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Chem 102 > Exam 3 > Flashcards

Exam 3 Flashcards

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1
Q

Ka =

A

(concentration products) / (concentration reactants)

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2
Q

pKa =

A
  • log (Ka)
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3
Q

Ka =

A

10 ^ -(pKa)

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4
Q

if there is a buffer, you use…

A

HH: pH = pKa + log (B-/HB)

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5
Q

a diprotic acid will have __ equivalence points, midpoints, and buffer regions

A

2

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6
Q

a triprotic acid will have __ equivalence points, midpoints, and buffer regions

A

3

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7
Q

How does pH relate to pKa at any point in the buffer regime of titration curve?

A

HH equation: pH = pKa + Log(B-/HB)

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8
Q

when “removing” multiple H+ protons, which is the hardest to remove?

A
  • first H+
  • Ka1 > Ka2 > Ka3
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9
Q

steps for solving a polyprotic acid titration:

A
  1. equation (NIE)
  2. calculate mm.mol
  3. ICE table
  4. buffer? –> HH equation
    • NO? –> pKa2/Ka2 –> ICE table –> HH
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10
Q

solubility product (Ksp) steps to solve:

A
  1. eon
  2. Ksp = (products)/(reactants) (aq)
  3. ICE table
  4. Ksp =
  5. x = solubility = (M)
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11
Q

would precipitate form? (steps:)

A
  1. NIE (s –> aq + aq)
  2. Ksp = # = (products)/(reactants)
  3. new Ms (calculate Psp = products/reactants)
  4. p </= K or p > K
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12
Q

would precipitate form? p </= K

A

no, ions in solution

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13
Q

would precipitate form? p > K

A

precipitation reaction

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14
Q

If something is a bronzed Lowry CA or CB it is also always a ___-

A

complex lewis structure (LB / LA)

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15
Q

Lewis Acid/Base: LB (Lewis Base)

A

has a lone pair that is “loses”

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16
Q

Lewis Acid/Base: LA (Lewis Acid)

A

“gains” an H+

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17
Q

ALL anions (-) that attach to central metal ion =

A

Lewis Bases

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18
Q

ALL cations (+) that attach to central atom =

A

Lewis Acids

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19
Q

H2O is a…

A

lewis base

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20
Q

H3O+ is a…

A

lewis acid

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21
Q

ligand

A

species that bonds to central atom in lewis A/B
- contains 2+ lone pairs (compounds) OR
- anions (-) ions attached

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22
Q

Cl-, Br-, CN-, and OH- are examples of

A

ligands (anions -)

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23
Q

coordination number

A

of species (ligands) around/by central atom

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24
Q

the more lone pairs…

A

the more H+ “donating” capability

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25
Q

PH (at equivalence point) =

A

1/2 (pka1 + pka2)

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26
Q

ΔS order for solid, liquid, gas

A

ΔSgas > ΔSliquid > ΔSsolid

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27
Q

if there are more gas moles on the RHS (products) > LHS (reactants), then ΔS =

A

(+)

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28
Q

if there are more gas moles on the LHS (reactants) > RHS (products), then ΔS =

A

(-)

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29
Q

if ΔS > 0 (+), the reaction is moving towards

A

disorganization, spontaneity, diffusion

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30
Q

if ΔS < 0 (-), the reaction is moving towards

A

organization

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31
Q

Gibbs Energy equation:

A

ΔGrxn = ΔHrxn - T*ΔSrxn

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32
Q

if ΔG > 0 (+) , the reaction is

A

not spontaneous

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33
Q

if ΔG < 0 (-), the reaction is

A

spontaneous

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34
Q

if ΔG = 0, the reaction is

A

at equilibrium

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35
Q

HH equation(s):

A

pH = pKa + log [B-/HB]
OR
pH = pKa - Log [HB/B-]

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36
Q

not buffer WA/WB pH and pOH equation(s):

A

pH = 1/2 (pKa - log (Ma))
pOH = 1/2 (pKb - log (Mb))

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37
Q

pKa =

A

-log(Ka)
OR
-log(Ksp)

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38
Q

Ka (OR Ksp) =

A

10^ -(pKa)

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39
Q

if a compound is very (-), it has a __ pH

A

high pH
- the more (-) = the higher pH

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40
Q

if a compound is (+), it has a ___ pH

A

low pH

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41
Q

pH + pOH =

A

14

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42
Q

(@ T=25C) Kw =

A

10^-14 = [H3O+][OH-]

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43
Q

(CA/CB): pKa + pKb =
- @ T=25C

A

14

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44
Q

(WA/WB): x = [H3O+] =

A

sqrt[Ka*Ma]
- GJ eqn

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45
Q

WB : x = [OH-] =

A

sqrt[Kb*Mb]
- GJ eqn

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46
Q

central metal ions are generally ___ charge

A

2+

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47
Q

Ag charge

A

1+

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48
Q

H2O charge

A

0

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49
Q

nh3 charge

A

0

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50
Q

CO charge

A

0

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51
Q

the __ molecule is listed first

A

central metal ion

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52
Q

Zn charge

A

2+

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53
Q

the charge at the end of a compound applies to…

A

the ENTIRE compound

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54
Q

“total charge” of a compound must add up to equal…

A

0
- (charge cation) + (charge anion) = 0
- (charge central ion) + (charge rest of compound) = 0

