Chemistry
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ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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![**Buffer Solution pH Change Calculation**
A buffer solution contains 0.298 M of CH₃NH₃Br and 0.350 M of CH₃NH₂ (methylamine). The task is to determine the pH change when 0.089 mol of HI is added to 1.00 L of this buffer.
- **Assumption:** \( K_b \) (CH₃NH₂) = \( 4.2 \times 10^{-4} \).
- **Calculation required:**
- pH after addition – pH before addition = pH change = [Blank Box for Input]
This calculation involves the use of the Henderson-Hasselbalch equation and the application of buffer capacity concepts to find the change in pH due to the addition of a strong acid (HI).](https://content.bartleby.com/qna-images/question/f0a8a901-2497-4ce7-b3d7-44550ff0e1ad/857edbbe-9db8-4577-b81e-5283b3414e56/1zjhmib_processed.png)
Transcribed Image Text:**Buffer Solution pH Change Calculation**
A buffer solution contains 0.298 M of CH₃NH₃Br and 0.350 M of CH₃NH₂ (methylamine). The task is to determine the pH change when 0.089 mol of HI is added to 1.00 L of this buffer.
- **Assumption:** \( K_b \) (CH₃NH₂) = \( 4.2 \times 10^{-4} \).
- **Calculation required:**
- pH after addition – pH before addition = pH change = [Blank Box for Input]
This calculation involves the use of the Henderson-Hasselbalch equation and the application of buffer capacity concepts to find the change in pH due to the addition of a strong acid (HI).
Transcribed Image Text:The problem involves a buffer solution containing 0.368 M NaH₂PO₄ (sodium dihydrogen phosphate) and 0.232 M K₂HPO₄ (dipotassium hydrogen phosphate). The task is to determine the pH change when 0.055 mol of HClO₄ (perchloric acid) is added to 1.00 L of this buffer.
The solution indicates that the pH change is 0.05.
**Explanation for Educational Website:**
This example illustrates the impact of adding a strong acid to a buffer solution. Here, NaH₂PO₄ acts as the acid component and K₂HPO₄ as the base component of the buffer. Buffers resist changes in pH when small amounts of acid or base are added. In this scenario, when 0.055 mol of HClO₄ is introduced, the buffer neutralizes it, resulting in a modest pH change of 0.05, showcasing the buffer’s effectiveness in maintaining pH stability.
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