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Chemsitry Qualitative > Inorganic Tests > Flashcards

Inorganic Tests Flashcards

1
Q

Blue crystalline solid

A

Possibly contains Cu2+ ions / copper compound

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2
Q

Pale green crystalline solid

A

Possibly contains Fe2+ ions

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3
Q

Red-brown crystalline solid

A

Possibly contains Fe3+ ions

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4
Q

Dissolves in water to form a colourless solution

A

Soluble in water

Compound of G1/G2/ Al / Zn / NH4

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5
Q

Dissolves in water to give a coloured solution

A

Soluble in water

Blue -> Cu2+
Pale Green -> Fe2+
Yellow/ Orange -> Fe3+

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6
Q

Flame tests

A

Calcium etc

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7
Q

White crystalline solid

A

Not a transition metal compound

Compound of: Group 1/2
Ammonium

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8
Q

Conc H2SO4 testing for halide ions

Misty fumes with conc H2SO4

White smoke when glass rod dipped in conc ammonia solution applied

A

Chloride ions present

Misty fumes are HCL

White smoke is Ammonium Chloride

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9
Q

Misty fumes and red brown vapour with conc H2SO4

A

Bromide ions present

Misty fumes is HBr

Red brown fumes = bromine

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10
Q

Misty fumes and purple vapour

Smell of rotten eggs

Yellow solid

Grey black solid on sides of test tube

With conc H2SO4

A

Iodide ions present

Misty fumes = HI

Purple vapour= iodine

Rotten eggs = hydrogen sulphide

Yellow solid = sulphur

Grey black solid = iodine

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11
Q

Testing for halide ions with Silver Nitrate solution

Method

White ppt

Cream ppt

Yellow ppt

No ppt

A

Method: dissolve a spatula measure of sample in dilute nitric acid. Add a few cm3 of silver nitrate solution. Add dil NH3 then Conc NH3?*

White= Cl- AgCl
Redissolves in dil and conc ammonia to form a colourless solution

Cream= Br- AgBr
Not dissolve in dil
Dissolve in conc

Yellow ppt=I- AgI
No dissolve in conc or dil

No ppt = no halide ions present

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12
Q

Testing for Sulfate ions using barium chloride

Method

White ppt

No ppt

A

Dissolve a spatula measure of the sample in dil nitric acid (or HCl)
Add a few drops barium chloride solution

White ppt = SO4/2- present
BaSO4

No ppt= no sulphate ions

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13
Q

Testing for carbonate and hydrogen carbonate ions using nitric acid

Gas?
Negative result?

A

Place a few cm3 of dil nitric acid in a test tube and add a spatula measure of the sample

Effervescence/ solid disappears= CO3/2- or HCO3-

Gas evolved can be passed through limewater (colourless -> milky)

Carbon dioxide released from a reaction of CO3/2-/HCO3- + Acid

***A negative result can be used as the first part of the silver nitrate and halide ions test or the barium chloride and SO4/2- test

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14
Q

Distinguishing between CO3/2- and HCO3- using magnesium nitrate solution (or MgCl)

White ppt

Colourless then white

A

Dissolve a spatula measure of the sample in deionised water
Add a few drops magnesium nitrate solution
* if no ppt appears immediately, boil contents of the test tube

White PPT = CO3/2- MgCO3

Colourless solution= HCO3
No immediate ppt but in boiling white ppt MgCO3

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15
Q

Testing for Fe3+ using potassium thiocyanate (KSCN)

A

Dissolve spatula measure of the sample in deionised water
Add a few drops of potassium thiocyanate (KSCN)

Blood red solution = Fe3+ present

No change = no Fe3+ present

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16
Q

Testing for barium ions using Potassium (VI)Chromate*

Method

Colour

A

Dissolve a spatula measure of the sample in deionised water
Add a few cm3 potassium chromate solution

Yellow ppt- redissolves in HCl to give a yellow solution = Ba2+

No ppt = no Ba2+

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17
Q

Testing for metal cations with sodium hydroxide solution

Method

Pale Green ppt
Brown ppt
White ppt (dissolves in excess)
White ppt (does not dissolve in excess)

A

Dissolve a spatula measure of the sample in deionised water
Add a few drops of NaOH solution
Add until excess

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18
Q

Testing for NH4/+ (ammonium ion) with NaOH

Method

Gas

A 
Place a few cm3 NaOH in test tube
Add spatula measure of the sample 
Warm gently
Test any gas evolved using:
1. Damp red litmus paper
2. Damp universal indicator paper
3. A glass rod dipped in conc HCl

Pungent gas evolved
Damp indicator turns blue
White smoke with HCl

NH4/+ ion present
Ammonia released from action of alkali on an ammonium compound
White smoke is ammonium chloride from reaction of NH3*g + HCl

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19
Q

Testing for metal cations with aqueous (dil) ammonia

White ppt (no dissolve in excess)
White ppt (dissolve in excess gives colourless solution)
Blue ppt (dissolves in excess deep blue solution)
A

