How to Analyse the Ions in a Mixture of Copper II tetraoxosulphate VI and Ammonium trioxocarbonate IV
Copper sulphate(copper II tetraoxosulphate VI) is one of the soluble compounds of copper, it is a blue crystal solid with five molecules of water of crystallization. It can lose its water of crystallization on strong heating to form anhydrous salt which is white in colour. For more detailed information on the analysis of copper sulphate, click Here.
Ammonium carbonate (ammonium trioxocarbonate
IV) is a white crystal solid and it is very soluble in water, Click here for more information.
A mixture
of ammonium Carbonate and copper sulphate will undergo double decomposition to
give ammonium sulphate and copper carbonate. Double decomposition is a type of
reaction in which two soluble compounds react by the exchange of radicals to form
one soluble compound and one insoluble compound.
CuSO4 + (NH4)2CO3
------- CuCO3 + (NH4)2SO4
Copper carbonate is a green powder and insoluble
while ammonium sulphate is a white crystal solid and soluble in water.
How
to Identify the Two Cations in the Mixture
To the mixture, add about 10 ml of distilled water,
stir thoroughly and filter keeping both residue and the filtrate. Since the
mixture is a product of double decomposition, the cations are in both filtrate
and residue. The analysis must be carried out on both residue and filtrate
in other to identify each of the ions.
Firstly the filtrate, divide the filtrate into two
portions, and to one of the portions, add sodium hydroxide, The appearance of a pale blue precipitate or deep blue colour may be a result of copper sulphate
as an impurity in the filtrate, Heat the mixture and dip a glass rod into
potassium dichromate VI solution let it make contact with the gas given off, if
the gas has a pungent smell and changes the orange colour of potassium dichromate
VI to light green, it means that the gas is a reducing agent and it may be
sulphur IV oxide or ammonium gas. Then bring damp litmus paper close to the gas,
if it turns litmus blue then the gas is ammonia gas. Another test is to dip a
glass rod into dilute hydrochloric acid and let it make contact with the gas evolving;
dense white formed at the point of contact confirms ammonium ion or ammonia gas.
Secondly, the residue is divided into two, To one portion of the residue, add dilute hydrochloric acid then aqueous ammonia solution in drops then excess
pale blue gelatinous precipitate which is soluble in excess to form a deep
solution confirms copper ion. Sodium hydroxide can be used but in this case, the
pale blue gelatinous precipitate remains insoluble in excess sodium hydroxide solution.
For more information on copper ion analysis, click here.
How
to Identify the Anion in the Mixture
Again add the filtrate in the test tube, then add
barium chloride solution, if a white precipitate is formed, it might be
trioxocarbonate IV ions, trioxosulphate IV ion or tetraoxosulphate VI because
all these radicals can give white precipitate barium chloride. Add dilute hydrochloric
acid, if the precipitate remains, it means that the ion is tetraoxosulphate VI
ions.
Finally, put the residue into a test tube, and add
dilute hydrochloric acid, a colourless, odourless gas which turns damp litmus
paper red and also turns lime water milky confirms trioxocarbonate IV ion
Example
Question
H is a mixture of two inorganic compounds. Carry out
the following exercise on H. Record your observations and identify any gases that evolved. State the conclusion you draw from the result of each test.
|
Test |
Observation |
Inference |
a(I) |
H
plus water stir thoroughly and filter, then divide the filtrate into two
portions. Keep the residue |
Green
residue and clear filtrate. |
|
II |
To
the first portion, add dilute NaOH and heat |
|
NH3,
SO2, and HCl gases are likely to be present |
III |
Dip
a glass rod into acidified potassium dichromate VI solutions and bring in contact
with the gas given off from (II)above |
The
orange colour turns to light green |
|
IV |
Dip
a glass rod into dilute HCl and bring it closer to the gas then damp litmus
paper |
|
The
gas is NH3 , NH4+
present or confirmed |
V |
To
the second portion of the filtrate, add BaCl2 + dilute HCl |
White
precipitate insoluble in dilute HCl |
|
B(I) |
To
the residue, add dilute HCl, test with litmus paper then bubble into lime
water |
|
CO2,
gas, CO32- present |
(II) |
To
the mixture above b(I)add aqueous ammonia solution in drops and in excess |
Pale
blue gelatinous precipitate soluble in excess to form a deep blue solution |
|
|
Test |
Observation |
Inference |
a(I) |
H
plus water stir thoroughly and filter, then divide the filtrate into two
portions. Keep the residue |
Green
residue and clear filtrate. |
H is a mixture of soluble and insoluble compounds, and transition ions are likely to be present. |
II |
To
the first portion, add dilute NaOH and heat |
Gas
with a pungent smell |
NH3,
SO2, and HCl gases are likely to be present |
III |
Dip
a glass rod into acidified potassium dichromate VI solution and bring in contact
with the gas given off from (II)above |
The
orange colour turns to light green |
The
gas is a reducing agent, SO2, and NH3 are likely to be present |
IV |
Dip
a glass rod into dilute HCl and bring it closer to the gas then damp litmus
paper |
Dense
white fumes formed, and red litmus paper turned blue |
The
gas is NH3 , NH4+
present or confirmed |
V |
To
the second portion of the filtrate, add BaCl2 + dilute HCl |
White
precipitate insoluble in dilute HCl |
SO42-
present or confirmed |
B(I) |
To
the residue, add dilute HCl, test with litmus paper then bubble into lime
water |
Blue
litmus turns red and lime water turns milky |
CO2,
gas, CO32- present |
(II) |
To
the mixture above b(I)add aqueous ammonia solution in drops and in excess |
Pale
blue gelatinous precipitate soluble in excess to form a deep blue solution |
Cu2+
confirmed |
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