Brainscape's Knowledge GenomeTM

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


See full index

Chemistry Unit 2 > Acids and Bases > Flashcards

Acids and Bases Flashcards

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

Properties of acids (acidic solutions)?

A
  • sour/bitter
  • corrosive
  • neutralise bases
  • pH < 7
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

Properties of bases (alkaline solutions)?

A
  • slippery
  • corrosive
  • neutralise acids
  • pH > 7
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

properties of Neutral solutions?

A
  • pH = 7
  • Indicators can be used to determine if a solution is acid, basic or neutral.
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

what are Lab acids?

A

HCl, HNO3, H2SO4

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

Bronsted-Lowry theory of acids?

A

“An acid is a substance that is able to donate a proton/hydrogen ion (H+) to another substance.”

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

conjugate base of HCl ?

A

Cl-

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

conjugate base of HNO3 ?

A

NO3-

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

conjugate base of H2SO4?

A

HSO4-

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

Lab bases?

A

NaOH, KOH, NH3

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

Bronsted-Lowry theory of base?

A

“A base is a substance that is able to accept a proton/hydrogen ion (H+) from another substance.”

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

conjugate acid of NH3?

A

NH4+

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

conjugate acid of HCO3- ?

A

H2CO3

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

conjugate acid of OH-?

A

H2O

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

what are Acid-base reactions often called?

A

Often called “neutralisation” reactions

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

what pattern do Acid-base reactions follow?

A

Follow the pattern: acid + base → salt + water
eg. HCl + NaOH → NaCl + H2O

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

what is another version of the acid-base reactions?

A

Bronsted-Lowry acids and bases

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

is water an acid or a base?

A

Water is amphiprotic. How it behaves will depend on what its mixed with.

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

define Amphiprotic

A

species that can act as both an acid and a base

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

what is H3O+?

A

hydronium ion

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

what is OH- ?

A

hydroxide ion

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

what do Strong acids do?

A

donate all available protons

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

Strong Lab acids?

A

HCl, HNO3, H2SO4

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

what are the two types of strong lab acids?

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

what is Monoprotic?

A

1 x H+ to donate

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

what is diprotic?

A

2 x H+ to donate

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

strong acids features?

A
  • Reactions go to completion
  • There is no acid (eg HCl) in hydrochloric acid solution
  • H3O+ (hydronium ion) is what identifies an acidic solution
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
27
Q

what are Weak acids?

A

donate only a few of the available protons

28
Q

what are some weak acids?

A

Most other acids that are not strong acids, carboxylic acids, CH3COOH

29
Q

weak acids features?

A
  • Reactions are not complete
  • All species present
  • H3O+ still identifies acidic solution
30
Q

what are Strong bases?

A

accept all available protons

31
Q

strong lab bases?

A

NaOH, KOH, Cu(OH)2

32
Q

strong bases features?

A
  • Reactions go to completion
  • Water over the arrow
  • OH- (hydroxide ion) is what identifies an basic solution
33
Q

what are Weak bases?

A

accept only a few of the available protons

34
Q

lab weak bases?

A

Most other bases are weak eg. NH3, carbonates

35
Q

weak bases features?

A
  • Reactions are not complete
  • All species present
  • OH- still identifies basic solution
36
Q

how does water react with itself?

A
  • Water is amphiprotic (can act as an acid or a base).
    H2O + H2O ⇄ OH- + H3O+
  • Water reacts with itself, you will find H2O, OH- and H3O+ species in pure water.
37
Q

what is water reacting with itself called?

A

This is called the self ionisation (or autodissociation) of water.

38
Q

what type of acid/base is water and what does this mean?

A

Water is a weak acid and a weak base.
- Water donates only a few available protons/H+ ions
- Water accepts only a few available protons/H+ ions
This actually only occurs very very rarely!

39
Q

what makes water neutral in water reaction?

A

[H3O+] = [OH-] This makes water neutral.

40
Q

what is the concentration of H3O+ and OH- of water at 25 degrees?

