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If the Kp of a weak base is 7.3 x 10-6, what is the pH of a 0.28 M solution of this base? pH =

If the Kp of a weak base is 7.3 x 10-6, what is the pH of a 0.28 M solution of this base? pH =

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
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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### Calculation of pH for a Weak Base Solution **Problem Statement:** If the \( K_b \) of a weak base is \( 7.3 \times 10^{-6} \), what is the pH of a 0.28 M solution of this base? **Answer Box:** \( \text{pH} = \) **Instructions for Solving:** 1. **Determine the Concentration of Hydroxide Ions (\(OH^-\))**: - Use the base dissociation constant (\(K_b\)) and the concentration of the base to find \([OH^-]\). 2. **Use the Formula:** \[ K_b = \frac{[OH^-]^2}{[B] - [OH^-]} \] - Since \( [OH^-] \) is usually very small compared to the initial concentration of the base, the formula can be approximated to: \[ K_b \approx \frac{[OH^-]^2}{[B]} \] 3. **Calculate \([OH^-]\):** - Substitute the values: \[ 7.3 \times 10^{-6} \approx \frac{[OH^-]^2}{0.28} \] - Solve for \([OH^-]\): \[ [OH^-]^2 = (7.3 \times 10^{-6}) \times 0.28 \] \[ [OH^-] = \sqrt{(7.3 \times 10^{-6}) \times 0.28} \] 4. **Find \([OH^-]\)**: - Compute the value of \([OH^-]\). 5. **Calculate pOH**: \[ \text{pOH} = -\log [OH^-] \] 6. **Find pH**: - Use the relationship between pH and pOH: \[ \text{pH} = 14 - \text{pOH} \] By following these steps, you can determine the pH of a 0.28 M solution of the weak base. Input the calculated pH value in the provided answer box.
Transcribed Image Text:### Calculation of pH for a Weak Base Solution **Problem Statement:** If the \( K_b \) of a weak base is \( 7.3 \times 10^{-6} \), what is the pH of a 0.28 M solution of this base? **Answer Box:** \( \text{pH} = \) **Instructions for Solving:** 1. **Determine the Concentration of Hydroxide Ions (\(OH^-\))**: - Use the base dissociation constant (\(K_b\)) and the concentration of the base to find \([OH^-]\). 2. **Use the Formula:** \[ K_b = \frac{[OH^-]^2}{[B] - [OH^-]} \] - Since \( [OH^-] \) is usually very small compared to the initial concentration of the base, the formula can be approximated to: \[ K_b \approx \frac{[OH^-]^2}{[B]} \] 3. **Calculate \([OH^-]\):** - Substitute the values: \[ 7.3 \times 10^{-6} \approx \frac{[OH^-]^2}{0.28} \] - Solve for \([OH^-]\): \[ [OH^-]^2 = (7.3 \times 10^{-6}) \times 0.28 \] \[ [OH^-] = \sqrt{(7.3 \times 10^{-6}) \times 0.28} \] 4. **Find \([OH^-]\)**: - Compute the value of \([OH^-]\). 5. **Calculate pOH**: \[ \text{pOH} = -\log [OH^-] \] 6. **Find pH**: - Use the relationship between pH and pOH: \[ \text{pH} = 14 - \text{pOH} \] By following these steps, you can determine the pH of a 0.28 M solution of the weak base. Input the calculated pH value in the provided answer box.
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