chemistry record book 2018-19 - amazon s3record+book+2018...page 35 of 78 chemistry practicals...

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CHEMISTRY PRACTICALS

INDEX EXPT.

NO EXPERIMENT ALPHA, NEW ALPHA,

BETA, CHROME, DELTA EULER, FOUCS, GAMMA,

ZENITH-1, ZENITH-2 DATE DATE

1 BUNSEN BURNER 12.06-2017 13.06-2017

2 Melting and Boiling point determination 10.07.2017 11.07.2017

3 LAB APPARATUE 16.08.2017 18.07.2017

4 Reaction of ANION 15.09-2017 17.09.2017

5 Reaction of CATIONS 23.10.2017 24.10.2017

6 Titration of Na2CO3 and HCl 06.06.2018 07.06.2018

7 Titration of NaOH and Oxalic acid 13.06.2018 14.06.2018

8 Titration of KMnO4 and Mohr's salt 19.06.2018 20.06.2018

9 Titration of KMnO4 and Oxalic acid 26.06.2018 27.06.2018

10 Analysis of Simple Salt - 1 02.07.2018 04.07.2018









19 Analysis of Simple Salt – 10 27.08.2018 29.08.2018




23 Analysis of Organic functional group-1 25.09.2018 26.09.2018








31 Chromatography 29.10.2018 30.10.2018

32 Carbohydrate test 10.11.2018 12.11.2018

33 Protein test 10.11.2018 12.11.2018

34 Lyphilic sol preparation 27.11.2018 28.11.2018

35 Lyphobic sol preparation 27.11.2018 28.11.2018

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EXPERIMENT-1

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EXPERIMENT-2

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EXPERIMENT-3

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EXPERIMENT-4

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EXPERIMENT-5

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EXPERIMENT - 6

TITRATION-1 (SODIUM CARBONATE AND HYDROCHLORIC ACID) AIM- To estimate the amount of hydrochloric acid present in 1000ml of given solution, 0.05M sodium carbonate solution is supplied. APPARATUS REQUIRED- Burette, Pipette, Conical flask, Burette stand, Tile,Wash bottle, and Beakers. CHEMICALS REQUIRED- Hydrochloric acid solution , Sodium carbonate solution(0.05M). INDICATOR- Methyl orange . PRINCIPLE-

2 3 2 22 2HCl Na CO NaCl H O CO

END POINT- Pale yellow to Pale pink.

FORMULA- 1 1

1

M Vn

= 2 2

2

M Vn

,

Sodium carbonate Hydrochloric acid

111

M molarityV volumen noofmoles

22

2


21000wM

M V

36.51000

M GMWV volumew weight

PROCEDURE- 1. Burette is filled with HCl solution till zero mark including nozzle part with out any air bubble in

the column 2. 20 ml of sodium carbonate solution is pipetted out and transferred in to conical flask . 3. One or two drops of methyl orange indicator is added to the conical flask. The colour of solution

turns pale yellow. 4. The solution in the flask is now titrated with HCl solution until the colour of solution turns pale

pink .this is the end point. 5. Note down the final burette reading. 6. Repeat the processes until two constant congruent reading obtained.

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TABLE-

CALCULATION- Sodium carbonate Hydrochloric acid M1=0.05M M2= x V1=20ml V2=20.8ml n1=1 n2=2 using formula,

1 1

1

M Vn

= 2 2

2

M Vn

,

1 1 2

21 2

0.05 20 2 0.0961 20.8

M V nM Mn V

Molarity of HCl solution is =0.096M Using formula,

21000wM

M V

2 0.096 1000 36.5 3.51

1000 1000M V Mw g

REPORT- The molarity of given HCl solution is =0.096 Weight of HCl in 1000ml of given solution is =3.51 gm

Serial no Volume of sodiumcarbonate in ml

Burette reading Initial Final (a) (b)

Volume of HCl solution in ml (a–b)

1 20 0 20.9 20.9

2 20 0 20.8 20.8

3 20 0 20.8 20.8

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EXPERIMENT - 7

TITRATION-2 (SODIUM HYDROXIDE AND OXALIC ACID) AIM- To estimate the amount of Sodium hydroxide present in 500ml of given solution, 0.1M oxalic acid solution is supplied. APPARATUS REQUIRED- Burette, Pipette, Conical flask, Burette stand, Tile,Wash bottle, and Beakers. CHEMICALS REQUIRED- oxalic acid acid solution(0.1M) , Sodium hydroxide solution INDICATOR- Phenolphthalein . PRINCIPLE-

2 4 2 2 4 2 22 2 2NaOH C O H C O Na H O

END POINT- Colour less to Pale pink.

FORMULA- 1 1

1

M Vn

= 2 2

2

M Vn

,

Oxalic acid Sodium hydroxide

111


22

2


21000wM

M V

40500

M GMWV volume mlw weight

PROCEDURE-

1. Burette is filled with NaOH solution till zero mark including nozzle part with out any air bubble in the column

2. 20 ml of oxalic acid solution is pipetted out and transferred in to conical flask . 3. One or two drops of phenolphthalein indicator is added to the conical flask. The colour of

solution remains colour less. 4. The solution in the flask is now titrated with NaOH solution until the colour of solution turns to

permanent pale pink.this is the end point. 5. Note down the final burette reading. 6. Repeat the processes until two constant congruent reading obtained.

