Chemistry - Ch 13 Flashcards
Hydration
interactions between solute/solvent when the solvent is water
Solvation
Interactions between solute and solvent molecules
Entropy
degree of randomness in the system (AKA disorder); thermodynamic quantity
Hydrates
salt and water combined in definite proportions, like FeCl3 + 6H2O
Water of hydration
water associated with hydrates
Crystallization
opposite of solution process; solute particle reattaches to solid
Saturated
solution in equilibrium with undissolved solute
Solubility
Amount of solute needed to form a saturated solution in a given quantity of solvent
Unsaturated
if less solute is dissolved than is needed to form a saturated solution
Supersaturated
solutions with a greater amount of solute than needed to form a saturated solution
Miscible
pairs of liquids (ex. acetone & water) that mix in all proportions
Immiscible
Pairs of liquids that do not dissolve in one another
Henry’s Law
relationship between pressure and the solubility of a gas; Sg (solubility of gas in solution) = k (Constant) times Pg (partial pressure of the gas over the solution); K is different for each solute-solvent pair
Mass percentage
(Mass of component in solution divided by total mass of solution) x 100%
Parts per million (ppm)
how concentrations of very dilute solution are expressed
Mole fraction
moles of component divided by total moles of all components
Molality (m)
number of moles of solute divided by kilograms of solvent
Colligative properties (“depending on the collection”)
properties that depend on the collective effect of the number of solute particles
Raoult’s Law
partial pressure is exerted by solvent vapor above a solution (P subscript A) = the product of the mole fraction of the solvent in the solution (X subscript A) times the vapor pressure of the pure solvent (P degree subscript A)
Ideal solution
obeys Raoult’s Law
Molal boiling-point-elevation constant
(Kb) a constant characteristic of a particular solvent that gives the increase in boiling point as a function of solution molality
Molal freezing-point-depression
(Kf) a constant characteristic of a particular solvent that gives the decrease in freezing point as a function of solution molality
Osmosis
Net movement of solvent is always toward the solution with the higher solute concentration
Osmotic pressure
pressure required to prevent osmosis by pure solvent
Isotonic
if 2 solutions of identical osmotic pressure are separate by a semipermeable membrane, no osmosis will occur
Hypotonic
if one solution is of lower osmotic pressure, it is _______ with respect to the more concentrated solution
Hypertonic
the more concentrated solution is ________ with respect to the dilute solution
Crenation
osmosis causing a cell to shrivel
Hemolysis
Osmosis causing a cell to rupture
Active transport
in some cases, substances must be moved across the cell membrane from an area of low concentration to one of high concentration; not spontaneous
Colloidal dispersions (colloids)
mixtures containing particles larger than normal solutes but small enough to remain suspended in the dispersing medium
Tyndall Effect
scattering of light by colloidal particles
Hydrophilic colloid
water-loving
Hydrophobic colloid
Water-fearing
Adsorption
to adhere to a surface
Emulsion
suspension of one liquid in another
Coagulation
process of enlarging colloidal particles
Dialysis
using semipermeable membranes to separate ions from colloidal particles
