An analytical chemist is titrating 167.1 mL of a 0.6100M solution of butanoic acid (HC,H,CO₂) with a 0.7300M solution of NaOH. The pk of butanoic acid is 4.82. Calculate the pH of the acid solution after the chemist has added 60.14 mL of the NaOH solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of NaOH solution added. Round your answer to 2 decimal places. PH-
An analytical chemist is titrating 167.1 mL of a 0.6100M solution of butanoic acid (HC,H,CO₂) with a 0.7300M solution of NaOH. The pk of butanoic acid is 4.82. Calculate the pH of the acid solution after the chemist has added 60.14 mL of the NaOH solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of NaOH solution added. Round your answer to 2 decimal places. PH-
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Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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![**Titration of Butanoic Acid with Sodium Hydroxide**
An analytical chemist is titrating 167.1 mL of a 0.6100 M solution of butanoic acid (HC₄H₇CO₂) with a 0.7300 M solution of NaOH. The pKa of butanoic acid is 4.82. Calculate the pH of the acid solution after the chemist has added 60.14 mL of the NaOH solution to it.
**Note for advanced students:** You may assume the final volume equals the initial volume of the solution plus the volume of NaOH solution added.
*Round your answer to 2 decimal places.*
![Input Box with Check and Reset Buttons]
**pH = [_____ X ⟲]**
---
In this task, you're expected to determine the pH of a solution resulting from the titration of butanoic acid with sodium hydroxide. Following these steps:
1. **Determine the moles of butanoic acid (HC₄H₇CO₂) initially present:**
\[
\text{Moles of } HC₄H₇CO₂ = Molarity \times Volume
\]
\[
\text{Moles of HC₄H₇CO₂} = 0.6100\ M \times 0.1671\ L = 0.1019\ \text{moles}
\]
2. **Determine the moles of NaOH added:**
\[
\text{Moles of NaOH} = Molarity \times Volume
\]
\[
\text{Moles of NaOH} = 0.7300\ M \times 0.06014\ L = 0.0439\ \text{moles}
\]
3. **Determine the moles of butanoic acid and butanoate ions after the reaction:**
- Since NaOH is a strong base, it will react completely with the butanoic acid.
- Moles of HC₄H₇CO₂ remaining:
\[
\text{Moles of HC₄H₇CO₂ remaining} = 0.1019\ \text{moles} - 0.0439\ \text{moles} = 0.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F816cc47c-f059-4914-940d-8196a7c7af6b%2F5f3bece9-2713-4175-9c7d-7d13a1f8938f%2Fneiwf9d_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Titration of Butanoic Acid with Sodium Hydroxide**
An analytical chemist is titrating 167.1 mL of a 0.6100 M solution of butanoic acid (HC₄H₇CO₂) with a 0.7300 M solution of NaOH. The pKa of butanoic acid is 4.82. Calculate the pH of the acid solution after the chemist has added 60.14 mL of the NaOH solution to it.
**Note for advanced students:** You may assume the final volume equals the initial volume of the solution plus the volume of NaOH solution added.
*Round your answer to 2 decimal places.*
![Input Box with Check and Reset Buttons]
**pH = [_____ X ⟲]**
---
In this task, you're expected to determine the pH of a solution resulting from the titration of butanoic acid with sodium hydroxide. Following these steps:
1. **Determine the moles of butanoic acid (HC₄H₇CO₂) initially present:**
\[
\text{Moles of } HC₄H₇CO₂ = Molarity \times Volume
\]
\[
\text{Moles of HC₄H₇CO₂} = 0.6100\ M \times 0.1671\ L = 0.1019\ \text{moles}
\]
2. **Determine the moles of NaOH added:**
\[
\text{Moles of NaOH} = Molarity \times Volume
\]
\[
\text{Moles of NaOH} = 0.7300\ M \times 0.06014\ L = 0.0439\ \text{moles}
\]
3. **Determine the moles of butanoic acid and butanoate ions after the reaction:**
- Since NaOH is a strong base, it will react completely with the butanoic acid.
- Moles of HC₄H₇CO₂ remaining:
\[
\text{Moles of HC₄H₇CO₂ remaining} = 0.1019\ \text{moles} - 0.0439\ \text{moles} = 0.
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