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Chemistry > Chapter 8: Acids and Bases > Flashcards

Chapter 8: Acids and Bases Flashcards

1
Q

What are hydrochloric acid HCl and sulfuric acid H2SO4 an example of?

A

Acids

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2
Q

What are sodium hydroxide NaOH and ammonia NH3 an example of?

A

Bases

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3
Q

What atom leads to the characteristic properties of an acid?

A

At least one hydrogen atom
* All acids contain at least one

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3
Q

What atom leads to the characteristic properties of an acid?

A

At least one hydrogen atom
* All acids contain at least one

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4
Q

What is the simplest definition of acids and bases?

A

Acid: a substance that produces hydrogen ions in solution
Base: a substance that produces hydroxide ions in solution

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5
Q

What is the Bronsted-Lowry definition of acids and bases?

A
  • An acid is a proton (H+) donor
  • A base/alkali is a proton (H+) acceptor
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5
Q

What is the Bronsted-Lowry definition of acids and bases?

A
  • An acid is a proton (H+) donor
  • A base/alkali is a proton (H+) acceptor
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6
Q

What is the formula of hydrochloric acid?

A

HCl

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7
Q

What is the formula of sulfuric acid?

A

H2SO4

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8
Q

What is the formula of nitric acid?

A

HNO3

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8
Q

What is the formula of carbonic acid?

A

H2CO3

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9
Q

What is the formula of ethanoic acid?

A

CH3COOH

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10
Q

What is the formula of benzoic acid?

A

C6H5COOH

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11
Q

If H2O accepts a proton when CH3COOH donates a proton, which one acts as a base and which for acid?

A

H2O for acid
CH3COOH for base

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12
Q

What do conjugate acid-base pairs always differ by?

A

One proton H+

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13
Q

What is a conjugate acid-base pair?

A

When the acid of a compound donates a proton and it forms a base
The original acid and the base it is now are conjugate acid-base pairs

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14
Q

What is the term amphiprotic and amphoteric used to describe?

A

A substance that can act as both an acid and a base

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15
Q

What does amphiprotic refer to?

A

The Bronsted-Lowry definition of acids and bases and indicates a species that can donate (acting as an acid) or accept (acting as a base) a proton.

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16
Q

What does amphiprotic refer to?

A

The Bronsted-Lowry definition of acids and bases and indicates a species that can donate (acting as an acid) or accept (acting as a base) a proton.

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17
Q

What is a amphiprotic substance?

A

Water
because it can act as a proton donor (to form OH-) with NH3 but as a proton acceptor (to form H3O+) in its reaction with CH3COOH

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18
Q

What does amphoteric refer to?

A

It is a more general term and refers to a substance that can act as an acid and a base

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19
Q

What does amphoteric refer to?

A

It is a more general term and refers to a substance that can act as an acid and a base

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20
Q

What is the relationship between amphoteric and amphiteric

A

All amphiprotic substances are also amphoteric but not all amphoteric substances are amphiteric

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20
Q

What is the relationship between amphoteric and amphiteric

A

All amphiprotic substances are also amphoteric but not all amphoteric substances are amphiteric

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21
Q

Where does the difference arise between the term amphiteric and amphoteric?

A

Because there is another, more general, definition of acids and bases (the Lewis definition), which does not require the transfer of a proton

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21
Q

Where does the difference arise between the term amphiteric and amphoteric?

A

Because there is another, more general, definition of acids and bases (the Lewis definition), which does not require the transfer of a proton

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22
Q

What is replaced in an acid to form salt?

A

The hydrogen ion (H+) in an acid can be replaced by a metal ion (or ammonium ion) to for salt

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22
Q

What is replaced in an acid to form salt?

A

The hydrogen ion (H+) in an acid can be replaced by a metal ion (or ammonium ion) to for salt

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23
Q

What is the name of salt when hydrochloric acid loses a hydrogen ion?

A

Chloride
HCl -> NaCl (sodium chloride)

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24
Q

What is the name of salt when sulfuric acid loses a hydrogen ion?

A

Sulfate
H2SO4 -> Na2SO4 (sodium sulfate)

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25
Q

What is the name of salt when nitric acid loses a hydrogen ion?

A

nitrate
HNO3 -> NH4NO3 (ammonium nitrate)

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26
Q

What is the name of salt when carbonic acid loses a hydrogen ion?

A

carbonate
H2CO3 -> K2CO3 (potassium carbonate)

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27
Q

What is the name of salt when ethanoic acid loses a hydrogen ion?

A

Ethanoate
CH3COOH -> Ca(CH3COO)2 (calcium ethanoate)

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27
Q

What is the name of salt when ethanoic acid loses a hydrogen ion?

A

Ethanoate
CH3COOH -> Ca(CH3COO)2 (calcium ethanoate)

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28
Q

What does a metal + acid reaction produce?

A

metal + acid -> salt + hydrogen

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29
Q

What does acid + carbonate/hydrogencarbonate reaction produce?

A

acid + carbonate/hydrogencarbonate -> salt + carbon dioxide + water

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30
Q

What does a base + water reaction form?

A

Base + acid -> Salt + water

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31
Q

What are metal oxides or metal hydroxides?

A

Bases

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32
Q

What are alkalis?

A

Solutions obtained when a metal hydroxide (such as sodium hydroxide) dissolves in water or when certain bases react with water

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33
Q

What are alkalis?

A

Solutions obtained when a metal hydroxide (such as sodium hydroxide) dissolves in water or when certain bases react with water

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34
Q

What does the fact that there are very few soluble metal hydroxides mean for alkalis?

A

There are very few alkalis

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35
Q

What does the fact that there are very few soluble metal hydroxides mean for alkalis?

A

There are very few alkalis

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36
Q

Base vs alkali which is the most general term?

A

Base

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37
Q

What is the reaction between an acid and an alkali?

A

It is similar to that between an acid and a base

Alkali + acid -> salt + water

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37
Q

What is the reaction between an acid and an alkali?

A

It is similar to that between an acid and a base

Alkali + acid -> salt + water

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38
Q

What are the reactions between acids and bases or acids and alkalis called?

A

Neutralisation reactions

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38
Q

What are the reactions between acids and bases or acids and alkalis called?

A

Neutralisation reactions

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39
Q

What are neutralisation reactions?

A

When the H+ ions from the acid reacts with the OH- ions from the alkali to form a neutral substance water

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40
Q

What are neutralisation reactions?

A

When the H+ ions from the acid reacts with the OH- ions from the alkali to form a neutral substance water

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41
Q

Is neutralisation reactions exo or endo?

A

Exothermic and typically give out about 57kJ per mole of water formed

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41
Q

Is neutralisation reactions exo or endo?

A

Exothermic and typically give out about 57kJ per mole of water formed

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42
Q

What do neutralisation reactions produce?

A

a salt and water only

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43
Q

What do neutralisation reactions produce?

A

a salt and water only

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44
Q

What is ammonia solution equivalent to? (NH3 aq)

A

to ammonium hydroxide (NH4OH)
in some labs it is labelled as ammonia solution and ammonium hydroxide in others

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44
Q

What is ammonia solution equivalent to? (NH3 aq)

A

to ammonium hydroxide (NH4OH)
in some labs it is labelled as ammonia solution and ammonium hydroxide in others

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45
Q

What is ammonia in equilibrium with?

A

the ammonium ion and the hydroxide ion

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45
Q

What is ammonia in equilibrium with?

A

the ammonium ion and the hydroxide ion

46
Q

Generally where does the metal part of the salt come from and the non-metal part?

A

Metal part comes from a metal oxide or hydroxide and th enon-metal part from the acid

e.g.
cooper sulfate can be made from the reaction between the base copper oxide and the sulfuric acid

47
Q

WHat is one common way of making a soluble salt?

A

By tritrating an acid against an alkali
* a known amount of acid is measured out using a pipette and then an indicator is added
* the alkali is then added from a burette until the indicator just changes colour

48
Q

What are indicators?

A

essentially substances that have different colours in acidic and alkaline solutions
* used commonly in titrations

48
Q

What are indicators?

A

essentially substances that have different colours in acidic and alkaline solutions
* used commonly in titrations

49
Q

How are different indicators chosen for a titration?

