Determine the pH of a buffer that is 0.25 M NH, and 0.15 M NH.CI. The value of pKb for NH, is 4.75. PREV NEXT Based on your ICE table and definition of Kb, set up the expression for Kb in order to determine the unknown. Do not combine or simplify terms. Kp
Determine the pH of a buffer that is 0.25 M NH, and 0.15 M NH.CI. The value of pKb for NH, is 4.75. PREV NEXT Based on your ICE table and definition of Kb, set up the expression for Kb in order to determine the unknown. Do not combine or simplify terms. Kp
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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And what is the pH?
![**Buffer pH Determination Exercise**
**Question 3 of 16**
**Task:** Determine the pH of a buffer solution containing 0.25 M NH₃ and 0.15 M NH₄Cl. The pKₚ value for NH₃ is given as 4.75.
Using your ICE (Initial, Change, Equilibrium) table and the definition of the base dissociation constant (Kₚ), construct the expression for Kₚ to determine the unknown variable, ensuring not to combine or simplify terms.
**Equation Setup:**
\[ K_ b = \dfrac{[NH₄^+][OH^-]}{[NH₃]} \]
**Interactive Tools:**
- A series of buttons with various values and expressions such as [0], [0.25], [0.15], [4.75], [x], [2x], [2x²], [0.25 + x], [0.25 - x], 1.78 x 10⁻⁵, 5.62 x 10⁻¹⁰, 1.79 x 10⁻⁹, and others are provided for constructing the Kₚ expression.
- There's a "RESET" button to clear your inputs and start over as needed.
**Additional Features:**
- Navigation buttons to move between questions.
- A progress bar indicating the current question status (Question 2 out of 3 has been highlighted).
**Instructions for Students:**
1. Analyze the given concentrations for NH₃ and NH₄Cl.
2. Apply the values to the ICE table and utilize the Kₚ formula to determine the unknown.
3. Input your expressions using the provided interactive buttons.
This exercise aids in mastering buffer solutions and equilibrium calculations in a chemistry setting.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F315f2cc5-843f-4088-b4c8-06378b03d38c%2F7e488365-9a68-4cc7-b864-1c31a18d1015%2Ffigh8sr_processed.png&w=3840&q=75)
Transcribed Image Text:**Buffer pH Determination Exercise**
**Question 3 of 16**
**Task:** Determine the pH of a buffer solution containing 0.25 M NH₃ and 0.15 M NH₄Cl. The pKₚ value for NH₃ is given as 4.75.
Using your ICE (Initial, Change, Equilibrium) table and the definition of the base dissociation constant (Kₚ), construct the expression for Kₚ to determine the unknown variable, ensuring not to combine or simplify terms.
**Equation Setup:**
\[ K_ b = \dfrac{[NH₄^+][OH^-]}{[NH₃]} \]
**Interactive Tools:**
- A series of buttons with various values and expressions such as [0], [0.25], [0.15], [4.75], [x], [2x], [2x²], [0.25 + x], [0.25 - x], 1.78 x 10⁻⁵, 5.62 x 10⁻¹⁰, 1.79 x 10⁻⁹, and others are provided for constructing the Kₚ expression.
- There's a "RESET" button to clear your inputs and start over as needed.
**Additional Features:**
- Navigation buttons to move between questions.
- A progress bar indicating the current question status (Question 2 out of 3 has been highlighted).
**Instructions for Students:**
1. Analyze the given concentrations for NH₃ and NH₄Cl.
2. Apply the values to the ICE table and utilize the Kₚ formula to determine the unknown.
3. Input your expressions using the provided interactive buttons.
This exercise aids in mastering buffer solutions and equilibrium calculations in a chemistry setting.
![**Buffer pH Determination**
**Objective:**
Determine the pH of a buffer consisting of 0.25 M NH₃ and 0.15 M NH₄Cl. The pK_b value for NH₃ is 4.75.
**Instructions:**
Based on the provided values, construct an ICE (Initial, Change, Equilibrium) table to determine the unknown.
**ICE Table Setup:**
- **Reaction:**
\[ \text{NH}_3(aq) + \text{H}_2\text{O}(l) \rightleftharpoons \text{OH}^-(aq) + \text{NH}_4^+(aq) \]
- **Initial Concentrations (M):**
\[ \text{NH}_3: \] (input field)
\[ \text{OH}^-: \] (input field)
\[ \text{NH}_4^+: \] (input field)
- **Change in Concentrations (M):**
\[ \text{NH}_3: \] (input field)
\[ \text{OH}^-: \] (input field)
\[ \text{NH}_4^+: \] (input field)
- **Equilibrium Concentrations (M):**
\[ \text{NH}_3: \] (input field)
\[ \text{OH}^-: \] (input field)
\[ \text{NH}_4^+: \] (input field)
**Available Values to Use:**
- 0
- 0.25
- 0.15
- 4.75
- \( +x \)
- \( -x \)
- \( +2x \)
- \(-2x \)
- \( 0.25 + x \)
- \( 0.25 - x \)
- \( 0.15 - x \)
- \( 0.15 + 2x \)
- \( 0.15 - 2x \)
**Reset Option:**
If necessary, click "RESET" to clear inputs and start over.
**Conclusion:**
Use the ICE table to solve for the unknown variable and determine the pH of the buffer system.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F315f2cc5-843f-4088-b4c8-06378b03d38c%2F7e488365-9a68-4cc7-b864-1c31a18d1015%2Fet7cdh4_processed.png&w=3840&q=75)
Transcribed Image Text:**Buffer pH Determination**
**Objective:**
Determine the pH of a buffer consisting of 0.25 M NH₃ and 0.15 M NH₄Cl. The pK_b value for NH₃ is 4.75.
**Instructions:**
Based on the provided values, construct an ICE (Initial, Change, Equilibrium) table to determine the unknown.
**ICE Table Setup:**
- **Reaction:**
\[ \text{NH}_3(aq) + \text{H}_2\text{O}(l) \rightleftharpoons \text{OH}^-(aq) + \text{NH}_4^+(aq) \]
- **Initial Concentrations (M):**
\[ \text{NH}_3: \] (input field)
\[ \text{OH}^-: \] (input field)
\[ \text{NH}_4^+: \] (input field)
- **Change in Concentrations (M):**
\[ \text{NH}_3: \] (input field)
\[ \text{OH}^-: \] (input field)
\[ \text{NH}_4^+: \] (input field)
- **Equilibrium Concentrations (M):**
\[ \text{NH}_3: \] (input field)
\[ \text{OH}^-: \] (input field)
\[ \text{NH}_4^+: \] (input field)
**Available Values to Use:**
- 0
- 0.25
- 0.15
- 4.75
- \( +x \)
- \( -x \)
- \( +2x \)
- \(-2x \)
- \( 0.25 + x \)
- \( 0.25 - x \)
- \( 0.15 - x \)
- \( 0.15 + 2x \)
- \( 0.15 - 2x \)
**Reset Option:**
If necessary, click "RESET" to clear inputs and start over.
**Conclusion:**
Use the ICE table to solve for the unknown variable and determine the pH of the buffer system.
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