Stenberg Chemistry Solutions Unit

Front 1

alkaline

Back 1

a solution formed when a base completely dissociates in water to yield aqueous OH- ions

Front 2

amphoteric

Back 2

any species that can react as either an acid or a base

Front 3

Arrhenius acid

Back 3

a chemical compound that increases the concentration of hydrogen ions in aqueous solution

Front 4

Arrhenius base

Back 4

a chemical compound that increases the concentration of hydroxide ions in aqueous solution

Front 5

binary acid

Back 5

an acid that contains only two different elements: hydrogen and one of the more-electronegative elements

Front 6

boiling-point elevation

Back 6

the difference between the boiling points of the pure solvent and a solution of a nonelectrolyte in that solvent

Front 7

Brønsted-Lowry acid

Back 7

a molecule or ion that is a proton donor

Front 8

Brønsted-Lowry base

Back 8

a molecule or ion that is a proton acceptor

Front 9

colligative properties

Back 9

properties that depend on the concentration of solute particles but not on their identity

Front 10

Colloid

Back 10

a mixture involving solute particles of intermediate size

Front 11

Concentration

Back 11

a measure of the amount of solute in a given amount of solution or solvent

Front 12

conjugate acid

Back 12

the species that forms when an Brønsted-Lowry base accepts a proton

Front 13

conjugate base

Back 13

the species that remains after a Brønsted-Lowry acid has given up a proton

Front 14

dissociation

Back 14

the separation of ions that occurs when an ionic compound dissolves

Front 15

Effervescence

Back 15

The rapid escape of a gas from a liquid in which it is dissolved

Front 16

Electrolyte

Back 16

a substance that dissolves in water to give a solution that conducts electricity

Front 17

freezing-point depression

Back 17

the difference between the freezing points of the pure solvent and a solution of a nonelectrolyte in that solvent

Front 18

heat of solution

Back 18

The amount of heat energy absorbed or released when a specific amount of solute dissolves in a solvent

Front 19

Henry’s law

Back 19

The solubility of a gas in a liquid is directly proportional to the partial pressure of that gas on the surface of the liquid

Front 20

hydronium ion

Back 20

H3O+

Front 21

Immiscible

Back 21

Liquid solutes and solvents that are not soluble in each other

Front 22

ionization

Back 22

ions are formed from solute molecules by the action of the solvent

Front 23

Miscible

Back 23

Liquids that dissolve freely in one another

Front 24

molal boiling-point constant

Back 24

the boiling-point elevation of the solvent in a 1-molal solution of a nonvolatile, nonelectrolyte solute

Front 25

molal freezing-point constant

Back 25

the freezing-point depression of the solvent in a 1-molal solution of a nonvolatile, nonelectrolyte solute

Front 26

molality

Back 26

the concentration of a solution expressed in moles of solute per kilogram of solvent

Front 27

Molarity

Back 27

the number of moles of solute in one liter of solution

Front 28

monoprotic acid

Back 28

an acid that can donate only one proton per molecule

Front 29

net ionic equation

Back 29

An equation that includes only those compounds and ions that undergo a chemical change in a reaction in an aqueous solution

Front 30

neutralization

Back 30

the reaction of hydronium and hydroxide ions to form water

Front 31

nonvolatile substance

Back 31

a substance that has little tendency to become a gas under existing conditions

Front 32

osmosis

Back 32

The movement of solvent through a semipermeable membrane from the side of lower solute concentration to the side of higher solute concentration

Front 33

osmotic pressure

Back 33

the pressure required to stop the process of osmosis

Front 34

Oxyacid

Back 34

an acid consisting of hydrogen, oxygen, and a third element, usually a nonmetal

Front 35

pH

Back 35

defined as the negative of the common logarithm of the hydronium ion concentration

Front 36

pOH

Back 36

defined as the negative of the common logarithm of the hydroxide ion concentration

Front 37

polyprotic acid

Back 37

an acid that can donate more than one proton per molecule

Front 38

salt

Back 38

an ionic compound composed of a cation from a base and an anion from an acid

Front 39

semipermeable membrane

Back 39

a barrier that allows some substances to pass through while preventing the movement of others

Front 40

Solubility

Back 40

the amount of a substance required to form a saturated solution with a specific amount of solvent at a specified temperature

Front 41

Soluble

Back 41

capable of being dissolved

Front 42

Solute

Back 42

The substance dissolved in a solution

Front 43

Solution

Back 43

a homogeneous mixture of two or more substances in a single phase

Front 44

Solvent

Back 44

The dissolving medium in a solution

Front 45

spectator ions

Back 45

ions that do not undergo a chemical change when a reaction occurs in an aqueous solution

Front 46

strong acid

Back 46

acids that are strong electrolytes

Front 47

strong electrolyte

Back 47

a compound of which all or almost all of the dissolved compound exists as ions in an aqueous solution

Front 48

supersaturated solution

Back 48

A solution that contains more of a solute than can be dissolved at a given temperature and pressure

Front 49

Suspension

Back 49

A mixture where the particles in a solvent are so large that they settle out unless the mixture is constantly stirred or agitated

Front 50

titration

Back 50

the controlled addition and measurement of the amount of a solution of known concentration required to react completely with a measured amount of a solution of unknown concentration

Front 51

unsaturated solution

Back 51

A solution that contains less solute than a saturated solution under the existing conditions

Front 52

weak acid

Back 52

acids that are weak electrolytes

Front 53

weak electrolyte

Back 53

a compound of which a relatively small amount of the dissolved compound exists as ions in an aqueous solution