How do you solve this titration calculation?
35.0 g of hydrated iron(II) ammonium sulfate #sf(Fe(NH_4)_2(SO_4)_(2).6H_2O)# is dissolved in 1 litre of water. 25.00 ml is added to a flask and acidified. When titrated against #sf(KMnO_4)# solution an average titre of 21.00 ml was recorded. What is the concentration of the Mn(VII) solution in g/l ?
35.0 g of hydrated iron(II) ammonium sulfate
1 Answer
You can do it like this:
Explanation:
Start with the two 1/2 equations:
To get the electrons to balance we multiply
This tells us that 1 mole Mn(VII) reacts with 5 moles Fe(II).
The
The no. moles of iron(II) in 1000 ml is therefore
From the mole ratio we can say that:
In grams/litre the concentration is given by:
This is equal to 0.335 g/100 ml or 0.33% (w/v) to 2 sig fig.