Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

AP Chemistry > Chapter 14 > Flashcards

Chapter 14 Flashcards

You may prefer our related Brainscape-certified flashcards:
AP® Chemistry flashcards Periodic Table flashcards Chemistry 101 flashcards Organic Chemistry 101 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
Q

Organic acids

A

acids containing the middle acidic carboxyl group

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
26
Q

Organic acids are generally?

A

weak acids with equilibrium to the left

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
27
Q

Water can be both a _______ because ________?

A

acid and base because it self-ionizes

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
28
Q

Ion product constant

A

a dissociation constant that we use whenever we are working with an acid/base/or water

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
29
Q

Water is our baseline for any pH situation because?

A

the pH is 7 due to equilibrium between the Hydrogen and Hydroxide ion concentration

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
30
Q

What is typically temperature we measure ion-product constant at?

A

25 degrees Celsius

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
31
Q

Amphoteric

A

able to react both as a base and as an acid

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
32
Q

pH+ and pOH- adds to?

A

1.0 x 10^-14

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
33
Q

From an ion point of view neutral solutions are at equilibrium with?

A

an equal concentration of Hydrogen and Hydroxide Ions

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
34
Q

acids have a greater?

A

Hydrogen ion concentration

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
35
Q

bases have a greater?

A

Hydroxide ion concentration or an absence of hydrogen ions

36
Q

Why do bases have an absence of hydrogen ions?

A

the base has accepted them and removed them from solution

37
Q

Acids have more hydrogen ions than water so the pH is?

A

less than 7

38
Q

Bases have an absence of Hydrogen ions so the pH is?

A

greater than 7

39
Q

Each change in pH is a _____ magnitude in each direction.

A

x10

40
Q

Measurement of the strength of an acid is based on?

A

-identity of the acid
-If Kₐ is given

41
Q

Increase in temperature, causes?

A

increase in Kw

42
Q

What is Kw at 25 degrees Celsius?

A

1.0 x 10-14

43
Q

At high concentrations of strong acids, the?

A

auto ionization of water is negligible

44
Q

the auto ionization of water

A

a proton is transferred from one water molecule to another to produce a hydronium ion and hydroxide ion,

44
Q

For strong acids, the assumption we always make is?

A

the acid has completely ionized.

45
Q

Weak acids form?

A

strong conjugate bases

46
Q

If % dissociation is above 5% we should use?

A

quadratic formula

47
Q

% dissociation increases as _____?

A

acid is diluted

48
Q

Strong base examples

A

-group 1 metal hydroxids
-group 2 metal hydroxides

49
Q

group 2 metal hydroxides are?

A

less soluble than group 1, allowing them to be used as antacids.

50
Q

group 2 metal hydroxides can be used as?

A

antacids

51
Q

antacids

A

neutralize the acid in your stomach to relieve indigestion and heartburn

52
Q

weak bases

A

-ammoia and other covalent bases
-compounds that have low Kb values

53
Q

base dissociation constant symbol

A

Kb

54
Q

acid dissociation constant symbol

A

Ka

55
Q

polyprotic acid

A

An acid that contains more than one acidic hydrogen atom

56
Q

In polyprotic acids they can only lose?

A

one hydrogen atom per round

57
Q

Polyprotic acids example.

A

Sulfuric (1): H₂SO₄
Sulfuric (2): HSO₄

58
Q

Polyprotic acids have no effect on?

A

speed or strength

59
Q

In polyprotic acids, no matter what use?

A

the first reaction as the base for pH

60
Q

Why do we use the first reaction from polyprotic acids?

A

where the majority of the hydrogens come from.

61
Q

If a salt is made of the cation of a strong base and the anion of a strong acid then?

A

it will have no effect on pH when dissolved in water because it is weak

62
Q

Cations of strong bases

A

Na⁺, K⁺

63
Q

Cations of strong bases and anions of strong acids have?

A

no affinity for hydrogen ions

64
Q

anions of strong acids

A

Cl⁻, NO3⁻

65
Q

In both cases if cation strong base or anion strong acid is present pH?

A

does not change due to presence of these ions

66
Q

salts that produce basic solutions

A

salt whose cation has neutral properties and whose anion is the conjugate base of a weak acids

67
Q

In salts that produce basic solutions the conjugate base is _____ and comes from where?

A

strong and from the dissociation of the weak acid.

68
Q

salts that produce acidic solutions

A

situation where the cation conjugate acid is from a weak base and anion is neutral.

69
Q

salts that produce acidic solutions is due to?

A

the dissociation of a weak base that produces strong conjugate acid ion

70
Q

Salts that produce acidic solutions are also found when a salt?

A

dissociates into a highly charged metallic ion such as Al⁺³

71
Q

In salts that produce acid solutions, the highly charged cation or conjugate acid?

A

polarizes water and one hydrogen from the water molecule will become H⁺.

72
Q

Salts with acidic and basic ions (acidic)

A

If Ka ion greater than Kb ion, the solution will be acidic

73
Q

Salts with acidic and basic ions (basic)

A

If Kb ion is greater than Ka ion,the solution will be basic.

74
Q

Salts with acidic and basic ions (neutral)

A

If Kb ion is the same as Ka ion, the solution will be neutral.

75
Q

conjugate acid base pair example

A

-H2O (base) and H3O (conjugate acid)
-HA (acid) and A (conjugate base)

76
Q

conjugate acid base pair

A

consists of two substances related to each other by the donating and accepting of a single proton.

77
Q

calculation for the pH of a typical weak polyprotic acids is identical to?

A

a solution of a weak monoprotic acid

78
Q

sulfuric acid is unique in being?

A

a strong acid in its first dissociation step and a weak acids in its second step.

79
Q

If cation reacts and anions does not the salt is?

A

acidic

80
Q

If the cation does not react and the anion does the salt is?

A

basic

81
Q

for oxyacids an increase in electronegativity does what to acid strength?

A

increase

82
Q

for oxyacids an decrease in electronegativity does what to acid strength?

A

decrease

83
Q

decrease in bond strength does what to acid strength?

A

Increase

84
Q

increase in bond strength does what to acid strength?

A

decrease

85
Q

equilibrium favors the side with the?

A

weak acids and base

AP Chemistry (16 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions