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Lesson 2
Water and Acid-Base Chemisty
Term | Definition |
---|---|
Important Features of Water | - dipole (O is partial negative, H is partial positive) - tetrahedral arrangement, allows for H bonds -H bonds are weak, "flickering bonds" |
Number of H bonds in Water | -3.4 in liquid -4 in ice |
H-bond donors | N-H, O-H |
H-bond acceptors | O:, N: |
Where are H-bonds used in the body? | Peptide bonds (proteins) and DNA base pairing |
Ionic Interactions | Negative and Positive will attract each other Same charge will repel |
Hydrophobic | multiple hydrophobic molecules will cluster together to stay away from water, this frees water |
van der Waals | happen between any molecule that get close |
Weakest interactions (.4-4 kJ/mol) | hydrophobic, pi-stacking, van der waals |
Intermediate interactions (4-40 kJ/mol) | electrostatic (ionic) and H-bonding |
Strongest interactions (40-400 kJ/mol) | salt bridges (H bonding plus ionic) |
Amphipathic Molecule | has both hydrophobic (nonpolar) and hydrophilic (polar or charged) regions |
How does entropy relate to hydrophobic interactions? | Water forms cages around hydrophobic molecules. Water would rather move freely (randomly = more entropy). Hydrophobic molecules minimize the surface area in contact with water. |
Water equilibrium | H2O <=> H+ and OH- |
Keq of water | [H+][OH-]/[H2O], = 1.8 x 10^-16 at 25 degrees C |
Kw of water | Keq x [H2O], = 1 x 10^-14 |
Concentration of H+ and OH- at neutral pH? | [H+] = [OH-] = 1 x 10^-7 |
Equilibrium Reaction of an H+ donor | HA + H2O <-> A- + H3O+ |
Ka | [H3O+][A-] / [HA] |
When does pKa = pH | at half equivalence, when [A-] = [HA] |
What is the buffering region of a weak acid? | +/- 1 of the pKa |
Henderson Hasselbach Equation | pH = pKa + log[A-]/[HA] |
Pepsin | digestive enzyme in gastric acid, operates at pH 1.5 |
Trypsin | digestive enzyme in small intestine, operates at pH 6.5 |