combination of two or more substances not reacted
heterogeneous mixture
two or more substances mixed not chemically combined (uniform throughout)
homogeneous mixture
<1nm, no tyndall, no settle, no filter, Homogeneous
solution in terms of particle size, etc
1-1000 nm, yes tyndall, no settle, no filter, heterogeneous
colloids in terms of particle size, etc
1000 nm, yes tyndall, yes settle, yes filter, heterogeneous
suspension in terms of particle size, etc
type of suspension where when setting the solid is at the bottom and the liquid is on top but when its stirred the solid flows like a liquid
thixotrophic mixture
particles in a colloid are changed, the dispersion medium has opposite charges, these attractions and repulsions keep the particles suspended
why dont particles settle out in a colloid
add ions of opposite charge to break attractions
what causes a colloid to settle out
erratic movement of colloid particles due to collisions of particles
brownian motion
scattering of light by particles
tyndall effect
liquid/liquid colloid held together by an emulsifying agent
emulsion
“like dissolves like”
how to determine if a substance will dissolve
a substance that dissolves in solvent
soluble
a substance that does not dissolve in a solvent
insoluble
two liquids soluble in each other in any proportion
miscible
two liquids that can be mixed but separate shortly after
immiscible
amount of solute that will dissolve in a given amount of solvent
solubility
full of solute
saturated solution
not full of solute
unsaturated solution
overfull of solute
supersaturated solution
measure of how much solute is dissolved in a specific amount of solvent or solution
concentration
is dissolved
solute
does the dissolving
solvent
solvent particles attract to solute particle, pull off a solute particle, completely surround that solute particle, continues until solute dissolved or solvent full of solute, only happens at attraction of solvent for solute is stronger than solute particle attractions
describe how a solute dissolves in a solvent
speeds it up, exposes solute to fresh unsaturated solvent continuously
stirring
higher temp speeds it up, more ke=faster solvent=more dissolving
temperature
smaller is faster, more surface area
particle size
increase temp=increase solubility
how does temperature affect solubility for solids?
increase temp=decrease solubility
how does temperature affect solubility for gases
increase pressure=increase solubility
how does pressure affect solubility for gases
a property that depends only upon the number of solute particles not the identity of the solute
define a colligative property
vapor pressure of a solution is less than that of pure solvent, less water with enough KE to escape surface= less vapor pressure
vapor pressure lowering
freezing point of a solution is lower than the freezing point of the pure solvent, solute disrupts the formation of orderly pattern in a solid
freezing point depression
boiling point of a solution is higher than that of a pure solvent, adding solute decreases VP must add more KE to raise VP of liquid to atmospheric pressure
Boiling point elevation
water moves to make concentrations equal side with more particles applies more pressure to the membrane, more particles=more water moves=higher pressure
osmotic pressure