Talk:Iron(II) sulfate

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What are the side effects[edit]

if contact with the eye server itches and pains, Precautions are, wash out with water, seek for medicle attension

Molecular weight[edit]

The molecular weight will differ depending on which hydrate is used. (mass of the water must be factored in). I'm too lazy to add/look them all up... --128.32.8.164 19:29, 11 July 2006 (UTC)

Odor[edit]

I just opened up a bottle of the heptahydrate in the lab and noticed a distinct Maple syrup odor. Whoever maintains this article should add this detail somewhere.Beakerboy 18:38, 19 April 2007 (UTC)

This won't be from the iron(II) sulfate itself, it must be some sort of impurity. The iron(II) sulfate should be pretty much odorless. Walkerma 21:14, 19 April 2007 (UTC)

Further heating[edit]

The article mentions that heating solid iron (II) sulfate gives water. Further heating produces a condensate of quite pure sulfuric acid. Is this worthy of mention? Not least as a potential hazard for anyone contemplating actually heating the solid. Dajwilkinson 23:37, 3 June 2007 (UTC)

The point is well taken, but many compounds when subjected to high temperatures release dangerously reactive substances. IMHO, WE-chem would need to dedicate inordinate space to describe every possible precaution against every possible way of treating a given chemical.--Smokefoot 03:44, 4 June 2007 (UTC)
Couldn't you simply add the decomposition temperature in the table of information shown at right? Many, if not most chemicals on WP list their melting, boiling and decomposition temperatures. This one doesn't, but I don't think adding one more line to the table constitutes dedicating inordinate space, as you put it. Plus, it's good info to know - most importantly for those interested in completeness, those interested in safety, and those who might want to decompose the substance. For the record, it decomposes at 300 °C 97.82.247.200 06:40, 8 August 2007 (UTC)

Indigo[edit]

Was it really used as an oxidizer with indigo dye? That sounds like ferrIC sulfate. Admittedly, some Fe(III) may be present, but then, that isn't Fe(II) sulfate either.

24.159.247.111 03:25, 12 June 2007 (UTC)

Good point. The same error occurred in the indigo dye article. Although I haven't used FeSO4, I run a lab every year with indigo, and it's clear from that and the indigo dye article that the author meant "reduced" not oxidized. You have to reduce indigo to a soluble form in a bath to get it onto the fabric, and that's the harder part (that required urine in the old days - you can guess why they developed this process!). The oxidation of leuco-indigo back to indigo happens in air in a minute or two. So I've rewritten it as something much more plausible, but I'd still like to see a ref for this. Thanks, Walkerma 04:47, 12 June 2007 (UTC)

Minor cleanup[edit]

Just did a few minor edits on this article. Cleaned up a few poorly-formed sentences and added some missing punctuation. 97.82.247.200 01:45, 21 August 2007 (UTC)

Nice work, thanks. Walkerma 03:27, 21 August 2007 (UTC)

Reactions[edit]

In the article it mentions that iron(II) sulfate is a reducing agent and then says "For example, it reduces nitric acid to nitrogen oxide and chlorine." Now, call me crazy, but the last I checked there is no chlorine present in either reactants, so where the heck does chlorine come from? I think it should read nitrogen oxide and water. Maybe chlorine is released if you are using iron(II) chloride, but this is an article about the sulfate... 75.170.50.130 (talk) 00:25, 13 October 2008 (UTC)