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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

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
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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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.
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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