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Experimental Procedure, Part B.1. What is the purpose of adding NaHCO, to the reaction mixture? Explain....
3. Experimental Pro perimental Procedure, Part B.1. What is the purpose of adding NaHCO, to th...
3. Experimental Pro perimental Procedure, Part B.1. What is the purpose of adding NaHCO, to th balanced equation for its reaction. Iding NaHCO, to the reaction mixture? Explain. Write a Experimental Procedure, Part C. What is the oxidizins arent in the titration? b. What is the color change of the starch indicator that signals the stoichiometric point in 5a. Eight ounces (1 fl. oz = 29.57 mL) of orange juice contains 160% of the recommended daily allowance of vitamin (RDA...
Laboratory Questions Circle the questions that have been assigned. 1. Part A.1. The KIO, sample was...
Laboratory Questions Circle the questions that have been assigned. 1. Part A.1. The KIO, sample was not sur klo, sample was not sufficiently dried. Will the reported molar concentration of the KIO, solution (Part B.3) be too high, too low, or unaffected? Explain. 2. Part A.1. The mass of KIO, used to prepare he mass of KIO, used to renare the solution was measured to be 0.585 g instead of the calculated 0.535 a. Will the molar concentration of th...
I have inputted the experimental data, and now all I need is the info for the...
I have inputted the experimental data, and now all I need is
the info for the yellow cells. :) please help!
Part A: Standarization of Iodine Molar Mass of Ascorbic Acid 176.12 Trial 1 0.1002 Trial 2 0.0995 Trial 3 0.1020 Mass of ascorbic acid (g) Moles of ascobic acid Initial Buret Reading (mL) Final Buret Reading (mL) Net Iodine Added (mL) Ascorbic Acid Back Titration Mass (g) Iodine Molarity 0.00 11.40 11.40 22.75 22.75 34.34 0.0000 0.0000 0.0000 Mean...
I understand part a, I need help with B and C. Thanks! 6-B. Vitamin C (ascorbic...
I understand part a, I need help with B and C. Thanks!
6-B. Vitamin C (ascorbic acid) from foods can be measured by titration with 13: CH4O6 + + H2O = C,H,O + 30 + 2H Ascorbic acid Triiodide Dehydroascorbic acid FM 176.126 Starch is used as an indicator in the reaction. The end point is marked by the appearance of a deep blue starch-iodine complex when unreacted 15 is present. (a) If 29.41 mL of Iz solution are required...
THE COPPER CYCLE: A Series of Reactions Experimental Data From Experimental Procedure - Part A 1....
THE COPPER CYCLE: A Series of Reactions Experimental Data From Experimental Procedure - Part A 1. A student weighed a 25-ml Erlenmeyer flask and found it to be 22.683 g. 2. She added a piece of copper metal to the flask, and found the new mass to be 22.802 g, From Experimental Procedure - Part E 32. The student weighed a watch glass and a clean piece of filter paper, and found the mass to be 55.542 g. 37. After...
1) What chemical is the titrant in this experiment? What chemical is the analyte in this experiment? Experi...
1) What chemical is the titrant in this experiment? What
chemical is the analyte in this
experiment?
Experiment #8: Measuring the Vitamin C Content of Emergen-C™ Objectives: • Students will learn how to use a burette. • Students will learn how to use the iodine starch indicator system to monitor oxidation/reduction reactions. Students will learn how to conduct a titration to determine the amount of analyte in an unknown solution. • Students will learn about ascorbic acid's role as a...
2) What chemical reaction does the titrant contribute to this experiment? CHEM 1A Experiment #8: Measuring the Vit...
2)
What chemical reaction does the titrant contribute to this
experiment?
CHEM 1A Experiment #8: Measuring the Vitamin C Content of Emergen-C™ Objectives: Students will learn how to use a burette. Students will learn how to use the iodine starch indicator system to monitor oxidation/reduction reactions. • Students will learn how to conduct a titration to determine the amount of analyte in an unknown solution. • Students will learn about ascorbic acid's role as a biological reducing agent. Introduction: Vitamin...
Vitamin C Project Lab: Part B: Data analysis Calculate the grams of Vitamin C in your...
Vitamin C Project Lab: Part B: Data analysis Calculate the grams of Vitamin C in your Erlenmeyer. (as in titration #1 ) Calculate the grams of Vitamin C per tablet. Calculate a percent error by comparing your result to the tablet dose above. Determine the % composition of vitamin C in the tablet Build a data table similar to the one you used for titration # 1 to calculate the following: 1. 2 3. 4. Show all your work Trial...
calculate Quantitative Analysis Exp. #5. Determination of Cu % by Using Complexation Reaction 0.01 mol xoSLX...
calculate
Quantitative Analysis Exp. #5. Determination of Cu % by Using Complexation Reaction 0.01 mol xoSLX Part 1. Preparation of reagents. Preparation of EDTA (0.01M) Dry EDTA in the oven for 2 hours. Dissolve needed grams in a 500 ml volumetric flask. 786/2 PESTA Preparation of known copper solution Place 0.2 8 to 0.25 g of pure Cu wire (or shot) in a 100 ml beaker. Add 15 ml conc. HNO, and 1 ml conc. H,SO. Place a watch glass...
Experiment 9 Analysis of an Antacid using the ideal gas law. Calculations: 1) Find moles of...
