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Chemistry GCSE > Chemical Analysis - Flashcards > Flashcards

Chemical Analysis - Flashcards

1
Q

Pure substance

A

A pure substance only contains one type of element or compound throughout

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2
Q

Pure / Impure
Sea Water

A

Impure

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3
Q

Pure / Impure
Ethanol

A

Pure

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4
Q

Pure / Impure
Graphite

A

Pure

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5
Q

Pure / Impure
Fresh mountain air

A

Impure

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6
Q

Impurities result on boiling point of a compound?

A

Boiling point increases
Boil at a range of temperatures

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7
Q

Same ingredients but different formulations? Explain..

A

Formulations contain specific quantities of their components. The medicines have the same ingredients, but if they’re mixed in different ratios, the formulations aren’t the same

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8
Q

Everyday products that are formulations?

A

Paint, Cleaning products, fuels, medicines, cosmetics, fertilisers, alloys

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9
Q

Formula for Rf value of a spot on a chromatography paper?

A

Rf = Distance travelled by substance / Distance travelled by solvent

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10
Q

Insoluble component to mixture, used in chromotography?

A

Will stay on the baseline

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11
Q

Pure substance melting point

A

Sharp, occurs quickly

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12
Q

Mixture melting point

A

Occurs over a range of temperatures

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13
Q

Chromatography:
What to draw baseline in?

A

Pencil

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14
Q

Impurities effect on melting point?

A

Lower the melting point

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15
Q

Examples of pure substances?

A

Water, Copper sulphate, Glucose, Oxygen Gas, Sodium Chloride

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16
Q

How to make sure that a formulation has the correct properties?

A

Chemical components must be present in exact quantities

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17
Q

mixtures of chemical components that are designed to create useful products

A

Formulations

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18
Q

2 phases in chromotography

A

Mobile phase
Stationary phase

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19
Q

What is the mobile phase?

A

Liquid or Gas that carries the the substance up the paper

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20
Q

What is the stationary phase?

A

Solid or Viscous Liquid that the mobile phase moves through

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21
Q

Why does a substance move further in chromotography?

A

It is more attracted to the mobile phase

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22
Q

Why doesn’t a substance move far in chromotography?

A

It is more attracted to the stationary phase

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23
Q

Describe solvent movement in chromotography?

A

Solvent travels up chromatography paper.
As solvent moves, picks up and transports the substances being tested in the chromatography paper.

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24
Q

Higher distance travelled in chromotography?

A

Highly soluble in solvent as they are highly attracted to the mobile phase.
Minimally attracted to chromatography paper and stationary phase

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25
Q

Reference substance

A

pure substance that is run next to tested substance to see if it’s a component in mixture

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26
Q

What does chromatography produce which can be analysed?

A

Chromatogram

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27
Q

Test for hydrogen?

A

Lighted splint placed at mouth of test tube with gas
Positive: Squeaky pop

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28
Q

Why is there is squeaky pop in hydrogen test?

A

Hydrogen burns rapidly in presence of oxygen to produce H2O

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29
Q

Test for oxygen?

A

Glowing splint held at mouth of test tube with gas
Splint will relight

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30
Q

What is limewater?

A

Calcium Hydroxide

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31
Q

Carbon dioxide test:
What type of Calcium Hydroxide (lime water) is needed?

A

Aqueous solution

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32
Q

What is the text for carbon dioxide?

A

Bubble lime water through gas.
If Carbon present lime water turns from clear to cloudy

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33
Q

What type of litmus paper is used to test for Chlorine?

A

Damp blue litmus paper

34
Q

What is the test for Chlorine?

A

Insert damp blue litmus paper into test tube with gas.
If chlorine present the paper is turned from red to bleached white.

35
Q

Flame tests - Potassium (K+)

A

Lilac Flame

36
Q

Flame tests - Lilac

A

Potassium (K+)

37
Q

Flame tests - Sodium (Na+)

A

Yellow flame

38
Q

Flame tests - Yellow

A

Sodium (Na+)

39
Q

Flame tests - Calcium (Ca2+)

A

Orange-red flame

40
Q

Flame tests - Orange-red

A

Calcium (Ca2+)

41
Q

Flame Tests - Copper (Cu2+)

A

Green flame

42
Q

Flame tests - Green

A

Copper (Cu2+)

43
Q

Flame Tests - Lithium (Li+)

A

Crimson flame

44
Q

Flame tests - Crimson

A

Lithium (Li+)

45
Q

Name of wire loop used in flame tests?

