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Finally, using the formula to convert between standard states, show that that your calculated values of AG and A.Gº¹ are in agreement.

Finally, using the formula to convert between standard states, show that that your calculated values of AG and A.Gº¹ are in agreement.

Biochemistry
Biochemistry
9th Edition
ISBN:9781319114671
Author:Lubert Stryer, Jeremy M. Berg, John L. Tymoczko, Gregory J. Gatto Jr.
Publisher:Lubert Stryer, Jeremy M. Berg, John L. Tymoczko, Gregory J. Gatto Jr.
Chapter1: Biochemistry: An Evolving Science
Section: Chapter Questions
Problem 1P
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**The Equilibrium Reaction for the Aqueous Dissociation of Acetic Acid** The equilibrium reaction for the aqueous dissociation of acetic acid is shown below: \[ \text{CH}_3\text{COOH(aq)} \rightleftharpoons \text{CH}_3\text{COO}^-(\text{aq}) + \text{H}^+(\text{aq}) \] Given the data in the table below and your knowledge of the "chemical standard state" (X°) and the "biochemical standard state" (X'°), answer parts a) to e). ### Questions **a)** For the dissociation of acetic acid at 298.15 K, calculate \( \Delta_rG^\circ \) and the corresponding \( pK_a \). **b)** Even though by definition, \( \Delta_fG^\circ(\text{H}^+(\text{aq})) = 0 \) and \( \Delta_fG'^\circ(\text{H}^+(\text{aq})) = 0 \), these are different physical quantities. What precisely does each represent? **c)** Calculate at 298.15 K, \( \Delta_fG'^\circ \) for \( \text{CH}_3\text{COOH(aq)} \) and \( \text{CH}_3\text{COO}^-(\text{aq}) \). **d)** For the dissociation of acetic acid at 298.15 K, calculate \( \Delta_rG'^\circ \). **e)** Finally, using the formula to convert between standard states, show that your calculated values of \( \Delta_rG^\circ \) and \( \Delta_rG'^\circ \) are in agreement. ### Table of Gibbs Free Energy of Formation The table below provides the Gibbs free energy of formation, in units of kJ mol\(^{-1}\), at \( T = 298.15 \, \text{K} \): | Substance | \( \Delta_fG^\circ \) | \( \Delta_fG'^\circ \) | |--------------------|-----------------------|------------------------| | \( \text{CH}_3\text{COOH(aq)} \) | -396.5 | | | \( \text{CH}_3\text{COO}^-(
Transcribed Image Text:**The Equilibrium Reaction for the Aqueous Dissociation of Acetic Acid** The equilibrium reaction for the aqueous dissociation of acetic acid is shown below: \[ \text{CH}_3\text{COOH(aq)} \rightleftharpoons \text{CH}_3\text{COO}^-(\text{aq}) + \text{H}^+(\text{aq}) \] Given the data in the table below and your knowledge of the "chemical standard state" (X°) and the "biochemical standard state" (X'°), answer parts a) to e). ### Questions **a)** For the dissociation of acetic acid at 298.15 K, calculate \( \Delta_rG^\circ \) and the corresponding \( pK_a \). **b)** Even though by definition, \( \Delta_fG^\circ(\text{H}^+(\text{aq})) = 0 \) and \( \Delta_fG'^\circ(\text{H}^+(\text{aq})) = 0 \), these are different physical quantities. What precisely does each represent? **c)** Calculate at 298.15 K, \( \Delta_fG'^\circ \) for \( \text{CH}_3\text{COOH(aq)} \) and \( \text{CH}_3\text{COO}^-(\text{aq}) \). **d)** For the dissociation of acetic acid at 298.15 K, calculate \( \Delta_rG'^\circ \). **e)** Finally, using the formula to convert between standard states, show that your calculated values of \( \Delta_rG^\circ \) and \( \Delta_rG'^\circ \) are in agreement. ### Table of Gibbs Free Energy of Formation The table below provides the Gibbs free energy of formation, in units of kJ mol\(^{-1}\), at \( T = 298.15 \, \text{K} \): | Substance | \( \Delta_fG^\circ \) | \( \Delta_fG'^\circ \) | |--------------------|-----------------------|------------------------| | \( \text{CH}_3\text{COOH(aq)} \) | -396.5 | | | \( \text{CH}_3\text{COO}^-(
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