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(Solved) Experiment 1: Standardize the Iodine Solution Part 1: Prepare the Materials added 0.


Experiment1:StandardizetheIodineSolution Part1:PreparetheMaterials added0.100g ofascorbicacidto100mLvolumetricflask added30mLwatertovolumettric totalvolume waterinvolumetric=100mL added20mLascorbicacidsolutionintoerlenmeyer added 1.0mLstarchindicatorsolutionintoerlenmeyer Part2:PerformaCoarseTitration added 50mLof0.015Mofiodinesolutionintoburette initialburettereading=50mL lastdispensedvolumecolorless=6.43mL firstdispensedvolumecolorchanged(black)=7.78mL Part3:PerformaFineTitration 1sttrial: added20mLascorbicacidsolutionintoerlenmeyer added1.0mLstarchindicatorsolutionintoerlenmeyer added50mLof0.015Mofiodine solutionintoburette initialburettereading=50mL finaldispensedvolume=7.61mL 2nd trial: added20mLascorbicacidsolutionintoerlenmeyer added1.0mLstarchindicatorsolutionintoerlenmeyer added50mLof0.015Mofiodinesolutionintoburette initialburette reading=50mL finaldispensedvolume=7.59mL 3rdtrial: added20mLascorbicacidsolutionintoerlenmeyer added1.0mLstarchindicatorsolutionintoerlenmeyer added50mL of0.015Mofiodinesolutionintoburette initialburettereading= 50mL finaldispensedvolume=7.61mL Finalanswer: iodinesolutionremainedinburetteaftercolorchanged=42.4 mL iodinesolutionnecessarytochangedcolor=7.6mL Experiment2:DeterminetheConcentrationofAscorbicAcidinOrangeJuice Part1:PrepareaSampleofFreshOrange Juice added40.0mLOJ-freshtoerlenmeyer added1.0starchindicatorsolutionintoerlenmeyer Part2:PerformaCoarseTitration added50mL0.015Miodinesolutionintoburette initialburettevolume=50mL lastvolumedispensed(orange)=6.26mL firstvolumedispensed(darkredorange)=7.49mL Part3:PerformaFineTitration 1sttrial: added50mL 0.015Miodinesolutionintoburette initialburettevolume=50mL firstvolumedispensed (darkredorange)=6.71mL 2ndtrial: firstvolumedispensed(darkredorange)=6.70mL 3rdtrial: firstvolumedispensed(darkredorange)=6.72mL Finalanswer: Iodinesolution remainedinburetteaftercolorchanged=43.0mL Iodinenecessarytochangedcolor= 7.0mL OLDORANGEJUICE Part1:PrepareaSampleofOLDOrangeJuice added40.0 mLOJ-weekOLDtoerlenmeyer added1.0starchindicatorsolutionintoerlenmeyer Part 2:PerformaCoarseTitration added50mL0.015Miodinesolutionintoburette initialburettevolume=50mL lastvolumedispensed(orange)=2.12mL firstvolumedispensed (darkredorange)=3.28mL Part3:PerformaFineTitration 1sttrial: added50mL0.015M iodinesolutionintoburette initialburettevolume=50mL firstvolumedispensed(darkred orange)=2.69mL 2ndtrial: firstvolumedispensed(darkredorange)=2.68mL 3rdtrial: firstvolumedispensed(darkredorange)=2.71mL Finalanswer: Iodinesolutionremained inburetteaftercolorchanged=47.30mL Iodinesolutionnecessarytochangedcolor=2.7 mL

SHORT ANSWER

Experiment 1: Standardize the Iodine Solution

Lab Results

1. For each titration, record the following data in the table below. If you had to perform the fine titration three times, discard the

volume that is different. Record volumes using all the digits provided by the lab even if they are zero.

Coarse Titration Fine Titration #1 Fine Titration #2 initial volume in the burette

final volume in the burette

volume dispensed in the titration

volume of ascorbic acid solution

volume of indicator Data Analysis

2. Calculate the molarity of the ascorbic acid solution. The molar mass of ascorbic acid is 176.12 g/mol.

3. For each titration, calculate and record the following data. If you had to perform the fine titration three times, discard the volume

that is different. Record volumes using all the digits provided by the lab even if they are zero. Please note that in a standardization

titration the molarity of the analyte (ascorbic acid) is known, whereas the molarity of the titrant (I2) needs to be calculated.

Coarse Titration Fine Titration #1 Fine Titration #2 volume of I2 dispensed (mL)

moles of ascorbic acid

moles of I2 based on the reaction stoichiometry

molarity of I2 (mol/L)

average molarity of I2 using the fine titrations (mol/L) Experiment 2: Determine the Concentration of Ascorbic Acid in Orange Juice

Lab Results

1. For each titration of the fresh orange juice, record the following data in the table below. If you had to perform the fine titration three

times, discard the volume that is different. Record volumes using all the digits provided by the lab even if they are zero.

Coarse Titration Fine Titration #1 Fine Titration #2 initial volume in the burette

final volume in the burette

volume dispensed in the titration

volume of fresh orange juice

volume of indicator 2. For each titration of the week old orange juice, record the following data in the table below. If you had to perform the fine titration

three times, discard the volume that is different. Record volumes using all the digits provided by the lab even if they are zero.

Coarse Titration about:blank Fine Titration #1 Fine Titration #2 Page 1 of 3 4/29/16, 7:25 PM initial volume in the burette

final volume in the burette

volume dispensed in the titration

volume of fresh orange juice

volume of indicator Data Analysis

3. For each of the fresh orange juice titrations, calculate and record the following data. If you had to perform the fine titration three

times, discard the volume that is different. Record volumes using all the digits provided by the lab even if they are zero.

Coarse Titration Fine Titration #1 Fine Titration #2 volume of I2 dispensed (mL)

moles of I2

moles of ascorbic acid based on the reaction stoichiometry

molarity of ascorbic acid in orange juice (mol/L)

average molarity of I2 using the fine titrations (mol/L) 4. For each of the week old orange juice titrations, calculate and record the following data. If you had to perform the fine titration three

times, discard the volume that is different. Record volumes using all the digits provided by the lab even if they are zero.

Coarse Titration Fine Titration #1 Fine Titration #2 volume of I2 dispensed (mL)

moles of I2

moles of ascorbic acid based on the reaction stoichiometry

molarity of ascorbic acid in orange juice (mol/L)

average molarity of I2 using the fine titrations (mol/L) 5. Calculate the average concentration (C) of ascorbic acid in the sample of fresh orange juice used in this lab in mg/mL. The molar

mass of ascorbic acid is 176.12 g/mol. 6. Calculate the average concentration (C) of ascorbic acid in the sample of week old orange juice used in this lab in mg/mL. The

molar mass of ascorbic acid is 176.12 g/mol. Conclusions

1. Suppose a student calculates a concentration of 0.25 mg/mL for a sample of commercial orange juice. How many cups (240 mL)

does she have to drink to reach the minimum requirement of 75 mg? 2. What do you think happens to the ascorbic acid over time? Hint: oxygen, an oxidizing agent, makes up 20% of our air. 3. Orange juice is not the only juice containing vitamin C. Grapefruit juice, the pink-red juice in the figure below, contains 93.90 mg of

vitamin C per cup. about:blank Page 2 of 3 4/29/16, 7:25 PM How many mL of 0.0150 M iodine solution will be needed to oxidize all the vitamin C in ½ cup of grapefruit juice? The molar mass

of ascorbic acid is 176.12 g/mol. 4. Balance the redox reaction below. about:blank Page 3 of 3

 


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