Brainscape's Knowledge GenomeTM

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


See full index

CHEM 1154 > Chapter 15 > Flashcards

Chapter 15 Flashcards

You may prefer our related Brainscape-certified flashcards:
AP® Chemistry flashcards Periodic Table flashcards Chemistry 101 flashcards Organic Chemistry 101 flashcards
1
Q

Define carboxylic acid

A

the Organic acid containing the functional group -COOH

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

What is the Arrhenius definition of an acid?

A

A substance that produces H+ ions in aqueous solution

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

What is the Arrhenius definition of a base?

A

A substance that produces OH- ions in aqueous solution

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

Define Arrhenius definition

A

The definitions of an acid as a substance that produces H+ ions in aqueous solution and a base as a substance that produces OH- ions in an aqueous solution

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

Define hydronium ion

A

H₃0⁺, the ion formed from the association of a water molecule with an H+ ion donated by an acid

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

Can H+ and H₃0⁺ be used interchangeably?

A

Yes

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

Do H+ ions associate with water molecules to form hydronium ions?

A

Yes! Always!

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

When covalently bonded acids are dissolved in water they _____. When ionically bonded bases are dissolved in water they _____.

A

ionize

dissociate

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

Under the Arrhenius definition the combination of acid and base results in ____ because…?

A

water because H+ and OH- naturally combine to form neutral water

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

Define Brønsted-Lowry definition

A

The definitions of an acid as a proton (H+ ion) donor and a base as a proton acceptor.

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

What is the Brønsted-Lowry definition of an acid?

A

A proton donor (where a proton is an H+ ion)

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

What is the Brønsted-Lowry definition of a base?

A

A proton acceptor (where a proton is an H+ ion)

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

Define amphoteric

A

Able to act as either a base or an acid (like water)

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

Define conjugate acid-base pair

A

Two substance related to each other by the transfer of a proton

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

Define conjugate acid

A

Any base to which a proton has been added

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

Define conjugate base

A

Any acid from which a proton has been removed

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

A(n) ____ accepts a proton and becomes a conjugate ____.

A

base

acid

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

A(n) ____ donates a proton and becomes a conjugate ____.

A

acid

base

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

Define strong acid

A

An acid that complete;y ionizes in solution

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

A ____ acid completely ionizes in solution.

A

strong

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

A _____ acid only partially ionizes in solution.

A

weak

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

The degree to which an acid is strong or weak depends on …?

A

The attraction between the anion of the acid (the conjugate base) and the hydrogen ion, relative to the attractions of these ions to water

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

In general, the stronger the acid, the ____ the conjugate base and vice versa

A

weaker

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

If the the forward reaction (that of the acid) has a high tendency to occur, then the reverse reaction (that of the conjugate base) has a ____ tendency to occur

A

low

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
25
Q

Define acid ionization constant (Ka)

A

The equilibrium constant for the ionization of a weak acid; used to compare the relative strengths of weak acids

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

How can we quantify the relative strengths of weak acids?

A

Using the acid ionization constant (Ka)

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

The ____ _____ ___ is the equilibrium constant for the ionization reaction of a weak acid

A

acid ionization constant

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

A ____ base is a base that completely dissociates in solution

A

strong

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

Most strong bases are ____ ____ from group 1 or 2

A

metal hydroxides

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

What groups are most strong bases formed from (in the form of metal hydroxides)?

A

Group 1 or 2

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

Define weak base

A

A base that only partially ionizes in water

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

The most common weak bases produce OH- by …?

A

accepting a proton from water, ionizing water to form OH-

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

Define base ionization constant (Kb)

A

The equilibrium constant for the ionization reaction of a weak base; used to compare the relative strength of weak bases

34
Q

The smaller the value of Kb, the _____ the base

A

weaker

35
Q

Define autoionization

A

The process by which water acts as an acid and a base with itself.

36
Q

Define ion product constant for water (Kw)

A

The equilibrium constant for the auto ionization of water

37
Q

What is the ion product constant for water alternatively called?

A

dissociation constant for water

38
Q

What is the value of Kw at 25ºC?

A

1.0 x 10⁻¹⁴

39
Q

define neutral

A

The state of a solution where the concentrations of H₃0⁺ and OH- are equal

40
Q

Define acidic solution

A

a solution containing an acid that creates additional H₃0⁺ ions, causing [H₃0⁺] to increase

41
Q

If the concentration of H₃0⁺ is greater than the concentration of OH- is [H₃0⁺][OH⁻] = Kw = 1.0 x 10⁻¹⁴ still true?

