To perform this experiment, we will utilize emission spectra, titrations, and thermal gravimetric analysis, using knowledge from Experiments 10, 4, Titrations of Na2CO3 and NAHCO3 by HCl (hydrochloric acid) will be performed to determine the concentration of HCl, as well as the number of moles of HCl present within the sample of baking soda. As a result, we will be able to determine the molar concentration of HCl by determining its equivalence point (the point on the graph where the exact amount of rectant needed to perform a reaction has been added) from graphical analysis. Na2CO3(aq.) + HCl(aq.) ==> NaHCO3(aq.)
This particular reaction is a strong acid and a strong base which means that when the reaction reaches the equivalence point, the moles of the acid and the base are equal and the solution is neutral so the pH should be around 7.0 depending on the final volume of each solution. To get this data, we will titrate an HCl solution with NaOH solution of which is a known concentration. We will record the initial and final reading of the NaOH while we record the pH of the titrated solution in the beaker. We will repeat this process with a solution of acetic acid which is a weak acid with NaOH and record the initial and final reading of NaOH and the pH of the solution in the beaker. Procedure Preview Calibrate the pH meter.
However, the alcohol remains fairly constant in the form of glycerol or in other words propane -1,2,3- triol. This form of alcohol contains a hydroxyl allowing longer chains to form of carbon. 7. A common commercial use for esters is in the perfume industry where a synthetic scent is created within labs through the process of esterfication. For example, Benzyl Acetate is one form of an ester that can be used as to create a perfume
EXPERIMENT 4 DETERMINATION OF NICOTINE IN TOBACCO RESULTS STANDARDIZATION OF APPROXIMATELY 0.025M PERCHLORIC ACID Element/Compound | Molecular weight(g/mol) | Errors(g/mol) | Error of analytical balance(g) | 8C | 96.0856 | 0.0005 | 0.0001 | 5H | 5.0397 | 0.0004 | | K | 39.0983 | 0.0006 | | 4O | 63.9976 | 0.0002 | | KHP | 204.2212 | 0.0005 | | Errors(g/mol) = error of molecular weight X coefficient √3 For example: Error Carbon = 0.0008g/mol *8 = 0.00046188 = 0.0005g/mol √3 Titration of KHP by Perchloric acid. Flask number | Initial volume(mL) | Correction initial volume | Initial volume + correction | Final volume (mL) | Correction final volume | Final volume + correction | Total volume(mL) | 1 | 0.04 | 0.0004 | 0.0404 | 25.3 | 0.037 | 25.337 | 25.2966 | 2 | 25.3 | 0.037 | 25.337 | 47.32 | 0.056 | 47.376 | 22.039 | 3 | 1.19 | 0.0045 | 1.1945 | 23.02 | 0.036 | 23.056 | 21.8615 | Calculation for the concentration of perchloric acid Flask number | mass of KHP(g) | number of moles KHP(mol) | Error number of moles(mol) | Concentration of perchloric acid(M) | 1 | 0.1049 | 0.000513659 | 0.001 | 0.02 | 2 | 0.1044 | 0.00051121 | 0.001 | 0.02 | 3 | 0.103 | 0.000504355 | 0.001 | 0.02 | Number of moles KHP(mol) = mass molecular weight Number of moles flask 1 = mass = 0.1049g = 0.0005mol molecular weight 204.22g/mol Error number of moles KHP = √(error analytical balance/mass flask1)^2 + (error molecular weight/molecular weight)^2 Number of moles KHP = number of moles perchloric acid * Concentration of perchloric acid = number of moles KHP X 1000
Smith R, McKee J, Zanger M. The electrophilic bromination of toluene: Determination of the ortho, meta, and para ratios by quantitative FTIR spectrometry. JOURNAL OF CHEMICAL EDUCATION. 2002;79:227-229. 2. Zachariou M, ebrary eBooks, Springer Protocols.
Experiment 5: Preparation of Cyclohexene- Acid Catalyzed Elimination of Cyclohexanol Ball State University Organic Chemistry Lab 231 (Sec. 5) Dr. Bock/Daniel Miller Tiffany Raber 5 November 2012 Purpose: To prepare an alkene by an elimination reaction of an alcohol in the presence of sulfuric acid as a catalyst to produce a successful yield and desired results for the purity of the alkene. Introduction: The dehydration of an alcohol such as cyclohexanol is a useful technique for generating alkenes. The success of this reaction relies on a dehydration, such as the presence of a strong acid (sulfuric acid). Because this reaction is reversible, a fractional distillation is necessary to produce cyclohexene, water, and some impurities and a simple distillation is followed to further purify the product.
