3.1.12 Acids and bases Flashcards

1
Q

what is a Brønsted-Lowry acid?

A

a proton donor. e.g; Ammonium ions.

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2
Q

what is a Brønsted-Lowry ​base?

A

a proton acceptor. e.g; hydroxide ions

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3
Q

definition of a strong acid

A

an acid the completely dissociated to ions when in solution with pH 3-5

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4
Q

definition of a weak acid

A

an acid that only slightly dissociated when in solution with pH 0-1

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5
Q

what is a monoprotic acid?

A

an acid that donates one H+ from each molecule

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6
Q

what is a diprotic acid?

A

an acid that donates two H+ from each molecule

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7
Q

how do you find the pH of a strong acid?

A

pH = -log[H+]

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8
Q

how do you find the concentration of a strong acid?

A

[H+] = 10^-pH

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9
Q

how do you convert pKa into Ka?

A

Ka = 10^-pKa

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10
Q

what is the value of Kw?

A

10^-14

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11
Q

how do you find the concentration of a weak acid?

A

[HA] = [H+]^2

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12
Q

how do you find the concentration of a weak acid?

A

[HA] = [H+]^2/ Ka

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13
Q

what is the general equation for a weak acid before rearranging it?

A

Ka = [H+]^2/ [HA]

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14
Q

how do you work out the concentration of a weak base?

A

[H+] = Kw/ [OH-]

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15
Q

how do you work out the concentration of a strong base?

A

[OH-] = Kw/ [H+]

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16
Q

what is the equation for the ionic product of water?

A

Kw = [H+][OH-]

17
Q

what affects the value of Kw?

A

the temperature

18
Q

what is the reaction equation between a weak acid and a weak base?

A

HA H+ + A-

19
Q

what is the equation for the reaction between a weak acid and a weak base?

A

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

20
Q

what is the equation when there is excess HA (H+) in a mixture of a weak acid and weak base?

A

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

21
Q

what does [HA] refer to in the equation: Ka = [H+][A-]/ [HA]

A
22
Q

if you are given the pH of a diprotic substance, what do you do?

A

half it

23
Q

if you are given the conc of a diprotic substance, what do you do?

A

double it

24
Q

what equation can be used for all aqueous solutions?

A

kW = [H+][OH-]

25
Q

what equation can be used for all solutions containing a weak acid?

A

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

26
Q

what equation can be used for a weak acid in water?

A

Ka = [H+]^2/ [HA]

27
Q

how do you convert pKa into Ka?

A

Ka = 10^-pKa

28
Q

what is the equation for excess [OH-] in a solution of a strong base and strong acid?

A

[H+] = Kw/ [OH-]

29
Q

what is the equation for excess [H+] in a solution of a strong acid and strong base?

A

[H+] = n/ v

30
Q

what does [H+] mean in Kw = [H+][OH-]

A
31
Q

give simple steps about how to find the pH when HA is in excess in a solution of a weak acid and weak base

A

use [HA] and [A-] along with the Ka (normally given) to find [H+], then pH
[H+] = Ka [HA]/ [A-]
pH = -log[H+]

32
Q

give simple steps about how to find the pH when A- is in excess in a solution of a weak acid and weak base

A

use Kw to find [H+], then pH
Kw = [H+]^2
pH = -log[H+]

33
Q

give simple steps about how to find the pH when HA = A- in a solution of a weak acid and weak base

A

pKa = pH

find pKa

34
Q

equation for the dissociation of water

A

H20 H+ + OH- (in eqm)