panacetin. In doing this lab we used NaOH and diethyl either‚ along with water. We used a centrifuge
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dissolve it in 50 mL of diethyl ether. Be sure to dissolve the entire mix since it is not homogeneous. 2) Pour the solution into a separatory funnel. 3) To extract the nicotinamide from the mixture‚ add 5 mL of 5% HCl and shake gently. Draw off the lower aqueous layer into 125 mL Erlenmeyer flask and repeat the extraction with a second portion of HCl. Combine the three extracts and then set this mixture aside. 4) To separate the trans-cinnamic acid from the mixture‚ extract the ether solution twice with
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polarity) • Petroleum ether (C5 isomer compounds‚ like pentane; not a true “ether”) • Ligroin (C6 isomer compounds‚ such as hexane) • Diethyl Ether (CH3CH2OCH2CH3) • Dichloromethane (CH2Cl2) • Ethyl Acetate (ester: CH3CH2OC(O)CH3) • Methanol (alcohol: CH3OH) • Acetic Acid (carboxylic acid: CH3CO2H) And of course – mixtures of the above solvents can be used. Consider the following example: Compound A is a non-polar compound and compound B is a polar compound. Add Petroleum ether (non-polar!) –
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the much stronger base‚ sodium hydroxide‚ to remove the hydroxide hydrogen from 2-naphthol. Both of the sodium salts formed from the base extractions will be soluble in water‚ while naphthalene will only be soluble in the original solvent‚ diethyl ether. Introducing the two sodium salts to hydrochloric acid will effectively replace the original proton benzoic acid and 2-naphthol lost. In a chilled environment‚ both compounds will not be soluble in water‚ because the solubility of benzoic acid
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Infrared Spectroscopy Organic Chemistry Lab 301A B. The purpose of this lab is to study Infrared Spectroscopy‚ which focuses on the study of the electromagnetic spectrum. The area to be studied is the infrared region‚ which is made up of gamma‚ X‚ and UV rays. We want to be able to identify spectra’s to their complementary structures. The background of this experiment particularly deals with the study of compound structure determination‚ and traits. We must be aware of the functional groups
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hydrocarbon-like. They are all equally soluble in hexane. D. 5. Part C. Miscible or Immiscible Pairs. Use your observations to complete the following table‚ rating each pair as miscible or immiscible. System Water and ethyl alcohol Water and diethyl ether Water and methylene chloride Water and hexane Hexane and
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p. 1 Megan Ly Chemistry 231L February 20‚ 2013 SOLUBILITY Purpose: To better comprehend solubility behavior by investigating the solubility of various substances in different solvents‚ looking at miscible and immiscible pairs of liquids‚ and observing the solubility of organic acids and bases. Reference:
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Abstract: The purpose of this laboratory is to convert benzophenone to diphenylmethanol. This was done by using sodium borohydride to reduce benzophenone. The product was then crystalized from hexanes then using the melting point and IR testing it was possible to characterize it. The melting point range was… Introduction: This lab is possible because of oxidation and reduction reactions. In organic chemistry oxidation is the loss of electron density around a carbon‚ while reduction is an increase
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Thin Layer Chromatography Submitted in partial fulfillment of the requirements for: CHE 324 Organic Chemistry Laboratory Dr. Robert Duncan Fall Semester 2012 Caitlin Inman‚ Team Leader October 9‚ 2012 Tyler Byrd‚ Data Collection Shared Role‚ Technique Expert Introduction: “Chromatography is used to separate components of a mixture. For example‚ imagine a mixture of wood pieces‚ pebbles‚ and large rocks to be separated and the chromatography setup as a stream. Flowing water
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and purify cholesterol from egg yolks. Two hard boiled egg yolks were twice extracted with diethyl ether and methanol‚ with the filtrate collected via vacuum filtration. Potassium hydroxide pellets were added to the filtrate‚ the ether was distilled off‚ and the mixture was saponified by reflux. The crude cholesterol was isolated through a series of ether extractions and aqueous washes; then the ether was dried with MgSO4 and removed by rotary evaporation. The melting point of the yellow‚ sticky
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