Solution A was prepared from 0.2703g of ferrous ammonium sulfate [Fe(SO4)2(NH4)2• 6H20; Molar mass = 392.2g/mole]...

Question:

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. (Hint: MAVA = MBVB)

(c) How many millimoles of Fe2+ are present in a 10.00 mL sample of solution B ? (Hint: millimoles in solution B = mL x molarity of solution B)

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