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A Level Chemistry Year 2 > Acids, Bases and pH > Flashcards

Acids, Bases and pH Flashcards

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1
Q

What is the Brønsted-Lowry theory?

A

A theory that describes acid-base interactions in terms of proton transfer between chemical species

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2
Q

What are Brønsted-Lowry acids?

A

Proton donors

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3
Q

Why are Brønsted-Lowry acids called proton donors?

A

They release hydrogen ions when they’re mixed with water

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4
Q

Write the general equation for a general Brønsted-Lowry acid (HA) mixed with water

A

HA(aq) + H2O(l) ⇌ H3O+(aq) + A-(aq)

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5
Q

What are Brønsted-Lowry bases?

A

Proton acceptors

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6
Q

Why are Brønsted-Lowry bases called proton acceptors?

A

When they’re in a solution, they grab hydrogen ions from water molecules

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7
Q

Write the general equation for a general Brønsted-Lowry base (B) in a solution

A

B(aq) + H2O(l) ⇌ BH+(aq) + OH-(aq)

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8
Q

What do acids and bases do in water?

A

Break up into positive and negative ions (called dissociation)

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9
Q

What do strong acids do in water?

A

They dissociate almost completely in water - nearly all H+ ions are released

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10
Q

What do strong bases do in water?

A

They dissociate almost completely in water

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11
Q

What do weak acids do in water?

A

They dissociate only partially - so only a small amount of H+ ions are formed

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12
Q

What do weak bases do in water?

A

They only slightly dissociate

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13
Q

Describe the equilibrium position in the reversible reaction when a strong acid mixes with a water

A

The equilibrium lies far to the right, which is why nearly all the H+ ions are released

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14
Q

Describe the equilibrium position in the reversible reaction when a weak acid mixes with a water

A

The equilibrium lies far to the left, which is why only a small amount of the H+ ions are released

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15
Q

What are monobasic acids?

A

An acid that releases one H+ ion per molecule

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16
Q

What are monobasic acids also called?

A

Monoprotic acids (because an H+ ion is just a proton)

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17
Q

Give 2 examples of monobasic acids

A

HCl

HNO3

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18
Q

What are dibasic acids?

A

An acid that releases two H+ ion per molecule

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19
Q

Give an example of dibasic acids

A

H2SO4

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20
Q

What are tribasic acids?

A

An acid that releases three H+ ions per molecule

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21
Q

Give an example of a tribasic acid

A

H3PO4

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22
Q

What are tribasic and dibasic acids examples of?

A

Polyprotic acids

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23
Q

What is a species?

A

A type of chemical - could be a molecule, atom or an ion

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24
Q

What are conjugate pairs?

A

Species that are linked by the transfer of a proton (H+ ion)

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25
Q

What is the general equation for the equilibrium reaction between an acid and a base? Show the conjugate pairs

A

HA + B ⇌ BH+ + A-

HA ⇌ A- is conjugate pair 1 (acid1 —> base1)
B ⇌ BH+ is conjugate pair 2 (base2 —> acid2)

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26
Q

In a balanced chemical equation, where will you find conjugate pairs?

A

On either side of the chemical equation

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27
Q

Describe a conjugate pair and the proton transfer between them

A

When a conjugate acid loses a proton, it forms a conjugate base. But when this conjugate base gains a proton, it forms a conjugate acid

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28
Q

What is the conjugate acid when water reacts with acids?

A

H3O+

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29
Q

What is the conjugate base when water reacts with bases?

A

OH-

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30
Q

What is the general equation for when an acid dissolves in water? State the conjugate pairs

A

HA + H2O ⇌ H3O+ + A-

HA (acid1) ⇌ A- (base1)
H2O (base2) ⇌ H3O+ (acid2)

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31
Q

What is the general equation for when a base dissolves in water? State the conjugate pairs

A

B + H2O ⇌ BH+ + OH-

B (base1) ⇌ BH+ (acid1)
H20 (acid2) ⇌ OH- (base2)

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32
Q

How do you identify conjugate pairs?

A

By looking at the chemical equation for 2 species that are linked by proton transfer

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33
Q

Two species can’t be a conjugate pair if…?