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55
Q

ligands are classified by

A

the # of shared e- w/ central atom

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56
Q

monodentate

A

only bind at 1 site
- share 1 pair of e-

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57
Q

polydentate

A

ligands that are more than 1 pair of e-
- can bind to central atom at multiple points

58
Q

bidentates bind at…
and their coordination number is…

A

2 sites
- # = 2

59
Q

4 bidentates

A

oxalate (ox), ethylenediamine (en), acetylacetonate (acac), phenanthroline (phen)

60
Q

oxalate (ox): formula, formal charge, coordination #

A
  • formula: (C2O4)^(2-)
  • charge: (2-)
  • coordination #: (2)
61
Q

ethylenediamine (en): formal charge and coordination #

A
  • charge: (0)
  • coordination #: (2)
62
Q

acetylacetonate (acac): formal charge and coordination #

A
  • charge: (1-)
  • coordination #: (2)
63
Q

phenanthroline (phen): formal charge and coordination #

A
  • charge: (0)
  • coordination #: (2)
64
Q

chelating agent

A

polydentate ligands used to extract a metal from solution
- ex: hexadentate ligand in EDTA

65
Q

naming: anion (-) ligands

A

suffix-“o”
- Cl- = chloro-
- OH- = hydroxo-
- CN- = cyano-
- CH3CO2- = acetato-
- SO4^2- = sulfato-
- CO3^2- = carbonato-

66
Q

naming: molecular ligands

A

their name
EXCEPT:
- H2O = aqua-
- NH3 = ammin-

67
Q

naming: # of same type of ligands =

A

prefix
- di (2), tri (3), tetra (4), penta (5), hexa (6)

68
Q

naming: complex ligand prefix

A

bis, tris

69
Q

naming: complex ligand prefix

A

bis, tris

70
Q

naming: if there are different ligands…

A

name them in alphabetical order

71
Q

naming: the oxidation number is represented by

A

roman numerals at the end
- charge of central metal ion

72
Q

naming: complex ion = anion (-) …..

A

suffix = “-ate”

73
Q

Fe(ox)3

A

trisoxalate ferrate IV

74
Q

CuI4

A

tetriodo cuprate II

75
Q

You titrate 30 mL of 0.1 M selenious acid, H2SeO3 (pKa1 = 2.6, pka2 = 8.3) w/ 0.1 M NaOH to the 1st MIDPOINT of the titration. What expression is the correct way to find the pH?

A

pH = pKa1

76
Q

CN charge

A

1-

77
Q

enthalpy change (ΔH) =

A

(products) - (reactants)

78
Q

entropy change (ΔS) =

A

(products) - (reactants)

79
Q

ΔH and ΔG become equal at what temp?

A

0 K

80
Q

at equilibrium, ΔG =

A

0

81
Q

at a phase transition, ΔG =

A

0

82
Q

phase transitions

A

vaporization: liquid –> gas
fusion: solid –> liquid
Boiling: 100C (liquid —> gas)
Melting: (solid —> liquid)

83
Q

if ΔG = 0, then ____ equation is true

A

ΔH = T*ΔS

84
Q

ΔG =

A

ΔH - T*ΔS

85
Q

ΔS increase,

A

randomness/diversity increases

86
Q

2nd Law: ΔSuniverse >

A

> 0
- always
- always moving towards spontaneity

87
Q

2nd Law: entropy of the universe

A

ΔSrxn - ΔH/T > 0

88
Q

criteria for spontaneity:

A

ΔHrxn - T*ΔSrxn < 0

89
Q

an increase in volume causes a ___ in ΔS

A

increase in ΔS

90
Q

ΔS ___ w/ increasing mass

A

increases

91
Q

ΔG and ΔS have what relationship?

A

inverse
- ΔS = (+), ΔG = (-)

92
Q

at 1 atm Gibbs equation states:

A

ΔGrxn = ΔH - T*ΔS

93
Q

at equilibrium Gibbs equation states:

A

K = e^(-ΔG/RT)
- K = equilibrium constant
- R = 8.314 J/Kmol = 0.008314 kj/Kmol
- T = temp (K)

94
Q

low temperatures are…

A

endothermic (-) = not spontaneous

95
Q

high temperatures are…

A

exothermic (+) = spontaneous

96
Q

common ion effect

A

solution w/ 2 compounds (1 similar ion)
- NIE = compound (1) –> ion + ion
- similar ion [M] starts w/ M amount
- solve SICE table
- can ignore “x” for common ion in Ksp = (E(common ion) = M)

97
Q

@ pKa1, there is ___ amount of CA/CB(1)

A

50/50

98
Q

@ pKa2, there is ___ amount of CA/CB(2)

A

50/50

99
Q

when calculating the “end” row of the “SICE” table, you follow ____ format

A

(initial) +/- (stoichiometry)(x)

