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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![**Buffer Solution pH Calculation**
**Scenario:**
A volume of 500.0 mL of 0.160 M NaOH is added to 605 mL of 0.200 M weak acid (\(K_a = 6.12 \times 10^{-5}\)). What is the pH of the resulting buffer solution?
**Chemical Equation:**
\[
HA(aq) + OH^-(aq) \rightarrow H_2O(l) + A^-(aq)
\]
**Calculation:**
To find the pH of the buffer solution, you can use the equation for a buffer system which typically involves calculating the concentrations of the acid (\([HA]\)) and the conjugate base (\([A^-]\)) after the reaction and applying the Henderson-Hasselbalch equation.
**pH =** [To be calculated]
---
**Explanation:**
This problem involves a buffer solution created by mixing a strong base (NaOH) with a weak acid. The equation illustrates the reaction between the weak acid and hydroxide ions. The pH will depend on the concentrations of the acid and its conjugate base remaining in the solution.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fe413ba53-b36f-40cd-9f3b-7507865f79d2%2F8b56374b-f160-4be2-a324-77166dc10022%2F86g2vdq.jpeg&w=3840&q=75)
Transcribed Image Text:**Buffer Solution pH Calculation**
**Scenario:**
A volume of 500.0 mL of 0.160 M NaOH is added to 605 mL of 0.200 M weak acid (\(K_a = 6.12 \times 10^{-5}\)). What is the pH of the resulting buffer solution?
**Chemical Equation:**
\[
HA(aq) + OH^-(aq) \rightarrow H_2O(l) + A^-(aq)
\]
**Calculation:**
To find the pH of the buffer solution, you can use the equation for a buffer system which typically involves calculating the concentrations of the acid (\([HA]\)) and the conjugate base (\([A^-]\)) after the reaction and applying the Henderson-Hasselbalch equation.
**pH =** [To be calculated]
---
**Explanation:**
This problem involves a buffer solution created by mixing a strong base (NaOH) with a weak acid. The equation illustrates the reaction between the weak acid and hydroxide ions. The pH will depend on the concentrations of the acid and its conjugate base remaining in the solution.
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