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Chapter 2 Chemistry, Matter, and Life 33<br />
proton acceptors (hydroxide ions), and the pH is 7. Pure water<br />
is a neutral solution with a pH of 7. Solutions that are acidic<br />
have a pH of less than 7, and the lower is the pH, the stronger<br />
is the acid. Basic or alkaline solutions have a pH greater than<br />
7, and the higher the pH, the stronger it is. Because the scale<br />
is logarithmic, each unit on the pH scale represents a 10-fold<br />
difference in the hydrogen ion concentration. For example, a<br />
solution with a pH of 6 has 10 times the hydrogen ion concentration<br />
as a solution with a pH of 7, and a solution with a pH of<br />
5 has 10 times more than a solution with a pH of 6. A solution<br />
with a pH of 5 has 100 times the hydrogen ion concentration of<br />
a pH 7 solution. Figure 2-14 compares the pH values for some<br />
familiar acids and bases.<br />
Quick Applications<br />
The pH of human milk ranges from 7.0 to 7.4. The<br />
initial breast secretion, colostrum, has a pH of 7.45.<br />
This drops to a low of 7.0 for milk during the second<br />
week of lactation. The pH remains near this level for<br />
about 3 months, then increases gradually to 7.4 at<br />
about 10 months.<br />
In this way the hydrogen ions from the strong acid are incorporated<br />
into the weak acid and will have less effect on the pH.<br />
If a base such as NaOH is added to the buffer system, it will be<br />
neutralized by the acid to form water and a salt:<br />
NaOH + H 2<br />
CO 3<br />
→ NaHCO 3<br />
+ H 2<br />
O<br />
Base Buffer acid Buffer salt Water<br />
When either an acid or a base is added to a buffered solution,<br />
something neutral (water or salt) and a component of the buffer<br />
(weak acid or its salt) are formed. The pH does not change.<br />
Buffers are very important physiologically. Even a slight deviation<br />
from the normal pH range can cause pronounced changes<br />
in the rate of cellular chemical reactions and thus threaten survival.<br />
Buffers provide one of the homeostatic control mechanisms<br />
that maintain normal pH.<br />
Quick Applications<br />
In the human body, acid-base balance is regulated by<br />
chemical buffer systems, the lungs, and the kidneys.<br />
Neutralization Reactions<br />
Neutralization is the reaction between an acid and a<br />
base. The hydrogen ion (H + ) from the acid reacts with the<br />
hydroxide ion (OH − ) from the base to form water. The acid<br />
removes or neutralizes the effect of the base and vice versa.<br />
The other product is called a salt. Salts are ionic compounds<br />
produced from neutralization reactions and consist of cations<br />
other than H + and anions other than OH − . They are<br />
formed from the positive ion of the base and the negative<br />
ion of the acid:<br />
HCl + NaOH → NaCl + H 2<br />
O<br />
Acid Base Salt Water<br />
Neutralization reactions help maintain the proper pH of the<br />
blood. They also have many practical applications. One such<br />
application involves antacid medications. Antacids are basic<br />
and are often used to neutralize excess acid in the stomach.<br />
Buffers<br />
If you add a few drops of a strong acid to some distilled water<br />
(pH = 7), the pH of the solution will decrease because hydrogen<br />
ions have been added. If a few drops of acid are placed in a<br />
buffer solution, the pH will change only slightly. A buffer is a<br />
solution that resists change in pH when either an acid or a base<br />
is added.<br />
A buffer solution contains a weak acid and a salt of that same<br />
acid, the salt functions as a weak base. One of the most common<br />
buffering systems and one that is important in human<br />
physiology involves carbonic acid (H 2<br />
CO 3<br />
) and its salt, sodium<br />
bicarbonate (NaHCO 3<br />
). When hydrogen ions from a strong<br />
acid are added, they react with the salt to form a weaker acid<br />
and a neutral salt:<br />
HCl + NaHCO 3<br />
→ H 2<br />
CO 3<br />
+ NaCl<br />
Strong acid Buffer salt Weak acid Neutral salt<br />
Quick Check<br />
2.12 Black coffee is an acid. Is its pH greater or less than 7.0?<br />
2.13 Many of the foods we eat are acids, yet the pH of body<br />
fluids remains relatively constant. Why?<br />
Organic Compounds<br />
The term organic chemistry is inherited from the day when the<br />
science of chemistry was comparatively primitive. Compounds<br />
formed by living processes were termed organic. In the nineteenth<br />
century, it was discovered that organic compounds can<br />
be created artificially in the laboratory from substances that do<br />
not arise from life processes. Since then, the field of organic<br />
chemistry has grown until today more than 1 million different<br />
organic compounds have been identified.<br />
Organic compounds are important because they are associated<br />
with all living matter in both plants and animals. Nearly all<br />
compounds related to living substances contain carbon; thus,<br />
organic compounds are carbon compounds. Carbohydrates,<br />
fats, proteins, hormones, vitamins, enzymes, and many drugs<br />
are organic compounds. Wool, silk, linen, cotton, nylon, and<br />
rayon all contain organic compounds. Add to this the perfumes,<br />
dyes, flavorings, soaps, gasoline, and oils and you see<br />
that the study of organic compounds is extensive.<br />
The most important groups of organic compounds in the<br />
body are the carbohydrates, proteins, lipids, nucleic acids, and<br />
adenosine triphosphate.<br />
Carbohydrates<br />
Carbohydrate (kar-boh-HYE-drayt) molecules are composed<br />
of carbon, hydrogen, and oxygen. They are the product of photosynthesis,<br />
a process by which plants convert solar energy into<br />
chemical energy. Carbohydrate molecules range in size from<br />
small to very large. They are an important energy source in the