16.5
緩衝液の有効性
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Q1: What determines how well a buffer resists pH changes?
Buffer effectiveness depends on the concentration ratio of weak acid to conjugate base (or vice versa) and their absolute concentrations. The ratio should stay between 10:1 and 1:10 for optimal buffering. Higher concentrations of both components allow the buffer to neutralize more added acid or base before significant pH change occurs.
Q2: What is the buffer range and why does it matter?
The buffer range is the pH span where a buffer effectively resists significant pH changes, extending one unit above and below the pKa value. Within this range, the ratio of weak acid to base remains between 10:1 and 1:10. Outside this range, the buffer loses effectiveness because one component becomes too dilute to neutralize added strong acid or base.
Q3: When is a buffer most effective at resisting pH change?
A buffer is most effective when the concentrations of weak acid and conjugate base are equal, making the pH equal to the pKa. This midpoint of the buffer range provides optimal resistance to pH changes. As the ratio deviates from 1:1, buffer effectiveness decreases because one component becomes depleted faster when acid or base is added.
Q4: How does absolute concentration affect buffer capacity?
Buffer capacity increases with higher absolute concentrations of both the weak acid and its conjugate base. A buffer containing 1 molar each of formic acid and formate can neutralize more strong acid or base than one with 0.1 molar each, even if both have the same ratio. Greater concentrations provide more buffering molecules to react with added acid or base.
Q5: What happens to a buffer when one component becomes too dilute?
When one component of the buffer pair drops below about 10 percent of the other, the buffer loses its usefulness. The diluted component cannot effectively neutralize added strong acid or base, causing significant pH changes. At this point, the buffer pair ratio falls outside the effective 10:1 to 1:10 range, compromising buffering action.
Q6: How does blood maintain a stable pH despite metabolic changes?
Blood uses a carbonic acid and bicarbonate buffer system to maintain pH near 7.35. When hydronium ions enter the bloodstream, bicarbonate ions neutralize them by converting H3O+ to H2CO3. When hydroxide ions are added, carbonic acid converts OH− to bicarbonate. This buffer pair effectively resists pH changes, keeping normal blood pH variations below 0.1 units.
Q7: Why should weak acids and bases be chosen based on desired pH?
Weak acids and their salts work best as buffers for pH values below 7, while weak bases and their salts are better for pH values above 7. This is because a buffer is most effective near its pKa, which falls within the desired pH range. Choosing the correct weak acid or base ensures the buffer operates in its optimal range where the ratio of components remains between 10:1 and 1:10.