Buffer Solutions and Their Properties

This video tutorial covers the concept of buffer solutions, their importance in maintaining pH balance in biological systems, and their properties. It explains the types of buffer solutions, including acidic and basic buffers, and how they function to resist changes in pH. The tutorial also provides methods for calculating the pH of buffer solutions and includes examples and exercises to reinforce understanding.

What is the optimal pH level for blood to function effectively in oxygen transport?

• 6.5

• 5.0

• 7.4

• 10.0

Which of the following best describes a buffer solution?

• A solution that changes pH drastically with small additions of acid or base

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

• A solution that only contains strong acids

• A solution that only contains strong bases

What are the components of an acidic buffer solution?

• Strong acid and strong base

• Strong base and weak acid

• Weak acid and its conjugate base

• Weak base and its conjugate acid

How does an acidic buffer solution respond to the addition of a small amount of acid?

• The solution becomes neutral

• The pH remains relatively stable

• The pH decreases significantly

• The pH increases significantly

What are the components of a basic buffer solution?

• Strong base and weak acid

• Weak acid and its conjugate base

• Strong acid and strong base

• Weak base and its conjugate acid

How does a basic buffer solution respond to the addition of a small amount of base?

• The pH increases significantly

• The pH decreases significantly

• The pH remains relatively stable

• The solution becomes acidic

Which of the following mixtures can form a buffer solution?

• Strong base and weak acid

• Strong acid and strong base

• Weak acid and its conjugate base

• Weak base and strong acid

What is the pH of a buffer solution made by mixing 50 ml of NH3 0.1 M with 100 ml of NH4Cl 0.5 M?

• 6

• 8

• 10

• 7

How much CH3COONa is needed to be added to 100 ml of CH3COOH 0.5 M to achieve a pH of 4?

• 5 ml

• 10 ml

• 15 ml

• 20 ml

What is the mass of (NH4)2SO4 needed to be added to 200 ml of NH3 0.1 M to achieve a pH of 9 + log 2?

• 600 mg

• 500 mg

• 660 mg

• 700 mg