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Buffer Solutions Study
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Buffer Solutions Study
📚 Part 1: Buffer Theory and Concepts
1. What is a buffer solution?
A solution that maintains constant temperature
A solution that resists changes in pH when small amounts of acid or alkali are added
A solution that neutralises all acids and bases
A solution with a pH of exactly 7
2. An acidic buffer consists of:
A strong acid and its salt
A weak acid and its conjugate base
A weak base and its conjugate acid
Two different weak acids
3. Which of the following are examples of buffer systems? (Select all that apply)
Ethanoic acid and sodium ethanoate
Hydrochloric acid and sodium chloride
Ammonia and ammonium chloride
Blood bicarbonate system
4. Explain how a buffer solution resists pH changes when a small amount of acid is added:
🧮 Part 2: Henderson-Hasselbalch Calculations
5. The Henderson-Hasselbalch equation is: pH = pKₐ + log([A⁻]/[HA])
Calculate the pH of a buffer solution containing 0.10 M ethanoic acid (CH₃COOH) and 0.15 M sodium ethanoate (CH₃COONa). The pKₐ of ethanoic acid is 4.76.
6. A buffer solution has a pH of 9.25 and contains 0.20 M NH₃ and 0.10 M NH₄Cl. What is the pKₐ of NH₄⁺?
7. What would happen to the pH of the buffer in question 5 if you added a small amount of NaOH? Explain your reasoning:
🌍 Part 3: Real-World Applications
8. Match each buffer system to its biological or industrial application:
Bicarbonate buffer (HCO₃⁻/H₂CO₃)
Phosphate buffer (HPO₄²⁻/H₂PO₄⁻)
Acetate buffer
Food preservation
Blood pH regulation
Intracellular pH control
9. Why is it important that blood pH remains between 7.35-7.45? What could happen if this buffer system fails?
10. Design a simple experiment to demonstrate buffer action. Include the materials needed and expected results:
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