Acids and Bases Flashcards

1
Q

Equation for calculating pH

A

-log10[H+(aq)]

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2
Q

A small pH=

A

a high concentration of H+ ions (so a low concentration of OH- ions).

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3
Q

A large pH=

A

a low concentration of H+ ions (so a high concentration of OH- ions).

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4
Q

What does one pH unit correspond to?

A

A decrease in pH means an increase in H+ ions by a factor 10.

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5
Q

Equation for concentration of H+ ions

A

[H+] = 10^-pH

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6
Q

Kw equation

A

Kw = [H+] x [OH-] mol2dm-6
It is the ionic product of water (water ionises slightly).

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7
Q

Kw at 298K

A

1x10^-14 mol2dm-6.

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8
Q

What is required in a neutral solution in terms of ions?

A

[H+] = [OH-]
For every mole of water that dissociates, you would get an equal amount of H+ and OH- ions.

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9
Q

How does a low temperature affect pH?

A

A low temperature increases the pH because the concentration of H+ ions decrease. This is because the reaction is exothermic, so the backward reaction is favoured at equilibrium and more reactants are made (H2O).

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10
Q

How does a high temperature affect pH?

A

A high temperature decreases pH because the concentration of H+ ions increases. The reaction is endothermic so the forward reaction is favoured.

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11
Q

Kw equation (only for pure water)

A

Kw = [H+]^2

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12
Q

pKw equation

A

pKw = -log10Kw
To convert, use 10^-pKw

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13
Q

Strong monobasic alkalis

A

[OH-] = [alkali]
Releases 1 OH- ion.

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14
Q

Strong dibasic alkalis

A

[OH-] = 2[alkali]
Releases 2 OH- ions, have to multiply the [H+] concentration by 2 during calculations.

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15
Q

Weak acids and bases definition

A

They only partially dissociate into their ions when dissolved in water.

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16
Q

Strong acids and bases definition

A

They fully dissociate into their ions when dissolved in water.

17
Q

Examples of weak acids

A

Carboxylic acids and carbonic acids.

18
Q

Weak bases examples

A

Ammonia and amines.

19
Q

A Bronsted-Lowry acid is …

A

A proton donor

20
Q

A Bronsted-Lowry base is …

A

A proton acceptor

21
Q

What is Ka?

A

The acid dissociation constant, same formula as Kc ([products]/[reactants]) moldm-3.

22
Q

pKa =

A

-log10Ka
10^-pKa to convert

23
Q

How does Ka affect the strength of acids?

A

The larger the value of Ka, the stronger the acid. In general, acids with Ka much smaller than 1 are classes as week and those with Ka much greater than 1 are strong.

24
Q

General equation for a weak acid.

A

HA (reversible) H+ + A-
At equilibrium, there is a high concentration of reactants and a low concentration of products.

25
Q

Weak acid assumption.

A

[HA] initially = [HA] equilibrium.
The position of equilibrium lies heavily to the reactant side - as very few acid molecules dissociate.

26
Q

Weak acid key point

A

[H+] = [A-]

27
Q

Ka =

A

[H+] x [A-]
[HA]

28
Q

Ka if only weak acids are present

A

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