Salt Analysis

SALT ANALYSIS

1)ORGANIC 2)INORGANIC Subpages (2): INORGANIC ORGANIC

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:- CO32-, S2-, SO32-, NO2-,CrO42Group B:- Cl-, Br-, I-, NO3-, CH3COO-, C2O42Group C:- SO42-, PO43-

Basic Radical:Group 0:- NH4+

Group 1:- Pb2+ , Ag+ Group 2:- Pb2+, Cu2+, As+ Group 3:- Fe3+, Al3+ Group 4:- Mn2+, Zn2+, Ni2+, Co2+ Group 5:- Ca2+, Ba2+, Sr2+ Group 6:- Mg2+

Result:- The given salt contains ________ as acidic radical and ________ as basic radical.

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CARBONATE Preliminary Test:-

Experiment Added dilute sulphuric acid to given salt.

Observation Gas with brisk effervescence evolved.

Inference Carbonate may be present.

Observation Lime water turns milky.

Inference Carbonate confirmed.

Confirmatory Test:Experiment Pass the above evolved gas through lime water.

Chemical Equations:Ionic equation:CO32-(s) + 2H+(aq) -->H2O(l) + CO2(g) CO2(g) + Ca(OH)2(aq)  CaCO3(s)(milky) + H2O(l)

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SULPHIDE Preliminary Test:Experiment Added dilute sulphuric acid to given salt.

Observation Gas with smell of rotten eggs evolved.

Inference Sulphide may be present.

Confirmatory Test:Experiment Added a few drops lead(II) of ethanoate solution.

Observation Inference Black precipitate of lead Sulphide confirmed. sulphide formed.

Chemical Equations:Ionic equation:MS(s) + 2H+(aq)  M2+(aq) + H2S(g

Pb2+(aq) + S2-(aq)--> PbS(s) Sign in|Recent Site Activity|Report Abuse|Print Page|Remove Access|Powered By Google Site

SULPHITE Preliminary Test:Experiment Added dilute sulphuric acid to given salt.

Observation Gas with smell of burning sulphur evolved.

Inference Sulphite may be present.

Observation A white ppt. of barium sulphite formed which dissolved in excess hydrochloric acid to give a clear colourless solution.

Inference Sulphite confirmed.

Confirmatory Test:Experiment Add barium chloride to the salt.

Chemical Equations:Ionic equation:Ba2+(aq) + SO32-(aq) --> BaSO3(s)

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NITRITE Preliminary Test:Experiment Added dilute sulphuric acid to given salt.

Observation Reddish brown gas with pungent smell evolved.

Inference Nitrite may be present.

Observation Pink colour of potassium permanganate discharged.

Inference Nitrite confirmed.

Confirmatory Test:Experiment Added potassium permanganate solution.

Chemical Equations:Ionic equation:NO2- + H2SO4(aq)



NO(g) + SO42- + H2O(l)

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

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CHROMATE Preliminary Test:Experiment Added dilute sulphuric

Observation Solution turned yellow.

Inference Chromate may be present.

acid to given salt.

Confirmatory Test:Experiment Added barium chloride solution.

Observation Yellow precipitate formed.

Inference Chromate confirmed.

Chemical Equations:Ionic equation:CrO42-(aq) + 2H+(aq)  Cr2O72-(aq)(yellow) Ba2+(aq) + CrO42-(aq)  BaCrO4(s)(yellow) Sign in|Recent Site Activity|Report Abuse|Print Page|Remove Access|Powered By Google Sites

CHLORIDE Preliminary Test:Experiment Added dilute sulphuric acid to given salt.

Observation No effect.

Added concentrated sulphuric Colourless gas with pungent acid to given salt. smell evolved.

Inference Carbonate, sulphide , sulphite, nitrate absent. Chloride may be present.

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

Observation Yellow coloured precipitate is formed.

Inference Chloride confirmed.

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)

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BROMIDE Preliminary Test:Experiment Added dilute sulphuric acid to given salt. Added concentrated sulphuric acid to given salt. Added copper turnings.

Observation No effect. Brown colour gas evolved.

Inference Carbonate, sulphide , sulphite, nitrate absent. Nitrate or Bromide may be present.

No effect.

Bromide may be present.

Observation A pale yellow precipitate formed.

Inference Bromide confirmed.

Confirmatory Test:Experiment Added dilute nitric acid and silver nitrate solution

Chemical Equations:Ionic equation:Ag+(aq) + Br-(aq) AgBr(s)(yellow) Sign in|Recent Site Activity|Report Abuse|Print Page|Remove Access|Powered By Google Sites

ODIDE Preliminary Test:Experiment Added dilute sulphuric acid to given salt. Added concentrated sulphuric acid to given salt.

Observation No effect.

Inference Carbonate, sulphide , sulphite, nitrate absent. Violet colour gas evolved. Iodide may be present.

Confirmatory Test:Experiment Added dilute nitric acid and silver nitrate solution

Observation A pale yellow precipitate formed.

Inference Iodide confirmed.

Chemical Equations:Ionic equation:Ag+(aq) + I-(aq)  AgI(s)(yellow) Sign in|Recent Site Activity|Report Abuse|Print Page|Remove Access|Powered By Google Sites

NITRATE Preliminary Test:Experiment Added dilute sulphuric acid to given salt. Added concentrated sulphuric acid to given salt. Added copper turnings.

Observation No effect. Brown colour gas evolved.

Inference Carbonate, sulphide , sulphite, nitrate absent. Nitrate or Bromide may be present.

Brown colour intensifies.

Nitrate may be present.

Observation Brown coloured ring is formed.

Inference Nitrate confirmed.

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

Chemical Equations:Ionic equation:NO3- + 3Fe2+ + 4H+ → 3Fe3+ + NO + 2H2O [Fe(H2O)6]2+ + NO → [Fe(H2O)5(NO)]2+

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ACETATE Preliminary Test:Experiment

Observation

Inference

Added dilute sulphuric acid to given salt. Added concentrated sulphuric acid to given salt.

No effect. Vinegar like smell.

Carbonate, sulphide , sulphite, nitrate absent. Acetate may be present.

Observation Evolution of fruity smell.

Inference Acetate confirmed.

Confirmatory Test:Experiment Added ethanol to the salt, then added drops of concentrated sulphuric acid.

Chemical Equations:Ionic equation:CH3COOH- + H2SO4 --> HSO4- + CH3COOH Sign in|Recent Site Activity|Report Abuse|Print Page|Remove Access|Powered By Google Sites

OXALATE Preliminary Test:Experiment Added dilute sulphuric acid to given salt. Added concentrated sulphuric acid to given salt.

Confirmatory Test:-

Observation No effect. Colourless gas with brisk effervescence evolved.

Inference Carbonate, sulphide , sulphite, nitrate absent. Oxalate may be present.

Experiment Passed the above evolved gas through lime water .

Observation Lime water turned milky.

Inference Oxalate confirmed.

Chemical Equations:C2O42- + H2SO4(aq)  CO(g) + CO2(g) + H2O(l) + SO42CO2(g) + Ca(OH)2(aq) CaCO3(s)(milky) + H2O(l)

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SULPHATE Preliminary Test:Experiment Added dilute sulphuric acid to given salt. Added concentrated sulphuric acid to given salt.

Observation No effect. No effect.

Inference Carbonate, sulphide , sulphite, nitrate absent. Nitrate,Bromide, Chloride,Acetate, absent. Sulphate or phosphate may be present.

Confirmatory Test:Experiment Added barium chloride solution.

Chemical Equations:-

Observation Inference White coloured precipitate Sulphate confirmed. is formed.

Ionic equation:Ba2+(aq) + SO42-(aq) ==> BaSO4(s)(white) Sign in|Recent Site Activity|Report Abuse|Print Page|Remove Access|Powered By Google Sites

PHOSPHATE Preliminary Test:Experiment Added dilute sulphuric acid to given salt. Added concentrated sulphuric acid to given salt.

Observation No effect. No effect.

Inference Carbonate, sulphide , sulphite, nitrate absent. Nitrate,Bromide, Chloride,Acetate, absent. Sulphate or phosphate may be present.

