3.9 Acid-Base Equilibria Flashcards

1
Q

What is the Lowry-Brønsted theory?

A

The Lowry-Brønsted theory states that acid-base equilibria involves the transfer of protons between substances and substances can be classified as acids or bases depending on their interaction with protons.

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2
Q

Define a Lowry-Brønsted acid and give an example

A

A Lowry-Brønsted acid is a proton donor.
Example: Ammonium ions (NH +)

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3
Q

Define a Lowry-Brønsted base and give an example

A

A Lowry-Brønsted base is a proton acceptor.
Example: Hydroxide ions (OH-)

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4
Q

Describe the difference between a strong acid and a weak acid

A

A strong acid dissociates almost completely in water which means nearly all the H+ ions are released.
A weak acid only partially dissociates in water so only a small number of H+ ions are released.

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5
Q

Describe the difference between a strong base and a weak base

A

A strong base dissociates almost completely in water so nearly all the OH- ions are released.
A weak base only partially dissociates in water so only a small number of OH- ions are released.

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6
Q

Give an expression for pH in terms of [H+]

A

pH = -log10[H+]
Equivalently: [H+] = 10-pH

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7
Q

What is the relationship between pH and hydrogen ion concentration, [H+]?

A

The pH scale is a measure of hydrogen ion concentration. The lower the pH, the higher the concentration of hydrogen ions.

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8
Q

What is the hydrogen ion concentration of a solution of hydrochloric acid which has a pH of 2.0?

A

[H+] = 10(-pH) = 10(-2)
=0.01 mol dm-3

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9
Q

Give examples of strong acids and state the pH range which indicates a strong acid

A

Hydrochloric acid (HCl), sulfuric acid (H2SO4), nitric acid (HNO3)
pH range of strong acids: 0-3

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10
Q

Give examples of weak acids and state the pH range which indicates a weak acid

A

Ethanoic acid (CH3COOH), hydrogen sulfide (H2S), any organic carboxylic acid
pH range of weak acids: 4 to just below 7

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11
Q

Give examples of strong bases and state the pH range which indicates a strong base

A

Sodium hydroxide (NaOH), potassium hydroxide (KOH), calcium hydroxide (Ca(OH)2)
pH range of strong bases: 12-14

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12
Q

Give examples of weak bases and state the pH range which indicates a weak base

A

Ammonia (NH3), methylamine (CH3NH2)
pH range for weak bases: just above 7 up to 11

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13
Q

What is the acid dissociation constant, Ka?

A

The acid dissociation constant, Ka, is a measure of how strong an acid is in a solution.

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14
Q
A
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15
Q

What are the units for Ka?

A

mol dm-3

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16
Q

How does the strength of an acid relate to the value of Ka?

A

Ka is the equilibrium constant for the dissociation of an acid: HA ⇌ H+ + A-
The stronger the acid, the further to the right the equilibrium lies so there is a higher concentration of products. This causes Ka to increase.

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17
Q

Why is Ka used to find the pH of a weak acid?

A

Weak acids only partially dissociate in water so the concentration of H+ ions is not the same as the acid concentration (as with strong acids). This means the pH cannot be found using [H+] and so Ka is used instead.

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18
Q

Give the formula used to find Ka of a weak acid

A
19
Q

Given that Ka for propanoic acid at 298 K is 1.3 x 10-5 mol dm-3, what is the pH of 0.02 mol dm-3 of propanoic acid at 298 K?

A
20
Q

What is the difference between describing an acid/base as ‘concentrated’ compared to ‘strong’?

A

‘Concentrated’ implies there are many moles per dm3.
‘Strong’ relates to the dissociation of the substance and implies the acid/base almost completely dissociates in water.

21
Q

Give the formulas used to convert between Ka and pKa

A

pKa = -log10[Ka]
Ka = 10(-pKa)

22
Q

What is the pKa of an acid which has a Ka value of 1.60 x 10-2 mol dm-3?

A

pKa = -log10(Ka)
= -log10(1.6 x 10-2)
= 1.80 (3.s.f)

23
Q

Give the equation for the ionic product of water

A
24
Q

Derive the ionic product of water using the equation for the ionisation of water

A
25
Q

What is the pH of pure water at room temperature?

A

7

26
Q

How does the pH at which water is neutral ([OH] = [H+]) change as temperature increases?

A

In the equilibrium of water, the forwards reaction is endothermic and is therefore favoured when the temperature of the water is increased. So, the pH at which water is neutral (when the concentration of H+ and OH- is the same) decreases when the temperature is increased.

27
Q

Given that Kw at 298 K is 1.0 x 10-14 mol2 dm-6, what is the pH of 0.10 mol dm-3 NaOH at 298 K?

A
28
Q

What is a pH curve?

A

Graphs which plot pH against volume of acid or base added are called pH curves and can be used to help identify the point of neutralisation of a solution.

29
Q

What is the equivalence point on a pH curve?

A
30
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31
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32
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33
Q

What is a buffer solution?

A

A buffer solution is a solution which is able to resist changes in pH when small volumes of acid or base are added.
A buffer solution is commonly formed from a weak acid and its salt or a weak base and its salt. This produces a mixture containing H+ ions and a large pool of OH- ions which helps to resist any change in pH.

34
Q

How is an acidic buffer solution made by mixing sodium ethanoate with ethanoic acid?

A
35
Q

Consider the buffer solution made by mixing sodium ethanoate with ethanoic acid. How does the pH change when a small amount of acid is added?

A
36
Q

Explain the significance of buffer solutions in nature

A

Buffer solutions are common in nature in order to keep systems regulated. Enzymes in living organisms often require an optimum pH and this can be maintained by a buffer solution.

37
Q

Why are buffers used in industrial processes?

A

Industrial processes use buffer solutions to maintain the optimum reaction conditions for large scale manufacturing.

38
Q

Give an example of where buffer solutions are used in industrial processes

A

Buffers are used in fermentation. Buffer solutions are added before fermentation begins to prevent the solution becoming too acidic.
They are also used in fabric dyeing processes and to perform chemical analysis.

39
Q

Define salt hydrolysis

A

A reaction where one of the ions from a salt reacts with water to form an acidic or basic solution.

40
Q

What needs to be considered when selecting an indicator for a titration?

A

The indicator chosen for a titration must change colour at exactly the end point of the titration. The indicator should change colour over a narrow pH range, which coincides with the vertical section of the pH curve.

41
Q

Give an example of an indicator which can be used in a titration and describe its colour change

A
42
Q

Why should a pH meter be used instead of an indicator in weak acid/weak base titrations?

A

In weak acid/weak base titrations there is no sharp pH change so it is very difficult to successfully use an indicator to get an accurate point of neutralisation. A pH meter should be used instead since it will be more accurate and precise.

43
Q
A