### 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.#### Instructions:Based on the given values, fill in the ICE (Initial, Change, Equilibrium) table to determine the concentrations of all reactants and products.#### Reaction:\[ \text{HA(aq)} + \text{H}_2\text{O(l)} \rightleftharpoons \text{H}_3\text{O}^+(\text{aq}) + \text{A}^-(\text{aq}) \]#### ICE Table:| | HA(aq) | + | H₂O(l) | ⇌ | H₃O⁺(aq) | + | A⁻(aq) ||----------------|--------|---|--------|---|-----------|---|----------|| **Initial (M)** | | | | | | | || **Change (M)** | | | | | | | || **Equilibrium (M)**| | | | | | | |#### Values:Select from the following values to fill in the table:- -0.0030- 0.0970- -0.0970- 0.0097- -0.0097- 0.1000- 3.0- -3.0- 0.030- -0.030- 0.0030To reset your values, click the RESET button.**Note:** The values will help in calculating the equilibrium concentrations, which can further be used to find the $ K_a $ of the weak acid. ### Determining the $ K_a $ of a Weak Acid#### Problem Statement:A 0.1000 M solution of a weak acid, HA, is 3.0% dissociated. Determine the value of $ K_a $ for the weak acid.#### Instructions:Based on your ICE table and definition of $ K_a $, set up the expression for $ K_a $ and then evaluate it. Do not combine or simplify terms.#### Expression for $ K_a $:- $ K_a = \dfrac{[H^+][A^-]}{[HA]} $#### Available Values:For constructing the ICE table and calculating $ K_a $, the provided options include:- Concentration values: [0], [0.1000], [3.0], [0.030], [0.0030], [0.0970], [0.0097], [0.48]- Calculated values: [2.5], 0.31, $ 9.3 \times 10^{-4} $, $ 1.1 \times 10^{3} $, 3.2, $ 9.3 \times 10^{-5} $#### Steps:1. **Initial Concentration (I):** $ [HA] = 0.1000 \, \text{M} $2. **Change in Concentration (C):** Based on 3.0% dissociation, calculate concentration changes.3. **Equilibrium Concentration (E):** Calculate the equilibrium concentrations for [HA], [H⁺], and [A⁻] using the initial concentration and the percentage dissociation.4. **Evaluate $ K_a $:** Use the equilibrium concentrations to set up and calculate the expression for $ K_a $.#### Reset Button:Selecting RESET will clear existing selections and calculations, allowing you to start over.

Answered: Image /qna-images/answer/62c95d27-dc8a-4231-a87e-6645006059e7.jpg

A 0.1000 M solution of a weak acid, HA, is 3.0% dissociated. Determine the value of Ka for the weak acid. 1 2 NEXT > Based on the given values, fill in the ICE table to determine concentrations of all reactants and products. НА(ag) H:O(1) H:O*(aq) А (аq) + Initial (M) Change (M) Equilibrium (M) 5 RESET 0.1000 3.0 -3.0 0.030 -0.030 0.0030 -0.0030 0.0970 -0.0970 0.0097 -0.0097

A 0.1000 M solution of a weak acid, HA, is 3.0% dissociated. Determine the value of Ka for the weak acid. 1 2 NEXT > Based on the given values, fill in the ICE table to determine concentrations of all reactants and products. НА(ag) H:O(1) H:O*(aq) А (аq) + Initial (M) Change (M) Equilibrium (M) 5 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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