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Polymerisation, Esterification, Saponification - Coggle Diagram
Polymerisation, Esterification, Saponification
Esterification
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This is the production of an ester by the reaction between an alcohol and a carboxylic acid. Water is produced as a by-product so this reaction is sometimes called a condensation/dehydration reaction. Concentrated H2SO4 is used as a catalyst
Reflux
reactants are heated in a flask w/ a cooling condenser attached to the top of the flask vertically - allows for the continuous boiling of the reaction mixture w/out loss of reactants or products
As all of the reactants and products are volatile (easily converted to a gas) this ensures that they fall back into the flask instead of being released into the environment
Safety
Some organic compounds have very strong odours that can be unpleasant.
Some are hazardous to your health, they may cause headaches and irritate the respiratory system. Many are flammable, so would be a fire hazard if released into the environment. The concentrated H2SO4 is extremely corrosive
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Saponification
Formation of soap molecules, base catalysed hydrolysis of esters
Base hydrolysis of an ester is used to produce soap. The ester used in this case is usually a triglyceride (long chain fatty acid, joined by an ester link to glycerol)
Soaps are usually formed from fats and oils. The chemical reaction is the hydrolysis (addition of water) of triglycerides in basic conditions. The products that are formed are glycerol and a salt (which is used to make soap)
Synthesis of soaps
Boiling a fat or oil with NaOH, using ethanol as a solvent to allow both substances to combine (non-polar and polar)
Soap curdles and forms a solid that can be scraped, dried and pressed
Soap ions are forced to precipatate by washing the solution in concentrated brine (salt) = salting out
Soaps
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The hydrocarbon tail is non polar (hydrophobic) and will bond to other non-polar substances (dispersion forces)
The ionic head is polar (hydrophilic) due to the presence of the carboxylate ion (COO-) and will form ion-dipole bonds with water
Soaps and Detergents
Used as cleaning products due to their ability to remove dirt, oil and stains
They lower the surface tension of the water when dissolved. They break the hydrogen bonding between the molecules and the water spreads out onto the surface, rather than remaining in a droplet.
Changes the surface area, allowing it to attach on and drag it across the surface
A liquid will wet a surface if there is strong intermolecular attraction between the liquid and the surface. A liquid will bead on the surface if there are strong cohesive forces within the liquid, rather than between the liquid and the surface
Detergents
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Detergents replaced soaps, since soaps find it difficult to make a lather in hard water
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How they work
surround the dirt (oil/grease/stain) with their hydrophobic tails forming dispersion forces - allows the hydrophilic head to bound with the water molecules
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Miscelles
When the water is agitated the water molecules pill on the soap (ion-dipole) which lifts the dirt away from the surface
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Polymerisation
Addition Polymers are long chain molecules formed from an addition reaction of one or more unsaturated monomer
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