The standard solutions used in this lab were made using a Fe2+ stock solution co

Question

The standard solutions used in this lab were made using a Fe2+ stock solution containing 0.1756 g of (NH4)2Fe(SO4)26H2O in 250.0 mL. The molar mass of (NH4)2Fe(SO4)26H2O is 392.15 g/mol. a. Calculate the molarity of (NH4)2Fe(SO4)26H2O in this stock solution. b. Calculate the molarity of Fe2+ in this stock solution. c. Calculate the concentration of (NH4)2Fe(SO4)26H2O in the stock solution in units of g/L. d. Calculate the concentration of Fe2+ in the stock solution in units of g/L. e. Calculate the concentration of (NH4)2Fe(SO4)26H2O in the stock solution in units of g/dL. f. Calculate the concentration of Fe2+ in the stock solution in units of g/dL.

Explanation / Answer

a)

moles of (NH4)2Fe(SO4)26H2O = 0.1756 / 392.15

                                                    = 4.48 x 10^-4 mol

Moalrity of (NH4)2Fe(SO4)26H2O = 4.48 x 10^-4 / 0.250

Moalrity of (NH4)2Fe(SO4)26H2O = 1.791 x 10^-3 M

b)

conentration of Fe+2 = 1.791 x 10^-3 M

c)

concnetration of (NH4)2Fe(SO4)26H2O = 1.791 x 10^-3 x 392.15

concnetration of (NH4)2Fe(SO4)26H2O = 0.7024 g/ L

d)

Calculate the concentration of Fe2+ = 0.7024 g /L

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