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HDSO Chemistry REDOX A > Acids And Bases Part 1 > Flashcards

Acids And Bases Part 1 Flashcards

1
Q

What does bronsted Lowry theory describe acids and bases in terms of

A

Protons

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2
Q

What does an acid-base reaction involve

A

Proton transfer

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3
Q

Acid

A

A substance that donates H+ ions

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4
Q

What are acids classified as strong or weak depending on

A

The extent of dissociation

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5
Q

Strong acid

A

Completely dissociates in solution

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6
Q

Weak acid

A

Partially dissociates in solution

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7
Q

Base

A

A substance that accepts H+ ions

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8
Q

Alkali

A

A base that releases hydroxide ions in aqueous solution

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9
Q

What type of reaction is that of acids with metals

A

Redox

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10
Q

What is the role of H+ ions in the reaction of acids with metals

A

Oxidising agent

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11
Q

What are acid base equilibria

A

Reversible reactions involving the transfer of protons

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12
Q

pH

A

-log[H+]

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13
Q

What does a low pH mean

A

Larger concentration of H+ ions

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14
Q

What does a high pH mean

A

A small concentration of H+ ions

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15
Q

[H+]

A

10 ttp -pH

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16
Q

How many moles of H+ ions does one mole of a monoprotic acid donate

A

One mole

17
Q

What do you assume in pH calculations for strong acids

A

Complete ionisation

18
Q

What does it mean that for pH calculations of strong acids, you assume complete ionisation

A

[H+]=original conc of acid

19
Q

Is sulfuric monoprotic

A

Diprotic

[H+]=2[HA]

20
Q

What are a weak acids undissociated molecules in equilibrium with

A

It’s ions

21
Q

Acid dissociation constant

A

Ka

22
Q

Ka

A

Conc product/conc reactants

23
Q

Units of Ka

A

Moldm-3

24
Q

What is the value of Ka a quantitative measure of

A

The strength of a weak acid

25
Q

What is the relationship between degree of dissociation and Ka value and why

A

Greater degree of dissociation, higher conc of H+ and larger Ka value

26
Q

What is pKa sometimes used for

A

To compare the relative strengths of acids

27
Q

pKa

A

-logKa

28
Q

Relationship between Ka value and strength of acid

A

Higher Ka value = stronger acid

29
Q

Relationship between pKa value and acid strength

A

Lower pKa value = stronger acid

30
Q

Expression for ionisation of water

A

h20 > H+ + OH-

31
Q

To what extent does pure water ionise to

A

A very small extent

32
Q

What is Kw derived from

A

The equilibrium constant for the dissociation of water into H+ ions and OH-

33
Q

Definition of Kw

A

[H+][OH]

34
Q

What is Kw at 298K

A

1x10-14 mol2dm-6

35
Q

Why is the dissociation of water an endothermic process

A

Energy is required to break bonds

36
Q

Why does Kw increase when temperature increases

A

The equilibrium moves to the right

37
Q

Assumptions to make to calculate the pH of a strong base

A
  • assume complete ionisation

- assume Kw= 1x10-14

HDSO Chemistry REDOX A (5 decks)

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