Acid Base Titration Purpose: The purpose is to calculate the molarity of a NaOH solution by titrating the base with 5mL of standard HCl solution in each trial. By adding the base with unknown molarity to the acid with 0.10M the molarity of NaOH can be calculated. The base, NaOH, helps bring the pH of the acid, HCl, closer to seven, which neutralizes it. When using the buret the amount of NaOH used is able to be determined. Then by writing a balanced chemical equation and using the titration formula, Nb+Ma+Va=Na+MbVb , the molarity is able to be determined.
After the measurement is done, a linear graph of the signal data against analyte concentration is plotted. The concentration of the unknown sample is then determined using the equation of the calibration curve. Data Collection: (i) Concentration of benzene (% volume) 5 10 20 30 40 60 70 80 Benzene /chloroform mixture Volume of benzene added 0.5 mL 1 mL 2 mL 3 mL 4 mL 6 mL 7 mL 8 mL Wave number(cm1) 1586.712262 1586.712262 1586.712262 1586.712262 1586.712262 1586.712262 1586.712262 1586.712262 Peak counts 62.9508 48.53701 107.7373 137.6723 183.4448 279.8358 360.6083 392.8723 Concentration Volume of of chlorine (% chloroform volume) added 95 90 80 70 60 40 30 20 9.5 mL 9 mL 8 mL 7 mL 6 mL 4 mL 3 mL 2 mL Wave number(cm1) 760.5276014 760.5276014 760.5276014 760.5276014 760.5276014 760.5276014 760.5276014 760.5276014 Peak counts 854.4691 629.294 742.5334 655.9348 613.8774 440.0543 374.7844 270.9479 Unknown benzene/chloroform sample wave number (cm-1) peak counts 1586.712262 293.2169 760.5276014 431.0592 (ii) Ethanol Concentration of ethanol (% volume) 10 15 20 30 40 50 60 70 80 Volume of ethanol added 1.0 mL 1.5 mL 2.0 mL 3.0 mL 4.0 mL 5.0 mL 6.0 mL 7.0 mL 8.0 mL Volume of water added 9.0 mL 8.5 mL 8.0 mL 7.0 mL 6.0
Add 0.5 ml concentrated HCl and 1.0 ml 15% KI solution. Mixed exactly 1 minute and leave for 5 minutes in a dark place. Add 0.5 ml starch solution, 20 ml distilled water. Mix and titrate with sodium thiosufate solution. Calculate the exact normality of Na2S2O3 knowing that in this chemical reaction 1 gram-equivalent of K2Cr2O7 react with 1 gram-equivalent of Na2S2O3 (1 mole K2Cr2O7 react with 6 moles Na2S2O3).
Chemistry Department Chemistry 221 Lab Report Lab report #2 Name: Fatima Mustafa Student Number: 1120705 Date: 8/7/2014 Simple Distillation & Fractional Distillation Objectives: 1) To purify a compound by separating it from a non-volatile or less-volatile material. 2) To separate a mixture of two miscible liquids (liquids that mix in all proportions) Procedure: Simple distillation: 1- Make a mixture of (acetone-water) 50 mL each and pour it into a 250 mL round bottomed flask. 2- Add 3-4 boiling chips to avoid bumping. 3- Put together the set up as shown in the figure below 4- Record the temperature at each 5-mL interval. Do not distill to dryness.
