Chapter 14 Chemistry Test

Front 1

percent by mass equation

Back 1

mass of solute X 100
mass of solution

Front 2

percent by volume equation

Back 2

volume of solute X 100
volume of soluion

Front 3

Molarity (M) equation

Back 3

moles of solute
liters of solution

Front 4

Dilution equation

Back 4

M1V1 = M2V2

Front 5

mole fraction equation

Back 5

moles of solute
moles of solute + moles of solvent

Front 6

Concentration

Back 6

a measure of how much solute is dissolved in a specific amount of solvent or solution

Front 7

percent by mass

Back 7

the ratio of the solute's mass to the solution's mass expressed as a percent

Front 8

percent by volume

Back 8

the ration of the volume to the solute to the volume of the solution, expressed as a percent(usually describes solutions in which both the solute and solvent are liquids)

Front 9

molarity

Back 9

the number of moles of solute dissolved per liters of solution (also known as molar concentration)

Front 10

molality

Back 10

the ratio of the number of moles of solute dissolved in one kg of solvent

Front 11

molality (m) equation

Back 11

moles of solute
kg of solvent

Front 12

mole fraction

Back 12

the ratio of the number of moles of solute of solvent in a solution to the number of moles of solute and solvent

Front 13

solvation

Back 13

the process of surrounding solute particleswith solvent particles to form a solution

Front 14

heat of solution

Back 14

the overall energy change that occurs during the solution formation process

Front 15

unsaturated solution

Back 15

one that contains less dissolve solute for a given temperature and pressure than a saturated solution

Front 16

saturated solution

Back 16

contains the maximum amount of dissolved solute for a given amount of solvent at a specific temperature and pressure

Front 17

supersaturated solution

Back 17

contains more dissolved solute than a saturated solution at the same temperature

Front 18

Henry's Law

Back 18

states that at a given temperature, the solubility of a gas is directly proportional to the pressure of the gas above the liquid

Front 19

Henry's Law equation

Back 19

S1/P1 = S2/P2

Front 20

colligative properties

Back 20

physical properties of solutions that are affected by the number of particles but not by the identity of dissolved solute particles

Front 21

vapor pressure lowering

Back 21

due to the number of solute particles in solution and is a colligative property of solutions (the greater the number of solute particles in a solvent, the lower the resulting vapor pressure)

Front 22

boiling point elevation

Back 22

the temperature difference between a solution's boiling point and a pure solvent's boiling point

Front 23

freezing point depression

Back 23

difference in temperature between its freezing point and the freezing point of its pure solvent

Front 24

osmosis

Back 24

the diffusion of a solvent through a semi-permeable membrane

Front 25

osmotic pressure

Back 25

the amount of additional pressure caused by the water molecules that moved into the concentrated solution (depends on the number of solute particles in a given volume of solution and is a colligative property of solutions)

Front 26

boiling point elevation equation

Back 26

▲Tb = Kb * m

Front 27

freezing point depression equation

Back 27

▲Tf = Kf * m

Front 28

suspension

Back 28

a mixture containing particles that settle out if left undisturbed

Front 29

colloid

Back 29

a heterogeneous mixture of intermediate-sized particles (between 1nm and 1000 nm in diameter and do not settle out)

Front 30

Brownian motion

Back 30

erratic movement of dispersed particles of liquid colloids

Front 31

Tyndall effect

Back 31

dispersed colloid particles scattering

Front 32

soluble

Back 32

a substance that dissolves in a solvent

Front 33

miscible

Back 33

two liquids that are soluble in each other in any proportion

Front 34

insoluble

Back 34

a substance that does not dissolve in a solvent

Front 35

immiscible

Back 35

two liquids that can be mixed together but separate shortly after

Front 36

thixotropic mixtures

Back 36

when suspensions separate into a solidlike mixtureon the bottom and water on the top. when the solidlike mixture is stirred or agitated, it flows like a liquid

Front 37

agitation

Back 37

stirring or shaking of the mixture that moves dissolved particles away from the contact surfaces more quickly and therby allows new collisions between solute and solvent particles to occur

Front 38

surface area

Back 38

if this increases, more collisions can occur

Front 39

factors that affect solvation

Back 39

agitation, surface area, temperature

Front 40

fact about solubility of gases

Back 40

as a solution's temperature increases, the solubility of a gaseous solute decreases

Front 41

quantitative descriptions of concentration

Back 41

percent by mass, percent by volume, molarity, and molality