100-Methyl Benzoate Lab

This experiment was started with a clear solution of sodium benzoate and HCl was added to it, ultimately producing benzoic acid. First, .3395 g of sodium benzoate was weighed, then it was dissolved in water, causing it to disassociate into ions. Next, 3M of HCl were added drop wise to the solution until it reached a pH of 2, thus introducing the hydronium ion. This addition caused a white, solid benzoic acid to precipitate out of the solution. A vacuum filtration system was used to separate the solid from the liquid. What was once

Samples of benzophenone, malonic acid, and biphenyl were each tested with water, methyl alcohol, and hexane. Benzophenone was insoluble in water as it is nonpolar while water is highly polar. Benzophenone was soluble in methyl alcohol, dissolving in 15 seconds, because methyl alcohol is intermediately polar as benzophenone is nonpolar. Methyl alcohol is polar but not as much as water. Thus, the nonpolar benzophenone was soluble in methyl alcohol. Benzophenone was partially soluble in hexane because hexane is nonpolar as is benzophenone. Thus, benzophenone was dissolved in hexane. Malonic acid was soluble in water because both malonic acid and water are polar. It took 25 seconds for malonic acid to dissolve in water. Malonic acid was soluble in methyl alcohol because malonic acid is polar and methyl alcohol is intermediately polar, allowing malonic acid to dissolve in the methanol in 15 seconds. Malonic acid was insoluble in hexane because hexane is nonpolar while malonic acid is polar. Biphenyl was insoluble in water as water is highly polar whilst biphenyl is nonpolar. Biphenyl was partially soluble in methanol which is intermediately polar whilst biphenyl is nonpolar, allowing it to dissolve a little. Biphenyl was soluble in hexane because both biphenyl and hexane are nonpolar molecules. Biphenyl dissolved in hexane in 10 seconds.

In order to isolate benzoic acid, benzocaine and 9-fluorenone, each component needed to be separated from one another. All three compounds began together in one culture tube, dissolved in methylene chloride and formed into a homogenous mixture. In this culture tube, two milliliters of aqueous three molar hydrochloric acid was added, which immediately formed two layers, the top acidic aqueous layer was clear in color and contained benzocaine, and the bottom organic formed was yellow and contained benzoic acid and 9-fluorenone. Benzocaine’s amino group is protonated by the aqueous layer hydronium. This protonation forms the conjugate acid of benzocaine, benzocaine hydrochloride. Thus, the conjugate acid, benzocaine hydrochloride is a salt in which is soluble in water and furthermore can be isolated from the organic mixture. When testing out the pH levels in benzocaine, the pH test strip was dark blue in color, indicating a pH level of around 5 to 7. When isolating benzoic acid, two milliliters of aqueous three molar sodium hydroxide was added, which deprotonates the carboxylic group in benzoic acid, forming its conjugate base, sodium benzoate. As with benzocaine hydrochloride, sodium benzoate is a water soluble ionic salt in the aqueous layer that can then be separated from the bottom organic layer containing the 9-fluorenone. The pH test strip was a vibrant red for benzoic acid, indicating a pH of 2. Now the 9-fluorenone is left, deionized water is added to remove any excess

This experiment examines the solubility characteristics of organic and inorganic species. The specific substance being tested first, is the organic compound benzoic acid. The objective of the first set trials is to acquire data which can be used to determine the best solvent for the recrystallization of benzoic acid. Next, potassium permanganate, an inorganic salt, will be dissolved in a variety of organic solvents, with the aid of phase transfer agents.

After the mixture finished refluxing, the flask was then cooled on ice. A sulfuric acid solution was then prepared by pouring 4.5 mL of concentrated H2SO4 over 50 grams of ice and then diluted to 75 mL by adding enough tap water to reach 75 mL. The sulfuric acid solution was then cooled on ice.

