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Chemistry module 6 > MOD6-INQ1 > Flashcards

MOD6-INQ1 Flashcards

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1
Q

What colour does acid change litmus paper to

A

It’s turns blue litmus red

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2
Q

Why does H+ ions join with H30+ ions so quickly in reactions

A

A H+ ion is a bare proton with the charge of +1 making it extremely concentrated so in water it would combine with a water molecule to form a more stable molecule - H3O+

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3
Q

A base that dissolves in water is also known as

A

Alkalis

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4
Q

Which group base is all soluble

A

Group 1

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5
Q

Acid strength

A

The extent of ionisation or dissociation in water

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6
Q

Name 5 common strong acids

A

HCl, HBr, HI, H2SO4, HNO3

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7
Q

Name 4 strong bases

A

NaOH, KOH, Ca(OH)2, Ba(OH)2

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8
Q

Which group bases are strong but poorly soluble

A

Group 2

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9
Q

Many bases are _____ in ionic compounds

A

Anions

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10
Q

Because weak bases are anions in ionic compounds what must you do before showing it reacting with water

A

Dissociate the weak base

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11
Q

How is acid strength and concentration different

A

Acid strength refers to the extent of ionisation while acid concentration is the amount of acid in a given volume

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12
Q

What is generally the number which we consider as a concentrated acid

A

10M

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13
Q

What does Ka represent

A

Ka represent the position of the equilibrium for the dissociation of an acid in water

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14
Q

When talking about Ka reactions, is it dynamic or static reactions

A

Dynamic - never goes to completion

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15
Q

The stronger the acid = [Ka question]

A

The stronger the acid the more the equilibrium will lie on the right (product side) and the Ka will increase

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16
Q

Ka is only dependent on what factor

A

Temperature

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17
Q

Which Ka is higher 4.6x10^-5 or 4.6^-8

A

4.6^10-5

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18
Q

As the base strength increases= [Kb question]

A

Equilibrium will lie on the right due to the increase in concentration of products and Kb value will increase

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19
Q

Name a natural and synthetic indicators

A

Litmus paper comes from lichens and phenolphthalein from synthetic chemicals

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20
Q

Most indicators are made from what

A

Weak acids or base

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21
Q

In what state do indicators exist in

A

Dynamic equilibrium - incomplete reaction

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22
Q

What colour is methyl orange at low pH

A

Red

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23
Q

What colour is methyl orange is at a high pH

A

Yellow

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24
Q

What is the pH range is methyl orange

A

3.1-4.4

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25
Q

What colour is methyl red is at low pH

A

Red

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26
Q

What colour is methyl red at a high pH

A

Yellow

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27
Q

What is the pH of colour change range of methyl red

A

4.8-6.0

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28
Q

What colour does litmus turn into at low pH

A

Red

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29
Q

What colour does litmus turn to at high pH

A

Blue

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30
Q

What is the pH of colour change range for litmus

A

4.5-8.3

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31
Q

What colour is bromothymol blue at low pH

A

Yellow

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32
Q

What colour is bromothymol blue at high pH

A

Blue

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33
Q

What is the pH of colour change range of bromothymol blue

A

6.0-7.6

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34
Q

What colour is phenol red at low pH

A

Yellow

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35
Q

What colour is phenol red at high pH

A

Red

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36
Q

What is the pH of colour change range of phenol red

A

6.8-8.4

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37
Q

What colour is phenolphthalein at low pH

A

Colourless

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38
Q

What colour is phenolphthalein at high pH

A

Pink

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39
Q

What is the pH of colour change range for phenolphthalein

A

8.2-10.0

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40
Q

When an acid reacts with ammonia what does it not produce that other reactions produce

A

Water

41
Q

Why does ammonia not produce water in reactions

A

It does not contain oxygen in its formula

42
Q

What is enthalpy of neutralisation

A

The amount of energy released or absorbed per mole of water formed

43
Q

Neutralisation between a strong acid and strong base is what type of reaction

A

Exothermic

44
Q

Weak acids and bases are what type of reactions

A

Less exothermic potentially even endothermic

45
Q

Why are weak acid and base less exothermic than strong acid and bases

A

Because it is not completely dissociated in water the weak acid have to dissociate to release H+ ions to react with the OH- ions
- dissociation is slightly endothermic

46
Q

What is calorimetry

A

Procedure used to measure amount of heat transferred to (or from) a substance

47
Q

What is Lavoisier idea of acids and base

A

Acids must contain oxygen

48
Q

What is Davy idea of acids and bases

A

HCl does not have oxygen but is an acid
- hydrogen is the main bitch not oxygen in acids

49
Q

What is Liebig idea of acid and base

A

Proposed acids contained hydrogen which could be replaced by a reactive metal [expanded definition

50
Q

What was Arrhenius idea of acids and bases

A

Acids and bases in aqueous solutions are electrolytes (conduct electricity)
- acids ionise to produce H+ ions
- bases ionise to produce OH- ions

51
Q

Name a limitation of Arrhenius definition

A

It does not explain the basic behaviour of ammonia which doesn’t produce OH- ions in a reaction

