Before (mol) Change (mol) After (mol) A student was titrating a solution of HC,H,O₂ with a Sr(OH), solution. Determine the pH at a particular point in the titration. Do this by constructing a BCA table and determining the pH. The value of Ka for HC₂H₂O₂ is 1.5 x 10. Complete Parts 1-2 before submitting your answer. NEXT > 40.0 mL of a 0.200 M HC₂H₂O₂ solution was titrated with 100.0 mL of 0.100 M Sr(OH)₂ (a strong base). Fill in the ICE table with the appropriate value for each involved species to determine the moles of reactant and product after the reaction of the acid and base. You can ignore the amount of water in the reaction. HC,H,Oz(aq) 1.00 x 10 0 -1.00 x 10 + 0.100 1.20 x 10 0.200 OH(aq) -1.20 x 10¹¹ 2.00 x 10 2.00 x 10⁰ 2 -2.00 x 10* -2.00 x 10² H₂O(l) 8.00 x 10 RESET -8.00 x 10- C.H,Or(aq)
Before (mol) Change (mol) After (mol) A student was titrating a solution of HC,H,O₂ with a Sr(OH), solution. Determine the pH at a particular point in the titration. Do this by constructing a BCA table and determining the pH. The value of Ka for HC₂H₂O₂ is 1.5 x 10. Complete Parts 1-2 before submitting your answer. NEXT > 40.0 mL of a 0.200 M HC₂H₂O₂ solution was titrated with 100.0 mL of 0.100 M Sr(OH)₂ (a strong base). Fill in the ICE table with the appropriate value for each involved species to determine the moles of reactant and product after the reaction of the acid and base. You can ignore the amount of water in the reaction. HC,H,Oz(aq) 1.00 x 10 0 -1.00 x 10 + 0.100 1.20 x 10 0.200 OH(aq) -1.20 x 10¹¹ 2.00 x 10 2.00 x 10⁰ 2 -2.00 x 10* -2.00 x 10² H₂O(l) 8.00 x 10 RESET -8.00 x 10- C.H,Or(aq)
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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Transcribed Image Text:**Titration of HC2H3O2 with Sr(OH)2**
A student was titrating a solution of HC₂H₃O₂ (acetic acid) with an Sr(OH)₂ (strontium hydroxide) solution. The task is to determine the pH at a specific point in the titration using a BCA (Before, Change, After) table to find the moles of reactant and product. The Ka value for HC₂H₃O₂ is given as 1.5 x 10⁻⁵.
**Procedure:**
1. **Initial Setup:**
- **Volume and Concentration:** 40.0 mL of a 0.200 M HC₂H₃O₂ solution is titrated with 100.0 mL of 0.100 M Sr(OH)₂.
- You will fill in the BCA table based on the reaction: HC₂H₃O₂(aq) + OH⁻(aq) → H₂O(l) + C₂H₃O₂⁻(aq).
2. **ICE Table to Calculate Moles:**
- **HC₂H₃O₂ (Acetic Acid):** Initial moles, change in moles during reaction, and moles after the reaction.
- **OH⁻ (Hydroxide Ion):** Initial moles, change, and final moles.
- **C₂H₃O₂⁻ (Acetate Ion):** Formed as a result of the reaction.
- **H₂O:** A product formed, not involved in calculations for changes in concentration.
**Interactive BCA Table:**
- Boxes are provided to input moles for each species before, during, and after the reaction.
- Numerical options include values like 1.00 x 10⁻², -1.00 x 10⁻², 0.100, 0.200 increasing or decreasing by 2.00 x 10⁻² each time.
**Graph/Diagram Explanation (if applicable):**
- The interactive section allows students to adjust initial and change values to see how they affect the moles of reactants and products.
- A 'Reset' button is provided for recalibrating the table inputs.
**Note:** This activity helps students understand the stoichiometry of acid-base reactions
Expert Solution
Step 1: Determine the number of moles of each species remaining by using given data:
Given,
Molarity of HC4H7O2 = 0.200 M
Volume of HC4H7O2 = 40.0 mL
Molarity of Sr(OH)2 = 0.100 M
Volume of Sr(OH)2 = 100.0 mL
Ka of HC4H7O2 = 1.5 x 10-5
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