Salt Analysis

(1)

SALT ANALYSIS

1)ORGANIC

2)INORGANIC

Subpages (2): INORGANICORGANIC INORGANIC

Aim: - To identify the given inorganic compound for its acidic

and basic radical.

Apparatus: - Chemical Reagent, Test Tube, Test Tube holder,

Spatula, Burner

Procedure:- ( Click On The Required Radical to see the

procedure )

Acidic

Radical:-Group A:-

CO

₃2-

,

S

2-

,

SO

₃2-

,

NO

₂-

,

CrO

4

2-Group B:-

Cl

-

,

Br

-

,

I

-

,

NO

3-

,

CH

3

COO

-

,

C

2

O

4

2-Group C:-

SO

42-

,

PO

4

3-Basic

Radical:-Group 0:-

NH

4+

(2)

Group 1:-

Pb

2+

,

Ag

+

Group 2:-

Pb

2+

,

Cu

2+

,

As

+

Group 3:-

Fe

3+

,

Al

3+

Group 4:-

Mn

2+

,

Zn

2+

,

Ni

2+

,

Co

2+

Group 5:-

Ca

2+

,

Ba

2+

,

Sr

2+

Group 6:-

Mg

2+

Result:- The given salt contains ________ as acidic

radical and ________ as basic radical.

Subpages (29): View All

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Experiment Observation Inference Added dilute sulphuric

acid to given salt.

Gas with brisk

effervescence evolved.

Carbonate may be present.

Confirmatory Test:-

Experiment Observation Inference

Pass the above evolved gas through lime water.

Lime water turns milky. Carbonate confirmed.

Chemical Equations:- Ionic equation:-CO3 2-(s) + 2H + (aq) -->H2O(l) + CO2(g)

CO2(g) + Ca(OH)2(aq)  CaCO3(s)(milky) + H2O(l)

Preliminary Test:-

Added dilute sulphuric acid to given salt.

Gas with smell of rotten eggs evolved.

Sulphide may be present.

Added a few drops lead(II) of ethanoate solution.

Black precipitate of lead sulphide formed.

(4)

Chemical Equations:- Ionic equation:-MS(s) + 2H + (aq)  M 2+ (aq) + H2S(g Pb2+(aq) + S 2-(aq)--> PbS(s)

Gas with smell of burning sulphur evolved.

Sulphite may be present.

Add barium chloride to the salt.

A white ppt. of barium sulphite formed which dissolved in excess hydrochloric acid to give a clear colourless solution. Sulphite confirmed. Chemical Equations:- Ionic equation:-Ba2+(aq) + SO3 2-(aq) --> BaSO3(s)

(5)

Reddish brown gas with pungent smell evolved.

Nitrite may be present.

Added potassium permanganate solution. Pink colour of potassium permanganate discharged. Nitrite confirmed. Chemical Equations:- Ionic equation:-NO2- + H2SO4(aq) _ NO(g) + SO42- + H2O(l)

2KMnO4(Pink) + 3H2SO4 + 5KNO2 --> K2SO4(Colourless) + 2MnSO4 + 5KNO3 + 3H2O

(6)

acid to given salt.

Added barium chloride solution. Yellow precipitate formed. Chromate confirmed. Chemical Equations:- Ionic equation:-CrO4 2-(aq) + 2H + (aq)  Cr2O7 2-(aq)(yellow)

Ba2+(aq) + CrO42-(aq)  BaCrO4(s)(yellow)

No effect. Carbonate, sulphide , sulphite, nitrate absent. Added concentrated sulphuric

acid to given salt.

Colourless gas with pungent smell evolved.

Chloride may be present.

Added few potassium dichromate crystals and concentrated sulphuric acid and heated. Passed the vapors through the test tube which

Yellow coloured precipitate is formed.

(7)

contains sodium hydroxide solution. To this yellow solution, added dilute CH3COOH and lead

acetate solution.