52
Q

What is Brønsted-Lowry idea of acids and base

A

An acid is a proton downer
A base is a proton acceptor

53
Q

What does Brønsted-Lowry definition do that Arrenhius can’t

A

It explains the basic behaviour of ionic compound solutions

54
Q

Amphiprotic substance

A

A molecule or ion that is capable of both donating and accepting protons

55
Q

Name 5 amphiprotic substances

A

HCO3-, HSO4-, H2PO4-, H2O+ , NH3

56
Q

In labs what is commonly used for acids spills

A

Sodium hydrogen carbonate

57
Q

Why is sodium hydrogen carbonate used for acids spills

A

It is weak, amphiprotic and produce carbon dioxide during neutralisation
- safe to handle
- does not increase the volume of liquid [its a solid]

58
Q

Amphiprotic substances are a subset of what

A

Amphoteric substance

59
Q

What are amphoteric substances

A

They can react with both acids and bases

60
Q

Name a limitation of Brønsted-Lowry definition

A

IT cannot explain the acidic behaviours of some things that do not contain hydrogen [mainly non-metal oxides - CO2, So2, So3]

61
Q

Two species in conjugate pairs differ by what

A

Differ by a proton (H+)

62
Q

A strong acid will have

A

An extremely weak conjugate base

63
Q

A weak acids will have a

A

Relatively strong conjugate base

64
Q

Strong bases are what groups hydroxides

A

Group 1 and 2

65
Q

What are 2 advantages of a pH meter over an indicator

A

It is more precise
It does not alter the composition of solution like indicators do

66
Q

What are 2 disadvantages of pH meter over an indicator

A

It requires calibration
It’s cost is very high

67
Q

Foods are generally _____
Cleaning products are generally ____

A

Acidic
Basic

68
Q

Aside from pH what else can a pH meter determine

A

Strength of acids and bases

69
Q

Why are calculations for weak acids and base more complex

A

Equilibrium shifts after dilution (becoming more ionised)

70
Q

Two strong acid solution or
Two strong base solution = [related to moles]

A

Total moles of H+ or OH- will be the sum of ions from original solutions

71
Q

What is a buffer solution

A

It resists changes in pH when small amounts of acid or base are added

72
Q

What are buffers commonly made of

A

Weak acid and its conjugate base
Or
Weak base and its conjugate acid

73
Q

What is the effectiveness of a buffer called

A

Buffer capacity

74
Q

What does buffer capacity depend on

A

The total concentration of weak acid and conjugate base (vice versa)
And
The pH of buffer solution

75
Q

Buffer capacity increases when

A

There are higher concentration of the weak acid and its conjugate base
[more of each is available to buffer the addition of H3O+ and OH-]

76
Q

When is a buffer most effective

A

When the pH is within 1 unit of its pKa

77
Q

A buffer is most effect when what

A

The amounts of weak acid and conjugate base present are similar

78
Q

What are 3 examples of a natural system where buffers play a major role

A

Our blood, in cells, large bodies of water (lakes)

79
Q

Aliquot

A

Accurately known volume of liquid [usually the one transferred via pipette to the conical flask]

80
Q

Analyte

A

A substance being analysed in titration [usually the one with unknown concentration - the one putting us through all this shit to find a number yeah its her]

81
Q

Equivalence point

A

The point in neutralisation where
the amounts of reactants are just sufficient to consume both reactants without excess of either
[stoichiometric ratio is equal]

82
Q

Titrand

A

The solution to which another solution (titrant) is added to during titration
[usually in the conical flask]

83
Q

Titrant

A

The solution that is being added into something else
[usually in the burette]

84
Q

Titre

A

The volume of the titrant used [in the burette]

85
Q

Standard solution

A

A solution of precisely known composition and concentration

86
Q

When is a primary standard produced

A

When a known mass of a substance of known high purity is dissolves to make A KNOWN VOLUME OF SOLUTION

87
Q

What are features a primary standard solution should have

A
  • high purity
  • unaffected by air exposure
  • non-hygroscopic {she don’t absorb water from air}
  • large molecular mass —> reduce percentage errors
  • be a solid
  • cheap + accessible
  • high water solubility (to be able to dissolve)
88
Q

Name 3 common primary standard solutions

A

Sodium carbonate
Potassium hydrogen phthalate
Benzoic acid

89
Q

Why is NaOH not a good primary standard

A

It’s hygroscopic—> absorbs water from air and the mass will then change

90
Q

When is a secondary standard produced

A

When its concentration is determined via stoichiometry

91
Q

The process of producing a secondary standard is called

A

Standardisation

92
Q

Strong acid + metal carbonate (weak base) produce what type of salt

A

A natural salt (BUT solution is still acidic)

93
Q

In pure water what is the [ ] of H+ and OH-

A

In pure water at 25C the pH=7 hence [H3O+] = [OH-] = 1.0x 10^-7M

94
Q

What is Kw

A

Ionisation constant of water

95
Q

If pH of a solution increases by 3, what happens to [ ] of H+ ions

A

Decreases by 1000 fold

96
Q

If a pH solution increases by 3, what happens to the [ ] of OH ions

A

It increases by 1000 fold

97
Q

What does ammonia dissociate into

A

Ammonium and hydroxide ion

98
Q

What determines the pH of a buffer solution

A

The pKa of the acid and the relative concentration of the acids and its conjugate base

Chemistry module 6 (1 decks)

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