Synthesis of Cyclohexanol Author: Ahmed Ayyash 06/06/13 Introduction: In this experiment‚ cyclohexanol was prepared from an initial cyclohexene. However‚ this occurred over a number of steps‚ these are out lined below. 1. Cyclohexene + aqueous acid cyclohexyl cation 2. cyclohexyl cation + hydrogen sulphate + water protonated cyclohexanol + cyclohexyl hydrogen sulphate 3. cyclohexyl hydrogen sulphate protonated cyclohexanol + HSO4 4. protonated cyclohexanol + HSO4
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Determining the value of molar mass of chosen compound Marta Dürrigl 1mmA Chemical reaction: b.) CaCO3 (s) + 2HCl (aq) ----------- CaCl2 (aq) + CO2 (g) + H2O(l) AIM: The aim of this investigation is to experimentally determine the molar mass of carbon dioxide (CO2) by measuring its volume and calculating its mass. CO2 which we will measure will arise as a product of a chemical reaction between Calcium Carbonate (CaCO3) and Hydrochloric acid (HCl) as it is shown in the chemical
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molar mass of an unknown volatile liquid. Heating a flask filled with an unknown‚ easily evaporated liquid will allow for measurements that can be taken to work out the ideal gas equation. This lab will require knowledge of basic equations used in chemistry. Using these equations‚ such as density and number of moles(n)‚ we can substitute different values into the ideal gas law to manipulate it. II. Materials: 250-mL Erlenmeyer flask Needle or pin Unknown liquid
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10mL of distilled water to the flask. 9. Then they added 3 drops of phenolphthalein to the flask‚ and swirl the flask to mix thoroughly. 10. Then they started to move the flask‚ next observed the substance until the substance until the substance changes his color. 11. They began the titration by added NaOH to the flask. For the initial trial they may want to add the base fairly quickly until they notice a pink colour appearing in the flask. Swirling the flask should make the pink colour
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vigorously in a sealed vial. (Caution! Be sure the vial is sealed because oxone is a strong oxidizer.) Dissolve 50 L of cyclohexene in 2.0 mL of acetone in a small Erlenmeyer flask. Cool the cyclohexene solution in an icebath‚ then add the oxone solution dropwise over 5 minutes with swirling in the icebath. Remove the Erlenmeyer flask from the icebath and allow the reaction to sit for 15-30 minutes. (To save time‚ this is a good place to start the potassium permanganate reaction.) Add two drops
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Lab Report # 11 By: Andrew Hoitt CHEM 105 Lab 11/29/2012 Lab # 11 – Acid - Base Titration Introduction: The purpose of this lab is to determine the molarity (M) of an unknown HCl solution. A NaOH solution will be made and its molarity calculated. A sample of the NaOH solution will be titrated against the unknown HCl solution to calculated the volume needed to neutralize it. With these volumes the unknown molarity can be calculated. Theory: Solutions
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used to measure out 15 mL of glacial (concentrated) acetic acid. This was poured into a 125 mL Erlenmeyer flask. Both graduated cylinders were rinsed thoroughly with acetone several times. The 2‚6-dimethylaniline was added via a Pasteur pipet to the acetic acid. The graduated cylinder was rinsed with acetone and left to air dry. 2 mL of 2-chloroacetyl chloride was measured and poured into the Erlenmeyer flask. A thermometer was placed to record any temperature change during this process. A large graduated
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The methods used were quiet precise. The burette and pipette have some limitations due to being less precise. The volume of burette limited the amount of trial that were attempted and it needed to be refilled. The Erlenmeyer flask resisted the splashing of the solution outside the flask which would have been occurred due to swirling. This caused the value‚ of the number of moles of HCl needed to neutralize NaOH‚ to be more accurate. Experimental errors could possibly be as follow:•NAOH was lost to
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two different temperatures. If the volume-to-temperature ratios are the same at both temperatures‚ Charles’s law is verified. The gas you will use in this experiment is air. You will find the volume of air in an Erlenmeyer flask at two different temperatures. First‚ the air in the flask will be heated to the
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A. Goal and Purpose: Session 1: In this lab‚ we will achieve a simple Friedel-Crafts alkylation of anthracene. The choice of anthracene as an aromatic substrate stems from two considerations. First‚ there is a question of regioselectivity. Second‚ anthracene and its derivatives are highly visible under UV light. Session 2: In this lab‚ we will complete a partial conversion of 9-acetylanthracene using m-chloroperoxybenzoic acid (mCPBA). We will also determine by NMR‚ the regiochemistry of the
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