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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7. Please answer and show all work, thank you!! :)
![**Chemical Equilibrium and Taste Perception**
**Equation and Explanation:**
7) \( \text{HX} \rightleftharpoons \text{H}^+ + \text{X}^{-1} \) \( (K_a = 2.5 \times 10^{-4}) \)
- **HX (sour)**
- **X⁻ (sweet)**
The chemical equation represents the equilibrium of a compound HX, which dissociates into H⁺ ions and X⁻. HX is known for having a sour taste, while X⁻ has a sweet taste. The equilibrium constant, \( K_a \), is \( 2.5 \times 10^{-4} \).
**Problem Statement:**
"At what pH would this system start to taste sweet (1 HX/ 100 X⁻)?"
This question asks for the pH at which the concentration of the sour-tasting HX becomes negligible compared to the sweet-tasting X⁻. Specifically, for every one molecule of HX, there should be 100 molecules of X⁻.
**Understanding the System:**
- The equilibrium constant \( K_a \) informs us about the ratio of the products to the reactants at equilibrium.
- The concentration of hydrogen ions \([H^+]\) will determine the pH of the solution.
- The system will taste sweet when the concentration ratio \([\text{HX}]/[\text{X}^-] = 1/100\).
To find the pH, use the equilibrium relationship and the provided concentration ratio.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F17525826-644e-4b54-80a2-4cc5c7d853ae%2F184efadb-264a-4481-8d5b-00cee51347cc%2Fkijq3ge_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Chemical Equilibrium and Taste Perception**
**Equation and Explanation:**
7) \( \text{HX} \rightleftharpoons \text{H}^+ + \text{X}^{-1} \) \( (K_a = 2.5 \times 10^{-4}) \)
- **HX (sour)**
- **X⁻ (sweet)**
The chemical equation represents the equilibrium of a compound HX, which dissociates into H⁺ ions and X⁻. HX is known for having a sour taste, while X⁻ has a sweet taste. The equilibrium constant, \( K_a \), is \( 2.5 \times 10^{-4} \).
**Problem Statement:**
"At what pH would this system start to taste sweet (1 HX/ 100 X⁻)?"
This question asks for the pH at which the concentration of the sour-tasting HX becomes negligible compared to the sweet-tasting X⁻. Specifically, for every one molecule of HX, there should be 100 molecules of X⁻.
**Understanding the System:**
- The equilibrium constant \( K_a \) informs us about the ratio of the products to the reactants at equilibrium.
- The concentration of hydrogen ions \([H^+]\) will determine the pH of the solution.
- The system will taste sweet when the concentration ratio \([\text{HX}]/[\text{X}^-] = 1/100\).
To find the pH, use the equilibrium relationship and the provided concentration ratio.
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