Chemical Equations:-

K2Cr2O7 + 4NaCl + 6H2SO4 ————→ 2KHSO4 + 4NaHSO3 + 2CrO2Cl2

chromyl chloride

(orange-red vapours)

No effect. Carbonate, sulphide , sulphite, nitrate absent. Added concentrated

sulphuric acid to given salt.

Brown colour gas evolved.

Nitrate or Bromide may be present.

Added copper turnings. No effect. Bromide may be present.

Added dilute nitric acid and silver nitrate solution

A pale yellow precipitate formed.

(8)

Ionic equation:-Ag+(aq) + Br

-(aq) AgBr(s)(yellow)

Violet colour gas evolved. Iodide may be present.

Added dilute nitric acid and silver nitrate solution

A pale yellow precipitate formed. Iodide confirmed. Chemical Equations:- Ionic equation:-Ag+(aq) + I

-(aq)  AgI(s)(yellow)

(9)

NITRATE

Brown colour gas evolved.

Nitrate or Bromide may be present.

Added copper turnings. Brown colour intensifies. Nitrate may be present.

Added fresh ferrous sulphate, nitric acid to salt. Added concentrated sulphuric acid alsong the walls of test tube.

Brown coloured ring is formed.

Nitrate confirmed.

Ionic

equation:-NO3- + 3Fe2+ + 4H+ → 3Fe3+ + NO + 2H2O

[Fe(H2O)6]2+ + NO → [Fe(H2O)5(NO)]2+

(10)

Vinegar like smell. Acetate may be present.

Added ethanol to the salt, then added drops of concentrated sulphuric acid.

Evolution of fruity smell. Acetate confirmed.

Ionic

equation:-CH3COOH- + H2SO4 --> HSO4- + CH3COOH

Colourless gas with brisk effervescence evolved.

Oxalate may be present.

(11)

Experiment Observation Inference Passed the above evolved

gas through lime water .

Lime water turned milky. Oxalate confirmed.

C2O42- + H2SO4(aq)  CO(g) + CO2(g) + H2O(l) + SO4

2-CO2(g) + Ca(OH)2(aq) CaCO3(s)(milky) + H2O(l)

sulphuric acid to given salt. No effect. Nitrate,Bromide, Chloride,Acetate, absent. Sulphate or phosphate may be present. Confirmatory Test:-

Added barium chloride solution.

White coloured precipitate is formed.

Sulphate confirmed.

(12)

Ionic equation:-Ba2+(aq) + SO4

2-(aq) ==> BaSO4(s)(white)

sulphuric acid to given salt. No effect. Nitrate,Bromide, Chloride,Acetate, absent. Sulphate or phosphate may be present. Confirmatory Test:-

Added soda extract1 and dilute nitric acid and then added Ammonium Molybdate solution. A canary yellow precipitate formed. Phosphate confirmed. Chemical Equations:-

(NH4)2(NO3)+2Na2(PO4) --> 2(NH4)(PO4)+2Na2(NO3)

(13)

Experiment Observation Inference Smelled the salt. Ammonical smell. Ammonium may be

present.

Added sodium

hydroxide solution to the salt.

Ammonical smelling gas evolved. Ammonium confirmed. Chemical Equations:- Ionic equation:-NH4 + (aq) + OH -(aq)  NH3(g) + H2O(l)

Smelled the salt. No Ammonical smell. Ammonium absent. Added dilute hydrochloric

acid to original solution.

Lead(II) may be present.

Added potassium iodide. Yellow coloured precipitate formed.

(14)

Ionic

equation:-Pb2+(aq) + HCl(aq)  PbCl2(White)

Pb2+(aq) +2I-(aq) PbI2(s)(Yellow)

Lead(II), Ag(I) may be present.

Added precipitate in hot water.

No effect. Ag(I) may be present.

Added potassium chromate to original solution.

Brick red coloured precipitate formed.

Ag(I) confirmed.

Ionic

equation:-Ag+ + HCl(aq) --> AgCl(s)(white) + H +

(15)

No Effect. Lead(II)may be present.

Added hydrogen

disulphide, hydrochloric acid to original solution.

Black coloured precipitate formed.

Lead(II)may be present.

Added potassium iodide to original solution. Yellow coloured precipitate formed. Lead(II) confirmed. Chemical Equations:- Ionic equation:-Pb2+ + HCl(aq) --> PbCl2(l) + 2H+

Pb2+ + KI(aq) PbI2(s)(yellow) + 2K+

(16)

Added dilute hydrochloric acid to original solution.

Added hydrogen

Cu(II) ,Pb(II),As(III) may be present.

Added sodium hydroxide to original solution.

Blue coloured precipitate formed.

Cu(II) may be present.

Added ammonium hydroxide to original solution.

Blue coloured precipitate formed. Cu(II) confirmed. Chemical Equations:- Ionic equation:-Cu2+(aq) + 2OH

-(aq) --> Cu(OH)2(s)(blue)

Cu(OH)2(s) + 4NH3(aq) --> [Cu(NH3)4] 2+

(aq)(blue) + 2OH

-(aq)

Added hydrogen

disulphide, hydrochloric

Yellow coloured precipitate formed.

(17)

Added dilute

hydrochloric acid to above solution. Yellow coloured precipitate formed. As(III) confirmed. Chemical Equations:- Ionic

equation:-2As3+ + 3H2S(g) As2S3(s)(yellow) + 6H+

2As2S3(s)(yellow) + 12HCl(l) 4AsCl3(s)(yellow) + 6H2S

Added hydrogen

No Effect. Pb(II), Cu(II) , As(III) absent.

Added dilute hydrochloric acid, concentrated nitric acid and boiled solution. Then cooled it and added solid ammonium

Reddish Brown precipitate formed.

(18)

hydroxide.

Dissolved the precipitate formed with hydrochloric . Added potassium

sulphocyanide.

Blood red colouration. Fe (III) confirmed.

Ionic equation:-Fe3+(aq) + 3OH

-(aq) Fe(OH)3(s)(Reddish Brown)

Fe3+(aq) +3HCl(l) FeCl3(aq) + 3H2O(aq)

FeCl3(aq) + 6KCNS(aq) K3[Fe(CNS)6](Blood Red) + 3KCl(aq)

Added hydrogen

Added dilute hydrochloric acid, concentrated nitric acid and boiled solution. Then cooled it and added

Gelatinous white precipitate formed.

(19)

solid ammonium hydroxide.

Dissolved the precipitate formed with hydrochloric acid and added drops of blue litmus. Then added ammonium hydroxide till alkaline.

Blue coloured precipitate floated on surface . Al(III) confirmed. Chemical Equations:- Ionic equation:-Al3+(aq) + 3OH

-(aq) Al(OH)3(s)(white)(adsorb blue colour)

Al3+(aq) +3HCl(l) AlCl3(aq) + 3H2O(aq)

Added hydrogen

Added dilute hydrochloric acid, concentrated nitric acid and boiled solution.

(20)

Then cooled it and added solid ammonium

hydroxide.

Passed Hydrogen disulphide gas through above formed solution.

Flesh(buff) coloured precipitate formed.

Mn (II) may be present.

Added lead dioxide to above solution, then added concentrated nitric acid. Boiled it.

Pink Colouration formed. Mn (II) Confirmed.

Ionic

equation:-Mn 2++ H2S(aq) MnS(s)(Flesh) + 2H+

MnS(aq) + 2HCl(aq) MnCl2 + 2H+ + S

2-2Mn 2+ + 4H+ + 5PbO2(s) 2MnO4-(aq) + 5Pb2+(aq) + 2H2O(aq)

(21)

Added hydrogen

hydroxide.

No Effect. Al(III) ,Fe(III) absent.

White coloured precipitate formed.

Zn (II) may be present.

Dissolved the precipitate in concentrated

hydrochloric acid and boiled it.Added potassium ferrocyanide to it

Bluish white coloured precipitate formed. Zn (II) Confirmed. Chemical Equations:- Ionic equation:-Zn 2++ H2S(aq) ZnS(s)(White) + 2H+ ZnS(aq) + 2HCl(aq) ZnCl2 + 2H+ + S

2-2Zn 2+ + K4[Fe(CN)6] Zn2[Fe(CN)6](Bluish White) + 4K+

(22)

NICKEL

Added hydrogen

hydroxide.