A

[H3O+] = 1 x 10-7 molL-1
[OH-] = 1 x 10-7 molL-1
Kw = [H3O+] x [OH-] = 1 x 10-14 molL-1

41
Q

what makes a solution acidic?

A

Since [H3O+] > [OH-] solution is acidic.

42
Q

when does water react with itself in equations?

A

almost always as a second step when no more acid/base can be reacted with (in solutions)

43
Q

strong vs weak acids Electrical conductivity?

A

Strong acid - Higher
Weak acid - Lower

44
Q

strong vs weak acids Rate of reaction with metals, carbonates?

A

Strong acid - Higher
Weak acid - Lower

45
Q

strong vs weak acids pH?

A

Strong acid - Lower (0 - 3)
Weak acid - Higher (4 - 6.9)

46
Q

relationship between acids and their conjugate bases?

A

a strong acid will always have a weak conjugate base and vice versa

47
Q

Relationships in water based solutions of acids and bases?

A

Pure water at 250C:
[H3O+] = [OH-]

An acidic solution at 250C:
[H3O+] > [OH-]

An basic/alkaline solution at 250C:
[H3O+] < [OH-]

48
Q

what does Kw equal?

A

Kw = [H3O+] x [OH-] = 1 x 10-14 molL-1

49
Q

what is pH?

A

pH is actually a measure of the [H3O+] in a solution

50
Q

relationships of pH?

A

↑ [H3O+] ∴ ↓ pH ↓ [H3O+] ∴ ↑ pH

51
Q

how is pH calculated?

A

pH = - log[H3O+]

52
Q

For any strong acid solution equation?

A

HA + H2O → A- + H3O+

53
Q

what happens to pH in strong acid solutions?

A

Notice that HA : H3O+ is 1 : 1
This means that [HA] = [H3O+] given that strong acids donate their H+/proton very very effectively

NB: there is a tiny bit extra H3O+ due to self ionisation of water but we will ignore it as it is so small. There is also traces of OH-.

54
Q

how do calculate [H3O+] from pH?

A

[H3O+] = 10-pH

55
Q

pattern of Acid + Oxide/Hydroxide (base) reaction?

A

acid + oxide/hydroxide → salt + water

56
Q

what are Oxides and hydroxides?

A

Oxides and hydroxides are bases

57
Q

Observations of Acid + Oxide/Hydroxide (base) reaction?

A

Observations will vary depending on the concentration of the solutions or state of chemicals.

58
Q

pattern of Acid + Carbonate (base) reaction?

A

acid + carbonate → salt + carbon dioxide + water

59
Q

what are Carbonates and bicarbonates?

A

bases

60
Q

Observations of Acid + Carbonate (base) reaction?

A

Bubbles (due to CO2(g))

61
Q

what do full equations show?

A

Full equations show all species present in a reaction (both ionic and covalent species), irrespective of their state.

62
Q

what do ionic equations show?

A

Ionic equations are simplified versions of an equation.
Ionic equations do not include spectator ions.

63
Q

what are spectator ions?

A

Spectator ions are ions that stay in the same state (often (aq)) throughout the reaction, hence do not form part of a new product.

64
Q

what are Acid + base reactions often called?

A

Acid + base reactions are often called neutralisation reactions.

65
Q

Do acids and bases cancel?

A

Acids and bases “cancel” each other out.
So given: acid + base → salt + water
The products of an acid + base reaction must be neutral, right?
Meaning pH = 7
Well sometimes!

66
Q

Do all acids and bases cancel?

A
  • Acid + base reactions involving either a weak acid and/or a weak base do not result in neutral products with a pH = 7
  • Even if you use the correct ratio of acid to base (eg. concentrations, volumes and moles).
67
Q

why do weak acid/base reactions never neutralise?

A

This occurs because the salt product (eg. NH4Cl) has either acidic or basic characteristics itself.

Chemistry Unit 2 (5 decks)

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