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TABLE-

CALCULATION- Oxalic acid Sodium hydroxide M1=0.1M M2= x V1=20ml V2=19.5ml n1=1 n2=2 using formula,

1 1

1

M Vn

= 2 2

2

M Vn

,

1 1 2

21 2

0.1 20 2 0.2051 19.5

M V nM Mn V


21000wM

M V

2 0.205 500 40 4.1

1000 1000M V Mw g

REPORT- The molarity of given NaOH solution is =0.205M Weight of NaOH in 500ml of given solution is =4.1 gm

Serial no Volume of oxalic acid in ml


Volume of NaOH solution in ml (a–b)

1 20 0 19.6 19.6

2 20 0 19.5 19.5

3 20 0 19.5 19.5

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EXPERIMENT - 8

TITRATION-3 (POTASSIUM PERMANGANATE AND MOHR’S SALT SOLUTION) AIM- To estimate the amount of KMnO4 present in 500ml of given solution, 0.1M ferrous ammonium sulphate solution is supplied. APPARATUS REQUIRED- Burette, Pipette, Conical flask, Burette stand, Tile,Wash bottle, and Beakers. CHEMICALS REQUIRED- KmnO4solution , morh’s salt solution(0.1M), dilute H2SO4 INDICATOR- KmnO4 is self indicator. PRINCIPLE-

4 2 4 4 2 4 4 2 4 3 22 8 10 2 2 5 (SO ) 8KMnO H SO FeSO K SO MnSO Fe H O


FORMULA- 1 1

1

M Vn

= 2 2

2

M Vn

,

Mohr’s salt Solution KmnO 4 solution

111


22

2


21000wM

M V

158500


PROCEDURE-

1. Burette is filled with KmnO4 solution till zero mark including nozzle part with out any air bubble in the column

2. 20 ml of Mohr’s salt solution is pipetted out and transferred in to conical flask . 3. 20 ml of dilute H2SO4 is added to the conical flask. The colour of solution remains colour less. 4. The solution in the flask is now titrated with KmnO4 solution until the colour of solution turns to

permanent pale pink. This is the end point. 5. Note down the final burette reading. 6. Repeat the processes until two constant congruent reading obtained.

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TABLE-

CALCULATION- Mohr’s salt solution KmnO4 solution M1=0.1M M2= x V1=20ml V2=19.8ml n1=10 n2=2 using formula,

1 1

1

M Vn

= 2 2

2

M Vn

,

1 1 2

21 2

0.1 20 2 0.0210 19.8

M V nM Mn V


21000wM

M V

2 0.02 500 158 1.58

1000 1000M V Mw g

REPORT- The molarity of given KmnO4 solution is =0.02M Weight of KmnO4 in 500ml of given solution is =1.58gm

Serial no Volume of mohr’s salt solution in ml


Volume of KmnO4 solution in ml (a–b)

1 20 0 19.9 19.9

2 20 0 19.8 19.8

3 20 0 19.8 19.8

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EXPERIMENT - 9

TITRATION-4 (POTASSIUM PERMANGANATE AND OXALIC ACID) AIM- To estimate the amount of oxalic acid present in 100ml of given solution, 0.02M KMnO4 solution is supplied. APPARATUS REQUIRED- Burette, Pipette, Conical flask, Burette stand, Tile,Wash bottle, and Beakers. CHEMICALS REQUIRED- oxalic acid acid solution , KMnO4 solution(0.02M), dilute H2SO4 solution INDICATOR- KMnO4 is self indicator PRINCIPLE-

4 2 4 2 2 4 2 4 4 2 22 8 5 2 2 10 8KMnO H SO C H O K SO MnSO CO H O


FORMULA- 1 1

1

M Vn

= 2 2

2

M Vn

,

KMnO4 solution Oxalic acid

111


22

2


21000wM

M V

126100


PROCEDURE- 1. Burette is filled with KMnO4 solution till zero mark including nozzle part with out any air bubble

in the column 2. 20 ml of oxalic acid solution is pipetted out and transferred in to conical flask . 3. 20 ml of dilute H2SO4 is added to the conical flask and heated till 600C. The colour of solution

remains colour less. 4. The solution in the flask is now titrated with KMnO4 solution in hot condition until the colour of

solution turns to permanent pale pink.this is the end point. 5. Note down the final burette reading. 6. Repeat the processes until two constant congruent reading obtained.

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TABLE-

CALCULATION- KMnO4 solution Oxalic acid M1=0.1M M2= x V1=20ml V2=19.5ml n1=1 n2=2 using formula,

1 1

1

M Vn

= 2 2

2

M Vn

,

1 1 2

21 2

0.02 20.6 5 0.052 20

M V nM Mn V


21000wM

M V

2 0.05 100 126 0.65

1000 1000M V Mw g

REPORT- The molarity of given oxalic acid solution is =0.05M Weight of oxalic acid in 500ml of given solution is = 0.65 gm

Serial no Volume of oxalic acid in ml


Volume of KMnO4 solution in ml (a–b)

1 20 0 20.6 20.6

2 20 0 20.5 20.5

3 20 0 20.5 20.5

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EXPERIMENT - 10

ANALYSIS OF SIMPLE SALT -1

EXPERIMENT OBSERVATION INFERENCE

I. PRELIMINARY TESTS

(a) Physical state Crystalline -

(b) Colour White Cu2+ , Fe2+,Mn2+ and Ni2+are

absent

(c) Flame test – A small of paste of the salt with conc. HCl is prepared and put into the flame with the help of a platinum wire.

No flame colour observed No particular inference

(d) Action of heat: The salt is taken in a dry test tube and it is heated.

Water particles are observed on the walls of the test tube

May be Hydrated salt

II. IDENTIFICATION OF ANION:

Reaction with dil. HCl To the salt dil. HCl is added.

No reaction 23CO and 3CH COO are

absent

Reaction with conc. H2SO4 To the salt Conc. H2SO4 is added.