A

… they are on the same side of the chemical equation

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34
Q

What are the products of the reaction between a reactive metal and acid?

A

Salt and Hydrogen gas

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35
Q

In the reaction between a metal and an acid, what is oxidised and what is reduced?

A

The metal atoms donate electrons to the H+ ions in the acid solution. The metal atoms are oxidised and the H+ ions are reduced

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36
Q

What are the products of the reaction between an acid and a carbonate?

A

Carbon dioxide, water and a salt

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37
Q

What is the product when an acid reacts with a base or an alkali?

A

Water

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38
Q

What ions are produced in the reaction between an acid and an alkali?

A

Acids produce H+ ions and the alkalis produce OH- ions when dissolved in water

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39
Q

What is an alkali?

A

A base that releases OH- ions when they dissolve in water

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40
Q

What type of reaction is Acid + Base?

A

Neutralisation

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41
Q

What is the ionic equation for the reaction between an acid and an alkali?

A

H+(aq) + OH-(aq) —> H2O(l)

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42
Q

What is the ionic equation for the reaction between an acid and an insoluble base?

A

H+(aq) + O2-(s) —> H2O(l)

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43
Q

What is pH?

A

A measure of the hydrogen ion concentration in a solution

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44
Q

What is the equation for pH?

A

-log[H+]

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45
Q

What is the range of the pH scale?

A

0 (very acidic) to 14 (very alkaline)

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46
Q

What is the pH of water?

A

pH7 (neutral)

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47
Q

For a monobasic acid, how can you work out the concentration of the H+ ion if you know the concertation of the acid?

A

Each mole of acid produces one mole of hydrogen ions, so the H+ concentration is the same as the acid concentration

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48
Q

What are the products when water dissociates?

A

Hydroxonium ions and Hydroxide ions

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49
Q

What equilibrium exists in water, then simplify it?

A

H2O(l) + H2O(l) ⇌ H3O+(aq) + OH-(aq)

remove H2O from both sides:

H2O ⇌ OH-(aq) + H+(aq)

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50
Q

Why does the equilibrium for the dissociation of water lie far to the left?

A

Because water only dissociates a tiny bit, so most is just H2O

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51
Q

What is the ionic product of water?

A

An equilibrium constant specific to the dissociation of water at a constant temperature

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52
Q

What is the equation for the ionic product of water?

A

Kw = [H+][OH-]

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53
Q

What are the units of Kw?

A

mol^2dm^-6 (always because you’re multiplying 2 concentrations together)

54
Q

What type of process is the dissociation of water?

A

Endothermic (+ΔH)

55
Q

What happens to the value of Kw at a fixed temperature?

A

It remains constant

56
Q

What happens to the position of the equilibrium (and value of Kw) when the temperature of the solution is increased?

A

The dissociation of water is endothermic, therefore the equilibrium shifts to the right to (dissociates more) so the value of Kw increases

57
Q

What happens to the position of the equilibrium (and value of Kw) when the temperature of the solution is decreased?

A

The dissociation of water is endothermic, therefore the equilibrium shifts to the left to (dissociates less) so the value of Kw decreases

58
Q

What can be said about the pH of water?

A

It is not always 7, it changes depending on the temperature

59
Q

How do you find the ionic product of pure water?

A

Kw = [H+]^2

60
Q

Why is the equation for the ionic product of pure water, Kw = [H+]^2?

A

In pure water, there is always one H+ ion for each OH- ion, so the concentrations are the same so equal to [H+]^2

61
Q

How do you find the pH of a strong base?

A
  • Find the values of Kw and [OH-]
  • Substitute into equation for ionic product of water and solve for [H+]
  • Substitute this value into the equation for pH
62
Q

For a strong base, how do you find [OH-] if you know the concentration of the base?

A

Strong bases fully ionise in water - donating one mole of OH- ions per mole of base. Therefore concentration of base = [OH-]

63
Q

How do you find the concentration of a strong base if you know the pH?

A

-Use equation [H+] = 10^-pH to find the value of [H+]
-Substitute value of [H+] and Kw into equation for ionic product of water to work out [OH-]
= [OH-] = concentration of base

64
Q

What is the acid dissociation constant, Ka?

