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28 Cards in this Set
- Front
- Back
- 3rd side (hint)
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Solution |
Homogenous mix of solvent and one or more solute. |
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Unsaturated Solution |
Solution that contains less solute than the solvent. Has the capacity to dissolve at a specific temperature. |
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Saturated Solution |
One that contains the max amount of solute that will dissolve in solvent at a specific temperature. |
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Super Saturated Solution |
Contain more dissolved solute than is present in a saturated Solution and are generally unstable. |
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Solvation |
Occurs when solute molecules are separated from one another and surrounded by solvent molecules. |
Depends on 3 type of reactions. 1.) Solute-solute interactions 2.) Solvent-Solvent interactions 3.) Solute-solvent interactions |
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Ion-Dipole |
The charge of an ion is attracted to the partial charge on a polar molecule. (NaCl or Ki in water) |
Intermolecular interaction |
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Dipole-Induced Dipole |
The partial charge on a polar molecule induces a temporary partial charge on a neighboring Nonpolar molecule or atom. (He or CO2 in water) |
Intermolecular Force |
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Ion-Induced Dipole |
The charge of an ion induces a temporary partial charge on a neighboring Nonpolar molecule or atom. (Fe II and O2.) |
Intermolecular Force |
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Entropy |
A measure of how the dispersed or spread out its energy is. |
There is a natural tendency for the energy of the system to become dispersed. |
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Miscible |
When 2 liquids are completely soluble in each other in all proportions. |
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Molarity |
The amount of solute relative to the volume of a solution or to the amount of solvent in a solution. (called concentration). |
Molarity= Moles of solute/Liters of solution. |
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Mole Fraction |
Moles of A/Sum of moles of all components. |
Concentration unit. |
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Molality |
Moles of Solute/Kg of solvent |
Concentration Unit |
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Percent by Mass |
Independent of temperature. |
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Solubility |
Temperature affects solubility of most substances. |
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Henry's Law |
States that the solubility of a gas in a liquid is proportional to the pressure of the gas over the solution. |
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Colligative Properties |
Properties that depend on the number of solute particles in solution. Do not depend on the nature of the solute particles. |
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Raoults Law |
states that the partial pressure of a solvent over solution is given by the vapor pressure of the pure solvent X the mole fraction of the solvent in the solution. |
Ideal solutions obey Raoults Law |
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Volatile |
The vapor pressure of the solution is the sum of the individual partial pressures. |
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Boiling Point Elevation |
Solution boils At a higher temperature than the pure solvent. |
Colligative Property |
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Freezing Point Depression |
Solution freezes at a lower temperature than the pure solvent. |
Colligative Property |
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Osmosis |
Selective passage of solvent molecules through a porous membrane from a more dilute solution to a more concentrated one. |
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Osmotic Pressure |
The pressure required to stop osmosis. |
P=MRT |
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Van's Hoff Factor (i) |
Ion particles dissolved in a solution. 1 is for nonelectrolytes. 2 is for strong electrolytes 3 is for strong electrolytes. |
Usually smaller than predicted due to formation of ion pairs. |
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Ion pair |
made up of one or more cations and one or more anions held together by electrostatic forces. |
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Percent Dissasociation |
The percentage of dissolved molecules that separate into ions in a solution and this can be found using colligative properties. |
Strong Electrolytes should have complete 100% dissociation. But experimentally determined is not the case. More complete at lower concentration. |
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Colloid |
A Dispersion of particles of one substance throughout another substance. Colloid particles are much larger than the normal solute molecules. |
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Emulsification |
The process of stabilizing a colloid that would otherwise not stay dispersed. |
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