What is a key criterion for making an effective buffer solution?

What is a key criterion for making an effective buffer solution?

• A. Using strong acids and bases
• B. Selecting a weak acid with pKa far from desired pH
• C. Using equal amounts of weak acid and its conjugate base
• D. Mixing varying concentrations of different weak acids

Answer: (C)

An effective buffer solution is characterized by its ability to resist changes in pH upon the addition of small amounts of acid or base. The correct answer highlights the importance of using equal amounts of a weak acid and its conjugate base, which establishes an optimal ratio for maintaining the desired pH. When a weak acid and its conjugate base are present in roughly equal concentrations, the buffer system can effectively neutralize added acids or bases. If an acid is added, the conjugate base can react with it to minimize the change in pH, and similarly, if a base is added, the weak acid can react to counteract the change. This is described by the Henderson-Hasselbalch equation, which shows that the pH of the buffer solution is determined by the ratio of the concentrations of the weak acid and its conjugate base. Using strong acids and bases, as mentioned in another option, would not create an effective buffer because strong acids and bases completely dissociate in solution and cannot provide the gradual pH control that weak acids and bases offer. Selecting a weak acid with a pKa far from the desired pH would result in poor buffering capacity, as the weak acid's ability to neutralize pH shifts is diminished. Lastly,

An effective buffer solution is characterized by its ability to resist changes in pH upon the addition of small amounts of acid or base. The correct answer highlights the importance of using equal amounts of a weak acid and its conjugate base, which establishes an optimal ratio for maintaining the desired pH.

When a weak acid and its conjugate base are present in roughly equal concentrations, the buffer system can effectively neutralize added acids or bases. If an acid is added, the conjugate base can react with it to minimize the change in pH, and similarly, if a base is added, the weak acid can react to counteract the change. This is described by the Henderson-Hasselbalch equation, which shows that the pH of the buffer solution is determined by the ratio of the concentrations of the weak acid and its conjugate base.

Using strong acids and bases, as mentioned in another option, would not create an effective buffer because strong acids and bases completely dissociate in solution and cannot provide the gradual pH control that weak acids and bases offer. Selecting a weak acid with a pKa far from the desired pH would result in poor buffering capacity, as the weak acid's ability to neutralize pH shifts is diminished. Lastly,