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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

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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

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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

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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)

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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

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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

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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

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8
Q

cations

A

NH4+ and h30+

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9
Q

Anions

A

hso4- and ch3coo-

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10
Q

neutral

A

HCL and NH3

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11
Q

protolytic RXN

A

is protolysis

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

this is a IONIZATION Rxn

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12
Q

types of rxn

A

neutralization
hydrolysis
displacement

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13
Q

NH4+ +OH- —> h20 + NH3

A

neutralization

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14
Q

H30+ + OH- —> h20 + h20

A

neutralization

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15
Q

HCL + NH3—–> nh4+ + cl-

A

neutralization

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16
Q

h20 + ch2coo- —-> ch2cooh + oh-

A

hydrolysis

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17
Q

NH4+ + H20—->H30+ + NH3

A

HYDROLYSIS

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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)

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19
Q

h30+

A

hydronnuim ions, hydrated proton

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20
Q

displacement rxn

A

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

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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
Acid base equilbria of acetic acid
HAc + h20 -><- h30+ + Ac-
26
Rf
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
Rr
the reverse reaction of reformation of unionized acetic acid is proportional to concentration of reactants Rr= K2 x [h30+]1 x [Ac-]1
28
Rf=Rr
k1 x [HAc]1 x [h20]1=K2 x [h30+]1 x [Ac-]1 k=k1/k2=product=reactants
29
dissociation constant
ka=55.3 k=product/HAc
30
summary of ionization of weak acids
uncharged weak acid (HB) in water HB + H2O ---><--- H30+B- Dissociation constant: Ka= [h30+][b-]/ HB [H30+] =sqrt kaC
31
x^2/c-x
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
dissociation of Salt
ammonium chloride in water Nh4+cl- ---> NH4+ + Cl- NH4+ +H20 --><--- H30+ + NH3 ka= [h30+] [NH3]/[NH4+]
33
Summary of ionization of weak acids
charged weak acid BH+ in water BH+ +H20--><--- h30+ +B dissociation contant [h30+][B]/ bh+
34
ionization of weak bases
NON-ionized weak base,B, in water B + H20---><--- OH- +BH+ KB= [OH-] [BH+]/[B] [oh-] =sqrt KbC
35
dissociation of salt (base)
sodium acetate in water Na+ CH3COO- ---> Na+ +CH3COO- dissociation: CH3COO- + h20---> OH- + CH3COOH Kb= [OH-][CH3COOH]/CH3COO-
36
summary of ionization of weak bases
anionic base (B-) in water B- +H2O --><-- OH- +HB Dissociation constant kb= [OH]- [HB ]/ B-
37
ionization of water
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
ion product of water at varying temps
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
relationship between Kb and ka
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
ionization of polyprotric electrolytes
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
ampholyte
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
H2PO4- AND H2PO4 2-
ampholytes- acid or base
43
+NH3CH2COO-
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
isoelectric point
is the net movement of the solute molecules in the electric field is negligible. ph at which the zwitterion concentration is maximum
45
Sorensens pH scale
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
the pH and corresponding hydrogen and hydroxyl ion concentrations
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
pk and pOH
pH + pOH= pKw pKa +pKb= pKw
48
pKa
pH, -logka
49
pKb
pOH, -log[oh-]
50
pk
is dissociation exponent
51
hydrogen ion concentration of weak acid
[h30+] = sq rt KaC
52
hydroxyl ion concentration of weak base
[OH-]= sq rt KbC

CF3 (6 decks)

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