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Definitions |
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colligative properties
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properties that depend on the number of solute particles and not on their type
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ion pair
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one or more cations and one or more anions held together by electrostatic forces, reduces number of particles in the solution
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moles solute/kg solvent
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molality
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dipole-dipole
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attractive forces between polar molecules, larger the dipole moment, greater the force
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hypertonic
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higher concentration than osmotic pressure
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semipermeable membrane
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allows the passage of solvent molecules but blocks the passage of solute molecules
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cohesion
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intermolecular attraction between like molecules
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supersaturated solution
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contains more solute than is present in a saturated solution
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separation of solvent molecules, separation of solute molecules, mixing of solute and solvent molecules
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3 steps in solution process
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phase
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homogenous part of the system in contact with other parts of the system but separated from them by a well-defined boundary
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liquid
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definite volume but assume shapes of container ,high density, slightly compressible, slide past one another
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fractional crystallization
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separation of a mixture of substances into pure components on the basis of differing solubilities
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adhesion
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attraction between unlike molecules
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phase diagram
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shows the conditions at which a substance exists as solid, liquid, or gas
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intermolecular forces
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attractive forces between molecules, weaker
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capillary action
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occurs when the surface tension of water causes film of liquid attached to side of container to contract, pulling water up tube
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nonvolatile
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describes a solution that does not have a measurable vapor pressure
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final number of particles in solution/number of units initially dissolved
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equation for vant hoff factor
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solvation
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process in which an ion or molecule is surrounded by solvent molecules arranged in a specific manner
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electrons
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greater number of these increases strength of dispersion forces
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Henry's Law
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the solubility of a gas in a liquid is proportional to the pressure of the gas over the solution
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moles/total moles
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mole fraction
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surface tension
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amount of energy required to stretch/increase surface of liquid by one unit area, higher for liquids with strong intermolecular forces
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volatile
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describes a solution that has a measurable vapor pressure
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isotonic
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equal concentration and osmotic pressure
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ion-dipole forces
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attract an anion or cation and polar molecule, strength depends on size and charge of ion, magnitude of dipole, size of molecule
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gas
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assumes volume and shape of container, low density, very compressible, very free motion
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2
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vant hoff factor for electrolytes which yield two ions
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saturated solution
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contains maximum amount of solute that will dissolve in a given solvent at a specific temperature
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polarizability
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ease with which electron distribution can be distorted, determines likelihood of dipole moment with charge of ion and strength of dipole
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osmotic pressure
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pressure required to stop osmosis
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concave meniscus
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formed when adhesion is stronger than cohesion and pulls upward
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viscosity
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measure of a liquid's resistance to flow, increases if strong intermolecular forces
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dispersion forces
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attractive forces that form because of a temporary dipole induced in atoms or molecules, between everything including nonpolar molecules
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convex meniscus
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formed when cohesion is stronger than adhesion and pulls downward
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moles solute/liters solution
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molarity
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hydrogen bond
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special type of dipole-dipole between hydrogen atom in a polar bond and oxygen, nitrogen, or flourine, VERY strong
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1
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vant hoff factor for nonelectrolytes
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osmosis
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selective passage of solvent molecules through a porous membrane from a dilute solution to a more concentrated one
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hypotonic
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lower concentration than osmotic pressure
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triple point
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only condition under which all three phases can be in equilibrium with one another
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condensation
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transition from gaseous to liquid state caused by drop in average kinetic energy as temperature decreases
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3
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vant hoff factor for electrolytes which yield three ions
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induced dipole
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dipole in atom or nonpolar molecule due to separation of positive and negative charges because of proximity of ion/polar molecule
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unsaturated solution
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contains less solute than it has the capacity to dissolve
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solid
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definite volume and shape,, high density, incompressible, vibrate in fixed position
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mass of solute/mass of solution
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percent by mass
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Raoult's Law
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the partial pressure of a solvent over a solution is given by vp pure solvent times mole fraction of solvent
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cation
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creates a stronger ion-dipole forces because its charge is more concentrated
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concentration
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amount of solute present in a given amount of solution
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miscible
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two liquids are completely soluble in each other in all proportions
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intramolecular forces
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hold atoms together in a molecule, stronger
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