A

Based on whether the acid or the alkali is weak or strong

50
Q

What does a universal indicator contain?

A

a mixture of indicators and cannot be used to monitor titrations because it changes gradually from one colour to the next

50
Q

What does a universal indicator contain?

A

a mixture of indicators and cannot be used to monitor titrations because it changes gradually from one colour to the next

51
Q

What can the pH scale be used for?

A

to indicate whether a solution is acidic, alkaline or neutral

51
Q

What can the pH scale be used for?

A

to indicate whether a solution is acidic, alkaline or neutral

52
Q

What can the pH of a solution be determined by?

A

A pH meter or by using universal indicator solution or paper

53
Q

What can the pH of a solution be determined by?

A

A pH meter or by using universal indicator solution or paper

54
Q

What is pH a measure of?

A

the concentratino of H+ ions in a solution

54
Q

What is pH a measure of?

A

the concentratino of H+ ions in a solution

55
Q

What is the unit of pH?

A

there is no units

56
Q

What is the unit of pH?

A

there is no units

57
Q

What does it mean when water dissociates ( or ionsises)?

58
Q

What is the relatinship of H+ to OH- in a neutral solution?

59
Q

What is the relatinship of H+ to OH- in a acidic solution?

60
Q

What is the relatinship of H+ to OH- in a alkaline solution?

61
Q

What can be assumed for strong acids to do in aqueous solutions?

A

Strong acids can be assiumed to dissociate fully in aqueous solution

62
Q

What can be assumed for strong acids to do in aqueous solutions?

A

Strong acids can be assiumed to dissociate fully in aqueous solution

63
Q

Because strong acids can be assumed to dissociate fully in aqueous solution, what is the concentration of H+ ions and the concentration of the acid?

A

the conc. of H+ ions is the same as the concentration of the acid

64
Q

What happens when an acid reacts with water?

A

It dissociates, or ionises

65
Q

Why does an acid dissociate when reacting with water?

A

Using the Bronsted-Lowry theory
* the acid donates a proton to water
* acid dissociates into H+ and A- ions

65
Q

Why does an acid dissociate when reacting with water?

A

Using the Bronsted-Lowry theory
* the acid donates a proton to water
* acid dissociates into H+ and A- ions
* and the H+ from the acid is donates to H2O

66
Q

How can we classify how strong or weak an acid is?

A

By how much they dissociate in aqueous solution

67
Q

What are 3 strong acids that dissociate completely in aqueous solution?

A
  • hydrochloric acid (HCl)
  • sulfuric acid (H2SO4)
  • nitric acid (HNO3)
68
Q

What is a monoprotic acid and what is an example of it?

A

HCl is a monoprotic acid
* it dissociates to form one proton per molecule

68
Q

What is a monoprotic acid and what is an example of it?

A

HCl is a monoprotic acid
* it dissociates to form one proton per molecule

69
Q

What is a diprotic acid and what is an example of it?

A

H2SO4 is a diprotic acid
* it can dissociate to form two protons per molecule

70
Q

What is the difference between a monoprotic acid and a diprotic acid?

A

when it dissociates to either forms one proton per molecule (monoprotic) or two proton per molecule (diprotic)

71
Q

How do weak acids dissociate in aqueous solutions?

A

Only partially

72
Q

How do weak acids dissociate in aqueous solutions?

A

Only partially

73
Q

What is sulfuric acid a strong acid for?

A

for the first dissociation only

74
Q

What are examples of weak acids?

A
  • carbonic acid (H2CO3)
  • carboxylic acids such as ethanoic acid (CH3COOH)
75
Q

How can we spot a weak or strong acid dissociating from an equation?

A

by the arrow
* the non-reversible arrow (->) is used to indicate that the dissociation is essentially complete
* the equilibrium arrow indicates that the reaction is reversible and does not go to completion

76
Q

Is HCO3- amphiprotic?

A

the hyrogen carbonate ion is amphiprotic. it accepts a proton in the reverse reaction in the first equation (acts as a base) and donates a proton (acts as an acid) in the second

76
Q

Is HCO3- amphiprotic?

