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A buffer solution contains 0.298 M CH3NH3 Br and 0.350 M CH3NH2 (methylamine). Determine the pH change when 0.089 mol HI is added to 1.00 L of the buffer. (Assume Kb (CH3NH₂) = 4.2 x 10-4.) pH after addition - pH before addition = pH change = ||

A buffer solution contains 0.298 M CH3NH3 Br and 0.350 M CH3NH2 (methylamine). Determine the pH change when 0.089 mol HI is added to 1.00 L of the buffer. (Assume Kb (CH3NH₂) = 4.2 x 10-4.) pH after addition - pH before addition = pH change = ||

Chemistry
Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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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).
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).
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.
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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