[joel0201]

hi i have a chemistry sac tomorrow. i have t find the iron (2) content in fertiliser as a percentage by mass
background info.
the amount of 40.304g/l of fertilisers is 20ml. that was mixed with 20ml of h2SO4 which was a 1M solution. it was titrated with potassium permanganate 0.001M solution the average titrate was 1.63ml.
acording the equation 5Fe2+ + Mn04- + 8H- ------> 5Fe3+ + Mn2+ + 4H2O.
 

[sjb]

hi i have a chemistry sac tomorrow. i have t find the iron (2) content in fertiliser as a percentage by mass
background info.
the amount of 40.304g/l of fertilisers is 20ml. that was mixed with 20ml of H₂SO₄ which was a 1M solution. it was titrated with potassium permanganate 0.001M solution the average titrate was 1.63ml.
acording the equation 5Fe²⁺ + MnO₄^- + 8H⁺  5Fe³⁺ + Mn²⁺ + 4H₂O.
 

What mass of fertilizer did you titrate? How much permanganate was there in your titre?

[joel0201]

i titrated 1.63ml of KMnO4 against a solution containing 20ml of H2SO4 and 20ml of the fertiliser.

[Borek]

i titrated 1.63ml of KMnO4 against a solution containing 20ml of H2SO4 and 20ml of the fertiliser.

That's not the answer to the question sjb asked, you have just repeated what is given in the problem.

Titration is all about stoichiometry. So, first of all - how much permanganate was there in the titre?

http://www.titrations.info/titration-calculation

[joel0201]

there was 1.6ml in the titrate

[Borek]

1.63 mL is the volume of the solution, not the amount of the substance present. How many moles of permanganate in these 1.63 mL?