Brainscape's Knowledge GenomeTM


Top Flashcards (Certified)
All Flashcards

GCSE Chemistry > C3.3/4 - Acids/Electrolysis > Flashcards

C3.3/4 - Acids/Electrolysis Flashcards

1
Q

Metals and acid always make…

A

Salt and hydrogen (MASH)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

Metal oxides (bases) and acid always makes

A

Water and salt (BAWS)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

Metal hydroxides (alkalis) and acid always makes

A

Water and salt (AAWS)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

Metal carbonates and acid always makes

A

Water and carbon dioxide and salts (CAWCS)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

How do you know if acids are strong or weak?

A

It depends on how well they ionise one water

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

What are some examples of strong acids

A 
Hydrochloride acid (HCL) 
Sulphuric acid (H2SO4)
Nitric acid (HNO3)
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

What are some examples of a weak acid

A

Acetic acid (CH3COOH)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

Which acids ionise or dissociate completely in water

A

Strong acids

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

Which acids have only a few of acid molecules that ionise

A

Weak

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

What are chemicals made up of and what are they

A

Chemicals are substances

They are also made up of elements, compounds and mixtures

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

What are elements

A

Pure substances containing one type of atom

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

What are compounds

A

Chemically joined elements e.g. alloy is more than 2 metas joined

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

Mixtures can be what?

A

Can be separated e.g. evaporation

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

What are 3 examples of compounds

A

•acids ( all contain hydrogen and make H+)

  • alloy
  • covalent molecules
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

What are neutralisation reactions

A

When an acid reacts with an alkali or base to form a salt plus water

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

What can aqueous neutralisations be generalised as

A

H+ (aq) + OH- (aq) —> H2O (l)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

What happens to the ph value of a solution when hydrogen ion concentration increases by a factor of ten

A

The pH value of a solution decreases by a factor of one

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

What are bases

A

Bases are substances that react with acids to neutralise them

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

What are 2 examples of bases

A
  • metal oxides e.g. caO (solid)

* metal hydroxides e.g. Ca (OH) 2 (aqueous)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

If some metals e.g. Ca only react with acids, is this a base

A

NO

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

What are alkalis

A

Alkalis are substances that dissolve (and ionise) in water to form hydroxide ions. An alkali is a double base

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

What are 2 examples of alkalis

A
  • NaOH —> Na+ + OH-

* ca (OH) 2 —> Ca 2+ + 2OH-

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

NH3 is an alkali because…

A

It forms OH- ions when added to water

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
24
Q

What is the word equation for the thermite reaction

A

Iron oxide + aluminium -> aluminium oxide + iron

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
25
What is a redox reaction
When electrons are exchanged in the thermite reaction
26
What do redox reactions involve
Redox reactions involve the transfer of electrons
27
What is a titration
A titration is a reaction in which we measure exactly what volume of two solutions will react together e.g. measuring the volume of acid needed to neutralise a measured volume of alkali
28
What is the endpoint of a reaction
The endpoint is the point where a reaction finishes - for acid-base titrations this is where the pH reaches neutral
29
What is concentration always measured in
Mol/dm3
30
1 dm 3 = ? = ?
1dm3 = 1000cm3 = 1000ml
31
MOLE EQUATION | How do I work out moles?
Concentration X volume
32
MOLE EQUATION | How do I work out the concentration?
Moles divided by volume
33
MOLE EQUATION | How do I work out volume?
Moles divided by concentration
34
What is the equation for the full dissociation of HCI
HCI -> H+ + Cl -
35
What is the equation for the partial dissociation for CH3COOH
CH3COOH —> CH3COOH- + H+
36
What is the ionic equation for neutralisation
H+ (aq) + OH- (aq) —> H2O (L)
37
What is acid strength
Acid strength (strong / weak) tells you what proportion of the acid molecules ionise in water
38
What does acid concentration measure
Concentration measures how much acid there is in a litre (1dm3) if water. Concentration is basically how watered down your acid is
39
How can acid concentration and strength affect pH
Because both affect the concentration of H+ ions e.g. W strong acid can be diluted to obtain a pH like that of a weak acid
40
What is a pH curve
A graph of pH (vertical axis) against total volume of acid or alkali added (on horizontal axis)
41
What do titration curves show and what are they used to show
Titration curves show pH changes with volume and titration curves are used to show where neutralisation happens during a titration
42
What happens at the vertical point in a titration or pH curve
The solution is neutral (at pH 7). This is called the end point of the titration
43
What is stage 1 of copper being purified by electrolysis
The positive electrode is impure copper ; the negative electrode is pure copper : the electrolyte is copper sulfate solution
44
What is stage 2 of copper being purified by electrolysis
The positive electrode gets smaller as it dissolves ; the negative electrode gets bigger as it’s coated with copper
45
What is stage 3 of copper being purified by electrolysis
Copper ions (cu2+) in the electrolyte are attracted to the negative electrode. Each cu2+ gains two electrons to form a copper stool, which sticks to the electrode. This is reduction
46
What is stage 4 of copper being purified by electrolysis
Copper atoms in the positive electrode can lose two electrons to form copper ions (cu2+) which dissolve into the electrolyte. This is oxidation
47
What is stage 5 of copper being purified by electrolysis
As the copper ions (cu2+) are released at the positive electrode, atoms of impurities in the impure copper also become free. The mud they form is collected as it may contain silver and gold
48
What is oxidation
If electrons are lost (Mg2+)
49
What is reduction
If the electrons are gained (2Cl-)
50
What is electrolysis
The process by which ionic substances are broken down into simpler substances by passing an electric current through them
51
What is an electrolyte
A liquid in which a current can pass through (e.g. a molten ionic substance or an aqueous ionic solution). This is the liquid that the electrodes are placed in
52
What is an electrode
A conductor (e.g. metal) which allows electricity (electrons) to pass through. This is the solid substance placed into the electrolyte. Commonly made from graphite is high is inert
53
Electrons move towards the...
Negative cathode. Here positive ions can gain the electrons they need - reduction occurs
54
Electrons are lost from negative ions during oxidation at the...
Positive anode and the electrons flow form the positive anode to the negative cathode
55
In your electrolyte you have cations. What are cations?
Positively charged ions
56
In your electrolyte you have anions. What are anions?
Negatively charged ions
57
Opposite charges attract, so what will the anions be attracted to?
The anions will be attracted to the anode (positive electrode) these ions will LOSE electrons - oxidation occurs
58
Opposite charges attract so what will the cations be attracted to?
The cations will be attracted to the cathode (negative electrode). These ions will gain electrons - reduction occurs
59
What do you need for electrolysis to occur
A power source for example a battery
60
What do +anode attract
Attracts -ions (anions)
61
What do -cathode attract
Attracts +ions (cations)
62
What happens if -ions are halogens I.e. Chloride CL- Bromide Br- Iodine I-
The halogen is produced
63
If +ions (metals) are more reactive than hydrogen for example K,Na, Ca,Mg,Zn,Fe What happens?
Hydrogen is produced
64
If -ions are not halogens e.g. Sulphate SO42- Nitrate NO3- Carbonate CO32- What happens
Oxygen is produced from the OH-
65
If +ions (metals) are less reactive than hydrogen for example Cu, Ag, Au What happens?
Then the metal is produced

GCSE Chemistry (12 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2025 Bold Learning Solutions. Terms and Conditions