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38 Cards in this Set
- Front
- Back
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colligative properties |
properties of a solution that depend only on the number of solute particles per solvent molecule and not on the nature of the solute or solvent ex) molality, mole fraction, weight percent |
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solute |
the minor component in a solution, dissolved in the solvent |
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solvent |
substance that dissolves a solute, resulting in a solution |
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solution |
a homogeneous mixture composed of only one phase |
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molality |
amount of solute (mol) / mass of solvent (kg) |
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mole fraction |
moles of A / moles A + moles B + moles C +.... |
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weight percent |
mass of A / mass of A + mass of B + ... * 100% |
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ppm |
mg solute/ kg solution |
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saturated |
a stable solution in which the maximum amount of solute has been dissolved |
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miscible |
if two liquids can be mixed in any proportion to form a homogeneous mixture ex) two polar compounds (unequal distribution) or two nonpolar compounds ( equal distribution) |
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immiscible |
liquids that do not fully mix in all proportions, they exist in contact with each other as separate layers ex) a polar and nonpolar compound |
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enthalpy of a solution |
= -change in lattice H + change in Hydration H |
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hydration |
when water is the solvent, and is strongly exothermic |
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solvation |
the process of attraction and association of molecules of a solvent with molecules or ions of a solute. As ions dissolve in a solvent they spread out and become surrounded by solvent molecules |
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henry's law |
the concentration of a gas dissolved in a liquid at a given temperature is directly proportional to the partial pressure of the gas above the liquid Sg = Kh Pg Sg= gas solutbility (mol/kg) Kh = henry's law constant Pg= patrial pressure of the gaseous state |
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Raoult's law |
The vapor pressure of the solvent is proportional to the mole fraction of the solvent in solution Psolvent = Xsolvent P*solvent psolvent = vapor pressure xsolvent = mole fraction |
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Ideal Solution |
a solution that obeys Raoult's law |
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Elevation in Boiling point |
= change in Tbp = Kbp * msolute Kbp = molal boing point elevation constant |
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Freezing point depression |
= change in Tfp = Kfp * msolute Kfp = molal freezing point depression constant |
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osmosis |
the movement of solvent molecules through a semipermeable membrane from a region of lower solute concentration to a region of higher solute concentration |
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osmotic pressure |
the pressure exerted by osmosis in a solution system at equilibruim = cRT c = molar concentration (moles per liter) R = gas constant (.082057 L*atm/k) T = absolute temperature (kelvins) |
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van Hofts Factor |
change in Tfp measured = kfp * m * i
or i = change in Tfp measured / change in Tfp calculated |
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tyndall effect |
is light scattering by particles in a colloid or particles in a fine suspension |
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hydrophobic |
colloids with water as the dispersing medium |
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hydrophilic |
only weak attractive forces exist between the water and the surfaces of the colloidal particles |
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emulsions |
a colloidal dispersion of liquid in another |
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surfactants |
a substance that changes the properties of a surface, typically in a colloidal dispersion |
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chemical kinetics |
the study of the rates of chemical reactions |
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catalysts |
substances that accelerate chemical reactions but are not themselves consumed |
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rate equation / rate law |
the resulting relationship between reactant concentrations and reaction rate rate = k[A]^m[B]^n m is the order in A and n is the order in B the overall order is m+n |
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rate constant |
the proportionality constant, k relates rate and concentration at a given temperature |
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order of reaction |
the exponent of it's concentration term in the rate law experssion doubles = 1st order no change = zero order quadruples = 2nd order |
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Integrated Rate equation |
an equation relating the concentration of a reactant to its initial concentration and the elapsed time ln ( [R]t / [R]0 ) = -Kt |
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half life / t1/2 |
the time required for the concentration of a reactant to decrease to one half its initial value t1/2 = 0.693 / k |
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collision theory |
1 ) the reacting molecules must collide with one another 2) the reacting molecules must collide with sufficient energy to initiate the process of breaking and forming bonds 3) the molecules must collide in an orientation that can lead to rearrangement of the atoms and the formation of products |
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transition state |
sufficient energy has been concentrated in the appropriate bonds |
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Activation energy (Ea) |
The minimum amount of energy that must be absorbed by a system to cause it to react |
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Arrhenius equation |
k = Ae ^(-Ea/RT) A= frequency factor T = kelvin temperature R= gas constant (8.314462E-3 kj/k*mol) |
