Homework Help: science

Posted by ngela on Sunday, January 27, 2013 at 10:39pm.

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?

science - bobpursley, Sunday, January 27, 2013 at 10:51pm
find the formula mass of ferrous sulfate 7hydrate.

then, percent= atomicmassFe/formulamass

and percent=massFe/masscompound

masscompound=atomicmassFe*massFe/formulamass

Answer this Question

Related Questions

chemistry - an iron supplement is used to treat anaemia and 50mg of iron 2 is ...
chemistry - Question is: If you gain your iron from an iron citrate (Fe(C6H7O7)2...
Chemistry - What mass of 3.0 wt% H2O2 solution is required to provide a 25% ...
Chemistry - If each tablet of a dietary supplement contains ~20 mg of iron how ...
Chemistry - Calculate mass of iron in tablet by spectroscopy? I have to ...
chemistry - You extract the iron from a tablet and dilute that to 600.0 ml in a ...
Chemistry - The experiment requires 1 mg per ml of iron. what masss of iron (III...
Chem. - The experiment requires 1 mg per ml of iron (Fe3+). What mass of iron (...
chemistry - You extract the iron from a tablet and dilute that to 350.0 ml in ...
Chemistry - Pharmacists sell tablets containing magnesium hydroxide, Mg(OH)2, to...

For Further Reading

First Name:
School Subject:
Answer: