FIND THE PERCENTAGE YIELD, and include the moles of the reaction (part 2) Part 2:Running the reaction:1.15 g of the acetanilide and 4.8 mL acetic acid were placed in a 50 mL Erlenmeyer flask2.80 mL of 4.1 M bromine in acetic acid (1:4) were added dropwise with a Pasteur pipette.The mixture was swirled until everything dissolved (~20 minutes)The solution was transferred to a 150 mL beaker containing 30 mL of waterA solution of sodium bisulfite was added until the mixture was clear (~2 mL)Product isolation:The solids were isolated using a vacuum filtration with a small Büchner funnel, washedwith 5 mL of ice-cold waterThe crude was dissolved in 6 mL of hot ethanolHot water (3 mL) was added which caused a solid to formThe mixture was allowed to cool to room temperature (~15 minutes) before being placedin an ice bath (15 minutes)White crystals were isolated by vacuum filtration and driedProduct characterization:1.55 g of the productМ.р.: 164.8-166.2 °C tool in organic chemistry, especially in multi-step synthesis. In this experiment, p-bromoanilinewas synthesized in three steps starting from aniline.Equation 1:NH2NH,Br-BrBr2Brplus mono-and disubstitution productsEquation 2:NH2NHEquation 3:`NHNHBr2BrEquation 4:NHNH2Acid hydrolysisBrBr

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Answered: FIND THE PERCENTAGE YIELD, and include…

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Chemistry

FIND THE PERCENTAGE YIELD, and include the moles of the reaction (part 2)

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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6.20 mL of tap water sample is taken in a conical flask and 1 mL of pH 10 buffer and 3 drops of iochrome black-T indicator are added and when titrated with 0.001 M EDTA solution, 16 mL EDTA is spent, so the hardness of the water is determined by French Hardness and German Hardness Calculate in terms.
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Standardization of 0.10 M HCl1. Take three (3) clean and properly labeled 250-mL Erlenmeyer flasks. Into the three flasks, weigh 0.1 g of the primary standard Na2CO3 to the nearest 0.1 mg. Record the weights of the primary standard.2. Add about 75.0 mL of boiled distilled water and swirl to dissolve the solids.3. Add 2 to 3 drops of phenolphthalein indicator. Record the initial burette reading and titrate with the prepared 0.10 M HCl solution until phenolphthalein endpoint.4. Record the final burette reading for each titration in your data sheetDetermination of Ksp and Molar Solubility1. Add Ca(OH)2 to 250.0 mL distilled water with stirring until equilibrium is achieved. 2. Filter the undissolved precipitate. Measure out 50.0 mL of the supernate into a 250-mL Erlenmeyer flask using a pipette.3. Add a few drops of phenolphthalein indicator and titrate with standardized HCl solution until endpoint is achieved.4. Record the volume the HCl solution used. Perform two more trials.…
Standardization of 0.10 M HCl1. Take three (3) clean and properly labeled 250-mL Erlenmeyer flasks. Into the three flasks, weigh 0.1 g of the primary standard Na2CO3 to the nearest 0.1 mg. Record the weights of the primary standard.2. Add about 75.0 mL of boiled distilled water and swirl to dissolve the solids.3. Add 2 to 3 drops of phenolphthalein indicator. Record the initial burette reading and titrate with the prepared 0.10 M HCl solution until phenolphthalein endpoint.4. Record the final burette reading for each titration in your data sheetDetermination of Ksp and Molar Solubility1. Add Ca(OH)2 to 250.0 mL distilled water with stirring until equilibrium is achieved. 2. Filter the undissolved precipitate. Measure out 50.0 mL of the supernate into a 250-mL Erlenmeyer flask using a pipette.3. Add a few drops of phenolphthalein indicator and titrate with standardized HCl solution until endpoint is achieved.4. Record the volume the HCl solution used. Perform two more trials.…
1. A 50.00 mL stock CaCl2 solution was diluted with water in a 250.0-mL volumetric flask. A 25.00 mL aliquot of this was further diluted to a final volume of 100.0 mL. Finally, 20.00-mL aliquot of the resulting solution was analyzed and found to contain 0.1500 M CaCh2 Solve for the concentration of the stock solution in M. 2. A 50.00 mL stock CaCl2 solution was diluted with water in a 250.0-mL volumetric flask. A 25.00 mL aliquot of this was further diluted to a final volume of 100.0 mL. Finally, 20.00-mL aliquot of the resulting solution was analyzed and found to contain 0.1200 g CaCl2 Solve for %w/v CaCl2 in the stock solution.
A 0.1 g amine-containing compound is dissolved in water then diluted to 100 mL. You subject it to spectroscopic analysis, in order to get the concentration of amine in this compound. Next, you get 1 mL of the previously diluted sample then dilute it again to 250 mL for measurement. Then, you fill 3/4 of a 1-cm cuvette with this diluted sample, and you run an analysis using an AAS. The recorded absorbance is 0.545 at 410 nm. What is the molecular weight of the compound? (The molar absorptivity is 1.23 x 104 cm-1 mol-1 L.)
1. What is the MW of the analyte?2. What is the meq of the analyte?3. What will be the weight (in grams) of the analyte if the standardization is to be quartered?4. What will be Normality of the solution if 7.5ml of the titrant was consumed in the standardization?5. What is the average Normality if two or more trials were conducted with the values of 0.102N and 0.105N?
TITRIMETRIC DATA SAMPLE: CANE VINEGAR % acidity in label: 4.5% %purity of KHP: 99.80% FORMULA WEIGHT of KHP: 204.22 g/mol STANDARDIZATION OF NaOH SOLUTION TRIAL 1 TRIAL 2 TRIAL 3 Weight of KHP, g 0.1012 0.1004 0.09987 Initial volume of NaOH, mL 5.00 10.01 Final volume of NaOH, mL 4.95 9.99 14.93 Molarity of NaOH Average Molarity of NaOH ANALYSIS OF ACETIC ACID IN A VINEGAR SAMPLE TRIAL 1 TRIAL 2 TRIAL 3 Volume of vinegar, mL Initial volume of NaOH, mL 1.00 1.00 1.00 14.98 22.90 30.87 Final volume of NaOH, mL 22.84 30.77 38.75 Molarity of acetic acid Average molarity of acetic acid ANALYSIS OF CARBONIC ACID IN A SODA SAMPLE TRIAL 1 TRIAL 2 TRIAL 3 Volume of soda, mL 20.0 20.0 20.0 Initial volume of NaOH, mL 20.20 22.05 23.93 Final volume of NaOH, mL 22.03 23.89 25.8 Molarity of carbonic acid Average molarity of carbonic acid
Read the problem and answer the following questions. Reactions are attached in the picture Yuno wants to assess the quality of water in the Clover Kingdom and the Heart Kingdom. In order to do this, he took a 200.0 ml sample (T= 20oC) from the two areas and titrated them with sodium thiosulfate. The water from the Clover Kingdom used up 7.15 ml of the titrant while 7.65 ml where used on the Heart Kingdom’s water. Prior to this, 0.1000g of potassium iodate (FM: 214.01 g/mol; 99.97% purity) was weighed and subsequently dissolved in 150.0 ml of distilled water. He took 20.00 ml aliquot of this solution and added 20.00 ml of distilled water. He then treated the solution with potassium iodide and sulfuric acid. Finally, Yuno titrated the solution with 13.7 ml sodium thiosulfate titrant. Determine the concentration of the titrant in M. Calculate the dissolved oxygen (DO) content of the two water samples in ppm O2.