Experiment 9 Analysis of an Antacid using the ideal gas law.
Calculations:
1) Find moles of CO2
2) Find moles of NaHCO3
3) Find mass of NaHCO3
4) Find mass % of NaHCO3
5) Find average mass % NaHCO3 in Alka-Seltzer
Sheet 23° torr Atmospheric pressure, mmHg 755.0 Temperature of H,O, "C Vapor pressure of H.O at this temperature 21.1 Calculated pressure of CO, in the system, mmHg 733.9 Balanced reaction of NaHCO, and HCl (see Pre-Laboratory Question 4a) =...
3. Experimental Pro perimental Procedure, Part B.1. What is the purpose of adding NaHCO, to th balanced equation for its reaction. Iding NaHCO, to the reaction mixture? Explain. Write a Experimental Procedure, Part C. What is the oxidizins arent in the titration? b. What is the color change of the starch indicator that signals the stoichiometric point in 5a. Eight ounces (1 fl. oz = 29.57 mL) of orange juice contains 160% of the recommended daily allowance of vitamin (RDA...
Laboratory Questions Circle the questions that have been assigned. 1. Part A.1. The KIO, sample was not sur klo, sample was not sufficiently dried. Will the reported molar concentration of the KIO, solution (Part B.3) be too high, too low, or unaffected? Explain. 2. Part A.1. The mass of KIO, used to prepare he mass of KIO, used to renare the solution was measured to be 0.585 g instead of the calculated 0.535 a. Will the molar concentration of th...
I have inputted the experimental data, and now all I need is
the info for the yellow cells. :) please help!
Part A: Standarization of Iodine Molar Mass of Ascorbic Acid 176.12 Trial 1 0.1002 Trial 2 0.0995 Trial 3 0.1020 Mass of ascorbic acid (g) Moles of ascobic acid Initial Buret Reading (mL) Final Buret Reading (mL) Net Iodine Added (mL) Ascorbic Acid Back Titration Mass (g) Iodine Molarity 0.00 11.40 11.40 22.75 22.75 34.34 0.0000 0.0000 0.0000 Mean...
I understand part a, I need help with B and C. Thanks!
6-B. Vitamin C (ascorbic acid) from foods can be measured by titration with 13: CH4O6 + + H2O = C,H,O + 30 + 2H Ascorbic acid Triiodide Dehydroascorbic acid FM 176.126 Starch is used as an indicator in the reaction. The end point is marked by the appearance of a deep blue starch-iodine complex when unreacted 15 is present. (a) If 29.41 mL of Iz solution are required...
THE COPPER CYCLE: A Series of Reactions Experimental Data From Experimental Procedure - Part A 1. A student weighed a 25-ml Erlenmeyer flask and found it to be 22.683 g. 2. She added a piece of copper metal to the flask, and found the new mass to be 22.802 g, From Experimental Procedure - Part E 32. The student weighed a watch glass and a clean piece of filter paper, and found the mass to be 55.542 g. 37. After...
1) What chemical is the titrant in this experiment? What
chemical is the analyte in this
experiment?
Experiment #8: Measuring the Vitamin C Content of Emergen-C™ Objectives: • Students will learn how to use a burette. • Students will learn how to use the iodine starch indicator system to monitor oxidation/reduction reactions. Students will learn how to conduct a titration to determine the amount of analyte in an unknown solution. • Students will learn about ascorbic acid's role as a...
2)
What chemical reaction does the titrant contribute to this
experiment?
CHEM 1A Experiment #8: Measuring the Vitamin C Content of Emergen-C™ Objectives: Students will learn how to use a burette. Students will learn how to use the iodine starch indicator system to monitor oxidation/reduction reactions. • Students will learn how to conduct a titration to determine the amount of analyte in an unknown solution. • Students will learn about ascorbic acid's role as a biological reducing agent. Introduction: Vitamin...
Vitamin C Project Lab: Part B: Data analysis Calculate the grams of Vitamin C in your Erlenmeyer. (as in titration #1 ) Calculate the grams of Vitamin C per tablet. Calculate a percent error by comparing your result to the tablet dose above. Determine the % composition of vitamin C in the tablet Build a data table similar to the one you used for titration # 1 to calculate the following: 1. 2 3. 4. Show all your work Trial...
calculate
Quantitative Analysis Exp. #5. Determination of Cu % by Using Complexation Reaction 0.01 mol xoSLX Part 1. Preparation of reagents. Preparation of EDTA (0.01M) Dry EDTA in the oven for 2 hours. Dissolve needed grams in a 500 ml volumetric flask. 786/2 PESTA Preparation of known copper solution Place 0.2 8 to 0.25 g of pure Cu wire (or shot) in a 100 ml beaker. Add 15 ml conc. HNO, and 1 ml conc. H,SO. Place a watch glass...
Experiment 9 Analysis of an Antacid using the ideal gas law.
Calculations:
1) Find moles of CO2
2) Find moles of NaHCO3
3) Find mass of NaHCO3
4) Find mass % of NaHCO3
5) Find average mass % NaHCO3 in Alka-Seltzer
Sheet 23° torr Atmospheric pressure, mmHg 755.0 Temperature of H,O, "C Vapor pressure of H.O at this temperature 21.1 Calculated pressure of CO, in the system, mmHg 733.9 Balanced reaction of NaHCO, and HCl (see Pre-Laboratory Question 4a) =...
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