Question 3 of 23 Submit A0.1000 M solution of a weak acid, HA, is 3.0% dissociated. Determine the value of Ka for the weak acid. NEXT > Based on the given values, fill in the ICE table to determine concentrations of all reactants and products. HA(aq) H:O(1) H:O (aq) A"(aq) + + Initial (M) Change (M) Equilibrium (M) O RESET 0.1000 3.0 -3.0 0.030 -0.030 0.0030 0.0030 0.0970 -0.0970 0.0097 0.0097
Question 3 of 23 Submit A0.1000 M solution of a weak acid, HA, is 3.0% dissociated. Determine the value of Ka for the weak acid. NEXT > Based on the given values, fill in the ICE table to determine concentrations of all reactants and products. HA(aq) H:O(1) H:O (aq) A"(aq) + + Initial (M) Change (M) Equilibrium (M) O RESET 0.1000 3.0 -3.0 0.030 -0.030 0.0030 0.0030 0.0970 -0.0970 0.0097 0.0097
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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Transcribed Image Text:**ICE Table Problem for Weak Acid Dissociation**
**Question 3 of 23:**
*A 0.1000 M solution of a weak acid, HA, is 3.0% dissociated. Determine the value of Ka for the weak acid.*
**Instructions:**
Based on the given values, fill in the ICE (Initial, Change, Equilibrium) table to determine concentrations of all reactants and products.
**Chemical Equation:**
HA(aq) + H2O(l) ⇌ H3O+(aq) + A-(aq)
**ICE Table:**
| | HA(aq) | + | H2O(l) | ⇌ | H3O+(aq) | + | A-(aq) |
|---------------|--------|---------------|--------|----|----------|---------------|--------|
| Initial (M) | | | | | | | |
| Change (M) | | | | | | | |
| Equilibrium (M)| | | | | | | |
**Option Buttons:**
- -0.0030
- 0.0970
- 0.1000
- 3.0
- -3.0
- 0.030
- -0.030
- 0.0030
**Reset Button:** A reset option is available to start over if needed.
**Note:** Understanding the ICE table and the dissociation percentage is crucial in calculating the acid dissociation constant, \( K_a \), for the weak acid. The table should be used to track changes in molarity throughout the reaction to reach equilibrium.
![**Question 3 of 23**
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 your ICE table and definition of Ka, set up the expression for Ka and then evaluate it. Do not combine or simplify terms.
\( K_a = \)
**Answer Options:**
- [0]
- [0.1000]
- [3.0]
- [0.030]
- [0.0030]
- [0.0970]
- [0.0097]
- [0.48]
- [2.5]
- [0.31]
- [9.3 x 10^-6]
- [1.1 x 10^-6]
- [3.2]
- [9.3 x 10^-5]
**Features:**
- “PREV” and “Submit” buttons available for navigating questions.
- A “RESET” button to clear selections.
- A progress bar indicating question 2 out of 23 is currently active.
Make sure to use the knowledge of equilibrium constants and ICE tables to select the correct values from the given options.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F315f2cc5-843f-4088-b4c8-06378b03d38c%2Fc21b214f-d8b6-44b8-b268-65d4a10a1519%2Fbz4qltj_processed.png&w=3840&q=75)
Transcribed Image Text:**Question 3 of 23**
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 your ICE table and definition of Ka, set up the expression for Ka and then evaluate it. Do not combine or simplify terms.
\( K_a = \)
**Answer Options:**
- [0]
- [0.1000]
- [3.0]
- [0.030]
- [0.0030]
- [0.0970]
- [0.0097]
- [0.48]
- [2.5]
- [0.31]
- [9.3 x 10^-6]
- [1.1 x 10^-6]
- [3.2]
- [9.3 x 10^-5]
**Features:**
- “PREV” and “Submit” buttons available for navigating questions.
- A “RESET” button to clear selections.
- A progress bar indicating question 2 out of 23 is currently active.
Make sure to use the knowledge of equilibrium constants and ICE tables to select the correct values from the given options.
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