Brainscape's Knowledge GenomeTM


Top Flashcards (Certified)
All Flashcards

AP Chemistry > Chapter 14 > Flashcards

Chapter 14 Flashcards

1
Q

Arrhenius Model acids

A

release hydrogen ions when placed in water

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

The Arrhenius Model applies only to?

A

aqueous solutions and allows for only one type of base

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

Arrhenius Model bases

A

release hydroxide ions when placed in an aqueous solution

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

Bronsted-Lowry model acids

A

proton donors (hydrogen ions)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

Bronsted-Lowry model bases

A

proton acceptors (accepts hydrogen ions)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

Conjugate acids

A

what the base becomes on the product side of a reaction when the base has accepted the proton.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

Conjugate base

A

what the acid becomes on the product side of the reaction when the acid has donated its proton.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

acid dissociation constant refers to?

A

the dissociation or ionization of an acid.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

In the dissociation what is not included and why?

A

water because in dilute solutions the concentration of water is high and changes very little.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

For strong acids the equilibrium lies so far to?

A

the right that the acid cannot be accurately measured and cannot calculate of Kₐ.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

Strong acids

A

acids with a large Kₐ value

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

strong acids equilibrium lies to?

A

the right

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

a strong acid will yield a?

A

weak conjugate base (low proton affinity)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

Common strong acids

A

HCl, H2SO4, H3PO4

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

With strong acids we assume?

A

they undergo complete dissociation so very little of the original strong acid is left.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

Weak acid

A

acids that do not ionize/dissociate completely with a small Ka value

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

Weak acids will yield a?

A

strong conjugate bases (high proton affinity)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

in weak acids equilibrium lies?

A

to the left

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

In weak acids, most of the acid remains?

A

in an unionized state in solution

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

If given a Kₐ value, the acid is?

A

weak

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

Monoprotic

A

1 acidic proton

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

Diprotic

A

2 acidic donors

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

Triprotic

A

3 acidic donors

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
24
Q

Oxyacids

A

acids in which the acidic proton is attached to an oxygen atom

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
25
Organic acids
acids containing the middle acidic carboxyl group
26
Organic acids are generally?
weak acids with equilibrium to the left
27
Water can be both a _______ because ________?
acid and base because it self-ionizes
28
Ion product constant
a dissociation constant that we use whenever we are working with an acid/base/or water
29
Water is our baseline for any pH situation because?
the pH is 7 due to equilibrium between the Hydrogen and Hydroxide ion concentration
30
What is typically temperature we measure ion-product constant at?
25 degrees Celsius
31
Amphoteric
able to react both as a base and as an acid
32
pH+ and pOH- adds to?
1.0 x 10^-14
33
From an ion point of view neutral solutions are at equilibrium with?
an equal concentration of Hydrogen and Hydroxide Ions
34
acids have a greater?
Hydrogen ion concentration
35
bases have a greater?
Hydroxide ion concentration or an absence of hydrogen ions
36
Why do bases have an absence of hydrogen ions?
the base has accepted them and removed them from solution
37
Acids have more hydrogen ions than water so the pH is?
less than 7
38
Bases have an absence of Hydrogen ions so the pH is?
greater than 7
39
Each change in pH is a _____ magnitude in each direction.
x10
40
Measurement of the strength of an acid is based on?
-identity of the acid -If Kₐ is given
41
Increase in temperature, causes?
increase in Kw
42
What is Kw at 25 degrees Celsius?
1.0 x 10-14
43
At high concentrations of strong acids, the?
auto ionization of water is negligible
44
the auto ionization of water
a proton is transferred from one water molecule to another to produce a hydronium ion and hydroxide ion,
44
For strong acids, the assumption we always make is?
the acid has completely ionized.
45
Weak acids form?
strong conjugate bases
46
If % dissociation is above 5% we should use?
quadratic formula
47
% dissociation increases as _____?
acid is diluted
48
Strong base examples
-group 1 metal hydroxids -group 2 metal hydroxides
49
group 2 metal hydroxides are?
less soluble than group 1, allowing them to be used as antacids.
50
group 2 metal hydroxides can be used as?
antacids
51
antacids
neutralize the acid in your stomach to relieve indigestion and heartburn
52
weak bases
-ammoia and other covalent bases -compounds that have low Kb values
53
base dissociation constant symbol
Kb
54
acid dissociation constant symbol
Ka
55
polyprotic acid
An acid that contains more than one acidic hydrogen atom
56
In polyprotic acids they can only lose?
one hydrogen atom per round
57
Polyprotic acids example.
Sulfuric (1): H₂SO₄ Sulfuric (2): HSO₄
58
Polyprotic acids have no effect on?
speed or strength
59
In polyprotic acids, no matter what use?
the first reaction as the base for pH
60
Why do we use the first reaction from polyprotic acids?
where the majority of the hydrogens come from.
61
If a salt is made of the cation of a strong base and the anion of a strong acid then?
it will have no effect on pH when dissolved in water because it is weak
62
Cations of strong bases
Na⁺, K⁺
63
Cations of strong bases and anions of strong acids have?
no affinity for hydrogen ions
64
anions of strong acids
Cl⁻, NO3⁻
65
In both cases if cation strong base or anion strong acid is present pH?
does not change due to presence of these ions
66
salts that produce basic solutions
salt whose cation has neutral properties and whose anion is the conjugate base of a weak acids
67
In salts that produce basic solutions the conjugate base is _____ and comes from where?
strong and from the dissociation of the weak acid.
68
salts that produce acidic solutions
situation where the cation conjugate acid is from a weak base and anion is neutral.
69
salts that produce acidic solutions is due to?
the dissociation of a weak base that produces strong conjugate acid ion
70
Salts that produce acidic solutions are also found when a salt?
dissociates into a highly charged metallic ion such as Al⁺³
71
In salts that produce acid solutions, the highly charged cation or conjugate acid?
polarizes water and one hydrogen from the water molecule will become H⁺.
72
Salts with acidic and basic ions (acidic)
If Ka ion greater than Kb ion, the solution will be acidic
73
Salts with acidic and basic ions (basic)
If Kb ion is greater than Ka ion,the solution will be basic.
74
Salts with acidic and basic ions (neutral)
If Kb ion is the same as Ka ion, the solution will be neutral.
75
conjugate acid base pair example
-H2O (base) and H3O (conjugate acid) -HA (acid) and A (conjugate base)
76
conjugate acid base pair
consists of two substances related to each other by the donating and accepting of a single proton.
77
calculation for the pH of a typical weak polyprotic acids is identical to?
a solution of a weak monoprotic acid
78
sulfuric acid is unique in being?
a strong acid in its first dissociation step and a weak acids in its second step.
79
If cation reacts and anions does not the salt is?
acidic
80
If the cation does not react and the anion does the salt is?
basic
81
for oxyacids an increase in electronegativity does what to acid strength?
increase
82
for oxyacids an decrease in electronegativity does what to acid strength?
decrease
83
decrease in bond strength does what to acid strength?
Increase
84
increase in bond strength does what to acid strength?
decrease
85
equilibrium favors the side with the?
weak acids and base

AP Chemistry (16 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2025 Bold Learning Solutions. Terms and Conditions