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Chemistry - Year 12 > Module 6: Acids and Bases Reactions > Flashcards

Module 6: Acids and Bases Reactions Flashcards

1
Q

Hydrochloric acid

A

HCl

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2
Q

Sulphuric acid

A

H2SO4

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3
Q

Nitric acid

A

HNO3

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4
Q

Ethanoic/acetic acid

A

CH3COOH

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5
Q

Carbonic acid

A

H2CO3

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6
Q

Phosphoric acid

A

H3PO4

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7
Q

Citric acid

A

C6H8O7

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8
Q

Ascorbic acid (vitamin c)

A

C8H8O6

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9
Q

Sodium hydroxide

A

NaOH

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10
Q

Ammonia

A

NH3

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11
Q

Calcium hydroxide

A

Ca(OH)2

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12
Q

Magnesium hydroxide

A

Mg(OH)2

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13
Q

Sodium carbonate

A

Na2CO3

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14
Q

How do you know if something is an acid?

A

It has a H+

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15
Q

How do you know if something is a base?

A

It has OH- or O2-

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16
Q

What are the 5 properties of acids?

A
  1. Sour taste
  2. Sting or burn the skin
  3. Are electrolytes
  4. Turn litmus paper red
  5. PH less than 7
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17
Q

What are the 5 properties of bases?

A
  1. Bitter taste
  2. Soapy or caustic feel
  3. Are electrolytes
  4. Turn litmus paper blue
  5. PH greater than 7
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18
Q

What are monoprotic acids?

A

Acids capable of donating one proton only

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19
Q

What are diprotic acids?

A

Acids capable of donating two protons

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21
Q

What are the 3 strong acids that need to be memorised?

A

HCl, H2SO4, HNO3

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21
Q

What are weak acids?

A

All other acids which aren’t HCl, H2SO4 or HNO3

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22
Q

What are strong bases?

A

Any which have hydroxides in them

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23
Q

What are weak bases?

A

Any which don’t have hydroxides in them

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24
Q

What type of arrow is used when there is a strong acid or base in a reaction?

A

→

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25
Q

What type of arrow is used if both the acid and the base are weak?

A

⇌

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26
Q

Do acids lose or gain a proton to form its conjugate base?

A

Lose a proton

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27
Q

Do bases lose or gain a proton to form its conjugate acid?

A

Gain a proton

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28
Q

What is the acid metal hydroxide word equation?

A

Acid + Metal Hydroxide → Salt + Water

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29
Q

What is the acid metal word equation?

A

Acid + Metal → Salt + Hydrogen

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30
Q

What is the acid and metal carbonate word equation?

A

Acid + Metal Carbonate → Salt + CO2 + Water

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31
Q

How did Boyle describe acids and bases?

A

Described acids and bases by there property

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32
Q

What did Boyle notice about acids and bases?

A

Bases could reverse colour change of indicators mixed with acids

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33
Q

What did Lavoisier conclude about acids?

A

Acids contain oxygen

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34
Q

Why wasn’t Lavoisier’s conclusion that acids contain oxygen correct?

A

HCl and HCN are also acids

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35
Q

What did Davy conclude about about acids?

A

All known acids contain hydrogen

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36
Q

What did Davy conclude about bases?

A

Metal compounds with oxygen are bases

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37
Q

What is an Arrhenius acid?

A

A molecule that contains hydrogen and can produce H+ ions in water

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38
Q

What is an Arrhenius base?

A

A molecule that dissociates in water to produce OH-

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39
Q

What did Arrhenius suggest about mixing bases and acids?

A

That they will produce water

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40
Q

What were the four main limitations of Arrhenius’ idea?

A
  • Could not explain NH3 which has no OH- but is a base
  • Could only be applied to aqueous solutions
  • Did not explain strength of acids and bases
  • Could not explain why some reactions did not form neutral solutions
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41
Q

What is a Bronsted - Lowry acid?

A

A molecule which is a proton (H+) donor

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42
Q

What is a Bronsted - Lowry base?

A

A molecule which is a proton (H+) acceptor

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43
Q

What was an advantage of the Bronsted - Lowry theory?

A

Reactions were no longer limited to aqueous solutions

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44
Q

What were four disadvantages of the Bronsted - Lowry theory?

A
  • A proton that can be transferd must be present for a substance to be an acid or a base
  • Model requires a solvent
  • Could not explain reaction where no protons are involved
  • Could not explain reactions between acidic oxides and basic oxides
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45
Q

What is a Lewis acid?

A

A molecule that is an electron pair receptor

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46
Q

What is a Lewis base?

A

A molecule that is an electron pair donor

47
Q

What were two advantages of the Lewis theory?

A
  • Broader definition to explain more acid and base reactions
    Does not require a proton or a solvent
48
Q

Do acids lose or gain a proton to form a conjugate base?

49
Q

Do bases lose or gain a proton to form a conjugate acid?

50
Q

What is an amphiprotic substance?

A

A substance that can either donate or accept protons

51
Q

What are two examples of amphiprotic substances?

A

H2O
H2PO4 -

52
Q

What is a monoprotic acid?

A

Can only donate one proton

53
Q

What is a diprotic acid?

A

Can donate two protons

54
Q

What is a triprotic acid?

A

Can donate three protons

55
Q

What is a polyprotic acid?

A

Can donate more than one proton

56
Q

What makes an acid strong?

A

Readily dissociates in water and donate protons to form hydronium

57
Q

What is ionisation?

