Analysis Of Ions And Gases Flashcards

1
Q

Describe how to do a flame test.

A

1) Clean the end of the Nichrome wire by dipping into HCL, place in a roaring Bunsen. Repeat until wire no longer produces a colour.
2) Dip end of wire into fresh HCL and then into solid sample.
3) Place wire into non roaring, non luminous flame.
4) Record colour of the flame

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2
Q

Flame test: Lithium

Li +

A

Pink/Red

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3
Q

Flame test: Sodium

Na+

A

Orangey-yellow

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4
Q

Flame test: Potassium

K+

A

Lilac

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5
Q

Flame test: Copper (II)

Cu2+

A

Greeney-blue

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6
Q

Flame test: Calcium

Ca2+

A

Brick red

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7
Q

Describe how to work out the analysis of metal cations.

A
  • Add NaOH a drop at a time to a solution of you cation.
  • The OH- ions in the solution react with some positive metal ions in precipitation reactions to produce coloured insoluble metal hydroxide precipitates.
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8
Q

Observation of Copper (II) and Sodium Hydroxide -

A

Blue precipitate formed

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9
Q

Observations of Iron (II) and Sodium Hydroxide-

A

Green precipitate formed (murkyish)

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10
Q

Observations of Iron (III) and Sodium Hydroxide -

A

Orangey-browny precipitate formed.

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11
Q

Describe the analysis of ammonium (NH4+).

A
  • Add 2cm3 of sodium hydroxide to the solid/solution under test.
  • Warm the mixture, in a water bath.
  • If ammonium ions are present, then ammonia gas (NH3) will be produced.
    - This is a pungent smelling gas, which turns damp red litmus paper blue.
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12
Q

Describe the analysis of positive ions.

A
  • Add small amount of NaOH to a solution of you +be ions.
    The OH- ions in the solution react with some positive metal ions in precipitation reactions to produce coloured insoluble metal hydroxide precipitates.
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13
Q

How do you identify a carbonate?

A
  • Add dilute HCl (2cm depth) to the solid carbonate or its aqueous solution.
  • Use delivery tube to bubble the gas through lime water.
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14
Q

Observations of Calcium Carbonate with dilute HCl

A
  • Limewater turns cloudy

- Bubbles of gas

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15
Q

How do you identify sulphates?

A
  • Add dilute HCl (2cm depth) and Barium Chloride solution (2cm depth) to a solution of a sulphate (2cm depth).
  • HCl is added first to remove any carbonate ions that might be present - would also produce the same observation, giving false positive test.
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16
Q

Observations of Sodium Sulphate with dilute HCl and Barium Chloride -

A

Solution turns cloudy

17
Q

How do you identify Chlorides, Bromides and Iodides?

A
  • Add dilute nitric acid (1cm depth) and silver nitrate solution (2cm depth) of chloride or a bromide or an iodide (2cm depth).
  • Nitric acid reacts with any other ions that might give a confusing precipitate (produces nitrates, and all nitrates are soluble)
18
Q

Observation of chloride with dilute nitric acid and silver nitrate solution -

A

Forms a white precipitate.

19
Q

Observation of bromide with dilute nitric acid and silver nitrate -

A

Forms a cream precipitate.

20
Q

Observation of iodide with dilute nitric acid and silver nitrate -

A

Forms a yellow precipitate.

21
Q

When is upwards delivery used?

A
  • For gases less dense than air e.g H2, NH3
22
Q

What happens in upwards delivery?

A

The gas produced pushes the air in the gas jar/test tube out the bottom

23
Q

When is downwards delivery used?

A

For gases more dense then air e.g CO2 and Cl2.

24
Q

What happens in downwards delivery?

A

The gas produced pushes the air in the gas jar/test tube out of the top.

25
Q

What happens when the gas is “over water” (displacement occurs)?

A

The gas produced in the reaction is bubbled through a trough of water into a upside down jar filled with water. The gas displaces the water, pushing it out the bottom. A ‘beehive shelf’ directs the gas into the gas jar.

26
Q

When is over water (displacement) used?

A

Only works for insoluble gases/slightly soluble gases.
H2 is insoluble, O2 and CO2 are only slightly soluble in water.
- Wouldn’t work for NH3 and Cl2 as they are soluble.

27
Q

When is a gas syringe used?

A

Can be used to collect any gas. For testing the gas must be transferred to a test tube using one of the first 3 methods.

28
Q

Test for chlorine and result

A

Damp blue litmus paper

  • Will turn red
  • Bleach it
29
Q

Test for hydrogen and result

A

Put a lit splint in a test tube

- squeaky pop

30
Q

Test for ammonia and result

A

Use damp red litmus paper

- Turns blue

31
Q

Test for Carbon Dioxide and result

A

Bubble gas through lime water

- Limewater turns cloudy/milky

32
Q

Test for oxygen and result

A

Put glowing splint in test tube

- Splint relighting

33
Q

Where should the preparation and testing of chlorine and ammonia occur? Why?

A

Both are toxic, therefore going to be released in the atmosphere.
Should be done in a fume cupboard.

34
Q

Chemical test for water

A

Water turns white anhydrous copper (II) sulphate BLUE.

- Only confirms water is present not pure.

35
Q

How to test if water is pure?

A

It should melt at 0ºC and boil at 100ºC.