A

the hyrogen carbonate ion is amphiprotic. it accepts a proton in the reverse reaction in the first equation (acts as a base) and donates a proton (acts as an acid) in the second

76
Q

Is HCO3- amphiprotic?

A

the hyrogen carbonate ion is amphiprotic. it accepts a proton in the reverse reaction in the first equation (acts as a base) and donates a proton (acts as an acid) in the second

76
Q

Is HCO3- amphiprotic?

A

the hyrogen carbonate ion is amphiprotic. it accepts a proton in the reverse reaction in the first equation (acts as a base) and donates a proton (acts as an acid) in the second

77
Q

What happens when a base reacts with water?

A

It accepts a proton from the water and ionises

78
Q

How are bases defined as strong or weak?

A

depending on how much they ionic in aqueous solution

79
Q

What do strong bases do in aqueous solution?

A

They ionise completely

80
Q

What do strong bases do in aqueous solution?

A

They ionise completely

81
Q

What do weak bases do in aqueous solution?

A

Ionise only partially

82
Q

Is ammonia a base or acid?

A

It is a typical weak base

83
Q

Is ammonia a base or acid?

A

It is a typical weak base

84
Q

What are examples of weak bases?

A
  • ammonia
  • amines such as ehylamine (ethanamine) CH3CH2NH2
85
Q

WHat is the relationship between the strength of an acid and the strength of its conjugate base?

A

The stronger an acid, the weaker its conjugate base

86
Q

What is the relationship between the strength of an acid and the strength of its conjugate base?

A

The stronger an acid, the weaker its conjugate base

87
Q

What is the relationship between the strength of a base and the strength of its conjugate acid?

A

The stronger a base, the weaker its conjugate acid

88
Q

What does the methods for distinguishing between acids rely on?

A

on the fact that strong acids dissociate more than weak acids

89
Q

How is a strong acid a better conductgor of electricity than a weak acid?

A
  • strong acids dissociates fully
  • so the concentration of ions is high
  • making it a good conductor of electricity
  • A weak acid only dissociates partially and so the conc. of ions is lower and does not conduct electricity as ell
90
Q

Because strong acids are good conductors of electricity, what may they be described as?

A

strong electrolytes
weak electrolytes for weak acids

91
Q

If the pH is lower, what does it mean for the concentration of H+?

A

the lower the pH, the higher the concentration of H+ ions

91
Q

If the pH is lower, what does it mean for the concentration of H+?

A

the lower the pH, the higher the concentration of H+ ions

92
Q

Why do strong acids react more rapidly with metals such as magnesium to form hydrogen?

A

Because strong acids have a higher concentration of free H+ ions and therefore react more rapidly

93
Q

What is effervescence?

A

rapid bubbling

93
Q

What is effervescence?

A

rapid bubbling

94
Q

What are rapid reactions shown by?

A

effervescence

95
Q

What does the concentration of an acid refer to?

A

the number of moles of acid in a certain volumr

96
Q

What does the strength of an acid refer to?

A

How much it dissociayes in squeous solution

97
Q

Can a more concentrated solution become a stronger acid?

A

No matter how concentrated the solution of ethanoic acid is, it will never become a storng acid because it always dissociayes partially

simlarily, diluting a strong acid does not make it anything other than a strong acid because it always dissociates fully

97
Q

Can a more concentrated solution become a stronger acid?

A

No matter how concentrated the solution of ethanoic acid is, it will never become a storng acid because it always dissociayes partially

simlarily, diluting a strong acid does not make it anything other than a strong acid because it always dissociates fully

98
Q

Does a lower pH mean a stronger acid?

A

No pH is simple a measure of the concentration of H+ ions. It is possible for a dilute solution of a strong acid to have a higher pH than a concentration nsolution of a weak acid.

98
Q

Does a lower pH mean a stronger acid?

A

No pH is simple a measure of the concentration of H+ ions. It is possible for a dilute solution of a strong acid to have a higher pH than a concentration nsolution of a weak acid.

99
Q

How is a more concentrated soltuion of a weak acid able to have a lower pH?

