chemistry test

combination of two or more substances not reacted

heterogeneous mixture

two or more substances mixed not chemically combined (uniform throughout)

homogeneous mixture

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