Chapter 11 Key Terms

alloy

solid mixture of a metallic element and one or more other components

ampiphilic

molecules possessing both hydrophobic (nonpolar) parts and hydrophilic (polar) parts

boiling point elevation

elevation of the boiling point of a liquid by addition of a solute

boiling point elevation constant

the proportionality constant in the equation relating boiling point elevation to solute molality

colligative property

property of a solution that depends only on the concentration of a solute speciescol

colloid

mixture in which relatively large solid or liquid particles are dispersed uniformly throughout a gas, liquid, or solidcr

enation

process by which biological cells become shriveled due to loss of water by osmosis

dispersed phase

substance present as relatively large solid or liquid particles in a colloid

dispersion medium

solid, liquid, or gas in which colloidal particles are disposed

dissociation

physical process accompanying the dissolution of an ionic compound in which the compounds constituents ions are solvated and dispersed throughout the solution

electrolyte

substance that produces ions when dissolved in waterem

emulsifying agent

amphiphilic substance used to stabilize the particles of some emulsions

freezing point depression

lower of the freezing point of a liquid by addition of a solute

freezing point depression constant

proportionality constant in the equation relating freezing point depression to some molality

gel

colloidal dispersion of a liquid in a solid

hemolysis

rupture of red blood cells due to accumulation of excess water by osmosis

Henry’s Law

the proportional relationship between the concentration of dissolved gas in a solution and the partial pressure of the gas in contact with the solutionH

hypertonic

of greater osmotic pressure

hypotonic

of lesser osmotic pressurei

isotonic

of equal osmotic pressure

ideal solution

solution that forms with no accompanying energy change

immiscible

of negligible mutual solubility

ion pair

solvated anion/cation pair held together by moderate electrostatic attraction

ion-dipole attraction

electrostatic attraction between an ion and a polar molecule

miscible

mutually soluble in all proportions

molality (m)

a concentration unit defined as the ratio of the number of moles of solute to the mass of the solvent in kilograms

nonelectrolyte

substance that does not produce ions when dissolved in water

osmosis

diffusion of a solvent molecules through a semipermeable membrane

osmotic pressure

opposing pressure required to prevent bulk transfer of solvent molecules through a semipermeable membrane

partially miscible

of moderate mutual solubility

Raoult’s Law

the relationship between a solution’s vapor pressure and the vapor pressures and concentrations of its components

saturated

containing the max concentration of solute possible for a given temperature and pressure

semipermeable membrane

a membrane that selectively permits passage of certain ions or molecules

solubility

extent to which a solute may be dissolved in water, or any solvent

solvation

exothermic process in which intermolecular attractive forces between the solute and solvent in a solution are stabalized

spontaneou process

physical or chemical change that occurs without the addition of energy from an outside source

strong electrolyte

dissociates or ionizes completely when dissolved in water

suspension

concentration that exceeds solubility

suspension

heterogenous mixture in which relatively large components particles are temporarily dispersed but settle out over time

Tyndall effect

scattering of visible light by a colloidal dispersion

unsaturated

of concentration that is less than solubility

Van’t hoff factor (i)

the ratio between the number of moles of particles in a solution to the number of moles of formula units dissolved in the solution

weak electrolyte

substance that ionizes only partially when dissolved in water

defining traits of a solution

1. homogenous

2. physical state of solution is same as that of the solvent

3. components are dispersed in a molecular state

4. the dissolved solute in a solution will not settle out or separate from the solvent

5. the composition of a solution can be varied continuously

True or false

any gas, liquid, or solid can be a solvent

true

true or false

if gas bubbles are present, it is a solution and homogenous

false

why is water a bad conductor

it is only slightly ionized

why do air bubbles appear in cold water warmed to room temp

solubility of dissolved air decreases

what causes large scale fish die offs from thermal pollution

decreased solubility of oxygen

what happens when you open a carbonated drink and see bubbles

a decrease in pressure of gaseous CO2 and dissolved carbon leaving as bubbles

true or false

gasses can form supersaturated solutions

true

true or false

liquids that are polar are incapable of hydrogen bonding

false

the presence of nonvolatile solutes lowers the vapor pressure of a solution how

by impeding the evaporation of the solvent molecules

how is crude oil separated

by large scale functional distillation to isolate various simpler mixtures

what happens to vapor pressure as the temperature increases

it increases

what process revitalizes wilted carrots and celery

osmosis letting water move to the vegetables cells