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PSU Freshman > Chem112B Exam 3 > Flashcards

Chem112B Exam 3 Flashcards

1
Q

7 strong acids

A

HCl, HBr, HI, HClO3, HClO4, H2SO4, HNO3

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2
Q

8 strong bases

A

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

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3
Q

Strong acids/bases dissociation rule

A

Strong electrolytes and dissociate 100%

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4
Q

Group 1A and heavy 2A hydroxides are…

A

strong bases

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5
Q

The conjugate base of a strong acid is a

A

negligible base

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6
Q

The conjugate acid of a strong base is a

A

negligible acid

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7
Q

For weaker acids and bases, the stronger the the acid, the

A

weaker its conjugate base

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8
Q

Amines functional group is

A

weak base

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9
Q

Carboxylic acids and thiol functional groups are

A

weak acids

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10
Q

acid –>

A

H + conjugate base

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11
Q

Arrhenius acid

A

Produce H+ when dissolved in water

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12
Q

Arrhenius base

A

Produce OH- when dissolved in water

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13
Q

Bronsted acids donate

A

H

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14
Q

Bronsted bases accept

A

H

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15
Q

Amphoteric

A

Can act as either acid or base (H2O)

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16
Q

H + group 1A/2A metals =

A

basic in water

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17
Q

H + nonmetal

A

acidic in water

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18
Q

Regarding H + nonmetal, if same group…

A

larger atoms=more acidic

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19
Q

Regarding H + nonmetal, if same row,

A

more electronegativity=more acidic

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20
Q

Oxide + 1A/2A =

A

Basic

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21
Q

Oxide + nonmetal =

A

Acidic

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22
Q

Oxide + border metals/nonmetals =

A

Amphoteric

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23
Q

Lewis acids

A

accept electrons

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24
Q

Lewis bases

A

donate electrons and must have at least 1 lone pair

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25
Q

Lewis acids charge

A

+ or neutral

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26
Q

Lewis bases charge

A
  • or neutral
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27
Q

Lewis acids common examples

A

Transition metals, group III and small group II cations, incomplete octets (BF3)

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28
Q

Lewis bases common examples

A

NH3, H20, F-, CN-

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29
Q

Group 1A and heavy group 2A oxides/hydroxides are

A

basic

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30
Q

Non-metal oxides/hydroxides are

A

acidic

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31
Q

Al 2 O3 and Al(OH) 3 are

A

amphoteric

32
Q

Acidity increases as electronegativity of central atom

A

increases

33
Q

For oxyacids and carboxylic acids: the more
electronegative the central atom, the higher the number
of oxygen (and other electronegative) atoms attached,
the

A

stronger the acid

34
Q

Kw of 25 celcius

A

1 * 10^-14

35
Q

pH=

A

-log(H)

36
Q

pOH=

A

-log(OH)

37
Q

(14 at 25 celcius) pKw=

A

pH+pOH

38
Q

Acidic pH

A

less than 7 (more H than OH)

39
Q

Basic pH

A

More than 7 (more OH than H)

40
Q

For pure water, [OH −] =

A

H+

41
Q

How to calculate the pH of a weak acid

A

1) Write acid dissociation reaction
2) Set-up ICE table to solve for [H +].
3) Solve for Ka. Weaker acids have smaller Ka (larger pKa)

42
Q

pKa=

A

-log(pKa)

43
Q

Calculate % ionization of a weak acid

A

% ionization = (HA ionized) / (HA initial) * 100
If in water, HA ionized = H+ equilibrium (Similar definition can be applied to %hydrolysis of a weak base)

44
Q

calculate pH or concentrations of ions for a polyprotic acid

A

Set up stepwise removal of one proton at a time (multiple ICE tables)
Write Ka for each ICE table

Amphoteric species are present in the polyprotic acid
solutions
If Ka1 > Ka2 by 3 orders of magnitude or more, the pH is
determined using Ka1 only

