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Required practicals > Required practical 4 > Flashcards

Required practical 4 Flashcards

1
Q

Testing for Group 2

A
  1. Add dilute NaOH drop wise to test tube containing solution
    - Observe the precipitate formed
  2. Continue adding dilute NaOH until it is in excess
    - Observe the precipitate formed
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2
Q

Group 2 - results

A

Mg - Slight white –> White
Ca - slight white –> slight white
Sr - slight white –> slight white
Ba - no change –> no change

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3
Q

Testing for Ammonium ions

A
  1. Add dilute NaOH to solution
  2. Heat gently
  3. Hold damp red litmus paper above test tube
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4
Q

Ammonium ions - results

A

If Ammonia gas is given off then ammonium ions are present - this is shown by red litmus paper turns blue

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5
Q

Why must litmus paper be damp when testing for ammonium ions

A

To allow the ammonia gas to dissolve

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6
Q

Ammonium ions - equation

A

NH4+ + OH- –> NH3 + H2O

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7
Q

Testing for sulfate ions

A
  1. Add dilute HCL
  2. Add Barium chloride
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8
Q

Sulfate ions - result

A

White precipitate of BaSO4 is produced

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9
Q

Sulfate ions - equation

A

Ba2+ + SO42- –> BaSO4

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10
Q

Testing for hydroxide ions

A
  1. Add universal indicator
    Or
  2. Dip red litmus paper into solution
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11
Q

Hydroxide ions result

A
  1. Universal indicator turns blue
  2. Red litmus paper turns blue
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12
Q

Testing for Halide ions

A
  1. Add dilute nitric acid
  2. Add silver nitrate
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13
Q

Halide ions - results

A

Chloride - white precipitate that dissolves with dilute ammonia Bromide - cream precipitate that dissolves with concentrated ammonia
Iodide - yellow precipitate

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14
Q

What is the purpose of dilute nitric acid when testing for halide ions

A

Removes any carbonate ions which may form silver carbonate - precipitate

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15
Q

Testing for carbonate ions

A
  1. Add dilute acid
  2. Bubble gas produced through limewater
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16
Q

Carbonate ions - results

A
  1. Effervescence
  2. Carbon dioxide turns limewater cloudy
17
Q

Carbonate ions - equation

A

CO32- + 2H+ –> CO2 + H2O

Required practicals (16 decks)

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