Calculate [OH ], [H*], and the pH of 0.41 M solutions of each of the following amines (K, for aniline is 3.8 × 10-10, K½ for methylamine is 4.38 × 104). a. aniline [OH¯] =[ м [H*] = [ pH = b. methylamine [OH¯] = [ |M [H*] =[ M pH =
Calculate [OH ], [H*], and the pH of 0.41 M solutions of each of the following amines (K, for aniline is 3.8 × 10-10, K½ for methylamine is 4.38 × 104). a. aniline [OH¯] =[ м [H*] = [ pH = b. methylamine [OH¯] = [ |M [H*] =[ M pH =
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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![**Calculation of Hydroxide Ion Concentration \([OH^-]\), Hydrogen Ion Concentration \([H^+]\), and pH of Amine Solutions**
On this page, we demonstrate the process of calculating \( [OH^-] \), \( [H^+] \), and the pH of 0.41 M solutions of two different amines. We use the base dissociation constants (\( K_b \)) for each amine to facilitate these calculations.
Given:
- For aniline: \( K_b = 3.8 \times 10^{-10} \)
- For methylamine: \( K_b = 4.38 \times 10^{-4} \)
### a. Aniline
1. **Hydroxide Ion Concentration \([OH^-]\)**:
Input area for result: \_\_\_\_\_\_ M
2. **Hydrogen Ion Concentration \([H^+]\)**:
Input area for result: \_\_\_\_\_\_ M
3. **pH**:
Input area for result: \_\_\_\_\_\_
### b. Methylamine
1. **Hydroxide Ion Concentration \([OH^-]\)**:
Input area for result: \_\_\_\_\_\_ M
2. **Hydrogen Ion Concentration \([H^+]\)**:
Input area for result: \_\_\_\_\_\_ M
3. **pH**:
Input area for result: \_\_\_\_\_\_
For each amine, you can calculate the hydroxide ion concentration \([OH^-]\) using the \( K_b \) value and the initial concentration of the amine solution. Once \([OH^-]\) is determined, you can calculate \([H^+]\) using the water dissociation constant \( K_w = 1.0 \times 10^{-14} \) at 25°C. Finally, the pH of the solution can be calculated using the formula:
\[ \text{pH} = -\log [H^+] \]
This framework helps in understanding the influence of different \( K_b \) values on the pH of amine solutions.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fe97458c2-7e02-460f-9567-4103232c1712%2Fa461b93e-d48c-4fd6-8401-11de373429fa%2F8n1obld.png&w=3840&q=75)
Transcribed Image Text:**Calculation of Hydroxide Ion Concentration \([OH^-]\), Hydrogen Ion Concentration \([H^+]\), and pH of Amine Solutions**
On this page, we demonstrate the process of calculating \( [OH^-] \), \( [H^+] \), and the pH of 0.41 M solutions of two different amines. We use the base dissociation constants (\( K_b \)) for each amine to facilitate these calculations.
Given:
- For aniline: \( K_b = 3.8 \times 10^{-10} \)
- For methylamine: \( K_b = 4.38 \times 10^{-4} \)
### a. Aniline
1. **Hydroxide Ion Concentration \([OH^-]\)**:
Input area for result: \_\_\_\_\_\_ M
2. **Hydrogen Ion Concentration \([H^+]\)**:
Input area for result: \_\_\_\_\_\_ M
3. **pH**:
Input area for result: \_\_\_\_\_\_
### b. Methylamine
1. **Hydroxide Ion Concentration \([OH^-]\)**:
Input area for result: \_\_\_\_\_\_ M
2. **Hydrogen Ion Concentration \([H^+]\)**:
Input area for result: \_\_\_\_\_\_ M
3. **pH**:
Input area for result: \_\_\_\_\_\_
For each amine, you can calculate the hydroxide ion concentration \([OH^-]\) using the \( K_b \) value and the initial concentration of the amine solution. Once \([OH^-]\) is determined, you can calculate \([H^+]\) using the water dissociation constant \( K_w = 1.0 \times 10^{-14} \) at 25°C. Finally, the pH of the solution can be calculated using the formula:
\[ \text{pH} = -\log [H^+] \]
This framework helps in understanding the influence of different \( K_b \) values on the pH of amine solutions.
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