pH = 6.9 small can be neutralized can not be neutralized is not dissolved large Reset Help When strong acid is added to a buffer, there is a small pH change because the added acid by one of the components in the buffer. Therefore, the effect on the [H3O+] in the solution is When strong acid is added to pure water, there is a large pH change because the added acid in pure water. This will result in a effect on the [H3O+] in the solution.
pH = 6.9 small can be neutralized can not be neutralized is not dissolved large Reset Help When strong acid is added to a buffer, there is a small pH change because the added acid by one of the components in the buffer. Therefore, the effect on the [H3O+] in the solution is When strong acid is added to pure water, there is a large pH change because the added acid in pure water. This will result in a effect on the [H3O+] in the solution.
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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![**Buffer Systems in Chemistry**
*Understanding the Role of Buffers in pH Regulation*
**Figure Explanation:**
- **Water vs. Buffer Response to Acid:**
- On the left, two beakers labeled "Water" show the pH change when acid is added:
- Initial pH = 7.0
- After acid addition, pH = 3.0
- On the right, two beakers labeled "Buffer" display:
- Initial pH = 7.0
- After acid addition, pH = 6.9
This figure illustrates that adding a few drops of a strong acid significantly lowers the pH of pure water, but only slightly alters the pH of a buffer solution.
**Text Explanation:**
- **Buffer System:**
- Buffers resist significant changes in pH upon the addition of acids or bases.
- In the given scenario, the buffer limits the pH change to 0.1 units compared to a much larger change in pure water.
**Interactive Exercise:**
- **Fill in the Blanks:**
*Options:* `small`, `large`, `can be neutralized`, `cannot be neutralized`
1. When strong acid is added to a buffer, there is a **small** pH change because the added acid **can be neutralized** by one of the components in the buffer. Therefore, the effect on the \([H_3O^+]\) in the solution is **small**.
2. When strong acid is added to pure water, there is a **large** pH change because the added acid **cannot be neutralized** in pure water. This will result in a **large** effect on the \([H_3O^+]\) in the solution.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fb4d4e6a3-fd83-4270-b000-89a89a72868b%2F146f5a04-2688-4bee-a629-9161fea03da8%2Fgud9tj_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Buffer Systems in Chemistry**
*Understanding the Role of Buffers in pH Regulation*
**Figure Explanation:**
- **Water vs. Buffer Response to Acid:**
- On the left, two beakers labeled "Water" show the pH change when acid is added:
- Initial pH = 7.0
- After acid addition, pH = 3.0
- On the right, two beakers labeled "Buffer" display:
- Initial pH = 7.0
- After acid addition, pH = 6.9
This figure illustrates that adding a few drops of a strong acid significantly lowers the pH of pure water, but only slightly alters the pH of a buffer solution.
**Text Explanation:**
- **Buffer System:**
- Buffers resist significant changes in pH upon the addition of acids or bases.
- In the given scenario, the buffer limits the pH change to 0.1 units compared to a much larger change in pure water.
**Interactive Exercise:**
- **Fill in the Blanks:**
*Options:* `small`, `large`, `can be neutralized`, `cannot be neutralized`
1. When strong acid is added to a buffer, there is a **small** pH change because the added acid **can be neutralized** by one of the components in the buffer. Therefore, the effect on the \([H_3O^+]\) in the solution is **small**.
2. When strong acid is added to pure water, there is a **large** pH change because the added acid **cannot be neutralized** in pure water. This will result in a **large** effect on the \([H_3O^+]\) in the solution.
Expert Solution
Step 1 Concept
Buffer solution — A solution which prevents change in pH on adding small amount of any acid or base
e. g. Mixture of weak acid and Salt of weak acid, salt of weak base
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