What is Microscale Chemistry?

Why Microscale Chemistry?

Basic Equipment.

Synthesis of Aspirin.

Synthesis of E –Benzal

Synthesis of Azodyes

Synthesis of 1-Bromo-3-chloro-5-iodobenzene

Separation Of Component Mixture

Microscale chemistry is an environmentally safe pollution prevention method of performing chemical processes using small quantities of chemicals with out compromising the quality and standard of chemical applications in education and industry.

The best way to succeed in this effort is by eliminating chemical waste at the source. Reduction of chemical use to the minimum level at which experiments can be effectively performed

Microscale Chemistry is performed by using:

1-Drastically reduced amounts of chemicals2-Safe and easy manipulative techniques

3-Miniature labware and high quality skills

Microscale Chemistry amounts to a Total Quality Management (TQM) approach to the use of chemicals.

Microscale Chemistry is recognized as Small scale Chemistry by the International Union of Pure and Applied Chemistry

Microscale Chemistry offers many benefits:

It reduces chemical use promoting waste reduction at the source.It offers vastly improved laboratory safety by Better Laboratory Air Quality.Least Exposure to Toxic Chemicals.No Fire and Explosion Hazards.No Spills and Accidents.It sharply reduces laboratory cost.It requires shorter experiment time.It implements excellent lab manipulative techniques.It lowers glass breakage cost.It saves storage space.It improves laboratory skills.It provides clean and productive environment.It promotes the principle of 3Rs: Reduce, Recover&Recycle.It creates the sense of 'Green Chemistry'.It is user friendly to people with physical disabilities.

1- CONICAL VIALS:

•These take the place of large, round-bottom flasks used in the traditional laboratory.

• It is used as a reaction vessel, for extractions, and as a storage container.

2- CONDENSERS:

•Air Condensers: These are glass tubes with an inner joint at the bottom and an outer joint at the top. They are usually attached to a reaction vial (conical vial) and used to prevent vapors from escaping from a hot or boiling reaction

•Water-cooled or Jacketed Condensers: These serve the same purpose as the air condensers, except that cooling is made more efficient by circulating cold tap water through an outer glass jacket. Water goes into the bottom connector and out the top to prevent trapping air in the water jacket. For lower-boiling liquids, this additional cooling is necessary to prevent the escape of vapors.

3-RECRYSTALLIZATION TUBES:

Craig Tube: The Craig tube is used for small-scale recrystallization, which is a

method for the purification of small quantities of solid compounds.

It has two parts: an outer body, which functions like a vial or test tube; and an inner plunger, which fits partly into the

body and rests on a ground-glass surface.

The ground-glass joint is not greased, so that liquids can leak through it but solids

cannot pass.

4-DISTIALLATION HEADS:Claisen Head

Hickman

Head

Claisen Head or Claisen Adaptor: allows introducing chemical reagents (usually liquids) into a reaction mixture without taking apart the whole apparatus.

Hickman Distilling Head: The purpose of a still is to heat a liquid until is passes into the gas

(vapor) phase, and then allow the vapor to cool and condense back into the liquid phase, with

the condensed liquid trapped in a second container.

The Hickman still functions like the air condenser in condensing vapors with the cool glass

surface, but the liquid drips down the inside to be trapped in a small circular depression, or

collar, in the lower part of the tube.

5-DRYING TUBE:

The tube is used to protect the reaction from moisture in the atmosphere while still allowing the passage of air to equalize pressure. To accomplish this the tube is packed with a glass wool plug, a quantity of moisture-absorbing solid (the "drying agent"), and another glass wool plug.

The flat, long blade can be used to weigh out solids, stir mixtures, remove "O" rings, scratch glass surfaces to induce crystallization

6-MICRO-SPATULA:

•Disposable Pasteur pipettes: are used for dispensing small quantities of liquids, as filtration devices, and as columns for small-scale column chromatography.

•A Filtering Pipette: is used to remove solid impurities from a liquid with a volume less than 10-mL. To prepare it, a small piece of cotton is inserted into the top of a Pasteur pipette and pushed down to the beginning of the lower constriction in the pipette.

•A Filter-tip Pipette: is useful for transferring volatile solvents during extractions and in filtering very small amounts of solid impurities from solutions.

7-PIPETTES:

BACKGROUND:

•Aspirin is the trade name for the molecule acetylsalicylic acid The earliest known use of this molecule has been traced back to the fifth century B.C.

• The Greek physician Hippocrates described an extract of willow tree bark, a bitter powder that could be used to reduce fevers.

