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Chemistry > CC8 > Flashcards

CC8 Flashcards

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1
Q

What can all aqueous solutions be?

A

Acidic, Alkaline or Neutral.

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2
Q

How is the acidity or alkalinity of a solution measured?

A

It is measured on the pH scale. Most solutions lie between 0 and 14 on the scale.

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3
Q

What pH is a neutral solution?

A

A neutral solution has a pH of 7.

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4
Q

What pH is an acidic solution?

A

An acidic solution has a pH lower than 7 (0-6 including pH6).

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5
Q

What pH is an alkaline solution?

A

An alkaline solution has a pH greater than 7.

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6
Q

How can the pH of a solution be found out?

A

By using indicators.

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7
Q

What is an indicator?

A

A substance which can change colour depending on the pH of a solution.

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8
Q

What are some examples of indicators?

A
  • Litmus paper
  • Methyl orange
  • Phenolphthalein
  • Universal indicator
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9
Q

What colour is litmus paper in alkaline and acidic solutions?

A

Alkaline solutions: Blue
Acidic solutions: Red

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10
Q

What colour is methyl orange in alkaline and acidic solutions?

A

Alkaline solutions: Yellow
Acidic solutions: Red

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11
Q

What colour is phenolphthalein in alkaline and acidic solutions?

A

Alkaline solutions: Pink
Acidic solutions: Colourless

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12
Q

What ions do acids produce when dissolved in water?

A

Acids produce an excess of hydrogen ions (H+) when they dissolve in water.

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13
Q

What ions do alkalis produce when dissolved in water?

A

Alkalis produce excess Hydroxide ions (OH-) in water.

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14
Q

How does the amount of hydrogen ions affect the pH of a solution?

A

The higher the number of hydrogen ions in a certain volume, the higher their concentration. The higher their concentration, the more acidic the solution and the lower the pH.

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15
Q

How does the amount of hydroxide ions affect the pH of a solution?

A

The higher the concentration of hydroxide ions, the more alkaline the solution and the higher the pH.

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16
Q

How does the amount of hydrogen and hydroxide ions affect the pH of a neutral solution?

A

Neutral solutions have a pH of 7 and contain low, equal concentrations of hydrogen ions and hydroxide ions.

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17
Q

What is a concentrated solution?

A

A solution that contains a lot of dissolved solute per unit volume.

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18
Q

What is a dilute solution?

A

A solution that contains only a small amount of solute.

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19
Q

What is the formula for concentration?

A

Concentration = amount dissolved/volume of solution

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20
Q

How does the concentration of hydrogen ions affect the pH of a solution?

A

If the concentration of hydrogen ions is increased by a factor of 10 (x10), the pH decreases by 1. If the concentration decreases by a factor of 10 (x10), the pH increases by 1.

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21
Q

What is a strong acid?

A

An acid that dissociates completely into ions when it dissolves.

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22
Q

What are some examples of strong acids?

A

Hydrochloric acid, Sulfuric acid, Nitric acid.

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23
Q

What is a weak acid?

A

An acid that does not dissociate completely into ions when it dissolves.

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24
Q

What are some examples of weak acids?

A

Carbonic acid, Ethanoic acid, Boric acid.

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25
Q

What does the chemical properties of an acid depend on?

A

It depends on both the type of acid and its concentration.

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26
Q

What are bases?

A

Substances that neutralise acids to form a salt and water only.

27
Q

Are all metal oxides bases?

A

Yes, all metal oxides are bases.

28
Q

What are the state symbols for equations?

A

Solid(s), Liquid(l), Gas(g), Aqueous/dissolved in water(aq)

29
Q

What is the equations for the neutralisation of all metal oxides?

A

metal oxide + acid –> salt + water

30
Q

What happens to hydrogen ions in neutralisation and how does that affect pH?

A

During neutralisation, hydrogen ions in the acid combine with oxide ions to form water. This removes hydrogen ions and so the pH increases and becomes more neutral.

31
Q

Why must you always add excess of the base when preparing soluble salts?

A

To make sure all of the acid is used up.

32
Q

How can you make sure salt is pure when neutralising a substance?

A

To make sure the prepared salt is pure, the mixture is filtered to remove the residue (the unreacted metal oxide) from the filtrate, leaving only salt and water.

33
Q

What is a base that can dissolve in water called?

A

An alkali.

34
Q

What are some common alkalis (bases)?

A
  • Sodium hydroxide, NaOH, and other group 1 hydroxides
  • Calcium hydroxide, Ca(OH) ², and other group 2 hydroxides
35
Q

Why are there 2 ‘OH’ ions for the chemical formulae of group 2 alkalis and only one for group 1 alkalis?

