READY REFERENCE CHART.pdf

Ready reference

1. READY REFERENCE CHART FOR QUALITATIVE ANALYSIS OF BASIC RADICALS
Make the solution of the given mixture in distilled water, in dil. HCl or conc. HCl cold or hot. Label it original solution (O.S.). To the O.S., add dil. HCl.
If group I is absent, pass H₂S gas through O.S. for suf?icient time after acidiication with dil. HCl & Filter.White ppt.
(Pb²⁺)
Con?irmation of Pb²⁺
Boil white ppt. with distilled
water and divide the solution
into two parts :
(i) Add KI solution to one
part of above solution.
con?irms Pb²⁺. Yellow ppt.
(ii) Add K₂CrO₄ solution to
the second part of the
above solution. Yellow
con?irms Pb²⁺ppt.
Ppt. -Group II
Black ppt. - (Pb²⁺, Cu²⁺)
Yellow ppt. - (As³⁺)
Dissolve, the black ppt. in minimum quan-
tity of 50% HNO₃₊To one part of the above
solution add dil. H₂SO₄ and alcohol. If a
white ppt. is formed Pb²⁺ is indicated. If no
white ppt. is formed, add excess NH₄OH to
the second part of solution - Blue coloured
solution indicates Cu²⁺
Con?irmation of Cu²⁺
(i) Add excess of NH₄OH solution to
original solution. Deep blue solution.

(ii) Acidify the above deep blue solution
with dil. acetic acid. Add Pot.
ferrocyanide solution. Chocolate
brown ppt. con?irms Cu²⁺
Con?irmation of Pb²⁺
(i) To the O.S. add KIPot. iodide test.
solution Yellow ppt.
(ii) To the O.S. addPot. chromate test.
K₂CrO₄ Yellow ppt.
If the ppt. obtained is yellow in colour - As³⁺
is indicated.
Con?irmation of As³⁺
(i) Yellow ppt.Amm. molybdate test.
+ conc. HNO₃ + Amm. molybdate
solution - Yellow ppt.
Magnesia mixture test. (ii) To the O.S.
add magnesia mixture - White ppt.
If group II is absent, add solid NH₄Cl, O.5 ml conc. HNO₃ to the O.S. Boil and cool & add NH₄OH till it smells of ammonia. If a ppt. is formed, group III is present.
Reddish brown ppt. - (Fe³⁺)
White ppt. - (Al³⁺)
Con?irmation of (Fe³⁺)
Dissolve the brown ppt. in dil. HCl and
divide the solution into two parts.
(i) To one part of solution add pot.
ferrocyanide solution. A prussion
blue colourppt. or
(iii) To second part of solution add
pot. sulphocyanide solution - A
blood red colouration.
Con?irmation of Al³⁺
(i) Perform charcoal cavity - cobalt
nitrate test with white ppt. Blue
mass.
(ii) White ppt. + dil. HCl + aLake test.
few drops of blue litmus solution +
NH₄OH Solution in excess. A blue
ppt., suspended in a colourless
medium (called a lake).
If group III is absent, through a part of the solution obtained in Group III pass H₂S gas. if a ppt. is obtained
group IV is present.
White ppt - (Zn²⁺)
Black ppt. - (Ni²⁺ and Co²⁺)
Flesh coloured ppt. - (Mn²⁺)
Con?irmation of Zn²⁺
Dissolve a part of white ppt. in dil. HCl and
divide the solution in two parts
(i) To one part of solution add pot.
ferrocyanide solution- Bluish
white ppt.
(ii) To second part of solution add NaOH
White ppt. soluble in excess. solution.
Con?irmation of Ni²⁺ and Co²⁺
+
If the ppt. obtained is black Ni²⁺or Co²is
indicated. Note the colour of the salt, if the
salt is greenish - Ni²⁺ is indicated and if

