Butanol And Ethanoic Acid

This reaction is spontaneous for almost all esters but can be very slow under typical conditions of temperature and pressure. The reaction occurs at a much faster rate if there is a significant amount of base (OH-) in the solution. In this lab experiment, the rate of this reaction will be studied using an ester called para-nitrophenyl acetate (PNA), which produces an alcohol,

The Hydroxyl group on alcohols relates to their reactivity. This concept was explored by answering the question “Does each alcohol undergo halogenation and controlled oxidation?” . Using three isomers of butanol; the primary 1-butanol, the secondary 2-butanol and the tertiary 2-methyl-2-propanol, also referred to as T-butanol, two experiments were performed to test the capabilities of the alcohols. When mixed with hydrochloric acid in a glass test tube, the primary alcohol and secondary alcohols were expected to halogenate, however the secondary and tertiary ended up doing so. This may have been because of the orientation of the Hydroxyl group when butanol is in a different

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.

At room temperature (25°C), esterification reactions are relatively slow, therefore requiring the rate of the chemical reaction to be increased for the products to be formed efficiently. This is implemented, by using a catalyst, such as concentrated sulphuric acid (H2SO4 (aq)), as well as by heating the mixture: using a heating mantle. As a result, the energy of the reactants can be greater than the activation energy, increasing the rate of reaction. Hence, as the reactants are relatively volatile, so reflux apparatus such as a pear-shaped flask and a Liebig condenser were used, to minimise the amount of reactants lost, as well as allow the reaction to take place at the highest temperature possible. In addition, boiling chips were added prior to reflux, to prevent bumping and a decrease a loss of volatile reactants, during the reflux

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.

GC shows me peaks and to identify them we use polarity. In the experiment, we used a non-polar column. 1-bromobutane is a colorless liquid that is insoluble in water and is a non-polar. Non-polar compounds leave longer retention time and polar compound leaves shorter retention time. My GC shows me peaks with high intensity with a longer retention time at 4.437 because that a higher intensity and a longer retention time we knew that that peak belongs to my 1-bromobutane. 1-butanol was also present in my GC because is more polar leaves a short retention time there before the peak that belongs to 1-butanol is at 3.762 retention time

The products of interest within this experiment are 2-methyl-1-butene and 2-methyl-2-butene from sulfuric acid and phosphoric acid catalyzed dehydration of 2-methyl-2-butanol. The reaction mixture was then separated into its separate alkene components by steam distillation and then analyzed by gas chromatography (GC), Infrared Radiation (IR) spectroscopy, and Nuclear Magnetic Resonance (NMR) imaging. Gas chromatography is an analytical technique that is able to characterize if specific compounds exist in a reaction mixture, even if they are in low quantities, assess how much of a compound exists within a reaction mixture relative to other components within the sample, and determine the purity of an isolated product. In the case of this experiment, gas chromatography is used to analyze how pure the alkene reaction sample was and if any remnants of impurities or 2-methyl-2-butanol remained in the sample after isolation of alkene components.

The purpose of this experiment is to prepare isopentyl acetate by direct esterification of acetic acid with isopentyl alcohol. After refluxing there is an isolation procedure where excess acetic acid and remaining isopentyl alcohol are easily removed by extraction with sodium bicarbonate and water. The ester is then purified by simple distillation and the IR is then obtained.

Based on the lab’s results, lipids are soluble in both Acetone and Methanol. However, they are more soluble in the Acetone, and only slightly soluble in the Methanol. Because of the chemical structures, this makes sense, since lipids are insoluble in polar solvents (like methanol), but are very soluble in non-polar organic solvents, such as acetone (Hunt).

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.

Stationary phase in HILIC are required to be polar, and water can act as a stationary phase. The stationary phase is more polar than the mobile liquid, and these two liquids must be immiscible with each other. By the process of partitioning between the water molecules in the stationary phase and any solvent used as the mobile phase, separation of the analytes can occur. The different solubilities of the components in the mobile phase and different adsorption forces is what causes the process of partitioning to occur and bring out separation. Separation occurs when the mobile phase consists of a water miscible organic solvent such as acetonitrile and to promote hydrophilic interactions between the analyte and the water stationary phase.

In short, this signifies that water's polarity allows it to dissolve other polar substances with ease. So that when a polar substance is put in water, the positive ends of its molecules are attracted to the

Each of the co-solvents have hydroxyl groups that allow them to hydrogen bond with water, accounting for their miscibility with water. To some extent the hydroxyl groups also allow the solvents to hydrogen bond with the carbonyl and hydroxyl groups of paracetamol (Appendix I). Because of the stable hydrophobic aromatic ring in paracetamol, it would better dissolve in more non-polar solvents. Thus ethanol, with only one polar hydroxyl group, is the most effective solvent. Propylene glycol has two hydroxyl groups and glycerol has three, slightly reducing each solvent’s ability to dissolve paracetamol. Sucrose (syrup) has eight hydroxyl groups which may explain its minute effect on improving paracetamol

Water is one of the most common solvents used in the world. We found that when mineral oil (decane) is added to water the two repel each other and separate, leaving the oil on the surface of the water. Water is polar and decane is nonpolar and because opposites do not attract the decade does not dissolve not the water. When isopropyl alcohol is added to water it formed little sting like structures as it dissolved. Both the solvent and solute are polar which is why the alcohol dissolved so nicely into the water. When copper (II) chloride was added to the water it turned a bright blue-green colour, but did not dissolve. This is because copper (II) chloride is an ionic compound and the forces of attraction holding it together are stronger than the force of attraction between water and the positive and negative ions. The coconut oil did not dissolve when added to the water because coconut oil is very nonpolar, so the water could not pull apart any of the positive or negative sides. When the glucose was added to the water, it dissolved immediately. The glucose is polar and so is water, so the water will pull the slightly positive and negative sides decomposing the crystals.

Water is a great solvent. According to the article it says, “ Water is an excellent solvent.”Many different types of materials can dissolve in water - forming solutions. Water is the solvent that transports many essential molecules and other particles around the body. These include nutrients and waste products from the body's metabolic processes. Water is known as the universal solvent due to a greater number of substances that disintegrate in water than in some other compound. This needs to do with the extremity of each water particle. The hydrogen side of each water (H2O) particle conveys a positive slight electric charge while the oxygen side conveys a negative slight electric charge. This enables water to separate ionic mixes into their positive and negative particles. The positive piece of an ionic compound is pulled in to the oxygen side of water while the negative part of the compound is pulled in to the hydrogen side of the water.