[JBake010]

Hello all, I am taking a Chemistry I class, and I am currently doing a prelab for my titration lab tomorrow, but I'm stuck.

The first thing I had to do was balance the formula: Fe⁺² + MNO₄^-  Fe⁺³ + Mn⁺², and I balanced it to look like this: 8H⁺ + 5Fe⁺² + MnO₄^-  5Fe⁺³ + Mn⁺² + 4H₂O

then it moves on to tell me that 1.2523g of iron (II) ammonium sulfate hexahydrate (Fe(NH₄)₂(SO₄)₂ times 6H₂O was dissolved in water and titrated with a permanganate solution of unknown concentration. The initial buret reading for the titration was 0.37mL and the buret reading at the point when the reaction was complete was 27.87mL. Calculate the molarity of the permanganate solution.

Now I know I need to conver 1.2523g to mols, so I did (and got 0.003193 mols), but I am stuck as to what I do from here.

Could anyone please offer some help?

[UG]

Now I know I need to conver 1.2523g to mols, so I did (and got 0.003193 mols), but I am stuck as to what I do from here.

Ok, so from your balanced equation, how many moles of MnO₄^- reacted with the Fe²⁺? And what volume of permanganate solution was used in the titration? With these two pieces of information, you should be able to work out the molarity. See how you go.