how many grams of iron (111) sulfite pentahydrate are required to prepare a solution that has the equivalence of 0.339g of iron dissolved?

mm = molar mass

am = atomic mass

0.339 g Fe x (mm Fe2(SO3)2/2*am Fe) = ?

To determine the number of grams of iron (III) sulfite pentahydrate required to prepare a solution with the equivalence of 0.339g of iron dissolved, we need to know the molar mass of iron (III) sulfite pentahydrate and the stoichiometry of iron in the compound.

1. Find the molar mass of iron (III) sulfite pentahydrate:
Iron (III) sulfite pentahydrate has the chemical formula Fe2(SO3)3·5H2O.
The molar mass can be calculated by summing the atomic masses of each element in the formula:
Fe2 (55.85 g/mol) + S (32.07 g/mol) + O3 (3x16 g/mol) + 5H2O (5x18.02 g/mol) = molar mass of Fe2(SO3)3·5H2O

2. Calculate the number of moles of iron in 0.339g of iron:
Use the molar mass of iron (55.85 g/mol) to convert the mass of iron to moles:
Moles of iron = Mass of iron / Molar mass of iron

3. Determine the stoichiometry of iron in iron (III) sulfite pentahydrate:
In the chemical formula Fe2(SO3)3·5H2O, there are two iron atoms.

4. Calculate the molar mass of iron (III) sulfite pentahydrate:
Multiply the molar mass calculated in step 1 by the stoichiometry of iron:
Molar mass of iron (III) sulfite pentahydrate = Molar mass of Fe2(SO3)3·5H2O x (2/1)

5. Calculate the number of moles of iron (III) sulfite pentahydrate needed:
Use the moles of iron and the molar ratio between iron and iron (III) sulfite pentahydrate:
Moles of iron (III) sulfite pentahydrate = Moles of iron / Stoichiometry of iron

6. Convert moles of iron (III) sulfite pentahydrate to grams:
Calculate the mass of iron (III) sulfite pentahydrate using its molar mass:
Mass of iron (III) sulfite pentahydrate = Moles of iron (III) sulfite pentahydrate x Molar mass of Fe2(SO3)3·5H2O

By following these steps, you will be able to calculate the number of grams of iron (III) sulfite pentahydrate required.