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Organic ChemistryLaboratory manual

3rd semester pharmacy students Winter 2015-2016

Faculty of Pharmacy & Biotechnology

Lab 6: Qualitative Analysis of Organic Compounds

Background:

Qualitative Analysis of Organic Compounds

The analysis and identification of unknown organic compounds constitutes a very important aspect of experimental organic chemistry. There is no definite set procedure that can be applied overall to organic qualitative analysis.

Some basic experimental tests and physical constants are necessary for identifying an unknown compound. It is important that you understand just what information can and cannot be obtained from each of them.

The identification and characterization of an unknown organic compound normally refers to those processes or test that need to be preformed in order to answer the following important questions:

1. What kind of elements (carbon, hydrogen, nitrogen, ….. ) are in the compound?

2. What kind of functional groups are in the compound?

3. Where in the molecule are these functional groups located?

Identification of organic compounds consists in a systematic procedure, this procedure

may be carried out in steps are:

1. Preliminary examination or investigation: The preliminary investigation

consists in the study of physical properties of organic compound. of steps.

The various physical properties include condition (state), color, odor, and

solubility.

2. Determination of physical properties such as melting point, melting point.

3. Classification by solubility

4. Functional-group classifications

5. Elemental analysis (detection of Carbon, nitrogen, sulfur, halogen

elements using sodium fusion test).

6. Confirmation through the preparation of derivatives.

7. Special tests.

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Identification and Classification of organic compounds based on functional groups.

Most organic liquids are less dense than water, but alkyl halides, polyhalogenated

compounds, and many aryl halides are denser. If an organic liquid is denser than water, it

probably contains halogen.

Note physical characteristics: solid, liquid, color, and odor. Compounds that are yellow to

red in color are often highly conjugated.

1) Condition:

The simple observation as to whether the material is solid or liquid is an important first

guide for the unknown substance

The solid material should be examined to notice whether it is crystalline, amorphous or

fine powder.

In case of the liquid state, the constancy of the liquid material should be observed

(mobile, oily or viscous). Also, determine if the unknown is true liquid or solution by

adding anhydrous copper sulphate placed in a watch glass. The color will not be changed

with true liquids while with solutions it turns blue color.

2) Color:

The color of the original sample is noted, some compounds show color due to impurities,

while many others show colors due to the presence of chromophoric groups

(Conjugation System) in them Such as diene group. The color observation may help to

expect the unknown compound. Many chemical compounds are coloured because they

absorb visible light

3) Odor:Some organic compounds have characteristic odors, others have disagreeable odors. Any

advantage from the minimal information obtained in this manner is heavily offset by the

risks involved; therefore strong smelling of the sample must be avoided.

The characteristic odors of some compounds are:

1. Alcoholic odor: methanol and ethanol.

2. Bitter almond odor: benzaldehyde and nitrobenzene

3. Mice like odor: Acetamide.

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General Scheme of

A. Preliminary Test:

4. Pleasant fruity or floral smell odor: Esters

5. Vinegar like odor; acetic acid.

6. Fishy odor: Amines.

7. Phenolic odor: Many phenols

4) Solubility:The solubility of the unknown in the following reagents provides very useful information.

In general

The solubility of organic compounds can be divided into two major categories:

Solubility in which a chemical reaction is the driving force

Example:

Solubility in acidic solution (such as carboxylic acids or phenols)

Solubility in basic solution (such as basic organic compounds, Amines)

Solubility in which simple solubility or miscibility due to Dipole-dipole 

Interaction, Hydrogen bonding - special case of dipole-dipole when there is a

hydrogen bonded to a N, O, or F. (or Ion-dipole - interaction of an ion with a

polar molecule)

examples: dissolving any ionic compound in water), such as

o miscibility of Methanol (CH3OH) with water (H2O)

o dissolving of oxalic acid in water

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The solubility is tested in different media: water, sodium hydroxide, and hydrochloric acid. The

solubility testing is carried out at room temperature.