Ideal Gas Behavior Instructor: Nieves Montano Chem 151, Section 002G Date Work Performed: February 12, 2014 Date Report Submitted: February 20, 2014 Abstract: This paper reports a lab experiment done on the ideal gas law to determine differences in gas based upon their “R” constant difference to 0.082057. A total of seven gases were tested, which included, Ethanol, Hexane, Cyclohexane, Pentane, Ethyl Acetate, Butane and Acetone. These gases were each heated and then condensed to liquid gas to find specific values and determined Ethanol as the gas closest to ideal behavior in this experiment. Introduction: The Ideal Gas Law demonstrates the relationship of the properties of gases. This relationship is specific to the gases that are considered “ideal”.
Methylene chloride: ethanol (1:1 solution) What solvent system will you be using to "develop" your TLC plates in the TLC of Analgesics lab? ethyl acetate with 0.5% solution of acetic acid How will you be visualizing your TLC plates in the TLC of Analgesics Lab? an UV lamp or a UV light What is the name of the hydrogenation catalyst used in the Hydrogenation of Olive Oil Lab? 10% Palladium on
Experiment F: Dehydration of Cyclohexanol to Cyclohexene March 18, 2013 OBJECTIVES * Gain familiarity of dehydration mechanism and refractive index * Synthesize cyclohexene through dehydration of cyclohexanol by using phosphoric acid as catalyst * Grow in familiarity in reading IR spectra and data BALACED CHEMICAL EQUATION FOR THE DEHYDRATION C6H12O + H3O4P C6H10 + H2O TABLE OF PROPERTIES AND EQUIVALENTS NameCASChemical FormulaStructure | FW (g/mole) | BP/MP (° C) | Density (g/mL) | Refractive index | Molar amounts added (mol/L) | Limiting reagent | Hazards | Cyclohexanol108-93-0C6H12O | 100.16 | 161.125.15 | 0.96 | n20/D 1.465 | | Yes | Results in skin, respiratory tract and eye irritation; hazardous if swallowed |
Date: 6/3/2012 Title : Synthesis of an Active Pharmaceutical Ingredient, Aspirin ( Including Raw Materials and Product Purity Checks ) Name: Class: Lab partners: Aim: The aim of this experiment is to prepare and recrystallise Aspirin, determine the percentage yield by mass of product, preform a test to check for phenols, and characterise it by its melting point. The following is the reactions scheme: Method: -[Lab Manual Pages 3, 4 & 5]- Results and Calculations: Compound Salicylic Acid Acetic Anhydride Aspirin Appearance White Powder Clear, Colourless liquid White Crystals Molar Mass (g/mol) 138g/mol 102g/mol 180g/mol Density if liquid (g/cm3) 1.08g/cm3 Weight used (g) 2.868g 5.4g N/A Moles used (mol) 0.0207mol 0.0529mol N/A Limiting Reagent N/A Theoretical Yield of Products in moles N/A N/A 0.0207M Theoretical Yield of Product in Grams N/A N/A 3.726g • Calculations from table ^ : Moles of Salicylic Acid : Moles= Mass X Mr => M = 2.868 X 138 = 0.0207moles Moles of Acetic Anhydride : M = 5.4 X 102 = 0.0529moles Theoretical Yield in moles : moles of limiting reagent = 0.0207moles Theoretical Yield in Grams : Moles of limiting reagent X Mr of Product : = 0.0207mol X 180g/mol = 3.726g • Melting Points Compound Salicylic acid (raw material) Recrystallised Aspirin Expected MP Value 157-161oC 138-140oC Actual MP Value 158-160oC 137-139oC • Percentage yield: Percentage yield = 2.214/3.72 ₓ 100 = 59.52% => 60% • Test for phenols: Samples Crude Aspirin Recrystallised Aspirin Salicylic Acid Colour change of Samples + 1cmoC methanol Yellowish Yellowish Purple Inference Phenol not present Phenol not present Phenol Present Post- Practical Questions : Q1 What did your melting point indicate about the purity of your product? Explain your answer.