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calculate the Ka For CH 3 NH 3* If the Kb For CH₂NH₂ 15 4.4*10-4

calculate the Ka For CH 3 NH 3* If the Kb For CH₂NH₂ 15 4.4*10-4

Chemistry
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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**Calculation of Acid Dissociation Constant (Ka) for CH₃NH₃⁺** To calculate the Ka for CH₃NH₃⁺, use the provided Kb value for CH₃NH₂, which is 4.4 x 10⁻⁴. ### Key Concepts: - **Kb (Base Dissociation Constant):** A measure of the strength of a base in solution. - **Ka (Acid Dissociation Constant):** A measure of the strength of an acid in solution. - **Relationship between Ka and Kb:** \[ K_w = Ka \times Kb \] where \( K_w \) is the ion product of water, equal to \( 1.0 \times 10^{-14} \) at 25°C. ### Calculation Steps: 1. **Given:** - Kb for CH₃NH₂ = \( 4.4 \times 10^{-4} \) - \( K_w = 1.0 \times 10^{-14} \) 2. **Formula:** \[ Ka = \frac{K_w}{Kb} \] 3. **Calculate Ka:** \[ Ka = \frac{1.0 \times 10^{-14}}{4.4 \times 10^{-4}} \] 4. **Result:** - Calculate the value using the above formula to determine the Ka for CH₃NH₃⁺. This calculation illustrates how to convert between the base dissociation constant and the acid dissociation constant using the ion product of water.
Transcribed Image Text:**Calculation of Acid Dissociation Constant (Ka) for CH₃NH₃⁺** To calculate the Ka for CH₃NH₃⁺, use the provided Kb value for CH₃NH₂, which is 4.4 x 10⁻⁴. ### Key Concepts: - **Kb (Base Dissociation Constant):** A measure of the strength of a base in solution. - **Ka (Acid Dissociation Constant):** A measure of the strength of an acid in solution. - **Relationship between Ka and Kb:** \[ K_w = Ka \times Kb \] where \( K_w \) is the ion product of water, equal to \( 1.0 \times 10^{-14} \) at 25°C. ### Calculation Steps: 1. **Given:** - Kb for CH₃NH₂ = \( 4.4 \times 10^{-4} \) - \( K_w = 1.0 \times 10^{-14} \) 2. **Formula:** \[ Ka = \frac{K_w}{Kb} \] 3. **Calculate Ka:** \[ Ka = \frac{1.0 \times 10^{-14}}{4.4 \times 10^{-4}} \] 4. **Result:** - Calculate the value using the above formula to determine the Ka for CH₃NH₃⁺. This calculation illustrates how to convert between the base dissociation constant and the acid dissociation constant using the ion product of water.
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