A

An equilibrium constant specific to weak acids that relates the acid concentration to the [H+] concentration

65
Q

What are the units of the acid dissociation constant?

A

mol dm^-3

66
Q

What is the equation for the acid dissociation constant?

A

Ka = [A-][H+] / [HA]start = [H+]^2 / [HA]

67
Q

What are the 2 assumptions made when finding Ka?

A
  • Only works for weak acids

- Because strong acids dissociate more, there is a significant difference between [HA] start and [HA] equilibrium

68
Q

How does temperature affect Ka?

A

The Ka is fixed at a given temeprature

69
Q

If dissociation is endothermic, what effect on Ka does increasing the temperature have?

A

Shifts the equilibrium to the right (dissociates more), so Ka increases

70
Q

If dissociation is endothermic, what effect on Ka does decreasing the temperature have?

A

Shifts the equilibrium to the left (dissociates less), so Ka decreases

71
Q

If dissociation is exothermic, what effect on Ka does increasing the temperature have?

A

Shifts the equilibrium to the left (dissociates less), so Ka decreases

72
Q

If dissociation is exothermic, what effect on Ka does decreasing the temperature have?

A

Shifts the equilibrium to the right (dissociates more), so Ka increases

73
Q

What are the 4 steps to find the pH using Ka?

A

1: Write an expression for Ka for the weak acid
2: Rearrange to solve for [H+]^2
3: Take the square root of the number to find [H+]
4: Substitute [H+] into the pH equation

74
Q

What are the 4 steps to find the concentration of a weak acid using pH and Ka?

A

1: Substitute pH into the inverse pH equation to get [H+]
2: Write an expression for Ka
3: Rearrange equation to give concentration of acid
4: Substitute values of Ka and [H+] to solve for [HA]

75
Q

What are the 3 steps to find Ka of weak acid from concentration and pH?

A

1: Use the pH to find [H+]
2: Write an expression for Ka
Substitute values of [H+] and [HA] to find Ka

76
Q

What is pKa?

A

Logarithmic constant

77
Q

Why do scientists often use pKa instead of Ka?

A

Because Ka varies so much between different acids, it makes it easier to handle numbers

78
Q

What is the equation for pKa?

A

pKa = -log(Ka)

79
Q

What is the equation for Ka if given the value of pKa?

A

Ka = 10^-pKa (inverse log)

80
Q

The larger the value of pKa, the…?

A

weaker the acid

81
Q

What are the usual pH values for a weak acid?

A

pH2-pH5

82
Q

What is a buffer?

A

A solution that minimises changes in pH when small amounts of acid or base are added

83
Q

What is the job of a buffer?

A

To not stop the pH from changing, but to make the change very slight when an acid or base are added

84
Q

In what situation do buffers only work in?

A

When small amounts of acid or base are added

85
Q

Why do buffers only work for small amounts of acid or bases?

A

Because if add too much acid or base, the buffer won’t be able to cope

86
Q

What are the 2 types of buffers?

A

Acidic buffers

Basic buffers

87
Q

What is the pH range of an acidic buffer?

A
88
Q

What are the 2 ways of making an acidic buffer?

A
  • From a weak acid and the salt of its conjugate base

- From an excess of weak acid and some strong alkali

89
Q

How do you make an acidic buffer from a weak acid and the salt of its conjugate base?

A

Mix a weak acid and the salt of its conjugate base. A small amount of the acid will dissociate, but most will be undissociated. The salt will fully dissociate to form the conjugate base of the acid in the solution. The solution will contain a mixture of weak acid and its conjugate base, so would act as an acidic buffer

90
Q

How do you make an acidic buffer from an excess of weak acid and some strong alkali?

A

Mix the excess of weak acid and some strong alkali. Some of the acid neutralises to make a salt, but some is left un-neutralised. The reaction mixture would then contain a weak acid and its conjugate base, so would act as an acidic buffer

91
Q

When making an acidic buffer from an excess of weak acid and some strong alkali, why do you need to have an excess amount of acid rather than an excess amount of alkali?