No reaction 3Cl ,Br ,NO are absent

IV. Test for 24SO :

1. To the salt solution 2/3 drops of BaCl2 sol. Is added 2. To the above ppt con. HCl is added

White ppt is formed

Ppt is insoluble in con. HCl

24SO may be present

24SO is confirmed

Conformation test for 24SO : To the

salt solution Lead acetate added White ppt of PbSO4 is formed 2

4SO is confirmed

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III. IDENTIFICATION OF CATION:

2 ml of Salt solution taken in a test tube. Few drops of .dil HCl added No ppt is formed

I group cations 2Pb is absent

2 ml of Salt solution taken in a test tube. Few drops of .dil HCl added and 2H S gas is passed

No ppt is formed II group cations 2Cu is absent

2 ml of Salt solution taken in a test tube. Solid NH Cl4 added followed by 2 drops of

NH OH4 No ppt is formed

III group cations 3Al and 2Fe are absent


NH OH4 . H S2 gas passed No ppt is formed

IV group cations 2Zn , 2Mn , 2Ni are absent


NH OH4 . Then NH CO4 32 solution is

added

No ppt is formed V group cations 2Ca ,

2Br , 2Sr are absent

VI GROUP:

Test for 4NH ION :

To small amount of salt 2 drops of NaOH solution is added and heated.

Test for 2Mg : To the salt solution NH4Cl (solid) added and 2 drops of NH4OH, 2 drops of Na2(HPO4) sol is added. Conformation test: To salt solution NH4OH solution or NaOH solution is added.

No reaction

White ppt is formed

White ppt is formed

4NH is absent

May be 2Mg

2Mg is conformed

REPORT: The anion present in given salt is SULPHATE. 24SO

The cation present in given salt is MAGNESIUM. 2Mg

The given salt is MAGNESIUM SULPHATE. 4MgSO

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EXPERIMENT – 11

ANALYSIS OF SIMPLE SALT-2

EXPERIMENT OBSERVATION INFERENCE I. PRELIMINARY EXAMINATIONS:

(a) Physical state Crystalline

(b) Colour White

Cu2+ , Fe2+,Mn2+ and Ni2+ ions are absent


Brick red colour flame observed May be 2Ca


Loss of water of crystallisation

Hydrated salt


Reaction with dil. HCl To the salt dil. HCl is added. No reaction

23CO and 3CH COO are

absent

Action with con. H2SO4: To the salt Conc. H2SO4 is added.

A colourless gas is evolved with pungent smell it gives dense white fumes when a glass rod dipped in

NH3 solution is exposed

Cl may be present

Confirmation Test’s for Cl : 1) Action with MnO2 To the small amount of salt a pinch of MnO2 is added and 2 or 3 drops of conc. H2SO4 is added. 2) Action with AgNO3. To the salt sol 2/3 drops of AgNO3 sol. Is added

Greenish yellow gas is evolved with

pungent smell.

A white ppt is formed it is completely soluble in NH3 sol.

Cl is formed

Cl is confirmed

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I GROUP: To the salt solution few drops of dil. HCl is added

No reaction I group cations are absent

II GROUP: To the salt solution dil. HCl is added and H2S gas is passed

No reaction

II group cation ( 2Cu ) is absent.

III GROUP: To the salt solution NH4Cl (solid) and NH4OH (sol) is added.

No reaction IIIrd group cations are

absent

IV GROUP: To the salt sol. NH4Cl (solid) +NH4OH (sol) are added & H2S gas is passed.

No ppt is formed IV group cations are

absent.

V. GROUP: To the salt solution NH4Cl(solid) NH4OH(sol) and (NH4)2CO3solution is added

Confirmation test for 2Ca

To the salt solution K2CrO4 solution is added To the salt solution (NH4)2C2O4 Ammonium oxalate solution is added

White ppt is formed

Yellow transparent sol. is observed

A white ppt is formed Insoluble in acetic acid

V group cations 2Ca may be present

2Ca is confirmed

2Ca is confirmed

REPORT : The anion present in given salt is CHLORIDE. 1Cl

The cation present in given salt is CALCIUM. 2Ca The salt is CALCIUM CHLORIDE 2CaCl

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EXPERIMENT – 12


EXPERIMENT OBSERVATION INFERENCE I. PRELIMINARY TESTS


(b) Colour White Cu2+ , Fe2+,Mn2+ and Ni2+

ions are absent


Apple green colour flame observed

May be 2Ba


Water particles are observed on the inner walls

of Test Tube May be Hydrated salt



No reaction 23CO and 3CH COO

are absent

Action with con. H2SO4: To the salt Conc. H2SO4 is added.

A reddish brown vapours evolved

Br may be present

Confirmation Test’s for Br- :- 1) Action with MnO2: To the small amount of salt add pinch of MnO2 and 2/3 drops of con. H2SO4 added 2) Action with AgNO3: To the salt sol 2/3 drops of AgNO3 sol. added

Reddish brown gas is

evolved.

Pale yellow ppt is formed it is partially soluble in NH3 sol.

Br is confirmed

Br is confirmed

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No reaction I group cations is absent

II. GROUP: To the salt solution dil. HCl is added and H2S gas is passed

No reaction II group cation is absent.

