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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![**Problem Statement:**
Calculate the pH when 32.0 mL of 0.150 M KOH is mixed with 20.0 mL of 0.300 M HBrO (Ka = 2.5 × 10⁻⁹).
**Explanation:**
This problem involves the mixing of a strong base (KOH) with a weak acid (HBrO). The given volumes and concentrations allow us to calculate the moles of each reactant.
**Steps for Calculation:**
1. **Calculate the moles of KOH:**
- Volume = 32.0 mL = 0.0320 L
- Concentration = 0.150 M
- Moles of KOH = Volume × Concentration = 0.0320 L × 0.150 mol/L
2. **Calculate the moles of HBrO:**
- Volume = 20.0 mL = 0.0200 L
- Concentration = 0.300 M
- Moles of HBrO = Volume × Concentration = 0.0200 L × 0.300 mol/L
3. **Determine the reaction:**
- KOH + HBrO → KBrO + H₂O
- This is a neutralization reaction where the base (KOH) reacts with the weak acid (HBrO).
4. **Calculate the remaining moles:**
- Compare the moles of KOH and HBrO to find the limiting reactant.
- Calculate the amount of HBrO left after the reaction.
5. **Use the Henderson-Hasselbalch Equation:**
- With the remaining moles, determine the pH using the formula:
- pH = pKa + log([A⁻]/[HA])
- Where pKa = -log(Ka).
The focus will be on understanding the reaction between a strong base and a weak acid, determining the limiting reactant, and using the Henderson-Hasselbalch equation to find the final pH.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Faeef920a-b7fc-42c4-a405-16f92aebf3b1%2F3a8c7826-7757-470f-8c8c-34c4f3ec98c2%2Fde85btdp_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Problem Statement:**
Calculate the pH when 32.0 mL of 0.150 M KOH is mixed with 20.0 mL of 0.300 M HBrO (Ka = 2.5 × 10⁻⁹).
**Explanation:**
This problem involves the mixing of a strong base (KOH) with a weak acid (HBrO). The given volumes and concentrations allow us to calculate the moles of each reactant.
**Steps for Calculation:**
1. **Calculate the moles of KOH:**
- Volume = 32.0 mL = 0.0320 L
- Concentration = 0.150 M
- Moles of KOH = Volume × Concentration = 0.0320 L × 0.150 mol/L
2. **Calculate the moles of HBrO:**
- Volume = 20.0 mL = 0.0200 L
- Concentration = 0.300 M
- Moles of HBrO = Volume × Concentration = 0.0200 L × 0.300 mol/L
3. **Determine the reaction:**
- KOH + HBrO → KBrO + H₂O
- This is a neutralization reaction where the base (KOH) reacts with the weak acid (HBrO).
4. **Calculate the remaining moles:**
- Compare the moles of KOH and HBrO to find the limiting reactant.
- Calculate the amount of HBrO left after the reaction.
5. **Use the Henderson-Hasselbalch Equation:**
- With the remaining moles, determine the pH using the formula:
- pH = pKa + log([A⁻]/[HA])
- Where pKa = -log(Ka).
The focus will be on understanding the reaction between a strong base and a weak acid, determining the limiting reactant, and using the Henderson-Hasselbalch equation to find the final pH.
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