Consider the titration of 25.0 mL of 0.125 M acetic acid (CH, COOH, pKa = 4.75) with 0.102 M NaOH. CH,CООН(aq)+NaOH(aq) CH, СОО" (аq) + H,О() + Na*(aq) Determine the initial pH of the 0.125 M acetic acid solution before NaOH is added. pH Determine the pH of the solution after 10.0 mL of 0.102 M NAOH is added. pH Determine the volume of 0.102 M NaOH required to reach halfway to the stoichiometric point of the titration.
Consider the titration of 25.0 mL of 0.125 M acetic acid (CH, COOH, pKa = 4.75) with 0.102 M NaOH. CH,CООН(aq)+NaOH(aq) CH, СОО" (аq) + H,О() + Na*(aq) Determine the initial pH of the 0.125 M acetic acid solution before NaOH is added. pH Determine the pH of the solution after 10.0 mL of 0.102 M NAOH is added. pH Determine the volume of 0.102 M NaOH required to reach halfway to the stoichiometric point of the titration.
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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**Determining Volumes and pH in Acid-Base Titration**
---
**Question 1:**
**Volume of NaOH:**
[ _ ] mL
**Task:**
Determine the pH of the solution when enough NaOH has been added to reach halfway to the stoichiometric point.
**pH:**
[ _ ]
---
**Question 2:**
**Task:**
Determine the volume of 0.102 M NaOH that is required to reach the stoichiometric point of the reaction.
**Volume of NaOH:**
[ _ ] mL
---
**Question 3:**
**Task:**
Calculate the pH of the solution when the stoichiometric point of the titration has been reached.
**pH:**
[ _ ]
---
To solve the problems above, consider the following steps:
- **Calculating the pH at the Halfway Point:**
At the halfway point to the stoichiometric point in a titration, the molarity of the weak acid (HA) and its conjugate base (A-) are equal, resulting in a pH equal to the pKa of the acid.
- **Determining Volume for Stoichiometric Point:**
Use the stoichiometric calculations to find the required volume of NaOH to completely neutralize the acid. This involves the molarity and volume of the given NaOH and the amount of substance in the acid solution.
- **pH at Stoichiometric Point:**
At the stoichiometric point, the pH depends on the nature of the remaining solution. For a strong acid-strong base titration, the pH will be neutral (pH = 7), while for other cases, additional calculations considering the resulting ions in the solution may be necessary.
These questions and steps help in understanding the essential concepts of titration, stoichiometry, and equilibrium in acid-base reactions.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F96b52401-77ae-42e3-bef0-cdd66c230602%2Fb89fbe9d-1e4a-4d08-86db-d55ae93741cc%2F3mknpgm_processed.png&w=3840&q=75)
Transcribed Image Text:---
**Determining Volumes and pH in Acid-Base Titration**
---
**Question 1:**
**Volume of NaOH:**
[ _ ] mL
**Task:**
Determine the pH of the solution when enough NaOH has been added to reach halfway to the stoichiometric point.
**pH:**
[ _ ]
---
**Question 2:**
**Task:**
Determine the volume of 0.102 M NaOH that is required to reach the stoichiometric point of the reaction.
**Volume of NaOH:**
[ _ ] mL
---
**Question 3:**
**Task:**
Calculate the pH of the solution when the stoichiometric point of the titration has been reached.
**pH:**
[ _ ]
---
To solve the problems above, consider the following steps:
- **Calculating the pH at the Halfway Point:**
At the halfway point to the stoichiometric point in a titration, the molarity of the weak acid (HA) and its conjugate base (A-) are equal, resulting in a pH equal to the pKa of the acid.
- **Determining Volume for Stoichiometric Point:**
Use the stoichiometric calculations to find the required volume of NaOH to completely neutralize the acid. This involves the molarity and volume of the given NaOH and the amount of substance in the acid solution.
- **pH at Stoichiometric Point:**
At the stoichiometric point, the pH depends on the nature of the remaining solution. For a strong acid-strong base titration, the pH will be neutral (pH = 7), while for other cases, additional calculations considering the resulting ions in the solution may be necessary.
These questions and steps help in understanding the essential concepts of titration, stoichiometry, and equilibrium in acid-base reactions.
![### Titration of Acetic Acid with Sodium Hydroxide
Consider the titration of 25.0 mL of 0.125 M acetic acid (\( CH_3COOH \), \( pK_a = 4.75 \)) with 0.102 M NaOH.
\[ CH_3COOH(aq) + NaOH(aq) \rightarrow CH_3COO^−(aq) + H_2O(l) + Na^+(aq) \]
#### Task 1: Initial pH Calculation
**Determine the initial pH of the 0.125 M acetic acid solution before NaOH is added.**
\[ \text{pH} = \underline{\hspace{10cm}} \]
#### Task 2: pH After Addition of NaOH
**Determine the pH of the solution after 10.0 mL of 0.102 M NaOH is added.**
\[ \text{pH} = \underline{\hspace{10cm}} \]
#### Task 3: Volume Calculation at Halfway Stoichiometric Point
**Determine the volume of 0.102 M NaOH required to reach halfway to the stoichiometric point of the titration.**
\[ \text{Volume} = \underline{\hspace{10cm}} \]
---
### Explanation of Graphs and Diagrams (None in this Case)
**Note:** This page contains instructions for determining and calculating pH values during a titration process of acetic acid with sodium hydroxide, but no graphs or diagrams are provided in the given content.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F96b52401-77ae-42e3-bef0-cdd66c230602%2Fb89fbe9d-1e4a-4d08-86db-d55ae93741cc%2F4e6uk7w_processed.png&w=3840&q=75)
Transcribed Image Text:### Titration of Acetic Acid with Sodium Hydroxide
Consider the titration of 25.0 mL of 0.125 M acetic acid (\( CH_3COOH \), \( pK_a = 4.75 \)) with 0.102 M NaOH.
\[ CH_3COOH(aq) + NaOH(aq) \rightarrow CH_3COO^−(aq) + H_2O(l) + Na^+(aq) \]
#### Task 1: Initial pH Calculation
**Determine the initial pH of the 0.125 M acetic acid solution before NaOH is added.**
\[ \text{pH} = \underline{\hspace{10cm}} \]
#### Task 2: pH After Addition of NaOH
**Determine the pH of the solution after 10.0 mL of 0.102 M NaOH is added.**
\[ \text{pH} = \underline{\hspace{10cm}} \]
#### Task 3: Volume Calculation at Halfway Stoichiometric Point
**Determine the volume of 0.102 M NaOH required to reach halfway to the stoichiometric point of the titration.**
\[ \text{Volume} = \underline{\hspace{10cm}} \]
---
### Explanation of Graphs and Diagrams (None in this Case)
**Note:** This page contains instructions for determining and calculating pH values during a titration process of acetic acid with sodium hydroxide, but no graphs or diagrams are provided in the given content.
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