Question

The unknowns are a mixture of ferrous ammonium sulfate and ammonium sulfate. calculate the amount of ferrous ammonium sulfate and the amount of ammonium sulfate needed to prepare a sample that is 10% fe with a total mass of 0.2 g

Answer 1

Answer: -

Molar mass of ferrous ammonium sulfate =392 g / mol

Mass of iron present in ferrous ammonium sulfate = 56 g/mol

Total mass required = 0.2 g

Total mass of iron Fe required = 10% of 0.2 g

                                           = $\frac{10}{100}$x0.2

                                            = 0.02 g

Only ferrous ammonium sulfate has iron. So all iron must be present only as ferrous ammonium sulfate.

56 g of iron is present in 392 g of ferrous ammonium sulfate

0.02 g of iron is present in $\frac{392}{56}$ x 0.02

                                                       = 0.14 g

Mass of ammonium sulfate = 0.2 - 0.14 = 0.06 g

Thus the required composition must be 0.06 g ammonium sulfate and 0.14 g ferrous ammonium sulfate.