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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![**Question 2: Buffer and Indicator Dependence**
What are the two factors that an indicator depends upon?
By equations, show how the buffer resists the change in pH when acid or base are added.
---
In educational context, this question is exploring the chemistry behind indicators and buffer solutions:
- **Indicators** primarily depend on:
1. The pH range in which they change color.
2. The specific equilibrium constant, \(K_{\text{a}}\), of the indicator.
- **Buffer Solutions** work to resist changes in pH through:
- The presence of both a weak acid and its conjugate base (or a weak base and its conjugate acid). This allows buffer solutions to neutralize small amounts of added acid or base.
**Equations Demonstrating Buffer Action:**
1. **Weak Acid \( (HA) \) Reaction:**
\[ \text{HA} \rightleftharpoons \text{H}^+ + \text{A}^- \]
2. **Buffer Action Against Added Acid \( (H^+) \):**
\[ \text{A}^- + \text{H}^+ \rightarrow \text{HA} \]
3. **Buffer Action Against Added Base \( (OH^-) \):**
\[ \text{HA} + \text{OH}^- \rightarrow \text{A}^- + \text{H}_2\text{O} \]
These reactions showcase how a buffer maintains pH by utilizing the weak acid/base pair to neutralize added H⁺ or OH⁻ ions, preventing significant pH shifts.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F816b840c-3165-49ec-880b-7eda3f3e03a8%2Fba6b13f1-fa47-4e3a-9807-0a7282cd9fe1%2Fc6xuooe_processed.png&w=3840&q=75)
Transcribed Image Text:**Question 2: Buffer and Indicator Dependence**
What are the two factors that an indicator depends upon?
By equations, show how the buffer resists the change in pH when acid or base are added.
---
In educational context, this question is exploring the chemistry behind indicators and buffer solutions:
- **Indicators** primarily depend on:
1. The pH range in which they change color.
2. The specific equilibrium constant, \(K_{\text{a}}\), of the indicator.
- **Buffer Solutions** work to resist changes in pH through:
- The presence of both a weak acid and its conjugate base (or a weak base and its conjugate acid). This allows buffer solutions to neutralize small amounts of added acid or base.
**Equations Demonstrating Buffer Action:**
1. **Weak Acid \( (HA) \) Reaction:**
\[ \text{HA} \rightleftharpoons \text{H}^+ + \text{A}^- \]
2. **Buffer Action Against Added Acid \( (H^+) \):**
\[ \text{A}^- + \text{H}^+ \rightarrow \text{HA} \]
3. **Buffer Action Against Added Base \( (OH^-) \):**
\[ \text{HA} + \text{OH}^- \rightarrow \text{A}^- + \text{H}_2\text{O} \]
These reactions showcase how a buffer maintains pH by utilizing the weak acid/base pair to neutralize added H⁺ or OH⁻ ions, preventing significant pH shifts.
Expert Solution
Step 1
Indicators are the chemical species which indicate the completion of the reaction by showing the colour change.
Indicator depends on the two factors they are:
(1) pH of the solution, the colour change of the indicator in the solution depends on the pH of the solution. The colour of the indicators is different in acidic and basic medium indicating the solutions as acidic or basic in nature.
(2) In redox reactions the exchange of electrons also causes the change in colour of the indicators.
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