Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

CF3 > CH 7 > Flashcards

CH 7 Flashcards

1
Q

Arrhenius Theory 1887

A

Acid: a substance that liberate (free) hydrogen ions
Base: substance that supplies hydroxyl ions on dissociation

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

Bronsted Lowry theory 1923

A

is more useful than the Arrhenius theory because it represents the ionization in both an aqueous and non-aqueous system

Acid: is a substance both charged or uncharged capable of donating a proton

Base: is a substance charger or uncharged capable if accepting a proton from an acid

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

strength of acids and bases

A

the relative tendencies of the substances to give up and take on protons

strength varies with the solvent

acid is strong= (high tendency) readily gives up protons
base is strong= readily accepts protons
acid is weak= (low tendency) readily gives up protons to SMALL extent

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

strength of acid

A

it depends on not only the ability to give up protons but also ability of solvent to accept the protons from the acid (aka: BASIC STRENGTH of solvent)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

HCL

A

is a strong acid in water, because it readily gives up a proton

is a weak acid in glacial acetic acid

shows that strong and weak acid DEPENDS on solvent

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

Acetic Acid

A

is a weak acid in water because it gives up protons readily only to a small extent

is a strong acid in liquid ammonia

shows that strong and weak acid DEPENDS on solvent

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

solvent classifications

A

protophilic - basic solvent, accepting protons from solute (acetone, ether, liquid ammonia)

protogenic- proton donating compound (formic acid, acetic acid, sulfuric acid, liquid HCL, liquid HF)

amphiprotic- proton acceptors and proton donors (water and alcohol)

aprotic- hydrocarbons, neither accept or donate protons and is neutral, they can be useful for studying reaction free of solvent effects

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

cations

A

NH4+ and h30+

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

Anions

A

hso4- and ch3coo-

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

neutral

A

HCL and NH3

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

protolytic RXN

A

is protolysis

HCL+ H2O —> H30+ +Cl-
(acid 1)(base2)(acid 2)(base 1)

this is a IONIZATION Rxn

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

types of rxn

A

neutralization
hydrolysis
displacement

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

NH4+ +OH- —> h20 + NH3

A

neutralization

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

H30+ + OH- —> h20 + h20

A

neutralization

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

HCL + NH3—–> nh4+ + cl-

A

neutralization

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

h20 + ch2coo- —-> ch2cooh + oh-

A

hydrolysis

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

NH4+ + H20—->H30+ + NH3

A

HYDROLYSIS

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

acid-base rxn

A

acid reacts with acid to form a new acid and base (transfer of protons, so it is also called protolytic or protlysis)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

h30+

A

hydronnuim ions, hydrated proton

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

displacement rxn

A

a special type of neutralization involves the displacement of a weaker acid such as acetic acid from its salt.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

Lewis electronic theory

A

acid is a molecule or ions that accepts an electron pair to form a covalent bond

base is a substance provides the pair of unshared electrons by which the base coordinates with an acid

the H+ proton(acid) will attach to the unshared electron pair of N on NH3 to make NH4+

you do not need to contain hydrogen ions or hydroxyl ions to be and acid or base according to LET

22
Q

acid-base equilibria

A

equilibrium: a balance between two opposing forces of action. it is dynamic equilibrium of the two velocities

reversible reaction (weak electrolytes)

concentration of reactants and products are constant

23
Q

Ionic equilbria

A

bronsted lowry

24
Q

irreversible

A

to completetion

25
Q

Acid base equilbria of acetic acid

A

HAc + h20 -><- h30+ + Ac-

26
Q

Rf

A

the rate/velocity/speed of the forward reaction is proportional to the concentration of the reactants

Rf= k1 x [HAc]1 x [h20]1

k= specific reaction rate

27
Q

Rr

A

the reverse reaction of reformation of unionized acetic acid is proportional to concentration of reactants

Rr= K2 x [h30+]1 x [Ac-]1

28
Q

Rf=Rr

A

k1 x [HAc]1 x [h20]1=K2 x [h30+]1 x [Ac-]1

k=k1/k2=product=reactants

29
Q

dissociation constant

A

ka=55.3 k=product/HAc

30
Q

summary of ionization of weak acids

A

uncharged weak acid (HB) in water

HB + H2O —><— H30+B-

Dissociation constant:
Ka= [h30+][b-]/ HB

[H30+] =sqrt kaC

31
Q

x^2/c-x

A

x^2 is the value in moles of two products dissociated

x is dissociation # in moles

c is original amount in moles/liter or M

32
Q

dissociation of Salt

A

ammonium chloride in water

Nh4+cl- —> NH4+ + Cl-

NH4+ +H20 –><— H30+ + NH3

ka= [h30+] [NH3]/[NH4+]

33
Q

Summary of ionization of weak acids

A

charged weak acid BH+ in water
BH+ +H20–><— h30+ +B

dissociation contant [h30+][B]/ bh+

34
Q

ionization of weak bases

A

NON-ionized weak base,B, in water

B + H20—><— OH- +BH+

KB= [OH-] [BH+]/[B]

