Ch. 11

Question 1

what are BL acids? BL bases?

Answer 1

bases: proton acceptors
acids: proton donors

Question 2

what are L acids? L bases?

Answer 2

bases: electron donors
acids: electron acceptors

Question 3

what are conjugate acids/bases

Answer 3

new species that develop when they accept an e- or H+

Question 4

dissociation of acids or bases can be found

Answer 4

Ka= (H) (A)/ (HA) where HA+H2O=H+A same for Kb= (HB) (OH)/ B) where B+H2O=OH+ HB

Question 5

what are the strong acids

Answer 5

HI, HBr, HCl, HClO4 (perchloric acid) H2SO4 (Sulfuric acid), and HNO3 (nitric acid)

Question 6

what are strong bases

Answer 6

Group one hydroxides: NaOH
Group one oxides: Li2O
some group 2 hydroxides: BaOH2 SrOH2
and some metal amide (NaNH2)

Question 7

the conjugate base/acid of strong acid/base has what properties in water?

Answer 7

no basic or acidic properties because they do not interact with water

Question 8

what are amphoteric substance? what are polyprotic substances?

Answer 8

amphoteric: compounds that can act both as base or acid like water
polyprotic: can donate more than 1 proton to donate

Question 9

pH measures what, what formulas you need

Answer 9

measure H+ conc where ph=-log(h) and 10^-ph

Question 10

pOH measures what, what formulas you need

Answer 10

measures OH conc where pOH=-log(oh) and 10^pOH

Question 11

what is a salt?

Answer 11

an ionic compound with an anion and cation

Question 12

what is a buffer

Answer 12

solution that resists changing pH when a little bit of acid or base is added

Question 13

what is an indicator

Answer 13

a weak acid that undergoes a color change when its converted to its conjugate base

Question 14

what is an acid base titration

Answer 14

it helps you determine an unknown weak acid/base by determining its pKa/Kb

Question 15

the known acid/base in titration is called? what titrant do you use for an unknown acid

Answer 15

titrant. you add a base for unknown acid and vise versa

Question 16

what is buffer domain/ region

Answer 16

area where pH changes gradually

Question 17

what is the equivalence point

Answer 17

area with drastic ph increase,where moles of added strong acid/base is equal tp moles of unk base/acid at beginning

Question 18

for a weak acid (strong base) where is equivalence point

Answer 18

ph>7

Question 19

for a weak base (strong acid ) where is equivalence point

Answer 19

ph<7

Question 20

for a strong acid (strong base) and vice versa where is equivalence point

Answer 20

ph=7

Question 21

what is half equivalence point? what is important to note in this area

Answer 21

the half equivalence point is where 1/2 was added and only 1/2 was converted/ pKa of unknown substance is equal to pH at this point (straight line up on graph)

Question 22

for pH calculations, how do you solve for a strong acid/base? weak acid/base?

Answer 22

strong acid/base will have H+ conc= acid conc ex. H+= 0.01 M gives pH= 2 when you use -log of H+
weak acid/base: you need to fill table out with initial conc and use formula

Question 23

what does Ka or Kb need to be for x to be negligible in a pH calculation

Answer 23

less than 10^-4

Question 24

what is a neutralizing rxn?

Answer 24

when an acid and base combine and creates a salt and water

Question 25

in a neutralizing rxn, what do strong acids/bases to do pH? weak acids/bases?

Answer 25

strong acids with strong bases will produce a neutral pH. weak bases with weak acids will NOT produce a solution with a neutral pH

Question 26

what is important to note about ALL neutralizing rxns?

Answer 26

they will all go to completion

Question 27

what cation do NOT interact with water

Answer 27

group 1 ions and large group 2 ions

Question 28

what cations DO interact with water

Answer 28

metals in black D like Cr, Cu, etc because they are strong acids

Question 29

what anions do NOT interact with water

Answer 29

conjugate base of a strong acid because its weak

Question 30

what anions DO interact with water

Answer 30

strong conj base than H2O of weak acids

Question 31

an ideal buffer has

Answer 31

pH=pKa

Question 32

with an indicator, if you have H+> Ka, what color do we see?

Answer 32

color #1 because it favors reverse rxn

Question 33

with an indicator, if you have H+< Ka, what color do we see?

Answer 33

color #2 because it favors forward rxn

Question 34

with an indicator, if you have H+= Ka, what color do we see?

Answer 34

mixing of both colors

Question 35

what is a half equivalence point

Answer 35

where strong acid/base neutralized all unk base/acid and Ph=pKa

Question 36

at the beginning of a titration where there isnt much pH change, what is this called

Answer 36

buffering region

Question 36

what is equivalence point

Answer 36

moles of added strong acid/base is equal to moles of unk base or acid at the beginning

Question 37

what is equation that we use when we want to know how much of something we need to neutralize or titrate?

Answer 37

a * [A] * Va= b *[B] * Vb where V is volume, a is one, and [A/B] moles of substance

Question 38

Ka and Kb have what kind of relationship?

Answer 38

inverse

Question 39

when you hyperventilate, what occurs to bicarb ions

Answer 39

decrease

Question 40

what is the only thing that will affect Kw

Answer 40

temp