Organic Lab

After each of the solids were completely dry, each was placed into a MelTemp device. The temperature at which each solid began to melt and completed melting was recorded.

In determining the melting point range of the aspirin, a capillary tube (sealed at one end) was one-third-filled with the dried aspirin. The capillary tube and a thermometer were immersed in an oil bath. The temperature at which the solid started to melt and the temperature when the entire sample was completely liquefied were recorded as the melting point temperature range.

IV) Part C Results: 1) Complete the following table by rating each pair of liquids as either miscible or immiscible. (2 Points)

In the extraction of certain compounds, solubility plays an important factor in how the procedure is performed. The identification of which solvent is best for the substance is crucial. The relation of polarity between the solute and solvent is determined at a molecular level. The relationship between the solvent and solute needed shared similar characteristics. Polar solutes are dissolved in polar solvents while nonpolar solutes are dissolved in nonpolar solvents. From a chemical level, molecules are attracted to other similar molecules closest to their properties. Polar molecules are only attracted to polar molecules in both the solute and the solvent, and the same goes for nonpolar molecules. This explanation

Part B involved monitoring and analyzing the freezing point depression of an unknown ionic solid, the identity of the solid being either NaCl or KI. Unknown #1 was

After the solid is separated from the liquid it is allowed to dry so any liquid stuck to the substance will just evaporate away and you are left with a pure substance.

Pure cinnamic acid and pure urea both have melting points around 132-135 ˚C, which was consistent to the experimental data collected (Cinnamic). However, the impure compounds: 75% cinnamic acid to 25% urea by mass and 25% cinnamic acid to 75% urea by mass had melting point ranges of 96-119˚C and 97-123˚C respectively. This is since impure compounds do not have a perfect/tight molecular structure compared to the pure version because the intramolecular bonds have been replaced with weaker intermolecular bonds, which results in a lower and broader melting

The results from Part D of this experiment provide the conclusion that when two immiscible liquids are placed in a vial, the organic solvent is the one that sets at the bottom while the inorganic solutes remain at the top of the vial. When dichloromethane and water are compared, dichloromethane is the organic solvent. When diethyl ether and water are compared, water is the organic solvent. When two solvents are compared, the solvent with the lower density is the inorganic

Therefore, the three solvents that follow the four rules are HCl, NaOH, and ethyl acetate which are used to extract the unknown base, acid, and neutral compound respectively. The experiment then consisted of the separation of 1g of an unknown mixture that was supposed to be in a 1:1:1 ratio of acid, base and neutral compounds dissolved in 30 mL of ethyl acetate. Once it dissolved it was to be put in a separatory funnel. The separatory funnel is essentially used to separate the two immiscible phases. The extractions of the acid, base, and neutral compound should

In one of my freshman chemistry labs,I had to find the correlation between impurities and the melting point of the organic molecule. Before the lab, I had a vague knowledge about how the intermolecular forces affect the melting point of an organic molecule. The strength of the intermolecular forces in the compound are directly proportional to the melting point of the molecule. In this experiment,

This will let the filtrate through but leave the sand behind. The filtrate is the liquid that passes through the funnel during filtration. In this experiment, the saltwater solution is the filtrate. The solution remaining in the beaker will then be heated over a Bunsen burner. As the solution is being heated, the water in the saltwater solution will evaporate off until only the salt is remaining in the beaker. Evaporation is a process where a soluble solid is separated from a liquid. The lab ends with the sand on the filter paper, and the salt remaining in the beaker.

Paisley Shultz December 21, 2016 Chemistry- Savalli p. 6-7 Solubility and Bond Type Laboratory Conclusion The purpose of this laboratory was to learn the solubility of different liquid substances. We also learned how to use the aforementioned information to classify each of the substances’ bond type. Essential contextual knowledge includes understanding solubility itself.

Because of this latter factor, some sulfanilamide will remain dissolved in the mother liquor (the liquid remaining after crystallization has taken

If a development solvent of too high of a polarity is utilised , all components in the mixture will move along with the solvent and no separation will occur. If the solvent is of too low of a polarity, the components will not move enough and no separation will be observed.

-First a saturated solution is made(a compound containing impurities is dissolved in a hot solvent)