Fill in the blanks to show how you would solve for the pH of a 0.10 M aqueous solution of the weak base B. For the table and the equilibrium expression, do not ignore x. 0.10 POH Initial Concentration (M) Change 0.10-x Equilibrium 2x² 0.10 - 2x 4x² B(aq) X (0.10 - x)² + 2x (0.10 - 2x)² H₂O(l) H + 0 4x HB*(aq) x² 0.10- x² + pH 0.10 + x OH(aq)
Fill in the blanks to show how you would solve for the pH of a 0.10 M aqueous solution of the weak base B. For the table and the equilibrium expression, do not ignore x. 0.10 POH Initial Concentration (M) Change 0.10-x Equilibrium 2x² 0.10 - 2x 4x² B(aq) X (0.10 - x)² + 2x (0.10 - 2x)² H₂O(l) H + 0 4x HB*(aq) x² 0.10- x² + pH 0.10 + x OH(aq)
Introductory Chemistry: A Foundation
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Author:Steven S. Zumdahl, Donald J. DeCoste
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Chapter16: Acids And Bases
Section: Chapter Questions
Problem 65AP: . The concepts of acid-base equilibria were developed in this chapter for aqueous solutions (in...
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![### Solving the pH of a 0.10 M Aqueous Solution of a Weak Base B
To determine the pH of a 0.10 M aqueous solution of the weak base B, follow these steps and fill in the blanks in the table and equilibrium expression without ignoring \( x \).
#### Equilibrium Expression
- **B(aq)**: The concentration of the weak base in aqueous solution.
- **H₂O(l)**: Water, the solvent, playing its usual role in dissociation.
- **HB⁺(aq)**: The conjugate acid of the weak base after gaining a proton.
- **OH⁻(aq)**: Hydroxide ion, indicating the basic nature of the solution.
### Table of Concentrations (M)
Below is the general table format to be filled out, showing the relationships between initial concentrations, changes, and equilibrium concentrations.
| | B(aq) | + | H₂O(l) | ⇌ | HB⁺(aq) | + | OH⁻(aq) |
|---------|------------|---|--------|---|---------|---|----------|
| **Initial** | [Blank 1] | | | | [Blank 2] | | [Blank 3] |
| **Change** | [Blank 4] | | | | [Blank 5] | | [Blank 6] |
| **Equilibrium** | [Blank 7] | | | | [Blank 8] | | [Blank 9] |
### Equilibrium Constant Expression
\[ K_b = \frac{[HB^+][OH^-]}{[B]} \]
\[ pH = - \log [ x ] \]
### Explanation of the Blanks
- Fill in the blank values using the principles of chemical equilibrium where initial concentrations decrease or increase by a factor denoted as \( x \).
### Instructions for Filling the Table
1. **Identify initial concentrations:**
- Initial concentration of \( B \): 0.10 M (Blank 1).
- \( H₂O \) is not normally included in the expression as its concentration is large and constant (thus not provided).
- Initial concentrations of \( HB^+ \) and \( OH^- \) are zero before dissociation starts (Blank 2 and Blank 3).
2.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fc8fc0129-1b11-49f3-869a-8ad1c019dc55%2F272d0bf3-7218-4464-81af-9ff6e721aac6%2Fq3uhxq_processed.jpeg&w=3840&q=75)
Transcribed Image Text:### Solving the pH of a 0.10 M Aqueous Solution of a Weak Base B
To determine the pH of a 0.10 M aqueous solution of the weak base B, follow these steps and fill in the blanks in the table and equilibrium expression without ignoring \( x \).
#### Equilibrium Expression
- **B(aq)**: The concentration of the weak base in aqueous solution.
- **H₂O(l)**: Water, the solvent, playing its usual role in dissociation.
- **HB⁺(aq)**: The conjugate acid of the weak base after gaining a proton.
- **OH⁻(aq)**: Hydroxide ion, indicating the basic nature of the solution.
### Table of Concentrations (M)
Below is the general table format to be filled out, showing the relationships between initial concentrations, changes, and equilibrium concentrations.
| | B(aq) | + | H₂O(l) | ⇌ | HB⁺(aq) | + | OH⁻(aq) |
|---------|------------|---|--------|---|---------|---|----------|
| **Initial** | [Blank 1] | | | | [Blank 2] | | [Blank 3] |
| **Change** | [Blank 4] | | | | [Blank 5] | | [Blank 6] |
| **Equilibrium** | [Blank 7] | | | | [Blank 8] | | [Blank 9] |
### Equilibrium Constant Expression
\[ K_b = \frac{[HB^+][OH^-]}{[B]} \]
\[ pH = - \log [ x ] \]
### Explanation of the Blanks
- Fill in the blank values using the principles of chemical equilibrium where initial concentrations decrease or increase by a factor denoted as \( x \).
### Instructions for Filling the Table
1. **Identify initial concentrations:**
- Initial concentration of \( B \): 0.10 M (Blank 1).
- \( H₂O \) is not normally included in the expression as its concentration is large and constant (thus not provided).
- Initial concentrations of \( HB^+ \) and \( OH^- \) are zero before dissociation starts (Blank 2 and Blank 3).
2.
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