III. GROUP: To the salt solution NH4Cl (solid) and NH4OH (sol) is added.

No reaction III group cations are

absent

IV. GROUP: To the salt solution NH4Cl (solid) followed by NH4OH(sol) are added and H2S gas is passed.

No ppt is formed

IV group cations are absent

V. GROUP: To the salt solution NH4Cl (solid) NH4OH (sol) and (NH4)2CO3sol. is added Confirmation test for ,2 2Ca Ba

To the salt solution K2CrO4 solution is added

White ppt is formed

Yellow ppt is formed

V group cations 2Ba may be present

2Ba is confirmed

REPORT: The anion present in given salt is BROMIDE. 1Br

The cation present in given salt is BARIIUM. 2Ba The given salt is BARIUM BROMIDE. 2BaBr

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EXPERIMENT – 13






ions are absent


Light green flashes observed May be 2Zn


Loss of water of crystallisation Hydrated salt



No reaction


absent



Test for 24SO :

To the salt solution 2/3 drops of BaCl2 sol. Is added

To the above ppt con. HCl is added

White ppt is formed

Ppt is insoluble in con. HCl

24SO may be present

24SO is confirmed

Conformation test for 24SO :

To the salt solution. Lead acetate White ppt of PbSO4 is formed 2

4SO is confirmed

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III. IDENTIFICATION OF CATION :


No reaction

I group cations are absent

II. GROUP: To the salt solution dil. HCl is added and H2S gas is passed.

No reaction II group cation ( 2Cu ) is

absent.


No ppt is formed

IIIrd group cations are absent

IV GROUP: To the salt solution NH4Cl (solid) NH4OH(sol) are added and H2S gas is passed Conformation Test: To the salt sol. NaOH solution is added

White ppt is formed

Curdy white ppt is formed it is soluble in excess NaOH

2Zn may be present

2Zn is confirmed


The cation present in given salt is ZINC. 2Zn The salt is ZINC SULPHATE 4ZnSO

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EXPERIMENT – 14 ANALYSIS OF SIMPLE SALT-5


I. PRELIMINARY EXAMINATIONS


(b) Colour Green Ni2 salt may be present




Reddish Brown vapours are evolved

May be Nitrate salt



No reaction 23CO is absent


Reddish Brown gas evolved on heating 3NO are absent

Test for 3NO :

To the small amount of salt 2/3 drops of con. H2SO4. ½ pieces of Cu turnings are added and then heated strongly

Reddish brown gas is evolved and the liquid present in the tube

turns to blue or light green May be 3NO

Conformation Test for 3NO :

Brown – Ring Test: To the Salt Solution freshly prepared FeSO4 sol. is added. The test tube is kept in an inclined position and con. H2SO4 is added slowly along the walls of the test tube.

A brown ring is formed at the junction of aqueous and acid layers. (FeSO4.NO) nitroso ferrous sulphate is formed

3NO is conformed

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III. IDENTIFICATION OF CATION :


No reaction


II. GROUP: To the salt solution dil. HCl is added and H2S gas is passed.


absent.


No ppt is formed

IIIrd group cations are absent

IV GROUP: To the salt solution NH4Cl (solid) NH4OH(sol) are added and H2S gas is passed Conformation Test: To the salt sol, NH4OH solution is added followed by dimethyl glyoxime

Black ppt is formed

Red ppt is formed

2Ni may be present

2Ni is confirmed

REPORT : The anion present in given salt is NITRATE (NO3)–.

The cation present in given salt is Ni+2. The salt is NICKEL NITRATE 3 2Ni NO

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(b) Colour Pale Pink May be 2Mn Salt


Light green flashes observed May be 2Mn

(d) Action of heat: A small amount of salt is taken in a dry test tube and it is heated.

Loss of water of crystallisation Hydrated salt



23CO and 3CH COO

are absent

Reaction with con. H2SO4: To the salt Conc. H2SO4 is added.

A colourless gas is evolved with pungent smell it gives dense

white fumes when a glass rod dipped in NH3 solution is

exposed

Cl may be present

Confirmation Test’s for Cl : 1) Action with MnO2 To the small amount of salt a pinch of MnO2 is added and 2 or 3 drops of conc. H2SO4 is added. 2) Action with AgNO3. To the salt sol 2/3 drops of AgNO3 solution Is added

Greenish yellow gas is evolved

with pungent smell.

A white ppt is formed it is completely soluble in NH3

solution

Cl is confirmed

Cl is confirmed

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No reaction


II. GROUP: To the salt solution dil. HCl is added and H2S gas is passed


absent.


No reaction

III group cations are absent

IV GROUP: To the salt solution NH4Cl (solid) NH4OH(sol) are added and H2S gas is passed Conformation Test: To the salt sol. NaOH solution is added

Flesh coloured ppt is formed

b) White ppt is formed it turns into light brown

colour.

2Mn may be present

2Mn is confirmed

REPORT: The anion present in given salt is CHLORIDE. Cl

The cation present in given salt is MANGANOUS. 2Mn The salt is MANGANOUS CHLORIDE 2MnCl

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(b) Colour White

Cu2+ , Fe2+,Mn2+ and Ni2+ ions are absent


Crimson red colour flame observed May be 2Sr


Loss of water of crystallisation

Hydrated salt

(e) Flame test: Make the paste of the salt with conc HCl and take on to the loop of platinum loop holder. Heat on a flame for few minutes

Crimson red colored flame is observed Sr2 may be present



No reaction 23 3CO ,CH COO is

absent

Reaction with con. H2SO4: To the salt Conc. H2SO4 is added.

A colourless gas is evolved with pungent smell it gives dense white

fumes when a glass rod dipped in NH3 solution is exposed

Cl may be present

Confirmation Test’s for Cl : 1) Action with MnO2 To the small amount of salt a pinch of MnO2 is added and 2 or 3 drops of conc. H2SO4 is added. 2) Action with AgNO3.

Greenish yellow gas is evolved with

pungent smell.

A white ppt is formed it is completely

Cl is formed

Cl is confirmed

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I GROUP: To the salt sol few drops of dil. HCl is added

No reaction I group cations are

absent

II GROUP: To the salt sol dil. HCl is added and H2S gas is passed

No reaction


III GROUP: To the salt solution NH4Cl (solid) and NH4OH (sol) is added.

No reaction IIIrd group cations are

absent

IV GROUP: To the salt solution NH4Cl (solid) followed by NH4OH (sol) are added & H2S gas is passed.

