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A 31.7 mL sample of a 0.399 M aqueous acetic acid solution is titrated with a 0.244 M aqueous sodium hydroxide solution. What is the pH after 29.2 mL of base have been added? pH =

A 31.7 mL sample of a 0.399 M aqueous acetic acid solution is titrated with a 0.244 M aqueous sodium hydroxide solution. What is the pH after 29.2 mL of base have been added? 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
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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**Titration of Acetic Acid with Sodium Hydroxide: Calculating pH** In this exercise, we are tasked with determining the pH of a solution during a titration process. Specifically, the scenario provided is as follows: A 31.7 mL sample of a 0.399 M aqueous acetic acid (CH₃COOH) solution is titrated with a 0.244 M aqueous sodium hydroxide (NaOH) solution. Our goal is to find the pH after 29.2 mL of the base has been added. We start by performing the necessary calculations to achieve the pH of the solution at the given point in the titration: 1. **Identify the initial moles of Acetic Acid (\( \text{CH}_3\text{COOH} \))**: - Volume of acetic acid solution: \( 31.7 \) mL \( = 0.0317 \) L - Concentration of acetic acid: \( 0.399 \) M - Moles of acetic acid: \( 0.399 \times 0.0317 \) moles 2. **Identify the moles of Sodium Hydroxide (\( \text{NaOH} \)) added**: - Volume of sodium hydroxide solution: \( 29.2 \) mL \( = 0.0292 \) L - Concentration of sodium hydroxide: \( 0.244 \) M - Moles of sodium hydroxide: \( 0.244 \times 0.0292 \) moles 3. **Determine the moles of acetic acid remaining**: - Calculate the moles of acetic acid that react with the moles of \( \text{NaOH} \) - Since acetic acid reacts with sodium hydroxide in a 1:1 molar ratio, subtract the moles of \( \text{NaOH} \) from the initial moles of acetic acid 4. **Calculate the concentration of acetic acid and acetate ion (\( \text{CH}_3\text{COO}^- \)) in the solution**: - After the titration, the solution will contain unreacted acetic acid and the acetate ion (\( \text{CH}_3\text{COO}^- \
Transcribed Image Text:**Titration of Acetic Acid with Sodium Hydroxide: Calculating pH** In this exercise, we are tasked with determining the pH of a solution during a titration process. Specifically, the scenario provided is as follows: A 31.7 mL sample of a 0.399 M aqueous acetic acid (CH₃COOH) solution is titrated with a 0.244 M aqueous sodium hydroxide (NaOH) solution. Our goal is to find the pH after 29.2 mL of the base has been added. We start by performing the necessary calculations to achieve the pH of the solution at the given point in the titration: 1. **Identify the initial moles of Acetic Acid (\( \text{CH}_3\text{COOH} \))**: - Volume of acetic acid solution: \( 31.7 \) mL \( = 0.0317 \) L - Concentration of acetic acid: \( 0.399 \) M - Moles of acetic acid: \( 0.399 \times 0.0317 \) moles 2. **Identify the moles of Sodium Hydroxide (\( \text{NaOH} \)) added**: - Volume of sodium hydroxide solution: \( 29.2 \) mL \( = 0.0292 \) L - Concentration of sodium hydroxide: \( 0.244 \) M - Moles of sodium hydroxide: \( 0.244 \times 0.0292 \) moles 3. **Determine the moles of acetic acid remaining**: - Calculate the moles of acetic acid that react with the moles of \( \text{NaOH} \) - Since acetic acid reacts with sodium hydroxide in a 1:1 molar ratio, subtract the moles of \( \text{NaOH} \) from the initial moles of acetic acid 4. **Calculate the concentration of acetic acid and acetate ion (\( \text{CH}_3\text{COO}^- \)) in the solution**: - After the titration, the solution will contain unreacted acetic acid and the acetate ion (\( \text{CH}_3\text{COO}^- \
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