Acids and Bases Lec Slides

Question 1

Arrhenius acid

Answer 1

a substance that dissociated in water to produce hydrogen ions

Question 2

arrhenius base

Question 3

what does the arrhenius theory not apply to

Answer 3

non-aqueous solutions

Question 4

bronsted-lowry acid

Answer 4

a substance that can give a hydrogen ion
-proton donor

Question 5

bronsted-lowry base

Answer 5

a substance that can take a hydrogen ion
-proton acceptor

Question 6

Ka

Answer 6

describes the reaction of an acid with the solvent H2O as the base
-the stronger the acid, the LARGER the Ka

Question 7

Kb

Answer 7

only describes the rxn of a base with the solvent H2O as the acid
-the stronger the base, the LARGER the Kb

Question 8

amphoteric

Answer 8

when something acts as both an acid and base

Question 9

Kw

Answer 9

ion-product constant for water

constant in aq sol at 25 dec C

=1.0x10^-14

Question 10

basic solution

Answer 10

pH>7

Question 11

acidic solution

Answer 11

pH<7

Question 12

strong acid

Answer 12

fully dissociates in water

Question 13

weak acid

Answer 13

partially dissociates in water

Question 14

inert acid

Answer 14

doesn’t dissociate in water

Question 15

the slight dissociation of a weak acid still results in …

Answer 15

a much greater H3O+ conc relative to pure water

Question 16

strong acid –> conjugate

Answer 16

inert base

Question 17

weak acid –> conjugate

Answer 17

weak base

Question 18

inert acid –> conjugate

Answer 18

strong base

Question 19

strong acid and strong bases are …

Answer 19

strong electrolytes

-assume they ionize completely in water

Question 20

HClO4, H2SO4, HNO3, HCl, HBr, HI

Answer 20

strong acids

Question 21

LiOH, NaOH, KOH, Ca(OH)2, Sr(OH)2, Ba(OH)2

Answer 21

strong bases

Question 22

weak acids and weak bases are…

Answer 22

weak electrolytes
-they ionize to a limited (but detectable) extent in water

Question 23

levelling effect

Answer 23

-different strong acids have different Ka’s
-in water, they exhibit the similar acidic properties
i.e. the acid strength of H3O+

Question 24

degree of polarity of H-A bond:

Answer 24

depends upon the electronegativity of A

Question 25

the more polar the H-A bond...

Answer 25

the stronger the acid

Question 26

the strength of the H-A bond...

Answer 26

depends on the size of the A atom

Question 27

the larger the A atom...

Answer 27

the longer/weaker the bond--> the stronger the acid

Question 28

across the period, electronegativity increases, so acidity..

Answer 28

increases

Question 29

down the group, bond strength decreases, so acidity...

Answer 29

increases

Question 30

in oxoacids, why does the acid strength increase as the electronegativity of y increases

Answer 30

a more electronegative y pulls electron density away from O-H bonds, making it easier for H+ to dissociate

Question 31

why does the strength of oxoacids increase with m(# of lone oxygen atoms)

Answer 31

the electronegative oxygen atoms pull electron density from the chlorine, making it more positive, which in turn weakens the O-H bond

Question 32

if same structure in oxoacids,

Answer 32

different y

Question 33

if same y in oxoacids,

Answer 33

different structure

Question 34

why do salts that are derived from a weak base and a strong acid yield acidic solutions? (e.g. NH4Cl)

Answer 34

solutions of NH4Cl are acidic because the ammonium ion will generate some hydronium while the chloride ion (Cl-) does NOT dissociate

Question 35

salts that are derived from a strong base and a weak acid yield...

Answer 35

basic solutions

Question 36

Ka>Kb

Answer 36

acidic

Question 37

Ka

Answer 37

basic

Question 38

lewis acid

Answer 38

species that accepts an electron-pair

Question 39

lewis base

Answer 39

species that donates an electron pair

Question 40

true or false all bronsted lowry acids are also lewis acids

Answer 40

true

Question 41

small, highly charged metal ions form complexes in water -the resulting complexes are...

Answer 41

proton donors