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Lab Report #3-2-4: 0.1 M NaC2H3O2 solution, using the given pH data, calculate value of (Ka or Kb) O 1.7 x 10-9 O 1.7 x 10-7 O 1.7 x 10-6 O 1.7 x 10-8

Lab Report #3-2-4: 0.1 M NaC2H3O2 solution, using the given pH data, calculate value of (Ka or Kb) O 1.7 x 10-9 O 1.7 x 10-7 O 1.7 x 10-6 O 1.7 x 10-8

Chemistry
Chemistry
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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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## Lab Report #3-2-4: ### Calculation of \( K_a \) or \( K_b \) from pH Data A 0.1 M solution of sodium acetate (NaC\(_2\)H\(_3\)O\(_2\)) is used in this exercise. Using the given pH data, determine the value of the acid dissociation constant (\( K_a \)) or the base dissociation constant (\( K_b \)): - [ ] \( 1.7 \times 10^{-9} \) - [ ] \( 1.7 \times 10^{-7} \) - [ ] \( 1.7 \times 10^{-6} \) - [ ] \( 1.7 \times 10^{-8} \) Instructions: 1. Calculate the concentration of hydronium ions \([H_3O^+]\) using the pH data. 2. Use the relationship between the pH and \([H_3O^+]\) ions to determine whether you need \( K_a \) or \( K_b \). 3. Apply the respective formula to calculate the dissociation constant. ### Steps to Follow: 1. **Determine the pH of the solution.** 2. **Calculate the hydronium ion concentration, \([H_3O^+]\), using the formula:** \[ [H_3O^+] = 10^{-\text{pH}} \] 3. **Use the appropriate formula for \( K_a \) or \( K_b \):** For \( K_a \): \[ K_a = \frac{[H_3O^+][A^-]}{[HA]} \] For \( K_b \): \[ K_b = \frac{[OH^-][B^+]}{[BOH]} \] 4. **Select the correct dissociation constant value based on your calculations.** This exercise will help in understanding the dissociation of weak acids or bases and the relationship between pH, \( K_a \), and \( K_b \).
Transcribed Image Text:## Lab Report #3-2-4: ### Calculation of \( K_a \) or \( K_b \) from pH Data A 0.1 M solution of sodium acetate (NaC\(_2\)H\(_3\)O\(_2\)) is used in this exercise. Using the given pH data, determine the value of the acid dissociation constant (\( K_a \)) or the base dissociation constant (\( K_b \)): - [ ] \( 1.7 \times 10^{-9} \) - [ ] \( 1.7 \times 10^{-7} \) - [ ] \( 1.7 \times 10^{-6} \) - [ ] \( 1.7 \times 10^{-8} \) Instructions: 1. Calculate the concentration of hydronium ions \([H_3O^+]\) using the pH data. 2. Use the relationship between the pH and \([H_3O^+]\) ions to determine whether you need \( K_a \) or \( K_b \). 3. Apply the respective formula to calculate the dissociation constant. ### Steps to Follow: 1. **Determine the pH of the solution.** 2. **Calculate the hydronium ion concentration, \([H_3O^+]\), using the formula:** \[ [H_3O^+] = 10^{-\text{pH}} \] 3. **Use the appropriate formula for \( K_a \) or \( K_b \):** For \( K_a \): \[ K_a = \frac{[H_3O^+][A^-]}{[HA]} \] For \( K_b \): \[ K_b = \frac{[OH^-][B^+]}{[BOH]} \] 4. **Select the correct dissociation constant value based on your calculations.** This exercise will help in understanding the dissociation of weak acids or bases and the relationship between pH, \( K_a \), and \( K_b \).
### Solutions and Their pH Values Below is a table showing the pH values of various solutions: | **Solutions** | **pH values** | |---------------------|---------------| | H₂O (unboiled) | 3.5 | | H₂O (boiled) | 7.0 | | NaCl | 7.0 | | NaC₂H₃O₂ | 9.1 | | NH₄Cl | 4.5 | | NaHCO₃ | 9.5 | | Na₃PO₄ | 11.9 | | Na₂CO₃ | 11.0 | #### Explanation: - **H₂O (unboiled)**: The pH value is 3.5, indicating that unboiled water is slightly acidic. - **H₂O (boiled)**: Boiled water has a neutral pH value of 7.0. - **NaCl (Sodium Chloride)**: The solution of sodium chloride has a neutral pH value of 7.0. - **NaC₂H₃O₂ (Sodium Acetate)**: This solution is basic with a pH value of 9.1. - **NH₄Cl (Ammonium Chloride)**: The pH value of ammonium chloride solution is 4.5, indicating it is acidic. - **NaHCO₃ (Sodium Bicarbonate)**: This solution is basic with a pH of 9.5. - **Na₃PO₄ (Sodium Phosphate)**: The solution is highly basic with a pH of 11.9. - **Na₂CO₃ (Sodium Carbonate)**: Sodium carbonate solution is also basic with a pH value of 11.0. This table helps in understanding the acidity or basicity of common solutions, which is essential for various scientific and educational purposes.
Transcribed Image Text:### Solutions and Their pH Values Below is a table showing the pH values of various solutions: | **Solutions** | **pH values** | |---------------------|---------------| | H₂O (unboiled) | 3.5 | | H₂O (boiled) | 7.0 | | NaCl | 7.0 | | NaC₂H₃O₂ | 9.1 | | NH₄Cl | 4.5 | | NaHCO₃ | 9.5 | | Na₃PO₄ | 11.9 | | Na₂CO₃ | 11.0 | #### Explanation: - **H₂O (unboiled)**: The pH value is 3.5, indicating that unboiled water is slightly acidic. - **H₂O (boiled)**: Boiled water has a neutral pH value of 7.0. - **NaCl (Sodium Chloride)**: The solution of sodium chloride has a neutral pH value of 7.0. - **NaC₂H₃O₂ (Sodium Acetate)**: This solution is basic with a pH value of 9.1. - **NH₄Cl (Ammonium Chloride)**: The pH value of ammonium chloride solution is 4.5, indicating it is acidic. - **NaHCO₃ (Sodium Bicarbonate)**: This solution is basic with a pH of 9.5. - **Na₃PO₄ (Sodium Phosphate)**: The solution is highly basic with a pH of 11.9. - **Na₂CO₃ (Sodium Carbonate)**: Sodium carbonate solution is also basic with a pH value of 11.0. This table helps in understanding the acidity or basicity of common solutions, which is essential for various scientific and educational purposes.
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