No ppt is formed IV group cations are

absent.

V. GROUP: To the salt solution NH4Cl(solid) NH4OH(sol) and (NH4)2CO3sol. is added

Confirmatory test for Sr2 : To the salt solution, ammonium sulphate solution is added.

White ppt is formed

White ppt is formed

V group cations may be present

Sr2 confirmed.

REPORT : The anion present in given salt is CHLORIDE 1Cl

The cation present in given salt is STRONTIUM 2Sr The salt is STRONTIUM CHLORIDE 2SrCl

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EXPERIMENT OBSERVATION INFERENCE I. PRELIMINARY EXAMINATIONS


(b) Colour White

Cu2+ , Fe2+,Mn2+, 2+Ni ions are absent




Reddish Brown vapours are evolved

May be Nitrate salt


Reaction with dilute HCl To the salt dil. HCl is added. No reaction

23CO and -1

3CH COO are

absent


Reddish Brown gas evolved on heating

13NO may be present

Test for 3NO :


Reddish brown gas is evolved and the liquid present in the tube turns

to blue or light green May be 3NO


Brown – Ring Test: To the Salt Sol freshly prepared FeSO4 sol. is added. The test tube is kept in an inclined position and con. H2SO4 is added slowly along the walls of the test tube.

A brown ring is formed at the junction of aqueous and acid layers. (FeSO4.NO) nitroso ferrous sulphate

is formed

3NO is conformed

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No reaction I group cations are absent

II. GROUP: To the salt sol dil. HCl is added and H2S gas is passed No reaction


III. GROUP: To the salt sol NH4Cl (solid) and NH4OH (sol) is added.

Conformation Test for 3Al : S.S.+ NaOH solution is added

White gelatinous ppt is formed

White gelatinous ppt is formed which is soluble in excess of NaOH

3Al may be present

3Al confirmed

REPORT : The anion present in given salt is NITRATE. 13NO

The cation present in given salt is ALLUMINIUM. 3Al

The salt is ALLUMINIUM NITRATE 3 3Al NO

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EXPERIMENT – 18





(b) Colour Pale Green May be Fe+2 Salt




Water particles are observed on the walls of the test tube

May be Hydrated salt



No reaction 23CO is absent

Reaction with conc. 2 4H SO

To the salt Conc. H2SO4 is added.


IV. Test for 24SO :

1. To the salt solution 2/3 drops of BaCl2 solution Is added 2. To the above ppt con. HCl is added

White ppt is formed

Precipitate is insoluble in con.

HCl

24SO may be present

24SO is confirmed

Conformation test for 24SO : To

the salt solution Lead acetate added

White ppt of PbSO4 is formed 24SO is confirmed

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absent

II GROUP: To the salt solution 2/3 drops of dil. HCl is added and H2S gas is passed


absent.

III. GROUP: To the salt solution NH4Cl (solid) and NH4OH (sol) is added. Conformation Test: To the salt solution K4[Fe(CN)6] Solution is added.

Dirty Green colour ppt is formed

Light Blue colour ppt is formed

2Fe may be present

2Fe is confirmed


The cation present in given salt is FERROUS. 2Fe The given salt is FERROUS SULPHATE. 4FeSO

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EXPERIMENT – 19

ANALYSIS OF SIMPLE SALT -10




(b) Colour Blue May be Cu2+ Salt


Bluish green colour flame observed May be 2Cu


Reddish brown Vapours are evolved

May be Nitrate salt




absent


No reaction 3NO are absent

Test for 3NO :


Reddish brown gas is evolved and the liquid present in the tube

turns to blue or light green

May be 3NO


Brown – Ring Test: To the Salt Solution freshly prepared FeSO4 solution is added. The test tube is kept in an inclined position and con. H2SO4 is added slowly along the walls of the test tube.

A brown ring is formed at the junction of aqueous and acid layers. (FeSO4.NO) nitroso ferrous sulphate is formed

3NO is confirmed

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absent

II GROUP: To the salt solution 2/3 drops of dil. HCl is added and H2S gas is passed Conformation Test :

To the salt solution 4 6K Fe CN

solution is added.

Black ppt is formed

Chocolate Brown colour ppt is formed

2Cu may be present

2Cu is confirmed

REPORT: The anion present in given salt is NITRATE. 13NO

The cation present in given salt is COPPER. 2Cu The given salt is COPPER NITRATE. 3 2Cu NO

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EXPERIMENT – 20 ANALYSIS OF SIMPLE SALT -11





ions are absent


Silver white colour flame is observed May be 2Pb


Reddish brown vapours are evolved with cracking sound

May be Lead Nitrate



No reaction 23CO and 3CH COO are

absent

Reaction with conc. H2SO4: To the salt Conc. H2SO4 is added.

Reddish Brown gas evolved on heating 3NO may be present

Test for 3NO :


Reddish brown gas is evolved and the liquid present in the tube turns

to blue or light green

May be 3NO


Brown – Ring Test: To the Salt Sol freshly prepared FeSO4 sol. is added. The test tube is kept in an inclined position and con. H2SO4 is added slowly along the walls of the test tube.

A brown ring is formed at the junction of aqueous and acid layers. (FeSO4.NO) nitroso ferrous sulphate

is formed

3NO is conformed

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I GROUP: To the salt solution few drops of dil. HCl is added Conformation test: To the salt solution K2CrO4 solution Is added

White ppt is formed

Yellow ppt is formed

I group cations may be present 2Pb


2Pb is confirmed

REPORT:

The anion present in given salt is NITRATE. 13NO

The cation present in given salt is LEAD. 2Pb

The salt is LEAD NITRATE. 3 2Pb NO

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EXPERIMENT – 21





ions are absent




Smell of ammonia is evolved May be ammonium salt


Reaction with dil. HCl: To the salt dil. HCl is added.

