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AS-Level Chemistry Unit 1 > 1.7- Simple Equilibria and Acid Base Reactions > Flashcards

1.7- Simple Equilibria and Acid Base Reactions Flashcards

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1
Q

-What are reversible reactions?

A

where the reactants react to form products, which then react to reform the initial reactants

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2
Q

How is a reversible reaction shown in an equation?

A

double arrow

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3
Q

What does dynamic equilibrium mean?

A

the rate of the forward reactions equals the rate of the reverse reaction

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4
Q

concentrations at equilibrium?

A

reactants and products remain constant

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5
Q

When can dynamic equilibrium occur?

A

in closed systems where no substances can get in or out in order to influence the reactions

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6
Q

What is Le Chatelier’s principle?

A

when a system in dynamic equilibrium is subjected to a change
the position of equilibrium will shift to minimise the change

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7
Q

What is the position of equilibrium if the temperature increases?

A

it will shift to favour the endothermic route as the excess heat needs to be removed from the system to lessen the effect of the initial increase
therefore it will increase the yield of the products in the endothermic route

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8
Q

What is the position of equilibrium if the temperature decreases?

A

it will shift to favour the exothermic route as the heat needs to be gained
so the yield of the products in the exothermic route will increase

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9
Q

What is the position of equilibrium if pressure increases?

A

it will shift to favour the side with the least number of moles, to reduce the pressure
increasing the yield of the products on this side of the reaction

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10
Q

What is the position of equilibrium if pressure decreases?

A

it will shift to favour the side with the most number of moles, as the pressure has been lost
increasing the yield of the products on this side of the reaction

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11
Q

What is the position of equilibrium if concentration of the reactants increases?

A

it will shift to favour the forward reaction that produces the products as more molecules
increases the yield of products

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12
Q

What is the position of equilibrium if concentration of the products increases?

A

it will shift to favour the backward reaction that reforms the reactants

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13
Q

What affect does catalysts have to reactions?

A

no effect to the position of equilibrium as they increase the rate of the forward and backward reaction equally
they do allow equilibrium to be reached faster

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14
Q

What is equilibrium constant?

A

known as Kc
indicates the position of equilibrium in terms of concentration

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15
Q

What can change Kc for an equilibrium?

A

temperature

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16
Q

What is the equation for Kc?

A

(C)^c x (D)^d / (A)^a x (B)^b

17
Q

What is Bronsted/Lowry theory?

A

Acids will act as donors of protons H+ (aq)
Bases will react in order to accept a proton H+ (aq)

18
Q

What is water said to be in terms of acid and base?

A

amphoteric
as it can react as an acid and a base depending on conditions

19
Q

What does dissociation mean?

A

refers to a reaction where a molecule or substance breaks apart into smaller units

20
Q

What is ionisation?

A

refers to a reaction which forms ions from charged particles

21
Q

What is pH?

A

-log[H^+(aq)]

22
Q

What does H^+ refer to in pH equation?

A

concentration

23
Q

What is a strong acid?

A

an acid that fully dissociates into ions

24
Q

What is a weak acid?

A

an acid that only partially dissociates into ions

25
Q

What does concentrated mean?

A

more acid particles in relation to water particles

26
Q

What does dilute mean?

A

more water particles in relation to acid particles

27
Q

Describe a dilute solution of weak acid?

A

less acid particles in relation to water particles
will only partially dissociate

28
Q

Describe a concentrated solution of strong alkali/base?

A

more alkali particles to water particles
will fully dissociate

29
Q

Describe a dilute solution of strong acid?

A

less acid particles to water particles
will fully dissociate

30
Q

What is a tritiation?

A

a practical method used to determine the unknown concentration of an acid or base by finding its neutralisation point

31
Q

What is an indicator?

A

used to help determine the neutralisation point of a reaction

32
Q

What are two common indicators?

A

methyl orange
phenolphthalein

33
Q

What are examples of acids?

A

hydrochloric acid
sulphuric acid
nitric acid

34
Q

how do you calculate Kc?

A

product/reactant

35
Q

What are the features of a primary standard?

A

extremely pure
very stable (low reactivity)
doesn’t absorb water easily
high Mr in order to minimise weighing errors

AS-Level Chemistry Unit 1 (8 decks)

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