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Chemistry > Topic 3 - Reactions Of Acids > Flashcards

Topic 3 - Reactions Of Acids Flashcards

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1
Q

State both mass concentration formulas

A

Mass concentration = Mass(g) / Volume(dm^3)

Mass concentration = Mole concentration x mass of one mole

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2
Q

State the formula used to find mole concentration

A

Mole concentration = Number of Moles / Volume (dm^3)

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3
Q

State the formula used to find number of moles using concentration

A

Number of moles = Concentration x Volume

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4
Q

State the general equation for when an acid reacts with a metal oxide

A

Acid + Metal Oxide –> Salt + Water

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5
Q

State the general equation for when an acid reacts with a metal hydroxide

A

Acid + metal hydroxide –> Salt + water

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6
Q

State the general equation for when an acid reacts with a metal carbonate

A

Acid + metal carbonate –> salt + water + carbon dioxide

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7
Q

State the general equation for when an acid reacts with a metal

A

Acid + Metal –> salt + hydrogen

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8
Q

What type of salt is made from hydrochloric acid?

A

Chloride

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9
Q

What type of salt is made from sulfuric acid?

A

Sulfate

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10
Q

What type of salt is made from nitric acid?

A

Nitrate

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11
Q

What type of salt is made from ethanoic acid

A

Ethanoate

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12
Q

What is the ionic equation for neutralisation?

A

OH- + H+ –> H20

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13
Q

Just a reminder that you need to how to do titration calculations

A

Go do a practice question

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14
Q

What do you find out by doing a titration?

A

The concentration of a substance

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15
Q

How does the colour of phenolphthalein change during a titration?

A

In an acid it is colourless, in an alkali solution it is pink.

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16
Q

How does the colour of methyl orange change during a titration?

A

In an acid it is red, an a neutral solution it is orange, in an alkali solution it is yellow.

17
Q

What can soluble salts be made from?

A

Either:

An acid and an insoluble base

An acid and a soluble base

18
Q

How do you get a pure, dry sample of an insoluble salt?

A

Mix the reactants, making sure the base is in excess. Warm the solution to speed up the rate of reaction. Filter off the excess base using a funnel and filter paper. Heat up the filtrate until two thirds of the water has evaporated. Leave in a cool dry place for the crystals to form.

19
Q

What is the pH of a neutral solution?

A

7

20
Q

What is the pH of an acid

A

1-6

21
Q

What is the pH of an Alkali?

A

8-14

22
Q

What is an alkali?

A

A soluble base dissolved in water

23
Q

What does an alkali release when dissolved in water?

A

OH- (hydroxide ions)

24
Q

What does an acid release when dissolved in water?

A

H+ (hydrogen ions)

25
Q

What happens to the concentration of H+ ions when the pH decreases by 1

A

The concentration of H+ ions increases by 10 times

26
Q

What happens to the concentration of OH- ions when the pH decreases by 1

A

The concentration of OH- ions decreases by 10 times.

27
Q

What is the concentration of H+ ions at pH 1?

A

0.1 mol dm^-3

28
Q

Are common salts of sodium, potassium and ammonium soluble or insoluble?

A

Soluble

29
Q

Are nitrates soluble or insoluble?

A

Soluble

30
Q

Which chlorides are insoluble?

A

Silver chloride and lead chloride

31
Q

Which sulphates are insoluble?

A

Lead, barium and calcium chloride

32
Q

Which carbonates and hydroxides are soluble?

A

Sodium, potassium and ammonium

33
Q

During electrolysis of a solution, when the metal is more reactive then hydrogen, what will be produced at the cathode?

A

Hydrogen gas

34
Q

During electrolysis of a solution, when the metal is less reactive then hydrogen, what will be produced at the cathode?

A

The metal

35
Q

During electrolysis of a solution, if a halide is present, what will be produced at the anode?

A

The halide

36
Q

During electrolysis of a solution, if a halide is not present, what will be produced at the anode?

A

Oxygen

Chemistry (11 decks)

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