A

Because the partial dissociation of the weak acid produces a high concentration of H+ than the complete dissociation of the strong acid HCl

100
Q

How can pH be used to compare acid strength?

A

Only if equal concentrations of acids are being compared

101
Q

How can pH be used to compare acid strength?

A

Only if equal concentrations of acids are being compared

102
Q

What do oxides of non-metals, if soluble in water produce?

A

Acidic solutions
* oxides of non-metals are acidic

103
Q

How is rain naturally acidic?

A

Because of dissolved carbon dioxide

104
Q

How is rain naturally acidic?

A

Because of dissolved carbon dioxide

105
Q

What is acidic deposition?

A
  • any process in which acidic substances (particles, gases and preipitation) leave the atmosphere to be deposited on the surface of the earth
  • divided into wet depoition (acid rain, fog and snow) and dry deposition (acidic gases and particles)
106
Q

What do acidic pollutants include?

A

Oxides of sulfur and nitrogen

107
Q

What can sulfur dioxide be formed by?

A

various natrual and anthropogenic processes - such as burning of sulfuer-containing fuels

108
Q

What are the main anthropogenic sources of nitrogen oxides?

A

internal combustion engine, coal, gas, oil-fuelled power stations and heavy industry power generation

109
Q

How can sulfuric acid be formed?

110
Q

How is nitric acid formed?

A

When NO2 react with a hydroxyl free radical

111
Q

What are the problems associated with acid deposition?

A

Effect on vegetation
* the acid can displace metal ions from the soil that are consequently washed away
* Mg2+ is need to produce chlorophyll but its washed away by acid displacing it and so plants could be prevented from phootsynthesising properly
* Aluminium ions are dissolved from rocks which damages plant roots and limits water uptake. Cause stunted growth and thinning or yellowing of leaves on trees

Lakes and rivers
* aquatic life is sensitive to the pH falling below 6
* insect larvae, fish and invertebrates and others cannot survive below pH 5.2
* below pH 4, virtually no life will survive
* dissolve haardous minerals from rocks and acculate in lakes and damage aqautic life (Al3+ ions damage fish gills)

buildings
* Limestone and marble are eroded and sisolve away expsoing a fresh surface to react with more acid

human health
* irritates mucous membranes
* cause respiratory illnesses such as asthma and bronchitis
* can dissolve heavy metal compounds releasing poisonous ions which ay be linked to Alzheimer’s disease

111
Q

What are the problems associated with acid deposition?

A

Effect on vegetation
* the acid can displace metal ions from the soil that are consequently washed away
* Mg2+ is need to produce chlorophyll but its washed away by acid displacing it and so plants could be prevented from phootsynthesising properly
* Aluminium ions are dissolved from rocks which damages plant roots and limits water uptake. Cause stunted growth and thinning or yellowing of leaves on trees

Lakes and rivers
* aquatic life is sensitive to the pH falling below 6
* insect larvae, fish and invertebrates and others cannot survive below pH 5.2
* below pH 4, virtually no life will survive
* dissolve haardous minerals from rocks and acculate in lakes and damage aqautic life (Al3+ ions damage fish gills)

buildings
* Limestone and marble are eroded and sisolve away expsoing a fresh surface to react with more acid

human health
* irritates mucous membranes
* cause respiratory illnesses such as asthma and bronchitis
* can dissolve heavy metal compounds releasing poisonous ions which ay be linked to Alzheimer’s disease

112
Q

What are the methods of dealing with acid deposition?

A
  • improving the design. ofbehicle engines
  • using catalytic converters
  • removing sulfur before burning fuels
  • using renewable power supplies
  • making greater use of public transport
  • designing more efficient power stations
  • ‘liming’ of lakes - calcium oxide or hydroxide neutralises acidity
113
Q

What is pre-combustion desulfurisation?

A

removing sulfur before the fuel is burnt to produce a more environmentally-friendly fuel

113
Q

What is pre-combustion desulfurisation?

A

removing sulfur before the fuel is burnt to produce a more environmentally-friendly fuel

114
Q

What is post-combustion desulfurisation?

A

removing SO2 after the fuel is burnt

Chemistry (12 decks)

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