The main purpose of this lab is to determine whether or not the number of carbon molecules relate to the amount of energy emitted measured through the temperature change over the course of 2 minutes. The main three tested fuels are fuels methanol (CH3OH), ethanol (C2H5OH), propanol (C3H7OH). Based on those formulas, Propanol alcohol has 3 carbons, Ethanol alcohol has 2 carbons and methanol has 1 carbon. Based on the hypothesis mentioned above “If the number of Carbon molecules in the fuel increases, the amount of energy over 2 minutes is going to increase”. Based on the data shown above, propanol fuel had the most temperature change meaning that it burned with the most energy. Following that is ethanol fuel having the second greatest temperature

Pour 40ml of sodium thiosulphate into the 50ml-measuring cylinder then transfer the sodium thiosulphate into the conical flask. Place conical flask right above the dot on the

In this experiment Benzpinacolone was synthesized in a process that contained two steps. First the photoreduction of benzophenone in 2-propanol, which was done by placing the flask under sunlightfor the absorption of the UV rays to carry out the reaction. Then the second part was the dehydration of benzpinacol to benzpinacolone, where the benzpinacol product was converted to a ketone by the acid catalyzed rearrangement of the benzpinacol to the benzpinacolone; this was done by adding iodine and acetic acid to benzpinacol. The reaction was then refluxed, cooled in an ice bath, filtered and washed with ethanol. After

The goal of this lab was to determine the effects of different amounts of Vinegar on the temperature in the reaction NaHCO3 + HC2H3O2 → NaC2H3O2 + H2O + CO2.

Abstract: In this experiment, our team analyzed an unknown acid and a sample of vinegar solution by the process of titration using a 0.1 M sodium hydroxide solution as the titrant, as this solution is a strong base. In addition, our team members used phenolphthalein as indicator in the reaction.

To start, a water beaker bath and an ice beaker bath were prepared. The water beaker bath was placed on a hotplate. Then 5.00 grams (plus or minus a hundredth of a gram) of tert-butanol was obtained and put in a large test tube. Then a thermocouple connected to a LabQuest was positioned in the sample. The test tube was balanced in the water bath with the tert-butanol below the water level and the hot plate was turned on. The water bath was heated until the thermocouple read above 50 °C. Once the sample was above 50 °C, the LabQuest was set to record temperature data at 10 samples per minute. After some data was gathered, the sample was removed from the water bath and positioned in the ice bath. Once the temperature measurements steadied for a few minutes and there was ice formed in the test tube, the trial was concluded.

The aim of this investigation is to measure the the storage of beverages at different temperatures (10 °C, 20 °C, 30°C and 40 °C) affect their total acid concentration.

The purpose of this experiment is to learn concepts that explain the effect of solutes on the properties of liquids and to determine the molar mass of an unknown substance by using freezing points determined by a digital temperature probe. The molar mass of the unknown substance will be determined by measuring the freezing point of the lauric acid and lauric acid mixed with an unknown solute, then plugging those results into the freezing point depression equation (∆T = i*Kf*m). This equation will solve for the molality, number of moles, and the molecular weight of an unknown solute. The unknown substance will ultimately be determined based on matching the calculated molecular weight to the possible substance’s molecular weights.

The aim of this experiment was to find out how temperature affects the rate of reaction between Sodium thiosulfate (hypo) and hydrochloric acid.

The first part of the experiment involves determining the effect on the ionization of acids and bases. In six different test tubes, solutions were prepared respectively. In both test tubes A and B, 10 mL of 0.1M hydrochloric acid was added; and 2 mL of water and 2mL of 0.1M sodium chloride were added, respectively. Acetic acid with concentration of 0.1M and volume 10 mL was added to: test tube C which was mixed with 2mL of water; and D with 2mL 0.1M sodium acetate. Test tube E contained 10mL of 0.1M sodium hydroxide and 2mL of water. And test tube F, also contained 10mL of 0.1M sodium hydroxide, but was added with 2mL of 0.1M sodium chloride instead.