Friggin definitions...
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| Effloresce | To lose water of hydration; the process occurs when the hydrate has a vapor pressure higher than that of water vapor in the air.
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| Solvation | A process that occurs when an ionic solute dissolves; in solution, solvent molecules surround the positive and negative ions
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| Solute | Dissolved particles in a solution
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| Solvent | The dissolving medium in a solution
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| Surfactants | Any substance that interferes with the hydrogen bonding between water molecules and thereby reduces surface tension; soaps and detergents are surfactants.
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| Desiccants | A hygroscopic substance used as a drying agent
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| Colloids | A mixture whose particles are intermediate in size between those of suspension and a solute solution
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| Hygroscopic | A term describing salts and other compounds that remove moisture from the air.\
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| Aqueous | Water that contains dissolved substances
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| Nonelectrolytes | A compound that does not conduct an electric current in aqueous solution or in the molten state
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| Liquids that have strong intermolecular attraction have what kind of surface tension? | High Surface Tension
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| Why does ice float on water? |
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| What is the difference between solvent and solute? |
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| Why do ionic compounds dissolve more easily? | Because of free floating ions.
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| Colligative Properties | A property of solution that depends only upon the number of solute particles, and not upon their identities; boiling-point elevation, freezing-point depression, and vapor-pressure lowering are colligative properties
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| Henry's Law | At a given temperature the solubility of a gas in a liquid is directly proportional to the pressure of the gas above the liquid
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| Boiling Point Elevation | The difference in temperature between the boiling point of a solution and the boiling point of the pure solvent
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| Supersaturated Solution | A solution that contains more solute than it can theoretically hold at a given temperature; excess solute precipitates if a seed crystal is added
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| Molality | The concentration of solute in a solution expressed as the number of moles of solute dissolved in 1 kilogram (100 g) of solvent
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| Saturated Solution | A solution containing the maximum amount of solute for a given amount of solvent at a constant temperature and pressure; an equilibrium exists between undissolved solute and ions in solution
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| Molarity | The concentration of solute in a solution expressed as the number of moles of solute dissolved in 1 liter of solution
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| Miscible | Describes liquids that dissolve in one another in all proportions
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| Electrolytes | A compound that conducts an electric current when it is in an aqueous solution or in the molten state; all ionic compounds are electrolytes, but most covalent compounds are not
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| Homogeneous | A mixture that is uniform in composition; components are evenly distributed and not easily distinguished
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| Heterogeneous | A mixture that is not uniform in composition; components are not evenly distributed and not easily distinguished
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| Suspension | A mixture from which some of the particles settle out slowly upon standing
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| Solution | A homogeneous mixture; consists of solutes dissolved in solvent
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| Brownian Motion | The chaotic movement of colloidal particles, caused by collision with particles of the solvent in which they are dispersed
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| Tyndall Effect | Scattering of light particles in a colloid or suspension, which causes a beam of light to become visible
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| Emulsion | The colloidal dispersion of one liquid in another
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| Deliquescence | Describes a substance that removes sufficient water from the air to form a solution; the solution formed has a lower vapor pressure than that of the water in the air
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| Freezing Point Depression | The difference in temperature between the freezing point of a solution and the freezing point of the pure solvent
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| Concentration | A measurement of the amount of solute that is dissolved in a given quantity of solvent; usually expressed as mol/L
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| 3 Factors That Affect Dissolution |
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| What increases Solubility? |
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| Mole Fraction |
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