If the organic compound is insoluble in water, acid and alkali, therefor, these compounds are

hydrocarbons, nitrohydro-carbon, Alkyl or Aryl halides, esters and ethers. higher molecular weight

Alcohols, Aldehydes and ketones.

Because hydrocarbons are insoluble in water, indicates that a non-polar functional group is present.

Salts are extremely polar and are usually water soluble.

Acids and amines are more soluble than non-polar compounds (due to H-bonding).

Solubility of amines decreases as the basicity decreases. (solubility decreases with the increase in the

number of carbon atoms)

After analysis of the previous tests (preliminary test), further information can be deduced

by performing carefully selected functional group classification tests.

Qualitative tests for Alkanes and Alkenes

I. Unsaturated compounds:

Two common types of unsaturated compounds are alkenes (Example cyclohexene) and alkynes

characterized by the carbon-carbon double and triple bond, respectively, as the functional group.

The two common qualitative tests for unsaturation are the reactions of the compounds with

1. Bromine in carbon tetrachloride.

2. Potassium permanganate.

(a) Bromine in carbon tetrachloride test:

Dissolve the compound and add the bromine and shake. rapid disappearance of the bromine

color to give a colorless solution is a positive test for unsaturation.

(b) Aqueous potassium permanganate test (Bayer test):

The reaction is based on the ability of potassium permanganate to oxidize double bond to diols.

Dissolve the compound and add the potassium permanganate solution dropwise and observe the

result.

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B. Group Classification Tests:

The reagent is potentially dangerous. Keep it off your skin and clothes; protect your eyes and nose

Qualitative tests for Alkyl halides (Halogenated hydrocarbons)

n-Butyl bromide Sec. Butyl bromide Tertiary Butyl bromide

Qualitative tests for alkyl halides are useful in deciding whether the compound in question is a

primary, secondary, or tertiary halide.

Alcoholic Silver Nitrate The overall reaction is shown in the following equation:

Such a reaction will be of the SN1 type. Tertiary halides are more reactive in an SN1 reaction than

secondary halides, which are in turn more reactive than primary halides. Differing rates of silver

halide precipitation would be expected from halogen in each of these environments, namely,

primary < secondary < tertiary. These differences are best determined by testing with silver

nitrate and observing the results.

Add the alkyl halide to solution of silver nitrate, If no reaction is observed within five minutes at

room temperature, warm the mixture and observe any change.

Qualitative tests for Alcohols (R-OH)

The identifying of alcohol is the hydroxyl functional group, -OH bonded to carbon. Alcohols are neutral and are classified into:

1. Monohydric alcoholsThey are almost colourless neutral liquids, alcohols less than six carbon atoms are miscible with water, but more than six carbon atoms are sparingly solublee.g., methyl alcohol, Ethyl alcohol and Tertiary butanol

2. Polyhydric alcoholse.g. glycerol. The poly-hydric alcohols are colourless, neutral, viscous liquids having sweet taste and are soluble in water.

3. Aromatic alcoholse.g. benzyl alcohol, aromatic alcohols are oily colourless liquids, insoluble in water and

The monohydric alcohols are divided to…1. Primary alcohols 2. Secondary alcohols 3. tertiary alcohols

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RX + AgNO3 AgX + RONO2

General class reactions:

The tests for the hydroxyl group not only detect the presence of the group, but may also indicate

whether it is primary, secondary or tertiary.

1- Jones Reagent (CrO 3-H2SO4 in H2O)This reagent distinguishes primary and secondary alcohols from tertiary alcohols; the test

is based on the much greater resistance to oxidation of tertiary alcohols compared to the

other two types.

Dissolve one drop of your alcohol in acetone and add one drop of the jones reagent, and

shake the tube to mix the contents. Primary and secondary alcohols react within two

seconds as indicated by the disappearance of the orange color of the jones reagent and the

formation of a green or blue-green precipitate or emulsion. Tertiary alcohols do not react

even after 3 minutes.

(I) RCH2OH RCHO RCOOH

(II) R2CHOH R2C=O

(III) R3COH no visible reaction.

