Acids and Bases Flashcards

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

22
Q

is sulphuric acid strong or weak

23
Q

is nitric acid strong or weak

24
Q

name a diprotic acid

A

sulphuric acid

25
is barium hydroxide strong or weak
strong
26
is potassium hydroxide strong or weak
strong
27
is ammonia strong or weak
weak
28
is sodium hydroxide strong or weak
strong
29
name a dibasic base
barium hydroxide
30
for a weak acid Ka =
[H+][A-]/[HA]
31
for a weak acid pKa =
-log Ka
32
units for Ka
moldm^-3
33
relationship between Ka and strength of acid
the bigger the value the stronger the acid
34
relationship between pKa and strength of acid
the smaller the value the stronger the acid
35
in a solution of a weak acid in water with nothing else added [H+] =
[A-]
36
in a solution of a weak acid in water with nothing else added [HA] initial =`
[HA]
37
in a solution of a weak acid in water with nothing else added Ka =`
[H+]^2/[HA]
38
equation for reaction of a weak acid and a strong base
HA + OH- -> A- + H2O
39
steps to finding the pH in reactions between weak acids and strong bases for XS HA
``` calculate mols HA calculate mols OH- calculate mols XS calculate mols HA left and A- formed use Ka to find [H+] find pH ```
40
steps to finding the pH in reactions between weak acids and strong bases for XS OH-
``` calculate mols HA calculate mols OH- calculate mols XS calculate conc. OH- use Kw to find H+ find pH ```
41
steps to finding the pH in reactions between weak acids and strong bases for when HA = OH-
calculate mols HA calculate mols OH- calculate mols XS pH = pKa of weak acid
42
2H+ +CO3 2- ->
H2O + CO2
43
H+ + HCO3- ->
H2O + CO2
44
H+ + NH3 ->
NH4+
45
define equivalence point
mols of alkali equals mols of acid present
46
define buffer solutions
solution resists changes in pH when small amounts of acid or alkali are added
47
what sort of buffer solutions have pH > 7
basic buffer solutions
48
what sort of buffer solutions have pH < 7
acidic buffer solutions
49
component in acidic buffer solution
weak acid + one of its salts
50
component of basic buffer solution
weak base and one of its salts
51
which equation can you use to find pH of acidic buffer solutions
Ka = [HA]/[A-]