Add a spatula measure of the sample to a test tube
Dissolve in deionised water
Add a few drops dil ammonia
Add in excess (5cm3)

White ppt (no dissolve in excess) =Al3+ or Mg2+ Al(OH)3 or Mg(OH)2

White ppt (dissolve in excess gives colourless solution) =Zn2+ Zn(OH)2

Blue ppt (dissolves in excess deep blue solution) = Cu2+ Cu(OH)2

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20
Q

NaOH

White ppt
Does not dissolve in excess

A

Mg2+ ions

White ppt is Mg(OH)2

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21
Q

NaOH

White ppt
Dissolves in excess to give a colourless solution

A

Al3+ ions

Ppt is Al(OH)3 and colourless solution is [Al(OH)4]-

Or

Zn2+ ions

Ppt is Zn(OH)2
Colourless solution is [Zn(OH)4]-

22
Q

NaOH

White ppt that slowly changes to brown on standing

Does not dissolve in excess

A

Mn2+

White ppt is Mn(OH)2

23
Q

NaOH

Blue ppt
Does not dissolve in excess

A

Cu2+ ions if original solution is blue

Blue ppt is Cu(OH)2

Or

CO2+ ions if original solution is pink

Blue ppt is Co(OH)2

24
Q

NaOH

Green ppt
Does not dissolve in excess

A

Ni2+ ions

Green ppt is Ni(OH)2

25
NH3 White ppt Does not dissolve in excess
Al3+ Ppt is Al(OH)3 Or Mg2+ Ppt is Mg(OH)2
26
NH3 White ppt Dissolves in excess to form a colourless solution
Zn2+ White ppt is Zn(OH)2
27
NH3 White ppt Slowly darkens to brown on standing Does not dissolve in excess
Mn2+ ions White ppt is Mn(OH)2
28
NH3 Green ppt Does not dissolve in excess
Fe2+ Green ppt is Fe(OH)2
29
NH3 Brown ppt Does not dissolve in excess
Fe3+ ions Brown ppt is Fe(OH)3
30
NH3 Blue ppt Dissolves in excess to form a yellow solution
Co2+ ions Blue ppt is Co(OH)2 Yellow solution is [Co(NH3)6]2+
31
NH3 Green ppt that dissolves in excess to form a blue solution
Ni2+ ions Green ppt is Ni(OH)2 Blue solution is [Ni(NH3)6]2+
32
NH3 Blue ppt Dissolves in excess to form a deep blue solution
Cu2+ ions Blue ppt is Cu(OH)2 Deep blue solution is [Cu(NH3)4(H2O)2]2+
33
Edta solution testing for Ni2+
Dissolve a spatula measure of the sample in deionised water and add a few cm3 of edta solution Green solution changes to blue if Ni2+ is present Green solution is [Ni(h2o)6]2+
34
1,2-diaminoethane (en) solution testing for Ni2+ ions
Dissolve a spatula measure of the same in deionised water and add a few cm3 of en solution Green solution changes to pink if Ni2+ ions are present Green solution is [Ni(H2O)6]2+ Pink solution is [Ni(en)3]2+
35
Heating a sample of the solid
Place a spatula measure of the sample in a test tube and heat gently Colourless liquid forms on upper walls of test tube Change in solid appearance and possible change in colour Water of crystallisation Hydrated salt
36
Pink crystalline solid
CO2+ ions
37
Pale pink crystalline solid
Mn2+ ions
38
Green crystalline solid
Ni2+ ions or Cr3+ ions
39
Green/violet crystalline solid
Cr3+ ions
40
Orange crystalline solid
Cr2O7 2- ions dichromate(vi)
41
Yellow crystalline solid
CrO4 2- ions chromate(vi)
42
Water Dissolves to form a colourless solution
Soluble in water Compound of G1/G2/aluminium/Zinc/ammonium
43
Water Dissolves in water to form a blue solution
Soluble in water Cu2+ ions or VO 2+ ions
44
Water Dissolves to form a green solution
Soluble in water Fe2+ ions Ni2+ ions Cr3+ ions V 3+
45
Water Dissolves to form a (pale) pink solution
Soluble in water Mn2+ ions Co2+ ions
46
Water Dissolves to form a Yellow solution
Soluble in water CrO4 2- chromate(vi) or VO2 + vanadium(v)
47
Water Dissolves to form an orange solution
Soluble in water Cr2O7 2- dichromate(vi) ions
48
Water Dissolves to form a yellow/ orange solution
Soluble in water Fe3+
49
Water Dissolves to form a violet solution
Soluble in water V2+ ions vanadium(II)
50
Water Does not dissolve
Insoluble in water
51
Barium chloride testing for sulphate ions
Dissolve a spatula measure of sample in dilute nitric acid (or HCl) and add a few cm3 barium chloride White ppt= sulfate ions White ppt is BaSO4 No ppt= no sulfate ions

Chemsitry Qualitative (4 decks)

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