T Pentyl Chloride Lab Report Essay

All standardizations are performed in triplicate. Weigh out .1000-.1200 gram KIO3. Add 70-80 mL of deionized water. Swirl and dissolve. Add 3 mL of 6M HCl. Swirl and mix. Quickly titrated the brow-red solution with 0.1M Na2S2O3 until it is light yellow. Then add 3.5 mL of starch indicator. Titrate again until the dark color first disappears.

In this experiment, a mixture of unknown #3 was used. That mixture had acid, base, and neutral. We added solvent to the unknown. It is important to know the density of the solvent in order to determine which is the aqueous layer and which is the organic layer. If the solvent that has more density than water, so the organic layer will be the lower layer, while if the solvent has lower density than water, the organic layer will be the upper layer. This will make an error if the determination of the layers was wrong after added the strong acid or the strong base. We added 5% HCl to the mixture in order to separate the base in the aqueous layer and form its salt. Same thing, we add 5% NaOH to the mixture in order to separate the acid and form its salt. In order to recover the base, we add 10% NaOH to the HCl extraction. The result will be salt with a base. Same thing for the acid, in order to recovered it, we added 10% HCl. The reaction will give us salt with an acid. For the neutral, we added sodium sulfate as a drying reagent in order to dry water and separate the neutral part as pure.

1. Carefully measure the volume of the trapped gas using the graduations (markings) on the side of the container.

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.

9.Repeat the procedure with a new mass of baking soda. Before beginning, rinse the reaction vessel with water. Refill the graduated cylinder with water. Check water level in collection box so it has room for the water from the graduated cylinder.

alcohol (2-methyl-2-butanol, MW _ 88.2, d _ 0.805 g/mL) and 25 mL of concentrated hydrochloric acid (d _ 1.18 g/mL). Do not stopper the funnel. Gently swirl the mixture in the separatory funnel for about 1 minute. After this period of swirling, stopper the separatory funnel and carefully invert it. Without shaking the separatory funnel, immediately open

The mixture was heated at 120°C using an aluminum block and was stirred gently. After all of the solid dissolved, it was heated for 20 additional minutes to ensure the reaction was complete.

1.) Transfer the distillate to separatory funnel. Fluid didn’t seem very clear but sufficient to finish our lab on time.

The reaction is carried out in saturated aqueous ammonium chloride solution. Thus no special drying of solvents, reagents, or glassware is required. The reaction mechanism for this experiment can be seen below (Fig. 2)

In the separating funnel, a heterogeneous mixture was formed: resulting in an organic layer (top) and a solvent layer (bottom). This effectively allowed the draining of the solvent, in order to isolate the organic layer, the impure ester (1-pentyl ethanoate)

If necessary the centrifuge can also be used to further separate the two layers. A final means of drying the ester product is the addition of granular sodium sulfate.

This process was then repeated two more times with subsequent additions of 10 mL of the 0.5M aqueous NaHCO3 and the aqueous layers drained off into the above mention labeled 100-mL beaker. Finally 5 mL of deionized water was placed into the funnel and mixed. The water was then drained off into the beaker containing the aqueous solution extracts. The solution was then saved until need later in the experiment.

Chlorine is used for many useful purposes in the world of medicine. For this reason, it is important to understand what chlorine is and how it works at the atomic level. The first notable piece of information taken from Figure 1 is the shells of the model. Each shell can be thought of as an orbit around an atom's nucleus. The shells, from the inside out, are labeled as the 1 shell, 2 shell and 3 shell. They can also be called K shell, L shell and M shell, respectively. The first most important piece of information taken from Figure 1 are the shells. Each shell has a fixed number of electrons that it can hold. 1 shell can hold up to two electrons, 2 shell can hold up to eight electrons and 3 shell can hold up to 18 electrons. The number of shells

The effects of Trichlorethylene and Perchloroethylene, just with any other chemical can depend on the time of your exposure, for example during pregnancy or in infancy. It can also depend on the length of your exposure.Trichloroethylene is an organic chemical that has been used in dry cleaning, for metal degreasing, and as a solvent for oils and resins. It has been shown to cause liver and kidney cancer proven by experimentation in animals.[2] Health defects that happen when one comes in contact with TCE include Parkinson disease, Liver cancer, Scleroderma and most importantly Leukemia. Health defects that happen when one comes in contact with PCE include “Bladder cancer, non-Hodgkin lymphoma and End-stage renal disease”.[1]

NaCl is short for Sodium Chloride. Its commonly known as Salt, It is known for being the saltiness in seawater. In the form of table salt it is commonly used as a condiment and food preservative.Large quantities of sodium chloride is used in many industrial processes, and it is a major source of sodium and chlorine compounds. A second major application of sodium chloride is de-icing of roadways in sub-freezing weather.