Understanding Buffer Solutions

What is a buffer solution?

• A buffer solution is a solution that changes pH dramatically when acids or bases are added.

• A buffer solution is a solution that maintains a relatively constant pH when small amounts of acid or base are added.

• A buffer solution is a type of solvent used for dissolving solids.

• A buffer solution is a mixture that only contains water and salt.

What are the two main types of buffer solutions?

• Dilute buffer solutions and Concentrated buffer solutions

• Acidic buffer solutions and Basic buffer solutions

• Neutral buffer solutions and Strong buffer solutions

• Organic buffer solutions and Inorganic buffer solutions

Explain the role of a weak acid in a buffer solution.

• A weak acid completely dissociates in water.

• A weak acid helps maintain pH stability in a buffer solution by reacting with added acids or bases.

• A weak acid has no effect on pH changes.

• A weak acid increases the pH of a solution.

What is the Henderson-Hasselbalch equation used for?

• To calculate the volume of gases in reactions.

• To measure the temperature of solutions.

• To determine the concentration of acids only.

• To calculate the pH of buffer solutions.

How does the Henderson-Hasselbalch equation relate pH to pKa?

• The Henderson-Hasselbalch equation states that pH is equal to pKa minus the logarithm of the ratio of the concentrations of the acid to the conjugate base.

• The Henderson-Hasselbalch equation relates pH to pKa by stating that pH is equal to the concentration of the acid divided by the concentration of the conjugate base.

• The Henderson-Hasselbalch equation shows that pH is equal to pKa plus the logarithm of the ratio of the concentrations of the conjugate base to the acid.

• The Henderson-Hasselbalch equation indicates that pH is directly proportional to pKa without any logarithmic relationship.

What is the significance of buffer capacity?

• Buffer capacity indicates the effectiveness of a buffer solution in maintaining pH stability.

• Buffer capacity indicates the color change of a solution.

• Buffer capacity is the amount of solute in a solution.

• Buffer capacity measures the temperature of a solution.

How does buffer capacity change with concentration?

• Buffer capacity decreases with concentration.

• Buffer capacity remains constant regardless of concentration.

• Buffer capacity increases with concentration.

• Buffer capacity is unaffected by the presence of acids or bases.

What factors affect the pH of a buffer solution?

• Presence of carbon dioxide

• Volume of the solution

• Concentration of strong acid only

• Concentration of weak acid and conjugate base, temperature, ionic strength

Describe how to prepare a simple buffer solution.

• Use only distilled water without any additives.

• Mix a weak acid with its conjugate base in a specific ratio, e.g., acetic acid and sodium acetate.

• Combine two strong bases in equal parts.

• Mix a strong acid with water only.

What is the difference between an acidic and a basic buffer?

• An acidic buffer resists pH changes in acidic conditions, while a basic buffer does so in basic conditions.

• Both buffers are identical in function and composition.

• A basic buffer can only resist changes in acidic conditions.

• An acidic buffer is only effective in neutral conditions.