2.12 Qualitative Analysis

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Test for Water: Add to anhydrous copper (II) sulfate
White copper (II) sulfate turns blue
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Test for Water: Add to anhydrous cobalt (II) chloride
Blue cobalt (II) chloride turns pink
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CO2: Pass through limewater
Changes from colourless to milky (if in excess, milky precipitate will redissolve to form colourless solution)
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H2: Put a burning splint into a sample of the gas
Burns with a pop
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O2: Put a glowing splint into a sample of the gas
Splint relights
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Cl2: Damp universal indicator paper or damp litmus paper
(Turns red then) bleaches
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SO2: Filter paper dipped in acidified potassium dichromate (VI) solution
Orange to green
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NH3: (1) Damp universal indicator paper (2) Glass rod dipped in conc. hydrochloric acid
(1) Turns blue (2) White fumes
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HCl: (1) Damp universal indicator paper (2) Glass rod dipped in conc. ammonia solution
(1) Turns red (2) White fumes
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White crystalline solid
Does not contain transition metal ions
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Blue crystalline solid
Contains copper (II) ions
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Pale green crystalline solid
Contains iron (II) ions
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Red-brown crystalline solid
Contains iron (III) ions
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Dissolves to form a colourless solution
Soluble in water
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Dissolves to form a coloured solution
Blue - Copper (II) ions. Pale green - Iron (II) ions. Yellow/orange - Iron (III) ions
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Does not dissolve
Insoluble in water
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Crimson Flame
Lithium ions
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Yellow/orange Flame
Sodium ions
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Lilac Flame
Potassium ions
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Brick red Flame
Calcium ions
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Green Flame
Barium ions
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Blue-green Flame
Copper ions
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Concentrated sulfuric acid: Misty fumes; white smoke when glass rod dipped in conc. ammonia solution
Chloride ions: Misty fumes are HCl: White smoke = Ammonium chloride; hydrogen chloride gas released
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Concentrated sulfuric acid: Misty fumes; red-brown vapour
Bromide ions; Misty fumes are HBr; Red-brown fumes are bromine
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Concentrated sulfuric acid: Misty fumes; purple vapour; smell of rotten eggs; yellow solid; black solid on side of test tube
Iodide ions; Misty fumes are HI; purple vapour is iodine' smell of rotten eggs is hydrogen sulfide; yellow solid is sulfur; black solid is iodine
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Silver Nitrate Solution: White precipitate that redissolves in dilute and conc. ammonia solution to form a colourless solution
Chloride ions; White precipitate is AgCl
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Silver Nitrate Solution: Cream precipitate that does not redissolve in dilute ammonia solution but does redissolve in conc. ammonia solution to form a colourless solution
Bromide ions; Cream precipitate is AgBr
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Silver Nitrate Solution: Yellow precipitate that does not redissolve in either diltue or conc. ammonia solution
Iodide ions; Yellow precipitate in AgI
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Barium chloride solution:White precipitate
Sulfate ions; White precipitate is BaSO4
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Barium chloride solution: No precipitate
No Sulfate ions
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Dilute nitric acid: Effervescence; solid disappears; Gas eveolved can be passed through limewater to change it from colourless to milky
Carbonate ions or Hydrogencarbonate ions
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Dilute nitric acid: No effervescence; no gas produced
No Carbonate ions or Hydrogencarbonate ions
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Magnesium nitrate solution: White precipitate appears
Carbonate ions present; White precipitate is magnesium carbonate
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Magnesium nitrate solution: White precipitate appears on boiling from a colourless solution
Hyrdorgencarbonate ions present; white precipitate is magnesium hydrocarbonate
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Magnesium nitrate solution: No precipitate
No carbonate or hydrogencarbonate ions present
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Potassium thiocyanate (KSCN): Blood red solution
Iron (III) ions present
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Potassium thiocyanate (KSCN): No change
No iron (III) ions present
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Potassium chromate (VI) solution: Yellow precipitate that redissolves in dilute hydrochloric acid to form a yellow solution
Barium ions present; Yellow precipitate is Barium chromate (VI)
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Potassium chromate (VI) solution: No precipitate
No Barium ions present
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Sodium hydroxide solution: Pale green precipitate that does not dissolve in excess sodium hydroxide
Iron (II) ions present; Green precipitate is iron (II) hyroxide
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Sodium hydroxide solution: Brown precipitate that does not dissolve in excess sodium hydroxide
Iron (III) ions present; Brown precipitate is iron (III) hyroxide
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Sodium hydroxide solution: White precipitate that does not dissolve in excess sodium hydroxide
Magnesium ions present; White precipitate is magnesium hydroxide
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Sodium hydroxide solution: White precipitate that does dissolve in excess sodium hydroxide solution to form a colourless solution
Either Aluminium, or zinc ions present; White precipitate is their hydroxides
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Sodium hydroxide solution; Pungent gas evolved; damp indicator paper changes to blue; white smoke with glass rod dipped in conc. hydrochloric acid
Ammonium ions present
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Aqueous ammonia; White precipitate that does not dissolve in excess aqueous ammonia
Aluminium or magnesium ions present
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Aqueous ammonia; White precipitate that does dissolve in excess aqueous ammonia
Zinc ions present
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Aqueous ammonia; Blue precipitate that dissolves in excess ammonia solution to form a deep blue solution
Copper ions present
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Other cards in this set

Card 2

Front

Blue cobalt (II) chloride turns pink

Back

Test for Water: Add to anhydrous cobalt (II) chloride

Card 3

Front

Changes from colourless to milky (if in excess, milky precipitate will redissolve to form colourless solution)

Back

Preview of the back of card 3

Card 4

Front

Burns with a pop

Back

Preview of the back of card 4

Card 5

Front

Splint relights

Back

Preview of the back of card 5
View more cards

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