Chapter 15 Flashcards

(85 cards)

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
Oxy acid
Contains 3 elements, one of which is oxygen
26
HCl
Strong acid
27
HBr
Strong acid
28
HI
Strong acid
29
HNO3
Strong acid
30
HClO4
Strong acid
31
H2SO4
Strong acid
32
Weak acid
Weak electrolyte, partial ionization, vary in strength and percent ionization, donate a small amount of H+, coexist with their ions
33
Weak acids
Monoprotic Diprotic Polyprotic Any that aren’t the 6
34
Strong base
Strong electrolyte, complete dissociation or acceptance of H+
35
LiOH
Strong base
36
NaOH
Strong base
37
KOH
Strong base
38
Ca(OH)2
Strong base
39
Ba(OH)2
Strong base
40
Sr(OH)2
Strong base
41
Stronger A/B means
Weaker conjugate
42
Weak base
Small fraction of molecules accept H+, weak electrolyte
43
Binary acid strength
More polarized bond with H= weaker acid Increases across the period and down the group (molecules get larger)
44
Oxy acid strength
More electronegative atom = more strong acid More oxygens present = more strong acid
45
Ka
Acid ionization constant Measures acid strength Larger value = stronger acidity Strong acids lack a Ka
46
Base dissociation
One step
47
Kb
Base ionization constant Measures base strength Larger value = stronger basicity Strong bases lack a Kb
48
Neutralization reactions
Acid + base —> salt + water Basically the reaction of H+ and OH-
49
Salt from neutralization reaction
Cation of base, anion of acid
50
Overall ionic equation
Dissociable molecules are shown as ions, includes all spectator ions
51
Net ionic equation
Removing spectator ions from overall ionic equation
52
Kw
Ion product of water 1x10^-14
53
Kw of acids
H+ will be greater than OH-
54
Kw if based
H+ will be less than OH-
55
pH scale
Quantifying acidity and basicity From 0-14, may be outside range
56
Low pH
Acid
57
High pH
Base
58
pOH
Opposite of pH 14 - pH
59
Taking the log results in how many sig figs?
Sig figs= decimal places and vice versa
60
Weak acid equilibrium
Use an ICE table OH from water is negligible ( don’t worry about adding it to calculations)
61
Monoprotic acid
Dissociates in one step
62
Diprotic acid
Dissociates in 2 steps (one H+ at a time)
63
Polyprotic acid
Dissociates in more than 3 steps Theoretical
64
Triprotic acid
Dissociates in 3 steps
65
Dissociation of Polyprotic acids
Each step has its own Ka that is smaller than the previous step
66
Largest Ka value in step wise ionization determines
pH All other Ka values don’t affect pH greatly
67
Salts
Water soluble ionic compounds
68
Salts producing basic solutions
Cation if strong base and anion of weak acid Dissociation results in OH- in solution
69
Salts producing acidic solutions
Cation if weak base and anion of strong acid Dissociation results in H+ in solution
70
Each anion is a
Conjugate base to an acid
71
Stronger acid results in
A weaker conjugate base
72
Strong acid conjugate bases produce
pH neutral anions
73
Weak acid conjugate bases produce
Basic solutions
74
Strong acid + strong base
Neutral solution
75
Strong acid + weak base
Acidic solution
76
Weak acid + strong base
Basic solution
77
Weak acid + weak base
Neutral, acidic, or basic depending on Ka values
78
Salt solutions
Anion of acid Cation of base
79
Cations of strong bases produce
pH neutral solutions
80
Metal cations
Small charged molecules Weak acids
81
Lewis acid
Electron pair acceptor Empty orbital to accept electrons
82
Lewis acids and bases
Concerned with electrons, not protons (H+) Broadens scope of acids
83
Lewis base
Electron pair donor Has lone pair of electrons
84
Electrophile
Accepts electron pair Lewis acid
85
Nucleophile
Electron pair acceptor Lewis base