To What Extent Do You Predict That The Boiling Point Of Glycerol

The products of the primary alcohol reaction, 1-butanol and HCl, are 1-chlorobutane and water; products of the secondary alcohol, 2-butanol and HCl are 2-chlorobutane and water; products of the tertiary alcohol, 2-methyl-2-propanol are 2-methyl-2-chloropropane and water.

Of the two alkane liquids studied n-Hexane was determined to have the stronger IMF of attraction by virtue of its experimentally determined lower ?T. Conversely n-Pentane has weaker IMF of attraction due to its larger ?T. As explained at length above, this is because it takes more energy to excite a molecule in liquid to leave (vaporize or become gaseous), when there are stronger IMF of attraction holding the molecules together in liquid form.

Attractions between water and other molecules, which is adhesion, is also possible because of the polarity as well. In relation to hydrogen bonds, water’s high specific heat is changed when hydrogen bonds are made or broken. When a hydrogen bond breaks, heat is absorbed whereas when a hydrogen bond forms, heat is released. In addition to HSH, ice is able to float in liquid water because hydrogen bonds in ice is more structured than in water, making the ice less dense. Also, water is a versatile solvent because of its polarity, which helps it form hydrogen bonds (mentioned above). The structure of water molecules also affects the dissociation of water, where H2O breaks into H+ and OH- due to the polarity of the

Benzophenone was soluble in methyl alcohol whiles biphenyl was partially soluble. Benzophenone and biphenyl are both nonpolar molecules. Methanol is intermediately polar, allowing both nonpolar molecules to be dissolved as it is not too polar or nonpolar. However, biphenyl is less polar than benzophenone. Since methyl alcohol is somewhat polar, the more polar benzophenone is more soluble in methyl alcohol than biphenyl. Also, benzophenone can make hydrogen bonds. Thus, benzophenone is more soluble in methyl alcohol than

I hypothesize that salicylic acid will react with acetic anhydride to produce acetylsalicylic acid (aspirin) and acetic acid (vinegar).

6. The solubility of the solids were tested using a micro tray, by placing them in water and oil to observe their polarity,

Substance A and B were weighed; Substance A weighed 0.502 g and substance B weighed 0.503 g. Both substances were put into two different test tube with approximately 8 ml of DI water into the test tub. Substance A and B were stirred and B dissolved while A did not. This shows that B is soluble in water compared to A. Thus, shows that B is soluble in water than A. The reason why B is soluble in water is because it has a higher dipole moment than A. With a higher dipole moment, it shows that it is soluble in water since it is polar and the bonds were easily broken.

By identifying the solubility of the unknown, it could lead to a closer interpretation as to what the functional group the unknown may be. Solubility is determined based on intermolecular attractive forces, such as hydrogen bonding, dipole-dipole, and London dispersion forces. Intermolecular attractive forces arise due to different electron environments in different molecules. For example, water molecules are good at dissolving

A biomolecule can dissolve in water if it can form significant non-covalent interactions with the solvent molecules.

In this experiment, trimyristin will be extracted from ground nutmeg the reflux, filtration, and recrystallization methods. The conducted experiment abides by two parts: the extraction of the nutmeg using methylene chloride, and the recrystallization of trimyristin. The goal of the experiment is to yield trimyristin with high purity. List of Techniques: • Reflux (Condensation of vapors and the return to the condensed state.)

Non-polar covalent bonds cannot dissolve in water because all that the water can do is try to attract the non-polar molecules, but it will only result in a strong hydrogen bond. In addition, since the solvent’s (polar) and solute’s (non-polar) polarity are unalike from each other, that also indicates that it will not dissolve. Also, the non-polar molecules lack positive and negative ends (dipoles), making it hard to form bonds with the water molecules. The reason why non-polar compounds have very low melting points as their only intermolecular force that they posses is London dispersion, which only requires a little amount of energy to split the bond; seeing how electrons in a London dispersion force are distributed all around the nucleus, this factor provides one side of the molecule with more electron density than the opposite side. Just like polar molecules, non-polar bonds cannot conduct electric current as non-polar compounds lack a charge when they are in their molten or solid forms.

A - With couple of special cases (e.g., deoxyribose), monosaccharides have this equation: Cx (H2O) y, where customarily x ≥ 3. Monosaccharides can be ordered by the number x of carbon particles they contain: triose (3) tetrose (4), pentose (5), hexose (6), heptose (7), etc. whereas glycerol is prochiral as for responses of one of the two essential alcohols and it is a basic polyol compound. The number of carbon and hydrogen atoms are different.

(RD, 2016) The size of the compounds can also affect the solubility in the respective mobile phase. For example, Phosphatidylglycerol is the substance that travelled the most also because of its small size. (Mitnick, DeMarco and Gibbons,

When we tested the solubility of the soap’s starting materials as indicated in Table 1, we based our results and conclusion off of the theory that nonpolar substances are hydrophobic and that polar substances are hydrophilic¬2. With hydrophobic meaning water hating and hydrophilic

As mentioned in the discussion, olive oil, vegetable oil, crisco, and lard were soluble in nonpolar solvents and insoluble in polar solvents. This is due to the chemical composition of polar and nonpolar substances which results from the molecular shape as well as properties of dissolving solutes in solution. Polar substances are hydrophilic and contain polar Van Der Waals interactions (intermolecular forces) such as dipole-dipole forces, ion-dipole forces, and hydrogen bonding. Nonpolar substances are hydrophobic and contain non-polar Van Der Waals interactions. ‘Like dissolve like’ is the reason only polar solutes dissolve in polar solvents and why nonpolar solutes dissolve in nonpolar solvents. Molecules with similar polarity have similar intermolecular forces and therefore, can interact with each, or in this case dissolve9. Additionally, the solubility of a compound is determined by the length of the hydrocarbon chain. Long hydrocarbon chains such as the one found in oleic acid makes a compound more insoluble10. Therefore, since the lipids used in this experiment were hydrophobic substances and each lipid has long hydrocarbon chains, the results were consistent with the scientific literature and principles.