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Ka for acetic acid, CH3COOH, is 1.80 x 10-5. K₁ for nitrous acid, HNO₂, is 4.50 × 10-4. K₁ for phenol (a weak acid), C6H5OH, is 1.00 × 10-¹0 What is the formula for the strongest conjugate base?

Ka for acetic acid, CH3COOH, is 1.80 x 10-5. K₁ for nitrous acid, HNO₂, is 4.50 × 10-4. K₁ for phenol (a weak acid), C6H5OH, is 1.00 × 10-¹0 What is the formula for the strongest conjugate base?

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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**Determining the Strongest Conjugate Base** In this exercise, we will analyze the provided acid dissociation constants (\( K_a \)) for different acids and determine the formula for the strongest conjugate base. 1. **Acetic Acid, \( \text{CH}_3\text{COOH} \)** - \(K_a = 1.80 \times 10^{-5} \) 2. **Nitrous Acid, \( \text{HNO}_2 \)** - \(K_a = 4.50 \times 10^{-4} \) 3. **Phenol (a weak acid), \( \text{C}_6\text{H}_5\text{OH} \)** - \(K_a = 1.00 \times 10^{-10} \) **Question: What is the formula for the strongest conjugate base?** To address this question, recall that the strength of the conjugate base is inversely related to the acid dissociation constant of its corresponding acid. A lower \( K_a \) signifies a weaker acid and thus a stronger conjugate base. Given the \( K_a \) values listed: - \( K_a \) for acetic acid: \( 1.80 \times 10^{-5} \) - \( K_a \) for nitrous acid: \( 4.50 \times 10^{-4} \) - \( K_a \) for phenol: \( 1.00 \times 10^{-10} \) Among these, phenol has the lowest \( K_a \) value, indicating that its conjugate base is the strongest. Therefore, the conjugate base of phenol is: **Answer: \( \text{C}_6\text{H}_5\text{O}^- \)**
Transcribed Image Text:**Determining the Strongest Conjugate Base** In this exercise, we will analyze the provided acid dissociation constants (\( K_a \)) for different acids and determine the formula for the strongest conjugate base. 1. **Acetic Acid, \( \text{CH}_3\text{COOH} \)** - \(K_a = 1.80 \times 10^{-5} \) 2. **Nitrous Acid, \( \text{HNO}_2 \)** - \(K_a = 4.50 \times 10^{-4} \) 3. **Phenol (a weak acid), \( \text{C}_6\text{H}_5\text{OH} \)** - \(K_a = 1.00 \times 10^{-10} \) **Question: What is the formula for the strongest conjugate base?** To address this question, recall that the strength of the conjugate base is inversely related to the acid dissociation constant of its corresponding acid. A lower \( K_a \) signifies a weaker acid and thus a stronger conjugate base. Given the \( K_a \) values listed: - \( K_a \) for acetic acid: \( 1.80 \times 10^{-5} \) - \( K_a \) for nitrous acid: \( 4.50 \times 10^{-4} \) - \( K_a \) for phenol: \( 1.00 \times 10^{-10} \) Among these, phenol has the lowest \( K_a \) value, indicating that its conjugate base is the strongest. Therefore, the conjugate base of phenol is: **Answer: \( \text{C}_6\text{H}_5\text{O}^- \)**
**Buffer Systems in Aqueous Solutions** *Which of the following aqueous solutions are good buffer systems?* *(Select all that apply.)* - [ ] 0.17 M nitrous acid + 0.12 M potassium nitrite - [ ] 0.26 M hydrobromic acid + 0.24 M sodium bromide - [ ] 0.25 M ammonium nitrate + 0.36 M ammonia - [ ] 0.15 M potassium hydroxide + 0.25 M potassium chloride - [ ] 0.31 M acetic acid + 0.22 M sodium acetate
Transcribed Image Text:**Buffer Systems in Aqueous Solutions** *Which of the following aqueous solutions are good buffer systems?* *(Select all that apply.)* - [ ] 0.17 M nitrous acid + 0.12 M potassium nitrite - [ ] 0.26 M hydrobromic acid + 0.24 M sodium bromide - [ ] 0.25 M ammonium nitrate + 0.36 M ammonia - [ ] 0.15 M potassium hydroxide + 0.25 M potassium chloride - [ ] 0.31 M acetic acid + 0.22 M sodium acetate
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