**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.

A buffer is a solution which resists any change in pH on adding a small amount of acid or base.It is…

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

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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Concept explainers

Acid Base Titration

An acid-base titration is the method of quantitative analysis for determining the concentration of an acid and base by exactly neutralizing it with a standard solution of base or acid having known concentration.

Question

**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.

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