A

Because there was an excess amount of alkali, all of the acid would react, so there’d be no acid left

92
Q

What does an acidic buffer solution contain?

A

Lots of dissociated acid and the acids conjugate base

93
Q

When you prepare an acidic buffer, what equilibrium is set up between the weak acid and the conjugate base?

A

HA ⇌ H+ + A-

94
Q

How does an acidic buffer work?

A

When you alter the concentration for H+ or OH- ions in the buffer solution, the equilibrium position shifts to counteract the change. The conjugate base can react to ‘mop up’ excess H+ ions and the conjugate acid can dissociate to release H+ ions if there’s too much base

95
Q

How does an acidic buffer resist an acid?

A

If you add a small amount of acid, the H+ concentration increases. Most of the extra H+ ions join the A- ions to form HA. This causes the equilibrium to shift to the left, meaning the H+ concentration reduces to its original level, so the pH stays the same

96
Q

How does an acidic buffer resist a base?

A

If a small amount of base is added, the OH- concentration increases. Most of the extra OH- ions react with the H+ ions to form water, decreasing the H+ concentration. This causes the equilibrium to shift to the right, so that more of the acid dissociates and releases H+ ions, increasing the H+ concentration to its original value, so the pH stays the same

97
Q

What range of pH does blood need to be kept at?

A

Between pH 7.35 and pH 7.45

98
Q

What is the name of the buffer that controls the pH in our blood?

A

Carbonic acid-hydrogencarbonate buffer

99
Q

What is the equilibrium set up in the blood by the buffer?

A

H2CO3 ⇌ H+ + HCO3-

100
Q

How does the buffer system in the blood keep the pH the same if a small amount of acid is added?

A

The HCO3- ions from the carbonic acid-hydrogencarbonate buffer will react with the excess H+ ions, causing the equilibrium to shift left, reducing the H+ concentration

101
Q

How does the buffer system in the blood keep the pH the same if the concentration of H+ ions drops?

A

More H2CO3 molecules from the carbonic acid-hydrogencarbonate buffer will dissociate, so the equilibrium will shift to the right meaning that the concentration of H+ ions increases

102
Q

What process controls the levels of H2CO3 (carbonic acid) in the blood?

A

Respiration

103
Q

How does respiration control the levels of H2CO3 (carbonic acid) in the blood, and state the equilibrium set up?

A

By breathing out CO2, the level of H2CO3 is reduced because it moves the equilibrium to the right

H2CO3 ⇌ H2O + CO2

104
Q

How are the levels of HCO3- controlled in the body?

A

By the kidneys, if there is excess HCO3-, it is excreted out the body as urine

105
Q

What are the 2 assumptions you need to make when calculating the pH of an acidic buffer?

A
  • The salt of the conjugate base is fully dissociated, so the equilibrium concentration of A- is the same as the initial concentration of the salt
  • HA is only slightly dissociated, so its equilibrium concentration is the same as its initial concentration
106
Q

What are the 4 steps to calculate the pH of a buffer?

A

1: Write out the expression for Ka of a weak acid, and rearrange to solve for [H+]
2: Substitute the value of Ka and equilibrium concentrations into the expression
3: Solve the equation for [H+]
4: Substitute the value of [H+] into pH equation

107
Q

What are the 5 steps to calculate the equilibrium concentrations if, to make the buffer, you mixed an acid with a base?

A

1: Write out the equation for the neutralisation reaction
2: Calculate number of moles of acid and base at the start using volumes and concentration given in question
3: Use the molar ratios in the equation to work out the moles of acid and salt left at the end of the reaction
4: Calculate concentration of acid and salt in the buffer solution by dividing by the volume of the solution
5: Use these to calculate pH by using the Ka equation and pH equation

108
Q

What is a pH meter?

A

An electronic device that measures the pH of a solution

109
Q

How do you calibrate a pH meter?

A
  • Place the bulb of the pH meter into distilled water and allow the reading to settle, then adjust the reading to pH7
  • Do the same with 2 standard solutions of pH4 and pH10, making sure to rinse the probe off with distilled water each time
110
Q

What does a pH meter look like?