Smell of vinegar is observed

CH COO3 may be

present

To this solution freshly prepared neutral FeCl3 is added

Red colour solution formed

CH COO3 may be

present

Boil the above solution with water on hot water bath.

Brown colour ppt is formed

CH COO3 may be

present

Confirmatory Test: To the original salt solution 1 ml of ethyl alcohol is added along with concentrated H SO2 4 and boiled for few minutes.

A fruity smell due to ester is observed.

CH COO3 confirmed


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III. IDENTIFICATION OF CATION: Group-I 2 ml of Salt solution taken in a test tube. Few drops of .dil HCl added

No ppt is formed I group cations 2Pb is

absent

Group-II 2 ml of Salt solution taken in a test tube. Few drops of .dil HCl added and 2H S gas is passed


Group-III 2 ml of Salt solution taken in a test tube. Solid NH Cl4 added followed by 2 drops of

NH OH4

No ppt is formed III group cations 3Al and

2Fe are absent

Group-IV 2 ml of Salt solution taken in a test tube. Solid NH Cl4 added followed by 2 drops of

NH OH4 . H S2 gas passed

No ppt is formed IV group cations 2Zn ,

2Mn , 2Ni are absent

Group-V 2 ml of Salt solution taken in a test tube. Solid NH Cl4 added followed by 2 drops of


added



Group-VI No particular reagent.

Test for 4NH ION:

To the small amount of salt 2/3 drops of NaOH solution is added and heated.

Conformation Test: 4NH

To the salt solution Nessler’s (K2HgI4/ KOH) reagent is added

Smell of NH3 gas is evolved. It gives dense

white fumes when a glass rod dipped in con.

HCl is exposed.

Reddish brown ppt is formed

4NH may be present

4NH is conformed

REPORT :

1) The anion present in given salt is ACETATE. 13CH COO

2) The cation present in given salt is AMMONIUM. 14NH

3) The salt is AMMONIUM ACETATE. 4 3NH CH COO

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(a) Physical state Amorphous


ions are absent




Smell of ammonia is evolved May be ammonium salt


Reaction with dil. HCl 1) Action with dil. HCl To the small amount of salt 2 or 3 drops of dil. HCl is added. This is gas produced above reaction is passed into lime water.

Colourless gas is evolved with brisk

effervescences.

The lime water turns to milky

23CO may be present

23CO may be present

2) Conformation Tests for 23CO

Action with BaCl2: To the salt sol. 2/3 drops of BaCl2(sol) is added Solubility Test. To the above ppt dil HCl is added

White ppt is formed

Ppt is completely soluble in dil. HCl

23CO may be present

23CO is confirmed


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III. IDENTIFICATION OF CATION: Group-I 2 ml of Salt solution taken in a test tube. Few drops of .dil HCl added

No ppt is formed I group cations 2Pb is

absent

Group-II 2 ml of Salt solution taken in a test tube. Few drops of .dil HCl added and 2H S gas is passed


Group-III 2 ml of Salt solution taken in a test tube. Solid NH Cl4 added followed by 2 drops of

NH OH4

No ppt is formed III group cations 3Al and

2Fe are absent

Group-IV 2 ml of Salt solution taken in a test tube. Solid NH Cl4 added followed by 2 drops of

NH OH4 . H S2 gas passed

No ppt is formed IV group cations 2Zn ,

2Mn , 2Ni are absent

Group-V 2 ml of Salt solution taken in a test tube. Solid NH Cl4 added followed by 2 drops of


added



Group-VI No particular reagent.

Test for 4NH ION:

To the small amount of salt 2/3 drops of NaOH solution is added and heated.

Conformation Test: 4NH

To the salt solution Nessler’s (K2HgI4/ KOH) reagent is added

Smell of NH3 gas is evolved. It gives dense

white fumes when a glass rod dipped in con.

HCl is exposed.

Reddish brown ppt is formed

4NH may be present

4NH is conformed

REPORT :

1) The anion present in given salt is CARBONATE. 23CO

2) The cation present in given salt is AMMONIUM. 14NH

3) The salt is AMMONIUM CARBONATE. 4 32NH CO

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EXPERIMENT – 23

ANALYSIS OF ORGANIC FUNCTIONAL GROUP -1


1.PRELIMINARY TEST- a. Physical state- b. Ignition test- A small amount of compound is burnt in a spatula. c.Solubility- In Ether Water Dilute Sodium bicarbonate Dilute Sodium hydroxide Dilute hydrochloric acid

Liquid Non sooty flame was observed + + + + +

The given compound is aliphatic The given organic compoumd is netral

2.IDENTIFICATION TEST-(esterification test) To the small amount of compound in a test tube acetic acid is added follwed by few dropes of concentrated sulphuric acid and heated on water bath.

Fruity smell observed

Alcoholic group may be present

3.CONFIRMATION TEST- (iodoform test) to the small amount of compound in a test tube iodine is added followed by few drops of sodium hydroxide solution and heated on a water bath.

Yellow colour crystalline precipitate is observed

Alcoholic functional group is confirmed

REPORT- The given organic compound contain “aliphatic alcoholic” functional group

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EXPERIMENT – 24




Liquid Non sooty flame was observed + + + + –

The given compound is aliphatic The given organic compoumd is strongly acidic

2.IDENTIFICATION TEST-( neutral ferric chloride test) To the small amount of compound in a test tube neutral ferric chloride solution is added

Red colour precipitate observed

Carboxylic group may be present

3.CONFIRMATION TEST-(esterification test) To the small amount of compound in a test tube ethyl alcohol is added follwed by few dropes of concentrated sulphuric acid and heated on water bath.

