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What is a buffer solution?
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A buffer solution is a special type of solution that resists changes in pH when small amounts of an acid or a base are added.
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What are the two main components of a buffer solution?
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A buffer solution typically contains a weak acid and its conjugate base, or a weak base and its conjugate acid.
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How does a buffer solution resist changes in pH?
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A buffer resists pH changes by neutralizing added acids (H+) with its base component and added bases (OH-) with its acid component.
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What is the role of the Henderson-Hasselbalch equation in buffer solutions?
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The Henderson-Hasselbalch equation relates the pH of a buffer solution to the concentration of the acid and its conjugate base.
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Why is a buffer solution important in biological systems?
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Biological systems rely on buffer solutions to maintain optimal pH levels for enzyme activity and other biochemical processes.
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What is an example of a commonly used buffer solution in laboratories?
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Phosphate buffer is commonly used in laboratories due to its ability to maintain pH across a moderate range.
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Can the pH of a buffer solution be changed easily?
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The pH of a buffer solution can be changed by altering the ratio of the concentrations of acid and conjugate base.
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What happens when the buffering capacity is exceeded?
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When buffer capacity is exceeded, the solution's pH will rapidly change with the addition of more acid or base.
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What determines the strength of a buffer?
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The strength of a buffer is determined by its concentration and the pKa of the acid component relative to the desired pH range.
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What is buffer capacity?
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Buffer capacity is a measure of a buffer solution's ability to resist pH change when acidic or basic components are added.
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Why are weak acids/bases used in buffer solutions instead of strong acids/bases?
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Weak acids/bases are used in buffers because they only partially ionize, allowing equilibrium between the acid/base and its conjugate, providing a buffering effect.
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Can water act as a buffer?
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No, water cannot act as a buffer because it lacks significant concentrations of a conjugate acid-base pair necessary for buffering action.
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What is a real-life example of a natural buffer?
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An example of a natural buffer is the bicarbonate buffer system in human blood, which maintains blood pH around 7.4.
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How is a buffer solution prepared?
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To prepare a buffer, mix a weak acid with its conjugate base in required proportions, or a weak base with its conjugate acid, and adjust the pH to the desired level.
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How does a buffer work in maintaining the pH of blood?
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In blood, the bicarbonate buffer system maintains pH by converting between bicarbonate and carbonic acid, moderating changes from CO2 levels.
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