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28 Sep 2019
I am working on this lab but can't seem to figure out how tofinish it.
1. For the NEW bottle of hydrogenperoxide, record and calculate the following:
a
Volumeof potassium permanganate used in each titration (mL)
50mL
b
Thevolume of potassium permanganate required to titrate 10 mL of thenew hydrogen peroxide (mL) 18.04mL
c
How many moles of potassiumpermanganate were required to titrate 10mL of the new hydrogenperoxide (moles)
0.013mol
d
Given the stoichiometry of thereaction, how many moles of hydrogen peroxide were in the 10mL ofthe solution (moles)
e
How many grams ofH2O2 were in the hydrogen peroxide solution(MW of H2O2 is 34.01) (grams)
f
1 mL ofwater weighs 1 g. Using this information and the numberof grams of H2O2 produced in the reaction, calculate the percentmass of H2O2 in the NEW solution. (% mass = (mass H2O2 /mass water) * 100%)
2. Repeat the calculations for the OLD bottle ofH2O2:
a
Volumeof potassium permanganate used in each titration (mL): 50mL
b
Thevolume of potassium permanganate required to titrate 10 mL of theold hydrogen peroxide (mL) 12.60mL
c
How many moles of potassiumpermanganate were required to titrate 10mL of the old hydrogenperoxide (moles) 0.013mol
d
Given the stoichiometry of thereaction, how many moles of hydrogen peroxide were in the 10mL ofthe solution (moles)
e
How many grams ofH2O2 were in the hydrogen peroxide solution(MW of H2O2 is 34.01) (grams)
f
1 mL ofwater weighs 1 g. Using this information and the numberof grams of H2O2 produced in the reaction, calculate the percentmass of H2O2 in the OLD solution. (% mass = (mass H2O2 /mass water) * 100%)
I am working on this lab but can't seem to figure out how tofinish it.
1. For the NEW bottle of hydrogenperoxide, record and calculate the following:
a | Volumeof potassium permanganate used in each titration (mL) | 50mL |
b | Thevolume of potassium permanganate required to titrate 10 mL of thenew hydrogen peroxide (mL) | 18.04mL |
c | How many moles of potassiumpermanganate were required to titrate 10mL of the new hydrogenperoxide (moles) | 0.013mol |
d | Given the stoichiometry of thereaction, how many moles of hydrogen peroxide were in the 10mL ofthe solution (moles) | |
e | How many grams ofH2O2 were in the hydrogen peroxide solution(MW of H2O2 is 34.01) (grams) | |
f | 1 mL ofwater weighs 1 g. Using this information and the numberof grams of H2O2 produced in the reaction, calculate the percentmass of H2O2 in the NEW solution. (% mass = (mass H2O2 /mass water) * 100%) |
2. Repeat the calculations for the OLD bottle ofH2O2:
a | Volumeof potassium permanganate used in each titration (mL): | 50mL |
b | Thevolume of potassium permanganate required to titrate 10 mL of theold hydrogen peroxide (mL) | 12.60mL |
c | How many moles of potassiumpermanganate were required to titrate 10mL of the old hydrogenperoxide (moles) | 0.013mol |
d | Given the stoichiometry of thereaction, how many moles of hydrogen peroxide were in the 10mL ofthe solution (moles) | |
e | How many grams ofH2O2 were in the hydrogen peroxide solution(MW of H2O2 is 34.01) (grams) | |
f | 1 mL ofwater weighs 1 g. Using this information and the numberof grams of H2O2 produced in the reaction, calculate the percentmass of H2O2 in the OLD solution. (% mass = (mass H2O2 /mass water) * 100%) |
papayaprofessorLv10
12 Oct 2022
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Deanna HettingerLv2
28 Sep 2019
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