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chemistry > chemical analysis > Flashcards

chemical analysis Flashcards

1
Q

whats a pure substance

A

one type of element or compound with a set melting and boiling point

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2
Q

whats an unpure substance

A

2 or more type of elements or compounds with varied melting and boiling points

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3
Q

whats a formulation

A

a mixture designed to have specific properties

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4
Q

what are formulation uses

A

shampoo
paint ect

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5
Q

the components in a formulation are …

A

carefully controlled

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6
Q

what are the 2 phases in chromatography

A

stationary
mobile

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7
Q

what does chromatography do

A

separates mixtures into compounds

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8
Q

whats the process of chromatography and what does the movement depend on

A

solvent dissolves samples and carries them up the paper

movement depends on its attraction to the solvent and paper

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9
Q

how to calculate rf values

A

distance compound moved
/distance solvent moved

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10
Q

how to test for hydrogen

A

squeaky pop

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11
Q

how to test for oxygen

A

glowing splint re lit

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12
Q

how do test for chlorine

A

damp litmus paper is beached

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13
Q

how to text for carbon dioxide

A

limewater goes milky

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14
Q

what is flame emission spectroscopy used for

A

more accurate results of a flame test

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15
Q

what are the advantages for instrumental methods (3)

A
  • quicker
  • sensitive
  • accurate
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16
Q

what are the disadvantages for industrial methods

A
  • complex
  • expensive
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17
Q

how does light emission spectroscopy work

A

light from the flame, reflected through concave mirror and then separated by a prism into individual lights which can determine the metal

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18
Q

what are flame tests used for

A

to identify metal ions

19
Q

colours for a flame test

COPPER

A

GREEN

20
Q

colours for a flame test

CALCIUM

A

BRICK RED

21
Q

colours for a flame test

SODIUM

A

YELLOW

22
Q

colours for a flame test

POTASSIUM

A

LILAC

23
Q

colours for a flame test

LITHIUM

A

CRIMSON

24
Q

how’s does a flame test work

A
  • clean metal rod with HCL to get rid of any past metal ions
  • dip rod in solution of metal and place under flame
25
Q

what is the disadvantage of a flame test

A

if there is more then one metal ion present they can be masked to give inaccurate results

26
Q

what is the test for reacting carbonates

A

dilute HCL added to a carbonate would form carbon dioxide which can be tested with lime water

27
Q

general ionic equation for reacting carbonates

A

Ca 2+ + CO3 2- = CaCO3

28
Q

test for reacting sulphates

A

mixing HCL and barium chloride with mixture, if sulphate is present white precipitate is formed

29
Q

general ionic equation for reacting sulphates

A

Ba 2+ + SO4 2- = BaSO4

30
Q

test for reacting halides

A

mixing with dilute nitric acid and silver nitrate, if a hale is present a coloured precipitate would form

31
Q

general ionic equation for reacting halides
Where X is the halide

A

Ag + + X - = AgX

32
Q

when chlorine is present when reacting halides what colour is shown

A

white

33
Q

when Bromine is present when reacting halides what colour is shown

A

cream

34
Q

when Iodine is present when reacting halides what colour is shown

A

yellow

35
Q

whats the test for metal ions (not flame)

A

adding sodium hydroxide to form a coloured precipitate

36
Q

what colour precipitate does calcium go in a metal test

A

White

37
Q

what colour precipitate does copper (II) go in a metal test

A

Blue

38
Q

what colour precipitate foes does iron (II) go in a metal test

A

Green

39
Q

what colour precipitate does iron (III) go in a metal test

A

Brown

40
Q

what colour precipitate does Aluminium go in a metal test

A

White

41
Q

what colour precipitate does magnesium go in a metal test

A

White

42
Q

how do you differentiate from calcium, magnesium and aluminium in a test for metal ions

A

aluminium - dissolves when excess sodium hydroxide is added

calcium - brick red in flame test

magnesium - no colour change in flame test

43
Q

what is an example of an ionic equation for iron (II) and aluminium

A

Fe 2+ + 2OH 2- = Fe(OH)2

Al 2+ + 2OH 2- = Al(OH)2

chemistry (5 decks)

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