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Water
Chapter 3
Water Life began in water 2/3’s of an organisms body Organisms grow or reproduce in a
water-rich environment.
Water Molecule Covalent bonding Oxygen is more electronegative Polar molecule Polarity of water underlies its
chemistry Chemistry of life.
Polar molecule
Polar molecule
Hydrogen bonding
Fig. 3-2
Hydrogenbond
–H
+
H
O
——
——
+ +
+
–
–
–
Properties of water• Cohesion: • Attraction between water
molecules • Responsible for surface tension of
water
Properties of water Adhesion: Attraction of water between other
molecules Capillary action
Properties of water Moderation of water temperature Water is a liquid at moderate
temperatures Specific heat: Amount of heat needed to a raise
1 gram of a substance 10 Celsius Water’s specific heat is
1 calorie/gram/0C (4.18Joules)
Properties of water Evaporative cooling Heat of vaporization: Amount of heat needed to change
1 gram of a substance from a liquid to a gas.
586 Calories (2260 Joules)
Properties of water Ice floats Less dense
Fig. 3-6a
Hydrogenbond
Liquid waterHydrogen bonds break and re-form
IceHydrogen bonds are stable
Properties of water Solvent Water surrounds ionic & polar
molecules Table salt or sugar Aqueous solution Molarity
Fig. 3-7
Cl–
Na
Cl–
+
+
+
+
+
+
++
––
–
–
–
–
––
Na+
–
––
+
Hydrophobic “fear” of water Common in non-polar molecules Non-polar molecules tend to
aggregate in water Hydrophobic exclusion
Hydrophilic “water-loving” Common in polar molecules
Fig. 3-UN2
Hydroniumion (H3O+)
Hydroxideion (OH–)
2H2O
H
H
H
H
H
H
H
H
OOOO
Ionization
Process of spontaneous ion formation H2O H+ + OH-
Dissociation
pH Measurement of the concentration of
hydrogen ion. pH = -log[H+] Acid: Increase concentration of H+ ions or a
lower pH. Base: Decrease in concentration of H+ions or
a higher pH.
Fig. 3-UN5
Bases donate OH–
or accept H+ inaqueous solutions
Acids donate H+ inaqueous solutions
Acidic[H+] > [OH–]
Neutral[H+] = [OH–]
Basic[H+] < [OH–]
14
7
0
pH
Fig. 3-9
Neutral solution
Acidic solution
Basic solution
OH–
OH–
OH–
OH–
OH–OH–
OH–
H+
H+
H+
OH–
H+ H+
H+ H+
OH–
OH–
OH–OH–
H+
OH–
H+
H+
H+
H+
H+
H+
H+
OH–
Neutral [H+] = [OH–]
Incr
easi
ng
ly A
cid
ic [
H+]
> [
OH
–]
Incr
easi
ng
ly B
asic
[H
+]
< [
OH
–]
pH Scale0
1
2
3
4
5
6
7
8
Battery acid
Gastric juice,lemon juice
Vinegar, beer,wine, cola
Tomato juice
Black coffee
Rainwater
Urine
SalivaPure water
Human blood, tears
Seawater
9
10
Milk of magnesia
Household ammonia
Householdbleach
Oven cleaner
11
12
13
14
Buffer Substance helps maintain a
balanced pH Accepts H+ ions when excess Donates when there are too few.
Buffer Blood pH is approximately 7.4. Bicarbonate ion helps maintain
the pH of the blood. Blood acidosis: pH drops 0.2 to 0.4
points on the pH scale Blood alkalosis: pH goes up 0.2 to
0.4 points on the pH scale
Buffer Bicarbonate ion
H2CO3 ⇌ HCO3- + H+
Acid rain Sulfuric acid Nitric acid
Acid rain