2- Esterification The esters are flavoring or odor concentrates.

The esters may be formed by the direct reaction of a carboxylic acid with an alcohol.

Such a reaction is called an esterification reaction.

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Methyl alcohol react with Salicylic Acid yield wintergreen odour of methyl Salicylate

Ethyl alcohol react with Acetic Acid yield fruity odour of ethyl Acetate

3- Iodoform test : (Presence of three alpha hydrogens)

This experiment shows how methanol and ethanol behave differently when treated

with iodine solution and sodium hydroxide solution. Ethanol reacts to form a yellow

solid, triiodomethane, often called iodoform.

Dissolve your compound in water; Add NaOH solution and warm, then introduce the potassium

iodide - iodine reagent dropwise with shaking, the test is positive if a yellow precipitate of

iodoform is deposited.

Qualitative tests for Phenols (Ar-OH)

Phenols are a class of organic compounds consisting of a hydroxyl group (-O H ) bonded directly

to benzene ring.

The identification of phenols by

(1) FeCl3 test:

Phenols react with FeCl3 to form a colored complex with the Fe3+ ion. The color varies

from purple to orange depending on the structure of the phenol tested.

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The Secondary alcohols with a CH3 on the carbon carrying the OH (eg propan-2-ol) give positive

iodoform test

OH

FeCl3

O O

O

OO

O Fe3+

Phenol + FeCl3 give violet

Cresol + FeCl3 give blue

Hydroquinine (quinol) + FeCl3 give blue

α-naphthol +FeCl3 give green

β-naphthol + FeCl3 give green

(2) With Chloroform and Sodium hydroxide reaction (formylation)(Reimann-

Timann reaction)

When phenol is react with chloroform and sodium hydroxide and heat gently, a formyl group –

CHO is introduced, and colored polymer formation.

Qualitative tests for Carbonyl compounds (Aldehyde and Ketone)

Identification of carbonyl functional groups:

2,4-Dinitrophenyl hydrazine test (DNP)

(as Brady's reagent),

R R

O

Aldehyde or ketone

+

NHNH2

NO2

NO2

2,4 dintrophenylhydrazine

NHN

NO2

NO2

CR

R

H+

2,4 dintrophenylhydrazone derivativeorange/red precipitate

Transfer two drops of unknown to a small test tube and add 4 or 7 drops of 2,4 DNP reagent and

shake. Formation of a red - yellow precipitate (a positive test) indicates the presence of an

aldehyde or ketone functional group.

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O

R H

O

C C

O

Carbonyl group Aldehyde structureKetone structure

Distinguishing between aldehyde and ketone functional group:

Fehling's solution .

Aldehydes reduce Fehling's solution to yellow or red copper (I) oxide, but ketone do not react.

Identification of presence of CH3CO- group in aldehyde and ketone

Iodoform reaction:

The iodoform test indicates the presence of an aldehyde or ketone in which one of the groups

directly attached to the carbonyl carbon is a methyl group (presence of three alpha hydrogens).

R CH3

O

R O

O

+I2 / -OH HCI3

The nitroprusside ion forms a coloured complex with methyl ketones. In presence of alkali

Example, acetone is converted to CH3COCH2- ion which reacts with nitroprusside ion

[Fe(CN)5NO]2- to give highly coloured ion [Fe(CN)5NOCH2COCH3]2-.

 

The reaction of salicylic acid with formaldehyde in the presence of catalytic amounts of strong

mineral acid (such as Sulphuric acid) results in the condensation product, and polymer formation.

The final polymer is inevitably highly colored (the crimson red color are produced). COOH

OHH H

O

H+2

OHHO

COOHHOOC

Qualitative tests for carboxylic AcidsGeneral Reactions of Carboxylic Acids:

(1) Na2CO3 test:

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Salicylic acid test:

Sodium nitroprusside reaction

They decompose Na2CO3 to CO2 and sodium salt of the corresponding acid (distinction from most

phenols).

