an iron supplement is used to treat anemia and 50 mg of FE is required per tablet. If the iron compound used in th tablet is FeSO4.7H2O,what mass of this compound would be required per tablet to provide the desired amount of Fe?
find the formula mass of ferrous sulfate 7hydrate.
then, percent= atomicmassFe/formulamass
and percent=massFe/masscompound
masscompound=atomicmassFe*massFe/formulamass
To determine the mass of FeSO4.7H2O required per tablet, we need to consider the molar mass of FeSO4.7H2O and the molar mass of Fe.
1. Find the molar mass of FeSO4.7H2O:
- The molar mass of Fe is approximately 55.84 g/mol.
- The molar mass of S is approximately 32.06 g/mol.
- The molar mass of O is approximately 16.00 g/mol.
- The molar mass of H is approximately 1.01 g/mol.
- Since FeSO4.7H2O contains 7 water molecules, we need to add their molar mass as well. The molar mass of H2O is approximately 18.02 g/mol.
- Therefore, the molar mass of FeSO4.7H2O is:
(1 x molar mass of Fe) + (1 x molar mass of S) + (4 x molar mass of O) + (7 x molar mass of H2O)
2. Calculate the molar mass of FeSO4.7H2O:
Molar mass of FeSO4.7H2O = (1 x 55.84) + (1 x 32.06) + (4 x 16.00) + (7 x 18.02)
3. Determine the mass of FeSO4.7H2O required per tablet:
Mass of FeSO4.7H2O per tablet = (Mass of Fe required per tablet) / (Molar mass of FeSO4.7H2O)
Let's substitute the values:
Mass of FeSO4.7H2O per tablet = 50 mg / (Molar mass of FeSO4.7H2O in g/mol)
By following these steps, you can obtain the mass of FeSO4.7H2O required per tablet to provide the desired amount of Fe.