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1. A student dissolves 2.006 g of FeSO4 7 H₂O in 40 mL of sulfuric acid and then dilutes it to 100.00 mL in a volumetric flask as described is Procedure steps 3-7. He then uses a pipet to transfer 10.00 mL of this solution into a flask for titration as in Procedure step 11. What mass of FeSO4-7 H₂O was transferred into the titration flask? (Keep this question in mind as you do your calculations for Pre-Lab Question 2 and for your calculations with your own data.) 2. Your partner has completed three acceptable titrations for standardizing the dilute potassium permanganate solution and he gives you all of the data. The solid standard used was FeSO4-7 H₂O, and it was dissolved and diluted to 100.00 mL. a. Calculate the molarities for the trials (Hint: you are going to need the balanced ionic equation and the formula mass of ferrous sulfate heptahydrate.) Mass of Standard Volume of Blank Volume of Standard Initial Buret Reading Final Buret Reading Volume of Titrant Molarity KMnO4 2.047 g 0.04 mL Trial 1 10.00 mL 1.57 mL 19.75 mL Trial 2 10.00 mL 2.15 mL 20.98 mL Trial 3 10.00 mL 1.30 mL 19.33 mL Trial 4 10.00 mL 3.53 mL 21.93 mL b. Examine your partner's results and determine which three trials should be used to determine the average molarity of the permanganate solution; then using the appropriate values calculate the average molarity of the potassium permanganate solution.

1. A student dissolves 2.006 g of FeSO4 7 H₂O in 40 mL of sulfuric acid and then dilutes it to 100.00 mL in a volumetric flask as described is Procedure steps 3-7. He then uses a pipet to transfer 10.00 mL of this solution into a flask for titration as in Procedure step 11. What mass of FeSO4-7 H₂O was transferred into the titration flask? (Keep this question in mind as you do your calculations for Pre-Lab Question 2 and for your calculations with your own data.) 2. Your partner has completed three acceptable titrations for standardizing the dilute potassium permanganate solution and he gives you all of the data. The solid standard used was FeSO4-7 H₂O, and it was dissolved and diluted to 100.00 mL. a. Calculate the molarities for the trials (Hint: you are going to need the balanced ionic equation and the formula mass of ferrous sulfate heptahydrate.) Mass of Standard Volume of Blank Volume of Standard Initial Buret Reading Final Buret Reading Volume of Titrant Molarity KMnO4 2.047 g 0.04 mL Trial 1 10.00 mL 1.57 mL 19.75 mL Trial 2 10.00 mL 2.15 mL 20.98 mL Trial 3 10.00 mL 1.30 mL 19.33 mL Trial 4 10.00 mL 3.53 mL 21.93 mL b. Examine your partner's results and determine which three trials should be used to determine the average molarity of the permanganate solution; then using the appropriate values calculate the average molarity of the potassium permanganate solution.

Chemistry & Chemical Reactivity
Chemistry & Chemical Reactivity
10th Edition
ISBN:9781337399074
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter7: The Structure Of Atoms And Periodic Trends
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Problem 65IL: Nickel(II) formate [Ni(HCO2)2] is widely used as a catalyst precursor and to make metallic nickel....
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PRE-LAB QUESTIONS 1. A student dissolves 2.006 g of FeSO4-7 H₂O in 40 mL of sulfuric acid and then dilutes it to 100.00 mL in a volumetric flask as described is Procedure steps 3-7. He then uses a pipet to transfer 10.00 mL of this solution into a flask for titration as in Procedure step 11. What mass of FeSO4-7 H₂O was transferred into the titration flask? (Keep this question in mind as you do your calculations for Pre-Lab Question 2 and for your calculations with your own data.) 2. Your partner has completed three acceptable titrations for standardizing the dilute potassium permanganate solution and he gives you all of the data. The solid standard used was FeSO4-7 H₂O, and it was dissolved and diluted to 100.00 mL. a. Calculate the molarities for the trials (Hint: you are going to need the balanced ionic equation and the formula mass of ferrous sulfate heptahydrate.) Mass of Standard Volume of Blank Volume of Standard Initial Buret Reading Final Buret Reading Volume of Titrant Molarity KMnO4 2.047 g 0.04 mL Trial 1 10.00 mL 1.57 mL 19.75 mL Trial 2 10.00 mL 2.15 mL 20.98 mL Trial 3 10.00 mL 1.30 mL 19.33 mL Trial 4 10.00 mL 3.53 mL 21.93 mL b. Examine your partner's results and determine which three trials should be used to determine the average molarity of the permanganate solution; then using the appropriate values calculate the average molarity of the potassium permanganate solution.
Transcribed Image Text:PRE-LAB QUESTIONS 1. A student dissolves 2.006 g of FeSO4-7 H₂O in 40 mL of sulfuric acid and then dilutes it to 100.00 mL in a volumetric flask as described is Procedure steps 3-7. He then uses a pipet to transfer 10.00 mL of this solution into a flask for titration as in Procedure step 11. What mass of FeSO4-7 H₂O was transferred into the titration flask? (Keep this question in mind as you do your calculations for Pre-Lab Question 2 and for your calculations with your own data.) 2. Your partner has completed three acceptable titrations for standardizing the dilute potassium permanganate solution and he gives you all of the data. The solid standard used was FeSO4-7 H₂O, and it was dissolved and diluted to 100.00 mL. a. Calculate the molarities for the trials (Hint: you are going to need the balanced ionic equation and the formula mass of ferrous sulfate heptahydrate.) Mass of Standard Volume of Blank Volume of Standard Initial Buret Reading Final Buret Reading Volume of Titrant Molarity KMnO4 2.047 g 0.04 mL Trial 1 10.00 mL 1.57 mL 19.75 mL Trial 2 10.00 mL 2.15 mL 20.98 mL Trial 3 10.00 mL 1.30 mL 19.33 mL Trial 4 10.00 mL 3.53 mL 21.93 mL b. Examine your partner's results and determine which three trials should be used to determine the average molarity of the permanganate solution; then using the appropriate values calculate the average molarity of the potassium permanganate solution.
c. You have titrated the first sample of your unknown sample. Using the average molarity of the permanganate solution from Question 1b, complete Trial 1 column. In your calculation, don't forget that only part of the unknown solution is used in the titration. Mass of Unknown #100 Initial Buret Reading Final Buret Reading Volume of Blank Volume of Titrant Mass of Fe(II) in sample % Fe in sample Trial 1 1.103 g 2.17 mL 24.91 mL 0.03 mL 3. Calculate how much 6 M H₂SO4 you will need to add to water to make 200 mL of a 1 M H₂SO4 solution.
Transcribed Image Text:c. You have titrated the first sample of your unknown sample. Using the average molarity of the permanganate solution from Question 1b, complete Trial 1 column. In your calculation, don't forget that only part of the unknown solution is used in the titration. Mass of Unknown #100 Initial Buret Reading Final Buret Reading Volume of Blank Volume of Titrant Mass of Fe(II) in sample % Fe in sample Trial 1 1.103 g 2.17 mL 24.91 mL 0.03 mL 3. Calculate how much 6 M H₂SO4 you will need to add to water to make 200 mL of a 1 M H₂SO4 solution.
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