first to calculate mass of Fe.
then to calculate it's mole.
then, moles of Fe = moles of compound.
then, to find mass of compound.
Calculate the mass amount of Fe(NH4)2(SO4)2•6H2O needed to prepare 100mL 1000mg Fe/L stock solution?
Calculate the amount of Fe(NH4)2(SO4)2·6H2O needed to make 250mL of a 0.002M iron solution. (2 points)
5.012g of Fe(NH4)2(SO4)4. 6H2O Find the mass of K3[Fe(C2O4)3]·3H2O in g Fe(NH4)2(SO4)4. 6H2O + H2C2O4=FeC2O4(s) + H2SO4 + (NH4)2SO4 + 6H2O(l) FeC2O4 +K2C2O4 + H2O= Fe(OH)3(s) + .....etc Fe(OH)3 + H2O2 + K2C2O4=K3[Fe(C2O4)3]·3H2O + ..etc
A solution is prepared by dissolving 0.300 g Fe(NH4)2(SO4)2*6H2O in sufficient water to produce 250.0 mL of solution. a. What is the molar concentration of Fe2+? b. What is the molar concentration of NH4+? c. What is the concentration of sulfur in mg/L?
Calculate the mass of FeSO4 (NH4)2 6H2O that is required to prepare 500mL of a 6.00*10^4M solution?
1.1 Accurately (using an analytical balance ONLY) weigh 1.4 g of Fe(NH4)2(SO4) 2-6H20 1.2 Dissolve in 50 mL of 4% sylturisacid in a beaker. 1.3 Transfer into a 1 L volumetric flask; adjust the volume and mix well. Note the purity of the Fe(NH4)2(SO4)2.6H20 given on the label of the container. 1.4 Transfer this solution into a 1 L glass bottle. Preparation of working iron standard solution: 1.5 Pipet 10.00 mL of the iron standard stock solution into a 500.0...
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.
2. (2 points) Calculate the percentage of Fe in pure iron(I) ammonium sulfate hexahydrate: (NH4)2[Fe(SO4)2]. 6 H2O.
Solution A was prepared from 0.2703g of ferrous ammonium sulfate [Fe(SO4)2(NH4)2• 6H20; Molar mass = 392.2g/mole] dissolved in 100.0 mL of distilled water. Show all work for full credit. (a) Calculate the molarity of solution A. (Remember molarity = moles/Liter) Solution B was prepared by pipeting 25.00 mL of solution A into a 250.0 mL volumetric flask, and then the flask was diluted to the mark (exactly 250.0 mL, Vb) with distilled water. (b) Calculate the molarity of solution B....
Calculate the mass needed to make 100mL of a 2.0mM sodium sulfate solution
Calculate the amount of 0.1 M sucrose solution and the amount of dH2O needed to prepare 100 mL of unbuffered 20 mM sucrose. (Hint: use the formula c1v1=c2v2 to calculate the amount of sucrose stock solution needed) Amount of 0.1 M sucrose solution needed? Amount of dH2O needed?