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Chemistry > Equilibrium, acid base and pH > Flashcards

Equilibrium, acid base and pH Flashcards

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1
Q

Whats a homogeneous Equilibria?

A

When all species in the equilibrium equation have the same states

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2
Q

Whats a heterogeneous Equilibria?

A

When species in the equation have different states

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3
Q

What states are included in Kc?

A

gas (g) and aqueous (aq)

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4
Q

What states are included for Kp

A

Gases (g) only

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5
Q

Give the expression for Kc

A

Kc = [C]^c [D]^d / [A]^a [B]^b

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6
Q

How do you calculate concentration at equilibrium?

A

Equilibrium moles / Total volume (dm3)

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7
Q

What is Kc?

A

Equilibrium constant for concentration

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8
Q

What is Kp?

A

The equilibrium constant in terms of partial pressure

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9
Q

What is mole fraction?

A

Proportion of volume of gas with total volume of gas in a gas mixture.

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10
Q

What is partial pressure

A

The contribution the gas makes to the total pressure

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11
Q

How do you calculate mole fraction?

A

Equilibrium moles / total moles

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12
Q

How do you calculate partial pressure?

A

mole fraction x total pressure

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13
Q

The sum of the partial pressures = ?

A

The total pressure

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14
Q

KPa x KPa =

A

KPa^2

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15
Q

What information does the value of K give you?

A

the position of the equilibrium

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16
Q

where is the equilibrium when K = 1?

A

Halfway

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17
Q

where is the equilibrium when K > 1?

A

To the right

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18
Q

where is the equilibrium when K < 1?

A

To the left

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19
Q

When will K change?

A

ONLY CHANGE IN TEMPERATURE

20
Q

If concentration of products increase where does equilibrium shift and why?

A

To the reactants (left). Because it opposes change in order to keep K the same.

21
Q

If pressure increases where does equilibrium shift and why?

A

To the side with least moles because K stays the same.

22
Q

How does a catalyst change K?

A

It doesn’t

23
Q

What’s a Bronsted-Lowry Acid

A

A proton donor

24
Q

What’s a Bronsted-Lowry Base

A

A proton acceptor

25
Q

What’s a conjugate acid-base pair

A

Two species that can be inter converted by the transfer of a proton

26
Q

What’s H3O+

A

Hydronium

27
Q

What’s a monobasic acid?

A

When 1 mol of protons are donated per mol of acid.

28
Q

What’s a diprotic acid?

A

When 2 mols of protons are donated per mol of acid

29
Q

What’s triprotic acid?

A

When 3 mols of protons are donated per mol of acid

30
Q

How do you calculate a diluted concentration?

A

origional conc of whats wanted x volume of whats wanted/ total volume of solution

31
Q

How do you calculate pH?

A

-log [H+]

32
Q

How do you calculate [H+] from pH?

A

10^-pH

33
Q

will a low concentration of [H+] have a high or low pH

A

High pH

34
Q

How should you round pH?

A

To 2dp

35
Q

How many more H+ is there in pH1 than in pH2?

A

x10

36
Q

Whats Ka?

A

Acid dissociation constant

37
Q

The expression for Ka?

A

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

38
Q

Will a strong acid have a small or big pKa?

A

Small pKa

39
Q

What is pKa?

A

A negative logarithm used to compare weak acids more easily

40
Q

What assumption can you make for using strong acids?

A

[H+] = [Acid]

41
Q

What two assumptions can you make for weak acids?

A

1) [H+] = [A-]

2) [HA] equib = [HA] start

42
Q

What is Ka for weak acids?

A

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

43
Q

Why don’t the assumptions for weak acids always work?

A

1) When there is dissociation of H2O [H+] does not = [A-]

2) In strong acids there is a lot of dissociation so [HA] equib does not = [HA]start

44
Q

What is Kw?

A

Ionic Product of water

45
Q

What is the expression for Kw?

A

Kw= [H+][OH-]

46
Q

What is Kw at room temperature?

A

1 x 10^-14

47
Q

What assumption can you make for Strong bases?

A

That [OH-] = [HA]

Chemistry (6 decks)

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