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AL. OCR Chemistry > acids + bases > Flashcards

acids + bases Flashcards

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1
Q

Ka =

A

[H+] [A-] / [HA]

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2
Q

Kc =

A

[products] / [reactants]

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3
Q

Gibbs free energy (Δ G) =

A

= Δ H − T Δ S

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4
Q

pH =

A

-log[H+]

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5
Q

[H+] =

A

10 -pH

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6
Q

ionic product of water (KW) at 298K

A

1x10-14 mol2dm-6

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7
Q

why is [H+] larger at higher temps (for water)

A

because temp increase favours endothermic reaction, shifting equilibrium to right ∴ KW increases ∴ [H+] increases

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8
Q

how can you tell if something is a catalyst

A

it is expressed in the rate equation but not in the stoichiometric equation

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9
Q

assumptions made about weak acids (2)

A

1) [HA] at equ. ≈ [HA] initial

2) [A-] ≈ [H+] because [H+] from water is negligable

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10
Q

eq. ionic product of water (Kw)

A

[H+][OH-]

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11
Q

eq. pH of water

A

[H+] = √Kw

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12
Q

eq. pH of diluted strong acid

A

[H+] x (old vol / new vol) —> -log(ans)

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13
Q

effect of temperature on pH of water

A

temp increase = equilibrium shift to the right
[H+] and [OH-] INCREASE
Kw increase, pH decrease

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14
Q

effect of temp on neutrality of water

A

no effect, as [H+] = {OH-] still

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15
Q

eq. for calculating pH of a strong base

A

[H+] = Kw/ [OH-]

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16
Q

eq. Ka of weak acids in aqueous solution with nothing else added

A

Ka = [H+]² / [HA]

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17
Q

bronsted-lowrey acid

A

a proton donor

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18
Q

bronsted-lowrey base

A

a proton acceptor

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19
Q

monobasic acid

and eg.

A

an acid that releases 1 H+ ion per molecule

eg. = HCl

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20
Q

dibasic acid

and eg.

A

an acid which releases 2 H+ ions per molecules

eg. H2SO4

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21
Q

acid + metal =

A

salt and hydrogen

22
Q

acid + carbonate =

A

salt + water + CO2

23
Q

acid + base =

A

salt + water

24
Q

conjugate acid-base pair

A

2 species which can be converted Ito each other by the transfer of a proton

25
Q

2 ways of making an acidic buffer

A

1) weak acid and one of its salts

2) mix of excess weak acid and strong base

26
Q

2 ways of making an basic buffer

A

1) weak base and one of its salts

2) mixture of an excess of weak base and strong

27
Q

pH blood plasma has to be

A

7.35-7.45

28
Q

buffer system in the body

A

carbonic acid-hydrogen carbonate

29
Q

equilibrium for body buffer system

A

H2CO3 ⇌ H+ + HCO3

30
Q

what happens to body equilibrium when H+ added

A

[H+] increases
[H+] reacts with conjugate base HCO3-
eq. moves left, making more H2CO3, removing H+

31
Q

what happens to body equilibrium when OH- added

A

[OH-] increases
small conc go H+ react w OH-
H2CO3 dissociates to restore H+ ions
eq. shifts right, making more HCO3- and H+

32
Q

how does body prevent build up of H2CO3

A

converts it to CO2 which is exhaled by lungs

33
Q

weak acid

A

do not fully dissociate

34
Q

derivatives of carboxylic acid (4)

A
  • ester
  • acyl chloride
  • acid anhydride
  • amide
35
Q

methyl orange can always be used with….

A

strong acid

36
Q

phenolphalien can always be used with…

A

strong base

37
Q

pH weak acid

A

[H+] = √ KA x [HA]

38
Q

d. indicator

A

weak acids which have a different colour to their conjugate base

39
Q

relationship between PKa and Ka

A

PKa = -log(Ka)

40
Q

equation for: pH of mixture when H+ is in excess

weak acid

A

= H+ = Ka x [HA]/[A-]

41
Q

equation for: pH of mixture when OH- is in excess

A

H+ = KW/[OH-]

42
Q

equation for: pH of mixture when H+ is in excess

strong acid

A

pH = -log(H+)

43
Q

acid + metal ->

A

salt + hydrogen

44
Q

acid + carbonate ->

A

salt + CO2 + H2O

45
Q

acid + base ->

A

salt + water

46
Q

acid + alkali ->

A

salt + water

47
Q

the bigger the value of Ka the further the eq is to the….

A

RIGHT

48
Q

stronger acids have …

A

larger Ka , smaller pKA

49
Q

what is pKa used for?

A

comparing

50
Q

equivalence point

A

the point in a titration where a volume of one solution has reacted exactly with a volume of the other

51
Q

end point of titration

A

indicator contains equal vols of HA and A-

AL. OCR Chemistry (20 decks)

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