Co(II) or Ni(II) may be present.

Dissolved the precipitate in aqua regia.Evaporated residue.

Yellow coloured residue remained.

Ni(II) may be present.

Dissolved the yellow residue in water. Added ammonium hydroxide till alkaline then added dimethylglyxoglime solution.

Bright red precipitate formed.

Ni(II) confirmed.

(23)

Ionic

equation:-Ni2++ H2S(aq) NiS(s)(black) + 2H+

NiS(s)(black) + 2HCl(aq) + [O] NiCl2(aq) + H2O(l) + S

Added hydrogen

hydroxide.

Co(II) or Ni(II) may be present.

Dissolved the precipitate in aqua regia.Evaporated residue.

Blue coloured residue remained.

Co(II) may be present.

Dissolved the blue residue in water.Added

Blue coloured layer floated on surface .

(24)

ammonium sulphocyanide to it.

Ionic

equation:-Co2++ H2S(aq) CoS(s)(black) + 2H+

CoS(s)(black) + 2HCl(aq) + [O] CoCl2(aq) + H2O(l) + S

Co2+ + 4KCNS K2[Co(CNS)4](blue colouration) + 2K+

Added hydrogen

hydroxide.

No Effect. Zn (II) ,Mn(II), Ni(II), Co(II) absent. Added ammonium carbonate to above solution. White precipitate is formed.

Ba(II), Sr(II), Ca(II) may be present.

(25)

Dissolved precipitate in acetic acid and boiled it. Added few drops of ammonium oxalate to above solution and then added ammonium hydroxide. White precipitate is formed. Ca(II) Confirmed. Chemical Equations:- Ionic

equation:-Ca2+ + (NH4)2CO3 (aq) CaCO3(s)(white) + 2NH4+(aq)

CaCO3(s) + 2CH3COOH (aq) (CH3COO)2Ca + CO2(g) + H2O(l)

Ca2+(aq) + (NH4)2C2O4(aq) CaC2O4(s)(white) + 2NH4+(aq)

No Effect. Lead(II)may be present. Added hydrogen disulphide,

hydrochloric acid to original solution.

Added dilute hydrochloric acid, concentrated nitric acid and boiled solution. Then cooled it and added solid ammonium hydroxide.

No Effect. Zn (II) ,Mn(II), Ni(II), Co(II) absent.

(26)

to above solution. present.

Dissolved precipitate in acetic acid and boiled it.Added few drops of

potassium chromate to above solution.

Yellow precipitate is formed. Ba (II) Confirmed.

Ionic

equation:-Ba2+ + (NH4)2CO3 (aq) BaCO3(s)(white) + 2NH4+(aq)

BaCO3(s) + 2CH3COOH (aq) (CH3COO)2Ba + CO2(g) + H2O(l)

Ba2+(aq) + K2CrO4(aq) BaCrO4(s)(yellow) + 2K+

Added hydrogen

(27)

hydroxide.

No Effect. Zn (II) ,Mn(II), Ni(II), Co(II) absent. Added ammonium carbonate to above solution. White precipitate is formed.

Ba(II), Sr(II), Ca(II) may be present.

Dissolved precipitate in acetic acid and boiled it. Added few drops of ammonium sulphate to above solution and then added ammonium hydroxide. White precipitate is formed. Sr(II) Confirmed. Chemical Equations:- Ionic

equation:-Sr2+ + (NH4)2CO3 (aq) SrCO3(s)(white) + 2NH4+(aq)

SrCO3(s) + 2CH3COOH (aq) (CH3COO)2Sr + CO2(g) + H2O(l)

Sr2+(aq) + (NH4)2SO4(aq) SrSO4(s)(white) + 2NH4+(aq)

(28)

No Effect. Lead(II)may be present. Added hydrogen disulphide,

hydrochloric acid to original solution.

