Water Is Water Much More Polar Than Isopropyl Alcohol

Next, aspirin was extracted from the filtrate. When the filtrate was first mixed with the sodium hydroxide and inverted a couple times, an organic layer formed underneath an aqueous layer in the separatory funnel. Dichloromethane was present in the organic layer because it has a higher density than sodium hydroxide, therefore, it’s in the bottom layer. Aspirin reacts with bases like sodium hydroxide, and it forms the salt sodium acetylsalicylate. The polar salt molecules migrate from the organic layer, where they are insoluble, to the aqueous layer, where they are soluble. After the two layers were separated into two different containers, the aqueous layer, which contained sodium acetylsalicylate, was mixed with hydrochloric acid. A white, cloudy precipitate formed, which was a purer form of the salt. The HCl

During the halogenation reactions of 1-butanol, 2-butanol, and 2-methyl-2-propanol, there is a formation of water from the OH atom of the alcohol, and the H atom from the HCl solution. The OH bond of the alcohol is then substituted with the Cl atom. Therefore all of the degrees of alcohol undergo halogenation reactions, and form alkyl halides as products. This is because the functional group of alkyl halides is a carbon-halogen bond. A common halogen is chlorine, as used in this experiment.

Of the alcohols tested 1-Butanol was found to contain the strongest intermolecular forces (IMF) of attraction, with Methanol containing the weakest. It was discovered through experimentation that Methanol induced the highest ?T of all alcohols tested, and that conversely 1-Butanol induced the lowest ?T. The atomic structure of all four alcohols is very similar, as starting with 1-Butanol a CH2 group is lost as you move from 1-Butanol to 1-Propanol to Ethanol and then again to Methanol. Each structure is fairly linear and contains an H-bond with Oxygen, so the real change is found in the loss of the CH2 group, this lowers the liquid’s Molecular Mass, thus lowering the London forces as you move from 1-Butanol through

A salt crystal dropped into a beaker of water becomes smaller and eventually seems to disappear. However, the same salt crystal remains intact at the bottom of a beaker of octane because Sodium Chloride is ionic and would get attracted to the water. The octane is hydrophobic and has nothing for the salt crystal to bond with. The water is polar and hydrophobic, which gives the salt the ability for the oxygen atoms in the water to be attracted to the Sodium ion, and the hydrogen atoms to the chloride ion.

Water (H2O) is a good solvent because it is partially polarized. The hydrogen ends of the water molecule have a partial positive charge, and the oxygen end of the molecule has a partial negative charge. This is because the oxygen atom holds on more tightly to the electrons it shares with the hydrogen atoms. The partial charges make it possible for water molecules to arrange themselves around charged atoms (ions) in solution, like the sodium (Na+) and chloride (Cl−) ions that dissociate when table salt dissolves in water.

in general is more hydrated and doesn’t react or process the alcohol as quickly. Thus

As a result of the water molecule bond, each (hydrogen; oxygen) has a slightly negative charge and each (hydrogen; oxygen) has a slightly positive charge.

The purpose of this experiment was to synthesize t-pentyl chloride from the reaction of t-pentyl alcohol and concentrated HCl. This reaction occurred through an SN1 reaction, a unimolecular nucleophilic substitution reaction. This was a First Order Rate Reaction where the rate of t-pentyl chloride was dependent only on the concentration of t-pentyl alcohol. After the reaction was completed, the products were achieved via 3 liquid-liquid extractions and then after by simple distillation. In the liquid- liquid extractions a solute was transferred from one solvent to another. Then in the simple distillation the miscible liquids or the solution, was separated by differences in boiling points. After this the product was determined through infrared spectroscopy.

2) Explain your result of miscibility / immiscibility for water and diethyl ether. Make use of the concepts of polarity and of the

Hence the boat conformer is able to dissolve in water but stabilizes soon and turns into the chair conformer making it non-polar and separating it from water.

The purpose of this experiment is to determine the nucleophilic strength of chloride and bromide ions as it reacts with 1-butanol (n-butyl) and 2-methyl-2-propanol (t-butyl alcohol) under SN1 and SN2 conditions.

The eluting solvent passed down the column by the gravity and an equilibrium was established between the solute absorbed by the absorbent (silica gel in this experiment) and the eluting solving flowing down. Since the components in the sample had different polarity and they interacted with the stationary phase and the mobile phase differently, the components would be carried by the solvent to a different extent and a separation of the components could be achieved.

When sodium carbonate was added to the separating funnel, effervescence occurred, inferring the release of carbon dioxide gas as a product of the neutralisation reaction. As the process continued, pressure built within the separating funnel, so it was vital to open the tap, after continuously inverting it.

Glycerol is ranked higher than water because it is more polar than water due to it having a stronger intermolecular force and it’s also being more viscous. Water is ranked higher than Isopropyl Alcohol because the water is harder to separate while the isopropyl alcohol is looser. But also the water is more polar than the isopropyl alcohol because the water does not have non-polar carbon-carbon

An alcohol bath was prepared with an ethanol solution and dry ice, the solution was measured using a thermometer, at approximately -15˚ the bath was placed under a Polaroid filter and above a stable jar upon a white piece of paper. The capillary level holder with the frozen capillary tubes was placed carefully into the bath (at an angle to reduce effervescence). A lamp was placed 20 cm away from the setup and shone on the Polaroid filter. This setup ensured the ethanol solution didn’t heat up too rapidly.