Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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![### Determining the Ka of a Weak Acid
#### Problem Statement
A 0.1000 M solution of a weak acid, HA, is 3.0% dissociated. Determine the value of Ka for the weak acid.
#### Instruction
Based on the given values, fill in the ICE (Initial, Change, Equilibrium) table to determine concentrations of all reactants and products.
#### Reaction
HA(aq) + H2O(l) ⇌ H3O+(aq) + A−(aq)
#### ICE Table Framework
| | HA(aq) | H2O(l) | H3O+(aq) | A−(aq) |
|-----------------------|-------------------|----------------|----------------|----------------|
| **Initial (M)** | | | | |
| **Change (M)** | | | | |
| **Equilibrium (M)** | | | | |
#### Explanation
- **Initial Concentration (M):** This is the initial molarity of each species before the reaction begins. Initially, [HA] is 0.1000 M, while [H3O+] and [A−] are 0 M as the reaction has not proceeded yet.
- **Change in Concentration (M):** Indicates the change in concentration as the reaction reaches equilibrium. Since HA is 3.0% dissociated, the change is 3% of 0.1000 M for HA, and the same amount will appear as products H3O+ and A−.
- **Equilibrium Concentration (M):** The remaining concentration of each species at equilibrium. This is calculated based on the changes from the initial concentrations.
Fill in this table using these details to find the equilibrium concentrations and then calculate the acid dissociation constant, Ka, using the formula:
\[ \text{Ka} = \frac{[\text{H}_3\text{O}^+][\text{A}^-]}{[\text{HA}]} \]](https://content.bartleby.com/qna-images/question/c276033a-7e95-4c42-bb2e-bc19111e69ab/e9057eb3-1d67-425e-8af3-271f5c1be4f9/azlanyd_processed.png)
Transcribed Image Text:### Determining the Ka of a Weak Acid
#### Problem Statement
A 0.1000 M solution of a weak acid, HA, is 3.0% dissociated. Determine the value of Ka for the weak acid.
#### Instruction
Based on the given values, fill in the ICE (Initial, Change, Equilibrium) table to determine concentrations of all reactants and products.
#### Reaction
HA(aq) + H2O(l) ⇌ H3O+(aq) + A−(aq)
#### ICE Table Framework
| | HA(aq) | H2O(l) | H3O+(aq) | A−(aq) |
|-----------------------|-------------------|----------------|----------------|----------------|
| **Initial (M)** | | | | |
| **Change (M)** | | | | |
| **Equilibrium (M)** | | | | |
#### Explanation
- **Initial Concentration (M):** This is the initial molarity of each species before the reaction begins. Initially, [HA] is 0.1000 M, while [H3O+] and [A−] are 0 M as the reaction has not proceeded yet.
- **Change in Concentration (M):** Indicates the change in concentration as the reaction reaches equilibrium. Since HA is 3.0% dissociated, the change is 3% of 0.1000 M for HA, and the same amount will appear as products H3O+ and A−.
- **Equilibrium Concentration (M):** The remaining concentration of each species at equilibrium. This is calculated based on the changes from the initial concentrations.
Fill in this table using these details to find the equilibrium concentrations and then calculate the acid dissociation constant, Ka, using the formula:
\[ \text{Ka} = \frac{[\text{H}_3\text{O}^+][\text{A}^-]}{[\text{HA}]} \]
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