Fruity smell is observed

carboxylic functional group is confirmed

REPORT- The given organic compound contain “aliphatic carboxylic ” functional group

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EXPERIMENT – 25 ANALYSIS OF ORGANIC FUNCTIONAL GROUP -3



Liquid Sooty flame was observed + + + + –

The given compound is aromatic The given organic compoumd is strongly acidic

2.IDENTIFICATION TEST-( neutral ferric chloride test) To the small amount of compound in a test tube neutral ferric chloride solution is added

Red colour precipitate observed

Carboxylic group may be present

3.CONFIRMATION TEST-(esterification test) To the small amount of compound in a test tube ethylalcohol is added follwed by few dropes of concentrated sulphuric acid and heated on water bath.

Fruity smell is observed

carboxylic functional group is confirmed

REPORT- The given organic compound contain “aliphatic carboxylic ” functional group

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EXPERIMENT – 26





The given compound is aliphatic The given organic compoumd is neutral

2.IDENTIFICATION TEST-( 2,4 DNP test) To the small amount of compound in a test tube 2,4 DNP solution is added

Orange yellow precipitate is observed

Carbonyl group may be present

3.CONFIRMATION TEST-(Schiff test) To the small amount of compound in a test tube few drops of schiff reagent is added

Pink colour is observed

Aldehydic functional group is confirmed

REPORT- The given organic compound contain “aliphatic aldehydic ” functional group

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Solid Sooty flame was observed + – – + –

The given compound is aromatic The given organic compoumd is weakly acidic

2.IDENTIFICATION TEST-( neutral ferric chloride test) To the small amount of compound in a test tube neutralferric chloride solution is added

Violet colour is observed

Phenolic group may be present

3.CONFIRMATION TEST-(libberman nitroso test) To the small amount of compound in a test tube sodium nitrite is added followed by concentrated sulphuric acid is added

Blue green colour solution is observsd which on dilution turned red.on adding sodium hydroxide solution deep blue colour is observed

phenolic functional group is confirmed

REPORT- The given organic compound contain “phenolic ” functional group

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Liquid Sooty flame was observed + – – – +

The given compound is aromatic The given organic compoumd is basic

2.IDENTIFICATION TEST-( azo dye test) To the small amount of compound in a test tube sodium nitrite solution is added followed by few drops of concentrated hydrochloric acid(0-5 temperature).now alpha naphthol solution is added

Formation of Orange red dye is observed

Primery amino group may be present

3.CONFIRMATION TEST-(carbylamine test) To the small amount of compound in a test tube few drops of chloroform is added followed by few drops of NaOH solution and heated on a water bath.

Foul smell of isocyanide compound is observed

Primery amino functional group is confirmed

REPORT- The given organic compound contain “aromatic primery amino” functional group

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Liquid Sooty flame was observed +

– – – –

The given compound is aromatic The given organic compoumd is neutral





Pink colour is observed

Aldehydic functional group is confirmed

REPORT- The given organic compound contain “aromatic aldehydic ” functional group

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EXPERIMENT – 30





The given compound is aliphatic The given organic compoumd is neutral





No Pink colour is observed

Keton functional group is confirmed

REPORT- The given organic compound contain “aliphatic ketone ” functional group

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EXPERIMENT – 31

CHROMATOGRAPHY

1. SEPARATION OF PIGMENTS PRESENT IN LEAF AND FLOWERS BY PAPER CHROMATOGRAPHY

AIM : To separate the leaf pigments of spinach and to calculate fR values of

pigments

APPARATUS : Chromatographic paper of 20 3cm (Whatman No. 1), Mortar, Pestle, Funnel, Beakers, Capillery tube, covering pad, pencil

CHEMICALS : Fresh spinach leaves, anhydrous 2CaCl , petroleum ether and acetone

PROCEDURE : Small pieces of spinach leaves are mixed with petroleum ether and acetone taken in 80 : 20 volume ratio. In a mortar leaves are grind well by a pestle.

The supernant liquid is decanted into a beaker. The contents of beaker is dried over in a chamber containing anhydrous 2CaCl . Cut the Whatman no.1 filter paper into 20 3cm cm size. Draw a pencil line at one end of the chromatographic filter paper. Apply the extracted solution from leaves as a spot on the pencil line using capillary tube. Wait till the spot is dried. Hang the filter paper in a beaker consisting of solvent mixture of 95ml petroleum ether and 5ml of acetone. The spot should be just above the solvent level in the beaker. Cover the beaker with a pad. The solvent while ascending the filter paper elutes the components of the mixture. Different components and solvent move on the filter paper to different heights.

Distance travelled by the component

Distance travelled by the solventfR

Once the chromatographic paper is developed, the heights of different colored spots and solvents levels are measured using a scale.

Distance traveled by solvent =8 cm Distance traveled by yellow spot = 7.2cm Distance traveled by green spot = 6.5cm Distance traveled by olive green spot = 6.2cm RESULT : 1) Yellow spot - fr 7.2/8 = 0.9

2) Green spot - fr 6.5/8 = 0.81

3) Olive Green spot - fr 6.2/8 = 0.77

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2. SEPARATION OF 2Pb AND 2Cd IONS BY PAPER CHROMATOGRAPHY

AIM : To separate the 2Pb and 2Cd ions by chromatography and to calculate fR

values

APPARATUS : Chromatographic paper of 20 6cm (Whatman No. 1), Beakers Capillery tube, covering pad, pencil

CHEMICALS : 3 32 2Pb NO Cd NO aqueous solutions, distilled water, acetone conc.