[oh-] =sqrt KbC

35
Q

dissociation of salt (base)

A

sodium acetate in water

Na+ CH3COO- —> Na+ +CH3COO-

dissociation:
CH3COO- + h20—> OH- + CH3COOH

Kb= [OH-][CH3COOH]/CH3COO-

36
Q

summary of ionization of weak bases

A

anionic base (B-) in water

B- +H2O –><– OH- +HB

Dissociation constant
kb= [OH]- [HB ]/ B-

37
Q

ionization of water

A

water
h20 + h20 —><— h30+ + OH-

dissociation constant and concentration
k= [h30+] [ OH-]/[h20]^2
kw= K x [h20]^2

kw= [h30+] [ OH-]= 1 x 10^-14 at 25 c
[h30+]= [oh-]= 1 x 10^-7

water concentration is 1 x 10^-7 meaning can be OH- and H30+

Kw or constant of water is 1 x 10^-14

if we add more acid to pure water, the increase in hydrogen ions will decrease the hydroxyl ions so that water remain constant Kw at 1 x 10-14 at 25c

38
Q

ion product of water at varying temps

A

25C, kw= 1 x 10^-14
pKw= 14 at 25C

if you add heat to an endothermic process, the position of equilibrium moves to the right (in forward). Ka increases! Since pKa=−logKa , an increase in Ka means a decrease in pKa .

increasing the temp from 60 to 70C, the Kw or constant of water will INCREASE( increase in temp, increases the rate of the forward rxn and dissociation constant). but the pkw will decrease with increasing temp

decrease in temp= increase Pka and decrease the ka, it production of ions REDUCE

Kw will increase temp rxn and is endothermic, more product is being favored in the forward rxn at high temp

at high temp more water molecules gain enough energy to break and dissociate and this leads to increase in concentration of OH- and H+ ions

39
Q

relationship between Kb and ka

A

dissociation constant of weak acid (uncharged) HB and H20
HB +H20= h30+ + B
Ka= [B][h30+]/[HB]

dissociation constant of anionic base, B-
B- +h20= oh- hb
kb=[oh-][hb]/[b-]

=KaKb
=[OH-][HB]/[B-]=[B][h30+]/[HB]
=[OH-][H3O+]=Kw

=Kw= KaKb
=kb=kw/ka
=ka= kw/kb

40
Q

ionization of polyprotric electrolytes

A

monoprotic electrolytes :
acids donate a single proton
bases accept a single proton

Polyprotic electrolytes: capable of donating and accepting two or protons
-diprotic (disbasic) acid (ex. carbonic acid) ionizes in 2 stages
-triprotic acid (trisbasic) acid (ex.phospohric acid) -ionizes in 3 stages

  • look at notes for phosphoric acid equations and Ka and Kb values
41
Q

ampholyte

A

a species can function either as a acid or base, amphoteric in nature

ex. glycine hydrochloride in water

+NH3CH2COOH +H20= +NH3CH2COO- +H3O+

+NH3CH2COO- +H20= NH2CH2COO- +H30+

+NH3CH2COO- +H30+= +nh3ch2cooh +OH-

api can be a weak acid or base

+NH3CH2COO- can act as a acid or base

42
Q

H2PO4- AND H2PO4 2-

A

ampholytes- acid or base

43
Q

+NH3CH2COO-

A

is the amphoteric species, is called a zwitterion, it is different from the phosphoric species(amphoteric specifies) in that it carries a positive and negative charge. the whole molecule is electrically neutral

44
Q

isoelectric point

A

is the net movement of the solute molecules in the electric field is negligible.

ph at which the zwitterion concentration is maximum

45
Q

Sorensens pH scale

A

the common logarithm of the reciprocal of the hydrogen ion concentration, aka hydrogen ion potential.

pH= log (1/H30+)
pH=log 1-log [H30+]
pH= -log[h3o+]

value of log 1 is 0

46
Q

the pH and corresponding hydrogen and hydroxyl ion concentrations

A

pH of 7 (NEUTRAL) the [h30+] and [oh-] are 10^-7moles/liter

at pH of 0 (highly acidic), [h30+] 10^0=1and [OH-]=10^-14 moles/liter

at a pH=14, [H30+] 10^-14, 10^0=1[OH-]

A pH of 7 is neutral. A decrease in pH below 7 shows an increase in acidity (hydrogen ions), while an increase in pH above 7 shows an increase in alkalinity (hydroxyl ions). Each pH unit represents a 10-fold change in concentration.

47
Q

pk and pOH

A

pH + pOH= pKw
pKa +pKb= pKw

48
Q

pKa

A

pH,
-logka

49
Q

pKb

A

pOH,
-log[oh-]

50
Q

pk

A

is dissociation exponent

51
Q

hydrogen ion concentration of weak acid

A

[h30+] = sq rt KaC

52
Q

hydroxyl ion concentration of weak base

A

[OH-]= sq rt KbC

CF3 (6 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions