Aldehydes And Ketones Lab Report

3.Introduction- In order to do this experiment you must know certain terms and formulas. Molar mass is defined as one mole of this substance. The molar mass is what we are trying to find.One equation use d to find molar mass is MW=m/n. Another thing needed to know is the Ideal Gas Law. The equation used for this is PV=nRT.

However, since it was not immediate, and did not turn cloudy at ~5-10mins, it was unclear if unknown #305 was indeed an alcohol. Therefore, to confirm whether unknown #305 is an alcohol, a Jones test was used. 3 test tubes were used: one with unknown, one with 1-butanol, and one with p-tolualdehyde. The test tube with unknown and 1-butanol had the same results, they both turned blue/green, while the test tube with p-tolualdehyde formed a precipitate. Therefore, it is confirmed that unknown #305 was an alcohol. Then, another Lucas test was used, to determine whether unknown #305 was a primary, secondary, or tertiary alcohol, since the first Lucas Test did not give clear results. The second Lucas test of unknown did not show any change. No layers or cloudiness formed immediately, and no cloudy mixture was present within 5-10 minutes. At this point, unknown #305 is confirmed to not be a tertiary alcohol, since no layers or cloudiness formed immediately. Unknown #305 may seem like it is not secondary as well, since no cloudiness formed within 5-10 minutes, however, it is possible it is a hindered secondary alcohol, and will need heating. At this point, the plan is to heat test tube with Lucas test of unknown, if necessary, after taking melting point and boiling point of derivative. At this point, unknown #305 can either be a hindered secondary alcohol or

The purpose of this lab was to see how certain substances; Naphthalene, Toulene, and and 2 unknowns (one liquid, one solid) react with 3 different solvents. To identify the two unknowns, testing needs to be done to find the density of both the liquid and the solid, determine the melting point of the solid, and the boiling point of the liquid. The Physical Properties of Pure Substances Table can then be used to compare the observed results with the accurate properties from the table. If testing is done correctly, accurate assumptions can be made to figure out what the unknown substances were.

To identify the unknown solution, the physical properties were observed such as state, color, odor, and boiling point. Then, the functional group tests were performed.

The Carbonyl group, found on the ketone, is a polar group due to the oxygen atom being more electronegative than the carbon atom. This creates a molecule that is slightly polar. It is a relatively stable molecule with a relatively high boiling point. All three Ketones on the table have a boiling point close to water or substantially higher. The carbon atom in the carbonyl group is not electronegative enough to give a partial charge large enough for hydrogen bonding to the hydrogen atoms in Pentanone.

A colorless vapor was observed rising towards the fractionating column. Other droplets were observed to drip back into the flask from the cold glass inside the fractionating column. After a colorless distillate was observed dripping in beaker A, which was identified as ethanol because its boiling point (78°C) corresponded to that of the liquid (ethanol). Within a short while, the temperature of the mixture increased to 100 0 C, suggesting that the first distillate had been extracted from the mixture. Beaker A was replaced with beaker B to collect the second colorless distillate whose boiling point corresponded to that of water (100 0

it was concluded that this was a chemical change because gas was formed and the mixture heated after coming into contact with each other. For the third lab, lauric acid in a test tube was dipped into hot water, the reaction changed the lauric acid, which was at first a white powder, was converted to a clear liquid when heated, and after the acid ran under cold water, the acid returned to powder form. It was concluded that this was a physical change because there was lauric acid in the beginning and there was lauric acid at the end. For the fourth lab, about ten drops of silver nitrate and about ten drops of sodium chloride solution were mixed , both of these liquids were clear, but when mixed, the mixture was cloudy, at the end of all of the labs, it was observed that a precipitate formed and collected at the bottom of the test tube, this means that the change was chemical because of the precipitate forming. For the fifth lab a copper chloride solution

Discussion of Results and Scientific Explanation of Claims The goal of this experiment was to identify our unknown compound using a series of experiments that revealed its chemical and physical properties. Our unknown compound was made of small clear crystals. The compound was odorless. The first experiment we conducted was a qualitative solubility test.

In this second half of the laboratory experiment, various experiments were performed to identify the neat liquid and two components of the binary liquid. A total of three compounds were identified by analyzing information such as the boiling point, density, chemical reactivity, gas chromatography (GC), infrared spectroscopy (IR) and mass spectrometry (MS).

The main purpose of this lab was to discover the proof of alcohol in the given unknown solution. The proof of alcohol in a solution is double its volume percent. Therefore if a bottle of grey goose vodka is 80 proof then its liquid solution has a volume of 40% alcohol. To find the proof in this experiment many steps were taken to separate the ethanol from the solution. Since ethanol is c in water it needs to be separated by adding diethyl ether and sodium acetate to cause a chemical reaction. The chemical reaction results in separation of ethanol form water. Since the ethanol and water is chemically separated the ethanol floats on top of the water, which allows them to be easily extracted separately using a separatory

In the lab, the oxidation is from a primary alcohol into an aldehyde. Specifically, 4-nitrobenzyl alcohol is being oxidized and Pyridinium chlorochromate (PCC)

The experiment was divided into three parts. Firstly, to record the aroma of each alcohol and carboxylic acid that would be used in the experiment. Secondly, to prepare five different esters and record the results. Finally, reporting the balanced equations for each of the

The product was not pure, which can be seen on the H NMR spectra of the product, containing impurities that resulted in the integrations to be slightly off. On the H NMR spectrum, it appears that the H’s farther away from the carbonyl and ester have the impurities since those are the slightly off integrations. Moreover, the splitting patterns for these H’s show some irregularities, which may be due to the impurities. Although the some integrations are inconsistent with the predicted product, when adjusted to account for impurities, the spectrum does confirm the isolation of an ester with the number of H’s (18 H’s) and constitutionally inequivalent H’s (5 H’s) matching. On the other hand, the identification of the unknown alcohol, found to be 1-pentanol, was easier in the respect that the H NMR was not contaminated. The H NMR showed 12 H’s and 5 constitutionally inequivalent H’s with 6 of the H’s having quartets in the ppm range of alkanes, as well as having a H in the ppm range of a C-OH. In addition to the IR spectrum, which showed an OH stretch at 3328.20 cm-1, a CH stretch for alkanes around 2850-2930 cm-1, and a CO stretch for alcohols at 1053.75 cm-1, the proposed alcohol of 1-pentanol could be confirmed to be the unknown alcohol. In order of discovery, the unknown alcohol was first found in order to predict the product of the

The experiment performed included the use of sodium hypochlorite (bleach) to oxidize an unknown secondary alcohol and the determination of the identity of the alcohol and the ketone product by IR spectroscopy. To begin the experiment, approximately 1.75 g of the assigned alcohol, unknown D, was added to a 50 mL Erlenmeyer flask along with 1 mL of acetic acid. After 15 mL of household bleach were dispensed into a graduated cylinder, it was added in small increments with a pipette to the alcohol mixture, which was simultaneously stirred. The temperature was monitored extremely closely with a thermocouple as the bleach was added to the solution to make sure that it did not exceed 45 oC. An ice bath was made to cool the solution as a precautionary measure. The thermocouple seemed to malfunction occasionally because the temperatures that it displayed fluctuated and increased rapidly with the additions of bleach, leading to the flask being submerged into the ice water bath. However, the temperature finally rose at a slower rate and stabilized between 40 and 45 oC after all the bleach was added. Since the exact concentration of the added bleach and millimoles of starting unknown alcohol were unknown, potassium iodide-starch paper was used to make sure that an excess amount of oxidant (bleach) was present. The starch paper turned a blue-black color when a drop of sample was added, which meant that there was excess bleach in the solution to oxidize all of the alcohol. Next,

The initial step on the experiment was to mix isopentyl alcohol with acetic acid and reflux for an hour. Concentrated sulfuric acid was also added to the solution to act as a catalyst, which increased the rate of the reaction during reflux. Excess acetic acid was added to shift the equilibrium toward the products because if the reaction started with equal amounts of reactants, only two-thirds of each reactant would be converted to isopentyl acetate. This means isopentyl alcohol is the limiting reagent.