Confirmatory Test:Experiment Added soda extract1 and

Observation A canary yellow precipitate formed.

Inference Phosphate confirmed.

dilute nitric acid and then added Ammonium Molybdate solution.

Chemical Equations:(NH4)2(NO3)+2Na2(PO4) --> 2(NH4)(PO4)+2Na2(NO3) Sign in|Recent Site Activity|Report Abuse|Print Page|Remove Access|Powered By Google Sites

AMMONIUM Preliminary Test:-

Experiment Smelled the salt.

Observation Ammonical smell.

Inference Ammonium may be present.

Observation Ammonical smelling gas evolved.

Inference Ammonium confirmed.

Confirmatory Test:Experiment Added sodium hydroxide solution to the salt.

Chemical Equations:Ionic equation:NH4+(aq) + OH-(aq)  NH3(g) + H2O(l) Sign in|Recent Site Activity|Report Abuse|Print Page|Remove Access|Powered By Google Sites

LEAD1 Preliminary Test:Experiment Observation Inference Smelled the salt. No Ammonical smell. Ammonium absent. Added dilute hydrochloric White coloured precipitate Lead(II) may be present. acid to original solution. is formed.

Confirmatory Test:Experiment Added potassium iodide.

Observation Yellow coloured precipitate formed.

Inference Lead(II) confirmed.

Chemical Equations:Ionic equation:Pb2+(aq) + HCl(aq)  PbCl2(White) Pb2+(aq) +2I-(aq) PbI2(s)(Yellow) Sign in|Recent Site Activity|Report Abuse|Print Page|Remove Access|Powered By Google Sites

SILVER Preliminary Test:Experiment Smelled the salt. Added dilute hydrochloric acid to original solution. Added precipitate in hot water.

Observation No Ammonical smell. White coloured precipitate is formed. No effect.

Inference Ammonium absent. Lead(II), Ag(I) may be present. Ag(I) may be present.

Observation Brick red coloured precipitate formed.

Inference Ag(I) confirmed.

Confirmatory Test:Experiment Added potassium chromate to original solution.

Chemical Equations:Ionic equation:Ag+ + HCl(aq) --> AgCl(s)(white) + H+ 2AgCl(s)(white) + K2CrO4 Ag2CrO4(s)(yellow) + 2KCl(aq)

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LEAD2 Preliminary Test:Experiment Smelled the salt. Added dilute hydrochloric acid to original solution. Added hydrogen disulphide, hydrochloric acid to original solution.

Observation No Ammonical smell. No Effect.

Inference Ammonium absent. Lead(II)may be present.

Black coloured precipitate Lead(II)may be present. formed.

Confirmatory Test:Experiment Added potassium iodide to original solution.

Observation Yellow coloured precipitate formed.

Inference Lead(II) confirmed.

Chemical Equations:Ionic equation:Pb2+ + HCl(aq) --> PbCl2(l) + 2H+

Pb2+ + KI(aq) PbI2(s)(yellow) + 2K+ Sign in|Recent Site Activity|Report Abuse|Print Page|Remove Access|Powered By Google Sites

COPPER Preliminary Test:Experiment Smelled the salt.

Observation No Ammonical smell.

Inference Ammonium absent.

Added dilute hydrochloric acid to original solution. Added hydrogen disulphide, hydrochloric acid to original solution. Added sodium hydroxide to original solution.

No Effect.

Lead(II)may be present.

Black coloured precipitate Cu(II) ,Pb(II),As(III) may formed. be present. Blue coloured precipitate formed.

Cu(II) may be present.

Observation Blue coloured precipitate formed.

Inference Cu(II) confirmed.

Confirmatory Test:Experiment Added ammonium hydroxide to original solution.

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)

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ARSENIC Preliminary Test:Experiment Smelled the salt. Added dilute hydrochloric acid to original solution. Added hydrogen disulphide, hydrochloric

Observation No Ammonical smell. No Effect.

Inference Ammonium absent. Lead(II)may be present.

Yellow coloured precipitate formed.

As(III) may be present.

acid to original solution.

Confirmatory Test:Experiment Observation Added dilute Yellow coloured hydrochloric acid to above precipitate formed. solution.