R-COOH + Na2CO3 → RCOONa + CO2 + H2O

The warm aqueous Na2CO3 is treated with few crystals (or few drops of acid). Effervescence due

the evolution of CO2 indicates the presence of COOH group.

(2) Ferric Chloride Reaction (fe 3+ complex carboxylic acid):

FeCl3 will indicate the presence of aliphatic acids turning the solution a yellow color. Aromatic

acids will test as a beige-tan color.

For the success of this reaction it is important that the solution should be-neutral. Excess of acid

usually inhibits the production of color or precipitate, and excess of alkali gives gelatinous

reddish-brown precipitate of ferric hydroxide.

To the cold neutral solution of the acid add a few drops of FeCl3, solution and observe the colour

or the ppt. formed.

R COOHFeCl3

R COO3 ( )3 Fe + 3 HCl + H2O

heating

R COO( )(OH)2Fe

Examples

Formic acid is the only one, which possesses both carboxyl and aldehyde groups activities

OH

H

O

OH

H

O

Carboxyl group

Aldehyde group

Formic acid is the only carboxylic acid that reduce Fehling reagent, mercuric chloride and

KMnO4

Mercuric chloride test (HgCl2):

Add mercuric chloride solution to formic acid or a solution of formate and warm. A white ppt. of

mercurous chloride Hg2Cl2, insoluble in dil. HCl, is produced.

HCOOH + 2 HgCl2 Hg2Cl2 + CO2 + 2 HCl

Iodoform Test:

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1- Formic acid, HCOOH

2-Lactic Acid CH3CH(OH)COOH

Lactic acid gives positive iodoform test because it contain the CH3CH(OH) group. This test is

done by adding exess NaOH till alkali and blue litmus to the liquid lactic acid. the add excess

iodine solution and warm gently to give yellow ppt of iodoform.

H3CCH

COOH

OH

H3CC

COOH

O

CHI3

Yellow ppt

NaOH

I2 /

NaOH

I2 /

Action of CaCl2;

When a neutral solution of a tartarate is treated with CaC12 solution a white ppt. of calcium

tartarate is separated on the cold after scratching and stirring

2- Fenton's Reagent: (Oxidation of tartaric acid in the presence of iron)

To a solution of tartaric acid or a tartarate add 1 drop of freshly prepared ferrous sulphate

solution, 1 drop of hydrogen peroxide solution and excess of NaOH solution. An intense violet

colour is produced due to the ferrous salt of dihydroxyfumaric acid, (HOOC-C(OH)=C(OH)-

COOH). This test is positive to tartaric and tartarates only.

CHOH

COOH

CHOH

COOH

Fe(II) Fe(III)

H2O2 OH· + OH-

ferrous salt of dihydroxyfumaric acid

Qualitative tests for salts of carboxylic AcidsCarboxylic acid salt is the salt (RCOO-M+) formed when a carboxylic acid reacts with a base. carboxylic acid salts are ionic compounds and soluble in water

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4-Tartaric acid

Qualitative tests for salts of carboxylic Acids Ester (R-CO-OR - ) Hydroxamic acid test

R-CO-OR' + H2N-OH R-CO-NH-OH + R'-OH

Esters react with hydroxylamine in the presence of sodium hydroxide to form the sodium salt of

the corresponding hydroxamic acid. On acidification and addition of ferric chloride the magenta-

coloured iron (III) complex of the hydroxamic acid is formed.

It is always advisable to ensure that an unknown compound does not give a colour with iron (III)

chloride before carrying out the hydroxamic acid test.

Qualitative tests for salts of Amines Reaction with benzenesulphonyl chlorideBenzenesulphonyl chloride reacts with primary and secondary but not with

tertiary amines to yield substituted sulphonamides.

a) C6H5SO2Cl + H-NHR + NaOH C6H5SO2NHR + NaCl + H2O

b) C6H5SO2Cl + H-NR2 + NaOH C6H5SO2NR2 + NaCl + H2O

The substituted sulphonamide formed from a primary amine dissolves in the alkali medium whilst

that produced from a secondary amine is insoluble in alkali.

