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IB Chemistry HL > 8 acids and bases > Flashcards

8 acids and bases Flashcards

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1
Q

metal oxides are

A

bases

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2
Q

non metal oxides are

A

acids

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3
Q

precision -

A

how close results are to eachother

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4
Q

accuracy -

A

how close results are to the true value

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5
Q

which acids are monoproteoic

A

HCl
HNO3
CH3COOH

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6
Q

which acid is duoproteoic

A

H2SO4

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7
Q

whicha cid is triproteoic

A

H3PO4

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8
Q

which substances do you divide into ions in writing ionic equations from balanced chemical equation

A

ioniclly bonded ones

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9
Q

bronsted lowry acid

A

donates proton

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10
Q

bronsted lowry base

A

proton acceptor

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11
Q

amphiprotic means

A

a species able to act as a bronsted lowry base or acid

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12
Q

amphoteric

A

a species able to act as a base or acid

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13
Q

what defines pH

A

[H+]

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14
Q

pH =

A

-log[H+]

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15
Q

how to work out pH from [H+]

A

-log[H+]

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16
Q

how to work out [H+]

A

10 to the power of -pH

aka shift log -

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17
Q

how can you calculate a new conc when the old one has been diluted

A

conc1 x vol1 = conc2 x vol2

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18
Q

Kw =

A

[H+] [OH-] = 1 x 10^ -14

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19
Q

when would you use Kw

A

when you need to calculate pH and only have the conc of [OH-] ions
work out [H+] using equation and then -log it

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20
Q

differentiate between strong and weak acids

A

strong acids fully ionise in water

weak acids only partially ionise in water

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21
Q

what is the electrical conductivity of a strong acid

A

high

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22
Q

what is the electrical conductivity of a weak acid

A

low

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23
Q

relative reaction of a strong acid with magnesium and calcium carbonate

A

fast

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24
Q

relative reaction of a weak acid with magnesium and calcium carbonate

A

slow

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25
Q

what is the electrical conductivity of a strong alkali

A

high

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26
Q

what is the electrical conductivity of a weak alkali

A

low

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27
Q

describe the strengths within conjugate acid pairs

A

strong acids have relatively weak conjugate bases and weak acids have relatively strong conjugate bases

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28
Q

problems with combustion

A

incomplete combustion (formation of toxic gas CO)
respiratory problems with carbon
makes buildings black
complete combustion forming CO2
sulfur dioxide formation from coal (sulphur impurities removed)
N2 + O2 –> 2NO at high car engine temps

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29
Q

problems with the CO2 formed from complete combustion

A

greenhouse gas –> global warming.

reduce this by burning less fossil fuels

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30
Q

CO formed by incomplete combustion results in…

A

toxic gas that can cause health problems.

fix by ensuring a good supply of air/oxygen when burned

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31
Q

problems with the C formed by incomplete combusiton

A

blackens building
global dimming
fix by ensuring a good supply of air/oxygen when burned

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32
Q

problems with the sulfur dioxide fomred by combustion of sulfur

A

acid rain

fix by removing s from fume before burning or removing SO2 from fumes after burning (flue gas desulfurization)

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33
Q

problems with nitrogen oxides formed by the reacton of N2 in air with O2 in air at very high temperatures (often engines or furnaces)

A

acid rain.

fix by using a catalytic converter in cars

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34
Q

give the equation of the reaction carried out by a catalytic converter

A

NO + CO –> 1/2N2 + CO2

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35
Q

why is rain naturally acidic

A

becase of the dissolved CO2 .

has a pH of 5.6

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36
Q

pH of acid deposition

A

below 5.6

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37
Q

when is acid deposition formed

A

when nitrogen or sulfur oxides dissolve in water to form HNO3, HNO2, H2SO4 and H2SO3

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38
Q

Describe what happens when acid droplets are present in the atmosphere

A

They can combine with clouds or be washed out of the air with rain to fall as acid rain

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39
Q

Effects of acid rain

A

Enters leaves and damages them
Acid gases damage stonework and metals then changes the biology of lakes acid lakes often very clear as they lack the minute plants and animals
On Sandy soils acid rain dissolves aluminium ions which can reduce tree growth by damaging root hairs
Aluminium ions can kill fish and destroy fish eggs

