CHEM 126 Final
Quiz yourself by thinking what should be in
each of the black spaces below before clicking
on it to display the answer.
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| IMAFs on protein | - secondary: form shape
- tertiary: overall 3D shape
** determines function
- quanternary: arrangement of two or more polypeptide chains in protein
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| IMAFs on DNA | - created by nucleic acids, two chains wrapped around each other in a double helix
- polar exterior: PO4 groups interact with ion dipole & h bonds
- polar interior: N containing bases, interact by dispersion forces
- h bonds: keep chains together
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| colloid | - dispersed (solute-like) substance distributed throughout a dispersing (solvent-like) substances
- particles are larger than simple molecules but too small to settle out
- EX: G-G (all gases)
G-L (foam)
L-L (milk)
S-L (jelly)
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| Osmotic Pressure (concentration effects) | - increases with number of solute particles
- OP = (n solute/ v solution) *RT
* n = moles of solute, R = gas constant, T = temp, V = volume of solution)
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| Freezing Point (concentration effects) | - decreases with increasing solute particles
-∆T f = ∆Kf*M
*m = molality, Kf = freezing point depression constant, ∆Tf = Tf solvent - Tf solution
- ∆T > 0 -> decrease in freezing point
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| Boiling Point (concentration effects) | - increases when solute particles increase
- boiling point elevation: ∆Tb = Kb * m
* Kb = boiling point elevation constant, m = molality, ∆Tb = Tb solution - Tb solvent
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| Vapor Pressure (concentration effects) | - decreases with number of particles of solute (more particles -> lower VP)
-P solvent (∆P) = X solvent * P0 solvent
* X solvent = 1 - X solute
∆P > 0 -> decrease in VP
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| Parts by Mass (or volume) | - Volume of solute (L)/ volume of solution (L)
- composition
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| Mole Fraction | - amount of solute (mol)/ (amount of solute (mol) + amount of solution (mol))
-Vapor-Pressure Determination, Composition
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| Molality | - m
- amount of solute (mol)/ mass of solvent (kg)
- colligative behavior
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| Molarity | - M
- (amount of solute (mol)/volume of solution (L))
- moles of solute that would be dissolved in 1 L of a solution
- stoichiometry equations & analysis
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| Henry's Law | - determines gas solubility at given pressures
- S gas = K h * P gas
* s= solubility (mol/L) Kh = Henry's Law Constant, P = pressure
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| effect of pressure on solubility | - increase pressure -> increase GAS solubility
- increase pressure -> decrease does not affect solid of liquid solubility
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| effect of temp on solubility | - increase temp -> increase solid solubility
- increase temp -> decrease gas solubility
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| supersaturated | - amount dissolved is more than max dissolved possible
- unstable solution & will easily seperate out
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| unsaturated | - amount dissolved is less than max dissolved possible
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| saturated | - max amount of dissolved solid
- crystallization rate = dissolving rate
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| sontaneity | energy contribution - entropy contribution
* help determine if process occurs spontaneously
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| entropy | distribution of energy over larger number of states
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| ∆H equations | ∆H solution = ∆H solute + ∆ H solvation/hydration (always < 0)
∆H solvation = ∆H solvant + ∆H mixing
∆H solute = -∆H lattice (always > 0)
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| Solubility | - S
- max amount that dissolveds in a fixed quantity of a given solvent at a given temp
- excess of solute is present
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| different types of solution | L-S (salt water)
L-L (gasoline)
G-G (natural gas)
G-L (soda)
G-S (H2 + Pd)
S-S (alloys)
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| 2 substances form a solution? | ∆H = exothermic -> unfavorable, will not mix
* breaking strong for weak
∆H = endothermic -> favorable & will mix
* breaking weak for strong
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