The measured pH of a 0.300 M HBr solution at 25 °C is 0.632. Calculate the activity coefficient for H* in this solution. YH* = The measured pH of a 0.300 M HNO, solution at 25 °C is 0.657. Calculate the activity coefficient for H* in this solution. YH+ =
The measured pH of a 0.300 M HBr solution at 25 °C is 0.632. Calculate the activity coefficient for H* in this solution. YH* = The measured pH of a 0.300 M HNO, solution at 25 °C is 0.657. Calculate the activity coefficient for H* in this solution. YH+ =
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Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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![## Calculation of Activity Coefficient for H⁺
### Problem 1:
**Measured pH of a 0.300 M HBr Solution**
The measured pH of a 0.300 M HBr solution at 25 °C is 0.632. Calculate the activity coefficient for H⁺ in this solution.
**Activity Coefficient \(\gamma_{H^+}\):**
\[ \gamma_{H^+} = \]
### Problem 2:
**Measured pH of a 0.300 M HNO₃ Solution**
The measured pH of a 0.300 M HNO₃ solution at 25 °C is 0.657. Calculate the activity coefficient for H⁺ in this solution.
**Activity Coefficient \(\gamma_{H^+}\):**
\[ \gamma_{H^+} = \]
---
### Explanation:
To calculate the activity coefficient for \( H^+ \) in these solutions, follow these steps:
1. **Determine the concentration of \( H^+ \) from the pH:**
\[ [H^+] = 10^{-\text{pH}} \]
2. **Calculate the activity coefficient \(\gamma_{H^+}\):**
\[ \gamma_{H^+} = \frac{[H^+]_{\text{calc}}}{[H^+]_{\text{measured}}} \]
Here,
- \([H^+]_{\text{calc}}\) is the concentration of \( H^+ \) ions assuming full dissociation.
- \([H^+]_{\text{measured}}\) is the concentration of \( H^+ \) ions derived from the measured pH.
For a 0.300 M solution of a strong acid like HBr or HNO₃, we assume full dissociation:
\[ \text{Initial} \ [H^+] = 0.300 \ M \]
By substituting the measured pH values into the calculations, you can find \(\gamma_{H^+}\).
---
To provide a more comprehensive understanding, these will result in numerical answers when the pH measurements are plugged into the equations.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fbd6e2cac-a13e-4af0-8d42-5fb7a66b94d3%2F3508444a-4143-4a22-8281-911d8cc3a61e%2Fr19o2be_processed.png&w=3840&q=75)
Transcribed Image Text:## Calculation of Activity Coefficient for H⁺
### Problem 1:
**Measured pH of a 0.300 M HBr Solution**
The measured pH of a 0.300 M HBr solution at 25 °C is 0.632. Calculate the activity coefficient for H⁺ in this solution.
**Activity Coefficient \(\gamma_{H^+}\):**
\[ \gamma_{H^+} = \]
### Problem 2:
**Measured pH of a 0.300 M HNO₃ Solution**
The measured pH of a 0.300 M HNO₃ solution at 25 °C is 0.657. Calculate the activity coefficient for H⁺ in this solution.
**Activity Coefficient \(\gamma_{H^+}\):**
\[ \gamma_{H^+} = \]
---
### Explanation:
To calculate the activity coefficient for \( H^+ \) in these solutions, follow these steps:
1. **Determine the concentration of \( H^+ \) from the pH:**
\[ [H^+] = 10^{-\text{pH}} \]
2. **Calculate the activity coefficient \(\gamma_{H^+}\):**
\[ \gamma_{H^+} = \frac{[H^+]_{\text{calc}}}{[H^+]_{\text{measured}}} \]
Here,
- \([H^+]_{\text{calc}}\) is the concentration of \( H^+ \) ions assuming full dissociation.
- \([H^+]_{\text{measured}}\) is the concentration of \( H^+ \) ions derived from the measured pH.
For a 0.300 M solution of a strong acid like HBr or HNO₃, we assume full dissociation:
\[ \text{Initial} \ [H^+] = 0.300 \ M \]
By substituting the measured pH values into the calculations, you can find \(\gamma_{H^+}\).
---
To provide a more comprehensive understanding, these will result in numerical answers when the pH measurements are plugged into the equations.
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