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40
Q

Natural rainwater pH

A

5.6 because dissolved CO2 is slightly acidic

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41
Q

Give the reaction equation for carbon dioxide and water

A

CO2 + H2O

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42
Q

Where is battery acid on the pH scale

A

1&2

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43
Q

What is acid rain pH

A

3,4,5.5

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44
Q

What is normal rain to pure water on the pH scale

A

5,6,7

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45
Q

Whar is ocean water pH

A

8

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46
Q

What is liquid drain cleaner pH

A

9 upwards

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47
Q

How can nitrogen monoxide be formed

A

Lightning or internal combustion engines

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48
Q

Give the equation to form NO

A

N2 + O2 –> 2NO

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49
Q

Give the equation to form 2NO2

A

2NO + O2 –> 2NO2

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50
Q

How is nitrous acid formed (4HNO2)

A

4NO + 2H2O + O2 –> 4HNO2

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51
Q

Give the equation resulting in the formation of HNO2

A

2NO2 + H2O –> HNO3 + HNO2

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52
Q

Give the equation resulting in nitric acid (4NHO3)

A

4NO2 + 2H2O + O2 –> 4HNO3

53
Q

How is sulphur dioxide produced

A

Released in volcanic eruptions

When coal and oil are burned in power stations

54
Q

How is H2SO3 formed

A

SO2 + H2O –> H2SO3

55
Q

How is 2SO3 formed (give equation)

A

2SO2 + O2 –> 2SO3

56
Q

How is sulfric acid (H2SO4) formed (give equation)

A

SO3 + H2O –> H2SO4

57
Q

What is dry deposition

A

Acid deposition in the form of acidic particles and gases

58
Q

pH =

A
  • log [H+]
59
Q

pOH =

A

-log [OH]

60
Q

Kw =

A

[H+] [OH-]

61
Q

pH + pOH =

A

14

62
Q

A Brønsted–Lowry acid is

A

a proton/H+ donor

63
Q

a Brønsted–Lowry base is

A

a proton/H+ acceptor

64
Q

An amphiprotic species is able to act as

A

a Brønsted–Lowry acid and a Brønsted–Lowry base depending on what it is reacting with.

65
Q

Benzoic acid

A

C6H5COOH (s)

66
Q

Phosphoric acid

A

H3PO4 (aq)

67
Q

Carbonic acid

A

H2CO3 (aq)

68
Q

Ethanoic acid

A

CH3COOH (aq)

69
Q

what determines whether an acid is monoprotic, diprotic or tripotic

A

number of hydrogen ions or protons

70
Q

Ammonia

A

NH3

71
Q

Ethanamine

A

CH3CH2NH2 (g)

72
Q

what does a conjugate acid base differ by

A

a proton (H+)

73
Q

examples of amphiprotic species

A

Hydrogen carbonate ion HCO3−

Hydrogen sulfate ion HSO4−

Dihydrogen phosphate H2PO4−

Hydrogen phosphate HPO42−

74
Q

metal + acid →

A

salt + hydrogen

75
Q

what are alkalis

A

soluble bases

76
Q

metal oxide + acid →

A

salt and water

77
Q

metal hydroxide + acid →

A

salt and water

78
Q

metal carbonate + acid →

A

salt + water + carbon dioxide

79
Q

metal hydrogencarbonate + acid →

A

salt + water + carbon dioxide

80
Q

acid + base (or alkali) →

A

salt + water

81
Q

what type of reaction is acid and base

A

exothermic. this is known as the enthalpy change of neutrlaistion

82
Q

the higher the concentration of H+ ions in solution,

A

the lower the pH scale

83
Q

describe the change in litmus paper of an acidic solution

A

blue litmus changes to red

84
Q

describe the change in litmus paper in an acidic solution

A

blue litmus changes to red

85
Q

colour oflitmus in acid

A

red

86
Q

colour of litmus in alkali

A

blue

87
Q

colour of methyl orange in acid

A

red

88
Q

colour of methyl orange in alkali

A

yellow

89
Q

colour of Phenolphthalein in acid

A

colourless

90
Q

colour of Phenolphthalein in alkali

A

pink/purple

91
Q

if water cannot conduct electricity very well, it must have

A

a low concentration of mobile ions responsible for the electrical conductivity of solutions

92
Q

what is it calle when water molecules dissociate

A

auto-ionisation of water

93
Q

what is the ionic product of water (Kw)

A

the product of the [H+] and [OH-] in water at a particular temperature.