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Qualitative tests for salts of Amides (R-CO-NH2) Example: Urea

Action of nitric acid:

When nitric acid is presented, it ionizes. A hydrogen ion [proton] contributed by the acid is

attracted to the oxygen and forms a covalent bond [electrophile H+]. The electronegative NO3- ion

then is attracted to the positive hydrogen ion. This forms an ionic bond and hence the compound

urea nitrate (white ppt).

H2N NH2

O

+ HNO3H2N NH2

OH NO3

Acidity test:

(1) When the Unknown is Liquid In your test tube place 2 ml of the unknown, and then add ½ spatula of Na2CO3 powder.

(2) When the Unknown is Solid In your test tube place 2 ml Na2CO3 Solution and heat it in the water bath, and then add ½ spatula of unknown.

Preparation of the Neutral Solution:

(1) When the unknown is liquid: In small beaker, 5 ml Water+ 3 ml of Unknown + Add Ammonia dropwise until neutralization occur, using the Litmus Paper

(2) When the unknown is Solid (soluble or insoluble in water): In small beaker, 10 ml water, + ½ spatula of the unknown + add 6 drops of Ammonia, and then stir well vigorous.

Solubility and Miscibility tests:

1 ml Unk. (or quarter spatula)+ 3 ml H2O Then shake well….

Brady’s test:(In Dry test tube)

When the Unknown is Liquid2 ml Brady’s reagent+ 3 or 4 drop Unk.

N-FeCl3 test:

1 ml Unk. (or Unk. Soln.)+ add 3 – 4 drops of N-FeCl3 drop by drop(whit and watching the colour)

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If Red L.P (Acidic) ..............................................................add NH3

If Blue L.P (Alkali)…………….…………………………..…add unk.If yellow L.P (neutral) …………………………………….… PH ≈7

For Liquid Unk.if One layer formed………..……………….………....….Miscible with waterif Two layers formed..………… ………………….…..Immiscible with water

For Solid Unk.if soluble in water……………………………….……..…..….Soluble in waterif ppt with vigorous shake ……………………………..…..Insoluble in water

If you have Acidic Unknown, Use its Neutral Soln.

Fehling test:

1 ml Unk.+ 1ml Fehling A + 1 ml Fehling B Then Shake well, and boil in water bath for 5 min.

CaCl2 test:

1 ml Unk. (or Unk. Soln.)+ 2 ml CaCl2

Jones test:

4 – 5 drops of Unk.+ 1 ml of acetone+ 1 ml of jones reagentand shake

KMnO4 test:(for Differentiation between Saturated and Unsaturated hydrocarbons)…

2 ml of unk. + 3-4 drops of KMnO4

Hydroxamic Acid testConfirmatory of ethyl acetate.

0.5 ml of Unk. + 1 ml of hydroxyl amine HCl+ 1 ml of 30% NaOH Then heat in water bath for 5 min

Then cool the test tube and 2 ml of dil. HCl + 2 ml of ethanol+ 2 – 3 drops of 5% FeCl3 Soln.

Chloroform (CHCl3/NaOH) test:For resoncinol and quinol..

One spatula of Unk. (solid)+ 2 ml 30% NaOH+ 2 ml chloroformThen heat gently with shaking.

Sodium Nitroprusside test:(for Differentiation between Formaldehyde and Acetaldehyde)…

1 ml of Unk.+ 2 ml of sodium nitroprusside solutionThen add 10% NaOH in excess

Alkaline KMnO4:Confirmatory of formic Acid(or Formate salts)

2 ml Unk. (or Unk. Soln.)+ 1 ml 10% NaOHWarm in water bath 5 min Then, add 1 ml KMnO4

Conc. HNO3 test:Confirmatory of urea..

1 ml of conc. Solution of the Unk.+ 2 ml HNO3

Fenton testConfirmatory of Tartaric acid and Tartrate salts

1 ml of Unk. soln.+ 1 – 2 drops of FeSO4

+ 1 drop of H2O2

Then shake well Then add 2 ml of 10% NaOH

Salicylic Acid test:Confirmatory of Formaldehyde….

