8.6 Properties of Buffers

• Give an example of a weak acid and its conjugate base in a buffer.

  Acetic acid and acetate ion
• Name a conjugate acid-base pair in which the conjugate acid is ammonium ion.

  Ammonium ion and ammonia
• What are the key properties of buffers in maintaining pH?

  pH resistance and range
• Within what range do buffers maintain a relatively constant pH?

  Specific range
• In a buffer, the weak acid donates a proton to neutralize added bases
• In the Henderson-Hasselbalch equation, `pKa` is the negative logarithm of the acid dissociation constant
• What is a buffer solution designed to resist changes in?

  pH
• Buffers are primarily used to maintain a desired pH in chemical reactions.


  True
• Conjugate acid-base pairs in a buffer keep the pH constant by neutralizing excess acids only.

  False
• What is a buffer solution designed to resist changes in pH from?

  Added acids or bases
• Buffers are crucial for maintaining stable pH in chemical and biological processes.


  True
• Arrange the steps by which buffers maintain pH when acid or base is added:

  1️⃣ Acid is added to the buffer

  2️⃣ Conjugate base accepts a proton

  3️⃣ pH remains stable
• What is the primary benefit of the Henderson-Hasselbalch equation for calculating pH?

  Simple, direct calculation
• Buffers maintain a constant pH regardless of the amount of acid or base added.

  False
• What is the conjugate base of acetic acid?

  Acetate ion
• Order the steps in how a buffer maintains pH when an acid is added:

  1️⃣ The conjugate base accepts a proton

  2️⃣ pH decreases but remains within range

  3️⃣ Equilibrium shifts to neutralize
• A buffer contains a weak acid and its conjugate base, or a weak base and its conjugate acid.

  True
• Match the buffer composition with an example:

  Weak acid + Conjugate base ↔️ Acetic acid + Acetate ion

  Weak base + Conjugate acid ↔️ Ammonia + Ammonium ion
• What does the Henderson-Hasselbalch equation relate?

  pH to concentrations
• Match the pH calculation method with its use case:

  Henderson-Hasselbalch ↔️ Buffer solutions with known concentrations

  Titration Curves ↔️ Determining pH during titration
• A buffer solution can be composed of a weak acid and its conjugate
• In a buffer, conjugate acid-base pairs work together to neutralize added acids or bases
• When a base is added to a buffer, the conjugate acid donates a proton
• Buffers resist changes in pH when small amounts of acid or base are added
• What are conjugate acid-base pairs composed of in a buffer solution?

  Weak acid and conjugate base
• The Henderson-Hasselbalch equation includes the term pKa, which is the negative logarithm of the acid dissociation constant.


  True