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17 Cards in this Set
- Front
- Back
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Moles
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grams/ MW
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Molarity (M)
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moles/ liters
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Molality (m)
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moles of solute/ kilograms of solvent
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Mole fraction
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moles of solute/ total moles
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Mass %
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(mass of solute/ total mass of solution) * 100
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Parts per million (ppm)
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(mass of solute/ total mass of solution) x 10^6
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Molecular weight
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grams/mole
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When solutions form
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Entropy increases
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A negative heat of solution
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results in stronger intermolecular bonds and lower vapor pressure
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A positive heat of solution
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results in a weaker intermolecular bonds and higher vapor pressure
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Vapor pressure
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Pressure necessary to bring the liquid and gas phases of a compound to equilibrium
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Nonvolatile solute
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A solute with no vapor pressure
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Volatile solute
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A solute with vapor pressure
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Raoult's law for nonvolatile solutes
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If 97% of the solution is solvent, then the vapor pressure will be 97% of the vapor pressure of the pure solvent
P (total) = χaPa χ = partial pressure |
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Raoult's law for volatile solutes
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If 97% of the solution is solvent, then the vapor pressure will be 97% of the vapor pressure of the pure solvent PLUS 3% of the vapor pressure of the pure solute
P (total) = χaPa + χbPb |
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Spectator ions
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Have no effect on equilibrium
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Common ion effect
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Affect the equilibrium
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