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Chemistry 115 > Chapter 15 > Flashcards

Chapter 15 Flashcards

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1
Q

Vital to biological systems normal function

A

Acid-base balance

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2
Q

Regulated by the reversible chemical reactions

A

The amount of acid-base in a system

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3
Q

Arrhenius acid

A

Dissociate in water to produce H+

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4
Q

Dissociate in water to produce H+

A

Arrhenius acid

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5
Q

Arrhenius base

A

Ionizes or dissociates in water to produce OH-

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6
Q

Ionizes or dissociates in water to produce OH-

A

Arrhenius base

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7
Q

Arrhenius acid-base reactions

A

Cation from base plus anion of acid forms salt in water (from OH + H)

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8
Q

Cation from base plus anion of acid forms salt in water (from OH + H)

A

Arrhenius acid-base reaction

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9
Q

Problems with Arrhenius theory

A

Doesn’t explain basicity/acidity of molecules or compounds lacking OH- or those lacking H+
Can’t explain acid-base reactions that take place outside aqueous solution

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10
Q

Brønsted-Lowry acid

A

Proton (H+) donors

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11
Q

Proton (H+) donors

A

Brønsted-Lowry acid

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12
Q

Brønsted-Lowry base

A

Proton (H+) acceptors

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13
Q

Proton (H+) acceptors

A

Brønsted-Lowry base

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14
Q

Amphoteric substance

A

Acts as an acid or a base, water is most common

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15
Q

Acts as an acid or a base, water is most common

A

Amphoteric substance

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16
Q

Nonmetal oxides

A

Form acids when placed in water
Ex: SO2, SO3, CO2 (all gases)

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17
Q

Conjugate acid-base pairs

A

Exist on the other side of equilibrium, opposite of left hand side, only possible in Brønsted-Lowery theory, not Arrhenius

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18
Q

Conjugate acid

A

From original base, add H+

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19
Q

From original base, add H+

A

Conjugate acid

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20
Q

Conjugate base

A

From original acid, minus H+

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21
Q

From original acid, minus H+

A

Conjugate base

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22
Q

Strong acid

A

Strong electrolyte, complete ionization, more willing to donate H+

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23
Q

Strong acids

A

3 binary, 3 oxy acids
5 monoprotic, 1diprotic

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24
Q

Binary acid

A

Consists of only 2 elements

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25
Q

Oxy acid

A

Contains 3 elements, one of which is oxygen

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26
Q

HCl

A

Strong acid

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27
Q

HBr

A

Strong acid

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28
Q

HI

A

Strong acid

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29
Q

HNO3

A

Strong acid

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30
Q

HClO4

A

Strong acid

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31
Q

H2SO4

A

Strong acid

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32
Q

Weak acid

A

Weak electrolyte, partial ionization, vary in strength and percent ionization, donate a small amount of H+, coexist with their ions

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33
Q

Weak acids

A

Monoprotic
Diprotic
Polyprotic
Any that aren’t the 6

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34
Q

Strong base

A

Strong electrolyte, complete dissociation or acceptance of H+

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35
Q

LiOH

A

Strong base

36
Q

NaOH

A

Strong base

37
Q

KOH

A

Strong base

38
Q

Ca(OH)2

A

Strong base

39
Q

Ba(OH)2

A

Strong base

40
Q

Sr(OH)2

A

Strong base

41
Q

Stronger A/B means

A

Weaker conjugate

42
Q

Weak base

A

Small fraction of molecules accept H+, weak electrolyte

43
Q

Binary acid strength

A

More polarized bond with H= weaker acid
Increases across the period and down the group (molecules get larger)

44
Q

Oxy acid strength

A

More electronegative atom = more strong acid
More oxygens present = more strong acid

45
Q

Ka

A

Acid ionization constant
Measures acid strength
Larger value = stronger acidity
Strong acids lack a Ka

46
Q

Base dissociation

A

One step

47
Q

Kb

A

Base ionization constant
Measures base strength
Larger value = stronger basicity
Strong bases lack a Kb

48
Q

Neutralization reactions

A

Acid + base —> salt + water
Basically the reaction of H+ and OH-

49
Q

Salt from neutralization reaction

A

Cation of base, anion of acid

50
Q

Overall ionic equation

A

Dissociable molecules are shown as ions, includes all spectator ions

51
Q

Net ionic equation

A

Removing spectator ions from overall ionic equation

52
Q

Kw

A

Ion product of water
1x10^-14

53
Q

Kw of acids

A

H+ will be greater than OH-

54
Q

Kw if based

A

H+ will be less than OH-

55
Q

pH scale

A

Quantifying acidity and basicity
From 0-14, may be outside range

56
Q

Low pH

A

Acid

57
Q

High pH

A

Base

58
Q

pOH

A

Opposite of pH
14 - pH

59
Q

Taking the log results in how many sig figs?

A

Sig figs= decimal places and vice versa

60
Q

Weak acid equilibrium

A

Use an ICE table
OH from water is negligible ( don’t worry about adding it to calculations)

61
Q

Monoprotic acid

A

Dissociates in one step

62
Q

Diprotic acid

A

Dissociates in 2 steps (one H+ at a time)

63
Q

Polyprotic acid

A

Dissociates in more than 3 steps
Theoretical

64
Q

Triprotic acid

A

Dissociates in 3 steps

65
Q

Dissociation of Polyprotic acids

A

Each step has its own Ka that is smaller than the previous step

66
Q

Largest Ka value in step wise ionization determines

A

pH
All other Ka values don’t affect pH greatly

67
Q

Salts

A

Water soluble ionic compounds

68
Q

Salts producing basic solutions

A

Cation if strong base and anion of weak acid
Dissociation results in OH- in solution

69
Q

Salts producing acidic solutions

A

Cation if weak base and anion of strong acid
Dissociation results in H+ in solution

70
Q

Each anion is a

A

Conjugate base to an acid

71
Q

Stronger acid results in

A

A weaker conjugate base

72
Q

Strong acid conjugate bases produce

A

pH neutral anions

73
Q

Weak acid conjugate bases produce

A

Basic solutions

74
Q

Strong acid + strong base

A

Neutral solution

75
Q

Strong acid + weak base

A

Acidic solution

76
Q

Weak acid + strong base

A

Basic solution

77
Q

Weak acid + weak base

A

Neutral, acidic, or basic depending on Ka values

78
Q

Salt solutions

A

Anion of acid
Cation of base

79
Q

Cations of strong bases produce

A

pH neutral solutions

80
Q

Metal cations

A

Small charged molecules
Weak acids

81
Q

Lewis acid

A

Electron pair acceptor
Empty orbital to accept electrons

82
Q

Lewis acids and bases

A

Concerned with electrons, not protons (H+)
Broadens scope of acids

83
Q

Lewis base

A

Electron pair donor
Has lone pair of electrons

84
Q

Electrophile

A

Accepts electron pair
Lewis acid

85
Q

Nucleophile

A

Electron pair acceptor
Lewis base

Chemistry 115 (8 decks)

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