When a 20.9 mL sample of a 0.387 M aqueous hydrofluoric acid solution is titrated with a 0.372 M aqueous barium hydroxide solution, what is the pH at the midpoint in the titration?
When a 20.9 mL sample of a 0.387 M aqueous hydrofluoric acid solution is titrated with a 0.372 M aqueous barium hydroxide solution, what is the pH at the midpoint in 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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**Titration of Hydrofluoric Acid with Barium Hydroxide**
**Problem Statement:**
When a 20.9 mL sample of a 0.387 M aqueous hydrofluoric acid solution is titrated with a 0.372 M aqueous barium hydroxide solution, what is the pH at the midpoint in the titration?
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In a typical educational setting, we'd analyze the relationship between the acid (hydrofluoric acid) and the base (barium hydroxide) and determine the pH at the midpoint of the titration. This involves understanding the concept of titration, the acid-base neutralization reactions, and the chemical equilibrium.
At the midpoint of the titration, half of the hydrofluoric acid has been neutralized by the barium hydroxide. This point is crucial as it allows us to determine the pKa of the weak acid (HF).
**Step-by-Step Process:**
1. **Balanced Equation:**
The balanced chemical equation for the reaction is:
\[ 2 HF + Ba(OH)_2 \rightarrow BaF_2 + 2 H_2O \]
2. **Moles of HF:**
Using the volume and molarity, calculate the moles of HF:
\[ \text{Moles of HF} = 20.9 \text{ mL} \times \frac{1 \text{ L}}{1000 \text{ mL}} \times 0.387 \text{ M} = 0.00809 \text{ moles} \]
3. **Moles of Ba(OH)_2:**
The concentration of Ba(OH)_2 is 0.372 M and is to be found at the midpoint of the titration.
4. **Midpoint Calculation:**
At the midpoint, the amount of Ba(OH)_2 added is equal to half the moles of HF:
\[ \text{Moles of Ba(OH)_2} = \frac{0.00809 \text{ moles}}{2} = 0.004045 \text{ moles} \]
5. **pH Calculation:**
At the midpoint, the pH is closely related to the pKa of the weak acid (HF). HF has a known pKa value of approximately 3.17. Using the given information and the relationship between the midpoint](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F6ab0bbaf-7c6a-41d9-a28d-d2a0ce6f8c93%2Ffbe6ed89-fc0d-49f9-b411-87319efecb3e%2F9zfvhvi_processed.png&w=3840&q=75)
Transcribed Image Text:---
**Titration of Hydrofluoric Acid with Barium Hydroxide**
**Problem Statement:**
When a 20.9 mL sample of a 0.387 M aqueous hydrofluoric acid solution is titrated with a 0.372 M aqueous barium hydroxide solution, what is the pH at the midpoint in the titration?
---
In a typical educational setting, we'd analyze the relationship between the acid (hydrofluoric acid) and the base (barium hydroxide) and determine the pH at the midpoint of the titration. This involves understanding the concept of titration, the acid-base neutralization reactions, and the chemical equilibrium.
At the midpoint of the titration, half of the hydrofluoric acid has been neutralized by the barium hydroxide. This point is crucial as it allows us to determine the pKa of the weak acid (HF).
**Step-by-Step Process:**
1. **Balanced Equation:**
The balanced chemical equation for the reaction is:
\[ 2 HF + Ba(OH)_2 \rightarrow BaF_2 + 2 H_2O \]
2. **Moles of HF:**
Using the volume and molarity, calculate the moles of HF:
\[ \text{Moles of HF} = 20.9 \text{ mL} \times \frac{1 \text{ L}}{1000 \text{ mL}} \times 0.387 \text{ M} = 0.00809 \text{ moles} \]
3. **Moles of Ba(OH)_2:**
The concentration of Ba(OH)_2 is 0.372 M and is to be found at the midpoint of the titration.
4. **Midpoint Calculation:**
At the midpoint, the amount of Ba(OH)_2 added is equal to half the moles of HF:
\[ \text{Moles of Ba(OH)_2} = \frac{0.00809 \text{ moles}}{2} = 0.004045 \text{ moles} \]
5. **pH Calculation:**
At the midpoint, the pH is closely related to the pKa of the weak acid (HF). HF has a known pKa value of approximately 3.17. Using the given information and the relationship between the midpoint
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