A

When a free H+ combines with water to form H3O+

58
Q

What makes an acid weak?

A

Does not dissociate readily and reacts only partially with water

59
Q

What makes a base strong?

A

O2 or OH- readily dissociate in water to make hydroxide ions which can accept protons

60
Q

What makes a base weak?

A

Only have a small amount of molecules that have accepted a proton to form ions

61
Q

How is the strength of a base or acid impact the conjugate base or acid?

A

The stronger the acid or base the weaker the conjugate base or acid will be

62
Q

What does strength of an acid/base relate to?

A

Relates to its ability to dissociate

63
Q

What does concentration of an acid/base show?

A

The number of mol/L

64
Q

What does Kw stand for?

A

Ionic product constant of water

65
Q

What can change the Kw?

A

Slightly changes with temperature or pressure

66
Q

What is the Kw at normal (25C) of H3O+?

A

1 x 10^-7 mol/L

67
Q

What is the Kw at normal (25C) of OH-?

A

1 x 10^-7 mol/L

68
Q

What is the Kw of water at normal (25C)?

A

1 x 10^-14 mol/L

69
Q

What is the pH scale?

A

Is a measure of acidity related to the concentration of hyrdonium ions

70
Q

What are the formulas for pH and pOH?

A

pH = -log[H3O+]
pOH = -log[OH-]

71
Q

What are the formulas to find the concentration of H3O+ and OH- from pH and pOH?

A

[H3O+] = 10^-pH
[OH-] = 10^-pOH

72
Q

What does pH + pOH = at normal (25C)

73
Q

What is a standard solution?

A

A solution with an accuratly known concentration

74
Q

What is the standard solution called in a titration?

75
Q

How is a standard solution made?

A

By dissolving a primary standard in a known volume of water

76
Q

What are 7 characteristics of a primary standard?

A
  1. Is a solid
  2. Easily obtained in pure form
  3. Stable and easy to store
  4. Has a high molar mass
  5. Has high solubility in water
  6. Should react instantaneously
  7. Should be inexpensive
77
Q

What is a titration?

A

A method to determine the concentration of an unknown solution

78
Q

What is the analyte?

A

Is the solution of unknown concentration

79
Q

What is the analyte usually put in?

A

A conical flask

80
Q

What is the titrant usually put in?

81
Q

What is the titre?

A

The minimum quantity of a solution required to complete a titration

82
Q

What is an aliquot?

A

A small sample of analyte usually 25mL

83
Q

What is the endpoint of a titration?

A

The point at which the indicator changes colour

84
Q

What should the burette be rinsed with?

A

With the titrant

85
Q

What should the pipette be rinsed with?

A

With the analyte

86
Q

What should the conical flask be rinsed with?

A

With distilled water

87
Q

What should the volumetric flask be rinsed with?

A

With distilled water

88
Q

What is the chemical representation of the indicator in a chemical equation?

89
Q

What is the pH of a strong acid + strong base?

90
Q

What is the pH of a weak acid + weak base?

91
Q

What is the pH of a strong acid + weak base?

92
Q

What is the pH of a weak acid + strong base?

93
Q

What are the three indicators usually used?

A

Methyl orange
Bromothymol blue
Phenolphthalein

94
Q

What is the pH colour change range of methyl orange?

95
Q

What colour is methyl orange in acid, base and neutral?

A

Acid: Red
Neutral: Orange
Base: Yellow

96
Q

What is the pH colour change range of bromothymol blue?

97
Q

What colour is bromothymol blue in acid, base and neutral?

A

Acid: Yellow
Neutral: Green
Base: Blue

98
Q

What is the pH colour change range of phenolphthalein?

A

8.3 - 10.0

99
Q

What colour is phenolphthalein in acid, base and neutral?

A

Acid: Colourless
Neutral: Light pink
Base: Pink

100
Q

How does pKa influence PH?

A

The lower the pKa the lower the PH

101
Q

What does pKa determine?

A

The strength of an acid

102
Q

How is pKa calculated?

103
Q

How do you calculate Ka from a known pH?

A

Use a rice table and make the change x and then calculate [H3O+] using the given pH

104
Q

What is the formula for Ka?

A

PORK but only with aqueous solution

105
Q

What happens to the pH when an acid is diluted?

A

pH increases

106
Q

What happens to the pH when a base is diluted?

A

pH decreases

107
Q

What determines the pH of a buffer solution?

A

Determined by the pKa of the acid and the relative concentration of the acid and its conjugate base

108
Q

What flask is used when creating a standard solution?

A

Volumetric flask

109
Q

How do you identify conjugate acid/base pairs?

A

There should only be a difference of H+

110
Q

How do Aboriginal and Torres Strait Islander Peoples use their knowledge of acids and bases?

A

They use it for both medicinal and nutritional purposes

111
Q

What is an example of how Aboriginal and Torres Strait Islanders used their knowledge of acids and bases for nutritional purposes?

A

They ate Quandong a plant that contains high levels of nutritional vitamin C

112
Q

What is an example of how Aboriginal and Torres Strait Islanders used their knowledge of acids and bases for medicinal purposes?

A

They used clays which are alkaline to treat stomach issues as basic clays would neutralise the stomach acid

113
Q

What is the equivalent point?

A

When the reaction has reached a specific stoichiometric ratio of reactants. The number of H+ is equal to the number of OH-

Chemistry - Year 12 (5 decks)

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