highspeed7458

29.06.2019 • 

Chemistry

Asample of 1.55 g of iron ore is dissolved in an acid solution in which the iron is converted into
fe2+. the solution formed is then titrated with kmno4 which oxidises fe2+ to fe3+ while the mno4-
ions are reduced to mn2+ ions. 92.95 ml of 0.020 m kmno4 is required for the titration to reach
the equivalence point.
a) write the balanced equation for the titration.
b) calculate the percentage of iron in the sample.

Ответ:

kaciewelkerouwdfa

10.03.2022

Chemistry

---

a) 8H2SO4+2KMnO4+10FeSO4→5Fe2(SO4)3+8H2O+2MnSO4+K2SO4

B) nKMno4 = 0.001859 mol

=>nFeso4=0.009295 mol

nFe= 0.009295 mol

mFe=0.52052 g

=>percentage of iron in the sample: 33.5819%

Explanation:a) 8H2SO4+2KMnO4+10FeSO4→5Fe2(SO4)3+8H2O+2MnSO4+K2SO4

B) nKMno4 = 0.001859 mol

=>nFeso4=0.009295 mol

nFe= 0.009295 mol

mFe=0.52052 g

---

0,0(0 оценок)

Ответ:

Cheyenneross366

20.12.2020

Chemistry

---

It should be rocky surfaces!

---

0,0(0 оценок)