Weak Interactions
in Aqueous Systems
Hydrogen
Bonding Gives Water Its Unusual Properties
Water Forms
Hydrogen Bonds with Solutes
Water
Interacts Electrostatically with Charged Solutes
Entropy
Increases as Crystalline Substances Dissolve
Nonpolar
Gases Are Poorly Soluble in Water
Nonpolar
Compounds Force Energetically Unfavorable Changes
in the Structure of Water
van der
Waals Interactions Are Weak Interatomic
Attractions
Weak
Interactions Are Crucial to Macromolecular
Structure and Function
Ionization of
Water, Weak Acids, and Weak Bases
The
Equilibrium Point of Reversible Reactions Is
Expressed by an Equilibrium Constant
The
Ionization of Water Is Expressed by an
Equilibrium Constant
BOX 4-1 The Ion
Product of Water : Two Illustrative Problems
The pH
Scale Designates the H+ and OH-- Concentrations
Weak Acids
and Bases Have Characteristic Dissociation
Constants
Titration
Curves Reveal the pK8 of Weak Acids
Buffering against
pH Changes in Biological Systems
Buffers
Are Mixtures of Weak Acids and Their Conjugate
Bases
A Simple
Expression Relates pH, pK, and Buffer
Concentration
BOX 4-2 Solving
Problems with the Henderson-Hasselbalch Equation
Weak Acids
or Bases Buffer Cells and Tissues against pH
Changes
Phosphate
and Bicarbonate Are Important Biological Buffers
BOX 4-3 Blood,
Lungs, and Buffer: The Bicarbonate Buffer System
Water as a
Reactant
The Fitness of the
Aqueous Environment for Living Organisms
SUMMARY
Further Reading
Problems
