Understanding Buffers and Their Role in pH Regulation

What happens to the pH of a non-buffered solution when a strong acid is added?

• The pH increases significantly.

• The pH decreases significantly.

• The pH remains unchanged.

• The pH fluctuates slightly.

How does a buffered solution respond to the addition of a strong base?

• The pH increases significantly.

• The pH decreases significantly.

• The pH remains relatively stable.

• The pH fluctuates slightly.

What are the two main components of a buffered solution?

• A strong acid and a strong base

• A weak acid and its conjugate base

• A weak base and a strong acid

• A strong base and a weak acid

In a buffered solution, what happens to the hydrogen ions from a strong acid?

• They decrease the pH.

• They remain free in the solution.

• They are neutralized by the conjugate base.

• They increase the pH.

What role does the weak acid play when a strong base is added to a buffered solution?

• It increases the pH.

• It donates a hydrogen ion to form water.

• It remains unchanged.

• It decreases the pH.

Why is it crucial for human blood to maintain a pH around 7.4?

• To prevent dehydration.

• To ensure proper oxygen transport.

• To avoid life-threatening conditions.

• To maintain blood pressure.

What happens when carbon dioxide reacts with water in the bloodstream?

• It forms carbonic acid.

• It forms acetic acid.

• It forms hydrochloric acid.

• It forms sodium hydroxide.

How does the conjugate base in blood help maintain pH?

• By increasing the alkalinity.

• By binding to oxygen.

• By neutralizing excess hydrogen ions.

• By increasing the acidity.

What is the conjugate base of carbonic acid in the blood?

• Sodium chloride

• Sodium bicarbonate

• Sodium hydroxide

• Sodium acetate

What is the primary function of buffers in biological systems?

• To regulate temperature.

• To stabilize pH levels.

• To enhance nutrient absorption.

• To increase metabolic rate.