2. (2 points) Calculate the percentage of Fe in pure iron(I) ammonium sulfate hexahydrate: (NH4)2[Fe(SO4)2]. 6...
2.5g of AR ammonium iron (ll) sulfate hexahydrate crystals are dissolved in 40mL of 1M sulfuric acid solution. Solution is then titrated with 6.4mL of 0.02M potassium permanganate (VII) solution. a) Write an overall equation for the reaction. b) How many moles of permanganate are present in the titre value? c) How many moles of Fe^2+ are present in the solution? d) What mass of Fe^2+ is present in the ammonium iron (ll) sulfate hexahydrate? e) What is the percentage...
calculate the ppm of Fe2+ in a 0.6321g/2L solution of iron(II)ammonium sulfate hexahydrate.
Calculate the amount of Fe(NH4)2(SO4)2·6H2O needed to make 250mL of a 0.002M iron solution. (2 points)
HULIOL QUESTION 7 The formula for ammonium sulfate is a. NH4(SO4)2 b. NH4504 c. (NH4)2(SO4)2 d. (NH4)2SO4
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.
What is the formula mass of iron(II) ammonium sulfate hexahydrate? submit your answer to 6 significant figures
write the balanced equation for this reaction and calculate the percentage yield. Iron (I) Chloride hexahydrate 5mL Methanol 1.64g 7 A 2.56g &nh of H₂O sodium acetate 7 B gives Veild of 1.579 ol Fe (Cs H₂O₂) (FeCl 3.6H2O) Iron (II) Chloride hexahydrate lisng} A 8 mL H2O add solution to A 2.56g of sodium acetate 5 mL methonal gives Veild of 1.579 of Fe (Cs H₂O2)
Please help me balance the equation: ___ Fe(NH4)2(SO4)2 · 6 H2O + ___ H2C2O4 + ___ K2C2O4 + ___ H2O2 → ___ K3Fe1(C2O4)3 * 6 H2O + ___ (NH4)2SO4 + ___ H2SO4 + ___ H2O (Hint given: Remember H2O2, an oxidizing agent, was used in the synthesis, so you’ll need to do a redox balance. Start with just the iron ions, balance the reaction, and then add the full formulas.)
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....
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?