100
Q

to calculate a new M for ions in a solution…

A

[1] = (1st mL)(M)/(total mL)

101
Q

CN-, CO, NO2-, en =

A

strong ligands
- largest energy:
- CN- > CO > NO2- > en

102
Q

H2O, ox, F-, Cl-, Br-, I- =

A

weak ligands
- largest –> smallest energy:
- en > H2O > ox > F- > Cl- > Br- > I-

103
Q

ΔG units

A

kJ / mol

104
Q

“spontaneity switch temp” =

A

ΔG = 0
- T = ΔH/ΔS

105
Q

if ΔH and ΔS are both (+), the reaction is…

A
  • low temp = not spontaneous
  • high temp = spontaneous
106
Q

if ΔH = (-) and ΔS = (+), the reaction is…

A

always spontaneous
- ΔG = (-)

107
Q

if ΔH = (+) and ΔS = (-), the reaction is…

A

never spontaneous
- ΔG = (+)

108
Q

if ΔH and ΔS are both (-), the reaction is…

A
  • low temp = spontaneous
  • high temp = not spontaneous
109
Q

if ΔH and ΔS have the same sign, Temperature =

A

T spontaneity = switchable
- T = ΔH/ΔS
- below T and above T; spontaneity switches
- if ΔH = (+), ΔG = (+)

110
Q

if you combine a solid with H2O, it is likely a…

A

dissociation reaction
- solid –> aq + aq

111
Q

if you combine 2 solids w/ a common ion….

A

NIE can ignore 2nd solid
- initial M for common ion in “SICE” table = M of 2nd solid

112
Q

SCN- name

A

thiocyanate ion

113
Q

change in enthalpy

A

ΔH

114
Q

change in entropy

A

ΔS

115
Q

ΔS units

A

J/ kmol = kJ/kmol

116
Q

ΔG units

A

kJ (or J) / mol or just kJ (energy change)

117
Q

ΔH units

A

kJ/mol

118
Q

J –> kJ

A

J * 10^(-3)

119
Q

ΔH and ΔG are equal at what temperature?

A

0 K

120
Q

What is the significance of the superscript in symbol ΔG∅?

A

superscript means gaseous species are at 1 atm partial pressure and ions are at 1 M conc’n

121
Q

phase transition: M(s) –> M (g)
- what can be said about the Gibb energies of the solid and gaseous forms of substance M?
- Name of phase transformation?)

A
  • G(M(s)) = G (M(g)).
  • sublimation
122
Q

∆H = (+) and ∆S = (-)….

A

will NEVER be spontaneous

123
Q

What is the difference between ΔGrxn and ΔSrxn?

A
  • ΔSrxn = rxn increases disorder or not
  • ΔGrxn = would rxn ever happen under the conditions specified
124
Q

Give the 2nd Law of thermodynamics in terms of entropy change of the universe.

A

a reaction is spontaneous only if
ΔSuniv > 0

125
Q

What is the relation between ΔGrxn and ΔSuniverse?

A

ΔGrxn ≡ -T(ΔSuniv)

126
Q

when calculating Δ from a table of values….

A

P - R
- (-) carries through!! to all reactants
- ((#)P + (#)P) - (#)R - (#)R

127
Q

Relation b/w ΔG∅ and standard voltage, E∅:

A

ΔG∅ = -nFE∅
- n = # of e- transferred (given)
- F = Faraday’s constant ~ 96.5 kJ/mol*V
- E∅ = voltage

128
Q

entropy increases w/

A

increasing mass

129
Q

pKa > 7 =

A

Base!!

130
Q

diprotic titration: pKa1 occurs at what volume?

A

1/2 mL of acidic species (given mL)

131
Q

diprotic titration: equivalence point 1 occurs at what volume?

A

mL of acidic species (given mL)

132
Q

diprotic titration (same M): pka2 occurs at what volume?

A

given mL (*1.5)

133
Q

diprotic titration (same M): equivalence point 2 occurs at what volume?

A
  • given mL. (*2)
134
Q

LA and LB are always…

A

reactants

135
Q

in the reaction quotient Q, the [] can be replaced w/ given…

A

concentration (M) or partial pressure (atm)

136
Q

when given ΔS, you MUST ALWAYS…

A

CONVERT TO KJ

137
Q

magnesium phosphate

A

Mg3(PO4)2

138
Q

to make a buffer…

A

you need: CA/CB or WA/SB or SA/WB
- pka ≈ pH

139
Q

polyprotic titration: to find mL titrant at equivalence point (1, 2, 3)…

A

m1v1 (analyte) = m2v2 (titrant)
- v2 = equivalence point 1
- v2 * 2 = equivalence point 2
- v2 * 3 = equivalence point 3

140
Q

polyprotic titration: to find mL at pKa (1, 2, 3)…

A
  • pka1 = 1/2 (mL equivalence point 1)
  • pka2 = 1/2 (mL equivalence point 2)
  • pka3 = 1/2 (mL equivalence point 3)

Chem 102 (6 decks)

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