A

Yes! This is always true!

42
Q

If the concentration of H₃0⁺ is less than the concentration of OH- is [H₃0⁺][OH⁻] = Kw = 1.0 x 10⁻¹⁴ still true?

A

Yes! This is always true!

43
Q

In an acidic solution [H₃0⁺] is ___ than [OH⁻].

A

greater

44
Q

In a basic solution [H₃0⁺] is ___ than [OH⁻].

A

less

45
Q

Define basic solution

A

A solution containing a base that creates additional OH- ions, causing the [OH-] to increase

46
Q

A(n) ____ solution contains [H₃0⁺] = [OH⁻] = 1.0 x 10⁻⁷ mol/L (at 25ºC)

A

neutral

47
Q

A(n) ____ solution contains [H₃0⁺] > [OH⁻]

A

acidic

48
Q

A(n) ____ solution contains [H₃0⁺] < [OH⁻]

A

basic

49
Q

In all ____ solutions both H₃0⁺ and OH⁻ are present, with [H₃0⁺][OH⁻] = Kw = 1.0 x 10⁻¹⁴ (at 25ºC)

A

aqueous

50
Q

Define pH

A

The negative log of the concentration of H₃0⁺ in solution; the pH sclae is a compact way to specify the acidity of solutions

51
Q

pH =…?

A

-log[H₃0⁺]

52
Q

In general at 25ºC if pH is less than 7 the solution is ____.

A

acidic

53
Q

In general at 25ºC if pH is greater than 7 the solution is ____.

A

basic

54
Q

In general at 25ºC if pH is equal than 7 the solution is ____.

A

neutral

55
Q

pOH=…?

A

-log[OH⁻]

56
Q

On the pOH scale a pOH of less than 7 is ___ and pOH of greater than 7 is _____.

A

basic

acidic

57
Q

pH + pOH = …? (at 25ºC)

A

14.00

58
Q

The pKa of a weak acid is another way to quantify its _____.

A

strength

59
Q

The smaller the value of pKa, the _____ the acid.

A

stronger

60
Q

pKa = …?

A

-log Ka

61
Q

Why can the autoionization of water be ignored in most strong acid and weak acid solutions?

A

Because the autoionization of water produces even less H₃0⁺ than in pure water

62
Q

The concentration of H₃0⁺ in a strong acid solution is simply equal to the concentration of the ____ ____

A

strong acid

63
Q

Define percent ionization

A

The concentration of ionized acid in a solution divided by the initial concentration of acid, multiplied by 100%.

64
Q

The equilibrium H₃0⁺ concentration of a weak acid ___ with increasing initial concentration of acid.

A

increases

65
Q

The percent ionization of a weak acid ____ with increasing concentration of the acid .

A

decreases

66
Q

In general an anion that is the conjugate base of a weak acid is itself a ____ ____.

A

weak base

67
Q

In general an anion that is the conjugate base of a strong acid is ____-____.

A

pH-neutral

68
Q

Ka x Kb = …?

A

Kw

69
Q

Anions can act as weak ____.

A

Bases

70
Q

Cations can act as weak ____.

A

Acids

71
Q

What are the three main categories cations can be divided into?

A
  1. Cations that are the counterions of strong bases
  2. Cations that are the conjugate acids of weak bases
  3. Cations that are small, highly charged metals.
72
Q

Why Is HF a weak acid?

A

Because the F- ion has a significant affinity for H+ ions and so when F- is in water it takes the H+ off the water (acts as a weak base).

73
Q

Strong bases generally contain ____ ions and a _____

A

hydroxide

counterion

74
Q

Do counterions (from a strong base) interact with water? How?

A

Yes through ion-dipole forces, but THEY DO NOT IONIZE WATER and therefore they do not contribute to the acidity or basicity of the solution

75
Q

In general cations that are counterions of strong bases are themselves ____ _____

A

pH neutral

76
Q

In general, a cation that is a conjugate acid of a weak base is a weak ____

A

acid

77
Q

Small highly charged metal cations form weakly ____- solutions

A

acidic

78
Q

Salts in which neither the cation nor the anion acts as a base or an acid form ____ ____ solutions

A

pH neutral

79
Q

Salts in which the cation does not act as an acid and the anion acts as a base form ____ solutions

A

basic

80
Q

Salts in which the cation acts as an acid and the anion does not act as a base form ____ solutions

A

acidic

81
Q

Salts in which the cation acts as an acid and the anion acts as a base form solutions in which the pH depends on the relative strengths of the ____ and the _____

A

acid

base

CHEM 1154 (15 decks)

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