Inference As(III) confirmed.

Chemical Equations:Ionic equation:2As3+ + 3H2S(g) As2S3(s)(yellow) + 6H+ 2As2S3(s)(yellow) + 12HCl(l) 4AsCl3(s)(yellow) + 6H2S

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IRON Preliminary Test:Experiment Smelled the salt. Added dilute hydrochloric acid to original solution. 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

Observation No Ammonical smell. No Effect.

Inference Ammonium absent. Lead(II)may be present.

No Effect.

Pb(II), Cu(II) , As(III) absent.

Reddish Brown precipitate formed.

Fe(III) may be present.

hydroxide.

Confirmatory Test:Experiment Dissolved the precipitate formed with hydrochloric . Added potassium sulphocyanide.

Observation Blood red colouration.

Inference Fe (III) confirmed.

Chemical Equations: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) Sign in|Recent Site Activity|Report Abuse|Print Page|Remove Access|Powered By Google Sites

ALUMINIUM Preliminary Test:Experiment Smelled the salt. Added dilute hydrochloric acid to original solution. Added hydrogen disulphide, hydrochloric acid to original solution. Added dilute hydrochloric acid, concentrated nitric acid and boiled solution. Then cooled it and added

Observation No Ammonical smell. No Effect.

Inference Ammonium absent. Lead(II)may be present.

No Effect.

Pb(II), Cu(II) , As(III) absent.

Gelatinous white precipitate formed.

Al(III) may be present.

solid ammonium hydroxide.

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

Observation Blue coloured precipitate floated on surface .

Inference 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) Sign in|Recent Site Activity|Report Abuse|Print Page|Remove Access|Powered By Google Site

Preliminary Test:Experiment Smelled the salt. Added dilute hydrochloric acid to original solution. Added hydrogen disulphide, hydrochloric acid to original solution. Added dilute hydrochloric acid, concentrated nitric acid and boiled solution.

Observation No Ammonical smell. No Effect.

Inference Ammonium absent. Lead(II)may be present.

No Effect.

Pb(II), Cu(II) , As(III) absent.

No Effect.

Al(III) ,Fe(III) absent.

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.

Observation Pink Colouration formed.

Inference Mn (II) Confirmed.

Confirmatory Test:Experiment Added lead dioxide to above solution, then added concentrated nitric acid. Boiled it.

Chemical Equations:Ionic equation:Mn 2+ + H2S(aq) MnS(s)(Flesh) + 2H+ MnS(aq) + 2HCl(aq) MnCl2 + 2H+ + S22Mn 2+ + 4H+ + 5PbO2(s) 2MnO4-(aq) + 5Pb2+(aq) + 2H2O(aq)

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ZINC Preliminary Test:Experiment Observation Smelled the salt. No Ammonical smell. Added dilute hydrochloric No Effect. acid to original solution.

Inference Ammonium absent. 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. Passed Hydrogen disulphide gas through above formed solution.

No Effect.

Pb(II), Cu(II) , As(III) absent.

No Effect.

Al(III) ,Fe(III) absent.

White coloured precipitate Zn (II) may be present. formed.

Confirmatory Test:Experiment Observation Dissolved the precipitate Bluish white coloured in concentrated precipitate formed. hydrochloric acid and boiled it.Added potassium ferrocyanide to it

Inference Zn (II) Confirmed.

Chemical Equations:Ionic equation:Zn 2+ + H2S(aq) ZnS(s)(White) + 2H+ ZnS(aq) + 2HCl(aq) ZnCl2 + 2H+ + S22Zn 2+ + K4[Fe(CN)6] Zn2[Fe(CN)6](Bluish White) + 4K+

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NICKEL Preliminary Test:Experiment Smelled the salt. Added dilute hydrochloric acid to original solution. 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. Passed Hydrogen disulphide gas through above formed solution. Dissolved the precipitate in aqua regia.Evaporated residue.

Observation No Ammonical smell. No Effect.

Inference Ammonium absent. Lead(II)may be present.

No Effect.

Pb(II), Cu(II) , As(III) absent.

No Effect.

Al(III) ,Fe(III) absent.

