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18 Cards in this Set
- Front
- Back
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boiling point elevation
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the temperature at which the vapor pressure of the solution equals the external (atmospheric) pressure
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colligative properties
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properties dependent on the collection of particles and not their unique identity
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freezing point depression
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the temperature at which the solid and liquid phases of a substance coexist (equilibrium)
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heat of solution
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?? **as "heat", according to notes online: the process of energy transfer from one body or system to another as a result of a difference of temperature
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Henry's law
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the concentration of a gas in a solution at any given temperature is directly proportional to the partial pressure of the gas over the solution
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ideal solution
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A solution most suited for something.
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hydration energy
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amount of energy released upon solvation of gas-phase ions in water.
**This can happen when salt is placed in water. The outer ions move away and are covered by the water molecules surrounding them. |
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mass fraction
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mass of component/total mass
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mass percent
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mass of compound divided by the total mass of solution times 100%
[(mass of compound/totalmass) x 100%] |
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molality
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(m) moles of solute/kilograms of solvent; mass-based
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molarity
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(M) moles of solute/liter of solution; volume-based
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mole fraction
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(X) moles of component/total moles of solution
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nonelectrolyte
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a substance that does not produce ions when dissolved in water
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osmosis
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flow of solvent through a semipermeable membrane
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osmotic pressure
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the pressure required to stop osmosis
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Raoult's law
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the vapor pressure of a solution containing a nonvolatile solute is equal to the vapor pressure of the pure solvent times the mole fraction of the solvent.
[ P soln = P solv x X solv ] |
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solvation energy
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the enthalpy released when a solute dissolves in solvent.
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van't Hoff factor
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moles of particles in solution/moles of solute dissolved
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