45
Q

Calculate pH of a weak base

A

Write the base hydrolysis reaction: B (aq) + H 2O () ⇌ OH − (aq) + HB + (aq)
* Weaker bases have smaller Kb (larger pKb)
* Set up ice table to solve for [OH−]
* pH=14-pOH

46
Q

Larger Ka, smaller

A

pKa

47
Q

Smaller Kb, larger

A

pKb

48
Q

For conjugate acid/base pair, Kw=

A

Ka * Kb

49
Q

Salts are strong electrolytes, so

A

they dissociate completely

50
Q

Calculate pH of a salt solution

A

Dissociate salt completely to obtain the correct
concentration of ions
* Write acid dissociation of cation, or base hydrolysis reaction of anion.
* Follow steps for weak acid or weak base equilibrium to solve for pH. Use Ka x K b = Kw for a conjugate acid/base pair to find the correct Keq

51
Q

If Ka is 10-5 or smaller, assume

A

negligible

52
Q

Larger Kb means stronger

A

base

53
Q

Strong acid + Strong base favors

A

products

54
Q

Strong acid + Weak base favors

A

products

55
Q

Weak acid + Strong base favors

A

products

56
Q

Weak acid + Weak base favors

A

Depends on Ka

57
Q

Larger Keq favors

A

products

58
Q

For cations, conjugate acid of weak base makes

A

weak acid, so acidic solution

59
Q

For cations, cations of group 1A/heavy 2A have

A

no pH effect

60
Q

For cations of transition metals, group 3A, light 2A

A

acidic solution

61
Q

For anions, conjugate base of strong acid have

A

no pH effect (HSO4- exception)

62
Q

For anions, conjugate base of weak acid has

A

weak base, so basic solution

63
Q

For anions, if has ionizable protons, it is

A

amphoteric, so pH effect depends on Ka and Kb (HSO4- exception, always acidic)

64
Q

Addition of common ion decreases

A

ionization

65
Q

Buffer definition

A

Solution that contains
* a weak acid and salt of its conjugate base
* a weak base and salt of its conjugate acid

66
Q

Make a buffer (2 methods)

A

Simply combine a weak acid and salt of its conjugate
base; or a weak base and salt of its conjugate acid

Use neutralization to combine a excess weak acid
with a strong base, or a excess weak base with a
strong acid.

67
Q

Optimal pH of a buffer =

A

pKa

68
Q

More concentrated buffer solution has

A

greater buffer capacity

69
Q

Use H-H equation to calculate pH of a buffer

A

pH = pKa + log([X-] / [HX])
* [X –] is the concentration of the conjugate base;
* [HX] is the concentration of the conjugate acid

70
Q

How to find pH of buffer mixture after addition of small amount of strong
acid or base.

A

Neutralization of the added strong acid or base: write balanced reaction and make ICF table of moles
Add strong acid:
X –(aq) + H +(aq) → HX(aq)
Add strong base:
HX(aq) + OH – (aq) → X – (aq) + H 2O(l)

  • Calculate concentration of HX and X – species present in the resultant solution, and use H-H equation to calculate the new pH
71
Q

On a titration curve, initial pH indicates

A

strength of acid or base

72
Q

On a titration curve, Equivalence point is when

A

stoichiometrically equivalent quantities of acid and base reacted (straight up/down)

73
Q

On a titration curve, Buffer mixture are produced between

A

initial and equivalence point

74
Q

On a titration curve, At half equivalence point pH=

A

= pKa

75
Q

Describe a polytropic titration curve

A

Polyprotic has multiple equivalence points, and multiple
buffer regions

76
Q

How to choose appropriate indicator

A

Indicator must change color within the vertical range of pH change

77
Q

How to find pH of acid/base mixture at any point during a titration

A
  • Make ICF table of moles for neutralization,
  • Calculate moles and concentration of species present in
    the final solution,
  • Identify whether the final solution is a buffer mixture, has
    a weak base or a weak acid only, or has excess strong acid
    or base, and find pH accordingly.

PSU Freshman (12 decks)

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