• In 1829, Salicin was isolated from willow bark and used as a pain reliever. Unfortunately Salicin was not very popular since it was found to be very acidic and a stomach irritant.

• In 1897 a German chemist named Felix Hoffman was working for the Bayer chemical company. Hoffman was looking for a less acidic pain reliever that his father could take for his arthritis.

•His research led to the synthesis of acetylsalicylic acid (ASA) or aspirin.

•Today 80 billion aspirin tablets are consumed every year across the globe to reduce fevers,relieve pain, and even help prevent heart attacks.

BACKGROUND (Cont.):

In commercial aspirin products, a small amount of ASA (300 to 400 mg) is bound together with a starch binder and sometimes caffeine and buffers to make an aspirin tablet. The basic conditions in the small intestine break down the ASA to yield salicylic acid, which is absorbed into the bloodstream. The addition of a buffer reduces

the irritation caused by the carboxylic acid group of the aspirin molecule.

Aspirin can be produced in a one step chemical process by reacting salicylic acid with acetyl chloride, according

to the reaction:

Aspirin is a white solid that is almost completely insoluble in water. We will use this physical property of our product to separate it from the final solution.If time allows, we will synthesize methyl salicylate, which is another ester of salicylic acid. It occurs in a wide range of plants and is known as ‘oil of wintergreen’.It is still used in candies and in ointments for joint and muscle pains. Salicylic acid methanol Methyl salicylate (wintergreen).

Thin layer chromatography (TLC) is used to separate and identify aspirin.

• Safety Notes:

• 1. The acetyl chloride and pyridine should only be dispensed in a hood.

• 2. Always wear appropriate eye protection and gloves while handling the chemicals.

Safety Notes:1. The acetyl chloride and pyridine should only be dispensed in a hood.2. Always wear appropriate eye protection and gloves while handling the chemicals.

Materials:Materials:

Procedure:Procedure:

1. Place 150 mg (0.001 mol) of salicylic acid in a 10 mL test tube and add 0.1 mL of pyridine (just sufficient to dissolve it) while the tube rests in a ice-cold water bath. Keep the test tube in a hood while you are doing this.

2. For the next step, be sure that the open end of the tube is not pointing toward you or anybody else. Occasionally the reaction goes quickly and shoots material out of the tube! Add one-tenth milliliter of acetyl chloride (slight excess over 0.001 mol )in one portion to the test tube. Again, keep the mixture in a hood!

3. The mixture becomes viscous at this stage. Let the mixture sit in a beaker of cold water bath for 15 min. – it does not need to be in the hood. While waiting, set up a vacuum filter flask with a Buchner funnel and a piece of filter paper which just fits the bottom of the funnel

4. Now add 5 mL of cold water to the test tube and cap it with a rubber stopper. Shake the mixture. Do this cautiously at first until you are sure that no violent reaction is occurring. The mixture should turn cloudy. Shaking is continued until a white product appears (it may takes several minutes, be patient!)

5. Turn on the water faucet all the way and check to be sure you have good suction. Break the suction by disconnecting the tube from the flask (leave the water running). Pour the mixture into the funnel,trying to get as much of the solid transferred as possible.Connect the hose and apply full suction for at least 30 seconds.Wash the crystals with cold water.Break the suction.Do not just turn off the water; Dry them on the filter paper for about 5 min.

Part B- Recrystallization6. Carefully scrape off most of your crystals into a 50 mL beaker. SAVE THE FILTER PAPER! Add about 3 mL of cold water and place the mixture on a hot plate in a hood.Heat until all of the crystals dissolve (check with the instructor if complete solution does not seem to be happening.) When the crystals are completely dissolved in the hot solution, remove the beaker and allow it to cool. You should see nice crystals of aspirin beginning to form! When the recrystallization is complete, filter again, and dry.SAVE THE FILTER PAPER for the next step!Part C- Oil of Wintergreen1. Place 1.00 gram of salicylic acid in a test tube. (record the actual mass used)2. Add 5 ml of methyl alcohol and 3 drops of concentrated sulfuric acid.3. Heat this mixture in a boiling water bath for 15 min.4. Note the odor of the liquid in your tube.

Procedure (cont’d):Procedure (cont’d):

1. Benzaldehyde(FW106.1) 208mg(2m mole )

2. Hydroxyl amine hydrochloride (FW69.5) 189mg(2.4m mole)

3. Sodium hydroxide pellets 140mg (3.5m mole)

4. Ethanoyic acid

5. Diethyl ether

Reagents:Reagents:

Safety Notes: Benzaldehyde is irritant,Hydroxyle amine hydrochloride is corrosive,Sodium hydroxyle pellets is corrosive & hygroscopic,Ethanoyic acid is corrosive,Diethyl ether is flammable & irritant.