HCl 4 2NH S yellow solution

PROCEDURE : Prepare a solution of 2Pb and 2Cd ions by dissolving 3 2Pb NO and

3 2Cd NO salts in 20ml of distilled water. Cut a Whatman no. 1 filter paper

into 20 6cm size. Draw a line with a pencil at one end of the paper. Apply the solution as a spot on the pencil line of chromatographic paper using a capillary tube. Dry the spot, then hang the filter paper in a beaker consisting of 86 ml acetone 8 ml HCl and 6 ml 2H O as eluting solvent. The spot should be just above the eluting solvent level. After developing the chromatogram, measure the heights of yellow, black spots and solvent levels using a scale. Calculate fR values using the formula.

Height of coloured spot

Height of solventfR

Distance traveled by solvent =7 cm Distance traveled by yellow spot = 6.7 cm Distance traveled by black spot = 5.5cm RESULT : fR values of

1) Yellow spot i.e. 2Cd ions fR 6.7/7 = 0.95

2) Black spot i.e. 2Pb ion fR 5.5/7 = 0.78

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EXPERIMENT – 32

TEST FOR CARBOHYDRATE


1.TEST WITH CONCENTRATED SULPURIC ACID- To the small amount of compound in a watch glass few drops of concentrated sulphuric acid is added

The compound got chrared

The given compoumd may be carbohydrate

MOLISCH’S TEST- To the small amount of compound in a test tube Alkaline beta napthol is added follwed by few dropes of concentrated sulphuric acid added to the walls of the test tube .

Violet colour ring is observed

Carbohydrate is confirmed

3.BENEDICT’STEST- To the small amount of compound in a test tube Benedict’s reagent is added and heated on a water bath.

Red colour precipitate is observed

Carbohydrate is confirmed

REPORT- The given organic compound is “Carbohydrate” .

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EXPERIMENT – 33

TEST FOR PROTEIN


1.BIURET TEST - To the small amount of compound in a test tube few small amount of copper sulphate solution and sodium hydroxide solution is added

Violet colouration observed

The given compoumd may be protein

XANTHOPROTEIC TEST- To the small amount of compound in a test tube concentrated nitric acid is added .

Orange colour is observed in alkaline medium

Protein is confirmed

3.NINHYDRIN TEST- To the small amount of compound in a test tube Ninhydrin reagent is added and heated on a water bath.

violet colour is observed

Protein is confirmed

REPORT- The given organic compound is “Protein” .

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EXPERIMENT – 34 PREPARATION OF COLLOIDS

PREPARATION OF LYOPHILIC COLLOID SOLUTION (a) Preparation of Starch Colloidal Solution AIM : To prepare Lyophilic Starch Colloidial Solution APPARATUS : Beaker, Glass Rod, Funnel, Filter Paper CHEMICALS : Water Soluble Starch, Distilled Water PROCEDURE : Powdered one gram water soluble starch is made into paste by adding

water. 100 ml. of distilled water is heated in a beaker. The paste of starch is added to boiling water and constantly stirred well. The solution is filtered. The filtrate is colloidal solution of starch.

RESULT : Colloidal Starch solution is prepared. PRECAUTIONS : 1) Distilled water should be used

2) Constant stirring is necessary.

b) Preparation of GUM Colloidal Solution AIM : To prepare lyophilic colloid of gum? APPARATUS : Beaker, Glass Rod, Funnel, Filter Paper CHEMICALS : Raw Gum or Gum, Distilled Water PROCEDURE : One gram of gum is taken in a beaker. 100 ml of distilled water is added to

it. The beaker is strongly heated on a burner. The solution is constantly stirred. After cooling the solution is filtered. Colloidal Gum is obtained.

RESULT : Lyophilic colloidial sol of gum is prepared PRECAUTIONS : 1) Distilled water should be used

2) Constant stirring is necessary.

(c) Preparation of Colloidal Sol of Egg Albumin AIM : To prepare lyophilic colloid of egg albumin? APPARATUS : Beaker, Glass Rod, Funnel, Filter Paper CHEMICALS : Egg albumin, distilled water, NaCl solution PROCEDURE : Albumin is collected from egg by omitting yellow yolk completely. To this

100 ml of 5% (w/v) of NaCl solution is added. The solution is constantly stirred for 3-5 minutes, then it is filtered to collect lyophilic colloidal sol of Egg albumin.

RESULT : Lyophilic albumin solution is prepared. PRECAUTIONS : 1) Constant stirring is necessary

2) The albumin sol is prepared in cold condition only.

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EXPERIMENT – 35

PREPARATION OF LYOPHOBIC COLLOID SOLUTION a) Preparation of Ferric Hydroxide sol. AIM : To prepare 3Fe OH colloidal solution

APPARATUS : Beaker, Burner, Glass rod CHEMICALS : 3FeCl solution, distilled water.

PROCEDURE : Take 100ml of distilled water in a 250 ml beaker and heat to boiling. Add the solution of 3FeCl to the water with constant stirring. A wine red sol of is obtained.

3 2 33 3FeCl H O Fe OH HCl

3 33 3Fe OH Fe Fe OH Fe

RESULT : Colloidal solution of ferric hydroxide is prepared. PRECAUTIONS : 1) Distilled water is necessary 2) It should be subjected to dialysis

b) Preparation of Aluminum Hydroxide Sol. AIM : To prepare aluminum hydroxide sol in the laboratory APPARATUS : Beaker, Glass Rod, Burner CHEMICALS : 2% aluminum chloride, distilled water PROCEDURE : Take 100ml of distilled water in a beaker. And boil it on water bath to

100 c then add 2% of 3AlCl solution step wise with constant stirring. A

colour less 3Al OH sol is obtained.

3 2 33 3AlCl H O Al OH HCl

3 33 3Al OH Al Al OH Al

RESULT : 3Al OH colloidal sol has been prepared.

PRECAUTIONS : 1) Distilled water is necessary 2) It should be subjected to dialysis

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