A

They have a probe that you place in the solution, and at the bottom of the probe there is a delicate bulb

111
Q

How do you use a pH meter after it has been calibrated?

A

Place the probe in the liquid and let the reading settle down

112
Q

What should you do to the pH meter after having taken a reading?

A

Rinse the probe with distilled water

113
Q

How do you plot a pH curve for a titration?

A

By plotting the pH of the titration mixture against the amount of base added as the titration goes on

114
Q

Compare the starting point for the pH graphs of strong acids and weak acids

A

A strong acid titration will start at a much lower pH than a weak acid titration

115
Q

Why does the graph on a pH curve increase by a large amount straight away?

A

To start with, adding small amounts of base has little effect on the pH of the solution

116
Q

For all of the pH graphs for the titration of an acid, except from the weak acid/weak base curve, what does the midpoint of the vertical part of the graph mean?

A

That is the end point of the titration, when all the acid is neutralised

117
Q

What can be said about the amount of weak base that needs to be added to a strong acid, compared to a strong base, for the pH to start increasing to pH7?

A

You need to add more weak base than strong base to a strong acid to cause a change in pH

118
Q

What can be said about the amount of weak base that needs to be added to a weak acid, compared to a strong base, for the pH to start increasing to pH7?

A

You need to add less strong base to a weak acid to see a large change in pH

119
Q

For a pH graph, what does the final pH depend on?

A

The strength of the base- the stronger the base the higher the pH is at the end

120
Q

What is an indicator?

A

A solution that changes colour to show you when the sample has been neutralised

121
Q

What are indicators and how doe they work?

A

They’re weak acids that have different coloured conjugate pairs. As the pH of the solution changes during a titration, the equilibrium concentrations of the conjugate pairs will also change

122
Q

What 2 indicators are used in acid-base titrations?

A

Methyl orange

Phenolphthalein

123
Q

How does phenolphthalein work as an indicator?

A

The protonated form is colourless, and the conjugate base is pink. At low pH, the concentration of H+ ions is high so most of the phenolphthalein is protonated, so the solution is colourless. As the pH rises, the concentration of H+ ions decreases, shifting the equilibrium to the right, so more of the phenolphthalein deprotonates, causing the solution to turn pink

124
Q

What is the equilibrium set up for the indicator phenolphthalein?

A

phenolphthalein-H ⇌ phenolphthalein- + H+

125
Q

How does methyl orange work as an indicator?

A

The protonated form is red and the conjugate base is yellow. At low pH, the concentration of H+ ions is high, so most pf the methyl orange is protonated, so the solution is red. As the pH increases, the concentration of H+ decreases, so the equilibrium shifts to the right, meaning more of the methyl orange deprotonates, causing the solution to start turning yellow

126
Q

What factors affect which indicator you should use for a titration?

A

You want an indicator that change colour over a narrow pH range, and one that changes colour at the end point of the titration

127
Q

For a strong acid/strong alkali titration, should you use methyl orange (colour change between pH3.1 and pH4.4), phenolphthalein (colour change between pH8.3 and pH10) or either?

A

Either, because there’s a rapid pH change over the range of both indicators

128
Q

For a strong acid/weak alkali titration, should you use methyl orange (colour change between pH3.1 and pH4.4), phenolphthalein (colour change between pH8.3 and pH10) or either?

A

On methyl orange, because the pH changes rapidly in the range of methyl orange, but not phenolphthalein

129
Q

For a weak acid/strong alkali titration, should you use methyl orange (colour change between pH3.1 and pH4.4), phenolphthalein (colour change between pH8.3 and pH10) or either?

A

Phenolphthalein, because the rapid pH change occurs over the phenolphthalein range, but not methyl orange

130
Q

For a weak acid/weak alkali titration, should you use methyl orange (colour change between pH3.1 and pH4.4), phenolphthalein (colour change between pH8.3 and pH10) or neither?

A

Neither, because there is no sharp change in pH, so neither indicator will work

131
Q

What do you have to use to find the end point of a weak acid/weak alkali titration?

A

A pH meter

132
Q

What is the pH range of an indicator?

A

The range in which the colour changes

A Level Chemistry Year 2 (7 decks)

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