:
b) \([\text{HCHO}_2]\) decreases.
This detailed analysis helps in understanding how equilibrium shifts in response to changes in concentrations of products or reactants, a crucial concept in chemical reactions and equilibrium dynamics.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F11cb493f-74d8-445b-bfd0-ead085c73a2d%2Fe63daf53-1e8d-447b-a707-d3df5888c800%2F9pfux9e_processed.jpeg&w=3840&q=75)
Transcribed Image Text:### Equilibrium and Reaction Dynamics
Consider the following chemical reaction at equilibrium:
\[ \text{HCHO}_2 + \text{H}_2\text{O} \leftrightarrow \text{CHO}_2^- + \text{H}_3\text{O}^+ \]
The question concerns the changes in reactant and product concentrations when the concentration of the formate ion (\(\text{CHO}_2^-\)) is increased.
#### Question
If the concentration of \([\text{CHO}_2^-]\) is increased, which of the following will occur?
a) \([\text{H}_2\text{O}]\) increases.
b) \([\text{HCHO}_2]\) decreases.
c) \([\text{H}_3\text{O}^+]\) increases.
d) They all increase.
### Explanation
Based on Le Chatelier's Principle, increasing the concentration of one of the products of a reaction at equilibrium will shift the equilibrium position to the left, favoring the formation of reactants. Consequently, the relevant changes can be inferred:
- \(\text{HCHO}_2\) concentration (\([\text{HCHO}_2]\)) is likely to increase as the system shifts to produce more reactants.
- \(\text{H}_2\text{O}\) concentration (\([\text{H}_2\text{O}]\)), assuming it's in large excess as a solvent, will likely remain relatively unchanged or increase slightly.
- \(\text{H}_3\text{O}^+\) concentration (\([\text{H}_3\text{O}^+]\)) will decrease as the system shifts to the left, consuming \(\text{H}_3\text{O}^+\) to form more \(\text{HCHO}_2\) and \(\text{H}_2\text{O}\).
Therefore, the correct answer is:
b) \([\text{HCHO}_2]\) decreases.
This detailed analysis helps in understanding how equilibrium shifts in response to changes in concentrations of products or reactants, a crucial concept in chemical reactions and equilibrium dynamics.
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