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pH and Buffer Essentials

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pH and Buffer Essentials

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Core concepts of pH and buffers

Created by

Jacquelyn Mae Adolfo
Jacquelyn Mae Adolfo
United States

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pH and Buffer Essentials
 

pH and Buffer EssentialsOnline version

Core concepts of pH and buffers

by Jacquelyn Mae Adolfo
1

What is pH a measure of in a solution?

2

Which statement describes a buffer?

3

Henderson–Hasselbalch equation relates pH to which factors?

4

What happens to buffer capacity if you double the amount of both HA and A- while keeping pH near pKa?

5

Which addition most strongly challenges a buffer?

6

If a buffer has pKa = 7.0 and pH = 7.0, what is the ratio [A-]/[HA]?

7

What is the effect of carbonic acid/bicarbonate buffer in blood?

8

Which buffer component is the conjugate base in an acetic acid buffer?

9

Why does a buffer work best near its pKa?

10

What would be the immediate effect of adding a small amount of HCl to a buffered solution near its pKa?

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pH quantifies [H+]; acidity rises as H+ increases.

Buffers minimize pH changes by neutralizing added H+ or OH-.

The equation links pH to acid/base ratio and its pKa.

More total buffer species offer greater capacity to absorb added acids/bases.

Strong species overwhelm the buffer system, causing large pH shifts.

At pH = pKa, Equal concentrations of conjugate base and acid form a 1:1 ratio.

Blood uses the bicarbonate system to buffer CO2 produced by metabolism.

In an acetate buffer, HA is acetic acid and A- is acetate.

Maximum buffering occurs when the ratio is near 1, near pKa.

Buffer neutralizes some added H+, limiting pH rise, until capacity is exceeded.

 
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