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chemistry > 8-purity, Formulations, Chromatography > Flashcards

8-purity, Formulations, Chromatography Flashcards

1
Q

Lithium flame test

A

Crimson (red) flame

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2
Q

Sodiium flame test

A

Yellow flame

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3
Q

Potassium ion flame test

A

Lilac flame

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4
Q

Copper ions (+2) flame test

A

Green flame

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5
Q

Copper (+2) sodium hydroxide added

A

Blue precipitate- copper hydroxide formed

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6
Q

Calcium ions

A

Flame test-orange-red flame

Sodium hydroxide- white precipitate which does not dissolve when more sodium hydroxide added

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7
Q

Magnesium ions +sodium hydroxide

A

White precipitate which does not dissolve when more sodium hydroxide is added

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8
Q

Aluminium ions and sodium hydroxide

A

White precipitate which dissolves when more sodium hydroxide is addedd

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9
Q

Iron(II) ions and sodium hydroxide

A

Green precipitate - iron hydroxide

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10
Q

Iron (III) and sodium hydroxide

A

Brown precipitate-iron hydroxide

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11
Q

How to test for carbonate ions CO3 2-

A

Dilute acid- bubbles of gas, that would turn limewater cloudy
Barium chloride with hydrochloric acid/silver nitrate with nitric acid- bubbles of gas when acid added

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12
Q

How to test for sulfate ions SO4 2-

A

Forms white precipitate when barium chloride with hcl added (barium sulfate formed)

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13
Q

How to test for chloride ions

A

White precipitate formed when silver nitrate with nitric acid is added (silver chloride)

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14
Q

How to test for bromide ions

A

Cream precipitate formed when silver nitrate with nitric acid is added (silver bromide)

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15
Q

How to test for Iodide ions

A

Yellow precipitate formed when silver nitrate with nitric acid is added (silver iodide)

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16
Q

Crimson (red) flame

A

Lithium ion flame test

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17
Q

Yellow flame

A

Sodium ions flame test

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18
Q

Lilac flame

A

Potassium ions flame test

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19
Q

Green flame

A

Copper 2+ ions flame test

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20
Q

Orange-red flame

A

Calcium 2+ ions

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21
Q

White precipitate which does not dissolve when more sodium hydroxide is added

A

Calcium ions (but can check with orange-red flame) or magnesium ions

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22
Q

White precipitate which does dissolve when more sodium hydroxide added

A

Aluminium ions

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23
Q

Green precipitate

A

Iron (II) ions when sodium hydroxide added

24
Q

Brown precipitate

A

Iron(III) ions with sodium hydroxide

25
Q

Dilute acid added and bubbles of gas which turn limewater cloudy are produced

A

Carbonate (CO3 2-) ions

26
Q

Barium chloride with hcl form white precipitate formed

A

Sulfate so4 2- ions

27
Q

Silver nitrate with nitric acid -white precipitate formed

A

Chloride ions

28
Q

Silver nitrate with nitric acid-cream precipitate

A

Bromide ions

29
Q

Silver nitrate with nitric acid- yellow precipitate

A

Iodide ions

30
Q

Flame emission spectroscopy

A
  • example of aninstrumental method used to analyse metal ions in solution
  • sample put it a flame
  • light given out
    • passed thorugh spectroscope
  • out put line specimin
    • analysed to -identify metal ions ina solution
      - measure their conc
31
Q

Chemical methods

A

Resulsts chemical reactions

32
Q

Eg/. Chemical methods

A
  • flame tests

- adding reagants to give precipitates

33
Q

Pros of chemical methods

A

Often simple to do

34
Q

Cons of chemical methods

A

Uses up sample

35
Q

Pros of instrumental methods

A
  • small sample used
  • cost
  • accurate
  • gives lots info
  • sensitive
36
Q

Cons of instrumental methods

A

-machines;instruments can be expensive

37
Q

Identification of hydrogen

A

Burning splint held at the open end of a test tube of the gas
Hdrogen burns rapidly with a pop sound

38
Q

Identification of oxygen

A

-glowing split inserted into a test tube of the gas relights in the presence of oxygen

39
Q

Identification of co2

A
  • aqueous solution of calcium hydroxide(lime water)

- when co2 is bubbled through it- turns cloudy/miilky

40
Q

Identification of chlorine

A

-damp litmus paper put in chlorine gas, litmus paper is bleached and turns white

41
Q

Solute

A

Soldi that dissolves into the solvent

42
Q

Solvent

A

The liqy=uid that solute dissolves into

43
Q

Solution

A

A solute and solvent mixed together

44
Q

Formulation

A

-a mixture which has a purpose
0mixture must be in fixed proportion
-eg. Fuels, cleaning agent, paints

45
Q

Pure substance

A
  • single element or compound
  • not a mixture
  • eg. Pure milk
  • melting and boiling point can distinguish pure substanceds from mixtures
46
Q

Precipitates

A

-insoluble product that forms when two solutions are mixed and react together

47
Q

Chromatography

A
  • as solvent moves up paper it takes solute
    • dont use wateer as too polar
  • solute dissolves into solvent
  • solute moves in and out of mobile and stationary phase
  • distance moved by solute depends on solubility and attractive forces between solute and chromatography paper
48
Q

Rf value

A
  • quantative approach

- d by solute/d by solvent

49
Q

Why does pure substances look like

A

Single spot in all solvents

50
Q

What are the uses of chromatography

A
  • seperating mixtures

- help identify substances

51
Q

Why some spots may not be seen

A
  • components are colourless in solution

- dyes/chemicals same rf value

52
Q

Flame tets

A
  • used to identify osme metal ions (cations)
  • if sample containing a mixture of ions is used
    • some flame colours may be mixed
53
Q

Metal hydroxides

A
  • used to identifysome metal ions

- when mixed with metal ions- insoluble hydroxide precipitate may be producedd

54
Q

Carbonates

A
  • dilute acids + carbonate ——> co2

- co2 tested with limewater

55
Q

Halides test

A

Halide ions + silver nitrate solution+ dilute nitric acid

-forms precipitate

56
Q

Sulfates test

A

Sulfate ions + barium chromium solution + HCL

-white precipitate

chemistry (14 decks)

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