1 ml Unk. + ⅓ spatula salicylic Acid+ add 4 drops conc. H2SO4 (on the wall)

Iodoform test:

(1) For Acetaldehyde 1 ml Unk.+ 1 ml H2O+ 2 ml Na2CO3 solutionBoil in water bath for 3 min, and then add 4 or 5 ml Iodine (I2) soln.

(2) For Acetone 1 ml Unk.+ 1 ml H2O

Basic Radical test : ) for Differentiation between Ammonium and Sodium Salts .…(

Half spatula Unk (solid) +3 ml 30% NaOH

Then shake well

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Change of the Blue into Reddish brown is the +ve test

If you have Acidic Unk., Use the Neutral Soln.

The formed white ppt will dissolve in excess water

Observe the odour carefully If Ammonia odour………………………....... Ammonium Salt. (R-COO- NH4

+)If No Ammonia odour ……………………………....Sodium Salt. (R-COO- Na+)

The Decolourization ≡ the yellow-orange colour of the jones turns green

The Decolourization ≡ the purple colour of the permanganate turns brown

+ 2 ml 10% NaOH solutionBoil in water bath for 5 min, and then add 4 or 5 ml Iodine (I2) soln.

(3) For Lactic Acid 1 ml Unk.+ 2 ml H2O+ 4 ml 30% NaOH Boil in water bath for 5 min, and then add 3 or 4 ml Iodine (I2) soln.

(4) For Differentiation between Methanol and Ethanol1 ml Unk.+ 2 ml H2O+ 2 ml 10% NaOH solutionBoil in water bath for 10 min, and then add 4 or 5 ml Iodine (I2) soln.

Esterification test:

(1) Confirmatory of Alcohols…. 4 ml Unk.+ 1 ml appropriate Acid (or ¼ spatula)+ 3 drops conc. H2SO4, then boil in water bath for 10 min.Then, pour the contents of the test tube on beaker containing Na2CO3 soln.

You will exam the following tests:1. The physical characteristicss of each sample:

The condition: ……solid or liquid……………………..………………….……………………………………………………………..

The colour: …………………………………………………………………………………….………………………………………………………..

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Name: ……………………………………………………………………………………………………..……………….........................................................................................................……….…………………………………………………………………………………… ID: ………………………………………...................................………..………………………………………………… T: …………………....................................………………………………………………

Lab Report:Lab 6Identification

For all Iodoform test:Leave the test tube (stand) for 5 -10 minutes to see the yellow ppt in the bottom

The solubility: ………………………………………………………………………………………………………………………………………..

With Litmus paper: …………………………………………………………..…………………………………………………………………...

2. The chemical tests…

The test The samples observation

1. Solubility test

Soluble sample Insoluble sample Miscible sample Immscible sample

………………………………………………….…………………………………………………..…………………………………………………………………..……………………………………………..……………..…………………………………………………..…………………………………………….……………………………………………………………………..……………………………………………………………....……………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………..……………………………………………….……………………………………………………………..…………………………………………………..……………………………………………………………………………………………………………………………………………………………………………………………………………………………..……………………………………………………………………………………………………………………………………………………………………………..

………………………………………………………………………………………………………………….…………………………………………………………………………………………………………………..

2. Unsaturated test(With KMnO4)

Cyclohexane Cyclohexene

……………………………………………………..……………………………………………..……………..…………………………………………………..…………………………………………….……………………………………………………………………..……………………………………………………………....……………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………..……………………………………………….……………………………………………………………..…………………………………………………..…………………………………………………………

3. Alcoholic AgNO3 test

n-Butyl bromide Tert-butyl bromide

………………………………………………….…………………………………………………..…………………………………………………………………..……………………………………………..……………..…………………………………………………..…………………………………………….……………………………………………………………………..……………………………………………………………....……………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………..……………………………………………….……………………………………………………………..…………………………………………………..…………………………………………………………………………………………………………………………………………………………………………