CHE 131 Spring 2008 Experiment 4 - Determination of acetic acid in vinegar Preliminary Reading: Chang, 9th ed., section 4.7, pp. 150-153 Introduction: The principal component of vinegar (besides water) is acetic acid, HC2H3O2, a weak acid. In this experiment you will determine the concentration of acetic acid in a vinegar sample by titrating the acetic acid with the strong base sodium hydroxide, NaOH. The stoichiometry of the neutralization reaction is as follows: Molecular: Net Ionic: Neutralization: HC2H3O2(aq) + NaOH(aq) → NaC2H3O2(aq) + H2O HC2H3O2(aq) + OH¯ (aq) → C2H3O2+ (aq) + H2O H+(aq) + OH¯(aq) → H2O(aq) (1) (2) (3) Definition: The end point (also known as the equivalence point) of a titration occurs when the initial number of moles of H+ from the acid has been exactly neutralized by an equal number of moles of OH¯ ion from the sodium hydroxide: moles H+ = moles OH¯ (4) The only species present at the end point are the products, sodium acetate and water. For reasons that are beyond the scope of the material covered so far (but which will be covered in CHE 132), the solution is very slightly basic at the end point of a weak acid-strong base titration.
Table of content No | Title | Pages | 1 | Abstract | 2 | 2 | Introduction | 2,3 | 3 | Objectives | 3 | 4 | Theory | 4,5 | 5 | Apparatus | 6 | 6 | Experimental procedure | 7,8 | 7 | Results | 8 - 13 | 8 | Sample calculations | 14 - 17 | 9 | Discussion | 18,19 | 10 | Conclusion | 19 | 11 | Recommendations | 20 | 12 | References | 20 | 13 | Appendices | 20 | Abstract Acetic acid is an organic compound with chemical formula CH3COOH. Apart from water, acetic acid is the main component of vinegar. In this experiment, the concentration of acetic acid in vinegar can be determined by performing titration process. In the first experiment , solution of KHP is being titrated with NaOH solution. To get accurate result, this titration process are repeated for another two times.
The third test will utilize thin layer chromatography to evaluate the purity of the aspirin as well as testing for the presence of leftover salicylic acid or other by products of the reactions. Experimental: Week 1: For the synthesis of the aspirin, 250 mL of water was boiled. 1.5 g. of salicylic acid were poured on a test tube. Then, 3.5 mL of acetic anhydride and four drops of 85% phosphoric acid were added. A cotton ball was placed to prevent vapor escape.
LIQUID-LIQUID EXTRACTION OF BENZOIC ACID J Wright Organic Chem Lab 1 Tuesday 1:40-5 Ian Stubbs LIQUID-LIQUID EXTRACTION OF BENZOIC ACID PURPOSE: The purpose of this experiment was to extract benzoic acid from an aqueous of benzoic acid using methylene chloride, use liquid-liquid extraction to calculate the distribution coefficient of benzoic acid and to determine whether a single extraction or multiple extractions are more efficient. Add in the table of physical constants. See the attachment for the lab format. PROCEDURE: Gather a two stock solution that includes; 0.02M of sodium hydroxide (NaOH) aqueous solution and 0.02M of benzoic acid aqueous solution. For a single extraction, use a 50mL graduated cylinder and measure out 50mL of the benzoic acid solution into a 125mL separatory funnel.
At this point the volume of base used to neutralized the acid can be determined. Phenolphthalein is the indicator which is colorless in an acid but changes to a faint and permanent pink color in base. The purpose of this experiment is to prepare a sample for titration with a base, become familiar with a buret while using proper titration technique in reaching an end point. Hypothesis : If I titrate a base of known concentration with an acid of unknown concentration then I can determine the concentration can be calculated because of the titration calculation. Materials : • Vinegar • Two small beakers (150mL) • 250-mL Erlenmeyer flask • 10-mL graduated cylinder • 50-mL buret • Buret clamp • Small funnel • M NaOH Hazards : • Chemical spill • Broken glass
Experiment 3 Title: Fluid Properties: Density and Viscosity Date: 20th October 2011 Abstract: Introduction: Experimental Procedure: Five liquids were tested for Density measurements. These liquids included Vegetable oil, corn syrup, shampoo and glycerol. For viscosity measurement only three liquids were tested such as shampoo, glycerol and vegetable oil. Part I – Density Measurement The density of the test fluid was found by weighing a known volume of the liquid using the graduated cylinder. The cylinder was weighed empty, and then graduated cylinder was filled to a certain volume according to the graduations on it and weighed again.