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Buffer Solutions Quiz

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Questions and Answers

What is a buffer solution?

A solution that cannot resist changes in pH

A solution that has a variable pH depending on the temperature

A solution that maintains a constant pH even on dilution or addition of acid/base (correct)

A solution that undergoes significant pH changes upon dilution

How does a buffer solution resist pH change?

By shifting the equilibrium to the left when strong acid is added (correct)

By decreasing the hydrogen ion concentration when strong acid is added

By shifting the equilibrium to the right when strong alkali is added

By increasing the hydrogen ion concentration when strong acid is added

Which chemical equilibrium is responsible for the resistance to pH change in a buffer solution?

Equilibrium between a strong acid and its conjugate base

Equilibrium between a weak base and its conjugate acid

Equilibrium between a weak acid and its conjugate base (correct)

Equilibrium between a strong base and its conjugate acid

In the buffer solution, what happens when strong alkali is added to the mixture?

<p>The hydrogen ion concentration decreases by less than expected</p> Signup and view all the answers

What living system uses the bicarbonate buffering system for pH regulation?

<p>Animals</p> Signup and view all the answers

Study Notes

Buffer Solution

A buffer solution is a mixture that resists changes in pH when an acid or base is added to it.
It consists of a weak acid and its conjugate base, or a weak base and its conjugate acid.

pH Change Resistance

A buffer solution resists pH change because it can absorb excess hydrogen ions (H+) or hydroxide ions (OH-).
This is possible due to the equilibrium between the weak acid and its conjugate base, or the weak base and its conjugate acid.

Chemical Equilibrium

The equilibrium responsible for the resistance to pH change in a buffer solution is the equilibrium between the weak acid (HA) and its conjugate base (A-): HA + H2O ⇌ H3O+ + A-

Strong Alkali Addition

When strong alkali is added to a buffer solution, the hydroxide ions (OH-) react with the hydrogen ions (H+) to form water, reducing the pH change.

Bicarbonate Buffering System

The bicarbonate buffering system is used for pH regulation in the human blood and other living systems.
It consists of carbonic acid (H2CO3) and its conjugate base, bicarbonate (HCO3-), which helps maintain a stable pH.

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Description

Test your knowledge about buffer solutions with this quiz. Learn about their properties, applications, and importance in pH regulation in various systems.