Before we go ahead with this analysis, it will be necessary to note that ammonium ferrous sulphate ((NH4)2Fe(SO4)2.6H2O)
is a double salt which has ammonium ions, iron (II)ions and tetraoxosulphate VI
ions. It has six molecules of water of crystallization and it is also a
reducing agent.
Materials
required for the analysis
The materials and regents we are going to use in
this analysis are as follows:
·
Dilute hydrochloric acid
·
Dilute sodium hydroxide solution
·
Aqueous barium chloride
·
Red and blue litmus paper
·
Distilled water
·
Test tubes and boiling tubes
·
Acidified potassium dichromate
solution
·
Aqueous ammonia
·
Dilute tetraoxosulphate VI acid
·
Source of heat
·
Glass rod
Analysis
of Ammonium Ferrous Sulphate
To analyse the unknown sample, add some samples of the unknown compound into a test tube then add about 10cm3
of distilled water and shake vigorously. Note that the unknown sample is soluble
in water and it gives a slightly yellow solution. The coloured solution is a
characteristic of transition ions which means that transition compounds may be present
as other soluble compounds like K+, and Na+, Divide the
solution into four portions for comprehensive analysis.
To the
first portion, add about 3cm3 of dilute tetraoxosulphate (VI) acid
then potassium dichromate (VI) solution, and the orange colour of the K2Cr2O7
turns green. This means that the unknown sample is a reducing agent, Fe2+,
I-, and NH4+, likely present.
To the second portion, add dilute sodium hydroxide solution, a dirty green gelatinous precipitate is formed, warm gently, effervescence occurs, a gas which has a pungent smell and colourless evolves and turns red litmus paper blue, indicates the presence of ammonium ions while the precipitate shows that iron (II) ions are likely to be present.
To the mixture above, dip a glass rod into
dilute hydrochloric acid, and place it just above the rim of the test tube, if a dense
white fume is formed, that means ammonium ions are confirmed.
To the third
portion, add aqueous ammonia in drops then in an excess, dirty green gelatinous precipitate
which is insoluble in excess confirms that iron (II) ions are present.
To the
fourth portion, add aqueous barium chloride white precipitate formed is an
indication that trioxocarbonate IV ions or trioxosulphate IV ions or
tetraoxosulphate VI ions may be present. Add dilute hydrochloric acid, if the precipitate
remains, then it means the tetraoxosulphate VI ions are confirmed.
Example
Question
The table below is an incomplete test on an
unknown sample G. Carry out the
tests then copy and completes the table.
s/n |
Test |
Observation |
inference |
1 |
G plus
water, shake vigorously and divide into four portions |
Soluble,
the solution has a slightly yellow colour |
|
2 |
To
the first portion, add dilute H2SO4 and K2Cr2O7
solution |
|
G is a
reducing agent, Fe2+, I-, NH4+
likely present |
3 |
To
the second portion, add dilute NaOH solution and warm gently |
A dirty green gelatinous precipitate formed, on heating, a colourless gas with a pungent
smell which turned damp red litmus paper blue |
|
4 |
To
the mixture above (3), dip a glass rod into dilute hydrochloric acid then
place the glass rod just above the rim of the test tube |
|
NH3,
NH4+ confirmed |
5 |
To
the third portion, add aqueous ammonia in drops then excess |
Dirty
green gelatinous precipitate insoluble in excess |
|
6 |
To
the fourth portion, add aqueous barium chloride then dilute HCl acid |
|
CO32-,
SO32-, SO42- likely present SO42-
confirmed |
Answers
s/n |
Test |
Observation |
inference |
1 |
G
plus water, shake vigorously and divide into four portions |
Soluble,
the solution has a slightly yellow colour |
Soluble
ions of K, Na, NH4 and transition ions are likely to be present |
2 |
To
the first portion, add dilute H2SO4 and K2Cr2O7
solution |
The orange colour of K2Cr2O7 turns green |
G
is a reducing agent, Fe2+, I-, NH4+
likely present |
3 |
To
the second portion, add dilute NaOH solution and warm gently |
A dirty green gelatinous precipitate formed, on heating, a colourless gas with a pungent
smell which turned damp red litmus paper blue |
Fe2+
likely present, NH4+, NH3 present |
4 |
To
the mixture above (3), dip a glass rod into dilute hydrochloric acid then
place the glass rod just above the rim of the test tube |
Dense
white fumes formed |
NH3,
NH4+ confirmed |
5 |
To
the third portion, add aqueous ammonia in drops then excess |
Dirty
green gelatinous precipitate insoluble in excess |
Fe2+
confirmed |
6 |
To
the fourth portion, add aqueous barium chloride then dilute HCl acid |
White
precipitate formed Insoluble
in dilute HCl |
CO32-,
SO32-, SO42- likely present SO42-
confirmed |
Interesting.
ReplyDeletethanks
Thanks for the update
ReplyDeleteGood analytical job here
ReplyDelete