Chem Subject Test 345 "acid Base"

Front 1

arrhenius acid

Back 1

only aqueous solution

produce H in an aqueous solution, proton donoer

Front 2

arrhenius base

Back 2

only aqueous solution

produce OH-
Hydroxide ion donor

Front 3

Bronsted-Lowry acid

Back 3

donate proton

Front 4

Bronsted-Lowry base

Back 4

accepts proton

Front 5

lewis acid

Back 5

lectron pair acceptor
electrophile

Front 6

lewis base

Back 6

electron pair donnor
nucleophile

Front 7

amphoteric

Back 7

can act as either base or acid

H2O

Front 8

The sronger the acid the () its conjugate base

Back 8

weaker

Front 9

Kw

Back 9

eq constant for ionization of water

Kw=[H3O+][OH-]=10^-14 at 25C

Front 10

pH

Back 10

-log[H3O] = -log[H+]
=log (1/[H+])

Front 11

pOH

Back 11

-log[OH-] =log(1/[H+])

Front 12

if [H+] =1x10^-3 then ph is

Back 12

3

Front 13

strong acid and base

Back 13

sissociate completely into component ions in solution

Front 14

strong acid is

Back 14

strong electrolyte

Front 15

HClO4

Back 15

strong acid

Front 16

HNO3

Back 16

strong acid

Front 17

H2SO4

Back 17

strong acid

Front 18

HCl

Back 18

strong acid

Front 19

HBr

Back 19

strong acid

Front 20

HI

Back 20

strong acid

Front 21

NaOH

Back 21

strong base

Front 22

KOH

Back 22

strong base

Front 23

other soluble hydroxides of group 1A and 2A

Back 23

strong base

Front 24

weaker acid and base

Back 24

do not ionize completely
weak electrolyte

Front 25

Ka (Kb)

Back 25

equilibrium constant for acid ionization
measure of the degree to which an acid dissociates

weaker the acid lower the Ka

Ka= conc product /reactant does not contain pure liq or sol

Front 26

neuralization rxn

Back 26

acid and base react to form salt and often water

Front 27

titration

Back 27

the addition of a solution of known concentration and volume to another solution to determine its unknown concentration

determine the Molarity of an acid or base

VaMa =VbMb or VaCa=VbCb

C=concentration

Front 28

equivalalence point

Back 28

point at which the amt of acid equals the amt of base

located at the center of the stepest region on the tiration curve

Front 29

titration of polyprotic acid

Back 29

more than one equivalence point

Front 30

Normality (N)

Back 30

is always equal to the whole number multiple of molarity

equivalent of an acid is the quantity that can supply 1 mole of proton

1M H2SO4 =2N

Front 31

buffer solution

Back 31

consists of a mixture of weak acid and its salt (conjugate base) or mixture of weak base and its salt (conjugate acid)

resist pH change when small amoutns of acids or base are added

Front 32

Henderson-hasselbach equation

Back 32

PH=PKa+log ([conju base]/[weak acid])

POH = pKb + log([conju acid]/[weak base])

when [cojugate base]=[conjugate acid]
PH=Pka bc log 1=0

estimate the ph of a solution in the fugger region where the concentration of the species and its conjugate are present in approximately equal concentration

Front 33

CN-

Back 33

stong base

Front 34

NH2-

Back 34

strong base

Front 35

nutralization use

Back 35

normality

N1V1 = N2V2

Front 36

dilution use

Back 36

use before and after

Front 37

more acidic ph? ka? pka?

Back 37

how ph
high ka
low pka