Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

A LEVEL INORGANIC CHEMISTRY > Acids, bases and buffers > Flashcards

Acids, bases and buffers Flashcards

1
Q

Lewis acid

A

electron pair acceptor

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

Lewis base

A

electron pair donor

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

Bronsted Lowry base

A

proton acceptor

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

Bronsted-Lowry acid

A

proton donor

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

Dibasic acid

A

can form 2 conjugate bases

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

Conjugate acid base

A

HA + B -> HB+ + A-
acid + base
Conjugate acid + conjugate base

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

tribasic acid

A

can form 3 conjugate bases

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

Strong acid

A

completely dissociate in aqueous solutions to produce H+ ions

large Ka
smaller pKa

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

Weak acid

A

partially dissociate in aqueous solutions to produce H+ ions

small Ka
larger pKa

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

Acid dissociation constant

A

ka = [H+][A-] / [HA] = [H+]^2/[HA]

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

pH

A

-log10[H+]

measure of hydrogen ion concentration in solution

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

[H+] from pH

A

10^-pH

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

[H+] from acid dissociation constant

A

√(ka x [HA])

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

pKa

A

-log10Ka

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

Ionic product of water formula

A

Kw = [OH-][H+] = 1 x 10^-14

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

Buffer solution

A
  1. solution that resists change in pH
  2. when small quantity of acid or alkali is added
17
Q

Ka of buffer solution

A

[salt] x [H+] / [HA]

18
Q

Concentrations after dilution

A

(intital volume/total volume) x conc

19
Q

End point

A

point where pH changes rapidly

20
Q

Equivalence point

A

point where enough acid has been added to react completely with all the base

21
Q

Larger Ka, smaller pKa

A
  1. stronger acid
  2. dissociates more readily in solution
  3. equilibrium lies more to the right
22
Q

Limitations of Ka for stronger weak acids

A
  1. [HA] equilibirum ~ [HA] undissociated
  2. [HA] is bigger than [H+]
  3. Negligible dissociation of H2O
23
Q

Buffer explanation

A
  1. weak acid and soluble salt of weak acid
  2. H+ added, conjugate base reacts, equilibrium shift to the left
    3.OH- added, H+ bond, equilibrium shifts to the right
24
Q

Carbonic acid hydrogencarbonate

A

CO2(g) +H2O(l) ⇌ H2CO3(aq) ⇌ H+(aq) +HCO3-(aq)

  1. maintains blood pH 7.4
  2. H+ shifts both equilibrium to the left
  3. OH- shifts equilibrium to the right
25
Q

Phenopthalein

A

base - colourless
acid- pink
pH change 9
kln 10^-9

26
Q

Methyl orange

A

base - orange
acid- yellow
pH change 4
kln 10^-4

27
Q

Equilibrium shift of indicators

A

kln = [H+][ln-] / [Hln]

Halfway point [ln-] = [Hln]

28
Q

Draw strong base, strong acid

A
29
Q

Draw strong base, weak acid

A
30
Q

Draw weak base, weak acid

A
31
Q

Draw weak base, strong acid

A

A LEVEL INORGANIC CHEMISTRY (16 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions