Qualitative
analysis is the type of chemical analysis which its objective is to identify
the ions, atoms or functional groups in an unknown substance.
To
identify the ions, the chemical properties of the unknown substance are
determined by carefully reacting the unknown substance with different reagents.
By defining what the particular reaction will be if a particular ion is
present, the ions that are presence in the solution of the unknown substance
can be identified. For example, adding barium chloride in a solution of a
compound containing tetraoxosulphate (VI), trioxosulphate (IV) or
trioxocarbonate (IV) gives a white precipitate. The precipitate from the last
two will dissolve in dilute acid to produce sulphur (IV) oxide and carbon (IV)
oxide respectively. These reactions help to differentiate between trioxocarbonate
(IV) and trioxosulphate (IV) radicals.
Another method
employed in qualitative analysis is checking the solubility of the various compounds
in water, this is because solubility of different compounds vary in water. The
solubility of some substances in water is listed below:
·
All trioxonitrate (V) salts, NO3-
are soluble
·
All hydrogen trioxocarbonate (IV),
HCO3- are soluble
·
All chlorides Cl- except those of silver, copper and
lead
·
All tetraoxosulphate(VI) salts, SO42-
except those of barium, calcium,silver, lead and mercury.
·
All salts of sodium and potassium
are soluble in water
·
All ammonium salts
Examples of
substances which are not soluble in water is listed below:
·
All trioxocarbonate (IV), CO32-
except those of potassium, sodium and ammonium
·
All hydroxide, OH-,
except those of sodium, potassium and ammonia
It is important to note that coloured ions
are characteristics of transition elements or ions. Most transition elements
form coloured ions in solution due to d-block electrons. This is a very
important hint for identifying transition ions in solution.
Example
Question
Specimen X is an
inorganic compound carry out the following tests and identify and any gas
evolved.
S\N |
Test
|
Observation |
inference |
a |
X
plus heating |
Water
condenses at the cooler part of the test tube, its colour changes from dark
brownish yellow to dark green |
X
has water of crystallization, it is coloured, transition ions likely present |
b |
X
+ water and divide into four portions |
Soluble
in water,and gives a light brownish yellow solution |
Transition
ions Fe2+, Fe3+ etc. likely present |
c
|
To
the first portion, add concentrated H2SO4 + MnO2 + heating, and
place damp starch- iodide paper at tip of the test-tube |
A
greenish yellow gas evolved, with pungent smell and darken starch-iodide
paper |
Chloride
ions, chlorine likely present |
d(I) |
To
the second portion, add dilute HNO3 and silver trioxonitrate
(V)solution |
White
precipitate formed which is insoluble in excess acid and the precipitate
decolourized on exposure to sunlight |
Chloride
ions, chlorine likely present |
d(II) |
To
the mixture above d(i) add ammonia solution in excess |
The
white precipitate dissolved and gives a colourless solution |
Chloride
confirmed and chlorine present |
e |
To
the third portion, add dilute NaOH solution |
Reddish-brown
gelatinous precipitate formed |
Fe3+
present |
f |
To
four portion, add ammonia solution |
Reddish-brown
gelatinous precipitate formed |
Fe3+
confirmed |
Other tests for
Iron (III) ions include:
1.
Test with potassium hexacyanoferrate
(II) solution: iron (III)ions produce a deep blue precipitate with the reagent
2.
Test with potassium thiocyanate
solution or ammonium thiocyanate solution: if the unknown solution contains iron(III)ions,
it will form deep blood red colouration
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