A

Nichrome

46
Q

How to clean the nichrome wire loop?

A

Dip in dilute hydrochloric acid

47
Q

Which type of flame to use in ion flame test?

A

Blue

48
Q

Hydroxide precipitate test - Aluminium (Al3+)

A

White (dissolves in excess sodium hydroxide solution)

49
Q

Hydroxide precipitate test - White (dissolves in excess sodium hydroxide solution)

A

Aluminium (Al3+)

50
Q

Colour once white precipitate (Aluminium Hydroxide) dissolves in Sodium Hydroxide solution

A

Colourless

51
Q

Sodium Hydroxide formula

A

NaOH

52
Q

Hydroxide precipitate test - Calcium (Ca2+)

A

White

53
Q

Hydroxide precipitate test - white (2)

A

Calcium (Ca2+)
Magnesium (Mg2+)

54
Q

Hydroxide precipitate test - Magnesium (Mg2+)

A

White

55
Q

Hydroxide precipitate test - Copper (Cu2+)

A

Blue

56
Q

Hydroxide precipitate test - Blue

A

Copper (Cu2+)

57
Q

Hydroxide precipitate test - Iron (II) (Fe2+)

A

Green

58
Q

Hydroxide precipitate test - Green

A

Iron (II)
(Fe2+)

59
Q

Hydroxide precipitate test - Brown

A

Iron (III)
(Fe3+)

60
Q

Hydroxide precipitate test - Iron (III) (Fe3+)

A

Brown

61
Q

Hydroxide precipitate test - 3 white precipitates

A

Calcium Hydroxide
Aluminium Hydroxide
Magnesium Hydroxide

62
Q

Test for Carbonate ions

A

Add dilute hydrochloric acid. If bubbles produced its positive.

63
Q

Carbonate ions

A

CO3^-2

64
Q

Test for Halide Ions:

A

Add dilute nitric acid
Add a few drops of silver nitrate solution

65
Q

Halide Ion test - Chloride (Cl-)

A

White

66
Q

Hailde Ion test - White

A

Chloride (Cl-)

67
Q

Halide Ion test - Bromide (Br-)

A

Cream

68
Q

Halide Ion test - Cream

A

Bromide (Br-)

69
Q

Halide Ion test - Yellow

A

Iodine (I-)

70
Q

Halide Ion test - Iodine (I-)

A

Yellow

71
Q

Why add nitric acid in halide test?

A

Removes any carbonate ions

72
Q

Test for sulphates:

A

Add dilute hydrochloric acid
Add barium Chloride
Becomes barium Sulphate
White precipitate forms (positive)

73
Q

Why add Hydrochloric acid in test for sulphates?

A

Remove carbonate ions

74
Q

Dilute Acid + Carbonate –>

A

Salt + Carbon Dioxide + Water

75
Q

Test for sulphate:
Properties of Barium Sulphate formed?

A

Insoluble
White

76
Q

Sulphates ions?

A

SO4^-2

77
Q

Disadvantages of Instrumental methods?

A
  • Need training
  • Expensive
  • Results only useful when compared to data of known substances
78
Q

Advantages of Instrumental methods?

A
  • Greater sensitivity
  • Greater accuracy
  • Able to analyse tiny samples
  • Quicker at analysing results
79
Q

Steps of Flame Emission Spectroscopy?

A
  • Place sample of metal solution being tested into flame, light will be given off
  • Light given off is captured by spectroscope and read as wavelengths
80
Q

What does Flame Emission Spectroscopy identify?

A

Metal Ions

81
Q

Spectroscopy:
Concentration of Ion?

A

Intensity of line spectra

82
Q

Reference spectra in Spectroscopy?

A

Allows to compare the ions in mixtures

Chemistry GCSE (10 decks)

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