1. Acids and Bases--pH

2. Concept 3.3: Acidic and basic conditions affect living organisms
A hydrogen atom in a hydrogen bond between two water molecules can shift from one to the other:
The hydrogen atom leaves its electron behind and is transferred as a proton, or hydrogen ion (H+)
The molecule with the extra proton is now a hydronium ion (H3O+), though it is often represented as H+
The molecule that lost the proton is now a hydroxide ion (OH–)
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3. 2H2O Hydronium ion (H3O+) Hydroxide ion (OH–)
Fig. 3-UN2 H H O O O H O H H H H H
2H2O
Hydronium
ion (H3O+)
Hydroxide
ion (OH–)

4. Water is in a state of dynamic equilibrium in which water molecules dissociate at the same rate at which they are being reformed
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5. Dissociation of water: very rare—but very important
Changes in concentrations of H+ and OH– can drastically affect the chemistry of a cell
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6. Effects of Changes in pH
Concentrations of H+ and OH– are equal in pure water
Adding certain solutes, called acids and bases, modifies the concentrations of H+ and OH–
Biologists use something called the pH scale to describe whether a solution is acidic or basic (the opposite of acidic)
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7. Acids and Bases
An acid is any substance that increases the H+ concentration of a solution (give off H+)
A base is any substance that reduces the H+ concentration of a solution (sucks up H+)
Copyright © 2008 Pearson Education, Inc., publishing as Pearson Benjamin Cummings

8. Acidic [H+] > [OH–] Neutral [H+] = [OH–] 7 Basic [H+] < [OH–] 14
Fig. 3-UN5
Acidic
[H+] > [OH–]
Acids donate H+ in
aqueous solutions
Neutral
[H+] = [OH–] 7
Bases donate OH–
or accept H+ in
aqueous solutions
Basic
[H+] < [OH–] 14

9. For a neutral aqueous solution [H+] is 10–7 = –(–7) = 7
The pH Scale
In water the product of H+ and OH– is constant and can be written as [H+][OH–] = 10–14
The pH of a solution is defined by the negative logarithm of H+ concentration, written as pH = –log [H+]
For a neutral aqueous solution [H+] is 10–7 = –(–7) = 7
10-7 means 1/10,000,000 so very rare
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10. Acidic solutions have pH values less than 7
Basic solutions have pH values greater than 7
Most biological fluids have pH values in the range of 6 to 8
Copyright © 2008 Pearson Education, Inc., publishing as Pearson Benjamin Cummings

11. Figure 3.9 The pH scale and pH values of some aqueous solutions1
Battery acid
Gastric juice,
lemon juice 2 H+ H+ H+ H+
OH– 3
Vinegar, beer,
wine, cola
OH– H+ H+
Increasingly Acidic
[H+] > [OH–] H+ H+ 4
Acidic
solution
Tomato juice
Black coffee 5
Rainwater 6
Urine
OH–
Saliva
OH–
Neutral
[H+] = [OH–] H+ H+
OH– 7
Pure water
OH–
OH– H+
Human blood, tears H+ H+ 8
Seawater
Neutral
solution 9
Figure 3.9 The pH scale and pH values of some aqueous solutions 10
Increasingly Basic
[H+] < [OH–]
Milk of magnesia
OH–
OH– 11
OH– H+
OH–
OH–
Household ammonia
OH– H+
OH– 12
Basic
solution
Household
bleach 13
Oven cleaner 14

12. The internal pH of most living cells must remain close to pH 7
Buffers
The internal pH of most living cells must remain close to pH 7
Buffers are substances that minimize changes in concentrations of H+ and OH– in a solution
Copyright © 2008 Pearson Education, Inc., publishing as Pearson Benjamin Cummings