Purpose: The purpose of distillation is to purify a liquid. Distillations are use to purify contaminates out of water to obtain clean pure water‚ as well as‚ to separate mixtures of liquids into their individual components; e.g. methanol and water. Objective: Distill methanol from water using a simple distillation apparatus and fractional distillation apparatus to determine which is a more accurate form of distillation. Chemical reaction and mechanism: N/A Procedure: This experiment is conducted
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viscosity of given liquids. Two different methods were employed‚ the first measures time of flow of several methanol-water solutions‚ from point A to point B. The second method involves dropping a foreign object‚ in this case a sphere‚ into a cylinder of glycerol and measuring the time it takes for it to travel a specific distance down the tube. The viscosity of a 0%‚ 20%‚ 40%‚ 60%‚ 80% and 100% methanol by volume solutions was measured to be 0.89‚ 1.28‚ 1.53‚ 1.46‚ 1.11 and 0.54±0.001P‚ respectively. The
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to 10 mL with methanol. One mL of the above solution was diluted to 100 times in a 100 mL volumetric flask with methanol to produce stock solution of 10 g/mL. From this solution 1‚ 2‚ 3‚ 4‚ 5‚ 6‚ 7‚ 8‚ 9 and 10 mL were withdrawn separately in different 10 mL volumetric flasks and volume was made up in each case up to 10mL with methanol to produce the concentrations 1‚ 2‚ 3‚ 4‚ 5‚ 6‚ 7‚ 8‚ 9 and 10 g/mL. Absorbances of these solutions were recorded at max 405.9 nm against methanol as blank using
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evaporate. To test this‚ the temperature change from the evaporation of 4 different alcohols was measured and compared‚ along with cyclohexane. Methanol had the largest change in temperature‚ 18.9 ºC. This indicates that methanol has the weakest intermolecular attractions out of the 4 alcohols‚ because it evaporated the most. This may be because methanol is a small molecule so it has less electrons and therefore is not as polarizable as
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molecules‚ ions‚ and atoms together. The intermolecular forces that can be present in a solution are london dispersion forces‚ dipole-dipole force‚ hydrogen bonding and ion-dipole forces. In this experiment the substances that were used were acetone‚ methanol‚ water‚ 1- butanol and ethyl acetate. Acetone is the organic compound with the formula (CH₃)₂CO. It is a colorless‚ volatile‚ flammable liquid‚ and is the simplest ketone. It takes 21 seconds for it to completely disappear. It was the first to evaporate
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25% alcohol had .022‚ and 50% alcohol had .177. The highest concentration of acetone inflicted more damage on the membrane of the beetroot causing it to leak its betacyanin in a higher intensity than any of the other solvents had caused. Acetone and methanol can both cause damage to the membrane of the beetroot but acetone has a greater ability and is more damaging. The beet root model system shows the effects of chemical stress on membranes. Introduction: The membrane of the cell contains
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graduated volumetric pipets (0.01 ml markings) B. A 1ml graduated volumetric pipet is the best to use if you want 0.15 ml of reactant C. 1ml plastic pipets (used 2 times) are best to use when you want 2 ml of solvent Safety Hazards: 1. Methanol is flammable and toxic. Don’t breathe it in or drink it. 2. All organic waste goes in the waste containers and not down a sink Drug | Melting Point | Acetylsalicylic acid (Aspirin) | 135°-136° C | Acetaminophen (Tylenol) | 169°-170
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Benzophenone’s nonpolar nature makes it insoluble with water (which is polar)‚ soluble with methanol (which is of intermediate polarity) and soluble with hexane (which is nonpolar). This is because generally‚ like dissolves like -- nonpolar will dissolve nonpolar but not polar‚ and vice versa. But note that this is an imperfect science -- you would expect hexane to dissolve faster and more completely than methanol (because of the differing polarities)‚ but the opposite occurred. This may be because of
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Synthesis of Methyl Salicylate from Aspirin Esters are a class of organic compounds. An ester compromises an organic or inorganic acid in which one or more hydroxy (OH) groups have been replaced by and alkoxy (O-alkyl) group. For example‚ the simplest ester‚ methyl formate (CHOOCH3)‚ is made up of formic acid (CHO-OH) in which the hydroxyl group has been replaced by a methoxy group (-OCH3). Similarly‚ ethyl acetate (CH3CO-OCH2CH3) is made up of acetic acid (CH3CO-OH) in which the hydroxy group
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Viscosity of Liquids Part I: Low Viscosities Mona Kanj Harakeh 1 Objectives • To measure and analyze the viscosities of ideal (Toluene/p-Xylene) and nonideal (Methanol/Water) binary solutions and their components. • To determine the Activation Energy to viscous flow. • The effect of temperature change on the viscosity will be studied. Method: The viscosities of liquids are determined by measuring the flow time for various liquids in an Ostwald viscometer. 2 Ostwald viscometer 3
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