94
Q

uses of sulfuric acid

A

fertilisers,
paints and pigments,
soaps and detergents,
fibres and dyes,

95
Q

what does the srength of acids and bases depend on

A

their degree of dissociation or ionisation in aqueous solution

96
Q

strong acids do what in aqueous solution

A

completely dissociate or ionise

97
Q

weak acids do what in aquous solution

A

partially dissociate or ionise

98
Q

what does dissociate mean

A

break apart an ionic compound into its constituent ions

99
Q

For a strong acid, the concentration of H+ ions, [H+], is equal to

A

the initial concentration of the strong acid.

100
Q

what does HCL dissociate to give

A

H+ (aq) + Cl– (aq)

101
Q

what does H2SO4 dissociate to give

A

H+ (aq) + HSO4– (aq)

102
Q

what does HNO3 dissociate to give

A

H+ (aq) + NO3– (aq)

103
Q

are organic acids usually strong or weak

A

usually weak (Kc small)

104
Q

do weak acids have small or large Kc’s

A

small

105
Q

what does NaOH dissociate to give

A

Na+ (aq) + OH– (aq)

106
Q

what does KOH dissociate to give

A

K+ (aq) + OH– (aq)

107
Q

what does Ba(OH)2 dissociate to give

A

Ba2+ (aq) + 2OH– (aq)

108
Q

For a strong base, the concentration of OH– ions, [OH–], is equal to

A

the initial concentration of the strong base.

109
Q

which bases are weak

A

all of them except for the hydroxides of groups 1 and 2

110
Q

which bases are strong

A

hydroxides of groups 1 and 2

111
Q

equimolar solutions

A

same concentrations

112
Q

elec conductitvity of strong acids

A

high

113
Q

elec conductitvity of weak acids

A

low

114
Q

relative rate of reaction with magneium and strong acid

A

fast

115
Q

relative rate of reaction with magneium and weak acid

A

slow

116
Q

relative rate of reaction with calcium carbonate and a strong acid

A

fast

117
Q

relative rate of reaction with calcium carbonate and a weak acid

A

slow

118
Q

if one part of the conjugate acid base pair is weak the othe rpart is

A

strong. one will be weak and one will be strong, or both will be moderate

119
Q

what is hydrodesulfurisation

A

a pre-combustion method of reducing sulfur dioxide emissions

120
Q

State the name of the conjugate base of water. Give the name of the ion, not the formula.

A

hydroxide

121
Q

how come you can use a conductivity metre in ionic solutions but not covalent

A

Since aqueous ionic compounds involve the dissociation of ions into their solvent, water, the ions will move around as individual ions. covalent compounds do not dissociate into ions so you cannot measure them using a conductivity metre

122
Q

outline a precombustion method

A

Hydrodesulfurisation is a pre-combustion method by which the sulfur is removed from refined petroleum products such as gasoline, jet fuel, kerosene and diesel fuel before combustion. This process takes place at high temperatures and pressures (300-400 oC at pressures of between 300000 - 1300000 Pa) in the presence of a catalyst. The sulfur is removed from the product in the form of hydrogen sulfide (H2S).

123
Q

outline a post combustion method

A

A post-combustion method utilised in power stations is flue gas desulfurisation. The levels of sulfur dioxide emissions in the flue gases can be reduced by passing them into a flue gas desulfurisation tower, also known as a ‘scrubber’ In the scrubbing tower, the gases are passed through a sprayed aqueous suspension of calcium carbonate and calcium oxide. The product is calcium sulfite (sulfate(IV)) which is further oxidised to produce calcium sulfate.

124
Q

give the equation to show how nitrogen oxide (NO) forms nitric acid, HNO3, and nitrous acid, HNO2

A

2NO2 + H2O –> HNO3 + HNO2

125
Q

give the equations to show how sulfur dioxide, SO2, forms sulfuric acid (H2SO4) and sulphurous acid (H2SO3)

A

SO2 + H2O –> H2SO3

SO2 + O2 +H 2O → H 2SO4

126
Q

describe and explain how acid rain affects the growth of trees

A

acid rain enters the leaves and damages them

on some sandy soils, acid rain dissolves aluminium ions which can reduce the tree growth by damaging root hairs

127
Q

acid rain formula

A

HNO3

H2SO4

128
Q

what does calcium oxide dissolve in water to form

A

calcium hydroxide

IB Chemistry HL (12 decks)

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