A powder contains FeSO4⋅7H2O (molar mass=278.01 g/mol),(molar mass=278.01 g/mol), among other components. A 3.455 g sample...
A powder contains FeSO4⋅7H2O (molar mass=278.01 g/mol),(molar mass=278.01 g/mol), among other components. A 3.455 g sample of the powder was dissolved in HNO3 and heated to convert all iron to Fe3+. The addition of NH3 precipitated Fe2O3⋅?H2O, which was subsequently ignited to produce 0.502 g Fe2O3.
What was the mass of FeSO4⋅7H2O in the 3.455 g sample?
Please include every step.
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A powder contains FeSO4⋅7H2O (molar mass=278.01 g/mol),(molar
mass=278.01 g/mol), among other components. A 3.455 g sample...
A powder contains FeSO4⋅7H2OFeSO4⋅7H2O (molar mass=278.01 g/mol),(molar mass=278.01 g/mol), among other components. A 2.595 g2.595 g...
A powder contains FeSO4⋅7H2OFeSO4⋅7H2O (molar mass=278.01 g/mol),(molar mass=278.01 g/mol), among other components. A 2.595 g2.595 g sample of the powder was dissolved in HNO3HNO3 and heated to convert all iron to Fe3+.Fe3+. The addition of NH3NH3 precipitated Fe2O3⋅xH2O,Fe2O3⋅xH2O, which was subsequently ignited to produce 0.413 g Fe2O3.0.413 g Fe2O3. What was the mass of FeSO4⋅7H2OFeSO4⋅7H2O in the 2.595 g2.595 g sample? mass of FeSO4⋅7H2OFeSO4⋅7H2O:
A powder contains FeSO4 7 H,O (molar mass = 278.01 g/mol), among other components. A 3.995...
A powder contains FeSO4 7 H,O (molar mass = 278.01 g/mol), among other components. A 3.995 g sample of the powder was dissolved in HNO2 and heated to convert all iron to Fe3*. The addition of NH3 precipitated Fe,O2 - xH,O, which was subsequently ignited to produce 0.210 g Fe2O3. What was the mass of FeSO4 7H,0 in the 3.995 g sample? mass of FeSO4 7H,O: ge
A powder contains FeSO4 7 H,O (molar mass = 278.01 g/mol), among other...
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21 Twenty dietary iron tablets with a total mass of 20.131 g were ground and mixed thoroughly. Then 2.998 g of the powder were dissolved in HNO3 and heated to convert all the iron (FeSO4.7H20) to Fe2O3.XH20. Addition of NH3 precipitated Fe,O3.XH20, which was ignited to give 0.264 g of Fe2O3 (M.wt. = 159.69 g/mol). What is the average mass of FeSO4.7H20 (M.wt. = 278.01 g/mol) in each tablet? * (2 points)
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6. a. What is the percent by mass of water in iron(II) sulfate heptahydrate, FeSO4•7H2O (or what percent of the molar mass of FeSO4•7H2O is due to the waters of crystallization)? b. What mass due to waters of crystallization is present in a 3.38-g sample of FeSO4•7H2O?
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The active ingredient in a zinc nutritional supplement is ZnSO4 .7H2O (molar mass 287.58 g/mol). Ten zinc tablets containing a mix of the active ingredient and an inactive filler were ground and mixed together thoroughly. The total mass of these 10 tablets was 10.600 g. A 1.980 g sample of the finely ground tablets was dissolved in an acidic solution. The solution tion of (NH4)PO to the s the precipitation of ZnNH,PO4. The precipitate was filtered and dried, then ignited...
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A 0.52900.5290 g solid sample containing a mixture of LaCl3LaCl3 (molar mass = 245.26 g/mol) and Ce(NO3)3Ce(NO3)3 (molar mass = 326.13 g/mol) was dissolved in water. The solution was titrated with KIO3KIO3, producing the precipitates La(IO3)3La(IO3)3 and Ce(IO3)3Ce(IO3)3. For the complete titration of both La3+La3+ and Ce3+Ce3+, 42.2742.27 mL of 0.12130.1213 M KIO3KIO3 was required. Calculate the mass fraction of LaLa and CeCe in the sample. mass fraction La:______ g LA/ g Sample mass fraction Ce:______ g Ce/ g Sample
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A powder contains FeSO4 7 H,O (molar mass = 278.01 g/mol), among other components. A 3.995 g sample of the powder was dissolved in HNO2 and heated to convert all iron to Fe3*. The addition of NH3 precipitated Fe,O2 - xH,O, which was subsequently ignited to produce 0.210 g Fe2O3. What was the mass of FeSO4 7H,0 in the 3.995 g sample? mass of FeSO4 7H,O: ge
A powder contains FeSO4 7 H,O (molar mass = 278.01 g/mol), among other...
21 Twenty dietary iron tablets with a total mass of 20.131 g were ground and mixed thoroughly. Then 2.998 g of the powder were dissolved in HNO3 and heated to convert all the iron (FeSO4.7H20) to Fe2O3.XH20. Addition of NH3 precipitated Fe,O3.XH20, which was ignited to give 0.264 g of Fe2O3 (M.wt. = 159.69 g/mol). What is the average mass of FeSO4.7H20 (M.wt. = 278.01 g/mol) in each tablet? * (2 points)
The active ingredient in a zinc nutritional supplement is ZnSO4 .7H2O (molar mass 287.58 g/mol). Ten zinc tablets containing a mix of the active ingredient and an inactive filler were ground and mixed together thoroughly. The total mass of these 10 tablets was 10.600 g. A 1.980 g sample of the finely ground tablets was dissolved in an acidic solution. The solution tion of (NH4)PO to the s the precipitation of ZnNH,PO4. The precipitate was filtered and dried, then ignited...
28 > The active ingredient in a zinc nutritional supplement is ZnSO, 7H, (molar mass=287.58 g/mol). Ten zinc tablets containing a mix of the active ingredient and an inactive filler were ground and mixed together thoroughly. The total mass of these 10 tablets was 11.285 g. A 2.056 g sample of the finely ground tablets was dissolved in an acidic solution. The solution was neutralized with ammonia and subsequently warmed in a water bath. Addition of (NH), PO, to the...
A 0.5137 g solid sample containing a mixture of LaCl, (molar mass = 245.26 g/mol) and Ce(NO3), (molar mass = 326.13 g/mol) was dissolved in water. The solution was titrated with KIO, producing the precipitates La(IO,), and Ce(IO). For the complete titration of both La and Ce+, 42.25 mL of 0.1204 M KIO, was required. Calculate the mass fraction of La and Ce in the sample. mass fraction La: g La g sample mass fraction Ce: g Ce g sample
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25. FeO, (molar mass = 159.7 g/mol) reacts with CO (molar maw28.0 /mol) according to the equation below. Calculate the number of moles of iron produced when 185,5 g CO reacts with excess F,O Fe(s) + 3 CO(g) - 300,() +2 Fe(s) A. 2.208 mol B. 13.25 mol C. 4.415 mol D. 9.93 mol E 3.311 mol 26. Tin(II) fluoride is added to some dental prod- ucts to prevent cavities. How many grams of tin(II) fluoride can be made from...
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