Chemistry Forum

Posted: **Sun Oct 22, 2017 12:17 pm**

I am having trouble wrapping my head around this problem, how do I even get started?

5 Fe+2 +MnO4 + 8H+ = 5Fe+3 +Mn+2 + 4H2O

Suppose 1.507g of

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FeCl2

is placed in a 250 ml Erlenmeyer flask to which 50 mL of water and 10 mL of

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H2SO4

are added. This solution will be titrated by adding 0.1227 M

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KMnO4

. I would like to figure out moles of

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Fe+2

are initially present.
Do you use a new equation with

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 FeCl2 + KMnO4 + H2O + H2SO4?

Need something to make sense so I can work though this. Couldn't figure out the superscripts, sorry!

Posted: **Sun Oct 22, 2017 12:40 pm**

1 mol FeCl₂ corresponds to 1 mol Fe₂+

n = m/M n = 1,507 g/126,75 g/mol = 0,0119 mol

This the molarity of Fe₂+

0,12227 M KMnO₄ = 0,12227 mol/l MnO₄-

Calculate with this.

Posted: **Sun Oct 22, 2017 1:03 pm**

thanks, the whole Cl₂ addition was confusing me.

Posted: **Mon Jan 15, 2018 1:22 am**

I'm think this website focus on the small process . Limit on minimun step on calculation or specific on well-known chemistry equation .

Chemistry Forum

Iron by Titration - Redox Rxn

Iron by Titration - Redox Rxn