## Lab Report #3-2-4: ### Calculation of \( K_a \) or \( K_b \) from pH DataA 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 ValuesBelow 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.

pH of a solution, depends on concentration of hydronium ion. Similarly poh depends on concentration…

Answered: Lab Report #3-2-4: 0.1 M NaC2H3O2…

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

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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