General Chemistry Ii, Chapter 12

Front 1

the substance doing the dissolving

Back 1

solvent

Front 2

the substance being dissolved

Back 2

solute

Front 3

relatively little solute in a given amount of solvent

Back 3

dilute

Front 4

relatively large amount of solute in a given amount of solvent

Back 4

concentrated

Front 5

a solute in which the solvent has absorbed as much solute as possible

Back 5

saturated solution

Front 6

all solutions have four things in common:

Back 6

1. homogeneity
2. absence of settling
3. molecular or ionic state of subdivision of solute
4. composition can be varied wtihin limits

Front 7

solubility of a gas in a liquid depends on

Back 7

1. the nature of the gas
2. the pressure on the gas
3. temperature

Front 8

mutually soluble liquids are said to be...

Back 8

miscible

Front 9

mutually insoluble liquids are said to be...

Back 9

immiscible

Front 10

the separation of two liquids on the basis of their boiling point

Back 10

fractional distillation

Front 11

solution which distills without a change in the composition or temperature

Back 11

azeotrope

Front 12

the vapor pressure of a mixture can be:

Back 12

1) between the vapor pressures of either pure component
2) higher than the vapor pressure of either pure component
3) lower than the vapor pressure of either pure component

Front 13

the attraction of the + or – end of a polar molecule for an oppositely charged ion.

Back 13

ion-dipole interaction

Front 14

the association of solvent molecules with solute particles

Back 14

solvation

Front 15

solution with dissolved ions. Can conduct electricity

Back 15

Electrolytes

Front 16

solution which contains no dissolved ions. Cannot conduct electricity

Back 16

Nonelectrolytes

Front 17

Compounds dissolve spontaneously (w/out catalyst or heat) if:

Back 17

1) there is a decrease in the internal energy of the system
2) there is an increase in the entropy of the system
one of these two qualities can override the other.

Front 18

The removal of the particles from the crystal lattice is

Back 18

endothermic

Front 19

The solvation of the dissolved particles is

Back 19

exothermic

Front 20

a solution in which the solvent has dissolved as much solute as possible.

Back 20

Saturated solution

Front 21

a solution in which there is an equilibrium between dissolved and undissolved solute

Back 21

saturated solution

Front 22

Factors effecting the rate of solution:

Back 22

1) solubility – the more soluble, the faster it dissolves
2) degree of subdivision – increase in degree of subdivision increases rate of dissolution
3) stirring
4) heating

Front 23

solution whose concentration is known

Back 23

standard solution

Front 24

grams of solute over grams of solution times 100

Back 24

mass percent or weight percent

Front 25

moles of solute over moles of solution

Back 25

mole fraction

Front 26

mole fraction times one hundred

Back 26

mole percent

Front 27

moles of solute per liter of solution

Back 27

molarity

Front 28

given in terms of the number of equivalents of solute per liter of solution

Back 28

normality

Front 29

moles of solute per kg of solvent

Back 29

molality

Front 30

the amount of that acid that provides 1 mol of H+ or protons in an acid-base reaction

Back 30

equivalent of an acid

Front 31

the amount of that base that provides 1 mol of hydroxide ions or reacts with 1 mol of H+ in acid-base reactions

Back 31

equivalent of a base

Front 32

Mconc x Lconc = Mdilute x Ldilute this equation works with all concentration terms (m, M, etc.) and terms of volume.

Back 32

dilution of solutions

Front 33

uses a set of burets

Back 33

Titration

Front 34

reaction of equivalent amounts of an acid and a base.

Back 34

Neutralization

Front 35

an organic dye that shows different colors in different media

Back 35

Indicator

Front 36

that point at which neutralization occurs (meq acid = meq base)

Back 36

Endpoint

Front 37

The addition of non-volatile solute to a solvent ________ the vapor pressure of the solvent

Back 37

lowers

Front 38

the addition of a non-volatile solution a solvent ________ the boiling point of the solvent

Back 38

raises

Front 39

the addition of a non-volatile solution a solvent ________ the freezing point of the solvent

Back 39

lowers

Front 40

the vapor pressure of any component of an ideal solution is equal to the vapor pressure of the pure component multiplied by the mole fraction in the solution. Change in pressure = mole fraction of solute times the pressure of pure solvent.

Back 40

Raoult’s law

Front 41

those that are determined by the number of particles in a solute and in a solution and not the size, type, or mass of the particle.

Back 41

Colligative property

Front 42

the boiling point elevation due to the addition of 1 mol of a non-volatile non-electrolyte to 1 kg solvent.

Back 42

Molal boiling point elevation constant (Kb)

Front 43

the freezing point depression due to the addition of 1 mol of a non-volatile non-electrolyte to 1 kg solvent.

Back 43

Molal freezing point depression constant (Kf)

Front 44

the diffusion of solvent molecules through a semipermeable membrane from an area of high concentration to an area of low concentration.

Back 44

Osmosis

Front 45

pressure required to stop osmosis of solvent molecules through the semipermeable membrane. Π=MRT

Back 45

Osmotic pressure (π)

Front 46

a pair of oppositely charged ions that remain associated with one another in solution

Back 46

Ion pair