Objective: The objective of this lab was to find and examine the viscosities of ideal and non-ideal solutions. The ideal being the toluene/p-xylene and the non-ideal being the methanol/water. The second objective of this lab was to investigate the temperature dependence of viscosity (Halpern‚ 17-1). Introduction: Viscosity is the resistance to flow of a certain fluid. In this experiment two solutions are used. According to the definition of viscosity mobile liquids have a relatively
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higher % of the solvent that the higher the colour intensity will be shown on the ph colour scale. The lower the solvent then the less colour shown. Materials: *Test Tubes (4) *Cork Borer *Beets *Water *1% Acetone *50% Acetone *1% Methanol *50% Methanol Procedure: *Cut 4 uniform cylinders of beet using a cork borer with a 5-mm inside diameter. Trim each cylinder to 15-mm in length. *Place these cylinders of beet tissues in a beaker and run tap water over then for 2 minutes to wash
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indicated that the drug was freely soluble in methanol‚ methylene chloride and insoluble in water‚ ether and slightly soluble in PBS (pH 7.4)‚ dichloromethane and very slightly soluble in chloroform‚ alcohol etc. Partition coefficient of the drug was found to be 5.057 in n-octanol: Phosphate buffer solution (pH 7.4) suggesting the drug to be lipophilic in nature. Standard curves of Ketoconazole were prepared in different fluids i.e. PBS (pH 7.4) and methanol. The R2 values are 0.9987‚ 0.9983 and a
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this served as a measurement of the boiling point. The average measured boiling point was 60.2°C. The measured data was inadequate to identify the liquid with. The unknown liquid was revealed to be methanol; the revealed identity could then be used to compare the data to the actual information for methanol. The molar mass was found to have a percent error of 55.6%‚ the density had a percent error of 68.1% and the boiling point had one of 6.95%. The measured data for the boiling point was fairly accurate
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Alcohols Aim The aim of this experiment is to investigate the combustion of various alcohols. The alcohols will be burnt to heat up a test tube of water‚ I aim is to find out how much energy is produced when burning the following alcohols: Methanol‚ Ethanol‚ Propanol‚ Butanol‚ and Pentanol. Any form of burning is an exothermic reaction (heat is given out)‚ this means that the reactants energy is higher than that of the product. Alcohols react with oxygen in the air to form water and
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PEP Process Module 1 19 Aug 1999 SRI Consulting Process Summary This Aspen Plus model simulates the production of acetic acid by low pressure methanol carbonylation in the presence of a heterogeneous rhodium (Rh) catalyst and the promoter methyl iodide. It is intended to resemble the Chiyoda/UOP Acetica™ process‚ a novel heterogeneous methanol process for the production of acetic acid. This technology is based on a heterogeneous Rh catalyst in which the active Rh complex is chemically immobilized
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other two systems were immiscible can be made. Methanol was a polar molecule while pentane was nonpolar. This matches the hypothesis which states that like dissolves like‚ polar cannot mix with nonpolar. Ex. oil and water cannot mix because water is polar while oil is nonpolar. The third system allowed 3 substances to be ranked from least to a greater polar molecule. Water is more polar than pentane and pentane is less of a polar molecule than methanol when it comes to comparing the mixture of water/pentane
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independent variable of alcohol to affect the dependant variable of the amount of DNA extracted. This was done to find out if primary or secondary alcohol would create more DNA precipitate than the other. For this the primary alcohols used were; methanol and ethanol‚ and the secondary alcohol was; isopropyl. Of this the secondary alcohol‚ isopropyl was discovered to be the most effect alcohol to make DNA precipitate‚ as it produced the most amount of DNA. This investigation of extracting DNA is significant
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the higher the absorbance. This experiment incorporated Beer’s Law and is focused on determining the stress that various alcohols have on biological membranes. Using five solutions of differing alcohol concentration for each of the three alcohols; methanol‚ ethanol‚ and 1-propanol and a small slice of beet‚ the stirred solution was placed into a plastic cuvette and then into a spectrophotometer and the absorbance of alcohol solutions were determined in order to conclude which alcohol and concentration
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thiourea‚ methanol‚ ethanol‚ propanol‚ ethylene glycol‚ diethylene glycol‚ and triethylene glycol‚ and the mean hemolysis times can be seen below in Figure 1. The mean hemolysis time for urea was 11.90 seconds (±2.65 sec‚ n = 11). Thiourea took an average of 92.72 seconds (±12.41 sec‚ n = 11) to hemolyze 75% of erythrocytes‚ while methanol took 9.19 seconds (± 1.66 sec‚ n = 11). The black line was seen through
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