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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![**Title: Calculation of pH and pOH for a Mixed Acid Solution**
**Introduction:**
Understanding the pH and pOH of solutions is crucial in various branches of chemistry, particularly when dealing with acids and bases. This exercise outlines the steps to calculate the pH and pOH of an aqueous solution containing specific concentrations of hydrochloric acid (HCl) and hydrobromic acid (HBr) at a temperature of 25°C.
---
**Problem Statement:**
Calculate the pH and the pOH of an aqueous solution that is 0.030 M in HCl(aq) and 0.060 M in HBr(aq) at 25 °C.
---
**Step-by-Step Solution:**
**1. Combined Concentration of Hydronium Ions:**
Both HCl and HBr are strong acids and dissociate completely in water. Therefore, the total concentration of the hydronium ions (\([H_3O^+]\)) in the solution is the sum of the concentrations of the individual acids.
\[
[H_3O^+] = [HCl] + [HBr] = 0.030\, \text{M} + 0.060\, \text{M} = 0.090\, \text{M}
\]
**2. Calculation of pH:**
The pH of the solution is calculated using the formula:
\[
\text{pH} = -\log[H_3O^+]
\]
Substituting the value from the previous step:
\[
\text{pH} = -\log(0.090)
\]
Using a calculator:
\[
\text{pH} \approx 1.05
\]
**3. Calculation of pOH:**
The relationship between pH and pOH for any aqueous solution at 25 °C is given by:
\[
\text{pH} + \text{pOH} = 14
\]
Rearranging to solve for pOH:
\[
\text{pOH} = 14 - \text{pH}
\]
Substituting the calculated pH:
\[
\text{pOH} = 14 - 1.05 = 12.95
\]
---
**Conclusion:**
For the given solution with concentrations of 0.030 M HCl and 0.060 M HBr at](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fbd6e2cac-a13e-4af0-8d42-5fb7a66b94d3%2F6ca2d4ad-d6f7-46e8-b505-655e2479208d%2Fvhnav95_processed.png&w=3840&q=75)
Transcribed Image Text:**Title: Calculation of pH and pOH for a Mixed Acid Solution**
**Introduction:**
Understanding the pH and pOH of solutions is crucial in various branches of chemistry, particularly when dealing with acids and bases. This exercise outlines the steps to calculate the pH and pOH of an aqueous solution containing specific concentrations of hydrochloric acid (HCl) and hydrobromic acid (HBr) at a temperature of 25°C.
---
**Problem Statement:**
Calculate the pH and the pOH of an aqueous solution that is 0.030 M in HCl(aq) and 0.060 M in HBr(aq) at 25 °C.
---
**Step-by-Step Solution:**
**1. Combined Concentration of Hydronium Ions:**
Both HCl and HBr are strong acids and dissociate completely in water. Therefore, the total concentration of the hydronium ions (\([H_3O^+]\)) in the solution is the sum of the concentrations of the individual acids.
\[
[H_3O^+] = [HCl] + [HBr] = 0.030\, \text{M} + 0.060\, \text{M} = 0.090\, \text{M}
\]
**2. Calculation of pH:**
The pH of the solution is calculated using the formula:
\[
\text{pH} = -\log[H_3O^+]
\]
Substituting the value from the previous step:
\[
\text{pH} = -\log(0.090)
\]
Using a calculator:
\[
\text{pH} \approx 1.05
\]
**3. Calculation of pOH:**
The relationship between pH and pOH for any aqueous solution at 25 °C is given by:
\[
\text{pH} + \text{pOH} = 14
\]
Rearranging to solve for pOH:
\[
\text{pOH} = 14 - \text{pH}
\]
Substituting the calculated pH:
\[
\text{pOH} = 14 - 1.05 = 12.95
\]
---
**Conclusion:**
For the given solution with concentrations of 0.030 M HCl and 0.060 M HBr at
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