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GCSE Chemistry COPY > C6.4 - Electrolysis of aqueous solutions > Flashcards

C6.4 - Electrolysis of aqueous solutions Flashcards

1
Q

Brine

A

Brine is a concentrated sodium chloride solution

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2
Q

What is the electrolysis of brine in relation to industry?

A

The electrolysis of brine is a very important large-scale industrial process

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3
Q

When brine is electrolysed, what 3 useful products do you get that are used to make other chemicals?

A

When brine is electrolysed, the 3 useful products you get that are used to make other chemicals are:

  1. Chlorine gas
  2. Hydrogen gas
  3. Sodium hydroxide solution
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4
Q

When brine is electrolysed, why is sodium hydroxide left in the solution?

A

When brine is electrolysed, sodium hydroxide is left in the solution, because there are 4 different ions in brine - Na+, Cl-, H+ and OH-, all aqueous

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5
Q

Whenever hydrogen is produced at the cathode during electrolysis, what do the hydrogen atoms formed do?

A

Whenever hydrogen is produced at the cathode during electrolysis, the hydrogen atoms formed:

  1. Bond together in pairs
  2. Are given off as hydrogen gas, H2
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6
Q

In the electrolysis of brine, you can test the solution around the cathode with what?

A

In the electrolysis of brine, you can test the solution around the cathode with an acid/base indicator

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7
Q

In the electrolysis of brine, if you test the solution around the cathode with an acid/base indicator, what will it show?

A

In the electrolysis of brine, if you test the solution around the cathode with an acid/base indicator, it will show that the solution is alkaline

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8
Q

What should be considered in relation to brine?

A

The environmental impacts of the electrolysis of brine on a large scale should be considered

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9
Q

What does the process of the electrolysis of brine use?

A

The process of the electrolysis of brine uses a lot of electricity that is mainly produced by the burning of fossil fuels

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10
Q

What must be in contact with the solution of brine during the actual process of electrolysis?

A

A metal must be in contact with the solution of brine during the actual process of electrolysis

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11
Q

A metal must be in contact with the solution of brine during the actual process of electrolysis.
What is a metal most commonly used?

A

A metal most commonly used is mercury

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12
Q

Ions present in a solution of potassium bromide

A

The ions present in a solution of potassium bromide are:

  1. K+
  2. Br-
  3. H+
  4. OH-
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13
Q

The product at the cathode in the electrolysis of a solution of potassium bromide

A

The product at the cathode in the electrolysis of a solution of potassium bromide is hydrogen gas

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14
Q

The product at the anode in the electrolysis of a solution of potassium bromide

A

The product at the anode in the electrolysis of a solution of potassium bromide is bromine

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15
Q

Observations you can see at the anode in the electrolysis of a solution of potassium bromide

A

The observations you can see at the anode in the electrolysis of a solution of potassium bromide are:

  1. Bubbles
  2. A reddish-brown solution of bromine
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16
Q

Ions present in a solution of sodium sulfate

A

The ions present in a solution of sodium sulfate are:

  1. Na+
  2. S2-
  3. H+
  4. OH-
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17
Q

The product at the cathode in the electrolysis of a solution of sodium sulfate

A

The product at the cathode in the electrolysis of a solution of sodium sulfate is hydrogen gas

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18
Q

The product at the anode in the electrolysis of a solution of sodium sulfate

A

The product at the anode in the electrolysis of a solution of sodium sulfate is oxygen gas

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19
Q

Ions present in a solution of copper(II) chloride

A

The ions present in a solution of copper(II) chloride are:

  1. Cu2+
  2. Cl-
  3. H+
  4. OH-
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20
Q

The product at the cathode in the electrolysis of a solution of copper(II) chloride

A

The product at the cathode in the electrolysis of a solution of copper(II) chloride is copper

21
Q

The product at the anode in the electrolysis of a solution of copper(II) chloride

A

The product at the anode in the electrolysis of a solution of copper(II) chloride is chlorine gas

22
Q

Observations you can see at the anode in the electrolysis of a solution of copper(II) chloride

A

The observations you can see at the anode in the electrolysis of a solution of copper(II) chloride are that damp litmus paper is bleached, turning white

23
Q

When brine is electrolysed, what is produced at the anode?

A

When brine is electrolysed, chlorine gas is produced at the anode

24
Q

When brine is electrolysed, chlorine gas is produced at the anode.
When brine is electrolysed, what is produced at the cathode?

A

When brine is electrolysed, hydrogen gas is produced at the cathode

25
Q

When brine is electrolysed, chlorine gas is produced at the anode.
When brine is electrolysed, hydrogen gas is produced at the cathode.
When brine is electrolysed, what is the remaining solution?

A

When brine is electrolysed, the remaining solution is sodium hydroxide solution

26
Q

When brine is electrolysed, why is hydrogen gas produced at the cathode?

A

When brine is electrolysed, hydrogen gas is produced at the cathode, because sodium is more reactive than hydrogen

27
Q

Aluminium is extracted by electrolysis.

Why can aluminium not be extracted by heating aluminium oxide with carbon?

A

Aluminium can not be extracted by heating aluminium oxide with carbon, because aluminium is more reactive than carbon in the reactivity series

28
Q

In the electrolysis of aluminium oxide, what is formed at the negative electrode?

A

In the electrolysis of aluminium oxide, molten aluminium is formed at the negative electrode

29
Q

What observations would you see if hydrogen gas or oxygen gas is produced?