Black coloured precipitate Co(II) or Ni(II) may be formed. present. Yellow coloured residue remained.

Ni(II) may be present.

Observation Bright red precipitate formed.

Inference Ni(II) confirmed.

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

Chemical Equations:-

Ionic equation:Ni 2+ + H2S(aq) NiS(s)(black) + 2H+ NiS(s)(black) + 2HCl(aq) + [O] NiCl2(aq) + H2O(l) + S

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COBALT Preliminary Test:Experiment Smelled the salt. Added dilute hydrochloric acid to original solution. 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. Passed Hydrogen disulphide gas through above formed solution. Dissolved the precipitate in aqua regia.Evaporated residue.

Observation No Ammonical smell. No Effect.

Inference Ammonium absent. Lead(II)may be present.

No Effect.

Pb(II), Cu(II) , As(III) absent.

No Effect.

Al(III) ,Fe(III) absent.

Black coloured precipitate Co(II) or Ni(II) may be formed. present. Blue coloured residue remained.

Co(II) may be present.

Confirmatory Test:Experiment Observation Dissolved the blue residue Blue coloured layer in water.Added floated on surface .

Inference Co(II)confirmed.

ammonium sulphocyanide to it.

Chemical Equations: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+ Sign in|Recent Site Activity|Report Abuse|Print Page|Remove Access|Powered By Google Sites

Preliminary Test:Experiment Smelled the salt. Added dilute hydrochloric acid to original solution. 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. Passed Hydrogen disulphide gas through above formed solution. Added ammonium carbonate to above solution.

Observation No Ammonical smell. No Effect.

Inference Ammonium absent. Lead(II)may be present.

No Effect.

Pb(II), Cu(II) , As(III) absent.

No Effect.

Al(III) ,Fe(III) absent.

No Effect.

Zn (II) ,Mn(II), Ni(II), Co(II) absent.

White precipitate is formed.

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

Confirmatory Test:Experiment Dissolved precipitate in acetic acid and boiled it. Added few drops of ammonium oxalate to above solution and then added ammonium hydroxide.

Observation White precipitate is formed.

Inference 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) Sign in|Recent Site Activity|Report Abuse|Print Page|Remove Access|Powered By Google Sites reliminary Test:Experiment Smelled the salt. Added dilute hydrochloric acid to original solution. 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. Passed Hydrogen disulphide gas through above formed solution. Added ammonium carbonate

Observation No Ammonical smell. No Effect.

Inference Ammonium absent. Lead(II)may be present.

No Effect.

Pb(II), Cu(II) , As(III) absent.

No Effect.

Al(III) ,Fe(III) absent.

No Effect.

Zn (II) ,Mn(II), Ni(II), Co(II) absent.

White precipitate is formed.

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

to above solution.

present.

Confirmatory Test:Experiment Dissolved precipitate in acetic acid and boiled it.Added few drops of potassium chromate to above solution.

Observation Yellow precipitate is formed.

Inference Ba (II) Confirmed.

Chemical Equations: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+ Sign in|Recent Site Activity|Report Abuse|Print Page|Remove Access|Powered By Google Sites

STRONTIUM Preliminary Test:Experiment Smelled the salt. Added dilute hydrochloric acid to original solution. 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

Observation No Ammonical smell. No Effect.

Inference Ammonium absent. Lead(II)may be present.

No Effect.

Pb(II), Cu(II) , As(III) absent.

No Effect.

Al(III) ,Fe(III) absent.

hydroxide. Passed Hydrogen disulphide gas through above formed solution. Added ammonium carbonate to above solution.

No Effect.

Zn (II) ,Mn(II), Ni(II), Co(II) absent.

White precipitate is formed.

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

Observation White precipitate is formed.

Inference Sr(II) Confirmed.

Confirmatory Test:Experiment Dissolved precipitate in acetic acid and boiled it. Added few drops of ammonium sulphate to above solution and then added ammonium hydroxide.

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)

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MAGNESIUM Preliminary Test:Experiment

Observation

Inference

Smelled the salt. Added dilute hydrochloric acid to original solution. 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. Passed Hydrogen disulphide gas through above formed solution. Added ammonium carbonate to above solution.