Added dilute hydrochloric acid, concentrated nitric acid and boiled solution. Then cooled it and added solid ammonium hydroxide.

No Effect. Zn (II) ,Mn(II), Ni(II), Co(II) absent.

Added ammonium carbonate to above solution.

No Effect. Mg (II) may be present.

Added ammonium chloride, ammonium hydroxide and disodium hydrogen phosphate to original solution.

White precipitate is formed. Mg(II) Confirmed.

Ionic

equation:-Mg2+ + HPO42-(aq) + NH4+(aq) Mg(NH4)PO4(white) + H+

(29)

2) ALDEHYDE

3) AMINE

4) CARBOXYLIC ACID

5) KETONE

6) PHENOL

Subpages (6): ALCOHOLALDEHYDEAMINECARBOXYLIC ACIDKETONEPHENOL

Added bromine water to solution

No Effect

Or

Pink colour of Bromine water changed to colourless. Compound is saturated. Or Compound is unsaturated. Confirmatory Test:-

Warmed with acetic acid and a few drops of concentrated sulphuric acid.

(30)

R3C-CR3 + Br2 No Effect

OR

R2C=CR2 + Br2  BrR2C-CR2Br

CH3COOH + ROH CH3COOR + H2O

No Effect

Or

Pink colour of Bromine water changed to colourless.

Compound is saturated.

Or

Compound is unsaturated.

Added drop of blue Litmus to solution.

No Effect. Carboxylic Acid and Phenol absent.

Added a few drops 2,4-dinitrophenylhydrazine to the solution.

Yellowish -orange precipitate formed.

Aldehyde or ketone may be present.

(31)

Added a few drops of Fehling's solution A & B.

Formation Of red colour. Aldehyde confirmed.

OR

R2C=CR2 + Br2  BrR2C-CR2Br

R-CHO + (NO2)2C6H3NHNH2  (NO2)2C6H3NHN=CRH(Yellowish Orange) +

H2O

RCHO + 2Cu2+ + 2H2O RCOOH + Cu2O(Red) + 4H+

AIM: To test the presence of amino group in the given organic compound.

PROCEDURE:

S.No EXPERIMENT OBSERVATION INFERENCE

1 LITMUS TEST

Organic compound + few drops of red litmus solution.

Red litmus turns blue

Amino group present.

(32)

2 SOLUBILITY TEST

Organic compound + 1-2 ml of dil.HCl. Shake well.

Organic compound dissolves. Amino group present 3 CARBYLAMINE TEST Organic compound + CHCl3 + Alc.KOH. Heat An obnoxious smell is obtained. Primary amine present.

4 AZO DYE TEST

Dissolve organic compound in dil.HCl and cool in ice. Add ice cold NaNO2 solution to it. Mix

well. Add ice cold solution of β- naphthol + NaOH. A red or orange dye is obtained. Primary aromatic amino group present.

EQUATIONS: (ON BLANK SIDE USING A PENCIL)

1. R-NH2 + HCl → R- NH3+Cl-

amine amine salt

1. R-NH2 + CHCl3 + 3KOH → R- N≡ C + 3KCl + 3H2O

Isocyanide

or

carbylamine

(33)

ArNH2 + HNO2 + HCl → Ar- N +_{≡ N}

-Cl + 2H2O

Aromatic Aryldiazonium chloride

10amine (stable between 0- 50C)

β- naphthol (draw structure) + Ar- N+_{≡ N}-_{Cl → (draw structure of the azo dye}

obtained) + NaCl + H2O

RESULT: : (ON RULED SIDE ) Amino present in the given organic compound.

No Effect

Or

Pink colour of Bromine water changed to colourless.

Compound is saturated.

Or

Compound is unsaturated.

Added drop of blue Litmus to solution.

Solution turned Red. Carboxylic Acid may be present.

Added sodium

bicarbonate to solution.

Gas with brisk

effervescence evolved.

Carboxylic acid confirmed.

(34)

OR

R2C=CR2 + Br2 BrR2C-CR2Br

RCOOH + NaHCO3 RCOONa + H2O + CO2