Procedure:Procedure:

VIAL e’ 0.12 ml water

NAOH

COOL

1-Benzaldehyde

2-hydroxylamine hydrochloride

Stir vigorously

Neutralize the mixture by the addition of ethanoic acid

extracting with diethyl ether Dry with MgSO4

1-Dissolve NaoH in water(0.12ml ) in 1ml reaction vial containing a spin value allow the solution to cool and add ca. 0.02ml of the benzaldehyde followed by ca. 20mg hydroxylamine hydrochloride .

2-Stopper the flack and stir vigorously, briefly stopping the stirring at 5min interval to add further position of benzaldehyde &hydroxylamine until both reagents have been added completely.The reaction mixture will become warm giving a homogenous solution with almond odor indicating the total consumption of the benzaldehyde.

3-Neutralize the mixture by the addition of ethanoic acid &allow the mixture to cool before extracting with diethyl ether.

4-Separate the organic extracts, dry by passing through a column of MgSo4 into a preweighed reaction vial and remove the solvent then record the yield of the product.

The reactions are:

1-Diazotization:

NH2

H c l/N a N o 2

< 5 °C

N+

N cl

2-Coupling:

azo dye

Procedure:Procedure:1-Put eight drops of aminobenzene in a 10 cm3 beaker and add 30 drops ofdeionised water followed by 15 drops of concentrated hydrochloric acid. Swirlthe beaker and then put it in an ice bath.

2-Weigh 0.15 g of sodium nitrite into another beaker and add 1 cm3 of deionisedwater. Cool the beaker in the ice bath. Add one spatula of urea (this preventsside reactions occurring).

3-Mix the contents of the two beakers together and keep in the ice bath.

4-Weigh 0.45 g of 2-naphthol into another beaker and add 3 cm3 of sodiumhydroxide solution. Swirl to dissolve.

5-Take a piece of cotton cloth 2 x 2 cm2 and, using tweezers, dip it into the2-naphthol solution. Allow the solution to completely soak the cotton.

6-Dip the cloth completely into the diazonium salt solution. A red dye forms inthe fibers, dyeing the cloth.

An Improved Deamination of 4-Bromo-2-chloro-6-iodoanilineNH2

Br

Cl

IBr

Cl

Iiso a m yl n it ra t e

D M F

Reductive deamination step---the final step

Br

NH

O

CH3

N a c lo 4

Br

Cl

NH

O

CH3

1 )H c l,C H 3 C H 2 O H

2)50%NaOH

NH2

Cl

Br

IC IC H 3 C O 2 H

NH2Cl

Br

I1 ) Iso a m yl n it r it e

D M F ,6 5 °C

2 )H C L ,H 2 O

ClI

Br

1-Under a fume hood, 1.65 mL of a 0.75 M isoamylnitrite_DMF solution is added to a 10-mL round-bottomedflask containing a magnetic spin vane.

2-A reflux condenser is placed on the flask and the flask is clamped in a sand bathheated to 65◦C.

3-With the isoamyl nitrite solution stirring rapidly, a solution of 4-bromo-2-chloro-6-iodoaniline (0.25g, 0.75 mmol) dissolved in a minimal amount of DMF (2mL) is added dropwise to the reaction solution over a period of 5 min.The evolution of nitrogen gas is immediate and continues until all of the aniline solution is added.

4-After the gas evolution is complete (15 min), the reaction mixtureis allowed to cool to room temperature and then carefullytransferred to a 25-mL Erlenmeyer flask.

5-15mL of 20% aqueous hydrochloric acid solution is added to thereaction mixture and the product is extracted from the reactionmixture into two, 10-mL portions of ether.The combinedorganic extract is washed with 15 mL of 10% aqueoushydrochloric acid solution, dried over anhydrous magnesiumsulfate, filtered, and concentrated to yield the product as apale copper-colored solid.

6-The crude product is recrystallized from methanol, using a ratio of 6 mL of methanol per gram of product, to give 1-bromo-3-chloro-5-iodobenzeneas long, colorless needles (75–80%, m.p. 85–86 ◦C).

Procedure:

Liquid-liquid extraction is one of the most used methods for isolating an organic compound from a mixture.This technique is commonly used to isolate and purify products from chemical reactions and is also used to isolate natural products.The process can be categorized into two types of liquid-liquid extraction:

-The first type takes advantage of the polarity of compounds and uses water to extract or “wash” an organic mixture by removing highly polar materials, such as inorganic salts, strong acids or bases, etc.

