Chemistry Forum

Thanks to the 'expert' for his advice on my other queries..! It would appear that the Chlorine dioxide / sodium chlorite reaction with H₂S is a tricky one to iron out...! If you pardon the pun i have another query for all those out there. This one relates to Iron sulphide as a secondary reaction with the chlorine dioxide formed...!

5 FeS(s) + 9 ClO₂ + 2 H₂O --> 5 Fe₃+ + 5 SO₄₂- + 9 Cl- + 4 H+

I'm not sure if this rection is possible, due to oxidation states and electron transfer.

There wouldn't appear to be enough electron present..? Or is there..?!?

What would the iron react with and what would the sulphate ion react with as i gather they can't just exist on there own..?!?

I maybe wrong here, but through and comments are always welcome...!

As you can tell i'm struggling with the reaction of sodium chlorite applied to an alkaline stream containing H₂S

In acid conditions I think sodium chlorite reacting with H₂S gives

2H₂S + NaClO₂ --> 2S + NaCl + 2H₂O

However in an alkali environment (lot of Sulphide, S₂-, ions present) I have read the reaction for the chlorite with H₂S as…

S₂- + 2 NaClO₂  SO₄ 2- + 2NaCL

I am hearing that NaClO₂, temporarily form Chlorine Dioxide which then reacts with the H₂S in an alkaline environment, but not sure...?

Anyone any ideas...?

Chemist₇₆

"5 FeS(s) + 9 ClO₂ + 2 H₂O --> 5 Fe₃+ + 5 SO₄₂- + 9 Cl- + 4 H+

I'm not sure if this reaction is possible, due to oxidation states and electron transfer."

This is certainly possible, I'm not sure about the coefficients though. The main rule is that the given electrons in the reaction should be exactly equal to the taken electrons