Calculate the amount of Iron standard needed to make 1L of 15 ppm iron (Fe2+), from ferrous ammonium sulfate hexahydrate
We need at least 10 more requests to produce the answer.
0 / 10 have requested this problem solution
The more requests, the faster the answer.
Calculate the amount of Iron standard needed to make 1L of 15 ppm iron (Fe2+), from...
calculate the ppm of Fe2+ in a 0.6321g/2L solution of iron(II)ammonium sulfate hexahydrate.
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?
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.
Calculate
the amount of Iron(II) sulfate and the amount of phenanthroline
that needs to be weighed out and added to 100 mL of deionised water
to make a stock solution of the iron-phenanthroline complex which
has an iron concentration of 150 mg/L. Show your workings.
1801. -- + Fe" — ortho-phenanthroline Ferrous tris-o-phenanthroline |
8. If 45.52 mL of a potassium permanganate solution is needed to titrate 2.145 g of iron(II) ammonium sulfate hexahydrate, calculate the molarity of the KMnO4 solution
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. (2 points) Calculate the percentage of Fe in pure iron(I) ammonium sulfate hexahydrate: (NH4)2[Fe(SO4)2]. 6 H2O.
Calculate ppm from 1.86 g of NaCl, 1L of solution with a density of 1g/L
Spring 2019 CSUSM CHEM 175 8. Which statements are true? Select ALL. that apply. a) Dissolution of ammonium nitrate is an endothermic reactio b) Hydrogen gas evolves when calcium carbonate reacts with hydrochloric acid. c) The acid-base neutralization reaction is exothermic. ) The value of enthalpy change, AH, of calcium chloride dissolution is positive. sample contains an unknown amount of Fe?'which is titrated with a KMnO, solution in acidie tions to determine the iron composition by mass. A standardized KMnOs...
Calculate the concentration of each standard in terms of ppm iron. FW= 55.845 g/mol. Please show your work. First prepare standard solution from a standard Fe stock of 0.13 M. Make 100x dilution (1 mL of stock into 100 mL of water) Then, using a pipet deliver the following volumes of your Fe standard diluted solution into 10 mL volumetric flasks: 0 microliters, 150 micro liters, 300 microliters, 450 microliters, and 600 microliters.