-Second, acid and base extraction, takes advantage of chemical properties of compounds.

Acid extractions are intended to separate basic compounds from an organic mixture. Organic bases, amines, are converted to their corresponding cationic salts by reacting with acids. These salts are then soluble in water and can be separated from the organic mixture.

 

HClN(CH2CH3)3 N(CH2CH3)3H

Cl-

cationic salt/water-soluble

 

Base extractions have a concept similar to acid extractions. They are intended to separate acidic compounds from an organic mixture. Organic acids, carboxylic acids, are converted to their corresponding anionic salts by reacting with bases. These anionic salts are usually soluble in water and can be extracted from the organic mixture.

 

RCO2HNaOH

RCO2 Na

Anionic salt/water-soluble

 

Purpose:

In this experiment you will be given a three-component mixture, an acid (benzoic acid), a base (ethyl- 4-aminobenzoate) and a neutral organic compound (9-fluorenone). You will have to separate these three compounds individually from the mixture

C

OO H

C

OO CH2CH3

NH2

O

 

benzoic acid ethyl-4-aminobenzoate 9-fluorenone

•-Weigh approximately 300 mg of the three-component mixture, which contains 100 mg of each: amine, carboxylic acid and neutral.

•-Place the solid into a 5 mL conical vial and add 2 mL of diethyl ether.

•-Top the vial with a teflon disk (slippery teflon side facing in) secured with a screw cap and thoroughly shake its contents until the sample dissolves.

•-To this solution add 1 mL of 3M HCl.

Procedure:

Procedure: (cont’d)Procedure:

1. Cap the vial and thoroughly shake its contents to complete the reaction that selectively converts the amine to its water-soluble cationic salts.

2. Allow the layers to settle in a beaker of ice. Carefully transfer just the bottom (water) layer to a 3 mL conical vial using a Pasteur pipet. To the smaller vial add 1 mL of pure ether, cap and shake the vial. Transfer just the lower layer from this vial to a 10 ml beaker.

3. Add 6 M NaOH to this beaker until the solution is basic to pH paper. The appearance of a white cloudiness indicates the reformation of the amine, ethyl-4-aminobenzoate.

4. Transfer the basic solution into a 5 mL conical vial. Add 1mL of diethyl ether, cap and shake its content.Allow the layers to settle and separate the two layers.Remove the bottom layer and place it in the same 10 mL beaker.Remove the top layer and transfer it to a 10 mL Erlenmeyer flask.Extract the aqueous bottom layer two more times with 1 mL diethyl ether each.

Procedure (cont’d):5-Combine the organic layer, dry the organic layer with Na2SO4[i][1] and

evaporate solvent on the steam bath.3  6-The yellow ether solutions remaining in the vials are recombined into the

5 mL vial. Add 1 mL of pure water, shake its content and then allow the layers to settle. Remove and discard the bottom aqueous layer.

 7-Add 1 mL of 3 M NaOH into the 5 mL conical vial that has the yellow ether

solution (benzoic acid and 9-fluorenone).  8-Cap and thoroughly shake the vial to allow completion of the reaction and

the dissolution of the compounds in their respective solvents. Allow the layers to separate.

 9-Carefully transfer the bottom layer to a 3 mL conical vial using a Pasteur

pipet.To the 3 mL vial add one ml of diethyl ether.Cap and shake its contents.As before, transfer the lower layer, this time to a 10 mL beaker.By now the contents of the beaker should be very pale or colorless.

10-Add dropwise 6 M HCl to the beaker until the mixture is acidic to pH paper.  11-Transfer the acidic solution into the 5 mL conical vial and extract the aqueous solution three times with 1 mL of diethyl ether each. Combine the diethyl ether layers and dry over Na2SO4.  12-Combine the previous left yellow ether layers into a 5 mL conical vial. Add 1 mL of water, cap and shake its contents. Remove and discard the water layer with a pipette. Dry the organic layer with Na2SO4 and evaporate the ether on the steam bath.

 

Procedure (cont’d):

Summary of the procedure:

By Na2SO4

In 5 ml vial

In

beaker

using a Hirsch funnel

adding 1 mL of deionized

water

Conclusion:

The benefits of microscale are perhaps greatest for biology & biochemistry majors as microscale borrows techniques which are have been standard in biochemistry for years also,converting to microscale is one of the best ways to deal with the problem of chemical wastes in academic labs.

The bottom line : Microscale is a cost effective, productive and pollution prevention program.