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AQA GCSE - Chemistry > 2.5 - Salts And Electrolysis > Flashcards

2.5 - Salts And Electrolysis Flashcards

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1
Q

What is the ionic equation for neutralisation?

A

H + OH -> H2O

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2
Q

What does a pH meter do?

A

Gives an accurate numerical value for pH

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3
Q

What is concentrated and dilute acids/alkalis?

A

Concentrated- many particles

Dilute - fewer particles

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4
Q

What is strong and weak acids/alkalis?

A

Strong - completely ionises

Weak - partially ionises

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5
Q

What does acid + metal produce?

A

Soluable salt + hydrogen gas

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6
Q

What does acid + base(metal oxide) produce?

A

Soluable salt + water

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7
Q

What does acid + metal carbonate produce?

A

Soluable salt + carbon dioxide + water

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8
Q

What does acid + alkali produce?

A

Soluable salt + water

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9
Q

Name the salts for:
Hydrochloric acid
Sulfuric acid
Nitric acid

A

Chloride salts
Sulfate salts
Nitrate salts

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10
Q

Why do you need excessive amounts of metals, bases or carbonates?

A

To make sure all the acid reacts

Excess solid can be removed by filtration

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11
Q

What are ammonium salts used for?

A

Fertilisers

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12
Q

What does soluable salt + soluable salt produce?

A

Soluable salt + insoluable salt (precipitate)

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13
Q

Give an example of two soluable salts reaction

A

Potassium Iodide + Silver Nitrate -> Potassium Nitrate + Silver Iodide (precipitate)

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14
Q

How do you know what the precipitate is in 2 soluable salt reaction?

A

The least reactive product made

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15
Q

What is electrolysis?

A

The breaking down of an ionic substance into it’s elements using electricity

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16
Q

What does the substance have to be for electrolysis to work and why?

A

It has to be dissolved in water or molten. This is because the ions need to be free to move

17
Q

What does the negatively charged electrode attract?

A

Positively charged ions (usually metal)

17
Q

What is the negatively charged electrode called?

A

Cathode

18
Q

What does the positively charged electrode attract?

A

Negatively charged ions

19
Q

What is the positively charge electrode called?

A

Anode

21
Q

What happens at the negative electrode?

A

Reduction which is the gain of electrons

22
Q

What happens at the positive electrode?

A

Oxidation which is the loss of electron(s)

23
Q

If in a solution what could be produced at the negative electrode?

A

The positive ion
Metal or Hydrogen
Whichever is the least reactive out of the two

24
Q

If in a solution what could be produced at the positive electrode?

A

A halide element (group 7) if not then oxygen

25
Q

What is produced in the electrolysis of Brine (Sodium Chloride)

A

Positive electrode: Chlorine
Negative: Hydrogen
Left over: Sodium Hydroxide

26
Q

How can you test for hydrogen?

A

Put a lit split into the gas it should make a squeaky pop

27
Q

How do you test for chlorine?

A

It bleaches litmus paper

28
Q

What is chlorine, Hydrogen and sodium hydroxide used in

A

Chlorine: disinfectant, killing bacteria
Hydrogen: alternative fuel, margarine
Sodium Hydroxide: soap, ceramics, paper, nautralisation

29
Q

Describe extraction of Aluminium Oxide?

A

Using electrolysis:
Insoluable so has to be melted
Cryolite added to reduce boiling point from 2700 to 970
This saves energy costs

30
Q

What is produced at each electrode in the extraction of Aluminium?

A

Positive: oxygen
Negative: aluminium

31
Q

If oxygen is produced at the positive electrode in extraction of aluminium oxide what could happen?

A

As the electrode is made of graphite that is made of carbon
The carbon reacts with the oxygen to produce Carbon dioxide
The electrodes will burn away and have to be replaced

32
Q

What is electroplating?

A

Puts a thin coating of metal in an object

To make it more attractive, protect from corrosion or increase hardness

33
Q

Where is the object placed in electrolysis?

A

Used as the negative electrode so metal atoms are deposited from the solution on to the object

AQA GCSE - Chemistry (19 decks)

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