No Ammonical smell. No Effect.

Ammonium absent. Lead(II)may be present.

No Effect.

Pb(II), Cu(II) , As(III) absent.

No Effect.

Al(III) ,Fe(III) absent.

No Effect.

Zn (II) ,Mn(II), Ni(II), Co(II) absent.

No Effect.

Mg (II) may be present.

Observation White precipitate is formed.

Inference Mg(II) Confirmed.

Confirmatory Test:Experiment Added ammonium chloride, ammonium hydroxide and disodium hydrogen phosphate to original solution.

Chemical Equations:Ionic equation:-

Mg2+ + HPO42-(aq) + NH4+(aq) Mg(NH4)PO4(white) + H+ Sign in|Recent Site Activity|Report Abuse|Print Page|Remove Access|Powered By Google Sites

ORGANIC

1) ALCOHOL

2) ALDEHYDE 3) AMINE 4) CARBOXYLIC ACID 5) KETONE 6) PHENOL Subpages (6): ALCOHOL ALDEHYDE AMINE CARBOXYLIC ACID KETONE PHENOL Sign in|Recent Site Activity|Report Abuse|Print Page|Remove Access|Powered By Google Sites

ALCOHOL Preliminary Test:Experiment Added bromine water to solution

Observation No Effect Or

Inference Compound is saturated. Or

Pink colour of Bromine water changed to colourless.

Compound is unsaturated.

Observation Fruity smell is formed.

Inference Alcohol confirmed.

Confirmatory Test:Experiment Warmed with acetic acid and a few drops of concentrated sulphuric acid.

Chemical Equations:R3C-CR3 + Br2 No Effect OR R2C=CR2 + Br2  BrR2C-CR2Br

CH3COOH + ROH CH3COOR + H2O

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ALDEHYDE Preliminary Test:Experiment Added bromine water to solution

Observation No Effect Or

Pink colour of Bromine water changed to colourless. Added drop of blue Litmus No Effect. to solution. Added a few drops 2,4- Yellowish -orange dinitrophenylhydrazine precipitate formed. to the solution.

Inference Compound is saturated. Or Compound is unsaturated.

Carboxylic Acid and Phenol absent. Aldehyde or ketone may be present.

Confirmatory Test:Experiment

Observation

Inference

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

Formation Of red colour.

Aldehyde confirmed.

Chemical Equations:R3C-CR3 + Br2 No Effect OR R2C=CR2 + Br2  BrR2C-CR2Br

R-CHO + (NO2)2C6H3NHNH2  (NO2)2C6H3NHN=CRH(Yellowish Orange) + H2O

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

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

PROCEDURE:

S.No 1

EXPERIMENT LITMUS TEST Organic compound + few drops of red litmus solution.

OBSERVATION Red litmus turns blue

INFERENCE Amino group present.

2

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

3

4

Organic compound dissolves.

Amino group present

An obnoxious smell is obtained.

Primary amine present.

CARBYLAMINE TEST Organic compound + CHCl3 + Alc.KOH. Heat AZO DYE TEST

Dissolve organic compound in A red or orange dil.HCl and cool in ice. Add ice dye is obtained. cold NaNO2 solution to it. Mix well. Add ice cold solution of βnaphthol + NaOH.

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 1. NaNO2 + HCl → HNO2 + NaCl

Primary aromatic amino group present.

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.

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CARBOXYLIC ACID Preliminary Test:Experiment Added bromine water to solution

Observation No Effect Or

Added drop of blue Litmus to solution.

Inference Compound is saturated. Or

Pink colour of Bromine water changed to colourless. Solution turned Red.

Compound is unsaturated.

Observation Gas with brisk effervescence evolved.

Inference Carboxylic acid confirmed.

Carboxylic Acid may be present.

Confirmatory Test:Experiment Added sodium bicarbonate to solution.

Chemical Equations:R3C-CR3 + Br2 No Effect OR R2C=CR2 + Br2 BrR2C-CR2Br

RCOOH + NaHCO3 RCOONa + H2O + CO2 Sign in|Recent Site Activity|Report Abuse|Print Page|Remove Access|Powered By Google Sites