This requires the preparation of a 100 ppm Fe standard in a 500 mL standard flask....
This requires the preparation of a 100 ppm Fe standard in a 500 mL standard flask. The iron will be from a ferrous ammonium sulfate hexahydrate salt which has the formula Fe(NH4)2(SO4)2.6H2O with a molar mass of 392.14 g mol-1. If the atomic mass of Fe is 55.84 g mol-1, what mass of salt is needed?
What steps do i need to take for this?
Homework Answers
100 ppm=100mg/L or 50 mg in 500 mL solution.
50 mg De solution needed.
55.84 g Fe is in 392.14 g salt
0.05 g Fe is in (392.14×0.05)/55.84=0.35 g salt needed.
Weigh 0.35 g salt and dissolve in 500 mL solvent to prepare 100 ppm Fe solution.
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This requires the preparation of a 100 ppm Fe standard in a 500
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You wish to prepare 250.0250.0 mL of a 225.0225.0 ppm w/v Fe2+Fe2+ (MW=55.845 g/molMW=55.845 g/mol) solution. How many grams of ferrous ammonium sulfate hexahydrate (Fe(NH4)2(SO4)2⋅6H2O(Fe(NH4)2(SO4)2⋅6H2O, MW=392.14 g/molMW=392.14 g/mol) are needed to prepare this solution? Assume the final solution has a density of 1.00 g/mL.
1.1 Accurately (using an analytical balance ONLY) weigh 1.4 g of Fe(NH4)2(SO4) 2-6H20 1.2 Dissolve in...
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Can you answer question 4 & 5? The experiment and porcedure is posted below Question 4...
Can
you answer question 4 & 5? The experiment and porcedure is
posted below
Question 4 & 5
CHM3120C Analytical Chemistry Lab Lab 7. Spectrophotometric Determination of Iron in Mohr's Salt with o-Phenanthroline Required Reagents and Supplies: 50 mL of 0.0005M -0.0006 M of Mohr's solution (unknown), 10 g of Hydroxylamine hydrochloride (NH2OH, HCI), 500 mL of o-phenanthroline solution (contains 0.5 g of o-phenanthroline monohydrate), 83 g of sodium acetate (NaOAc. 3H20) in 500 mL of water (for 1.2 M...
1. A solid sample containing some Fe2+ weighs 2.360 g. It required 36.44 mL 0.0244 M...
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2. (a) What is the formula and color of the complex that forms when Fe" reacts...
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Can
you answer question 4 & 5? The experiment and porcedure is
posted below
Question 4 & 5
CHM3120C Analytical Chemistry Lab Lab 7. Spectrophotometric Determination of Iron in Mohr's Salt with o-Phenanthroline Required Reagents and Supplies: 50 mL of 0.0005M -0.0006 M of Mohr's solution (unknown), 10 g of Hydroxylamine hydrochloride (NH2OH, HCI), 500 mL of o-phenanthroline solution (contains 0.5 g of o-phenanthroline monohydrate), 83 g of sodium acetate (NaOAc. 3H20) in 500 mL of water (for 1.2 M...
1. A solid sample containing some Fe2+ weighs 2.360 g. It required 36.44 mL 0.0244 M KMnO, to titrate the Fe- in the dissolved sample to a pink end point. The balanced redox reaction is shown below. 8 H + MnO4 + 5 Fe2+ + Mn2+ + 5 Fe3+ + 4H20 Calculate each of the following quantities. 2. (2 points) Calculate the percentage of Fe in pure iron(II) ammonium sulfate hexahydrate: (NH4)2[Fe(SO4)2]• 6 H20.
2. (a) What is the formula and color of the complex that forms when Fe" reacts with 1,10- phenanthroline? (b) This complex absorbs strongly at which wavelength (in nm) of visible light? Indicate the color of light having this wavelength. (c) Is the color of the complex the same as th color of the light of maximum absorption? Would you expect them to be the same? Explain 3. What is the molar mass (in g/mol) of Fe(NH)(SO4): 6 H,0? 4....
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- Determine the theoretical yield in grams of iron(II) oxalate dihydrate, FeC204.2H20. Balance the following chemical equations: Feat =R2 N- Fe(NH)-(SO)2 + 6H-0+ 2.H.C0. - 2 FC 02H0+ (NH.)50. + HS0+ & HO H=22 N=2 C2 Fel 0=15 S=2 FeC204. 2H2O + H2C2O4 + H2O2 + 3 K.CO. - KiſFcc0bf-3H30 Transfer the balanced chemical reactions to page 6. 4. Use the first of the above balanced chemical equations to determine the following a. The reaction mixture initially contains 2.5 g...
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