Question 234604

A student begins preparing the Fe2+ stock solution by weighing 0.1756 g of (NH4)2Fe(SO4)2∙6H2O. The
solid is dissolved in a small amount of deionized water then transferred to a 250 mL volumetric flask.
The solution is brought to a volume of 250.0 mL with deionized water and mixed. The molar mass of
(NH4)2Fe(SO4)2∙6H2O is 392.15 g/mol.
a. Calculate the molarity of (NH4)2Fe(SO4)2∙6H2O in this stock solution.
b. Calculate the molarity of Fe2+ in this stock solution.
c. Calculate the concentration of Fe2+ in the stock solution in units of g/L.
d. Calculate the concentration of Fe2+ in the stock solution in units of μg/dL.

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