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Chemistry > Equilibrium (AS/A level) > Flashcards

Equilibrium (AS/A level) Flashcards

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1
Q

four charactertistics of equilibrium

A

dynamic
forward = backward reaction at same rate
concentration of r/p remain constant
closed system

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2
Q

what is la chateliar’s principle

A

If one or more factors that affect an equilibrium is changed, the position of equilibrium shifts in the direction that reduces the change

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3
Q

decreasing concentration of reactants causes

A

equilibrium to move left

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4
Q

whichever side you take stuff off, equilibrium shifts to the side to restore ok

A

ok

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5
Q

increasing pressure causes

A

equilibrium moves to less molecules side

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6
Q

how does temperature affect equilibrium

A

depending on exo/endo

both forward/backward rate increases

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7
Q

which factor is Kc dependant

A

temperature

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8
Q

how does catalyst affect equilibrium

A

no effect

no effect on delta H

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9
Q

remember to practice mole ratios

A

ok

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10
Q

what is homogeneous equilibrium

A

everything present in the same phase

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11
Q

what is heterogeneous equilibrium

A

things present in more than one phase

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12
Q

definition of an acid

A

proton donor

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13
Q

definition of a base

A

proton acceptor

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14
Q

what are conjugate pairs

A

HCl (acid) = cl- (conjugate base)

differ by one proton

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15
Q

definition of ionic product of water

A

[H+][OH-]mol2dm-6 (Kw)

1 x 10^-14

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16
Q

definition of pH

A

-log[H+]

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17
Q

how to find pH of strong acids

A

[H+] = concentration of acid

18
Q

how to find pH of strong bases

A

using Kw

[OH-] = concentration of base

19
Q

how to find pH of weak acids

A

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

20
Q

what does high value of Ka mean

A

equilibrium toward right = stronger acid

21
Q

pKa formula

A

-log[Ka] (less positive = more acidic)

22
Q

definition of indicator

A

Acid-base indicator is a dye/mixture that changes colour over a specific pH range. The weak acid and conjugate base has different colours. Hln ⇌ H+ + ln-

23
Q

what does pKa show

A

transition of colour

24
Q

where is equivalence point

A

midpoint of fall

25
Q

strong acid + strong base

equivalence point + pH range

A

7

10.5 - 3.5

26
Q

strong acid + weak base

equivalence point + pH range

A

5

7.5 - 3.5

27
Q

weak acid + strong base

equivalence point + pH range

A

9

11 - 7.5

28
Q

how to find Ka of buffer solution

A

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

29
Q

definition of buffer solution

A

a solution that resists in pH changes when small amounts of H+ or OH- are added;

30
Q

uses of buffer solution

A

electroplating

dyes

31
Q

how to find equations in buffer solution

A

acid partially dissociates so conjugate base is not enough - salt is needed
A (acid) ⇌ B + C
D (salt) → E + F (conjugate base)

32
Q

look at examples of buffer solutions now

A

ok

33
Q

how to find pH of buffer solution

A

pKa + log [A-]/[HA]

34
Q

definition of solubility product

A

product of concentrations of each ion in a saturated solution of a sparingly soluble salt at 298K raised to the power of their relative concentrations

35
Q

definition of saturated solution

A

solution in contact with its undissolved solid

36
Q

smaller Ksp means

A

less soluble

37
Q

what is Ksp dependant

A

temperature

38
Q

definition of common ion effect

A

the reduction in the solubility of a dissolved salt achieved by adding a solution of a compound which has an ion in common with the dissolved salt, often resulting in precipitation.

39
Q

definition of partition coefficient

A

equilibrium constant that relates the concentration of solute partitioned between two immiscible solvents at a particular temperature.

40
Q

how to find Kpc

A

[organic solvent]/[in water]

Chemistry (15 decks)

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