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Chemistry > Acids and Bases > Flashcards

Acids and Bases Flashcards

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1
Q

strong acid - [H+] =

A

10^-pH

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2
Q

strong acid - -log(pH) =

A

[H+]

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3
Q

define Bronsted-Lowry acid

A

proton donor

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4
Q

define Bronsted-Lowry base

A

proton acceptor

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5
Q

number of protons in a molecule of monoprotic acid

A

1

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6
Q

number of protons in a molecule of diprotic acid

A

2

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7
Q

equation of Kw in the ionic production of water

A

Kw = [H+][OH-] = Kc[H2O]

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8
Q

Equation of Kc in the ionic production of water

A

Kc = [H+][OH-]/[H2O]

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9
Q

the effect of temperature on the pH of water and why

A

as temperature increases, pH decreases (as more [H+])

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10
Q

the effect of temperature on the ionic equilibrium of water

A

equilibrium moves to the right to oppose change

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11
Q

equation for ionic production of water

A

H2O -> H+ + OH-

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12
Q

is enthalpy change of the ionic product of water endo or exothermic

A

endothermic

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13
Q

how can water have a lower pH but still be neutral?

A

because H+ increases but it still = OH-

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14
Q

in pure water what does [OH-] =

A

[H+]

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15
Q

in pure water, what does Kw =

A

[H+]^2

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16
Q

in a strong base what does [H+] =

A

Kw/[OH-] or 10^-14/[OH-]

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17
Q

steps in calculating pH of mixtures of strong acids and strong bases

A

calculate mols of H+ and OH-
calculate XS mols H+ or OH-
calculate conc. of XS H+ or OH-
calculate pH

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18
Q

equation for a strong acid

A

HX -> H+ + X-

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19
Q

equation for a weak acid

A

HX H+ + X-

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20
Q

is HCl strong or weak

A

strong

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21
Q

are carboxylic acids strong or weak

A

weak

22
Q

is sulphuric acid strong or weak

A

strong

23
Q

is nitric acid strong or weak

A

strong

24
Q

name a diprotic acid

A

sulphuric acid

25
Q

is barium hydroxide strong or weak

A

strong

26
Q

is potassium hydroxide strong or weak

A

strong

27
Q

is ammonia strong or weak

A

weak

28
Q

is sodium hydroxide strong or weak

A

strong

29
Q

name a dibasic base

A

barium hydroxide

30
Q

for a weak acid Ka =

A

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

31
Q

for a weak acid pKa =

A

-log Ka

32
Q

units for Ka

A

moldm^-3

33
Q

relationship between Ka and strength of acid

A

the bigger the value the stronger the acid

34
Q

relationship between pKa and strength of acid

A

the smaller the value the stronger the acid

35
Q

in a solution of a weak acid in water with nothing else added [H+] =

A

[A-]

36
Q

in a solution of a weak acid in water with nothing else added [HA] initial =`

A

[HA]

37
Q

in a solution of a weak acid in water with nothing else added Ka =`

A

[H+]^2/[HA]

38
Q

equation for reaction of a weak acid and a strong base

A

HA + OH- -> A- + H2O

39
Q

steps to finding the pH in reactions between weak acids and strong bases for XS HA

A 
calculate mols HA
calculate mols OH-
calculate mols XS
calculate mols HA left and A- formed
use Ka to find [H+]
find pH
40
Q

steps to finding the pH in reactions between weak acids and strong bases for XS OH-

A 
calculate mols HA
calculate mols OH-
calculate mols XS
calculate conc. OH-
use Kw to find H+
find pH
41
Q

steps to finding the pH in reactions between weak acids and strong bases for when HA = OH-

A

calculate mols HA
calculate mols OH-
calculate mols XS
pH = pKa of weak acid

42
Q

2H+ +CO3 2- ->

A

H2O + CO2

43
Q

H+ + HCO3- ->

A

H2O + CO2

44
Q

H+ + NH3 ->

A

NH4+

45
Q

define equivalence point

A

mols of alkali equals mols of acid present

46
Q

define buffer solutions

A

solution resists changes in pH when small amounts of acid or alkali are added

47
Q

what sort of buffer solutions have pH > 7

A

basic buffer solutions

48
Q

what sort of buffer solutions have pH < 7

A

acidic buffer solutions

49
Q

component in acidic buffer solution

A

weak acid + one of its salts

50
Q

component of basic buffer solution

A

weak base and one of its salts

51
Q

which equation can you use to find pH of acidic buffer solutions

A

Ka = [HA]/[A-]

Chemistry (24 decks)

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