Talk:Iron(II) hydroxide

Comments

could someone please state the uses and application of such substance? if there's no actual uses of Fe(OH)2, at least give the chemical formula of which Fe(OH)2 can be produced. looks like a lot of extra infomation is needed here. —The preceding unsigned comment was added by 219.79.186.57 (talk • contribs) .

Does this mean you're volunteering to improve the article? Thanks! =P I'll help you along with it. —Keenan Pepper 01:15, 18 May 2006 (UTC)[reply]

Why should anyone care about iron(II) hydroxide?

I notice someone removed the importance tag without actually adding anything important. The uses section is not a stub, it is empty. E-M-P-T-Y. Could someone please add any reason at all why anyone should care about this compound? —Keenan Pepper 15:32, 20 July 2006 (UTC)[reply]

You're right, I did some other repair work earlier today, I have now also reinserted the importance tag, and removed the not too filled uses section. --Dirk Beetstra ^{T C} 15:40, 20 July 2006 (UTC)[reply]

Okay. I'll try to do some research today and find out what this stuff is good fer. —Keenan Pepper 15:54, 20 July 2006 (UTC)[reply]

Early Earth's oceans

The earths oceans may have a lot of iron hydroxide in them, because the comets or asteroid that contain water mixed with iron. As a result, Earth's early oceans may have a greenish color, until the iron banded formation removed most of the iron to form rock.

For one thing, this needs a source, and for another the grammar is so bad I'm afraid I'll misinterpret it if I try to correct it. What time period is this talking about? Is "iron banded formation" the same as banded iron formation? —Keenan Pepper 22:59, 31 July 2006 (UTC)[reply]

Solubility

Trying to make sense of the solubilities listed (1.43 mg/liter and 0.72 g/100 ml). If Ksp = [Fe++][OH-]²= 8 x 10^-16 as given in the chembox, then at pH=7, you would have [OH]=10^-7 (since Kw=[H+][OH-]=10^-14 and [H+]=[OH-] at pH=7) and so [Fe++]=0.08 mole/liter. The molar mass is 89.86 gm/mole, so thats 7.19 gm/liter, or 0.719 gm/100 ml). So ok, thats good.

If you just put the oxide into water, and let the pH be whatever it turns out to be, then [OH-]=2[Fe++], and Ksp=[Fe++][2 Fe++]^2 so [Fe++]=5.85 x 10^-6 mole/liter or 0.53 mg/liter, not 1.43 mg/liter.

Am I doing the calculation wrong, or is the article inconsistent? PAR (talk) 23:52, 22 March 2017 (UTC)[reply]

Possible error in calculations

An anonymous editor recently added the following visible note to the "Preparation and reactions" section, which I have now hidden from public view: "somehow these values don't match the ones in the table on the right. Someone please verify where the 0,72 g/100mL comes from".

The same editor recalculated some of the numbers in the article; you can see the change here. It would be great if someone way smarter than me could take a look at this and determine whether it's legit, and whether any other numbers in the article need fixing. Thank you. Jessicapierce (talk) 18:43, 7 April 2018 (UTC)[reply]