the salt is purple Co²⁺is indicated
Con?irmation of Co²⁺
(i) Take O.S. and neutralise the acid by
adding NH₄OH. Add a pinch of potassium
nitrite and acidify with dil. acetic acid
- Yellow ppt.
(ii) Perform borax bead test with salt
Blue bead.
Con?irmation of Ni²⁺
(i) Take O.S. and make alkaline by adding
NH₄OH and then add a few drops of
dimethyl glyoxime - Bright red ppt.
(ii) Perform borax bead test with salt-
Brown bead in oxidising ?lame
and grey bead in reducing lame.
Con?irmation of Mn²⁺
(i) Dissolve lesh coloured ppt. in dil. HCI,
boil off H₂S , add NaOH and Br₂ water
- White ppt. turning grey.
(ii) Perform borex bead test with group
ppt - in oxidising lame and Pink bead
colourless in reducing lame.
If group IV is absent, to the O.S. add solid NH₄CI, NH₄OH and (NH₄)₂CO₃ Solution.
White ppt. - (Ba, Sr, Ca)²⁺²⁺²⁺
Dissolve a part of white ppt. in dil. acetic
acid & boil off CO.₂
(i) To one part of the above solution add
Con?irmsK₂CrO₄ solution. Yellow ppt.
Ba²⁺
(ii) If Ba²⁺ is absent, then to the second
part of above solution add ammonium
sulphate solution. White ppt. -A con
irms Sr.²⁺
(iii) If Both Baand Srare absent, then²⁺ ²⁺
to the third part of the above solution
add ammonium oxlate solution. A
white ppt. con?irms Ca .²⁺
Perform the lame test with a part of the
salt.
(i) con?irmed. Light green lame-Ba²⁺
Crimson red lame- Sr (ii) con?irmed.²⁺
(iii) con?irmed.Brick red lame - Ca²⁺
If group V is absent, test for Mg²⁺
(i) To the O.S. add a pinch of NH₄Cl, a
few drops of NH₄OH and excess of
solution - amm. phosphate White
ppt.- Mg ²⁺

(ii) Perform charcoal cavity cobalt
nitrate test with white ppt. - A Pink
mass.
Test for NH₄⁺
Heat the salt and sodium hydroxide
solution. If ammonia gas evolves, NH ₄⁺
is present.
Pass the gas through Nessler's reagent.
A brownish ppt. or colouration is
obtained.
Note. NH₄⁺ may be tested in the beginning
of analysis of basic redicals as zero group.

2. READY REFERENCE CHART FOR QUALITATIVE ANALYSIS OF ACID RADICALS
Dil. H₂SO₄ Test
Treat the salt with dil. H₂SO₄
(i) CO₂ gas, turns lime water milky - CO₃²
2
(ii) H₂S gas (smells like rotten eggs), turns lead acetate paper black - S
2
(iii) SO₂ gas, turns acidiied potassium dichromate paper green - SO₃
(iv) NO₂ gas (reddish brown), turns FeSO₄ solution black - NO₂
CONFIRMATORY TESTS
Conirmation of CO₃²

Try to dissolve the salt in water. If the salt dissolves is indicated.soluble CO
-
₃²
(i) To the solution add dil. HCl - evolves with brisk effervescence. CO₂ gas
(ii) To the solution add MgSO₄ solution conirms soluble carbonate.- White ppt.
If the salt does not dissolve in water - is indicated. insoluble carbonate
To the solid salt add dil. HCl - CO₂ gas evolves with brisk effervescence - conirms
insoluble carbonate.
-
Conirmation of S²
(i) W.E. or S.E. + acetic acid + lead acetate solution - Black ppt.
colouration.(ii) W.E. or S.E. + Sod. nitroprusside solution - A purple or violet
- A yellow ppt.(ii) W.E. or S.E. + suspension of CdCO₃
-
Conirmation of SO₃²
(i) W.E. or S.E. + BaCl₂ solution - which dissolves with evolution of White ppt.
SO₂ on adding dil. HCl.
(ii) Salt + a few drops of acidiied KMnO₄ - Pink colour of KMnO₄ disappears.
-
Conirmation of NO₂
(i) W.E. + acetic acid + FeSO₄ -Dark brown or black colour.
- Blue(ii) W.E. + 2-3 drops of H₂SO₄ + KI solution + 2-3 drops of starch solution
colouration.
(iii) W.E. + a few drops of acidiied KMnO₄ solution - Pink colour disappears.
If no gas is evolved when the salt is treated with dilute sulphuric acid.

