1. What is Buffer Capacity?

Buffer capacity (β) is a quantitative measure of a solution's resistance to pH change when an acid or base is added. It's defined as the amount of strong acid or base required to change the pH of 1 liter of solution by 1 unit.

2. Buffer Capacity of Water

Pure water has negligible buffer capacity:

Explanation: Water lacks conjugate acid-base pairs that could absorb added H⁺ or OH⁻ ions, making its pH highly sensitive to added acids or bases.

3. Importance of Buffer Capacity

Details: Understanding buffer capacity is crucial in chemistry, biology, and environmental science where pH stability is important.

4. Using the Calculator

Tips: This calculator demonstrates that pure water has no buffer capacity regardless of volume. Enter any positive volume of water to confirm β ≈ 0.

5. Frequently Asked Questions (FAQ)

Q1: Why does water have no buffer capacity?
A: Water lacks conjugate acid-base pairs that could neutralize added acids or bases.

Q2: How can water's buffer capacity be increased?
A: By adding buffer components like weak acids/bases and their salts (e.g., carbonates, phosphates).

Q3: What's the practical significance of water's low β?
A: It explains why pure water's pH changes dramatically with small additions of acid or base.

Q4: Does temperature affect water's buffer capacity?
A: Temperature affects water's self-ionization but not its fundamental lack of buffer capacity.

Q5: How does this compare to biological buffers?
A: Biological systems use buffers like bicarbonate (β ≈ 0.03) or phosphate (β ≈ 0.05) to maintain pH.