Topic 12: Acid-base Equilibria 1️⃣ Flashcards

1
Q

Define a bronsted lowry acid

A

Proton donor

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2
Q

Define a bronsted lowry base

A

Proton acceptor

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3
Q

Define a bronsted lowry conjugate acid

A

Species formed when a base accepts a proton

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4
Q

Define a bronsted lowry conjugate base

A

The species formed when a proton is removed from a base

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5
Q

Define strong acids

A

An acid that almost completely dissociates into ions when in aqueous solution

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6
Q

Define a weak acid

A

An acid that only partially dissociates when in aqueous solution

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7
Q

Give the equation to calculate pH

A

pH = -log[H+]

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8
Q

Give the equation to calculate conc of H+ ions using pH

A

[H+] = 10^-pH

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9
Q

Give the equation to calculate the [H+] in weak acids

A

[H+] [A-]
Ka = ————-
[HA]

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10
Q

Give the equation to calculate pKa

A

pKa = -logKa

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11
Q

How do you calculate Ka from pKa

A

Ka = 10^-pKa

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12
Q

What does a low pKa value indicate

A

Strong acid

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13
Q

What is the effect of diluting strong acids

A

If you dilute a strong acid 10 times its pH will increase by one unit
Diluting it 100 times would therefore increase the pH by two units

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14
Q

How do weak acids behave upon dilution

A

Weak acids are not fully dissociated in solution so diluting them causes the equilibrium to shift to oppose the change.
This means a 10 times dilution of a weak acid would increase the pH by less than one unit

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15
Q

What is the equilibrium constant for Kw

A

Kw = [H+][OH-]

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16
Q

How does temp affect the value of Kw

A

The forward reaction in the equilibrium of water is endothermic and is therefore favoured when the temp of water is increased.
As a result as temp increases, more H+ ions are produced making water more acidic

17
Q

Give the equation for pKw

A

pKw = -log Kw

18
Q

Give the equation for Kw from pKw

A

Kw = 10^-pKw

19
Q

What is the equivalence point

A

When the acid and base have reacted together in the same proportions as dictated by the stoichiometric equation

20
Q

What does the end point refer to

A

When the colour of the indicator just changes colour

21
Q

What does the pH at the equivalence point depend on ?

A

The combination of acid and base used
Eg strong acid strong base, weak acid strong base etc.

22
Q

Describe the pH titration curve for a strong acid strong base titration

A
  • starts at approx pH 14 finishes at approx pH 0.5 (uses full scale)
  • pH only falls by a very small amount until large steep section quite near the equivalence point
23
Q

What is plotted on the x and y axis of a pH titration curve ?

A

x axis = volume of acid added
y axis = pH

24
Q

Describe the pH titration curve for a weak acid strong base titration

A
  • starts at approx pH 14 finishes at approx pH 3 (uses 3/4 of scale)
  • curve like that of strong acid strong base pH titration up to equivalence point
  • past the equivalence point the mixture acts as a buffer resisting any fluctuations in pH upon further addition of acid
25
Q

Describe the pH titration curve for a strong acid weak base titration

A
  • curve starts at approx pH 11 finishes at approx pH 0.5 (uses 3/4 of scale)
  • when acid is first added curve starts to fall but then levels out because buffer solution has been formed
  • steep section to meet equivalence point
26
Q

Describe the pH titration curve for a weak acid weak base titration

A
  • starts at approx pH 11 finishes at approx pH 3
  • no steep section to curve , instead ‘point of inflexion’ - why it is difficult to do titration of weak acid weak base with indicator
27
Q

An acid-base indicator is either…

A

A weak acid or weak base
Most are weak acids (HIn)

28
Q

How is the dissociation of an indicator that is a weak acid in aq solution represented

A

HIn (aq) ⇌ H+ (aq) + In- (aq)

HIn and In- have different colours in aqueous solution

29
Q

What does the equilibrium constant KIn give us

A

There will be a stage where [HIn] = [In-] indicator in the case of methyl orange will appear orange
The exact pH when this is reached can be determined using KIn

30
Q

How can we determine a suitable indicator for an acid-base titration using the pH titration curve

A

Each indicator has an exact pH range
So long as the exact pH range of the indicator falls within the steep section of the curve it is a suitable indicator

31
Q

Give the Henderson-Hasselbalch equation used to calculate the pH of a buffer solution

A

pH = pKa + log [salt] / [acid]

32
Q

What is a buffer solution

A

A solution that minimises the change in pH when a small amount of either acid or alkali is added