Validation: questions about buffers and pH Flashcards

1
Q

What is a buffer solution?

A

A buffer solution is a solution that is able to resist pH change when small amounts of acid or base is added.

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2
Q

What are the two main components of a buffer solution?

A

A weak acid and its conjugate base (e.g. CH3COOH and CH3COO-) or a weak base and its conjugate acid (e.g. NH3 and NH4)

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3
Q

How does a buffer solution resist changes in pH when a small amount of acid is added?

A

The conjugate base in the buffer reacts with the added H+ to neutralise it by forming the weak acid. This prevents a significant pH change.

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4
Q

How does a buffer solution resist changes in pH when a small amount of base is added?

A

The weak acid in the buffer reacts with the added OH- to neutralise it by forming water and the conjugate base. This prevents a significant pH change.

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5
Q

Why is a mixture of a strong acid/base and its conjugate pair not a buffer?

A

Because a strong acid/base fully dissociates in water meaning there is no equilibrium to resist pH change

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6
Q

What happens to the pH of a buffer when a strong acid like HCl is added?

A

The conjugate base reacts with H+ ions to neutralise it, preventing a large pH drop

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7
Q

What happens to the pH of a buffer when a strong base like NaOH is added?

A

The weak acid reacts with OH- to neutralise it, preventing a large pH increase

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8
Q

Why do biological systems, like blood, need buffers?

A

Buffers maintain a stable pH so enzymes and proteins can function properly.

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9
Q

What is the main buffer system in human blood?

A

carbonic acid-bicarbonate buffer system (H2CO3 / HCO3)

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10
Q

Why does adding too much strong acid or base overwhelm a buffer system?

A

The buffer components run out, so they can no longer neutralise the added acid or base.

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11
Q

How does the blood buffer system respond when the blood becomes too acidic (talk about the buffer system)?

A

If blood becomes too acidic, bicarbonate reacts with excess H+ ions to form carbonic acid. Carbonic acid then breaks down into CO2 and H2O which is exhaled by the lungs

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12
Q

How does the blood buffer system respond when the blood becomes too basic?

A

If the blood becomes too basic, carbonic acid dissociated to release H+ ions and counteract the increase in pH

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13
Q

Why is the blood buffer system important for enzyme function in the body?

A

Enzymes only function within a narrow pH range. If pH changes too much, enzyme structure and function are disrupted.

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14
Q

What is the primary buffer system that regulates ocean pH?

A

Carbonate buffer system (HCO3 / CO3)

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15
Q

Write the chemical equilibrium equation for the carbonate buffer system in the ocean.

A

CO2 + H2O ⇌ H2CO3
H2CO3 ⇌ HCO3 + H
HCO3 + H ⇌ CO3 + 2H

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16
Q

How does increasing atmospheric CO₂ affect ocean pH?

A

More CO₂ dissolves in seawater, forming carbonic acid, which lowers ocean pH (acidification)

17
Q

What is ocean acidification and why is it a problem?

A

-Ocean acidification occurs when excess CO₂ dissolves in seawater, forming carbonic acid and lowering pH.
-It reduces carbonate levels, making it harder for marine organisms to form shells and skeletons.

18
Q

How does the carbonate buffer system help maintain ocean pH?

A

-When pH drops, carbonate ions (CO3) react with H+ to form bicarbonate, removing excess H⁺.
-When pH rises, bicarbonate (H2CO3) dissociates into carbonate and H+ releasing H⁺ to lower pH.

20
Q

How does temperature affect the buffering capacity of seawater?

A

Higher temperatures reduce the solubility of CO₂ in water, weakening the ocean’s ability to buffer pH changes.