Chapter 14 Mixtures and Solutions Flashcards
a type of heterogeneous mixture containing particles that settle out over time and can be separtated from the mixture by filtration
suspension
a heterogeneous mixture of intermedeiate-sized particles (not all the way dissolved)
colloid
the erratic, random movements of colloid particles that results from collisions of particles of the dispersion medium with the dispersed particles
Brownian motion
the sacttering of light by colloidal particles (ex. headlights going through fog)
Tyndall effect
describes a substance that can be dissolved in a given solvent
soluble
two liquids that are soluble in each other in any proportion
miscible
a substance that does not dissolve in a given solvent
insoluble
describes two liquids that can be mixed together but separate shortly after you’re done mixing them
immiscible
a measure of how much solute is dissolved in a specific amount of solvent or solution
concentration
the number of moles of solute dissolved per liter of a solution; also known as molar concentration
molarity (M)
the ratio of the # of moles of solute dissolved in one kilogram of solvent; also known as molal concentration
molality (m)
the ratio of the number of moles of solute or solvent in solution to the total number of moles of solute and solvent
mole fraction
the process of surrounding solute particles wit solvent particles to form a solution; occurs only where and when the solute/solvent particles come in contact with each other
solvation
the overall energy change that occurs during the solution formation process
heat of solution
contains less dissolved solute for a given temperature and pressure than a saturated solution; has further capacity to hold more dissolved solute
unsaturated solution
contains the maximum amount of dissolved solute for a given amount of solvent at a specific temperature and pressure
saturated solution
contains more dissolved solute than a saturated solution at the same temperature
supersaturated solution
states that @ a given temp, the solubility (S) of a gas in a liquid is directly proportional to the pressure (P) of the gas above the liquid; equation–> S1/P1=S2/P2
Henry’s law
a physical property of a solution that depends on the number of particles but not the type/identity of the dissolved solute particles
colligative property
the temperature difference between a solution’s boiling point and a pure solvent’s boiling point
boiling point elevation
the difference in temperature between a solution’s feezing point and the freezing point of its pure solvent
freezing point depression
the equation for molarity
(M)= # moles solute/L of solution
the equation for molality
(m)= # moles solute/1 kg of solvent