5.2.2 Buffer solutions

• The purpose of a buffer solution is to resist changes in pH
• Basic buffers maintain a slightly basic pH.


  True
• Basic buffers maintain a slightly basic pH
• Which example is an acidic buffer?

  Acetic acid and acetate ions
• A basic buffer consists of ammonia and ammonium ions
• Which type of buffer contains a weak base and its conjugate acid?

  Basic buffer
• What is a buffer solution composed of?

  Weak acid and conjugate base ||| Weak base and conjugate acid
• Acidic buffers maintain a slightly acidic pH.


  True
• What type of buffer maintains a slightly acidic pH?

  Acidic buffer
• Buffer solutions consist of a weak acid/base and its conjugate.


  True
• What does the mechanism of buffer action explain?

  How buffers resist pH changes
• An acidic buffer has a pH less than 7.


  True
• What two components are necessary for a buffer solution?

  Weak acid/base and conjugate
• Buffer solutions help maintain stable pH values despite small additions of acid or base.


  True
• Basic buffers maintain a slightly basic pH
• What does a weak acid neutralize in a buffer solution?

  OH-
• In an acidic buffer, the conjugate base neutralizes H+
• A basic buffer is composed of a weak base and its conjugate acid
• What three variables are related in the Henderson-Hasselbalch equation?

  pH, pKa, concentrations
• What is the primary function of a buffer solution?

  Resist changes in pH
• Both acidic and basic buffers maintain stable pH values.


  True
• Basic buffers maintain a slightly basic pH
• What does the conjugate acid neutralize in a basic buffer?

  OH-
• There are two main types of buffer solutions: acidic and basic
• Basic buffers maintain a slightly basic pH.


  True
• Match the buffer type with its composition:

  Acidic Buffer ↔️ Weak acid + Conjugate base

  Basic Buffer ↔️ Weak base + Conjugate acid
• The Henderson-Hasselbalch equation is $pH =$$pKa +$$log\left(\frac{[A^ - ]}{[HA]}\right)$


  True
• In the Henderson-Hasselbalch equation, $[HA]$ represents the concentration of the weak acid
• Summarize the key elements of the Henderson-Hasselbalch equation:

  1️⃣ pH is the measure of acidity or alkalinity

  2️⃣ pKa indicates the strength of the weak acid

  3️⃣ $[A^ - ]$ and $[HA]$ are the concentrations of the conjugate base and weak acid
• The Henderson-Hasselbalch equation is written as $pH =$$pKa +$$log\left(\frac{[A^ - ]}{[HA]}\right)$, where $[A^ - ]$ is the concentration of the conjugate base
• In the Henderson-Hasselbalch equation, what does $[HA]$ represent?


  Concentration of the weak acid
• Match the application of buffer solutions with its importance:

  Chemical Reactions ↔️ Ensures desired pH conditions for reactions

  Analytical Chemistry ↔️ Provides stable pH environment for measurements
• Buffer solutions are used in environmental monitoring to maintain consistent pH levels in water samples
• A basic buffer has a pH greater than 7.

  True
• Acidic buffers maintain a slightly acidic pH
• What is the pH range of an acidic buffer?

  < 7
• Buffers neutralize added acid or base to maintain stable pH.


  True
• What two components make up an acidic buffer?

  Weak acid and conjugate base
• Buffers maintain stable pH by neutralizing added acid or base.


  True
• The Henderson-Hasselbalch equation is pH = pKa + log\left(\frac{[conjugate\,base]}{[weak\,acid]}\right)</latex>, where pKa is the negative logarithm of the acid