How many moles are in FeSO4?
How many moles are in FeSO4?
1 moles
What is the mass of 1 molar mass Fe?
about 55.845 g/mol
What is the formula for FeSO4?
Iron(II) sulfate
| Names | |
|---|---|
| Chemical formula | FeSO4 |
| Molar mass | 151.91 g/mol (anhydrous) 169.93 g/mol (monohydrate) 241.99 g/mol (pentahydrate) 260.00 g/mol (hexahydrate) 278.02 g/mol (heptahydrate) |
| Appearance | White crystals (anhydrous) White-yellow crystals (monohydrate) Blue-green crystals (heptahydrate) |
| Odor | Odorless |
How do you make Fe2+ solution?
Prepare a ferrous iron stock solution (100 mg/L Fe2+) by dissolving 0.7022 grams of ferrous ammonium sulfate, hexahydrate, in deionized water. Dilute to 1 liter. Prepare immediately before use. Dilute 1.00 mL of this solution to 100 mL with deionized water to make a 1.00 mg/L standard solution.
What will happen if we drink Ferrous ammonium sulphate?
It causes gastrointestinal pains, may cause kidney failure or liver poisoning, and also its a mild eye and skin irritant.
How do you make 0.05 M Ferrous ammonium sulphate?
Procedure
- Prepare 250 ml of M/20 Mohr’s salt solution by dissolving 4.9 g of Mohr’s salt in water 20 as described in experiment 11.3.
- Rinse and fill the burette with the given KMn04 solution.
- Add one test-tube (~ 20 ml) full of dilute sulphuric acid (~ 2 M) to the solution in titration flask.
Why Mohr’s salt is used instead of ferrous sulphate?
Mohr’s salt is used in analytical chemistry as the preferred source of ferrous ions due to the solid’s extended shelf life and resistance to oxidation. Sulfuric acid is often added to solutions using ferrous ammonium sulfate in order to reduce the oxidation of the ferric iron.
Why FeSO4 is not used in titration?
FeSO4 easily oxidises to Fe2(SO4)3 especially when it is dissolved in water to make a solution. The titration involves the coversion of Fe2+ to Fe3+ and the conversion will give an error in the determination.
What is the commercial name of FAS?
Free alongside
Why Sulphuric acid is used in titration?
Answer. Sulphuric Acid (H2SO4) is used in the redox titration process because it provides the H(+) ions necessary for the reaction to occur more quickly whilst the sulphate(-) ions barely react during the reaction. Therefore, sulfuric acid is added to make the solution acidic.