- Absence of CO₃², S², SO₃²and NO₂
- - - -
Conc. H₂SO₄ Test
Heat a pinch of the salt with conc. H₂SO₄
-
(i) HCl gas gives white ppt. (soluble in NH₄OH) with AgNO₃ - Cl
-(ii) Br₂ gas turns starch paper yellow or orange - Br..
-
(iii) I₂ vapours turns starch paper blue - I.
-
(iv) NO₂ gas (on adding a paper pellet) turns FeSO₄ solution black - NO₃
2-
(v) A colourless, odourless gas (CO₂) - C₂O₄
-
(vi) Colourless vapours with vinegar smell - CH₃COO
CONFIRMATORY TESTS
-
Conirmation of Cl
(i) To the salt solution add conc. HNO₃ and AgNO₃ solution -A solublewhite ppt.
in NH₄OH solution.
(ii) To the salt add MnO₂ and conc. H₂SO₄ and heat - Cl₂ gas evolves.
(iii) Salt + K₂Cr₂O₇ solid + conc. H₂SO₄, heat - Red vapours. Pass the vapours
through NaOH solution. To the yellow solution obtained add acetic acid and
-
lead acetate solution conirms Cl- yellow ppt.
-
Conirmation of Br
(i) Salt solution + conc. HNO₃ + AgNO₃ solution - Pale yellow ppt. partially
soluble in NH₄OH.
(ii) Salt solution + dil. HCl + 1-2 ml of carbon disulphide +Chlorine water test.
chlorine water, shake - Orange colour in CS₂ layer.
-
Conirmation of I
(i) Salt solution + conc. HNO₃+ AgNO₃ solution - Yellow ppt. insoluble in NH₄OH.
(ii) Salt solution + dil. HCl + 1-2 ml of CS₂+ ChlorineChlorine water test.
water, shake - violet colour in CS₂ layer.
-
Conirmation of CH₃COO
(i) Solid salt + oxalic acid + 2-3 drops of water, rub - Oxalic acid test. Vinegar
smell.
(ii) Ester test. - Fruity smell.Salt + conc. H₂SO₄ + Ethyl alcohol, heat
2-
Conirmation of C₂O₄
(i) Salt solution + acetic acid + CaCl₂ solution - White ppt.
- Pink colour is(ii) Salt + dil. H₂SO₄, warm and add 2-3 drops of KMnO₄ solution
discharged.
-
Conirmation of NO₃
(i) Mixture + conc. H₂SO₄+ Cu chips. Heat - Reddish brown gas.
- Dark brown(ii) W.E. + FeSO₄ solution + conc. H₂SO₄ by the sides of the tube
ring.
If no gas is evolved when mixture is heated with conc. H₂SO₄₊
- -- - - -
Absence of Cl, Br , I, NO₃, CH₃COO and C₂O₄²
If the salt does not react with dil. H₂SO₄ as well as conc. H₂SO₄ test for
- -
SO₄²and PO₄ ³
-
Conirmation of SO₄²
(i) W.E.or S.E. + dil. HCl + BaCl₂ Solution - Barium chloride test. White ppt.
insoluble in dil HCl
(ii) Mix the salt with Na₂CO₃. Make its paste. Fuse a littleMatch stick test.
paste on the end of match stick. Dip the fused mass in sod. nitroprusside
solution - Purple steaks.
-
Conirmation of PO₄³
(i) S.E. + conc. HNO₃ and boil. Now add amm.Ammonium molybdate test.
molybdate sol. and heat - Yellow ppt.
(ii) W.E. or neutral S.E.+ Magnesia mixture Magnesia mixture test. - White
ppt.

3. Table : Physical Examination
1. Colour
Experiment Observations Inference
2. Smell
3. Density
4. Deliquescence
Blue or bluish green
Greenish
Light green
Dark brown
Pink
Light pink, lesh colour or earthy colour
White
Ammonical smell
Vinegar like smell
Smell like that of rotten eggs
(i) Heavy
(ii) Light luffy powder
Salt absorbs moisture and
becomes paste like

Cu²⁺or Ni²⁺

Ni²⁺
Fe ²⁺
Fe ³⁺

Co²⁺

Mn²⁺
Shows the absence of

Cu²⁺, Ni²⁺, Fe²⁺, Fe ³⁺,

Mn²⁺, Co²⁺
NH₄⁺
-
CH₃COO
-
S²

Salt of Pb ²⁺ or Ba²⁺
Carbonate
(i) If coloured, may be
Cu(NO₃)₂ , FeCl₃
(ii) If colourless, may be
Zn(NO₃)₂ , chlorides of
Zn²⁺, Mg²⁺ etc.
Take a pinch of the
salt between your
?ingers and rub with
a drop of water

4. Take a small quantity of the salt in a test-tube and add 1-2 ml of dilute sulphuric acid.
Identify the gas and draw inferences from Table
DILUTE SULPHURIC ACID TEST
Table : Dilute Sulphuric Acid Test
Inference
Gas Radical
Observations
1. Colourless, odourless gas with brisk effervescence,
turns lime water milky.
2. Colourless gas, pungent smell, turns acidiied
potassium dichromate paper or solution green.
3. Colourless gas, with smell, like that of rotten eggs,
turns lead acetate paper black.
4. Reddish brown gas, punget smell, turns ferrous
sulphate solution black.
5. No gas is evolved.
CO₂
SO₂
H₂S
NO₂
-------
-
CO₃²
-
SO₃²
-
S²
-
NO₂
- - -
CO₃², SO₃², S²
-
NO₂ absent
Note :
1. Do not treat the salt with a large quantity of dilute acid.
2. Do not heat the salt with dilute acid.

5. This test is performed by treating small quantity of salt with conc. sulphuric acid (2-3 ml) in a
test tube. Identify the gas evolved in cold and then on heating. Draw inferences from table.
CONCENTRATED SULPHURIC ACID TEST
Table : Conc. Sulphuric Acid Test
Inference
Gas Radical
Observations
1. Colourless, gas with pungent smell, white fumes with aqueous
ammonia (NH₄OH), white ppt. with AgNO₃ solution.
2. Reddish brown vapours with pungent smell, turns starch paper
yellow. It does not turn FeSO₄ solution black.
3. Deep violet vapours with pungent smell, turns starch paper blue.
A sublimate is formed on the sides of the tube.

4. Reddish brown gas with pungent smell, turns FeSO₄ solution black.

5. Colourless vapours, vinegar smell, turns blue litmus red.
6. A colourless gas which turns lime water milky and also a gas which
burns with pale - bluish lame
7. No gas/vapours evolved.

HCl
Br₂
I₂ vapours
NO₂
CH₃COOH
vapours.
CO₂ + CO
--------
-
Cl
-
Br
-
I
- -- -
Cl,Br I , NO₃,
-
CH₃CHOO absent
-
C₂O₄²
-
NO₃
-
CH₃COO
1. Do not boil the salt with conc. sulphuric acid. On boiling the acid may decompose to give SO₂ gas.
2. Nitrates give vapours of nitric acid (colourless) when heated with conc. sulphuric acid. When a paper pellet or
copper chips is added. dense brown fumes evolve. Paper pellet acts as a reducing agent and reduces nitric
acid to NO₂ (Reddish brown gas.)
12.9.
Note:

6. The following table will help the students in the choice of a suitable solvent :
12.9.
QUALITATIVE ANALYSIS
Solvent
1. Cold water
2. Hot water
3. Dil. HCl
Salts which dissolve
+ + +
(a) All NH₄ , Na and K salts.
(b) All nitrites, nitrates and acetates.
(c) Most of the sulphates except that those of Pb, Ba, Ca, Sr.
(d) All chlorides except that of lead.
Lead chloride, lead nitrate.
All carbonates which do not dissolve in water i.e.,
Carbonates of Ca, Ba, Sr, Mg, Zn, Al, Cu, Ni, Mn, Fe etc.
but not of Pb.
The separation of cations into various groups by making use of suitable reagents (known as a group reagents) is based on the
differences in chemical properties of cations. For example, if hydrochloric acid is added to a solution containing all cations,
only the chlorides of lead, silver and mercury (ous) will precipitate, since all other chlorides are soluble. Thus, these cations
form a group of ions which may be precipitated from solution by addition of group reagent HCl. Similarly, H₂S is a group
reagent for group II. The following Table clearly shows the group reagents for different groups and the form in which cations
of the particular group are precipitated out.
Group Group reagent Cations
Form in which cations
are precipitated
Group Zero No
Group I
Group II
Group III
Group IV
Group V
Group VI
Dilute HCl
H₂S in the presence of dilute HCl
NH₄OH in the presence of NH₄Cl
H₂S in the presence of NH₄OH
(NH₄)₂CO₃ in the presence of NH₄OH
No
-----
Chlorides
Sulphides
Hydroxides
Sulphides
NH₄⁺
Pb ²⁺
Mg ²⁺

Pb²⁺

Cu²⁺, As ³⁺

Fe³⁺, Al ³⁺

Ni ²⁺, Mn ²⁺, Zn²⁺

Co²⁺

Ca²⁺, Ba ²⁺, Sr²⁺ Carbonates
-----