Chemistry: Acids And Bases

Front 1

acids produce

Back 1

H+ ions

Front 2

acids conduct ___ and form

Back 2

electricity and electrolytes

Front 3

acids react with metal by being

Back 3

corrosive

Front 4

acids turn litnus paper

Back 4

red

Front 5

acids with phenolphthaletin

Back 5

is clear

Front 6

acids usually begin with

Back 6

H

Front 7

bases produce

Back 7

OH- hydroxide)

Front 8

bases conduct

Back 8

electricity--form electrolytes

Front 9

bases are corosive T or F

Back 9

True

Front 10

bases turn litmus paper

Back 10

blue

Front 11

bases with phenolphthalein

Back 11

turn it pink

Front 12

bases end in

Back 12

OH

Front 13

strong bases

Back 13

dissociate (break down)

Front 14

strong bases dissociate in

Back 14

water

Front 15

strong acid

Back 15

ionizes (forms ions)

Front 16

strong acids ionize in

Back 16

water

Front 17

acids and bases ionize/dissociate by

Back 17

breaking apart to form (+) (-) ions

Front 18

strong bases/acids have more or less ions

Back 18

more

Front 19

strong acids/bases are better or worse electrolytes

Back 19

better

Front 20

strong acids/bases conduct more or less electricity

Back 20

more

Front 21

pH sclae shows

Back 21

strength and concentration

Front 22

the pH numbers

Back 22

0-14 (7 neutral)

Front 23

neutralization is

Back 23

a reaction b/t an acid and base to form salt and water

Front 24

Arrhenius theory says acids

Back 24

ionize to give off hydrogen ions in aqueous solution

Front 25

Arrhenius theory says bases

Back 25

ionize to give off hydroxide in aqueous solution

Front 26

monoprotic acids have

Back 26

one ionizable H; di, tri, etc

Front 27

not all compounds that contain H are___; it depends on

Back 27

acids--electronegativity

Front 28

Bronsted-Lowery theory says acids

Back 28

are a H ion donor

Front 29

Bronsted-Lowery theory says bases

Back 29

are a H ion acceptor

Front 30

Bronsted-Lowery theory follows what other theory

Back 30

Arrhenius

Front 31

conjugate acids are

Back 31

compounds formed when a base gains a H ion

Front 32

conjugate bases are

Back 32

compounds formed when an acid has donated a H ion

Front 33

amphoteric act as

Back 33

an acid or base (water)

Front 34

Lewis theory says acids

Back 34

accept a pair of electrons to form a covalent bond

Front 35

Lewis theory says bases

Back 35

can donate a pair of electrons to form a covalent bond

Front 36

strong acids do what in water

Back 36

completely ionize

Front 37

strong acids are any

Back 37

Binary Acid (HCl, HF, HBr)

Front 38

strong acids are any acid with

Back 38

2 or more oxygen than Hydrogen (H2SO4, HNO3)

Front 39

strong bases and any

Back 39

group I or II Hydroxide (except Be)

Front 40

titration is a process of

Back 40

adding a known amount of solution of known concentration to determine the concentration of another solution

Front 41

standard solution is one of

Back 41

known concentration

Front 42

an end point is the point

Back 42

at which the indicator changes color

Front 43

buffers are solutions in which the

Back 43

pH remains relatively constant when small ammounts of acid or base are added

Front 44

calculating molarity and concentration

Back 44

moles/Liter
M1V1=M2V2