3 4-(N-Morpholino)butanesulfonic acid (MOBS) is a weak acid frequently utilized to prepare buffers for biological samples through combination with a strong base. How many milliliters of 0.626 M KOH should be added to 5.00 g of MOBS (pKa =7.48; formula mass: 223.29 g/mol) to give a pH of 7.40? Show your work!
3 4-(N-Morpholino)butanesulfonic acid (MOBS) is a weak acid frequently utilized to prepare buffers for biological samples through combination with a strong base. How many milliliters of 0.626 M KOH should be added to 5.00 g of MOBS (pKa =7.48; formula mass: 223.29 g/mol) to give a pH of 7.40? Show your work!
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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![**Buffer Preparation with MOBS and KOH**
**Problem Statement:**
4-(N-Morpholino)butanesulfonic acid (MOBS) is a weak acid frequently utilized to prepare buffers for biological samples through combination with a strong base. How many milliliters of 0.626 M KOH should be added to 5.00 g of MOBS (pKa = 7.48; formula mass: 223.29 g/mol) to give a pH of 7.40? Show your work!
**Solution Approach:**
To solve this problem, follow these steps:
1. **Calculate the Moles of MOBS:**
- Use the formula mass of MOBS to convert the given mass to moles:
\[
\text{moles of MOBS} = \frac{\text{mass of MOBS}}{\text{formula mass of MOBS}} = \frac{5.00 \, \text{g}}{223.29 \, \text{g/mol}}
\]
2. **Use the Henderson-Hasselbalch Equation:**
- The equation is:
\[
\text{pH} = \text{pKa} + \log\left(\frac{[\text{A}^-]}{[\text{HA}]}\right)
\]
- Here, \([\text{A}^-]\) is the concentration of the conjugate base (moles of KOH added), and \([\text{HA}]\) is the concentration of the acid (moles of MOBS).
- Rearrange the equation to solve for the ratio \(\frac{[\text{A}^-]}{[\text{HA}]}\).
3. **Determine Moles of KOH Needed:**
- From the rearranged Henderson-Hasselbalch equation, calculate how many moles of KOH are needed.
4. **Convert Moles of KOH to Volume:**
- Use the concentration of the KOH solution to convert moles to volume in milliliters:
\[
\text{Volume of KOH (mL)} = \frac{\text{moles of KOH}}{0.626 \, \text{mol/L}} \times 1000 \, \text{mL/L}
\]
**Conclusion:**
These steps provide a systematic approach to](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Faf8dd5bb-1368-4a10-9929-9294802d0b74%2F5906d678-626f-4c40-ade3-bd3a9cd09e89%2Fnptk7kc_processed.png&w=3840&q=75)
Transcribed Image Text:**Buffer Preparation with MOBS and KOH**
**Problem Statement:**
4-(N-Morpholino)butanesulfonic acid (MOBS) is a weak acid frequently utilized to prepare buffers for biological samples through combination with a strong base. How many milliliters of 0.626 M KOH should be added to 5.00 g of MOBS (pKa = 7.48; formula mass: 223.29 g/mol) to give a pH of 7.40? Show your work!
**Solution Approach:**
To solve this problem, follow these steps:
1. **Calculate the Moles of MOBS:**
- Use the formula mass of MOBS to convert the given mass to moles:
\[
\text{moles of MOBS} = \frac{\text{mass of MOBS}}{\text{formula mass of MOBS}} = \frac{5.00 \, \text{g}}{223.29 \, \text{g/mol}}
\]
2. **Use the Henderson-Hasselbalch Equation:**
- The equation is:
\[
\text{pH} = \text{pKa} + \log\left(\frac{[\text{A}^-]}{[\text{HA}]}\right)
\]
- Here, \([\text{A}^-]\) is the concentration of the conjugate base (moles of KOH added), and \([\text{HA}]\) is the concentration of the acid (moles of MOBS).
- Rearrange the equation to solve for the ratio \(\frac{[\text{A}^-]}{[\text{HA}]}\).
3. **Determine Moles of KOH Needed:**
- From the rearranged Henderson-Hasselbalch equation, calculate how many moles of KOH are needed.
4. **Convert Moles of KOH to Volume:**
- Use the concentration of the KOH solution to convert moles to volume in milliliters:
\[
\text{Volume of KOH (mL)} = \frac{\text{moles of KOH}}{0.626 \, \text{mol/L}} \times 1000 \, \text{mL/L}
\]
**Conclusion:**
These steps provide a systematic approach to
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