A

As the ions formed by group 2 atoms have a 2+ charge, but hydroxide ions have a 1- charge. The brackets show that two OH- ions are needed to produce a neutral compounds.

36
Q

What happens to the ions from acids and alkalis during neutralisation?

A

In neutralisation, hydrogen ions from the acid react with hydroxide ions from the alkali. Water, a simple molecular substance containing covalent bonds, is formed in the reaction, H²0(l). The other ions from the acid and alkali stay in the solution as ions of the dissolved salt. These ions combine to form solid sodium chloride, NaCl(s), when the water evaporates.

37
Q

How can you obtain dry soluble salt form its solution?

A

By crystallisation.

38
Q

Why is it important to have a neutral solution before evaporating the water?

A

As if you don’t, you will contaminate the salt with an excess of one reactant.

39
Q

What is titration?

A

A technique in volumetric analysis that is used to find the exact volumes of solutions which react with each other.

40
Q

How can you obtain a neutral solution?

A

By mixing an acid and an alkali in the correct proportions so that you end up with a solution that contains only water and the desired salt.

41
Q

What is a burette?

A

It is a tall glassware with 0.1cm³ graduations. You can control the flow using a tap at the bottom. It is possible to add just one drop at a time.

42
Q

What is a pipette?

A

It is a piece of glassware which is more accurate than a burette as it is smaller and has more precise measurements.

43
Q

What equipment is used for titration?

A
  • A pipette
  • A burette
44
Q

How can you make a pure, dry salt?

A
  1. Carry out a titration
  2. Note the exact volume of acid needed to neutralise the alkali
  3. Use the burette to add the correct volume of acid without the indicator
  4. Evaporate the water from the solution formed
45
Q

What is the reactivity series?

A

A list of metals in order of reactivity with the most reactive at the top.

46
Q

What does the reaction of a metal and an acid produce?

A

Metal + Acid –> Salt + Hydrogen

47
Q

How is the salt produced from a reaction named?

A

The first name of the salt comes from the metal and the second name comes from the acid (e.g. Magnesium reacts with sulfuric acid to form magnesium sulfate)

48
Q

What is an ionic equation?

A

An equation which we only show the ions that change in the reaction (e.g. Mg(s) + 2H+(aq) –> Mg2+(aq) + H²(g)).

49
Q

What are spectator ions?

A

Other ions from the acid that do not change during the reaction.

50
Q

What is an oxidation reaction?

A

A reaction resulting in the loss of electrons.

51
Q

What is a reduction reaction?

A

A reaction resulting in the gain of electrons.

52
Q

What do acids react with metal carbonates to form?

A

A salt, water and carbon dioxide.

53
Q

What does metal carbonate and acid react together to make?

A

Metal carbonate + Acid –> Salt + Water + Carbon dioxide

54
Q

What happens during reactions of metal carbonate and acids?

A

During these reactions, the hydrogen ions from the acids react with the carbonate ions to form water and carbon dioxide molecules.

55
Q

What is a precipitation reaction?

A

A reaction which soluble substances in solutions cause an insoluble precipitate to form.

56
Q

What is a precipitate?

A

An insoluble substance that is formed when two soluble substances react together in a solution.

57
Q

What are some solubility rules for salts?

A

All common sodium, potassium and ammonium salts are soluble in water.

58
Q

What are some solubility rules for nitrates?

A

All nitrates are soluble in water.

59
Q

What are some solubility rules for chlorides?

A

Most chlorides are soluble in water, except for sliver and lead chlorides which are insoluble in water.

60
Q

What are some solubility rules for sulfates?

A

Most sulfates are soluble in water, except for lead, barium and calcium sulfates which are insoluble in water.

61
Q

What are some solubility rules for carbonates?

A

Most carbonates are insoluble in water, except for sodium, potassium and ammonium carbonates which are soluble in water.

62
Q

What are some solubility rules for hydroxides?

A

Most hydroxides are insoluble in water, except for sodium, potassium and ammonium hydroxides which are soluble in water.

63
Q

How can pure, insoluble salt be prepared from two soluble salts?

A
  1. Wear eye protection
  2. Mix the two solutions in a beaker, then filter the mixture
  3. Rinse the beaker with a little distilled water and pour this through the funnel
  4. Pour a little distilled water over the precipitate in the funnel
  5. Carefully remove the filter paper containing the precipitate and dry it in a warm oven

Chemistry (17 decks)

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