4. Jones test Methanol Tert-butanol

………………………………………………….…………………………………………………..…………………………………………………………………..……………………………………………..……………..…………………………………………………..…………………………………………….……………………………………………………………………..……………………………………………………………....……………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………..……………………………………………….……………………………………………………………..…………………………………………………..…………………………………………………………

5. Iodoform test Methanol Ethanol Lactic Acid

………………………………………………….…………………………………………………..…………………………………………………………………..……………………………………………..……………..…………………………………………………..…………………………………………….……………………………………………………………………..……………………………………………………………....……………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………..……………………………………………….……………………………………………………………..…………………………………………………..……………………………………………………………………………………………………………………………………………………………………………………………………………………………..……………………………………………………………

6. N-Fecl3 test Resorcinol Formic Acid Lactic Acid Tartric Acid

………………………………………………….…………………………………………………..…………………………………………………………………..……………………………………………..……………..…………………………………………………..…………………………………………….……………………………………………………………………..……………………………………………………………....……………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………..……………………………………………….……………………………………………………………..…………………………………………………..……………………………………………………………………………………………………………………………………………………………………………………………………………………………..……………………………………………………………

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7. Brady’s test Formaldehyde or Acetone non-carbonyl sample

………………………………………………….…………………………………………………..…………………………………………………………………..……………………………………………..……………..…………………………………………………..…………………………………………….……………………………………………………………………..……………………………………………………………....……………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………..……………………………………………….……………………………………………………………..…………………………………………………..……………………………………………………………………………………………………………………………………………………………………………………………………………………………..……………………………………………………………

8. Fehling test Formaldehyde Acetone

………………………………………………….…………………………………………………..…………………………………………………………………..……………………………………………..……………..…………………………………………………..…………………………………………….……………………………………………………………………..……………………………………………………………....……………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………..……………………………………………….……………………………………………………………..…………………………………………………..……………………………………………………………………………………………………………………………………………………………………………………………………………………………..……………………………………………………………

9. Sodium Carbonate test

An acidic sample Non-acidic sample Sodium formate

………………………………………………….…………………………………………………..…………………………………………………………………..……………………………………………..……………..…………………………………………………..…………………………………………….……………………………………………………………………..……………………………………………………………....……………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………..……………………………………………….……………………………………………………………..…………………………………………………..……………………………………………………………………………………………………………………………………………………………………………………………………………………………..……………………………………………………………

10. Basic radical test

Sodium Salt Ammonium Salt

………………………………………………….…………………………………………………..…………………………………………………………………..……………………………………………..……………..…………………………………………………..…………………………………………….……………………………………………………………………..……………………………………………………………....……………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………..……………………………………………….……………………………………………………………..…………………………………………………..……………………………………………………………………………………………………………………………………………………………………………………………………………………………..……………………………………………………………

11. Hydroxamic acid test Ethyl Acetae

………………………………………………….…………………………………………………..…………………………………………………………………..……………………………………………..……………..…………………………………………………..…………………………………………….……………………………………………………………………..……………………………………………………………....……………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………..……………………………………………….……………………………………………………………..…………………………………………………..……………………………………………………………………………………………………………………………………………………………………………………………………………………………..……………………………………………………………

12. Hinsberg test n-butyl amine Tri-butyl amine

………………………………………………….…………………………………………………..…………………………………………………………………..……………………………………………..……………..…………………………………………………..…………………………………………….……………………………………………………………………..……………………………………………………………....……………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………..……………………………………………….……………………………………………………………..…………………………………………………..……………………………………………………………………………………………………………………………………………………………………………………………………………………………..……………………………………………………………

Cyclohexane Cyclohexene n- Butyl Bromide Tertiary Butyl Bromide Methanol

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Ethanol Tertiary Butyl Alcohol Resorcinol Formaldehyde Acetaldehyde Acetone

Formic acid Lactic Acid Tartaric Acid Ethyl Acetate n-Butyl Amine

Tri-Butyl Amine Urea Salts of Acids

Wherw, the M is Cation (Sodium or Ammonium)

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