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a level chem > chapter 20 > Flashcards

chapter 20 Flashcards

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1
Q

what do acids do in water?

A

dissociate and release H+ ions into solution

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2
Q

what do alkalis do in water?

A

dissolves in water and releases OH- ions

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3
Q

what is a neutralisation reaction?

A

when an acid reacts with a base to produce salt and water

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4
Q

what is something important about ionic equations?

A

contains only ions that take part in the reaction
anything s/l/g goes into the equation

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5
Q

what does a metal + acid produce?

A

salt + H2
M A S H

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6
Q

what is a bronsted-lowry acid?

A

proton/H+ donor

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7
Q

what is a bronsted-lowry base?

A

proton/H+ acceptor

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8
Q

What is a conjugate acid-base pair?

A

Contains 2 species
Can be interconverted by transfer of a proton

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9
Q

What happens during dissociation?

A

Only takes place when water is present
Acids donate protons to water to form hydronium ion

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10
Q

what are strong acids?

A

completely dissociate in aqueous solutions

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11
Q

what are weak acids?

A

partially dissociate in aqueous solutions

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12
Q

what is pH?

A

measure of concentration of H+ ions in a solution
or
-log [H+]

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13
Q

what does the smaller the pH mean?

A

the more acidic/larger concentration of H+

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14
Q

what is the assumption for strong monobasic acids?

A

[HA] = [H+]

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15
Q

what is the Ka equation?

A

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

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16
Q

what is the equation for pKa?

A

-logKa

17
Q

how do you find Ka from pKa?

A

10^-pKa

18
Q

what is the assumptions for weak acids?

A

[H+] = [A-]
[HA]eqm = [HA]start

19
Q

what is the assumed equation for Ka for weak acids?

A

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

20
Q

what are the limitations of the approx [H+]=[A-]?

A

if pH>6 then [H+] from dissociation of water becomes more significant
approx breaks down for very weak acids

21
Q

what are the limitations of the approx [HA]eqm=[HA]start?

A

breaks down when [HA]eqm becomes more significant
not justified for stronger weak acid

22
Q

can water be both an acid and base?

A

water ionises very slightly so can act as both an acid and a base

23
Q

what is the equation for Kw?

A

Kw = [H+][OH-]

24
Q

when water is neutral what are the concentrations of H+ and OH- ions?

A

[H+] = [OH-]

25
Q

what does Kw do?

A

controls concentrations of H+ and OH- in a solution

26
Q

how is pH of a strong base calculated?

A

concentration of base
ionic product of water Kw

27
Q

how do you calculate the new concentration of a solution?

A

original conc x volume of reagent/total volume

a level chem (22 decks)

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