A

The observations you would see if hydrogen gas or oxygen gas is produced are:

  1. Bubbles
  2. Fizzing
30
Q

If a metal is too reactive to be reduced with carbon or reacts with carbon, then electrolysis can be used to extract it.
What is extracting metals via this method?

A

Extracting metals via the method of electrolysis is very expensive

31
Q

At the negative electrode (cathode) when is hydrogen produced?

A

At the negative electrode (cathode), hydrogen is produced if the metal is more reactive than hydrogen

32
Q

At the positive electrode (anode), what is produced unless the solution contains halide ions?

A

At the positive electrode (anode), oxygen gas is produced, unless the solution contains halide ions

33
Q

At the positive electrode (anode), oxygen gas is produced, unless the solution contains halide ions.
What would happen if halide ions are present?

A

If halide ions are present, the halide would be formed

34
Q

Industrial uses of electrolysis

A

Industrial uses of electrolysis are:

  1. To manufacture chlorine, sodium hydroxide, hydrogen and sodium
  2. Electroplating of steel
35
Q

What is bleach made from?

A

Bleach is made from:
1. Chlorine
2. Sodium hydroxide
obtained from the electrolysis of brine

36
Q

What is the chlorine made when you electrolyse brine in industry used to do?

A

The chlorine made when you electrolyse brine in industry is used to kill bacteria in:

  1. Drinking water
  2. In some swimming pools
37
Q

When brine is electrolysed, the 3 useful products you get that are used to make other chemicals are chlorine gas, hydrogen gas and sodium hydroxide solution.
Chlorine gas is produced at the what?

A

Chlorine gas is produced at the anode

38
Q

When brine is electrolysed, the 3 useful products you get that are used to make other chemicals are chlorine gas, hydrogen gas and sodium hydroxide solution.
Hydrogen gas is produced at the what?

A

Hydrogen gas is produced at the cathode

39
Q

When brine is electrolysed, sodium hydroxide is left in the solution, because there are 4 different ions in brine - Na+, Cl-, H+ and OH-, all aqueous.
The Cl- and H+ ions are removed during electrolysis as they move to what?

A

The Cl- and H+ ions are removed during electrolysis as they move to the:

  1. Anode
  2. Cathode
40
Q

When brine is electrolysed, sodium hydroxide is left in the solution, because there are 4 different ions in brine - Na+, Cl-, H+ and OH-, all aqueous.
The Cl- and H+ ions are removed during electrolysis as they move to the anode and cathode, because what?

A

The Cl- and H+ ions are removed during electrolysis as they move to the anode and cathode, because:

  1. Halide ions are first in the order of discharge at the anode
  2. Sodium is more reactive than hydrogen
41
Q

When brine is electrolysed, sodium hydroxide is left in the solution, because there are 4 different ions in brine - Na+, Cl-, H+ and OH-, all aqueous.
The Cl- and H+ ions are removed during electrolysis as they move to the anode and cathode, because halide ions are first in the order of discharge at the anode and sodium is more reactive than hydrogen, so this leaves a solution of what?

A

The Cl- and H+ ions are removed during electrolysis as they move to the anode and cathode, because:
1. Halide ions are first in the order of discharge at the anode
2. Sodium is more reactive than hydrogen
,so this leaves a solution of sodium hydroxide, NaOH

42
Q

In the electrolysis of brine, if you test the solution around the cathode with an acid/base indicator, it will show that the solution is alkaline, because what?

A

In the electrolysis of brine, if you test the solution around the cathode with an acid/base indicator, it will show that the solution is alkaline, because sodium hydroxide solution is alkaline

43
Q

A metal must be in contact with the solution of brine during the actual process of electrolysis.
A metal most commonly used is mercury, which is what?

A

A metal most commonly used is mercury, which is toxic

44
Q

A metal must be in contact with the solution of brine during the actual process of electrolysis.
A metal most commonly used is mercury, which is toxic and some mercury does what?

A

A metal most commonly used is mercury, which is toxic and some mercury escapes into the:

  1. Solution
  2. Environment
45
Q

The observations you can see at the anode in the electrolysis of a solution of copper(II) chloride are that damp litmus paper is bleached, turning white, but if you use blue litmus paper, it may turn what for a moment first?

A

The observations you can see at the anode in the electrolysis of a solution of copper(II) chloride are that damp litmus paper is bleached, turning white, but if you use blue litmus paper, it may turn red for a moment first

46
Q

The observations you can see at the anode in the electrolysis of a solution of copper(II) chloride are that damp litmus paper is bleached, turning white, but if you use blue litmus paper, it may turn red for a moment first, because what?

A

The observations you can see at the anode in the electrolysis of a solution of copper(II) chloride are that damp litmus paper is bleached, turning white, but if you use blue litmus paper, it may turn red for a moment first, because a solution of chlorine is acidic

47
Q

Aluminium can not be extracted by heating aluminium oxide with carbon, because aluminium is more reactive than carbon in the reactivity series, so what has to be used?

A

Aluminium can not be extracted by heating aluminium oxide with carbon, because aluminium is more reactive than carbon in the reactivity series, so electrolysis has to be used

48
Q

In the electrolysis of aluminium oxide, molten aluminium is formed at the negative electrode.
The liquid aluminium does what?

A

The liquid aluminium runs to the bottom of the cell, where it is tapped off

49
Q

If a metal is too reactive to be reduced with carbon or reacts with carbon, then electrolysis can be used to extract it.
Extracting metals via the method of electrolysis is very expensive, because what?

A

Extracting metals via the method of electrolysis is very expensive, because lots of energy is required to:

  1. Melt the ore
  2. Produce the required current

GCSE Chemistry COPY (70 decks)

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